Date of experiment: 04/02/12 Date of report: 04/03/12
Title: Oxidation – Reduction Activity Series
Purpose: To determine relative oxidizing and reducing strengths of a series of metals and ions. Oxidation and reduction reaction occur simultaneously side by side. A reduction reaction occurs only if an oxidation reaction occurs and vise-versa. Electrons are given in oxidation while in reduction electrons are gained. Oxidizing agent is a chemical substance which has a large tendency to gain electrons, while reducing agent is a chemical substance causes other substances to be reduced and itself oxidized. Procedure: For this lab was used metals and substances provided in the lab oxidation-reduction pack, and some extra materials. Using the well-plate and the correct amount of drops and the right metal on the right well, to see the reaction with each different substance. Observations: This experiment required some time and patience to analyze the results. For each well required a different substance and a different metal to be inserted in the well. Different metals react faster or slower depending the substance they are added. Na2SO3 with magnesium bubbles appeared around the magnesium piece and we could predict a reaction. MgSO4 with zinc No reaction observed Zn (NO3)2 with lead and aluminum No reaction observed FeCl3 with lead and aluminum reacts with foil, the piece dissolves in the solution and the lead piece seems to be oxidizing. CuSO4 with iron the screw seems to be oxidized quickly; it changes the color of it to a pinkish tone.
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. Aluminum [continues]
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