The $pH$ of a $0.01 \, M$ solution of acetic acid having a degree of dissociation of $12.5 \%$ is:

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.

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

Calculate the $pH$ of a solution containing $6.0 \ g$ of acetic acid $(CH_3COOH)$ in $250 \ mL$ of water. Given: $K_a = 1.8 \times 10^{-5}$ at $298 \ K$,and atomic masses are $C = 12, H = 1, O = 16$. (in $.57$)

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)

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