The molar solubility of SrSO₄ (Ksp = 7.6 × 10^-7) is:

Question

Quizplus · Accepted Answer

The general equation for the dissolution of strontium sulfide (SrS) in water is:

SrS (s) ↔ Sr2+ (aq) + S2- (aq)

The Ksp expression for this equilibrium is:

Ksp = [Sr2+] [S2-]

We are given that Ksp = 7.6 × 10^-7. Since SrS dissociates into one Sr2+ ion and one S2- ion, their concentrations are equal and can be represented as x. Therefore:

Ksp = x^2

Solving for x:

x = sqrt(Ksp) = sqrt(7.6 × 10^-7) = 8.7 × 10^-4 M

This is the molar solubility of SrS in water, so the answer is D.

The Molar Solubility of SrSO4 (Ksp = 7

The Molar Solubility of SrSO₄ (Ksp = 7