The hydrogen ion concentration of $0.1\,N$ solution of $C{H_3}COOH,$ which is $30\%$ dissociated, is
$0.03$
$3$
$0.3$
$30$
$pH$ of an aqueous solution $H_2CO_3$ is $3.3$. If ${K_{{a_1}}} = {10^{ - 3}}$and ${K_{{a_2}}} = {10^{ - 13}}$ then $[HCO_3^-]$ is
Calculate the $pH$ of a $0.10 \,M$ ammonia solution. Calculate the pH after $50.0 \,mL$ of this solution is treated with $25.0 \,mL$ of $0.10 \,M$ $HCl$. The dissociation constant of ammonia, $K_{b}=1.77 \times 10^{-5}$
Assuming that the degree of hydrolysis is small, the $pH$ of $0.1\, M$ solution of sodium acetate $(K_a\, = 1.0\times10^{- 5})$ will be
Derive the equation of ionization constant $({K_b})$ of weak base.
The ionization constant of acetic acid is $1.74 \times 10^{-5}$. Calculate the degree of dissociation of acetic acid in its $0.05\, M$ solution. Calculate the concentration of acetate ion in the solution and its $pH$.