The percentage of pyridine $(C_5H_5N)$ that forms pyridinium ion $(C_5H_5N^{+}H)$ in a $0.10 \ M$ aqueous pyridine solution ($K_b$ for $C_5H_5N = 1.7 \times 10^{-9}$) is (in $\%$)

Which of the following compounds has the maximum $K_{a}$ value?

$A$ monobasic weak acid dissociates to $1.2 \%$ in its $0.01 \ M$ solution at $298 \ K$. Calculate the dissociation constant of it.

The $pH$ of a $0.01 \ M$ weak acid $HX$ $(K_{a}=4 \times 10^{-10})$ is found to be $5$. Now the acid solution is diluted with excess of water so that the $pH$ of the solution changes to $6$. The new concentration of the diluted weak acid is given as $x \times 10^{-4} \ M$. The value of $x$ is $...........$ (nearest integer)

For a $10^{-3} \ M \ H_2CO_3$ solution,if the degree of dissociation $\alpha = 10\%$,what will be the value of $pH$?

Derive the expression for the ionization constant $(K_b)$ of a weak base.