On addition of AgNO3 slowly to 0.1 M each of NaCl and NaBr in a solution, what percentage of Br− ions get precipitated when Cl− ion starts precipitating ? KSP(AgCl)=1.0×10−10KSP(AgBr)=1×10−13
A
0.11
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B
99.9
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C
0.01
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D
9.99
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Solution
The correct option is B99.9 For precipitation of AgCl, [Ag+] required=KSP(AgCl)[Cl−]=1.0×10−100.1=1.0×10−9M [Br−]left=KSP(AgBr)[Ag+]=1.0×10−131.0×10−9=1.0×10−4M % of remaining, [Br−]=1.0×10−40.1×100=0.1 % of [Br−] which get precipitated =100−0.1=99.9