$A$ white powder soluble in $NH_4OH$ but insoluble in water is:

At $25\,^{\circ}C$,the solubility product of $Mg(OH)_2$ is $1.0 \times 10^{-11}$. At which $pH$ will $Mg^{2+}$ ions start precipitating in the form of $Mg(OH)_2$ from a solution of $0.001\, M\, Mg^{2+}$ ions?

The solubility of a salt of a weak acid $MX$ (e.g.,phosphoric acid salts) increases at lower $pH$. Explain with equations.

Which of the following salts is insoluble in water?

The solubility of salt $AX_2$ is $6 \times 10^{-12} \text{ mol dm}^{-3}$. What is the solubility product $(K_{sp})$ of the salt?

If the solubility of $Ca_3(PO_4)_2$ in water is $x \ mol \ L^{-1}$, its solubility product in $mol^5 \ L^{-5}$ is (in $x^5$)