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Topic: Common Ion Effect and HCl  (Read 3113 times)

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Offline nonlinear

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Common Ion Effect and HCl
« on: February 27, 2010, 08:19:59 PM »
Hi, I have a question about the common ion effect.
In general, if I dissolved AgCl2 in a strong acid, it wouldn't make a difference in its solubility, correct? HCl is a strong acid so the Cl- ions would not have any significant affinity for the H+.
My question is this: What if AgCl2 were put into a solution of HCl? HCl would fully dissociate, so there would be an initial concentration of Cl- in the solution. Wouldn't that decrease AgCl2's solubility in HCl (aq)?
I want to know if my thinking is correct, that's all. Thank you!
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Offline Borek

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Re: Common Ion Effect and HCl
« Reply #1 on: February 27, 2010, 08:44:02 PM »
What is AgCl2?

You are right about strong acid not making any difference. You are also right about presence of chlorides lowring solubility of silver chloride.
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Offline nonlinear

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Re: Common Ion Effect and HCl
« Reply #2 on: February 27, 2010, 09:03:30 PM »
Oh! sorry, AgCl. I don't know what I was thinking.
Alright, thanks!
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