Homework Help is Here – Start Your Trial Now!
Science
Chemistry
In an experiment the equilibrium between ethanol, acetic acid, ethyl acetate, and water is studied, and the reaction is catalyzed by the addition of hydrochloric acid.   Following mixtures were prepared and titrated with 0.953M NaOH solution to calculate equilibrium constant of the reaction.   Mixture 1. 2.5ml 3M HCl+ 2.5ml Water   Mixture 2. 2.5mL 3M HCl + 2ml Ethyl Acetate + 0.5ml Acetic Acid   End points were reached at 6.68 ml and 24.36 ml, respectively. Calculate the equilibrium constant using mole fractions for the reaction (MWHCl: 36.46g/mol, MWCH3COOH: 60.05g/mol, MWH2O: 18.02g/mol, MWCH3COOC2H5: 88.11g/mol, ρwater = ρHCl =0.998g/ml, ρCH3COOH = 1.05g/ml, ρCH3COC2H5 =0.902g/ml)

In an experiment the equilibrium between ethanol, acetic acid, ethyl acetate, and water is studied, and the reaction is catalyzed by the addition of hydrochloric acid.   Following mixtures were prepared and titrated with 0.953M NaOH solution to calculate equilibrium constant of the reaction.   Mixture 1. 2.5ml 3M HCl+ 2.5ml Water   Mixture 2. 2.5mL 3M HCl + 2ml Ethyl Acetate + 0.5ml Acetic Acid   End points were reached at 6.68 ml and 24.36 ml, respectively. Calculate the equilibrium constant using mole fractions for the reaction (MWHCl: 36.46g/mol, MWCH3COOH: 60.05g/mol, MWH2O: 18.02g/mol, MWCH3COOC2H5: 88.11g/mol, ρwater = ρHCl =0.998g/ml, ρCH3COOH = 1.05g/ml, ρCH3COC2H5 =0.902g/ml)

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...
See similar textbooks
icon
Related questions
Question

In an experiment the equilibrium between ethanol, acetic acid, ethyl acetate, and water is studied, and the reaction is catalyzed by the addition of hydrochloric acid.

 

Following mixtures were prepared and titrated with 0.953M NaOH solution to calculate equilibrium constant of the reaction.

 

Mixture 1. 2.5ml 3M HCl+ 2.5ml Water

 

Mixture 2. 2.5mL 3M HCl + 2ml Ethyl Acetate + 0.5ml Acetic Acid

 

End points were reached at 6.68 ml and 24.36 ml, respectively. Calculate the equilibrium constant using mole fractions for the reaction (MWHCl: 36.46g/mol, MWCH3COOH: 60.05g/mol, MWH2O: 18.02g/mol, MWCH3COOC2H5: 88.11g/mol, ρwater = ρHCl =0.998g/ml, ρCH3COOH = 1.05g/ml, ρCH3COC2H5 =0.902g/ml)

Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 7 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Applications of Molecular Spectroscopy
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
  • SEE MORE QUESTIONS
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS