Equilibrium Labv4
INVESTIGATING EQUILIBRIUM EXPERIMENT
Objectives
1. To recognize the macroscopic properties of three chemical systems at equilibrium.
2. To observe shifts in equilibrium concentrations as stresses are applied to the systems.
3. To explain observations by applying LeChatelier’s Principle.
Materials
12 test tubes test tube rack 2 -100mL beakers beaker tongs safety glasses stand ring clamp wire gauze bunsen burner sparker 2 -250mL beakers 10mL grad cylinder
0.2M FeCl3 0.2M KSCN 0.2M KCl 0.2M Fe(NO3)3
6.0M NaOH CoCl26H2O 6.0M HCl water
0.1M K2CrO4 0.1M K2Cr2O7 1M NaOH 1M HCl
0.1M Ba(NO3)2
Procedure
PART I
1. Use a 10mL graduated cylinder to measure 1mL of 0.2M FeCl3 and pour it into a 250mL beaker. Using another 10mL graduated cylinder, measure 1mL of 0.2M KSCN. Record the colour of each solution under the equilibrium reaction in Data and Observations.
2. Add the 1mL portion of 0.2M KSCN to the beaker containing 0.2M FeCl3. Swirl the mixture and record the colour of FeSCN2+ under the equilibrium reaction in Data and Observations. Add enough water to the solution (80-120mL) to dilute the intense colour to a light amber colour.
3. Pour approximately 5mL of this solution into each of 5 test tubes labeled A to E. Test tube A serves as a control.
4. For each of the following reactions (steps 5-8), record the results in Table 1.
5. To test tube B, add 10 drops of 0.2M KCl.
6. To test tube C, add 10 drops of 0.2M Fe(NO3)3.
7. To test tube D, add 10 drops of 0.2M KSCN.
8. To test tube E, add 10 drops of 6.0M NaOH.
9. All solutions can go down the sink with plenty of water.
PART II
1. Place a pea-sized sample of CoCl26H2O into each of two 100mL beakers.
2. To the first beaker, add 10mL of 6.0M HCl and label the
Objectives
1. To recognize the macroscopic properties of three chemical systems at equilibrium.
2. To observe shifts in equilibrium concentrations as stresses are applied to the systems.
3. To explain observations by applying LeChatelier’s Principle.
Materials
12 test tubes test tube rack 2 -100mL beakers beaker tongs safety glasses stand ring clamp wire gauze bunsen burner sparker 2 -250mL beakers 10mL grad cylinder
0.2M FeCl3 0.2M KSCN 0.2M KCl 0.2M Fe(NO3)3
6.0M NaOH CoCl26H2O 6.0M HCl water
0.1M K2CrO4 0.1M K2Cr2O7 1M NaOH 1M HCl
0.1M Ba(NO3)2
Procedure
PART I
1. Use a 10mL graduated cylinder to measure 1mL of 0.2M FeCl3 and pour it into a 250mL beaker. Using another 10mL graduated cylinder, measure 1mL of 0.2M KSCN. Record the colour of each solution under the equilibrium reaction in Data and Observations.
2. Add the 1mL portion of 0.2M KSCN to the beaker containing 0.2M FeCl3. Swirl the mixture and record the colour of FeSCN2+ under the equilibrium reaction in Data and Observations. Add enough water to the solution (80-120mL) to dilute the intense colour to a light amber colour.
3. Pour approximately 5mL of this solution into each of 5 test tubes labeled A to E. Test tube A serves as a control.
4. For each of the following reactions (steps 5-8), record the results in Table 1.
5. To test tube B, add 10 drops of 0.2M KCl.
6. To test tube C, add 10 drops of 0.2M Fe(NO3)3.
7. To test tube D, add 10 drops of 0.2M KSCN.
8. To test tube E, add 10 drops of 6.0M NaOH.
9. All solutions can go down the sink with plenty of water.
PART II
1. Place a pea-sized sample of CoCl26H2O into each of two 100mL beakers.
2. To the first beaker, add 10mL of 6.0M HCl and label the