What is the $pH$ of the resulting solution when equal volumes of $0.1\, M\, NaOH$ and $0.01\, M\, HCl$ are mixed?
$2$
$7$
$1.04$
$12.65$
The percentage of pyridine $(C_5H_5N)$ that forms pyridinium ion $(C_5H_5N^+H)$ in a $0.10\, M$ aqueous pyridine solution ($K_b$ for $C_5H_5N = 1.7 \times 10^{-9}$) is
$pH$ 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
The $pH$ of $0.005 \,M$ codeine $\left( C _{18} H _{21} NO _{3}\right)$ solution is $9.95 .$ Calculate its ionization constant and $p K_{ b }$
A monoprotic acid in a $0.1\,\,M$ solution ionizes to $0.001\%$. Its ionisation constant is
Concentration $C{N^ - }$ in $0.1\,M\,HCN$ is $[{K_a} = 4 \times {10^{ - 10}}]$