pH (calculated and theoretical) of prepared buffer solutions Show all work with units. The answers must have the correct units and the correct number of significant figures.
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Experiment 1: Preparation and pH of Buffer Solutions
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 |
- pH (calculated and theoretical) of prepared buffer solutions
Show all work with units. The answers must have the correct units and the correct number of significant figures.
|
Buffer Solution |
Acetic Acid; Molarity* |
Sodium Acetate Molarity* |
Recorded pH |
Calculated pH |
A |
||||
B |
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C |
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D |
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E |
*Concentration in the buffer solution
Ka (acetic acid) = 1.8 x 10-5
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