A solution which remains in equilibrium with undissolved solute is said to be saturated. The concentration of a saturated solution at a given temperature is called solubility. The product of concentration of ions in a saturated solution of an electrolyte at a given temperature, is called solubility product `(K_(sp))`. For the electrolyte, `A_(x),B_(y),:A_(x),B_(y(s)) rarr xA^(y+)+ y^(Bx-)`, with solubility S, the solubility product `(K_(sp)) =x^(x)xxy^(y) xx s^(x+y)`. While calculating the solubility of a sparingly soluble salt in the presence of some strong electrolyte containing a common ion, the common ion concentration is practically equal to that of strong electrolyte. If in a solution, the ionic product of an clectrolyte exceeds its `K_(sp)`, value at a particular temperature, then precipitation occurs.
The solubility of `PbSO_(4)`, in water is 0.303 g/l at `25^(@)`C, its solubility product at that temperature is

Options

A. ` 10^(-4) M^(2) `
B. ` 9.18 xx 10^(-4) M`
C. ` 10^(-6) M^(2)`
D. ` 9.18 xx 10^(-8) M^(2)`

Answer

C

Explanation

` S = 0.303 g // lit `
` Mol . wt = 207 + 32 + 64 =303 `
moles ` =( 0.303)/( 303) =10 ^(-3) `
` S = 10 ^(-3) " mole " // "lit"`
` pbSO_4 hArr Punderset(S) b^(+2) +Sunderset( S) O ^(-2) , S =10 ^(-3) `
` K_(sp) = ( 10 ^(-3) M)^(2) =10 ^(-6) M^(2) `