hydrogen peroxide and potassium permanganate experiment

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Elephant Toothpaste – Two Ways to Make It

Elephant toothpaste is a chemical reaction that makes a volcano of foam when soapy water traps gases from the rapid decomposition of hydrogen peroxide. There are two easy methods for making elephant toothpaste. One makes a giant mountain of foam, while the other produces a smaller effect but is safe enough for kids to touch. The dramatic reaction uses strong peroxide and potassium iodide, while the kid-friendly version uses dilute peroxide and replaces potassium iodide with yeast. Here are instructions for both methods and a look at the chemistry involved.

Why Is It Called Elephant Toothpaste?

First, you may wonder why the reaction has the name “elephant toothpaste.” It’s because the thick column of foam escaping a tube looks like toothpaste big enough for an elephant to use. Also, it’s a lot easier and more descriptive than calling the reaction “rapid decomposition of peroxide”. After all, the point of elephant toothpaste is engaging people in the wonder of science. Even if someone doesn’t understand the chemistry, the project is fun and entertaining.

How to Make Giant Elephant Toothpaste

When you see videos of the world’s largest elephant toothpaste, you’re viewing the classic version of the demonstration.

This version uses concentrated hydrogen peroxide, potassium iodide or sodium iodide, liquid dishwashing detergent, water, and (if desired) food coloring:

• 30% hydrogen peroxide (H 2 O 2 )
• Potassium iodide (KI) or sodium iodide (NaI)
• Liquid dishwashing detergent
• Food coloring (optional)
• Large graduated cylinder or Erlenmeyer flask
• Tray or tarp to catch the foam

The chemicals are available online, although it’s easier to just pick up the peroxide at a beauty supply store. Choose any tall container for the demonstration, but use glass and not plastic because the reaction generates heat.

Start by putting on proper safety gear, including safety goggles and gloves.

• First, prepare a saturated solution of potassium iodide or sodium iodide in water. In a beaker, dissolve crystals of either chemical in about 120 ml (4 ounces) of water. Continue stirring in the solid until no more dissolves. It takes about a tablespoon of the dry chemical. But, measurements are not critical here. Set aside the solution for now.
• Set the cylinder or flask in a tray or on a tarp. Pour about 60 ml (2 ounces) of 30% hydrogen peroxide into the glass tube. Add a squirt (about 5 ml) of dishwashing liquid to the tube. If you want colored foam, add a few drops of food coloring. Swirl the liquids to mix them. Here again, exact measurements are unnecessary.
• When you’re ready for the reaction, pour about 15 ml (one tablespoon) of the iodide solution and stand back. Foam forms within seconds and rapidly escapes the tube.
• After the reaction ends, wash the contents of the tray and tube down the drain with water.

Kid-Friendly Elephant Toothpaste

The classic chemistry demonstration is for chemistry educators, but the kid-friendly elephant toothpaste is safe enough for parents and children to perform and touch. Also, this version uses easy-to-find ingredients.

• 3% household peroxide
• 1-2 packet of dry yeast
• Food coloring
• Empty plastic soft drink bottle
• Cookie sheet or pan to catch the foam (optional)

It’s not necessary to don safety gear for this reaction and it’s fine to use either a plastic or glass container. Just make sure the bottle has a narrow opening because this channels the foam and improves the effect.

Don’t worry about measuring ingredients precisely.

• Pour about a cup of 3% hydrogen peroxide into an empty bottle. If the bottle opening is small, use a funnel.
• Add a couple of squirts of dishwashing liquid and a few drops of food coloring to the bottle. Swish the liquid around to mix it.
• In a separate container, mix together yeast with enough warm water that the liquid is easy to pour. A paper cup is a great container choice because you can pinch its rim and make pouring the yeast mixture easier. Wait a couple of minutes before proceeding so the yeast has a chance to activate.
• When you’re ready, place the bottle on a cookie sheet or pan and pour yeast mixture into the bottle
• Clean-up using warm, soapy water.

Is Elephant Toothpaste Safe to Touch?

You can handle the ingredients and the foam from the kid-friendly elephant toothpaste project. However, don’t touch either the ingredients or the foam from the classic giant elephant toothpaste. This is because the peroxide is concentrated enough to cause a chemical burn, while the giant toothpaste is hot enough to cause a thermal burn.

How Elephant Toothpaste Works

The basis for the elephant toothpaste display is the rapid decomposition of hydrogen peroxide (H 2 O 2 ). Hydrogen peroxide naturally decomposes into water and oxygen gas according to this chemical reaction:

2H 2 O 2 (l) → 2H 2 O(l) + O 2 (g)

In a decomposition reaction , a larger molecule breaks down into two or more smaller molecules. The normally slow progression of the reaction is why a bottle of peroxide has a shelf life . Exposure to light accelerates the decomposition, which is why peroxide comes in opaque containers.

Either potassium iodide or the enzyme catalase (found in yeast) acts as a catalyst for the reaction. In other words, either of these chemicals supercharges the reaction so it proceeds very quickly. Breaking chemical bonds in peroxide releases a lot of energy. Only a fraction of this energy goes back into forming chemical bonds making water and oxygen. What this means is that elephant toothpaste is an exothermic reaction or one that releases heat. How hot the reaction gets depends on how much peroxide you start with and how efficiently the catalyst speeds up the reaction. So, the classic version of the project gets hot enough to steam. The kid-friendly version of elephant toothpaste gets warm, but not hot enough to cause a burn.

Producing gas isn’t enough to make a foamy volcano. Adding liquid soap or dishwashing detergent to the mixture traps the gas bubbles. Normally, the reaction doesn’t have much color. Using food coloring makes the foam more interesting. Depending on your choice of colors, it also makes the foam resemble toothpaste.

• Dirren, Glen; Gilbert, George; Juergens, Frederick; Page, Philip; Ramette, Richard; Schreiner, Rodney; Scott, Earle; Testen, May; Williams, Lloyd. (1983).  Chemical Demonstrations: A Handbook for Teachers of Chemistry. Vol. 1.  University of Wisconsin Press. Madison, Wisconsin. doi:10.1021/ed062pA31.2
• “ Elephant’s Toothpaste .”  University of Utah Chemistry Demonstrations . University of Utah.
• Hernando, Franco; Laperuta, Santiago; Kuijl, Jeanine Van; Laurin, Nihuel; Sacks, Federico; Ciolino, Andrés (2017). “Elephant Toothpaste”.  Journal of Chemical Education . 94 (7): 907–910. doi: 10.1021/acs.jchemed.7b00040
• IUPAC (1997). “Chemical decomposition”. Compendium of Chemical Terminology (the “Gold Book”) (2nd ed.). Oxford: Blackwell Scientific Publications. ISBN 0-9678550-9-8. doi: 10.1351/goldbook

Related Posts

Elephant Toothpaste Chemistry Demonstration

A fun science experiment that looks like pachyderm dental care

Jasper White / Getty Images

• Ph.D., Biomedical Sciences, University of Tennessee at Knoxville
• B.A., Physics and Mathematics, Hastings College

The dramatic elephant toothpaste chemistry demonstration produces copious amounts of steaming foam that looks like the kind of toothpaste an elephant might use to brush his tusks. To see how to set up this demo and learn the science of the reaction behind it, read on.

Elephant Toothpaste Materials

The chemical reaction in this demonstration is between the hydrogen peroxide and a solution of potassium iodide and dishwashing detergent that captures the gases to make bubbles.

• 50-100 ml of 30% hydrogen peroxide (H 2 O 2 ) solution (Note: This hydrogen peroxide solution is much more concentrated than the kind you'd generally purchase at a pharmacy. You can find 30% peroxide at a beauty supply store, science supply store, or online.)
• Saturated potassium iodide (KI) solution
• Liquid dishwashing detergent
• Food coloring
• 500 mL graduated cylinder
• Splint (optional)

For this demonstration, it's advisable to wear disposable gloves and safety glasses. Since oxygen is involved in this reaction, do not perform this demonstration near an open flame. Also, the reaction is exothermic , producing a fair amount of heat, so do not lean over the graduated cylinder when the solutions are mixed. Leave your gloves on following the demonstration to aid with cleanup. The solution and foam may be rinsed down the drain with water.

Elephant Toothpaste Procedure

• Put on gloves and safety glasses. The iodine from the reaction may stain surfaces so you might want to cover your workspace with an open garbage bag or a layer of paper towels.
• Pour ~50 mL of 30% hydrogen peroxide solution into the graduated cylinder.
• Squirt in a little dishwashing detergent and swirl it around.
• You can place 5-10 drops of food coloring along the wall of the cylinder to make the foam resemble striped toothpaste.
• Add ~10 mL of potassium iodide solution. Do not lean over the cylinder when you do this, as the reaction is very vigorous and you may get splashed or possibly burned by steam.
• You may touch a glowing splint to the foam to relight it, indicating the presence of oxygen.

Variations of the Elephant Toothpaste Demonstration

• You can add 5 grams of starch to the hydrogen peroxide. When the potassium iodide is added, the resulting foam will have light and dark patches from the reaction of some of the starch to form triiodide.
• You can use yeast instead of potassium iodide. Foam is produced more slowly, but you can add a fluorescent dye to this reaction to produce elephant toothpaste that will glow very brightly under a black light .
• You can color the demonstration and make it into an Elephant Toothpaste Christmas Tree for the holidays.
• There's also a kid-friendly version of the elephant toothpaste demo that's safe for little hands.

Elephant Toothpaste Chemistry

The overall equation for this reaction is:

2 H 2 O 2 (aq) → 2 H 2 O(l) + O 2 (g)

However, the decomposition of the hydrogen peroxide into water and oxygen is catalyzed by the iodide ion.

H 2 O 2 (aq) + I - (aq) → OI - (aq) + H 2 O(l)

H 2 O 2 (aq) + OI - (aq) → I - (aq) + H 2 O(l) + O 2 (g)

The dishwashing detergent captures the oxygen as bubbles. Food coloring can color the foam. The heat from this exothermic reaction is such that the foam may steam. If the demonstration is performed using a plastic bottle, you can expect a slight distortion of the bottle due to the heat.

Elephant Toothpaste Experiment Fast Facts

• Materials: 30% hydrogen peroxide, concentrated potassium iodide solution or a packet of dry yeast, liquid dishwashing detergent, food coloring (optional), starch (optional)
• Concepts Illustrated: This demonstration illustrates exothermic reactions, chemical changes, catalysis, and decomposition reactions. Usually, the demo is performed less to discuss the chemistry and more to raise interest in chemistry. It is one of the easiest and most dramatic chemistry demonstrations available.
• Time Required: The reaction is instantaneous. Set-up can be completed in under half an hour.
• Level: The demonstration is suitable for all age groups, particularly to raise interest in science and chemical reactions. Because the hydrogen peroxide is a strong oxidizer and because heat is generated by the reaction, the demonstration is best performed by an experienced science teacher. It should not be performed by unsupervised children.
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YouTubers are battling for the world record of foam with the elephant toothpaste experiment. Here's how to make a smaller, kid-safe version at home.

• Nick Uhas and David Dobrik stunned the internet with their successful attempt at breaking the world record for largest amount of foam produced via the elephant toothpaste experiment.
• Before their attempt, science YouTubers Mark Rober and ScienceBob did their own record-breaking stunt in Rober's backyard pool, using a different catalyst.
• If you want to replicate their attempt on a smaller scale at home, ScienceBob put together instructions on his website that are cheap and easy to follow.
• Uhas told Insider that the experiment is safe and environmentally friendly, as long as you use the right materials and follow some basic safety precautions.
• Visit Insider's homepage for more stories.

Science YouTubers are engaging in a bit of a " foam arms race " this week with gargantuan versions of the elephant toothpaste experiment.

Nick Uhas and David Dobrik claimed the world record for the most foam produced via the demonstration, which combines hydrogen peroxide, dish soap, food coloring, and potassium iodide to result in a massive volcano of foam.

Before the pair pulled off their successful attempt, YouTubers Mark Rober and ScienceBob did a version with yeast in Rober's backyard swimming pool that overflowed .

If you're inspired and want to make a significantly smaller version of elephant toothpaste at home, you can. ScienceBob put some cheap, easy-to-follow instructions on his website , and the experiment is kid-friendly as long as you follow some basic safety precautions. With the right clean-up, it's environmentally sound, too.

You only need a few materials to make a foam volcano.

To start, you just need to gather a few materials.

To make ScienceBob's at-home version, you'll need: 

• 1/2 cup of liquid hydrogen peroxide
• 10 drops of liquid food coloring
• 1 tablespoon of liquid dish soap
• 1 packet of dry yeast
• A 16-ounce plastic soda or water bottle OR a bucket that size
• A small cup to hold your yeast and at least 3 tablespoons of warm water
• Plastic gloves and safety googles

Optionally, you can also put a plastic tarp down to catch all the foam.

The reaction starts with liquid hydrogen peroxide, and you can use different strengths for more or less foam.

The YouTubers use 20-Volume hydrogen peroxide, which is a 6% solution that's stronger than the kind found in pharmacies or drug stores. It creates more foam than the standard 3% solution, and can be used to lighten hair, so many beauty supply stores carry it.

However, the 6% solution can irritate skin and eyes, so if you're using it, you should wear gloves and safety goggles. You also wouldn't want to touch the foam afterward, because there may be un-reacted peroxide in it. If you use the 3% solution found in pharmacies, you can touch the foam afterward.

ScienceBob's instructions call for 1/2 cup of hydrogen peroxide, and he recommends using a 16-ounce plastic soda bottle or water bottle to mix the solution at home. A container with a funneled top makes the foam shoot out in a steady stream, whereas a container like a bucket causes it to spill over the sides.

If using a funneled top, you should definitely do the experiment outside, because the stream can reach several feet in the air.

Either way, it's a good idea to do the experiment outside, since it involves so much spillover. But if you want to do it inside, be sure to line the area with plastic.

Add food coloring and dish soap to the hydrogen peroxide mixture to create colored foam.

ScienceBob suggests 10 drops of food coloring and about 1 tablespoon of liquid dish soap to make the foam colorful. You can also do the demonstration without dish soap, and the reaction will still take place, but it won't create the bubbly foam.

You should swish the ingredients around in the container to create a mixture.

If you use dye, it can stain ceilings to the point where it's almost impossible to clean. Uhas told Insider that he tried the experiment inside Dobrik's house, and the stained ceiling now rejects new coats of paint because the iodide seeps through.

In a separate cup, combine dry yeast and warm water for the at-home catalyst, instead of the potassium iodide that Uhas used.

The potassium iodide in Uhas and Dobrik's experiment is a more powerful catalyst that produces an explosion effect, as opposed to the rising foam that filled Rober's pool. Uhas told Insider that the iodide isn't toxic, and is actually edible, but it's used for medical purposes and is more expensive than yeast.

ScienceBob recommends using a tablespoon of dry yeast, or one packet. He combines it with three or more tablespoons of warm water in a separate small container, and mixes it for about 30 seconds, until the mixture has the consistency of "melted ice cream." You can add more water to reach that consistency.

Uhas and Rober used huge contraptions that required multiple people to pour the catalyst into the peroxide, but you can just use a funnel at home.

As both videos exhibited, all you need to do to jump-start the chemical reaction is combine the catalyst with the peroxide mixture. That means you can just use a funnel or pour the dissolved yeast into the hydrogen peroxide.

The reaction starts almost immediately, so step back or point the container away from yourself to avoid getting splashed with foam. Another important thing to note is that the reaction is exothermic, meaning that the foam will be hot.

You should be mindful not to hold on to the container where the reaction is taking place unless you're wearing gloves or another covering that will shield you from heat. You also shouldn't touch the foam right away, but you can touch it if you used a 3% solution after it's cooled down.

Uhas told Insider that the foam is "self-cleaning."

After the reaction concludes, you're left with a lot of soapy foam. If you use potassium iodide as the catalyst, Uhas told Insider that it becomes iodine, which leaves a powerful stain – another reason to do the elephant toothpaste experiment outside and away from your house or any sort of concrete or plaster.

If you're using the yeast, it shouldn't stain as badly, but you should still exhibit caution. Fortunately, the foam is just water, soap, and oxygen, and will release oxygen on its own until you're left with soapy, colored water.

You can sop that up and recycle the plastic you put down, like Uhas and Dobrik did. The remaining liquid is also drain-safe. If you have enough materials on hand, you can try different variations of the experiment like Rober did in his video — or see how much foam you can produce by increasing the quantity of materials.

See the full instructions from ScienceBob here »

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In association with Nuffield Foundation

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Entertain your students with a series of loud bangs as evolved oxygen increases the rate of burning

In this exothermic reaction, a series of loud, but harmless, bangs are heard as the oxygen that is evolved increases the rate of burning.

Demonstration

Potassium manganate(VII) powder is sprinkled on to a burning mixture of hydrogen peroxide solution and ethanol . In the exothermic reaction which follows, a series of loud, but harmless, bangs are heard as the oxygen that is evolved increases the rate of burning.

Lesson organisation

The demonstration is spectacularly noisy, producing sharp, crackling bursts of noise and flame which sometimes seem to build rhythmically. A trial run is recommended for those trying it for the first time.

The demonstration can also be rather messy as splashes of the mixture in the basin are ejected. It is advisable to protect the bench area around the heat resistant mat with some non-flammable, washable material to aid clearing up afterwards.

The demonstration takes about 3 minutes.

• Eye protection
• Safety screens
• Evaporating dish (10 cm diameter)
• Heat-resistant mats
• Wooden splint
• Potassium manganate, 0.5g
• Hydrogen peroxide, 20-vol, 30 cm 3
• Ethanol, 20 cm 3

Health, safety and technical notes

• Read our standard health & safety guidance
• Wear eye protection. Use safety screens throughout to protect the audience and the demonstrator.  (See CLEAPSS Supplementary Risk Assessment SRA05 on the CLEAPSS website). 
• Potassium manganate(VII), KMnO 4 (s), (OXIDISING, HARMFUL, DANGEROUS FOR THE ENVIRONMENT) - see CLEAPSS Hazcard HC081 .
• Hydrogen peroxide solution, H 2 O 2 (aq), (IRRITANT) - see CLEAPSS Hazcard HC050 and CLEAPSS Recipe Book.
• Ethanol (IDA, Industrial Denatured Alcohol), C 2 H 5 OH(l), (HIGHLY FLAMMABLE, HARMFUL) - see CLEAPSS Hazcard HC040a . 
• Put the evaporating dish on a large heat resistant mat (or use several smaller mats) to protect the bench. Place a safety screen between the mat and the audience.
• Add 30 cm 3  of 20-volume hydrogen peroxide solution and 20 cm 3  of ethanol to the dish.
• Light the mixture with a burning splint. The ethanol vapour should ignite and burn with an almost invisible flame.
• Now, at arm’s length, sprinkle from a spatula or wooden splint about 0.5 g of potassium manganate(VII) crystals into the dish. Do not sprinkle directly from the bottle.
• Immediately there will be a series of loud bangs, giving the effect of a volley of gunshot and the flames will leap up. The noise will subside into crackling, which can last for up to a minute.
• When the noisy reaction is over, extinguish the burning ethanol (if still alight) by placing a heat resistant mat or tile over the evaporating basin. Do not repeat the demonstration unless you have first rinsed the dish with plenty of water. It can be very difficult to see the ethanol flame under some lighting conditions.
• A residue of brown, solid manganese dioxide will be seen in the evaporating dish – and possibly in the area immediately surrounding it.

Teaching notes

Coarse potassium manganate(VII) crystals give fewer but louder bangs, while fine crystals give more but smaller ones.

It is strongly recommended  not  to use more concentrated solutions of hydrogen peroxide or to alter the other quantities in any other way.

The reaction between manganate(VII) ions and hydrogen peroxide is as follows:

2MnO 4 – (aq) + 3H 2 O 2 (aq) → 2MnO 2 (s) + 2H 2 O(l) + 3O 2 (g) + 2OH – (aq)

The localized evolution of oxygen accelerates the burning of the ethanol, and this produces pockets of evolved energy which manifest themselves in the mini-explosions produced.

Additional information

This Practical Chemistry resource was developed by the Nuffield Foundation and the Royal Society of Chemistry.

© Nuffield Foundation and the Royal Society of Chemistry

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Specification

• A reaction or process that releases heat energy is described as exothermic.

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Amaze a Science Class With Elephant Toothpaste

Introduction: Amaze a Science Class With Elephant Toothpaste

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Reaction of Potassium Permanganate and Hydrogen Peroxide solution

• Thread starter neilparker62
• Start date Aug 22, 2020
• Tags Hydrogen Hydrogen peroxide Reaction
• Aug 22, 2020
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You happened to choose a very complicated reaction (paywalled Inorg. Chem. article): https://pubs.acs.org/doi/pdfplus/10.1021/ic00224a030 Typically, for elementary reactions (where the stoichiometry reflects the reaction mechanism faithfully), reactions are either unimolecular, in which case the rate is linear in the concentration, or bimolecular, in which case the rate is quadratic. (NB--higher order elementary reactions are exceedingly rare, a reflection of the fact that correctly-oriented triple (or more) collisions of molecules are exceedingly rare.) In the case of permanganate reacting with hydrogen peroxide: $$2MnO_4^-+5H_2O_2+6H^+\rightarrow2Mn^{2+}+5O_2+8H_2O$$ the stoichiometry does not reflect the reaction mechanism faithfully. The article above states that the reaction proceeds in three phases: 1) a fast initial phase which is roughly bimolecular (##Rate \propto [MnO_4^-][H_2O_2]##), 2) a slow induction phase that sees a buildup of ##Mn^{2+}##, and 3) an autocatalytic phase, where the manganous ion catalyzes the reduction of the permanganate via a hypothesized Mn(III) pathway, producing more manganous ion, etc., etc. The article goes into much more detail than this, but suffice it to say that the answer to your question isn't straightforward.  

A PF Planet

TeethWhitener said: You happened to choose a very complicated reaction (paywalled Inorg. Chem. article): https://pubs.acs.org/doi/pdfplus/10.1021/ic00224a030 Typically, for elementary reactions (where the stoichiometry reflects the reaction mechanism faithfully), reactions are either unimolecular, in which case the rate is linear in the concentration, or bimolecular, in which case the rate is quadratic. (NB--higher order elementary reactions are exceedingly rare, a reflection of the fact that correctly-oriented triple (or more) collisions of molecules are exceedingly rare.) In the case of permanganate reacting with hydrogen peroxide: $$2MnO_4^-+5H_2O_2+6H^+\rightarrow2Mn^{2+}+5O_2+8H_2O$$ the stoichiometry does not reflect the reaction mechanism faithfully. The article above states that the reaction proceeds in three phases: 1) a fast initial phase which is roughly bimolecular (##Rate \propto [MnO_4^-][H_2O_2]##), 2) a slow induction phase that sees a buildup of ##Mn^{2+}##, and 3) an autocatalytic phase, where the manganous ion catalyzes the reduction of the permanganate via a hypothesized Mn(III) pathway, producing more manganous ion, etc., etc. The article goes into much more detail than this, but suffice it to say that the answer to your question isn't straightforward.

Certainly if the permanganate is dilute enough, it might all get used up before the necessary complexes build up to a level where autocatalysis starts to become a significant factor. And yes, the proper course of action is to keep as many of the reagents at as constant a concentration as possible in order to accurately assess kinetics. This can be tough to do if you’re adding multiple solutions together (since adding one solution dilutes the other solution).  

• Aug 24, 2020

TeethWhitener said: Certainly if the permanganate is dilute enough, it might all get used up before the necessary complexes build up to a level where autocatalysis starts to become a significant factor. And yes, the proper course of action is to keep as many of the reagents at as constant a concentration as possible in order to accurately assess kinetics. This can be tough to do if you’re adding multiple solutions together (since adding one solution dilutes the other solution).

neilparker62 said: The concentration formula is essentially grams or moles/volume. So as not to change either peroxide or acid concentration the experiment used 10ml peroxide , 10 ml vinegar and 10 ml of various concentrations of Permanganate. That is the experiment was carried out at constant volume.

neilparker62 said: Is there a general formula which relates reaction time to volume and/or dilution factor under the above conditions ?

• Aug 25, 2020

TeethWhitener said: This sounds fine. I’m assuming, since this is permanganate and it’s a school experiment, that the basic procedure is 1) mix reagents, 2) monitor the permanganate absorbance using UV-Vis spectrometry. Correct me if I’m wrong.

TeethWhitener said: The reaction will always depend on concentration, but as I mentioned earlier, the dependence isn’t simple for this reaction. The reaction shouldn’t depend on absolute volume (unless you’re using a container with dimensions comparable to the molecules themselves). Also, keep in mind that (assuming I was right about the procedure) you’re only seeing the portion of the reaction where the purple Mn(VII) color fades. That’s fine, but it just means that you’re not monitoring the concentrations of the other species during the course of the reaction. So if you’re trying to judge the entire reaction from Mn(VII) to Mn(II), you’ll be missing a lot of information about the intermediate steps.

neilparker62 said: Appreciate from what you've said that the reaction is complex. But if we keep n moles of all reagents exactly the same, then exactly the same reaction path should occur whatever the dilution. So then the time difference (for different dilution factors) will be due to an increased 'average time' for successful collisions. Well that was my thinking anyway - don't know if it makes any sense ?

FAQ: Reaction of Potassium Permanganate and Hydrogen Peroxide solution

1. what is the chemical equation for the reaction of potassium permanganate and hydrogen peroxide solution.

The chemical equation for this reaction is KMnO 4 + H 2 O 2 → K 2 MnO 4 + H 2 O + O 2 . This means that one molecule of Potassium Permanganate (KMnO 4 ) reacts with one molecule of Hydrogen Peroxide (H 2 O 2 ) to produce one molecule of Potassium Manganate (K 2 MnO 4 ), one molecule of water (H 2 O), and one molecule of oxygen gas (O 2 ).

2. What is the purpose of this reaction?

The reaction of Potassium Permanganate and Hydrogen Peroxide is often used as a test for the presence of certain compounds, such as alcohols and aldehydes. It can also be used as a way to produce oxygen gas in a laboratory setting.

3. How does the reaction of Potassium Permanganate and Hydrogen Peroxide occur?

This reaction is a redox (oxidation-reduction) reaction, meaning that the oxidation state of at least one element changes. In this case, the manganese (Mn) in Potassium Permanganate is reduced from a +7 oxidation state to a +6 oxidation state, while the oxygen (O) in Hydrogen Peroxide is oxidized from a -1 oxidation state to a 0 oxidation state.

4. What are the physical properties of the products of this reaction?

Potassium Manganate is a dark green solid, water is a clear liquid, and oxygen gas is a colorless gas. These products can be easily identified and separated based on their physical properties.

5. Are there any safety precautions to take when conducting this reaction?

Yes, both Potassium Permanganate and Hydrogen Peroxide are strong oxidizing agents and can be hazardous if not handled properly. It is important to wear protective gear, such as gloves and goggles, and to work in a well-ventilated area. It is also important to properly dispose of any leftover chemicals after the reaction is complete.

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Reaction of hydrogen peroxide with acetic acid and potassium permanganate

I conducted an experiment where I mixed hydrogen peroxide $\ce{H2O2}$ , acetic acid $\ce{CH3COOH}$ and potassium permanganate $\ce{KMnO4}$ under vigorous stirring. The reaction hasn't stopped after 15 min and the colour is cycling between pink and colourless whenever I add more potassium permanganate.

What reaction is going on? I think despite a medium created with weak acid, acidified potassium permanganate is a much stronger oxidising agent and it should react with a lot of peroxide rather than the opposite.

But hydrogen peroxide and acetic acid react to form peracetic acid $\ce{CH3CO3H}$ (PAA) . I don’t know if PAA reacts with potassium permanganate or something entirely different occurs.

I am concerned about the reaction and products. The mix smells strongly of acetic acid and most of the permanganate is still in there. Could it be the manganese oxide formed in the reaction being oxidised? Well first of all no bubbles the limiting reagent of the reaction was hydrogen peroxide and I used aqueous potassium permanganate. And by most of the permanganate was still there I meant I added half a teaspoon of permanganate and I used less than 1% acetic acid and 6.5 percent peroxide. I was trying an acid catalysed reaction between and oxidiser permanganate and and reductant peroxide. When I drained the solution (by excess of water)a most of the amount added of permanganate was in the solution with manganese oxide indication it reacted with the peroxide.

• organic-chemistry
• inorganic-chemistry
• aqueous-solution
• 3 $\begingroup$ Try to better explain what you have done. In which order have you mixed the three components ? And how much of each ? How many times ? Did you use solid permanganate or its solution ? In this case which concentration ? The same question for hydrogen peroxide : have you used $30$% or $3$% hydrogen peroxide ? Did you use pure acetic acid, or an aqueous solution ? Which concentration ? What is the meaning of "most of the permanganate was still in there" ? Please explain thoroughly all what you have done ! $\endgroup$ –  Maurice Commented Sep 19, 2022 at 12:16
• 2 $\begingroup$ Please be careful, peroxide and permanganate are strong oxidizers. Acetic acid is potential fuel. But what you may be doing is oxidizing the peroxide (with permanganate). Did you see bubbles? $\endgroup$ –  Robert DiGiovanni Commented Sep 19, 2022 at 15:25
• 1 $\begingroup$ The limiting reagent was not defined. Acetic acid is a suitable solvent for permanganate or chromate oxidations at low temperatures but still should be used very carefully. This idea of mixing peroxides with a strong oxidzer and a possible reductant sounds like potential bomb making. This person is playing with chemicals not "conducting an experiment" $\endgroup$ –  jimchmst Commented Sep 19, 2022 at 17:59
• 1 $\begingroup$ The Kinetics of the Acid-Catalyzed Formation of Peracetic Acid from Acetic Acid and Hydrogen Peroxide has been studied in details as early as 1965. $\endgroup$ –  Mathew Mahindaratne Commented Sep 19, 2022 at 19:20
• $\begingroup$ Well first of all no bubbles the limiting reagent of the reaction was hydrogen peroxide and I used aqueous potassium permanganate. And by most of the permanganate was still there I meant I added half a teaspoon of permanganate and I used less than 1% acetic acid and 6.5 percent peroxide. I was trying an acid catalysed reaction between and oxidiser permanganate and and reductant peroxide. When I drained the solution (by excess of water)a most of the amount added of permanganate was in the solution with manganese oxide indication it reacted with the peroxide. $\endgroup$ –  user127378 Commented Sep 20, 2022 at 13:09

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Carbon Sequestration by Potassium-Modified Bagasse Biochar in Manganese-Contaminated Sugarcane Field Soils

• Original Paper
• Published: 03 September 2024

Cite this article

• Yu Yang 1 , 2 ,
• Xuehui Liu 1 , 2 ,
• Haiping Luo 4 ,
• Lening Hu 1 , 2 ,
• Shuangli Li 5 &
• Hua Deng 1 , 2  

This study aims to investigate the transformation and carbon sequestration mechanisms of soil organic carbon in manganese-contaminated farmland. A 100-day constant temperature incubation experiment was conducted using potassium dihydrogen phosphate-modified bagasse biochar (BC-K) at concentrations of 0%, 0.5%, 2%, and 5%. The effects of BC-K on the mineralization of organic carbon and the changes in the physicochemical properties of manganese-contaminated soils were examined. The results demonstrated that applying 0.5%, 2%, and 5% BC-K to manganese-contaminated soils significantly reduced cumulative CO 2 emissions by 411.94 mg·kg − 1 , 47.33 mg·kg − 1 , and 105.24 mg·kg − 1 , respectively. The greatest reduction was observed with the 0.5% BC-K application compared to the control. The application of 2% and 5% BC-K to manganese-contaminated soil increased SOC by 121.50–165.23%, DOC by 24.46–30.05%, and MBC by 5.41 to 6.19 times. However, ROC decreased by 29.83–30.04%. In addition, the application of BC-K in manganese-contaminated soil can increase soil AP, AK, CEC, pH, and catalase. The application of BC-K can effectively reduce CO 2 emissions in manganese-contaminated farmland soil while significantly increasing soil organic carbon content and improving its physical and chemical properties. The findings of this study offer a scientific foundation for developing carbon sequestration and soil nutrient management strategies in manganese-contaminated farmland soils. These insights are crucial for enhancing soil environmental quality.

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This work was supported by the Guangxi Natural Science Foundation project of China (2022GXNSFAA035555); the Key Laboratory of Ecology of Rare and Endangered Species and Environmental Protection (Guangxi Normal University), Ministry of Education, China (ERESEP2021Z13); Funded by the Research Fund Program of Guangdong Provincial Key Laboratory of Environmental Pollution Control and Remediation Technology (2023K0025).

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Key Laboratory of Ecology of Rare and Endangered Species and Environmental Protection, Ministry of Education, Guangxi Normal University & College of Environment and Resources, Guangxi Normal University, Guilin, 541004, China

Yu Yang, Xuehui Liu, Lening Hu & Hua Deng

Guangxi Key Laboratory of Environmental Processes and Remediation in Ecologically Fragile Regions, Guangxi Normal University, Guilin, 541004, China

College of Civil Engineering and Architecture, Guilin University of Technology, Guilin, 541004, China

Guangdong Provincial Key Laboratory of Environmental Pollution Control and Remediation Technology, School of Environmental Science and Engineering, Sun Yat-sen University, Guangzhou, 510006, China

Haiping Luo

Shenzhen Institute of Technology, Shenzhen, 518116, China

Shuangli Li

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Yu Yang: software, writing original draft preparation, and data curation. Xuehui Liu: data curation and supervision. Ke Li and Haiping Luo: supervision. Lening Hu, SHuangli Li, and Hua Deng: supervised the experiment project and approved the final version. All authors have read and agreed to the published version of the manuscript.

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Yang, Y., Liu, X., Li, K. et al. Carbon Sequestration by Potassium-Modified Bagasse Biochar in Manganese-Contaminated Sugarcane Field Soils. J Soil Sci Plant Nutr (2024). https://doi.org/10.1007/s42729-024-02000-8

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Received : 11 March 2024

Accepted : 26 August 2024

Published : 03 September 2024

DOI : https://doi.org/10.1007/s42729-024-02000-8

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