Monochloroacetic acid, HC 2 H 2 ClO 2 , is a skin irritant that is used in “chemical peels” intended to remove the top layer of dead skin from the face and ultimately improve the complexion. The value of K a for monochloroacetic acid is 1.35 × 10 −3 . Calculate the pH of a 0.10 -M solution of monochloroacetic acid.

Q: Expert Answer

Interpretation Introduction Interpretation: The pH of the given 0.10 M solution of monochloroacetic acid, with the given value of K a , is to be calculated. Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution. A logarithmic scale is used on which, the value 7 corresponds to a neutral species, a value less than 7 corresponds to an acid and a value greater than 7 corresponds to a base. The pH of a solution is calculated by the formula, pH = − log [ H + ] At equilibrium, the equilibrium constant expression is expressed by the formula, K a = Concentration of products Concentration of reactants Explanation Explanation To determine: The pH of the given 0.10 M solution of monochloroacetic acid. The equilibrium constant expression for the stated dissociation reaction is, K a = [ H + ] [ C 2 H 2 ClO 2 − ] [ HC 2 H 2 ClO 2 ] The dominant equilibrium reaction for the given case is, HC 2 H 2 ClO 2 ( a q ) ⇌ H + ( a q ) + C 2 H 2 ClO 2 − ( a q ) At equilibrium, the equilibrium constant expression is expressed by the formula, K a = Concentration of products Concentration of reactants Where, K a is the acid dissociation constant. The equilibrium constant expression for the given reaction is, K a = [ H + ] [ C 2 H 2 ClO 2 − ] [ HC 2 H 2 ClO 2 ] (1) The [ H + ] is 1 . 2 × 1 0 - 2 M _ . The change in concentration of HC 2 H 2 ClO 2 is assumed to be x . The ICE table for the stated reaction is, HC 2 H 2 ClO 2 ( a q ) ⇌ H + ( a q ) + C 2 H 2 ClO 2 − ( a q ) Inititial concentration 0.10 0 0 Change − x + x + x Equilibrium concentration 0.10 − x x x The equilibrium concentration of [ HC 2 H 2 ClO 2 ] is ( 0.10 − x ) M . The equilibrium concentration of [ H + ] is x M

Question

Still sussing out bartleby?

Answer 1

BuyFind

Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

Solutions

Chapter

Section

Answer 2

BuyFind

Chemistry: An Atoms First Approach

2nd Edition

Steven S. Zumdahl + 1 other

Publisher: Cengage Learning

ISBN: 9781305079243

Solutions

Chapter

Section

Answer 3

Solutions

Chapter

Section

Answer 4

Chapter

Section

Answer 5

Interpretation Introduction

Interpretation: The pH of the given 0.10 M solution of monochloroacetic acid, with the given value of Ka , is to be calculated.

Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution. A logarithmic scale is used on which, the value 7 corresponds to a neutral species, a value less than 7 corresponds to an acid and a value greater than 7 corresponds to a base.

The pH of a solution is calculated by the formula, pH=−log[H+]

At equilibrium, the equilibrium constant expression is expressed by the formula,

Ka=Concentration of productsConcentration of reactants

Explanation of Solution

Explanation

To determine: The pH of the given 0.10 M solution of monochloroacetic acid.

The equilibrium constant expression for the stated dissociation reaction is,

Ka=[H+][C2H2ClO2−][HC2H2ClO2]

The dominant equilibrium reaction for the given case is,

HC2H2ClO2(aq)⇌H+(aq)+C2H2ClO2−(aq)

At equilibrium, the equilibrium constant expression is expressed by the formula,

Ka=Concentration of productsConcentration of reactants

Where,

Ka is the acid dissociation constant.

The equilibrium constant expression for the given reaction is,

Ka=[H+][C2H2ClO2−][HC2H2ClO2] (1)

The [H+] is 1.2×10-2 M_ .

The change in concentration of HC2H2ClO2 is assumed to be x .

The ICE table for the stated reaction is,

HC2H2ClO2(aq)⇌H+(aq)+C2H2ClO2−(aq)Inititial concentration0.1000Change−x+x+xEquilibrium concentration0.10−xxx

The equilibrium concentration of [HC2H2ClO2] is (0.10−x) M .

The equilibrium concentration of [H+] is x M

Chemistry: An Atoms First Approach

Solutions

Chemistry: An Atoms First Approach

Explanation of Solution

Still sussing out bartleby?

The Solution to Your Study Problems

Chapter 13 Solutions

Additional Science Textbook Solutions