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Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
11th Edition
ISBN: 9781285869759
Author: Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher: Cengage Learning
Not helpful? See similar books
Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
Reaction Rates And Chemical Equilibrium. 7.63P

(a) Interpretation: The equilibrium concentrations of H+ and CH 3 COO- have to be determined given the initial concentration and final concentration of the weak acid, CH 3 COOH. Concept Introduction: CH 3 COOH is a weak acid which partially ionizes in solution. The products of ionization, CH 3 COO- and H+ exist in equilibrium with the weak acid. The change in concentration of the weak acid when the system reaches equilibrium will be equal to the concentration of the ionization products.

Question
Chapter 7, Problem 7.63P
Interpretation Introduction

(a)

Interpretation:

The equilibrium concentrations of H+ and CH3 COO- have to be determined given the initial concentration and final concentration of the weak acid, CH3 COOH.

Concept Introduction:

CH3COOH is a weak acid which partially ionizes in solution. The products of ionization, CH3 COO- and H+ exist in equilibrium with the weak acid. The change in concentration of the weak acid when the system reaches equilibrium will be equal to the concentration of the ionization products.

Expert Solution

Answer to Problem 7.63P

[H+]equilbrium=[CH3COO]equilibrium=0.0020M.

Explanation of Solution

The equilibrium reaction representing the ionization of weak acid, CH3COOH is,

CH3COOH(aq)H+(aq)+CH3COO(aq)

The initial concentration of the acid = 0.10 M.

Concentration of acid at equilibrium = 0.098 M.

Change in concentration of CH3COOH

=(0.100.098)M=0.0020M

This change in concentration of CH3 COOH will be equal to the concentration of [H+] and [CH3COO] formed during the ionization of CH3 COOH.

Therefore, [H+]equilbrium=[CH3COO]equilibrium=0.0020M.

Interpretation Introduction

(b)

Interpretation:

The expected equilibrium constant for the above reaction has to be calculated.

Concept Introduction:

Equilibrium constant is the ratio of the concentrations of products to the reactants concentrations, each term raised to the power equal to the stoichiometric coefficient.

CH3COOH(aq)H+(aq)+CH3COO(aq)K=[CH3COO][H+][CH3COOH].

Expert Solution

Answer to Problem 7.63P

The expected equilibrium constant for the reaction is 4.1×105.

Explanation of Solution

The given equilibrium ionization reaction is,

CH3COOH(aq)H+(aq)+CH3COO(aq)K=[CH3COO][H+][CH3COOH]

Plugging in the equilibrium concentrations to calculate the K value,

K=[CH3COO][H+][CH3COOH]=(0.0020)(0.0020)(0.098)=4.08×1054.1×105(Onroundingto twosignificantfigures).

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Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
11th Edition
ISBN: 9781285869759
Author: Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher: Cengage Learning
Not helpful? See similar books
Introduction to General, Organic and Biochemistry
Introduction to General, Organic and Biochemistry
Reaction Rates And Chemical Equilibrium. 7.63P
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