   Chapter 15, Problem 93AE

Chapter
Section
Textbook Problem

# A certain acetic acid solution has pH = 2.68. Calculate the volume of 0.0975 M KOH required to reach the equivalence point in the titration of 25.0 mL of the acetic acid solution.

Interpretation Introduction

Interpretation:

The pH value of certain acetic acid solution is given. The volume of 0.0975M KOH required to reach the equivalence point in the given titration is to be calculated.

Concept introduction:

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=ConcentrationofproductsConcentrationofreactants

To determine: The buffered solutions form the given solutions.

Explanation

Explanation

To find the [H+]

Given

The value of pH is 2.68 .

Volume of acetic acid is 25.0mL .

The pH of a solution is calculated by the formula,

pH=log[H+]

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

[H+]=10pH

Substitute the value of pH in the above expression.

[H+]=102.68=0.0021M_

To find the concentration of acetic acid

The ICE table is formed for the given reaction.

CH3COOH(aq)H+(aq)+CH3COO(aq)Initialconcentrationx00Changey+y+yEquilibriumconcentrationxyyy

The equilibrium concentration of [CH3COOH] is (xy)M .

The equilibrium concentration of [CH3COO] is yM .

The equilibrium concentration of [H+] is yM .

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

Ka=ConcentrationofproductsConcentrationofreactants

Where,

• Ka is the acid dissociation constant

### Still sussing out bartleby?

Check out a sample textbook solution.

See a sample solution

#### The Solution to Your Study Problems

Bartleby provides explanations to thousands of textbook problems written by our experts, many with advanced degrees!

Get Started

#### Find more solutions based on key concepts 