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

`E_(cell)=0.059/1 "log"([Ag^(+)]_(RHS))/([Ag^(+)]_(LHS))`
`0.164=0.059/1"log" 0.1/([Ag^(+)]_(LHS))`
or `[Ag^(+)]_(LHS)=1.66xx10^(-4) M`
So, `[CrO_(4)^(2-)]=(1.66xx10^(-4))/2`
`K_(sp(Ag_(2)CrO_(4)))=[Ag^(+)]^(2) [CrO_(4)^(2-)]`
`=(1.66xx10^(-4))^(2) ((1.66xx10^(-4))/2)`
`=2.287xx10^(-12) mol^(3) L^(-3)`