The correct indicator was added to 25.00 ml of a 0.1345 M solution of propanoic acid (CH,CH;COOH) (K. = 1.3 × 10) in a flask, and this was titrated with a 0.1895 M solution of sodium hydroxide from a burette. 2.1 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. 2.1.2 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.

The correct indicator was added to 25.00 ml of a 0.1345 M solution of propanoic acid (CH,CH;COOH) (K. = 1.3 × 10) in a flask, and this was titrated with a 0.1895 M solution of sodium hydroxide from a burette. 2.1 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. 2.1.2 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

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

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