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Solubility Product Constant (Ksp) Problem

  1. Jul 5, 2014 #1
    5g of AuBr3 (Ksp = 4.0 x 10^-36) are placed in 25 ml of water, how many grams of Au ions are dissolved in the 25 ml?

    My instructor used the conversion factor (6.2 x 10^-10 mol Au ions) to get from 25 ml H2O to grams Au. I believe the conversion from ml of H2O to grams of Au is: 25ml H2O x (6.2 x10^-10 mol Au / 1000ml) (197 g Au / 1 mol Au) = 3.05 x 10^-9 g Au.
    I'm confused about the conversion factor 6.2 x 10^-10 though, can anyone explain to me where this number comes from? Thank you.
     
  2. jcsd
  3. Jul 5, 2014 #2

    Borek

    User Avatar

    Staff: Mentor

    Use Ksp given to calculate molar solubility of AuBr3.
     
  4. Jul 25, 2014 #3
    Remember that Ksp for a compound AxBy equals [Ion of A]x[Ion of B]y.
     
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