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Calucating the solubility product of Silver Chloride

  1. Apr 16, 2012 #1
    1. The problem statement, all variables and given/known data
    A sample of AgCl was treated with 5ml of 2M Na2CO3 solution to produce Ag2CO3. The remaining solution contained 0.003 g of Cl- per litre. Calculate the solubility product of AgCl.(Ksp of Ag2CO3 = 8.2 ×10-12)

    2. Relevant equations
    ksp of AgCl = [Ag+]×[Cl-]
    ksp of Ag2CO3 = [2Ag+]2×[CO3--]



    3. The attempt at a solution

    I couldn't think of any idea. So, entered this forum. Please help.
     
  2. jcsd
  3. Apr 16, 2012 #2

    Borek

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    Staff: Mentor

    Can you calculate concentration of Cl-?

    There was a huge excess of carbonate. Did it concentration change much?
     
  4. Apr 16, 2012 #3
    Yes. I calculated the concentration by dividing gm/litre by 35.5 to give molarity. But, I don't know where to go beyond.
     
  5. Apr 17, 2012 #4

    Borek

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    Staff: Mentor

    I asked you a question, have you tried to answer it?
     
  6. Apr 17, 2012 #5
    I don't know how to start.
     
  7. Apr 17, 2012 #6

    Borek

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    Staff: Mentor

    Try to describe what is happening in the solution when the carbonate is added.
     
  8. Apr 17, 2012 #7
    I tried this:
    Ksp of Ag2CO3 = [2xSolub.]2x[Solub.]
    => Solubility = 1.270334x10-4 = [Ag+]
    Now,
    [Cl-]=0.003/35.5 M = 8.45 x 10-5
    Ksp of AgCl = 1.270334x10-4 x 8.45 x 10-5 = 1.073 X 10-8.

    Why was concentration and volume of Na2CO3 was given if this is correct?
     
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