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Solubility question?

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What is the solubility of mercury, Hg2

2+, in a solution of 0.045 M HBr(aq) knowing that

Ksp(Hg2Br2) = 1.3 × 10-21?

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  1. Hg2Br2  <==>  Hg22+  +  2Br-

    Ksp = [Hg22+][Br-]^2

    1.3 x 10^-21 = [Hg22+](0.045)^2

    6.4 x 10^-19 = [Hg22+]


  2. Hg2Br2 --> Hg2+ + 2Br-

    Ksp = [Hg2+][Br-] 2

    [Hg2+](0.045)2 = 1.3 x 10-21

    [Hg2+] = 6.4 x 10^-19
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