In redox processes, sulfur dioxide can be both an oxidizing agent and a reducing agent because the atom in this compound has an intermediate oxidation state of +4.

How does the oxidizing agent SO 2 react with stronger reducing agents, for example with:

SO 2 + 2H 2 S \u003d 3S ↓ + 2H 2 O

How does the reducing agent SO 2 react with stronger oxidizing agents, for example with in the presence of a catalyst, with, etc.:

2SO 2 + O 2 \u003d 2SO 3

SO 2 + Cl 2 + 2H 2 O \u003d H 2 SO 3 + 2HCl

Receipt

1) Sulfur dioxide is formed during the combustion of sulfur:

2) In industry, it is obtained by firing pyrite:

3) In the laboratory, sulfur dioxide can be obtained:

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

Application

Sulfur dioxide is widely used in the textile industry for bleaching various products. Moreover, it is used in agriculture for the destruction of harmful microorganisms in greenhouses and cellars. In large quantities, SO 2 is used to produce sulfuric acid.

Sulfur oxide (VI) – SO 3 (sulfuric anhydride)

Sulfuric anhydride SO 3 is a colorless liquid, which at temperatures below 17 ° C turns into a white crystalline mass. It absorbs moisture very well (hygroscopic).

Chemical properties

Acid-base properties

How a typical acid oxide sulfuric anhydride interacts:

SO 3 + CaO = CaSO 4

c) with water:

SO 3 + H 2 O \u003d H 2 SO 4

A special property of SO 3 is its ability to dissolve well in sulfuric acid. A solution of SO 3 in sulfuric acid is called oleum.

Oleum formation: H 2 SO 4 + n SO 3 \u003d H 2 SO 4 ∙ n SO 3

redox properties

Sulfur oxide (VI) is characterized by strong oxidizing properties (usually reduced to SO 2):

3SO 3 + H 2 S \u003d 4SO 2 + H 2 O

Getting and using

Sulfuric anhydride is formed during the oxidation of sulfur dioxide:

2SO 2 + O 2 \u003d 2SO 3

AT pure form sulfuric anhydride has no practical value. It is obtained as an intermediate in the production of sulfuric acid.

H2SO4

Mention of sulfuric acid is first found among Arab and European alchemists. It was obtained by calcining iron sulfate (FeSO 4 ∙ 7H 2 O) in air: 2FeSO 4 \u003d Fe 2 O 3 + SO 3 + SO 2 or a mixture with: 6KNO 3 + 5S \u003d 3K 2 SO 4 + 2SO 3 + 3N 2, and the emitted vapors of sulfuric anhydride were condensed. Absorbing moisture, they turned into oleum. Depending on the method of preparation, H 2 SO 4 was called vitriol oil or sulfur oil. In 1595, the alchemist Andreas Libavius ​​established the identity of both substances.

For a long time, vitriol oil did not find wide application. Interest in it greatly increased after the 18th century. Indigo carmine, a stable blue dye, was discovered. The first factory for the production of sulfuric acid was founded near London in 1736. The process was carried out in lead chambers, at the bottom of which water was poured. A molten mixture of saltpeter with sulfur was burned in the upper part of the chamber, then air was let in there. The procedure was repeated until an acid of the required concentration was formed at the bottom of the container.

In the 19th century the method was improved: instead of saltpeter, nitric acid was used (it gives when decomposed in the chamber). To return nitrous gases to the system, special towers were designed, which gave the name to the whole process - the tower process. Factories operating according to the tower method still exist today.

Sulfuric acid is a heavy oily liquid, colorless and odorless, hygroscopic; dissolves well in water. When concentrated sulfuric acid is dissolved in water, a large amount of heat is released, so it must be carefully poured into water (and not vice versa!) And mix the solution.

A solution of sulfuric acid in water with an H2SO4 content of less than 70% is usually called dilute sulfuric acid, and a solution of more than 70% is called concentrated sulfuric acid.

Chemical properties

Acid-base properties

Dilute sulfuric acid exhibits all the characteristic properties of strong acids. She reacts:

H 2 SO 4 + NaOH \u003d Na 2 SO 4 + 2H 2 O

H 2 SO 4 + BaCl 2 \u003d BaSO 4 ↓ + 2HCl

The process of interaction of Ba 2+ ions with sulfate ions SO 4 2+ leads to the formation of a white insoluble precipitate BaSO 4 . it qualitative reaction to sulfate ion.

Redox properties

In dilute H 2 SO 4 , H + ions are oxidizing agents, and in concentrated H 2 SO 4 sulfate ions are SO 4 2+ . SO 4 2+ ions are stronger oxidizing agents than H + ions (see diagram).

AT dilute sulfuric acid dissolve metals that are in the electrochemical series of voltages to hydrogen. In this case, metal sulfates are formed and released:

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

Metals that are in the electrochemical series of voltages after hydrogen do not react with dilute sulfuric acid:

Cu + H 2 SO 4 ≠

concentrated sulfuric acid is a strong oxidizing agent, especially when heated. It oxidizes many, and some organic substances.

When concentrated sulfuric acid interacts with metals that are in the electrochemical series of voltages after hydrogen (Cu, Ag, Hg), metal sulfates are formed, as well as the reduction product of sulfuric acid - SO 2.

Reaction of sulfuric acid with zinc

With more active metals (Zn, Al, Mg), concentrated sulfuric acid can be reduced to free. For example, when sulfuric acid interacts with, depending on the concentration of the acid, various products of sulfuric acid reduction can simultaneously form - SO 2, S, H 2 S:

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

3Zn + 4H 2 SO 4 = 3ZnSO 4 + S↓ + 4H 2 O

4Zn + 5H 2 SO 4 = 4ZnSO 4 + H 2 S + 4H 2 O

In the cold, concentrated sulfuric acid passivates some metals, for example, and therefore it is transported in iron tanks:

Fe + H 2 SO 4 ≠

Concentrated sulfuric acid oxidizes some non-metals (, etc.), recovering to sulfur oxide (IV) SO 2:

S + 2H 2 SO 4 \u003d 3SO 2 + 2H 2 O

C + 2H 2 SO 4 \u003d 2SO 2 + CO 2 + 2H 2 O

Getting and using

In industry, sulfuric acid is obtained by contact. The acquisition process takes place in three stages:

1. Obtaining SO 2 by roasting pyrite:

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

1. Oxidation of SO 2 to SO 3 in the presence of a catalyst - vanadium (V) oxide:

2SO 2 + O 2 \u003d 2SO 3

1. Dissolution of SO 3 in sulfuric acid:

H2SO4+ n SO 3 \u003d H 2 SO 4 ∙ n SO 3

The resulting oleum is transported in iron tanks. Sulfuric acid of the required concentration is obtained from oleum by pouring it into water. This can be expressed in a diagram:

H 2 SO 4 ∙ n SO 3 + H 2 O \u003d H 2 SO 4

Sulfuric acid finds various applications in various fields of the national economy. It is used for drying gases, in the production of other acids, for the production of fertilizers, various dyes and medicines.

Salts of sulfuric acid

Most sulfates are highly soluble in water (slightly soluble CaSO 4 , even less PbSO 4 and practically insoluble BaSO 4). Some sulfates containing water of crystallization are called vitriol:

CuSO 4 ∙ 5H 2 O copper sulfate

FeSO 4 ∙ 7H 2 O ferrous sulfate

Salts of sulfuric acid have everything. Their relation to heating is special.

Sulfates of active metals ( , ) do not decompose even at 1000 ° C, while others (Cu, Al, Fe) - decompose upon slight heating into metal oxide and SO 3:

CuSO 4 \u003d CuO + SO 3

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*on the image of the record is a photograph of copper sulphate

It is one of the most famous and widespread chemical compounds . This is explained primarily by its pronounced properties. Its formula is H2SO4. It is a dibasic acid with higher sulfur +6.

Under normal conditions, sulfuric acid is an odorless and colorless liquid with oily properties. It has become quite widespread in technology and various industries.

At the moment, this substance is one of the most important and most common products. chemical industry. In nature, deposits of native sulfur are not so common, as a rule, it is found only in compounds with other substances. Sulfur extraction from various compounds, including various industrial wastes, is currently being developed. In some cases, even gases can be adapted to produce sulfur and various compounds with it.

Properties

Sulfuric acid has a detrimental effect on any. It takes water out of them very quickly, so that tissues and various compounds begin to char. 100% acid is one of the strongest, while the compound does not smoke or destroy

Reacts with all metals except lead. In concentrated form, it begins to oxidize many elements.

The use of sulfuric acid

Sulfuric acid is mainly used in the chemical industry, where nitrogen is produced on its basis, including superphosphate, which is currently considered one of the most common fertilizers. Up to several million tons of this substance are produced annually.

In metallurgy, H2SO4 is used to check the quality of the products obtained. When rolling steel, microcracks can occur; in order to detect them, the part is placed in a lead bath and etched with a 25% acid solution. After that, even the smallest cracks can be seen with the naked eye.

Before applying electroplating to the metal, it must first be prepared - cleaned and degreased. Since sulfuric acid reacts with metals, it dissolves the thinnest layer, and with it any traces of contamination are removed. In addition, the metal surface becomes rougher, which is better suited for nickel, chrome or copper plating.

Sulfuric acid is used in the processing of some ores, and a significant amount of it is required in the oil industry, where it is used mainly for the purification of various products. It is often used in the chemical industry, which is constantly evolving. As a result, additional possibilities and applications are discovered. This substance can be used for the production of lead-acid - various batteries.

Getting sulfuric acid

The main raw materials for the production of acid are sulfur and various compounds based on it. In addition, as already mentioned, the use of industrial waste for sulfur production is now developing. During oxidative roasting of sulfide ores, the off-gases contain SO2. It is adapted to produce sulfuric acid. Although in Russia the leading positions are still occupied by production based on the processing of sulfur pyrite, which is burned in furnaces. When air is blown through burning pyrites, vapors with a high SO2 content are formed. Electrostatic precipitators are used to remove other impurities and dangerous vapors. Now actively used in production different ways production of acid, and many of them are associated with the processing of waste, although the share of traditional industries is high.

Sulfuric acid is one of the strongest acids, which is an oily liquid. The chemical properties of sulfuric acid make it widely used in industry.

general description

Sulfuric acid (H 2 SO 4) has the characteristic properties of acids and is a strong oxidizing agent. It is the most active inorganic acid with a melting point of 10°C. The acid boils at 296°C with the release of water and sulfur oxide SO 3 . It is able to absorb water vapor, so it is used to dry gases.

Rice. 1. Sulfuric acid.

Sulfuric acid is produced industrially from sulfur dioxide (SO 2 ), which is formed during the combustion of sulfur or pyrites. The two main ways in which acid is formed are:

• contact (concentration 94%) - oxidation of sulfur dioxide to sulfur trioxide (SO 3) followed by hydrolysis:

  2SO 2 + O 2 → 2SO3; SO 3 + H 2 O → H 2 SO 4;

• nitrous (concentration 75%) - oxidation of sulfur dioxide with nitrogen dioxide during the interaction of water:

  SO 2 + NO 2 + H 2 O → H 2 SO 4 + NO.

A solution of SO 3 in sulfuric acid is called oleum. It is also used to produce sulfuric acid.

Rice. 2. The process of obtaining sulfuric acid.

The reaction with water promotes the release of a large amount of heat. Therefore, acid is mixed with water, and not vice versa. Water is lighter than acid and stays on the surface. If you add water to acid, the water will instantly boil, causing the acid to splatter.

Properties

Sulfuric acid forms two types of salts:

• sour - hydrosulfates (NaHSO 4 , KHSO 4);
• medium - sulfates (BaSO 4, CaSO 4).

The chemical properties of concentrated sulfuric acid are presented in the table.

Reaction	What is formed	Example
with metals	Sulfur oxide; hydrogen sulfide	With active: 2H 2 SO 4 + Mg → MgSO 4 + SO 2 + 2H 2 O With metals of medium activity: 4H 2 SO 4 + 2Cr → Cr 2 (SO 4) 3 + 4H 2 O + S; With inactive: 2H 2 SO 4 + Cu → CuSO 4 + SO 2 + 2H 2 O
with non-metals	Acid; Sulfur oxide	2P + 5H 2 SO 4 → 2H 3 PO 4 + 5SO 2 + 2H 2 O
With oxides	Sulfur oxide	Metals: H 2 SO 4 + CuO → CuSO 4 + H 2 O; Non-metals: H 2 SO 4 + CO → CO 2 + SO 2 + H 2 O
With bases		H 2 SO 4 + 2NaOH → Na 2 SO 4 + 2H 2 O
	Carbon dioxide; Acid	Na 2 CO 3 + H 2 SO 4 → Na 2 SO 4 + CO 2 + H 2 O Qualitative reaction: H 2 SO 4 + BaCl 2 → BaSO 4 (white precipitate) + 2HCl
Oxidation of complex substances	Free halogens; Sulfur oxide;	H 2 SO 4 + 2HBr → Br 2 + SO 2 + 2H 2 O; H 2 SO 4 + 2HI → I 2 + 2H 2 O + SO 2
Charring of sugars (cellulose, starch, glucose)	Sulfur oxide; Carbon dioxide;	C 6 H 12 O 6 + 12H 2 SO 4 → 18H 2 O + 12SO 2 + 6CO 2

Rice. 3. Reaction with sugar.

A dilute acid does not oxidize low-active metals that are in the electrochemical series after hydrogen. When interacting with active metals (lithium, potassium, sodium, magnesium), hydrogen is released and a salt is formed. Concentrated acid exhibits oxidizing properties with heavy, alkali and alkaline earth metals when heated. There is no reaction with gold and platinum.

Sulfuric acid (diluted and concentrated) in the cold does not interact with iron, chromium, aluminum, titanium, nickel. Due to the passivation of metals (the formation of a protective oxide film), sulfuric acid can be transported in metal tanks. Iron oxide is destroyed when heated.

What have we learned?

From the 9th grade lesson, we learned about the properties of sulfuric acid. It is a powerful oxidizing agent that reacts with metals, non-metals, organic compounds, salts, bases, oxides. When interacting with water, heat is released. Sulfuric acid is obtained from sulfur oxide. Concentrated acid without heating does not interact with some metals, which allows the acid to be transported in a metal container.

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Sulfurous acid is an inorganic, dibasic, unstable acid of medium strength. An unstable compound, known only in aqueous solutions at a concentration of not more than six percent. When trying to isolate pure sulfurous acid, it decomposes into sulfur oxide (SO2) and water (H2O). For example, when sulfuric acid (H2SO4) in concentrated form is exposed to sodium sulfite (Na2SO3), sulfur oxide (SO2) is released instead of sulfurous acid. This is what the reaction looks like:

Na2SO3 (sodium sulfite) + H2SO4 (sulfuric acid) = Na2SO4 (sodium sulfate) + SO2 (sulfur dioxide) + H2O (water)

Sulfuric acid solution

When storing it, it is necessary to exclude air access. Otherwise, sulfurous acid, slowly absorbing oxygen (O2), will turn into sulfuric acid.

2H2SO3 (sulphurous acid) + O2 (oxygen) = 2H2SO4 (sulfuric acid)

Sulfuric acid solutions have a rather specific smell (reminiscent of the smell left after lighting a match), the presence of which can be explained by the presence of sulfur oxide (SO2), which is not chemically bound by water.

Chemical properties of sulfurous acid

1. H2SO3) can be used as a reducing agent or an oxidizing agent.

H2SO3 is a good reducing agent. With its help, it is possible to obtain hydrogen halides from free halogens. For example:

H2SO3 (sulphurous acid) + Cl2 (chlorine, gas) + H2O (water) = H2SO4 (sulfuric acid) + 2HCl (hydrochloric acid)

But when interacting with strong reducing agents, this acid will act as an oxidizing agent. An example is the reaction of sulfurous acid with hydrogen sulfide:

H2SO3 (sulphurous acid) + 2H2S (hydrogen sulfide) = 3S (sulfur) + 3H2O (water)

2. The chemical compound we are considering forms two - sulfites (medium) and hydrosulfites (acid). These salts are reducing agents, as is (H2SO3)sulphurous acid. When they are oxidized, salts of sulfuric acid are formed. When sulfites of active metals are calcined, sulfates and sulfides are formed. This is a self-oxidation-self-healing reaction. For example:

4Na2SO3 (sodium sulfite) = Na2S + 3Na2SO4 (sodium sulfate)

Sulfites of sodium and potassium (Na2SO3 and K2SO3) are used in dyeing fabrics in the textile industry, in bleaching metals, and also in photography. Calcium hydrosulfite (Ca(HSO3)2), which exists only in solution, is used to process wood material into special sulfite pulp. It is then made into paper.

The use of sulfuric acid

Sulfuric acid is used:

For bleaching wool, silk, wood pulp, paper and other similar materials that cannot withstand bleaching with stronger oxidizing agents (eg chlorine);

As a preservative and antiseptic, for example, to prevent the fermentation of grain in the production of starch or to prevent the fermentation process in wine barrels;

To preserve food, for example, when canning vegetables and fruits;

In processing into sulfite pulp, from which paper is then obtained. In this case, a solution of calcium hydrosulfite (Ca(HSO3)2) is used, which dissolves lignin, a special substance that binds cellulose fibers.

Sulfuric acid: obtaining

This acid can be obtained by dissolving sulfur dioxide (SO2) in water (H2O). You will need concentrated sulfuric acid (H2SO4), copper (Cu) and a test tube. Action algorithm:

1. Carefully pour concentrated sulfuric acid into a test tube and then place a piece of copper into it. Heat up. The following reaction occurs:

Cu (copper) + 2H2SO4 (sulfuric acid) = CuSO4 (sulphur sulfate) + SO2 (sulfur dioxide) + H2O (water)

2. The flow of sulfur dioxide must be directed into a test tube with water. When it dissolves, it partially occurs with water, as a result of which sulfurous acid is formed:

SO2 (sulfur dioxide) + H2O (water) = H2SO3

So, by passing sulfur dioxide through water, sulfurous acid can be obtained. It is worth considering that this gas has an irritating effect on the membranes of the respiratory tract, can cause inflammation, as well as loss of appetite. With prolonged inhalation, loss of consciousness is possible. This gas must be handled with the utmost care and attention.

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 the oxidation of sulfur dioxide (SO2) by the contact method.

At a temperature of + 10.5 ° C, sulfuric acid turns into a frozen glassy crystalline mass, greedily, like a sponge, absorbing moisture from environment. In industry and chemistry, sulfuric acid is one of the main chemical compounds and occupies a leading position in terms of production in tons. That is why sulfuric acid is called the "blood of chemistry". Sulfuric acid is used to make fertilizers medications, other acids, large , fertilizers and much more.

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 massive release of heat.
2. H2SO4 is a strong acid.
3. Sulfuric acid is called monohydrate - it contains 1 mol of H2O (water) per 1 mol of SO3. Because of its impressive hygroscopic properties, it is used to extract moisture from gases.
4. Boiling point - 330 ° C. In this case, the acid is decomposed into SO3 and water. Density - 1.84. Melting point - 10.3 ° C /.
5. Concentrated sulfuric acid is a powerful oxidizing agent. To start the 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 differently with metals. In a dilute state, sulfuric acid is capable of oxidizing all metals that are in the series of voltages to hydrogen. An exception is made as 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 series of voltages, and silver too.
7. Sulfuric acid forms two types of salts: acidic (hydrosulfates) and medium (sulfates)
8. H2SO4 actively reacts with organic matter and non-metals, some of which it can turn into coal.
9. Sulfuric anhydrite is perfectly soluble 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 water in a small stream, and not vice versa. This is done to avoid boiling water and splashing acid.

Concentrated and dilute sulfuric acids

Concentrated solutions of sulfuric acid include solutions from 40%, capable of dissolving silver or palladium.

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

Getting sulfuric acid

The production of sulfuric acid on an industrial scale was launched in the 15th century, but at that time it was called "vitriol". If earlier humanity consumed only a few tens of liters of sulfuric acid, then in 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. nitrous method
3. Other Methods

Let's talk in detail about each of them.

contact production method

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

• It turns out a product that satisfies the needs of the maximum number of consumers.
• During production, harm to the environment is reduced.

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

• pyrite (sulfur pyrites);
• sulfur;
• vanadium oxide (this substance causes the role of 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, pyrite is subjected to grinding, which allows, due to an increase in the area of ​​​​contact of the active substances, to accelerate 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. They are removed at the end of the process.

The production part is divided into several stages:

1. After crushing, pyrite is cleaned and sent to the furnace - where it is fired at temperatures up to 800 ° C. According to the principle of counterflow, air is supplied to the chamber from below, and this ensures that the pyrite is in a suspended state. Today, this process takes a few seconds, but earlier it took several hours to fire. During the roasting process, wastes appear in the form of iron oxide, which are removed and subsequently transferred to the enterprises of the metallurgical industry. During firing, water vapor, O2 and SO2 gases are released. When the purification from water vapor and the smallest impurities is completed, pure sulfur oxide and oxygen are obtained.
2. In the second stage, an exothermic reaction takes place under pressure using a vanadium catalyst. The start of the reaction starts when the temperature reaches 420 °C, but it can be increased to 550 °C in order 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: the absorption of SO3 in the absorption tower, during which the 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 user.

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 that use the exhaust steam to generate additional electricity.

Nitrous process for the production of sulfuric acid

Despite the advantages of the contact method of production, 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, sulfur dioxide acts as the initial substance, both in the contact and in the nitrous method. It is obtained specifically for these purposes by burning sulfur or roasting sulfurous metals.

The conversion of sulfur dioxide into sulfurous acid consists in 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 directly react with oxygen, therefore, with the nitrous method, the oxidation of sulfur dioxide is carried out using nitrogen oxides. Higher oxides of nitrogen (we are talking about nitrogen dioxide NO2, nitrogen trioxide NO3) in this process are reduced to nitric oxide NO, which is subsequently oxidized again with 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:

• It turns out 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.
• The possibility of processing SO2 at 100%.
• Simplicity of hardware design.

Major Russian Sulfuric Acid Plants

The annual production of H2SO4 in our country is calculated in six figures - 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".

Crimean Titan, the largest producer of titanium dioxide in Eastern Europe, operates in Armyansk, Crimea. In addition, the plant is engaged in the production of sulfuric acid, mineral fertilizers, iron sulphate, etc.

sulfuric acid various kinds produced by many factories. 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 Production Association, etc.

Sulfuric acid of high purity is produced by UCC Shchekinoazot, Component-Reaktiv.

Spent sulfuric acid can be bought at the plants ZSS, HaloPolymer Kirovo-Chepetsk.

Commercial sulfuric acid producers 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 plants.

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

Scope of sulfuric acid

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

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

• Sulfuric acid is used in huge volumes for the production of mineral fertilizers, and it takes about 40% of the total tonnage. For this reason, plants producing H2SO4 are being built next to fertilizer plants. These are ammonium sulfate, superphosphate, etc. In their production, sulfuric acid is taken in its pure form (100% concentration). It will take 600 liters of H2SO4 to produce a ton of ammophos or superphosphate. These fertilizers are mostly used in agriculture.
• H2SO4 is used to make explosives.
• Purification of petroleum products. To obtain kerosene, gasoline, mineral oils, hydrocarbon purification is required, which occurs with the use of sulfuric acid. In the process of refining oil for the purification of 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 is used in metallurgy to remove scale and rust from wire, sheet metal, as well as for the recovery of aluminum in the production of non-ferrous metals. Before covering metal surfaces copper, chromium or nickel, the surface is etched with sulfuric acid.
• In the manufacture of medicines.
• in the production of paints.
• in the chemical industry. H2SO4 is used in the production of detergents, ethyl detergent, insecticides, etc., and these processes are impossible without it.
• To obtain other known acids, organic and inorganic compounds used for industrial purposes.

Sulfuric acid salts and their uses

The most important salts of sulfuric acid are:

• 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, 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. With gypsum, when heated to a temperature of 150 - 170 ° C, partial dehydration occurs, as a result of which burnt gypsum, known to us as alabaster, is obtained. Kneading alabaster with water to the consistency of 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 molds are made from it. In plastering work, alabaster is indispensable as a binder. Patients of trauma departments are given special fixing solid bandages - they are made on the basis of alabaster.
• Ferrous vitriol FeSO4 7H2O is used for the preparation of ink, impregnation of wood, and also in agricultural activities for the destruction of pests.
• Alum KCr(SO4)2 12H2O, KAl(SO4)2 12H2O, etc. are used in the production of paints and the leather industry (tanning).
• Many of you know copper sulfate CuSO4 5H2O firsthand. It is an active assistant in agriculture in the fight against plant diseases and pests - aqueous solution CuSO4 · 5H2O is treated with grain and sprayed with plants. It is also used to prepare some mineral paints. And in everyday life it is used to remove mold from the walls.
• Aluminum sulfate - it is used in the pulp and paper industry.

Sulfuric acid in dilute form is used as an electrolyte in lead-acid 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 (other oleum formulas can also be found).

Amazing fact! Oleum is more reactive 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 sphere of use of the “queen of acids” is truly large-scale, and it is difficult to tell about all the ways in which it is used in industry. It is also used as an emulsifier in the food industry, for water treatment, in the synthesis of explosives, and for many other purposes.

History of sulfuric acid

Who among us has never heard of blue vitriol? So, it was studied in antiquity, and in some works the beginnings new era scientists discussed the origin of vitriol and their properties. Vitriol was studied by the Greek physician Dioscorides, the Roman explorer of nature Pliny the Elder, and in their writings they wrote about the ongoing experiments. For medical purposes, various vitriol substances were used by the ancient healer Ibn Sina. How vitriol was used in metallurgy, was said in the works of alchemists 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 XIII century. At that time, the composition of alum and the essence of the process were not known to alchemists, but already in the 15th century, they began to engage in the chemical synthesis of sulfuric acid purposefully. 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 "vitriol oil", but then the name changed to vitriol.

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

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

In Russia, vitriol appeared 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 strong large lead-lined chambers, which were cheaper than glass containers.

In industry, this method held positions for almost 200 years, and 65% sulfuric acid was obtained in the 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, for example, of dyes.

In the early 19th century, new methods were discovered for oxidizing sulfur dioxide to 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 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 was called the nitrous method for producing sulfuric acid.

It was not until 1831 that the British acetic acid dealer Peregrine Philips patented an economical process for the production of sulfur oxide (VI) and concentrated sulfuric acid, and it is he who is today known to the world as a contact method for obtaining it.

The production of superphosphate 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 hazardous chemicals, and upon contact with the skin causes severe burns. In addition, it can cause chemical poisoning of a person. If certain rules are not followed during transportation, then sulfuric acid, due to its explosive nature, can cause a lot of harm to both people and the environment.

Sulfuric acid has been assigned a hazard class 8 and transportation must be carried out by specially trained and trained professionals. An important condition for the delivery of sulfuric acid is compliance with specially developed Rules for the transport of dangerous goods.

Transportation by road is carried out according to the following rules:

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

Dangerous properties of sulfuric acid for humans

Sulfuric acid is increased danger for the human body. Its toxic effect occurs not only by direct contact with the skin, but by inhalation of its vapors, when sulfur dioxide is released. The hazard applies to:

• respiratory system;
• Integuments;
• Mucous membranes.

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

Important! As you know, when acid comes into contact with the skin, severe burns occur. No less dangerous is poisoning with sulfuric acid vapors. A 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 on the skin, a severe burn appears, which does not heal well. If the burn is impressive 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, it is problematic to “experience for yourself” the toxic effect of acid in ordinary life. Most often, acid poisoning occurs due to neglect of industrial safety when working with a solution.

Mass poisoning with sulfuric acid vapor can occur due to technical problems in production or negligence, and a massive release into the atmosphere occurs. To prevent such situations, special services are working, the task of which is to control the functioning of production where hazardous acid is used.

What are the symptoms of sulfuric acid intoxication?

If the acid was ingested:

• Pain in the region of the digestive organs.
• Nausea and vomiting.
• Violation of the stool, as a result of severe intestinal disorders.
• Strong secretion of saliva.
• Due to the toxic effects on the kidneys, the urine becomes reddish.
• Swelling of the larynx and throat. There are wheezing, hoarseness. This can lead to death from suffocation.
• Brown spots appear on the gums.
• The skin turns blue.

With a burn of the skin, there can be all the complications inherent in a burn disease.

When poisoning in pairs, the following picture is observed:

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

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

First aid and therapeutic procedures for damage by sulfuric acid

Proceed as follows when in contact with sulfuric acid:

• Call first ambulance. If the liquid got inside, then do a gastric lavage with warm water. After that, in small sips you will need to drink 100 grams of sunflower or olive oil. 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 the eyes, rinse them with running water, and then drip with a solution of dicaine and novocaine.
• If acid gets on the skin, the burned area should be washed well under running water and bandaged with soda. 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 far as possible.

In a hospital setting, treatment will depend on the area of ​​the burn and the degree of poisoning. Anesthesia is carried out only with novocaine. In order to avoid the development of an infection in the affected area, a course of antibiotic therapy is selected for the patient.

In gastric bleeding, plasma is injected or blood is transfused. The source of bleeding can be removed surgically.

1. Sulfuric acid in its pure 100% form is found in nature. For example, in Italy, Sicily in the Dead Sea, you can see a unique phenomenon - sulfuric acid seeps right from the bottom! And this is what happens: pyrite from 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 up to it!
2. After large volcanic eruptions, drops of sulfuric acid can often be found in the earth's atmosphere, and in such cases, the "culprit" can bring negative consequences for the environment and cause serious climate change.
3. Sulfuric acid is an active water absorber, so it is used as a gas dryer. In the old days, in order to prevent windows from fogging up in the rooms, this acid was poured into jars and placed between the panes of window openings.
4. Sulfuric acid is the main cause of acid rain. main reason Acid rain is air pollution with sulfur dioxide, and when dissolved in water, it forms sulfuric acid. In turn, sulfur dioxide is emitted when fossil fuels are burned. In acid rains studied in recent years, the content of nitric acid. The reason for this phenomenon is the reduction of sulfur dioxide emissions. Despite this fact, sulfuric acid remains the main cause of acid rain.

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

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. The most interesting thing happens next. The mass begins to grow rapidly and climb out of the flask. At the output, we get a proud substance, similar to porous charcoal, exceeding the original volume by 3-4 times.

The author of the video suggests comparing the reaction of Coca-Cola with hydrochloric acid and sulfuric acid. When mixing Coca-Cola 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 gets on toilet paper. Toilet paper is made from cellulose. When acid enters, cellulose molecules instantly break down with the release of free carbon. Similar charring can be observed when acid gets on the 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, lights up and explodes, cutting into pieces.

In the next experiment, when sulfuric acid hits a match, it flares up. In the second part of the experiment, aluminum foil is immersed with acetone and a match inside. There is an instantaneous heating of the foil with the release of a huge amount of smoke and its complete dissolution.

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

We categorically do not advise to carry out all the above experiments at home. Sulfuric acid is a very corrosive and toxic substance. Such experiments must be carried out in special rooms that are equipped with forced ventilation. The gases released in reactions with sulfuric acid are highly toxic and can cause damage to the respiratory tract and poison the body. In addition, similar experiments are carried out in the means personal protection skin and respiratory organs. Take care of yourself!