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Solubility Problems

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A solution contains 0.01 M Ag+, 0.04 M Hg22+ and 0.1 M Pb2+. NaCl is gradually added to precipitate the Ag+ as AgCl, the Hg22+ as Hg2Cl2, and the Pb2+ as PbCl2. Given the following Ksp values: AgCl (Ksp = 1.6 x 10-10); Hg2Cl2 (Ksp = 3.5 x 10-18); PbCl2 (Ksp = 2.4 x 10-4).
a) at what [Cl-] will precipitation of each salt begin. Start with the following UNBALANCED equations:
i) AgCl (s) --> Ag+ (aq) + Cl- (aq)
ii) Hg2Cl2 (s) --> Hg22+ (aq) + Cl- (aq)
i) PbCl2 (s) --> Pb2+ (aq) + Cl- (aq)
b) What is the concentration of Hg22+ in solution when AgCl begins to precipitate?
c) What are the concentrations of Ag+ and Hg22+ when Pb2+ begins to precipitate?
d) Discuss the suitability of fractional precipitation using NaCl for the separation of Ag+, Hg22+ and Pb2+.

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This solution helps explore solubility problems with regards to chemistry.

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