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Solubility Problems with Ksp

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Q#1 (Common ion problem)
What is the solubility,in mg/mL of BaF2 in
a)Pure Water
b)in a solution containing 5.0mg/mL of KF
Ksp of BaF2=1.0*10^-6

Q#2 Effect of pH on solubility
a)Calculate the solubility of a saturated solution og Mg(OH)2 on pure water.(My answer is 1.65096*10^-4M
b)Calculate the solubility of the same saturated solution of Mg(OH)2 in a solution with pH of 10.49.
Mg(OH)2 Ksp= 1.8*10^-11

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See attached word file for proper formating...

Q#1 (Common ion problem)
What is the solubility,in mg/mL of BaF2 in
a)Pure Water
b)in a solution containing 5.0mg/mL of KF
Ksp of BaF2=1.0*10^-6

For this question, you will have to write both the (1) reaction equation for the important solid dissolving (BaF2):
BaF2 (s)  Ba2+ + 2F-
-s s 2s

So we can see that if s amount of BaF2 dissolves, we will have s amount of barium ions and 2s amount of fluoride ions. But in this ...

Solution Summary

Almost 370 words to explain the calculation needed to find the solubility of compounds in water and a solution with a different Ksp, as well as pH's effect on solubility

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Solubility Problems

Please refer to the attachment for the complete solution.

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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