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Ionization constant of acetic acid is 1.8 * 10-5. The concentration of H+ ions in 0.1 M solution is
- a)1.8 x 10-3 M
- b)1.8 x 10-5 M
- c)1.3 * 1 0-3 M
- d)1.34 * 10-3 M
Correct answer is option 'D'. Can you explain this answer?
Most Upvoted Answer
Ionization constant of acetic acid is 1.8 * 10-5. The concentration of...
Calculating the concentration of H+ ions in a 0.1M acetic acid solution
Given:
Ionization constant of acetic acid (Ka) = 1.8 * 10^-5
Concentration of acetic acid (CH3COOH) = 0.1M
Step 1: Writing the dissociation equation of acetic acid
CH3COOH + H2O ⇌ CH3COO- + H3O+
Step 2: Writing the equilibrium expression for the dissociation reaction
Ka = [CH3COO-][H3O+] / [CH3COOH]
Step 3: Assuming that the dissociation of acetic acid is small compared to its initial concentration, we can assume that the concentration of the undissociated acetic acid is approximately equal to its initial concentration (0.1M).
Step 4: Using the equilibrium expression and the given Ka value, we can calculate the concentration of H+ ions in the solution.
Ka = [CH3COO-][H3O+] / [CH3COOH]
1.8 * 10^-5 = [x][x] / [0.1]
x^2 = 1.8 * 10^-6
x = 1.34 * 10^-3 M
Therefore, the concentration of H+ ions in the 0.1M acetic acid solution is 1.34 * 10^-3 M, which is closest to option D.
Given:
Ionization constant of acetic acid (Ka) = 1.8 * 10^-5
Concentration of acetic acid (CH3COOH) = 0.1M
Step 1: Writing the dissociation equation of acetic acid
CH3COOH + H2O ⇌ CH3COO- + H3O+
Step 2: Writing the equilibrium expression for the dissociation reaction
Ka = [CH3COO-][H3O+] / [CH3COOH]
Step 3: Assuming that the dissociation of acetic acid is small compared to its initial concentration, we can assume that the concentration of the undissociated acetic acid is approximately equal to its initial concentration (0.1M).
Step 4: Using the equilibrium expression and the given Ka value, we can calculate the concentration of H+ ions in the solution.
Ka = [CH3COO-][H3O+] / [CH3COOH]
1.8 * 10^-5 = [x][x] / [0.1]
x^2 = 1.8 * 10^-6
x = 1.34 * 10^-3 M
Therefore, the concentration of H+ ions in the 0.1M acetic acid solution is 1.34 * 10^-3 M, which is closest to option D.
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Ionization constant of acetic acid is 1.8 * 10-5. The concentration of...
Since, acetic acid is a weak electrolyte, hence
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Ionization constant of acetic acid is 1.8 * 10-5. The concentration of H+ ions in 0.1 M solution isa)1.8 x 10-3 Mb)1.8 x 10-5 Mc)1.3 * 1 0-3 Md)1.34 * 10-3 MCorrect answer is option 'D'. Can you explain this answer?
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Ionization constant of acetic acid is 1.8 * 10-5. The concentration of H+ ions in 0.1 M solution isa)1.8 x 10-3 Mb)1.8 x 10-5 Mc)1.3 * 1 0-3 Md)1.34 * 10-3 MCorrect answer is option 'D'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Ionization constant of acetic acid is 1.8 * 10-5. The concentration of H+ ions in 0.1 M solution isa)1.8 x 10-3 Mb)1.8 x 10-5 Mc)1.3 * 1 0-3 Md)1.34 * 10-3 MCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Ionization constant of acetic acid is 1.8 * 10-5. The concentration of H+ ions in 0.1 M solution isa)1.8 x 10-3 Mb)1.8 x 10-5 Mc)1.3 * 1 0-3 Md)1.34 * 10-3 MCorrect answer is option 'D'. Can you explain this answer?.
Ionization constant of acetic acid is 1.8 * 10-5. The concentration of H+ ions in 0.1 M solution isa)1.8 x 10-3 Mb)1.8 x 10-5 Mc)1.3 * 1 0-3 Md)1.34 * 10-3 MCorrect answer is option 'D'. Can you explain this answer? for JEE 2025 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about Ionization constant of acetic acid is 1.8 * 10-5. The concentration of H+ ions in 0.1 M solution isa)1.8 x 10-3 Mb)1.8 x 10-5 Mc)1.3 * 1 0-3 Md)1.34 * 10-3 MCorrect answer is option 'D'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Ionization constant of acetic acid is 1.8 * 10-5. The concentration of H+ ions in 0.1 M solution isa)1.8 x 10-3 Mb)1.8 x 10-5 Mc)1.3 * 1 0-3 Md)1.34 * 10-3 MCorrect answer is option 'D'. Can you explain this answer?.
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Ionization constant of acetic acid is 1.8 * 10-5. The concentration of H+ ions in 0.1 M solution isa)1.8 x 10-3 Mb)1.8 x 10-5 Mc)1.3 * 1 0-3 Md)1.34 * 10-3 MCorrect answer is option 'D'. Can you explain this answer?, a detailed solution for Ionization constant of acetic acid is 1.8 * 10-5. The concentration of H+ ions in 0.1 M solution isa)1.8 x 10-3 Mb)1.8 x 10-5 Mc)1.3 * 1 0-3 Md)1.34 * 10-3 MCorrect answer is option 'D'. Can you explain this answer? has been provided alongside types of Ionization constant of acetic acid is 1.8 * 10-5. The concentration of H+ ions in 0.1 M solution isa)1.8 x 10-3 Mb)1.8 x 10-5 Mc)1.3 * 1 0-3 Md)1.34 * 10-3 MCorrect answer is option 'D'. Can you explain this answer? theory, EduRev gives you an
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