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Silver chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12× 10–12. What is the solubility (in mol/L) of silver chromate in 1.00 M potassium chromate aqueous solution?

  • chemistry -

    This is an example of the common ion effect. The common ion in this case is CrO4^2- from K2CrO4.
    ............Ag2CrO4 ==> 2Ag^+ + CrO4^2-
    solubility.....x........2x.........x

    .......K2CrO4 ==> 2K^+ + CrO4^2-
    initial..1M.........0......0
    change...-1M........1M.....1M
    equil.....0.........1M.......1M

    Ksp Ag2CrO4 = (Ag^+)^2(CrO4^2-)
    (Ag^+) = 2x from Ag2CrO4--see chart above.
    (CrO4^2-) = x from Ag2CrO4 + 1M from K2CrO4
    Substitute into Ksp expression and solve for x.
    Post your work if you get stuck.

  • chemistry -

    I got to 4x^3 + 6x^2=1.12x10^-12 (my moles of potassium chromate is 1.5 instead of 1) but now I'm stuck

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