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2.1 The correct indicator was added to 25.00 mL of a 0.1345 M solution of propanoic acid (CH3CH2COOH) (Ka = 1.3 x 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.

2.1 The correct indicator was added to 25.00 mL of a 0.1345 M solution of propanoic acid (CH3CH2COOH) (Ka = 1.3 x 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.

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...
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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 x 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 x 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.
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