At $25\,^oC\,,\, K_{sp}$ for $PbBr_2$ is equal to $8 \times 10^{-5}$ . If the salt is $80\%$ dissociated, what is the solubility of $PbBr_2$ in $mol/litre$ ?

${K_{sp}}$ of $Pb$ $I_{2}$ is $ 1.4 \times {10^{ – 8}}$. The molecular mass of $Pb$ $I_{2}$ is $461$ $g$ $mol^{-1}$ Then molecular mass of $Pb{\left( {N{O_3}} \right)_2}$ is $331.9$ $mol^{-1}$ So, $(a)$ In $500$ $mL$ water $(b)$ $500$ $mL$ $0.10$ $M$ $KI$ $(c)$ What is the weight of $PbI_{2}$ when soluble in $1.33$ $g$ $Pb{\left( {N{O_3}} \right)_2}$ containing $500$ $mL$ solution ?

What is the $pH$ of a saturated solution of $Cu(OH)_2$ ? $(K_{sp} = 4.0 \times 10^{-6}$ )

The $K _{ sp }$ for bismuth sulphide $\left( Bi _{2} S _{3}\right)$ is $1.08 \times 10^{-73}$. The solubility of $Bi _{2} S _{3}$ in $mol \,L ^{-1}$ at $298 \,K$ is ……

What would be the concentration of ${H_2}S{O_4}$ necessary to precipitate $BaS{O_4}$ from a solution of $0.01\,M\,B{a^{2 + }}$ions ($K_sp=$ $1.0 \times {10^{ – 9}}$ )