Teacher Notes

Oxidation–Reduction Titrations

Laboratory Kit for AP® Chemistry

Materials Included In Kit

Ferrous ammonium sulfate, Fe(NH4)2(SO4)2•6H2O, 50 g
Manganese sulfate, MnSO4•H2O, 1.0 M, 100 mL
Oxalic acid, H2C2O4, 0.25 M, 100 mL
Potassium permanganate, KMnO4, 0.10 M, 500 mL
Sulfuric acid, H2SO4, 6 M, 1 L

Additional Materials Required

Beakers, 100-mL, 36
Burets, 50-mL, 12
Erlenmeyer flask, 250-mL, 36
Graduated cylinders, 10-mL, 12
Hot plates, 6
Ring stands and buret clamps, 12
Thermometers, 12
Volumetric pipets, 10-mL, 12
Volumetric pipets, 25-mL, 12
Wash bottles, 12

Prelab Preparation

Fe2+ standard solution, 0.100 M (Make fresh day of laboratory.)
To prepare 1 liter of 0.100 M Fe2+

  1. Weigh out 39.210 g of Fe(NH4)2(SO4)2•6H2O on an analytical balance and transfer to a clean 1-L volumetric flask.
  2. Fill the flask with approximately 700 mL of deionized water.
  3. Cap and mix until the solid is completely dissolved.
  4. Fill to mark with deionized water. Cap and mix thoroughly.
Oxalic acid solution, approximately 0.025 M
To prepare 1 liter of solution
  1. Using a clean graduated cylinder, transfer 100 mL of 0.25 M oxalic acid solution to a clean 1-L volumetric flask.
  2. Fill the flask to mark with deionized water.
  3. Cap and mix thoroughly.
Potassium permanganate solution, 0.020 M
To prepare 1 liter of solution
  1. Using a clean graduated cylinder, transfer 200 mL of 0.10 M potassium permanganate solution to a clean 1-L volumetric flask.
  2. Fill to mark with deionized water.
  3. Cap and mix thoroughly.
  4. Approximately 1 liter of 0.020 M potassium permanganate solution is needed for 12 groups of students.

Safety Precautions

Sulfuric acid (6 M) is corrosive to eyes, skin, and other tissue; always add acid to water, never the reverse. Potassium permanganate solution may be a skin irritant. The oxalic acid solution is a skin and eye irritant; it is moderately toxic by ingestion. The manganese sulfate solution is a body tissue irritant. Wear chemical splash goggles and chemical-resistant gloves and apron. Have students wash their hands thoroughly with soap and water before leaving the laboratory. Please consult current Safety Data Sheets for additional safety information.

Disposal

Please consult your current Flinn Scientific Catalog/Reference Manual for general guidelines and specific procedures, and review all federal, state and local regulations that may apply, before proceeding. The potassium permanganate solution may be disposed of according to Flinn Suggested Disposal Method #12a. The Part 1 and 2 titration solutions and the manganous sulfate solution may be disposed of according to Flinn Suggested Disposal Method #27f. The 6 M sulfuric acid solution may be disposed of according to Flinn Suggested Disposal Method #24b. The oxalic acid and its solution may be disposed of according to Flinn Suggested Disposal Method #24a. The ferrous ammonium sulfate may be disposed of according to Flinn Suggested Disposal Method #26a; its solution by #26b.

Lab Hints

  • The actual experimental work for this lab typically takes two 45-minute lab periods.
  • The titration lab teaches students how to use volumetric glassware and encourages them to develop proper laboratory techniques. Review and demonstrate these titration techniques.
  • Students can expect very precise results (to 3 significant figures) that are relatively easy to obtain.
  • If no volumetric pipets are available, a separate buret can be used. Be sure students clean this buret between uses.

Teacher Tips

  • Have students approximate the amount of MnO4 solution needed to titrate the iron solution in Part 1 before they titrate. The approximate molarity for the MnO4 solution can be given as between 0.015 M and 0.025 M.
  • Quantitative analysis represents a nearly invisible application of chemistry in daily life. To illustrate this, ask students how they would react if they could not trust the water they drink or medicines they take had been tested to assure their quality and safety.

Further Extensions

AP Chemistry Standards
This lab fulfills the requirement for the College Board recommended AP Experiment #8: Determination of Concentration by Oxidation–Reduction Titration. In addition, this lab provides the recommended familiarity with the process of titration.

Correlation to Next Generation Science Standards (NGSS)

Science & Engineering Practices

Asking questions and defining problems
Developing and using models
Planning and carrying out investigations
Analyzing and interpreting data
Using mathematics and computational thinking
Engaging in argument from evidence

Disciplinary Core Ideas

HS-PS1.A: Structure and Properties of Matter
HS-PS1.B: Chemical Reactions

Crosscutting Concepts

Patterns
Cause and effect
Scale, proportion, and quantity
Systems and system models
Energy and matter
Stability and change

Performance Expectations

HS-PS1-1. Use the periodic table as a model to predict the relative properties of elements based on the patterns of electrons in the outermost energy level of atoms.
HS-PS1-2. Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.
HS-PS1-7. Use mathematical representations to support the claim that atoms, and therefore mass, are conserved during a chemical reaction.

Answers to Prelab Questions

  1. Write the balanced net ionic equation for the reaction between MnO4 ions and H2C2O4 in acid solution. 
    First, write out each half-reaction. 
    {12972_Pre-Lab_Equation_8}
    Next, balance the electrons, then add the half-reactions. 
    {12972_Pre-Lab_Equation_9}
  2. How many moles of Fe2+ ions can be oxidized by 0.043 moles of MnO4 ions? 

    From the balanced oxidation–reduction reaction, five moles of Fe2+ ions are oxidized by one mole of MnO4 ions. Therefore, the moles of Fe2+ ions oxidized are
     
    {12972_Pre-Lab_Equation_10}
  3. 1.630 g of iron ore is dissolved in an acidic solution. This solution is titrated to a pink endpoint with 27.15 mL of a 0.020 M KMnO4 solution.
    1. How many moles of MnO4 ions were consumed?
      {12972_Pre-Lab_Equation_11}
    2. How many moles of Fe2+ were in the iron ore sample?
      {12972_Pre-Lab_Equation_12}
    3. What is the percent of iron in the iron ore sample?
      {12972_Pre-Lab Equation_13}

Sample Data

Part 1
Molarity of Fe2+0.100 M 

{12972_Data_Table_1}

Part 2
Molarity of MnO4- solution: 0.0206 M
{12972_Data_Table_2}

Molarity of H2C2O4 solution: 0.0260 M

Answers to Questions

  1. From the Part 1 standardization data, calculate the molarity of the MnO4 solution for each trial. Average the values and enter the average in the Part 2 Data Table.
    {12972_Answers_Equation_14}
  2. From the Part 2 titration data, calculate the molarity of the H2C2O4 solution for each trial. Average the values and enter the average in the Part 2 Data Table.

    The balanced reaction has 5 moles of H2C2O4(aq) reacting with 2 moles of MnO4(aq). At the equivalence point.
    {12972_Answers_Equation_15}
    The molarity of the oxalic acid solution is equal to:
    {12972_Answers_Equation_16}
  3. How many moles of Fe2+ ions and MnO4 ions were titrated in each Part 2 trial?
    {12972_Answers_Equation_17}
  4. How many moles of oxalic acid, H2C2O4 were titrated in each Part 2 trial?
    {12972_Answers_Equation_18}

Student Pages

Oxidation–Reduction Titrations

Introduction

A common task in analytical chemistry is the determination of the amount of a substance present in a sample or product. If the product contains a substance that can be oxidized, then it is possible to determine the number of moles of that substance by titrating the sample with a solution of a strong oxidizing agent. In this lab, an oxidizing solution will be standardized and then use to determine the number of moles of oxalic acid, a reducing agent.

Concepts

  • Oxidation–reduction reaction
  • Titration
  • Half-reaction
  • Equivalence point

Background

Oxidation–reduction reactions occur by electron transfer. The balanced chemical reaction can be written as the combination of two half-reactions, representing the oxidation reaction and the reduction reaction, respectively.

For example: If solid iron is placed in a solution of gold(III) ions, the gold(III) ions are reduced to solid gold and the iron oxidized to iron(III) ions, according to the following half-reactions:

{12972_Background_Reaction_1}

In this experiment, potassium permanganate, KMnO4, is used as the oxidizing agent. In an acidic solution, the MnO4 ion is reduced from Mn(VII) to Mn(II) according to the following half-reaction:
{12972_Background_Half-Reaction_2}

In Part 1, a solution of KMnO4 is standardized by titration with a solution containing a known concentration of iron(II) ions, (Fe2+).
In the corresponding oxidation half-reaction, the Fe2+ ion is oxidized to Fe3+:
{12972_Background_Half-Reaction_3}

Combining half-reactions 2 and 3 and balancing the number of electrons transferred gives the overall reaction equation:
{12972_Background_Reaction_4}

The balanced equation shows that 5 moles of Fe2+ are required to react with 1 mole of MnO4.

For this redox titration, the equivalence point occurs when the exact number of moles of Fe2+ ions has been added to react completely with all the MnO4 ions in solution. At this point:
{12972_Background_Equation_1}

If the volume and molarity of the Fe2+ solution are known, then:
{12972_Background_Equation_2}

Rearranging Equation 2 yields the equation for the concentration of the potassium permanganate solution.
{12972_Background_Equation_7}

The indicator for this titration is the MnO4 ion itself. The MnO4 ion is purple in solution. At the endpoint of the titration, the solution changes from light pink to colorless.

In Part 2, the concentration of an oxalic acid solution is determined by titration with the permanganate solution standardized in Part 1. In this case, the endpoint occurs when the pink color of the MnO4 ion persists. The half-reaction for the oxidation of oxalic acid is:
{12972_Background_Half-Reaction_5}

The oxidation state of carbon changes from (+3) in H2C2O4 to (+4) in H2CO3.

Experiment Overview

The purpose of this lab is to standardize a solution of potassium permanganate by redox titration with a standard solution of iron(II) ions. A solution of oxalic acid is then titrated with the permanganate solution to determine the exact concentration of oxalic acid.

Materials

Ferrous ammonium sulfate, Fe(NH4)2SO4•6H2O, 0.100 M, 50 mL
Manganese sulfate, MnSO4•H2O, 1.0 M, 5 mL
Oxalic acid solution, H2C2O4, 60 mL
Potassium permanganate, KMnO4, ≈0.02 M, 100 mL
Sulfuric acid, H2SO4, 6 M, 50 mL
Water, distilled or deionized
Beakers, 100-mL,3
Buret, 50-mL
Buret clamp
Erlenmeyer flasks, 250-mL, 3
Graduated cylinder, 10-mL
Hot plate
Ring stand
Thermometer
Volumetric pipet, 10-mL
Volumetric pipet, 25-mL
Wash bottle

Prelab Questions

  1. Write the balanced net ionic equation for the reaction between MnO4 ions and H2C2O4 in acid solution.
  2. How many moles of Fe2+ ions can be oxidized by 0.043 moles of MnO4 ions?
  3. 1.630 g of iron ore is dissolved in an acidic solution. This solution is titrated to a pink endpoint with 27.15 mL of a 0.020 M KMnO4 solution.
    1. How many moles of MnO4 ions were consumed?
    2. How many moles of Fe2+ were in the iron ore sample?
    3. What is the percent of iron in the iron ore sample?

Safety Precautions

Sulfuric acid (6 M) is corrosive to eyes, skin, and other tissue; always add acid to water, never the reverse. Potassium permanganate solution may be a skin irritant. The oxalic acid solution is a skin and eye irritant; it is moderately toxic by ingestion. The manganese sulfate solution is a body tissue irritant. Wear chemical splash goggles and chemical-resistant gloves and apron. Wash hands thoroughly with soap and water before leaving the laboratory.

Procedure

Part 1. Standardization of a Potassium Permanganate Solution

  1. Obtain approximately 80 mL of the potassium permanganate solution in a 100-mL beaker. Obtain 50 mL of the 0.100 M ferrous ammonium sulfate solution in another 100-mL beaker. Label both beakers.
  2. Set up a clean, 50-mL buret in the ring stand and buret clamp.
  3. Rinse the buret with approximately 10 mL of distilled or deionized water and then with two 5 mL portions of the MnO4– solution (potassium permanganate solution, KMnO4).
  4. Close the stopcock and fill the buret to above the zero mark with MnO4 solution.
  5. Open the stopcock to allow any air bubbles to escape from the tip. Close the stopcock when the liquid level is between the 0- and 10-mL marks.
  6. Record the precise level of the solution in the buret in the Part 1 Data Table. This is the initial volume of the MnO4 solution. (See Figure 1 for reading buret level.)
    {12972_Procedure_Figure_1}
  7. With the volumetric pipet, transfer 10 mL of the 0.100 M Fe2+ solution to a clean 250-mL Erlenmeyer flask. Record this volume in the Part 1 Data Table.
  8. Measure out 10 mL of the 6 M H2SO4 into a clean 10-mL graduated cylinder and add this to the Erlenmeyer flask. Swirl to mix.
  9. Position the flask under the buret so that the tip of the buret is within the flask but at least 2 cm above the liquid surface.
  10. Titrate the ferrous ammonium sulfate solution with the MnO4 solution until the first trace of pink color persists for 30 seconds. Remember to swirl the flask and to rinse the walls of the flask with distilled water before the endpoint is reached.
  11. Record final buret reading as the final volume of the MnO4 solution in the Part 1 Data Table.
  12. Repeat the standardization titration two more times.
Part 2. Determination of Concentration of an Oxalic Acid Solution
  1. Obtain approximately 60 mL of the oxalic acid solution in a clean 100-mL beaker.
  2. With a 25-mL volumetric pipet, transfer 25 mL samples of the oxalic acid solution to each of two clean 250-mL Erlenmeyer flasks. Record the volume in the Part 2 Data Table.
  3. Add 5 drops of the 1.0 M MnSO4 solution to each flask. (The Mn2+ ion acts as a catalyst for the reaction.)
  4. Measure out 10 mL of 6 M H2SO4 into a graduated cylinder and add this amount to each of the 250-mL Erlenmeyer flasks. Add 20 mL of distilled water to each flask and swirl.
  5. Warm the first flask to about 85 °C on the hot plate.
  6. Immediately titrate this solution with the standardized MnO4 solution from Part 1. Record both the initial and final buret readings in the Part 2 Data Table.
  7. Repeat steps 5 and 6 with the second flask.
  8. Your instructor will provide disposal instructions.

Student Worksheet PDF

12972_Student1.pdf

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