The solubility product of a sparingly soluble salt $AB$ at room temperature is $1.21 \times 10^{-6}$. Its molar solubility is

What is the molar solubility of $Ag_{2}CO_{3}$ $(K_{sp} = 4 \times 10^{-13})$ in $0.1 \ M \ Na_{2}CO_{3}$ solution?

At $298 \, K$,the solubility product $(K_{sp})$ of $M_2SO_4$ (where $M^+$ is a monovalent metal ion) is $1.2 \times 10^{-5}$. What is the maximum concentration of $M^+$ ions in a saturated solution of this salt at $298 \, K$?

The molar solubility of $CaF_2$ $(K_{sp} = 5.3 \times 10^{-11})$ in $0.1 \ M$ solution of $NaF$ will be:

The saturated solution of $Ag_2SO_4$ is $2.5 \times 10^{-2} \ M$. Its solubility product $(K_{sp})$ is

Why is only $As^{3+}$ precipitated as $As_2S_3$ when $H_2S$ is passed through an acidic solution containing $As^{3+}$ and $Zn^{2+}$,while $Zn^{2+}$ is not precipitated as $ZnS$?