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




10th Edition
Steven S. Zumdahl + 2 others
ISBN: 9781305957404
Textbook Problem

Calculate the pH of a buffered solution prepared by dissolving 21.5 g benzoic acid (HC7H5O2) and 37.7 g sodium benzoate in 200.0 mL of solution.

Interpretation Introduction


The mass of benzoic acid, sodium benzoate and volume of their solution is given. The pH value of this solution is to be calculated.

Concept introduction:

The pH value is the measure of H+ ions. The relation between pH and pKa is given by Henderson-Hassel Bach equation. According to this equation,




To determine the number of moles of benzoic acid and sodium benzoate

Mass of benzoic acid is 21.5g .

Mass of sodium benzoate is 37.7g .

The molar mass of benzoic acid is 122.12g/mol .

The molar mass of sodium benzoate is 144.10g/mol .


The number of moles is calculated using the formula,

Numberofmoles=MassofcomoundMolarmassofcompound (1)

Substitute the values of mass and molar mass of benzoic acid in the above equation.


Substitute the values of mass and molar mass of sodium benzoate in equation (1).


To determine the concentration of benzoic acid and of sodium benzoate

Moles of benzoic acid is 0.176mol .

Moles of sodium benzoate is 0.261mol .

Volume of solution is 200mL .

The conversion of milliliter (mL) into liter (L) is done as,



The conversion of 200mL into liter is,


The concentration of compound in a solution is calculated using the formula,

Concentrationofcompound=MolesofcompoundVolumeofsolution (2)

Substitute the values of moles of benzoic acid and volume of solution in the above equation.


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