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?

AgBr MW=188

M=(13.5x10^-5)/(188)=7.18x10^-7

Ksp=[Ag]

=x^2=[7.18x10^-7]^2= 5.15x10^-13

2. Solubility of Silver(I) Carbonate is 3.2x10^-2 g/100mL What is the Ksp?

Ag2CO3 MW=276

g/L=(3.2x10^-2)(1000mL)/(100mL)=.32

M=.32/276=1.16x10^-3

Ksp=[Ag]^2[CO3]=4x^3=4(1.16x10^-3)^3=6.23x10^-9

3. The solubility product constant for Strontium Chromate is 3.6x10^-5. What is the solubility in g/100mL

MW=204

Ksp=[Sr][CrO4]=x^2

x^2=3.6x10^-5

x=6x10^-3=M

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

MW=367

Ksp=PbBr2=[ x][2x]^2=4x^3

4x^3=4.6x10^-6

x=.01047

g/L=(.01047)(367)=3.8

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?

1.8x10^-9=(.1)x

x=1.8x10^-8

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

Ksp=[Ba][SO4]=[2x10^-2][ x]

[2x10^-2][ x]=1.5x10^-9

x>7.5x10^-8

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

Ksp=[Pb][IO3]^2=4x^3=4(.00004)^3=2.56x10^-13

b. Calculate the molar solubility of Pb(IO3)2 in a .1M Pb(NO3)2 solution

2.56x10^-13=[ x][.1]^2

x=2.56x10^-11

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

Pb(NO3)=.12x.333L=.03396moles

KIO3=.435x.667mL=.29 moles

Pb+2IO3

.04 moles + .3 moles = .22 moles excess IO3

2.56x10^-13=[Pb][IO3]^2

2.56x10^-13=[Pb][.22]^2

x=5.3x10^-12

8. The Ksp for Fe(OH)3 is 5x10^-38, calculate the pH of a saturated solution of Fe(OH)3

Ksp=[Fe][OH]^3=[ x][3x]^3=27x^4

5x10^-38=27x^4

x=2.0744

-log (3x) = pOH = 9.2

pH = 4.79

EDIT: Corrected #4,8 (divide, then take the nth root)