Calculate the pH of a centimolar solution of a monoacidic weak base which is $10 \%$ dissociated in its aqueous solution.

The $K_a$ of monobasic acid $A, B$ and $C$ are $10^{-6}, 10^{-8}$ and $10^{-10}$ respectively. The concentrations of $A, B$ and $C$ are respectively $0.1 \ M, 0.01 \ M$ and $0.001 \ M$. Which of the following is correct for $pOH$ of $A, B$ and $C$?

An acid solution of $pH=6$ is diluted $1000$ times,the $pH$ of the final solution becomes

The $pH$ of $0.004 \, M$ hydrazine solution is $9.7$. Calculate its ionization constant $K_{b}$ and $pK_{b}$.

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

Calculate the $pH$ of $0.02 \ M$ monobasic acid having $2 \%$ dissociation.