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Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097

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BuyFindarrow_forward

Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
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

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