In this lesson students will review oxidation states, half-reactions, balancing reactions and understand how to complete calculations and perform a redox titration.
High School (AP Chemistry)
This lesson will help prepare your students to meet the performance expectations in the following standards:
- 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 representation to support the claim that atoms, and therefore mass, are conserved during a chemical reaction.
- Scientific and Engineering Practices:
- Using Mathematics and Computational Thinking
- Analyzing and Interpreting Data
- Engaging in Argument from Evidence
AP Chemistry Curriculum Framework
This lesson supports the following unit, topics and learning objectives:
- Unit 4: Chemical Reactions
- Topic 4.6: Introduction to Titration
- SPQ-4.B: Identify the equivalence point in a titration based on the amounts of the titrant and analyte, assuming the titration reaction goes to completion.
- Topic 4.7: Types of Chemical Reactions
- TRA-2.A: Identify a reaction as acid-base, oxidation-reduction, or precipitation.
- Topic 4.9: Oxidation-Reduction (Redox)Reactions
- TRA-2.C: Represent a balanced redox reaction equation using half-reactions.
- Topic 4.6: Introduction to Titration
By the end of this lesson, students should be able to
- Understand oxidation and reduction reactions
- Assign oxidation states
- Be able to balance redox reactions for charge and mass
- Understand redox titration
- Perform redox titration calculations
- Perform a redox titration experiment
This lesson supports students’ understanding of
- Redox Reaction
- Oxidation and reduction process
- Half Reactions
- Stoichiometric calculations
- End point
Teacher Preparation: 60 minutes
Lesson: 120-150 minutes (approximate times)
- Demo-15 minutes
- Inquiry-45 minutes
- Lab-60 minutes
- Demonstration: Chemical Chameleon
- Potassium Permanganate (2mg) dissolved in 500 mL distilled water
- Sodium Hydroxide (10 g)
- Sugar (6g)
- 3 Erlenmeyer flasks
- Lab: Analysis of Hydrogen Peroxide (listed as enough for each lab group)
- Distilled water (100 ml)
- Commercial Hydrogen Peroxide (3%) (3.0 mL)
- 0.025 M Potassium Permanganate (75 mL)
- 6 M Sulfuric Acid (15mL)
- Titration set up, ring stand with buret clamp and 50 mL buret
- 1.00 mL Volumetric pipet
- 125 mL Erlenmeyer flask
- 100 mL beaker
- 10 mL graduated cylinder
- 250 mL waste beaker
- Always wear safety goggles when handling chemicals in the lab.
- Students should wash their hands thoroughly before leaving the lab.
- When students complete the lab, instruct them how to clean up their materials and dispose of any chemicals.
- When working with acids, if any solution gets on students’ skin, they should immediately alert you and thoroughly flush their skin with water.
- When diluting acids, always add acid to water.
- Students should wear proper safety gear during chemistry demonstrations. Safety goggles and lab apron are required.
- The demonstration results may be flushed down the sink with plenty of water as the permanganate is reduced to manganese dioxide.
- Sulfuric acid solution is severely corrosive to eyes, skin, and other body tissues.
- Potassium permanganate solution is a skin and eye irritant and a strong stain-it will stain skin and clothing.
- This lesson assumes that the students have some background knowledge of redox reactions although the Guided Inquiry activity reviews important information. Students should have prior experience with acid-base titrations before completing this lesson.
- Introduction/Engagement: To review oxidation states with students, begin the lesson with a quick demo. Students are not expected to know the color changes for manganese oxidation states. Always practice demonstrations before performing for students. Check out this video if you have never done this demonstration.
Chameleon” Demo Procedure (5-10 minutes): Various Colors of Manganese Oxidation
- Create two different solutions to be used during the demonstration. (prep time: 10-15 minutes)
- Solution A: dissolve 2 mg KMnO 4 with 500 mL of distilled water in an Erlenmeyer flask.
- Solution B: warm (do NOT allow to come to a boil) 500 mL of water on hot plate in an Erlenmeyer Flask , add 10g NaOH and 6g of sugar and stir to dissolve. Allow the solution to cool before performing the experiment.
- In an empty Erlenmeyer add about half of the sodium hydroxide/sugar solution. Then add a small amount of the potassium permanganate solution, start with 10-20ml. Swirl the solution and watch the color change as the permanganate ion is reduced. Play around with the amounts and swirling to change the speed of the color change.
- The color changes are due to the oxidation state changes of the permanganate ion. The students do not need to understand the chemistry involved in the color change.
- Tell students which reactions are taking place for each color change and have them determine the oxidation state of the manganese.
permanganate ion appears purple but soon reduces to the hypomanganate ion which
- Purple: MnO4- + e- → MnO4-2
- Blue: Due to gradual colour transition from MnO4- (purple) toMnO4-2 (green)
- Green: MnO4-2
- The hypomanganate reduces to manganese dioxide which is a yellowish color
- Orange/Yellow: MnO4-2 + 2H2O + 2e- → MnO2 + 4OH-
Redox titration guided inquiry (30-40 minutes)
- For the guided inquiry activity, randomly divide students into teams of 2-4. Students should work through this activity together and divide the work among the members as noted in the activity.
- After the groups have finished, discuss the answers and be certain all questions have been addressed.
Analysis of Hydrogen Peroxide with Potassium Permanganate
- The lab activity should be finished in one 50 minute period with students working in pairs.
- Students should have performed an acid/base titration prior to this lab so that they understand the titration process and outcome.
- If materials are not available, there is also a virtual lab activity at Learn Chemistry (Royal Society of Chemistry) which is free for teachers and students.
- Discuss pre-lab questions prior to allowing students to participate in the activity.
- It is important that they understand how to observe the endpoint. The endpoint should be a very faint pink color. Use white paper under the flask to help determine the endpoint. The color should remain at least 30 seconds. If the color is not faint pink, discard this sample.
- Students should have practice balancing redox reactions in acidic environments prior to the lab. Try this free animated practice balancer.
- The teacher should prepare all solutions prior to the lab period.
|6 M sulfuric acid||It is preferable that you purchase 6M rather than concentrated 17.8 M due to safety hazards. If you need to dilute the concentrated you will need a minimum of 15mL of acid per group. Dilute 5.05 mL of concentrated 17.8 M sulfuric acid per 9.94 mL of distilled water you need. Remember always slowly add acid to water. This is a highly exothermic reaction.|
If you need to create the
0.025 M solution you will need 75 mL per group. Dissolve 0.30 g of solid KMnO
in each 75mL of distilled water you need.
Note: Potassium Permanganate should not be poured in a drain, follow Flinn Disposal Method #12a. If you do not have a Flinn Catalog/Reference Manual they are free and can be ordered here.
For the Student
Download all documents for this lesson, including the teacher guide, from the "Downloads box" at the top of the page.