Information Stock acetic acid concentration: 1.0184 mol/L Stock sodium acetate concentration: 1.0166 mol/L pKa of acetic acid = 4.75 a) Calculate the pH of the stock acetic acid solution and the pH of the stock sodium acetate solution b) Calculate the pH of the undiluted buffer c) Calculate the pH of the 50% buffer *The file included explains how the buffers were prepared
Information Stock acetic acid concentration: 1.0184 mol/L Stock sodium acetate concentration: 1.0166 mol/L pKa of acetic acid = 4.75 a) Calculate the pH of the stock acetic acid solution and the pH of the stock sodium acetate solution b) Calculate the pH of the undiluted buffer c) Calculate the pH of the 50% buffer *The file included explains how the buffers were prepared
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
Information
Stock acetic acid concentration: 1.0184 mol/L
Stock sodium acetate concentration: 1.0166 mol/L
pKa of acetic acid = 4.75
a) Calculate the pH of the stock acetic acid solution and the pH of the stock sodium acetate solution
b) Calculate the pH of the undiluted buffer
c) Calculate the pH of the 50% buffer
*The file included explains how the buffers were prepared
![Part C: Preparation and Dilution of a Buffer
Use a graduated cylinder to measure volumes.
• Obtain 100 mL of 1 M acetic acid and 100 mL of 1 M sodium acetate solutions from the stock
bottles. Record the actual concentrations of these solutions as indicated on the stock bottles.
Measure the pH of these two solutions using the pH meter.
Prepare a buffer solution by mixing 100 mL 1 M acetic acid with 100 mL 1 M sodium acetate
solution. Stir.
Prepare a 50% buffer solution by adding 100 mL of this buffer to 100 mL deionized water;
stir.
Prepare a 25% buffer solution by adding 100 mL of 50% buffer to 100 mL deionized water;
stir.
• Measure the pH of the 3 buffer solutions. Save buffer solutions for next part.
Addition of strong base to buffered and unbuffered solutions:
• Clean the burette used in part A/B, rinse and then fill with 3 M NaOH
• With a graduated cylinder, measure 75 mL of the original buffer solution into a 200 mL
Berzelius beaker and place the magnetic stir bar in this solution. Set up your burette, stirrer
and pH probe as in part A/B. Using the burette, add ~1 mL of 3 M NaOH to the buffer, read
and record the pH. Continue adding base in 1 mL increments until 15 mL of NaOH has been
added. Record the pH after each 1 mL addition of NaOH.
Repeat the addition of NaOH in the same manner, using 75 mL of the 50% buffer. Record
the pH after every 1 mL addition until a total of 15 mL of NaOH has been added.
Repeat the addition of NaOH in the same manner, using 75 mL of the 25% buffer. Record
the pH after every 1 mL addition until a total of 15 mL of NaOH has been added.
• Repeat the addition of NaOH in the same manner, using 75 mL of deionized water.
Record the pH after every 1 mL addition until a total of 15 mL of NaOH has been added.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa01bd448-144d-4db2-affa-97c00487c9fd%2F55bea019-1fdc-4fde-9022-7a3f1ee9e4ad%2F00k2gcb_processed.png&w=3840&q=75)
Transcribed Image Text:Part C: Preparation and Dilution of a Buffer
Use a graduated cylinder to measure volumes.
• Obtain 100 mL of 1 M acetic acid and 100 mL of 1 M sodium acetate solutions from the stock
bottles. Record the actual concentrations of these solutions as indicated on the stock bottles.
Measure the pH of these two solutions using the pH meter.
Prepare a buffer solution by mixing 100 mL 1 M acetic acid with 100 mL 1 M sodium acetate
solution. Stir.
Prepare a 50% buffer solution by adding 100 mL of this buffer to 100 mL deionized water;
stir.
Prepare a 25% buffer solution by adding 100 mL of 50% buffer to 100 mL deionized water;
stir.
• Measure the pH of the 3 buffer solutions. Save buffer solutions for next part.
Addition of strong base to buffered and unbuffered solutions:
• Clean the burette used in part A/B, rinse and then fill with 3 M NaOH
• With a graduated cylinder, measure 75 mL of the original buffer solution into a 200 mL
Berzelius beaker and place the magnetic stir bar in this solution. Set up your burette, stirrer
and pH probe as in part A/B. Using the burette, add ~1 mL of 3 M NaOH to the buffer, read
and record the pH. Continue adding base in 1 mL increments until 15 mL of NaOH has been
added. Record the pH after each 1 mL addition of NaOH.
Repeat the addition of NaOH in the same manner, using 75 mL of the 50% buffer. Record
the pH after every 1 mL addition until a total of 15 mL of NaOH has been added.
Repeat the addition of NaOH in the same manner, using 75 mL of the 25% buffer. Record
the pH after every 1 mL addition until a total of 15 mL of NaOH has been added.
• Repeat the addition of NaOH in the same manner, using 75 mL of deionized water.
Record the pH after every 1 mL addition until a total of 15 mL of NaOH has been added.
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
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 2 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
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](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Elementary Principles of Chemical Processes, Bind…](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY