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10 February, 10:31

A saturated aqueous solution of Ag2SO3 contains 3.2x10-5 M Ag+. What is the solubility-product equilibrium constant for Ag2SO3? A) 2.0x10-2 B) 1.6x10-2 C) 1.3x10-13 D) 1.6x10-14 E) 4.1x10-15

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  1. 10 February, 12:36
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    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.
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