A solution of weak acid $HA$ containing $0.01$ moles of acid per litre of solutions has $pH = 4$. The percentage degree of ionisation of the acid and the ionisation constant of acid are respectively.
A solution of weak acid $HA$ containing $0.01$ moles of acid per litre of solutions has $pH = 4$. The percentage degree of ionisation of the acid and the ionisation constant of acid are respectively.
- A
$1\% ,\,{10^{ - 6}}$
- B
$0.01\% ,\,{10^{ - 4}}$
- C
$1\% ,\,{10^{ - 4}}$
- D
$0.01\% ,\,{10^{ - 6}}$
Similar Questions
$0.01\, M \,HA(aq.)$ is $2\%$ ionized, $[OH^-]$ of solution is :-
$0.01\, M \,HA(aq.)$ is $2\%$ ionized, $[OH^-]$ of solution is :-
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
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
$50\ ml$ of $0.02\ M$ $NaHSO_4$ is mixed with $50$ $ml$ of $0.02\ M\ Na_2SO_4$. Calculate $pH$ of the resulting solution.$[pKa_2 (H_2SO_4) = 2]$
$50\ ml$ of $0.02\ M$ $NaHSO_4$ is mixed with $50$ $ml$ of $0.02\ M\ Na_2SO_4$. Calculate $pH$ of the resulting solution.$[pKa_2 (H_2SO_4) = 2]$
For a weak acid $HA,$ Ostwald's dilution law is represented by the equation
For a weak acid $HA,$ Ostwald's dilution law is represented by the equation
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
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
- [NEET 2016]