If the solubility of a sparingly soluble salt of the type $BA_2$ (giving three ions on dissociation of a molecule) is $x \ mol \ L^{-1}$,then its solubility product is given by

The saturated solution of $Ag_2SO_4$ is $2.5 \times 10^{-2} \ M$. Its solubility product $(K_{sp})$ is

If the solubility product of $CaSO_4$ is $2.5 \times 10^{-5}$,then its solubility will be .......

For the precipitation reaction of $Ag^{+}$ ions with $NaCl$,which of the following statements is correct?

Which one of the following is most soluble?

Using the Gibbs energy change,$\Delta G^{o} = +63.3 \ kJ \ mol^{-1}$,for the following reaction in water at $25 \ ^{\circ}C$,calculate the solubility product constant $(K_{sp})$:
$Ag_{2}CO_{3(s)} \rightleftharpoons 2Ag^{+}_{(aq)} + C{O_{3}}^{2-}_{(aq)}$
$(R = 8.314 \ J \ K^{-1} \ mol^{-1})$