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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