General Chemistry 2: Solubility Product

By experiment, it is found that of 6.2 x 10##^{-12}## moles of Pb##_3##(PO##_4##)##_2## dissolves in 1 L of aqueous solution at 25##^\circ##C. What is the solubility product constant, K##_{sp}##, at this temperature?

Calculate the solubility (in grams per liter) of PbI##_2## in water from the solubility product constant 1.4 x 10##^{-8}##.

What are the concentrations of the ionic species in a saturated solution of Ag##_2##CrO##_4##
K##_{sp}## = 1.1 x 10##^{-12}##

Calculate the equilibrium concentration of Pb##^{2+}##, I##^-##, Na(\^+##, and NO##_3^-## when 100.0 mL of 0.0500 M Pb(NO##_3##)##_2## and 200.0 mL of 0.100 M NaI are mixed.
PbI##_2## K##_{sp}## = 1.4 x 10##^{-8}##

What is the molar solubility of Ag##_2##CrO##_4## in 0.100 M AgNO##_3##? Compare this to the molar solubility of Ag##_2##CrO##_4## in water, 1.3 x 10##^{-4}## M
Ag##_2##CrO##_4## K##_{sp}## = 9.0 x 10##^{-12}##

The concentration of Mg(NO##_3##)##_2## is 4 x 10##^{-4}## M and the concentration of NaOH is 2 x 10##^{-4}##, do you expect Mg(OH)##_2## to precipitate?
Mg(OH)##_2## K##_{sp}## = 8.9 x 10##^{-12}##

A solution contains 1.0 x 10##^{-4}## M Cu##^+## and 2.0 x 10##^{-3}## M Pb##^{2+}##. When I##^{-}## is added, which will precipitate first? How much I##^-## is needed to cause a precipitate to form?When CuI is added to PbI##_2##
CuI K##_{sp}## = 5.3 x 10##^{-12}##
PbI##_2## K##_{sp}## = 1.4 x 10##^{-8}##

What is the solubility of AgCl in 0.020 M NaCN?
AgCl K##_{sp}## = 1.8 x 10##^{-10}##
Ag(CN)##_2^-## K##_{f}## = 5.6 x 10##^{18}##

0.25 moles of AgNO##_3## are dissolved in 1 L of 0.60 M NaCN and 1 mole of NaCl is added. Will AgCl precipitate?
AgCl K##_{sp}## = 1.8 x 10##^{-10}##
Ag(CN)##_2^-## K##_{f}## = 5.6 x 10##^{18}##

How many moles of Mg(OH)##_2## can be dissolved in a 1 L solution that already contains 0.52 moles Mg##^{2+}##.
Mg(OH)##_2## K##_{sp}## = 8.9 x 10##^{-12}##

The solubility of Ce(IO##_3##)##_3## in a 0.20 M KIO##_3## solution is 4.4 x 10##^{-8}## mol/L. Calculate K##_{sp}## for Ce(IO##_3##)##_3##.

Calculate the concentrations of Ag##^+##, Ag(S##_2##O##_3##)##^-##, and Ag(S##_2##O##_3##)##_2^{3-}## in a solution prepared by mixing 150.0 mL of 1.00 x 10##^{-3}## M AgNO##_3## with 200.0 mL of 5.00 M Na##_2##S##_2##O##_3##. The stepwise formation equilibria are:
Ag##^+## + S##_2##O##_3^{2-}## ##\leftrightharpoons## Ag(S##_2##O##_3##)##^-##    K##_{f1}## = 7.4 x 10##^{8}##
Ag(S##_2##O##_3##)##^-## + S##_2##O##_3^{2-}## ##\leftrightharpoons## Ag(S##_2##O##_3##)##_2^{3-}##    K##_{f2}## = 3.9 x 10##^{4}##