I worked most of these out, I think I understand them all, but I would really like someone to verify my answers. It would make me feel much better about my upcoming test.
1. Solubility of Silver(I) Bromide is 13.5x10^-5 g/L What is the Ksp?
2. Solubility of Silver(I) Carbonate is 3.2x10^-2 g/100mL What is the Ksp?
3. The solubility product constant for Strontium Chromate is 3.6x10^-5. What is the solubility in g/100mL
g/L=(6x10^-3)(204)=1.224)(.1L)/(100mL)= 1.224x10^-4 g/100mL
4. The Ksp for Lead(II) Bromide is 4.6x10^-6 What is solubility in g/L
5. If the concentration of chloride ion remaining in solution after silver chloride has been precipitate is .1M, what is the concentration of the silver ion?
6. A solution of salt contains 2x10^-2 moles per liter of sulfate ion, calculate the concentration of the Barium ion that must be exceeded before the barium sulfate precipitates. Ksp of Barium sulfate = 1.5x10^-9
7. A saturated solution of Lead(II) Iodate in pure water has a Lead ion concentration of .00004 moles/L
a. Calculate the Ksp of Pb(IO3)2
b. Calculate the molar solubility of Pb(IO3)2 in a .1M Pb(NO3)2 solution
c. 667ml of .435M KIO3 is added to 333ml of a .12M Pb(NO3)2 solution. Calculate the concentations of Pb and IO3 in the solution at equilibrium
.04 moles + .3 moles = .22 moles excess IO3
8. The Ksp for Fe(OH)3 is 5x10^-38, calculate the pH of a saturated solution of Fe(OH)3
-log (3x) = pOH = 9.2
pH = 4.79
EDIT: Corrected #4,8 (divide, then take the nth root)