Q. A saturated solution of $Ag_{2}SO_{4}\ is\ 2.5 \times 10^{- 2}\ M$. The value of its solubility product is
A) $62.5 \times 10^{- 6}$
B) $6.25 \times 10^{- 4}$
C) $15.625 \times 10^{- 6}$
D) $3.125 \times 10^{- 6}$
Explanation
(a)
$Ag_{2}SO_{4} \rightarrow 2{Ag}^{+} + {SO}_{4}^{2 -}$
$Ag_{2}SO_{4}$ is a $2:1$ type electrolyte $i.e$., it gives two ${Ag}^{+}$ ions and one ${SO}_{4}^{2 -}$ion on ionisation.
Given, $s = 2.5 \times 10^{- 2}\ M$
Hence, its $K_{sp} = 4s^{3}$
(where, $s =$ molar solubility)
$K_{sp} = 4\left( 2.5 \times 10^{- 2} \right)^{3}$
$= 4 \times 15.63 \times 10^{- 6}$
$= 62.5 \times 10^{- 6}$
Reviewed by Dr. Abubacker
Physics Educator & NEET/JEE Specialist
Ph.D. in Physics with 19+ years of teaching experience.