Chemistry

Calculate the molar solubility of calcium phosphate [Ca3(PO4)2 in a solution which is 0.10M in sodium phosphate (Na3PO4). Ksp for calcium phosphate is 1.1x10^-26

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  1. ................Ca3(PO4)2 ==> 3Ca^2+ + 2[PO4]^3-
    I...............solid.....................0...................0
    C..............solid.....................3x.................2x
    E................solid...................3x..................2x

    Then Na3PO4 is completely (100%) ionized
    .............Na3PO4==> 3Na^+ + [PO4]^3-
    I............0.1 M..............0...............0
    C...........-0.1...............0.3............0.1
    E.............0.0............0.3...............0.1
    Ksp = 1.1E-26 = (Ca^2+)^3[(PO4)^3-]^2
    Ca^2+ is 3x from the Ca3(PO4)2
    [PO4]^3- is 2x from the Ca3PO4)2 + 0.1 for the Na3PO4 for a total of 2x + 0.1
    so Ksp = 1.1E-26 = (3x)^3(2x + 0.1)^2
    Solve for x and that gives you the molar solubility of Ca3(PO4)2
    Post your work if you get stuck. I think you can ignore the 2x in 2x+0.1. Try it at least and see if you can because it will simplify the math.

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    DrBob222

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