Any acid is a complex substance whose molecule contains one or more hydrogen atoms and an acid residue.

The formula of sulfuric acid is H2SO4. Consequently, the sulfuric acid molecule contains two hydrogen atoms and the acidic residue SO4.

Sulfuric acid is formed when sulfur oxide reacts with water

SO3+H2O -> H2SO4

Pure 100% sulfuric acid (monohydrate) is a heavy liquid, viscous like oil, colorless and odorless, with a sour “copper” taste. Already at a temperature of +10 ° C it hardens and turns into a crystalline mass.

Concentrated sulfuric acid contains approximately 95% H2SO4. And it hardens at temperatures below –20°C.

Interaction with water

Sulfuric acid dissolves well in water, mixing with it in any proportion. This releases a large amount of heat.

Sulfuric acid can absorb water vapor from the air. This property is used in industry for drying gases. The gases are dried by passing them through special containers with sulfuric acid. Of course, this method can only be used for those gases that do not react with it.

It is known that when sulfuric acid comes into contact with many organic substances, especially carbohydrates, these substances become charred. The fact is that carbohydrates, like water, contain both hydrogen and oxygen. Sulfuric acid takes these elements away from them. What remains is coal.

In an aqueous solution of H2SO4, the indicators litmus and methyl orange turn red, which indicates that this solution has a sour taste.

Interaction with metals

Like any other acid, sulfuric acid is capable of replacing hydrogen atoms with metal atoms in its molecule. It interacts with almost all metals.

Diluted sulfuric acid reacts with metals like an ordinary acid. As a result of the reaction, a salt with an acidic residue SO4 and hydrogen is formed.

Zn + H2SO4 = ZnSO4 + H2

A concentrated sulfuric acid is a very strong oxidizing agent. It oxidizes all metals, regardless of their position in the voltage series. And when reacting with metals, it itself is reduced to SO2. Hydrogen is not released.

Сu + 2 H2SO4 (conc) = CuSO4 + SO2 + 2H2O

Zn + 2 H2SO4 (conc) = ZnSO4 + SO2 + 2H2O

But gold, iron, aluminum, and platinum group metals do not oxidize in sulfuric acid. Therefore, sulfuric acid is transported in steel tanks.

The sulfuric acid salts that are obtained as a result of such reactions are called sulfates. They are colorless and easily crystallize. Some of them are highly soluble in water. Only CaSO4 and PbSO4 are slightly soluble. BaSO4 is almost insoluble in water.

Interaction with bases

The reaction between acids and bases is called neutralization reaction. As a result of the neutralization reaction of sulfuric acid, a salt containing the acid residue SO4 and water H2O are formed.

Examples of sulfuric acid neutralization reactions:

H2SO4 + 2 NaOH = Na2SO4 + 2 H2O

H2SO4 + CaOH = CaSO4 + 2 H2O

Sulfuric acid reacts with neutralization with both soluble and insoluble bases.

Since the sulfuric acid molecule has two hydrogen atoms, and two bases are required to neutralize it, it is classified as a dibasic acid.

Interaction with basic oxides

From the school chemistry course we know that oxides are complex substances that contain two chemical elements, one of which is oxygen in the oxidation state -2. Basic oxides are called oxides of 1, 2 and some 3 valence metals. Examples of basic oxides: Li2O, Na2O, CuO, Ag2O, MgO, CaO, FeO, NiO.

Sulfuric acid reacts with basic oxides in a neutralization reaction. As a result of this reaction, as in the reaction with bases, salt and water are formed. The salt contains the acidic residue SO4.

CuO + H2SO4 = CuSO4 + H2O

Interaction with salts

Sulfuric acid reacts with salts of weaker or volatile acids, displacing these acids from them. As a result of this reaction, a salt with an acidic residue SO4 and an acid are formed

H2SO4+BaCl2=BaSO4+2HCl

Application of sulfuric acid and its compounds

Barium porridge BaSO4 is capable of blocking X-rays. Filling the hollow organs of the human body with it, radiologists examine them.

In medicine and construction, natural gypsum CaSO4 * 2H2O and calcium sulfate crystalline hydrate are widely used. Glauber's salt Na2SO4 * 10H2O is used in medicine and veterinary medicine, in the chemical industry - for the production of soda and glass. Copper sulfate CuSO4 * 5H2O is known to gardeners and agronomists, who use it to combat pests and plant diseases.

Sulfuric acid is widely used in various industries: chemical, metalworking, oil, textile, leather and others.

New topic: Sulfuric acid –H 2 SO 4

1. Electronic and structural formulas of sulfuric acid

*S - sulfur is in an excited state 1S 2 2S 2 2P 6 3S 1 3P 3 3d 2

Electronic formula of a sulfuric acid molecule:

Structural formula of the sulfuric acid molecule:

1 H - -2 O -2 O

1 H - -2 O -2 O

2.Receipt:

The chemical processes for the production of sulfuric acid can be represented as the following diagram:

S +O 2 +O 2 +H 2 O

FeS 2 SO 2 SO 3 H 2 SO 4

Sulfuric acid is prepared in three stages:

Stage 1. Sulfur, iron pyrite or hydrogen sulfide are used as raw materials.

4 FeS 2 + 11 O 2 = 2Fe 2 O 3 + 8SO 2

2 stage. Oxidation of SO 2 to SO 3 with oxygen using a V 2 O 5 catalyst

2SO 2 +O 2 =2SO 3 +Q

Stage 3. To convert SO 3 into sulfuric acid, it is not water that is used. strong heating occurs, and a concentrated solution of sulfuric acid.

SO 3 +H 2 O H 2 SO 4

The result is oleum - a solutionSO 3 in sulfuric acid.

Device circuit diagram(see textbook p. 105)

3.Physical properties.

a) liquid b) colorless c) heavy (oil of vitriol) d) non-volatile

d) when dissolved in water, strong heating occurs ( therefore, sulfuric acid must certainly be poured intowater,Anot the other way around!)

4. Chemical properties of sulfuric acid.

DilutedH 2 SO 4	ConcentratedH 2 SO 4
Has all the properties of acids	Has specific properties
1.Changes the color of the indicator: H 2 SO 4 H + +HSO 4 - HSO 4 - H + +SO 4 2- 2. Reacts with metals standing before hydrogen: Zn+ H 2 SO 4 ZnSO 4 +H 2 3. Reacts with basic and amphoteric oxides: MgO+ H 2 SO 4 MgSO 4 +H 2 O 4. Interacts with bases (neutralization reaction) 2NaOH+H 2 SO 4 Na 2 SO 4 +2H 2 O When there is an excess of acid, acid salts are formed NaOH+H 2 SO 4 NaHSO 4 +H 2 O 5. Reacts with dry salts, displacing other acids from them (this is the strongest and most non-volatile acid): 2NaCl+H 2 SO 4 Na 2 SO 4 +2HCl 6. Reacts with salt solutions, if an insoluble salt is formed: BaCl 2 +H 2 SO 4 BaSO 4 +2HCl - whitesediment qualitative reaction to ionSO 4 2- 7.When heated, it decomposes: H2SO4H2O+SO3	1. Concentrated H 2 SO 4 is a strong oxidizing agent; when heated, it reacts with all metals (except Au and Pt). In these reactions, depending on the activity of the metal and conditions, S,SO 2 or H 2 S is released For example: Cu+ conc 2H 2 SO 4 CuSO 4 +SO 2 +H 2 O 2.conc. H 2 SO 4 passivates iron and aluminum, therefore it can be transported in steel and aluminum tanks. 3. conc. H 2 SO 4 absorbs water well H 2 SO 4 +H 2 O H 2 SO 4 *2H 2 O Therefore, it chars organic matter

5.Application: Sulfuric acid is one of the most important products used in various industries. Its main consumers are the production of mineral fertilizers, metallurgy, and refining of petroleum products. Sulfuric acid is used in the production of other acids, detergents, explosives, medicines, paints, and as electrolytes for lead batteries. (Textbook p. 103).

6.Salts of sulfuric acid

Sulfuric acid dissociates stepwise

H 2 SO 4 H + +HSO 4 -

HSO 4 - H + +SO 4 2-

therefore, it forms two types of salts - sulfates and hydrosulfates

For example: Na 2 SO 4 - sodium sulfate (medium salt)

Na HSO 4 - sodium hydrogen sulfate (acid salt)

The most widely used are:

Na 2 SO 4 * 10H 2 O – Glauber's salt (used in the production of soda, glass, in medicine and

veterinary medicine

СaSO 4 *2H 2 O – gypsum

СuSO 4 *5H 2 O – copper sulfate (used in agriculture).

Laboratory experience

Chemical properties of sulfuric acid.

Equipment: Test tubes.

Reagents: sulfuric acid, methyl orange, zinc, magnesium oxide, sodium hydroxide and phenolphthalein, sodium carbonate, barium chloride.

b) Fill out the observation table

Lesson objectives: students should know the structure, physical and chemical properties of H 2 SO 4; be able, based on knowledge of the rate of chemical reactions and chemical equilibrium, to justify the choice of reaction conditions underlying the production of sulfuric acid; determine sulfate and sulfide ions in practice.

Basic concepts: sulfur dioxide, sulfuric anhydride, complex use of raw materials.

During the classes

I. Organizational moment; checking homework

II. New material

1. Electronic and structural formulas. Since sulfur is in the 3rd period of the periodic table, the octet rule is not observed and a sulfur atom can acquire up to twelve electrons.

(Sulfur's six electrons are indicated by an asterisk.)

2. Receipt. Sulfuric acid is formed by the reaction of sulfur oxide (VI) with water (SO 3 + H 2 O H 2 SO 4). A description of the production of sulfuric acid is given in § 16 (, pp. 37 - 42).

3. Physical properties. Sulfuric acid is a colorless, heavy (=1.84 g/cm3), non-volatile liquid. When it is dissolved in water, very strong heating occurs. Remember that you cannot pour water into concentrated sulfuric acid (Fig. 2)! Concentrated sulfuric acid absorbs water vapor from the air. This can be verified if an open vessel with concentrated sulfuric acid is balanced on a scale: after some time the cup with the vessel will drop.

Rice. 2.

4. Chemical properties. Dilute sulfuric acid has general properties, characteristic of acids and specific (Table 7).

Table 7

Chemical properties of sulfuric acid
Common with other acids	Specific
1. An aqueous solution changes the color of the indicators.	1. Concentrated sulfuric acid is a strong oxidizing agent: when heated, it reacts with almost all metals (except Au, Pt and some others). In these reactions, depending on the activity of the metal and conditions, SO2, H2S, S are released, for example: Cu+2H 2 SO 4 CuSO 4 +SO 2 +2H 2 O
2. Dilute sulfuric acid reacts with metals: H 2 SO 4 +Zn ZnSO 4 +H 2 2H + + SO 4 2- +Zn 0 Zn 2+ + SO 4 2- +H 2 0 2H + + Zn 0 Zn 2+ + H 2 0	2. Concentrated sulfuric acid reacts vigorously with water to form hydrates: H 2 SO 4 + nH 2 O H 2 SO 4 nH 2 O+ Q Concentrated sulfuric acid is capable of removing hydrogen and oxygen from organic substances in the form of water, charring organic substances
3. Reacts with basic and amphoteric oxides: H 2 SO 4 + MgO MgSO 4 + H 2 O 2H + +SO 4 2- +MgOMg 2+ +SO 4 2- +H 2 O 2H + + MgO Mg 2+ + H 2 O	3. A characteristic reaction to sulfuric acid and its salts is interaction with soluble barium salts: H 2 SO 4 + BaCl 2 BaSO 4 + 2HCl 2H + + SO 4 2- + Ba 2+ + 2Cl - BaSO 4 + 2H + + 2Cl - Ba 2+ + SO 4 2- BaSO 4 A white precipitate forms, which is insoluble in either water or concentrated nitric acid.
4. Interacts with bases: H 2 SO 4 + 2KOH K 2 SO 4 + 2H 2 O 2H + + SO 4 2- + 2K + + 2OH - 2K + + SO 4 2- + 2H 2 O 2H + + 2OH - 2H 2 O If the acid is taken in excess, an acid salt is formed: H 2 SO 4 +NaOH NaHSO 4 +H 2 O
5. Reacts with salts, displacing other acids from them: 3H 2 SO 4 +Ca 3 (PO 4) 2 3CaSO 4 +2H 3 PO 4

Application. Sulfuric acid is widely used (Fig. 3); it is the main product of the chemical industry.

Rice. 3. Application of sulfuric acid: 1 - production of dyes; 2 - mineral fertilizers; 3 - purification of petroleum products; 4 - electrolytic production of copper; 5 - electrolyte in batteries; 6 - production of explosives; 7 - dyes; 8 - artificial silk; 9 -- glucose; 10 -- salts; 11 - acids.

Sulfuric acid forms two series of salts - medium and acidic:

Na 2 SO 4 NaHSО 4

sodium sulfate sodium hydrogen sulfate

(medium salt) (sour salt)

Salts of sulfuric acid are widely used, for example, Na 2 SO 4 10H 2 O - sodium sulfate crystal hydrate (Glauber's salt) is used in the production of soda, glass, in medicine and veterinary medicine. CaSO 4 2H 2 O - calcium sulfate crystal hydrate (natural gypsum) - is used to produce semi-hydrous gypsum, necessary in construction, and in medicine - for applying plaster bandages. CuSO 4 5H 2 O - crystalline hydrate of copper (II) sulfate (copper sulfate) - is used in the fight against plant pests.

III. Consolidating new material

1. In winter, a vessel with concentrated sulfuric acid is sometimes placed between the window frames. For what purpose is this done, why can’t the vessel be filled to the top with acid?

2. Concentrated sulfuric acid, when heated, reacts with mercury and silver, similar to how it reacts with copper. Write down equations for these reactions and indicate the oxidizing agent and reducing agent.

3. How to recognize sulfides? Where are they used?

4. Create reaction equations that are practically feasible using the given diagrams:

Hg + H2SO4(conc)

MgCl 2 + H 2 SO 4 (conc.)

Na 2 SO 3 + H 2 SO 4

Al(OH) 3 + H 2 SO 4

When drawing up reaction equations, indicate the conditions for their implementation. Where required, write the equations in ionic and abbreviated ionic form.

5. Name the oxidizing agent in the reactions of: a) dilute sulfuric acid with metals; b) concentrated sulfuric acid with metals.

6. What do you know about sulfurous acid?

7. Why is concentrated sulfuric acid a strong oxidizing agent? What are the special properties of concentrated sulfuric acid?

8. How does concentrated sulfuric acid react with metals?

9. Where are sulfuric acid and its salts used?

1. What volume of oxygen will be required to burn: a) 3.4 kg of hydrogen sulfide; b) 6500 m 3 of hydrogen sulfide?

2. What is the mass of a solution containing 0.2 mass fractions of sulfuric acid, which is consumed in the reaction with 4.5 g of aluminum?

Laboratory experiments

VI. Recognition of sulfate ions in solution. Pour 1-2 ml of sodium sulfate solution into one test tube, the same amount of zinc sulfate into another, and a dilute sulfuric acid solution into the third. Place a zinc granule in each test tube, and then add a few drops of barium chloride or barium nitrate solution.

Tasks. 1. How can you distinguish sulfuric acid from its salts? 2. How to distinguish sulfates from other salts? Write down equations for the reactions you performed in molecular, ionic, and abbreviated ionic form.

IV. Homework

Sulfuric acid (H2SO4) is one of the most caustic acids and dangerous reagents known to man, especially in concentrated form. Chemically pure sulfuric acid is a heavy toxic liquid of oily consistency, odorless and colorless. It is obtained by contact oxidation of sulfur dioxide (SO2).

At a temperature of + 10.5 °C, sulfuric acid turns into a frozen glassy crystalline mass, greedily, like a sponge, absorbing moisture from the environment. In industry and chemistry, sulfuric acid is one of the main chemical compounds and occupies a leading position in terms of production volume in tons. This is why sulfuric acid is called the “blood of chemistry.” With the help of sulfuric acid, fertilizers, medicines, other acids, large quantities of fertilizers and much more are obtained.

Basic physical and chemical properties of sulfuric acid

1. Sulfuric acid in its pure form (formula H2SO4), at a concentration of 100%, is a colorless, thick liquid. The most important property of H2SO4 is its high hygroscopicity - the ability to remove water from the air. This process is accompanied by a large-scale release of heat.
2. H2SO4 is a strong acid.
3. Sulfuric acid is called a monohydrate - it contains 1 mole of H2O (water) per 1 mole of SO3. Due to its impressive hygroscopic properties, it is used to extract moisture from gases.
4. Boiling point – 330 °C. In this case, the acid decomposes into SO3 and water. Density – 1.84. Melting point – 10.3 °C/.
5. Concentrated sulfuric acid is a powerful oxidizing agent. To initiate a redox reaction, the acid must be heated. The result of the reaction is SO2. S+2H2SO4=3SO2+2H2O
6. Depending on the concentration, sulfuric acid reacts with metals differently. In a dilute state, sulfuric acid is capable of oxidizing all metals that are in the voltage series before hydrogen. The exception is the most resistant to oxidation. Dilute sulfuric acid reacts with salts, bases, amphoteric and basic oxides. Concentrated sulfuric acid is capable of oxidizing all metals in the voltage series, including silver.
7. Sulfuric acid forms two types of salts: acidic (these are hydrosulfates) and intermediate (sulfates)
8. H2SO4 reacts actively with organic substances and non-metals, and it can turn some of them into coal.
9. Sulfuric anhydrite dissolves well in H2SO4, and in this case oleum is formed - a solution of SO3 in sulfuric acid. Outwardly, it looks like this: fuming sulfuric acid, releasing sulfuric anhydrite.
10. Sulfuric acid in aqueous solutions is a strong dibasic acid, and when it is added to water, a huge amount of heat is released. When preparing dilute solutions of H2SO4 from concentrated ones, it is necessary to add a heavier acid to the water in a small stream, and not vice versa. This is done to prevent the water from boiling and splashing the acid.

Concentrated and diluted sulfuric acids

Concentrated solutions of sulfuric acid include solutions from 40% that can dissolve silver or palladium.

Dilute sulfuric acid includes solutions whose concentration is less than 40%. These are not such active solutions, but they are capable of reacting with brass and copper.

Preparation of sulfuric acid

The production of sulfuric acid on an industrial scale began in the 15th century, but at that time it was called “oil of vitriol.” If earlier humanity consumed only a few tens of liters of sulfuric acid, then in the modern world the calculation goes to millions of tons per year.

The production of sulfuric acid is carried out industrially, and there are three of them:

1. Contact method.
2. Nitrose method
3. Other methods

Let's talk in detail about each of them.

Contact production method

The contact production method is the most common, and it performs the following tasks:

• The result is a product that satisfies the needs of the maximum number of consumers.
• During production, environmental damage is reduced.

In the contact method, the following substances are used as raw materials:

• pyrite (sulfur pyrite);
• sulfur;
• vanadium oxide (this substance acts as a catalyst);
• hydrogen sulfide;
• sulfides of various metals.

Before starting the production process, raw materials are pre-prepared. To begin with, in special crushing plants, the pyrite is crushed, which allows, by increasing the contact area of ​​the active substances, to speed up the reaction. Pyrite undergoes purification: it is lowered into large containers of water, during which waste rock and all kinds of impurities float to the surface. At the end of the process they are removed.

The production part is divided into several stages:

1. After crushing, the pyrite is cleaned and sent to the furnace, where it is fired at temperatures up to 800 °C. According to the counterflow principle, air is supplied into the chamber from below, and this ensures that the pyrite is in a suspended state. Today, this process takes a few seconds, but previously it took several hours to fire. During the roasting process, waste appears in the form of iron oxide, which is removed and subsequently transferred to the metallurgical industry. During firing, water vapor, O2 and SO2 gases are released. When purification from water vapor and tiny impurities is completed, pure sulfur oxide and oxygen are obtained.
2. In the second stage, an exothermic reaction occurs under pressure using a vanadium catalyst. The reaction starts when the temperature reaches 420 °C, but it can be increased to 550 °C to increase efficiency. During the reaction, catalytic oxidation occurs and SO2 becomes SO3.
3. The essence of the third stage of production is as follows: absorption of SO3 in an absorption tower, during which oleum H2SO4 is formed. In this form, H2SO4 is poured into special containers (it does not react with steel) and is ready to meet the end consumer.

During production, as we said above, a lot of thermal energy is generated, which is used for heating purposes. Many sulfuric acid plants install steam turbines, which use the released steam to generate additional electricity.

Nitrous method for producing sulfuric acid

Despite the advantages of the contact production method, which produces more concentrated and pure sulfuric acid and oleum, quite a lot of H2SO4 is produced by the nitrous method. In particular, at superphosphate plants.

For the production of H2SO4, the starting material, both in the contact and nitrose methods, is sulfur dioxide. It is obtained specifically for these purposes by burning sulfur or roasting sulfur metals.

Processing sulfur dioxide into sulfurous acid involves the oxidation of sulfur dioxide and the addition of water. The formula looks like this:
SO2 + 1|2 O2 + H2O = H2SO4

But sulfur dioxide does not react directly with oxygen, therefore, with the nitrous method, sulfur dioxide is oxidized using nitrogen oxides. Higher oxides of nitrogen (we are talking about nitrogen dioxide NO2, nitrogen trioxide NO3) during this process are reduced to nitrogen oxide NO, which is subsequently oxidized again by oxygen to higher oxides.

The production of sulfuric acid by the nitrous method is technically formalized in two ways:

• Chamber.
• Tower.

The nitrous method has a number of advantages and disadvantages.

Disadvantages of the nitrous method:

• The result is 75% sulfuric acid.
• Product quality is low.
• Incomplete return of nitrogen oxides (addition of HNO3). Their emissions are harmful.
• The acid contains iron, nitrogen oxides and other impurities.

Advantages of the nitrous method:

• The cost of the process is lower.
• Possibility of SO2 recycling at 100%.
• Simplicity of hardware design.

Main Russian sulfuric acid plants

The annual production of H2SO4 in our country is in the six-digit range - about 10 million tons. The leading producers of sulfuric acid in Russia are companies that are, in addition, its main consumers. We are talking about companies whose field of activity is the production of mineral fertilizers. For example, “Balakovo mineral fertilizers”, “Ammophos”.

In Crimea, in Armyansk, the largest titanium dioxide producer in Eastern Europe, Crimean Titan, operates. In addition, the plant produces sulfuric acid, mineral fertilizers, iron sulfate, etc.

Many factories produce various types of sulfuric acid. For example, battery sulfuric acid is produced by: Karabashmed, FKP Biysk Oleum Plant, Svyatogor, Slavia, Severkhimprom, etc.

Oleum is produced by UCC Shchekinoazot, FKP Biysk Oleum Plant, Ural Mining and Metallurgical Company, Kirishinefteorgsintez PA, etc.

Sulfuric acid of special purity is produced by OHC Shchekinoazot, Component-Reaktiv.

Spent sulfuric acid can be purchased at the ZSS and HaloPolymer Kirovo-Chepetsk plants.

Manufacturers of technical sulfuric acid are Promsintez, Khiprom, Svyatogor, Apatit, Karabashmed, Slavia, Lukoil-Permnefteorgsintez, Chelyabinsk Zinc Plant, Electrozinc, etc.

Due to the fact that pyrite is the main raw material in the production of H2SO4, and this is a waste of enrichment enterprises, its suppliers are the Norilsk and Talnakh enrichment factories.

The world's leading positions in H2SO4 production are occupied by the USA and China, which account for 30 million tons and 60 million tons, respectively.

Scope of application of sulfuric acid

The world consumes about 200 million tons of H2SO4 annually, from which a wide range of products are produced. Sulfuric acid rightfully holds the palm among other acids in terms of the scale of use for industrial purposes.

As you already know, sulfuric acid is one of the most important products of the chemical industry, so the scope of sulfuric acid is quite wide. The main areas of use of H2SO4 are as follows:

• Sulfuric acid is used in enormous volumes for the production of mineral fertilizers, and this consumes about 40% of the total tonnage. For this reason, factories that produce H2SO4 are built next to factories that produce fertilizers. These are ammonium sulfate, superphosphate, etc. During their production, sulfuric acid is taken in its pure form (100% concentration). To produce a ton of ammophos or superphosphate you will need 600 liters of H2SO4. These fertilizers are in most cases used in agriculture.
• H2SO4 is used to produce explosives.
• Purification of petroleum products. To obtain kerosene, gasoline and mineral oils, purification of hydrocarbons is required, which occurs using sulfuric acid. In the process of refining oil to purify hydrocarbons, this industry “takes” as much as 30% of the world’s tonnage of H2SO4. In addition, the octane number of fuel is increased with sulfuric acid and wells are treated during oil production.
• In the metallurgical industry. Sulfuric acid in metallurgy is used to remove scale and rust from wire and sheet metal, as well as to restore aluminum in the production of non-ferrous metals. Before coating metal surfaces with copper, chromium or nickel, the surface is etched with sulfuric acid.
• In the production of medicines.
• In the production of paints.
• In the chemical industry. H2SO4 is used in the production of detergents, ethylene, insecticides, etc., and without it these processes are impossible.
• For the production of other known acids, organic and inorganic compounds used for industrial purposes.

Salts of sulfuric acid and their use

The most important salts of sulfuric acid:

• Glauber's salt Na2SO4 · 10H2O (crystalline sodium sulfate). The scope of its application is quite capacious: the production of glass, soda, in veterinary medicine and medicine.
• Barium sulfate BaSO4 is used in the production of rubber, paper, and white mineral paint. In addition, it is indispensable in medicine for fluoroscopy of the stomach. It is used to make “barium porridge” for this procedure.
• Calcium sulfate CaSO4. In nature, it can be found in the form of gypsum CaSO4 2H2O and anhydrite CaSO4. Gypsum CaSO4 · 2H2O and calcium sulfate are used in medicine and construction. When gypsum is heated to a temperature of 150 - 170 °C, partial dehydration occurs, resulting in burnt gypsum, known to us as alabaster. By mixing alabaster with water to the consistency of a batter, the mass quickly hardens and turns into a kind of stone. It is this property of alabaster that is actively used in construction work: casts and casting molds are made from it. In plastering work, alabaster is indispensable as a binding material. Patients in trauma departments are given special fixing hard bandages - they are made on the basis of alabaster.
• Iron sulfate FeSO4 · 7H2O is used to prepare ink, impregnate wood, and also in agricultural activities to kill pests.
• Alum KCr(SO4)2 · 12H2O, KAl(SO4)2 · 12H2O, etc. are used in the production of paints and the leather industry (leather tanning).
• Many of you know copper sulfate CuSO4 · 5H2O firsthand. This is an active assistant in agriculture in the fight against plant diseases and pests - grain is treated with an aqueous solution of CuSO4 · 5H2O and sprayed on plants. It is also used to prepare some mineral paints. And in everyday life it is used to remove mold from walls.
• Aluminum sulfate – it is used in the pulp and paper industry.

Sulfuric acid in diluted form is used as an electrolyte in lead batteries. In addition, it is used to produce detergents and fertilizers. But in most cases it comes in the form of oleum - this is a solution of SO3 in H2SO4 (you can also find other formulas of oleum).

Amazing fact! Oleum is more chemically active than concentrated sulfuric acid, but despite this, it does not react with steel! It is for this reason that it is easier to transport than sulfuric acid itself.

The scope of use of the “queen of acids” is truly large-scale, and it is difficult to talk about all the ways it is used in industry. It is also used as an emulsifier in the food industry, for water purification, in the synthesis of explosives and many other purposes.

The history of sulfuric acid

Who among us has not at least once heard of copper sulfate? So, it was studied in ancient times, and in some works of the beginning of the new era, scientists discussed the origin of vitriol and their properties. Vitriol was studied by the Greek physician Dioscorides and the Roman nature explorer Pliny the Elder, and in their works they wrote about the experiments they carried out. For medical purposes, various vitriol substances were used by the ancient physician Ibn Sina. How vitriol was used in metallurgy was discussed in the works of the alchemists of Ancient Greece Zosimas of Panopolis.

The first way to obtain sulfuric acid is the process of heating potassium alum, and there is information about this in the alchemical literature of the 13th century. At that time, the composition of alum and the essence of the process were unknown to alchemists, but already in the 15th century, the chemical synthesis of sulfuric acid began to be deliberately studied. The process was as follows: alchemists treated a mixture of sulfur and antimony (III) sulfide Sb2S3 by heating with nitric acid.

In medieval times in Europe, sulfuric acid was called "oil of vitriol", but then the name changed to vitriol acid.

In the 17th century, Johann Glauber obtained sulfuric acid as a result of burning potassium nitrate and native sulfur in the presence of water vapor. As a result of the oxidation of sulfur with saltpeter, sulfur oxide was obtained, which reacted with water vapor, resulting in a liquid with an oily consistency. This was oil of vitriol, and this name for sulfuric acid still exists today.

In the thirties of the 18th century, a pharmacist from London, Ward Joshua, used this reaction for the industrial production of sulfuric acid, but in the Middle Ages its consumption was limited to several tens of kilograms. The scope of use was narrow: for alchemical experiments, purification of precious metals and in pharmacy. Concentrated sulfuric acid in small volumes was used in the production of special matches that contained bertholite salt.

Vitriol acid appeared in Rus' only in the 17th century.

In Birmingham, England, John Roebuck adapted the above method for producing sulfuric acid in 1746 and launched production. At the same time, he used durable large leaded chambers, which were cheaper than glass containers.

This method held its position in industry for almost 200 years, and 65% sulfuric acid was obtained in chambers.

After a while, the English Glover and the French chemist Gay-Lussac improved the process itself, and sulfuric acid began to be obtained with a concentration of 78%. But such an acid was not suitable for the production of, for example, dyes.

At the beginning of the 19th century, new methods were discovered for oxidizing sulfur dioxide into sulfuric anhydride.

Initially this was done using nitrogen oxides, and then platinum was used as a catalyst. These two methods of oxidizing sulfur dioxide have been further improved. The oxidation of sulfur dioxide on platinum and other catalysts became known as the contact method. And the oxidation of this gas with nitrogen oxides is called the nitrous method for producing sulfuric acid.

The British acetic acid merchant Peregrine Philips patented an economical process for the production of sulfur oxide (VI) and concentrated sulfuric acid only in 1831, and it is this method that is familiar to the world today as a contact method for its production.

Superphosphate production began in 1864.

In the eighties of the nineteenth century in Europe, the production of sulfuric acid reached 1 million tons. The main producers were Germany and England, producing 72% of the total volume of sulfuric acid in the world.

Transportation of sulfuric acid is a labor-intensive and responsible undertaking.

Sulfuric acid belongs to the class of dangerous chemicals, and upon contact with the skin causes severe burns. In addition, it can cause chemical poisoning in humans. If certain rules are not followed during transportation, sulfuric acid, due to its explosiveness, can cause a lot of harm to both people and the environment.

Sulfuric acid has been assigned a hazard class of 8 and must be transported by specially trained and trained professionals. An important condition for the delivery of sulfuric acid is compliance with specially developed Rules for the Transportation of Dangerous Goods.

Transportation by road is carried out in accordance with the following rules:

1. For transportation, special containers are made from a special steel alloy that does not react with sulfuric acid or titanium. Such containers do not oxidize. Dangerous sulfuric acid is transported in special sulfuric acid chemical tanks. They differ in design and are selected for transportation depending on the type of sulfuric acid.
2. When transporting fuming acid, specialized isothermal thermos tanks are taken, in which the required temperature regime is maintained to preserve the chemical properties of the acid.
3. If ordinary acid is transported, then a sulfuric acid tank is selected.
4. Transportation of sulfuric acid by road, such types as fuming, anhydrous, concentrated, for batteries, glover, is carried out in special containers: tanks, barrels, containers.
5. The transportation of dangerous goods can only be carried out by drivers who have an ADR certificate.
6. Travel time has no restrictions, since during transportation you must strictly adhere to the permissible speed.
7. During transportation, a special route is built, which should pass places of large crowds of people and production facilities.
8. Transport must have special markings and danger signs.

Dangerous properties of sulfuric acid for humans

Sulfuric acid poses an increased danger to the human body. Its toxic effect occurs not only upon direct contact with the skin, but upon inhalation of its vapors, when sulfur dioxide is released. Hazardous effects include:

• Respiratory system;
• Skin;
• Mucous membranes.

Intoxication of the body can be enhanced by arsenic, which is often included in sulfuric acid.

Important! As you know, severe burns occur when acid comes into contact with the skin. Poisoning by sulfuric acid vapors is no less dangerous. The safe dose of sulfuric acid in the air is only 0.3 mg per 1 square meter.

If sulfuric acid gets on the mucous membranes or skin, a severe burn appears that does not heal well. If the burn is significant in scale, the victim develops a burn disease, which can even lead to death if qualified medical care is not provided in a timely manner.

Important! For an adult, the lethal dose of sulfuric acid is only 0.18 cm per 1 liter.

Of course, “experiencing” the toxic effects of acid in everyday life is problematic. Most often, acid poisoning occurs due to neglect of industrial safety precautions when working with the solution.

Mass poisoning with sulfuric acid vapor may occur due to technical problems at work or negligence, and a massive release into the atmosphere occurs. To prevent such situations, special services operate whose task is to monitor the functioning of production where dangerous acid is used.

What symptoms are observed during sulfuric acid intoxication?

If the acid was ingested:

• Pain in the area of ​​the digestive organs.
• Nausea and vomiting.
• Abnormal bowel movements as a result of severe intestinal disorders.
• Heavy secretion of saliva.
• Due to toxic effects on the kidneys, the urine becomes reddish.
• Swelling of the larynx and throat. Wheezing and hoarseness occur. This can be fatal from suffocation.
• Brown spots appear on the gums.
• The skin turns blue.

When the skin is burned, there can be all the complications inherent in a burn disease.

In case of vapor poisoning, the following picture is observed:

• Burn of the mucous membrane of the eyes.
• Nose bleed.
• Burn of the mucous membranes of the respiratory tract. In this case, the victim experiences severe pain.
• Swelling of the larynx with symptoms of suffocation (lack of oxygen, skin turns blue).
• If the poisoning is severe, there may be nausea and vomiting.

It is important to know! Acid poisoning after ingestion is much more dangerous than intoxication from inhalation of vapors.

First aid and therapeutic procedures for sulfuric acid injury

Proceed as follows when in contact with sulfuric acid:

• First of all, call an ambulance. If liquid gets inside, rinse the stomach with warm water. After this, you will need to drink 100 grams of sunflower or olive oil in small sips. In addition, you should swallow a piece of ice, drink milk or burnt magnesia. This must be done to reduce the concentration of sulfuric acid and alleviate the human condition.
• If acid gets into your eyes, you need to rinse them with running water and then drip them with a solution of dicaine and novocaine.
• If acid gets on the skin, rinse the burned area well under running water and apply a bandage with soda. You need to rinse for about 10-15 minutes.
• In case of vapor poisoning, you need to go out into fresh air, and also rinse the affected mucous membranes with water as soon as possible.

In a hospital setting, treatment will depend on the area of ​​the burn and the degree of poisoning. Pain relief is carried out only with novocaine. To avoid the development of infection in the affected area, the patient is given a course of antibiotic therapy.

In case of gastric bleeding, plasma or blood transfusion is administered. The source of bleeding can be eliminated surgically.

1. Sulfuric acid occurs in nature in its 100% pure form. For example, in Italy, Sicily, in the Dead Sea, you can see a unique phenomenon - sulfuric acid seeps straight from the bottom! What happens is this: pyrite from the earth’s crust serves in this case as a raw material for its formation. This place is also called the Lake of Death, and even insects are afraid to fly near it!
2. After large volcanic eruptions, droplets of sulfuric acid can often be found in the earth's atmosphere, and in such cases the culprit can cause negative environmental consequences and cause serious climate change.
3. Sulfuric acid is an active absorbent of water, so it is used as a gas desiccant. In the old days, to prevent indoor windows from fogging up, this acid was poured into jars and placed between the glass of window openings.
4. Sulfuric acid is the main cause of acid rain. The main cause of acid rain is air pollution from sulfur dioxide, which when dissolved in water forms sulfuric acid. Sulfur dioxide, in turn, is released when fossil fuels are burned. In acid rain studied in recent years, the content of nitric acid has increased. The reason for this phenomenon is the reduction of sulfur dioxide emissions. Despite this fact, the main cause of acid rain remains sulfuric acid.

We offer you a video selection of interesting experiments with sulfuric acid.

Let's consider the reaction of sulfuric acid when it is poured into sugar. In the first seconds of sulfuric acid entering the flask with sugar, the mixture darkens. After a few seconds the substance turns black. Then the most interesting thing happens. The mass begins to grow rapidly and climb outside the flask. The output is a proud substance, similar to porous charcoal, 3-4 times larger than the original volume.

The author of the video suggests comparing the reaction of Coca-Cola with hydrochloric acid and sulfuric acid. When Coca-Cola is mixed with hydrochloric acid, no visual changes are observed, but when mixed with sulfuric acid, Coca-Cola begins to boil.

An interesting interaction can be observed when sulfuric acid comes into contact with toilet paper. Toilet paper is made of cellulose. When acid hits the cellulose molecule, it instantly breaks down releasing free carbon. Similar charring can be observed when acid comes into contact with wood.

I add a small piece of potassium to a flask with concentrated acid. In the first second, smoke is released, after which the metal instantly flares up, ignites and explodes, breaking into pieces.

In the following experiment, when sulfuric acid hits a match, it ignites. In the second part of the experiment, aluminum foil with acetone and a match inside is immersed. The foil is instantly heated, releasing a huge amount of smoke and completely dissolving it.

An interesting effect is observed when baking soda is added to sulfuric acid. The baking soda instantly turns yellow. The reaction proceeds with rapid boiling and an increase in volume.

We strongly advise against carrying out all of the above experiments at home. Sulfuric acid is a very aggressive and toxic substance. Such experiments must be carried out in special rooms equipped with forced ventilation. The gases released in reactions with sulfuric acid are very toxic and can cause damage to the respiratory tract and poisoning of the body. In addition, similar experiments are carried out using personal protective equipment for the skin and respiratory system. Take care of yourself!

Undiluted sulfuric acid is a covalent compound.

In the molecule, sulfuric acid is tetrahedrally surrounded by four oxygen atoms, two of which are part of the hydroxyl groups. The S–O bonds are double, and the S–OH bonds are single.

The colorless, ice-like crystals have a layered structure: each H 2 SO 4 molecule is connected to four neighboring strong hydrogen bonds, forming a single spatial framework.

The structure of liquid sulfuric acid is similar to the structure of solid one, only the integrity of the spatial framework is broken.

Physical properties of sulfuric acid

Under normal conditions, sulfuric acid is a heavy, oily liquid without color or odor. In technology, sulfuric acid is a mixture of both water and sulfuric anhydride. If the molar ratio of SO 3: H 2 O is less than 1, then it is an aqueous solution of sulfuric acid; if it is greater than 1, it is a solution of SO 3 in sulfuric acid.

100% H 2 SO 4 crystallizes at 10.45 ° C; T kip = 296.2 °C; density 1.98 g/cm3. H 2 SO 4 mixes with H 2 O and SO 3 in any ratio to form hydrates; the heat of hydration is so high that the mixture can boil, splash and cause burns. Therefore, it is necessary to add acid to water, and not vice versa, since when water is added to acid, lighter water will end up on the surface of the acid, where all the heat generated will be concentrated.

When aqueous solutions of sulfuric acid containing up to 70% H 2 SO 4 are heated and boiled, only water vapor is released into the vapor phase. Sulfuric acid vapor also appears above more concentrated solutions.

In terms of structural features and anomalies, liquid sulfuric acid is similar to water. There is the same system of hydrogen bonds, almost the same spatial framework.

Chemical properties of sulfuric acid

Sulfuric acid is one of the strongest mineral acids; due to its high polarity, the H–O bond is easily broken.

Sulfuric acid dissociates in aqueous solution , forming a hydrogen ion and an acidic residue:

H 2 SO 4 = H + + HSO 4 - ;

HSO 4 - = H + + SO 4 2- .

Summary equation:

H 2 SO 4 = 2H + + SO 4 2- .

Shows properties of acids , reacts with metals, metal oxides, bases and salts.

Dilute sulfuric acid does not exhibit oxidizing properties; when it interacts with metals, hydrogen and a salt containing the metal in the lowest oxidation state are released. In the cold, the acid is inert towards metals such as iron, aluminum and even barium.

Concentrated acid has oxidizing properties. Possible products of the interaction of simple substances with concentrated sulfuric acid are given in the table. The dependence of the reduction product on the acid concentration and the degree of activity of the metal is shown: the more active the metal, the more deeply it reduces the sulfate ion of sulfuric acid.

Interaction with oxides:

CaO + H 2 SO 4 = CaSO 4 = H 2 O.

Interaction with bases:

2NaOH + H 2 SO 4 = Na 2 SO 4 + 2H 2 O.

Interaction with salts:

Na 2 CO 3 + H 2 SO 4 = Na 2 SO 4 + CO 2 + H 2 O.

Oxidative properties

Sulfuric acid oxidizes HI and HBr to free halogens:

H 2 SO 4 + 2HI = I 2 + 2H 2 O + SO 2.

Sulfuric acid removes chemically bound water from organic compounds containing hydroxyl groups. Dehydration of ethyl alcohol in the presence of concentrated sulfuric acid produces ethylene:

C 2 H 5 OH = C 2 H 4 + H 2 O.

The charring of sugar, cellulose, starch and other carbohydrates upon contact with sulfuric acid is also explained by their dehydration:

C 6 H 12 O 6 + 12H 2 SO 4 = 18H 2 O + 12SO 2 + 6CO 2.