Values of dissociation constant, $K_a$ are given as follows

Acid	$K_a$
$HCN$	$6.2\times 10^{-10}$
$HF$	$7.2\times 10^{-4}$
$HNO_2$	$4.0\times 10^{-4}$

Correct order of increasing base strength of the base $CN^-,F^-$ and $NO_2^-$ will be

$0.01$ moles of a weak acid $HA \left( K _{ a }=2.0 \times 10^{-6}\right)$ is dissolved in $1.0\, L$ of $0.1\, M\, HCl$ solution. The degree of dissociation of $HA$ is ............. $\times 10^{-5}$

(Round off to the Nearest Integer).

[Neglect volume change on adding $HA$. Assume degree of dissociation $<< 1]$

$K _{ a_1,}, K _{ a_2 }$ and $K _{ a_3}$ are the respective ionization constants for the following reactions $(a), (b),$ and $(c)$.

$(a)$ $H _{2} C _{2} O _{4} \rightleftharpoons H ^{+}+ HC _{2} O _{4}^{-}$

$(b)$ $HC _{2} O _{4}^{-} \rightleftharpoons H ^{+}+ HC _{2} O _{4}^{2-}$

$(c)$ $H _{2} C _{2} O _{4} \rightleftharpoons 2 H ^{+}+ C _{2} O _{4}^{2-}$

The relationship between $K_{a_{1}}, K_{ a _{2}}$ and $K_{ a _{3}}$ is given as

$p{K_a}$ value for acetic acid at the experimental temperature is $5$. The percentage hydrolysis of $0.1\,\,M$ sodium acetate solution will be

The ionization constant of $0.1$ $M$ weak acid is $1.74 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate $pH$ of its $0.1$ $M$ solution.

In its $0.2\,\, M$ solution, an acid ionises to an extent of $60\%$. Its hydrogen ion concentration is.....$M$