$A$ solution of $0.01 \ M$ $MgCl_2$ will form a precipitate of $Mg(OH)_2$ at a limiting $pH$ of: (Given: $K_{sp}$ of $Mg(OH)_2 = 1 \times 10^{-12}$)

$A$ very dilute acidic solution of $Cd^{2+}$ and $Ni^{2+}$ gives only yellow precipitate of $CdS$ on passing $H_2S$ gas. This is due to:

Precipitation occurs if the ionic product is ........

The solubility product of $AgCl$ is $10^{-10} \, M^2$. The minimum volume (in $m^3$) of water required to dissolve $14.35 \, mg$ of $AgCl$ is approximately

The $K_{sp}$ for the following dissociation is $1.6 \times 10^{-5}$:
$PbCl_{2(s)} \rightleftharpoons Pb^{2+}_{(aq)} + 2Cl^-_{(aq)}$
Which of the following choices is correct for a mixture of $300 \ mL$ of $0.134 \ M \ Pb(NO_3)_2$ and $100 \ mL$ of $0.4 \ M \ NaCl$?

In which of the following solvents will $AgBr$ have the highest solubility?