Lehninger Principles of Biochemistry 6th Edition

Published by W.H. Freeman
ISBN 10: 1-42923-414-8
ISBN 13: 978-1-42923-414-6

Chapter 2 - Water - Problems: 10

Answer

3.3mL of acetic acid for 1 liter of vinegar.

Work Step by Step

pH of vinegar must be 3. What is the volume of acetic acid required to make a pH 3? Henderson-Hasselbalch equation, $pH =pK_{a} +log([A]/[HA])$ pK_{a} of acetic acid = 4.76 3 = 4.76 +log([A]/[HA]) log([A]/[HA]) =1.76 [A]/[HA] =$10^{1.76}$ =58 [HA] =58 [A] [A] = [H]= $10^{-pH} =10^{-3}$ = [HA] =58 [A] = 58 $\times10^{-3}$ =0.058 M Molecular weight of acetic acid = 60g/mol Density =1.049 g/mL Concentration of acetic acid = Density /molecular weight = 1.049 / 60 =0.017 mol/mL Volume of acetic acid to prepare 1 L of vinegar = [HA]/ Concentration = 0.058/0.017 = 3.3 mL
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