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Buffers

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    282534

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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

    1. 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.















     

    1. 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.

     

     

     

     

     

     

     

     

     

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    This page titled Buffers is shared under a CC BY-NC-SA 4.0 license and was authored, remixed, and/or curated by Contributor via source content that was edited to the style and standards of the LibreTexts platform; a detailed edit history is available upon request.