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2 January, 01:42

What is the remaining concentration of the cation that precipitates first, when the other cation just begins to precipitate? consider a solution that is 2.3*10-2 m in fe2 + and 2.0*10-2 m in mg2+?

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  1. 2 January, 03:39
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    Ksp for FeCO₃ is 3.07 x 10⁻¹¹

    Ksp for MgCO₃ is 6.82 x 10⁻⁶

    So Fe²⁺ will precipitated first as solubility product of FeCO₃ is lower than solubility product of MgCO₃

    Ksp FeCO₃ = [Fe²⁺][CO₃²⁻]

    3.07 x 10⁻¹¹ = (2.3 x 10⁻²) [CO₃²⁻]

    [CO₃²⁻] = 1.33 x 10⁻⁹ M to precipitate Fe²⁺ ions

    Ksp MgCO₃ = [Mg²⁺][CO₃²⁻]

    6.82 x 10⁻⁶ = (2.0 x 10⁻²) [CO₃²⁻]

    [CO₃²⁻] = 3.4 x 10⁻⁴ M to precipitate the Mg²⁺ ions

    Ksp FeCO₃ = [Fe²⁺][CO₃²⁻]

    3.07 x 10⁻¹¹ = [Fe²⁺] (3.4 x 10⁻⁴)

    [Fe²⁺] = 9 x 10⁻⁸ M when Mg²⁺ ions precipitate
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