The solubility of $PbI_2$ at $25\,^{\circ}C$ is $0.7\, g\, L^{-1}$. The solubility product of $PbI_2$ at this temperature is (molar mass of $PbI_2 = 461.2\, g\, mol^{-1}$)

If the solubility product of $PbS$ is $3.4 \times 10^{-28}$,what is the minimum concentration of sulfide ions required to precipitate $PbS$ from a $0.001 \ M \ Pb^{2+}$ solution?

The $K_{sp}$ of $Ag_2CrO_4$ is $1.1 \times 10^{-12}$ at $298 \ K$. The solubility (in $mol/L$) of $Ag_2CrO_4$ in a $0.1 \ M \ AgNO_3$ solution is

The solubility product of $M(OH)_2$ is $10^{-14}$. What will be the concentration of $M^{+2}$ in a $0.1 \, M$ solution of $NH_4OH$,if $NH_4OH$ is $10\%$ ionized?

What is the correct representation of the solubility product of $Ag_2CrO_4$?

Determine the solubilities of silver chromate,barium chromate,ferric hydroxide,lead chloride,and mercurous iodide at $298 \, K$ from their solubility product constants. Determine also the molarities of individual ions. (Given $K_{sp}$ values: $Ag_{2}CrO_{4} = 1.1 \times 10^{-12}$,$BaCrO_{4} = 1.2 \times 10^{-10}$,$Fe(OH)_{3} = 1.0 \times 10^{-38}$,$PbCl_{2} = 1.6 \times 10^{-5}$,$Hg_{2}I_{2} = 4.5 \times 10^{-29}$)