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Question

Solid AgNO3 is added to a solution which is 0.1 M in Cl and 0.1 M in CrO24. If Ksp values for AgCl and Ag2CrO4 solutions are 1.7×1010 and 1.9×1012 respectively. Find the minimum concentration of Cl when Ag2CrO4 starts precipitating.

A
1.1×107 M
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B
2.1×108 M
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C
3.9×105 M
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D
5.1×109 M
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Solution

The correct option is C 3.9×105 M
The concentration of Ag+ required to precipitate AgCl and Ag2CrO4 can be calculated as follows:
Ksp(AgCl)=[Ag+][Cl][Ag+]=1.7×10100.1=1.7×109 M.
To precipitate Ag+ in Ag2CrO4 :
Ksp(Ag2CrO4)=[Ag+]2[CrO24][Ag+]=1.9×10120.1=4.35×106 M.
Since [Ag+] required to precipitate AgCl is less than that required to precipitate Ag2CrO4, AgCl will precipitate first.
Now since [Ag+]=4.35×106 M when Ag2CrO4 starts precipitating, [Cl] at that state can be calculated as follows:
Ksp(AgCl)=[Ag+][Cl]1.7×1010=(4.35×106)[Cl][Cl]=3.9×105 M

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