[pure-silver] Re: baking soda as wash aid
- From: "Koch, Gerald" <gkoch02@xxxxxxxxxx>
- To: <pure-silver@xxxxxxxxxxxxx>
- Date: Thu, 17 Feb 2005 17:32:35 -0500
In a solution of sodium bicarbonate the principal species is the HC03-
ion. There is a very small amount of CO3-2 ion present from further
dissociation of HC03-. My question is where on the HC03- ion are you
intending to put the extra C02 that you say is absorbed?
I quote from the Food Chemicals Codex; "Its solutions, when freshly
prepared with cold water, without shaking, are alkaline to litmus. The
alkalinity INCREASES as the solutions stand, are agitated or are
heated."
You will find a similar statement in any detailed discussion of sodium
bicarbonate.
-----Original Message-----
From: pure-silver-bounce@xxxxxxxxxxxxx
[mailto:pure-silver-bounce@xxxxxxxxxxxxx] On Behalf Of Ryuji Suzuki
Sent: Thursday, February 17, 2005 4:34 PM
To: pure-silver@xxxxxxxxxxxxx
Subject: [pure-silver] Re: baking soda as wash aid
From: "Koch, Gerald" <gkoch02@xxxxxxxxxx>
Subject: [pure-silver] Re: baking soda as wash aid
Date: Thu, 17 Feb 2005 16:15:31 -0500
> As I said, I think you misread my statement; it's easy to read=20
> carbonate instead of bicarbonate, especially after reading a lot of=20
> emails.
I didn't misread, and I don't agree with what you said. Bicarbonate
solution may decrease pH but not increase.
> I think you will agree that sodium bicarbonate is already the acid=20
> salt of carbonic acid and cannot absorb C02.
I disagree. Bicarbonate is a base form of carbonic acid. Carbonate is
another base form of carbonic acid. Carbonic acid will lower the pH of
either solution. Review of the freshman chem textbook is in order.
--
Ryuji Suzuki
"Keep a good head and always carry a light camera."
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=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=
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=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D=3D
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