(D) Given: $K_{a} = 1 \times 10^{-5}$,$c = 0.1 \ M$. For a weak acid,the dissociation constant is given by $K_{a} = \alpha^2 c$. Therefore,$\alpha = \

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

(D) Given: $K_{a} = 1 \times 10^{-5}$,$c = 0.1 \ M$. For a weak acid,the dissociation constant is given by $K_{a} = \alpha^2 c$. Therefore,$\alpha = \sqrt{\frac{K_{a}}{c}} = \sqrt{\frac{1 \times 10^{-5}}{0.1}} = \sqrt{1 \times 10^{-4}} = 0.01$. Percent dissociation $= \alpha \times 100$. Percent dissociation $= 0.01 \times 100 = 1.0 \%$.

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

Medium

Weak acid $HX$ has dissociation constant $1 \times 10^{-5}$. Calculate the percent dissociation in its $0.1 \ M$ solution. (in $\%$)

MHT CET 2023 All MHT CET

A
$2.2$
B
$3.5$
C
$4.2$
D
$1.0$

Explore More

Browse All

Question Bank

All Subjects

Class 11 Questions

Class 11

Chemistry Questions

Chapter

2 Equilibrium: Ionic Equilibrium

Subtopic

pH of weak Acids and weak Bases

Previous Year

MHT CET 2023 Paper All MHT CET years →

If the $pH$ of $0.10 \ M$ monoacidic base at $298 \ K$ is $9.0$,the value of $K_{b}$ and $pK_{b}$ at the same temperature are respectively:

MediumAP EAMCET 2018

View Solution

An organic monobasic acid has a dissociation constant of $1.96 \times 10^{-8}$. What is its percentage dissociation in a $0.01 \text{ M}$ solution (in $\%$)?

DifficultMHT CET 2026

View Solution

Calculate the dissociation constant of a weak monobasic acid if it is $0.05 \%$ dissociated in a $0.02 \ M$ solution.

DifficultMHT CET 2024

View Solution

The ionization constant of $0.1$ $M$ weak acid is $1.74 \times 10^{-5}$ at $298$ $K$ temperature. Calculate the $pH$ of its $0.1$ $M$ solution. (in $.88$)

Difficult

View Solution

Which of the following compounds has the maximum $K_{a}$ value?

Medium

View Solution

Vedclass Products

For Students

Vedclass Test Series

Mock tests in real JEE/NEET style with performance analysis. 5-day free trial.

Start Free Trial

For Teachers

Exam Paper Generator

Generate Set A/B/C/D exam papers from 7.5L+ questions in 2 minutes. 3 chapters free.

Try Free

For Institutes

Online Exam Module

Live online exams with unlimited students, 360° analytics & white-label branding.

See Demo

Weak acid $HX$ has dissociation constant $1 \times 10^{-5}$. Calculate the percent dissociation in its $0.1 \ M$ solution. (in $\%$)

Similar Questions

If the $pH$ of $0.10 \ M$ monoacidic base at $298 \ K$ is $9.0$,the value of $K_{b}$ and $pK_{b}$ at the same temperature are respectively:

An organic monobasic acid has a dissociation constant of $1.96 \times 10^{-8}$. What is its percentage dissociation in a $0.01 \text{ M}$ solution (in $\%$)?

Calculate the dissociation constant of a weak monobasic acid if it is $0.05 \%$ dissociated in a $0.02 \ M$ solution.

The ionization constant of $0.1$ $M$ weak acid is $1.74 \times 10^{-5}$ at $298$ $K$ temperature. Calculate the $pH$ of its $0.1$ $M$ solution. (in $.88$)

Which of the following compounds has the maximum $K_{a}$ value?

Vedclass Test Series

Exam Paper Generator

Online Exam Module