When equal volumes of the following solutions are mixed, precipitation of $AgCl\,({K_{sp}} = 1.8 \times {10^{ – 10}})$ will occur only with

Solubility of $16 \times {10^{ – 4}}\,m/s$ at ${20\,^o}C$ is $1.435 \times {10^{ – 3}}\,gm\,per\,litre$. The solubility product of $AgCl$ is

The ${K_{sp}}$ of $Mg{\left( {OH} \right)_2}$, is $1.0 \times {10^{ – 12}}$. At which $pH$ the $0.01$ $M$ $Mg{\left( {OH} \right)_2}$ begins to precipitate ? Calculate solubility.

The precipitation occurs if ionic concentration is

An acidified solution of $0.05 M Zn ^{2+}$ is saturated with $0.1 M H _2 S$. What is the minimum molar concentration ($M$) of $H ^{+}$required to prevent the precipitation of $ZnS$ ?

Use $K_{ sp }( ZnS )=1.25 \times 10^{-22}$ and

Overall dissociation constant of $H _2 S , K_{ NET }=K_1 K_2=1 \times 10^{-21}$