A compound whose aqueous solution will have the highest $pH$
$NaCl$
$N{a_2}C{O_3}$
$N{H_4}Cl$
$NaHC{O_3}$
The degree of dissociation of $0.1\,M\,HCN$ solution is $0.01\%$ . Its ionisation constant would be
The first and second dissociation constants of an acid $H_2A$ are $1.0 \times 10^{-5}$ and $5.0 \times 10^{-10}$ respectively. The overall dissociation constant of the acid will be
Determine the degree of ionization and $pH$ of a $0.05 \,M$ of ammonia solution. The ionization constant of ammonia can be taken from Table $7.7 .$ Also, calculate the ionization constant of the conjugate acid of ammonia.
The $pH$ of a $0.1\ M$ aqueous solution of a very weak acid $(HA)$ is $3$. What is its degree of dissociation ?......$\%$
$pH$ 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