1. What is the pH of a buffer prepared by mixing 20.0 g of acetic acid (HC₂H302) and 20.0 g of sodium acetate (NaC₂H302) in enough water to form 2.00L of solution. The Ka of acetic acid is 1.82 x 10-5.
1. What is the pH of a buffer prepared by mixing 20.0 g of acetic acid (HC₂H302) and 20.0 g of sodium acetate (NaC₂H302) in enough water to form 2.00L of solution. The Ka of acetic acid is 1.82 x 10-5.
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
![**Buffer pH Calculation**
**Question:**
1. What is the pH of a buffer prepared by mixing 20.0 g of acetic acid (HC₂H₃O₂) and 20.0 g of sodium acetate (NaC₂H₃O₂) in enough water to form 2.00 L of solution? The Kₐ of acetic acid is 1.82 × 10⁻⁵.
**Description:**
This problem involves calculating the pH of a buffer solution. A buffer solution consists of a weak acid, acetic acid (HC₂H₃O₂), and its conjugate base, sodium acetate (NaC₂H₃O₂). To solve this, you need to use the Henderson-Hasselbalch equation, which relates the pH of a buffer to the concentration of acid and its conjugate base:
\[ \text{pH} = \text{pK}_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]
Where:
- \([\text{A}^-]\) is the concentration of the conjugate base (sodium acetate).
- \([\text{HA}]\) is the concentration of the weak acid (acetic acid).
- \(\text{pK}_a = -\log(\text{K}_a)\).
To find the concentrations:
1. Convert grams of acetic acid and sodium acetate to moles.
2. Divide the moles by the volume of the solution in liters (2.00 L) to find molarity.
Calculate pH using the Henderson-Hasselbalch equation after determining the concentrations and \(\text{pK}_a\).](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5b8356a3-8ffd-4b0d-99e3-2fe5523dae0d%2F381ba5d2-207e-4552-b9dd-9415c16604f9%2Fzhuvojd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Buffer pH Calculation**
**Question:**
1. What is the pH of a buffer prepared by mixing 20.0 g of acetic acid (HC₂H₃O₂) and 20.0 g of sodium acetate (NaC₂H₃O₂) in enough water to form 2.00 L of solution? The Kₐ of acetic acid is 1.82 × 10⁻⁵.
**Description:**
This problem involves calculating the pH of a buffer solution. A buffer solution consists of a weak acid, acetic acid (HC₂H₃O₂), and its conjugate base, sodium acetate (NaC₂H₃O₂). To solve this, you need to use the Henderson-Hasselbalch equation, which relates the pH of a buffer to the concentration of acid and its conjugate base:
\[ \text{pH} = \text{pK}_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]
Where:
- \([\text{A}^-]\) is the concentration of the conjugate base (sodium acetate).
- \([\text{HA}]\) is the concentration of the weak acid (acetic acid).
- \(\text{pK}_a = -\log(\text{K}_a)\).
To find the concentrations:
1. Convert grams of acetic acid and sodium acetate to moles.
2. Divide the moles by the volume of the solution in liters (2.00 L) to find molarity.
Calculate pH using the Henderson-Hasselbalch equation after determining the concentrations and \(\text{pK}_a\).
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 3 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.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