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)