The $K_b$ of ammonia $(NH_3)$ is $1.8 \times 10^{-5}$ at $298 \ K$. Calculate the $pH$ of a $0.1 \ M$ ammonia solution. (in $.13$)

The ionization constant of $CH_3COOH$ is $1.7 \times 10^{-5}$. In a certain solution of acetic acid,the concentration of $H^+$ is $3.4 \times 10^{-4} \ M$. The concentration of the acetic acid solution is ............ .

$A$ monobasic weak acid dissociates $2 \%$ in its $0.002 \ M$ solution. Calculate the dissociation constant of the weak acid.

The degree of dissociation of $0.1 \, N \, CH_3COOH$ is (Dissociation constant $K_a = 1 \times 10^{-5}$)

For a diprotic organic acid in aqueous solution,the ionization constants are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$. For a $0.034 \ M$ solution of this acid,select the correct statement.

Sulphurous acid $(H_{2}SO_{3})$ has $Ka_{1} = 1.7 \times 10^{-2}$ and $Ka_{2} = 6.4 \times 10^{-8}$. The $pH$ of $0.588 \ M \ H_{2}SO_{3}$ is ..... . (Round off to the Nearest Integer)