In other words...run a batch of CS with a salt starter and see if the PH
goes more towards basic than acid?
Or add salt to a batch of CS and see if the ph goes towards basic and
there is a AGCL precipitate? [or white milkyness]
Ken
>
> The concern was over chlorine not sodium. However, if the chlorine
> does react with the silver,,,what happens to the sodium? Sodium
> hydroxide [lye] would be my guess
>
> Ken >>
>
>Ken: I guess it depends on the anion one assumes to be associated with the
>Ag+ when it was generated while making CS. Since both Ag+ and silver
>particulate are produced during CS electrolysis, and it is the charge on the
>CS particles that maintains their separation, it is not unreasonable to
>assume that Ag+ is present on the surface of these particles, and may not be
>associated with a corresponding anion such as OH-. Could the following
>reaction occur when NaCl solution is added to precipitate silver chloride?
>
>NaCl + [Ag+] + H2O ---------------> AgCl(s) + NaOH + [H+]
>
>Since NaOH is soluble, what may occur is that Na+ ties up the OH- part of
the
>water molecule, releasing H+ as silver drops out. Since the Na+ would "tie
>up" OH- much, much more tightly than H+, the pH may actually fall not rise.
>In other words, after silver drops out, the Na+ may reduce the activity
>coefficient of OH- and increase the activity coefficient of H+. Therefore,
It
>would be interesting the check pH before and after precipitating silver
>chloride to see if my hypothesis holds water (pun definitely intended,
ha,ha)
>Roger
>
>
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