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Buffers

Last updated

Oct 20, 2020
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- Biofuels Titration
- Buret Calibration and Stardardization of NaOH Solution

Contributor
Analytical Sciences Digital Library

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Learning Objectives

After completing this exercise, students will be able to:

Identify a buffer solution.
Calculate the pH of a buffer solution.
Calculate the amount of reagents required to prepare a buffer solution.
Design an acid/base titration.
Choose a proper acid/base indicator.

Part 1. Buffer Solutions

Determine if each of the following results in the formation of a buffer solution. Justify your answer. Calculate the pH of the buffer solutions.
1. A solution containing 0.100 M acetic acid and 0.150 M sodium acetate
2. A solution containing 1.2 mM NH₃ and 0.40 M NH₄Cl.
3. A solution containing 0.25 M NaOH and 0.25 M HCl.
4. A solution prepared by mixing 10.00 mL of 0.100 M NaHCO₃ and 10.00 mL of 0.200 M Na₂CO₃.
5. A solution prepared by mixing 25.00 mL of 0.50 M citric acid with 75.00 mL of 0.50 M NaOH.

Describe how you would prepare 250 mL of a 100 mM acetate buffer with a pH of 5.0. You have the following available to you in the lab: 17.4 M acetic acid, solid sodium acetate, 1.0 M NaOH, and 1.0 M HCl.

Contributors and Attributions

Susan Oxley, St. Mary’s University (San Antonio) (soxley@stmarytx.edu)
Sourced from the Analytical Sciences Digital Library

Contributors and Attributions

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