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The pH of a 0.01 M solution of a weak acid having degree of dissociation 12.5% is ____. (Answer up to 1 decimal place)
Correct answer is '2.9'. Can you explain this answer?
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The pH of a 0.01 M solution of a weak acid having degree of dissociati...
Understanding the Problem
To find the pH of a weak acid solution, we need to understand its dissociation. Given a 0.01 M solution with a degree of dissociation of 12.5%, we can calculate the concentration of hydrogen ions.
Calculating Degree of Dissociation
- Degree of dissociation (α) = 12.5% = 0.125
- For a weak acid, the dissociation can be represented as:
HA ⇌ H⁺ + A⁻
- If the initial concentration of HA is 0.01 M, the concentration of H⁺ ions produced can be calculated as follows:
- H⁺ produced = 0.01 M × 0.125 = 0.00125 M
Calculating pH
- pH is calculated using the formula:
pH = -log[H⁺]
- Substituting the concentration of H⁺ ions:
pH = -log(0.00125)
Final Calculation
- To find -log(0.00125):
- log(0.00125) ≈ -2.9 (using logarithmic properties)
- Therefore, pH = 2.9.
Conclusion
Thus, the pH of a 0.01 M solution of the weak acid with a degree of dissociation of 12.5% is approximately 2.9. This indicates that the solution is acidic, as expected for a weak acid.
To find the pH of a weak acid solution, we need to understand its dissociation. Given a 0.01 M solution with a degree of dissociation of 12.5%, we can calculate the concentration of hydrogen ions.
Calculating Degree of Dissociation
- Degree of dissociation (α) = 12.5% = 0.125
- For a weak acid, the dissociation can be represented as:
HA ⇌ H⁺ + A⁻
- If the initial concentration of HA is 0.01 M, the concentration of H⁺ ions produced can be calculated as follows:
- H⁺ produced = 0.01 M × 0.125 = 0.00125 M
Calculating pH
- pH is calculated using the formula:
pH = -log[H⁺]
- Substituting the concentration of H⁺ ions:
pH = -log(0.00125)
Final Calculation
- To find -log(0.00125):
- log(0.00125) ≈ -2.9 (using logarithmic properties)
- Therefore, pH = 2.9.
Conclusion
Thus, the pH of a 0.01 M solution of the weak acid with a degree of dissociation of 12.5% is approximately 2.9. This indicates that the solution is acidic, as expected for a weak acid.
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The pH of a 0.01 M solution of a weak acid having degree of dissociation 12.5% is ____. (Answer up to 1 decimal place)Correct answer is '2.9'. Can you explain this answer?
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The pH of a 0.01 M solution of a weak acid having degree of dissociation 12.5% is ____. (Answer up to 1 decimal place)Correct answer is '2.9'. 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 The pH of a 0.01 M solution of a weak acid having degree of dissociation 12.5% is ____. (Answer up to 1 decimal place)Correct answer is '2.9'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The pH of a 0.01 M solution of a weak acid having degree of dissociation 12.5% is ____. (Answer up to 1 decimal place)Correct answer is '2.9'. Can you explain this answer?.
The pH of a 0.01 M solution of a weak acid having degree of dissociation 12.5% is ____. (Answer up to 1 decimal place)Correct answer is '2.9'. 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 The pH of a 0.01 M solution of a weak acid having degree of dissociation 12.5% is ____. (Answer up to 1 decimal place)Correct answer is '2.9'. Can you explain this answer? covers all topics & solutions for JEE 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for The pH of a 0.01 M solution of a weak acid having degree of dissociation 12.5% is ____. (Answer up to 1 decimal place)Correct answer is '2.9'. Can you explain this answer?.
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