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.
Which of the following statements wrong?

Options

A. `K_(sp)` of salt depends upon temperature
B. `K_(sp)`of a salt has no units
C. The `K_(sp)` of salt, `A_(x)B_(y)` can be given as :`x^(x)y^(y)(s)^(x+y)` where s is the mole/litre solubility of salt.
D. Solubility of `BaF_(2)` in a solution of `Ba(NO_(3))_(2)` can be given by `(1)/2[F^(-)]`.

Answer

b