Using Ksp to find the concentration

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SUMMARY

The discussion focuses on calculating the concentrations of Ag+, Cl-, and Br- ions after equilibrium in a solution containing 0.1100 mol of AgNO3 mixed with 0.1000 moles each of NaCl and NaBr. The solubility products are given as Ksp(AgCl) = 1.82 x 10-10 and Ksp(AgBr) = 5.0 x 10-13. The key to solving the problem involves using the solubility product equations and mass balance principles to determine which salt precipitates first and the extent of precipitation based on the limiting reagent.

PREREQUISITES
  • Understanding of solubility product constants (Ksp)
  • Knowledge of mass balance equations in chemical equilibria
  • Familiarity with precipitation reactions
  • Basic concepts of limiting reagents in chemical reactions
NEXT STEPS
  • Study the calculation of ion concentrations in saturated solutions using Ksp
  • Learn about the principles of precipitation and solubility equilibria
  • Explore mass balance equations in the context of chemical reactions
  • Investigate the concept of limiting reagents in stoichiometry
USEFUL FOR

Chemistry students, educators, and anyone involved in analytical chemistry or chemical equilibrium studies will benefit from this discussion.

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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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