$25.0\,mL$ of $0.050\,M\,Ba \left( NO _3\right)_2$ is mixed with $25.0\,mL$ of $0.020\,M$ $NaF$,$K _{ sp }$ of $BaF _2$ is $0.5 \times 10^{-6}$ at $298\,K$. The ratio of $\left[ Ba ^{2+}\right]\left[F^{-}\right]^2$ and $K _{ sp }$ is $…….$. (Nearest integer)

$K_{sp}$ for $BaSO_4$ at $25\,^oC$ is $1.1 \times 10^{-10}$. To make the new solubility equal to $1.1 \times 10^{-8}$, it is necessary to use the solution of $Na_2SO_4$ of the following concentration….$M$

What will be the solubility of $AlCl_3$ in solution of $CaCl_2$ with concentration $C$

If the solubility product of $BaS{O_4}$ is $1.5 \times {10^{ – 9}} $ in water, its solubility in moles per litre, is

The $pH$ at which $\mathrm{Mg}(\mathrm{OH})_2\left[\mathrm{~K}_{\mathrm{sp}}=1 \times 10^{-11}\right]$ begins to precipitate from a solution containing $0.10 \ \mathrm{M}$ $\mathrm{Mg}^{2+}$ ions is_____