The solubility product of $BaSO_4$ is $1.5 \times 10^{-9}$. The precipitation in a $0.01 \ M \ Ba^{2+}$ solution will start,on adding $H_2SO_4$ of concentration:

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 $(K_{sp})$:
$Ag_{2}CO_{3(s)} \rightleftharpoons 2Ag^{+}_{(aq)} + C{O_{3}}^{2-}_{(aq)}$
$(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

When equal volumes of the following solutions are mixed,precipitation of $AgCl$ will occur in - ($K_{sp}$ of $AgCl = 1.8 \times 10^{-10}$)

Solubility products of $CuI$ and $Ag_{2}CrO_{4}$ have almost the same value $(\sim 4 \times 10^{-12})$. The ratio of solubilities of the two salts $(CuI : Ag_{2}CrO_{4})$ is closest to $....$

The solubility of a sparingly soluble salt $AB_2$ in water is $1.0 \times 10^{-5} \ mol \ L^{-1}$. Its solubility product is .......?

The solubility product of $AgCl$ is $4.0 \times 10^{-10}$ at $298 \ K$. The solubility of $AgCl$ in $0.04 \ m \ CaCl_2$ will be