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The ratio of volumes of CH3COOH 0.1(N) to CH3COONa 0.1(N) required to prepare a buffer solution of pH 5.74 is(given pKa of CH3COOH is 4.74):?
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The ratio of volumes of CH3COOH 0.1(N) to CH3COONa 0.1(N) required to ...
Introduction:
To prepare a buffer solution of pH 5.74 using acetic acid (CH3COOH) and sodium acetate (CH3COONa), we need to calculate the ratio of their volumes. The ratio depends on the Henderson-Hasselbalch equation, which relates the pH of a buffer solution to the pKa of the weak acid and the concentrations of the acid and its conjugate base.
Henderson-Hasselbalch equation:
The Henderson-Hasselbalch equation is given as follows:
Where:
- pH is the desired pH of the buffer solution
- pKa is the dissociation constant of the weak acid
- [A-] is the concentration of the conjugate base (CH3COO-)
- [HA] is the concentration of the weak acid (CH3COOH)
Given information:
- pKa of acetic acid (CH3COOH) = 4.74
- pH of the buffer solution = 5.74
Calculating the ratio:
1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio [A-]/[HA]:
pH - pKa = log([A-]/[HA])
2. Substitute the given values:
5.74 - 4.74 = log([A-]/[HA])
3. Solve for the ratio:
[A-]/[HA] = 10^(5.74 - 4.74)
4. Calculate the exponent:
[A-]/[HA] = 10^1
5. Simplify:
[A-]/[HA] = 10
Interpreting the ratio:
The ratio of the volumes of CH3COOH and CH3COONa required to prepare a buffer solution of pH 5.74 is 10. This means that for every 1 volume of acetic acid (CH3COOH), we need to add 10 volumes of sodium acetate (CH3COONa) to create the desired buffer solution.
Conclusion:
To prepare a buffer solution of pH 5.74 using acetic acid and sodium acetate, the ratio of their volumes is 1:10. This ratio is derived from the Henderson-Hasselbalch equation by substituting the given values of pH and pKa. The obtained ratio indicates that we need to add 10 times more sodium acetate than acetic acid to achieve the desired pH.
To prepare a buffer solution of pH 5.74 using acetic acid (CH3COOH) and sodium acetate (CH3COONa), we need to calculate the ratio of their volumes. The ratio depends on the Henderson-Hasselbalch equation, which relates the pH of a buffer solution to the pKa of the weak acid and the concentrations of the acid and its conjugate base.
Henderson-Hasselbalch equation:
The Henderson-Hasselbalch equation is given as follows:
Where:
- pH is the desired pH of the buffer solution
- pKa is the dissociation constant of the weak acid
- [A-] is the concentration of the conjugate base (CH3COO-)
- [HA] is the concentration of the weak acid (CH3COOH)
Given information:
- pKa of acetic acid (CH3COOH) = 4.74
- pH of the buffer solution = 5.74
Calculating the ratio:
1. Rearrange the Henderson-Hasselbalch equation to solve for the ratio [A-]/[HA]:
pH - pKa = log([A-]/[HA])
2. Substitute the given values:
5.74 - 4.74 = log([A-]/[HA])
3. Solve for the ratio:
[A-]/[HA] = 10^(5.74 - 4.74)
4. Calculate the exponent:
[A-]/[HA] = 10^1
5. Simplify:
[A-]/[HA] = 10
Interpreting the ratio:
The ratio of the volumes of CH3COOH and CH3COONa required to prepare a buffer solution of pH 5.74 is 10. This means that for every 1 volume of acetic acid (CH3COOH), we need to add 10 volumes of sodium acetate (CH3COONa) to create the desired buffer solution.
Conclusion:
To prepare a buffer solution of pH 5.74 using acetic acid and sodium acetate, the ratio of their volumes is 1:10. This ratio is derived from the Henderson-Hasselbalch equation by substituting the given values of pH and pKa. The obtained ratio indicates that we need to add 10 times more sodium acetate than acetic acid to achieve the desired pH.
Community Answer
The ratio of volumes of CH3COOH 0.1(N) to CH3COONa 0.1(N) required to ...
1:10
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The ratio of volumes of CH3COOH 0.1(N) to CH3COONa 0.1(N) required to prepare a buffer solution of pH 5.74 is(given pKa of CH3COOH is 4.74):?
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The ratio of volumes of CH3COOH 0.1(N) to CH3COONa 0.1(N) required to prepare a buffer solution of pH 5.74 is(given pKa of CH3COOH is 4.74):? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about The ratio of volumes of CH3COOH 0.1(N) to CH3COONa 0.1(N) required to prepare a buffer solution of pH 5.74 is(given pKa of CH3COOH is 4.74):? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The ratio of volumes of CH3COOH 0.1(N) to CH3COONa 0.1(N) required to prepare a buffer solution of pH 5.74 is(given pKa of CH3COOH is 4.74):?.
The ratio of volumes of CH3COOH 0.1(N) to CH3COONa 0.1(N) required to prepare a buffer solution of pH 5.74 is(given pKa of CH3COOH is 4.74):? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about The ratio of volumes of CH3COOH 0.1(N) to CH3COONa 0.1(N) required to prepare a buffer solution of pH 5.74 is(given pKa of CH3COOH is 4.74):? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The ratio of volumes of CH3COOH 0.1(N) to CH3COONa 0.1(N) required to prepare a buffer solution of pH 5.74 is(given pKa of CH3COOH is 4.74):?.
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