The molar solubility of $PbI_2$ in $0.2 \ M \ Pb(NO_3)_2$ solution in terms of $K_{sp}$ (solubility product) is

The solubility of $BaCl_2$ is $4 \times 10^{-6} \ M$. Calculate its $K_{sp}$. Also,find its new solubility in the presence of $10^{-2} \ M \ Ba(OH)_2$.

The solubility product of $As_2S_3$ is $2.8 \times 10^{-72}$. What is the solubility of $As_2S_3$?

$PbCl_2$ has a maximum concentration of $1.0 \times 10^{-3} \ M$ in its saturated aqueous solution at $25 \ ^oC$. Its solubility in a $0.1 \ M \ NaCl$ solution will be:

Concentration of $H_2SO_4$ and $Na_2SO_4$ in a solution is $1 \ M$ and $1.8 \times 10^{-2} \ M$,respectively. Molar solubility of $PbSO_4$ in the same solution is $X \times 10^{-Y} \ M$ (expressed in scientific notation). The value of $Y$ is. . . .
[Given: Solubility product of $PbSO_4$ $(K_{sp})=1.6 \times 10^{-8}$. For $H_2SO_4$,$K_{a1}$ is very large and $K_{a2}=1.2 \times 10^{-2}$]

Precipitation of $CaF_2$ $(K_{sp} = 1.7 \times 10^{-10})$ occurs when equal volumes of which of the following are mixed?