In an aqueous solution $SCN^{-1}, B^{-1}, I^{-1}$ and $Cl^-$ are present. Which will get precipitated first, when $AgNO_3$ is mixed with each of them? Given that 
$Ksp$ of $AgCl = 1.2 \times 10^{-10}$,
$Ksp$ of $AgI = 1.7 \times 10^{-16}$
$Ksp$ of $AgSCN = 7.1 \times 10^{-7}$,
$Ksp$ of $AgBr = 3.5 \times10^{-13}$

At $298\,K$, the solubility of silver chloride in water is $1.434 \times 10^{-3}\,g\,L ^{-1}$. The value of $-\log K _{ sp }$ for silver chloride is $……..$ (Given mass of $Ag$ is $107.9\,g\,mol ^{-1}$ and mass of $Cl$ is $35.5\,g\,mol ^{-1}$ )

Predict whether a precipitate of $(PbI_{2})$ will be formed or not on mixing $20$ $mL$ of $3 \times {10^{ – 3}}$ $M$ $Pb{\left( {N{O_3}} \right)_2}$ solution with $80$ $mL$ of $2 \times {10^{ – 3}}$ $M$ $NaI$ solution. $K_{sp}$ for lead iodide ( $PbI_{2}$ ) is $6.0 \times {10^{ – 9}}$

If the solubility product ${K_{sp}}$ of a sparingly soluble salt $M{X_2}$ at $25\,^oC$ is $1.0 \times {10^{ – 11}}$, the solubility of the salt in mole litre$^{-1}$ at this temperature will be

The solubility product of magnesium hydroxide $Mg{\left( {OH} \right)_2}$ is $1.2 \times {10^{ – 11}}$. Calculate its solubility in pure water and $0.05$ $M$ $NaOH$.