The $pH$ of a $0.1 \ M$ solution of a monobasic acid is $2.34$. Calculate the degree of dissociation of the acid.

Calculate the $pH$ of $0.02 \ M$ $ClCH_2COOH$. Given its $K_a = 1.36 \times 10^{-3}$,calculate its $pK_b$.

An organic monobasic acid has a dissociation constant of $1.96 \times 10^{-8}$. What is its percentage dissociation in a $0.01 \text{ M}$ solution (in $\%$)?

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 ............ .

The $pH$ of $0.1 \, M$ acetic acid solution is closest to $.....$ [Dissociation constant of the acid,$K_{a} = 1.8 \times 10^{-5}$]

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 $.13$)