`Ag_(2)SO_(4) and SrSO_(4)` are shaken up with pure water. Calculate the concentration of `Ag^(+) and Sr^(2+)` in mole/litre in the resulting saturated solution. `K_(sp) (Ag_(2)SO_(4))=1.5 xx 10^(-5), K_(sp) (SrSO_(4))=2.8 xx 10^(-7)`

Explanation

From the `K_(sp)` data, it is clear that `SO_(4)^(2-)` are mainly produced by `Ag_2SO_4` because `K_(sp) (Ag_2SO_4)` is much greater than `K_(sp) (SrSO_4) and K_(sp) (Ag_2SO_4)` is the product of three ion concentrations.
Let `[SO_(4)^(2-)]="S for "Ag_(2)SO_4`
`K_(sp) (Ag_(2)SO_(4))=(2S)^2 S=1.5 xx 10^(-5)`
`S=1.55 xx 10^(-2)`
`[Ag^(+)]=2S=3.1 xx 10^(-2)`,
And for `SrSO_(4), K_(sp)=[Sr^(2+)] [SO_(4)^(2-)]`
`2.8xx 10^(-7)=[Sr^(2+)] (1.55 xx 10^(-2))`
`[Sr^(2+)]=1.8 xx 10^(-5)`