Solubility product constant ( $\mathrm{K}_{\mathrm{sp}}$ ) of salts of types $\mathrm{MX}, \mathrm{MX}_2$ and $\mathrm{M}_3 \mathrm{X}$ at temperature ' $\mathrm{T}$ ' are $4.0 \times 10^{-8}, 3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$, respectively. Solubilities (mole dm ${ }^{-3}$ ) of the salts at temperature ' $\mathrm{T}$ ' are in the order

If the solubility product of $AgBr{O_3}$ and $A{g_2}S{O_4}$ are $5.5 \times {10^{ – 5}}$ and $2 \times {10^{ – 5}}$ respectively, the relationship between the solubilities of these can be correctly represented as

Solubility product $(K_{sp})$ of the salts $MX\,,\, MX_2\,,\, M_3X$ at temperature $'T'$ are $4 \times 10^{-8}\,,\, 3.2 \times 10^{-14}$ and $2.7 \times 10^{-15}$ respectively. Solubilities of the salt at temperature $'T'$ are in the order

The solubility product of $BaS{O_4}$ is $1.3 \times {10^{ – 9}}$. The solubility of this salt in pure water will be

Solubility product of silver bromide is $5.0 \,\,\times \,\,10^{-13}$ . The quantity of potassium
bromide (molar mass taken as $120\,\,g\,mol^{-1}$ ) to be added to $1\,L$  of  $0.05\,\,M$  solution of silver nitrate to start the precipitation of  $AgBr$  is