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21 October, 21:32

Calculate the solubility (in g/l) of silver chromate in water at 25°c if the ksp for ag2cro4 is 1.1 * 10-12. 2.7 * 10-2 g/l 2.2 * 10-2 g/l 3.4 * 10-2 g/l 3.5 * 10-4 g/l

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  1. 21 October, 23:00
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    Answer is: solubility of silver chromate is 2.2 * 10-2 g/l.

    Chemical reaction (dissociation) of silver chromate in water:

    Ag ₂CrO₄ (s) → 2Ag⁺ (aq) + CrO₄²⁻ (aq).

    Ksp (Ag ₂CrO₄) = [Ag⁺]²·[CrO₄²⁻].

    [CrO ₄²⁻] = x.

    [Ag ⁺] = 2[CrO₄²⁻] = 2x

    1,1 ·10⁻¹² = (2x) ² · x = 4x³.

    x = ∛1,1·10⁻¹² : 4.

    x = 6,5·10⁻⁵ M.

    solubility of silver chromate: 6,5·10⁻⁵ mol/L · 331,73 g/mol = 0,022 g/L.

    Ksp is the solubility product constant for a solid substance dissolving in an aqueous solution.

    [Ag ⁺] is equilibrium concentration of silver cations.

    [CrO ₄²⁻] is equilibrium concentration of chromate anions.
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