Group Quiz: Solubility Unit Problems (Due Monday)



2Group Quiz: Solubility Unit Problems (Due Monday)

1. Calculate the Ksp for each of the salts whose solubility is listed below. 

a) CaSO4 = =5.0 x 10-3 mol/= x^2 =2.50E-05

b) MgF2 = 2.7 x 10-3 mol/L 4x^3= 7.873E-08

c) AgC2H3O2 = 1.02 g/100 mL  x^2=3.73E-3 (MM=166.9)

d) SrF2 = 12.2 mg/100 mL 4x^3= 3.66E-9 (MM 125.6)

2. Calculate 

a) the solubility in moles/L of each of three salts and 

b) the concentration of the cations in mg/mL in each of the saturated solutions.

i) AgCN Ksp = 2.0 x 10-12 1.414E-06 M 1.53E-04 mg/ml MM= 107.9

ii) BaSO4 Ksp = 1.5 x 10-9 3.873E-05 M 5.32E-03 mg/ml MM= 137.3

iii) FeS Ksp = 3.7 x 10-19 6.083E-10 M 3,40E-8 mg/ml MM= 55.8

iv) Mg(OH)2 Ksp = 9.0 x 10-12 1.310E-04M 3,20E-3 mg/ml MM 24.3

v) Ag2S Ksp = 1.6 x 10-49 3.420E-17 M 7.38E-15 mg/ml MM= 107.9

vi) CaF2 Ksp = 4.9 x 10-11 2.305E-04 M 9.24E-03 mg/ml MM= 40.1

3. Consider these slightly soluble salts: 

     i) PbS Ksp = 8.4 x 10-28 x= 2.898E-14 M

    ii) PbSO4 Ksp = 1.8 x 10-8 x= 1.342E-04 M

   iii) Pb(IO3)2 Ksp = 2.6 x 10-13 x= 4.021E-05 M

a)Which is the most soluble? ) PbSO4 Ksp = 1.8 x 10-8

b) Calculate the solubility in moles/L for PbSO4.  1.342E-04 M

c) How many grams of PbSO4 dissolve in 1 L of solution?  1.342E-04*303.3 =4.07E-02

d) How can you decrease the concentration of Pb2+(aq) in a saturated solution of PbSO4 solution?  Add SO4

e) What is the concentration in moles/L of PbS in a saturated solution of the salt? 2.898E-14

4.   For each of these substances, calculate the milligrams of metallic ion that can remain at equilibrium in a solution having a [OH-] = 1.0 x 10-4 mol/L.  which would be a pH= 10

a) Cu(OH)2 Ksp = 1.6 x 10-9 x*(10-4)^2 =Ksp x= 1.60E-01M 10.17 g/L of Cu

b) Fe(OH)3 Ksp = 6.0 x 10-38 x*(10-4)^3 =Ksp x=6.00E-26=M 3.35E-24 g/L of Fe

c) Mg(OH)2 Ksp = 6.0 x 10-12 x*(10-4)^2 =Ksp x=6.00E-04M 1.46E-2 g/L of Mg

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