What is the percent ionization $(\alpha)$ of a $0.01 \ M \ HA$ solution? $......\%$ $(K_a = 10^{-6})$

At $298 \ K$ temperature,calculate the $pH$ of a $0.25 \ M$ solution of $(CH_3)_2NH$ given that its $K_b$ is $5.4 \times 10^{-4}$.

The dissociation constants of monobasic acids $A$,$B$,$C$ and $D$ are $6 \times 10^{-4}$,$5 \times 10^{-5}$,$3.6 \times 10^{-6}$ and $7 \times 10^{-10}$ respectively. The $pH$ values of their $0.1 \ M$ aqueous solutions are in the order

For a $10 \ M \ CH_3COOH$ solution,if $K_a = 10^{-5}$,what will be the values of $[H^{+}]$ and $pH$ respectively?

For a $10^{-2} \ M \ Ca(OH)_2$ solution with a degree of dissociation $\alpha = 10\%$,what are the values of $pOH$ and $pH$ respectively?

The dissociation constant of propionic acid is $1.32 \times 10^{-5}$. Calculate the degree of dissociation of the acid in a $0.05 \ M$ solution.