For a $10^{-3} \ M \ H_2CO_3$ solution,if the degree of dissociation $\alpha = 10\%$,what will be the value of $pH$?

What is the dissociation constant for $NH_4OH$ if at a given temperature its $0.1 \ N$ solution has $pH = 11.27$ and the ionic product of water is $7.1 \times 10^{-15}$ (antilog $0.73 = 5.37$)?

Find $pH$ of $5 \times 10^{-3} \ M$ $H_2CO_3$ solution having $10\%$ dissociation.

The dissociation constant of a weak monobasic acid is $3.2 \times 10^{-4}$. Calculate the degree of dissociation in its $0.04 \ M$ solution.

The $pH$ of $0.01 \ M$ solution of acetic acid is $5.0$. What are the values of $[H^{+}]$ and $K_a$ respectively?

The $K_a$ of a weak acid $HA$ is $1.00 \times 10^{-5}$. If $0.100 \ mol$ of this acid is dissolved in $1 \ L$ of water,what is the percentage dissociation of the acid at equilibrium?