The $pH $ of a $0.01\,M$ solution of acetic acid having degree of dissociation $12.5\%$ is

$2\, gm$ acetic acid and $3\, gm$ sodium acetate are present in $100\, ml$. aqueous solution then what will be the $pH$ of solution if ionisation constant of acetic acid is $1.8 \times 10^{-5}$

For a weak acid, the incorrect statement is

$p{K_a}$ value for acetic acid at the experimental temperature is $5$. The percentage hydrolysis of $0.1\,\,M$ sodium acetate solution will be

Derive the equation of ionization constant $({K_b})$ of weak base.

A $0.1\,N $ solution of an acid at room temperature has a degree of ionisation $ 0.1$ . The concentration of $O{H^ - }$ would be