Calculate $[H_3O^{+}]$ of a monobasic acid if it is $0.04 \%$ dissociated in $0.05 \ M$ solution.

The $pH$ of $0.1 \ M$ monobasic acid is $4.50$. Calculate the concentration of species $H^{+}$,$A^{-}$ and $HA$ at equilibrium. Also,determine the value of $K_{a}$ and $pK_{a}$ of the monobasic acid.

The $pH$ of $0.005 \, M$ codeine $(C_{18}H_{21}NO_{3})$ solution is $9.95$. Calculate its ionization constant and $pK_{b}$.

The $pH$ of $0.01 \ M \ BOH$ solution is $10$. What is its degree of dissociation (in $\%$)? (Given $K_{b}$ of $BOH$ is $1 \times 10^{-6}$)

An organic monobasic acid has a dissociation constant of $2.25 \times 10^{-6}$. What is the percent dissociation in its $0.01 \ M$ solution (in $\%$)?

At $25^{\circ} C$,the percentage of ionization of '$x$' $M$ acetic acid is $4.242$. What is the value of $x$? $(K_a = 1.8 \times 10^{-5})$