Solubility Equilibria
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1. The Solubility Product Constant. PbBr2 is a slightly soluble salt. Write the chemical equilibrium equation that describes the salt partially dissolving in water and the solubility product expression. Calculate the Ksp value for lead(II) bromide if the molar solubility in pure water is 1.3 x 10-2 M.
2. Molar Solubility. Calculate the molar solubility of the following compounds from the Ksp values given on pages 772 - 773.
a. Zn(OH)2
b. Fe(OH)3
3. Solubility and the Common-Ion Effect. In problem 1 it was stated that the molar solubility of PbBr2 in pure water is 1.3 x 10-2 M. Calculate the molar solubility of PbBr2 in 0.20 M KBr and in 0.20 M Pb(NO3)2.
4. Precipitation Calculations. Will a precipitate of calcium sulfate (Ksp = 2.4 x 10-5) form when 50.0 mL of 0.00150 M calcium chloride and 25.0 mL of 0.0100 M sodium sulfate are mixed? Why or why not?
5. Complex-Ion Equilibria. When sufficient ammonia is added to a 0.00500 M silver nitrate solution to initially give 0.100 M aqueous ammonia, what is the molarity of the silver ion (Ag+) after the complex ion Ag(NH3)2+ has been formed at equilibrium?
Ag+(aq) + 2 NH3(aq)  Ag(NH3)2+(aq)
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Solution Summary
The solution involves calculations of solubility product constants, molar solubility, precipitation, and molarities at equilibrium. Detailed descriptions are provided along with the calculations.
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