Ionization of Acids and Bases

The ionization of base MOH can be represented by the equation:

$\mathrm{MOH}\left(\mathrm{aq}\right)\rightleftharpoons {\mathrm{M}}^{-}\left(\mathrm{aq}\right)+{\mathrm{OH}}^{+}\left(\mathrm{aq}\right)$

Which of the following equation follows for base ionization constant is expressed in terms of concentration in molarity of various species in equilibrium.

Define base ionization constant.

The $\mathrm{pH}$ of an aqueous solution of ${10}^{-8}\mathrm{MHCl}$ is

The correct order of increasing $\left[{\mathrm{H}}_3{\mathrm{O}}^{+}\right]$ in the following aqueous solution is 

The degree of ionization of 0.4 M acetic acid will be $({\mathrm{K}}_{\mathrm{a}}=1.8\times {10}^{-5})$ .

What will be the $\mathrm{pH}$ of a $0.01 \mathrm{M}$ ammonia solution which is $5 \%$ ionised?

In an aqueous solution, the ionization constants for carbonic acid are

${\text{K}}_1=\text{4.2}\times 10^{-7}$ and ${\text{ K}}_2=\text{4.8}\times 10^{-11}$

Select the correct statement for a saturated $\text{0.034 M}$ solution of the carbonic acid:

Given, $\text{HF}+{\text{H}}_2\text{O}\stackrel{{\text{K}}_{\text{a}}}{⟶}{\text{H}}_3{\text{O}}^{+}+{\text{F}}^{-};$  ${\text{F}}^{-}+{\text{H}}_2\text{O}\stackrel{{\text{K}}_{\text{b}}}{⟶}\text{H}\text{F}+{\text{OH}}^{-}$.  Which of the following relation is correct?