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 $pH$ of a $0.01 \ M$ weak acid $HX$ $(K_{a}=4 \times 10^{-10})$ is found to be $5$. Now the acid solution is diluted with excess of water so that the $pH$ of the solution changes to $6$. The new concentration of the diluted weak acid is given as $x \times 10^{-4} \ M$. The value of $x$ is $...........$ (nearest integer)

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.

Dimethyl amine $(CH_3)_2NH$ is a weak base and its ionization constant is $5.4 \times 10^{-5}$. Calculate $[OH^{-}]$,$[H_3O^{+}]$,$pOH$ and $pH$ of its $0.2 \ M$ solution at equilibrium.

Accumulation of lactic acid $(HC_3H_5O_3),$ a monobasic acid in tissues,leads to pain and a feeling of fatigue. In a $0.10 \ M$ aqueous solution,lactic acid is $3.7 \%$ dissociated. The value of the dissociation constant,$K_a,$ for this acid will be:

If the $pH$ of $0.10 \ M$ monobasic acid at $298 \ K$ is $5.0$,the value of $p K_a$ at the same temperature is