   # Consider a weak acid, HX. If a 0.10 -M solution of HX has a pH of 5.83 at 25°C. what is ∆ G ° for the acid’s dissociation reaction at 25°C? ### Chemistry

10th Edition
Steven S. Zumdahl + 2 others
Publisher: Cengage Learning
ISBN: 9781305957404

#### Solutions

Chapter
Section ### Chemistry

10th Edition
Steven S. Zumdahl + 2 others
Publisher: Cengage Learning
ISBN: 9781305957404
Chapter 17, Problem 125CP
Textbook Problem
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## Consider a weak acid, HX. If a 0.10-M solution of HX has a pH of 5.83 at 25°C. what is ∆G° for the acid’s dissociation reaction at 25°C?

Interpretation Introduction

Interpretation: The concentration and pH value of weak acid HX at 25°C is given. The value of ΔG° for the acid dissociation reaction is to be calculated.

Concept introduction: At equilibrium, the acid dissociation constant expression is expressed by the formula,

Ka=ConcentrationofproductsConcentrationofreactants

### Explanation of Solution

Explanation

Given

The pH value is 5.83 .

The pH is calculated by the formula,

pH=log[H+]

Rearrange the above expression to calculate the value of [H+] .

[H+]=10pH

Substitute the given value of pH in the above expression.

[H+]=105.83=1.48×106M_

Given

The pH value is 5.83 .

Concentration of HX is 0.10M .

The dissociation reaction of HX is,

HX(aq)H+(aq)+X(aq)

The concentration of H+ ion is assumed to be x .

The ICE table is formed for the given reaction.

HX(aq)H+(aq)+X(aq)Initial (M)         0.1000Change(M)        x+x+xEquilibrium(M)0.10xxx

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

The equilibrium concentration of [H+] is xM .

The equilibrium concentration of [X] is (x)M .

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

Ka=ConcentrationofproductsConcentrationofreactants

Where,

• Ka is the acid dissociation constant.

The given value of the equilibrium constant is 1.0×1023 .

The equilibrium constant expression for the given reaction is,

Ka=[X][H+][HX]=(x)(x)(0

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