What is the molar solubility of PbCl2 in a solution of 0.23 M CaCl2? Ksp = 1.6 10-5 for PbCl2.

Question

idk how to do this because of the Cl2

Answer 1

It's a common ion and you just add it in.
PbCl2==>Pb^+2 + 2Cl^-
So Ksp = (Pb^+2)(Cl^-)^2
(Pb^+2) = x
(Cl^-) = 2x (from the PbCl2 solubility + 2*0.23 from the CaCl2.
Plug in the numbers and solve for x.
You can avoid a quadratic equation by making the simplifying assumption that x + 0.46 = 0.46 (but since the solubility of PbCl2 is high (ksp is relatively large) that may lead to an error. At any rate, you can try it an see if there is much error or you can go ahead and solve the quadratic equation since most calculators handle that easily now.

Answer 2

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