$K_{sp}$ of a salt $Ni(OH)_2$ is $2 \times 10^{-15}$,then molar solubility of $Ni(OH)_2$ in $0.01 \ M \ NaOH$ is $:-$

The solubility product of $AB_2$ is $8 \times 10^{-5} \ M^3$. If the salt is $80 \ \%$ dissociated in a saturated solution,find the solubility of the salt in $M$.

The solubility of $CdSO_{4}$ in water is $8.0 \times 10^{-4} \ mol \ L^{-1}$. Its solubility in $0.01 \ M \ H_{2}SO_{4}$ solution is $..... \ \times 10^{-6} \ mol \ L^{-1}$.
(Round off to the Nearest integer) (Assume that solubility is much less than $0.01 \ M$)

The solubility product of salt $B_2A$ is $3.2 \times 10^{-11}$ at $298 \ K$. What is the solubility of the salt at the same temperature?

If the concentration of sodium ions in a saturated solution of $Na_2SO_4$ is $10^{-5} \ mol/L$,find the solubility product $(K_{sp})$.

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,$AgCl$?
$(Given \ K_{sp} \ of \ AgCl = 1 \times 10^{-10})$