Electrochemistry and the Nerst Equation
1. Measure the electrical potential of a zinc/iron battery cell at differing concentrations.
2. Construct an electrolytic cell.
1. Prepare a 100mL of 0.1M Iron (II) Sulfate solution in a 150mL beaker and place the iron strip in the solution.
2. Prepare a 100mL of 0.1M Zinc Sulfate solution in a 150mL beaker and place the zinc strip in the solution.
3. Connect the beakers using the plastic bridge, which must be filled with a KCl solution and cotton wads on either end.
4. Place the positive end of the electrical meter on the Iron strip, and the negative on the end of the Zinc strip. The meter must be set to the 2V scale.
5. Record and then repeat the voltaic cell procedure using a solution of diluted Iron (II) Sulfate: 1mL of 0.1M.
1. Prepare a solution in a 150mL beaker containing 10g NaCl and 100mL of distilled water.
2. Insert two copper wire conductors.
3. Connect the power supply to the conductors.
4. Add phenolphthalein to the solution.
5. Set the power supply to two Volts.
6. Observe reaction.
Data Tables for Electrochemistry Lab:
|Cells:||Standard Zinc/Iron||Non-Standard Z/I|
|Electric Potential (V)||0.490||0.323|
|Percent Error %|