Which of the following base is weakest
$N{H_4}OH:{K_b} = 1.6 \times {10^{ - 6}}$
${C_6}{H_5}N{H_2}:{K_b} = 3.8 \times {10^{ - 10}}$
${C_2}{H_5}N{H_2}:{K_b} = 5.6 \times {10^{ - 4}}$
${C_6}{H_7}N:{K_b} = 6.3 \times {10^{ - 10}}$
A weak monoprotic acid of $0.1\, M,$ ionizes to $1\% $ in solution. What will be the $pH $ of solution
$p{K_a}$ of a weak acid is defined as
Find $pH$ of $5 \times 10^{-3}\, M$ $H_2CO_3$ solution having $10\%$ dissociation
The $pH$ of $0.1$ $M$ solution of cyanic acid $(HCNO)$ is $2.34$. Calculate the ionization constant of the acid and its degree of ionization in the solution.
$pH$ 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