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Question
100 mL of a clear saturated solution of Ag2SO4 is added to 250 mL of a clear saturated solution of PbCrO4. What is the precipitate formed? Given, Ksp values for Ag2SO4,Ag2CrO4,PbCrO4 and PbSO4 are 1.4×10−5, 2.4×10−12, 2.8×10−13 and 1.6×10−5 respectively.
100 mL of a clear saturated solution of Ag2SO4 is added to 250 mL of a clear saturated solution of PbCrO4. What is the precipitate formed? Given, Ksp values for Ag2SO4,Ag2CrO4,PbCrO4 and PbSO4 are 1.4×10−5, 2.4×10−12, 2.8×10−13 and 1.6×10−5 respectively.
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Solution
The correct option is A Ag2CrO4 will precipitate
For Ag2SO4(s)⇌2Ag+(aq)2S+SO2−4S(aq)
Ksp=4s3 or s=3√Ksp4=3√1.4×10−54=1.52×10−2 M
For PbCrO4(s)⇌Pb2+(aq)+CrO2−4(aq)
Ksp=st2 or S1=√Ksp=√2.8×10−13=5.29×10−7 M
In solution, concentration of each ion can be given as:
Thus, [Ag+]=2s×100350=2×1.52×10−2×100350=0.869×10−2 M
[SO2−4]=s×100350=1.52×10−2×100350=0.43×10−2 M
[Pb2+]=s1×250350=5.29×10−7×250350=3.78×10−7 M
[CrO2−4]=s1×250350=5.29×10−7×250350=3.78×10−7 M
It is thus evident that,
[Ag+]2[CrO2−4]=(0.869×10−2)2×(3.78×10−7)=2.85×10−11(>Ksp Ag2CrO4)
Thus Ag2CrO4 will precipitate.
For Ag2SO4(s)⇌2Ag+(aq)2S+SO2−4S(aq)
Ksp=4s3 or s=3√Ksp4=3√1.4×10−54=1.52×10−2 M
For PbCrO4(s)⇌Pb2+(aq)+CrO2−4(aq)
Ksp=st2 or S1=√Ksp=√2.8×10−13=5.29×10−7 M
In solution, concentration of each ion can be given as:
Thus, [Ag+]=2s×100350=2×1.52×10−2×100350=0.869×10−2 M
[SO2−4]=s×100350=1.52×10−2×100350=0.43×10−2 M
[Pb2+]=s1×250350=5.29×10−7×250350=3.78×10−7 M
[CrO2−4]=s1×250350=5.29×10−7×250350=3.78×10−7 M
It is thus evident that,
[Ag+]2[CrO2−4]=(0.869×10−2)2×(3.78×10−7)=2.85×10−11(>Ksp Ag2CrO4)
Thus Ag2CrO4 will precipitate.
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