Question

The solubility of silver sulfate, Ag₂SO₄, in water has been determined to be 8.00 g/L. What is the solubility of silver sulfate in 0.600 M of sodium sulfate, Na₂SO₄?

____________g/L

What is the solubility (in grams per liter) of strontium sulfate, SrSO₄, in 0.34 M sodium sulfate, Na₂SO₄? K_sp for SrSO₄ is 2.5×10^-7.

s =___________g/L

Answer 1

The molar mass of Ag2SO4 is: 311.8 g/mol. Hence, 8.0 g/L is equivalent to (8.0/311.8) M or 0.02566 M concentration.
Ksp = [Ag+]^2[SO4--] = (2*0.02566)^2*0.02566 = 6.756*10^-5 (M^3)

Let the solubility of silver sulfate, Ag2SO4, in 0.6 M sodium sulfate, Na2SO4, be X M. We have:
Ksp = 6.756*10^-5 = (2*X)^2(0.6+X)
or: X = 0.00283 (M)
Hence the solubility of silver sulfate, Ag2SO4, in 0.91 M sodium sulfate, Na2SO4, is:
0.00283*311.8 = 0.8835(g/L)

2 .Ksp for SrSO4 is 2.5×10-7. c = 0.34

SOLUBILITY ?

S = k_S.P /c =2.5×10-7 / 0.34 = 7.3529X10^-7