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
Oxidation-Reduction Series Essay Example
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 copper (II) sulfate. Record your observations. 13. Place a paper towel over the drain of your sink and pour the contents of the well plate through it. 14. Throw the paper towel and metal pieces in the trash
15. . Rinse the well plate and your drain with running water. Data Table Oxidation-reduction table (below)
Reactions Mg in Na2SO4 → sodium is stronger than magnesium, turned iron duller, little amount of bubbles Zn in MgSO4 → Little to no reaction Pb in Zn(NO3)2 → Less of an reaction than the Fecl3, but kind of changed color Pb in FeCl3 → Changed its color made it slimy green Fe in CuSO4 → Completely stripped nail, turned the tip orange
Conclusion I was surprised at the reaction that Iron had because although I did expect some reaction I didn’t expect that much of a reaction. I was also surprise at how subtle Pb and Zinc and Pb in Iron could be, I feel that this lab was beneficial in honing our observational skills as some of the reactions where harder to see at first, such as Zinc in Magnesium.
Potential Sources of Error I feel that human error could destroy this experiment because if you don’t clean the well you wouldn’t get an accurate response from the metal. I also thought that the pipet was hard to get the accurate amount of drops out (10). Also the time could play a role, if you recorded your observation at different points of the reduction series you might get different answers. Questions
A. Based on your observations make an activity series of the metals used. List them in such a way that the most active metal is on the left and the least active metal is on the right. Remember, sodium and copper are metals, too.
1. Iron, Zinc, Lead, Magnesium B. Suppose you inserted a piece of copper into a solution of nickel chloride and observed no reaction. Then if you inserted a piece of iron into the solution of nickel chloride a nickel deposit formed on the bottom of the well in the well plate. Where does nickel fit into your activity series?
1. Iron, Nickel, Zinc, Lead, Magnesium C. Suppose you inserted a piece of an unknown metal into a solution of zinc (II) nitrate and observed no reaction. Then if you inserted the unknown piece of the metal into the solution of iron (III) chloride a deposit formed on the bottom of the well in the well plate. Where does the unknown metal fit into your activity series?
1. The unknown metal would fit in between Zinc and Lead. For the reaction (Fe (s) + NiCl2 (aq) à 2 Ni (s) + Fe Cl2 (aq) identify: 1. The oxidation number of Ni (s) =0 2. The oxidation number of Fe in the FeCl2 (aq)=+2 3. The oxidation number of Cl in the FeCl2 (aq)=-1 4. The oxidation number of Fe (s)=0 5. The oxidation number of Ni in the NiCl2 (aq) =+2 6. The oxidation number of Cl in the NiCl2 (aq) =-1 7. The element that is oxidized and the element that is reduced: Iron(Fe) was oxidized and the Ni was reduced. 8. The oxidizing agent and the reducing agent Iron was the reducing agent and the Ni was the oxidizing agent.