A 40.00 solution of 0.1430 M chloroacetic acid (pK a = 2.865) is titrated with a 0.1500 M solution of NaOH. a. Find the initial pH of the solution. b. Find the pH of the resulting solution at the half-equivalence point. c. Find the pH of the resulting solution at the equivalence point. d. Find the pH of the resulting solution at 0.50 mL past the equivalence point.

A 40.00 solution of 0.1430 M chloroacetic acid (pK a = 2.865) is titrated with a 0.1500 M solution of NaOH. a. Find the initial pH of the solution. b. Find the pH of the resulting solution at the half-equivalence point. c. Find the pH of the resulting solution at the equivalence point. d. Find the pH of the resulting solution at 0.50 mL past the equivalence point.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter15: Acid-base Equilibria

Section: Chapter Questions

Problem 59E: Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 105) by 0.100 M KOH. Calculate...

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