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Question

15 mL of 0.05 M AgNO3 is mixed with 45 mL of 0.03 M K2CrO4. Then, which of the following is correct regarding Ag2CrO4 . Ksp of Ag2CrO4=1.9×1012.
  1. Precipitation  does not occur
  2. Can't be determined from given data 
  3. Precipitation occurs 
  4. None of these


Solution

The correct option is C Precipitation occurs 
Final volume=15+45=60 mL=0.06 L

Using these volume finding out the final concentrations:
c=molevolume in L
[Ag+]=0.015×0.050.060=1.25×102 M

[CrO4]=0.045×0.030.060=2.25×102 M

Ionic product for Ag2CrO4
Ag2CrO4(s)2Ag+(s)+CrO24(s)

Ionic product =[Ag+]2[CrO24]
=(1.25×102)2(2.25×102)
=3.51×106

Ionic product >Ksp
precipitation occurs. 

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