   Chapter 14, Problem 117E

Chapter
Section
Textbook Problem

# Determine [OH−], [H+], and the pH of each of the following solutions.a. 1.0 M KClb. 1.0 M KC2H3O2

(a)

Interpretation Introduction

Interpretation: The [OH] , [H+] and the pH value for each of the given solutions to be calculated.

Concept introduction: The pH of a solution is defined as a figure that expresses the acidity of the alkalinity of a given solution.

The pOH of a solution is calculated by the formula, pOH=log[OH]

The sum, pH+pOH=14

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

Ka=ConcentrationofproductsConcentrationofreactants

The value of Kw is calculated by the formula,

Kw=KaKb

To determine: The [OH] , [H+] and the pH value for the given solutions of 1.0M KCl .

Explanation

Explanation

The equilibrium constant expression for the given reaction is, Kb=[HCl][OH][Cl]

The dominant equilibrium reaction is,

Cl-(aq)HCl(aq)+OH-(aq)

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

Kb=ConcentrationofproductsConcentrationofreactants

Where,

• Kb is the base ionization constant.

The equilibrium constant expression for the given reaction is,

Kb=[HCl][OH][Cl] (1)

The Kb value is 7.692×10-9_ .

The value, Kw=KaKb

The value of Ka for HCl is 1.3×106 .

The value of Kb is calculated by the formula,

Kb=KwKa

Substitute the value of Ka in the above expression.

Kb=1.0×10141.3×106=7.692×10-9_

The [OH] is 8.77×10-5M_ .

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

The liquid components do not affect the value of the rate constant.

The ICE table for the stated reaction is,

Cl(aq)HCl(aq)+OH(aq)Inititialconcentration1.000Changex+x+xEquilibriumconcentration1.0xxx

The equilibrium concentration of [Cl] is (1.0x)M .

The equilibrium concentration of [HCl] is xM .

The equilibrium concentration of [OH] is xM .

The calculated value of Kb is 7.692×109 .

Substitute the value of Kb , [Cl] , [HCl] and [OH] in equation (1)

(b)

Interpretation Introduction

Interpretation: The [OH] , [H+] and the pH value for each of the given solutions to be calculated.

Concept introduction: The pH of a solution is defined as a figure that expresses the acidity of the alkalinity of a given solution.

The pOH of a solution is calculated by the formula, pOH=log[OH]

The sum, pH+pOH=14

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

Ka=ConcentrationofproductsConcentrationofreactants

The value of Kw is calculated by the formula,

Kw=KaKb

To determine: The [OH] , [H+] and the pH value for the given solutions of 1.0M KC2H3O2 .

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