$K_{sp}$ for $CaSO_4$ is $9 \times 10^{-6}$. The minimum volume of water needed to dissolve $1 \ g$ of $CaSO_4$ at $298 \ K$ temperature is ...... (in $L$)

Observe the following solutions:
$(i)$ $1 \ L$ of $10^{-6} \ M \ AgNO_3$
$(ii)$ $1 \ L$ of $10^{-7} \ M \ AgNO_3$
$(iii)$ $1 \ L$ of $10^{-9} \ M \ AgNO_3$
$(iv)$ $1 \ L$ of $10^{-3} \ M \ AgNO_3$
$(v)$ $1 \ L$ of $10^{-5} \ M \ NaCl$
Which of the above two solutions when mixed will give a white precipitate,$AgCl$?
$(Given \ K_{sp} \ of \ AgCl = 1 \times 10^{-10})$

$M_{3}A_{2}$ is a sparingly soluble salt of molar mass $y \text{ g mol}^{-1}$ and solubility $x \text{ g L}^{-1}$. The ratio of the molar concentration of the anion $(A^{3-})$ to the solubility product of the salt is

Solubility product $(K_{sp})$ of the salts $MX$,$MX_2$,and $M_3X$ at temperature $T$ are $4 \times 10^{-8}$,$3.2 \times 10^{-14}$,and $2.7 \times 10^{-15}$ respectively. The solubilities of these salts at temperature $T$ are in the order:

The solubility of $CaF_2$ in a solution of $0.1 \ M \ Ca(NO_3)_2$ is.

The solubility product of a salt with the general formula $MX_2$ is $4.0 \times 10^{-12}$. What is the concentration of the $M^{2+}$ ion in a saturated solution of this salt?