The `K_(sp)` of `AgCI` at `25^(@)C` is `1.5 xx 10^(-10)`. Find the solubility (in `g^(-1)L^(-1))` in an aqueous solution containing `0.01M AgNO_(3)`.

Explanation

`AgNO_(3)` is completely ionised. Due to common ion`(Ag^(o+))`, the dissociation of `AgCI` is supressed and hence, the solubility decreases.
Since `K_(sp)` is small, `S lt lt 0.01M`.
Thus, `(0.01 +S) ~~ 0.01`.
[For uni-univalent salt]
`S_(new) = (K_(sp))/((C)^(n)) = (1.5 xx 10^(-10))/((0.01)^(1)) = 1.5 xx 10^(-8)M`
`= 1.5 xx 10^(-8) xx 143.5`
`= 2.15 xx 10^(-6)gL^(-1)`
The solubility of `AgCI` in water contianing `Ag^(o+)` (a common ions) is much less than that in pure water.