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1 December, 00:33

At a certain temperature, the solubility of strontium arsenate, sr3 (aso4) 2, is 0.0590 g/l. what is the ksp of this salt at this temperature?

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  1. 1 December, 02:24
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    First, we have to change Sr3 (ASO4) 2 from 0.059 g/L to moles:

    and when the molar mass of Sr3 (ASO4) 2 = 87.6*3 + 74.9*2 + 16*8

    = 540.6 g/mol

    Molarity (X) = 0.059 g/L * 1 mol / 540.6 g/mol

    = 1.1 x 10^-4 moles

    When the solubility equation is:

    Sr3 (ASO4) 2 ↔ 3Sr + + (aq) + 2ASO-3 (aq)

    so, Ksp = [Sr++]^3[ASO-3]^2

    from ICE table and the balanced equation:

    [Sr++] = 3 X

    = 3 * 1.1 x 10^-4 = 3.3x10^-4 M

    [ASO-3] = 2X

    = 2 * 1.1 x 10^-4 = 2.2 x 10^-4 M

    So, by substitution:

    ∴Ksp = (3.3 x 10^-4) ^3 * (2.2 x 10^-4) ^2

    = 1.74 x 10^-18
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