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Question

The Ksp of Ag2CrO4 is 1.1 × 1012 at 298K. The solubility (in mol/L) of Ag2CrO4 in a 0.1 M AgNO3 solution is

A
1.1×1011
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B
1.1×1010
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C
1.1×1012
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D
1.1×109
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Solution

The correct option is B 1.1×1010
PLAN In presence common ion (in this case Ag+ ion) solubiility of sparingly soluble salt is decreased.

Let solubility of Ag2CrO4 in presence of 0.1 M
AgNO3=x
Ag2CrO42Ag++CrO24
AgNO3Ag+0.1+NO30.1
Total [Ag+] = (2x + 0.1) M 0.1 M
as x <<< 0.1 M
[CrO24]=xM
Thus, [Ag+]2[CrO24]=Ksp
(0.1)2(x)=1.1×1012
x=1.1×1010M

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