2. Buffer capacity has a rather loose definition, yet it is an important property of buffers. A commonly seen definition of buffer capacity is: "The amount of H* or OH that can be neutralized before the pH changes to a significant degree." Use your data to determine the buffer capacity of Buffer A and Buffer B. 3. Say, for example, that you had prepared a Buffer C, in which you mixed 8.203 g of sodium acetate, NaC₂H3O2, with 100.0 mL of 1.0 M acetic acid. a. What would be the initial pH of Buffer C? b. If you add 5.0 mL of 0.5 M NaOH solution to 20.0 ml. affer B

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...
icon
Related questions
icon
Concept explainers
Question
Hello can you help me answer question 2,3.a, and 3.b please? Thank you!
**DATA ANALYSIS**

1. Write reaction equations to explain how your acetic acid-acetate buffer reacts with a base.

2. Buffer capacity has a rather loose definition, yet it is an important property of buffers. A buffer capacity is the amount of \[H^+\] or \[OH^-\] that can be neutralized before the pH changes significantly. Use your data to determine the buffer capacity of Buffer A and Buffer B.

3. Say, for example, that you had prepared a Buffer C, in which you mixed 8.203 g of sodium acetate, NaC2H3O2, with 100.0 mL of 1.00 M acetic acid.

   a. What would be the initial pH of Buffer C?

   b. If you add mL of 0.5 M NaOH solution to 20.0 mL each of Buffer B and Buffer C, which buffer's pH would change less? Explain.

**DATA TABLE**

| Mass of NaC2H3O2 used to prepare buffer (g) | Volume of buffer prepared (mL) | Molar concentration of HCl/Na2O2 buffer (M) | Initial pH of buffer | Volume of 0.5 M HCl to lower pH by 2 units (mL) | Volume of 0.5 M NaOH to raise pH by 2 units (mL) | Volume of 0.5 M NaOH at equivalence point (mL) |
|---------------------------------------------|--------------------------------|---------------------------------------------|----------------------|-------------------------------------------------|--------------------------------------------------|-----------------------------------------------|
| Buffer A                                    | 0.15139                        | 100.0                                      | 1.5 mL               | 4.79                                            | 1.0 mL                                            | 1.5 mL                                        |
| Buffer B                                    | 1.50018                        | 100.0                                      | 10                   | 4.73                                            | 1.9 mL                                           | 2 mL                                           | 4.5 mL                                        | 90 mL                                         |

The above table provides detailed data regarding the preparation and characterization of two different buffers, Buffer A and Buffer B, including their initial pH levels and their reactions with acid and base solutions.
Transcribed Image Text:**DATA ANALYSIS** 1. Write reaction equations to explain how your acetic acid-acetate buffer reacts with a base. 2. Buffer capacity has a rather loose definition, yet it is an important property of buffers. A buffer capacity is the amount of \[H^+\] or \[OH^-\] that can be neutralized before the pH changes significantly. Use your data to determine the buffer capacity of Buffer A and Buffer B. 3. Say, for example, that you had prepared a Buffer C, in which you mixed 8.203 g of sodium acetate, NaC2H3O2, with 100.0 mL of 1.00 M acetic acid. a. What would be the initial pH of Buffer C? b. If you add mL of 0.5 M NaOH solution to 20.0 mL each of Buffer B and Buffer C, which buffer's pH would change less? Explain. **DATA TABLE** | Mass of NaC2H3O2 used to prepare buffer (g) | Volume of buffer prepared (mL) | Molar concentration of HCl/Na2O2 buffer (M) | Initial pH of buffer | Volume of 0.5 M HCl to lower pH by 2 units (mL) | Volume of 0.5 M NaOH to raise pH by 2 units (mL) | Volume of 0.5 M NaOH at equivalence point (mL) | |---------------------------------------------|--------------------------------|---------------------------------------------|----------------------|-------------------------------------------------|--------------------------------------------------|-----------------------------------------------| | Buffer A | 0.15139 | 100.0 | 1.5 mL | 4.79 | 1.0 mL | 1.5 mL | | Buffer B | 1.50018 | 100.0 | 10 | 4.73 | 1.9 mL | 2 mL | 4.5 mL | 90 mL | The above table provides detailed data regarding the preparation and characterization of two different buffers, Buffer A and Buffer B, including their initial pH levels and their reactions with acid and base solutions.
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 6 steps with 1 images

Blurred answer
Knowledge Booster
Ionic Equilibrium
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
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY