The degree of dissociation is inversely proportional to the square root of the concentration of the weak base.

$0.01$ moles of a weak acid $\mathrm{HA} \left({\mathrm{K}}_{\mathrm{a}}=2.0\times {10}^{-6}\right)$ is dissolved in $1.0 \mathrm{L}$ of $0.1\mathrm{M} \mathrm{HCl}$ solution. The degree of dissociation of $\mathrm{HA}$ is __________ $\times {10}^{-5}$ (Round off to the Nearest Integer). [Neglect volume change on adding $\mathrm{HA}$ and assume degree of dissociation $<<1$]

The degree of dissociation of $0.1\mathrm{mol} {\mathrm{L}}^{-1}$acetic acid in water is

( $\mathrm{K}$ of acetic acid is ${10}^{-5}$ ) 

Identify the appropriate option for the following reaction.

$\text{HF}+{\text{H}}_2\text{O}\stackrel{{\text{K}}_{\text{a}}}{⟶}{\text{H}}_3{\text{O}}^{+}+{\text{F}}^{-}$ 

 ${\text{F}}^{-}+{\text{H}}_2\text{O}\stackrel{{\text{K}}_{\text{b}}}{⟶}\text{H}\text{F}+{\text{OH}}^{-}$

Directions: Each of these questions contains an Assertion followed by reason. Read them carefully and answer the question on the basis of following options. You have to select the one that best describes the two statements.

$\mathrm{Assertion}:$ The degree of dissociation of ${\mathrm{CH}}_3\mathrm{COOH}$ is more in a solution which is basic than in water.
$\mathrm{Reason}:$ ${\mathrm{K}}_{\mathrm{a}}$ of ${\mathrm{CH}}_3\mathrm{COOH}$ increases in basic solution.

If ${\mathrm{K}}_{\mathrm{a}}$ of $\mathrm{HOCN}=1.2 \mathrm{X} {10}^{-4}$ and ${\mathrm{K}}_{\mathrm{a}}$ of $\mathrm{HCN}=4.2 \mathrm{X} {10}^{-4}$, then the ratio of acidic strength of $\mathrm{HOCN}$ and $\mathrm{HCN}$ is: