Oxidation-Reduction Series
Purpose The purpose of this lab is to identify the different features that come about by using oxidation reduction and recording the observations, these tests will help determine the specific qualities each solution has.
Hypothesis
I theorize that nothing will happen with Magnesium because it is such a soft metal. Zinc should turn a greener color, because that’s what happens to a lot of statues and sculptures. I theorize that iron will tarnish badly because in air it can get tarnished so oxidation must do something as well.
Materials
1 Paper towels
1 Well-Plate
1 Tweezers, plastic
Experiment Bag Oxidation-Reduction
Activity Series 1 Copper (II) Sulfate, 1 M - 3 mL in Pipet
1 Iron (III) Chloride, 2 M - 3 mL in Pipet
1 Iron Metal, 2 pc in Bag 2"x 3" Magnesium Metal (ribbon) - 2 Small Pieces in Bag 2"x 3"
1 Magnesium Sulfate, 2 M - 3 mL in Pipet
1 Lead metal, 4 small pieces in bag 2 x 3”
1 Sodium Sulfate, 1 M - 3 mL in Pipet
1 Zinc Metal - 2 Small Pieces in Bag 2"x 3"
1 Zinc Nitrate, 2 M - 3 mL in Pipet
Procedure
1. Get all the materials
2. Place 10 drops of Sodium sulfate, Na2SO4 into well A1 of the 24-well plate.
3. Place 10 drops of Magnesium sulfate, Mg SO4 into well A2 of the 24-well plate.
4. Place 10 drops of Zinc nitrate, Zn(NO3)2 into well A3 of the 24-well plate.
5. Place 10 drops of Iron (III) chloride, FeCl3 into well A4 of the 24-well plate.
6. Place 10 drops of Copper (II) sulfate, Cu SO4 into well A5 of the 24-well plate.
7. Take the metal solids from your LabPaq
8. Use your tweezers to pick up and carefully insert the piece of magnesium into the sodium sulfate. Record your observations.
9. Carefully insert a piece of zinc into the magnesium sulfate. Record your observations.
10. Carefully insert a piece of lead into the zinc nitrate. Record your observations.
11. Carefully insert the lead into the iron (III) chloride. Record your observations.
12. In the same way carefully insert the iron into the
Hypothesis
I theorize that nothing will happen with Magnesium because it is such a soft metal. Zinc should turn a greener color, because that’s what happens to a lot of statues and sculptures. I theorize that iron will tarnish badly because in air it can get tarnished so oxidation must do something as well.
Materials
1 Paper towels
1 Well-Plate
1 Tweezers, plastic
Experiment Bag Oxidation-Reduction
Activity Series 1 Copper (II) Sulfate, 1 M - 3 mL in Pipet
1 Iron (III) Chloride, 2 M - 3 mL in Pipet
1 Iron Metal, 2 pc in Bag 2"x 3" Magnesium Metal (ribbon) - 2 Small Pieces in Bag 2"x 3"
1 Magnesium Sulfate, 2 M - 3 mL in Pipet
1 Lead metal, 4 small pieces in bag 2 x 3”
1 Sodium Sulfate, 1 M - 3 mL in Pipet
1 Zinc Metal - 2 Small Pieces in Bag 2"x 3"
1 Zinc Nitrate, 2 M - 3 mL in Pipet
Procedure
1. Get all the materials
2. Place 10 drops of Sodium sulfate, Na2SO4 into well A1 of the 24-well plate.
3. Place 10 drops of Magnesium sulfate, Mg SO4 into well A2 of the 24-well plate.
4. Place 10 drops of Zinc nitrate, Zn(NO3)2 into well A3 of the 24-well plate.
5. Place 10 drops of Iron (III) chloride, FeCl3 into well A4 of the 24-well plate.
6. Place 10 drops of Copper (II) sulfate, Cu SO4 into well A5 of the 24-well plate.
7. Take the metal solids from your LabPaq
8. Use your tweezers to pick up and carefully insert the piece of magnesium into the sodium sulfate. Record your observations.
9. Carefully insert a piece of zinc into the magnesium sulfate. Record your observations.
10. Carefully insert a piece of lead into the zinc nitrate. Record your observations.
11. Carefully insert the lead into the iron (III) chloride. Record your observations.
12. In the same way carefully insert the iron into the