Experiments with potassium permanganate at home. Entertaining experiences

Interesting chemical experiments can be carried out from improvised things that are usually stored at home in the medicine cabinet. In this article we will talk about experiments with potassium permanganate and hydrogen peroxide.

What is peroxide and potassium permanganate?

These two reagents can be bought in almost every pharmacy.

Hydrogen peroxide is the simplest peroxide with the formula H₂O₂. It is a colorless liquid with a faint odor that dissolves in water and some organic liquids. The substance is used in all areas of life: in medicine, beauty and industry.

Hydrogen peroxide is usually sold in glass or plastic jars with a dispenser, and this substance has a different concentration: from 1-6 to 98 percent. The hydrogen peroxide produced in tablets is called hydroperit (peroxide in a tablet is mixed with urea).

The same experiment can be repeated with hydroperit. To do this, crush the tablets into powder and prepare a highly concentrated solution by mixing hydroperite with warm water. However, in this case, the foam will turn out not so thick. The density of the foam and the intensity of the reaction depend on the soap used and the proportions, as well as on the concentration of peroxide (you can even use three percent, but instead of a snake you will see just a plentiful foam).

To make the experiment exciting, use food coloring and mix them with a soap-based product.

When manganese and hydrogen peroxide are mixed, abundant oxygen evolution begins. Only in this case it is released inside the detergent, thereby provoking an abundant release of foam.

Hydrogen peroxide itself decomposes into oxygen, and potassium permanganate is only a catalyst that accelerates the process.

Drop of blood and hydrogen peroxide

Also, oxygen from the peroxide is liberated liberally in contact with blood, so when treating wounds, you can see a rapid release of bubbles and hear hissing.

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Every day we take care of our children - we cook porridge in the morning and iron clothes. But after 20 years, they will remember not our domestic chores, but the moments spent together.

site collected 16 experiments that will tear off from the affairs of adults and captivate children. They do not need much time and some special preparation, and there will be a lot of pleasure. And then you can cook porridge. Together.

Solid liquid

You will need:

• starch
• plastic container
• food coloring, board, hammer and nails for additional experiments

Stir in a container of water and starch until a creamy consistency. The result is a “non-Newtonian" fluid. You can easily dip your fingers into it, but if you hit the surface with your fist, you will feel that it is hard. Put a board on the surface of the liquid, and you will easily hammer a nail, but it is worth drowning one corner of it in the liquid, as the board will easily sink to the bottom. If desired, “solid liquid” can be colored with food colors.

DIY kinetic sand

You will need:

• 4 tsp boric alcohol
• 2 tsp stationery glue
• 1 tsp dye
• 100 g of sand for chinchillas
• glass bowl

Pour all liquid ingredients into a bowl, add sand and mix thoroughly. Done, you can create!

Pharaoh snake

You will need:

• sand
• alcohol
• sugar
• matches
• plate for "snake"

Pour sand into a plate with a slide, soak it with alcohol, and on top put a mixture of sugar and soda. Set it on fire. "Snake" grows instantly!

Wire and Battery Train

You will need:

• a coil of thick copper wire (the more wire, the longer the "tunnel")
• 1 AA battery
• 2 round neodymium magnets suitable for the battery in diameter
• ordinary pen

Wind the wire around the handle to make a long spring. Fasten the magnets at both ends of the battery. Launch the train. He will ride by himself!

Candle swing

You will need:

• candle
• thick needle
• lighter
• two glasses
• pliers

Cut the lower end of the candle by a centimeter and a half to release the wick. Clamp the needle in the pliers and heat it with a lighter, and then pierce the candle in the middle. Put it on the edges of the two cups and set it on both sides. Swing lightly, and then the candle starts to rotate itself.

Paper towel rainbow

You will need:

• food colorings
• paper towels
• 5 glasses

Put the cups in a row and pour water into the 1st, 3rd and 5th. In the 1st and 5th, drip red food coloring, in the 3rd - yellow, in the 5th - blue. Fold 4 paper towels 4 times to make strips, and then bend them in half. Insert the ends into different cups - one between the 1st and 2nd cups, the second between the 2nd and 3rd, etc. After a couple of hours, you can enjoy the rainbow!

Elephant toothpaste

You will need:

• 3/4 cup water
• 1 tsp potassium permanganate
• 1 tbsp. l liquid soap
• hydrogen peroxide
• glass flask
• disposable gloves

Dissolve potassium permanganate in water, add liquid soap and pour the mixture into a glass flask. Carefully but quickly pour in peroxide. Rough foam spills up from the flask - a real elephant toothpaste!

Very slow ball

You will need:

• steel ball
• transparent plastic ball container of two halves
• liquid honey

Put a steel ball in a container, pour honey and run the entire structure from the slide. Hmm, what if you try with a shower gel?

Smoke rings

You will need:

• plastic bottle (0.5 l)
• balloon
• incense stick
• lighter
• scissors

Cut the bottom of the plastic bottle and half of the balloon. Slide the wide part of the ball over the cut of the bottle. Insert the wand into the bottle, cover its opening with your hand and wait for it to fill with smoke. Smoke rings by tapping your finger on the stretched ball.

Self-inflating Balls

You will need:

• 4 plastic bottles
• table vinegar
• 3 tbsp. l soda
• 3 balloons
• liquid food coloring

Cut the top off the plastic bottle, pull all the balls in turn on the hole, and pour a spoonful of soda into each ball through the resulting funnel. Pour vinegar on the bottoms of the bottles, drop the food coloring there and carefully, so that soda does not spill into the bottle, pull the balls into the holes. It remains to raise them - the soda will pour out, react with vinegar, and the balls are inflated themselves.

Acetic soda rocket

You will need:

• plastic bottle (2 l)
• 3 simple pencils
• 2 tbsp. l soda
• 200 ml of vinegar 9%
• wide tape
• wine cork
• paper towel

Make sure in advance that the cork fits snugly against the neck of the bottle. Use adhesive tape to stick the pencils to the top of the bottle so that it can stand. Pour vinegar into the bottle. Wrap soda tightly in a paper towel and tighten the ends carefully. Go outside, lower the package with soda into the bottle and plug it with a cork, pressing one end of the package to the neck. Turn the rocket over, put it on the ground and run! Take-off must be observed from 15–20 meters, no less.

Hello!

With this article I want to complete the "potassium permanganate" cycle and talk about several experiments that you can do yourself, show your children, for example, when you tell them about this wonderful substance.

The experiments with potassium permanganate, for the most part, are simple and do not require any exotic reagents. Let me remind you that I originally created my blog in order to try and publish on it such experiences that are easy to do at home.

I have already described almost all of these experiments in various articles; now I will collect them in a heap and generalize.

Acid discoloration

You will need:

• Potassium permanganate,
• Acetic essence
• Hydrogen peroxide 3%.

We make a pink solution of permanganate, add 2-3 tablespoons of vinegar to it, and then 3-4 tablespoons of peroxide. The solution gradually brightens.

The reactions that take place are based on the properties of permanganate to decolorize upon interaction with acids. Therefore, dirty things are advised to wipe with various acids.

Alkali discoloration

You will need:

• A pink solution of permanganate, as in the previous experiment,
• A concentrated solution of "Mole", that is, sodium hydroxide (what it is and how to make it).

We mix these two solutions and after a few minutes we observe how the color changes from pink to green. It is also, as in the previous experiment, associated with the chemical properties of potassium permanganate. In an alkaline environment (and a solution of sodium hydroxide is an alkali), manganese compounds have a green color.

Note a little off topic. If you want to learn more about what an acidic and alkaline environment is and how you can independently determine them at home, here are articles about home-made indicators.

Color change when interacting with components of tobacco smoke

One of my favorite experiences. We were shown it at the university on the subject of something like "Environmental Education", I don’t remember exactly.

I thought for a long time how to replace the instruments and utensils that are in the university laboratory, but which are not at home, and finally came up with. In my opinion, it turned out well and, most importantly, easily and visually.

Here are photographs of the potassium permanganate solution before and after interacting with the smoker's lungs:

The color change is due to the fact that tobacco smoke contains various substances: nitrogen oxides, pyridine, ammonia, aromatic amines, nicotine, tar (tobacco tar). They react with permanganate, changing its color.

Thermal decomposition of potassium permanganate

I do not really like this experiment. I feel bad about experiments with fire, flashes, etc., I can not help myself. 🙂

You will need:

• Potassium permanganate is dry,
• Pharmacy glycerin,
• Heat resistant stand.

Everything is described in detail here in this article. The general sense is to mix permanganate crystals with glycerin in the right proportions, and they will flare up.

Hydroperite decomposes under the influence of potassium permanganate

You will need:

• Hydroperite tablets.
• Potassium permanganate,
• Dishwashing liquid.

The experience is described in detail in this article, so I won’t repeat it. I can only say that it is simple and effective. You just need to work out, choose the right concentration - and you will get even more foam than you expected.

That's all for today. How do you like the experiences? Can you hold them yourself?

I wish you all a good chemistry!

See you in the next article!

Natalya Bryantseva

An interesting science of chemistry does not cease to amaze us with its interesting chemical reactions. You can conduct some chemical experiments at home yourself. Do you know how to make a lot of foam from a cup of liquid? In fact, this is very simple and informative.

With children, you can still try to do it.

To make foam, you will need:

• potassium permanganate - half a teaspoon,
• hydroperite tablets (20-30 pcs.),
• liquid soap - 30 ml.,
• hot water - 100 ml
• cones and hammer.

Chemical Experience for Children - Making Foam at Home

1. The first thing to do is beat the hydroperit tablets with a hammer. If you do not use a hammer, then in the normal form they will dissolve for a long time. Then pour the resulting powder with hot water (50 ml). Mix the solution. As a result, we get a 30% hydrogen peroxide solution.

3. In another vessel, it is necessary to make a solution of potassium permanganate in water, that is, potassium permanganate. You need to take potassium permanganate a little, literally on the tip of a teaspoon and dissolve in warm water (50 ml). Mix well.

4. Now we need to connect two liquids in the flask: Hydrogen peroxide with soap + potassium permanganate solution.

You will see a lot of foam appear instantly.

Such a process occurs because potassium permanganate, water and hydrogen peroxide interact with each other releasing a lot of oxygen. And the soap liquid added to them does not allow oxygen to “fly away”. Soap molecules envelop the released oxygen to form a thick foam.

A lot of foam. Chemical experience for children at home - Video:

  The same foam can be made from a solution of copper sulfate and hydroperite. But, in comparison with the experiment with potassium permanganate, the foam of copper sulfate has a more pronounced smell.

In order to make such a foam it is necessary:

1. mix liquid soap and 30% hydrogen peroxide.
2. Then mix ammonia with copper sulfate and get ammonium sulfate.
3. After mixing the two mixtures and observe the foaming.

This chemical reaction shows the spontaneous decomposition of hydrogen peroxide into water and oxygen. Through the action of catalysts, decomposition is faster. In this case, the catalyst produces copper ammonia, which is formed when ammonia is added to the solution of copper sulfate. Soaps with water and hydrogen peroxide do not allow oxygen to “leave”. Oxygen released in the form of bubbles is enveloped by soap molecules, and then rises. Bubbles form a foam in contact with each other. Due to the low water content, the foam does not settle for a long time.

To make the foam more beautiful and interesting, you can add dyes.

Why fruit knives turn black?!

Why fruit knives turn black

If you add a solution of iron salt to some fruit juice (a solution of iron salt can be easily obtained at home, if you drop in a copper sulfate for half an hour, for example, a nail or several buttons, clips), then the liquid will immediately darken. We will get a solution of weak ink. Fruits contain tannic acidwhich forms an ink with a salt of iron. In order to get a solution of iron salt at home, dip a nail in a solution of copper sulfate and wait ten minutes. Then drain the greenish solution. The resulting solution of iron sulfate (FeSO 4) can be used in the reactions.

Tea also contains tannic acid. A solution of iron salt added to a weak solution of tea, change the color of tea to black. That is why it is not recommended to brew tea in a metal teapot!

Chemical reactions with sodium chloride

Sometimes table salt is specially iodized, that is, sodium or potassium iodides are added to it. This is done because iodine is part of various enzymes in the body, and when it is deficient, the thyroid gland deteriorates.

   Solutions of copper sulfate with table salt (green)

Finding the supplement is easy enough. It is necessary to cook starch paste: dilute a quarter of a teaspoon of starch in a glass of cold water, heat to a boil, boil for five minutes and cool. A paste is much more sensitive to iodine than dry starch. Next, a third of a teaspoon of salt is dissolved in a teaspoon of water, a few drops of vinegar essence (or half a teaspoon of vinegar) are added to the resulting solution, half a teaspoon of hydrogen peroxide and after two to three minutes a few drops of paste. If the salt was iodized, then hydrogen peroxide will displace free iodine:

2I - + H 2 O 2 + 2CH 3 COOH → I 2 + 2H 2 O + 2CH 3 COO -,

which will starch blue. (The experiment will not work if KClO 3 was used instead of KI for iodination of the salt). Can hold experience with copper sulphate and table salt. None of the above reactions will occur here. But the reaction is beautiful ... When mixing vitriol and salt, observe the formation of a beautiful green solution of sodium tetrachlorocuprate Na 2

Entertaining experiments with potassium permanganate:

Dissolve several crystals of potassium permanganate in water and wait a while. You will notice that the raspberry color of the solution (due to the presence of permanganate ions in the solution) will gradually become paler, and then completely disappear, on the walls of the vessel a brown coating of manganese oxide (IV) is formed:

4КMnО 4 + 2Н 2 О → 4MnO 2 + 4КОН + 3О 2

The dishes in which you conducted the experiment, it is easy to clean from plaque with a solution of citric or oxalic acid. These substances reduce manganese to an oxidation state of +2 and convert it to water-soluble complex compounds. In dark flasks, potassium permanganate solutions can persist for years. Many believe that potassium permanganate is highly soluble in water. In fact, the solubility of this salt at room temperature (20 ° C) is only 6.4 g per 100 g of water. However, the solution has such an intense color that it seems concentrated.

If the potassium permanganate is heated to 200 0 C, then potassium permanganate will turn into a dark green potassium manganate (K 2 MnO 4). At the same time, a large amount of pure oxygen is released, which can be collected and used for other chemical reactions. Particularly quickly, the potassium permanganate solution deteriorates (decomposes) in the presence of reducing agents. For example, the reducing agent is ethyl alcohol C 2 H 5 OH. The reaction of potassium permanganate with alcohol  proceeds as follows:

2KMnO 4 + 3C 2 H 5 OH → 2KOH + 2MnO 2 + 3CH 3 CHO + 2H 2 O.

Detergent from potassium permanganate:

In order to get a home-made “detergent”, you need to mix potassium permanganate with acid. Of course, not with everyone. Some acids may oxidize themselves; in particular, if you take hydrochloric acid, toxic chlorine will be released from it:

2KMnO 4 + 16HCl → 2MnCl 2 + 5Cl 2 + 2KCl + 8H 2 O.

So it is often obtained in the laboratory. Therefore, for our purposes, it is better to use diluted (about 5 percent) sulfuric acid. In extreme cases, it can be replaced with diluted acetic acid - table vinegar. Take about 50 ml (a quarter cup) of the acid solution, add 1-2 g of potassium permanganate (at the tip of the knife) and mix thoroughly with a wooden stick. Then we wash it under a stream of water and tie a piece of foam sponge to the end. With this “brush”, quickly, but gently spread the oxidizing mixture over the contaminated area of \u200b\u200bthe sink. Soon, the liquid will begin to change color to dark cherry, and then to brown. So, the oxidation reaction is in full swing. There are a few points to make here. It is necessary to work very carefully so that the mixture does not get on hands and clothes; it would be nice to put on an oilcloth apron. And you should not hesitate, since the oxidizing mixture is very caustic and eventually “eats” even foam rubber. After use, the foam "brush" must be immersed in a pre-prepared jar of water, rinse and discard. During such cleaning of the sink, an unpleasant odor may appear, emitted by the products of incomplete oxidation of organic pollutants on faience and acetic acid itself, so the room should be ventilated. After 15-20 minutes we rinse the browned mixture with a stream of water. And although the shell will appear in a terrible form - all in brown spots, you should not worry: the product of the reduction of potassium permanganate - manganese dioxide MnO 2 is easy to remove, restoring insoluble manganese (IV) to a well-soluble manganese salt in water.
   But when potassium permanganate interacts with concentrated sulfuric acid, manganese oxide (VII) Mn 2 O 7 is formed - an oily dark green liquid. This is the only liquid metal oxide under normal conditions (mp \u003d 5.9 ° C). It is very unstable and explodes easily with slight heating (t decom \u003d 55 ° C) or with shaking. Mn 2 O 7 is an even stronger oxidizing agent than KMnO 4. Contact with it ignites many organic substances, such as ethyl alcohol. This, by the way, is one of the ways to light an alcohol lamp without having matches!

Interesting experiments with hydrogen peroxide

Hydrogen peroxide can be both an oxidizing agent (this property is widely known) and a reducing agent! In the latter case, it reacts with oxidizing substances:
H 2 O 2 -2e → 2H + + O 2. Manganese dioxide is just such a substance. Chemists call such reactions "reductive decomposition of hydrogen peroxide." Instead of pharmaceutical peroxide, you can use tablets of hydroperite - a compound of hydrogen peroxide with urea of \u200b\u200bthe composition CO (NH 2) 2 H 2 O 2. This is not a chemical compound since there are no chemical bonds between the urea and hydrogen peroxide molecules; H 2 O 2 molecules are, as it were, included in long narrow channels in urea crystals and cannot leave it until the substance is dissolved in water. Therefore, such compounds are called channel inclusion compounds. One tablet of hydroperite corresponds to 15 ml (tablespoon) of a 3% solution of H 2 O 2. To obtain a 1 percent solution of H 2 O 2 take two tablets of hydroperite and 100 ml of water. Using manganese dioxide as an oxidizing agent of hydrogen peroxide, you need to know one subtlety. MnO 2 is a good catalyst for the decomposition of H 2 O 2 into water and oxygen:

2H 2 O 2 → 2H 2 O + O 2.

And if you simply treat the sink with a solution of H 2 O 2, then it will instantly “boil”, releasing oxygen, and the brown coating will remain, because the catalyst should not be consumed during the reaction. To avoid the catalytic decomposition of H 2 O 2, an acidic environment is needed. Vinegar is also suitable here. Strongly dilute the pharmacy peroxide with water, add a little vinegar and wipe the sink with this mixture. A real miracle will happen: a dirty brown surface will sparkle with whiteness and become like new. A miracle happened in full accordance with the reaction

MnO 2 + H 2 O 2 + 2H + → Mn 2+ + 2H 2 O + O 2.

It remains only to wash off the well-soluble salt of manganese with a stream of water. In the same way, you can try to clean a contaminated aluminum pan: in the presence of strong oxidizing agents, a strong protective film of oxide is formed on the surface of this metal, which will protect it from dissolution in acid. But cleaning the enameled products (pots, bathtubs) with this method is not worth it: the acidic environment slowly destroys the enamel. To remove MnO 2 plaque, one can also use aqueous solutions of organic acids: oxalic, citric, tartaric, etc. Moreover, they do not need to be specially acidified - the acids themselves create a sufficiently acidic environment in the aqueous solution.

Entertaining experiences

Gold in the flask

Of course, gold is not real, but the experience is beautiful! For the chemical reaction, we need a soluble lead salt (suitable is blue acid (CH 3 COO) 2 Pb - a salt formed by dissolving lead in acetic acid) and an iodine salt (for example, potassium iodide KI). Lead acetate can also be obtained at home by dropping a piece of lead in acetic acid. Potassium iodide is sometimes used to pickle electronic circuit boards.

Potassium iodide and acetic acid in lead are two transparent liquids that do not differ in appearance from water.

Let's start the reaction: add a solution of lead acetic acid to a solution of potassium iodide. By combining two transparent liquids, we observe the formation of a golden yellow precipitate - lead iodide PbI 2 - spectacularly! The reaction proceeds as follows:

(CH 3 COO) 2 Pb + KI → CH 3 COOK + PbI 2

Entertaining experiences with clerical glue

Clerical glue is nothing more than liquid glue or its chemical name "sodium silicate" Na 2 SiO 3 It can also be said - it is a sodium salt of silicic acid. If you add a solution of acetic acid to the silicate glue, insoluble silicic acid - hydrated silicon oxide - will precipitate.

Na 2 SiO 3 + 2CH 3 COOH → 2CH 3 COONa + H 2 SiO 3.

The resulting precipitate of H 2 SiO 3 can be dried in the oven and diluted with a diluted solution of water-soluble ink. As a result, ink will settle on the surface of silicon oxide, and they cannot be washed off. This phenomenon is called adsorption (from Latin ad - “on” and sorbeo - “absorb”)

Another beautiful entertaining experience with liquid glass. We need copper sulfate CuSO 4, nickel sulfate NiS0 4, iron chloride FeCl 3. Let's make a chemical aquarium. In a high glass jar with silicate glue diluted in half with water, diluted aqueous solutions of nickel sulfate and iron chloride are poured simultaneously from two glasses. The silicate “algae” of yellow-green color gradually grows in the bank, which, interwoven, fall from top to bottom. Now add dropwise a solution of copper sulfate to the jar, populate the aquarium with "starfish". Algae growth is the result of crystallization of hydroxides and silicates of iron, copper and nickel, which are formed as a result of metabolic reactions.

Interesting experiments with iodine

Add to the iodine tincture a few drops of hydrogen peroxide H 2 O 2 and mix. After a while, a black glistening precipitate will precipitate from the solution. it crystalline iodine - poorly soluble in water substance. Iodine precipitates faster if the solution is slightly warmed up with hot water. Peroxide is needed in order to oxidize potassium iodide KI contained in the tincture (it is added in order to increase the solubility of iodine). Another poor ability of iodine in water is related to its ability to extract from water with liquids consisting of non-polar molecules (oil, gasoline, etc.). In a teaspoon of water, add a few drops of sunflower oil. Stir and see that the oil does not mix with water. If now two or three drops of iodine tincture are added there and shaken vigorously, the oil layer will turn dark brown, and the water layer will become pale yellow, i.e. most of the iodine will turn into oil.

Iodine is a very corrosive substance. To verify this, put a few drops of iodine tincture on a metal surface. After some time, the liquid will discolor, and a stain will remain on the metal surface. The metal reacted with iodine to form a salt - iodide. One of the methods for inscribing metal is based on this property of iodine.

Color entertaining experience with ammonia

By the substance "ammonia" we mean an aqueous solution of ammonia (ammonia). In fact, ammonia is a gas, when dissolved in water, which forms a new class of chemical compounds - the "base". It is with reason that we will experiment. A spectacular experiment can be done with a solution of ammonia (ammonia). Ammonia forms a colored compound with copper ions. Take a bronze or copper coin with a dark coating and fill it with ammonia. Immediately or after a few minutes, the solution will turn blue. This, under the action of air oxygen, copper formed a complex compound - ammonia:

2Cu + 8NH 3 + 3H 2 O + O 2 → 2 (OH)

Entertaining experiments: slaking lime

Slaking lime is a chemical reaction between calcium oxide (CaO - quicklime) and water. It proceeds as follows: