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Question

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


Ag2CrO4 is a weak electrolyte and will clearly ionize to a small extent compared to the strong electrolyte AgNO3, which will complete dissociate into Ag+ and NO3 ions. So the majority concentration of - in fact, for all practical purposes - comes from AgNO3. Hence, for the calculation,
[Ag+]=0.1 M
Ksp=[Ag+]2[CrO24]=(0.1)2 (s)
Solving, s=1.1×1010


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