47
6
CHEM 104 LAB 2
Notebook
Experiment #: 2
Title: Equilibrium Reactions
Purpose: To learn about equilibrium reaction and be able to calculate the equilibrium
constant KC. Also to examine how various equilibrium reactions shift when subjected to
changes in temperature or concentration.
Procedure:
Experiment #1 : Esterification reaction between acetic and propyl alcohol titrated with sodium
hydroxide
1. Mix 10 ml of acetic acid and 10 ml of propyl alcohol in a flask
2. Pipette 1 ml sample of mixture into a beaker and add 25 ml water and several drops of
indicator
3. Titrate solution with sodium hydroxide (NaOH)
4. Observe and record amount of NaOH required to neutralize acetic acid
5. Add sulfuric acid catalyst to original solution
6. Pipette 1 ml sample of mixture with catalyst into a beaker and add 25 ml water and
several drops of indicator
7. Titrate solution with sodium hydroxide (NaOH)
8. Observe and record amount of NaOH required to acetic acid
9. Heat the mixture of acetic acid, propyl alcohol, and sulfuric acid catalyst for 1 hour
with Bunsen burner and reflux condenser, which will bring the reaction to
equilibrium and form propyl acetate
and water
10. Once it has come to equilibrium, pipette 1 ml sample of mixture with catalyst into
a beaker and add 25 ml water and several drops of indicator
11. Observe and record amount of NaOH required to acetic acid
12. Use values to solve for concentration of acetic acid present and use those to calculate KC
Experiment #2
1. Yellow Fe+3 + colorless 6SCN- ↔ Dark red Fe(SCN)6-3
2. Blue Cu(H2O)4+2 + 4Cl- ↔ green Cu(Cl)4-2
3. Yellow 2CrO
-2
+ 2H3O+ ↔ orange
Cr2O -2
+ 3H2O
4. White solid NaCl(s) ↔ colorless solution Na+ + Cl-
5. Yellow solid 2BaCrO4 + 2H3O ↔ orange solution 2Ba+2 + Cr2O7-2 + 3H2O
6. Pink Co(H2O) +2 + colorless 4Cl- + heat ↔blue CoCl4-2
