Ionisation constant of $CH_3COOH$ is $1.7 \times 10^{-5}$ and concentration of $H^+$ ions is $3.4 \times 10^{-4}$. Then find out initial concentration of $CH_3COOH$ Molecules
$3.4 \times {10^{ - 4}}$
$3.4 \times {10^{ - 3}}$
$6.8 \times {10^{ - 4}}$
$6.8 \times {10^{ - 3}}$
The $pH$ value of decinormal solution of $N{H_4}OH$ which is $20\%$ ionised, is
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
At $298$ $K$ temperature, the ${K_b}$ of ${\left( {C{H_3}} \right)_2}NH$ is $5.4 \times {10^{ - 4}}$ $0.25$ $M$ solution.
$5.0$ $pH$ containing solution is dilute $100$ times. Calculate $pH$ of dilute solution.