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A solution of chloroacetic acid, ClCH2COOH containing 9.45 grams in 500 ml of the solution has a pH of 2.0. What is the degree of ionization the acid.
- a)α = 0.09
- b)α = 0.05
- c)α = 0.07
- d)α = 0.15
Correct answer is option 'B'. Can you explain this answer?
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Verified Answer
A solution of chloroacetic acid, ClCH2COOH containing 9.45 grams in 50...
MW of ClCH2COOH = 44.5
∴ [acid] = 0.1 × 2 = 0.2 M
∴ [acid] = 0.1 × 2 = 0.2 M
Most Upvoted Answer
A solution of chloroacetic acid, ClCH2COOH containing 9.45 grams in 50...
PH of the solution can be calculated using the equation:
pH = -log[H+]
where [H+] is the concentration of hydrogen ions in the solution.
To find the concentration of hydrogen ions, we need to consider the dissociation of chloroacetic acid:
ClCH2COOH ⇌ ClCH2COO- + H+
The degree of ionization, α, is defined as the ratio of the concentration of dissociated acid to the initial concentration of the acid:
α = [H+] / [ClCH2COOH]
Given that the initial concentration of chloroacetic acid is 9.45 grams in 500 ml of solution, we need to convert the mass to moles and the volume to liters.
Step 1: Convert mass to moles
Molar mass of chloroacetic acid (ClCH2COOH) = 2(1.01) + 12.01 + 2(1.01) + 12.01 + 16.00 + 1.01 = 94.50 g/mol
Number of moles of chloroacetic acid = mass / molar mass
= 9.45 g / 94.50 g/mol
= 0.10 mol
Step 2: Convert volume to liters
Volume of solution = 500 ml = 500/1000 L
= 0.50 L
Step 3: Calculate the concentration of chloroacetic acid
Concentration (C) = moles / volume
= 0.10 mol / 0.50 L
= 0.20 M
Now, we can substitute the values into the equation for α:
α = [H+] / [ClCH2COOH]
α = 10^(-pH)
α = 10^(-2)
α = 0.01
Therefore, the degree of ionization of chloroacetic acid in the given solution is 0.01 or 1%.
However, the correct answer provided is option B, which states that the degree of ionization is 0.05 or 5%. This is not correct based on the calculations. It is possible that there is an error in the answer key or in the options provided.
pH = -log[H+]
where [H+] is the concentration of hydrogen ions in the solution.
To find the concentration of hydrogen ions, we need to consider the dissociation of chloroacetic acid:
ClCH2COOH ⇌ ClCH2COO- + H+
The degree of ionization, α, is defined as the ratio of the concentration of dissociated acid to the initial concentration of the acid:
α = [H+] / [ClCH2COOH]
Given that the initial concentration of chloroacetic acid is 9.45 grams in 500 ml of solution, we need to convert the mass to moles and the volume to liters.
Step 1: Convert mass to moles
Molar mass of chloroacetic acid (ClCH2COOH) = 2(1.01) + 12.01 + 2(1.01) + 12.01 + 16.00 + 1.01 = 94.50 g/mol
Number of moles of chloroacetic acid = mass / molar mass
= 9.45 g / 94.50 g/mol
= 0.10 mol
Step 2: Convert volume to liters
Volume of solution = 500 ml = 500/1000 L
= 0.50 L
Step 3: Calculate the concentration of chloroacetic acid
Concentration (C) = moles / volume
= 0.10 mol / 0.50 L
= 0.20 M
Now, we can substitute the values into the equation for α:
α = [H+] / [ClCH2COOH]
α = 10^(-pH)
α = 10^(-2)
α = 0.01
Therefore, the degree of ionization of chloroacetic acid in the given solution is 0.01 or 1%.
However, the correct answer provided is option B, which states that the degree of ionization is 0.05 or 5%. This is not correct based on the calculations. It is possible that there is an error in the answer key or in the options provided.
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A solution of chloroacetic acid, ClCH2COOH containing 9.45 grams in 500 ml of the solution has a pH of 2.0. What is the degree of ionization the acid.a)α = 0.09b)α = 0.05c)α = 0.07d)α = 0.15Correct answer is option 'B'. Can you explain this answer?
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A solution of chloroacetic acid, ClCH2COOH containing 9.45 grams in 500 ml of the solution has a pH of 2.0. What is the degree of ionization the acid.a)α = 0.09b)α = 0.05c)α = 0.07d)α = 0.15Correct answer is option 'B'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about A solution of chloroacetic acid, ClCH2COOH containing 9.45 grams in 500 ml of the solution has a pH of 2.0. What is the degree of ionization the acid.a)α = 0.09b)α = 0.05c)α = 0.07d)α = 0.15Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A solution of chloroacetic acid, ClCH2COOH containing 9.45 grams in 500 ml of the solution has a pH of 2.0. What is the degree of ionization the acid.a)α = 0.09b)α = 0.05c)α = 0.07d)α = 0.15Correct answer is option 'B'. Can you explain this answer?.
A solution of chloroacetic acid, ClCH2COOH containing 9.45 grams in 500 ml of the solution has a pH of 2.0. What is the degree of ionization the acid.a)α = 0.09b)α = 0.05c)α = 0.07d)α = 0.15Correct answer is option 'B'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about A solution of chloroacetic acid, ClCH2COOH containing 9.45 grams in 500 ml of the solution has a pH of 2.0. What is the degree of ionization the acid.a)α = 0.09b)α = 0.05c)α = 0.07d)α = 0.15Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A solution of chloroacetic acid, ClCH2COOH containing 9.45 grams in 500 ml of the solution has a pH of 2.0. What is the degree of ionization the acid.a)α = 0.09b)α = 0.05c)α = 0.07d)α = 0.15Correct answer is option 'B'. Can you explain this answer?.
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