What is the percentage dissociation of $0.1 \ M$ acetic acid (in $\%$)? $(K_a = 10^{-5})$

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

The $pH$ of $0.05 \ M$ acetic acid is $(K_a = 2 \times 10^{-5})$.

The $pH$ of a $0.1 \ M$ solution of a weak monoprotic acid that is $1\%$ ionized is:

$0.02 \, M$ monobasic acid dissociates $2 \%$,hence,$pH$ of the solution is

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