(A) Given,concentration $C = 0.01 \ mol/L = 10^{-2} \ mol/L$ and $pH = 4$. The concentration of hydrogen ions is $[H^{+}] = 10^{-pH} = 10^{-4} \ mol/L

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(A) Given,concentration $C = 0.01 \ mol/L = 10^{-2} \ mol/L$ and $pH = 4$. The concentration of hydrogen ions is $[H^{+}] = 10^{-pH} = 10^{-4} \ mol/L$. The degree of ionisation $\alpha$ is given by $\alpha = \frac{[H^{+}]}{C} = \frac{10^{-4}}{10^{-2}} = 10^{-2}$. Percentage degree of ionisation = $\alpha \times 100 = 10^{-2} \times 100 = 1\%$. The ionisation constant $K_a$ is given by $K_a = C \alpha^2 = 10^{-2} \times (10^{-2})^2 = 10^{-2} \times 10^{-4} = 10^{-6}$.

Class 11 Chemistry 2 Equilibrium: Ionic Equilibrium pH of weak Acids and weak Bases

Medium

$A$ solution of weak acid $HA$ containing $0.01 \ mol/L$ of acid 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
$0.01\%, \ 10^{-6}$

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2 Equilibrium: Ionic Equilibrium

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pH of weak Acids and weak Bases

For an aqueous solution of $H_2CO_3$,the ionization constants are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$. Which statement is correct for a $0.034 \ M$ saturated solution of carbonic acid?

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The ionization constant of benzoic acid is $6.5 \times 10^{-5}$ at $298 \ K$ temperature. Calculate $pH$ of its $0.15 \ M$ solution. (in $.5$)

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For a $0.1 \ M$ solution of a weak acid $HQ$,the $pH$ is $3$. The ionization constant $K_a$ of the acid is:

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$0.02 \, M$ monobasic acid dissociates $2 \%$,hence,$pH$ of the solution is

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The $K_a$ of monobasic acid $A, B$ and $C$ are $10^{-6}, 10^{-8}$ and $10^{-10}$ respectively. The concentrations of $A, B$ and $C$ are respectively $0.1 \ M, 0.01 \ M$ and $0.001 \ M$. Which of the following is correct for $pOH$ of $A, B$ and $C$?

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$A$ solution of weak acid $HA$ containing $0.01 \ mol/L$ of acid has $pH = 4$. The percentage degree of ionisation of the acid and the ionisation constant of acid are respectively.

Similar Questions

For an aqueous solution of $H_2CO_3$,the ionization constants are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$. Which statement is correct for a $0.034 \ M$ saturated solution of carbonic acid?

The ionization constant of benzoic acid is $6.5 \times 10^{-5}$ at $298 \ K$ temperature. Calculate $pH$ of its $0.15 \ M$ solution. (in $.5$)

For a $0.1 \ M$ solution of a weak acid $HQ$,the $pH$ is $3$. The ionization constant $K_a$ of the acid is:

$0.02 \, M$ monobasic acid dissociates $2 \%$,hence,$pH$ of the solution is

The $K_a$ of monobasic acid $A, B$ and $C$ are $10^{-6}, 10^{-8}$ and $10^{-10}$ respectively. The concentrations of $A, B$ and $C$ are respectively $0.1 \ M, 0.01 \ M$ and $0.001 \ M$. Which of the following is correct for $pOH$ of $A, B$ and $C$?

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