Le Châtelier Principle Lab Report
Applications of Le Châtelier's Principle
(September 11 - 15, 2014)
**The purpose of this experiment was to visually observe the effects of how changing certain aspects of the reaction affected the observed equilibrium.
PROCEDURE:
Introductory activity
Part A: Effect of Concentration:
Two different temperature water baths were created, one at 65-70oC, the other ice, and set aside for Part B.
20 mL of potassium thiocyanate solution were poured into a petri dish. The initial color and all subsequent observations were recorded in the data table.
Three drops of iron (III) nitrate were added to different spots in the petri dish, and the resulting solution was swirled until the color was consistent.
Approximately ½ pea-sized sample of potassium …show more content…
2 mL of the cobalt chloride solution was added to three separate test tubes (A, B, and C).
1 mL of silver nitrate (milky white color) was added in test tube A
Three gains of calcium chloride was added to test tube B
1 mL of Hydrochloric Acid was added to test tube C
Activity D: Solubility of Carbon Dioxide:
Approximately 10 mL of fresh seltzer water has mixed with 20 drops of 0.04 % bromcresol green indicator. The initial color was compared to a pH chart.
The solution was drawn up into a syringe, the excess air squeezed out, and the syringe capped.
A vacuum was generated by pulling out the syringe, and the solution was shaken.
The solution was then compared against a color coded pH chart to determine any change.
Activity E: Solubility of Magnesium Hydroxide
10 mL of milk of magnesia was added to 50 mL or deionized water in a beaker with 5 - 10 drops of universal indicator solution. This mixture was placed on a magnetic stirrer, to ensure consistent …show more content…
When adding a reactant into the solution, the volume of the solution (and as a result the concentration of the reactants in the solution) was immediately changed. Using Le Châtelier's Principle we were able to predict which side the reaction would be shifted. The delineation between the reactant and products colors allowed for this. Changes in equilibrium could easily be observed though visible, qualitative color changes. These color changes were indications of Le Châtelier's Principle, which states that if a system is subject to stress, the system will react to remove the stress. To remove the stress, reactions either shift to the right and form more products, or to the left adding more reactants to the
(September 11 - 15, 2014)
**The purpose of this experiment was to visually observe the effects of how changing certain aspects of the reaction affected the observed equilibrium.
PROCEDURE:
Introductory activity
Part A: Effect of Concentration:
Two different temperature water baths were created, one at 65-70oC, the other ice, and set aside for Part B.
20 mL of potassium thiocyanate solution were poured into a petri dish. The initial color and all subsequent observations were recorded in the data table.
Three drops of iron (III) nitrate were added to different spots in the petri dish, and the resulting solution was swirled until the color was consistent.
Approximately ½ pea-sized sample of potassium …show more content…
2 mL of the cobalt chloride solution was added to three separate test tubes (A, B, and C).
1 mL of silver nitrate (milky white color) was added in test tube A
Three gains of calcium chloride was added to test tube B
1 mL of Hydrochloric Acid was added to test tube C
Activity D: Solubility of Carbon Dioxide:
Approximately 10 mL of fresh seltzer water has mixed with 20 drops of 0.04 % bromcresol green indicator. The initial color was compared to a pH chart.
The solution was drawn up into a syringe, the excess air squeezed out, and the syringe capped.
A vacuum was generated by pulling out the syringe, and the solution was shaken.
The solution was then compared against a color coded pH chart to determine any change.
Activity E: Solubility of Magnesium Hydroxide
10 mL of milk of magnesia was added to 50 mL or deionized water in a beaker with 5 - 10 drops of universal indicator solution. This mixture was placed on a magnetic stirrer, to ensure consistent …show more content…
When adding a reactant into the solution, the volume of the solution (and as a result the concentration of the reactants in the solution) was immediately changed. Using Le Châtelier's Principle we were able to predict which side the reaction would be shifted. The delineation between the reactant and products colors allowed for this. Changes in equilibrium could easily be observed though visible, qualitative color changes. These color changes were indications of Le Châtelier's Principle, which states that if a system is subject to stress, the system will react to remove the stress. To remove the stress, reactions either shift to the right and form more products, or to the left adding more reactants to the