At $298\,K$ a $0.1 \,M $ $C{H_3}COOH$ solution is $ 1.34\%$ ionized. The ionization constant ${K_a}$ for acetic acid will be
$1.82 \times {10^{ - 5}}$
$18.2 \times {10^{ - 5}}$
$0.182 \times {10^{ - 5}}$
None of these
The $pH$ of $0.1\, M$ monobasic acid is $4.50$ Calculate the concentration of species $H ^{+},$ $A^{-}$ and $HA$ at equilibrium. Also, determine the value of $K_{a}$ and $pK _{a}$ of the monobasic acid.
At $25\,^oC$, the dissociation constant of $CH_3COOH$ and $NH_4OH$ in aqueous solution are almost the same. The $pH$ of a solution $0.01\, N\, CH_3COOH$ is $4.0$ at $25\,^oC$. The $pH$ of $0.01\, N\, NH_4OH$ solution at the same temperature would be
In its $0.2\,\, M$ solution, an acid ionises to an extent of $60\%$. Its hydrogen ion concentration is.....$M$
Heat of neutralisation of weak acid and strong base is less than the heat of neutralisation of strong acid and strong base due to
The ionization constant of benzoic acid is $6.5 \times {10^{ - 5}}$ at $298$ $K$ temperature. Calculate $pH$ of its $0.15$ $M$ solution.