Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
Related questions
Question
![**Problem Statement:**
What is the pH of a 0.660 M solution of C₅H₅NHBr? (Kₙ of C₅H₅N is 1.7 × 10⁻⁹)
**Explanation:**
To find the pH of the solution, we first need to consider the nature of C₅H₅NHBr.
- **C₅H₅NHBr** is the salt formed from the weak base **C₅H₅N (pyridine)** and a strong acid **HBr**.
- In solution, C₅H₅NHBr dissociates into C₅H₅NH⁺ and Br⁻. The bromide ion (Br⁻) does not affect pH as it is the conjugate base of a strong acid. Therefore, the focus is on the acidic nature due to C₅H₅NH⁺.
**Steps for Calculation:**
1. **Calculate the Ka of C₅H₅NH⁺:**
\[
K_w = 1.0 \times 10^{-14}
\]
\[
K_a \times K_b = K_w \Rightarrow K_a = \frac{K_w}{K_b} = \frac{1.0 \times 10^{-14}}{1.7 \times 10^{-9}}
\]
2. **Determine the pH using Ka:**
Set up the equilibrium expression for dissociation of C₅H₅NH⁺ and use the concentration to find the pH of the solution.
These calculations involve substituting values in the formulas above, approximating where necessary (for concentrations much greater than x), and finally computing the pH using \(-\log[H⁺]\).
This process allows students to understand applications of equilibrium constants in real-world scenarios involving solution chemistry.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcf594692-d96b-4ff4-ac1a-31ce1d3fad0a%2Fa8be614f-4f8e-42e4-afcf-79e613a4423f%2Fn4vezrf_processed.png&w=3840&q=75)
Transcribed Image Text:**Problem Statement:**
What is the pH of a 0.660 M solution of C₅H₅NHBr? (Kₙ of C₅H₅N is 1.7 × 10⁻⁹)
**Explanation:**
To find the pH of the solution, we first need to consider the nature of C₅H₅NHBr.
- **C₅H₅NHBr** is the salt formed from the weak base **C₅H₅N (pyridine)** and a strong acid **HBr**.
- In solution, C₅H₅NHBr dissociates into C₅H₅NH⁺ and Br⁻. The bromide ion (Br⁻) does not affect pH as it is the conjugate base of a strong acid. Therefore, the focus is on the acidic nature due to C₅H₅NH⁺.
**Steps for Calculation:**
1. **Calculate the Ka of C₅H₅NH⁺:**
\[
K_w = 1.0 \times 10^{-14}
\]
\[
K_a \times K_b = K_w \Rightarrow K_a = \frac{K_w}{K_b} = \frac{1.0 \times 10^{-14}}{1.7 \times 10^{-9}}
\]
2. **Determine the pH using Ka:**
Set up the equilibrium expression for dissociation of C₅H₅NH⁺ and use the concentration to find the pH of the solution.
These calculations involve substituting values in the formulas above, approximating where necessary (for concentrations much greater than x), and finally computing the pH using \(-\log[H⁺]\).
This process allows students to understand applications of equilibrium constants in real-world scenarios involving solution chemistry.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 steps with 1 images
Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY