Homework Help is Here – Start Your Trial Now!
Science
Chemistry
1. Using a graduated cylinder to measure volumes, prepare a buffer solution from 20.0 mL of 0.10 M acetic acid and 30.0 mL of 0.10 sodium acetate. a Calculate the pH of the buffer. (Ka = 1.8 x 105) (b. Measure the actual pH of the solution using your pH meter. c. Compare the experimental result in (b) to the calculated value in (a). Determine the % error.

1. Using a graduated cylinder to measure volumes, prepare a buffer solution from 20.0 mL of 0.10 M acetic acid and 30.0 mL of 0.10 sodium acetate. a Calculate the pH of the buffer. (Ka = 1.8 x 105) (b. Measure the actual pH of the solution using your pH meter. c. Compare the experimental result in (b) to the calculated value in (a). Determine the % error.

Principles of Modern Chemistry
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter15: Acid–base Equilibria
Section: Chapter Questions
Problem 99AP
See similar textbooks
icon
Related questions
Question
I need help with 1a, 1c, 2c
Table I: Acetic acid/sodium acetate Buffer Buffer pH pH theoretical experimental pH pH pH theoretical pH Error theoretical after experimental Error after adding base experimental Error Initially Initially adding after adding after adding acid acid base HC2H3O2/ C2H3O2 H2O 4.95 4.516 5.14 8.62 Hand write ALL of your calculations under the table. 2. 30 1.960
Transcribed Image Text:Table I: Acetic acid/sodium acetate Buffer Buffer pH pH theoretical experimental pH pH pH theoretical pH Error theoretical after experimental Error after adding base experimental Error Initially Initially adding after adding after adding acid acid base HC2H3O2/ C2H3O2 H2O 4.95 4.516 5.14 8.62 Hand write ALL of your calculations under the table. 2. 30 1.960
Note: For each experiment requiring a calculation show the method and logic used in the calculation. Be sure to completely show all steps and units in each step. Use a pH meter to measure pHs. Prepare appropriate tables for each experiment to record your lab data. Remember to carefully record all procedures and observations. 1. Using a graduated cylinder to measure volumes, prepare a buffer solution from 20.0 mL of 0.10 M acetic acid and 30.0 mL of 0.10 sodium acetate. a Calculate the pH of the buffer. (Ka = 1.8 x 10-5) (b. Measure the actual pH of the solution using your pH meter. c. Compare the experimental result in (b) to the calculated value in (a). Determine the % error. 2. Divide your buffer solution in (1) into two equal 25.0 mL volumes. Calculate the expected pH of the following solutions and then measure the pH of each. a. To one of the 25.0 ml solutions add 5.0 mL of 0.10 M HCl and measure the pH. (b To the second add 5.0 mL of 0.10 M NAOH and record the pH. c. Compare the experimental results with the theoretical results. Why are there differences in their pHs? 3. Carry out the following measurements and also calculate the expected pH of the following solutions: Measure the pH of deionized water. (b. Add 5.0 mL of 0.10 M HCl to 25.0 mL of water and measure pH Add 5.0 mL of 0.10 M NAOH to a new sample of 25.0 mL of water and measure pH. Based on this data, is water a buffer?
Transcribed Image Text:Note: For each experiment requiring a calculation show the method and logic used in the calculation. Be sure to completely show all steps and units in each step. Use a pH meter to measure pHs. Prepare appropriate tables for each experiment to record your lab data. Remember to carefully record all procedures and observations. 1. Using a graduated cylinder to measure volumes, prepare a buffer solution from 20.0 mL of 0.10 M acetic acid and 30.0 mL of 0.10 sodium acetate. a Calculate the pH of the buffer. (Ka = 1.8 x 10-5) (b. Measure the actual pH of the solution using your pH meter. c. Compare the experimental result in (b) to the calculated value in (a). Determine the % error. 2. Divide your buffer solution in (1) into two equal 25.0 mL volumes. Calculate the expected pH of the following solutions and then measure the pH of each. a. To one of the 25.0 ml solutions add 5.0 mL of 0.10 M HCl and measure the pH. (b To the second add 5.0 mL of 0.10 M NAOH and record the pH. c. Compare the experimental results with the theoretical results. Why are there differences in their pHs? 3. Carry out the following measurements and also calculate the expected pH of the following solutions: Measure the pH of deionized water. (b. Add 5.0 mL of 0.10 M HCl to 25.0 mL of water and measure pH Add 5.0 mL of 0.10 M NAOH to a new sample of 25.0 mL of water and measure pH. Based on this data, is water a buffer?
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 3 steps with 1 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Precipitation Titrations
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
Principles of Modern Chemistry
Principles of Modern Chemistry
Chemistry
ISBN:
9781305079113
Author:
David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781133611097
Author:
Steven S. Zumdahl
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemical Principles in the Laboratory
Chemical Principles in the Laboratory
Chemistry
ISBN:
9781305264434
Author:
Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher:
Brooks Cole
SEE MORE TEXTBOOKS