Using the procedure in Determination of an Equilibrium Constant, a student combines equimolar amounts of acetic acid and ethanol to react as shown by the following equation. acetic acid + ethanol = ethyl acetate + water To determine the initial concentration of acetic acid, 1.00 mL of the resulting mixture was titrated with 0.1905 M NaOH, requiring 32.50 mL . What is the molarity of the acetic acid? Type answer:

Using the procedure in Determination of an Equilibrium Constant, a student combines equimolar amounts of acetic acid and ethanol to react as shown by the following equation. acetic acid + ethanol = ethyl acetate + water To determine the initial concentration of acetic acid, 1.00 mL of the resulting mixture was titrated with 0.1905 M NaOH, requiring 32.50 mL . What is the molarity of the acetic acid? Type answer:

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter16: Solubility And Precipitation Equilibria

Section: Chapter Questions

Problem 70AP

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