Predict the molar solubility of the following salt in an aqueous solution that contains the given concentration of one of its ions:
BaSO₄;[SO₄^2-] = 4.3 × 10^-5 M;K_sp = 1.1 × 10^-10

Question

Predict the molar solubility of the following salt in an aqueous solution that contains the given concentration of one of its ions: BaSO₄;[SO₄^2-] = 4.3 × 10^-5 M;K_sp = 1.1 × 10^-10

Quizplus · Accepted Answer

First, write the balanced equation for the dissolution of BaSO4:
BaSO4(s) ⇌ Ba2+(aq) + SO42-(aq)

The solubility product expression is:
Ksp = [Ba2+][SO42-]

We are given the concentration of SO42-, which we can assume comes entirely from the dissociation of BaSO4. Therefore, [SO42-] = 4.3 × 10-5 M.

Using the Ksp value provided, we can set up an ICE table to calculate the concentration of Ba2+ in solution, and thus the molar solubility of BaSO4.

Initial:	0	 	 	 
Change:	+x	-x	-x	 	 
Equilibrium:	x	4.3 × 10-5	4.3 × 10-5

Ksp = [Ba2+][SO42-] = x(4.3 × 10-5)(4.3 × 10-5) = 1.1 × 10-10

Solving for x, we get:
x = 2.6 × 10-6 M

Therefore, the molar solubility of BaSO4 is 2.6 × 10-6 M.

The correct answer is choice D.

Predict the Molar Solubility of the Following Salt in an Aqueous