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Question

A solution contains 0.1M Cl and 0.001M CrO24. If solid AgNO3 is gradually added to this solution, which will precipitate first, AgCl or Ag2CrO4? Assume that the addition causes no change in volume. Given
KspAgCl=1.7×1010M2
KspAg2CrO4=1.79×1012M3
What percent of Cl remains in the solution when CrO24 starts precipitating?

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Solution

Ag+ ion concentration required for precipitation
For AgCl:
[Ag+]=KspAgCl[Cl]=1.7×10100.1=1.7×109M
For Ag2CrO4:
[Ag+]2=KspAg2CrO4[CrO24]=1.79×1012[0.001]
[Ag+]=[1.79×109M2]1/2=4.23×105M
AgCl will precipitate first because it required low conc. of Ag+
Remaining conc. of [Cl]=KspAgCl[Ag+]=1.7×10104.23×105=4.01×106M
% Remaining conc. of [Cl]=4.01×1060.1×100=4×103%

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