If the solubility product of silver chloride is `1.8xx10^(-10)`. What is the solubility of silver ion if concentration of `Cl^(-)` is 0.01 molar.

Explanation

`K_(sp)=[Ag^(+)][Cl^(-)]" "1.8xx10^(-10)=[Ag^(+)]0.01`
`[Ag^(+)]=(1.8xx10^(-10))/(0.01)=180xx10^(-10)=1.8xx10^(-8)"mol"//dm^(3)`