CHEMICAL REACTIONS
Objective:
Students will identify and write net ionic equations for synthesis, precipitation, decomposition,
redox, anhydrides, combustion, acid base, and complex ion reactions.
Safety
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Do not look directly into the flame when burning magnesium
Tie back long hair
Wear safety goggles and aprons
If you are allegoric to sulfur, tell the instructor immediately
Equipment
3-50 ml beakers
2-gas collecting bottles
Pipettes (droppers)
1-graduated cylinder
Deflagrating spoon
Bunsen burner
2-wide mouth bottles
6-test tube
2-watch glasses
2-straws
1-generator bottle with tubing
water trough
crucible tongs
Chemicals
Magnesium oxide
Universal indicator
0.1 M sodium hydroxide
0.1 M aluminum nitrate
Hydrogen peroxide
Magnesium metal
Copper metal
Charcoal
0.1 M copper (II) nitrate
Solid sodium metal
phenolphthalein
0.1 M iron (III) nitrate
0.1 M zinc metal
magnesium dioxide
sulfur
0.1 M silver nitrate
0.1 M 0.1 M hydrochloric acid
6.0 M ammonia
0.1 M sodium hydroxide
Procedure
Experiment 1
Place 2.00 g of magnesium oxide in a 50.0 ml beaker. Add 20.0 ml of water and mix. Place 2
drops of phenolphthalein into the mixture. Record your observations. Phenolphthalein is used to
test for a base.
Experiment 2
Place 20.0 ml of water in a 50.0 ml beaker. Use a straw and blow into the water for at least 5
minutes. Do not forget to breath. Partners may use two straws and take turns. Place 2 drops of
universal indicator in the solution. Record your observations and compare it to the pH color
chart.
Experiment 3
Using crucible tongs place approximately 4.00 cm of magnesium metal into the flame of the
Bunsen burner using tongs. Do not look directly into the flame. Record your observation.
Experiment 4
Place 20 drops of iron III nitrate in a test tube. Add 20 drops of sodium hydroxide. Record your
observations.
Experiment 5
Place 1 small pieces of zinc metal in a 50.0 ml beaker. Add 10.0 ml of lead II nitrate. Do not
dispose by pouring down the sink. Place disposal beaker under the hood.
Experiment 6
Place 3 small pieces of copper in a 50 ml beaker. Add 10.0 ml of zinc nitrate. Do not dispose by
pouring down the sink. Place disposal beaker under the hood.
Experiment 7
Set up a gas-generating flask. Fill two wide mouth bottles full of water. Fill the water trough to
the top with water. Make sure the overflow tubes are in the sink. Place 10.0 g of manganese
dioxide in the generator bottle. Pour in 100.0 ml of hydrogen peroxide. Quickly stopper and
collect the gas by water displacement as demonstrated by the instructor. Take the bottle from the
water and cover with a watch glass. There should be enough gas generated to collect a second
bottle of gas. Leave about 2 cm of water in the second bottle. Record your observations. The
gas you collected is flammable. Keep away from open flames.
Experiment 8
Fill a deflagrating spoon about half full with charcoal. Place the charcoal in the flame for 3
minutes. Quickly remove from the flame and insert into a bottle of the gas you collected. Do
not pour the charcoal in the bottle. It should stay in the spoon. Record your observations.
Experiment 9
Using your crucible tongs ignite a small piece of steel wool. When it ignites, quickly place it in
the second bottle of gas with the 2 cm of water. Do not submerge the steel wool into the water.
Record your observations.
Experiment 10 - Teacher demonstration
If you are allergic to sulfur, inform your instructor. Obtain a pea size amount of sulfur in a
deflagrating spoon. Ignite the spoon and sulfur in the Bunsen burner. Slowly lower it into a
bottle containing the same unknown gas collected in experiment 6. Record your observations.
Experiment 11
Add 5 ml of iron (II) sulfate (it is acidified) to a beaker. Add potassium permanganate drop wise
until you get a color change
Experiment 12
Add 2 ml of silver nitrate to 2 ml of HCl.
Experiment 13
To the above reaction add 5 ml of 6 M ammonia
Experiment 14
Add 2 ml of copper II nitrate to 2 ml of sodium hydroxide.
Experiment 15
To the test tube above add 3 ml of 6 M ammonia.
Experiment 16 (teacher demonstration)
Add a piece of sodium in a beaker of water. After the reaction has occurred, add a drop of
phenolphthalein.
Observations:
Exp. 1
Exp. 2
Exp. 3
Exp. 4
Exp. 5
Exp. 6
Exp. 7
Exp. 8
Exp. 9
Exp 10
Exp 11
Exp 12
Exp 13
Exp 14
Exp 15
Reaction Type
Questions
1. Write a balanced net ionic equation for the reaction in experiment 1.
2. Why was phenolphthalein used in experiment 1?
4. Write a balanced net ionic equation for the reaction in experiment 2.
5. After comparing your results with the pH chart in experiment 2, what should you
Conclude about the solution produced?
7. Write a balanced net ionic chemical equation for the reaction that occurred in experiment 3.
8. Write a balanced net ionic equation for the reaction that occurred in experiment 4.
9. Write a balanced net ionic equation for the reaction that occurred in experiment 5.
10. Write a balanced net ionic equation for the reaction that occurred in experiment 6.
11. What flammable gas was produced in experiment 7?
12. Why was manganese dioxide used in experiment 7?
13.
Write a balanced net ionic equation for experiment 7.
14. What element is the major component of charcoal?
15. Write a balanced net ionic equation for the reaction that occurred in experiment 8.
16. Name the nonflammable gas produced in experiment 8?
17. Write a balanced net ionic equation equation for the reaction that occurred in experiment 9.
18. Write a balanced net ionic equation for the reaction in step 10.
19. Write a balanced net ionic equation or the reaction in step 11.
20. Write a balanced net ionic equation for the reaction in step 12.
21.
Write a balanced net ionic equation for the reaction in step 13.
22. Write a balanced net ionic equation for the reaction in step 14.
23. Write a balanced net ionic equation for the reaction in step 15.
24. Write a balanced net ionic equation for the reaction in step 16.
25. Write a balanced chemical equation for the reaction that occurred while the Bunsen
burner was lit. Hint: The gas used in the lab was methane (CH4)