NEET Exam > NEET Questions > If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– ...
Start Learning for Free
If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.
- a)2.09
- b)5.14
- c)2.65
- d)3.98
Correct answer is option 'B'. Can you explain this answer?
| FREE This question is part of | Download PDF Attempt this Test |
Most Upvoted Answer
If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer so...
Understanding Buffer Solutions
Buffer solutions resist changes in pH when small amounts of acid or base are added. In this case, we have acetic acid (CH3COOH) and its conjugate base, acetate (CH3COO–), forming a buffer.
Given Data
- Concentration of CH3COOH = 0.20 mol/L
- Concentration of CH3COO– = 0.50 mol/L
- Acid dissociation constant (Ka) of CH3COOH = 1.8 × 10⁻⁵
Calculating pKa
To find pH, we first need to calculate the pKa from the given Ka:
- pKa = -log(Ka)
- pKa = -log(1.8 × 10⁻⁵) ≈ 4.74
Using the Henderson-Hasselbalch Equation
The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation:
Where:
- [A⁻] = concentration of the conjugate base (CH3COO–)
- [HA] = concentration of the weak acid (CH3COOH)
Substituting the Values
Now we substitute in the values:
- pH = 4.74 + log(0.50 / 0.20)
Calculating the Logarithm
- Log(0.50 / 0.20) = log(2.5) ≈ 0.39794
Final pH Calculation
Now, substituting this back into the equation:
- pH = 4.74 + 0.39794 ≈ 5.14
Conclusion
The calculated pH of the buffer solution is approximately 5.14, which corresponds to option 'B'.
Buffer solutions resist changes in pH when small amounts of acid or base are added. In this case, we have acetic acid (CH3COOH) and its conjugate base, acetate (CH3COO–), forming a buffer.
Given Data
- Concentration of CH3COOH = 0.20 mol/L
- Concentration of CH3COO– = 0.50 mol/L
- Acid dissociation constant (Ka) of CH3COOH = 1.8 × 10⁻⁵
Calculating pKa
To find pH, we first need to calculate the pKa from the given Ka:
- pKa = -log(Ka)
- pKa = -log(1.8 × 10⁻⁵) ≈ 4.74
Using the Henderson-Hasselbalch Equation
The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation:
Where:
- [A⁻] = concentration of the conjugate base (CH3COO–)
- [HA] = concentration of the weak acid (CH3COOH)
Substituting the Values
Now we substitute in the values:
- pH = 4.74 + log(0.50 / 0.20)
Calculating the Logarithm
- Log(0.50 / 0.20) = log(2.5) ≈ 0.39794
Final pH Calculation
Now, substituting this back into the equation:
- pH = 4.74 + 0.39794 ≈ 5.14
Conclusion
The calculated pH of the buffer solution is approximately 5.14, which corresponds to option 'B'.
Free Test
FREE
| Start Free Test |
Community Answer
If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer so...
We have the Henderson-Hasselbalch equation as pH = pKa + log[salt]/[acid]. So by substituting the concentrations of salt and acid along with the acid dissociation constant, we get pH = -log[1.8 × 10-5] + log [0.50 mol/L]/[0.20 mol/L] = 5.14.
Attention NEET Students!
To make sure you are not studying endlessly, EduRev has designed NEET study material, with Structured Courses, Videos, & Test Series. Plus get personalized analysis, doubt solving and improvement plans to achieve a great score in NEET.
|
Explore Courses for NEET exam
|
|
Similar NEET Doubts
Top Courses for NEETView all
If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer?
Question Description
If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer?.
If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer? for NEET 2024 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for NEET 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer?.
Solutions for If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer? in English & in Hindi are available as part of our courses for NEET.
Download more important topics, notes, lectures and mock test series for NEET Exam by signing up for free.
Here you can find the meaning of If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer?, a detailed solution for If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer? has been provided alongside types of If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice If 0.20 mol/L CH3COOH and 0.50 mol/L CH3COO– together make a buffer solution, calculate the pH of the solution if the acid dissociation constant of CH3COOH is 1.8 × 10-5.a)2.09b)5.14c)2.65d)3.98Correct answer is option 'B'. Can you explain this answer? tests, examples and also practice NEET tests.
|
|
Explore Courses for NEET exam
|
|
Suggested Free Tests
Signup for Free!
Signup to see your scores go up within 7 days! Learn & Practice with 1000+ FREE Notes, Videos & Tests.
|
© EduRev
|
Education Revolution
|
|
Signup to see your scores
go up within 7 days!
Access 1000+ FREE Docs, Videos and Tests
Takes less than 10 seconds to signup