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Concentrations of Pb2+ and Cl2 at equilibrium

  1. Nov 9, 2008 #1
    1. The problem statement, all variables and given/known data
    A solution is prepared by mixing 50.0 mL of 0.36 M Pb(NO3)2 with 50.0 mL of 1.7 M KCl. Calculate the concentrations of Pb2+ and Cl2 at equilibrium. Ksp for PbCl2(s) is 1.6 x 10-5.

    2. Relevant equations
    I think its Ksp = [Pb(NO3)2][KCl]2

    Pb(NO3)2 = 0.018 mol
    KCl = 0.085 mol

    Is this right? what do i solve for?
  2. jcsd
  3. Nov 9, 2008 #2


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    Staff: Mentor

    Re: Solubility

    Your Ksp is wrong. It should be made of ions concentrations.

    Otherwise it is limiting reagent question. Once everything precipitates out, you will be left with the excess of one of the ions involved. Use this concentration to calculate concentration of the other using (correct) Ksp formula.
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