The `K_(sp)` of `Ag_(2)CrO_(4)` is `1.1xx10^(-12)` at `298K`. The solubility (in mol/L) of `Ag_(2)CrO_(4)` in a `0.1 M AgNO_(3)` solution is

Options

A. `1.1 xx 10^(-11)`
B. `1.1 xx 10^(-10)`
C. `1.1 xx 10^(-12)`
D. `1.1 xx 10^(9)`

Answer

B

Explanation

`Ag_(2)CrO_(4) underset((0.1"from"AgNO_(3)))underset(2s+0.1)(2Ag^(+))+CrO_(4)^(2-)`
`=0.1 M `(as s is negligible as compared 0.1 )
`K_(sp)=|Ag^(+)|^(2)[CrO_(4)^(2-)]`
`1.1 xx 10^(-12)=(0.1)^(2) xx s `or `s =1.1 xx 10^(-10)M`