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

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 $pH$ of $0.01 \ M$ solution of acetic acid is $5.0$. What are the values of $[H^{+}]$ and $K_a$ respectively?

The amount of acetic acid in $1 \ L$ of solution having $\alpha = 1\%$ and $K_a = 1.8 \times 10^{-5}$ is ............. $g$.

What will be the hydrogen ion concentration of $0.006 \ M$ benzoic acid? $(K_a = 6 \times 10^{-5})$

Calculate the value of the dissociation constant $(K_b)$ of a weak monoacidic base if it dissociates to $2 \%$ in a $0.1 \ M$ solution.