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Calculate the pH of a mixture of 0.10M acetic acid and 0.20M sodium acetate. The pKa of acetic acid is 4.76.
- a)5.1
- b)4.1
- c)6.1
- d)7.1
Correct answer is option 'A'. Can you explain this answer?
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Verified Answer
Calculate the pH of a mixture of 0.10M acetic acid and 0.20M sodium ac...
pH = pKa + log [acetate]/[acetic acid] = 4.76 + log (0.2/0.1)
= 4.76 + 0.30
= 5.1.
= 4.76 + 0.30
= 5.1.
Most Upvoted Answer
Calculate the pH of a mixture of 0.10M acetic acid and 0.20M sodium ac...
Given:
- Concentration of acetic acid (CH3COOH): 0.10 M
- Concentration of sodium acetate (CH3COONa): 0.20 M
- pKa of acetic acid: 4.76
To find:
The pH of the mixture of acetic acid and sodium acetate.
Explanation:
The given mixture contains both a weak acid (acetic acid) and its conjugate base (acetate ion). When a weak acid and its conjugate base are present together in a solution, they undergo a reaction known as a buffer reaction. The buffer can resist changes in pH when small amounts of acid or base are added.
The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation:
Where:
- pH is the hydrogen ion concentration
- pKa is the logarithmic acid dissociation constant
- [A-] is the concentration of the conjugate base (acetate ion)
- [HA] is the concentration of the weak acid (acetic acid)
Step 1: Calculate the ratio of [A-]/[HA]:
[A-]/[HA] = (concentration of acetate ion) / (concentration of acetic acid)
= 0.20 M / 0.10 M
= 2
Step 2: Calculate the pH:
pH = pKa + log ([A-]/[HA])
= 4.76 + log (2)
= 4.76 + 0.301
= 5.061
Answer:
The pH of the mixture of 0.10 M acetic acid and 0.20 M sodium acetate is approximately 5.1. Therefore, the correct option is (A).
- Concentration of acetic acid (CH3COOH): 0.10 M
- Concentration of sodium acetate (CH3COONa): 0.20 M
- pKa of acetic acid: 4.76
To find:
The pH of the mixture of acetic acid and sodium acetate.
Explanation:
The given mixture contains both a weak acid (acetic acid) and its conjugate base (acetate ion). When a weak acid and its conjugate base are present together in a solution, they undergo a reaction known as a buffer reaction. The buffer can resist changes in pH when small amounts of acid or base are added.
The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation:
Where:
- pH is the hydrogen ion concentration
- pKa is the logarithmic acid dissociation constant
- [A-] is the concentration of the conjugate base (acetate ion)
- [HA] is the concentration of the weak acid (acetic acid)
Step 1: Calculate the ratio of [A-]/[HA]:
[A-]/[HA] = (concentration of acetate ion) / (concentration of acetic acid)
= 0.20 M / 0.10 M
= 2
Step 2: Calculate the pH:
pH = pKa + log ([A-]/[HA])
= 4.76 + log (2)
= 4.76 + 0.301
= 5.061
Answer:
The pH of the mixture of 0.10 M acetic acid and 0.20 M sodium acetate is approximately 5.1. Therefore, the correct option is (A).
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Calculate the pH of a mixture of 0.10M acetic acid and 0.20M sodium acetate. The pKa of acetic acid is 4.76.a)5.1b)4.1c)6.1d)7.1Correct answer is option 'A'. Can you explain this answer?
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Calculate the pH of a mixture of 0.10M acetic acid and 0.20M sodium acetate. The pKa of acetic acid is 4.76.a)5.1b)4.1c)6.1d)7.1Correct answer is option 'A'. Can you explain this answer? for IIT JAM 2024 is part of IIT JAM preparation. The Question and answers have been prepared according to the IIT JAM exam syllabus. Information about Calculate the pH of a mixture of 0.10M acetic acid and 0.20M sodium acetate. The pKa of acetic acid is 4.76.a)5.1b)4.1c)6.1d)7.1Correct answer is option 'A'. Can you explain this answer? covers all topics & solutions for IIT JAM 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for Calculate the pH of a mixture of 0.10M acetic acid and 0.20M sodium acetate. The pKa of acetic acid is 4.76.a)5.1b)4.1c)6.1d)7.1Correct answer is option 'A'. Can you explain this answer?.
Solutions for Calculate the pH of a mixture of 0.10M acetic acid and 0.20M sodium acetate. The pKa of acetic acid is 4.76.a)5.1b)4.1c)6.1d)7.1Correct answer is option 'A'. Can you explain this answer? in English & in Hindi are available as part of our courses for IIT JAM.
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