Posted by Claus on Thursday, April 3, 2008 at 9:11pm.
AgCl <==> Ag^+ + Cl^
NaCl ==> Na^+ + Cl^
Ksp = (Ag^+)(Cl^) = 1.8 x 10^10
Let S = solubility of AgCl, then
(Ag^+) = S
(Cl^) = S+0.01
Solve for S.
Note: A similar problem to this post (0.1 M NaCl instead of 0.01 M NaCl) was on a couple of days ago; the one who posted said that the answer came back incorrect. Check my work. Check myu thinking.
Should the continuing work look like this?
S = 1.8 x 10^10 + 1
= 1.00?
Please help I am very confused

chemistry  DrBob222, Thursday, April 3, 2008 at 9:40pm
I don't understand how you can be confused.
(S)(S + 0.01) = 1.8 x 10^10
You can solve the quadratic, OR you can make the simplifying assumption that S + 0.01 is about 0.01 (that is, that S is very small in comparison so 0.01 is not really different than S + 0.01).
If we make the assumption, then
S(0.01) = 1.8 x 10^10
and S = 1.8 x 10^8 M = (AgCl).
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