Using Ksp to find the concentration

AI Thread Summary
The discussion revolves around calculating the concentrations of Ag+, Cl-, and Br- in a solution after equilibrium, given the solubility products for AgCl and AgBr. Participants emphasize the need to apply the solubility product equations and mass balance principles to determine which salt will precipitate first and the amount that can precipitate based on the limiting reagent. The original poster expresses confusion about the assignment and seeks guidance on the necessary equations. Ultimately, the topic was resolved, and the poster requested to delete the thread.
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Homework Statement


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

Homework Equations




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.
 
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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).
 
I have made the task. Delete the topic, thanks ! :-)
 
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