KC. Also to examine how various equilibrium reactions shift when subjected to changes in

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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

• Mix 10 ml of acetic acid and 10 ml of propyl alcohol in a flask
• Pipette 1 ml sample of mixture into a beaker and add 25 ml water and several drops of indicator
• Titrate solution with sodium hydroxide (NaOH)
• Observe and record amount of NaOH required to neutralize acetic acid
• Add sulfuric acid catalyst to original solution
• Pipette 1 ml sample of mixture with catalyst into a beaker and add 25 ml water and

several drops of indicator

• Titrate solution with sodium hydroxide (NaOH)
• Observe and record amount of NaOH required to acetic acid
• 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

• 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

• Observe and record amount of NaOH required to acetic acid
• Use values to solve for concentration of acetic acid present and use those to calculate KC

Experiment #2

• Yellow Fe

+3

• colorless 6SCN

- ↔ Dark red Fe(SCN)6 -3

• Blue Cu(H2O)4

+2

• 4Cl

- ↔ green Cu(Cl)4 -2

• Yellow 2CrO

- 2

• 2H3O+ ↔ orange Cr2O

-2

+ 3H2O

• White solid NaCl(s) ↔ colorless solution Na

+

• Cl

-

• Yellow solid 2BaCrO4 + 2H3O ↔ orange solution 2Ba

+2

• Cr2O7

-2

+ 3H2O

• Pink Co(H2O)

+2

• colorless 4Cl

-

• heat ↔blue

CoCl4 -2

+ 6H2O

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Data/Results/Calculations:

Reaction equation: CH3COOH + C3H7OH ↔ CH3COOCC3H7 + H2O

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