alkalinity

[Dinky]

I'm having some difficulty wrapping my brain around alkalinity and it's
relationship to PH. Can anyone explain it in "Aquaria for idiots" fashion,
or point me to a place where it's explained? I'm starting to feel like I
need to take a couple BioChem classes.

tia

billy

--

--

[stoutman]

pH = -log[+H]. This is a measure of the free hydrogen ion concentration in
solution. pH > 7 is basic pH < 7 is acidic.

Think of alkalinity as 'buffering capacity'. Or the ability of a solution
to resist a drop in pH due to the addition of acid. The presence of Ca+
ions and CO3-2 ions in solution add to the buffering system.

The concentration of CaCO3 in solution accounts for 'most' of the observed
alkalinity.

Alkalinity is important because it prevents a sharp drop in pH due to the
addition of acid.

Did that help?


"Dinky" > wrote in message
hlink.net...
> I'm having some difficulty wrapping my brain around alkalinity and it's
> relationship to PH. Can anyone explain it in "Aquaria for idiots" fashion,
> or point me to a place where it's explained? I'm starting to feel like I
> need to take a couple BioChem classes.
>
> tia
>
> billy
>
> --
>
> --
>
>

[stoutman]

This may help to clear things up.

A solution with high pH and a strong buffering capacity will drop in pH much
slower with the addition of acid than a solution of the same pH and no
buffering capacity.




"stoutman" <.@.> wrote in message news:0kgVb.114897$U%5.595597@attbi_s03...
> pH = -log[+H]. This is a measure of the free hydrogen ion concentration
in
> solution. pH > 7 is basic pH < 7 is acidic.
>
> Think of alkalinity as 'buffering capacity'. Or the ability of a solution
> to resist a drop in pH due to the addition of acid. The presence of Ca+
> ions and CO3-2 ions in solution add to the buffering system.
>
> The concentration of CaCO3 in solution accounts for 'most' of the observed
> alkalinity.
>
> Alkalinity is important because it prevents a sharp drop in pH due to the
> addition of acid.
>
> Did that help?
>
>
> "Dinky" > wrote in message
> hlink.net...
> > I'm having some difficulty wrapping my brain around alkalinity and it's
> > relationship to PH. Can anyone explain it in "Aquaria for idiots"
fashion,
> > or point me to a place where it's explained? I'm starting to feel like I
> > need to take a couple BioChem classes.
> >
> > tia
> >
> > billy
> >
> > --
> >
> > --
> >
> >
>
>

[Dinky]

"stoutman" <.@.> wrote in message news:0kgVb.114897$U%5.595597@attbi_s03...

>
> Did that help?
>

Yes! Very much so. I'm not sure why I didn't get it before, I've been
running FW planted tanks, and am quite familiar with the concept of
buffering capacity. Thank you very much.

billy

[Boomer]

We need to make something clear about pH drops and Alk. You can have all the alk you want
in the world and it won't help, in regards to CO2. If CO2 increases the pH will drop, no
mater what the Alk is. Same thing if you remove the CO2, the pH will rise an there will be
no effect on the Alk.


"buffering capacity "

Bad term as Buffering Capacity isn't Alkalinity. Alk is more on the order of ANC (Acid
Neutralizing Capacity). BC is the ability to withstand upward and downward trends in pH do
to the addition of an acid or base.There is also a measurement called Acidity ( B_aseNC
and test kits for it). So the combination of the two more or les is BC. But I know what
you mean, may use the term ALK and BC interchangeably
--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
www.coralrealm.com

If You See Me Running You Better Catch-Up
"stoutman" <.@.> wrote in message news:XygVb.245342$xy6.1306359@attbi_s02...
: This may help to clear things up.
:
: A solution with high pH and a strong buffering capacity will drop in pH much
: slower with the addition of acid than a solution of the same pH and no
: buffering capacity.
:
:
:
:
: "stoutman" <.@.> wrote in message news:0kgVb.114897$U%5.595597@attbi_s03...
: > pH = -log[+H]. This is a measure of the free hydrogen ion concentration
: in
: > solution. pH > 7 is basic pH < 7 is acidic.
: >
: > Think of alkalinity as 'buffering capacity'. Or the ability of a solution
: > to resist a drop in pH due to the addition of acid. The presence of Ca+
: > ions and CO3-2 ions in solution add to the buffering system.
: >
: > The concentration of CaCO3 in solution accounts for 'most' of the observed
: > alkalinity.
: >
: > Alkalinity is important because it prevents a sharp drop in pH due to the
: > addition of acid.
: >
: > Did that help?
: >
: >
: > "Dinky" > wrote in message
: > hlink.net...
: > > I'm having some difficulty wrapping my brain around alkalinity and it's
: > > relationship to PH. Can anyone explain it in "Aquaria for idiots"
: fashion,
: > > or point me to a place where it's explained? I'm starting to feel like I
: > > need to take a couple BioChem classes.
: > >
: > > tia
: > >
: > > billy
: > >
: > > --
: > >
: > > --
: > >
: > >
: >
: >
:
:

[stoutman]

>If CO2 increases the pH will drop, no mater what the Alk is. Same thing if
you remove the CO2, the pH will rise an there will be no effect on the Alk.

Yes, the pH will drop with the addition of CO2. Remove CO2 will cause the
pH to rise? How do you remove CO2? Once it is in solution it forms
carbonic acid and neutralizes some of your 'buffer'.

>You can have all the alk you want in the world and it won't help, in
regards to CO2.

Wrong. Alkalinity increases your tank's ability to RESIST sharp changes in
pH. This is what is meant by 'buffering capacity'.

Alkalinity is the direct measurement of 'buffering capacity'.

..




"Boomer" > wrote in message
...
> We need to make something clear about pH drops and Alk. You can have all
the alk you want
> in the world and it won't help, in regards to CO2. If CO2 increases the pH
will drop, no
> mater what the Alk is. Same thing if you remove the CO2, the pH will rise
an there will be
> no effect on the Alk.
>
>
> "buffering capacity "
>
> Bad term as Buffering Capacity isn't Alkalinity. Alk is more on the order
of ANC (Acid
> Neutralizing Capacity). BC is the ability to withstand upward and downward
trends in pH do
> to the addition of an acid or base.There is also a measurement called
Acidity ( B_aseNC
> and test kits for it). So the combination of the two more or les is BC.
But I know what
> you mean, may use the term ALK and BC interchangeably
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message
news:XygVb.245342$xy6.1306359@attbi_s02...
> : This may help to clear things up.
> :
> : A solution with high pH and a strong buffering capacity will drop in pH
much
> : slower with the addition of acid than a solution of the same pH and no
> : buffering capacity.
> :
> :
> :
> :
> : "stoutman" <.@.> wrote in message
news:0kgVb.114897$U%5.595597@attbi_s03...
> : > pH = -log[+H]. This is a measure of the free hydrogen ion
concentration
> : in
> : > solution. pH > 7 is basic pH < 7 is acidic.
> : >
> : > Think of alkalinity as 'buffering capacity'. Or the ability of a
solution
> : > to resist a drop in pH due to the addition of acid. The presence of
Ca+
> : > ions and CO3-2 ions in solution add to the buffering system.
> : >
> : > The concentration of CaCO3 in solution accounts for 'most' of the
observed
> : > alkalinity.
> : >
> : > Alkalinity is important because it prevents a sharp drop in pH due to
the
> : > addition of acid.
> : >
> : > Did that help?
> : >
> : >
> : > "Dinky" > wrote in message
> : > hlink.net...
> : > > I'm having some difficulty wrapping my brain around alkalinity and
it's
> : > > relationship to PH. Can anyone explain it in "Aquaria for idiots"
> : fashion,
> : > > or point me to a place where it's explained? I'm starting to feel
like I
> : > > need to take a couple BioChem classes.
> : > >
> : > > tia
> : > >
> : > > billy
> : > >
> : > > --
> : > >
> : > > --
> : > >
> : > >
> : >
> : >
> :
> :
>
>

[stoutman]

Just to clear things up a little better. I'm not sure how else to make this
any easier to understand.

alkalinity is a measurement of 'buffering capacity'
pH is a measurement of 'acidity/basicity'.


"Boomer" > wrote in message
...
> We need to make something clear about pH drops and Alk. You can have all
the alk you want
> in the world and it won't help, in regards to CO2. If CO2 increases the pH
will drop, no
> mater what the Alk is. Same thing if you remove the CO2, the pH will rise
an there will be
> no effect on the Alk.
>
>
> "buffering capacity "
>
> Bad term as Buffering Capacity isn't Alkalinity. Alk is more on the order
of ANC (Acid
> Neutralizing Capacity). BC is the ability to withstand upward and downward
trends in pH do
> to the addition of an acid or base.There is also a measurement called
Acidity ( B_aseNC
> and test kits for it). So the combination of the two more or les is BC.
But I know what
> you mean, may use the term ALK and BC interchangeably
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message
news:XygVb.245342$xy6.1306359@attbi_s02...
> : This may help to clear things up.
> :
> : A solution with high pH and a strong buffering capacity will drop in pH
much
> : slower with the addition of acid than a solution of the same pH and no
> : buffering capacity.
> :
> :
> :
> :
> : "stoutman" <.@.> wrote in message
news:0kgVb.114897$U%5.595597@attbi_s03...
> : > pH = -log[+H]. This is a measure of the free hydrogen ion
concentration
> : in
> : > solution. pH > 7 is basic pH < 7 is acidic.
> : >
> : > Think of alkalinity as 'buffering capacity'. Or the ability of a
solution
> : > to resist a drop in pH due to the addition of acid. The presence of
Ca+
> : > ions and CO3-2 ions in solution add to the buffering system.
> : >
> : > The concentration of CaCO3 in solution accounts for 'most' of the
observed
> : > alkalinity.
> : >
> : > Alkalinity is important because it prevents a sharp drop in pH due to
the
> : > addition of acid.
> : >
> : > Did that help?
> : >
> : >
> : > "Dinky" > wrote in message
> : > hlink.net...
> : > > I'm having some difficulty wrapping my brain around alkalinity and
it's
> : > > relationship to PH. Can anyone explain it in "Aquaria for idiots"
> : fashion,
> : > > or point me to a place where it's explained? I'm starting to feel
like I
> : > > need to take a couple BioChem classes.
> : > >
> : > > tia
> : > >
> : > > billy
> : > >
> : > > --
> : > >
> : > > --
> : > >
> : > >
> : >
> : >
> :
> :
>
>

[Boomer]

Let me make this clear you don't know what you are taking about

"alkalinity is a measurement of 'buffering capacity'"

No, it is the ability to neutralize an acid. BC is the ability to withstand both upward
and downward trends in pH.

"pH is a measurement of 'acidity/basicity'.

No, pH is a measurement of acidity and pOH is a measurement of Basicity, if you want to
get picky, which seems you do.


"How do you remove CO2? "

It is called "blowing it off" , such as with an airstone. If you have high CO2 and add an
airstone it will drive the CO2 off raising the pH. It can be proven with a glass of water,
a straw, some pH color indicator and an Alk test kit and if you must a CO2 test kit

>You can have all the alk you want in the world and it won't help, in
regards to CO2

"Wrong. Alkalinity increases your tank's ability to RESIST sharp changes in
pH. This is what is meant by 'buffering capacity'"

No you are wrong and very lost. If Alk resists changes in pH then why does CO2 lower the
pH without affecting the Alk ? CO2 has no effect on alk and alk has no effect on CO2. When
CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At any pH no matter what
the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3

..
Go ahead and pick a seawater pH and I will tell you what that ratio is. Tell me the pH and
Alk and I will give the CO2 concentration. Give me the Alk and CO2 and I will give you
the pH. Don't forget the temperature and Salinity.

Alk is defined as;

TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] + [HPO4--] +
2[PO4---] - [H+]


Buffering Capacity is defined as;

BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka + [H3O+])²

In any aqueous solution maximum BC is reached when pH= pKa. Seawaters maximum BC is at a
pH of 6 & 9. For all practically purposes seawater has very little Buffering Capacity, if
any at all.


Alkalinity and Buffer Capacity are closely tied but are NOT the same thing, it is a
misunderstanding and use of the term. Do you think water chemistry books would have
separate sections on Alkalinity and Buffering Capacity if they were the same thing ?

By the way do you know who you are talking to ?

--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
www.coralrealm.com

If You See Me Running You Better Catch-Up

[Richard Reynolds]

I am sorry ahead of time I couldnt resist

> By the way do you know who you are talking to ?


DUH of course he doesnt or he wouldnt have argued :D


now ive done it the king is gona slap me around for messing with the oracle :D

--
Richard Reynolds

[Toni]

"Richard Reynolds" > wrote in message
news:0lHVb.16203$gl2.2728@lakeread05...
> I am sorry ahead of time I couldnt resist
>
> > By the way do you know who you are talking to ?
>
>
> DUH of course he doesnt or he wouldnt have argued :D
>
>


But it's fun for all the rest of us to stand back and watch....
And maybe learn something, too!


--
Toni
http://www.cearbhaill.com/reef.htm

[Dragon Slayer]

> DUH of course he doesnt or he wouldnt have argued :D

i'm glad he didnt, made for a nice laugh to see someone tell the Great
Oracle "YOUR WRONG" even if they were full of it. :)

[stoutman]

Oh brother. Where to start.

pH is the -log of the hydronium ion concentration. When the hydronium ion
concentration is very low, your system is basic (high pH). When the
hydronium ion concentration is very large, your system is acidic (low pH).

pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice versa.
But a pH of < 7 means acidic. pH > 7 means basic.
pH can tell you something about acidity and basicity. It is a measurement
of both, or the entire pH scale (1-14) if you will.

>It is called "blowing it off" , such as with an airstone. If you have high
CO2 and add an airstone it will drive the CO2 off raising the pH.

Ok, you are going to try and 'purge' (the correct term) your CO2 out with
air. Yeah, I guess that would work. If you intentionally put the CO2 in
there to begin with because you must have a higher concentration of CO2 in
your tank than in the atmosphere. I don't intentionally put CO2 in my tank.
But I know some of you reef people due in Kalk reactors.

>If Alk resists changes in pH then why does CO2 lower the pH without
affecting the Alk.

Alkalinity is buffering capacity. Your buffers begin to get weakened with
the addition of acid until they reach a point when they can no longer
'buffer' and the pH crashes.

>But I know what you mean, may use the term ALK and BC interchangeably

Do you remember writing this in an earlier post? If you believe that
alkalinity and buffering capacity can be used interchangeably than I must be
getting through to you.

>When CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
any pH no matter what the Alk or CO2 there will be an exact ratio of
CO2:HCO3:CO3

Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is your
point here?

> Go ahead and pick a seawater pH and I will tell you what that ratio is.
Tell me the pH and
> Alk and I will give the CO2 concentration. Give me the Alk and CO2 and I
will give you
> the pH. Don't forget the temperature and Salinity.

Not interested. I can find my own software to do this too.

> Alk is defined as;
>
> TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
[HPO4--] +
> 2[PO4---] - [H+]

Ahh, now we are getting somewhere. What you are showing are components of a
'BUFFER'. Which are used in the over all 'buffering capacity'. Are we
going in circles here? Anyway, I think you are learning something.

> In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
maximum BC is at a
> pH of 6 & 9. For all practically purposes seawater has very little
Buffering Capacity, if
> any at all.

This is the 'primary buffer' in sea water:

H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1

If you REALLY believe that sea water has little buffering capacity, than you
need to do some reading on your own. I wont be able to convince you.

> In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
maximum BC is at a
> pH of 6 & 9. For all practically purposes seawater has very little
Buffering Capacity, if
> any at all.

This would be true if a monoprotic acid where used in the 'buffer', but
carbonic acid (the primary buffering component in seawater) is a polyprotic
acid. It has two protons that can dissociate. Therefore, it has two pKa's
(pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35. The
pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
right in there. Is that magic? :)

Remember that seawater is more than a mixture of just carbonate and CO2,
there are other buffers involved that make it even more complicated I'm
sure.

> By the way do you know who you are talking to ?

No. Do you?




"Boomer" > wrote in message
...
> Let me make this clear you don't know what you are taking about
>
> "alkalinity is a measurement of 'buffering capacity'"
>
> No, it is the ability to neutralize an acid. BC is the ability to
withstand both upward
> and downward trends in pH.
>
> "pH is a measurement of 'acidity/basicity'.
>
> No, pH is a measurement of acidity and pOH is a measurement of Basicity,
if you want to
> get picky, which seems you do.
>
>
> "How do you remove CO2? "
>
> It is called "blowing it off" , such as with an airstone. If you have high
CO2 and add an
> airstone it will drive the CO2 off raising the pH. It can be proven with a
glass of water,
> a straw, some pH color indicator and an Alk test kit and if you must a CO2
test kit
>
> >You can have all the alk you want in the world and it won't help, in
> regards to CO2
>
> "Wrong. Alkalinity increases your tank's ability to RESIST sharp changes
in
> pH. This is what is meant by 'buffering capacity'"
>
> No you are wrong and very lost. If Alk resists changes in pH then why does
CO2 lower the
> pH without affecting the Alk ? CO2 has no effect on alk and alk has no
effect on CO2. When
> CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At any
pH no matter what
> the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
>
> .
> Go ahead and pick a seawater pH and I will tell you what that ratio is.
Tell me the pH and
> Alk and I will give the CO2 concentration. Give me the Alk and CO2 and I
will give you
> the pH. Don't forget the temperature and Salinity.
>
> Alk is defined as;
>
> TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
[HPO4--] +
> 2[PO4---] - [H+]
>
>
> Buffering Capacity is defined as;
>
> BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka + [H3O+])²
>
> In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
maximum BC is at a
> pH of 6 & 9. For all practically purposes seawater has very little
Buffering Capacity, if
> any at all.
>
>
> Alkalinity and Buffer Capacity are closely tied but are NOT the same
thing, it is a
> misunderstanding and use of the term. Do you think water chemistry books
would have
> separate sections on Alkalinity and Buffering Capacity if they were the
same thing ?
>
> By the way do you know who you are talking to ?
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
>
>

[Dragon Slayer]

Boomer when you read that, just let it go.............no need bashing heads
here, the group knows what's going on.

kc

"stoutman" <.@.> wrote in message news:SFNVb.204571$Rc4.1681932@attbi_s54...
> Oh brother. Where to start.
>
> pH is the -log of the hydronium ion concentration. When the hydronium ion
> concentration is very low, your system is basic (high pH). When the
> hydronium ion concentration is very large, your system is acidic (low pH).
>
> pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice versa.
> But a pH of < 7 means acidic. pH > 7 means basic.
> pH can tell you something about acidity and basicity. It is a measurement
> of both, or the entire pH scale (1-14) if you will.
>
> >It is called "blowing it off" , such as with an airstone. If you have
high
> CO2 and add an airstone it will drive the CO2 off raising the pH.
>
> Ok, you are going to try and 'purge' (the correct term) your CO2 out with
> air. Yeah, I guess that would work. If you intentionally put the CO2 in
> there to begin with because you must have a higher concentration of CO2 in
> your tank than in the atmosphere. I don't intentionally put CO2 in my
tank.
> But I know some of you reef people due in Kalk reactors.
>
> >If Alk resists changes in pH then why does CO2 lower the pH without
> affecting the Alk.
>
> Alkalinity is buffering capacity. Your buffers begin to get weakened with
> the addition of acid until they reach a point when they can no longer
> 'buffer' and the pH crashes.
>
> >But I know what you mean, may use the term ALK and BC interchangeably
>
> Do you remember writing this in an earlier post? If you believe that
> alkalinity and buffering capacity can be used interchangeably than I must
be
> getting through to you.
>
> >When CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
> any pH no matter what the Alk or CO2 there will be an exact ratio of
> CO2:HCO3:CO3
>
> Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
your
> point here?
>
> > Go ahead and pick a seawater pH and I will tell you what that ratio is.
> Tell me the pH and
> > Alk and I will give the CO2 concentration. Give me the Alk and CO2 and
I
> will give you
> > the pH. Don't forget the temperature and Salinity.
>
> Not interested. I can find my own software to do this too.
>
> > Alk is defined as;
> >
> > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> [HPO4--] +
> > 2[PO4---] - [H+]
>
> Ahh, now we are getting somewhere. What you are showing are components of
a
> 'BUFFER'. Which are used in the over all 'buffering capacity'. Are we
> going in circles here? Anyway, I think you are learning something.
>
> > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> maximum BC is at a
> > pH of 6 & 9. For all practically purposes seawater has very little
> Buffering Capacity, if
> > any at all.
>
> This is the 'primary buffer' in sea water:
>
> H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
>
> If you REALLY believe that sea water has little buffering capacity, than
you
> need to do some reading on your own. I wont be able to convince you.
>
> > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> maximum BC is at a
> > pH of 6 & 9. For all practically purposes seawater has very little
> Buffering Capacity, if
> > any at all.
>
> This would be true if a monoprotic acid where used in the 'buffer', but
> carbonic acid (the primary buffering component in seawater) is a
polyprotic
> acid. It has two protons that can dissociate. Therefore, it has two
pKa's
> (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
The
> pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> right in there. Is that magic? :)
>
> Remember that seawater is more than a mixture of just carbonate and CO2,
> there are other buffers involved that make it even more complicated I'm
> sure.
>
> > By the way do you know who you are talking to ?
>
> No. Do you?
>
>
>
>
> "Boomer" > wrote in message
> ...
> > Let me make this clear you don't know what you are taking about
> >
> > "alkalinity is a measurement of 'buffering capacity'"
> >
> > No, it is the ability to neutralize an acid. BC is the ability to
> withstand both upward
> > and downward trends in pH.
> >
> > "pH is a measurement of 'acidity/basicity'.
> >
> > No, pH is a measurement of acidity and pOH is a measurement of Basicity,
> if you want to
> > get picky, which seems you do.
> >
> >
> > "How do you remove CO2? "
> >
> > It is called "blowing it off" , such as with an airstone. If you have
high
> CO2 and add an
> > airstone it will drive the CO2 off raising the pH. It can be proven with
a
> glass of water,
> > a straw, some pH color indicator and an Alk test kit and if you must a
CO2
> test kit
> >
> > >You can have all the alk you want in the world and it won't help, in
> > regards to CO2
> >
> > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
changes
> in
> > pH. This is what is meant by 'buffering capacity'"
> >
> > No you are wrong and very lost. If Alk resists changes in pH then why
does
> CO2 lower the
> > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
> effect on CO2. When
> > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At any
> pH no matter what
> > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> >
> > .
> > Go ahead and pick a seawater pH and I will tell you what that ratio is.
> Tell me the pH and
> > Alk and I will give the CO2 concentration. Give me the Alk and CO2 and
I
> will give you
> > the pH. Don't forget the temperature and Salinity.
> >
> > Alk is defined as;
> >
> > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> [HPO4--] +
> > 2[PO4---] - [H+]
> >
> >
> > Buffering Capacity is defined as;
> >
> > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka + [H3O+])²
> >
> > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> maximum BC is at a
> > pH of 6 & 9. For all practically purposes seawater has very little
> Buffering Capacity, if
> > any at all.
> >
> >
> > Alkalinity and Buffer Capacity are closely tied but are NOT the same
> thing, it is a
> > misunderstanding and use of the term. Do you think water chemistry books
> would have
> > separate sections on Alkalinity and Buffering Capacity if they were the
> same thing ?
> >
> > By the way do you know who you are talking to ?
> >
> > --
> > Boomer
> >
> > Want to talk chemistry ? The Reef Chemistry Forum
> > http://www.reefcentral.com/vbulletin/index.php
> >
> > Want to See More ?
> > Please Join Our Growing Membership
> > www.coralrealm.com
> >
> > If You See Me Running You Better Catch-Up
> >
> >
>
>

[stoutman]

If you knew my credentials you would laugh at yourself.


"Dragon Slayer" > wrote in message
...
> Boomer when you read that, just let it go.............no need bashing
heads
> here, the group knows what's going on.
>
> kc
>
> "stoutman" <.@.> wrote in message
news:SFNVb.204571$Rc4.1681932@attbi_s54...
> > Oh brother. Where to start.
> >
> > pH is the -log of the hydronium ion concentration. When the hydronium
ion
> > concentration is very low, your system is basic (high pH). When the
> > hydronium ion concentration is very large, your system is acidic (low
pH).
> >
> > pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice
versa.
> > But a pH of < 7 means acidic. pH > 7 means basic.
> > pH can tell you something about acidity and basicity. It is a
measurement
> > of both, or the entire pH scale (1-14) if you will.
> >
> > >It is called "blowing it off" , such as with an airstone. If you have
> high
> > CO2 and add an airstone it will drive the CO2 off raising the pH.
> >
> > Ok, you are going to try and 'purge' (the correct term) your CO2 out
with
> > air. Yeah, I guess that would work. If you intentionally put the CO2
in
> > there to begin with because you must have a higher concentration of CO2
in
> > your tank than in the atmosphere. I don't intentionally put CO2 in my
> tank.
> > But I know some of you reef people due in Kalk reactors.
> >
> > >If Alk resists changes in pH then why does CO2 lower the pH without
> > affecting the Alk.
> >
> > Alkalinity is buffering capacity. Your buffers begin to get weakened
with
> > the addition of acid until they reach a point when they can no longer
> > 'buffer' and the pH crashes.
> >
> > >But I know what you mean, may use the term ALK and BC interchangeably
> >
> > Do you remember writing this in an earlier post? If you believe that
> > alkalinity and buffering capacity can be used interchangeably than I
must
> be
> > getting through to you.
> >
> > >When CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3.
At
> > any pH no matter what the Alk or CO2 there will be an exact ratio of
> > CO2:HCO3:CO3
> >
> > Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
> your
> > point here?
> >
> > > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> > Tell me the pH and
> > > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and
> I
> > will give you
> > > the pH. Don't forget the temperature and Salinity.
> >
> > Not interested. I can find my own software to do this too.
> >
> > > Alk is defined as;
> > >
> > > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> > [HPO4--] +
> > > 2[PO4---] - [H+]
> >
> > Ahh, now we are getting somewhere. What you are showing are components
of
> a
> > 'BUFFER'. Which are used in the over all 'buffering capacity'. Are we
> > going in circles here? Anyway, I think you are learning something.
> >
> > > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> > maximum BC is at a
> > > pH of 6 & 9. For all practically purposes seawater has very little
> > Buffering Capacity, if
> > > any at all.
> >
> > This is the 'primary buffer' in sea water:
> >
> > H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
> >
> > If you REALLY believe that sea water has little buffering capacity, than
> you
> > need to do some reading on your own. I wont be able to convince you.
> >
> > > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> > maximum BC is at a
> > > pH of 6 & 9. For all practically purposes seawater has very little
> > Buffering Capacity, if
> > > any at all.
> >
> > This would be true if a monoprotic acid where used in the 'buffer', but
> > carbonic acid (the primary buffering component in seawater) is a
> polyprotic
> > acid. It has two protons that can dissociate. Therefore, it has two
> pKa's
> > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
> The
> > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> > right in there. Is that magic? :)
> >
> > Remember that seawater is more than a mixture of just carbonate and CO2,
> > there are other buffers involved that make it even more complicated I'm
> > sure.
> >
> > > By the way do you know who you are talking to ?
> >
> > No. Do you?
> >
> >
> >
> >
> > "Boomer" > wrote in message
> > ...
> > > Let me make this clear you don't know what you are taking about
> > >
> > > "alkalinity is a measurement of 'buffering capacity'"
> > >
> > > No, it is the ability to neutralize an acid. BC is the ability to
> > withstand both upward
> > > and downward trends in pH.
> > >
> > > "pH is a measurement of 'acidity/basicity'.
> > >
> > > No, pH is a measurement of acidity and pOH is a measurement of
Basicity,
> > if you want to
> > > get picky, which seems you do.
> > >
> > >
> > > "How do you remove CO2? "
> > >
> > > It is called "blowing it off" , such as with an airstone. If you have
> high
> > CO2 and add an
> > > airstone it will drive the CO2 off raising the pH. It can be proven
with
> a
> > glass of water,
> > > a straw, some pH color indicator and an Alk test kit and if you must a
> CO2
> > test kit
> > >
> > > >You can have all the alk you want in the world and it won't help, in
> > > regards to CO2
> > >
> > > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
> changes
> > in
> > > pH. This is what is meant by 'buffering capacity'"
> > >
> > > No you are wrong and very lost. If Alk resists changes in pH then why
> does
> > CO2 lower the
> > > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
> > effect on CO2. When
> > > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
any
> > pH no matter what
> > > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> > >
> > > .
> > > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> > Tell me the pH and
> > > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and
> I
> > will give you
> > > the pH. Don't forget the temperature and Salinity.
> > >
> > > Alk is defined as;
> > >
> > > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> > [HPO4--] +
> > > 2[PO4---] - [H+]
> > >
> > >
> > > Buffering Capacity is defined as;
> > >
> > > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
[H3O+])²
> > >
> > > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> > maximum BC is at a
> > > pH of 6 & 9. For all practically purposes seawater has very little
> > Buffering Capacity, if
> > > any at all.
> > >
> > >
> > > Alkalinity and Buffer Capacity are closely tied but are NOT the same
> > thing, it is a
> > > misunderstanding and use of the term. Do you think water chemistry
books
> > would have
> > > separate sections on Alkalinity and Buffering Capacity if they were
the
> > same thing ?
> > >
> > > By the way do you know who you are talking to ?
> > >
> > > --
> > > Boomer
> > >
> > > Want to talk chemistry ? The Reef Chemistry Forum
> > > http://www.reefcentral.com/vbulletin/index.php
> > >
> > > Want to See More ?
> > > Please Join Our Growing Membership
> > > www.coralrealm.com
> > >
> > > If You See Me Running You Better Catch-Up
> > >
> > >
> >
> >
>
>

[stoutman]

Let me just ad.

At the pH of seawater, the buffering capacity of carbonate is at it's
weakest. It's strongest buffering is at a pH of 6.4 and 10.3.

There are still other buffers in seawater other than carbonate. It is a
very complicated system.




"stoutman" <.@.> wrote in message news:SFNVb.204571$Rc4.1681932@attbi_s54...
> Oh brother. Where to start.
>
> pH is the -log of the hydronium ion concentration. When the hydronium ion
> concentration is very low, your system is basic (high pH). When the
> hydronium ion concentration is very large, your system is acidic (low pH).
>
> pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice versa.
> But a pH of < 7 means acidic. pH > 7 means basic.
> pH can tell you something about acidity and basicity. It is a measurement
> of both, or the entire pH scale (1-14) if you will.
>
> >It is called "blowing it off" , such as with an airstone. If you have
high
> CO2 and add an airstone it will drive the CO2 off raising the pH.
>
> Ok, you are going to try and 'purge' (the correct term) your CO2 out with
> air. Yeah, I guess that would work. If you intentionally put the CO2 in
> there to begin with because you must have a higher concentration of CO2 in
> your tank than in the atmosphere. I don't intentionally put CO2 in my
tank.
> But I know some of you reef people due in Kalk reactors.
>
> >If Alk resists changes in pH then why does CO2 lower the pH without
> affecting the Alk.
>
> Alkalinity is buffering capacity. Your buffers begin to get weakened with
> the addition of acid until they reach a point when they can no longer
> 'buffer' and the pH crashes.
>
> >But I know what you mean, may use the term ALK and BC interchangeably
>
> Do you remember writing this in an earlier post? If you believe that
> alkalinity and buffering capacity can be used interchangeably than I must
be
> getting through to you.
>
> >When CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
> any pH no matter what the Alk or CO2 there will be an exact ratio of
> CO2:HCO3:CO3
>
> Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
your
> point here?
>
> > Go ahead and pick a seawater pH and I will tell you what that ratio is.
> Tell me the pH and
> > Alk and I will give the CO2 concentration. Give me the Alk and CO2 and
I
> will give you
> > the pH. Don't forget the temperature and Salinity.
>
> Not interested. I can find my own software to do this too.
>
> > Alk is defined as;
> >
> > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> [HPO4--] +
> > 2[PO4---] - [H+]
>
> Ahh, now we are getting somewhere. What you are showing are components of
a
> 'BUFFER'. Which are used in the over all 'buffering capacity'. Are we
> going in circles here? Anyway, I think you are learning something.
>
> > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> maximum BC is at a
> > pH of 6 & 9. For all practically purposes seawater has very little
> Buffering Capacity, if
> > any at all.
>
> This is the 'primary buffer' in sea water:
>
> H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
>
> If you REALLY believe that sea water has little buffering capacity, than
you
> need to do some reading on your own. I wont be able to convince you.
>
> > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> maximum BC is at a
> > pH of 6 & 9. For all practically purposes seawater has very little
> Buffering Capacity, if
> > any at all.
>
> This would be true if a monoprotic acid where used in the 'buffer', but
> carbonic acid (the primary buffering component in seawater) is a
polyprotic
> acid. It has two protons that can dissociate. Therefore, it has two
pKa's
> (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
The
> pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> right in there. Is that magic? :)
>
> Remember that seawater is more than a mixture of just carbonate and CO2,
> there are other buffers involved that make it even more complicated I'm
> sure.
>
> > By the way do you know who you are talking to ?
>
> No. Do you?
>
>
>
>
> "Boomer" > wrote in message
> ...
> > Let me make this clear you don't know what you are taking about
> >
> > "alkalinity is a measurement of 'buffering capacity'"
> >
> > No, it is the ability to neutralize an acid. BC is the ability to
> withstand both upward
> > and downward trends in pH.
> >
> > "pH is a measurement of 'acidity/basicity'.
> >
> > No, pH is a measurement of acidity and pOH is a measurement of Basicity,
> if you want to
> > get picky, which seems you do.
> >
> >
> > "How do you remove CO2? "
> >
> > It is called "blowing it off" , such as with an airstone. If you have
high
> CO2 and add an
> > airstone it will drive the CO2 off raising the pH. It can be proven with
a
> glass of water,
> > a straw, some pH color indicator and an Alk test kit and if you must a
CO2
> test kit
> >
> > >You can have all the alk you want in the world and it won't help, in
> > regards to CO2
> >
> > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
changes
> in
> > pH. This is what is meant by 'buffering capacity'"
> >
> > No you are wrong and very lost. If Alk resists changes in pH then why
does
> CO2 lower the
> > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
> effect on CO2. When
> > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At any
> pH no matter what
> > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> >
> > .
> > Go ahead and pick a seawater pH and I will tell you what that ratio is.
> Tell me the pH and
> > Alk and I will give the CO2 concentration. Give me the Alk and CO2 and
I
> will give you
> > the pH. Don't forget the temperature and Salinity.
> >
> > Alk is defined as;
> >
> > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> [HPO4--] +
> > 2[PO4---] - [H+]
> >
> >
> > Buffering Capacity is defined as;
> >
> > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka + [H3O+])²
> >
> > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> maximum BC is at a
> > pH of 6 & 9. For all practically purposes seawater has very little
> Buffering Capacity, if
> > any at all.
> >
> >
> > Alkalinity and Buffer Capacity are closely tied but are NOT the same
> thing, it is a
> > misunderstanding and use of the term. Do you think water chemistry books
> would have
> > separate sections on Alkalinity and Buffering Capacity if they were the
> same thing ?
> >
> > By the way do you know who you are talking to ?
> >
> > --
> > Boomer
> >
> > Want to talk chemistry ? The Reef Chemistry Forum
> > http://www.reefcentral.com/vbulletin/index.php
> >
> > Want to See More ?
> > Please Join Our Growing Membership
> > www.coralrealm.com
> >
> > If You See Me Running You Better Catch-Up
> >
> >
>
>

[Boomer]

<Alkalinity is buffering capacity. >

No it is not, they are not calculated the same. I already gave the equations please, you
seem to avoiding them. Please consult an aquatic chemistry book.

">But I know what you mean, many use the term ALK and BC interchangeably"

Yes, I most certainly do and stated it is incorrect but I know what you mean


<If you believe that
alkalinity and buffering capacity can be used interchangeably than I must be
getting through to you.>

Please don't make me laugh. No I'm not getting through


<Which are used in the over all 'buffering capacity'. Are we
going in circles here? Anyway, I think you are learning something>

No I'm not learning anything but you need to. No I'm not talking in a circle but maybe you
are. You must have missed it, so here it is again. Buffer capacity is the ability to with
stand upward & downward trends in pH. Alkalinity only deals with downward trends and says
nothing of upward trends. Ever hear of an Acidity test kit ?

<This is the 'primary buffer' in sea water:>

H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1"

You are lost, the reaction that it is inherent to is;........... and you are missing some
things

2HCO3 <--->CO2 + H20 + ***CO3***


As far as primary "buffers" in seawater you are lost again. The principle buffers of
seawater are HCO3, CO3 and
B(OH4). I might add that Ion pairs are also part of the Buffer Capacity. About 1/3 of
seawaters Buffer Capacity is due to MgCO3. Like I said you don't understand Buffer
Capacity and Alkalinity. Seawater manuals and text books are filled with this kind of
data.Would you like me to give a list of some ?? :-)

"If you REALLY believe that sea water has little buffering capacity, than you
need to do some reading on your own. I wont be able to convince you."

It doesn't if you understand the issue and it is quite clear you don't. You are the one
that need to do allllllllllllot of reading

***For terms are commonly used to describe various aspects of the seawater buffer system:

1.pH

2. Buffering Capacity

3. Alkalinity or Total Alkalinity

4. Carbonate Alkalinity***

From;
Spotte, Seawater Aquariums the Captive Environment ( a technical text book on seawater and
seawater aquariums)


***In seawater, for example, maximum Buffering Capacity appears at pH values near 6 and 9
and seawater is buffered very little , if at all, at its normal pH of 8.2***

From;
Skirrow, 1975 Chemical Oceanography Vol 2

<but
carbonic acid (the primary buffering component in seawater) >

Bicarbonate is the primary buffer not carbonic acid ,where on God's earth did you get that
from. At normal temp, salinity, pH and Alk it is;

@ 20C and 34.3 ppt salinity

CO2 = 0.52 %

HCO3 = 86.4 %

CO3 = 13.09 %

From;
Practical Handbook of Marine Science, M.J. Kennish

<Therefore, it has two pKa's
(pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35. The
pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
right in there. Is that magic? :)>

Magic !!!! it must be by your account. That is FW there pal, not seawater, lets get the
water straight here that we are dealing with, so you aren't so lost.

The;
pKa1 = 6.0

pKa2 = 9.1

From;
Introduction to Marine Chemistry by Riley and Chester. Also from, An Introduction to the
Chemistry of the Sea, by Pilson

So your equation does not work as you gave it.

(6.0 + 9.1) / 2 = 7.55 pH Hum, maybe you would care to explain that since you seem to
think you have all the answers.

<Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is your
point here?>

It means that if the pH is 8.3 and the Alk is 4.0 meq/ l or if the is pH 8.3 and the Alk
1.5 Meq /l, or no mater what the Alk level is, if the pH is the same, the ratio's of CO2
to HCO3 to CO3 will be the same. So you are not lost here :-)

pH = 8.2

Alk = 4.0 meq /l

or

pH = *.2

Alk = 1.5 meq /

The percentage or ratio is still the same for both, both will be . 0.52% CO2, 86.4 % HCO3
and 13.09 % @ 34.3 ppt and @ 20 C

<Yeah, I guess that would work. If you intentionally put the CO2 in
there to begin with because you must have a higher concentration of CO2 in
your tank than in the atmosphere. I don't intentionally put CO2 in my tank>

It does work it is not a maybe. Intentionally !!!!! where are you coming from or where
have you been ??? CO2 is produced by normal biological activity and is the resaon behind
many low pH's in tanks, as is room air CO2

<you must have a higher concentration of CO2 in
your tank than in the atmosphere>

What !!! CO2 does not have to be higher than ambient air .Quite often CO2 is produced in
the water and can't leave fast enough, has one would normally expect , by simple diffusion
to the atmosphere. It is the reason why CO2 can get so high in almost any aquatic system
and is the same reason CO2 can get so low. Why do you think Planted FW Aquarium guys use
CO2 injection ? As the plants can remove the CO2 faster than it can diffuse across the
water air interface. Same for a FOT, the CO2 can accumulate faster than it can diffuse,
thus crashing the pH

<Not interested. I can find my own software to do this too.>

Well go get some, as you need it, that is for sure.
--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
www.coralrealm.com

If You See Me Running You Better Catch-Up
"stoutman" <.@.> wrote in message news:SFNVb.204571$Rc4.1681932@attbi_s54...
: Oh brother. Where to start.
:
: pH is the -log of the hydronium ion concentration. When the hydronium ion
: concentration is very low, your system is basic (high pH). When the
: hydronium ion concentration is very large, your system is acidic (low pH).
:
: pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice versa.
: But a pH of < 7 means acidic. pH > 7 means basic.
: pH can tell you something about acidity and basicity. It is a measurement
: of both, or the entire pH scale (1-14) if you will.
:
: >It is called "blowing it off" , such as with an airstone. If you have high
: CO2 and add an airstone it will drive the CO2 off raising the pH.
:
: Ok, you are going to try and 'purge' (the correct term) your CO2 out with
: air. Yeah, I guess that would work. If you intentionally put the CO2 in
: there to begin with because you must have a higher concentration of CO2 in
: your tank than in the atmosphere. I don't intentionally put CO2 in my tank.
: But I know some of you reef people due in Kalk reactors.
:
: >If Alk resists changes in pH then why does CO2 lower the pH without
: affecting the Alk.
:
: Alkalinity is buffering capacity. Your buffers begin to get weakened with
: the addition of acid until they reach a point when they can no longer
: 'buffer' and the pH crashes.
:
: >But I know what you mean, may use the term ALK and BC interchangeably
:
: Do you remember writing this in an earlier post? If you believe that
: alkalinity and buffering capacity can be used interchangeably than I must be
: getting through to you.
:
: >When CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
: any pH no matter what the Alk or CO2 there will be an exact ratio of
: CO2:HCO3:CO3
:
: Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is your
: point here?
:
: > Go ahead and pick a seawater pH and I will tell you what that ratio is.
: Tell me the pH and
: > Alk and I will give the CO2 concentration. Give me the Alk and CO2 and I
: will give you
: > the pH. Don't forget the temperature and Salinity.
:
: Not interested. I can find my own software to do this too.
:
: > Alk is defined as;
: >
: > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
: [HPO4--] +
: > 2[PO4---] - [H+]
:
: Ahh, now we are getting somewhere. What you are showing are components of a
: 'BUFFER'. Which are used in the over all 'buffering capacity'. Are we
: going in circles here? Anyway, I think you are learning something.
:
: > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: maximum BC is at a
: > pH of 6 & 9. For all practically purposes seawater has very little
: Buffering Capacity, if
: > any at all.
:
: This is the 'primary buffer' in sea water:
:
: H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
:
: If you REALLY believe that sea water has little buffering capacity, than you
: need to do some reading on your own. I wont be able to convince you.
:
: > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: maximum BC is at a
: > pH of 6 & 9. For all practically purposes seawater has very little
: Buffering Capacity, if
: > any at all.
:
: This would be true if a monoprotic acid where used in the 'buffer', but
: carbonic acid (the primary buffering component in seawater) is a polyprotic
: acid. It has two protons that can dissociate. Therefore, it has two pKa's
: (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35. The
: pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
: right in there. Is that magic? :)
:
: Remember that seawater is more than a mixture of just carbonate and CO2,
: there are other buffers involved that make it even more complicated I'm
: sure.
:
: > By the way do you know who you are talking to ?
:
: No. Do you?
:
:
:
:
: "Boomer" > wrote in message
: ...
: > Let me make this clear you don't know what you are taking about
: >
: > "alkalinity is a measurement of 'buffering capacity'"
: >
: > No, it is the ability to neutralize an acid. BC is the ability to
: withstand both upward
: > and downward trends in pH.
: >
: > "pH is a measurement of 'acidity/basicity'.
: >
: > No, pH is a measurement of acidity and pOH is a measurement of Basicity,
: if you want to
: > get picky, which seems you do.
: >
: >
: > "How do you remove CO2? "
: >
: > It is called "blowing it off" , such as with an airstone. If you have high
: CO2 and add an
: > airstone it will drive the CO2 off raising the pH. It can be proven with a
: glass of water,
: > a straw, some pH color indicator and an Alk test kit and if you must a CO2
: test kit
: >
: > >You can have all the alk you want in the world and it won't help, in
: > regards to CO2
: >
: > "Wrong. Alkalinity increases your tank's ability to RESIST sharp changes
: in
: > pH. This is what is meant by 'buffering capacity'"
: >
: > No you are wrong and very lost. If Alk resists changes in pH then why does
: CO2 lower the
: > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
: effect on CO2. When
: > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At any
: pH no matter what
: > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
: >
: > .
: > Go ahead and pick a seawater pH and I will tell you what that ratio is.
: Tell me the pH and
: > Alk and I will give the CO2 concentration. Give me the Alk and CO2 and I
: will give you
: > the pH. Don't forget the temperature and Salinity.
: >
: > Alk is defined as;
: >
: > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
: [HPO4--] +
: > 2[PO4---] - [H+]
: >
: >
: > Buffering Capacity is defined as;
: >
: > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka + [H3O+])²
: >
: > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: maximum BC is at a
: > pH of 6 & 9. For all practically purposes seawater has very little
: Buffering Capacity, if
: > any at all.
: >
: >
: > Alkalinity and Buffer Capacity are closely tied but are NOT the same
: thing, it is a
: > misunderstanding and use of the term. Do you think water chemistry books
: would have
: > separate sections on Alkalinity and Buffering Capacity if they were the
: same thing ?
: >
: > By the way do you know who you are talking to ?
: >
: > --
: > Boomer
: >
: > Want to talk chemistry ? The Reef Chemistry Forum
: > http://www.reefcentral.com/vbulletin/index.php
: >
: > Want to See More ?
: > Please Join Our Growing Membership
: > www.coralrealm.com
: >
: > If You See Me Running You Better Catch-Up
: >
: >
:
:

[Boomer]

Sorry DS to late, before I say your post so Sorry in delay

--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
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If You See Me Running You Better Catch-Up
"Dragon Slayer" > wrote in message
...
: Boomer when you read that, just let it go.............no need bashing heads
: here, the group knows what's going on.
:
: kc
:
: "stoutman" <.@.> wrote in message news:SFNVb.204571$Rc4.1681932@attbi_s54...
: > Oh brother. Where to start.
: >
: > pH is the -log of the hydronium ion concentration. When the hydronium ion
: > concentration is very low, your system is basic (high pH). When the
: > hydronium ion concentration is very large, your system is acidic (low pH).
: >
: > pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice versa.
: > But a pH of < 7 means acidic. pH > 7 means basic.
: > pH can tell you something about acidity and basicity. It is a measurement
: > of both, or the entire pH scale (1-14) if you will.
: >
: > >It is called "blowing it off" , such as with an airstone. If you have
: high
: > CO2 and add an airstone it will drive the CO2 off raising the pH.
: >
: > Ok, you are going to try and 'purge' (the correct term) your CO2 out with
: > air. Yeah, I guess that would work. If you intentionally put the CO2 in
: > there to begin with because you must have a higher concentration of CO2 in
: > your tank than in the atmosphere. I don't intentionally put CO2 in my
: tank.
: > But I know some of you reef people due in Kalk reactors.
: >
: > >If Alk resists changes in pH then why does CO2 lower the pH without
: > affecting the Alk.
: >
: > Alkalinity is buffering capacity. Your buffers begin to get weakened with
: > the addition of acid until they reach a point when they can no longer
: > 'buffer' and the pH crashes.
: >
: > >But I know what you mean, may use the term ALK and BC interchangeably
: >
: > Do you remember writing this in an earlier post? If you believe that
: > alkalinity and buffering capacity can be used interchangeably than I must
: be
: > getting through to you.
: >
: > >When CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
: > any pH no matter what the Alk or CO2 there will be an exact ratio of
: > CO2:HCO3:CO3
: >
: > Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
: your
: > point here?
: >
: > > Go ahead and pick a seawater pH and I will tell you what that ratio is.
: > Tell me the pH and
: > > Alk and I will give the CO2 concentration. Give me the Alk and CO2 and
: I
: > will give you
: > > the pH. Don't forget the temperature and Salinity.
: >
: > Not interested. I can find my own software to do this too.
: >
: > > Alk is defined as;
: > >
: > > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
: > [HPO4--] +
: > > 2[PO4---] - [H+]
: >
: > Ahh, now we are getting somewhere. What you are showing are components of
: a
: > 'BUFFER'. Which are used in the over all 'buffering capacity'. Are we
: > going in circles here? Anyway, I think you are learning something.
: >
: > > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: > maximum BC is at a
: > > pH of 6 & 9. For all practically purposes seawater has very little
: > Buffering Capacity, if
: > > any at all.
: >
: > This is the 'primary buffer' in sea water:
: >
: > H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
: >
: > If you REALLY believe that sea water has little buffering capacity, than
: you
: > need to do some reading on your own. I wont be able to convince you.
: >
: > > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: > maximum BC is at a
: > > pH of 6 & 9. For all practically purposes seawater has very little
: > Buffering Capacity, if
: > > any at all.
: >
: > This would be true if a monoprotic acid where used in the 'buffer', but
: > carbonic acid (the primary buffering component in seawater) is a
: polyprotic
: > acid. It has two protons that can dissociate. Therefore, it has two
: pKa's
: > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
: The
: > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
: > right in there. Is that magic? :)
: >
: > Remember that seawater is more than a mixture of just carbonate and CO2,
: > there are other buffers involved that make it even more complicated I'm
: > sure.
: >
: > > By the way do you know who you are talking to ?
: >
: > No. Do you?
: >
: >
: >
: >
: > "Boomer" > wrote in message
: > ...
: > > Let me make this clear you don't know what you are taking about
: > >
: > > "alkalinity is a measurement of 'buffering capacity'"
: > >
: > > No, it is the ability to neutralize an acid. BC is the ability to
: > withstand both upward
: > > and downward trends in pH.
: > >
: > > "pH is a measurement of 'acidity/basicity'.
: > >
: > > No, pH is a measurement of acidity and pOH is a measurement of Basicity,
: > if you want to
: > > get picky, which seems you do.
: > >
: > >
: > > "How do you remove CO2? "
: > >
: > > It is called "blowing it off" , such as with an airstone. If you have
: high
: > CO2 and add an
: > > airstone it will drive the CO2 off raising the pH. It can be proven with
: a
: > glass of water,
: > > a straw, some pH color indicator and an Alk test kit and if you must a
: CO2
: > test kit
: > >
: > > >You can have all the alk you want in the world and it won't help, in
: > > regards to CO2
: > >
: > > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
: changes
: > in
: > > pH. This is what is meant by 'buffering capacity'"
: > >
: > > No you are wrong and very lost. If Alk resists changes in pH then why
: does
: > CO2 lower the
: > > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
: > effect on CO2. When
: > > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At any
: > pH no matter what
: > > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
: > >
: > > .
: > > Go ahead and pick a seawater pH and I will tell you what that ratio is.
: > Tell me the pH and
: > > Alk and I will give the CO2 concentration. Give me the Alk and CO2 and
: I
: > will give you
: > > the pH. Don't forget the temperature and Salinity.
: > >
: > > Alk is defined as;
: > >
: > > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
: > [HPO4--] +
: > > 2[PO4---] - [H+]
: > >
: > >
: > > Buffering Capacity is defined as;
: > >
: > > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka + [H3O+])²
: > >
: > > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: > maximum BC is at a
: > > pH of 6 & 9. For all practically purposes seawater has very little
: > Buffering Capacity, if
: > > any at all.
: > >
: > >
: > > Alkalinity and Buffer Capacity are closely tied but are NOT the same
: > thing, it is a
: > > misunderstanding and use of the term. Do you think water chemistry books
: > would have
: > > separate sections on Alkalinity and Buffering Capacity if they were the
: > same thing ?
: > >
: > > By the way do you know who you are talking to ?
: > >
: > > --
: > > Boomer
: > >
: > > Want to talk chemistry ? The Reef Chemistry Forum
: > > http://www.reefcentral.com/vbulletin/index.php
: > >
: > > Want to See More ?
: > > Please Join Our Growing Membership
: > > www.coralrealm.com
: > >
: > > If You See Me Running You Better Catch-Up
: > >
: > >
: >
: >
:
:

[Boomer]

I don't care about credentials, they are meaningless, it is what is the answer and the
merit of the answer, credentials or not.

--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
www.coralrealm.com

If You See Me Running You Better Catch-Up
"stoutman" <.@.> wrote in message news:YeOVb.204890$Rc4.1682472@attbi_s54...
: If you knew my credentials you would laugh at yourself.
:
:
: "Dragon Slayer" > wrote in message
: ...
: > Boomer when you read that, just let it go.............no need bashing
: heads
: > here, the group knows what's going on.
: >
: > kc
: >
: > "stoutman" <.@.> wrote in message
: news:SFNVb.204571$Rc4.1681932@attbi_s54...
: > > Oh brother. Where to start.
: > >
: > > pH is the -log of the hydronium ion concentration. When the hydronium
: ion
: > > concentration is very low, your system is basic (high pH). When the
: > > hydronium ion concentration is very large, your system is acidic (low
: pH).
: > >
: > > pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice
: versa.
: > > But a pH of < 7 means acidic. pH > 7 means basic.
: > > pH can tell you something about acidity and basicity. It is a
: measurement
: > > of both, or the entire pH scale (1-14) if you will.
: > >
: > > >It is called "blowing it off" , such as with an airstone. If you have
: > high
: > > CO2 and add an airstone it will drive the CO2 off raising the pH.
: > >
: > > Ok, you are going to try and 'purge' (the correct term) your CO2 out
: with
: > > air. Yeah, I guess that would work. If you intentionally put the CO2
: in
: > > there to begin with because you must have a higher concentration of CO2
: in
: > > your tank than in the atmosphere. I don't intentionally put CO2 in my
: > tank.
: > > But I know some of you reef people due in Kalk reactors.
: > >
: > > >If Alk resists changes in pH then why does CO2 lower the pH without
: > > affecting the Alk.
: > >
: > > Alkalinity is buffering capacity. Your buffers begin to get weakened
: with
: > > the addition of acid until they reach a point when they can no longer
: > > 'buffer' and the pH crashes.
: > >
: > > >But I know what you mean, may use the term ALK and BC interchangeably
: > >
: > > Do you remember writing this in an earlier post? If you believe that
: > > alkalinity and buffering capacity can be used interchangeably than I
: must
: > be
: > > getting through to you.
: > >
: > > >When CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3.
: At
: > > any pH no matter what the Alk or CO2 there will be an exact ratio of
: > > CO2:HCO3:CO3
: > >
: > > Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
: > your
: > > point here?
: > >
: > > > Go ahead and pick a seawater pH and I will tell you what that ratio
: is.
: > > Tell me the pH and
: > > > Alk and I will give the CO2 concentration. Give me the Alk and CO2
: and
: > I
: > > will give you
: > > > the pH. Don't forget the temperature and Salinity.
: > >
: > > Not interested. I can find my own software to do this too.
: > >
: > > > Alk is defined as;
: > > >
: > > > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
: > > [HPO4--] +
: > > > 2[PO4---] - [H+]
: > >
: > > Ahh, now we are getting somewhere. What you are showing are components
: of
: > a
: > > 'BUFFER'. Which are used in the over all 'buffering capacity'. Are we
: > > going in circles here? Anyway, I think you are learning something.
: > >
: > > > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: > > maximum BC is at a
: > > > pH of 6 & 9. For all practically purposes seawater has very little
: > > Buffering Capacity, if
: > > > any at all.
: > >
: > > This is the 'primary buffer' in sea water:
: > >
: > > H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
: > >
: > > If you REALLY believe that sea water has little buffering capacity, than
: > you
: > > need to do some reading on your own. I wont be able to convince you.
: > >
: > > > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: > > maximum BC is at a
: > > > pH of 6 & 9. For all practically purposes seawater has very little
: > > Buffering Capacity, if
: > > > any at all.
: > >
: > > This would be true if a monoprotic acid where used in the 'buffer', but
: > > carbonic acid (the primary buffering component in seawater) is a
: > polyprotic
: > > acid. It has two protons that can dissociate. Therefore, it has two
: > pKa's
: > > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
: > The
: > > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
: > > right in there. Is that magic? :)
: > >
: > > Remember that seawater is more than a mixture of just carbonate and CO2,
: > > there are other buffers involved that make it even more complicated I'm
: > > sure.
: > >
: > > > By the way do you know who you are talking to ?
: > >
: > > No. Do you?
: > >
: > >
: > >
: > >
: > > "Boomer" > wrote in message
: > > ...
: > > > Let me make this clear you don't know what you are taking about
: > > >
: > > > "alkalinity is a measurement of 'buffering capacity'"
: > > >
: > > > No, it is the ability to neutralize an acid. BC is the ability to
: > > withstand both upward
: > > > and downward trends in pH.
: > > >
: > > > "pH is a measurement of 'acidity/basicity'.
: > > >
: > > > No, pH is a measurement of acidity and pOH is a measurement of
: Basicity,
: > > if you want to
: > > > get picky, which seems you do.
: > > >
: > > >
: > > > "How do you remove CO2? "
: > > >
: > > > It is called "blowing it off" , such as with an airstone. If you have
: > high
: > > CO2 and add an
: > > > airstone it will drive the CO2 off raising the pH. It can be proven
: with
: > a
: > > glass of water,
: > > > a straw, some pH color indicator and an Alk test kit and if you must a
: > CO2
: > > test kit
: > > >
: > > > >You can have all the alk you want in the world and it won't help, in
: > > > regards to CO2
: > > >
: > > > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
: > changes
: > > in
: > > > pH. This is what is meant by 'buffering capacity'"
: > > >
: > > > No you are wrong and very lost. If Alk resists changes in pH then why
: > does
: > > CO2 lower the
: > > > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
: > > effect on CO2. When
: > > > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
: any
: > > pH no matter what
: > > > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
: > > >
: > > > .
: > > > Go ahead and pick a seawater pH and I will tell you what that ratio
: is.
: > > Tell me the pH and
: > > > Alk and I will give the CO2 concentration. Give me the Alk and CO2
: and
: > I
: > > will give you
: > > > the pH. Don't forget the temperature and Salinity.
: > > >
: > > > Alk is defined as;
: > > >
: > > > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
: > > [HPO4--] +
: > > > 2[PO4---] - [H+]
: > > >
: > > >
: > > > Buffering Capacity is defined as;
: > > >
: > > > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
: [H3O+])²
: > > >
: > > > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: > > maximum BC is at a
: > > > pH of 6 & 9. For all practically purposes seawater has very little
: > > Buffering Capacity, if
: > > > any at all.
: > > >
: > > >
: > > > Alkalinity and Buffer Capacity are closely tied but are NOT the same
: > > thing, it is a
: > > > misunderstanding and use of the term. Do you think water chemistry
: books
: > > would have
: > > > separate sections on Alkalinity and Buffering Capacity if they were
: the
: > > same thing ?
: > > >
: > > > By the way do you know who you are talking to ?
: > > >
: > > > --
: > > > Boomer
: > > >
: > > > Want to talk chemistry ? The Reef Chemistry Forum
: > > > http://www.reefcentral.com/vbulletin/index.php
: > > >
: > > > Want to See More ?
: > > > Please Join Our Growing Membership
: > > > www.coralrealm.com
: > > >
: > > > If You See Me Running You Better Catch-Up
: > > >
: > > >
: > >
: > >
: >
: >
:
:

[stoutman]

>Alkalinity only deals with downward trends and says nothing of upward
trends. Ever hear of an Acidity test kit ?

Downwards trends of what? Acidity? Basicity? Have I ever heard of an
acidity test? Yeah, it's called pH paper. or a pH meter.

> As far as primary "buffers" in seawater you are lost again. The principle
buffers of seawater are HCO3, CO3.

Ever heard of the Henderson-Hasselbach equation?

pH = pKa + log [HA]/[A-]

The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this example)
you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium will
be shifted to HCO3-2 by a ratio of 1:100.

8.3 = 10.3 + log [HCO3-2]/[CO3-2]
-2 = log [HCO3-2]/[CO3-2]

take antilog of both sides and you get:

..01 = [HCO3-2]/[CO3-2]

Therefore, at a pH of 8.3 (seawater for this example) the majority of
carbonate in solution exists as HCO3-2 not CO3-2. That is why I did not
include it in my buffer example.

You said:
>The principle buffers of seawater are HCO3, CO3 and B(OH4).

and You said in a previous post:

>For all practically purposes seawater has very little Buffering Capacity,
if any at all.

STOP contradicting yourself, you are confusing the matter for yourself and
others. How can HCO3, CO3 and B(OH4) be buffers in seawater if "For all
practically purposes seawater has very little Buffering Capacity" AND if
"About 1/3 of seawaters Buffer Capacity is due to MgCO3" ?????

You are saying seawater has no buffering capacity and you are saying 1/3 of
seawaters Buffer Capacity is due to MgCO3 ??

Are you on drugs? Just kidding. I just want to help you understand.

Can I make a suggestion for you? Stop getting your chemistry knowledge from
aquarium books. Most are written by Marine Biologists, not CHEMISTS, like
myself. I have seen NUMEROUS chemistry flaws in aquarium books. This is
why this topic so muddied.

> It does work it is not a maybe. Intentionally !!!!! where are you coming
from or where
> have you been ??? CO2 is produced by normal biological activity and is the
reason behind
> many low pH's in tanks, as is room air CO2

Oh, man. Interesting. Here is another contradiction of yours. You said
before you purge CO2 from your tank with air to raise the pH. Here you are
telling me that CO2 from air is the reason behind many low pH's.


> pKa1 = 6.0 pKa2 = 9.1
> From Introduction to Marine Chemistry by Riley and Chester. Also from, An
Introduction to the Chemistry of the Sea, by Pilson

STOP GETTING YOUR CHEMISTRY FROM AQUARIUM BOOKS. Get a CHEMISTRY book.

> Well go get some, as you need it, that is for sure.

Not likely.







"Boomer" > wrote in message
...
> <Alkalinity is buffering capacity. >
>
> No it is not, they are not calculated the same. I already gave the
equations please, you
> seem to avoiding them. Please consult an aquatic chemistry book.
>
> ">But I know what you mean, many use the term ALK and BC interchangeably"
>
> Yes, I most certainly do and stated it is incorrect but I know what you
mean
>
>
> <If you believe that
> alkalinity and buffering capacity can be used interchangeably than I must
be
> getting through to you.>
>
> Please don't make me laugh. No I'm not getting through
>
>
> <Which are used in the over all 'buffering capacity'. Are we
> going in circles here? Anyway, I think you are learning something>
>
> No I'm not learning anything but you need to. No I'm not talking in a
circle but maybe you
> are. You must have missed it, so here it is again. Buffer capacity is the
ability to with
> stand upward & downward trends in pH. Alkalinity only deals with downward
trends and says
> nothing of upward trends. Ever hear of an Acidity test kit ?
>
> <This is the 'primary buffer' in sea water:>
>
> H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1"
>
> You are lost, the reaction that it is inherent to is;........... and you
are missing some
> things
>
> 2HCO3 <--->CO2 + H20 + ***CO3***
>
>
> As far as primary "buffers" in seawater you are lost again. The principle
buffers of
> seawater are HCO3, CO3 and
> B(OH4). I might add that Ion pairs are also part of the Buffer Capacity.
About 1/3 of
> seawaters Buffer Capacity is due to MgCO3. Like I said you don't
understand Buffer
> Capacity and Alkalinity. Seawater manuals and text books are filled with
this kind of
> data.Would you like me to give a list of some ?? :-)
>
> "If you REALLY believe that sea water has little buffering capacity, than
you
> need to do some reading on your own. I wont be able to convince you."
>
> It doesn't if you understand the issue and it is quite clear you don't.
You are the one
> that need to do allllllllllllot of reading
>
> ***For terms are commonly used to describe various aspects of the seawater
buffer system:
>
> 1.pH
>
> 2. Buffering Capacity
>
> 3. Alkalinity or Total Alkalinity
>
> 4. Carbonate Alkalinity***
>
> From;
> Spotte, Seawater Aquariums the Captive Environment ( a technical text book
on seawater and
> seawater aquariums)
>
>
> ***In seawater, for example, maximum Buffering Capacity appears at pH
values near 6 and 9
> and seawater is buffered very little , if at all, at its normal pH of
8.2***
>
> From;
> Skirrow, 1975 Chemical Oceanography Vol 2
>
> <but
> carbonic acid (the primary buffering component in seawater) >
>
> Bicarbonate is the primary buffer not carbonic acid ,where on God's earth
did you get that
> from. At normal temp, salinity, pH and Alk it is;
>
> @ 20C and 34.3 ppt salinity
>
> CO2 = 0.52 %
>
> HCO3 = 86.4 %
>
> CO3 = 13.09 %
>
> From;
> Practical Handbook of Marine Science, M.J. Kennish
>
> <Therefore, it has two pKa's
> (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
The
> pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> right in there. Is that magic? :)>
>
> Magic !!!! it must be by your account. That is FW there pal, not
seawater, lets get the
> water straight here that we are dealing with, so you aren't so lost.
>
> The;
> pKa1 = 6.0
>
> pKa2 = 9.1
>
> From;
> Introduction to Marine Chemistry by Riley and Chester. Also from, An
Introduction to the
> Chemistry of the Sea, by Pilson
>
> So your equation does not work as you gave it.
>
> (6.0 + 9.1) / 2 = 7.55 pH Hum, maybe you would care to explain that
since you seem to
> think you have all the answers.
>
> <Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
your
> point here?>
>
> It means that if the pH is 8.3 and the Alk is 4.0 meq/ l or if the is pH
8.3 and the Alk
> 1.5 Meq /l, or no mater what the Alk level is, if the pH is the same, the
ratio's of CO2
> to HCO3 to CO3 will be the same. So you are not lost here :-)
>
> pH = 8.2
>
> Alk = 4.0 meq /l
>
> or
>
> pH = *.2
>
> Alk = 1.5 meq /
>
> The percentage or ratio is still the same for both, both will be . 0.52%
CO2, 86.4 % HCO3
> and 13.09 % @ 34.3 ppt and @ 20 C
>
> <Yeah, I guess that would work. If you intentionally put the CO2 in
> there to begin with because you must have a higher concentration of CO2 in
> your tank than in the atmosphere. I don't intentionally put CO2 in my
tank>
>
> It does work it is not a maybe. Intentionally !!!!! where are you coming
from or where
> have you been ??? CO2 is produced by normal biological activity and is the
resaon behind
> many low pH's in tanks, as is room air CO2
>
> <you must have a higher concentration of CO2 in
> your tank than in the atmosphere>
>
> What !!! CO2 does not have to be higher than ambient air .Quite often CO2
is produced in
> the water and can't leave fast enough, has one would normally expect , by
simple diffusion
> to the atmosphere. It is the reason why CO2 can get so high in almost any
aquatic system
> and is the same reason CO2 can get so low. Why do you think Planted FW
Aquarium guys use
> CO2 injection ? As the plants can remove the CO2 faster than it can
diffuse across the
> water air interface. Same for a FOT, the CO2 can accumulate faster than it
can diffuse,
> thus crashing the pH
>
> <Not interested. I can find my own software to do this too.>
>
> Well go get some, as you need it, that is for sure.
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message
news:SFNVb.204571$Rc4.1681932@attbi_s54...
> : Oh brother. Where to start.
> :
> : pH is the -log of the hydronium ion concentration. When the hydronium
ion
> : concentration is very low, your system is basic (high pH). When the
> : hydronium ion concentration is very large, your system is acidic (low
pH).
> :
> : pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice
versa.
> : But a pH of < 7 means acidic. pH > 7 means basic.
> : pH can tell you something about acidity and basicity. It is a
measurement
> : of both, or the entire pH scale (1-14) if you will.
> :
> : >It is called "blowing it off" , such as with an airstone. If you have
high
> : CO2 and add an airstone it will drive the CO2 off raising the pH.
> :
> : Ok, you are going to try and 'purge' (the correct term) your CO2 out
with
> : air. Yeah, I guess that would work. If you intentionally put the CO2
in
> : there to begin with because you must have a higher concentration of CO2
in
> : your tank than in the atmosphere. I don't intentionally put CO2 in my
tank.
> : But I know some of you reef people due in Kalk reactors.
> :
> : >If Alk resists changes in pH then why does CO2 lower the pH without
> : affecting the Alk.
> :
> : Alkalinity is buffering capacity. Your buffers begin to get weakened
with
> : the addition of acid until they reach a point when they can no longer
> : 'buffer' and the pH crashes.
> :
> : >But I know what you mean, may use the term ALK and BC interchangeably
> :
> : Do you remember writing this in an earlier post? If you believe that
> : alkalinity and buffering capacity can be used interchangeably than I
must be
> : getting through to you.
> :
> : >When CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3.
At
> : any pH no matter what the Alk or CO2 there will be an exact ratio of
> : CO2:HCO3:CO3
> :
> : Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
your
> : point here?
> :
> : > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> : Tell me the pH and
> : > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and I
> : will give you
> : > the pH. Don't forget the temperature and Salinity.
> :
> : Not interested. I can find my own software to do this too.
> :
> : > Alk is defined as;
> : >
> : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> : [HPO4--] +
> : > 2[PO4---] - [H+]
> :
> : Ahh, now we are getting somewhere. What you are showing are components
of a
> : 'BUFFER'. Which are used in the over all 'buffering capacity'. Are we
> : going in circles here? Anyway, I think you are learning something.
> :
> : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> : maximum BC is at a
> : > pH of 6 & 9. For all practically purposes seawater has very little
> : Buffering Capacity, if
> : > any at all.
> :
> : This is the 'primary buffer' in sea water:
> :
> : H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
> :
> : If you REALLY believe that sea water has little buffering capacity, than
you
> : need to do some reading on your own. I wont be able to convince you.
> :
> : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> : maximum BC is at a
> : > pH of 6 & 9. For all practically purposes seawater has very little
> : Buffering Capacity, if
> : > any at all.
> :
> : This would be true if a monoprotic acid where used in the 'buffer', but
> : carbonic acid (the primary buffering component in seawater) is a
polyprotic
> : acid. It has two protons that can dissociate. Therefore, it has two
pKa's
> : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
The
> : pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> : right in there. Is that magic? :)
> :
> : Remember that seawater is more than a mixture of just carbonate and CO2,
> : there are other buffers involved that make it even more complicated I'm
> : sure.
> :
> : > By the way do you know who you are talking to ?
> :
> : No. Do you?
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > Let me make this clear you don't know what you are taking about
> : >
> : > "alkalinity is a measurement of 'buffering capacity'"
> : >
> : > No, it is the ability to neutralize an acid. BC is the ability to
> : withstand both upward
> : > and downward trends in pH.
> : >
> : > "pH is a measurement of 'acidity/basicity'.
> : >
> : > No, pH is a measurement of acidity and pOH is a measurement of
Basicity,
> : if you want to
> : > get picky, which seems you do.
> : >
> : >
> : > "How do you remove CO2? "
> : >
> : > It is called "blowing it off" , such as with an airstone. If you have
high
> : CO2 and add an
> : > airstone it will drive the CO2 off raising the pH. It can be proven
with a
> : glass of water,
> : > a straw, some pH color indicator and an Alk test kit and if you must a
CO2
> : test kit
> : >
> : > >You can have all the alk you want in the world and it won't help, in
> : > regards to CO2
> : >
> : > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
changes
> : in
> : > pH. This is what is meant by 'buffering capacity'"
> : >
> : > No you are wrong and very lost. If Alk resists changes in pH then why
does
> : CO2 lower the
> : > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
> : effect on CO2. When
> : > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
any
> : pH no matter what
> : > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> : >
> : > .
> : > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> : Tell me the pH and
> : > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and I
> : will give you
> : > the pH. Don't forget the temperature and Salinity.
> : >
> : > Alk is defined as;
> : >
> : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> : [HPO4--] +
> : > 2[PO4---] - [H+]
> : >
> : >
> : > Buffering Capacity is defined as;
> : >
> : > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
[H3O+])²
> : >
> : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> : maximum BC is at a
> : > pH of 6 & 9. For all practically purposes seawater has very little
> : Buffering Capacity, if
> : > any at all.
> : >
> : >
> : > Alkalinity and Buffer Capacity are closely tied but are NOT the same
> : thing, it is a
> : > misunderstanding and use of the term. Do you think water chemistry
books
> : would have
> : > separate sections on Alkalinity and Buffering Capacity if they were
the
> : same thing ?
> : >
> : > By the way do you know who you are talking to ?
> : >
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : >
> : >
> :
> :
>
>

[stoutman]

>Alkalinity only deals with downward trends and says nothing of upward
trends. Ever hear of an Acidity test kit ?

Downwards trends of what? Acidity? Basicity? Have I ever heard of an
acidity test? Yeah, it's called pH paper. or a pH meter.

> As far as primary "buffers" in seawater you are lost again. The principle
buffers of seawater are HCO3, CO3.

Ever heard of the Henderson-Hasselbach equation?

pH = pKa + log [A-]/[HA]

The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this example)
you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium will
be shifted to HCO3-2 by a ratio of 1:100.

8.3 = 10.3 + log [HCO3-2]/[CO3-2]
-2 = log [HCO3-2]/[CO3-2]

take antilog of both sides and you get:

..01 = [HCO3-2]/[CO3-2]

Therefore, at a pH of 8.3 (seawater for this example) the majority of
carbonate in solution exists as HCO3-2 not CO3-2. That is why I did not
include it in my buffer example.

You said:
>The principle buffers of seawater are HCO3, CO3 and B(OH4).

and You said in a previous post:

>For all practically purposes seawater has very little Buffering Capacity,
if any at all.

STOP contradicting yourself, you are confusing the matter for yourself and
others. How can HCO3, CO3 and B(OH4) be buffers in seawater if "For all
practically purposes seawater has very little Buffering Capacity" AND if
"About 1/3 of seawaters Buffer Capacity is due to MgCO3" ?????

You are saying seawater has no buffering capacity and you are saying 1/3 of
seawaters Buffer Capacity is due to MgCO3 ??

Are you on drugs? Just kidding. I just want to help you understand.

Can I make a suggestion for you? Stop getting your chemistry knowledge from
aquarium books. Most are written by Marine Biologists, not CHEMISTS, like
myself. I have seen NUMEROUS chemistry flaws in aquarium books. This is
why this topic so muddied.

> It does work it is not a maybe. Intentionally !!!!! where are you coming
from or where
> have you been ??? CO2 is produced by normal biological activity and is the
reason behind
> many low pH's in tanks, as is room air CO2

Oh, man. Interesting. Here is another contradiction of yours. You said
before you purge CO2 from your tank with air to raise the pH. Here you are
telling me that CO2 from air is the reason behind many low pH's.


> pKa1 = 6.0 pKa2 = 9.1
> From Introduction to Marine Chemistry by Riley and Chester. Also from, An
Introduction to the Chemistry of the Sea, by Pilson

STOP GETTING YOUR CHEMISTRY FROM AQUARIUM BOOKS. Get a CHEMISTRY book.

> Well go get some, as you need it, that is for sure.

Not likely.










"Boomer" > wrote in message
...
> <Alkalinity is buffering capacity. >
>
> No it is not, they are not calculated the same. I already gave the
equations please, you
> seem to avoiding them. Please consult an aquatic chemistry book.
>
> ">But I know what you mean, many use the term ALK and BC interchangeably"
>
> Yes, I most certainly do and stated it is incorrect but I know what you
mean
>
>
> <If you believe that
> alkalinity and buffering capacity can be used interchangeably than I must
be
> getting through to you.>
>
> Please don't make me laugh. No I'm not getting through
>
>
> <Which are used in the over all 'buffering capacity'. Are we
> going in circles here? Anyway, I think you are learning something>
>
> No I'm not learning anything but you need to. No I'm not talking in a
circle but maybe you
> are. You must have missed it, so here it is again. Buffer capacity is the
ability to with
> stand upward & downward trends in pH. Alkalinity only deals with downward
trends and says
> nothing of upward trends. Ever hear of an Acidity test kit ?
>
> <This is the 'primary buffer' in sea water:>
>
> H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1"
>
> You are lost, the reaction that it is inherent to is;........... and you
are missing some
> things
>
> 2HCO3 <--->CO2 + H20 + ***CO3***
>
>
> As far as primary "buffers" in seawater you are lost again. The principle
buffers of
> seawater are HCO3, CO3 and
> B(OH4). I might add that Ion pairs are also part of the Buffer Capacity.
About 1/3 of
> seawaters Buffer Capacity is due to MgCO3. Like I said you don't
understand Buffer
> Capacity and Alkalinity. Seawater manuals and text books are filled with
this kind of
> data.Would you like me to give a list of some ?? :-)
>
> "If you REALLY believe that sea water has little buffering capacity, than
you
> need to do some reading on your own. I wont be able to convince you."
>
> It doesn't if you understand the issue and it is quite clear you don't.
You are the one
> that need to do allllllllllllot of reading
>
> ***For terms are commonly used to describe various aspects of the seawater
buffer system:
>
> 1.pH
>
> 2. Buffering Capacity
>
> 3. Alkalinity or Total Alkalinity
>
> 4. Carbonate Alkalinity***
>
> From;
> Spotte, Seawater Aquariums the Captive Environment ( a technical text book
on seawater and
> seawater aquariums)
>
>
> ***In seawater, for example, maximum Buffering Capacity appears at pH
values near 6 and 9
> and seawater is buffered very little , if at all, at its normal pH of
8.2***
>
> From;
> Skirrow, 1975 Chemical Oceanography Vol 2
>
> <but
> carbonic acid (the primary buffering component in seawater) >
>
> Bicarbonate is the primary buffer not carbonic acid ,where on God's earth
did you get that
> from. At normal temp, salinity, pH and Alk it is;
>
> @ 20C and 34.3 ppt salinity
>
> CO2 = 0.52 %
>
> HCO3 = 86.4 %
>
> CO3 = 13.09 %
>
> From;
> Practical Handbook of Marine Science, M.J. Kennish
>
> <Therefore, it has two pKa's
> (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
The
> pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> right in there. Is that magic? :)>
>
> Magic !!!! it must be by your account. That is FW there pal, not
seawater, lets get the
> water straight here that we are dealing with, so you aren't so lost.
>
> The;
> pKa1 = 6.0
>
> pKa2 = 9.1
>
> From;
> Introduction to Marine Chemistry by Riley and Chester. Also from, An
Introduction to the
> Chemistry of the Sea, by Pilson
>
> So your equation does not work as you gave it.
>
> (6.0 + 9.1) / 2 = 7.55 pH Hum, maybe you would care to explain that
since you seem to
> think you have all the answers.
>
> <Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
your
> point here?>
>
> It means that if the pH is 8.3 and the Alk is 4.0 meq/ l or if the is pH
8.3 and the Alk
> 1.5 Meq /l, or no mater what the Alk level is, if the pH is the same, the
ratio's of CO2
> to HCO3 to CO3 will be the same. So you are not lost here :-)
>
> pH = 8.2
>
> Alk = 4.0 meq /l
>
> or
>
> pH = *.2
>
> Alk = 1.5 meq /
>
> The percentage or ratio is still the same for both, both will be . 0.52%
CO2, 86.4 % HCO3
> and 13.09 % @ 34.3 ppt and @ 20 C
>
> <Yeah, I guess that would work. If you intentionally put the CO2 in
> there to begin with because you must have a higher concentration of CO2 in
> your tank than in the atmosphere. I don't intentionally put CO2 in my
tank>
>
> It does work it is not a maybe. Intentionally !!!!! where are you coming
from or where
> have you been ??? CO2 is produced by normal biological activity and is the
resaon behind
> many low pH's in tanks, as is room air CO2
>
> <you must have a higher concentration of CO2 in
> your tank than in the atmosphere>
>
> What !!! CO2 does not have to be higher than ambient air .Quite often CO2
is produced in
> the water and can't leave fast enough, has one would normally expect , by
simple diffusion
> to the atmosphere. It is the reason why CO2 can get so high in almost any
aquatic system
> and is the same reason CO2 can get so low. Why do you think Planted FW
Aquarium guys use
> CO2 injection ? As the plants can remove the CO2 faster than it can
diffuse across the
> water air interface. Same for a FOT, the CO2 can accumulate faster than it
can diffuse,
> thus crashing the pH
>
> <Not interested. I can find my own software to do this too.>
>
> Well go get some, as you need it, that is for sure.
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message
news:SFNVb.204571$Rc4.1681932@attbi_s54...
> : Oh brother. Where to start.
> :
> : pH is the -log of the hydronium ion concentration. When the hydronium
ion
> : concentration is very low, your system is basic (high pH). When the
> : hydronium ion concentration is very large, your system is acidic (low
pH).
> :
> : pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice
versa.
> : But a pH of < 7 means acidic. pH > 7 means basic.
> : pH can tell you something about acidity and basicity. It is a
measurement
> : of both, or the entire pH scale (1-14) if you will.
> :
> : >It is called "blowing it off" , such as with an airstone. If you have
high
> : CO2 and add an airstone it will drive the CO2 off raising the pH.
> :
> : Ok, you are going to try and 'purge' (the correct term) your CO2 out
with
> : air. Yeah, I guess that would work. If you intentionally put the CO2
in
> : there to begin with because you must have a higher concentration of CO2
in
> : your tank than in the atmosphere. I don't intentionally put CO2 in my
tank.
> : But I know some of you reef people due in Kalk reactors.
> :
> : >If Alk resists changes in pH then why does CO2 lower the pH without
> : affecting the Alk.
> :
> : Alkalinity is buffering capacity. Your buffers begin to get weakened
with
> : the addition of acid until they reach a point when they can no longer
> : 'buffer' and the pH crashes.
> :
> : >But I know what you mean, may use the term ALK and BC interchangeably
> :
> : Do you remember writing this in an earlier post? If you believe that
> : alkalinity and buffering capacity can be used interchangeably than I
must be
> : getting through to you.
> :
> : >When CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3.
At
> : any pH no matter what the Alk or CO2 there will be an exact ratio of
> : CO2:HCO3:CO3
> :
> : Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
your
> : point here?
> :
> : > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> : Tell me the pH and
> : > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and I
> : will give you
> : > the pH. Don't forget the temperature and Salinity.
> :
> : Not interested. I can find my own software to do this too.
> :
> : > Alk is defined as;
> : >
> : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> : [HPO4--] +
> : > 2[PO4---] - [H+]
> :
> : Ahh, now we are getting somewhere. What you are showing are components
of a
> : 'BUFFER'. Which are used in the over all 'buffering capacity'. Are we
> : going in circles here? Anyway, I think you are learning something.
> :
> : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> : maximum BC is at a
> : > pH of 6 & 9. For all practically purposes seawater has very little
> : Buffering Capacity, if
> : > any at all.
> :
> : This is the 'primary buffer' in sea water:
> :
> : H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
> :
> : If you REALLY believe that sea water has little buffering capacity, than
you
> : need to do some reading on your own. I wont be able to convince you.
> :
> : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> : maximum BC is at a
> : > pH of 6 & 9. For all practically purposes seawater has very little
> : Buffering Capacity, if
> : > any at all.
> :
> : This would be true if a monoprotic acid where used in the 'buffer', but
> : carbonic acid (the primary buffering component in seawater) is a
polyprotic
> : acid. It has two protons that can dissociate. Therefore, it has two
pKa's
> : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
The
> : pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> : right in there. Is that magic? :)
> :
> : Remember that seawater is more than a mixture of just carbonate and CO2,
> : there are other buffers involved that make it even more complicated I'm
> : sure.
> :
> : > By the way do you know who you are talking to ?
> :
> : No. Do you?
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > Let me make this clear you don't know what you are taking about
> : >
> : > "alkalinity is a measurement of 'buffering capacity'"
> : >
> : > No, it is the ability to neutralize an acid. BC is the ability to
> : withstand both upward
> : > and downward trends in pH.
> : >
> : > "pH is a measurement of 'acidity/basicity'.
> : >
> : > No, pH is a measurement of acidity and pOH is a measurement of
Basicity,
> : if you want to
> : > get picky, which seems you do.
> : >
> : >
> : > "How do you remove CO2? "
> : >
> : > It is called "blowing it off" , such as with an airstone. If you have
high
> : CO2 and add an
> : > airstone it will drive the CO2 off raising the pH. It can be proven
with a
> : glass of water,
> : > a straw, some pH color indicator and an Alk test kit and if you must a
CO2
> : test kit
> : >
> : > >You can have all the alk you want in the world and it won't help, in
> : > regards to CO2
> : >
> : > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
changes
> : in
> : > pH. This is what is meant by 'buffering capacity'"
> : >
> : > No you are wrong and very lost. If Alk resists changes in pH then why
does
> : CO2 lower the
> : > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
> : effect on CO2. When
> : > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
any
> : pH no matter what
> : > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> : >
> : > .
> : > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> : Tell me the pH and
> : > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and I
> : will give you
> : > the pH. Don't forget the temperature and Salinity.
> : >
> : > Alk is defined as;
> : >
> : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> : [HPO4--] +
> : > 2[PO4---] - [H+]
> : >
> : >
> : > Buffering Capacity is defined as;
> : >
> : > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
[H3O+])²
> : >
> : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> : maximum BC is at a
> : > pH of 6 & 9. For all practically purposes seawater has very little
> : Buffering Capacity, if
> : > any at all.
> : >
> : >
> : > Alkalinity and Buffer Capacity are closely tied but are NOT the same
> : thing, it is a
> : > misunderstanding and use of the term. Do you think water chemistry
books
> : would have
> : > separate sections on Alkalinity and Buffering Capacity if they were
the
> : same thing ?
> : >
> : > By the way do you know who you are talking to ?
> : >
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : >
> : >
> :
> :
>
>

[stoutman]

I screwed up my math the first and second time I posted this and tried to
cancel them, so here it is again.

>Alkalinity only deals with downward trends and says nothing of upward
trends. Ever hear of an Acidity test kit ?

Downwards trends of what? Acidity? Basicity? Have I ever heard of an
acidity test? Yeah, it's called pH paper. or a pH meter.

> As far as primary "buffers" in seawater you are lost again. The principle
buffers of seawater are HCO3, CO3.

Ever heard of the Henderson-Hasselbach equation?

pH = pKa + log [A-]/[HA]

The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this example)
you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium will
be shifted to HCO3-2 by a ratio of 1:100.

8.3 = 10.3 + log [CO3-2]/[HCO3-2]
-2 = log [CO3-2]/[HCO3-2]

take antilog of both sides and you get:

..01 = [CO3-2]/[HCO3-2]

Therefore, at a pH of 8.3 (seawater for this example) the majority of
carbonate in solution exists as HCO3-2 not CO3-2. That is why I did not
include it in my buffer example.

You said:
>The principle buffers of seawater are HCO3, CO3 and B(OH4).

and You said in a previous post:

>For all practically purposes seawater has very little Buffering Capacity,
if any at all.

STOP contradicting yourself, you are confusing the matter for yourself and
others. How can HCO3, CO3 and B(OH4) be buffers in seawater if "For all
practically purposes seawater has very little Buffering Capacity" AND if
"About 1/3 of seawaters Buffer Capacity is due to MgCO3" ?????

You are saying seawater has no buffering capacity and you are saying 1/3 of
seawaters Buffer Capacity is due to MgCO3 ??

Are you on drugs? Just kidding. I just want to help you understand.

Can I make a suggestion for you? Stop getting your chemistry knowledge from
aquarium books. Most are written by Marine Biologists, not CHEMISTS, like
myself. I have seen NUMEROUS chemistry flaws in aquarium books. This is
why this topic so muddied.

> It does work it is not a maybe. Intentionally !!!!! where are you coming
from or where
> have you been ??? CO2 is produced by normal biological activity and is the
reason behind
> many low pH's in tanks, as is room air CO2

Oh, man. Interesting. Here is another contradiction of yours. You said
before you purge CO2 from your tank with air to raise the pH. Here you are
telling me that CO2 from air is the reason behind many low pH's.


> pKa1 = 6.0 pKa2 = 9.1
> From Introduction to Marine Chemistry by Riley and Chester. Also from, An
Introduction to the Chemistry of the Sea, by Pilson

STOP GETTING YOUR CHEMISTRY FROM AQUARIUM BOOKS. Get a CHEMISTRY book.

> Well go get some, as you need it, that is for sure.

Not likely.










"Boomer" > wrote in message
...
> <Alkalinity is buffering capacity. >
>
> No it is not, they are not calculated the same. I already gave the
equations please, you
> seem to avoiding them. Please consult an aquatic chemistry book.
>
> ">But I know what you mean, many use the term ALK and BC interchangeably"
>
> Yes, I most certainly do and stated it is incorrect but I know what you
mean
>
>
> <If you believe that
> alkalinity and buffering capacity can be used interchangeably than I must
be
> getting through to you.>
>
> Please don't make me laugh. No I'm not getting through
>
>
> <Which are used in the over all 'buffering capacity'. Are we
> going in circles here? Anyway, I think you are learning something>
>
> No I'm not learning anything but you need to. No I'm not talking in a
circle but maybe you
> are. You must have missed it, so here it is again. Buffer capacity is the
ability to with
> stand upward & downward trends in pH. Alkalinity only deals with downward
trends and says
> nothing of upward trends. Ever hear of an Acidity test kit ?
>
> <This is the 'primary buffer' in sea water:>
>
> H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1"
>
> You are lost, the reaction that it is inherent to is;........... and you
are missing some
> things
>
> 2HCO3 <--->CO2 + H20 + ***CO3***
>
>
> As far as primary "buffers" in seawater you are lost again. The principle
buffers of
> seawater are HCO3, CO3 and
> B(OH4). I might add that Ion pairs are also part of the Buffer Capacity.
About 1/3 of
> seawaters Buffer Capacity is due to MgCO3. Like I said you don't
understand Buffer
> Capacity and Alkalinity. Seawater manuals and text books are filled with
this kind of
> data.Would you like me to give a list of some ?? :-)
>
> "If you REALLY believe that sea water has little buffering capacity, than
you
> need to do some reading on your own. I wont be able to convince you."
>
> It doesn't if you understand the issue and it is quite clear you don't.
You are the one
> that need to do allllllllllllot of reading
>
> ***For terms are commonly used to describe various aspects of the seawater
buffer system:
>
> 1.pH
>
> 2. Buffering Capacity
>
> 3. Alkalinity or Total Alkalinity
>
> 4. Carbonate Alkalinity***
>
> From;
> Spotte, Seawater Aquariums the Captive Environment ( a technical text book
on seawater and
> seawater aquariums)
>
>
> ***In seawater, for example, maximum Buffering Capacity appears at pH
values near 6 and 9
> and seawater is buffered very little , if at all, at its normal pH of
8.2***
>
> From;
> Skirrow, 1975 Chemical Oceanography Vol 2
>
> <but
> carbonic acid (the primary buffering component in seawater) >
>
> Bicarbonate is the primary buffer not carbonic acid ,where on God's earth
did you get that
> from. At normal temp, salinity, pH and Alk it is;
>
> @ 20C and 34.3 ppt salinity
>
> CO2 = 0.52 %
>
> HCO3 = 86.4 %
>
> CO3 = 13.09 %
>
> From;
> Practical Handbook of Marine Science, M.J. Kennish
>
> <Therefore, it has two pKa's
> (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
The
> pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> right in there. Is that magic? :)>
>
> Magic !!!! it must be by your account. That is FW there pal, not
seawater, lets get the
> water straight here that we are dealing with, so you aren't so lost.
>
> The;
> pKa1 = 6.0
>
> pKa2 = 9.1
>
> From;
> Introduction to Marine Chemistry by Riley and Chester. Also from, An
Introduction to the
> Chemistry of the Sea, by Pilson
>
> So your equation does not work as you gave it.
>
> (6.0 + 9.1) / 2 = 7.55 pH Hum, maybe you would care to explain that
since you seem to
> think you have all the answers.
>
> <Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
your
> point here?>
>
> It means that if the pH is 8.3 and the Alk is 4.0 meq/ l or if the is pH
8.3 and the Alk
> 1.5 Meq /l, or no mater what the Alk level is, if the pH is the same, the
ratio's of CO2
> to HCO3 to CO3 will be the same. So you are not lost here :-)
>
> pH = 8.2
>
> Alk = 4.0 meq /l
>
> or
>
> pH = *.2
>
> Alk = 1.5 meq /
>
> The percentage or ratio is still the same for both, both will be . 0.52%
CO2, 86.4 % HCO3
> and 13.09 % @ 34.3 ppt and @ 20 C
>
> <Yeah, I guess that would work. If you intentionally put the CO2 in
> there to begin with because you must have a higher concentration of CO2 in
> your tank than in the atmosphere. I don't intentionally put CO2 in my
tank>
>
> It does work it is not a maybe. Intentionally !!!!! where are you coming
from or where
> have you been ??? CO2 is produced by normal biological activity and is the
resaon behind
> many low pH's in tanks, as is room air CO2
>
> <you must have a higher concentration of CO2 in
> your tank than in the atmosphere>
>
> What !!! CO2 does not have to be higher than ambient air .Quite often CO2
is produced in
> the water and can't leave fast enough, has one would normally expect , by
simple diffusion
> to the atmosphere. It is the reason why CO2 can get so high in almost any
aquatic system
> and is the same reason CO2 can get so low. Why do you think Planted FW
Aquarium guys use
> CO2 injection ? As the plants can remove the CO2 faster than it can
diffuse across the
> water air interface. Same for a FOT, the CO2 can accumulate faster than it
can diffuse,
> thus crashing the pH
>
> <Not interested. I can find my own software to do this too.>
>
> Well go get some, as you need it, that is for sure.
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message
news:SFNVb.204571$Rc4.1681932@attbi_s54...
> : Oh brother. Where to start.
> :
> : pH is the -log of the hydronium ion concentration. When the hydronium
ion
> : concentration is very low, your system is basic (high pH). When the
> : hydronium ion concentration is very large, your system is acidic (low
pH).
> :
> : pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice
versa.
> : But a pH of < 7 means acidic. pH > 7 means basic.
> : pH can tell you something about acidity and basicity. It is a
measurement
> : of both, or the entire pH scale (1-14) if you will.
> :
> : >It is called "blowing it off" , such as with an airstone. If you have
high
> : CO2 and add an airstone it will drive the CO2 off raising the pH.
> :
> : Ok, you are going to try and 'purge' (the correct term) your CO2 out
with
> : air. Yeah, I guess that would work. If you intentionally put the CO2
in
> : there to begin with because you must have a higher concentration of CO2
in
> : your tank than in the atmosphere. I don't intentionally put CO2 in my
tank.
> : But I know some of you reef people due in Kalk reactors.
> :
> : >If Alk resists changes in pH then why does CO2 lower the pH without
> : affecting the Alk.
> :
> : Alkalinity is buffering capacity. Your buffers begin to get weakened
with
> : the addition of acid until they reach a point when they can no longer
> : 'buffer' and the pH crashes.
> :
> : >But I know what you mean, may use the term ALK and BC interchangeably
> :
> : Do you remember writing this in an earlier post? If you believe that
> : alkalinity and buffering capacity can be used interchangeably than I
must be
> : getting through to you.
> :
> : >When CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3.
At
> : any pH no matter what the Alk or CO2 there will be an exact ratio of
> : CO2:HCO3:CO3
> :
> : Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
your
> : point here?
> :
> : > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> : Tell me the pH and
> : > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and I
> : will give you
> : > the pH. Don't forget the temperature and Salinity.
> :
> : Not interested. I can find my own software to do this too.
> :
> : > Alk is defined as;
> : >
> : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> : [HPO4--] +
> : > 2[PO4---] - [H+]
> :
> : Ahh, now we are getting somewhere. What you are showing are components
of a
> : 'BUFFER'. Which are used in the over all 'buffering capacity'. Are we
> : going in circles here? Anyway, I think you are learning something.
> :
> : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> : maximum BC is at a
> : > pH of 6 & 9. For all practically purposes seawater has very little
> : Buffering Capacity, if
> : > any at all.
> :
> : This is the 'primary buffer' in sea water:
> :
> : H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
> :
> : If you REALLY believe that sea water has little buffering capacity, than
you
> : need to do some reading on your own. I wont be able to convince you.
> :
> : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> : maximum BC is at a
> : > pH of 6 & 9. For all practically purposes seawater has very little
> : Buffering Capacity, if
> : > any at all.
> :
> : This would be true if a monoprotic acid where used in the 'buffer', but
> : carbonic acid (the primary buffering component in seawater) is a
polyprotic
> : acid. It has two protons that can dissociate. Therefore, it has two
pKa's
> : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
The
> : pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> : right in there. Is that magic? :)
> :
> : Remember that seawater is more than a mixture of just carbonate and CO2,
> : there are other buffers involved that make it even more complicated I'm
> : sure.
> :
> : > By the way do you know who you are talking to ?
> :
> : No. Do you?
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > Let me make this clear you don't know what you are taking about
> : >
> : > "alkalinity is a measurement of 'buffering capacity'"
> : >
> : > No, it is the ability to neutralize an acid. BC is the ability to
> : withstand both upward
> : > and downward trends in pH.
> : >
> : > "pH is a measurement of 'acidity/basicity'.
> : >
> : > No, pH is a measurement of acidity and pOH is a measurement of
Basicity,
> : if you want to
> : > get picky, which seems you do.
> : >
> : >
> : > "How do you remove CO2? "
> : >
> : > It is called "blowing it off" , such as with an airstone. If you have
high
> : CO2 and add an
> : > airstone it will drive the CO2 off raising the pH. It can be proven
with a
> : glass of water,
> : > a straw, some pH color indicator and an Alk test kit and if you must a
CO2
> : test kit
> : >
> : > >You can have all the alk you want in the world and it won't help, in
> : > regards to CO2
> : >
> : > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
changes
> : in
> : > pH. This is what is meant by 'buffering capacity'"
> : >
> : > No you are wrong and very lost. If Alk resists changes in pH then why
does
> : CO2 lower the
> : > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
> : effect on CO2. When
> : > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
any
> : pH no matter what
> : > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> : >
> : > .
> : > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> : Tell me the pH and
> : > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and I
> : will give you
> : > the pH. Don't forget the temperature and Salinity.
> : >
> : > Alk is defined as;
> : >
> : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> : [HPO4--] +
> : > 2[PO4---] - [H+]
> : >
> : >
> : > Buffering Capacity is defined as;
> : >
> : > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
[H3O+])²
> : >
> : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> : maximum BC is at a
> : > pH of 6 & 9. For all practically purposes seawater has very little
> : Buffering Capacity, if
> : > any at all.
> : >
> : >
> : > Alkalinity and Buffer Capacity are closely tied but are NOT the same
> : thing, it is a
> : > misunderstanding and use of the term. Do you think water chemistry
books
> : would have
> : > separate sections on Alkalinity and Buffering Capacity if they were
the
> : same thing ?
> : >
> : > By the way do you know who you are talking to ?
> : >
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : >
> : >
> :
> :
>
>

[stoutman]

I wasn't asking you, but...

If credentials were meaningless than I wasted 7 years of my life getting a
Ph.D. Bummer.



"Boomer" > wrote in message
...
> I don't care about credentials, they are meaningless, it is what is the
answer and the
> merit of the answer, credentials or not.
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message
news:YeOVb.204890$Rc4.1682472@attbi_s54...
> : If you knew my credentials you would laugh at yourself.
> :
> :
> : "Dragon Slayer" > wrote in message
> : ...
> : > Boomer when you read that, just let it go.............no need bashing
> : heads
> : > here, the group knows what's going on.
> : >
> : > kc
> : >
> : > "stoutman" <.@.> wrote in message
> : news:SFNVb.204571$Rc4.1681932@attbi_s54...
> : > > Oh brother. Where to start.
> : > >
> : > > pH is the -log of the hydronium ion concentration. When the
hydronium
> : ion
> : > > concentration is very low, your system is basic (high pH). When the
> : > > hydronium ion concentration is very large, your system is acidic
(low
> : pH).
> : > >
> : > > pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice
> : versa.
> : > > But a pH of < 7 means acidic. pH > 7 means basic.
> : > > pH can tell you something about acidity and basicity. It is a
> : measurement
> : > > of both, or the entire pH scale (1-14) if you will.
> : > >
> : > > >It is called "blowing it off" , such as with an airstone. If you
have
> : > high
> : > > CO2 and add an airstone it will drive the CO2 off raising the pH.
> : > >
> : > > Ok, you are going to try and 'purge' (the correct term) your CO2 out
> : with
> : > > air. Yeah, I guess that would work. If you intentionally put the
CO2
> : in
> : > > there to begin with because you must have a higher concentration of
CO2
> : in
> : > > your tank than in the atmosphere. I don't intentionally put CO2 in
my
> : > tank.
> : > > But I know some of you reef people due in Kalk reactors.
> : > >
> : > > >If Alk resists changes in pH then why does CO2 lower the pH without
> : > > affecting the Alk.
> : > >
> : > > Alkalinity is buffering capacity. Your buffers begin to get
weakened
> : with
> : > > the addition of acid until they reach a point when they can no
longer
> : > > 'buffer' and the pH crashes.
> : > >
> : > > >But I know what you mean, may use the term ALK and BC
interchangeably
> : > >
> : > > Do you remember writing this in an earlier post? If you believe
that
> : > > alkalinity and buffering capacity can be used interchangeably than I
> : must
> : > be
> : > > getting through to you.
> : > >
> : > > >When CO2 is added or remove it just changes the ratio of
CO2:HCO3:CO3.
> : At
> : > > any pH no matter what the Alk or CO2 there will be an exact ratio of
> : > > CO2:HCO3:CO3
> : > >
> : > > Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What
is
> : > your
> : > > point here?
> : > >
> : > > > Go ahead and pick a seawater pH and I will tell you what that
ratio
> : is.
> : > > Tell me the pH and
> : > > > Alk and I will give the CO2 concentration. Give me the Alk and
CO2
> : and
> : > I
> : > > will give you
> : > > > the pH. Don't forget the temperature and Salinity.
> : > >
> : > > Not interested. I can find my own software to do this too.
> : > >
> : > > > Alk is defined as;
> : > > >
> : > > > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] +
[MgOH+] +
> : > > [HPO4--] +
> : > > > 2[PO4---] - [H+]
> : > >
> : > > Ahh, now we are getting somewhere. What you are showing are
components
> : of
> : > a
> : > > 'BUFFER'. Which are used in the over all 'buffering capacity'. Are
we
> : > > going in circles here? Anyway, I think you are learning something.
> : > >
> : > > > In any aqueous solution maximum BC is reached when pH= pKa.
Seawaters
> : > > maximum BC is at a
> : > > > pH of 6 & 9. For all practically purposes seawater has very little
> : > > Buffering Capacity, if
> : > > > any at all.
> : > >
> : > > This is the 'primary buffer' in sea water:
> : > >
> : > > H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
> : > >
> : > > If you REALLY believe that sea water has little buffering capacity,
than
> : > you
> : > > need to do some reading on your own. I wont be able to convince
you.
> : > >
> : > > > In any aqueous solution maximum BC is reached when pH= pKa.
Seawaters
> : > > maximum BC is at a
> : > > > pH of 6 & 9. For all practically purposes seawater has very little
> : > > Buffering Capacity, if
> : > > > any at all.
> : > >
> : > > This would be true if a monoprotic acid where used in the 'buffer',
but
> : > > carbonic acid (the primary buffering component in seawater) is a
> : > polyprotic
> : > > acid. It has two protons that can dissociate. Therefore, it has
two
> : > pKa's
> : > > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH =
8.35.
> : > The
> : > > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated
is
> : > > right in there. Is that magic? :)
> : > >
> : > > Remember that seawater is more than a mixture of just carbonate and
CO2,
> : > > there are other buffers involved that make it even more complicated
I'm
> : > > sure.
> : > >
> : > > > By the way do you know who you are talking to ?
> : > >
> : > > No. Do you?
> : > >
> : > >
> : > >
> : > >
> : > > "Boomer" > wrote in message
> : > > ...
> : > > > Let me make this clear you don't know what you are taking about
> : > > >
> : > > > "alkalinity is a measurement of 'buffering capacity'"
> : > > >
> : > > > No, it is the ability to neutralize an acid. BC is the ability to
> : > > withstand both upward
> : > > > and downward trends in pH.
> : > > >
> : > > > "pH is a measurement of 'acidity/basicity'.
> : > > >
> : > > > No, pH is a measurement of acidity and pOH is a measurement of
> : Basicity,
> : > > if you want to
> : > > > get picky, which seems you do.
> : > > >
> : > > >
> : > > > "How do you remove CO2? "
> : > > >
> : > > > It is called "blowing it off" , such as with an airstone. If you
have
> : > high
> : > > CO2 and add an
> : > > > airstone it will drive the CO2 off raising the pH. It can be
proven
> : with
> : > a
> : > > glass of water,
> : > > > a straw, some pH color indicator and an Alk test kit and if you
must a
> : > CO2
> : > > test kit
> : > > >
> : > > > >You can have all the alk you want in the world and it won't help,
in
> : > > > regards to CO2
> : > > >
> : > > > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
> : > changes
> : > > in
> : > > > pH. This is what is meant by 'buffering capacity'"
> : > > >
> : > > > No you are wrong and very lost. If Alk resists changes in pH then
why
> : > does
> : > > CO2 lower the
> : > > > pH without affecting the Alk ? CO2 has no effect on alk and alk
has no
> : > > effect on CO2. When
> : > > > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3.
At
> : any
> : > > pH no matter what
> : > > > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> : > > >
> : > > > .
> : > > > Go ahead and pick a seawater pH and I will tell you what that
ratio
> : is.
> : > > Tell me the pH and
> : > > > Alk and I will give the CO2 concentration. Give me the Alk and
CO2
> : and
> : > I
> : > > will give you
> : > > > the pH. Don't forget the temperature and Salinity.
> : > > >
> : > > > Alk is defined as;
> : > > >
> : > > > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] +
[MgOH+] +
> : > > [HPO4--] +
> : > > > 2[PO4---] - [H+]
> : > > >
> : > > >
> : > > > Buffering Capacity is defined as;
> : > > >
> : > > > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
> : [H3O+])²
> : > > >
> : > > > In any aqueous solution maximum BC is reached when pH= pKa.
Seawaters
> : > > maximum BC is at a
> : > > > pH of 6 & 9. For all practically purposes seawater has very little
> : > > Buffering Capacity, if
> : > > > any at all.
> : > > >
> : > > >
> : > > > Alkalinity and Buffer Capacity are closely tied but are NOT the
same
> : > > thing, it is a
> : > > > misunderstanding and use of the term. Do you think water chemistry
> : books
> : > > would have
> : > > > separate sections on Alkalinity and Buffering Capacity if they
were
> : the
> : > > same thing ?
> : > > >
> : > > > By the way do you know who you are talking to ?
> : > > >
> : > > > --
> : > > > Boomer
> : > > >
> : > > > Want to talk chemistry ? The Reef Chemistry Forum
> : > > > http://www.reefcentral.com/vbulletin/index.php
> : > > >
> : > > > Want to See More ?
> : > > > Please Join Our Growing Membership
> : > > > www.coralrealm.com
> : > > >
> : > > > If You See Me Running You Better Catch-Up
> : > > >
> : > > >
> : > >
> : > >
> : >
> : >
> :
> :
>
>

[Dragon Slayer]

>..........I wasted 7 years of my life getting a
> Ph.D.

you said it I didn't have to. I hope it wasn't in "Post Hole Digging".

you should have spent that time studding marine reef keeping and reading
what Boomer has added to this NG in that time. he may be old, but he knows
his stuff and the majority of this NG is going to back him on this.

kc

[Dragon Slayer]

I'll let ya slip by this time :)

kc

"Boomer" > wrote in message
...
> Sorry DS to late, before I say your post so Sorry in delay
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "Dragon Slayer" > wrote in message
> ...
> : Boomer when you read that, just let it go.............no need bashing
heads
> : here, the group knows what's going on.
> :
> : kc
> :
> : "stoutman" <.@.> wrote in message
news:SFNVb.204571$Rc4.1681932@attbi_s54...
> : > Oh brother. Where to start.
> : >
> : > pH is the -log of the hydronium ion concentration. When the hydronium
ion
> : > concentration is very low, your system is basic (high pH). When the
> : > hydronium ion concentration is very large, your system is acidic (low
pH).
> : >
> : > pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice
versa.
> : > But a pH of < 7 means acidic. pH > 7 means basic.
> : > pH can tell you something about acidity and basicity. It is a
measurement
> : > of both, or the entire pH scale (1-14) if you will.
> : >
> : > >It is called "blowing it off" , such as with an airstone. If you have
> : high
> : > CO2 and add an airstone it will drive the CO2 off raising the pH.
> : >
> : > Ok, you are going to try and 'purge' (the correct term) your CO2 out
with
> : > air. Yeah, I guess that would work. If you intentionally put the CO2
in
> : > there to begin with because you must have a higher concentration of
CO2 in
> : > your tank than in the atmosphere. I don't intentionally put CO2 in my
> : tank.
> : > But I know some of you reef people due in Kalk reactors.
> : >
> : > >If Alk resists changes in pH then why does CO2 lower the pH without
> : > affecting the Alk.
> : >
> : > Alkalinity is buffering capacity. Your buffers begin to get weakened
with
> : > the addition of acid until they reach a point when they can no longer
> : > 'buffer' and the pH crashes.
> : >
> : > >But I know what you mean, may use the term ALK and BC interchangeably
> : >
> : > Do you remember writing this in an earlier post? If you believe that
> : > alkalinity and buffering capacity can be used interchangeably than I
must
> : be
> : > getting through to you.
> : >
> : > >When CO2 is added or remove it just changes the ratio of
CO2:HCO3:CO3. At
> : > any pH no matter what the Alk or CO2 there will be an exact ratio of
> : > CO2:HCO3:CO3
> : >
> : > Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What
is
> : your
> : > point here?
> : >
> : > > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> : > Tell me the pH and
> : > > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and
> : I
> : > will give you
> : > > the pH. Don't forget the temperature and Salinity.
> : >
> : > Not interested. I can find my own software to do this too.
> : >
> : > > Alk is defined as;
> : > >
> : > > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+]
+
> : > [HPO4--] +
> : > > 2[PO4---] - [H+]
> : >
> : > Ahh, now we are getting somewhere. What you are showing are
components of
> : a
> : > 'BUFFER'. Which are used in the over all 'buffering capacity'. Are
we
> : > going in circles here? Anyway, I think you are learning something.
> : >
> : > > In any aqueous solution maximum BC is reached when pH= pKa.
Seawaters
> : > maximum BC is at a
> : > > pH of 6 & 9. For all practically purposes seawater has very little
> : > Buffering Capacity, if
> : > > any at all.
> : >
> : > This is the 'primary buffer' in sea water:
> : >
> : > H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
> : >
> : > If you REALLY believe that sea water has little buffering capacity,
than
> : you
> : > need to do some reading on your own. I wont be able to convince you.
> : >
> : > > In any aqueous solution maximum BC is reached when pH= pKa.
Seawaters
> : > maximum BC is at a
> : > > pH of 6 & 9. For all practically purposes seawater has very little
> : > Buffering Capacity, if
> : > > any at all.
> : >
> : > This would be true if a monoprotic acid where used in the 'buffer',
but
> : > carbonic acid (the primary buffering component in seawater) is a
> : polyprotic
> : > acid. It has two protons that can dissociate. Therefore, it has two
> : pKa's
> : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
> : The
> : > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated
is
> : > right in there. Is that magic? :)
> : >
> : > Remember that seawater is more than a mixture of just carbonate and
CO2,
> : > there are other buffers involved that make it even more complicated
I'm
> : > sure.
> : >
> : > > By the way do you know who you are talking to ?
> : >
> : > No. Do you?
> : >
> : >
> : >
> : >
> : > "Boomer" > wrote in message
> : > ...
> : > > Let me make this clear you don't know what you are taking about
> : > >
> : > > "alkalinity is a measurement of 'buffering capacity'"
> : > >
> : > > No, it is the ability to neutralize an acid. BC is the ability to
> : > withstand both upward
> : > > and downward trends in pH.
> : > >
> : > > "pH is a measurement of 'acidity/basicity'.
> : > >
> : > > No, pH is a measurement of acidity and pOH is a measurement of
Basicity,
> : > if you want to
> : > > get picky, which seems you do.
> : > >
> : > >
> : > > "How do you remove CO2? "
> : > >
> : > > It is called "blowing it off" , such as with an airstone. If you
have
> : high
> : > CO2 and add an
> : > > airstone it will drive the CO2 off raising the pH. It can be proven
with
> : a
> : > glass of water,
> : > > a straw, some pH color indicator and an Alk test kit and if you must
a
> : CO2
> : > test kit
> : > >
> : > > >You can have all the alk you want in the world and it won't help,
in
> : > > regards to CO2
> : > >
> : > > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
> : changes
> : > in
> : > > pH. This is what is meant by 'buffering capacity'"
> : > >
> : > > No you are wrong and very lost. If Alk resists changes in pH then
why
> : does
> : > CO2 lower the
> : > > pH without affecting the Alk ? CO2 has no effect on alk and alk has
no
> : > effect on CO2. When
> : > > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
any
> : > pH no matter what
> : > > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> : > >
> : > > .
> : > > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> : > Tell me the pH and
> : > > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and
> : I
> : > will give you
> : > > the pH. Don't forget the temperature and Salinity.
> : > >
> : > > Alk is defined as;
> : > >
> : > > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+]
+
> : > [HPO4--] +
> : > > 2[PO4---] - [H+]
> : > >
> : > >
> : > > Buffering Capacity is defined as;
> : > >
> : > > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
[H3O+])²
> : > >
> : > > In any aqueous solution maximum BC is reached when pH= pKa.
Seawaters
> : > maximum BC is at a
> : > > pH of 6 & 9. For all practically purposes seawater has very little
> : > Buffering Capacity, if
> : > > any at all.
> : > >
> : > >
> : > > Alkalinity and Buffer Capacity are closely tied but are NOT the same
> : > thing, it is a
> : > > misunderstanding and use of the term. Do you think water chemistry
books
> : > would have
> : > > separate sections on Alkalinity and Buffering Capacity if they were
the
> : > same thing ?
> : > >
> : > > By the way do you know who you are talking to ?
> : > >
> : > > --
> : > > Boomer
> : > >
> : > > Want to talk chemistry ? The Reef Chemistry Forum
> : > > http://www.reefcentral.com/vbulletin/index.php
> : > >
> : > > Want to See More ?
> : > > Please Join Our Growing Membership
> : > > www.coralrealm.com
> : > >
> : > > If You See Me Running You Better Catch-Up
> : > >
> : > >
> : >
> : >
> :
> :
>
>

[stoutman]

"Post Hole Digging".

Good one. very original. No actually Organic Chem.

> you should have spent that time studding marine reef keeping and reading
> what Boomer has added to this NG in that time.

Based on what I have read of his posts thus far, I wouldn't recommend that
to anyone.








"Dragon Slayer" > wrote in message
...
> >..........I wasted 7 years of my life getting a
> > Ph.D.
>
> you said it I didn't have to. I hope it wasn't in "Post Hole Digging".
>
> you should have spent that time studding marine reef keeping and reading
> what Boomer has added to this NG in that time. he may be old, but he
knows
> his stuff and the majority of this NG is going to back him on this.
>
> kc
>
>
>
>
>
>

[stoutman]

>By the way do you know who you are talking to ?

This cracks me up. Someone is a little pompous. I gather from the
responders in this thread that Boomer is some kind of self proclaimed
aquarium guru.

I can only assume that he is a Marine Biologist that needs to take a few
more chemistry courses. Boomer, if you are an author of aquarium
literature, than I would like to be acknowledged in your next manuscript for
helping you see the light.

I too can be pompous.

-Stoutman












"Boomer" > wrote in message
...
> Let me make this clear you don't know what you are taking about
>
> "alkalinity is a measurement of 'buffering capacity'"
>
> No, it is the ability to neutralize an acid. BC is the ability to
withstand both upward
> and downward trends in pH.
>
> "pH is a measurement of 'acidity/basicity'.
>
> No, pH is a measurement of acidity and pOH is a measurement of Basicity,
if you want to
> get picky, which seems you do.
>
>
> "How do you remove CO2? "
>
> It is called "blowing it off" , such as with an airstone. If you have high
CO2 and add an
> airstone it will drive the CO2 off raising the pH. It can be proven with a
glass of water,
> a straw, some pH color indicator and an Alk test kit and if you must a CO2
test kit
>
> >You can have all the alk you want in the world and it won't help, in
> regards to CO2
>
> "Wrong. Alkalinity increases your tank's ability to RESIST sharp changes
in
> pH. This is what is meant by 'buffering capacity'"
>
> No you are wrong and very lost. If Alk resists changes in pH then why does
CO2 lower the
> pH without affecting the Alk ? CO2 has no effect on alk and alk has no
effect on CO2. When
> CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At any
pH no matter what
> the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
>
> .
> Go ahead and pick a seawater pH and I will tell you what that ratio is.
Tell me the pH and
> Alk and I will give the CO2 concentration. Give me the Alk and CO2 and I
will give you
> the pH. Don't forget the temperature and Salinity.
>
> Alk is defined as;
>
> TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
[HPO4--] +
> 2[PO4---] - [H+]
>
>
> Buffering Capacity is defined as;
>
> BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka + [H3O+])²
>
> In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
maximum BC is at a
> pH of 6 & 9. For all practically purposes seawater has very little
Buffering Capacity, if
> any at all.
>
>
> Alkalinity and Buffer Capacity are closely tied but are NOT the same
thing, it is a
> misunderstanding and use of the term. Do you think water chemistry books
would have
> separate sections on Alkalinity and Buffering Capacity if they were the
same thing ?
>
> By the way do you know who you are talking to ?
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
>
>

[Boomer]

You are so funny you make me laugh, it is just a riot .

I said seawater has very little buffering capacity, I did not say it had very little Alk .
What ever it is there is still a % of x ,y and z that make it up.You are sill confusing
Buffering Capacity and Alk, so I would suggest to give it up as you are clueless

"Downwards trends of what? Acidity? Basicity? "

Alkalinity is the ability to slow down or inhibit downward trends in pH. I think you are
smart enough to know what a downward trend in pH is correct, as in lowering the pH. ?
Acidity is the ability to inhibit or slow down upward trends in pH, or to slow down
rising pH. It is only **common sense ** there is an opposite to Alkalinity, which is
Acidity

"Have I ever heard of an
acidity test? "

Well, then you don't know much about water chemistry.

Acidity = A std alkali titration to methyl orange or phenolphthalein endpoint

Alkalinity = A std acid titration to phenolphthalein endpoint



Well, then you don't know much. Please consult a water chemistry book, I DID NOT POST
AQUARIUM BOOKS. I posted college and graduate level seawater chemistry books, so it tells
me just how much you don't know about water chemistry, let alone seawater chemistry .Do
search on those authors, forget it, as I have them. Please pay attention.

An Introduction to the Chemistry of the Sea, by Michael E. Q. Pilson, Ph.D. 432pages
Graduate School of Oceanography
University of Rode Island

Chemical Oceanography, by Frank J.Millero, Ph.D, 531 pages
Rosenstiel School of Marine and Atmospheric Science.
University of Miami.

Introduction to Marine Chemistry, J.P Riley,Ph.D, 465 pages.
Department of Oceanography, University of Liverpool, England

Chemical Oceanography Vol 2, by J.P Riley, Ph.D and G Skirrow,Ph.D, 712pages
Same for Riley above.
Skirrow
Department of Inorganic, Physical and Industrial Chemistry
University of Liverpool. England

Practice Handbook of Marine Science, Michael J. Kennish, Ph.D
Senior Environmental Scientist
GPU Nuclear Corporation and
Professor of Fisheries and Aquaculture, Rutgers University.

Seawater: its Composition, Properties and Behavior,. Staff, Open University, 165 pages

Seawater Aquariums: The Captive Environment, by Stephen Spotte,Ph.D, 413 pages
Vice President, Sea Research Foundation and Director Mystic Marinelife Aquarium
( this is not a so called "aquarium book", it is a very advanced textbook)

Please consult the graduate level text book, high on theory and application, by J.F.
Pankow, Ph.D. Aquatic Chemistry Concepts. Chapter 8 is on Buffering Capacity and Chapter 9
deals with Alkalinity and Acidity. Hum, if they are the same, why then are they discussed
separately and defined differently

To continue with you lack of understanding.

First, quite trying to twist thing as they suit you.


"Ever heard of the Henderson-Hasselbach equation?"

Yes, and you seem to have missed that they are also a faction of salinity and temperature.
Seawater "skews" the pKa1 and pKa2 to the left, giving LOWER values in seawater.Almost any
seawater text book gives those pKa's for seawater vs FW at x salinity and temp. Buy the
way just to show you where I am and where you are.Ever hear of ;

pH(NIST), pH(NSW), pKa (NIST), pKa (NSW). Do you also know that in seawater a pH meter
does not give the proper value, it is called "salt error affect" and that is what pKa
(NSW). & pH(NSW), is all about.032

Pilson gives s full pages of tables for pKa's from 0-40 C and 0 -40 ppt Salinity. But I
suppose he doesn't know what he is taking about.

"Therefore, at a pH of 8.3 (seawater for this example) the majority of
carbonate in solution exists as HCO3-2 not CO3-2"


I never said the majority was as CO3, so where did that come from. Please re-read what I
said....here again ..you still need lots of help

@ 20C and 34.3 ppt salinity

CO2 = 0.52 %

HCO3 = 86.4 %

CO3 = 13.09 %

so you aren't confused any more


@ 20 C, pH 8.2 and 30.7ppt Salinity

CO2 = .55 %,

HCO3 = 87.8 %

CO3 = 11.60 %

Take note at the same temp and pH as the salinity falls there is an increase in the CO2
and increase in the HCO3 and decrease in CO3. So take your equation and stick it.When
dealing with seawater you MUST calculate pKa's differently more or less, although you
could use these for FW with a 0 salinity plugged in. For seawater the pKa1;

pK1* = pK1 + ( -840.39/T + 19.894 - 3.0189 lnT) S *1/2 + .00668S

where

pK1 =- 6320.81T - 126.3405 + 19.568 lnT

Where T =temp in Kelvin and S =salinity in ppt and ln = natural log

From
Millero, 1992, Chemical Oceanography.

"This is
why this topic so muddied."

Hum, you are the one today mudding it all up

"You are saying seawater has no buffering capacity and you are saying 1/3 of
seawaters Buffer Capacity is due to MgCO3 ??"

I see you are still lost. It is about nil Buffering Capacity, which means there is very
little to stop upward or downward shifts in pH. If seawater was at a pH of 6 or 9 it would
be very, very high Buffering Capacity and would be difficult to cause the pH shifts up or
down, as half of the buffer on either side of 6 of 9 is an acid and the other half a base.

"Oh, man. Interesting. Here is another contradiction of yours. You said
before you purge CO2 from your tank with air to raise the pH. Here you are
telling me that CO2 from air is the reason behind many low pH.

You are really lost aren't you and trying one of the Mr. Twister tactics.

I said you can raise the pH by blowing of the CO2. Most of the CO2 in water is not
hydrated but is free CO2. There will always be some CO2 in the water. The more there is
the easier it is to purge off . Not ALL tanks have excess CO2. The more there is the
higher the pH will rise if you blow it off. Many aquariums have excess CO2, from normal
biological activity, which can/will lower the tank pH ( nothing to do with air). It is a
common problem in this hobby. Others often think they have tank CO2 problems, when the
real issue is not CO2 generation in the tank but have very low tank CO2. It is high room
air CO2, which can be quite high, especially in the winter, much more so than the tank, so
it can diffuses much easier into the tank water, giving the false idea they have excess
load problems producing CO2, when they actually don't and lowering the pH .Using outside
air CO2 will greatly reduce this problem. Some tanks have higher CO2 tanks others which
may be low or maybe some are in the middle. Tanks with large amounts of plants will
usually suck up all the CO2 and begin to feed of the HCO3 and CO3 for their C needs, which
will raise the pH. FOT usually have excess CO2. Having a party in your house by itself can
lower the pH of your tank do excess room air CO2 build-up. It all depends on the
circumstances of the tank, the room air, the bio-load, skimming and even the type of
animals and plants.

Please get out of those "general" chemistry books and check a water, aquatic or seawater
chemistry book, before you speak about something you don't know. If you did, we would not
be having this debate but you would be agreeing with me. And to disagree with me is to
disagree with all the authors I posted above. By the way, feel free to contact or e-mail
Dr. Frank J, Millero. Here is his website. I have talked to him a number of times in the
past on these issues.

http://www.rsmas.miami.edu/groups/jmc/fla-bay/fbay.html

By the way there is always a link below my name, you may want to go there and do a search
on me and what I know and don't know. No, I sure as hell don't know everything, we all
make mistakes, as you have here.

Articles by;
Dr. Randy Holmes-Farely (Harvard graduate chemist) and Dr. Craig Bingman from Columbia
University, Department of Chemistry ( he runs the lab there last time I checked) Please
review Randy's credentials, as you like them things :-)

One finally note or question to see where you are. Does CO2 have an effect on Alk, YES or
NO. If you say yes, go back to the books you have.

From your last post;

"The equilibrium will
be shifted to HCO3-2 by a ratio of 1:100."

No it won't, that is for freshwater NOT seawater, how many time do I have to tell you that

"Based on what I have read of his posts thus far, I wouldn't recommend that
to anyone."

Hum, we all know that it is me and not you that knows their P's & Q's. I have info and all
that data to back me yup, yours is a lack of understanding of seawater chemistry and the
issues at hand .I have posted this info on many forums, to include here, where Craig
Bingman use to come often. To include on the Reef Chemistry Forum at RC, none have
challenged what I said and many are chemists with Ph.D's.

Finally

But I know what
you mean, man*y use the term ALK and BC interchangeably.

I said this as many do but it is incorrect from a chemical point but I understand what you
mean. Many in this hobby say Alk in one breath and buffering capacity in another breath,
technically they are not the same as I have defined in words and equations.This hobby is
plagued with myths and misconceptions and I like to have thing in order as what they
really are.

So, so much for your Ph.D in chemistry :-)

I don't even have a degree in chemistry or biology.I don't need one to understand it, you
do and you are still lost.

Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
www.coralrealm.com

If You See Me Running You Better Catch-Up
"stoutman" <.@.> wrote in message news:8mQVb.212632$nt4.990652@attbi_s51...
: >Alkalinity only deals with downward trends and says nothing of upward
: trends. Ever hear of an Acidity test kit ?
:
: Downwards trends of what? Acidity? Basicity? Have I ever heard of an
: acidity test? Yeah, it's called pH paper. or a pH meter.
:
: > As far as primary "buffers" in seawater you are lost again. The principle
: buffers of seawater are HCO3, CO3.
:
: Ever heard of the Henderson-Hasselbach equation?
:
: pH = pKa + log [HA]/[A-]
:
: The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this example)
: you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium will
: be shifted to HCO3-2 by a ratio of 1:100.
:
: 8.3 = 10.3 + log [HCO3-2]/[CO3-2]
: -2 = log [HCO3-2]/[CO3-2]
:
: take antilog of both sides and you get:
:
: .01 = [HCO3-2]/[CO3-2]
:
: Therefore, at a pH of 8.3 (seawater for this example) the majority of
: carbonate in solution exists as HCO3-2 not CO3-2. That is why I did not
: include it in my buffer example.
:
: You said:
: >The principle buffers of seawater are HCO3, CO3 and B(OH4).
:
: and You said in a previous post:
:
: >For all practically purposes seawater has very little Buffering Capacity,
: if any at all.
:
: STOP contradicting yourself, you are confusing the matter for yourself and
: others. How can HCO3, CO3 and B(OH4) be buffers in seawater if "For all
: practically purposes seawater has very little Buffering Capacity" AND if
: "About 1/3 of seawaters Buffer Capacity is due to MgCO3" ?????
:
: You are saying seawater has no buffering capacity and you are saying 1/3 of
: seawaters Buffer Capacity is due to MgCO3 ??
:
: Are you on drugs? Just kidding. I just want to help you understand.
:
: Can I make a suggestion for you? Stop getting your chemistry knowledge from
: aquarium books. Most are written by Marine Biologists, not CHEMISTS, like
: myself. I have seen NUMEROUS chemistry flaws in aquarium books. This is
: why this topic so muddied.
:
: > It does work it is not a maybe. Intentionally !!!!! where are you coming
: from or where
: > have you been ??? CO2 is produced by normal biological activity and is the
: reason behind
: > many low pH's in tanks, as is room air CO2
:
: Oh, man. Interesting. Here is another contradiction of yours. You said
: before you purge CO2 from your tank with air to raise the pH. Here you are
: telling me that CO2 from air is the reason behind many low pH's.
:
:
: > pKa1 = 6.0 pKa2 = 9.1
: > From Introduction to Marine Chemistry by Riley and Chester. Also from, An
: Introduction to the Chemistry of the Sea, by Pilson
:
: STOP GETTING YOUR CHEMISTRY FROM AQUARIUM BOOKS. Get a CHEMISTRY book.
:
: > Well go get some, as you need it, that is for sure.
:
: Not likely.
:
:
:
:
:
:
:
: "Boomer" > wrote in message
: ...
: > <Alkalinity is buffering capacity. >
: >
: > No it is not, they are not calculated the same. I already gave the
: equations please, you
: > seem to avoiding them. Please consult an aquatic chemistry book.
: >
: > ">But I know what you mean, many use the term ALK and BC interchangeably"
: >
: > Yes, I most certainly do and stated it is incorrect but I know what you
: mean
: >
: >
: > <If you believe that
: > alkalinity and buffering capacity can be used interchangeably than I must
: be
: > getting through to you.>
: >
: > Please don't make me laugh. No I'm not getting through
: >
: >
: > <Which are used in the over all 'buffering capacity'. Are we
: > going in circles here? Anyway, I think you are learning something>
: >
: > No I'm not learning anything but you need to. No I'm not talking in a
: circle but maybe you
: > are. You must have missed it, so here it is again. Buffer capacity is the
: ability to with
: > stand upward & downward trends in pH. Alkalinity only deals with downward
: trends and says
: > nothing of upward trends. Ever hear of an Acidity test kit ?
: >
: > <This is the 'primary buffer' in sea water:>
: >
: > H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1"
: >
: > You are lost, the reaction that it is inherent to is;........... and you
: are missing some
: > things
: >
: > 2HCO3 <--->CO2 + H20 + ***CO3***
: >
: >
: > As far as primary "buffers" in seawater you are lost again. The principle
: buffers of
: > seawater are HCO3, CO3 and
: > B(OH4). I might add that Ion pairs are also part of the Buffer Capacity.
: About 1/3 of
: > seawaters Buffer Capacity is due to MgCO3. Like I said you don't
: understand Buffer
: > Capacity and Alkalinity. Seawater manuals and text books are filled with
: this kind of
: > data.Would you like me to give a list of some ?? :-)
: >
: > "If you REALLY believe that sea water has little buffering capacity, than
: you
: > need to do some reading on your own. I wont be able to convince you."
: >
: > It doesn't if you understand the issue and it is quite clear you don't.
: You are the one
: > that need to do allllllllllllot of reading
: >
: > ***For terms are commonly used to describe various aspects of the seawater
: buffer system:
: >
: > 1.pH
: >
: > 2. Buffering Capacity
: >
: > 3. Alkalinity or Total Alkalinity
: >
: > 4. Carbonate Alkalinity***
: >
: > From;
: > Spotte, Seawater Aquariums the Captive Environment ( a technical text book
: on seawater and
: > seawater aquariums)
: >
: >
: > ***In seawater, for example, maximum Buffering Capacity appears at pH
: values near 6 and 9
: > and seawater is buffered very little , if at all, at its normal pH of
: 8.2***
: >
: > From;
: > Skirrow, 1975 Chemical Oceanography Vol 2
: >
: > <but
: > carbonic acid (the primary buffering component in seawater) >
: >
: > Bicarbonate is the primary buffer not carbonic acid ,where on God's earth
: did you get that
: > from. At normal temp, salinity, pH and Alk it is;
: >
: > @ 20C and 34.3 ppt salinity
: >
: > CO2 = 0.52 %
: >
: > HCO3 = 86.4 %
: >
: > CO3 = 13.09 %
: >
: > From;
: > Practical Handbook of Marine Science, M.J. Kennish
: >
: > <Therefore, it has two pKa's
: > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
: The
: > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
: > right in there. Is that magic? :)>
: >
: > Magic !!!! it must be by your account. That is FW there pal, not
: seawater, lets get the
: > water straight here that we are dealing with, so you aren't so lost.
: >
: > The;
: > pKa1 = 6.0
: >
: > pKa2 = 9.1
: >
: > From;
: > Introduction to Marine Chemistry by Riley and Chester. Also from, An
: Introduction to the
: > Chemistry of the Sea, by Pilson
: >
: > So your equation does not work as you gave it.
: >
: > (6.0 + 9.1) / 2 = 7.55 pH Hum, maybe you would care to explain that
: since you seem to
: > think you have all the answers.
: >
: > <Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
: your
: > point here?>
: >
: > It means that if the pH is 8.3 and the Alk is 4.0 meq/ l or if the is pH
: 8.3 and the Alk
: > 1.5 Meq /l, or no mater what the Alk level is, if the pH is the same, the
: ratio's of CO2
: > to HCO3 to CO3 will be the same. So you are not lost here :-)
: >
: > pH = 8.2
: >
: > Alk = 4.0 meq /l
: >
: > or
: >
: > pH = *.2
: >
: > Alk = 1.5 meq /
: >
: > The percentage or ratio is still the same for both, both will be . 0.52%
: CO2, 86.4 % HCO3
: > and 13.09 % @ 34.3 ppt and @ 20 C
: >
: > <Yeah, I guess that would work. If you intentionally put the CO2 in
: > there to begin with because you must have a higher concentration of CO2 in
: > your tank than in the atmosphere. I don't intentionally put CO2 in my
: tank>
: >
: > It does work it is not a maybe. Intentionally !!!!! where are you coming
: from or where
: > have you been ??? CO2 is produced by normal biological activity and is the
: resaon behind
: > many low pH's in tanks, as is room air CO2
: >
: > <you must have a higher concentration of CO2 in
: > your tank than in the atmosphere>
: >
: > What !!! CO2 does not have to be higher than ambient air .Quite often CO2
: is produced in
: > the water and can't leave fast enough, has one would normally expect , by
: simple diffusion
: > to the atmosphere. It is the reason why CO2 can get so high in almost any
: aquatic system
: > and is the same reason CO2 can get so low. Why do you think Planted FW
: Aquarium guys use
: > CO2 injection ? As the plants can remove the CO2 faster than it can
: diffuse across the
: > water air interface. Same for a FOT, the CO2 can accumulate faster than it
: can diffuse,
: > thus crashing the pH
: >
: > <Not interested. I can find my own software to do this too.>
: >
: > Well go get some, as you need it, that is for sure.
: > --
: > Boomer
: >
: > Want to talk chemistry ? The Reef Chemistry Forum
: > http://www.reefcentral.com/vbulletin/index.php
: >
: > Want to See More ?
: > Please Join Our Growing Membership
: > www.coralrealm.com
: >
: > If You See Me Running You Better Catch-Up
: > "stoutman" <.@.> wrote in message
: news:SFNVb.204571$Rc4.1681932@attbi_s54...
: > : Oh brother. Where to start.
: > :
: > : pH is the -log of the hydronium ion concentration. When the hydronium
: ion
: > : concentration is very low, your system is basic (high pH). When the
: > : hydronium ion concentration is very large, your system is acidic (low
: pH).
: > :
: > : pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice
: versa.
: > : But a pH of < 7 means acidic. pH > 7 means basic.
: > : pH can tell you something about acidity and basicity. It is a
: measurement
: > : of both, or the entire pH scale (1-14) if you will.
: > :
: > : >It is called "blowing it off" , such as with an airstone. If you have
: high
: > : CO2 and add an airstone it will drive the CO2 off raising the pH.
: > :
: > : Ok, you are going to try and 'purge' (the correct term) your CO2 out
: with
: > : air. Yeah, I guess that would work. If you intentionally put the CO2
: in
: > : there to begin with because you must have a higher concentration of CO2
: in
: > : your tank than in the atmosphere. I don't intentionally put CO2 in my
: tank.
: > : But I know some of you reef people due in Kalk reactors.
: > :
: > : >If Alk resists changes in pH then why does CO2 lower the pH without
: > : affecting the Alk.
: > :
: > : Alkalinity is buffering capacity. Your buffers begin to get weakened
: with
: > : the addition of acid until they reach a point when they can no longer
: > : 'buffer' and the pH crashes.
: > :
: > : >But I know what you mean, may use the term ALK and BC interchangeably
: > :
: > : Do you remember writing this in an earlier post? If you believe that
: > : alkalinity and buffering capacity can be used interchangeably than I
: must be
: > : getting through to you.
: > :
: > : >When CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3.
: At
: > : any pH no matter what the Alk or CO2 there will be an exact ratio of
: > : CO2:HCO3:CO3
: > :
: > : Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
: your
: > : point here?
: > :
: > : > Go ahead and pick a seawater pH and I will tell you what that ratio
: is.
: > : Tell me the pH and
: > : > Alk and I will give the CO2 concentration. Give me the Alk and CO2
: and I
: > : will give you
: > : > the pH. Don't forget the temperature and Salinity.
: > :
: > : Not interested. I can find my own software to do this too.
: > :
: > : > Alk is defined as;
: > : >
: > : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
: > : [HPO4--] +
: > : > 2[PO4---] - [H+]
: > :
: > : Ahh, now we are getting somewhere. What you are showing are components
: of a
: > : 'BUFFER'. Which are used in the over all 'buffering capacity'. Are we
: > : going in circles here? Anyway, I think you are learning something.
: > :
: > : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: > : maximum BC is at a
: > : > pH of 6 & 9. For all practically purposes seawater has very little
: > : Buffering Capacity, if
: > : > any at all.
: > :
: > : This is the 'primary buffer' in sea water:
: > :
: > : H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
: > :
: > : If you REALLY believe that sea water has little buffering capacity, than
: you
: > : need to do some reading on your own. I wont be able to convince you.
: > :
: > : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: > : maximum BC is at a
: > : > pH of 6 & 9. For all practically purposes seawater has very little
: > : Buffering Capacity, if
: > : > any at all.
: > :
: > : This would be true if a monoprotic acid where used in the 'buffer', but
: > : carbonic acid (the primary buffering component in seawater) is a
: polyprotic
: > : acid. It has two protons that can dissociate. Therefore, it has two
: pKa's
: > : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
: The
: > : pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
: > : right in there. Is that magic? :)
: > :
: > : Remember that seawater is more than a mixture of just carbonate and CO2,
: > : there are other buffers involved that make it even more complicated I'm
: > : sure.
: > :
: > : > By the way do you know who you are talking to ?
: > :
: > : No. Do you?
: > :
: > :
: > :
: > :
: > : "Boomer" > wrote in message
: > : ...
: > : > Let me make this clear you don't know what you are taking about
: > : >
: > : > "alkalinity is a measurement of 'buffering capacity'"
: > : >
: > : > No, it is the ability to neutralize an acid. BC is the ability to
: > : withstand both upward
: > : > and downward trends in pH.
: > : >
: > : > "pH is a measurement of 'acidity/basicity'.
: > : >
: > : > No, pH is a measurement of acidity and pOH is a measurement of
: Basicity,
: > : if you want to
: > : > get picky, which seems you do.
: > : >
: > : >
: > : > "How do you remove CO2? "
: > : >
: > : > It is called "blowing it off" , such as with an airstone. If you have
: high
: > : CO2 and add an
: > : > airstone it will drive the CO2 off raising the pH. It can be proven
: with a
: > : glass of water,
: > : > a straw, some pH color indicator and an Alk test kit and if you must a
: CO2
: > : test kit
: > : >
: > : > >You can have all the alk you want in the world and it won't help, in
: > : > regards to CO2
: > : >
: > : > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
: changes
: > : in
: > : > pH. This is what is meant by 'buffering capacity'"
: > : >
: > : > No you are wrong and very lost. If Alk resists changes in pH then why
: does
: > : CO2 lower the
: > : > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
: > : effect on CO2. When
: > : > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
: any
: > : pH no matter what
: > : > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
: > : >
: > : > .
: > : > Go ahead and pick a seawater pH and I will tell you what that ratio
: is.
: > : Tell me the pH and
: > : > Alk and I will give the CO2 concentration. Give me the Alk and CO2
: and I
: > : will give you
: > : > the pH. Don't forget the temperature and Salinity.
: > : >
: > : > Alk is defined as;
: > : >
: > : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
: > : [HPO4--] +
: > : > 2[PO4---] - [H+]
: > : >
: > : >
: > : > Buffering Capacity is defined as;
: > : >
: > : > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
: [H3O+])²
: > : >
: > : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: > : maximum BC is at a
: > : > pH of 6 & 9. For all practically purposes seawater has very little
: > : Buffering Capacity, if
: > : > any at all.
: > : >
: > : >
: > : > Alkalinity and Buffer Capacity are closely tied but are NOT the same
: > : thing, it is a
: > : > misunderstanding and use of the term. Do you think water chemistry
: books
: > : would have
: > : > separate sections on Alkalinity and Buffering Capacity if they were
: the
: > : same thing ?
: > : >
: > : > By the way do you know who you are talking to ?
: > : >
: > : > --
: > : > Boomer
: > : >
: > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > http://www.reefcentral.com/vbulletin/index.php
: > : >
: > : > Want to See More ?
: > : > Please Join Our Growing Membership
: > : > www.coralrealm.com
: > : >
: > : > If You See Me Running You Better Catch-Up
: > : >
: > : >
: > :
: > :
: >
: >
:
:

[Boomer]

No, I don't write anything. I explain things to people such as yourself that don't
understand the issue.


"By the way do you know who you are talking to ?"

This was more on the order of a joke to get your attention. I have been around about 35
years. I also get a real charge of people like yourself , that come here or forums and
toot your BS, assuming you must be right and we are all idiots lol

"Someone is a little pompous"

Now here we go with the name calling. I can see where you are coming from, does it make
you feel better or do you think that makes you correct. It is rather childless don't you
think ?

If I did you would be the last , as you are way to lost on seawater chemistry

What's interesting and I'm sure to everyone it is, the big hole you just keep digging for
yourself. lol

You must be nervous, you sure seem be bothered by these post and my drilling you with info
from refs, Seawater Chemistry books, written by seawater chemists. I must make you look
bad,Ph.D and all :-) I think Millero has been at it about 40 years and has written 3
advanced textbooks on chemical oceanography. Hum, you may also want to check out Stumm &
Morgan .Of course there are others, i.e Morel, Benjamin(the newest water chemistry book
2002) and lets not forget the "old great book" by Snoeyink and Jenkins, still in print. I
have them all :-)

A smart guy MAY want to go look at my ref, especially a Ph.D chemist such as yourself :-)
--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
www.coralrealm.com

If You See Me Running You Better Catch-Up
"stoutman" <.@.> wrote in message news:EfSVb.12701$QA2.22009@attbi_s52...
: >By the way do you know who you are talking to ?
:
: This cracks me up. Someone is a little pompous. I gather from the
: responders in this thread that Boomer is some kind of self proclaimed
: aquarium guru.
:
: I can only assume that he is a Marine Biologist that needs to take a few
: more chemistry courses. Boomer, if you are an author of aquarium
: literature, than I would like to be acknowledged in your next manuscript for
: helping you see the light.
:
: I too can be pompous.
:
: -Stoutman
:
:
:
:
:
:
:
:
:
:
:
:
: "Boomer" > wrote in message
: ...
: > Let me make this clear you don't know what you are taking about
: >
: > "alkalinity is a measurement of 'buffering capacity'"
: >
: > No, it is the ability to neutralize an acid. BC is the ability to
: withstand both upward
: > and downward trends in pH.
: >
: > "pH is a measurement of 'acidity/basicity'.
: >
: > No, pH is a measurement of acidity and pOH is a measurement of Basicity,
: if you want to
: > get picky, which seems you do.
: >
: >
: > "How do you remove CO2? "
: >
: > It is called "blowing it off" , such as with an airstone. If you have high
: CO2 and add an
: > airstone it will drive the CO2 off raising the pH. It can be proven with a
: glass of water,
: > a straw, some pH color indicator and an Alk test kit and if you must a CO2
: test kit
: >
: > >You can have all the alk you want in the world and it won't help, in
: > regards to CO2
: >
: > "Wrong. Alkalinity increases your tank's ability to RESIST sharp changes
: in
: > pH. This is what is meant by 'buffering capacity'"
: >
: > No you are wrong and very lost. If Alk resists changes in pH then why does
: CO2 lower the
: > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
: effect on CO2. When
: > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At any
: pH no matter what
: > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
: >
: > .
: > Go ahead and pick a seawater pH and I will tell you what that ratio is.
: Tell me the pH and
: > Alk and I will give the CO2 concentration. Give me the Alk and CO2 and I
: will give you
: > the pH. Don't forget the temperature and Salinity.
: >
: > Alk is defined as;
: >
: > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
: [HPO4--] +
: > 2[PO4---] - [H+]
: >
: >
: > Buffering Capacity is defined as;
: >
: > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka + [H3O+])²
: >
: > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: maximum BC is at a
: > pH of 6 & 9. For all practically purposes seawater has very little
: Buffering Capacity, if
: > any at all.
: >
: >
: > Alkalinity and Buffer Capacity are closely tied but are NOT the same
: thing, it is a
: > misunderstanding and use of the term. Do you think water chemistry books
: would have
: > separate sections on Alkalinity and Buffering Capacity if they were the
: same thing ?
: >
: > By the way do you know who you are talking to ?
: >
: > --
: > Boomer
: >
: > Want to talk chemistry ? The Reef Chemistry Forum
: > http://www.reefcentral.com/vbulletin/index.php
: >
: > Want to See More ?
: > Please Join Our Growing Membership
: > www.coralrealm.com
: >
: > If You See Me Running You Better Catch-Up
: >
: >
:
:

[stoutman]

I am going to have to start charging you a fee after this. Ok?


>Alkalinity is the ability to slow down or inhibit downward trends in pH.

Agreed. This is an effect of 'buffering'

Oh wait, you have another definition of alkalinity.

> Alkalinity = A std acid titration to phenolphthalein endpoint

You are VERY confused.

> Please consult the graduate level text book, high on theory and
application, by J.F.
> Pankow, Ph.D. Aquatic Chemistry Concepts. Chapter 8 is on Buffering
Capacity and Chapter 9
> deals with Alkalinity and Acidity.

Believe me, I don't need to. I have plenty of chem books that cover the
topic quite well.

>Hum, if they are the same, why then are they discussed separately and
defined differently
probably because they were not written by a CHEMIST.

> Acidity = A std alkali titration to methyl orange or phenolphthalein
endpoint

Wrong. Acidity is the property of an acid. yes, you can titrate a
solution, usually to determine it's molar concentration of an acid. you can
also do this with bases (but you need a different indicator and titrant).

> I said you can raise the pH by blowing of the CO2.

I know what you said, I didn't delete the posts. Lets go over what you said
again:

> 1.) If you have high CO2 and add an airstone it will drive the CO2 off
raising the pH.
> 2.) CO2 is produced by normal biological activity and is the resaon
behind many low pH's in tanks, as is room air CO2

Why in one case does CO2 from air lower pH and in the other case it raises
it? Doesn't make sense.

I know very well that co2 will lower pH, I am not arguing this point.

> Take note at the same temp and pH as the salinity falls there is an
increase in the CO2 and increase in the HCO3 and decrease in CO3.

Yep, that goes back to the Henderson-Haaselback equation. Very good.

> Please get out of those "general" chemistry books .

Now you are making me laugh. Most of my chem books are far form "general".

>If you did, we would not be having this debate but you would be agreeing
with me.

I do not agree with you because you have NOT convinced me. You never will
because your WRONG on MOST respects.

>And to disagree with me is to disagree with all the authors I posted above.

ALL MARINE BIOLOGIST. So I guess I disagree with them as well. Now what?
If you had any chem knowledge other than what you learned in Marine aquarium
books, you might be making more sense right now. Trust me.

>you may want to go there and do a search on me and what I know and don't
know.

Na, I'm not interested in you.

>No, I sure as hell don't know everything, we all make mistakes, as you have
here.

You have not convinced me that I have made any mistakes on the topic in
question.

>yours is a lack of understanding of seawater chemistry

Your is the lack of understanding very BASIC chemistry terms.

Such as pH, alkalinity and buffering capacity.

>Does CO2 have an effect on Alk, YES or NO. If you say yes, go back to the
books you have.
No, CO2 doesn't remove any of the buffer. It simply neutralizes some of it
as the system becomes more acidic. Alkalinity is a measure of BUFFERING
CAPACITY.

>This hobby is plagued with myths and misconceptions and I like to have
thing in order as what they really are.

You are partially to blame.

> So, so much for your Ph.D in chemistry :-)

I'm doing very well, thank you.

> I don't even have a degree in chemistry or biology.I don't need one to
understand it, you
> do and you are still lost.

Oh boy.

My posts speak for them selves. The laymen may not know the difference
between your junk posts and mine. That's to be expected.

Lets go back to some of your other posts you avoided explaining shall we?

>You can have all the alk you want in the world and it won't help, in
regards to CO2

WRONG.

One of your many definitions of alkalinity:
Alk is defined as;

TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
[HPO4--] +
2[PO4---] - [H+]

Those are COMPONENTS of BUFFERS. Are they not?












"Boomer" > wrote in message
...
> You are so funny you make me laugh, it is just a riot .
>
> I said seawater has very little buffering capacity, I did not say it had
very little Alk .
> What ever it is there is still a % of x ,y and z that make it up.You are
sill confusing
> Buffering Capacity and Alk, so I would suggest to give it up as you are
clueless
>
> "Downwards trends of what? Acidity? Basicity? "
>
> Alkalinity is the ability to slow down or inhibit downward trends in pH. I
think you are
> smart enough to know what a downward trend in pH is correct, as in
lowering the pH. ?
> Acidity is the ability to inhibit or slow down upward trends in pH, or to
slow down
> rising pH. It is only **common sense ** there is an opposite to
Alkalinity, which is
> Acidity
>
> "Have I ever heard of an
> acidity test? "
>
> Well, then you don't know much about water chemistry.
>
> Acidity = A std alkali titration to methyl orange or phenolphthalein
endpoint
>
> Alkalinity = A std acid titration to phenolphthalein endpoint
>
>
>
> Well, then you don't know much. Please consult a water chemistry book, I
DID NOT POST
> AQUARIUM BOOKS. I posted college and graduate level seawater chemistry
books, so it tells
> me just how much you don't know about water chemistry, let alone seawater
chemistry .Do
> search on those authors, forget it, as I have them. Please pay attention.
>
> An Introduction to the Chemistry of the Sea, by Michael E. Q. Pilson,
Ph.D. 432pages
> Graduate School of Oceanography
> University of Rode Island
>
> Chemical Oceanography, by Frank J.Millero, Ph.D, 531 pages
> Rosenstiel School of Marine and Atmospheric Science.
> University of Miami.
>
> Introduction to Marine Chemistry, J.P Riley,Ph.D, 465 pages.
> Department of Oceanography, University of Liverpool, England
>
> Chemical Oceanography Vol 2, by J.P Riley, Ph.D and G Skirrow,Ph.D, 712pag
es
> Same for Riley above.
> Skirrow
> Department of Inorganic, Physical and Industrial Chemistry
> University of Liverpool. England
>
> Practice Handbook of Marine Science, Michael J. Kennish, Ph.D
> Senior Environmental Scientist
> GPU Nuclear Corporation and
> Professor of Fisheries and Aquaculture, Rutgers University.
>
> Seawater: its Composition, Properties and Behavior,. Staff, Open
University, 165 pages
>
> Seawater Aquariums: The Captive Environment, by Stephen Spotte,Ph.D, 413
pages
> Vice President, Sea Research Foundation and Director Mystic Marinelife
Aquarium
> ( this is not a so called "aquarium book", it is a very advanced textbook)
>
> Please consult the graduate level text book, high on theory and
application, by J.F.
> Pankow, Ph.D. Aquatic Chemistry Concepts. Chapter 8 is on Buffering
Capacity and Chapter 9
> deals with Alkalinity and Acidity. Hum, if they are the same, why then are
they discussed
> separately and defined differently
>
> To continue with you lack of understanding.
>
> First, quite trying to twist thing as they suit you.
>
>
> "Ever heard of the Henderson-Hasselbach equation?"
>
> Yes, and you seem to have missed that they are also a faction of salinity
and temperature.
> Seawater "skews" the pKa1 and pKa2 to the left, giving LOWER values in
seawater.Almost any
> seawater text book gives those pKa's for seawater vs FW at x salinity and
temp. Buy the
> way just to show you where I am and where you are.Ever hear of ;
>
> pH(NIST), pH(NSW), pKa (NIST), pKa (NSW). Do you also know that in
seawater a pH meter
> does not give the proper value, it is called "salt error affect" and that
is what pKa
> (NSW). & pH(NSW), is all about.032
>
> Pilson gives s full pages of tables for pKa's from 0-40 C and 0 -40 ppt
Salinity. But I
> suppose he doesn't know what he is taking about.
>
> "Therefore, at a pH of 8.3 (seawater for this example) the majority of
> carbonate in solution exists as HCO3-2 not CO3-2"
>
>
> I never said the majority was as CO3, so where did that come from. Please
re-read what I
> said....here again ..you still need lots of help
>
> @ 20C and 34.3 ppt salinity
>
> CO2 = 0.52 %
>
> HCO3 = 86.4 %
>
> CO3 = 13.09 %
>
> so you aren't confused any more
>
>
> @ 20 C, pH 8.2 and 30.7ppt Salinity
>
> CO2 = .55 %,
>
> HCO3 = 87.8 %
>
> CO3 = 11.60 %
>
> Take note at the same temp and pH as the salinity falls there is an
increase in the CO2
> and increase in the HCO3 and decrease in CO3. So take your equation and
stick it.When
> dealing with seawater you MUST calculate pKa's differently more or less,
although you
> could use these for FW with a 0 salinity plugged in. For seawater the
pKa1;
>
> pK1* = pK1 + ( -840.39/T + 19.894 - 3.0189 lnT) S *1/2 + .00668S
>
> where
>
> pK1 =- 6320.81T - 126.3405 + 19.568 lnT
>
> Where T =temp in Kelvin and S =salinity in ppt and ln = natural log
>
> From
> Millero, 1992, Chemical Oceanography.
>
> "This is
> why this topic so muddied."
>
> Hum, you are the one today mudding it all up
>
> "You are saying seawater has no buffering capacity and you are saying 1/3
of
> seawaters Buffer Capacity is due to MgCO3 ??"
>
> I see you are still lost. It is about nil Buffering Capacity, which means
there is very
> little to stop upward or downward shifts in pH. If seawater was at a pH of
6 or 9 it would
> be very, very high Buffering Capacity and would be difficult to cause the
pH shifts up or
> down, as half of the buffer on either side of 6 of 9 is an acid and the
other half a base.
>
> "Oh, man. Interesting. Here is another contradiction of yours. You said
> before you purge CO2 from your tank with air to raise the pH. Here you
are
> telling me that CO2 from air is the reason behind many low pH.
>
> You are really lost aren't you and trying one of the Mr. Twister tactics.
>
> I said you can raise the pH by blowing of the CO2. Most of the CO2 in
water is not
> hydrated but is free CO2. There will always be some CO2 in the water. The
more there is
> the easier it is to purge off . Not ALL tanks have excess CO2. The more
there is the
> higher the pH will rise if you blow it off. Many aquariums have excess
CO2, from normal
> biological activity, which can/will lower the tank pH ( nothing to do with
air). It is a
> common problem in this hobby. Others often think they have tank CO2
problems, when the
> real issue is not CO2 generation in the tank but have very low tank CO2.
It is high room
> air CO2, which can be quite high, especially in the winter, much more so
than the tank, so
> it can diffuses much easier into the tank water, giving the false idea
they have excess
> load problems producing CO2, when they actually don't and lowering the pH
..Using outside
> air CO2 will greatly reduce this problem. Some tanks have higher CO2
tanks others which
> may be low or maybe some are in the middle. Tanks with large amounts of
plants will
> usually suck up all the CO2 and begin to feed of the HCO3 and CO3 for
their C needs, which
> will raise the pH. FOT usually have excess CO2. Having a party in your
house by itself can
> lower the pH of your tank do excess room air CO2 build-up. It all depends
on the
> circumstances of the tank, the room air, the bio-load, skimming and even
the type of
> animals and plants.
>
> Please get out of those "general" chemistry books and check a water,
aquatic or seawater
> chemistry book, before you speak about something you don't know. If you
did, we would not
> be having this debate but you would be agreeing with me. And to disagree
with me is to
> disagree with all the authors I posted above. By the way, feel free to
contact or e-mail
> Dr. Frank J, Millero. Here is his website. I have talked to him a number
of times in the
> past on these issues.
>
> http://www.rsmas.miami.edu/groups/jmc/fla-bay/fbay.html
>
> By the way there is always a link below my name, you may want to go there
and do a search
> on me and what I know and don't know. No, I sure as hell don't know
everything, we all
> make mistakes, as you have here.
>
> Articles by;
> Dr. Randy Holmes-Farely (Harvard graduate chemist) and Dr. Craig Bingman
from Columbia
> University, Department of Chemistry ( he runs the lab there last time I
checked) Please
> review Randy's credentials, as you like them things :-)
>
> One finally note or question to see where you are. Does CO2 have an effect
on Alk, YES or
> NO. If you say yes, go back to the books you have.
>
> From your last post;
>
> "The equilibrium will
> be shifted to HCO3-2 by a ratio of 1:100."
>
> No it won't, that is for freshwater NOT seawater, how many time do I have
to tell you that
>
> "Based on what I have read of his posts thus far, I wouldn't recommend
that
> to anyone."
>
> Hum, we all know that it is me and not you that knows their P's & Q's. I
have info and all
> that data to back me yup, yours is a lack of understanding of seawater
chemistry and the
> issues at hand .I have posted this info on many forums, to include here,
where Craig
> Bingman use to come often. To include on the Reef Chemistry Forum at RC,
none have
> challenged what I said and many are chemists with Ph.D's.
>
> Finally
>
> But I know what
> you mean, man*y use the term ALK and BC interchangeably.
>
> I said this as many do but it is incorrect from a chemical point but I
understand what you
> mean. Many in this hobby say Alk in one breath and buffering capacity in
another breath,
> technically they are not the same as I have defined in words and
equations.This hobby is
> plagued with myths and misconceptions and I like to have thing in order as
what they
> really are.
>
> So, so much for your Ph.D in chemistry :-)
>
> I don't even have a degree in chemistry or biology.I don't need one to
understand it, you
> do and you are still lost.
>
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message
news:8mQVb.212632$nt4.990652@attbi_s51...
> : >Alkalinity only deals with downward trends and says nothing of upward
> : trends. Ever hear of an Acidity test kit ?
> :
> : Downwards trends of what? Acidity? Basicity? Have I ever heard of an
> : acidity test? Yeah, it's called pH paper. or a pH meter.
> :
> : > As far as primary "buffers" in seawater you are lost again. The
principle
> : buffers of seawater are HCO3, CO3.
> :
> : Ever heard of the Henderson-Hasselbach equation?
> :
> : pH = pKa + log [HA]/[A-]
> :
> : The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this
example)
> : you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium
will
> : be shifted to HCO3-2 by a ratio of 1:100.
> :
> : 8.3 = 10.3 + log [HCO3-2]/[CO3-2]
> : -2 = log [HCO3-2]/[CO3-2]
> :
> : take antilog of both sides and you get:
> :
> : .01 = [HCO3-2]/[CO3-2]
> :
> : Therefore, at a pH of 8.3 (seawater for this example) the majority of
> : carbonate in solution exists as HCO3-2 not CO3-2. That is why I did not
> : include it in my buffer example.
> :
> : You said:
> : >The principle buffers of seawater are HCO3, CO3 and B(OH4).
> :
> : and You said in a previous post:
> :
> : >For all practically purposes seawater has very little Buffering
Capacity,
> : if any at all.
> :
> : STOP contradicting yourself, you are confusing the matter for yourself
and
> : others. How can HCO3, CO3 and B(OH4) be buffers in seawater if "For
all
> : practically purposes seawater has very little Buffering Capacity" AND if
> : "About 1/3 of seawaters Buffer Capacity is due to MgCO3" ?????
> :
> : You are saying seawater has no buffering capacity and you are saying 1/3
of
> : seawaters Buffer Capacity is due to MgCO3 ??
> :
> : Are you on drugs? Just kidding. I just want to help you understand.
> :
> : Can I make a suggestion for you? Stop getting your chemistry knowledge
from
> : aquarium books. Most are written by Marine Biologists, not CHEMISTS,
like
> : myself. I have seen NUMEROUS chemistry flaws in aquarium books. This
is
> : why this topic so muddied.
> :
> : > It does work it is not a maybe. Intentionally !!!!! where are you
coming
> : from or where
> : > have you been ??? CO2 is produced by normal biological activity and is
the
> : reason behind
> : > many low pH's in tanks, as is room air CO2
> :
> : Oh, man. Interesting. Here is another contradiction of yours. You
said
> : before you purge CO2 from your tank with air to raise the pH. Here you
are
> : telling me that CO2 from air is the reason behind many low pH's.
> :
> :
> : > pKa1 = 6.0 pKa2 = 9.1
> : > From Introduction to Marine Chemistry by Riley and Chester. Also from,
An
> : Introduction to the Chemistry of the Sea, by Pilson
> :
> : STOP GETTING YOUR CHEMISTRY FROM AQUARIUM BOOKS. Get a CHEMISTRY book.
> :
> : > Well go get some, as you need it, that is for sure.
> :
> : Not likely.
> :
> :
> :
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > <Alkalinity is buffering capacity. >
> : >
> : > No it is not, they are not calculated the same. I already gave the
> : equations please, you
> : > seem to avoiding them. Please consult an aquatic chemistry book.
> : >
> : > ">But I know what you mean, many use the term ALK and BC
interchangeably"
> : >
> : > Yes, I most certainly do and stated it is incorrect but I know what
you
> : mean
> : >
> : >
> : > <If you believe that
> : > alkalinity and buffering capacity can be used interchangeably than I
must
> : be
> : > getting through to you.>
> : >
> : > Please don't make me laugh. No I'm not getting through
> : >
> : >
> : > <Which are used in the over all 'buffering capacity'. Are we
> : > going in circles here? Anyway, I think you are learning something>
> : >
> : > No I'm not learning anything but you need to. No I'm not talking in a
> : circle but maybe you
> : > are. You must have missed it, so here it is again. Buffer capacity is
the
> : ability to with
> : > stand upward & downward trends in pH. Alkalinity only deals with
downward
> : trends and says
> : > nothing of upward trends. Ever hear of an Acidity test kit ?
> : >
> : > <This is the 'primary buffer' in sea water:>
> : >
> : > H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1"
> : >
> : > You are lost, the reaction that it is inherent to is;........... and
you
> : are missing some
> : > things
> : >
> : > 2HCO3 <--->CO2 + H20 + ***CO3***
> : >
> : >
> : > As far as primary "buffers" in seawater you are lost again. The
principle
> : buffers of
> : > seawater are HCO3, CO3 and
> : > B(OH4). I might add that Ion pairs are also part of the Buffer
Capacity.
> : About 1/3 of
> : > seawaters Buffer Capacity is due to MgCO3. Like I said you don't
> : understand Buffer
> : > Capacity and Alkalinity. Seawater manuals and text books are filled
with
> : this kind of
> : > data.Would you like me to give a list of some ?? :-)
> : >
> : > "If you REALLY believe that sea water has little buffering capacity,
than
> : you
> : > need to do some reading on your own. I wont be able to convince you."
> : >
> : > It doesn't if you understand the issue and it is quite clear you
don't.
> : You are the one
> : > that need to do allllllllllllot of reading
> : >
> : > ***For terms are commonly used to describe various aspects of the
seawater
> : buffer system:
> : >
> : > 1.pH
> : >
> : > 2. Buffering Capacity
> : >
> : > 3. Alkalinity or Total Alkalinity
> : >
> : > 4. Carbonate Alkalinity***
> : >
> : > From;
> : > Spotte, Seawater Aquariums the Captive Environment ( a technical text
book
> : on seawater and
> : > seawater aquariums)
> : >
> : >
> : > ***In seawater, for example, maximum Buffering Capacity appears at pH
> : values near 6 and 9
> : > and seawater is buffered very little , if at all, at its normal pH of
> : 8.2***
> : >
> : > From;
> : > Skirrow, 1975 Chemical Oceanography Vol 2
> : >
> : > <but
> : > carbonic acid (the primary buffering component in seawater) >
> : >
> : > Bicarbonate is the primary buffer not carbonic acid ,where on God's
earth
> : did you get that
> : > from. At normal temp, salinity, pH and Alk it is;
> : >
> : > @ 20C and 34.3 ppt salinity
> : >
> : > CO2 = 0.52 %
> : >
> : > HCO3 = 86.4 %
> : >
> : > CO3 = 13.09 %
> : >
> : > From;
> : > Practical Handbook of Marine Science, M.J. Kennish
> : >
> : > <Therefore, it has two pKa's
> : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
> : The
> : > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated
is
> : > right in there. Is that magic? :)>
> : >
> : > Magic !!!! it must be by your account. That is FW there pal, not
> : seawater, lets get the
> : > water straight here that we are dealing with, so you aren't so lost.
> : >
> : > The;
> : > pKa1 = 6.0
> : >
> : > pKa2 = 9.1
> : >
> : > From;
> : > Introduction to Marine Chemistry by Riley and Chester. Also from, An
> : Introduction to the
> : > Chemistry of the Sea, by Pilson
> : >
> : > So your equation does not work as you gave it.
> : >
> : > (6.0 + 9.1) / 2 = 7.55 pH Hum, maybe you would care to explain that
> : since you seem to
> : > think you have all the answers.
> : >
> : > <Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What
is
> : your
> : > point here?>
> : >
> : > It means that if the pH is 8.3 and the Alk is 4.0 meq/ l or if the is
pH
> : 8.3 and the Alk
> : > 1.5 Meq /l, or no mater what the Alk level is, if the pH is the same,
the
> : ratio's of CO2
> : > to HCO3 to CO3 will be the same. So you are not lost here :-)
> : >
> : > pH = 8.2
> : >
> : > Alk = 4.0 meq /l
> : >
> : > or
> : >
> : > pH = *.2
> : >
> : > Alk = 1.5 meq /
> : >
> : > The percentage or ratio is still the same for both, both will be .
0.52%
> : CO2, 86.4 % HCO3
> : > and 13.09 % @ 34.3 ppt and @ 20 C
> : >
> : > <Yeah, I guess that would work. If you intentionally put the CO2 in
> : > there to begin with because you must have a higher concentration of
CO2 in
> : > your tank than in the atmosphere. I don't intentionally put CO2 in my
> : tank>
> : >
> : > It does work it is not a maybe. Intentionally !!!!! where are you
coming
> : from or where
> : > have you been ??? CO2 is produced by normal biological activity and is
the
> : resaon behind
> : > many low pH's in tanks, as is room air CO2
> : >
> : > <you must have a higher concentration of CO2 in
> : > your tank than in the atmosphere>
> : >
> : > What !!! CO2 does not have to be higher than ambient air .Quite often
CO2
> : is produced in
> : > the water and can't leave fast enough, has one would normally expect ,
by
> : simple diffusion
> : > to the atmosphere. It is the reason why CO2 can get so high in almost
any
> : aquatic system
> : > and is the same reason CO2 can get so low. Why do you think Planted FW
> : Aquarium guys use
> : > CO2 injection ? As the plants can remove the CO2 faster than it can
> : diffuse across the
> : > water air interface. Same for a FOT, the CO2 can accumulate faster
than it
> : can diffuse,
> : > thus crashing the pH
> : >
> : > <Not interested. I can find my own software to do this too.>
> : >
> : > Well go get some, as you need it, that is for sure.
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : > "stoutman" <.@.> wrote in message
> : news:SFNVb.204571$Rc4.1681932@attbi_s54...
> : > : Oh brother. Where to start.
> : > :
> : > : pH is the -log of the hydronium ion concentration. When the
hydronium
> : ion
> : > : concentration is very low, your system is basic (high pH). When the
> : > : hydronium ion concentration is very large, your system is acidic
(low
> : pH).
> : > :
> : > : pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice
> : versa.
> : > : But a pH of < 7 means acidic. pH > 7 means basic.
> : > : pH can tell you something about acidity and basicity. It is a
> : measurement
> : > : of both, or the entire pH scale (1-14) if you will.
> : > :
> : > : >It is called "blowing it off" , such as with an airstone. If you
have
> : high
> : > : CO2 and add an airstone it will drive the CO2 off raising the pH.
> : > :
> : > : Ok, you are going to try and 'purge' (the correct term) your CO2 out
> : with
> : > : air. Yeah, I guess that would work. If you intentionally put the
CO2
> : in
> : > : there to begin with because you must have a higher concentration of
CO2
> : in
> : > : your tank than in the atmosphere. I don't intentionally put CO2 in
my
> : tank.
> : > : But I know some of you reef people due in Kalk reactors.
> : > :
> : > : >If Alk resists changes in pH then why does CO2 lower the pH without
> : > : affecting the Alk.
> : > :
> : > : Alkalinity is buffering capacity. Your buffers begin to get
weakened
> : with
> : > : the addition of acid until they reach a point when they can no
longer
> : > : 'buffer' and the pH crashes.
> : > :
> : > : >But I know what you mean, may use the term ALK and BC
interchangeably
> : > :
> : > : Do you remember writing this in an earlier post? If you believe
that
> : > : alkalinity and buffering capacity can be used interchangeably than I
> : must be
> : > : getting through to you.
> : > :
> : > : >When CO2 is added or remove it just changes the ratio of
CO2:HCO3:CO3.
> : At
> : > : any pH no matter what the Alk or CO2 there will be an exact ratio of
> : > : CO2:HCO3:CO3
> : > :
> : > : Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What
is
> : your
> : > : point here?
> : > :
> : > : > Go ahead and pick a seawater pH and I will tell you what that
ratio
> : is.
> : > : Tell me the pH and
> : > : > Alk and I will give the CO2 concentration. Give me the Alk and
CO2
> : and I
> : > : will give you
> : > : > the pH. Don't forget the temperature and Salinity.
> : > :
> : > : Not interested. I can find my own software to do this too.
> : > :
> : > : > Alk is defined as;
> : > : >
> : > : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] +
[MgOH+] +
> : > : [HPO4--] +
> : > : > 2[PO4---] - [H+]
> : > :
> : > : Ahh, now we are getting somewhere. What you are showing are
components
> : of a
> : > : 'BUFFER'. Which are used in the over all 'buffering capacity'. Are
we
> : > : going in circles here? Anyway, I think you are learning something.
> : > :
> : > : > In any aqueous solution maximum BC is reached when pH= pKa.
Seawaters
> : > : maximum BC is at a
> : > : > pH of 6 & 9. For all practically purposes seawater has very little
> : > : Buffering Capacity, if
> : > : > any at all.
> : > :
> : > : This is the 'primary buffer' in sea water:
> : > :
> : > : H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
> : > :
> : > : If you REALLY believe that sea water has little buffering capacity,
than
> : you
> : > : need to do some reading on your own. I wont be able to convince
you.
> : > :
> : > : > In any aqueous solution maximum BC is reached when pH= pKa.
Seawaters
> : > : maximum BC is at a
> : > : > pH of 6 & 9. For all practically purposes seawater has very little
> : > : Buffering Capacity, if
> : > : > any at all.
> : > :
> : > : This would be true if a monoprotic acid where used in the 'buffer',
but
> : > : carbonic acid (the primary buffering component in seawater) is a
> : polyprotic
> : > : acid. It has two protons that can dissociate. Therefore, it has
two
> : pKa's
> : > : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH =
8.35.
> : The
> : > : pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated
is
> : > : right in there. Is that magic? :)
> : > :
> : > : Remember that seawater is more than a mixture of just carbonate and
CO2,
> : > : there are other buffers involved that make it even more complicated
I'm
> : > : sure.
> : > :
> : > : > By the way do you know who you are talking to ?
> : > :
> : > : No. Do you?
> : > :
> : > :
> : > :
> : > :
> : > : "Boomer" > wrote in message
> : > : ...
> : > : > Let me make this clear you don't know what you are taking about
> : > : >
> : > : > "alkalinity is a measurement of 'buffering capacity'"
> : > : >
> : > : > No, it is the ability to neutralize an acid. BC is the ability to
> : > : withstand both upward
> : > : > and downward trends in pH.
> : > : >
> : > : > "pH is a measurement of 'acidity/basicity'.
> : > : >
> : > : > No, pH is a measurement of acidity and pOH is a measurement of
> : Basicity,
> : > : if you want to
> : > : > get picky, which seems you do.
> : > : >
> : > : >
> : > : > "How do you remove CO2? "
> : > : >
> : > : > It is called "blowing it off" , such as with an airstone. If you
have
> : high
> : > : CO2 and add an
> : > : > airstone it will drive the CO2 off raising the pH. It can be
proven
> : with a
> : > : glass of water,
> : > : > a straw, some pH color indicator and an Alk test kit and if you
must a
> : CO2
> : > : test kit
> : > : >
> : > : > >You can have all the alk you want in the world and it won't help,
in
> : > : > regards to CO2
> : > : >
> : > : > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
> : changes
> : > : in
> : > : > pH. This is what is meant by 'buffering capacity'"
> : > : >
> : > : > No you are wrong and very lost. If Alk resists changes in pH then
why
> : does
> : > : CO2 lower the
> : > : > pH without affecting the Alk ? CO2 has no effect on alk and alk
has no
> : > : effect on CO2. When
> : > : > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3.
At
> : any
> : > : pH no matter what
> : > : > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> : > : >
> : > : > .
> : > : > Go ahead and pick a seawater pH and I will tell you what that
ratio
> : is.
> : > : Tell me the pH and
> : > : > Alk and I will give the CO2 concentration. Give me the Alk and
CO2
> : and I
> : > : will give you
> : > : > the pH. Don't forget the temperature and Salinity.
> : > : >
> : > : > Alk is defined as;
> : > : >
> : > : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] +
[MgOH+] +
> : > : [HPO4--] +
> : > : > 2[PO4---] - [H+]
> : > : >
> : > : >
> : > : > Buffering Capacity is defined as;
> : > : >
> : > : > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
> : [H3O+])²
> : > : >
> : > : > In any aqueous solution maximum BC is reached when pH= pKa.
Seawaters
> : > : maximum BC is at a
> : > : > pH of 6 & 9. For all practically purposes seawater has very little
> : > : Buffering Capacity, if
> : > : > any at all.
> : > : >
> : > : >
> : > : > Alkalinity and Buffer Capacity are closely tied but are NOT the
same
> : > : thing, it is a
> : > : > misunderstanding and use of the term. Do you think water chemistry
> : books
> : > : would have
> : > : > separate sections on Alkalinity and Buffering Capacity if they
were
> : the
> : > : same thing ?
> : > : >
> : > : > By the way do you know who you are talking to ?
> : > : >
> : > : > --
> : > : > Boomer
> : > : >
> : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : >
> : > : > Want to See More ?
> : > : > Please Join Our Growing Membership
> : > : > www.coralrealm.com
> : > : >
> : > : > If You See Me Running You Better Catch-Up
> : > : >
> : > : >
> : > :
> : > :
> : >
> : >
> :
> :
>
>

[stoutman]

Boomers very first post in this thread:

>If CO2 increases the pH will drop, no mater what the Alk is.

A later post made by Boomer:

>Alkalinity is the ability to slow down or inhibit downward trends in pH.

With the exception of CO2?









"Boomer" > wrote in message
...
> No, I don't write anything. I explain things to people such as yourself
that don't
> understand the issue.
>
>
> "By the way do you know who you are talking to ?"
>
> This was more on the order of a joke to get your attention. I have been
around about 35
> years. I also get a real charge of people like yourself , that come here
or forums and
> toot your BS, assuming you must be right and we are all idiots lol
>
> "Someone is a little pompous"
>
> Now here we go with the name calling. I can see where you are coming from,
does it make
> you feel better or do you think that makes you correct. It is rather
childless don't you
> think ?
>
> If I did you would be the last , as you are way to lost on seawater
chemistry
>
> What's interesting and I'm sure to everyone it is, the big hole you just
keep digging for
> yourself. lol
>
> You must be nervous, you sure seem be bothered by these post and my
drilling you with info
> from refs, Seawater Chemistry books, written by seawater chemists. I must
make you look
> bad,Ph.D and all :-) I think Millero has been at it about 40 years and
has written 3
> advanced textbooks on chemical oceanography. Hum, you may also want to
check out Stumm &
> Morgan .Of course there are others, i.e Morel, Benjamin(the newest water
chemistry book
> 2002) and lets not forget the "old great book" by Snoeyink and Jenkins,
still in print. I
> have them all :-)
>
> A smart guy MAY want to go look at my ref, especially a Ph.D chemist such
as yourself :-)
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message news:EfSVb.12701$QA2.22009@attbi_s52...
> : >By the way do you know who you are talking to ?
> :
> : This cracks me up. Someone is a little pompous. I gather from the
> : responders in this thread that Boomer is some kind of self proclaimed
> : aquarium guru.
> :
> : I can only assume that he is a Marine Biologist that needs to take a few
> : more chemistry courses. Boomer, if you are an author of aquarium
> : literature, than I would like to be acknowledged in your next manuscript
for
> : helping you see the light.
> :
> : I too can be pompous.
> :
> : -Stoutman
> :
> :
> :
> :
> :
> :
> :
> :
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > Let me make this clear you don't know what you are taking about
> : >
> : > "alkalinity is a measurement of 'buffering capacity'"
> : >
> : > No, it is the ability to neutralize an acid. BC is the ability to
> : withstand both upward
> : > and downward trends in pH.
> : >
> : > "pH is a measurement of 'acidity/basicity'.
> : >
> : > No, pH is a measurement of acidity and pOH is a measurement of
Basicity,
> : if you want to
> : > get picky, which seems you do.
> : >
> : >
> : > "How do you remove CO2? "
> : >
> : > It is called "blowing it off" , such as with an airstone. If you have
high
> : CO2 and add an
> : > airstone it will drive the CO2 off raising the pH. It can be proven
with a
> : glass of water,
> : > a straw, some pH color indicator and an Alk test kit and if you must a
CO2
> : test kit
> : >
> : > >You can have all the alk you want in the world and it won't help, in
> : > regards to CO2
> : >
> : > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
changes
> : in
> : > pH. This is what is meant by 'buffering capacity'"
> : >
> : > No you are wrong and very lost. If Alk resists changes in pH then why
does
> : CO2 lower the
> : > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
> : effect on CO2. When
> : > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
any
> : pH no matter what
> : > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> : >
> : > .
> : > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> : Tell me the pH and
> : > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and I
> : will give you
> : > the pH. Don't forget the temperature and Salinity.
> : >
> : > Alk is defined as;
> : >
> : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> : [HPO4--] +
> : > 2[PO4---] - [H+]
> : >
> : >
> : > Buffering Capacity is defined as;
> : >
> : > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
[H3O+])²
> : >
> : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> : maximum BC is at a
> : > pH of 6 & 9. For all practically purposes seawater has very little
> : Buffering Capacity, if
> : > any at all.
> : >
> : >
> : > Alkalinity and Buffer Capacity are closely tied but are NOT the same
> : thing, it is a
> : > misunderstanding and use of the term. Do you think water chemistry
books
> : would have
> : > separate sections on Alkalinity and Buffering Capacity if they were
the
> : same thing ?
> : >
> : > By the way do you know who you are talking to ?
> : >
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : >
> : >
> :
> :
>
>

[Bill Kirkpatrick]

Guys, guys, isn't this group "rec..."?

While all this is surely "recreational" in a chemical sort
of way, the rest of the group's naming suggests that
"...aquaria.marine.reefs" is the topic in which we are,
generally, focusing on said recreation.

While I love to watch a good debate, particularly around
random theoretical values of "drop", poor Dinky was asking
for an explanation in "Aquaria for idiots" fashion.

Maybe the typical, if hidiously flawed, high school
explanation might serve? One limited to a world view where
Dinky's $5.00 LFS test kits are the definitive science?

(Sorry, Dinky, if I've impugned the honor of your test kits.)

********************************
stoutman wrote:
> Boomers very first post in this thread:
>
>
>>If CO2 increases the pH will drop, no mater what the Alk is.
>
>
> A later post made by Boomer:
>
>
>>Alkalinity is the ability to slow down or inhibit downward trends in pH.
>
>
> With the exception of CO2?
>

[Boomer]

I see you are lost case. It is really bad one someone is incorrect and they try to find a
way to escape


"Agreed. This is an effect of 'buffering"

Agreed, that is "buffering" not Buffering Capacity as defined by the equation I gave from;

Analytical Chemistry, by Robert.V Dilts, Ph.D
Department of Chemistry, Vanderbilt University.

I guess he is also clueless as is Pankow. Dr. Pankow being one of the worlds foremost
Aquatic Chemists.

"Oh wait, you have another definition of alkalinity"

I think you are a nut case. That is how Alk is tested. It is tested by titration with a
std acid to phenolphthalein (P) or Total (T) alkalinity endpoint. Hydroxide determination
(OH) uses Barium pretreatment to eliminate carbonate interference.

"Believe me, I don't need to. I have plenty of chem books that cover the
topic quite well."

Then why all the mistakes ???

"> Acidity = A std alkali titration to methyl orange or phenolphthalein
endpoint>

That is how is tested, are you so clueless, that as a proclaimed Ph.D chemist, you don't
know that simple thing ???


"Wrong. Acidity is the property of an acid"

Hum, well then you can go argue with HACH and LaMotte, about how messed up they are on
their test kits, which follow EPA, NPDWR and NPDES testing procedures and those found in

Standard Methods for the Examination of Water and Wastewater

Acidity is a property of an acid, it is also the ability of a solution to slow down or
inhibit pH rises do to the presence or introduction of an Alkali substances. A higher
Acidity means you are less likely to increase the pH with the addition of a base. Just
like a higher Alkalinity is the ability you are less likely to lower the pH with the
addition of an acid. Get it !!!

.. "Why in one case does CO2 from air lower pH and in the other case it raises
it? Doesn't make sense."

Quite twisting things around to suit your fancy. I said CO2 from air can lower the pH and
if CO2 is in water it can driven off, via aeration, blown off, it will thus raise the pH.
Where did you get this "air lower pH and other air raises pH , I said no such thing as CO2
in air raises pH, get the facts straight, knock off the BS line.

Maybe I should explain it to you in Dick & Jane Terms. The Boomer Glass Trick, is quite
popular and always proves my point

First get two glasses and fill with sample water. Measure the pH and Alk Put some pH
indicator in one and not the other. In the indicator glass now blow in it with a straw,
magic the indicator changes to a lower pH. Now put in an airstone and boil the water and
watch the pH rise. Do the same to the other glass, you know the pH is going to go down.
Now after you blow, measure the Alk, it has not changed from the first measurement. Fauna
produce CO2, in which case the rate can rise faster than it can leave to the atmosphere.
Such increases in CO2 will drop the pH . Pretend your blowing is all that fauna in the
tank expelling CO2. The airstone, drives it of the CO2, in which case the ph of the glass
will go back up.If you aerate the indicator glass you will see the indicator go back to a
more base pH. CO2 goes very easy into water , but is a little harder to drive off, it
takes more time. Now as with the glass, pretend your tank water has high CO2 and you
aerate the water, what happens, the CO2 is driven of and the pH goes up. This is why good
circulation and agitation of the surface is important ......to drive off CO2. Now if the
house is high in CO2 it will have a much higher partial pressure and will be harder to
drive off. If it is high enough and the CO2 in-tank is low enough the CO2 will go right
into solution, increase and lower the pH I don't care what your Alk is.

You have lost it. All the books I posted are College chemistry books. Get off on your hype
of "marine aquarium". What kind of stunt are you trying to pull ? That we are all so dumb
we don't know who those authors are. They are all chemists, most that I posted are
Seawater Chemists. Go do a search on them, see what they write and where they write, where
they work sand what degree they have They don't write in aquarium books at all, so lets
get that straight.

"ALL MARINE BIOLOGIST. So I guess I disagree with them as well. Now what?
If you had any chem knowledge other than what you learned in Marine aquarium
books, you might be making more sense right now. Trust me"

Are you trying to get me or tell us that Dr. Frank Millero is Marine Biologist, what drugs
are you on. He is the worlds foremost Chemical oceanographer. That is a CHEMIST, just to
clue you in there pal. Before him it was Riley and Chester and others like Horne and
Harvey. Did you even go to Millero's website ? He has been teaching chemistry for 40 years
at the University of Miami, especially seawater chemistry.

Here let me help you with a quick search on just Millero;

http://www.google.com/search?hl=en&ie=UTF-8&oe=UTF-8&q=frank+J+Millero&btnG=Google+Search


Make sure you copy and paste it all

">You can have all the alk you want in the world and it won't help, in
regards to CO2

WRONG.

One of your many definitions of alkalinity:
Alk is defined as;

TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
[HPO4--] +
2[PO4---] - [H+]

Those are COMPONENTS of BUFFERS. Are they not?

Yes, those are components of buffers, not arguing that . You are confusing buffers with
Buffering Capacity and Alkalinity. As I stated before the two are very closely related as
they are also very closely related to Acidity.

From;

Dilts, Analytical Chemistry;

"The amount of ***acid or base that a buffer*** can consume is called Buffering Capacity
or Buffer Index. The capacity of a buffer solution is defined as the number of equivalents
of an acid or base that must be added to one liter of the buffer to cause a change in the
pH of the solution by one unit. Mathematically the capacity is measured by;

B = dCb / dpH = - dCa / dpH


Or as we have stated above, it is the change in the concentration of acid or of base per
pH unit.
given by

B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa [H3O+] / (Ka =
H3O+])² )

where C =[HA] + [A-] in the case of an acid and its conjugate, and C = [BH] + [B}when the
buffer is composed of a base and its conjugate. C represents the total concentration of
**both acid and conjugate base *** in the buffer system."

Alk tells you how much is added in meq / l, to bring the solution to a endpoint of about
a pH of 4.

By the way an few years ago two guys in FAMA were arguing the same thing as we are. I
called Dr. Frank Millero for an answer,which was. "The chemist was right the biologist was
wrong. Buffering Capacity and Alkalinity are not the same thing. Alkalify is the ability
to withstand only downward trends in pH and BC is the ability to withstand both upward
trends and downward trends in pH.You can calculate Alk if you know the BC.

Feel free to give him a buzz, read the statement above and see what kinda' answer you
get. Here is his phone number. Also, try and tell him the pKa's of seawater are 10.3 & 6.4
and the ratio is1 : 100 ratio of CO3-2 and HCO3-2, as you claim. Hum, Millero is the
leading authority on the seawater CO2/Carbonate System. Check some of his articles :-) It
is Millero that is always fine tuning seawater pKa's.

1-305-361-4707, University of Miami


Have a nice day, no sense in posting to you anymore till you get some facts straight.


Boomer


Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

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Please Join Our Growing Membership
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If You See Me Running You Better Catch-Up

[Boomer]

"With the exception of CO2?"

Yes that is correct. It is something many don't understand. CO2 is not an ion but a
molecule, it cares no charge.

TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
[HPO4--] +
2[PO4---] - [H+]


Hum, where is the CO2 here, hummmmm I can't find it.


Alk is a function of Ions and how they are affected by other charged ions. CO2 has no
effect on alk and vise versa. You seemed to have already acknowledged that. So what is the
point ? Or is it you think Alk is affected by CO2 or vise-versa. I invite you to our Chem
Forum, full of chemists, ask the question and see what kind of answers you get or just
call Millero.

Nuff said

--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
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If You See Me Running You Better Catch-Up
"stoutman" <.@.> wrote in message news:NIUVb.13104$QA2.22029@attbi_s52...
: Boomers very first post in this thread:
:
: >If CO2 increases the pH will drop, no mater what the Alk is.
:
: A later post made by Boomer:
:
: >Alkalinity is the ability to slow down or inhibit downward trends in pH.
:
: With the exception of CO2?
:
:
:
:
:
:
:
:
:
: "Boomer" > wrote in message
: ...
: > No, I don't write anything. I explain things to people such as yourself
: that don't
: > understand the issue.
: >
: >
: > "By the way do you know who you are talking to ?"
: >
: > This was more on the order of a joke to get your attention. I have been
: around about 35
: > years. I also get a real charge of people like yourself , that come here
: or forums and
: > toot your BS, assuming you must be right and we are all idiots lol
: >
: > "Someone is a little pompous"
: >
: > Now here we go with the name calling. I can see where you are coming from,
: does it make
: > you feel better or do you think that makes you correct. It is rather
: childless don't you
: > think ?
: >
: > If I did you would be the last , as you are way to lost on seawater
: chemistry
: >
: > What's interesting and I'm sure to everyone it is, the big hole you just
: keep digging for
: > yourself. lol
: >
: > You must be nervous, you sure seem be bothered by these post and my
: drilling you with info
: > from refs, Seawater Chemistry books, written by seawater chemists. I must
: make you look
: > bad,Ph.D and all :-) I think Millero has been at it about 40 years and
: has written 3
: > advanced textbooks on chemical oceanography. Hum, you may also want to
: check out Stumm &
: > Morgan .Of course there are others, i.e Morel, Benjamin(the newest water
: chemistry book
: > 2002) and lets not forget the "old great book" by Snoeyink and Jenkins,
: still in print. I
: > have them all :-)
: >
: > A smart guy MAY want to go look at my ref, especially a Ph.D chemist such
: as yourself :-)
: > --
: > Boomer
: >
: > Want to talk chemistry ? The Reef Chemistry Forum
: > http://www.reefcentral.com/vbulletin/index.php
: >
: > Want to See More ?
: > Please Join Our Growing Membership
: > www.coralrealm.com
: >
: > If You See Me Running You Better Catch-Up
: > "stoutman" <.@.> wrote in message news:EfSVb.12701$QA2.22009@attbi_s52...
: > : >By the way do you know who you are talking to ?
: > :
: > : This cracks me up. Someone is a little pompous. I gather from the
: > : responders in this thread that Boomer is some kind of self proclaimed
: > : aquarium guru.
: > :
: > : I can only assume that he is a Marine Biologist that needs to take a few
: > : more chemistry courses. Boomer, if you are an author of aquarium
: > : literature, than I would like to be acknowledged in your next manuscript
: for
: > : helping you see the light.
: > :
: > : I too can be pompous.
: > :
: > : -Stoutman
: > :
: > :
: > :
: > :
: > :
: > :
: > :
: > :
: > :
: > :
: > :
: > :
: > : "Boomer" > wrote in message
: > : ...
: > : > Let me make this clear you don't know what you are taking about
: > : >
: > : > "alkalinity is a measurement of 'buffering capacity'"
: > : >
: > : > No, it is the ability to neutralize an acid. BC is the ability to
: > : withstand both upward
: > : > and downward trends in pH.
: > : >
: > : > "pH is a measurement of 'acidity/basicity'.
: > : >
: > : > No, pH is a measurement of acidity and pOH is a measurement of
: Basicity,
: > : if you want to
: > : > get picky, which seems you do.
: > : >
: > : >
: > : > "How do you remove CO2? "
: > : >
: > : > It is called "blowing it off" , such as with an airstone. If you have
: high
: > : CO2 and add an
: > : > airstone it will drive the CO2 off raising the pH. It can be proven
: with a
: > : glass of water,
: > : > a straw, some pH color indicator and an Alk test kit and if you must a
: CO2
: > : test kit
: > : >
: > : > >You can have all the alk you want in the world and it won't help, in
: > : > regards to CO2
: > : >
: > : > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
: changes
: > : in
: > : > pH. This is what is meant by 'buffering capacity'"
: > : >
: > : > No you are wrong and very lost. If Alk resists changes in pH then why
: does
: > : CO2 lower the
: > : > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
: > : effect on CO2. When
: > : > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
: any
: > : pH no matter what
: > : > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
: > : >
: > : > .
: > : > Go ahead and pick a seawater pH and I will tell you what that ratio
: is.
: > : Tell me the pH and
: > : > Alk and I will give the CO2 concentration. Give me the Alk and CO2
: and I
: > : will give you
: > : > the pH. Don't forget the temperature and Salinity.
: > : >
: > : > Alk is defined as;
: > : >
: > : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
: > : [HPO4--] +
: > : > 2[PO4---] - [H+]
: > : >
: > : >
: > : > Buffering Capacity is defined as;
: > : >
: > : > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
: [H3O+])²
: > : >
: > : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
: > : maximum BC is at a
: > : > pH of 6 & 9. For all practically purposes seawater has very little
: > : Buffering Capacity, if
: > : > any at all.
: > : >
: > : >
: > : > Alkalinity and Buffer Capacity are closely tied but are NOT the same
: > : thing, it is a
: > : > misunderstanding and use of the term. Do you think water chemistry
: books
: > : would have
: > : > separate sections on Alkalinity and Buffering Capacity if they were
: the
: > : same thing ?
: > : >
: > : > By the way do you know who you are talking to ?
: > : >
: > : > --
: > : > Boomer
: > : >
: > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > http://www.reefcentral.com/vbulletin/index.php
: > : >
: > : > Want to See More ?
: > : > Please Join Our Growing Membership
: > : > www.coralrealm.com
: > : >
: > : > If You See Me Running You Better Catch-Up
: > : >
: > : >
: > :
: > :
: >
: >
:
:

[stoutman]

This debate is over. If you want me to continue to explain this to you, I
want to be compensated. Do you have a PayPal account?



"Boomer" > wrote in message
...
> I see you are lost case. It is really bad one someone is incorrect and
they try to find a
> way to escape
>
>
> "Agreed. This is an effect of 'buffering"
>
> Agreed, that is "buffering" not Buffering Capacity as defined by the
equation I gave from;
>
> Analytical Chemistry, by Robert.V Dilts, Ph.D
> Department of Chemistry, Vanderbilt University.
>
> I guess he is also clueless as is Pankow. Dr. Pankow being one of the
worlds foremost
> Aquatic Chemists.
>
> "Oh wait, you have another definition of alkalinity"
>
> I think you are a nut case. That is how Alk is tested. It is tested by
titration with a
> std acid to phenolphthalein (P) or Total (T) alkalinity endpoint.
Hydroxide determination
> (OH) uses Barium pretreatment to eliminate carbonate interference.
>
> "Believe me, I don't need to. I have plenty of chem books that cover the
> topic quite well."
>
> Then why all the mistakes ???
>
> "> Acidity = A std alkali titration to methyl orange or phenolphthalein
> endpoint>
>
> That is how is tested, are you so clueless, that as a proclaimed Ph.D
chemist, you don't
> know that simple thing ???
>
>
> "Wrong. Acidity is the property of an acid"
>
> Hum, well then you can go argue with HACH and LaMotte, about how messed up
they are on
> their test kits, which follow EPA, NPDWR and NPDES testing procedures and
those found in
>
> Standard Methods for the Examination of Water and Wastewater
>
> Acidity is a property of an acid, it is also the ability of a solution to
slow down or
> inhibit pH rises do to the presence or introduction of an Alkali
substances. A higher
> Acidity means you are less likely to increase the pH with the addition of
a base. Just
> like a higher Alkalinity is the ability you are less likely to lower the
pH with the
> addition of an acid. Get it !!!
>
> . "Why in one case does CO2 from air lower pH and in the other case it
raises
> it? Doesn't make sense."
>
> Quite twisting things around to suit your fancy. I said CO2 from air can
lower the pH and
> if CO2 is in water it can driven off, via aeration, blown off, it will
thus raise the pH.
> Where did you get this "air lower pH and other air raises pH , I said no
such thing as CO2
> in air raises pH, get the facts straight, knock off the BS line.
>
> Maybe I should explain it to you in Dick & Jane Terms. The Boomer Glass
Trick, is quite
> popular and always proves my point
>
> First get two glasses and fill with sample water. Measure the pH and Alk
Put some pH
> indicator in one and not the other. In the indicator glass now blow in it
with a straw,
> magic the indicator changes to a lower pH. Now put in an airstone and boil
the water and
> watch the pH rise. Do the same to the other glass, you know the pH is
going to go down.
> Now after you blow, measure the Alk, it has not changed from the first
measurement. Fauna
> produce CO2, in which case the rate can rise faster than it can leave to
the atmosphere.
> Such increases in CO2 will drop the pH . Pretend your blowing is all that
fauna in the
> tank expelling CO2. The airstone, drives it of the CO2, in which case the
ph of the glass
> will go back up.If you aerate the indicator glass you will see the
indicator go back to a
> more base pH. CO2 goes very easy into water , but is a little harder to
drive off, it
> takes more time. Now as with the glass, pretend your tank water has high
CO2 and you
> aerate the water, what happens, the CO2 is driven of and the pH goes up.
This is why good
> circulation and agitation of the surface is important ......to drive off
CO2. Now if the
> house is high in CO2 it will have a much higher partial pressure and will
be harder to
> drive off. If it is high enough and the CO2 in-tank is low enough the CO2
will go right
> into solution, increase and lower the pH I don't care what your Alk is.
>
> You have lost it. All the books I posted are College chemistry books. Get
off on your hype
> of "marine aquarium". What kind of stunt are you trying to pull ? That we
are all so dumb
> we don't know who those authors are. They are all chemists, most that I
posted are
> Seawater Chemists. Go do a search on them, see what they write and where
they write, where
> they work sand what degree they have They don't write in aquarium books at
all, so lets
> get that straight.
>
> "ALL MARINE BIOLOGIST. So I guess I disagree with them as well. Now
what?
> If you had any chem knowledge other than what you learned in Marine
aquarium
> books, you might be making more sense right now. Trust me"
>
> Are you trying to get me or tell us that Dr. Frank Millero is Marine
Biologist, what drugs
> are you on. He is the worlds foremost Chemical oceanographer. That is a
CHEMIST, just to
> clue you in there pal. Before him it was Riley and Chester and others like
Horne and
> Harvey. Did you even go to Millero's website ? He has been teaching
chemistry for 40 years
> at the University of Miami, especially seawater chemistry.
>
> Here let me help you with a quick search on just Millero;
>
>
http://www.google.com/search?hl=en&ie=UTF-8&oe=UTF-8&q=frank+J+Millero&btnG=
Google+Search
>
>
> Make sure you copy and paste it all
>
> ">You can have all the alk you want in the world and it won't help, in
> regards to CO2
>
> WRONG.
>
> One of your many definitions of alkalinity:
> Alk is defined as;
>
> TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> [HPO4--] +
> 2[PO4---] - [H+]
>
> Those are COMPONENTS of BUFFERS. Are they not?
>
> Yes, those are components of buffers, not arguing that . You are confusing
buffers with
> Buffering Capacity and Alkalinity. As I stated before the two are very
closely related as
> they are also very closely related to Acidity.
>
> From;
>
> Dilts, Analytical Chemistry;
>
> "The amount of ***acid or base that a buffer*** can consume is called
Buffering Capacity
> or Buffer Index. The capacity of a buffer solution is defined as the
number of equivalents
> of an acid or base that must be added to one liter of the buffer to cause
a change in the
> pH of the solution by one unit. Mathematically the capacity is measured
by;
>
> B = dCb / dpH = - dCa / dpH
>
>
> Or as we have stated above, it is the change in the concentration of acid
or of base per
> pH unit.
> given by
>
> B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> where C =[HA] + [A-] in the case of an acid and its conjugate, and C =
[BH] + [B}when the
> buffer is composed of a base and its conjugate. C represents the total
concentration of
> **both acid and conjugate base *** in the buffer system."
>
> Alk tells you how much is added in meq / l, to bring the solution to a
endpoint of about
> a pH of 4.
>
> By the way an few years ago two guys in FAMA were arguing the same thing
as we are. I
> called Dr. Frank Millero for an answer,which was. "The chemist was right
the biologist was
> wrong. Buffering Capacity and Alkalinity are not the same thing. Alkalify
is the ability
> to withstand only downward trends in pH and BC is the ability to withstand
both upward
> trends and downward trends in pH.You can calculate Alk if you know the BC.
>
> Feel free to give him a buzz, read the statement above and see what
kinda' answer you
> get. Here is his phone number. Also, try and tell him the pKa's of
seawater are 10.3 & 6.4
> and the ratio is1 : 100 ratio of CO3-2 and HCO3-2, as you claim. Hum,
Millero is the
> leading authority on the seawater CO2/Carbonate System. Check some of his
articles :-) It
> is Millero that is always fine tuning seawater pKa's.
>
> 1-305-361-4707, University of Miami
>
>
> Have a nice day, no sense in posting to you anymore till you get some
facts straight.
>
>
> Boomer
>
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
>
>

[stoutman]

Ok, Im bored, I will give you a free response.

> Agreed, that is "buffering" not Buffering Capacity as defined by the
equation I gave from;

Don't the components of a buffer account for the buffering capacity? Yes.

>It is tested by titration with a std acid to phenolphthalein (P) or Total
(T) alkalinity endpoint. Hydroxide determination (OH) uses Barium
pretreatment to eliminate carbonate interference.

I know how to do a titration, In fact I have done several. How many have
you actually done? I don't mean by counting drops, I mean with a buret?

> Then why all the mistakes ???

You must be referring to your mistakes.

> "> Acidity = A std alkali titration to methyl orange or phenolphthalein
> endpoint

Acidity is simply the opposite of basicity. To increase acidity you lower
the pH by adding more acid to the solution. To increase the basicity, you
add more base effectively increasing the pH.

You can measure the basicity and acidity of a solution by determining it's
pH.

> Acidity is a property of an acid, it is also the ability of a solution to
slow down or
> inhibit pH rises do to the presence or introduction of an Alkali
substances.

Wrong. Acidity has nothing to do with buffering. See above. Oh, I see,
you think acidity is the opposite of alkalinity. In the world of CHEMISTRY
it's not. Maybe in aquarium newsgroups it is.

In your Boomer water experiment, the blowing into the glass drops the pH
because of the CO2:

CO2(g) <------> CO2(aq) + H2O <--(1)----> H2CO3 <--(2)----> HCO3-1 + H3O
<---(3)----> CO3-2 + 2H3O

These are all in equilibrium with each other. An initial high pH (above
6.4) will shift the equilibrium to the right to form HCO3-1. If the pH of
the solution is above 10.3 (pKa2) the equilibrium will be shifted even
further to CO3-2. In the aquarium (pH = 8-8.5) the equilibrium is shifted
towards HCO3-1. At this pH it will be VERY difficult to purge out CO2 with
air. If you lower the pH to below 6.4, most of the CO2(aq) will be in the
form of H2CO3. At this point the H2CO3 is in equilibrium with CO2(aq) and
is purged with more ease.

In your glass experiment you lowered the pH enough to allow for the CO2 to
be 'boiled off'. If you had increased the solution more basic before you
boiled, you would have NOT driven off the CO2 as easily. In the aquarium we
are at a much higher pH.and the CO2 is less likely to 'purge' off with air.

If you go back to the henderson-hasselbach equation:

at a pH of 8.3 :

pH = pKa + log [A-]/[HA]
8.3 = 6.4 + log [HCO3-1]/[H2CO3]
1.9 = log [HCO3-1]/[H2CO3]
antilogs
79.43 = [HCO3-1]/[H2CO3]

This means that at a pH of 8.3, the majority of the CO2(aq) is in the form
of HCO3-1 by 79-fold. In order to 'purge' CO2 you would need to lower the
pH to shift the equilibrium to below 6.4

In your glass experiment you managed to lower the pH enough to purge out CO2
by boiling. Not sure what pH you got it to, you didn't say.

I hope this helps. I'm getting VERY bored of this discussion.










"Boomer" > wrote in message
...
> I see you are lost case. It is really bad one someone is incorrect and
they try to find a
> way to escape
>
>
> "Agreed. This is an effect of 'buffering"
>
> Agreed, that is "buffering" not Buffering Capacity as defined by the
equation I gave from;
>
> Analytical Chemistry, by Robert.V Dilts, Ph.D
> Department of Chemistry, Vanderbilt University.
>
> I guess he is also clueless as is Pankow. Dr. Pankow being one of the
worlds foremost
> Aquatic Chemists.
>
> "Oh wait, you have another definition of alkalinity"
>
> I think you are a nut case. That is how Alk is tested. It is tested by
titration with a
> std acid to phenolphthalein (P) or Total (T) alkalinity endpoint.
Hydroxide determination
> (OH) uses Barium pretreatment to eliminate carbonate interference.
>
> "Believe me, I don't need to. I have plenty of chem books that cover the
> topic quite well."
>
> Then why all the mistakes ???
>
> "> Acidity = A std alkali titration to methyl orange or phenolphthalein
> endpoint>
>
> That is how is tested, are you so clueless, that as a proclaimed Ph.D
chemist, you don't
> know that simple thing ???
>
>
> "Wrong. Acidity is the property of an acid"
>
> Hum, well then you can go argue with HACH and LaMotte, about how messed up
they are on
> their test kits, which follow EPA, NPDWR and NPDES testing procedures and
those found in
>
> Standard Methods for the Examination of Water and Wastewater
>
> Acidity is a property of an acid, it is also the ability of a solution to
slow down or
> inhibit pH rises do to the presence or introduction of an Alkali
substances. A higher
> Acidity means you are less likely to increase the pH with the addition of
a base. Just
> like a higher Alkalinity is the ability you are less likely to lower the
pH with the
> addition of an acid. Get it !!!
>
> . "Why in one case does CO2 from air lower pH and in the other case it
raises
> it? Doesn't make sense."
>
> Quite twisting things around to suit your fancy. I said CO2 from air can
lower the pH and
> if CO2 is in water it can driven off, via aeration, blown off, it will
thus raise the pH.
> Where did you get this "air lower pH and other air raises pH , I said no
such thing as CO2
> in air raises pH, get the facts straight, knock off the BS line.
>
> Maybe I should explain it to you in Dick & Jane Terms. The Boomer Glass
Trick, is quite
> popular and always proves my point
>
> First get two glasses and fill with sample water. Measure the pH and Alk
Put some pH
> indicator in one and not the other. In the indicator glass now blow in it
with a straw,
> magic the indicator changes to a lower pH. Now put in an airstone and boil
the water and
> watch the pH rise. Do the same to the other glass, you know the pH is
going to go down.
> Now after you blow, measure the Alk, it has not changed from the first
measurement. Fauna
> produce CO2, in which case the rate can rise faster than it can leave to
the atmosphere.
> Such increases in CO2 will drop the pH . Pretend your blowing is all that
fauna in the
> tank expelling CO2. The airstone, drives it of the CO2, in which case the
ph of the glass
> will go back up.If you aerate the indicator glass you will see the
indicator go back to a
> more base pH. CO2 goes very easy into water , but is a little harder to
drive off, it
> takes more time. Now as with the glass, pretend your tank water has high
CO2 and you
> aerate the water, what happens, the CO2 is driven of and the pH goes up.
This is why good
> circulation and agitation of the surface is important ......to drive off
CO2. Now if the
> house is high in CO2 it will have a much higher partial pressure and will
be harder to
> drive off. If it is high enough and the CO2 in-tank is low enough the CO2
will go right
> into solution, increase and lower the pH I don't care what your Alk is.
>
> You have lost it. All the books I posted are College chemistry books. Get
off on your hype
> of "marine aquarium". What kind of stunt are you trying to pull ? That we
are all so dumb
> we don't know who those authors are. They are all chemists, most that I
posted are
> Seawater Chemists. Go do a search on them, see what they write and where
they write, where
> they work sand what degree they have They don't write in aquarium books at
all, so lets
> get that straight.
>
> "ALL MARINE BIOLOGIST. So I guess I disagree with them as well. Now
what?
> If you had any chem knowledge other than what you learned in Marine
aquarium
> books, you might be making more sense right now. Trust me"
>
> Are you trying to get me or tell us that Dr. Frank Millero is Marine
Biologist, what drugs
> are you on. He is the worlds foremost Chemical oceanographer. That is a
CHEMIST, just to
> clue you in there pal. Before him it was Riley and Chester and others like
Horne and
> Harvey. Did you even go to Millero's website ? He has been teaching
chemistry for 40 years
> at the University of Miami, especially seawater chemistry.
>
> Here let me help you with a quick search on just Millero;
>
>
http://www.google.com/search?hl=en&ie=UTF-8&oe=UTF-8&q=frank+J+Millero&btnG=
Google+Search
>
>
> Make sure you copy and paste it all
>
> ">You can have all the alk you want in the world and it won't help, in
> regards to CO2
>
> WRONG.
>
> One of your many definitions of alkalinity:
> Alk is defined as;
>
> TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> [HPO4--] +
> 2[PO4---] - [H+]
>
> Those are COMPONENTS of BUFFERS. Are they not?
>
> Yes, those are components of buffers, not arguing that . You are confusing
buffers with
> Buffering Capacity and Alkalinity. As I stated before the two are very
closely related as
> they are also very closely related to Acidity.
>
> From;
>
> Dilts, Analytical Chemistry;
>
> "The amount of ***acid or base that a buffer*** can consume is called
Buffering Capacity
> or Buffer Index. The capacity of a buffer solution is defined as the
number of equivalents
> of an acid or base that must be added to one liter of the buffer to cause
a change in the
> pH of the solution by one unit. Mathematically the capacity is measured
by;
>
> B = dCb / dpH = - dCa / dpH
>
>
> Or as we have stated above, it is the change in the concentration of acid
or of base per
> pH unit.
> given by
>
> B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> where C =[HA] + [A-] in the case of an acid and its conjugate, and C =
[BH] + [B}when the
> buffer is composed of a base and its conjugate. C represents the total
concentration of
> **both acid and conjugate base *** in the buffer system."
>
> Alk tells you how much is added in meq / l, to bring the solution to a
endpoint of about
> a pH of 4.
>
> By the way an few years ago two guys in FAMA were arguing the same thing
as we are. I
> called Dr. Frank Millero for an answer,which was. "The chemist was right
the biologist was
> wrong. Buffering Capacity and Alkalinity are not the same thing. Alkalify
is the ability
> to withstand only downward trends in pH and BC is the ability to withstand
both upward
> trends and downward trends in pH.You can calculate Alk if you know the BC.
>
> Feel free to give him a buzz, read the statement above and see what
kinda' answer you
> get. Here is his phone number. Also, try and tell him the pKa's of
seawater are 10.3 & 6.4
> and the ratio is1 : 100 ratio of CO3-2 and HCO3-2, as you claim. Hum,
Millero is the
> leading authority on the seawater CO2/Carbonate System. Check some of his
articles :-) It
> is Millero that is always fine tuning seawater pKa's.
>
> 1-305-361-4707, University of Miami
>
>
> Have a nice day, no sense in posting to you anymore till you get some
facts straight.
>
>
> Boomer
>
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
>
>

[stoutman]

Because I can't show you my references and because I know you will not look
them up here are some useful web pages to help you along with the chemical
terms ACIDITY and BASICITY. I tried to find web pages for you that are not
overly complicated. Most come from UNIVERSITIES (.edu)

http://www.chemistry.montana.edu/~martint/BCHM122/pH.htm

http://www.chem.ucalgary.ca/courses/350/Carey5th/useful/acidbase.html

http://www.chem.uwa.edu.au/enrolled_students/Chem100/Chem100_sect3/sect3.3.h
tml








"Boomer" > wrote in message
...
> No, I don't write anything. I explain things to people such as yourself
that don't
> understand the issue.
>
>
> "By the way do you know who you are talking to ?"
>
> This was more on the order of a joke to get your attention. I have been
around about 35
> years. I also get a real charge of people like yourself , that come here
or forums and
> toot your BS, assuming you must be right and we are all idiots lol
>
> "Someone is a little pompous"
>
> Now here we go with the name calling. I can see where you are coming from,
does it make
> you feel better or do you think that makes you correct. It is rather
childless don't you
> think ?
>
> If I did you would be the last , as you are way to lost on seawater
chemistry
>
> What's interesting and I'm sure to everyone it is, the big hole you just
keep digging for
> yourself. lol
>
> You must be nervous, you sure seem be bothered by these post and my
drilling you with info
> from refs, Seawater Chemistry books, written by seawater chemists. I must
make you look
> bad,Ph.D and all :-) I think Millero has been at it about 40 years and
has written 3
> advanced textbooks on chemical oceanography. Hum, you may also want to
check out Stumm &
> Morgan .Of course there are others, i.e Morel, Benjamin(the newest water
chemistry book
> 2002) and lets not forget the "old great book" by Snoeyink and Jenkins,
still in print. I
> have them all :-)
>
> A smart guy MAY want to go look at my ref, especially a Ph.D chemist such
as yourself :-)
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message news:EfSVb.12701$QA2.22009@attbi_s52...
> : >By the way do you know who you are talking to ?
> :
> : This cracks me up. Someone is a little pompous. I gather from the
> : responders in this thread that Boomer is some kind of self proclaimed
> : aquarium guru.
> :
> : I can only assume that he is a Marine Biologist that needs to take a few
> : more chemistry courses. Boomer, if you are an author of aquarium
> : literature, than I would like to be acknowledged in your next manuscript
for
> : helping you see the light.
> :
> : I too can be pompous.
> :
> : -Stoutman
> :
> :
> :
> :
> :
> :
> :
> :
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > Let me make this clear you don't know what you are taking about
> : >
> : > "alkalinity is a measurement of 'buffering capacity'"
> : >
> : > No, it is the ability to neutralize an acid. BC is the ability to
> : withstand both upward
> : > and downward trends in pH.
> : >
> : > "pH is a measurement of 'acidity/basicity'.
> : >
> : > No, pH is a measurement of acidity and pOH is a measurement of
Basicity,
> : if you want to
> : > get picky, which seems you do.
> : >
> : >
> : > "How do you remove CO2? "
> : >
> : > It is called "blowing it off" , such as with an airstone. If you have
high
> : CO2 and add an
> : > airstone it will drive the CO2 off raising the pH. It can be proven
with a
> : glass of water,
> : > a straw, some pH color indicator and an Alk test kit and if you must a
CO2
> : test kit
> : >
> : > >You can have all the alk you want in the world and it won't help, in
> : > regards to CO2
> : >
> : > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
changes
> : in
> : > pH. This is what is meant by 'buffering capacity'"
> : >
> : > No you are wrong and very lost. If Alk resists changes in pH then why
does
> : CO2 lower the
> : > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
> : effect on CO2. When
> : > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
any
> : pH no matter what
> : > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> : >
> : > .
> : > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> : Tell me the pH and
> : > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and I
> : will give you
> : > the pH. Don't forget the temperature and Salinity.
> : >
> : > Alk is defined as;
> : >
> : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> : [HPO4--] +
> : > 2[PO4---] - [H+]
> : >
> : >
> : > Buffering Capacity is defined as;
> : >
> : > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
[H3O+])²
> : >
> : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> : maximum BC is at a
> : > pH of 6 & 9. For all practically purposes seawater has very little
> : Buffering Capacity, if
> : > any at all.
> : >
> : >
> : > Alkalinity and Buffer Capacity are closely tied but are NOT the same
> : thing, it is a
> : > misunderstanding and use of the term. Do you think water chemistry
books
> : would have
> : > separate sections on Alkalinity and Buffering Capacity if they were
the
> : same thing ?
> : >
> : > By the way do you know who you are talking to ?
> : >
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : >
> : >
> :
> :
>
>

[stoutman]

Because I can't show you my references and because I know you will not look
them up here are some useful web pages to help you along with the chemical
terms ACIDITY and BASICITY. I tried to find web pages for you that are not
overly complicated. Most come from UNIVERSITIES (.edu)

http://www.chemistry.montana.edu/~martint/BCHM122/pH.htm

http://www.chem.ucalgary.ca/courses/350/Carey5th/useful/acidbase.html

http://www.chem.uwa.edu.au/enrolled_students/Chem100/Chem100_sect3/sect3.3.h
tml



















"stoutman" <.@.> wrote in message news:mvYVb.14427$QA2.60571@attbi_s52...
> Ok, Im bored, I will give you a free response.
>
> > Agreed, that is "buffering" not Buffering Capacity as defined by the
> equation I gave from;
>
> Don't the components of a buffer account for the buffering capacity? Yes.
>
> >It is tested by titration with a std acid to phenolphthalein (P) or Total
> (T) alkalinity endpoint. Hydroxide determination (OH) uses Barium
> pretreatment to eliminate carbonate interference.
>
> I know how to do a titration, In fact I have done several. How many have
> you actually done? I don't mean by counting drops, I mean with a buret?
>
> > Then why all the mistakes ???
>
> You must be referring to your mistakes.
>
> > "> Acidity = A std alkali titration to methyl orange or phenolphthalein
> > endpoint
>
> Acidity is simply the opposite of basicity. To increase acidity you lower
> the pH by adding more acid to the solution. To increase the basicity, you
> add more base effectively increasing the pH.
>
> You can measure the basicity and acidity of a solution by determining it's
> pH.
>
> > Acidity is a property of an acid, it is also the ability of a solution
to
> slow down or
> > inhibit pH rises do to the presence or introduction of an Alkali
> substances.
>
> Wrong. Acidity has nothing to do with buffering. See above. Oh, I see,
> you think acidity is the opposite of alkalinity. In the world of
CHEMISTRY
> it's not. Maybe in aquarium newsgroups it is.
>
> In your Boomer water experiment, the blowing into the glass drops the pH
> because of the CO2:
>
> CO2(g) <------> CO2(aq) + H2O <--(1)----> H2CO3 <--(2)----> HCO3-1 + H3O
> <---(3)----> CO3-2 + 2H3O
>
> These are all in equilibrium with each other. An initial high pH (above
> 6.4) will shift the equilibrium to the right to form HCO3-1. If the pH of
> the solution is above 10.3 (pKa2) the equilibrium will be shifted even
> further to CO3-2. In the aquarium (pH = 8-8.5) the equilibrium is shifted
> towards HCO3-1. At this pH it will be VERY difficult to purge out CO2
with
> air. If you lower the pH to below 6.4, most of the CO2(aq) will be in the
> form of H2CO3. At this point the H2CO3 is in equilibrium with CO2(aq) and
> is purged with more ease.
>
> In your glass experiment you lowered the pH enough to allow for the CO2 to
> be 'boiled off'. If you had increased the solution more basic before you
> boiled, you would have NOT driven off the CO2 as easily. In the aquarium
we
> are at a much higher pH.and the CO2 is less likely to 'purge' off with
air.
>
> If you go back to the henderson-hasselbach equation:
>
> at a pH of 8.3 :
>
> pH = pKa + log [A-]/[HA]
> 8.3 = 6.4 + log [HCO3-1]/[H2CO3]
> 1.9 = log [HCO3-1]/[H2CO3]
> antilogs
> 79.43 = [HCO3-1]/[H2CO3]
>
> This means that at a pH of 8.3, the majority of the CO2(aq) is in the form
> of HCO3-1 by 79-fold. In order to 'purge' CO2 you would need to lower the
> pH to shift the equilibrium to below 6.4
>
> In your glass experiment you managed to lower the pH enough to purge out
CO2
> by boiling. Not sure what pH you got it to, you didn't say.
>
> I hope this helps. I'm getting VERY bored of this discussion.
>
>
>
>
>
>
>
>
>
>
> "Boomer" > wrote in message
> ...
> > I see you are lost case. It is really bad one someone is incorrect and
> they try to find a
> > way to escape
> >
> >
> > "Agreed. This is an effect of 'buffering"
> >
> > Agreed, that is "buffering" not Buffering Capacity as defined by the
> equation I gave from;
> >
> > Analytical Chemistry, by Robert.V Dilts, Ph.D
> > Department of Chemistry, Vanderbilt University.
> >
> > I guess he is also clueless as is Pankow. Dr. Pankow being one of the
> worlds foremost
> > Aquatic Chemists.
> >
> > "Oh wait, you have another definition of alkalinity"
> >
> > I think you are a nut case. That is how Alk is tested. It is tested by
> titration with a
> > std acid to phenolphthalein (P) or Total (T) alkalinity endpoint.
> Hydroxide determination
> > (OH) uses Barium pretreatment to eliminate carbonate interference.
> >
> > "Believe me, I don't need to. I have plenty of chem books that cover
the
> > topic quite well."
> >
> > Then why all the mistakes ???
> >
> > "> Acidity = A std alkali titration to methyl orange or phenolphthalein
> > endpoint>
> >
> > That is how is tested, are you so clueless, that as a proclaimed Ph.D
> chemist, you don't
> > know that simple thing ???
> >
> >
> > "Wrong. Acidity is the property of an acid"
> >
> > Hum, well then you can go argue with HACH and LaMotte, about how messed
up
> they are on
> > their test kits, which follow EPA, NPDWR and NPDES testing procedures
and
> those found in
> >
> > Standard Methods for the Examination of Water and Wastewater
> >
> > Acidity is a property of an acid, it is also the ability of a solution
to
> slow down or
> > inhibit pH rises do to the presence or introduction of an Alkali
> substances. A higher
> > Acidity means you are less likely to increase the pH with the addition
of
> a base. Just
> > like a higher Alkalinity is the ability you are less likely to lower the
> pH with the
> > addition of an acid. Get it !!!
> >
> > . "Why in one case does CO2 from air lower pH and in the other case it
> raises
> > it? Doesn't make sense."
> >
> > Quite twisting things around to suit your fancy. I said CO2 from air can
> lower the pH and
> > if CO2 is in water it can driven off, via aeration, blown off, it will
> thus raise the pH.
> > Where did you get this "air lower pH and other air raises pH , I said no
> such thing as CO2
> > in air raises pH, get the facts straight, knock off the BS line.
> >
> > Maybe I should explain it to you in Dick & Jane Terms. The Boomer Glass
> Trick, is quite
> > popular and always proves my point
> >
> > First get two glasses and fill with sample water. Measure the pH and Alk
> Put some pH
> > indicator in one and not the other. In the indicator glass now blow in
it
> with a straw,
> > magic the indicator changes to a lower pH. Now put in an airstone and
boil
> the water and
> > watch the pH rise. Do the same to the other glass, you know the pH is
> going to go down.
> > Now after you blow, measure the Alk, it has not changed from the first
> measurement. Fauna
> > produce CO2, in which case the rate can rise faster than it can leave to
> the atmosphere.
> > Such increases in CO2 will drop the pH . Pretend your blowing is all
that
> fauna in the
> > tank expelling CO2. The airstone, drives it of the CO2, in which case
the
> ph of the glass
> > will go back up.If you aerate the indicator glass you will see the
> indicator go back to a
> > more base pH. CO2 goes very easy into water , but is a little harder to
> drive off, it
> > takes more time. Now as with the glass, pretend your tank water has high
> CO2 and you
> > aerate the water, what happens, the CO2 is driven of and the pH goes up.
> This is why good
> > circulation and agitation of the surface is important ......to drive off
> CO2. Now if the
> > house is high in CO2 it will have a much higher partial pressure and
will
> be harder to
> > drive off. If it is high enough and the CO2 in-tank is low enough the
CO2
> will go right
> > into solution, increase and lower the pH I don't care what your Alk is.
> >
> > You have lost it. All the books I posted are College chemistry books.
Get
> off on your hype
> > of "marine aquarium". What kind of stunt are you trying to pull ? That
we
> are all so dumb
> > we don't know who those authors are. They are all chemists, most that I
> posted are
> > Seawater Chemists. Go do a search on them, see what they write and where
> they write, where
> > they work sand what degree they have They don't write in aquarium books
at
> all, so lets
> > get that straight.
> >
> > "ALL MARINE BIOLOGIST. So I guess I disagree with them as well. Now
> what?
> > If you had any chem knowledge other than what you learned in Marine
> aquarium
> > books, you might be making more sense right now. Trust me"
> >
> > Are you trying to get me or tell us that Dr. Frank Millero is Marine
> Biologist, what drugs
> > are you on. He is the worlds foremost Chemical oceanographer. That is a
> CHEMIST, just to
> > clue you in there pal. Before him it was Riley and Chester and others
like
> Horne and
> > Harvey. Did you even go to Millero's website ? He has been teaching
> chemistry for 40 years
> > at the University of Miami, especially seawater chemistry.
> >
> > Here let me help you with a quick search on just Millero;
> >
> >
>
http://www.google.com/search?hl=en&ie=UTF-8&oe=UTF-8&q=frank+J+Millero&btnG=
> Google+Search
> >
> >
> > Make sure you copy and paste it all
> >
> > ">You can have all the alk you want in the world and it won't help, in
> > regards to CO2
> >
> > WRONG.
> >
> > One of your many definitions of alkalinity:
> > Alk is defined as;
> >
> > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> > [HPO4--] +
> > 2[PO4---] - [H+]
> >
> > Those are COMPONENTS of BUFFERS. Are they not?
> >
> > Yes, those are components of buffers, not arguing that . You are
confusing
> buffers with
> > Buffering Capacity and Alkalinity. As I stated before the two are very
> closely related as
> > they are also very closely related to Acidity.
> >
> > From;
> >
> > Dilts, Analytical Chemistry;
> >
> > "The amount of ***acid or base that a buffer*** can consume is called
> Buffering Capacity
> > or Buffer Index. The capacity of a buffer solution is defined as the
> number of equivalents
> > of an acid or base that must be added to one liter of the buffer to
cause
> a change in the
> > pH of the solution by one unit. Mathematically the capacity is measured
> by;
> >
> > B = dCb / dpH = - dCa / dpH
> >
> >
> > Or as we have stated above, it is the change in the concentration of
acid
> or of base per
> > pH unit.
> > given by
> >
> > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
> [H3O+] / (Ka =
> > H3O+])² )
> >
> > where C =[HA] + [A-] in the case of an acid and its conjugate, and C =
> [BH] + [B}when the
> > buffer is composed of a base and its conjugate. C represents the total
> concentration of
> > **both acid and conjugate base *** in the buffer system."
> >
> > Alk tells you how much is added in meq / l, to bring the solution to a
> endpoint of about
> > a pH of 4.
> >
> > By the way an few years ago two guys in FAMA were arguing the same thing
> as we are. I
> > called Dr. Frank Millero for an answer,which was. "The chemist was right
> the biologist was
> > wrong. Buffering Capacity and Alkalinity are not the same thing.
Alkalify
> is the ability
> > to withstand only downward trends in pH and BC is the ability to
withstand
> both upward
> > trends and downward trends in pH.You can calculate Alk if you know the
BC.
> >
> > Feel free to give him a buzz, read the statement above and see what
> kinda' answer you
> > get. Here is his phone number. Also, try and tell him the pKa's of
> seawater are 10.3 & 6.4
> > and the ratio is1 : 100 ratio of CO3-2 and HCO3-2, as you claim. Hum,
> Millero is the
> > leading authority on the seawater CO2/Carbonate System. Check some of
his
> articles :-) It
> > is Millero that is always fine tuning seawater pKa's.
> >
> > 1-305-361-4707, University of Miami
> >
> >
> > Have a nice day, no sense in posting to you anymore till you get some
> facts straight.
> >
> >
> > Boomer
> >
> >
> > Want to talk chemistry ? The Reef Chemistry Forum
> > http://www.reefcentral.com/vbulletin/index.php
> >
> > Want to See More ?
> > Please Join Our Growing Membership
> > www.coralrealm.com
> >
> > If You See Me Running You Better Catch-Up
> >
> >
>
>

[Marc Levenson]

The King finds humor in this situation, and allows it to continue.

For now.

King Marc. :)

Richard Reynolds wrote:

> now ive done it the king is gona slap me around for messing with the oracle :D
>

--
Personal Page: http://www.sparklingfloorservice.com/oanda/index.html
Business Page: http://www.sparklingfloorservice.com
Marine Hobbyist: http://www.melevsreef.com

[Marc Levenson]

Boomer, we all have our strengths and weaknesses. Why is chemistry so fascinating to you? I
was following along for a while, but it just got to close to molecular biology for me to
continue... ;) My son had some chemistry homework a few days ago, and we were trying to
determine covalent ions and such. My interest only peaked when I found out the book started
explaining NSW.

LOL

As I read some of the chapter in question, it talked about how various elements from the
periodic table sometimes shared electrons and sometimes did not (causing a tug-of-war, in
effect). Still, after all that excitement, I didn't pick up the book to keep reading. You've
been studying this stuff for decades!!

Marc


Boomer wrote:

> "With the exception of CO2?"
>
> Yes that is correct. It is something many don't understand. CO2 is not an ion but a
> molecule, it cares no charge.
>
> TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> [HPO4--] +
> 2[PO4---] - [H+]
>
> Hum, where is the CO2 here, hummmmm I can't find it.
>
> Alk is a function of Ions and how they are affected by other charged ions. CO2 has no
> effect on alk and vise versa. You seemed to have already acknowledged that. So what is the
> point ? Or is it you think Alk is affected by CO2 or vise-versa. I invite you to our Chem
> Forum, full of chemists, ask the question and see what kind of answers you get or just
> call Millero.
>
> Nuff said
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message news:NIUVb.13104$QA2.22029@attbi_s52...
> : Boomers very first post in this thread:
> :
> : >If CO2 increases the pH will drop, no mater what the Alk is.
> :
> : A later post made by Boomer:
> :
> : >Alkalinity is the ability to slow down or inhibit downward trends in pH.
> :
> : With the exception of CO2?
> :
> :
> :
> :
> :
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > No, I don't write anything. I explain things to people such as yourself
> : that don't
> : > understand the issue.
> : >
> : >
> : > "By the way do you know who you are talking to ?"
> : >
> : > This was more on the order of a joke to get your attention. I have been
> : around about 35
> : > years. I also get a real charge of people like yourself , that come here
> : or forums and
> : > toot your BS, assuming you must be right and we are all idiots lol
> : >
> : > "Someone is a little pompous"
> : >
> : > Now here we go with the name calling. I can see where you are coming from,
> : does it make
> : > you feel better or do you think that makes you correct. It is rather
> : childless don't you
> : > think ?
> : >
> : > If I did you would be the last , as you are way to lost on seawater
> : chemistry
> : >
> : > What's interesting and I'm sure to everyone it is, the big hole you just
> : keep digging for
> : > yourself. lol
> : >
> : > You must be nervous, you sure seem be bothered by these post and my
> : drilling you with info
> : > from refs, Seawater Chemistry books, written by seawater chemists. I must
> : make you look
> : > bad,Ph.D and all :-) I think Millero has been at it about 40 years and
> : has written 3
> : > advanced textbooks on chemical oceanography. Hum, you may also want to
> : check out Stumm &
> : > Morgan .Of course there are others, i.e Morel, Benjamin(the newest water
> : chemistry book
> : > 2002) and lets not forget the "old great book" by Snoeyink and Jenkins,
> : still in print. I
> : > have them all :-)
> : >
> : > A smart guy MAY want to go look at my ref, especially a Ph.D chemist such
> : as yourself :-)
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : > "stoutman" <.@.> wrote in message news:EfSVb.12701$QA2.22009@attbi_s52...
> : > : >By the way do you know who you are talking to ?
> : > :
> : > : This cracks me up. Someone is a little pompous. I gather from the
> : > : responders in this thread that Boomer is some kind of self proclaimed
> : > : aquarium guru.
> : > :
> : > : I can only assume that he is a Marine Biologist that needs to take a few
> : > : more chemistry courses. Boomer, if you are an author of aquarium
> : > : literature, than I would like to be acknowledged in your next manuscript
> : for
> : > : helping you see the light.
> : > :
> : > : I too can be pompous.
> : > :
> : > : -Stoutman
> : > :
> : > :
> : > :
> : > :
> : > :
> : > :
> : > :
> : > :
> : > :
> : > :
> : > :
> : > :
> : > : "Boomer" > wrote in message
> : > : ...
> : > : > Let me make this clear you don't know what you are taking about
> : > : >
> : > : > "alkalinity is a measurement of 'buffering capacity'"
> : > : >
> : > : > No, it is the ability to neutralize an acid. BC is the ability to
> : > : withstand both upward
> : > : > and downward trends in pH.
> : > : >
> : > : > "pH is a measurement of 'acidity/basicity'.
> : > : >
> : > : > No, pH is a measurement of acidity and pOH is a measurement of
> : Basicity,
> : > : if you want to
> : > : > get picky, which seems you do.
> : > : >
> : > : >
> : > : > "How do you remove CO2? "
> : > : >
> : > : > It is called "blowing it off" , such as with an airstone. If you have
> : high
> : > : CO2 and add an
> : > : > airstone it will drive the CO2 off raising the pH. It can be proven
> : with a
> : > : glass of water,
> : > : > a straw, some pH color indicator and an Alk test kit and if you must a
> : CO2
> : > : test kit
> : > : >
> : > : > >You can have all the alk you want in the world and it won't help, in
> : > : > regards to CO2
> : > : >
> : > : > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
> : changes
> : > : in
> : > : > pH. This is what is meant by 'buffering capacity'"
> : > : >
> : > : > No you are wrong and very lost. If Alk resists changes in pH then why
> : does
> : > : CO2 lower the
> : > : > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
> : > : effect on CO2. When
> : > : > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
> : any
> : > : pH no matter what
> : > : > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> : > : >
> : > : > .
> : > : > Go ahead and pick a seawater pH and I will tell you what that ratio
> : is.
> : > : Tell me the pH and
> : > : > Alk and I will give the CO2 concentration. Give me the Alk and CO2
> : and I
> : > : will give you
> : > : > the pH. Don't forget the temperature and Salinity.
> : > : >
> : > : > Alk is defined as;
> : > : >
> : > : > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> : > : [HPO4--] +
> : > : > 2[PO4---] - [H+]
> : > : >
> : > : >
> : > : > Buffering Capacity is defined as;
> : > : >
> : > : > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
> : [H3O+])²
> : > : >
> : > : > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> : > : maximum BC is at a
> : > : > pH of 6 & 9. For all practically purposes seawater has very little
> : > : Buffering Capacity, if
> : > : > any at all.
> : > : >
> : > : >
> : > : > Alkalinity and Buffer Capacity are closely tied but are NOT the same
> : > : thing, it is a
> : > : > misunderstanding and use of the term. Do you think water chemistry
> : books
> : > : would have
> : > : > separate sections on Alkalinity and Buffering Capacity if they were
> : the
> : > : same thing ?
> : > : >
> : > : > By the way do you know who you are talking to ?
> : > : >
> : > : > --
> : > : > Boomer
> : > : >
> : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : >
> : > : > Want to See More ?
> : > : > Please Join Our Growing Membership
> : > : > www.coralrealm.com
> : > : >
> : > : > If You See Me Running You Better Catch-Up
> : > : >
> : > : >
> : > :
> : > :
> : >
> : >
> :
> :

--
Personal Page: http://www.sparklingfloorservice.com/oanda/index.html
Business Page: http://www.sparklingfloorservice.com
Marine Hobbyist: http://www.melevsreef.com

[ReefTech]

It looks like boomer went down like a sack of potatoes.


"Richard Reynolds" > wrote in message
news:0lHVb.16203$gl2.2728@lakeread05...
> I am sorry ahead of time I couldnt resist
>
> > By the way do you know who you are talking to ?
>
>
> DUH of course he doesnt or he wouldnt have argued :D
>
>
> now ive done it the king is gona slap me around for messing with the
oracle :D
>
> --
> Richard Reynolds
>
>
>

[ReefTech]

Looks to me like Boomer lost this one.


"Dragon Slayer" > wrote in message
...
> Boomer when you read that, just let it go.............no need bashing
heads
> here, the group knows what's going on.
>
> kc
>
> "stoutman" <.@.> wrote in message
news:SFNVb.204571$Rc4.1681932@attbi_s54...
> > Oh brother. Where to start.
> >
> > pH is the -log of the hydronium ion concentration. When the hydronium
ion
> > concentration is very low, your system is basic (high pH). When the
> > hydronium ion concentration is very large, your system is acidic (low
pH).
> >
> > pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice
versa.
> > But a pH of < 7 means acidic. pH > 7 means basic.
> > pH can tell you something about acidity and basicity. It is a
measurement
> > of both, or the entire pH scale (1-14) if you will.
> >
> > >It is called "blowing it off" , such as with an airstone. If you have
> high
> > CO2 and add an airstone it will drive the CO2 off raising the pH.
> >
> > Ok, you are going to try and 'purge' (the correct term) your CO2 out
with
> > air. Yeah, I guess that would work. If you intentionally put the CO2
in
> > there to begin with because you must have a higher concentration of CO2
in
> > your tank than in the atmosphere. I don't intentionally put CO2 in my
> tank.
> > But I know some of you reef people due in Kalk reactors.
> >
> > >If Alk resists changes in pH then why does CO2 lower the pH without
> > affecting the Alk.
> >
> > Alkalinity is buffering capacity. Your buffers begin to get weakened
with
> > the addition of acid until they reach a point when they can no longer
> > 'buffer' and the pH crashes.
> >
> > >But I know what you mean, may use the term ALK and BC interchangeably
> >
> > Do you remember writing this in an earlier post? If you believe that
> > alkalinity and buffering capacity can be used interchangeably than I
must
> be
> > getting through to you.
> >
> > >When CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3.
At
> > any pH no matter what the Alk or CO2 there will be an exact ratio of
> > CO2:HCO3:CO3
> >
> > Yes, at any pH there will be 'SOME' ratio of CO2:HCO3-1:CO3-2. What is
> your
> > point here?
> >
> > > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> > Tell me the pH and
> > > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and
> I
> > will give you
> > > the pH. Don't forget the temperature and Salinity.
> >
> > Not interested. I can find my own software to do this too.
> >
> > > Alk is defined as;
> > >
> > > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> > [HPO4--] +
> > > 2[PO4---] - [H+]
> >
> > Ahh, now we are getting somewhere. What you are showing are components
of
> a
> > 'BUFFER'. Which are used in the over all 'buffering capacity'. Are we
> > going in circles here? Anyway, I think you are learning something.
> >
> > > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> > maximum BC is at a
> > > pH of 6 & 9. For all practically purposes seawater has very little
> > Buffering Capacity, if
> > > any at all.
> >
> > This is the 'primary buffer' in sea water:
> >
> > H2O + CO2 <---> H2CO3 <---> H+ + HCO3-1
> >
> > If you REALLY believe that sea water has little buffering capacity, than
> you
> > need to do some reading on your own. I wont be able to convince you.
> >
> > > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> > maximum BC is at a
> > > pH of 6 & 9. For all practically purposes seawater has very little
> > Buffering Capacity, if
> > > any at all.
> >
> > This would be true if a monoprotic acid where used in the 'buffer', but
> > carbonic acid (the primary buffering component in seawater) is a
> polyprotic
> > acid. It has two protons that can dissociate. Therefore, it has two
> pKa's
> > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
> The
> > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> > right in there. Is that magic? :)
> >
> > Remember that seawater is more than a mixture of just carbonate and CO2,
> > there are other buffers involved that make it even more complicated I'm
> > sure.
> >
> > > By the way do you know who you are talking to ?
> >
> > No. Do you?
> >
> >
> >
> >
> > "Boomer" > wrote in message
> > ...
> > > Let me make this clear you don't know what you are taking about
> > >
> > > "alkalinity is a measurement of 'buffering capacity'"
> > >
> > > No, it is the ability to neutralize an acid. BC is the ability to
> > withstand both upward
> > > and downward trends in pH.
> > >
> > > "pH is a measurement of 'acidity/basicity'.
> > >
> > > No, pH is a measurement of acidity and pOH is a measurement of
Basicity,
> > if you want to
> > > get picky, which seems you do.
> > >
> > >
> > > "How do you remove CO2? "
> > >
> > > It is called "blowing it off" , such as with an airstone. If you have
> high
> > CO2 and add an
> > > airstone it will drive the CO2 off raising the pH. It can be proven
with
> a
> > glass of water,
> > > a straw, some pH color indicator and an Alk test kit and if you must a
> CO2
> > test kit
> > >
> > > >You can have all the alk you want in the world and it won't help, in
> > > regards to CO2
> > >
> > > "Wrong. Alkalinity increases your tank's ability to RESIST sharp
> changes
> > in
> > > pH. This is what is meant by 'buffering capacity'"
> > >
> > > No you are wrong and very lost. If Alk resists changes in pH then why
> does
> > CO2 lower the
> > > pH without affecting the Alk ? CO2 has no effect on alk and alk has no
> > effect on CO2. When
> > > CO2 is added or remove it just changes the ratio of CO2:HCO3:CO3. At
any
> > pH no matter what
> > > the Alk or CO2 there will be an exact ratio of CO2:HCO3:CO3
> > >
> > > .
> > > Go ahead and pick a seawater pH and I will tell you what that ratio
is.
> > Tell me the pH and
> > > Alk and I will give the CO2 concentration. Give me the Alk and CO2
and
> I
> > will give you
> > > the pH. Don't forget the temperature and Salinity.
> > >
> > > Alk is defined as;
> > >
> > > TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
> > [HPO4--] +
> > > 2[PO4---] - [H+]
> > >
> > >
> > > Buffering Capacity is defined as;
> > >
> > > BC = dCb/dpH = 2.303 (Kw/ [H3O+] + [H30+] + CKa[H3O+] / (Ka +
[H3O+])²
> > >
> > > In any aqueous solution maximum BC is reached when pH= pKa. Seawaters
> > maximum BC is at a
> > > pH of 6 & 9. For all practically purposes seawater has very little
> > Buffering Capacity, if
> > > any at all.
> > >
> > >
> > > Alkalinity and Buffer Capacity are closely tied but are NOT the same
> > thing, it is a
> > > misunderstanding and use of the term. Do you think water chemistry
books
> > would have
> > > separate sections on Alkalinity and Buffering Capacity if they were
the
> > same thing ?
> > >
> > > By the way do you know who you are talking to ?
> > >
> > > --
> > > Boomer
> > >
> > > Want to talk chemistry ? The Reef Chemistry Forum
> > > http://www.reefcentral.com/vbulletin/index.php
> > >
> > > Want to See More ?
> > > Please Join Our Growing Membership
> > > www.coralrealm.com
> > >
> > > If You See Me Running You Better Catch-Up
> > >
> > >
> >
> >
>
>

[Boomer]

Now I am getting bored

"Don't the components of a buffer account for the buffering capacity? Yes."

Yes, agreed but you seem to fail what I'm saying. Buffering Capacity and Alkalinity are
not the same, that has always been the issue. I gave the equation does that look like an
Alkalinity equation or how Alk is determined. I see you had now comments on it what's
wrong, why no comments on the equations I gave. Don't understand them or what ? Again this
is the equation for Buffering Capacity, also called Buffer Index or Buffer Intensity. It
is defined in most water chemistry and chemical oceanography text books.

B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa [H3O+] / (Ka =
H3O+])² )

This is not Alkalinity now is it ?

"I know how to do a titration, In fact I have done several. How many have
you actually done? I don't mean by counting drops, I mean with a buret?"

Well good for you, I use a Digital Titrator

"Oh, I see,
you think acidity is the opposite of alkalinity. In the world of CHEMISTRY
it's not. Maybe in aquarium newsgroups it is.

Hum no, maybe you should go for a look at HACH's or LaMotte website or the book I
suggested earlier. Please view a copy.

Standard Methods for the Examination of Water and Wastewater

This book, over 2000 pages, is the guide for water testing. If you are reporting water
test to the EPA you must use approved std from this text.I t is prepared and published by
the EPA, American Water Works Association and American Public Health Association. You
mean you don't have one and the issue is water chemistry

You are confusing Acidity and Acidity as you know little about water chemistry and
procedures and test methods

From SMEWW, section 2-30, 2310 ACIDITY

"Acidity of water is its quantative capacity to react with a strong base to a designated
pH"

This is how you test for it

A std alkali titration to methyl orange or phenolphthalein
endpoint.

BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write this book, there are
over 100 of them, they are wrong.

Like Buffering Capacity you have your Acidity's mixed up
In water measurement if you have a high Alk you also usually have a high Acidity.
Normally a high Alk also gives a higher CO2 level. Get a WATER CHEMISTRY BOOK there pal.


"These are all in equilibrium with each other. An initial high pH (above
6.4) will shift the equilibrium to the right to form HCO3-1. If the pH of
the solution is above 10.3 (pKa2) the .........."


Christ, there you go again with the FW ****. All your numbers are wrong we are dealing
with SEAWATER

This means that at a pH of 8.3, the majority of the CO2(aq) is in the form
of HCO3-1 .

I have already pointed that out and gave actual values at know seawater levels, go back
and re-read it you aren't telling me anything here.Of course most is HCO3 see...


@ 20C and 34.3 ppt salinity

CO2 = 0.52 %

HCO3 = 86.4 %

CO3 = 13.09 %


"In your glass experiment you managed to lower the pH enough to purge out CO2
by boiling"

The purpose behind the glass is to show that alk is not affect by CO2 and vise-versa and
how Co2 affects pH.

Now, in a real life seawater aquarium, with a pH of 8.3 and that pH drops to say 8.1 it is
usually due to excess CO2. If you took a glass of that water and aerated it you WILL drive
off the CO2 and raise the pH. It has been done a proven a million times.

"In order to 'purge' CO2 you would need to lower the
pH to shift the equilibrium to below 6.4"

The hell you do !!!.Do you know who many times people on this NG to include Dr. Craig
Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a sample of aquarium
water and aerate it to see if the pH GOES UP AND when they come back with the test it is
often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST excess CO2 in the tank
water, increase the circulation for better gas exchange at the surface, reduce feeding,
and try to improve on better skimming, thus reducing the bio-load and pH decline due to
CO2.


"I hope this helps. "

Help, how can you when you miss everything. I should be charging you

Oh, by the way. Your websites, I have about 50 on these issues, I could post them, not to
mention I have all those water chemistry books, so there is no need to view your sites.

Finally are you afraid to come to our Chemistry Forum, afraid to get slapped by REAL
chemists. I get a charge out of you can't post your ref .I have posted the same or similar
stuff on his forum and I wasn't pointed out WRONG pal. I have 1500 posts there and am the
biggest contributor to his forum other than himself or maybe Habib Sheka

Hum, here are Randy's ref that he posted. He hosts the website

S. RANDY HOLMES-FARLEY
Arlington, Massachusetts

EDUCATION

1982-1986 Harvard University Cambridge, MA
PhD in Chemistry
Research Advisor: George Whitesides

Investigated the relationship between polymer surface chemistry and physical properties
through controlled surface modification and testing.

1980-1982 Cornell University Ithaca, NY
BA in Chemistry and Biology
Graduated Summa Cum Laude
Distinction in All Subjects
Grade Point: 3.94/4.0
Honors research: isolation and characterization of the subunit of CF1 enzyme


1978-1979 Stanford University Palo Alto, CA
Grade Point: 3.55/4.0


EXPERIENCE

1992- present Genzyme Drug Disvcovery and Development Waltham, MA
(bought out GelTex Pharmaceuticals in 2001)
Vice President, Chemical Research 2001-present
Senior Director, Chemical Research 1999-2001
Director of Chemical Research 1997-1999
Manager of Chemical Research 1995-1997
Group Leader 1994-1995
Senior Research Scientist 1992-1994

Helped start GelTex as second employee

Managed various research programs with multi-million dollar budgets

Supervised research chemists (17+)

Co-inventor of several polymeric pharmaceuticals and pharmaceutical candidates including
Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride (FDA approved)

Company Safety Officer for 3 years

Chemical Hygiene Officer 2000-present




1990-1992 GTE Corporation Waltham, MA
Senior Member of Technical Staff
Applied research involving polymer interfaces
Metallization of plastics
Polymer/polymer adhesion
Optical coatings



1986-1990 Lord Corporation Cary, NC
Senior Research Scientist 1988-1990
Research Scientist 1986-1988
Basic and applied research on surface chemical bonding
Developed new adhesive compositions
Developed new sol-gel coatings for corrosion resistance


HONORS AND AWARDS

Industrial Innovations Award by Northeast Region of American Chemical Society (6/2001)

National Kidney Foundation of Northern California Honoree (5/2001)

American Chemical Society/Polymer Chemistry Division Industrial Sponsors
Award (8/2000)

R&D 100 Award from R&D magazine (1999)

Sherwin Williams Award in applied polymer science (9/85)

IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)

Award for highest GPA in Chemistry Department (6/82)

Summa Cum Laude Honors in Chemistry (6/82)

Phi Lamda Epsilon (6/82)

Phi Beta Kappa (2/82)

Cornell University Dean's List (1981, 1982)

Harvard Book Club Award for highest GPA senior year (1978)

First Place in western NY ACS high school chemistry exam (1977)

1978-1979


__________________
Randy Holmes-Farley
Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central

Hobby Experience: 8 years with reefs
Current Tanks: 90 gal mixed reef
Interests: Reefkeeping, science, photography


Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM

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06/27/2003 02:44 PM

Randy Holmes-Farley
Chemistry Moderator

Registered: Apr 2001
Location: Arlington, Massachusetts
Occupation: Chemist (Drug Discovery at Genzyme)
Posts: 15282



Publications


ISSUED UNITED STATES PATENTS


1. Method for reducing oxalate. Holmes-Farley, Stephen Randall; Mandeville, III; W. Harry.
US 6,566,407; 5/20/2003

2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen Randall; Huval, Chad
Cori.
U.S. 6,517,825; 2/11/2003.

3. Method of making phosphate-binding polymers for oral administration. Holmes-Farley,
Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S. 6,509,013; 1/21/2003.

4. Combination therapy for treating hypercholesterolemia using a bile acid sequestrant
polymer
and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley, Stephen Randall;
Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.

5. Method for treating hypercholesterolemia with polyallylamine polymers. Holmes-Farley,
Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.; Goldberg, Dennis I. , US
6,423,754; 7/23/2002.

6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III; Neenan, Thomas X..;
Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.

7. Combination therapy for treating hypercholesterolemia and atherosclerosis. Huval, Chad
Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep K. U.S. 6,365,186;
4/2/2002.

8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.; Mandeville, W. H., III;
Huval; C.
C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868; 10/9/2001.

9. Polymers containing guanidinium groups as bile acid sequestrants. Dhal; P. K.; Holmes-
Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001

10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H., III.; US
6,281,252;
8/28/2001.

11. Combination therapy for treating hypercholestrolemia. Huval; C. C.; Holmes-Farley; S.
R. ;
Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.

12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.; Holmes-Farley, S.
R.; US
6,264,937; 7/24/2001.

13. Method for treating hypercholesterolemia with unsubstituted polydiallylamine polymers.
Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US 6,248,318;
6/19/2001.

14. Process for removing bile salts from a patient and alkylated compositions therefore.
Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.

15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S. R.; Dhal, P. K.;
Petersen,
J. S.; US 6,203,785; 3/20/2001.

16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.; Huval, C. C.; US
6,190,649;
2/20/2001.

17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H., III.; US
6,177,478;
1/23/2001.

18. Water-insoluble noncrosslinked bile acid sequestrants. Holmes-Farley, S. R.;
Mandeville, W.
H., III.; US 6,129,910; 10/10/2000.

19. Method for treating hypercholesterolemia with unsubstituted polydiallylamine polymers.
Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US 6,083,497;
7/4/2000.

20. Method of making phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495; 7/4/2000.

21. Process for removing bile salts from a patient and alkylated compositions therefore.
Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678; 5/23/2000.

22. Process for removing bile salts from a patient and compositions therefor. Mandeville,
W. H.,
III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.

23. Ionic polymers as anti-infective agents. Mandeville, III; W. H; Neenan; T. X.; Holmes-
Farley; S. R. US 6,034,129; 3/7/2000.

24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H., III.; US
5,985,938;
11/16/99.

25. Process for removing bile salts from a patient and compositions therefor. Mandeville,
W. H.,
III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.

26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W. H., III.;
Holmes-Farley;
S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.

27. Hydrophilic nonamine-containing and amine-containing copolymers and their use as bile
acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US 5,929,184; 7/27/99.

28. Interpenetrating polymer networks for sequestration of bile acids. Mandeville, W. H.,
III.;
Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379; 7/20/99.

29. Amine polymer sequestrant and method of cholesterol depletion. Mandeville, W. H.,
III.;
Holmes-Farley, S. R.; US 5,919,832; 7/6/99.

30. Process for removing bile salts from a patient and compositions therefor. Mandeville,
W. H.,
III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.

31. Polyamine salt hydrophobic sequestrant for cholesterol depletion. Mandeville, W. H.,
III.;
Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.

32. Process for removing bile salts from a patient and compositions therefor. Mandeville,
W. H.,
III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.

33. Preparation of polymeric sequestrants for bile acid salts. Mandeville, W. H., III.;
Holmes-
Farley, S. R.; US 5,703,188; 12/30/97.

34. Oral administration of iron-binding crosslinked amine polymers. Mandeville, W. H.,
III.;
Holmes-Farley, S. R.; US 5,702,696; 12/30/97.

35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley, S. R.; US 5,693,675;
12/2/97.

36. Method for removing bile salts from a patient with alkylated crosslinked amine
polymers,
and preparation of the polymers. Mandeville, W. H., III.; Holmes-Farley, S. R.; US
5,679,717; 10/21/97.

37. Phosphate-binding polymers for oral administration. Holmes-Farley, S. R.; Mandeville,
W.
H., III.; US 5,667,775; 9/16/97.

38. Ion-exchange process using highly crosslinked polymers for removing bile salts from a
patient, preparation of the polymers, and compositions containing them. Mandeville, W. H.,
III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.

39. Hydrophobic amine polymer sequestrant and method of cholesterol depletion. Mandeville,
W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530; 4/8/97.

40. Amine polymer sequestrant and method of cholesterol depletion. Mandeville, W. H.,
III.;
Holmes-Farley, S. R.; US 5,607,669; 3/4/97.

41. Phosphate-binding polymers for oral administration. Holmes-Farley, S. R.; Mandeville,
W.
H., III.; US 5,496,545; 3/5/96.

42. Iron-binding polymers for oral administration. Mandeville, W. H., III.; Holmes-Farley,
S. R.;
US 5,487,888; 1/30/96.

43. Ultra-thin, uniform sol-gel coating of a substrate having active hydrogens on the
surface.
Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.

44. Layered sol-gel coatings from organisilicon compounds. Holmes-Farley, S. R.; Yanyo, L.
C.;
US 5,182,143; 1/26/93.

45. Method for metal bonding using ultrathin primer coating. Holmes-Farley, S. R.; Yanyo,
L.
C.; Thuer, A. M.; US 5,139,601; 8/18/92.

46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.; US 5,096,962;
3/17/92.

47. Modified halogenatedpolyolefin adhesives for polyolefin elastomer-metal bonding.
Holmes-
Farley, S. R.; US 5,102,956; 4/7/92.



PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)


1. Aryl boronate functionalized polymers for treating obesity and inhibiting fat uptake.
Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal, Pradeep K.; Huval, Chad
Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92 pp. WO 0302571.

2. Preparation of aryl boronic acids for treating obesity. Holmes-Farley, Stephen Randall;
Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep K. (Geltex
Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.

3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley, Stephen Randall.
(Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO 0302130.

4. Method for reducing copper levels and treating copper toxicosis. Holmes-Farley, Stephen
Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002), 45 pp. WO
0285383.

5. Method for treating gout and binding uric acid. Holmes-Farley, Stephen Randall; Burke,
Steven K. WO 0285381 10/31/2002.

6. Method for treating gout and reducing serum uric acid. Holmes-Farley, Stephen Randall;
Burke, Steven K WO 0285380 10/31/2002.

7. Amine condensation polymer bile acid sequestrants. Huval, C. C.; Holmes-Farley, S. R.;
Whitesides, G. M. WO 1999-US30469; 7/6/2000.

8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and Holmes-Farley, S.
R.;
WO 1999-US5662; 9/23/1999.

9. Amine-containing copolymers as bile acid sequestrants. Holmes-Farley, S. R.; Petersen,
J. S.;
WO 9933452; 7/8/1999.

10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III and Holmes-Farley, S.
R.;
WO 9922743; 5/14/1999.

11. Polyallylamine polymers for removing bile salts and treating hypercholesterolemia, and
polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III; Burke, S. K.; Goldberg,
D. I.; WO 9857652; 12/23/98.

12. Phosphate-bidning polymers combined with a calcium supplement for oral administration.
Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley, S. R.; WO 9842355;
10/1/98.

13. Hydrophobic heteroatom-containing sequestrant for cholesterol depletion. Mandeville,
W.
H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.

14. Process for adjusting ion concentration in a patient and compositions therefor.
Mandeville,
W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.

15. Vacuum-deposited silver on polycarbonate with a chromium interlayer for improved
metal-
substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512; 1/20/94.

16. Process for increased metal-substrate bond strength in metalized plastics.
Holmes-Farley, S.
R.; Ger. Offen. 4322516; 7/6/93.

17. Electrorheological fluids and preparation of particles useful in the fluids.
Troughton,
Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J. David; Bares, Joseph
E.;
Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP 394049;
10/24/1990.

JOURNAL PUBLICATIONS

1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov, Eugene; Guo, Amy;
Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.; Mandeville, W. Harry;
Holmes-Farley, S. Randall. Kidney International (2002), 62(2), 611-619.

2. Amine functionalized polyethers as bile acid sequestrants: synthesis and biological
evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S. Randall; Mandeville, W.
Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K. Journal of
Macromolecular Science, Pure and Applied Chemistry (2001), A38(12), 1559-1574.

3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular Imprinting. Huval,
Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S. Randall; Mandeville,
W.
Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert J.; Chen, Xi; Dhal,
Pradeep K. Macromolecules (2001), 34(6), 1548-1550.

4. Synthetic polymers for the binding of fat in the intestinal tract. Jozefiak, Thomas H.;
Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia; Huval, Chad C.;
Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia. Abstracts of
Papers, 222nd ACS National Meeting, Chicago, IL, United States, August 26-30, 2001
(2001), POLY-047 and Polymer Preprints (American Chemical Society, Division of
Polymer Chemistry) (2001), 42(2), 98.

5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer gel pharmaceutical.
Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.; Ward, J.; Sacchiero,
B.;
Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.; Chen, X.; Mazzeo, J.
R.. Polym. Preprints (2000), 41(1), 735-736.

6. In vitro comparison of bile acid binding to colesevelam HCl and other bile acid
sequestrants.
Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.; Hook, P.; Holmes-
Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.

7. Novel polymeric pharmaceuticals: From startup to market. Holmes-Farley, S. R; Polym.
Mater. Sci. Eng (1999), 80, 246-247.

8. Design and characterization of of Sevelamer Hydrochloride: a novel phosphate-binding
pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward, J.; Miller, K. L.;
Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure and Appl. Chem.,
A36(7&8), p. 1085 (1999).

9. Three generations of bile acid sequestrants. Mandeville, W. H., III; Braunlin, W.;
Dhal, P.;
Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.; Rosenbaum, D.;
Sacchiero,
R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999), 550, 3-15.

10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric phosphate binder, on
urinary
phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.; Mandeville, W. H.,
III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant. (1997), 12(5)
961-964.

11. Thin anisotropic coatings based on sol-gel technology. Holmes-Farley, S. R.; Yanyo, L.
C;
Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4), 439-444.

12. The mechanism of cure initiation of a surface activated adhesive. Holmes-Farley, S.
R.;
Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.

13. Adhesion promotion and corrosion prevention using thin anisotropic coatings. Holmes-
Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2), 131-151.

14. Wetting of functionalized polyethylene having ionizable organic acids and bases at the
polymer-water interface: relations between functional group polarity, extent of
ionization,
and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.; Whitesides, G. M.;
Langmuir
(1988), 4(4), 921-937.

15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a single hydroxy group.
Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.

16. Reconstruction of the interface of oxidatively functionalized polyethylene (PE-CO2H)
and
derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo, R.; McCarthy, T. J.;
Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report (1987), AD-
A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).

17. Surface-modified polyethylene film: the relationship between surface chemistry and
physical
properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11), 4537.

18. Reactivity of carboxylic acid and ester groups in the functionalized interfacial
region of
"polyethylene carboxylic acid" (PE-CO2H) and its derivatives: differentiation of the
functional groups into shallow and deep subsets based on a comparison of contact angle and
ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir (1987), 3(1), 62-
76.

19. Fluorescence properties of dansyl groups covalently bonded tot he surface of
oxidatively
functionalized low-density polyethylene film. Holmes-Farley, S. R.; Whitesides, G. M.;
Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2; AD-A162435/2/GAR,
Gov. Rep. Announce. Index (U. S.) 1986, 86(7).

20. Acid-base behavior of carboxylic acid groups covalently attached at the surface of
polyethylene: The usefulness of contact angle in following the ionization of surface
functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.; Deutch, J.;
Whitesides,
G. M.; Langmuir (1985), 1(6), 725-740.

21. The thermal stability of a surface modified solid organic polymer. Holmes-Farley, S.
R.;
Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.



CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)

1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced Aquarist. June 2003.

2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R. Advanced Aquarist.
May
2003.

3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R. Reefkeeping May
2003.

4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping April 2003.

5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth. Holmes-Farley, R.
Advanced Aquarist; April 2003.

6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth. Holmes-Farley, R.
Advanced Aquarist; April 2003.

7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced Aquarist; March 2003.

8. How to Select a Calcium and Alkalinity Supplementation Scheme. Holmes-Farley, R.
Advanced Aquarist; February 2003.

9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January 2003.

10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; December 2002.

11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R. Advanced Aquarist; November
2002.

12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R. Advanced Aquarist;
November 2002.

13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced Aquarist, September 2002.

14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August 2002.

15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April 2002.

16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced Aquarist; July 2002

17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist; June 2002.

18. The Relationship Between Alkalinity and pH. Holmes-Farley, R. Advanced Aquarist, May
2002.

19. The Chemical & Biochemical Mechanisms of Calcification in Corals. Holmes-Farley, R.
Advanced Aquarist, April 2002.

20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.

21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.

22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January 2002.

23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers 2000.

24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium Frontiers 2000.

25. Phosphate..What is it and why should you care. Holmes-Farley, R. Aquarium Frontiers
2000.
26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium Frontiers 2000.

27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers 2000.

28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.

29. Protein Skimming: How it Works. Fishnet Library 1998.







Boomer

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[stoutman]

I never said alkalinity and buffering capacity are the same thing. When did
I say that? Now you are twisting my words.

What I said was :alkalinity is a measurement of 'buffering capacity' GET
IT?

> Hum no, maybe you should go for a look at HACH's or LaMotte website or the
book I
> suggested earlier. Please view a copy.

Another Marine Biologist. I don't think so.


> You are confusing Acidity and Acidity as you know little about water
chemistry and
> procedures and test methods

I'm confusing 'Acidity' and 'Acidity' What? Ok, now I really think you
are an idiot.

> Like Buffering Capacity you have your Acidity's mixed up

ACIDITY IS the opposite of BASICITY. You are an idiot!

> BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write this
book, there are
> over 100 of them, they are wrong.


Ok, if that's what they think than they are wrong. I haven't read there
books, I will take your word for it. If their logic is the same as yours,
their WRONG as well.

> Christ, there you go again with the FW ****. All your numbers are wrong we
are dealing
> with SEAWATER

You didn't say in your experiment that sea water was being used. The HH
equation STILL applies.

> Oh, by the way. Your websites, I have about 50 on these issues, I could
post them, not to
> mention I have all those water chemistry books, so there is no need to
view your sites.

I could of posted more web sites for ya, but I didn't want you to get even
more confused than you already are. I tried to keep it simple for ya. Did
you go to those web pages and actually read them? Maybe you should send
them an e-mail and tell them their web pages are wrong and that they are
offending all the marine biologists across the country.

> Finally are you afraid to come to our Chemistry Forum, afraid to get
slapped by REAL
> chemists. I get a charge out of you can't post your ref .I have posted the
same or similar
> stuff on his forum and I wasn't pointed out WRONG pal. I have 1500 posts
there and am the
> biggest contributor to his forum other than himself or maybe Habib Sheka

No Boomer. I'm not afraid, just VERY uninterested in explaining chemistry
to other LAYMAN such as yourself. I use to get paid this in grad school
(tutoring).

Why are you posting someone elses C.V.? Is that meant to impress me? I'm
writing to Boomer right? Not RANDY HOLMES-FARLEY. Right? If you want to
post a C.V., why not post yours? I'm sure it's just as impressive, right?

GET A CLUE!







"Boomer" > wrote in message
...
> Now I am getting bored
>
> "Don't the components of a buffer account for the buffering capacity?
Yes."
>
> Yes, agreed but you seem to fail what I'm saying. Buffering Capacity and
Alkalinity are
> not the same, that has always been the issue. I gave the equation does
that look like an
> Alkalinity equation or how Alk is determined. I see you had now comments
on it what's
> wrong, why no comments on the equations I gave. Don't understand them or
what ? Again this
> is the equation for Buffering Capacity, also called Buffer Index or Buffer
Intensity. It
> is defined in most water chemistry and chemical oceanography text books.
>
> B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> This is not Alkalinity now is it ?
>
> "I know how to do a titration, In fact I have done several. How many have
> you actually done? I don't mean by counting drops, I mean with a buret?"
>
> Well good for you, I use a Digital Titrator
>
> "Oh, I see,
> you think acidity is the opposite of alkalinity. In the world of
CHEMISTRY
> it's not. Maybe in aquarium newsgroups it is.
>
> Hum no, maybe you should go for a look at HACH's or LaMotte website or the
book I
> suggested earlier. Please view a copy.
>
> Standard Methods for the Examination of Water and Wastewater
>
> This book, over 2000 pages, is the guide for water testing. If you are
reporting water
> test to the EPA you must use approved std from this text.I t is prepared
and published by
> the EPA, American Water Works Association and American Public Health
Association. You
> mean you don't have one and the issue is water chemistry
>
> You are confusing Acidity and Acidity as you know little about water
chemistry and
> procedures and test methods
>
> From SMEWW, section 2-30, 2310 ACIDITY
>
> "Acidity of water is its quantative capacity to react with a strong base
to a designated
> pH"
>
> This is how you test for it
>
> A std alkali titration to methyl orange or phenolphthalein
> endpoint.
>
> BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write this
book, there are
> over 100 of them, they are wrong.
>
> Like Buffering Capacity you have your Acidity's mixed up
> In water measurement if you have a high Alk you also usually have a high
Acidity.
> Normally a high Alk also gives a higher CO2 level. Get a WATER CHEMISTRY
BOOK there pal.
>
>
> "These are all in equilibrium with each other. An initial high pH (above
> 6.4) will shift the equilibrium to the right to form HCO3-1. If the pH of
> the solution is above 10.3 (pKa2) the .........."
>
>
> Christ, there you go again with the FW ****. All your numbers are wrong we
are dealing
> with SEAWATER
>
> This means that at a pH of 8.3, the majority of the CO2(aq) is in the form
> of HCO3-1 .
>
> I have already pointed that out and gave actual values at know seawater
levels, go back
> and re-read it you aren't telling me anything here.Of course most is HCO3
see...
>
>
> @ 20C and 34.3 ppt salinity
>
> CO2 = 0.52 %
>
> HCO3 = 86.4 %
>
> CO3 = 13.09 %
>
>
> "In your glass experiment you managed to lower the pH enough to purge out
CO2
> by boiling"
>
> The purpose behind the glass is to show that alk is not affect by CO2 and
vise-versa and
> how Co2 affects pH.
>
> Now, in a real life seawater aquarium, with a pH of 8.3 and that pH drops
to say 8.1 it is
> usually due to excess CO2. If you took a glass of that water and aerated
it you WILL drive
> off the CO2 and raise the pH. It has been done a proven a million times.
>
> "In order to 'purge' CO2 you would need to lower the
> pH to shift the equilibrium to below 6.4"
>
> The hell you do !!!.Do you know who many times people on this NG to
include Dr. Craig
> Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
sample of aquarium
> water and aerate it to see if the pH GOES UP AND when they come back with
the test it is
> often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST excess
CO2 in the tank
> water, increase the circulation for better gas exchange at the surface,
reduce feeding,
> and try to improve on better skimming, thus reducing the bio-load and pH
decline due to
> CO2.
>
>
> "I hope this helps. "
>
> Help, how can you when you miss everything. I should be charging you
>
> Oh, by the way. Your websites, I have about 50 on these issues, I could
post them, not to
> mention I have all those water chemistry books, so there is no need to
view your sites.
>
> Finally are you afraid to come to our Chemistry Forum, afraid to get
slapped by REAL
> chemists. I get a charge out of you can't post your ref .I have posted the
same or similar
> stuff on his forum and I wasn't pointed out WRONG pal. I have 1500 posts
there and am the
> biggest contributor to his forum other than himself or maybe Habib Sheka
>
> Hum, here are Randy's ref that he posted. He hosts the website
>
> S. RANDY HOLMES-FARLEY
> Arlington, Massachusetts
>
> EDUCATION
>
> 1982-1986 Harvard University Cambridge, MA
> PhD in Chemistry
> Research Advisor: George Whitesides
>
> Investigated the relationship between polymer surface chemistry and
physical properties
> through controlled surface modification and testing.
>
> 1980-1982 Cornell University Ithaca, NY
> BA in Chemistry and Biology
> Graduated Summa Cum Laude
> Distinction in All Subjects
> Grade Point: 3.94/4.0
> Honors research: isolation and characterization of the subunit of CF1
enzyme
>
>
> 1978-1979 Stanford University Palo Alto, CA
> Grade Point: 3.55/4.0
>
>
> EXPERIENCE
>
> 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> (bought out GelTex Pharmaceuticals in 2001)
> Vice President, Chemical Research 2001-present
> Senior Director, Chemical Research 1999-2001
> Director of Chemical Research 1997-1999
> Manager of Chemical Research 1995-1997
> Group Leader 1994-1995
> Senior Research Scientist 1992-1994
>
> Helped start GelTex as second employee
>
> Managed various research programs with multi-million dollar budgets
>
> Supervised research chemists (17+)
>
> Co-inventor of several polymeric pharmaceuticals and pharmaceutical
candidates including
> Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride (FDA
approved)
>
> Company Safety Officer for 3 years
>
> Chemical Hygiene Officer 2000-present
>
>
>
>
> 1990-1992 GTE Corporation Waltham, MA
> Senior Member of Technical Staff
> Applied research involving polymer interfaces
> Metallization of plastics
> Polymer/polymer adhesion
> Optical coatings
>
>
>
> 1986-1990 Lord Corporation Cary, NC
> Senior Research Scientist 1988-1990
> Research Scientist 1986-1988
> Basic and applied research on surface chemical bonding
> Developed new adhesive compositions
> Developed new sol-gel coatings for corrosion resistance
>
>
> HONORS AND AWARDS
>
> Industrial Innovations Award by Northeast Region of American Chemical
Society (6/2001)
>
> National Kidney Foundation of Northern California Honoree (5/2001)
>
> American Chemical Society/Polymer Chemistry Division Industrial Sponsors
> Award (8/2000)
>
> R&D 100 Award from R&D magazine (1999)
>
> Sherwin Williams Award in applied polymer science (9/85)
>
> IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
>
> Award for highest GPA in Chemistry Department (6/82)
>
> Summa Cum Laude Honors in Chemistry (6/82)
>
> Phi Lamda Epsilon (6/82)
>
> Phi Beta Kappa (2/82)
>
> Cornell University Dean's List (1981, 1982)
>
> Harvard Book Club Award for highest GPA senior year (1978)
>
> First Place in western NY ACS high school chemistry exam (1977)
>
> 1978-1979
>
>
> __________________
> Randy Holmes-Farley
> Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
>
> Hobby Experience: 8 years with reefs
> Current Tanks: 90 gal mixed reef
> Interests: Reefkeeping, science, photography
>
>
> Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
>
> Open this post in a new window | Report this post to a moderator | IP:
Logged
>
>
>
> 06/27/2003 02:44 PM
>
> Randy Holmes-Farley
> Chemistry Moderator
>
> Registered: Apr 2001
> Location: Arlington, Massachusetts
> Occupation: Chemist (Drug Discovery at Genzyme)
> Posts: 15282
>
>
>
> Publications
>
>
> ISSUED UNITED STATES PATENTS
>
>
> 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
Mandeville, III; W. Harry.
> US 6,566,407; 5/20/2003
>
> 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen Randall;
Huval, Chad
> Cori.
> U.S. 6,517,825; 2/11/2003.
>
> 3. Method of making phosphate-binding polymers for oral administration.
Holmes-Farley,
> Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
6,509,013; 1/21/2003.
>
> 4. Combination therapy for treating hypercholesterolemia using a bile acid
sequestrant
> polymer
> and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley, Stephen
Randall;
> Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
>
> 5. Method for treating hypercholesterolemia with polyallylamine polymers.
Holmes-Farley,
> Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.; Goldberg,
Dennis I. , US
> 6,423,754; 7/23/2002.
>
> 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
Neenan, Thomas X..;
> Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
>
> 7. Combination therapy for treating hypercholesterolemia and
atherosclerosis. Huval, Chad
> Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep K.
U.S. 6,365,186;
> 4/2/2002.
>
> 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.; Mandeville,
W. H., III;
> Huval; C.
> C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
10/9/2001.
>
> 9. Polymers containing guanidinium groups as bile acid sequestrants. Dhal;
P. K.; Holmes-
> Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
>
> 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 6,281,252;
> 8/28/2001.
>
> 11. Combination therapy for treating hypercholestrolemia. Huval; C. C.;
Holmes-Farley; S.
> R. ;
> Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
>
> 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
Holmes-Farley, S.
> R.; US
> 6,264,937; 7/24/2001.
>
> 13. Method for treating hypercholesterolemia with unsubstituted
polydiallylamine polymers.
> Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
6,248,318;
> 6/19/2001.
>
> 14. Process for removing bile salts from a patient and alkylated
compositions therefore.
> Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
>
> 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S. R.;
Dhal, P. K.;
> Petersen,
> J. S.; US 6,203,785; 3/20/2001.
>
> 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.; Huval,
C. C.; US
> 6,190,649;
> 2/20/2001.
>
> 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 6,177,478;
> 1/23/2001.
>
> 18. Water-insoluble noncrosslinked bile acid sequestrants. Holmes-Farley,
S. R.;
> Mandeville, W.
> H., III.; US 6,129,910; 10/10/2000.
>
> 19. Method for treating hypercholesterolemia with unsubstituted
polydiallylamine polymers.
> Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
6,083,497;
> 7/4/2000.
>
> 20. Method of making phosphate-binding polymers for oral administration.
Holmes-Farley, S.
> R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495; 7/4/2000.
>
> 21. Process for removing bile salts from a patient and alkylated
compositions therefore.
> Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678; 5/23/2000.
>
> 22. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
>
> 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
Neenan; T. X.; Holmes-
> Farley; S. R. US 6,034,129; 3/7/2000.
>
> 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 5,985,938;
> 11/16/99.
>
> 25. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
>
> 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W. H.,
III.;
> Holmes-Farley;
> S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
>
> 27. Hydrophilic nonamine-containing and amine-containing copolymers and
their use as bile
> acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US 5,929,184;
7/27/99.
>
> 28. Interpenetrating polymer networks for sequestration of bile acids.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
7/20/99.
>
> 29. Amine polymer sequestrant and method of cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
>
> 30. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
>
> 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
>
> 32. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
>
> 33. Preparation of polymeric sequestrants for bile acid salts. Mandeville,
W. H., III.;
> Holmes-
> Farley, S. R.; US 5,703,188; 12/30/97.
>
> 34. Oral administration of iron-binding crosslinked amine polymers.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
>
> 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley, S.
R.; US 5,693,675;
> 12/2/97.
>
> 36. Method for removing bile salts from a patient with alkylated
crosslinked amine
> polymers,
> and preparation of the polymers. Mandeville, W. H., III.; Holmes-Farley,
S. R.; US
> 5,679,717; 10/21/97.
>
> 37. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville,
> W.
> H., III.; US 5,667,775; 9/16/97.
>
> 38. Ion-exchange process using highly crosslinked polymers for removing
bile salts from a
> patient, preparation of the polymers, and compositions containing them.
Mandeville, W. H.,
> III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
>
> 39. Hydrophobic amine polymer sequestrant and method of cholesterol
depletion. Mandeville,
> W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530; 4/8/97.
>
> 40. Amine polymer sequestrant and method of cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
>
> 41. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville,
> W.
> H., III.; US 5,496,545; 3/5/96.
>
> 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
III.; Holmes-Farley,
> S. R.;
> US 5,487,888; 1/30/96.
>
> 43. Ultra-thin, uniform sol-gel coating of a substrate having active
hydrogens on the
> surface.
> Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
>
> 44. Layered sol-gel coatings from organisilicon compounds. Holmes-Farley,
S. R.; Yanyo, L.
> C.;
> US 5,182,143; 1/26/93.
>
> 45. Method for metal bonding using ultrathin primer coating.
Holmes-Farley, S. R.; Yanyo,
> L.
> C.; Thuer, A. M.; US 5,139,601; 8/18/92.
>
> 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.; US
5,096,962;
> 3/17/92.
>
> 47. Modified halogenatedpolyolefin adhesives for polyolefin
elastomer-metal bonding.
> Holmes-
> Farley, S. R.; US 5,102,956; 4/7/92.
>
>
>
> PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
>
>
> 1. Aryl boronate functionalized polymers for treating obesity and
inhibiting fat uptake.
> Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal, Pradeep
K.; Huval, Chad
> Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92 pp. WO
0302571.
>
> 2. Preparation of aryl boronic acids for treating obesity. Holmes-Farley,
Stephen Randall;
> Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep K.
(Geltex
> Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
>
> 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
Stephen Randall.
> (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
0302130.
>
> 4. Method for reducing copper levels and treating copper toxicosis.
Holmes-Farley, Stephen
> Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002), 45
pp. WO
> 0285383.
>
> 5. Method for treating gout and binding uric acid. Holmes-Farley, Stephen
Randall; Burke,
> Steven K. WO 0285381 10/31/2002.
>
> 6. Method for treating gout and reducing serum uric acid. Holmes-Farley,
Stephen Randall;
> Burke, Steven K WO 0285380 10/31/2002.
>
> 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
Holmes-Farley, S. R.;
> Whitesides, G. M. WO 1999-US30469; 7/6/2000.
>
> 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
Holmes-Farley, S.
> R.;
> WO 1999-US5662; 9/23/1999.
>
> 9. Amine-containing copolymers as bile acid sequestrants. Holmes-Farley,
S. R.; Petersen,
> J. S.;
> WO 9933452; 7/8/1999.
>
> 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III and
Holmes-Farley, S.
> R.;
> WO 9922743; 5/14/1999.
>
> 11. Polyallylamine polymers for removing bile salts and treating
hypercholesterolemia, and
> polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III; Burke,
S. K.; Goldberg,
> D. I.; WO 9857652; 12/23/98.
>
> 12. Phosphate-bidning polymers combined with a calcium supplement for oral
administration.
> Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley, S.
R.; WO 9842355;
> 10/1/98.
>
> 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
depletion. Mandeville,
> W.
> H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
>
> 14. Process for adjusting ion concentration in a patient and compositions
therefor.
> Mandeville,
> W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
>
> 15. Vacuum-deposited silver on polycarbonate with a chromium interlayer
for improved
> metal-
> substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512; 1/20/94.
>
> 16. Process for increased metal-substrate bond strength in metalized
plastics.
> Holmes-Farley, S.
> R.; Ger. Offen. 4322516; 7/6/93.
>
> 17. Electrorheological fluids and preparation of particles useful in the
fluids.
> Troughton,
> Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
David; Bares, Joseph
> E.;
> Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
394049;
> 10/24/1990.
>
> JOURNAL PUBLICATIONS
>
> 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov, Eugene;
Guo, Amy;
> Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
Mandeville, W. Harry;
> Holmes-Farley, S. Randall. Kidney International (2002), 62(2), 611-619.
>
> 2. Amine functionalized polyethers as bile acid sequestrants: synthesis
and biological
> evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S. Randall;
Mandeville, W.
> Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
Journal of
> Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
1559-1574.
>
> 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
Imprinting. Huval,
> Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
Randall; Mandeville,
> W.
> Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert J.;
Chen, Xi; Dhal,
> Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
>
> 4. Synthetic polymers for the binding of fat in the intestinal tract.
Jozefiak, Thomas H.;
> Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia; Huval,
Chad C.;
> Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
Abstracts of
> Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
26-30, 2001
> (2001), POLY-047 and Polymer Preprints (American Chemical Society,
Division of
> Polymer Chemistry) (2001), 42(2), 98.
>
> 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer gel
pharmaceutical.
> Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.; Ward,
J.; Sacchiero,
> B.;
> Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.; Chen,
X.; Mazzeo, J.
> R.. Polym. Preprints (2000), 41(1), 735-736.
>
> 6. In vitro comparison of bile acid binding to colesevelam HCl and other
bile acid
> sequestrants.
> Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
Hook, P.; Holmes-
> Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
>
> 7. Novel polymeric pharmaceuticals: From startup to market. Holmes-Farley,
S. R; Polym.
> Mater. Sci. Eng (1999), 80, 246-247.
>
> 8. Design and characterization of of Sevelamer Hydrochloride: a novel
phosphate-binding
> pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward, J.;
Miller, K. L.;
> Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure and
Appl. Chem.,
> A36(7&8), p. 1085 (1999).
>
> 9. Three generations of bile acid sequestrants. Mandeville, W. H., III;
Braunlin, W.;
> Dhal, P.;
> Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
Rosenbaum, D.;
> Sacchiero,
> R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
550, 3-15.
>
> 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric phosphate
binder, on
> urinary
> phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
Mandeville, W. H.,
> III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
(1997), 12(5)
> 961-964.
>
> 11. Thin anisotropic coatings based on sol-gel technology. Holmes-Farley,
S. R.; Yanyo, L.
> C;
> Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4), 439-444.
>
> 12. The mechanism of cure initiation of a surface activated adhesive.
Holmes-Farley, S.
> R.;
> Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
>
> 13. Adhesion promotion and corrosion prevention using thin anisotropic
coatings. Holmes-
> Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
131-151.
>
> 14. Wetting of functionalized polyethylene having ionizable organic acids
and bases at the
> polymer-water interface: relations between functional group polarity,
extent of
> ionization,
> and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
Whitesides, G. M.;
> Langmuir
> (1988), 4(4), 921-937.
>
> 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
single hydroxy group.
> Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
>
> 16. Reconstruction of the interface of oxidatively functionalized
polyethylene (PE-CO2H)
> and
> derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo, R.;
McCarthy, T. J.;
> Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report (1987),
AD-
> A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
>
> 17. Surface-modified polyethylene film: the relationship between surface
chemistry and
> physical
> properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11), 4537.
>
> 18. Reactivity of carboxylic acid and ester groups in the functionalized
interfacial
> region of
> "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
differentiation of the
> functional groups into shallow and deep subsets based on a comparison of
contact angle and
> ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
(1987), 3(1), 62-
> 76.
>
> 19. Fluorescence properties of dansyl groups covalently bonded tot he
surface of
> oxidatively
> functionalized low-density polyethylene film. Holmes-Farley, S. R.;
Whitesides, G. M.;
> Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
AD-A162435/2/GAR,
> Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
>
> 20. Acid-base behavior of carboxylic acid groups covalently attached at
the surface of
> polyethylene: The usefulness of contact angle in following the ionization
of surface
> functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
Deutch, J.;
> Whitesides,
> G. M.; Langmuir (1985), 1(6), 725-740.
>
> 21. The thermal stability of a surface modified solid organic polymer.
Holmes-Farley, S.
> R.;
> Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
>
>
>
> CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
>
> 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
Aquarist. June 2003.
>
> 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
Advanced Aquarist.
> May
> 2003.
>
> 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
Reefkeeping May
> 2003.
>
> 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
April 2003.
>
> 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
Holmes-Farley, R.
> Advanced Aquarist; April 2003.
>
> 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
Holmes-Farley, R.
> Advanced Aquarist; April 2003.
>
> 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced Aquarist;
March 2003.
>
> 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
Holmes-Farley, R.
> Advanced Aquarist; February 2003.
>
> 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
2003.
>
> 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; December
2002.
>
> 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R. Advanced
Aquarist; November
> 2002.
>
> 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
Advanced Aquarist;
> November 2002.
>
> 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced Aquarist,
September 2002.
>
> 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
2002.
>
> 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
2002.
>
> 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
Aquarist; July 2002
>
> 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist; June
2002.
>
> 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R. Advanced
Aquarist, May
> 2002.
>
> 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
Holmes-Farley, R.
> Advanced Aquarist, April 2002.
>
> 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
>
> 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
>
> 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January 2002.
>
> 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
2000.
>
> 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
Frontiers 2000.
>
> 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
Aquarium Frontiers
> 2000.
> 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium Frontiers
2000.
>
> 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers 2000.
>
> 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
>
> 29. Protein Skimming: How it Works. Fishnet Library 1998.
>
>
>
>
>
>
>
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
>
>

[stoutman]

http://kywater.org/ww/ramp/rmalk.htm

READ THE VERY FIRST LINE BOOMER!!!!!













"Boomer" > wrote in message
...
> Now I am getting bored
>
> "Don't the components of a buffer account for the buffering capacity?
Yes."
>
> Yes, agreed but you seem to fail what I'm saying. Buffering Capacity and
Alkalinity are
> not the same, that has always been the issue. I gave the equation does
that look like an
> Alkalinity equation or how Alk is determined. I see you had now comments
on it what's
> wrong, why no comments on the equations I gave. Don't understand them or
what ? Again this
> is the equation for Buffering Capacity, also called Buffer Index or Buffer
Intensity. It
> is defined in most water chemistry and chemical oceanography text books.
>
> B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> This is not Alkalinity now is it ?
>
> "I know how to do a titration, In fact I have done several. How many have
> you actually done? I don't mean by counting drops, I mean with a buret?"
>
> Well good for you, I use a Digital Titrator
>
> "Oh, I see,
> you think acidity is the opposite of alkalinity. In the world of
CHEMISTRY
> it's not. Maybe in aquarium newsgroups it is.
>
> Hum no, maybe you should go for a look at HACH's or LaMotte website or the
book I
> suggested earlier. Please view a copy.
>
> Standard Methods for the Examination of Water and Wastewater
>
> This book, over 2000 pages, is the guide for water testing. If you are
reporting water
> test to the EPA you must use approved std from this text.I t is prepared
and published by
> the EPA, American Water Works Association and American Public Health
Association. You
> mean you don't have one and the issue is water chemistry
>
> You are confusing Acidity and Acidity as you know little about water
chemistry and
> procedures and test methods
>
> From SMEWW, section 2-30, 2310 ACIDITY
>
> "Acidity of water is its quantative capacity to react with a strong base
to a designated
> pH"
>
> This is how you test for it
>
> A std alkali titration to methyl orange or phenolphthalein
> endpoint.
>
> BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write this
book, there are
> over 100 of them, they are wrong.
>
> Like Buffering Capacity you have your Acidity's mixed up
> In water measurement if you have a high Alk you also usually have a high
Acidity.
> Normally a high Alk also gives a higher CO2 level. Get a WATER CHEMISTRY
BOOK there pal.
>
>
> "These are all in equilibrium with each other. An initial high pH (above
> 6.4) will shift the equilibrium to the right to form HCO3-1. If the pH of
> the solution is above 10.3 (pKa2) the .........."
>
>
> Christ, there you go again with the FW ****. All your numbers are wrong we
are dealing
> with SEAWATER
>
> This means that at a pH of 8.3, the majority of the CO2(aq) is in the form
> of HCO3-1 .
>
> I have already pointed that out and gave actual values at know seawater
levels, go back
> and re-read it you aren't telling me anything here.Of course most is HCO3
see...
>
>
> @ 20C and 34.3 ppt salinity
>
> CO2 = 0.52 %
>
> HCO3 = 86.4 %
>
> CO3 = 13.09 %
>
>
> "In your glass experiment you managed to lower the pH enough to purge out
CO2
> by boiling"
>
> The purpose behind the glass is to show that alk is not affect by CO2 and
vise-versa and
> how Co2 affects pH.
>
> Now, in a real life seawater aquarium, with a pH of 8.3 and that pH drops
to say 8.1 it is
> usually due to excess CO2. If you took a glass of that water and aerated
it you WILL drive
> off the CO2 and raise the pH. It has been done a proven a million times.
>
> "In order to 'purge' CO2 you would need to lower the
> pH to shift the equilibrium to below 6.4"
>
> The hell you do !!!.Do you know who many times people on this NG to
include Dr. Craig
> Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
sample of aquarium
> water and aerate it to see if the pH GOES UP AND when they come back with
the test it is
> often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST excess
CO2 in the tank
> water, increase the circulation for better gas exchange at the surface,
reduce feeding,
> and try to improve on better skimming, thus reducing the bio-load and pH
decline due to
> CO2.
>
>
> "I hope this helps. "
>
> Help, how can you when you miss everything. I should be charging you
>
> Oh, by the way. Your websites, I have about 50 on these issues, I could
post them, not to
> mention I have all those water chemistry books, so there is no need to
view your sites.
>
> Finally are you afraid to come to our Chemistry Forum, afraid to get
slapped by REAL
> chemists. I get a charge out of you can't post your ref .I have posted the
same or similar
> stuff on his forum and I wasn't pointed out WRONG pal. I have 1500 posts
there and am the
> biggest contributor to his forum other than himself or maybe Habib Sheka
>
> Hum, here are Randy's ref that he posted. He hosts the website
>
> S. RANDY HOLMES-FARLEY
> Arlington, Massachusetts
>
> EDUCATION
>
> 1982-1986 Harvard University Cambridge, MA
> PhD in Chemistry
> Research Advisor: George Whitesides
>
> Investigated the relationship between polymer surface chemistry and
physical properties
> through controlled surface modification and testing.
>
> 1980-1982 Cornell University Ithaca, NY
> BA in Chemistry and Biology
> Graduated Summa Cum Laude
> Distinction in All Subjects
> Grade Point: 3.94/4.0
> Honors research: isolation and characterization of the subunit of CF1
enzyme
>
>
> 1978-1979 Stanford University Palo Alto, CA
> Grade Point: 3.55/4.0
>
>
> EXPERIENCE
>
> 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> (bought out GelTex Pharmaceuticals in 2001)
> Vice President, Chemical Research 2001-present
> Senior Director, Chemical Research 1999-2001
> Director of Chemical Research 1997-1999
> Manager of Chemical Research 1995-1997
> Group Leader 1994-1995
> Senior Research Scientist 1992-1994
>
> Helped start GelTex as second employee
>
> Managed various research programs with multi-million dollar budgets
>
> Supervised research chemists (17+)
>
> Co-inventor of several polymeric pharmaceuticals and pharmaceutical
candidates including
> Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride (FDA
approved)
>
> Company Safety Officer for 3 years
>
> Chemical Hygiene Officer 2000-present
>
>
>
>
> 1990-1992 GTE Corporation Waltham, MA
> Senior Member of Technical Staff
> Applied research involving polymer interfaces
> Metallization of plastics
> Polymer/polymer adhesion
> Optical coatings
>
>
>
> 1986-1990 Lord Corporation Cary, NC
> Senior Research Scientist 1988-1990
> Research Scientist 1986-1988
> Basic and applied research on surface chemical bonding
> Developed new adhesive compositions
> Developed new sol-gel coatings for corrosion resistance
>
>
> HONORS AND AWARDS
>
> Industrial Innovations Award by Northeast Region of American Chemical
Society (6/2001)
>
> National Kidney Foundation of Northern California Honoree (5/2001)
>
> American Chemical Society/Polymer Chemistry Division Industrial Sponsors
> Award (8/2000)
>
> R&D 100 Award from R&D magazine (1999)
>
> Sherwin Williams Award in applied polymer science (9/85)
>
> IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
>
> Award for highest GPA in Chemistry Department (6/82)
>
> Summa Cum Laude Honors in Chemistry (6/82)
>
> Phi Lamda Epsilon (6/82)
>
> Phi Beta Kappa (2/82)
>
> Cornell University Dean's List (1981, 1982)
>
> Harvard Book Club Award for highest GPA senior year (1978)
>
> First Place in western NY ACS high school chemistry exam (1977)
>
> 1978-1979
>
>
> __________________
> Randy Holmes-Farley
> Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
>
> Hobby Experience: 8 years with reefs
> Current Tanks: 90 gal mixed reef
> Interests: Reefkeeping, science, photography
>
>
> Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
>
> Open this post in a new window | Report this post to a moderator | IP:
Logged
>
>
>
> 06/27/2003 02:44 PM
>
> Randy Holmes-Farley
> Chemistry Moderator
>
> Registered: Apr 2001
> Location: Arlington, Massachusetts
> Occupation: Chemist (Drug Discovery at Genzyme)
> Posts: 15282
>
>
>
> Publications
>
>
> ISSUED UNITED STATES PATENTS
>
>
> 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
Mandeville, III; W. Harry.
> US 6,566,407; 5/20/2003
>
> 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen Randall;
Huval, Chad
> Cori.
> U.S. 6,517,825; 2/11/2003.
>
> 3. Method of making phosphate-binding polymers for oral administration.
Holmes-Farley,
> Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
6,509,013; 1/21/2003.
>
> 4. Combination therapy for treating hypercholesterolemia using a bile acid
sequestrant
> polymer
> and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley, Stephen
Randall;
> Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
>
> 5. Method for treating hypercholesterolemia with polyallylamine polymers.
Holmes-Farley,
> Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.; Goldberg,
Dennis I. , US
> 6,423,754; 7/23/2002.
>
> 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
Neenan, Thomas X..;
> Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
>
> 7. Combination therapy for treating hypercholesterolemia and
atherosclerosis. Huval, Chad
> Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep K.
U.S. 6,365,186;
> 4/2/2002.
>
> 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.; Mandeville,
W. H., III;
> Huval; C.
> C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
10/9/2001.
>
> 9. Polymers containing guanidinium groups as bile acid sequestrants. Dhal;
P. K.; Holmes-
> Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
>
> 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 6,281,252;
> 8/28/2001.
>
> 11. Combination therapy for treating hypercholestrolemia. Huval; C. C.;
Holmes-Farley; S.
> R. ;
> Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
>
> 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
Holmes-Farley, S.
> R.; US
> 6,264,937; 7/24/2001.
>
> 13. Method for treating hypercholesterolemia with unsubstituted
polydiallylamine polymers.
> Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
6,248,318;
> 6/19/2001.
>
> 14. Process for removing bile salts from a patient and alkylated
compositions therefore.
> Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
>
> 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S. R.;
Dhal, P. K.;
> Petersen,
> J. S.; US 6,203,785; 3/20/2001.
>
> 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.; Huval,
C. C.; US
> 6,190,649;
> 2/20/2001.
>
> 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 6,177,478;
> 1/23/2001.
>
> 18. Water-insoluble noncrosslinked bile acid sequestrants. Holmes-Farley,
S. R.;
> Mandeville, W.
> H., III.; US 6,129,910; 10/10/2000.
>
> 19. Method for treating hypercholesterolemia with unsubstituted
polydiallylamine polymers.
> Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
6,083,497;
> 7/4/2000.
>
> 20. Method of making phosphate-binding polymers for oral administration.
Holmes-Farley, S.
> R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495; 7/4/2000.
>
> 21. Process for removing bile salts from a patient and alkylated
compositions therefore.
> Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678; 5/23/2000.
>
> 22. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
>
> 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
Neenan; T. X.; Holmes-
> Farley; S. R. US 6,034,129; 3/7/2000.
>
> 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 5,985,938;
> 11/16/99.
>
> 25. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
>
> 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W. H.,
III.;
> Holmes-Farley;
> S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
>
> 27. Hydrophilic nonamine-containing and amine-containing copolymers and
their use as bile
> acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US 5,929,184;
7/27/99.
>
> 28. Interpenetrating polymer networks for sequestration of bile acids.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
7/20/99.
>
> 29. Amine polymer sequestrant and method of cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
>
> 30. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
>
> 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
>
> 32. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
>
> 33. Preparation of polymeric sequestrants for bile acid salts. Mandeville,
W. H., III.;
> Holmes-
> Farley, S. R.; US 5,703,188; 12/30/97.
>
> 34. Oral administration of iron-binding crosslinked amine polymers.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
>
> 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley, S.
R.; US 5,693,675;
> 12/2/97.
>
> 36. Method for removing bile salts from a patient with alkylated
crosslinked amine
> polymers,
> and preparation of the polymers. Mandeville, W. H., III.; Holmes-Farley,
S. R.; US
> 5,679,717; 10/21/97.
>
> 37. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville,
> W.
> H., III.; US 5,667,775; 9/16/97.
>
> 38. Ion-exchange process using highly crosslinked polymers for removing
bile salts from a
> patient, preparation of the polymers, and compositions containing them.
Mandeville, W. H.,
> III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
>
> 39. Hydrophobic amine polymer sequestrant and method of cholesterol
depletion. Mandeville,
> W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530; 4/8/97.
>
> 40. Amine polymer sequestrant and method of cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
>
> 41. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville,
> W.
> H., III.; US 5,496,545; 3/5/96.
>
> 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
III.; Holmes-Farley,
> S. R.;
> US 5,487,888; 1/30/96.
>
> 43. Ultra-thin, uniform sol-gel coating of a substrate having active
hydrogens on the
> surface.
> Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
>
> 44. Layered sol-gel coatings from organisilicon compounds. Holmes-Farley,
S. R.; Yanyo, L.
> C.;
> US 5,182,143; 1/26/93.
>
> 45. Method for metal bonding using ultrathin primer coating.
Holmes-Farley, S. R.; Yanyo,
> L.
> C.; Thuer, A. M.; US 5,139,601; 8/18/92.
>
> 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.; US
5,096,962;
> 3/17/92.
>
> 47. Modified halogenatedpolyolefin adhesives for polyolefin
elastomer-metal bonding.
> Holmes-
> Farley, S. R.; US 5,102,956; 4/7/92.
>
>
>
> PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
>
>
> 1. Aryl boronate functionalized polymers for treating obesity and
inhibiting fat uptake.
> Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal, Pradeep
K.; Huval, Chad
> Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92 pp. WO
0302571.
>
> 2. Preparation of aryl boronic acids for treating obesity. Holmes-Farley,
Stephen Randall;
> Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep K.
(Geltex
> Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
>
> 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
Stephen Randall.
> (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
0302130.
>
> 4. Method for reducing copper levels and treating copper toxicosis.
Holmes-Farley, Stephen
> Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002), 45
pp. WO
> 0285383.
>
> 5. Method for treating gout and binding uric acid. Holmes-Farley, Stephen
Randall; Burke,
> Steven K. WO 0285381 10/31/2002.
>
> 6. Method for treating gout and reducing serum uric acid. Holmes-Farley,
Stephen Randall;
> Burke, Steven K WO 0285380 10/31/2002.
>
> 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
Holmes-Farley, S. R.;
> Whitesides, G. M. WO 1999-US30469; 7/6/2000.
>
> 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
Holmes-Farley, S.
> R.;
> WO 1999-US5662; 9/23/1999.
>
> 9. Amine-containing copolymers as bile acid sequestrants. Holmes-Farley,
S. R.; Petersen,
> J. S.;
> WO 9933452; 7/8/1999.
>
> 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III and
Holmes-Farley, S.
> R.;
> WO 9922743; 5/14/1999.
>
> 11. Polyallylamine polymers for removing bile salts and treating
hypercholesterolemia, and
> polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III; Burke,
S. K.; Goldberg,
> D. I.; WO 9857652; 12/23/98.
>
> 12. Phosphate-bidning polymers combined with a calcium supplement for oral
administration.
> Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley, S.
R.; WO 9842355;
> 10/1/98.
>
> 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
depletion. Mandeville,
> W.
> H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
>
> 14. Process for adjusting ion concentration in a patient and compositions
therefor.
> Mandeville,
> W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
>
> 15. Vacuum-deposited silver on polycarbonate with a chromium interlayer
for improved
> metal-
> substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512; 1/20/94.
>
> 16. Process for increased metal-substrate bond strength in metalized
plastics.
> Holmes-Farley, S.
> R.; Ger. Offen. 4322516; 7/6/93.
>
> 17. Electrorheological fluids and preparation of particles useful in the
fluids.
> Troughton,
> Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
David; Bares, Joseph
> E.;
> Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
394049;
> 10/24/1990.
>
> JOURNAL PUBLICATIONS
>
> 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov, Eugene;
Guo, Amy;
> Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
Mandeville, W. Harry;
> Holmes-Farley, S. Randall. Kidney International (2002), 62(2), 611-619.
>
> 2. Amine functionalized polyethers as bile acid sequestrants: synthesis
and biological
> evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S. Randall;
Mandeville, W.
> Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
Journal of
> Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
1559-1574.
>
> 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
Imprinting. Huval,
> Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
Randall; Mandeville,
> W.
> Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert J.;
Chen, Xi; Dhal,
> Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
>
> 4. Synthetic polymers for the binding of fat in the intestinal tract.
Jozefiak, Thomas H.;
> Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia; Huval,
Chad C.;
> Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
Abstracts of
> Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
26-30, 2001
> (2001), POLY-047 and Polymer Preprints (American Chemical Society,
Division of
> Polymer Chemistry) (2001), 42(2), 98.
>
> 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer gel
pharmaceutical.
> Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.; Ward,
J.; Sacchiero,
> B.;
> Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.; Chen,
X.; Mazzeo, J.
> R.. Polym. Preprints (2000), 41(1), 735-736.
>
> 6. In vitro comparison of bile acid binding to colesevelam HCl and other
bile acid
> sequestrants.
> Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
Hook, P.; Holmes-
> Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
>
> 7. Novel polymeric pharmaceuticals: From startup to market. Holmes-Farley,
S. R; Polym.
> Mater. Sci. Eng (1999), 80, 246-247.
>
> 8. Design and characterization of of Sevelamer Hydrochloride: a novel
phosphate-binding
> pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward, J.;
Miller, K. L.;
> Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure and
Appl. Chem.,
> A36(7&8), p. 1085 (1999).
>
> 9. Three generations of bile acid sequestrants. Mandeville, W. H., III;
Braunlin, W.;
> Dhal, P.;
> Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
Rosenbaum, D.;
> Sacchiero,
> R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
550, 3-15.
>
> 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric phosphate
binder, on
> urinary
> phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
Mandeville, W. H.,
> III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
(1997), 12(5)
> 961-964.
>
> 11. Thin anisotropic coatings based on sol-gel technology. Holmes-Farley,
S. R.; Yanyo, L.
> C;
> Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4), 439-444.
>
> 12. The mechanism of cure initiation of a surface activated adhesive.
Holmes-Farley, S.
> R.;
> Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
>
> 13. Adhesion promotion and corrosion prevention using thin anisotropic
coatings. Holmes-
> Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
131-151.
>
> 14. Wetting of functionalized polyethylene having ionizable organic acids
and bases at the
> polymer-water interface: relations between functional group polarity,
extent of
> ionization,
> and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
Whitesides, G. M.;
> Langmuir
> (1988), 4(4), 921-937.
>
> 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
single hydroxy group.
> Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
>
> 16. Reconstruction of the interface of oxidatively functionalized
polyethylene (PE-CO2H)
> and
> derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo, R.;
McCarthy, T. J.;
> Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report (1987),
AD-
> A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
>
> 17. Surface-modified polyethylene film: the relationship between surface
chemistry and
> physical
> properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11), 4537.
>
> 18. Reactivity of carboxylic acid and ester groups in the functionalized
interfacial
> region of
> "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
differentiation of the
> functional groups into shallow and deep subsets based on a comparison of
contact angle and
> ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
(1987), 3(1), 62-
> 76.
>
> 19. Fluorescence properties of dansyl groups covalently bonded tot he
surface of
> oxidatively
> functionalized low-density polyethylene film. Holmes-Farley, S. R.;
Whitesides, G. M.;
> Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
AD-A162435/2/GAR,
> Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
>
> 20. Acid-base behavior of carboxylic acid groups covalently attached at
the surface of
> polyethylene: The usefulness of contact angle in following the ionization
of surface
> functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
Deutch, J.;
> Whitesides,
> G. M.; Langmuir (1985), 1(6), 725-740.
>
> 21. The thermal stability of a surface modified solid organic polymer.
Holmes-Farley, S.
> R.;
> Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
>
>
>
> CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
>
> 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
Aquarist. June 2003.
>
> 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
Advanced Aquarist.
> May
> 2003.
>
> 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
Reefkeeping May
> 2003.
>
> 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
April 2003.
>
> 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
Holmes-Farley, R.
> Advanced Aquarist; April 2003.
>
> 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
Holmes-Farley, R.
> Advanced Aquarist; April 2003.
>
> 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced Aquarist;
March 2003.
>
> 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
Holmes-Farley, R.
> Advanced Aquarist; February 2003.
>
> 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
2003.
>
> 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; December
2002.
>
> 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R. Advanced
Aquarist; November
> 2002.
>
> 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
Advanced Aquarist;
> November 2002.
>
> 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced Aquarist,
September 2002.
>
> 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
2002.
>
> 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
2002.
>
> 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
Aquarist; July 2002
>
> 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist; June
2002.
>
> 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R. Advanced
Aquarist, May
> 2002.
>
> 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
Holmes-Farley, R.
> Advanced Aquarist, April 2002.
>
> 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
>
> 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
>
> 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January 2002.
>
> 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
2000.
>
> 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
Frontiers 2000.
>
> 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
Aquarium Frontiers
> 2000.
> 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium Frontiers
2000.
>
> 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers 2000.
>
> 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
>
> 29. Protein Skimming: How it Works. Fishnet Library 1998.
>
>
>
>
>
>
>
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
>
>

[stoutman]

Boomer, here is another link.

http://bcn.boulder.co.us/basin/data/NUTRIENTS/info/Alk.html



So I guess everyone is wrong but you, right?






"Boomer" > wrote in message
...
> Now I am getting bored
>
> "Don't the components of a buffer account for the buffering capacity?
Yes."
>
> Yes, agreed but you seem to fail what I'm saying. Buffering Capacity and
Alkalinity are
> not the same, that has always been the issue. I gave the equation does
that look like an
> Alkalinity equation or how Alk is determined. I see you had now comments
on it what's
> wrong, why no comments on the equations I gave. Don't understand them or
what ? Again this
> is the equation for Buffering Capacity, also called Buffer Index or Buffer
Intensity. It
> is defined in most water chemistry and chemical oceanography text books.
>
> B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> This is not Alkalinity now is it ?
>
> "I know how to do a titration, In fact I have done several. How many have
> you actually done? I don't mean by counting drops, I mean with a buret?"
>
> Well good for you, I use a Digital Titrator
>
> "Oh, I see,
> you think acidity is the opposite of alkalinity. In the world of
CHEMISTRY
> it's not. Maybe in aquarium newsgroups it is.
>
> Hum no, maybe you should go for a look at HACH's or LaMotte website or the
book I
> suggested earlier. Please view a copy.
>
> Standard Methods for the Examination of Water and Wastewater
>
> This book, over 2000 pages, is the guide for water testing. If you are
reporting water
> test to the EPA you must use approved std from this text.I t is prepared
and published by
> the EPA, American Water Works Association and American Public Health
Association. You
> mean you don't have one and the issue is water chemistry
>
> You are confusing Acidity and Acidity as you know little about water
chemistry and
> procedures and test methods
>
> From SMEWW, section 2-30, 2310 ACIDITY
>
> "Acidity of water is its quantative capacity to react with a strong base
to a designated
> pH"
>
> This is how you test for it
>
> A std alkali titration to methyl orange or phenolphthalein
> endpoint.
>
> BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write this
book, there are
> over 100 of them, they are wrong.
>
> Like Buffering Capacity you have your Acidity's mixed up
> In water measurement if you have a high Alk you also usually have a high
Acidity.
> Normally a high Alk also gives a higher CO2 level. Get a WATER CHEMISTRY
BOOK there pal.
>
>
> "These are all in equilibrium with each other. An initial high pH (above
> 6.4) will shift the equilibrium to the right to form HCO3-1. If the pH of
> the solution is above 10.3 (pKa2) the .........."
>
>
> Christ, there you go again with the FW ****. All your numbers are wrong we
are dealing
> with SEAWATER
>
> This means that at a pH of 8.3, the majority of the CO2(aq) is in the form
> of HCO3-1 .
>
> I have already pointed that out and gave actual values at know seawater
levels, go back
> and re-read it you aren't telling me anything here.Of course most is HCO3
see...
>
>
> @ 20C and 34.3 ppt salinity
>
> CO2 = 0.52 %
>
> HCO3 = 86.4 %
>
> CO3 = 13.09 %
>
>
> "In your glass experiment you managed to lower the pH enough to purge out
CO2
> by boiling"
>
> The purpose behind the glass is to show that alk is not affect by CO2 and
vise-versa and
> how Co2 affects pH.
>
> Now, in a real life seawater aquarium, with a pH of 8.3 and that pH drops
to say 8.1 it is
> usually due to excess CO2. If you took a glass of that water and aerated
it you WILL drive
> off the CO2 and raise the pH. It has been done a proven a million times.
>
> "In order to 'purge' CO2 you would need to lower the
> pH to shift the equilibrium to below 6.4"
>
> The hell you do !!!.Do you know who many times people on this NG to
include Dr. Craig
> Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
sample of aquarium
> water and aerate it to see if the pH GOES UP AND when they come back with
the test it is
> often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST excess
CO2 in the tank
> water, increase the circulation for better gas exchange at the surface,
reduce feeding,
> and try to improve on better skimming, thus reducing the bio-load and pH
decline due to
> CO2.
>
>
> "I hope this helps. "
>
> Help, how can you when you miss everything. I should be charging you
>
> Oh, by the way. Your websites, I have about 50 on these issues, I could
post them, not to
> mention I have all those water chemistry books, so there is no need to
view your sites.
>
> Finally are you afraid to come to our Chemistry Forum, afraid to get
slapped by REAL
> chemists. I get a charge out of you can't post your ref .I have posted the
same or similar
> stuff on his forum and I wasn't pointed out WRONG pal. I have 1500 posts
there and am the
> biggest contributor to his forum other than himself or maybe Habib Sheka
>
> Hum, here are Randy's ref that he posted. He hosts the website
>
> S. RANDY HOLMES-FARLEY
> Arlington, Massachusetts
>
> EDUCATION
>
> 1982-1986 Harvard University Cambridge, MA
> PhD in Chemistry
> Research Advisor: George Whitesides
>
> Investigated the relationship between polymer surface chemistry and
physical properties
> through controlled surface modification and testing.
>
> 1980-1982 Cornell University Ithaca, NY
> BA in Chemistry and Biology
> Graduated Summa Cum Laude
> Distinction in All Subjects
> Grade Point: 3.94/4.0
> Honors research: isolation and characterization of the subunit of CF1
enzyme
>
>
> 1978-1979 Stanford University Palo Alto, CA
> Grade Point: 3.55/4.0
>
>
> EXPERIENCE
>
> 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> (bought out GelTex Pharmaceuticals in 2001)
> Vice President, Chemical Research 2001-present
> Senior Director, Chemical Research 1999-2001
> Director of Chemical Research 1997-1999
> Manager of Chemical Research 1995-1997
> Group Leader 1994-1995
> Senior Research Scientist 1992-1994
>
> Helped start GelTex as second employee
>
> Managed various research programs with multi-million dollar budgets
>
> Supervised research chemists (17+)
>
> Co-inventor of several polymeric pharmaceuticals and pharmaceutical
candidates including
> Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride (FDA
approved)
>
> Company Safety Officer for 3 years
>
> Chemical Hygiene Officer 2000-present
>
>
>
>
> 1990-1992 GTE Corporation Waltham, MA
> Senior Member of Technical Staff
> Applied research involving polymer interfaces
> Metallization of plastics
> Polymer/polymer adhesion
> Optical coatings
>
>
>
> 1986-1990 Lord Corporation Cary, NC
> Senior Research Scientist 1988-1990
> Research Scientist 1986-1988
> Basic and applied research on surface chemical bonding
> Developed new adhesive compositions
> Developed new sol-gel coatings for corrosion resistance
>
>
> HONORS AND AWARDS
>
> Industrial Innovations Award by Northeast Region of American Chemical
Society (6/2001)
>
> National Kidney Foundation of Northern California Honoree (5/2001)
>
> American Chemical Society/Polymer Chemistry Division Industrial Sponsors
> Award (8/2000)
>
> R&D 100 Award from R&D magazine (1999)
>
> Sherwin Williams Award in applied polymer science (9/85)
>
> IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
>
> Award for highest GPA in Chemistry Department (6/82)
>
> Summa Cum Laude Honors in Chemistry (6/82)
>
> Phi Lamda Epsilon (6/82)
>
> Phi Beta Kappa (2/82)
>
> Cornell University Dean's List (1981, 1982)
>
> Harvard Book Club Award for highest GPA senior year (1978)
>
> First Place in western NY ACS high school chemistry exam (1977)
>
> 1978-1979
>
>
> __________________
> Randy Holmes-Farley
> Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
>
> Hobby Experience: 8 years with reefs
> Current Tanks: 90 gal mixed reef
> Interests: Reefkeeping, science, photography
>
>
> Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
>
> Open this post in a new window | Report this post to a moderator | IP:
Logged
>
>
>
> 06/27/2003 02:44 PM
>
> Randy Holmes-Farley
> Chemistry Moderator
>
> Registered: Apr 2001
> Location: Arlington, Massachusetts
> Occupation: Chemist (Drug Discovery at Genzyme)
> Posts: 15282
>
>
>
> Publications
>
>
> ISSUED UNITED STATES PATENTS
>
>
> 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
Mandeville, III; W. Harry.
> US 6,566,407; 5/20/2003
>
> 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen Randall;
Huval, Chad
> Cori.
> U.S. 6,517,825; 2/11/2003.
>
> 3. Method of making phosphate-binding polymers for oral administration.
Holmes-Farley,
> Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
6,509,013; 1/21/2003.
>
> 4. Combination therapy for treating hypercholesterolemia using a bile acid
sequestrant
> polymer
> and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley, Stephen
Randall;
> Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
>
> 5. Method for treating hypercholesterolemia with polyallylamine polymers.
Holmes-Farley,
> Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.; Goldberg,
Dennis I. , US
> 6,423,754; 7/23/2002.
>
> 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
Neenan, Thomas X..;
> Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
>
> 7. Combination therapy for treating hypercholesterolemia and
atherosclerosis. Huval, Chad
> Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep K.
U.S. 6,365,186;
> 4/2/2002.
>
> 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.; Mandeville,
W. H., III;
> Huval; C.
> C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
10/9/2001.
>
> 9. Polymers containing guanidinium groups as bile acid sequestrants. Dhal;
P. K.; Holmes-
> Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
>
> 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 6,281,252;
> 8/28/2001.
>
> 11. Combination therapy for treating hypercholestrolemia. Huval; C. C.;
Holmes-Farley; S.
> R. ;
> Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
>
> 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
Holmes-Farley, S.
> R.; US
> 6,264,937; 7/24/2001.
>
> 13. Method for treating hypercholesterolemia with unsubstituted
polydiallylamine polymers.
> Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
6,248,318;
> 6/19/2001.
>
> 14. Process for removing bile salts from a patient and alkylated
compositions therefore.
> Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
>
> 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S. R.;
Dhal, P. K.;
> Petersen,
> J. S.; US 6,203,785; 3/20/2001.
>
> 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.; Huval,
C. C.; US
> 6,190,649;
> 2/20/2001.
>
> 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 6,177,478;
> 1/23/2001.
>
> 18. Water-insoluble noncrosslinked bile acid sequestrants. Holmes-Farley,
S. R.;
> Mandeville, W.
> H., III.; US 6,129,910; 10/10/2000.
>
> 19. Method for treating hypercholesterolemia with unsubstituted
polydiallylamine polymers.
> Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
6,083,497;
> 7/4/2000.
>
> 20. Method of making phosphate-binding polymers for oral administration.
Holmes-Farley, S.
> R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495; 7/4/2000.
>
> 21. Process for removing bile salts from a patient and alkylated
compositions therefore.
> Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678; 5/23/2000.
>
> 22. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
>
> 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
Neenan; T. X.; Holmes-
> Farley; S. R. US 6,034,129; 3/7/2000.
>
> 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 5,985,938;
> 11/16/99.
>
> 25. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
>
> 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W. H.,
III.;
> Holmes-Farley;
> S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
>
> 27. Hydrophilic nonamine-containing and amine-containing copolymers and
their use as bile
> acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US 5,929,184;
7/27/99.
>
> 28. Interpenetrating polymer networks for sequestration of bile acids.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
7/20/99.
>
> 29. Amine polymer sequestrant and method of cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
>
> 30. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
>
> 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
>
> 32. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
>
> 33. Preparation of polymeric sequestrants for bile acid salts. Mandeville,
W. H., III.;
> Holmes-
> Farley, S. R.; US 5,703,188; 12/30/97.
>
> 34. Oral administration of iron-binding crosslinked amine polymers.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
>
> 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley, S.
R.; US 5,693,675;
> 12/2/97.
>
> 36. Method for removing bile salts from a patient with alkylated
crosslinked amine
> polymers,
> and preparation of the polymers. Mandeville, W. H., III.; Holmes-Farley,
S. R.; US
> 5,679,717; 10/21/97.
>
> 37. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville,
> W.
> H., III.; US 5,667,775; 9/16/97.
>
> 38. Ion-exchange process using highly crosslinked polymers for removing
bile salts from a
> patient, preparation of the polymers, and compositions containing them.
Mandeville, W. H.,
> III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
>
> 39. Hydrophobic amine polymer sequestrant and method of cholesterol
depletion. Mandeville,
> W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530; 4/8/97.
>
> 40. Amine polymer sequestrant and method of cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
>
> 41. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville,
> W.
> H., III.; US 5,496,545; 3/5/96.
>
> 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
III.; Holmes-Farley,
> S. R.;
> US 5,487,888; 1/30/96.
>
> 43. Ultra-thin, uniform sol-gel coating of a substrate having active
hydrogens on the
> surface.
> Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
>
> 44. Layered sol-gel coatings from organisilicon compounds. Holmes-Farley,
S. R.; Yanyo, L.
> C.;
> US 5,182,143; 1/26/93.
>
> 45. Method for metal bonding using ultrathin primer coating.
Holmes-Farley, S. R.; Yanyo,
> L.
> C.; Thuer, A. M.; US 5,139,601; 8/18/92.
>
> 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.; US
5,096,962;
> 3/17/92.
>
> 47. Modified halogenatedpolyolefin adhesives for polyolefin
elastomer-metal bonding.
> Holmes-
> Farley, S. R.; US 5,102,956; 4/7/92.
>
>
>
> PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
>
>
> 1. Aryl boronate functionalized polymers for treating obesity and
inhibiting fat uptake.
> Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal, Pradeep
K.; Huval, Chad
> Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92 pp. WO
0302571.
>
> 2. Preparation of aryl boronic acids for treating obesity. Holmes-Farley,
Stephen Randall;
> Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep K.
(Geltex
> Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
>
> 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
Stephen Randall.
> (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
0302130.
>
> 4. Method for reducing copper levels and treating copper toxicosis.
Holmes-Farley, Stephen
> Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002), 45
pp. WO
> 0285383.
>
> 5. Method for treating gout and binding uric acid. Holmes-Farley, Stephen
Randall; Burke,
> Steven K. WO 0285381 10/31/2002.
>
> 6. Method for treating gout and reducing serum uric acid. Holmes-Farley,
Stephen Randall;
> Burke, Steven K WO 0285380 10/31/2002.
>
> 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
Holmes-Farley, S. R.;
> Whitesides, G. M. WO 1999-US30469; 7/6/2000.
>
> 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
Holmes-Farley, S.
> R.;
> WO 1999-US5662; 9/23/1999.
>
> 9. Amine-containing copolymers as bile acid sequestrants. Holmes-Farley,
S. R.; Petersen,
> J. S.;
> WO 9933452; 7/8/1999.
>
> 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III and
Holmes-Farley, S.
> R.;
> WO 9922743; 5/14/1999.
>
> 11. Polyallylamine polymers for removing bile salts and treating
hypercholesterolemia, and
> polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III; Burke,
S. K.; Goldberg,
> D. I.; WO 9857652; 12/23/98.
>
> 12. Phosphate-bidning polymers combined with a calcium supplement for oral
administration.
> Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley, S.
R.; WO 9842355;
> 10/1/98.
>
> 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
depletion. Mandeville,
> W.
> H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
>
> 14. Process for adjusting ion concentration in a patient and compositions
therefor.
> Mandeville,
> W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
>
> 15. Vacuum-deposited silver on polycarbonate with a chromium interlayer
for improved
> metal-
> substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512; 1/20/94.
>
> 16. Process for increased metal-substrate bond strength in metalized
plastics.
> Holmes-Farley, S.
> R.; Ger. Offen. 4322516; 7/6/93.
>
> 17. Electrorheological fluids and preparation of particles useful in the
fluids.
> Troughton,
> Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
David; Bares, Joseph
> E.;
> Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
394049;
> 10/24/1990.
>
> JOURNAL PUBLICATIONS
>
> 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov, Eugene;
Guo, Amy;
> Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
Mandeville, W. Harry;
> Holmes-Farley, S. Randall. Kidney International (2002), 62(2), 611-619.
>
> 2. Amine functionalized polyethers as bile acid sequestrants: synthesis
and biological
> evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S. Randall;
Mandeville, W.
> Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
Journal of
> Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
1559-1574.
>
> 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
Imprinting. Huval,
> Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
Randall; Mandeville,
> W.
> Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert J.;
Chen, Xi; Dhal,
> Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
>
> 4. Synthetic polymers for the binding of fat in the intestinal tract.
Jozefiak, Thomas H.;
> Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia; Huval,
Chad C.;
> Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
Abstracts of
> Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
26-30, 2001
> (2001), POLY-047 and Polymer Preprints (American Chemical Society,
Division of
> Polymer Chemistry) (2001), 42(2), 98.
>
> 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer gel
pharmaceutical.
> Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.; Ward,
J.; Sacchiero,
> B.;
> Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.; Chen,
X.; Mazzeo, J.
> R.. Polym. Preprints (2000), 41(1), 735-736.
>
> 6. In vitro comparison of bile acid binding to colesevelam HCl and other
bile acid
> sequestrants.
> Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
Hook, P.; Holmes-
> Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
>
> 7. Novel polymeric pharmaceuticals: From startup to market. Holmes-Farley,
S. R; Polym.
> Mater. Sci. Eng (1999), 80, 246-247.
>
> 8. Design and characterization of of Sevelamer Hydrochloride: a novel
phosphate-binding
> pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward, J.;
Miller, K. L.;
> Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure and
Appl. Chem.,
> A36(7&8), p. 1085 (1999).
>
> 9. Three generations of bile acid sequestrants. Mandeville, W. H., III;
Braunlin, W.;
> Dhal, P.;
> Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
Rosenbaum, D.;
> Sacchiero,
> R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
550, 3-15.
>
> 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric phosphate
binder, on
> urinary
> phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
Mandeville, W. H.,
> III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
(1997), 12(5)
> 961-964.
>
> 11. Thin anisotropic coatings based on sol-gel technology. Holmes-Farley,
S. R.; Yanyo, L.
> C;
> Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4), 439-444.
>
> 12. The mechanism of cure initiation of a surface activated adhesive.
Holmes-Farley, S.
> R.;
> Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
>
> 13. Adhesion promotion and corrosion prevention using thin anisotropic
coatings. Holmes-
> Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
131-151.
>
> 14. Wetting of functionalized polyethylene having ionizable organic acids
and bases at the
> polymer-water interface: relations between functional group polarity,
extent of
> ionization,
> and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
Whitesides, G. M.;
> Langmuir
> (1988), 4(4), 921-937.
>
> 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
single hydroxy group.
> Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
>
> 16. Reconstruction of the interface of oxidatively functionalized
polyethylene (PE-CO2H)
> and
> derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo, R.;
McCarthy, T. J.;
> Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report (1987),
AD-
> A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
>
> 17. Surface-modified polyethylene film: the relationship between surface
chemistry and
> physical
> properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11), 4537.
>
> 18. Reactivity of carboxylic acid and ester groups in the functionalized
interfacial
> region of
> "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
differentiation of the
> functional groups into shallow and deep subsets based on a comparison of
contact angle and
> ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
(1987), 3(1), 62-
> 76.
>
> 19. Fluorescence properties of dansyl groups covalently bonded tot he
surface of
> oxidatively
> functionalized low-density polyethylene film. Holmes-Farley, S. R.;
Whitesides, G. M.;
> Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
AD-A162435/2/GAR,
> Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
>
> 20. Acid-base behavior of carboxylic acid groups covalently attached at
the surface of
> polyethylene: The usefulness of contact angle in following the ionization
of surface
> functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
Deutch, J.;
> Whitesides,
> G. M.; Langmuir (1985), 1(6), 725-740.
>
> 21. The thermal stability of a surface modified solid organic polymer.
Holmes-Farley, S.
> R.;
> Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
>
>
>
> CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
>
> 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
Aquarist. June 2003.
>
> 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
Advanced Aquarist.
> May
> 2003.
>
> 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
Reefkeeping May
> 2003.
>
> 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
April 2003.
>
> 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
Holmes-Farley, R.
> Advanced Aquarist; April 2003.
>
> 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
Holmes-Farley, R.
> Advanced Aquarist; April 2003.
>
> 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced Aquarist;
March 2003.
>
> 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
Holmes-Farley, R.
> Advanced Aquarist; February 2003.
>
> 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
2003.
>
> 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; December
2002.
>
> 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R. Advanced
Aquarist; November
> 2002.
>
> 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
Advanced Aquarist;
> November 2002.
>
> 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced Aquarist,
September 2002.
>
> 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
2002.
>
> 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
2002.
>
> 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
Aquarist; July 2002
>
> 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist; June
2002.
>
> 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R. Advanced
Aquarist, May
> 2002.
>
> 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
Holmes-Farley, R.
> Advanced Aquarist, April 2002.
>
> 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
>
> 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
>
> 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January 2002.
>
> 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
2000.
>
> 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
Frontiers 2000.
>
> 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
Aquarium Frontiers
> 2000.
> 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium Frontiers
2000.
>
> 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers 2000.
>
> 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
>
> 29. Protein Skimming: How it Works. Fishnet Library 1998.
>
>
>
>
>
>
>
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
>
>

[stoutman]

Man here is another, google is a wonderful thing. I'm not filtering any
out, just posting what I find by GOOGLING for you.

http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML


Wow, a gov link. Even the government is wrong, this must be a conspiracy
against Boomer.




"Boomer" > wrote in message
...
> Now I am getting bored
>
> "Don't the components of a buffer account for the buffering capacity?
Yes."
>
> Yes, agreed but you seem to fail what I'm saying. Buffering Capacity and
Alkalinity are
> not the same, that has always been the issue. I gave the equation does
that look like an
> Alkalinity equation or how Alk is determined. I see you had now comments
on it what's
> wrong, why no comments on the equations I gave. Don't understand them or
what ? Again this
> is the equation for Buffering Capacity, also called Buffer Index or Buffer
Intensity. It
> is defined in most water chemistry and chemical oceanography text books.
>
> B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> This is not Alkalinity now is it ?
>
> "I know how to do a titration, In fact I have done several. How many have
> you actually done? I don't mean by counting drops, I mean with a buret?"
>
> Well good for you, I use a Digital Titrator
>
> "Oh, I see,
> you think acidity is the opposite of alkalinity. In the world of
CHEMISTRY
> it's not. Maybe in aquarium newsgroups it is.
>
> Hum no, maybe you should go for a look at HACH's or LaMotte website or the
book I
> suggested earlier. Please view a copy.
>
> Standard Methods for the Examination of Water and Wastewater
>
> This book, over 2000 pages, is the guide for water testing. If you are
reporting water
> test to the EPA you must use approved std from this text.I t is prepared
and published by
> the EPA, American Water Works Association and American Public Health
Association. You
> mean you don't have one and the issue is water chemistry
>
> You are confusing Acidity and Acidity as you know little about water
chemistry and
> procedures and test methods
>
> From SMEWW, section 2-30, 2310 ACIDITY
>
> "Acidity of water is its quantative capacity to react with a strong base
to a designated
> pH"
>
> This is how you test for it
>
> A std alkali titration to methyl orange or phenolphthalein
> endpoint.
>
> BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write this
book, there are
> over 100 of them, they are wrong.
>
> Like Buffering Capacity you have your Acidity's mixed up
> In water measurement if you have a high Alk you also usually have a high
Acidity.
> Normally a high Alk also gives a higher CO2 level. Get a WATER CHEMISTRY
BOOK there pal.
>
>
> "These are all in equilibrium with each other. An initial high pH (above
> 6.4) will shift the equilibrium to the right to form HCO3-1. If the pH of
> the solution is above 10.3 (pKa2) the .........."
>
>
> Christ, there you go again with the FW ****. All your numbers are wrong we
are dealing
> with SEAWATER
>
> This means that at a pH of 8.3, the majority of the CO2(aq) is in the form
> of HCO3-1 .
>
> I have already pointed that out and gave actual values at know seawater
levels, go back
> and re-read it you aren't telling me anything here.Of course most is HCO3
see...
>
>
> @ 20C and 34.3 ppt salinity
>
> CO2 = 0.52 %
>
> HCO3 = 86.4 %
>
> CO3 = 13.09 %
>
>
> "In your glass experiment you managed to lower the pH enough to purge out
CO2
> by boiling"
>
> The purpose behind the glass is to show that alk is not affect by CO2 and
vise-versa and
> how Co2 affects pH.
>
> Now, in a real life seawater aquarium, with a pH of 8.3 and that pH drops
to say 8.1 it is
> usually due to excess CO2. If you took a glass of that water and aerated
it you WILL drive
> off the CO2 and raise the pH. It has been done a proven a million times.
>
> "In order to 'purge' CO2 you would need to lower the
> pH to shift the equilibrium to below 6.4"
>
> The hell you do !!!.Do you know who many times people on this NG to
include Dr. Craig
> Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
sample of aquarium
> water and aerate it to see if the pH GOES UP AND when they come back with
the test it is
> often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST excess
CO2 in the tank
> water, increase the circulation for better gas exchange at the surface,
reduce feeding,
> and try to improve on better skimming, thus reducing the bio-load and pH
decline due to
> CO2.
>
>
> "I hope this helps. "
>
> Help, how can you when you miss everything. I should be charging you
>
> Oh, by the way. Your websites, I have about 50 on these issues, I could
post them, not to
> mention I have all those water chemistry books, so there is no need to
view your sites.
>
> Finally are you afraid to come to our Chemistry Forum, afraid to get
slapped by REAL
> chemists. I get a charge out of you can't post your ref .I have posted the
same or similar
> stuff on his forum and I wasn't pointed out WRONG pal. I have 1500 posts
there and am the
> biggest contributor to his forum other than himself or maybe Habib Sheka
>
> Hum, here are Randy's ref that he posted. He hosts the website
>
> S. RANDY HOLMES-FARLEY
> Arlington, Massachusetts
>
> EDUCATION
>
> 1982-1986 Harvard University Cambridge, MA
> PhD in Chemistry
> Research Advisor: George Whitesides
>
> Investigated the relationship between polymer surface chemistry and
physical properties
> through controlled surface modification and testing.
>
> 1980-1982 Cornell University Ithaca, NY
> BA in Chemistry and Biology
> Graduated Summa Cum Laude
> Distinction in All Subjects
> Grade Point: 3.94/4.0
> Honors research: isolation and characterization of the subunit of CF1
enzyme
>
>
> 1978-1979 Stanford University Palo Alto, CA
> Grade Point: 3.55/4.0
>
>
> EXPERIENCE
>
> 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> (bought out GelTex Pharmaceuticals in 2001)
> Vice President, Chemical Research 2001-present
> Senior Director, Chemical Research 1999-2001
> Director of Chemical Research 1997-1999
> Manager of Chemical Research 1995-1997
> Group Leader 1994-1995
> Senior Research Scientist 1992-1994
>
> Helped start GelTex as second employee
>
> Managed various research programs with multi-million dollar budgets
>
> Supervised research chemists (17+)
>
> Co-inventor of several polymeric pharmaceuticals and pharmaceutical
candidates including
> Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride (FDA
approved)
>
> Company Safety Officer for 3 years
>
> Chemical Hygiene Officer 2000-present
>
>
>
>
> 1990-1992 GTE Corporation Waltham, MA
> Senior Member of Technical Staff
> Applied research involving polymer interfaces
> Metallization of plastics
> Polymer/polymer adhesion
> Optical coatings
>
>
>
> 1986-1990 Lord Corporation Cary, NC
> Senior Research Scientist 1988-1990
> Research Scientist 1986-1988
> Basic and applied research on surface chemical bonding
> Developed new adhesive compositions
> Developed new sol-gel coatings for corrosion resistance
>
>
> HONORS AND AWARDS
>
> Industrial Innovations Award by Northeast Region of American Chemical
Society (6/2001)
>
> National Kidney Foundation of Northern California Honoree (5/2001)
>
> American Chemical Society/Polymer Chemistry Division Industrial Sponsors
> Award (8/2000)
>
> R&D 100 Award from R&D magazine (1999)
>
> Sherwin Williams Award in applied polymer science (9/85)
>
> IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
>
> Award for highest GPA in Chemistry Department (6/82)
>
> Summa Cum Laude Honors in Chemistry (6/82)
>
> Phi Lamda Epsilon (6/82)
>
> Phi Beta Kappa (2/82)
>
> Cornell University Dean's List (1981, 1982)
>
> Harvard Book Club Award for highest GPA senior year (1978)
>
> First Place in western NY ACS high school chemistry exam (1977)
>
> 1978-1979
>
>
> __________________
> Randy Holmes-Farley
> Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
>
> Hobby Experience: 8 years with reefs
> Current Tanks: 90 gal mixed reef
> Interests: Reefkeeping, science, photography
>
>
> Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
>
> Open this post in a new window | Report this post to a moderator | IP:
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>
>
>
> 06/27/2003 02:44 PM
>
> Randy Holmes-Farley
> Chemistry Moderator
>
> Registered: Apr 2001
> Location: Arlington, Massachusetts
> Occupation: Chemist (Drug Discovery at Genzyme)
> Posts: 15282
>
>
>
> Publications
>
>
> ISSUED UNITED STATES PATENTS
>
>
> 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
Mandeville, III; W. Harry.
> US 6,566,407; 5/20/2003
>
> 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen Randall;
Huval, Chad
> Cori.
> U.S. 6,517,825; 2/11/2003.
>
> 3. Method of making phosphate-binding polymers for oral administration.
Holmes-Farley,
> Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
6,509,013; 1/21/2003.
>
> 4. Combination therapy for treating hypercholesterolemia using a bile acid
sequestrant
> polymer
> and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley, Stephen
Randall;
> Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
>
> 5. Method for treating hypercholesterolemia with polyallylamine polymers.
Holmes-Farley,
> Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.; Goldberg,
Dennis I. , US
> 6,423,754; 7/23/2002.
>
> 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
Neenan, Thomas X..;
> Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
>
> 7. Combination therapy for treating hypercholesterolemia and
atherosclerosis. Huval, Chad
> Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep K.
U.S. 6,365,186;
> 4/2/2002.
>
> 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.; Mandeville,
W. H., III;
> Huval; C.
> C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
10/9/2001.
>
> 9. Polymers containing guanidinium groups as bile acid sequestrants. Dhal;
P. K.; Holmes-
> Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
>
> 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 6,281,252;
> 8/28/2001.
>
> 11. Combination therapy for treating hypercholestrolemia. Huval; C. C.;
Holmes-Farley; S.
> R. ;
> Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
>
> 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
Holmes-Farley, S.
> R.; US
> 6,264,937; 7/24/2001.
>
> 13. Method for treating hypercholesterolemia with unsubstituted
polydiallylamine polymers.
> Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
6,248,318;
> 6/19/2001.
>
> 14. Process for removing bile salts from a patient and alkylated
compositions therefore.
> Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
>
> 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S. R.;
Dhal, P. K.;
> Petersen,
> J. S.; US 6,203,785; 3/20/2001.
>
> 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.; Huval,
C. C.; US
> 6,190,649;
> 2/20/2001.
>
> 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 6,177,478;
> 1/23/2001.
>
> 18. Water-insoluble noncrosslinked bile acid sequestrants. Holmes-Farley,
S. R.;
> Mandeville, W.
> H., III.; US 6,129,910; 10/10/2000.
>
> 19. Method for treating hypercholesterolemia with unsubstituted
polydiallylamine polymers.
> Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
6,083,497;
> 7/4/2000.
>
> 20. Method of making phosphate-binding polymers for oral administration.
Holmes-Farley, S.
> R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495; 7/4/2000.
>
> 21. Process for removing bile salts from a patient and alkylated
compositions therefore.
> Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678; 5/23/2000.
>
> 22. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
>
> 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
Neenan; T. X.; Holmes-
> Farley; S. R. US 6,034,129; 3/7/2000.
>
> 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 5,985,938;
> 11/16/99.
>
> 25. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
>
> 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W. H.,
III.;
> Holmes-Farley;
> S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
>
> 27. Hydrophilic nonamine-containing and amine-containing copolymers and
their use as bile
> acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US 5,929,184;
7/27/99.
>
> 28. Interpenetrating polymer networks for sequestration of bile acids.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
7/20/99.
>
> 29. Amine polymer sequestrant and method of cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
>
> 30. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
>
> 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
>
> 32. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
>
> 33. Preparation of polymeric sequestrants for bile acid salts. Mandeville,
W. H., III.;
> Holmes-
> Farley, S. R.; US 5,703,188; 12/30/97.
>
> 34. Oral administration of iron-binding crosslinked amine polymers.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
>
> 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley, S.
R.; US 5,693,675;
> 12/2/97.
>
> 36. Method for removing bile salts from a patient with alkylated
crosslinked amine
> polymers,
> and preparation of the polymers. Mandeville, W. H., III.; Holmes-Farley,
S. R.; US
> 5,679,717; 10/21/97.
>
> 37. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville,
> W.
> H., III.; US 5,667,775; 9/16/97.
>
> 38. Ion-exchange process using highly crosslinked polymers for removing
bile salts from a
> patient, preparation of the polymers, and compositions containing them.
Mandeville, W. H.,
> III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
>
> 39. Hydrophobic amine polymer sequestrant and method of cholesterol
depletion. Mandeville,
> W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530; 4/8/97.
>
> 40. Amine polymer sequestrant and method of cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
>
> 41. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville,
> W.
> H., III.; US 5,496,545; 3/5/96.
>
> 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
III.; Holmes-Farley,
> S. R.;
> US 5,487,888; 1/30/96.
>
> 43. Ultra-thin, uniform sol-gel coating of a substrate having active
hydrogens on the
> surface.
> Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
>
> 44. Layered sol-gel coatings from organisilicon compounds. Holmes-Farley,
S. R.; Yanyo, L.
> C.;
> US 5,182,143; 1/26/93.
>
> 45. Method for metal bonding using ultrathin primer coating.
Holmes-Farley, S. R.; Yanyo,
> L.
> C.; Thuer, A. M.; US 5,139,601; 8/18/92.
>
> 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.; US
5,096,962;
> 3/17/92.
>
> 47. Modified halogenatedpolyolefin adhesives for polyolefin
elastomer-metal bonding.
> Holmes-
> Farley, S. R.; US 5,102,956; 4/7/92.
>
>
>
> PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
>
>
> 1. Aryl boronate functionalized polymers for treating obesity and
inhibiting fat uptake.
> Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal, Pradeep
K.; Huval, Chad
> Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92 pp. WO
0302571.
>
> 2. Preparation of aryl boronic acids for treating obesity. Holmes-Farley,
Stephen Randall;
> Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep K.
(Geltex
> Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
>
> 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
Stephen Randall.
> (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
0302130.
>
> 4. Method for reducing copper levels and treating copper toxicosis.
Holmes-Farley, Stephen
> Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002), 45
pp. WO
> 0285383.
>
> 5. Method for treating gout and binding uric acid. Holmes-Farley, Stephen
Randall; Burke,
> Steven K. WO 0285381 10/31/2002.
>
> 6. Method for treating gout and reducing serum uric acid. Holmes-Farley,
Stephen Randall;
> Burke, Steven K WO 0285380 10/31/2002.
>
> 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
Holmes-Farley, S. R.;
> Whitesides, G. M. WO 1999-US30469; 7/6/2000.
>
> 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
Holmes-Farley, S.
> R.;
> WO 1999-US5662; 9/23/1999.
>
> 9. Amine-containing copolymers as bile acid sequestrants. Holmes-Farley,
S. R.; Petersen,
> J. S.;
> WO 9933452; 7/8/1999.
>
> 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III and
Holmes-Farley, S.
> R.;
> WO 9922743; 5/14/1999.
>
> 11. Polyallylamine polymers for removing bile salts and treating
hypercholesterolemia, and
> polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III; Burke,
S. K.; Goldberg,
> D. I.; WO 9857652; 12/23/98.
>
> 12. Phosphate-bidning polymers combined with a calcium supplement for oral
administration.
> Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley, S.
R.; WO 9842355;
> 10/1/98.
>
> 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
depletion. Mandeville,
> W.
> H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
>
> 14. Process for adjusting ion concentration in a patient and compositions
therefor.
> Mandeville,
> W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
>
> 15. Vacuum-deposited silver on polycarbonate with a chromium interlayer
for improved
> metal-
> substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512; 1/20/94.
>
> 16. Process for increased metal-substrate bond strength in metalized
plastics.
> Holmes-Farley, S.
> R.; Ger. Offen. 4322516; 7/6/93.
>
> 17. Electrorheological fluids and preparation of particles useful in the
fluids.
> Troughton,
> Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
David; Bares, Joseph
> E.;
> Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
394049;
> 10/24/1990.
>
> JOURNAL PUBLICATIONS
>
> 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov, Eugene;
Guo, Amy;
> Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
Mandeville, W. Harry;
> Holmes-Farley, S. Randall. Kidney International (2002), 62(2), 611-619.
>
> 2. Amine functionalized polyethers as bile acid sequestrants: synthesis
and biological
> evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S. Randall;
Mandeville, W.
> Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
Journal of
> Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
1559-1574.
>
> 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
Imprinting. Huval,
> Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
Randall; Mandeville,
> W.
> Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert J.;
Chen, Xi; Dhal,
> Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
>
> 4. Synthetic polymers for the binding of fat in the intestinal tract.
Jozefiak, Thomas H.;
> Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia; Huval,
Chad C.;
> Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
Abstracts of
> Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
26-30, 2001
> (2001), POLY-047 and Polymer Preprints (American Chemical Society,
Division of
> Polymer Chemistry) (2001), 42(2), 98.
>
> 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer gel
pharmaceutical.
> Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.; Ward,
J.; Sacchiero,
> B.;
> Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.; Chen,
X.; Mazzeo, J.
> R.. Polym. Preprints (2000), 41(1), 735-736.
>
> 6. In vitro comparison of bile acid binding to colesevelam HCl and other
bile acid
> sequestrants.
> Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
Hook, P.; Holmes-
> Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
>
> 7. Novel polymeric pharmaceuticals: From startup to market. Holmes-Farley,
S. R; Polym.
> Mater. Sci. Eng (1999), 80, 246-247.
>
> 8. Design and characterization of of Sevelamer Hydrochloride: a novel
phosphate-binding
> pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward, J.;
Miller, K. L.;
> Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure and
Appl. Chem.,
> A36(7&8), p. 1085 (1999).
>
> 9. Three generations of bile acid sequestrants. Mandeville, W. H., III;
Braunlin, W.;
> Dhal, P.;
> Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
Rosenbaum, D.;
> Sacchiero,
> R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
550, 3-15.
>
> 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric phosphate
binder, on
> urinary
> phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
Mandeville, W. H.,
> III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
(1997), 12(5)
> 961-964.
>
> 11. Thin anisotropic coatings based on sol-gel technology. Holmes-Farley,
S. R.; Yanyo, L.
> C;
> Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4), 439-444.
>
> 12. The mechanism of cure initiation of a surface activated adhesive.
Holmes-Farley, S.
> R.;
> Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
>
> 13. Adhesion promotion and corrosion prevention using thin anisotropic
coatings. Holmes-
> Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
131-151.
>
> 14. Wetting of functionalized polyethylene having ionizable organic acids
and bases at the
> polymer-water interface: relations between functional group polarity,
extent of
> ionization,
> and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
Whitesides, G. M.;
> Langmuir
> (1988), 4(4), 921-937.
>
> 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
single hydroxy group.
> Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
>
> 16. Reconstruction of the interface of oxidatively functionalized
polyethylene (PE-CO2H)
> and
> derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo, R.;
McCarthy, T. J.;
> Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report (1987),
AD-
> A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
>
> 17. Surface-modified polyethylene film: the relationship between surface
chemistry and
> physical
> properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11), 4537.
>
> 18. Reactivity of carboxylic acid and ester groups in the functionalized
interfacial
> region of
> "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
differentiation of the
> functional groups into shallow and deep subsets based on a comparison of
contact angle and
> ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
(1987), 3(1), 62-
> 76.
>
> 19. Fluorescence properties of dansyl groups covalently bonded tot he
surface of
> oxidatively
> functionalized low-density polyethylene film. Holmes-Farley, S. R.;
Whitesides, G. M.;
> Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
AD-A162435/2/GAR,
> Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
>
> 20. Acid-base behavior of carboxylic acid groups covalently attached at
the surface of
> polyethylene: The usefulness of contact angle in following the ionization
of surface
> functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
Deutch, J.;
> Whitesides,
> G. M.; Langmuir (1985), 1(6), 725-740.
>
> 21. The thermal stability of a surface modified solid organic polymer.
Holmes-Farley, S.
> R.;
> Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
>
>
>
> CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
>
> 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
Aquarist. June 2003.
>
> 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
Advanced Aquarist.
> May
> 2003.
>
> 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
Reefkeeping May
> 2003.
>
> 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
April 2003.
>
> 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
Holmes-Farley, R.
> Advanced Aquarist; April 2003.
>
> 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
Holmes-Farley, R.
> Advanced Aquarist; April 2003.
>
> 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced Aquarist;
March 2003.
>
> 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
Holmes-Farley, R.
> Advanced Aquarist; February 2003.
>
> 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
2003.
>
> 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; December
2002.
>
> 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R. Advanced
Aquarist; November
> 2002.
>
> 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
Advanced Aquarist;
> November 2002.
>
> 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced Aquarist,
September 2002.
>
> 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
2002.
>
> 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
2002.
>
> 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
Aquarist; July 2002
>
> 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist; June
2002.
>
> 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R. Advanced
Aquarist, May
> 2002.
>
> 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
Holmes-Farley, R.
> Advanced Aquarist, April 2002.
>
> 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
>
> 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
>
> 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January 2002.
>
> 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
2000.
>
> 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
Frontiers 2000.
>
> 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
Aquarium Frontiers
> 2000.
> 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium Frontiers
2000.
>
> 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers 2000.
>
> 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
>
> 29. Protein Skimming: How it Works. Fishnet Library 1998.
>
>
>
>
>
>
>
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
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> Please Join Our Growing Membership
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>

[stoutman]

I really want to help you understand.

Here is one of your alk definitions which I do not disagree with. I want to
explain to you why this tells you something about the buffering capacity.

Alkalinity = A std acid titration to phenolphthalein endpoint

During the titration to your end point, if buffers are present, they will
slow down the fall of the pH. This will require a certain amount of acid to
reach the endpoint. If no buffers are present, less acid will be needed.
Therefore, you now can have an idea of the strength of the buffer, which can
be calculated and expressed.

The buffers are alkaline (basic) components which make up the "buffering
capacity". The combined alkaline components (individual buffer components)
compose your Total Alkalinity.

As you described here:

TA = [HCO3-] + 2[CO3--] + [B(OH)4-] + [OH-] + [Si(OH)3O-] + [MgOH+] +
[HPO4--] + > > 2[PO4---] - [H+]

Therefore, measuring alkalinity tells you something about your 'buffering
capacity'.

alkalinity is an expression of or measurement of 'buffering capacity'.


DOES THIS HELP?

RESISTANCE IS FUTILE! <----I thought you might relate to this expression.
lol




"Boomer" > wrote in message
...
> Now I am getting bored
>
> "Don't the components of a buffer account for the buffering capacity?
Yes."
>
> Yes, agreed but you seem to fail what I'm saying. Buffering Capacity and
Alkalinity are
> not the same, that has always been the issue. I gave the equation does
that look like an
> Alkalinity equation or how Alk is determined. I see you had now comments
on it what's
> wrong, why no comments on the equations I gave. Don't understand them or
what ? Again this
> is the equation for Buffering Capacity, also called Buffer Index or Buffer
Intensity. It
> is defined in most water chemistry and chemical oceanography text books.
>
> B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> This is not Alkalinity now is it ?
>
> "I know how to do a titration, In fact I have done several. How many have
> you actually done? I don't mean by counting drops, I mean with a buret?"
>
> Well good for you, I use a Digital Titrator
>
> "Oh, I see,
> you think acidity is the opposite of alkalinity. In the world of
CHEMISTRY
> it's not. Maybe in aquarium newsgroups it is.
>
> Hum no, maybe you should go for a look at HACH's or LaMotte website or the
book I
> suggested earlier. Please view a copy.
>
> Standard Methods for the Examination of Water and Wastewater
>
> This book, over 2000 pages, is the guide for water testing. If you are
reporting water
> test to the EPA you must use approved std from this text.I t is prepared
and published by
> the EPA, American Water Works Association and American Public Health
Association. You
> mean you don't have one and the issue is water chemistry
>
> You are confusing Acidity and Acidity as you know little about water
chemistry and
> procedures and test methods
>
> From SMEWW, section 2-30, 2310 ACIDITY
>
> "Acidity of water is its quantative capacity to react with a strong base
to a designated
> pH"
>
> This is how you test for it
>
> A std alkali titration to methyl orange or phenolphthalein
> endpoint.
>
> BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write this
book, there are
> over 100 of them, they are wrong.
>
> Like Buffering Capacity you have your Acidity's mixed up
> In water measurement if you have a high Alk you also usually have a high
Acidity.
> Normally a high Alk also gives a higher CO2 level. Get a WATER CHEMISTRY
BOOK there pal.
>
>
> "These are all in equilibrium with each other. An initial high pH (above
> 6.4) will shift the equilibrium to the right to form HCO3-1. If the pH of
> the solution is above 10.3 (pKa2) the .........."
>
>
> Christ, there you go again with the FW ****. All your numbers are wrong we
are dealing
> with SEAWATER
>
> This means that at a pH of 8.3, the majority of the CO2(aq) is in the form
> of HCO3-1 .
>
> I have already pointed that out and gave actual values at know seawater
levels, go back
> and re-read it you aren't telling me anything here.Of course most is HCO3
see...
>
>
> @ 20C and 34.3 ppt salinity
>
> CO2 = 0.52 %
>
> HCO3 = 86.4 %
>
> CO3 = 13.09 %
>
>
> "In your glass experiment you managed to lower the pH enough to purge out
CO2
> by boiling"
>
> The purpose behind the glass is to show that alk is not affect by CO2 and
vise-versa and
> how Co2 affects pH.
>
> Now, in a real life seawater aquarium, with a pH of 8.3 and that pH drops
to say 8.1 it is
> usually due to excess CO2. If you took a glass of that water and aerated
it you WILL drive
> off the CO2 and raise the pH. It has been done a proven a million times.
>
> "In order to 'purge' CO2 you would need to lower the
> pH to shift the equilibrium to below 6.4"
>
> The hell you do !!!.Do you know who many times people on this NG to
include Dr. Craig
> Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
sample of aquarium
> water and aerate it to see if the pH GOES UP AND when they come back with
the test it is
> often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST excess
CO2 in the tank
> water, increase the circulation for better gas exchange at the surface,
reduce feeding,
> and try to improve on better skimming, thus reducing the bio-load and pH
decline due to
> CO2.
>
>
> "I hope this helps. "
>
> Help, how can you when you miss everything. I should be charging you
>
> Oh, by the way. Your websites, I have about 50 on these issues, I could
post them, not to
> mention I have all those water chemistry books, so there is no need to
view your sites.
>
> Finally are you afraid to come to our Chemistry Forum, afraid to get
slapped by REAL
> chemists. I get a charge out of you can't post your ref .I have posted the
same or similar
> stuff on his forum and I wasn't pointed out WRONG pal. I have 1500 posts
there and am the
> biggest contributor to his forum other than himself or maybe Habib Sheka
>
> Hum, here are Randy's ref that he posted. He hosts the website
>
> S. RANDY HOLMES-FARLEY
> Arlington, Massachusetts
>
> EDUCATION
>
> 1982-1986 Harvard University Cambridge, MA
> PhD in Chemistry
> Research Advisor: George Whitesides
>
> Investigated the relationship between polymer surface chemistry and
physical properties
> through controlled surface modification and testing.
>
> 1980-1982 Cornell University Ithaca, NY
> BA in Chemistry and Biology
> Graduated Summa Cum Laude
> Distinction in All Subjects
> Grade Point: 3.94/4.0
> Honors research: isolation and characterization of the subunit of CF1
enzyme
>
>
> 1978-1979 Stanford University Palo Alto, CA
> Grade Point: 3.55/4.0
>
>
> EXPERIENCE
>
> 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> (bought out GelTex Pharmaceuticals in 2001)
> Vice President, Chemical Research 2001-present
> Senior Director, Chemical Research 1999-2001
> Director of Chemical Research 1997-1999
> Manager of Chemical Research 1995-1997
> Group Leader 1994-1995
> Senior Research Scientist 1992-1994
>
> Helped start GelTex as second employee
>
> Managed various research programs with multi-million dollar budgets
>
> Supervised research chemists (17+)
>
> Co-inventor of several polymeric pharmaceuticals and pharmaceutical
candidates including
> Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride (FDA
approved)
>
> Company Safety Officer for 3 years
>
> Chemical Hygiene Officer 2000-present
>
>
>
>
> 1990-1992 GTE Corporation Waltham, MA
> Senior Member of Technical Staff
> Applied research involving polymer interfaces
> Metallization of plastics
> Polymer/polymer adhesion
> Optical coatings
>
>
>
> 1986-1990 Lord Corporation Cary, NC
> Senior Research Scientist 1988-1990
> Research Scientist 1986-1988
> Basic and applied research on surface chemical bonding
> Developed new adhesive compositions
> Developed new sol-gel coatings for corrosion resistance
>
>
> HONORS AND AWARDS
>
> Industrial Innovations Award by Northeast Region of American Chemical
Society (6/2001)
>
> National Kidney Foundation of Northern California Honoree (5/2001)
>
> American Chemical Society/Polymer Chemistry Division Industrial Sponsors
> Award (8/2000)
>
> R&D 100 Award from R&D magazine (1999)
>
> Sherwin Williams Award in applied polymer science (9/85)
>
> IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
>
> Award for highest GPA in Chemistry Department (6/82)
>
> Summa Cum Laude Honors in Chemistry (6/82)
>
> Phi Lamda Epsilon (6/82)
>
> Phi Beta Kappa (2/82)
>
> Cornell University Dean's List (1981, 1982)
>
> Harvard Book Club Award for highest GPA senior year (1978)
>
> First Place in western NY ACS high school chemistry exam (1977)
>
> 1978-1979
>
>
> __________________
> Randy Holmes-Farley
> Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
>
> Hobby Experience: 8 years with reefs
> Current Tanks: 90 gal mixed reef
> Interests: Reefkeeping, science, photography
>
>
> Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
>
> Open this post in a new window | Report this post to a moderator | IP:
Logged
>
>
>
> 06/27/2003 02:44 PM
>
> Randy Holmes-Farley
> Chemistry Moderator
>
> Registered: Apr 2001
> Location: Arlington, Massachusetts
> Occupation: Chemist (Drug Discovery at Genzyme)
> Posts: 15282
>
>
>
> Publications
>
>
> ISSUED UNITED STATES PATENTS
>
>
> 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
Mandeville, III; W. Harry.
> US 6,566,407; 5/20/2003
>
> 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen Randall;
Huval, Chad
> Cori.
> U.S. 6,517,825; 2/11/2003.
>
> 3. Method of making phosphate-binding polymers for oral administration.
Holmes-Farley,
> Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
6,509,013; 1/21/2003.
>
> 4. Combination therapy for treating hypercholesterolemia using a bile acid
sequestrant
> polymer
> and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley, Stephen
Randall;
> Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
>
> 5. Method for treating hypercholesterolemia with polyallylamine polymers.
Holmes-Farley,
> Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.; Goldberg,
Dennis I. , US
> 6,423,754; 7/23/2002.
>
> 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
Neenan, Thomas X..;
> Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
>
> 7. Combination therapy for treating hypercholesterolemia and
atherosclerosis. Huval, Chad
> Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep K.
U.S. 6,365,186;
> 4/2/2002.
>
> 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.; Mandeville,
W. H., III;
> Huval; C.
> C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
10/9/2001.
>
> 9. Polymers containing guanidinium groups as bile acid sequestrants. Dhal;
P. K.; Holmes-
> Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
>
> 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 6,281,252;
> 8/28/2001.
>
> 11. Combination therapy for treating hypercholestrolemia. Huval; C. C.;
Holmes-Farley; S.
> R. ;
> Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
>
> 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
Holmes-Farley, S.
> R.; US
> 6,264,937; 7/24/2001.
>
> 13. Method for treating hypercholesterolemia with unsubstituted
polydiallylamine polymers.
> Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
6,248,318;
> 6/19/2001.
>
> 14. Process for removing bile salts from a patient and alkylated
compositions therefore.
> Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
>
> 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S. R.;
Dhal, P. K.;
> Petersen,
> J. S.; US 6,203,785; 3/20/2001.
>
> 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.; Huval,
C. C.; US
> 6,190,649;
> 2/20/2001.
>
> 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 6,177,478;
> 1/23/2001.
>
> 18. Water-insoluble noncrosslinked bile acid sequestrants. Holmes-Farley,
S. R.;
> Mandeville, W.
> H., III.; US 6,129,910; 10/10/2000.
>
> 19. Method for treating hypercholesterolemia with unsubstituted
polydiallylamine polymers.
> Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
6,083,497;
> 7/4/2000.
>
> 20. Method of making phosphate-binding polymers for oral administration.
Holmes-Farley, S.
> R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495; 7/4/2000.
>
> 21. Process for removing bile salts from a patient and alkylated
compositions therefore.
> Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678; 5/23/2000.
>
> 22. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
>
> 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
Neenan; T. X.; Holmes-
> Farley; S. R. US 6,034,129; 3/7/2000.
>
> 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 5,985,938;
> 11/16/99.
>
> 25. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
>
> 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W. H.,
III.;
> Holmes-Farley;
> S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
>
> 27. Hydrophilic nonamine-containing and amine-containing copolymers and
their use as bile
> acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US 5,929,184;
7/27/99.
>
> 28. Interpenetrating polymer networks for sequestration of bile acids.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
7/20/99.
>
> 29. Amine polymer sequestrant and method of cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
>
> 30. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
>
> 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
>
> 32. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
>
> 33. Preparation of polymeric sequestrants for bile acid salts. Mandeville,
W. H., III.;
> Holmes-
> Farley, S. R.; US 5,703,188; 12/30/97.
>
> 34. Oral administration of iron-binding crosslinked amine polymers.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
>
> 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley, S.
R.; US 5,693,675;
> 12/2/97.
>
> 36. Method for removing bile salts from a patient with alkylated
crosslinked amine
> polymers,
> and preparation of the polymers. Mandeville, W. H., III.; Holmes-Farley,
S. R.; US
> 5,679,717; 10/21/97.
>
> 37. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville,
> W.
> H., III.; US 5,667,775; 9/16/97.
>
> 38. Ion-exchange process using highly crosslinked polymers for removing
bile salts from a
> patient, preparation of the polymers, and compositions containing them.
Mandeville, W. H.,
> III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
>
> 39. Hydrophobic amine polymer sequestrant and method of cholesterol
depletion. Mandeville,
> W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530; 4/8/97.
>
> 40. Amine polymer sequestrant and method of cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
>
> 41. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville,
> W.
> H., III.; US 5,496,545; 3/5/96.
>
> 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
III.; Holmes-Farley,
> S. R.;
> US 5,487,888; 1/30/96.
>
> 43. Ultra-thin, uniform sol-gel coating of a substrate having active
hydrogens on the
> surface.
> Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
>
> 44. Layered sol-gel coatings from organisilicon compounds. Holmes-Farley,
S. R.; Yanyo, L.
> C.;
> US 5,182,143; 1/26/93.
>
> 45. Method for metal bonding using ultrathin primer coating.
Holmes-Farley, S. R.; Yanyo,
> L.
> C.; Thuer, A. M.; US 5,139,601; 8/18/92.
>
> 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.; US
5,096,962;
> 3/17/92.
>
> 47. Modified halogenatedpolyolefin adhesives for polyolefin
elastomer-metal bonding.
> Holmes-
> Farley, S. R.; US 5,102,956; 4/7/92.
>
>
>
> PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
>
>
> 1. Aryl boronate functionalized polymers for treating obesity and
inhibiting fat uptake.
> Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal, Pradeep
K.; Huval, Chad
> Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92 pp. WO
0302571.
>
> 2. Preparation of aryl boronic acids for treating obesity. Holmes-Farley,
Stephen Randall;
> Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep K.
(Geltex
> Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
>
> 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
Stephen Randall.
> (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
0302130.
>
> 4. Method for reducing copper levels and treating copper toxicosis.
Holmes-Farley, Stephen
> Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002), 45
pp. WO
> 0285383.
>
> 5. Method for treating gout and binding uric acid. Holmes-Farley, Stephen
Randall; Burke,
> Steven K. WO 0285381 10/31/2002.
>
> 6. Method for treating gout and reducing serum uric acid. Holmes-Farley,
Stephen Randall;
> Burke, Steven K WO 0285380 10/31/2002.
>
> 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
Holmes-Farley, S. R.;
> Whitesides, G. M. WO 1999-US30469; 7/6/2000.
>
> 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
Holmes-Farley, S.
> R.;
> WO 1999-US5662; 9/23/1999.
>
> 9. Amine-containing copolymers as bile acid sequestrants. Holmes-Farley,
S. R.; Petersen,
> J. S.;
> WO 9933452; 7/8/1999.
>
> 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III and
Holmes-Farley, S.
> R.;
> WO 9922743; 5/14/1999.
>
> 11. Polyallylamine polymers for removing bile salts and treating
hypercholesterolemia, and
> polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III; Burke,
S. K.; Goldberg,
> D. I.; WO 9857652; 12/23/98.
>
> 12. Phosphate-bidning polymers combined with a calcium supplement for oral
administration.
> Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley, S.
R.; WO 9842355;
> 10/1/98.
>
> 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
depletion. Mandeville,
> W.
> H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
>
> 14. Process for adjusting ion concentration in a patient and compositions
therefor.
> Mandeville,
> W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
>
> 15. Vacuum-deposited silver on polycarbonate with a chromium interlayer
for improved
> metal-
> substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512; 1/20/94.
>
> 16. Process for increased metal-substrate bond strength in metalized
plastics.
> Holmes-Farley, S.
> R.; Ger. Offen. 4322516; 7/6/93.
>
> 17. Electrorheological fluids and preparation of particles useful in the
fluids.
> Troughton,
> Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
David; Bares, Joseph
> E.;
> Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
394049;
> 10/24/1990.
>
> JOURNAL PUBLICATIONS
>
> 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov, Eugene;
Guo, Amy;
> Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
Mandeville, W. Harry;
> Holmes-Farley, S. Randall. Kidney International (2002), 62(2), 611-619.
>
> 2. Amine functionalized polyethers as bile acid sequestrants: synthesis
and biological
> evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S. Randall;
Mandeville, W.
> Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
Journal of
> Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
1559-1574.
>
> 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
Imprinting. Huval,
> Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
Randall; Mandeville,
> W.
> Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert J.;
Chen, Xi; Dhal,
> Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
>
> 4. Synthetic polymers for the binding of fat in the intestinal tract.
Jozefiak, Thomas H.;
> Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia; Huval,
Chad C.;
> Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
Abstracts of
> Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
26-30, 2001
> (2001), POLY-047 and Polymer Preprints (American Chemical Society,
Division of
> Polymer Chemistry) (2001), 42(2), 98.
>
> 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer gel
pharmaceutical.
> Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.; Ward,
J.; Sacchiero,
> B.;
> Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.; Chen,
X.; Mazzeo, J.
> R.. Polym. Preprints (2000), 41(1), 735-736.
>
> 6. In vitro comparison of bile acid binding to colesevelam HCl and other
bile acid
> sequestrants.
> Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
Hook, P.; Holmes-
> Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
>
> 7. Novel polymeric pharmaceuticals: From startup to market. Holmes-Farley,
S. R; Polym.
> Mater. Sci. Eng (1999), 80, 246-247.
>
> 8. Design and characterization of of Sevelamer Hydrochloride: a novel
phosphate-binding
> pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward, J.;
Miller, K. L.;
> Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure and
Appl. Chem.,
> A36(7&8), p. 1085 (1999).
>
> 9. Three generations of bile acid sequestrants. Mandeville, W. H., III;
Braunlin, W.;
> Dhal, P.;
> Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
Rosenbaum, D.;
> Sacchiero,
> R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
550, 3-15.
>
> 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric phosphate
binder, on
> urinary
> phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
Mandeville, W. H.,
> III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
(1997), 12(5)
> 961-964.
>
> 11. Thin anisotropic coatings based on sol-gel technology. Holmes-Farley,
S. R.; Yanyo, L.
> C;
> Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4), 439-444.
>
> 12. The mechanism of cure initiation of a surface activated adhesive.
Holmes-Farley, S.
> R.;
> Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
>
> 13. Adhesion promotion and corrosion prevention using thin anisotropic
coatings. Holmes-
> Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
131-151.
>
> 14. Wetting of functionalized polyethylene having ionizable organic acids
and bases at the
> polymer-water interface: relations between functional group polarity,
extent of
> ionization,
> and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
Whitesides, G. M.;
> Langmuir
> (1988), 4(4), 921-937.
>
> 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
single hydroxy group.
> Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
>
> 16. Reconstruction of the interface of oxidatively functionalized
polyethylene (PE-CO2H)
> and
> derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo, R.;
McCarthy, T. J.;
> Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report (1987),
AD-
> A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
>
> 17. Surface-modified polyethylene film: the relationship between surface
chemistry and
> physical
> properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11), 4537.
>
> 18. Reactivity of carboxylic acid and ester groups in the functionalized
interfacial
> region of
> "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
differentiation of the
> functional groups into shallow and deep subsets based on a comparison of
contact angle and
> ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
(1987), 3(1), 62-
> 76.
>
> 19. Fluorescence properties of dansyl groups covalently bonded tot he
surface of
> oxidatively
> functionalized low-density polyethylene film. Holmes-Farley, S. R.;
Whitesides, G. M.;
> Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
AD-A162435/2/GAR,
> Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
>
> 20. Acid-base behavior of carboxylic acid groups covalently attached at
the surface of
> polyethylene: The usefulness of contact angle in following the ionization
of surface
> functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
Deutch, J.;
> Whitesides,
> G. M.; Langmuir (1985), 1(6), 725-740.
>
> 21. The thermal stability of a surface modified solid organic polymer.
Holmes-Farley, S.
> R.;
> Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
>
>
>
> CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
>
> 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
Aquarist. June 2003.
>
> 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
Advanced Aquarist.
> May
> 2003.
>
> 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
Reefkeeping May
> 2003.
>
> 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
April 2003.
>
> 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
Holmes-Farley, R.
> Advanced Aquarist; April 2003.
>
> 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
Holmes-Farley, R.
> Advanced Aquarist; April 2003.
>
> 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced Aquarist;
March 2003.
>
> 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
Holmes-Farley, R.
> Advanced Aquarist; February 2003.
>
> 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
2003.
>
> 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; December
2002.
>
> 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R. Advanced
Aquarist; November
> 2002.
>
> 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
Advanced Aquarist;
> November 2002.
>
> 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced Aquarist,
September 2002.
>
> 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
2002.
>
> 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
2002.
>
> 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
Aquarist; July 2002
>
> 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist; June
2002.
>
> 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R. Advanced
Aquarist, May
> 2002.
>
> 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
Holmes-Farley, R.
> Advanced Aquarist, April 2002.
>
> 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
>
> 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
>
> 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January 2002.
>
> 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
2000.
>
> 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
Frontiers 2000.
>
> 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
Aquarium Frontiers
> 2000.
> 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium Frontiers
2000.
>
> 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers 2000.
>
> 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
>
> 29. Protein Skimming: How it Works. Fishnet Library 1998.
>
>
>
>
>
>
>
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
>
>

[stoutman]

Boomer, sorry for the name calling in the previous post.


Let me respond to your equation question that you are stuck on.

B (Buffering Index) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa [H3O+]
/ (Ka + H3O+])² )


C = total concentration of the acid + conjugate base = [HA] + [A-]
Unknown
Ka = acid dissociation constant. Found in a table
[H3O] = Determined from pH. where pH = -log [H+]

Only unknown in the equation is C which is [HA] + [A-].

In this case the conjugate base is CO3- and the acid is HCO3-2 and Ka is
Ka2 for carbonic acid.

One way to solve the equation is to determine the combined concentrations of
:[CO3-] and [HCO3-2] in solution.

Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes, your
alkalinity equation.

So when we measure ALKALINITY we are indirectly measuring BUFFERING
CAPACITY.

Because aquarium and sea water have other buffers in solution, you need to
determine the BUFFERING INDEX for each buffer in solution.

Does this help? Or are we NEVER going to agree on anything?




"Boomer" > wrote in message
...
> Now I am getting bored
>
> "Don't the components of a buffer account for the buffering capacity?
Yes."
>
> Yes, agreed but you seem to fail what I'm saying. Buffering Capacity and
Alkalinity are
> not the same, that has always been the issue. I gave the equation does
that look like an
> Alkalinity equation or how Alk is determined. I see you had now comments
on it what's
> wrong, why no comments on the equations I gave. Don't understand them or
what ? Again this
> is the equation for Buffering Capacity, also called Buffer Index or Buffer
Intensity. It
> is defined in most water chemistry and chemical oceanography text books.
>
> B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> This is not Alkalinity now is it ?
>
> "I know how to do a titration, In fact I have done several. How many have
> you actually done? I don't mean by counting drops, I mean with a buret?"
>
> Well good for you, I use a Digital Titrator
>
> "Oh, I see,
> you think acidity is the opposite of alkalinity. In the world of
CHEMISTRY
> it's not. Maybe in aquarium newsgroups it is.
>
> Hum no, maybe you should go for a look at HACH's or LaMotte website or the
book I
> suggested earlier. Please view a copy.
>
> Standard Methods for the Examination of Water and Wastewater
>
> This book, over 2000 pages, is the guide for water testing. If you are
reporting water
> test to the EPA you must use approved std from this text.I t is prepared
and published by
> the EPA, American Water Works Association and American Public Health
Association. You
> mean you don't have one and the issue is water chemistry
>
> You are confusing Acidity and Acidity as you know little about water
chemistry and
> procedures and test methods
>
> From SMEWW, section 2-30, 2310 ACIDITY
>
> "Acidity of water is its quantative capacity to react with a strong base
to a designated
> pH"
>
> This is how you test for it
>
> A std alkali titration to methyl orange or phenolphthalein
> endpoint.
>
> BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write this
book, there are
> over 100 of them, they are wrong.
>
> Like Buffering Capacity you have your Acidity's mixed up
> In water measurement if you have a high Alk you also usually have a high
Acidity.
> Normally a high Alk also gives a higher CO2 level. Get a WATER CHEMISTRY
BOOK there pal.
>
>
> "These are all in equilibrium with each other. An initial high pH (above
> 6.4) will shift the equilibrium to the right to form HCO3-1. If the pH of
> the solution is above 10.3 (pKa2) the .........."
>
>
> Christ, there you go again with the FW ****. All your numbers are wrong we
are dealing
> with SEAWATER
>
> This means that at a pH of 8.3, the majority of the CO2(aq) is in the form
> of HCO3-1 .
>
> I have already pointed that out and gave actual values at know seawater
levels, go back
> and re-read it you aren't telling me anything here.Of course most is HCO3
see...
>
>
> @ 20C and 34.3 ppt salinity
>
> CO2 = 0.52 %
>
> HCO3 = 86.4 %
>
> CO3 = 13.09 %
>
>
> "In your glass experiment you managed to lower the pH enough to purge out
CO2
> by boiling"
>
> The purpose behind the glass is to show that alk is not affect by CO2 and
vise-versa and
> how Co2 affects pH.
>
> Now, in a real life seawater aquarium, with a pH of 8.3 and that pH drops
to say 8.1 it is
> usually due to excess CO2. If you took a glass of that water and aerated
it you WILL drive
> off the CO2 and raise the pH. It has been done a proven a million times.
>
> "In order to 'purge' CO2 you would need to lower the
> pH to shift the equilibrium to below 6.4"
>
> The hell you do !!!.Do you know who many times people on this NG to
include Dr. Craig
> Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
sample of aquarium
> water and aerate it to see if the pH GOES UP AND when they come back with
the test it is
> often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST excess
CO2 in the tank
> water, increase the circulation for better gas exchange at the surface,
reduce feeding,
> and try to improve on better skimming, thus reducing the bio-load and pH
decline due to
> CO2.
>
>
> "I hope this helps. "
>
> Help, how can you when you miss everything. I should be charging you
>
> Oh, by the way. Your websites, I have about 50 on these issues, I could
post them, not to
> mention I have all those water chemistry books, so there is no need to
view your sites.
>
> Finally are you afraid to come to our Chemistry Forum, afraid to get
slapped by REAL
> chemists. I get a charge out of you can't post your ref .I have posted the
same or similar
> stuff on his forum and I wasn't pointed out WRONG pal. I have 1500 posts
there and am the
> biggest contributor to his forum other than himself or maybe Habib Sheka
>
> Hum, here are Randy's ref that he posted. He hosts the website
>
> S. RANDY HOLMES-FARLEY
> Arlington, Massachusetts
>
> EDUCATION
>
> 1982-1986 Harvard University Cambridge, MA
> PhD in Chemistry
> Research Advisor: George Whitesides
>
> Investigated the relationship between polymer surface chemistry and
physical properties
> through controlled surface modification and testing.
>
> 1980-1982 Cornell University Ithaca, NY
> BA in Chemistry and Biology
> Graduated Summa Cum Laude
> Distinction in All Subjects
> Grade Point: 3.94/4.0
> Honors research: isolation and characterization of the subunit of CF1
enzyme
>
>
> 1978-1979 Stanford University Palo Alto, CA
> Grade Point: 3.55/4.0
>
>
> EXPERIENCE
>
> 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> (bought out GelTex Pharmaceuticals in 2001)
> Vice President, Chemical Research 2001-present
> Senior Director, Chemical Research 1999-2001
> Director of Chemical Research 1997-1999
> Manager of Chemical Research 1995-1997
> Group Leader 1994-1995
> Senior Research Scientist 1992-1994
>
> Helped start GelTex as second employee
>
> Managed various research programs with multi-million dollar budgets
>
> Supervised research chemists (17+)
>
> Co-inventor of several polymeric pharmaceuticals and pharmaceutical
candidates including
> Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride (FDA
approved)
>
> Company Safety Officer for 3 years
>
> Chemical Hygiene Officer 2000-present
>
>
>
>
> 1990-1992 GTE Corporation Waltham, MA
> Senior Member of Technical Staff
> Applied research involving polymer interfaces
> Metallization of plastics
> Polymer/polymer adhesion
> Optical coatings
>
>
>
> 1986-1990 Lord Corporation Cary, NC
> Senior Research Scientist 1988-1990
> Research Scientist 1986-1988
> Basic and applied research on surface chemical bonding
> Developed new adhesive compositions
> Developed new sol-gel coatings for corrosion resistance
>
>
> HONORS AND AWARDS
>
> Industrial Innovations Award by Northeast Region of American Chemical
Society (6/2001)
>
> National Kidney Foundation of Northern California Honoree (5/2001)
>
> American Chemical Society/Polymer Chemistry Division Industrial Sponsors
> Award (8/2000)
>
> R&D 100 Award from R&D magazine (1999)
>
> Sherwin Williams Award in applied polymer science (9/85)
>
> IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
>
> Award for highest GPA in Chemistry Department (6/82)
>
> Summa Cum Laude Honors in Chemistry (6/82)
>
> Phi Lamda Epsilon (6/82)
>
> Phi Beta Kappa (2/82)
>
> Cornell University Dean's List (1981, 1982)
>
> Harvard Book Club Award for highest GPA senior year (1978)
>
> First Place in western NY ACS high school chemistry exam (1977)
>
> 1978-1979
>
>
> __________________
> Randy Holmes-Farley
> Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
>
> Hobby Experience: 8 years with reefs
> Current Tanks: 90 gal mixed reef
> Interests: Reefkeeping, science, photography
>
>
> Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
>
> Open this post in a new window | Report this post to a moderator | IP:
Logged
>
>
>
> 06/27/2003 02:44 PM
>
> Randy Holmes-Farley
> Chemistry Moderator
>
> Registered: Apr 2001
> Location: Arlington, Massachusetts
> Occupation: Chemist (Drug Discovery at Genzyme)
> Posts: 15282
>
>
>
> Publications
>
>
> ISSUED UNITED STATES PATENTS
>
>
> 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
Mandeville, III; W. Harry.
> US 6,566,407; 5/20/2003
>
> 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen Randall;
Huval, Chad
> Cori.
> U.S. 6,517,825; 2/11/2003.
>
> 3. Method of making phosphate-binding polymers for oral administration.
Holmes-Farley,
> Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
6,509,013; 1/21/2003.
>
> 4. Combination therapy for treating hypercholesterolemia using a bile acid
sequestrant
> polymer
> and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley, Stephen
Randall;
> Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
>
> 5. Method for treating hypercholesterolemia with polyallylamine polymers.
Holmes-Farley,
> Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.; Goldberg,
Dennis I. , US
> 6,423,754; 7/23/2002.
>
> 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
Neenan, Thomas X..;
> Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
>
> 7. Combination therapy for treating hypercholesterolemia and
atherosclerosis. Huval, Chad
> Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep K.
U.S. 6,365,186;
> 4/2/2002.
>
> 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.; Mandeville,
W. H., III;
> Huval; C.
> C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
10/9/2001.
>
> 9. Polymers containing guanidinium groups as bile acid sequestrants. Dhal;
P. K.; Holmes-
> Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
>
> 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 6,281,252;
> 8/28/2001.
>
> 11. Combination therapy for treating hypercholestrolemia. Huval; C. C.;
Holmes-Farley; S.
> R. ;
> Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
>
> 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
Holmes-Farley, S.
> R.; US
> 6,264,937; 7/24/2001.
>
> 13. Method for treating hypercholesterolemia with unsubstituted
polydiallylamine polymers.
> Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
6,248,318;
> 6/19/2001.
>
> 14. Process for removing bile salts from a patient and alkylated
compositions therefore.
> Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
>
> 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S. R.;
Dhal, P. K.;
> Petersen,
> J. S.; US 6,203,785; 3/20/2001.
>
> 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.; Huval,
C. C.; US
> 6,190,649;
> 2/20/2001.
>
> 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 6,177,478;
> 1/23/2001.
>
> 18. Water-insoluble noncrosslinked bile acid sequestrants. Holmes-Farley,
S. R.;
> Mandeville, W.
> H., III.; US 6,129,910; 10/10/2000.
>
> 19. Method for treating hypercholesterolemia with unsubstituted
polydiallylamine polymers.
> Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
6,083,497;
> 7/4/2000.
>
> 20. Method of making phosphate-binding polymers for oral administration.
Holmes-Farley, S.
> R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495; 7/4/2000.
>
> 21. Process for removing bile salts from a patient and alkylated
compositions therefore.
> Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678; 5/23/2000.
>
> 22. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
>
> 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
Neenan; T. X.; Holmes-
> Farley; S. R. US 6,034,129; 3/7/2000.
>
> 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
III.; US
> 5,985,938;
> 11/16/99.
>
> 25. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
>
> 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W. H.,
III.;
> Holmes-Farley;
> S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
>
> 27. Hydrophilic nonamine-containing and amine-containing copolymers and
their use as bile
> acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US 5,929,184;
7/27/99.
>
> 28. Interpenetrating polymer networks for sequestration of bile acids.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
7/20/99.
>
> 29. Amine polymer sequestrant and method of cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
>
> 30. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
>
> 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
>
> 32. Process for removing bile salts from a patient and compositions
therefor. Mandeville,
> W. H.,
> III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
>
> 33. Preparation of polymeric sequestrants for bile acid salts. Mandeville,
W. H., III.;
> Holmes-
> Farley, S. R.; US 5,703,188; 12/30/97.
>
> 34. Oral administration of iron-binding crosslinked amine polymers.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
>
> 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley, S.
R.; US 5,693,675;
> 12/2/97.
>
> 36. Method for removing bile salts from a patient with alkylated
crosslinked amine
> polymers,
> and preparation of the polymers. Mandeville, W. H., III.; Holmes-Farley,
S. R.; US
> 5,679,717; 10/21/97.
>
> 37. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville,
> W.
> H., III.; US 5,667,775; 9/16/97.
>
> 38. Ion-exchange process using highly crosslinked polymers for removing
bile salts from a
> patient, preparation of the polymers, and compositions containing them.
Mandeville, W. H.,
> III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
>
> 39. Hydrophobic amine polymer sequestrant and method of cholesterol
depletion. Mandeville,
> W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530; 4/8/97.
>
> 40. Amine polymer sequestrant and method of cholesterol depletion.
Mandeville, W. H.,
> III.;
> Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
>
> 41. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
R.; Mandeville,
> W.
> H., III.; US 5,496,545; 3/5/96.
>
> 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
III.; Holmes-Farley,
> S. R.;
> US 5,487,888; 1/30/96.
>
> 43. Ultra-thin, uniform sol-gel coating of a substrate having active
hydrogens on the
> surface.
> Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
>
> 44. Layered sol-gel coatings from organisilicon compounds. Holmes-Farley,
S. R.; Yanyo, L.
> C.;
> US 5,182,143; 1/26/93.
>
> 45. Method for metal bonding using ultrathin primer coating.
Holmes-Farley, S. R.; Yanyo,
> L.
> C.; Thuer, A. M.; US 5,139,601; 8/18/92.
>
> 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.; US
5,096,962;
> 3/17/92.
>
> 47. Modified halogenatedpolyolefin adhesives for polyolefin
elastomer-metal bonding.
> Holmes-
> Farley, S. R.; US 5,102,956; 4/7/92.
>
>
>
> PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
>
>
> 1. Aryl boronate functionalized polymers for treating obesity and
inhibiting fat uptake.
> Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal, Pradeep
K.; Huval, Chad
> Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92 pp. WO
0302571.
>
> 2. Preparation of aryl boronic acids for treating obesity. Holmes-Farley,
Stephen Randall;
> Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep K.
(Geltex
> Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
>
> 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
Stephen Randall.
> (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
0302130.
>
> 4. Method for reducing copper levels and treating copper toxicosis.
Holmes-Farley, Stephen
> Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002), 45
pp. WO
> 0285383.
>
> 5. Method for treating gout and binding uric acid. Holmes-Farley, Stephen
Randall; Burke,
> Steven K. WO 0285381 10/31/2002.
>
> 6. Method for treating gout and reducing serum uric acid. Holmes-Farley,
Stephen Randall;
> Burke, Steven K WO 0285380 10/31/2002.
>
> 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
Holmes-Farley, S. R.;
> Whitesides, G. M. WO 1999-US30469; 7/6/2000.
>
> 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
Holmes-Farley, S.
> R.;
> WO 1999-US5662; 9/23/1999.
>
> 9. Amine-containing copolymers as bile acid sequestrants. Holmes-Farley,
S. R.; Petersen,
> J. S.;
> WO 9933452; 7/8/1999.
>
> 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III and
Holmes-Farley, S.
> R.;
> WO 9922743; 5/14/1999.
>
> 11. Polyallylamine polymers for removing bile salts and treating
hypercholesterolemia, and
> polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III; Burke,
S. K.; Goldberg,
> D. I.; WO 9857652; 12/23/98.
>
> 12. Phosphate-bidning polymers combined with a calcium supplement for oral
administration.
> Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley, S.
R.; WO 9842355;
> 10/1/98.
>
> 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
depletion. Mandeville,
> W.
> H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
>
> 14. Process for adjusting ion concentration in a patient and compositions
therefor.
> Mandeville,
> W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
>
> 15. Vacuum-deposited silver on polycarbonate with a chromium interlayer
for improved
> metal-
> substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512; 1/20/94.
>
> 16. Process for increased metal-substrate bond strength in metalized
plastics.
> Holmes-Farley, S.
> R.; Ger. Offen. 4322516; 7/6/93.
>
> 17. Electrorheological fluids and preparation of particles useful in the
fluids.
> Troughton,
> Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
David; Bares, Joseph
> E.;
> Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
394049;
> 10/24/1990.
>
> JOURNAL PUBLICATIONS
>
> 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov, Eugene;
Guo, Amy;
> Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
Mandeville, W. Harry;
> Holmes-Farley, S. Randall. Kidney International (2002), 62(2), 611-619.
>
> 2. Amine functionalized polyethers as bile acid sequestrants: synthesis
and biological
> evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S. Randall;
Mandeville, W.
> Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
Journal of
> Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
1559-1574.
>
> 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
Imprinting. Huval,
> Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
Randall; Mandeville,
> W.
> Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert J.;
Chen, Xi; Dhal,
> Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
>
> 4. Synthetic polymers for the binding of fat in the intestinal tract.
Jozefiak, Thomas H.;
> Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia; Huval,
Chad C.;
> Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
Abstracts of
> Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
26-30, 2001
> (2001), POLY-047 and Polymer Preprints (American Chemical Society,
Division of
> Polymer Chemistry) (2001), 42(2), 98.
>
> 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer gel
pharmaceutical.
> Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.; Ward,
J.; Sacchiero,
> B.;
> Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.; Chen,
X.; Mazzeo, J.
> R.. Polym. Preprints (2000), 41(1), 735-736.
>
> 6. In vitro comparison of bile acid binding to colesevelam HCl and other
bile acid
> sequestrants.
> Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
Hook, P.; Holmes-
> Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
>
> 7. Novel polymeric pharmaceuticals: From startup to market. Holmes-Farley,
S. R; Polym.
> Mater. Sci. Eng (1999), 80, 246-247.
>
> 8. Design and characterization of of Sevelamer Hydrochloride: a novel
phosphate-binding
> pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward, J.;
Miller, K. L.;
> Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure and
Appl. Chem.,
> A36(7&8), p. 1085 (1999).
>
> 9. Three generations of bile acid sequestrants. Mandeville, W. H., III;
Braunlin, W.;
> Dhal, P.;
> Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
Rosenbaum, D.;
> Sacchiero,
> R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
550, 3-15.
>
> 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric phosphate
binder, on
> urinary
> phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
Mandeville, W. H.,
> III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
(1997), 12(5)
> 961-964.
>
> 11. Thin anisotropic coatings based on sol-gel technology. Holmes-Farley,
S. R.; Yanyo, L.
> C;
> Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4), 439-444.
>
> 12. The mechanism of cure initiation of a surface activated adhesive.
Holmes-Farley, S.
> R.;
> Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
>
> 13. Adhesion promotion and corrosion prevention using thin anisotropic
coatings. Holmes-
> Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
131-151.
>
> 14. Wetting of functionalized polyethylene having ionizable organic acids
and bases at the
> polymer-water interface: relations between functional group polarity,
extent of
> ionization,
> and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
Whitesides, G. M.;
> Langmuir
> (1988), 4(4), 921-937.
>
> 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
single hydroxy group.
> Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
>
> 16. Reconstruction of the interface of oxidatively functionalized
polyethylene (PE-CO2H)
> and
> derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo, R.;
McCarthy, T. J.;
> Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report (1987),
AD-
> A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
>
> 17. Surface-modified polyethylene film: the relationship between surface
chemistry and
> physical
> properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11), 4537.
>
> 18. Reactivity of carboxylic acid and ester groups in the functionalized
interfacial
> region of
> "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
differentiation of the
> functional groups into shallow and deep subsets based on a comparison of
contact angle and
> ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
(1987), 3(1), 62-
> 76.
>
> 19. Fluorescence properties of dansyl groups covalently bonded tot he
surface of
> oxidatively
> functionalized low-density polyethylene film. Holmes-Farley, S. R.;
Whitesides, G. M.;
> Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
AD-A162435/2/GAR,
> Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
>
> 20. Acid-base behavior of carboxylic acid groups covalently attached at
the surface of
> polyethylene: The usefulness of contact angle in following the ionization
of surface
> functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
Deutch, J.;
> Whitesides,
> G. M.; Langmuir (1985), 1(6), 725-740.
>
> 21. The thermal stability of a surface modified solid organic polymer.
Holmes-Farley, S.
> R.;
> Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
>
>
>
> CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
>
> 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
Aquarist. June 2003.
>
> 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
Advanced Aquarist.
> May
> 2003.
>
> 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
Reefkeeping May
> 2003.
>
> 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
April 2003.
>
> 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
Holmes-Farley, R.
> Advanced Aquarist; April 2003.
>
> 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
Holmes-Farley, R.
> Advanced Aquarist; April 2003.
>
> 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced Aquarist;
March 2003.
>
> 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
Holmes-Farley, R.
> Advanced Aquarist; February 2003.
>
> 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
2003.
>
> 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; December
2002.
>
> 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R. Advanced
Aquarist; November
> 2002.
>
> 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
Advanced Aquarist;
> November 2002.
>
> 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced Aquarist,
September 2002.
>
> 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
2002.
>
> 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
2002.
>
> 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
Aquarist; July 2002
>
> 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist; June
2002.
>
> 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R. Advanced
Aquarist, May
> 2002.
>
> 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
Holmes-Farley, R.
> Advanced Aquarist, April 2002.
>
> 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
>
> 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
>
> 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January 2002.
>
> 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
2000.
>
> 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
Frontiers 2000.
>
> 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
Aquarium Frontiers
> 2000.
> 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium Frontiers
2000.
>
> 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers 2000.
>
> 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
>
> 29. Protein Skimming: How it Works. Fishnet Library 1998.
>
>
>
>
>
>
>
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
>
>

[Boomer]

Allot of things to answer now lets see what you accept or don't expect, based on std ref,
all by chemists, not by me. I have lots of problems with these last few posts, so I guess
it is time I put you somewhat in place in comments you made, WITHOUT you even checking the
ref. Bad move on your part, so lets see what you have to say when I'm done, no name
calling by me, just trying to get you to see a few things.......and help YOU on
something's you seem not to know about.


"I never said alkalinity and buffering capacity are the same thing. When did
I say that? Now you are twisting my words."


***alkalinity is a measurement of 'buffering capacity'***

Which comes across to me that they are the same thing. Alkalinity is not a measurement of
BC(see below)

I don't need the links I have many and some are the same as yours. I think we are on a
word game, lets call it that, maybe a misunderstanding. As I had posted earlier,
(Millero/per com), Bc is the ability to withstand both upward and downward trends in pH
and Alk is the ability to withstand downward trends in pH


From

Benjamin,Water Chemistry (2002, pages 262-263).Dr. Benjamin is a civil and environmental
engineering chemist at the U.of Washington

Alk = *** The amount of a stung acid to titrate a solution to a preselected pH of near
4.7............For this reason, the alkalinity is sometimes referred to as the acid
neutralizing capacity (ANC) of the water, based on the assumption that once this capacity
is used up, sever ecological effects become much more likely.***

"ACIDITY IS the opposite of BASICITY. You are an idiot!

"Ok, if that's what they think than they are wrong. I haven't read there
books, I will take your word for it. If their logic is the same as yours,
their WRONG as well."

"I'm confusing 'Acidity' and 'Acidity' What? Ok, now I really think you
are an idiot."


This shows me how little about water chemistry you know with this statement or are you
just trying to make all other chemists wrong and you wright, as that is real joke. All of
the worlds most well know water chemists are wrong and you are right. Take note how you
jumped to a conclusion without even lookin' or thinkin' of what you said, doesn't speak
much of yourself. This will be one example, how many do I need and from how many water
chemistry books do I need, to post or explain to you.

***Benjamin,Water Chemistry (2002, pages 262-263).***

***A concept that is exactly analogous to alkalinity but measures the base neutralizing
capacity (BNC) of a solution is Acidity. The quantitative represents the concentration of
OH- ions that must be added to titrate the solution to a pH near 10.5***

So that means that not only in Benjamin wrong but, so are Stumm & Morgan, Millero, Pilosn,
Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I said, you have your
acidity and Acidy mixed up. Acidity as defined above is covered in most water chemistry
books, written by chemists, who's field of expertise is water chemistry. You can even buy
Acidity test kits from, HACH, LaMotte, etc..

Please explain where the HELL you get this idea from these guys are flipin' marine
biologists. Do a dam search on them or shut the hell up. All of my ref but one are from
chemists......PERIOD and most have been in their field for more than a decade and some for
4 decades. And most of them teach chemistry and are professors of chemistry.Point one out
that's not.There are NO marine biologist that have ever written a water chemistry book I
collect them, it is a hobby of mine.

Like I said you have your acidity and Acidity mixed up. You never asked to have me
explain, as other chemists do, not familiar with water chemistry, just jump the gun and
start the dam name calling. BUT I see you have apologized. I don't hold grudges, just like
to have things straight. I also don't; mind me correct, I don't like giving out incorrect
info..come to be correct, if needed. How about YOU. This hobby is plagued with myths and
misconception and other things beside chemistry


"> Christ, there you go again with the FW ****. All your numbers are wrong we
are dealing
> with SEAWATER

You didn't say in your experiment that sea water was being used. The HH
equation STILL applies"

YOU, YOU keep posting pKa's for FW and are applying them to seawater, in YOUR examples.
You can't use FW pKa's of Freshwater when dealing with seawater. I told you before they
are not the same and are skewed to the left. NSW at @25 C and 35 ppt, are as given in my
other post. pKa1= 6.00 and pKa 2 = 9.1.If you are going to be making calculations use the
right pKa's. pKa's are a faction of salinity and temp. At least twice, YOU have used FW
pKa's for seawater examples, need I point them out ? Here is just one

"The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this example)
you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium will
be shifted to HCO3-2 by a ratio of 1:100"

"Maybe you should send
them an e-mail and tell them their web pages are wrong and that they are
offending all the marine biologists across the country."

More of your BS line. What marine biologists have I mentioned or posted, please show
me.Their is acidy and basicty and there is Alkalinity and Acidity

"Therefore, measuring alkalinity tells you something about your 'buffering
capacity'.


Yes, agreed. If you go back a check one of my post I said Millero said if you know the BC
you can calculate the Alk. Matter of fact I believe he also said there was conversion for
it. The only method we have to give us an idea of the buffering capacity is Alk. However,
if you took Alk and Acidity you will have even a better idea for both up and down the
scale


"So when we measure ALKALINITY we are indirectly measuring BUFFERING
CAPACITY.

Because aquarium and sea water have other buffers in solution, you need to
determine the BUFFERING INDEX for each buffer in solution"


Yes, I would agree to that and is why I said BC isn't the same as Alk However, it is only
telling us half of the story in regards to BC, nothing of the Acidity, which in most cases
is something we don't need to worry about or even measure, as our problems 95 % of the
times are falling pH and not rising pH ( but this does happen in systems high in
plants/algae)

I think that covers it for now


Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

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If You See Me Running You Better Catch-Up

[Boomer]

Alkalinity a measure of the amount of anions of weak acid in water and of the cations
balanced against them
Take note it says ***acid***

Buffering capacity the ability of a solution to resist or dampen changes in pH upon the
addition of acids or bases.
Take note its says ***the addition of acids or bases***

One more

http://www.waterontheweb.org/resources/glossary.html

We could go on like this all day, so what is the point ?

You will LOVE this one
http://www.kyantec.com/Tips/phbuffering.htm

Don't you just lovbe PDF's
http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf

Don't fall out of your chair
http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm




--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

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If You See Me Running You Better Catch-Up
"stoutman" <.@.> wrote in message news:XB7Wb.19339$QA2.62332@attbi_s52...
: Man here is another, google is a wonderful thing. I'm not filtering any
: out, just posting what I find by GOOGLING for you.
:
: http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
:
:
: Wow, a gov link. Even the government is wrong, this must be a conspiracy
: against Boomer.
:
:
:
:
: "Boomer" > wrote in message
: ...
: > Now I am getting bored
: >
: > "Don't the components of a buffer account for the buffering capacity?
: Yes."
: >
: > Yes, agreed but you seem to fail what I'm saying. Buffering Capacity and
: Alkalinity are
: > not the same, that has always been the issue. I gave the equation does
: that look like an
: > Alkalinity equation or how Alk is determined. I see you had now comments
: on it what's
: > wrong, why no comments on the equations I gave. Don't understand them or
: what ? Again this
: > is the equation for Buffering Capacity, also called Buffer Index or Buffer
: Intensity. It
: > is defined in most water chemistry and chemical oceanography text books.
: >
: > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
: [H3O+] / (Ka =
: > H3O+])² )
: >
: > This is not Alkalinity now is it ?
: >
: > "I know how to do a titration, In fact I have done several. How many have
: > you actually done? I don't mean by counting drops, I mean with a buret?"
: >
: > Well good for you, I use a Digital Titrator
: >
: > "Oh, I see,
: > you think acidity is the opposite of alkalinity. In the world of
: CHEMISTRY
: > it's not. Maybe in aquarium newsgroups it is.
: >
: > Hum no, maybe you should go for a look at HACH's or LaMotte website or the
: book I
: > suggested earlier. Please view a copy.
: >
: > Standard Methods for the Examination of Water and Wastewater
: >
: > This book, over 2000 pages, is the guide for water testing. If you are
: reporting water
: > test to the EPA you must use approved std from this text.I t is prepared
: and published by
: > the EPA, American Water Works Association and American Public Health
: Association. You
: > mean you don't have one and the issue is water chemistry
: >
: > You are confusing Acidity and Acidity as you know little about water
: chemistry and
: > procedures and test methods
: >
: > From SMEWW, section 2-30, 2310 ACIDITY
: >
: > "Acidity of water is its quantative capacity to react with a strong base
: to a designated
: > pH"
: >
: > This is how you test for it
: >
: > A std alkali titration to methyl orange or phenolphthalein
: > endpoint.
: >
: > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write this
: book, there are
: > over 100 of them, they are wrong.
: >
: > Like Buffering Capacity you have your Acidity's mixed up
: > In water measurement if you have a high Alk you also usually have a high
: Acidity.
: > Normally a high Alk also gives a higher CO2 level. Get a WATER CHEMISTRY
: BOOK there pal.
: >
: >
: > "These are all in equilibrium with each other. An initial high pH (above
: > 6.4) will shift the equilibrium to the right to form HCO3-1. If the pH of
: > the solution is above 10.3 (pKa2) the .........."
: >
: >
: > Christ, there you go again with the FW ****. All your numbers are wrong we
: are dealing
: > with SEAWATER
: >
: > This means that at a pH of 8.3, the majority of the CO2(aq) is in the form
: > of HCO3-1 .
: >
: > I have already pointed that out and gave actual values at know seawater
: levels, go back
: > and re-read it you aren't telling me anything here.Of course most is HCO3
: see...
: >
: >
: > @ 20C and 34.3 ppt salinity
: >
: > CO2 = 0.52 %
: >
: > HCO3 = 86.4 %
: >
: > CO3 = 13.09 %
: >
: >
: > "In your glass experiment you managed to lower the pH enough to purge out
: CO2
: > by boiling"
: >
: > The purpose behind the glass is to show that alk is not affect by CO2 and
: vise-versa and
: > how Co2 affects pH.
: >
: > Now, in a real life seawater aquarium, with a pH of 8.3 and that pH drops
: to say 8.1 it is
: > usually due to excess CO2. If you took a glass of that water and aerated
: it you WILL drive
: > off the CO2 and raise the pH. It has been done a proven a million times.
: >
: > "In order to 'purge' CO2 you would need to lower the
: > pH to shift the equilibrium to below 6.4"
: >
: > The hell you do !!!.Do you know who many times people on this NG to
: include Dr. Craig
: > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
: sample of aquarium
: > water and aerate it to see if the pH GOES UP AND when they come back with
: the test it is
: > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST excess
: CO2 in the tank
: > water, increase the circulation for better gas exchange at the surface,
: reduce feeding,
: > and try to improve on better skimming, thus reducing the bio-load and pH
: decline due to
: > CO2.
: >
: >
: > "I hope this helps. "
: >
: > Help, how can you when you miss everything. I should be charging you
: >
: > Oh, by the way. Your websites, I have about 50 on these issues, I could
: post them, not to
: > mention I have all those water chemistry books, so there is no need to
: view your sites.
: >
: > Finally are you afraid to come to our Chemistry Forum, afraid to get
: slapped by REAL
: > chemists. I get a charge out of you can't post your ref .I have posted the
: same or similar
: > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500 posts
: there and am the
: > biggest contributor to his forum other than himself or maybe Habib Sheka
: >
: > Hum, here are Randy's ref that he posted. He hosts the website
: >
: > S. RANDY HOLMES-FARLEY
: > Arlington, Massachusetts
: >
: > EDUCATION
: >
: > 1982-1986 Harvard University Cambridge, MA
: > PhD in Chemistry
: > Research Advisor: George Whitesides
: >
: > Investigated the relationship between polymer surface chemistry and
: physical properties
: > through controlled surface modification and testing.
: >
: > 1980-1982 Cornell University Ithaca, NY
: > BA in Chemistry and Biology
: > Graduated Summa Cum Laude
: > Distinction in All Subjects
: > Grade Point: 3.94/4.0
: > Honors research: isolation and characterization of the subunit of CF1
: enzyme
: >
: >
: > 1978-1979 Stanford University Palo Alto, CA
: > Grade Point: 3.55/4.0
: >
: >
: > EXPERIENCE
: >
: > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
: > (bought out GelTex Pharmaceuticals in 2001)
: > Vice President, Chemical Research 2001-present
: > Senior Director, Chemical Research 1999-2001
: > Director of Chemical Research 1997-1999
: > Manager of Chemical Research 1995-1997
: > Group Leader 1994-1995
: > Senior Research Scientist 1992-1994
: >
: > Helped start GelTex as second employee
: >
: > Managed various research programs with multi-million dollar budgets
: >
: > Supervised research chemists (17+)
: >
: > Co-inventor of several polymeric pharmaceuticals and pharmaceutical
: candidates including
: > Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride (FDA
: approved)
: >
: > Company Safety Officer for 3 years
: >
: > Chemical Hygiene Officer 2000-present
: >
: >
: >
: >
: > 1990-1992 GTE Corporation Waltham, MA
: > Senior Member of Technical Staff
: > Applied research involving polymer interfaces
: > Metallization of plastics
: > Polymer/polymer adhesion
: > Optical coatings
: >
: >
: >
: > 1986-1990 Lord Corporation Cary, NC
: > Senior Research Scientist 1988-1990
: > Research Scientist 1986-1988
: > Basic and applied research on surface chemical bonding
: > Developed new adhesive compositions
: > Developed new sol-gel coatings for corrosion resistance
: >
: >
: > HONORS AND AWARDS
: >
: > Industrial Innovations Award by Northeast Region of American Chemical
: Society (6/2001)
: >
: > National Kidney Foundation of Northern California Honoree (5/2001)
: >
: > American Chemical Society/Polymer Chemistry Division Industrial Sponsors
: > Award (8/2000)
: >
: > R&D 100 Award from R&D magazine (1999)
: >
: > Sherwin Williams Award in applied polymer science (9/85)
: >
: > IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
: >
: > Award for highest GPA in Chemistry Department (6/82)
: >
: > Summa Cum Laude Honors in Chemistry (6/82)
: >
: > Phi Lamda Epsilon (6/82)
: >
: > Phi Beta Kappa (2/82)
: >
: > Cornell University Dean's List (1981, 1982)
: >
: > Harvard Book Club Award for highest GPA senior year (1978)
: >
: > First Place in western NY ACS high school chemistry exam (1977)
: >
: > 1978-1979
: >
: >
: > __________________
: > Randy Holmes-Farley
: > Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
: >
: > Hobby Experience: 8 years with reefs
: > Current Tanks: 90 gal mixed reef
: > Interests: Reefkeeping, science, photography
: >
: >
: > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
: >
: > Open this post in a new window | Report this post to a moderator | IP:
: Logged
: >
: >
: >
: > 06/27/2003 02:44 PM
: >
: > Randy Holmes-Farley
: > Chemistry Moderator
: >
: > Registered: Apr 2001
: > Location: Arlington, Massachusetts
: > Occupation: Chemist (Drug Discovery at Genzyme)
: > Posts: 15282
: >
: >
: >
: > Publications
: >
: >
: > ISSUED UNITED STATES PATENTS
: >
: >
: > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
: Mandeville, III; W. Harry.
: > US 6,566,407; 5/20/2003
: >
: > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen Randall;
: Huval, Chad
: > Cori.
: > U.S. 6,517,825; 2/11/2003.
: >
: > 3. Method of making phosphate-binding polymers for oral administration.
: Holmes-Farley,
: > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
: 6,509,013; 1/21/2003.
: >
: > 4. Combination therapy for treating hypercholesterolemia using a bile acid
: sequestrant
: > polymer
: > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley, Stephen
: Randall;
: > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
: >
: > 5. Method for treating hypercholesterolemia with polyallylamine polymers.
: Holmes-Farley,
: > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.; Goldberg,
: Dennis I. , US
: > 6,423,754; 7/23/2002.
: >
: > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
: Neenan, Thomas X..;
: > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
: >
: > 7. Combination therapy for treating hypercholesterolemia and
: atherosclerosis. Huval, Chad
: > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep K.
: U.S. 6,365,186;
: > 4/2/2002.
: >
: > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.; Mandeville,
: W. H., III;
: > Huval; C.
: > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
: 10/9/2001.
: >
: > 9. Polymers containing guanidinium groups as bile acid sequestrants. Dhal;
: P. K.; Holmes-
: > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
: >
: > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
: III.; US
: > 6,281,252;
: > 8/28/2001.
: >
: > 11. Combination therapy for treating hypercholestrolemia. Huval; C. C.;
: Holmes-Farley; S.
: > R. ;
: > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
: >
: > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
: Holmes-Farley, S.
: > R.; US
: > 6,264,937; 7/24/2001.
: >
: > 13. Method for treating hypercholesterolemia with unsubstituted
: polydiallylamine polymers.
: > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
: 6,248,318;
: > 6/19/2001.
: >
: > 14. Process for removing bile salts from a patient and alkylated
: compositions therefore.
: > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
: >
: > 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S. R.;
: Dhal, P. K.;
: > Petersen,
: > J. S.; US 6,203,785; 3/20/2001.
: >
: > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.; Huval,
: C. C.; US
: > 6,190,649;
: > 2/20/2001.
: >
: > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
: III.; US
: > 6,177,478;
: > 1/23/2001.
: >
: > 18. Water-insoluble noncrosslinked bile acid sequestrants. Holmes-Farley,
: S. R.;
: > Mandeville, W.
: > H., III.; US 6,129,910; 10/10/2000.
: >
: > 19. Method for treating hypercholesterolemia with unsubstituted
: polydiallylamine polymers.
: > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
: 6,083,497;
: > 7/4/2000.
: >
: > 20. Method of making phosphate-binding polymers for oral administration.
: Holmes-Farley, S.
: > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495; 7/4/2000.
: >
: > 21. Process for removing bile salts from a patient and alkylated
: compositions therefore.
: > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678; 5/23/2000.
: >
: > 22. Process for removing bile salts from a patient and compositions
: therefor. Mandeville,
: > W. H.,
: > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
: >
: > 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
: Neenan; T. X.; Holmes-
: > Farley; S. R. US 6,034,129; 3/7/2000.
: >
: > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
: III.; US
: > 5,985,938;
: > 11/16/99.
: >
: > 25. Process for removing bile salts from a patient and compositions
: therefor. Mandeville,
: > W. H.,
: > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
: >
: > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W. H.,
: III.;
: > Holmes-Farley;
: > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
: >
: > 27. Hydrophilic nonamine-containing and amine-containing copolymers and
: their use as bile
: > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US 5,929,184;
: 7/27/99.
: >
: > 28. Interpenetrating polymer networks for sequestration of bile acids.
: Mandeville, W. H.,
: > III.;
: > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
: 7/20/99.
: >
: > 29. Amine polymer sequestrant and method of cholesterol depletion.
: Mandeville, W. H.,
: > III.;
: > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
: >
: > 30. Process for removing bile salts from a patient and compositions
: therefor. Mandeville,
: > W. H.,
: > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
: >
: > 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
: Mandeville, W. H.,
: > III.;
: > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
: >
: > 32. Process for removing bile salts from a patient and compositions
: therefor. Mandeville,
: > W. H.,
: > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
: >
: > 33. Preparation of polymeric sequestrants for bile acid salts. Mandeville,
: W. H., III.;
: > Holmes-
: > Farley, S. R.; US 5,703,188; 12/30/97.
: >
: > 34. Oral administration of iron-binding crosslinked amine polymers.
: Mandeville, W. H.,
: > III.;
: > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
: >
: > 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley, S.
: R.; US 5,693,675;
: > 12/2/97.
: >
: > 36. Method for removing bile salts from a patient with alkylated
: crosslinked amine
: > polymers,
: > and preparation of the polymers. Mandeville, W. H., III.; Holmes-Farley,
: S. R.; US
: > 5,679,717; 10/21/97.
: >
: > 37. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
: R.; Mandeville,
: > W.
: > H., III.; US 5,667,775; 9/16/97.
: >
: > 38. Ion-exchange process using highly crosslinked polymers for removing
: bile salts from a
: > patient, preparation of the polymers, and compositions containing them.
: Mandeville, W. H.,
: > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
: >
: > 39. Hydrophobic amine polymer sequestrant and method of cholesterol
: depletion. Mandeville,
: > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530; 4/8/97.
: >
: > 40. Amine polymer sequestrant and method of cholesterol depletion.
: Mandeville, W. H.,
: > III.;
: > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
: >
: > 41. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
: R.; Mandeville,
: > W.
: > H., III.; US 5,496,545; 3/5/96.
: >
: > 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
: III.; Holmes-Farley,
: > S. R.;
: > US 5,487,888; 1/30/96.
: >
: > 43. Ultra-thin, uniform sol-gel coating of a substrate having active
: hydrogens on the
: > surface.
: > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
: >
: > 44. Layered sol-gel coatings from organisilicon compounds. Holmes-Farley,
: S. R.; Yanyo, L.
: > C.;
: > US 5,182,143; 1/26/93.
: >
: > 45. Method for metal bonding using ultrathin primer coating.
: Holmes-Farley, S. R.; Yanyo,
: > L.
: > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
: >
: > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.; US
: 5,096,962;
: > 3/17/92.
: >
: > 47. Modified halogenatedpolyolefin adhesives for polyolefin
: elastomer-metal bonding.
: > Holmes-
: > Farley, S. R.; US 5,102,956; 4/7/92.
: >
: >
: >
: > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
: >
: >
: > 1. Aryl boronate functionalized polymers for treating obesity and
: inhibiting fat uptake.
: > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal, Pradeep
: K.; Huval, Chad
: > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92 pp. WO
: 0302571.
: >
: > 2. Preparation of aryl boronic acids for treating obesity. Holmes-Farley,
: Stephen Randall;
: > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep K.
: (Geltex
: > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
: >
: > 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
: Stephen Randall.
: > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
: 0302130.
: >
: > 4. Method for reducing copper levels and treating copper toxicosis.
: Holmes-Farley, Stephen
: > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002), 45
: pp. WO
: > 0285383.
: >
: > 5. Method for treating gout and binding uric acid. Holmes-Farley, Stephen
: Randall; Burke,
: > Steven K. WO 0285381 10/31/2002.
: >
: > 6. Method for treating gout and reducing serum uric acid. Holmes-Farley,
: Stephen Randall;
: > Burke, Steven K WO 0285380 10/31/2002.
: >
: > 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
: Holmes-Farley, S. R.;
: > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
: >
: > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
: Holmes-Farley, S.
: > R.;
: > WO 1999-US5662; 9/23/1999.
: >
: > 9. Amine-containing copolymers as bile acid sequestrants. Holmes-Farley,
: S. R.; Petersen,
: > J. S.;
: > WO 9933452; 7/8/1999.
: >
: > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III and
: Holmes-Farley, S.
: > R.;
: > WO 9922743; 5/14/1999.
: >
: > 11. Polyallylamine polymers for removing bile salts and treating
: hypercholesterolemia, and
: > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III; Burke,
: S. K.; Goldberg,
: > D. I.; WO 9857652; 12/23/98.
: >
: > 12. Phosphate-bidning polymers combined with a calcium supplement for oral
: administration.
: > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley, S.
: R.; WO 9842355;
: > 10/1/98.
: >
: > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
: depletion. Mandeville,
: > W.
: > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
: >
: > 14. Process for adjusting ion concentration in a patient and compositions
: therefor.
: > Mandeville,
: > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
: >
: > 15. Vacuum-deposited silver on polycarbonate with a chromium interlayer
: for improved
: > metal-
: > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512; 1/20/94.
: >
: > 16. Process for increased metal-substrate bond strength in metalized
: plastics.
: > Holmes-Farley, S.
: > R.; Ger. Offen. 4322516; 7/6/93.
: >
: > 17. Electrorheological fluids and preparation of particles useful in the
: fluids.
: > Troughton,
: > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
: David; Bares, Joseph
: > E.;
: > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
: 394049;
: > 10/24/1990.
: >
: > JOURNAL PUBLICATIONS
: >
: > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov, Eugene;
: Guo, Amy;
: > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
: Mandeville, W. Harry;
: > Holmes-Farley, S. Randall. Kidney International (2002), 62(2), 611-619.
: >
: > 2. Amine functionalized polyethers as bile acid sequestrants: synthesis
: and biological
: > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S. Randall;
: Mandeville, W.
: > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
: Journal of
: > Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
: 1559-1574.
: >
: > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
: Imprinting. Huval,
: > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
: Randall; Mandeville,
: > W.
: > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert J.;
: Chen, Xi; Dhal,
: > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
: >
: > 4. Synthetic polymers for the binding of fat in the intestinal tract.
: Jozefiak, Thomas H.;
: > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia; Huval,
: Chad C.;
: > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
: Abstracts of
: > Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
: 26-30, 2001
: > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
: Division of
: > Polymer Chemistry) (2001), 42(2), 98.
: >
: > 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer gel
: pharmaceutical.
: > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.; Ward,
: J.; Sacchiero,
: > B.;
: > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.; Chen,
: X.; Mazzeo, J.
: > R.. Polym. Preprints (2000), 41(1), 735-736.
: >
: > 6. In vitro comparison of bile acid binding to colesevelam HCl and other
: bile acid
: > sequestrants.
: > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
: Hook, P.; Holmes-
: > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
: >
: > 7. Novel polymeric pharmaceuticals: From startup to market. Holmes-Farley,
: S. R; Polym.
: > Mater. Sci. Eng (1999), 80, 246-247.
: >
: > 8. Design and characterization of of Sevelamer Hydrochloride: a novel
: phosphate-binding
: > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward, J.;
: Miller, K. L.;
: > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure and
: Appl. Chem.,
: > A36(7&8), p. 1085 (1999).
: >
: > 9. Three generations of bile acid sequestrants. Mandeville, W. H., III;
: Braunlin, W.;
: > Dhal, P.;
: > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
: Rosenbaum, D.;
: > Sacchiero,
: > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
: 550, 3-15.
: >
: > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric phosphate
: binder, on
: > urinary
: > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
: Mandeville, W. H.,
: > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
: (1997), 12(5)
: > 961-964.
: >
: > 11. Thin anisotropic coatings based on sol-gel technology. Holmes-Farley,
: S. R.; Yanyo, L.
: > C;
: > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4), 439-444.
: >
: > 12. The mechanism of cure initiation of a surface activated adhesive.
: Holmes-Farley, S.
: > R.;
: > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
: >
: > 13. Adhesion promotion and corrosion prevention using thin anisotropic
: coatings. Holmes-
: > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
: 131-151.
: >
: > 14. Wetting of functionalized polyethylene having ionizable organic acids
: and bases at the
: > polymer-water interface: relations between functional group polarity,
: extent of
: > ionization,
: > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
: Whitesides, G. M.;
: > Langmuir
: > (1988), 4(4), 921-937.
: >
: > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
: single hydroxy group.
: > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
: >
: > 16. Reconstruction of the interface of oxidatively functionalized
: polyethylene (PE-CO2H)
: > and
: > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo, R.;
: McCarthy, T. J.;
: > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report (1987),
: AD-
: > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
: >
: > 17. Surface-modified polyethylene film: the relationship between surface
: chemistry and
: > physical
: > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11), 4537.
: >
: > 18. Reactivity of carboxylic acid and ester groups in the functionalized
: interfacial
: > region of
: > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
: differentiation of the
: > functional groups into shallow and deep subsets based on a comparison of
: contact angle and
: > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
: (1987), 3(1), 62-
: > 76.
: >
: > 19. Fluorescence properties of dansyl groups covalently bonded tot he
: surface of
: > oxidatively
: > functionalized low-density polyethylene film. Holmes-Farley, S. R.;
: Whitesides, G. M.;
: > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
: AD-A162435/2/GAR,
: > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
: >
: > 20. Acid-base behavior of carboxylic acid groups covalently attached at
: the surface of
: > polyethylene: The usefulness of contact angle in following the ionization
: of surface
: > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
: Deutch, J.;
: > Whitesides,
: > G. M.; Langmuir (1985), 1(6), 725-740.
: >
: > 21. The thermal stability of a surface modified solid organic polymer.
: Holmes-Farley, S.
: > R.;
: > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
: >
: >
: >
: > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
: >
: > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
: Aquarist. June 2003.
: >
: > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
: Advanced Aquarist.
: > May
: > 2003.
: >
: > 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
: Reefkeeping May
: > 2003.
: >
: > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
: April 2003.
: >
: > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
: Holmes-Farley, R.
: > Advanced Aquarist; April 2003.
: >
: > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
: Holmes-Farley, R.
: > Advanced Aquarist; April 2003.
: >
: > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced Aquarist;
: March 2003.
: >
: > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
: Holmes-Farley, R.
: > Advanced Aquarist; February 2003.
: >
: > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
: 2003.
: >
: > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; December
: 2002.
: >
: > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R. Advanced
: Aquarist; November
: > 2002.
: >
: > 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
: Advanced Aquarist;
: > November 2002.
: >
: > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced Aquarist,
: September 2002.
: >
: > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
: 2002.
: >
: > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
: 2002.
: >
: > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
: Aquarist; July 2002
: >
: > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist; June
: 2002.
: >
: > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R. Advanced
: Aquarist, May
: > 2002.
: >
: > 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
: Holmes-Farley, R.
: > Advanced Aquarist, April 2002.
: >
: > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
: >
: > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
: >
: > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January 2002.
: >
: > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
: 2000.
: >
: > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
: Frontiers 2000.
: >
: > 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
: Aquarium Frontiers
: > 2000.
: > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium Frontiers
: 2000.
: >
: > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers 2000.
: >
: > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
: >
: > 29. Protein Skimming: How it Works. Fishnet Library 1998.
: >
: >
: >
: >
: >
: >
: >
: > Boomer
: >
: > Want to talk chemistry ? The Reef Chemistry Forum
: > http://www.reefcentral.com/vbulletin/index.php
: >
: > Want to See More ?
: > Please Join Our Growing Membership
: > www.coralrealm.com
: >
: >
: >
:
:

[Dragon Slayer]

"Boomer" > wrote in message
...


> Do a dam search on them or shut the hell up.

I'll second that.

kc

[Boomer]

Dam, how did I forget my favorite book

Carbon Dioxide Equilibrium and Their Applications by J.N. Butler (professor emeritus
Harvard University)


You should really look for a copy of this master piece. Page 67 has a pC/pH diagram of
BC's for FW. He also gives the long mathematically expression of Alkalinity. His review of
Acidity is rather short though but long on Alk. 5 pages of BC
--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
www.coralrealm.com

If You See Me Running You Better Catch-Up
"Boomer" > wrote in message
...
: Alkalinity a measure of the amount of anions of weak acid in water and of the cations
: balanced against them
: Take note it says ***acid***
:
: Buffering capacity the ability of a solution to resist or dampen changes in pH upon the
: addition of acids or bases.
: Take note its says ***the addition of acids or bases***
:
: One more
:
: http://www.waterontheweb.org/resources/glossary.html
:
: We could go on like this all day, so what is the point ?
:
: You will LOVE this one
: http://www.kyantec.com/Tips/phbuffering.htm
:
: Don't you just lovbe PDF's
: http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
:
: Don't fall out of your chair
: http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
:
:
:
:
: --
: Boomer
:
: Want to talk chemistry ? The Reef Chemistry Forum
: http://www.reefcentral.com/vbulletin/index.php
:
: Want to See More ?
: Please Join Our Growing Membership
: www.coralrealm.com
:
: If You See Me Running You Better Catch-Up
: "stoutman" <.@.> wrote in message news:XB7Wb.19339$QA2.62332@attbi_s52...
: : Man here is another, google is a wonderful thing. I'm not filtering any
: : out, just posting what I find by GOOGLING for you.
: :
: : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
: :
: :
: : Wow, a gov link. Even the government is wrong, this must be a conspiracy
: : against Boomer.
: :
: :
: :
: :
: : "Boomer" > wrote in message
: : ...
: : > Now I am getting bored
: : >
: : > "Don't the components of a buffer account for the buffering capacity?
: : Yes."
: : >
: : > Yes, agreed but you seem to fail what I'm saying. Buffering Capacity and
: : Alkalinity are
: : > not the same, that has always been the issue. I gave the equation does
: : that look like an
: : > Alkalinity equation or how Alk is determined. I see you had now comments
: : on it what's
: : > wrong, why no comments on the equations I gave. Don't understand them or
: : what ? Again this
: : > is the equation for Buffering Capacity, also called Buffer Index or Buffer
: : Intensity. It
: : > is defined in most water chemistry and chemical oceanography text books.
: : >
: : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
: : [H3O+] / (Ka =
: : > H3O+])² )
: : >
: : > This is not Alkalinity now is it ?
: : >
: : > "I know how to do a titration, In fact I have done several. How many have
: : > you actually done? I don't mean by counting drops, I mean with a buret?"
: : >
: : > Well good for you, I use a Digital Titrator
: : >
: : > "Oh, I see,
: : > you think acidity is the opposite of alkalinity. In the world of
: : CHEMISTRY
: : > it's not. Maybe in aquarium newsgroups it is.
: : >
: : > Hum no, maybe you should go for a look at HACH's or LaMotte website or the
: : book I
: : > suggested earlier. Please view a copy.
: : >
: : > Standard Methods for the Examination of Water and Wastewater
: : >
: : > This book, over 2000 pages, is the guide for water testing. If you are
: : reporting water
: : > test to the EPA you must use approved std from this text.I t is prepared
: : and published by
: : > the EPA, American Water Works Association and American Public Health
: : Association. You
: : > mean you don't have one and the issue is water chemistry
: : >
: : > You are confusing Acidity and Acidity as you know little about water
: : chemistry and
: : > procedures and test methods
: : >
: : > From SMEWW, section 2-30, 2310 ACIDITY
: : >
: : > "Acidity of water is its quantative capacity to react with a strong base
: : to a designated
: : > pH"
: : >
: : > This is how you test for it
: : >
: : > A std alkali titration to methyl orange or phenolphthalein
: : > endpoint.
: : >
: : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write this
: : book, there are
: : > over 100 of them, they are wrong.
: : >
: : > Like Buffering Capacity you have your Acidity's mixed up
: : > In water measurement if you have a high Alk you also usually have a high
: : Acidity.
: : > Normally a high Alk also gives a higher CO2 level. Get a WATER CHEMISTRY
: : BOOK there pal.
: : >
: : >
: : > "These are all in equilibrium with each other. An initial high pH (above
: : > 6.4) will shift the equilibrium to the right to form HCO3-1. If the pH of
: : > the solution is above 10.3 (pKa2) the .........."
: : >
: : >
: : > Christ, there you go again with the FW ****. All your numbers are wrong we
: : are dealing
: : > with SEAWATER
: : >
: : > This means that at a pH of 8.3, the majority of the CO2(aq) is in the form
: : > of HCO3-1 .
: : >
: : > I have already pointed that out and gave actual values at know seawater
: : levels, go back
: : > and re-read it you aren't telling me anything here.Of course most is HCO3
: : see...
: : >
: : >
: : > @ 20C and 34.3 ppt salinity
: : >
: : > CO2 = 0.52 %
: : >
: : > HCO3 = 86.4 %
: : >
: : > CO3 = 13.09 %
: : >
: : >
: : > "In your glass experiment you managed to lower the pH enough to purge out
: : CO2
: : > by boiling"
: : >
: : > The purpose behind the glass is to show that alk is not affect by CO2 and
: : vise-versa and
: : > how Co2 affects pH.
: : >
: : > Now, in a real life seawater aquarium, with a pH of 8.3 and that pH drops
: : to say 8.1 it is
: : > usually due to excess CO2. If you took a glass of that water and aerated
: : it you WILL drive
: : > off the CO2 and raise the pH. It has been done a proven a million times.
: : >
: : > "In order to 'purge' CO2 you would need to lower the
: : > pH to shift the equilibrium to below 6.4"
: : >
: : > The hell you do !!!.Do you know who many times people on this NG to
: : include Dr. Craig
: : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
: : sample of aquarium
: : > water and aerate it to see if the pH GOES UP AND when they come back with
: : the test it is
: : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST excess
: : CO2 in the tank
: : > water, increase the circulation for better gas exchange at the surface,
: : reduce feeding,
: : > and try to improve on better skimming, thus reducing the bio-load and pH
: : decline due to
: : > CO2.
: : >
: : >
: : > "I hope this helps. "
: : >
: : > Help, how can you when you miss everything. I should be charging you
: : >
: : > Oh, by the way. Your websites, I have about 50 on these issues, I could
: : post them, not to
: : > mention I have all those water chemistry books, so there is no need to
: : view your sites.
: : >
: : > Finally are you afraid to come to our Chemistry Forum, afraid to get
: : slapped by REAL
: : > chemists. I get a charge out of you can't post your ref .I have posted the
: : same or similar
: : > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500 posts
: : there and am the
: : > biggest contributor to his forum other than himself or maybe Habib Sheka
: : >
: : > Hum, here are Randy's ref that he posted. He hosts the website
: : >
: : > S. RANDY HOLMES-FARLEY
: : > Arlington, Massachusetts
: : >
: : > EDUCATION
: : >
: : > 1982-1986 Harvard University Cambridge, MA
: : > PhD in Chemistry
: : > Research Advisor: George Whitesides
: : >
: : > Investigated the relationship between polymer surface chemistry and
: : physical properties
: : > through controlled surface modification and testing.
: : >
: : > 1980-1982 Cornell University Ithaca, NY
: : > BA in Chemistry and Biology
: : > Graduated Summa Cum Laude
: : > Distinction in All Subjects
: : > Grade Point: 3.94/4.0
: : > Honors research: isolation and characterization of the subunit of CF1
: : enzyme
: : >
: : >
: : > 1978-1979 Stanford University Palo Alto, CA
: : > Grade Point: 3.55/4.0
: : >
: : >
: : > EXPERIENCE
: : >
: : > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
: : > (bought out GelTex Pharmaceuticals in 2001)
: : > Vice President, Chemical Research 2001-present
: : > Senior Director, Chemical Research 1999-2001
: : > Director of Chemical Research 1997-1999
: : > Manager of Chemical Research 1995-1997
: : > Group Leader 1994-1995
: : > Senior Research Scientist 1992-1994
: : >
: : > Helped start GelTex as second employee
: : >
: : > Managed various research programs with multi-million dollar budgets
: : >
: : > Supervised research chemists (17+)
: : >
: : > Co-inventor of several polymeric pharmaceuticals and pharmaceutical
: : candidates including
: : > Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride (FDA
: : approved)
: : >
: : > Company Safety Officer for 3 years
: : >
: : > Chemical Hygiene Officer 2000-present
: : >
: : >
: : >
: : >
: : > 1990-1992 GTE Corporation Waltham, MA
: : > Senior Member of Technical Staff
: : > Applied research involving polymer interfaces
: : > Metallization of plastics
: : > Polymer/polymer adhesion
: : > Optical coatings
: : >
: : >
: : >
: : > 1986-1990 Lord Corporation Cary, NC
: : > Senior Research Scientist 1988-1990
: : > Research Scientist 1986-1988
: : > Basic and applied research on surface chemical bonding
: : > Developed new adhesive compositions
: : > Developed new sol-gel coatings for corrosion resistance
: : >
: : >
: : > HONORS AND AWARDS
: : >
: : > Industrial Innovations Award by Northeast Region of American Chemical
: : Society (6/2001)
: : >
: : > National Kidney Foundation of Northern California Honoree (5/2001)
: : >
: : > American Chemical Society/Polymer Chemistry Division Industrial Sponsors
: : > Award (8/2000)
: : >
: : > R&D 100 Award from R&D magazine (1999)
: : >
: : > Sherwin Williams Award in applied polymer science (9/85)
: : >
: : > IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
: : >
: : > Award for highest GPA in Chemistry Department (6/82)
: : >
: : > Summa Cum Laude Honors in Chemistry (6/82)
: : >
: : > Phi Lamda Epsilon (6/82)
: : >
: : > Phi Beta Kappa (2/82)
: : >
: : > Cornell University Dean's List (1981, 1982)
: : >
: : > Harvard Book Club Award for highest GPA senior year (1978)
: : >
: : > First Place in western NY ACS high school chemistry exam (1977)
: : >
: : > 1978-1979
: : >
: : >
: : > __________________
: : > Randy Holmes-Farley
: : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
: : >
: : > Hobby Experience: 8 years with reefs
: : > Current Tanks: 90 gal mixed reef
: : > Interests: Reefkeeping, science, photography
: : >
: : >
: : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
: : >
: : > Open this post in a new window | Report this post to a moderator | IP:
: : Logged
: : >
: : >
: : >
: : > 06/27/2003 02:44 PM
: : >
: : > Randy Holmes-Farley
: : > Chemistry Moderator
: : >
: : > Registered: Apr 2001
: : > Location: Arlington, Massachusetts
: : > Occupation: Chemist (Drug Discovery at Genzyme)
: : > Posts: 15282
: : >
: : >
: : >
: : > Publications
: : >
: : >
: : > ISSUED UNITED STATES PATENTS
: : >
: : >
: : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
: : Mandeville, III; W. Harry.
: : > US 6,566,407; 5/20/2003
: : >
: : > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen Randall;
: : Huval, Chad
: : > Cori.
: : > U.S. 6,517,825; 2/11/2003.
: : >
: : > 3. Method of making phosphate-binding polymers for oral administration.
: : Holmes-Farley,
: : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
: : 6,509,013; 1/21/2003.
: : >
: : > 4. Combination therapy for treating hypercholesterolemia using a bile acid
: : sequestrant
: : > polymer
: : > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley, Stephen
: : Randall;
: : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
: : >
: : > 5. Method for treating hypercholesterolemia with polyallylamine polymers.
: : Holmes-Farley,
: : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.; Goldberg,
: : Dennis I. , US
: : > 6,423,754; 7/23/2002.
: : >
: : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
: : Neenan, Thomas X..;
: : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
: : >
: : > 7. Combination therapy for treating hypercholesterolemia and
: : atherosclerosis. Huval, Chad
: : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep K.
: : U.S. 6,365,186;
: : > 4/2/2002.
: : >
: : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.; Mandeville,
: : W. H., III;
: : > Huval; C.
: : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
: : 10/9/2001.
: : >
: : > 9. Polymers containing guanidinium groups as bile acid sequestrants. Dhal;
: : P. K.; Holmes-
: : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
: : >
: : > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
: : III.; US
: : > 6,281,252;
: : > 8/28/2001.
: : >
: : > 11. Combination therapy for treating hypercholestrolemia. Huval; C. C.;
: : Holmes-Farley; S.
: : > R. ;
: : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
: : >
: : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
: : Holmes-Farley, S.
: : > R.; US
: : > 6,264,937; 7/24/2001.
: : >
: : > 13. Method for treating hypercholesterolemia with unsubstituted
: : polydiallylamine polymers.
: : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
: : 6,248,318;
: : > 6/19/2001.
: : >
: : > 14. Process for removing bile salts from a patient and alkylated
: : compositions therefore.
: : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
: : >
: : > 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S. R.;
: : Dhal, P. K.;
: : > Petersen,
: : > J. S.; US 6,203,785; 3/20/2001.
: : >
: : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.; Huval,
: : C. C.; US
: : > 6,190,649;
: : > 2/20/2001.
: : >
: : > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
: : III.; US
: : > 6,177,478;
: : > 1/23/2001.
: : >
: : > 18. Water-insoluble noncrosslinked bile acid sequestrants. Holmes-Farley,
: : S. R.;
: : > Mandeville, W.
: : > H., III.; US 6,129,910; 10/10/2000.
: : >
: : > 19. Method for treating hypercholesterolemia with unsubstituted
: : polydiallylamine polymers.
: : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
: : 6,083,497;
: : > 7/4/2000.
: : >
: : > 20. Method of making phosphate-binding polymers for oral administration.
: : Holmes-Farley, S.
: : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495; 7/4/2000.
: : >
: : > 21. Process for removing bile salts from a patient and alkylated
: : compositions therefore.
: : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678; 5/23/2000.
: : >
: : > 22. Process for removing bile salts from a patient and compositions
: : therefor. Mandeville,
: : > W. H.,
: : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
: : >
: : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
: : Neenan; T. X.; Holmes-
: : > Farley; S. R. US 6,034,129; 3/7/2000.
: : >
: : > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W. H.,
: : III.; US
: : > 5,985,938;
: : > 11/16/99.
: : >
: : > 25. Process for removing bile salts from a patient and compositions
: : therefor. Mandeville,
: : > W. H.,
: : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
: : >
: : > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W. H.,
: : III.;
: : > Holmes-Farley;
: : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
: : >
: : > 27. Hydrophilic nonamine-containing and amine-containing copolymers and
: : their use as bile
: : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US 5,929,184;
: : 7/27/99.
: : >
: : > 28. Interpenetrating polymer networks for sequestration of bile acids.
: : Mandeville, W. H.,
: : > III.;
: : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
: : 7/20/99.
: : >
: : > 29. Amine polymer sequestrant and method of cholesterol depletion.
: : Mandeville, W. H.,
: : > III.;
: : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
: : >
: : > 30. Process for removing bile salts from a patient and compositions
: : therefor. Mandeville,
: : > W. H.,
: : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
: : >
: : > 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
: : Mandeville, W. H.,
: : > III.;
: : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
: : >
: : > 32. Process for removing bile salts from a patient and compositions
: : therefor. Mandeville,
: : > W. H.,
: : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
: : >
: : > 33. Preparation of polymeric sequestrants for bile acid salts. Mandeville,
: : W. H., III.;
: : > Holmes-
: : > Farley, S. R.; US 5,703,188; 12/30/97.
: : >
: : > 34. Oral administration of iron-binding crosslinked amine polymers.
: : Mandeville, W. H.,
: : > III.;
: : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
: : >
: : > 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley, S.
: : R.; US 5,693,675;
: : > 12/2/97.
: : >
: : > 36. Method for removing bile salts from a patient with alkylated
: : crosslinked amine
: : > polymers,
: : > and preparation of the polymers. Mandeville, W. H., III.; Holmes-Farley,
: : S. R.; US
: : > 5,679,717; 10/21/97.
: : >
: : > 37. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
: : R.; Mandeville,
: : > W.
: : > H., III.; US 5,667,775; 9/16/97.
: : >
: : > 38. Ion-exchange process using highly crosslinked polymers for removing
: : bile salts from a
: : > patient, preparation of the polymers, and compositions containing them.
: : Mandeville, W. H.,
: : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
: : >
: : > 39. Hydrophobic amine polymer sequestrant and method of cholesterol
: : depletion. Mandeville,
: : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530; 4/8/97.
: : >
: : > 40. Amine polymer sequestrant and method of cholesterol depletion.
: : Mandeville, W. H.,
: : > III.;
: : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
: : >
: : > 41. Phosphate-binding polymers for oral administration. Holmes-Farley, S.
: : R.; Mandeville,
: : > W.
: : > H., III.; US 5,496,545; 3/5/96.
: : >
: : > 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
: : III.; Holmes-Farley,
: : > S. R.;
: : > US 5,487,888; 1/30/96.
: : >
: : > 43. Ultra-thin, uniform sol-gel coating of a substrate having active
: : hydrogens on the
: : > surface.
: : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
: : >
: : > 44. Layered sol-gel coatings from organisilicon compounds. Holmes-Farley,
: : S. R.; Yanyo, L.
: : > C.;
: : > US 5,182,143; 1/26/93.
: : >
: : > 45. Method for metal bonding using ultrathin primer coating.
: : Holmes-Farley, S. R.; Yanyo,
: : > L.
: : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
: : >
: : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.; US
: : 5,096,962;
: : > 3/17/92.
: : >
: : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
: : elastomer-metal bonding.
: : > Holmes-
: : > Farley, S. R.; US 5,102,956; 4/7/92.
: : >
: : >
: : >
: : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
: : >
: : >
: : > 1. Aryl boronate functionalized polymers for treating obesity and
: : inhibiting fat uptake.
: : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal, Pradeep
: : K.; Huval, Chad
: : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92 pp. WO
: : 0302571.
: : >
: : > 2. Preparation of aryl boronic acids for treating obesity. Holmes-Farley,
: : Stephen Randall;
: : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep K.
: : (Geltex
: : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
: : >
: : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
: : Stephen Randall.
: : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
: : 0302130.
: : >
: : > 4. Method for reducing copper levels and treating copper toxicosis.
: : Holmes-Farley, Stephen
: : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002), 45
: : pp. WO
: : > 0285383.
: : >
: : > 5. Method for treating gout and binding uric acid. Holmes-Farley, Stephen
: : Randall; Burke,
: : > Steven K. WO 0285381 10/31/2002.
: : >
: : > 6. Method for treating gout and reducing serum uric acid. Holmes-Farley,
: : Stephen Randall;
: : > Burke, Steven K WO 0285380 10/31/2002.
: : >
: : > 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
: : Holmes-Farley, S. R.;
: : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
: : >
: : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
: : Holmes-Farley, S.
: : > R.;
: : > WO 1999-US5662; 9/23/1999.
: : >
: : > 9. Amine-containing copolymers as bile acid sequestrants. Holmes-Farley,
: : S. R.; Petersen,
: : > J. S.;
: : > WO 9933452; 7/8/1999.
: : >
: : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III and
: : Holmes-Farley, S.
: : > R.;
: : > WO 9922743; 5/14/1999.
: : >
: : > 11. Polyallylamine polymers for removing bile salts and treating
: : hypercholesterolemia, and
: : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III; Burke,
: : S. K.; Goldberg,
: : > D. I.; WO 9857652; 12/23/98.
: : >
: : > 12. Phosphate-bidning polymers combined with a calcium supplement for oral
: : administration.
: : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley, S.
: : R.; WO 9842355;
: : > 10/1/98.
: : >
: : > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
: : depletion. Mandeville,
: : > W.
: : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
: : >
: : > 14. Process for adjusting ion concentration in a patient and compositions
: : therefor.
: : > Mandeville,
: : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
: : >
: : > 15. Vacuum-deposited silver on polycarbonate with a chromium interlayer
: : for improved
: : > metal-
: : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512; 1/20/94.
: : >
: : > 16. Process for increased metal-substrate bond strength in metalized
: : plastics.
: : > Holmes-Farley, S.
: : > R.; Ger. Offen. 4322516; 7/6/93.
: : >
: : > 17. Electrorheological fluids and preparation of particles useful in the
: : fluids.
: : > Troughton,
: : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
: : David; Bares, Joseph
: : > E.;
: : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
: : 394049;
: : > 10/24/1990.
: : >
: : > JOURNAL PUBLICATIONS
: : >
: : > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov, Eugene;
: : Guo, Amy;
: : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
: : Mandeville, W. Harry;
: : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2), 611-619.
: : >
: : > 2. Amine functionalized polyethers as bile acid sequestrants: synthesis
: : and biological
: : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S. Randall;
: : Mandeville, W.
: : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
: : Journal of
: : > Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
: : 1559-1574.
: : >
: : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
: : Imprinting. Huval,
: : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
: : Randall; Mandeville,
: : > W.
: : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert J.;
: : Chen, Xi; Dhal,
: : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
: : >
: : > 4. Synthetic polymers for the binding of fat in the intestinal tract.
: : Jozefiak, Thomas H.;
: : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia; Huval,
: : Chad C.;
: : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
: : Abstracts of
: : > Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
: : 26-30, 2001
: : > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
: : Division of
: : > Polymer Chemistry) (2001), 42(2), 98.
: : >
: : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer gel
: : pharmaceutical.
: : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.; Ward,
: : J.; Sacchiero,
: : > B.;
: : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.; Chen,
: : X.; Mazzeo, J.
: : > R.. Polym. Preprints (2000), 41(1), 735-736.
: : >
: : > 6. In vitro comparison of bile acid binding to colesevelam HCl and other
: : bile acid
: : > sequestrants.
: : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
: : Hook, P.; Holmes-
: : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
: : >
: : > 7. Novel polymeric pharmaceuticals: From startup to market. Holmes-Farley,
: : S. R; Polym.
: : > Mater. Sci. Eng (1999), 80, 246-247.
: : >
: : > 8. Design and characterization of of Sevelamer Hydrochloride: a novel
: : phosphate-binding
: : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward, J.;
: : Miller, K. L.;
: : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure and
: : Appl. Chem.,
: : > A36(7&8), p. 1085 (1999).
: : >
: : > 9. Three generations of bile acid sequestrants. Mandeville, W. H., III;
: : Braunlin, W.;
: : > Dhal, P.;
: : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
: : Rosenbaum, D.;
: : > Sacchiero,
: : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
: : 550, 3-15.
: : >
: : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric phosphate
: : binder, on
: : > urinary
: : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
: : Mandeville, W. H.,
: : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
: : (1997), 12(5)
: : > 961-964.
: : >
: : > 11. Thin anisotropic coatings based on sol-gel technology. Holmes-Farley,
: : S. R.; Yanyo, L.
: : > C;
: : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4), 439-444.
: : >
: : > 12. The mechanism of cure initiation of a surface activated adhesive.
: : Holmes-Farley, S.
: : > R.;
: : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
: : >
: : > 13. Adhesion promotion and corrosion prevention using thin anisotropic
: : coatings. Holmes-
: : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
: : 131-151.
: : >
: : > 14. Wetting of functionalized polyethylene having ionizable organic acids
: : and bases at the
: : > polymer-water interface: relations between functional group polarity,
: : extent of
: : > ionization,
: : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
: : Whitesides, G. M.;
: : > Langmuir
: : > (1988), 4(4), 921-937.
: : >
: : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
: : single hydroxy group.
: : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
: : >
: : > 16. Reconstruction of the interface of oxidatively functionalized
: : polyethylene (PE-CO2H)
: : > and
: : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo, R.;
: : McCarthy, T. J.;
: : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report (1987),
: : AD-
: : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
: : >
: : > 17. Surface-modified polyethylene film: the relationship between surface
: : chemistry and
: : > physical
: : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11), 4537.
: : >
: : > 18. Reactivity of carboxylic acid and ester groups in the functionalized
: : interfacial
: : > region of
: : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
: : differentiation of the
: : > functional groups into shallow and deep subsets based on a comparison of
: : contact angle and
: : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
: : (1987), 3(1), 62-
: : > 76.
: : >
: : > 19. Fluorescence properties of dansyl groups covalently bonded tot he
: : surface of
: : > oxidatively
: : > functionalized low-density polyethylene film. Holmes-Farley, S. R.;
: : Whitesides, G. M.;
: : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
: : AD-A162435/2/GAR,
: : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
: : >
: : > 20. Acid-base behavior of carboxylic acid groups covalently attached at
: : the surface of
: : > polyethylene: The usefulness of contact angle in following the ionization
: : of surface
: : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
: : Deutch, J.;
: : > Whitesides,
: : > G. M.; Langmuir (1985), 1(6), 725-740.
: : >
: : > 21. The thermal stability of a surface modified solid organic polymer.
: : Holmes-Farley, S.
: : > R.;
: : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
: : >
: : >
: : >
: : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
: : >
: : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
: : Aquarist. June 2003.
: : >
: : > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
: : Advanced Aquarist.
: : > May
: : > 2003.
: : >
: : > 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
: : Reefkeeping May
: : > 2003.
: : >
: : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
: : April 2003.
: : >
: : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
: : Holmes-Farley, R.
: : > Advanced Aquarist; April 2003.
: : >
: : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
: : Holmes-Farley, R.
: : > Advanced Aquarist; April 2003.
: : >
: : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced Aquarist;
: : March 2003.
: : >
: : > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
: : Holmes-Farley, R.
: : > Advanced Aquarist; February 2003.
: : >
: : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
: : 2003.
: : >
: : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; December
: : 2002.
: : >
: : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R. Advanced
: : Aquarist; November
: : > 2002.
: : >
: : > 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
: : Advanced Aquarist;
: : > November 2002.
: : >
: : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced Aquarist,
: : September 2002.
: : >
: : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
: : 2002.
: : >
: : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
: : 2002.
: : >
: : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
: : Aquarist; July 2002
: : >
: : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist; June
: : 2002.
: : >
: : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R. Advanced
: : Aquarist, May
: : > 2002.
: : >
: : > 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
: : Holmes-Farley, R.
: : > Advanced Aquarist, April 2002.
: : >
: : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
: : >
: : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
: : >
: : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January 2002.
: : >
: : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
: : 2000.
: : >
: : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
: : Frontiers 2000.
: : >
: : > 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
: : Aquarium Frontiers
: : > 2000.
: : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium Frontiers
: : 2000.
: : >
: : > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers 2000.
: : >
: : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
: : >
: : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
: : >
: : >
: : >
: : >
: : >
: : >
: : >
: : > Boomer
: : >
: : > Want to talk chemistry ? The Reef Chemistry Forum
: : > http://www.reefcentral.com/vbulletin/index.php
: : >
: : > Want to See More ?
: : > Please Join Our Growing Membership
: : > www.coralrealm.com
: : >
: : >
: : >
: :
: :
:
:

[stoutman]

Boomer,

I am not sure if you are just messing with me or if you are truly confused.
I hope the latter. Please read from Top to Bottom.


From YOUR first link:

http://www.waterontheweb.org/resources/glossary.html

Acidity:
A measure of how acid a solution may be. A solution with a pH of less than
7.0 is considered acidic. Solutions with a pH of less than 4.5 contain
mineral acidity (due to strong inorganic acids), while a solution having a
pH greater than 8.3 contains no acidity.

Yes,

Good definition (for the most part). pH <7 is indeed acidic. pH > 7 is
basic. Your web page had a definition for acidity, but not basicity.
Strange. That's like defining GOOD and not defining BAD.

Here is the IUPAC (International Union of Pure and Applied Chemistry)
definition of acidity:

http://www.chem.qmul.ac.uk/iupac/index.html

acidity

(1) Of a compound:

For Brønsted acids it means the tendency of a compound to act as a hydron
donor. It can be quantitatively expressed by the acid dissociation constant
of the compound in water or some other specified medium. For Lewis acids it
relates to the association constants of Lewis adducts and -adducts.

(2) Of a medium:

The use of the term is mainly restricted to a medium containing Brønsted
acids, where it means the tendency of the medium to hydronate a specific
reference base

basicity

For Brønsted bases it means the tendency of a compound to act as hydron
(proton) acceptor. The basicity of a chemical species is normally expressed
by the acidity of the conjugate acid (see conjugate acid-base pair). For
Lewis bases it relates to the association constants of Lewis adducts
and -adducts



Another definition from the same web page YOU cited: (this is the same web
page you cited above)

Alkalinity:
Acid neutralizing or buffering capacity of water; a measure of the ability
of water to resist changes in pH caused by the addition of acids or bases
and therefore, the main indicator of susceptibility to acid rain; in natural
waters it is due primarily to the presence of bicarbonates, carbonates and
to a much lesser extent occasionally borates, silicates and phosphates. It
is expressed in units of milligrams per liter (mg/l) of CaCO3 (calcium
carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l = 1 mg/l
of CaCO3. A solution having a pH below about 5 contains no alkalinity.

Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and says
that alkalinity is the measure of ...(description of a buffer)

A BUFFER IS : a measure of the ability of water to resist changes in pH
caused by the addition of acids or bases (from definition below)


I said:
***alkalinity is a measurement of 'buffering capacity'***

You said:
***Alkalinity is not a measurement of BC

WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is not
logical.

(THIS FROM THE SAME WEB PAGE YOU CITED):

Buffer:
A substance which tends to keep pH levels fairly constant when acids or
bases are added.

THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.

a measure of the ability of water to resist changes in pH caused by the
addition of acids or bases

SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A BUFFER.


I went to all four links. None contradict what I have said. But the first
one you cited contradicts YOU!

I know what a buffer is. I know what acidity means. I know what alkalinity
means. No need to cite web pages that describe what I know and what I wrote
in this discussion. Show me one that says alkalinity is not a measure of
buffering capacity from a credible source.






"Boomer" > wrote in message
...
> Alkalinity a measure of the amount of anions of weak acid in water and of
the cations
> balanced against them
> Take note it says ***acid***
>
> Buffering capacity the ability of a solution to resist or dampen changes
in pH upon the
> addition of acids or bases.
> Take note its says ***the addition of acids or bases***
>
> One more
>
> http://www.waterontheweb.org/resources/glossary.html
>
> We could go on like this all day, so what is the point ?
>
> You will LOVE this one
> http://www.kyantec.com/Tips/phbuffering.htm
>
> Don't you just lovbe PDF's
> http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
>
> Don't fall out of your chair
> http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
>
>
>
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message news:XB7Wb.19339$QA2.62332@attbi_s52...
> : Man here is another, google is a wonderful thing. I'm not filtering any
> : out, just posting what I find by GOOGLING for you.
> :
> : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> :
> :
> : Wow, a gov link. Even the government is wrong, this must be a
conspiracy
> : against Boomer.
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > Now I am getting bored
> : >
> : > "Don't the components of a buffer account for the buffering capacity?
> : Yes."
> : >
> : > Yes, agreed but you seem to fail what I'm saying. Buffering Capacity
and
> : Alkalinity are
> : > not the same, that has always been the issue. I gave the equation does
> : that look like an
> : > Alkalinity equation or how Alk is determined. I see you had now
comments
> : on it what's
> : > wrong, why no comments on the equations I gave. Don't understand them
or
> : what ? Again this
> : > is the equation for Buffering Capacity, also called Buffer Index or
Buffer
> : Intensity. It
> : > is defined in most water chemistry and chemical oceanography text
books.
> : >
> : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] +
CKa
> : [H3O+] / (Ka =
> : > H3O+])² )
> : >
> : > This is not Alkalinity now is it ?
> : >
> : > "I know how to do a titration, In fact I have done several. How many
have
> : > you actually done? I don't mean by counting drops, I mean with a
buret?"
> : >
> : > Well good for you, I use a Digital Titrator
> : >
> : > "Oh, I see,
> : > you think acidity is the opposite of alkalinity. In the world of
> : CHEMISTRY
> : > it's not. Maybe in aquarium newsgroups it is.
> : >
> : > Hum no, maybe you should go for a look at HACH's or LaMotte website or
the
> : book I
> : > suggested earlier. Please view a copy.
> : >
> : > Standard Methods for the Examination of Water and Wastewater
> : >
> : > This book, over 2000 pages, is the guide for water testing. If you are
> : reporting water
> : > test to the EPA you must use approved std from this text.I t is
prepared
> : and published by
> : > the EPA, American Water Works Association and American Public Health
> : Association. You
> : > mean you don't have one and the issue is water chemistry
> : >
> : > You are confusing Acidity and Acidity as you know little about water
> : chemistry and
> : > procedures and test methods
> : >
> : > From SMEWW, section 2-30, 2310 ACIDITY
> : >
> : > "Acidity of water is its quantative capacity to react with a strong
base
> : to a designated
> : > pH"
> : >
> : > This is how you test for it
> : >
> : > A std alkali titration to methyl orange or phenolphthalein
> : > endpoint.
> : >
> : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write
this
> : book, there are
> : > over 100 of them, they are wrong.
> : >
> : > Like Buffering Capacity you have your Acidity's mixed up
> : > In water measurement if you have a high Alk you also usually have a
high
> : Acidity.
> : > Normally a high Alk also gives a higher CO2 level. Get a WATER
CHEMISTRY
> : BOOK there pal.
> : >
> : >
> : > "These are all in equilibrium with each other. An initial high pH
(above
> : > 6.4) will shift the equilibrium to the right to form HCO3-1. If the
pH of
> : > the solution is above 10.3 (pKa2) the .........."
> : >
> : >
> : > Christ, there you go again with the FW ****. All your numbers are
wrong we
> : are dealing
> : > with SEAWATER
> : >
> : > This means that at a pH of 8.3, the majority of the CO2(aq) is in the
form
> : > of HCO3-1 .
> : >
> : > I have already pointed that out and gave actual values at know
seawater
> : levels, go back
> : > and re-read it you aren't telling me anything here.Of course most is
HCO3
> : see...
> : >
> : >
> : > @ 20C and 34.3 ppt salinity
> : >
> : > CO2 = 0.52 %
> : >
> : > HCO3 = 86.4 %
> : >
> : > CO3 = 13.09 %
> : >
> : >
> : > "In your glass experiment you managed to lower the pH enough to purge
out
> : CO2
> : > by boiling"
> : >
> : > The purpose behind the glass is to show that alk is not affect by CO2
and
> : vise-versa and
> : > how Co2 affects pH.
> : >
> : > Now, in a real life seawater aquarium, with a pH of 8.3 and that pH
drops
> : to say 8.1 it is
> : > usually due to excess CO2. If you took a glass of that water and
aerated
> : it you WILL drive
> : > off the CO2 and raise the pH. It has been done a proven a million
times.
> : >
> : > "In order to 'purge' CO2 you would need to lower the
> : > pH to shift the equilibrium to below 6.4"
> : >
> : > The hell you do !!!.Do you know who many times people on this NG to
> : include Dr. Craig
> : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
> : sample of aquarium
> : > water and aerate it to see if the pH GOES UP AND when they come back
with
> : the test it is
> : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST
excess
> : CO2 in the tank
> : > water, increase the circulation for better gas exchange at the
surface,
> : reduce feeding,
> : > and try to improve on better skimming, thus reducing the bio-load and
pH
> : decline due to
> : > CO2.
> : >
> : >
> : > "I hope this helps. "
> : >
> : > Help, how can you when you miss everything. I should be charging you
> : >
> : > Oh, by the way. Your websites, I have about 50 on these issues, I
could
> : post them, not to
> : > mention I have all those water chemistry books, so there is no need to
> : view your sites.
> : >
> : > Finally are you afraid to come to our Chemistry Forum, afraid to get
> : slapped by REAL
> : > chemists. I get a charge out of you can't post your ref .I have posted
the
> : same or similar
> : > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500
posts
> : there and am the
> : > biggest contributor to his forum other than himself or maybe Habib
Sheka
> : >
> : > Hum, here are Randy's ref that he posted. He hosts the website
> : >
> : > S. RANDY HOLMES-FARLEY
> : > Arlington, Massachusetts
> : >
> : > EDUCATION
> : >
> : > 1982-1986 Harvard University Cambridge, MA
> : > PhD in Chemistry
> : > Research Advisor: George Whitesides
> : >
> : > Investigated the relationship between polymer surface chemistry and
> : physical properties
> : > through controlled surface modification and testing.
> : >
> : > 1980-1982 Cornell University Ithaca, NY
> : > BA in Chemistry and Biology
> : > Graduated Summa Cum Laude
> : > Distinction in All Subjects
> : > Grade Point: 3.94/4.0
> : > Honors research: isolation and characterization of the subunit of CF1
> : enzyme
> : >
> : >
> : > 1978-1979 Stanford University Palo Alto, CA
> : > Grade Point: 3.55/4.0
> : >
> : >
> : > EXPERIENCE
> : >
> : > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> : > (bought out GelTex Pharmaceuticals in 2001)
> : > Vice President, Chemical Research 2001-present
> : > Senior Director, Chemical Research 1999-2001
> : > Director of Chemical Research 1997-1999
> : > Manager of Chemical Research 1995-1997
> : > Group Leader 1994-1995
> : > Senior Research Scientist 1992-1994
> : >
> : > Helped start GelTex as second employee
> : >
> : > Managed various research programs with multi-million dollar budgets
> : >
> : > Supervised research chemists (17+)
> : >
> : > Co-inventor of several polymeric pharmaceuticals and pharmaceutical
> : candidates including
> : > Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride
(FDA
> : approved)
> : >
> : > Company Safety Officer for 3 years
> : >
> : > Chemical Hygiene Officer 2000-present
> : >
> : >
> : >
> : >
> : > 1990-1992 GTE Corporation Waltham, MA
> : > Senior Member of Technical Staff
> : > Applied research involving polymer interfaces
> : > Metallization of plastics
> : > Polymer/polymer adhesion
> : > Optical coatings
> : >
> : >
> : >
> : > 1986-1990 Lord Corporation Cary, NC
> : > Senior Research Scientist 1988-1990
> : > Research Scientist 1986-1988
> : > Basic and applied research on surface chemical bonding
> : > Developed new adhesive compositions
> : > Developed new sol-gel coatings for corrosion resistance
> : >
> : >
> : > HONORS AND AWARDS
> : >
> : > Industrial Innovations Award by Northeast Region of American Chemical
> : Society (6/2001)
> : >
> : > National Kidney Foundation of Northern California Honoree (5/2001)
> : >
> : > American Chemical Society/Polymer Chemistry Division Industrial
Sponsors
> : > Award (8/2000)
> : >
> : > R&D 100 Award from R&D magazine (1999)
> : >
> : > Sherwin Williams Award in applied polymer science (9/85)
> : >
> : > IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
> : >
> : > Award for highest GPA in Chemistry Department (6/82)
> : >
> : > Summa Cum Laude Honors in Chemistry (6/82)
> : >
> : > Phi Lamda Epsilon (6/82)
> : >
> : > Phi Beta Kappa (2/82)
> : >
> : > Cornell University Dean's List (1981, 1982)
> : >
> : > Harvard Book Club Award for highest GPA senior year (1978)
> : >
> : > First Place in western NY ACS high school chemistry exam (1977)
> : >
> : > 1978-1979
> : >
> : >
> : > __________________
> : > Randy Holmes-Farley
> : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
> : >
> : > Hobby Experience: 8 years with reefs
> : > Current Tanks: 90 gal mixed reef
> : > Interests: Reefkeeping, science, photography
> : >
> : >
> : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> : >
> : > Open this post in a new window | Report this post to a moderator | IP:
> : Logged
> : >
> : >
> : >
> : > 06/27/2003 02:44 PM
> : >
> : > Randy Holmes-Farley
> : > Chemistry Moderator
> : >
> : > Registered: Apr 2001
> : > Location: Arlington, Massachusetts
> : > Occupation: Chemist (Drug Discovery at Genzyme)
> : > Posts: 15282
> : >
> : >
> : >
> : > Publications
> : >
> : >
> : > ISSUED UNITED STATES PATENTS
> : >
> : >
> : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
> : Mandeville, III; W. Harry.
> : > US 6,566,407; 5/20/2003
> : >
> : > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen
Randall;
> : Huval, Chad
> : > Cori.
> : > U.S. 6,517,825; 2/11/2003.
> : >
> : > 3. Method of making phosphate-binding polymers for oral
administration.
> : Holmes-Farley,
> : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
> : 6,509,013; 1/21/2003.
> : >
> : > 4. Combination therapy for treating hypercholesterolemia using a bile
acid
> : sequestrant
> : > polymer
> : > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley,
Stephen
> : Randall;
> : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> : >
> : > 5. Method for treating hypercholesterolemia with polyallylamine
polymers.
> : Holmes-Farley,
> : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
Goldberg,
> : Dennis I. , US
> : > 6,423,754; 7/23/2002.
> : >
> : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
> : Neenan, Thomas X..;
> : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> : >
> : > 7. Combination therapy for treating hypercholesterolemia and
> : atherosclerosis. Huval, Chad
> : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep
K.
> : U.S. 6,365,186;
> : > 4/2/2002.
> : >
> : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
Mandeville,
> : W. H., III;
> : > Huval; C.
> : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
> : 10/9/2001.
> : >
> : > 9. Polymers containing guanidinium groups as bile acid sequestrants.
Dhal;
> : P. K.; Holmes-
> : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> : >
> : > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III.; US
> : > 6,281,252;
> : > 8/28/2001.
> : >
> : > 11. Combination therapy for treating hypercholestrolemia. Huval; C.
C.;
> : Holmes-Farley; S.
> : > R. ;
> : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> : >
> : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
> : Holmes-Farley, S.
> : > R.; US
> : > 6,264,937; 7/24/2001.
> : >
> : > 13. Method for treating hypercholesterolemia with unsubstituted
> : polydiallylamine polymers.
> : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
> : 6,248,318;
> : > 6/19/2001.
> : >
> : > 14. Process for removing bile salts from a patient and alkylated
> : compositions therefore.
> : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
> : >
> : > 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S.
R.;
> : Dhal, P. K.;
> : > Petersen,
> : > J. S.; US 6,203,785; 3/20/2001.
> : >
> : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.;
Huval,
> : C. C.; US
> : > 6,190,649;
> : > 2/20/2001.
> : >
> : > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III.; US
> : > 6,177,478;
> : > 1/23/2001.
> : >
> : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
Holmes-Farley,
> : S. R.;
> : > Mandeville, W.
> : > H., III.; US 6,129,910; 10/10/2000.
> : >
> : > 19. Method for treating hypercholesterolemia with unsubstituted
> : polydiallylamine polymers.
> : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
> : 6,083,497;
> : > 7/4/2000.
> : >
> : > 20. Method of making phosphate-binding polymers for oral
administration.
> : Holmes-Farley, S.
> : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495;
7/4/2000.
> : >
> : > 21. Process for removing bile salts from a patient and alkylated
> : compositions therefore.
> : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
5/23/2000.
> : >
> : > 22. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> : >
> : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
> : Neenan; T. X.; Holmes-
> : > Farley; S. R. US 6,034,129; 3/7/2000.
> : >
> : > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III.; US
> : > 5,985,938;
> : > 11/16/99.
> : >
> : > 25. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> : >
> : > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W.
H.,
> : III.;
> : > Holmes-Farley;
> : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> : >
> : > 27. Hydrophilic nonamine-containing and amine-containing copolymers
and
> : their use as bile
> : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
5,929,184;
> : 7/27/99.
> : >
> : > 28. Interpenetrating polymer networks for sequestration of bile acids.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
> : 7/20/99.
> : >
> : > 29. Amine polymer sequestrant and method of cholesterol depletion.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> : >
> : > 30. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> : >
> : > 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> : >
> : > 32. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> : >
> : > 33. Preparation of polymeric sequestrants for bile acid salts.
Mandeville,
> : W. H., III.;
> : > Holmes-
> : > Farley, S. R.; US 5,703,188; 12/30/97.
> : >
> : > 34. Oral administration of iron-binding crosslinked amine polymers.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> : >
> : > 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley,
S.
> : R.; US 5,693,675;
> : > 12/2/97.
> : >
> : > 36. Method for removing bile salts from a patient with alkylated
> : crosslinked amine
> : > polymers,
> : > and preparation of the polymers. Mandeville, W. H., III.;
Holmes-Farley,
> : S. R.; US
> : > 5,679,717; 10/21/97.
> : >
> : > 37. Phosphate-binding polymers for oral administration. Holmes-Farley,
S.
> : R.; Mandeville,
> : > W.
> : > H., III.; US 5,667,775; 9/16/97.
> : >
> : > 38. Ion-exchange process using highly crosslinked polymers for
removing
> : bile salts from a
> : > patient, preparation of the polymers, and compositions containing
them.
> : Mandeville, W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> : >
> : > 39. Hydrophobic amine polymer sequestrant and method of cholesterol
> : depletion. Mandeville,
> : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530;
4/8/97.
> : >
> : > 40. Amine polymer sequestrant and method of cholesterol depletion.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> : >
> : > 41. Phosphate-binding polymers for oral administration. Holmes-Farley,
S.
> : R.; Mandeville,
> : > W.
> : > H., III.; US 5,496,545; 3/5/96.
> : >
> : > 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
> : III.; Holmes-Farley,
> : > S. R.;
> : > US 5,487,888; 1/30/96.
> : >
> : > 43. Ultra-thin, uniform sol-gel coating of a substrate having active
> : hydrogens on the
> : > surface.
> : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> : >
> : > 44. Layered sol-gel coatings from organisilicon compounds.
Holmes-Farley,
> : S. R.; Yanyo, L.
> : > C.;
> : > US 5,182,143; 1/26/93.
> : >
> : > 45. Method for metal bonding using ultrathin primer coating.
> : Holmes-Farley, S. R.; Yanyo,
> : > L.
> : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> : >
> : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.;
US
> : 5,096,962;
> : > 3/17/92.
> : >
> : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> : elastomer-metal bonding.
> : > Holmes-
> : > Farley, S. R.; US 5,102,956; 4/7/92.
> : >
> : >
> : >
> : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
> : >
> : >
> : > 1. Aryl boronate functionalized polymers for treating obesity and
> : inhibiting fat uptake.
> : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal,
Pradeep
> : K.; Huval, Chad
> : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92
pp. WO
> : 0302571.
> : >
> : > 2. Preparation of aryl boronic acids for treating obesity.
Holmes-Farley,
> : Stephen Randall;
> : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep
K.
> : (Geltex
> : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
> : >
> : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
> : Stephen Randall.
> : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
> : 0302130.
> : >
> : > 4. Method for reducing copper levels and treating copper toxicosis.
> : Holmes-Farley, Stephen
> : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002),
45
> : pp. WO
> : > 0285383.
> : >
> : > 5. Method for treating gout and binding uric acid. Holmes-Farley,
Stephen
> : Randall; Burke,
> : > Steven K. WO 0285381 10/31/2002.
> : >
> : > 6. Method for treating gout and reducing serum uric acid.
Holmes-Farley,
> : Stephen Randall;
> : > Burke, Steven K WO 0285380 10/31/2002.
> : >
> : > 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
> : Holmes-Farley, S. R.;
> : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> : >
> : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
> : Holmes-Farley, S.
> : > R.;
> : > WO 1999-US5662; 9/23/1999.
> : >
> : > 9. Amine-containing copolymers as bile acid sequestrants.
Holmes-Farley,
> : S. R.; Petersen,
> : > J. S.;
> : > WO 9933452; 7/8/1999.
> : >
> : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III
and
> : Holmes-Farley, S.
> : > R.;
> : > WO 9922743; 5/14/1999.
> : >
> : > 11. Polyallylamine polymers for removing bile salts and treating
> : hypercholesterolemia, and
> : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III;
Burke,
> : S. K.; Goldberg,
> : > D. I.; WO 9857652; 12/23/98.
> : >
> : > 12. Phosphate-bidning polymers combined with a calcium supplement for
oral
> : administration.
> : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley,
S.
> : R.; WO 9842355;
> : > 10/1/98.
> : >
> : > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
> : depletion. Mandeville,
> : > W.
> : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
> : >
> : > 14. Process for adjusting ion concentration in a patient and
compositions
> : therefor.
> : > Mandeville,
> : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> : >
> : > 15. Vacuum-deposited silver on polycarbonate with a chromium
interlayer
> : for improved
> : > metal-
> : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
1/20/94.
> : >
> : > 16. Process for increased metal-substrate bond strength in metalized
> : plastics.
> : > Holmes-Farley, S.
> : > R.; Ger. Offen. 4322516; 7/6/93.
> : >
> : > 17. Electrorheological fluids and preparation of particles useful in
the
> : fluids.
> : > Troughton,
> : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
> : David; Bares, Joseph
> : > E.;
> : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
> : 394049;
> : > 10/24/1990.
> : >
> : > JOURNAL PUBLICATIONS
> : >
> : > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov,
Eugene;
> : Guo, Amy;
> : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
> : Mandeville, W. Harry;
> : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
611-619.
> : >
> : > 2. Amine functionalized polyethers as bile acid sequestrants:
synthesis
> : and biological
> : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S.
Randall;
> : Mandeville, W.
> : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
> : Journal of
> : > Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
> : 1559-1574.
> : >
> : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
> : Imprinting. Huval,
> : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
> : Randall; Mandeville,
> : > W.
> : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert
J.;
> : Chen, Xi; Dhal,
> : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> : >
> : > 4. Synthetic polymers for the binding of fat in the intestinal tract.
> : Jozefiak, Thomas H.;
> : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia;
Huval,
> : Chad C.;
> : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
> : Abstracts of
> : > Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
> : 26-30, 2001
> : > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
> : Division of
> : > Polymer Chemistry) (2001), 42(2), 98.
> : >
> : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer
gel
> : pharmaceutical.
> : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.;
Ward,
> : J.; Sacchiero,
> : > B.;
> : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.;
Chen,
> : X.; Mazzeo, J.
> : > R.. Polym. Preprints (2000), 41(1), 735-736.
> : >
> : > 6. In vitro comparison of bile acid binding to colesevelam HCl and
other
> : bile acid
> : > sequestrants.
> : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
> : Hook, P.; Holmes-
> : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
> : >
> : > 7. Novel polymeric pharmaceuticals: From startup to market.
Holmes-Farley,
> : S. R; Polym.
> : > Mater. Sci. Eng (1999), 80, 246-247.
> : >
> : > 8. Design and characterization of of Sevelamer Hydrochloride: a novel
> : phosphate-binding
> : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward,
J.;
> : Miller, K. L.;
> : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure
and
> : Appl. Chem.,
> : > A36(7&8), p. 1085 (1999).
> : >
> : > 9. Three generations of bile acid sequestrants. Mandeville, W. H.,
III;
> : Braunlin, W.;
> : > Dhal, P.;
> : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
> : Rosenbaum, D.;
> : > Sacchiero,
> : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
> : 550, 3-15.
> : >
> : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric
phosphate
> : binder, on
> : > urinary
> : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
> : Mandeville, W. H.,
> : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
> : (1997), 12(5)
> : > 961-964.
> : >
> : > 11. Thin anisotropic coatings based on sol-gel technology.
Holmes-Farley,
> : S. R.; Yanyo, L.
> : > C;
> : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4),
439-444.
> : >
> : > 12. The mechanism of cure initiation of a surface activated adhesive.
> : Holmes-Farley, S.
> : > R.;
> : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
> : >
> : > 13. Adhesion promotion and corrosion prevention using thin anisotropic
> : coatings. Holmes-
> : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
> : 131-151.
> : >
> : > 14. Wetting of functionalized polyethylene having ionizable organic
acids
> : and bases at the
> : > polymer-water interface: relations between functional group polarity,
> : extent of
> : > ionization,
> : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
> : Whitesides, G. M.;
> : > Langmuir
> : > (1988), 4(4), 921-937.
> : >
> : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
> : single hydroxy group.
> : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> : >
> : > 16. Reconstruction of the interface of oxidatively functionalized
> : polyethylene (PE-CO2H)
> : > and
> : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo,
R.;
> : McCarthy, T. J.;
> : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report
(1987),
> : AD-
> : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> : >
> : > 17. Surface-modified polyethylene film: the relationship between
surface
> : chemistry and
> : > physical
> : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11),
4537.
> : >
> : > 18. Reactivity of carboxylic acid and ester groups in the
functionalized
> : interfacial
> : > region of
> : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> : differentiation of the
> : > functional groups into shallow and deep subsets based on a comparison
of
> : contact angle and
> : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
> : (1987), 3(1), 62-
> : > 76.
> : >
> : > 19. Fluorescence properties of dansyl groups covalently bonded tot he
> : surface of
> : > oxidatively
> : > functionalized low-density polyethylene film. Holmes-Farley, S. R.;
> : Whitesides, G. M.;
> : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
> : AD-A162435/2/GAR,
> : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> : >
> : > 20. Acid-base behavior of carboxylic acid groups covalently attached
at
> : the surface of
> : > polyethylene: The usefulness of contact angle in following the
ionization
> : of surface
> : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
> : Deutch, J.;
> : > Whitesides,
> : > G. M.; Langmuir (1985), 1(6), 725-740.
> : >
> : > 21. The thermal stability of a surface modified solid organic polymer.
> : Holmes-Farley, S.
> : > R.;
> : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
> : >
> : >
> : >
> : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> : >
> : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
> : Aquarist. June 2003.
> : >
> : > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
> : Advanced Aquarist.
> : > May
> : > 2003.
> : >
> : > 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
> : Reefkeeping May
> : > 2003.
> : >
> : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
> : April 2003.
> : >
> : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> : Holmes-Farley, R.
> : > Advanced Aquarist; April 2003.
> : >
> : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> : Holmes-Farley, R.
> : > Advanced Aquarist; April 2003.
> : >
> : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced
Aquarist;
> : March 2003.
> : >
> : > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
> : Holmes-Farley, R.
> : > Advanced Aquarist; February 2003.
> : >
> : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
> : 2003.
> : >
> : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
December
> : 2002.
> : >
> : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
Advanced
> : Aquarist; November
> : > 2002.
> : >
> : > 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
> : Advanced Aquarist;
> : > November 2002.
> : >
> : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced
Aquarist,
> : September 2002.
> : >
> : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
> : 2002.
> : >
> : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
> : 2002.
> : >
> : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
> : Aquarist; July 2002
> : >
> : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist;
June
> : 2002.
> : >
> : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R.
Advanced
> : Aquarist, May
> : > 2002.
> : >
> : > 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
> : Holmes-Farley, R.
> : > Advanced Aquarist, April 2002.
> : >
> : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> : >
> : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
> : >
> : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January
2002.
> : >
> : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
> : 2000.
> : >
> : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
> : Frontiers 2000.
> : >
> : > 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
> : Aquarium Frontiers
> : > 2000.
> : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
Frontiers
> : 2000.
> : >
> : > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers
2000.
> : >
> : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
> : >
> : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> : >
> : >
> : >
> : >
> : >
> : >
> : >
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : >
> : >
> :
> :
>
>

[stoutman]

Boomer,

I am not sure if you are just messing with me or if you are truly confused.
I hope the latter. Please read from Top to Bottom.


From YOUR first link:

http://www.waterontheweb.org/resources/glossary.html

Acidity:
A measure of how acid a solution may be. A solution with a pH of less than
7.0 is considered acidic. Solutions with a pH of less than 4.5 contain
mineral acidity (due to strong inorganic acids), while a solution having a
pH greater than 8.3 contains no acidity.

Yes,

Good definition (for the most part). pH <7 is indeed acidic. pH > 7 is
basic. Your web page had a definition for acidity, but not basicity.
Strange. That's like defining GOOD and not defining BAD.

Here is the IUPAC (International Union of Pure and Applied Chemistry)
definition of acidity:

http://www.chem.qmul.ac.uk/iupac/index.html

acidity

(1) Of a compound:

For Brønsted acids it means the tendency of a compound to act as a hydron
donor. It can be quantitatively expressed by the acid dissociation constant
of the compound in water or some other specified medium. For Lewis acids it
relates to the association constants of Lewis adducts and -adducts.

(2) Of a medium:

The use of the term is mainly restricted to a medium containing Brønsted
acids, where it means the tendency of the medium to hydronate a specific
reference base

basicity

For Brønsted bases it means the tendency of a compound to act as hydron
(proton) acceptor. The basicity of a chemical species is normally expressed
by the acidity of the conjugate acid (see conjugate acid-base pair). For
Lewis bases it relates to the association constants of Lewis adducts
and -adducts



Another definition from the same web page YOU cited: (this is the same web
page you cited above)

Alkalinity:
Acid neutralizing or buffering capacity of water; a measure of the ability
of water to resist changes in pH caused by the addition of acids or bases
and therefore, the main indicator of susceptibility to acid rain; in natural
waters it is due primarily to the presence of bicarbonates, carbonates and
to a much lesser extent occasionally borates, silicates and phosphates. It
is expressed in units of milligrams per liter (mg/l) of CaCO3 (calcium
carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l = 1 mg/l
of CaCO3. A solution having a pH below about 5 contains no alkalinity.

Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and says
that alkalinity is the measure of ...(the properties of a buffer)


I said:
***alkalinity is a measurement of 'buffering capacity'***

You said:
***Alkalinity is not a measurement of BC

WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is not
logical.

(THIS FROM THE SAME WEB PAGE YOU CITED):

Buffer:
A substance which tends to keep pH levels fairly constant when acids or
bases are added.

THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.

a measure of the ability of water to resist changes in pH caused by the
addition of acids or bases

SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A BUFFER.


I went to all four links. None contradict what I have said. But the first
one you cited contradicts YOU!

I know what a buffer is. I know what acidity means. I know what alkalinity
means. No need to cite web pages that describe what I know and what I wrote
in this discussion. Show me one that says alkalinity is not a measure of
buffering capacity from a credible source.




"Boomer" > wrote in message
...
> Alkalinity a measure of the amount of anions of weak acid in water and of
the cations
> balanced against them
> Take note it says ***acid***
>
> Buffering capacity the ability of a solution to resist or dampen changes
in pH upon the
> addition of acids or bases.
> Take note its says ***the addition of acids or bases***
>
> One more
>
> http://www.waterontheweb.org/resources/glossary.html
>
> We could go on like this all day, so what is the point ?
>
> You will LOVE this one
> http://www.kyantec.com/Tips/phbuffering.htm
>
> Don't you just lovbe PDF's
> http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
>
> Don't fall out of your chair
> http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
>
>
>
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message news:XB7Wb.19339$QA2.62332@attbi_s52...
> : Man here is another, google is a wonderful thing. I'm not filtering any
> : out, just posting what I find by GOOGLING for you.
> :
> : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> :
> :
> : Wow, a gov link. Even the government is wrong, this must be a
conspiracy
> : against Boomer.
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > Now I am getting bored
> : >
> : > "Don't the components of a buffer account for the buffering capacity?
> : Yes."
> : >
> : > Yes, agreed but you seem to fail what I'm saying. Buffering Capacity
and
> : Alkalinity are
> : > not the same, that has always been the issue. I gave the equation does
> : that look like an
> : > Alkalinity equation or how Alk is determined. I see you had now
comments
> : on it what's
> : > wrong, why no comments on the equations I gave. Don't understand them
or
> : what ? Again this
> : > is the equation for Buffering Capacity, also called Buffer Index or
Buffer
> : Intensity. It
> : > is defined in most water chemistry and chemical oceanography text
books.
> : >
> : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] +
CKa
> : [H3O+] / (Ka =
> : > H3O+])² )
> : >
> : > This is not Alkalinity now is it ?
> : >
> : > "I know how to do a titration, In fact I have done several. How many
have
> : > you actually done? I don't mean by counting drops, I mean with a
buret?"
> : >
> : > Well good for you, I use a Digital Titrator
> : >
> : > "Oh, I see,
> : > you think acidity is the opposite of alkalinity. In the world of
> : CHEMISTRY
> : > it's not. Maybe in aquarium newsgroups it is.
> : >
> : > Hum no, maybe you should go for a look at HACH's or LaMotte website or
the
> : book I
> : > suggested earlier. Please view a copy.
> : >
> : > Standard Methods for the Examination of Water and Wastewater
> : >
> : > This book, over 2000 pages, is the guide for water testing. If you are
> : reporting water
> : > test to the EPA you must use approved std from this text.I t is
prepared
> : and published by
> : > the EPA, American Water Works Association and American Public Health
> : Association. You
> : > mean you don't have one and the issue is water chemistry
> : >
> : > You are confusing Acidity and Acidity as you know little about water
> : chemistry and
> : > procedures and test methods
> : >
> : > From SMEWW, section 2-30, 2310 ACIDITY
> : >
> : > "Acidity of water is its quantative capacity to react with a strong
base
> : to a designated
> : > pH"
> : >
> : > This is how you test for it
> : >
> : > A std alkali titration to methyl orange or phenolphthalein
> : > endpoint.
> : >
> : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write
this
> : book, there are
> : > over 100 of them, they are wrong.
> : >
> : > Like Buffering Capacity you have your Acidity's mixed up
> : > In water measurement if you have a high Alk you also usually have a
high
> : Acidity.
> : > Normally a high Alk also gives a higher CO2 level. Get a WATER
CHEMISTRY
> : BOOK there pal.
> : >
> : >
> : > "These are all in equilibrium with each other. An initial high pH
(above
> : > 6.4) will shift the equilibrium to the right to form HCO3-1. If the
pH of
> : > the solution is above 10.3 (pKa2) the .........."
> : >
> : >
> : > Christ, there you go again with the FW ****. All your numbers are
wrong we
> : are dealing
> : > with SEAWATER
> : >
> : > This means that at a pH of 8.3, the majority of the CO2(aq) is in the
form
> : > of HCO3-1 .
> : >
> : > I have already pointed that out and gave actual values at know
seawater
> : levels, go back
> : > and re-read it you aren't telling me anything here.Of course most is
HCO3
> : see...
> : >
> : >
> : > @ 20C and 34.3 ppt salinity
> : >
> : > CO2 = 0.52 %
> : >
> : > HCO3 = 86.4 %
> : >
> : > CO3 = 13.09 %
> : >
> : >
> : > "In your glass experiment you managed to lower the pH enough to purge
out
> : CO2
> : > by boiling"
> : >
> : > The purpose behind the glass is to show that alk is not affect by CO2
and
> : vise-versa and
> : > how Co2 affects pH.
> : >
> : > Now, in a real life seawater aquarium, with a pH of 8.3 and that pH
drops
> : to say 8.1 it is
> : > usually due to excess CO2. If you took a glass of that water and
aerated
> : it you WILL drive
> : > off the CO2 and raise the pH. It has been done a proven a million
times.
> : >
> : > "In order to 'purge' CO2 you would need to lower the
> : > pH to shift the equilibrium to below 6.4"
> : >
> : > The hell you do !!!.Do you know who many times people on this NG to
> : include Dr. Craig
> : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
> : sample of aquarium
> : > water and aerate it to see if the pH GOES UP AND when they come back
with
> : the test it is
> : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST
excess
> : CO2 in the tank
> : > water, increase the circulation for better gas exchange at the
surface,
> : reduce feeding,
> : > and try to improve on better skimming, thus reducing the bio-load and
pH
> : decline due to
> : > CO2.
> : >
> : >
> : > "I hope this helps. "
> : >
> : > Help, how can you when you miss everything. I should be charging you
> : >
> : > Oh, by the way. Your websites, I have about 50 on these issues, I
could
> : post them, not to
> : > mention I have all those water chemistry books, so there is no need to
> : view your sites.
> : >
> : > Finally are you afraid to come to our Chemistry Forum, afraid to get
> : slapped by REAL
> : > chemists. I get a charge out of you can't post your ref .I have posted
the
> : same or similar
> : > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500
posts
> : there and am the
> : > biggest contributor to his forum other than himself or maybe Habib
Sheka
> : >
> : > Hum, here are Randy's ref that he posted. He hosts the website
> : >
> : > S. RANDY HOLMES-FARLEY
> : > Arlington, Massachusetts
> : >
> : > EDUCATION
> : >
> : > 1982-1986 Harvard University Cambridge, MA
> : > PhD in Chemistry
> : > Research Advisor: George Whitesides
> : >
> : > Investigated the relationship between polymer surface chemistry and
> : physical properties
> : > through controlled surface modification and testing.
> : >
> : > 1980-1982 Cornell University Ithaca, NY
> : > BA in Chemistry and Biology
> : > Graduated Summa Cum Laude
> : > Distinction in All Subjects
> : > Grade Point: 3.94/4.0
> : > Honors research: isolation and characterization of the subunit of CF1
> : enzyme
> : >
> : >
> : > 1978-1979 Stanford University Palo Alto, CA
> : > Grade Point: 3.55/4.0
> : >
> : >
> : > EXPERIENCE
> : >
> : > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> : > (bought out GelTex Pharmaceuticals in 2001)
> : > Vice President, Chemical Research 2001-present
> : > Senior Director, Chemical Research 1999-2001
> : > Director of Chemical Research 1997-1999
> : > Manager of Chemical Research 1995-1997
> : > Group Leader 1994-1995
> : > Senior Research Scientist 1992-1994
> : >
> : > Helped start GelTex as second employee
> : >
> : > Managed various research programs with multi-million dollar budgets
> : >
> : > Supervised research chemists (17+)
> : >
> : > Co-inventor of several polymeric pharmaceuticals and pharmaceutical
> : candidates including
> : > Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride
(FDA
> : approved)
> : >
> : > Company Safety Officer for 3 years
> : >
> : > Chemical Hygiene Officer 2000-present
> : >
> : >
> : >
> : >
> : > 1990-1992 GTE Corporation Waltham, MA
> : > Senior Member of Technical Staff
> : > Applied research involving polymer interfaces
> : > Metallization of plastics
> : > Polymer/polymer adhesion
> : > Optical coatings
> : >
> : >
> : >
> : > 1986-1990 Lord Corporation Cary, NC
> : > Senior Research Scientist 1988-1990
> : > Research Scientist 1986-1988
> : > Basic and applied research on surface chemical bonding
> : > Developed new adhesive compositions
> : > Developed new sol-gel coatings for corrosion resistance
> : >
> : >
> : > HONORS AND AWARDS
> : >
> : > Industrial Innovations Award by Northeast Region of American Chemical
> : Society (6/2001)
> : >
> : > National Kidney Foundation of Northern California Honoree (5/2001)
> : >
> : > American Chemical Society/Polymer Chemistry Division Industrial
Sponsors
> : > Award (8/2000)
> : >
> : > R&D 100 Award from R&D magazine (1999)
> : >
> : > Sherwin Williams Award in applied polymer science (9/85)
> : >
> : > IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
> : >
> : > Award for highest GPA in Chemistry Department (6/82)
> : >
> : > Summa Cum Laude Honors in Chemistry (6/82)
> : >
> : > Phi Lamda Epsilon (6/82)
> : >
> : > Phi Beta Kappa (2/82)
> : >
> : > Cornell University Dean's List (1981, 1982)
> : >
> : > Harvard Book Club Award for highest GPA senior year (1978)
> : >
> : > First Place in western NY ACS high school chemistry exam (1977)
> : >
> : > 1978-1979
> : >
> : >
> : > __________________
> : > Randy Holmes-Farley
> : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
> : >
> : > Hobby Experience: 8 years with reefs
> : > Current Tanks: 90 gal mixed reef
> : > Interests: Reefkeeping, science, photography
> : >
> : >
> : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> : >
> : > Open this post in a new window | Report this post to a moderator | IP:
> : Logged
> : >
> : >
> : >
> : > 06/27/2003 02:44 PM
> : >
> : > Randy Holmes-Farley
> : > Chemistry Moderator
> : >
> : > Registered: Apr 2001
> : > Location: Arlington, Massachusetts
> : > Occupation: Chemist (Drug Discovery at Genzyme)
> : > Posts: 15282
> : >
> : >
> : >
> : > Publications
> : >
> : >
> : > ISSUED UNITED STATES PATENTS
> : >
> : >
> : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
> : Mandeville, III; W. Harry.
> : > US 6,566,407; 5/20/2003
> : >
> : > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen
Randall;
> : Huval, Chad
> : > Cori.
> : > U.S. 6,517,825; 2/11/2003.
> : >
> : > 3. Method of making phosphate-binding polymers for oral
administration.
> : Holmes-Farley,
> : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
> : 6,509,013; 1/21/2003.
> : >
> : > 4. Combination therapy for treating hypercholesterolemia using a bile
acid
> : sequestrant
> : > polymer
> : > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley,
Stephen
> : Randall;
> : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> : >
> : > 5. Method for treating hypercholesterolemia with polyallylamine
polymers.
> : Holmes-Farley,
> : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
Goldberg,
> : Dennis I. , US
> : > 6,423,754; 7/23/2002.
> : >
> : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
> : Neenan, Thomas X..;
> : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> : >
> : > 7. Combination therapy for treating hypercholesterolemia and
> : atherosclerosis. Huval, Chad
> : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep
K.
> : U.S. 6,365,186;
> : > 4/2/2002.
> : >
> : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
Mandeville,
> : W. H., III;
> : > Huval; C.
> : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
> : 10/9/2001.
> : >
> : > 9. Polymers containing guanidinium groups as bile acid sequestrants.
Dhal;
> : P. K.; Holmes-
> : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> : >
> : > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III.; US
> : > 6,281,252;
> : > 8/28/2001.
> : >
> : > 11. Combination therapy for treating hypercholestrolemia. Huval; C.
C.;
> : Holmes-Farley; S.
> : > R. ;
> : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> : >
> : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
> : Holmes-Farley, S.
> : > R.; US
> : > 6,264,937; 7/24/2001.
> : >
> : > 13. Method for treating hypercholesterolemia with unsubstituted
> : polydiallylamine polymers.
> : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
> : 6,248,318;
> : > 6/19/2001.
> : >
> : > 14. Process for removing bile salts from a patient and alkylated
> : compositions therefore.
> : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
> : >
> : > 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S.
R.;
> : Dhal, P. K.;
> : > Petersen,
> : > J. S.; US 6,203,785; 3/20/2001.
> : >
> : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.;
Huval,
> : C. C.; US
> : > 6,190,649;
> : > 2/20/2001.
> : >
> : > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III.; US
> : > 6,177,478;
> : > 1/23/2001.
> : >
> : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
Holmes-Farley,
> : S. R.;
> : > Mandeville, W.
> : > H., III.; US 6,129,910; 10/10/2000.
> : >
> : > 19. Method for treating hypercholesterolemia with unsubstituted
> : polydiallylamine polymers.
> : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
> : 6,083,497;
> : > 7/4/2000.
> : >
> : > 20. Method of making phosphate-binding polymers for oral
administration.
> : Holmes-Farley, S.
> : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495;
7/4/2000.
> : >
> : > 21. Process for removing bile salts from a patient and alkylated
> : compositions therefore.
> : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
5/23/2000.
> : >
> : > 22. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> : >
> : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
> : Neenan; T. X.; Holmes-
> : > Farley; S. R. US 6,034,129; 3/7/2000.
> : >
> : > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III.; US
> : > 5,985,938;
> : > 11/16/99.
> : >
> : > 25. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> : >
> : > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W.
H.,
> : III.;
> : > Holmes-Farley;
> : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> : >
> : > 27. Hydrophilic nonamine-containing and amine-containing copolymers
and
> : their use as bile
> : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
5,929,184;
> : 7/27/99.
> : >
> : > 28. Interpenetrating polymer networks for sequestration of bile acids.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
> : 7/20/99.
> : >
> : > 29. Amine polymer sequestrant and method of cholesterol depletion.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> : >
> : > 30. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> : >
> : > 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> : >
> : > 32. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> : >
> : > 33. Preparation of polymeric sequestrants for bile acid salts.
Mandeville,
> : W. H., III.;
> : > Holmes-
> : > Farley, S. R.; US 5,703,188; 12/30/97.
> : >
> : > 34. Oral administration of iron-binding crosslinked amine polymers.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> : >
> : > 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley,
S.
> : R.; US 5,693,675;
> : > 12/2/97.
> : >
> : > 36. Method for removing bile salts from a patient with alkylated
> : crosslinked amine
> : > polymers,
> : > and preparation of the polymers. Mandeville, W. H., III.;
Holmes-Farley,
> : S. R.; US
> : > 5,679,717; 10/21/97.
> : >
> : > 37. Phosphate-binding polymers for oral administration. Holmes-Farley,
S.
> : R.; Mandeville,
> : > W.
> : > H., III.; US 5,667,775; 9/16/97.
> : >
> : > 38. Ion-exchange process using highly crosslinked polymers for
removing
> : bile salts from a
> : > patient, preparation of the polymers, and compositions containing
them.
> : Mandeville, W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> : >
> : > 39. Hydrophobic amine polymer sequestrant and method of cholesterol
> : depletion. Mandeville,
> : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530;
4/8/97.
> : >
> : > 40. Amine polymer sequestrant and method of cholesterol depletion.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> : >
> : > 41. Phosphate-binding polymers for oral administration. Holmes-Farley,
S.
> : R.; Mandeville,
> : > W.
> : > H., III.; US 5,496,545; 3/5/96.
> : >
> : > 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
> : III.; Holmes-Farley,
> : > S. R.;
> : > US 5,487,888; 1/30/96.
> : >
> : > 43. Ultra-thin, uniform sol-gel coating of a substrate having active
> : hydrogens on the
> : > surface.
> : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> : >
> : > 44. Layered sol-gel coatings from organisilicon compounds.
Holmes-Farley,
> : S. R.; Yanyo, L.
> : > C.;
> : > US 5,182,143; 1/26/93.
> : >
> : > 45. Method for metal bonding using ultrathin primer coating.
> : Holmes-Farley, S. R.; Yanyo,
> : > L.
> : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> : >
> : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.;
US
> : 5,096,962;
> : > 3/17/92.
> : >
> : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> : elastomer-metal bonding.
> : > Holmes-
> : > Farley, S. R.; US 5,102,956; 4/7/92.
> : >
> : >
> : >
> : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
> : >
> : >
> : > 1. Aryl boronate functionalized polymers for treating obesity and
> : inhibiting fat uptake.
> : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal,
Pradeep
> : K.; Huval, Chad
> : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92
pp. WO
> : 0302571.
> : >
> : > 2. Preparation of aryl boronic acids for treating obesity.
Holmes-Farley,
> : Stephen Randall;
> : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep
K.
> : (Geltex
> : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
> : >
> : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
> : Stephen Randall.
> : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
> : 0302130.
> : >
> : > 4. Method for reducing copper levels and treating copper toxicosis.
> : Holmes-Farley, Stephen
> : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002),
45
> : pp. WO
> : > 0285383.
> : >
> : > 5. Method for treating gout and binding uric acid. Holmes-Farley,
Stephen
> : Randall; Burke,
> : > Steven K. WO 0285381 10/31/2002.
> : >
> : > 6. Method for treating gout and reducing serum uric acid.
Holmes-Farley,
> : Stephen Randall;
> : > Burke, Steven K WO 0285380 10/31/2002.
> : >
> : > 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
> : Holmes-Farley, S. R.;
> : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> : >
> : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
> : Holmes-Farley, S.
> : > R.;
> : > WO 1999-US5662; 9/23/1999.
> : >
> : > 9. Amine-containing copolymers as bile acid sequestrants.
Holmes-Farley,
> : S. R.; Petersen,
> : > J. S.;
> : > WO 9933452; 7/8/1999.
> : >
> : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III
and
> : Holmes-Farley, S.
> : > R.;
> : > WO 9922743; 5/14/1999.
> : >
> : > 11. Polyallylamine polymers for removing bile salts and treating
> : hypercholesterolemia, and
> : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III;
Burke,
> : S. K.; Goldberg,
> : > D. I.; WO 9857652; 12/23/98.
> : >
> : > 12. Phosphate-bidning polymers combined with a calcium supplement for
oral
> : administration.
> : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley,
S.
> : R.; WO 9842355;
> : > 10/1/98.
> : >
> : > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
> : depletion. Mandeville,
> : > W.
> : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
> : >
> : > 14. Process for adjusting ion concentration in a patient and
compositions
> : therefor.
> : > Mandeville,
> : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> : >
> : > 15. Vacuum-deposited silver on polycarbonate with a chromium
interlayer
> : for improved
> : > metal-
> : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
1/20/94.
> : >
> : > 16. Process for increased metal-substrate bond strength in metalized
> : plastics.
> : > Holmes-Farley, S.
> : > R.; Ger. Offen. 4322516; 7/6/93.
> : >
> : > 17. Electrorheological fluids and preparation of particles useful in
the
> : fluids.
> : > Troughton,
> : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
> : David; Bares, Joseph
> : > E.;
> : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
> : 394049;
> : > 10/24/1990.
> : >
> : > JOURNAL PUBLICATIONS
> : >
> : > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov,
Eugene;
> : Guo, Amy;
> : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
> : Mandeville, W. Harry;
> : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
611-619.
> : >
> : > 2. Amine functionalized polyethers as bile acid sequestrants:
synthesis
> : and biological
> : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S.
Randall;
> : Mandeville, W.
> : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
> : Journal of
> : > Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
> : 1559-1574.
> : >
> : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
> : Imprinting. Huval,
> : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
> : Randall; Mandeville,
> : > W.
> : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert
J.;
> : Chen, Xi; Dhal,
> : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> : >
> : > 4. Synthetic polymers for the binding of fat in the intestinal tract.
> : Jozefiak, Thomas H.;
> : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia;
Huval,
> : Chad C.;
> : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
> : Abstracts of
> : > Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
> : 26-30, 2001
> : > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
> : Division of
> : > Polymer Chemistry) (2001), 42(2), 98.
> : >
> : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer
gel
> : pharmaceutical.
> : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.;
Ward,
> : J.; Sacchiero,
> : > B.;
> : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.;
Chen,
> : X.; Mazzeo, J.
> : > R.. Polym. Preprints (2000), 41(1), 735-736.
> : >
> : > 6. In vitro comparison of bile acid binding to colesevelam HCl and
other
> : bile acid
> : > sequestrants.
> : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
> : Hook, P.; Holmes-
> : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
> : >
> : > 7. Novel polymeric pharmaceuticals: From startup to market.
Holmes-Farley,
> : S. R; Polym.
> : > Mater. Sci. Eng (1999), 80, 246-247.
> : >
> : > 8. Design and characterization of of Sevelamer Hydrochloride: a novel
> : phosphate-binding
> : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward,
J.;
> : Miller, K. L.;
> : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure
and
> : Appl. Chem.,
> : > A36(7&8), p. 1085 (1999).
> : >
> : > 9. Three generations of bile acid sequestrants. Mandeville, W. H.,
III;
> : Braunlin, W.;
> : > Dhal, P.;
> : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
> : Rosenbaum, D.;
> : > Sacchiero,
> : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
> : 550, 3-15.
> : >
> : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric
phosphate
> : binder, on
> : > urinary
> : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
> : Mandeville, W. H.,
> : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
> : (1997), 12(5)
> : > 961-964.
> : >
> : > 11. Thin anisotropic coatings based on sol-gel technology.
Holmes-Farley,
> : S. R.; Yanyo, L.
> : > C;
> : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4),
439-444.
> : >
> : > 12. The mechanism of cure initiation of a surface activated adhesive.
> : Holmes-Farley, S.
> : > R.;
> : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
> : >
> : > 13. Adhesion promotion and corrosion prevention using thin anisotropic
> : coatings. Holmes-
> : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
> : 131-151.
> : >
> : > 14. Wetting of functionalized polyethylene having ionizable organic
acids
> : and bases at the
> : > polymer-water interface: relations between functional group polarity,
> : extent of
> : > ionization,
> : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
> : Whitesides, G. M.;
> : > Langmuir
> : > (1988), 4(4), 921-937.
> : >
> : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
> : single hydroxy group.
> : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> : >
> : > 16. Reconstruction of the interface of oxidatively functionalized
> : polyethylene (PE-CO2H)
> : > and
> : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo,
R.;
> : McCarthy, T. J.;
> : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report
(1987),
> : AD-
> : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> : >
> : > 17. Surface-modified polyethylene film: the relationship between
surface
> : chemistry and
> : > physical
> : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11),
4537.
> : >
> : > 18. Reactivity of carboxylic acid and ester groups in the
functionalized
> : interfacial
> : > region of
> : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> : differentiation of the
> : > functional groups into shallow and deep subsets based on a comparison
of
> : contact angle and
> : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
> : (1987), 3(1), 62-
> : > 76.
> : >
> : > 19. Fluorescence properties of dansyl groups covalently bonded tot he
> : surface of
> : > oxidatively
> : > functionalized low-density polyethylene film. Holmes-Farley, S. R.;
> : Whitesides, G. M.;
> : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
> : AD-A162435/2/GAR,
> : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> : >
> : > 20. Acid-base behavior of carboxylic acid groups covalently attached
at
> : the surface of
> : > polyethylene: The usefulness of contact angle in following the
ionization
> : of surface
> : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
> : Deutch, J.;
> : > Whitesides,
> : > G. M.; Langmuir (1985), 1(6), 725-740.
> : >
> : > 21. The thermal stability of a surface modified solid organic polymer.
> : Holmes-Farley, S.
> : > R.;
> : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
> : >
> : >
> : >
> : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> : >
> : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
> : Aquarist. June 2003.
> : >
> : > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
> : Advanced Aquarist.
> : > May
> : > 2003.
> : >
> : > 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
> : Reefkeeping May
> : > 2003.
> : >
> : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
> : April 2003.
> : >
> : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> : Holmes-Farley, R.
> : > Advanced Aquarist; April 2003.
> : >
> : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> : Holmes-Farley, R.
> : > Advanced Aquarist; April 2003.
> : >
> : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced
Aquarist;
> : March 2003.
> : >
> : > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
> : Holmes-Farley, R.
> : > Advanced Aquarist; February 2003.
> : >
> : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
> : 2003.
> : >
> : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
December
> : 2002.
> : >
> : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
Advanced
> : Aquarist; November
> : > 2002.
> : >
> : > 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
> : Advanced Aquarist;
> : > November 2002.
> : >
> : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced
Aquarist,
> : September 2002.
> : >
> : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
> : 2002.
> : >
> : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
> : 2002.
> : >
> : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
> : Aquarist; July 2002
> : >
> : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist;
June
> : 2002.
> : >
> : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R.
Advanced
> : Aquarist, May
> : > 2002.
> : >
> : > 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
> : Holmes-Farley, R.
> : > Advanced Aquarist, April 2002.
> : >
> : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> : >
> : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
> : >
> : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January
2002.
> : >
> : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
> : 2000.
> : >
> : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
> : Frontiers 2000.
> : >
> : > 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
> : Aquarium Frontiers
> : > 2000.
> : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
Frontiers
> : 2000.
> : >
> : > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers
2000.
> : >
> : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
> : >
> : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> : >
> : >
> : >
> : >
> : >
> : >
> : >
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : >
> : >
> :
> :
>
>

[stoutman]

>Alkalinity a measure of the amount of anions of weak acid in water and of
the cations balanced against them
>Take note it says ***acid***

Take note, it also says ***bases***

Acid neutralizing or buffering capacity of water; a measure of the ability
of water to resist changes in pH caused by the addition of acids or bases



maybe this is the problem. Boomer do you know what a base is?






"Boomer" > wrote in message
...
> Alkalinity a measure of the amount of anions of weak acid in water and of
the cations
> balanced against them
> Take note it says ***acid***
>
> Buffering capacity the ability of a solution to resist or dampen changes
in pH upon the
> addition of acids or bases.
> Take note its says ***the addition of acids or bases***
>
> One more
>
> http://www.waterontheweb.org/resources/glossary.html
>
> We could go on like this all day, so what is the point ?
>
> You will LOVE this one
> http://www.kyantec.com/Tips/phbuffering.htm
>
> Don't you just lovbe PDF's
> http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
>
> Don't fall out of your chair
> http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
>
>
>
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message news:XB7Wb.19339$QA2.62332@attbi_s52...
> : Man here is another, google is a wonderful thing. I'm not filtering any
> : out, just posting what I find by GOOGLING for you.
> :
> : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> :
> :
> : Wow, a gov link. Even the government is wrong, this must be a
conspiracy
> : against Boomer.
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > Now I am getting bored
> : >
> : > "Don't the components of a buffer account for the buffering capacity?
> : Yes."
> : >
> : > Yes, agreed but you seem to fail what I'm saying. Buffering Capacity
and
> : Alkalinity are
> : > not the same, that has always been the issue. I gave the equation does
> : that look like an
> : > Alkalinity equation or how Alk is determined. I see you had now
comments
> : on it what's
> : > wrong, why no comments on the equations I gave. Don't understand them
or
> : what ? Again this
> : > is the equation for Buffering Capacity, also called Buffer Index or
Buffer
> : Intensity. It
> : > is defined in most water chemistry and chemical oceanography text
books.
> : >
> : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] +
CKa
> : [H3O+] / (Ka =
> : > H3O+])² )
> : >
> : > This is not Alkalinity now is it ?
> : >
> : > "I know how to do a titration, In fact I have done several. How many
have
> : > you actually done? I don't mean by counting drops, I mean with a
buret?"
> : >
> : > Well good for you, I use a Digital Titrator
> : >
> : > "Oh, I see,
> : > you think acidity is the opposite of alkalinity. In the world of
> : CHEMISTRY
> : > it's not. Maybe in aquarium newsgroups it is.
> : >
> : > Hum no, maybe you should go for a look at HACH's or LaMotte website or
the
> : book I
> : > suggested earlier. Please view a copy.
> : >
> : > Standard Methods for the Examination of Water and Wastewater
> : >
> : > This book, over 2000 pages, is the guide for water testing. If you are
> : reporting water
> : > test to the EPA you must use approved std from this text.I t is
prepared
> : and published by
> : > the EPA, American Water Works Association and American Public Health
> : Association. You
> : > mean you don't have one and the issue is water chemistry
> : >
> : > You are confusing Acidity and Acidity as you know little about water
> : chemistry and
> : > procedures and test methods
> : >
> : > From SMEWW, section 2-30, 2310 ACIDITY
> : >
> : > "Acidity of water is its quantative capacity to react with a strong
base
> : to a designated
> : > pH"
> : >
> : > This is how you test for it
> : >
> : > A std alkali titration to methyl orange or phenolphthalein
> : > endpoint.
> : >
> : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write
this
> : book, there are
> : > over 100 of them, they are wrong.
> : >
> : > Like Buffering Capacity you have your Acidity's mixed up
> : > In water measurement if you have a high Alk you also usually have a
high
> : Acidity.
> : > Normally a high Alk also gives a higher CO2 level. Get a WATER
CHEMISTRY
> : BOOK there pal.
> : >
> : >
> : > "These are all in equilibrium with each other. An initial high pH
(above
> : > 6.4) will shift the equilibrium to the right to form HCO3-1. If the
pH of
> : > the solution is above 10.3 (pKa2) the .........."
> : >
> : >
> : > Christ, there you go again with the FW ****. All your numbers are
wrong we
> : are dealing
> : > with SEAWATER
> : >
> : > This means that at a pH of 8.3, the majority of the CO2(aq) is in the
form
> : > of HCO3-1 .
> : >
> : > I have already pointed that out and gave actual values at know
seawater
> : levels, go back
> : > and re-read it you aren't telling me anything here.Of course most is
HCO3
> : see...
> : >
> : >
> : > @ 20C and 34.3 ppt salinity
> : >
> : > CO2 = 0.52 %
> : >
> : > HCO3 = 86.4 %
> : >
> : > CO3 = 13.09 %
> : >
> : >
> : > "In your glass experiment you managed to lower the pH enough to purge
out
> : CO2
> : > by boiling"
> : >
> : > The purpose behind the glass is to show that alk is not affect by CO2
and
> : vise-versa and
> : > how Co2 affects pH.
> : >
> : > Now, in a real life seawater aquarium, with a pH of 8.3 and that pH
drops
> : to say 8.1 it is
> : > usually due to excess CO2. If you took a glass of that water and
aerated
> : it you WILL drive
> : > off the CO2 and raise the pH. It has been done a proven a million
times.
> : >
> : > "In order to 'purge' CO2 you would need to lower the
> : > pH to shift the equilibrium to below 6.4"
> : >
> : > The hell you do !!!.Do you know who many times people on this NG to
> : include Dr. Craig
> : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
> : sample of aquarium
> : > water and aerate it to see if the pH GOES UP AND when they come back
with
> : the test it is
> : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST
excess
> : CO2 in the tank
> : > water, increase the circulation for better gas exchange at the
surface,
> : reduce feeding,
> : > and try to improve on better skimming, thus reducing the bio-load and
pH
> : decline due to
> : > CO2.
> : >
> : >
> : > "I hope this helps. "
> : >
> : > Help, how can you when you miss everything. I should be charging you
> : >
> : > Oh, by the way. Your websites, I have about 50 on these issues, I
could
> : post them, not to
> : > mention I have all those water chemistry books, so there is no need to
> : view your sites.
> : >
> : > Finally are you afraid to come to our Chemistry Forum, afraid to get
> : slapped by REAL
> : > chemists. I get a charge out of you can't post your ref .I have posted
the
> : same or similar
> : > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500
posts
> : there and am the
> : > biggest contributor to his forum other than himself or maybe Habib
Sheka
> : >
> : > Hum, here are Randy's ref that he posted. He hosts the website
> : >
> : > S. RANDY HOLMES-FARLEY
> : > Arlington, Massachusetts
> : >
> : > EDUCATION
> : >
> : > 1982-1986 Harvard University Cambridge, MA
> : > PhD in Chemistry
> : > Research Advisor: George Whitesides
> : >
> : > Investigated the relationship between polymer surface chemistry and
> : physical properties
> : > through controlled surface modification and testing.
> : >
> : > 1980-1982 Cornell University Ithaca, NY
> : > BA in Chemistry and Biology
> : > Graduated Summa Cum Laude
> : > Distinction in All Subjects
> : > Grade Point: 3.94/4.0
> : > Honors research: isolation and characterization of the subunit of CF1
> : enzyme
> : >
> : >
> : > 1978-1979 Stanford University Palo Alto, CA
> : > Grade Point: 3.55/4.0
> : >
> : >
> : > EXPERIENCE
> : >
> : > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> : > (bought out GelTex Pharmaceuticals in 2001)
> : > Vice President, Chemical Research 2001-present
> : > Senior Director, Chemical Research 1999-2001
> : > Director of Chemical Research 1997-1999
> : > Manager of Chemical Research 1995-1997
> : > Group Leader 1994-1995
> : > Senior Research Scientist 1992-1994
> : >
> : > Helped start GelTex as second employee
> : >
> : > Managed various research programs with multi-million dollar budgets
> : >
> : > Supervised research chemists (17+)
> : >
> : > Co-inventor of several polymeric pharmaceuticals and pharmaceutical
> : candidates including
> : > Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride
(FDA
> : approved)
> : >
> : > Company Safety Officer for 3 years
> : >
> : > Chemical Hygiene Officer 2000-present
> : >
> : >
> : >
> : >
> : > 1990-1992 GTE Corporation Waltham, MA
> : > Senior Member of Technical Staff
> : > Applied research involving polymer interfaces
> : > Metallization of plastics
> : > Polymer/polymer adhesion
> : > Optical coatings
> : >
> : >
> : >
> : > 1986-1990 Lord Corporation Cary, NC
> : > Senior Research Scientist 1988-1990
> : > Research Scientist 1986-1988
> : > Basic and applied research on surface chemical bonding
> : > Developed new adhesive compositions
> : > Developed new sol-gel coatings for corrosion resistance
> : >
> : >
> : > HONORS AND AWARDS
> : >
> : > Industrial Innovations Award by Northeast Region of American Chemical
> : Society (6/2001)
> : >
> : > National Kidney Foundation of Northern California Honoree (5/2001)
> : >
> : > American Chemical Society/Polymer Chemistry Division Industrial
Sponsors
> : > Award (8/2000)
> : >
> : > R&D 100 Award from R&D magazine (1999)
> : >
> : > Sherwin Williams Award in applied polymer science (9/85)
> : >
> : > IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
> : >
> : > Award for highest GPA in Chemistry Department (6/82)
> : >
> : > Summa Cum Laude Honors in Chemistry (6/82)
> : >
> : > Phi Lamda Epsilon (6/82)
> : >
> : > Phi Beta Kappa (2/82)
> : >
> : > Cornell University Dean's List (1981, 1982)
> : >
> : > Harvard Book Club Award for highest GPA senior year (1978)
> : >
> : > First Place in western NY ACS high school chemistry exam (1977)
> : >
> : > 1978-1979
> : >
> : >
> : > __________________
> : > Randy Holmes-Farley
> : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
> : >
> : > Hobby Experience: 8 years with reefs
> : > Current Tanks: 90 gal mixed reef
> : > Interests: Reefkeeping, science, photography
> : >
> : >
> : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> : >
> : > Open this post in a new window | Report this post to a moderator | IP:
> : Logged
> : >
> : >
> : >
> : > 06/27/2003 02:44 PM
> : >
> : > Randy Holmes-Farley
> : > Chemistry Moderator
> : >
> : > Registered: Apr 2001
> : > Location: Arlington, Massachusetts
> : > Occupation: Chemist (Drug Discovery at Genzyme)
> : > Posts: 15282
> : >
> : >
> : >
> : > Publications
> : >
> : >
> : > ISSUED UNITED STATES PATENTS
> : >
> : >
> : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
> : Mandeville, III; W. Harry.
> : > US 6,566,407; 5/20/2003
> : >
> : > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen
Randall;
> : Huval, Chad
> : > Cori.
> : > U.S. 6,517,825; 2/11/2003.
> : >
> : > 3. Method of making phosphate-binding polymers for oral
administration.
> : Holmes-Farley,
> : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
> : 6,509,013; 1/21/2003.
> : >
> : > 4. Combination therapy for treating hypercholesterolemia using a bile
acid
> : sequestrant
> : > polymer
> : > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley,
Stephen
> : Randall;
> : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> : >
> : > 5. Method for treating hypercholesterolemia with polyallylamine
polymers.
> : Holmes-Farley,
> : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
Goldberg,
> : Dennis I. , US
> : > 6,423,754; 7/23/2002.
> : >
> : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
> : Neenan, Thomas X..;
> : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> : >
> : > 7. Combination therapy for treating hypercholesterolemia and
> : atherosclerosis. Huval, Chad
> : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep
K.
> : U.S. 6,365,186;
> : > 4/2/2002.
> : >
> : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
Mandeville,
> : W. H., III;
> : > Huval; C.
> : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
> : 10/9/2001.
> : >
> : > 9. Polymers containing guanidinium groups as bile acid sequestrants.
Dhal;
> : P. K.; Holmes-
> : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> : >
> : > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III.; US
> : > 6,281,252;
> : > 8/28/2001.
> : >
> : > 11. Combination therapy for treating hypercholestrolemia. Huval; C.
C.;
> : Holmes-Farley; S.
> : > R. ;
> : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> : >
> : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
> : Holmes-Farley, S.
> : > R.; US
> : > 6,264,937; 7/24/2001.
> : >
> : > 13. Method for treating hypercholesterolemia with unsubstituted
> : polydiallylamine polymers.
> : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
> : 6,248,318;
> : > 6/19/2001.
> : >
> : > 14. Process for removing bile salts from a patient and alkylated
> : compositions therefore.
> : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
> : >
> : > 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S.
R.;
> : Dhal, P. K.;
> : > Petersen,
> : > J. S.; US 6,203,785; 3/20/2001.
> : >
> : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.;
Huval,
> : C. C.; US
> : > 6,190,649;
> : > 2/20/2001.
> : >
> : > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III.; US
> : > 6,177,478;
> : > 1/23/2001.
> : >
> : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
Holmes-Farley,
> : S. R.;
> : > Mandeville, W.
> : > H., III.; US 6,129,910; 10/10/2000.
> : >
> : > 19. Method for treating hypercholesterolemia with unsubstituted
> : polydiallylamine polymers.
> : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
> : 6,083,497;
> : > 7/4/2000.
> : >
> : > 20. Method of making phosphate-binding polymers for oral
administration.
> : Holmes-Farley, S.
> : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495;
7/4/2000.
> : >
> : > 21. Process for removing bile salts from a patient and alkylated
> : compositions therefore.
> : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
5/23/2000.
> : >
> : > 22. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> : >
> : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
> : Neenan; T. X.; Holmes-
> : > Farley; S. R. US 6,034,129; 3/7/2000.
> : >
> : > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III.; US
> : > 5,985,938;
> : > 11/16/99.
> : >
> : > 25. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> : >
> : > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W.
H.,
> : III.;
> : > Holmes-Farley;
> : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> : >
> : > 27. Hydrophilic nonamine-containing and amine-containing copolymers
and
> : their use as bile
> : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
5,929,184;
> : 7/27/99.
> : >
> : > 28. Interpenetrating polymer networks for sequestration of bile acids.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
> : 7/20/99.
> : >
> : > 29. Amine polymer sequestrant and method of cholesterol depletion.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> : >
> : > 30. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> : >
> : > 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> : >
> : > 32. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> : >
> : > 33. Preparation of polymeric sequestrants for bile acid salts.
Mandeville,
> : W. H., III.;
> : > Holmes-
> : > Farley, S. R.; US 5,703,188; 12/30/97.
> : >
> : > 34. Oral administration of iron-binding crosslinked amine polymers.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> : >
> : > 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley,
S.
> : R.; US 5,693,675;
> : > 12/2/97.
> : >
> : > 36. Method for removing bile salts from a patient with alkylated
> : crosslinked amine
> : > polymers,
> : > and preparation of the polymers. Mandeville, W. H., III.;
Holmes-Farley,
> : S. R.; US
> : > 5,679,717; 10/21/97.
> : >
> : > 37. Phosphate-binding polymers for oral administration. Holmes-Farley,
S.
> : R.; Mandeville,
> : > W.
> : > H., III.; US 5,667,775; 9/16/97.
> : >
> : > 38. Ion-exchange process using highly crosslinked polymers for
removing
> : bile salts from a
> : > patient, preparation of the polymers, and compositions containing
them.
> : Mandeville, W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> : >
> : > 39. Hydrophobic amine polymer sequestrant and method of cholesterol
> : depletion. Mandeville,
> : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530;
4/8/97.
> : >
> : > 40. Amine polymer sequestrant and method of cholesterol depletion.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> : >
> : > 41. Phosphate-binding polymers for oral administration. Holmes-Farley,
S.
> : R.; Mandeville,
> : > W.
> : > H., III.; US 5,496,545; 3/5/96.
> : >
> : > 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
> : III.; Holmes-Farley,
> : > S. R.;
> : > US 5,487,888; 1/30/96.
> : >
> : > 43. Ultra-thin, uniform sol-gel coating of a substrate having active
> : hydrogens on the
> : > surface.
> : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> : >
> : > 44. Layered sol-gel coatings from organisilicon compounds.
Holmes-Farley,
> : S. R.; Yanyo, L.
> : > C.;
> : > US 5,182,143; 1/26/93.
> : >
> : > 45. Method for metal bonding using ultrathin primer coating.
> : Holmes-Farley, S. R.; Yanyo,
> : > L.
> : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> : >
> : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.;
US
> : 5,096,962;
> : > 3/17/92.
> : >
> : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> : elastomer-metal bonding.
> : > Holmes-
> : > Farley, S. R.; US 5,102,956; 4/7/92.
> : >
> : >
> : >
> : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
> : >
> : >
> : > 1. Aryl boronate functionalized polymers for treating obesity and
> : inhibiting fat uptake.
> : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal,
Pradeep
> : K.; Huval, Chad
> : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92
pp. WO
> : 0302571.
> : >
> : > 2. Preparation of aryl boronic acids for treating obesity.
Holmes-Farley,
> : Stephen Randall;
> : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep
K.
> : (Geltex
> : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
> : >
> : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
> : Stephen Randall.
> : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
> : 0302130.
> : >
> : > 4. Method for reducing copper levels and treating copper toxicosis.
> : Holmes-Farley, Stephen
> : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002),
45
> : pp. WO
> : > 0285383.
> : >
> : > 5. Method for treating gout and binding uric acid. Holmes-Farley,
Stephen
> : Randall; Burke,
> : > Steven K. WO 0285381 10/31/2002.
> : >
> : > 6. Method for treating gout and reducing serum uric acid.
Holmes-Farley,
> : Stephen Randall;
> : > Burke, Steven K WO 0285380 10/31/2002.
> : >
> : > 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
> : Holmes-Farley, S. R.;
> : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> : >
> : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
> : Holmes-Farley, S.
> : > R.;
> : > WO 1999-US5662; 9/23/1999.
> : >
> : > 9. Amine-containing copolymers as bile acid sequestrants.
Holmes-Farley,
> : S. R.; Petersen,
> : > J. S.;
> : > WO 9933452; 7/8/1999.
> : >
> : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III
and
> : Holmes-Farley, S.
> : > R.;
> : > WO 9922743; 5/14/1999.
> : >
> : > 11. Polyallylamine polymers for removing bile salts and treating
> : hypercholesterolemia, and
> : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III;
Burke,
> : S. K.; Goldberg,
> : > D. I.; WO 9857652; 12/23/98.
> : >
> : > 12. Phosphate-bidning polymers combined with a calcium supplement for
oral
> : administration.
> : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley,
S.
> : R.; WO 9842355;
> : > 10/1/98.
> : >
> : > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
> : depletion. Mandeville,
> : > W.
> : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
> : >
> : > 14. Process for adjusting ion concentration in a patient and
compositions
> : therefor.
> : > Mandeville,
> : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> : >
> : > 15. Vacuum-deposited silver on polycarbonate with a chromium
interlayer
> : for improved
> : > metal-
> : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
1/20/94.
> : >
> : > 16. Process for increased metal-substrate bond strength in metalized
> : plastics.
> : > Holmes-Farley, S.
> : > R.; Ger. Offen. 4322516; 7/6/93.
> : >
> : > 17. Electrorheological fluids and preparation of particles useful in
the
> : fluids.
> : > Troughton,
> : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
> : David; Bares, Joseph
> : > E.;
> : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
> : 394049;
> : > 10/24/1990.
> : >
> : > JOURNAL PUBLICATIONS
> : >
> : > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov,
Eugene;
> : Guo, Amy;
> : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
> : Mandeville, W. Harry;
> : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
611-619.
> : >
> : > 2. Amine functionalized polyethers as bile acid sequestrants:
synthesis
> : and biological
> : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S.
Randall;
> : Mandeville, W.
> : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
> : Journal of
> : > Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
> : 1559-1574.
> : >
> : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
> : Imprinting. Huval,
> : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
> : Randall; Mandeville,
> : > W.
> : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert
J.;
> : Chen, Xi; Dhal,
> : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> : >
> : > 4. Synthetic polymers for the binding of fat in the intestinal tract.
> : Jozefiak, Thomas H.;
> : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia;
Huval,
> : Chad C.;
> : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
> : Abstracts of
> : > Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
> : 26-30, 2001
> : > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
> : Division of
> : > Polymer Chemistry) (2001), 42(2), 98.
> : >
> : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer
gel
> : pharmaceutical.
> : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.;
Ward,
> : J.; Sacchiero,
> : > B.;
> : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.;
Chen,
> : X.; Mazzeo, J.
> : > R.. Polym. Preprints (2000), 41(1), 735-736.
> : >
> : > 6. In vitro comparison of bile acid binding to colesevelam HCl and
other
> : bile acid
> : > sequestrants.
> : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
> : Hook, P.; Holmes-
> : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
> : >
> : > 7. Novel polymeric pharmaceuticals: From startup to market.
Holmes-Farley,
> : S. R; Polym.
> : > Mater. Sci. Eng (1999), 80, 246-247.
> : >
> : > 8. Design and characterization of of Sevelamer Hydrochloride: a novel
> : phosphate-binding
> : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward,
J.;
> : Miller, K. L.;
> : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure
and
> : Appl. Chem.,
> : > A36(7&8), p. 1085 (1999).
> : >
> : > 9. Three generations of bile acid sequestrants. Mandeville, W. H.,
III;
> : Braunlin, W.;
> : > Dhal, P.;
> : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
> : Rosenbaum, D.;
> : > Sacchiero,
> : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
> : 550, 3-15.
> : >
> : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric
phosphate
> : binder, on
> : > urinary
> : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
> : Mandeville, W. H.,
> : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
> : (1997), 12(5)
> : > 961-964.
> : >
> : > 11. Thin anisotropic coatings based on sol-gel technology.
Holmes-Farley,
> : S. R.; Yanyo, L.
> : > C;
> : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4),
439-444.
> : >
> : > 12. The mechanism of cure initiation of a surface activated adhesive.
> : Holmes-Farley, S.
> : > R.;
> : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
> : >
> : > 13. Adhesion promotion and corrosion prevention using thin anisotropic
> : coatings. Holmes-
> : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
> : 131-151.
> : >
> : > 14. Wetting of functionalized polyethylene having ionizable organic
acids
> : and bases at the
> : > polymer-water interface: relations between functional group polarity,
> : extent of
> : > ionization,
> : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
> : Whitesides, G. M.;
> : > Langmuir
> : > (1988), 4(4), 921-937.
> : >
> : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
> : single hydroxy group.
> : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> : >
> : > 16. Reconstruction of the interface of oxidatively functionalized
> : polyethylene (PE-CO2H)
> : > and
> : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo,
R.;
> : McCarthy, T. J.;
> : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report
(1987),
> : AD-
> : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> : >
> : > 17. Surface-modified polyethylene film: the relationship between
surface
> : chemistry and
> : > physical
> : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11),
4537.
> : >
> : > 18. Reactivity of carboxylic acid and ester groups in the
functionalized
> : interfacial
> : > region of
> : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> : differentiation of the
> : > functional groups into shallow and deep subsets based on a comparison
of
> : contact angle and
> : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
> : (1987), 3(1), 62-
> : > 76.
> : >
> : > 19. Fluorescence properties of dansyl groups covalently bonded tot he
> : surface of
> : > oxidatively
> : > functionalized low-density polyethylene film. Holmes-Farley, S. R.;
> : Whitesides, G. M.;
> : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
> : AD-A162435/2/GAR,
> : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> : >
> : > 20. Acid-base behavior of carboxylic acid groups covalently attached
at
> : the surface of
> : > polyethylene: The usefulness of contact angle in following the
ionization
> : of surface
> : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
> : Deutch, J.;
> : > Whitesides,
> : > G. M.; Langmuir (1985), 1(6), 725-740.
> : >
> : > 21. The thermal stability of a surface modified solid organic polymer.
> : Holmes-Farley, S.
> : > R.;
> : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
> : >
> : >
> : >
> : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> : >
> : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
> : Aquarist. June 2003.
> : >
> : > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
> : Advanced Aquarist.
> : > May
> : > 2003.
> : >
> : > 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
> : Reefkeeping May
> : > 2003.
> : >
> : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
> : April 2003.
> : >
> : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> : Holmes-Farley, R.
> : > Advanced Aquarist; April 2003.
> : >
> : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> : Holmes-Farley, R.
> : > Advanced Aquarist; April 2003.
> : >
> : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced
Aquarist;
> : March 2003.
> : >
> : > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
> : Holmes-Farley, R.
> : > Advanced Aquarist; February 2003.
> : >
> : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
> : 2003.
> : >
> : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
December
> : 2002.
> : >
> : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
Advanced
> : Aquarist; November
> : > 2002.
> : >
> : > 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
> : Advanced Aquarist;
> : > November 2002.
> : >
> : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced
Aquarist,
> : September 2002.
> : >
> : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
> : 2002.
> : >
> : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
> : 2002.
> : >
> : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
> : Aquarist; July 2002
> : >
> : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist;
June
> : 2002.
> : >
> : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R.
Advanced
> : Aquarist, May
> : > 2002.
> : >
> : > 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
> : Holmes-Farley, R.
> : > Advanced Aquarist, April 2002.
> : >
> : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> : >
> : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
> : >
> : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January
2002.
> : >
> : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
> : 2000.
> : >
> : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
> : Frontiers 2000.
> : >
> : > 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
> : Aquarium Frontiers
> : > 2000.
> : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
Frontiers
> : 2000.
> : >
> : > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers
2000.
> : >
> : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
> : >
> : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> : >
> : >
> : >
> : >
> : >
> : >
> : >
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : >
> : >
> :
> :
>
>

[stoutman]

Good one Dragon Slayer. Do people STILL play D&D?????????????


"Dragon Slayer" > wrote in message
...
>
> "Boomer" > wrote in message
> ...
>
>
> > Do a dam search on them or shut the hell up.
>
> I'll second that.
>
> kc
>
>

[stoutman]

I want sure were you got that from, but I see now.

My reply is response to your CITED WEB PAGE's definition of alkalinity.

Alkalinity:
Acid neutralizing or buffering capacity of water; a measure of the ability
of water to resist changes in pH caused by the addition of acids or bases




"stoutman" <.@.> wrote in message news:1YuWb.273293$I06.2926488@attbi_s01...
> >Alkalinity a measure of the amount of anions of weak acid in water and of
> the cations balanced against them
> >Take note it says ***acid***
>
> Take note, it also says ***bases***
>
> Acid neutralizing or buffering capacity of water; a measure of the ability
> of water to resist changes in pH caused by the addition of acids or bases
>
>
>
> maybe this is the problem. Boomer do you know what a base is?
>
>
>
>
>
>
> "Boomer" > wrote in message
> ...
> > Alkalinity a measure of the amount of anions of weak acid in water and
of
> the cations
> > balanced against them
> > Take note it says ***acid***
> >
> > Buffering capacity the ability of a solution to resist or dampen changes
> in pH upon the
> > addition of acids or bases.
> > Take note its says ***the addition of acids or bases***
> >
> > One more
> >
> > http://www.waterontheweb.org/resources/glossary.html
> >
> > We could go on like this all day, so what is the point ?
> >
> > You will LOVE this one
> > http://www.kyantec.com/Tips/phbuffering.htm
> >
> > Don't you just lovbe PDF's
> > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
> >
> > Don't fall out of your chair
> > http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
> >
> >
> >
> >
> > --
> > Boomer
> >
> > Want to talk chemistry ? The Reef Chemistry Forum
> > http://www.reefcentral.com/vbulletin/index.php
> >
> > Want to See More ?
> > Please Join Our Growing Membership
> > www.coralrealm.com
> >
> > If You See Me Running You Better Catch-Up
> > "stoutman" <.@.> wrote in message
news:XB7Wb.19339$QA2.62332@attbi_s52...
> > : Man here is another, google is a wonderful thing. I'm not filtering
any
> > : out, just posting what I find by GOOGLING for you.
> > :
> > : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> > :
> > :
> > : Wow, a gov link. Even the government is wrong, this must be a
> conspiracy
> > : against Boomer.
> > :
> > :
> > :
> > :
> > : "Boomer" > wrote in message
> > : ...
> > : > Now I am getting bored
> > : >
> > : > "Don't the components of a buffer account for the buffering
capacity?
> > : Yes."
> > : >
> > : > Yes, agreed but you seem to fail what I'm saying. Buffering Capacity
> and
> > : Alkalinity are
> > : > not the same, that has always been the issue. I gave the equation
does
> > : that look like an
> > : > Alkalinity equation or how Alk is determined. I see you had now
> comments
> > : on it what's
> > : > wrong, why no comments on the equations I gave. Don't understand
them
> or
> > : what ? Again this
> > : > is the equation for Buffering Capacity, also called Buffer Index or
> Buffer
> > : Intensity. It
> > : > is defined in most water chemistry and chemical oceanography text
> books.
> > : >
> > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] +
> CKa
> > : [H3O+] / (Ka =
> > : > H3O+])² )
> > : >
> > : > This is not Alkalinity now is it ?
> > : >
> > : > "I know how to do a titration, In fact I have done several. How
many
> have
> > : > you actually done? I don't mean by counting drops, I mean with a
> buret?"
> > : >
> > : > Well good for you, I use a Digital Titrator
> > : >
> > : > "Oh, I see,
> > : > you think acidity is the opposite of alkalinity. In the world of
> > : CHEMISTRY
> > : > it's not. Maybe in aquarium newsgroups it is.
> > : >
> > : > Hum no, maybe you should go for a look at HACH's or LaMotte website
or
> the
> > : book I
> > : > suggested earlier. Please view a copy.
> > : >
> > : > Standard Methods for the Examination of Water and Wastewater
> > : >
> > : > This book, over 2000 pages, is the guide for water testing. If you
are
> > : reporting water
> > : > test to the EPA you must use approved std from this text.I t is
> prepared
> > : and published by
> > : > the EPA, American Water Works Association and American Public Health
> > : Association. You
> > : > mean you don't have one and the issue is water chemistry
> > : >
> > : > You are confusing Acidity and Acidity as you know little about water
> > : chemistry and
> > : > procedures and test methods
> > : >
> > : > From SMEWW, section 2-30, 2310 ACIDITY
> > : >
> > : > "Acidity of water is its quantative capacity to react with a strong
> base
> > : to a designated
> > : > pH"
> > : >
> > : > This is how you test for it
> > : >
> > : > A std alkali titration to methyl orange or phenolphthalein
> > : > endpoint.
> > : >
> > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write
> this
> > : book, there are
> > : > over 100 of them, they are wrong.
> > : >
> > : > Like Buffering Capacity you have your Acidity's mixed up
> > : > In water measurement if you have a high Alk you also usually have a
> high
> > : Acidity.
> > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
> CHEMISTRY
> > : BOOK there pal.
> > : >
> > : >
> > : > "These are all in equilibrium with each other. An initial high pH
> (above
> > : > 6.4) will shift the equilibrium to the right to form HCO3-1. If the
> pH of
> > : > the solution is above 10.3 (pKa2) the .........."
> > : >
> > : >
> > : > Christ, there you go again with the FW ****. All your numbers are
> wrong we
> > : are dealing
> > : > with SEAWATER
> > : >
> > : > This means that at a pH of 8.3, the majority of the CO2(aq) is in
the
> form
> > : > of HCO3-1 .
> > : >
> > : > I have already pointed that out and gave actual values at know
> seawater
> > : levels, go back
> > : > and re-read it you aren't telling me anything here.Of course most is
> HCO3
> > : see...
> > : >
> > : >
> > : > @ 20C and 34.3 ppt salinity
> > : >
> > : > CO2 = 0.52 %
> > : >
> > : > HCO3 = 86.4 %
> > : >
> > : > CO3 = 13.09 %
> > : >
> > : >
> > : > "In your glass experiment you managed to lower the pH enough to
purge
> out
> > : CO2
> > : > by boiling"
> > : >
> > : > The purpose behind the glass is to show that alk is not affect by
CO2
> and
> > : vise-versa and
> > : > how Co2 affects pH.
> > : >
> > : > Now, in a real life seawater aquarium, with a pH of 8.3 and that pH
> drops
> > : to say 8.1 it is
> > : > usually due to excess CO2. If you took a glass of that water and
> aerated
> > : it you WILL drive
> > : > off the CO2 and raise the pH. It has been done a proven a million
> times.
> > : >
> > : > "In order to 'purge' CO2 you would need to lower the
> > : > pH to shift the equilibrium to below 6.4"
> > : >
> > : > The hell you do !!!.Do you know who many times people on this NG to
> > : include Dr. Craig
> > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take
a
> > : sample of aquarium
> > : > water and aerate it to see if the pH GOES UP AND when they come back
> with
> > : the test it is
> > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST
> excess
> > : CO2 in the tank
> > : > water, increase the circulation for better gas exchange at the
> surface,
> > : reduce feeding,
> > : > and try to improve on better skimming, thus reducing the bio-load
and
> pH
> > : decline due to
> > : > CO2.
> > : >
> > : >
> > : > "I hope this helps. "
> > : >
> > : > Help, how can you when you miss everything. I should be charging you
> > : >
> > : > Oh, by the way. Your websites, I have about 50 on these issues, I
> could
> > : post them, not to
> > : > mention I have all those water chemistry books, so there is no need
to
> > : view your sites.
> > : >
> > : > Finally are you afraid to come to our Chemistry Forum, afraid to get
> > : slapped by REAL
> > : > chemists. I get a charge out of you can't post your ref .I have
posted
> the
> > : same or similar
> > : > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500
> posts
> > : there and am the
> > : > biggest contributor to his forum other than himself or maybe Habib
> Sheka
> > : >
> > : > Hum, here are Randy's ref that he posted. He hosts the website
> > : >
> > : > S. RANDY HOLMES-FARLEY
> > : > Arlington, Massachusetts
> > : >
> > : > EDUCATION
> > : >
> > : > 1982-1986 Harvard University Cambridge, MA
> > : > PhD in Chemistry
> > : > Research Advisor: George Whitesides
> > : >
> > : > Investigated the relationship between polymer surface chemistry and
> > : physical properties
> > : > through controlled surface modification and testing.
> > : >
> > : > 1980-1982 Cornell University Ithaca, NY
> > : > BA in Chemistry and Biology
> > : > Graduated Summa Cum Laude
> > : > Distinction in All Subjects
> > : > Grade Point: 3.94/4.0
> > : > Honors research: isolation and characterization of the subunit of
CF1
> > : enzyme
> > : >
> > : >
> > : > 1978-1979 Stanford University Palo Alto, CA
> > : > Grade Point: 3.55/4.0
> > : >
> > : >
> > : > EXPERIENCE
> > : >
> > : > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> > : > (bought out GelTex Pharmaceuticals in 2001)
> > : > Vice President, Chemical Research 2001-present
> > : > Senior Director, Chemical Research 1999-2001
> > : > Director of Chemical Research 1997-1999
> > : > Manager of Chemical Research 1995-1997
> > : > Group Leader 1994-1995
> > : > Senior Research Scientist 1992-1994
> > : >
> > : > Helped start GelTex as second employee
> > : >
> > : > Managed various research programs with multi-million dollar budgets
> > : >
> > : > Supervised research chemists (17+)
> > : >
> > : > Co-inventor of several polymeric pharmaceuticals and pharmaceutical
> > : candidates including
> > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride
> (FDA
> > : approved)
> > : >
> > : > Company Safety Officer for 3 years
> > : >
> > : > Chemical Hygiene Officer 2000-present
> > : >
> > : >
> > : >
> > : >
> > : > 1990-1992 GTE Corporation Waltham, MA
> > : > Senior Member of Technical Staff
> > : > Applied research involving polymer interfaces
> > : > Metallization of plastics
> > : > Polymer/polymer adhesion
> > : > Optical coatings
> > : >
> > : >
> > : >
> > : > 1986-1990 Lord Corporation Cary, NC
> > : > Senior Research Scientist 1988-1990
> > : > Research Scientist 1986-1988
> > : > Basic and applied research on surface chemical bonding
> > : > Developed new adhesive compositions
> > : > Developed new sol-gel coatings for corrosion resistance
> > : >
> > : >
> > : > HONORS AND AWARDS
> > : >
> > : > Industrial Innovations Award by Northeast Region of American
Chemical
> > : Society (6/2001)
> > : >
> > : > National Kidney Foundation of Northern California Honoree (5/2001)
> > : >
> > : > American Chemical Society/Polymer Chemistry Division Industrial
> Sponsors
> > : > Award (8/2000)
> > : >
> > : > R&D 100 Award from R&D magazine (1999)
> > : >
> > : > Sherwin Williams Award in applied polymer science (9/85)
> > : >
> > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
> > : >
> > : > Award for highest GPA in Chemistry Department (6/82)
> > : >
> > : > Summa Cum Laude Honors in Chemistry (6/82)
> > : >
> > : > Phi Lamda Epsilon (6/82)
> > : >
> > : > Phi Beta Kappa (2/82)
> > : >
> > : > Cornell University Dean's List (1981, 1982)
> > : >
> > : > Harvard Book Club Award for highest GPA senior year (1978)
> > : >
> > : > First Place in western NY ACS high school chemistry exam (1977)
> > : >
> > : > 1978-1979
> > : >
> > : >
> > : > __________________
> > : > Randy Holmes-Farley
> > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
> > : >
> > : > Hobby Experience: 8 years with reefs
> > : > Current Tanks: 90 gal mixed reef
> > : > Interests: Reefkeeping, science, photography
> > : >
> > : >
> > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> > : >
> > : > Open this post in a new window | Report this post to a moderator |
IP:
> > : Logged
> > : >
> > : >
> > : >
> > : > 06/27/2003 02:44 PM
> > : >
> > : > Randy Holmes-Farley
> > : > Chemistry Moderator
> > : >
> > : > Registered: Apr 2001
> > : > Location: Arlington, Massachusetts
> > : > Occupation: Chemist (Drug Discovery at Genzyme)
> > : > Posts: 15282
> > : >
> > : >
> > : >
> > : > Publications
> > : >
> > : >
> > : > ISSUED UNITED STATES PATENTS
> > : >
> > : >
> > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
> > : Mandeville, III; W. Harry.
> > : > US 6,566,407; 5/20/2003
> > : >
> > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen
> Randall;
> > : Huval, Chad
> > : > Cori.
> > : > U.S. 6,517,825; 2/11/2003.
> > : >
> > : > 3. Method of making phosphate-binding polymers for oral
> administration.
> > : Holmes-Farley,
> > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
> > : 6,509,013; 1/21/2003.
> > : >
> > : > 4. Combination therapy for treating hypercholesterolemia using a
bile
> acid
> > : sequestrant
> > : > polymer
> > : > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley,
> Stephen
> > : Randall;
> > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> > : >
> > : > 5. Method for treating hypercholesterolemia with polyallylamine
> polymers.
> > : Holmes-Farley,
> > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
> Goldberg,
> > : Dennis I. , US
> > : > 6,423,754; 7/23/2002.
> > : >
> > : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry,
III;
> > : Neenan, Thomas X..;
> > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> > : >
> > : > 7. Combination therapy for treating hypercholesterolemia and
> > : atherosclerosis. Huval, Chad
> > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal,
Pradeep
> K.
> > : U.S. 6,365,186;
> > : > 4/2/2002.
> > : >
> > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
> Mandeville,
> > : W. H., III;
> > : > Huval; C.
> > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
> > : 10/9/2001.
> > : >
> > : > 9. Polymers containing guanidinium groups as bile acid sequestrants.
> Dhal;
> > : P. K.; Holmes-
> > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> > : >
> > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville,
W.
> H.,
> > : III.; US
> > : > 6,281,252;
> > : > 8/28/2001.
> > : >
> > : > 11. Combination therapy for treating hypercholestrolemia. Huval; C.
> C.;
> > : Holmes-Farley; S.
> > : > R. ;
> > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> > : >
> > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G.
M.;
> > : Holmes-Farley, S.
> > : > R.; US
> > : > 6,264,937; 7/24/2001.
> > : >
> > : > 13. Method for treating hypercholesterolemia with unsubstituted
> > : polydiallylamine polymers.
> > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ;
US
> > : 6,248,318;
> > : > 6/19/2001.
> > : >
> > : > 14. Process for removing bile salts from a patient and alkylated
> > : compositions therefore.
> > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355;
5/1/2001.
> > : >
> > : > 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley,
S.
> R.;
> > : Dhal, P. K.;
> > : > Petersen,
> > : > J. S.; US 6,203,785; 3/20/2001.
> > : >
> > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.;
> Huval,
> > : C. C.; US
> > : > 6,190,649;
> > : > 2/20/2001.
> > : >
> > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville,
W.
> H.,
> > : III.; US
> > : > 6,177,478;
> > : > 1/23/2001.
> > : >
> > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
> Holmes-Farley,
> > : S. R.;
> > : > Mandeville, W.
> > : > H., III.; US 6,129,910; 10/10/2000.
> > : >
> > : > 19. Method for treating hypercholesterolemia with unsubstituted
> > : polydiallylamine polymers.
> > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ;
US
> > : 6,083,497;
> > : > 7/4/2000.
> > : >
> > : > 20. Method of making phosphate-binding polymers for oral
> administration.
> > : Holmes-Farley, S.
> > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495;
> 7/4/2000.
> > : >
> > : > 21. Process for removing bile salts from a patient and alkylated
> > : compositions therefore.
> > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
> 5/23/2000.
> > : >
> > : > 22. Process for removing bile salts from a patient and compositions
> > : therefor. Mandeville,
> > : > W. H.,
> > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> > : >
> > : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
> > : Neenan; T. X.; Holmes-
> > : > Farley; S. R. US 6,034,129; 3/7/2000.
> > : >
> > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville,
W.
> H.,
> > : III.; US
> > : > 5,985,938;
> > : > 11/16/99.
> > : >
> > : > 25. Process for removing bile salts from a patient and compositions
> > : therefor. Mandeville,
> > : > W. H.,
> > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> > : >
> > : > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville,
W.
> H.,
> > : III.;
> > : > Holmes-Farley;
> > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> > : >
> > : > 27. Hydrophilic nonamine-containing and amine-containing copolymers
> and
> > : their use as bile
> > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
> 5,929,184;
> > : 7/27/99.
> > : >
> > : > 28. Interpenetrating polymer networks for sequestration of bile
acids.
> > : Mandeville, W. H.,
> > : > III.;
> > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
> > : 7/20/99.
> > : >
> > : > 29. Amine polymer sequestrant and method of cholesterol depletion.
> > : Mandeville, W. H.,
> > : > III.;
> > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> > : >
> > : > 30. Process for removing bile salts from a patient and compositions
> > : therefor. Mandeville,
> > : > W. H.,
> > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> > : >
> > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
depletion.
> > : Mandeville, W. H.,
> > : > III.;
> > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> > : >
> > : > 32. Process for removing bile salts from a patient and compositions
> > : therefor. Mandeville,
> > : > W. H.,
> > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> > : >
> > : > 33. Preparation of polymeric sequestrants for bile acid salts.
> Mandeville,
> > : W. H., III.;
> > : > Holmes-
> > : > Farley, S. R.; US 5,703,188; 12/30/97.
> > : >
> > : > 34. Oral administration of iron-binding crosslinked amine polymers.
> > : Mandeville, W. H.,
> > : > III.;
> > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> > : >
> > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
Holmes-Farley,
> S.
> > : R.; US 5,693,675;
> > : > 12/2/97.
> > : >
> > : > 36. Method for removing bile salts from a patient with alkylated
> > : crosslinked amine
> > : > polymers,
> > : > and preparation of the polymers. Mandeville, W. H., III.;
> Holmes-Farley,
> > : S. R.; US
> > : > 5,679,717; 10/21/97.
> > : >
> > : > 37. Phosphate-binding polymers for oral administration.
Holmes-Farley,
> S.
> > : R.; Mandeville,
> > : > W.
> > : > H., III.; US 5,667,775; 9/16/97.
> > : >
> > : > 38. Ion-exchange process using highly crosslinked polymers for
> removing
> > : bile salts from a
> > : > patient, preparation of the polymers, and compositions containing
> them.
> > : Mandeville, W. H.,
> > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> > : >
> > : > 39. Hydrophobic amine polymer sequestrant and method of cholesterol
> > : depletion. Mandeville,
> > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530;
> 4/8/97.
> > : >
> > : > 40. Amine polymer sequestrant and method of cholesterol depletion.
> > : Mandeville, W. H.,
> > : > III.;
> > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> > : >
> > : > 41. Phosphate-binding polymers for oral administration.
Holmes-Farley,
> S.
> > : R.; Mandeville,
> > : > W.
> > : > H., III.; US 5,496,545; 3/5/96.
> > : >
> > : > 42. Iron-binding polymers for oral administration. Mandeville, W.
H.,
> > : III.; Holmes-Farley,
> > : > S. R.;
> > : > US 5,487,888; 1/30/96.
> > : >
> > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having active
> > : hydrogens on the
> > : > surface.
> > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> > : >
> > : > 44. Layered sol-gel coatings from organisilicon compounds.
> Holmes-Farley,
> > : S. R.; Yanyo, L.
> > : > C.;
> > : > US 5,182,143; 1/26/93.
> > : >
> > : > 45. Method for metal bonding using ultrathin primer coating.
> > : Holmes-Farley, S. R.; Yanyo,
> > : > L.
> > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> > : >
> > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K.
J.;
> US
> > : 5,096,962;
> > : > 3/17/92.
> > : >
> > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> > : elastomer-metal bonding.
> > : > Holmes-
> > : > Farley, S. R.; US 5,102,956; 4/7/92.
> > : >
> > : >
> > : >
> > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
> > : >
> > : >
> > : > 1. Aryl boronate functionalized polymers for treating obesity and
> > : inhibiting fat uptake.
> > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal,
> Pradeep
> > : K.; Huval, Chad
> > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92
> pp. WO
> > : 0302571.
> > : >
> > : > 2. Preparation of aryl boronic acids for treating obesity.
> Holmes-Farley,
> > : Stephen Randall;
> > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal,
Pradeep
> K.
> > : (Geltex
> > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO
0302570.
> > : >
> > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
> > : Stephen Randall.
> > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp.
WO
> > : 0302130.
> > : >
> > : > 4. Method for reducing copper levels and treating copper toxicosis.
> > : Holmes-Farley, Stephen
> > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002),
> 45
> > : pp. WO
> > : > 0285383.
> > : >
> > : > 5. Method for treating gout and binding uric acid. Holmes-Farley,
> Stephen
> > : Randall; Burke,
> > : > Steven K. WO 0285381 10/31/2002.
> > : >
> > : > 6. Method for treating gout and reducing serum uric acid.
> Holmes-Farley,
> > : Stephen Randall;
> > : > Burke, Steven K WO 0285380 10/31/2002.
> > : >
> > : > 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
> > : Holmes-Farley, S. R.;
> > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> > : >
> > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III
and
> > : Holmes-Farley, S.
> > : > R.;
> > : > WO 1999-US5662; 9/23/1999.
> > : >
> > : > 9. Amine-containing copolymers as bile acid sequestrants.
> Holmes-Farley,
> > : S. R.; Petersen,
> > : > J. S.;
> > : > WO 9933452; 7/8/1999.
> > : >
> > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III
> and
> > : Holmes-Farley, S.
> > : > R.;
> > : > WO 9922743; 5/14/1999.
> > : >
> > : > 11. Polyallylamine polymers for removing bile salts and treating
> > : hypercholesterolemia, and
> > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III;
> Burke,
> > : S. K.; Goldberg,
> > : > D. I.; WO 9857652; 12/23/98.
> > : >
> > : > 12. Phosphate-bidning polymers combined with a calcium supplement
for
> oral
> > : administration.
> > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
Holmes-Farley,
> S.
> > : R.; WO 9842355;
> > : > 10/1/98.
> > : >
> > : > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
> > : depletion. Mandeville,
> > : > W.
> > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449;
12/12/96.
> > : >
> > : > 14. Process for adjusting ion concentration in a patient and
> compositions
> > : therefor.
> > : > Mandeville,
> > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> > : >
> > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
> interlayer
> > : for improved
> > : > metal-
> > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
> 1/20/94.
> > : >
> > : > 16. Process for increased metal-substrate bond strength in metalized
> > : plastics.
> > : > Holmes-Farley, S.
> > : > R.; Ger. Offen. 4322516; 7/6/93.
> > : >
> > : > 17. Electrorheological fluids and preparation of particles useful in
> the
> > : fluids.
> > : > Troughton,
> > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
> > : David; Bares, Joseph
> > : > E.;
> > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell.
EP
> > : 394049;
> > : > 10/24/1990.
> > : >
> > : > JOURNAL PUBLICATIONS
> > : >
> > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov,
> Eugene;
> > : Guo, Amy;
> > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
> > : Mandeville, W. Harry;
> > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
> 611-619.
> > : >
> > : > 2. Amine functionalized polyethers as bile acid sequestrants:
> synthesis
> > : and biological
> > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S.
> Randall;
> > : Mandeville, W.
> > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
> > : Journal of
> > : > Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
> > : 1559-1574.
> > : >
> > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
> > : Imprinting. Huval,
> > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
> > : Randall; Mandeville,
> > : > W.
> > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert
> J.;
> > : Chen, Xi; Dhal,
> > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> > : >
> > : > 4. Synthetic polymers for the binding of fat in the intestinal
tract.
> > : Jozefiak, Thomas H.;
> > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia;
> Huval,
> > : Chad C.;
> > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
> > : Abstracts of
> > : > Papers, 222nd ACS National Meeting, Chicago, IL, United States,
August
> > : 26-30, 2001
> > : > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
> > : Division of
> > : > Polymer Chemistry) (2001), 42(2), 98.
> > : >
> > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel
polymer
> gel
> > : pharmaceutical.
> > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.;
> Ward,
> > : J.; Sacchiero,
> > : > B.;
> > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.;
> Chen,
> > : X.; Mazzeo, J.
> > : > R.. Polym. Preprints (2000), 41(1), 735-736.
> > : >
> > : > 6. In vitro comparison of bile acid binding to colesevelam HCl and
> other
> > : bile acid
> > : > sequestrants.
> > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu,
Q.;
> > : Hook, P.; Holmes-
> > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1),
708-709.
> > : >
> > : > 7. Novel polymeric pharmaceuticals: From startup to market.
> Holmes-Farley,
> > : S. R; Polym.
> > : > Mater. Sci. Eng (1999), 80, 246-247.
> > : >
> > : > 8. Design and characterization of of Sevelamer Hydrochloride: a
novel
> > : phosphate-binding
> > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward,
> J.;
> > : Miller, K. L.;
> > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pur
e
> and
> > : Appl. Chem.,
> > : > A36(7&8), p. 1085 (1999).
> > : >
> > : > 9. Three generations of bile acid sequestrants. Mandeville, W. H.,
> III;
> > : Braunlin, W.;
> > : > Dhal, P.;
> > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
> > : Rosenbaum, D.;
> > : > Sacchiero,
> > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc.
(1999),
> > : 550, 3-15.
> > : >
> > : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric
> phosphate
> > : binder, on
> > : > urinary
> > : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S.
R.;
> > : Mandeville, W. H.,
> > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
Transplant.
> > : (1997), 12(5)
> > : > 961-964.
> > : >
> > : > 11. Thin anisotropic coatings based on sol-gel technology.
> Holmes-Farley,
> > : S. R.; Yanyo, L.
> > : > C;
> > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4),
> 439-444.
> > : >
> > : > 12. The mechanism of cure initiation of a surface activated
adhesive.
> > : Holmes-Farley, S.
> > : > R.;
> > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
> > : >
> > : > 13. Adhesion promotion and corrosion prevention using thin
anisotropic
> > : coatings. Holmes-
> > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
> > : 131-151.
> > : >
> > : > 14. Wetting of functionalized polyethylene having ionizable organic
> acids
> > : and bases at the
> > : > polymer-water interface: relations between functional group
polarity,
> > : extent of
> > : > ionization,
> > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
> > : Whitesides, G. M.;
> > : > Langmuir
> > : > (1988), 4(4), 921-937.
> > : >
> > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
> > : single hydroxy group.
> > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> > : >
> > : > 16. Reconstruction of the interface of oxidatively functionalized
> > : polyethylene (PE-CO2H)
> > : > and
> > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo,
> R.;
> > : McCarthy, T. J.;
> > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report
> (1987),
> > : AD-
> > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> > : >
> > : > 17. Surface-modified polyethylene film: the relationship between
> surface
> > : chemistry and
> > : > physical
> > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11),
> 4537.
> > : >
> > : > 18. Reactivity of carboxylic acid and ester groups in the
> functionalized
> > : interfacial
> > : > region of
> > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> > : differentiation of the
> > : > functional groups into shallow and deep subsets based on a
comparison
> of
> > : contact angle and
> > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.;
Langmuir
> > : (1987), 3(1), 62-
> > : > 76.
> > : >
> > : > 19. Fluorescence properties of dansyl groups covalently bonded tot
he
> > : surface of
> > : > oxidatively
> > : > functionalized low-density polyethylene film. Holmes-Farley, S. R.;
> > : Whitesides, G. M.;
> > : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
> > : AD-A162435/2/GAR,
> > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> > : >
> > : > 20. Acid-base behavior of carboxylic acid groups covalently attached
> at
> > : the surface of
> > : > polyethylene: The usefulness of contact angle in following the
> ionization
> > : of surface
> > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
> > : Deutch, J.;
> > : > Whitesides,
> > : > G. M.; Langmuir (1985), 1(6), 725-740.
> > : >
> > : > 21. The thermal stability of a surface modified solid organic
polymer.
> > : Holmes-Farley, S.
> > : > R.;
> > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
> > : >
> > : >
> > : >
> > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> > : >
> > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R.
Advanced
> > : Aquarist. June 2003.
> > : >
> > : > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley,
R.
> > : Advanced Aquarist.
> > : > May
> > : > 2003.
> > : >
> > : > 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley,
R.
> > : Reefkeeping May
> > : > 2003.
> > : >
> > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
Reefkeeping
> > : April 2003.
> > : >
> > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> > : Holmes-Farley, R.
> > : > Advanced Aquarist; April 2003.
> > : >
> > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> > : Holmes-Farley, R.
> > : > Advanced Aquarist; April 2003.
> > : >
> > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced
> Aquarist;
> > : March 2003.
> > : >
> > : > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
> > : Holmes-Farley, R.
> > : > Advanced Aquarist; February 2003.
> > : >
> > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
January
> > : 2003.
> > : >
> > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> December
> > : 2002.
> > : >
> > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
> Advanced
> > : Aquarist; November
> > : > 2002.
> > : >
> > : > 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley,
R.
> > : Advanced Aquarist;
> > : > November 2002.
> > : >
> > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced
> Aquarist,
> > : September 2002.
> > : >
> > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist,
August
> > : 2002.
> > : >
> > : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com,
April
> > : 2002.
> > : >
> > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
> > : Aquarist; July 2002
> > : >
> > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist;
> June
> > : 2002.
> > : >
> > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R.
> Advanced
> > : Aquarist, May
> > : > 2002.
> > : >
> > : > 19. The Chemical & Biochemical Mechanisms of Calcification in
Corals.
> > : Holmes-Farley, R.
> > : > Advanced Aquarist, April 2002.
> > : >
> > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> > : >
> > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
> > : >
> > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January
> 2002.
> > : >
> > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium
Frontiers
> > : 2000.
> > : >
> > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
> > : Frontiers 2000.
> > : >
> > : > 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
> > : Aquarium Frontiers
> > : > 2000.
> > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
> Frontiers
> > : 2000.
> > : >
> > : > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers
> 2000.
> > : >
> > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers
1999.
> > : >
> > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> > : >
> > : >
> > : >
> > : >
> > : >
> > : >
> > : >
> > : > Boomer
> > : >
> > : > Want to talk chemistry ? The Reef Chemistry Forum
> > : > http://www.reefcentral.com/vbulletin/index.php
> > : >
> > : > Want to See More ?
> > : > Please Join Our Growing Membership
> > : > www.coralrealm.com
> > : >
> > : >
> > : >
> > :
> > :
> >
> >
>
>

[stoutman]

I have a suspicion that you are dragging this out and debating me because
you don't want to admit you are wrong in front of everyone else. I have
NOTHING to prove. I have never written in this newsgroup until very
recently. Based on some of the comments others have made, I suspect that
you are a long time contributor to this NG and to some aquarium forum and
you feel you have a reputation to uphold. I am almost 100% sure you know
you are wrong with respect to our disagreements and you just want to keep
fighting me hoping I make a mistake. You have made SEVERAL mistakes and
contradictions. Even cited web pages that contradict yourself.

If you are unsure were you have contradicted yourself, I will take the time
to show you.

I am truly sorry that I soiled your GURU reputation. I can only suggest you
read some general CHEMISTRY books. I bet you would enjoy and benefit from
them. You seem to have an interest in chem. and aquariums. Most aquarium
enthusiasts don't care what's going on at a chemical level, they just dump A
into their tank and measure X. You do, and I'm glad for you. Feed your
chemical knowledge by getting the basics down and then build. Your
chemistry knowledge you have learned thus far is on a VERY shaky foundation.
This can be corrected.

Take care,
-Stoutman



"Boomer" > wrote in message
...
> Alkalinity a measure of the amount of anions of weak acid in water and of
the cations
> balanced against them
> Take note it says ***acid***
>
> Buffering capacity the ability of a solution to resist or dampen changes
in pH upon the
> addition of acids or bases.
> Take note its says ***the addition of acids or bases***
>
> One more
>
> http://www.waterontheweb.org/resources/glossary.html
>
> We could go on like this all day, so what is the point ?
>
> You will LOVE this one
> http://www.kyantec.com/Tips/phbuffering.htm
>
> Don't you just lovbe PDF's
> http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
>
> Don't fall out of your chair
> http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
>
>
>
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message news:XB7Wb.19339$QA2.62332@attbi_s52...
> : Man here is another, google is a wonderful thing. I'm not filtering any
> : out, just posting what I find by GOOGLING for you.
> :
> : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> :
> :
> : Wow, a gov link. Even the government is wrong, this must be a
conspiracy
> : against Boomer.
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > Now I am getting bored
> : >
> : > "Don't the components of a buffer account for the buffering capacity?
> : Yes."
> : >
> : > Yes, agreed but you seem to fail what I'm saying. Buffering Capacity
and
> : Alkalinity are
> : > not the same, that has always been the issue. I gave the equation does
> : that look like an
> : > Alkalinity equation or how Alk is determined. I see you had now
comments
> : on it what's
> : > wrong, why no comments on the equations I gave. Don't understand them
or
> : what ? Again this
> : > is the equation for Buffering Capacity, also called Buffer Index or
Buffer
> : Intensity. It
> : > is defined in most water chemistry and chemical oceanography text
books.
> : >
> : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] +
CKa
> : [H3O+] / (Ka =
> : > H3O+])² )
> : >
> : > This is not Alkalinity now is it ?
> : >
> : > "I know how to do a titration, In fact I have done several. How many
have
> : > you actually done? I don't mean by counting drops, I mean with a
buret?"
> : >
> : > Well good for you, I use a Digital Titrator
> : >
> : > "Oh, I see,
> : > you think acidity is the opposite of alkalinity. In the world of
> : CHEMISTRY
> : > it's not. Maybe in aquarium newsgroups it is.
> : >
> : > Hum no, maybe you should go for a look at HACH's or LaMotte website or
the
> : book I
> : > suggested earlier. Please view a copy.
> : >
> : > Standard Methods for the Examination of Water and Wastewater
> : >
> : > This book, over 2000 pages, is the guide for water testing. If you are
> : reporting water
> : > test to the EPA you must use approved std from this text.I t is
prepared
> : and published by
> : > the EPA, American Water Works Association and American Public Health
> : Association. You
> : > mean you don't have one and the issue is water chemistry
> : >
> : > You are confusing Acidity and Acidity as you know little about water
> : chemistry and
> : > procedures and test methods
> : >
> : > From SMEWW, section 2-30, 2310 ACIDITY
> : >
> : > "Acidity of water is its quantative capacity to react with a strong
base
> : to a designated
> : > pH"
> : >
> : > This is how you test for it
> : >
> : > A std alkali titration to methyl orange or phenolphthalein
> : > endpoint.
> : >
> : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write
this
> : book, there are
> : > over 100 of them, they are wrong.
> : >
> : > Like Buffering Capacity you have your Acidity's mixed up
> : > In water measurement if you have a high Alk you also usually have a
high
> : Acidity.
> : > Normally a high Alk also gives a higher CO2 level. Get a WATER
CHEMISTRY
> : BOOK there pal.
> : >
> : >
> : > "These are all in equilibrium with each other. An initial high pH
(above
> : > 6.4) will shift the equilibrium to the right to form HCO3-1. If the
pH of
> : > the solution is above 10.3 (pKa2) the .........."
> : >
> : >
> : > Christ, there you go again with the FW ****. All your numbers are
wrong we
> : are dealing
> : > with SEAWATER
> : >
> : > This means that at a pH of 8.3, the majority of the CO2(aq) is in the
form
> : > of HCO3-1 .
> : >
> : > I have already pointed that out and gave actual values at know
seawater
> : levels, go back
> : > and re-read it you aren't telling me anything here.Of course most is
HCO3
> : see...
> : >
> : >
> : > @ 20C and 34.3 ppt salinity
> : >
> : > CO2 = 0.52 %
> : >
> : > HCO3 = 86.4 %
> : >
> : > CO3 = 13.09 %
> : >
> : >
> : > "In your glass experiment you managed to lower the pH enough to purge
out
> : CO2
> : > by boiling"
> : >
> : > The purpose behind the glass is to show that alk is not affect by CO2
and
> : vise-versa and
> : > how Co2 affects pH.
> : >
> : > Now, in a real life seawater aquarium, with a pH of 8.3 and that pH
drops
> : to say 8.1 it is
> : > usually due to excess CO2. If you took a glass of that water and
aerated
> : it you WILL drive
> : > off the CO2 and raise the pH. It has been done a proven a million
times.
> : >
> : > "In order to 'purge' CO2 you would need to lower the
> : > pH to shift the equilibrium to below 6.4"
> : >
> : > The hell you do !!!.Do you know who many times people on this NG to
> : include Dr. Craig
> : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
> : sample of aquarium
> : > water and aerate it to see if the pH GOES UP AND when they come back
with
> : the test it is
> : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST
excess
> : CO2 in the tank
> : > water, increase the circulation for better gas exchange at the
surface,
> : reduce feeding,
> : > and try to improve on better skimming, thus reducing the bio-load and
pH
> : decline due to
> : > CO2.
> : >
> : >
> : > "I hope this helps. "
> : >
> : > Help, how can you when you miss everything. I should be charging you
> : >
> : > Oh, by the way. Your websites, I have about 50 on these issues, I
could
> : post them, not to
> : > mention I have all those water chemistry books, so there is no need to
> : view your sites.
> : >
> : > Finally are you afraid to come to our Chemistry Forum, afraid to get
> : slapped by REAL
> : > chemists. I get a charge out of you can't post your ref .I have posted
the
> : same or similar
> : > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500
posts
> : there and am the
> : > biggest contributor to his forum other than himself or maybe Habib
Sheka
> : >
> : > Hum, here are Randy's ref that he posted. He hosts the website
> : >
> : > S. RANDY HOLMES-FARLEY
> : > Arlington, Massachusetts
> : >
> : > EDUCATION
> : >
> : > 1982-1986 Harvard University Cambridge, MA
> : > PhD in Chemistry
> : > Research Advisor: George Whitesides
> : >
> : > Investigated the relationship between polymer surface chemistry and
> : physical properties
> : > through controlled surface modification and testing.
> : >
> : > 1980-1982 Cornell University Ithaca, NY
> : > BA in Chemistry and Biology
> : > Graduated Summa Cum Laude
> : > Distinction in All Subjects
> : > Grade Point: 3.94/4.0
> : > Honors research: isolation and characterization of the subunit of CF1
> : enzyme
> : >
> : >
> : > 1978-1979 Stanford University Palo Alto, CA
> : > Grade Point: 3.55/4.0
> : >
> : >
> : > EXPERIENCE
> : >
> : > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> : > (bought out GelTex Pharmaceuticals in 2001)
> : > Vice President, Chemical Research 2001-present
> : > Senior Director, Chemical Research 1999-2001
> : > Director of Chemical Research 1997-1999
> : > Manager of Chemical Research 1995-1997
> : > Group Leader 1994-1995
> : > Senior Research Scientist 1992-1994
> : >
> : > Helped start GelTex as second employee
> : >
> : > Managed various research programs with multi-million dollar budgets
> : >
> : > Supervised research chemists (17+)
> : >
> : > Co-inventor of several polymeric pharmaceuticals and pharmaceutical
> : candidates including
> : > Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride
(FDA
> : approved)
> : >
> : > Company Safety Officer for 3 years
> : >
> : > Chemical Hygiene Officer 2000-present
> : >
> : >
> : >
> : >
> : > 1990-1992 GTE Corporation Waltham, MA
> : > Senior Member of Technical Staff
> : > Applied research involving polymer interfaces
> : > Metallization of plastics
> : > Polymer/polymer adhesion
> : > Optical coatings
> : >
> : >
> : >
> : > 1986-1990 Lord Corporation Cary, NC
> : > Senior Research Scientist 1988-1990
> : > Research Scientist 1986-1988
> : > Basic and applied research on surface chemical bonding
> : > Developed new adhesive compositions
> : > Developed new sol-gel coatings for corrosion resistance
> : >
> : >
> : > HONORS AND AWARDS
> : >
> : > Industrial Innovations Award by Northeast Region of American Chemical
> : Society (6/2001)
> : >
> : > National Kidney Foundation of Northern California Honoree (5/2001)
> : >
> : > American Chemical Society/Polymer Chemistry Division Industrial
Sponsors
> : > Award (8/2000)
> : >
> : > R&D 100 Award from R&D magazine (1999)
> : >
> : > Sherwin Williams Award in applied polymer science (9/85)
> : >
> : > IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
> : >
> : > Award for highest GPA in Chemistry Department (6/82)
> : >
> : > Summa Cum Laude Honors in Chemistry (6/82)
> : >
> : > Phi Lamda Epsilon (6/82)
> : >
> : > Phi Beta Kappa (2/82)
> : >
> : > Cornell University Dean's List (1981, 1982)
> : >
> : > Harvard Book Club Award for highest GPA senior year (1978)
> : >
> : > First Place in western NY ACS high school chemistry exam (1977)
> : >
> : > 1978-1979
> : >
> : >
> : > __________________
> : > Randy Holmes-Farley
> : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
> : >
> : > Hobby Experience: 8 years with reefs
> : > Current Tanks: 90 gal mixed reef
> : > Interests: Reefkeeping, science, photography
> : >
> : >
> : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> : >
> : > Open this post in a new window | Report this post to a moderator | IP:
> : Logged
> : >
> : >
> : >
> : > 06/27/2003 02:44 PM
> : >
> : > Randy Holmes-Farley
> : > Chemistry Moderator
> : >
> : > Registered: Apr 2001
> : > Location: Arlington, Massachusetts
> : > Occupation: Chemist (Drug Discovery at Genzyme)
> : > Posts: 15282
> : >
> : >
> : >
> : > Publications
> : >
> : >
> : > ISSUED UNITED STATES PATENTS
> : >
> : >
> : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
> : Mandeville, III; W. Harry.
> : > US 6,566,407; 5/20/2003
> : >
> : > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen
Randall;
> : Huval, Chad
> : > Cori.
> : > U.S. 6,517,825; 2/11/2003.
> : >
> : > 3. Method of making phosphate-binding polymers for oral
administration.
> : Holmes-Farley,
> : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
> : 6,509,013; 1/21/2003.
> : >
> : > 4. Combination therapy for treating hypercholesterolemia using a bile
acid
> : sequestrant
> : > polymer
> : > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley,
Stephen
> : Randall;
> : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> : >
> : > 5. Method for treating hypercholesterolemia with polyallylamine
polymers.
> : Holmes-Farley,
> : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
Goldberg,
> : Dennis I. , US
> : > 6,423,754; 7/23/2002.
> : >
> : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
> : Neenan, Thomas X..;
> : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> : >
> : > 7. Combination therapy for treating hypercholesterolemia and
> : atherosclerosis. Huval, Chad
> : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep
K.
> : U.S. 6,365,186;
> : > 4/2/2002.
> : >
> : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
Mandeville,
> : W. H., III;
> : > Huval; C.
> : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
> : 10/9/2001.
> : >
> : > 9. Polymers containing guanidinium groups as bile acid sequestrants.
Dhal;
> : P. K.; Holmes-
> : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> : >
> : > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III.; US
> : > 6,281,252;
> : > 8/28/2001.
> : >
> : > 11. Combination therapy for treating hypercholestrolemia. Huval; C.
C.;
> : Holmes-Farley; S.
> : > R. ;
> : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> : >
> : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
> : Holmes-Farley, S.
> : > R.; US
> : > 6,264,937; 7/24/2001.
> : >
> : > 13. Method for treating hypercholesterolemia with unsubstituted
> : polydiallylamine polymers.
> : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
> : 6,248,318;
> : > 6/19/2001.
> : >
> : > 14. Process for removing bile salts from a patient and alkylated
> : compositions therefore.
> : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
> : >
> : > 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S.
R.;
> : Dhal, P. K.;
> : > Petersen,
> : > J. S.; US 6,203,785; 3/20/2001.
> : >
> : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.;
Huval,
> : C. C.; US
> : > 6,190,649;
> : > 2/20/2001.
> : >
> : > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III.; US
> : > 6,177,478;
> : > 1/23/2001.
> : >
> : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
Holmes-Farley,
> : S. R.;
> : > Mandeville, W.
> : > H., III.; US 6,129,910; 10/10/2000.
> : >
> : > 19. Method for treating hypercholesterolemia with unsubstituted
> : polydiallylamine polymers.
> : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
> : 6,083,497;
> : > 7/4/2000.
> : >
> : > 20. Method of making phosphate-binding polymers for oral
administration.
> : Holmes-Farley, S.
> : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495;
7/4/2000.
> : >
> : > 21. Process for removing bile salts from a patient and alkylated
> : compositions therefore.
> : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
5/23/2000.
> : >
> : > 22. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> : >
> : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
> : Neenan; T. X.; Holmes-
> : > Farley; S. R. US 6,034,129; 3/7/2000.
> : >
> : > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III.; US
> : > 5,985,938;
> : > 11/16/99.
> : >
> : > 25. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> : >
> : > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W.
H.,
> : III.;
> : > Holmes-Farley;
> : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> : >
> : > 27. Hydrophilic nonamine-containing and amine-containing copolymers
and
> : their use as bile
> : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
5,929,184;
> : 7/27/99.
> : >
> : > 28. Interpenetrating polymer networks for sequestration of bile acids.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
> : 7/20/99.
> : >
> : > 29. Amine polymer sequestrant and method of cholesterol depletion.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> : >
> : > 30. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> : >
> : > 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> : >
> : > 32. Process for removing bile salts from a patient and compositions
> : therefor. Mandeville,
> : > W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> : >
> : > 33. Preparation of polymeric sequestrants for bile acid salts.
Mandeville,
> : W. H., III.;
> : > Holmes-
> : > Farley, S. R.; US 5,703,188; 12/30/97.
> : >
> : > 34. Oral administration of iron-binding crosslinked amine polymers.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> : >
> : > 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley,
S.
> : R.; US 5,693,675;
> : > 12/2/97.
> : >
> : > 36. Method for removing bile salts from a patient with alkylated
> : crosslinked amine
> : > polymers,
> : > and preparation of the polymers. Mandeville, W. H., III.;
Holmes-Farley,
> : S. R.; US
> : > 5,679,717; 10/21/97.
> : >
> : > 37. Phosphate-binding polymers for oral administration. Holmes-Farley,
S.
> : R.; Mandeville,
> : > W.
> : > H., III.; US 5,667,775; 9/16/97.
> : >
> : > 38. Ion-exchange process using highly crosslinked polymers for
removing
> : bile salts from a
> : > patient, preparation of the polymers, and compositions containing
them.
> : Mandeville, W. H.,
> : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> : >
> : > 39. Hydrophobic amine polymer sequestrant and method of cholesterol
> : depletion. Mandeville,
> : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530;
4/8/97.
> : >
> : > 40. Amine polymer sequestrant and method of cholesterol depletion.
> : Mandeville, W. H.,
> : > III.;
> : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> : >
> : > 41. Phosphate-binding polymers for oral administration. Holmes-Farley,
S.
> : R.; Mandeville,
> : > W.
> : > H., III.; US 5,496,545; 3/5/96.
> : >
> : > 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
> : III.; Holmes-Farley,
> : > S. R.;
> : > US 5,487,888; 1/30/96.
> : >
> : > 43. Ultra-thin, uniform sol-gel coating of a substrate having active
> : hydrogens on the
> : > surface.
> : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> : >
> : > 44. Layered sol-gel coatings from organisilicon compounds.
Holmes-Farley,
> : S. R.; Yanyo, L.
> : > C.;
> : > US 5,182,143; 1/26/93.
> : >
> : > 45. Method for metal bonding using ultrathin primer coating.
> : Holmes-Farley, S. R.; Yanyo,
> : > L.
> : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> : >
> : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.;
US
> : 5,096,962;
> : > 3/17/92.
> : >
> : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> : elastomer-metal bonding.
> : > Holmes-
> : > Farley, S. R.; US 5,102,956; 4/7/92.
> : >
> : >
> : >
> : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
> : >
> : >
> : > 1. Aryl boronate functionalized polymers for treating obesity and
> : inhibiting fat uptake.
> : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal,
Pradeep
> : K.; Huval, Chad
> : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92
pp. WO
> : 0302571.
> : >
> : > 2. Preparation of aryl boronic acids for treating obesity.
Holmes-Farley,
> : Stephen Randall;
> : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep
K.
> : (Geltex
> : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
> : >
> : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
> : Stephen Randall.
> : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
> : 0302130.
> : >
> : > 4. Method for reducing copper levels and treating copper toxicosis.
> : Holmes-Farley, Stephen
> : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002),
45
> : pp. WO
> : > 0285383.
> : >
> : > 5. Method for treating gout and binding uric acid. Holmes-Farley,
Stephen
> : Randall; Burke,
> : > Steven K. WO 0285381 10/31/2002.
> : >
> : > 6. Method for treating gout and reducing serum uric acid.
Holmes-Farley,
> : Stephen Randall;
> : > Burke, Steven K WO 0285380 10/31/2002.
> : >
> : > 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
> : Holmes-Farley, S. R.;
> : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> : >
> : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
> : Holmes-Farley, S.
> : > R.;
> : > WO 1999-US5662; 9/23/1999.
> : >
> : > 9. Amine-containing copolymers as bile acid sequestrants.
Holmes-Farley,
> : S. R.; Petersen,
> : > J. S.;
> : > WO 9933452; 7/8/1999.
> : >
> : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III
and
> : Holmes-Farley, S.
> : > R.;
> : > WO 9922743; 5/14/1999.
> : >
> : > 11. Polyallylamine polymers for removing bile salts and treating
> : hypercholesterolemia, and
> : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III;
Burke,
> : S. K.; Goldberg,
> : > D. I.; WO 9857652; 12/23/98.
> : >
> : > 12. Phosphate-bidning polymers combined with a calcium supplement for
oral
> : administration.
> : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley,
S.
> : R.; WO 9842355;
> : > 10/1/98.
> : >
> : > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
> : depletion. Mandeville,
> : > W.
> : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
> : >
> : > 14. Process for adjusting ion concentration in a patient and
compositions
> : therefor.
> : > Mandeville,
> : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> : >
> : > 15. Vacuum-deposited silver on polycarbonate with a chromium
interlayer
> : for improved
> : > metal-
> : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
1/20/94.
> : >
> : > 16. Process for increased metal-substrate bond strength in metalized
> : plastics.
> : > Holmes-Farley, S.
> : > R.; Ger. Offen. 4322516; 7/6/93.
> : >
> : > 17. Electrorheological fluids and preparation of particles useful in
the
> : fluids.
> : > Troughton,
> : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
> : David; Bares, Joseph
> : > E.;
> : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
> : 394049;
> : > 10/24/1990.
> : >
> : > JOURNAL PUBLICATIONS
> : >
> : > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov,
Eugene;
> : Guo, Amy;
> : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
> : Mandeville, W. Harry;
> : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
611-619.
> : >
> : > 2. Amine functionalized polyethers as bile acid sequestrants:
synthesis
> : and biological
> : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S.
Randall;
> : Mandeville, W.
> : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
> : Journal of
> : > Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
> : 1559-1574.
> : >
> : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
> : Imprinting. Huval,
> : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
> : Randall; Mandeville,
> : > W.
> : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert
J.;
> : Chen, Xi; Dhal,
> : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> : >
> : > 4. Synthetic polymers for the binding of fat in the intestinal tract.
> : Jozefiak, Thomas H.;
> : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia;
Huval,
> : Chad C.;
> : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
> : Abstracts of
> : > Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
> : 26-30, 2001
> : > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
> : Division of
> : > Polymer Chemistry) (2001), 42(2), 98.
> : >
> : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer
gel
> : pharmaceutical.
> : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.;
Ward,
> : J.; Sacchiero,
> : > B.;
> : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.;
Chen,
> : X.; Mazzeo, J.
> : > R.. Polym. Preprints (2000), 41(1), 735-736.
> : >
> : > 6. In vitro comparison of bile acid binding to colesevelam HCl and
other
> : bile acid
> : > sequestrants.
> : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
> : Hook, P.; Holmes-
> : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
> : >
> : > 7. Novel polymeric pharmaceuticals: From startup to market.
Holmes-Farley,
> : S. R; Polym.
> : > Mater. Sci. Eng (1999), 80, 246-247.
> : >
> : > 8. Design and characterization of of Sevelamer Hydrochloride: a novel
> : phosphate-binding
> : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward,
J.;
> : Miller, K. L.;
> : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure
and
> : Appl. Chem.,
> : > A36(7&8), p. 1085 (1999).
> : >
> : > 9. Three generations of bile acid sequestrants. Mandeville, W. H.,
III;
> : Braunlin, W.;
> : > Dhal, P.;
> : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
> : Rosenbaum, D.;
> : > Sacchiero,
> : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
> : 550, 3-15.
> : >
> : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric
phosphate
> : binder, on
> : > urinary
> : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
> : Mandeville, W. H.,
> : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
> : (1997), 12(5)
> : > 961-964.
> : >
> : > 11. Thin anisotropic coatings based on sol-gel technology.
Holmes-Farley,
> : S. R.; Yanyo, L.
> : > C;
> : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4),
439-444.
> : >
> : > 12. The mechanism of cure initiation of a surface activated adhesive.
> : Holmes-Farley, S.
> : > R.;
> : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
> : >
> : > 13. Adhesion promotion and corrosion prevention using thin anisotropic
> : coatings. Holmes-
> : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
> : 131-151.
> : >
> : > 14. Wetting of functionalized polyethylene having ionizable organic
acids
> : and bases at the
> : > polymer-water interface: relations between functional group polarity,
> : extent of
> : > ionization,
> : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
> : Whitesides, G. M.;
> : > Langmuir
> : > (1988), 4(4), 921-937.
> : >
> : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
> : single hydroxy group.
> : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> : >
> : > 16. Reconstruction of the interface of oxidatively functionalized
> : polyethylene (PE-CO2H)
> : > and
> : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo,
R.;
> : McCarthy, T. J.;
> : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report
(1987),
> : AD-
> : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> : >
> : > 17. Surface-modified polyethylene film: the relationship between
surface
> : chemistry and
> : > physical
> : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11),
4537.
> : >
> : > 18. Reactivity of carboxylic acid and ester groups in the
functionalized
> : interfacial
> : > region of
> : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> : differentiation of the
> : > functional groups into shallow and deep subsets based on a comparison
of
> : contact angle and
> : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
> : (1987), 3(1), 62-
> : > 76.
> : >
> : > 19. Fluorescence properties of dansyl groups covalently bonded tot he
> : surface of
> : > oxidatively
> : > functionalized low-density polyethylene film. Holmes-Farley, S. R.;
> : Whitesides, G. M.;
> : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
> : AD-A162435/2/GAR,
> : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> : >
> : > 20. Acid-base behavior of carboxylic acid groups covalently attached
at
> : the surface of
> : > polyethylene: The usefulness of contact angle in following the
ionization
> : of surface
> : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
> : Deutch, J.;
> : > Whitesides,
> : > G. M.; Langmuir (1985), 1(6), 725-740.
> : >
> : > 21. The thermal stability of a surface modified solid organic polymer.
> : Holmes-Farley, S.
> : > R.;
> : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
> : >
> : >
> : >
> : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> : >
> : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
> : Aquarist. June 2003.
> : >
> : > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
> : Advanced Aquarist.
> : > May
> : > 2003.
> : >
> : > 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
> : Reefkeeping May
> : > 2003.
> : >
> : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
> : April 2003.
> : >
> : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> : Holmes-Farley, R.
> : > Advanced Aquarist; April 2003.
> : >
> : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> : Holmes-Farley, R.
> : > Advanced Aquarist; April 2003.
> : >
> : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced
Aquarist;
> : March 2003.
> : >
> : > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
> : Holmes-Farley, R.
> : > Advanced Aquarist; February 2003.
> : >
> : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
> : 2003.
> : >
> : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
December
> : 2002.
> : >
> : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
Advanced
> : Aquarist; November
> : > 2002.
> : >
> : > 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
> : Advanced Aquarist;
> : > November 2002.
> : >
> : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced
Aquarist,
> : September 2002.
> : >
> : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
> : 2002.
> : >
> : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
> : 2002.
> : >
> : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
> : Aquarist; July 2002
> : >
> : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist;
June
> : 2002.
> : >
> : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R.
Advanced
> : Aquarist, May
> : > 2002.
> : >
> : > 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
> : Holmes-Farley, R.
> : > Advanced Aquarist, April 2002.
> : >
> : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> : >
> : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
> : >
> : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January
2002.
> : >
> : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
> : 2000.
> : >
> : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
> : Frontiers 2000.
> : >
> : > 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
> : Aquarium Frontiers
> : > 2000.
> : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
Frontiers
> : 2000.
> : >
> : > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers
2000.
> : >
> : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
> : >
> : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> : >
> : >
> : >
> : >
> : >
> : >
> : >
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : >
> : >
> :
> :
>
>

[CapFusion]

Ahhh, why did you jump in? I was soo sooo enjoying it and learning at the
same time. Very entertaining. AND at the same TIME getting big fat HEAHACHE
trying to understand the chemistry. BUT worth all the headache.

CapFusion,...




"Richard Reynolds" > wrote in message
news:0lHVb.16203$gl2.2728@lakeread05...
> I am sorry ahead of time I couldnt resist
>
> > By the way do you know who you are talking to ?
>
>
> DUH of course he doesnt or he wouldnt have argued :D
>
>
> now ive done it the king is gona slap me around for messing with the
oracle :D
>
> --
> Richard Reynolds
>
>
>

[Richard Reynolds]

> Ahhh, why did you jump in? I was soo sooo enjoying it and learning at the
> same time. Very entertaining. AND at the same TIME getting big fat HEAHACHE
> trying to understand the chemistry. BUT worth all the headache.
>
> CapFusion,...

damn cap your newsserver sux, i posted that before most of the responses. :D




--
Richard Reynolds

[Rod]

>
>We know who the winner is.....

Who, and what make you say so?.. My head is spinning.. One thing I will say,
this group has a way of taking certain posters messages as gospil whether that
person is right or wrong..
Rod Buehler
www.asplashoflife.com

[Richard Reynolds]

> I really want to help you understand.

ok so ive been following along :D

and just to fill anyone who doesnt know in, I cant get from an "h" a "2" and an "o" to
make water :D


but a few questions from all parts of the thread :D

there have been some references to FW vs SW equasions for THIS email everything is
sal****er as FW doesnt concern me this much.


--boomer--It is called "blowing it off" , such as with an airstone. If you have high
CO2 and add an airstone it will drive the CO2 off raising the pH.

--stoutman--Ok, you are going to try and 'purge' (the correct term) your CO2 out with
air. Yeah, I guess that would work. If you intentionally put the CO2 in
there to begin with because you must have a higher concentration of CO2 in
your tank than in the atmosphere. I don't intentionally put CO2 in my tank.
But I know some of you reef people due in Kalk reactors

what I understand boomer called "blowing it off" stoutman called it "purge" and a few
places I just checked call it degassing is that all the same thing or not ?? and if not
what is the difference??

IF i take 3L of asw put it in a tall conatiner and pump a lot of air into it the Ph rises,
but the Alk stays the same, I know thats what happens I do it daily. isnt this because
afterwards the water has less co2 than before?

alternatively IF i disconnect that air pump and plug in my co2 tank, the Ph falls, and the
Alk still stays the same, I also do this daily. isnt this because now the water has more
co2?

wont both of these happen regardless of the alkalinity of the water?? if not what
alkalinity do I need to put more co2 into the water and keep the ph > 7??



--boomer--Bad term as Buffering Capacity isn't Alkalinity. Alk is more on the order of ANC
(Acid
Neutralizing Capacity). BC is the ability to withstand upward and downward trends in pH do
to the addition of an acid or base.There is also a measurement called Acidity ( B_aseNC
and test kits for it). So the combination of the two more or les is BC. But I know what
you mean, may use the term ALK and BC interchangeably

--stoutman-- Yes, the pH will drop with the addition of CO2. Remove CO2 will cause the
pH to rise? How do you remove CO2? Once it is in solution it forms
carbonic acid and neutralizes some of your 'buffer'.

whats carbonic acid, where does it come from ??? and how does it neutralize some of my
'buffer' ? and can algae's still consume it now or not?? can i test the levels of
carbonic acid? and what could be considered low/normal/high??



--boomer--You can have all the alk you want in the world and it won't help, in
regards to CO2.

--stoutman--Wrong. Alkalinity increases your tank's ability to RESIST sharp changes in
pH. This is what is meant by 'buffering capacity'.

ok so how high does my alkalinity need to be to keep the ph from falling? and what is a
"sharp change" is not a starting Ph of 8.1 and an ending Ph of < 5.0(the lowest I can
test) a "sharp change" ? what time period does it have to happen in I know i can make the
change in under 5 minutes is that "sharp"?


--stoutman--pH is the -log of the hydronium ion concentration. When the hydronium ion
concentration is very low, your system is basic (high pH). When the
hydronium ion concentration is very large, your system is acidic (low pH).

where does the hydronium ion come from when I add co2 ??? how does it go away when the co2
goes away? extend that "goes away" to include consumption??

--stoutman--pH + pOH = 14. So yeah, you can calculate a pH from a pOH and vice versa.
But a pH of < 7 means acidic. pH > 7 means basic.
pH can tell you something about acidity and basicity. It is a measurement
of both, or the entire pH scale (1-14) if you will.

where does 14 come from ??? is that just the highest Ph level??

am I doing Ph wrong should it be pH?

--stoutman--Ok, you are going to try and 'purge' (the correct term) your CO2 out with
air. Yeah, I guess that would work. If you intentionally put the CO2 in
there to begin with because you must have a higher concentration of CO2 in
your tank than in the atmosphere. I don't intentionally put CO2 in my tank.
But I know some of you reef people due in Kalk reactors.

wouldnt this tie in from people that have high Ph in there homes?? not the outside air or
the air at sea level? and wouldnt this higher level make it into the tank water?? if not
how/why?

and if you use co2 and Kalk its a really bad thing (trust me I know ) I think you meant ca
or calcium reactor.

I add co2 to SW for a number of reasons mostly to help grow things, but also to break down
calcium in my calcium reactors.

--booomer--If Alk resists changes in pH then why does CO2 lower the pH without
affecting the Alk.

--stoutman--Alkalinity is buffering capacity. Your buffers begin to get weakened with
the addition of acid until they reach a point when they can no longer
'buffer' and the pH crashes.

I dont get this!

if by "buffer" your refering again to alkalinity how can I add co2 and test for the
alkalinity and get the same results ???



I ran out of time, i need to get real work done :( i know there were more questions ill
have to ask them later :) the formulas are making my head spin!!!





--
Richard Reynolds

[stoutman]

> --boomer--It is called "blowing it off" , such as with an airstone. If you
have high
> CO2 and add an airstone it will drive the CO2 off raising the pH.
>
> --stoutman--Ok, you are going to try and 'purge' (the correct term) your
CO2 out with
> air. Yeah, I guess that would work. If you intentionally put the CO2 in
> there to begin with because you must have a higher concentration of CO2 in
> your tank than in the atmosphere. I don't intentionally put CO2 in my
tank.
> But I know some of you reef people due in Kalk reactors
>
> what I understand boomer called "blowing it off" stoutman called it
"purge" and a few
> places I just checked call it degassing is that all the same thing or not
?? and if not
> what is the difference??

Purging and Degassing are the same. But I wouldn't degas a solution of a
specific gas (CO2) with a gas (this case he was using air) that contains the
same gas I am trying to purge. You could degas with nitrogen, but this
would also degas other gases in solution, like a very important one, OXYGEN.


> IF i take 3L of asw put it in a tall conatiner and pump a lot of air into
it the Ph rises,
> but the Alk stays the same, I know thats what happens I do it daily. isnt
this because
> afterwards the water has less co2 than before?

asw?? You lost me. Not familiar with this term.

> alternatively IF i disconnect that air pump and plug in my co2 tank, the
Ph falls, and the
> Alk still stays the same, I also do this daily. isnt this because now the
water has more
> co2?

> wont both of these happen regardless of the alkalinity of the water?? if
not what
> alkalinity do I need to put more co2 into the water and keep the ph > 7??
>
>

> whats carbonic acid, where does it come from ??? and how does it
neutralize some of my
> 'buffer' ? and can algae's still consume it now or not?? can i test the
levels of
> carbonic acid? and what could be considered low/normal/high??

Carbonic acid forms from the reaction of CO2 (aqueous) and water. it is
H2CO3. It is an acid. It will drive the pH down effectively neutralizing
some of your buffer. You couldn't test for it because once it forms it is
quickly turned into HCO3- which is in equilibrium with CO3-. At pH 8-8.5.
You can, however test for your HCO3- and CO3-2 concentration. This is your
carbonate hardness.


> ok so how high does my alkalinity need to be to keep the ph from falling?
and what is a
> "sharp change" is not a starting Ph of 8.1 and an ending Ph of < 5.0(the
lowest I can
> test) a "sharp change" ? what time period does it have to happen in I
know i can make the
> change in under 5 minutes is that "sharp"?

Your pH is always going to fall. Your alkalinity prevents a rapid fall in
pH. What is the desired level of alkalinity for aquariums? Not sure on
this. I'm a chemist, not a marine biologist. You ideally would want the
most alkalinity you can without raising the pH out of spec.


> where does the hydronium ion come from when I add co2 ??? how does it go
away when the co2
> goes away? extend that "goes away" to include consumption??

CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
HCO3-1 <-------> CO3-2

These are all in equilibrium, meaning they flow from left to right with
changes in pH. In order to remove CO2 (g) you ideally would want to shift
the equilibrium to the left by LOWERING the pH. This is where Boomer and I
disagree. I say you would have to lower the pH very low in order to
effectively remove CO2 by purging. Your fish would die first. But, I guess
if you purged for a VERY long time, you might be able to do it at a higer
pH. Not sure. Never tried it.

> where does 14 come from ??? is that just the highest Ph level??

The 14 comes from this relationship:

For pure water (contains no acids or bases): [OH-] = [H3O+] = 1.0 x10-7
mol/L. This means that the OH-1 concentration is the same as the H3O+
concentration and the concentration is 1x10-7

Kw for water = [OH-][H3O+] therefore Kw = 1.0 x10-14. = [OH-][H3O+] take
log of both sides and you get:

pOH + pH = 14.

> am I doing Ph wrong should it be pH?

pH. The p simply means negative log. You will also see pKa (negative log
of Ka). or pOH etc.

> --stoutman--Ok, you are going to try and 'purge' (the correct term) your
CO2 out with
> air. Yeah, I guess that would work. If you intentionally put the CO2 in
> there to begin with because you must have a higher concentration of CO2 in
> your tank than in the atmosphere. I don't intentionally put CO2 in my
tank.
> But I know some of you reef people due in Kalk reactors.
>
> wouldnt this tie in from people that have high Ph in there homes?? not the
outside air or
> the air at sea level? and wouldnt this higher level make it into the tank
water?? if not
> how/why?

Not sure what you mean by high pH in your home. A pH is the - log of the
hydronium ion CONCENTRATION. This usually refers to solutions.


>
> --stoutman--Alkalinity is buffering capacity. Your buffers begin to get
weakened with
> the addition of acid until they reach a point when they can no longer
> 'buffer' and the pH crashes.
>
> I dont get this!
>
> if by "buffer" your refering again to alkalinity how can I add co2 and
test for the
> alkalinity and get the same results ???

Your total alkalinity dosn't change. But it will be in a different form
depending on the pH

H2CO3 (carbonic acid) <------> HCO3-1 <-------> CO3-2
------------------------------------------>
increasing pH


>
>
> I ran out of time, i need to get real work done :( i know there were more
questions ill
> have to ask them later :) the formulas are making my head spin!!!
>

Ok.










>
>
>
> --
> Richard Reynolds
>
>
>

[stoutman]

Purging and Degassing are the same. But I wouldn't degas a solution of a
specific gas (CO2) with a gas (this case he was using air) that contains the
same gas I am trying to purge. You could degas with nitrogen, but this
would also degas other gases in solution, like a very important one, OXYGEN.


> IF i take 3L of asw put it in a tall conatiner and pump a lot of air into
it the Ph rises,
> but the Alk stays the same, I know thats what happens I do it daily. isnt
this because
> afterwards the water has less co2 than before?

asw?? You lost me. Not familiar with this term.

> alternatively IF i disconnect that air pump and plug in my co2 tank, the
Ph falls, and the
> Alk still stays the same, I also do this daily. isnt this because now the
water has more
> co2?

> wont both of these happen regardless of the alkalinity of the water?? if
not what
> alkalinity do I need to put more co2 into the water and keep the ph > 7??
>
>

> whats carbonic acid, where does it come from ??? and how does it
neutralize some of my
> 'buffer' ? and can algae's still consume it now or not?? can i test the
levels of
> carbonic acid? and what could be considered low/normal/high??

Carbonic acid forms from the reaction of CO2 (aqueous) and water. it is
H2CO3. It is an acid. It will drive the pH down effectively neutralizing
some of your buffer. You couldn't test for it because once it forms it is
quickly turned into HCO3- which is in equilibrium with CO3-. At pH 8-8.5.
You can, however test for your HCO3- and CO3-2 concentration. This is your
carbonate hardness also known as alkalinity.


> ok so how high does my alkalinity need to be to keep the ph from falling?
and what is a
> "sharp change" is not a starting Ph of 8.1 and an ending Ph of < 5.0(the
lowest I can
> test) a "sharp change" ? what time period does it have to happen in I
know i can make the
> change in under 5 minutes is that "sharp"?

Your pH is always going to fall. Your alkalinity prevents a rapid fall in
pH. What is the desired level of alkalinity for aquariums? Not sure on
this. I'm a chemist, not a marine biologist. You ideally would want the
most alkalinity you can without raising the pH out of spec.


> where does the hydronium ion come from when I add co2 ??? how does it go
away when the co2
> goes away? extend that "goes away" to include consumption??

CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
HCO3-1 <-------> CO3-2

These are all in equilibrium, meaning they flow from left to right with
changes in pH. In order to remove CO2 (g) you ideally would want to shift
the equilibrium to the left by LOWERING the pH. This is where Boomer and I
disagree. I say you would have to lower the pH very low in order to
effectively remove CO2 by purging. Your fish would die first. But, I guess
if you purged for a VERY long time, you might be able to do it at a higer
pH. Not sure. Never tried it.

> where does 14 come from ??? is that just the highest Ph level??

The 14 comes from this relationship:

For pure water (contains no acids or bases): [OH-] = [H3O+] = 1.0 x10-7
mol/L. This means that the OH-1 concentration is the same as the H3O+
concentration and the concentration is 1x10-7

Kw for water = [OH-][H3O+] therefore Kw = 1.0 x10-14. = [OH-][H3O+] take
log of both sides and you get:

pOH + pH = 14.

> am I doing Ph wrong should it be pH?

pH. The p simply means negative log. You will also see pKa (negative log
of Ka). or pOH etc.

> --stoutman--Ok, you are going to try and 'purge' (the correct term) your
CO2 out with
> air. Yeah, I guess that would work. If you intentionally put the CO2 in
> there to begin with because you must have a higher concentration of CO2 in
> your tank than in the atmosphere. I don't intentionally put CO2 in my
tank.
> But I know some of you reef people due in Kalk reactors.
>
> wouldnt this tie in from people that have high Ph in there homes?? not the
outside air or
> the air at sea level? and wouldnt this higher level make it into the tank
water?? if not
> how/why?

Not sure what you mean by high pH in your home. A pH is the - log of the
hydronium ion CONCENTRATION. This usually refers to solutions.


>
> --stoutman--Alkalinity is buffering capacity. Your buffers begin to get
weakened with
> the addition of acid until they reach a point when they can no longer
> 'buffer' and the pH crashes.
>
> I dont get this!
>
> if by "buffer" your refering again to alkalinity how can I add co2 and
test for the
> alkalinity and get the same results ???

Your total alkalinity dosn't change. But it will be in a different form
depending on the pH

H2CO3 (carbonic acid) <------> HCO3-1 <-------> CO3-2
------------------------------------------>
increasing pH


>
>
> I ran out of time, i need to get real work done :( i know there were more
questions ill
> have to ask them later :) the formulas are making my head spin!!!
>

Ok.























"Richard Reynolds" > wrote in message
news:NxAWb.21381$gl2.8769@lakeread05...
> > I really want to help you understand.
>
> ok so ive been following along :D
>
> and just to fill anyone who doesnt know in, I cant get from an "h" a "2"
and an "o" to
> make water :D
>
>
> but a few questions from all parts of the thread :D
>
> there have been some references to FW vs SW equasions for THIS email
everything is
> sal****er as FW doesnt concern me this much.
>
>
> --boomer--It is called "blowing it off" , such as with an airstone. If you
have high
> CO2 and add an airstone it will drive the CO2 off raising the pH.
>
> --stoutman--Ok, you are going to try and 'purge' (the correct term) your
CO2 out with
> air. Yeah, I guess that would work. If you intentionally put the CO2 in
> there to begin with because you must have a higher concentration of CO2 in
> your tank than in the atmosphere. I don't intentionally put CO2 in my
tank.
> But I know some of you reef people due in Kalk reactors
>
> what I understand boomer called "blowing it off" stoutman called it
"purge" and a few
> places I just checked call it degassing is that all the same thing or not
?? and if not
> what is the difference??
>
> IF i take 3L of asw put it in a tall conatiner and pump a lot of air into
it the Ph rises,
> but the Alk stays the same, I know thats what happens I do it daily. isnt
this because
> afterwards the water has less co2 than before?
>
> alternatively IF i disconnect that air pump and plug in my co2 tank, the
Ph falls, and the
> Alk still stays the same, I also do this daily. isnt this because now the
water has more
> co2?
>
> wont both of these happen regardless of the alkalinity of the water?? if
not what
> alkalinity do I need to put more co2 into the water and keep the ph > 7??
>
>
>
> --boomer--Bad term as Buffering Capacity isn't Alkalinity. Alk is more on
the order of ANC
> (Acid
> Neutralizing Capacity). BC is the ability to withstand upward and downward
trends in pH do
> to the addition of an acid or base.There is also a measurement called
Acidity ( B_aseNC
> and test kits for it). So the combination of the two more or les is BC.
But I know what
> you mean, may use the term ALK and BC interchangeably
>
> --stoutman-- Yes, the pH will drop with the addition of CO2. Remove CO2
will cause the
> pH to rise? How do you remove CO2? Once it is in solution it forms
> carbonic acid and neutralizes some of your 'buffer'.
>
> whats carbonic acid, where does it come from ??? and how does it
neutralize some of my
> 'buffer' ? and can algae's still consume it now or not?? can i test the
levels of
> carbonic acid? and what could be considered low/normal/high??
>
>
>
> --boomer--You can have all the alk you want in the world and it won't
help, in
> regards to CO2.
>
> --stoutman--Wrong. Alkalinity increases your tank's ability to RESIST
sharp changes in
> pH. This is what is meant by 'buffering capacity'.
>
> ok so how high does my alkalinity need to be to keep the ph from falling?
and what is a
> "sharp change" is not a starting Ph of 8.1 and an ending Ph of < 5.0(the
lowest I can
> test) a "sharp change" ? what time period does it have to happen in I
know i can make the
> change in under 5 minutes is that "sharp"?
>
>
> --stoutman--pH is the -log of the hydronium ion concentration. When the
hydronium ion
> concentration is very low, your system is basic (high pH). When the
> hydronium ion concentration is very large, your system is acidic (low pH).
>
> where does the hydronium ion come from when I add co2 ??? how does it go
away when the co2
> goes away? extend that "goes away" to include consumption??
>
> --stoutman--pH + pOH = 14. So yeah, you can calculate a pH from a pOH and
vice versa.
> But a pH of < 7 means acidic. pH > 7 means basic.
> pH can tell you something about acidity and basicity. It is a measurement
> of both, or the entire pH scale (1-14) if you will.
>
> where does 14 come from ??? is that just the highest Ph level??
>
> am I doing Ph wrong should it be pH?
>
> --stoutman--Ok, you are going to try and 'purge' (the correct term) your
CO2 out with
> air. Yeah, I guess that would work. If you intentionally put the CO2 in
> there to begin with because you must have a higher concentration of CO2 in
> your tank than in the atmosphere. I don't intentionally put CO2 in my
tank.
> But I know some of you reef people due in Kalk reactors.
>
> wouldnt this tie in from people that have high Ph in there homes?? not the
outside air or
> the air at sea level? and wouldnt this higher level make it into the tank
water?? if not
> how/why?
>
> and if you use co2 and Kalk its a really bad thing (trust me I know ) I
think you meant ca
> or calcium reactor.
>
> I add co2 to SW for a number of reasons mostly to help grow things, but
also to break down
> calcium in my calcium reactors.
>
> --booomer--If Alk resists changes in pH then why does CO2 lower the pH
without
> affecting the Alk.
>
> --stoutman--Alkalinity is buffering capacity. Your buffers begin to get
weakened with
> the addition of acid until they reach a point when they can no longer
> 'buffer' and the pH crashes.
>
> I dont get this!
>
> if by "buffer" your refering again to alkalinity how can I add co2 and
test for the
> alkalinity and get the same results ???
>
>
>
> I ran out of time, i need to get real work done :( i know there were more
questions ill
> have to ask them later :) the formulas are making my head spin!!!
>
>
>
>
>
> --
> Richard Reynolds
>
>
>

[Benjamin]

I think if this continues until everyone has a deeper understanding of
Alkalinity and we are using the same language to describe it and other terms
surrounding it all of us will end up winners.


I almost missed this thread! That would have made me a looser for sure.

--
--

My Web Site: http://showcase.netins.net/web/reefpage/


"Dinky" > wrote in message
hlink.net...
> I'm having some difficulty wrapping my brain around alkalinity and it's
> relationship to PH. Can anyone explain it in "Aquaria for idiots" fashion,
> or point me to a place where it's explained? I'm starting to feel like I
> need to take a couple BioChem classes.
>
> tia
>
> billy
>
> --
>
> --
>
>

[stoutman]

i didnt explain this part very good. Let me try again.

Kw for water = [OH-][H+] therefore Kw = 1.0 x10-14. = [OH-][H+] take
log of both sides and you get:

log[OH-] + log[H+] = -14

-log[OH-] - log[H+] = 14

(-log[OH-]) + (-log[H+]) = 14

pOH + pH = 14

p means take the negative log.












"stoutman" <.@.> wrote in message news:bhBWb.10208$jk2.32549@attbi_s53...
> Purging and Degassing are the same. But I wouldn't degas a solution of a
> specific gas (CO2) with a gas (this case he was using air) that contains
the
> same gas I am trying to purge. You could degas with nitrogen, but this
> would also degas other gases in solution, like a very important one,
OXYGEN.
>
>
> > IF i take 3L of asw put it in a tall conatiner and pump a lot of air
into
> it the Ph rises,
> > but the Alk stays the same, I know thats what happens I do it daily.
isnt
> this because
> > afterwards the water has less co2 than before?
>
> asw?? You lost me. Not familiar with this term.
>
> > alternatively IF i disconnect that air pump and plug in my co2 tank, the
> Ph falls, and the
> > Alk still stays the same, I also do this daily. isnt this because now
the
> water has more
> > co2?
>
> > wont both of these happen regardless of the alkalinity of the water?? if
> not what
> > alkalinity do I need to put more co2 into the water and keep the ph >
7??
> >
> >
>
> > whats carbonic acid, where does it come from ??? and how does it
> neutralize some of my
> > 'buffer' ? and can algae's still consume it now or not?? can i test the
> levels of
> > carbonic acid? and what could be considered low/normal/high??
>
> Carbonic acid forms from the reaction of CO2 (aqueous) and water. it is
> H2CO3. It is an acid. It will drive the pH down effectively neutralizing
> some of your buffer. You couldn't test for it because once it forms it is
> quickly turned into HCO3- which is in equilibrium with CO3-. At pH 8-8.5.
> You can, however test for your HCO3- and CO3-2 concentration. This is
your
> carbonate hardness also known as alkalinity.
>
>
> > ok so how high does my alkalinity need to be to keep the ph from
falling?
> and what is a
> > "sharp change" is not a starting Ph of 8.1 and an ending Ph of < 5.0(the
> lowest I can
> > test) a "sharp change" ? what time period does it have to happen in I
> know i can make the
> > change in under 5 minutes is that "sharp"?
>
> Your pH is always going to fall. Your alkalinity prevents a rapid fall in
> pH. What is the desired level of alkalinity for aquariums? Not sure on
> this. I'm a chemist, not a marine biologist. You ideally would want the
> most alkalinity you can without raising the pH out of spec.
>
>
> > where does the hydronium ion come from when I add co2 ??? how does it go
> away when the co2
> > goes away? extend that "goes away" to include consumption??
>
> CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
> HCO3-1 <-------> CO3-2
>
> These are all in equilibrium, meaning they flow from left to right with
> changes in pH. In order to remove CO2 (g) you ideally would want to shift
> the equilibrium to the left by LOWERING the pH. This is where Boomer and
I
> disagree. I say you would have to lower the pH very low in order to
> effectively remove CO2 by purging. Your fish would die first. But, I
guess
> if you purged for a VERY long time, you might be able to do it at a higer
> pH. Not sure. Never tried it.
>
> > where does 14 come from ??? is that just the highest Ph level??
>
> The 14 comes from this relationship:
>
> For pure water (contains no acids or bases): [OH-] = [H3O+] = 1.0 x10-7
> mol/L. This means that the OH-1 concentration is the same as the H3O+
> concentration and the concentration is 1x10-7
>
> Kw for water = [OH-][H3O+] therefore Kw = 1.0 x10-14. = [OH-][H3O+] take
> log of both sides and you get:
>
> pOH + pH = 14.
>
> > am I doing Ph wrong should it be pH?
>
> pH. The p simply means negative log. You will also see pKa (negative
log
> of Ka). or pOH etc.
>
> > --stoutman--Ok, you are going to try and 'purge' (the correct term) your
> CO2 out with
> > air. Yeah, I guess that would work. If you intentionally put the CO2
in
> > there to begin with because you must have a higher concentration of CO2
in
> > your tank than in the atmosphere. I don't intentionally put CO2 in my
> tank.
> > But I know some of you reef people due in Kalk reactors.
> >
> > wouldnt this tie in from people that have high Ph in there homes?? not
the
> outside air or
> > the air at sea level? and wouldnt this higher level make it into the
tank
> water?? if not
> > how/why?
>
> Not sure what you mean by high pH in your home. A pH is the - log of the
> hydronium ion CONCENTRATION. This usually refers to solutions.
>
>
> >
> > --stoutman--Alkalinity is buffering capacity. Your buffers begin to get
> weakened with
> > the addition of acid until they reach a point when they can no longer
> > 'buffer' and the pH crashes.
> >
> > I dont get this!
> >
> > if by "buffer" your refering again to alkalinity how can I add co2 and
> test for the
> > alkalinity and get the same results ???
>
> Your total alkalinity dosn't change. But it will be in a different form
> depending on the pH
>
> H2CO3 (carbonic acid) <------> HCO3-1 <-------> CO3-2
> ------------------------------------------>
> increasing pH
>
>
> >
> >
> > I ran out of time, i need to get real work done :( i know there were
more
> questions ill
> > have to ask them later :) the formulas are making my head spin!!!
> >
>
> Ok.
>
>
>
>
>
>
>
>
>
>
>
>
>
>
>
>
>
>
>
>
>
>
>
> "Richard Reynolds" > wrote in message
> news:NxAWb.21381$gl2.8769@lakeread05...
> > > I really want to help you understand.
> >
> > ok so ive been following along :D
> >
> > and just to fill anyone who doesnt know in, I cant get from an "h" a "2"
> and an "o" to
> > make water :D
> >
> >
> > but a few questions from all parts of the thread :D
> >
> > there have been some references to FW vs SW equasions for THIS email
> everything is
> > sal****er as FW doesnt concern me this much.
> >
> >
> > --boomer--It is called "blowing it off" , such as with an airstone. If
you
> have high
> > CO2 and add an airstone it will drive the CO2 off raising the pH.
> >
> > --stoutman--Ok, you are going to try and 'purge' (the correct term) your
> CO2 out with
> > air. Yeah, I guess that would work. If you intentionally put the CO2
in
> > there to begin with because you must have a higher concentration of CO2
in
> > your tank than in the atmosphere. I don't intentionally put CO2 in my
> tank.
> > But I know some of you reef people due in Kalk reactors
> >
> > what I understand boomer called "blowing it off" stoutman called it
> "purge" and a few
> > places I just checked call it degassing is that all the same thing or
not
> ?? and if not
> > what is the difference??
> >
> > IF i take 3L of asw put it in a tall conatiner and pump a lot of air
into
> it the Ph rises,
> > but the Alk stays the same, I know thats what happens I do it daily.
isnt
> this because
> > afterwards the water has less co2 than before?
> >
> > alternatively IF i disconnect that air pump and plug in my co2 tank, the
> Ph falls, and the
> > Alk still stays the same, I also do this daily. isnt this because now
the
> water has more
> > co2?
> >
> > wont both of these happen regardless of the alkalinity of the water?? if
> not what
> > alkalinity do I need to put more co2 into the water and keep the ph >
7??
> >
> >
> >
> > --boomer--Bad term as Buffering Capacity isn't Alkalinity. Alk is more
on
> the order of ANC
> > (Acid
> > Neutralizing Capacity). BC is the ability to withstand upward and
downward
> trends in pH do
> > to the addition of an acid or base.There is also a measurement called
> Acidity ( B_aseNC
> > and test kits for it). So the combination of the two more or les is BC.
> But I know what
> > you mean, may use the term ALK and BC interchangeably
> >
> > --stoutman-- Yes, the pH will drop with the addition of CO2. Remove CO2
> will cause the
> > pH to rise? How do you remove CO2? Once it is in solution it forms
> > carbonic acid and neutralizes some of your 'buffer'.
> >
> > whats carbonic acid, where does it come from ??? and how does it
> neutralize some of my
> > 'buffer' ? and can algae's still consume it now or not?? can i test the
> levels of
> > carbonic acid? and what could be considered low/normal/high??
> >
> >
> >
> > --boomer--You can have all the alk you want in the world and it won't
> help, in
> > regards to CO2.
> >
> > --stoutman--Wrong. Alkalinity increases your tank's ability to RESIST
> sharp changes in
> > pH. This is what is meant by 'buffering capacity'.
> >
> > ok so how high does my alkalinity need to be to keep the ph from
falling?
> and what is a
> > "sharp change" is not a starting Ph of 8.1 and an ending Ph of < 5.0(the
> lowest I can
> > test) a "sharp change" ? what time period does it have to happen in I
> know i can make the
> > change in under 5 minutes is that "sharp"?
> >
> >
> > --stoutman--pH is the -log of the hydronium ion concentration. When the
> hydronium ion
> > concentration is very low, your system is basic (high pH). When the
> > hydronium ion concentration is very large, your system is acidic (low
pH).
> >
> > where does the hydronium ion come from when I add co2 ??? how does it go
> away when the co2
> > goes away? extend that "goes away" to include consumption??
> >
> > --stoutman--pH + pOH = 14. So yeah, you can calculate a pH from a pOH
and
> vice versa.
> > But a pH of < 7 means acidic. pH > 7 means basic.
> > pH can tell you something about acidity and basicity. It is a
measurement
> > of both, or the entire pH scale (1-14) if you will.
> >
> > where does 14 come from ??? is that just the highest Ph level??
> >
> > am I doing Ph wrong should it be pH?
> >
> > --stoutman--Ok, you are going to try and 'purge' (the correct term) your
> CO2 out with
> > air. Yeah, I guess that would work. If you intentionally put the CO2
in
> > there to begin with because you must have a higher concentration of CO2
in
> > your tank than in the atmosphere. I don't intentionally put CO2 in my
> tank.
> > But I know some of you reef people due in Kalk reactors.
> >
> > wouldnt this tie in from people that have high Ph in there homes?? not
the
> outside air or
> > the air at sea level? and wouldnt this higher level make it into the
tank
> water?? if not
> > how/why?
> >
> > and if you use co2 and Kalk its a really bad thing (trust me I know ) I
> think you meant ca
> > or calcium reactor.
> >
> > I add co2 to SW for a number of reasons mostly to help grow things, but
> also to break down
> > calcium in my calcium reactors.
> >
> > --booomer--If Alk resists changes in pH then why does CO2 lower the pH
> without
> > affecting the Alk.
> >
> > --stoutman--Alkalinity is buffering capacity. Your buffers begin to get
> weakened with
> > the addition of acid until they reach a point when they can no longer
> > 'buffer' and the pH crashes.
> >
> > I dont get this!
> >
> > if by "buffer" your refering again to alkalinity how can I add co2 and
> test for the
> > alkalinity and get the same results ???
> >
> >
> >
> > I ran out of time, i need to get real work done :( i know there were
more
> questions ill
> > have to ask them later :) the formulas are making my head spin!!!
> >
> >
> >
> >
> >
> > --
> > Richard Reynolds
> >
> >
> >
>
>

[Richard Reynolds]

> > --boomer--It is called "blowing it off" , such as with an airstone. If you
> have high
> > CO2 and add an airstone it will drive the CO2 off raising the pH.
> >
> > --stoutman--Ok, you are going to try and 'purge' (the correct term) your
> CO2 out with
> > air. Yeah, I guess that would work. If you intentionally put the CO2 in
> > there to begin with because you must have a higher concentration of CO2 in
> > your tank than in the atmosphere. I don't intentionally put CO2 in my
> tank.
> > But I know some of you reef people due in Kalk reactors
> >
> > what I understand boomer called "blowing it off" stoutman called it
> "purge" and a few
> > places I just checked call it degassing is that all the same thing or not
> ?? and if not
> > what is the difference??
>
> Purging and Degassing are the same. But I wouldn't degas a solution of a
> specific gas (CO2) with a gas (this case he was using air) that contains the
> same gas I am trying to purge. You could degas with nitrogen, but this
> would also degas other gases in solution, like a very important one, OXYGEN.

now im way past lost. man i thought i was lost before.

are you saying if i bubble co2 it will lower the co2??? or if i bubble co2 itll lower the
oxygen ??

oxygen is overrated :D

> > IF i take 3L of asw put it in a tall conatiner and pump a lot of air into
> it the Ph rises,
> > but the Alk stays the same, I know thats what happens I do it daily. isnt
> this because
> > afterwards the water has less co2 than before?
>
> asw?? You lost me. Not familiar with this term.

generally refers to artificial salt water.

>
> > alternatively IF i disconnect that air pump and plug in my co2 tank, the
> Ph falls, and the
> > Alk still stays the same, I also do this daily. isnt this because now the
> water has more
> > co2?
>
> > wont both of these happen regardless of the alkalinity of the water?? if
> not what
> > alkalinity do I need to put more co2 into the water and keep the ph > 7??
> >
> >
>
> > whats carbonic acid, where does it come from ??? and how does it
> neutralize some of my
> > 'buffer' ? and can algae's still consume it now or not?? can i test the
> levels of
> > carbonic acid? and what could be considered low/normal/high??
>
> Carbonic acid forms from the reaction of CO2 (aqueous) and water. it is
> H2CO3. It is an acid. It will drive the pH down effectively neutralizing
> some of your buffer. You couldn't test for it because once it forms it is
> quickly turned into HCO3- which is in equilibrium with CO3-. At pH 8-8.5.
> You can, however test for your HCO3- and CO3-2 concentration. This is your
> carbonate hardness.

so what happens at ph 6? or less? understanding your not a biologist neither am I, but
can carbonic acid be consumed like co2 or not?

> > ok so how high does my alkalinity need to be to keep the ph from falling?
> and what is a
> > "sharp change" is not a starting Ph of 8.1 and an ending Ph of < 5.0(the
> lowest I can
> > test) a "sharp change" ? what time period does it have to happen in I
> know i can make the
> > change in under 5 minutes is that "sharp"?
>
> Your pH is always going to fall. Your alkalinity prevents a rapid fall in
> pH. What is the desired level of alkalinity for aquariums? Not sure on
> this. I'm a chemist, not a marine biologist. You ideally would want the
> most alkalinity you can without raising the pH out of spec.

so how much is that, can you work it backwards to keep my ph up but with tons of co2?

> > where does the hydronium ion come from when I add co2 ??? how does it go
> away when the co2
> > goes away? extend that "goes away" to include consumption??
>
> CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
> HCO3-1 <-------> CO3-2
>
> These are all in equilibrium, meaning they flow from left to right with
> changes in pH. In order to remove CO2 (g) you ideally would want to shift
> the equilibrium to the left by LOWERING the pH. This is where Boomer and I
> disagree. I say you would have to lower the pH very low in order to
> effectively remove CO2 by purging. Your fish would die first. But, I guess
> if you purged for a VERY long time, you might be able to do it at a higer
> pH. Not sure. Never tried it.

way past lost here, your saying if i lower the pH ill lower the co2???

> > where does 14 come from ??? is that just the highest Ph level??
>
> The 14 comes from this relationship:
>
> For pure water (contains no acids or bases): [OH-] = [H3O+] = 1.0 x10-7
> mol/L. This means that the OH-1 concentration is the same as the H3O+
> concentration and the concentration is 1x10-7
>
> Kw for water = [OH-][H3O+] therefore Kw = 1.0 x10-14. = [OH-][H3O+] take
> log of both sides and you get:
>
> pOH + pH = 14.
>
> > am I doing Ph wrong should it be pH?
>
> pH. The p simply means negative log. You will also see pKa (negative log
> of Ka). or pOH etc.

ok

>
> > --stoutman--Ok, you are going to try and 'purge' (the correct term) your
> CO2 out with
> > air. Yeah, I guess that would work. If you intentionally put the CO2 in
> > there to begin with because you must have a higher concentration of CO2 in
> > your tank than in the atmosphere. I don't intentionally put CO2 in my
> tank.
> > But I know some of you reef people due in Kalk reactors.
> >
> > wouldnt this tie in from people that have high Ph in there homes?? not the
> outside air or
> > the air at sea level? and wouldnt this higher level make it into the tank
> water?? if not
> > how/why?
>
> Not sure what you mean by high pH in your home. A pH is the - log of the
> hydronium ion CONCENTRATION. This usually refers to solutions.

sorry was meaining to say high co2 in the home. lowering the ph. its a common aquarium
problem

> > --stoutman--Alkalinity is buffering capacity. Your buffers begin to get
> weakened with
> > the addition of acid until they reach a point when they can no longer
> > 'buffer' and the pH crashes.
> >
> > I dont get this!
> >
> > if by "buffer" your refering again to alkalinity how can I add co2 and
> test for the
> > alkalinity and get the same results ???
>
> Your total alkalinity dosn't change. But it will be in a different form
> depending on the pH
>
> H2CO3 (carbonic acid) <------> HCO3-1 <-------> CO3-2
> ------------------------------------------>
> increasing pH

i guess i mis interpreted your statements I thought you said if i add co2 ill lower
alkalinity

>
>
> >
> >
> > I ran out of time, i need to get real work done :( i know there were more
> questions ill
> > have to ask them later :) the formulas are making my head spin!!!
> >
>
> Ok.

--
Richard Reynolds

[stoutman]

> > Purging and Degassing are the same. But I wouldn't degas a solution of
a
> > specific gas (CO2) with a gas (this case he was using air) that contains
the
> > same gas I am trying to purge. You could degas with nitrogen, but this
> > would also degas other gases in solution, like a very important one,
OXYGEN.
>
> now im way past lost. man i thought i was lost before.

Boomer was discussiing purging CO2 from his tank with by bubbling air. Air
contains CO2, as well as O2, N2 etc. Its a mixture of gases. I would think
that inorder to purge a gas from solution, you would not want the same gas
in the mixture you were using. In the case of air, CO2 is VERY low in
relation to the other gases. It's mostly nitrogen and oxygen. I'm NOT sure
if this would work or not. I never tried it. If you could I would think
you would need to LOWER the pH to do it effectively, but your fish, snails,
coral would hate you for ever! I wouldn't worry about removeing CO2.
Raise your alkalinity instead. I dont know about Boomer, but I use a
Venturi Skimmer, so I am already bubbling air into my tank like a mad man.



> are you saying if i bubble co2 it will lower the co2??? or if i bubble co2
itll lower the
> oxygen ??

Bubbling pure CO2 will raise your CO2(aq) levels effectively raising your
H2CO3 levels etc. No, with regard to oxygen, I said to purge effectively
you would ideally want to use a pure gas, like N2, but this would purge out
other gases as well. Dont worry about purging. Boomer didnt convince me it
works at the pH of an aquarium, but I never tried it and I'm not sure of
this. There are MORE effective things you can do to battle CO2. Maintain
a good ALKALINITY level.



> oxygen is overrated :D
>
> > > IF i take 3L of asw put it in a tall conatiner and pump a lot of air
into
> > it the Ph rises,
> > > but the Alk stays the same, I know thats what happens I do it daily.
isnt
> > this because
> > > afterwards the water has less co2 than before?
> >
> > asw?? You lost me. Not familiar with this term.
>
> generally refers to artificial salt water.
>

If the pH rises when you pump in air, than yeah, your most likely removeing
CO2. How long does it take?





> > > alternatively IF i disconnect that air pump and plug in my co2 tank,
the
> > Ph falls, and the
> > > Alk still stays the same, I also do this daily. isnt this because now
the
> > water has more
> > > co2?

YES.



> > > wont both of these happen regardless of the alkalinity of the water??
if
> > not what
> > > alkalinity do I need to put more co2 into the water and keep the ph >
7??
> > >
> > >
> >
> > > whats carbonic acid, where does it come from ??? and how does it
> > neutralize some of my
> > > 'buffer' ? and can algae's still consume it now or not?? can i test
the
> > levels of
> > > carbonic acid? and what could be considered low/normal/high??
> >
> > Carbonic acid forms from the reaction of CO2 (aqueous) and water. it is
> > H2CO3. It is an acid. It will drive the pH down effectively
neutralizing
> > some of your buffer. You couldn't test for it because once it forms it
is
> > quickly turned into HCO3- which is in equilibrium with CO3-. At pH
8-8.5.
> > You can, however test for your HCO3- and CO3-2 concentration. This is
your
> > carbonate hardness.
>
> so what happens at ph 6? or less? understanding your not a biologist
neither am I, but
> can carbonic acid be consumed like co2 or not?

Carbonic acid is in equilibrium with aqueous CO2. Can carbonic acid be
consumed? It gets consumed (neutralized) at higher pH's. It is still
there. Just its in a different form.



> > > ok so how high does my alkalinity need to be to keep the ph from
falling?
> > and what is a
> > > "sharp change" is not a starting Ph of 8.1 and an ending Ph of <
5.0(the
> > lowest I can
> > > test) a "sharp change" ? what time period does it have to happen in I
> > know i can make the
> > > change in under 5 minutes is that "sharp"?
> >
> > Your pH is always going to fall. Your alkalinity prevents a rapid fall
in
> > pH. What is the desired level of alkalinity for aquariums? Not sure on
> > this. I'm a chemist, not a marine biologist. You ideally would want
the
> > most alkalinity you can without raising the pH out of spec.
>
> so how much is that, can you work it backwards to keep my ph up but with
tons of co2?

In order to keep your pH up you need high alkalinity. To high alkalinity
will raise your pH out of spec.




> > > where does the hydronium ion come from when I add co2 ??? how does it
go
> > away when the co2
> > > goes away? extend that "goes away" to include consumption??
> >
> > CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
> > HCO3-1 <-------> CO3-2
> >
> > These are all in equilibrium, meaning they flow from left to right with
> > changes in pH. In order to remove CO2 (g) you ideally would want to
shift
> > the equilibrium to the left by LOWERING the pH. This is where Boomer
and I
> > disagree. I say you would have to lower the pH very low in order to
> > effectively remove CO2 by purging. Your fish would die first. But, I
guess
> > if you purged for a VERY long time, you might be able to do it at a
higer
> > pH. Not sure. Never tried it.
>
> way past lost here, your saying if i lower the pH ill lower the co2???


No, if you lower the pH you make it EASIER to purge out CO2. Remember, at
higher pH's the equilibrium (above) is shifted to the right, away from
CO2(solution)




> > > where does 14 come from ??? is that just the highest Ph level??
> >
> > The 14 comes from this relationship:
> >
> > For pure water (contains no acids or bases): [OH-] = [H3O+] = 1.0 x10-7
> > mol/L. This means that the OH-1 concentration is the same as the H3O+
> > concentration and the concentration is 1x10-7
> >
> > Kw for water = [OH-][H3O+] therefore Kw = 1.0 x10-14. = [OH-][H3O+]
take
> > log of both sides and you get:
> >
> > pOH + pH = 14.
> >
> > > am I doing Ph wrong should it be pH?
> >
> > pH. The p simply means negative log. You will also see pKa (negative
log
> > of Ka). or pOH etc.
>
> ok
>
> >
> > > --stoutman--Ok, you are going to try and 'purge' (the correct term)
your
> > CO2 out with
> > > air. Yeah, I guess that would work. If you intentionally put the CO2
in
> > > there to begin with because you must have a higher concentration of
CO2 in
> > > your tank than in the atmosphere. I don't intentionally put CO2 in my
> > tank.
> > > But I know some of you reef people due in Kalk reactors.
> > >
> > > wouldnt this tie in from people that have high Ph in there homes?? not
the
> > outside air or
> > > the air at sea level? and wouldnt this higher level make it into the
tank
> > water?? if not
> > > how/why?
> >
> > Not sure what you mean by high pH in your home. A pH is the - log of
the
> > hydronium ion CONCENTRATION. This usually refers to solutions.
>
> sorry was meaining to say high co2 in the home. lowering the ph. its a
common aquarium
> problem
>
> > > --stoutman--Alkalinity is buffering capacity. Your buffers begin to
get
> > weakened with
> > > the addition of acid until they reach a point when they can no longer
> > > 'buffer' and the pH crashes.
> > >
> > > I dont get this!
> > >
> > > if by "buffer" your refering again to alkalinity how can I add co2 and
> > test for the
> > > alkalinity and get the same results ???
> >
> > Your total alkalinity dosn't change. But it will be in a different form
> > depending on the pH
> >
> > H2CO3 (carbonic acid) <------> HCO3-1 <-------> CO3-2
> > ------------------------------------------>
> > increasing pH
>
> i guess i mis interpreted your statements I thought you said if i add co2
ill lower
> alkalinity


No, if you add CO2 you increase CO2(aq) and increase H2CO3 etc. And you
lower pH. Not alkalinity. If I said alkalinity, it was a misprint :)


> >
> >
> > >
> > >
> > > I ran out of time, i need to get real work done :( i know there were
more
> > questions ill
> > > have to ask them later :) the formulas are making my head spin!!!
> > >
> >
> > Ok.
>
> --
> Richard Reynolds
>
>
>

[Dragon Slayer]

"stoutman" <.@.> wrote in message news:o7vWb.8098$yE5.29639@attbi_s54...
> Good one Dragon Slayer. Do people STILL play D&D?????????????


I haven't a clue. do they teach chemistry and alkalinity in it?

kc

[Richard Reynolds]

I should inform you that I have a different reason for asking. I know what booomer says,
and I know what he says works cause ive done it :D and i know boomer has gone over some of
this with me before and even a little of that sunk in :D

> Boomer was discussiing purging CO2 from his tank with by bubbling air. Air
> contains CO2, as well as O2, N2 etc. Its a mixture of gases. I would think
> that inorder to purge a gas from solution, you would not want the same gas
> in the mixture you were using.

ok now I get what you are saying, now another question does every piece (molecule????) of
co2 endup in your carbonic acid??
i spent a few moments searching it *seems* that it doesnt all endup as carbonic acid,
mostly because carbonic acid is not bio available to microalgae(remember quick search),
and I know that the microalgae grows like mad when you add co2.

> In the case of air, CO2 is VERY low in
> relation to the other gases. It's mostly nitrogen and oxygen. I'm NOT sure
> if this would work or not. I never tried it. If you could I would think
> you would need to LOWER the pH to do it effectively, but your fish, snails,
> coral would hate you for ever! I wouldn't worry about removeing CO2.
> Raise your alkalinity instead. I dont know about Boomer, but I use a
> Venturi Skimmer, so I am already bubbling air into my tank like a mad man.

if your alkalinity is too high in a fish/reef tank you will have other problems. also
though outside air might be low in co2, co2 is a problem for people using certain types of
heating and other issues. and degassing for them does work. the same goes for a really
highly packed tank, think about 1000 clowns breathing in 50 gallons of water.

i have several issues, my microalgae I try to add as much co2 as i posssibly can, and
remove as much oxygen w/o removing nitrogen as I can. with my high densitie rotifer and
brine shrimp cultures (small invertibrates) i need to remove co2 and add oxygen without it
the cultures will crash. the air's co2 content means nothing as the culture consumes one
and releases the other. after all a tank full of salt water alone isnt very exciting :D

> Bubbling pure CO2 will raise your CO2(aq) levels effectively raising your
> H2CO3 levels etc. No, with regard to oxygen, I said to purge effectively
> you would ideally want to use a pure gas, like N2, but this would purge out
> other gases as well. Dont worry about purging. Boomer didnt convince me it
> works at the pH of an aquarium, but I never tried it and I'm not sure of
> this. There are MORE effective things you can do to battle CO2. Maintain
> a good ALKALINITY level.

IF your alk is too high you end up with calcium levels that are out of wack, also not
being the chemist ill leave boomer or someone else to explain that ratio.

> If the pH rises when you pump in air, than yeah, your most likely removeing
> CO2. How long does it take?

minutes. the exact time depends and I dont know enough about the variables to tell the
difference. under 1 when I use oxygen instead of room air.

> neutralizing
> > > some of your buffer. You couldn't test for it because once it forms it
> is
> > > quickly turned into HCO3- which is in equilibrium with CO3-. At pH
> 8-8.5.
> > > You can, however test for your HCO3- and CO3-2 concentration. This is
> your
> > > carbonate hardness.
> >
> > so what happens at ph 6? or less? understanding your not a biologist
> neither am I, but
> > can carbonic acid be consumed like co2 or not?
>
> Carbonic acid is in equilibrium with aqueous CO2. Can carbonic acid be
> consumed? It gets consumed (neutralized) at higher pH's. It is still
> there. Just its in a different form.

actually co2 consumed by algaes and other plant life. from a few moments of a search
carbonic acid is not, BUT it is possible that the algae/plants can seperate the two and
then consume the co2, they will do that for other things and I dont know yet about
carbonic acid.

> In order to keep your pH up you need high alkalinity. To high alkalinity
> will raise your pH out of spec.

ok but isnt that a reaction that can be measured the co2 will lower the pH how high does
my alkalinity need to be to keep the pH between 8 and 10?? with a high co2 level, I cant
find the chart boomer gave me to measure co2 levels but the with an alk of 3meq/l and a ph
of say 6

> No, if you lower the pH you make it EASIER to purge out CO2. Remember, at
> higher pH's the equilibrium (above) is shifted to the right, away from
> CO2(solution)

I still dont quite understand that part. but thats ok for now.

> No, if you add CO2 you increase CO2(aq) and increase H2CO3 etc. And you
> lower pH. Not alkalinity. If I said alkalinity, it was a misprint :)

aha


--
Richard Reynolds

[Dinky]

"Marc Levenson" > wrote in message
...
> Boomer, we all have our strengths and weaknesses. Why is chemistry so
fascinating to you? I
> was following along for a while, but it just got to close to molecular
biology for me to
> continue... ;)


As the OP, I felt some kind of responsibility to keep reading. I'm
hopelessly lost....Stout and Boomer gonna just kill each other and be done
with it, or what? <g>

billy

[stoutman]

> ok now I get what you are saying, now another question does every piece
(molecule????) of
> co2 endup in your carbonic acid??

NO. CO2(g) is in equilibrium with CO2(aq). The equilibrium is a FUNCTION
of pH.

Have you ever added an acid (vinegar) to a baking soda solution and watched
it bubble as a kid?? This is the reaction. The sodium ion is not included
in the equilibrium for simplicity. I think this will help.

CO2 (g) <-------> CO2 (aq) <-------> H2CO3 <-------> HCO3- <-------> H+ +
CO3-2

The baking soda (Na+ HCO3-) solution starts out to the RIGHT side of the
above equilibrium. When you add acid (vinegar) you are pushing the
equilibrium to the left. At low pH's carbonic acid is decomposes to give
CO2 (aq) which bubbles out of solution CO2(g). This is an example of what I
mean when I say that CO2 will purge out of solution EASIER at LOWER pH's.
As the pH gets lower (more vinegar added) the bubbling gets more vigorous.

> I should inform you that I have a different reason for asking.

Your sneaky :)

> minutes. the exact time depends and I dont know enough about the
variables to tell the
> difference. under 1 when I use oxygen instead of room air

As I mentioned earlier, it should be faster with a pure gas. You used pure
O2. Should be faster than using a room air and an air stone/pump.

> I still dont quite understand that part. but thats ok for now.
See above.


I don't know how many more posts I can make on this topic. Some are even
kill filing me, so some are not even seeing this. This may be my last post
in this thread. I think this topic has been exhausted and so am I.






"Richard Reynolds" > wrote in message
news:XjFWb.22012$gl2.17121@lakeread05...
> I should inform you that I have a different reason for asking. I know
what booomer says,
> and I know what he says works cause ive done it :D and i know boomer has
gone over some of
> this with me before and even a little of that sunk in :D
>
> > Boomer was discussiing purging CO2 from his tank with by bubbling air.
Air
> > contains CO2, as well as O2, N2 etc. Its a mixture of gases. I would
think
> > that inorder to purge a gas from solution, you would not want the same
gas
> > in the mixture you were using.
>
> ok now I get what you are saying, now another question does every piece
(molecule????) of
> co2 endup in your carbonic acid??
> i spent a few moments searching it *seems* that it doesnt all endup as
carbonic acid,
> mostly because carbonic acid is not bio available to microalgae(remember
quick search),
> and I know that the microalgae grows like mad when you add co2.
>
> > In the case of air, CO2 is VERY low in
> > relation to the other gases. It's mostly nitrogen and oxygen. I'm NOT
sure
> > if this would work or not. I never tried it. If you could I would
think
> > you would need to LOWER the pH to do it effectively, but your fish,
snails,
> > coral would hate you for ever! I wouldn't worry about removeing CO2.
> > Raise your alkalinity instead. I dont know about Boomer, but I use a
> > Venturi Skimmer, so I am already bubbling air into my tank like a mad
man.
>
> if your alkalinity is too high in a fish/reef tank you will have other
problems. also
> though outside air might be low in co2, co2 is a problem for people using
certain types of
> heating and other issues. and degassing for them does work. the same goes
for a really
> highly packed tank, think about 1000 clowns breathing in 50 gallons of
water.
>
> i have several issues, my microalgae I try to add as much co2 as i
posssibly can, and
> remove as much oxygen w/o removing nitrogen as I can. with my high
densitie rotifer and
> brine shrimp cultures (small invertibrates) i need to remove co2 and add
oxygen without it
> the cultures will crash. the air's co2 content means nothing as the
culture consumes one
> and releases the other. after all a tank full of salt water alone isnt
very exciting :D
>
> > Bubbling pure CO2 will raise your CO2(aq) levels effectively raising
your
> > H2CO3 levels etc. No, with regard to oxygen, I said to purge
effectively
> > you would ideally want to use a pure gas, like N2, but this would purge
out
> > other gases as well. Dont worry about purging. Boomer didnt convince
me it
> > works at the pH of an aquarium, but I never tried it and I'm not sure of
> > this. There are MORE effective things you can do to battle CO2.
Maintain
> > a good ALKALINITY level.
>
> IF your alk is too high you end up with calcium levels that are out of
wack, also not
> being the chemist ill leave boomer or someone else to explain that ratio.
>
> > If the pH rises when you pump in air, than yeah, your most likely
removeing
> > CO2. How long does it take?
>
> minutes. the exact time depends and I dont know enough about the
variables to tell the
> difference. under 1 when I use oxygen instead of room air.
>
> > neutralizing
> > > > some of your buffer. You couldn't test for it because once it forms
it
> > is
> > > > quickly turned into HCO3- which is in equilibrium with CO3-. At pH
> > 8-8.5.
> > > > You can, however test for your HCO3- and CO3-2 concentration. This
is
> > your
> > > > carbonate hardness.
> > >
> > > so what happens at ph 6? or less? understanding your not a biologist
> > neither am I, but
> > > can carbonic acid be consumed like co2 or not?
> >
> > Carbonic acid is in equilibrium with aqueous CO2. Can carbonic acid be
> > consumed? It gets consumed (neutralized) at higher pH's. It is still
> > there. Just its in a different form.
>
> actually co2 consumed by algaes and other plant life. from a few moments
of a search
> carbonic acid is not, BUT it is possible that the algae/plants can
seperate the two and
> then consume the co2, they will do that for other things and I dont know
yet about
> carbonic acid.
>
> > In order to keep your pH up you need high alkalinity. To high
alkalinity
> > will raise your pH out of spec.
>
> ok but isnt that a reaction that can be measured the co2 will lower the pH
how high does
> my alkalinity need to be to keep the pH between 8 and 10?? with a high co2
level, I cant
> find the chart boomer gave me to measure co2 levels but the with an alk of
3meq/l and a ph
> of say 6
>
> > No, if you lower the pH you make it EASIER to purge out CO2. Remember,
at
> > higher pH's the equilibrium (above) is shifted to the right, away from
> > CO2(solution)
>
> I still dont quite understand that part. but thats ok for now.
>
> > No, if you add CO2 you increase CO2(aq) and increase H2CO3 etc. And you
> > lower pH. Not alkalinity. If I said alkalinity, it was a misprint :)
>
> aha
>
>
> --
> Richard Reynolds
>
>
>

[Boomer]

"I am not sure if you are just messing with me "

Yes, messing with you, it is called trolling a troll, to see where the hell you would go
and what you would say in regards to last posts. It is called honesty, of which you have
none off to say the least,that I can see.You always like to post what suits you and just
avoid ref I give. So lets start where you are WRONG and have a great lack of understanding
of things, to include pointing out all your gross error which you still FAIL to
acknowledge and which can be prove in many water chem. ref. .I doubt like hell you are a
chemist at all.You seem to want to con people into thinkin' you are. But then again, I
have seen chemists like you before, they are not familiar with the, but they ASK to have
it explained and ask for REF.YOU just shoot from the hip. WHAT GETS YOU IN TROUBLE. You
remind me of snoot-noise kid that come here and other NG's and forums...that think they
know, buy hey, maybe I'm wrong :-)



1). Acidity

"***Benjamin,Water Chemistry (2002, pages 262-263).***

***Acidity A concept that is exactly analogous to alkalinity but measures the base
neutralizing
capacity (BNC) of a solution is Acidity. The quantitative represents the concentration of
OH- ions that must be added to titrate the solution to a pH near 10.5***

So that means that not only in Benjamin wrong but, so are Stumm & Morgan, Millero, Pilosn,
Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I said, you have your
acidity and Acidy mixed up. Acidity as defined above is covered in most water chemistry
books, written by chemists, who's field of expertise is water chemistry. You can even buy
Acidity test kits from, HACH, LaMotte, etc..

You mean you didn't read this or are you just avoiding it .The same definition can be
found in almost any std water chemistry book.

I have run into few chemists, that are NOT familiar with the above. Some water reports
require the above Acidity measuring. The issue with you is you do not understand WATER
CHEMISTRY. Everything you have posted can be found a general chemistry book




2) Alk and BC

From the link

Alkalinity
***Acid neutralizing or buffering capacity of water; a measure of the ability of water to
resist changes in pH caused by the addition of acids or bases ***

This is a Buffering Capacity definition not Alk

Humm, since when does Alk have anything to do in regards to the addition of BASE. As I
pointed out in the first post the term is often miss used. Even in YOUR own posts you say
it is based on a acid addition, no mention of **base or acid** addition by you. Are you
getting confused or what. Or is more you are trying to confuse everyone you are right. The
above is a definition for Buffer Capacity NOT Alk

From Drew, Geochemistry of Natural Waters

"alkalinity, which is formally defined as the equivalent sum of bases that are titratable
with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH of the solution is
progressively lowered by the addition of a strong acid (HCL), all the anions on the right
will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4, H2S,organic acids, H20)"

This follows almost all description of Alk, that it is acid neutralizing reaction and has
nothing to do with base neutralizing, which is Acidity (BNC) .I defined these before you
had no comment


Even the links that give the Buffering Capacity definition is wrong, as is the UIPAC on
Alkalinity. Alkalinity has nothing to do with the addition of bases only acids. When you
use the words "base and acid" it becomes BC

Even YOU MUST disagree with these definitions, from YOUR own post

Think of alkalinity as 'buffering capacity'. Or the ability of a solution
***to resist a drop in pH due to the addition of acid***

Where the flip is the base addition forget it ?

From Butler; Carbon Dioxide Equilibrium and Their Applications (professor emeritus
Harvard University) an expert on the subject.

Buffering Index (Buffering Capacity, Buffer Intensity).

***This concept was first developed for mixtures of approximately equal proportions of
conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such buffer solutions
strongly resist changes in pH when acids or bases are added and are useful as pH
standards. The Buffer Index tells how great the resistance to pH changes will be.**

also from Butler

Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]

Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]

Acidity is in fact just the negative of Alkalinity ***

http://www.lagoonsonline.com/acid.htm

http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.htm?E+mystore

It sure is funny how all of the chemist that write water chemistry textbooks never say Alk
is the Buffering Capacity of a solution. They are always treated and defined separately.

If you or others choose to treat Alk and BC as the same, well, just have at it. As I said
in first post I know what you mean.

"No need to cite web pages that describe what I know and what I wrote
in this discussion"

No you don't know, who are you trying to convince any way, me, the guys here and/or all
the water chemists in this world. As I said before go get a dam WATER CHEMISTRY book or
shut the hell up.You keep trying to define things from a general chemistry book WE ARE IN
THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.





3). pKa's and what you don't know or seem to be confused on

"Therefore, it has two pKa's
(pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35. The
pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
right in there. Is that magic? :)"

Here it is agin that is twice at least

"The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this example)
you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium will
be shifted to HCO3-2 by a ratio of 1:100.

Oh wait , there is a third time LOL

"At the pH of seawater, the buffering capacity of carbonate is at it's
weakest. It's strongest buffering is at a pH of 6.4 and 10.3."


Lets just dunk you on this one. I am taking note you refuse to reply to YOUR errors

So you calculated the pH of seawater with freshwater pKa's, now that is a good trick. From
a number of seawater chemistry books the seawater pKa's are 6 & 9.1, so according to you,
seemingly not understanding your favorite Henderson-Hasselbach equation;

2 pH = (6 + 9.1) /2 pH = 7.55

I have never seen seawater with a pH of 7.55. There is no ocean with that pH. Humm how
come your equation is not working for you today.?


"That pH I calculated is
right in there. Is that magic? :)"

I roll on the floor when I see this = 8.35

Hum , just a brain far so excuse me for thinkin

(pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35

Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a pH of 8.35 there pal
? That 8.35 is what you are telling people the pH should be, but their meter says 6.4.
This how people will READ this.




4.) More on Buffering Capacity

"Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes, your
alkalinity equation."'


Yup, I see that and in this case the HCO3 is the acid and the CO3 is the base CORRECT. In
Alk you are only dealing with bases and how they react to an acid. Acidity deals acids and
how they recact to bases "Acidity, A concept that is exactly analogous to alkalinity but
measures the base neutralizing
capacity (BNC) of a solution is Acidity "Alk is the ANC Acid neutralizing capacity

"Don't the components of a buffer account for the buffering capacity? "

Yes, they do but so do the acids which work as buffers. NaHCO3 is a buffer and can act as
an acid or base

*** Buffering Capacity.**
The power of a substance in solution to absorb acid or alkali without change in pH; this
is highest at a pH value equal to the pKa value of the acid of the buffer pair.***

***Akalinity***
Measure of the power of a solution to neutralise hydrogen ions (H+), usually expressed as
the equivalent concentration (mg/L) of calcium carbonate (CaCO3).


If one wants to call Alk Buffering capacity then one sure as a hell can call Acidty
Buffering Capacity also. As it is the ability to neutralizes an acid that is a buffer.You
have a pH of 7 and you add a buffer to lower it to a pH of 4, you are buffering the water,
that buffer is a acid.

5) CO2

You are really confuse so it seems :-) You realllllllly indicate that CO2 is affected by
the Alk or vise-versa

"Yes, the pH will drop with the addition of CO2. Remove CO2 will cause the
pH to rise? How do you remove CO2? Once it is in solution it forms
carbonic acid and neutralizes some of your 'buffer'."

"With the exception of CO2?"

No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
Concepts)....PERIOD.You seem to think a that at least in two of your post that CO2 is
affected by the Alk or vise-versa. Please go back to school or seek professor

"Why in one case does CO2 from air lower pH and in the other case it raises
it? Doesn't make sense."

That is because you don't understand CO2 period. By the way I saved this, wanted to see
if you would bite on the post I gave. Not bite at first, so time to reel you in, as you
did bite in another post..

Lets make some sense of it for you, being that you have a pH.D in chemistry, so you say .

CO2 is naturally generated in a aquatic systems, it is capable of raise to various levels
depending on a number of circumstances .It can be measure (except in seawater) or
calculated using Buch/Park Equations (what we use for seawater. In sort if you know the pH
and Alk you can calculate the CO2). If you aerate a system or a sample of water, even if
the pH has only dropped a couple of tenths, due to an increase in CO2, the CO2 will leave
solution to the atmosphere.This will raise the pH. On the other hand if theCO2 level is
more of the norm and you have hikgh room air, such as in the winter, the partial pressure
of the CO2 in air will be much higher than that in water, in which case the CO2 will enter
the water and lower the pH. That is without an airstone. Adding an airstone will make it
even worse,as you are now forcefully driving the CO2 into solution even quicker. These
test /experiments have been proven many times, it is not that may work could work they do
work.Yet you want to disagree and in another post say you haven't tried it,.Seems to me
that based on what you say it can't work So, in short you don't know what the hell you are
taking about. Go get a glass of seawater with a pH of about 8.3 and lower it to about
8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK- UP ( that is if you
don't have a high room air CO2 problem.). This little test has been done thousands of
times in this hobby, with test kits, pH meters and even graphic printers.

"This is where Boomer and I
disagree. I say you would have to lower the pH very low in order to
effectively remove CO2 by purging."

You are 100 % wrong. Please come to our Chem forum and try and run that by Randy, don't
take my word on it. I already know what he will say.

"Boomer didnt convince me it
works at the pH of an aquarium, but I never tried it and I'm not sure of
this. "

Well then come too our chem. forum and tell Randy he doesn't know what he is talking about
LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it should be easy for
you to run the experiment LOL There are grade school kids that run the test and know what
happens and that I'm correct.


"The equilibrium is a FUNCTION
of pH."

It is also a function of Alk or don't you know that. At a pH of 8.3, Alk 2.25, the CO2 is
about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk to about .4 meq/ l
or so the CO2 will be around .99 mg / l CO2, When dealing with tanksCO2 is not always in
equilibrium with ambient air.


". But I wouldn't degas a solution of a
specific gas (CO2) with a gas (this case he was using air) that contains the
same gas I am trying to purge."

Why not ? We have a guy right now that is running tests on purging ambient air with a
solution to remove CO2 gas from the air, before it enters the tank per/Randy's suggestion.
The same guy is doing some of my test using a Clinoptilolite, a Zeolite mineral, that has
an affinity for CO2.This will be a dry CO2 scrubber


Sorry Soutman but you sure as hell don't seem to know much about aquatic chemistry. You
seem to be guessing at everything.

By the way have you read any of Randy's technical articles on water chemistry, been saving
these for last. There are a few on pH, Alk, CO2 .Here is a list

Try and answer them 1-5 and lets see where we get THIS TIME :-) or maybe we should just
drop it. I could care less at this point.

THE END


ARTICLES

The first two posts in this thread are lists of some of my articles that relate to reef
tank chemistry. In the next few posts are some of the articles published by Craig Bingman
and others on reef chemistry issues.

The first two posts in this thread are lists of some of my articles that relate to reef
tank chemistry. In the next few posts are some of the articles published by Craig Bingman
and others on reef chemistry issues.

Solving Common Problems

Solving Calcium and Alkalinity Problems
http://www.advancedaquarist.com/issues/nov2002/chem.htm

Solutions to pH Problems
http://www.advancedaquarist.com/iss...ne2002/chem.htm

How to Select a Calcium and Alkalinity Supplementation Scheme
http://www.advancedaquarist.com/issues/feb2003/chem.htm

Phosphate Issues
http://www.advancedaquarist.com/iss...pt2002/chem.htm

Nitrate Issues
http://www.advancedaquarist.com/iss...st2003/chem.htm



Calcium and Alkalinity

Solving Calcium and Alkalinity Problems
http://www.advancedaquarist.com/issues/nov2002/chem.htm

How to Select a Calcium and Alkalinity Supplementation Scheme
http://www.advancedaquarist.com/issues/feb2003/chem.htm

Calcium and Alkalinity Balance Issues
http://reefkeeping.com/issues/2002-...ature/index.htm

Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
http://www.advancedaquarist.com/iss...ly2002/chem.htm

The Relationship Between Alkalinity and pH.
http://www.advancedaquarist.com/issues/may2002/chem.htm

The Chemical & Biochemical Mechanisms of Calcification in Corals
http://www.advancedaquarist.com/issues/apr2002/chem.htm

Calcium
http://www.advancedaquarist.com/issues/mar2002/chem.htm

Alkalinity
http://www.advancedaquarist.com/iss...2/chemistry.htm


Iron

First Iron Article: Macroalgae and Dosing Recommendations
http://www.advancedaquarist.com/issues/aug2002/chem.htm

Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
http://www.advancedaquarist.com/issues/oct2002/chem.htm

Iodine

Iodine in Marine Aquaria: Part I
http://www.advancedaquarist.com/issues/mar2003/chem.htm

Iodine in Reef Tanks 2: Effects on Macroalgae Growth
http://www.advancedaquarist.com/iss...il2003/chem.htm


Magnesium and Strontium

Strontium
http://www.advancedaquarist.com/issues/nov2003/chem.htm

Magnesium
http://www.advancedaquarist.com/issues/oct2003/chem.htm

Magnesium and Strontium in Limewater
http://www.advancedaquarist.com/issues/dec2003/chem.htm


Limewater (kalkwasser)

The Self Purification of Limewater (Kalkwasser)
http://www.advancedaquarist.com/issues/may2003/chem.htm

The Degradation of Limewater (Kalkwasser) in Air
http://reefkeeping.com/issues/2003-...ature/index.htm

How to Select a Calcium and Alkalinity Supplementation Scheme
http://www.advancedaquarist.com/issues/feb2003/chem.htm

Metals in Aquaria

Aluminum and aluminum-based phosphate binders
http://www.advancedaquarist.com/iss...ly2003/chem.htm

Reef Aquaria with Low Soluble Metals
http://reefkeeping.com/issues/2003-...ature/index.htm

Tap Water in Reef Aquaria
http://www.advancedaquarist.com/issues/jan2004/chem.htm
First Iron Article: Macroalgae and Dosing Recommendations
http://www.advancedaquarist.com/issues/aug2002/chem.htm

Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
http://www.advancedaquarist.com/issues/oct2002/chem.htm


Test Kit Reviews

The Seachem Borate Alkalinity Test Kit
http://www.advancedaquarist.com/iss...ne2003/chem.htm

The Salifert Boron Test Kit
http://www.advancedaquarist.com/iss...pt2003/chem.htm

Boron and Borate (and pH buffering)

Boron in a Reef Tank (and its effect on pH buffering)
http://www.advancedaquarist.com/issues/dec2002/chem.htm

The Seachem Borate Alkalinity Test Kit
http://www.advancedaquarist.com/iss...ne2003/chem.htm

The Salifert Boron Test Kit
http://www.advancedaquarist.com/iss...pt2003/chem.htm



Others

Tap Water in Reef Aquaria
http://www.advancedaquarist.com/issues/jan2004/chem.htm

ORP
http://reefkeeping.com/issues/2003-...ature/index.htm

Chloramine
http://reefkeeping.com/issues/2003-...ature/index.htm

Silica in a Reef Tank
http://advancedaquarist.com/issues/jan2003/feature.htm

Specific Gravity (and temperature correction of hydrometers)
http://www.advancedaquarist.com/iss...2/chemistry.htm


The Complete Nitrogen Cycle
http://www.animalnetwork.com/fish/l...a&RecordNo=3090

Magnesium (older article with fonts screwed up)
http://www.aquariumfish.com/aquariu...cid=124&search=

Phosphate (older article now reproduced in a poor fashion)
http://www.aquariumfish.com/aquariu...cid=124&search=

Carbon Dioxide
http://www.animalnetwork.com/fish/l...a&RecordNo=2074

Using Conductivity to Measure Salinity
http://www.aquariumfish.com/aquariu...cid=124&search=

Understanding Seawater
http://www.animalnetwork.com/fish2/...s/1/default.asp

Protein Skimming: How It Works
http://home.mweb.co.za/jv/jv79/reef/skimmers2.html



Articles by Craig Bingman:

Carbon Dioxide tests
http://www.animalnetwork.com/fish/l...n=&RecordNo=279

Limewater, Acetic Acid and Sand Clumping
http://www.animalnetwork.com/fish/l...n=&RecordNo=181

Calcium and Alkalinity
http://www.animalnetwork.com/fish2/...bio/default.asp

Calculation of Calcium Carbonate Saturation States in Reef Aquaria
http://www.animalnetwork.com/fish2/...bio/default.asp


Calcification Rates in Several Tropical Coral Reef Aquaria
http://www.animalnetwork.com/fish2/...bio/default.asp

Limits To Limewater...Revisited
http://www.animalnetwork.com/fish2/...bio/default.asp

Expanding the Limits of Limewater: Adding Organic Carbon Sources (vinegar)
http://www.animalnetwork.com/fish2/...bio/default.asp


Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
http://www.animalnetwork.com/fish2/...bio/default.asp

Magnesium - Part I
http://www.animalnetwork.com/fish2/...bio/default.asp

Magnesium - Part II
http://www.animalnetwork.com/fish2/...bio/default.asp

A Homemade Magnesium Supplement
http://www.animalnetwork.com/fish2/...bio/default.asp

Simulating the Effect of Calcium Chloride and Sodium Bicarbonate Additions on Reef Systems
http://www.animalnetwork.com/fish2/...bio/default.asp

Additional Simulations: The Combined Effect Of Calcium Chloride
/Sodium Bicarbonate Additions And Water Exchanges
http://www.animalnetwork.com/fish2/...bio/default.asp


More articles by Craig Bingman:

The Halogens - Part I: Bromine in Seawater and Aquaria
http://www.animalnetwork.com/fish2/...bio/default.asp

The Halogens - Part II: Fluoride
http://www.animalnetwork.com/fish2/...bio/default.asp

Fluoride Depletion In Four Reef Aquariums
http://www.animalnetwork.com/fish2/...bio/default.asp

The Halogens - Part III: Iodine
http://www.animalnetwork.com/fish2/...bio/default.asp

Measuring Halides
http://www.animalnetwork.com/fish2/...bio/default.asp

How Test Kits Work
http://www.animalnetwork.com/fish2/...bio/default.asp

Borax pH Calibration
http://www.animalnetwork.com/fish2/...bio/default.asp

A pH Detective Story
http://www.animalnetwork.com/fish2/...bio/default.asp

How to Mix a Batch of Synthetic Seawater in Under Five Minutes
http://www.animalnetwork.com/fish2/...bio/default.asp

Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
http://www.animalnetwork.com/fish2/...bio/default.asp

SILICON - FOE OR FRIEND?
http://www.animalnetwork.com/fish2/...s/1/default.asp

The Composition Of Several Synthetic Seawater Mixes
http://www.animalnetwork.com/fish2/...s/1/default.asp

Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
http://www.animalnetwork.com/fish2/...bio/default.asp



Andy's calcium calculator
http://www.andy-hipkiss.co.uk/cacalc.htm

Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
http://www.aquariumfish.com/aquariu...cid=124&search=

Calcium Reactor Substrate -- Phosphate Levels
by Greg Hiller
http://www.advancedaquarist.com/iss...l2003/short.htm


Indoor CO2 Problems
http://www.advancedaquarist.com/iss...r2002/short.htm

Simon Huntington's CaCO3/CO2 reactor article

http://reefkeeping.com/issues/2002-...ature/index.htm

Ron Shimek's Tank Water Analysis Article
http://reefkeeping.com/issues/2002-...ature/index.htm




Home made salinity standards thread:

http://reefcentral.com/forums/showt...?threadid=65509

Reef Chemicals Calculator
http://www.kademani.com/reefchem.htm



Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php


Former US Army Bomb Technician (EOD)
Member; IABTI, NATEODA, WEODF, ISEE & IPS

If You See Me Running You Better Catch-Up


--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
www.coralrealm.com

If You See Me Running You Better Catch-Up
"stoutman" <.@.> wrote in message news:aGuWb.148227$U%5.676753@attbi_s03...
: Boomer,
:
: I am not sure if you are just messing with me or if you are truly confused.
: I hope the latter. Please read from Top to Bottom.
:
:
: From YOUR first link:
:
: http://www.waterontheweb.org/resources/glossary.html
:
: Acidity:
: A measure of how acid a solution may be. A solution with a pH of less than
: 7.0 is considered acidic. Solutions with a pH of less than 4.5 contain
: mineral acidity (due to strong inorganic acids), while a solution having a
: pH greater than 8.3 contains no acidity.
:
: Yes,
:
: Good definition (for the most part). pH <7 is indeed acidic. pH > 7 is
: basic. Your web page had a definition for acidity, but not basicity.
: Strange. That's like defining GOOD and not defining BAD.
:
: Here is the IUPAC (International Union of Pure and Applied Chemistry)
: definition of acidity:
:
: http://www.chem.qmul.ac.uk/iupac/index.html
:
: acidity
:
: (1) Of a compound:
:
: For Brønsted acids it means the tendency of a compound to act as a hydron
: donor. It can be quantitatively expressed by the acid dissociation constant
: of the compound in water or some other specified medium. For Lewis acids it
: relates to the association constants of Lewis adducts and -adducts.
:
: (2) Of a medium:
:
: The use of the term is mainly restricted to a medium containing Brønsted
: acids, where it means the tendency of the medium to hydronate a specific
: reference base
:
: basicity
:
: For Brønsted bases it means the tendency of a compound to act as hydron
: (proton) acceptor. The basicity of a chemical species is normally expressed
: by the acidity of the conjugate acid (see conjugate acid-base pair). For
: Lewis bases it relates to the association constants of Lewis adducts
: and -adducts
:
:
:
: Another definition from the same web page YOU cited: (this is the same web
: page you cited above)
:
: Alkalinity:
: Acid neutralizing or buffering capacity of water; a measure of the ability
: of water to resist changes in pH caused by the addition of acids or bases
: and therefore, the main indicator of susceptibility to acid rain; in natural
: waters it is due primarily to the presence of bicarbonates, carbonates and
: to a much lesser extent occasionally borates, silicates and phosphates. It
: is expressed in units of milligrams per liter (mg/l) of CaCO3 (calcium
: carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l = 1 mg/l
: of CaCO3. A solution having a pH below about 5 contains no alkalinity.
:
: Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and says
: that alkalinity is the measure of ...(description of a buffer)
:
: A BUFFER IS : a measure of the ability of water to resist changes in pH
: caused by the addition of acids or bases (from definition below)
:
:
: I said:
: ***alkalinity is a measurement of 'buffering capacity'***
:
: You said:
: ***Alkalinity is not a measurement of BC
:
: WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is not
: logical.
:
: (THIS FROM THE SAME WEB PAGE YOU CITED):
:
: Buffer:
: A substance which tends to keep pH levels fairly constant when acids or
: bases are added.
:
: THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
:
: a measure of the ability of water to resist changes in pH caused by the
: addition of acids or bases
:
: SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A BUFFER.
:
:
: I went to all four links. None contradict what I have said. But the first
: one you cited contradicts YOU!
:
: I know what a buffer is. I know what acidity means. I know what alkalinity
: means. No need to cite web pages that describe what I know and what I wrote
: in this discussion. Show me one that says alkalinity is not a measure of
: buffering capacity from a credible source.
:
:
:
:
:
:
: "Boomer" > wrote in message
: ...
: > Alkalinity a measure of the amount of anions of weak acid in water and of
: the cations
: > balanced against them
: > Take note it says ***acid***
: >
: > Buffering capacity the ability of a solution to resist or dampen changes
: in pH upon the
: > addition of acids or bases.
: > Take note its says ***the addition of acids or bases***
: >
: > One more
: >
: > http://www.waterontheweb.org/resources/glossary.html
: >
: > We could go on like this all day, so what is the point ?
: >
: > You will LOVE this one
: > http://www.kyantec.com/Tips/phbuffering.htm
: >
: > Don't you just lovbe PDF's
: > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
: >
: > Don't fall out of your chair
: > http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
: >
: >
: >
: >
: > --
: > Boomer
: >
: > Want to talk chemistry ? The Reef Chemistry Forum
: > http://www.reefcentral.com/vbulletin/index.php
: >
: > Want to See More ?
: > Please Join Our Growing Membership
: > www.coralrealm.com
: >
: > If You See Me Running You Better Catch-Up
: > "stoutman" <.@.> wrote in message news:XB7Wb.19339$QA2.62332@attbi_s52...
: > : Man here is another, google is a wonderful thing. I'm not filtering any
: > : out, just posting what I find by GOOGLING for you.
: > :
: > : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
: > :
: > :
: > : Wow, a gov link. Even the government is wrong, this must be a
: conspiracy
: > : against Boomer.
: > :
: > :
: > :
: > :
: > : "Boomer" > wrote in message
: > : ...
: > : > Now I am getting bored
: > : >
: > : > "Don't the components of a buffer account for the buffering capacity?
: > : Yes."
: > : >
: > : > Yes, agreed but you seem to fail what I'm saying. Buffering Capacity
: and
: > : Alkalinity are
: > : > not the same, that has always been the issue. I gave the equation does
: > : that look like an
: > : > Alkalinity equation or how Alk is determined. I see you had now
: comments
: > : on it what's
: > : > wrong, why no comments on the equations I gave. Don't understand them
: or
: > : what ? Again this
: > : > is the equation for Buffering Capacity, also called Buffer Index or
: Buffer
: > : Intensity. It
: > : > is defined in most water chemistry and chemical oceanography text
: books.
: > : >
: > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] +
: CKa
: > : [H3O+] / (Ka =
: > : > H3O+])² )
: > : >
: > : > This is not Alkalinity now is it ?
: > : >
: > : > "I know how to do a titration, In fact I have done several. How many
: have
: > : > you actually done? I don't mean by counting drops, I mean with a
: buret?"
: > : >
: > : > Well good for you, I use a Digital Titrator
: > : >
: > : > "Oh, I see,
: > : > you think acidity is the opposite of alkalinity. In the world of
: > : CHEMISTRY
: > : > it's not. Maybe in aquarium newsgroups it is.
: > : >
: > : > Hum no, maybe you should go for a look at HACH's or LaMotte website or
: the
: > : book I
: > : > suggested earlier. Please view a copy.
: > : >
: > : > Standard Methods for the Examination of Water and Wastewater
: > : >
: > : > This book, over 2000 pages, is the guide for water testing. If you are
: > : reporting water
: > : > test to the EPA you must use approved std from this text.I t is
: prepared
: > : and published by
: > : > the EPA, American Water Works Association and American Public Health
: > : Association. You
: > : > mean you don't have one and the issue is water chemistry
: > : >
: > : > You are confusing Acidity and Acidity as you know little about water
: > : chemistry and
: > : > procedures and test methods
: > : >
: > : > From SMEWW, section 2-30, 2310 ACIDITY
: > : >
: > : > "Acidity of water is its quantative capacity to react with a strong
: base
: > : to a designated
: > : > pH"
: > : >
: > : > This is how you test for it
: > : >
: > : > A std alkali titration to methyl orange or phenolphthalein
: > : > endpoint.
: > : >
: > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write
: this
: > : book, there are
: > : > over 100 of them, they are wrong.
: > : >
: > : > Like Buffering Capacity you have your Acidity's mixed up
: > : > In water measurement if you have a high Alk you also usually have a
: high
: > : Acidity.
: > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
: CHEMISTRY
: > : BOOK there pal.
: > : >
: > : >
: > : > "These are all in equilibrium with each other. An initial high pH
: (above
: > : > 6.4) will shift the equilibrium to the right to form HCO3-1. If the
: pH of
: > : > the solution is above 10.3 (pKa2) the .........."
: > : >
: > : >
: > : > Christ, there you go again with the FW ****. All your numbers are
: wrong we
: > : are dealing
: > : > with SEAWATER
: > : >
: > : > This means that at a pH of 8.3, the majority of the CO2(aq) is in the
: form
: > : > of HCO3-1 .
: > : >
: > : > I have already pointed that out and gave actual values at know
: seawater
: > : levels, go back
: > : > and re-read it you aren't telling me anything here.Of course most is
: HCO3
: > : see...
: > : >
: > : >
: > : > @ 20C and 34.3 ppt salinity
: > : >
: > : > CO2 = 0.52 %
: > : >
: > : > HCO3 = 86.4 %
: > : >
: > : > CO3 = 13.09 %
: > : >
: > : >
: > : > "In your glass experiment you managed to lower the pH enough to purge
: out
: > : CO2
: > : > by boiling"
: > : >
: > : > The purpose behind the glass is to show that alk is not affect by CO2
: and
: > : vise-versa and
: > : > how Co2 affects pH.
: > : >
: > : > Now, in a real life seawater aquarium, with a pH of 8.3 and that pH
: drops
: > : to say 8.1 it is
: > : > usually due to excess CO2. If you took a glass of that water and
: aerated
: > : it you WILL drive
: > : > off the CO2 and raise the pH. It has been done a proven a million
: times.
: > : >
: > : > "In order to 'purge' CO2 you would need to lower the
: > : > pH to shift the equilibrium to below 6.4"
: > : >
: > : > The hell you do !!!.Do you know who many times people on this NG to
: > : include Dr. Craig
: > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
: > : sample of aquarium
: > : > water and aerate it to see if the pH GOES UP AND when they come back
: with
: > : the test it is
: > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST
: excess
: > : CO2 in the tank
: > : > water, increase the circulation for better gas exchange at the
: surface,
: > : reduce feeding,
: > : > and try to improve on better skimming, thus reducing the bio-load and
: pH
: > : decline due to
: > : > CO2.
: > : >
: > : >
: > : > "I hope this helps. "
: > : >
: > : > Help, how can you when you miss everything. I should be charging you
: > : >
: > : > Oh, by the way. Your websites, I have about 50 on these issues, I
: could
: > : post them, not to
: > : > mention I have all those water chemistry books, so there is no need to
: > : view your sites.
: > : >
: > : > Finally are you afraid to come to our Chemistry Forum, afraid to get
: > : slapped by REAL
: > : > chemists. I get a charge out of you can't post your ref .I have posted
: the
: > : same or similar
: > : > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500
: posts
: > : there and am the
: > : > biggest contributor to his forum other than himself or maybe Habib
: Sheka
: > : >
: > : > Hum, here are Randy's ref that he posted. He hosts the website
: > : >
: > : > S. RANDY HOLMES-FARLEY
: > : > Arlington, Massachusetts
: > : >
: > : > EDUCATION
: > : >
: > : > 1982-1986 Harvard University Cambridge, MA
: > : > PhD in Chemistry
: > : > Research Advisor: George Whitesides
: > : >
: > : > Investigated the relationship between polymer surface chemistry and
: > : physical properties
: > : > through controlled surface modification and testing.
: > : >
: > : > 1980-1982 Cornell University Ithaca, NY
: > : > BA in Chemistry and Biology
: > : > Graduated Summa Cum Laude
: > : > Distinction in All Subjects
: > : > Grade Point: 3.94/4.0
: > : > Honors research: isolation and characterization of the subunit of CF1
: > : enzyme
: > : >
: > : >
: > : > 1978-1979 Stanford University Palo Alto, CA
: > : > Grade Point: 3.55/4.0
: > : >
: > : >
: > : > EXPERIENCE
: > : >
: > : > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
: > : > (bought out GelTex Pharmaceuticals in 2001)
: > : > Vice President, Chemical Research 2001-present
: > : > Senior Director, Chemical Research 1999-2001
: > : > Director of Chemical Research 1997-1999
: > : > Manager of Chemical Research 1995-1997
: > : > Group Leader 1994-1995
: > : > Senior Research Scientist 1992-1994
: > : >
: > : > Helped start GelTex as second employee
: > : >
: > : > Managed various research programs with multi-million dollar budgets
: > : >
: > : > Supervised research chemists (17+)
: > : >
: > : > Co-inventor of several polymeric pharmaceuticals and pharmaceutical
: > : candidates including
: > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride
: (FDA
: > : approved)
: > : >
: > : > Company Safety Officer for 3 years
: > : >
: > : > Chemical Hygiene Officer 2000-present
: > : >
: > : >
: > : >
: > : >
: > : > 1990-1992 GTE Corporation Waltham, MA
: > : > Senior Member of Technical Staff
: > : > Applied research involving polymer interfaces
: > : > Metallization of plastics
: > : > Polymer/polymer adhesion
: > : > Optical coatings
: > : >
: > : >
: > : >
: > : > 1986-1990 Lord Corporation Cary, NC
: > : > Senior Research Scientist 1988-1990
: > : > Research Scientist 1986-1988
: > : > Basic and applied research on surface chemical bonding
: > : > Developed new adhesive compositions
: > : > Developed new sol-gel coatings for corrosion resistance
: > : >
: > : >
: > : > HONORS AND AWARDS
: > : >
: > : > Industrial Innovations Award by Northeast Region of American Chemical
: > : Society (6/2001)
: > : >
: > : > National Kidney Foundation of Northern California Honoree (5/2001)
: > : >
: > : > American Chemical Society/Polymer Chemistry Division Industrial
: Sponsors
: > : > Award (8/2000)
: > : >
: > : > R&D 100 Award from R&D magazine (1999)
: > : >
: > : > Sherwin Williams Award in applied polymer science (9/85)
: > : >
: > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
: > : >
: > : > Award for highest GPA in Chemistry Department (6/82)
: > : >
: > : > Summa Cum Laude Honors in Chemistry (6/82)
: > : >
: > : > Phi Lamda Epsilon (6/82)
: > : >
: > : > Phi Beta Kappa (2/82)
: > : >
: > : > Cornell University Dean's List (1981, 1982)
: > : >
: > : > Harvard Book Club Award for highest GPA senior year (1978)
: > : >
: > : > First Place in western NY ACS high school chemistry exam (1977)
: > : >
: > : > 1978-1979
: > : >
: > : >
: > : > __________________
: > : > Randy Holmes-Farley
: > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
: > : >
: > : > Hobby Experience: 8 years with reefs
: > : > Current Tanks: 90 gal mixed reef
: > : > Interests: Reefkeeping, science, photography
: > : >
: > : >
: > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
: > : >
: > : > Open this post in a new window | Report this post to a moderator | IP:
: > : Logged
: > : >
: > : >
: > : >
: > : > 06/27/2003 02:44 PM
: > : >
: > : > Randy Holmes-Farley
: > : > Chemistry Moderator
: > : >
: > : > Registered: Apr 2001
: > : > Location: Arlington, Massachusetts
: > : > Occupation: Chemist (Drug Discovery at Genzyme)
: > : > Posts: 15282
: > : >
: > : >
: > : >
: > : > Publications
: > : >
: > : >
: > : > ISSUED UNITED STATES PATENTS
: > : >
: > : >
: > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
: > : Mandeville, III; W. Harry.
: > : > US 6,566,407; 5/20/2003
: > : >
: > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen
: Randall;
: > : Huval, Chad
: > : > Cori.
: > : > U.S. 6,517,825; 2/11/2003.
: > : >
: > : > 3. Method of making phosphate-binding polymers for oral
: administration.
: > : Holmes-Farley,
: > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
: > : 6,509,013; 1/21/2003.
: > : >
: > : > 4. Combination therapy for treating hypercholesterolemia using a bile
: acid
: > : sequestrant
: > : > polymer
: > : > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley,
: Stephen
: > : Randall;
: > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
: > : >
: > : > 5. Method for treating hypercholesterolemia with polyallylamine
: polymers.
: > : Holmes-Farley,
: > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
: Goldberg,
: > : Dennis I. , US
: > : > 6,423,754; 7/23/2002.
: > : >
: > : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
: > : Neenan, Thomas X..;
: > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
: > : >
: > : > 7. Combination therapy for treating hypercholesterolemia and
: > : atherosclerosis. Huval, Chad
: > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep
: K.
: > : U.S. 6,365,186;
: > : > 4/2/2002.
: > : >
: > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
: Mandeville,
: > : W. H., III;
: > : > Huval; C.
: > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
: > : 10/9/2001.
: > : >
: > : > 9. Polymers containing guanidinium groups as bile acid sequestrants.
: Dhal;
: > : P. K.; Holmes-
: > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
: > : >
: > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
: H.,
: > : III.; US
: > : > 6,281,252;
: > : > 8/28/2001.
: > : >
: > : > 11. Combination therapy for treating hypercholestrolemia. Huval; C.
: C.;
: > : Holmes-Farley; S.
: > : > R. ;
: > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
: > : >
: > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
: > : Holmes-Farley, S.
: > : > R.; US
: > : > 6,264,937; 7/24/2001.
: > : >
: > : > 13. Method for treating hypercholesterolemia with unsubstituted
: > : polydiallylamine polymers.
: > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
: > : 6,248,318;
: > : > 6/19/2001.
: > : >
: > : > 14. Process for removing bile salts from a patient and alkylated
: > : compositions therefore.
: > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
: > : >
: > : > 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S.
: R.;
: > : Dhal, P. K.;
: > : > Petersen,
: > : > J. S.; US 6,203,785; 3/20/2001.
: > : >
: > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.;
: Huval,
: > : C. C.; US
: > : > 6,190,649;
: > : > 2/20/2001.
: > : >
: > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
: H.,
: > : III.; US
: > : > 6,177,478;
: > : > 1/23/2001.
: > : >
: > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
: Holmes-Farley,
: > : S. R.;
: > : > Mandeville, W.
: > : > H., III.; US 6,129,910; 10/10/2000.
: > : >
: > : > 19. Method for treating hypercholesterolemia with unsubstituted
: > : polydiallylamine polymers.
: > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
: > : 6,083,497;
: > : > 7/4/2000.
: > : >
: > : > 20. Method of making phosphate-binding polymers for oral
: administration.
: > : Holmes-Farley, S.
: > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495;
: 7/4/2000.
: > : >
: > : > 21. Process for removing bile salts from a patient and alkylated
: > : compositions therefore.
: > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
: 5/23/2000.
: > : >
: > : > 22. Process for removing bile salts from a patient and compositions
: > : therefor. Mandeville,
: > : > W. H.,
: > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
: > : >
: > : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
: > : Neenan; T. X.; Holmes-
: > : > Farley; S. R. US 6,034,129; 3/7/2000.
: > : >
: > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
: H.,
: > : III.; US
: > : > 5,985,938;
: > : > 11/16/99.
: > : >
: > : > 25. Process for removing bile salts from a patient and compositions
: > : therefor. Mandeville,
: > : > W. H.,
: > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
: > : >
: > : > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W.
: H.,
: > : III.;
: > : > Holmes-Farley;
: > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
: > : >
: > : > 27. Hydrophilic nonamine-containing and amine-containing copolymers
: and
: > : their use as bile
: > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
: 5,929,184;
: > : 7/27/99.
: > : >
: > : > 28. Interpenetrating polymer networks for sequestration of bile acids.
: > : Mandeville, W. H.,
: > : > III.;
: > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
: > : 7/20/99.
: > : >
: > : > 29. Amine polymer sequestrant and method of cholesterol depletion.
: > : Mandeville, W. H.,
: > : > III.;
: > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
: > : >
: > : > 30. Process for removing bile salts from a patient and compositions
: > : therefor. Mandeville,
: > : > W. H.,
: > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
: > : >
: > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
: > : Mandeville, W. H.,
: > : > III.;
: > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
: > : >
: > : > 32. Process for removing bile salts from a patient and compositions
: > : therefor. Mandeville,
: > : > W. H.,
: > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
: > : >
: > : > 33. Preparation of polymeric sequestrants for bile acid salts.
: Mandeville,
: > : W. H., III.;
: > : > Holmes-
: > : > Farley, S. R.; US 5,703,188; 12/30/97.
: > : >
: > : > 34. Oral administration of iron-binding crosslinked amine polymers.
: > : Mandeville, W. H.,
: > : > III.;
: > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
: > : >
: > : > 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley,
: S.
: > : R.; US 5,693,675;
: > : > 12/2/97.
: > : >
: > : > 36. Method for removing bile salts from a patient with alkylated
: > : crosslinked amine
: > : > polymers,
: > : > and preparation of the polymers. Mandeville, W. H., III.;
: Holmes-Farley,
: > : S. R.; US
: > : > 5,679,717; 10/21/97.
: > : >
: > : > 37. Phosphate-binding polymers for oral administration. Holmes-Farley,
: S.
: > : R.; Mandeville,
: > : > W.
: > : > H., III.; US 5,667,775; 9/16/97.
: > : >
: > : > 38. Ion-exchange process using highly crosslinked polymers for
: removing
: > : bile salts from a
: > : > patient, preparation of the polymers, and compositions containing
: them.
: > : Mandeville, W. H.,
: > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
: > : >
: > : > 39. Hydrophobic amine polymer sequestrant and method of cholesterol
: > : depletion. Mandeville,
: > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530;
: 4/8/97.
: > : >
: > : > 40. Amine polymer sequestrant and method of cholesterol depletion.
: > : Mandeville, W. H.,
: > : > III.;
: > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
: > : >
: > : > 41. Phosphate-binding polymers for oral administration. Holmes-Farley,
: S.
: > : R.; Mandeville,
: > : > W.
: > : > H., III.; US 5,496,545; 3/5/96.
: > : >
: > : > 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
: > : III.; Holmes-Farley,
: > : > S. R.;
: > : > US 5,487,888; 1/30/96.
: > : >
: > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having active
: > : hydrogens on the
: > : > surface.
: > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
: > : >
: > : > 44. Layered sol-gel coatings from organisilicon compounds.
: Holmes-Farley,
: > : S. R.; Yanyo, L.
: > : > C.;
: > : > US 5,182,143; 1/26/93.
: > : >
: > : > 45. Method for metal bonding using ultrathin primer coating.
: > : Holmes-Farley, S. R.; Yanyo,
: > : > L.
: > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
: > : >
: > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.;
: US
: > : 5,096,962;
: > : > 3/17/92.
: > : >
: > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
: > : elastomer-metal bonding.
: > : > Holmes-
: > : > Farley, S. R.; US 5,102,956; 4/7/92.
: > : >
: > : >
: > : >
: > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
: > : >
: > : >
: > : > 1. Aryl boronate functionalized polymers for treating obesity and
: > : inhibiting fat uptake.
: > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal,
: Pradeep
: > : K.; Huval, Chad
: > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92
: pp. WO
: > : 0302571.
: > : >
: > : > 2. Preparation of aryl boronic acids for treating obesity.
: Holmes-Farley,
: > : Stephen Randall;
: > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep
: K.
: > : (Geltex
: > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
: > : >
: > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
: > : Stephen Randall.
: > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
: > : 0302130.
: > : >
: > : > 4. Method for reducing copper levels and treating copper toxicosis.
: > : Holmes-Farley, Stephen
: > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002),
: 45
: > : pp. WO
: > : > 0285383.
: > : >
: > : > 5. Method for treating gout and binding uric acid. Holmes-Farley,
: Stephen
: > : Randall; Burke,
: > : > Steven K. WO 0285381 10/31/2002.
: > : >
: > : > 6. Method for treating gout and reducing serum uric acid.
: Holmes-Farley,
: > : Stephen Randall;
: > : > Burke, Steven K WO 0285380 10/31/2002.
: > : >
: > : > 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
: > : Holmes-Farley, S. R.;
: > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
: > : >
: > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
: > : Holmes-Farley, S.
: > : > R.;
: > : > WO 1999-US5662; 9/23/1999.
: > : >
: > : > 9. Amine-containing copolymers as bile acid sequestrants.
: Holmes-Farley,
: > : S. R.; Petersen,
: > : > J. S.;
: > : > WO 9933452; 7/8/1999.
: > : >
: > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III
: and
: > : Holmes-Farley, S.
: > : > R.;
: > : > WO 9922743; 5/14/1999.
: > : >
: > : > 11. Polyallylamine polymers for removing bile salts and treating
: > : hypercholesterolemia, and
: > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III;
: Burke,
: > : S. K.; Goldberg,
: > : > D. I.; WO 9857652; 12/23/98.
: > : >
: > : > 12. Phosphate-bidning polymers combined with a calcium supplement for
: oral
: > : administration.
: > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley,
: S.
: > : R.; WO 9842355;
: > : > 10/1/98.
: > : >
: > : > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
: > : depletion. Mandeville,
: > : > W.
: > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
: > : >
: > : > 14. Process for adjusting ion concentration in a patient and
: compositions
: > : therefor.
: > : > Mandeville,
: > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
: > : >
: > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
: interlayer
: > : for improved
: > : > metal-
: > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
: 1/20/94.
: > : >
: > : > 16. Process for increased metal-substrate bond strength in metalized
: > : plastics.
: > : > Holmes-Farley, S.
: > : > R.; Ger. Offen. 4322516; 7/6/93.
: > : >
: > : > 17. Electrorheological fluids and preparation of particles useful in
: the
: > : fluids.
: > : > Troughton,
: > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
: > : David; Bares, Joseph
: > : > E.;
: > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
: > : 394049;
: > : > 10/24/1990.
: > : >
: > : > JOURNAL PUBLICATIONS
: > : >
: > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov,
: Eugene;
: > : Guo, Amy;
: > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
: > : Mandeville, W. Harry;
: > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
: 611-619.
: > : >
: > : > 2. Amine functionalized polyethers as bile acid sequestrants:
: synthesis
: > : and biological
: > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S.
: Randall;
: > : Mandeville, W.
: > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
: > : Journal of
: > : > Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
: > : 1559-1574.
: > : >
: > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
: > : Imprinting. Huval,
: > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
: > : Randall; Mandeville,
: > : > W.
: > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert
: J.;
: > : Chen, Xi; Dhal,
: > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
: > : >
: > : > 4. Synthetic polymers for the binding of fat in the intestinal tract.
: > : Jozefiak, Thomas H.;
: > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia;
: Huval,
: > : Chad C.;
: > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
: > : Abstracts of
: > : > Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
: > : 26-30, 2001
: > : > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
: > : Division of
: > : > Polymer Chemistry) (2001), 42(2), 98.
: > : >
: > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer
: gel
: > : pharmaceutical.
: > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.;
: Ward,
: > : J.; Sacchiero,
: > : > B.;
: > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.;
: Chen,
: > : X.; Mazzeo, J.
: > : > R.. Polym. Preprints (2000), 41(1), 735-736.
: > : >
: > : > 6. In vitro comparison of bile acid binding to colesevelam HCl and
: other
: > : bile acid
: > : > sequestrants.
: > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
: > : Hook, P.; Holmes-
: > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
: > : >
: > : > 7. Novel polymeric pharmaceuticals: From startup to market.
: Holmes-Farley,
: > : S. R; Polym.
: > : > Mater. Sci. Eng (1999), 80, 246-247.
: > : >
: > : > 8. Design and characterization of of Sevelamer Hydrochloride: a novel
: > : phosphate-binding
: > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward,
: J.;
: > : Miller, K. L.;
: > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure
: and
: > : Appl. Chem.,
: > : > A36(7&8), p. 1085 (1999).
: > : >
: > : > 9. Three generations of bile acid sequestrants. Mandeville, W. H.,
: III;
: > : Braunlin, W.;
: > : > Dhal, P.;
: > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
: > : Rosenbaum, D.;
: > : > Sacchiero,
: > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
: > : 550, 3-15.
: > : >
: > : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric
: phosphate
: > : binder, on
: > : > urinary
: > : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
: > : Mandeville, W. H.,
: > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
: > : (1997), 12(5)
: > : > 961-964.
: > : >
: > : > 11. Thin anisotropic coatings based on sol-gel technology.
: Holmes-Farley,
: > : S. R.; Yanyo, L.
: > : > C;
: > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4),
: 439-444.
: > : >
: > : > 12. The mechanism of cure initiation of a surface activated adhesive.
: > : Holmes-Farley, S.
: > : > R.;
: > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
: > : >
: > : > 13. Adhesion promotion and corrosion prevention using thin anisotropic
: > : coatings. Holmes-
: > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
: > : 131-151.
: > : >
: > : > 14. Wetting of functionalized polyethylene having ionizable organic
: acids
: > : and bases at the
: > : > polymer-water interface: relations between functional group polarity,
: > : extent of
: > : > ionization,
: > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
: > : Whitesides, G. M.;
: > : > Langmuir
: > : > (1988), 4(4), 921-937.
: > : >
: > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
: > : single hydroxy group.
: > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
: > : >
: > : > 16. Reconstruction of the interface of oxidatively functionalized
: > : polyethylene (PE-CO2H)
: > : > and
: > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo,
: R.;
: > : McCarthy, T. J.;
: > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report
: (1987),
: > : AD-
: > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
: > : >
: > : > 17. Surface-modified polyethylene film: the relationship between
: surface
: > : chemistry and
: > : > physical
: > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11),
: 4537.
: > : >
: > : > 18. Reactivity of carboxylic acid and ester groups in the
: functionalized
: > : interfacial
: > : > region of
: > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
: > : differentiation of the
: > : > functional groups into shallow and deep subsets based on a comparison
: of
: > : contact angle and
: > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
: > : (1987), 3(1), 62-
: > : > 76.
: > : >
: > : > 19. Fluorescence properties of dansyl groups covalently bonded tot he
: > : surface of
: > : > oxidatively
: > : > functionalized low-density polyethylene film. Holmes-Farley, S. R.;
: > : Whitesides, G. M.;
: > : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
: > : AD-A162435/2/GAR,
: > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
: > : >
: > : > 20. Acid-base behavior of carboxylic acid groups covalently attached
: at
: > : the surface of
: > : > polyethylene: The usefulness of contact angle in following the
: ionization
: > : of surface
: > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
: > : Deutch, J.;
: > : > Whitesides,
: > : > G. M.; Langmuir (1985), 1(6), 725-740.
: > : >
: > : > 21. The thermal stability of a surface modified solid organic polymer.
: > : Holmes-Farley, S.
: > : > R.;
: > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
: > : >
: > : >
: > : >
: > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
: > : >
: > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
: > : Aquarist. June 2003.
: > : >
: > : > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
: > : Advanced Aquarist.
: > : > May
: > : > 2003.
: > : >
: > : > 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
: > : Reefkeeping May
: > : > 2003.
: > : >
: > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
: > : April 2003.
: > : >
: > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
: > : Holmes-Farley, R.
: > : > Advanced Aquarist; April 2003.
: > : >
: > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
: > : Holmes-Farley, R.
: > : > Advanced Aquarist; April 2003.
: > : >
: > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced
: Aquarist;
: > : March 2003.
: > : >
: > : > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
: > : Holmes-Farley, R.
: > : > Advanced Aquarist; February 2003.
: > : >
: > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
: > : 2003.
: > : >
: > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
: December
: > : 2002.
: > : >
: > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
: Advanced
: > : Aquarist; November
: > : > 2002.
: > : >
: > : > 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
: > : Advanced Aquarist;
: > : > November 2002.
: > : >
: > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced
: Aquarist,
: > : September 2002.
: > : >
: > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
: > : 2002.
: > : >
: > : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
: > : 2002.
: > : >
: > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
: > : Aquarist; July 2002
: > : >
: > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist;
: June
: > : 2002.
: > : >
: > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R.
: Advanced
: > : Aquarist, May
: > : > 2002.
: > : >
: > : > 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
: > : Holmes-Farley, R.
: > : > Advanced Aquarist, April 2002.
: > : >
: > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
: > : >
: > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
: > : >
: > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January
: 2002.
: > : >
: > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
: > : 2000.
: > : >
: > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
: > : Frontiers 2000.
: > : >
: > : > 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
: > : Aquarium Frontiers
: > : > 2000.
: > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
: Frontiers
: > : 2000.
: > : >
: > : > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers
: 2000.
: > : >
: > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
: > : >
: > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
: > : >
: > : >
: > : >
: > : >
: > : >
: > : >
: > : >
: > : > Boomer
: > : >
: > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > http://www.reefcentral.com/vbulletin/index.php
: > : >
: > : > Want to See More ?
: > : > Please Join Our Growing Membership
: > : > www.coralrealm.com
: > : >
: > : >
: > : >
: > :
: > :
: >
: >
:
:
:

[Boomer]

"As it is the ability to neutralizes an acid that is a buffer"

sorry

As it is the ability to neutralizes a base that is a buffer

--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
www.coralrealm.com

If You See Me Running You Better Catch-Up
"Boomer" > wrote in message
...
:
: "I am not sure if you are just messing with me "
:
: Yes, messing with you, it is called trolling a troll, to see where the hell you would go
: and what you would say in regards to last posts. It is called honesty, of which you have
: none off to say the least,that I can see.You always like to post what suits you and just
: avoid ref I give. So lets start where you are WRONG and have a great lack of
understanding
: of things, to include pointing out all your gross error which you still FAIL to
: acknowledge and which can be prove in many water chem. ref. .I doubt like hell you are a
: chemist at all.You seem to want to con people into thinkin' you are. But then again, I
: have seen chemists like you before, they are not familiar with the, but they ASK to have
: it explained and ask for REF.YOU just shoot from the hip. WHAT GETS YOU IN TROUBLE. You
: remind me of snoot-noise kid that come here and other NG's and forums...that think they
: know, buy hey, maybe I'm wrong :-)
:
:
:
: 1). Acidity
:
: "***Benjamin,Water Chemistry (2002, pages 262-263).***
:
: ***Acidity A concept that is exactly analogous to alkalinity but measures the base
: neutralizing
: capacity (BNC) of a solution is Acidity. The quantitative represents the concentration
of
: OH- ions that must be added to titrate the solution to a pH near 10.5***
:
: So that means that not only in Benjamin wrong but, so are Stumm & Morgan, Millero,
Pilosn,
: Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I said, you have
your
: acidity and Acidy mixed up. Acidity as defined above is covered in most water chemistry
: books, written by chemists, who's field of expertise is water chemistry. You can even
buy
: Acidity test kits from, HACH, LaMotte, etc..
:
: You mean you didn't read this or are you just avoiding it .The same definition can be
: found in almost any std water chemistry book.
:
: I have run into few chemists, that are NOT familiar with the above. Some water reports
: require the above Acidity measuring. The issue with you is you do not understand WATER
: CHEMISTRY. Everything you have posted can be found a general chemistry book
:
:
:
:
: 2) Alk and BC
:
: From the link
:
: Alkalinity
: ***Acid neutralizing or buffering capacity of water; a measure of the ability of water
to
: resist changes in pH caused by the addition of acids or bases ***
:
: This is a Buffering Capacity definition not Alk
:
: Humm, since when does Alk have anything to do in regards to the addition of BASE. As I
: pointed out in the first post the term is often miss used. Even in YOUR own posts you
say
: it is based on a acid addition, no mention of **base or acid** addition by you. Are you
: getting confused or what. Or is more you are trying to confuse everyone you are right.
The
: above is a definition for Buffer Capacity NOT Alk
:
: From Drew, Geochemistry of Natural Waters
:
: "alkalinity, which is formally defined as the equivalent sum of bases that are
titratable
: with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH of the solution is
: progressively lowered by the addition of a strong acid (HCL), all the anions on the
right
: will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4, H2S,organic acids, H20)"
:
: This follows almost all description of Alk, that it is acid neutralizing reaction and
has
: nothing to do with base neutralizing, which is Acidity (BNC) .I defined these before you
: had no comment
:
:
: Even the links that give the Buffering Capacity definition is wrong, as is the UIPAC on
: Alkalinity. Alkalinity has nothing to do with the addition of bases only acids. When you
: use the words "base and acid" it becomes BC
:
: Even YOU MUST disagree with these definitions, from YOUR own post
:
: Think of alkalinity as 'buffering capacity'. Or the ability of a solution
: ***to resist a drop in pH due to the addition of acid***
:
: Where the flip is the base addition forget it ?
:
: From Butler; Carbon Dioxide Equilibrium and Their Applications (professor emeritus
: Harvard University) an expert on the subject.
:
: Buffering Index (Buffering Capacity, Buffer Intensity).
:
: ***This concept was first developed for mixtures of approximately equal proportions of
: conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such buffer solutions
: strongly resist changes in pH when acids or bases are added and are useful as pH
: standards. The Buffer Index tells how great the resistance to pH changes will be.**
:
: also from Butler
:
: Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
:
: Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
:
: Acidity is in fact just the negative of Alkalinity ***
:
: http://www.lagoonsonline.com/acid.htm
:
: http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.htm?E+mystore
:
: It sure is funny how all of the chemist that write water chemistry textbooks never say
Alk
: is the Buffering Capacity of a solution. They are always treated and defined separately.
:
: If you or others choose to treat Alk and BC as the same, well, just have at it. As I
said
: in first post I know what you mean.
:
: "No need to cite web pages that describe what I know and what I wrote
: in this discussion"
:
: No you don't know, who are you trying to convince any way, me, the guys here and/or all
: the water chemists in this world. As I said before go get a dam WATER CHEMISTRY book or
: shut the hell up.You keep trying to define things from a general chemistry book WE ARE
IN
: THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
:
:
:
:
:
: 3). pKa's and what you don't know or seem to be confused on
:
: "Therefore, it has two pKa's
: (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35. The
: pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
: right in there. Is that magic? :)"
:
: Here it is agin that is twice at least
:
: "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this example)
: you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium will
: be shifted to HCO3-2 by a ratio of 1:100.
:
: Oh wait , there is a third time LOL
:
: "At the pH of seawater, the buffering capacity of carbonate is at it's
: weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
:
:
: Lets just dunk you on this one. I am taking note you refuse to reply to YOUR errors
:
: So you calculated the pH of seawater with freshwater pKa's, now that is a good trick.
From
: a number of seawater chemistry books the seawater pKa's are 6 & 9.1, so according to
you,
: seemingly not understanding your favorite Henderson-Hasselbach equation;
:
: 2 pH = (6 + 9.1) /2 pH = 7.55
:
: I have never seen seawater with a pH of 7.55. There is no ocean with that pH. Humm how
: come your equation is not working for you today.?
:
:
: "That pH I calculated is
: right in there. Is that magic? :)"
:
: I roll on the floor when I see this = 8.35
:
: Hum , just a brain far so excuse me for thinkin
:
: (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
:
: Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a pH of 8.35 there
pal
: ? That 8.35 is what you are telling people the pH should be, but their meter says 6.4.
: This how people will READ this.
:
:
:
:
: 4.) More on Buffering Capacity
:
: "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes, your
: alkalinity equation."'
:
:
: Yup, I see that and in this case the HCO3 is the acid and the CO3 is the base CORRECT.
In
: Alk you are only dealing with bases and how they react to an acid. Acidity deals acids
and
: how they recact to bases "Acidity, A concept that is exactly analogous to alkalinity but
: measures the base neutralizing
: capacity (BNC) of a solution is Acidity "Alk is the ANC Acid neutralizing capacity
:
: "Don't the components of a buffer account for the buffering capacity? "
:
: Yes, they do but so do the acids which work as buffers. NaHCO3 is a buffer and can act
as
: an acid or base
:
: *** Buffering Capacity.**
: The power of a substance in solution to absorb acid or alkali without change in pH; this
: is highest at a pH value equal to the pKa value of the acid of the buffer pair.***
:
: ***Akalinity***
: Measure of the power of a solution to neutralise hydrogen ions (H+), usually expressed
as
: the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
:
:
: If one wants to call Alk Buffering capacity then one sure as a hell can call Acidty
: Buffering Capacity also. As it is the ability to neutralizes an acid that is a
buffer.You
: have a pH of 7 and you add a buffer to lower it to a pH of 4, you are buffering the
water,
: that buffer is a acid.
:
: 5) CO2
:
: You are really confuse so it seems :-) You realllllllly indicate that CO2 is affected by
: the Alk or vise-versa
:
: "Yes, the pH will drop with the addition of CO2. Remove CO2 will cause the
: pH to rise? How do you remove CO2? Once it is in solution it forms
: carbonic acid and neutralizes some of your 'buffer'."
:
: "With the exception of CO2?"
:
: No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
: Concepts)....PERIOD.You seem to think a that at least in two of your post that CO2 is
: affected by the Alk or vise-versa. Please go back to school or seek professor
:
: "Why in one case does CO2 from air lower pH and in the other case it raises
: it? Doesn't make sense."
:
: That is because you don't understand CO2 period. By the way I saved this, wanted to see
: if you would bite on the post I gave. Not bite at first, so time to reel you in, as you
: did bite in another post..
:
: Lets make some sense of it for you, being that you have a pH.D in chemistry, so you say
..
:
: CO2 is naturally generated in a aquatic systems, it is capable of raise to various
levels
: depending on a number of circumstances .It can be measure (except in seawater) or
: calculated using Buch/Park Equations (what we use for seawater. In sort if you know the
pH
: and Alk you can calculate the CO2). If you aerate a system or a sample of water, even if
: the pH has only dropped a couple of tenths, due to an increase in CO2, the CO2 will
leave
: solution to the atmosphere.This will raise the pH. On the other hand if theCO2 level is
: more of the norm and you have hikgh room air, such as in the winter, the partial
pressure
: of the CO2 in air will be much higher than that in water, in which case the CO2 will
enter
: the water and lower the pH. That is without an airstone. Adding an airstone will make it
: even worse,as you are now forcefully driving the CO2 into solution even quicker. These
: test /experiments have been proven many times, it is not that may work could work they
do
: work.Yet you want to disagree and in another post say you haven't tried it,.Seems to me
: that based on what you say it can't work So, in short you don't know what the hell you
are
: taking about. Go get a glass of seawater with a pH of about 8.3 and lower it to about
: 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK- UP ( that is if you
: don't have a high room air CO2 problem.). This little test has been done thousands of
: times in this hobby, with test kits, pH meters and even graphic printers.
:
: "This is where Boomer and I
: disagree. I say you would have to lower the pH very low in order to
: effectively remove CO2 by purging."
:
: You are 100 % wrong. Please come to our Chem forum and try and run that by Randy, don't
: take my word on it. I already know what he will say.
:
: "Boomer didnt convince me it
: works at the pH of an aquarium, but I never tried it and I'm not sure of
: this. "
:
: Well then come too our chem. forum and tell Randy he doesn't know what he is talking
about
: LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it should be easy for
: you to run the experiment LOL There are grade school kids that run the test and know
what
: happens and that I'm correct.
:
:
: "The equilibrium is a FUNCTION
: of pH."
:
: It is also a function of Alk or don't you know that. At a pH of 8.3, Alk 2.25, the CO2
is
: about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk to about .4 meq/ l
: or so the CO2 will be around .99 mg / l CO2, When dealing with tanksCO2 is not always in
: equilibrium with ambient air.
:
:
: ". But I wouldn't degas a solution of a
: specific gas (CO2) with a gas (this case he was using air) that contains the
: same gas I am trying to purge."
:
: Why not ? We have a guy right now that is running tests on purging ambient air with a
: solution to remove CO2 gas from the air, before it enters the tank per/Randy's
suggestion.
: The same guy is doing some of my test using a Clinoptilolite, a Zeolite mineral, that
has
: an affinity for CO2.This will be a dry CO2 scrubber
:
:
: Sorry Soutman but you sure as hell don't seem to know much about aquatic chemistry. You
: seem to be guessing at everything.
:
: By the way have you read any of Randy's technical articles on water chemistry, been
saving
: these for last. There are a few on pH, Alk, CO2 .Here is a list
:
: Try and answer them 1-5 and lets see where we get THIS TIME :-) or maybe we should just
: drop it. I could care less at this point.
:
: THE END
:
:
: ARTICLES
:
: The first two posts in this thread are lists of some of my articles that relate to reef
: tank chemistry. In the next few posts are some of the articles published by Craig
Bingman
: and others on reef chemistry issues.
:
: The first two posts in this thread are lists of some of my articles that relate to reef
: tank chemistry. In the next few posts are some of the articles published by Craig
Bingman
: and others on reef chemistry issues.
:
: Solving Common Problems
:
: Solving Calcium and Alkalinity Problems
: http://www.advancedaquarist.com/issues/nov2002/chem.htm
:
: Solutions to pH Problems
: http://www.advancedaquarist.com/iss...ne2002/chem.htm
:
: How to Select a Calcium and Alkalinity Supplementation Scheme
: http://www.advancedaquarist.com/issues/feb2003/chem.htm
:
: Phosphate Issues
: http://www.advancedaquarist.com/iss...pt2002/chem.htm
:
: Nitrate Issues
: http://www.advancedaquarist.com/iss...st2003/chem.htm
:
:
:
: Calcium and Alkalinity
:
: Solving Calcium and Alkalinity Problems
: http://www.advancedaquarist.com/issues/nov2002/chem.htm
:
: How to Select a Calcium and Alkalinity Supplementation Scheme
: http://www.advancedaquarist.com/issues/feb2003/chem.htm
:
: Calcium and Alkalinity Balance Issues
: http://reefkeeping.com/issues/2002-...ature/index.htm
:
: Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
: http://www.advancedaquarist.com/iss...ly2002/chem.htm
:
: The Relationship Between Alkalinity and pH.
: http://www.advancedaquarist.com/issues/may2002/chem.htm
:
: The Chemical & Biochemical Mechanisms of Calcification in Corals
: http://www.advancedaquarist.com/issues/apr2002/chem.htm
:
: Calcium
: http://www.advancedaquarist.com/issues/mar2002/chem.htm
:
: Alkalinity
: http://www.advancedaquarist.com/iss...2/chemistry.htm
:
:
: Iron
:
: First Iron Article: Macroalgae and Dosing Recommendations
: http://www.advancedaquarist.com/issues/aug2002/chem.htm
:
: Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
: http://www.advancedaquarist.com/issues/oct2002/chem.htm
:
: Iodine
:
: Iodine in Marine Aquaria: Part I
: http://www.advancedaquarist.com/issues/mar2003/chem.htm
:
: Iodine in Reef Tanks 2: Effects on Macroalgae Growth
: http://www.advancedaquarist.com/iss...il2003/chem.htm
:
:
: Magnesium and Strontium
:
: Strontium
: http://www.advancedaquarist.com/issues/nov2003/chem.htm
:
: Magnesium
: http://www.advancedaquarist.com/issues/oct2003/chem.htm
:
: Magnesium and Strontium in Limewater
: http://www.advancedaquarist.com/issues/dec2003/chem.htm
:
:
: Limewater (kalkwasser)
:
: The Self Purification of Limewater (Kalkwasser)
: http://www.advancedaquarist.com/issues/may2003/chem.htm
:
: The Degradation of Limewater (Kalkwasser) in Air
: http://reefkeeping.com/issues/2003-...ature/index.htm
:
: How to Select a Calcium and Alkalinity Supplementation Scheme
: http://www.advancedaquarist.com/issues/feb2003/chem.htm
:
: Metals in Aquaria
:
: Aluminum and aluminum-based phosphate binders
: http://www.advancedaquarist.com/iss...ly2003/chem.htm
:
: Reef Aquaria with Low Soluble Metals
: http://reefkeeping.com/issues/2003-...ature/index.htm
:
: Tap Water in Reef Aquaria
: http://www.advancedaquarist.com/issues/jan2004/chem.htm
: First Iron Article: Macroalgae and Dosing Recommendations
: http://www.advancedaquarist.com/issues/aug2002/chem.htm
:
: Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
: http://www.advancedaquarist.com/issues/oct2002/chem.htm
:
:
: Test Kit Reviews
:
: The Seachem Borate Alkalinity Test Kit
: http://www.advancedaquarist.com/iss...ne2003/chem.htm
:
: The Salifert Boron Test Kit
: http://www.advancedaquarist.com/iss...pt2003/chem.htm
:
: Boron and Borate (and pH buffering)
:
: Boron in a Reef Tank (and its effect on pH buffering)
: http://www.advancedaquarist.com/issues/dec2002/chem.htm
:
: The Seachem Borate Alkalinity Test Kit
: http://www.advancedaquarist.com/iss...ne2003/chem.htm
:
: The Salifert Boron Test Kit
: http://www.advancedaquarist.com/iss...pt2003/chem.htm
:
:
:
: Others
:
: Tap Water in Reef Aquaria
: http://www.advancedaquarist.com/issues/jan2004/chem.htm
:
: ORP
: http://reefkeeping.com/issues/2003-...ature/index.htm
:
: Chloramine
: http://reefkeeping.com/issues/2003-...ature/index.htm
:
: Silica in a Reef Tank
: http://advancedaquarist.com/issues/jan2003/feature.htm
:
: Specific Gravity (and temperature correction of hydrometers)
: http://www.advancedaquarist.com/iss...2/chemistry.htm
:
:
: The Complete Nitrogen Cycle
: http://www.animalnetwork.com/fish/l...a&RecordNo=3090
:
: Magnesium (older article with fonts screwed up)
: http://www.aquariumfish.com/aquariu...cid=124&search=
:
: Phosphate (older article now reproduced in a poor fashion)
: http://www.aquariumfish.com/aquariu...cid=124&search=
:
: Carbon Dioxide
: http://www.animalnetwork.com/fish/l...a&RecordNo=2074
:
: Using Conductivity to Measure Salinity
: http://www.aquariumfish.com/aquariu...cid=124&search=
:
: Understanding Seawater
: http://www.animalnetwork.com/fish2/...s/1/default.asp
:
: Protein Skimming: How It Works
: http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
:
:
:
: Articles by Craig Bingman:
:
: Carbon Dioxide tests
: http://www.animalnetwork.com/fish/l...n=&RecordNo=279
:
: Limewater, Acetic Acid and Sand Clumping
: http://www.animalnetwork.com/fish/l...n=&RecordNo=181
:
: Calcium and Alkalinity
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: Calculation of Calcium Carbonate Saturation States in Reef Aquaria
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
:
: Calcification Rates in Several Tropical Coral Reef Aquaria
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: Limits To Limewater...Revisited
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: Expanding the Limits of Limewater: Adding Organic Carbon Sources (vinegar)
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
:
: Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: Magnesium - Part I
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: Magnesium - Part II
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: A Homemade Magnesium Supplement
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: Simulating the Effect of Calcium Chloride and Sodium Bicarbonate Additions on Reef
Systems
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: Additional Simulations: The Combined Effect Of Calcium Chloride
: /Sodium Bicarbonate Additions And Water Exchanges
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
:
: More articles by Craig Bingman:
:
: The Halogens - Part I: Bromine in Seawater and Aquaria
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: The Halogens - Part II: Fluoride
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: Fluoride Depletion In Four Reef Aquariums
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: The Halogens - Part III: Iodine
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: Measuring Halides
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: How Test Kits Work
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: Borax pH Calibration
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: A pH Detective Story
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: How to Mix a Batch of Synthetic Seawater in Under Five Minutes
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
: SILICON - FOE OR FRIEND?
: http://www.animalnetwork.com/fish2/...s/1/default.asp
:
: The Composition Of Several Synthetic Seawater Mixes
: http://www.animalnetwork.com/fish2/...s/1/default.asp
:
: Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
: http://www.animalnetwork.com/fish2/...bio/default.asp
:
:
:
: Andy's calcium calculator
: http://www.andy-hipkiss.co.uk/cacalc.htm
:
: Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
: http://www.aquariumfish.com/aquariu...cid=124&search=
:
: Calcium Reactor Substrate -- Phosphate Levels
: by Greg Hiller
: http://www.advancedaquarist.com/iss...l2003/short.htm
:
:
: Indoor CO2 Problems
: http://www.advancedaquarist.com/iss...r2002/short.htm
:
: Simon Huntington's CaCO3/CO2 reactor article
:
: http://reefkeeping.com/issues/2002-...ature/index.htm
:
: Ron Shimek's Tank Water Analysis Article
: http://reefkeeping.com/issues/2002-...ature/index.htm
:
:
:
:
: Home made salinity standards thread:
:
: http://reefcentral.com/forums/showt...?threadid=65509
:
: Reef Chemicals Calculator
: http://www.kademani.com/reefchem.htm
:
:
:
: Boomer
:
: Want to talk chemistry ? The Reef Chemistry Forum
: http://www.reefcentral.com/vbulletin/index.php
:
:
: Former US Army Bomb Technician (EOD)
: Member; IABTI, NATEODA, WEODF, ISEE & IPS
:
: If You See Me Running You Better Catch-Up
:
:
: --
: Boomer
:
: Want to talk chemistry ? The Reef Chemistry Forum
: http://www.reefcentral.com/vbulletin/index.php
:
: Want to See More ?
: Please Join Our Growing Membership
: www.coralrealm.com
:
: If You See Me Running You Better Catch-Up
: "stoutman" <.@.> wrote in message news:aGuWb.148227$U%5.676753@attbi_s03...
: : Boomer,
: :
: : I am not sure if you are just messing with me or if you are truly confused.
: : I hope the latter. Please read from Top to Bottom.
: :
: :
: : From YOUR first link:
: :
: : http://www.waterontheweb.org/resources/glossary.html
: :
: : Acidity:
: : A measure of how acid a solution may be. A solution with a pH of less than
: : 7.0 is considered acidic. Solutions with a pH of less than 4.5 contain
: : mineral acidity (due to strong inorganic acids), while a solution having a
: : pH greater than 8.3 contains no acidity.
: :
: : Yes,
: :
: : Good definition (for the most part). pH <7 is indeed acidic. pH > 7 is
: : basic. Your web page had a definition for acidity, but not basicity.
: : Strange. That's like defining GOOD and not defining BAD.
: :
: : Here is the IUPAC (International Union of Pure and Applied Chemistry)
: : definition of acidity:
: :
: : http://www.chem.qmul.ac.uk/iupac/index.html
: :
: : acidity
: :
: : (1) Of a compound:
: :
: : For Brønsted acids it means the tendency of a compound to act as a hydron
: : donor. It can be quantitatively expressed by the acid dissociation constant
: : of the compound in water or some other specified medium. For Lewis acids it
: : relates to the association constants of Lewis adducts and -adducts.
: :
: : (2) Of a medium:
: :
: : The use of the term is mainly restricted to a medium containing Brønsted
: : acids, where it means the tendency of the medium to hydronate a specific
: : reference base
: :
: : basicity
: :
: : For Brønsted bases it means the tendency of a compound to act as hydron
: : (proton) acceptor. The basicity of a chemical species is normally expressed
: : by the acidity of the conjugate acid (see conjugate acid-base pair). For
: : Lewis bases it relates to the association constants of Lewis adducts
: : and -adducts
: :
: :
: :
: : Another definition from the same web page YOU cited: (this is the same web
: : page you cited above)
: :
: : Alkalinity:
: : Acid neutralizing or buffering capacity of water; a measure of the ability
: : of water to resist changes in pH caused by the addition of acids or bases
: : and therefore, the main indicator of susceptibility to acid rain; in natural
: : waters it is due primarily to the presence of bicarbonates, carbonates and
: : to a much lesser extent occasionally borates, silicates and phosphates. It
: : is expressed in units of milligrams per liter (mg/l) of CaCO3 (calcium
: : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l = 1 mg/l
: : of CaCO3. A solution having a pH below about 5 contains no alkalinity.
: :
: : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and says
: : that alkalinity is the measure of ...(description of a buffer)
: :
: : A BUFFER IS : a measure of the ability of water to resist changes in pH
: : caused by the addition of acids or bases (from definition below)
: :
: :
: : I said:
: : ***alkalinity is a measurement of 'buffering capacity'***
: :
: : You said:
: : ***Alkalinity is not a measurement of BC
: :
: : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is not
: : logical.
: :
: : (THIS FROM THE SAME WEB PAGE YOU CITED):
: :
: : Buffer:
: : A substance which tends to keep pH levels fairly constant when acids or
: : bases are added.
: :
: : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
: :
: : a measure of the ability of water to resist changes in pH caused by the
: : addition of acids or bases
: :
: : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A BUFFER.
: :
: :
: : I went to all four links. None contradict what I have said. But the first
: : one you cited contradicts YOU!
: :
: : I know what a buffer is. I know what acidity means. I know what alkalinity
: : means. No need to cite web pages that describe what I know and what I wrote
: : in this discussion. Show me one that says alkalinity is not a measure of
: : buffering capacity from a credible source.
: :
: :
: :
: :
: :
: :
: : "Boomer" > wrote in message
: : ...
: : > Alkalinity a measure of the amount of anions of weak acid in water and of
: : the cations
: : > balanced against them
: : > Take note it says ***acid***
: : >
: : > Buffering capacity the ability of a solution to resist or dampen changes
: : in pH upon the
: : > addition of acids or bases.
: : > Take note its says ***the addition of acids or bases***
: : >
: : > One more
: : >
: : > http://www.waterontheweb.org/resources/glossary.html
: : >
: : > We could go on like this all day, so what is the point ?
: : >
: : > You will LOVE this one
: : > http://www.kyantec.com/Tips/phbuffering.htm
: : >
: : > Don't you just lovbe PDF's
: : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
: : >
: : > Don't fall out of your chair
: : > http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
: : >
: : >
: : >
: : >
: : > --
: : > Boomer
: : >
: : > Want to talk chemistry ? The Reef Chemistry Forum
: : > http://www.reefcentral.com/vbulletin/index.php
: : >
: : > Want to See More ?
: : > Please Join Our Growing Membership
: : > www.coralrealm.com
: : >
: : > If You See Me Running You Better Catch-Up
: : > "stoutman" <.@.> wrote in message news:XB7Wb.19339$QA2.62332@attbi_s52...
: : > : Man here is another, google is a wonderful thing. I'm not filtering any
: : > : out, just posting what I find by GOOGLING for you.
: : > :
: : > : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
: : > :
: : > :
: : > : Wow, a gov link. Even the government is wrong, this must be a
: : conspiracy
: : > : against Boomer.
: : > :
: : > :
: : > :
: : > :
: : > : "Boomer" > wrote in message
: : > : ...
: : > : > Now I am getting bored
: : > : >
: : > : > "Don't the components of a buffer account for the buffering capacity?
: : > : Yes."
: : > : >
: : > : > Yes, agreed but you seem to fail what I'm saying. Buffering Capacity
: : and
: : > : Alkalinity are
: : > : > not the same, that has always been the issue. I gave the equation does
: : > : that look like an
: : > : > Alkalinity equation or how Alk is determined. I see you had now
: : comments
: : > : on it what's
: : > : > wrong, why no comments on the equations I gave. Don't understand them
: : or
: : > : what ? Again this
: : > : > is the equation for Buffering Capacity, also called Buffer Index or
: : Buffer
: : > : Intensity. It
: : > : > is defined in most water chemistry and chemical oceanography text
: : books.
: : > : >
: : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] +
: : CKa
: : > : [H3O+] / (Ka =
: : > : > H3O+])² )
: : > : >
: : > : > This is not Alkalinity now is it ?
: : > : >
: : > : > "I know how to do a titration, In fact I have done several. How many
: : have
: : > : > you actually done? I don't mean by counting drops, I mean with a
: : buret?"
: : > : >
: : > : > Well good for you, I use a Digital Titrator
: : > : >
: : > : > "Oh, I see,
: : > : > you think acidity is the opposite of alkalinity. In the world of
: : > : CHEMISTRY
: : > : > it's not. Maybe in aquarium newsgroups it is.
: : > : >
: : > : > Hum no, maybe you should go for a look at HACH's or LaMotte website or
: : the
: : > : book I
: : > : > suggested earlier. Please view a copy.
: : > : >
: : > : > Standard Methods for the Examination of Water and Wastewater
: : > : >
: : > : > This book, over 2000 pages, is the guide for water testing. If you are
: : > : reporting water
: : > : > test to the EPA you must use approved std from this text.I t is
: : prepared
: : > : and published by
: : > : > the EPA, American Water Works Association and American Public Health
: : > : Association. You
: : > : > mean you don't have one and the issue is water chemistry
: : > : >
: : > : > You are confusing Acidity and Acidity as you know little about water
: : > : chemistry and
: : > : > procedures and test methods
: : > : >
: : > : > From SMEWW, section 2-30, 2310 ACIDITY
: : > : >
: : > : > "Acidity of water is its quantative capacity to react with a strong
: : base
: : > : to a designated
: : > : > pH"
: : > : >
: : > : > This is how you test for it
: : > : >
: : > : > A std alkali titration to methyl orange or phenolphthalein
: : > : > endpoint.
: : > : >
: : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write
: : this
: : > : book, there are
: : > : > over 100 of them, they are wrong.
: : > : >
: : > : > Like Buffering Capacity you have your Acidity's mixed up
: : > : > In water measurement if you have a high Alk you also usually have a
: : high
: : > : Acidity.
: : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
: : CHEMISTRY
: : > : BOOK there pal.
: : > : >
: : > : >
: : > : > "These are all in equilibrium with each other. An initial high pH
: : (above
: : > : > 6.4) will shift the equilibrium to the right to form HCO3-1. If the
: : pH of
: : > : > the solution is above 10.3 (pKa2) the .........."
: : > : >
: : > : >
: : > : > Christ, there you go again with the FW ****. All your numbers are
: : wrong we
: : > : are dealing
: : > : > with SEAWATER
: : > : >
: : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is in the
: : form
: : > : > of HCO3-1 .
: : > : >
: : > : > I have already pointed that out and gave actual values at know
: : seawater
: : > : levels, go back
: : > : > and re-read it you aren't telling me anything here.Of course most is
: : HCO3
: : > : see...
: : > : >
: : > : >
: : > : > @ 20C and 34.3 ppt salinity
: : > : >
: : > : > CO2 = 0.52 %
: : > : >
: : > : > HCO3 = 86.4 %
: : > : >
: : > : > CO3 = 13.09 %
: : > : >
: : > : >
: : > : > "In your glass experiment you managed to lower the pH enough to purge
: : out
: : > : CO2
: : > : > by boiling"
: : > : >
: : > : > The purpose behind the glass is to show that alk is not affect by CO2
: : and
: : > : vise-versa and
: : > : > how Co2 affects pH.
: : > : >
: : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and that pH
: : drops
: : > : to say 8.1 it is
: : > : > usually due to excess CO2. If you took a glass of that water and
: : aerated
: : > : it you WILL drive
: : > : > off the CO2 and raise the pH. It has been done a proven a million
: : times.
: : > : >
: : > : > "In order to 'purge' CO2 you would need to lower the
: : > : > pH to shift the equilibrium to below 6.4"
: : > : >
: : > : > The hell you do !!!.Do you know who many times people on this NG to
: : > : include Dr. Craig
: : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
: : > : sample of aquarium
: : > : > water and aerate it to see if the pH GOES UP AND when they come back
: : with
: : > : the test it is
: : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST
: : excess
: : > : CO2 in the tank
: : > : > water, increase the circulation for better gas exchange at the
: : surface,
: : > : reduce feeding,
: : > : > and try to improve on better skimming, thus reducing the bio-load and
: : pH
: : > : decline due to
: : > : > CO2.
: : > : >
: : > : >
: : > : > "I hope this helps. "
: : > : >
: : > : > Help, how can you when you miss everything. I should be charging you
: : > : >
: : > : > Oh, by the way. Your websites, I have about 50 on these issues, I
: : could
: : > : post them, not to
: : > : > mention I have all those water chemistry books, so there is no need to
: : > : view your sites.
: : > : >
: : > : > Finally are you afraid to come to our Chemistry Forum, afraid to get
: : > : slapped by REAL
: : > : > chemists. I get a charge out of you can't post your ref .I have posted
: : the
: : > : same or similar
: : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500
: : posts
: : > : there and am the
: : > : > biggest contributor to his forum other than himself or maybe Habib
: : Sheka
: : > : >
: : > : > Hum, here are Randy's ref that he posted. He hosts the website
: : > : >
: : > : > S. RANDY HOLMES-FARLEY
: : > : > Arlington, Massachusetts
: : > : >
: : > : > EDUCATION
: : > : >
: : > : > 1982-1986 Harvard University Cambridge, MA
: : > : > PhD in Chemistry
: : > : > Research Advisor: George Whitesides
: : > : >
: : > : > Investigated the relationship between polymer surface chemistry and
: : > : physical properties
: : > : > through controlled surface modification and testing.
: : > : >
: : > : > 1980-1982 Cornell University Ithaca, NY
: : > : > BA in Chemistry and Biology
: : > : > Graduated Summa Cum Laude
: : > : > Distinction in All Subjects
: : > : > Grade Point: 3.94/4.0
: : > : > Honors research: isolation and characterization of the subunit of CF1
: : > : enzyme
: : > : >
: : > : >
: : > : > 1978-1979 Stanford University Palo Alto, CA
: : > : > Grade Point: 3.55/4.0
: : > : >
: : > : >
: : > : > EXPERIENCE
: : > : >
: : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
: : > : > (bought out GelTex Pharmaceuticals in 2001)
: : > : > Vice President, Chemical Research 2001-present
: : > : > Senior Director, Chemical Research 1999-2001
: : > : > Director of Chemical Research 1997-1999
: : > : > Manager of Chemical Research 1995-1997
: : > : > Group Leader 1994-1995
: : > : > Senior Research Scientist 1992-1994
: : > : >
: : > : > Helped start GelTex as second employee
: : > : >
: : > : > Managed various research programs with multi-million dollar budgets
: : > : >
: : > : > Supervised research chemists (17+)
: : > : >
: : > : > Co-inventor of several polymeric pharmaceuticals and pharmaceutical
: : > : candidates including
: : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride
: : (FDA
: : > : approved)
: : > : >
: : > : > Company Safety Officer for 3 years
: : > : >
: : > : > Chemical Hygiene Officer 2000-present
: : > : >
: : > : >
: : > : >
: : > : >
: : > : > 1990-1992 GTE Corporation Waltham, MA
: : > : > Senior Member of Technical Staff
: : > : > Applied research involving polymer interfaces
: : > : > Metallization of plastics
: : > : > Polymer/polymer adhesion
: : > : > Optical coatings
: : > : >
: : > : >
: : > : >
: : > : > 1986-1990 Lord Corporation Cary, NC
: : > : > Senior Research Scientist 1988-1990
: : > : > Research Scientist 1986-1988
: : > : > Basic and applied research on surface chemical bonding
: : > : > Developed new adhesive compositions
: : > : > Developed new sol-gel coatings for corrosion resistance
: : > : >
: : > : >
: : > : > HONORS AND AWARDS
: : > : >
: : > : > Industrial Innovations Award by Northeast Region of American Chemical
: : > : Society (6/2001)
: : > : >
: : > : > National Kidney Foundation of Northern California Honoree (5/2001)
: : > : >
: : > : > American Chemical Society/Polymer Chemistry Division Industrial
: : Sponsors
: : > : > Award (8/2000)
: : > : >
: : > : > R&D 100 Award from R&D magazine (1999)
: : > : >
: : > : > Sherwin Williams Award in applied polymer science (9/85)
: : > : >
: : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
: : > : >
: : > : > Award for highest GPA in Chemistry Department (6/82)
: : > : >
: : > : > Summa Cum Laude Honors in Chemistry (6/82)
: : > : >
: : > : > Phi Lamda Epsilon (6/82)
: : > : >
: : > : > Phi Beta Kappa (2/82)
: : > : >
: : > : > Cornell University Dean's List (1981, 1982)
: : > : >
: : > : > Harvard Book Club Award for highest GPA senior year (1978)
: : > : >
: : > : > First Place in western NY ACS high school chemistry exam (1977)
: : > : >
: : > : > 1978-1979
: : > : >
: : > : >
: : > : > __________________
: : > : > Randy Holmes-Farley
: : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
: : > : >
: : > : > Hobby Experience: 8 years with reefs
: : > : > Current Tanks: 90 gal mixed reef
: : > : > Interests: Reefkeeping, science, photography
: : > : >
: : > : >
: : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
: : > : >
: : > : > Open this post in a new window | Report this post to a moderator | IP:
: : > : Logged
: : > : >
: : > : >
: : > : >
: : > : > 06/27/2003 02:44 PM
: : > : >
: : > : > Randy Holmes-Farley
: : > : > Chemistry Moderator
: : > : >
: : > : > Registered: Apr 2001
: : > : > Location: Arlington, Massachusetts
: : > : > Occupation: Chemist (Drug Discovery at Genzyme)
: : > : > Posts: 15282
: : > : >
: : > : >
: : > : >
: : > : > Publications
: : > : >
: : > : >
: : > : > ISSUED UNITED STATES PATENTS
: : > : >
: : > : >
: : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
: : > : Mandeville, III; W. Harry.
: : > : > US 6,566,407; 5/20/2003
: : > : >
: : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen
: : Randall;
: : > : Huval, Chad
: : > : > Cori.
: : > : > U.S. 6,517,825; 2/11/2003.
: : > : >
: : > : > 3. Method of making phosphate-binding polymers for oral
: : administration.
: : > : Holmes-Farley,
: : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
: : > : 6,509,013; 1/21/2003.
: : > : >
: : > : > 4. Combination therapy for treating hypercholesterolemia using a bile
: : acid
: : > : sequestrant
: : > : > polymer
: : > : > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley,
: : Stephen
: : > : Randall;
: : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
: : > : >
: : > : > 5. Method for treating hypercholesterolemia with polyallylamine
: : polymers.
: : > : Holmes-Farley,
: : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
: : Goldberg,
: : > : Dennis I. , US
: : > : > 6,423,754; 7/23/2002.
: : > : >
: : > : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
: : > : Neenan, Thomas X..;
: : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
: : > : >
: : > : > 7. Combination therapy for treating hypercholesterolemia and
: : > : atherosclerosis. Huval, Chad
: : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep
: : K.
: : > : U.S. 6,365,186;
: : > : > 4/2/2002.
: : > : >
: : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
: : Mandeville,
: : > : W. H., III;
: : > : > Huval; C.
: : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
: : > : 10/9/2001.
: : > : >
: : > : > 9. Polymers containing guanidinium groups as bile acid sequestrants.
: : Dhal;
: : > : P. K.; Holmes-
: : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
: : > : >
: : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
: : H.,
: : > : III.; US
: : > : > 6,281,252;
: : > : > 8/28/2001.
: : > : >
: : > : > 11. Combination therapy for treating hypercholestrolemia. Huval; C.
: : C.;
: : > : Holmes-Farley; S.
: : > : > R. ;
: : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
: : > : >
: : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
: : > : Holmes-Farley, S.
: : > : > R.; US
: : > : > 6,264,937; 7/24/2001.
: : > : >
: : > : > 13. Method for treating hypercholesterolemia with unsubstituted
: : > : polydiallylamine polymers.
: : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
: : > : 6,248,318;
: : > : > 6/19/2001.
: : > : >
: : > : > 14. Process for removing bile salts from a patient and alkylated
: : > : compositions therefore.
: : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
: : > : >
: : > : > 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S.
: : R.;
: : > : Dhal, P. K.;
: : > : > Petersen,
: : > : > J. S.; US 6,203,785; 3/20/2001.
: : > : >
: : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.;
: : Huval,
: : > : C. C.; US
: : > : > 6,190,649;
: : > : > 2/20/2001.
: : > : >
: : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
: : H.,
: : > : III.; US
: : > : > 6,177,478;
: : > : > 1/23/2001.
: : > : >
: : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
: : Holmes-Farley,
: : > : S. R.;
: : > : > Mandeville, W.
: : > : > H., III.; US 6,129,910; 10/10/2000.
: : > : >
: : > : > 19. Method for treating hypercholesterolemia with unsubstituted
: : > : polydiallylamine polymers.
: : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
: : > : 6,083,497;
: : > : > 7/4/2000.
: : > : >
: : > : > 20. Method of making phosphate-binding polymers for oral
: : administration.
: : > : Holmes-Farley, S.
: : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495;
: : 7/4/2000.
: : > : >
: : > : > 21. Process for removing bile salts from a patient and alkylated
: : > : compositions therefore.
: : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
: : 5/23/2000.
: : > : >
: : > : > 22. Process for removing bile salts from a patient and compositions
: : > : therefor. Mandeville,
: : > : > W. H.,
: : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
: : > : >
: : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
: : > : Neenan; T. X.; Holmes-
: : > : > Farley; S. R. US 6,034,129; 3/7/2000.
: : > : >
: : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
: : H.,
: : > : III.; US
: : > : > 5,985,938;
: : > : > 11/16/99.
: : > : >
: : > : > 25. Process for removing bile salts from a patient and compositions
: : > : therefor. Mandeville,
: : > : > W. H.,
: : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
: : > : >
: : > : > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W.
: : H.,
: : > : III.;
: : > : > Holmes-Farley;
: : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
: : > : >
: : > : > 27. Hydrophilic nonamine-containing and amine-containing copolymers
: : and
: : > : their use as bile
: : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
: : 5,929,184;
: : > : 7/27/99.
: : > : >
: : > : > 28. Interpenetrating polymer networks for sequestration of bile acids.
: : > : Mandeville, W. H.,
: : > : > III.;
: : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
: : > : 7/20/99.
: : > : >
: : > : > 29. Amine polymer sequestrant and method of cholesterol depletion.
: : > : Mandeville, W. H.,
: : > : > III.;
: : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
: : > : >
: : > : > 30. Process for removing bile salts from a patient and compositions
: : > : therefor. Mandeville,
: : > : > W. H.,
: : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
: : > : >
: : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
: : > : Mandeville, W. H.,
: : > : > III.;
: : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
: : > : >
: : > : > 32. Process for removing bile salts from a patient and compositions
: : > : therefor. Mandeville,
: : > : > W. H.,
: : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
: : > : >
: : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
: : Mandeville,
: : > : W. H., III.;
: : > : > Holmes-
: : > : > Farley, S. R.; US 5,703,188; 12/30/97.
: : > : >
: : > : > 34. Oral administration of iron-binding crosslinked amine polymers.
: : > : Mandeville, W. H.,
: : > : > III.;
: : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
: : > : >
: : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley,
: : S.
: : > : R.; US 5,693,675;
: : > : > 12/2/97.
: : > : >
: : > : > 36. Method for removing bile salts from a patient with alkylated
: : > : crosslinked amine
: : > : > polymers,
: : > : > and preparation of the polymers. Mandeville, W. H., III.;
: : Holmes-Farley,
: : > : S. R.; US
: : > : > 5,679,717; 10/21/97.
: : > : >
: : > : > 37. Phosphate-binding polymers for oral administration. Holmes-Farley,
: : S.
: : > : R.; Mandeville,
: : > : > W.
: : > : > H., III.; US 5,667,775; 9/16/97.
: : > : >
: : > : > 38. Ion-exchange process using highly crosslinked polymers for
: : removing
: : > : bile salts from a
: : > : > patient, preparation of the polymers, and compositions containing
: : them.
: : > : Mandeville, W. H.,
: : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
: : > : >
: : > : > 39. Hydrophobic amine polymer sequestrant and method of cholesterol
: : > : depletion. Mandeville,
: : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530;
: : 4/8/97.
: : > : >
: : > : > 40. Amine polymer sequestrant and method of cholesterol depletion.
: : > : Mandeville, W. H.,
: : > : > III.;
: : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
: : > : >
: : > : > 41. Phosphate-binding polymers for oral administration. Holmes-Farley,
: : S.
: : > : R.; Mandeville,
: : > : > W.
: : > : > H., III.; US 5,496,545; 3/5/96.
: : > : >
: : > : > 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
: : > : III.; Holmes-Farley,
: : > : > S. R.;
: : > : > US 5,487,888; 1/30/96.
: : > : >
: : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having active
: : > : hydrogens on the
: : > : > surface.
: : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
: : > : >
: : > : > 44. Layered sol-gel coatings from organisilicon compounds.
: : Holmes-Farley,
: : > : S. R.; Yanyo, L.
: : > : > C.;
: : > : > US 5,182,143; 1/26/93.
: : > : >
: : > : > 45. Method for metal bonding using ultrathin primer coating.
: : > : Holmes-Farley, S. R.; Yanyo,
: : > : > L.
: : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
: : > : >
: : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.;
: : US
: : > : 5,096,962;
: : > : > 3/17/92.
: : > : >
: : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
: : > : elastomer-metal bonding.
: : > : > Holmes-
: : > : > Farley, S. R.; US 5,102,956; 4/7/92.
: : > : >
: : > : >
: : > : >
: : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
: : > : >
: : > : >
: : > : > 1. Aryl boronate functionalized polymers for treating obesity and
: : > : inhibiting fat uptake.
: : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal,
: : Pradeep
: : > : K.; Huval, Chad
: : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92
: : pp. WO
: : > : 0302571.
: : > : >
: : > : > 2. Preparation of aryl boronic acids for treating obesity.
: : Holmes-Farley,
: : > : Stephen Randall;
: : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep
: : K.
: : > : (Geltex
: : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
: : > : >
: : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
: : > : Stephen Randall.
: : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
: : > : 0302130.
: : > : >
: : > : > 4. Method for reducing copper levels and treating copper toxicosis.
: : > : Holmes-Farley, Stephen
: : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002),
: : 45
: : > : pp. WO
: : > : > 0285383.
: : > : >
: : > : > 5. Method for treating gout and binding uric acid. Holmes-Farley,
: : Stephen
: : > : Randall; Burke,
: : > : > Steven K. WO 0285381 10/31/2002.
: : > : >
: : > : > 6. Method for treating gout and reducing serum uric acid.
: : Holmes-Farley,
: : > : Stephen Randall;
: : > : > Burke, Steven K WO 0285380 10/31/2002.
: : > : >
: : > : > 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
: : > : Holmes-Farley, S. R.;
: : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
: : > : >
: : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
: : > : Holmes-Farley, S.
: : > : > R.;
: : > : > WO 1999-US5662; 9/23/1999.
: : > : >
: : > : > 9. Amine-containing copolymers as bile acid sequestrants.
: : Holmes-Farley,
: : > : S. R.; Petersen,
: : > : > J. S.;
: : > : > WO 9933452; 7/8/1999.
: : > : >
: : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III
: : and
: : > : Holmes-Farley, S.
: : > : > R.;
: : > : > WO 9922743; 5/14/1999.
: : > : >
: : > : > 11. Polyallylamine polymers for removing bile salts and treating
: : > : hypercholesterolemia, and
: : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III;
: : Burke,
: : > : S. K.; Goldberg,
: : > : > D. I.; WO 9857652; 12/23/98.
: : > : >
: : > : > 12. Phosphate-bidning polymers combined with a calcium supplement for
: : oral
: : > : administration.
: : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley,
: : S.
: : > : R.; WO 9842355;
: : > : > 10/1/98.
: : > : >
: : > : > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
: : > : depletion. Mandeville,
: : > : > W.
: : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
: : > : >
: : > : > 14. Process for adjusting ion concentration in a patient and
: : compositions
: : > : therefor.
: : > : > Mandeville,
: : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
: : > : >
: : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
: : interlayer
: : > : for improved
: : > : > metal-
: : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
: : 1/20/94.
: : > : >
: : > : > 16. Process for increased metal-substrate bond strength in metalized
: : > : plastics.
: : > : > Holmes-Farley, S.
: : > : > R.; Ger. Offen. 4322516; 7/6/93.
: : > : >
: : > : > 17. Electrorheological fluids and preparation of particles useful in
: : the
: : > : fluids.
: : > : > Troughton,
: : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
: : > : David; Bares, Joseph
: : > : > E.;
: : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
: : > : 394049;
: : > : > 10/24/1990.
: : > : >
: : > : > JOURNAL PUBLICATIONS
: : > : >
: : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov,
: : Eugene;
: : > : Guo, Amy;
: : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
: : > : Mandeville, W. Harry;
: : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
: : 611-619.
: : > : >
: : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
: : synthesis
: : > : and biological
: : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S.
: : Randall;
: : > : Mandeville, W.
: : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
: : > : Journal of
: : > : > Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
: : > : 1559-1574.
: : > : >
: : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
: : > : Imprinting. Huval,
: : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
: : > : Randall; Mandeville,
: : > : > W.
: : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert
: : J.;
: : > : Chen, Xi; Dhal,
: : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
: : > : >
: : > : > 4. Synthetic polymers for the binding of fat in the intestinal tract.
: : > : Jozefiak, Thomas H.;
: : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia;
: : Huval,
: : > : Chad C.;
: : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
: : > : Abstracts of
: : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
: : > : 26-30, 2001
: : > : > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
: : > : Division of
: : > : > Polymer Chemistry) (2001), 42(2), 98.
: : > : >
: : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer
: : gel
: : > : pharmaceutical.
: : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.;
: : Ward,
: : > : J.; Sacchiero,
: : > : > B.;
: : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.;
: : Chen,
: : > : X.; Mazzeo, J.
: : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
: : > : >
: : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl and
: : other
: : > : bile acid
: : > : > sequestrants.
: : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
: : > : Hook, P.; Holmes-
: : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
: : > : >
: : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
: : Holmes-Farley,
: : > : S. R; Polym.
: : > : > Mater. Sci. Eng (1999), 80, 246-247.
: : > : >
: : > : > 8. Design and characterization of of Sevelamer Hydrochloride: a novel
: : > : phosphate-binding
: : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward,
: : J.;
: : > : Miller, K. L.;
: : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure
: : and
: : > : Appl. Chem.,
: : > : > A36(7&8), p. 1085 (1999).
: : > : >
: : > : > 9. Three generations of bile acid sequestrants. Mandeville, W. H.,
: : III;
: : > : Braunlin, W.;
: : > : > Dhal, P.;
: : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
: : > : Rosenbaum, D.;
: : > : > Sacchiero,
: : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
: : > : 550, 3-15.
: : > : >
: : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric
: : phosphate
: : > : binder, on
: : > : > urinary
: : > : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
: : > : Mandeville, W. H.,
: : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
: : > : (1997), 12(5)
: : > : > 961-964.
: : > : >
: : > : > 11. Thin anisotropic coatings based on sol-gel technology.
: : Holmes-Farley,
: : > : S. R.; Yanyo, L.
: : > : > C;
: : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4),
: : 439-444.
: : > : >
: : > : > 12. The mechanism of cure initiation of a surface activated adhesive.
: : > : Holmes-Farley, S.
: : > : > R.;
: : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
: : > : >
: : > : > 13. Adhesion promotion and corrosion prevention using thin anisotropic
: : > : coatings. Holmes-
: : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
: : > : 131-151.
: : > : >
: : > : > 14. Wetting of functionalized polyethylene having ionizable organic
: : acids
: : > : and bases at the
: : > : > polymer-water interface: relations between functional group polarity,
: : > : extent of
: : > : > ionization,
: : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
: : > : Whitesides, G. M.;
: : > : > Langmuir
: : > : > (1988), 4(4), 921-937.
: : > : >
: : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
: : > : single hydroxy group.
: : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
: : > : >
: : > : > 16. Reconstruction of the interface of oxidatively functionalized
: : > : polyethylene (PE-CO2H)
: : > : > and
: : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo,
: : R.;
: : > : McCarthy, T. J.;
: : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report
: : (1987),
: : > : AD-
: : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
: : > : >
: : > : > 17. Surface-modified polyethylene film: the relationship between
: : surface
: : > : chemistry and
: : > : > physical
: : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11),
: : 4537.
: : > : >
: : > : > 18. Reactivity of carboxylic acid and ester groups in the
: : functionalized
: : > : interfacial
: : > : > region of
: : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
: : > : differentiation of the
: : > : > functional groups into shallow and deep subsets based on a comparison
: : of
: : > : contact angle and
: : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
: : > : (1987), 3(1), 62-
: : > : > 76.
: : > : >
: : > : > 19. Fluorescence properties of dansyl groups covalently bonded tot he
: : > : surface of
: : > : > oxidatively
: : > : > functionalized low-density polyethylene film. Holmes-Farley, S. R.;
: : > : Whitesides, G. M.;
: : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
: : > : AD-A162435/2/GAR,
: : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
: : > : >
: : > : > 20. Acid-base behavior of carboxylic acid groups covalently attached
: : at
: : > : the surface of
: : > : > polyethylene: The usefulness of contact angle in following the
: : ionization
: : > : of surface
: : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
: : > : Deutch, J.;
: : > : > Whitesides,
: : > : > G. M.; Langmuir (1985), 1(6), 725-740.
: : > : >
: : > : > 21. The thermal stability of a surface modified solid organic polymer.
: : > : Holmes-Farley, S.
: : > : > R.;
: : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
: : > : >
: : > : >
: : > : >
: : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
: : > : >
: : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
: : > : Aquarist. June 2003.
: : > : >
: : > : > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
: : > : Advanced Aquarist.
: : > : > May
: : > : > 2003.
: : > : >
: : > : > 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
: : > : Reefkeeping May
: : > : > 2003.
: : > : >
: : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
: : > : April 2003.
: : > : >
: : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
: : > : Holmes-Farley, R.
: : > : > Advanced Aquarist; April 2003.
: : > : >
: : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
: : > : Holmes-Farley, R.
: : > : > Advanced Aquarist; April 2003.
: : > : >
: : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced
: : Aquarist;
: : > : March 2003.
: : > : >
: : > : > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
: : > : Holmes-Farley, R.
: : > : > Advanced Aquarist; February 2003.
: : > : >
: : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
: : > : 2003.
: : > : >
: : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
: : December
: : > : 2002.
: : > : >
: : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
: : Advanced
: : > : Aquarist; November
: : > : > 2002.
: : > : >
: : > : > 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
: : > : Advanced Aquarist;
: : > : > November 2002.
: : > : >
: : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced
: : Aquarist,
: : > : September 2002.
: : > : >
: : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
: : > : 2002.
: : > : >
: : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
: : > : 2002.
: : > : >
: : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
: : > : Aquarist; July 2002
: : > : >
: : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist;
: : June
: : > : 2002.
: : > : >
: : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R.
: : Advanced
: : > : Aquarist, May
: : > : > 2002.
: : > : >
: : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
: : > : Holmes-Farley, R.
: : > : > Advanced Aquarist, April 2002.
: : > : >
: : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
: : > : >
: : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
: : > : >
: : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January
: : 2002.
: : > : >
: : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
: : > : 2000.
: : > : >
: : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
: : > : Frontiers 2000.
: : > : >
: : > : > 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
: : > : Aquarium Frontiers
: : > : > 2000.
: : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
: : Frontiers
: : > : 2000.
: : > : >
: : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers
: : 2000.
: : > : >
: : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
: : > : >
: : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
: : > : >
: : > : >
: : > : >
: : > : >
: : > : >
: : > : >
: : > : >
: : > : > Boomer
: : > : >
: : > : > Want to talk chemistry ? The Reef Chemistry Forum
: : > : > http://www.reefcentral.com/vbulletin/index.php
: : > : >
: : > : > Want to See More ?
: : > : > Please Join Our Growing Membership
: : > : > www.coralrealm.com
: : > : >
: : > : >
: : > : >
: : > :
: : > :
: : >
: : >
: :
: :
: :
:
:

[stoutman]

First let me address the main point (if there is a point) of this debate:

Is alkalinity a measure of buffering capacity?????

Buffering capacity is a function of both ALKALINITY and pH as described by
the equation YOU posted.

If you measure ALKALINITY and you know your pH you have determined your
BUFFERING CAPACITY.

Formula for BUFFERING CAPACITY:

B (Buffering Index) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa [H3O+]/
(Ka + H3O+])² )

Lets break it down ok?

B = 2.303 ( Kw/[H30+] + [H30+] + CKa [H3O+]/(Ka + H3O+])² )

with me so far?

these are the variables:

Kw = 1x10 -14
Ka = acid dissociation constant (from a table)
C = concentration of acid plus it's conjugate base.
[H3O+] = [H+] determined from pH which = -log[H+]

with me so far?

Kw is known, Ka comes from a table (you even gave it for sw at one point),
[H+] comes from pH. Only one we need to determine is C

C = concentration of acid plus it's conjugate base

acid = HCO3-
conjugate base = CO3-2

How can we determine the combined concentration of [HCO3-] and [CO3-2] ???
hmmmmm. Oh, wait a minute.

>Alkalinity = [HCO3-] + 2[CO3] +[OH] - [H+]

Most people consider the source of alkalinity as [HCO3-] and [CO3-2]
agreed?

So when we measure Alkalinity we are in effect determining the combined
concentration of HCO3- and CO3-2 (also called carbonate hardness)

Agreed?

Now we can plug these values into our BC equation and solve for BC.

So, when we measure ALKALINITY (and we know the pH) we are in effect
measuring BUFFERING CAPACITY.

Agreed? (of course you don't) lol


With regard to your other comments:

Yeah, I used the wrong Ka's. I used FW instead of SW. Ok. OOps. I can go
back and do the calculations over if you like. But it wont change the
overall point I was making at the time (with the exception of the actual
ratios).










"Boomer" > wrote in message
...
>
> "I am not sure if you are just messing with me "
>
> Yes, messing with you, it is called trolling a troll, to see where the
hell you would go
> and what you would say in regards to last posts. It is called honesty, of
which you have
> none off to say the least,that I can see.You always like to post what
suits you and just
> avoid ref I give. So lets start where you are WRONG and have a great lack
of understanding
> of things, to include pointing out all your gross error which you still
FAIL to
> acknowledge and which can be prove in many water chem. ref. .I doubt like
hell you are a
> chemist at all.You seem to want to con people into thinkin' you are. But
then again, I
> have seen chemists like you before, they are not familiar with the, but
they ASK to have
> it explained and ask for REF.YOU just shoot from the hip. WHAT GETS YOU IN
TROUBLE. You
> remind me of snoot-noise kid that come here and other NG's and
forums...that think they
> know, buy hey, maybe I'm wrong :-)
>
>
>
> 1). Acidity
>
> "***Benjamin,Water Chemistry (2002, pages 262-263).***
>
> ***Acidity A concept that is exactly analogous to alkalinity but measures
the base
> neutralizing
> capacity (BNC) of a solution is Acidity. The quantitative represents the
concentration of
> OH- ions that must be added to titrate the solution to a pH near 10.5***
>
> So that means that not only in Benjamin wrong but, so are Stumm & Morgan,
Millero, Pilosn,
> Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I
said, you have your
> acidity and Acidy mixed up. Acidity as defined above is covered in most
water chemistry
> books, written by chemists, who's field of expertise is water chemistry.
You can even buy
> Acidity test kits from, HACH, LaMotte, etc..
>
> You mean you didn't read this or are you just avoiding it .The same
definition can be
> found in almost any std water chemistry book.
>
> I have run into few chemists, that are NOT familiar with the above. Some
water reports
> require the above Acidity measuring. The issue with you is you do not
understand WATER
> CHEMISTRY. Everything you have posted can be found a general chemistry
book
>
>
>
>
> 2) Alk and BC
>
> From the link
>
> Alkalinity
> ***Acid neutralizing or buffering capacity of water; a measure of the
ability of water to
> resist changes in pH caused by the addition of acids or bases ***
>
> This is a Buffering Capacity definition not Alk
>
> Humm, since when does Alk have anything to do in regards to the addition
of BASE. As I
> pointed out in the first post the term is often miss used. Even in YOUR
own posts you say
> it is based on a acid addition, no mention of **base or acid** addition
by you. Are you
> getting confused or what. Or is more you are trying to confuse everyone
you are right. The
> above is a definition for Buffer Capacity NOT Alk
>
> From Drew, Geochemistry of Natural Waters
>
> "alkalinity, which is formally defined as the equivalent sum of bases that
are titratable
> with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH of
the solution is
> progressively lowered by the addition of a strong acid (HCL), all the
anions on the right
> will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4, H2S,organic
acids, H20)"
>
> This follows almost all description of Alk, that it is acid neutralizing
reaction and has
> nothing to do with base neutralizing, which is Acidity (BNC) .I defined
these before you
> had no comment
>
>
> Even the links that give the Buffering Capacity definition is wrong, as is
the UIPAC on
> Alkalinity. Alkalinity has nothing to do with the addition of bases only
acids. When you
> use the words "base and acid" it becomes BC
>
> Even YOU MUST disagree with these definitions, from YOUR own post
>
> Think of alkalinity as 'buffering capacity'. Or the ability of a solution
> ***to resist a drop in pH due to the addition of acid***
>
> Where the flip is the base addition forget it ?
>
> From Butler; Carbon Dioxide Equilibrium and Their Applications (professor
emeritus
> Harvard University) an expert on the subject.
>
> Buffering Index (Buffering Capacity, Buffer Intensity).
>
> ***This concept was first developed for mixtures of approximately equal
proportions of
> conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such
buffer solutions
> strongly resist changes in pH when acids or bases are added and are useful
as pH
> standards. The Buffer Index tells how great the resistance to pH changes
will be.**
>
> also from Butler
>
> Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
>
> Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
>
> Acidity is in fact just the negative of Alkalinity ***
>
> http://www.lagoonsonline.com/acid.htm
>
>
http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.h
tm?E+mystore
>
> It sure is funny how all of the chemist that write water chemistry
textbooks never say Alk
> is the Buffering Capacity of a solution. They are always treated and
defined separately.
>
> If you or others choose to treat Alk and BC as the same, well, just have
at it. As I said
> in first post I know what you mean.
>
> "No need to cite web pages that describe what I know and what I wrote
> in this discussion"
>
> No you don't know, who are you trying to convince any way, me, the guys
here and/or all
> the water chemists in this world. As I said before go get a dam WATER
CHEMISTRY book or
> shut the hell up.You keep trying to define things from a general chemistry
book WE ARE IN
> THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
>
>
>
>
>
> 3). pKa's and what you don't know or seem to be confused on
>
> "Therefore, it has two pKa's
> (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
The
> pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> right in there. Is that magic? :)"
>
> Here it is agin that is twice at least
>
> "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this
example)
> you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium will
> be shifted to HCO3-2 by a ratio of 1:100.
>
> Oh wait , there is a third time LOL
>
> "At the pH of seawater, the buffering capacity of carbonate is at it's
> weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
>
>
> Lets just dunk you on this one. I am taking note you refuse to reply to
YOUR errors
>
> So you calculated the pH of seawater with freshwater pKa's, now that is a
good trick. From
> a number of seawater chemistry books the seawater pKa's are 6 & 9.1, so
according to you,
> seemingly not understanding your favorite Henderson-Hasselbach equation;
>
> 2 pH = (6 + 9.1) /2 pH = 7.55
>
> I have never seen seawater with a pH of 7.55. There is no ocean with that
pH. Humm how
> come your equation is not working for you today.?
>
>
> "That pH I calculated is
> right in there. Is that magic? :)"
>
> I roll on the floor when I see this = 8.35
>
> Hum , just a brain far so excuse me for thinkin
>
> (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
>
> Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a pH of
8.35 there pal
> ? That 8.35 is what you are telling people the pH should be, but their
meter says 6.4.
> This how people will READ this.
>
>
>
>
> 4.) More on Buffering Capacity
>
> "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes, your
> alkalinity equation."'
>
>
> Yup, I see that and in this case the HCO3 is the acid and the CO3 is the
base CORRECT. In
> Alk you are only dealing with bases and how they react to an acid. Acidity
deals acids and
> how they recact to bases "Acidity, A concept that is exactly analogous to
alkalinity but
> measures the base neutralizing
> capacity (BNC) of a solution is Acidity "Alk is the ANC Acid neutralizing
capacity
>
> "Don't the components of a buffer account for the buffering capacity? "
>
> Yes, they do but so do the acids which work as buffers. NaHCO3 is a buffer
and can act as
> an acid or base
>
> *** Buffering Capacity.**
> The power of a substance in solution to absorb acid or alkali without
change in pH; this
> is highest at a pH value equal to the pKa value of the acid of the buffer
pair.***
>
> ***Akalinity***
> Measure of the power of a solution to neutralise hydrogen ions (H+),
usually expressed as
> the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
>
>
> If one wants to call Alk Buffering capacity then one sure as a hell can
call Acidty
> Buffering Capacity also. As it is the ability to neutralizes an acid that
is a buffer.You
> have a pH of 7 and you add a buffer to lower it to a pH of 4, you are
buffering the water,
> that buffer is a acid.
>
> 5) CO2
>
> You are really confuse so it seems :-) You realllllllly indicate that CO2
is affected by
> the Alk or vise-versa
>
> "Yes, the pH will drop with the addition of CO2. Remove CO2 will cause
the
> pH to rise? How do you remove CO2? Once it is in solution it forms
> carbonic acid and neutralizes some of your 'buffer'."
>
> "With the exception of CO2?"
>
> No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
> Concepts)....PERIOD.You seem to think a that at least in two of your post
that CO2 is
> affected by the Alk or vise-versa. Please go back to school or seek
professor
>
> "Why in one case does CO2 from air lower pH and in the other case it
raises
> it? Doesn't make sense."
>
> That is because you don't understand CO2 period. By the way I saved this,
wanted to see
> if you would bite on the post I gave. Not bite at first, so time to reel
you in, as you
> did bite in another post..
>
> Lets make some sense of it for you, being that you have a pH.D in
chemistry, so you say .
>
> CO2 is naturally generated in a aquatic systems, it is capable of raise to
various levels
> depending on a number of circumstances .It can be measure (except in
seawater) or
> calculated using Buch/Park Equations (what we use for seawater. In sort if
you know the pH
> and Alk you can calculate the CO2). If you aerate a system or a sample of
water, even if
> the pH has only dropped a couple of tenths, due to an increase in CO2, the
CO2 will leave
> solution to the atmosphere.This will raise the pH. On the other hand if
theCO2 level is
> more of the norm and you have hikgh room air, such as in the winter, the
partial pressure
> of the CO2 in air will be much higher than that in water, in which case
the CO2 will enter
> the water and lower the pH. That is without an airstone. Adding an
airstone will make it
> even worse,as you are now forcefully driving the CO2 into solution even
quicker. These
> test /experiments have been proven many times, it is not that may work
could work they do
> work.Yet you want to disagree and in another post say you haven't tried
it,.Seems to me
> that based on what you say it can't work So, in short you don't know what
the hell you are
> taking about. Go get a glass of seawater with a pH of about 8.3 and lower
it to about
> 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK- UP
( that is if you
> don't have a high room air CO2 problem.). This little test has been done
thousands of
> times in this hobby, with test kits, pH meters and even graphic printers.
>
> "This is where Boomer and I
> disagree. I say you would have to lower the pH very low in order to
> effectively remove CO2 by purging."
>
> You are 100 % wrong. Please come to our Chem forum and try and run that by
Randy, don't
> take my word on it. I already know what he will say.
>
> "Boomer didnt convince me it
> works at the pH of an aquarium, but I never tried it and I'm not sure of
> this. "
>
> Well then come too our chem. forum and tell Randy he doesn't know what he
is talking about
> LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it
should be easy for
> you to run the experiment LOL There are grade school kids that run the
test and know what
> happens and that I'm correct.
>
>
> "The equilibrium is a FUNCTION
> of pH."
>
> It is also a function of Alk or don't you know that. At a pH of 8.3, Alk
2.25, the CO2 is
> about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk to
about .4 meq/ l
> or so the CO2 will be around .99 mg / l CO2, When dealing with tanksCO2 is
not always in
> equilibrium with ambient air.
>
>
> ". But I wouldn't degas a solution of a
> specific gas (CO2) with a gas (this case he was using air) that contains
the
> same gas I am trying to purge."
>
> Why not ? We have a guy right now that is running tests on purging ambient
air with a
> solution to remove CO2 gas from the air, before it enters the tank
per/Randy's suggestion.
> The same guy is doing some of my test using a Clinoptilolite, a Zeolite
mineral, that has
> an affinity for CO2.This will be a dry CO2 scrubber
>
>
> Sorry Soutman but you sure as hell don't seem to know much about aquatic
chemistry. You
> seem to be guessing at everything.
>
> By the way have you read any of Randy's technical articles on water
chemistry, been saving
> these for last. There are a few on pH, Alk, CO2 .Here is a list
>
> Try and answer them 1-5 and lets see where we get THIS TIME :-) or maybe
we should just
> drop it. I could care less at this point.
>
> THE END
>
>
> ARTICLES
>
> The first two posts in this thread are lists of some of my articles that
relate to reef
> tank chemistry. In the next few posts are some of the articles published
by Craig Bingman
> and others on reef chemistry issues.
>
> The first two posts in this thread are lists of some of my articles that
relate to reef
> tank chemistry. In the next few posts are some of the articles published
by Craig Bingman
> and others on reef chemistry issues.
>
> Solving Common Problems
>
> Solving Calcium and Alkalinity Problems
> http://www.advancedaquarist.com/issues/nov2002/chem.htm
>
> Solutions to pH Problems
> http://www.advancedaquarist.com/iss...ne2002/chem.htm
>
> How to Select a Calcium and Alkalinity Supplementation Scheme
> http://www.advancedaquarist.com/issues/feb2003/chem.htm
>
> Phosphate Issues
> http://www.advancedaquarist.com/iss...pt2002/chem.htm
>
> Nitrate Issues
> http://www.advancedaquarist.com/iss...st2003/chem.htm
>
>
>
> Calcium and Alkalinity
>
> Solving Calcium and Alkalinity Problems
> http://www.advancedaquarist.com/issues/nov2002/chem.htm
>
> How to Select a Calcium and Alkalinity Supplementation Scheme
> http://www.advancedaquarist.com/issues/feb2003/chem.htm
>
> Calcium and Alkalinity Balance Issues
> http://reefkeeping.com/issues/2002-...ature/index.htm
>
> Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
> http://www.advancedaquarist.com/iss...ly2002/chem.htm
>
> The Relationship Between Alkalinity and pH.
> http://www.advancedaquarist.com/issues/may2002/chem.htm
>
> The Chemical & Biochemical Mechanisms of Calcification in Corals
> http://www.advancedaquarist.com/issues/apr2002/chem.htm
>
> Calcium
> http://www.advancedaquarist.com/issues/mar2002/chem.htm
>
> Alkalinity
> http://www.advancedaquarist.com/iss...2/chemistry.htm
>
>
> Iron
>
> First Iron Article: Macroalgae and Dosing Recommendations
> http://www.advancedaquarist.com/issues/aug2002/chem.htm
>
> Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> http://www.advancedaquarist.com/issues/oct2002/chem.htm
>
> Iodine
>
> Iodine in Marine Aquaria: Part I
> http://www.advancedaquarist.com/issues/mar2003/chem.htm
>
> Iodine in Reef Tanks 2: Effects on Macroalgae Growth
> http://www.advancedaquarist.com/iss...il2003/chem.htm
>
>
> Magnesium and Strontium
>
> Strontium
> http://www.advancedaquarist.com/issues/nov2003/chem.htm
>
> Magnesium
> http://www.advancedaquarist.com/issues/oct2003/chem.htm
>
> Magnesium and Strontium in Limewater
> http://www.advancedaquarist.com/issues/dec2003/chem.htm
>
>
> Limewater (kalkwasser)
>
> The Self Purification of Limewater (Kalkwasser)
> http://www.advancedaquarist.com/issues/may2003/chem.htm
>
> The Degradation of Limewater (Kalkwasser) in Air
> http://reefkeeping.com/issues/2003-...ature/index.htm
>
> How to Select a Calcium and Alkalinity Supplementation Scheme
> http://www.advancedaquarist.com/issues/feb2003/chem.htm
>
> Metals in Aquaria
>
> Aluminum and aluminum-based phosphate binders
> http://www.advancedaquarist.com/iss...ly2003/chem.htm
>
> Reef Aquaria with Low Soluble Metals
> http://reefkeeping.com/issues/2003-...ature/index.htm
>
> Tap Water in Reef Aquaria
> http://www.advancedaquarist.com/issues/jan2004/chem.htm
> First Iron Article: Macroalgae and Dosing Recommendations
> http://www.advancedaquarist.com/issues/aug2002/chem.htm
>
> Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> http://www.advancedaquarist.com/issues/oct2002/chem.htm
>
>
> Test Kit Reviews
>
> The Seachem Borate Alkalinity Test Kit
> http://www.advancedaquarist.com/iss...ne2003/chem.htm
>
> The Salifert Boron Test Kit
> http://www.advancedaquarist.com/iss...pt2003/chem.htm
>
> Boron and Borate (and pH buffering)
>
> Boron in a Reef Tank (and its effect on pH buffering)
> http://www.advancedaquarist.com/issues/dec2002/chem.htm
>
> The Seachem Borate Alkalinity Test Kit
> http://www.advancedaquarist.com/iss...ne2003/chem.htm
>
> The Salifert Boron Test Kit
> http://www.advancedaquarist.com/iss...pt2003/chem.htm
>
>
>
> Others
>
> Tap Water in Reef Aquaria
> http://www.advancedaquarist.com/issues/jan2004/chem.htm
>
> ORP
> http://reefkeeping.com/issues/2003-...ature/index.htm
>
> Chloramine
> http://reefkeeping.com/issues/2003-...ature/index.htm
>
> Silica in a Reef Tank
> http://advancedaquarist.com/issues/jan2003/feature.htm
>
> Specific Gravity (and temperature correction of hydrometers)
> http://www.advancedaquarist.com/iss...2/chemistry.htm
>
>
> The Complete Nitrogen Cycle
> http://www.animalnetwork.com/fish/l...a&RecordNo=3090
>
> Magnesium (older article with fonts screwed up)
> http://www.aquariumfish.com/aquariu...cid=124&search=
>
> Phosphate (older article now reproduced in a poor fashion)
> http://www.aquariumfish.com/aquariu...cid=124&search=
>
> Carbon Dioxide
> http://www.animalnetwork.com/fish/l...a&RecordNo=2074
>
> Using Conductivity to Measure Salinity
> http://www.aquariumfish.com/aquariu...cid=124&search=
>
> Understanding Seawater
> http://www.animalnetwork.com/fish2/...s/1/default.asp
>
> Protein Skimming: How It Works
> http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
>
>
>
> Articles by Craig Bingman:
>
> Carbon Dioxide tests
> http://www.animalnetwork.com/fish/l...n=&RecordNo=279
>
> Limewater, Acetic Acid and Sand Clumping
> http://www.animalnetwork.com/fish/l...n=&RecordNo=181
>
> Calcium and Alkalinity
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Calculation of Calcium Carbonate Saturation States in Reef Aquaria
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
>
> Calcification Rates in Several Tropical Coral Reef Aquaria
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Limits To Limewater...Revisited
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Expanding the Limits of Limewater: Adding Organic Carbon Sources (vinegar)
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
>
> Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Magnesium - Part I
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Magnesium - Part II
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> A Homemade Magnesium Supplement
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Simulating the Effect of Calcium Chloride and Sodium Bicarbonate Additions
on Reef Systems
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Additional Simulations: The Combined Effect Of Calcium Chloride
> /Sodium Bicarbonate Additions And Water Exchanges
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
>
> More articles by Craig Bingman:
>
> The Halogens - Part I: Bromine in Seawater and Aquaria
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> The Halogens - Part II: Fluoride
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Fluoride Depletion In Four Reef Aquariums
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> The Halogens - Part III: Iodine
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Measuring Halides
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> How Test Kits Work
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Borax pH Calibration
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> A pH Detective Story
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> How to Mix a Batch of Synthetic Seawater in Under Five Minutes
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> SILICON - FOE OR FRIEND?
> http://www.animalnetwork.com/fish2/...s/1/default.asp
>
> The Composition Of Several Synthetic Seawater Mixes
> http://www.animalnetwork.com/fish2/...s/1/default.asp
>
> Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
>
>
> Andy's calcium calculator
> http://www.andy-hipkiss.co.uk/cacalc.htm
>
> Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
> http://www.aquariumfish.com/aquariu...cid=124&search=
>
> Calcium Reactor Substrate -- Phosphate Levels
> by Greg Hiller
> http://www.advancedaquarist.com/iss...l2003/short.htm
>
>
> Indoor CO2 Problems
> http://www.advancedaquarist.com/iss...r2002/short.htm
>
> Simon Huntington's CaCO3/CO2 reactor article
>
> http://reefkeeping.com/issues/2002-...ature/index.htm
>
> Ron Shimek's Tank Water Analysis Article
> http://reefkeeping.com/issues/2002-...ature/index.htm
>
>
>
>
> Home made salinity standards thread:
>
> http://reefcentral.com/forums/showt...?threadid=65509
>
> Reef Chemicals Calculator
> http://www.kademani.com/reefchem.htm
>
>
>
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
>
> Former US Army Bomb Technician (EOD)
> Member; IABTI, NATEODA, WEODF, ISEE & IPS
>
> If You See Me Running You Better Catch-Up
>
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message
news:aGuWb.148227$U%5.676753@attbi_s03...
> : Boomer,
> :
> : I am not sure if you are just messing with me or if you are truly
confused.
> : I hope the latter. Please read from Top to Bottom.
> :
> :
> : From YOUR first link:
> :
> : http://www.waterontheweb.org/resources/glossary.html
> :
> : Acidity:
> : A measure of how acid a solution may be. A solution with a pH of less
than
> : 7.0 is considered acidic. Solutions with a pH of less than 4.5 contain
> : mineral acidity (due to strong inorganic acids), while a solution having
a
> : pH greater than 8.3 contains no acidity.
> :
> : Yes,
> :
> : Good definition (for the most part). pH <7 is indeed acidic. pH > 7 is
> : basic. Your web page had a definition for acidity, but not basicity.
> : Strange. That's like defining GOOD and not defining BAD.
> :
> : Here is the IUPAC (International Union of Pure and Applied Chemistry)
> : definition of acidity:
> :
> : http://www.chem.qmul.ac.uk/iupac/index.html
> :
> : acidity
> :
> : (1) Of a compound:
> :
> : For Brønsted acids it means the tendency of a compound to act as a
hydron
> : donor. It can be quantitatively expressed by the acid dissociation
constant
> : of the compound in water or some other specified medium. For Lewis acids
it
> : relates to the association constants of Lewis adducts and -adducts.
> :
> : (2) Of a medium:
> :
> : The use of the term is mainly restricted to a medium containing Brønsted
> : acids, where it means the tendency of the medium to hydronate a specific
> : reference base
> :
> : basicity
> :
> : For Brønsted bases it means the tendency of a compound to act as hydron
> : (proton) acceptor. The basicity of a chemical species is normally
expressed
> : by the acidity of the conjugate acid (see conjugate acid-base pair). For
> : Lewis bases it relates to the association constants of Lewis adducts
> : and -adducts
> :
> :
> :
> : Another definition from the same web page YOU cited: (this is the same
web
> : page you cited above)
> :
> : Alkalinity:
> : Acid neutralizing or buffering capacity of water; a measure of the
ability
> : of water to resist changes in pH caused by the addition of acids or
bases
> : and therefore, the main indicator of susceptibility to acid rain; in
natural
> : waters it is due primarily to the presence of bicarbonates, carbonates
and
> : to a much lesser extent occasionally borates, silicates and phosphates.
It
> : is expressed in units of milligrams per liter (mg/l) of CaCO3 (calcium
> : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l = 1
mg/l
> : of CaCO3. A solution having a pH below about 5 contains no alkalinity.
> :
> : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and says
> : that alkalinity is the measure of ...(description of a buffer)
> :
> : A BUFFER IS : a measure of the ability of water to resist changes in pH
> : caused by the addition of acids or bases (from definition below)
> :
> :
> : I said:
> : ***alkalinity is a measurement of 'buffering capacity'***
> :
> : You said:
> : ***Alkalinity is not a measurement of BC
> :
> : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is not
> : logical.
> :
> : (THIS FROM THE SAME WEB PAGE YOU CITED):
> :
> : Buffer:
> : A substance which tends to keep pH levels fairly constant when acids or
> : bases are added.
> :
> : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
> :
> : a measure of the ability of water to resist changes in pH caused by the
> : addition of acids or bases
> :
> : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A BUFFER.
> :
> :
> : I went to all four links. None contradict what I have said. But the
first
> : one you cited contradicts YOU!
> :
> : I know what a buffer is. I know what acidity means. I know what
alkalinity
> : means. No need to cite web pages that describe what I know and what I
wrote
> : in this discussion. Show me one that says alkalinity is not a measure
of
> : buffering capacity from a credible source.
> :
> :
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > Alkalinity a measure of the amount of anions of weak acid in water and
of
> : the cations
> : > balanced against them
> : > Take note it says ***acid***
> : >
> : > Buffering capacity the ability of a solution to resist or dampen
changes
> : in pH upon the
> : > addition of acids or bases.
> : > Take note its says ***the addition of acids or bases***
> : >
> : > One more
> : >
> : > http://www.waterontheweb.org/resources/glossary.html
> : >
> : > We could go on like this all day, so what is the point ?
> : >
> : > You will LOVE this one
> : > http://www.kyantec.com/Tips/phbuffering.htm
> : >
> : > Don't you just lovbe PDF's
> : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
> : >
> : > Don't fall out of your chair
> : > http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
> : >
> : >
> : >
> : >
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : > "stoutman" <.@.> wrote in message
news:XB7Wb.19339$QA2.62332@attbi_s52...
> : > : Man here is another, google is a wonderful thing. I'm not filtering
any
> : > : out, just posting what I find by GOOGLING for you.
> : > :
> : > : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> : > :
> : > :
> : > : Wow, a gov link. Even the government is wrong, this must be a
> : conspiracy
> : > : against Boomer.
> : > :
> : > :
> : > :
> : > :
> : > : "Boomer" > wrote in message
> : > : ...
> : > : > Now I am getting bored
> : > : >
> : > : > "Don't the components of a buffer account for the buffering
capacity?
> : > : Yes."
> : > : >
> : > : > Yes, agreed but you seem to fail what I'm saying. Buffering
Capacity
> : and
> : > : Alkalinity are
> : > : > not the same, that has always been the issue. I gave the equation
does
> : > : that look like an
> : > : > Alkalinity equation or how Alk is determined. I see you had now
> : comments
> : > : on it what's
> : > : > wrong, why no comments on the equations I gave. Don't understand
them
> : or
> : > : what ? Again this
> : > : > is the equation for Buffering Capacity, also called Buffer Index
or
> : Buffer
> : > : Intensity. It
> : > : > is defined in most water chemistry and chemical oceanography text
> : books.
> : > : >
> : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] +
> : CKa
> : > : [H3O+] / (Ka =
> : > : > H3O+])² )
> : > : >
> : > : > This is not Alkalinity now is it ?
> : > : >
> : > : > "I know how to do a titration, In fact I have done several. How
many
> : have
> : > : > you actually done? I don't mean by counting drops, I mean with a
> : buret?"
> : > : >
> : > : > Well good for you, I use a Digital Titrator
> : > : >
> : > : > "Oh, I see,
> : > : > you think acidity is the opposite of alkalinity. In the world of
> : > : CHEMISTRY
> : > : > it's not. Maybe in aquarium newsgroups it is.
> : > : >
> : > : > Hum no, maybe you should go for a look at HACH's or LaMotte
website or
> : the
> : > : book I
> : > : > suggested earlier. Please view a copy.
> : > : >
> : > : > Standard Methods for the Examination of Water and Wastewater
> : > : >
> : > : > This book, over 2000 pages, is the guide for water testing. If you
are
> : > : reporting water
> : > : > test to the EPA you must use approved std from this text.I t is
> : prepared
> : > : and published by
> : > : > the EPA, American Water Works Association and American Public
Health
> : > : Association. You
> : > : > mean you don't have one and the issue is water chemistry
> : > : >
> : > : > You are confusing Acidity and Acidity as you know little about
water
> : > : chemistry and
> : > : > procedures and test methods
> : > : >
> : > : > From SMEWW, section 2-30, 2310 ACIDITY
> : > : >
> : > : > "Acidity of water is its quantative capacity to react with a
strong
> : base
> : > : to a designated
> : > : > pH"
> : > : >
> : > : > This is how you test for it
> : > : >
> : > : > A std alkali titration to methyl orange or phenolphthalein
> : > : > endpoint.
> : > : >
> : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that
write
> : this
> : > : book, there are
> : > : > over 100 of them, they are wrong.
> : > : >
> : > : > Like Buffering Capacity you have your Acidity's mixed up
> : > : > In water measurement if you have a high Alk you also usually have
a
> : high
> : > : Acidity.
> : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
> : CHEMISTRY
> : > : BOOK there pal.
> : > : >
> : > : >
> : > : > "These are all in equilibrium with each other. An initial high pH
> : (above
> : > : > 6.4) will shift the equilibrium to the right to form HCO3-1. If
the
> : pH of
> : > : > the solution is above 10.3 (pKa2) the .........."
> : > : >
> : > : >
> : > : > Christ, there you go again with the FW ****. All your numbers are
> : wrong we
> : > : are dealing
> : > : > with SEAWATER
> : > : >
> : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is in
the
> : form
> : > : > of HCO3-1 .
> : > : >
> : > : > I have already pointed that out and gave actual values at know
> : seawater
> : > : levels, go back
> : > : > and re-read it you aren't telling me anything here.Of course most
is
> : HCO3
> : > : see...
> : > : >
> : > : >
> : > : > @ 20C and 34.3 ppt salinity
> : > : >
> : > : > CO2 = 0.52 %
> : > : >
> : > : > HCO3 = 86.4 %
> : > : >
> : > : > CO3 = 13.09 %
> : > : >
> : > : >
> : > : > "In your glass experiment you managed to lower the pH enough to
purge
> : out
> : > : CO2
> : > : > by boiling"
> : > : >
> : > : > The purpose behind the glass is to show that alk is not affect by
CO2
> : and
> : > : vise-versa and
> : > : > how Co2 affects pH.
> : > : >
> : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and that
pH
> : drops
> : > : to say 8.1 it is
> : > : > usually due to excess CO2. If you took a glass of that water and
> : aerated
> : > : it you WILL drive
> : > : > off the CO2 and raise the pH. It has been done a proven a million
> : times.
> : > : >
> : > : > "In order to 'purge' CO2 you would need to lower the
> : > : > pH to shift the equilibrium to below 6.4"
> : > : >
> : > : > The hell you do !!!.Do you know who many times people on this NG
to
> : > : include Dr. Craig
> : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to
take a
> : > : sample of aquarium
> : > : > water and aerate it to see if the pH GOES UP AND when they come
back
> : with
> : > : the test it is
> : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST
> : excess
> : > : CO2 in the tank
> : > : > water, increase the circulation for better gas exchange at the
> : surface,
> : > : reduce feeding,
> : > : > and try to improve on better skimming, thus reducing the bio-load
and
> : pH
> : > : decline due to
> : > : > CO2.
> : > : >
> : > : >
> : > : > "I hope this helps. "
> : > : >
> : > : > Help, how can you when you miss everything. I should be charging
you
> : > : >
> : > : > Oh, by the way. Your websites, I have about 50 on these issues, I
> : could
> : > : post them, not to
> : > : > mention I have all those water chemistry books, so there is no
need to
> : > : view your sites.
> : > : >
> : > : > Finally are you afraid to come to our Chemistry Forum, afraid to
get
> : > : slapped by REAL
> : > : > chemists. I get a charge out of you can't post your ref .I have
posted
> : the
> : > : same or similar
> : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500
> : posts
> : > : there and am the
> : > : > biggest contributor to his forum other than himself or maybe Habib
> : Sheka
> : > : >
> : > : > Hum, here are Randy's ref that he posted. He hosts the website
> : > : >
> : > : > S. RANDY HOLMES-FARLEY
> : > : > Arlington, Massachusetts
> : > : >
> : > : > EDUCATION
> : > : >
> : > : > 1982-1986 Harvard University Cambridge, MA
> : > : > PhD in Chemistry
> : > : > Research Advisor: George Whitesides
> : > : >
> : > : > Investigated the relationship between polymer surface chemistry
and
> : > : physical properties
> : > : > through controlled surface modification and testing.
> : > : >
> : > : > 1980-1982 Cornell University Ithaca, NY
> : > : > BA in Chemistry and Biology
> : > : > Graduated Summa Cum Laude
> : > : > Distinction in All Subjects
> : > : > Grade Point: 3.94/4.0
> : > : > Honors research: isolation and characterization of the subunit of
CF1
> : > : enzyme
> : > : >
> : > : >
> : > : > 1978-1979 Stanford University Palo Alto, CA
> : > : > Grade Point: 3.55/4.0
> : > : >
> : > : >
> : > : > EXPERIENCE
> : > : >
> : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> : > : > (bought out GelTex Pharmaceuticals in 2001)
> : > : > Vice President, Chemical Research 2001-present
> : > : > Senior Director, Chemical Research 1999-2001
> : > : > Director of Chemical Research 1997-1999
> : > : > Manager of Chemical Research 1995-1997
> : > : > Group Leader 1994-1995
> : > : > Senior Research Scientist 1992-1994
> : > : >
> : > : > Helped start GelTex as second employee
> : > : >
> : > : > Managed various research programs with multi-million dollar
budgets
> : > : >
> : > : > Supervised research chemists (17+)
> : > : >
> : > : > Co-inventor of several polymeric pharmaceuticals and
pharmaceutical
> : > : candidates including
> : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam
Hydrochloride
> : (FDA
> : > : approved)
> : > : >
> : > : > Company Safety Officer for 3 years
> : > : >
> : > : > Chemical Hygiene Officer 2000-present
> : > : >
> : > : >
> : > : >
> : > : >
> : > : > 1990-1992 GTE Corporation Waltham, MA
> : > : > Senior Member of Technical Staff
> : > : > Applied research involving polymer interfaces
> : > : > Metallization of plastics
> : > : > Polymer/polymer adhesion
> : > : > Optical coatings
> : > : >
> : > : >
> : > : >
> : > : > 1986-1990 Lord Corporation Cary, NC
> : > : > Senior Research Scientist 1988-1990
> : > : > Research Scientist 1986-1988
> : > : > Basic and applied research on surface chemical bonding
> : > : > Developed new adhesive compositions
> : > : > Developed new sol-gel coatings for corrosion resistance
> : > : >
> : > : >
> : > : > HONORS AND AWARDS
> : > : >
> : > : > Industrial Innovations Award by Northeast Region of American
Chemical
> : > : Society (6/2001)
> : > : >
> : > : > National Kidney Foundation of Northern California Honoree (5/2001)
> : > : >
> : > : > American Chemical Society/Polymer Chemistry Division Industrial
> : Sponsors
> : > : > Award (8/2000)
> : > : >
> : > : > R&D 100 Award from R&D magazine (1999)
> : > : >
> : > : > Sherwin Williams Award in applied polymer science (9/85)
> : > : >
> : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985;
1985-1986)
> : > : >
> : > : > Award for highest GPA in Chemistry Department (6/82)
> : > : >
> : > : > Summa Cum Laude Honors in Chemistry (6/82)
> : > : >
> : > : > Phi Lamda Epsilon (6/82)
> : > : >
> : > : > Phi Beta Kappa (2/82)
> : > : >
> : > : > Cornell University Dean's List (1981, 1982)
> : > : >
> : > : > Harvard Book Club Award for highest GPA senior year (1978)
> : > : >
> : > : > First Place in western NY ACS high school chemistry exam (1977)
> : > : >
> : > : > 1978-1979
> : > : >
> : > : >
> : > : > __________________
> : > : > Randy Holmes-Farley
> : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef
Central
> : > : >
> : > : > Hobby Experience: 8 years with reefs
> : > : > Current Tanks: 90 gal mixed reef
> : > : > Interests: Reefkeeping, science, photography
> : > : >
> : > : >
> : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> : > : >
> : > : > Open this post in a new window | Report this post to a moderator |
IP:
> : > : Logged
> : > : >
> : > : >
> : > : >
> : > : > 06/27/2003 02:44 PM
> : > : >
> : > : > Randy Holmes-Farley
> : > : > Chemistry Moderator
> : > : >
> : > : > Registered: Apr 2001
> : > : > Location: Arlington, Massachusetts
> : > : > Occupation: Chemist (Drug Discovery at Genzyme)
> : > : > Posts: 15282
> : > : >
> : > : >
> : > : >
> : > : > Publications
> : > : >
> : > : >
> : > : > ISSUED UNITED STATES PATENTS
> : > : >
> : > : >
> : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
> : > : Mandeville, III; W. Harry.
> : > : > US 6,566,407; 5/20/2003
> : > : >
> : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen
> : Randall;
> : > : Huval, Chad
> : > : > Cori.
> : > : > U.S. 6,517,825; 2/11/2003.
> : > : >
> : > : > 3. Method of making phosphate-binding polymers for oral
> : administration.
> : > : Holmes-Farley,
> : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
> : > : 6,509,013; 1/21/2003.
> : > : >
> : > : > 4. Combination therapy for treating hypercholesterolemia using a
bile
> : acid
> : > : sequestrant
> : > : > polymer
> : > : > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley,
> : Stephen
> : > : Randall;
> : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> : > : >
> : > : > 5. Method for treating hypercholesterolemia with polyallylamine
> : polymers.
> : > : Holmes-Farley,
> : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
> : Goldberg,
> : > : Dennis I. , US
> : > : > 6,423,754; 7/23/2002.
> : > : >
> : > : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry,
III;
> : > : Neenan, Thomas X..;
> : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> : > : >
> : > : > 7. Combination therapy for treating hypercholesterolemia and
> : > : atherosclerosis. Huval, Chad
> : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal,
Pradeep
> : K.
> : > : U.S. 6,365,186;
> : > : > 4/2/2002.
> : > : >
> : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
> : Mandeville,
> : > : W. H., III;
> : > : > Huval; C.
> : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
> : > : 10/9/2001.
> : > : >
> : > : > 9. Polymers containing guanidinium groups as bile acid
sequestrants.
> : Dhal;
> : > : P. K.; Holmes-
> : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> : > : >
> : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville,
W.
> : H.,
> : > : III.; US
> : > : > 6,281,252;
> : > : > 8/28/2001.
> : > : >
> : > : > 11. Combination therapy for treating hypercholestrolemia. Huval;
C.
> : C.;
> : > : Holmes-Farley; S.
> : > : > R. ;
> : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> : > : >
> : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G.
M.;
> : > : Holmes-Farley, S.
> : > : > R.; US
> : > : > 6,264,937; 7/24/2001.
> : > : >
> : > : > 13. Method for treating hypercholesterolemia with unsubstituted
> : > : polydiallylamine polymers.
> : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K.
; US
> : > : 6,248,318;
> : > : > 6/19/2001.
> : > : >
> : > : > 14. Process for removing bile salts from a patient and alkylated
> : > : compositions therefore.
> : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355;
5/1/2001.
> : > : >
> : > : > 15. Poly(diallylamine)-based bile acid sequestrants.
Holmes-Farley, S.
> : R.;
> : > : Dhal, P. K.;
> : > : > Petersen,
> : > : > J. S.; US 6,203,785; 3/20/2001.
> : > : >
> : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.;
> : Huval,
> : > : C. C.; US
> : > : > 6,190,649;
> : > : > 2/20/2001.
> : > : >
> : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville,
W.
> : H.,
> : > : III.; US
> : > : > 6,177,478;
> : > : > 1/23/2001.
> : > : >
> : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
> : Holmes-Farley,
> : > : S. R.;
> : > : > Mandeville, W.
> : > : > H., III.; US 6,129,910; 10/10/2000.
> : > : >
> : > : > 19. Method for treating hypercholesterolemia with unsubstituted
> : > : polydiallylamine polymers.
> : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K.
; US
> : > : 6,083,497;
> : > : > 7/4/2000.
> : > : >
> : > : > 20. Method of making phosphate-binding polymers for oral
> : administration.
> : > : Holmes-Farley, S.
> : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495;
> : 7/4/2000.
> : > : >
> : > : > 21. Process for removing bile salts from a patient and alkylated
> : > : compositions therefore.
> : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
> : 5/23/2000.
> : > : >
> : > : > 22. Process for removing bile salts from a patient and
compositions
> : > : therefor. Mandeville,
> : > : > W. H.,
> : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> : > : >
> : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W.
H;
> : > : Neenan; T. X.; Holmes-
> : > : > Farley; S. R. US 6,034,129; 3/7/2000.
> : > : >
> : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville,
W.
> : H.,
> : > : III.; US
> : > : > 5,985,938;
> : > : > 11/16/99.
> : > : >
> : > : > 25. Process for removing bile salts from a patient and
compositions
> : > : therefor. Mandeville,
> : > : > W. H.,
> : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> : > : >
> : > : > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville,
W.
> : H.,
> : > : III.;
> : > : > Holmes-Farley;
> : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> : > : >
> : > : > 27. Hydrophilic nonamine-containing and amine-containing
copolymers
> : and
> : > : their use as bile
> : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
> : 5,929,184;
> : > : 7/27/99.
> : > : >
> : > : > 28. Interpenetrating polymer networks for sequestration of bile
acids.
> : > : Mandeville, W. H.,
> : > : > III.;
> : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US
5,925,379;
> : > : 7/20/99.
> : > : >
> : > : > 29. Amine polymer sequestrant and method of cholesterol depletion.
> : > : Mandeville, W. H.,
> : > : > III.;
> : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> : > : >
> : > : > 30. Process for removing bile salts from a patient and
compositions
> : > : therefor. Mandeville,
> : > : > W. H.,
> : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> : > : >
> : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
depletion.
> : > : Mandeville, W. H.,
> : > : > III.;
> : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> : > : >
> : > : > 32. Process for removing bile salts from a patient and
compositions
> : > : therefor. Mandeville,
> : > : > W. H.,
> : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> : > : >
> : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
> : Mandeville,
> : > : W. H., III.;
> : > : > Holmes-
> : > : > Farley, S. R.; US 5,703,188; 12/30/97.
> : > : >
> : > : > 34. Oral administration of iron-binding crosslinked amine
polymers.
> : > : Mandeville, W. H.,
> : > : > III.;
> : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> : > : >
> : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
Holmes-Farley,
> : S.
> : > : R.; US 5,693,675;
> : > : > 12/2/97.
> : > : >
> : > : > 36. Method for removing bile salts from a patient with alkylated
> : > : crosslinked amine
> : > : > polymers,
> : > : > and preparation of the polymers. Mandeville, W. H., III.;
> : Holmes-Farley,
> : > : S. R.; US
> : > : > 5,679,717; 10/21/97.
> : > : >
> : > : > 37. Phosphate-binding polymers for oral administration.
Holmes-Farley,
> : S.
> : > : R.; Mandeville,
> : > : > W.
> : > : > H., III.; US 5,667,775; 9/16/97.
> : > : >
> : > : > 38. Ion-exchange process using highly crosslinked polymers for
> : removing
> : > : bile salts from a
> : > : > patient, preparation of the polymers, and compositions containing
> : them.
> : > : Mandeville, W. H.,
> : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> : > : >
> : > : > 39. Hydrophobic amine polymer sequestrant and method of
cholesterol
> : > : depletion. Mandeville,
> : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530;
> : 4/8/97.
> : > : >
> : > : > 40. Amine polymer sequestrant and method of cholesterol depletion.
> : > : Mandeville, W. H.,
> : > : > III.;
> : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> : > : >
> : > : > 41. Phosphate-binding polymers for oral administration.
Holmes-Farley,
> : S.
> : > : R.; Mandeville,
> : > : > W.
> : > : > H., III.; US 5,496,545; 3/5/96.
> : > : >
> : > : > 42. Iron-binding polymers for oral administration. Mandeville, W.
H.,
> : > : III.; Holmes-Farley,
> : > : > S. R.;
> : > : > US 5,487,888; 1/30/96.
> : > : >
> : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having
active
> : > : hydrogens on the
> : > : > surface.
> : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> : > : >
> : > : > 44. Layered sol-gel coatings from organisilicon compounds.
> : Holmes-Farley,
> : > : S. R.; Yanyo, L.
> : > : > C.;
> : > : > US 5,182,143; 1/26/93.
> : > : >
> : > : > 45. Method for metal bonding using ultrathin primer coating.
> : > : Holmes-Farley, S. R.; Yanyo,
> : > : > L.
> : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> : > : >
> : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K.
J.;
> : US
> : > : 5,096,962;
> : > : > 3/17/92.
> : > : >
> : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> : > : elastomer-metal bonding.
> : > : > Holmes-
> : > : > Farley, S. R.; US 5,102,956; 4/7/92.
> : > : >
> : > : >
> : > : >
> : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
> : > : >
> : > : >
> : > : > 1. Aryl boronate functionalized polymers for treating obesity and
> : > : inhibiting fat uptake.
> : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal,
> : Pradeep
> : > : K.; Huval, Chad
> : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003),
92
> : pp. WO
> : > : 0302571.
> : > : >
> : > : > 2. Preparation of aryl boronic acids for treating obesity.
> : Holmes-Farley,
> : > : Stephen Randall;
> : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal,
Pradeep
> : K.
> : > : (Geltex
> : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO
0302570.
> : > : >
> : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide.
Holmes-Farley,
> : > : Stephen Randall.
> : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp.
WO
> : > : 0302130.
> : > : >
> : > : > 4. Method for reducing copper levels and treating copper
toxicosis.
> : > : Holmes-Farley, Stephen
> : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl.
(2002),
> : 45
> : > : pp. WO
> : > : > 0285383.
> : > : >
> : > : > 5. Method for treating gout and binding uric acid. Holmes-Farley,
> : Stephen
> : > : Randall; Burke,
> : > : > Steven K. WO 0285381 10/31/2002.
> : > : >
> : > : > 6. Method for treating gout and reducing serum uric acid.
> : Holmes-Farley,
> : > : Stephen Randall;
> : > : > Burke, Steven K WO 0285380 10/31/2002.
> : > : >
> : > : > 7. Amine condensation polymer bile acid sequestrants. Huval, C.
C.;
> : > : Holmes-Farley, S. R.;
> : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> : > : >
> : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III
and
> : > : Holmes-Farley, S.
> : > : > R.;
> : > : > WO 1999-US5662; 9/23/1999.
> : > : >
> : > : > 9. Amine-containing copolymers as bile acid sequestrants.
> : Holmes-Farley,
> : > : S. R.; Petersen,
> : > : > J. S.;
> : > : > WO 9933452; 7/8/1999.
> : > : >
> : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H.,
III
> : and
> : > : Holmes-Farley, S.
> : > : > R.;
> : > : > WO 9922743; 5/14/1999.
> : > : >
> : > : > 11. Polyallylamine polymers for removing bile salts and treating
> : > : hypercholesterolemia, and
> : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III;
> : Burke,
> : > : S. K.; Goldberg,
> : > : > D. I.; WO 9857652; 12/23/98.
> : > : >
> : > : > 12. Phosphate-bidning polymers combined with a calcium supplement
for
> : oral
> : > : administration.
> : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
Holmes-Farley,
> : S.
> : > : R.; WO 9842355;
> : > : > 10/1/98.
> : > : >
> : > : > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
> : > : depletion. Mandeville,
> : > : > W.
> : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449;
12/12/96.
> : > : >
> : > : > 14. Process for adjusting ion concentration in a patient and
> : compositions
> : > : therefor.
> : > : > Mandeville,
> : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> : > : >
> : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
> : interlayer
> : > : for improved
> : > : > metal-
> : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
> : 1/20/94.
> : > : >
> : > : > 16. Process for increased metal-substrate bond strength in
metalized
> : > : plastics.
> : > : > Holmes-Farley, S.
> : > : > R.; Ger. Offen. 4322516; 7/6/93.
> : > : >
> : > : > 17. Electrorheological fluids and preparation of particles useful
in
> : the
> : > : fluids.
> : > : > Troughton,
> : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson,
J.
> : > : David; Bares, Joseph
> : > : > E.;
> : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell.
EP
> : > : 394049;
> : > : > 10/24/1990.
> : > : >
> : > : > JOURNAL PUBLICATIONS
> : > : >
> : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov,
> : Eugene;
> : > : Guo, Amy;
> : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
> : > : Mandeville, W. Harry;
> : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
> : 611-619.
> : > : >
> : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
> : synthesis
> : > : and biological
> : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S.
> : Randall;
> : > : Mandeville, W.
> : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep
K.
> : > : Journal of
> : > : > Macromolecular Science, Pure and Applied Chemistry (2001),
A38(12),
> : > : 1559-1574.
> : > : >
> : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by
Molecular
> : > : Imprinting. Huval,
> : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley,
S.
> : > : Randall; Mandeville,
> : > : > W.
> : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro,
Robert
> : J.;
> : > : Chen, Xi; Dhal,
> : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> : > : >
> : > : > 4. Synthetic polymers for the binding of fat in the intestinal
tract.
> : > : Jozefiak, Thomas H.;
> : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia;
> : Huval,
> : > : Chad C.;
> : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
> : > : Abstracts of
> : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United States,
August
> : > : 26-30, 2001
> : > : > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
> : > : Division of
> : > : > Polymer Chemistry) (2001), 42(2), 98.
> : > : >
> : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel
polymer
> : gel
> : > : pharmaceutical.
> : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen,
J.;
> : Ward,
> : > : J.; Sacchiero,
> : > : > B.;
> : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K.
A.;
> : Chen,
> : > : X.; Mazzeo, J.
> : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
> : > : >
> : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl and
> : other
> : > : bile acid
> : > : > sequestrants.
> : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu,
Q.;
> : > : Hook, P.; Holmes-
> : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1),
708-709.
> : > : >
> : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
> : Holmes-Farley,
> : > : S. R; Polym.
> : > : > Mater. Sci. Eng (1999), 80, 246-247.
> : > : >
> : > : > 8. Design and characterization of of Sevelamer Hydrochloride: a
novel
> : > : phosphate-binding
> : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III;
Ward,
> : J.;
> : > : Miller, K. L.;
> : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.-
Pure
> : and
> : > : Appl. Chem.,
> : > : > A36(7&8), p. 1085 (1999).
> : > : >
> : > : > 9. Three generations of bile acid sequestrants. Mandeville, W. H.,
> : III;
> : > : Braunlin, W.;
> : > : > Dhal, P.;
> : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
> : > : Rosenbaum, D.;
> : > : > Sacchiero,
> : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc.
(1999),
> : > : 550, 3-15.
> : > : >
> : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric
> : phosphate
> : > : binder, on
> : > : > urinary
> : > : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S.
R.;
> : > : Mandeville, W. H.,
> : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
Transplant.
> : > : (1997), 12(5)
> : > : > 961-964.
> : > : >
> : > : > 11. Thin anisotropic coatings based on sol-gel technology.
> : Holmes-Farley,
> : > : S. R.; Yanyo, L.
> : > : > C;
> : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4),
> : 439-444.
> : > : >
> : > : > 12. The mechanism of cure initiation of a surface activated
adhesive.
> : > : Holmes-Farley, S.
> : > : > R.;
> : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
> : > : >
> : > : > 13. Adhesion promotion and corrosion prevention using thin
anisotropic
> : > : coatings. Holmes-
> : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
> : > : 131-151.
> : > : >
> : > : > 14. Wetting of functionalized polyethylene having ionizable
organic
> : acids
> : > : and bases at the
> : > : > polymer-water interface: relations between functional group
polarity,
> : > : extent of
> : > : > ionization,
> : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
> : > : Whitesides, G. M.;
> : > : > Langmuir
> : > : > (1988), 4(4), 921-937.
> : > : >
> : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with
a
> : > : single hydroxy group.
> : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> : > : >
> : > : > 16. Reconstruction of the interface of oxidatively functionalized
> : > : polyethylene (PE-CO2H)
> : > : > and
> : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.;
Nuzzo,
> : R.;
> : > : McCarthy, T. J.;
> : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report
> : (1987),
> : > : AD-
> : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> : > : >
> : > : > 17. Surface-modified polyethylene film: the relationship between
> : surface
> : > : chemistry and
> : > : > physical
> : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11),
> : 4537.
> : > : >
> : > : > 18. Reactivity of carboxylic acid and ester groups in the
> : functionalized
> : > : interfacial
> : > : > region of
> : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> : > : differentiation of the
> : > : > functional groups into shallow and deep subsets based on a
comparison
> : of
> : > : contact angle and
> : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.;
Langmuir
> : > : (1987), 3(1), 62-
> : > : > 76.
> : > : >
> : > : > 19. Fluorescence properties of dansyl groups covalently bonded tot
he
> : > : surface of
> : > : > oxidatively
> : > : > functionalized low-density polyethylene film. Holmes-Farley, S.
R.;
> : > : Whitesides, G. M.;
> : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
> : > : AD-A162435/2/GAR,
> : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> : > : >
> : > : > 20. Acid-base behavior of carboxylic acid groups covalently
attached
> : at
> : > : the surface of
> : > : > polyethylene: The usefulness of contact angle in following the
> : ionization
> : > : of surface
> : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T.
J.;
> : > : Deutch, J.;
> : > : > Whitesides,
> : > : > G. M.; Langmuir (1985), 1(6), 725-740.
> : > : >
> : > : > 21. The thermal stability of a surface modified solid organic
polymer.
> : > : Holmes-Farley, S.
> : > : > R.;
> : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
> : > : >
> : > : >
> : > : >
> : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> : > : >
> : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R.
Advanced
> : > : Aquarist. June 2003.
> : > : >
> : > : > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley,
R.
> : > : Advanced Aquarist.
> : > : > May
> : > : > 2003.
> : > : >
> : > : > 3. The Degradation of Limewater (Kalkwasser) in Air.
Holmes-Farley, R.
> : > : Reefkeeping May
> : > : > 2003.
> : > : >
> : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
Reefkeeping
> : > : April 2003.
> : > : >
> : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> : > : Holmes-Farley, R.
> : > : > Advanced Aquarist; April 2003.
> : > : >
> : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> : > : Holmes-Farley, R.
> : > : > Advanced Aquarist; April 2003.
> : > : >
> : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced
> : Aquarist;
> : > : March 2003.
> : > : >
> : > : > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
> : > : Holmes-Farley, R.
> : > : > Advanced Aquarist; February 2003.
> : > : >
> : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
January
> : > : 2003.
> : > : >
> : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> : December
> : > : 2002.
> : > : >
> : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
> : Advanced
> : > : Aquarist; November
> : > : > 2002.
> : > : >
> : > : > 12. Iron: A Look at Organisms Other than Macroalgae.
Holmes-Farley, R.
> : > : Advanced Aquarist;
> : > : > November 2002.
> : > : >
> : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced
> : Aquarist,
> : > : September 2002.
> : > : >
> : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist,
August
> : > : 2002.
> : > : >
> : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com,
April
> : > : 2002.
> : > : >
> : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
> : > : Aquarist; July 2002
> : > : >
> : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist;
> : June
> : > : 2002.
> : > : >
> : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R.
> : Advanced
> : > : Aquarist, May
> : > : > 2002.
> : > : >
> : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in
Corals.
> : > : Holmes-Farley, R.
> : > : > Advanced Aquarist, April 2002.
> : > : >
> : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> : > : >
> : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February
2002.
> : > : >
> : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January
> : 2002.
> : > : >
> : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium
Frontiers
> : > : 2000.
> : > : >
> : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
> : > : Frontiers 2000.
> : > : >
> : > : > 25. Phosphate..What is it and why should you care. Holmes-Farley,
R.
> : > : Aquarium Frontiers
> : > : > 2000.
> : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
> : Frontiers
> : > : 2000.
> : > : >
> : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers
> : 2000.
> : > : >
> : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers
1999.
> : > : >
> : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> : > : >
> : > : >
> : > : >
> : > : >
> : > : >
> : > : >
> : > : >
> : > : > Boomer
> : > : >
> : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : >
> : > : > Want to See More ?
> : > : > Please Join Our Growing Membership
> : > : > www.coralrealm.com
> : > : >
> : > : >
> : > : >
> : > :
> : > :
> : >
> : >
> :
> :
> :
>
>

[Boomer]

I fogot getting old :-)

""Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes, your
alkalinity equation."'

How about if we use [HCl ] and [CO3], please point that out in the Alk equations
--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
www.coralrealm.com

If You See Me Running You Better Catch-Up
"Boomer" > wrote in message
...
: "As it is the ability to neutralizes an acid that is a buffer"
:
: sorry
:
: As it is the ability to neutralizes a base that is a buffer
:
: --
: Boomer
:
: Want to talk chemistry ? The Reef Chemistry Forum
: http://www.reefcentral.com/vbulletin/index.php
:
: Want to See More ?
: Please Join Our Growing Membership
: www.coralrealm.com
:
: If You See Me Running You Better Catch-Up
: "Boomer" > wrote in message
: ...
: :
: : "I am not sure if you are just messing with me "
: :
: : Yes, messing with you, it is called trolling a troll, to see where the hell you would
go
: : and what you would say in regards to last posts. It is called honesty, of which you
have
: : none off to say the least,that I can see.You always like to post what suits you and
just
: : avoid ref I give. So lets start where you are WRONG and have a great lack of
: understanding
: : of things, to include pointing out all your gross error which you still FAIL to
: : acknowledge and which can be prove in many water chem. ref. .I doubt like hell you are
a
: : chemist at all.You seem to want to con people into thinkin' you are. But then again, I
: : have seen chemists like you before, they are not familiar with the, but they ASK to
have
: : it explained and ask for REF.YOU just shoot from the hip. WHAT GETS YOU IN TROUBLE.
You
: : remind me of snoot-noise kid that come here and other NG's and forums...that think
they
: : know, buy hey, maybe I'm wrong :-)
: :
: :
: :
: : 1). Acidity
: :
: : "***Benjamin,Water Chemistry (2002, pages 262-263).***
: :
: : ***Acidity A concept that is exactly analogous to alkalinity but measures the base
: : neutralizing
: : capacity (BNC) of a solution is Acidity. The quantitative represents the concentration
: of
: : OH- ions that must be added to titrate the solution to a pH near 10.5***
: :
: : So that means that not only in Benjamin wrong but, so are Stumm & Morgan, Millero,
: Pilosn,
: : Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I said, you have
: your
: : acidity and Acidy mixed up. Acidity as defined above is covered in most water
chemistry
: : books, written by chemists, who's field of expertise is water chemistry. You can even
: buy
: : Acidity test kits from, HACH, LaMotte, etc..
: :
: : You mean you didn't read this or are you just avoiding it .The same definition can be
: : found in almost any std water chemistry book.
: :
: : I have run into few chemists, that are NOT familiar with the above. Some water reports
: : require the above Acidity measuring. The issue with you is you do not understand
WATER
: : CHEMISTRY. Everything you have posted can be found a general chemistry book
: :
: :
: :
: :
: : 2) Alk and BC
: :
: : From the link
: :
: : Alkalinity
: : ***Acid neutralizing or buffering capacity of water; a measure of the ability of water
: to
: : resist changes in pH caused by the addition of acids or bases ***
: :
: : This is a Buffering Capacity definition not Alk
: :
: : Humm, since when does Alk have anything to do in regards to the addition of BASE. As I
: : pointed out in the first post the term is often miss used. Even in YOUR own posts you
: say
: : it is based on a acid addition, no mention of **base or acid** addition by you. Are
you
: : getting confused or what. Or is more you are trying to confuse everyone you are right.
: The
: : above is a definition for Buffer Capacity NOT Alk
: :
: : From Drew, Geochemistry of Natural Waters
: :
: : "alkalinity, which is formally defined as the equivalent sum of bases that are
: titratable
: : with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH of the solution
is
: : progressively lowered by the addition of a strong acid (HCL), all the anions on the
: right
: : will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4, H2S,organic acids, H20)"
: :
: : This follows almost all description of Alk, that it is acid neutralizing reaction and
: has
: : nothing to do with base neutralizing, which is Acidity (BNC) .I defined these before
you
: : had no comment
: :
: :
: : Even the links that give the Buffering Capacity definition is wrong, as is the UIPAC
on
: : Alkalinity. Alkalinity has nothing to do with the addition of bases only acids. When
you
: : use the words "base and acid" it becomes BC
: :
: : Even YOU MUST disagree with these definitions, from YOUR own post
: :
: : Think of alkalinity as 'buffering capacity'. Or the ability of a solution
: : ***to resist a drop in pH due to the addition of acid***
: :
: : Where the flip is the base addition forget it ?
: :
: : From Butler; Carbon Dioxide Equilibrium and Their Applications (professor emeritus
: : Harvard University) an expert on the subject.
: :
: : Buffering Index (Buffering Capacity, Buffer Intensity).
: :
: : ***This concept was first developed for mixtures of approximately equal proportions of
: : conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such buffer solutions
: : strongly resist changes in pH when acids or bases are added and are useful as pH
: : standards. The Buffer Index tells how great the resistance to pH changes will be.**
: :
: : also from Butler
: :
: : Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
: :
: : Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
: :
: : Acidity is in fact just the negative of Alkalinity ***
: :
: : http://www.lagoonsonline.com/acid.htm
: :
: :
http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.htm?E+mystore
: :
: : It sure is funny how all of the chemist that write water chemistry textbooks never say
: Alk
: : is the Buffering Capacity of a solution. They are always treated and defined
separately.
: :
: : If you or others choose to treat Alk and BC as the same, well, just have at it. As I
: said
: : in first post I know what you mean.
: :
: : "No need to cite web pages that describe what I know and what I wrote
: : in this discussion"
: :
: : No you don't know, who are you trying to convince any way, me, the guys here and/or
all
: : the water chemists in this world. As I said before go get a dam WATER CHEMISTRY book
or
: : shut the hell up.You keep trying to define things from a general chemistry book WE ARE
: IN
: : THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
: :
: :
: :
: :
: :
: : 3). pKa's and what you don't know or seem to be confused on
: :
: : "Therefore, it has two pKa's
: : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35. The
: : pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
: : right in there. Is that magic? :)"
: :
: : Here it is agin that is twice at least
: :
: : "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this example)
: : you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium will
: : be shifted to HCO3-2 by a ratio of 1:100.
: :
: : Oh wait , there is a third time LOL
: :
: : "At the pH of seawater, the buffering capacity of carbonate is at it's
: : weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
: :
: :
: : Lets just dunk you on this one. I am taking note you refuse to reply to YOUR errors
: :
: : So you calculated the pH of seawater with freshwater pKa's, now that is a good trick.
: From
: : a number of seawater chemistry books the seawater pKa's are 6 & 9.1, so according to
: you,
: : seemingly not understanding your favorite Henderson-Hasselbach equation;
: :
: : 2 pH = (6 + 9.1) /2 pH = 7.55
: :
: : I have never seen seawater with a pH of 7.55. There is no ocean with that pH. Humm
how
: : come your equation is not working for you today.?
: :
: :
: : "That pH I calculated is
: : right in there. Is that magic? :)"
: :
: : I roll on the floor when I see this = 8.35
: :
: : Hum , just a brain far so excuse me for thinkin
: :
: : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
: :
: : Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a pH of 8.35 there
: pal
: : ? That 8.35 is what you are telling people the pH should be, but their meter says 6.4.
: : This how people will READ this.
: :
: :
: :
: :
: : 4.) More on Buffering Capacity
: :
: : "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes, your
: : alkalinity equation."'
: :
: :
: : Yup, I see that and in this case the HCO3 is the acid and the CO3 is the base CORRECT.
: In
: : Alk you are only dealing with bases and how they react to an acid. Acidity deals acids
: and
: : how they recact to bases "Acidity, A concept that is exactly analogous to alkalinity
but
: : measures the base neutralizing
: : capacity (BNC) of a solution is Acidity "Alk is the ANC Acid neutralizing capacity
: :
: : "Don't the components of a buffer account for the buffering capacity? "
: :
: : Yes, they do but so do the acids which work as buffers. NaHCO3 is a buffer and can act
: as
: : an acid or base
: :
: : *** Buffering Capacity.**
: : The power of a substance in solution to absorb acid or alkali without change in pH;
this
: : is highest at a pH value equal to the pKa value of the acid of the buffer pair.***
: :
: : ***Akalinity***
: : Measure of the power of a solution to neutralise hydrogen ions (H+), usually expressed
: as
: : the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
: :
: :
: : If one wants to call Alk Buffering capacity then one sure as a hell can call Acidty
: : Buffering Capacity also. As it is the ability to neutralizes an acid that is a
: buffer.You
: : have a pH of 7 and you add a buffer to lower it to a pH of 4, you are buffering the
: water,
: : that buffer is a acid.
: :
: : 5) CO2
: :
: : You are really confuse so it seems :-) You realllllllly indicate that CO2 is affected
by
: : the Alk or vise-versa
: :
: : "Yes, the pH will drop with the addition of CO2. Remove CO2 will cause the
: : pH to rise? How do you remove CO2? Once it is in solution it forms
: : carbonic acid and neutralizes some of your 'buffer'."
: :
: : "With the exception of CO2?"
: :
: : No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
: : Concepts)....PERIOD.You seem to think a that at least in two of your post that CO2 is
: : affected by the Alk or vise-versa. Please go back to school or seek professor
: :
: : "Why in one case does CO2 from air lower pH and in the other case it raises
: : it? Doesn't make sense."
: :
: : That is because you don't understand CO2 period. By the way I saved this, wanted to
see
: : if you would bite on the post I gave. Not bite at first, so time to reel you in, as
you
: : did bite in another post..
: :
: : Lets make some sense of it for you, being that you have a pH.D in chemistry, so you
say
: .
: :
: : CO2 is naturally generated in a aquatic systems, it is capable of raise to various
: levels
: : depending on a number of circumstances .It can be measure (except in seawater) or
: : calculated using Buch/Park Equations (what we use for seawater. In sort if you know
the
: pH
: : and Alk you can calculate the CO2). If you aerate a system or a sample of water, even
if
: : the pH has only dropped a couple of tenths, due to an increase in CO2, the CO2 will
: leave
: : solution to the atmosphere.This will raise the pH. On the other hand if theCO2 level
is
: : more of the norm and you have hikgh room air, such as in the winter, the partial
: pressure
: : of the CO2 in air will be much higher than that in water, in which case the CO2 will
: enter
: : the water and lower the pH. That is without an airstone. Adding an airstone will make
it
: : even worse,as you are now forcefully driving the CO2 into solution even quicker. These
: : test /experiments have been proven many times, it is not that may work could work they
: do
: : work.Yet you want to disagree and in another post say you haven't tried it,.Seems to
me
: : that based on what you say it can't work So, in short you don't know what the hell you
: are
: : taking about. Go get a glass of seawater with a pH of about 8.3 and lower it to about
: : 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK- UP ( that is if
you
: : don't have a high room air CO2 problem.). This little test has been done thousands of
: : times in this hobby, with test kits, pH meters and even graphic printers.
: :
: : "This is where Boomer and I
: : disagree. I say you would have to lower the pH very low in order to
: : effectively remove CO2 by purging."
: :
: : You are 100 % wrong. Please come to our Chem forum and try and run that by Randy,
don't
: : take my word on it. I already know what he will say.
: :
: : "Boomer didnt convince me it
: : works at the pH of an aquarium, but I never tried it and I'm not sure of
: : this. "
: :
: : Well then come too our chem. forum and tell Randy he doesn't know what he is talking
: about
: : LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it should be easy
for
: : you to run the experiment LOL There are grade school kids that run the test and know
: what
: : happens and that I'm correct.
: :
: :
: : "The equilibrium is a FUNCTION
: : of pH."
: :
: : It is also a function of Alk or don't you know that. At a pH of 8.3, Alk 2.25, the CO2
: is
: : about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk to about .4 meq/
l
: : or so the CO2 will be around .99 mg / l CO2, When dealing with tanksCO2 is not always
in
: : equilibrium with ambient air.
: :
: :
: : ". But I wouldn't degas a solution of a
: : specific gas (CO2) with a gas (this case he was using air) that contains the
: : same gas I am trying to purge."
: :
: : Why not ? We have a guy right now that is running tests on purging ambient air with a
: : solution to remove CO2 gas from the air, before it enters the tank per/Randy's
: suggestion.
: : The same guy is doing some of my test using a Clinoptilolite, a Zeolite mineral, that
: has
: : an affinity for CO2.This will be a dry CO2 scrubber
: :
: :
: : Sorry Soutman but you sure as hell don't seem to know much about aquatic chemistry.
You
: : seem to be guessing at everything.
: :
: : By the way have you read any of Randy's technical articles on water chemistry, been
: saving
: : these for last. There are a few on pH, Alk, CO2 .Here is a list
: :
: : Try and answer them 1-5 and lets see where we get THIS TIME :-) or maybe we should
just
: : drop it. I could care less at this point.
: :
: : THE END
: :
: :
: : ARTICLES
: :
: : The first two posts in this thread are lists of some of my articles that relate to
reef
: : tank chemistry. In the next few posts are some of the articles published by Craig
: Bingman
: : and others on reef chemistry issues.
: :
: : The first two posts in this thread are lists of some of my articles that relate to
reef
: : tank chemistry. In the next few posts are some of the articles published by Craig
: Bingman
: : and others on reef chemistry issues.
: :
: : Solving Common Problems
: :
: : Solving Calcium and Alkalinity Problems
: : http://www.advancedaquarist.com/issues/nov2002/chem.htm
: :
: : Solutions to pH Problems
: : http://www.advancedaquarist.com/iss...ne2002/chem.htm
: :
: : How to Select a Calcium and Alkalinity Supplementation Scheme
: : http://www.advancedaquarist.com/issues/feb2003/chem.htm
: :
: : Phosphate Issues
: : http://www.advancedaquarist.com/iss...pt2002/chem.htm
: :
: : Nitrate Issues
: : http://www.advancedaquarist.com/iss...st2003/chem.htm
: :
: :
: :
: : Calcium and Alkalinity
: :
: : Solving Calcium and Alkalinity Problems
: : http://www.advancedaquarist.com/issues/nov2002/chem.htm
: :
: : How to Select a Calcium and Alkalinity Supplementation Scheme
: : http://www.advancedaquarist.com/issues/feb2003/chem.htm
: :
: : Calcium and Alkalinity Balance Issues
: : http://reefkeeping.com/issues/2002-...ature/index.htm
: :
: : Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
: : http://www.advancedaquarist.com/iss...ly2002/chem.htm
: :
: : The Relationship Between Alkalinity and pH.
: : http://www.advancedaquarist.com/issues/may2002/chem.htm
: :
: : The Chemical & Biochemical Mechanisms of Calcification in Corals
: : http://www.advancedaquarist.com/issues/apr2002/chem.htm
: :
: : Calcium
: : http://www.advancedaquarist.com/issues/mar2002/chem.htm
: :
: : Alkalinity
: : http://www.advancedaquarist.com/iss...2/chemistry.htm
: :
: :
: : Iron
: :
: : First Iron Article: Macroalgae and Dosing Recommendations
: : http://www.advancedaquarist.com/issues/aug2002/chem.htm
: :
: : Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
: : http://www.advancedaquarist.com/issues/oct2002/chem.htm
: :
: : Iodine
: :
: : Iodine in Marine Aquaria: Part I
: : http://www.advancedaquarist.com/issues/mar2003/chem.htm
: :
: : Iodine in Reef Tanks 2: Effects on Macroalgae Growth
: : http://www.advancedaquarist.com/iss...il2003/chem.htm
: :
: :
: : Magnesium and Strontium
: :
: : Strontium
: : http://www.advancedaquarist.com/issues/nov2003/chem.htm
: :
: : Magnesium
: : http://www.advancedaquarist.com/issues/oct2003/chem.htm
: :
: : Magnesium and Strontium in Limewater
: : http://www.advancedaquarist.com/issues/dec2003/chem.htm
: :
: :
: : Limewater (kalkwasser)
: :
: : The Self Purification of Limewater (Kalkwasser)
: : http://www.advancedaquarist.com/issues/may2003/chem.htm
: :
: : The Degradation of Limewater (Kalkwasser) in Air
: : http://reefkeeping.com/issues/2003-...ature/index.htm
: :
: : How to Select a Calcium and Alkalinity Supplementation Scheme
: : http://www.advancedaquarist.com/issues/feb2003/chem.htm
: :
: : Metals in Aquaria
: :
: : Aluminum and aluminum-based phosphate binders
: : http://www.advancedaquarist.com/iss...ly2003/chem.htm
: :
: : Reef Aquaria with Low Soluble Metals
: : http://reefkeeping.com/issues/2003-...ature/index.htm
: :
: : Tap Water in Reef Aquaria
: : http://www.advancedaquarist.com/issues/jan2004/chem.htm
: : First Iron Article: Macroalgae and Dosing Recommendations
: : http://www.advancedaquarist.com/issues/aug2002/chem.htm
: :
: : Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
: : http://www.advancedaquarist.com/issues/oct2002/chem.htm
: :
: :
: : Test Kit Reviews
: :
: : The Seachem Borate Alkalinity Test Kit
: : http://www.advancedaquarist.com/iss...ne2003/chem.htm
: :
: : The Salifert Boron Test Kit
: : http://www.advancedaquarist.com/iss...pt2003/chem.htm
: :
: : Boron and Borate (and pH buffering)
: :
: : Boron in a Reef Tank (and its effect on pH buffering)
: : http://www.advancedaquarist.com/issues/dec2002/chem.htm
: :
: : The Seachem Borate Alkalinity Test Kit
: : http://www.advancedaquarist.com/iss...ne2003/chem.htm
: :
: : The Salifert Boron Test Kit
: : http://www.advancedaquarist.com/iss...pt2003/chem.htm
: :
: :
: :
: : Others
: :
: : Tap Water in Reef Aquaria
: : http://www.advancedaquarist.com/issues/jan2004/chem.htm
: :
: : ORP
: : http://reefkeeping.com/issues/2003-...ature/index.htm
: :
: : Chloramine
: : http://reefkeeping.com/issues/2003-...ature/index.htm
: :
: : Silica in a Reef Tank
: : http://advancedaquarist.com/issues/jan2003/feature.htm
: :
: : Specific Gravity (and temperature correction of hydrometers)
: : http://www.advancedaquarist.com/iss...2/chemistry.htm
: :
: :
: : The Complete Nitrogen Cycle
: : http://www.animalnetwork.com/fish/l...a&RecordNo=3090
: :
: : Magnesium (older article with fonts screwed up)
: : http://www.aquariumfish.com/aquariu...cid=124&search=
: :
: : Phosphate (older article now reproduced in a poor fashion)
: : http://www.aquariumfish.com/aquariu...cid=124&search=
: :
: : Carbon Dioxide
: : http://www.animalnetwork.com/fish/l...a&RecordNo=2074
: :
: : Using Conductivity to Measure Salinity
: : http://www.aquariumfish.com/aquariu...cid=124&search=
: :
: : Understanding Seawater
: : http://www.animalnetwork.com/fish2/...s/1/default.asp
: :
: : Protein Skimming: How It Works
: : http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
: :
: :
: :
: : Articles by Craig Bingman:
: :
: : Carbon Dioxide tests
: : http://www.animalnetwork.com/fish/l...n=&RecordNo=279
: :
: : Limewater, Acetic Acid and Sand Clumping
: : http://www.animalnetwork.com/fish/l...n=&RecordNo=181
: :
: : Calcium and Alkalinity
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : Calculation of Calcium Carbonate Saturation States in Reef Aquaria
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: :
: : Calcification Rates in Several Tropical Coral Reef Aquaria
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : Limits To Limewater...Revisited
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : Expanding the Limits of Limewater: Adding Organic Carbon Sources (vinegar)
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: :
: : Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : Magnesium - Part I
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : Magnesium - Part II
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : A Homemade Magnesium Supplement
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : Simulating the Effect of Calcium Chloride and Sodium Bicarbonate Additions on Reef
: Systems
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : Additional Simulations: The Combined Effect Of Calcium Chloride
: : /Sodium Bicarbonate Additions And Water Exchanges
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: :
: : More articles by Craig Bingman:
: :
: : The Halogens - Part I: Bromine in Seawater and Aquaria
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : The Halogens - Part II: Fluoride
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : Fluoride Depletion In Four Reef Aquariums
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : The Halogens - Part III: Iodine
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : Measuring Halides
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : How Test Kits Work
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : Borax pH Calibration
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : A pH Detective Story
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : How to Mix a Batch of Synthetic Seawater in Under Five Minutes
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: : SILICON - FOE OR FRIEND?
: : http://www.animalnetwork.com/fish2/...s/1/default.asp
: :
: : The Composition Of Several Synthetic Seawater Mixes
: : http://www.animalnetwork.com/fish2/...s/1/default.asp
: :
: : Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
: : http://www.animalnetwork.com/fish2/...bio/default.asp
: :
: :
: :
: : Andy's calcium calculator
: : http://www.andy-hipkiss.co.uk/cacalc.htm
: :
: : Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
: : http://www.aquariumfish.com/aquariu...cid=124&search=
: :
: : Calcium Reactor Substrate -- Phosphate Levels
: : by Greg Hiller
: : http://www.advancedaquarist.com/iss...l2003/short.htm
: :
: :
: : Indoor CO2 Problems
: : http://www.advancedaquarist.com/iss...r2002/short.htm
: :
: : Simon Huntington's CaCO3/CO2 reactor article
: :
: : http://reefkeeping.com/issues/2002-...ature/index.htm
: :
: : Ron Shimek's Tank Water Analysis Article
: : http://reefkeeping.com/issues/2002-...ature/index.htm
: :
: :
: :
: :
: : Home made salinity standards thread:
: :
: : http://reefcentral.com/forums/showt...?threadid=65509
: :
: : Reef Chemicals Calculator
: : http://www.kademani.com/reefchem.htm
: :
: :
: :
: : Boomer
: :
: : Want to talk chemistry ? The Reef Chemistry Forum
: : http://www.reefcentral.com/vbulletin/index.php
: :
: :
: : Former US Army Bomb Technician (EOD)
: : Member; IABTI, NATEODA, WEODF, ISEE & IPS
: :
: : If You See Me Running You Better Catch-Up
: :
: :
: : --
: : Boomer
: :
: : Want to talk chemistry ? The Reef Chemistry Forum
: : http://www.reefcentral.com/vbulletin/index.php
: :
: : Want to See More ?
: : Please Join Our Growing Membership
: : www.coralrealm.com
: :
: : If You See Me Running You Better Catch-Up
: : "stoutman" <.@.> wrote in message news:aGuWb.148227$U%5.676753@attbi_s03...
: : : Boomer,
: : :
: : : I am not sure if you are just messing with me or if you are truly confused.
: : : I hope the latter. Please read from Top to Bottom.
: : :
: : :
: : : From YOUR first link:
: : :
: : : http://www.waterontheweb.org/resources/glossary.html
: : :
: : : Acidity:
: : : A measure of how acid a solution may be. A solution with a pH of less than
: : : 7.0 is considered acidic. Solutions with a pH of less than 4.5 contain
: : : mineral acidity (due to strong inorganic acids), while a solution having a
: : : pH greater than 8.3 contains no acidity.
: : :
: : : Yes,
: : :
: : : Good definition (for the most part). pH <7 is indeed acidic. pH > 7 is
: : : basic. Your web page had a definition for acidity, but not basicity.
: : : Strange. That's like defining GOOD and not defining BAD.
: : :
: : : Here is the IUPAC (International Union of Pure and Applied Chemistry)
: : : definition of acidity:
: : :
: : : http://www.chem.qmul.ac.uk/iupac/index.html
: : :
: : : acidity
: : :
: : : (1) Of a compound:
: : :
: : : For Brønsted acids it means the tendency of a compound to act as a hydron
: : : donor. It can be quantitatively expressed by the acid dissociation constant
: : : of the compound in water or some other specified medium. For Lewis acids it
: : : relates to the association constants of Lewis adducts and -adducts.
: : :
: : : (2) Of a medium:
: : :
: : : The use of the term is mainly restricted to a medium containing Brønsted
: : : acids, where it means the tendency of the medium to hydronate a specific
: : : reference base
: : :
: : : basicity
: : :
: : : For Brønsted bases it means the tendency of a compound to act as hydron
: : : (proton) acceptor. The basicity of a chemical species is normally expressed
: : : by the acidity of the conjugate acid (see conjugate acid-base pair). For
: : : Lewis bases it relates to the association constants of Lewis adducts
: : : and -adducts
: : :
: : :
: : :
: : : Another definition from the same web page YOU cited: (this is the same web
: : : page you cited above)
: : :
: : : Alkalinity:
: : : Acid neutralizing or buffering capacity of water; a measure of the ability
: : : of water to resist changes in pH caused by the addition of acids or bases
: : : and therefore, the main indicator of susceptibility to acid rain; in natural
: : : waters it is due primarily to the presence of bicarbonates, carbonates and
: : : to a much lesser extent occasionally borates, silicates and phosphates. It
: : : is expressed in units of milligrams per liter (mg/l) of CaCO3 (calcium
: : : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l = 1 mg/l
: : : of CaCO3. A solution having a pH below about 5 contains no alkalinity.
: : :
: : : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and says
: : : that alkalinity is the measure of ...(description of a buffer)
: : :
: : : A BUFFER IS : a measure of the ability of water to resist changes in pH
: : : caused by the addition of acids or bases (from definition below)
: : :
: : :
: : : I said:
: : : ***alkalinity is a measurement of 'buffering capacity'***
: : :
: : : You said:
: : : ***Alkalinity is not a measurement of BC
: : :
: : : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is not
: : : logical.
: : :
: : : (THIS FROM THE SAME WEB PAGE YOU CITED):
: : :
: : : Buffer:
: : : A substance which tends to keep pH levels fairly constant when acids or
: : : bases are added.
: : :
: : : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
: : :
: : : a measure of the ability of water to resist changes in pH caused by the
: : : addition of acids or bases
: : :
: : : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A BUFFER.
: : :
: : :
: : : I went to all four links. None contradict what I have said. But the first
: : : one you cited contradicts YOU!
: : :
: : : I know what a buffer is. I know what acidity means. I know what alkalinity
: : : means. No need to cite web pages that describe what I know and what I wrote
: : : in this discussion. Show me one that says alkalinity is not a measure of
: : : buffering capacity from a credible source.
: : :
: : :
: : :
: : :
: : :
: : :
: : : "Boomer" > wrote in message
: : : ...
: : : > Alkalinity a measure of the amount of anions of weak acid in water and of
: : : the cations
: : : > balanced against them
: : : > Take note it says ***acid***
: : : >
: : : > Buffering capacity the ability of a solution to resist or dampen changes
: : : in pH upon the
: : : > addition of acids or bases.
: : : > Take note its says ***the addition of acids or bases***
: : : >
: : : > One more
: : : >
: : : > http://www.waterontheweb.org/resources/glossary.html
: : : >
: : : > We could go on like this all day, so what is the point ?
: : : >
: : : > You will LOVE this one
: : : > http://www.kyantec.com/Tips/phbuffering.htm
: : : >
: : : > Don't you just lovbe PDF's
: : : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
: : : >
: : : > Don't fall out of your chair
: : : > http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
: : : >
: : : >
: : : >
: : : >
: : : > --
: : : > Boomer
: : : >
: : : > Want to talk chemistry ? The Reef Chemistry Forum
: : : > http://www.reefcentral.com/vbulletin/index.php
: : : >
: : : > Want to See More ?
: : : > Please Join Our Growing Membership
: : : > www.coralrealm.com
: : : >
: : : > If You See Me Running You Better Catch-Up
: : : > "stoutman" <.@.> wrote in message news:XB7Wb.19339$QA2.62332@attbi_s52...
: : : > : Man here is another, google is a wonderful thing. I'm not filtering any
: : : > : out, just posting what I find by GOOGLING for you.
: : : > :
: : : > : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
: : : > :
: : : > :
: : : > : Wow, a gov link. Even the government is wrong, this must be a
: : : conspiracy
: : : > : against Boomer.
: : : > :
: : : > :
: : : > :
: : : > :
: : : > : "Boomer" > wrote in message
: : : > : ...
: : : > : > Now I am getting bored
: : : > : >
: : : > : > "Don't the components of a buffer account for the buffering capacity?
: : : > : Yes."
: : : > : >
: : : > : > Yes, agreed but you seem to fail what I'm saying. Buffering Capacity
: : : and
: : : > : Alkalinity are
: : : > : > not the same, that has always been the issue. I gave the equation does
: : : > : that look like an
: : : > : > Alkalinity equation or how Alk is determined. I see you had now
: : : comments
: : : > : on it what's
: : : > : > wrong, why no comments on the equations I gave. Don't understand them
: : : or
: : : > : what ? Again this
: : : > : > is the equation for Buffering Capacity, also called Buffer Index or
: : : Buffer
: : : > : Intensity. It
: : : > : > is defined in most water chemistry and chemical oceanography text
: : : books.
: : : > : >
: : : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] +
: : : CKa
: : : > : [H3O+] / (Ka =
: : : > : > H3O+])² )
: : : > : >
: : : > : > This is not Alkalinity now is it ?
: : : > : >
: : : > : > "I know how to do a titration, In fact I have done several. How many
: : : have
: : : > : > you actually done? I don't mean by counting drops, I mean with a
: : : buret?"
: : : > : >
: : : > : > Well good for you, I use a Digital Titrator
: : : > : >
: : : > : > "Oh, I see,
: : : > : > you think acidity is the opposite of alkalinity. In the world of
: : : > : CHEMISTRY
: : : > : > it's not. Maybe in aquarium newsgroups it is.
: : : > : >
: : : > : > Hum no, maybe you should go for a look at HACH's or LaMotte website or
: : : the
: : : > : book I
: : : > : > suggested earlier. Please view a copy.
: : : > : >
: : : > : > Standard Methods for the Examination of Water and Wastewater
: : : > : >
: : : > : > This book, over 2000 pages, is the guide for water testing. If you are
: : : > : reporting water
: : : > : > test to the EPA you must use approved std from this text.I t is
: : : prepared
: : : > : and published by
: : : > : > the EPA, American Water Works Association and American Public Health
: : : > : Association. You
: : : > : > mean you don't have one and the issue is water chemistry
: : : > : >
: : : > : > You are confusing Acidity and Acidity as you know little about water
: : : > : chemistry and
: : : > : > procedures and test methods
: : : > : >
: : : > : > From SMEWW, section 2-30, 2310 ACIDITY
: : : > : >
: : : > : > "Acidity of water is its quantative capacity to react with a strong
: : : base
: : : > : to a designated
: : : > : > pH"
: : : > : >
: : : > : > This is how you test for it
: : : > : >
: : : > : > A std alkali titration to methyl orange or phenolphthalein
: : : > : > endpoint.
: : : > : >
: : : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that write
: : : this
: : : > : book, there are
: : : > : > over 100 of them, they are wrong.
: : : > : >
: : : > : > Like Buffering Capacity you have your Acidity's mixed up
: : : > : > In water measurement if you have a high Alk you also usually have a
: : : high
: : : > : Acidity.
: : : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
: : : CHEMISTRY
: : : > : BOOK there pal.
: : : > : >
: : : > : >
: : : > : > "These are all in equilibrium with each other. An initial high pH
: : : (above
: : : > : > 6.4) will shift the equilibrium to the right to form HCO3-1. If the
: : : pH of
: : : > : > the solution is above 10.3 (pKa2) the .........."
: : : > : >
: : : > : >
: : : > : > Christ, there you go again with the FW ****. All your numbers are
: : : wrong we
: : : > : are dealing
: : : > : > with SEAWATER
: : : > : >
: : : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is in the
: : : form
: : : > : > of HCO3-1 .
: : : > : >
: : : > : > I have already pointed that out and gave actual values at know
: : : seawater
: : : > : levels, go back
: : : > : > and re-read it you aren't telling me anything here.Of course most is
: : : HCO3
: : : > : see...
: : : > : >
: : : > : >
: : : > : > @ 20C and 34.3 ppt salinity
: : : > : >
: : : > : > CO2 = 0.52 %
: : : > : >
: : : > : > HCO3 = 86.4 %
: : : > : >
: : : > : > CO3 = 13.09 %
: : : > : >
: : : > : >
: : : > : > "In your glass experiment you managed to lower the pH enough to purge
: : : out
: : : > : CO2
: : : > : > by boiling"
: : : > : >
: : : > : > The purpose behind the glass is to show that alk is not affect by CO2
: : : and
: : : > : vise-versa and
: : : > : > how Co2 affects pH.
: : : > : >
: : : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and that pH
: : : drops
: : : > : to say 8.1 it is
: : : > : > usually due to excess CO2. If you took a glass of that water and
: : : aerated
: : : > : it you WILL drive
: : : > : > off the CO2 and raise the pH. It has been done a proven a million
: : : times.
: : : > : >
: : : > : > "In order to 'purge' CO2 you would need to lower the
: : : > : > pH to shift the equilibrium to below 6.4"
: : : > : >
: : : > : > The hell you do !!!.Do you know who many times people on this NG to
: : : > : include Dr. Craig
: : : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to take a
: : : > : sample of aquarium
: : : > : > water and aerate it to see if the pH GOES UP AND when they come back
: : : with
: : : > : the test it is
: : : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST
: : : excess
: : : > : CO2 in the tank
: : : > : > water, increase the circulation for better gas exchange at the
: : : surface,
: : : > : reduce feeding,
: : : > : > and try to improve on better skimming, thus reducing the bio-load and
: : : pH
: : : > : decline due to
: : : > : > CO2.
: : : > : >
: : : > : >
: : : > : > "I hope this helps. "
: : : > : >
: : : > : > Help, how can you when you miss everything. I should be charging you
: : : > : >
: : : > : > Oh, by the way. Your websites, I have about 50 on these issues, I
: : : could
: : : > : post them, not to
: : : > : > mention I have all those water chemistry books, so there is no need to
: : : > : view your sites.
: : : > : >
: : : > : > Finally are you afraid to come to our Chemistry Forum, afraid to get
: : : > : slapped by REAL
: : : > : > chemists. I get a charge out of you can't post your ref .I have posted
: : : the
: : : > : same or similar
: : : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500
: : : posts
: : : > : there and am the
: : : > : > biggest contributor to his forum other than himself or maybe Habib
: : : Sheka
: : : > : >
: : : > : > Hum, here are Randy's ref that he posted. He hosts the website
: : : > : >
: : : > : > S. RANDY HOLMES-FARLEY
: : : > : > Arlington, Massachusetts
: : : > : >
: : : > : > EDUCATION
: : : > : >
: : : > : > 1982-1986 Harvard University Cambridge, MA
: : : > : > PhD in Chemistry
: : : > : > Research Advisor: George Whitesides
: : : > : >
: : : > : > Investigated the relationship between polymer surface chemistry and
: : : > : physical properties
: : : > : > through controlled surface modification and testing.
: : : > : >
: : : > : > 1980-1982 Cornell University Ithaca, NY
: : : > : > BA in Chemistry and Biology
: : : > : > Graduated Summa Cum Laude
: : : > : > Distinction in All Subjects
: : : > : > Grade Point: 3.94/4.0
: : : > : > Honors research: isolation and characterization of the subunit of CF1
: : : > : enzyme
: : : > : >
: : : > : >
: : : > : > 1978-1979 Stanford University Palo Alto, CA
: : : > : > Grade Point: 3.55/4.0
: : : > : >
: : : > : >
: : : > : > EXPERIENCE
: : : > : >
: : : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
: : : > : > (bought out GelTex Pharmaceuticals in 2001)
: : : > : > Vice President, Chemical Research 2001-present
: : : > : > Senior Director, Chemical Research 1999-2001
: : : > : > Director of Chemical Research 1997-1999
: : : > : > Manager of Chemical Research 1995-1997
: : : > : > Group Leader 1994-1995
: : : > : > Senior Research Scientist 1992-1994
: : : > : >
: : : > : > Helped start GelTex as second employee
: : : > : >
: : : > : > Managed various research programs with multi-million dollar budgets
: : : > : >
: : : > : > Supervised research chemists (17+)
: : : > : >
: : : > : > Co-inventor of several polymeric pharmaceuticals and pharmaceutical
: : : > : candidates including
: : : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam Hydrochloride
: : : (FDA
: : : > : approved)
: : : > : >
: : : > : > Company Safety Officer for 3 years
: : : > : >
: : : > : > Chemical Hygiene Officer 2000-present
: : : > : >
: : : > : >
: : : > : >
: : : > : >
: : : > : > 1990-1992 GTE Corporation Waltham, MA
: : : > : > Senior Member of Technical Staff
: : : > : > Applied research involving polymer interfaces
: : : > : > Metallization of plastics
: : : > : > Polymer/polymer adhesion
: : : > : > Optical coatings
: : : > : >
: : : > : >
: : : > : >
: : : > : > 1986-1990 Lord Corporation Cary, NC
: : : > : > Senior Research Scientist 1988-1990
: : : > : > Research Scientist 1986-1988
: : : > : > Basic and applied research on surface chemical bonding
: : : > : > Developed new adhesive compositions
: : : > : > Developed new sol-gel coatings for corrosion resistance
: : : > : >
: : : > : >
: : : > : > HONORS AND AWARDS
: : : > : >
: : : > : > Industrial Innovations Award by Northeast Region of American Chemical
: : : > : Society (6/2001)
: : : > : >
: : : > : > National Kidney Foundation of Northern California Honoree (5/2001)
: : : > : >
: : : > : > American Chemical Society/Polymer Chemistry Division Industrial
: : : Sponsors
: : : > : > Award (8/2000)
: : : > : >
: : : > : > R&D 100 Award from R&D magazine (1999)
: : : > : >
: : : > : > Sherwin Williams Award in applied polymer science (9/85)
: : : > : >
: : : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985; 1985-1986)
: : : > : >
: : : > : > Award for highest GPA in Chemistry Department (6/82)
: : : > : >
: : : > : > Summa Cum Laude Honors in Chemistry (6/82)
: : : > : >
: : : > : > Phi Lamda Epsilon (6/82)
: : : > : >
: : : > : > Phi Beta Kappa (2/82)
: : : > : >
: : : > : > Cornell University Dean's List (1981, 1982)
: : : > : >
: : : > : > Harvard Book Club Award for highest GPA senior year (1978)
: : : > : >
: : : > : > First Place in western NY ACS high school chemistry exam (1977)
: : : > : >
: : : > : > 1978-1979
: : : > : >
: : : > : >
: : : > : > __________________
: : : > : > Randy Holmes-Farley
: : : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef Central
: : : > : >
: : : > : > Hobby Experience: 8 years with reefs
: : : > : > Current Tanks: 90 gal mixed reef
: : : > : > Interests: Reefkeeping, science, photography
: : : > : >
: : : > : >
: : : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
: : : > : >
: : : > : > Open this post in a new window | Report this post to a moderator | IP:
: : : > : Logged
: : : > : >
: : : > : >
: : : > : >
: : : > : > 06/27/2003 02:44 PM
: : : > : >
: : : > : > Randy Holmes-Farley
: : : > : > Chemistry Moderator
: : : > : >
: : : > : > Registered: Apr 2001
: : : > : > Location: Arlington, Massachusetts
: : : > : > Occupation: Chemist (Drug Discovery at Genzyme)
: : : > : > Posts: 15282
: : : > : >
: : : > : >
: : : > : >
: : : > : > Publications
: : : > : >
: : : > : >
: : : > : > ISSUED UNITED STATES PATENTS
: : : > : >
: : : > : >
: : : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
: : : > : Mandeville, III; W. Harry.
: : : > : > US 6,566,407; 5/20/2003
: : : > : >
: : : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen
: : : Randall;
: : : > : Huval, Chad
: : : > : > Cori.
: : : > : > U.S. 6,517,825; 2/11/2003.
: : : > : >
: : : > : > 3. Method of making phosphate-binding polymers for oral
: : : administration.
: : : > : Holmes-Farley,
: : : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
: : : > : 6,509,013; 1/21/2003.
: : : > : >
: : : > : > 4. Combination therapy for treating hypercholesterolemia using a bile
: : : acid
: : : > : sequestrant
: : : > : > polymer
: : : > : > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley,
: : : Stephen
: : : > : Randall;
: : : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
: : : > : >
: : : > : > 5. Method for treating hypercholesterolemia with polyallylamine
: : : polymers.
: : : > : Holmes-Farley,
: : : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
: : : Goldberg,
: : : > : Dennis I. , US
: : : > : > 6,423,754; 7/23/2002.
: : : > : >
: : : > : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry, III;
: : : > : Neenan, Thomas X..;
: : : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
: : : > : >
: : : > : > 7. Combination therapy for treating hypercholesterolemia and
: : : > : atherosclerosis. Huval, Chad
: : : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal, Pradeep
: : : K.
: : : > : U.S. 6,365,186;
: : : > : > 4/2/2002.
: : : > : >
: : : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
: : : Mandeville,
: : : > : W. H., III;
: : : > : > Huval; C.
: : : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
: : : > : 10/9/2001.
: : : > : >
: : : > : > 9. Polymers containing guanidinium groups as bile acid sequestrants.
: : : Dhal;
: : : > : P. K.; Holmes-
: : : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
: : : > : >
: : : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
: : : H.,
: : : > : III.; US
: : : > : > 6,281,252;
: : : > : > 8/28/2001.
: : : > : >
: : : > : > 11. Combination therapy for treating hypercholestrolemia. Huval; C.
: : : C.;
: : : > : Holmes-Farley; S.
: : : > : > R. ;
: : : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
: : : > : >
: : : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G. M.;
: : : > : Holmes-Farley, S.
: : : > : > R.; US
: : : > : > 6,264,937; 7/24/2001.
: : : > : >
: : : > : > 13. Method for treating hypercholesterolemia with unsubstituted
: : : > : polydiallylamine polymers.
: : : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
: : : > : 6,248,318;
: : : > : > 6/19/2001.
: : : > : >
: : : > : > 14. Process for removing bile salts from a patient and alkylated
: : : > : compositions therefore.
: : : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355; 5/1/2001.
: : : > : >
: : : > : > 15. Poly(diallylamine)-based bile acid sequestrants. Holmes-Farley, S.
: : : R.;
: : : > : Dhal, P. K.;
: : : > : > Petersen,
: : : > : > J. S.; US 6,203,785; 3/20/2001.
: : : > : >
: : : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.;
: : : Huval,
: : : > : C. C.; US
: : : > : > 6,190,649;
: : : > : > 2/20/2001.
: : : > : >
: : : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
: : : H.,
: : : > : III.; US
: : : > : > 6,177,478;
: : : > : > 1/23/2001.
: : : > : >
: : : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
: : : Holmes-Farley,
: : : > : S. R.;
: : : > : > Mandeville, W.
: : : > : > H., III.; US 6,129,910; 10/10/2000.
: : : > : >
: : : > : > 19. Method for treating hypercholesterolemia with unsubstituted
: : : > : polydiallylamine polymers.
: : : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K. ; US
: : : > : 6,083,497;
: : : > : > 7/4/2000.
: : : > : >
: : : > : > 20. Method of making phosphate-binding polymers for oral
: : : administration.
: : : > : Holmes-Farley, S.
: : : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495;
: : : 7/4/2000.
: : : > : >
: : : > : > 21. Process for removing bile salts from a patient and alkylated
: : : > : compositions therefore.
: : : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
: : : 5/23/2000.
: : : > : >
: : : > : > 22. Process for removing bile salts from a patient and compositions
: : : > : therefor. Mandeville,
: : : > : > W. H.,
: : : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
: : : > : >
: : : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W. H;
: : : > : Neenan; T. X.; Holmes-
: : : > : > Farley; S. R. US 6,034,129; 3/7/2000.
: : : > : >
: : : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville, W.
: : : H.,
: : : > : III.; US
: : : > : > 5,985,938;
: : : > : > 11/16/99.
: : : > : >
: : : > : > 25. Process for removing bile salts from a patient and compositions
: : : > : therefor. Mandeville,
: : : > : > W. H.,
: : : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
: : : > : >
: : : > : > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville, W.
: : : H.,
: : : > : III.;
: : : > : > Holmes-Farley;
: : : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
: : : > : >
: : : > : > 27. Hydrophilic nonamine-containing and amine-containing copolymers
: : : and
: : : > : their use as bile
: : : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
: : : 5,929,184;
: : : > : 7/27/99.
: : : > : >
: : : > : > 28. Interpenetrating polymer networks for sequestration of bile acids.
: : : > : Mandeville, W. H.,
: : : > : > III.;
: : : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US 5,925,379;
: : : > : 7/20/99.
: : : > : >
: : : > : > 29. Amine polymer sequestrant and method of cholesterol depletion.
: : : > : Mandeville, W. H.,
: : : > : > III.;
: : : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
: : : > : >
: : : > : > 30. Process for removing bile salts from a patient and compositions
: : : > : therefor. Mandeville,
: : : > : > W. H.,
: : : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
: : : > : >
: : : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol depletion.
: : : > : Mandeville, W. H.,
: : : > : > III.;
: : : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
: : : > : >
: : : > : > 32. Process for removing bile salts from a patient and compositions
: : : > : therefor. Mandeville,
: : : > : > W. H.,
: : : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
: : : > : >
: : : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
: : : Mandeville,
: : : > : W. H., III.;
: : : > : > Holmes-
: : : > : > Farley, S. R.; US 5,703,188; 12/30/97.
: : : > : >
: : : > : > 34. Oral administration of iron-binding crosslinked amine polymers.
: : : > : Mandeville, W. H.,
: : : > : > III.;
: : : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
: : : > : >
: : : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.; Holmes-Farley,
: : : S.
: : : > : R.; US 5,693,675;
: : : > : > 12/2/97.
: : : > : >
: : : > : > 36. Method for removing bile salts from a patient with alkylated
: : : > : crosslinked amine
: : : > : > polymers,
: : : > : > and preparation of the polymers. Mandeville, W. H., III.;
: : : Holmes-Farley,
: : : > : S. R.; US
: : : > : > 5,679,717; 10/21/97.
: : : > : >
: : : > : > 37. Phosphate-binding polymers for oral administration. Holmes-Farley,
: : : S.
: : : > : R.; Mandeville,
: : : > : > W.
: : : > : > H., III.; US 5,667,775; 9/16/97.
: : : > : >
: : : > : > 38. Ion-exchange process using highly crosslinked polymers for
: : : removing
: : : > : bile salts from a
: : : > : > patient, preparation of the polymers, and compositions containing
: : : them.
: : : > : Mandeville, W. H.,
: : : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
: : : > : >
: : : > : > 39. Hydrophobic amine polymer sequestrant and method of cholesterol
: : : > : depletion. Mandeville,
: : : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530;
: : : 4/8/97.
: : : > : >
: : : > : > 40. Amine polymer sequestrant and method of cholesterol depletion.
: : : > : Mandeville, W. H.,
: : : > : > III.;
: : : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
: : : > : >
: : : > : > 41. Phosphate-binding polymers for oral administration. Holmes-Farley,
: : : S.
: : : > : R.; Mandeville,
: : : > : > W.
: : : > : > H., III.; US 5,496,545; 3/5/96.
: : : > : >
: : : > : > 42. Iron-binding polymers for oral administration. Mandeville, W. H.,
: : : > : III.; Holmes-Farley,
: : : > : > S. R.;
: : : > : > US 5,487,888; 1/30/96.
: : : > : >
: : : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having active
: : : > : hydrogens on the
: : : > : > surface.
: : : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
: : : > : >
: : : > : > 44. Layered sol-gel coatings from organisilicon compounds.
: : : Holmes-Farley,
: : : > : S. R.; Yanyo, L.
: : : > : > C.;
: : : > : > US 5,182,143; 1/26/93.
: : : > : >
: : : > : > 45. Method for metal bonding using ultrathin primer coating.
: : : > : Holmes-Farley, S. R.; Yanyo,
: : : > : > L.
: : : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
: : : > : >
: : : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K. J.;
: : : US
: : : > : 5,096,962;
: : : > : > 3/17/92.
: : : > : >
: : : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
: : : > : elastomer-metal bonding.
: : : > : > Holmes-
: : : > : > Farley, S. R.; US 5,102,956; 4/7/92.
: : : > : >
: : : > : >
: : : > : >
: : : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
: : : > : >
: : : > : >
: : : > : > 1. Aryl boronate functionalized polymers for treating obesity and
: : : > : inhibiting fat uptake.
: : : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal,
: : : Pradeep
: : : > : K.; Huval, Chad
: : : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003), 92
: : : pp. WO
: : : > : 0302571.
: : : > : >
: : : > : > 2. Preparation of aryl boronic acids for treating obesity.
: : : Holmes-Farley,
: : : > : Stephen Randall;
: : : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal, Pradeep
: : : K.
: : : > : (Geltex
: : : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO 0302570.
: : : > : >
: : : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide. Holmes-Farley,
: : : > : Stephen Randall.
: : : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp. WO
: : : > : 0302130.
: : : > : >
: : : > : > 4. Method for reducing copper levels and treating copper toxicosis.
: : : > : Holmes-Farley, Stephen
: : : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2002),
: : : 45
: : : > : pp. WO
: : : > : > 0285383.
: : : > : >
: : : > : > 5. Method for treating gout and binding uric acid. Holmes-Farley,
: : : Stephen
: : : > : Randall; Burke,
: : : > : > Steven K. WO 0285381 10/31/2002.
: : : > : >
: : : > : > 6. Method for treating gout and reducing serum uric acid.
: : : Holmes-Farley,
: : : > : Stephen Randall;
: : : > : > Burke, Steven K WO 0285380 10/31/2002.
: : : > : >
: : : > : > 7. Amine condensation polymer bile acid sequestrants. Huval, C. C.;
: : : > : Holmes-Farley, S. R.;
: : : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
: : : > : >
: : : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III and
: : : > : Holmes-Farley, S.
: : : > : > R.;
: : : > : > WO 1999-US5662; 9/23/1999.
: : : > : >
: : : > : > 9. Amine-containing copolymers as bile acid sequestrants.
: : : Holmes-Farley,
: : : > : S. R.; Petersen,
: : : > : > J. S.;
: : : > : > WO 9933452; 7/8/1999.
: : : > : >
: : : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H., III
: : : and
: : : > : Holmes-Farley, S.
: : : > : > R.;
: : : > : > WO 9922743; 5/14/1999.
: : : > : >
: : : > : > 11. Polyallylamine polymers for removing bile salts and treating
: : : > : hypercholesterolemia, and
: : : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III;
: : : Burke,
: : : > : S. K.; Goldberg,
: : : > : > D. I.; WO 9857652; 12/23/98.
: : : > : >
: : : > : > 12. Phosphate-bidning polymers combined with a calcium supplement for
: : : oral
: : : > : administration.
: : : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III; Holmes-Farley,
: : : S.
: : : > : R.; WO 9842355;
: : : > : > 10/1/98.
: : : > : >
: : : > : > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
: : : > : depletion. Mandeville,
: : : > : > W.
: : : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449; 12/12/96.
: : : > : >
: : : > : > 14. Process for adjusting ion concentration in a patient and
: : : compositions
: : : > : therefor.
: : : > : > Mandeville,
: : : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
: : : > : >
: : : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
: : : interlayer
: : : > : for improved
: : : > : > metal-
: : : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
: : : 1/20/94.
: : : > : >
: : : > : > 16. Process for increased metal-substrate bond strength in metalized
: : : > : plastics.
: : : > : > Holmes-Farley, S.
: : : > : > R.; Ger. Offen. 4322516; 7/6/93.
: : : > : >
: : : > : > 17. Electrorheological fluids and preparation of particles useful in
: : : the
: : : > : fluids.
: : : > : > Troughton,
: : : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson, J.
: : : > : David; Bares, Joseph
: : : > : > E.;
: : : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell. EP
: : : > : 394049;
: : : > : > 10/24/1990.
: : : > : >
: : : > : > JOURNAL PUBLICATIONS
: : : > : >
: : : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov,
: : : Eugene;
: : : > : Guo, Amy;
: : : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
: : : > : Mandeville, W. Harry;
: : : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
: : : 611-619.
: : : > : >
: : : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
: : : synthesis
: : : > : and biological
: : : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S.
: : : Randall;
: : : > : Mandeville, W.
: : : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep K.
: : : > : Journal of
: : : > : > Macromolecular Science, Pure and Applied Chemistry (2001), A38(12),
: : : > : 1559-1574.
: : : > : >
: : : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by Molecular
: : : > : Imprinting. Huval,
: : : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley, S.
: : : > : Randall; Mandeville,
: : : > : > W.
: : : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro, Robert
: : : J.;
: : : > : Chen, Xi; Dhal,
: : : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
: : : > : >
: : : > : > 4. Synthetic polymers for the binding of fat in the intestinal tract.
: : : > : Jozefiak, Thomas H.;
: : : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia;
: : : Huval,
: : : > : Chad C.;
: : : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
: : : > : Abstracts of
: : : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United States, August
: : : > : 26-30, 2001
: : : > : > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
: : : > : Division of
: : : > : > Polymer Chemistry) (2001), 42(2), 98.
: : : > : >
: : : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel polymer
: : : gel
: : : > : pharmaceutical.
: : : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen, J.;
: : : Ward,
: : : > : J.; Sacchiero,
: : : > : > B.;
: : : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K. A.;
: : : Chen,
: : : > : X.; Mazzeo, J.
: : : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
: : : > : >
: : : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl and
: : : other
: : : > : bile acid
: : : > : > sequestrants.
: : : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu, Q.;
: : : > : Hook, P.; Holmes-
: : : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1), 708-709.
: : : > : >
: : : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
: : : Holmes-Farley,
: : : > : S. R; Polym.
: : : > : > Mater. Sci. Eng (1999), 80, 246-247.
: : : > : >
: : : > : > 8. Design and characterization of of Sevelamer Hydrochloride: a novel
: : : > : phosphate-binding
: : : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III; Ward,
: : : J.;
: : : > : Miller, K. L.;
: : : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.- Pure
: : : and
: : : > : Appl. Chem.,
: : : > : > A36(7&8), p. 1085 (1999).
: : : > : >
: : : > : > 9. Three generations of bile acid sequestrants. Mandeville, W. H.,
: : : III;
: : : > : Braunlin, W.;
: : : > : > Dhal, P.;
: : : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
: : : > : Rosenbaum, D.;
: : : > : > Sacchiero,
: : : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc. (1999),
: : : > : 550, 3-15.
: : : > : >
: : : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric
: : : phosphate
: : : > : binder, on
: : : > : > urinary
: : : > : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S. R.;
: : : > : Mandeville, W. H.,
: : : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial., Transplant.
: : : > : (1997), 12(5)
: : : > : > 961-964.
: : : > : >
: : : > : > 11. Thin anisotropic coatings based on sol-gel technology.
: : : Holmes-Farley,
: : : > : S. R.; Yanyo, L.
: : : > : > C;
: : : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4),
: : : 439-444.
: : : > : >
: : : > : > 12. The mechanism of cure initiation of a surface activated adhesive.
: : : > : Holmes-Farley, S.
: : : > : > R.;
: : : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
: : : > : >
: : : > : > 13. Adhesion promotion and corrosion prevention using thin anisotropic
: : : > : coatings. Holmes-
: : : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
: : : > : 131-151.
: : : > : >
: : : > : > 14. Wetting of functionalized polyethylene having ionizable organic
: : : acids
: : : > : and bases at the
: : : > : > polymer-water interface: relations between functional group polarity,
: : : > : extent of
: : : > : > ionization,
: : : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
: : : > : Whitesides, G. M.;
: : : > : > Langmuir
: : : > : > (1988), 4(4), 921-937.
: : : > : >
: : : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with a
: : : > : single hydroxy group.
: : : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
: : : > : >
: : : > : > 16. Reconstruction of the interface of oxidatively functionalized
: : : > : polyethylene (PE-CO2H)
: : : > : > and
: : : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.; Nuzzo,
: : : R.;
: : : > : McCarthy, T. J.;
: : : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report
: : : (1987),
: : : > : AD-
: : : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
: : : > : >
: : : > : > 17. Surface-modified polyethylene film: the relationship between
: : : surface
: : : > : chemistry and
: : : > : > physical
: : : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11),
: : : 4537.
: : : > : >
: : : > : > 18. Reactivity of carboxylic acid and ester groups in the
: : : functionalized
: : : > : interfacial
: : : > : > region of
: : : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
: : : > : differentiation of the
: : : > : > functional groups into shallow and deep subsets based on a comparison
: : : of
: : : > : contact angle and
: : : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.; Langmuir
: : : > : (1987), 3(1), 62-
: : : > : > 76.
: : : > : >
: : : > : > 19. Fluorescence properties of dansyl groups covalently bonded tot he
: : : > : surface of
: : : > : > oxidatively
: : : > : > functionalized low-density polyethylene film. Holmes-Farley, S. R.;
: : : > : Whitesides, G. M.;
: : : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
: : : > : AD-A162435/2/GAR,
: : : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
: : : > : >
: : : > : > 20. Acid-base behavior of carboxylic acid groups covalently attached
: : : at
: : : > : the surface of
: : : > : > polyethylene: The usefulness of contact angle in following the
: : : ionization
: : : > : of surface
: : : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T. J.;
: : : > : Deutch, J.;
: : : > : > Whitesides,
: : : > : > G. M.; Langmuir (1985), 1(6), 725-740.
: : : > : >
: : : > : > 21. The thermal stability of a surface modified solid organic polymer.
: : : > : Holmes-Farley, S.
: : : > : > R.;
: : : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
: : : > : >
: : : > : >
: : : > : >
: : : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
: : : > : >
: : : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R. Advanced
: : : > : Aquarist. June 2003.
: : : > : >
: : : > : > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley, R.
: : : > : Advanced Aquarist.
: : : > : > May
: : : > : > 2003.
: : : > : >
: : : > : > 3. The Degradation of Limewater (Kalkwasser) in Air. Holmes-Farley, R.
: : : > : Reefkeeping May
: : : > : > 2003.
: : : > : >
: : : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R. Reefkeeping
: : : > : April 2003.
: : : > : >
: : : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
: : : > : Holmes-Farley, R.
: : : > : > Advanced Aquarist; April 2003.
: : : > : >
: : : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
: : : > : Holmes-Farley, R.
: : : > : > Advanced Aquarist; April 2003.
: : : > : >
: : : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced
: : : Aquarist;
: : : > : March 2003.
: : : > : >
: : : > : > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
: : : > : Holmes-Farley, R.
: : : > : > Advanced Aquarist; February 2003.
: : : > : >
: : : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist; January
: : : > : 2003.
: : : > : >
: : : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
: : : December
: : : > : 2002.
: : : > : >
: : : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
: : : Advanced
: : : > : Aquarist; November
: : : > : > 2002.
: : : > : >
: : : > : > 12. Iron: A Look at Organisms Other than Macroalgae. Holmes-Farley, R.
: : : > : Advanced Aquarist;
: : : > : > November 2002.
: : : > : >
: : : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced
: : : Aquarist,
: : : > : September 2002.
: : : > : >
: : : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist, August
: : : > : 2002.
: : : > : >
: : : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com, April
: : : > : 2002.
: : : > : >
: : : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
: : : > : Aquarist; July 2002
: : : > : >
: : : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist;
: : : June
: : : > : 2002.
: : : > : >
: : : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R.
: : : Advanced
: : : > : Aquarist, May
: : : > : > 2002.
: : : > : >
: : : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in Corals.
: : : > : Holmes-Farley, R.
: : : > : > Advanced Aquarist, April 2002.
: : : > : >
: : : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
: : : > : >
: : : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February 2002.
: : : > : >
: : : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January
: : : 2002.
: : : > : >
: : : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium Frontiers
: : : > : 2000.
: : : > : >
: : : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
: : : > : Frontiers 2000.
: : : > : >
: : : > : > 25. Phosphate..What is it and why should you care. Holmes-Farley, R.
: : : > : Aquarium Frontiers
: : : > : > 2000.
: : : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
: : : Frontiers
: : : > : 2000.
: : : > : >
: : : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers
: : : 2000.
: : : > : >
: : : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers 1999.
: : : > : >
: : : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
: : : > : >
: : : > : >
: : : > : >
: : : > : >
: : : > : >
: : : > : >
: : : > : >
: : : > : > Boomer
: : : > : >
: : : > : > Want to talk chemistry ? The Reef Chemistry Forum
: : : > : > http://www.reefcentral.com/vbulletin/index.php
: : : > : >
: : : > : > Want to See More ?
: : : > : > Please Join Our Growing Membership
: : : > : > www.coralrealm.com
: : : > : >
: : : > : >
: : : > : >
: : : > :
: : : > :
: : : >
: : : >
: : :
: : :
: : :
: :
: :
:
:

[stoutman]

> Humm, since when does Alk have anything to do in regards to the addition
of BASE.

You tell me. Your the one that posted a link to a web page that had this
definition of alkalinity. Looks like you put yourself in your own hole pal.

Remember posting this link:

http://www.waterontheweb.org/resources/glossary.html

Here is the definition of alkalinity from the web page YOU cited. (I
recommend you read the web pages you are citing before you cite them)
Alkalinity:
Acid neutralizing or buffering capacity of water; a measure of the ability
of water to resist changes in pH caused by the addition of acids or BASES.


> It sure is funny how all of the chemist that write water chemistry
textbooks never say Alk
> is the Buffering Capacity of a solution.

Neither did I. I said (for the umpth teen time) Alkalinity is a
measurement of BUFFERING CAPACITY.

When you measure alkalinity you know your BUFFERING CAPACITY (if you know
your pH). Its a two for one.

SEE MY OTHER POST FROM TODAY.



"Boomer" > wrote in message
...
>
> "I am not sure if you are just messing with me "
>
> Yes, messing with you, it is called trolling a troll, to see where the
hell you would go
> and what you would say in regards to last posts. It is called honesty, of
which you have
> none off to say the least,that I can see.You always like to post what
suits you and just
> avoid ref I give. So lets start where you are WRONG and have a great lack
of understanding
> of things, to include pointing out all your gross error which you still
FAIL to
> acknowledge and which can be prove in many water chem. ref. .I doubt like
hell you are a
> chemist at all.You seem to want to con people into thinkin' you are. But
then again, I
> have seen chemists like you before, they are not familiar with the, but
they ASK to have
> it explained and ask for REF.YOU just shoot from the hip. WHAT GETS YOU IN
TROUBLE. You
> remind me of snoot-noise kid that come here and other NG's and
forums...that think they
> know, buy hey, maybe I'm wrong :-)
>
>
>
> 1). Acidity
>
> "***Benjamin,Water Chemistry (2002, pages 262-263).***
>
> ***Acidity A concept that is exactly analogous to alkalinity but measures
the base
> neutralizing
> capacity (BNC) of a solution is Acidity. The quantitative represents the
concentration of
> OH- ions that must be added to titrate the solution to a pH near 10.5***
>
> So that means that not only in Benjamin wrong but, so are Stumm & Morgan,
Millero, Pilosn,
> Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I
said, you have your
> acidity and Acidy mixed up. Acidity as defined above is covered in most
water chemistry
> books, written by chemists, who's field of expertise is water chemistry.
You can even buy
> Acidity test kits from, HACH, LaMotte, etc..
>
> You mean you didn't read this or are you just avoiding it .The same
definition can be
> found in almost any std water chemistry book.
>
> I have run into few chemists, that are NOT familiar with the above. Some
water reports
> require the above Acidity measuring. The issue with you is you do not
understand WATER
> CHEMISTRY. Everything you have posted can be found a general chemistry
book
>
>
>
>
> 2) Alk and BC
>
> From the link
>
> Alkalinity
> ***Acid neutralizing or buffering capacity of water; a measure of the
ability of water to
> resist changes in pH caused by the addition of acids or bases ***
>
> This is a Buffering Capacity definition not Alk
>
> Humm, since when does Alk have anything to do in regards to the addition
of BASE. As I
> pointed out in the first post the term is often miss used. Even in YOUR
own posts you say
> it is based on a acid addition, no mention of **base or acid** addition
by you. Are you
> getting confused or what. Or is more you are trying to confuse everyone
you are right. The
> above is a definition for Buffer Capacity NOT Alk
>
> From Drew, Geochemistry of Natural Waters
>
> "alkalinity, which is formally defined as the equivalent sum of bases that
are titratable
> with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH of
the solution is
> progressively lowered by the addition of a strong acid (HCL), all the
anions on the right
> will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4, H2S,organic
acids, H20)"
>
> This follows almost all description of Alk, that it is acid neutralizing
reaction and has
> nothing to do with base neutralizing, which is Acidity (BNC) .I defined
these before you
> had no comment
>
>
> Even the links that give the Buffering Capacity definition is wrong, as is
the UIPAC on
> Alkalinity. Alkalinity has nothing to do with the addition of bases only
acids. When you
> use the words "base and acid" it becomes BC
>
> Even YOU MUST disagree with these definitions, from YOUR own post
>
> Think of alkalinity as 'buffering capacity'. Or the ability of a solution
> ***to resist a drop in pH due to the addition of acid***
>
> Where the flip is the base addition forget it ?
>
> From Butler; Carbon Dioxide Equilibrium and Their Applications (professor
emeritus
> Harvard University) an expert on the subject.
>
> Buffering Index (Buffering Capacity, Buffer Intensity).
>
> ***This concept was first developed for mixtures of approximately equal
proportions of
> conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such
buffer solutions
> strongly resist changes in pH when acids or bases are added and are useful
as pH
> standards. The Buffer Index tells how great the resistance to pH changes
will be.**
>
> also from Butler
>
> Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
>
> Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
>
> Acidity is in fact just the negative of Alkalinity ***
>
> http://www.lagoonsonline.com/acid.htm
>
>
http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.h
tm?E+mystore
>
> It sure is funny how all of the chemist that write water chemistry
textbooks never say Alk
> is the Buffering Capacity of a solution. They are always treated and
defined separately.
>
> If you or others choose to treat Alk and BC as the same, well, just have
at it. As I said
> in first post I know what you mean.
>
> "No need to cite web pages that describe what I know and what I wrote
> in this discussion"
>
> No you don't know, who are you trying to convince any way, me, the guys
here and/or all
> the water chemists in this world. As I said before go get a dam WATER
CHEMISTRY book or
> shut the hell up.You keep trying to define things from a general chemistry
book WE ARE IN
> THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
>
>
>
>
>
> 3). pKa's and what you don't know or seem to be confused on
>
> "Therefore, it has two pKa's
> (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
The
> pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> right in there. Is that magic? :)"
>
> Here it is agin that is twice at least
>
> "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this
example)
> you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium will
> be shifted to HCO3-2 by a ratio of 1:100.
>
> Oh wait , there is a third time LOL
>
> "At the pH of seawater, the buffering capacity of carbonate is at it's
> weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
>
>
> Lets just dunk you on this one. I am taking note you refuse to reply to
YOUR errors
>
> So you calculated the pH of seawater with freshwater pKa's, now that is a
good trick. From
> a number of seawater chemistry books the seawater pKa's are 6 & 9.1, so
according to you,
> seemingly not understanding your favorite Henderson-Hasselbach equation;
>
> 2 pH = (6 + 9.1) /2 pH = 7.55
>
> I have never seen seawater with a pH of 7.55. There is no ocean with that
pH. Humm how
> come your equation is not working for you today.?
>
>
> "That pH I calculated is
> right in there. Is that magic? :)"
>
> I roll on the floor when I see this = 8.35
>
> Hum , just a brain far so excuse me for thinkin
>
> (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
>
> Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a pH of
8.35 there pal
> ? That 8.35 is what you are telling people the pH should be, but their
meter says 6.4.
> This how people will READ this.
>
>
>
>
> 4.) More on Buffering Capacity
>
> "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes, your
> alkalinity equation."'
>
>
> Yup, I see that and in this case the HCO3 is the acid and the CO3 is the
base CORRECT. In
> Alk you are only dealing with bases and how they react to an acid. Acidity
deals acids and
> how they recact to bases "Acidity, A concept that is exactly analogous to
alkalinity but
> measures the base neutralizing
> capacity (BNC) of a solution is Acidity "Alk is the ANC Acid neutralizing
capacity
>
> "Don't the components of a buffer account for the buffering capacity? "
>
> Yes, they do but so do the acids which work as buffers. NaHCO3 is a buffer
and can act as
> an acid or base
>
> *** Buffering Capacity.**
> The power of a substance in solution to absorb acid or alkali without
change in pH; this
> is highest at a pH value equal to the pKa value of the acid of the buffer
pair.***
>
> ***Akalinity***
> Measure of the power of a solution to neutralise hydrogen ions (H+),
usually expressed as
> the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
>
>
> If one wants to call Alk Buffering capacity then one sure as a hell can
call Acidty
> Buffering Capacity also. As it is the ability to neutralizes an acid that
is a buffer.You
> have a pH of 7 and you add a buffer to lower it to a pH of 4, you are
buffering the water,
> that buffer is a acid.
>
> 5) CO2
>
> You are really confuse so it seems :-) You realllllllly indicate that CO2
is affected by
> the Alk or vise-versa
>
> "Yes, the pH will drop with the addition of CO2. Remove CO2 will cause
the
> pH to rise? How do you remove CO2? Once it is in solution it forms
> carbonic acid and neutralizes some of your 'buffer'."
>
> "With the exception of CO2?"
>
> No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
> Concepts)....PERIOD.You seem to think a that at least in two of your post
that CO2 is
> affected by the Alk or vise-versa. Please go back to school or seek
professor
>
> "Why in one case does CO2 from air lower pH and in the other case it
raises
> it? Doesn't make sense."
>
> That is because you don't understand CO2 period. By the way I saved this,
wanted to see
> if you would bite on the post I gave. Not bite at first, so time to reel
you in, as you
> did bite in another post..
>
> Lets make some sense of it for you, being that you have a pH.D in
chemistry, so you say .
>
> CO2 is naturally generated in a aquatic systems, it is capable of raise to
various levels
> depending on a number of circumstances .It can be measure (except in
seawater) or
> calculated using Buch/Park Equations (what we use for seawater. In sort if
you know the pH
> and Alk you can calculate the CO2). If you aerate a system or a sample of
water, even if
> the pH has only dropped a couple of tenths, due to an increase in CO2, the
CO2 will leave
> solution to the atmosphere.This will raise the pH. On the other hand if
theCO2 level is
> more of the norm and you have hikgh room air, such as in the winter, the
partial pressure
> of the CO2 in air will be much higher than that in water, in which case
the CO2 will enter
> the water and lower the pH. That is without an airstone. Adding an
airstone will make it
> even worse,as you are now forcefully driving the CO2 into solution even
quicker. These
> test /experiments have been proven many times, it is not that may work
could work they do
> work.Yet you want to disagree and in another post say you haven't tried
it,.Seems to me
> that based on what you say it can't work So, in short you don't know what
the hell you are
> taking about. Go get a glass of seawater with a pH of about 8.3 and lower
it to about
> 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK- UP
( that is if you
> don't have a high room air CO2 problem.). This little test has been done
thousands of
> times in this hobby, with test kits, pH meters and even graphic printers.
>
> "This is where Boomer and I
> disagree. I say you would have to lower the pH very low in order to
> effectively remove CO2 by purging."
>
> You are 100 % wrong. Please come to our Chem forum and try and run that by
Randy, don't
> take my word on it. I already know what he will say.
>
> "Boomer didnt convince me it
> works at the pH of an aquarium, but I never tried it and I'm not sure of
> this. "
>
> Well then come too our chem. forum and tell Randy he doesn't know what he
is talking about
> LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it
should be easy for
> you to run the experiment LOL There are grade school kids that run the
test and know what
> happens and that I'm correct.
>
>
> "The equilibrium is a FUNCTION
> of pH."
>
> It is also a function of Alk or don't you know that. At a pH of 8.3, Alk
2.25, the CO2 is
> about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk to
about .4 meq/ l
> or so the CO2 will be around .99 mg / l CO2, When dealing with tanksCO2 is
not always in
> equilibrium with ambient air.
>
>
> ". But I wouldn't degas a solution of a
> specific gas (CO2) with a gas (this case he was using air) that contains
the
> same gas I am trying to purge."
>
> Why not ? We have a guy right now that is running tests on purging ambient
air with a
> solution to remove CO2 gas from the air, before it enters the tank
per/Randy's suggestion.
> The same guy is doing some of my test using a Clinoptilolite, a Zeolite
mineral, that has
> an affinity for CO2.This will be a dry CO2 scrubber
>
>
> Sorry Soutman but you sure as hell don't seem to know much about aquatic
chemistry. You
> seem to be guessing at everything.
>
> By the way have you read any of Randy's technical articles on water
chemistry, been saving
> these for last. There are a few on pH, Alk, CO2 .Here is a list
>
> Try and answer them 1-5 and lets see where we get THIS TIME :-) or maybe
we should just
> drop it. I could care less at this point.
>
> THE END
>
>
> ARTICLES
>
> The first two posts in this thread are lists of some of my articles that
relate to reef
> tank chemistry. In the next few posts are some of the articles published
by Craig Bingman
> and others on reef chemistry issues.
>
> The first two posts in this thread are lists of some of my articles that
relate to reef
> tank chemistry. In the next few posts are some of the articles published
by Craig Bingman
> and others on reef chemistry issues.
>
> Solving Common Problems
>
> Solving Calcium and Alkalinity Problems
> http://www.advancedaquarist.com/issues/nov2002/chem.htm
>
> Solutions to pH Problems
> http://www.advancedaquarist.com/iss...ne2002/chem.htm
>
> How to Select a Calcium and Alkalinity Supplementation Scheme
> http://www.advancedaquarist.com/issues/feb2003/chem.htm
>
> Phosphate Issues
> http://www.advancedaquarist.com/iss...pt2002/chem.htm
>
> Nitrate Issues
> http://www.advancedaquarist.com/iss...st2003/chem.htm
>
>
>
> Calcium and Alkalinity
>
> Solving Calcium and Alkalinity Problems
> http://www.advancedaquarist.com/issues/nov2002/chem.htm
>
> How to Select a Calcium and Alkalinity Supplementation Scheme
> http://www.advancedaquarist.com/issues/feb2003/chem.htm
>
> Calcium and Alkalinity Balance Issues
> http://reefkeeping.com/issues/2002-...ature/index.htm
>
> Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
> http://www.advancedaquarist.com/iss...ly2002/chem.htm
>
> The Relationship Between Alkalinity and pH.
> http://www.advancedaquarist.com/issues/may2002/chem.htm
>
> The Chemical & Biochemical Mechanisms of Calcification in Corals
> http://www.advancedaquarist.com/issues/apr2002/chem.htm
>
> Calcium
> http://www.advancedaquarist.com/issues/mar2002/chem.htm
>
> Alkalinity
> http://www.advancedaquarist.com/iss...2/chemistry.htm
>
>
> Iron
>
> First Iron Article: Macroalgae and Dosing Recommendations
> http://www.advancedaquarist.com/issues/aug2002/chem.htm
>
> Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> http://www.advancedaquarist.com/issues/oct2002/chem.htm
>
> Iodine
>
> Iodine in Marine Aquaria: Part I
> http://www.advancedaquarist.com/issues/mar2003/chem.htm
>
> Iodine in Reef Tanks 2: Effects on Macroalgae Growth
> http://www.advancedaquarist.com/iss...il2003/chem.htm
>
>
> Magnesium and Strontium
>
> Strontium
> http://www.advancedaquarist.com/issues/nov2003/chem.htm
>
> Magnesium
> http://www.advancedaquarist.com/issues/oct2003/chem.htm
>
> Magnesium and Strontium in Limewater
> http://www.advancedaquarist.com/issues/dec2003/chem.htm
>
>
> Limewater (kalkwasser)
>
> The Self Purification of Limewater (Kalkwasser)
> http://www.advancedaquarist.com/issues/may2003/chem.htm
>
> The Degradation of Limewater (Kalkwasser) in Air
> http://reefkeeping.com/issues/2003-...ature/index.htm
>
> How to Select a Calcium and Alkalinity Supplementation Scheme
> http://www.advancedaquarist.com/issues/feb2003/chem.htm
>
> Metals in Aquaria
>
> Aluminum and aluminum-based phosphate binders
> http://www.advancedaquarist.com/iss...ly2003/chem.htm
>
> Reef Aquaria with Low Soluble Metals
> http://reefkeeping.com/issues/2003-...ature/index.htm
>
> Tap Water in Reef Aquaria
> http://www.advancedaquarist.com/issues/jan2004/chem.htm
> First Iron Article: Macroalgae and Dosing Recommendations
> http://www.advancedaquarist.com/issues/aug2002/chem.htm
>
> Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> http://www.advancedaquarist.com/issues/oct2002/chem.htm
>
>
> Test Kit Reviews
>
> The Seachem Borate Alkalinity Test Kit
> http://www.advancedaquarist.com/iss...ne2003/chem.htm
>
> The Salifert Boron Test Kit
> http://www.advancedaquarist.com/iss...pt2003/chem.htm
>
> Boron and Borate (and pH buffering)
>
> Boron in a Reef Tank (and its effect on pH buffering)
> http://www.advancedaquarist.com/issues/dec2002/chem.htm
>
> The Seachem Borate Alkalinity Test Kit
> http://www.advancedaquarist.com/iss...ne2003/chem.htm
>
> The Salifert Boron Test Kit
> http://www.advancedaquarist.com/iss...pt2003/chem.htm
>
>
>
> Others
>
> Tap Water in Reef Aquaria
> http://www.advancedaquarist.com/issues/jan2004/chem.htm
>
> ORP
> http://reefkeeping.com/issues/2003-...ature/index.htm
>
> Chloramine
> http://reefkeeping.com/issues/2003-...ature/index.htm
>
> Silica in a Reef Tank
> http://advancedaquarist.com/issues/jan2003/feature.htm
>
> Specific Gravity (and temperature correction of hydrometers)
> http://www.advancedaquarist.com/iss...2/chemistry.htm
>
>
> The Complete Nitrogen Cycle
> http://www.animalnetwork.com/fish/l...a&RecordNo=3090
>
> Magnesium (older article with fonts screwed up)
> http://www.aquariumfish.com/aquariu...cid=124&search=
>
> Phosphate (older article now reproduced in a poor fashion)
> http://www.aquariumfish.com/aquariu...cid=124&search=
>
> Carbon Dioxide
> http://www.animalnetwork.com/fish/l...a&RecordNo=2074
>
> Using Conductivity to Measure Salinity
> http://www.aquariumfish.com/aquariu...cid=124&search=
>
> Understanding Seawater
> http://www.animalnetwork.com/fish2/...s/1/default.asp
>
> Protein Skimming: How It Works
> http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
>
>
>
> Articles by Craig Bingman:
>
> Carbon Dioxide tests
> http://www.animalnetwork.com/fish/l...n=&RecordNo=279
>
> Limewater, Acetic Acid and Sand Clumping
> http://www.animalnetwork.com/fish/l...n=&RecordNo=181
>
> Calcium and Alkalinity
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Calculation of Calcium Carbonate Saturation States in Reef Aquaria
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
>
> Calcification Rates in Several Tropical Coral Reef Aquaria
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Limits To Limewater...Revisited
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Expanding the Limits of Limewater: Adding Organic Carbon Sources (vinegar)
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
>
> Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Magnesium - Part I
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Magnesium - Part II
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> A Homemade Magnesium Supplement
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Simulating the Effect of Calcium Chloride and Sodium Bicarbonate Additions
on Reef Systems
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Additional Simulations: The Combined Effect Of Calcium Chloride
> /Sodium Bicarbonate Additions And Water Exchanges
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
>
> More articles by Craig Bingman:
>
> The Halogens - Part I: Bromine in Seawater and Aquaria
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> The Halogens - Part II: Fluoride
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Fluoride Depletion In Four Reef Aquariums
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> The Halogens - Part III: Iodine
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Measuring Halides
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> How Test Kits Work
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Borax pH Calibration
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> A pH Detective Story
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> How to Mix a Batch of Synthetic Seawater in Under Five Minutes
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
> SILICON - FOE OR FRIEND?
> http://www.animalnetwork.com/fish2/...s/1/default.asp
>
> The Composition Of Several Synthetic Seawater Mixes
> http://www.animalnetwork.com/fish2/...s/1/default.asp
>
> Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
> http://www.animalnetwork.com/fish2/...bio/default.asp
>
>
>
> Andy's calcium calculator
> http://www.andy-hipkiss.co.uk/cacalc.htm
>
> Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
> http://www.aquariumfish.com/aquariu...cid=124&search=
>
> Calcium Reactor Substrate -- Phosphate Levels
> by Greg Hiller
> http://www.advancedaquarist.com/iss...l2003/short.htm
>
>
> Indoor CO2 Problems
> http://www.advancedaquarist.com/iss...r2002/short.htm
>
> Simon Huntington's CaCO3/CO2 reactor article
>
> http://reefkeeping.com/issues/2002-...ature/index.htm
>
> Ron Shimek's Tank Water Analysis Article
> http://reefkeeping.com/issues/2002-...ature/index.htm
>
>
>
>
> Home made salinity standards thread:
>
> http://reefcentral.com/forums/showt...?threadid=65509
>
> Reef Chemicals Calculator
> http://www.kademani.com/reefchem.htm
>
>
>
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
>
> Former US Army Bomb Technician (EOD)
> Member; IABTI, NATEODA, WEODF, ISEE & IPS
>
> If You See Me Running You Better Catch-Up
>
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message
news:aGuWb.148227$U%5.676753@attbi_s03...
> : Boomer,
> :
> : I am not sure if you are just messing with me or if you are truly
confused.
> : I hope the latter. Please read from Top to Bottom.
> :
> :
> : From YOUR first link:
> :
> : http://www.waterontheweb.org/resources/glossary.html
> :
> : Acidity:
> : A measure of how acid a solution may be. A solution with a pH of less
than
> : 7.0 is considered acidic. Solutions with a pH of less than 4.5 contain
> : mineral acidity (due to strong inorganic acids), while a solution having
a
> : pH greater than 8.3 contains no acidity.
> :
> : Yes,
> :
> : Good definition (for the most part). pH <7 is indeed acidic. pH > 7 is
> : basic. Your web page had a definition for acidity, but not basicity.
> : Strange. That's like defining GOOD and not defining BAD.
> :
> : Here is the IUPAC (International Union of Pure and Applied Chemistry)
> : definition of acidity:
> :
> : http://www.chem.qmul.ac.uk/iupac/index.html
> :
> : acidity
> :
> : (1) Of a compound:
> :
> : For Brønsted acids it means the tendency of a compound to act as a
hydron
> : donor. It can be quantitatively expressed by the acid dissociation
constant
> : of the compound in water or some other specified medium. For Lewis acids
it
> : relates to the association constants of Lewis adducts and -adducts.
> :
> : (2) Of a medium:
> :
> : The use of the term is mainly restricted to a medium containing Brønsted
> : acids, where it means the tendency of the medium to hydronate a specific
> : reference base
> :
> : basicity
> :
> : For Brønsted bases it means the tendency of a compound to act as hydron
> : (proton) acceptor. The basicity of a chemical species is normally
expressed
> : by the acidity of the conjugate acid (see conjugate acid-base pair). For
> : Lewis bases it relates to the association constants of Lewis adducts
> : and -adducts
> :
> :
> :
> : Another definition from the same web page YOU cited: (this is the same
web
> : page you cited above)
> :
> : Alkalinity:
> : Acid neutralizing or buffering capacity of water; a measure of the
ability
> : of water to resist changes in pH caused by the addition of acids or
bases
> : and therefore, the main indicator of susceptibility to acid rain; in
natural
> : waters it is due primarily to the presence of bicarbonates, carbonates
and
> : to a much lesser extent occasionally borates, silicates and phosphates.
It
> : is expressed in units of milligrams per liter (mg/l) of CaCO3 (calcium
> : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l = 1
mg/l
> : of CaCO3. A solution having a pH below about 5 contains no alkalinity.
> :
> : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and says
> : that alkalinity is the measure of ...(description of a buffer)
> :
> : A BUFFER IS : a measure of the ability of water to resist changes in pH
> : caused by the addition of acids or bases (from definition below)
> :
> :
> : I said:
> : ***alkalinity is a measurement of 'buffering capacity'***
> :
> : You said:
> : ***Alkalinity is not a measurement of BC
> :
> : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is not
> : logical.
> :
> : (THIS FROM THE SAME WEB PAGE YOU CITED):
> :
> : Buffer:
> : A substance which tends to keep pH levels fairly constant when acids or
> : bases are added.
> :
> : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
> :
> : a measure of the ability of water to resist changes in pH caused by the
> : addition of acids or bases
> :
> : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A BUFFER.
> :
> :
> : I went to all four links. None contradict what I have said. But the
first
> : one you cited contradicts YOU!
> :
> : I know what a buffer is. I know what acidity means. I know what
alkalinity
> : means. No need to cite web pages that describe what I know and what I
wrote
> : in this discussion. Show me one that says alkalinity is not a measure
of
> : buffering capacity from a credible source.
> :
> :
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > Alkalinity a measure of the amount of anions of weak acid in water and
of
> : the cations
> : > balanced against them
> : > Take note it says ***acid***
> : >
> : > Buffering capacity the ability of a solution to resist or dampen
changes
> : in pH upon the
> : > addition of acids or bases.
> : > Take note its says ***the addition of acids or bases***
> : >
> : > One more
> : >
> : > http://www.waterontheweb.org/resources/glossary.html
> : >
> : > We could go on like this all day, so what is the point ?
> : >
> : > You will LOVE this one
> : > http://www.kyantec.com/Tips/phbuffering.htm
> : >
> : > Don't you just lovbe PDF's
> : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
> : >
> : > Don't fall out of your chair
> : > http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
> : >
> : >
> : >
> : >
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : > "stoutman" <.@.> wrote in message
news:XB7Wb.19339$QA2.62332@attbi_s52...
> : > : Man here is another, google is a wonderful thing. I'm not filtering
any
> : > : out, just posting what I find by GOOGLING for you.
> : > :
> : > : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> : > :
> : > :
> : > : Wow, a gov link. Even the government is wrong, this must be a
> : conspiracy
> : > : against Boomer.
> : > :
> : > :
> : > :
> : > :
> : > : "Boomer" > wrote in message
> : > : ...
> : > : > Now I am getting bored
> : > : >
> : > : > "Don't the components of a buffer account for the buffering
capacity?
> : > : Yes."
> : > : >
> : > : > Yes, agreed but you seem to fail what I'm saying. Buffering
Capacity
> : and
> : > : Alkalinity are
> : > : > not the same, that has always been the issue. I gave the equation
does
> : > : that look like an
> : > : > Alkalinity equation or how Alk is determined. I see you had now
> : comments
> : > : on it what's
> : > : > wrong, why no comments on the equations I gave. Don't understand
them
> : or
> : > : what ? Again this
> : > : > is the equation for Buffering Capacity, also called Buffer Index
or
> : Buffer
> : > : Intensity. It
> : > : > is defined in most water chemistry and chemical oceanography text
> : books.
> : > : >
> : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] +
> : CKa
> : > : [H3O+] / (Ka =
> : > : > H3O+])² )
> : > : >
> : > : > This is not Alkalinity now is it ?
> : > : >
> : > : > "I know how to do a titration, In fact I have done several. How
many
> : have
> : > : > you actually done? I don't mean by counting drops, I mean with a
> : buret?"
> : > : >
> : > : > Well good for you, I use a Digital Titrator
> : > : >
> : > : > "Oh, I see,
> : > : > you think acidity is the opposite of alkalinity. In the world of
> : > : CHEMISTRY
> : > : > it's not. Maybe in aquarium newsgroups it is.
> : > : >
> : > : > Hum no, maybe you should go for a look at HACH's or LaMotte
website or
> : the
> : > : book I
> : > : > suggested earlier. Please view a copy.
> : > : >
> : > : > Standard Methods for the Examination of Water and Wastewater
> : > : >
> : > : > This book, over 2000 pages, is the guide for water testing. If you
are
> : > : reporting water
> : > : > test to the EPA you must use approved std from this text.I t is
> : prepared
> : > : and published by
> : > : > the EPA, American Water Works Association and American Public
Health
> : > : Association. You
> : > : > mean you don't have one and the issue is water chemistry
> : > : >
> : > : > You are confusing Acidity and Acidity as you know little about
water
> : > : chemistry and
> : > : > procedures and test methods
> : > : >
> : > : > From SMEWW, section 2-30, 2310 ACIDITY
> : > : >
> : > : > "Acidity of water is its quantative capacity to react with a
strong
> : base
> : > : to a designated
> : > : > pH"
> : > : >
> : > : > This is how you test for it
> : > : >
> : > : > A std alkali titration to methyl orange or phenolphthalein
> : > : > endpoint.
> : > : >
> : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that
write
> : this
> : > : book, there are
> : > : > over 100 of them, they are wrong.
> : > : >
> : > : > Like Buffering Capacity you have your Acidity's mixed up
> : > : > In water measurement if you have a high Alk you also usually have
a
> : high
> : > : Acidity.
> : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
> : CHEMISTRY
> : > : BOOK there pal.
> : > : >
> : > : >
> : > : > "These are all in equilibrium with each other. An initial high pH
> : (above
> : > : > 6.4) will shift the equilibrium to the right to form HCO3-1. If
the
> : pH of
> : > : > the solution is above 10.3 (pKa2) the .........."
> : > : >
> : > : >
> : > : > Christ, there you go again with the FW ****. All your numbers are
> : wrong we
> : > : are dealing
> : > : > with SEAWATER
> : > : >
> : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is in
the
> : form
> : > : > of HCO3-1 .
> : > : >
> : > : > I have already pointed that out and gave actual values at know
> : seawater
> : > : levels, go back
> : > : > and re-read it you aren't telling me anything here.Of course most
is
> : HCO3
> : > : see...
> : > : >
> : > : >
> : > : > @ 20C and 34.3 ppt salinity
> : > : >
> : > : > CO2 = 0.52 %
> : > : >
> : > : > HCO3 = 86.4 %
> : > : >
> : > : > CO3 = 13.09 %
> : > : >
> : > : >
> : > : > "In your glass experiment you managed to lower the pH enough to
purge
> : out
> : > : CO2
> : > : > by boiling"
> : > : >
> : > : > The purpose behind the glass is to show that alk is not affect by
CO2
> : and
> : > : vise-versa and
> : > : > how Co2 affects pH.
> : > : >
> : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and that
pH
> : drops
> : > : to say 8.1 it is
> : > : > usually due to excess CO2. If you took a glass of that water and
> : aerated
> : > : it you WILL drive
> : > : > off the CO2 and raise the pH. It has been done a proven a million
> : times.
> : > : >
> : > : > "In order to 'purge' CO2 you would need to lower the
> : > : > pH to shift the equilibrium to below 6.4"
> : > : >
> : > : > The hell you do !!!.Do you know who many times people on this NG
to
> : > : include Dr. Craig
> : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to
take a
> : > : sample of aquarium
> : > : > water and aerate it to see if the pH GOES UP AND when they come
back
> : with
> : > : the test it is
> : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST
> : excess
> : > : CO2 in the tank
> : > : > water, increase the circulation for better gas exchange at the
> : surface,
> : > : reduce feeding,
> : > : > and try to improve on better skimming, thus reducing the bio-load
and
> : pH
> : > : decline due to
> : > : > CO2.
> : > : >
> : > : >
> : > : > "I hope this helps. "
> : > : >
> : > : > Help, how can you when you miss everything. I should be charging
you
> : > : >
> : > : > Oh, by the way. Your websites, I have about 50 on these issues, I
> : could
> : > : post them, not to
> : > : > mention I have all those water chemistry books, so there is no
need to
> : > : view your sites.
> : > : >
> : > : > Finally are you afraid to come to our Chemistry Forum, afraid to
get
> : > : slapped by REAL
> : > : > chemists. I get a charge out of you can't post your ref .I have
posted
> : the
> : > : same or similar
> : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500
> : posts
> : > : there and am the
> : > : > biggest contributor to his forum other than himself or maybe Habib
> : Sheka
> : > : >
> : > : > Hum, here are Randy's ref that he posted. He hosts the website
> : > : >
> : > : > S. RANDY HOLMES-FARLEY
> : > : > Arlington, Massachusetts
> : > : >
> : > : > EDUCATION
> : > : >
> : > : > 1982-1986 Harvard University Cambridge, MA
> : > : > PhD in Chemistry
> : > : > Research Advisor: George Whitesides
> : > : >
> : > : > Investigated the relationship between polymer surface chemistry
and
> : > : physical properties
> : > : > through controlled surface modification and testing.
> : > : >
> : > : > 1980-1982 Cornell University Ithaca, NY
> : > : > BA in Chemistry and Biology
> : > : > Graduated Summa Cum Laude
> : > : > Distinction in All Subjects
> : > : > Grade Point: 3.94/4.0
> : > : > Honors research: isolation and characterization of the subunit of
CF1
> : > : enzyme
> : > : >
> : > : >
> : > : > 1978-1979 Stanford University Palo Alto, CA
> : > : > Grade Point: 3.55/4.0
> : > : >
> : > : >
> : > : > EXPERIENCE
> : > : >
> : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
> : > : > (bought out GelTex Pharmaceuticals in 2001)
> : > : > Vice President, Chemical Research 2001-present
> : > : > Senior Director, Chemical Research 1999-2001
> : > : > Director of Chemical Research 1997-1999
> : > : > Manager of Chemical Research 1995-1997
> : > : > Group Leader 1994-1995
> : > : > Senior Research Scientist 1992-1994
> : > : >
> : > : > Helped start GelTex as second employee
> : > : >
> : > : > Managed various research programs with multi-million dollar
budgets
> : > : >
> : > : > Supervised research chemists (17+)
> : > : >
> : > : > Co-inventor of several polymeric pharmaceuticals and
pharmaceutical
> : > : candidates including
> : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam
Hydrochloride
> : (FDA
> : > : approved)
> : > : >
> : > : > Company Safety Officer for 3 years
> : > : >
> : > : > Chemical Hygiene Officer 2000-present
> : > : >
> : > : >
> : > : >
> : > : >
> : > : > 1990-1992 GTE Corporation Waltham, MA
> : > : > Senior Member of Technical Staff
> : > : > Applied research involving polymer interfaces
> : > : > Metallization of plastics
> : > : > Polymer/polymer adhesion
> : > : > Optical coatings
> : > : >
> : > : >
> : > : >
> : > : > 1986-1990 Lord Corporation Cary, NC
> : > : > Senior Research Scientist 1988-1990
> : > : > Research Scientist 1986-1988
> : > : > Basic and applied research on surface chemical bonding
> : > : > Developed new adhesive compositions
> : > : > Developed new sol-gel coatings for corrosion resistance
> : > : >
> : > : >
> : > : > HONORS AND AWARDS
> : > : >
> : > : > Industrial Innovations Award by Northeast Region of American
Chemical
> : > : Society (6/2001)
> : > : >
> : > : > National Kidney Foundation of Northern California Honoree (5/2001)
> : > : >
> : > : > American Chemical Society/Polymer Chemistry Division Industrial
> : Sponsors
> : > : > Award (8/2000)
> : > : >
> : > : > R&D 100 Award from R&D magazine (1999)
> : > : >
> : > : > Sherwin Williams Award in applied polymer science (9/85)
> : > : >
> : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985;
1985-1986)
> : > : >
> : > : > Award for highest GPA in Chemistry Department (6/82)
> : > : >
> : > : > Summa Cum Laude Honors in Chemistry (6/82)
> : > : >
> : > : > Phi Lamda Epsilon (6/82)
> : > : >
> : > : > Phi Beta Kappa (2/82)
> : > : >
> : > : > Cornell University Dean's List (1981, 1982)
> : > : >
> : > : > Harvard Book Club Award for highest GPA senior year (1978)
> : > : >
> : > : > First Place in western NY ACS high school chemistry exam (1977)
> : > : >
> : > : > 1978-1979
> : > : >
> : > : >
> : > : > __________________
> : > : > Randy Holmes-Farley
> : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef
Central
> : > : >
> : > : > Hobby Experience: 8 years with reefs
> : > : > Current Tanks: 90 gal mixed reef
> : > : > Interests: Reefkeeping, science, photography
> : > : >
> : > : >
> : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> : > : >
> : > : > Open this post in a new window | Report this post to a moderator |
IP:
> : > : Logged
> : > : >
> : > : >
> : > : >
> : > : > 06/27/2003 02:44 PM
> : > : >
> : > : > Randy Holmes-Farley
> : > : > Chemistry Moderator
> : > : >
> : > : > Registered: Apr 2001
> : > : > Location: Arlington, Massachusetts
> : > : > Occupation: Chemist (Drug Discovery at Genzyme)
> : > : > Posts: 15282
> : > : >
> : > : >
> : > : >
> : > : > Publications
> : > : >
> : > : >
> : > : > ISSUED UNITED STATES PATENTS
> : > : >
> : > : >
> : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
> : > : Mandeville, III; W. Harry.
> : > : > US 6,566,407; 5/20/2003
> : > : >
> : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen
> : Randall;
> : > : Huval, Chad
> : > : > Cori.
> : > : > U.S. 6,517,825; 2/11/2003.
> : > : >
> : > : > 3. Method of making phosphate-binding polymers for oral
> : administration.
> : > : Holmes-Farley,
> : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
> : > : 6,509,013; 1/21/2003.
> : > : >
> : > : > 4. Combination therapy for treating hypercholesterolemia using a
bile
> : acid
> : > : sequestrant
> : > : > polymer
> : > : > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley,
> : Stephen
> : > : Randall;
> : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> : > : >
> : > : > 5. Method for treating hypercholesterolemia with polyallylamine
> : polymers.
> : > : Holmes-Farley,
> : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
> : Goldberg,
> : > : Dennis I. , US
> : > : > 6,423,754; 7/23/2002.
> : > : >
> : > : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry,
III;
> : > : Neenan, Thomas X..;
> : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> : > : >
> : > : > 7. Combination therapy for treating hypercholesterolemia and
> : > : atherosclerosis. Huval, Chad
> : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal,
Pradeep
> : K.
> : > : U.S. 6,365,186;
> : > : > 4/2/2002.
> : > : >
> : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
> : Mandeville,
> : > : W. H., III;
> : > : > Huval; C.
> : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
> : > : 10/9/2001.
> : > : >
> : > : > 9. Polymers containing guanidinium groups as bile acid
sequestrants.
> : Dhal;
> : > : P. K.; Holmes-
> : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> : > : >
> : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville,
W.
> : H.,
> : > : III.; US
> : > : > 6,281,252;
> : > : > 8/28/2001.
> : > : >
> : > : > 11. Combination therapy for treating hypercholestrolemia. Huval;
C.
> : C.;
> : > : Holmes-Farley; S.
> : > : > R. ;
> : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> : > : >
> : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G.
M.;
> : > : Holmes-Farley, S.
> : > : > R.; US
> : > : > 6,264,937; 7/24/2001.
> : > : >
> : > : > 13. Method for treating hypercholesterolemia with unsubstituted
> : > : polydiallylamine polymers.
> : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K.
; US
> : > : 6,248,318;
> : > : > 6/19/2001.
> : > : >
> : > : > 14. Process for removing bile salts from a patient and alkylated
> : > : compositions therefore.
> : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355;
5/1/2001.
> : > : >
> : > : > 15. Poly(diallylamine)-based bile acid sequestrants.
Holmes-Farley, S.
> : R.;
> : > : Dhal, P. K.;
> : > : > Petersen,
> : > : > J. S.; US 6,203,785; 3/20/2001.
> : > : >
> : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.;
> : Huval,
> : > : C. C.; US
> : > : > 6,190,649;
> : > : > 2/20/2001.
> : > : >
> : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville,
W.
> : H.,
> : > : III.; US
> : > : > 6,177,478;
> : > : > 1/23/2001.
> : > : >
> : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
> : Holmes-Farley,
> : > : S. R.;
> : > : > Mandeville, W.
> : > : > H., III.; US 6,129,910; 10/10/2000.
> : > : >
> : > : > 19. Method for treating hypercholesterolemia with unsubstituted
> : > : polydiallylamine polymers.
> : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K.
; US
> : > : 6,083,497;
> : > : > 7/4/2000.
> : > : >
> : > : > 20. Method of making phosphate-binding polymers for oral
> : administration.
> : > : Holmes-Farley, S.
> : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495;
> : 7/4/2000.
> : > : >
> : > : > 21. Process for removing bile salts from a patient and alkylated
> : > : compositions therefore.
> : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
> : 5/23/2000.
> : > : >
> : > : > 22. Process for removing bile salts from a patient and
compositions
> : > : therefor. Mandeville,
> : > : > W. H.,
> : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> : > : >
> : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W.
H;
> : > : Neenan; T. X.; Holmes-
> : > : > Farley; S. R. US 6,034,129; 3/7/2000.
> : > : >
> : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville,
W.
> : H.,
> : > : III.; US
> : > : > 5,985,938;
> : > : > 11/16/99.
> : > : >
> : > : > 25. Process for removing bile salts from a patient and
compositions
> : > : therefor. Mandeville,
> : > : > W. H.,
> : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> : > : >
> : > : > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville,
W.
> : H.,
> : > : III.;
> : > : > Holmes-Farley;
> : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> : > : >
> : > : > 27. Hydrophilic nonamine-containing and amine-containing
copolymers
> : and
> : > : their use as bile
> : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
> : 5,929,184;
> : > : 7/27/99.
> : > : >
> : > : > 28. Interpenetrating polymer networks for sequestration of bile
acids.
> : > : Mandeville, W. H.,
> : > : > III.;
> : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US
5,925,379;
> : > : 7/20/99.
> : > : >
> : > : > 29. Amine polymer sequestrant and method of cholesterol depletion.
> : > : Mandeville, W. H.,
> : > : > III.;
> : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> : > : >
> : > : > 30. Process for removing bile salts from a patient and
compositions
> : > : therefor. Mandeville,
> : > : > W. H.,
> : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> : > : >
> : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
depletion.
> : > : Mandeville, W. H.,
> : > : > III.;
> : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> : > : >
> : > : > 32. Process for removing bile salts from a patient and
compositions
> : > : therefor. Mandeville,
> : > : > W. H.,
> : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> : > : >
> : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
> : Mandeville,
> : > : W. H., III.;
> : > : > Holmes-
> : > : > Farley, S. R.; US 5,703,188; 12/30/97.
> : > : >
> : > : > 34. Oral administration of iron-binding crosslinked amine
polymers.
> : > : Mandeville, W. H.,
> : > : > III.;
> : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> : > : >
> : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
Holmes-Farley,
> : S.
> : > : R.; US 5,693,675;
> : > : > 12/2/97.
> : > : >
> : > : > 36. Method for removing bile salts from a patient with alkylated
> : > : crosslinked amine
> : > : > polymers,
> : > : > and preparation of the polymers. Mandeville, W. H., III.;
> : Holmes-Farley,
> : > : S. R.; US
> : > : > 5,679,717; 10/21/97.
> : > : >
> : > : > 37. Phosphate-binding polymers for oral administration.
Holmes-Farley,
> : S.
> : > : R.; Mandeville,
> : > : > W.
> : > : > H., III.; US 5,667,775; 9/16/97.
> : > : >
> : > : > 38. Ion-exchange process using highly crosslinked polymers for
> : removing
> : > : bile salts from a
> : > : > patient, preparation of the polymers, and compositions containing
> : them.
> : > : Mandeville, W. H.,
> : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> : > : >
> : > : > 39. Hydrophobic amine polymer sequestrant and method of
cholesterol
> : > : depletion. Mandeville,
> : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530;
> : 4/8/97.
> : > : >
> : > : > 40. Amine polymer sequestrant and method of cholesterol depletion.
> : > : Mandeville, W. H.,
> : > : > III.;
> : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> : > : >
> : > : > 41. Phosphate-binding polymers for oral administration.
Holmes-Farley,
> : S.
> : > : R.; Mandeville,
> : > : > W.
> : > : > H., III.; US 5,496,545; 3/5/96.
> : > : >
> : > : > 42. Iron-binding polymers for oral administration. Mandeville, W.
H.,
> : > : III.; Holmes-Farley,
> : > : > S. R.;
> : > : > US 5,487,888; 1/30/96.
> : > : >
> : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having
active
> : > : hydrogens on the
> : > : > surface.
> : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> : > : >
> : > : > 44. Layered sol-gel coatings from organisilicon compounds.
> : Holmes-Farley,
> : > : S. R.; Yanyo, L.
> : > : > C.;
> : > : > US 5,182,143; 1/26/93.
> : > : >
> : > : > 45. Method for metal bonding using ultrathin primer coating.
> : > : Holmes-Farley, S. R.; Yanyo,
> : > : > L.
> : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> : > : >
> : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K.
J.;
> : US
> : > : 5,096,962;
> : > : > 3/17/92.
> : > : >
> : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> : > : elastomer-metal bonding.
> : > : > Holmes-
> : > : > Farley, S. R.; US 5,102,956; 4/7/92.
> : > : >
> : > : >
> : > : >
> : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
> : > : >
> : > : >
> : > : > 1. Aryl boronate functionalized polymers for treating obesity and
> : > : inhibiting fat uptake.
> : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal,
> : Pradeep
> : > : K.; Huval, Chad
> : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003),
92
> : pp. WO
> : > : 0302571.
> : > : >
> : > : > 2. Preparation of aryl boronic acids for treating obesity.
> : Holmes-Farley,
> : > : Stephen Randall;
> : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal,
Pradeep
> : K.
> : > : (Geltex
> : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO
0302570.
> : > : >
> : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide.
Holmes-Farley,
> : > : Stephen Randall.
> : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp.
WO
> : > : 0302130.
> : > : >
> : > : > 4. Method for reducing copper levels and treating copper
toxicosis.
> : > : Holmes-Farley, Stephen
> : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl.
(2002),
> : 45
> : > : pp. WO
> : > : > 0285383.
> : > : >
> : > : > 5. Method for treating gout and binding uric acid. Holmes-Farley,
> : Stephen
> : > : Randall; Burke,
> : > : > Steven K. WO 0285381 10/31/2002.
> : > : >
> : > : > 6. Method for treating gout and reducing serum uric acid.
> : Holmes-Farley,
> : > : Stephen Randall;
> : > : > Burke, Steven K WO 0285380 10/31/2002.
> : > : >
> : > : > 7. Amine condensation polymer bile acid sequestrants. Huval, C.
C.;
> : > : Holmes-Farley, S. R.;
> : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> : > : >
> : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III
and
> : > : Holmes-Farley, S.
> : > : > R.;
> : > : > WO 1999-US5662; 9/23/1999.
> : > : >
> : > : > 9. Amine-containing copolymers as bile acid sequestrants.
> : Holmes-Farley,
> : > : S. R.; Petersen,
> : > : > J. S.;
> : > : > WO 9933452; 7/8/1999.
> : > : >
> : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H.,
III
> : and
> : > : Holmes-Farley, S.
> : > : > R.;
> : > : > WO 9922743; 5/14/1999.
> : > : >
> : > : > 11. Polyallylamine polymers for removing bile salts and treating
> : > : hypercholesterolemia, and
> : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III;
> : Burke,
> : > : S. K.; Goldberg,
> : > : > D. I.; WO 9857652; 12/23/98.
> : > : >
> : > : > 12. Phosphate-bidning polymers combined with a calcium supplement
for
> : oral
> : > : administration.
> : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
Holmes-Farley,
> : S.
> : > : R.; WO 9842355;
> : > : > 10/1/98.
> : > : >
> : > : > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
> : > : depletion. Mandeville,
> : > : > W.
> : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449;
12/12/96.
> : > : >
> : > : > 14. Process for adjusting ion concentration in a patient and
> : compositions
> : > : therefor.
> : > : > Mandeville,
> : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> : > : >
> : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
> : interlayer
> : > : for improved
> : > : > metal-
> : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
> : 1/20/94.
> : > : >
> : > : > 16. Process for increased metal-substrate bond strength in
metalized
> : > : plastics.
> : > : > Holmes-Farley, S.
> : > : > R.; Ger. Offen. 4322516; 7/6/93.
> : > : >
> : > : > 17. Electrorheological fluids and preparation of particles useful
in
> : the
> : > : fluids.
> : > : > Troughton,
> : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson,
J.
> : > : David; Bares, Joseph
> : > : > E.;
> : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell.
EP
> : > : 394049;
> : > : > 10/24/1990.
> : > : >
> : > : > JOURNAL PUBLICATIONS
> : > : >
> : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov,
> : Eugene;
> : > : Guo, Amy;
> : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
> : > : Mandeville, W. Harry;
> : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
> : 611-619.
> : > : >
> : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
> : synthesis
> : > : and biological
> : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S.
> : Randall;
> : > : Mandeville, W.
> : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep
K.
> : > : Journal of
> : > : > Macromolecular Science, Pure and Applied Chemistry (2001),
A38(12),
> : > : 1559-1574.
> : > : >
> : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by
Molecular
> : > : Imprinting. Huval,
> : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley,
S.
> : > : Randall; Mandeville,
> : > : > W.
> : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro,
Robert
> : J.;
> : > : Chen, Xi; Dhal,
> : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> : > : >
> : > : > 4. Synthetic polymers for the binding of fat in the intestinal
tract.
> : > : Jozefiak, Thomas H.;
> : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia;
> : Huval,
> : > : Chad C.;
> : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
> : > : Abstracts of
> : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United States,
August
> : > : 26-30, 2001
> : > : > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
> : > : Division of
> : > : > Polymer Chemistry) (2001), 42(2), 98.
> : > : >
> : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel
polymer
> : gel
> : > : pharmaceutical.
> : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen,
J.;
> : Ward,
> : > : J.; Sacchiero,
> : > : > B.;
> : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K.
A.;
> : Chen,
> : > : X.; Mazzeo, J.
> : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
> : > : >
> : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl and
> : other
> : > : bile acid
> : > : > sequestrants.
> : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu,
Q.;
> : > : Hook, P.; Holmes-
> : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1),
708-709.
> : > : >
> : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
> : Holmes-Farley,
> : > : S. R; Polym.
> : > : > Mater. Sci. Eng (1999), 80, 246-247.
> : > : >
> : > : > 8. Design and characterization of of Sevelamer Hydrochloride: a
novel
> : > : phosphate-binding
> : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III;
Ward,
> : J.;
> : > : Miller, K. L.;
> : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.-
Pure
> : and
> : > : Appl. Chem.,
> : > : > A36(7&8), p. 1085 (1999).
> : > : >
> : > : > 9. Three generations of bile acid sequestrants. Mandeville, W. H.,
> : III;
> : > : Braunlin, W.;
> : > : > Dhal, P.;
> : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
> : > : Rosenbaum, D.;
> : > : > Sacchiero,
> : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc.
(1999),
> : > : 550, 3-15.
> : > : >
> : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric
> : phosphate
> : > : binder, on
> : > : > urinary
> : > : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S.
R.;
> : > : Mandeville, W. H.,
> : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
Transplant.
> : > : (1997), 12(5)
> : > : > 961-964.
> : > : >
> : > : > 11. Thin anisotropic coatings based on sol-gel technology.
> : Holmes-Farley,
> : > : S. R.; Yanyo, L.
> : > : > C;
> : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4),
> : 439-444.
> : > : >
> : > : > 12. The mechanism of cure initiation of a surface activated
adhesive.
> : > : Holmes-Farley, S.
> : > : > R.;
> : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
> : > : >
> : > : > 13. Adhesion promotion and corrosion prevention using thin
anisotropic
> : > : coatings. Holmes-
> : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
> : > : 131-151.
> : > : >
> : > : > 14. Wetting of functionalized polyethylene having ionizable
organic
> : acids
> : > : and bases at the
> : > : > polymer-water interface: relations between functional group
polarity,
> : > : extent of
> : > : > ionization,
> : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
> : > : Whitesides, G. M.;
> : > : > Langmuir
> : > : > (1988), 4(4), 921-937.
> : > : >
> : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with
a
> : > : single hydroxy group.
> : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> : > : >
> : > : > 16. Reconstruction of the interface of oxidatively functionalized
> : > : polyethylene (PE-CO2H)
> : > : > and
> : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.;
Nuzzo,
> : R.;
> : > : McCarthy, T. J.;
> : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report
> : (1987),
> : > : AD-
> : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> : > : >
> : > : > 17. Surface-modified polyethylene film: the relationship between
> : surface
> : > : chemistry and
> : > : > physical
> : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11),
> : 4537.
> : > : >
> : > : > 18. Reactivity of carboxylic acid and ester groups in the
> : functionalized
> : > : interfacial
> : > : > region of
> : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> : > : differentiation of the
> : > : > functional groups into shallow and deep subsets based on a
comparison
> : of
> : > : contact angle and
> : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.;
Langmuir
> : > : (1987), 3(1), 62-
> : > : > 76.
> : > : >
> : > : > 19. Fluorescence properties of dansyl groups covalently bonded tot
he
> : > : surface of
> : > : > oxidatively
> : > : > functionalized low-density polyethylene film. Holmes-Farley, S.
R.;
> : > : Whitesides, G. M.;
> : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
> : > : AD-A162435/2/GAR,
> : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> : > : >
> : > : > 20. Acid-base behavior of carboxylic acid groups covalently
attached
> : at
> : > : the surface of
> : > : > polyethylene: The usefulness of contact angle in following the
> : ionization
> : > : of surface
> : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T.
J.;
> : > : Deutch, J.;
> : > : > Whitesides,
> : > : > G. M.; Langmuir (1985), 1(6), 725-740.
> : > : >
> : > : > 21. The thermal stability of a surface modified solid organic
polymer.
> : > : Holmes-Farley, S.
> : > : > R.;
> : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
> : > : >
> : > : >
> : > : >
> : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> : > : >
> : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R.
Advanced
> : > : Aquarist. June 2003.
> : > : >
> : > : > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley,
R.
> : > : Advanced Aquarist.
> : > : > May
> : > : > 2003.
> : > : >
> : > : > 3. The Degradation of Limewater (Kalkwasser) in Air.
Holmes-Farley, R.
> : > : Reefkeeping May
> : > : > 2003.
> : > : >
> : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
Reefkeeping
> : > : April 2003.
> : > : >
> : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> : > : Holmes-Farley, R.
> : > : > Advanced Aquarist; April 2003.
> : > : >
> : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
> : > : Holmes-Farley, R.
> : > : > Advanced Aquarist; April 2003.
> : > : >
> : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced
> : Aquarist;
> : > : March 2003.
> : > : >
> : > : > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
> : > : Holmes-Farley, R.
> : > : > Advanced Aquarist; February 2003.
> : > : >
> : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
January
> : > : 2003.
> : > : >
> : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> : December
> : > : 2002.
> : > : >
> : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
> : Advanced
> : > : Aquarist; November
> : > : > 2002.
> : > : >
> : > : > 12. Iron: A Look at Organisms Other than Macroalgae.
Holmes-Farley, R.
> : > : Advanced Aquarist;
> : > : > November 2002.
> : > : >
> : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced
> : Aquarist,
> : > : September 2002.
> : > : >
> : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist,
August
> : > : 2002.
> : > : >
> : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com,
April
> : > : 2002.
> : > : >
> : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
> : > : Aquarist; July 2002
> : > : >
> : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist;
> : June
> : > : 2002.
> : > : >
> : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R.
> : Advanced
> : > : Aquarist, May
> : > : > 2002.
> : > : >
> : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in
Corals.
> : > : Holmes-Farley, R.
> : > : > Advanced Aquarist, April 2002.
> : > : >
> : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> : > : >
> : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February
2002.
> : > : >
> : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January
> : 2002.
> : > : >
> : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium
Frontiers
> : > : 2000.
> : > : >
> : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
> : > : Frontiers 2000.
> : > : >
> : > : > 25. Phosphate..What is it and why should you care. Holmes-Farley,
R.
> : > : Aquarium Frontiers
> : > : > 2000.
> : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
> : Frontiers
> : > : 2000.
> : > : >
> : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers
> : 2000.
> : > : >
> : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers
1999.
> : > : >
> : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> : > : >
> : > : >
> : > : >
> : > : >
> : > : >
> : > : >
> : > : >
> : > : > Boomer
> : > : >
> : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : >
> : > : > Want to See More ?
> : > : > Please Join Our Growing Membership
> : > : > www.coralrealm.com
> : > : >
> : > : >
> : > : >
> : > :
> : > :
> : >
> : >
> :
> :
> :
>
>

[Benjamin]

Boomer,

Why are you still dwelling on all this? Can't we talk about what you
really want the world to know about Reef Aquarium Chemistry now? Can you do
it in a language and manner that even a "snoot-noise kid" can grasp and
appreciate? Could you set aside your apparently cantankerous nature long
enough so many can learn something valuable from you without feeling... um
never mind I can't find the word for it.

--
--

My Web Site: http://showcase.netins.net/web/reefpage/


"Boomer" > wrote in message
...
> "As it is the ability to neutralizes an acid that is a buffer"
>
> sorry
>
> As it is the ability to neutralizes a base that is a buffer
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "Boomer" > wrote in message
> ...
> :
> : "I am not sure if you are just messing with me "
> :
> : Yes, messing with you, it is called trolling a troll, to see where the
hell you would go
> : and what you would say in regards to last posts. It is called honesty,
of which you have
> : none off to say the least,that I can see.You always like to post what
suits you and just
> : avoid ref I give. So lets start where you are WRONG and have a great
lack of
> understanding
> : of things, to include pointing out all your gross error which you still
FAIL to
> : acknowledge and which can be prove in many water chem. ref. .I doubt
like hell you are a
> : chemist at all.You seem to want to con people into thinkin' you are. But
then again, I
> : have seen chemists like you before, they are not familiar with the, but
they ASK to have
> : it explained and ask for REF.YOU just shoot from the hip. WHAT GETS YOU
IN TROUBLE. You
> : remind me of snoot-noise kid that come here and other NG's and
forums...that think they
> : know, buy hey, maybe I'm wrong :-)
> :
> :
> :
> : 1). Acidity
> :
> : "***Benjamin,Water Chemistry (2002, pages 262-263).***
> :
> : ***Acidity A concept that is exactly analogous to alkalinity but
measures the base
> : neutralizing
> : capacity (BNC) of a solution is Acidity. The quantitative represents the
concentration
> of
> : OH- ions that must be added to titrate the solution to a pH near 10.5***
> :
> : So that means that not only in Benjamin wrong but, so are Stumm &
Morgan, Millero,
> Pilosn,
> : Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I
said, you have
> your
> : acidity and Acidy mixed up. Acidity as defined above is covered in most
water chemistry
> : books, written by chemists, who's field of expertise is water chemistry.
You can even
> buy
> : Acidity test kits from, HACH, LaMotte, etc..
> :
> : You mean you didn't read this or are you just avoiding it .The same
definition can be
> : found in almost any std water chemistry book.
> :
> : I have run into few chemists, that are NOT familiar with the above. Some
water reports
> : require the above Acidity measuring. The issue with you is you do not
understand WATER
> : CHEMISTRY. Everything you have posted can be found a general chemistry
book
> :
> :
> :
> :
> : 2) Alk and BC
> :
> : From the link
> :
> : Alkalinity
> : ***Acid neutralizing or buffering capacity of water; a measure of the
ability of water
> to
> : resist changes in pH caused by the addition of acids or bases ***
> :
> : This is a Buffering Capacity definition not Alk
> :
> : Humm, since when does Alk have anything to do in regards to the addition
of BASE. As I
> : pointed out in the first post the term is often miss used. Even in YOUR
own posts you
> say
> : it is based on a acid addition, no mention of **base or acid** addition
by you. Are you
> : getting confused or what. Or is more you are trying to confuse everyone
you are right.
> The
> : above is a definition for Buffer Capacity NOT Alk
> :
> : From Drew, Geochemistry of Natural Waters
> :
> : "alkalinity, which is formally defined as the equivalent sum of bases
that are
> titratable
> : with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH of
the solution is
> : progressively lowered by the addition of a strong acid (HCL), all the
anions on the
> right
> : will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4,
H2S,organic acids, H20)"
> :
> : This follows almost all description of Alk, that it is acid neutralizing
reaction and
> has
> : nothing to do with base neutralizing, which is Acidity (BNC) .I defined
these before you
> : had no comment
> :
> :
> : Even the links that give the Buffering Capacity definition is wrong, as
is the UIPAC on
> : Alkalinity. Alkalinity has nothing to do with the addition of bases only
acids. When you
> : use the words "base and acid" it becomes BC
> :
> : Even YOU MUST disagree with these definitions, from YOUR own post
> :
> : Think of alkalinity as 'buffering capacity'. Or the ability of a
solution
> : ***to resist a drop in pH due to the addition of acid***
> :
> : Where the flip is the base addition forget it ?
> :
> : From Butler; Carbon Dioxide Equilibrium and Their Applications
(professor emeritus
> : Harvard University) an expert on the subject.
> :
> : Buffering Index (Buffering Capacity, Buffer Intensity).
> :
> : ***This concept was first developed for mixtures of approximately equal
proportions of
> : conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such
buffer solutions
> : strongly resist changes in pH when acids or bases are added and are
useful as pH
> : standards. The Buffer Index tells how great the resistance to pH changes
will be.**
> :
> : also from Butler
> :
> : Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
> :
> : Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
> :
> : Acidity is in fact just the negative of Alkalinity ***
> :
> : http://www.lagoonsonline.com/acid.htm
> :
> :
http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.htm?E+mystore
> :
> : It sure is funny how all of the chemist that write water chemistry
textbooks never say
> Alk
> : is the Buffering Capacity of a solution. They are always treated and
defined separately.
> :
> : If you or others choose to treat Alk and BC as the same, well, just have
at it. As I
> said
> : in first post I know what you mean.
> :
> : "No need to cite web pages that describe what I know and what I wrote
> : in this discussion"
> :
> : No you don't know, who are you trying to convince any way, me, the guys
here and/or all
> : the water chemists in this world. As I said before go get a dam WATER
CHEMISTRY book or
> : shut the hell up.You keep trying to define things from a general
chemistry book WE ARE
> IN
> : THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
> :
> :
> :
> :
> :
> : 3). pKa's and what you don't know or seem to be confused on
> :
> : "Therefore, it has two pKa's
> : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
The
> : pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
> : right in there. Is that magic? :)"
> :
> : Here it is agin that is twice at least
> :
> : "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this
example)
> : you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium
will
> : be shifted to HCO3-2 by a ratio of 1:100.
> :
> : Oh wait , there is a third time LOL
> :
> : "At the pH of seawater, the buffering capacity of carbonate is at it's
> : weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
> :
> :
> : Lets just dunk you on this one. I am taking note you refuse to reply to
YOUR errors
> :
> : So you calculated the pH of seawater with freshwater pKa's, now that is
a good trick.
> From
> : a number of seawater chemistry books the seawater pKa's are 6 & 9.1, so
according to
> you,
> : seemingly not understanding your favorite Henderson-Hasselbach equation;
> :
> : 2 pH = (6 + 9.1) /2 pH = 7.55
> :
> : I have never seen seawater with a pH of 7.55. There is no ocean with
that pH. Humm how
> : come your equation is not working for you today.?
> :
> :
> : "That pH I calculated is
> : right in there. Is that magic? :)"
> :
> : I roll on the floor when I see this = 8.35
> :
> : Hum , just a brain far so excuse me for thinkin
> :
> : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
> :
> : Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a pH
of 8.35 there
> pal
> : ? That 8.35 is what you are telling people the pH should be, but their
meter says 6.4.
> : This how people will READ this.
> :
> :
> :
> :
> : 4.) More on Buffering Capacity
> :
> : "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes,
your
> : alkalinity equation."'
> :
> :
> : Yup, I see that and in this case the HCO3 is the acid and the CO3 is the
base CORRECT.
> In
> : Alk you are only dealing with bases and how they react to an acid.
Acidity deals acids
> and
> : how they recact to bases "Acidity, A concept that is exactly analogous
to alkalinity but
> : measures the base neutralizing
> : capacity (BNC) of a solution is Acidity "Alk is the ANC Acid
neutralizing capacity
> :
> : "Don't the components of a buffer account for the buffering capacity? "
> :
> : Yes, they do but so do the acids which work as buffers. NaHCO3 is a
buffer and can act
> as
> : an acid or base
> :
> : *** Buffering Capacity.**
> : The power of a substance in solution to absorb acid or alkali without
change in pH; this
> : is highest at a pH value equal to the pKa value of the acid of the
buffer pair.***
> :
> : ***Akalinity***
> : Measure of the power of a solution to neutralise hydrogen ions (H+),
usually expressed
> as
> : the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
> :
> :
> : If one wants to call Alk Buffering capacity then one sure as a hell can
call Acidty
> : Buffering Capacity also. As it is the ability to neutralizes an acid
that is a
> buffer.You
> : have a pH of 7 and you add a buffer to lower it to a pH of 4, you are
buffering the
> water,
> : that buffer is a acid.
> :
> : 5) CO2
> :
> : You are really confuse so it seems :-) You realllllllly indicate that
CO2 is affected by
> : the Alk or vise-versa
> :
> : "Yes, the pH will drop with the addition of CO2. Remove CO2 will cause
the
> : pH to rise? How do you remove CO2? Once it is in solution it forms
> : carbonic acid and neutralizes some of your 'buffer'."
> :
> : "With the exception of CO2?"
> :
> : No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
> : Concepts)....PERIOD.You seem to think a that at least in two of your
post that CO2 is
> : affected by the Alk or vise-versa. Please go back to school or seek
professor
> :
> : "Why in one case does CO2 from air lower pH and in the other case it
raises
> : it? Doesn't make sense."
> :
> : That is because you don't understand CO2 period. By the way I saved
this, wanted to see
> : if you would bite on the post I gave. Not bite at first, so time to reel
you in, as you
> : did bite in another post..
> :
> : Lets make some sense of it for you, being that you have a pH.D in
chemistry, so you say
> .
> :
> : CO2 is naturally generated in a aquatic systems, it is capable of raise
to various
> levels
> : depending on a number of circumstances .It can be measure (except in
seawater) or
> : calculated using Buch/Park Equations (what we use for seawater. In sort
if you know the
> pH
> : and Alk you can calculate the CO2). If you aerate a system or a sample
of water, even if
> : the pH has only dropped a couple of tenths, due to an increase in CO2,
the CO2 will
> leave
> : solution to the atmosphere.This will raise the pH. On the other hand if
theCO2 level is
> : more of the norm and you have hikgh room air, such as in the winter, the
partial
> pressure
> : of the CO2 in air will be much higher than that in water, in which case
the CO2 will
> enter
> : the water and lower the pH. That is without an airstone. Adding an
airstone will make it
> : even worse,as you are now forcefully driving the CO2 into solution even
quicker. These
> : test /experiments have been proven many times, it is not that may work
could work they
> do
> : work.Yet you want to disagree and in another post say you haven't tried
it,.Seems to me
> : that based on what you say it can't work So, in short you don't know
what the hell you
> are
> : taking about. Go get a glass of seawater with a pH of about 8.3 and
lower it to about
> : 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK- UP
( that is if you
> : don't have a high room air CO2 problem.). This little test has been done
thousands of
> : times in this hobby, with test kits, pH meters and even graphic
printers.
> :
> : "This is where Boomer and I
> : disagree. I say you would have to lower the pH very low in order to
> : effectively remove CO2 by purging."
> :
> : You are 100 % wrong. Please come to our Chem forum and try and run that
by Randy, don't
> : take my word on it. I already know what he will say.
> :
> : "Boomer didnt convince me it
> : works at the pH of an aquarium, but I never tried it and I'm not sure of
> : this. "
> :
> : Well then come too our chem. forum and tell Randy he doesn't know what
he is talking
> about
> : LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it
should be easy for
> : you to run the experiment LOL There are grade school kids that run the
test and know
> what
> : happens and that I'm correct.
> :
> :
> : "The equilibrium is a FUNCTION
> : of pH."
> :
> : It is also a function of Alk or don't you know that. At a pH of 8.3, Alk
2.25, the CO2
> is
> : about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk to
about .4 meq/ l
> : or so the CO2 will be around .99 mg / l CO2, When dealing with tanksCO2
is not always in
> : equilibrium with ambient air.
> :
> :
> : ". But I wouldn't degas a solution of a
> : specific gas (CO2) with a gas (this case he was using air) that contains
the
> : same gas I am trying to purge."
> :
> : Why not ? We have a guy right now that is running tests on purging
ambient air with a
> : solution to remove CO2 gas from the air, before it enters the tank
per/Randy's
> suggestion.
> : The same guy is doing some of my test using a Clinoptilolite, a Zeolite
mineral, that
> has
> : an affinity for CO2.This will be a dry CO2 scrubber
> :
> :
> : Sorry Soutman but you sure as hell don't seem to know much about aquatic
chemistry. You
> : seem to be guessing at everything.
> :
> : By the way have you read any of Randy's technical articles on water
chemistry, been
> saving
> : these for last. There are a few on pH, Alk, CO2 .Here is a list
> :
> : Try and answer them 1-5 and lets see where we get THIS TIME :-) or maybe
we should just
> : drop it. I could care less at this point.
> :
> : THE END
> :
> :
> : ARTICLES
> :
> : The first two posts in this thread are lists of some of my articles that
relate to reef
> : tank chemistry. In the next few posts are some of the articles published
by Craig
> Bingman
> : and others on reef chemistry issues.
> :
> : The first two posts in this thread are lists of some of my articles that
relate to reef
> : tank chemistry. In the next few posts are some of the articles published
by Craig
> Bingman
> : and others on reef chemistry issues.
> :
> : Solving Common Problems
> :
> : Solving Calcium and Alkalinity Problems
> : http://www.advancedaquarist.com/issues/nov2002/chem.htm
> :
> : Solutions to pH Problems
> : http://www.advancedaquarist.com/iss...ne2002/chem.htm
> :
> : How to Select a Calcium and Alkalinity Supplementation Scheme
> : http://www.advancedaquarist.com/issues/feb2003/chem.htm
> :
> : Phosphate Issues
> : http://www.advancedaquarist.com/iss...pt2002/chem.htm
> :
> : Nitrate Issues
> : http://www.advancedaquarist.com/iss...st2003/chem.htm
> :
> :
> :
> : Calcium and Alkalinity
> :
> : Solving Calcium and Alkalinity Problems
> : http://www.advancedaquarist.com/issues/nov2002/chem.htm
> :
> : How to Select a Calcium and Alkalinity Supplementation Scheme
> : http://www.advancedaquarist.com/issues/feb2003/chem.htm
> :
> : Calcium and Alkalinity Balance Issues
> : http://reefkeeping.com/issues/2002-...ature/index.htm
> :
> : Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
> : http://www.advancedaquarist.com/iss...ly2002/chem.htm
> :
> : The Relationship Between Alkalinity and pH.
> : http://www.advancedaquarist.com/issues/may2002/chem.htm
> :
> : The Chemical & Biochemical Mechanisms of Calcification in Corals
> : http://www.advancedaquarist.com/issues/apr2002/chem.htm
> :
> : Calcium
> : http://www.advancedaquarist.com/issues/mar2002/chem.htm
> :
> : Alkalinity
> : http://www.advancedaquarist.com/iss...2/chemistry.htm
> :
> :
> : Iron
> :
> : First Iron Article: Macroalgae and Dosing Recommendations
> : http://www.advancedaquarist.com/issues/aug2002/chem.htm
> :
> : Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> : http://www.advancedaquarist.com/issues/oct2002/chem.htm
> :
> : Iodine
> :
> : Iodine in Marine Aquaria: Part I
> : http://www.advancedaquarist.com/issues/mar2003/chem.htm
> :
> : Iodine in Reef Tanks 2: Effects on Macroalgae Growth
> : http://www.advancedaquarist.com/iss...il2003/chem.htm
> :
> :
> : Magnesium and Strontium
> :
> : Strontium
> : http://www.advancedaquarist.com/issues/nov2003/chem.htm
> :
> : Magnesium
> : http://www.advancedaquarist.com/issues/oct2003/chem.htm
> :
> : Magnesium and Strontium in Limewater
> : http://www.advancedaquarist.com/issues/dec2003/chem.htm
> :
> :
> : Limewater (kalkwasser)
> :
> : The Self Purification of Limewater (Kalkwasser)
> : http://www.advancedaquarist.com/issues/may2003/chem.htm
> :
> : The Degradation of Limewater (Kalkwasser) in Air
> : http://reefkeeping.com/issues/2003-...ature/index.htm
> :
> : How to Select a Calcium and Alkalinity Supplementation Scheme
> : http://www.advancedaquarist.com/issues/feb2003/chem.htm
> :
> : Metals in Aquaria
> :
> : Aluminum and aluminum-based phosphate binders
> : http://www.advancedaquarist.com/iss...ly2003/chem.htm
> :
> : Reef Aquaria with Low Soluble Metals
> : http://reefkeeping.com/issues/2003-...ature/index.htm
> :
> : Tap Water in Reef Aquaria
> : http://www.advancedaquarist.com/issues/jan2004/chem.htm
> : First Iron Article: Macroalgae and Dosing Recommendations
> : http://www.advancedaquarist.com/issues/aug2002/chem.htm
> :
> : Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> : http://www.advancedaquarist.com/issues/oct2002/chem.htm
> :
> :
> : Test Kit Reviews
> :
> : The Seachem Borate Alkalinity Test Kit
> : http://www.advancedaquarist.com/iss...ne2003/chem.htm
> :
> : The Salifert Boron Test Kit
> : http://www.advancedaquarist.com/iss...pt2003/chem.htm
> :
> : Boron and Borate (and pH buffering)
> :
> : Boron in a Reef Tank (and its effect on pH buffering)
> : http://www.advancedaquarist.com/issues/dec2002/chem.htm
> :
> : The Seachem Borate Alkalinity Test Kit
> : http://www.advancedaquarist.com/iss...ne2003/chem.htm
> :
> : The Salifert Boron Test Kit
> : http://www.advancedaquarist.com/iss...pt2003/chem.htm
> :
> :
> :
> : Others
> :
> : Tap Water in Reef Aquaria
> : http://www.advancedaquarist.com/issues/jan2004/chem.htm
> :
> : ORP
> : http://reefkeeping.com/issues/2003-...ature/index.htm
> :
> : Chloramine
> : http://reefkeeping.com/issues/2003-...ature/index.htm
> :
> : Silica in a Reef Tank
> : http://advancedaquarist.com/issues/jan2003/feature.htm
> :
> : Specific Gravity (and temperature correction of hydrometers)
> : http://www.advancedaquarist.com/iss...2/chemistry.htm
> :
> :
> : The Complete Nitrogen Cycle
> : http://www.animalnetwork.com/fish/l...a&RecordNo=3090
> :
> : Magnesium (older article with fonts screwed up)
> : http://www.aquariumfish.com/aquariu...cid=124&search=
> :
> : Phosphate (older article now reproduced in a poor fashion)
> : http://www.aquariumfish.com/aquariu...cid=124&search=
> :
> : Carbon Dioxide
> : http://www.animalnetwork.com/fish/l...a&RecordNo=2074
> :
> : Using Conductivity to Measure Salinity
> : http://www.aquariumfish.com/aquariu...cid=124&search=
> :
> : Understanding Seawater
> : http://www.animalnetwork.com/fish2/...s/1/default.asp
> :
> : Protein Skimming: How It Works
> : http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
> :
> :
> :
> : Articles by Craig Bingman:
> :
> : Carbon Dioxide tests
> : http://www.animalnetwork.com/fish/l...n=&RecordNo=279
> :
> : Limewater, Acetic Acid and Sand Clumping
> : http://www.animalnetwork.com/fish/l...n=&RecordNo=181
> :
> : Calcium and Alkalinity
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : Calculation of Calcium Carbonate Saturation States in Reef Aquaria
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> :
> : Calcification Rates in Several Tropical Coral Reef Aquaria
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : Limits To Limewater...Revisited
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : Expanding the Limits of Limewater: Adding Organic Carbon Sources
(vinegar)
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> :
> : Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : Magnesium - Part I
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : Magnesium - Part II
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : A Homemade Magnesium Supplement
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : Simulating the Effect of Calcium Chloride and Sodium Bicarbonate
Additions on Reef
> Systems
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : Additional Simulations: The Combined Effect Of Calcium Chloride
> : /Sodium Bicarbonate Additions And Water Exchanges
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> :
> : More articles by Craig Bingman:
> :
> : The Halogens - Part I: Bromine in Seawater and Aquaria
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : The Halogens - Part II: Fluoride
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : Fluoride Depletion In Four Reef Aquariums
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : The Halogens - Part III: Iodine
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : Measuring Halides
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : How Test Kits Work
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : Borax pH Calibration
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : A pH Detective Story
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : How to Mix a Batch of Synthetic Seawater in Under Five Minutes
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> : SILICON - FOE OR FRIEND?
> : http://www.animalnetwork.com/fish2/...s/1/default.asp
> :
> : The Composition Of Several Synthetic Seawater Mixes
> : http://www.animalnetwork.com/fish2/...s/1/default.asp
> :
> : Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
> : http://www.animalnetwork.com/fish2/...bio/default.asp
> :
> :
> :
> : Andy's calcium calculator
> : http://www.andy-hipkiss.co.uk/cacalc.htm
> :
> : Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
> : http://www.aquariumfish.com/aquariu...cid=124&search=
> :
> : Calcium Reactor Substrate -- Phosphate Levels
> : by Greg Hiller
> : http://www.advancedaquarist.com/iss...l2003/short.htm
> :
> :
> : Indoor CO2 Problems
> : http://www.advancedaquarist.com/iss...r2002/short.htm
> :
> : Simon Huntington's CaCO3/CO2 reactor article
> :
> : http://reefkeeping.com/issues/2002-...ature/index.htm
> :
> : Ron Shimek's Tank Water Analysis Article
> : http://reefkeeping.com/issues/2002-...ature/index.htm
> :
> :
> :
> :
> : Home made salinity standards thread:
> :
> : http://reefcentral.com/forums/showt...?threadid=65509
> :
> : Reef Chemicals Calculator
> : http://www.kademani.com/reefchem.htm
> :
> :
> :
> : Boomer
> :
> : Want to talk chemistry ? The Reef Chemistry Forum
> : http://www.reefcentral.com/vbulletin/index.php
> :
> :
> : Former US Army Bomb Technician (EOD)
> : Member; IABTI, NATEODA, WEODF, ISEE & IPS
> :
> : If You See Me Running You Better Catch-Up
> :
> :
> : --
> : Boomer
> :
> : Want to talk chemistry ? The Reef Chemistry Forum
> : http://www.reefcentral.com/vbulletin/index.php
> :
> : Want to See More ?
> : Please Join Our Growing Membership
> : www.coralrealm.com
> :
> : If You See Me Running You Better Catch-Up
> : "stoutman" <.@.> wrote in message
news:aGuWb.148227$U%5.676753@attbi_s03...
> : : Boomer,
> : :
> : : I am not sure if you are just messing with me or if you are truly
confused.
> : : I hope the latter. Please read from Top to Bottom.
> : :
> : :
> : : From YOUR first link:
> : :
> : : http://www.waterontheweb.org/resources/glossary.html
> : :
> : : Acidity:
> : : A measure of how acid a solution may be. A solution with a pH of less
than
> : : 7.0 is considered acidic. Solutions with a pH of less than 4.5 contain
> : : mineral acidity (due to strong inorganic acids), while a solution
having a
> : : pH greater than 8.3 contains no acidity.
> : :
> : : Yes,
> : :
> : : Good definition (for the most part). pH <7 is indeed acidic. pH > 7
is
> : : basic. Your web page had a definition for acidity, but not basicity.
> : : Strange. That's like defining GOOD and not defining BAD.
> : :
> : : Here is the IUPAC (International Union of Pure and Applied Chemistry)
> : : definition of acidity:
> : :
> : : http://www.chem.qmul.ac.uk/iupac/index.html
> : :
> : : acidity
> : :
> : : (1) Of a compound:
> : :
> : : For Brønsted acids it means the tendency of a compound to act as a
hydron
> : : donor. It can be quantitatively expressed by the acid dissociation
constant
> : : of the compound in water or some other specified medium. For Lewis
acids it
> : : relates to the association constants of Lewis adducts and -adducts.
> : :
> : : (2) Of a medium:
> : :
> : : The use of the term is mainly restricted to a medium containing
Brønsted
> : : acids, where it means the tendency of the medium to hydronate a
specific
> : : reference base
> : :
> : : basicity
> : :
> : : For Brønsted bases it means the tendency of a compound to act as
hydron
> : : (proton) acceptor. The basicity of a chemical species is normally
expressed
> : : by the acidity of the conjugate acid (see conjugate acid-base pair).
For
> : : Lewis bases it relates to the association constants of Lewis adducts
> : : and -adducts
> : :
> : :
> : :
> : : Another definition from the same web page YOU cited: (this is the
same web
> : : page you cited above)
> : :
> : : Alkalinity:
> : : Acid neutralizing or buffering capacity of water; a measure of the
ability
> : : of water to resist changes in pH caused by the addition of acids or
bases
> : : and therefore, the main indicator of susceptibility to acid rain; in
natural
> : : waters it is due primarily to the presence of bicarbonates, carbonates
and
> : : to a much lesser extent occasionally borates, silicates and
phosphates. It
> : : is expressed in units of milligrams per liter (mg/l) of CaCO3 (calcium
> : : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l = 1
mg/l
> : : of CaCO3. A solution having a pH below about 5 contains no alkalinity.
> : :
> : : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and
says
> : : that alkalinity is the measure of ...(description of a buffer)
> : :
> : : A BUFFER IS : a measure of the ability of water to resist changes in
pH
> : : caused by the addition of acids or bases (from definition below)
> : :
> : :
> : : I said:
> : : ***alkalinity is a measurement of 'buffering capacity'***
> : :
> : : You said:
> : : ***Alkalinity is not a measurement of BC
> : :
> : : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is
not
> : : logical.
> : :
> : : (THIS FROM THE SAME WEB PAGE YOU CITED):
> : :
> : : Buffer:
> : : A substance which tends to keep pH levels fairly constant when acids
or
> : : bases are added.
> : :
> : : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
> : :
> : : a measure of the ability of water to resist changes in pH caused by
the
> : : addition of acids or bases
> : :
> : : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A
BUFFER.
> : :
> : :
> : : I went to all four links. None contradict what I have said. But the
first
> : : one you cited contradicts YOU!
> : :
> : : I know what a buffer is. I know what acidity means. I know what
alkalinity
> : : means. No need to cite web pages that describe what I know and what I
wrote
> : : in this discussion. Show me one that says alkalinity is not a measure
of
> : : buffering capacity from a credible source.
> : :
> : :
> : :
> : :
> : :
> : :
> : : "Boomer" > wrote in message
> : : ...
> : : > Alkalinity a measure of the amount of anions of weak acid in water
and of
> : : the cations
> : : > balanced against them
> : : > Take note it says ***acid***
> : : >
> : : > Buffering capacity the ability of a solution to resist or dampen
changes
> : : in pH upon the
> : : > addition of acids or bases.
> : : > Take note its says ***the addition of acids or bases***
> : : >
> : : > One more
> : : >
> : : > http://www.waterontheweb.org/resources/glossary.html
> : : >
> : : > We could go on like this all day, so what is the point ?
> : : >
> : : > You will LOVE this one
> : : > http://www.kyantec.com/Tips/phbuffering.htm
> : : >
> : : > Don't you just lovbe PDF's
> : : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
> : : >
> : : > Don't fall out of your chair
> : : >
http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
> : : >
> : : >
> : : >
> : : >
> : : > --
> : : > Boomer
> : : >
> : : > Want to talk chemistry ? The Reef Chemistry Forum
> : : > http://www.reefcentral.com/vbulletin/index.php
> : : >
> : : > Want to See More ?
> : : > Please Join Our Growing Membership
> : : > www.coralrealm.com
> : : >
> : : > If You See Me Running You Better Catch-Up
> : : > "stoutman" <.@.> wrote in message
news:XB7Wb.19339$QA2.62332@attbi_s52...
> : : > : Man here is another, google is a wonderful thing. I'm not
filtering any
> : : > : out, just posting what I find by GOOGLING for you.
> : : > :
> : : > :
http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> : : > :
> : : > :
> : : > : Wow, a gov link. Even the government is wrong, this must be a
> : : conspiracy
> : : > : against Boomer.
> : : > :
> : : > :
> : : > :
> : : > :
> : : > : "Boomer" > wrote in message
> : : > : ...
> : : > : > Now I am getting bored
> : : > : >
> : : > : > "Don't the components of a buffer account for the buffering
capacity?
> : : > : Yes."
> : : > : >
> : : > : > Yes, agreed but you seem to fail what I'm saying. Buffering
Capacity
> : : and
> : : > : Alkalinity are
> : : > : > not the same, that has always been the issue. I gave the
equation does
> : : > : that look like an
> : : > : > Alkalinity equation or how Alk is determined. I see you had now
> : : comments
> : : > : on it what's
> : : > : > wrong, why no comments on the equations I gave. Don't understand
them
> : : or
> : : > : what ? Again this
> : : > : > is the equation for Buffering Capacity, also called Buffer Index
or
> : : Buffer
> : : > : Intensity. It
> : : > : > is defined in most water chemistry and chemical oceanography
text
> : : books.
> : : > : >
> : : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+]
+
> : : CKa
> : : > : [H3O+] / (Ka =
> : : > : > H3O+])² )
> : : > : >
> : : > : > This is not Alkalinity now is it ?
> : : > : >
> : : > : > "I know how to do a titration, In fact I have done several. How
many
> : : have
> : : > : > you actually done? I don't mean by counting drops, I mean with
a
> : : buret?"
> : : > : >
> : : > : > Well good for you, I use a Digital Titrator
> : : > : >
> : : > : > "Oh, I see,
> : : > : > you think acidity is the opposite of alkalinity. In the world
of
> : : > : CHEMISTRY
> : : > : > it's not. Maybe in aquarium newsgroups it is.
> : : > : >
> : : > : > Hum no, maybe you should go for a look at HACH's or LaMotte
website or
> : : the
> : : > : book I
> : : > : > suggested earlier. Please view a copy.
> : : > : >
> : : > : > Standard Methods for the Examination of Water and Wastewater
> : : > : >
> : : > : > This book, over 2000 pages, is the guide for water testing. If
you are
> : : > : reporting water
> : : > : > test to the EPA you must use approved std from this text.I t is
> : : prepared
> : : > : and published by
> : : > : > the EPA, American Water Works Association and American Public
Health
> : : > : Association. You
> : : > : > mean you don't have one and the issue is water chemistry
> : : > : >
> : : > : > You are confusing Acidity and Acidity as you know little about
water
> : : > : chemistry and
> : : > : > procedures and test methods
> : : > : >
> : : > : > From SMEWW, section 2-30, 2310 ACIDITY
> : : > : >
> : : > : > "Acidity of water is its quantative capacity to react with a
strong
> : : base
> : : > : to a designated
> : : > : > pH"
> : : > : >
> : : > : > This is how you test for it
> : : > : >
> : : > : > A std alkali titration to methyl orange or phenolphthalein
> : : > : > endpoint.
> : : > : >
> : : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that
write
> : : this
> : : > : book, there are
> : : > : > over 100 of them, they are wrong.
> : : > : >
> : : > : > Like Buffering Capacity you have your Acidity's mixed up
> : : > : > In water measurement if you have a high Alk you also usually
have a
> : : high
> : : > : Acidity.
> : : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
> : : CHEMISTRY
> : : > : BOOK there pal.
> : : > : >
> : : > : >
> : : > : > "These are all in equilibrium with each other. An initial high
pH
> : : (above
> : : > : > 6.4) will shift the equilibrium to the right to form HCO3-1. If
the
> : : pH of
> : : > : > the solution is above 10.3 (pKa2) the .........."
> : : > : >
> : : > : >
> : : > : > Christ, there you go again with the FW ****. All your numbers
are
> : : wrong we
> : : > : are dealing
> : : > : > with SEAWATER
> : : > : >
> : : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is
in the
> : : form
> : : > : > of HCO3-1 .
> : : > : >
> : : > : > I have already pointed that out and gave actual values at know
> : : seawater
> : : > : levels, go back
> : : > : > and re-read it you aren't telling me anything here.Of course
most is
> : : HCO3
> : : > : see...
> : : > : >
> : : > : >
> : : > : > @ 20C and 34.3 ppt salinity
> : : > : >
> : : > : > CO2 = 0.52 %
> : : > : >
> : : > : > HCO3 = 86.4 %
> : : > : >
> : : > : > CO3 = 13.09 %
> : : > : >
> : : > : >
> : : > : > "In your glass experiment you managed to lower the pH enough to
purge
> : : out
> : : > : CO2
> : : > : > by boiling"
> : : > : >
> : : > : > The purpose behind the glass is to show that alk is not affect
by CO2
> : : and
> : : > : vise-versa and
> : : > : > how Co2 affects pH.
> : : > : >
> : : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and that
pH
> : : drops
> : : > : to say 8.1 it is
> : : > : > usually due to excess CO2. If you took a glass of that water and
> : : aerated
> : : > : it you WILL drive
> : : > : > off the CO2 and raise the pH. It has been done a proven a
million
> : : times.
> : : > : >
> : : > : > "In order to 'purge' CO2 you would need to lower the
> : : > : > pH to shift the equilibrium to below 6.4"
> : : > : >
> : : > : > The hell you do !!!.Do you know who many times people on this NG
to
> : : > : include Dr. Craig
> : : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to
take a
> : : > : sample of aquarium
> : : > : > water and aerate it to see if the pH GOES UP AND when they come
back
> : : with
> : : > : the test it is
> : : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST
> : : excess
> : : > : CO2 in the tank
> : : > : > water, increase the circulation for better gas exchange at the
> : : surface,
> : : > : reduce feeding,
> : : > : > and try to improve on better skimming, thus reducing the
bio-load and
> : : pH
> : : > : decline due to
> : : > : > CO2.
> : : > : >
> : : > : >
> : : > : > "I hope this helps. "
> : : > : >
> : : > : > Help, how can you when you miss everything. I should be charging
you
> : : > : >
> : : > : > Oh, by the way. Your websites, I have about 50 on these issues,
I
> : : could
> : : > : post them, not to
> : : > : > mention I have all those water chemistry books, so there is no
need to
> : : > : view your sites.
> : : > : >
> : : > : > Finally are you afraid to come to our Chemistry Forum, afraid to
get
> : : > : slapped by REAL
> : : > : > chemists. I get a charge out of you can't post your ref .I have
posted
> : : the
> : : > : same or similar
> : : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have
1500
> : : posts
> : : > : there and am the
> : : > : > biggest contributor to his forum other than himself or maybe
Habib
> : : Sheka
> : : > : >
> : : > : > Hum, here are Randy's ref that he posted. He hosts the website
> : : > : >
> : : > : > S. RANDY HOLMES-FARLEY
> : : > : > Arlington, Massachusetts
> : : > : >
> : : > : > EDUCATION
> : : > : >
> : : > : > 1982-1986 Harvard University Cambridge, MA
> : : > : > PhD in Chemistry
> : : > : > Research Advisor: George Whitesides
> : : > : >
> : : > : > Investigated the relationship between polymer surface chemistry
and
> : : > : physical properties
> : : > : > through controlled surface modification and testing.
> : : > : >
> : : > : > 1980-1982 Cornell University Ithaca, NY
> : : > : > BA in Chemistry and Biology
> : : > : > Graduated Summa Cum Laude
> : : > : > Distinction in All Subjects
> : : > : > Grade Point: 3.94/4.0
> : : > : > Honors research: isolation and characterization of the subunit
of CF1
> : : > : enzyme
> : : > : >
> : : > : >
> : : > : > 1978-1979 Stanford University Palo Alto, CA
> : : > : > Grade Point: 3.55/4.0
> : : > : >
> : : > : >
> : : > : > EXPERIENCE
> : : > : >
> : : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham,
MA
> : : > : > (bought out GelTex Pharmaceuticals in 2001)
> : : > : > Vice President, Chemical Research 2001-present
> : : > : > Senior Director, Chemical Research 1999-2001
> : : > : > Director of Chemical Research 1997-1999
> : : > : > Manager of Chemical Research 1995-1997
> : : > : > Group Leader 1994-1995
> : : > : > Senior Research Scientist 1992-1994
> : : > : >
> : : > : > Helped start GelTex as second employee
> : : > : >
> : : > : > Managed various research programs with multi-million dollar
budgets
> : : > : >
> : : > : > Supervised research chemists (17+)
> : : > : >
> : : > : > Co-inventor of several polymeric pharmaceuticals and
pharmaceutical
> : : > : candidates including
> : : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam
Hydrochloride
> : : (FDA
> : : > : approved)
> : : > : >
> : : > : > Company Safety Officer for 3 years
> : : > : >
> : : > : > Chemical Hygiene Officer 2000-present
> : : > : >
> : : > : >
> : : > : >
> : : > : >
> : : > : > 1990-1992 GTE Corporation Waltham, MA
> : : > : > Senior Member of Technical Staff
> : : > : > Applied research involving polymer interfaces
> : : > : > Metallization of plastics
> : : > : > Polymer/polymer adhesion
> : : > : > Optical coatings
> : : > : >
> : : > : >
> : : > : >
> : : > : > 1986-1990 Lord Corporation Cary, NC
> : : > : > Senior Research Scientist 1988-1990
> : : > : > Research Scientist 1986-1988
> : : > : > Basic and applied research on surface chemical bonding
> : : > : > Developed new adhesive compositions
> : : > : > Developed new sol-gel coatings for corrosion resistance
> : : > : >
> : : > : >
> : : > : > HONORS AND AWARDS
> : : > : >
> : : > : > Industrial Innovations Award by Northeast Region of American
Chemical
> : : > : Society (6/2001)
> : : > : >
> : : > : > National Kidney Foundation of Northern California Honoree
(5/2001)
> : : > : >
> : : > : > American Chemical Society/Polymer Chemistry Division Industrial
> : : Sponsors
> : : > : > Award (8/2000)
> : : > : >
> : : > : > R&D 100 Award from R&D magazine (1999)
> : : > : >
> : : > : > Sherwin Williams Award in applied polymer science (9/85)
> : : > : >
> : : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985;
1985-1986)
> : : > : >
> : : > : > Award for highest GPA in Chemistry Department (6/82)
> : : > : >
> : : > : > Summa Cum Laude Honors in Chemistry (6/82)
> : : > : >
> : : > : > Phi Lamda Epsilon (6/82)
> : : > : >
> : : > : > Phi Beta Kappa (2/82)
> : : > : >
> : : > : > Cornell University Dean's List (1981, 1982)
> : : > : >
> : : > : > Harvard Book Club Award for highest GPA senior year (1978)
> : : > : >
> : : > : > First Place in western NY ACS high school chemistry exam (1977)
> : : > : >
> : : > : > 1978-1979
> : : > : >
> : : > : >
> : : > : > __________________
> : : > : > Randy Holmes-Farley
> : : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef
Central
> : : > : >
> : : > : > Hobby Experience: 8 years with reefs
> : : > : > Current Tanks: 90 gal mixed reef
> : : > : > Interests: Reefkeeping, science, photography
> : : > : >
> : : > : >
> : : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> : : > : >
> : : > : > Open this post in a new window | Report this post to a moderator
| IP:
> : : > : Logged
> : : > : >
> : : > : >
> : : > : >
> : : > : > 06/27/2003 02:44 PM
> : : > : >
> : : > : > Randy Holmes-Farley
> : : > : > Chemistry Moderator
> : : > : >
> : : > : > Registered: Apr 2001
> : : > : > Location: Arlington, Massachusetts
> : : > : > Occupation: Chemist (Drug Discovery at Genzyme)
> : : > : > Posts: 15282
> : : > : >
> : : > : >
> : : > : >
> : : > : > Publications
> : : > : >
> : : > : >
> : : > : > ISSUED UNITED STATES PATENTS
> : : > : >
> : : > : >
> : : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
> : : > : Mandeville, III; W. Harry.
> : : > : > US 6,566,407; 5/20/2003
> : : > : >
> : : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley,
Stephen
> : : Randall;
> : : > : Huval, Chad
> : : > : > Cori.
> : : > : > U.S. 6,517,825; 2/11/2003.
> : : > : >
> : : > : > 3. Method of making phosphate-binding polymers for oral
> : : administration.
> : : > : Holmes-Farley,
> : : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M.
U.S.
> : : > : 6,509,013; 1/21/2003.
> : : > : >
> : : > : > 4. Combination therapy for treating hypercholesterolemia using a
bile
> : : acid
> : : > : sequestrant
> : : > : > polymer
> : : > : > and a cholesterol-lowering agent. Huval, Chad Cori;
Holmes-Farley,
> : : Stephen
> : : > : Randall;
> : : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> : : > : >
> : : > : > 5. Method for treating hypercholesterolemia with polyallylamine
> : : polymers.
> : : > : Holmes-Farley,
> : : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
> : : Goldberg,
> : : > : Dennis I. , US
> : : > : > 6,423,754; 7/23/2002.
> : : > : >
> : : > : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry,
III;
> : : > : Neenan, Thomas X..;
> : : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> : : > : >
> : : > : > 7. Combination therapy for treating hypercholesterolemia and
> : : > : atherosclerosis. Huval, Chad
> : : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal,
Pradeep
> : : K.
> : : > : U.S. 6,365,186;
> : : > : > 4/2/2002.
> : : > : >
> : : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
> : : Mandeville,
> : : > : W. H., III;
> : : > : > Huval; C.
> : : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US
6,299,868;
> : : > : 10/9/2001.
> : : > : >
> : : > : > 9. Polymers containing guanidinium groups as bile acid
sequestrants.
> : : Dhal;
> : : > : P. K.; Holmes-
> : : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> : : > : >
> : : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.;
Mandeville, W.
> : : H.,
> : : > : III.; US
> : : > : > 6,281,252;
> : : > : > 8/28/2001.
> : : > : >
> : : > : > 11. Combination therapy for treating hypercholestrolemia. Huval;
C.
> : : C.;
> : : > : Holmes-Farley; S.
> : : > : > R. ;
> : : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> : : > : >
> : : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides,
G. M.;
> : : > : Holmes-Farley, S.
> : : > : > R.; US
> : : > : > 6,264,937; 7/24/2001.
> : : > : >
> : : > : > 13. Method for treating hypercholesterolemia with unsubstituted
> : : > : polydiallylamine polymers.
> : : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
K. ; US
> : : > : 6,248,318;
> : : > : > 6/19/2001.
> : : > : >
> : : > : > 14. Process for removing bile salts from a patient and alkylated
> : : > : compositions therefore.
> : : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355;
5/1/2001.
> : : > : >
> : : > : > 15. Poly(diallylamine)-based bile acid sequestrants.
Holmes-Farley, S.
> : : R.;
> : : > : Dhal, P. K.;
> : : > : > Petersen,
> : : > : > J. S.; US 6,203,785; 3/20/2001.
> : : > : >
> : : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S.
R.;
> : : Huval,
> : : > : C. C.; US
> : : > : > 6,190,649;
> : : > : > 2/20/2001.
> : : > : >
> : : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.;
Mandeville, W.
> : : H.,
> : : > : III.; US
> : : > : > 6,177,478;
> : : > : > 1/23/2001.
> : : > : >
> : : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
> : : Holmes-Farley,
> : : > : S. R.;
> : : > : > Mandeville, W.
> : : > : > H., III.; US 6,129,910; 10/10/2000.
> : : > : >
> : : > : > 19. Method for treating hypercholesterolemia with unsubstituted
> : : > : polydiallylamine polymers.
> : : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
K. ; US
> : : > : 6,083,497;
> : : > : > 7/4/2000.
> : : > : >
> : : > : > 20. Method of making phosphate-binding polymers for oral
> : : administration.
> : : > : Holmes-Farley, S.
> : : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495;
> : : 7/4/2000.
> : : > : >
> : : > : > 21. Process for removing bile salts from a patient and alkylated
> : : > : compositions therefore.
> : : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
> : : 5/23/2000.
> : : > : >
> : : > : > 22. Process for removing bile salts from a patient and
compositions
> : : > : therefor. Mandeville,
> : : > : > W. H.,
> : : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> : : > : >
> : : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W.
H;
> : : > : Neenan; T. X.; Holmes-
> : : > : > Farley; S. R. US 6,034,129; 3/7/2000.
> : : > : >
> : : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.;
Mandeville, W.
> : : H.,
> : : > : III.; US
> : : > : > 5,985,938;
> : : > : > 11/16/99.
> : : > : >
> : : > : > 25. Process for removing bile salts from a patient and
compositions
> : : > : therefor. Mandeville,
> : : > : > W. H.,
> : : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> : : > : >
> : : > : > 26. Hydrophobic sequestrant for cholesterol depletion.
Mandeville, W.
> : : H.,
> : : > : III.;
> : : > : > Holmes-Farley;
> : : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> : : > : >
> : : > : > 27. Hydrophilic nonamine-containing and amine-containing
copolymers
> : : and
> : : > : their use as bile
> : : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
> : : 5,929,184;
> : : > : 7/27/99.
> : : > : >
> : : > : > 28. Interpenetrating polymer networks for sequestration of bile
acids.
> : : > : Mandeville, W. H.,
> : : > : > III.;
> : : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US
5,925,379;
> : : > : 7/20/99.
> : : > : >
> : : > : > 29. Amine polymer sequestrant and method of cholesterol
depletion.
> : : > : Mandeville, W. H.,
> : : > : > III.;
> : : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> : : > : >
> : : > : > 30. Process for removing bile salts from a patient and
compositions
> : : > : therefor. Mandeville,
> : : > : > W. H.,
> : : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> : : > : >
> : : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
depletion.
> : : > : Mandeville, W. H.,
> : : > : > III.;
> : : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> : : > : >
> : : > : > 32. Process for removing bile salts from a patient and
compositions
> : : > : therefor. Mandeville,
> : : > : > W. H.,
> : : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> : : > : >
> : : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
> : : Mandeville,
> : : > : W. H., III.;
> : : > : > Holmes-
> : : > : > Farley, S. R.; US 5,703,188; 12/30/97.
> : : > : >
> : : > : > 34. Oral administration of iron-binding crosslinked amine
polymers.
> : : > : Mandeville, W. H.,
> : : > : > III.;
> : : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> : : > : >
> : : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
Holmes-Farley,
> : : S.
> : : > : R.; US 5,693,675;
> : : > : > 12/2/97.
> : : > : >
> : : > : > 36. Method for removing bile salts from a patient with alkylated
> : : > : crosslinked amine
> : : > : > polymers,
> : : > : > and preparation of the polymers. Mandeville, W. H., III.;
> : : Holmes-Farley,
> : : > : S. R.; US
> : : > : > 5,679,717; 10/21/97.
> : : > : >
> : : > : > 37. Phosphate-binding polymers for oral administration.
Holmes-Farley,
> : : S.
> : : > : R.; Mandeville,
> : : > : > W.
> : : > : > H., III.; US 5,667,775; 9/16/97.
> : : > : >
> : : > : > 38. Ion-exchange process using highly crosslinked polymers for
> : : removing
> : : > : bile salts from a
> : : > : > patient, preparation of the polymers, and compositions
containing
> : : them.
> : : > : Mandeville, W. H.,
> : : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> : : > : >
> : : > : > 39. Hydrophobic amine polymer sequestrant and method of
cholesterol
> : : > : depletion. Mandeville,
> : : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US
5,618,530;
> : : 4/8/97.
> : : > : >
> : : > : > 40. Amine polymer sequestrant and method of cholesterol
depletion.
> : : > : Mandeville, W. H.,
> : : > : > III.;
> : : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> : : > : >
> : : > : > 41. Phosphate-binding polymers for oral administration.
Holmes-Farley,
> : : S.
> : : > : R.; Mandeville,
> : : > : > W.
> : : > : > H., III.; US 5,496,545; 3/5/96.
> : : > : >
> : : > : > 42. Iron-binding polymers for oral administration. Mandeville,
W. H.,
> : : > : III.; Holmes-Farley,
> : : > : > S. R.;
> : : > : > US 5,487,888; 1/30/96.
> : : > : >
> : : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having
active
> : : > : hydrogens on the
> : : > : > surface.
> : : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> : : > : >
> : : > : > 44. Layered sol-gel coatings from organisilicon compounds.
> : : Holmes-Farley,
> : : > : S. R.; Yanyo, L.
> : : > : > C.;
> : : > : > US 5,182,143; 1/26/93.
> : : > : >
> : : > : > 45. Method for metal bonding using ultrathin primer coating.
> : : > : Holmes-Farley, S. R.; Yanyo,
> : : > : > L.
> : : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> : : > : >
> : : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey,
K. J.;
> : : US
> : : > : 5,096,962;
> : : > : > 3/17/92.
> : : > : >
> : : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> : : > : elastomer-metal bonding.
> : : > : > Holmes-
> : : > : > Farley, S. R.; US 5,102,956; 4/7/92.
> : : > : >
> : : > : >
> : : > : >
> : : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT
ISSUED)
> : : > : >
> : : > : >
> : : > : > 1. Aryl boronate functionalized polymers for treating obesity
and
> : : > : inhibiting fat uptake.
> : : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal,
> : : Pradeep
> : : > : K.; Huval, Chad
> : : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003),
92
> : : pp. WO
> : : > : 0302571.
> : : > : >
> : : > : > 2. Preparation of aryl boronic acids for treating obesity.
> : : Holmes-Farley,
> : : > : Stephen Randall;
> : : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal,
Pradeep
> : : K.
> : : > : (Geltex
> : : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO
0302570.
> : : > : >
> : : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide.
Holmes-Farley,
> : : > : Stephen Randall.
> : : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32
pp. WO
> : : > : 0302130.
> : : > : >
> : : > : > 4. Method for reducing copper levels and treating copper
toxicosis.
> : : > : Holmes-Farley, Stephen
> : : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl.
(2002),
> : : 45
> : : > : pp. WO
> : : > : > 0285383.
> : : > : >
> : : > : > 5. Method for treating gout and binding uric acid.
Holmes-Farley,
> : : Stephen
> : : > : Randall; Burke,
> : : > : > Steven K. WO 0285381 10/31/2002.
> : : > : >
> : : > : > 6. Method for treating gout and reducing serum uric acid.
> : : Holmes-Farley,
> : : > : Stephen Randall;
> : : > : > Burke, Steven K WO 0285380 10/31/2002.
> : : > : >
> : : > : > 7. Amine condensation polymer bile acid sequestrants. Huval, C.
C.;
> : : > : Holmes-Farley, S. R.;
> : : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> : : > : >
> : : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H.,
III and
> : : > : Holmes-Farley, S.
> : : > : > R.;
> : : > : > WO 1999-US5662; 9/23/1999.
> : : > : >
> : : > : > 9. Amine-containing copolymers as bile acid sequestrants.
> : : Holmes-Farley,
> : : > : S. R.; Petersen,
> : : > : > J. S.;
> : : > : > WO 9933452; 7/8/1999.
> : : > : >
> : : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H.,
III
> : : and
> : : > : Holmes-Farley, S.
> : : > : > R.;
> : : > : > WO 9922743; 5/14/1999.
> : : > : >
> : : > : > 11. Polyallylamine polymers for removing bile salts and treating
> : : > : hypercholesterolemia, and
> : : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H.,
III;
> : : Burke,
> : : > : S. K.; Goldberg,
> : : > : > D. I.; WO 9857652; 12/23/98.
> : : > : >
> : : > : > 12. Phosphate-bidning polymers combined with a calcium
supplement for
> : : oral
> : : > : administration.
> : : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
Holmes-Farley,
> : : S.
> : : > : R.; WO 9842355;
> : : > : > 10/1/98.
> : : > : >
> : : > : > 13. Hydrophobic heteroatom-containing sequestrant for
cholesterol
> : : > : depletion. Mandeville,
> : : > : > W.
> : : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449;
12/12/96.
> : : > : >
> : : > : > 14. Process for adjusting ion concentration in a patient and
> : : compositions
> : : > : therefor.
> : : > : > Mandeville,
> : : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> : : > : >
> : : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
> : : interlayer
> : : > : for improved
> : : > : > metal-
> : : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
> : : 1/20/94.
> : : > : >
> : : > : > 16. Process for increased metal-substrate bond strength in
metalized
> : : > : plastics.
> : : > : > Holmes-Farley, S.
> : : > : > R.; Ger. Offen. 4322516; 7/6/93.
> : : > : >
> : : > : > 17. Electrorheological fluids and preparation of particles
useful in
> : : the
> : : > : fluids.
> : : > : > Troughton,
> : : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie;
Carlson, J.
> : : > : David; Bares, Joseph
> : : > : > E.;
> : : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra
Nell. EP
> : : > : 394049;
> : : > : > 10/24/1990.
> : : > : >
> : : > : > JOURNAL PUBLICATIONS
> : : > : >
> : : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William;
Zhorov,
> : : Eugene;
> : : > : Guo, Amy;
> : : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
> : : > : Mandeville, W. Harry;
> : : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
> : : 611-619.
> : : > : >
> : : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
> : : synthesis
> : : > : and biological
> : : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley,
S.
> : : Randall;
> : : > : Mandeville, W.
> : : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal,
Pradeep K.
> : : > : Journal of
> : : > : > Macromolecular Science, Pure and Applied Chemistry (2001),
A38(12),
> : : > : 1559-1574.
> : : > : >
> : : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by
Molecular
> : : > : Imprinting. Huval,
> : : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley,
S.
> : : > : Randall; Mandeville,
> : : > : > W.
> : : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro,
Robert
> : : J.;
> : : > : Chen, Xi; Dhal,
> : : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> : : > : >
> : : > : > 4. Synthetic polymers for the binding of fat in the intestinal
tract.
> : : > : Jozefiak, Thomas H.;
> : : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia;
> : : Huval,
> : : > : Chad C.;
> : : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney,
Cynthia.
> : : > : Abstracts of
> : : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United States,
August
> : : > : 26-30, 2001
> : : > : > (2001), POLY-047 and Polymer Preprints (American Chemical
Society,
> : : > : Division of
> : : > : > Polymer Chemistry) (2001), 42(2), 98.
> : : > : >
> : : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel
polymer
> : : gel
> : : > : pharmaceutical.
> : : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen,
J.;
> : : Ward,
> : : > : J.; Sacchiero,
> : : > : > B.;
> : : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K.
A.;
> : : Chen,
> : : > : X.; Mazzeo, J.
> : : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
> : : > : >
> : : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl
and
> : : other
> : : > : bile acid
> : : > : > sequestrants.
> : : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.;
Xu, Q.;
> : : > : Hook, P.; Holmes-
> : : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1),
708-709.
> : : > : >
> : : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
> : : Holmes-Farley,
> : : > : S. R; Polym.
> : : > : > Mater. Sci. Eng (1999), 80, 246-247.
> : : > : >
> : : > : > 8. Design and characterization of of Sevelamer Hydrochloride: a
novel
> : : > : phosphate-binding
> : : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III;
Ward,
> : : J.;
> : : > : Miller, K. L.;
> : : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.-
Pure
> : : and
> : : > : Appl. Chem.,
> : : > : > A36(7&8), p. 1085 (1999).
> : : > : >
> : : > : > 9. Three generations of bile acid sequestrants. Mandeville, W.
H.,
> : : III;
> : : > : Braunlin, W.;
> : : > : > Dhal, P.;
> : : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik,
S.;
> : : > : Rosenbaum, D.;
> : : > : > Sacchiero,
> : : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc.
(1999),
> : : > : 550, 3-15.
> : : > : >
> : : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric
> : : phosphate
> : : > : binder, on
> : : > : > urinary
> : : > : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley,
S. R.;
> : : > : Mandeville, W. H.,
> : : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
Transplant.
> : : > : (1997), 12(5)
> : : > : > 961-964.
> : : > : >
> : : > : > 11. Thin anisotropic coatings based on sol-gel technology.
> : : Holmes-Farley,
> : : > : S. R.; Yanyo, L.
> : : > : > C;
> : : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem.
4),
> : : 439-444.
> : : > : >
> : : > : > 12. The mechanism of cure initiation of a surface activated
adhesive.
> : : > : Holmes-Farley, S.
> : : > : > R.;
> : : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5),
409-420.
> : : > : >
> : : > : > 13. Adhesion promotion and corrosion prevention using thin
anisotropic
> : : > : coatings. Holmes-
> : : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991),
5(2),
> : : > : 131-151.
> : : > : >
> : : > : > 14. Wetting of functionalized polyethylene having ionizable
organic
> : : acids
> : : > : and bases at the
> : : > : > polymer-water interface: relations between functional group
polarity,
> : : > : extent of
> : : > : > ionization,
> : : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
> : : > : Whitesides, G. M.;
> : : > : > Langmuir
> : : > : > (1988), 4(4), 921-937.
> : : > : >
> : : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols
with a
> : : > : single hydroxy group.
> : : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> : : > : >
> : : > : > 16. Reconstruction of the interface of oxidatively
functionalized
> : : > : polyethylene (PE-CO2H)
> : : > : > and
> : : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.;
Nuzzo,
> : : R.;
> : : > : McCarthy, T. J.;
> : : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also
Report
> : : (1987),
> : : > : AD-
> : : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> : : > : >
> : : > : > 17. Surface-modified polyethylene film: the relationship between
> : : surface
> : : > : chemistry and
> : : > : > physical
> : : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987,
47(11),
> : : 4537.
> : : > : >
> : : > : > 18. Reactivity of carboxylic acid and ester groups in the
> : : functionalized
> : : > : interfacial
> : : > : > region of
> : : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> : : > : differentiation of the
> : : > : > functional groups into shallow and deep subsets based on a
comparison
> : : of
> : : > : contact angle and
> : : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.;
Langmuir
> : : > : (1987), 3(1), 62-
> : : > : > 76.
> : : > : >
> : : > : > 19. Fluorescence properties of dansyl groups covalently bonded
tot he
> : : > : surface of
> : : > : > oxidatively
> : : > : > functionalized low-density polyethylene film. Holmes-Farley, S.
R.;
> : : > : Whitesides, G. M.;
> : : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
> : : > : AD-A162435/2/GAR,
> : : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> : : > : >
> : : > : > 20. Acid-base behavior of carboxylic acid groups covalently
attached
> : : at
> : : > : the surface of
> : : > : > polyethylene: The usefulness of contact angle in following the
> : : ionization
> : : > : of surface
> : : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T.
J.;
> : : > : Deutch, J.;
> : : > : > Whitesides,
> : : > : > G. M.; Langmuir (1985), 1(6), 725-740.
> : : > : >
> : : > : > 21. The thermal stability of a surface modified solid organic
polymer.
> : : > : Holmes-Farley, S.
> : : > : > R.;
> : : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
> : : > : >
> : : > : >
> : : > : >
> : : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> : : > : >
> : : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R.
Advanced
> : : > : Aquarist. June 2003.
> : : > : >
> : : > : > 2. The Self Purification of Limewater (Kalkwasser).
Holmes-Farley, R.
> : : > : Advanced Aquarist.
> : : > : > May
> : : > : > 2003.
> : : > : >
> : : > : > 3. The Degradation of Limewater (Kalkwasser) in Air.
Holmes-Farley, R.
> : : > : Reefkeeping May
> : : > : > 2003.
> : : > : >
> : : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
Reefkeeping
> : : > : April 2003.
> : : > : >
> : : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae
Growth.
> : : > : Holmes-Farley, R.
> : : > : > Advanced Aquarist; April 2003.
> : : > : >
> : : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae
Growth.
> : : > : Holmes-Farley, R.
> : : > : > Advanced Aquarist; April 2003.
> : : > : >
> : : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced
> : : Aquarist;
> : : > : March 2003.
> : : > : >
> : : > : > 8. How to Select a Calcium and Alkalinity Supplementation
Scheme.
> : : > : Holmes-Farley, R.
> : : > : > Advanced Aquarist; February 2003.
> : : > : >
> : : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
January
> : : > : 2003.
> : : > : >
> : : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> : : December
> : : > : 2002.
> : : > : >
> : : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
> : : Advanced
> : : > : Aquarist; November
> : : > : > 2002.
> : : > : >
> : : > : > 12. Iron: A Look at Organisms Other than Macroalgae.
Holmes-Farley, R.
> : : > : Advanced Aquarist;
> : : > : > November 2002.
> : : > : >
> : : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced
> : : Aquarist,
> : : > : September 2002.
> : : > : >
> : : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist,
August
> : : > : 2002.
> : : > : >
> : : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com,
April
> : : > : 2002.
> : : > : >
> : : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R.
Advanced
> : : > : Aquarist; July 2002
> : : > : >
> : : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced
Aquarist;
> : : June
> : : > : 2002.
> : : > : >
> : : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley,
R.
> : : Advanced
> : : > : Aquarist, May
> : : > : > 2002.
> : : > : >
> : : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in
Corals.
> : : > : Holmes-Farley, R.
> : : > : > Advanced Aquarist, April 2002.
> : : > : >
> : : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> : : > : >
> : : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February
2002.
> : : > : >
> : : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist,
January
> : : 2002.
> : : > : >
> : : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium
Frontiers
> : : > : 2000.
> : : > : >
> : : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R.
Aquarium
> : : > : Frontiers 2000.
> : : > : >
> : : > : > 25. Phosphate..What is it and why should you care.
Holmes-Farley, R.
> : : > : Aquarium Frontiers
> : : > : > 2000.
> : : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
> : : Frontiers
> : : > : 2000.
> : : > : >
> : : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium
Frontiers
> : : 2000.
> : : > : >
> : : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers
1999.
> : : > : >
> : : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> : : > : >
> : : > : >
> : : > : >
> : : > : >
> : : > : >
> : : > : >
> : : > : >
> : : > : > Boomer
> : : > : >
> : : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : : > : > http://www.reefcentral.com/vbulletin/index.php
> : : > : >
> : : > : > Want to See More ?
> : : > : > Please Join Our Growing Membership
> : : > : > www.coralrealm.com
> : : > : >
> : : > : >
> : : > : >
> : : > :
> : : > :
> : : >
> : : >
> : :
> : :
> : :
> :
> :
>
>

[stoutman]

You spelled CANTANKEROUS correctly and misspelled SNOT-NOSED. Too funny.
LOL. :)



"Benjamin" > wrote in message
...
> Boomer,
>
> Why are you still dwelling on all this? Can't we talk about what you
> really want the world to know about Reef Aquarium Chemistry now? Can you
do
> it in a language and manner that even a "snoot-noise kid" can grasp and
> appreciate? Could you set aside your apparently cantankerous nature long
> enough so many can learn something valuable from you without feeling... um
> never mind I can't find the word for it.
>
> --
> --
>
> My Web Site: http://showcase.netins.net/web/reefpage/
>
>
> "Boomer" > wrote in message
> ...
> > "As it is the ability to neutralizes an acid that is a buffer"
> >
> > sorry
> >
> > As it is the ability to neutralizes a base that is a buffer
> >
> > --
> > Boomer
> >
> > Want to talk chemistry ? The Reef Chemistry Forum
> > http://www.reefcentral.com/vbulletin/index.php
> >
> > Want to See More ?
> > Please Join Our Growing Membership
> > www.coralrealm.com
> >
> > If You See Me Running You Better Catch-Up
> > "Boomer" > wrote in message
> > ...
> > :
> > : "I am not sure if you are just messing with me "
> > :
> > : Yes, messing with you, it is called trolling a troll, to see where the
> hell you would go
> > : and what you would say in regards to last posts. It is called honesty,
> of which you have
> > : none off to say the least,that I can see.You always like to post what
> suits you and just
> > : avoid ref I give. So lets start where you are WRONG and have a great
> lack of
> > understanding
> > : of things, to include pointing out all your gross error which you
still
> FAIL to
> > : acknowledge and which can be prove in many water chem. ref. .I doubt
> like hell you are a
> > : chemist at all.You seem to want to con people into thinkin' you are.
But
> then again, I
> > : have seen chemists like you before, they are not familiar with the,
but
> they ASK to have
> > : it explained and ask for REF.YOU just shoot from the hip. WHAT GETS
YOU
> IN TROUBLE. You
> > : remind me of snoot-noise kid that come here and other NG's and
> forums...that think they
> > : know, buy hey, maybe I'm wrong :-)
> > :
> > :
> > :
> > : 1). Acidity
> > :
> > : "***Benjamin,Water Chemistry (2002, pages 262-263).***
> > :
> > : ***Acidity A concept that is exactly analogous to alkalinity but
> measures the base
> > : neutralizing
> > : capacity (BNC) of a solution is Acidity. The quantitative represents
the
> concentration
> > of
> > : OH- ions that must be added to titrate the solution to a pH near
10.5***
> > :
> > : So that means that not only in Benjamin wrong but, so are Stumm &
> Morgan, Millero,
> > Pilosn,
> > : Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I
> said, you have
> > your
> > : acidity and Acidy mixed up. Acidity as defined above is covered in
most
> water chemistry
> > : books, written by chemists, who's field of expertise is water
chemistry.
> You can even
> > buy
> > : Acidity test kits from, HACH, LaMotte, etc..
> > :
> > : You mean you didn't read this or are you just avoiding it .The same
> definition can be
> > : found in almost any std water chemistry book.
> > :
> > : I have run into few chemists, that are NOT familiar with the above.
Some
> water reports
> > : require the above Acidity measuring. The issue with you is you do not
> understand WATER
> > : CHEMISTRY. Everything you have posted can be found a general chemistry
> book
> > :
> > :
> > :
> > :
> > : 2) Alk and BC
> > :
> > : From the link
> > :
> > : Alkalinity
> > : ***Acid neutralizing or buffering capacity of water; a measure of the
> ability of water
> > to
> > : resist changes in pH caused by the addition of acids or bases ***
> > :
> > : This is a Buffering Capacity definition not Alk
> > :
> > : Humm, since when does Alk have anything to do in regards to the
addition
> of BASE. As I
> > : pointed out in the first post the term is often miss used. Even in
YOUR
> own posts you
> > say
> > : it is based on a acid addition, no mention of **base or acid**
addition
> by you. Are you
> > : getting confused or what. Or is more you are trying to confuse
everyone
> you are right.
> > The
> > : above is a definition for Buffer Capacity NOT Alk
> > :
> > : From Drew, Geochemistry of Natural Waters
> > :
> > : "alkalinity, which is formally defined as the equivalent sum of bases
> that are
> > titratable
> > : with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH
of
> the solution is
> > : progressively lowered by the addition of a strong acid (HCL), all the
> anions on the
> > right
> > : will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4,
> H2S,organic acids, H20)"
> > :
> > : This follows almost all description of Alk, that it is acid
neutralizing
> reaction and
> > has
> > : nothing to do with base neutralizing, which is Acidity (BNC) .I
defined
> these before you
> > : had no comment
> > :
> > :
> > : Even the links that give the Buffering Capacity definition is wrong,
as
> is the UIPAC on
> > : Alkalinity. Alkalinity has nothing to do with the addition of bases
only
> acids. When you
> > : use the words "base and acid" it becomes BC
> > :
> > : Even YOU MUST disagree with these definitions, from YOUR own post
> > :
> > : Think of alkalinity as 'buffering capacity'. Or the ability of a
> solution
> > : ***to resist a drop in pH due to the addition of acid***
> > :
> > : Where the flip is the base addition forget it ?
> > :
> > : From Butler; Carbon Dioxide Equilibrium and Their Applications
> (professor emeritus
> > : Harvard University) an expert on the subject.
> > :
> > : Buffering Index (Buffering Capacity, Buffer Intensity).
> > :
> > : ***This concept was first developed for mixtures of approximately
equal
> proportions of
> > : conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such
> buffer solutions
> > : strongly resist changes in pH when acids or bases are added and are
> useful as pH
> > : standards. The Buffer Index tells how great the resistance to pH
changes
> will be.**
> > :
> > : also from Butler
> > :
> > : Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
> > :
> > : Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
> > :
> > : Acidity is in fact just the negative of Alkalinity ***
> > :
> > : http://www.lagoonsonline.com/acid.htm
> > :
> > :
>
http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.h
tm?E+mystore
> > :
> > : It sure is funny how all of the chemist that write water chemistry
> textbooks never say
> > Alk
> > : is the Buffering Capacity of a solution. They are always treated and
> defined separately.
> > :
> > : If you or others choose to treat Alk and BC as the same, well, just
have
> at it. As I
> > said
> > : in first post I know what you mean.
> > :
> > : "No need to cite web pages that describe what I know and what I wrote
> > : in this discussion"
> > :
> > : No you don't know, who are you trying to convince any way, me, the
guys
> here and/or all
> > : the water chemists in this world. As I said before go get a dam WATER
> CHEMISTRY book or
> > : shut the hell up.You keep trying to define things from a general
> chemistry book WE ARE
> > IN
> > : THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
> > :
> > :
> > :
> > :
> > :
> > : 3). pKa's and what you don't know or seem to be confused on
> > :
> > : "Therefore, it has two pKa's
> > : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
> The
> > : pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated
is
> > : right in there. Is that magic? :)"
> > :
> > : Here it is agin that is twice at least
> > :
> > : "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this
> example)
> > : you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium
> will
> > : be shifted to HCO3-2 by a ratio of 1:100.
> > :
> > : Oh wait , there is a third time LOL
> > :
> > : "At the pH of seawater, the buffering capacity of carbonate is at it's
> > : weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
> > :
> > :
> > : Lets just dunk you on this one. I am taking note you refuse to reply
to
> YOUR errors
> > :
> > : So you calculated the pH of seawater with freshwater pKa's, now that
is
> a good trick.
> > From
> > : a number of seawater chemistry books the seawater pKa's are 6 & 9.1,
so
> according to
> > you,
> > : seemingly not understanding your favorite Henderson-Hasselbach
equation;
> > :
> > : 2 pH = (6 + 9.1) /2 pH = 7.55
> > :
> > : I have never seen seawater with a pH of 7.55. There is no ocean with
> that pH. Humm how
> > : come your equation is not working for you today.?
> > :
> > :
> > : "That pH I calculated is
> > : right in there. Is that magic? :)"
> > :
> > : I roll on the floor when I see this = 8.35
> > :
> > : Hum , just a brain far so excuse me for thinkin
> > :
> > : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
> > :
> > : Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a
pH
> of 8.35 there
> > pal
> > : ? That 8.35 is what you are telling people the pH should be, but their
> meter says 6.4.
> > : This how people will READ this.
> > :
> > :
> > :
> > :
> > : 4.) More on Buffering Capacity
> > :
> > : "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes,
> your
> > : alkalinity equation."'
> > :
> > :
> > : Yup, I see that and in this case the HCO3 is the acid and the CO3 is
the
> base CORRECT.
> > In
> > : Alk you are only dealing with bases and how they react to an acid.
> Acidity deals acids
> > and
> > : how they recact to bases "Acidity, A concept that is exactly analogous
> to alkalinity but
> > : measures the base neutralizing
> > : capacity (BNC) of a solution is Acidity "Alk is the ANC Acid
> neutralizing capacity
> > :
> > : "Don't the components of a buffer account for the buffering capacity?
"
> > :
> > : Yes, they do but so do the acids which work as buffers. NaHCO3 is a
> buffer and can act
> > as
> > : an acid or base
> > :
> > : *** Buffering Capacity.**
> > : The power of a substance in solution to absorb acid or alkali without
> change in pH; this
> > : is highest at a pH value equal to the pKa value of the acid of the
> buffer pair.***
> > :
> > : ***Akalinity***
> > : Measure of the power of a solution to neutralise hydrogen ions (H+),
> usually expressed
> > as
> > : the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
> > :
> > :
> > : If one wants to call Alk Buffering capacity then one sure as a hell
can
> call Acidty
> > : Buffering Capacity also. As it is the ability to neutralizes an acid
> that is a
> > buffer.You
> > : have a pH of 7 and you add a buffer to lower it to a pH of 4, you are
> buffering the
> > water,
> > : that buffer is a acid.
> > :
> > : 5) CO2
> > :
> > : You are really confuse so it seems :-) You realllllllly indicate that
> CO2 is affected by
> > : the Alk or vise-versa
> > :
> > : "Yes, the pH will drop with the addition of CO2. Remove CO2 will
cause
> the
> > : pH to rise? How do you remove CO2? Once it is in solution it forms
> > : carbonic acid and neutralizes some of your 'buffer'."
> > :
> > : "With the exception of CO2?"
> > :
> > : No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
> > : Concepts)....PERIOD.You seem to think a that at least in two of your
> post that CO2 is
> > : affected by the Alk or vise-versa. Please go back to school or seek
> professor
> > :
> > : "Why in one case does CO2 from air lower pH and in the other case it
> raises
> > : it? Doesn't make sense."
> > :
> > : That is because you don't understand CO2 period. By the way I saved
> this, wanted to see
> > : if you would bite on the post I gave. Not bite at first, so time to
reel
> you in, as you
> > : did bite in another post..
> > :
> > : Lets make some sense of it for you, being that you have a pH.D in
> chemistry, so you say
> > .
> > :
> > : CO2 is naturally generated in a aquatic systems, it is capable of
raise
> to various
> > levels
> > : depending on a number of circumstances .It can be measure (except in
> seawater) or
> > : calculated using Buch/Park Equations (what we use for seawater. In
sort
> if you know the
> > pH
> > : and Alk you can calculate the CO2). If you aerate a system or a sample
> of water, even if
> > : the pH has only dropped a couple of tenths, due to an increase in CO2,
> the CO2 will
> > leave
> > : solution to the atmosphere.This will raise the pH. On the other hand
if
> theCO2 level is
> > : more of the norm and you have hikgh room air, such as in the winter,
the
> partial
> > pressure
> > : of the CO2 in air will be much higher than that in water, in which
case
> the CO2 will
> > enter
> > : the water and lower the pH. That is without an airstone. Adding an
> airstone will make it
> > : even worse,as you are now forcefully driving the CO2 into solution
even
> quicker. These
> > : test /experiments have been proven many times, it is not that may work
> could work they
> > do
> > : work.Yet you want to disagree and in another post say you haven't
tried
> it,.Seems to me
> > : that based on what you say it can't work So, in short you don't know
> what the hell you
> > are
> > : taking about. Go get a glass of seawater with a pH of about 8.3 and
> lower it to about
> > : 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK-
UP
> ( that is if you
> > : don't have a high room air CO2 problem.). This little test has been
done
> thousands of
> > : times in this hobby, with test kits, pH meters and even graphic
> printers.
> > :
> > : "This is where Boomer and I
> > : disagree. I say you would have to lower the pH very low in order to
> > : effectively remove CO2 by purging."
> > :
> > : You are 100 % wrong. Please come to our Chem forum and try and run
that
> by Randy, don't
> > : take my word on it. I already know what he will say.
> > :
> > : "Boomer didnt convince me it
> > : works at the pH of an aquarium, but I never tried it and I'm not sure
of
> > : this. "
> > :
> > : Well then come too our chem. forum and tell Randy he doesn't know what
> he is talking
> > about
> > : LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it
> should be easy for
> > : you to run the experiment LOL There are grade school kids that run the
> test and know
> > what
> > : happens and that I'm correct.
> > :
> > :
> > : "The equilibrium is a FUNCTION
> > : of pH."
> > :
> > : It is also a function of Alk or don't you know that. At a pH of 8.3,
Alk
> 2.25, the CO2
> > is
> > : about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk
to
> about .4 meq/ l
> > : or so the CO2 will be around .99 mg / l CO2, When dealing with
tanksCO2
> is not always in
> > : equilibrium with ambient air.
> > :
> > :
> > : ". But I wouldn't degas a solution of a
> > : specific gas (CO2) with a gas (this case he was using air) that
contains
> the
> > : same gas I am trying to purge."
> > :
> > : Why not ? We have a guy right now that is running tests on purging
> ambient air with a
> > : solution to remove CO2 gas from the air, before it enters the tank
> per/Randy's
> > suggestion.
> > : The same guy is doing some of my test using a Clinoptilolite, a
Zeolite
> mineral, that
> > has
> > : an affinity for CO2.This will be a dry CO2 scrubber
> > :
> > :
> > : Sorry Soutman but you sure as hell don't seem to know much about
aquatic
> chemistry. You
> > : seem to be guessing at everything.
> > :
> > : By the way have you read any of Randy's technical articles on water
> chemistry, been
> > saving
> > : these for last. There are a few on pH, Alk, CO2 .Here is a list
> > :
> > : Try and answer them 1-5 and lets see where we get THIS TIME :-) or
maybe
> we should just
> > : drop it. I could care less at this point.
> > :
> > : THE END
> > :
> > :
> > : ARTICLES
> > :
> > : The first two posts in this thread are lists of some of my articles
that
> relate to reef
> > : tank chemistry. In the next few posts are some of the articles
published
> by Craig
> > Bingman
> > : and others on reef chemistry issues.
> > :
> > : The first two posts in this thread are lists of some of my articles
that
> relate to reef
> > : tank chemistry. In the next few posts are some of the articles
published
> by Craig
> > Bingman
> > : and others on reef chemistry issues.
> > :
> > : Solving Common Problems
> > :
> > : Solving Calcium and Alkalinity Problems
> > : http://www.advancedaquarist.com/issues/nov2002/chem.htm
> > :
> > : Solutions to pH Problems
> > : http://www.advancedaquarist.com/iss...ne2002/chem.htm
> > :
> > : How to Select a Calcium and Alkalinity Supplementation Scheme
> > : http://www.advancedaquarist.com/issues/feb2003/chem.htm
> > :
> > : Phosphate Issues
> > : http://www.advancedaquarist.com/iss...pt2002/chem.htm
> > :
> > : Nitrate Issues
> > : http://www.advancedaquarist.com/iss...st2003/chem.htm
> > :
> > :
> > :
> > : Calcium and Alkalinity
> > :
> > : Solving Calcium and Alkalinity Problems
> > : http://www.advancedaquarist.com/issues/nov2002/chem.htm
> > :
> > : How to Select a Calcium and Alkalinity Supplementation Scheme
> > : http://www.advancedaquarist.com/issues/feb2003/chem.htm
> > :
> > : Calcium and Alkalinity Balance Issues
> > : http://reefkeeping.com/issues/2002-...ature/index.htm
> > :
> > : Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
> > : http://www.advancedaquarist.com/iss...ly2002/chem.htm
> > :
> > : The Relationship Between Alkalinity and pH.
> > : http://www.advancedaquarist.com/issues/may2002/chem.htm
> > :
> > : The Chemical & Biochemical Mechanisms of Calcification in Corals
> > : http://www.advancedaquarist.com/issues/apr2002/chem.htm
> > :
> > : Calcium
> > : http://www.advancedaquarist.com/issues/mar2002/chem.htm
> > :
> > : Alkalinity
> > : http://www.advancedaquarist.com/iss...2/chemistry.htm
> > :
> > :
> > : Iron
> > :
> > : First Iron Article: Macroalgae and Dosing Recommendations
> > : http://www.advancedaquarist.com/issues/aug2002/chem.htm
> > :
> > : Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> > : http://www.advancedaquarist.com/issues/oct2002/chem.htm
> > :
> > : Iodine
> > :
> > : Iodine in Marine Aquaria: Part I
> > : http://www.advancedaquarist.com/issues/mar2003/chem.htm
> > :
> > : Iodine in Reef Tanks 2: Effects on Macroalgae Growth
> > : http://www.advancedaquarist.com/iss...il2003/chem.htm
> > :
> > :
> > : Magnesium and Strontium
> > :
> > : Strontium
> > : http://www.advancedaquarist.com/issues/nov2003/chem.htm
> > :
> > : Magnesium
> > : http://www.advancedaquarist.com/issues/oct2003/chem.htm
> > :
> > : Magnesium and Strontium in Limewater
> > : http://www.advancedaquarist.com/issues/dec2003/chem.htm
> > :
> > :
> > : Limewater (kalkwasser)
> > :
> > : The Self Purification of Limewater (Kalkwasser)
> > : http://www.advancedaquarist.com/issues/may2003/chem.htm
> > :
> > : The Degradation of Limewater (Kalkwasser) in Air
> > : http://reefkeeping.com/issues/2003-...ature/index.htm
> > :
> > : How to Select a Calcium and Alkalinity Supplementation Scheme
> > : http://www.advancedaquarist.com/issues/feb2003/chem.htm
> > :
> > : Metals in Aquaria
> > :
> > : Aluminum and aluminum-based phosphate binders
> > : http://www.advancedaquarist.com/iss...ly2003/chem.htm
> > :
> > : Reef Aquaria with Low Soluble Metals
> > : http://reefkeeping.com/issues/2003-...ature/index.htm
> > :
> > : Tap Water in Reef Aquaria
> > : http://www.advancedaquarist.com/issues/jan2004/chem.htm
> > : First Iron Article: Macroalgae and Dosing Recommendations
> > : http://www.advancedaquarist.com/issues/aug2002/chem.htm
> > :
> > : Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> > : http://www.advancedaquarist.com/issues/oct2002/chem.htm
> > :
> > :
> > : Test Kit Reviews
> > :
> > : The Seachem Borate Alkalinity Test Kit
> > : http://www.advancedaquarist.com/iss...ne2003/chem.htm
> > :
> > : The Salifert Boron Test Kit
> > : http://www.advancedaquarist.com/iss...pt2003/chem.htm
> > :
> > : Boron and Borate (and pH buffering)
> > :
> > : Boron in a Reef Tank (and its effect on pH buffering)
> > : http://www.advancedaquarist.com/issues/dec2002/chem.htm
> > :
> > : The Seachem Borate Alkalinity Test Kit
> > : http://www.advancedaquarist.com/iss...ne2003/chem.htm
> > :
> > : The Salifert Boron Test Kit
> > : http://www.advancedaquarist.com/iss...pt2003/chem.htm
> > :
> > :
> > :
> > : Others
> > :
> > : Tap Water in Reef Aquaria
> > : http://www.advancedaquarist.com/issues/jan2004/chem.htm
> > :
> > : ORP
> > : http://reefkeeping.com/issues/2003-...ature/index.htm
> > :
> > : Chloramine
> > : http://reefkeeping.com/issues/2003-...ature/index.htm
> > :
> > : Silica in a Reef Tank
> > : http://advancedaquarist.com/issues/jan2003/feature.htm
> > :
> > : Specific Gravity (and temperature correction of hydrometers)
> > : http://www.advancedaquarist.com/iss...2/chemistry.htm
> > :
> > :
> > : The Complete Nitrogen Cycle
> > : http://www.animalnetwork.com/fish/l...a&RecordNo=3090
> > :
> > : Magnesium (older article with fonts screwed up)
> > : http://www.aquariumfish.com/aquariu...cid=124&search=
> > :
> > : Phosphate (older article now reproduced in a poor fashion)
> > : http://www.aquariumfish.com/aquariu...cid=124&search=
> > :
> > : Carbon Dioxide
> > : http://www.animalnetwork.com/fish/l...a&RecordNo=2074
> > :
> > : Using Conductivity to Measure Salinity
> > : http://www.aquariumfish.com/aquariu...cid=124&search=
> > :
> > : Understanding Seawater
> > : http://www.animalnetwork.com/fish2/...s/1/default.asp
> > :
> > : Protein Skimming: How It Works
> > : http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
> > :
> > :
> > :
> > : Articles by Craig Bingman:
> > :
> > : Carbon Dioxide tests
> > : http://www.animalnetwork.com/fish/l...n=&RecordNo=279
> > :
> > : Limewater, Acetic Acid and Sand Clumping
> > : http://www.animalnetwork.com/fish/l...n=&RecordNo=181
> > :
> > : Calcium and Alkalinity
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Calculation of Calcium Carbonate Saturation States in Reef Aquaria
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > :
> > : Calcification Rates in Several Tropical Coral Reef Aquaria
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Limits To Limewater...Revisited
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Expanding the Limits of Limewater: Adding Organic Carbon Sources
> (vinegar)
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > :
> > : Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Magnesium - Part I
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Magnesium - Part II
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : A Homemade Magnesium Supplement
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Simulating the Effect of Calcium Chloride and Sodium Bicarbonate
> Additions on Reef
> > Systems
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Additional Simulations: The Combined Effect Of Calcium Chloride
> > : /Sodium Bicarbonate Additions And Water Exchanges
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > :
> > : More articles by Craig Bingman:
> > :
> > : The Halogens - Part I: Bromine in Seawater and Aquaria
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : The Halogens - Part II: Fluoride
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Fluoride Depletion In Four Reef Aquariums
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : The Halogens - Part III: Iodine
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Measuring Halides
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : How Test Kits Work
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Borax pH Calibration
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : A pH Detective Story
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : How to Mix a Batch of Synthetic Seawater in Under Five Minutes
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : SILICON - FOE OR FRIEND?
> > : http://www.animalnetwork.com/fish2/...s/1/default.asp
> > :
> > : The Composition Of Several Synthetic Seawater Mixes
> > : http://www.animalnetwork.com/fish2/...s/1/default.asp
> > :
> > : Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > :
> > :
> > : Andy's calcium calculator
> > : http://www.andy-hipkiss.co.uk/cacalc.htm
> > :
> > : Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
> > : http://www.aquariumfish.com/aquariu...cid=124&search=
> > :
> > : Calcium Reactor Substrate -- Phosphate Levels
> > : by Greg Hiller
> > : http://www.advancedaquarist.com/iss...l2003/short.htm
> > :
> > :
> > : Indoor CO2 Problems
> > : http://www.advancedaquarist.com/iss...r2002/short.htm
> > :
> > : Simon Huntington's CaCO3/CO2 reactor article
> > :
> > : http://reefkeeping.com/issues/2002-...ature/index.htm
> > :
> > : Ron Shimek's Tank Water Analysis Article
> > : http://reefkeeping.com/issues/2002-...ature/index.htm
> > :
> > :
> > :
> > :
> > : Home made salinity standards thread:
> > :
> > : http://reefcentral.com/forums/showt...?threadid=65509
> > :
> > : Reef Chemicals Calculator
> > : http://www.kademani.com/reefchem.htm
> > :
> > :
> > :
> > : Boomer
> > :
> > : Want to talk chemistry ? The Reef Chemistry Forum
> > : http://www.reefcentral.com/vbulletin/index.php
> > :
> > :
> > : Former US Army Bomb Technician (EOD)
> > : Member; IABTI, NATEODA, WEODF, ISEE & IPS
> > :
> > : If You See Me Running You Better Catch-Up
> > :
> > :
> > : --
> > : Boomer
> > :
> > : Want to talk chemistry ? The Reef Chemistry Forum
> > : http://www.reefcentral.com/vbulletin/index.php
> > :
> > : Want to See More ?
> > : Please Join Our Growing Membership
> > : www.coralrealm.com
> > :
> > : If You See Me Running You Better Catch-Up
> > : "stoutman" <.@.> wrote in message
> news:aGuWb.148227$U%5.676753@attbi_s03...
> > : : Boomer,
> > : :
> > : : I am not sure if you are just messing with me or if you are truly
> confused.
> > : : I hope the latter. Please read from Top to Bottom.
> > : :
> > : :
> > : : From YOUR first link:
> > : :
> > : : http://www.waterontheweb.org/resources/glossary.html
> > : :
> > : : Acidity:
> > : : A measure of how acid a solution may be. A solution with a pH of
less
> than
> > : : 7.0 is considered acidic. Solutions with a pH of less than 4.5
contain
> > : : mineral acidity (due to strong inorganic acids), while a solution
> having a
> > : : pH greater than 8.3 contains no acidity.
> > : :
> > : : Yes,
> > : :
> > : : Good definition (for the most part). pH <7 is indeed acidic. pH >
7
> is
> > : : basic. Your web page had a definition for acidity, but not
basicity.
> > : : Strange. That's like defining GOOD and not defining BAD.
> > : :
> > : : Here is the IUPAC (International Union of Pure and Applied
Chemistry)
> > : : definition of acidity:
> > : :
> > : : http://www.chem.qmul.ac.uk/iupac/index.html
> > : :
> > : : acidity
> > : :
> > : : (1) Of a compound:
> > : :
> > : : For Brønsted acids it means the tendency of a compound to act as a
> hydron
> > : : donor. It can be quantitatively expressed by the acid dissociation
> constant
> > : : of the compound in water or some other specified medium. For Lewis
> acids it
> > : : relates to the association constants of Lewis adducts and -adducts.
> > : :
> > : : (2) Of a medium:
> > : :
> > : : The use of the term is mainly restricted to a medium containing
> Brønsted
> > : : acids, where it means the tendency of the medium to hydronate a
> specific
> > : : reference base
> > : :
> > : : basicity
> > : :
> > : : For Brønsted bases it means the tendency of a compound to act as
> hydron
> > : : (proton) acceptor. The basicity of a chemical species is normally
> expressed
> > : : by the acidity of the conjugate acid (see conjugate acid-base pair).
> For
> > : : Lewis bases it relates to the association constants of Lewis adducts
> > : : and -adducts
> > : :
> > : :
> > : :
> > : : Another definition from the same web page YOU cited: (this is the
> same web
> > : : page you cited above)
> > : :
> > : : Alkalinity:
> > : : Acid neutralizing or buffering capacity of water; a measure of the
> ability
> > : : of water to resist changes in pH caused by the addition of acids or
> bases
> > : : and therefore, the main indicator of susceptibility to acid rain; in
> natural
> > : : waters it is due primarily to the presence of bicarbonates,
carbonates
> and
> > : : to a much lesser extent occasionally borates, silicates and
> phosphates. It
> > : : is expressed in units of milligrams per liter (mg/l) of CaCO3
(calcium
> > : : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l =
1
> mg/l
> > : : of CaCO3. A solution having a pH below about 5 contains no
alkalinity.
> > : :
> > : : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and
> says
> > : : that alkalinity is the measure of ...(description of a buffer)
> > : :
> > : : A BUFFER IS : a measure of the ability of water to resist changes in
> pH
> > : : caused by the addition of acids or bases (from definition below)
> > : :
> > : :
> > : : I said:
> > : : ***alkalinity is a measurement of 'buffering capacity'***
> > : :
> > : : You said:
> > : : ***Alkalinity is not a measurement of BC
> > : :
> > : : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is
> not
> > : : logical.
> > : :
> > : : (THIS FROM THE SAME WEB PAGE YOU CITED):
> > : :
> > : : Buffer:
> > : : A substance which tends to keep pH levels fairly constant when acids
> or
> > : : bases are added.
> > : :
> > : : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
> > : :
> > : : a measure of the ability of water to resist changes in pH caused by
> the
> > : : addition of acids or bases
> > : :
> > : : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A
> BUFFER.
> > : :
> > : :
> > : : I went to all four links. None contradict what I have said. But
the
> first
> > : : one you cited contradicts YOU!
> > : :
> > : : I know what a buffer is. I know what acidity means. I know what
> alkalinity
> > : : means. No need to cite web pages that describe what I know and what
I
> wrote
> > : : in this discussion. Show me one that says alkalinity is not a
measure
> of
> > : : buffering capacity from a credible source.
> > : :
> > : :
> > : :
> > : :
> > : :
> > : :
> > : : "Boomer" > wrote in message
> > : : ...
> > : : > Alkalinity a measure of the amount of anions of weak acid in water
> and of
> > : : the cations
> > : : > balanced against them
> > : : > Take note it says ***acid***
> > : : >
> > : : > Buffering capacity the ability of a solution to resist or dampen
> changes
> > : : in pH upon the
> > : : > addition of acids or bases.
> > : : > Take note its says ***the addition of acids or bases***
> > : : >
> > : : > One more
> > : : >
> > : : > http://www.waterontheweb.org/resources/glossary.html
> > : : >
> > : : > We could go on like this all day, so what is the point ?
> > : : >
> > : : > You will LOVE this one
> > : : > http://www.kyantec.com/Tips/phbuffering.htm
> > : : >
> > : : > Don't you just lovbe PDF's
> > : : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
> > : : >
> > : : > Don't fall out of your chair
> > : : >
> http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
> > : : >
> > : : >
> > : : >
> > : : >
> > : : > --
> > : : > Boomer
> > : : >
> > : : > Want to talk chemistry ? The Reef Chemistry Forum
> > : : > http://www.reefcentral.com/vbulletin/index.php
> > : : >
> > : : > Want to See More ?
> > : : > Please Join Our Growing Membership
> > : : > www.coralrealm.com
> > : : >
> > : : > If You See Me Running You Better Catch-Up
> > : : > "stoutman" <.@.> wrote in message
> news:XB7Wb.19339$QA2.62332@attbi_s52...
> > : : > : Man here is another, google is a wonderful thing. I'm not
> filtering any
> > : : > : out, just posting what I find by GOOGLING for you.
> > : : > :
> > : : > :
> http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> > : : > :
> > : : > :
> > : : > : Wow, a gov link. Even the government is wrong, this must be a
> > : : conspiracy
> > : : > : against Boomer.
> > : : > :
> > : : > :
> > : : > :
> > : : > :
> > : : > : "Boomer" > wrote in message
> > : : > : ...
> > : : > : > Now I am getting bored
> > : : > : >
> > : : > : > "Don't the components of a buffer account for the buffering
> capacity?
> > : : > : Yes."
> > : : > : >
> > : : > : > Yes, agreed but you seem to fail what I'm saying. Buffering
> Capacity
> > : : and
> > : : > : Alkalinity are
> > : : > : > not the same, that has always been the issue. I gave the
> equation does
> > : : > : that look like an
> > : : > : > Alkalinity equation or how Alk is determined. I see you had
now
> > : : comments
> > : : > : on it what's
> > : : > : > wrong, why no comments on the equations I gave. Don't
understand
> them
> > : : or
> > : : > : what ? Again this
> > : : > : > is the equation for Buffering Capacity, also called Buffer
Index
> or
> > : : Buffer
> > : : > : Intensity. It
> > : : > : > is defined in most water chemistry and chemical oceanography
> text
> > : : books.
> > : : > : >
> > : : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] +
[H30+]
> +
> > : : CKa
> > : : > : [H3O+] / (Ka =
> > : : > : > H3O+])² )
> > : : > : >
> > : : > : > This is not Alkalinity now is it ?
> > : : > : >
> > : : > : > "I know how to do a titration, In fact I have done several.
How
> many
> > : : have
> > : : > : > you actually done? I don't mean by counting drops, I mean
with
> a
> > : : buret?"
> > : : > : >
> > : : > : > Well good for you, I use a Digital Titrator
> > : : > : >
> > : : > : > "Oh, I see,
> > : : > : > you think acidity is the opposite of alkalinity. In the world
> of
> > : : > : CHEMISTRY
> > : : > : > it's not. Maybe in aquarium newsgroups it is.
> > : : > : >
> > : : > : > Hum no, maybe you should go for a look at HACH's or LaMotte
> website or
> > : : the
> > : : > : book I
> > : : > : > suggested earlier. Please view a copy.
> > : : > : >
> > : : > : > Standard Methods for the Examination of Water and Wastewater
> > : : > : >
> > : : > : > This book, over 2000 pages, is the guide for water testing. If
> you are
> > : : > : reporting water
> > : : > : > test to the EPA you must use approved std from this text.I t
is
> > : : prepared
> > : : > : and published by
> > : : > : > the EPA, American Water Works Association and American Public
> Health
> > : : > : Association. You
> > : : > : > mean you don't have one and the issue is water chemistry
> > : : > : >
> > : : > : > You are confusing Acidity and Acidity as you know little about
> water
> > : : > : chemistry and
> > : : > : > procedures and test methods
> > : : > : >
> > : : > : > From SMEWW, section 2-30, 2310 ACIDITY
> > : : > : >
> > : : > : > "Acidity of water is its quantative capacity to react with a
> strong
> > : : base
> > : : > : to a designated
> > : : > : > pH"
> > : : > : >
> > : : > : > This is how you test for it
> > : : > : >
> > : : > : > A std alkali titration to methyl orange or phenolphthalein
> > : : > : > endpoint.
> > : : > : >
> > : : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that
> write
> > : : this
> > : : > : book, there are
> > : : > : > over 100 of them, they are wrong.
> > : : > : >
> > : : > : > Like Buffering Capacity you have your Acidity's mixed up
> > : : > : > In water measurement if you have a high Alk you also usually
> have a
> > : : high
> > : : > : Acidity.
> > : : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
> > : : CHEMISTRY
> > : : > : BOOK there pal.
> > : : > : >
> > : : > : >
> > : : > : > "These are all in equilibrium with each other. An initial
high
> pH
> > : : (above
> > : : > : > 6.4) will shift the equilibrium to the right to form HCO3-1.
If
> the
> > : : pH of
> > : : > : > the solution is above 10.3 (pKa2) the .........."
> > : : > : >
> > : : > : >
> > : : > : > Christ, there you go again with the FW ****. All your numbers
> are
> > : : wrong we
> > : : > : are dealing
> > : : > : > with SEAWATER
> > : : > : >
> > : : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is
> in the
> > : : form
> > : : > : > of HCO3-1 .
> > : : > : >
> > : : > : > I have already pointed that out and gave actual values at know
> > : : seawater
> > : : > : levels, go back
> > : : > : > and re-read it you aren't telling me anything here.Of course
> most is
> > : : HCO3
> > : : > : see...
> > : : > : >
> > : : > : >
> > : : > : > @ 20C and 34.3 ppt salinity
> > : : > : >
> > : : > : > CO2 = 0.52 %
> > : : > : >
> > : : > : > HCO3 = 86.4 %
> > : : > : >
> > : : > : > CO3 = 13.09 %
> > : : > : >
> > : : > : >
> > : : > : > "In your glass experiment you managed to lower the pH enough
to
> purge
> > : : out
> > : : > : CO2
> > : : > : > by boiling"
> > : : > : >
> > : : > : > The purpose behind the glass is to show that alk is not affect
> by CO2
> > : : and
> > : : > : vise-versa and
> > : : > : > how Co2 affects pH.
> > : : > : >
> > : : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and
that
> pH
> > : : drops
> > : : > : to say 8.1 it is
> > : : > : > usually due to excess CO2. If you took a glass of that water
and
> > : : aerated
> > : : > : it you WILL drive
> > : : > : > off the CO2 and raise the pH. It has been done a proven a
> million
> > : : times.
> > : : > : >
> > : : > : > "In order to 'purge' CO2 you would need to lower the
> > : : > : > pH to shift the equilibrium to below 6.4"
> > : : > : >
> > : : > : > The hell you do !!!.Do you know who many times people on this
NG
> to
> > : : > : include Dr. Craig
> > : : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned
to
> take a
> > : : > : sample of aquarium
> > : : > : > water and aerate it to see if the pH GOES UP AND when they
come
> back
> > : : with
> > : : > : the test it is
> > : : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D
CHEMIST
> > : : excess
> > : : > : CO2 in the tank
> > : : > : > water, increase the circulation for better gas exchange at the
> > : : surface,
> > : : > : reduce feeding,
> > : : > : > and try to improve on better skimming, thus reducing the
> bio-load and
> > : : pH
> > : : > : decline due to
> > : : > : > CO2.
> > : : > : >
> > : : > : >
> > : : > : > "I hope this helps. "
> > : : > : >
> > : : > : > Help, how can you when you miss everything. I should be
charging
> you
> > : : > : >
> > : : > : > Oh, by the way. Your websites, I have about 50 on these
issues,
> I
> > : : could
> > : : > : post them, not to
> > : : > : > mention I have all those water chemistry books, so there is no
> need to
> > : : > : view your sites.
> > : : > : >
> > : : > : > Finally are you afraid to come to our Chemistry Forum, afraid
to
> get
> > : : > : slapped by REAL
> > : : > : > chemists. I get a charge out of you can't post your ref .I
have
> posted
> > : : the
> > : : > : same or similar
> > : : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have
> 1500
> > : : posts
> > : : > : there and am the
> > : : > : > biggest contributor to his forum other than himself or maybe
> Habib
> > : : Sheka
> > : : > : >
> > : : > : > Hum, here are Randy's ref that he posted. He hosts the website
> > : : > : >
> > : : > : > S. RANDY HOLMES-FARLEY
> > : : > : > Arlington, Massachusetts
> > : : > : >
> > : : > : > EDUCATION
> > : : > : >
> > : : > : > 1982-1986 Harvard University Cambridge, MA
> > : : > : > PhD in Chemistry
> > : : > : > Research Advisor: George Whitesides
> > : : > : >
> > : : > : > Investigated the relationship between polymer surface
chemistry
> and
> > : : > : physical properties
> > : : > : > through controlled surface modification and testing.
> > : : > : >
> > : : > : > 1980-1982 Cornell University Ithaca, NY
> > : : > : > BA in Chemistry and Biology
> > : : > : > Graduated Summa Cum Laude
> > : : > : > Distinction in All Subjects
> > : : > : > Grade Point: 3.94/4.0
> > : : > : > Honors research: isolation and characterization of the subunit
> of CF1
> > : : > : enzyme
> > : : > : >
> > : : > : >
> > : : > : > 1978-1979 Stanford University Palo Alto, CA
> > : : > : > Grade Point: 3.55/4.0
> > : : > : >
> > : : > : >
> > : : > : > EXPERIENCE
> > : : > : >
> > : : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham,
> MA
> > : : > : > (bought out GelTex Pharmaceuticals in 2001)
> > : : > : > Vice President, Chemical Research 2001-present
> > : : > : > Senior Director, Chemical Research 1999-2001
> > : : > : > Director of Chemical Research 1997-1999
> > : : > : > Manager of Chemical Research 1995-1997
> > : : > : > Group Leader 1994-1995
> > : : > : > Senior Research Scientist 1992-1994
> > : : > : >
> > : : > : > Helped start GelTex as second employee
> > : : > : >
> > : : > : > Managed various research programs with multi-million dollar
> budgets
> > : : > : >
> > : : > : > Supervised research chemists (17+)
> > : : > : >
> > : : > : > Co-inventor of several polymeric pharmaceuticals and
> pharmaceutical
> > : : > : candidates including
> > : : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam
> Hydrochloride
> > : : (FDA
> > : : > : approved)
> > : : > : >
> > : : > : > Company Safety Officer for 3 years
> > : : > : >
> > : : > : > Chemical Hygiene Officer 2000-present
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > 1990-1992 GTE Corporation Waltham, MA
> > : : > : > Senior Member of Technical Staff
> > : : > : > Applied research involving polymer interfaces
> > : : > : > Metallization of plastics
> > : : > : > Polymer/polymer adhesion
> > : : > : > Optical coatings
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > 1986-1990 Lord Corporation Cary, NC
> > : : > : > Senior Research Scientist 1988-1990
> > : : > : > Research Scientist 1986-1988
> > : : > : > Basic and applied research on surface chemical bonding
> > : : > : > Developed new adhesive compositions
> > : : > : > Developed new sol-gel coatings for corrosion resistance
> > : : > : >
> > : : > : >
> > : : > : > HONORS AND AWARDS
> > : : > : >
> > : : > : > Industrial Innovations Award by Northeast Region of American
> Chemical
> > : : > : Society (6/2001)
> > : : > : >
> > : : > : > National Kidney Foundation of Northern California Honoree
> (5/2001)
> > : : > : >
> > : : > : > American Chemical Society/Polymer Chemistry Division
Industrial
> > : : Sponsors
> > : : > : > Award (8/2000)
> > : : > : >
> > : : > : > R&D 100 Award from R&D magazine (1999)
> > : : > : >
> > : : > : > Sherwin Williams Award in applied polymer science (9/85)
> > : : > : >
> > : : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985;
> 1985-1986)
> > : : > : >
> > : : > : > Award for highest GPA in Chemistry Department (6/82)
> > : : > : >
> > : : > : > Summa Cum Laude Honors in Chemistry (6/82)
> > : : > : >
> > : : > : > Phi Lamda Epsilon (6/82)
> > : : > : >
> > : : > : > Phi Beta Kappa (2/82)
> > : : > : >
> > : : > : > Cornell University Dean's List (1981, 1982)
> > : : > : >
> > : : > : > Harvard Book Club Award for highest GPA senior year (1978)
> > : : > : >
> > : : > : > First Place in western NY ACS high school chemistry exam
(1977)
> > : : > : >
> > : : > : > 1978-1979
> > : : > : >
> > : : > : >
> > : : > : > __________________
> > : : > : > Randy Holmes-Farley
> > : : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef
> Central
> > : : > : >
> > : : > : > Hobby Experience: 8 years with reefs
> > : : > : > Current Tanks: 90 gal mixed reef
> > : : > : > Interests: Reefkeeping, science, photography
> > : : > : >
> > : : > : >
> > : : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> > : : > : >
> > : : > : > Open this post in a new window | Report this post to a
moderator
> | IP:
> > : : > : Logged
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > 06/27/2003 02:44 PM
> > : : > : >
> > : : > : > Randy Holmes-Farley
> > : : > : > Chemistry Moderator
> > : : > : >
> > : : > : > Registered: Apr 2001
> > : : > : > Location: Arlington, Massachusetts
> > : : > : > Occupation: Chemist (Drug Discovery at Genzyme)
> > : : > : > Posts: 15282
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > Publications
> > : : > : >
> > : : > : >
> > : : > : > ISSUED UNITED STATES PATENTS
> > : : > : >
> > : : > : >
> > : : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen
Randall;
> > : : > : Mandeville, III; W. Harry.
> > : : > : > US 6,566,407; 5/20/2003
> > : : > : >
> > : : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley,
> Stephen
> > : : Randall;
> > : : > : Huval, Chad
> > : : > : > Cori.
> > : : > : > U.S. 6,517,825; 2/11/2003.
> > : : > : >
> > : : > : > 3. Method of making phosphate-binding polymers for oral
> > : : administration.
> > : : > : Holmes-Farley,
> > : : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M.
> U.S.
> > : : > : 6,509,013; 1/21/2003.
> > : : > : >
> > : : > : > 4. Combination therapy for treating hypercholesterolemia using
a
> bile
> > : : acid
> > : : > : sequestrant
> > : : > : > polymer
> > : : > : > and a cholesterol-lowering agent. Huval, Chad Cori;
> Holmes-Farley,
> > : : Stephen
> > : : > : Randall;
> > : : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> > : : > : >
> > : : > : > 5. Method for treating hypercholesterolemia with
polyallylamine
> > : : polymers.
> > : : > : Holmes-Farley,
> > : : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
> > : : Goldberg,
> > : : > : Dennis I. , US
> > : : > : > 6,423,754; 7/23/2002.
> > : : > : >
> > : : > : > 6. Ionic polymers as anti-infective agents Mandeville, W.
Harry,
> III;
> > : : > : Neenan, Thomas X..;
> > : : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> > : : > : >
> > : : > : > 7. Combination therapy for treating hypercholesterolemia and
> > : : > : atherosclerosis. Huval, Chad
> > : : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal,
> Pradeep
> > : : K.
> > : : > : U.S. 6,365,186;
> > : : > : > 4/2/2002.
> > : : > : >
> > : : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
> > : : Mandeville,
> > : : > : W. H., III;
> > : : > : > Huval; C.
> > : : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US
> 6,299,868;
> > : : > : 10/9/2001.
> > : : > : >
> > : : > : > 9. Polymers containing guanidinium groups as bile acid
> sequestrants.
> > : : Dhal;
> > : : > : P. K.; Holmes-
> > : : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> > : : > : >
> > : : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.;
> Mandeville, W.
> > : : H.,
> > : : > : III.; US
> > : : > : > 6,281,252;
> > : : > : > 8/28/2001.
> > : : > : >
> > : : > : > 11. Combination therapy for treating hypercholestrolemia.
Huval;
> C.
> > : : C.;
> > : : > : Holmes-Farley; S.
> > : : > : > R. ;
> > : : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> > : : > : >
> > : : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides,
> G. M.;
> > : : > : Holmes-Farley, S.
> > : : > : > R.; US
> > : : > : > 6,264,937; 7/24/2001.
> > : : > : >
> > : : > : > 13. Method for treating hypercholesterolemia with
unsubstituted
> > : : > : polydiallylamine polymers.
> > : : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
> K. ; US
> > : : > : 6,248,318;
> > : : > : > 6/19/2001.
> > : : > : >
> > : : > : > 14. Process for removing bile salts from a patient and
alkylated
> > : : > : compositions therefore.
> > : : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355;
> 5/1/2001.
> > : : > : >
> > : : > : > 15. Poly(diallylamine)-based bile acid sequestrants.
> Holmes-Farley, S.
> > : : R.;
> > : : > : Dhal, P. K.;
> > : : > : > Petersen,
> > : : > : > J. S.; US 6,203,785; 3/20/2001.
> > : : > : >
> > : : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S.
> R.;
> > : : Huval,
> > : : > : C. C.; US
> > : : > : > 6,190,649;
> > : : > : > 2/20/2001.
> > : : > : >
> > : : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.;
> Mandeville, W.
> > : : H.,
> > : : > : III.; US
> > : : > : > 6,177,478;
> > : : > : > 1/23/2001.
> > : : > : >
> > : : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
> > : : Holmes-Farley,
> > : : > : S. R.;
> > : : > : > Mandeville, W.
> > : : > : > H., III.; US 6,129,910; 10/10/2000.
> > : : > : >
> > : : > : > 19. Method for treating hypercholesterolemia with
unsubstituted
> > : : > : polydiallylamine polymers.
> > : : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
> K. ; US
> > : : > : 6,083,497;
> > : : > : > 7/4/2000.
> > : : > : >
> > : : > : > 20. Method of making phosphate-binding polymers for oral
> > : : administration.
> > : : > : Holmes-Farley, S.
> > : : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US
6,083,495;
> > : : 7/4/2000.
> > : : > : >
> > : : > : > 21. Process for removing bile salts from a patient and
alkylated
> > : : > : compositions therefore.
> > : : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
> > : : 5/23/2000.
> > : : > : >
> > : : > : > 22. Process for removing bile salts from a patient and
> compositions
> > : : > : therefor. Mandeville,
> > : : > : > W. H.,
> > : : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> > : : > : >
> > : : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III;
W.
> H;
> > : : > : Neenan; T. X.; Holmes-
> > : : > : > Farley; S. R. US 6,034,129; 3/7/2000.
> > : : > : >
> > : : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.;
> Mandeville, W.
> > : : H.,
> > : : > : III.; US
> > : : > : > 5,985,938;
> > : : > : > 11/16/99.
> > : : > : >
> > : : > : > 25. Process for removing bile salts from a patient and
> compositions
> > : : > : therefor. Mandeville,
> > : : > : > W. H.,
> > : : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> > : : > : >
> > : : > : > 26. Hydrophobic sequestrant for cholesterol depletion.
> Mandeville, W.
> > : : H.,
> > : : > : III.;
> > : : > : > Holmes-Farley;
> > : : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> > : : > : >
> > : : > : > 27. Hydrophilic nonamine-containing and amine-containing
> copolymers
> > : : and
> > : : > : their use as bile
> > : : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
> > : : 5,929,184;
> > : : > : 7/27/99.
> > : : > : >
> > : : > : > 28. Interpenetrating polymer networks for sequestration of
bile
> acids.
> > : : > : Mandeville, W. H.,
> > : : > : > III.;
> > : : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US
> 5,925,379;
> > : : > : 7/20/99.
> > : : > : >
> > : : > : > 29. Amine polymer sequestrant and method of cholesterol
> depletion.
> > : : > : Mandeville, W. H.,
> > : : > : > III.;
> > : : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> > : : > : >
> > : : > : > 30. Process for removing bile salts from a patient and
> compositions
> > : : > : therefor. Mandeville,
> > : : > : > W. H.,
> > : : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> > : : > : >
> > : : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
> depletion.
> > : : > : Mandeville, W. H.,
> > : : > : > III.;
> > : : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> > : : > : >
> > : : > : > 32. Process for removing bile salts from a patient and
> compositions
> > : : > : therefor. Mandeville,
> > : : > : > W. H.,
> > : : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> > : : > : >
> > : : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
> > : : Mandeville,
> > : : > : W. H., III.;
> > : : > : > Holmes-
> > : : > : > Farley, S. R.; US 5,703,188; 12/30/97.
> > : : > : >
> > : : > : > 34. Oral administration of iron-binding crosslinked amine
> polymers.
> > : : > : Mandeville, W. H.,
> > : : > : > III.;
> > : : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> > : : > : >
> > : : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
> Holmes-Farley,
> > : : S.
> > : : > : R.; US 5,693,675;
> > : : > : > 12/2/97.
> > : : > : >
> > : : > : > 36. Method for removing bile salts from a patient with
alkylated
> > : : > : crosslinked amine
> > : : > : > polymers,
> > : : > : > and preparation of the polymers. Mandeville, W. H., III.;
> > : : Holmes-Farley,
> > : : > : S. R.; US
> > : : > : > 5,679,717; 10/21/97.
> > : : > : >
> > : : > : > 37. Phosphate-binding polymers for oral administration.
> Holmes-Farley,
> > : : S.
> > : : > : R.; Mandeville,
> > : : > : > W.
> > : : > : > H., III.; US 5,667,775; 9/16/97.
> > : : > : >
> > : : > : > 38. Ion-exchange process using highly crosslinked polymers for
> > : : removing
> > : : > : bile salts from a
> > : : > : > patient, preparation of the polymers, and compositions
> containing
> > : : them.
> > : : > : Mandeville, W. H.,
> > : : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> > : : > : >
> > : : > : > 39. Hydrophobic amine polymer sequestrant and method of
> cholesterol
> > : : > : depletion. Mandeville,
> > : : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US
> 5,618,530;
> > : : 4/8/97.
> > : : > : >
> > : : > : > 40. Amine polymer sequestrant and method of cholesterol
> depletion.
> > : : > : Mandeville, W. H.,
> > : : > : > III.;
> > : : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> > : : > : >
> > : : > : > 41. Phosphate-binding polymers for oral administration.
> Holmes-Farley,
> > : : S.
> > : : > : R.; Mandeville,
> > : : > : > W.
> > : : > : > H., III.; US 5,496,545; 3/5/96.
> > : : > : >
> > : : > : > 42. Iron-binding polymers for oral administration. Mandeville,
> W. H.,
> > : : > : III.; Holmes-Farley,
> > : : > : > S. R.;
> > : : > : > US 5,487,888; 1/30/96.
> > : : > : >
> > : : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having
> active
> > : : > : hydrogens on the
> > : : > : > surface.
> > : : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> > : : > : >
> > : : > : > 44. Layered sol-gel coatings from organisilicon compounds.
> > : : Holmes-Farley,
> > : : > : S. R.; Yanyo, L.
> > : : > : > C.;
> > : : > : > US 5,182,143; 1/26/93.
> > : : > : >
> > : : > : > 45. Method for metal bonding using ultrathin primer coating.
> > : : > : Holmes-Farley, S. R.; Yanyo,
> > : : > : > L.
> > : : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> > : : > : >
> > : : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.;
Abbey,
> K. J.;
> > : : US
> > : : > : 5,096,962;
> > : : > : > 3/17/92.
> > : : > : >
> > : : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> > : : > : elastomer-metal bonding.
> > : : > : > Holmes-
> > : : > : > Farley, S. R.; US 5,102,956; 4/7/92.
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT
> ISSUED)
> > : : > : >
> > : : > : >
> > : : > : > 1. Aryl boronate functionalized polymers for treating obesity
> and
> > : : > : inhibiting fat uptake.
> > : : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III;
Dhal,
> > : : Pradeep
> > : : > : K.; Huval, Chad
> > : : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl.
(2003),
> 92
> > : : pp. WO
> > : : > : 0302571.
> > : : > : >
> > : : > : > 2. Preparation of aryl boronic acids for treating obesity.
> > : : Holmes-Farley,
> > : : > : Stephen Randall;
> > : : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal,
> Pradeep
> > : : K.
> > : : > : (Geltex
> > : : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO
> 0302570.
> > : : > : >
> > : : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide.
> Holmes-Farley,
> > : : > : Stephen Randall.
> > : : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32
> pp. WO
> > : : > : 0302130.
> > : : > : >
> > : : > : > 4. Method for reducing copper levels and treating copper
> toxicosis.
> > : : > : Holmes-Farley, Stephen
> > : : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl.
> (2002),
> > : : 45
> > : : > : pp. WO
> > : : > : > 0285383.
> > : : > : >
> > : : > : > 5. Method for treating gout and binding uric acid.
> Holmes-Farley,
> > : : Stephen
> > : : > : Randall; Burke,
> > : : > : > Steven K. WO 0285381 10/31/2002.
> > : : > : >
> > : : > : > 6. Method for treating gout and reducing serum uric acid.
> > : : Holmes-Farley,
> > : : > : Stephen Randall;
> > : : > : > Burke, Steven K WO 0285380 10/31/2002.
> > : : > : >
> > : : > : > 7. Amine condensation polymer bile acid sequestrants. Huval,
C.
> C.;
> > : : > : Holmes-Farley, S. R.;
> > : : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> > : : > : >
> > : : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H.,
> III and
> > : : > : Holmes-Farley, S.
> > : : > : > R.;
> > : : > : > WO 1999-US5662; 9/23/1999.
> > : : > : >
> > : : > : > 9. Amine-containing copolymers as bile acid sequestrants.
> > : : Holmes-Farley,
> > : : > : S. R.; Petersen,
> > : : > : > J. S.;
> > : : > : > WO 9933452; 7/8/1999.
> > : : > : >
> > : : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W.
H.,
> III
> > : : and
> > : : > : Holmes-Farley, S.
> > : : > : > R.;
> > : : > : > WO 9922743; 5/14/1999.
> > : : > : >
> > : : > : > 11. Polyallylamine polymers for removing bile salts and
treating
> > : : > : hypercholesterolemia, and
> > : : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H.,
> III;
> > : : Burke,
> > : : > : S. K.; Goldberg,
> > : : > : > D. I.; WO 9857652; 12/23/98.
> > : : > : >
> > : : > : > 12. Phosphate-bidning polymers combined with a calcium
> supplement for
> > : : oral
> > : : > : administration.
> > : : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
> Holmes-Farley,
> > : : S.
> > : : > : R.; WO 9842355;
> > : : > : > 10/1/98.
> > : : > : >
> > : : > : > 13. Hydrophobic heteroatom-containing sequestrant for
> cholesterol
> > : : > : depletion. Mandeville,
> > : : > : > W.
> > : : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449;
> 12/12/96.
> > : : > : >
> > : : > : > 14. Process for adjusting ion concentration in a patient and
> > : : compositions
> > : : > : therefor.
> > : : > : > Mandeville,
> > : : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> > : : > : >
> > : : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
> > : : interlayer
> > : : > : for improved
> > : : > : > metal-
> > : : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
> > : : 1/20/94.
> > : : > : >
> > : : > : > 16. Process for increased metal-substrate bond strength in
> metalized
> > : : > : plastics.
> > : : > : > Holmes-Farley, S.
> > : : > : > R.; Ger. Offen. 4322516; 7/6/93.
> > : : > : >
> > : : > : > 17. Electrorheological fluids and preparation of particles
> useful in
> > : : the
> > : : > : fluids.
> > : : > : > Troughton,
> > : : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie;
> Carlson, J.
> > : : > : David; Bares, Joseph
> > : : > : > E.;
> > : : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra
> Nell. EP
> > : : > : 394049;
> > : : > : > 10/24/1990.
> > : : > : >
> > : : > : > JOURNAL PUBLICATIONS
> > : : > : >
> > : : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William;
> Zhorov,
> > : : Eugene;
> > : : > : Guo, Amy;
> > : : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David
L.;
> > : : > : Mandeville, W. Harry;
> > : : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
> > : : 611-619.
> > : : > : >
> > : : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
> > : : synthesis
> > : : > : and biological
> > : : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley,
> S.
> > : : Randall;
> > : : > : Mandeville, W.
> > : : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal,
> Pradeep K.
> > : : > : Journal of
> > : : > : > Macromolecular Science, Pure and Applied Chemistry (2001),
> A38(12),
> > : : > : 1559-1574.
> > : : > : >
> > : : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by
> Molecular
> > : : > : Imprinting. Huval,
> > : : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.;
Holmes-Farley,
> S.
> > : : > : Randall; Mandeville,
> > : : > : > W.
> > : : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro,
> Robert
> > : : J.;
> > : : > : Chen, Xi; Dhal,
> > : : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> > : : > : >
> > : : > : > 4. Synthetic polymers for the binding of fat in the intestinal
> tract.
> > : : > : Jozefiak, Thomas H.;
> > : : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny,
Cynthia;
> > : : Huval,
> > : : > : Chad C.;
> > : : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney,
> Cynthia.
> > : : > : Abstracts of
> > : : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United
States,
> August
> > : : > : 26-30, 2001
> > : : > : > (2001), POLY-047 and Polymer Preprints (American Chemical
> Society,
> > : : > : Division of
> > : : > : > Polymer Chemistry) (2001), 42(2), 98.
> > : : > : >
> > : : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel
> polymer
> > : : gel
> > : : > : pharmaceutical.
> > : : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.;
Petersen,
> J.;
> > : : Ward,
> > : : > : J.; Sacchiero,
> > : : > : > B.;
> > : : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton,
K.
> A.;
> > : : Chen,
> > : : > : X.; Mazzeo, J.
> > : : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
> > : : > : >
> > : : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl
> and
> > : : other
> > : : > : bile acid
> > : : > : > sequestrants.
> > : : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.;
> Xu, Q.;
> > : : > : Hook, P.; Holmes-
> > : : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1),
> 708-709.
> > : : > : >
> > : : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
> > : : Holmes-Farley,
> > : : > : S. R; Polym.
> > : : > : > Mater. Sci. Eng (1999), 80, 246-247.
> > : : > : >
> > : : > : > 8. Design and characterization of of Sevelamer Hydrochloride:
a
> novel
> > : : > : phosphate-binding
> > : : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III;
> Ward,
> > : : J.;
> > : : > : Miller, K. L.;
> > : : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M.
S.-
> Pure
> > : : and
> > : : > : Appl. Chem.,
> > : : > : > A36(7&8), p. 1085 (1999).
> > : : > : >
> > : : > : > 9. Three generations of bile acid sequestrants. Mandeville, W.
> H.,
> > : : III;
> > : : > : Braunlin, W.;
> > : : > : > Dhal, P.;
> > : : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik,
> S.;
> > : : > : Rosenbaum, D.;
> > : : > : > Sacchiero,
> > : : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc.
> (1999),
> > : : > : 550, 3-15.
> > : : > : >
> > : : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked,
polymeric
> > : : phosphate
> > : : > : binder, on
> > : : > : > urinary
> > : : > : > phosphorous excretion in rats. Rosenbaum, D. P.;
Holmes-Farley,
> S. R.;
> > : : > : Mandeville, W. H.,
> > : : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
> Transplant.
> > : : > : (1997), 12(5)
> > : : > : > 961-964.
> > : : > : >
> > : : > : > 11. Thin anisotropic coatings based on sol-gel technology.
> > : : Holmes-Farley,
> > : : > : S. R.; Yanyo, L.
> > : : > : > C;
> > : : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem.
> 4),
> > : : 439-444.
> > : : > : >
> > : : > : > 12. The mechanism of cure initiation of a surface activated
> adhesive.
> > : : > : Holmes-Farley, S.
> > : : > : > R.;
> > : : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5),
> 409-420.
> > : : > : >
> > : : > : > 13. Adhesion promotion and corrosion prevention using thin
> anisotropic
> > : : > : coatings. Holmes-
> > : : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991),
> 5(2),
> > : : > : 131-151.
> > : : > : >
> > : : > : > 14. Wetting of functionalized polyethylene having ionizable
> organic
> > : : acids
> > : : > : and bases at the
> > : : > : > polymer-water interface: relations between functional group
> polarity,
> > : : > : extent of
> > : : > : > ionization,
> > : : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C.
D.;
> > : : > : Whitesides, G. M.;
> > : : > : > Langmuir
> > : : > : > (1988), 4(4), 921-937.
> > : : > : >
> > : : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols
> with a
> > : : > : single hydroxy group.
> > : : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> > : : > : >
> > : : > : > 16. Reconstruction of the interface of oxidatively
> functionalized
> > : : > : polyethylene (PE-CO2H)
> > : : > : > and
> > : : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.;
> Nuzzo,
> > : : R.;
> > : : > : McCarthy, T. J.;
> > : : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also
> Report
> > : : (1987),
> > : : > : AD-
> > : : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> > : : > : >
> > : : > : > 17. Surface-modified polyethylene film: the relationship
between
> > : : surface
> > : : > : chemistry and
> > : : > : > physical
> > : : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987,
> 47(11),
> > : : 4537.
> > : : > : >
> > : : > : > 18. Reactivity of carboxylic acid and ester groups in the
> > : : functionalized
> > : : > : interfacial
> > : : > : > region of
> > : : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> > : : > : differentiation of the
> > : : > : > functional groups into shallow and deep subsets based on a
> comparison
> > : : of
> > : : > : contact angle and
> > : : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.;
> Langmuir
> > : : > : (1987), 3(1), 62-
> > : : > : > 76.
> > : : > : >
> > : : > : > 19. Fluorescence properties of dansyl groups covalently bonded
> tot he
> > : : > : surface of
> > : : > : > oxidatively
> > : : > : > functionalized low-density polyethylene film. Holmes-Farley,
S.
> R.;
> > : : > : Whitesides, G. M.;
> > : : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985),
TR-85-2;
> > : : > : AD-A162435/2/GAR,
> > : : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> > : : > : >
> > : : > : > 20. Acid-base behavior of carboxylic acid groups covalently
> attached
> > : : at
> > : : > : the surface of
> > : : > : > polyethylene: The usefulness of contact angle in following the
> > : : ionization
> > : : > : of surface
> > : : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy,
T.
> J.;
> > : : > : Deutch, J.;
> > : : > : > Whitesides,
> > : : > : > G. M.; Langmuir (1985), 1(6), 725-740.
> > : : > : >
> > : : > : > 21. The thermal stability of a surface modified solid organic
> polymer.
> > : : > : Holmes-Farley, S.
> > : : > : > R.;
> > : : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53,
127-131.
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> > : : > : >
> > : : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R.
> Advanced
> > : : > : Aquarist. June 2003.
> > : : > : >
> > : : > : > 2. The Self Purification of Limewater (Kalkwasser).
> Holmes-Farley, R.
> > : : > : Advanced Aquarist.
> > : : > : > May
> > : : > : > 2003.
> > : : > : >
> > : : > : > 3. The Degradation of Limewater (Kalkwasser) in Air.
> Holmes-Farley, R.
> > : : > : Reefkeeping May
> > : : > : > 2003.
> > : : > : >
> > : : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
> Reefkeeping
> > : : > : April 2003.
> > : : > : >
> > : : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae
> Growth.
> > : : > : Holmes-Farley, R.
> > : : > : > Advanced Aquarist; April 2003.
> > : : > : >
> > : : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae
> Growth.
> > : : > : Holmes-Farley, R.
> > : : > : > Advanced Aquarist; April 2003.
> > : : > : >
> > : : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R.
Advanced
> > : : Aquarist;
> > : : > : March 2003.
> > : : > : >
> > : : > : > 8. How to Select a Calcium and Alkalinity Supplementation
> Scheme.
> > : : > : Holmes-Farley, R.
> > : : > : > Advanced Aquarist; February 2003.
> > : : > : >
> > : : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> January
> > : : > : 2003.
> > : : > : >
> > : : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> > : : December
> > : : > : 2002.
> > : : > : >
> > : : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
> > : : Advanced
> > : : > : Aquarist; November
> > : : > : > 2002.
> > : : > : >
> > : : > : > 12. Iron: A Look at Organisms Other than Macroalgae.
> Holmes-Farley, R.
> > : : > : Advanced Aquarist;
> > : : > : > November 2002.
> > : : > : >
> > : : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.;
Advanced
> > : : Aquarist,
> > : : > : September 2002.
> > : : > : >
> > : : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist,
> August
> > : : > : 2002.
> > : : > : >
> > : : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.;
Reefkeeping.com,
> April
> > : : > : 2002.
> > : : > : >
> > : : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R.
> Advanced
> > : : > : Aquarist; July 2002
> > : : > : >
> > : : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced
> Aquarist;
> > : : June
> > : : > : 2002.
> > : : > : >
> > : : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley,
> R.
> > : : Advanced
> > : : > : Aquarist, May
> > : : > : > 2002.
> > : : > : >
> > : : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in
> Corals.
> > : : > : Holmes-Farley, R.
> > : : > : > Advanced Aquarist, April 2002.
> > : : > : >
> > : : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> > : : > : >
> > : : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February
> 2002.
> > : : > : >
> > : : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist,
> January
> > : : 2002.
> > : : > : >
> > : : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium
> Frontiers
> > : : > : 2000.
> > : : > : >
> > : : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R.
> Aquarium
> > : : > : Frontiers 2000.
> > : : > : >
> > : : > : > 25. Phosphate..What is it and why should you care.
> Holmes-Farley, R.
> > : : > : Aquarium Frontiers
> > : : > : > 2000.
> > : : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
> > : : Frontiers
> > : : > : 2000.
> > : : > : >
> > : : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium
> Frontiers
> > : : 2000.
> > : : > : >
> > : : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium
Frontiers
> 1999.
> > : : > : >
> > : : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > Boomer
> > : : > : >
> > : : > : > Want to talk chemistry ? The Reef Chemistry Forum
> > : : > : > http://www.reefcentral.com/vbulletin/index.php
> > : : > : >
> > : : > : > Want to See More ?
> > : : > : > Please Join Our Growing Membership
> > : : > : > www.coralrealm.com
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > :
> > : : > :
> > : : >
> > : : >
> > : :
> > : :
> > : :
> > :
> > :
> >
> >
>
>

[stoutman]

You spelled CANTANKEROUS correctly and misspelled SNOT-NOSED. Too funny.
LOL. :)





"Benjamin" > wrote in message
...
> Boomer,
>
> Why are you still dwelling on all this? Can't we talk about what you
> really want the world to know about Reef Aquarium Chemistry now? Can you
do
> it in a language and manner that even a "snoot-noise kid" can grasp and
> appreciate? Could you set aside your apparently cantankerous nature long
> enough so many can learn something valuable from you without feeling... um
> never mind I can't find the word for it.
>
> --
> --
>
> My Web Site: http://showcase.netins.net/web/reefpage/
>
>
> "Boomer" > wrote in message
> ...
> > "As it is the ability to neutralizes an acid that is a buffer"
> >
> > sorry
> >
> > As it is the ability to neutralizes a base that is a buffer
> >
> > --
> > Boomer
> >
> > Want to talk chemistry ? The Reef Chemistry Forum
> > http://www.reefcentral.com/vbulletin/index.php
> >
> > Want to See More ?
> > Please Join Our Growing Membership
> > www.coralrealm.com
> >
> > If You See Me Running You Better Catch-Up
> > "Boomer" > wrote in message
> > ...
> > :
> > : "I am not sure if you are just messing with me "
> > :
> > : Yes, messing with you, it is called trolling a troll, to see where the
> hell you would go
> > : and what you would say in regards to last posts. It is called honesty,
> of which you have
> > : none off to say the least,that I can see.You always like to post what
> suits you and just
> > : avoid ref I give. So lets start where you are WRONG and have a great
> lack of
> > understanding
> > : of things, to include pointing out all your gross error which you
still
> FAIL to
> > : acknowledge and which can be prove in many water chem. ref. .I doubt
> like hell you are a
> > : chemist at all.You seem to want to con people into thinkin' you are.
But
> then again, I
> > : have seen chemists like you before, they are not familiar with the,
but
> they ASK to have
> > : it explained and ask for REF.YOU just shoot from the hip. WHAT GETS
YOU
> IN TROUBLE. You
> > : remind me of snoot-noise kid that come here and other NG's and
> forums...that think they
> > : know, buy hey, maybe I'm wrong :-)
> > :
> > :
> > :
> > : 1). Acidity
> > :
> > : "***Benjamin,Water Chemistry (2002, pages 262-263).***
> > :
> > : ***Acidity A concept that is exactly analogous to alkalinity but
> measures the base
> > : neutralizing
> > : capacity (BNC) of a solution is Acidity. The quantitative represents
the
> concentration
> > of
> > : OH- ions that must be added to titrate the solution to a pH near
10.5***
> > :
> > : So that means that not only in Benjamin wrong but, so are Stumm &
> Morgan, Millero,
> > Pilosn,
> > : Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I
> said, you have
> > your
> > : acidity and Acidy mixed up. Acidity as defined above is covered in
most
> water chemistry
> > : books, written by chemists, who's field of expertise is water
chemistry.
> You can even
> > buy
> > : Acidity test kits from, HACH, LaMotte, etc..
> > :
> > : You mean you didn't read this or are you just avoiding it .The same
> definition can be
> > : found in almost any std water chemistry book.
> > :
> > : I have run into few chemists, that are NOT familiar with the above.
Some
> water reports
> > : require the above Acidity measuring. The issue with you is you do not
> understand WATER
> > : CHEMISTRY. Everything you have posted can be found a general chemistry
> book
> > :
> > :
> > :
> > :
> > : 2) Alk and BC
> > :
> > : From the link
> > :
> > : Alkalinity
> > : ***Acid neutralizing or buffering capacity of water; a measure of the
> ability of water
> > to
> > : resist changes in pH caused by the addition of acids or bases ***
> > :
> > : This is a Buffering Capacity definition not Alk
> > :
> > : Humm, since when does Alk have anything to do in regards to the
addition
> of BASE. As I
> > : pointed out in the first post the term is often miss used. Even in
YOUR
> own posts you
> > say
> > : it is based on a acid addition, no mention of **base or acid**
addition
> by you. Are you
> > : getting confused or what. Or is more you are trying to confuse
everyone
> you are right.
> > The
> > : above is a definition for Buffer Capacity NOT Alk
> > :
> > : From Drew, Geochemistry of Natural Waters
> > :
> > : "alkalinity, which is formally defined as the equivalent sum of bases
> that are
> > titratable
> > : with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH
of
> the solution is
> > : progressively lowered by the addition of a strong acid (HCL), all the
> anions on the
> > right
> > : will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4,
> H2S,organic acids, H20)"
> > :
> > : This follows almost all description of Alk, that it is acid
neutralizing
> reaction and
> > has
> > : nothing to do with base neutralizing, which is Acidity (BNC) .I
defined
> these before you
> > : had no comment
> > :
> > :
> > : Even the links that give the Buffering Capacity definition is wrong,
as
> is the UIPAC on
> > : Alkalinity. Alkalinity has nothing to do with the addition of bases
only
> acids. When you
> > : use the words "base and acid" it becomes BC
> > :
> > : Even YOU MUST disagree with these definitions, from YOUR own post
> > :
> > : Think of alkalinity as 'buffering capacity'. Or the ability of a
> solution
> > : ***to resist a drop in pH due to the addition of acid***
> > :
> > : Where the flip is the base addition forget it ?
> > :
> > : From Butler; Carbon Dioxide Equilibrium and Their Applications
> (professor emeritus
> > : Harvard University) an expert on the subject.
> > :
> > : Buffering Index (Buffering Capacity, Buffer Intensity).
> > :
> > : ***This concept was first developed for mixtures of approximately
equal
> proportions of
> > : conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such
> buffer solutions
> > : strongly resist changes in pH when acids or bases are added and are
> useful as pH
> > : standards. The Buffer Index tells how great the resistance to pH
changes
> will be.**
> > :
> > : also from Butler
> > :
> > : Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
> > :
> > : Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
> > :
> > : Acidity is in fact just the negative of Alkalinity ***
> > :
> > : http://www.lagoonsonline.com/acid.htm
> > :
> > :
>
http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.h
tm?E+mystore
> > :
> > : It sure is funny how all of the chemist that write water chemistry
> textbooks never say
> > Alk
> > : is the Buffering Capacity of a solution. They are always treated and
> defined separately.
> > :
> > : If you or others choose to treat Alk and BC as the same, well, just
have
> at it. As I
> > said
> > : in first post I know what you mean.
> > :
> > : "No need to cite web pages that describe what I know and what I wrote
> > : in this discussion"
> > :
> > : No you don't know, who are you trying to convince any way, me, the
guys
> here and/or all
> > : the water chemists in this world. As I said before go get a dam WATER
> CHEMISTRY book or
> > : shut the hell up.You keep trying to define things from a general
> chemistry book WE ARE
> > IN
> > : THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
> > :
> > :
> > :
> > :
> > :
> > : 3). pKa's and what you don't know or seem to be confused on
> > :
> > : "Therefore, it has two pKa's
> > : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
> The
> > : pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated
is
> > : right in there. Is that magic? :)"
> > :
> > : Here it is agin that is twice at least
> > :
> > : "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this
> example)
> > : you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium
> will
> > : be shifted to HCO3-2 by a ratio of 1:100.
> > :
> > : Oh wait , there is a third time LOL
> > :
> > : "At the pH of seawater, the buffering capacity of carbonate is at it's
> > : weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
> > :
> > :
> > : Lets just dunk you on this one. I am taking note you refuse to reply
to
> YOUR errors
> > :
> > : So you calculated the pH of seawater with freshwater pKa's, now that
is
> a good trick.
> > From
> > : a number of seawater chemistry books the seawater pKa's are 6 & 9.1,
so
> according to
> > you,
> > : seemingly not understanding your favorite Henderson-Hasselbach
equation;
> > :
> > : 2 pH = (6 + 9.1) /2 pH = 7.55
> > :
> > : I have never seen seawater with a pH of 7.55. There is no ocean with
> that pH. Humm how
> > : come your equation is not working for you today.?
> > :
> > :
> > : "That pH I calculated is
> > : right in there. Is that magic? :)"
> > :
> > : I roll on the floor when I see this = 8.35
> > :
> > : Hum , just a brain far so excuse me for thinkin
> > :
> > : (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
> > :
> > : Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a
pH
> of 8.35 there
> > pal
> > : ? That 8.35 is what you are telling people the pH should be, but their
> meter says 6.4.
> > : This how people will READ this.
> > :
> > :
> > :
> > :
> > : 4.) More on Buffering Capacity
> > :
> > : "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes,
> your
> > : alkalinity equation."'
> > :
> > :
> > : Yup, I see that and in this case the HCO3 is the acid and the CO3 is
the
> base CORRECT.
> > In
> > : Alk you are only dealing with bases and how they react to an acid.
> Acidity deals acids
> > and
> > : how they recact to bases "Acidity, A concept that is exactly analogous
> to alkalinity but
> > : measures the base neutralizing
> > : capacity (BNC) of a solution is Acidity "Alk is the ANC Acid
> neutralizing capacity
> > :
> > : "Don't the components of a buffer account for the buffering capacity?
"
> > :
> > : Yes, they do but so do the acids which work as buffers. NaHCO3 is a
> buffer and can act
> > as
> > : an acid or base
> > :
> > : *** Buffering Capacity.**
> > : The power of a substance in solution to absorb acid or alkali without
> change in pH; this
> > : is highest at a pH value equal to the pKa value of the acid of the
> buffer pair.***
> > :
> > : ***Akalinity***
> > : Measure of the power of a solution to neutralise hydrogen ions (H+),
> usually expressed
> > as
> > : the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
> > :
> > :
> > : If one wants to call Alk Buffering capacity then one sure as a hell
can
> call Acidty
> > : Buffering Capacity also. As it is the ability to neutralizes an acid
> that is a
> > buffer.You
> > : have a pH of 7 and you add a buffer to lower it to a pH of 4, you are
> buffering the
> > water,
> > : that buffer is a acid.
> > :
> > : 5) CO2
> > :
> > : You are really confuse so it seems :-) You realllllllly indicate that
> CO2 is affected by
> > : the Alk or vise-versa
> > :
> > : "Yes, the pH will drop with the addition of CO2. Remove CO2 will
cause
> the
> > : pH to rise? How do you remove CO2? Once it is in solution it forms
> > : carbonic acid and neutralizes some of your 'buffer'."
> > :
> > : "With the exception of CO2?"
> > :
> > : No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
> > : Concepts)....PERIOD.You seem to think a that at least in two of your
> post that CO2 is
> > : affected by the Alk or vise-versa. Please go back to school or seek
> professor
> > :
> > : "Why in one case does CO2 from air lower pH and in the other case it
> raises
> > : it? Doesn't make sense."
> > :
> > : That is because you don't understand CO2 period. By the way I saved
> this, wanted to see
> > : if you would bite on the post I gave. Not bite at first, so time to
reel
> you in, as you
> > : did bite in another post..
> > :
> > : Lets make some sense of it for you, being that you have a pH.D in
> chemistry, so you say
> > .
> > :
> > : CO2 is naturally generated in a aquatic systems, it is capable of
raise
> to various
> > levels
> > : depending on a number of circumstances .It can be measure (except in
> seawater) or
> > : calculated using Buch/Park Equations (what we use for seawater. In
sort
> if you know the
> > pH
> > : and Alk you can calculate the CO2). If you aerate a system or a sample
> of water, even if
> > : the pH has only dropped a couple of tenths, due to an increase in CO2,
> the CO2 will
> > leave
> > : solution to the atmosphere.This will raise the pH. On the other hand
if
> theCO2 level is
> > : more of the norm and you have hikgh room air, such as in the winter,
the
> partial
> > pressure
> > : of the CO2 in air will be much higher than that in water, in which
case
> the CO2 will
> > enter
> > : the water and lower the pH. That is without an airstone. Adding an
> airstone will make it
> > : even worse,as you are now forcefully driving the CO2 into solution
even
> quicker. These
> > : test /experiments have been proven many times, it is not that may work
> could work they
> > do
> > : work.Yet you want to disagree and in another post say you haven't
tried
> it,.Seems to me
> > : that based on what you say it can't work So, in short you don't know
> what the hell you
> > are
> > : taking about. Go get a glass of seawater with a pH of about 8.3 and
> lower it to about
> > : 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK-
UP
> ( that is if you
> > : don't have a high room air CO2 problem.). This little test has been
done
> thousands of
> > : times in this hobby, with test kits, pH meters and even graphic
> printers.
> > :
> > : "This is where Boomer and I
> > : disagree. I say you would have to lower the pH very low in order to
> > : effectively remove CO2 by purging."
> > :
> > : You are 100 % wrong. Please come to our Chem forum and try and run
that
> by Randy, don't
> > : take my word on it. I already know what he will say.
> > :
> > : "Boomer didnt convince me it
> > : works at the pH of an aquarium, but I never tried it and I'm not sure
of
> > : this. "
> > :
> > : Well then come too our chem. forum and tell Randy he doesn't know what
> he is talking
> > about
> > : LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it
> should be easy for
> > : you to run the experiment LOL There are grade school kids that run the
> test and know
> > what
> > : happens and that I'm correct.
> > :
> > :
> > : "The equilibrium is a FUNCTION
> > : of pH."
> > :
> > : It is also a function of Alk or don't you know that. At a pH of 8.3,
Alk
> 2.25, the CO2
> > is
> > : about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk
to
> about .4 meq/ l
> > : or so the CO2 will be around .99 mg / l CO2, When dealing with
tanksCO2
> is not always in
> > : equilibrium with ambient air.
> > :
> > :
> > : ". But I wouldn't degas a solution of a
> > : specific gas (CO2) with a gas (this case he was using air) that
contains
> the
> > : same gas I am trying to purge."
> > :
> > : Why not ? We have a guy right now that is running tests on purging
> ambient air with a
> > : solution to remove CO2 gas from the air, before it enters the tank
> per/Randy's
> > suggestion.
> > : The same guy is doing some of my test using a Clinoptilolite, a
Zeolite
> mineral, that
> > has
> > : an affinity for CO2.This will be a dry CO2 scrubber
> > :
> > :
> > : Sorry Soutman but you sure as hell don't seem to know much about
aquatic
> chemistry. You
> > : seem to be guessing at everything.
> > :
> > : By the way have you read any of Randy's technical articles on water
> chemistry, been
> > saving
> > : these for last. There are a few on pH, Alk, CO2 .Here is a list
> > :
> > : Try and answer them 1-5 and lets see where we get THIS TIME :-) or
maybe
> we should just
> > : drop it. I could care less at this point.
> > :
> > : THE END
> > :
> > :
> > : ARTICLES
> > :
> > : The first two posts in this thread are lists of some of my articles
that
> relate to reef
> > : tank chemistry. In the next few posts are some of the articles
published
> by Craig
> > Bingman
> > : and others on reef chemistry issues.
> > :
> > : The first two posts in this thread are lists of some of my articles
that
> relate to reef
> > : tank chemistry. In the next few posts are some of the articles
published
> by Craig
> > Bingman
> > : and others on reef chemistry issues.
> > :
> > : Solving Common Problems
> > :
> > : Solving Calcium and Alkalinity Problems
> > : http://www.advancedaquarist.com/issues/nov2002/chem.htm
> > :
> > : Solutions to pH Problems
> > : http://www.advancedaquarist.com/iss...ne2002/chem.htm
> > :
> > : How to Select a Calcium and Alkalinity Supplementation Scheme
> > : http://www.advancedaquarist.com/issues/feb2003/chem.htm
> > :
> > : Phosphate Issues
> > : http://www.advancedaquarist.com/iss...pt2002/chem.htm
> > :
> > : Nitrate Issues
> > : http://www.advancedaquarist.com/iss...st2003/chem.htm
> > :
> > :
> > :
> > : Calcium and Alkalinity
> > :
> > : Solving Calcium and Alkalinity Problems
> > : http://www.advancedaquarist.com/issues/nov2002/chem.htm
> > :
> > : How to Select a Calcium and Alkalinity Supplementation Scheme
> > : http://www.advancedaquarist.com/issues/feb2003/chem.htm
> > :
> > : Calcium and Alkalinity Balance Issues
> > : http://reefkeeping.com/issues/2002-...ature/index.htm
> > :
> > : Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
> > : http://www.advancedaquarist.com/iss...ly2002/chem.htm
> > :
> > : The Relationship Between Alkalinity and pH.
> > : http://www.advancedaquarist.com/issues/may2002/chem.htm
> > :
> > : The Chemical & Biochemical Mechanisms of Calcification in Corals
> > : http://www.advancedaquarist.com/issues/apr2002/chem.htm
> > :
> > : Calcium
> > : http://www.advancedaquarist.com/issues/mar2002/chem.htm
> > :
> > : Alkalinity
> > : http://www.advancedaquarist.com/iss...2/chemistry.htm
> > :
> > :
> > : Iron
> > :
> > : First Iron Article: Macroalgae and Dosing Recommendations
> > : http://www.advancedaquarist.com/issues/aug2002/chem.htm
> > :
> > : Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> > : http://www.advancedaquarist.com/issues/oct2002/chem.htm
> > :
> > : Iodine
> > :
> > : Iodine in Marine Aquaria: Part I
> > : http://www.advancedaquarist.com/issues/mar2003/chem.htm
> > :
> > : Iodine in Reef Tanks 2: Effects on Macroalgae Growth
> > : http://www.advancedaquarist.com/iss...il2003/chem.htm
> > :
> > :
> > : Magnesium and Strontium
> > :
> > : Strontium
> > : http://www.advancedaquarist.com/issues/nov2003/chem.htm
> > :
> > : Magnesium
> > : http://www.advancedaquarist.com/issues/oct2003/chem.htm
> > :
> > : Magnesium and Strontium in Limewater
> > : http://www.advancedaquarist.com/issues/dec2003/chem.htm
> > :
> > :
> > : Limewater (kalkwasser)
> > :
> > : The Self Purification of Limewater (Kalkwasser)
> > : http://www.advancedaquarist.com/issues/may2003/chem.htm
> > :
> > : The Degradation of Limewater (Kalkwasser) in Air
> > : http://reefkeeping.com/issues/2003-...ature/index.htm
> > :
> > : How to Select a Calcium and Alkalinity Supplementation Scheme
> > : http://www.advancedaquarist.com/issues/feb2003/chem.htm
> > :
> > : Metals in Aquaria
> > :
> > : Aluminum and aluminum-based phosphate binders
> > : http://www.advancedaquarist.com/iss...ly2003/chem.htm
> > :
> > : Reef Aquaria with Low Soluble Metals
> > : http://reefkeeping.com/issues/2003-...ature/index.htm
> > :
> > : Tap Water in Reef Aquaria
> > : http://www.advancedaquarist.com/issues/jan2004/chem.htm
> > : First Iron Article: Macroalgae and Dosing Recommendations
> > : http://www.advancedaquarist.com/issues/aug2002/chem.htm
> > :
> > : Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> > : http://www.advancedaquarist.com/issues/oct2002/chem.htm
> > :
> > :
> > : Test Kit Reviews
> > :
> > : The Seachem Borate Alkalinity Test Kit
> > : http://www.advancedaquarist.com/iss...ne2003/chem.htm
> > :
> > : The Salifert Boron Test Kit
> > : http://www.advancedaquarist.com/iss...pt2003/chem.htm
> > :
> > : Boron and Borate (and pH buffering)
> > :
> > : Boron in a Reef Tank (and its effect on pH buffering)
> > : http://www.advancedaquarist.com/issues/dec2002/chem.htm
> > :
> > : The Seachem Borate Alkalinity Test Kit
> > : http://www.advancedaquarist.com/iss...ne2003/chem.htm
> > :
> > : The Salifert Boron Test Kit
> > : http://www.advancedaquarist.com/iss...pt2003/chem.htm
> > :
> > :
> > :
> > : Others
> > :
> > : Tap Water in Reef Aquaria
> > : http://www.advancedaquarist.com/issues/jan2004/chem.htm
> > :
> > : ORP
> > : http://reefkeeping.com/issues/2003-...ature/index.htm
> > :
> > : Chloramine
> > : http://reefkeeping.com/issues/2003-...ature/index.htm
> > :
> > : Silica in a Reef Tank
> > : http://advancedaquarist.com/issues/jan2003/feature.htm
> > :
> > : Specific Gravity (and temperature correction of hydrometers)
> > : http://www.advancedaquarist.com/iss...2/chemistry.htm
> > :
> > :
> > : The Complete Nitrogen Cycle
> > : http://www.animalnetwork.com/fish/l...a&RecordNo=3090
> > :
> > : Magnesium (older article with fonts screwed up)
> > : http://www.aquariumfish.com/aquariu...cid=124&search=
> > :
> > : Phosphate (older article now reproduced in a poor fashion)
> > : http://www.aquariumfish.com/aquariu...cid=124&search=
> > :
> > : Carbon Dioxide
> > : http://www.animalnetwork.com/fish/l...a&RecordNo=2074
> > :
> > : Using Conductivity to Measure Salinity
> > : http://www.aquariumfish.com/aquariu...cid=124&search=
> > :
> > : Understanding Seawater
> > : http://www.animalnetwork.com/fish2/...s/1/default.asp
> > :
> > : Protein Skimming: How It Works
> > : http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
> > :
> > :
> > :
> > : Articles by Craig Bingman:
> > :
> > : Carbon Dioxide tests
> > : http://www.animalnetwork.com/fish/l...n=&RecordNo=279
> > :
> > : Limewater, Acetic Acid and Sand Clumping
> > : http://www.animalnetwork.com/fish/l...n=&RecordNo=181
> > :
> > : Calcium and Alkalinity
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Calculation of Calcium Carbonate Saturation States in Reef Aquaria
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > :
> > : Calcification Rates in Several Tropical Coral Reef Aquaria
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Limits To Limewater...Revisited
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Expanding the Limits of Limewater: Adding Organic Carbon Sources
> (vinegar)
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > :
> > : Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Magnesium - Part I
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Magnesium - Part II
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : A Homemade Magnesium Supplement
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Simulating the Effect of Calcium Chloride and Sodium Bicarbonate
> Additions on Reef
> > Systems
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Additional Simulations: The Combined Effect Of Calcium Chloride
> > : /Sodium Bicarbonate Additions And Water Exchanges
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > :
> > : More articles by Craig Bingman:
> > :
> > : The Halogens - Part I: Bromine in Seawater and Aquaria
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : The Halogens - Part II: Fluoride
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Fluoride Depletion In Four Reef Aquariums
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : The Halogens - Part III: Iodine
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Measuring Halides
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : How Test Kits Work
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Borax pH Calibration
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : A pH Detective Story
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : How to Mix a Batch of Synthetic Seawater in Under Five Minutes
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > : SILICON - FOE OR FRIEND?
> > : http://www.animalnetwork.com/fish2/...s/1/default.asp
> > :
> > : The Composition Of Several Synthetic Seawater Mixes
> > : http://www.animalnetwork.com/fish2/...s/1/default.asp
> > :
> > : Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
> > : http://www.animalnetwork.com/fish2/...bio/default.asp
> > :
> > :
> > :
> > : Andy's calcium calculator
> > : http://www.andy-hipkiss.co.uk/cacalc.htm
> > :
> > : Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
> > : http://www.aquariumfish.com/aquariu...cid=124&search=
> > :
> > : Calcium Reactor Substrate -- Phosphate Levels
> > : by Greg Hiller
> > : http://www.advancedaquarist.com/iss...l2003/short.htm
> > :
> > :
> > : Indoor CO2 Problems
> > : http://www.advancedaquarist.com/iss...r2002/short.htm
> > :
> > : Simon Huntington's CaCO3/CO2 reactor article
> > :
> > : http://reefkeeping.com/issues/2002-...ature/index.htm
> > :
> > : Ron Shimek's Tank Water Analysis Article
> > : http://reefkeeping.com/issues/2002-...ature/index.htm
> > :
> > :
> > :
> > :
> > : Home made salinity standards thread:
> > :
> > : http://reefcentral.com/forums/showt...?threadid=65509
> > :
> > : Reef Chemicals Calculator
> > : http://www.kademani.com/reefchem.htm
> > :
> > :
> > :
> > : Boomer
> > :
> > : Want to talk chemistry ? The Reef Chemistry Forum
> > : http://www.reefcentral.com/vbulletin/index.php
> > :
> > :
> > : Former US Army Bomb Technician (EOD)
> > : Member; IABTI, NATEODA, WEODF, ISEE & IPS
> > :
> > : If You See Me Running You Better Catch-Up
> > :
> > :
> > : --
> > : Boomer
> > :
> > : Want to talk chemistry ? The Reef Chemistry Forum
> > : http://www.reefcentral.com/vbulletin/index.php
> > :
> > : Want to See More ?
> > : Please Join Our Growing Membership
> > : www.coralrealm.com
> > :
> > : If You See Me Running You Better Catch-Up
> > : "stoutman" <.@.> wrote in message
> news:aGuWb.148227$U%5.676753@attbi_s03...
> > : : Boomer,
> > : :
> > : : I am not sure if you are just messing with me or if you are truly
> confused.
> > : : I hope the latter. Please read from Top to Bottom.
> > : :
> > : :
> > : : From YOUR first link:
> > : :
> > : : http://www.waterontheweb.org/resources/glossary.html
> > : :
> > : : Acidity:
> > : : A measure of how acid a solution may be. A solution with a pH of
less
> than
> > : : 7.0 is considered acidic. Solutions with a pH of less than 4.5
contain
> > : : mineral acidity (due to strong inorganic acids), while a solution
> having a
> > : : pH greater than 8.3 contains no acidity.
> > : :
> > : : Yes,
> > : :
> > : : Good definition (for the most part). pH <7 is indeed acidic. pH >
7
> is
> > : : basic. Your web page had a definition for acidity, but not
basicity.
> > : : Strange. That's like defining GOOD and not defining BAD.
> > : :
> > : : Here is the IUPAC (International Union of Pure and Applied
Chemistry)
> > : : definition of acidity:
> > : :
> > : : http://www.chem.qmul.ac.uk/iupac/index.html
> > : :
> > : : acidity
> > : :
> > : : (1) Of a compound:
> > : :
> > : : For Brønsted acids it means the tendency of a compound to act as a
> hydron
> > : : donor. It can be quantitatively expressed by the acid dissociation
> constant
> > : : of the compound in water or some other specified medium. For Lewis
> acids it
> > : : relates to the association constants of Lewis adducts and -adducts.
> > : :
> > : : (2) Of a medium:
> > : :
> > : : The use of the term is mainly restricted to a medium containing
> Brønsted
> > : : acids, where it means the tendency of the medium to hydronate a
> specific
> > : : reference base
> > : :
> > : : basicity
> > : :
> > : : For Brønsted bases it means the tendency of a compound to act as
> hydron
> > : : (proton) acceptor. The basicity of a chemical species is normally
> expressed
> > : : by the acidity of the conjugate acid (see conjugate acid-base pair).
> For
> > : : Lewis bases it relates to the association constants of Lewis adducts
> > : : and -adducts
> > : :
> > : :
> > : :
> > : : Another definition from the same web page YOU cited: (this is the
> same web
> > : : page you cited above)
> > : :
> > : : Alkalinity:
> > : : Acid neutralizing or buffering capacity of water; a measure of the
> ability
> > : : of water to resist changes in pH caused by the addition of acids or
> bases
> > : : and therefore, the main indicator of susceptibility to acid rain; in
> natural
> > : : waters it is due primarily to the presence of bicarbonates,
carbonates
> and
> > : : to a much lesser extent occasionally borates, silicates and
> phosphates. It
> > : : is expressed in units of milligrams per liter (mg/l) of CaCO3
(calcium
> > : : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l =
1
> mg/l
> > : : of CaCO3. A solution having a pH below about 5 contains no
alkalinity.
> > : :
> > : : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and
> says
> > : : that alkalinity is the measure of ...(description of a buffer)
> > : :
> > : : A BUFFER IS : a measure of the ability of water to resist changes in
> pH
> > : : caused by the addition of acids or bases (from definition below)
> > : :
> > : :
> > : : I said:
> > : : ***alkalinity is a measurement of 'buffering capacity'***
> > : :
> > : : You said:
> > : : ***Alkalinity is not a measurement of BC
> > : :
> > : : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is
> not
> > : : logical.
> > : :
> > : : (THIS FROM THE SAME WEB PAGE YOU CITED):
> > : :
> > : : Buffer:
> > : : A substance which tends to keep pH levels fairly constant when acids
> or
> > : : bases are added.
> > : :
> > : : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
> > : :
> > : : a measure of the ability of water to resist changes in pH caused by
> the
> > : : addition of acids or bases
> > : :
> > : : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A
> BUFFER.
> > : :
> > : :
> > : : I went to all four links. None contradict what I have said. But
the
> first
> > : : one you cited contradicts YOU!
> > : :
> > : : I know what a buffer is. I know what acidity means. I know what
> alkalinity
> > : : means. No need to cite web pages that describe what I know and what
I
> wrote
> > : : in this discussion. Show me one that says alkalinity is not a
measure
> of
> > : : buffering capacity from a credible source.
> > : :
> > : :
> > : :
> > : :
> > : :
> > : :
> > : : "Boomer" > wrote in message
> > : : ...
> > : : > Alkalinity a measure of the amount of anions of weak acid in water
> and of
> > : : the cations
> > : : > balanced against them
> > : : > Take note it says ***acid***
> > : : >
> > : : > Buffering capacity the ability of a solution to resist or dampen
> changes
> > : : in pH upon the
> > : : > addition of acids or bases.
> > : : > Take note its says ***the addition of acids or bases***
> > : : >
> > : : > One more
> > : : >
> > : : > http://www.waterontheweb.org/resources/glossary.html
> > : : >
> > : : > We could go on like this all day, so what is the point ?
> > : : >
> > : : > You will LOVE this one
> > : : > http://www.kyantec.com/Tips/phbuffering.htm
> > : : >
> > : : > Don't you just lovbe PDF's
> > : : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
> > : : >
> > : : > Don't fall out of your chair
> > : : >
> http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
> > : : >
> > : : >
> > : : >
> > : : >
> > : : > --
> > : : > Boomer
> > : : >
> > : : > Want to talk chemistry ? The Reef Chemistry Forum
> > : : > http://www.reefcentral.com/vbulletin/index.php
> > : : >
> > : : > Want to See More ?
> > : : > Please Join Our Growing Membership
> > : : > www.coralrealm.com
> > : : >
> > : : > If You See Me Running You Better Catch-Up
> > : : > "stoutman" <.@.> wrote in message
> news:XB7Wb.19339$QA2.62332@attbi_s52...
> > : : > : Man here is another, google is a wonderful thing. I'm not
> filtering any
> > : : > : out, just posting what I find by GOOGLING for you.
> > : : > :
> > : : > :
> http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> > : : > :
> > : : > :
> > : : > : Wow, a gov link. Even the government is wrong, this must be a
> > : : conspiracy
> > : : > : against Boomer.
> > : : > :
> > : : > :
> > : : > :
> > : : > :
> > : : > : "Boomer" > wrote in message
> > : : > : ...
> > : : > : > Now I am getting bored
> > : : > : >
> > : : > : > "Don't the components of a buffer account for the buffering
> capacity?
> > : : > : Yes."
> > : : > : >
> > : : > : > Yes, agreed but you seem to fail what I'm saying. Buffering
> Capacity
> > : : and
> > : : > : Alkalinity are
> > : : > : > not the same, that has always been the issue. I gave the
> equation does
> > : : > : that look like an
> > : : > : > Alkalinity equation or how Alk is determined. I see you had
now
> > : : comments
> > : : > : on it what's
> > : : > : > wrong, why no comments on the equations I gave. Don't
understand
> them
> > : : or
> > : : > : what ? Again this
> > : : > : > is the equation for Buffering Capacity, also called Buffer
Index
> or
> > : : Buffer
> > : : > : Intensity. It
> > : : > : > is defined in most water chemistry and chemical oceanography
> text
> > : : books.
> > : : > : >
> > : : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] +
[H30+]
> +
> > : : CKa
> > : : > : [H3O+] / (Ka =
> > : : > : > H3O+])² )
> > : : > : >
> > : : > : > This is not Alkalinity now is it ?
> > : : > : >
> > : : > : > "I know how to do a titration, In fact I have done several.
How
> many
> > : : have
> > : : > : > you actually done? I don't mean by counting drops, I mean
with
> a
> > : : buret?"
> > : : > : >
> > : : > : > Well good for you, I use a Digital Titrator
> > : : > : >
> > : : > : > "Oh, I see,
> > : : > : > you think acidity is the opposite of alkalinity. In the world
> of
> > : : > : CHEMISTRY
> > : : > : > it's not. Maybe in aquarium newsgroups it is.
> > : : > : >
> > : : > : > Hum no, maybe you should go for a look at HACH's or LaMotte
> website or
> > : : the
> > : : > : book I
> > : : > : > suggested earlier. Please view a copy.
> > : : > : >
> > : : > : > Standard Methods for the Examination of Water and Wastewater
> > : : > : >
> > : : > : > This book, over 2000 pages, is the guide for water testing. If
> you are
> > : : > : reporting water
> > : : > : > test to the EPA you must use approved std from this text.I t
is
> > : : prepared
> > : : > : and published by
> > : : > : > the EPA, American Water Works Association and American Public
> Health
> > : : > : Association. You
> > : : > : > mean you don't have one and the issue is water chemistry
> > : : > : >
> > : : > : > You are confusing Acidity and Acidity as you know little about
> water
> > : : > : chemistry and
> > : : > : > procedures and test methods
> > : : > : >
> > : : > : > From SMEWW, section 2-30, 2310 ACIDITY
> > : : > : >
> > : : > : > "Acidity of water is its quantative capacity to react with a
> strong
> > : : base
> > : : > : to a designated
> > : : > : > pH"
> > : : > : >
> > : : > : > This is how you test for it
> > : : > : >
> > : : > : > A std alkali titration to methyl orange or phenolphthalein
> > : : > : > endpoint.
> > : : > : >
> > : : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that
> write
> > : : this
> > : : > : book, there are
> > : : > : > over 100 of them, they are wrong.
> > : : > : >
> > : : > : > Like Buffering Capacity you have your Acidity's mixed up
> > : : > : > In water measurement if you have a high Alk you also usually
> have a
> > : : high
> > : : > : Acidity.
> > : : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
> > : : CHEMISTRY
> > : : > : BOOK there pal.
> > : : > : >
> > : : > : >
> > : : > : > "These are all in equilibrium with each other. An initial
high
> pH
> > : : (above
> > : : > : > 6.4) will shift the equilibrium to the right to form HCO3-1.
If
> the
> > : : pH of
> > : : > : > the solution is above 10.3 (pKa2) the .........."
> > : : > : >
> > : : > : >
> > : : > : > Christ, there you go again with the FW ****. All your numbers
> are
> > : : wrong we
> > : : > : are dealing
> > : : > : > with SEAWATER
> > : : > : >
> > : : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is
> in the
> > : : form
> > : : > : > of HCO3-1 .
> > : : > : >
> > : : > : > I have already pointed that out and gave actual values at know
> > : : seawater
> > : : > : levels, go back
> > : : > : > and re-read it you aren't telling me anything here.Of course
> most is
> > : : HCO3
> > : : > : see...
> > : : > : >
> > : : > : >
> > : : > : > @ 20C and 34.3 ppt salinity
> > : : > : >
> > : : > : > CO2 = 0.52 %
> > : : > : >
> > : : > : > HCO3 = 86.4 %
> > : : > : >
> > : : > : > CO3 = 13.09 %
> > : : > : >
> > : : > : >
> > : : > : > "In your glass experiment you managed to lower the pH enough
to
> purge
> > : : out
> > : : > : CO2
> > : : > : > by boiling"
> > : : > : >
> > : : > : > The purpose behind the glass is to show that alk is not affect
> by CO2
> > : : and
> > : : > : vise-versa and
> > : : > : > how Co2 affects pH.
> > : : > : >
> > : : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and
that
> pH
> > : : drops
> > : : > : to say 8.1 it is
> > : : > : > usually due to excess CO2. If you took a glass of that water
and
> > : : aerated
> > : : > : it you WILL drive
> > : : > : > off the CO2 and raise the pH. It has been done a proven a
> million
> > : : times.
> > : : > : >
> > : : > : > "In order to 'purge' CO2 you would need to lower the
> > : : > : > pH to shift the equilibrium to below 6.4"
> > : : > : >
> > : : > : > The hell you do !!!.Do you know who many times people on this
NG
> to
> > : : > : include Dr. Craig
> > : : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned
to
> take a
> > : : > : sample of aquarium
> > : : > : > water and aerate it to see if the pH GOES UP AND when they
come
> back
> > : : with
> > : : > : the test it is
> > : : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D
CHEMIST
> > : : excess
> > : : > : CO2 in the tank
> > : : > : > water, increase the circulation for better gas exchange at the
> > : : surface,
> > : : > : reduce feeding,
> > : : > : > and try to improve on better skimming, thus reducing the
> bio-load and
> > : : pH
> > : : > : decline due to
> > : : > : > CO2.
> > : : > : >
> > : : > : >
> > : : > : > "I hope this helps. "
> > : : > : >
> > : : > : > Help, how can you when you miss everything. I should be
charging
> you
> > : : > : >
> > : : > : > Oh, by the way. Your websites, I have about 50 on these
issues,
> I
> > : : could
> > : : > : post them, not to
> > : : > : > mention I have all those water chemistry books, so there is no
> need to
> > : : > : view your sites.
> > : : > : >
> > : : > : > Finally are you afraid to come to our Chemistry Forum, afraid
to
> get
> > : : > : slapped by REAL
> > : : > : > chemists. I get a charge out of you can't post your ref .I
have
> posted
> > : : the
> > : : > : same or similar
> > : : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have
> 1500
> > : : posts
> > : : > : there and am the
> > : : > : > biggest contributor to his forum other than himself or maybe
> Habib
> > : : Sheka
> > : : > : >
> > : : > : > Hum, here are Randy's ref that he posted. He hosts the website
> > : : > : >
> > : : > : > S. RANDY HOLMES-FARLEY
> > : : > : > Arlington, Massachusetts
> > : : > : >
> > : : > : > EDUCATION
> > : : > : >
> > : : > : > 1982-1986 Harvard University Cambridge, MA
> > : : > : > PhD in Chemistry
> > : : > : > Research Advisor: George Whitesides
> > : : > : >
> > : : > : > Investigated the relationship between polymer surface
chemistry
> and
> > : : > : physical properties
> > : : > : > through controlled surface modification and testing.
> > : : > : >
> > : : > : > 1980-1982 Cornell University Ithaca, NY
> > : : > : > BA in Chemistry and Biology
> > : : > : > Graduated Summa Cum Laude
> > : : > : > Distinction in All Subjects
> > : : > : > Grade Point: 3.94/4.0
> > : : > : > Honors research: isolation and characterization of the subunit
> of CF1
> > : : > : enzyme
> > : : > : >
> > : : > : >
> > : : > : > 1978-1979 Stanford University Palo Alto, CA
> > : : > : > Grade Point: 3.55/4.0
> > : : > : >
> > : : > : >
> > : : > : > EXPERIENCE
> > : : > : >
> > : : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham,
> MA
> > : : > : > (bought out GelTex Pharmaceuticals in 2001)
> > : : > : > Vice President, Chemical Research 2001-present
> > : : > : > Senior Director, Chemical Research 1999-2001
> > : : > : > Director of Chemical Research 1997-1999
> > : : > : > Manager of Chemical Research 1995-1997
> > : : > : > Group Leader 1994-1995
> > : : > : > Senior Research Scientist 1992-1994
> > : : > : >
> > : : > : > Helped start GelTex as second employee
> > : : > : >
> > : : > : > Managed various research programs with multi-million dollar
> budgets
> > : : > : >
> > : : > : > Supervised research chemists (17+)
> > : : > : >
> > : : > : > Co-inventor of several polymeric pharmaceuticals and
> pharmaceutical
> > : : > : candidates including
> > : : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam
> Hydrochloride
> > : : (FDA
> > : : > : approved)
> > : : > : >
> > : : > : > Company Safety Officer for 3 years
> > : : > : >
> > : : > : > Chemical Hygiene Officer 2000-present
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > 1990-1992 GTE Corporation Waltham, MA
> > : : > : > Senior Member of Technical Staff
> > : : > : > Applied research involving polymer interfaces
> > : : > : > Metallization of plastics
> > : : > : > Polymer/polymer adhesion
> > : : > : > Optical coatings
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > 1986-1990 Lord Corporation Cary, NC
> > : : > : > Senior Research Scientist 1988-1990
> > : : > : > Research Scientist 1986-1988
> > : : > : > Basic and applied research on surface chemical bonding
> > : : > : > Developed new adhesive compositions
> > : : > : > Developed new sol-gel coatings for corrosion resistance
> > : : > : >
> > : : > : >
> > : : > : > HONORS AND AWARDS
> > : : > : >
> > : : > : > Industrial Innovations Award by Northeast Region of American
> Chemical
> > : : > : Society (6/2001)
> > : : > : >
> > : : > : > National Kidney Foundation of Northern California Honoree
> (5/2001)
> > : : > : >
> > : : > : > American Chemical Society/Polymer Chemistry Division
Industrial
> > : : Sponsors
> > : : > : > Award (8/2000)
> > : : > : >
> > : : > : > R&D 100 Award from R&D magazine (1999)
> > : : > : >
> > : : > : > Sherwin Williams Award in applied polymer science (9/85)
> > : : > : >
> > : : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985;
> 1985-1986)
> > : : > : >
> > : : > : > Award for highest GPA in Chemistry Department (6/82)
> > : : > : >
> > : : > : > Summa Cum Laude Honors in Chemistry (6/82)
> > : : > : >
> > : : > : > Phi Lamda Epsilon (6/82)
> > : : > : >
> > : : > : > Phi Beta Kappa (2/82)
> > : : > : >
> > : : > : > Cornell University Dean's List (1981, 1982)
> > : : > : >
> > : : > : > Harvard Book Club Award for highest GPA senior year (1978)
> > : : > : >
> > : : > : > First Place in western NY ACS high school chemistry exam
(1977)
> > : : > : >
> > : : > : > 1978-1979
> > : : > : >
> > : : > : >
> > : : > : > __________________
> > : : > : > Randy Holmes-Farley
> > : : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef
> Central
> > : : > : >
> > : : > : > Hobby Experience: 8 years with reefs
> > : : > : > Current Tanks: 90 gal mixed reef
> > : : > : > Interests: Reefkeeping, science, photography
> > : : > : >
> > : : > : >
> > : : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> > : : > : >
> > : : > : > Open this post in a new window | Report this post to a
moderator
> | IP:
> > : : > : Logged
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > 06/27/2003 02:44 PM
> > : : > : >
> > : : > : > Randy Holmes-Farley
> > : : > : > Chemistry Moderator
> > : : > : >
> > : : > : > Registered: Apr 2001
> > : : > : > Location: Arlington, Massachusetts
> > : : > : > Occupation: Chemist (Drug Discovery at Genzyme)
> > : : > : > Posts: 15282
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > Publications
> > : : > : >
> > : : > : >
> > : : > : > ISSUED UNITED STATES PATENTS
> > : : > : >
> > : : > : >
> > : : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen
Randall;
> > : : > : Mandeville, III; W. Harry.
> > : : > : > US 6,566,407; 5/20/2003
> > : : > : >
> > : : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley,
> Stephen
> > : : Randall;
> > : : > : Huval, Chad
> > : : > : > Cori.
> > : : > : > U.S. 6,517,825; 2/11/2003.
> > : : > : >
> > : : > : > 3. Method of making phosphate-binding polymers for oral
> > : : administration.
> > : : > : Holmes-Farley,
> > : : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M.
> U.S.
> > : : > : 6,509,013; 1/21/2003.
> > : : > : >
> > : : > : > 4. Combination therapy for treating hypercholesterolemia using
a
> bile
> > : : acid
> > : : > : sequestrant
> > : : > : > polymer
> > : : > : > and a cholesterol-lowering agent. Huval, Chad Cori;
> Holmes-Farley,
> > : : Stephen
> > : : > : Randall;
> > : : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> > : : > : >
> > : : > : > 5. Method for treating hypercholesterolemia with
polyallylamine
> > : : polymers.
> > : : > : Holmes-Farley,
> > : : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
> > : : Goldberg,
> > : : > : Dennis I. , US
> > : : > : > 6,423,754; 7/23/2002.
> > : : > : >
> > : : > : > 6. Ionic polymers as anti-infective agents Mandeville, W.
Harry,
> III;
> > : : > : Neenan, Thomas X..;
> > : : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> > : : > : >
> > : : > : > 7. Combination therapy for treating hypercholesterolemia and
> > : : > : atherosclerosis. Huval, Chad
> > : : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal,
> Pradeep
> > : : K.
> > : : > : U.S. 6,365,186;
> > : : > : > 4/2/2002.
> > : : > : >
> > : : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
> > : : Mandeville,
> > : : > : W. H., III;
> > : : > : > Huval; C.
> > : : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US
> 6,299,868;
> > : : > : 10/9/2001.
> > : : > : >
> > : : > : > 9. Polymers containing guanidinium groups as bile acid
> sequestrants.
> > : : Dhal;
> > : : > : P. K.; Holmes-
> > : : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> > : : > : >
> > : : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.;
> Mandeville, W.
> > : : H.,
> > : : > : III.; US
> > : : > : > 6,281,252;
> > : : > : > 8/28/2001.
> > : : > : >
> > : : > : > 11. Combination therapy for treating hypercholestrolemia.
Huval;
> C.
> > : : C.;
> > : : > : Holmes-Farley; S.
> > : : > : > R. ;
> > : : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> > : : > : >
> > : : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides,
> G. M.;
> > : : > : Holmes-Farley, S.
> > : : > : > R.; US
> > : : > : > 6,264,937; 7/24/2001.
> > : : > : >
> > : : > : > 13. Method for treating hypercholesterolemia with
unsubstituted
> > : : > : polydiallylamine polymers.
> > : : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
> K. ; US
> > : : > : 6,248,318;
> > : : > : > 6/19/2001.
> > : : > : >
> > : : > : > 14. Process for removing bile salts from a patient and
alkylated
> > : : > : compositions therefore.
> > : : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355;
> 5/1/2001.
> > : : > : >
> > : : > : > 15. Poly(diallylamine)-based bile acid sequestrants.
> Holmes-Farley, S.
> > : : R.;
> > : : > : Dhal, P. K.;
> > : : > : > Petersen,
> > : : > : > J. S.; US 6,203,785; 3/20/2001.
> > : : > : >
> > : : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S.
> R.;
> > : : Huval,
> > : : > : C. C.; US
> > : : > : > 6,190,649;
> > : : > : > 2/20/2001.
> > : : > : >
> > : : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.;
> Mandeville, W.
> > : : H.,
> > : : > : III.; US
> > : : > : > 6,177,478;
> > : : > : > 1/23/2001.
> > : : > : >
> > : : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
> > : : Holmes-Farley,
> > : : > : S. R.;
> > : : > : > Mandeville, W.
> > : : > : > H., III.; US 6,129,910; 10/10/2000.
> > : : > : >
> > : : > : > 19. Method for treating hypercholesterolemia with
unsubstituted
> > : : > : polydiallylamine polymers.
> > : : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
> K. ; US
> > : : > : 6,083,497;
> > : : > : > 7/4/2000.
> > : : > : >
> > : : > : > 20. Method of making phosphate-binding polymers for oral
> > : : administration.
> > : : > : Holmes-Farley, S.
> > : : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US
6,083,495;
> > : : 7/4/2000.
> > : : > : >
> > : : > : > 21. Process for removing bile salts from a patient and
alkylated
> > : : > : compositions therefore.
> > : : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
> > : : 5/23/2000.
> > : : > : >
> > : : > : > 22. Process for removing bile salts from a patient and
> compositions
> > : : > : therefor. Mandeville,
> > : : > : > W. H.,
> > : : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> > : : > : >
> > : : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III;
W.
> H;
> > : : > : Neenan; T. X.; Holmes-
> > : : > : > Farley; S. R. US 6,034,129; 3/7/2000.
> > : : > : >
> > : : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.;
> Mandeville, W.
> > : : H.,
> > : : > : III.; US
> > : : > : > 5,985,938;
> > : : > : > 11/16/99.
> > : : > : >
> > : : > : > 25. Process for removing bile salts from a patient and
> compositions
> > : : > : therefor. Mandeville,
> > : : > : > W. H.,
> > : : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> > : : > : >
> > : : > : > 26. Hydrophobic sequestrant for cholesterol depletion.
> Mandeville, W.
> > : : H.,
> > : : > : III.;
> > : : > : > Holmes-Farley;
> > : : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> > : : > : >
> > : : > : > 27. Hydrophilic nonamine-containing and amine-containing
> copolymers
> > : : and
> > : : > : their use as bile
> > : : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
> > : : 5,929,184;
> > : : > : 7/27/99.
> > : : > : >
> > : : > : > 28. Interpenetrating polymer networks for sequestration of
bile
> acids.
> > : : > : Mandeville, W. H.,
> > : : > : > III.;
> > : : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US
> 5,925,379;
> > : : > : 7/20/99.
> > : : > : >
> > : : > : > 29. Amine polymer sequestrant and method of cholesterol
> depletion.
> > : : > : Mandeville, W. H.,
> > : : > : > III.;
> > : : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> > : : > : >
> > : : > : > 30. Process for removing bile salts from a patient and
> compositions
> > : : > : therefor. Mandeville,
> > : : > : > W. H.,
> > : : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> > : : > : >
> > : : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
> depletion.
> > : : > : Mandeville, W. H.,
> > : : > : > III.;
> > : : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> > : : > : >
> > : : > : > 32. Process for removing bile salts from a patient and
> compositions
> > : : > : therefor. Mandeville,
> > : : > : > W. H.,
> > : : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> > : : > : >
> > : : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
> > : : Mandeville,
> > : : > : W. H., III.;
> > : : > : > Holmes-
> > : : > : > Farley, S. R.; US 5,703,188; 12/30/97.
> > : : > : >
> > : : > : > 34. Oral administration of iron-binding crosslinked amine
> polymers.
> > : : > : Mandeville, W. H.,
> > : : > : > III.;
> > : : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> > : : > : >
> > : : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
> Holmes-Farley,
> > : : S.
> > : : > : R.; US 5,693,675;
> > : : > : > 12/2/97.
> > : : > : >
> > : : > : > 36. Method for removing bile salts from a patient with
alkylated
> > : : > : crosslinked amine
> > : : > : > polymers,
> > : : > : > and preparation of the polymers. Mandeville, W. H., III.;
> > : : Holmes-Farley,
> > : : > : S. R.; US
> > : : > : > 5,679,717; 10/21/97.
> > : : > : >
> > : : > : > 37. Phosphate-binding polymers for oral administration.
> Holmes-Farley,
> > : : S.
> > : : > : R.; Mandeville,
> > : : > : > W.
> > : : > : > H., III.; US 5,667,775; 9/16/97.
> > : : > : >
> > : : > : > 38. Ion-exchange process using highly crosslinked polymers for
> > : : removing
> > : : > : bile salts from a
> > : : > : > patient, preparation of the polymers, and compositions
> containing
> > : : them.
> > : : > : Mandeville, W. H.,
> > : : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> > : : > : >
> > : : > : > 39. Hydrophobic amine polymer sequestrant and method of
> cholesterol
> > : : > : depletion. Mandeville,
> > : : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US
> 5,618,530;
> > : : 4/8/97.
> > : : > : >
> > : : > : > 40. Amine polymer sequestrant and method of cholesterol
> depletion.
> > : : > : Mandeville, W. H.,
> > : : > : > III.;
> > : : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> > : : > : >
> > : : > : > 41. Phosphate-binding polymers for oral administration.
> Holmes-Farley,
> > : : S.
> > : : > : R.; Mandeville,
> > : : > : > W.
> > : : > : > H., III.; US 5,496,545; 3/5/96.
> > : : > : >
> > : : > : > 42. Iron-binding polymers for oral administration. Mandeville,
> W. H.,
> > : : > : III.; Holmes-Farley,
> > : : > : > S. R.;
> > : : > : > US 5,487,888; 1/30/96.
> > : : > : >
> > : : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having
> active
> > : : > : hydrogens on the
> > : : > : > surface.
> > : : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> > : : > : >
> > : : > : > 44. Layered sol-gel coatings from organisilicon compounds.
> > : : Holmes-Farley,
> > : : > : S. R.; Yanyo, L.
> > : : > : > C.;
> > : : > : > US 5,182,143; 1/26/93.
> > : : > : >
> > : : > : > 45. Method for metal bonding using ultrathin primer coating.
> > : : > : Holmes-Farley, S. R.; Yanyo,
> > : : > : > L.
> > : : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> > : : > : >
> > : : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.;
Abbey,
> K. J.;
> > : : US
> > : : > : 5,096,962;
> > : : > : > 3/17/92.
> > : : > : >
> > : : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> > : : > : elastomer-metal bonding.
> > : : > : > Holmes-
> > : : > : > Farley, S. R.; US 5,102,956; 4/7/92.
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT
> ISSUED)
> > : : > : >
> > : : > : >
> > : : > : > 1. Aryl boronate functionalized polymers for treating obesity
> and
> > : : > : inhibiting fat uptake.
> > : : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III;
Dhal,
> > : : Pradeep
> > : : > : K.; Huval, Chad
> > : : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl.
(2003),
> 92
> > : : pp. WO
> > : : > : 0302571.
> > : : > : >
> > : : > : > 2. Preparation of aryl boronic acids for treating obesity.
> > : : Holmes-Farley,
> > : : > : Stephen Randall;
> > : : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal,
> Pradeep
> > : : K.
> > : : > : (Geltex
> > : : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO
> 0302570.
> > : : > : >
> > : : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide.
> Holmes-Farley,
> > : : > : Stephen Randall.
> > : : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32
> pp. WO
> > : : > : 0302130.
> > : : > : >
> > : : > : > 4. Method for reducing copper levels and treating copper
> toxicosis.
> > : : > : Holmes-Farley, Stephen
> > : : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl.
> (2002),
> > : : 45
> > : : > : pp. WO
> > : : > : > 0285383.
> > : : > : >
> > : : > : > 5. Method for treating gout and binding uric acid.
> Holmes-Farley,
> > : : Stephen
> > : : > : Randall; Burke,
> > : : > : > Steven K. WO 0285381 10/31/2002.
> > : : > : >
> > : : > : > 6. Method for treating gout and reducing serum uric acid.
> > : : Holmes-Farley,
> > : : > : Stephen Randall;
> > : : > : > Burke, Steven K WO 0285380 10/31/2002.
> > : : > : >
> > : : > : > 7. Amine condensation polymer bile acid sequestrants. Huval,
C.
> C.;
> > : : > : Holmes-Farley, S. R.;
> > : : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> > : : > : >
> > : : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H.,
> III and
> > : : > : Holmes-Farley, S.
> > : : > : > R.;
> > : : > : > WO 1999-US5662; 9/23/1999.
> > : : > : >
> > : : > : > 9. Amine-containing copolymers as bile acid sequestrants.
> > : : Holmes-Farley,
> > : : > : S. R.; Petersen,
> > : : > : > J. S.;
> > : : > : > WO 9933452; 7/8/1999.
> > : : > : >
> > : : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W.
H.,
> III
> > : : and
> > : : > : Holmes-Farley, S.
> > : : > : > R.;
> > : : > : > WO 9922743; 5/14/1999.
> > : : > : >
> > : : > : > 11. Polyallylamine polymers for removing bile salts and
treating
> > : : > : hypercholesterolemia, and
> > : : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H.,
> III;
> > : : Burke,
> > : : > : S. K.; Goldberg,
> > : : > : > D. I.; WO 9857652; 12/23/98.
> > : : > : >
> > : : > : > 12. Phosphate-bidning polymers combined with a calcium
> supplement for
> > : : oral
> > : : > : administration.
> > : : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
> Holmes-Farley,
> > : : S.
> > : : > : R.; WO 9842355;
> > : : > : > 10/1/98.
> > : : > : >
> > : : > : > 13. Hydrophobic heteroatom-containing sequestrant for
> cholesterol
> > : : > : depletion. Mandeville,
> > : : > : > W.
> > : : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449;
> 12/12/96.
> > : : > : >
> > : : > : > 14. Process for adjusting ion concentration in a patient and
> > : : compositions
> > : : > : therefor.
> > : : > : > Mandeville,
> > : : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> > : : > : >
> > : : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
> > : : interlayer
> > : : > : for improved
> > : : > : > metal-
> > : : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
> > : : 1/20/94.
> > : : > : >
> > : : > : > 16. Process for increased metal-substrate bond strength in
> metalized
> > : : > : plastics.
> > : : > : > Holmes-Farley, S.
> > : : > : > R.; Ger. Offen. 4322516; 7/6/93.
> > : : > : >
> > : : > : > 17. Electrorheological fluids and preparation of particles
> useful in
> > : : the
> > : : > : fluids.
> > : : > : > Troughton,
> > : : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie;
> Carlson, J.
> > : : > : David; Bares, Joseph
> > : : > : > E.;
> > : : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra
> Nell. EP
> > : : > : 394049;
> > : : > : > 10/24/1990.
> > : : > : >
> > : : > : > JOURNAL PUBLICATIONS
> > : : > : >
> > : : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William;
> Zhorov,
> > : : Eugene;
> > : : > : Guo, Amy;
> > : : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David
L.;
> > : : > : Mandeville, W. Harry;
> > : : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
> > : : 611-619.
> > : : > : >
> > : : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
> > : : synthesis
> > : : > : and biological
> > : : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley,
> S.
> > : : Randall;
> > : : > : Mandeville, W.
> > : : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal,
> Pradeep K.
> > : : > : Journal of
> > : : > : > Macromolecular Science, Pure and Applied Chemistry (2001),
> A38(12),
> > : : > : 1559-1574.
> > : : > : >
> > : : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by
> Molecular
> > : : > : Imprinting. Huval,
> > : : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.;
Holmes-Farley,
> S.
> > : : > : Randall; Mandeville,
> > : : > : > W.
> > : : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro,
> Robert
> > : : J.;
> > : : > : Chen, Xi; Dhal,
> > : : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> > : : > : >
> > : : > : > 4. Synthetic polymers for the binding of fat in the intestinal
> tract.
> > : : > : Jozefiak, Thomas H.;
> > : : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny,
Cynthia;
> > : : Huval,
> > : : > : Chad C.;
> > : : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney,
> Cynthia.
> > : : > : Abstracts of
> > : : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United
States,
> August
> > : : > : 26-30, 2001
> > : : > : > (2001), POLY-047 and Polymer Preprints (American Chemical
> Society,
> > : : > : Division of
> > : : > : > Polymer Chemistry) (2001), 42(2), 98.
> > : : > : >
> > : : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel
> polymer
> > : : gel
> > : : > : pharmaceutical.
> > : : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.;
Petersen,
> J.;
> > : : Ward,
> > : : > : J.; Sacchiero,
> > : : > : > B.;
> > : : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton,
K.
> A.;
> > : : Chen,
> > : : > : X.; Mazzeo, J.
> > : : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
> > : : > : >
> > : : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl
> and
> > : : other
> > : : > : bile acid
> > : : > : > sequestrants.
> > : : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.;
> Xu, Q.;
> > : : > : Hook, P.; Holmes-
> > : : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1),
> 708-709.
> > : : > : >
> > : : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
> > : : Holmes-Farley,
> > : : > : S. R; Polym.
> > : : > : > Mater. Sci. Eng (1999), 80, 246-247.
> > : : > : >
> > : : > : > 8. Design and characterization of of Sevelamer Hydrochloride:
a
> novel
> > : : > : phosphate-binding
> > : : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III;
> Ward,
> > : : J.;
> > : : > : Miller, K. L.;
> > : : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M.
S.-
> Pure
> > : : and
> > : : > : Appl. Chem.,
> > : : > : > A36(7&8), p. 1085 (1999).
> > : : > : >
> > : : > : > 9. Three generations of bile acid sequestrants. Mandeville, W.
> H.,
> > : : III;
> > : : > : Braunlin, W.;
> > : : > : > Dhal, P.;
> > : : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik,
> S.;
> > : : > : Rosenbaum, D.;
> > : : > : > Sacchiero,
> > : : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc.
> (1999),
> > : : > : 550, 3-15.
> > : : > : >
> > : : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked,
polymeric
> > : : phosphate
> > : : > : binder, on
> > : : > : > urinary
> > : : > : > phosphorous excretion in rats. Rosenbaum, D. P.;
Holmes-Farley,
> S. R.;
> > : : > : Mandeville, W. H.,
> > : : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
> Transplant.
> > : : > : (1997), 12(5)
> > : : > : > 961-964.
> > : : > : >
> > : : > : > 11. Thin anisotropic coatings based on sol-gel technology.
> > : : Holmes-Farley,
> > : : > : S. R.; Yanyo, L.
> > : : > : > C;
> > : : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem.
> 4),
> > : : 439-444.
> > : : > : >
> > : : > : > 12. The mechanism of cure initiation of a surface activated
> adhesive.
> > : : > : Holmes-Farley, S.
> > : : > : > R.;
> > : : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5),
> 409-420.
> > : : > : >
> > : : > : > 13. Adhesion promotion and corrosion prevention using thin
> anisotropic
> > : : > : coatings. Holmes-
> > : : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991),
> 5(2),
> > : : > : 131-151.
> > : : > : >
> > : : > : > 14. Wetting of functionalized polyethylene having ionizable
> organic
> > : : acids
> > : : > : and bases at the
> > : : > : > polymer-water interface: relations between functional group
> polarity,
> > : : > : extent of
> > : : > : > ionization,
> > : : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C.
D.;
> > : : > : Whitesides, G. M.;
> > : : > : > Langmuir
> > : : > : > (1988), 4(4), 921-937.
> > : : > : >
> > : : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols
> with a
> > : : > : single hydroxy group.
> > : : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> > : : > : >
> > : : > : > 16. Reconstruction of the interface of oxidatively
> functionalized
> > : : > : polyethylene (PE-CO2H)
> > : : > : > and
> > : : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.;
> Nuzzo,
> > : : R.;
> > : : > : McCarthy, T. J.;
> > : : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also
> Report
> > : : (1987),
> > : : > : AD-
> > : : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> > : : > : >
> > : : > : > 17. Surface-modified polyethylene film: the relationship
between
> > : : surface
> > : : > : chemistry and
> > : : > : > physical
> > : : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987,
> 47(11),
> > : : 4537.
> > : : > : >
> > : : > : > 18. Reactivity of carboxylic acid and ester groups in the
> > : : functionalized
> > : : > : interfacial
> > : : > : > region of
> > : : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> > : : > : differentiation of the
> > : : > : > functional groups into shallow and deep subsets based on a
> comparison
> > : : of
> > : : > : contact angle and
> > : : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.;
> Langmuir
> > : : > : (1987), 3(1), 62-
> > : : > : > 76.
> > : : > : >
> > : : > : > 19. Fluorescence properties of dansyl groups covalently bonded
> tot he
> > : : > : surface of
> > : : > : > oxidatively
> > : : > : > functionalized low-density polyethylene film. Holmes-Farley,
S.
> R.;
> > : : > : Whitesides, G. M.;
> > : : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985),
TR-85-2;
> > : : > : AD-A162435/2/GAR,
> > : : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> > : : > : >
> > : : > : > 20. Acid-base behavior of carboxylic acid groups covalently
> attached
> > : : at
> > : : > : the surface of
> > : : > : > polyethylene: The usefulness of contact angle in following the
> > : : ionization
> > : : > : of surface
> > : : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy,
T.
> J.;
> > : : > : Deutch, J.;
> > : : > : > Whitesides,
> > : : > : > G. M.; Langmuir (1985), 1(6), 725-740.
> > : : > : >
> > : : > : > 21. The thermal stability of a surface modified solid organic
> polymer.
> > : : > : Holmes-Farley, S.
> > : : > : > R.;
> > : : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53,
127-131.
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> > : : > : >
> > : : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R.
> Advanced
> > : : > : Aquarist. June 2003.
> > : : > : >
> > : : > : > 2. The Self Purification of Limewater (Kalkwasser).
> Holmes-Farley, R.
> > : : > : Advanced Aquarist.
> > : : > : > May
> > : : > : > 2003.
> > : : > : >
> > : : > : > 3. The Degradation of Limewater (Kalkwasser) in Air.
> Holmes-Farley, R.
> > : : > : Reefkeeping May
> > : : > : > 2003.
> > : : > : >
> > : : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
> Reefkeeping
> > : : > : April 2003.
> > : : > : >
> > : : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae
> Growth.
> > : : > : Holmes-Farley, R.
> > : : > : > Advanced Aquarist; April 2003.
> > : : > : >
> > : : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae
> Growth.
> > : : > : Holmes-Farley, R.
> > : : > : > Advanced Aquarist; April 2003.
> > : : > : >
> > : : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R.
Advanced
> > : : Aquarist;
> > : : > : March 2003.
> > : : > : >
> > : : > : > 8. How to Select a Calcium and Alkalinity Supplementation
> Scheme.
> > : : > : Holmes-Farley, R.
> > : : > : > Advanced Aquarist; February 2003.
> > : : > : >
> > : : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> January
> > : : > : 2003.
> > : : > : >
> > : : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> > : : December
> > : : > : 2002.
> > : : > : >
> > : : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
> > : : Advanced
> > : : > : Aquarist; November
> > : : > : > 2002.
> > : : > : >
> > : : > : > 12. Iron: A Look at Organisms Other than Macroalgae.
> Holmes-Farley, R.
> > : : > : Advanced Aquarist;
> > : : > : > November 2002.
> > : : > : >
> > : : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.;
Advanced
> > : : Aquarist,
> > : : > : September 2002.
> > : : > : >
> > : : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist,
> August
> > : : > : 2002.
> > : : > : >
> > : : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.;
Reefkeeping.com,
> April
> > : : > : 2002.
> > : : > : >
> > : : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R.
> Advanced
> > : : > : Aquarist; July 2002
> > : : > : >
> > : : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced
> Aquarist;
> > : : June
> > : : > : 2002.
> > : : > : >
> > : : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley,
> R.
> > : : Advanced
> > : : > : Aquarist, May
> > : : > : > 2002.
> > : : > : >
> > : : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in
> Corals.
> > : : > : Holmes-Farley, R.
> > : : > : > Advanced Aquarist, April 2002.
> > : : > : >
> > : : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> > : : > : >
> > : : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February
> 2002.
> > : : > : >
> > : : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist,
> January
> > : : 2002.
> > : : > : >
> > : : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium
> Frontiers
> > : : > : 2000.
> > : : > : >
> > : : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R.
> Aquarium
> > : : > : Frontiers 2000.
> > : : > : >
> > : : > : > 25. Phosphate..What is it and why should you care.
> Holmes-Farley, R.
> > : : > : Aquarium Frontiers
> > : : > : > 2000.
> > : : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
> > : : Frontiers
> > : : > : 2000.
> > : : > : >
> > : : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium
> Frontiers
> > : : 2000.
> > : : > : >
> > : : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium
Frontiers
> 1999.
> > : : > : >
> > : : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > : > Boomer
> > : : > : >
> > : : > : > Want to talk chemistry ? The Reef Chemistry Forum
> > : : > : > http://www.reefcentral.com/vbulletin/index.php
> > : : > : >
> > : : > : > Want to See More ?
> > : : > : > Please Join Our Growing Membership
> > : : > : > www.coralrealm.com
> > : : > : >
> > : : > : >
> > : : > : >
> > : : > :
> > : : > :
> > : : >
> > : : >
> > : :
> > : :
> > : :
> > :
> > :
> >
> >
>
>

[Boomer]

Yes, of cause I remember, as I said I posted it for a reason. I see you have used only
that link for your definition, as it makes you look right.You have avoided all Alk
definitions in a chemistry book, to include your own definition *****to resist a drop in
pH due to the addition of acid***, which is the same as the others I posted .Agreed, of
course not.You know that Alk isn't defined as "by the addition of acids or bases "and is
only the " addition of an acid", so why are you accepting the definition ?.You know that
when you titrate it is an acid added and never a base. In one breath it says Alk is "Acid
neutralizing " and then they say "by the addition of acids or bases ".You can't have it
both ways and YOU know that Agreed . If the word "base" was left out I would not have much
to say. Agreed


"Alkalinity is a
measurement of BUFFERING CAPACITY."

No it is not a measurement of BUFFERING CAPACITY, it is a indication of BC. I have said
this at least twice. If you know your BC you can calculate Alk and if you can do one you
can do the other agreed. What I have tried to convey from the beginning is that Alk and BC
are not the same thing. You in one of your other posts have said they are not the same
thing and never said they were. Now you seem to be saying they are the same thing

"So, when we measure ALKALINITY (and we know the pH) we are in effect
measuring BUFFERING CAPACITY.

More or less YES in an "effect" but Alk tells you not much of anything when a base is
added Agreed. That is called Acidity, which I see you have avoided again as if there is
no such thing. I also said that for us the only thing we need to be concerned about is
Alk, so BC would fit in, as we could care less about the ability to neutralize a base or
measure Acidity. So, if you knew your pH , Alk or Acy you would really know what you BC is
doing for you Agreed.

On Bc, we have both left something from my first equation, so I thought I would post it
again for you, as I like being honest .I'm surprised you didn't catch it :-)

B = dCb / dpH = - dCa / dpH

So;

B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa [H3O+] / (Ka =
H3O+])² )

or

B (Buffering Capacity) = - dCa / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa [H3O+] / (Ka =
H3O+])² )

There are number of was to mathematically express BC. Two of the most common are the
change in Alk with the pH at constant total carbonate, the other is change in Alk with pH
constant CO2 pp. In some examples of Bc, Bc is the inverse slope of the Alk titration
curve ( I'm sure yo
u will love this) In the other over the pH range, while BC is going through minimum, Bpp
increases linearly. This difference is caused by the uptake of CO2 by the solution, which
increases Ct as pH increases.To bad we can't or my server won't allow me, to post
attachments. I have a nice BC cure of various species as a function of pC/pH diagrams, set
to a pKa. curve


On another issue

"In order to remove CO2 (g) you ideally would want to shift
the equilibrium to the left by LOWERING the pH"


You may want to try and re-explain this

CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
HCO3-1 <-------> CO3-2


As the reaction shifts to left the pH gets higher as CO2 leaves the system.You don't have
to lower the pH to remove CO2. Case in point plants. As they remove CO2 the pH rises,
continued removal of the Sigma CO2 ( CO2, H2CO3, HCO3,CO3) cause further rising until
there is mostly only carbonate (CO3) left and a high pH. Another case, at a pH of 8.00 and
Alk of 4 meq / l ( 1.4 mg / l CO2) you have much more CO2 than at 2 meq/ l (0.65mg / l).
.. Aeration of the water can drive off the CO, no lowering of the pH required., the removal
will cause the pH to rise .On the other hand, trying to remove CO2 @ 2 meq / l won't get
you much of anywhere in this case. Also, even a low pH doesn't mean you can drive of CO2.
If the seawater pH was say 7.5, you would think not problem to drive off CO2. If the Alk
was 0.25 there would be about .35 mg / l CO2 to blow off. At the alk of 4.00 meq / l the
CO2 is 5 mg / l.Usually, when people have a lower pH, say 7.9 or so, it is do to CO2, so
the pH has lowered, increasing the CO2, to allow one to blow it off easier and bring the
pH back up.

CO2 = [CA(Carbonate Alk) x aH ] / [pK1(1 + 2pK2 /aH)]

I think we just got off on the wrong foot, hope things look better.

I'll be gone for the weekend, leaving in an hour, so have a nice weekend :-)




--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

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Please Join Our Growing Membership
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If You See Me Running You Better Catch-Up
"stoutman" <.@.> wrote in message news:lcRWb.299984$na.451117@attbi_s04...
: > Humm, since when does Alk have anything to do in regards to the addition
: of BASE.
:
: You tell me. Your the one that posted a link to a web page that had this
: definition of alkalinity. Looks like you put yourself in your own hole pal.
:
: Remember posting this link:
:
: http://www.waterontheweb.org/resources/glossary.html
:
: Here is the definition of alkalinity from the web page YOU cited. (I
: recommend you read the web pages you are citing before you cite them)
: Alkalinity:
: Acid neutralizing or buffering capacity of water; a measure of the ability
: of water to resist changes in pH caused by the addition of acids or BASES.
:
:
: > It sure is funny how all of the chemist that write water chemistry
: textbooks never say Alk
: > is the Buffering Capacity of a solution.
:
: Neither did I. I said (for the umpth teen time) Alkalinity is a
: measurement of BUFFERING CAPACITY.
:
: When you measure alkalinity you know your BUFFERING CAPACITY (if you know
: your pH). Its a two for one.
:
: SEE MY OTHER POST FROM TODAY.
:
:
:
: "Boomer" > wrote in message
: ...
: >
: > "I am not sure if you are just messing with me "
: >
: > Yes, messing with you, it is called trolling a troll, to see where the
: hell you would go
: > and what you would say in regards to last posts. It is called honesty, of
: which you have
: > none off to say the least,that I can see.You always like to post what
: suits you and just
: > avoid ref I give. So lets start where you are WRONG and have a great lack
: of understanding
: > of things, to include pointing out all your gross error which you still
: FAIL to
: > acknowledge and which can be prove in many water chem. ref. .I doubt like
: hell you are a
: > chemist at all.You seem to want to con people into thinkin' you are. But
: then again, I
: > have seen chemists like you before, they are not familiar with the, but
: they ASK to have
: > it explained and ask for REF.YOU just shoot from the hip. WHAT GETS YOU IN
: TROUBLE. You
: > remind me of snoot-noise kid that come here and other NG's and
: forums...that think they
: > know, buy hey, maybe I'm wrong :-)
: >
: >
: >
: > 1). Acidity
: >
: > "***Benjamin,Water Chemistry (2002, pages 262-263).***
: >
: > ***Acidity A concept that is exactly analogous to alkalinity but measures
: the base
: > neutralizing
: > capacity (BNC) of a solution is Acidity. The quantitative represents the
: concentration of
: > OH- ions that must be added to titrate the solution to a pH near 10.5***
: >
: > So that means that not only in Benjamin wrong but, so are Stumm & Morgan,
: Millero, Pilosn,
: > Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I
: said, you have your
: > acidity and Acidy mixed up. Acidity as defined above is covered in most
: water chemistry
: > books, written by chemists, who's field of expertise is water chemistry.
: You can even buy
: > Acidity test kits from, HACH, LaMotte, etc..
: >
: > You mean you didn't read this or are you just avoiding it .The same
: definition can be
: > found in almost any std water chemistry book.
: >
: > I have run into few chemists, that are NOT familiar with the above. Some
: water reports
: > require the above Acidity measuring. The issue with you is you do not
: understand WATER
: > CHEMISTRY. Everything you have posted can be found a general chemistry
: book
: >
: >
: >
: >
: > 2) Alk and BC
: >
: > From the link
: >
: > Alkalinity
: > ***Acid neutralizing or buffering capacity of water; a measure of the
: ability of water to
: > resist changes in pH caused by the addition of acids or bases ***
: >
: > This is a Buffering Capacity definition not Alk
: >
: > Humm, since when does Alk have anything to do in regards to the addition
: of BASE. As I
: > pointed out in the first post the term is often miss used. Even in YOUR
: own posts you say
: > it is based on a acid addition, no mention of **base or acid** addition
: by you. Are you
: > getting confused or what. Or is more you are trying to confuse everyone
: you are right. The
: > above is a definition for Buffer Capacity NOT Alk
: >
: > From Drew, Geochemistry of Natural Waters
: >
: > "alkalinity, which is formally defined as the equivalent sum of bases that
: are titratable
: > with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH of
: the solution is
: > progressively lowered by the addition of a strong acid (HCL), all the
: anions on the right
: > will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4, H2S,organic
: acids, H20)"
: >
: > This follows almost all description of Alk, that it is acid neutralizing
: reaction and has
: > nothing to do with base neutralizing, which is Acidity (BNC) .I defined
: these before you
: > had no comment
: >
: >
: > Even the links that give the Buffering Capacity definition is wrong, as is
: the UIPAC on
: > Alkalinity. Alkalinity has nothing to do with the addition of bases only
: acids. When you
: > use the words "base and acid" it becomes BC
: >
: > Even YOU MUST disagree with these definitions, from YOUR own post
: >
: > Think of alkalinity as 'buffering capacity'. Or the ability of a solution
: > ***to resist a drop in pH due to the addition of acid***
: >
: > Where the flip is the base addition forget it ?
: >
: > From Butler; Carbon Dioxide Equilibrium and Their Applications (professor
: emeritus
: > Harvard University) an expert on the subject.
: >
: > Buffering Index (Buffering Capacity, Buffer Intensity).
: >
: > ***This concept was first developed for mixtures of approximately equal
: proportions of
: > conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such
: buffer solutions
: > strongly resist changes in pH when acids or bases are added and are useful
: as pH
: > standards. The Buffer Index tells how great the resistance to pH changes
: will be.**
: >
: > also from Butler
: >
: > Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
: >
: > Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
: >
: > Acidity is in fact just the negative of Alkalinity ***
: >
: > http://www.lagoonsonline.com/acid.htm
: >
: >
: http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.h
: tm?E+mystore
: >
: > It sure is funny how all of the chemist that write water chemistry
: textbooks never say Alk
: > is the Buffering Capacity of a solution. They are always treated and
: defined separately.
: >
: > If you or others choose to treat Alk and BC as the same, well, just have
: at it. As I said
: > in first post I know what you mean.
: >
: > "No need to cite web pages that describe what I know and what I wrote
: > in this discussion"
: >
: > No you don't know, who are you trying to convince any way, me, the guys
: here and/or all
: > the water chemists in this world. As I said before go get a dam WATER
: CHEMISTRY book or
: > shut the hell up.You keep trying to define things from a general chemistry
: book WE ARE IN
: > THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
: >
: >
: >
: >
: >
: > 3). pKa's and what you don't know or seem to be confused on
: >
: > "Therefore, it has two pKa's
: > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
: The
: > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated is
: > right in there. Is that magic? :)"
: >
: > Here it is agin that is twice at least
: >
: > "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this
: example)
: > you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium will
: > be shifted to HCO3-2 by a ratio of 1:100.
: >
: > Oh wait , there is a third time LOL
: >
: > "At the pH of seawater, the buffering capacity of carbonate is at it's
: > weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
: >
: >
: > Lets just dunk you on this one. I am taking note you refuse to reply to
: YOUR errors
: >
: > So you calculated the pH of seawater with freshwater pKa's, now that is a
: good trick. From
: > a number of seawater chemistry books the seawater pKa's are 6 & 9.1, so
: according to you,
: > seemingly not understanding your favorite Henderson-Hasselbach equation;
: >
: > 2 pH = (6 + 9.1) /2 pH = 7.55
: >
: > I have never seen seawater with a pH of 7.55. There is no ocean with that
: pH. Humm how
: > come your equation is not working for you today.?
: >
: >
: > "That pH I calculated is
: > right in there. Is that magic? :)"
: >
: > I roll on the floor when I see this = 8.35
: >
: > Hum , just a brain far so excuse me for thinkin
: >
: > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
: >
: > Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a pH of
: 8.35 there pal
: > ? That 8.35 is what you are telling people the pH should be, but their
: meter says 6.4.
: > This how people will READ this.
: >
: >
: >
: >
: > 4.) More on Buffering Capacity
: >
: > "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes, your
: > alkalinity equation."'
: >
: >
: > Yup, I see that and in this case the HCO3 is the acid and the CO3 is the
: base CORRECT. In
: > Alk you are only dealing with bases and how they react to an acid. Acidity
: deals acids and
: > how they recact to bases "Acidity, A concept that is exactly analogous to
: alkalinity but
: > measures the base neutralizing
: > capacity (BNC) of a solution is Acidity "Alk is the ANC Acid neutralizing
: capacity
: >
: > "Don't the components of a buffer account for the buffering capacity? "
: >
: > Yes, they do but so do the acids which work as buffers. NaHCO3 is a buffer
: and can act as
: > an acid or base
: >
: > *** Buffering Capacity.**
: > The power of a substance in solution to absorb acid or alkali without
: change in pH; this
: > is highest at a pH value equal to the pKa value of the acid of the buffer
: pair.***
: >
: > ***Akalinity***
: > Measure of the power of a solution to neutralise hydrogen ions (H+),
: usually expressed as
: > the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
: >
: >
: > If one wants to call Alk Buffering capacity then one sure as a hell can
: call Acidty
: > Buffering Capacity also. As it is the ability to neutralizes an acid that
: is a buffer.You
: > have a pH of 7 and you add a buffer to lower it to a pH of 4, you are
: buffering the water,
: > that buffer is a acid.
: >
: > 5) CO2
: >
: > You are really confuse so it seems :-) You realllllllly indicate that CO2
: is affected by
: > the Alk or vise-versa
: >
: > "Yes, the pH will drop with the addition of CO2. Remove CO2 will cause
: the
: > pH to rise? How do you remove CO2? Once it is in solution it forms
: > carbonic acid and neutralizes some of your 'buffer'."
: >
: > "With the exception of CO2?"
: >
: > No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
: > Concepts)....PERIOD.You seem to think a that at least in two of your post
: that CO2 is
: > affected by the Alk or vise-versa. Please go back to school or seek
: professor
: >
: > "Why in one case does CO2 from air lower pH and in the other case it
: raises
: > it? Doesn't make sense."
: >
: > That is because you don't understand CO2 period. By the way I saved this,
: wanted to see
: > if you would bite on the post I gave. Not bite at first, so time to reel
: you in, as you
: > did bite in another post..
: >
: > Lets make some sense of it for you, being that you have a pH.D in
: chemistry, so you say .
: >
: > CO2 is naturally generated in a aquatic systems, it is capable of raise to
: various levels
: > depending on a number of circumstances .It can be measure (except in
: seawater) or
: > calculated using Buch/Park Equations (what we use for seawater. In sort if
: you know the pH
: > and Alk you can calculate the CO2). If you aerate a system or a sample of
: water, even if
: > the pH has only dropped a couple of tenths, due to an increase in CO2, the
: CO2 will leave
: > solution to the atmosphere.This will raise the pH. On the other hand if
: theCO2 level is
: > more of the norm and you have hikgh room air, such as in the winter, the
: partial pressure
: > of the CO2 in air will be much higher than that in water, in which case
: the CO2 will enter
: > the water and lower the pH. That is without an airstone. Adding an
: airstone will make it
: > even worse,as you are now forcefully driving the CO2 into solution even
: quicker. These
: > test /experiments have been proven many times, it is not that may work
: could work they do
: > work.Yet you want to disagree and in another post say you haven't tried
: it,.Seems to me
: > that based on what you say it can't work So, in short you don't know what
: the hell you are
: > taking about. Go get a glass of seawater with a pH of about 8.3 and lower
: it to about
: > 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK- UP
: ( that is if you
: > don't have a high room air CO2 problem.). This little test has been done
: thousands of
: > times in this hobby, with test kits, pH meters and even graphic printers.
: >
: > "This is where Boomer and I
: > disagree. I say you would have to lower the pH very low in order to
: > effectively remove CO2 by purging."
: >
: > You are 100 % wrong. Please come to our Chem forum and try and run that by
: Randy, don't
: > take my word on it. I already know what he will say.
: >
: > "Boomer didnt convince me it
: > works at the pH of an aquarium, but I never tried it and I'm not sure of
: > this. "
: >
: > Well then come too our chem. forum and tell Randy he doesn't know what he
: is talking about
: > LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it
: should be easy for
: > you to run the experiment LOL There are grade school kids that run the
: test and know what
: > happens and that I'm correct.
: >
: >
: > "The equilibrium is a FUNCTION
: > of pH."
: >
: > It is also a function of Alk or don't you know that. At a pH of 8.3, Alk
: 2.25, the CO2 is
: > about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk to
: about .4 meq/ l
: > or so the CO2 will be around .99 mg / l CO2, When dealing with tanksCO2 is
: not always in
: > equilibrium with ambient air.
: >
: >
: > ". But I wouldn't degas a solution of a
: > specific gas (CO2) with a gas (this case he was using air) that contains
: the
: > same gas I am trying to purge."
: >
: > Why not ? We have a guy right now that is running tests on purging ambient
: air with a
: > solution to remove CO2 gas from the air, before it enters the tank
: per/Randy's suggestion.
: > The same guy is doing some of my test using a Clinoptilolite, a Zeolite
: mineral, that has
: > an affinity for CO2.This will be a dry CO2 scrubber
: >
: >
: > Sorry Soutman but you sure as hell don't seem to know much about aquatic
: chemistry. You
: > seem to be guessing at everything.
: >
: > By the way have you read any of Randy's technical articles on water
: chemistry, been saving
: > these for last. There are a few on pH, Alk, CO2 .Here is a list
: >
: > Try and answer them 1-5 and lets see where we get THIS TIME :-) or maybe
: we should just
: > drop it. I could care less at this point.
: >
: > THE END
: >
: >
: > ARTICLES
: >
: > The first two posts in this thread are lists of some of my articles that
: relate to reef
: > tank chemistry. In the next few posts are some of the articles published
: by Craig Bingman
: > and others on reef chemistry issues.
: >
: > The first two posts in this thread are lists of some of my articles that
: relate to reef
: > tank chemistry. In the next few posts are some of the articles published
: by Craig Bingman
: > and others on reef chemistry issues.
: >
: > Solving Common Problems
: >
: > Solving Calcium and Alkalinity Problems
: > http://www.advancedaquarist.com/issues/nov2002/chem.htm
: >
: > Solutions to pH Problems
: > http://www.advancedaquarist.com/iss...ne2002/chem.htm
: >
: > How to Select a Calcium and Alkalinity Supplementation Scheme
: > http://www.advancedaquarist.com/issues/feb2003/chem.htm
: >
: > Phosphate Issues
: > http://www.advancedaquarist.com/iss...pt2002/chem.htm
: >
: > Nitrate Issues
: > http://www.advancedaquarist.com/iss...st2003/chem.htm
: >
: >
: >
: > Calcium and Alkalinity
: >
: > Solving Calcium and Alkalinity Problems
: > http://www.advancedaquarist.com/issues/nov2002/chem.htm
: >
: > How to Select a Calcium and Alkalinity Supplementation Scheme
: > http://www.advancedaquarist.com/issues/feb2003/chem.htm
: >
: > Calcium and Alkalinity Balance Issues
: > http://reefkeeping.com/issues/2002-...ature/index.htm
: >
: > Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
: > http://www.advancedaquarist.com/iss...ly2002/chem.htm
: >
: > The Relationship Between Alkalinity and pH.
: > http://www.advancedaquarist.com/issues/may2002/chem.htm
: >
: > The Chemical & Biochemical Mechanisms of Calcification in Corals
: > http://www.advancedaquarist.com/issues/apr2002/chem.htm
: >
: > Calcium
: > http://www.advancedaquarist.com/issues/mar2002/chem.htm
: >
: > Alkalinity
: > http://www.advancedaquarist.com/iss...2/chemistry.htm
: >
: >
: > Iron
: >
: > First Iron Article: Macroalgae and Dosing Recommendations
: > http://www.advancedaquarist.com/issues/aug2002/chem.htm
: >
: > Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
: > http://www.advancedaquarist.com/issues/oct2002/chem.htm
: >
: > Iodine
: >
: > Iodine in Marine Aquaria: Part I
: > http://www.advancedaquarist.com/issues/mar2003/chem.htm
: >
: > Iodine in Reef Tanks 2: Effects on Macroalgae Growth
: > http://www.advancedaquarist.com/iss...il2003/chem.htm
: >
: >
: > Magnesium and Strontium
: >
: > Strontium
: > http://www.advancedaquarist.com/issues/nov2003/chem.htm
: >
: > Magnesium
: > http://www.advancedaquarist.com/issues/oct2003/chem.htm
: >
: > Magnesium and Strontium in Limewater
: > http://www.advancedaquarist.com/issues/dec2003/chem.htm
: >
: >
: > Limewater (kalkwasser)
: >
: > The Self Purification of Limewater (Kalkwasser)
: > http://www.advancedaquarist.com/issues/may2003/chem.htm
: >
: > The Degradation of Limewater (Kalkwasser) in Air
: > http://reefkeeping.com/issues/2003-...ature/index.htm
: >
: > How to Select a Calcium and Alkalinity Supplementation Scheme
: > http://www.advancedaquarist.com/issues/feb2003/chem.htm
: >
: > Metals in Aquaria
: >
: > Aluminum and aluminum-based phosphate binders
: > http://www.advancedaquarist.com/iss...ly2003/chem.htm
: >
: > Reef Aquaria with Low Soluble Metals
: > http://reefkeeping.com/issues/2003-...ature/index.htm
: >
: > Tap Water in Reef Aquaria
: > http://www.advancedaquarist.com/issues/jan2004/chem.htm
: > First Iron Article: Macroalgae and Dosing Recommendations
: > http://www.advancedaquarist.com/issues/aug2002/chem.htm
: >
: > Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
: > http://www.advancedaquarist.com/issues/oct2002/chem.htm
: >
: >
: > Test Kit Reviews
: >
: > The Seachem Borate Alkalinity Test Kit
: > http://www.advancedaquarist.com/iss...ne2003/chem.htm
: >
: > The Salifert Boron Test Kit
: > http://www.advancedaquarist.com/iss...pt2003/chem.htm
: >
: > Boron and Borate (and pH buffering)
: >
: > Boron in a Reef Tank (and its effect on pH buffering)
: > http://www.advancedaquarist.com/issues/dec2002/chem.htm
: >
: > The Seachem Borate Alkalinity Test Kit
: > http://www.advancedaquarist.com/iss...ne2003/chem.htm
: >
: > The Salifert Boron Test Kit
: > http://www.advancedaquarist.com/iss...pt2003/chem.htm
: >
: >
: >
: > Others
: >
: > Tap Water in Reef Aquaria
: > http://www.advancedaquarist.com/issues/jan2004/chem.htm
: >
: > ORP
: > http://reefkeeping.com/issues/2003-...ature/index.htm
: >
: > Chloramine
: > http://reefkeeping.com/issues/2003-...ature/index.htm
: >
: > Silica in a Reef Tank
: > http://advancedaquarist.com/issues/jan2003/feature.htm
: >
: > Specific Gravity (and temperature correction of hydrometers)
: > http://www.advancedaquarist.com/iss...2/chemistry.htm
: >
: >
: > The Complete Nitrogen Cycle
: > http://www.animalnetwork.com/fish/l...a&RecordNo=3090
: >
: > Magnesium (older article with fonts screwed up)
: > http://www.aquariumfish.com/aquariu...cid=124&search=
: >
: > Phosphate (older article now reproduced in a poor fashion)
: > http://www.aquariumfish.com/aquariu...cid=124&search=
: >
: > Carbon Dioxide
: > http://www.animalnetwork.com/fish/l...a&RecordNo=2074
: >
: > Using Conductivity to Measure Salinity
: > http://www.aquariumfish.com/aquariu...cid=124&search=
: >
: > Understanding Seawater
: > http://www.animalnetwork.com/fish2/...s/1/default.asp
: >
: > Protein Skimming: How It Works
: > http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
: >
: >
: >
: > Articles by Craig Bingman:
: >
: > Carbon Dioxide tests
: > http://www.animalnetwork.com/fish/l...n=&RecordNo=279
: >
: > Limewater, Acetic Acid and Sand Clumping
: > http://www.animalnetwork.com/fish/l...n=&RecordNo=181
: >
: > Calcium and Alkalinity
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > Calculation of Calcium Carbonate Saturation States in Reef Aquaria
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: >
: > Calcification Rates in Several Tropical Coral Reef Aquaria
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > Limits To Limewater...Revisited
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > Expanding the Limits of Limewater: Adding Organic Carbon Sources (vinegar)
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: >
: > Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > Magnesium - Part I
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > Magnesium - Part II
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > A Homemade Magnesium Supplement
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > Simulating the Effect of Calcium Chloride and Sodium Bicarbonate Additions
: on Reef Systems
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > Additional Simulations: The Combined Effect Of Calcium Chloride
: > /Sodium Bicarbonate Additions And Water Exchanges
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: >
: > More articles by Craig Bingman:
: >
: > The Halogens - Part I: Bromine in Seawater and Aquaria
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > The Halogens - Part II: Fluoride
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > Fluoride Depletion In Four Reef Aquariums
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > The Halogens - Part III: Iodine
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > Measuring Halides
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > How Test Kits Work
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > Borax pH Calibration
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > A pH Detective Story
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > How to Mix a Batch of Synthetic Seawater in Under Five Minutes
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: > SILICON - FOE OR FRIEND?
: > http://www.animalnetwork.com/fish2/...s/1/default.asp
: >
: > The Composition Of Several Synthetic Seawater Mixes
: > http://www.animalnetwork.com/fish2/...s/1/default.asp
: >
: > Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
: > http://www.animalnetwork.com/fish2/...bio/default.asp
: >
: >
: >
: > Andy's calcium calculator
: > http://www.andy-hipkiss.co.uk/cacalc.htm
: >
: > Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
: > http://www.aquariumfish.com/aquariu...cid=124&search=
: >
: > Calcium Reactor Substrate -- Phosphate Levels
: > by Greg Hiller
: > http://www.advancedaquarist.com/iss...l2003/short.htm
: >
: >
: > Indoor CO2 Problems
: > http://www.advancedaquarist.com/iss...r2002/short.htm
: >
: > Simon Huntington's CaCO3/CO2 reactor article
: >
: > http://reefkeeping.com/issues/2002-...ature/index.htm
: >
: > Ron Shimek's Tank Water Analysis Article
: > http://reefkeeping.com/issues/2002-...ature/index.htm
: >
: >
: >
: >
: > Home made salinity standards thread:
: >
: > http://reefcentral.com/forums/showt...?threadid=65509
: >
: > Reef Chemicals Calculator
: > http://www.kademani.com/reefchem.htm
: >
: >
: >
: > Boomer
: >
: > Want to talk chemistry ? The Reef Chemistry Forum
: > http://www.reefcentral.com/vbulletin/index.php
: >
: >
: > Former US Army Bomb Technician (EOD)
: > Member; IABTI, NATEODA, WEODF, ISEE & IPS
: >
: > If You See Me Running You Better Catch-Up
: >
: >
: > --
: > Boomer
: >
: > Want to talk chemistry ? The Reef Chemistry Forum
: > http://www.reefcentral.com/vbulletin/index.php
: >
: > Want to See More ?
: > Please Join Our Growing Membership
: > www.coralrealm.com
: >
: > If You See Me Running You Better Catch-Up
: > "stoutman" <.@.> wrote in message
: news:aGuWb.148227$U%5.676753@attbi_s03...
: > : Boomer,
: > :
: > : I am not sure if you are just messing with me or if you are truly
: confused.
: > : I hope the latter. Please read from Top to Bottom.
: > :
: > :
: > : From YOUR first link:
: > :
: > : http://www.waterontheweb.org/resources/glossary.html
: > :
: > : Acidity:
: > : A measure of how acid a solution may be. A solution with a pH of less
: than
: > : 7.0 is considered acidic. Solutions with a pH of less than 4.5 contain
: > : mineral acidity (due to strong inorganic acids), while a solution having
: a
: > : pH greater than 8.3 contains no acidity.
: > :
: > : Yes,
: > :
: > : Good definition (for the most part). pH <7 is indeed acidic. pH > 7 is
: > : basic. Your web page had a definition for acidity, but not basicity.
: > : Strange. That's like defining GOOD and not defining BAD.
: > :
: > : Here is the IUPAC (International Union of Pure and Applied Chemistry)
: > : definition of acidity:
: > :
: > : http://www.chem.qmul.ac.uk/iupac/index.html
: > :
: > : acidity
: > :
: > : (1) Of a compound:
: > :
: > : For Brønsted acids it means the tendency of a compound to act as a
: hydron
: > : donor. It can be quantitatively expressed by the acid dissociation
: constant
: > : of the compound in water or some other specified medium. For Lewis acids
: it
: > : relates to the association constants of Lewis adducts and -adducts.
: > :
: > : (2) Of a medium:
: > :
: > : The use of the term is mainly restricted to a medium containing Brønsted
: > : acids, where it means the tendency of the medium to hydronate a specific
: > : reference base
: > :
: > : basicity
: > :
: > : For Brønsted bases it means the tendency of a compound to act as hydron
: > : (proton) acceptor. The basicity of a chemical species is normally
: expressed
: > : by the acidity of the conjugate acid (see conjugate acid-base pair). For
: > : Lewis bases it relates to the association constants of Lewis adducts
: > : and -adducts
: > :
: > :
: > :
: > : Another definition from the same web page YOU cited: (this is the same
: web
: > : page you cited above)
: > :
: > : Alkalinity:
: > : Acid neutralizing or buffering capacity of water; a measure of the
: ability
: > : of water to resist changes in pH caused by the addition of acids or
: bases
: > : and therefore, the main indicator of susceptibility to acid rain; in
: natural
: > : waters it is due primarily to the presence of bicarbonates, carbonates
: and
: > : to a much lesser extent occasionally borates, silicates and phosphates.
: It
: > : is expressed in units of milligrams per liter (mg/l) of CaCO3 (calcium
: > : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l = 1
: mg/l
: > : of CaCO3. A solution having a pH below about 5 contains no alkalinity.
: > :
: > : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and says
: > : that alkalinity is the measure of ...(description of a buffer)
: > :
: > : A BUFFER IS : a measure of the ability of water to resist changes in pH
: > : caused by the addition of acids or bases (from definition below)
: > :
: > :
: > : I said:
: > : ***alkalinity is a measurement of 'buffering capacity'***
: > :
: > : You said:
: > : ***Alkalinity is not a measurement of BC
: > :
: > : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is not
: > : logical.
: > :
: > : (THIS FROM THE SAME WEB PAGE YOU CITED):
: > :
: > : Buffer:
: > : A substance which tends to keep pH levels fairly constant when acids or
: > : bases are added.
: > :
: > : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
: > :
: > : a measure of the ability of water to resist changes in pH caused by the
: > : addition of acids or bases
: > :
: > : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A BUFFER.
: > :
: > :
: > : I went to all four links. None contradict what I have said. But the
: first
: > : one you cited contradicts YOU!
: > :
: > : I know what a buffer is. I know what acidity means. I know what
: alkalinity
: > : means. No need to cite web pages that describe what I know and what I
: wrote
: > : in this discussion. Show me one that says alkalinity is not a measure
: of
: > : buffering capacity from a credible source.
: > :
: > :
: > :
: > :
: > :
: > :
: > : "Boomer" > wrote in message
: > : ...
: > : > Alkalinity a measure of the amount of anions of weak acid in water and
: of
: > : the cations
: > : > balanced against them
: > : > Take note it says ***acid***
: > : >
: > : > Buffering capacity the ability of a solution to resist or dampen
: changes
: > : in pH upon the
: > : > addition of acids or bases.
: > : > Take note its says ***the addition of acids or bases***
: > : >
: > : > One more
: > : >
: > : > http://www.waterontheweb.org/resources/glossary.html
: > : >
: > : > We could go on like this all day, so what is the point ?
: > : >
: > : > You will LOVE this one
: > : > http://www.kyantec.com/Tips/phbuffering.htm
: > : >
: > : > Don't you just lovbe PDF's
: > : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
: > : >
: > : > Don't fall out of your chair
: > : > http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
: > : >
: > : >
: > : >
: > : >
: > : > --
: > : > Boomer
: > : >
: > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > http://www.reefcentral.com/vbulletin/index.php
: > : >
: > : > Want to See More ?
: > : > Please Join Our Growing Membership
: > : > www.coralrealm.com
: > : >
: > : > If You See Me Running You Better Catch-Up
: > : > "stoutman" <.@.> wrote in message
: news:XB7Wb.19339$QA2.62332@attbi_s52...
: > : > : Man here is another, google is a wonderful thing. I'm not filtering
: any
: > : > : out, just posting what I find by GOOGLING for you.
: > : > :
: > : > : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
: > : > :
: > : > :
: > : > : Wow, a gov link. Even the government is wrong, this must be a
: > : conspiracy
: > : > : against Boomer.
: > : > :
: > : > :
: > : > :
: > : > :
: > : > : "Boomer" > wrote in message
: > : > : ...
: > : > : > Now I am getting bored
: > : > : >
: > : > : > "Don't the components of a buffer account for the buffering
: capacity?
: > : > : Yes."
: > : > : >
: > : > : > Yes, agreed but you seem to fail what I'm saying. Buffering
: Capacity
: > : and
: > : > : Alkalinity are
: > : > : > not the same, that has always been the issue. I gave the equation
: does
: > : > : that look like an
: > : > : > Alkalinity equation or how Alk is determined. I see you had now
: > : comments
: > : > : on it what's
: > : > : > wrong, why no comments on the equations I gave. Don't understand
: them
: > : or
: > : > : what ? Again this
: > : > : > is the equation for Buffering Capacity, also called Buffer Index
: or
: > : Buffer
: > : > : Intensity. It
: > : > : > is defined in most water chemistry and chemical oceanography text
: > : books.
: > : > : >
: > : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] +
: > : CKa
: > : > : [H3O+] / (Ka =
: > : > : > H3O+])² )
: > : > : >
: > : > : > This is not Alkalinity now is it ?
: > : > : >
: > : > : > "I know how to do a titration, In fact I have done several. How
: many
: > : have
: > : > : > you actually done? I don't mean by counting drops, I mean with a
: > : buret?"
: > : > : >
: > : > : > Well good for you, I use a Digital Titrator
: > : > : >
: > : > : > "Oh, I see,
: > : > : > you think acidity is the opposite of alkalinity. In the world of
: > : > : CHEMISTRY
: > : > : > it's not. Maybe in aquarium newsgroups it is.
: > : > : >
: > : > : > Hum no, maybe you should go for a look at HACH's or LaMotte
: website or
: > : the
: > : > : book I
: > : > : > suggested earlier. Please view a copy.
: > : > : >
: > : > : > Standard Methods for the Examination of Water and Wastewater
: > : > : >
: > : > : > This book, over 2000 pages, is the guide for water testing. If you
: are
: > : > : reporting water
: > : > : > test to the EPA you must use approved std from this text.I t is
: > : prepared
: > : > : and published by
: > : > : > the EPA, American Water Works Association and American Public
: Health
: > : > : Association. You
: > : > : > mean you don't have one and the issue is water chemistry
: > : > : >
: > : > : > You are confusing Acidity and Acidity as you know little about
: water
: > : > : chemistry and
: > : > : > procedures and test methods
: > : > : >
: > : > : > From SMEWW, section 2-30, 2310 ACIDITY
: > : > : >
: > : > : > "Acidity of water is its quantative capacity to react with a
: strong
: > : base
: > : > : to a designated
: > : > : > pH"
: > : > : >
: > : > : > This is how you test for it
: > : > : >
: > : > : > A std alkali titration to methyl orange or phenolphthalein
: > : > : > endpoint.
: > : > : >
: > : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that
: write
: > : this
: > : > : book, there are
: > : > : > over 100 of them, they are wrong.
: > : > : >
: > : > : > Like Buffering Capacity you have your Acidity's mixed up
: > : > : > In water measurement if you have a high Alk you also usually have
: a
: > : high
: > : > : Acidity.
: > : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
: > : CHEMISTRY
: > : > : BOOK there pal.
: > : > : >
: > : > : >
: > : > : > "These are all in equilibrium with each other. An initial high pH
: > : (above
: > : > : > 6.4) will shift the equilibrium to the right to form HCO3-1. If
: the
: > : pH of
: > : > : > the solution is above 10.3 (pKa2) the .........."
: > : > : >
: > : > : >
: > : > : > Christ, there you go again with the FW ****. All your numbers are
: > : wrong we
: > : > : are dealing
: > : > : > with SEAWATER
: > : > : >
: > : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is in
: the
: > : form
: > : > : > of HCO3-1 .
: > : > : >
: > : > : > I have already pointed that out and gave actual values at know
: > : seawater
: > : > : levels, go back
: > : > : > and re-read it you aren't telling me anything here.Of course most
: is
: > : HCO3
: > : > : see...
: > : > : >
: > : > : >
: > : > : > @ 20C and 34.3 ppt salinity
: > : > : >
: > : > : > CO2 = 0.52 %
: > : > : >
: > : > : > HCO3 = 86.4 %
: > : > : >
: > : > : > CO3 = 13.09 %
: > : > : >
: > : > : >
: > : > : > "In your glass experiment you managed to lower the pH enough to
: purge
: > : out
: > : > : CO2
: > : > : > by boiling"
: > : > : >
: > : > : > The purpose behind the glass is to show that alk is not affect by
: CO2
: > : and
: > : > : vise-versa and
: > : > : > how Co2 affects pH.
: > : > : >
: > : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and that
: pH
: > : drops
: > : > : to say 8.1 it is
: > : > : > usually due to excess CO2. If you took a glass of that water and
: > : aerated
: > : > : it you WILL drive
: > : > : > off the CO2 and raise the pH. It has been done a proven a million
: > : times.
: > : > : >
: > : > : > "In order to 'purge' CO2 you would need to lower the
: > : > : > pH to shift the equilibrium to below 6.4"
: > : > : >
: > : > : > The hell you do !!!.Do you know who many times people on this NG
: to
: > : > : include Dr. Craig
: > : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned to
: take a
: > : > : sample of aquarium
: > : > : > water and aerate it to see if the pH GOES UP AND when they come
: back
: > : with
: > : > : the test it is
: > : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D CHEMIST
: > : excess
: > : > : CO2 in the tank
: > : > : > water, increase the circulation for better gas exchange at the
: > : surface,
: > : > : reduce feeding,
: > : > : > and try to improve on better skimming, thus reducing the bio-load
: and
: > : pH
: > : > : decline due to
: > : > : > CO2.
: > : > : >
: > : > : >
: > : > : > "I hope this helps. "
: > : > : >
: > : > : > Help, how can you when you miss everything. I should be charging
: you
: > : > : >
: > : > : > Oh, by the way. Your websites, I have about 50 on these issues, I
: > : could
: > : > : post them, not to
: > : > : > mention I have all those water chemistry books, so there is no
: need to
: > : > : view your sites.
: > : > : >
: > : > : > Finally are you afraid to come to our Chemistry Forum, afraid to
: get
: > : > : slapped by REAL
: > : > : > chemists. I get a charge out of you can't post your ref .I have
: posted
: > : the
: > : > : same or similar
: > : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have 1500
: > : posts
: > : > : there and am the
: > : > : > biggest contributor to his forum other than himself or maybe Habib
: > : Sheka
: > : > : >
: > : > : > Hum, here are Randy's ref that he posted. He hosts the website
: > : > : >
: > : > : > S. RANDY HOLMES-FARLEY
: > : > : > Arlington, Massachusetts
: > : > : >
: > : > : > EDUCATION
: > : > : >
: > : > : > 1982-1986 Harvard University Cambridge, MA
: > : > : > PhD in Chemistry
: > : > : > Research Advisor: George Whitesides
: > : > : >
: > : > : > Investigated the relationship between polymer surface chemistry
: and
: > : > : physical properties
: > : > : > through controlled surface modification and testing.
: > : > : >
: > : > : > 1980-1982 Cornell University Ithaca, NY
: > : > : > BA in Chemistry and Biology
: > : > : > Graduated Summa Cum Laude
: > : > : > Distinction in All Subjects
: > : > : > Grade Point: 3.94/4.0
: > : > : > Honors research: isolation and characterization of the subunit of
: CF1
: > : > : enzyme
: > : > : >
: > : > : >
: > : > : > 1978-1979 Stanford University Palo Alto, CA
: > : > : > Grade Point: 3.55/4.0
: > : > : >
: > : > : >
: > : > : > EXPERIENCE
: > : > : >
: > : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham, MA
: > : > : > (bought out GelTex Pharmaceuticals in 2001)
: > : > : > Vice President, Chemical Research 2001-present
: > : > : > Senior Director, Chemical Research 1999-2001
: > : > : > Director of Chemical Research 1997-1999
: > : > : > Manager of Chemical Research 1995-1997
: > : > : > Group Leader 1994-1995
: > : > : > Senior Research Scientist 1992-1994
: > : > : >
: > : > : > Helped start GelTex as second employee
: > : > : >
: > : > : > Managed various research programs with multi-million dollar
: budgets
: > : > : >
: > : > : > Supervised research chemists (17+)
: > : > : >
: > : > : > Co-inventor of several polymeric pharmaceuticals and
: pharmaceutical
: > : > : candidates including
: > : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam
: Hydrochloride
: > : (FDA
: > : > : approved)
: > : > : >
: > : > : > Company Safety Officer for 3 years
: > : > : >
: > : > : > Chemical Hygiene Officer 2000-present
: > : > : >
: > : > : >
: > : > : >
: > : > : >
: > : > : > 1990-1992 GTE Corporation Waltham, MA
: > : > : > Senior Member of Technical Staff
: > : > : > Applied research involving polymer interfaces
: > : > : > Metallization of plastics
: > : > : > Polymer/polymer adhesion
: > : > : > Optical coatings
: > : > : >
: > : > : >
: > : > : >
: > : > : > 1986-1990 Lord Corporation Cary, NC
: > : > : > Senior Research Scientist 1988-1990
: > : > : > Research Scientist 1986-1988
: > : > : > Basic and applied research on surface chemical bonding
: > : > : > Developed new adhesive compositions
: > : > : > Developed new sol-gel coatings for corrosion resistance
: > : > : >
: > : > : >
: > : > : > HONORS AND AWARDS
: > : > : >
: > : > : > Industrial Innovations Award by Northeast Region of American
: Chemical
: > : > : Society (6/2001)
: > : > : >
: > : > : > National Kidney Foundation of Northern California Honoree (5/2001)
: > : > : >
: > : > : > American Chemical Society/Polymer Chemistry Division Industrial
: > : Sponsors
: > : > : > Award (8/2000)
: > : > : >
: > : > : > R&D 100 Award from R&D magazine (1999)
: > : > : >
: > : > : > Sherwin Williams Award in applied polymer science (9/85)
: > : > : >
: > : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985;
: 1985-1986)
: > : > : >
: > : > : > Award for highest GPA in Chemistry Department (6/82)
: > : > : >
: > : > : > Summa Cum Laude Honors in Chemistry (6/82)
: > : > : >
: > : > : > Phi Lamda Epsilon (6/82)
: > : > : >
: > : > : > Phi Beta Kappa (2/82)
: > : > : >
: > : > : > Cornell University Dean's List (1981, 1982)
: > : > : >
: > : > : > Harvard Book Club Award for highest GPA senior year (1978)
: > : > : >
: > : > : > First Place in western NY ACS high school chemistry exam (1977)
: > : > : >
: > : > : > 1978-1979
: > : > : >
: > : > : >
: > : > : > __________________
: > : > : > Randy Holmes-Farley
: > : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef
: Central
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: > : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
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: > : > : > 06/27/2003 02:44 PM
: > : > : >
: > : > : > Randy Holmes-Farley
: > : > : > Chemistry Moderator
: > : > : >
: > : > : > Registered: Apr 2001
: > : > : > Location: Arlington, Massachusetts
: > : > : > Occupation: Chemist (Drug Discovery at Genzyme)
: > : > : > Posts: 15282
: > : > : >
: > : > : >
: > : > : >
: > : > : > Publications
: > : > : >
: > : > : >
: > : > : > ISSUED UNITED STATES PATENTS
: > : > : >
: > : > : >
: > : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen Randall;
: > : > : Mandeville, III; W. Harry.
: > : > : > US 6,566,407; 5/20/2003
: > : > : >
: > : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley, Stephen
: > : Randall;
: > : > : Huval, Chad
: > : > : > Cori.
: > : > : > U.S. 6,517,825; 2/11/2003.
: > : > : >
: > : > : > 3. Method of making phosphate-binding polymers for oral
: > : administration.
: > : > : Holmes-Farley,
: > : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M. U.S.
: > : > : 6,509,013; 1/21/2003.
: > : > : >
: > : > : > 4. Combination therapy for treating hypercholesterolemia using a
: bile
: > : acid
: > : > : sequestrant
: > : > : > polymer
: > : > : > and a cholesterol-lowering agent. Huval, Chad Cori; Holmes-Farley,
: > : Stephen
: > : > : Randall;
: > : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
: > : > : >
: > : > : > 5. Method for treating hypercholesterolemia with polyallylamine
: > : polymers.
: > : > : Holmes-Farley,
: > : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
: > : Goldberg,
: > : > : Dennis I. , US
: > : > : > 6,423,754; 7/23/2002.
: > : > : >
: > : > : > 6. Ionic polymers as anti-infective agents Mandeville, W. Harry,
: III;
: > : > : Neenan, Thomas X..;
: > : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
: > : > : >
: > : > : > 7. Combination therapy for treating hypercholesterolemia and
: > : > : atherosclerosis. Huval, Chad
: > : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal,
: Pradeep
: > : K.
: > : > : U.S. 6,365,186;
: > : > : > 4/2/2002.
: > : > : >
: > : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
: > : Mandeville,
: > : > : W. H., III;
: > : > : > Huval; C.
: > : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US 6,299,868;
: > : > : 10/9/2001.
: > : > : >
: > : > : > 9. Polymers containing guanidinium groups as bile acid
: sequestrants.
: > : Dhal;
: > : > : P. K.; Holmes-
: > : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
: > : > : >
: > : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville,
: W.
: > : H.,
: > : > : III.; US
: > : > : > 6,281,252;
: > : > : > 8/28/2001.
: > : > : >
: > : > : > 11. Combination therapy for treating hypercholestrolemia. Huval;
: C.
: > : C.;
: > : > : Holmes-Farley; S.
: > : > : > R. ;
: > : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
: > : > : >
: > : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides, G.
: M.;
: > : > : Holmes-Farley, S.
: > : > : > R.; US
: > : > : > 6,264,937; 7/24/2001.
: > : > : >
: > : > : > 13. Method for treating hypercholesterolemia with unsubstituted
: > : > : polydiallylamine polymers.
: > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K.
: ; US
: > : > : 6,248,318;
: > : > : > 6/19/2001.
: > : > : >
: > : > : > 14. Process for removing bile salts from a patient and alkylated
: > : > : compositions therefore.
: > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355;
: 5/1/2001.
: > : > : >
: > : > : > 15. Poly(diallylamine)-based bile acid sequestrants.
: Holmes-Farley, S.
: > : R.;
: > : > : Dhal, P. K.;
: > : > : > Petersen,
: > : > : > J. S.; US 6,203,785; 3/20/2001.
: > : > : >
: > : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S. R.;
: > : Huval,
: > : > : C. C.; US
: > : > : > 6,190,649;
: > : > : > 2/20/2001.
: > : > : >
: > : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville,
: W.
: > : H.,
: > : > : III.; US
: > : > : > 6,177,478;
: > : > : > 1/23/2001.
: > : > : >
: > : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
: > : Holmes-Farley,
: > : > : S. R.;
: > : > : > Mandeville, W.
: > : > : > H., III.; US 6,129,910; 10/10/2000.
: > : > : >
: > : > : > 19. Method for treating hypercholesterolemia with unsubstituted
: > : > : polydiallylamine polymers.
: > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P. K.
: ; US
: > : > : 6,083,497;
: > : > : > 7/4/2000.
: > : > : >
: > : > : > 20. Method of making phosphate-binding polymers for oral
: > : administration.
: > : > : Holmes-Farley, S.
: > : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US 6,083,495;
: > : 7/4/2000.
: > : > : >
: > : > : > 21. Process for removing bile salts from a patient and alkylated
: > : > : compositions therefore.
: > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
: > : 5/23/2000.
: > : > : >
: > : > : > 22. Process for removing bile salts from a patient and
: compositions
: > : > : therefor. Mandeville,
: > : > : > W. H.,
: > : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
: > : > : >
: > : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III; W.
: H;
: > : > : Neenan; T. X.; Holmes-
: > : > : > Farley; S. R. US 6,034,129; 3/7/2000.
: > : > : >
: > : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.; Mandeville,
: W.
: > : H.,
: > : > : III.; US
: > : > : > 5,985,938;
: > : > : > 11/16/99.
: > : > : >
: > : > : > 25. Process for removing bile salts from a patient and
: compositions
: > : > : therefor. Mandeville,
: > : > : > W. H.,
: > : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
: > : > : >
: > : > : > 26. Hydrophobic sequestrant for cholesterol depletion. Mandeville,
: W.
: > : H.,
: > : > : III.;
: > : > : > Holmes-Farley;
: > : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
: > : > : >
: > : > : > 27. Hydrophilic nonamine-containing and amine-containing
: copolymers
: > : and
: > : > : their use as bile
: > : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
: > : 5,929,184;
: > : > : 7/27/99.
: > : > : >
: > : > : > 28. Interpenetrating polymer networks for sequestration of bile
: acids.
: > : > : Mandeville, W. H.,
: > : > : > III.;
: > : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US
: 5,925,379;
: > : > : 7/20/99.
: > : > : >
: > : > : > 29. Amine polymer sequestrant and method of cholesterol depletion.
: > : > : Mandeville, W. H.,
: > : > : > III.;
: > : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
: > : > : >
: > : > : > 30. Process for removing bile salts from a patient and
: compositions
: > : > : therefor. Mandeville,
: > : > : > W. H.,
: > : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
: > : > : >
: > : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
: depletion.
: > : > : Mandeville, W. H.,
: > : > : > III.;
: > : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
: > : > : >
: > : > : > 32. Process for removing bile salts from a patient and
: compositions
: > : > : therefor. Mandeville,
: > : > : > W. H.,
: > : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
: > : > : >
: > : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
: > : Mandeville,
: > : > : W. H., III.;
: > : > : > Holmes-
: > : > : > Farley, S. R.; US 5,703,188; 12/30/97.
: > : > : >
: > : > : > 34. Oral administration of iron-binding crosslinked amine
: polymers.
: > : > : Mandeville, W. H.,
: > : > : > III.;
: > : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
: > : > : >
: > : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
: Holmes-Farley,
: > : S.
: > : > : R.; US 5,693,675;
: > : > : > 12/2/97.
: > : > : >
: > : > : > 36. Method for removing bile salts from a patient with alkylated
: > : > : crosslinked amine
: > : > : > polymers,
: > : > : > and preparation of the polymers. Mandeville, W. H., III.;
: > : Holmes-Farley,
: > : > : S. R.; US
: > : > : > 5,679,717; 10/21/97.
: > : > : >
: > : > : > 37. Phosphate-binding polymers for oral administration.
: Holmes-Farley,
: > : S.
: > : > : R.; Mandeville,
: > : > : > W.
: > : > : > H., III.; US 5,667,775; 9/16/97.
: > : > : >
: > : > : > 38. Ion-exchange process using highly crosslinked polymers for
: > : removing
: > : > : bile salts from a
: > : > : > patient, preparation of the polymers, and compositions containing
: > : them.
: > : > : Mandeville, W. H.,
: > : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
: > : > : >
: > : > : > 39. Hydrophobic amine polymer sequestrant and method of
: cholesterol
: > : > : depletion. Mandeville,
: > : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US 5,618,530;
: > : 4/8/97.
: > : > : >
: > : > : > 40. Amine polymer sequestrant and method of cholesterol depletion.
: > : > : Mandeville, W. H.,
: > : > : > III.;
: > : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
: > : > : >
: > : > : > 41. Phosphate-binding polymers for oral administration.
: Holmes-Farley,
: > : S.
: > : > : R.; Mandeville,
: > : > : > W.
: > : > : > H., III.; US 5,496,545; 3/5/96.
: > : > : >
: > : > : > 42. Iron-binding polymers for oral administration. Mandeville, W.
: H.,
: > : > : III.; Holmes-Farley,
: > : > : > S. R.;
: > : > : > US 5,487,888; 1/30/96.
: > : > : >
: > : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having
: active
: > : > : hydrogens on the
: > : > : > surface.
: > : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
: > : > : >
: > : > : > 44. Layered sol-gel coatings from organisilicon compounds.
: > : Holmes-Farley,
: > : > : S. R.; Yanyo, L.
: > : > : > C.;
: > : > : > US 5,182,143; 1/26/93.
: > : > : >
: > : > : > 45. Method for metal bonding using ultrathin primer coating.
: > : > : Holmes-Farley, S. R.; Yanyo,
: > : > : > L.
: > : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
: > : > : >
: > : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.; Abbey, K.
: J.;
: > : US
: > : > : 5,096,962;
: > : > : > 3/17/92.
: > : > : >
: > : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
: > : > : elastomer-metal bonding.
: > : > : > Holmes-
: > : > : > Farley, S. R.; US 5,102,956; 4/7/92.
: > : > : >
: > : > : >
: > : > : >
: > : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT ISSUED)
: > : > : >
: > : > : >
: > : > : > 1. Aryl boronate functionalized polymers for treating obesity and
: > : > : inhibiting fat uptake.
: > : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III; Dhal,
: > : Pradeep
: > : > : K.; Huval, Chad
: > : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl. (2003),
: 92
: > : pp. WO
: > : > : 0302571.
: > : > : >
: > : > : > 2. Preparation of aryl boronic acids for treating obesity.
: > : Holmes-Farley,
: > : > : Stephen Randall;
: > : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal,
: Pradeep
: > : K.
: > : > : (Geltex
: > : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO
: 0302570.
: > : > : >
: > : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide.
: Holmes-Farley,
: > : > : Stephen Randall.
: > : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32 pp.
: WO
: > : > : 0302130.
: > : > : >
: > : > : > 4. Method for reducing copper levels and treating copper
: toxicosis.
: > : > : Holmes-Farley, Stephen
: > : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl.
: (2002),
: > : 45
: > : > : pp. WO
: > : > : > 0285383.
: > : > : >
: > : > : > 5. Method for treating gout and binding uric acid. Holmes-Farley,
: > : Stephen
: > : > : Randall; Burke,
: > : > : > Steven K. WO 0285381 10/31/2002.
: > : > : >
: > : > : > 6. Method for treating gout and reducing serum uric acid.
: > : Holmes-Farley,
: > : > : Stephen Randall;
: > : > : > Burke, Steven K WO 0285380 10/31/2002.
: > : > : >
: > : > : > 7. Amine condensation polymer bile acid sequestrants. Huval, C.
: C.;
: > : > : Holmes-Farley, S. R.;
: > : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
: > : > : >
: > : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H., III
: and
: > : > : Holmes-Farley, S.
: > : > : > R.;
: > : > : > WO 1999-US5662; 9/23/1999.
: > : > : >
: > : > : > 9. Amine-containing copolymers as bile acid sequestrants.
: > : Holmes-Farley,
: > : > : S. R.; Petersen,
: > : > : > J. S.;
: > : > : > WO 9933452; 7/8/1999.
: > : > : >
: > : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W. H.,
: III
: > : and
: > : > : Holmes-Farley, S.
: > : > : > R.;
: > : > : > WO 9922743; 5/14/1999.
: > : > : >
: > : > : > 11. Polyallylamine polymers for removing bile salts and treating
: > : > : hypercholesterolemia, and
: > : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H., III;
: > : Burke,
: > : > : S. K.; Goldberg,
: > : > : > D. I.; WO 9857652; 12/23/98.
: > : > : >
: > : > : > 12. Phosphate-bidning polymers combined with a calcium supplement
: for
: > : oral
: > : > : administration.
: > : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
: Holmes-Farley,
: > : S.
: > : > : R.; WO 9842355;
: > : > : > 10/1/98.
: > : > : >
: > : > : > 13. Hydrophobic heteroatom-containing sequestrant for cholesterol
: > : > : depletion. Mandeville,
: > : > : > W.
: > : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449;
: 12/12/96.
: > : > : >
: > : > : > 14. Process for adjusting ion concentration in a patient and
: > : compositions
: > : > : therefor.
: > : > : > Mandeville,
: > : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
: > : > : >
: > : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
: > : interlayer
: > : > : for improved
: > : > : > metal-
: > : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
: > : 1/20/94.
: > : > : >
: > : > : > 16. Process for increased metal-substrate bond strength in
: metalized
: > : > : plastics.
: > : > : > Holmes-Farley, S.
: > : > : > R.; Ger. Offen. 4322516; 7/6/93.
: > : > : >
: > : > : > 17. Electrorheological fluids and preparation of particles useful
: in
: > : the
: > : > : fluids.
: > : > : > Troughton,
: > : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie; Carlson,
: J.
: > : > : David; Bares, Joseph
: > : > : > E.;
: > : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra Nell.
: EP
: > : > : 394049;
: > : > : > 10/24/1990.
: > : > : >
: > : > : > JOURNAL PUBLICATIONS
: > : > : >
: > : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William; Zhorov,
: > : Eugene;
: > : > : Guo, Amy;
: > : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David L.;
: > : > : Mandeville, W. Harry;
: > : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
: > : 611-619.
: > : > : >
: > : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
: > : synthesis
: > : > : and biological
: > : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley, S.
: > : Randall;
: > : > : Mandeville, W.
: > : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal, Pradeep
: K.
: > : > : Journal of
: > : > : > Macromolecular Science, Pure and Applied Chemistry (2001),
: A38(12),
: > : > : 1559-1574.
: > : > : >
: > : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by
: Molecular
: > : > : Imprinting. Huval,
: > : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.; Holmes-Farley,
: S.
: > : > : Randall; Mandeville,
: > : > : > W.
: > : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro,
: Robert
: > : J.;
: > : > : Chen, Xi; Dhal,
: > : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
: > : > : >
: > : > : > 4. Synthetic polymers for the binding of fat in the intestinal
: tract.
: > : > : Jozefiak, Thomas H.;
: > : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny, Cynthia;
: > : Huval,
: > : > : Chad C.;
: > : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney, Cynthia.
: > : > : Abstracts of
: > : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United States,
: August
: > : > : 26-30, 2001
: > : > : > (2001), POLY-047 and Polymer Preprints (American Chemical Society,
: > : > : Division of
: > : > : > Polymer Chemistry) (2001), 42(2), 98.
: > : > : >
: > : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel
: polymer
: > : gel
: > : > : pharmaceutical.
: > : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.; Petersen,
: J.;
: > : Ward,
: > : > : J.; Sacchiero,
: > : > : > B.;
: > : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton, K.
: A.;
: > : Chen,
: > : > : X.; Mazzeo, J.
: > : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
: > : > : >
: > : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl and
: > : other
: > : > : bile acid
: > : > : > sequestrants.
: > : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.; Xu,
: Q.;
: > : > : Hook, P.; Holmes-
: > : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1),
: 708-709.
: > : > : >
: > : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
: > : Holmes-Farley,
: > : > : S. R; Polym.
: > : > : > Mater. Sci. Eng (1999), 80, 246-247.
: > : > : >
: > : > : > 8. Design and characterization of of Sevelamer Hydrochloride: a
: novel
: > : > : phosphate-binding
: > : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III;
: Ward,
: > : J.;
: > : > : Miller, K. L.;
: > : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M. S.-
: Pure
: > : and
: > : > : Appl. Chem.,
: > : > : > A36(7&8), p. 1085 (1999).
: > : > : >
: > : > : > 9. Three generations of bile acid sequestrants. Mandeville, W. H.,
: > : III;
: > : > : Braunlin, W.;
: > : > : > Dhal, P.;
: > : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik, S.;
: > : > : Rosenbaum, D.;
: > : > : > Sacchiero,
: > : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc.
: (1999),
: > : > : 550, 3-15.
: > : > : >
: > : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked, polymeric
: > : phosphate
: > : > : binder, on
: > : > : > urinary
: > : > : > phosphorous excretion in rats. Rosenbaum, D. P.; Holmes-Farley, S.
: R.;
: > : > : Mandeville, W. H.,
: > : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
: Transplant.
: > : > : (1997), 12(5)
: > : > : > 961-964.
: > : > : >
: > : > : > 11. Thin anisotropic coatings based on sol-gel technology.
: > : Holmes-Farley,
: > : > : S. R.; Yanyo, L.
: > : > : > C;
: > : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem. 4),
: > : 439-444.
: > : > : >
: > : > : > 12. The mechanism of cure initiation of a surface activated
: adhesive.
: > : > : Holmes-Farley, S.
: > : > : > R.;
: > : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5), 409-420.
: > : > : >
: > : > : > 13. Adhesion promotion and corrosion prevention using thin
: anisotropic
: > : > : coatings. Holmes-
: > : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991), 5(2),
: > : > : 131-151.
: > : > : >
: > : > : > 14. Wetting of functionalized polyethylene having ionizable
: organic
: > : acids
: > : > : and bases at the
: > : > : > polymer-water interface: relations between functional group
: polarity,
: > : > : extent of
: > : > : > ionization,
: > : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C. D.;
: > : > : Whitesides, G. M.;
: > : > : > Langmuir
: > : > : > (1988), 4(4), 921-937.
: > : > : >
: > : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols with
: a
: > : > : single hydroxy group.
: > : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
: > : > : >
: > : > : > 16. Reconstruction of the interface of oxidatively functionalized
: > : > : polyethylene (PE-CO2H)
: > : > : > and
: > : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.;
: Nuzzo,
: > : R.;
: > : > : McCarthy, T. J.;
: > : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also Report
: > : (1987),
: > : > : AD-
: > : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
: > : > : >
: > : > : > 17. Surface-modified polyethylene film: the relationship between
: > : surface
: > : > : chemistry and
: > : > : > physical
: > : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987, 47(11),
: > : 4537.
: > : > : >
: > : > : > 18. Reactivity of carboxylic acid and ester groups in the
: > : functionalized
: > : > : interfacial
: > : > : > region of
: > : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
: > : > : differentiation of the
: > : > : > functional groups into shallow and deep subsets based on a
: comparison
: > : of
: > : > : contact angle and
: > : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.;
: Langmuir
: > : > : (1987), 3(1), 62-
: > : > : > 76.
: > : > : >
: > : > : > 19. Fluorescence properties of dansyl groups covalently bonded tot
: he
: > : > : surface of
: > : > : > oxidatively
: > : > : > functionalized low-density polyethylene film. Holmes-Farley, S.
: R.;
: > : > : Whitesides, G. M.;
: > : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985), TR-85-2;
: > : > : AD-A162435/2/GAR,
: > : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
: > : > : >
: > : > : > 20. Acid-base behavior of carboxylic acid groups covalently
: attached
: > : at
: > : > : the surface of
: > : > : > polyethylene: The usefulness of contact angle in following the
: > : ionization
: > : > : of surface
: > : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy, T.
: J.;
: > : > : Deutch, J.;
: > : > : > Whitesides,
: > : > : > G. M.; Langmuir (1985), 1(6), 725-740.
: > : > : >
: > : > : > 21. The thermal stability of a surface modified solid organic
: polymer.
: > : > : Holmes-Farley, S.
: > : > : > R.;
: > : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53, 127-131.
: > : > : >
: > : > : >
: > : > : >
: > : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
: > : > : >
: > : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R.
: Advanced
: > : > : Aquarist. June 2003.
: > : > : >
: > : > : > 2. The Self Purification of Limewater (Kalkwasser). Holmes-Farley,
: R.
: > : > : Advanced Aquarist.
: > : > : > May
: > : > : > 2003.
: > : > : >
: > : > : > 3. The Degradation of Limewater (Kalkwasser) in Air.
: Holmes-Farley, R.
: > : > : Reefkeeping May
: > : > : > 2003.
: > : > : >
: > : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
: Reefkeeping
: > : > : April 2003.
: > : > : >
: > : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
: > : > : Holmes-Farley, R.
: > : > : > Advanced Aquarist; April 2003.
: > : > : >
: > : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae Growth.
: > : > : Holmes-Farley, R.
: > : > : > Advanced Aquarist; April 2003.
: > : > : >
: > : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R. Advanced
: > : Aquarist;
: > : > : March 2003.
: > : > : >
: > : > : > 8. How to Select a Calcium and Alkalinity Supplementation Scheme.
: > : > : Holmes-Farley, R.
: > : > : > Advanced Aquarist; February 2003.
: > : > : >
: > : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
: January
: > : > : 2003.
: > : > : >
: > : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
: > : December
: > : > : 2002.
: > : > : >
: > : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
: > : Advanced
: > : > : Aquarist; November
: > : > : > 2002.
: > : > : >
: > : > : > 12. Iron: A Look at Organisms Other than Macroalgae.
: Holmes-Farley, R.
: > : > : Advanced Aquarist;
: > : > : > November 2002.
: > : > : >
: > : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.; Advanced
: > : Aquarist,
: > : > : September 2002.
: > : > : >
: > : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist,
: August
: > : > : 2002.
: > : > : >
: > : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.; Reefkeeping.com,
: April
: > : > : 2002.
: > : > : >
: > : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R. Advanced
: > : > : Aquarist; July 2002
: > : > : >
: > : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced Aquarist;
: > : June
: > : > : 2002.
: > : > : >
: > : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley, R.
: > : Advanced
: > : > : Aquarist, May
: > : > : > 2002.
: > : > : >
: > : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in
: Corals.
: > : > : Holmes-Farley, R.
: > : > : > Advanced Aquarist, April 2002.
: > : > : >
: > : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
: > : > : >
: > : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February
: 2002.
: > : > : >
: > : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist, January
: > : 2002.
: > : > : >
: > : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium
: Frontiers
: > : > : 2000.
: > : > : >
: > : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R. Aquarium
: > : > : Frontiers 2000.
: > : > : >
: > : > : > 25. Phosphate..What is it and why should you care. Holmes-Farley,
: R.
: > : > : Aquarium Frontiers
: > : > : > 2000.
: > : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
: > : Frontiers
: > : > : 2000.
: > : > : >
: > : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium Frontiers
: > : 2000.
: > : > : >
: > : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium Frontiers
: 1999.
: > : > : >
: > : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
: > : > : >
: > : > : >
: > : > : >
: > : > : >
: > : > : >
: > : > : >
: > : > : >
: > : > : > Boomer
: > : > : >
: > : > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > : > http://www.reefcentral.com/vbulletin/index.php
: > : > : >
: > : > : > Want to See More ?
: > : > : > Please Join Our Growing Membership
: > : > : > www.coralrealm.com
: > : > : >
: > : > : >
: > : > : >
: > : > :
: > : > :
: > : >
: > : >
: > :
: > :
: > :
: >
: >
:
:

[stoutman]

Boomer,

I think this discussion has shifted from SCIENCE to SEMANTICS.

I say: Alkalinity is a measurement of Buffering capacity.....
you say: Alkalinity is an indication of Buffering capacity.....

Have a good weekend Boomer.

-Stoutman






"Boomer" > wrote in message
...
> Yes, of cause I remember, as I said I posted it for a reason. I see you
have used only
> that link for your definition, as it makes you look right.You have avoided
all Alk
> definitions in a chemistry book, to include your own definition *****to
resist a drop in
> pH due to the addition of acid***, which is the same as the others I
posted .Agreed, of
> course not.You know that Alk isn't defined as "by the addition of acids or
bases "and is
> only the " addition of an acid", so why are you accepting the definition
?.You know that
> when you titrate it is an acid added and never a base. In one breath it
says Alk is "Acid
> neutralizing " and then they say "by the addition of acids or bases ".You
can't have it
> both ways and YOU know that Agreed . If the word "base" was left out I
would not have much
> to say. Agreed
>
>
> "Alkalinity is a
> measurement of BUFFERING CAPACITY."
>
> No it is not a measurement of BUFFERING CAPACITY, it is a indication of
BC. I have said
> this at least twice. If you know your BC you can calculate Alk and if you
can do one you
> can do the other agreed. What I have tried to convey from the beginning is
that Alk and BC
> are not the same thing. You in one of your other posts have said they are
not the same
> thing and never said they were. Now you seem to be saying they are the
same thing
>
> "So, when we measure ALKALINITY (and we know the pH) we are in effect
> measuring BUFFERING CAPACITY.
>
> More or less YES in an "effect" but Alk tells you not much of anything
when a base is
> added Agreed. That is called Acidity, which I see you have avoided again
as if there is
> no such thing. I also said that for us the only thing we need to be
concerned about is
> Alk, so BC would fit in, as we could care less about the ability to
neutralize a base or
> measure Acidity. So, if you knew your pH , Alk or Acy you would really
know what you BC is
> doing for you Agreed.
>
> On Bc, we have both left something from my first equation, so I thought I
would post it
> again for you, as I like being honest .I'm surprised you didn't catch it
:-)
>
> B = dCb / dpH = - dCa / dpH
>
> So;
>
> B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> or
>
> B (Buffering Capacity) = - dCa / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> There are number of was to mathematically express BC. Two of the most
common are the
> change in Alk with the pH at constant total carbonate, the other is change
in Alk with pH
> constant CO2 pp. In some examples of Bc, Bc is the inverse slope of the
Alk titration
> curve ( I'm sure yo
> u will love this) In the other over the pH range, while BC is going
through minimum, Bpp
> increases linearly. This difference is caused by the uptake of CO2 by the
solution, which
> increases Ct as pH increases.To bad we can't or my server won't allow me,
to post
> attachments. I have a nice BC cure of various species as a function of
pC/pH diagrams, set
> to a pKa. curve
>
>
> On another issue
>
> "In order to remove CO2 (g) you ideally would want to shift
> the equilibrium to the left by LOWERING the pH"
>
>
> You may want to try and re-explain this
>
> CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
> HCO3-1 <-------> CO3-2
>
>
> As the reaction shifts to left the pH gets higher as CO2 leaves the
system.You don't have
> to lower the pH to remove CO2. Case in point plants. As they remove CO2
the pH rises,
> continued removal of the Sigma CO2 ( CO2, H2CO3, HCO3,CO3) cause further
rising until
> there is mostly only carbonate (CO3) left and a high pH. Another case, at
a pH of 8.00 and
> Alk of 4 meq / l ( 1.4 mg / l CO2) you have much more CO2 than at 2 meq/
l (0.65mg / l).
> . Aeration of the water can drive off the CO, no lowering of the pH
required., the removal
> will cause the pH to rise .On the other hand, trying to remove CO2 @ 2 meq
/ l won't get
> you much of anywhere in this case. Also, even a low pH doesn't mean you
can drive of CO2.
> If the seawater pH was say 7.5, you would think not problem to drive off
CO2. If the Alk
> was 0.25 there would be about .35 mg / l CO2 to blow off. At the alk of
4.00 meq / l the
> CO2 is 5 mg / l.Usually, when people have a lower pH, say 7.9 or so, it is
do to CO2, so
> the pH has lowered, increasing the CO2, to allow one to blow it off easier
and bring the
> pH back up.
>
> CO2 = [CA(Carbonate Alk) x aH ] / [pK1(1 + 2pK2 /aH)]
>
> I think we just got off on the wrong foot, hope things look better.
>
> I'll be gone for the weekend, leaving in an hour, so have a nice weekend
:-)
>
>
>
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message news:lcRWb.299984$na.451117@attbi_s04...
> : > Humm, since when does Alk have anything to do in regards to the
addition
> : of BASE.
> :
> : You tell me. Your the one that posted a link to a web page that had
this
> : definition of alkalinity. Looks like you put yourself in your own hole
pal.
> :
> : Remember posting this link:
> :
> : http://www.waterontheweb.org/resources/glossary.html
> :
> : Here is the definition of alkalinity from the web page YOU cited. (I
> : recommend you read the web pages you are citing before you cite them)
> : Alkalinity:
> : Acid neutralizing or buffering capacity of water; a measure of the
ability
> : of water to resist changes in pH caused by the addition of acids or
BASES.
> :
> :
> : > It sure is funny how all of the chemist that write water chemistry
> : textbooks never say Alk
> : > is the Buffering Capacity of a solution.
> :
> : Neither did I. I said (for the umpth teen time) Alkalinity is a
> : measurement of BUFFERING CAPACITY.
> :
> : When you measure alkalinity you know your BUFFERING CAPACITY (if you
know
> : your pH). Its a two for one.
> :
> : SEE MY OTHER POST FROM TODAY.
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : >
> : > "I am not sure if you are just messing with me "
> : >
> : > Yes, messing with you, it is called trolling a troll, to see where the
> : hell you would go
> : > and what you would say in regards to last posts. It is called honesty,
of
> : which you have
> : > none off to say the least,that I can see.You always like to post what
> : suits you and just
> : > avoid ref I give. So lets start where you are WRONG and have a great
lack
> : of understanding
> : > of things, to include pointing out all your gross error which you
still
> : FAIL to
> : > acknowledge and which can be prove in many water chem. ref. .I doubt
like
> : hell you are a
> : > chemist at all.You seem to want to con people into thinkin' you are.
But
> : then again, I
> : > have seen chemists like you before, they are not familiar with the,
but
> : they ASK to have
> : > it explained and ask for REF.YOU just shoot from the hip. WHAT GETS
YOU IN
> : TROUBLE. You
> : > remind me of snoot-noise kid that come here and other NG's and
> : forums...that think they
> : > know, buy hey, maybe I'm wrong :-)
> : >
> : >
> : >
> : > 1). Acidity
> : >
> : > "***Benjamin,Water Chemistry (2002, pages 262-263).***
> : >
> : > ***Acidity A concept that is exactly analogous to alkalinity but
measures
> : the base
> : > neutralizing
> : > capacity (BNC) of a solution is Acidity. The quantitative represents
the
> : concentration of
> : > OH- ions that must be added to titrate the solution to a pH near
10.5***
> : >
> : > So that means that not only in Benjamin wrong but, so are Stumm &
Morgan,
> : Millero, Pilosn,
> : > Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I
> : said, you have your
> : > acidity and Acidy mixed up. Acidity as defined above is covered in
most
> : water chemistry
> : > books, written by chemists, who's field of expertise is water
chemistry.
> : You can even buy
> : > Acidity test kits from, HACH, LaMotte, etc..
> : >
> : > You mean you didn't read this or are you just avoiding it .The same
> : definition can be
> : > found in almost any std water chemistry book.
> : >
> : > I have run into few chemists, that are NOT familiar with the above.
Some
> : water reports
> : > require the above Acidity measuring. The issue with you is you do not
> : understand WATER
> : > CHEMISTRY. Everything you have posted can be found a general chemistry
> : book
> : >
> : >
> : >
> : >
> : > 2) Alk and BC
> : >
> : > From the link
> : >
> : > Alkalinity
> : > ***Acid neutralizing or buffering capacity of water; a measure of the
> : ability of water to
> : > resist changes in pH caused by the addition of acids or bases ***
> : >
> : > This is a Buffering Capacity definition not Alk
> : >
> : > Humm, since when does Alk have anything to do in regards to the
addition
> : of BASE. As I
> : > pointed out in the first post the term is often miss used. Even in
YOUR
> : own posts you say
> : > it is based on a acid addition, no mention of **base or acid**
addition
> : by you. Are you
> : > getting confused or what. Or is more you are trying to confuse
everyone
> : you are right. The
> : > above is a definition for Buffer Capacity NOT Alk
> : >
> : > From Drew, Geochemistry of Natural Waters
> : >
> : > "alkalinity, which is formally defined as the equivalent sum of bases
that
> : are titratable
> : > with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH
of
> : the solution is
> : > progressively lowered by the addition of a strong acid (HCL), all the
> : anions on the right
> : > will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4,
H2S,organic
> : acids, H20)"
> : >
> : > This follows almost all description of Alk, that it is acid
neutralizing
> : reaction and has
> : > nothing to do with base neutralizing, which is Acidity (BNC) .I
defined
> : these before you
> : > had no comment
> : >
> : >
> : > Even the links that give the Buffering Capacity definition is wrong,
as is
> : the UIPAC on
> : > Alkalinity. Alkalinity has nothing to do with the addition of bases
only
> : acids. When you
> : > use the words "base and acid" it becomes BC
> : >
> : > Even YOU MUST disagree with these definitions, from YOUR own post
> : >
> : > Think of alkalinity as 'buffering capacity'. Or the ability of a
solution
> : > ***to resist a drop in pH due to the addition of acid***
> : >
> : > Where the flip is the base addition forget it ?
> : >
> : > From Butler; Carbon Dioxide Equilibrium and Their Applications
(professor
> : emeritus
> : > Harvard University) an expert on the subject.
> : >
> : > Buffering Index (Buffering Capacity, Buffer Intensity).
> : >
> : > ***This concept was first developed for mixtures of approximately
equal
> : proportions of
> : > conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such
> : buffer solutions
> : > strongly resist changes in pH when acids or bases are added and are
useful
> : as pH
> : > standards. The Buffer Index tells how great the resistance to pH
changes
> : will be.**
> : >
> : > also from Butler
> : >
> : > Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
> : >
> : > Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
> : >
> : > Acidity is in fact just the negative of Alkalinity ***
> : >
> : > http://www.lagoonsonline.com/acid.htm
> : >
> : >
> :
http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.h
> : tm?E+mystore
> : >
> : > It sure is funny how all of the chemist that write water chemistry
> : textbooks never say Alk
> : > is the Buffering Capacity of a solution. They are always treated and
> : defined separately.
> : >
> : > If you or others choose to treat Alk and BC as the same, well, just
have
> : at it. As I said
> : > in first post I know what you mean.
> : >
> : > "No need to cite web pages that describe what I know and what I wrote
> : > in this discussion"
> : >
> : > No you don't know, who are you trying to convince any way, me, the
guys
> : here and/or all
> : > the water chemists in this world. As I said before go get a dam WATER
> : CHEMISTRY book or
> : > shut the hell up.You keep trying to define things from a general
chemistry
> : book WE ARE IN
> : > THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
> : >
> : >
> : >
> : >
> : >
> : > 3). pKa's and what you don't know or seem to be confused on
> : >
> : > "Therefore, it has two pKa's
> : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
> : The
> : > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated
is
> : > right in there. Is that magic? :)"
> : >
> : > Here it is agin that is twice at least
> : >
> : > "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this
> : example)
> : > you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium
will
> : > be shifted to HCO3-2 by a ratio of 1:100.
> : >
> : > Oh wait , there is a third time LOL
> : >
> : > "At the pH of seawater, the buffering capacity of carbonate is at it's
> : > weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
> : >
> : >
> : > Lets just dunk you on this one. I am taking note you refuse to reply
to
> : YOUR errors
> : >
> : > So you calculated the pH of seawater with freshwater pKa's, now that
is a
> : good trick. From
> : > a number of seawater chemistry books the seawater pKa's are 6 & 9.1,
so
> : according to you,
> : > seemingly not understanding your favorite Henderson-Hasselbach equatio
n;
> : >
> : > 2 pH = (6 + 9.1) /2 pH = 7.55
> : >
> : > I have never seen seawater with a pH of 7.55. There is no ocean with
that
> : pH. Humm how
> : > come your equation is not working for you today.?
> : >
> : >
> : > "That pH I calculated is
> : > right in there. Is that magic? :)"
> : >
> : > I roll on the floor when I see this = 8.35
> : >
> : > Hum , just a brain far so excuse me for thinkin
> : >
> : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
> : >
> : > Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a
pH of
> : 8.35 there pal
> : > ? That 8.35 is what you are telling people the pH should be, but their
> : meter says 6.4.
> : > This how people will READ this.
> : >
> : >
> : >
> : >
> : > 4.) More on Buffering Capacity
> : >
> : > "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes,
your
> : > alkalinity equation."'
> : >
> : >
> : > Yup, I see that and in this case the HCO3 is the acid and the CO3 is
the
> : base CORRECT. In
> : > Alk you are only dealing with bases and how they react to an acid.
Acidity
> : deals acids and
> : > how they recact to bases "Acidity, A concept that is exactly analogous
to
> : alkalinity but
> : > measures the base neutralizing
> : > capacity (BNC) of a solution is Acidity "Alk is the ANC Acid
neutralizing
> : capacity
> : >
> : > "Don't the components of a buffer account for the buffering capacity?
"
> : >
> : > Yes, they do but so do the acids which work as buffers. NaHCO3 is a
buffer
> : and can act as
> : > an acid or base
> : >
> : > *** Buffering Capacity.**
> : > The power of a substance in solution to absorb acid or alkali without
> : change in pH; this
> : > is highest at a pH value equal to the pKa value of the acid of the
buffer
> : pair.***
> : >
> : > ***Akalinity***
> : > Measure of the power of a solution to neutralise hydrogen ions (H+),
> : usually expressed as
> : > the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
> : >
> : >
> : > If one wants to call Alk Buffering capacity then one sure as a hell
can
> : call Acidty
> : > Buffering Capacity also. As it is the ability to neutralizes an acid
that
> : is a buffer.You
> : > have a pH of 7 and you add a buffer to lower it to a pH of 4, you are
> : buffering the water,
> : > that buffer is a acid.
> : >
> : > 5) CO2
> : >
> : > You are really confuse so it seems :-) You realllllllly indicate that
CO2
> : is affected by
> : > the Alk or vise-versa
> : >
> : > "Yes, the pH will drop with the addition of CO2. Remove CO2 will
cause
> : the
> : > pH to rise? How do you remove CO2? Once it is in solution it forms
> : > carbonic acid and neutralizes some of your 'buffer'."
> : >
> : > "With the exception of CO2?"
> : >
> : > No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
> : > Concepts)....PERIOD.You seem to think a that at least in two of your
post
> : that CO2 is
> : > affected by the Alk or vise-versa. Please go back to school or seek
> : professor
> : >
> : > "Why in one case does CO2 from air lower pH and in the other case it
> : raises
> : > it? Doesn't make sense."
> : >
> : > That is because you don't understand CO2 period. By the way I saved
this,
> : wanted to see
> : > if you would bite on the post I gave. Not bite at first, so time to
reel
> : you in, as you
> : > did bite in another post..
> : >
> : > Lets make some sense of it for you, being that you have a pH.D in
> : chemistry, so you say .
> : >
> : > CO2 is naturally generated in a aquatic systems, it is capable of
raise to
> : various levels
> : > depending on a number of circumstances .It can be measure (except in
> : seawater) or
> : > calculated using Buch/Park Equations (what we use for seawater. In
sort if
> : you know the pH
> : > and Alk you can calculate the CO2). If you aerate a system or a sample
of
> : water, even if
> : > the pH has only dropped a couple of tenths, due to an increase in CO2,
the
> : CO2 will leave
> : > solution to the atmosphere.This will raise the pH. On the other hand
if
> : theCO2 level is
> : > more of the norm and you have hikgh room air, such as in the winter,
the
> : partial pressure
> : > of the CO2 in air will be much higher than that in water, in which
case
> : the CO2 will enter
> : > the water and lower the pH. That is without an airstone. Adding an
> : airstone will make it
> : > even worse,as you are now forcefully driving the CO2 into solution
even
> : quicker. These
> : > test /experiments have been proven many times, it is not that may work
> : could work they do
> : > work.Yet you want to disagree and in another post say you haven't
tried
> : it,.Seems to me
> : > that based on what you say it can't work So, in short you don't know
what
> : the hell you are
> : > taking about. Go get a glass of seawater with a pH of about 8.3 and
lower
> : it to about
> : > 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK-
UP
> : ( that is if you
> : > don't have a high room air CO2 problem.). This little test has been
done
> : thousands of
> : > times in this hobby, with test kits, pH meters and even graphic
printers.
> : >
> : > "This is where Boomer and I
> : > disagree. I say you would have to lower the pH very low in order to
> : > effectively remove CO2 by purging."
> : >
> : > You are 100 % wrong. Please come to our Chem forum and try and run
that by
> : Randy, don't
> : > take my word on it. I already know what he will say.
> : >
> : > "Boomer didnt convince me it
> : > works at the pH of an aquarium, but I never tried it and I'm not sure
of
> : > this. "
> : >
> : > Well then come too our chem. forum and tell Randy he doesn't know what
he
> : is talking about
> : > LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it
> : should be easy for
> : > you to run the experiment LOL There are grade school kids that run the
> : test and know what
> : > happens and that I'm correct.
> : >
> : >
> : > "The equilibrium is a FUNCTION
> : > of pH."
> : >
> : > It is also a function of Alk or don't you know that. At a pH of 8.3,
Alk
> : 2.25, the CO2 is
> : > about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk
to
> : about .4 meq/ l
> : > or so the CO2 will be around .99 mg / l CO2, When dealing with
tanksCO2 is
> : not always in
> : > equilibrium with ambient air.
> : >
> : >
> : > ". But I wouldn't degas a solution of a
> : > specific gas (CO2) with a gas (this case he was using air) that
contains
> : the
> : > same gas I am trying to purge."
> : >
> : > Why not ? We have a guy right now that is running tests on purging
ambient
> : air with a
> : > solution to remove CO2 gas from the air, before it enters the tank
> : per/Randy's suggestion.
> : > The same guy is doing some of my test using a Clinoptilolite, a
Zeolite
> : mineral, that has
> : > an affinity for CO2.This will be a dry CO2 scrubber
> : >
> : >
> : > Sorry Soutman but you sure as hell don't seem to know much about
aquatic
> : chemistry. You
> : > seem to be guessing at everything.
> : >
> : > By the way have you read any of Randy's technical articles on water
> : chemistry, been saving
> : > these for last. There are a few on pH, Alk, CO2 .Here is a list
> : >
> : > Try and answer them 1-5 and lets see where we get THIS TIME :-) or
maybe
> : we should just
> : > drop it. I could care less at this point.
> : >
> : > THE END
> : >
> : >
> : > ARTICLES
> : >
> : > The first two posts in this thread are lists of some of my articles
that
> : relate to reef
> : > tank chemistry. In the next few posts are some of the articles
published
> : by Craig Bingman
> : > and others on reef chemistry issues.
> : >
> : > The first two posts in this thread are lists of some of my articles
that
> : relate to reef
> : > tank chemistry. In the next few posts are some of the articles
published
> : by Craig Bingman
> : > and others on reef chemistry issues.
> : >
> : > Solving Common Problems
> : >
> : > Solving Calcium and Alkalinity Problems
> : > http://www.advancedaquarist.com/issues/nov2002/chem.htm
> : >
> : > Solutions to pH Problems
> : > http://www.advancedaquarist.com/iss...ne2002/chem.htm
> : >
> : > How to Select a Calcium and Alkalinity Supplementation Scheme
> : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
> : >
> : > Phosphate Issues
> : > http://www.advancedaquarist.com/iss...pt2002/chem.htm
> : >
> : > Nitrate Issues
> : > http://www.advancedaquarist.com/iss...st2003/chem.htm
> : >
> : >
> : >
> : > Calcium and Alkalinity
> : >
> : > Solving Calcium and Alkalinity Problems
> : > http://www.advancedaquarist.com/issues/nov2002/chem.htm
> : >
> : > How to Select a Calcium and Alkalinity Supplementation Scheme
> : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
> : >
> : > Calcium and Alkalinity Balance Issues
> : > http://reefkeeping.com/issues/2002-...ature/index.htm
> : >
> : > Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
> : > http://www.advancedaquarist.com/iss...ly2002/chem.htm
> : >
> : > The Relationship Between Alkalinity and pH.
> : > http://www.advancedaquarist.com/issues/may2002/chem.htm
> : >
> : > The Chemical & Biochemical Mechanisms of Calcification in Corals
> : > http://www.advancedaquarist.com/issues/apr2002/chem.htm
> : >
> : > Calcium
> : > http://www.advancedaquarist.com/issues/mar2002/chem.htm
> : >
> : > Alkalinity
> : > http://www.advancedaquarist.com/iss...2/chemistry.htm
> : >
> : >
> : > Iron
> : >
> : > First Iron Article: Macroalgae and Dosing Recommendations
> : > http://www.advancedaquarist.com/issues/aug2002/chem.htm
> : >
> : > Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> : > http://www.advancedaquarist.com/issues/oct2002/chem.htm
> : >
> : > Iodine
> : >
> : > Iodine in Marine Aquaria: Part I
> : > http://www.advancedaquarist.com/issues/mar2003/chem.htm
> : >
> : > Iodine in Reef Tanks 2: Effects on Macroalgae Growth
> : > http://www.advancedaquarist.com/iss...il2003/chem.htm
> : >
> : >
> : > Magnesium and Strontium
> : >
> : > Strontium
> : > http://www.advancedaquarist.com/issues/nov2003/chem.htm
> : >
> : > Magnesium
> : > http://www.advancedaquarist.com/issues/oct2003/chem.htm
> : >
> : > Magnesium and Strontium in Limewater
> : > http://www.advancedaquarist.com/issues/dec2003/chem.htm
> : >
> : >
> : > Limewater (kalkwasser)
> : >
> : > The Self Purification of Limewater (Kalkwasser)
> : > http://www.advancedaquarist.com/issues/may2003/chem.htm
> : >
> : > The Degradation of Limewater (Kalkwasser) in Air
> : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : >
> : > How to Select a Calcium and Alkalinity Supplementation Scheme
> : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
> : >
> : > Metals in Aquaria
> : >
> : > Aluminum and aluminum-based phosphate binders
> : > http://www.advancedaquarist.com/iss...ly2003/chem.htm
> : >
> : > Reef Aquaria with Low Soluble Metals
> : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : >
> : > Tap Water in Reef Aquaria
> : > http://www.advancedaquarist.com/issues/jan2004/chem.htm
> : > First Iron Article: Macroalgae and Dosing Recommendations
> : > http://www.advancedaquarist.com/issues/aug2002/chem.htm
> : >
> : > Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> : > http://www.advancedaquarist.com/issues/oct2002/chem.htm
> : >
> : >
> : > Test Kit Reviews
> : >
> : > The Seachem Borate Alkalinity Test Kit
> : > http://www.advancedaquarist.com/iss...ne2003/chem.htm
> : >
> : > The Salifert Boron Test Kit
> : > http://www.advancedaquarist.com/iss...pt2003/chem.htm
> : >
> : > Boron and Borate (and pH buffering)
> : >
> : > Boron in a Reef Tank (and its effect on pH buffering)
> : > http://www.advancedaquarist.com/issues/dec2002/chem.htm
> : >
> : > The Seachem Borate Alkalinity Test Kit
> : > http://www.advancedaquarist.com/iss...ne2003/chem.htm
> : >
> : > The Salifert Boron Test Kit
> : > http://www.advancedaquarist.com/iss...pt2003/chem.htm
> : >
> : >
> : >
> : > Others
> : >
> : > Tap Water in Reef Aquaria
> : > http://www.advancedaquarist.com/issues/jan2004/chem.htm
> : >
> : > ORP
> : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : >
> : > Chloramine
> : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : >
> : > Silica in a Reef Tank
> : > http://advancedaquarist.com/issues/jan2003/feature.htm
> : >
> : > Specific Gravity (and temperature correction of hydrometers)
> : > http://www.advancedaquarist.com/iss...2/chemistry.htm
> : >
> : >
> : > The Complete Nitrogen Cycle
> : > http://www.animalnetwork.com/fish/l...a&RecordNo=3090
> : >
> : > Magnesium (older article with fonts screwed up)
> : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : >
> : > Phosphate (older article now reproduced in a poor fashion)
> : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : >
> : > Carbon Dioxide
> : > http://www.animalnetwork.com/fish/l...a&RecordNo=2074
> : >
> : > Using Conductivity to Measure Salinity
> : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : >
> : > Understanding Seawater
> : > http://www.animalnetwork.com/fish2/...s/1/default.asp
> : >
> : > Protein Skimming: How It Works
> : > http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
> : >
> : >
> : >
> : > Articles by Craig Bingman:
> : >
> : > Carbon Dioxide tests
> : > http://www.animalnetwork.com/fish/l...n=&RecordNo=279
> : >
> : > Limewater, Acetic Acid and Sand Clumping
> : > http://www.animalnetwork.com/fish/l...n=&RecordNo=181
> : >
> : > Calcium and Alkalinity
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Calculation of Calcium Carbonate Saturation States in Reef Aquaria
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : >
> : > Calcification Rates in Several Tropical Coral Reef Aquaria
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Limits To Limewater...Revisited
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Expanding the Limits of Limewater: Adding Organic Carbon Sources
(vinegar)
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : >
> : > Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Magnesium - Part I
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Magnesium - Part II
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > A Homemade Magnesium Supplement
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Simulating the Effect of Calcium Chloride and Sodium Bicarbonate
Additions
> : on Reef Systems
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Additional Simulations: The Combined Effect Of Calcium Chloride
> : > /Sodium Bicarbonate Additions And Water Exchanges
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : >
> : > More articles by Craig Bingman:
> : >
> : > The Halogens - Part I: Bromine in Seawater and Aquaria
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > The Halogens - Part II: Fluoride
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Fluoride Depletion In Four Reef Aquariums
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > The Halogens - Part III: Iodine
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Measuring Halides
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > How Test Kits Work
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Borax pH Calibration
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > A pH Detective Story
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > How to Mix a Batch of Synthetic Seawater in Under Five Minutes
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > SILICON - FOE OR FRIEND?
> : > http://www.animalnetwork.com/fish2/...s/1/default.asp
> : >
> : > The Composition Of Several Synthetic Seawater Mixes
> : > http://www.animalnetwork.com/fish2/...s/1/default.asp
> : >
> : > Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : >
> : >
> : > Andy's calcium calculator
> : > http://www.andy-hipkiss.co.uk/cacalc.htm
> : >
> : > Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
> : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : >
> : > Calcium Reactor Substrate -- Phosphate Levels
> : > by Greg Hiller
> : > http://www.advancedaquarist.com/iss...l2003/short.htm
> : >
> : >
> : > Indoor CO2 Problems
> : > http://www.advancedaquarist.com/iss...r2002/short.htm
> : >
> : > Simon Huntington's CaCO3/CO2 reactor article
> : >
> : > http://reefkeeping.com/issues/2002-...ature/index.htm
> : >
> : > Ron Shimek's Tank Water Analysis Article
> : > http://reefkeeping.com/issues/2002-...ature/index.htm
> : >
> : >
> : >
> : >
> : > Home made salinity standards thread:
> : >
> : > http://reefcentral.com/forums/showt...?threadid=65509
> : >
> : > Reef Chemicals Calculator
> : > http://www.kademani.com/reefchem.htm
> : >
> : >
> : >
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : >
> : > Former US Army Bomb Technician (EOD)
> : > Member; IABTI, NATEODA, WEODF, ISEE & IPS
> : >
> : > If You See Me Running You Better Catch-Up
> : >
> : >
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : > "stoutman" <.@.> wrote in message
> : news:aGuWb.148227$U%5.676753@attbi_s03...
> : > : Boomer,
> : > :
> : > : I am not sure if you are just messing with me or if you are truly
> : confused.
> : > : I hope the latter. Please read from Top to Bottom.
> : > :
> : > :
> : > : From YOUR first link:
> : > :
> : > : http://www.waterontheweb.org/resources/glossary.html
> : > :
> : > : Acidity:
> : > : A measure of how acid a solution may be. A solution with a pH of
less
> : than
> : > : 7.0 is considered acidic. Solutions with a pH of less than 4.5
contain
> : > : mineral acidity (due to strong inorganic acids), while a solution
having
> : a
> : > : pH greater than 8.3 contains no acidity.
> : > :
> : > : Yes,
> : > :
> : > : Good definition (for the most part). pH <7 is indeed acidic. pH >
7 is
> : > : basic. Your web page had a definition for acidity, but not
basicity.
> : > : Strange. That's like defining GOOD and not defining BAD.
> : > :
> : > : Here is the IUPAC (International Union of Pure and Applied
Chemistry)
> : > : definition of acidity:
> : > :
> : > : http://www.chem.qmul.ac.uk/iupac/index.html
> : > :
> : > : acidity
> : > :
> : > : (1) Of a compound:
> : > :
> : > : For Brønsted acids it means the tendency of a compound to act as a
> : hydron
> : > : donor. It can be quantitatively expressed by the acid dissociation
> : constant
> : > : of the compound in water or some other specified medium. For Lewis
acids
> : it
> : > : relates to the association constants of Lewis adducts and -adducts.
> : > :
> : > : (2) Of a medium:
> : > :
> : > : The use of the term is mainly restricted to a medium containing
Brønsted
> : > : acids, where it means the tendency of the medium to hydronate a
specific
> : > : reference base
> : > :
> : > : basicity
> : > :
> : > : For Brønsted bases it means the tendency of a compound to act as
hydron
> : > : (proton) acceptor. The basicity of a chemical species is normally
> : expressed
> : > : by the acidity of the conjugate acid (see conjugate acid-base pair).
For
> : > : Lewis bases it relates to the association constants of Lewis adducts
> : > : and -adducts
> : > :
> : > :
> : > :
> : > : Another definition from the same web page YOU cited: (this is the
same
> : web
> : > : page you cited above)
> : > :
> : > : Alkalinity:
> : > : Acid neutralizing or buffering capacity of water; a measure of the
> : ability
> : > : of water to resist changes in pH caused by the addition of acids or
> : bases
> : > : and therefore, the main indicator of susceptibility to acid rain; in
> : natural
> : > : waters it is due primarily to the presence of bicarbonates,
carbonates
> : and
> : > : to a much lesser extent occasionally borates, silicates and
phosphates.
> : It
> : > : is expressed in units of milligrams per liter (mg/l) of CaCO3
(calcium
> : > : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l =
1
> : mg/l
> : > : of CaCO3. A solution having a pH below about 5 contains no
alkalinity.
> : > :
> : > : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and
says
> : > : that alkalinity is the measure of ...(description of a buffer)
> : > :
> : > : A BUFFER IS : a measure of the ability of water to resist changes in
pH
> : > : caused by the addition of acids or bases (from definition below)
> : > :
> : > :
> : > : I said:
> : > : ***alkalinity is a measurement of 'buffering capacity'***
> : > :
> : > : You said:
> : > : ***Alkalinity is not a measurement of BC
> : > :
> : > : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is
not
> : > : logical.
> : > :
> : > : (THIS FROM THE SAME WEB PAGE YOU CITED):
> : > :
> : > : Buffer:
> : > : A substance which tends to keep pH levels fairly constant when acids
or
> : > : bases are added.
> : > :
> : > : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
> : > :
> : > : a measure of the ability of water to resist changes in pH caused by
the
> : > : addition of acids or bases
> : > :
> : > : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A
BUFFER.
> : > :
> : > :
> : > : I went to all four links. None contradict what I have said. But
the
> : first
> : > : one you cited contradicts YOU!
> : > :
> : > : I know what a buffer is. I know what acidity means. I know what
> : alkalinity
> : > : means. No need to cite web pages that describe what I know and what
I
> : wrote
> : > : in this discussion. Show me one that says alkalinity is not a
measure
> : of
> : > : buffering capacity from a credible source.
> : > :
> : > :
> : > :
> : > :
> : > :
> : > :
> : > : "Boomer" > wrote in message
> : > : ...
> : > : > Alkalinity a measure of the amount of anions of weak acid in water
and
> : of
> : > : the cations
> : > : > balanced against them
> : > : > Take note it says ***acid***
> : > : >
> : > : > Buffering capacity the ability of a solution to resist or dampen
> : changes
> : > : in pH upon the
> : > : > addition of acids or bases.
> : > : > Take note its says ***the addition of acids or bases***
> : > : >
> : > : > One more
> : > : >
> : > : > http://www.waterontheweb.org/resources/glossary.html
> : > : >
> : > : > We could go on like this all day, so what is the point ?
> : > : >
> : > : > You will LOVE this one
> : > : > http://www.kyantec.com/Tips/phbuffering.htm
> : > : >
> : > : > Don't you just lovbe PDF's
> : > : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
> : > : >
> : > : > Don't fall out of your chair
> : > : >
http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
> : > : >
> : > : >
> : > : >
> : > : >
> : > : > --
> : > : > Boomer
> : > : >
> : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : >
> : > : > Want to See More ?
> : > : > Please Join Our Growing Membership
> : > : > www.coralrealm.com
> : > : >
> : > : > If You See Me Running You Better Catch-Up
> : > : > "stoutman" <.@.> wrote in message
> : news:XB7Wb.19339$QA2.62332@attbi_s52...
> : > : > : Man here is another, google is a wonderful thing. I'm not
filtering
> : any
> : > : > : out, just posting what I find by GOOGLING for you.
> : > : > :
> : > : > :
http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> : > : > :
> : > : > :
> : > : > : Wow, a gov link. Even the government is wrong, this must be a
> : > : conspiracy
> : > : > : against Boomer.
> : > : > :
> : > : > :
> : > : > :
> : > : > :
> : > : > : "Boomer" > wrote in message
> : > : > : ...
> : > : > : > Now I am getting bored
> : > : > : >
> : > : > : > "Don't the components of a buffer account for the buffering
> : capacity?
> : > : > : Yes."
> : > : > : >
> : > : > : > Yes, agreed but you seem to fail what I'm saying. Buffering
> : Capacity
> : > : and
> : > : > : Alkalinity are
> : > : > : > not the same, that has always been the issue. I gave the
equation
> : does
> : > : > : that look like an
> : > : > : > Alkalinity equation or how Alk is determined. I see you had
now
> : > : comments
> : > : > : on it what's
> : > : > : > wrong, why no comments on the equations I gave. Don't
understand
> : them
> : > : or
> : > : > : what ? Again this
> : > : > : > is the equation for Buffering Capacity, also called Buffer
Index
> : or
> : > : Buffer
> : > : > : Intensity. It
> : > : > : > is defined in most water chemistry and chemical oceanography
text
> : > : books.
> : > : > : >
> : > : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] +
[H30+] +
> : > : CKa
> : > : > : [H3O+] / (Ka =
> : > : > : > H3O+])² )
> : > : > : >
> : > : > : > This is not Alkalinity now is it ?
> : > : > : >
> : > : > : > "I know how to do a titration, In fact I have done several.
How
> : many
> : > : have
> : > : > : > you actually done? I don't mean by counting drops, I mean
with a
> : > : buret?"
> : > : > : >
> : > : > : > Well good for you, I use a Digital Titrator
> : > : > : >
> : > : > : > "Oh, I see,
> : > : > : > you think acidity is the opposite of alkalinity. In the world
of
> : > : > : CHEMISTRY
> : > : > : > it's not. Maybe in aquarium newsgroups it is.
> : > : > : >
> : > : > : > Hum no, maybe you should go for a look at HACH's or LaMotte
> : website or
> : > : the
> : > : > : book I
> : > : > : > suggested earlier. Please view a copy.
> : > : > : >
> : > : > : > Standard Methods for the Examination of Water and Wastewater
> : > : > : >
> : > : > : > This book, over 2000 pages, is the guide for water testing. If
you
> : are
> : > : > : reporting water
> : > : > : > test to the EPA you must use approved std from this text.I t
is
> : > : prepared
> : > : > : and published by
> : > : > : > the EPA, American Water Works Association and American Public
> : Health
> : > : > : Association. You
> : > : > : > mean you don't have one and the issue is water chemistry
> : > : > : >
> : > : > : > You are confusing Acidity and Acidity as you know little about
> : water
> : > : > : chemistry and
> : > : > : > procedures and test methods
> : > : > : >
> : > : > : > From SMEWW, section 2-30, 2310 ACIDITY
> : > : > : >
> : > : > : > "Acidity of water is its quantative capacity to react with a
> : strong
> : > : base
> : > : > : to a designated
> : > : > : > pH"
> : > : > : >
> : > : > : > This is how you test for it
> : > : > : >
> : > : > : > A std alkali titration to methyl orange or phenolphthalein
> : > : > : > endpoint.
> : > : > : >
> : > : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that
> : write
> : > : this
> : > : > : book, there are
> : > : > : > over 100 of them, they are wrong.
> : > : > : >
> : > : > : > Like Buffering Capacity you have your Acidity's mixed up
> : > : > : > In water measurement if you have a high Alk you also usually
have
> : a
> : > : high
> : > : > : Acidity.
> : > : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
> : > : CHEMISTRY
> : > : > : BOOK there pal.
> : > : > : >
> : > : > : >
> : > : > : > "These are all in equilibrium with each other. An initial
high pH
> : > : (above
> : > : > : > 6.4) will shift the equilibrium to the right to form HCO3-1.
If
> : the
> : > : pH of
> : > : > : > the solution is above 10.3 (pKa2) the .........."
> : > : > : >
> : > : > : >
> : > : > : > Christ, there you go again with the FW ****. All your numbers
are
> : > : wrong we
> : > : > : are dealing
> : > : > : > with SEAWATER
> : > : > : >
> : > : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is
in
> : the
> : > : form
> : > : > : > of HCO3-1 .
> : > : > : >
> : > : > : > I have already pointed that out and gave actual values at know
> : > : seawater
> : > : > : levels, go back
> : > : > : > and re-read it you aren't telling me anything here.Of course
most
> : is
> : > : HCO3
> : > : > : see...
> : > : > : >
> : > : > : >
> : > : > : > @ 20C and 34.3 ppt salinity
> : > : > : >
> : > : > : > CO2 = 0.52 %
> : > : > : >
> : > : > : > HCO3 = 86.4 %
> : > : > : >
> : > : > : > CO3 = 13.09 %
> : > : > : >
> : > : > : >
> : > : > : > "In your glass experiment you managed to lower the pH enough
to
> : purge
> : > : out
> : > : > : CO2
> : > : > : > by boiling"
> : > : > : >
> : > : > : > The purpose behind the glass is to show that alk is not affect
by
> : CO2
> : > : and
> : > : > : vise-versa and
> : > : > : > how Co2 affects pH.
> : > : > : >
> : > : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and
that
> : pH
> : > : drops
> : > : > : to say 8.1 it is
> : > : > : > usually due to excess CO2. If you took a glass of that water
and
> : > : aerated
> : > : > : it you WILL drive
> : > : > : > off the CO2 and raise the pH. It has been done a proven a
million
> : > : times.
> : > : > : >
> : > : > : > "In order to 'purge' CO2 you would need to lower the
> : > : > : > pH to shift the equilibrium to below 6.4"
> : > : > : >
> : > : > : > The hell you do !!!.Do you know who many times people on this
NG
> : to
> : > : > : include Dr. Craig
> : > : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned
to
> : take a
> : > : > : sample of aquarium
> : > : > : > water and aerate it to see if the pH GOES UP AND when they
come
> : back
> : > : with
> : > : > : the test it is
> : > : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D
CHEMIST
> : > : excess
> : > : > : CO2 in the tank
> : > : > : > water, increase the circulation for better gas exchange at the
> : > : surface,
> : > : > : reduce feeding,
> : > : > : > and try to improve on better skimming, thus reducing the
bio-load
> : and
> : > : pH
> : > : > : decline due to
> : > : > : > CO2.
> : > : > : >
> : > : > : >
> : > : > : > "I hope this helps. "
> : > : > : >
> : > : > : > Help, how can you when you miss everything. I should be
charging
> : you
> : > : > : >
> : > : > : > Oh, by the way. Your websites, I have about 50 on these
issues, I
> : > : could
> : > : > : post them, not to
> : > : > : > mention I have all those water chemistry books, so there is no
> : need to
> : > : > : view your sites.
> : > : > : >
> : > : > : > Finally are you afraid to come to our Chemistry Forum, afraid
to
> : get
> : > : > : slapped by REAL
> : > : > : > chemists. I get a charge out of you can't post your ref .I
have
> : posted
> : > : the
> : > : > : same or similar
> : > : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have
1500
> : > : posts
> : > : > : there and am the
> : > : > : > biggest contributor to his forum other than himself or maybe
Habib
> : > : Sheka
> : > : > : >
> : > : > : > Hum, here are Randy's ref that he posted. He hosts the website
> : > : > : >
> : > : > : > S. RANDY HOLMES-FARLEY
> : > : > : > Arlington, Massachusetts
> : > : > : >
> : > : > : > EDUCATION
> : > : > : >
> : > : > : > 1982-1986 Harvard University Cambridge, MA
> : > : > : > PhD in Chemistry
> : > : > : > Research Advisor: George Whitesides
> : > : > : >
> : > : > : > Investigated the relationship between polymer surface
chemistry
> : and
> : > : > : physical properties
> : > : > : > through controlled surface modification and testing.
> : > : > : >
> : > : > : > 1980-1982 Cornell University Ithaca, NY
> : > : > : > BA in Chemistry and Biology
> : > : > : > Graduated Summa Cum Laude
> : > : > : > Distinction in All Subjects
> : > : > : > Grade Point: 3.94/4.0
> : > : > : > Honors research: isolation and characterization of the subunit
of
> : CF1
> : > : > : enzyme
> : > : > : >
> : > : > : >
> : > : > : > 1978-1979 Stanford University Palo Alto, CA
> : > : > : > Grade Point: 3.55/4.0
> : > : > : >
> : > : > : >
> : > : > : > EXPERIENCE
> : > : > : >
> : > : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham,
MA
> : > : > : > (bought out GelTex Pharmaceuticals in 2001)
> : > : > : > Vice President, Chemical Research 2001-present
> : > : > : > Senior Director, Chemical Research 1999-2001
> : > : > : > Director of Chemical Research 1997-1999
> : > : > : > Manager of Chemical Research 1995-1997
> : > : > : > Group Leader 1994-1995
> : > : > : > Senior Research Scientist 1992-1994
> : > : > : >
> : > : > : > Helped start GelTex as second employee
> : > : > : >
> : > : > : > Managed various research programs with multi-million dollar
> : budgets
> : > : > : >
> : > : > : > Supervised research chemists (17+)
> : > : > : >
> : > : > : > Co-inventor of several polymeric pharmaceuticals and
> : pharmaceutical
> : > : > : candidates including
> : > : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam
> : Hydrochloride
> : > : (FDA
> : > : > : approved)
> : > : > : >
> : > : > : > Company Safety Officer for 3 years
> : > : > : >
> : > : > : > Chemical Hygiene Officer 2000-present
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > 1990-1992 GTE Corporation Waltham, MA
> : > : > : > Senior Member of Technical Staff
> : > : > : > Applied research involving polymer interfaces
> : > : > : > Metallization of plastics
> : > : > : > Polymer/polymer adhesion
> : > : > : > Optical coatings
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > 1986-1990 Lord Corporation Cary, NC
> : > : > : > Senior Research Scientist 1988-1990
> : > : > : > Research Scientist 1986-1988
> : > : > : > Basic and applied research on surface chemical bonding
> : > : > : > Developed new adhesive compositions
> : > : > : > Developed new sol-gel coatings for corrosion resistance
> : > : > : >
> : > : > : >
> : > : > : > HONORS AND AWARDS
> : > : > : >
> : > : > : > Industrial Innovations Award by Northeast Region of American
> : Chemical
> : > : > : Society (6/2001)
> : > : > : >
> : > : > : > National Kidney Foundation of Northern California Honoree
(5/2001)
> : > : > : >
> : > : > : > American Chemical Society/Polymer Chemistry Division
Industrial
> : > : Sponsors
> : > : > : > Award (8/2000)
> : > : > : >
> : > : > : > R&D 100 Award from R&D magazine (1999)
> : > : > : >
> : > : > : > Sherwin Williams Award in applied polymer science (9/85)
> : > : > : >
> : > : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985;
> : 1985-1986)
> : > : > : >
> : > : > : > Award for highest GPA in Chemistry Department (6/82)
> : > : > : >
> : > : > : > Summa Cum Laude Honors in Chemistry (6/82)
> : > : > : >
> : > : > : > Phi Lamda Epsilon (6/82)
> : > : > : >
> : > : > : > Phi Beta Kappa (2/82)
> : > : > : >
> : > : > : > Cornell University Dean's List (1981, 1982)
> : > : > : >
> : > : > : > Harvard Book Club Award for highest GPA senior year (1978)
> : > : > : >
> : > : > : > First Place in western NY ACS high school chemistry exam
(1977)
> : > : > : >
> : > : > : > 1978-1979
> : > : > : >
> : > : > : >
> : > : > : > __________________
> : > : > : > Randy Holmes-Farley
> : > : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef
> : Central
> : > : > : >
> : > : > : > Hobby Experience: 8 years with reefs
> : > : > : > Current Tanks: 90 gal mixed reef
> : > : > : > Interests: Reefkeeping, science, photography
> : > : > : >
> : > : > : >
> : > : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> : > : > : >
> : > : > : > Open this post in a new window | Report this post to a
moderator |
> : IP:
> : > : > : Logged
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > 06/27/2003 02:44 PM
> : > : > : >
> : > : > : > Randy Holmes-Farley
> : > : > : > Chemistry Moderator
> : > : > : >
> : > : > : > Registered: Apr 2001
> : > : > : > Location: Arlington, Massachusetts
> : > : > : > Occupation: Chemist (Drug Discovery at Genzyme)
> : > : > : > Posts: 15282
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > Publications
> : > : > : >
> : > : > : >
> : > : > : > ISSUED UNITED STATES PATENTS
> : > : > : >
> : > : > : >
> : > : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen
Randall;
> : > : > : Mandeville, III; W. Harry.
> : > : > : > US 6,566,407; 5/20/2003
> : > : > : >
> : > : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley,
Stephen
> : > : Randall;
> : > : > : Huval, Chad
> : > : > : > Cori.
> : > : > : > U.S. 6,517,825; 2/11/2003.
> : > : > : >
> : > : > : > 3. Method of making phosphate-binding polymers for oral
> : > : administration.
> : > : > : Holmes-Farley,
> : > : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M.
U.S.
> : > : > : 6,509,013; 1/21/2003.
> : > : > : >
> : > : > : > 4. Combination therapy for treating hypercholesterolemia using
a
> : bile
> : > : acid
> : > : > : sequestrant
> : > : > : > polymer
> : > : > : > and a cholesterol-lowering agent. Huval, Chad Cori;
Holmes-Farley,
> : > : Stephen
> : > : > : Randall;
> : > : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> : > : > : >
> : > : > : > 5. Method for treating hypercholesterolemia with
polyallylamine
> : > : polymers.
> : > : > : Holmes-Farley,
> : > : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
> : > : Goldberg,
> : > : > : Dennis I. , US
> : > : > : > 6,423,754; 7/23/2002.
> : > : > : >
> : > : > : > 6. Ionic polymers as anti-infective agents Mandeville, W.
Harry,
> : III;
> : > : > : Neenan, Thomas X..;
> : > : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> : > : > : >
> : > : > : > 7. Combination therapy for treating hypercholesterolemia and
> : > : > : atherosclerosis. Huval, Chad
> : > : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal,
> : Pradeep
> : > : K.
> : > : > : U.S. 6,365,186;
> : > : > : > 4/2/2002.
> : > : > : >
> : > : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
> : > : Mandeville,
> : > : > : W. H., III;
> : > : > : > Huval; C.
> : > : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US
6,299,868;
> : > : > : 10/9/2001.
> : > : > : >
> : > : > : > 9. Polymers containing guanidinium groups as bile acid
> : sequestrants.
> : > : Dhal;
> : > : > : P. K.; Holmes-
> : > : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> : > : > : >
> : > : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.;
Mandeville,
> : W.
> : > : H.,
> : > : > : III.; US
> : > : > : > 6,281,252;
> : > : > : > 8/28/2001.
> : > : > : >
> : > : > : > 11. Combination therapy for treating hypercholestrolemia.
Huval;
> : C.
> : > : C.;
> : > : > : Holmes-Farley; S.
> : > : > : > R. ;
> : > : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> : > : > : >
> : > : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides,
G.
> : M.;
> : > : > : Holmes-Farley, S.
> : > : > : > R.; US
> : > : > : > 6,264,937; 7/24/2001.
> : > : > : >
> : > : > : > 13. Method for treating hypercholesterolemia with
unsubstituted
> : > : > : polydiallylamine polymers.
> : > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
K.
> : ; US
> : > : > : 6,248,318;
> : > : > : > 6/19/2001.
> : > : > : >
> : > : > : > 14. Process for removing bile salts from a patient and
alkylated
> : > : > : compositions therefore.
> : > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355;
> : 5/1/2001.
> : > : > : >
> : > : > : > 15. Poly(diallylamine)-based bile acid sequestrants.
> : Holmes-Farley, S.
> : > : R.;
> : > : > : Dhal, P. K.;
> : > : > : > Petersen,
> : > : > : > J. S.; US 6,203,785; 3/20/2001.
> : > : > : >
> : > : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S.
R.;
> : > : Huval,
> : > : > : C. C.; US
> : > : > : > 6,190,649;
> : > : > : > 2/20/2001.
> : > : > : >
> : > : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.;
Mandeville,
> : W.
> : > : H.,
> : > : > : III.; US
> : > : > : > 6,177,478;
> : > : > : > 1/23/2001.
> : > : > : >
> : > : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
> : > : Holmes-Farley,
> : > : > : S. R.;
> : > : > : > Mandeville, W.
> : > : > : > H., III.; US 6,129,910; 10/10/2000.
> : > : > : >
> : > : > : > 19. Method for treating hypercholesterolemia with
unsubstituted
> : > : > : polydiallylamine polymers.
> : > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
K.
> : ; US
> : > : > : 6,083,497;
> : > : > : > 7/4/2000.
> : > : > : >
> : > : > : > 20. Method of making phosphate-binding polymers for oral
> : > : administration.
> : > : > : Holmes-Farley, S.
> : > : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US
6,083,495;
> : > : 7/4/2000.
> : > : > : >
> : > : > : > 21. Process for removing bile salts from a patient and
alkylated
> : > : > : compositions therefore.
> : > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
> : > : 5/23/2000.
> : > : > : >
> : > : > : > 22. Process for removing bile salts from a patient and
> : compositions
> : > : > : therefor. Mandeville,
> : > : > : > W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> : > : > : >
> : > : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III;
W.
> : H;
> : > : > : Neenan; T. X.; Holmes-
> : > : > : > Farley; S. R. US 6,034,129; 3/7/2000.
> : > : > : >
> : > : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.;
Mandeville,
> : W.
> : > : H.,
> : > : > : III.; US
> : > : > : > 5,985,938;
> : > : > : > 11/16/99.
> : > : > : >
> : > : > : > 25. Process for removing bile salts from a patient and
> : compositions
> : > : > : therefor. Mandeville,
> : > : > : > W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> : > : > : >
> : > : > : > 26. Hydrophobic sequestrant for cholesterol depletion.
Mandeville,
> : W.
> : > : H.,
> : > : > : III.;
> : > : > : > Holmes-Farley;
> : > : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> : > : > : >
> : > : > : > 27. Hydrophilic nonamine-containing and amine-containing
> : copolymers
> : > : and
> : > : > : their use as bile
> : > : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
> : > : 5,929,184;
> : > : > : 7/27/99.
> : > : > : >
> : > : > : > 28. Interpenetrating polymer networks for sequestration of
bile
> : acids.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US
> : 5,925,379;
> : > : > : 7/20/99.
> : > : > : >
> : > : > : > 29. Amine polymer sequestrant and method of cholesterol
depletion.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> : > : > : >
> : > : > : > 30. Process for removing bile salts from a patient and
> : compositions
> : > : > : therefor. Mandeville,
> : > : > : > W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> : > : > : >
> : > : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
> : depletion.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> : > : > : >
> : > : > : > 32. Process for removing bile salts from a patient and
> : compositions
> : > : > : therefor. Mandeville,
> : > : > : > W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> : > : > : >
> : > : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
> : > : Mandeville,
> : > : > : W. H., III.;
> : > : > : > Holmes-
> : > : > : > Farley, S. R.; US 5,703,188; 12/30/97.
> : > : > : >
> : > : > : > 34. Oral administration of iron-binding crosslinked amine
> : polymers.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> : > : > : >
> : > : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
> : Holmes-Farley,
> : > : S.
> : > : > : R.; US 5,693,675;
> : > : > : > 12/2/97.
> : > : > : >
> : > : > : > 36. Method for removing bile salts from a patient with
alkylated
> : > : > : crosslinked amine
> : > : > : > polymers,
> : > : > : > and preparation of the polymers. Mandeville, W. H., III.;
> : > : Holmes-Farley,
> : > : > : S. R.; US
> : > : > : > 5,679,717; 10/21/97.
> : > : > : >
> : > : > : > 37. Phosphate-binding polymers for oral administration.
> : Holmes-Farley,
> : > : S.
> : > : > : R.; Mandeville,
> : > : > : > W.
> : > : > : > H., III.; US 5,667,775; 9/16/97.
> : > : > : >
> : > : > : > 38. Ion-exchange process using highly crosslinked polymers for
> : > : removing
> : > : > : bile salts from a
> : > : > : > patient, preparation of the polymers, and compositions
containing
> : > : them.
> : > : > : Mandeville, W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> : > : > : >
> : > : > : > 39. Hydrophobic amine polymer sequestrant and method of
> : cholesterol
> : > : > : depletion. Mandeville,
> : > : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US
5,618,530;
> : > : 4/8/97.
> : > : > : >
> : > : > : > 40. Amine polymer sequestrant and method of cholesterol
depletion.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> : > : > : >
> : > : > : > 41. Phosphate-binding polymers for oral administration.
> : Holmes-Farley,
> : > : S.
> : > : > : R.; Mandeville,
> : > : > : > W.
> : > : > : > H., III.; US 5,496,545; 3/5/96.
> : > : > : >
> : > : > : > 42. Iron-binding polymers for oral administration. Mandeville,
W.
> : H.,
> : > : > : III.; Holmes-Farley,
> : > : > : > S. R.;
> : > : > : > US 5,487,888; 1/30/96.
> : > : > : >
> : > : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having
> : active
> : > : > : hydrogens on the
> : > : > : > surface.
> : > : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> : > : > : >
> : > : > : > 44. Layered sol-gel coatings from organisilicon compounds.
> : > : Holmes-Farley,
> : > : > : S. R.; Yanyo, L.
> : > : > : > C.;
> : > : > : > US 5,182,143; 1/26/93.
> : > : > : >
> : > : > : > 45. Method for metal bonding using ultrathin primer coating.
> : > : > : Holmes-Farley, S. R.; Yanyo,
> : > : > : > L.
> : > : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> : > : > : >
> : > : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.;
Abbey, K.
> : J.;
> : > : US
> : > : > : 5,096,962;
> : > : > : > 3/17/92.
> : > : > : >
> : > : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> : > : > : elastomer-metal bonding.
> : > : > : > Holmes-
> : > : > : > Farley, S. R.; US 5,102,956; 4/7/92.
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT
ISSUED)
> : > : > : >
> : > : > : >
> : > : > : > 1. Aryl boronate functionalized polymers for treating obesity
and
> : > : > : inhibiting fat uptake.
> : > : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III;
Dhal,
> : > : Pradeep
> : > : > : K.; Huval, Chad
> : > : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl.
(2003),
> : 92
> : > : pp. WO
> : > : > : 0302571.
> : > : > : >
> : > : > : > 2. Preparation of aryl boronic acids for treating obesity.
> : > : Holmes-Farley,
> : > : > : Stephen Randall;
> : > : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal,
> : Pradeep
> : > : K.
> : > : > : (Geltex
> : > : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO
> : 0302570.
> : > : > : >
> : > : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide.
> : Holmes-Farley,
> : > : > : Stephen Randall.
> : > : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32
pp.
> : WO
> : > : > : 0302130.
> : > : > : >
> : > : > : > 4. Method for reducing copper levels and treating copper
> : toxicosis.
> : > : > : Holmes-Farley, Stephen
> : > : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl.
> : (2002),
> : > : 45
> : > : > : pp. WO
> : > : > : > 0285383.
> : > : > : >
> : > : > : > 5. Method for treating gout and binding uric acid.
Holmes-Farley,
> : > : Stephen
> : > : > : Randall; Burke,
> : > : > : > Steven K. WO 0285381 10/31/2002.
> : > : > : >
> : > : > : > 6. Method for treating gout and reducing serum uric acid.
> : > : Holmes-Farley,
> : > : > : Stephen Randall;
> : > : > : > Burke, Steven K WO 0285380 10/31/2002.
> : > : > : >
> : > : > : > 7. Amine condensation polymer bile acid sequestrants. Huval,
C.
> : C.;
> : > : > : Holmes-Farley, S. R.;
> : > : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> : > : > : >
> : > : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H.,
III
> : and
> : > : > : Holmes-Farley, S.
> : > : > : > R.;
> : > : > : > WO 1999-US5662; 9/23/1999.
> : > : > : >
> : > : > : > 9. Amine-containing copolymers as bile acid sequestrants.
> : > : Holmes-Farley,
> : > : > : S. R.; Petersen,
> : > : > : > J. S.;
> : > : > : > WO 9933452; 7/8/1999.
> : > : > : >
> : > : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W.
H.,
> : III
> : > : and
> : > : > : Holmes-Farley, S.
> : > : > : > R.;
> : > : > : > WO 9922743; 5/14/1999.
> : > : > : >
> : > : > : > 11. Polyallylamine polymers for removing bile salts and
treating
> : > : > : hypercholesterolemia, and
> : > : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H.,
III;
> : > : Burke,
> : > : > : S. K.; Goldberg,
> : > : > : > D. I.; WO 9857652; 12/23/98.
> : > : > : >
> : > : > : > 12. Phosphate-bidning polymers combined with a calcium
supplement
> : for
> : > : oral
> : > : > : administration.
> : > : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
> : Holmes-Farley,
> : > : S.
> : > : > : R.; WO 9842355;
> : > : > : > 10/1/98.
> : > : > : >
> : > : > : > 13. Hydrophobic heteroatom-containing sequestrant for
cholesterol
> : > : > : depletion. Mandeville,
> : > : > : > W.
> : > : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449;
> : 12/12/96.
> : > : > : >
> : > : > : > 14. Process for adjusting ion concentration in a patient and
> : > : compositions
> : > : > : therefor.
> : > : > : > Mandeville,
> : > : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> : > : > : >
> : > : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
> : > : interlayer
> : > : > : for improved
> : > : > : > metal-
> : > : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
> : > : 1/20/94.
> : > : > : >
> : > : > : > 16. Process for increased metal-substrate bond strength in
> : metalized
> : > : > : plastics.
> : > : > : > Holmes-Farley, S.
> : > : > : > R.; Ger. Offen. 4322516; 7/6/93.
> : > : > : >
> : > : > : > 17. Electrorheological fluids and preparation of particles
useful
> : in
> : > : the
> : > : > : fluids.
> : > : > : > Troughton,
> : > : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie;
Carlson,
> : J.
> : > : > : David; Bares, Joseph
> : > : > : > E.;
> : > : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra
Nell.
> : EP
> : > : > : 394049;
> : > : > : > 10/24/1990.
> : > : > : >
> : > : > : > JOURNAL PUBLICATIONS
> : > : > : >
> : > : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William;
Zhorov,
> : > : Eugene;
> : > : > : Guo, Amy;
> : > : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David
L.;
> : > : > : Mandeville, W. Harry;
> : > : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
> : > : 611-619.
> : > : > : >
> : > : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
> : > : synthesis
> : > : > : and biological
> : > : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley,
S.
> : > : Randall;
> : > : > : Mandeville, W.
> : > : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal,
Pradeep
> : K.
> : > : > : Journal of
> : > : > : > Macromolecular Science, Pure and Applied Chemistry (2001),
> : A38(12),
> : > : > : 1559-1574.
> : > : > : >
> : > : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by
> : Molecular
> : > : > : Imprinting. Huval,
> : > : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.;
Holmes-Farley,
> : S.
> : > : > : Randall; Mandeville,
> : > : > : > W.
> : > : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro,
> : Robert
> : > : J.;
> : > : > : Chen, Xi; Dhal,
> : > : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> : > : > : >
> : > : > : > 4. Synthetic polymers for the binding of fat in the intestinal
> : tract.
> : > : > : Jozefiak, Thomas H.;
> : > : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny,
Cynthia;
> : > : Huval,
> : > : > : Chad C.;
> : > : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney,
Cynthia.
> : > : > : Abstracts of
> : > : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United
States,
> : August
> : > : > : 26-30, 2001
> : > : > : > (2001), POLY-047 and Polymer Preprints (American Chemical
Society,
> : > : > : Division of
> : > : > : > Polymer Chemistry) (2001), 42(2), 98.
> : > : > : >
> : > : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel
> : polymer
> : > : gel
> : > : > : pharmaceutical.
> : > : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.;
Petersen,
> : J.;
> : > : Ward,
> : > : > : J.; Sacchiero,
> : > : > : > B.;
> : > : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton,
K.
> : A.;
> : > : Chen,
> : > : > : X.; Mazzeo, J.
> : > : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
> : > : > : >
> : > : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl
and
> : > : other
> : > : > : bile acid
> : > : > : > sequestrants.
> : > : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.;
Xu,
> : Q.;
> : > : > : Hook, P.; Holmes-
> : > : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1),
> : 708-709.
> : > : > : >
> : > : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
> : > : Holmes-Farley,
> : > : > : S. R; Polym.
> : > : > : > Mater. Sci. Eng (1999), 80, 246-247.
> : > : > : >
> : > : > : > 8. Design and characterization of of Sevelamer Hydrochloride:
a
> : novel
> : > : > : phosphate-binding
> : > : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III;
> : Ward,
> : > : J.;
> : > : > : Miller, K. L.;
> : > : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M.
S.-
> : Pure
> : > : and
> : > : > : Appl. Chem.,
> : > : > : > A36(7&8), p. 1085 (1999).
> : > : > : >
> : > : > : > 9. Three generations of bile acid sequestrants. Mandeville, W.
H.,
> : > : III;
> : > : > : Braunlin, W.;
> : > : > : > Dhal, P.;
> : > : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik,
S.;
> : > : > : Rosenbaum, D.;
> : > : > : > Sacchiero,
> : > : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc.
> : (1999),
> : > : > : 550, 3-15.
> : > : > : >
> : > : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked,
polymeric
> : > : phosphate
> : > : > : binder, on
> : > : > : > urinary
> : > : > : > phosphorous excretion in rats. Rosenbaum, D. P.;
Holmes-Farley, S.
> : R.;
> : > : > : Mandeville, W. H.,
> : > : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
> : Transplant.
> : > : > : (1997), 12(5)
> : > : > : > 961-964.
> : > : > : >
> : > : > : > 11. Thin anisotropic coatings based on sol-gel technology.
> : > : Holmes-Farley,
> : > : > : S. R.; Yanyo, L.
> : > : > : > C;
> : > : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem.
4),
> : > : 439-444.
> : > : > : >
> : > : > : > 12. The mechanism of cure initiation of a surface activated
> : adhesive.
> : > : > : Holmes-Farley, S.
> : > : > : > R.;
> : > : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5),
409-420.
> : > : > : >
> : > : > : > 13. Adhesion promotion and corrosion prevention using thin
> : anisotropic
> : > : > : coatings. Holmes-
> : > : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991),
5(2),
> : > : > : 131-151.
> : > : > : >
> : > : > : > 14. Wetting of functionalized polyethylene having ionizable
> : organic
> : > : acids
> : > : > : and bases at the
> : > : > : > polymer-water interface: relations between functional group
> : polarity,
> : > : > : extent of
> : > : > : > ionization,
> : > : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C.
D.;
> : > : > : Whitesides, G. M.;
> : > : > : > Langmuir
> : > : > : > (1988), 4(4), 921-937.
> : > : > : >
> : > : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols
with
> : a
> : > : > : single hydroxy group.
> : > : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> : > : > : >
> : > : > : > 16. Reconstruction of the interface of oxidatively
functionalized
> : > : > : polyethylene (PE-CO2H)
> : > : > : > and
> : > : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.;
> : Nuzzo,
> : > : R.;
> : > : > : McCarthy, T. J.;
> : > : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also
Report
> : > : (1987),
> : > : > : AD-
> : > : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> : > : > : >
> : > : > : > 17. Surface-modified polyethylene film: the relationship
between
> : > : surface
> : > : > : chemistry and
> : > : > : > physical
> : > : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987,
47(11),
> : > : 4537.
> : > : > : >
> : > : > : > 18. Reactivity of carboxylic acid and ester groups in the
> : > : functionalized
> : > : > : interfacial
> : > : > : > region of
> : > : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> : > : > : differentiation of the
> : > : > : > functional groups into shallow and deep subsets based on a
> : comparison
> : > : of
> : > : > : contact angle and
> : > : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.;
> : Langmuir
> : > : > : (1987), 3(1), 62-
> : > : > : > 76.
> : > : > : >
> : > : > : > 19. Fluorescence properties of dansyl groups covalently bonded
tot
> : he
> : > : > : surface of
> : > : > : > oxidatively
> : > : > : > functionalized low-density polyethylene film. Holmes-Farley,
S.
> : R.;
> : > : > : Whitesides, G. M.;
> : > : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985),
TR-85-2;
> : > : > : AD-A162435/2/GAR,
> : > : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> : > : > : >
> : > : > : > 20. Acid-base behavior of carboxylic acid groups covalently
> : attached
> : > : at
> : > : > : the surface of
> : > : > : > polyethylene: The usefulness of contact angle in following the
> : > : ionization
> : > : > : of surface
> : > : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy,
T.
> : J.;
> : > : > : Deutch, J.;
> : > : > : > Whitesides,
> : > : > : > G. M.; Langmuir (1985), 1(6), 725-740.
> : > : > : >
> : > : > : > 21. The thermal stability of a surface modified solid organic
> : polymer.
> : > : > : Holmes-Farley, S.
> : > : > : > R.;
> : > : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53,
127-131.
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> : > : > : >
> : > : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R.
> : Advanced
> : > : > : Aquarist. June 2003.
> : > : > : >
> : > : > : > 2. The Self Purification of Limewater (Kalkwasser).
Holmes-Farley,
> : R.
> : > : > : Advanced Aquarist.
> : > : > : > May
> : > : > : > 2003.
> : > : > : >
> : > : > : > 3. The Degradation of Limewater (Kalkwasser) in Air.
> : Holmes-Farley, R.
> : > : > : Reefkeeping May
> : > : > : > 2003.
> : > : > : >
> : > : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
> : Reefkeeping
> : > : > : April 2003.
> : > : > : >
> : > : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae
Growth.
> : > : > : Holmes-Farley, R.
> : > : > : > Advanced Aquarist; April 2003.
> : > : > : >
> : > : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae
Growth.
> : > : > : Holmes-Farley, R.
> : > : > : > Advanced Aquarist; April 2003.
> : > : > : >
> : > : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R.
Advanced
> : > : Aquarist;
> : > : > : March 2003.
> : > : > : >
> : > : > : > 8. How to Select a Calcium and Alkalinity Supplementation
Scheme.
> : > : > : Holmes-Farley, R.
> : > : > : > Advanced Aquarist; February 2003.
> : > : > : >
> : > : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> : January
> : > : > : 2003.
> : > : > : >
> : > : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> : > : December
> : > : > : 2002.
> : > : > : >
> : > : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
> : > : Advanced
> : > : > : Aquarist; November
> : > : > : > 2002.
> : > : > : >
> : > : > : > 12. Iron: A Look at Organisms Other than Macroalgae.
> : Holmes-Farley, R.
> : > : > : Advanced Aquarist;
> : > : > : > November 2002.
> : > : > : >
> : > : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.;
Advanced
> : > : Aquarist,
> : > : > : September 2002.
> : > : > : >
> : > : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist,
> : August
> : > : > : 2002.
> : > : > : >
> : > : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.;
Reefkeeping.com,
> : April
> : > : > : 2002.
> : > : > : >
> : > : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R.
Advanced
> : > : > : Aquarist; July 2002
> : > : > : >
> : > : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced
Aquarist;
> : > : June
> : > : > : 2002.
> : > : > : >
> : > : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley,
R.
> : > : Advanced
> : > : > : Aquarist, May
> : > : > : > 2002.
> : > : > : >
> : > : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in
> : Corals.
> : > : > : Holmes-Farley, R.
> : > : > : > Advanced Aquarist, April 2002.
> : > : > : >
> : > : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> : > : > : >
> : > : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February
> : 2002.
> : > : > : >
> : > : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist,
January
> : > : 2002.
> : > : > : >
> : > : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium
> : Frontiers
> : > : > : 2000.
> : > : > : >
> : > : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R.
Aquarium
> : > : > : Frontiers 2000.
> : > : > : >
> : > : > : > 25. Phosphate..What is it and why should you care.
Holmes-Farley,
> : R.
> : > : > : Aquarium Frontiers
> : > : > : > 2000.
> : > : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
> : > : Frontiers
> : > : > : 2000.
> : > : > : >
> : > : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium
Frontiers
> : > : 2000.
> : > : > : >
> : > : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium
Frontiers
> : 1999.
> : > : > : >
> : > : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > Boomer
> : > : > : >
> : > : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : > : >
> : > : > : > Want to See More ?
> : > : > : > Please Join Our Growing Membership
> : > : > : > www.coralrealm.com
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > :
> : > : > :
> : > : >
> : > : >
> : > :
> : > :
> : > :
> : >
> : >
> :
> :
>
>

[stoutman]

one more thing,

Let me comment on the CO2 equilibrium.

CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
HCO3-1 <-------> CO3-2


I said, and still say, that if you lower the pH the equilibrium will shift
to the left making it EASIER to purge CO2.

Yes, as the CO2(g) leaves the system the equilibrium will shift to the right
and pH goes up and CO2 leaves less readily. If you lower the pH again it
will shift to the left again, and CO2 will purge more readily. Then as CO2
leaves the system, the pH will go up and equilibrium starts to shift to the
right. If you lower the pH again the equilibrium will shift to the left,
and CO2 will purge more readily. Then as CO2 leaves the system, the pH will
go up and the equilibrium ...

This is the point to this story:

At low pH's (acidic) the equilibrium is left shifted. CO2 leaves MORE
readily
At high pH's (basic) the equilibrium is right shifted. CO2 leaves LESS
readily.

-Stoutman







"Boomer" > wrote in message
...
> Yes, of cause I remember, as I said I posted it for a reason. I see you
have used only
> that link for your definition, as it makes you look right.You have avoided
all Alk
> definitions in a chemistry book, to include your own definition *****to
resist a drop in
> pH due to the addition of acid***, which is the same as the others I
posted .Agreed, of
> course not.You know that Alk isn't defined as "by the addition of acids or
bases "and is
> only the " addition of an acid", so why are you accepting the definition
?.You know that
> when you titrate it is an acid added and never a base. In one breath it
says Alk is "Acid
> neutralizing " and then they say "by the addition of acids or bases ".You
can't have it
> both ways and YOU know that Agreed . If the word "base" was left out I
would not have much
> to say. Agreed
>
>
> "Alkalinity is a
> measurement of BUFFERING CAPACITY."
>
> No it is not a measurement of BUFFERING CAPACITY, it is a indication of
BC. I have said
> this at least twice. If you know your BC you can calculate Alk and if you
can do one you
> can do the other agreed. What I have tried to convey from the beginning is
that Alk and BC
> are not the same thing. You in one of your other posts have said they are
not the same
> thing and never said they were. Now you seem to be saying they are the
same thing
>
> "So, when we measure ALKALINITY (and we know the pH) we are in effect
> measuring BUFFERING CAPACITY.
>
> More or less YES in an "effect" but Alk tells you not much of anything
when a base is
> added Agreed. That is called Acidity, which I see you have avoided again
as if there is
> no such thing. I also said that for us the only thing we need to be
concerned about is
> Alk, so BC would fit in, as we could care less about the ability to
neutralize a base or
> measure Acidity. So, if you knew your pH , Alk or Acy you would really
know what you BC is
> doing for you Agreed.
>
> On Bc, we have both left something from my first equation, so I thought I
would post it
> again for you, as I like being honest .I'm surprised you didn't catch it
:-)
>
> B = dCb / dpH = - dCa / dpH
>
> So;
>
> B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> or
>
> B (Buffering Capacity) = - dCa / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> There are number of was to mathematically express BC. Two of the most
common are the
> change in Alk with the pH at constant total carbonate, the other is change
in Alk with pH
> constant CO2 pp. In some examples of Bc, Bc is the inverse slope of the
Alk titration
> curve ( I'm sure yo
> u will love this) In the other over the pH range, while BC is going
through minimum, Bpp
> increases linearly. This difference is caused by the uptake of CO2 by the
solution, which
> increases Ct as pH increases.To bad we can't or my server won't allow me,
to post
> attachments. I have a nice BC cure of various species as a function of
pC/pH diagrams, set
> to a pKa. curve
>
>
> On another issue
>
> "In order to remove CO2 (g) you ideally would want to shift
> the equilibrium to the left by LOWERING the pH"
>
>
> You may want to try and re-explain this
>
> CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
> HCO3-1 <-------> CO3-2
>
>
> As the reaction shifts to left the pH gets higher as CO2 leaves the
system.You don't have
> to lower the pH to remove CO2. Case in point plants. As they remove CO2
the pH rises,
> continued removal of the Sigma CO2 ( CO2, H2CO3, HCO3,CO3) cause further
rising until
> there is mostly only carbonate (CO3) left and a high pH. Another case, at
a pH of 8.00 and
> Alk of 4 meq / l ( 1.4 mg / l CO2) you have much more CO2 than at 2 meq/
l (0.65mg / l).
> . Aeration of the water can drive off the CO, no lowering of the pH
required., the removal
> will cause the pH to rise .On the other hand, trying to remove CO2 @ 2 meq
/ l won't get
> you much of anywhere in this case. Also, even a low pH doesn't mean you
can drive of CO2.
> If the seawater pH was say 7.5, you would think not problem to drive off
CO2. If the Alk
> was 0.25 there would be about .35 mg / l CO2 to blow off. At the alk of
4.00 meq / l the
> CO2 is 5 mg / l.Usually, when people have a lower pH, say 7.9 or so, it is
do to CO2, so
> the pH has lowered, increasing the CO2, to allow one to blow it off easier
and bring the
> pH back up.
>
> CO2 = [CA(Carbonate Alk) x aH ] / [pK1(1 + 2pK2 /aH)]
>
> I think we just got off on the wrong foot, hope things look better.
>
> I'll be gone for the weekend, leaving in an hour, so have a nice weekend
:-)
>
>
>
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message news:lcRWb.299984$na.451117@attbi_s04...
> : > Humm, since when does Alk have anything to do in regards to the
addition
> : of BASE.
> :
> : You tell me. Your the one that posted a link to a web page that had
this
> : definition of alkalinity. Looks like you put yourself in your own hole
pal.
> :
> : Remember posting this link:
> :
> : http://www.waterontheweb.org/resources/glossary.html
> :
> : Here is the definition of alkalinity from the web page YOU cited. (I
> : recommend you read the web pages you are citing before you cite them)
> : Alkalinity:
> : Acid neutralizing or buffering capacity of water; a measure of the
ability
> : of water to resist changes in pH caused by the addition of acids or
BASES.
> :
> :
> : > It sure is funny how all of the chemist that write water chemistry
> : textbooks never say Alk
> : > is the Buffering Capacity of a solution.
> :
> : Neither did I. I said (for the umpth teen time) Alkalinity is a
> : measurement of BUFFERING CAPACITY.
> :
> : When you measure alkalinity you know your BUFFERING CAPACITY (if you
know
> : your pH). Its a two for one.
> :
> : SEE MY OTHER POST FROM TODAY.
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : >
> : > "I am not sure if you are just messing with me "
> : >
> : > Yes, messing with you, it is called trolling a troll, to see where the
> : hell you would go
> : > and what you would say in regards to last posts. It is called honesty,
of
> : which you have
> : > none off to say the least,that I can see.You always like to post what
> : suits you and just
> : > avoid ref I give. So lets start where you are WRONG and have a great
lack
> : of understanding
> : > of things, to include pointing out all your gross error which you
still
> : FAIL to
> : > acknowledge and which can be prove in many water chem. ref. .I doubt
like
> : hell you are a
> : > chemist at all.You seem to want to con people into thinkin' you are.
But
> : then again, I
> : > have seen chemists like you before, they are not familiar with the,
but
> : they ASK to have
> : > it explained and ask for REF.YOU just shoot from the hip. WHAT GETS
YOU IN
> : TROUBLE. You
> : > remind me of snoot-noise kid that come here and other NG's and
> : forums...that think they
> : > know, buy hey, maybe I'm wrong :-)
> : >
> : >
> : >
> : > 1). Acidity
> : >
> : > "***Benjamin,Water Chemistry (2002, pages 262-263).***
> : >
> : > ***Acidity A concept that is exactly analogous to alkalinity but
measures
> : the base
> : > neutralizing
> : > capacity (BNC) of a solution is Acidity. The quantitative represents
the
> : concentration of
> : > OH- ions that must be added to titrate the solution to a pH near
10.5***
> : >
> : > So that means that not only in Benjamin wrong but, so are Stumm &
Morgan,
> : Millero, Pilosn,
> : > Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I
> : said, you have your
> : > acidity and Acidy mixed up. Acidity as defined above is covered in
most
> : water chemistry
> : > books, written by chemists, who's field of expertise is water
chemistry.
> : You can even buy
> : > Acidity test kits from, HACH, LaMotte, etc..
> : >
> : > You mean you didn't read this or are you just avoiding it .The same
> : definition can be
> : > found in almost any std water chemistry book.
> : >
> : > I have run into few chemists, that are NOT familiar with the above.
Some
> : water reports
> : > require the above Acidity measuring. The issue with you is you do not
> : understand WATER
> : > CHEMISTRY. Everything you have posted can be found a general chemistry
> : book
> : >
> : >
> : >
> : >
> : > 2) Alk and BC
> : >
> : > From the link
> : >
> : > Alkalinity
> : > ***Acid neutralizing or buffering capacity of water; a measure of the
> : ability of water to
> : > resist changes in pH caused by the addition of acids or bases ***
> : >
> : > This is a Buffering Capacity definition not Alk
> : >
> : > Humm, since when does Alk have anything to do in regards to the
addition
> : of BASE. As I
> : > pointed out in the first post the term is often miss used. Even in
YOUR
> : own posts you say
> : > it is based on a acid addition, no mention of **base or acid**
addition
> : by you. Are you
> : > getting confused or what. Or is more you are trying to confuse
everyone
> : you are right. The
> : > above is a definition for Buffer Capacity NOT Alk
> : >
> : > From Drew, Geochemistry of Natural Waters
> : >
> : > "alkalinity, which is formally defined as the equivalent sum of bases
that
> : are titratable
> : > with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH
of
> : the solution is
> : > progressively lowered by the addition of a strong acid (HCL), all the
> : anions on the right
> : > will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4,
H2S,organic
> : acids, H20)"
> : >
> : > This follows almost all description of Alk, that it is acid
neutralizing
> : reaction and has
> : > nothing to do with base neutralizing, which is Acidity (BNC) .I
defined
> : these before you
> : > had no comment
> : >
> : >
> : > Even the links that give the Buffering Capacity definition is wrong,
as is
> : the UIPAC on
> : > Alkalinity. Alkalinity has nothing to do with the addition of bases
only
> : acids. When you
> : > use the words "base and acid" it becomes BC
> : >
> : > Even YOU MUST disagree with these definitions, from YOUR own post
> : >
> : > Think of alkalinity as 'buffering capacity'. Or the ability of a
solution
> : > ***to resist a drop in pH due to the addition of acid***
> : >
> : > Where the flip is the base addition forget it ?
> : >
> : > From Butler; Carbon Dioxide Equilibrium and Their Applications
(professor
> : emeritus
> : > Harvard University) an expert on the subject.
> : >
> : > Buffering Index (Buffering Capacity, Buffer Intensity).
> : >
> : > ***This concept was first developed for mixtures of approximately
equal
> : proportions of
> : > conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such
> : buffer solutions
> : > strongly resist changes in pH when acids or bases are added and are
useful
> : as pH
> : > standards. The Buffer Index tells how great the resistance to pH
changes
> : will be.**
> : >
> : > also from Butler
> : >
> : > Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
> : >
> : > Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
> : >
> : > Acidity is in fact just the negative of Alkalinity ***
> : >
> : > http://www.lagoonsonline.com/acid.htm
> : >
> : >
> :
http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.h
> : tm?E+mystore
> : >
> : > It sure is funny how all of the chemist that write water chemistry
> : textbooks never say Alk
> : > is the Buffering Capacity of a solution. They are always treated and
> : defined separately.
> : >
> : > If you or others choose to treat Alk and BC as the same, well, just
have
> : at it. As I said
> : > in first post I know what you mean.
> : >
> : > "No need to cite web pages that describe what I know and what I wrote
> : > in this discussion"
> : >
> : > No you don't know, who are you trying to convince any way, me, the
guys
> : here and/or all
> : > the water chemists in this world. As I said before go get a dam WATER
> : CHEMISTRY book or
> : > shut the hell up.You keep trying to define things from a general
chemistry
> : book WE ARE IN
> : > THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
> : >
> : >
> : >
> : >
> : >
> : > 3). pKa's and what you don't know or seem to be confused on
> : >
> : > "Therefore, it has two pKa's
> : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
> : The
> : > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated
is
> : > right in there. Is that magic? :)"
> : >
> : > Here it is agin that is twice at least
> : >
> : > "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this
> : example)
> : > you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium
will
> : > be shifted to HCO3-2 by a ratio of 1:100.
> : >
> : > Oh wait , there is a third time LOL
> : >
> : > "At the pH of seawater, the buffering capacity of carbonate is at it's
> : > weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
> : >
> : >
> : > Lets just dunk you on this one. I am taking note you refuse to reply
to
> : YOUR errors
> : >
> : > So you calculated the pH of seawater with freshwater pKa's, now that
is a
> : good trick. From
> : > a number of seawater chemistry books the seawater pKa's are 6 & 9.1,
so
> : according to you,
> : > seemingly not understanding your favorite Henderson-Hasselbach
equation;
> : >
> : > 2 pH = (6 + 9.1) /2 pH = 7.55
> : >
> : > I have never seen seawater with a pH of 7.55. There is no ocean with
that
> : pH. Humm how
> : > come your equation is not working for you today.?
> : >
> : >
> : > "That pH I calculated is
> : > right in there. Is that magic? :)"
> : >
> : > I roll on the floor when I see this = 8.35
> : >
> : > Hum , just a brain far so excuse me for thinkin
> : >
> : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
> : >
> : > Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a
pH of
> : 8.35 there pal
> : > ? That 8.35 is what you are telling people the pH should be, but their
> : meter says 6.4.
> : > This how people will READ this.
> : >
> : >
> : >
> : >
> : > 4.) More on Buffering Capacity
> : >
> : > "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes,
your
> : > alkalinity equation."'
> : >
> : >
> : > Yup, I see that and in this case the HCO3 is the acid and the CO3 is
the
> : base CORRECT. In
> : > Alk you are only dealing with bases and how they react to an acid.
Acidity
> : deals acids and
> : > how they recact to bases "Acidity, A concept that is exactly analogous
to
> : alkalinity but
> : > measures the base neutralizing
> : > capacity (BNC) of a solution is Acidity "Alk is the ANC Acid
neutralizing
> : capacity
> : >
> : > "Don't the components of a buffer account for the buffering capacity?
"
> : >
> : > Yes, they do but so do the acids which work as buffers. NaHCO3 is a
buffer
> : and can act as
> : > an acid or base
> : >
> : > *** Buffering Capacity.**
> : > The power of a substance in solution to absorb acid or alkali without
> : change in pH; this
> : > is highest at a pH value equal to the pKa value of the acid of the
buffer
> : pair.***
> : >
> : > ***Akalinity***
> : > Measure of the power of a solution to neutralise hydrogen ions (H+),
> : usually expressed as
> : > the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
> : >
> : >
> : > If one wants to call Alk Buffering capacity then one sure as a hell
can
> : call Acidty
> : > Buffering Capacity also. As it is the ability to neutralizes an acid
that
> : is a buffer.You
> : > have a pH of 7 and you add a buffer to lower it to a pH of 4, you are
> : buffering the water,
> : > that buffer is a acid.
> : >
> : > 5) CO2
> : >
> : > You are really confuse so it seems :-) You realllllllly indicate that
CO2
> : is affected by
> : > the Alk or vise-versa
> : >
> : > "Yes, the pH will drop with the addition of CO2. Remove CO2 will
cause
> : the
> : > pH to rise? How do you remove CO2? Once it is in solution it forms
> : > carbonic acid and neutralizes some of your 'buffer'."
> : >
> : > "With the exception of CO2?"
> : >
> : > No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
> : > Concepts)....PERIOD.You seem to think a that at least in two of your
post
> : that CO2 is
> : > affected by the Alk or vise-versa. Please go back to school or seek
> : professor
> : >
> : > "Why in one case does CO2 from air lower pH and in the other case it
> : raises
> : > it? Doesn't make sense."
> : >
> : > That is because you don't understand CO2 period. By the way I saved
this,
> : wanted to see
> : > if you would bite on the post I gave. Not bite at first, so time to
reel
> : you in, as you
> : > did bite in another post..
> : >
> : > Lets make some sense of it for you, being that you have a pH.D in
> : chemistry, so you say .
> : >
> : > CO2 is naturally generated in a aquatic systems, it is capable of
raise to
> : various levels
> : > depending on a number of circumstances .It can be measure (except in
> : seawater) or
> : > calculated using Buch/Park Equations (what we use for seawater. In
sort if
> : you know the pH
> : > and Alk you can calculate the CO2). If you aerate a system or a sample
of
> : water, even if
> : > the pH has only dropped a couple of tenths, due to an increase in CO2,
the
> : CO2 will leave
> : > solution to the atmosphere.This will raise the pH. On the other hand
if
> : theCO2 level is
> : > more of the norm and you have hikgh room air, such as in the winter,
the
> : partial pressure
> : > of the CO2 in air will be much higher than that in water, in which
case
> : the CO2 will enter
> : > the water and lower the pH. That is without an airstone. Adding an
> : airstone will make it
> : > even worse,as you are now forcefully driving the CO2 into solution
even
> : quicker. These
> : > test /experiments have been proven many times, it is not that may work
> : could work they do
> : > work.Yet you want to disagree and in another post say you haven't
tried
> : it,.Seems to me
> : > that based on what you say it can't work So, in short you don't know
what
> : the hell you are
> : > taking about. Go get a glass of seawater with a pH of about 8.3 and
lower
> : it to about
> : > 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK-
UP
> : ( that is if you
> : > don't have a high room air CO2 problem.). This little test has been
done
> : thousands of
> : > times in this hobby, with test kits, pH meters and even graphic
printers.
> : >
> : > "This is where Boomer and I
> : > disagree. I say you would have to lower the pH very low in order to
> : > effectively remove CO2 by purging."
> : >
> : > You are 100 % wrong. Please come to our Chem forum and try and run
that by
> : Randy, don't
> : > take my word on it. I already know what he will say.
> : >
> : > "Boomer didnt convince me it
> : > works at the pH of an aquarium, but I never tried it and I'm not sure
of
> : > this. "
> : >
> : > Well then come too our chem. forum and tell Randy he doesn't know what
he
> : is talking about
> : > LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it
> : should be easy for
> : > you to run the experiment LOL There are grade school kids that run the
> : test and know what
> : > happens and that I'm correct.
> : >
> : >
> : > "The equilibrium is a FUNCTION
> : > of pH."
> : >
> : > It is also a function of Alk or don't you know that. At a pH of 8.3,
Alk
> : 2.25, the CO2 is
> : > about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk
to
> : about .4 meq/ l
> : > or so the CO2 will be around .99 mg / l CO2, When dealing with
tanksCO2 is
> : not always in
> : > equilibrium with ambient air.
> : >
> : >
> : > ". But I wouldn't degas a solution of a
> : > specific gas (CO2) with a gas (this case he was using air) that
contains
> : the
> : > same gas I am trying to purge."
> : >
> : > Why not ? We have a guy right now that is running tests on purging
ambient
> : air with a
> : > solution to remove CO2 gas from the air, before it enters the tank
> : per/Randy's suggestion.
> : > The same guy is doing some of my test using a Clinoptilolite, a
Zeolite
> : mineral, that has
> : > an affinity for CO2.This will be a dry CO2 scrubber
> : >
> : >
> : > Sorry Soutman but you sure as hell don't seem to know much about
aquatic
> : chemistry. You
> : > seem to be guessing at everything.
> : >
> : > By the way have you read any of Randy's technical articles on water
> : chemistry, been saving
> : > these for last. There are a few on pH, Alk, CO2 .Here is a list
> : >
> : > Try and answer them 1-5 and lets see where we get THIS TIME :-) or
maybe
> : we should just
> : > drop it. I could care less at this point.
> : >
> : > THE END
> : >
> : >
> : > ARTICLES
> : >
> : > The first two posts in this thread are lists of some of my articles
that
> : relate to reef
> : > tank chemistry. In the next few posts are some of the articles
published
> : by Craig Bingman
> : > and others on reef chemistry issues.
> : >
> : > The first two posts in this thread are lists of some of my articles
that
> : relate to reef
> : > tank chemistry. In the next few posts are some of the articles
published
> : by Craig Bingman
> : > and others on reef chemistry issues.
> : >
> : > Solving Common Problems
> : >
> : > Solving Calcium and Alkalinity Problems
> : > http://www.advancedaquarist.com/issues/nov2002/chem.htm
> : >
> : > Solutions to pH Problems
> : > http://www.advancedaquarist.com/iss...ne2002/chem.htm
> : >
> : > How to Select a Calcium and Alkalinity Supplementation Scheme
> : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
> : >
> : > Phosphate Issues
> : > http://www.advancedaquarist.com/iss...pt2002/chem.htm
> : >
> : > Nitrate Issues
> : > http://www.advancedaquarist.com/iss...st2003/chem.htm
> : >
> : >
> : >
> : > Calcium and Alkalinity
> : >
> : > Solving Calcium and Alkalinity Problems
> : > http://www.advancedaquarist.com/issues/nov2002/chem.htm
> : >
> : > How to Select a Calcium and Alkalinity Supplementation Scheme
> : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
> : >
> : > Calcium and Alkalinity Balance Issues
> : > http://reefkeeping.com/issues/2002-...ature/index.htm
> : >
> : > Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
> : > http://www.advancedaquarist.com/iss...ly2002/chem.htm
> : >
> : > The Relationship Between Alkalinity and pH.
> : > http://www.advancedaquarist.com/issues/may2002/chem.htm
> : >
> : > The Chemical & Biochemical Mechanisms of Calcification in Corals
> : > http://www.advancedaquarist.com/issues/apr2002/chem.htm
> : >
> : > Calcium
> : > http://www.advancedaquarist.com/issues/mar2002/chem.htm
> : >
> : > Alkalinity
> : > http://www.advancedaquarist.com/iss...2/chemistry.htm
> : >
> : >
> : > Iron
> : >
> : > First Iron Article: Macroalgae and Dosing Recommendations
> : > http://www.advancedaquarist.com/issues/aug2002/chem.htm
> : >
> : > Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> : > http://www.advancedaquarist.com/issues/oct2002/chem.htm
> : >
> : > Iodine
> : >
> : > Iodine in Marine Aquaria: Part I
> : > http://www.advancedaquarist.com/issues/mar2003/chem.htm
> : >
> : > Iodine in Reef Tanks 2: Effects on Macroalgae Growth
> : > http://www.advancedaquarist.com/iss...il2003/chem.htm
> : >
> : >
> : > Magnesium and Strontium
> : >
> : > Strontium
> : > http://www.advancedaquarist.com/issues/nov2003/chem.htm
> : >
> : > Magnesium
> : > http://www.advancedaquarist.com/issues/oct2003/chem.htm
> : >
> : > Magnesium and Strontium in Limewater
> : > http://www.advancedaquarist.com/issues/dec2003/chem.htm
> : >
> : >
> : > Limewater (kalkwasser)
> : >
> : > The Self Purification of Limewater (Kalkwasser)
> : > http://www.advancedaquarist.com/issues/may2003/chem.htm
> : >
> : > The Degradation of Limewater (Kalkwasser) in Air
> : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : >
> : > How to Select a Calcium and Alkalinity Supplementation Scheme
> : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
> : >
> : > Metals in Aquaria
> : >
> : > Aluminum and aluminum-based phosphate binders
> : > http://www.advancedaquarist.com/iss...ly2003/chem.htm
> : >
> : > Reef Aquaria with Low Soluble Metals
> : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : >
> : > Tap Water in Reef Aquaria
> : > http://www.advancedaquarist.com/issues/jan2004/chem.htm
> : > First Iron Article: Macroalgae and Dosing Recommendations
> : > http://www.advancedaquarist.com/issues/aug2002/chem.htm
> : >
> : > Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> : > http://www.advancedaquarist.com/issues/oct2002/chem.htm
> : >
> : >
> : > Test Kit Reviews
> : >
> : > The Seachem Borate Alkalinity Test Kit
> : > http://www.advancedaquarist.com/iss...ne2003/chem.htm
> : >
> : > The Salifert Boron Test Kit
> : > http://www.advancedaquarist.com/iss...pt2003/chem.htm
> : >
> : > Boron and Borate (and pH buffering)
> : >
> : > Boron in a Reef Tank (and its effect on pH buffering)
> : > http://www.advancedaquarist.com/issues/dec2002/chem.htm
> : >
> : > The Seachem Borate Alkalinity Test Kit
> : > http://www.advancedaquarist.com/iss...ne2003/chem.htm
> : >
> : > The Salifert Boron Test Kit
> : > http://www.advancedaquarist.com/iss...pt2003/chem.htm
> : >
> : >
> : >
> : > Others
> : >
> : > Tap Water in Reef Aquaria
> : > http://www.advancedaquarist.com/issues/jan2004/chem.htm
> : >
> : > ORP
> : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : >
> : > Chloramine
> : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : >
> : > Silica in a Reef Tank
> : > http://advancedaquarist.com/issues/jan2003/feature.htm
> : >
> : > Specific Gravity (and temperature correction of hydrometers)
> : > http://www.advancedaquarist.com/iss...2/chemistry.htm
> : >
> : >
> : > The Complete Nitrogen Cycle
> : > http://www.animalnetwork.com/fish/l...a&RecordNo=3090
> : >
> : > Magnesium (older article with fonts screwed up)
> : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : >
> : > Phosphate (older article now reproduced in a poor fashion)
> : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : >
> : > Carbon Dioxide
> : > http://www.animalnetwork.com/fish/l...a&RecordNo=2074
> : >
> : > Using Conductivity to Measure Salinity
> : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : >
> : > Understanding Seawater
> : > http://www.animalnetwork.com/fish2/...s/1/default.asp
> : >
> : > Protein Skimming: How It Works
> : > http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
> : >
> : >
> : >
> : > Articles by Craig Bingman:
> : >
> : > Carbon Dioxide tests
> : > http://www.animalnetwork.com/fish/l...n=&RecordNo=279
> : >
> : > Limewater, Acetic Acid and Sand Clumping
> : > http://www.animalnetwork.com/fish/l...n=&RecordNo=181
> : >
> : > Calcium and Alkalinity
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Calculation of Calcium Carbonate Saturation States in Reef Aquaria
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : >
> : > Calcification Rates in Several Tropical Coral Reef Aquaria
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Limits To Limewater...Revisited
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Expanding the Limits of Limewater: Adding Organic Carbon Sources
(vinegar)
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : >
> : > Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Magnesium - Part I
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Magnesium - Part II
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > A Homemade Magnesium Supplement
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Simulating the Effect of Calcium Chloride and Sodium Bicarbonate
Additions
> : on Reef Systems
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Additional Simulations: The Combined Effect Of Calcium Chloride
> : > /Sodium Bicarbonate Additions And Water Exchanges
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : >
> : > More articles by Craig Bingman:
> : >
> : > The Halogens - Part I: Bromine in Seawater and Aquaria
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > The Halogens - Part II: Fluoride
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Fluoride Depletion In Four Reef Aquariums
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > The Halogens - Part III: Iodine
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Measuring Halides
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > How Test Kits Work
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Borax pH Calibration
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > A pH Detective Story
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > How to Mix a Batch of Synthetic Seawater in Under Five Minutes
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > SILICON - FOE OR FRIEND?
> : > http://www.animalnetwork.com/fish2/...s/1/default.asp
> : >
> : > The Composition Of Several Synthetic Seawater Mixes
> : > http://www.animalnetwork.com/fish2/...s/1/default.asp
> : >
> : > Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : >
> : >
> : > Andy's calcium calculator
> : > http://www.andy-hipkiss.co.uk/cacalc.htm
> : >
> : > Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
> : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : >
> : > Calcium Reactor Substrate -- Phosphate Levels
> : > by Greg Hiller
> : > http://www.advancedaquarist.com/iss...l2003/short.htm
> : >
> : >
> : > Indoor CO2 Problems
> : > http://www.advancedaquarist.com/iss...r2002/short.htm
> : >
> : > Simon Huntington's CaCO3/CO2 reactor article
> : >
> : > http://reefkeeping.com/issues/2002-...ature/index.htm
> : >
> : > Ron Shimek's Tank Water Analysis Article
> : > http://reefkeeping.com/issues/2002-...ature/index.htm
> : >
> : >
> : >
> : >
> : > Home made salinity standards thread:
> : >
> : > http://reefcentral.com/forums/showt...?threadid=65509
> : >
> : > Reef Chemicals Calculator
> : > http://www.kademani.com/reefchem.htm
> : >
> : >
> : >
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : >
> : > Former US Army Bomb Technician (EOD)
> : > Member; IABTI, NATEODA, WEODF, ISEE & IPS
> : >
> : > If You See Me Running You Better Catch-Up
> : >
> : >
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : > "stoutman" <.@.> wrote in message
> : news:aGuWb.148227$U%5.676753@attbi_s03...
> : > : Boomer,
> : > :
> : > : I am not sure if you are just messing with me or if you are truly
> : confused.
> : > : I hope the latter. Please read from Top to Bottom.
> : > :
> : > :
> : > : From YOUR first link:
> : > :
> : > : http://www.waterontheweb.org/resources/glossary.html
> : > :
> : > : Acidity:
> : > : A measure of how acid a solution may be. A solution with a pH of
less
> : than
> : > : 7.0 is considered acidic. Solutions with a pH of less than 4.5
contain
> : > : mineral acidity (due to strong inorganic acids), while a solution
having
> : a
> : > : pH greater than 8.3 contains no acidity.
> : > :
> : > : Yes,
> : > :
> : > : Good definition (for the most part). pH <7 is indeed acidic. pH >
7 is
> : > : basic. Your web page had a definition for acidity, but not
basicity.
> : > : Strange. That's like defining GOOD and not defining BAD.
> : > :
> : > : Here is the IUPAC (International Union of Pure and Applied
Chemistry)
> : > : definition of acidity:
> : > :
> : > : http://www.chem.qmul.ac.uk/iupac/index.html
> : > :
> : > : acidity
> : > :
> : > : (1) Of a compound:
> : > :
> : > : For Brønsted acids it means the tendency of a compound to act as a
> : hydron
> : > : donor. It can be quantitatively expressed by the acid dissociation
> : constant
> : > : of the compound in water or some other specified medium. For Lewis
acids
> : it
> : > : relates to the association constants of Lewis adducts and -adducts.
> : > :
> : > : (2) Of a medium:
> : > :
> : > : The use of the term is mainly restricted to a medium containing
Brønsted
> : > : acids, where it means the tendency of the medium to hydronate a
specific
> : > : reference base
> : > :
> : > : basicity
> : > :
> : > : For Brønsted bases it means the tendency of a compound to act as
hydron
> : > : (proton) acceptor. The basicity of a chemical species is normally
> : expressed
> : > : by the acidity of the conjugate acid (see conjugate acid-base pair).
For
> : > : Lewis bases it relates to the association constants of Lewis adducts
> : > : and -adducts
> : > :
> : > :
> : > :
> : > : Another definition from the same web page YOU cited: (this is the
same
> : web
> : > : page you cited above)
> : > :
> : > : Alkalinity:
> : > : Acid neutralizing or buffering capacity of water; a measure of the
> : ability
> : > : of water to resist changes in pH caused by the addition of acids or
> : bases
> : > : and therefore, the main indicator of susceptibility to acid rain; in
> : natural
> : > : waters it is due primarily to the presence of bicarbonates,
carbonates
> : and
> : > : to a much lesser extent occasionally borates, silicates and
phosphates.
> : It
> : > : is expressed in units of milligrams per liter (mg/l) of CaCO3
(calcium
> : > : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l =
1
> : mg/l
> : > : of CaCO3. A solution having a pH below about 5 contains no
alkalinity.
> : > :
> : > : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and
says
> : > : that alkalinity is the measure of ...(description of a buffer)
> : > :
> : > : A BUFFER IS : a measure of the ability of water to resist changes in
pH
> : > : caused by the addition of acids or bases (from definition below)
> : > :
> : > :
> : > : I said:
> : > : ***alkalinity is a measurement of 'buffering capacity'***
> : > :
> : > : You said:
> : > : ***Alkalinity is not a measurement of BC
> : > :
> : > : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is
not
> : > : logical.
> : > :
> : > : (THIS FROM THE SAME WEB PAGE YOU CITED):
> : > :
> : > : Buffer:
> : > : A substance which tends to keep pH levels fairly constant when acids
or
> : > : bases are added.
> : > :
> : > : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
> : > :
> : > : a measure of the ability of water to resist changes in pH caused by
the
> : > : addition of acids or bases
> : > :
> : > : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A
BUFFER.
> : > :
> : > :
> : > : I went to all four links. None contradict what I have said. But
the
> : first
> : > : one you cited contradicts YOU!
> : > :
> : > : I know what a buffer is. I know what acidity means. I know what
> : alkalinity
> : > : means. No need to cite web pages that describe what I know and what
I
> : wrote
> : > : in this discussion. Show me one that says alkalinity is not a
measure
> : of
> : > : buffering capacity from a credible source.
> : > :
> : > :
> : > :
> : > :
> : > :
> : > :
> : > : "Boomer" > wrote in message
> : > : ...
> : > : > Alkalinity a measure of the amount of anions of weak acid in water
and
> : of
> : > : the cations
> : > : > balanced against them
> : > : > Take note it says ***acid***
> : > : >
> : > : > Buffering capacity the ability of a solution to resist or dampen
> : changes
> : > : in pH upon the
> : > : > addition of acids or bases.
> : > : > Take note its says ***the addition of acids or bases***
> : > : >
> : > : > One more
> : > : >
> : > : > http://www.waterontheweb.org/resources/glossary.html
> : > : >
> : > : > We could go on like this all day, so what is the point ?
> : > : >
> : > : > You will LOVE this one
> : > : > http://www.kyantec.com/Tips/phbuffering.htm
> : > : >
> : > : > Don't you just lovbe PDF's
> : > : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
> : > : >
> : > : > Don't fall out of your chair
> : > : >
http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
> : > : >
> : > : >
> : > : >
> : > : >
> : > : > --
> : > : > Boomer
> : > : >
> : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : >
> : > : > Want to See More ?
> : > : > Please Join Our Growing Membership
> : > : > www.coralrealm.com
> : > : >
> : > : > If You See Me Running You Better Catch-Up
> : > : > "stoutman" <.@.> wrote in message
> : news:XB7Wb.19339$QA2.62332@attbi_s52...
> : > : > : Man here is another, google is a wonderful thing. I'm not
filtering
> : any
> : > : > : out, just posting what I find by GOOGLING for you.
> : > : > :
> : > : > :
http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> : > : > :
> : > : > :
> : > : > : Wow, a gov link. Even the government is wrong, this must be a
> : > : conspiracy
> : > : > : against Boomer.
> : > : > :
> : > : > :
> : > : > :
> : > : > :
> : > : > : "Boomer" > wrote in message
> : > : > : ...
> : > : > : > Now I am getting bored
> : > : > : >
> : > : > : > "Don't the components of a buffer account for the buffering
> : capacity?
> : > : > : Yes."
> : > : > : >
> : > : > : > Yes, agreed but you seem to fail what I'm saying. Buffering
> : Capacity
> : > : and
> : > : > : Alkalinity are
> : > : > : > not the same, that has always been the issue. I gave the
equation
> : does
> : > : > : that look like an
> : > : > : > Alkalinity equation or how Alk is determined. I see you had
now
> : > : comments
> : > : > : on it what's
> : > : > : > wrong, why no comments on the equations I gave. Don't
understand
> : them
> : > : or
> : > : > : what ? Again this
> : > : > : > is the equation for Buffering Capacity, also called Buffer
Index
> : or
> : > : Buffer
> : > : > : Intensity. It
> : > : > : > is defined in most water chemistry and chemical oceanography
text
> : > : books.
> : > : > : >
> : > : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] +
[H30+] +
> : > : CKa
> : > : > : [H3O+] / (Ka =
> : > : > : > H3O+])² )
> : > : > : >
> : > : > : > This is not Alkalinity now is it ?
> : > : > : >
> : > : > : > "I know how to do a titration, In fact I have done several.
How
> : many
> : > : have
> : > : > : > you actually done? I don't mean by counting drops, I mean
with a
> : > : buret?"
> : > : > : >
> : > : > : > Well good for you, I use a Digital Titrator
> : > : > : >
> : > : > : > "Oh, I see,
> : > : > : > you think acidity is the opposite of alkalinity. In the world
of
> : > : > : CHEMISTRY
> : > : > : > it's not. Maybe in aquarium newsgroups it is.
> : > : > : >
> : > : > : > Hum no, maybe you should go for a look at HACH's or LaMotte
> : website or
> : > : the
> : > : > : book I
> : > : > : > suggested earlier. Please view a copy.
> : > : > : >
> : > : > : > Standard Methods for the Examination of Water and Wastewater
> : > : > : >
> : > : > : > This book, over 2000 pages, is the guide for water testing. If
you
> : are
> : > : > : reporting water
> : > : > : > test to the EPA you must use approved std from this text.I t
is
> : > : prepared
> : > : > : and published by
> : > : > : > the EPA, American Water Works Association and American Public
> : Health
> : > : > : Association. You
> : > : > : > mean you don't have one and the issue is water chemistry
> : > : > : >
> : > : > : > You are confusing Acidity and Acidity as you know little about
> : water
> : > : > : chemistry and
> : > : > : > procedures and test methods
> : > : > : >
> : > : > : > From SMEWW, section 2-30, 2310 ACIDITY
> : > : > : >
> : > : > : > "Acidity of water is its quantative capacity to react with a
> : strong
> : > : base
> : > : > : to a designated
> : > : > : > pH"
> : > : > : >
> : > : > : > This is how you test for it
> : > : > : >
> : > : > : > A std alkali titration to methyl orange or phenolphthalein
> : > : > : > endpoint.
> : > : > : >
> : > : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that
> : write
> : > : this
> : > : > : book, there are
> : > : > : > over 100 of them, they are wrong.
> : > : > : >
> : > : > : > Like Buffering Capacity you have your Acidity's mixed up
> : > : > : > In water measurement if you have a high Alk you also usually
have
> : a
> : > : high
> : > : > : Acidity.
> : > : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
> : > : CHEMISTRY
> : > : > : BOOK there pal.
> : > : > : >
> : > : > : >
> : > : > : > "These are all in equilibrium with each other. An initial
high pH
> : > : (above
> : > : > : > 6.4) will shift the equilibrium to the right to form HCO3-1.
If
> : the
> : > : pH of
> : > : > : > the solution is above 10.3 (pKa2) the .........."
> : > : > : >
> : > : > : >
> : > : > : > Christ, there you go again with the FW ****. All your numbers
are
> : > : wrong we
> : > : > : are dealing
> : > : > : > with SEAWATER
> : > : > : >
> : > : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is
in
> : the
> : > : form
> : > : > : > of HCO3-1 .
> : > : > : >
> : > : > : > I have already pointed that out and gave actual values at know
> : > : seawater
> : > : > : levels, go back
> : > : > : > and re-read it you aren't telling me anything here.Of course
most
> : is
> : > : HCO3
> : > : > : see...
> : > : > : >
> : > : > : >
> : > : > : > @ 20C and 34.3 ppt salinity
> : > : > : >
> : > : > : > CO2 = 0.52 %
> : > : > : >
> : > : > : > HCO3 = 86.4 %
> : > : > : >
> : > : > : > CO3 = 13.09 %
> : > : > : >
> : > : > : >
> : > : > : > "In your glass experiment you managed to lower the pH enough
to
> : purge
> : > : out
> : > : > : CO2
> : > : > : > by boiling"
> : > : > : >
> : > : > : > The purpose behind the glass is to show that alk is not affect
by
> : CO2
> : > : and
> : > : > : vise-versa and
> : > : > : > how Co2 affects pH.
> : > : > : >
> : > : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and
that
> : pH
> : > : drops
> : > : > : to say 8.1 it is
> : > : > : > usually due to excess CO2. If you took a glass of that water
and
> : > : aerated
> : > : > : it you WILL drive
> : > : > : > off the CO2 and raise the pH. It has been done a proven a
million
> : > : times.
> : > : > : >
> : > : > : > "In order to 'purge' CO2 you would need to lower the
> : > : > : > pH to shift the equilibrium to below 6.4"
> : > : > : >
> : > : > : > The hell you do !!!.Do you know who many times people on this
NG
> : to
> : > : > : include Dr. Craig
> : > : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned
to
> : take a
> : > : > : sample of aquarium
> : > : > : > water and aerate it to see if the pH GOES UP AND when they
come
> : back
> : > : with
> : > : > : the test it is
> : > : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D
CHEMIST
> : > : excess
> : > : > : CO2 in the tank
> : > : > : > water, increase the circulation for better gas exchange at the
> : > : surface,
> : > : > : reduce feeding,
> : > : > : > and try to improve on better skimming, thus reducing the
bio-load
> : and
> : > : pH
> : > : > : decline due to
> : > : > : > CO2.
> : > : > : >
> : > : > : >
> : > : > : > "I hope this helps. "
> : > : > : >
> : > : > : > Help, how can you when you miss everything. I should be
charging
> : you
> : > : > : >
> : > : > : > Oh, by the way. Your websites, I have about 50 on these
issues, I
> : > : could
> : > : > : post them, not to
> : > : > : > mention I have all those water chemistry books, so there is no
> : need to
> : > : > : view your sites.
> : > : > : >
> : > : > : > Finally are you afraid to come to our Chemistry Forum, afraid
to
> : get
> : > : > : slapped by REAL
> : > : > : > chemists. I get a charge out of you can't post your ref .I
have
> : posted
> : > : the
> : > : > : same or similar
> : > : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have
1500
> : > : posts
> : > : > : there and am the
> : > : > : > biggest contributor to his forum other than himself or maybe
Habib
> : > : Sheka
> : > : > : >
> : > : > : > Hum, here are Randy's ref that he posted. He hosts the website
> : > : > : >
> : > : > : > S. RANDY HOLMES-FARLEY
> : > : > : > Arlington, Massachusetts
> : > : > : >
> : > : > : > EDUCATION
> : > : > : >
> : > : > : > 1982-1986 Harvard University Cambridge, MA
> : > : > : > PhD in Chemistry
> : > : > : > Research Advisor: George Whitesides
> : > : > : >
> : > : > : > Investigated the relationship between polymer surface
chemistry
> : and
> : > : > : physical properties
> : > : > : > through controlled surface modification and testing.
> : > : > : >
> : > : > : > 1980-1982 Cornell University Ithaca, NY
> : > : > : > BA in Chemistry and Biology
> : > : > : > Graduated Summa Cum Laude
> : > : > : > Distinction in All Subjects
> : > : > : > Grade Point: 3.94/4.0
> : > : > : > Honors research: isolation and characterization of the subunit
of
> : CF1
> : > : > : enzyme
> : > : > : >
> : > : > : >
> : > : > : > 1978-1979 Stanford University Palo Alto, CA
> : > : > : > Grade Point: 3.55/4.0
> : > : > : >
> : > : > : >
> : > : > : > EXPERIENCE
> : > : > : >
> : > : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham,
MA
> : > : > : > (bought out GelTex Pharmaceuticals in 2001)
> : > : > : > Vice President, Chemical Research 2001-present
> : > : > : > Senior Director, Chemical Research 1999-2001
> : > : > : > Director of Chemical Research 1997-1999
> : > : > : > Manager of Chemical Research 1995-1997
> : > : > : > Group Leader 1994-1995
> : > : > : > Senior Research Scientist 1992-1994
> : > : > : >
> : > : > : > Helped start GelTex as second employee
> : > : > : >
> : > : > : > Managed various research programs with multi-million dollar
> : budgets
> : > : > : >
> : > : > : > Supervised research chemists (17+)
> : > : > : >
> : > : > : > Co-inventor of several polymeric pharmaceuticals and
> : pharmaceutical
> : > : > : candidates including
> : > : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam
> : Hydrochloride
> : > : (FDA
> : > : > : approved)
> : > : > : >
> : > : > : > Company Safety Officer for 3 years
> : > : > : >
> : > : > : > Chemical Hygiene Officer 2000-present
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > 1990-1992 GTE Corporation Waltham, MA
> : > : > : > Senior Member of Technical Staff
> : > : > : > Applied research involving polymer interfaces
> : > : > : > Metallization of plastics
> : > : > : > Polymer/polymer adhesion
> : > : > : > Optical coatings
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > 1986-1990 Lord Corporation Cary, NC
> : > : > : > Senior Research Scientist 1988-1990
> : > : > : > Research Scientist 1986-1988
> : > : > : > Basic and applied research on surface chemical bonding
> : > : > : > Developed new adhesive compositions
> : > : > : > Developed new sol-gel coatings for corrosion resistance
> : > : > : >
> : > : > : >
> : > : > : > HONORS AND AWARDS
> : > : > : >
> : > : > : > Industrial Innovations Award by Northeast Region of American
> : Chemical
> : > : > : Society (6/2001)
> : > : > : >
> : > : > : > National Kidney Foundation of Northern California Honoree
(5/2001)
> : > : > : >
> : > : > : > American Chemical Society/Polymer Chemistry Division
Industrial
> : > : Sponsors
> : > : > : > Award (8/2000)
> : > : > : >
> : > : > : > R&D 100 Award from R&D magazine (1999)
> : > : > : >
> : > : > : > Sherwin Williams Award in applied polymer science (9/85)
> : > : > : >
> : > : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985;
> : 1985-1986)
> : > : > : >
> : > : > : > Award for highest GPA in Chemistry Department (6/82)
> : > : > : >
> : > : > : > Summa Cum Laude Honors in Chemistry (6/82)
> : > : > : >
> : > : > : > Phi Lamda Epsilon (6/82)
> : > : > : >
> : > : > : > Phi Beta Kappa (2/82)
> : > : > : >
> : > : > : > Cornell University Dean's List (1981, 1982)
> : > : > : >
> : > : > : > Harvard Book Club Award for highest GPA senior year (1978)
> : > : > : >
> : > : > : > First Place in western NY ACS high school chemistry exam
(1977)
> : > : > : >
> : > : > : > 1978-1979
> : > : > : >
> : > : > : >
> : > : > : > __________________
> : > : > : > Randy Holmes-Farley
> : > : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef
> : Central
> : > : > : >
> : > : > : > Hobby Experience: 8 years with reefs
> : > : > : > Current Tanks: 90 gal mixed reef
> : > : > : > Interests: Reefkeeping, science, photography
> : > : > : >
> : > : > : >
> : > : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> : > : > : >
> : > : > : > Open this post in a new window | Report this post to a
moderator |
> : IP:
> : > : > : Logged
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > 06/27/2003 02:44 PM
> : > : > : >
> : > : > : > Randy Holmes-Farley
> : > : > : > Chemistry Moderator
> : > : > : >
> : > : > : > Registered: Apr 2001
> : > : > : > Location: Arlington, Massachusetts
> : > : > : > Occupation: Chemist (Drug Discovery at Genzyme)
> : > : > : > Posts: 15282
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > Publications
> : > : > : >
> : > : > : >
> : > : > : > ISSUED UNITED STATES PATENTS
> : > : > : >
> : > : > : >
> : > : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen
Randall;
> : > : > : Mandeville, III; W. Harry.
> : > : > : > US 6,566,407; 5/20/2003
> : > : > : >
> : > : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley,
Stephen
> : > : Randall;
> : > : > : Huval, Chad
> : > : > : > Cori.
> : > : > : > U.S. 6,517,825; 2/11/2003.
> : > : > : >
> : > : > : > 3. Method of making phosphate-binding polymers for oral
> : > : administration.
> : > : > : Holmes-Farley,
> : > : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M.
U.S.
> : > : > : 6,509,013; 1/21/2003.
> : > : > : >
> : > : > : > 4. Combination therapy for treating hypercholesterolemia using
a
> : bile
> : > : acid
> : > : > : sequestrant
> : > : > : > polymer
> : > : > : > and a cholesterol-lowering agent. Huval, Chad Cori;
Holmes-Farley,
> : > : Stephen
> : > : > : Randall;
> : > : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> : > : > : >
> : > : > : > 5. Method for treating hypercholesterolemia with
polyallylamine
> : > : polymers.
> : > : > : Holmes-Farley,
> : > : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
> : > : Goldberg,
> : > : > : Dennis I. , US
> : > : > : > 6,423,754; 7/23/2002.
> : > : > : >
> : > : > : > 6. Ionic polymers as anti-infective agents Mandeville, W.
Harry,
> : III;
> : > : > : Neenan, Thomas X..;
> : > : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> : > : > : >
> : > : > : > 7. Combination therapy for treating hypercholesterolemia and
> : > : > : atherosclerosis. Huval, Chad
> : > : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal,
> : Pradeep
> : > : K.
> : > : > : U.S. 6,365,186;
> : > : > : > 4/2/2002.
> : > : > : >
> : > : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
> : > : Mandeville,
> : > : > : W. H., III;
> : > : > : > Huval; C.
> : > : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US
6,299,868;
> : > : > : 10/9/2001.
> : > : > : >
> : > : > : > 9. Polymers containing guanidinium groups as bile acid
> : sequestrants.
> : > : Dhal;
> : > : > : P. K.; Holmes-
> : > : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> : > : > : >
> : > : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.;
Mandeville,
> : W.
> : > : H.,
> : > : > : III.; US
> : > : > : > 6,281,252;
> : > : > : > 8/28/2001.
> : > : > : >
> : > : > : > 11. Combination therapy for treating hypercholestrolemia.
Huval;
> : C.
> : > : C.;
> : > : > : Holmes-Farley; S.
> : > : > : > R. ;
> : > : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> : > : > : >
> : > : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides,
G.
> : M.;
> : > : > : Holmes-Farley, S.
> : > : > : > R.; US
> : > : > : > 6,264,937; 7/24/2001.
> : > : > : >
> : > : > : > 13. Method for treating hypercholesterolemia with
unsubstituted
> : > : > : polydiallylamine polymers.
> : > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
K.
> : ; US
> : > : > : 6,248,318;
> : > : > : > 6/19/2001.
> : > : > : >
> : > : > : > 14. Process for removing bile salts from a patient and
alkylated
> : > : > : compositions therefore.
> : > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355;
> : 5/1/2001.
> : > : > : >
> : > : > : > 15. Poly(diallylamine)-based bile acid sequestrants.
> : Holmes-Farley, S.
> : > : R.;
> : > : > : Dhal, P. K.;
> : > : > : > Petersen,
> : > : > : > J. S.; US 6,203,785; 3/20/2001.
> : > : > : >
> : > : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S.
R.;
> : > : Huval,
> : > : > : C. C.; US
> : > : > : > 6,190,649;
> : > : > : > 2/20/2001.
> : > : > : >
> : > : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.;
Mandeville,
> : W.
> : > : H.,
> : > : > : III.; US
> : > : > : > 6,177,478;
> : > : > : > 1/23/2001.
> : > : > : >
> : > : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
> : > : Holmes-Farley,
> : > : > : S. R.;
> : > : > : > Mandeville, W.
> : > : > : > H., III.; US 6,129,910; 10/10/2000.
> : > : > : >
> : > : > : > 19. Method for treating hypercholesterolemia with
unsubstituted
> : > : > : polydiallylamine polymers.
> : > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
K.
> : ; US
> : > : > : 6,083,497;
> : > : > : > 7/4/2000.
> : > : > : >
> : > : > : > 20. Method of making phosphate-binding polymers for oral
> : > : administration.
> : > : > : Holmes-Farley, S.
> : > : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US
6,083,495;
> : > : 7/4/2000.
> : > : > : >
> : > : > : > 21. Process for removing bile salts from a patient and
alkylated
> : > : > : compositions therefore.
> : > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
> : > : 5/23/2000.
> : > : > : >
> : > : > : > 22. Process for removing bile salts from a patient and
> : compositions
> : > : > : therefor. Mandeville,
> : > : > : > W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> : > : > : >
> : > : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III;
W.
> : H;
> : > : > : Neenan; T. X.; Holmes-
> : > : > : > Farley; S. R. US 6,034,129; 3/7/2000.
> : > : > : >
> : > : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.;
Mandeville,
> : W.
> : > : H.,
> : > : > : III.; US
> : > : > : > 5,985,938;
> : > : > : > 11/16/99.
> : > : > : >
> : > : > : > 25. Process for removing bile salts from a patient and
> : compositions
> : > : > : therefor. Mandeville,
> : > : > : > W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> : > : > : >
> : > : > : > 26. Hydrophobic sequestrant for cholesterol depletion.
Mandeville,
> : W.
> : > : H.,
> : > : > : III.;
> : > : > : > Holmes-Farley;
> : > : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> : > : > : >
> : > : > : > 27. Hydrophilic nonamine-containing and amine-containing
> : copolymers
> : > : and
> : > : > : their use as bile
> : > : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
> : > : 5,929,184;
> : > : > : 7/27/99.
> : > : > : >
> : > : > : > 28. Interpenetrating polymer networks for sequestration of
bile
> : acids.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US
> : 5,925,379;
> : > : > : 7/20/99.
> : > : > : >
> : > : > : > 29. Amine polymer sequestrant and method of cholesterol
depletion.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> : > : > : >
> : > : > : > 30. Process for removing bile salts from a patient and
> : compositions
> : > : > : therefor. Mandeville,
> : > : > : > W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> : > : > : >
> : > : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
> : depletion.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> : > : > : >
> : > : > : > 32. Process for removing bile salts from a patient and
> : compositions
> : > : > : therefor. Mandeville,
> : > : > : > W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> : > : > : >
> : > : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
> : > : Mandeville,
> : > : > : W. H., III.;
> : > : > : > Holmes-
> : > : > : > Farley, S. R.; US 5,703,188; 12/30/97.
> : > : > : >
> : > : > : > 34. Oral administration of iron-binding crosslinked amine
> : polymers.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> : > : > : >
> : > : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
> : Holmes-Farley,
> : > : S.
> : > : > : R.; US 5,693,675;
> : > : > : > 12/2/97.
> : > : > : >
> : > : > : > 36. Method for removing bile salts from a patient with
alkylated
> : > : > : crosslinked amine
> : > : > : > polymers,
> : > : > : > and preparation of the polymers. Mandeville, W. H., III.;
> : > : Holmes-Farley,
> : > : > : S. R.; US
> : > : > : > 5,679,717; 10/21/97.
> : > : > : >
> : > : > : > 37. Phosphate-binding polymers for oral administration.
> : Holmes-Farley,
> : > : S.
> : > : > : R.; Mandeville,
> : > : > : > W.
> : > : > : > H., III.; US 5,667,775; 9/16/97.
> : > : > : >
> : > : > : > 38. Ion-exchange process using highly crosslinked polymers for
> : > : removing
> : > : > : bile salts from a
> : > : > : > patient, preparation of the polymers, and compositions
containing
> : > : them.
> : > : > : Mandeville, W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> : > : > : >
> : > : > : > 39. Hydrophobic amine polymer sequestrant and method of
> : cholesterol
> : > : > : depletion. Mandeville,
> : > : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US
5,618,530;
> : > : 4/8/97.
> : > : > : >
> : > : > : > 40. Amine polymer sequestrant and method of cholesterol
depletion.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> : > : > : >
> : > : > : > 41. Phosphate-binding polymers for oral administration.
> : Holmes-Farley,
> : > : S.
> : > : > : R.; Mandeville,
> : > : > : > W.
> : > : > : > H., III.; US 5,496,545; 3/5/96.
> : > : > : >
> : > : > : > 42. Iron-binding polymers for oral administration. Mandeville,
W.
> : H.,
> : > : > : III.; Holmes-Farley,
> : > : > : > S. R.;
> : > : > : > US 5,487,888; 1/30/96.
> : > : > : >
> : > : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having
> : active
> : > : > : hydrogens on the
> : > : > : > surface.
> : > : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> : > : > : >
> : > : > : > 44. Layered sol-gel coatings from organisilicon compounds.
> : > : Holmes-Farley,
> : > : > : S. R.; Yanyo, L.
> : > : > : > C.;
> : > : > : > US 5,182,143; 1/26/93.
> : > : > : >
> : > : > : > 45. Method for metal bonding using ultrathin primer coating.
> : > : > : Holmes-Farley, S. R.; Yanyo,
> : > : > : > L.
> : > : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> : > : > : >
> : > : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.;
Abbey, K.
> : J.;
> : > : US
> : > : > : 5,096,962;
> : > : > : > 3/17/92.
> : > : > : >
> : > : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> : > : > : elastomer-metal bonding.
> : > : > : > Holmes-
> : > : > : > Farley, S. R.; US 5,102,956; 4/7/92.
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT
ISSUED)
> : > : > : >
> : > : > : >
> : > : > : > 1. Aryl boronate functionalized polymers for treating obesity
and
> : > : > : inhibiting fat uptake.
> : > : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III;
Dhal,
> : > : Pradeep
> : > : > : K.; Huval, Chad
> : > : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl.
(2003),
> : 92
> : > : pp. WO
> : > : > : 0302571.
> : > : > : >
> : > : > : > 2. Preparation of aryl boronic acids for treating obesity.
> : > : Holmes-Farley,
> : > : > : Stephen Randall;
> : > : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal,
> : Pradeep
> : > : K.
> : > : > : (Geltex
> : > : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO
> : 0302570.
> : > : > : >
> : > : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide.
> : Holmes-Farley,
> : > : > : Stephen Randall.
> : > : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32
pp.
> : WO
> : > : > : 0302130.
> : > : > : >
> : > : > : > 4. Method for reducing copper levels and treating copper
> : toxicosis.
> : > : > : Holmes-Farley, Stephen
> : > : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl.
> : (2002),
> : > : 45
> : > : > : pp. WO
> : > : > : > 0285383.
> : > : > : >
> : > : > : > 5. Method for treating gout and binding uric acid.
Holmes-Farley,
> : > : Stephen
> : > : > : Randall; Burke,
> : > : > : > Steven K. WO 0285381 10/31/2002.
> : > : > : >
> : > : > : > 6. Method for treating gout and reducing serum uric acid.
> : > : Holmes-Farley,
> : > : > : Stephen Randall;
> : > : > : > Burke, Steven K WO 0285380 10/31/2002.
> : > : > : >
> : > : > : > 7. Amine condensation polymer bile acid sequestrants. Huval,
C.
> : C.;
> : > : > : Holmes-Farley, S. R.;
> : > : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> : > : > : >
> : > : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H.,
III
> : and
> : > : > : Holmes-Farley, S.
> : > : > : > R.;
> : > : > : > WO 1999-US5662; 9/23/1999.
> : > : > : >
> : > : > : > 9. Amine-containing copolymers as bile acid sequestrants.
> : > : Holmes-Farley,
> : > : > : S. R.; Petersen,
> : > : > : > J. S.;
> : > : > : > WO 9933452; 7/8/1999.
> : > : > : >
> : > : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W.
H.,
> : III
> : > : and
> : > : > : Holmes-Farley, S.
> : > : > : > R.;
> : > : > : > WO 9922743; 5/14/1999.
> : > : > : >
> : > : > : > 11. Polyallylamine polymers for removing bile salts and
treating
> : > : > : hypercholesterolemia, and
> : > : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H.,
III;
> : > : Burke,
> : > : > : S. K.; Goldberg,
> : > : > : > D. I.; WO 9857652; 12/23/98.
> : > : > : >
> : > : > : > 12. Phosphate-bidning polymers combined with a calcium
supplement
> : for
> : > : oral
> : > : > : administration.
> : > : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
> : Holmes-Farley,
> : > : S.
> : > : > : R.; WO 9842355;
> : > : > : > 10/1/98.
> : > : > : >
> : > : > : > 13. Hydrophobic heteroatom-containing sequestrant for
cholesterol
> : > : > : depletion. Mandeville,
> : > : > : > W.
> : > : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449;
> : 12/12/96.
> : > : > : >
> : > : > : > 14. Process for adjusting ion concentration in a patient and
> : > : compositions
> : > : > : therefor.
> : > : > : > Mandeville,
> : > : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> : > : > : >
> : > : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
> : > : interlayer
> : > : > : for improved
> : > : > : > metal-
> : > : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
> : > : 1/20/94.
> : > : > : >
> : > : > : > 16. Process for increased metal-substrate bond strength in
> : metalized
> : > : > : plastics.
> : > : > : > Holmes-Farley, S.
> : > : > : > R.; Ger. Offen. 4322516; 7/6/93.
> : > : > : >
> : > : > : > 17. Electrorheological fluids and preparation of particles
useful
> : in
> : > : the
> : > : > : fluids.
> : > : > : > Troughton,
> : > : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie;
Carlson,
> : J.
> : > : > : David; Bares, Joseph
> : > : > : > E.;
> : > : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra
Nell.
> : EP
> : > : > : 394049;
> : > : > : > 10/24/1990.
> : > : > : >
> : > : > : > JOURNAL PUBLICATIONS
> : > : > : >
> : > : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William;
Zhorov,
> : > : Eugene;
> : > : > : Guo, Amy;
> : > : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David
L.;
> : > : > : Mandeville, W. Harry;
> : > : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
> : > : 611-619.
> : > : > : >
> : > : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
> : > : synthesis
> : > : > : and biological
> : > : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley,
S.
> : > : Randall;
> : > : > : Mandeville, W.
> : > : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal,
Pradeep
> : K.
> : > : > : Journal of
> : > : > : > Macromolecular Science, Pure and Applied Chemistry (2001),
> : A38(12),
> : > : > : 1559-1574.
> : > : > : >
> : > : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by
> : Molecular
> : > : > : Imprinting. Huval,
> : > : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.;
Holmes-Farley,
> : S.
> : > : > : Randall; Mandeville,
> : > : > : > W.
> : > : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro,
> : Robert
> : > : J.;
> : > : > : Chen, Xi; Dhal,
> : > : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> : > : > : >
> : > : > : > 4. Synthetic polymers for the binding of fat in the intestinal
> : tract.
> : > : > : Jozefiak, Thomas H.;
> : > : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny,
Cynthia;
> : > : Huval,
> : > : > : Chad C.;
> : > : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney,
Cynthia.
> : > : > : Abstracts of
> : > : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United
States,
> : August
> : > : > : 26-30, 2001
> : > : > : > (2001), POLY-047 and Polymer Preprints (American Chemical
Society,
> : > : > : Division of
> : > : > : > Polymer Chemistry) (2001), 42(2), 98.
> : > : > : >
> : > : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel
> : polymer
> : > : gel
> : > : > : pharmaceutical.
> : > : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.;
Petersen,
> : J.;
> : > : Ward,
> : > : > : J.; Sacchiero,
> : > : > : > B.;
> : > : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton,
K.
> : A.;
> : > : Chen,
> : > : > : X.; Mazzeo, J.
> : > : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
> : > : > : >
> : > : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl
and
> : > : other
> : > : > : bile acid
> : > : > : > sequestrants.
> : > : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.;
Xu,
> : Q.;
> : > : > : Hook, P.; Holmes-
> : > : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1),
> : 708-709.
> : > : > : >
> : > : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
> : > : Holmes-Farley,
> : > : > : S. R; Polym.
> : > : > : > Mater. Sci. Eng (1999), 80, 246-247.
> : > : > : >
> : > : > : > 8. Design and characterization of of Sevelamer Hydrochloride:
a
> : novel
> : > : > : phosphate-binding
> : > : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III;
> : Ward,
> : > : J.;
> : > : > : Miller, K. L.;
> : > : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M.
S.-
> : Pure
> : > : and
> : > : > : Appl. Chem.,
> : > : > : > A36(7&8), p. 1085 (1999).
> : > : > : >
> : > : > : > 9. Three generations of bile acid sequestrants. Mandeville, W.
H.,
> : > : III;
> : > : > : Braunlin, W.;
> : > : > : > Dhal, P.;
> : > : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik,
S.;
> : > : > : Rosenbaum, D.;
> : > : > : > Sacchiero,
> : > : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc.
> : (1999),
> : > : > : 550, 3-15.
> : > : > : >
> : > : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked,
polymeric
> : > : phosphate
> : > : > : binder, on
> : > : > : > urinary
> : > : > : > phosphorous excretion in rats. Rosenbaum, D. P.;
Holmes-Farley, S.
> : R.;
> : > : > : Mandeville, W. H.,
> : > : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
> : Transplant.
> : > : > : (1997), 12(5)
> : > : > : > 961-964.
> : > : > : >
> : > : > : > 11. Thin anisotropic coatings based on sol-gel technology.
> : > : Holmes-Farley,
> : > : > : S. R.; Yanyo, L.
> : > : > : > C;
> : > : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem.
4),
> : > : 439-444.
> : > : > : >
> : > : > : > 12. The mechanism of cure initiation of a surface activated
> : adhesive.
> : > : > : Holmes-Farley, S.
> : > : > : > R.;
> : > : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5),
409-420.
> : > : > : >
> : > : > : > 13. Adhesion promotion and corrosion prevention using thin
> : anisotropic
> : > : > : coatings. Holmes-
> : > : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991),
5(2),
> : > : > : 131-151.
> : > : > : >
> : > : > : > 14. Wetting of functionalized polyethylene having ionizable
> : organic
> : > : acids
> : > : > : and bases at the
> : > : > : > polymer-water interface: relations between functional group
> : polarity,
> : > : > : extent of
> : > : > : > ionization,
> : > : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C.
D.;
> : > : > : Whitesides, G. M.;
> : > : > : > Langmuir
> : > : > : > (1988), 4(4), 921-937.
> : > : > : >
> : > : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols
with
> : a
> : > : > : single hydroxy group.
> : > : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> : > : > : >
> : > : > : > 16. Reconstruction of the interface of oxidatively
functionalized
> : > : > : polyethylene (PE-CO2H)
> : > : > : > and
> : > : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.;
> : Nuzzo,
> : > : R.;
> : > : > : McCarthy, T. J.;
> : > : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also
Report
> : > : (1987),
> : > : > : AD-
> : > : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> : > : > : >
> : > : > : > 17. Surface-modified polyethylene film: the relationship
between
> : > : surface
> : > : > : chemistry and
> : > : > : > physical
> : > : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987,
47(11),
> : > : 4537.
> : > : > : >
> : > : > : > 18. Reactivity of carboxylic acid and ester groups in the
> : > : functionalized
> : > : > : interfacial
> : > : > : > region of
> : > : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> : > : > : differentiation of the
> : > : > : > functional groups into shallow and deep subsets based on a
> : comparison
> : > : of
> : > : > : contact angle and
> : > : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.;
> : Langmuir
> : > : > : (1987), 3(1), 62-
> : > : > : > 76.
> : > : > : >
> : > : > : > 19. Fluorescence properties of dansyl groups covalently bonded
tot
> : he
> : > : > : surface of
> : > : > : > oxidatively
> : > : > : > functionalized low-density polyethylene film. Holmes-Farley,
S.
> : R.;
> : > : > : Whitesides, G. M.;
> : > : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985),
TR-85-2;
> : > : > : AD-A162435/2/GAR,
> : > : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> : > : > : >
> : > : > : > 20. Acid-base behavior of carboxylic acid groups covalently
> : attached
> : > : at
> : > : > : the surface of
> : > : > : > polyethylene: The usefulness of contact angle in following the
> : > : ionization
> : > : > : of surface
> : > : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy,
T.
> : J.;
> : > : > : Deutch, J.;
> : > : > : > Whitesides,
> : > : > : > G. M.; Langmuir (1985), 1(6), 725-740.
> : > : > : >
> : > : > : > 21. The thermal stability of a surface modified solid organic
> : polymer.
> : > : > : Holmes-Farley, S.
> : > : > : > R.;
> : > : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53,
127-131.
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> : > : > : >
> : > : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R.
> : Advanced
> : > : > : Aquarist. June 2003.
> : > : > : >
> : > : > : > 2. The Self Purification of Limewater (Kalkwasser).
Holmes-Farley,
> : R.
> : > : > : Advanced Aquarist.
> : > : > : > May
> : > : > : > 2003.
> : > : > : >
> : > : > : > 3. The Degradation of Limewater (Kalkwasser) in Air.
> : Holmes-Farley, R.
> : > : > : Reefkeeping May
> : > : > : > 2003.
> : > : > : >
> : > : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
> : Reefkeeping
> : > : > : April 2003.
> : > : > : >
> : > : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae
Growth.
> : > : > : Holmes-Farley, R.
> : > : > : > Advanced Aquarist; April 2003.
> : > : > : >
> : > : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae
Growth.
> : > : > : Holmes-Farley, R.
> : > : > : > Advanced Aquarist; April 2003.
> : > : > : >
> : > : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R.
Advanced
> : > : Aquarist;
> : > : > : March 2003.
> : > : > : >
> : > : > : > 8. How to Select a Calcium and Alkalinity Supplementation
Scheme.
> : > : > : Holmes-Farley, R.
> : > : > : > Advanced Aquarist; February 2003.
> : > : > : >
> : > : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> : January
> : > : > : 2003.
> : > : > : >
> : > : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> : > : December
> : > : > : 2002.
> : > : > : >
> : > : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
> : > : Advanced
> : > : > : Aquarist; November
> : > : > : > 2002.
> : > : > : >
> : > : > : > 12. Iron: A Look at Organisms Other than Macroalgae.
> : Holmes-Farley, R.
> : > : > : Advanced Aquarist;
> : > : > : > November 2002.
> : > : > : >
> : > : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.;
Advanced
> : > : Aquarist,
> : > : > : September 2002.
> : > : > : >
> : > : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist,
> : August
> : > : > : 2002.
> : > : > : >
> : > : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.;
Reefkeeping.com,
> : April
> : > : > : 2002.
> : > : > : >
> : > : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R.
Advanced
> : > : > : Aquarist; July 2002
> : > : > : >
> : > : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced
Aquarist;
> : > : June
> : > : > : 2002.
> : > : > : >
> : > : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley,
R.
> : > : Advanced
> : > : > : Aquarist, May
> : > : > : > 2002.
> : > : > : >
> : > : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in
> : Corals.
> : > : > : Holmes-Farley, R.
> : > : > : > Advanced Aquarist, April 2002.
> : > : > : >
> : > : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> : > : > : >
> : > : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February
> : 2002.
> : > : > : >
> : > : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist,
January
> : > : 2002.
> : > : > : >
> : > : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium
> : Frontiers
> : > : > : 2000.
> : > : > : >
> : > : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R.
Aquarium
> : > : > : Frontiers 2000.
> : > : > : >
> : > : > : > 25. Phosphate..What is it and why should you care.
Holmes-Farley,
> : R.
> : > : > : Aquarium Frontiers
> : > : > : > 2000.
> : > : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
> : > : Frontiers
> : > : > : 2000.
> : > : > : >
> : > : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium
Frontiers
> : > : 2000.
> : > : > : >
> : > : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium
Frontiers
> : 1999.
> : > : > : >
> : > : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > Boomer
> : > : > : >
> : > : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : > : >
> : > : > : > Want to See More ?
> : > : > : > Please Join Our Growing Membership
> : > : > : > www.coralrealm.com
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > :
> : > : > :
> : > : >
> : > : >
> : > :
> : > :
> : > :
> : >
> : >
> :
> :
>
>

[stoutman]

One more thing.

> No it is not a measurement of BUFFERING CAPACITY, it is a indication of
BC. I have said
> this at least twice.

I just checked. You NEVER said:

Alkalinity was an indication of buffering capacity until this post.

In fact, you never use the word INDICATION until this post.

I did a keyword search on indication and Boomer.


"Boomer" > wrote in message
...
> Yes, of cause I remember, as I said I posted it for a reason. I see you
have used only
> that link for your definition, as it makes you look right.You have avoided
all Alk
> definitions in a chemistry book, to include your own definition *****to
resist a drop in
> pH due to the addition of acid***, which is the same as the others I
posted .Agreed, of
> course not.You know that Alk isn't defined as "by the addition of acids or
bases "and is
> only the " addition of an acid", so why are you accepting the definition
?.You know that
> when you titrate it is an acid added and never a base. In one breath it
says Alk is "Acid
> neutralizing " and then they say "by the addition of acids or bases ".You
can't have it
> both ways and YOU know that Agreed . If the word "base" was left out I
would not have much
> to say. Agreed
>
>
> "Alkalinity is a
> measurement of BUFFERING CAPACITY."
>
> No it is not a measurement of BUFFERING CAPACITY, it is a indication of
BC. I have said
> this at least twice. If you know your BC you can calculate Alk and if you
can do one you
> can do the other agreed. What I have tried to convey from the beginning is
that Alk and BC
> are not the same thing. You in one of your other posts have said they are
not the same
> thing and never said they were. Now you seem to be saying they are the
same thing
>
> "So, when we measure ALKALINITY (and we know the pH) we are in effect
> measuring BUFFERING CAPACITY.
>
> More or less YES in an "effect" but Alk tells you not much of anything
when a base is
> added Agreed. That is called Acidity, which I see you have avoided again
as if there is
> no such thing. I also said that for us the only thing we need to be
concerned about is
> Alk, so BC would fit in, as we could care less about the ability to
neutralize a base or
> measure Acidity. So, if you knew your pH , Alk or Acy you would really
know what you BC is
> doing for you Agreed.
>
> On Bc, we have both left something from my first equation, so I thought I
would post it
> again for you, as I like being honest .I'm surprised you didn't catch it
:-)
>
> B = dCb / dpH = - dCa / dpH
>
> So;
>
> B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> or
>
> B (Buffering Capacity) = - dCa / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
[H3O+] / (Ka =
> H3O+])² )
>
> There are number of was to mathematically express BC. Two of the most
common are the
> change in Alk with the pH at constant total carbonate, the other is change
in Alk with pH
> constant CO2 pp. In some examples of Bc, Bc is the inverse slope of the
Alk titration
> curve ( I'm sure yo
> u will love this) In the other over the pH range, while BC is going
through minimum, Bpp
> increases linearly. This difference is caused by the uptake of CO2 by the
solution, which
> increases Ct as pH increases.To bad we can't or my server won't allow me,
to post
> attachments. I have a nice BC cure of various species as a function of
pC/pH diagrams, set
> to a pKa. curve
>
>
> On another issue
>
> "In order to remove CO2 (g) you ideally would want to shift
> the equilibrium to the left by LOWERING the pH"
>
>
> You may want to try and re-explain this
>
> CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
> HCO3-1 <-------> CO3-2
>
>
> As the reaction shifts to left the pH gets higher as CO2 leaves the
system.You don't have
> to lower the pH to remove CO2. Case in point plants. As they remove CO2
the pH rises,
> continued removal of the Sigma CO2 ( CO2, H2CO3, HCO3,CO3) cause further
rising until
> there is mostly only carbonate (CO3) left and a high pH. Another case, at
a pH of 8.00 and
> Alk of 4 meq / l ( 1.4 mg / l CO2) you have much more CO2 than at 2 meq/
l (0.65mg / l).
> . Aeration of the water can drive off the CO, no lowering of the pH
required., the removal
> will cause the pH to rise .On the other hand, trying to remove CO2 @ 2 meq
/ l won't get
> you much of anywhere in this case. Also, even a low pH doesn't mean you
can drive of CO2.
> If the seawater pH was say 7.5, you would think not problem to drive off
CO2. If the Alk
> was 0.25 there would be about .35 mg / l CO2 to blow off. At the alk of
4.00 meq / l the
> CO2 is 5 mg / l.Usually, when people have a lower pH, say 7.9 or so, it is
do to CO2, so
> the pH has lowered, increasing the CO2, to allow one to blow it off easier
and bring the
> pH back up.
>
> CO2 = [CA(Carbonate Alk) x aH ] / [pK1(1 + 2pK2 /aH)]
>
> I think we just got off on the wrong foot, hope things look better.
>
> I'll be gone for the weekend, leaving in an hour, so have a nice weekend
:-)
>
>
>
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message news:lcRWb.299984$na.451117@attbi_s04...
> : > Humm, since when does Alk have anything to do in regards to the
addition
> : of BASE.
> :
> : You tell me. Your the one that posted a link to a web page that had
this
> : definition of alkalinity. Looks like you put yourself in your own hole
pal.
> :
> : Remember posting this link:
> :
> : http://www.waterontheweb.org/resources/glossary.html
> :
> : Here is the definition of alkalinity from the web page YOU cited. (I
> : recommend you read the web pages you are citing before you cite them)
> : Alkalinity:
> : Acid neutralizing or buffering capacity of water; a measure of the
ability
> : of water to resist changes in pH caused by the addition of acids or
BASES.
> :
> :
> : > It sure is funny how all of the chemist that write water chemistry
> : textbooks never say Alk
> : > is the Buffering Capacity of a solution.
> :
> : Neither did I. I said (for the umpth teen time) Alkalinity is a
> : measurement of BUFFERING CAPACITY.
> :
> : When you measure alkalinity you know your BUFFERING CAPACITY (if you
know
> : your pH). Its a two for one.
> :
> : SEE MY OTHER POST FROM TODAY.
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : >
> : > "I am not sure if you are just messing with me "
> : >
> : > Yes, messing with you, it is called trolling a troll, to see where the
> : hell you would go
> : > and what you would say in regards to last posts. It is called honesty,
of
> : which you have
> : > none off to say the least,that I can see.You always like to post what
> : suits you and just
> : > avoid ref I give. So lets start where you are WRONG and have a great
lack
> : of understanding
> : > of things, to include pointing out all your gross error which you
still
> : FAIL to
> : > acknowledge and which can be prove in many water chem. ref. .I doubt
like
> : hell you are a
> : > chemist at all.You seem to want to con people into thinkin' you are.
But
> : then again, I
> : > have seen chemists like you before, they are not familiar with the,
but
> : they ASK to have
> : > it explained and ask for REF.YOU just shoot from the hip. WHAT GETS
YOU IN
> : TROUBLE. You
> : > remind me of snoot-noise kid that come here and other NG's and
> : forums...that think they
> : > know, buy hey, maybe I'm wrong :-)
> : >
> : >
> : >
> : > 1). Acidity
> : >
> : > "***Benjamin,Water Chemistry (2002, pages 262-263).***
> : >
> : > ***Acidity A concept that is exactly analogous to alkalinity but
measures
> : the base
> : > neutralizing
> : > capacity (BNC) of a solution is Acidity. The quantitative represents
the
> : concentration of
> : > OH- ions that must be added to titrate the solution to a pH near
10.5***
> : >
> : > So that means that not only in Benjamin wrong but, so are Stumm &
Morgan,
> : Millero, Pilosn,
> : > Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I
> : said, you have your
> : > acidity and Acidy mixed up. Acidity as defined above is covered in
most
> : water chemistry
> : > books, written by chemists, who's field of expertise is water
chemistry.
> : You can even buy
> : > Acidity test kits from, HACH, LaMotte, etc..
> : >
> : > You mean you didn't read this or are you just avoiding it .The same
> : definition can be
> : > found in almost any std water chemistry book.
> : >
> : > I have run into few chemists, that are NOT familiar with the above.
Some
> : water reports
> : > require the above Acidity measuring. The issue with you is you do not
> : understand WATER
> : > CHEMISTRY. Everything you have posted can be found a general chemistry
> : book
> : >
> : >
> : >
> : >
> : > 2) Alk and BC
> : >
> : > From the link
> : >
> : > Alkalinity
> : > ***Acid neutralizing or buffering capacity of water; a measure of the
> : ability of water to
> : > resist changes in pH caused by the addition of acids or bases ***
> : >
> : > This is a Buffering Capacity definition not Alk
> : >
> : > Humm, since when does Alk have anything to do in regards to the
addition
> : of BASE. As I
> : > pointed out in the first post the term is often miss used. Even in
YOUR
> : own posts you say
> : > it is based on a acid addition, no mention of **base or acid**
addition
> : by you. Are you
> : > getting confused or what. Or is more you are trying to confuse
everyone
> : you are right. The
> : > above is a definition for Buffer Capacity NOT Alk
> : >
> : > From Drew, Geochemistry of Natural Waters
> : >
> : > "alkalinity, which is formally defined as the equivalent sum of bases
that
> : are titratable
> : > with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH
of
> : the solution is
> : > progressively lowered by the addition of a strong acid (HCL), all the
> : anions on the right
> : > will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4,
H2S,organic
> : acids, H20)"
> : >
> : > This follows almost all description of Alk, that it is acid
neutralizing
> : reaction and has
> : > nothing to do with base neutralizing, which is Acidity (BNC) .I
defined
> : these before you
> : > had no comment
> : >
> : >
> : > Even the links that give the Buffering Capacity definition is wrong,
as is
> : the UIPAC on
> : > Alkalinity. Alkalinity has nothing to do with the addition of bases
only
> : acids. When you
> : > use the words "base and acid" it becomes BC
> : >
> : > Even YOU MUST disagree with these definitions, from YOUR own post
> : >
> : > Think of alkalinity as 'buffering capacity'. Or the ability of a
solution
> : > ***to resist a drop in pH due to the addition of acid***
> : >
> : > Where the flip is the base addition forget it ?
> : >
> : > From Butler; Carbon Dioxide Equilibrium and Their Applications
(professor
> : emeritus
> : > Harvard University) an expert on the subject.
> : >
> : > Buffering Index (Buffering Capacity, Buffer Intensity).
> : >
> : > ***This concept was first developed for mixtures of approximately
equal
> : proportions of
> : > conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such
> : buffer solutions
> : > strongly resist changes in pH when acids or bases are added and are
useful
> : as pH
> : > standards. The Buffer Index tells how great the resistance to pH
changes
> : will be.**
> : >
> : > also from Butler
> : >
> : > Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
> : >
> : > Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
> : >
> : > Acidity is in fact just the negative of Alkalinity ***
> : >
> : > http://www.lagoonsonline.com/acid.htm
> : >
> : >
> :
http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.h
> : tm?E+mystore
> : >
> : > It sure is funny how all of the chemist that write water chemistry
> : textbooks never say Alk
> : > is the Buffering Capacity of a solution. They are always treated and
> : defined separately.
> : >
> : > If you or others choose to treat Alk and BC as the same, well, just
have
> : at it. As I said
> : > in first post I know what you mean.
> : >
> : > "No need to cite web pages that describe what I know and what I wrote
> : > in this discussion"
> : >
> : > No you don't know, who are you trying to convince any way, me, the
guys
> : here and/or all
> : > the water chemists in this world. As I said before go get a dam WATER
> : CHEMISTRY book or
> : > shut the hell up.You keep trying to define things from a general
chemistry
> : book WE ARE IN
> : > THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
> : >
> : >
> : >
> : >
> : >
> : > 3). pKa's and what you don't know or seem to be confused on
> : >
> : > "Therefore, it has two pKa's
> : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
> : The
> : > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated
is
> : > right in there. Is that magic? :)"
> : >
> : > Here it is agin that is twice at least
> : >
> : > "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this
> : example)
> : > you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium
will
> : > be shifted to HCO3-2 by a ratio of 1:100.
> : >
> : > Oh wait , there is a third time LOL
> : >
> : > "At the pH of seawater, the buffering capacity of carbonate is at it's
> : > weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
> : >
> : >
> : > Lets just dunk you on this one. I am taking note you refuse to reply
to
> : YOUR errors
> : >
> : > So you calculated the pH of seawater with freshwater pKa's, now that
is a
> : good trick. From
> : > a number of seawater chemistry books the seawater pKa's are 6 & 9.1,
so
> : according to you,
> : > seemingly not understanding your favorite Henderson-Hasselbach
equation;
> : >
> : > 2 pH = (6 + 9.1) /2 pH = 7.55
> : >
> : > I have never seen seawater with a pH of 7.55. There is no ocean with
that
> : pH. Humm how
> : > come your equation is not working for you today.?
> : >
> : >
> : > "That pH I calculated is
> : > right in there. Is that magic? :)"
> : >
> : > I roll on the floor when I see this = 8.35
> : >
> : > Hum , just a brain far so excuse me for thinkin
> : >
> : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
> : >
> : > Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a
pH of
> : 8.35 there pal
> : > ? That 8.35 is what you are telling people the pH should be, but their
> : meter says 6.4.
> : > This how people will READ this.
> : >
> : >
> : >
> : >
> : > 4.) More on Buffering Capacity
> : >
> : > "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes,
your
> : > alkalinity equation."'
> : >
> : >
> : > Yup, I see that and in this case the HCO3 is the acid and the CO3 is
the
> : base CORRECT. In
> : > Alk you are only dealing with bases and how they react to an acid.
Acidity
> : deals acids and
> : > how they recact to bases "Acidity, A concept that is exactly analogous
to
> : alkalinity but
> : > measures the base neutralizing
> : > capacity (BNC) of a solution is Acidity "Alk is the ANC Acid
neutralizing
> : capacity
> : >
> : > "Don't the components of a buffer account for the buffering capacity?
"
> : >
> : > Yes, they do but so do the acids which work as buffers. NaHCO3 is a
buffer
> : and can act as
> : > an acid or base
> : >
> : > *** Buffering Capacity.**
> : > The power of a substance in solution to absorb acid or alkali without
> : change in pH; this
> : > is highest at a pH value equal to the pKa value of the acid of the
buffer
> : pair.***
> : >
> : > ***Akalinity***
> : > Measure of the power of a solution to neutralise hydrogen ions (H+),
> : usually expressed as
> : > the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
> : >
> : >
> : > If one wants to call Alk Buffering capacity then one sure as a hell
can
> : call Acidty
> : > Buffering Capacity also. As it is the ability to neutralizes an acid
that
> : is a buffer.You
> : > have a pH of 7 and you add a buffer to lower it to a pH of 4, you are
> : buffering the water,
> : > that buffer is a acid.
> : >
> : > 5) CO2
> : >
> : > You are really confuse so it seems :-) You realllllllly indicate that
CO2
> : is affected by
> : > the Alk or vise-versa
> : >
> : > "Yes, the pH will drop with the addition of CO2. Remove CO2 will
cause
> : the
> : > pH to rise? How do you remove CO2? Once it is in solution it forms
> : > carbonic acid and neutralizes some of your 'buffer'."
> : >
> : > "With the exception of CO2?"
> : >
> : > No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
> : > Concepts)....PERIOD.You seem to think a that at least in two of your
post
> : that CO2 is
> : > affected by the Alk or vise-versa. Please go back to school or seek
> : professor
> : >
> : > "Why in one case does CO2 from air lower pH and in the other case it
> : raises
> : > it? Doesn't make sense."
> : >
> : > That is because you don't understand CO2 period. By the way I saved
this,
> : wanted to see
> : > if you would bite on the post I gave. Not bite at first, so time to
reel
> : you in, as you
> : > did bite in another post..
> : >
> : > Lets make some sense of it for you, being that you have a pH.D in
> : chemistry, so you say .
> : >
> : > CO2 is naturally generated in a aquatic systems, it is capable of
raise to
> : various levels
> : > depending on a number of circumstances .It can be measure (except in
> : seawater) or
> : > calculated using Buch/Park Equations (what we use for seawater. In
sort if
> : you know the pH
> : > and Alk you can calculate the CO2). If you aerate a system or a sample
of
> : water, even if
> : > the pH has only dropped a couple of tenths, due to an increase in CO2,
the
> : CO2 will leave
> : > solution to the atmosphere.This will raise the pH. On the other hand
if
> : theCO2 level is
> : > more of the norm and you have hikgh room air, such as in the winter,
the
> : partial pressure
> : > of the CO2 in air will be much higher than that in water, in which
case
> : the CO2 will enter
> : > the water and lower the pH. That is without an airstone. Adding an
> : airstone will make it
> : > even worse,as you are now forcefully driving the CO2 into solution
even
> : quicker. These
> : > test /experiments have been proven many times, it is not that may work
> : could work they do
> : > work.Yet you want to disagree and in another post say you haven't
tried
> : it,.Seems to me
> : > that based on what you say it can't work So, in short you don't know
what
> : the hell you are
> : > taking about. Go get a glass of seawater with a pH of about 8.3 and
lower
> : it to about
> : > 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK-
UP
> : ( that is if you
> : > don't have a high room air CO2 problem.). This little test has been
done
> : thousands of
> : > times in this hobby, with test kits, pH meters and even graphic
printers.
> : >
> : > "This is where Boomer and I
> : > disagree. I say you would have to lower the pH very low in order to
> : > effectively remove CO2 by purging."
> : >
> : > You are 100 % wrong. Please come to our Chem forum and try and run
that by
> : Randy, don't
> : > take my word on it. I already know what he will say.
> : >
> : > "Boomer didnt convince me it
> : > works at the pH of an aquarium, but I never tried it and I'm not sure
of
> : > this. "
> : >
> : > Well then come too our chem. forum and tell Randy he doesn't know what
he
> : is talking about
> : > LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it
> : should be easy for
> : > you to run the experiment LOL There are grade school kids that run the
> : test and know what
> : > happens and that I'm correct.
> : >
> : >
> : > "The equilibrium is a FUNCTION
> : > of pH."
> : >
> : > It is also a function of Alk or don't you know that. At a pH of 8.3,
Alk
> : 2.25, the CO2 is
> : > about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk
to
> : about .4 meq/ l
> : > or so the CO2 will be around .99 mg / l CO2, When dealing with
tanksCO2 is
> : not always in
> : > equilibrium with ambient air.
> : >
> : >
> : > ". But I wouldn't degas a solution of a
> : > specific gas (CO2) with a gas (this case he was using air) that
contains
> : the
> : > same gas I am trying to purge."
> : >
> : > Why not ? We have a guy right now that is running tests on purging
ambient
> : air with a
> : > solution to remove CO2 gas from the air, before it enters the tank
> : per/Randy's suggestion.
> : > The same guy is doing some of my test using a Clinoptilolite, a
Zeolite
> : mineral, that has
> : > an affinity for CO2.This will be a dry CO2 scrubber
> : >
> : >
> : > Sorry Soutman but you sure as hell don't seem to know much about
aquatic
> : chemistry. You
> : > seem to be guessing at everything.
> : >
> : > By the way have you read any of Randy's technical articles on water
> : chemistry, been saving
> : > these for last. There are a few on pH, Alk, CO2 .Here is a list
> : >
> : > Try and answer them 1-5 and lets see where we get THIS TIME :-) or
maybe
> : we should just
> : > drop it. I could care less at this point.
> : >
> : > THE END
> : >
> : >
> : > ARTICLES
> : >
> : > The first two posts in this thread are lists of some of my articles
that
> : relate to reef
> : > tank chemistry. In the next few posts are some of the articles
published
> : by Craig Bingman
> : > and others on reef chemistry issues.
> : >
> : > The first two posts in this thread are lists of some of my articles
that
> : relate to reef
> : > tank chemistry. In the next few posts are some of the articles
published
> : by Craig Bingman
> : > and others on reef chemistry issues.
> : >
> : > Solving Common Problems
> : >
> : > Solving Calcium and Alkalinity Problems
> : > http://www.advancedaquarist.com/issues/nov2002/chem.htm
> : >
> : > Solutions to pH Problems
> : > http://www.advancedaquarist.com/iss...ne2002/chem.htm
> : >
> : > How to Select a Calcium and Alkalinity Supplementation Scheme
> : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
> : >
> : > Phosphate Issues
> : > http://www.advancedaquarist.com/iss...pt2002/chem.htm
> : >
> : > Nitrate Issues
> : > http://www.advancedaquarist.com/iss...st2003/chem.htm
> : >
> : >
> : >
> : > Calcium and Alkalinity
> : >
> : > Solving Calcium and Alkalinity Problems
> : > http://www.advancedaquarist.com/issues/nov2002/chem.htm
> : >
> : > How to Select a Calcium and Alkalinity Supplementation Scheme
> : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
> : >
> : > Calcium and Alkalinity Balance Issues
> : > http://reefkeeping.com/issues/2002-...ature/index.htm
> : >
> : > Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
> : > http://www.advancedaquarist.com/iss...ly2002/chem.htm
> : >
> : > The Relationship Between Alkalinity and pH.
> : > http://www.advancedaquarist.com/issues/may2002/chem.htm
> : >
> : > The Chemical & Biochemical Mechanisms of Calcification in Corals
> : > http://www.advancedaquarist.com/issues/apr2002/chem.htm
> : >
> : > Calcium
> : > http://www.advancedaquarist.com/issues/mar2002/chem.htm
> : >
> : > Alkalinity
> : > http://www.advancedaquarist.com/iss...2/chemistry.htm
> : >
> : >
> : > Iron
> : >
> : > First Iron Article: Macroalgae and Dosing Recommendations
> : > http://www.advancedaquarist.com/issues/aug2002/chem.htm
> : >
> : > Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> : > http://www.advancedaquarist.com/issues/oct2002/chem.htm
> : >
> : > Iodine
> : >
> : > Iodine in Marine Aquaria: Part I
> : > http://www.advancedaquarist.com/issues/mar2003/chem.htm
> : >
> : > Iodine in Reef Tanks 2: Effects on Macroalgae Growth
> : > http://www.advancedaquarist.com/iss...il2003/chem.htm
> : >
> : >
> : > Magnesium and Strontium
> : >
> : > Strontium
> : > http://www.advancedaquarist.com/issues/nov2003/chem.htm
> : >
> : > Magnesium
> : > http://www.advancedaquarist.com/issues/oct2003/chem.htm
> : >
> : > Magnesium and Strontium in Limewater
> : > http://www.advancedaquarist.com/issues/dec2003/chem.htm
> : >
> : >
> : > Limewater (kalkwasser)
> : >
> : > The Self Purification of Limewater (Kalkwasser)
> : > http://www.advancedaquarist.com/issues/may2003/chem.htm
> : >
> : > The Degradation of Limewater (Kalkwasser) in Air
> : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : >
> : > How to Select a Calcium and Alkalinity Supplementation Scheme
> : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
> : >
> : > Metals in Aquaria
> : >
> : > Aluminum and aluminum-based phosphate binders
> : > http://www.advancedaquarist.com/iss...ly2003/chem.htm
> : >
> : > Reef Aquaria with Low Soluble Metals
> : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : >
> : > Tap Water in Reef Aquaria
> : > http://www.advancedaquarist.com/issues/jan2004/chem.htm
> : > First Iron Article: Macroalgae and Dosing Recommendations
> : > http://www.advancedaquarist.com/issues/aug2002/chem.htm
> : >
> : > Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
> : > http://www.advancedaquarist.com/issues/oct2002/chem.htm
> : >
> : >
> : > Test Kit Reviews
> : >
> : > The Seachem Borate Alkalinity Test Kit
> : > http://www.advancedaquarist.com/iss...ne2003/chem.htm
> : >
> : > The Salifert Boron Test Kit
> : > http://www.advancedaquarist.com/iss...pt2003/chem.htm
> : >
> : > Boron and Borate (and pH buffering)
> : >
> : > Boron in a Reef Tank (and its effect on pH buffering)
> : > http://www.advancedaquarist.com/issues/dec2002/chem.htm
> : >
> : > The Seachem Borate Alkalinity Test Kit
> : > http://www.advancedaquarist.com/iss...ne2003/chem.htm
> : >
> : > The Salifert Boron Test Kit
> : > http://www.advancedaquarist.com/iss...pt2003/chem.htm
> : >
> : >
> : >
> : > Others
> : >
> : > Tap Water in Reef Aquaria
> : > http://www.advancedaquarist.com/issues/jan2004/chem.htm
> : >
> : > ORP
> : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : >
> : > Chloramine
> : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : >
> : > Silica in a Reef Tank
> : > http://advancedaquarist.com/issues/jan2003/feature.htm
> : >
> : > Specific Gravity (and temperature correction of hydrometers)
> : > http://www.advancedaquarist.com/iss...2/chemistry.htm
> : >
> : >
> : > The Complete Nitrogen Cycle
> : > http://www.animalnetwork.com/fish/l...a&RecordNo=3090
> : >
> : > Magnesium (older article with fonts screwed up)
> : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : >
> : > Phosphate (older article now reproduced in a poor fashion)
> : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : >
> : > Carbon Dioxide
> : > http://www.animalnetwork.com/fish/l...a&RecordNo=2074
> : >
> : > Using Conductivity to Measure Salinity
> : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : >
> : > Understanding Seawater
> : > http://www.animalnetwork.com/fish2/...s/1/default.asp
> : >
> : > Protein Skimming: How It Works
> : > http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
> : >
> : >
> : >
> : > Articles by Craig Bingman:
> : >
> : > Carbon Dioxide tests
> : > http://www.animalnetwork.com/fish/l...n=&RecordNo=279
> : >
> : > Limewater, Acetic Acid and Sand Clumping
> : > http://www.animalnetwork.com/fish/l...n=&RecordNo=181
> : >
> : > Calcium and Alkalinity
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Calculation of Calcium Carbonate Saturation States in Reef Aquaria
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : >
> : > Calcification Rates in Several Tropical Coral Reef Aquaria
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Limits To Limewater...Revisited
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Expanding the Limits of Limewater: Adding Organic Carbon Sources
(vinegar)
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : >
> : > Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Magnesium - Part I
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Magnesium - Part II
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > A Homemade Magnesium Supplement
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Simulating the Effect of Calcium Chloride and Sodium Bicarbonate
Additions
> : on Reef Systems
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Additional Simulations: The Combined Effect Of Calcium Chloride
> : > /Sodium Bicarbonate Additions And Water Exchanges
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : >
> : > More articles by Craig Bingman:
> : >
> : > The Halogens - Part I: Bromine in Seawater and Aquaria
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > The Halogens - Part II: Fluoride
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Fluoride Depletion In Four Reef Aquariums
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > The Halogens - Part III: Iodine
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Measuring Halides
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > How Test Kits Work
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Borax pH Calibration
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > A pH Detective Story
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > How to Mix a Batch of Synthetic Seawater in Under Five Minutes
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : > SILICON - FOE OR FRIEND?
> : > http://www.animalnetwork.com/fish2/...s/1/default.asp
> : >
> : > The Composition Of Several Synthetic Seawater Mixes
> : > http://www.animalnetwork.com/fish2/...s/1/default.asp
> : >
> : > Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
> : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : >
> : >
> : >
> : > Andy's calcium calculator
> : > http://www.andy-hipkiss.co.uk/cacalc.htm
> : >
> : > Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
> : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : >
> : > Calcium Reactor Substrate -- Phosphate Levels
> : > by Greg Hiller
> : > http://www.advancedaquarist.com/iss...l2003/short.htm
> : >
> : >
> : > Indoor CO2 Problems
> : > http://www.advancedaquarist.com/iss...r2002/short.htm
> : >
> : > Simon Huntington's CaCO3/CO2 reactor article
> : >
> : > http://reefkeeping.com/issues/2002-...ature/index.htm
> : >
> : > Ron Shimek's Tank Water Analysis Article
> : > http://reefkeeping.com/issues/2002-...ature/index.htm
> : >
> : >
> : >
> : >
> : > Home made salinity standards thread:
> : >
> : > http://reefcentral.com/forums/showt...?threadid=65509
> : >
> : > Reef Chemicals Calculator
> : > http://www.kademani.com/reefchem.htm
> : >
> : >
> : >
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : >
> : > Former US Army Bomb Technician (EOD)
> : > Member; IABTI, NATEODA, WEODF, ISEE & IPS
> : >
> : > If You See Me Running You Better Catch-Up
> : >
> : >
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : > "stoutman" <.@.> wrote in message
> : news:aGuWb.148227$U%5.676753@attbi_s03...
> : > : Boomer,
> : > :
> : > : I am not sure if you are just messing with me or if you are truly
> : confused.
> : > : I hope the latter. Please read from Top to Bottom.
> : > :
> : > :
> : > : From YOUR first link:
> : > :
> : > : http://www.waterontheweb.org/resources/glossary.html
> : > :
> : > : Acidity:
> : > : A measure of how acid a solution may be. A solution with a pH of
less
> : than
> : > : 7.0 is considered acidic. Solutions with a pH of less than 4.5
contain
> : > : mineral acidity (due to strong inorganic acids), while a solution
having
> : a
> : > : pH greater than 8.3 contains no acidity.
> : > :
> : > : Yes,
> : > :
> : > : Good definition (for the most part). pH <7 is indeed acidic. pH >
7 is
> : > : basic. Your web page had a definition for acidity, but not
basicity.
> : > : Strange. That's like defining GOOD and not defining BAD.
> : > :
> : > : Here is the IUPAC (International Union of Pure and Applied
Chemistry)
> : > : definition of acidity:
> : > :
> : > : http://www.chem.qmul.ac.uk/iupac/index.html
> : > :
> : > : acidity
> : > :
> : > : (1) Of a compound:
> : > :
> : > : For Brønsted acids it means the tendency of a compound to act as a
> : hydron
> : > : donor. It can be quantitatively expressed by the acid dissociation
> : constant
> : > : of the compound in water or some other specified medium. For Lewis
acids
> : it
> : > : relates to the association constants of Lewis adducts and -adducts.
> : > :
> : > : (2) Of a medium:
> : > :
> : > : The use of the term is mainly restricted to a medium containing
Brønsted
> : > : acids, where it means the tendency of the medium to hydronate a
specific
> : > : reference base
> : > :
> : > : basicity
> : > :
> : > : For Brønsted bases it means the tendency of a compound to act as
hydron
> : > : (proton) acceptor. The basicity of a chemical species is normally
> : expressed
> : > : by the acidity of the conjugate acid (see conjugate acid-base pair).
For
> : > : Lewis bases it relates to the association constants of Lewis adducts
> : > : and -adducts
> : > :
> : > :
> : > :
> : > : Another definition from the same web page YOU cited: (this is the
same
> : web
> : > : page you cited above)
> : > :
> : > : Alkalinity:
> : > : Acid neutralizing or buffering capacity of water; a measure of the
> : ability
> : > : of water to resist changes in pH caused by the addition of acids or
> : bases
> : > : and therefore, the main indicator of susceptibility to acid rain; in
> : natural
> : > : waters it is due primarily to the presence of bicarbonates,
carbonates
> : and
> : > : to a much lesser extent occasionally borates, silicates and
phosphates.
> : It
> : > : is expressed in units of milligrams per liter (mg/l) of CaCO3
(calcium
> : > : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l =
1
> : mg/l
> : > : of CaCO3. A solution having a pH below about 5 contains no
alkalinity.
> : > :
> : > : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and
says
> : > : that alkalinity is the measure of ...(description of a buffer)
> : > :
> : > : A BUFFER IS : a measure of the ability of water to resist changes in
pH
> : > : caused by the addition of acids or bases (from definition below)
> : > :
> : > :
> : > : I said:
> : > : ***alkalinity is a measurement of 'buffering capacity'***
> : > :
> : > : You said:
> : > : ***Alkalinity is not a measurement of BC
> : > :
> : > : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is
not
> : > : logical.
> : > :
> : > : (THIS FROM THE SAME WEB PAGE YOU CITED):
> : > :
> : > : Buffer:
> : > : A substance which tends to keep pH levels fairly constant when acids
or
> : > : bases are added.
> : > :
> : > : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
> : > :
> : > : a measure of the ability of water to resist changes in pH caused by
the
> : > : addition of acids or bases
> : > :
> : > : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A
BUFFER.
> : > :
> : > :
> : > : I went to all four links. None contradict what I have said. But
the
> : first
> : > : one you cited contradicts YOU!
> : > :
> : > : I know what a buffer is. I know what acidity means. I know what
> : alkalinity
> : > : means. No need to cite web pages that describe what I know and what
I
> : wrote
> : > : in this discussion. Show me one that says alkalinity is not a
measure
> : of
> : > : buffering capacity from a credible source.
> : > :
> : > :
> : > :
> : > :
> : > :
> : > :
> : > : "Boomer" > wrote in message
> : > : ...
> : > : > Alkalinity a measure of the amount of anions of weak acid in water
and
> : of
> : > : the cations
> : > : > balanced against them
> : > : > Take note it says ***acid***
> : > : >
> : > : > Buffering capacity the ability of a solution to resist or dampen
> : changes
> : > : in pH upon the
> : > : > addition of acids or bases.
> : > : > Take note its says ***the addition of acids or bases***
> : > : >
> : > : > One more
> : > : >
> : > : > http://www.waterontheweb.org/resources/glossary.html
> : > : >
> : > : > We could go on like this all day, so what is the point ?
> : > : >
> : > : > You will LOVE this one
> : > : > http://www.kyantec.com/Tips/phbuffering.htm
> : > : >
> : > : > Don't you just lovbe PDF's
> : > : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
> : > : >
> : > : > Don't fall out of your chair
> : > : >
http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
> : > : >
> : > : >
> : > : >
> : > : >
> : > : > --
> : > : > Boomer
> : > : >
> : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : >
> : > : > Want to See More ?
> : > : > Please Join Our Growing Membership
> : > : > www.coralrealm.com
> : > : >
> : > : > If You See Me Running You Better Catch-Up
> : > : > "stoutman" <.@.> wrote in message
> : news:XB7Wb.19339$QA2.62332@attbi_s52...
> : > : > : Man here is another, google is a wonderful thing. I'm not
filtering
> : any
> : > : > : out, just posting what I find by GOOGLING for you.
> : > : > :
> : > : > :
http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> : > : > :
> : > : > :
> : > : > : Wow, a gov link. Even the government is wrong, this must be a
> : > : conspiracy
> : > : > : against Boomer.
> : > : > :
> : > : > :
> : > : > :
> : > : > :
> : > : > : "Boomer" > wrote in message
> : > : > : ...
> : > : > : > Now I am getting bored
> : > : > : >
> : > : > : > "Don't the components of a buffer account for the buffering
> : capacity?
> : > : > : Yes."
> : > : > : >
> : > : > : > Yes, agreed but you seem to fail what I'm saying. Buffering
> : Capacity
> : > : and
> : > : > : Alkalinity are
> : > : > : > not the same, that has always been the issue. I gave the
equation
> : does
> : > : > : that look like an
> : > : > : > Alkalinity equation or how Alk is determined. I see you had
now
> : > : comments
> : > : > : on it what's
> : > : > : > wrong, why no comments on the equations I gave. Don't
understand
> : them
> : > : or
> : > : > : what ? Again this
> : > : > : > is the equation for Buffering Capacity, also called Buffer
Index
> : or
> : > : Buffer
> : > : > : Intensity. It
> : > : > : > is defined in most water chemistry and chemical oceanography
text
> : > : books.
> : > : > : >
> : > : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] +
[H30+] +
> : > : CKa
> : > : > : [H3O+] / (Ka =
> : > : > : > H3O+])² )
> : > : > : >
> : > : > : > This is not Alkalinity now is it ?
> : > : > : >
> : > : > : > "I know how to do a titration, In fact I have done several.
How
> : many
> : > : have
> : > : > : > you actually done? I don't mean by counting drops, I mean
with a
> : > : buret?"
> : > : > : >
> : > : > : > Well good for you, I use a Digital Titrator
> : > : > : >
> : > : > : > "Oh, I see,
> : > : > : > you think acidity is the opposite of alkalinity. In the world
of
> : > : > : CHEMISTRY
> : > : > : > it's not. Maybe in aquarium newsgroups it is.
> : > : > : >
> : > : > : > Hum no, maybe you should go for a look at HACH's or LaMotte
> : website or
> : > : the
> : > : > : book I
> : > : > : > suggested earlier. Please view a copy.
> : > : > : >
> : > : > : > Standard Methods for the Examination of Water and Wastewater
> : > : > : >
> : > : > : > This book, over 2000 pages, is the guide for water testing. If
you
> : are
> : > : > : reporting water
> : > : > : > test to the EPA you must use approved std from this text.I t
is
> : > : prepared
> : > : > : and published by
> : > : > : > the EPA, American Water Works Association and American Public
> : Health
> : > : > : Association. You
> : > : > : > mean you don't have one and the issue is water chemistry
> : > : > : >
> : > : > : > You are confusing Acidity and Acidity as you know little about
> : water
> : > : > : chemistry and
> : > : > : > procedures and test methods
> : > : > : >
> : > : > : > From SMEWW, section 2-30, 2310 ACIDITY
> : > : > : >
> : > : > : > "Acidity of water is its quantative capacity to react with a
> : strong
> : > : base
> : > : > : to a designated
> : > : > : > pH"
> : > : > : >
> : > : > : > This is how you test for it
> : > : > : >
> : > : > : > A std alkali titration to methyl orange or phenolphthalein
> : > : > : > endpoint.
> : > : > : >
> : > : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that
> : write
> : > : this
> : > : > : book, there are
> : > : > : > over 100 of them, they are wrong.
> : > : > : >
> : > : > : > Like Buffering Capacity you have your Acidity's mixed up
> : > : > : > In water measurement if you have a high Alk you also usually
have
> : a
> : > : high
> : > : > : Acidity.
> : > : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
> : > : CHEMISTRY
> : > : > : BOOK there pal.
> : > : > : >
> : > : > : >
> : > : > : > "These are all in equilibrium with each other. An initial
high pH
> : > : (above
> : > : > : > 6.4) will shift the equilibrium to the right to form HCO3-1.
If
> : the
> : > : pH of
> : > : > : > the solution is above 10.3 (pKa2) the .........."
> : > : > : >
> : > : > : >
> : > : > : > Christ, there you go again with the FW ****. All your numbers
are
> : > : wrong we
> : > : > : are dealing
> : > : > : > with SEAWATER
> : > : > : >
> : > : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is
in
> : the
> : > : form
> : > : > : > of HCO3-1 .
> : > : > : >
> : > : > : > I have already pointed that out and gave actual values at know
> : > : seawater
> : > : > : levels, go back
> : > : > : > and re-read it you aren't telling me anything here.Of course
most
> : is
> : > : HCO3
> : > : > : see...
> : > : > : >
> : > : > : >
> : > : > : > @ 20C and 34.3 ppt salinity
> : > : > : >
> : > : > : > CO2 = 0.52 %
> : > : > : >
> : > : > : > HCO3 = 86.4 %
> : > : > : >
> : > : > : > CO3 = 13.09 %
> : > : > : >
> : > : > : >
> : > : > : > "In your glass experiment you managed to lower the pH enough
to
> : purge
> : > : out
> : > : > : CO2
> : > : > : > by boiling"
> : > : > : >
> : > : > : > The purpose behind the glass is to show that alk is not affect
by
> : CO2
> : > : and
> : > : > : vise-versa and
> : > : > : > how Co2 affects pH.
> : > : > : >
> : > : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and
that
> : pH
> : > : drops
> : > : > : to say 8.1 it is
> : > : > : > usually due to excess CO2. If you took a glass of that water
and
> : > : aerated
> : > : > : it you WILL drive
> : > : > : > off the CO2 and raise the pH. It has been done a proven a
million
> : > : times.
> : > : > : >
> : > : > : > "In order to 'purge' CO2 you would need to lower the
> : > : > : > pH to shift the equilibrium to below 6.4"
> : > : > : >
> : > : > : > The hell you do !!!.Do you know who many times people on this
NG
> : to
> : > : > : include Dr. Craig
> : > : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned
to
> : take a
> : > : > : sample of aquarium
> : > : > : > water and aerate it to see if the pH GOES UP AND when they
come
> : back
> : > : with
> : > : > : the test it is
> : > : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D
CHEMIST
> : > : excess
> : > : > : CO2 in the tank
> : > : > : > water, increase the circulation for better gas exchange at the
> : > : surface,
> : > : > : reduce feeding,
> : > : > : > and try to improve on better skimming, thus reducing the
bio-load
> : and
> : > : pH
> : > : > : decline due to
> : > : > : > CO2.
> : > : > : >
> : > : > : >
> : > : > : > "I hope this helps. "
> : > : > : >
> : > : > : > Help, how can you when you miss everything. I should be
charging
> : you
> : > : > : >
> : > : > : > Oh, by the way. Your websites, I have about 50 on these
issues, I
> : > : could
> : > : > : post them, not to
> : > : > : > mention I have all those water chemistry books, so there is no
> : need to
> : > : > : view your sites.
> : > : > : >
> : > : > : > Finally are you afraid to come to our Chemistry Forum, afraid
to
> : get
> : > : > : slapped by REAL
> : > : > : > chemists. I get a charge out of you can't post your ref .I
have
> : posted
> : > : the
> : > : > : same or similar
> : > : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have
1500
> : > : posts
> : > : > : there and am the
> : > : > : > biggest contributor to his forum other than himself or maybe
Habib
> : > : Sheka
> : > : > : >
> : > : > : > Hum, here are Randy's ref that he posted. He hosts the website
> : > : > : >
> : > : > : > S. RANDY HOLMES-FARLEY
> : > : > : > Arlington, Massachusetts
> : > : > : >
> : > : > : > EDUCATION
> : > : > : >
> : > : > : > 1982-1986 Harvard University Cambridge, MA
> : > : > : > PhD in Chemistry
> : > : > : > Research Advisor: George Whitesides
> : > : > : >
> : > : > : > Investigated the relationship between polymer surface
chemistry
> : and
> : > : > : physical properties
> : > : > : > through controlled surface modification and testing.
> : > : > : >
> : > : > : > 1980-1982 Cornell University Ithaca, NY
> : > : > : > BA in Chemistry and Biology
> : > : > : > Graduated Summa Cum Laude
> : > : > : > Distinction in All Subjects
> : > : > : > Grade Point: 3.94/4.0
> : > : > : > Honors research: isolation and characterization of the subunit
of
> : CF1
> : > : > : enzyme
> : > : > : >
> : > : > : >
> : > : > : > 1978-1979 Stanford University Palo Alto, CA
> : > : > : > Grade Point: 3.55/4.0
> : > : > : >
> : > : > : >
> : > : > : > EXPERIENCE
> : > : > : >
> : > : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham,
MA
> : > : > : > (bought out GelTex Pharmaceuticals in 2001)
> : > : > : > Vice President, Chemical Research 2001-present
> : > : > : > Senior Director, Chemical Research 1999-2001
> : > : > : > Director of Chemical Research 1997-1999
> : > : > : > Manager of Chemical Research 1995-1997
> : > : > : > Group Leader 1994-1995
> : > : > : > Senior Research Scientist 1992-1994
> : > : > : >
> : > : > : > Helped start GelTex as second employee
> : > : > : >
> : > : > : > Managed various research programs with multi-million dollar
> : budgets
> : > : > : >
> : > : > : > Supervised research chemists (17+)
> : > : > : >
> : > : > : > Co-inventor of several polymeric pharmaceuticals and
> : pharmaceutical
> : > : > : candidates including
> : > : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam
> : Hydrochloride
> : > : (FDA
> : > : > : approved)
> : > : > : >
> : > : > : > Company Safety Officer for 3 years
> : > : > : >
> : > : > : > Chemical Hygiene Officer 2000-present
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > 1990-1992 GTE Corporation Waltham, MA
> : > : > : > Senior Member of Technical Staff
> : > : > : > Applied research involving polymer interfaces
> : > : > : > Metallization of plastics
> : > : > : > Polymer/polymer adhesion
> : > : > : > Optical coatings
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > 1986-1990 Lord Corporation Cary, NC
> : > : > : > Senior Research Scientist 1988-1990
> : > : > : > Research Scientist 1986-1988
> : > : > : > Basic and applied research on surface chemical bonding
> : > : > : > Developed new adhesive compositions
> : > : > : > Developed new sol-gel coatings for corrosion resistance
> : > : > : >
> : > : > : >
> : > : > : > HONORS AND AWARDS
> : > : > : >
> : > : > : > Industrial Innovations Award by Northeast Region of American
> : Chemical
> : > : > : Society (6/2001)
> : > : > : >
> : > : > : > National Kidney Foundation of Northern California Honoree
(5/2001)
> : > : > : >
> : > : > : > American Chemical Society/Polymer Chemistry Division
Industrial
> : > : Sponsors
> : > : > : > Award (8/2000)
> : > : > : >
> : > : > : > R&D 100 Award from R&D magazine (1999)
> : > : > : >
> : > : > : > Sherwin Williams Award in applied polymer science (9/85)
> : > : > : >
> : > : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985;
> : 1985-1986)
> : > : > : >
> : > : > : > Award for highest GPA in Chemistry Department (6/82)
> : > : > : >
> : > : > : > Summa Cum Laude Honors in Chemistry (6/82)
> : > : > : >
> : > : > : > Phi Lamda Epsilon (6/82)
> : > : > : >
> : > : > : > Phi Beta Kappa (2/82)
> : > : > : >
> : > : > : > Cornell University Dean's List (1981, 1982)
> : > : > : >
> : > : > : > Harvard Book Club Award for highest GPA senior year (1978)
> : > : > : >
> : > : > : > First Place in western NY ACS high school chemistry exam
(1977)
> : > : > : >
> : > : > : > 1978-1979
> : > : > : >
> : > : > : >
> : > : > : > __________________
> : > : > : > Randy Holmes-Farley
> : > : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef
> : Central
> : > : > : >
> : > : > : > Hobby Experience: 8 years with reefs
> : > : > : > Current Tanks: 90 gal mixed reef
> : > : > : > Interests: Reefkeeping, science, photography
> : > : > : >
> : > : > : >
> : > : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
> : > : > : >
> : > : > : > Open this post in a new window | Report this post to a
moderator |
> : IP:
> : > : > : Logged
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > 06/27/2003 02:44 PM
> : > : > : >
> : > : > : > Randy Holmes-Farley
> : > : > : > Chemistry Moderator
> : > : > : >
> : > : > : > Registered: Apr 2001
> : > : > : > Location: Arlington, Massachusetts
> : > : > : > Occupation: Chemist (Drug Discovery at Genzyme)
> : > : > : > Posts: 15282
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > Publications
> : > : > : >
> : > : > : >
> : > : > : > ISSUED UNITED STATES PATENTS
> : > : > : >
> : > : > : >
> : > : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen
Randall;
> : > : > : Mandeville, III; W. Harry.
> : > : > : > US 6,566,407; 5/20/2003
> : > : > : >
> : > : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley,
Stephen
> : > : Randall;
> : > : > : Huval, Chad
> : > : > : > Cori.
> : > : > : > U.S. 6,517,825; 2/11/2003.
> : > : > : >
> : > : > : > 3. Method of making phosphate-binding polymers for oral
> : > : administration.
> : > : > : Holmes-Farley,
> : > : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M.
U.S.
> : > : > : 6,509,013; 1/21/2003.
> : > : > : >
> : > : > : > 4. Combination therapy for treating hypercholesterolemia using
a
> : bile
> : > : acid
> : > : > : sequestrant
> : > : > : > polymer
> : > : > : > and a cholesterol-lowering agent. Huval, Chad Cori;
Holmes-Farley,
> : > : Stephen
> : > : > : Randall;
> : > : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
> : > : > : >
> : > : > : > 5. Method for treating hypercholesterolemia with
polyallylamine
> : > : polymers.
> : > : > : Holmes-Farley,
> : > : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
> : > : Goldberg,
> : > : > : Dennis I. , US
> : > : > : > 6,423,754; 7/23/2002.
> : > : > : >
> : > : > : > 6. Ionic polymers as anti-infective agents Mandeville, W.
Harry,
> : III;
> : > : > : Neenan, Thomas X..;
> : > : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> : > : > : >
> : > : > : > 7. Combination therapy for treating hypercholesterolemia and
> : > : > : atherosclerosis. Huval, Chad
> : > : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal,
> : Pradeep
> : > : K.
> : > : > : U.S. 6,365,186;
> : > : > : > 4/2/2002.
> : > : > : >
> : > : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
> : > : Mandeville,
> : > : > : W. H., III;
> : > : > : > Huval; C.
> : > : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US
6,299,868;
> : > : > : 10/9/2001.
> : > : > : >
> : > : > : > 9. Polymers containing guanidinium groups as bile acid
> : sequestrants.
> : > : Dhal;
> : > : > : P. K.; Holmes-
> : > : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> : > : > : >
> : > : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.;
Mandeville,
> : W.
> : > : H.,
> : > : > : III.; US
> : > : > : > 6,281,252;
> : > : > : > 8/28/2001.
> : > : > : >
> : > : > : > 11. Combination therapy for treating hypercholestrolemia.
Huval;
> : C.
> : > : C.;
> : > : > : Holmes-Farley; S.
> : > : > : > R. ;
> : > : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> : > : > : >
> : > : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides,
G.
> : M.;
> : > : > : Holmes-Farley, S.
> : > : > : > R.; US
> : > : > : > 6,264,937; 7/24/2001.
> : > : > : >
> : > : > : > 13. Method for treating hypercholesterolemia with
unsubstituted
> : > : > : polydiallylamine polymers.
> : > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
K.
> : ; US
> : > : > : 6,248,318;
> : > : > : > 6/19/2001.
> : > : > : >
> : > : > : > 14. Process for removing bile salts from a patient and
alkylated
> : > : > : compositions therefore.
> : > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355;
> : 5/1/2001.
> : > : > : >
> : > : > : > 15. Poly(diallylamine)-based bile acid sequestrants.
> : Holmes-Farley, S.
> : > : R.;
> : > : > : Dhal, P. K.;
> : > : > : > Petersen,
> : > : > : > J. S.; US 6,203,785; 3/20/2001.
> : > : > : >
> : > : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S.
R.;
> : > : Huval,
> : > : > : C. C.; US
> : > : > : > 6,190,649;
> : > : > : > 2/20/2001.
> : > : > : >
> : > : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.;
Mandeville,
> : W.
> : > : H.,
> : > : > : III.; US
> : > : > : > 6,177,478;
> : > : > : > 1/23/2001.
> : > : > : >
> : > : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
> : > : Holmes-Farley,
> : > : > : S. R.;
> : > : > : > Mandeville, W.
> : > : > : > H., III.; US 6,129,910; 10/10/2000.
> : > : > : >
> : > : > : > 19. Method for treating hypercholesterolemia with
unsubstituted
> : > : > : polydiallylamine polymers.
> : > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
K.
> : ; US
> : > : > : 6,083,497;
> : > : > : > 7/4/2000.
> : > : > : >
> : > : > : > 20. Method of making phosphate-binding polymers for oral
> : > : administration.
> : > : > : Holmes-Farley, S.
> : > : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US
6,083,495;
> : > : 7/4/2000.
> : > : > : >
> : > : > : > 21. Process for removing bile salts from a patient and
alkylated
> : > : > : compositions therefore.
> : > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
> : > : 5/23/2000.
> : > : > : >
> : > : > : > 22. Process for removing bile salts from a patient and
> : compositions
> : > : > : therefor. Mandeville,
> : > : > : > W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> : > : > : >
> : > : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III;
W.
> : H;
> : > : > : Neenan; T. X.; Holmes-
> : > : > : > Farley; S. R. US 6,034,129; 3/7/2000.
> : > : > : >
> : > : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.;
Mandeville,
> : W.
> : > : H.,
> : > : > : III.; US
> : > : > : > 5,985,938;
> : > : > : > 11/16/99.
> : > : > : >
> : > : > : > 25. Process for removing bile salts from a patient and
> : compositions
> : > : > : therefor. Mandeville,
> : > : > : > W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> : > : > : >
> : > : > : > 26. Hydrophobic sequestrant for cholesterol depletion.
Mandeville,
> : W.
> : > : H.,
> : > : > : III.;
> : > : > : > Holmes-Farley;
> : > : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> : > : > : >
> : > : > : > 27. Hydrophilic nonamine-containing and amine-containing
> : copolymers
> : > : and
> : > : > : their use as bile
> : > : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
> : > : 5,929,184;
> : > : > : 7/27/99.
> : > : > : >
> : > : > : > 28. Interpenetrating polymer networks for sequestration of
bile
> : acids.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US
> : 5,925,379;
> : > : > : 7/20/99.
> : > : > : >
> : > : > : > 29. Amine polymer sequestrant and method of cholesterol
depletion.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> : > : > : >
> : > : > : > 30. Process for removing bile salts from a patient and
> : compositions
> : > : > : therefor. Mandeville,
> : > : > : > W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> : > : > : >
> : > : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
> : depletion.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
> : > : > : >
> : > : > : > 32. Process for removing bile salts from a patient and
> : compositions
> : > : > : therefor. Mandeville,
> : > : > : > W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> : > : > : >
> : > : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
> : > : Mandeville,
> : > : > : W. H., III.;
> : > : > : > Holmes-
> : > : > : > Farley, S. R.; US 5,703,188; 12/30/97.
> : > : > : >
> : > : > : > 34. Oral administration of iron-binding crosslinked amine
> : polymers.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> : > : > : >
> : > : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
> : Holmes-Farley,
> : > : S.
> : > : > : R.; US 5,693,675;
> : > : > : > 12/2/97.
> : > : > : >
> : > : > : > 36. Method for removing bile salts from a patient with
alkylated
> : > : > : crosslinked amine
> : > : > : > polymers,
> : > : > : > and preparation of the polymers. Mandeville, W. H., III.;
> : > : Holmes-Farley,
> : > : > : S. R.; US
> : > : > : > 5,679,717; 10/21/97.
> : > : > : >
> : > : > : > 37. Phosphate-binding polymers for oral administration.
> : Holmes-Farley,
> : > : S.
> : > : > : R.; Mandeville,
> : > : > : > W.
> : > : > : > H., III.; US 5,667,775; 9/16/97.
> : > : > : >
> : > : > : > 38. Ion-exchange process using highly crosslinked polymers for
> : > : removing
> : > : > : bile salts from a
> : > : > : > patient, preparation of the polymers, and compositions
containing
> : > : them.
> : > : > : Mandeville, W. H.,
> : > : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> : > : > : >
> : > : > : > 39. Hydrophobic amine polymer sequestrant and method of
> : cholesterol
> : > : > : depletion. Mandeville,
> : > : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US
5,618,530;
> : > : 4/8/97.
> : > : > : >
> : > : > : > 40. Amine polymer sequestrant and method of cholesterol
depletion.
> : > : > : Mandeville, W. H.,
> : > : > : > III.;
> : > : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> : > : > : >
> : > : > : > 41. Phosphate-binding polymers for oral administration.
> : Holmes-Farley,
> : > : S.
> : > : > : R.; Mandeville,
> : > : > : > W.
> : > : > : > H., III.; US 5,496,545; 3/5/96.
> : > : > : >
> : > : > : > 42. Iron-binding polymers for oral administration. Mandeville,
W.
> : H.,
> : > : > : III.; Holmes-Farley,
> : > : > : > S. R.;
> : > : > : > US 5,487,888; 1/30/96.
> : > : > : >
> : > : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having
> : active
> : > : > : hydrogens on the
> : > : > : > surface.
> : > : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
> : > : > : >
> : > : > : > 44. Layered sol-gel coatings from organisilicon compounds.
> : > : Holmes-Farley,
> : > : > : S. R.; Yanyo, L.
> : > : > : > C.;
> : > : > : > US 5,182,143; 1/26/93.
> : > : > : >
> : > : > : > 45. Method for metal bonding using ultrathin primer coating.
> : > : > : Holmes-Farley, S. R.; Yanyo,
> : > : > : > L.
> : > : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> : > : > : >
> : > : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.;
Abbey, K.
> : J.;
> : > : US
> : > : > : 5,096,962;
> : > : > : > 3/17/92.
> : > : > : >
> : > : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
> : > : > : elastomer-metal bonding.
> : > : > : > Holmes-
> : > : > : > Farley, S. R.; US 5,102,956; 4/7/92.
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT
ISSUED)
> : > : > : >
> : > : > : >
> : > : > : > 1. Aryl boronate functionalized polymers for treating obesity
and
> : > : > : inhibiting fat uptake.
> : > : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III;
Dhal,
> : > : Pradeep
> : > : > : K.; Huval, Chad
> : > : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl.
(2003),
> : 92
> : > : pp. WO
> : > : > : 0302571.
> : > : > : >
> : > : > : > 2. Preparation of aryl boronic acids for treating obesity.
> : > : Holmes-Farley,
> : > : > : Stephen Randall;
> : > : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal,
> : Pradeep
> : > : K.
> : > : > : (Geltex
> : > : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO
> : 0302570.
> : > : > : >
> : > : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide.
> : Holmes-Farley,
> : > : > : Stephen Randall.
> : > : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32
pp.
> : WO
> : > : > : 0302130.
> : > : > : >
> : > : > : > 4. Method for reducing copper levels and treating copper
> : toxicosis.
> : > : > : Holmes-Farley, Stephen
> : > : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl.
> : (2002),
> : > : 45
> : > : > : pp. WO
> : > : > : > 0285383.
> : > : > : >
> : > : > : > 5. Method for treating gout and binding uric acid.
Holmes-Farley,
> : > : Stephen
> : > : > : Randall; Burke,
> : > : > : > Steven K. WO 0285381 10/31/2002.
> : > : > : >
> : > : > : > 6. Method for treating gout and reducing serum uric acid.
> : > : Holmes-Farley,
> : > : > : Stephen Randall;
> : > : > : > Burke, Steven K WO 0285380 10/31/2002.
> : > : > : >
> : > : > : > 7. Amine condensation polymer bile acid sequestrants. Huval,
C.
> : C.;
> : > : > : Holmes-Farley, S. R.;
> : > : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> : > : > : >
> : > : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H.,
III
> : and
> : > : > : Holmes-Farley, S.
> : > : > : > R.;
> : > : > : > WO 1999-US5662; 9/23/1999.
> : > : > : >
> : > : > : > 9. Amine-containing copolymers as bile acid sequestrants.
> : > : Holmes-Farley,
> : > : > : S. R.; Petersen,
> : > : > : > J. S.;
> : > : > : > WO 9933452; 7/8/1999.
> : > : > : >
> : > : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W.
H.,
> : III
> : > : and
> : > : > : Holmes-Farley, S.
> : > : > : > R.;
> : > : > : > WO 9922743; 5/14/1999.
> : > : > : >
> : > : > : > 11. Polyallylamine polymers for removing bile salts and
treating
> : > : > : hypercholesterolemia, and
> : > : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H.,
III;
> : > : Burke,
> : > : > : S. K.; Goldberg,
> : > : > : > D. I.; WO 9857652; 12/23/98.
> : > : > : >
> : > : > : > 12. Phosphate-bidning polymers combined with a calcium
supplement
> : for
> : > : oral
> : > : > : administration.
> : > : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
> : Holmes-Farley,
> : > : S.
> : > : > : R.; WO 9842355;
> : > : > : > 10/1/98.
> : > : > : >
> : > : > : > 13. Hydrophobic heteroatom-containing sequestrant for
cholesterol
> : > : > : depletion. Mandeville,
> : > : > : > W.
> : > : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449;
> : 12/12/96.
> : > : > : >
> : > : > : > 14. Process for adjusting ion concentration in a patient and
> : > : compositions
> : > : > : therefor.
> : > : > : > Mandeville,
> : > : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> : > : > : >
> : > : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
> : > : interlayer
> : > : > : for improved
> : > : > : > metal-
> : > : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
> : > : 1/20/94.
> : > : > : >
> : > : > : > 16. Process for increased metal-substrate bond strength in
> : metalized
> : > : > : plastics.
> : > : > : > Holmes-Farley, S.
> : > : > : > R.; Ger. Offen. 4322516; 7/6/93.
> : > : > : >
> : > : > : > 17. Electrorheological fluids and preparation of particles
useful
> : in
> : > : the
> : > : > : fluids.
> : > : > : > Troughton,
> : > : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie;
Carlson,
> : J.
> : > : > : David; Bares, Joseph
> : > : > : > E.;
> : > : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra
Nell.
> : EP
> : > : > : 394049;
> : > : > : > 10/24/1990.
> : > : > : >
> : > : > : > JOURNAL PUBLICATIONS
> : > : > : >
> : > : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William;
Zhorov,
> : > : Eugene;
> : > : > : Guo, Amy;
> : > : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David
L.;
> : > : > : Mandeville, W. Harry;
> : > : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
> : > : 611-619.
> : > : > : >
> : > : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
> : > : synthesis
> : > : > : and biological
> : > : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley,
S.
> : > : Randall;
> : > : > : Mandeville, W.
> : > : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal,
Pradeep
> : K.
> : > : > : Journal of
> : > : > : > Macromolecular Science, Pure and Applied Chemistry (2001),
> : A38(12),
> : > : > : 1559-1574.
> : > : > : >
> : > : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by
> : Molecular
> : > : > : Imprinting. Huval,
> : > : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.;
Holmes-Farley,
> : S.
> : > : > : Randall; Mandeville,
> : > : > : > W.
> : > : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro,
> : Robert
> : > : J.;
> : > : > : Chen, Xi; Dhal,
> : > : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> : > : > : >
> : > : > : > 4. Synthetic polymers for the binding of fat in the intestinal
> : tract.
> : > : > : Jozefiak, Thomas H.;
> : > : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny,
Cynthia;
> : > : Huval,
> : > : > : Chad C.;
> : > : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney,
Cynthia.
> : > : > : Abstracts of
> : > : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United
States,
> : August
> : > : > : 26-30, 2001
> : > : > : > (2001), POLY-047 and Polymer Preprints (American Chemical
Society,
> : > : > : Division of
> : > : > : > Polymer Chemistry) (2001), 42(2), 98.
> : > : > : >
> : > : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel
> : polymer
> : > : gel
> : > : > : pharmaceutical.
> : > : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.;
Petersen,
> : J.;
> : > : Ward,
> : > : > : J.; Sacchiero,
> : > : > : > B.;
> : > : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton,
K.
> : A.;
> : > : Chen,
> : > : > : X.; Mazzeo, J.
> : > : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
> : > : > : >
> : > : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl
and
> : > : other
> : > : > : bile acid
> : > : > : > sequestrants.
> : > : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.;
Xu,
> : Q.;
> : > : > : Hook, P.; Holmes-
> : > : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1),
> : 708-709.
> : > : > : >
> : > : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
> : > : Holmes-Farley,
> : > : > : S. R; Polym.
> : > : > : > Mater. Sci. Eng (1999), 80, 246-247.
> : > : > : >
> : > : > : > 8. Design and characterization of of Sevelamer Hydrochloride:
a
> : novel
> : > : > : phosphate-binding
> : > : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III;
> : Ward,
> : > : J.;
> : > : > : Miller, K. L.;
> : > : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M.
S.-
> : Pure
> : > : and
> : > : > : Appl. Chem.,
> : > : > : > A36(7&8), p. 1085 (1999).
> : > : > : >
> : > : > : > 9. Three generations of bile acid sequestrants. Mandeville, W.
H.,
> : > : III;
> : > : > : Braunlin, W.;
> : > : > : > Dhal, P.;
> : > : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik,
S.;
> : > : > : Rosenbaum, D.;
> : > : > : > Sacchiero,
> : > : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc.
> : (1999),
> : > : > : 550, 3-15.
> : > : > : >
> : > : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked,
polymeric
> : > : phosphate
> : > : > : binder, on
> : > : > : > urinary
> : > : > : > phosphorous excretion in rats. Rosenbaum, D. P.;
Holmes-Farley, S.
> : R.;
> : > : > : Mandeville, W. H.,
> : > : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
> : Transplant.
> : > : > : (1997), 12(5)
> : > : > : > 961-964.
> : > : > : >
> : > : > : > 11. Thin anisotropic coatings based on sol-gel technology.
> : > : Holmes-Farley,
> : > : > : S. R.; Yanyo, L.
> : > : > : > C;
> : > : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem.
4),
> : > : 439-444.
> : > : > : >
> : > : > : > 12. The mechanism of cure initiation of a surface activated
> : adhesive.
> : > : > : Holmes-Farley, S.
> : > : > : > R.;
> : > : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5),
409-420.
> : > : > : >
> : > : > : > 13. Adhesion promotion and corrosion prevention using thin
> : anisotropic
> : > : > : coatings. Holmes-
> : > : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991),
5(2),
> : > : > : 131-151.
> : > : > : >
> : > : > : > 14. Wetting of functionalized polyethylene having ionizable
> : organic
> : > : acids
> : > : > : and bases at the
> : > : > : > polymer-water interface: relations between functional group
> : polarity,
> : > : > : extent of
> : > : > : > ionization,
> : > : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C.
D.;
> : > : > : Whitesides, G. M.;
> : > : > : > Langmuir
> : > : > : > (1988), 4(4), 921-937.
> : > : > : >
> : > : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols
with
> : a
> : > : > : single hydroxy group.
> : > : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> : > : > : >
> : > : > : > 16. Reconstruction of the interface of oxidatively
functionalized
> : > : > : polyethylene (PE-CO2H)
> : > : > : > and
> : > : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.;
> : Nuzzo,
> : > : R.;
> : > : > : McCarthy, T. J.;
> : > : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also
Report
> : > : (1987),
> : > : > : AD-
> : > : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
> : > : > : >
> : > : > : > 17. Surface-modified polyethylene film: the relationship
between
> : > : surface
> : > : > : chemistry and
> : > : > : > physical
> : > : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987,
47(11),
> : > : 4537.
> : > : > : >
> : > : > : > 18. Reactivity of carboxylic acid and ester groups in the
> : > : functionalized
> : > : > : interfacial
> : > : > : > region of
> : > : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
> : > : > : differentiation of the
> : > : > : > functional groups into shallow and deep subsets based on a
> : comparison
> : > : of
> : > : > : contact angle and
> : > : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.;
> : Langmuir
> : > : > : (1987), 3(1), 62-
> : > : > : > 76.
> : > : > : >
> : > : > : > 19. Fluorescence properties of dansyl groups covalently bonded
tot
> : he
> : > : > : surface of
> : > : > : > oxidatively
> : > : > : > functionalized low-density polyethylene film. Holmes-Farley,
S.
> : R.;
> : > : > : Whitesides, G. M.;
> : > : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985),
TR-85-2;
> : > : > : AD-A162435/2/GAR,
> : > : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> : > : > : >
> : > : > : > 20. Acid-base behavior of carboxylic acid groups covalently
> : attached
> : > : at
> : > : > : the surface of
> : > : > : > polyethylene: The usefulness of contact angle in following the
> : > : ionization
> : > : > : of surface
> : > : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy,
T.
> : J.;
> : > : > : Deutch, J.;
> : > : > : > Whitesides,
> : > : > : > G. M.; Langmuir (1985), 1(6), 725-740.
> : > : > : >
> : > : > : > 21. The thermal stability of a surface modified solid organic
> : polymer.
> : > : > : Holmes-Farley, S.
> : > : > : > R.;
> : > : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53,
127-131.
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> : > : > : >
> : > : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R.
> : Advanced
> : > : > : Aquarist. June 2003.
> : > : > : >
> : > : > : > 2. The Self Purification of Limewater (Kalkwasser).
Holmes-Farley,
> : R.
> : > : > : Advanced Aquarist.
> : > : > : > May
> : > : > : > 2003.
> : > : > : >
> : > : > : > 3. The Degradation of Limewater (Kalkwasser) in Air.
> : Holmes-Farley, R.
> : > : > : Reefkeeping May
> : > : > : > 2003.
> : > : > : >
> : > : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
> : Reefkeeping
> : > : > : April 2003.
> : > : > : >
> : > : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae
Growth.
> : > : > : Holmes-Farley, R.
> : > : > : > Advanced Aquarist; April 2003.
> : > : > : >
> : > : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae
Growth.
> : > : > : Holmes-Farley, R.
> : > : > : > Advanced Aquarist; April 2003.
> : > : > : >
> : > : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R.
Advanced
> : > : Aquarist;
> : > : > : March 2003.
> : > : > : >
> : > : > : > 8. How to Select a Calcium and Alkalinity Supplementation
Scheme.
> : > : > : Holmes-Farley, R.
> : > : > : > Advanced Aquarist; February 2003.
> : > : > : >
> : > : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> : January
> : > : > : 2003.
> : > : > : >
> : > : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
> : > : December
> : > : > : 2002.
> : > : > : >
> : > : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
> : > : Advanced
> : > : > : Aquarist; November
> : > : > : > 2002.
> : > : > : >
> : > : > : > 12. Iron: A Look at Organisms Other than Macroalgae.
> : Holmes-Farley, R.
> : > : > : Advanced Aquarist;
> : > : > : > November 2002.
> : > : > : >
> : > : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.;
Advanced
> : > : Aquarist,
> : > : > : September 2002.
> : > : > : >
> : > : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist,
> : August
> : > : > : 2002.
> : > : > : >
> : > : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.;
Reefkeeping.com,
> : April
> : > : > : 2002.
> : > : > : >
> : > : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R.
Advanced
> : > : > : Aquarist; July 2002
> : > : > : >
> : > : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced
Aquarist;
> : > : June
> : > : > : 2002.
> : > : > : >
> : > : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley,
R.
> : > : Advanced
> : > : > : Aquarist, May
> : > : > : > 2002.
> : > : > : >
> : > : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in
> : Corals.
> : > : > : Holmes-Farley, R.
> : > : > : > Advanced Aquarist, April 2002.
> : > : > : >
> : > : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
> : > : > : >
> : > : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February
> : 2002.
> : > : > : >
> : > : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist,
January
> : > : 2002.
> : > : > : >
> : > : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium
> : Frontiers
> : > : > : 2000.
> : > : > : >
> : > : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R.
Aquarium
> : > : > : Frontiers 2000.
> : > : > : >
> : > : > : > 25. Phosphate..What is it and why should you care.
Holmes-Farley,
> : R.
> : > : > : Aquarium Frontiers
> : > : > : > 2000.
> : > : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
> : > : Frontiers
> : > : > : 2000.
> : > : > : >
> : > : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium
Frontiers
> : > : 2000.
> : > : > : >
> : > : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium
Frontiers
> : 1999.
> : > : > : >
> : > : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > Boomer
> : > : > : >
> : > : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : > : >
> : > : > : > Want to See More ?
> : > : > : > Please Join Our Growing Membership
> : > : > : > www.coralrealm.com
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > :
> : > : > :
> : > : >
> : > : >
> : > :
> : > :
> : > :
> : >
> : >
> :
> :
>
>

[Boomer]

Stout

I'm late getting out and had to come here before I left


"I think this discussion has shifted from SCIENCE to SEMANTICS"

I think I said that a few posts back, "a word game " LOL


I think one of us, Ok me , is getting to picky.

Remember what Dr.Millero said in regards to the argument in FAMA a few years back. "The
chemist is right the marine biologist is wrong, Bc is not the same thing as Alk. Alk is
the ability of water to resist changes in pH caused by the addition of acid and Bc is the
ability to resist changes in pH caused by the addition of acid or base. The arguemnet in
FAMA was about the same as ours

I would like to have you call Dr.. Millero or e-mail him to see what he says, maybe I'm
off and you are more right.Yes, I mean that seriously. It would solve the issue, I will go
with what ever he says...period. I have no problem if he agrees with you 100 %.

1-305-361-4707




--
Boomer

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http://www.reefcentral.com/vbulletin/index.php

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If You See Me Running You Better Catch-Up
"stoutman" <.@.> wrote in message news:4u9Xb.303758$xy6.1488597@attbi_s02...
: Boomer,
:
: I think this discussion has shifted from SCIENCE to SEMANTICS.
:
: I say: Alkalinity is a measurement of Buffering capacity.....
: you say: Alkalinity is an indication of Buffering capacity.....
:
: Have a good weekend Boomer.
:
: -Stoutman
:
:
:
:
:
:
: "Boomer" > wrote in message
: ...
: > Yes, of cause I remember, as I said I posted it for a reason. I see you
: have used only
: > that link for your definition, as it makes you look right.You have avoided
: all Alk
: > definitions in a chemistry book, to include your own definition *****to
: resist a drop in
: > pH due to the addition of acid***, which is the same as the others I
: posted .Agreed, of
: > course not.You know that Alk isn't defined as "by the addition of acids or
: bases "and is
: > only the " addition of an acid", so why are you accepting the definition
: ?.You know that
: > when you titrate it is an acid added and never a base. In one breath it
: says Alk is "Acid
: > neutralizing " and then they say "by the addition of acids or bases ".You
: can't have it
: > both ways and YOU know that Agreed . If the word "base" was left out I
: would not have much
: > to say. Agreed
: >
: >
: > "Alkalinity is a
: > measurement of BUFFERING CAPACITY."
: >
: > No it is not a measurement of BUFFERING CAPACITY, it is a indication of
: BC. I have said
: > this at least twice. If you know your BC you can calculate Alk and if you
: can do one you
: > can do the other agreed. What I have tried to convey from the beginning is
: that Alk and BC
: > are not the same thing. You in one of your other posts have said they are
: not the same
: > thing and never said they were. Now you seem to be saying they are the
: same thing
: >
: > "So, when we measure ALKALINITY (and we know the pH) we are in effect
: > measuring BUFFERING CAPACITY.
: >
: > More or less YES in an "effect" but Alk tells you not much of anything
: when a base is
: > added Agreed. That is called Acidity, which I see you have avoided again
: as if there is
: > no such thing. I also said that for us the only thing we need to be
: concerned about is
: > Alk, so BC would fit in, as we could care less about the ability to
: neutralize a base or
: > measure Acidity. So, if you knew your pH , Alk or Acy you would really
: know what you BC is
: > doing for you Agreed.
: >
: > On Bc, we have both left something from my first equation, so I thought I
: would post it
: > again for you, as I like being honest .I'm surprised you didn't catch it
: :-)
: >
: > B = dCb / dpH = - dCa / dpH
: >
: > So;
: >
: > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
: [H3O+] / (Ka =
: > H3O+])² )
: >
: > or
: >
: > B (Buffering Capacity) = - dCa / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
: [H3O+] / (Ka =
: > H3O+])² )
: >
: > There are number of was to mathematically express BC. Two of the most
: common are the
: > change in Alk with the pH at constant total carbonate, the other is change
: in Alk with pH
: > constant CO2 pp. In some examples of Bc, Bc is the inverse slope of the
: Alk titration
: > curve ( I'm sure yo
: > u will love this) In the other over the pH range, while BC is going
: through minimum, Bpp
: > increases linearly. This difference is caused by the uptake of CO2 by the
: solution, which
: > increases Ct as pH increases.To bad we can't or my server won't allow me,
: to post
: > attachments. I have a nice BC cure of various species as a function of
: pC/pH diagrams, set
: > to a pKa. curve
: >
: >
: > On another issue
: >
: > "In order to remove CO2 (g) you ideally would want to shift
: > the equilibrium to the left by LOWERING the pH"
: >
: >
: > You may want to try and re-explain this
: >
: > CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
: > HCO3-1 <-------> CO3-2
: >
: >
: > As the reaction shifts to left the pH gets higher as CO2 leaves the
: system.You don't have
: > to lower the pH to remove CO2. Case in point plants. As they remove CO2
: the pH rises,
: > continued removal of the Sigma CO2 ( CO2, H2CO3, HCO3,CO3) cause further
: rising until
: > there is mostly only carbonate (CO3) left and a high pH. Another case, at
: a pH of 8.00 and
: > Alk of 4 meq / l ( 1.4 mg / l CO2) you have much more CO2 than at 2 meq/
: l (0.65mg / l).
: > . Aeration of the water can drive off the CO, no lowering of the pH
: required., the removal
: > will cause the pH to rise .On the other hand, trying to remove CO2 @ 2 meq
: / l won't get
: > you much of anywhere in this case. Also, even a low pH doesn't mean you
: can drive of CO2.
: > If the seawater pH was say 7.5, you would think not problem to drive off
: CO2. If the Alk
: > was 0.25 there would be about .35 mg / l CO2 to blow off. At the alk of
: 4.00 meq / l the
: > CO2 is 5 mg / l.Usually, when people have a lower pH, say 7.9 or so, it is
: do to CO2, so
: > the pH has lowered, increasing the CO2, to allow one to blow it off easier
: and bring the
: > pH back up.
: >
: > CO2 = [CA(Carbonate Alk) x aH ] / [pK1(1 + 2pK2 /aH)]
: >
: > I think we just got off on the wrong foot, hope things look better.
: >
: > I'll be gone for the weekend, leaving in an hour, so have a nice weekend
: :-)
: >
: >
: >
: >
: > --
: > Boomer
: >
: > Want to talk chemistry ? The Reef Chemistry Forum
: > http://www.reefcentral.com/vbulletin/index.php
: >
: > Want to See More ?
: > Please Join Our Growing Membership
: > www.coralrealm.com
: >
: > If You See Me Running You Better Catch-Up
: > "stoutman" <.@.> wrote in message news:lcRWb.299984$na.451117@attbi_s04...
: > : > Humm, since when does Alk have anything to do in regards to the
: addition
: > : of BASE.
: > :
: > : You tell me. Your the one that posted a link to a web page that had
: this
: > : definition of alkalinity. Looks like you put yourself in your own hole
: pal.
: > :
: > : Remember posting this link:
: > :
: > : http://www.waterontheweb.org/resources/glossary.html
: > :
: > : Here is the definition of alkalinity from the web page YOU cited. (I
: > : recommend you read the web pages you are citing before you cite them)
: > : Alkalinity:
: > : Acid neutralizing or buffering capacity of water; a measure of the
: ability
: > : of water to resist changes in pH caused by the addition of acids or
: BASES.
: > :
: > :
: > : > It sure is funny how all of the chemist that write water chemistry
: > : textbooks never say Alk
: > : > is the Buffering Capacity of a solution.
: > :
: > : Neither did I. I said (for the umpth teen time) Alkalinity is a
: > : measurement of BUFFERING CAPACITY.
: > :
: > : When you measure alkalinity you know your BUFFERING CAPACITY (if you
: know
: > : your pH). Its a two for one.
: > :
: > : SEE MY OTHER POST FROM TODAY.
: > :
: > :
: > :
: > : "Boomer" > wrote in message
: > : ...
: > : >
: > : > "I am not sure if you are just messing with me "
: > : >
: > : > Yes, messing with you, it is called trolling a troll, to see where the
: > : hell you would go
: > : > and what you would say in regards to last posts. It is called honesty,
: of
: > : which you have
: > : > none off to say the least,that I can see.You always like to post what
: > : suits you and just
: > : > avoid ref I give. So lets start where you are WRONG and have a great
: lack
: > : of understanding
: > : > of things, to include pointing out all your gross error which you
: still
: > : FAIL to
: > : > acknowledge and which can be prove in many water chem. ref. .I doubt
: like
: > : hell you are a
: > : > chemist at all.You seem to want to con people into thinkin' you are.
: But
: > : then again, I
: > : > have seen chemists like you before, they are not familiar with the,
: but
: > : they ASK to have
: > : > it explained and ask for REF.YOU just shoot from the hip. WHAT GETS
: YOU IN
: > : TROUBLE. You
: > : > remind me of snoot-noise kid that come here and other NG's and
: > : forums...that think they
: > : > know, buy hey, maybe I'm wrong :-)
: > : >
: > : >
: > : >
: > : > 1). Acidity
: > : >
: > : > "***Benjamin,Water Chemistry (2002, pages 262-263).***
: > : >
: > : > ***Acidity A concept that is exactly analogous to alkalinity but
: measures
: > : the base
: > : > neutralizing
: > : > capacity (BNC) of a solution is Acidity. The quantitative represents
: the
: > : concentration of
: > : > OH- ions that must be added to titrate the solution to a pH near
: 10.5***
: > : >
: > : > So that means that not only in Benjamin wrong but, so are Stumm &
: Morgan,
: > : Millero, Pilosn,
: > : > Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I
: > : said, you have your
: > : > acidity and Acidy mixed up. Acidity as defined above is covered in
: most
: > : water chemistry
: > : > books, written by chemists, who's field of expertise is water
: chemistry.
: > : You can even buy
: > : > Acidity test kits from, HACH, LaMotte, etc..
: > : >
: > : > You mean you didn't read this or are you just avoiding it .The same
: > : definition can be
: > : > found in almost any std water chemistry book.
: > : >
: > : > I have run into few chemists, that are NOT familiar with the above.
: Some
: > : water reports
: > : > require the above Acidity measuring. The issue with you is you do not
: > : understand WATER
: > : > CHEMISTRY. Everything you have posted can be found a general chemistry
: > : book
: > : >
: > : >
: > : >
: > : >
: > : > 2) Alk and BC
: > : >
: > : > From the link
: > : >
: > : > Alkalinity
: > : > ***Acid neutralizing or buffering capacity of water; a measure of the
: > : ability of water to
: > : > resist changes in pH caused by the addition of acids or bases ***
: > : >
: > : > This is a Buffering Capacity definition not Alk
: > : >
: > : > Humm, since when does Alk have anything to do in regards to the
: addition
: > : of BASE. As I
: > : > pointed out in the first post the term is often miss used. Even in
: YOUR
: > : own posts you say
: > : > it is based on a acid addition, no mention of **base or acid**
: addition
: > : by you. Are you
: > : > getting confused or what. Or is more you are trying to confuse
: everyone
: > : you are right. The
: > : > above is a definition for Buffer Capacity NOT Alk
: > : >
: > : > From Drew, Geochemistry of Natural Waters
: > : >
: > : > "alkalinity, which is formally defined as the equivalent sum of bases
: that
: > : are titratable
: > : > with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH
: of
: > : the solution is
: > : > progressively lowered by the addition of a strong acid (HCL), all the
: > : anions on the right
: > : > will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4,
: H2S,organic
: > : acids, H20)"
: > : >
: > : > This follows almost all description of Alk, that it is acid
: neutralizing
: > : reaction and has
: > : > nothing to do with base neutralizing, which is Acidity (BNC) .I
: defined
: > : these before you
: > : > had no comment
: > : >
: > : >
: > : > Even the links that give the Buffering Capacity definition is wrong,
: as is
: > : the UIPAC on
: > : > Alkalinity. Alkalinity has nothing to do with the addition of bases
: only
: > : acids. When you
: > : > use the words "base and acid" it becomes BC
: > : >
: > : > Even YOU MUST disagree with these definitions, from YOUR own post
: > : >
: > : > Think of alkalinity as 'buffering capacity'. Or the ability of a
: solution
: > : > ***to resist a drop in pH due to the addition of acid***
: > : >
: > : > Where the flip is the base addition forget it ?
: > : >
: > : > From Butler; Carbon Dioxide Equilibrium and Their Applications
: (professor
: > : emeritus
: > : > Harvard University) an expert on the subject.
: > : >
: > : > Buffering Index (Buffering Capacity, Buffer Intensity).
: > : >
: > : > ***This concept was first developed for mixtures of approximately
: equal
: > : proportions of
: > : > conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such
: > : buffer solutions
: > : > strongly resist changes in pH when acids or bases are added and are
: useful
: > : as pH
: > : > standards. The Buffer Index tells how great the resistance to pH
: changes
: > : will be.**
: > : >
: > : > also from Butler
: > : >
: > : > Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
: > : >
: > : > Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
: > : >
: > : > Acidity is in fact just the negative of Alkalinity ***
: > : >
: > : > http://www.lagoonsonline.com/acid.htm
: > : >
: > : >
: > :
: http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.h
: > : tm?E+mystore
: > : >
: > : > It sure is funny how all of the chemist that write water chemistry
: > : textbooks never say Alk
: > : > is the Buffering Capacity of a solution. They are always treated and
: > : defined separately.
: > : >
: > : > If you or others choose to treat Alk and BC as the same, well, just
: have
: > : at it. As I said
: > : > in first post I know what you mean.
: > : >
: > : > "No need to cite web pages that describe what I know and what I wrote
: > : > in this discussion"
: > : >
: > : > No you don't know, who are you trying to convince any way, me, the
: guys
: > : here and/or all
: > : > the water chemists in this world. As I said before go get a dam WATER
: > : CHEMISTRY book or
: > : > shut the hell up.You keep trying to define things from a general
: chemistry
: > : book WE ARE IN
: > : > THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
: > : >
: > : >
: > : >
: > : >
: > : >
: > : > 3). pKa's and what you don't know or seem to be confused on
: > : >
: > : > "Therefore, it has two pKa's
: > : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
: > : The
: > : > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated
: is
: > : > right in there. Is that magic? :)"
: > : >
: > : > Here it is agin that is twice at least
: > : >
: > : > "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this
: > : example)
: > : > you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium
: will
: > : > be shifted to HCO3-2 by a ratio of 1:100.
: > : >
: > : > Oh wait , there is a third time LOL
: > : >
: > : > "At the pH of seawater, the buffering capacity of carbonate is at it's
: > : > weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
: > : >
: > : >
: > : > Lets just dunk you on this one. I am taking note you refuse to reply
: to
: > : YOUR errors
: > : >
: > : > So you calculated the pH of seawater with freshwater pKa's, now that
: is a
: > : good trick. From
: > : > a number of seawater chemistry books the seawater pKa's are 6 & 9.1,
: so
: > : according to you,
: > : > seemingly not understanding your favorite Henderson-Hasselbach equatio
: n;
: > : >
: > : > 2 pH = (6 + 9.1) /2 pH = 7.55
: > : >
: > : > I have never seen seawater with a pH of 7.55. There is no ocean with
: that
: > : pH. Humm how
: > : > come your equation is not working for you today.?
: > : >
: > : >
: > : > "That pH I calculated is
: > : > right in there. Is that magic? :)"
: > : >
: > : > I roll on the floor when I see this = 8.35
: > : >
: > : > Hum , just a brain far so excuse me for thinkin
: > : >
: > : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
: > : >
: > : > Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a
: pH of
: > : 8.35 there pal
: > : > ? That 8.35 is what you are telling people the pH should be, but their
: > : meter says 6.4.
: > : > This how people will READ this.
: > : >
: > : >
: > : >
: > : >
: > : > 4.) More on Buffering Capacity
: > : >
: > : > "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes,
: your
: > : > alkalinity equation."'
: > : >
: > : >
: > : > Yup, I see that and in this case the HCO3 is the acid and the CO3 is
: the
: > : base CORRECT. In
: > : > Alk you are only dealing with bases and how they react to an acid.
: Acidity
: > : deals acids and
: > : > how they recact to bases "Acidity, A concept that is exactly analogous
: to
: > : alkalinity but
: > : > measures the base neutralizing
: > : > capacity (BNC) of a solution is Acidity "Alk is the ANC Acid
: neutralizing
: > : capacity
: > : >
: > : > "Don't the components of a buffer account for the buffering capacity?
: "
: > : >
: > : > Yes, they do but so do the acids which work as buffers. NaHCO3 is a
: buffer
: > : and can act as
: > : > an acid or base
: > : >
: > : > *** Buffering Capacity.**
: > : > The power of a substance in solution to absorb acid or alkali without
: > : change in pH; this
: > : > is highest at a pH value equal to the pKa value of the acid of the
: buffer
: > : pair.***
: > : >
: > : > ***Akalinity***
: > : > Measure of the power of a solution to neutralise hydrogen ions (H+),
: > : usually expressed as
: > : > the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
: > : >
: > : >
: > : > If one wants to call Alk Buffering capacity then one sure as a hell
: can
: > : call Acidty
: > : > Buffering Capacity also. As it is the ability to neutralizes an acid
: that
: > : is a buffer.You
: > : > have a pH of 7 and you add a buffer to lower it to a pH of 4, you are
: > : buffering the water,
: > : > that buffer is a acid.
: > : >
: > : > 5) CO2
: > : >
: > : > You are really confuse so it seems :-) You realllllllly indicate that
: CO2
: > : is affected by
: > : > the Alk or vise-versa
: > : >
: > : > "Yes, the pH will drop with the addition of CO2. Remove CO2 will
: cause
: > : the
: > : > pH to rise? How do you remove CO2? Once it is in solution it forms
: > : > carbonic acid and neutralizes some of your 'buffer'."
: > : >
: > : > "With the exception of CO2?"
: > : >
: > : > No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
: > : > Concepts)....PERIOD.You seem to think a that at least in two of your
: post
: > : that CO2 is
: > : > affected by the Alk or vise-versa. Please go back to school or seek
: > : professor
: > : >
: > : > "Why in one case does CO2 from air lower pH and in the other case it
: > : raises
: > : > it? Doesn't make sense."
: > : >
: > : > That is because you don't understand CO2 period. By the way I saved
: this,
: > : wanted to see
: > : > if you would bite on the post I gave. Not bite at first, so time to
: reel
: > : you in, as you
: > : > did bite in another post..
: > : >
: > : > Lets make some sense of it for you, being that you have a pH.D in
: > : chemistry, so you say .
: > : >
: > : > CO2 is naturally generated in a aquatic systems, it is capable of
: raise to
: > : various levels
: > : > depending on a number of circumstances .It can be measure (except in
: > : seawater) or
: > : > calculated using Buch/Park Equations (what we use for seawater. In
: sort if
: > : you know the pH
: > : > and Alk you can calculate the CO2). If you aerate a system or a sample
: of
: > : water, even if
: > : > the pH has only dropped a couple of tenths, due to an increase in CO2,
: the
: > : CO2 will leave
: > : > solution to the atmosphere.This will raise the pH. On the other hand
: if
: > : theCO2 level is
: > : > more of the norm and you have hikgh room air, such as in the winter,
: the
: > : partial pressure
: > : > of the CO2 in air will be much higher than that in water, in which
: case
: > : the CO2 will enter
: > : > the water and lower the pH. That is without an airstone. Adding an
: > : airstone will make it
: > : > even worse,as you are now forcefully driving the CO2 into solution
: even
: > : quicker. These
: > : > test /experiments have been proven many times, it is not that may work
: > : could work they do
: > : > work.Yet you want to disagree and in another post say you haven't
: tried
: > : it,.Seems to me
: > : > that based on what you say it can't work So, in short you don't know
: what
: > : the hell you are
: > : > taking about. Go get a glass of seawater with a pH of about 8.3 and
: lower
: > : it to about
: > : > 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK-
: UP
: > : ( that is if you
: > : > don't have a high room air CO2 problem.). This little test has been
: done
: > : thousands of
: > : > times in this hobby, with test kits, pH meters and even graphic
: printers.
: > : >
: > : > "This is where Boomer and I
: > : > disagree. I say you would have to lower the pH very low in order to
: > : > effectively remove CO2 by purging."
: > : >
: > : > You are 100 % wrong. Please come to our Chem forum and try and run
: that by
: > : Randy, don't
: > : > take my word on it. I already know what he will say.
: > : >
: > : > "Boomer didnt convince me it
: > : > works at the pH of an aquarium, but I never tried it and I'm not sure
: of
: > : > this. "
: > : >
: > : > Well then come too our chem. forum and tell Randy he doesn't know what
: he
: > : is talking about
: > : > LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it
: > : should be easy for
: > : > you to run the experiment LOL There are grade school kids that run the
: > : test and know what
: > : > happens and that I'm correct.
: > : >
: > : >
: > : > "The equilibrium is a FUNCTION
: > : > of pH."
: > : >
: > : > It is also a function of Alk or don't you know that. At a pH of 8.3,
: Alk
: > : 2.25, the CO2 is
: > : > about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk
: to
: > : about .4 meq/ l
: > : > or so the CO2 will be around .99 mg / l CO2, When dealing with
: tanksCO2 is
: > : not always in
: > : > equilibrium with ambient air.
: > : >
: > : >
: > : > ". But I wouldn't degas a solution of a
: > : > specific gas (CO2) with a gas (this case he was using air) that
: contains
: > : the
: > : > same gas I am trying to purge."
: > : >
: > : > Why not ? We have a guy right now that is running tests on purging
: ambient
: > : air with a
: > : > solution to remove CO2 gas from the air, before it enters the tank
: > : per/Randy's suggestion.
: > : > The same guy is doing some of my test using a Clinoptilolite, a
: Zeolite
: > : mineral, that has
: > : > an affinity for CO2.This will be a dry CO2 scrubber
: > : >
: > : >
: > : > Sorry Soutman but you sure as hell don't seem to know much about
: aquatic
: > : chemistry. You
: > : > seem to be guessing at everything.
: > : >
: > : > By the way have you read any of Randy's technical articles on water
: > : chemistry, been saving
: > : > these for last. There are a few on pH, Alk, CO2 .Here is a list
: > : >
: > : > Try and answer them 1-5 and lets see where we get THIS TIME :-) or
: maybe
: > : we should just
: > : > drop it. I could care less at this point.
: > : >
: > : > THE END
: > : >
: > : >
: > : > ARTICLES
: > : >
: > : > The first two posts in this thread are lists of some of my articles
: that
: > : relate to reef
: > : > tank chemistry. In the next few posts are some of the articles
: published
: > : by Craig Bingman
: > : > and others on reef chemistry issues.
: > : >
: > : > The first two posts in this thread are lists of some of my articles
: that
: > : relate to reef
: > : > tank chemistry. In the next few posts are some of the articles
: published
: > : by Craig Bingman
: > : > and others on reef chemistry issues.
: > : >
: > : > Solving Common Problems
: > : >
: > : > Solving Calcium and Alkalinity Problems
: > : > http://www.advancedaquarist.com/issues/nov2002/chem.htm
: > : >
: > : > Solutions to pH Problems
: > : > http://www.advancedaquarist.com/iss...ne2002/chem.htm
: > : >
: > : > How to Select a Calcium and Alkalinity Supplementation Scheme
: > : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
: > : >
: > : > Phosphate Issues
: > : > http://www.advancedaquarist.com/iss...pt2002/chem.htm
: > : >
: > : > Nitrate Issues
: > : > http://www.advancedaquarist.com/iss...st2003/chem.htm
: > : >
: > : >
: > : >
: > : > Calcium and Alkalinity
: > : >
: > : > Solving Calcium and Alkalinity Problems
: > : > http://www.advancedaquarist.com/issues/nov2002/chem.htm
: > : >
: > : > How to Select a Calcium and Alkalinity Supplementation Scheme
: > : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
: > : >
: > : > Calcium and Alkalinity Balance Issues
: > : > http://reefkeeping.com/issues/2002-...ature/index.htm
: > : >
: > : > Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
: > : > http://www.advancedaquarist.com/iss...ly2002/chem.htm
: > : >
: > : > The Relationship Between Alkalinity and pH.
: > : > http://www.advancedaquarist.com/issues/may2002/chem.htm
: > : >
: > : > The Chemical & Biochemical Mechanisms of Calcification in Corals
: > : > http://www.advancedaquarist.com/issues/apr2002/chem.htm
: > : >
: > : > Calcium
: > : > http://www.advancedaquarist.com/issues/mar2002/chem.htm
: > : >
: > : > Alkalinity
: > : > http://www.advancedaquarist.com/iss...2/chemistry.htm
: > : >
: > : >
: > : > Iron
: > : >
: > : > First Iron Article: Macroalgae and Dosing Recommendations
: > : > http://www.advancedaquarist.com/issues/aug2002/chem.htm
: > : >
: > : > Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
: > : > http://www.advancedaquarist.com/issues/oct2002/chem.htm
: > : >
: > : > Iodine
: > : >
: > : > Iodine in Marine Aquaria: Part I
: > : > http://www.advancedaquarist.com/issues/mar2003/chem.htm
: > : >
: > : > Iodine in Reef Tanks 2: Effects on Macroalgae Growth
: > : > http://www.advancedaquarist.com/iss...il2003/chem.htm
: > : >
: > : >
: > : > Magnesium and Strontium
: > : >
: > : > Strontium
: > : > http://www.advancedaquarist.com/issues/nov2003/chem.htm
: > : >
: > : > Magnesium
: > : > http://www.advancedaquarist.com/issues/oct2003/chem.htm
: > : >
: > : > Magnesium and Strontium in Limewater
: > : > http://www.advancedaquarist.com/issues/dec2003/chem.htm
: > : >
: > : >
: > : > Limewater (kalkwasser)
: > : >
: > : > The Self Purification of Limewater (Kalkwasser)
: > : > http://www.advancedaquarist.com/issues/may2003/chem.htm
: > : >
: > : > The Degradation of Limewater (Kalkwasser) in Air
: > : > http://reefkeeping.com/issues/2003-...ature/index.htm
: > : >
: > : > How to Select a Calcium and Alkalinity Supplementation Scheme
: > : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
: > : >
: > : > Metals in Aquaria
: > : >
: > : > Aluminum and aluminum-based phosphate binders
: > : > http://www.advancedaquarist.com/iss...ly2003/chem.htm
: > : >
: > : > Reef Aquaria with Low Soluble Metals
: > : > http://reefkeeping.com/issues/2003-...ature/index.htm
: > : >
: > : > Tap Water in Reef Aquaria
: > : > http://www.advancedaquarist.com/issues/jan2004/chem.htm
: > : > First Iron Article: Macroalgae and Dosing Recommendations
: > : > http://www.advancedaquarist.com/issues/aug2002/chem.htm
: > : >
: > : > Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
: > : > http://www.advancedaquarist.com/issues/oct2002/chem.htm
: > : >
: > : >
: > : > Test Kit Reviews
: > : >
: > : > The Seachem Borate Alkalinity Test Kit
: > : > http://www.advancedaquarist.com/iss...ne2003/chem.htm
: > : >
: > : > The Salifert Boron Test Kit
: > : > http://www.advancedaquarist.com/iss...pt2003/chem.htm
: > : >
: > : > Boron and Borate (and pH buffering)
: > : >
: > : > Boron in a Reef Tank (and its effect on pH buffering)
: > : > http://www.advancedaquarist.com/issues/dec2002/chem.htm
: > : >
: > : > The Seachem Borate Alkalinity Test Kit
: > : > http://www.advancedaquarist.com/iss...ne2003/chem.htm
: > : >
: > : > The Salifert Boron Test Kit
: > : > http://www.advancedaquarist.com/iss...pt2003/chem.htm
: > : >
: > : >
: > : >
: > : > Others
: > : >
: > : > Tap Water in Reef Aquaria
: > : > http://www.advancedaquarist.com/issues/jan2004/chem.htm
: > : >
: > : > ORP
: > : > http://reefkeeping.com/issues/2003-...ature/index.htm
: > : >
: > : > Chloramine
: > : > http://reefkeeping.com/issues/2003-...ature/index.htm
: > : >
: > : > Silica in a Reef Tank
: > : > http://advancedaquarist.com/issues/jan2003/feature.htm
: > : >
: > : > Specific Gravity (and temperature correction of hydrometers)
: > : > http://www.advancedaquarist.com/iss...2/chemistry.htm
: > : >
: > : >
: > : > The Complete Nitrogen Cycle
: > : > http://www.animalnetwork.com/fish/l...a&RecordNo=3090
: > : >
: > : > Magnesium (older article with fonts screwed up)
: > : > http://www.aquariumfish.com/aquariu...cid=124&search=
: > : >
: > : > Phosphate (older article now reproduced in a poor fashion)
: > : > http://www.aquariumfish.com/aquariu...cid=124&search=
: > : >
: > : > Carbon Dioxide
: > : > http://www.animalnetwork.com/fish/l...a&RecordNo=2074
: > : >
: > : > Using Conductivity to Measure Salinity
: > : > http://www.aquariumfish.com/aquariu...cid=124&search=
: > : >
: > : > Understanding Seawater
: > : > http://www.animalnetwork.com/fish2/...s/1/default.asp
: > : >
: > : > Protein Skimming: How It Works
: > : > http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
: > : >
: > : >
: > : >
: > : > Articles by Craig Bingman:
: > : >
: > : > Carbon Dioxide tests
: > : > http://www.animalnetwork.com/fish/l...n=&RecordNo=279
: > : >
: > : > Limewater, Acetic Acid and Sand Clumping
: > : > http://www.animalnetwork.com/fish/l...n=&RecordNo=181
: > : >
: > : > Calcium and Alkalinity
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Calculation of Calcium Carbonate Saturation States in Reef Aquaria
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : >
: > : > Calcification Rates in Several Tropical Coral Reef Aquaria
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Limits To Limewater...Revisited
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Expanding the Limits of Limewater: Adding Organic Carbon Sources
: (vinegar)
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : >
: > : > Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Magnesium - Part I
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Magnesium - Part II
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > A Homemade Magnesium Supplement
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Simulating the Effect of Calcium Chloride and Sodium Bicarbonate
: Additions
: > : on Reef Systems
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Additional Simulations: The Combined Effect Of Calcium Chloride
: > : > /Sodium Bicarbonate Additions And Water Exchanges
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : >
: > : > More articles by Craig Bingman:
: > : >
: > : > The Halogens - Part I: Bromine in Seawater and Aquaria
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > The Halogens - Part II: Fluoride
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Fluoride Depletion In Four Reef Aquariums
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > The Halogens - Part III: Iodine
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Measuring Halides
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > How Test Kits Work
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Borax pH Calibration
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > A pH Detective Story
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > How to Mix a Batch of Synthetic Seawater in Under Five Minutes
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > SILICON - FOE OR FRIEND?
: > : > http://www.animalnetwork.com/fish2/...s/1/default.asp
: > : >
: > : > The Composition Of Several Synthetic Seawater Mixes
: > : > http://www.animalnetwork.com/fish2/...s/1/default.asp
: > : >
: > : > Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : >
: > : >
: > : > Andy's calcium calculator
: > : > http://www.andy-hipkiss.co.uk/cacalc.htm
: > : >
: > : > Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
: > : > http://www.aquariumfish.com/aquariu...cid=124&search=
: > : >
: > : > Calcium Reactor Substrate -- Phosphate Levels
: > : > by Greg Hiller
: > : > http://www.advancedaquarist.com/iss...l2003/short.htm
: > : >
: > : >
: > : > Indoor CO2 Problems
: > : > http://www.advancedaquarist.com/iss...r2002/short.htm
: > : >
: > : > Simon Huntington's CaCO3/CO2 reactor article
: > : >
: > : > http://reefkeeping.com/issues/2002-...ature/index.htm
: > : >
: > : > Ron Shimek's Tank Water Analysis Article
: > : > http://reefkeeping.com/issues/2002-...ature/index.htm
: > : >
: > : >
: > : >
: > : >
: > : > Home made salinity standards thread:
: > : >
: > : > http://reefcentral.com/forums/showt...?threadid=65509
: > : >
: > : > Reef Chemicals Calculator
: > : > http://www.kademani.com/reefchem.htm
: > : >
: > : >
: > : >
: > : > Boomer
: > : >
: > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > http://www.reefcentral.com/vbulletin/index.php
: > : >
: > : >
: > : > Former US Army Bomb Technician (EOD)
: > : > Member; IABTI, NATEODA, WEODF, ISEE & IPS
: > : >
: > : > If You See Me Running You Better Catch-Up
: > : >
: > : >
: > : > --
: > : > Boomer
: > : >
: > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > http://www.reefcentral.com/vbulletin/index.php
: > : >
: > : > Want to See More ?
: > : > Please Join Our Growing Membership
: > : > www.coralrealm.com
: > : >
: > : > If You See Me Running You Better Catch-Up
: > : > "stoutman" <.@.> wrote in message
: > : news:aGuWb.148227$U%5.676753@attbi_s03...
: > : > : Boomer,
: > : > :
: > : > : I am not sure if you are just messing with me or if you are truly
: > : confused.
: > : > : I hope the latter. Please read from Top to Bottom.
: > : > :
: > : > :
: > : > : From YOUR first link:
: > : > :
: > : > : http://www.waterontheweb.org/resources/glossary.html
: > : > :
: > : > : Acidity:
: > : > : A measure of how acid a solution may be. A solution with a pH of
: less
: > : than
: > : > : 7.0 is considered acidic. Solutions with a pH of less than 4.5
: contain
: > : > : mineral acidity (due to strong inorganic acids), while a solution
: having
: > : a
: > : > : pH greater than 8.3 contains no acidity.
: > : > :
: > : > : Yes,
: > : > :
: > : > : Good definition (for the most part). pH <7 is indeed acidic. pH >
: 7 is
: > : > : basic. Your web page had a definition for acidity, but not
: basicity.
: > : > : Strange. That's like defining GOOD and not defining BAD.
: > : > :
: > : > : Here is the IUPAC (International Union of Pure and Applied
: Chemistry)
: > : > : definition of acidity:
: > : > :
: > : > : http://www.chem.qmul.ac.uk/iupac/index.html
: > : > :
: > : > : acidity
: > : > :
: > : > : (1) Of a compound:
: > : > :
: > : > : For Brønsted acids it means the tendency of a compound to act as a
: > : hydron
: > : > : donor. It can be quantitatively expressed by the acid dissociation
: > : constant
: > : > : of the compound in water or some other specified medium. For Lewis
: acids
: > : it
: > : > : relates to the association constants of Lewis adducts and -adducts.
: > : > :
: > : > : (2) Of a medium:
: > : > :
: > : > : The use of the term is mainly restricted to a medium containing
: Brønsted
: > : > : acids, where it means the tendency of the medium to hydronate a
: specific
: > : > : reference base
: > : > :
: > : > : basicity
: > : > :
: > : > : For Brønsted bases it means the tendency of a compound to act as
: hydron
: > : > : (proton) acceptor. The basicity of a chemical species is normally
: > : expressed
: > : > : by the acidity of the conjugate acid (see conjugate acid-base pair).
: For
: > : > : Lewis bases it relates to the association constants of Lewis adducts
: > : > : and -adducts
: > : > :
: > : > :
: > : > :
: > : > : Another definition from the same web page YOU cited: (this is the
: same
: > : web
: > : > : page you cited above)
: > : > :
: > : > : Alkalinity:
: > : > : Acid neutralizing or buffering capacity of water; a measure of the
: > : ability
: > : > : of water to resist changes in pH caused by the addition of acids or
: > : bases
: > : > : and therefore, the main indicator of susceptibility to acid rain; in
: > : natural
: > : > : waters it is due primarily to the presence of bicarbonates,
: carbonates
: > : and
: > : > : to a much lesser extent occasionally borates, silicates and
: phosphates.
: > : It
: > : > : is expressed in units of milligrams per liter (mg/l) of CaCO3
: (calcium
: > : > : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l =
: 1
: > : mg/l
: > : > : of CaCO3. A solution having a pH below about 5 contains no
: alkalinity.
: > : > :
: > : > : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and
: says
: > : > : that alkalinity is the measure of ...(description of a buffer)
: > : > :
: > : > : A BUFFER IS : a measure of the ability of water to resist changes in
: pH
: > : > : caused by the addition of acids or bases (from definition below)
: > : > :
: > : > :
: > : > : I said:
: > : > : ***alkalinity is a measurement of 'buffering capacity'***
: > : > :
: > : > : You said:
: > : > : ***Alkalinity is not a measurement of BC
: > : > :
: > : > : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is
: not
: > : > : logical.
: > : > :
: > : > : (THIS FROM THE SAME WEB PAGE YOU CITED):
: > : > :
: > : > : Buffer:
: > : > : A substance which tends to keep pH levels fairly constant when acids
: or
: > : > : bases are added.
: > : > :
: > : > : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
: > : > :
: > : > : a measure of the ability of water to resist changes in pH caused by
: the
: > : > : addition of acids or bases
: > : > :
: > : > : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A
: BUFFER.
: > : > :
: > : > :
: > : > : I went to all four links. None contradict what I have said. But
: the
: > : first
: > : > : one you cited contradicts YOU!
: > : > :
: > : > : I know what a buffer is. I know what acidity means. I know what
: > : alkalinity
: > : > : means. No need to cite web pages that describe what I know and what
: I
: > : wrote
: > : > : in this discussion. Show me one that says alkalinity is not a
: measure
: > : of
: > : > : buffering capacity from a credible source.
: > : > :
: > : > :
: > : > :
: > : > :
: > : > :
: > : > :
: > : > : "Boomer" > wrote in message
: > : > : ...
: > : > : > Alkalinity a measure of the amount of anions of weak acid in water
: and
: > : of
: > : > : the cations
: > : > : > balanced against them
: > : > : > Take note it says ***acid***
: > : > : >
: > : > : > Buffering capacity the ability of a solution to resist or dampen
: > : changes
: > : > : in pH upon the
: > : > : > addition of acids or bases.
: > : > : > Take note its says ***the addition of acids or bases***
: > : > : >
: > : > : > One more
: > : > : >
: > : > : > http://www.waterontheweb.org/resources/glossary.html
: > : > : >
: > : > : > We could go on like this all day, so what is the point ?
: > : > : >
: > : > : > You will LOVE this one
: > : > : > http://www.kyantec.com/Tips/phbuffering.htm
: > : > : >
: > : > : > Don't you just lovbe PDF's
: > : > : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
: > : > : >
: > : > : > Don't fall out of your chair
: > : > : >
: http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
: > : > : >
: > : > : >
: > : > : >
: > : > : >
: > : > : > --
: > : > : > Boomer
: > : > : >
: > : > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > : > http://www.reefcentral.com/vbulletin/index.php
: > : > : >
: > : > : > Want to See More ?
: > : > : > Please Join Our Growing Membership
: > : > : > www.coralrealm.com
: > : > : >
: > : > : > If You See Me Running You Better Catch-Up
: > : > : > "stoutman" <.@.> wrote in message
: > : news:XB7Wb.19339$QA2.62332@attbi_s52...
: > : > : > : Man here is another, google is a wonderful thing. I'm not
: filtering
: > : any
: > : > : > : out, just posting what I find by GOOGLING for you.
: > : > : > :
: > : > : > :
: http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
: > : > : > :
: > : > : > :
: > : > : > : Wow, a gov link. Even the government is wrong, this must be a
: > : > : conspiracy
: > : > : > : against Boomer.
: > : > : > :
: > : > : > :
: > : > : > :
: > : > : > :
: > : > : > : "Boomer" > wrote in message
: > : > : > : ...
: > : > : > : > Now I am getting bored
: > : > : > : >
: > : > : > : > "Don't the components of a buffer account for the buffering
: > : capacity?
: > : > : > : Yes."
: > : > : > : >
: > : > : > : > Yes, agreed but you seem to fail what I'm saying. Buffering
: > : Capacity
: > : > : and
: > : > : > : Alkalinity are
: > : > : > : > not the same, that has always been the issue. I gave the
: equation
: > : does
: > : > : > : that look like an
: > : > : > : > Alkalinity equation or how Alk is determined. I see you had
: now
: > : > : comments
: > : > : > : on it what's
: > : > : > : > wrong, why no comments on the equations I gave. Don't
: understand
: > : them
: > : > : or
: > : > : > : what ? Again this
: > : > : > : > is the equation for Buffering Capacity, also called Buffer
: Index
: > : or
: > : > : Buffer
: > : > : > : Intensity. It
: > : > : > : > is defined in most water chemistry and chemical oceanography
: text
: > : > : books.
: > : > : > : >
: > : > : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] +
: [H30+] +
: > : > : CKa
: > : > : > : [H3O+] / (Ka =
: > : > : > : > H3O+])² )
: > : > : > : >
: > : > : > : > This is not Alkalinity now is it ?
: > : > : > : >
: > : > : > : > "I know how to do a titration, In fact I have done several.
: How
: > : many
: > : > : have
: > : > : > : > you actually done? I don't mean by counting drops, I mean
: with a
: > : > : buret?"
: > : > : > : >
: > : > : > : > Well good for you, I use a Digital Titrator
: > : > : > : >
: > : > : > : > "Oh, I see,
: > : > : > : > you think acidity is the opposite of alkalinity. In the world
: of
: > : > : > : CHEMISTRY
: > : > : > : > it's not. Maybe in aquarium newsgroups it is.
: > : > : > : >
: > : > : > : > Hum no, maybe you should go for a look at HACH's or LaMotte
: > : website or
: > : > : the
: > : > : > : book I
: > : > : > : > suggested earlier. Please view a copy.
: > : > : > : >
: > : > : > : > Standard Methods for the Examination of Water and Wastewater
: > : > : > : >
: > : > : > : > This book, over 2000 pages, is the guide for water testing. If
: you
: > : are
: > : > : > : reporting water
: > : > : > : > test to the EPA you must use approved std from this text.I t
: is
: > : > : prepared
: > : > : > : and published by
: > : > : > : > the EPA, American Water Works Association and American Public
: > : Health
: > : > : > : Association. You
: > : > : > : > mean you don't have one and the issue is water chemistry
: > : > : > : >
: > : > : > : > You are confusing Acidity and Acidity as you know little about
: > : water
: > : > : > : chemistry and
: > : > : > : > procedures and test methods
: > : > : > : >
: > : > : > : > From SMEWW, section 2-30, 2310 ACIDITY
: > : > : > : >
: > : > : > : > "Acidity of water is its quantative capacity to react with a
: > : strong
: > : > : base
: > : > : > : to a designated
: > : > : > : > pH"
: > : > : > : >
: > : > : > : > This is how you test for it
: > : > : > : >
: > : > : > : > A std alkali titration to methyl orange or phenolphthalein
: > : > : > : > endpoint.
: > : > : > : >
: > : > : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that
: > : write
: > : > : this
: > : > : > : book, there are
: > : > : > : > over 100 of them, they are wrong.
: > : > : > : >
: > : > : > : > Like Buffering Capacity you have your Acidity's mixed up
: > : > : > : > In water measurement if you have a high Alk you also usually
: have
: > : a
: > : > : high
: > : > : > : Acidity.
: > : > : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
: > : > : CHEMISTRY
: > : > : > : BOOK there pal.
: > : > : > : >
: > : > : > : >
: > : > : > : > "These are all in equilibrium with each other. An initial
: high pH
: > : > : (above
: > : > : > : > 6.4) will shift the equilibrium to the right to form HCO3-1.
: If
: > : the
: > : > : pH of
: > : > : > : > the solution is above 10.3 (pKa2) the .........."
: > : > : > : >
: > : > : > : >
: > : > : > : > Christ, there you go again with the FW ****. All your numbers
: are
: > : > : wrong we
: > : > : > : are dealing
: > : > : > : > with SEAWATER
: > : > : > : >
: > : > : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is
: in
: > : the
: > : > : form
: > : > : > : > of HCO3-1 .
: > : > : > : >
: > : > : > : > I have already pointed that out and gave actual values at know
: > : > : seawater
: > : > : > : levels, go back
: > : > : > : > and re-read it you aren't telling me anything here.Of course
: most
: > : is
: > : > : HCO3
: > : > : > : see...
: > : > : > : >
: > : > : > : >
: > : > : > : > @ 20C and 34.3 ppt salinity
: > : > : > : >
: > : > : > : > CO2 = 0.52 %
: > : > : > : >
: > : > : > : > HCO3 = 86.4 %
: > : > : > : >
: > : > : > : > CO3 = 13.09 %
: > : > : > : >
: > : > : > : >
: > : > : > : > "In your glass experiment you managed to lower the pH enough
: to
: > : purge
: > : > : out
: > : > : > : CO2
: > : > : > : > by boiling"
: > : > : > : >
: > : > : > : > The purpose behind the glass is to show that alk is not affect
: by
: > : CO2
: > : > : and
: > : > : > : vise-versa and
: > : > : > : > how Co2 affects pH.
: > : > : > : >
: > : > : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and
: that
: > : pH
: > : > : drops
: > : > : > : to say 8.1 it is
: > : > : > : > usually due to excess CO2. If you took a glass of that water
: and
: > : > : aerated
: > : > : > : it you WILL drive
: > : > : > : > off the CO2 and raise the pH. It has been done a proven a
: million
: > : > : times.
: > : > : > : >
: > : > : > : > "In order to 'purge' CO2 you would need to lower the
: > : > : > : > pH to shift the equilibrium to below 6.4"
: > : > : > : >
: > : > : > : > The hell you do !!!.Do you know who many times people on this
: NG
: > : to
: > : > : > : include Dr. Craig
: > : > : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned
: to
: > : take a
: > : > : > : sample of aquarium
: > : > : > : > water and aerate it to see if the pH GOES UP AND when they
: come
: > : back
: > : > : with
: > : > : > : the test it is
: > : > : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D
: CHEMIST
: > : > : excess
: > : > : > : CO2 in the tank
: > : > : > : > water, increase the circulation for better gas exchange at the
: > : > : surface,
: > : > : > : reduce feeding,
: > : > : > : > and try to improve on better skimming, thus reducing the
: bio-load
: > : and
: > : > : pH
: > : > : > : decline due to
: > : > : > : > CO2.
: > : > : > : >
: > : > : > : >
: > : > : > : > "I hope this helps. "
: > : > : > : >
: > : > : > : > Help, how can you when you miss everything. I should be
: charging
: > : you
: > : > : > : >
: > : > : > : > Oh, by the way. Your websites, I have about 50 on these
: issues, I
: > : > : could
: > : > : > : post them, not to
: > : > : > : > mention I have all those water chemistry books, so there is no
: > : need to
: > : > : > : view your sites.
: > : > : > : >
: > : > : > : > Finally are you afraid to come to our Chemistry Forum, afraid
: to
: > : get
: > : > : > : slapped by REAL
: > : > : > : > chemists. I get a charge out of you can't post your ref .I
: have
: > : posted
: > : > : the
: > : > : > : same or similar
: > : > : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have
: 1500
: > : > : posts
: > : > : > : there and am the
: > : > : > : > biggest contributor to his forum other than himself or maybe
: Habib
: > : > : Sheka
: > : > : > : >
: > : > : > : > Hum, here are Randy's ref that he posted. He hosts the website
: > : > : > : >
: > : > : > : > S. RANDY HOLMES-FARLEY
: > : > : > : > Arlington, Massachusetts
: > : > : > : >
: > : > : > : > EDUCATION
: > : > : > : >
: > : > : > : > 1982-1986 Harvard University Cambridge, MA
: > : > : > : > PhD in Chemistry
: > : > : > : > Research Advisor: George Whitesides
: > : > : > : >
: > : > : > : > Investigated the relationship between polymer surface
: chemistry
: > : and
: > : > : > : physical properties
: > : > : > : > through controlled surface modification and testing.
: > : > : > : >
: > : > : > : > 1980-1982 Cornell University Ithaca, NY
: > : > : > : > BA in Chemistry and Biology
: > : > : > : > Graduated Summa Cum Laude
: > : > : > : > Distinction in All Subjects
: > : > : > : > Grade Point: 3.94/4.0
: > : > : > : > Honors research: isolation and characterization of the subunit
: of
: > : CF1
: > : > : > : enzyme
: > : > : > : >
: > : > : > : >
: > : > : > : > 1978-1979 Stanford University Palo Alto, CA
: > : > : > : > Grade Point: 3.55/4.0
: > : > : > : >
: > : > : > : >
: > : > : > : > EXPERIENCE
: > : > : > : >
: > : > : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham,
: MA
: > : > : > : > (bought out GelTex Pharmaceuticals in 2001)
: > : > : > : > Vice President, Chemical Research 2001-present
: > : > : > : > Senior Director, Chemical Research 1999-2001
: > : > : > : > Director of Chemical Research 1997-1999
: > : > : > : > Manager of Chemical Research 1995-1997
: > : > : > : > Group Leader 1994-1995
: > : > : > : > Senior Research Scientist 1992-1994
: > : > : > : >
: > : > : > : > Helped start GelTex as second employee
: > : > : > : >
: > : > : > : > Managed various research programs with multi-million dollar
: > : budgets
: > : > : > : >
: > : > : > : > Supervised research chemists (17+)
: > : > : > : >
: > : > : > : > Co-inventor of several polymeric pharmaceuticals and
: > : pharmaceutical
: > : > : > : candidates including
: > : > : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam
: > : Hydrochloride
: > : > : (FDA
: > : > : > : approved)
: > : > : > : >
: > : > : > : > Company Safety Officer for 3 years
: > : > : > : >
: > : > : > : > Chemical Hygiene Officer 2000-present
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > 1990-1992 GTE Corporation Waltham, MA
: > : > : > : > Senior Member of Technical Staff
: > : > : > : > Applied research involving polymer interfaces
: > : > : > : > Metallization of plastics
: > : > : > : > Polymer/polymer adhesion
: > : > : > : > Optical coatings
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > 1986-1990 Lord Corporation Cary, NC
: > : > : > : > Senior Research Scientist 1988-1990
: > : > : > : > Research Scientist 1986-1988
: > : > : > : > Basic and applied research on surface chemical bonding
: > : > : > : > Developed new adhesive compositions
: > : > : > : > Developed new sol-gel coatings for corrosion resistance
: > : > : > : >
: > : > : > : >
: > : > : > : > HONORS AND AWARDS
: > : > : > : >
: > : > : > : > Industrial Innovations Award by Northeast Region of American
: > : Chemical
: > : > : > : Society (6/2001)
: > : > : > : >
: > : > : > : > National Kidney Foundation of Northern California Honoree
: (5/2001)
: > : > : > : >
: > : > : > : > American Chemical Society/Polymer Chemistry Division
: Industrial
: > : > : Sponsors
: > : > : > : > Award (8/2000)
: > : > : > : >
: > : > : > : > R&D 100 Award from R&D magazine (1999)
: > : > : > : >
: > : > : > : > Sherwin Williams Award in applied polymer science (9/85)
: > : > : > : >
: > : > : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985;
: > : 1985-1986)
: > : > : > : >
: > : > : > : > Award for highest GPA in Chemistry Department (6/82)
: > : > : > : >
: > : > : > : > Summa Cum Laude Honors in Chemistry (6/82)
: > : > : > : >
: > : > : > : > Phi Lamda Epsilon (6/82)
: > : > : > : >
: > : > : > : > Phi Beta Kappa (2/82)
: > : > : > : >
: > : > : > : > Cornell University Dean's List (1981, 1982)
: > : > : > : >
: > : > : > : > Harvard Book Club Award for highest GPA senior year (1978)
: > : > : > : >
: > : > : > : > First Place in western NY ACS high school chemistry exam
: (1977)
: > : > : > : >
: > : > : > : > 1978-1979
: > : > : > : >
: > : > : > : >
: > : > : > : > __________________
: > : > : > : > Randy Holmes-Farley
: > : > : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef
: > : Central
: > : > : > : >
: > : > : > : > Hobby Experience: 8 years with reefs
: > : > : > : > Current Tanks: 90 gal mixed reef
: > : > : > : > Interests: Reefkeeping, science, photography
: > : > : > : >
: > : > : > : >
: > : > : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
: > : > : > : >
: > : > : > : > Open this post in a new window | Report this post to a
: moderator |
: > : IP:
: > : > : > : Logged
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > 06/27/2003 02:44 PM
: > : > : > : >
: > : > : > : > Randy Holmes-Farley
: > : > : > : > Chemistry Moderator
: > : > : > : >
: > : > : > : > Registered: Apr 2001
: > : > : > : > Location: Arlington, Massachusetts
: > : > : > : > Occupation: Chemist (Drug Discovery at Genzyme)
: > : > : > : > Posts: 15282
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > Publications
: > : > : > : >
: > : > : > : >
: > : > : > : > ISSUED UNITED STATES PATENTS
: > : > : > : >
: > : > : > : >
: > : > : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen
: Randall;
: > : > : > : Mandeville, III; W. Harry.
: > : > : > : > US 6,566,407; 5/20/2003
: > : > : > : >
: > : > : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley,
: Stephen
: > : > : Randall;
: > : > : > : Huval, Chad
: > : > : > : > Cori.
: > : > : > : > U.S. 6,517,825; 2/11/2003.
: > : > : > : >
: > : > : > : > 3. Method of making phosphate-binding polymers for oral
: > : > : administration.
: > : > : > : Holmes-Farley,
: > : > : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M.
: U.S.
: > : > : > : 6,509,013; 1/21/2003.
: > : > : > : >
: > : > : > : > 4. Combination therapy for treating hypercholesterolemia using
: a
: > : bile
: > : > : acid
: > : > : > : sequestrant
: > : > : > : > polymer
: > : > : > : > and a cholesterol-lowering agent. Huval, Chad Cori;
: Holmes-Farley,
: > : > : Stephen
: > : > : > : Randall;
: > : > : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
: > : > : > : >
: > : > : > : > 5. Method for treating hypercholesterolemia with
: polyallylamine
: > : > : polymers.
: > : > : > : Holmes-Farley,
: > : > : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
: > : > : Goldberg,
: > : > : > : Dennis I. , US
: > : > : > : > 6,423,754; 7/23/2002.
: > : > : > : >
: > : > : > : > 6. Ionic polymers as anti-infective agents Mandeville, W.
: Harry,
: > : III;
: > : > : > : Neenan, Thomas X..;
: > : > : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
: > : > : > : >
: > : > : > : > 7. Combination therapy for treating hypercholesterolemia and
: > : > : > : atherosclerosis. Huval, Chad
: > : > : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal,
: > : Pradeep
: > : > : K.
: > : > : > : U.S. 6,365,186;
: > : > : > : > 4/2/2002.
: > : > : > : >
: > : > : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
: > : > : Mandeville,
: > : > : > : W. H., III;
: > : > : > : > Huval; C.
: > : > : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US
: 6,299,868;
: > : > : > : 10/9/2001.
: > : > : > : >
: > : > : > : > 9. Polymers containing guanidinium groups as bile acid
: > : sequestrants.
: > : > : Dhal;
: > : > : > : P. K.; Holmes-
: > : > : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
: > : > : > : >
: > : > : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.;
: Mandeville,
: > : W.
: > : > : H.,
: > : > : > : III.; US
: > : > : > : > 6,281,252;
: > : > : > : > 8/28/2001.
: > : > : > : >
: > : > : > : > 11. Combination therapy for treating hypercholestrolemia.
: Huval;
: > : C.
: > : > : C.;
: > : > : > : Holmes-Farley; S.
: > : > : > : > R. ;
: > : > : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
: > : > : > : >
: > : > : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides,
: G.
: > : M.;
: > : > : > : Holmes-Farley, S.
: > : > : > : > R.; US
: > : > : > : > 6,264,937; 7/24/2001.
: > : > : > : >
: > : > : > : > 13. Method for treating hypercholesterolemia with
: unsubstituted
: > : > : > : polydiallylamine polymers.
: > : > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
: K.
: > : ; US
: > : > : > : 6,248,318;
: > : > : > : > 6/19/2001.
: > : > : > : >
: > : > : > : > 14. Process for removing bile salts from a patient and
: alkylated
: > : > : > : compositions therefore.
: > : > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355;
: > : 5/1/2001.
: > : > : > : >
: > : > : > : > 15. Poly(diallylamine)-based bile acid sequestrants.
: > : Holmes-Farley, S.
: > : > : R.;
: > : > : > : Dhal, P. K.;
: > : > : > : > Petersen,
: > : > : > : > J. S.; US 6,203,785; 3/20/2001.
: > : > : > : >
: > : > : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S.
: R.;
: > : > : Huval,
: > : > : > : C. C.; US
: > : > : > : > 6,190,649;
: > : > : > : > 2/20/2001.
: > : > : > : >
: > : > : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.;
: Mandeville,
: > : W.
: > : > : H.,
: > : > : > : III.; US
: > : > : > : > 6,177,478;
: > : > : > : > 1/23/2001.
: > : > : > : >
: > : > : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
: > : > : Holmes-Farley,
: > : > : > : S. R.;
: > : > : > : > Mandeville, W.
: > : > : > : > H., III.; US 6,129,910; 10/10/2000.
: > : > : > : >
: > : > : > : > 19. Method for treating hypercholesterolemia with
: unsubstituted
: > : > : > : polydiallylamine polymers.
: > : > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
: K.
: > : ; US
: > : > : > : 6,083,497;
: > : > : > : > 7/4/2000.
: > : > : > : >
: > : > : > : > 20. Method of making phosphate-binding polymers for oral
: > : > : administration.
: > : > : > : Holmes-Farley, S.
: > : > : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US
: 6,083,495;
: > : > : 7/4/2000.
: > : > : > : >
: > : > : > : > 21. Process for removing bile salts from a patient and
: alkylated
: > : > : > : compositions therefore.
: > : > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
: > : > : 5/23/2000.
: > : > : > : >
: > : > : > : > 22. Process for removing bile salts from a patient and
: > : compositions
: > : > : > : therefor. Mandeville,
: > : > : > : > W. H.,
: > : > : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
: > : > : > : >
: > : > : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III;
: W.
: > : H;
: > : > : > : Neenan; T. X.; Holmes-
: > : > : > : > Farley; S. R. US 6,034,129; 3/7/2000.
: > : > : > : >
: > : > : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.;
: Mandeville,
: > : W.
: > : > : H.,
: > : > : > : III.; US
: > : > : > : > 5,985,938;
: > : > : > : > 11/16/99.
: > : > : > : >
: > : > : > : > 25. Process for removing bile salts from a patient and
: > : compositions
: > : > : > : therefor. Mandeville,
: > : > : > : > W. H.,
: > : > : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
: > : > : > : >
: > : > : > : > 26. Hydrophobic sequestrant for cholesterol depletion.
: Mandeville,
: > : W.
: > : > : H.,
: > : > : > : III.;
: > : > : > : > Holmes-Farley;
: > : > : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
: > : > : > : >
: > : > : > : > 27. Hydrophilic nonamine-containing and amine-containing
: > : copolymers
: > : > : and
: > : > : > : their use as bile
: > : > : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
: > : > : 5,929,184;
: > : > : > : 7/27/99.
: > : > : > : >
: > : > : > : > 28. Interpenetrating polymer networks for sequestration of
: bile
: > : acids.
: > : > : > : Mandeville, W. H.,
: > : > : > : > III.;
: > : > : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US
: > : 5,925,379;
: > : > : > : 7/20/99.
: > : > : > : >
: > : > : > : > 29. Amine polymer sequestrant and method of cholesterol
: depletion.
: > : > : > : Mandeville, W. H.,
: > : > : > : > III.;
: > : > : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
: > : > : > : >
: > : > : > : > 30. Process for removing bile salts from a patient and
: > : compositions
: > : > : > : therefor. Mandeville,
: > : > : > : > W. H.,
: > : > : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
: > : > : > : >
: > : > : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
: > : depletion.
: > : > : > : Mandeville, W. H.,
: > : > : > : > III.;
: > : > : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
: > : > : > : >
: > : > : > : > 32. Process for removing bile salts from a patient and
: > : compositions
: > : > : > : therefor. Mandeville,
: > : > : > : > W. H.,
: > : > : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
: > : > : > : >
: > : > : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
: > : > : Mandeville,
: > : > : > : W. H., III.;
: > : > : > : > Holmes-
: > : > : > : > Farley, S. R.; US 5,703,188; 12/30/97.
: > : > : > : >
: > : > : > : > 34. Oral administration of iron-binding crosslinked amine
: > : polymers.
: > : > : > : Mandeville, W. H.,
: > : > : > : > III.;
: > : > : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
: > : > : > : >
: > : > : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
: > : Holmes-Farley,
: > : > : S.
: > : > : > : R.; US 5,693,675;
: > : > : > : > 12/2/97.
: > : > : > : >
: > : > : > : > 36. Method for removing bile salts from a patient with
: alkylated
: > : > : > : crosslinked amine
: > : > : > : > polymers,
: > : > : > : > and preparation of the polymers. Mandeville, W. H., III.;
: > : > : Holmes-Farley,
: > : > : > : S. R.; US
: > : > : > : > 5,679,717; 10/21/97.
: > : > : > : >
: > : > : > : > 37. Phosphate-binding polymers for oral administration.
: > : Holmes-Farley,
: > : > : S.
: > : > : > : R.; Mandeville,
: > : > : > : > W.
: > : > : > : > H., III.; US 5,667,775; 9/16/97.
: > : > : > : >
: > : > : > : > 38. Ion-exchange process using highly crosslinked polymers for
: > : > : removing
: > : > : > : bile salts from a
: > : > : > : > patient, preparation of the polymers, and compositions
: containing
: > : > : them.
: > : > : > : Mandeville, W. H.,
: > : > : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
: > : > : > : >
: > : > : > : > 39. Hydrophobic amine polymer sequestrant and method of
: > : cholesterol
: > : > : > : depletion. Mandeville,
: > : > : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US
: 5,618,530;
: > : > : 4/8/97.
: > : > : > : >
: > : > : > : > 40. Amine polymer sequestrant and method of cholesterol
: depletion.
: > : > : > : Mandeville, W. H.,
: > : > : > : > III.;
: > : > : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
: > : > : > : >
: > : > : > : > 41. Phosphate-binding polymers for oral administration.
: > : Holmes-Farley,
: > : > : S.
: > : > : > : R.; Mandeville,
: > : > : > : > W.
: > : > : > : > H., III.; US 5,496,545; 3/5/96.
: > : > : > : >
: > : > : > : > 42. Iron-binding polymers for oral administration. Mandeville,
: W.
: > : H.,
: > : > : > : III.; Holmes-Farley,
: > : > : > : > S. R.;
: > : > : > : > US 5,487,888; 1/30/96.
: > : > : > : >
: > : > : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having
: > : active
: > : > : > : hydrogens on the
: > : > : > : > surface.
: > : > : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
: > : > : > : >
: > : > : > : > 44. Layered sol-gel coatings from organisilicon compounds.
: > : > : Holmes-Farley,
: > : > : > : S. R.; Yanyo, L.
: > : > : > : > C.;
: > : > : > : > US 5,182,143; 1/26/93.
: > : > : > : >
: > : > : > : > 45. Method for metal bonding using ultrathin primer coating.
: > : > : > : Holmes-Farley, S. R.; Yanyo,
: > : > : > : > L.
: > : > : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
: > : > : > : >
: > : > : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.;
: Abbey, K.
: > : J.;
: > : > : US
: > : > : > : 5,096,962;
: > : > : > : > 3/17/92.
: > : > : > : >
: > : > : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
: > : > : > : elastomer-metal bonding.
: > : > : > : > Holmes-
: > : > : > : > Farley, S. R.; US 5,102,956; 4/7/92.
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT
: ISSUED)
: > : > : > : >
: > : > : > : >
: > : > : > : > 1. Aryl boronate functionalized polymers for treating obesity
: and
: > : > : > : inhibiting fat uptake.
: > : > : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III;
: Dhal,
: > : > : Pradeep
: > : > : > : K.; Huval, Chad
: > : > : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl.
: (2003),
: > : 92
: > : > : pp. WO
: > : > : > : 0302571.
: > : > : > : >
: > : > : > : > 2. Preparation of aryl boronic acids for treating obesity.
: > : > : Holmes-Farley,
: > : > : > : Stephen Randall;
: > : > : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal,
: > : Pradeep
: > : > : K.
: > : > : > : (Geltex
: > : > : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO
: > : 0302570.
: > : > : > : >
: > : > : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide.
: > : Holmes-Farley,
: > : > : > : Stephen Randall.
: > : > : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32
: pp.
: > : WO
: > : > : > : 0302130.
: > : > : > : >
: > : > : > : > 4. Method for reducing copper levels and treating copper
: > : toxicosis.
: > : > : > : Holmes-Farley, Stephen
: > : > : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl.
: > : (2002),
: > : > : 45
: > : > : > : pp. WO
: > : > : > : > 0285383.
: > : > : > : >
: > : > : > : > 5. Method for treating gout and binding uric acid.
: Holmes-Farley,
: > : > : Stephen
: > : > : > : Randall; Burke,
: > : > : > : > Steven K. WO 0285381 10/31/2002.
: > : > : > : >
: > : > : > : > 6. Method for treating gout and reducing serum uric acid.
: > : > : Holmes-Farley,
: > : > : > : Stephen Randall;
: > : > : > : > Burke, Steven K WO 0285380 10/31/2002.
: > : > : > : >
: > : > : > : > 7. Amine condensation polymer bile acid sequestrants. Huval,
: C.
: > : C.;
: > : > : > : Holmes-Farley, S. R.;
: > : > : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
: > : > : > : >
: > : > : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H.,
: III
: > : and
: > : > : > : Holmes-Farley, S.
: > : > : > : > R.;
: > : > : > : > WO 1999-US5662; 9/23/1999.
: > : > : > : >
: > : > : > : > 9. Amine-containing copolymers as bile acid sequestrants.
: > : > : Holmes-Farley,
: > : > : > : S. R.; Petersen,
: > : > : > : > J. S.;
: > : > : > : > WO 9933452; 7/8/1999.
: > : > : > : >
: > : > : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W.
: H.,
: > : III
: > : > : and
: > : > : > : Holmes-Farley, S.
: > : > : > : > R.;
: > : > : > : > WO 9922743; 5/14/1999.
: > : > : > : >
: > : > : > : > 11. Polyallylamine polymers for removing bile salts and
: treating
: > : > : > : hypercholesterolemia, and
: > : > : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H.,
: III;
: > : > : Burke,
: > : > : > : S. K.; Goldberg,
: > : > : > : > D. I.; WO 9857652; 12/23/98.
: > : > : > : >
: > : > : > : > 12. Phosphate-bidning polymers combined with a calcium
: supplement
: > : for
: > : > : oral
: > : > : > : administration.
: > : > : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
: > : Holmes-Farley,
: > : > : S.
: > : > : > : R.; WO 9842355;
: > : > : > : > 10/1/98.
: > : > : > : >
: > : > : > : > 13. Hydrophobic heteroatom-containing sequestrant for
: cholesterol
: > : > : > : depletion. Mandeville,
: > : > : > : > W.
: > : > : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449;
: > : 12/12/96.
: > : > : > : >
: > : > : > : > 14. Process for adjusting ion concentration in a patient and
: > : > : compositions
: > : > : > : therefor.
: > : > : > : > Mandeville,
: > : > : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
: > : > : > : >
: > : > : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
: > : > : interlayer
: > : > : > : for improved
: > : > : > : > metal-
: > : > : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
: > : > : 1/20/94.
: > : > : > : >
: > : > : > : > 16. Process for increased metal-substrate bond strength in
: > : metalized
: > : > : > : plastics.
: > : > : > : > Holmes-Farley, S.
: > : > : > : > R.; Ger. Offen. 4322516; 7/6/93.
: > : > : > : >
: > : > : > : > 17. Electrorheological fluids and preparation of particles
: useful
: > : in
: > : > : the
: > : > : > : fluids.
: > : > : > : > Troughton,
: > : > : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie;
: Carlson,
: > : J.
: > : > : > : David; Bares, Joseph
: > : > : > : > E.;
: > : > : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra
: Nell.
: > : EP
: > : > : > : 394049;
: > : > : > : > 10/24/1990.
: > : > : > : >
: > : > : > : > JOURNAL PUBLICATIONS
: > : > : > : >
: > : > : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William;
: Zhorov,
: > : > : Eugene;
: > : > : > : Guo, Amy;
: > : > : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David
: L.;
: > : > : > : Mandeville, W. Harry;
: > : > : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
: > : > : 611-619.
: > : > : > : >
: > : > : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
: > : > : synthesis
: > : > : > : and biological
: > : > : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley,
: S.
: > : > : Randall;
: > : > : > : Mandeville, W.
: > : > : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal,
: Pradeep
: > : K.
: > : > : > : Journal of
: > : > : > : > Macromolecular Science, Pure and Applied Chemistry (2001),
: > : A38(12),
: > : > : > : 1559-1574.
: > : > : > : >
: > : > : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by
: > : Molecular
: > : > : > : Imprinting. Huval,
: > : > : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.;
: Holmes-Farley,
: > : S.
: > : > : > : Randall; Mandeville,
: > : > : > : > W.
: > : > : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro,
: > : Robert
: > : > : J.;
: > : > : > : Chen, Xi; Dhal,
: > : > : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
: > : > : > : >
: > : > : > : > 4. Synthetic polymers for the binding of fat in the intestinal
: > : tract.
: > : > : > : Jozefiak, Thomas H.;
: > : > : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny,
: Cynthia;
: > : > : Huval,
: > : > : > : Chad C.;
: > : > : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney,
: Cynthia.
: > : > : > : Abstracts of
: > : > : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United
: States,
: > : August
: > : > : > : 26-30, 2001
: > : > : > : > (2001), POLY-047 and Polymer Preprints (American Chemical
: Society,
: > : > : > : Division of
: > : > : > : > Polymer Chemistry) (2001), 42(2), 98.
: > : > : > : >
: > : > : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel
: > : polymer
: > : > : gel
: > : > : > : pharmaceutical.
: > : > : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.;
: Petersen,
: > : J.;
: > : > : Ward,
: > : > : > : J.; Sacchiero,
: > : > : > : > B.;
: > : > : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton,
: K.
: > : A.;
: > : > : Chen,
: > : > : > : X.; Mazzeo, J.
: > : > : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
: > : > : > : >
: > : > : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl
: and
: > : > : other
: > : > : > : bile acid
: > : > : > : > sequestrants.
: > : > : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.;
: Xu,
: > : Q.;
: > : > : > : Hook, P.; Holmes-
: > : > : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1),
: > : 708-709.
: > : > : > : >
: > : > : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
: > : > : Holmes-Farley,
: > : > : > : S. R; Polym.
: > : > : > : > Mater. Sci. Eng (1999), 80, 246-247.
: > : > : > : >
: > : > : > : > 8. Design and characterization of of Sevelamer Hydrochloride:
: a
: > : novel
: > : > : > : phosphate-binding
: > : > : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III;
: > : Ward,
: > : > : J.;
: > : > : > : Miller, K. L.;
: > : > : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M.
: S.-
: > : Pure
: > : > : and
: > : > : > : Appl. Chem.,
: > : > : > : > A36(7&8), p. 1085 (1999).
: > : > : > : >
: > : > : > : > 9. Three generations of bile acid sequestrants. Mandeville, W.
: H.,
: > : > : III;
: > : > : > : Braunlin, W.;
: > : > : > : > Dhal, P.;
: > : > : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik,
: S.;
: > : > : > : Rosenbaum, D.;
: > : > : > : > Sacchiero,
: > : > : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc.
: > : (1999),
: > : > : > : 550, 3-15.
: > : > : > : >
: > : > : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked,
: polymeric
: > : > : phosphate
: > : > : > : binder, on
: > : > : > : > urinary
: > : > : > : > phosphorous excretion in rats. Rosenbaum, D. P.;
: Holmes-Farley, S.
: > : R.;
: > : > : > : Mandeville, W. H.,
: > : > : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
: > : Transplant.
: > : > : > : (1997), 12(5)
: > : > : > : > 961-964.
: > : > : > : >
: > : > : > : > 11. Thin anisotropic coatings based on sol-gel technology.
: > : > : Holmes-Farley,
: > : > : > : S. R.; Yanyo, L.
: > : > : > : > C;
: > : > : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem.
: 4),
: > : > : 439-444.
: > : > : > : >
: > : > : > : > 12. The mechanism of cure initiation of a surface activated
: > : adhesive.
: > : > : > : Holmes-Farley, S.
: > : > : > : > R.;
: > : > : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5),
: 409-420.
: > : > : > : >
: > : > : > : > 13. Adhesion promotion and corrosion prevention using thin
: > : anisotropic
: > : > : > : coatings. Holmes-
: > : > : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991),
: 5(2),
: > : > : > : 131-151.
: > : > : > : >
: > : > : > : > 14. Wetting of functionalized polyethylene having ionizable
: > : organic
: > : > : acids
: > : > : > : and bases at the
: > : > : > : > polymer-water interface: relations between functional group
: > : polarity,
: > : > : > : extent of
: > : > : > : > ionization,
: > : > : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C.
: D.;
: > : > : > : Whitesides, G. M.;
: > : > : > : > Langmuir
: > : > : > : > (1988), 4(4), 921-937.
: > : > : > : >
: > : > : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols
: with
: > : a
: > : > : > : single hydroxy group.
: > : > : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
: > : > : > : >
: > : > : > : > 16. Reconstruction of the interface of oxidatively
: functionalized
: > : > : > : polyethylene (PE-CO2H)
: > : > : > : > and
: > : > : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.;
: > : Nuzzo,
: > : > : R.;
: > : > : > : McCarthy, T. J.;
: > : > : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also
: Report
: > : > : (1987),
: > : > : > : AD-
: > : > : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
: > : > : > : >
: > : > : > : > 17. Surface-modified polyethylene film: the relationship
: between
: > : > : surface
: > : > : > : chemistry and
: > : > : > : > physical
: > : > : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987,
: 47(11),
: > : > : 4537.
: > : > : > : >
: > : > : > : > 18. Reactivity of carboxylic acid and ester groups in the
: > : > : functionalized
: > : > : > : interfacial
: > : > : > : > region of
: > : > : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
: > : > : > : differentiation of the
: > : > : > : > functional groups into shallow and deep subsets based on a
: > : comparison
: > : > : of
: > : > : > : contact angle and
: > : > : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.;
: > : Langmuir
: > : > : > : (1987), 3(1), 62-
: > : > : > : > 76.
: > : > : > : >
: > : > : > : > 19. Fluorescence properties of dansyl groups covalently bonded
: tot
: > : he
: > : > : > : surface of
: > : > : > : > oxidatively
: > : > : > : > functionalized low-density polyethylene film. Holmes-Farley,
: S.
: > : R.;
: > : > : > : Whitesides, G. M.;
: > : > : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985),
: TR-85-2;
: > : > : > : AD-A162435/2/GAR,
: > : > : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
: > : > : > : >
: > : > : > : > 20. Acid-base behavior of carboxylic acid groups covalently
: > : attached
: > : > : at
: > : > : > : the surface of
: > : > : > : > polyethylene: The usefulness of contact angle in following the
: > : > : ionization
: > : > : > : of surface
: > : > : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy,
: T.
: > : J.;
: > : > : > : Deutch, J.;
: > : > : > : > Whitesides,
: > : > : > : > G. M.; Langmuir (1985), 1(6), 725-740.
: > : > : > : >
: > : > : > : > 21. The thermal stability of a surface modified solid organic
: > : polymer.
: > : > : > : Holmes-Farley, S.
: > : > : > : > R.;
: > : > : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53,
: 127-131.
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
: > : > : > : >
: > : > : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R.
: > : Advanced
: > : > : > : Aquarist. June 2003.
: > : > : > : >
: > : > : > : > 2. The Self Purification of Limewater (Kalkwasser).
: Holmes-Farley,
: > : R.
: > : > : > : Advanced Aquarist.
: > : > : > : > May
: > : > : > : > 2003.
: > : > : > : >
: > : > : > : > 3. The Degradation of Limewater (Kalkwasser) in Air.
: > : Holmes-Farley, R.
: > : > : > : Reefkeeping May
: > : > : > : > 2003.
: > : > : > : >
: > : > : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
: > : Reefkeeping
: > : > : > : April 2003.
: > : > : > : >
: > : > : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae
: Growth.
: > : > : > : Holmes-Farley, R.
: > : > : > : > Advanced Aquarist; April 2003.
: > : > : > : >
: > : > : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae
: Growth.
: > : > : > : Holmes-Farley, R.
: > : > : > : > Advanced Aquarist; April 2003.
: > : > : > : >
: > : > : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R.
: Advanced
: > : > : Aquarist;
: > : > : > : March 2003.
: > : > : > : >
: > : > : > : > 8. How to Select a Calcium and Alkalinity Supplementation
: Scheme.
: > : > : > : Holmes-Farley, R.
: > : > : > : > Advanced Aquarist; February 2003.
: > : > : > : >
: > : > : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
: > : January
: > : > : > : 2003.
: > : > : > : >
: > : > : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
: > : > : December
: > : > : > : 2002.
: > : > : > : >
: > : > : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
: > : > : Advanced
: > : > : > : Aquarist; November
: > : > : > : > 2002.
: > : > : > : >
: > : > : > : > 12. Iron: A Look at Organisms Other than Macroalgae.
: > : Holmes-Farley, R.
: > : > : > : Advanced Aquarist;
: > : > : > : > November 2002.
: > : > : > : >
: > : > : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.;
: Advanced
: > : > : Aquarist,
: > : > : > : September 2002.
: > : > : > : >
: > : > : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist,
: > : August
: > : > : > : 2002.
: > : > : > : >
: > : > : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.;
: Reefkeeping.com,
: > : April
: > : > : > : 2002.
: > : > : > : >
: > : > : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R.
: Advanced
: > : > : > : Aquarist; July 2002
: > : > : > : >
: > : > : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced
: Aquarist;
: > : > : June
: > : > : > : 2002.
: > : > : > : >
: > : > : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley,
: R.
: > : > : Advanced
: > : > : > : Aquarist, May
: > : > : > : > 2002.
: > : > : > : >
: > : > : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in
: > : Corals.
: > : > : > : Holmes-Farley, R.
: > : > : > : > Advanced Aquarist, April 2002.
: > : > : > : >
: > : > : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
: > : > : > : >
: > : > : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February
: > : 2002.
: > : > : > : >
: > : > : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist,
: January
: > : > : 2002.
: > : > : > : >
: > : > : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium
: > : Frontiers
: > : > : > : 2000.
: > : > : > : >
: > : > : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R.
: Aquarium
: > : > : > : Frontiers 2000.
: > : > : > : >
: > : > : > : > 25. Phosphate..What is it and why should you care.
: Holmes-Farley,
: > : R.
: > : > : > : Aquarium Frontiers
: > : > : > : > 2000.
: > : > : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
: > : > : Frontiers
: > : > : > : 2000.
: > : > : > : >
: > : > : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium
: Frontiers
: > : > : 2000.
: > : > : > : >
: > : > : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium
: Frontiers
: > : 1999.
: > : > : > : >
: > : > : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > Boomer
: > : > : > : >
: > : > : > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > : > : > http://www.reefcentral.com/vbulletin/index.php
: > : > : > : >
: > : > : > : > Want to See More ?
: > : > : > : > Please Join Our Growing Membership
: > : > : > : > www.coralrealm.com
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > :
: > : > : > :
: > : > : >
: > : > : >
: > : > :
: > : > :
: > : > :
: > : >
: > : >
: > :
: > :
: >
: >
:
:

[Boomer]

Yes, I agree but you don't have to lower the pH to remove CO2 but there is more CO2 at
lower pH so it would be easier to degas when there is more. But a higher Alk is almost
always accompanied by a higher CO2 at the same pH. If it wasn't the pH would shift.

"Alkalinity was an indication of buffering capacity until this post."

I'm not saying I use those exact words. I said if you know the BC you can calculate the
Alk.. correct., which is about the same thing,as thaw would be an indication.

One more thing that I just found on BC

Bc = d SigmaCO2/dpH

I'll have to look further but must get the hell out of here. Sigma CO2 = CO2, H2CO3, HCO3
and CO3. CO2 is not part of the Alk equation, so I'm wondering, if one throws in CO2 then
it tells us about what CO2, and Alk will do to the pH. Alk says nothing of what CO2 does
to pH, as CO2 has 0 effect on Alk., where it appears CO2 has an effect on Bc

I have so for PM 'ed Randy and asked him to review Pankow and Millero's texts for an
answer on Bc vs Alk. So did you e-mail Millero ?

So if you want to continue on about who said what where, then when are you going to
comment on the Acidity measurement post and that it is the opposite of Alk but I'm an
idiot for saying such a thing. You seem to think you have this Bc thing all sewed up, so
Staut is going for it. Where are your answers on the posts on Acidity measurement. I think
this is about the fourth time I have asked you to answer it. You have still failed. Is it
because it is real and you said it not, thus making me correct and your wrong. I don't
care what the outcome is here, who is right or who wrong, so what is your beef on it or
e-mailing Millero. I want real answers don't you. If you won't email Millero, then I will
and post both his and Randy's answer here next week


--
Boomer

Want to talk chemistry ? The Reef Chemistry Forum
http://www.reefcentral.com/vbulletin/index.php

Want to See More ?
Please Join Our Growing Membership
www.coralrealm.com

If You See Me Running You Better Catch-Up
"stoutman" <.@.> wrote in message news:_X9Xb.304005$xy6.1488576@attbi_s02...
: one more thing,
:
: Let me comment on the CO2 equilibrium.
:
: CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
: HCO3-1 <-------> CO3-2
:
:
: I said, and still say, that if you lower the pH the equilibrium will shift
: to the left making it EASIER to purge CO2.
:
: Yes, as the CO2(g) leaves the system the equilibrium will shift to the right
: and pH goes up and CO2 leaves less readily. If you lower the pH again it
: will shift to the left again, and CO2 will purge more readily. Then as CO2
: leaves the system, the pH will go up and equilibrium starts to shift to the
: right. If you lower the pH again the equilibrium will shift to the left,
: and CO2 will purge more readily. Then as CO2 leaves the system, the pH will
: go up and the equilibrium ...
:
: This is the point to this story:
:
: At low pH's (acidic) the equilibrium is left shifted. CO2 leaves MORE
: readily
: At high pH's (basic) the equilibrium is right shifted. CO2 leaves LESS
: readily.
:
: -Stoutman
:
:
:
:
:
:
:
: "Boomer" > wrote in message
: ...
: > Yes, of cause I remember, as I said I posted it for a reason. I see you
: have used only
: > that link for your definition, as it makes you look right.You have avoided
: all Alk
: > definitions in a chemistry book, to include your own definition *****to
: resist a drop in
: > pH due to the addition of acid***, which is the same as the others I
: posted .Agreed, of
: > course not.You know that Alk isn't defined as "by the addition of acids or
: bases "and is
: > only the " addition of an acid", so why are you accepting the definition
: ?.You know that
: > when you titrate it is an acid added and never a base. In one breath it
: says Alk is "Acid
: > neutralizing " and then they say "by the addition of acids or bases ".You
: can't have it
: > both ways and YOU know that Agreed . If the word "base" was left out I
: would not have much
: > to say. Agreed
: >
: >
: > "Alkalinity is a
: > measurement of BUFFERING CAPACITY."
: >
: > No it is not a measurement of BUFFERING CAPACITY, it is a indication of
: BC. I have said
: > this at least twice. If you know your BC you can calculate Alk and if you
: can do one you
: > can do the other agreed. What I have tried to convey from the beginning is
: that Alk and BC
: > are not the same thing. You in one of your other posts have said they are
: not the same
: > thing and never said they were. Now you seem to be saying they are the
: same thing
: >
: > "So, when we measure ALKALINITY (and we know the pH) we are in effect
: > measuring BUFFERING CAPACITY.
: >
: > More or less YES in an "effect" but Alk tells you not much of anything
: when a base is
: > added Agreed. That is called Acidity, which I see you have avoided again
: as if there is
: > no such thing. I also said that for us the only thing we need to be
: concerned about is
: > Alk, so BC would fit in, as we could care less about the ability to
: neutralize a base or
: > measure Acidity. So, if you knew your pH , Alk or Acy you would really
: know what you BC is
: > doing for you Agreed.
: >
: > On Bc, we have both left something from my first equation, so I thought I
: would post it
: > again for you, as I like being honest .I'm surprised you didn't catch it
: :-)
: >
: > B = dCb / dpH = - dCa / dpH
: >
: > So;
: >
: > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
: [H3O+] / (Ka =
: > H3O+])² )
: >
: > or
: >
: > B (Buffering Capacity) = - dCa / dpH = 2.303 ( Kw/[H30+] + [H30+] + CKa
: [H3O+] / (Ka =
: > H3O+])² )
: >
: > There are number of was to mathematically express BC. Two of the most
: common are the
: > change in Alk with the pH at constant total carbonate, the other is change
: in Alk with pH
: > constant CO2 pp. In some examples of Bc, Bc is the inverse slope of the
: Alk titration
: > curve ( I'm sure yo
: > u will love this) In the other over the pH range, while BC is going
: through minimum, Bpp
: > increases linearly. This difference is caused by the uptake of CO2 by the
: solution, which
: > increases Ct as pH increases.To bad we can't or my server won't allow me,
: to post
: > attachments. I have a nice BC cure of various species as a function of
: pC/pH diagrams, set
: > to a pKa. curve
: >
: >
: > On another issue
: >
: > "In order to remove CO2 (g) you ideally would want to shift
: > the equilibrium to the left by LOWERING the pH"
: >
: >
: > You may want to try and re-explain this
: >
: > CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
: > HCO3-1 <-------> CO3-2
: >
: >
: > As the reaction shifts to left the pH gets higher as CO2 leaves the
: system.You don't have
: > to lower the pH to remove CO2. Case in point plants. As they remove CO2
: the pH rises,
: > continued removal of the Sigma CO2 ( CO2, H2CO3, HCO3,CO3) cause further
: rising until
: > there is mostly only carbonate (CO3) left and a high pH. Another case, at
: a pH of 8.00 and
: > Alk of 4 meq / l ( 1.4 mg / l CO2) you have much more CO2 than at 2 meq/
: l (0.65mg / l).
: > . Aeration of the water can drive off the CO, no lowering of the pH
: required., the removal
: > will cause the pH to rise .On the other hand, trying to remove CO2 @ 2 meq
: / l won't get
: > you much of anywhere in this case. Also, even a low pH doesn't mean you
: can drive of CO2.
: > If the seawater pH was say 7.5, you would think not problem to drive off
: CO2. If the Alk
: > was 0.25 there would be about .35 mg / l CO2 to blow off. At the alk of
: 4.00 meq / l the
: > CO2 is 5 mg / l.Usually, when people have a lower pH, say 7.9 or so, it is
: do to CO2, so
: > the pH has lowered, increasing the CO2, to allow one to blow it off easier
: and bring the
: > pH back up.
: >
: > CO2 = [CA(Carbonate Alk) x aH ] / [pK1(1 + 2pK2 /aH)]
: >
: > I think we just got off on the wrong foot, hope things look better.
: >
: > I'll be gone for the weekend, leaving in an hour, so have a nice weekend
: :-)
: >
: >
: >
: >
: > --
: > Boomer
: >
: > Want to talk chemistry ? The Reef Chemistry Forum
: > http://www.reefcentral.com/vbulletin/index.php
: >
: > Want to See More ?
: > Please Join Our Growing Membership
: > www.coralrealm.com
: >
: > If You See Me Running You Better Catch-Up
: > "stoutman" <.@.> wrote in message news:lcRWb.299984$na.451117@attbi_s04...
: > : > Humm, since when does Alk have anything to do in regards to the
: addition
: > : of BASE.
: > :
: > : You tell me. Your the one that posted a link to a web page that had
: this
: > : definition of alkalinity. Looks like you put yourself in your own hole
: pal.
: > :
: > : Remember posting this link:
: > :
: > : http://www.waterontheweb.org/resources/glossary.html
: > :
: > : Here is the definition of alkalinity from the web page YOU cited. (I
: > : recommend you read the web pages you are citing before you cite them)
: > : Alkalinity:
: > : Acid neutralizing or buffering capacity of water; a measure of the
: ability
: > : of water to resist changes in pH caused by the addition of acids or
: BASES.
: > :
: > :
: > : > It sure is funny how all of the chemist that write water chemistry
: > : textbooks never say Alk
: > : > is the Buffering Capacity of a solution.
: > :
: > : Neither did I. I said (for the umpth teen time) Alkalinity is a
: > : measurement of BUFFERING CAPACITY.
: > :
: > : When you measure alkalinity you know your BUFFERING CAPACITY (if you
: know
: > : your pH). Its a two for one.
: > :
: > : SEE MY OTHER POST FROM TODAY.
: > :
: > :
: > :
: > : "Boomer" > wrote in message
: > : ...
: > : >
: > : > "I am not sure if you are just messing with me "
: > : >
: > : > Yes, messing with you, it is called trolling a troll, to see where the
: > : hell you would go
: > : > and what you would say in regards to last posts. It is called honesty,
: of
: > : which you have
: > : > none off to say the least,that I can see.You always like to post what
: > : suits you and just
: > : > avoid ref I give. So lets start where you are WRONG and have a great
: lack
: > : of understanding
: > : > of things, to include pointing out all your gross error which you
: still
: > : FAIL to
: > : > acknowledge and which can be prove in many water chem. ref. .I doubt
: like
: > : hell you are a
: > : > chemist at all.You seem to want to con people into thinkin' you are.
: But
: > : then again, I
: > : > have seen chemists like you before, they are not familiar with the,
: but
: > : they ASK to have
: > : > it explained and ask for REF.YOU just shoot from the hip. WHAT GETS
: YOU IN
: > : TROUBLE. You
: > : > remind me of snoot-noise kid that come here and other NG's and
: > : forums...that think they
: > : > know, buy hey, maybe I'm wrong :-)
: > : >
: > : >
: > : >
: > : > 1). Acidity
: > : >
: > : > "***Benjamin,Water Chemistry (2002, pages 262-263).***
: > : >
: > : > ***Acidity A concept that is exactly analogous to alkalinity but
: measures
: > : the base
: > : > neutralizing
: > : > capacity (BNC) of a solution is Acidity. The quantitative represents
: the
: > : concentration of
: > : > OH- ions that must be added to titrate the solution to a pH near
: 10.5***
: > : >
: > : > So that means that not only in Benjamin wrong but, so are Stumm &
: Morgan,
: > : Millero, Pilosn,
: > : > Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few. As I
: > : said, you have your
: > : > acidity and Acidy mixed up. Acidity as defined above is covered in
: most
: > : water chemistry
: > : > books, written by chemists, who's field of expertise is water
: chemistry.
: > : You can even buy
: > : > Acidity test kits from, HACH, LaMotte, etc..
: > : >
: > : > You mean you didn't read this or are you just avoiding it .The same
: > : definition can be
: > : > found in almost any std water chemistry book.
: > : >
: > : > I have run into few chemists, that are NOT familiar with the above.
: Some
: > : water reports
: > : > require the above Acidity measuring. The issue with you is you do not
: > : understand WATER
: > : > CHEMISTRY. Everything you have posted can be found a general chemistry
: > : book
: > : >
: > : >
: > : >
: > : >
: > : > 2) Alk and BC
: > : >
: > : > From the link
: > : >
: > : > Alkalinity
: > : > ***Acid neutralizing or buffering capacity of water; a measure of the
: > : ability of water to
: > : > resist changes in pH caused by the addition of acids or bases ***
: > : >
: > : > This is a Buffering Capacity definition not Alk
: > : >
: > : > Humm, since when does Alk have anything to do in regards to the
: addition
: > : of BASE. As I
: > : > pointed out in the first post the term is often miss used. Even in
: YOUR
: > : own posts you say
: > : > it is based on a acid addition, no mention of **base or acid**
: addition
: > : by you. Are you
: > : > getting confused or what. Or is more you are trying to confuse
: everyone
: > : you are right. The
: > : > above is a definition for Buffer Capacity NOT Alk
: > : >
: > : > From Drew, Geochemistry of Natural Waters
: > : >
: > : > "alkalinity, which is formally defined as the equivalent sum of bases
: that
: > : are titratable
: > : > with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the pH
: of
: > : the solution is
: > : > progressively lowered by the addition of a strong acid (HCL), all the
: > : anions on the right
: > : > will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4,
: H2S,organic
: > : acids, H20)"
: > : >
: > : > This follows almost all description of Alk, that it is acid
: neutralizing
: > : reaction and has
: > : > nothing to do with base neutralizing, which is Acidity (BNC) .I
: defined
: > : these before you
: > : > had no comment
: > : >
: > : >
: > : > Even the links that give the Buffering Capacity definition is wrong,
: as is
: > : the UIPAC on
: > : > Alkalinity. Alkalinity has nothing to do with the addition of bases
: only
: > : acids. When you
: > : > use the words "base and acid" it becomes BC
: > : >
: > : > Even YOU MUST disagree with these definitions, from YOUR own post
: > : >
: > : > Think of alkalinity as 'buffering capacity'. Or the ability of a
: solution
: > : > ***to resist a drop in pH due to the addition of acid***
: > : >
: > : > Where the flip is the base addition forget it ?
: > : >
: > : > From Butler; Carbon Dioxide Equilibrium and Their Applications
: (professor
: > : emeritus
: > : > Harvard University) an expert on the subject.
: > : >
: > : > Buffering Index (Buffering Capacity, Buffer Intensity).
: > : >
: > : > ***This concept was first developed for mixtures of approximately
: equal
: > : proportions of
: > : > conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3. Such
: > : buffer solutions
: > : > strongly resist changes in pH when acids or bases are added and are
: useful
: > : as pH
: > : > standards. The Buffer Index tells how great the resistance to pH
: changes
: > : will be.**
: > : >
: > : > also from Butler
: > : >
: > : > Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
: > : >
: > : > Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
: > : >
: > : > Acidity is in fact just the negative of Alkalinity ***
: > : >
: > : > http://www.lagoonsonline.com/acid.htm
: > : >
: > : >
: > :
: http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.h
: > : tm?E+mystore
: > : >
: > : > It sure is funny how all of the chemist that write water chemistry
: > : textbooks never say Alk
: > : > is the Buffering Capacity of a solution. They are always treated and
: > : defined separately.
: > : >
: > : > If you or others choose to treat Alk and BC as the same, well, just
: have
: > : at it. As I said
: > : > in first post I know what you mean.
: > : >
: > : > "No need to cite web pages that describe what I know and what I wrote
: > : > in this discussion"
: > : >
: > : > No you don't know, who are you trying to convince any way, me, the
: guys
: > : here and/or all
: > : > the water chemists in this world. As I said before go get a dam WATER
: > : CHEMISTRY book or
: > : > shut the hell up.You keep trying to define things from a general
: chemistry
: > : book WE ARE IN
: > : > THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
: > : >
: > : >
: > : >
: > : >
: > : >
: > : > 3). pKa's and what you don't know or seem to be confused on
: > : >
: > : > "Therefore, it has two pKa's
: > : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35.
: > : The
: > : > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I calculated
: is
: > : > right in there. Is that magic? :)"
: > : >
: > : > Here it is agin that is twice at least
: > : >
: > : > "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for this
: > : example)
: > : > you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The equilibrium
: will
: > : > be shifted to HCO3-2 by a ratio of 1:100.
: > : >
: > : > Oh wait , there is a third time LOL
: > : >
: > : > "At the pH of seawater, the buffering capacity of carbonate is at it's
: > : > weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
: > : >
: > : >
: > : > Lets just dunk you on this one. I am taking note you refuse to reply
: to
: > : YOUR errors
: > : >
: > : > So you calculated the pH of seawater with freshwater pKa's, now that
: is a
: > : good trick. From
: > : > a number of seawater chemistry books the seawater pKa's are 6 & 9.1,
: so
: > : according to you,
: > : > seemingly not understanding your favorite Henderson-Hasselbach
: equation;
: > : >
: > : > 2 pH = (6 + 9.1) /2 pH = 7.55
: > : >
: > : > I have never seen seawater with a pH of 7.55. There is no ocean with
: that
: > : pH. Humm how
: > : > come your equation is not working for you today.?
: > : >
: > : >
: > : > "That pH I calculated is
: > : > right in there. Is that magic? :)"
: > : >
: > : > I roll on the floor when I see this = 8.35
: > : >
: > : > Hum , just a brain far so excuse me for thinkin
: > : >
: > : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH = 8.35
: > : >
: > : > Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at a
: pH of
: > : 8.35 there pal
: > : > ? That 8.35 is what you are telling people the pH should be, but their
: > : meter says 6.4.
: > : > This how people will READ this.
: > : >
: > : >
: > : >
: > : >
: > : > 4.) More on Buffering Capacity
: > : >
: > : > "Do you recognize [HCO3-1] and [CO3-2] from another equation ? Yes,
: your
: > : > alkalinity equation."'
: > : >
: > : >
: > : > Yup, I see that and in this case the HCO3 is the acid and the CO3 is
: the
: > : base CORRECT. In
: > : > Alk you are only dealing with bases and how they react to an acid.
: Acidity
: > : deals acids and
: > : > how they recact to bases "Acidity, A concept that is exactly analogous
: to
: > : alkalinity but
: > : > measures the base neutralizing
: > : > capacity (BNC) of a solution is Acidity "Alk is the ANC Acid
: neutralizing
: > : capacity
: > : >
: > : > "Don't the components of a buffer account for the buffering capacity?
: "
: > : >
: > : > Yes, they do but so do the acids which work as buffers. NaHCO3 is a
: buffer
: > : and can act as
: > : > an acid or base
: > : >
: > : > *** Buffering Capacity.**
: > : > The power of a substance in solution to absorb acid or alkali without
: > : change in pH; this
: > : > is highest at a pH value equal to the pKa value of the acid of the
: buffer
: > : pair.***
: > : >
: > : > ***Akalinity***
: > : > Measure of the power of a solution to neutralise hydrogen ions (H+),
: > : usually expressed as
: > : > the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
: > : >
: > : >
: > : > If one wants to call Alk Buffering capacity then one sure as a hell
: can
: > : call Acidty
: > : > Buffering Capacity also. As it is the ability to neutralizes an acid
: that
: > : is a buffer.You
: > : > have a pH of 7 and you add a buffer to lower it to a pH of 4, you are
: > : buffering the water,
: > : > that buffer is a acid.
: > : >
: > : > 5) CO2
: > : >
: > : > You are really confuse so it seems :-) You realllllllly indicate that
: CO2
: > : is affected by
: > : > the Alk or vise-versa
: > : >
: > : > "Yes, the pH will drop with the addition of CO2. Remove CO2 will
: cause
: > : the
: > : > pH to rise? How do you remove CO2? Once it is in solution it forms
: > : > carbonic acid and neutralizes some of your 'buffer'."
: > : >
: > : > "With the exception of CO2?"
: > : >
: > : > No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic Chemistry
: > : > Concepts)....PERIOD.You seem to think a that at least in two of your
: post
: > : that CO2 is
: > : > affected by the Alk or vise-versa. Please go back to school or seek
: > : professor
: > : >
: > : > "Why in one case does CO2 from air lower pH and in the other case it
: > : raises
: > : > it? Doesn't make sense."
: > : >
: > : > That is because you don't understand CO2 period. By the way I saved
: this,
: > : wanted to see
: > : > if you would bite on the post I gave. Not bite at first, so time to
: reel
: > : you in, as you
: > : > did bite in another post..
: > : >
: > : > Lets make some sense of it for you, being that you have a pH.D in
: > : chemistry, so you say .
: > : >
: > : > CO2 is naturally generated in a aquatic systems, it is capable of
: raise to
: > : various levels
: > : > depending on a number of circumstances .It can be measure (except in
: > : seawater) or
: > : > calculated using Buch/Park Equations (what we use for seawater. In
: sort if
: > : you know the pH
: > : > and Alk you can calculate the CO2). If you aerate a system or a sample
: of
: > : water, even if
: > : > the pH has only dropped a couple of tenths, due to an increase in CO2,
: the
: > : CO2 will leave
: > : > solution to the atmosphere.This will raise the pH. On the other hand
: if
: > : theCO2 level is
: > : > more of the norm and you have hikgh room air, such as in the winter,
: the
: > : partial pressure
: > : > of the CO2 in air will be much higher than that in water, in which
: case
: > : the CO2 will enter
: > : > the water and lower the pH. That is without an airstone. Adding an
: > : airstone will make it
: > : > even worse,as you are now forcefully driving the CO2 into solution
: even
: > : quicker. These
: > : > test /experiments have been proven many times, it is not that may work
: > : could work they do
: > : > work.Yet you want to disagree and in another post say you haven't
: tried
: > : it,.Seems to me
: > : > that based on what you say it can't work So, in short you don't know
: what
: > : the hell you are
: > : > taking about. Go get a glass of seawater with a pH of about 8.3 and
: lower
: > : it to about
: > : > 8.0.-81 with CO2, then aerated it and watch the pH go the HELL-BACK-
: UP
: > : ( that is if you
: > : > don't have a high room air CO2 problem.). This little test has been
: done
: > : thousands of
: > : > times in this hobby, with test kits, pH meters and even graphic
: printers.
: > : >
: > : > "This is where Boomer and I
: > : > disagree. I say you would have to lower the pH very low in order to
: > : > effectively remove CO2 by purging."
: > : >
: > : > You are 100 % wrong. Please come to our Chem forum and try and run
: that by
: > : Randy, don't
: > : > take my word on it. I already know what he will say.
: > : >
: > : > "Boomer didnt convince me it
: > : > works at the pH of an aquarium, but I never tried it and I'm not sure
: of
: > : > this. "
: > : >
: > : > Well then come too our chem. forum and tell Randy he doesn't know what
: he
: > : is talking about
: > : > LOL. It is a realllllllllly easy test, having a Ph.D in chemistry, it
: > : should be easy for
: > : > you to run the experiment LOL There are grade school kids that run the
: > : test and know what
: > : > happens and that I'm correct.
: > : >
: > : >
: > : > "The equilibrium is a FUNCTION
: > : > of pH."
: > : >
: > : > It is also a function of Alk or don't you know that. At a pH of 8.3,
: Alk
: > : 2.25, the CO2 is
: > : > about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the Alk
: to
: > : about .4 meq/ l
: > : > or so the CO2 will be around .99 mg / l CO2, When dealing with
: tanksCO2 is
: > : not always in
: > : > equilibrium with ambient air.
: > : >
: > : >
: > : > ". But I wouldn't degas a solution of a
: > : > specific gas (CO2) with a gas (this case he was using air) that
: contains
: > : the
: > : > same gas I am trying to purge."
: > : >
: > : > Why not ? We have a guy right now that is running tests on purging
: ambient
: > : air with a
: > : > solution to remove CO2 gas from the air, before it enters the tank
: > : per/Randy's suggestion.
: > : > The same guy is doing some of my test using a Clinoptilolite, a
: Zeolite
: > : mineral, that has
: > : > an affinity for CO2.This will be a dry CO2 scrubber
: > : >
: > : >
: > : > Sorry Soutman but you sure as hell don't seem to know much about
: aquatic
: > : chemistry. You
: > : > seem to be guessing at everything.
: > : >
: > : > By the way have you read any of Randy's technical articles on water
: > : chemistry, been saving
: > : > these for last. There are a few on pH, Alk, CO2 .Here is a list
: > : >
: > : > Try and answer them 1-5 and lets see where we get THIS TIME :-) or
: maybe
: > : we should just
: > : > drop it. I could care less at this point.
: > : >
: > : > THE END
: > : >
: > : >
: > : > ARTICLES
: > : >
: > : > The first two posts in this thread are lists of some of my articles
: that
: > : relate to reef
: > : > tank chemistry. In the next few posts are some of the articles
: published
: > : by Craig Bingman
: > : > and others on reef chemistry issues.
: > : >
: > : > The first two posts in this thread are lists of some of my articles
: that
: > : relate to reef
: > : > tank chemistry. In the next few posts are some of the articles
: published
: > : by Craig Bingman
: > : > and others on reef chemistry issues.
: > : >
: > : > Solving Common Problems
: > : >
: > : > Solving Calcium and Alkalinity Problems
: > : > http://www.advancedaquarist.com/issues/nov2002/chem.htm
: > : >
: > : > Solutions to pH Problems
: > : > http://www.advancedaquarist.com/iss...ne2002/chem.htm
: > : >
: > : > How to Select a Calcium and Alkalinity Supplementation Scheme
: > : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
: > : >
: > : > Phosphate Issues
: > : > http://www.advancedaquarist.com/iss...pt2002/chem.htm
: > : >
: > : > Nitrate Issues
: > : > http://www.advancedaquarist.com/iss...st2003/chem.htm
: > : >
: > : >
: > : >
: > : > Calcium and Alkalinity
: > : >
: > : > Solving Calcium and Alkalinity Problems
: > : > http://www.advancedaquarist.com/issues/nov2002/chem.htm
: > : >
: > : > How to Select a Calcium and Alkalinity Supplementation Scheme
: > : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
: > : >
: > : > Calcium and Alkalinity Balance Issues
: > : > http://reefkeeping.com/issues/2002-...ature/index.htm
: > : >
: > : > Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
: > : > http://www.advancedaquarist.com/iss...ly2002/chem.htm
: > : >
: > : > The Relationship Between Alkalinity and pH.
: > : > http://www.advancedaquarist.com/issues/may2002/chem.htm
: > : >
: > : > The Chemical & Biochemical Mechanisms of Calcification in Corals
: > : > http://www.advancedaquarist.com/issues/apr2002/chem.htm
: > : >
: > : > Calcium
: > : > http://www.advancedaquarist.com/issues/mar2002/chem.htm
: > : >
: > : > Alkalinity
: > : > http://www.advancedaquarist.com/iss...2/chemistry.htm
: > : >
: > : >
: > : > Iron
: > : >
: > : > First Iron Article: Macroalgae and Dosing Recommendations
: > : > http://www.advancedaquarist.com/issues/aug2002/chem.htm
: > : >
: > : > Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
: > : > http://www.advancedaquarist.com/issues/oct2002/chem.htm
: > : >
: > : > Iodine
: > : >
: > : > Iodine in Marine Aquaria: Part I
: > : > http://www.advancedaquarist.com/issues/mar2003/chem.htm
: > : >
: > : > Iodine in Reef Tanks 2: Effects on Macroalgae Growth
: > : > http://www.advancedaquarist.com/iss...il2003/chem.htm
: > : >
: > : >
: > : > Magnesium and Strontium
: > : >
: > : > Strontium
: > : > http://www.advancedaquarist.com/issues/nov2003/chem.htm
: > : >
: > : > Magnesium
: > : > http://www.advancedaquarist.com/issues/oct2003/chem.htm
: > : >
: > : > Magnesium and Strontium in Limewater
: > : > http://www.advancedaquarist.com/issues/dec2003/chem.htm
: > : >
: > : >
: > : > Limewater (kalkwasser)
: > : >
: > : > The Self Purification of Limewater (Kalkwasser)
: > : > http://www.advancedaquarist.com/issues/may2003/chem.htm
: > : >
: > : > The Degradation of Limewater (Kalkwasser) in Air
: > : > http://reefkeeping.com/issues/2003-...ature/index.htm
: > : >
: > : > How to Select a Calcium and Alkalinity Supplementation Scheme
: > : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
: > : >
: > : > Metals in Aquaria
: > : >
: > : > Aluminum and aluminum-based phosphate binders
: > : > http://www.advancedaquarist.com/iss...ly2003/chem.htm
: > : >
: > : > Reef Aquaria with Low Soluble Metals
: > : > http://reefkeeping.com/issues/2003-...ature/index.htm
: > : >
: > : > Tap Water in Reef Aquaria
: > : > http://www.advancedaquarist.com/issues/jan2004/chem.htm
: > : > First Iron Article: Macroalgae and Dosing Recommendations
: > : > http://www.advancedaquarist.com/issues/aug2002/chem.htm
: > : >
: > : > Second Iron Article: Iron: A Look at Organisms Other than Macroalgae
: > : > http://www.advancedaquarist.com/issues/oct2002/chem.htm
: > : >
: > : >
: > : > Test Kit Reviews
: > : >
: > : > The Seachem Borate Alkalinity Test Kit
: > : > http://www.advancedaquarist.com/iss...ne2003/chem.htm
: > : >
: > : > The Salifert Boron Test Kit
: > : > http://www.advancedaquarist.com/iss...pt2003/chem.htm
: > : >
: > : > Boron and Borate (and pH buffering)
: > : >
: > : > Boron in a Reef Tank (and its effect on pH buffering)
: > : > http://www.advancedaquarist.com/issues/dec2002/chem.htm
: > : >
: > : > The Seachem Borate Alkalinity Test Kit
: > : > http://www.advancedaquarist.com/iss...ne2003/chem.htm
: > : >
: > : > The Salifert Boron Test Kit
: > : > http://www.advancedaquarist.com/iss...pt2003/chem.htm
: > : >
: > : >
: > : >
: > : > Others
: > : >
: > : > Tap Water in Reef Aquaria
: > : > http://www.advancedaquarist.com/issues/jan2004/chem.htm
: > : >
: > : > ORP
: > : > http://reefkeeping.com/issues/2003-...ature/index.htm
: > : >
: > : > Chloramine
: > : > http://reefkeeping.com/issues/2003-...ature/index.htm
: > : >
: > : > Silica in a Reef Tank
: > : > http://advancedaquarist.com/issues/jan2003/feature.htm
: > : >
: > : > Specific Gravity (and temperature correction of hydrometers)
: > : > http://www.advancedaquarist.com/iss...2/chemistry.htm
: > : >
: > : >
: > : > The Complete Nitrogen Cycle
: > : > http://www.animalnetwork.com/fish/l...a&RecordNo=3090
: > : >
: > : > Magnesium (older article with fonts screwed up)
: > : > http://www.aquariumfish.com/aquariu...cid=124&search=
: > : >
: > : > Phosphate (older article now reproduced in a poor fashion)
: > : > http://www.aquariumfish.com/aquariu...cid=124&search=
: > : >
: > : > Carbon Dioxide
: > : > http://www.animalnetwork.com/fish/l...a&RecordNo=2074
: > : >
: > : > Using Conductivity to Measure Salinity
: > : > http://www.aquariumfish.com/aquariu...cid=124&search=
: > : >
: > : > Understanding Seawater
: > : > http://www.animalnetwork.com/fish2/...s/1/default.asp
: > : >
: > : > Protein Skimming: How It Works
: > : > http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
: > : >
: > : >
: > : >
: > : > Articles by Craig Bingman:
: > : >
: > : > Carbon Dioxide tests
: > : > http://www.animalnetwork.com/fish/l...n=&RecordNo=279
: > : >
: > : > Limewater, Acetic Acid and Sand Clumping
: > : > http://www.animalnetwork.com/fish/l...n=&RecordNo=181
: > : >
: > : > Calcium and Alkalinity
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Calculation of Calcium Carbonate Saturation States in Reef Aquaria
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : >
: > : > Calcification Rates in Several Tropical Coral Reef Aquaria
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Limits To Limewater...Revisited
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Expanding the Limits of Limewater: Adding Organic Carbon Sources
: (vinegar)
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : >
: > : > Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Magnesium - Part I
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Magnesium - Part II
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > A Homemade Magnesium Supplement
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Simulating the Effect of Calcium Chloride and Sodium Bicarbonate
: Additions
: > : on Reef Systems
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Additional Simulations: The Combined Effect Of Calcium Chloride
: > : > /Sodium Bicarbonate Additions And Water Exchanges
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : >
: > : > More articles by Craig Bingman:
: > : >
: > : > The Halogens - Part I: Bromine in Seawater and Aquaria
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > The Halogens - Part II: Fluoride
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Fluoride Depletion In Four Reef Aquariums
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > The Halogens - Part III: Iodine
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Measuring Halides
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > How Test Kits Work
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Borax pH Calibration
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > A pH Detective Story
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > How to Mix a Batch of Synthetic Seawater in Under Five Minutes
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral Reefs
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : > SILICON - FOE OR FRIEND?
: > : > http://www.animalnetwork.com/fish2/...s/1/default.asp
: > : >
: > : > The Composition Of Several Synthetic Seawater Mixes
: > : > http://www.animalnetwork.com/fish2/...s/1/default.asp
: > : >
: > : > Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
: > : > http://www.animalnetwork.com/fish2/...bio/default.asp
: > : >
: > : >
: > : >
: > : > Andy's calcium calculator
: > : > http://www.andy-hipkiss.co.uk/cacalc.htm
: > : >
: > : > Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
: > : > http://www.aquariumfish.com/aquariu...cid=124&search=
: > : >
: > : > Calcium Reactor Substrate -- Phosphate Levels
: > : > by Greg Hiller
: > : > http://www.advancedaquarist.com/iss...l2003/short.htm
: > : >
: > : >
: > : > Indoor CO2 Problems
: > : > http://www.advancedaquarist.com/iss...r2002/short.htm
: > : >
: > : > Simon Huntington's CaCO3/CO2 reactor article
: > : >
: > : > http://reefkeeping.com/issues/2002-...ature/index.htm
: > : >
: > : > Ron Shimek's Tank Water Analysis Article
: > : > http://reefkeeping.com/issues/2002-...ature/index.htm
: > : >
: > : >
: > : >
: > : >
: > : > Home made salinity standards thread:
: > : >
: > : > http://reefcentral.com/forums/showt...?threadid=65509
: > : >
: > : > Reef Chemicals Calculator
: > : > http://www.kademani.com/reefchem.htm
: > : >
: > : >
: > : >
: > : > Boomer
: > : >
: > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > http://www.reefcentral.com/vbulletin/index.php
: > : >
: > : >
: > : > Former US Army Bomb Technician (EOD)
: > : > Member; IABTI, NATEODA, WEODF, ISEE & IPS
: > : >
: > : > If You See Me Running You Better Catch-Up
: > : >
: > : >
: > : > --
: > : > Boomer
: > : >
: > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > http://www.reefcentral.com/vbulletin/index.php
: > : >
: > : > Want to See More ?
: > : > Please Join Our Growing Membership
: > : > www.coralrealm.com
: > : >
: > : > If You See Me Running You Better Catch-Up
: > : > "stoutman" <.@.> wrote in message
: > : news:aGuWb.148227$U%5.676753@attbi_s03...
: > : > : Boomer,
: > : > :
: > : > : I am not sure if you are just messing with me or if you are truly
: > : confused.
: > : > : I hope the latter. Please read from Top to Bottom.
: > : > :
: > : > :
: > : > : From YOUR first link:
: > : > :
: > : > : http://www.waterontheweb.org/resources/glossary.html
: > : > :
: > : > : Acidity:
: > : > : A measure of how acid a solution may be. A solution with a pH of
: less
: > : than
: > : > : 7.0 is considered acidic. Solutions with a pH of less than 4.5
: contain
: > : > : mineral acidity (due to strong inorganic acids), while a solution
: having
: > : a
: > : > : pH greater than 8.3 contains no acidity.
: > : > :
: > : > : Yes,
: > : > :
: > : > : Good definition (for the most part). pH <7 is indeed acidic. pH >
: 7 is
: > : > : basic. Your web page had a definition for acidity, but not
: basicity.
: > : > : Strange. That's like defining GOOD and not defining BAD.
: > : > :
: > : > : Here is the IUPAC (International Union of Pure and Applied
: Chemistry)
: > : > : definition of acidity:
: > : > :
: > : > : http://www.chem.qmul.ac.uk/iupac/index.html
: > : > :
: > : > : acidity
: > : > :
: > : > : (1) Of a compound:
: > : > :
: > : > : For Brønsted acids it means the tendency of a compound to act as a
: > : hydron
: > : > : donor. It can be quantitatively expressed by the acid dissociation
: > : constant
: > : > : of the compound in water or some other specified medium. For Lewis
: acids
: > : it
: > : > : relates to the association constants of Lewis adducts and -adducts.
: > : > :
: > : > : (2) Of a medium:
: > : > :
: > : > : The use of the term is mainly restricted to a medium containing
: Brønsted
: > : > : acids, where it means the tendency of the medium to hydronate a
: specific
: > : > : reference base
: > : > :
: > : > : basicity
: > : > :
: > : > : For Brønsted bases it means the tendency of a compound to act as
: hydron
: > : > : (proton) acceptor. The basicity of a chemical species is normally
: > : expressed
: > : > : by the acidity of the conjugate acid (see conjugate acid-base pair).
: For
: > : > : Lewis bases it relates to the association constants of Lewis adducts
: > : > : and -adducts
: > : > :
: > : > :
: > : > :
: > : > : Another definition from the same web page YOU cited: (this is the
: same
: > : web
: > : > : page you cited above)
: > : > :
: > : > : Alkalinity:
: > : > : Acid neutralizing or buffering capacity of water; a measure of the
: > : ability
: > : > : of water to resist changes in pH caused by the addition of acids or
: > : bases
: > : > : and therefore, the main indicator of susceptibility to acid rain; in
: > : natural
: > : > : waters it is due primarily to the presence of bicarbonates,
: carbonates
: > : and
: > : > : to a much lesser extent occasionally borates, silicates and
: phosphates.
: > : It
: > : > : is expressed in units of milligrams per liter (mg/l) of CaCO3
: (calcium
: > : > : carbonate) or as microequivalents per liter (ueq/l) where 20 ueq/l =
: 1
: > : mg/l
: > : > : of CaCO3. A solution having a pH below about 5 contains no
: alkalinity.
: > : > :
: > : > : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER and
: says
: > : > : that alkalinity is the measure of ...(description of a buffer)
: > : > :
: > : > : A BUFFER IS : a measure of the ability of water to resist changes in
: pH
: > : > : caused by the addition of acids or bases (from definition below)
: > : > :
: > : > :
: > : > : I said:
: > : > : ***alkalinity is a measurement of 'buffering capacity'***
: > : > :
: > : > : You said:
: > : > : ***Alkalinity is not a measurement of BC
: > : > :
: > : > : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This is
: not
: > : > : logical.
: > : > :
: > : > : (THIS FROM THE SAME WEB PAGE YOU CITED):
: > : > :
: > : > : Buffer:
: > : > : A substance which tends to keep pH levels fairly constant when acids
: or
: > : > : bases are added.
: > : > :
: > : > : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
: > : > :
: > : > : a measure of the ability of water to resist changes in pH caused by
: the
: > : > : addition of acids or bases
: > : > :
: > : > : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A
: BUFFER.
: > : > :
: > : > :
: > : > : I went to all four links. None contradict what I have said. But
: the
: > : first
: > : > : one you cited contradicts YOU!
: > : > :
: > : > : I know what a buffer is. I know what acidity means. I know what
: > : alkalinity
: > : > : means. No need to cite web pages that describe what I know and what
: I
: > : wrote
: > : > : in this discussion. Show me one that says alkalinity is not a
: measure
: > : of
: > : > : buffering capacity from a credible source.
: > : > :
: > : > :
: > : > :
: > : > :
: > : > :
: > : > :
: > : > : "Boomer" > wrote in message
: > : > : ...
: > : > : > Alkalinity a measure of the amount of anions of weak acid in water
: and
: > : of
: > : > : the cations
: > : > : > balanced against them
: > : > : > Take note it says ***acid***
: > : > : >
: > : > : > Buffering capacity the ability of a solution to resist or dampen
: > : changes
: > : > : in pH upon the
: > : > : > addition of acids or bases.
: > : > : > Take note its says ***the addition of acids or bases***
: > : > : >
: > : > : > One more
: > : > : >
: > : > : > http://www.waterontheweb.org/resources/glossary.html
: > : > : >
: > : > : > We could go on like this all day, so what is the point ?
: > : > : >
: > : > : > You will LOVE this one
: > : > : > http://www.kyantec.com/Tips/phbuffering.htm
: > : > : >
: > : > : > Don't you just lovbe PDF's
: > : > : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
: > : > : >
: > : > : > Don't fall out of your chair
: > : > : >
: http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
: > : > : >
: > : > : >
: > : > : >
: > : > : >
: > : > : > --
: > : > : > Boomer
: > : > : >
: > : > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > : > http://www.reefcentral.com/vbulletin/index.php
: > : > : >
: > : > : > Want to See More ?
: > : > : > Please Join Our Growing Membership
: > : > : > www.coralrealm.com
: > : > : >
: > : > : > If You See Me Running You Better Catch-Up
: > : > : > "stoutman" <.@.> wrote in message
: > : news:XB7Wb.19339$QA2.62332@attbi_s52...
: > : > : > : Man here is another, google is a wonderful thing. I'm not
: filtering
: > : any
: > : > : > : out, just posting what I find by GOOGLING for you.
: > : > : > :
: > : > : > :
: http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
: > : > : > :
: > : > : > :
: > : > : > : Wow, a gov link. Even the government is wrong, this must be a
: > : > : conspiracy
: > : > : > : against Boomer.
: > : > : > :
: > : > : > :
: > : > : > :
: > : > : > :
: > : > : > : "Boomer" > wrote in message
: > : > : > : ...
: > : > : > : > Now I am getting bored
: > : > : > : >
: > : > : > : > "Don't the components of a buffer account for the buffering
: > : capacity?
: > : > : > : Yes."
: > : > : > : >
: > : > : > : > Yes, agreed but you seem to fail what I'm saying. Buffering
: > : Capacity
: > : > : and
: > : > : > : Alkalinity are
: > : > : > : > not the same, that has always been the issue. I gave the
: equation
: > : does
: > : > : > : that look like an
: > : > : > : > Alkalinity equation or how Alk is determined. I see you had
: now
: > : > : comments
: > : > : > : on it what's
: > : > : > : > wrong, why no comments on the equations I gave. Don't
: understand
: > : them
: > : > : or
: > : > : > : what ? Again this
: > : > : > : > is the equation for Buffering Capacity, also called Buffer
: Index
: > : or
: > : > : Buffer
: > : > : > : Intensity. It
: > : > : > : > is defined in most water chemistry and chemical oceanography
: text
: > : > : books.
: > : > : > : >
: > : > : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] +
: [H30+] +
: > : > : CKa
: > : > : > : [H3O+] / (Ka =
: > : > : > : > H3O+])² )
: > : > : > : >
: > : > : > : > This is not Alkalinity now is it ?
: > : > : > : >
: > : > : > : > "I know how to do a titration, In fact I have done several.
: How
: > : many
: > : > : have
: > : > : > : > you actually done? I don't mean by counting drops, I mean
: with a
: > : > : buret?"
: > : > : > : >
: > : > : > : > Well good for you, I use a Digital Titrator
: > : > : > : >
: > : > : > : > "Oh, I see,
: > : > : > : > you think acidity is the opposite of alkalinity. In the world
: of
: > : > : > : CHEMISTRY
: > : > : > : > it's not. Maybe in aquarium newsgroups it is.
: > : > : > : >
: > : > : > : > Hum no, maybe you should go for a look at HACH's or LaMotte
: > : website or
: > : > : the
: > : > : > : book I
: > : > : > : > suggested earlier. Please view a copy.
: > : > : > : >
: > : > : > : > Standard Methods for the Examination of Water and Wastewater
: > : > : > : >
: > : > : > : > This book, over 2000 pages, is the guide for water testing. If
: you
: > : are
: > : > : > : reporting water
: > : > : > : > test to the EPA you must use approved std from this text.I t
: is
: > : > : prepared
: > : > : > : and published by
: > : > : > : > the EPA, American Water Works Association and American Public
: > : Health
: > : > : > : Association. You
: > : > : > : > mean you don't have one and the issue is water chemistry
: > : > : > : >
: > : > : > : > You are confusing Acidity and Acidity as you know little about
: > : water
: > : > : > : chemistry and
: > : > : > : > procedures and test methods
: > : > : > : >
: > : > : > : > From SMEWW, section 2-30, 2310 ACIDITY
: > : > : > : >
: > : > : > : > "Acidity of water is its quantative capacity to react with a
: > : strong
: > : > : base
: > : > : > : to a designated
: > : > : > : > pH"
: > : > : > : >
: > : > : > : > This is how you test for it
: > : > : > : >
: > : > : > : > A std alkali titration to methyl orange or phenolphthalein
: > : > : > : > endpoint.
: > : > : > : >
: > : > : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist that
: > : write
: > : > : this
: > : > : > : book, there are
: > : > : > : > over 100 of them, they are wrong.
: > : > : > : >
: > : > : > : > Like Buffering Capacity you have your Acidity's mixed up
: > : > : > : > In water measurement if you have a high Alk you also usually
: have
: > : a
: > : > : high
: > : > : > : Acidity.
: > : > : > : > Normally a high Alk also gives a higher CO2 level. Get a WATER
: > : > : CHEMISTRY
: > : > : > : BOOK there pal.
: > : > : > : >
: > : > : > : >
: > : > : > : > "These are all in equilibrium with each other. An initial
: high pH
: > : > : (above
: > : > : > : > 6.4) will shift the equilibrium to the right to form HCO3-1.
: If
: > : the
: > : > : pH of
: > : > : > : > the solution is above 10.3 (pKa2) the .........."
: > : > : > : >
: > : > : > : >
: > : > : > : > Christ, there you go again with the FW ****. All your numbers
: are
: > : > : wrong we
: > : > : > : are dealing
: > : > : > : > with SEAWATER
: > : > : > : >
: > : > : > : > This means that at a pH of 8.3, the majority of the CO2(aq) is
: in
: > : the
: > : > : form
: > : > : > : > of HCO3-1 .
: > : > : > : >
: > : > : > : > I have already pointed that out and gave actual values at know
: > : > : seawater
: > : > : > : levels, go back
: > : > : > : > and re-read it you aren't telling me anything here.Of course
: most
: > : is
: > : > : HCO3
: > : > : > : see...
: > : > : > : >
: > : > : > : >
: > : > : > : > @ 20C and 34.3 ppt salinity
: > : > : > : >
: > : > : > : > CO2 = 0.52 %
: > : > : > : >
: > : > : > : > HCO3 = 86.4 %
: > : > : > : >
: > : > : > : > CO3 = 13.09 %
: > : > : > : >
: > : > : > : >
: > : > : > : > "In your glass experiment you managed to lower the pH enough
: to
: > : purge
: > : > : out
: > : > : > : CO2
: > : > : > : > by boiling"
: > : > : > : >
: > : > : > : > The purpose behind the glass is to show that alk is not affect
: by
: > : CO2
: > : > : and
: > : > : > : vise-versa and
: > : > : > : > how Co2 affects pH.
: > : > : > : >
: > : > : > : > Now, in a real life seawater aquarium, with a pH of 8.3 and
: that
: > : pH
: > : > : drops
: > : > : > : to say 8.1 it is
: > : > : > : > usually due to excess CO2. If you took a glass of that water
: and
: > : > : aerated
: > : > : > : it you WILL drive
: > : > : > : > off the CO2 and raise the pH. It has been done a proven a
: million
: > : > : times.
: > : > : > : >
: > : > : > : > "In order to 'purge' CO2 you would need to lower the
: > : > : > : > pH to shift the equilibrium to below 6.4"
: > : > : > : >
: > : > : > : > The hell you do !!!.Do you know who many times people on this
: NG
: > : to
: > : > : > : include Dr. Craig
: > : > : > : > Bingman a chemist and Dr. Randy Holmes-Farley have mentioned
: to
: > : take a
: > : > : > : sample of aquarium
: > : > : > : > water and aerate it to see if the pH GOES UP AND when they
: come
: > : back
: > : > : with
: > : > : > : the test it is
: > : > : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D
: CHEMIST
: > : > : excess
: > : > : > : CO2 in the tank
: > : > : > : > water, increase the circulation for better gas exchange at the
: > : > : surface,
: > : > : > : reduce feeding,
: > : > : > : > and try to improve on better skimming, thus reducing the
: bio-load
: > : and
: > : > : pH
: > : > : > : decline due to
: > : > : > : > CO2.
: > : > : > : >
: > : > : > : >
: > : > : > : > "I hope this helps. "
: > : > : > : >
: > : > : > : > Help, how can you when you miss everything. I should be
: charging
: > : you
: > : > : > : >
: > : > : > : > Oh, by the way. Your websites, I have about 50 on these
: issues, I
: > : > : could
: > : > : > : post them, not to
: > : > : > : > mention I have all those water chemistry books, so there is no
: > : need to
: > : > : > : view your sites.
: > : > : > : >
: > : > : > : > Finally are you afraid to come to our Chemistry Forum, afraid
: to
: > : get
: > : > : > : slapped by REAL
: > : > : > : > chemists. I get a charge out of you can't post your ref .I
: have
: > : posted
: > : > : the
: > : > : > : same or similar
: > : > : > : > stuff on his forum and I wasn't pointed out WRONG pal. I have
: 1500
: > : > : posts
: > : > : > : there and am the
: > : > : > : > biggest contributor to his forum other than himself or maybe
: Habib
: > : > : Sheka
: > : > : > : >
: > : > : > : > Hum, here are Randy's ref that he posted. He hosts the website
: > : > : > : >
: > : > : > : > S. RANDY HOLMES-FARLEY
: > : > : > : > Arlington, Massachusetts
: > : > : > : >
: > : > : > : > EDUCATION
: > : > : > : >
: > : > : > : > 1982-1986 Harvard University Cambridge, MA
: > : > : > : > PhD in Chemistry
: > : > : > : > Research Advisor: George Whitesides
: > : > : > : >
: > : > : > : > Investigated the relationship between polymer surface
: chemistry
: > : and
: > : > : > : physical properties
: > : > : > : > through controlled surface modification and testing.
: > : > : > : >
: > : > : > : > 1980-1982 Cornell University Ithaca, NY
: > : > : > : > BA in Chemistry and Biology
: > : > : > : > Graduated Summa Cum Laude
: > : > : > : > Distinction in All Subjects
: > : > : > : > Grade Point: 3.94/4.0
: > : > : > : > Honors research: isolation and characterization of the subunit
: of
: > : CF1
: > : > : > : enzyme
: > : > : > : >
: > : > : > : >
: > : > : > : > 1978-1979 Stanford University Palo Alto, CA
: > : > : > : > Grade Point: 3.55/4.0
: > : > : > : >
: > : > : > : >
: > : > : > : > EXPERIENCE
: > : > : > : >
: > : > : > : > 1992- present Genzyme Drug Disvcovery and Development Waltham,
: MA
: > : > : > : > (bought out GelTex Pharmaceuticals in 2001)
: > : > : > : > Vice President, Chemical Research 2001-present
: > : > : > : > Senior Director, Chemical Research 1999-2001
: > : > : > : > Director of Chemical Research 1997-1999
: > : > : > : > Manager of Chemical Research 1995-1997
: > : > : > : > Group Leader 1994-1995
: > : > : > : > Senior Research Scientist 1992-1994
: > : > : > : >
: > : > : > : > Helped start GelTex as second employee
: > : > : > : >
: > : > : > : > Managed various research programs with multi-million dollar
: > : budgets
: > : > : > : >
: > : > : > : > Supervised research chemists (17+)
: > : > : > : >
: > : > : > : > Co-inventor of several polymeric pharmaceuticals and
: > : pharmaceutical
: > : > : > : candidates including
: > : > : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam
: > : Hydrochloride
: > : > : (FDA
: > : > : > : approved)
: > : > : > : >
: > : > : > : > Company Safety Officer for 3 years
: > : > : > : >
: > : > : > : > Chemical Hygiene Officer 2000-present
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > 1990-1992 GTE Corporation Waltham, MA
: > : > : > : > Senior Member of Technical Staff
: > : > : > : > Applied research involving polymer interfaces
: > : > : > : > Metallization of plastics
: > : > : > : > Polymer/polymer adhesion
: > : > : > : > Optical coatings
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > 1986-1990 Lord Corporation Cary, NC
: > : > : > : > Senior Research Scientist 1988-1990
: > : > : > : > Research Scientist 1986-1988
: > : > : > : > Basic and applied research on surface chemical bonding
: > : > : > : > Developed new adhesive compositions
: > : > : > : > Developed new sol-gel coatings for corrosion resistance
: > : > : > : >
: > : > : > : >
: > : > : > : > HONORS AND AWARDS
: > : > : > : >
: > : > : > : > Industrial Innovations Award by Northeast Region of American
: > : Chemical
: > : > : > : Society (6/2001)
: > : > : > : >
: > : > : > : > National Kidney Foundation of Northern California Honoree
: (5/2001)
: > : > : > : >
: > : > : > : > American Chemical Society/Polymer Chemistry Division
: Industrial
: > : > : Sponsors
: > : > : > : > Award (8/2000)
: > : > : > : >
: > : > : > : > R&D 100 Award from R&D magazine (1999)
: > : > : > : >
: > : > : > : > Sherwin Williams Award in applied polymer science (9/85)
: > : > : > : >
: > : > : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985;
: > : 1985-1986)
: > : > : > : >
: > : > : > : > Award for highest GPA in Chemistry Department (6/82)
: > : > : > : >
: > : > : > : > Summa Cum Laude Honors in Chemistry (6/82)
: > : > : > : >
: > : > : > : > Phi Lamda Epsilon (6/82)
: > : > : > : >
: > : > : > : > Phi Beta Kappa (2/82)
: > : > : > : >
: > : > : > : > Cornell University Dean's List (1981, 1982)
: > : > : > : >
: > : > : > : > Harvard Book Club Award for highest GPA senior year (1978)
: > : > : > : >
: > : > : > : > First Place in western NY ACS high school chemistry exam
: (1977)
: > : > : > : >
: > : > : > : > 1978-1979
: > : > : > : >
: > : > : > : >
: > : > : > : > __________________
: > : > : > : > Randy Holmes-Farley
: > : > : > : > Want to talk chemistry? Try the Reef Chemistry Forum at Reef
: > : Central
: > : > : > : >
: > : > : > : > Hobby Experience: 8 years with reefs
: > : > : > : > Current Tanks: 90 gal mixed reef
: > : > : > : > Interests: Reefkeeping, science, photography
: > : > : > : >
: > : > : > : >
: > : > : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49 PM
: > : > : > : >
: > : > : > : > Open this post in a new window | Report this post to a
: moderator |
: > : IP:
: > : > : > : Logged
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > 06/27/2003 02:44 PM
: > : > : > : >
: > : > : > : > Randy Holmes-Farley
: > : > : > : > Chemistry Moderator
: > : > : > : >
: > : > : > : > Registered: Apr 2001
: > : > : > : > Location: Arlington, Massachusetts
: > : > : > : > Occupation: Chemist (Drug Discovery at Genzyme)
: > : > : > : > Posts: 15282
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > Publications
: > : > : > : >
: > : > : > : >
: > : > : > : > ISSUED UNITED STATES PATENTS
: > : > : > : >
: > : > : > : >
: > : > : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen
: Randall;
: > : > : > : Mandeville, III; W. Harry.
: > : > : > : > US 6,566,407; 5/20/2003
: > : > : > : >
: > : > : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley,
: Stephen
: > : > : Randall;
: > : > : > : Huval, Chad
: > : > : > : > Cori.
: > : > : > : > U.S. 6,517,825; 2/11/2003.
: > : > : > : >
: > : > : > : > 3. Method of making phosphate-binding polymers for oral
: > : > : administration.
: > : > : > : Holmes-Farley,
: > : > : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George M.
: U.S.
: > : > : > : 6,509,013; 1/21/2003.
: > : > : > : >
: > : > : > : > 4. Combination therapy for treating hypercholesterolemia using
: a
: > : bile
: > : > : acid
: > : > : > : sequestrant
: > : > : > : > polymer
: > : > : > : > and a cholesterol-lowering agent. Huval, Chad Cori;
: Holmes-Farley,
: > : > : Stephen
: > : > : > : Randall;
: > : > : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026; 8/13/2002.
: > : > : > : >
: > : > : > : > 5. Method for treating hypercholesterolemia with
: polyallylamine
: > : > : polymers.
: > : > : > : Holmes-Farley,
: > : > : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven K.;
: > : > : Goldberg,
: > : > : > : Dennis I. , US
: > : > : > : > 6,423,754; 7/23/2002.
: > : > : > : >
: > : > : > : > 6. Ionic polymers as anti-infective agents Mandeville, W.
: Harry,
: > : III;
: > : > : > : Neenan, Thomas X..;
: > : > : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
: > : > : > : >
: > : > : > : > 7. Combination therapy for treating hypercholesterolemia and
: > : > : > : atherosclerosis. Huval, Chad
: > : > : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.; Dhal,
: > : Pradeep
: > : > : K.
: > : > : > : U.S. 6,365,186;
: > : > : > : > 4/2/2002.
: > : > : > : >
: > : > : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S. R.;
: > : > : Mandeville,
: > : > : > : W. H., III;
: > : > : > : > Huval; C.
: > : > : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US
: 6,299,868;
: > : > : > : 10/9/2001.
: > : > : > : >
: > : > : > : > 9. Polymers containing guanidinium groups as bile acid
: > : sequestrants.
: > : > : Dhal;
: > : > : > : P. K.; Holmes-
: > : > : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
: > : > : > : >
: > : > : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.;
: Mandeville,
: > : W.
: > : > : H.,
: > : > : > : III.; US
: > : > : > : > 6,281,252;
: > : > : > : > 8/28/2001.
: > : > : > : >
: > : > : > : > 11. Combination therapy for treating hypercholestrolemia.
: Huval;
: > : C.
: > : > : C.;
: > : > : > : Holmes-Farley; S.
: > : > : > : > R. ;
: > : > : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
: > : > : > : >
: > : > : > : > 12. Fat-binding polymers. Mandeville, W. H., III.; Whitesides,
: G.
: > : M.;
: > : > : > : Holmes-Farley, S.
: > : > : > : > R.; US
: > : > : > : > 6,264,937; 7/24/2001.
: > : > : > : >
: > : > : > : > 13. Method for treating hypercholesterolemia with
: unsubstituted
: > : > : > : polydiallylamine polymers.
: > : > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
: K.
: > : ; US
: > : > : > : 6,248,318;
: > : > : > : > 6/19/2001.
: > : > : > : >
: > : > : > : > 14. Process for removing bile salts from a patient and
: alkylated
: > : > : > : compositions therefore.
: > : > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,225,355;
: > : 5/1/2001.
: > : > : > : >
: > : > : > : > 15. Poly(diallylamine)-based bile acid sequestrants.
: > : Holmes-Farley, S.
: > : > : R.;
: > : > : > : Dhal, P. K.;
: > : > : > : > Petersen,
: > : > : > : > J. S.; US 6,203,785; 3/20/2001.
: > : > : > : >
: > : > : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley, S.
: R.;
: > : > : Huval,
: > : > : > : C. C.; US
: > : > : > : > 6,190,649;
: > : > : > : > 2/20/2001.
: > : > : > : >
: > : > : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.;
: Mandeville,
: > : W.
: > : > : H.,
: > : > : > : III.; US
: > : > : > : > 6,177,478;
: > : > : > : > 1/23/2001.
: > : > : > : >
: > : > : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
: > : > : Holmes-Farley,
: > : > : > : S. R.;
: > : > : > : > Mandeville, W.
: > : > : > : > H., III.; US 6,129,910; 10/10/2000.
: > : > : > : >
: > : > : > : > 19. Method for treating hypercholesterolemia with
: unsubstituted
: > : > : > : polydiallylamine polymers.
: > : > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.; Dhal; P.
: K.
: > : ; US
: > : > : > : 6,083,497;
: > : > : > : > 7/4/2000.
: > : > : > : >
: > : > : > : > 20. Method of making phosphate-binding polymers for oral
: > : > : administration.
: > : > : > : Holmes-Farley, S.
: > : > : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US
: 6,083,495;
: > : > : 7/4/2000.
: > : > : > : >
: > : > : > : > 21. Process for removing bile salts from a patient and
: alkylated
: > : > : > : compositions therefore.
: > : > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US 6,066,678;
: > : > : 5/23/2000.
: > : > : > : >
: > : > : > : > 22. Process for removing bile salts from a patient and
: > : compositions
: > : > : > : therefor. Mandeville,
: > : > : > : > W. H.,
: > : > : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
: > : > : > : >
: > : > : > : > 23. Ionic polymers as anti-infective agents. Mandeville, III;
: W.
: > : H;
: > : > : > : Neenan; T. X.; Holmes-
: > : > : > : > Farley; S. R. US 6,034,129; 3/7/2000.
: > : > : > : >
: > : > : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.;
: Mandeville,
: > : W.
: > : > : H.,
: > : > : > : III.; US
: > : > : > : > 5,985,938;
: > : > : > : > 11/16/99.
: > : > : > : >
: > : > : > : > 25. Process for removing bile salts from a patient and
: > : compositions
: > : > : > : therefor. Mandeville,
: > : > : > : > W. H.,
: > : > : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
: > : > : > : >
: > : > : > : > 26. Hydrophobic sequestrant for cholesterol depletion.
: Mandeville,
: > : W.
: > : > : H.,
: > : > : > : III.;
: > : > : > : > Holmes-Farley;
: > : > : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
: > : > : > : >
: > : > : > : > 27. Hydrophilic nonamine-containing and amine-containing
: > : copolymers
: > : > : and
: > : > : > : their use as bile
: > : > : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S.. US
: > : > : 5,929,184;
: > : > : > : 7/27/99.
: > : > : > : >
: > : > : > : > 28. Interpenetrating polymer networks for sequestration of
: bile
: > : acids.
: > : > : > : Mandeville, W. H.,
: > : > : > : > III.;
: > : > : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US
: > : 5,925,379;
: > : > : > : 7/20/99.
: > : > : > : >
: > : > : > : > 29. Amine polymer sequestrant and method of cholesterol
: depletion.
: > : > : > : Mandeville, W. H.,
: > : > : > : > III.;
: > : > : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
: > : > : > : >
: > : > : > : > 30. Process for removing bile salts from a patient and
: > : compositions
: > : > : > : therefor. Mandeville,
: > : > : > : > W. H.,
: > : > : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
: > : > : > : >
: > : > : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
: > : depletion.
: > : > : > : Mandeville, W. H.,
: > : > : > : > III.;
: > : > : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475; 5/4/99.
: > : > : > : >
: > : > : > : > 32. Process for removing bile salts from a patient and
: > : compositions
: > : > : > : therefor. Mandeville,
: > : > : > : > W. H.,
: > : > : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
: > : > : > : >
: > : > : > : > 33. Preparation of polymeric sequestrants for bile acid salts.
: > : > : Mandeville,
: > : > : > : W. H., III.;
: > : > : > : > Holmes-
: > : > : > : > Farley, S. R.; US 5,703,188; 12/30/97.
: > : > : > : >
: > : > : > : > 34. Oral administration of iron-binding crosslinked amine
: > : polymers.
: > : > : > : Mandeville, W. H.,
: > : > : > : > III.;
: > : > : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
: > : > : > : >
: > : > : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
: > : Holmes-Farley,
: > : > : S.
: > : > : > : R.; US 5,693,675;
: > : > : > : > 12/2/97.
: > : > : > : >
: > : > : > : > 36. Method for removing bile salts from a patient with
: alkylated
: > : > : > : crosslinked amine
: > : > : > : > polymers,
: > : > : > : > and preparation of the polymers. Mandeville, W. H., III.;
: > : > : Holmes-Farley,
: > : > : > : S. R.; US
: > : > : > : > 5,679,717; 10/21/97.
: > : > : > : >
: > : > : > : > 37. Phosphate-binding polymers for oral administration.
: > : Holmes-Farley,
: > : > : S.
: > : > : > : R.; Mandeville,
: > : > : > : > W.
: > : > : > : > H., III.; US 5,667,775; 9/16/97.
: > : > : > : >
: > : > : > : > 38. Ion-exchange process using highly crosslinked polymers for
: > : > : removing
: > : > : > : bile salts from a
: > : > : > : > patient, preparation of the polymers, and compositions
: containing
: > : > : them.
: > : > : > : Mandeville, W. H.,
: > : > : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
: > : > : > : >
: > : > : > : > 39. Hydrophobic amine polymer sequestrant and method of
: > : cholesterol
: > : > : > : depletion. Mandeville,
: > : > : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US
: 5,618,530;
: > : > : 4/8/97.
: > : > : > : >
: > : > : > : > 40. Amine polymer sequestrant and method of cholesterol
: depletion.
: > : > : > : Mandeville, W. H.,
: > : > : > : > III.;
: > : > : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
: > : > : > : >
: > : > : > : > 41. Phosphate-binding polymers for oral administration.
: > : Holmes-Farley,
: > : > : S.
: > : > : > : R.; Mandeville,
: > : > : > : > W.
: > : > : > : > H., III.; US 5,496,545; 3/5/96.
: > : > : > : >
: > : > : > : > 42. Iron-binding polymers for oral administration. Mandeville,
: W.
: > : H.,
: > : > : > : III.; Holmes-Farley,
: > : > : > : > S. R.;
: > : > : > : > US 5,487,888; 1/30/96.
: > : > : > : >
: > : > : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate having
: > : active
: > : > : > : hydrogens on the
: > : > : > : > surface.
: > : > : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027; 12/29/92.
: > : > : > : >
: > : > : > : > 44. Layered sol-gel coatings from organisilicon compounds.
: > : > : Holmes-Farley,
: > : > : > : S. R.; Yanyo, L.
: > : > : > : > C.;
: > : > : > : > US 5,182,143; 1/26/93.
: > : > : > : >
: > : > : > : > 45. Method for metal bonding using ultrathin primer coating.
: > : > : > : Holmes-Farley, S. R.; Yanyo,
: > : > : > : > L.
: > : > : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
: > : > : > : >
: > : > : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.;
: Abbey, K.
: > : J.;
: > : > : US
: > : > : > : 5,096,962;
: > : > : > : > 3/17/92.
: > : > : > : >
: > : > : > : > 47. Modified halogenatedpolyolefin adhesives for polyolefin
: > : > : > : elastomer-metal bonding.
: > : > : > : > Holmes-
: > : > : > : > Farley, S. R.; US 5,102,956; 4/7/92.
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT
: ISSUED)
: > : > : > : >
: > : > : > : >
: > : > : > : > 1. Aryl boronate functionalized polymers for treating obesity
: and
: > : > : > : inhibiting fat uptake.
: > : > : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III;
: Dhal,
: > : > : Pradeep
: > : > : > : K.; Huval, Chad
: > : > : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl.
: (2003),
: > : 92
: > : > : pp. WO
: > : > : > : 0302571.
: > : > : > : >
: > : > : > : > 2. Preparation of aryl boronic acids for treating obesity.
: > : > : Holmes-Farley,
: > : > : > : Stephen Randall;
: > : > : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua; Dhal,
: > : Pradeep
: > : > : K.
: > : > : > : (Geltex
: > : > : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp. WO
: > : 0302570.
: > : > : > : >
: > : > : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide.
: > : Holmes-Farley,
: > : > : > : Stephen Randall.
: > : > : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 32
: pp.
: > : WO
: > : > : > : 0302130.
: > : > : > : >
: > : > : > : > 4. Method for reducing copper levels and treating copper
: > : toxicosis.
: > : > : > : Holmes-Farley, Stephen
: > : > : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl.
: > : (2002),
: > : > : 45
: > : > : > : pp. WO
: > : > : > : > 0285383.
: > : > : > : >
: > : > : > : > 5. Method for treating gout and binding uric acid.
: Holmes-Farley,
: > : > : Stephen
: > : > : > : Randall; Burke,
: > : > : > : > Steven K. WO 0285381 10/31/2002.
: > : > : > : >
: > : > : > : > 6. Method for treating gout and reducing serum uric acid.
: > : > : Holmes-Farley,
: > : > : > : Stephen Randall;
: > : > : > : > Burke, Steven K WO 0285380 10/31/2002.
: > : > : > : >
: > : > : > : > 7. Amine condensation polymer bile acid sequestrants. Huval,
: C.
: > : C.;
: > : > : > : Holmes-Farley, S. R.;
: > : > : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
: > : > : > : >
: > : > : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W. H.,
: III
: > : and
: > : > : > : Holmes-Farley, S.
: > : > : > : > R.;
: > : > : > : > WO 1999-US5662; 9/23/1999.
: > : > : > : >
: > : > : > : > 9. Amine-containing copolymers as bile acid sequestrants.
: > : > : Holmes-Farley,
: > : > : > : S. R.; Petersen,
: > : > : > : > J. S.;
: > : > : > : > WO 9933452; 7/8/1999.
: > : > : > : >
: > : > : > : > 10. Polydiallylamine-based phosphate binders. Mandeville, W.
: H.,
: > : III
: > : > : and
: > : > : > : Holmes-Farley, S.
: > : > : > : > R.;
: > : > : > : > WO 9922743; 5/14/1999.
: > : > : > : >
: > : > : > : > 11. Polyallylamine polymers for removing bile salts and
: treating
: > : > : > : hypercholesterolemia, and
: > : > : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W. H.,
: III;
: > : > : Burke,
: > : > : > : S. K.; Goldberg,
: > : > : > : > D. I.; WO 9857652; 12/23/98.
: > : > : > : >
: > : > : > : > 12. Phosphate-bidning polymers combined with a calcium
: supplement
: > : for
: > : > : oral
: > : > : > : administration.
: > : > : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
: > : Holmes-Farley,
: > : > : S.
: > : > : > : R.; WO 9842355;
: > : > : > : > 10/1/98.
: > : > : > : >
: > : > : > : > 13. Hydrophobic heteroatom-containing sequestrant for
: cholesterol
: > : > : > : depletion. Mandeville,
: > : > : > : > W.
: > : > : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO 9639449;
: > : 12/12/96.
: > : > : > : >
: > : > : > : > 14. Process for adjusting ion concentration in a patient and
: > : > : compositions
: > : > : > : therefor.
: > : > : > : > Mandeville,
: > : > : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
: > : > : > : >
: > : > : > : > 15. Vacuum-deposited silver on polycarbonate with a chromium
: > : > : interlayer
: > : > : > : for improved
: > : > : > : > metal-
: > : > : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen. 4322512;
: > : > : 1/20/94.
: > : > : > : >
: > : > : > : > 16. Process for increased metal-substrate bond strength in
: > : metalized
: > : > : > : plastics.
: > : > : > : > Holmes-Farley, S.
: > : > : > : > R.; Ger. Offen. 4322516; 7/6/93.
: > : > : > : >
: > : > : > : > 17. Electrorheological fluids and preparation of particles
: useful
: > : in
: > : > : the
: > : > : > : fluids.
: > : > : > : > Troughton,
: > : > : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie;
: Carlson,
: > : J.
: > : > : > : David; Bares, Joseph
: > : > : > : > E.;
: > : > : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker, Debra
: Nell.
: > : EP
: > : > : > : 394049;
: > : > : > : > 10/24/1990.
: > : > : > : >
: > : > : > : > JOURNAL PUBLICATIONS
: > : > : > : >
: > : > : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William;
: Zhorov,
: > : > : Eugene;
: > : > : > : Guo, Amy;
: > : > : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek, David
: L.;
: > : > : > : Mandeville, W. Harry;
: > : > : > : > Holmes-Farley, S. Randall. Kidney International (2002), 62(2),
: > : > : 611-619.
: > : > : > : >
: > : > : > : > 2. Amine functionalized polyethers as bile acid sequestrants:
: > : > : synthesis
: > : > : > : and biological
: > : > : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.; Holmes-Farley,
: S.
: > : > : Randall;
: > : > : > : Mandeville, W.
: > : > : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal,
: Pradeep
: > : K.
: > : > : > : Journal of
: > : > : > : > Macromolecular Science, Pure and Applied Chemistry (2001),
: > : A38(12),
: > : > : > : 1559-1574.
: > : > : > : >
: > : > : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by
: > : Molecular
: > : > : > : Imprinting. Huval,
: > : > : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.;
: Holmes-Farley,
: > : S.
: > : > : > : Randall; Mandeville,
: > : > : > : > W.
: > : > : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.; Sacchiro,
: > : Robert
: > : > : J.;
: > : > : > : Chen, Xi; Dhal,
: > : > : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
: > : > : > : >
: > : > : > : > 4. Synthetic polymers for the binding of fat in the intestinal
: > : tract.
: > : > : > : Jozefiak, Thomas H.;
: > : > : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny,
: Cynthia;
: > : > : Huval,
: > : > : > : Chad C.;
: > : > : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney,
: Cynthia.
: > : > : > : Abstracts of
: > : > : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United
: States,
: > : August
: > : > : > : 26-30, 2001
: > : > : > : > (2001), POLY-047 and Polymer Preprints (American Chemical
: Society,
: > : > : > : Division of
: > : > : > : > Polymer Chemistry) (2001), 42(2), 98.
: > : > : > : >
: > : > : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a novel
: > : polymer
: > : > : gel
: > : > : > : pharmaceutical.
: > : > : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.;
: Petersen,
: > : J.;
: > : > : Ward,
: > : > : > : J.; Sacchiero,
: > : > : > : > B.;
: > : > : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.; Norton,
: K.
: > : A.;
: > : > : Chen,
: > : > : > : X.; Mazzeo, J.
: > : > : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
: > : > : > : >
: > : > : > : > 6. In vitro comparison of bile acid binding to colesevelam HCl
: and
: > : > : other
: > : > : > : bile acid
: > : > : > : > sequestrants.
: > : > : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese, W.;
: Xu,
: > : Q.;
: > : > : > : Hook, P.; Holmes-
: > : > : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000), 41(1),
: > : 708-709.
: > : > : > : >
: > : > : > : > 7. Novel polymeric pharmaceuticals: From startup to market.
: > : > : Holmes-Farley,
: > : > : > : S. R; Polym.
: > : > : > : > Mater. Sci. Eng (1999), 80, 246-247.
: > : > : > : >
: > : > : > : > 8. Design and characterization of of Sevelamer Hydrochloride:
: a
: > : novel
: > : > : > : phosphate-binding
: > : > : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H., III;
: > : Ward,
: > : > : J.;
: > : > : > : Miller, K. L.;
: > : > : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J. M.
: S.-
: > : Pure
: > : > : and
: > : > : > : Appl. Chem.,
: > : > : > : > A36(7&8), p. 1085 (1999).
: > : > : > : >
: > : > : > : > 9. Three generations of bile acid sequestrants. Mandeville, W.
: H.,
: > : > : III;
: > : > : > : Braunlin, W.;
: > : > : > : > Dhal, P.;
: > : > : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.; Polomascanik,
: S.;
: > : > : > : Rosenbaum, D.;
: > : > : > : > Sacchiero,
: > : > : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp. Proc.
: > : (1999),
: > : > : > : 550, 3-15.
: > : > : > : >
: > : > : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked,
: polymeric
: > : > : phosphate
: > : > : > : binder, on
: > : > : > : > urinary
: > : > : > : > phosphorous excretion in rats. Rosenbaum, D. P.;
: Holmes-Farley, S.
: > : R.;
: > : > : > : Mandeville, W. H.,
: > : > : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
: > : Transplant.
: > : > : > : (1997), 12(5)
: > : > : > : > 961-964.
: > : > : > : >
: > : > : > : > 11. Thin anisotropic coatings based on sol-gel technology.
: > : > : Holmes-Farley,
: > : > : > : S. R.; Yanyo, L.
: > : > : > : > C;
: > : > : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram. Chem.
: 4),
: > : > : 439-444.
: > : > : > : >
: > : > : > : > 12. The mechanism of cure initiation of a surface activated
: > : adhesive.
: > : > : > : Holmes-Farley, S.
: > : > : > : > R.;
: > : > : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5),
: 409-420.
: > : > : > : >
: > : > : > : > 13. Adhesion promotion and corrosion prevention using thin
: > : anisotropic
: > : > : > : coatings. Holmes-
: > : > : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol. (1991),
: 5(2),
: > : > : > : 131-151.
: > : > : > : >
: > : > : > : > 14. Wetting of functionalized polyethylene having ionizable
: > : organic
: > : > : acids
: > : > : > : and bases at the
: > : > : > : > polymer-water interface: relations between functional group
: > : polarity,
: > : > : > : extent of
: > : > : > : > ionization,
: > : > : > : > and contact angle with water. Holmes-Farley, S. R.; Bain, C.
: D.;
: > : > : > : Whitesides, G. M.;
: > : > : > : > Langmuir
: > : > : > : > (1988), 4(4), 921-937.
: > : > : > : >
: > : > : > : > 15. Binding of phenols to aluminum oxide surfaces. 1. Phenols
: with
: > : a
: > : > : > : single hydroxy group.
: > : > : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
: > : > : > : >
: > : > : > : > 16. Reconstruction of the interface of oxidatively
: functionalized
: > : > : > : polyethylene (PE-CO2H)
: > : > : > : > and
: > : > : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R. H.;
: > : Nuzzo,
: > : > : R.;
: > : > : > : McCarthy, T. J.;
: > : > : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See also
: Report
: > : > : (1987),
: > : > : > : AD-
: > : > : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987, 87(15).
: > : > : > : >
: > : > : > : > 17. Surface-modified polyethylene film: the relationship
: between
: > : > : surface
: > : > : > : chemistry and
: > : > : > : > physical
: > : > : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987,
: 47(11),
: > : > : 4537.
: > : > : > : >
: > : > : > : > 18. Reactivity of carboxylic acid and ester groups in the
: > : > : functionalized
: > : > : > : interfacial
: > : > : > : > region of
: > : > : > : > "polyethylene carboxylic acid" (PE-CO2H) and its derivatives:
: > : > : > : differentiation of the
: > : > : > : > functional groups into shallow and deep subsets based on a
: > : comparison
: > : > : of
: > : > : > : contact angle and
: > : > : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G. M.;
: > : Langmuir
: > : > : > : (1987), 3(1), 62-
: > : > : > : > 76.
: > : > : > : >
: > : > : > : > 19. Fluorescence properties of dansyl groups covalently bonded
: tot
: > : he
: > : > : > : surface of
: > : > : > : > oxidatively
: > : > : > : > functionalized low-density polyethylene film. Holmes-Farley,
: S.
: > : R.;
: > : > : > : Whitesides, G. M.;
: > : > : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985),
: TR-85-2;
: > : > : > : AD-A162435/2/GAR,
: > : > : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
: > : > : > : >
: > : > : > : > 20. Acid-base behavior of carboxylic acid groups covalently
: > : attached
: > : > : at
: > : > : > : the surface of
: > : > : > : > polyethylene: The usefulness of contact angle in following the
: > : > : ionization
: > : > : > : of surface
: > : > : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.; McCarthy,
: T.
: > : J.;
: > : > : > : Deutch, J.;
: > : > : > : > Whitesides,
: > : > : > : > G. M.; Langmuir (1985), 1(6), 725-740.
: > : > : > : >
: > : > : > : > 21. The thermal stability of a surface modified solid organic
: > : polymer.
: > : > : > : Holmes-Farley, S.
: > : > : > : > R.;
: > : > : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53,
: 127-131.
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
: > : > : > : >
: > : > : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley, R.
: > : Advanced
: > : > : > : Aquarist. June 2003.
: > : > : > : >
: > : > : > : > 2. The Self Purification of Limewater (Kalkwasser).
: Holmes-Farley,
: > : R.
: > : > : > : Advanced Aquarist.
: > : > : > : > May
: > : > : > : > 2003.
: > : > : > : >
: > : > : > : > 3. The Degradation of Limewater (Kalkwasser) in Air.
: > : Holmes-Farley, R.
: > : > : > : Reefkeeping May
: > : > : > : > 2003.
: > : > : > : >
: > : > : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
: > : Reefkeeping
: > : > : > : April 2003.
: > : > : > : >
: > : > : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae
: Growth.
: > : > : > : Holmes-Farley, R.
: > : > : > : > Advanced Aquarist; April 2003.
: > : > : > : >
: > : > : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae
: Growth.
: > : > : > : Holmes-Farley, R.
: > : > : > : > Advanced Aquarist; April 2003.
: > : > : > : >
: > : > : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R.
: Advanced
: > : > : Aquarist;
: > : > : > : March 2003.
: > : > : > : >
: > : > : > : > 8. How to Select a Calcium and Alkalinity Supplementation
: Scheme.
: > : > : > : Holmes-Farley, R.
: > : > : > : > Advanced Aquarist; February 2003.
: > : > : > : >
: > : > : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
: > : January
: > : > : > : 2003.
: > : > : > : >
: > : > : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced Aquarist;
: > : > : December
: > : > : > : 2002.
: > : > : > : >
: > : > : > : > 11. Solving Calcium and Alkalinity Problems. Holmes-Farley, R.
: > : > : Advanced
: > : > : > : Aquarist; November
: > : > : > : > 2002.
: > : > : > : >
: > : > : > : > 12. Iron: A Look at Organisms Other than Macroalgae.
: > : Holmes-Farley, R.
: > : > : > : Advanced Aquarist;
: > : > : > : > November 2002.
: > : > : > : >
: > : > : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.;
: Advanced
: > : > : Aquarist,
: > : > : > : September 2002.
: > : > : > : >
: > : > : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced Aquarist,
: > : August
: > : > : > : 2002.
: > : > : > : >
: > : > : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.;
: Reefkeeping.com,
: > : April
: > : > : > : 2002.
: > : > : > : >
: > : > : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R.
: Advanced
: > : > : > : Aquarist; July 2002
: > : > : > : >
: > : > : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced
: Aquarist;
: > : > : June
: > : > : > : 2002.
: > : > : > : >
: > : > : > : > 18. The Relationship Between Alkalinity and pH. Holmes-Farley,
: R.
: > : > : Advanced
: > : > : > : Aquarist, May
: > : > : > : > 2002.
: > : > : > : >
: > : > : > : > 19. The Chemical & Biochemical Mechanisms of Calcification in
: > : Corals.
: > : > : > : Holmes-Farley, R.
: > : > : > : > Advanced Aquarist, April 2002.
: > : > : > : >
: > : > : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March 2002.
: > : > : > : >
: > : > : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist; February
: > : 2002.
: > : > : > : >
: > : > : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist,
: January
: > : > : 2002.
: > : > : > : >
: > : > : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R. Aquarium
: > : Frontiers
: > : > : > : 2000.
: > : > : > : >
: > : > : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R.
: Aquarium
: > : > : > : Frontiers 2000.
: > : > : > : >
: > : > : > : > 25. Phosphate..What is it and why should you care.
: Holmes-Farley,
: > : R.
: > : > : > : Aquarium Frontiers
: > : > : > : > 2000.
: > : > : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R. Aquarium
: > : > : Frontiers
: > : > : > : 2000.
: > : > : > : >
: > : > : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium
: Frontiers
: > : > : 2000.
: > : > : > : >
: > : > : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium
: Frontiers
: > : 1999.
: > : > : > : >
: > : > : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > : > Boomer
: > : > : > : >
: > : > : > : > Want to talk chemistry ? The Reef Chemistry Forum
: > : > : > : > http://www.reefcentral.com/vbulletin/index.php
: > : > : > : >
: > : > : > : > Want to See More ?
: > : > : > : > Please Join Our Growing Membership
: > : > : > : > www.coralrealm.com
: > : > : > : >
: > : > : > : >
: > : > : > : >
: > : > : > :
: > : > : > :
: > : > : >
: > : > : >
: > : > :
: > : > :
: > : > :
: > : >
: > : >
: > :
: > :
: >
: >
:
:

[stoutman]

Boomer,

>Yes, I agree but you don't have to lower the pH to remove CO2 but there is
more CO2 at
> lower pH so it would be easier to degas when there is more.

I NEVER said you HAD to lower the pH. I was unsure of this and said so.
What I did say was at lower pH's CO2 purges more readily. This is not
saying it doesn't purge at higher pH's. It purges LESS readily at higher
pH's

> One more thing that I just found on BC
>


>Where are your answers on the posts on Acidity measurement.

Ok, try to follow this. I HAVE A DIFFERENT DEFINITION OF ACIDITY THAN YOU.
Chemists, in general, use the definition I posted previously. We test for
ACIDITY by measuring pH. We don't have an Acidity test as you refer to it.
I was unaware there was another definition of acidity until you brought it
up.

In chemistry Acidity is the opposite of Basicity. To be completely honest,
I am not interested in your definition of Acidity. Mine has been working
quite well for me. If I were to change my definition of Acidity to yours,
my colleagues would look at me VERY funny. I can only guess that this would
also be the case for you. I don't mean this to be disrespectful. I think
maybe you should stick with your definition of Acidity and I will stick with
mine.

To be honest, I think you are using the Acidity argument to distract from
the original point to this thread, which is alkalinity and BC.

Based on your NEWEST statement about Alkalinity and Buffering Capacity
(Alkalinity is an indication of Buffering Capacity), I can only draw the
conclusion that I helped you understand. I am not saying this to be
pompous. If you had this statement in your head from the beginning, you
would of said it as soon as I said Alkalinity is a measurement of Buffering
Capacity. You only made that statement AFTER I explained it to you. You
never used the word indication until I explained things to you. Indication
of ... and measurement of... are an issue of semantics.

>I would like to have you call Dr.. Millero or e-mail him to see what he
says, maybe I'm
off and you are more right.Yes, I mean that seriously. It would solve the
issue.

No. And I will tell you why. I am not confused on this matter of
alkalinity and buffering capacity. It is PERFECTLY clear to me. For me,
the issue is already SOLVED. I have only been trying to explain it to YOU.
Please don't take this the wrong way. I am not sure if he will be of any
help to you or not. I do not know anything about him. If you want to
contact him for help, go ahead.

Because I honestly believe that I helped you (based on your recent
realization that alkalinity is an indication/measurement of buffering
capacity), this discussion has come to an END for me. You can continue to
debate this matter with everyone else on this NG. I will no longer be
responding to this thread. You and the other participants of this NG can
continue to have the debate and discuss how ignorant I am. You can also
discus with them how I'm just a Post Hole Digger. You guys can also debate
if whether or not I'm really a chemist. I don't care. I said it before, I
have NOTHING to prove. I just wanted to help the original OP and others
that have been following along with this debate. I knew from the start that
you are stubborn and would never admit to being wrong.

Good bye,

-Stoutman




"Boomer" > wrote in message
...
> Yes, I agree but you don't have to lower the pH to remove CO2 but there is
more CO2 at
> lower pH so it would be easier to degas when there is more. But a higher
Alk is almost
> always accompanied by a higher CO2 at the same pH. If it wasn't the pH
would shift.
>
> "Alkalinity was an indication of buffering capacity until this post."
>
> I'm not saying I use those exact words. I said if you know the BC you can
calculate the
> Alk.. correct., which is about the same thing,as thaw would be an
indication.
>
> One more thing that I just found on BC
>
> Bc = d SigmaCO2/dpH
>
> I'll have to look further but must get the hell out of here. Sigma CO2 =
CO2, H2CO3, HCO3
> and CO3. CO2 is not part of the Alk equation, so I'm wondering, if one
throws in CO2 then
> it tells us about what CO2, and Alk will do to the pH. Alk says nothing
of what CO2 does
> to pH, as CO2 has 0 effect on Alk., where it appears CO2 has an effect on
Bc
>
> I have so for PM 'ed Randy and asked him to review Pankow and Millero's
texts for an
> answer on Bc vs Alk. So did you e-mail Millero ?
>
> So if you want to continue on about who said what where, then when are you
going to
> comment on the Acidity measurement post and that it is the opposite of Alk
but I'm an
> idiot for saying such a thing. You seem to think you have this Bc thing
all sewed up, so
> Staut is going for it. Where are your answers on the posts on Acidity
measurement. I think
> this is about the fourth time I have asked you to answer it. You have
still failed. Is it
> because it is real and you said it not, thus making me correct and your
wrong. I don't
> care what the outcome is here, who is right or who wrong, so what is your
beef on it or
> e-mailing Millero. I want real answers don't you. If you won't email
Millero, then I will
> and post both his and Randy's answer here next week
>
>
> --
> Boomer
>
> Want to talk chemistry ? The Reef Chemistry Forum
> http://www.reefcentral.com/vbulletin/index.php
>
> Want to See More ?
> Please Join Our Growing Membership
> www.coralrealm.com
>
> If You See Me Running You Better Catch-Up
> "stoutman" <.@.> wrote in message
news:_X9Xb.304005$xy6.1488576@attbi_s02...
> : one more thing,
> :
> : Let me comment on the CO2 equilibrium.
> :
> : CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid) <------>
> : HCO3-1 <-------> CO3-2
> :
> :
> : I said, and still say, that if you lower the pH the equilibrium will
shift
> : to the left making it EASIER to purge CO2.
> :
> : Yes, as the CO2(g) leaves the system the equilibrium will shift to the
right
> : and pH goes up and CO2 leaves less readily. If you lower the pH again
it
> : will shift to the left again, and CO2 will purge more readily. Then as
CO2
> : leaves the system, the pH will go up and equilibrium starts to shift to
the
> : right. If you lower the pH again the equilibrium will shift to the
left,
> : and CO2 will purge more readily. Then as CO2 leaves the system, the pH
will
> : go up and the equilibrium ...
> :
> : This is the point to this story:
> :
> : At low pH's (acidic) the equilibrium is left shifted. CO2 leaves MORE
> : readily
> : At high pH's (basic) the equilibrium is right shifted. CO2 leaves LESS
> : readily.
> :
> : -Stoutman
> :
> :
> :
> :
> :
> :
> :
> : "Boomer" > wrote in message
> : ...
> : > Yes, of cause I remember, as I said I posted it for a reason. I see
you
> : have used only
> : > that link for your definition, as it makes you look right.You have
avoided
> : all Alk
> : > definitions in a chemistry book, to include your own definition
*****to
> : resist a drop in
> : > pH due to the addition of acid***, which is the same as the others I
> : posted .Agreed, of
> : > course not.You know that Alk isn't defined as "by the addition of
acids or
> : bases "and is
> : > only the " addition of an acid", so why are you accepting the
definition
> : ?.You know that
> : > when you titrate it is an acid added and never a base. In one breath
it
> : says Alk is "Acid
> : > neutralizing " and then they say "by the addition of acids or bases
".You
> : can't have it
> : > both ways and YOU know that Agreed . If the word "base" was left out I
> : would not have much
> : > to say. Agreed
> : >
> : >
> : > "Alkalinity is a
> : > measurement of BUFFERING CAPACITY."
> : >
> : > No it is not a measurement of BUFFERING CAPACITY, it is a indication
of
> : BC. I have said
> : > this at least twice. If you know your BC you can calculate Alk and if
you
> : can do one you
> : > can do the other agreed. What I have tried to convey from the
beginning is
> : that Alk and BC
> : > are not the same thing. You in one of your other posts have said they
are
> : not the same
> : > thing and never said they were. Now you seem to be saying they are the
> : same thing
> : >
> : > "So, when we measure ALKALINITY (and we know the pH) we are in effect
> : > measuring BUFFERING CAPACITY.
> : >
> : > More or less YES in an "effect" but Alk tells you not much of anything
> : when a base is
> : > added Agreed. That is called Acidity, which I see you have avoided
again
> : as if there is
> : > no such thing. I also said that for us the only thing we need to be
> : concerned about is
> : > Alk, so BC would fit in, as we could care less about the ability to
> : neutralize a base or
> : > measure Acidity. So, if you knew your pH , Alk or Acy you would really
> : know what you BC is
> : > doing for you Agreed.
> : >
> : > On Bc, we have both left something from my first equation, so I
thought I
> : would post it
> : > again for you, as I like being honest .I'm surprised you didn't catch
it
> : :-)
> : >
> : > B = dCb / dpH = - dCa / dpH
> : >
> : > So;
> : >
> : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] + [H30+] +
CKa
> : [H3O+] / (Ka =
> : > H3O+])² )
> : >
> : > or
> : >
> : > B (Buffering Capacity) = - dCa / dpH = 2.303 ( Kw/[H30+] + [H30+] +
CKa
> : [H3O+] / (Ka =
> : > H3O+])² )
> : >
> : > There are number of was to mathematically express BC. Two of the most
> : common are the
> : > change in Alk with the pH at constant total carbonate, the other is
change
> : in Alk with pH
> : > constant CO2 pp. In some examples of Bc, Bc is the inverse slope of
the
> : Alk titration
> : > curve ( I'm sure yo
> : > u will love this) In the other over the pH range, while BC is going
> : through minimum, Bpp
> : > increases linearly. This difference is caused by the uptake of CO2 by
the
> : solution, which
> : > increases Ct as pH increases.To bad we can't or my server won't allow
me,
> : to post
> : > attachments. I have a nice BC cure of various species as a function of
> : pC/pH diagrams, set
> : > to a pKa. curve
> : >
> : >
> : > On another issue
> : >
> : > "In order to remove CO2 (g) you ideally would want to shift
> : > the equilibrium to the left by LOWERING the pH"
> : >
> : >
> : > You may want to try and re-explain this
> : >
> : > CO2(gas) <---->CO2 (in solution) <-----> H2CO3 (carbonic acid)
<------>
> : > HCO3-1 <-------> CO3-2
> : >
> : >
> : > As the reaction shifts to left the pH gets higher as CO2 leaves the
> : system.You don't have
> : > to lower the pH to remove CO2. Case in point plants. As they remove
CO2
> : the pH rises,
> : > continued removal of the Sigma CO2 ( CO2, H2CO3, HCO3,CO3) cause
further
> : rising until
> : > there is mostly only carbonate (CO3) left and a high pH. Another case,
at
> : a pH of 8.00 and
> : > Alk of 4 meq / l ( 1.4 mg / l CO2) you have much more CO2 than at 2
meq/
> : l (0.65mg / l).
> : > . Aeration of the water can drive off the CO, no lowering of the pH
> : required., the removal
> : > will cause the pH to rise .On the other hand, trying to remove CO2 @ 2
meq
> : / l won't get
> : > you much of anywhere in this case. Also, even a low pH doesn't mean
you
> : can drive of CO2.
> : > If the seawater pH was say 7.5, you would think not problem to drive
off
> : CO2. If the Alk
> : > was 0.25 there would be about .35 mg / l CO2 to blow off. At the alk
of
> : 4.00 meq / l the
> : > CO2 is 5 mg / l.Usually, when people have a lower pH, say 7.9 or so,
it is
> : do to CO2, so
> : > the pH has lowered, increasing the CO2, to allow one to blow it off
easier
> : and bring the
> : > pH back up.
> : >
> : > CO2 = [CA(Carbonate Alk) x aH ] / [pK1(1 + 2pK2 /aH)]
> : >
> : > I think we just got off on the wrong foot, hope things look better.
> : >
> : > I'll be gone for the weekend, leaving in an hour, so have a nice
weekend
> : :-)
> : >
> : >
> : >
> : >
> : > --
> : > Boomer
> : >
> : > Want to talk chemistry ? The Reef Chemistry Forum
> : > http://www.reefcentral.com/vbulletin/index.php
> : >
> : > Want to See More ?
> : > Please Join Our Growing Membership
> : > www.coralrealm.com
> : >
> : > If You See Me Running You Better Catch-Up
> : > "stoutman" <.@.> wrote in message
news:lcRWb.299984$na.451117@attbi_s04...
> : > : > Humm, since when does Alk have anything to do in regards to the
> : addition
> : > : of BASE.
> : > :
> : > : You tell me. Your the one that posted a link to a web page that had
> : this
> : > : definition of alkalinity. Looks like you put yourself in your own
hole
> : pal.
> : > :
> : > : Remember posting this link:
> : > :
> : > : http://www.waterontheweb.org/resources/glossary.html
> : > :
> : > : Here is the definition of alkalinity from the web page YOU cited. (I
> : > : recommend you read the web pages you are citing before you cite
them)
> : > : Alkalinity:
> : > : Acid neutralizing or buffering capacity of water; a measure of the
> : ability
> : > : of water to resist changes in pH caused by the addition of acids or
> : BASES.
> : > :
> : > :
> : > : > It sure is funny how all of the chemist that write water chemistry
> : > : textbooks never say Alk
> : > : > is the Buffering Capacity of a solution.
> : > :
> : > : Neither did I. I said (for the umpth teen time) Alkalinity is a
> : > : measurement of BUFFERING CAPACITY.
> : > :
> : > : When you measure alkalinity you know your BUFFERING CAPACITY (if you
> : know
> : > : your pH). Its a two for one.
> : > :
> : > : SEE MY OTHER POST FROM TODAY.
> : > :
> : > :
> : > :
> : > : "Boomer" > wrote in message
> : > : ...
> : > : >
> : > : > "I am not sure if you are just messing with me "
> : > : >
> : > : > Yes, messing with you, it is called trolling a troll, to see where
the
> : > : hell you would go
> : > : > and what you would say in regards to last posts. It is called
honesty,
> : of
> : > : which you have
> : > : > none off to say the least,that I can see.You always like to post
what
> : > : suits you and just
> : > : > avoid ref I give. So lets start where you are WRONG and have a
great
> : lack
> : > : of understanding
> : > : > of things, to include pointing out all your gross error which you
> : still
> : > : FAIL to
> : > : > acknowledge and which can be prove in many water chem. ref. .I
doubt
> : like
> : > : hell you are a
> : > : > chemist at all.You seem to want to con people into thinkin' you
are.
> : But
> : > : then again, I
> : > : > have seen chemists like you before, they are not familiar with
the,
> : but
> : > : they ASK to have
> : > : > it explained and ask for REF.YOU just shoot from the hip. WHAT
GETS
> : YOU IN
> : > : TROUBLE. You
> : > : > remind me of snoot-noise kid that come here and other NG's and
> : > : forums...that think they
> : > : > know, buy hey, maybe I'm wrong :-)
> : > : >
> : > : >
> : > : >
> : > : > 1). Acidity
> : > : >
> : > : > "***Benjamin,Water Chemistry (2002, pages 262-263).***
> : > : >
> : > : > ***Acidity A concept that is exactly analogous to alkalinity but
> : measures
> : > : the base
> : > : > neutralizing
> : > : > capacity (BNC) of a solution is Acidity. The quantitative
represents
> : the
> : > : concentration of
> : > : > OH- ions that must be added to titrate the solution to a pH near
> : 10.5***
> : > : >
> : > : > So that means that not only in Benjamin wrong but, so are Stumm &
> : Morgan,
> : > : Millero, Pilosn,
> : > : > Riley & Chester, Pankow, Snoeyink & Jenkins, just to name a few.
As I
> : > : said, you have your
> : > : > acidity and Acidy mixed up. Acidity as defined above is covered in
> : most
> : > : water chemistry
> : > : > books, written by chemists, who's field of expertise is water
> : chemistry.
> : > : You can even buy
> : > : > Acidity test kits from, HACH, LaMotte, etc..
> : > : >
> : > : > You mean you didn't read this or are you just avoiding it .The
same
> : > : definition can be
> : > : > found in almost any std water chemistry book.
> : > : >
> : > : > I have run into few chemists, that are NOT familiar with the
above.
> : Some
> : > : water reports
> : > : > require the above Acidity measuring. The issue with you is you do
not
> : > : understand WATER
> : > : > CHEMISTRY. Everything you have posted can be found a general
chemistry
> : > : book
> : > : >
> : > : >
> : > : >
> : > : >
> : > : > 2) Alk and BC
> : > : >
> : > : > From the link
> : > : >
> : > : > Alkalinity
> : > : > ***Acid neutralizing or buffering capacity of water; a measure of
the
> : > : ability of water to
> : > : > resist changes in pH caused by the addition of acids or bases ***
> : > : >
> : > : > This is a Buffering Capacity definition not Alk
> : > : >
> : > : > Humm, since when does Alk have anything to do in regards to the
> : addition
> : > : of BASE. As I
> : > : > pointed out in the first post the term is often miss used. Even in
> : YOUR
> : > : own posts you say
> : > : > it is based on a acid addition, no mention of **base or acid**
> : addition
> : > : by you. Are you
> : > : > getting confused or what. Or is more you are trying to confuse
> : everyone
> : > : you are right. The
> : > : > above is a definition for Buffer Capacity NOT Alk
> : > : >
> : > : > From Drew, Geochemistry of Natural Waters
> : > : >
> : > : > "alkalinity, which is formally defined as the equivalent sum of
bases
> : that
> : > : are titratable
> : > : > with strong acid(Stumm & Morgan, 1966; Aquatic Chemistry). If the
pH
> : of
> : > : the solution is
> : > : > progressively lowered by the addition of a strong acid (HCL), all
the
> : > : anions on the right
> : > : > will be converted to uncharged species (H2CO3,B(OH)3, H4SiO4,
> : H2S,organic
> : > : acids, H20)"
> : > : >
> : > : > This follows almost all description of Alk, that it is acid
> : neutralizing
> : > : reaction and has
> : > : > nothing to do with base neutralizing, which is Acidity (BNC) .I
> : defined
> : > : these before you
> : > : > had no comment
> : > : >
> : > : >
> : > : > Even the links that give the Buffering Capacity definition is
wrong,
> : as is
> : > : the UIPAC on
> : > : > Alkalinity. Alkalinity has nothing to do with the addition of
bases
> : only
> : > : acids. When you
> : > : > use the words "base and acid" it becomes BC
> : > : >
> : > : > Even YOU MUST disagree with these definitions, from YOUR own post
> : > : >
> : > : > Think of alkalinity as 'buffering capacity'. Or the ability of a
> : solution
> : > : > ***to resist a drop in pH due to the addition of acid***
> : > : >
> : > : > Where the flip is the base addition forget it ?
> : > : >
> : > : > From Butler; Carbon Dioxide Equilibrium and Their Applications
> : (professor
> : > : emeritus
> : > : > Harvard University) an expert on the subject.
> : > : >
> : > : > Buffering Index (Buffering Capacity, Buffer Intensity).
> : > : >
> : > : > ***This concept was first developed for mixtures of approximately
> : equal
> : > : proportions of
> : > : > conjugate acid and base (i.e., 0.05 M NaHCO3 and .050 M Na2CO3.
Such
> : > : buffer solutions
> : > : > strongly resist changes in pH when acids or bases are added and
are
> : useful
> : > : as pH
> : > : > standards. The Buffer Index tells how great the resistance to pH
> : changes
> : > : will be.**
> : > : >
> : > : > also from Butler
> : > : >
> : > : > Alkalinity = {HCO3-] + 2[CO3] +[OH] - [H+]
> : > : >
> : > : > Acidity = [Cl-] - Na+] = [H+] - HCO3 - 2[CO3] - [OH-]
> : > : >
> : > : > Acidity is in fact just the negative of Alkalinity ***
> : > : >
> : > : > http://www.lagoonsonline.com/acid.htm
> : > : >
> : > : >
> : > :
> :
http://www.astm.org/cgi-bin/SoftCart.exe/DATABASE.CART/REDLINE_PAGES/D1067.h
> : > : tm?E+mystore
> : > : >
> : > : > It sure is funny how all of the chemist that write water chemistry
> : > : textbooks never say Alk
> : > : > is the Buffering Capacity of a solution. They are always treated
and
> : > : defined separately.
> : > : >
> : > : > If you or others choose to treat Alk and BC as the same, well,
just
> : have
> : > : at it. As I said
> : > : > in first post I know what you mean.
> : > : >
> : > : > "No need to cite web pages that describe what I know and what I
wrote
> : > : > in this discussion"
> : > : >
> : > : > No you don't know, who are you trying to convince any way, me, the
> : guys
> : > : here and/or all
> : > : > the water chemists in this world. As I said before go get a dam
WATER
> : > : CHEMISTRY book or
> : > : > shut the hell up.You keep trying to define things from a general
> : chemistry
> : > : book WE ARE IN
> : > : > THE WORLD OF WATER CHEMISTRY HERE. Get you definitions straight.
> : > : >
> : > : >
> : > : >
> : > : >
> : > : >
> : > : > 3). pKa's and what you don't know or seem to be confused on
> : > : >
> : > : > "Therefore, it has two pKa's
> : > : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH =
8.35.
> : > : The
> : > : > pH of seawater varies from 7.6 to 8.4. Hmmm. That pH I
calculated
> : is
> : > : > right in there. Is that magic? :)"
> : > : >
> : > : > Here it is agin that is twice at least
> : > : >
> : > : > "The pKa of CO3-2 is 10.3. Thus, at a pH of 8.3 (seawater for
this
> : > : example)
> : > : > you would have a 1 : 100 ratio of CO3-2 and HCO3-2. The
equilibrium
> : will
> : > : > be shifted to HCO3-2 by a ratio of 1:100.
> : > : >
> : > : > Oh wait , there is a third time LOL
> : > : >
> : > : > "At the pH of seawater, the buffering capacity of carbonate is at
it's
> : > : > weakest. It's strongest buffering is at a pH of 6.4 and 10.3."
> : > : >
> : > : >
> : > : > Lets just dunk you on this one. I am taking note you refuse to
reply
> : to
> : > : YOUR errors
> : > : >
> : > : > So you calculated the pH of seawater with freshwater pKa's, now
that
> : is a
> : > : good trick. From
> : > : > a number of seawater chemistry books the seawater pKa's are 6 &
9.1,
> : so
> : > : according to you,
> : > : > seemingly not understanding your favorite Henderson-Hasselbach
> : equation;
> : > : >
> : > : > 2 pH = (6 + 9.1) /2 pH = 7.55
> : > : >
> : > : > I have never seen seawater with a pH of 7.55. There is no ocean
with
> : that
> : > : pH. Humm how
> : > : > come your equation is not working for you today.?
> : > : >
> : > : >
> : > : > "That pH I calculated is
> : > : > right in there. Is that magic? :)"
> : > : >
> : > : > I roll on the floor when I see this = 8.35
> : > : >
> : > : > Hum , just a brain far so excuse me for thinkin
> : > : >
> : > : > (pKa1 and pKa2). pH = (pKa1 + pKa2)/2 pH = (6.4 + 10.3)/2 pH =
8.35
> : > : >
> : > : > Ok, we know those are FW pKa's. So, hummmmmm how come FW isn't at
a
> : pH of
> : > : 8.35 there pal
> : > : > ? That 8.35 is what you are telling people the pH should be, but
their
> : > : meter says 6.4.
> : > : > This how people will READ this.
> : > : >
> : > : >
> : > : >
> : > : >
> : > : > 4.) More on Buffering Capacity
> : > : >
> : > : > "Do you recognize [HCO3-1] and [CO3-2] from another equation ?
Yes,
> : your
> : > : > alkalinity equation."'
> : > : >
> : > : >
> : > : > Yup, I see that and in this case the HCO3 is the acid and the CO3
is
> : the
> : > : base CORRECT. In
> : > : > Alk you are only dealing with bases and how they react to an acid.
> : Acidity
> : > : deals acids and
> : > : > how they recact to bases "Acidity, A concept that is exactly
analogous
> : to
> : > : alkalinity but
> : > : > measures the base neutralizing
> : > : > capacity (BNC) of a solution is Acidity "Alk is the ANC Acid
> : neutralizing
> : > : capacity
> : > : >
> : > : > "Don't the components of a buffer account for the buffering
capacity?
> : "
> : > : >
> : > : > Yes, they do but so do the acids which work as buffers. NaHCO3 is
a
> : buffer
> : > : and can act as
> : > : > an acid or base
> : > : >
> : > : > *** Buffering Capacity.**
> : > : > The power of a substance in solution to absorb acid or alkali
without
> : > : change in pH; this
> : > : > is highest at a pH value equal to the pKa value of the acid of the
> : buffer
> : > : pair.***
> : > : >
> : > : > ***Akalinity***
> : > : > Measure of the power of a solution to neutralise hydrogen ions
(H+),
> : > : usually expressed as
> : > : > the equivalent concentration (mg/L) of calcium carbonate (CaCO3).
> : > : >
> : > : >
> : > : > If one wants to call Alk Buffering capacity then one sure as a
hell
> : can
> : > : call Acidty
> : > : > Buffering Capacity also. As it is the ability to neutralizes an
acid
> : that
> : > : is a buffer.You
> : > : > have a pH of 7 and you add a buffer to lower it to a pH of 4, you
are
> : > : buffering the water,
> : > : > that buffer is a acid.
> : > : >
> : > : > 5) CO2
> : > : >
> : > : > You are really confuse so it seems :-) You realllllllly indicate
that
> : CO2
> : > : is affected by
> : > : > the Alk or vise-versa
> : > : >
> : > : > "Yes, the pH will drop with the addition of CO2. Remove CO2 will
> : cause
> : > : the
> : > : > pH to rise? How do you remove CO2? Once it is in solution it
forms
> : > : > carbonic acid and neutralizes some of your 'buffer'."
> : > : >
> : > : > "With the exception of CO2?"
> : > : >
> : > : > No it doesn't, CO2 has ZERO effect on Alk (Pankow, Aquatic
Chemistry
> : > : > Concepts)....PERIOD.You seem to think a that at least in two of
your
> : post
> : > : that CO2 is
> : > : > affected by the Alk or vise-versa. Please go back to school or
seek
> : > : professor
> : > : >
> : > : > "Why in one case does CO2 from air lower pH and in the other case
it
> : > : raises
> : > : > it? Doesn't make sense."
> : > : >
> : > : > That is because you don't understand CO2 period. By the way I
saved
> : this,
> : > : wanted to see
> : > : > if you would bite on the post I gave. Not bite at first, so time
to
> : reel
> : > : you in, as you
> : > : > did bite in another post..
> : > : >
> : > : > Lets make some sense of it for you, being that you have a pH.D in
> : > : chemistry, so you say .
> : > : >
> : > : > CO2 is naturally generated in a aquatic systems, it is capable of
> : raise to
> : > : various levels
> : > : > depending on a number of circumstances .It can be measure (except
in
> : > : seawater) or
> : > : > calculated using Buch/Park Equations (what we use for seawater. In
> : sort if
> : > : you know the pH
> : > : > and Alk you can calculate the CO2). If you aerate a system or a
sample
> : of
> : > : water, even if
> : > : > the pH has only dropped a couple of tenths, due to an increase in
CO2,
> : the
> : > : CO2 will leave
> : > : > solution to the atmosphere.This will raise the pH. On the other
hand
> : if
> : > : theCO2 level is
> : > : > more of the norm and you have hikgh room air, such as in the
winter,
> : the
> : > : partial pressure
> : > : > of the CO2 in air will be much higher than that in water, in which
> : case
> : > : the CO2 will enter
> : > : > the water and lower the pH. That is without an airstone. Adding an
> : > : airstone will make it
> : > : > even worse,as you are now forcefully driving the CO2 into solution
> : even
> : > : quicker. These
> : > : > test /experiments have been proven many times, it is not that may
work
> : > : could work they do
> : > : > work.Yet you want to disagree and in another post say you haven't
> : tried
> : > : it,.Seems to me
> : > : > that based on what you say it can't work So, in short you don't
know
> : what
> : > : the hell you are
> : > : > taking about. Go get a glass of seawater with a pH of about 8.3
and
> : lower
> : > : it to about
> : > : > 8.0.-81 with CO2, then aerated it and watch the pH go the
HELL-BACK-
> : UP
> : > : ( that is if you
> : > : > don't have a high room air CO2 problem.). This little test has
been
> : done
> : > : thousands of
> : > : > times in this hobby, with test kits, pH meters and even graphic
> : printers.
> : > : >
> : > : > "This is where Boomer and I
> : > : > disagree. I say you would have to lower the pH very low in order
to
> : > : > effectively remove CO2 by purging."
> : > : >
> : > : > You are 100 % wrong. Please come to our Chem forum and try and run
> : that by
> : > : Randy, don't
> : > : > take my word on it. I already know what he will say.
> : > : >
> : > : > "Boomer didnt convince me it
> : > : > works at the pH of an aquarium, but I never tried it and I'm not
sure
> : of
> : > : > this. "
> : > : >
> : > : > Well then come too our chem. forum and tell Randy he doesn't know
what
> : he
> : > : is talking about
> : > : > LOL. It is a realllllllllly easy test, having a Ph.D in chemistry,
it
> : > : should be easy for
> : > : > you to run the experiment LOL There are grade school kids that run
the
> : > : test and know what
> : > : > happens and that I'm correct.
> : > : >
> : > : >
> : > : > "The equilibrium is a FUNCTION
> : > : > of pH."
> : > : >
> : > : > It is also a function of Alk or don't you know that. At a pH of
8.3,
> : Alk
> : > : 2.25, the CO2 is
> : > : > about .45 meq / l, in seawater, @25C and 35 ppt. If you raise the
Alk
> : to
> : > : about .4 meq/ l
> : > : > or so the CO2 will be around .99 mg / l CO2, When dealing with
> : tanksCO2 is
> : > : not always in
> : > : > equilibrium with ambient air.
> : > : >
> : > : >
> : > : > ". But I wouldn't degas a solution of a
> : > : > specific gas (CO2) with a gas (this case he was using air) that
> : contains
> : > : the
> : > : > same gas I am trying to purge."
> : > : >
> : > : > Why not ? We have a guy right now that is running tests on purging
> : ambient
> : > : air with a
> : > : > solution to remove CO2 gas from the air, before it enters the tank
> : > : per/Randy's suggestion.
> : > : > The same guy is doing some of my test using a Clinoptilolite, a
> : Zeolite
> : > : mineral, that has
> : > : > an affinity for CO2.This will be a dry CO2 scrubber
> : > : >
> : > : >
> : > : > Sorry Soutman but you sure as hell don't seem to know much about
> : aquatic
> : > : chemistry. You
> : > : > seem to be guessing at everything.
> : > : >
> : > : > By the way have you read any of Randy's technical articles on
water
> : > : chemistry, been saving
> : > : > these for last. There are a few on pH, Alk, CO2 .Here is a list
> : > : >
> : > : > Try and answer them 1-5 and lets see where we get THIS TIME :-) or
> : maybe
> : > : we should just
> : > : > drop it. I could care less at this point.
> : > : >
> : > : > THE END
> : > : >
> : > : >
> : > : > ARTICLES
> : > : >
> : > : > The first two posts in this thread are lists of some of my
articles
> : that
> : > : relate to reef
> : > : > tank chemistry. In the next few posts are some of the articles
> : published
> : > : by Craig Bingman
> : > : > and others on reef chemistry issues.
> : > : >
> : > : > The first two posts in this thread are lists of some of my
articles
> : that
> : > : relate to reef
> : > : > tank chemistry. In the next few posts are some of the articles
> : published
> : > : by Craig Bingman
> : > : > and others on reef chemistry issues.
> : > : >
> : > : > Solving Common Problems
> : > : >
> : > : > Solving Calcium and Alkalinity Problems
> : > : > http://www.advancedaquarist.com/issues/nov2002/chem.htm
> : > : >
> : > : > Solutions to pH Problems
> : > : > http://www.advancedaquarist.com/iss...ne2002/chem.htm
> : > : >
> : > : > How to Select a Calcium and Alkalinity Supplementation Scheme
> : > : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
> : > : >
> : > : > Phosphate Issues
> : > : > http://www.advancedaquarist.com/iss...pt2002/chem.htm
> : > : >
> : > : > Nitrate Issues
> : > : > http://www.advancedaquarist.com/iss...st2003/chem.htm
> : > : >
> : > : >
> : > : >
> : > : > Calcium and Alkalinity
> : > : >
> : > : > Solving Calcium and Alkalinity Problems
> : > : > http://www.advancedaquarist.com/issues/nov2002/chem.htm
> : > : >
> : > : > How to Select a Calcium and Alkalinity Supplementation Scheme
> : > : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
> : > : >
> : > : > Calcium and Alkalinity Balance Issues
> : > : > http://reefkeeping.com/issues/2002-...ature/index.htm
> : > : >
> : > : > Calcium Carbonate as a Supplement (Aragamight; Liquid Reactor)
> : > : > http://www.advancedaquarist.com/iss...ly2002/chem.htm
> : > : >
> : > : > The Relationship Between Alkalinity and pH.
> : > : > http://www.advancedaquarist.com/issues/may2002/chem.htm
> : > : >
> : > : > The Chemical & Biochemical Mechanisms of Calcification in Corals
> : > : > http://www.advancedaquarist.com/issues/apr2002/chem.htm
> : > : >
> : > : > Calcium
> : > : > http://www.advancedaquarist.com/issues/mar2002/chem.htm
> : > : >
> : > : > Alkalinity
> : > : > http://www.advancedaquarist.com/iss...2/chemistry.htm
> : > : >
> : > : >
> : > : > Iron
> : > : >
> : > : > First Iron Article: Macroalgae and Dosing Recommendations
> : > : > http://www.advancedaquarist.com/issues/aug2002/chem.htm
> : > : >
> : > : > Second Iron Article: Iron: A Look at Organisms Other than
Macroalgae
> : > : > http://www.advancedaquarist.com/issues/oct2002/chem.htm
> : > : >
> : > : > Iodine
> : > : >
> : > : > Iodine in Marine Aquaria: Part I
> : > : > http://www.advancedaquarist.com/issues/mar2003/chem.htm
> : > : >
> : > : > Iodine in Reef Tanks 2: Effects on Macroalgae Growth
> : > : > http://www.advancedaquarist.com/iss...il2003/chem.htm
> : > : >
> : > : >
> : > : > Magnesium and Strontium
> : > : >
> : > : > Strontium
> : > : > http://www.advancedaquarist.com/issues/nov2003/chem.htm
> : > : >
> : > : > Magnesium
> : > : > http://www.advancedaquarist.com/issues/oct2003/chem.htm
> : > : >
> : > : > Magnesium and Strontium in Limewater
> : > : > http://www.advancedaquarist.com/issues/dec2003/chem.htm
> : > : >
> : > : >
> : > : > Limewater (kalkwasser)
> : > : >
> : > : > The Self Purification of Limewater (Kalkwasser)
> : > : > http://www.advancedaquarist.com/issues/may2003/chem.htm
> : > : >
> : > : > The Degradation of Limewater (Kalkwasser) in Air
> : > : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : > : >
> : > : > How to Select a Calcium and Alkalinity Supplementation Scheme
> : > : > http://www.advancedaquarist.com/issues/feb2003/chem.htm
> : > : >
> : > : > Metals in Aquaria
> : > : >
> : > : > Aluminum and aluminum-based phosphate binders
> : > : > http://www.advancedaquarist.com/iss...ly2003/chem.htm
> : > : >
> : > : > Reef Aquaria with Low Soluble Metals
> : > : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : > : >
> : > : > Tap Water in Reef Aquaria
> : > : > http://www.advancedaquarist.com/issues/jan2004/chem.htm
> : > : > First Iron Article: Macroalgae and Dosing Recommendations
> : > : > http://www.advancedaquarist.com/issues/aug2002/chem.htm
> : > : >
> : > : > Second Iron Article: Iron: A Look at Organisms Other than
Macroalgae
> : > : > http://www.advancedaquarist.com/issues/oct2002/chem.htm
> : > : >
> : > : >
> : > : > Test Kit Reviews
> : > : >
> : > : > The Seachem Borate Alkalinity Test Kit
> : > : > http://www.advancedaquarist.com/iss...ne2003/chem.htm
> : > : >
> : > : > The Salifert Boron Test Kit
> : > : > http://www.advancedaquarist.com/iss...pt2003/chem.htm
> : > : >
> : > : > Boron and Borate (and pH buffering)
> : > : >
> : > : > Boron in a Reef Tank (and its effect on pH buffering)
> : > : > http://www.advancedaquarist.com/issues/dec2002/chem.htm
> : > : >
> : > : > The Seachem Borate Alkalinity Test Kit
> : > : > http://www.advancedaquarist.com/iss...ne2003/chem.htm
> : > : >
> : > : > The Salifert Boron Test Kit
> : > : > http://www.advancedaquarist.com/iss...pt2003/chem.htm
> : > : >
> : > : >
> : > : >
> : > : > Others
> : > : >
> : > : > Tap Water in Reef Aquaria
> : > : > http://www.advancedaquarist.com/issues/jan2004/chem.htm
> : > : >
> : > : > ORP
> : > : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : > : >
> : > : > Chloramine
> : > : > http://reefkeeping.com/issues/2003-...ature/index.htm
> : > : >
> : > : > Silica in a Reef Tank
> : > : > http://advancedaquarist.com/issues/jan2003/feature.htm
> : > : >
> : > : > Specific Gravity (and temperature correction of hydrometers)
> : > : > http://www.advancedaquarist.com/iss...2/chemistry.htm
> : > : >
> : > : >
> : > : > The Complete Nitrogen Cycle
> : > : > http://www.animalnetwork.com/fish/l...a&RecordNo=3090
> : > : >
> : > : > Magnesium (older article with fonts screwed up)
> : > : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : > : >
> : > : > Phosphate (older article now reproduced in a poor fashion)
> : > : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : > : >
> : > : > Carbon Dioxide
> : > : > http://www.animalnetwork.com/fish/l...a&RecordNo=2074
> : > : >
> : > : > Using Conductivity to Measure Salinity
> : > : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : > : >
> : > : > Understanding Seawater
> : > : > http://www.animalnetwork.com/fish2/...s/1/default.asp
> : > : >
> : > : > Protein Skimming: How It Works
> : > : > http://home.mweb.co.za/jv/jv79/reef/skimmers2.html
> : > : >
> : > : >
> : > : >
> : > : > Articles by Craig Bingman:
> : > : >
> : > : > Carbon Dioxide tests
> : > : > http://www.animalnetwork.com/fish/l...n=&RecordNo=279
> : > : >
> : > : > Limewater, Acetic Acid and Sand Clumping
> : > : > http://www.animalnetwork.com/fish/l...n=&RecordNo=181
> : > : >
> : > : > Calcium and Alkalinity
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > Calculation of Calcium Carbonate Saturation States in Reef Aquaria
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : >
> : > : > Calcification Rates in Several Tropical Coral Reef Aquaria
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > Limits To Limewater...Revisited
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > Expanding the Limits of Limewater: Adding Organic Carbon Sources
> : (vinegar)
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : >
> : > : > Magnesium Ion Precipitation in Reef Aquaria: A Tempest in a Teapot
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > Magnesium - Part I
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > Magnesium - Part II
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > A Homemade Magnesium Supplement
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > Simulating the Effect of Calcium Chloride and Sodium Bicarbonate
> : Additions
> : > : on Reef Systems
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > Additional Simulations: The Combined Effect Of Calcium Chloride
> : > : > /Sodium Bicarbonate Additions And Water Exchanges
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : >
> : > : > More articles by Craig Bingman:
> : > : >
> : > : > The Halogens - Part I: Bromine in Seawater and Aquaria
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > The Halogens - Part II: Fluoride
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > Fluoride Depletion In Four Reef Aquariums
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > The Halogens - Part III: Iodine
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > Measuring Halides
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > How Test Kits Work
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > Borax pH Calibration
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > A pH Detective Story
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > How to Mix a Batch of Synthetic Seawater in Under Five Minutes
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > Increasing Atmospheric Carbon Dioxide: Likely Effects on Coral
Reefs
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : > SILICON - FOE OR FRIEND?
> : > : > http://www.animalnetwork.com/fish2/...s/1/default.asp
> : > : >
> : > : > The Composition Of Several Synthetic Seawater Mixes
> : > : > http://www.animalnetwork.com/fish2/...s/1/default.asp
> : > : >
> : > : > Calcium Carbonate for CaCO3/CO2 Reactors: More Than Meets the Eye
> : > : > http://www.animalnetwork.com/fish2/...bio/default.asp
> : > : >
> : > : >
> : > : >
> : > : > Andy's calcium calculator
> : > : > http://www.andy-hipkiss.co.uk/cacalc.htm
> : > : >
> : > : > Greg Hillers analysis of limestone media for CaCO3/CO2 reactors
> : > : > http://www.aquariumfish.com/aquariu...cid=124&search=
> : > : >
> : > : > Calcium Reactor Substrate -- Phosphate Levels
> : > : > by Greg Hiller
> : > : > http://www.advancedaquarist.com/iss...l2003/short.htm
> : > : >
> : > : >
> : > : > Indoor CO2 Problems
> : > : > http://www.advancedaquarist.com/iss...r2002/short.htm
> : > : >
> : > : > Simon Huntington's CaCO3/CO2 reactor article
> : > : >
> : > : > http://reefkeeping.com/issues/2002-...ature/index.htm
> : > : >
> : > : > Ron Shimek's Tank Water Analysis Article
> : > : > http://reefkeeping.com/issues/2002-...ature/index.htm
> : > : >
> : > : >
> : > : >
> : > : >
> : > : > Home made salinity standards thread:
> : > : >
> : > : > http://reefcentral.com/forums/showt...?threadid=65509
> : > : >
> : > : > Reef Chemicals Calculator
> : > : > http://www.kademani.com/reefchem.htm
> : > : >
> : > : >
> : > : >
> : > : > Boomer
> : > : >
> : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : >
> : > : >
> : > : > Former US Army Bomb Technician (EOD)
> : > : > Member; IABTI, NATEODA, WEODF, ISEE & IPS
> : > : >
> : > : > If You See Me Running You Better Catch-Up
> : > : >
> : > : >
> : > : > --
> : > : > Boomer
> : > : >
> : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : >
> : > : > Want to See More ?
> : > : > Please Join Our Growing Membership
> : > : > www.coralrealm.com
> : > : >
> : > : > If You See Me Running You Better Catch-Up
> : > : > "stoutman" <.@.> wrote in message
> : > : news:aGuWb.148227$U%5.676753@attbi_s03...
> : > : > : Boomer,
> : > : > :
> : > : > : I am not sure if you are just messing with me or if you are
truly
> : > : confused.
> : > : > : I hope the latter. Please read from Top to Bottom.
> : > : > :
> : > : > :
> : > : > : From YOUR first link:
> : > : > :
> : > : > : http://www.waterontheweb.org/resources/glossary.html
> : > : > :
> : > : > : Acidity:
> : > : > : A measure of how acid a solution may be. A solution with a pH of
> : less
> : > : than
> : > : > : 7.0 is considered acidic. Solutions with a pH of less than 4.5
> : contain
> : > : > : mineral acidity (due to strong inorganic acids), while a
solution
> : having
> : > : a
> : > : > : pH greater than 8.3 contains no acidity.
> : > : > :
> : > : > : Yes,
> : > : > :
> : > : > : Good definition (for the most part). pH <7 is indeed acidic.
pH >
> : 7 is
> : > : > : basic. Your web page had a definition for acidity, but not
> : basicity.
> : > : > : Strange. That's like defining GOOD and not defining BAD.
> : > : > :
> : > : > : Here is the IUPAC (International Union of Pure and Applied
> : Chemistry)
> : > : > : definition of acidity:
> : > : > :
> : > : > : http://www.chem.qmul.ac.uk/iupac/index.html
> : > : > :
> : > : > : acidity
> : > : > :
> : > : > : (1) Of a compound:
> : > : > :
> : > : > : For Brønsted acids it means the tendency of a compound to act as
a
> : > : hydron
> : > : > : donor. It can be quantitatively expressed by the acid
dissociation
> : > : constant
> : > : > : of the compound in water or some other specified medium. For
Lewis
> : acids
> : > : it
> : > : > : relates to the association constants of Lewis adducts
and -adducts.
> : > : > :
> : > : > : (2) Of a medium:
> : > : > :
> : > : > : The use of the term is mainly restricted to a medium containing
> : Brønsted
> : > : > : acids, where it means the tendency of the medium to hydronate a
> : specific
> : > : > : reference base
> : > : > :
> : > : > : basicity
> : > : > :
> : > : > : For Brønsted bases it means the tendency of a compound to act as
> : hydron
> : > : > : (proton) acceptor. The basicity of a chemical species is
normally
> : > : expressed
> : > : > : by the acidity of the conjugate acid (see conjugate acid-base
pair).
> : For
> : > : > : Lewis bases it relates to the association constants of Lewis
adducts
> : > : > : and -adducts
> : > : > :
> : > : > :
> : > : > :
> : > : > : Another definition from the same web page YOU cited: (this is
the
> : same
> : > : web
> : > : > : page you cited above)
> : > : > :
> : > : > : Alkalinity:
> : > : > : Acid neutralizing or buffering capacity of water; a measure of
the
> : > : ability
> : > : > : of water to resist changes in pH caused by the addition of acids
or
> : > : bases
> : > : > : and therefore, the main indicator of susceptibility to acid
rain; in
> : > : natural
> : > : > : waters it is due primarily to the presence of bicarbonates,
> : carbonates
> : > : and
> : > : > : to a much lesser extent occasionally borates, silicates and
> : phosphates.
> : > : It
> : > : > : is expressed in units of milligrams per liter (mg/l) of CaCO3
> : (calcium
> : > : > : carbonate) or as microequivalents per liter (ueq/l) where 20
ueq/l =
> : 1
> : > : mg/l
> : > : > : of CaCO3. A solution having a pH below about 5 contains no
> : alkalinity.
> : > : > :
> : > : > : Your own post defines alkalinity as BUFFERING CAPACITY OF WATER
and
> : says
> : > : > : that alkalinity is the measure of ...(description of a buffer)
> : > : > :
> : > : > : A BUFFER IS : a measure of the ability of water to resist
changes in
> : pH
> : > : > : caused by the addition of acids or bases (from definition below)
> : > : > :
> : > : > :
> : > : > : I said:
> : > : > : ***alkalinity is a measurement of 'buffering capacity'***
> : > : > :
> : > : > : You said:
> : > : > : ***Alkalinity is not a measurement of BC
> : > : > :
> : > : > : WHY WOULD YOU POST A LINK THAT CONTRADICTS WHAT YOU SAID?? This
is
> : not
> : > : > : logical.
> : > : > :
> : > : > : (THIS FROM THE SAME WEB PAGE YOU CITED):
> : > : > :
> : > : > : Buffer:
> : > : > : A substance which tends to keep pH levels fairly constant when
acids
> : or
> : > : > : bases are added.
> : > : > :
> : > : > : THIS IS FROM THE DEFINITION OF ALKALINITY FROM SAME WEB PAGE.
> : > : > :
> : > : > : a measure of the ability of water to resist changes in pH caused
by
> : the
> : > : > : addition of acids or bases
> : > : > :
> : > : > : SO DON'T TELL ME THIS SENTENCE DOESN'T DESCRIBE THE ACTIONS OF A
> : BUFFER.
> : > : > :
> : > : > :
> : > : > : I went to all four links. None contradict what I have said.
But
> : the
> : > : first
> : > : > : one you cited contradicts YOU!
> : > : > :
> : > : > : I know what a buffer is. I know what acidity means. I know
what
> : > : alkalinity
> : > : > : means. No need to cite web pages that describe what I know and
what
> : I
> : > : wrote
> : > : > : in this discussion. Show me one that says alkalinity is not a
> : measure
> : > : of
> : > : > : buffering capacity from a credible source.
> : > : > :
> : > : > :
> : > : > :
> : > : > :
> : > : > :
> : > : > :
> : > : > : "Boomer" > wrote in message
> : > : > : ...
> : > : > : > Alkalinity a measure of the amount of anions of weak acid in
water
> : and
> : > : of
> : > : > : the cations
> : > : > : > balanced against them
> : > : > : > Take note it says ***acid***
> : > : > : >
> : > : > : > Buffering capacity the ability of a solution to resist or
dampen
> : > : changes
> : > : > : in pH upon the
> : > : > : > addition of acids or bases.
> : > : > : > Take note its says ***the addition of acids or bases***
> : > : > : >
> : > : > : > One more
> : > : > : >
> : > : > : > http://www.waterontheweb.org/resources/glossary.html
> : > : > : >
> : > : > : > We could go on like this all day, so what is the point ?
> : > : > : >
> : > : > : > You will LOVE this one
> : > : > : > http://www.kyantec.com/Tips/phbuffering.htm
> : > : > : >
> : > : > : > Don't you just lovbe PDF's
> : > : > : > http://www.inform.umd.edu/manurenet/reprints/98.1702.pdf
> : > : > : >
> : > : > : > Don't fall out of your chair
> : > : > : >
> : http://www.chemforlife.org/teacher/topics/chemistry_in_an_aquarium.htm
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : >
> : > : > : > --
> : > : > : > Boomer
> : > : > : >
> : > : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : > : >
> : > : > : > Want to See More ?
> : > : > : > Please Join Our Growing Membership
> : > : > : > www.coralrealm.com
> : > : > : >
> : > : > : > If You See Me Running You Better Catch-Up
> : > : > : > "stoutman" <.@.> wrote in message
> : > : news:XB7Wb.19339$QA2.62332@attbi_s52...
> : > : > : > : Man here is another, google is a wonderful thing. I'm not
> : filtering
> : > : any
> : > : > : > : out, just posting what I find by GOOGLING for you.
> : > : > : > :
> : > : > : > :
> : http://www.globe.gov/hq/trr_suppl/hydro/HY_SUP_ALK_INTRO_NOTES.HTML
> : > : > : > :
> : > : > : > :
> : > : > : > : Wow, a gov link. Even the government is wrong, this must be
a
> : > : > : conspiracy
> : > : > : > : against Boomer.
> : > : > : > :
> : > : > : > :
> : > : > : > :
> : > : > : > :
> : > : > : > : "Boomer" > wrote in message
> : > : > : > : ...
> : > : > : > : > Now I am getting bored
> : > : > : > : >
> : > : > : > : > "Don't the components of a buffer account for the
buffering
> : > : capacity?
> : > : > : > : Yes."
> : > : > : > : >
> : > : > : > : > Yes, agreed but you seem to fail what I'm saying.
Buffering
> : > : Capacity
> : > : > : and
> : > : > : > : Alkalinity are
> : > : > : > : > not the same, that has always been the issue. I gave the
> : equation
> : > : does
> : > : > : > : that look like an
> : > : > : > : > Alkalinity equation or how Alk is determined. I see you
had
> : now
> : > : > : comments
> : > : > : > : on it what's
> : > : > : > : > wrong, why no comments on the equations I gave. Don't
> : understand
> : > : them
> : > : > : or
> : > : > : > : what ? Again this
> : > : > : > : > is the equation for Buffering Capacity, also called Buffer
> : Index
> : > : or
> : > : > : Buffer
> : > : > : > : Intensity. It
> : > : > : > : > is defined in most water chemistry and chemical
oceanography
> : text
> : > : > : books.
> : > : > : > : >
> : > : > : > : > B (Buffering Capacity) = dCb / dpH = 2.303 ( Kw/[H30+] +
> : [H30+] +
> : > : > : CKa
> : > : > : > : [H3O+] / (Ka =
> : > : > : > : > H3O+])² )
> : > : > : > : >
> : > : > : > : > This is not Alkalinity now is it ?
> : > : > : > : >
> : > : > : > : > "I know how to do a titration, In fact I have done
several.
> : How
> : > : many
> : > : > : have
> : > : > : > : > you actually done? I don't mean by counting drops, I mean
> : with a
> : > : > : buret?"
> : > : > : > : >
> : > : > : > : > Well good for you, I use a Digital Titrator
> : > : > : > : >
> : > : > : > : > "Oh, I see,
> : > : > : > : > you think acidity is the opposite of alkalinity. In the
world
> : of
> : > : > : > : CHEMISTRY
> : > : > : > : > it's not. Maybe in aquarium newsgroups it is.
> : > : > : > : >
> : > : > : > : > Hum no, maybe you should go for a look at HACH's or
LaMotte
> : > : website or
> : > : > : the
> : > : > : > : book I
> : > : > : > : > suggested earlier. Please view a copy.
> : > : > : > : >
> : > : > : > : > Standard Methods for the Examination of Water and
Wastewater
> : > : > : > : >
> : > : > : > : > This book, over 2000 pages, is the guide for water
testing. If
> : you
> : > : are
> : > : > : > : reporting water
> : > : > : > : > test to the EPA you must use approved std from this text.I
t
> : is
> : > : > : prepared
> : > : > : > : and published by
> : > : > : > : > the EPA, American Water Works Association and American
Public
> : > : Health
> : > : > : > : Association. You
> : > : > : > : > mean you don't have one and the issue is water chemistry
> : > : > : > : >
> : > : > : > : > You are confusing Acidity and Acidity as you know little
about
> : > : water
> : > : > : > : chemistry and
> : > : > : > : > procedures and test methods
> : > : > : > : >
> : > : > : > : > From SMEWW, section 2-30, 2310 ACIDITY
> : > : > : > : >
> : > : > : > : > "Acidity of water is its quantative capacity to react with
a
> : > : strong
> : > : > : base
> : > : > : > : to a designated
> : > : > : > : > pH"
> : > : > : > : >
> : > : > : > : > This is how you test for it
> : > : > : > : >
> : > : > : > : > A std alkali titration to methyl orange or phenolphthalein
> : > : > : > : > endpoint.
> : > : > : > : >
> : > : > : > : > BUT YOU SAID THIS IS WRONG. Please tell all the chemist
that
> : > : write
> : > : > : this
> : > : > : > : book, there are
> : > : > : > : > over 100 of them, they are wrong.
> : > : > : > : >
> : > : > : > : > Like Buffering Capacity you have your Acidity's mixed up
> : > : > : > : > In water measurement if you have a high Alk you also
usually
> : have
> : > : a
> : > : > : high
> : > : > : > : Acidity.
> : > : > : > : > Normally a high Alk also gives a higher CO2 level. Get a
WATER
> : > : > : CHEMISTRY
> : > : > : > : BOOK there pal.
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > "These are all in equilibrium with each other. An initial
> : high pH
> : > : > : (above
> : > : > : > : > 6.4) will shift the equilibrium to the right to form
HCO3-1.
> : If
> : > : the
> : > : > : pH of
> : > : > : > : > the solution is above 10.3 (pKa2) the .........."
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > Christ, there you go again with the FW ****. All your
numbers
> : are
> : > : > : wrong we
> : > : > : > : are dealing
> : > : > : > : > with SEAWATER
> : > : > : > : >
> : > : > : > : > This means that at a pH of 8.3, the majority of the
CO2(aq) is
> : in
> : > : the
> : > : > : form
> : > : > : > : > of HCO3-1 .
> : > : > : > : >
> : > : > : > : > I have already pointed that out and gave actual values at
know
> : > : > : seawater
> : > : > : > : levels, go back
> : > : > : > : > and re-read it you aren't telling me anything here.Of
course
> : most
> : > : is
> : > : > : HCO3
> : > : > : > : see...
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > @ 20C and 34.3 ppt salinity
> : > : > : > : >
> : > : > : > : > CO2 = 0.52 %
> : > : > : > : >
> : > : > : > : > HCO3 = 86.4 %
> : > : > : > : >
> : > : > : > : > CO3 = 13.09 %
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > "In your glass experiment you managed to lower the pH
enough
> : to
> : > : purge
> : > : > : out
> : > : > : > : CO2
> : > : > : > : > by boiling"
> : > : > : > : >
> : > : > : > : > The purpose behind the glass is to show that alk is not
affect
> : by
> : > : CO2
> : > : > : and
> : > : > : > : vise-versa and
> : > : > : > : > how Co2 affects pH.
> : > : > : > : >
> : > : > : > : > Now, in a real life seawater aquarium, with a pH of 8.3
and
> : that
> : > : pH
> : > : > : drops
> : > : > : > : to say 8.1 it is
> : > : > : > : > usually due to excess CO2. If you took a glass of that
water
> : and
> : > : > : aerated
> : > : > : > : it you WILL drive
> : > : > : > : > off the CO2 and raise the pH. It has been done a proven a
> : million
> : > : > : times.
> : > : > : > : >
> : > : > : > : > "In order to 'purge' CO2 you would need to lower the
> : > : > : > : > pH to shift the equilibrium to below 6.4"
> : > : > : > : >
> : > : > : > : > The hell you do !!!.Do you know who many times people on
this
> : NG
> : > : to
> : > : > : > : include Dr. Craig
> : > : > : > : > Bingman a chemist and Dr. Randy Holmes-Farley have
mentioned
> : to
> : > : take a
> : > : > : > : sample of aquarium
> : > : > : > : > water and aerate it to see if the pH GOES UP AND when they
> : come
> : > : back
> : > : > : with
> : > : > : > : the test it is
> : > : > : > : > often YES the pH went back up. PROBLEM THERE MISTER PH.D
> : CHEMIST
> : > : > : excess
> : > : > : > : CO2 in the tank
> : > : > : > : > water, increase the circulation for better gas exchange at
the
> : > : > : surface,
> : > : > : > : reduce feeding,
> : > : > : > : > and try to improve on better skimming, thus reducing the
> : bio-load
> : > : and
> : > : > : pH
> : > : > : > : decline due to
> : > : > : > : > CO2.
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > "I hope this helps. "
> : > : > : > : >
> : > : > : > : > Help, how can you when you miss everything. I should be
> : charging
> : > : you
> : > : > : > : >
> : > : > : > : > Oh, by the way. Your websites, I have about 50 on these
> : issues, I
> : > : > : could
> : > : > : > : post them, not to
> : > : > : > : > mention I have all those water chemistry books, so there
is no
> : > : need to
> : > : > : > : view your sites.
> : > : > : > : >
> : > : > : > : > Finally are you afraid to come to our Chemistry Forum,
afraid
> : to
> : > : get
> : > : > : > : slapped by REAL
> : > : > : > : > chemists. I get a charge out of you can't post your ref .I
> : have
> : > : posted
> : > : > : the
> : > : > : > : same or similar
> : > : > : > : > stuff on his forum and I wasn't pointed out WRONG pal. I
have
> : 1500
> : > : > : posts
> : > : > : > : there and am the
> : > : > : > : > biggest contributor to his forum other than himself or
maybe
> : Habib
> : > : > : Sheka
> : > : > : > : >
> : > : > : > : > Hum, here are Randy's ref that he posted. He hosts the
website
> : > : > : > : >
> : > : > : > : > S. RANDY HOLMES-FARLEY
> : > : > : > : > Arlington, Massachusetts
> : > : > : > : >
> : > : > : > : > EDUCATION
> : > : > : > : >
> : > : > : > : > 1982-1986 Harvard University Cambridge, MA
> : > : > : > : > PhD in Chemistry
> : > : > : > : > Research Advisor: George Whitesides
> : > : > : > : >
> : > : > : > : > Investigated the relationship between polymer surface
> : chemistry
> : > : and
> : > : > : > : physical properties
> : > : > : > : > through controlled surface modification and testing.
> : > : > : > : >
> : > : > : > : > 1980-1982 Cornell University Ithaca, NY
> : > : > : > : > BA in Chemistry and Biology
> : > : > : > : > Graduated Summa Cum Laude
> : > : > : > : > Distinction in All Subjects
> : > : > : > : > Grade Point: 3.94/4.0
> : > : > : > : > Honors research: isolation and characterization of the
subunit
> : of
> : > : CF1
> : > : > : > : enzyme
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > 1978-1979 Stanford University Palo Alto, CA
> : > : > : > : > Grade Point: 3.55/4.0
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > EXPERIENCE
> : > : > : > : >
> : > : > : > : > 1992- present Genzyme Drug Disvcovery and Development
Waltham,
> : MA
> : > : > : > : > (bought out GelTex Pharmaceuticals in 2001)
> : > : > : > : > Vice President, Chemical Research 2001-present
> : > : > : > : > Senior Director, Chemical Research 1999-2001
> : > : > : > : > Director of Chemical Research 1997-1999
> : > : > : > : > Manager of Chemical Research 1995-1997
> : > : > : > : > Group Leader 1994-1995
> : > : > : > : > Senior Research Scientist 1992-1994
> : > : > : > : >
> : > : > : > : > Helped start GelTex as second employee
> : > : > : > : >
> : > : > : > : > Managed various research programs with multi-million
dollar
> : > : budgets
> : > : > : > : >
> : > : > : > : > Supervised research chemists (17+)
> : > : > : > : >
> : > : > : > : > Co-inventor of several polymeric pharmaceuticals and
> : > : pharmaceutical
> : > : > : > : candidates including
> : > : > : > : > Sevelamer Hydrochloride (FDA approved) and Colesevelam
> : > : Hydrochloride
> : > : > : (FDA
> : > : > : > : approved)
> : > : > : > : >
> : > : > : > : > Company Safety Officer for 3 years
> : > : > : > : >
> : > : > : > : > Chemical Hygiene Officer 2000-present
> : > : > : > : >
> : > : > : > : >
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > 1990-1992 GTE Corporation Waltham, MA
> : > : > : > : > Senior Member of Technical Staff
> : > : > : > : > Applied research involving polymer interfaces
> : > : > : > : > Metallization of plastics
> : > : > : > : > Polymer/polymer adhesion
> : > : > : > : > Optical coatings
> : > : > : > : >
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > 1986-1990 Lord Corporation Cary, NC
> : > : > : > : > Senior Research Scientist 1988-1990
> : > : > : > : > Research Scientist 1986-1988
> : > : > : > : > Basic and applied research on surface chemical bonding
> : > : > : > : > Developed new adhesive compositions
> : > : > : > : > Developed new sol-gel coatings for corrosion resistance
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > HONORS AND AWARDS
> : > : > : > : >
> : > : > : > : > Industrial Innovations Award by Northeast Region of
American
> : > : Chemical
> : > : > : > : Society (6/2001)
> : > : > : > : >
> : > : > : > : > National Kidney Foundation of Northern California Honoree
> : (5/2001)
> : > : > : > : >
> : > : > : > : > American Chemical Society/Polymer Chemistry Division
> : Industrial
> : > : > : Sponsors
> : > : > : > : > Award (8/2000)
> : > : > : > : >
> : > : > : > : > R&D 100 Award from R&D magazine (1999)
> : > : > : > : >
> : > : > : > : > Sherwin Williams Award in applied polymer science (9/85)
> : > : > : > : >
> : > : > : > : > IBM Predoctoral Fellowship in Polymer Science (1984-1985;
> : > : 1985-1986)
> : > : > : > : >
> : > : > : > : > Award for highest GPA in Chemistry Department (6/82)
> : > : > : > : >
> : > : > : > : > Summa Cum Laude Honors in Chemistry (6/82)
> : > : > : > : >
> : > : > : > : > Phi Lamda Epsilon (6/82)
> : > : > : > : >
> : > : > : > : > Phi Beta Kappa (2/82)
> : > : > : > : >
> : > : > : > : > Cornell University Dean's List (1981, 1982)
> : > : > : > : >
> : > : > : > : > Harvard Book Club Award for highest GPA senior year (1978)
> : > : > : > : >
> : > : > : > : > First Place in western NY ACS high school chemistry exam
> : (1977)
> : > : > : > : >
> : > : > : > : > 1978-1979
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > __________________
> : > : > : > : > Randy Holmes-Farley
> : > : > : > : > Want to talk chemistry? Try the Reef Chemistry Forum at
Reef
> : > : Central
> : > : > : > : >
> : > : > : > : > Hobby Experience: 8 years with reefs
> : > : > : > : > Current Tanks: 90 gal mixed reef
> : > : > : > : > Interests: Reefkeeping, science, photography
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > Last edited by Randy Holmes-Farley on 10/01/2003 at 07:49
PM
> : > : > : > : >
> : > : > : > : > Open this post in a new window | Report this post to a
> : moderator |
> : > : IP:
> : > : > : > : Logged
> : > : > : > : >
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > 06/27/2003 02:44 PM
> : > : > : > : >
> : > : > : > : > Randy Holmes-Farley
> : > : > : > : > Chemistry Moderator
> : > : > : > : >
> : > : > : > : > Registered: Apr 2001
> : > : > : > : > Location: Arlington, Massachusetts
> : > : > : > : > Occupation: Chemist (Drug Discovery at Genzyme)
> : > : > : > : > Posts: 15282
> : > : > : > : >
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > Publications
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > ISSUED UNITED STATES PATENTS
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > 1. Method for reducing oxalate. Holmes-Farley, Stephen
> : Randall;
> : > : > : > : Mandeville, III; W. Harry.
> : > : > : > : > US 6,566,407; 5/20/2003
> : > : > : > : >
> : > : > : > : > 2. Polyether-based bile acid sequestrants. Holmes-Farley,
> : Stephen
> : > : > : Randall;
> : > : > : > : Huval, Chad
> : > : > : > : > Cori.
> : > : > : > : > U.S. 6,517,825; 2/11/2003.
> : > : > : > : >
> : > : > : > : > 3. Method of making phosphate-binding polymers for oral
> : > : > : administration.
> : > : > : > : Holmes-Farley,
> : > : > : > : > Stephen R.; Mandeville, W. Harry, III; Whitesides; George
M.
> : U.S.
> : > : > : > : 6,509,013; 1/21/2003.
> : > : > : > : >
> : > : > : > : > 4. Combination therapy for treating hypercholesterolemia
using
> : a
> : > : bile
> : > : > : acid
> : > : > : > : sequestrant
> : > : > : > : > polymer
> : > : > : > : > and a cholesterol-lowering agent. Huval, Chad Cori;
> : Holmes-Farley,
> : > : > : Stephen
> : > : > : > : Randall;
> : > : > : > : > Petersen, John S.; Dhal, Pradeep K. U.S. 6,433,026;
8/13/2002.
> : > : > : > : >
> : > : > : > : > 5. Method for treating hypercholesterolemia with
> : polyallylamine
> : > : > : polymers.
> : > : > : > : Holmes-Farley,
> : > : > : > : > Stephen Randall; Mandeville, W. Harry, III; Burke, Steven
K.;
> : > : > : Goldberg,
> : > : > : > : Dennis I. , US
> : > : > : > : > 6,423,754; 7/23/2002.
> : > : > : > : >
> : > : > : > : > 6. Ionic polymers as anti-infective agents Mandeville, W.
> : Harry,
> : > : III;
> : > : > : > : Neenan, Thomas X..;
> : > : > : > : > Holmes-Farley, Stephen Randall;, US 6,395,777; 5/28/2002.
> : > : > : > : >
> : > : > : > : > 7. Combination therapy for treating hypercholesterolemia
and
> : > : > : > : atherosclerosis. Huval, Chad
> : > : > : > : > Cori; Holmes-Farley, Stephen Randall; Petersen, John S.;
Dhal,
> : > : Pradeep
> : > : > : K.
> : > : > : > : U.S. 6,365,186;
> : > : > : > : > 4/2/2002.
> : > : > : > : >
> : > : > : > : > 8. Fat binding polymers. Jozefiak, T.; Holmes-Farley; S.
R.;
> : > : > : Mandeville,
> : > : > : > : W. H., III;
> : > : > : > : > Huval; C.
> : > : > : > : > C.; Garigapati, V. R.; Shackett, K. K.; Concagh, D, US
> : 6,299,868;
> : > : > : > : 10/9/2001.
> : > : > : > : >
> : > : > : > : > 9. Polymers containing guanidinium groups as bile acid
> : > : sequestrants.
> : > : > : Dhal;
> : > : > : > : P. K.; Holmes-
> : > : > : > : > Farley; S. R.; Petersen; J. S. US 6,294,163; 9/25/2001
> : > : > : > : >
> : > : > : > : > 10. Method for reducing oxalate. Holmes-Farley, S. R.;
> : Mandeville,
> : > : W.
> : > : > : H.,
> : > : > : > : III.; US
> : > : > : > : > 6,281,252;
> : > : > : > : > 8/28/2001.
> : > : > : > : >
> : > : > : > : > 11. Combination therapy for treating hypercholestrolemia.
> : Huval;
> : > : C.
> : > : > : C.;
> : > : > : > : Holmes-Farley; S.
> : > : > : > : > R. ;
> : > : > : > : > Petersen; J. S.; Dhal; P. K. ; US 6,264,938; 7/24/2001.
> : > : > : > : >
> : > : > : > : > 12. Fat-binding polymers. Mandeville, W. H., III.;
Whitesides,
> : G.
> : > : M.;
> : > : > : > : Holmes-Farley, S.
> : > : > : > : > R.; US
> : > : > : > : > 6,264,937; 7/24/2001.
> : > : > : > : >
> : > : > : > : > 13. Method for treating hypercholesterolemia with
> : unsubstituted
> : > : > : > : polydiallylamine polymers.
> : > : > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.;
Dhal; P.
> : K.
> : > : ; US
> : > : > : > : 6,248,318;
> : > : > : > : > 6/19/2001.
> : > : > : > : >
> : > : > : > : > 14. Process for removing bile salts from a patient and
> : alkylated
> : > : > : > : compositions therefore.
> : > : > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US
6,225,355;
> : > : 5/1/2001.
> : > : > : > : >
> : > : > : > : > 15. Poly(diallylamine)-based bile acid sequestrants.
> : > : Holmes-Farley, S.
> : > : > : R.;
> : > : > : > : Dhal, P. K.;
> : > : > : > : > Petersen,
> : > : > : > : > J. S.; US 6,203,785; 3/20/2001.
> : > : > : > : >
> : > : > : > : > 16. Polyether-Based Bile Acid Sequestrants. Holmes-Farley,
S.
> : R.;
> : > : > : Huval,
> : > : > : > : C. C.; US
> : > : > : > : > 6,190,649;
> : > : > : > : > 2/20/2001.
> : > : > : > : >
> : > : > : > : > 17. Method for reducing oxalate. Holmes-Farley, S. R.;
> : Mandeville,
> : > : W.
> : > : > : H.,
> : > : > : > : III.; US
> : > : > : > : > 6,177,478;
> : > : > : > : > 1/23/2001.
> : > : > : > : >
> : > : > : > : > 18. Water-insoluble noncrosslinked bile acid sequestrants.
> : > : > : Holmes-Farley,
> : > : > : > : S. R.;
> : > : > : > : > Mandeville, W.
> : > : > : > : > H., III.; US 6,129,910; 10/10/2000.
> : > : > : > : >
> : > : > : > : > 19. Method for treating hypercholesterolemia with
> : unsubstituted
> : > : > : > : polydiallylamine polymers.
> : > : > : > : > Huval; C. C.; Holmes-Farley; S. R. ; Petersen; J. S.;
Dhal; P.
> : K.
> : > : ; US
> : > : > : > : 6,083,497;
> : > : > : > : > 7/4/2000.
> : > : > : > : >
> : > : > : > : > 20. Method of making phosphate-binding polymers for oral
> : > : > : administration.
> : > : > : > : Holmes-Farley, S.
> : > : > : > : > R.; Mandeville, W. H., III.; ; Whitesides, G. M. ; US
> : 6,083,495;
> : > : > : 7/4/2000.
> : > : > : > : >
> : > : > : > : > 21. Process for removing bile salts from a patient and
> : alkylated
> : > : > : > : compositions therefore.
> : > : > : > : > Mandeville, W. H., III.; Holmes-Farley, S. R.; US
6,066,678;
> : > : > : 5/23/2000.
> : > : > : > : >
> : > : > : > : > 22. Process for removing bile salts from a patient and
> : > : compositions
> : > : > : > : therefor. Mandeville,
> : > : > : > : > W. H.,
> : > : > : > : > III.; Holmes-Farley, S. R.; US 6,060,517; 5/9/2000.
> : > : > : > : >
> : > : > : > : > 23. Ionic polymers as anti-infective agents. Mandeville,
III;
> : W.
> : > : H;
> : > : > : > : Neenan; T. X.; Holmes-
> : > : > : > : > Farley; S. R. US 6,034,129; 3/7/2000.
> : > : > : > : >
> : > : > : > : > 24. Method for reducing oxalate. Holmes-Farley, S. R.;
> : Mandeville,
> : > : W.
> : > : > : H.,
> : > : > : > : III.; US
> : > : > : > : > 5,985,938;
> : > : > : > : > 11/16/99.
> : > : > : > : >
> : > : > : > : > 25. Process for removing bile salts from a patient and
> : > : compositions
> : > : > : > : therefor. Mandeville,
> : > : > : > : > W. H.,
> : > : > : > : > III.; Holmes-Farley, S. R.; US 5,981,693; 11/9/99.
> : > : > : > : >
> : > : > : > : > 26. Hydrophobic sequestrant for cholesterol depletion.
> : Mandeville,
> : > : W.
> : > : > : H.,
> : > : > : > : III.;
> : > : > : > : > Holmes-Farley;
> : > : > : > : > S. R.; Petersen; J. S.. US 5,969,090; 10/19/99.
> : > : > : > : >
> : > : > : > : > 27. Hydrophilic nonamine-containing and amine-containing
> : > : copolymers
> : > : > : and
> : > : > : > : their use as bile
> : > : > : > : > acid sequestrants. Holmes-Farley; S. R.; Petersen; J. S..
US
> : > : > : 5,929,184;
> : > : > : > : 7/27/99.
> : > : > : > : >
> : > : > : > : > 28. Interpenetrating polymer networks for sequestration of
> : bile
> : > : acids.
> : > : > : > : Mandeville, W. H.,
> : > : > : > : > III.;
> : > : > : > : > Holmes-Farley, S. R.; Neenan; T. X.; Whitesides; G. M. US
> : > : 5,925,379;
> : > : > : > : 7/20/99.
> : > : > : > : >
> : > : > : > : > 29. Amine polymer sequestrant and method of cholesterol
> : depletion.
> : > : > : > : Mandeville, W. H.,
> : > : > : > : > III.;
> : > : > : > : > Holmes-Farley, S. R.; US 5,919,832; 7/6/99.
> : > : > : > : >
> : > : > : > : > 30. Process for removing bile salts from a patient and
> : > : compositions
> : > : > : > : therefor. Mandeville,
> : > : > : > : > W. H.,
> : > : > : > : > III.; Holmes-Farley, S. R.; US 5,917,007; 6/29/99.
> : > : > : > : >
> : > : > : > : > 31. Polyamine salt hydrophobic sequestrant for cholesterol
> : > : depletion.
> : > : > : > : Mandeville, W. H.,
> : > : > : > : > III.;
> : > : > : > : > Holmes-Farley, S. R.; Petersen, J. S.; US 5,900,475;
5/4/99.
> : > : > : > : >
> : > : > : > : > 32. Process for removing bile salts from a patient and
> : > : compositions
> : > : > : > : therefor. Mandeville,
> : > : > : > : > W. H.,
> : > : > : > : > III.; Holmes-Farley, S. R.; US 5,840,766; 11/24/98.
> : > : > : > : >
> : > : > : > : > 33. Preparation of polymeric sequestrants for bile acid
salts.
> : > : > : Mandeville,
> : > : > : > : W. H., III.;
> : > : > : > : > Holmes-
> : > : > : > : > Farley, S. R.; US 5,703,188; 12/30/97.
> : > : > : > : >
> : > : > : > : > 34. Oral administration of iron-binding crosslinked amine
> : > : polymers.
> : > : > : > : Mandeville, W. H.,
> : > : > : > : > III.;
> : > : > : > : > Holmes-Farley, S. R.; US 5,702,696; 12/30/97.
> : > : > : > : >
> : > : > : > : > 35. Alkylated amine polymers. Mandeville, W. H., III.;
> : > : Holmes-Farley,
> : > : > : S.
> : > : > : > : R.; US 5,693,675;
> : > : > : > : > 12/2/97.
> : > : > : > : >
> : > : > : > : > 36. Method for removing bile salts from a patient with
> : alkylated
> : > : > : > : crosslinked amine
> : > : > : > : > polymers,
> : > : > : > : > and preparation of the polymers. Mandeville, W. H., III.;
> : > : > : Holmes-Farley,
> : > : > : > : S. R.; US
> : > : > : > : > 5,679,717; 10/21/97.
> : > : > : > : >
> : > : > : > : > 37. Phosphate-binding polymers for oral administration.
> : > : Holmes-Farley,
> : > : > : S.
> : > : > : > : R.; Mandeville,
> : > : > : > : > W.
> : > : > : > : > H., III.; US 5,667,775; 9/16/97.
> : > : > : > : >
> : > : > : > : > 38. Ion-exchange process using highly crosslinked polymers
for
> : > : > : removing
> : > : > : > : bile salts from a
> : > : > : > : > patient, preparation of the polymers, and compositions
> : containing
> : > : > : them.
> : > : > : > : Mandeville, W. H.,
> : > : > : > : > III.; Holmes-Farley, S. R.; US 5,624,963; 4/29/97.
> : > : > : > : >
> : > : > : > : > 39. Hydrophobic amine polymer sequestrant and method of
> : > : cholesterol
> : > : > : > : depletion. Mandeville,
> : > : > : > : > W. H., III.; Holmes-Farley, S. R.; Petersen, J. S.; US
> : 5,618,530;
> : > : > : 4/8/97.
> : > : > : > : >
> : > : > : > : > 40. Amine polymer sequestrant and method of cholesterol
> : depletion.
> : > : > : > : Mandeville, W. H.,
> : > : > : > : > III.;
> : > : > : > : > Holmes-Farley, S. R.; US 5,607,669; 3/4/97.
> : > : > : > : >
> : > : > : > : > 41. Phosphate-binding polymers for oral administration.
> : > : Holmes-Farley,
> : > : > : S.
> : > : > : > : R.; Mandeville,
> : > : > : > : > W.
> : > : > : > : > H., III.; US 5,496,545; 3/5/96.
> : > : > : > : >
> : > : > : > : > 42. Iron-binding polymers for oral administration.
Mandeville,
> : W.
> : > : H.,
> : > : > : > : III.; Holmes-Farley,
> : > : > : > : > S. R.;
> : > : > : > : > US 5,487,888; 1/30/96.
> : > : > : > : >
> : > : > : > : > 43. Ultra-thin, uniform sol-gel coating of a substrate
having
> : > : active
> : > : > : > : hydrogens on the
> : > : > : > : > surface.
> : > : > : > : > Holmes-Farley, S. R.; Yanyo, L. C.; US 5,175,027;
12/29/92.
> : > : > : > : >
> : > : > : > : > 44. Layered sol-gel coatings from organisilicon compounds.
> : > : > : Holmes-Farley,
> : > : > : > : S. R.; Yanyo, L.
> : > : > : > : > C.;
> : > : > : > : > US 5,182,143; 1/26/93.
> : > : > : > : >
> : > : > : > : > 45. Method for metal bonding using ultrathin primer
coating.
> : > : > : > : Holmes-Farley, S. R.; Yanyo,
> : > : > : > : > L.
> : > : > : > : > C.; Thuer, A. M.; US 5,139,601; 8/18/92.
> : > : > : > : >
> : > : > : > : > 46. Acrylic adhesive compositions. Holmes-Farley, S. R.;
> : Abbey, K.
> : > : J.;
> : > : > : US
> : > : > : > : 5,096,962;
> : > : > : > : > 3/17/92.
> : > : > : > : >
> : > : > : > : > 47. Modified halogenatedpolyolefin adhesives for
polyolefin
> : > : > : > : elastomer-metal bonding.
> : > : > : > : > Holmes-
> : > : > : > : > Farley, S. R.; US 5,102,956; 4/7/92.
> : > : > : > : >
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > PUBLISHED PATENT APPLICATIONS (FOREIGN ISSUED ONLY OR NOT
> : ISSUED)
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > 1. Aryl boronate functionalized polymers for treating
obesity
> : and
> : > : > : > : inhibiting fat uptake.
> : > : > : > : > Holmes-Farley, Stephen Randall; Mandeville, Harry W., III;
> : Dhal,
> : > : > : Pradeep
> : > : > : > : K.; Huval, Chad
> : > : > : > : > Cori; Li, Xinhua; Polomoscanik, Steven C. PCT Int. Appl.
> : (2003),
> : > : 92
> : > : > : pp. WO
> : > : > : > : 0302571.
> : > : > : > : >
> : > : > : > : > 2. Preparation of aryl boronic acids for treating obesity.
> : > : > : Holmes-Farley,
> : > : > : > : Stephen Randall;
> : > : > : > : > Mandeville, W. Harry, III; Huval, Chad Cori; Li, Xinhua;
Dhal,
> : > : Pradeep
> : > : > : K.
> : > : > : > : (Geltex
> : > : > : > : > Pharmaceuticals, Inc., USA). PCT Int. Appl. (2003), 62 pp.
WO
> : > : 0302570.
> : > : > : > : >
> : > : > : > : > 3. Fat-binding poly(diethanolaminopropyl)acrylamide.
> : > : Holmes-Farley,
> : > : > : > : Stephen Randall.
> : > : > : > : > (Geltex Pharmaceuticals, Inc., USA). PCT Int. Appl.
(2003), 32
> : pp.
> : > : WO
> : > : > : > : 0302130.
> : > : > : > : >
> : > : > : > : > 4. Method for reducing copper levels and treating copper
> : > : toxicosis.
> : > : > : > : Holmes-Farley, Stephen
> : > : > : > : > Randall. (Geltex Pharmaceuticals, Inc., USA). PCT Int.
Appl.
> : > : (2002),
> : > : > : 45
> : > : > : > : pp. WO
> : > : > : > : > 0285383.
> : > : > : > : >
> : > : > : > : > 5. Method for treating gout and binding uric acid.
> : Holmes-Farley,
> : > : > : Stephen
> : > : > : > : Randall; Burke,
> : > : > : > : > Steven K. WO 0285381 10/31/2002.
> : > : > : > : >
> : > : > : > : > 6. Method for treating gout and reducing serum uric acid.
> : > : > : Holmes-Farley,
> : > : > : > : Stephen Randall;
> : > : > : > : > Burke, Steven K WO 0285380 10/31/2002.
> : > : > : > : >
> : > : > : > : > 7. Amine condensation polymer bile acid sequestrants.
Huval,
> : C.
> : > : C.;
> : > : > : > : Holmes-Farley, S. R.;
> : > : > : > : > Whitesides, G. M. WO 1999-US30469; 7/6/2000.
> : > : > : > : >
> : > : > : > : > 8. Continuous crosslinking of polymer gels. Mandeville, W.
H.,
> : III
> : > : and
> : > : > : > : Holmes-Farley, S.
> : > : > : > : > R.;
> : > : > : > : > WO 1999-US5662; 9/23/1999.
> : > : > : > : >
> : > : > : > : > 9. Amine-containing copolymers as bile acid sequestrants.
> : > : > : Holmes-Farley,
> : > : > : > : S. R.; Petersen,
> : > : > : > : > J. S.;
> : > : > : > : > WO 9933452; 7/8/1999.
> : > : > : > : >
> : > : > : > : > 10. Polydiallylamine-based phosphate binders. Mandeville,
W.
> : H.,
> : > : III
> : > : > : and
> : > : > : > : Holmes-Farley, S.
> : > : > : > : > R.;
> : > : > : > : > WO 9922743; 5/14/1999.
> : > : > : > : >
> : > : > : > : > 11. Polyallylamine polymers for removing bile salts and
> : treating
> : > : > : > : hypercholesterolemia, and
> : > : > : > : > polymer preparation. Holmes-Farley, S. R.; Mandeville, W.
H.,
> : III;
> : > : > : Burke,
> : > : > : > : S. K.; Goldberg,
> : > : > : > : > D. I.; WO 9857652; 12/23/98.
> : > : > : > : >
> : > : > : > : > 12. Phosphate-bidning polymers combined with a calcium
> : supplement
> : > : for
> : > : > : oral
> : > : > : > : administration.
> : > : > : > : > Goldberg, D. I.; Burke, S. K.; Mandeville, W. H., III;
> : > : Holmes-Farley,
> : > : > : S.
> : > : > : > : R.; WO 9842355;
> : > : > : > : > 10/1/98.
> : > : > : > : >
> : > : > : > : > 13. Hydrophobic heteroatom-containing sequestrant for
> : cholesterol
> : > : > : > : depletion. Mandeville,
> : > : > : > : > W.
> : > : > : > : > H., III; Holmes-Farley, S. R.; Petersen, J. S.; WO
9639449;
> : > : 12/12/96.
> : > : > : > : >
> : > : > : > : > 14. Process for adjusting ion concentration in a patient
and
> : > : > : compositions
> : > : > : > : therefor.
> : > : > : > : > Mandeville,
> : > : > : > : > W. H., III; Holmes-Farley, S. R.; WO 9427619; 12/8/94.
> : > : > : > : >
> : > : > : > : > 15. Vacuum-deposited silver on polycarbonate with a
chromium
> : > : > : interlayer
> : > : > : > : for improved
> : > : > : > : > metal-
> : > : > : > : > substrate adhesion. Holmes-Farley, S. R.; Ger. Offen.
4322512;
> : > : > : 1/20/94.
> : > : > : > : >
> : > : > : > : > 16. Process for increased metal-substrate bond strength in
> : > : metalized
> : > : > : > : plastics.
> : > : > : > : > Holmes-Farley, S.
> : > : > : > : > R.; Ger. Offen. 4322516; 7/6/93.
> : > : > : > : >
> : > : > : > : > 17. Electrorheological fluids and preparation of particles
> : useful
> : > : in
> : > : > : the
> : > : > : > : fluids.
> : > : > : > : > Troughton,
> : > : > : > : > Barritt E., Jr.; Duclos, Theodore G.; Thuer, Anna Marie;
> : Carlson,
> : > : J.
> : > : > : > : David; Bares, Joseph
> : > : > : > : > E.;
> : > : > : > : > Yanyo, Lynn C.; Farley, Stephen Randall Holmes; Acker,
Debra
> : Nell.
> : > : EP
> : > : > : > : 394049;
> : > : > : > : > 10/24/1990.
> : > : > : > : >
> : > : > : > : > JOURNAL PUBLICATIONS
> : > : > : > : >
> : > : > : > : > 1. Bile acid binding to sevelamer HCl. Braunlin, William;
> : Zhorov,
> : > : > : Eugene;
> : > : > : > : Guo, Amy;
> : > : > : > : > Apruzzese, William; Xu, Qiuwei; Hook, Patrick; Smisek,
David
> : L.;
> : > : > : > : Mandeville, W. Harry;
> : > : > : > : > Holmes-Farley, S. Randall. Kidney International (2002),
62(2),
> : > : > : 611-619.
> : > : > : > : >
> : > : > : > : > 2. Amine functionalized polyethers as bile acid
sequestrants:
> : > : > : synthesis
> : > : > : > : and biological
> : > : > : > : > evaluation. Huval, Chad C.; Bailey, Matthew J.;
Holmes-Farley,
> : S.
> : > : > : Randall;
> : > : > : > : Mandeville, W.
> : > : > : > : > Harry; Miller-Gilmore, Karen; Sacchiero, Robert J.; Dhal,
> : Pradeep
> : > : K.
> : > : > : > : Journal of
> : > : > : > : > Macromolecular Science, Pure and Applied Chemistry (2001),
> : > : A38(12),
> : > : > : > : 1559-1574.
> : > : > : > : >
> : > : > : > : > 3. Novel Cholesterol Lowering Polymeric Drugs Obtained by
> : > : Molecular
> : > : > : > : Imprinting. Huval,
> : > : > : > : > Chad C.; Bailey, Mathew J.; Braunlin, William H.;
> : Holmes-Farley,
> : > : S.
> : > : > : > : Randall; Mandeville,
> : > : > : > : > W.
> : > : > : > : > Harry; Petersen, John S.; Polomoscanik, Steven C.;
Sacchiro,
> : > : Robert
> : > : > : J.;
> : > : > : > : Chen, Xi; Dhal,
> : > : > : > : > Pradeep K. Macromolecules (2001), 34(6), 1548-1550.
> : > : > : > : >
> : > : > : > : > 4. Synthetic polymers for the binding of fat in the
intestinal
> : > : tract.
> : > : > : > : Jozefiak, Thomas H.;
> : > : > : > : > Mandeville, W. Harry; Holmes-Farley, S. Randy; Arbeeny,
> : Cynthia;
> : > : > : Huval,
> : > : > : > : Chad C.;
> : > : > : > : > Sacchiero, Robert; Concagh, Danny; Yang, Kanwen; Maloney,
> : Cynthia.
> : > : > : > : Abstracts of
> : > : > : > : > Papers, 222nd ACS National Meeting, Chicago, IL, United
> : States,
> : > : August
> : > : > : > : 26-30, 2001
> : > : > : > : > (2001), POLY-047 and Polymer Preprints (American Chemical
> : Society,
> : > : > : > : Division of
> : > : > : > : > Polymer Chemistry) (2001), 42(2), 98.
> : > : > : > : >
> : > : > : > : > 5. Colesevelam hydrochloride: Synthesis and testing of a
novel
> : > : polymer
> : > : > : gel
> : > : > : > : pharmaceutical.
> : > : > : > : > Holmes-Farley, S. R; Mandeville, W. H.; Miller, K. L.;
> : Petersen,
> : > : J.;
> : > : > : Ward,
> : > : > : > : J.; Sacchiero,
> : > : > : > : > B.;
> : > : > : > : > Maloney, C.; Brochu, S.; Rosenbaum, D.; Goldberg, D.;
Norton,
> : K.
> : > : A.;
> : > : > : Chen,
> : > : > : > : X.; Mazzeo, J.
> : > : > : > : > R.. Polym. Preprints (2000), 41(1), 735-736.
> : > : > : > : >
> : > : > : > : > 6. In vitro comparison of bile acid binding to colesevelam
HCl
> : and
> : > : > : other
> : > : > : > : bile acid
> : > : > : > : > sequestrants.
> : > : > : > : > Braunliin, W.; Zhorov, E.; Smisek, D.; Guo, A.; Appruzese,
W.;
> : Xu,
> : > : Q.;
> : > : > : > : Hook, P.; Holmes-
> : > : > : > : > Farley, S. R; Mandeville, H. Polym. Preprints (2000),
41(1),
> : > : 708-709.
> : > : > : > : >
> : > : > : > : > 7. Novel polymeric pharmaceuticals: From startup to
market.
> : > : > : Holmes-Farley,
> : > : > : > : S. R; Polym.
> : > : > : > : > Mater. Sci. Eng (1999), 80, 246-247.
> : > : > : > : >
> : > : > : > : > 8. Design and characterization of of Sevelamer
Hydrochloride:
> : a
> : > : novel
> : > : > : > : phosphate-binding
> : > : > : > : > pharmaceutical. Holmes-Farley, S. R.; Mandeville, W. H.,
III;
> : > : Ward,
> : > : > : J.;
> : > : > : > : Miller, K. L.;
> : > : > : > : > Polym. Mater. Sci. Eng (1998), 79, 280-281 and also in J.
M.
> : S.-
> : > : Pure
> : > : > : and
> : > : > : > : Appl. Chem.,
> : > : > : > : > A36(7&8), p. 1085 (1999).
> : > : > : > : >
> : > : > : > : > 9. Three generations of bile acid sequestrants.
Mandeville, W.
> : H.,
> : > : > : III;
> : > : > : > : Braunlin, W.;
> : > : > : > : > Dhal, P.;
> : > : > : > : > Guo, A.; Huval, C.; Miller, K. L.; Petersen, J.;
Polomascanik,
> : S.;
> : > : > : > : Rosenbaum, D.;
> : > : > : > : > Sacchiero,
> : > : > : > : > R.; Ward, J.; Holmes-Farley, S. R.; Mat. Res. Soc. Symp.
Proc.
> : > : (1999),
> : > : > : > : 550, 3-15.
> : > : > : > : >
> : > : > : > : > 10. Effect of RenaGel, a non-absorbable, crosslinked,
> : polymeric
> : > : > : phosphate
> : > : > : > : binder, on
> : > : > : > : > urinary
> : > : > : > : > phosphorous excretion in rats. Rosenbaum, D. P.;
> : Holmes-Farley, S.
> : > : R.;
> : > : > : > : Mandeville, W. H.,
> : > : > : > : > III; Pitruzzello, M. .; Goldberg, D. I..; Nephrol., Dial.,
> : > : Transplant.
> : > : > : > : (1997), 12(5)
> : > : > : > : > 961-964.
> : > : > : > : >
> : > : > : > : > 11. Thin anisotropic coatings based on sol-gel technology.
> : > : > : Holmes-Farley,
> : > : > : > : S. R.; Yanyo, L.
> : > : > : > : > C;
> : > : > : > : > Mater. Res. Soc. Symp. Proc. (1990), 180 (Better Ceram.
Chem.
> : 4),
> : > : > : 439-444.
> : > : > : > : >
> : > : > : > : > 12. The mechanism of cure initiation of a surface
activated
> : > : adhesive.
> : > : > : > : Holmes-Farley, S.
> : > : > : > : > R.;
> : > : > : > : > Minichelli, J. L.; J. Adhes. Sci. Technol. (1991), 5(5),
> : 409-420.
> : > : > : > : >
> : > : > : > : > 13. Adhesion promotion and corrosion prevention using thin
> : > : anisotropic
> : > : > : > : coatings. Holmes-
> : > : > : > : > Farley, S. R.; Yanyo, L. C.; J. Adhes. Sci. Technol.
(1991),
> : 5(2),
> : > : > : > : 131-151.
> : > : > : > : >
> : > : > : > : > 14. Wetting of functionalized polyethylene having
ionizable
> : > : organic
> : > : > : acids
> : > : > : > : and bases at the
> : > : > : > : > polymer-water interface: relations between functional
group
> : > : polarity,
> : > : > : > : extent of
> : > : > : > : > ionization,
> : > : > : > : > and contact angle with water. Holmes-Farley, S. R.; Bain,
C.
> : D.;
> : > : > : > : Whitesides, G. M.;
> : > : > : > : > Langmuir
> : > : > : > : > (1988), 4(4), 921-937.
> : > : > : > : >
> : > : > : > : > 15. Binding of phenols to aluminum oxide surfaces. 1.
Phenols
> : with
> : > : a
> : > : > : > : single hydroxy group.
> : > : > : > : > Holmes-Farley, S. R.; Langmuir (1988), 4(3), 766-774.
> : > : > : > : >
> : > : > : > : > 16. Reconstruction of the interface of oxidatively
> : functionalized
> : > : > : > : polyethylene (PE-CO2H)
> : > : > : > : > and
> : > : > : > : > derivatives on heating. Holmes-Farley, S. R.; Reamey, R.
H.;
> : > : Nuzzo,
> : > : > : R.;
> : > : > : > : McCarthy, T. J.;
> : > : > : > : > Whitesides, G. M.; Langmuir (1987), 3(5), 799-815. See
also
> : Report
> : > : > : (1987),
> : > : > : > : AD-
> : > : > : > : > A179590/5/GAR, Gov. Rep. Announce. Index (U. S.) 1987,
87(15).
> : > : > : > : >
> : > : > : > : > 17. Surface-modified polyethylene film: the relationship
> : between
> : > : > : surface
> : > : > : > : chemistry and
> : > : > : > : > physical
> : > : > : > : > properties. Holmes-Farley, S. R; Diss. Abstr. Int. B 1987,
> : 47(11),
> : > : > : 4537.
> : > : > : > : >
> : > : > : > : > 18. Reactivity of carboxylic acid and ester groups in the
> : > : > : functionalized
> : > : > : > : interfacial
> : > : > : > : > region of
> : > : > : > : > "polyethylene carboxylic acid" (PE-CO2H) and its
derivatives:
> : > : > : > : differentiation of the
> : > : > : > : > functional groups into shallow and deep subsets based on a
> : > : comparison
> : > : > : of
> : > : > : > : contact angle and
> : > : > : > : > ATR-IR measurements. Holmes-Farley, S. R.; Whitesides, G.
M.;
> : > : Langmuir
> : > : > : > : (1987), 3(1), 62-
> : > : > : > : > 76.
> : > : > : > : >
> : > : > : > : > 19. Fluorescence properties of dansyl groups covalently
bonded
> : tot
> : > : he
> : > : > : > : surface of
> : > : > : > : > oxidatively
> : > : > : > : > functionalized low-density polyethylene film.
Holmes-Farley,
> : S.
> : > : R.;
> : > : > : > : Whitesides, G. M.;
> : > : > : > : > Langmuir (1986), 2(3), 266-281. See also Report (1985),
> : TR-85-2;
> : > : > : > : AD-A162435/2/GAR,
> : > : > : > : > Gov. Rep. Announce. Index (U. S.) 1986, 86(7).
> : > : > : > : >
> : > : > : > : > 20. Acid-base behavior of carboxylic acid groups
covalently
> : > : attached
> : > : > : at
> : > : > : > : the surface of
> : > : > : > : > polyethylene: The usefulness of contact angle in following
the
> : > : > : ionization
> : > : > : > : of surface
> : > : > : > : > functionality. Holmes-Farley, S. R.; Reamey, R. H.;
McCarthy,
> : T.
> : > : J.;
> : > : > : > : Deutch, J.;
> : > : > : > : > Whitesides,
> : > : > : > : > G. M.; Langmuir (1985), 1(6), 725-740.
> : > : > : > : >
> : > : > : > : > 21. The thermal stability of a surface modified solid
organic
> : > : polymer.
> : > : > : > : Holmes-Farley, S.
> : > : > : > : > R.;
> : > : > : > : > Whitesides, G. M.; Polym. Mater. Sci. Eng. (1985), 53,
> : 127-131.
> : > : > : > : >
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > CORAL REEF AQUARIA CHEMISTRY PUBLICATIONS (ON LINE)
> : > : > : > : >
> : > : > : > : > 1. The Seachem Borate Alkalinity Test Kit. Holmes-Farley,
R.
> : > : Advanced
> : > : > : > : Aquarist. June 2003.
> : > : > : > : >
> : > : > : > : > 2. The Self Purification of Limewater (Kalkwasser).
> : Holmes-Farley,
> : > : R.
> : > : > : > : Advanced Aquarist.
> : > : > : > : > May
> : > : > : > : > 2003.
> : > : > : > : >
> : > : > : > : > 3. The Degradation of Limewater (Kalkwasser) in Air.
> : > : Holmes-Farley, R.
> : > : > : > : Reefkeeping May
> : > : > : > : > 2003.
> : > : > : > : >
> : > : > : > : > 4. Reef Aquaria with Low Soluble Metals. Holmes-Farley, R.
> : > : Reefkeeping
> : > : > : > : April 2003.
> : > : > : > : >
> : > : > : > : > 5. Iodine in Marine Aquaria: Part II Effects on Macroalgae
> : Growth.
> : > : > : > : Holmes-Farley, R.
> : > : > : > : > Advanced Aquarist; April 2003.
> : > : > : > : >
> : > : > : > : > 6. Iodine in Marine Aquaria: Part II Effects on Macroalgae
> : Growth.
> : > : > : > : Holmes-Farley, R.
> : > : > : > : > Advanced Aquarist; April 2003.
> : > : > : > : >
> : > : > : > : > 7. Iodine in Marine Aquaria: Part I. Holmes-Farley, R.
> : Advanced
> : > : > : Aquarist;
> : > : > : > : March 2003.
> : > : > : > : >
> : > : > : > : > 8. How to Select a Calcium and Alkalinity Supplementation
> : Scheme.
> : > : > : > : Holmes-Farley, R.
> : > : > : > : > Advanced Aquarist; February 2003.
> : > : > : > : >
> : > : > : > : > 9. Silica in a Reef Tank. Holmes-Farley, R. Advanced
Aquarist;
> : > : January
> : > : > : > : 2003.
> : > : > : > : >
> : > : > : > : > 10. Boron in a Reef Tank. Holmes-Farley, R. Advanced
Aquarist;
> : > : > : December
> : > : > : > : 2002.
> : > : > : > : >
> : > : > : > : > 11. Solving Calcium and Alkalinity Problems.
Holmes-Farley, R.
> : > : > : Advanced
> : > : > : > : Aquarist; November
> : > : > : > : > 2002.
> : > : > : > : >
> : > : > : > : > 12. Iron: A Look at Organisms Other than Macroalgae.
> : > : Holmes-Farley, R.
> : > : > : > : Advanced Aquarist;
> : > : > : > : > November 2002.
> : > : > : > : >
> : > : > : > : > 13. Phosphorus: Algae's Best Friend. Holmes-Farley, R.;
> : Advanced
> : > : > : Aquarist,
> : > : > : > : September 2002.
> : > : > : > : >
> : > : > : > : > 14. Iron in a Reef Tank. Holmes-Farley, R.; Advanced
Aquarist,
> : > : August
> : > : > : > : 2002.
> : > : > : > : >
> : > : > : > : > 15. Calcium and Alkalinity. Holmes-Farley, R.;
> : Reefkeeping.com,
> : > : April
> : > : > : > : 2002.
> : > : > : > : >
> : > : > : > : > 16. Calcium Carbonate as a Supplement. Holmes-Farley, R.
> : Advanced
> : > : > : > : Aquarist; July 2002
> : > : > : > : >
> : > : > : > : > 17. Solutions to pH Problems. Holmes-Farley, R. Advanced
> : Aquarist;
> : > : > : June
> : > : > : > : 2002.
> : > : > : > : >
> : > : > : > : > 18. The Relationship Between Alkalinity and pH.
Holmes-Farley,
> : R.
> : > : > : Advanced
> : > : > : > : Aquarist, May
> : > : > : > : > 2002.
> : > : > : > : >
> : > : > : > : > 19. The Chemical & Biochemical Mechanisms of Calcification
in
> : > : Corals.
> : > : > : > : Holmes-Farley, R.
> : > : > : > : > Advanced Aquarist, April 2002.
> : > : > : > : >
> : > : > : > : > 20. Calcium. Holmes-Farley, R. Advanced Aquarist; March
2002.
> : > : > : > : >
> : > : > : > : > 21. Alkalinity. Holmes-Farley, R. Advanced Aquarist;
February
> : > : 2002.
> : > : > : > : >
> : > : > : > : > 22. Specific Gravity. Holmes-Farley, R. Advanced Aquarist,
> : January
> : > : > : 2002.
> : > : > : > : >
> : > : > : > : > 23. The Complete Nitrogen Cycle. Holmes-Farley, R.
Aquarium
> : > : Frontiers
> : > : > : > : 2000.
> : > : > : > : >
> : > : > : > : > 24. Magnesium: Calcium's little sister. Holmes-Farley, R.
> : Aquarium
> : > : > : > : Frontiers 2000.
> : > : > : > : >
> : > : > : > : > 25. Phosphate..What is it and why should you care.
> : Holmes-Farley,
> : > : R.
> : > : > : > : Aquarium Frontiers
> : > : > : > : > 2000.
> : > : > : > : > 26. Carbon Dioxide: Friend or Foe . Holmes-Farley, R.
Aquarium
> : > : > : Frontiers
> : > : > : > : 2000.
> : > : > : > : >
> : > : > : > : > 27. Using Conductivity To Measure Salinity, R. Aquarium
> : Frontiers
> : > : > : 2000.
> : > : > : > : >
> : > : > : > : > 28. Understanding Seawater. Holmes-Farley, R. Aquarium
> : Frontiers
> : > : 1999.
> : > : > : > : >
> : > : > : > : > 29. Protein Skimming: How it Works. Fishnet Library 1998.
> : > : > : > : >
> : > : > : > : >
> : > : > : > : >
> : > : > : > : >
> : > : > : > : >
> : > : > : > : >
> : > : > : > : >
> : > : > : > : > Boomer
> : > : > : > : >
> : > : > : > : > Want to talk chemistry ? The Reef Chemistry Forum
> : > : > : > : > http://www.reefcentral.com/vbulletin/index.php
> : > : > : > : >
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> : > : > : > : > Please Join Our Growing Membership
> : > : > : > : > www.coralrealm.com
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