If the degree of dissociation is $1.30\%$,what is the $K_a$ for $0.1 \ M \ CH_3COOH$?

At $25^{\circ} C$,the percentage of ionization of '$x$' $M$ acetic acid is $4.242$. What is the value of $x$? $(K_a = 1.8 \times 10^{-5})$

$0.2 \ M$ solution of formic acid is ionized $3.2 \%$. Its ionization constant is:

$A$ weak base is $1.42 \%$ dissociated in its $0.05 \ M$ solution. Calculate its dissociation constant.

$A$ weak base is $1.3\%$ dissociated in its aqueous solution. If $K_b$ for the weak base is $1.69 \times 10^{-5}$ at $298 \text{ K}$, find the concentration of the aqueous solution of the weak base. (in $\text{ M}$)

The ionization constant of benzoic acid is $6.5 \times 10^{-5}$ at $298 \ K$ temperature. Calculate $pH$ of its $0.15 \ M$ solution. (in $.5$)