9th Edition
Steven S. Zumdahl
ISBN: 9781133611097




9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
Textbook Problem

A buffer solution is prepared by mixing 75.0 mL of 0.275 M fluorobenzoic acid (C7H5O2F) with 55.0 mL of 0.472 M sodium fluorobenzoate. The pKa of this weak acid is 2.90. What is the pH of the buffer solution?

Interpretation Introduction

Interpretation: The formation of a buffer solution by the mixing of Fluorobenzoic acid and Sodium fluorobenzoate is given. The value of pH of buffer solution is to be calculated.

Concept introduction: The solution of weak acid and their conjugate base which upon addition of an acid or base resists the change in pH is called buffer solution. The pH of the buffer solution remains constant.

To determine: value of pH of given buffer solution is to be calculated.




The concentration of Fluorobenzoic acid is 0.275M .

The concentration of Sodium fluorobenzoate is 0.472M .

The volume of Fluorobenzoic acid is 75.0mL .

The volume of Sodium fluorobenzoate is 55.0mL .

The pKa is 2.90 .

The conversion of mL into L is done as,


The conversion of all the given species into L is done as,


The concentration of any species is given as,

Concentration=NumberofmolesVolumeofsolutioninlitres (1)

Rearrange the above equation to obtain the value of number of moles.

Numberofmoles=Concentration×Volumeofsolutioninlitres (2)

Substitute the value of concentration and volume of Fluorobenzoic acid in the equation (2).


Similarly, substitute the value of concentration and volume of Sodium fluorobenzoate in the equation (2).


The total volume =VolumeofFluorobenzoicacid+VolumeofSodiumfluorobenzoate=0

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