The $K_a$ of $CH_3COOH$ is $1.76 \times 10^{-5}$ at $298 \ K$. Calculate the dissociation constant $(K_b)$ of its conjugate base.

When $HClO_4$ is dissolved in the weak acid $HF$,the following equilibrium is established:
$HF + HClO_4 \rightleftharpoons H_2F^+ + ClO_4^-$
Which of the following is the correct set of conjugate acid-base pairs?

If the $pK_b$ of the fluoride ion $(F^-)$ at $25^{\circ}C$ is $10$,what is the ionization constant $(K_a)$ of hydrofluoric acid $(HF)$ at the same temperature?

$K_{a}$ values for acids $H_{2}SO_{3}$,$HNO_{2}$,$CH_{3}COOH$ and $HCN$ are respectively $1.3 \times 10^{-2}$,$4 \times 10^{-4}$,$1.8 \times 10^{-5}$ and $4 \times 10^{-10}$. Which of the above acids produces a stronger conjugate base in aqueous solution?

Neutralization of an acid with a base invariably results in the production of

What do you understand by the term 'auto-protolysis' of water? What is its significance?