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)