For the following equilibrium, if the concentration of the sulfate ion is X, what will be the molar solubility of strontium sulfate?

Question

For the following equilibrium, if the concentration of the sulfate ion is X, what will be the molar solubility of strontium sulfate?

SrSO4(s)↽−−⇀Sr2+(aq)+SO2−4(aq)

1. 
   

Answer 1

SrSO₄(s) ==> Sr²⁺(aq) + SO₄^2-(aq)

Ksp = [Sr²⁺][SO₄^2-]

If [SO₄^2-] = x , then [Sr²⁺] also = x

We need to know the Ksp for SrSO₄. Looking it up, I find it to be 3.4x10^-7

3.4x10^-7 = (x)(x) = x²

x = 5.8x10^-4 M