What is the $pH$ of a $1 \ M$ $CH_3COOH$ solution? Given that the $K_a$ of acetic acid $= 1.8 \times 10^{-5}$.

The ionisation constant of acetic acid is $1.8 \times 10^{-5}$. The concentration at which it will be dissociated to $2\%$,is (in $M$)

For a weak base $BOH$ at $25\,^oC$,the dissociation constant $K_b$ is $1.0 \times 10^{-12}$. The concentration of hydroxyl ions in its $0.01\,M$ aqueous solution will be:

The $pH$ of $0.01 \ M \ BOH$ solution is $10$. What is its degree of dissociation (in $\%$)? (Given $K_{b}$ of $BOH$ is $1 \times 10^{-6}$)

At $25^{\circ} C$,the percentage of ionization of $x \ M$ acetic acid is $4.242$. What is the pH of the acetic acid solution?
$(\log 4.242=0.6275) ;(\log 0.04242=-1.372) \quad (K_a=1.8 \times 10^{-5})$

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.