The first and second dissociation constants of an acid ${\mathrm{H}}_{2}A \mathrm{a}\mathrm{r}\mathrm{e}\mathrm{ }1.0\times {10}^{-5}\mathrm{ }\mathrm{a}\mathrm{n}\mathrm{d}\mathrm{ }5.0\times {10}^{-10}$ respectively. The overall dissociation constant of the acid will be

In a saturated solution of the sparingly soluble strong electrolyte ${\mathrm{AgIO}}_3$ (Molecular mass= $283$), the equilibrium which sets in is

${\mathrm{AgIO}}_3 \left(\mathrm{s}\right) \iff {\mathrm{Ag}}^{+} \left(\mathrm{aq}\right) + {{\mathrm{IO}}_3}^{-} \left(\mathrm{aq}\right)$

If the solubility product constant ${\mathrm{K}}_{\mathrm{sp}}$ of ${\mathrm{AgIO}}_3$ at a given temperature is $1.0\times {10}^{-8}$, what is the mass of ${\mathrm{AgIO}}_3$ contained in $100 \mathrm{ml}$ of its saturated solution?

In aqueous solution, the ionization constants for carbonic acid are ${\mathrm{K}}_1=4.2\times {10}^{-7}$ and ${\mathrm{K}}_2=4.8\times {10}^{-11}$. Select the correct statement for a saturated $0.034 \mathrm{M}$solution of the carbonic acid.

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