Acetic acid dissociates to $1.20 \%$ in its $0.01 \ M$ solution. What is the value of its dissociation constant?

The $K_a$ of propanoic acid is $1.4 \times 10^{-5}$. Calculate the $pH$ of a $0.1 \ M$ solution.

What is the molar concentration of a weak monobasic acid if its dissociation constant is $5 \times 10^{-8}$ and it undergoes $0.5 \%$ dissociation (in $M$)?

If $1 \ mM$ solution of ethylamine produces $pH = 9$,then the ionization constant $(K_b)$ of ethylamine is $10^{-x}$. The value of $x$ is . . . . . . (nearest integer). [The degree of ionization of ethylamine can be neglected with respect to unity.]

If two acids of equimolar concentration are taken,then which option is correct?

The first and second ionization constants of $H_2X$ are $2.5 \times 10^{-8}$ and $1.0 \times 10^{-13}$ respectively. The concentration of $X^{2-}$ in $0.1 \ M$ $H_2X$ solution is . . . . . . $\times 10^{-15} \ M$. The value of $Y$ is: