Calculate the solubilities of the following compounds in a 0.0344 M solution of

Question

Calculate the solubilities of the following compounds in a 0.0344 M solution of Mg(ClO4)2 using (1) activities and (2) molar concentrations:

A. AgSCN

(1) using activities:

Solubility =

(2) using molar concentrations:

Solubility =

B. PbI2

(1) using activities:

Solubility =

(2) using molar concentrations:

Solubility =

C. BaSO4

(1) using activities:

Solubility =

(2) using molar concentrations:

Solubility =

D. Cd2Fe(CN)6

(1) using activities:

Solubility =

(2) using molar concentrations:

Solubility =

Explanation / Answer

B) molar concentrations.

Ksp = [Pb2+][I- ] 2 = 3.0•10-16

[Pb2+] = s, [I- ] = 2s

Ksp = s.(2s)2 = 3.0•10-16

s = solubility = (3.0•10-16/4)1/3 = 4.22•10-6

2) µ = ½ ciZi2 = ½ [0.0333(2)2 + 0.0666(1)2 ] = 0.100

Pb2+ = 0.36, I- = 0.75

Ksp = [Pb2+][I- ] 2 Pb2+( I-) 2

K’sp = Ksp/ Pb2+( I-) 2 = 3.0•10-16/(0.36•0.752 ) = 1.48•10-15

[Pb2+]= s, [I- ] = 2s

Ksp = s(2s)2 = 1.48•10-15  

solubility = (1.48•10-15/4)1/3 = 7.18•10-6

SIMILARLY SOLVE FOR OTHER COMPOUNDS

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