$A$ weak monoprotic acid of $0.1 \ M$ ionizes to $1\%$ in solution. What will be the $pH$ of the solution?

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

Calculate the molar concentration of a weak monobasic acid if the acid dissociation constant $K_a = 1.8 \times 10^{-5}$ and the degree of dissociation $\alpha = 0.01$.

$1.0 \ mol$ of $HCl$ and $1.0 \ mol$ of $CH_3COONa$ are dissolved in water to make a $1 \ L$ solution. What is the concentration of $H^+$ in the solution? ($K_a$ for $CH_3COOH = 1.6 \times 10^{-5}$)

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

What is the molar concentration of a weak monobasic acid if its dissociation constant is $5 \times 10^{-8}$ and it undergoes $0.5 \%$ dissociation (in $M$)?