Determining the Charge of Iron ions

Copper sulfate reacts with copper (II) sulfate in solution forming solid copper. The purpose of this lab is to determine the charge on the iron atoms formed. The charge is a whole number and can be determined from the mass of copper formed if we are certain that copper is the excess reagent.

Materials

Iron filings Copper (II) sulfate pentahydrate crystals

Equipment

Analytical balance Triple beam balance burner

Beakers 250 mL Graduated cylinder 100 mL ring stand

Iron ring Wire gauze Goggles

Lab apron Oven Stirring Rod

Procedure

  1. Find and record the mass of a clean, dry, 100 mL beaker.
  2. Measure out approximately 2.2 g of iron filings on the analytical balance and record.
  3. Add enough CuSO4 · 5H2O to the 100 mL beaker to be certain that you have at least 3 times the moles of iron. Record the mass.
  4. Add approximately 50 mL of distilled water to the copper sulfate in the 100 mL beaker.
  5. Heat the copper sulfate crystals to just below the boiling point. DO NOT ALLOW THE LIQUID TO BOIL.
  6. Continue heating and stirring until all the crystals are dissolved. Turn of the gas.
  7. Slowly add the iron filings, small amounts at a time, to the hot copper sulfate solution. Continue stirring for 10 minutes as the reaction proceeds. Record your observations
  8. Decant the liquid into a 250 mL beaker
  9. Add 10 ml of distilled water to the solid and stir to wash of the solid. Let the solid settle and decant the liquid. Repeat the washing.
  10. Spread the solid out along the bottom and put in the oven to dry overnight.
  11. Find the mass of the beaker and the dry metal. Record.
  12. Repeat the procedure for a second sample.

Calculations.

  1. Find the moles of the reactants and the solid product.
  2. Use this to determine the charge of the iron ions in solution.
  3. Write a molecular equation, a complete ionic equation, and a net ionic equation for the reaction.
  4. Write the two half reactions.
  5. Identify the oxidizing and reducing agent, as well as the substance oxidized and the substance reduced.

Conclusion.

Summarize the results of this experiment and note any reasons for error.