$0.2$ molar solution of formic acid is ionized $3.2\%$. Its ionization constant is
$1 \times {10^{ - 12}}$
$2.1 \times {10^{ - 4}}$
$1.25 \times {10^{ - 6}}$
$1 \times {10^{ - 14}}$
The ionization constant of benzoic acid is $6.5 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate $pH$ of its $0.15$ $M$ solution.
Derive the equation of ionization constant $({K_b})$ of weak base.
The $pH$ value of decinormal solution of $N{H_4}OH$ which is $20\%$ ionised, is
For a weak acid $HA,$ Ostwald's dilution law is represented by the equation
Degree of dissociation is $10\%$ for $10^{-3}\, M$ solution of $H_2CO_3$ then $pH$ of solution is