Honors Chemistry
Name _________________________________
Chapter 7: Types of Chemical reactions Lab
Date _____/_____/_____
Period _____
Objectives
1. In the pre-laboratory work, students are to classify the reactions for each of the following laboratory
experiments and write a balanced equation that includes the states of the reactants and products for
each experiment.
2. During the experiments, students are expected to apply proper safety precautions, to record detailed
observations, and to indicate what part of the observations can be used to determine that a chemical
reaction has occurred.
Pre-Lab Questions
1. What are the 5 indications that a chemical reaction has taken place?
2. List the 6 different types of chemical reactions and how to determine each when given the reactants.
3. What is the hottest part of the Bunsen burner flame?
4. What type of reaction occurs in each of the experiments below? Write a balanced equation for each
experiment that includes the states of both the reactants and products and list the driving force and
spectator ions
Materials
Chemicals
0.1 M Barium nitrate
0.1 M Sodium sulfate
5 M Copper II Chloride
Aluminum foil
Methane gas
Sodium bicarbonate
Potassium chlorate
Glassware / Equipment
0.1 M Potassium hydroxide
0.1 M Nitric acid
Phenolphthalein Indicator
Magnesium ribbon
0.1 M Lead II nitrate
0.1 M Potassium iodide
Test tubes
Test tube clamp
Wood splints
10 mL graduated cylinders
Bunsen burner
Electronic balance
Ring stand
Crucible
Clay triangle
Safety
-
Wear safety goggles at all times.
Prevent solutions from contacting skin.
-
Wash your hands before you leave.
Properly dispose of all chemicals.
Experiments
1. Pour approximately 5 mL of 0.1 M Barium nitrate solution in the Barium nitrate test tube and approximately
5 mL of 0.1 M Sodium sulfate solution into the Sodium sulfate test tube. After recording your observations,
pour both solutions into the mix test tube. After recording your observations, pour the resulting product(s)
down the drain with excess water from and rinse out the test tubes.
2. Pour approximately 5 mL of 5 M Copper II Chloride and pour it into the Copper II Chloride test tube. Then
obtain a quarter sized piece of Aluminum foil and crumble it into a very loose ball. Take the test tube, test
tube rack, and aluminum ball back to your station. Drop the aluminum ball into the test tube of copper II
chloride. After recording your observations, pour the resulting liquid product down the drain with excess
water and throw the solid in the trash.
3. Attach the Bunsen burner to the gas jet, turn on the gas, light the Bunsen burner with the striker, and
record your observations.
4. Place approximately 1 inch of Sodium bicarbonate in the bottom of a test tube. Place the test tube in a
test tube clamp and gently tighten. Attach the test tube clamp to a ring stand. Make sure that the
test tube is turned toward the wall and away from everyone. Light a Bunsen burner, place it under the
test tube, and slowly heat the Sodium bicarbonate. After about a minute of heating, light a wood splint
and insert it into the test tube. After it has cooled, pour the resulting product(s) in the trash.
5. This experiment will be completed by the teacher in the fume hood: Approximately 4 – 5 grams of
Potassium chlorate will be placed in a test tube. The test tube will be placed in a test tube clamp which is
attached to a ring stand. A lit Bunsen burner will be place under the test tube and heated strongly. After
about a minute or two of heating, the embers of a lit wood splint will be insert into the test tube.
6. Place approximately 5 mL of 0.1 M Potassium hydroxide into the Potassium hydroxide test tube and
approximately 5 mL of 0.1 M Nitric acid into the Nitric acid test tube. After recording your observations,
pour both solutions into the mix test tube. After recording your observations, pour the resulting product(s)
down the drain with excess water and rinse out the test tubes.
7. Pour approximately 5 mL of 0.5 M Potassium hydroxide into the Potassium hydroxide test tube and add 1
drop of phenolphthalein. Pour approximately 5 mL of 0.5 M Nitric acid into the Nitric acid test tube. After
recording your observations, pour both solutions into the mix test tube. After recording your observations,
pour the resulting product(s) down the drain with excess water and rinse out the test tubes.
8. Weigh a sanded 2 cm piece of Magnesium, crucible, and lid on the electronic balance and record the
weight. Then take the crucible, with magnesium, back to your lab station and place the crucible on the clay
triangle that is placed on top of the ring that is attached to the ring stand. Light the Bunsen burner and
begin heating the crucible until the reaction is complete. Continue heating for an additional two minutes to
assure that all of the magnesium has reacted. Turn off the Bunsen burner and place the crucible on the
wire gauze to cool. Once it has cooled to room temperature, weigh and record the crucible, lid, and
resulting product(s). Scrape the products into the trash and wipe out the crucible with a wet paper towel.
9. Pour approximately 5 mL of 0.1 M Lead II nitrate solution into the Lead II nitrate test tube and approximately
5 mL of 0.1 M Potassium iodide solution into the Potassium iodide test tube. After recording your
observations, pour both solutions into the mix test tube. After recording your observations, pour the
resulting products down the drain with excess water and rinse out the test tubes.
10. Pour 5 mL of 3.0 M Hydrochloric acid in a test tube and take the test tube and test tube rack back to your
lab station. Drop one rolled up 2 cm piece of magnesium into the test tube. After about 30 seconds, light
a wood splint and place the flame above the opening of the test tube. After recording your observations,
pour the resulting products down the drain with excess water and rinse out the test tube.
Observation Table
Substances
Observations
Reactants
1. Barium nitrate + Sodium sulfate
2. Copper II Chloride + Aluminum
3. Methane + spark
4. Sodium bicarbonate + Heat
5. Potassium chlorate + Heat
6. Potassium hydroxide + Nitric acid
7. Potassium hydroxide + Nitric acid
+ indicator
8. Magnesium + Heat
9. Lead II nitrate + Potassium iodide
10. Hydrochloric Acid + Magnesium
Products
Teachers Notes
DD
1. Ba(NO3)2(aq)
SD
2. 3 CuCl2(aq)
C
3. CH4(g)
+
+
+

Na2SO4(aq)

2 Al(s)

2 O2(g)
2 NaNO3(aq)
2 AlCl3(aq)
CO2(g)
+
+
+
BaSO4(s)
3 Cu(s)
2 H2O(g)
4. The heating of sodium bicarbonate at lower temperature can produce the first reaction and at
higher temperature and a long period of time can produce both of the following reactions.
+

D
2 NaHCO3(s)
D
Na2CO3(s)
D
5. 2 KClO3(s)
N
6. KOH(aq)
+
HNO3(aq)

N
7. KOH(aq)
+
HNO3(aq)
+
S
8. 2 Mg(s)
DD
9. Pb(NO3)2(aq)
+
SD
10. 2 HCl(aq)
Mg(s)
+
Heat
Heat
+
+

+
Na2O(s)

Heat
O2(g)
+
Na2CO3(s)

H2O(g)
+
KNO3(aq)

+
H2O()
KNO3(aq)
+
H2O()
2 MgO(s)
PbI2(s)
MgCl2(aq)
CO2(g)
3 O2(g)
Indicator (phth) 

+
CO2(g)
2 KCl(s)
Heat
2 KI(aq)
+
+
+
+
2 KNO3(aq)
H2(g)
Preparing the Chemicals
0.1 M Ba(NO3)2
– 13.07 g of Ba(NO3)2 per 500 mL of 0.1 M Ba(NO3)2 solution
0.1 M Na2SO4
– 7.10 g of Na2SO4 per 500 mL of 0.1 M Na2SO4 solution
0.1 M HNO3
– 3.2 mL of concentrated HNO3 per 500 mL of 0.1 M of HNO3 solution
0.1 M KOH
– 2.8 g of KOH per 500 mL of 0.1 M KOH
0.1 M Pb(NO3)2
– 16.56 g of Pb(NO3)2 per 500 mL of 0.1 M Pb(NO3)2 solution
0.1 M KI
– 8.3 g of KI per 500 mL of 0.1 M KI solution
3.0 M HCl
– 125 mL of HCl per 500 mL of 3.0 M HCl solution