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The Ksp for PbCl2= 1.7x10^-5 Calculate the molar solubility of PbCl2 in a solution that is 0.1 M...

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Chemistry

TheKsp for PbCl2= 1.7x10^-5
Calculate the molar solubility of PbCl2 in a solution that is0.1 M of the soluble salt MgCl2

Answer & Explanation Solved by verified expert
3.8 Ratings (562 Votes)

Let 'S'(mol/L) be the solubility of PbCl2

PbCl2 -----> Pb2+ + 2Cl-

MgCl2 -----> Mg2+ + 2Cl-

[ Pb2+] = S

[Cl-] = [Cl-]PbCl2 + [Cl-]MgCl2

      = 2S + (2x0.1)

      = 2S + 0.2

[ Pb2+] = S

Solubility product constant , Ksp = [ Pb2+] [Cl-]2 = 1.7x10-5

                                               S x ( 2S+0.2)2 = 1.7x10-5

                                                   S = 4.25x10-4 mol/L

Therefore the molar solubility of PbCl2 is 4.25x10-4 mol/L
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