The conjugate base of $HCO_3^-$ is

$A$ salt of sulphurous acid is called

The enthalpies of neutralization of $HCN$ and $H_2S$ with a strong base are $12.13 \ kJ \ equi^{-1}$ and $15.9 \ kJ \ equi^{-1}$ respectively. Then:

The dissociation constant of a weak acid $HA$ is $1.8 \times 10^{-4}$. Calculate the dissociation constant of its conjugate base $A^{-}$.

An acid is a compound which furnishes ($Bronsted-Lowry$ concept):

Derive the equation of the relation between the weak base ionization constant $K_b$ and its conjugate acid ionization constant $K_a$.