Class 11 Exam > Class 11 Questions > A buffer solution is prepared in which the co...
Start Learning for Free
A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]
- a)9.08
- b)9.43
- c)11.72
- d)8.73
Correct answer is option 'B'. Can you explain this answer?
| FREE This question is part of | Download PDF Attempt this Test |
Verified Answer
A buffer solution is prepared in which the concentration of NH3 is 0.3...
Given [NH3] = 0.3 M, [NH4+] = 0.2 M, Kb = 1.8 × 10–5.
∴ pKb = 4.74
= 4.56
pH = 14 – 4.56 = 9.436
pH = 14 – 4.56 = 9.436
Most Upvoted Answer
A buffer solution is prepared in which the concentration of NH3 is 0.3...
To find the value of Kb for NH3, we need to set up the equilibrium expression for the reaction:
NH3 + H2O ⇌ NH4+ + OH-
The equilibrium constant expression is given by:
Kb = [NH4+][OH-] / [NH3]
We are given the concentration of NH3 as 0.30 M and NH4+ as 0.20 M. However, we are not given the concentration of OH-. In order to calculate Kb, we need to determine the concentration of OH- at equilibrium.
Since NH3 is a weak base, it reacts with water to form OH-. The reaction is as follows:
NH3 + H2O ⇌ NH4+ + OH-
We can assume that the concentration of OH- at equilibrium is x M. Therefore, the concentration of NH4+ at equilibrium is also x M.
Using the given concentrations and the assumption above, we can set up the following equation:
Kb = (x)(x) / (0.30)
Simplifying, we have:
1.8 = x^2 / 0.30
Multiplying both sides by 0.30, we get:
0.54 = x^2
Taking the square root of both sides, we find:
x ≈ 0.735
Therefore, the concentration of OH- at equilibrium is approximately 0.735 M.
Now, we can substitute the values into the equilibrium constant expression to find Kb:
Kb = (0.20)(0.735) / (0.30) = 0.490
Therefore, the value of Kb for NH3 is approximately 0.490.
NH3 + H2O ⇌ NH4+ + OH-
The equilibrium constant expression is given by:
Kb = [NH4+][OH-] / [NH3]
We are given the concentration of NH3 as 0.30 M and NH4+ as 0.20 M. However, we are not given the concentration of OH-. In order to calculate Kb, we need to determine the concentration of OH- at equilibrium.
Since NH3 is a weak base, it reacts with water to form OH-. The reaction is as follows:
NH3 + H2O ⇌ NH4+ + OH-
We can assume that the concentration of OH- at equilibrium is x M. Therefore, the concentration of NH4+ at equilibrium is also x M.
Using the given concentrations and the assumption above, we can set up the following equation:
Kb = (x)(x) / (0.30)
Simplifying, we have:
1.8 = x^2 / 0.30
Multiplying both sides by 0.30, we get:
0.54 = x^2
Taking the square root of both sides, we find:
x ≈ 0.735
Therefore, the concentration of OH- at equilibrium is approximately 0.735 M.
Now, we can substitute the values into the equilibrium constant expression to find Kb:
Kb = (0.20)(0.735) / (0.30) = 0.490
Therefore, the value of Kb for NH3 is approximately 0.490.
Attention Class 11 Students!
To make sure you are not studying endlessly, EduRev has designed Class 11 study material, with Structured Courses, Videos, & Test Series. Plus get personalized analysis, doubt solving and improvement plans to achieve a great score in Class 11.
|
Explore Courses for Class 11 exam
|
|
Similar Class 11 Doubts
Top Courses for Class 11View all
A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer?
Question Description
A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer?.
A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer? for Class 11 2024 is part of Class 11 preparation. The Question and answers have been prepared according to the Class 11 exam syllabus. Information about A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for Class 11 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer?.
Solutions for A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer? in English & in Hindi are available as part of our courses for Class 11.
Download more important topics, notes, lectures and mock test series for Class 11 Exam by signing up for free.
Here you can find the meaning of A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer? defined & explained in the simplest way possible. Besides giving the explanation of
A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer?, a detailed solution for A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer? has been provided alongside types of A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice A buffer solution is prepared in which the concentration of NH3 is 0.30M and the concentration of NH4+ is 0.20 M. If the equilibrium constant, Kb for NH3 equals 1.8 × 10–5, what is the pH of this solution ? (log 2.7 = 0.433). [2011]a)9.08b)9.43c)11.72d)8.73Correct answer is option 'B'. Can you explain this answer? tests, examples and also practice Class 11 tests.
|
|
Explore Courses for Class 11 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