Find the solubility product of a saturated solution of `Ag_(2)CrO_(4)` in water at `298K`, if the `EMF` of the cell `:`
`Ag|Ag^(o+)(satAg_(2)CrO_(4)sol)||Ag(0.1M)|Agis 0.164V` at `298K`.

Explanation

The cell is `Ag|Ag^(+)(c_(1))||Ag^(+)(0.1M)|Ag`
`E_(cell)=(0.0591)/(n)"log"(c_(2))/(c_(1))` (for concentration cell)
`0.164=(0.0591)/(1)"log"(0.1)/(c_(1))` or log`(0.1)/(c_(1))=2.7750` or `0.1//c_(1)=5.957xx10^(2)` o `c_(1)=1.679xx10^(-4)`
i.e., `[Ag^(+)]` in saturated `Ag_(2)CrO_(4)` sol.=`1.679xx10^(-4)M`
`Ag_(2)CrO_(4)hArr2Ag^(+)+CrO_(4)^(2-)`
`[Ag^(+)]=1.679xx10^(-4)M,[CrO_(4)^(2-)]=([Ag^(+)])/(2)=(1.679xx10^(-4))/(2)M`
`K_(sp)=[Ag^(+)]^(2)[CrO_(4)^(2-)]=(1.679xx10^(-4))^(2)xx((1.679xx10^(-4))/(2))=2.37xx10^(-12)`.