What was the volume of 6.12 M acetic acid HC2H3O2 needed to prepare the 250 mL acetic acid/acetate ion buffer solution required in this part? Show your calculations.

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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By the use of Henderson Hasselbalch equation;

pH  = pKa  + log{[acetate ion]/[acetic acid]}

4.5 = 4.75 + log{[0.10 M]/[acetic acid]}

-0.25 = log{[0.10 M]/[acetic acid]}

[Acetic acid]  = 0.10 M/ 10-0.25

[Acetic acid]  = 0.10 M/0.56

 [Acetic acid]   = 0.1786 M

Moles of sodium acetate dissolved in 250 mL buffer solution = 0.10 M× (250mL/1000mL) × 1L

  = 0.025 mol

Weight (w) of sodium acetate (purity 100%) dissolved to prepare 250 mL of solution with buffer concentration of 0.10 M is calculate as follow;

w100% =  0.025 mol × 82.0343 g/mol = 2.051 g

Weight (w) of sodium acetate (purity 99%)  is calculate as follow;

w99%   = 2.051 g× (100/99) = 2.072 g


What was the volume of 6.12 M acetic acid HC2H3O2 needed to prepare the 250 mL acetic acid/acetate ion buffer solution required in this part? Show your calculations.

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