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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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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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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 ...

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