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Question

# If 100 mL of 0.002 M AgNO3 solution is mixed with 100 mL of 0.05 M K2CrO4 solution. Then, select the correct option regarding the precipitation of Ag2CrO4 . Given : Ksp of Ag2CrO4=1.1×10−12.

A
Precipitation occurs
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B
Precipitation does not occur
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C
Can't be determined from given data
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D
None of these
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Solution

## The correct option is A Precipitation occurs Final volume of the solution =100+100=200 mL To calculate [Ag+] using the formula: M1V1=M2V2 0.002 M×(100 mL)=M2×(200 mL) [Ag+]=0.001 M Calculate [CrO2−4] using the formula: M1V1=M2V2 0.05 M×(100 mL)=M2×(200 mL) [CrO2−4]=0.025 M Ionic product for Ag2CrO4 solution : Ag2CrO4(s)⇌2Ag+(aq)+CrO2−4(aq) Ionic product =[Ag+]2[CrO2−4] =(1.0×10−3)2(2.25×102−) =2.25×10−8 Ionic product >Ksp ∴ precipitation occurs.

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