A solution has 0.1 M in each KCl, KBr and K2CrO4 and to this solution – InterviewSolution

1.	A solution has 0.1 M in each KCl, KBr and K2CrO4 and to this solution solid AgNO3 is gradually added. Assume there is no change in the volume of the solution given: Ksp(AgCl)=1.7×10−10 Ksp(AgBr)=5.0×10−13 and Ksp(K2CrO4)=1.9×10−12 The concentration of [Ag+] required to start the precipitation of AgBr is:
Answer» A solution has 0.1 M in each KCl, KBr and $K_{2} C r O_{4}$ and to this solution solid $A g N O_{3}$ is gradually added. Assume there is no change in the volume of the solution given: $K s p (A g C l) = 1.7 \times 10^{- 10}$ $K s p (A g B r) = 5.0 \times 10^{- 13} a n d K s p (K_{2} C r O_{4}) = 1.9 \times 10^{- 12}$ The concentration of $[A g^{+}]$ required to start the precipitation of AgBr is:

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