The solubility product of a soluble salt `A_(x)B_(y)` is given by: `K_(SP)= [A^(y+)]^(x) [B^(x-)]^(y)`. As soon as the product of concentration of `A^(y+)` and `B^(x-)` increases than its `K_(SP)`, the salt start precipitation. It may practically be noticed that AgCI is more soluble in water and its solublity decreases dramatically in `0.1M NaCI` or `0.1M AgNO_(3)` solution. It may therefore be conncluded that in presence of a common ion, the solubiolity of salt decreases.

Equal volumes of two solutions are mixed. The one in which `CaSO_(4) (K_(SP)= 2.4xx10^(-5))` is precipitated, is :

A. `0.02M CaCI_(2)+0.0004M Na_(2)SO_(4)`

B. `0.01M CaCI_(2)+0.0004M Na_(2)SO_(4)`

C. `0.02M CaCI_(2)+0.0002M Na_(2)SO_(4)`

D. `0.03M CaCI_(2)+0.004M Na_(2)SO_(4)`