ELECTROCHEMICAL CELLSPurpose: In this experiment, several half cells will be prepared and connected to find the voltages generated. Additionally, the concentration will be changed in one of the solutions to see how this affects the cell potential. Third, the electrical potential of a cell containing silver and silver chloride will be measured. Finally, a cell containing copper (II) and ammonia will be built. The potential and the Nernst equation will be used to calculate the formation constant of the tetraamminorame(II) complex ion. This experiment uses a microscale technique. Procedure:1. Gather materials and wear eye protection.2. Prepare a test cell to measure the voltage of the copper and zinc half cells.3. Place approximately 2 ml of 1.0 M zinc nitrate solution into one of the center wells of a 24-well plate.4. Place approximately 2 ml of 1.0 M copper(II) nitrate into an adjacent well. Polish small strips of zinc and copper metal and place the metal in the appropriate well containing the ion solution of that metal.5. Take a small strip of filter paper soaked in potassium nitration solution and drape it over the wells so that one end is immersed in the solution in each well. This will act as a salt bridge.6. Use a voltmeter to measure the potential difference between the two half-cells.7. Connect the meter so that the voltage reading is positive.8. Use the most sensitive scale that is practical. Make note of which electrode is the anode and which is the cathode.9. When the voltmeter reads a positive voltage, the electrode connected to the positive terminal is the cathode and is being reduced. Oxidation occurs at the electrode connected to the negative terminal, the anode.10. Prepare half cells in other wells of 24-well plates.11. First make a diagram of the order of the solutions in the wells so that the different solutions are not confused.12. Pour a 1.0 M solution of each of the ions into different wells.13. Polish the metals with sandpaper or steel wool so that they are shiny and insert them into the wells that contain the metal ion itself.14. Use new strips of filter paper soaked in 1.0 M potassium nitrate as salt bridges.15. The zinc electrode will be designated as the standard electrode. Measure the potential difference between the zinc electrode and each of the other electrodes.16. Record the data.17. Measure the potential difference between at least six combinations of the various electrodes.18. Use the electrode potential table to predict the voltage and which half-cell will be the anode and which will be the cathode.