The solubility of silver bromide is `7.7 xx 10^(-13) mol^(2) L^(-2).` Calculate the solubility of the salt.

Explanation

AgBr dissolves in water according to the following equilibrium :
`AgBr (s) overset(aq)(hArr) Ag^(+) (aq) + Br^(-) (aq)`
Let the solubility of the salt in water be S
`[Ag^(+)(aq)] =S and [Br^(-) (aq)] = S`
`K_(sp) =[Ag^(+) (aq)] [ Br^(-) (aq)]`
`7.7 xx 10^(-13) mol^(2) L^(-2) =S xx S`
`S=(7.7 xx 10^(-13) mol^(2) L^(-2))^(1//2)`
`=8.77 xx 10^(-7) mol L^(-1).`