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Constant of Solubility

  1. Dec 2, 2013 #1

    Qube

    User Avatar
    Gold Member

    1. The problem statement, all variables and given/known data

    A saturated solution of iron(II) hydroxide has a molar solubility of 3.65 x 10^-6 M. Calculate the Ksp for Fe(OH)2.

    2. Relevant equations

    Ksp = [A]^a^b

    3. The attempt at a solution

    Fe(OH)2 --> Fe^2+ + 2OH-

    Ksp = [3.65 x 10^-6 M] * (2*[3.65 x 10^-6 M])^2

    This, however, doesn't yield an answer. The professor's answer is equivalent to

    [3.65 x 10^-6 M] * ([3.65 x 10^-6 M])^2

    I'm assuming this is an error on his part because the concentration of hydroxide ions should be twice the concentration of iron ions, not the same.
     
  2. jcsd
  3. Dec 3, 2013 #2

    Borek

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    Staff: Mentor

    Your approach is the correct one.
     
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