Homework Help is Here – Start Your Trial Now!
Science
Chemistry
2.1 The correct indicator was added to 25.00 mL of a 0.1345 M solution of propanoic acid (CH3CH2COOH) (Ka = 1.3 × 10-5 ) in a flask, and this was titrated with a 0.1895 M solution of sodium hydroxide from a burette. 2.1.1 Write the net ionic balanced equation for the reaction taking place (include all phases) Determine the final concentrations of the acid-base conjugate pair present after the titration, and show that the ratio of these species' concentrations is 1:1 at half the equivalence point. Hint: Firstly, determine the volume of base (in mL) that is required to reach the equivalence point for this titration. You may make use of a table to determine the amounts of species present. Using the Henderson-Hasselbalch equation, determine the pH of the solution in the flask at this point.

2.1 The correct indicator was added to 25.00 mL of a 0.1345 M solution of propanoic acid (CH3CH2COOH) (Ka = 1.3 × 10-5 ) in a flask, and this was titrated with a 0.1895 M solution of sodium hydroxide from a burette. 2.1.1 Write the net ionic balanced equation for the reaction taking place (include all phases) Determine the final concentrations of the acid-base conjugate pair present after the titration, and show that the ratio of these species' concentrations is 1:1 at half the equivalence point. Hint: Firstly, determine the volume of base (in mL) that is required to reach the equivalence point for this titration. You may make use of a table to determine the amounts of species present. Using the Henderson-Hasselbalch equation, determine the pH of the solution in the flask at this point.

Chemistry: The Molecular Science
Chemistry: The Molecular Science
5th Edition
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:John W. Moore, Conrad L. Stanitski
Chapter3: Chemical Reactions
Section3.11: Stoichiometry In Aqueous Solutions
Problem 3.28E: Sodium chloride is used in intravenous solutions for medical applications. The NaCl concentration in...
See similar textbooks
icon
Related questions
Question
100%

Please answer as soon as possible, thank you very much for your assistance

Question 2 – Propanoic acid 2.1 The correct indicator was added to 25.00 mL of a 0.1345 M solution of propanoic acid (CH3CH2COOH) (Ka = 1.3 × 10–5 ) in a flask, and this was titrated with a 0.1895 M solution of sodium hydroxide from a burette. 2.1.1 Write the net ionic balanced equation for the reaction taking place (include all phases) 2.1.2 Determine the final concentrations of the acid-base conjugate pair present after the titration, and show that the ratio of these species' concentrations is 1:1 at half the equivalence point. Hint: Firstly, determine the volume of base (in mL) that is required to reach the equivalence point for this titration. You may make use of a table to determine the amounts of species present. 2.1.3 Using the Henderson-Hasselbalch equation, determine the pH of the solution in the flask at this point.
Transcribed Image Text:Question 2 – Propanoic acid 2.1 The correct indicator was added to 25.00 mL of a 0.1345 M solution of propanoic acid (CH3CH2COOH) (Ka = 1.3 × 10–5 ) in a flask, and this was titrated with a 0.1895 M solution of sodium hydroxide from a burette. 2.1.1 Write the net ionic balanced equation for the reaction taking place (include all phases) 2.1.2 Determine the final concentrations of the acid-base conjugate pair present after the titration, and show that the ratio of these species' concentrations is 1:1 at half the equivalence point. Hint: Firstly, determine the volume of base (in mL) that is required to reach the equivalence point for this titration. You may make use of a table to determine the amounts of species present. 2.1.3 Using the Henderson-Hasselbalch equation, determine the pH of the solution in the flask at this point.
Expert Solution
steps

Step by step

Solved in 7 steps with 7 images

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Basics of Titrimetric Analysis
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: The Molecular Science
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
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: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781133611097
Author:
Steven S. Zumdahl
Publisher:
Cengage Learning
SEE MORE TEXTBOOKS