Name _____________________________ Period _______ Teacher _____________

Physical Science

Unit 10 – Reactions

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Term Definition
Reaction
Equation

Reactants

Products

Mole

Molar Mass

Synthesis

Decomposition

2
Term Definition
Single
Replacement

Double
Replacement
Precipitation Neutralization

Acid

Base

Catalyst

Endothermic

Exothermic

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Chemical Reaction Introduction
Types of Chemical Reactions
Synthesis/Combination Decomposition
Single Displacement/Replacement Double Displacement/Replacement
Neutralization (Double Displacement/Replacement)

For each reaction below, identify the type of reaction

1. Na3(PO4) + 3 KOH  3 NaOH + K3(PO4) _____________________________________________

2. MgCl2 + Li2(CO3)  Mg(CO3) + 2 LiCl _____________________________________________

3. HCl + NaOH  H2O + NaCl _____________________________________________

4. Pb + Fe(SO4)  Pb(SO4) + Fe _____________________________________________

5. CaCO3  CaO + CO2 _____________________________________________

6. P4 + 3 O2  2 P2O3 _____________________________________________

7. 2 RbNO3 + BeF2  Be(NO3)2 + 2 RbF _____________________________________________

8. 2 AgNO3 + Cu  Cu(NO3)2 + 2 Ag _____________________________________________

9. 2 (C5H5) + Fe  Fe(C5H5)2 _____________________________________________

10. SeCl6 + O2  SeO2 + 3Cl2 _____________________________________________

11. 2 MgI2 + Mn(SO3)2  2 Mg(SO3) + MnI4 _____________________________________________

12. H2SO4 + Mg(OH)2  2 H2O + MgSO4 _____________________________________________

Observe the integers before the compounds in the reactions above (full size, whole numbers). These Type of RXN
numbers serve to balance the chemical reaction. Below, attempt to balance the given reaction: Circle One
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. ____ Fe + ____ AgCl  ____ FeCl3 + ____ Ag SR / DR
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. ____ AgNO3 + ____ NaCl  ____ AgCl + ____ NaNO3 SR / DR
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. ____ MgSO4 + ____ Pb(NO3)4  ____ Mg(NO3)2 + ____ Pb(SO4)2 SR / DR
16
. ____ Br2 + ____ NaI  ____ I2 + ____ NaBr SR / DR
17
. ____ HCl + ____ Zn  ____ ZnCl2 + ____ H2 SR / DR
18
. ____ NaOH + ____ CaBr2  ____ _______ + ____ _______ SR / DR
19
. ____ Mg + ____ NiCl2  ____ _______ + ____ _______ SR / DR

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Synthesis and Decomposition
Part 1 – Synthesis
-- Procedure
1. Collect-- a 4g sample of steel wool, 1 meter stick, 1 Al Foil tray, 1 note card, and 3 pennies
2. Observe the properties of the steel wool and record in analysis question 1
3. Follow classroom demonstration on how to create the mechanism for this lab
4. Ignite your steel wool and observe what happens while it is reacting
5. Observe the properties of the steel wool after reacting and compare it to the initial properties (Q1)
Analysis

1. Describe how the physical properties of the products are different from the reactants?

2. What happened to the mass of the steel wool?

3. Write a balanced chemical equation for the reaction. (Predict the formula of the product; assume iron
will have a +3 charge)

4. What was the limiting reactant? How do you know?

5. When the steel wool was burning, the expected mass was more than the mass that we actually had at
the end. Where did that mass go?

Part 2 – Decomposition
-- Procedure
1. Place --
1-2 cm of hydrogen peroxide into a test tube. Use a test tube holder.
2. Using a scoopula, add a pinch of manganese (IV) oxide as a catalyst for the reaction.
3. Place your thumb over the mouth of the test tube to trap the gas. Wait 2 minutes.
4. Test the gas that is being given off by placing a glowing splint into the tube. (Light a wooden splint,
blow the flame out. If the flame returns, the presence of oxygen is indicated.)
Analysis

1. What observations can be made from this reaction?

2. Was O2 produced? Explain how you know.

3. Write a complete balanced equation for this reaction (remember MnO2 is a catalyst)

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Single and Double Replacement Reactions
Part 1 – Single Replacement
1. What is the chemical formula for copper (II) nitrate? Consider the charges.

2. Fill a small test tube 2/3 full will a solution of copper (II) nitrate. Place a small piece of Zinc in the tube.
3. Record your observations.

4. Write the balanced chemical equation for the reaction between copper (II) nitrate and zinc metal. This
reaction is an example of Single Replacement.

5. In the reaction, what two chemical species are changing places?

Part 2 – Double Replacement

3. For calcium chloride, how much would you weigh out on a balance to measure out to get…

1 mole Calcium Chloride = ______________ g Calcium Chloride

0.5 mole Calcium Chloride = ______________ g Calcium Chloride

0.02 mole Calcium Chloride = ______________ g Calcium Chloride

Procedure

1. Weigh 0.020 moles of calcium chloride and place in one 100-250 mL beaker.
2. Weigh 0.020 moles of sodium sulfate and place in another 100-250 mL beaker.
3. Add 30 mL of distilled water to each beaker then stir with stir rods until the salts dissolve. This may take
a few minutes, but the solutions should be clear when dissolved.
4. When fully dissolved, pour the sodium sulfate solution into the calcium chloride solution. What do you
observe? It may take 3-5 minutes for the reaction to complete. ________________________________

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 ____________________________________________________________________________________
5. Obtain a piece of filter paper and make it into a funnel using the folding method. Record the mass in the
data table.
6. Add your group initials to the filter funnel with a pencil, then record the mass of the filter paper in the
data table.
7. Start filtering the solution. Rinse the filter paper with small amounts of distilled H 2O to ensure that the
entire chemical product is as pure as possible. Carefully rinse the product to the bottom center of the
filter paper.
8. Remove the filter paper and place onto the provided yellow tray to dry until next class.
9. Clean everything in you work area and dispose of remaining solutions, rinsing down the drain.
10. (Next day) Obtain the mass of the filter paper with the chemical product. Record this data. Dispose of
the product in the trashcan.

Data

Mass of the filter paper (g)

Mass of the filter paper + product (g)

Postlab Analysis

1. Calculate the amount of calcium sulfate in grams that was collected on the filter paper.

2. Based on the balanced chemical reaction, what is the ratio of the two reactants to the calcium sulfate
precipitate?

3. By reacting 0.020 moles of each reactant, ________________________ moles of CaSO4 should have been
formed.

4. Calculate the molar mass in g/mol of CaSO4.

5. Determine the theoretical mass of CaSO4 that should have been produced. Multiply the moles in question 3
with the molar mass in question 4.

6. Do your actual results agree with the theoretical mass? Calculate your percent error.

7. Draw particle representation of a single replacement and double replacement reactions below.

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Cabbage Juice pH Standardization
Creating the cabbage juice indicator
1. Chop up cabbage (enough thinly sliced cabbage to half-fill a 250 mL beaker)
2. Add cabbage to beaker and cover with water
3. Boil until the solution is purple. Decant the purple indicator solution into a small flask and seal.
4. Dispose of the cabbage in the trash can (not the sink).
Setup the pH probe
1. Install Vernier Graphical Analysis chrome app on your chromebook.
2. Plug in the LabQuest mini into the chromebook.
3. Plug a pH probe into the LabQuest (be sure to put it in the correct channel – not digital)
4. Run the Graphical Analysis app – switch the mode to Probe/Meter to get a large pH readout.
Color pH

Red

Pink (magenta)

Purple

Dark Purple

Blue

Turquoise

Green (emerald)

Green (apple)

Prepare cabbage juice for standardization

1. Measure 25 mL of indicator juice and add to a 250 mL beaker. Dilute with DI water to approximately
75mL.
2. Measure the pH of the indicator juice for the correct color .
3. With a pipet, add a small amount of hydrochloric acid to the solution in the beaker until it turns red.
4. Measure and record the pH of the solution.
5. Add a small amount of NaOH with a pipet. Watch for a color change. Add more base if needed. Record
the pH of each color and continue adjusting the solution color with additions of base (as acid if needed)
6. Dispense of the solution and rinse the beaker to prepare for the next part of the lab.

My Unknown is __________________________. It turned my Indicator ________________________ (color),

which corresponds to a pH of ________________ and is considered ______________________(acidic/basic).

Among all the unknowns, ranked from least acidic to most acidic, this solution is ranked:

1 2 3 4 5 6 7 8
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