If the solubility product of $CuS$ is $6 \times 10^{-16}$,calculate the maximum molarity of $CuS$ in aqueous solution.

Which of the following represents the correct solubility product expression for calcium phosphate?

Which of the following pairs of ions when mixed in dilute solutions may give a precipitate?

For a metal hydroxide with an oxidation state of $+3$,the solubility is $1 \times 10^{-5} \ mol/L$. What is its solubility product $(K_{sp})$?

The concentration of sulphide ion in $0.1 \ M \ HCl$ solution saturated with hydrogen sulphide is $1.0 \times 10^{-19} \ M$. If $10 \ mL$ of this is added to $5 \ mL$ of $0.04 \ M$ solution of the following: $FeSO_4, MnCl_2, ZnCl_2$ and $CdCl_2$,in which of these solutions will precipitation take place? Given $K_{sp}$ for $FeS = 6.3 \times 10^{-18}, MnS = 2.5 \times 10^{-13}, ZnS = 1.6 \times 10^{-24}, CdS = 8.0 \times 10^{-27}$.

If the $pH$ of a $0.001 \, M \, Mg(NO_3)_2$ solution is $9$,will precipitation occur? Given the $K_{sp}$ of $Mg(OH)_2 = 8.9 \times 10^{-12}$.