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.
Ionic Equilibrium
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.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
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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