Homework Help is Here – Start Your Trial Now!
Science
Chemistry
3. Buffers a) In choosing a buffer, it is necessary to select a weak acid that has a pKa near the target pH. Calculate the pka of each reaction below. Which one should be used to make a buffer at pH = 10.0.

3. Buffers a) In choosing a buffer, it is necessary to select a weak acid that has a pKa near the target pH. Calculate the pka of each reaction below. Which one should be used to make a buffer at pH = 10.0.

Chemistry
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...
See similar textbooks
icon
Related questions
Question
3
3. Buffers a) In choosing a buffer, it is necessary to select a weak acid that has a pka near the target pH. Calculate the pK, of each reaction below. Which one should be used to make a buffer at pH= 10.0. H₂CO3HCO3 + H+ HCO3 CO3² + H+ H3PO4→ H₂PO4 + H+ H₂PO4 →HPO4² + H+ HPO4²PO4³ + H+ Ka = 4.2 x 10-7 Ka 4.8 x 10-11 Ka = 7.5 x 10-³3 Ka = 6.2 x 10-8 Ka = 4.8 x 10-13 (available salts: NaHCO3) (available salts: NaHCO3/Na2CO3) (available salts: NaH₂PO4) (available salts: Na₂HPO4) (available salts: Na2HPO4, Na3PO4) b) Using the Henderson-Hasselbalch equation, calculate the concentration of the conjugate base using 0.10 M weak acid. pH = pKa + log ( [conjugate base] [weak acid] c) Using the buffer system that you selected in a) calculate the mass (in grams) of the conjugate base and weak acid needed to make 100 mL of the buffer. 4
Transcribed Image Text:3. Buffers a) In choosing a buffer, it is necessary to select a weak acid that has a pka near the target pH. Calculate the pK, of each reaction below. Which one should be used to make a buffer at pH= 10.0. H₂CO3HCO3 + H+ HCO3 CO3² + H+ H3PO4→ H₂PO4 + H+ H₂PO4 →HPO4² + H+ HPO4²PO4³ + H+ Ka = 4.2 x 10-7 Ka 4.8 x 10-11 Ka = 7.5 x 10-³3 Ka = 6.2 x 10-8 Ka = 4.8 x 10-13 (available salts: NaHCO3) (available salts: NaHCO3/Na2CO3) (available salts: NaH₂PO4) (available salts: Na₂HPO4) (available salts: Na2HPO4, Na3PO4) b) Using the Henderson-Hasselbalch equation, calculate the concentration of the conjugate base using 0.10 M weak acid. pH = pKa + log ( [conjugate base] [weak acid] c) Using the buffer system that you selected in a) calculate the mass (in grams) of the conjugate base and weak acid needed to make 100 mL of the buffer. 4
Expert Solution
steps

Step by step

Solved in 5 steps with 18 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Electroanalytical Techniques
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.
Similar questions
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
SEE MORE TEXTBOOKS