Calculate the ionic product of the solution formed by mixing equal volumes of $0.004 \, M \, CaSO_4$ and $0.002 \, M \, H_2SO_4$.

What is the ratio of the number of $H^{+}$ ions to the number of $H_2O$ molecules in $1 \ L$ of water?

If equivalent conductance of $1 \ M$ benzoic acid is $12.8 \ \Omega^{-1} \ cm^2 \ eq^{-1}$ and if the equivalent conductances of benzoate ion and $H^+$ ion at infinite dilution are $42$ and $288.42 \ \Omega^{-1} \ cm^2 \ eq^{-1}$ respectively,then its degree of dissociation is ............ $\%$

At $27^{\circ} C$,the degree of dissociation of $HA$ (weak acid) in $0.5 \ M$ of its solution is $1 \%$. The concentrations of $H_3O^{+}$,$A^{-}$,and $HA$ at equilibrium (in $mol \ L^{-1}$) are respectively

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$BaSO_4(s) + Na_2CO_3(aq) \longrightarrow BaCO_3(s) + Na_2SO_4(aq)$

$100 \ cm^3$ of $0.1 \ N \ HCl$ solution is mixed with $100 \ cm^3$ of $0.2 \ N \ NaOH$ solution. The resulting solution is