Reactions Lab
Introduction:
You will be completing and analyzing a series of reaction. For each reaction you will be
required to state what signs of a chemical reaction occurred, write a balanced equation, and state
what type of reaction it is and why.
Chemicals
 copper (II) carbonate
 potassium iodide
 lead (II) nitrate
 copper (II) sulfate
 Zinc
 Magnesium strips
 Copper wire
 Silver (I) nitrate
 Potassium carbonate
 Sodium bicarbonate
Materials
 Bunsen Burner
 Wood splints
 Well plate
 Pipettes
Safety:
You will be using Bunsen burners in some of these reactions and you will be working
with some chemicals that can be detrimental if used incorrectly. Please follow all safety rules
while completing this lab.
Conclusion:
1. Write out a balanced chemical equation for each of the reactions
2. State the type of chemical reaction that is occurring and explain why you think that
3. Explain why a chemical reaction occurred during each one of the reactions using the
signs of chemical change and your observations.
Procedures:
Reaction 1: Copper (II) carbonate decomposes into copper (II) oxide and carbon dioxide
1. You will need to get a small sample of copper (II) carbonate from the sample at
your station and place this in a glass test tube. Make any observations you can
about this substance. (IE: Color, texture, state of matter, etc.)
2. Hold the test tube with a test tube holder over your lit Bunsen burner and hold the
test tube over the fire for about 30 seconds. DO NOT HOLD THE TEST TUBE
IN THE FIRE!!! You will notice a color change in the powder; record this
change.
3. Remove the test tube from the fire and place a lit wood splint into the mouth of
test tube and observe what occurs. If the fire goes out, it shows the presence of
carbon dioxide gas.
4. Observe the final product and write down any observations you make
5. Dump this material in the garbage. Wash out and dry the test tube for the next
group.
Reaction 2: lead (II) nitrate and potassium iodide react in water to form solid lead (II) iodide and
potassium nitrate
1. Obtain the well plate at your station and place a few drops of the potassium iodide
solution in one of the well plates using a clean pipette. Make any observations
that you can of this substance
2. Find the lead (II) nitrate solution and make any observations that you can of this
substance
3. Using a new, clean pipette, place a few drops of the lead (II) nitrate solution into
the well plate containing the potassium iodide. Observe and record any changes
that occur
4. Dump the well plate’s content down the sink. Wash and dry the well plate for the
next group to use
Reaction 3: Zinc metal when placed in a solution of copper (II) sulfate will react to form zinc
(II) sulfate and copper metal
1. Using a pipette place several drops of the copper (II) sulfate solution into one of
the well plates. Make observations of the color of the solution and how it looks.
2. Obtain a small piece of zinc metal from your station and wash it off. Make any
observations of the metal
3. Place the piece of zinc into the well plate containing the copper (II) sulfate
solution and allow this to sit for several minutes
4. Make any observations that you notice about the piece of metal and the color of
the solution.
5. Dump the contents of the well plate into the garbage. Rinse the well plate out and
dry it for the next group to use.
Reaction 4: Magnesium metal when burned with oxygen in the air forms magnesium oxide
1. You will need to obtain a small piece of magnesium strip for the samples
provided at the center. Examine the strip and write down all observations about it.
2. One student will hold the piece of magnesium with a pair of tongs
3. The student holding the tongs will place the tip of the magnesium strip into the
fire and let it sit there until it burns brightly. DO NOT LOOK DIRECTLY AT
THIS LIGHT!!! It may cause serious eye damage if you do so.
4. Once the strip starts burning brightly, place the strip into the crucible and let it
burn it’s self out.
5. Look at what is left in the crucible once it has cooled and write down your new
observations. The crucible will be hot, so do not touch it right away.
6. Dump the contents of the crucibles into the garbage. Rinse and dry out the
crucibles for the next group.
Reaction 5: Copper wire when burned will react with oxygen to form copper (II) oxide
1. You will need to obtain a small piece of copper wire from the samples provided at
the center. Examine the wire and write down all observations about it.
2. Only one person is needed for this experiment, the rest of the group will need to
just watch and write down observations and notes.
3. Place the piece of copper into the fire for a short time. There will not be a bright
light or anything to identify that the reaction has occurred.
4. Place the wire into a clean crucible, examine it, and write down any new
observations.
5. Dump the contents of the crucibles into the garbage. Rinse and dry out the
crucibles for the next group.
Reaction 6: Silver (I) nitrate in water will react with copper metal to form copper (II) nitrate and
silver metal
1. Using a pipette place several drops of the silver (I) nitrate solution into one of the
well plates. Make observations of the color of the solution and how it looks.
2. Obtain a small piece of copper metal from you station and make any observations
of the metal
3. Place the piece of copper into the well plate containing the silver (I) nitrate
solution and allow this to site for several minutes
4. Make any observations that you notice about the piece of metal and the color of
the solution.
5. Dump the contents of the well plate into the garbage. Rinse the well plate out and
dry it for the next group to use.
Reaction 7: Potassium carbonate and copper (II) sulfate react in water to form solid Copper (II)
carbonate and potassium sulfate
1. Obtain the well plate at your station and place a few drops of the potassium
carbonate solution using a clean pipette. Make any observations that you can of
this substance
2. Find the copper (II) sulfate solution and make any observations that you can of
this substance
3. Using a new, clean pipette, place a few drops of the copper (II) sulfate solution
into the well plate containing the potassium carbonate. Observe and record any
changes that occur
4. Dump the well plate’s content down the sink. Wash and dry the well plate for the
next group to use
Reaction 8: Sodium bicarbonate (bicarbonate - HCO3-1) will decompose when heated into
sodium carbonate, water, and carbon dioxide
1.
2.
3.
4.
Obtain a test tube. Clean and dry it if necessary.
Place about 1 medium scoop of sodium bicarbonate in the test tube.
Use a test tube clamp to hold the test tube containing the sodium bicarbonate.
Hold the test tube at a slight angle and pass it slowly back and forth through a lit
Bunsen burner flame several times. Note any changes occurring in the tube. DO
NOT hold the test tube in the flame; this will cause the test tube to break.
5. Pass the tube back and forth several more times.
6. Then perform a flaming splint test. Light a wooden splint and hold it into the
mouth of the test tube, if the flame goes out it shows the presence of carbon
dioxide.
7. Let the test tube cool and then dump out the remaining substance into the trash
can. Wash out the test tube thoroughly and dry for the next group.
Conclusion:
1. Write out a balanced chemical equation for each of the reactions
2. State the type of chemical reaction that is occurring and explain why you think that
3. Explain why a chemical reaction occurred during each one of the reactions using the
signs of chemical change and your observations.