Calculate the degree of ionization and H3O' of 0.01M CH3COOH solution the equilibrium constant of acetic acid is 1.8 multiply 10'-5?

Question

Calculate the degree of ionization and H3O'  of 0.01M CH3COOH solution the equilibrium constant of acetic acid is 1.8 multiply 10'-5?

Answer

On balancing eq.we get 1.8*10^-5=cx^2/1-x
X^2/1-x=18*10-4
d.o.i.=4.3*10-2

Answer

Calculating the Degree of Ionization and H3O+ Concentration of a 0.01M CH3COOH Solution

Introduction

Acetic acid (CH3COOH) is a weak acid that partially dissociates in water. The degree of ionization (α) represents the fraction of the acid molecules that have ionized at equilibrium. To calculate the degree of ionization and the concentration of H3O+ ions in a 0.01M CH3COOH solution, we need to use the equilibrium constant (Ka) of acetic acid. The equilibrium constant expression for the dissociation of acetic acid is as follows:

CH3COOH ⇌ CH3COO- + H3O+

The equilibrium constant (Ka) for this reaction is given as 1.8 × 10^-5.

Calculating the Degree of Ionization (α)

The degree of ionization (α) can be calculated using the formula:

α = √(Ka * C)

Where Ka is the equilibrium constant and C is the initial concentration of the acid.

α = √(1.8 × 10^-5 * 0.01)

Calculating this expression will give us the degree of ionization (α).

Calculating the Concentration of H3O+ Ions

The concentration of H3O+ ions at equilibrium can be calculated using the formula:

[H3O+] = α * C

Where α is the degree of ionization and C is the initial concentration of the acid.

[H3O+] = α * 0.01

Calculating this expression will give us the concentration of H3O+ ions in the solution.

Results

By plugging in the values into the formulas, we can calculate the degree of ionization (α) and the concentration of H3O+ ions in the 0.01M CH3COOH solution.

α = √(1.8 × 10^-5 * 0.01)
α = √(1.8 × 10^-7)
α ≈ 0.0013 (rounded to four decimal places)

[H3O+] = 0.0013 * 0.01
[H3O+] ≈ 1.3 × 10^-5 M (rounded to four decimal places)

Conclusion

The degree of ionization of the 0.01M CH3COOH solution is approximately 0.0013, indicating that only a small fraction of the acetic acid molecules have ionized at equilibrium. The concentration of H3O+ ions in the solution is approximately 1.3 × 10^-5 M, representing the concentration of the hydronium ions formed from the ionization of acetic acid.

Similar Class 11 Doubts

The ionization constant of acetic acid is1.74 x 10−5. Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH.

Find the percentage ionization of 0.2M acetic acid solution,whose dissociation constant is 1.8*10-5

In aqueous solution the ionization constants for carbonic acid are and Selection the correct statement for a saturated 0.034 M solution of the carbonic acid. [AIEEE-2010]

At a temperature under high pressure equilibrium constant of water is 1×10^-10. A solution of pH 5.4 under these conditions is said to be?

One mole of PCl5 is heated with one litre of closed container. If 0.6 mole of chloride is found at equilibrium, calculate the value of equilibrium constant Related: Law of Chemical Equilibrium and Equilibrium Constant - Equilibrium, CBSE, Class 11, Chemistry

Top Courses for Class 11View all

Chemistry Class 11

CUET Mock Test: Humanities Subjects 2025

English Class 11

Mathematics (Maths) Class 11

Psychology Practice Tests: CUET Preparation

Top Courses for Class 11

Top Courses for Class 11

Suggested Free Tests

Related Content

Schools

Competitive Examinations

Quick Access Links

Technical Exams