Answer:
D) 1.6 x 10⁻¹⁴
Explanation:
The solubility-product equilibrium constant for Ag₂SO₃ is given by the expression
Ksp = [Ag⁺]² [SO₃²⁻]
where [Ag⁺] and [SO₃²⁻] are the concentration of the species dissolved in solution for the equlibrium
Ag₂SO₃ (s) ⇄ 2 Ag⁺ + SO₃²⁻
we are given the concentration of Ag⁺ and from the stoichiometry of the equilibrium, the concentration of SO₃²⁻ is half that value, so
[Ag⁺]² = 3.2 x 10⁻⁵ M
[SO₃²⁻] = 3.2 x 10⁻⁵ M / 2 = 1.6 x 10⁻⁵ M
plugging these values into the solubility product constant equation we have
Ksp = (3.2 x 10⁻⁵)² x (1.6 x 10⁻⁵) = 1.6 x 10¹⁴
Therefore D is the correct answer.
