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Lab 19a Investigating Chemical Equilibrium

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Lab 19A: Investigating Chemical Equilibrium

Purpose:

        To observe shifts in equilibrium concentrations when stresses such as temperature changes are applied through recognizing macroscopic properties of chemical systems and being able to explain the results using Le Chatelier's principle.


Materials:

        Please see page 209 of the “Heath Lab Manual.”


Note: Changes made to the materials/procedure include the optional use of microplates for parts 4 and 5, 250mL Erlenmeyer flasks for parts 1 and 2, 100mL graduated cylindres for part 3, and 10mL graduated cylindres for measuring.


Procedure:


        Please see pages 209-212 of the “Heath Lab Manual.”

Note: Changes made to the materials/procedure include the optional use of microplates for parts 4 and 5, 250mL Erlenmeyer flasks for parts 1 and 2, 100mL graduated cylindres for part 3, and 10mL graduated cylindres for measuring.

Data and Observations:

Table #1: Equilibrium Involving Thymol Blue

Reagent added

Stress (ion added)

Colour observation

Directon of equilibrium shift

HCl (step 3)

HCl (step 4)

NaOH (step 5)

NaOH (step 6)

Table #2: Equilibrium Involving Thiocyanatoiron (III) Ion

Reagent added

Stress (ion added)

Observation

Direction of equilibrium shift

KCl (test tube B)

Fe(No3)3 (test tube C)

KSCN (test tube D)

NaOH (test tube E)

Table #3: Equilibrium Involving Cobalt (II) Complexes

Stress

Observation

Direction of equilibrium shift

Step 4

Step 5

Step 6

Table #4: Equilibrium Involving Chromate and Dichromate Ions

Steps 2 and 3

0.1M K2CrO4

0.1M K2Cr2O7

Initial Colour

1M NaOH added

1M HCl added

Step 4

0.1M K2CrO4

0.1M K2Cr2O7

Initial Colour

1M HCl added

1M NaOH added

Steps 5 and 6

Initial Colour

+1M NaOH

+0.1M Ba(NO3)2

+1M HCl

0.1M K2CrO4

Steps 7 and 8

Initial Colour

+1M HCl

+0.1M Ba(NO3)2

+1M NaOH

0.1M K2CrO4

Step 9

0.1M K2CrO4

0.1M K2Cr2O7

Add 1.0M Ba(NO3)2

Table #5: Equilibrium Involving Copper (II) Complexes

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