1. What is a buffer? How does a buffer keep pH constant? Write the two reactions that are taking place in the sodium acetate/acetic acid buffer solution that you prepared in Experiment 1. Compare the calculated pH of buffers A, B, C, D, and E to the measured pH of each of these buffers in Experiment 1. What did you notice? Describe what may have accounted for any variations in pH if you saw any variations.
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Experiment 1: Preparation and pH of Buffer Solutions
- Test Data:
- Mass of Sodium Acetate :4.0 g
- Volume of Sodium Acetate Solution: 100.00mL
- Acetic Acid Concentration (mass percent from label) :4.5%
- pH of Prepared Buffer Solutions
Buffer Solution |
Acetic Acid; 4.5% |
Sodium Acetate Solution |
Recorded pH |
A |
5.0 mL |
5.0 mL |
4.3 |
B |
5.0 mL |
1.0 mL |
4.2 |
C |
10.0 mL |
1.0 mL |
3.4 |
D |
1.0 mL |
10.0 mL |
5.0 |
E |
1.0 mL |
5.0 mL |
4.5 |
- Calculations/Results
*Show all work with units. The answers must have the correct units and the correct number of significant figures
- Sodium acetate moles 0.049 mol
(molar mass = 82.0 g/mol)
- Molarity of sodium acetate = 0.49 M
- Concentration of acetic acid (from bottle) =4.5 %
- Molarity of acetic acid = 0.75 M
(molar mass = 60.0 g/mol; density of the solution is 1.0 g/mL)
questios
1. What is a buffer? How does a buffer keep pH constant? Write the two reactions that are taking place in the sodium acetate/acetic acid buffer solution that you prepared in Experiment 1.
- Compare the calculated pH of buffers A, B, C, D, and E to the measured pH of each of these buffers in Experiment 1. What did you notice? Describe what may have accounted for any variations in pH if you saw any variations.
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