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A saturated solution of Mg(OH)2 is prepared having a large excess of Mg(OH)2. Sn(NO3)2 is added to the solution. Ksp = 1.9 x 10^-11 for Mg(OH)2 and Ksp = 6.0x10^-26 for Sn(OH)2.

What [Sn2+] is required so that the [Mg2+] in solution will be 0.15 M?

  • Chemistry -

    I would do this.
    (Mg^+2)(OH^-)^2 = 1.9E-11
    Plug in 0.15 for Mg and solve for (OH^-)^2.

    Then (Sn^+2)(OH^-)^2 = 6.0E-26
    Plug in (OH^-)^2 from above and solve for (Sn^+2)

  • Chemistry -

    Thanks, I got it right!

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