Where to buy sulfuric acid? Points of sale and tips. Livejournal Where to get acid

Dissolution of sulfuric anhydride (sulfur trioxide) in water. And to obtain anhydride, sulfur dioxide formed, for example, after roasting sulfide ores, or obtained by a direct method (by burning sulfur in oxygen), is oxidized to sulfuric anhydride at a temperature of 500 degrees Celsius on catalysts made of platinum, vanadium oxide and the like. But, in order to get concentrated sulfuric acid in an artisanal way, it is not necessary to resort to the tricks described above. We buy a battery in a car store, take an ordinary glass jar and pour it there, then we take a pan, pour a motor into it (working off will do quite well) and put a jar there. Then we put it all on the electric stove.

Thus, water is evaporated from the electrolyte. The trick of the bath is that it is somewhat more than boiling water, and thus the water boils away calmly, but the oil does not boil and the glass jar remains intact, because. heats up evenly over the entire area. Even hot concentrated sulfuric acid does not interact with glass, so the amount of impurities in it is minimal. The process can be carried out in the temperature range from 100 to 300 degrees, but it is better not to exceed the boiling point of the oil. Continue the process until the water boils away. In principle, enrichment of sulfuric acid can be carried out in a solid metal container, but after that the acid will be heavily contaminated with impurities and will have a color, and besides, there is a possibility that the container will leak during the process.

note

Avoid sudden temperature changes, this applies to a glass jar, i.e. do not put a cold jar in hot oil and a hot jar on a cold surface, let it cool completely, otherwise it will burst without fail. Be sure to protect your eyes, skin, clothing, use gloves, goggles and other means. Hot concentrated sulfuric acid is a pretty scary thing.

Helpful advice

In automotive stores, in addition to the standard electrolyte with a density of 1.27, it is also sold with a density of 1.4, take it, the product yield will be greater. It is desirable to do such things in the air, because. When heated, the oil will smoke a little.

Sources:

production of sulfuric acid

In the automotive practice of every driver, there comes a time when, when using an old, battered car battery, it becomes necessary to drain the used electrolyte from cans. This is due to the fact that the plates of the old battery begin to crumble and, in order to prevent their short circuit, it is necessary to replace the electrolyte in order to add to its service life. This operation must be carried out with due care.

You will need

dishes where you will drain the spent electrolyte, a rubber bulb with a spout 10-12 cm, clean rags.

Instruction

Place the battery removed from the workbench (desktop). Thoroughly wipe the surface of the battery. Unscrew the plugs that close the battery banks. Place a container next to the battery to drain the used one. Take a rubber bulb, squeeze it, thereby releasing air from it and immerse the nose all the way into the battery jar. When the pear has regained its original shape, it is that it is full. Gently transfer the spout of the pear and, using the extrusion method, release the pear from the waste liquid, pouring it into the dishes for working off.

Repeat this operation until the final draining of all battery cans. If you need to fill in a new electrolyte, it is advisable to rinse the cans with distilled water. To this end, draw liquid into a rubber bulb, fill each jar with distilled water. After that, tighten the corks on the banks and turn the battery over several times. After that, you also select the used wash with a rubber bulb. Now you need to pour the prepared electrolyte with the required density into the jars. To do this, collect fresh electrolyte in a pear and fill the jars. They must be filled to the bottom cut of the neck. After you fill the battery with electrolyte, it must be put on charge.

If the electrolyte has got on open areas of the body, it is necessary to wash the affected area with running water, and if the lesions are small, smear the burn with sea buckthorn oil or its substitute. However, if the lesion is extensive, after mandatory washing, you must contact the burn department, where you will be provided with the necessary assistance.

note

In order to drain the electrolyte, it is necessary to know the conditions for working with toxic and harmful liquids. You must be dressed in work overalls, because. Electrolyte getting on the fabric will inevitably ruin the clothes. Hair must be removed under a working headgear, rubber gloves are prepared, in which you will drain the electrolyte. The workplace should be free from foreign objects that will interfere with work. Running water should be provided near the workplace. Near the workplace there should be a medical portable first-aid kit, or an automobile first-aid kit with bandages and sea buckthorn oil (Rescuer ointment). When working with toxic liquids, it is important to protect the eyes from accidental contact with electrolyte. For this purpose, work must be done in working glasses.

Helpful advice

Acid battery electrolyte is an aqueous solution of concentrated sulfuric acid. The electrolyte for the battery is prepared from dilute sulfuric acid with a density of 1.40 g / cu cm, to which distilled water is added, bringing the battery density to 1.27 in summer, and to 1.29-1.31 g / cu cm in winter.

Sources:

electrolyte drain

In order for the battery to always work reliably, monitor the level and density of the electrolyte in the banks. Top up with evaporating distilled water to a level of at least 10 mm above the plates. If during the next density measurements it does not reach the set values, then it's time to add electrolyte.

You will need

Electrolyte or battery acid, distilled water, hydrometer, enema, measuring cup, goggles, rubber gloves

In our country, there are many small and large companies, on the Internet you can find a website on chemistry that sell reagents. But often only a sufficient batch can be ordered, for example, solid and bulk chemicals can be sold from a kilogram, and acids in liter bottles. It is clear that in order to conduct entertaining chemical experiments for children, such volumes are not required. Therefore, let's try to figure out where to get chemical reagents for chemical experiments at home. The surest way is to ask in the school chemistry room. The purity of the reagent will be observed here and in the end you will be one hundred percent sure that it is sodium hydroxide, and not calcium hydroxide. But this method is not suitable for everyone, so let's still understand further.

Where to get metals

Aluminum. The source of this metal in everyday life are old aluminum spoons and plates, aluminum wire
Aluminum powder is silver paint, sold in hardware stores.
Copper - copper wire, mined from wires or from transformer windings.
Lead, in the form of neat sinkers, is easy to buy at a fishing store.
We buy tin in the form of solder for soldering in radio stores. True, there it is sold in the form of an alloy, but for home use, the percentage of tin in the solder is quite enough.
Magnesium can be obtained by drilling a magnesium anode (heating element) for a water heater. In Soviet times, the oil pans of Zaporozhets cars served as an inexhaustible source of magnesium.
Chrome can be stripped off an old metal bumper. The resulting chips are quite clean and well suited for experiments.
Tungsten is found in the filaments of light bulbs.
Cerium is the "silicon" for lighters, the one that sparks when rubbed.

Attention! On the Internet, we met sources offering to extract some metals, such as zinc, lithium, dismantling batteries. Do not try to do this yourself and in no case let children do it, otherwise you risk getting a chemical burn.

Where to get acid

Sulfuric acid in the form of a 25-30% solution for batteries ("Acid Electrolyte") is purchased at car dealerships. It is impossible to buy pure sulfuric acid.
Orthophosphoric acid is sold in radio supply stores under the name "soldering flux".
Acetic acid is common table vinegar, available at any grocery store.
Boric acid is freely sold in pharmacies
Citric acid is known to any housewife, we buy it at the grocery store.
Nitric acid 45% is sometimes found on radio markets.
Oxalic acid . We follow her to the hardware store.

Where to get bases

Sodium hydroxide under the names caustic soda, caustic soda, caustic soda is sold in radio, photo or household goods stores.
Calcium hydroxide is slaked lime, sold in household stores.
Ammonia solution in water is ammonia. It is sold in a pharmacy, though it is gradually becoming a rarity.

Where to get salt

Sodium hypochlorite - means "Whiteness", sold in hardware stores.
Ammonium nitrate, also known as ammonium nitrate, is looked for in stores for summer residents and household stores.
Barium nitrate - coating of Bengal candles.
Silver nitrate, also known as lapis, can sometimes still be found in pharmacies. It is necessary to choose pharmacies more locally, still with old stocks.
Sodium chloride is table salt.
Potassium chloride - sold in stores for summer residents and gardeners as a fertilizer.
Ammonium chloride - ammonia. Do not confuse with ammonia! Ammonia is an aqueous solution of ammonium hydroxide.
Cobalt chloride - can be bought in tablets. Sold in some veterinary pharmacies as a medicine for ruminant pets
Calcium chloride is sold in pharmacies in ampoules for injection.
Potassium iodide is part of the means against iodine deficiency, but in this case it is necessary to read the composition of the drug. We buy from a pharmacy.
Potassium sulfate - fertilizer, sold in household stores.
We are looking for copper sulfate or copper sulfate in a household store.
Magnesium sulfate or magnesia (bitter salt) is sold in pharmacies as a laxative or in household stores as a fertilizer.
Ammonium sulfate - fertilizer in the household store.
We buy barium sulfate, barium sulfate in a pharmacy.
Calcium sulfate = gypsum.
Iron(II) sulfate (iron vitriol) is sold at a hardware store.
Sodium bicarbonate - baking soda.
Sodium carbonate - soda ash or laundry soda. Used as a cleaning agent.
Calcium carbonate is common chalk or marble.
Lead acetate - lead lotions that are sold in pharmacies.
Sodium silicate - liquid glass, stationery silicate glue.
Potassium silicate is the same. Sold in stationery stores.
Potassium bromide is sold in pharmacies under the name Adonis Bromine.

Where to get other chemicals

Hydrogen peroxide can be bought at a pharmacy either in the form of a solution or in the form of hydroperite tablets.
Calcium oxide is quicklime, for which you need to go to the household.
Acetone - buy at the nearest hardware store. We need Technical Acetone.
Sulfur - sold in household stores and gardening stores in the form of lumps or in bags. In bags, sulfur is much more expensive than lumpy, but at the same time much cleaner. "Colloidal sulfur" is not suitable for our purposes at all, because contains too many impurities. And it’s better and cheaper to take fodder sulfur in pet supplies, it is generally almost perfectly clean.
Toluene - sold in household stores as a solvent 646. Distillation is necessary, because. it is a multi-component solvent with a toluene content of about 50%.
Glycerin - freely sold in a pharmacy.
Phenolphthalein tablets are sold in a pharmacy called purgen.
Litmus paper is sometimes sold in pet stores.
Urotropin is a dry fuel, sold in household stores and departments for tourists.
Chromium oxide can be bought in the Varnishes and paints department.
Indigo carmine is a blue food coloring found in grocery aisles.
Glucose - freely sold in pharmacies.

Let's make some summary. Most of the reagents you need can be bought either at a pharmacy or in stores for summer residents.

Reagents from the "Garden Garden" store and household stores

ammonium sulfate,
zinc sulfate,
iron sulfate,
copper sulfate,
magnesium sulfate,
manganese sulfate,
potassium sulfate,
ammonium nitrate,
potassium nitrate,
magnesium nitrate,
monopotassium phosphate,
sodium tetraborate,
boric acid (crystalline),
oxalic acid (crystalline),
urea,
succinic acid,
sulfur.

International name: Sulfuric acid

Chemical formula: H2SO4

Molar mass: 98.078 ± 0.006 g/mol

CAS.: 7664-93-9

Physical and chemical properties

Sulfuric acid is a caustic, toxic substance, dibasic (H 2 SO 4), having the highest oxidation state (+6). Concentrated sulfuric acid is an oily liquid that has a "coppery" taste and is odorless and colorless. Very hygroscopic, absorbs moisture from the air. Reacts with metal oxides. Strong oxidizer. Forms sulfates, hydrosulfites, ethers. Restores weaker acids from salts.

Mixes sulfuric acid with water and sulfuric anhydride is also called sulfuric acid.

Melting point 10.38 °C. Boiling point 279.6 °C

Precautionary measures

Sulfuric acid extremely caustic and toxic, belongs to the 2nd hazard class. Causes severe burns of the skin, mucous membranes and respiratory organs, so it is important to work with it in the most protected suits, shoes, masks, gloves, goggles.

Keep in mind that when this acid and water come into contact, steam, gas and heat are violently released.

Sulfuric acid is explosive and fireproof.

Storage conditions

It is required to store sulfuric acid in a special container made of steel, specialized steel or steel grade St3 according to GOST 380, lined with acid-resistant bricks, tiles or other acid-resistant material.

Small amounts of sulfuric acid can be stored in glass containers.

Application

In the chemical industry, sulfuric acid has found wide application for the production of:

explosive and smoke-forming substances;
chemical fibers;
dyes;
mineral fertilizers;
lead batteries;
mineral salts and acids

Sulfuric acid is a substance that belongs to strong dibasic acids. The chemical formula of sulfuric acid is H 2 SO 4. Pure sulfuric acid is a colorless oily liquid. The density is 1.84 g/cm 3 . The melting point is -10.4 degrees Celsius. The chemical properties of this substance have contributed to its widespread use in industry.

Remember the sulfuric acid equation

The sulfuric acid equations describing its production are based on the absorption of sulfur oxide (VI) by water. Sulfur oxide (VI) SO 3 is the highest sulfur oxide with high chemical activity. The interaction of this substance with water leads to the appearance of sulfuric acid. This process is accompanied by the release of a large amount of heat.

Sulfuric acid can be obtained, for example, from the mineral pyrite. This is one of the industrial methods for obtaining this substance. It is described by the following equations:

4FeS 2 + 11O 2 \u003d 2Fe 2 O 3 + 8SO 2
2SO 2 +O 2 \u003d 2SO 3
SO 3 + H 2 O \u003d H 2 SO 4

In this method, vanadium (V) oxide is used as a catalyst in the oxidation of SO 2 to SO 3. In addition, the catalysts for this reaction are iron oxide and platinum. However, in industry they are not used for reasons of rationality. So, platinum is a very expensive metal. And iron oxide for the manifestation of catalytic properties must be heated to a temperature of 625 degrees Celsius. Its use would require additional complication of the process.

Technical sulfuric acid is a mixture of sulfuric acid and water. The mechanism of oxidation of metals by sulfuric acid depends on its concentration. So, if the acid is highly diluted, then it oxidizes with a hydrogen ion. An example of such a reaction is shown below:

Zn + H 2 SO 4 \u003d ZnSO 4 + H 2

In this case, only those metals are oxidized, the activity of which exceeds the activity of hydrogen. If the acid concentration is high, then the oxidation takes place due to sulfur. Such an acid reacts with silver, as well as with metals that are in a series of voltages below this element. In this case, the final products depend on the activity of the metal and the reaction conditions. So, if the metal is inactive, then the acid is reduced to sulfur oxide (IV):

Cu + 2H 2 SO 4 \u003d CuSO 4 + SO 2 + 2H 2 O

More active metals can release either sulfur or hydrogen sulfide:

3Zn + 4H 2 SO 4 \u003d 3ZnSO 4 + S + 4H 2 O
4Zn + 5H 2 SO 4 \u003d 4ZnSO 4 + H 2 S + 4H 2 O

If you are interested in how to get sulfuric acid, the easiest way to do this is in the store. Since when producing it in a home laboratory, one cannot count on receiving a batch, the volume of which is suitable for practical use.

Sulfuric acid is an oily heavy liquid substance that is colorless and odorless. It is a strong oxidizing agent that interacts with many metals. A dilute compound also reacts with all metals located in the voltage series to the left of hydrogen, but does not have oxidizing properties.

Areas of use

In industry: in the extraction of ores, for the production of fertilizers, various chemical fibers, dyes and chemical mixtures.
In lead-acid batteries, it plays the role of an electrolyte.
In the food industry, it is used as an emulsifier E513.
Chemical enterprises receive titanium dioxide, ethyl alcohol and other substances with its help.

At the enterprises it is possible to buy technical sulfuric acid in bulk. The compound is transported by rail or road and stored in stainless steel tanks. Tanks are placed in a room where acid-resistant tiles or bricks are laid on the floor, there must be a canopy or roof on top to prevent precipitation. The substance is very hygroscopic and is able to absorb moisture from the air, so it is important that the container where it is stored is hermetically sealed. Shelf life - 1 month from the date of manufacture.

When working with this compound, you should observe safety measures and work in a special suit with a gas mask, safety shoes and gloves. It is a caustic chemical that, on contact with mucous membranes, skin and respiratory tract, causes chemical burns, difficulty breathing and coughing. Permissible content of the compound in the air of the working room is 1 mg/m? and 0.1 mg/m? in the atmosphere (per day). In contact with water, a large amount of smoke and heat is released. The substance is not explosive.