The solubility product of a soluble salt `A_(x)B_(y)` is given by : `K_(sp)=[A^(y+)]^(z)[B^(x-)]^(y)`. As soon as prodcut of concentration of `A^(y+)` and `B_(x-)`. Becomes more than its `K_(sp)`, the salt starts precipitation. It may practically be noticed that AgCI is more soluble in water and its solubility decreases dramatically in 0.1m NaCI or 0.1 m `AgNO_(3)` solution. It can be concluded that in presence of a common ion the solubility 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. `0.02MCaCI_(2)+0.0004MNa_(2)SO_(4)`
B. `0.01MCaCI_(2)+0.0004MNa_(2)SO_(4)`
C. `0.02MCaCI_(2)+0.0002MNa_(2)SO_(4)`
D. `0.03MCaCI_(2)+0.0002MNa_(2)SO_(4)`