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Using Ksp to find the concentration

  1. Sep 25, 2011 #1
    1. The problem statement, all variables and given/known data
    0.1100 mol AgNO3 translated into 500 mL of a solution containing 0.1000 moles of NaCl and NaBr 0.1000 moles. What are the concentrations of Ag+, Cl-, Br-, after equilibrium has occurred?

    Solubility product for AgCl: Ksp(AgCl) = 1,82*10^-10
    Solubility product for AgBr: Ksp(AgBr) = 5,0*10^-13

    2. Relevant equations


    3. The attempt at a solution

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    Is there anybody, who can help me with this. Which equations do I have to use?
    I am lost with this assignment.
     
  2. jcsd
  3. Sep 25, 2011 #2

    Borek

    User Avatar

    Staff: Mentor

    You will need formulas for both solubility products and mass balances.

    What will precipitate first? How much of that salt can precipitate? (hint: limiting reagent).
     
  4. Sep 25, 2011 #3
    I have made the task. Delete the topic, thanks ! :-)
     
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