The chemical formula of sulfuric acid is h2so4. Sulfuric acid and its chemical properties. Physical properties of sulfuric acid

Structural formula

True, empirical, or gross formula: H2SO4

Chemical composition of sulfuric acid

Molecular weight: 98.076

Sulphuric acid H 2 SO 4 is a strong dibasic acid, corresponding to the highest oxidation state of sulfur (+6). Under normal conditions, concentrated sulfuric acid is a heavy oily liquid, colorless and odorless, with a sour "coppery" taste. In technology, sulfuric acid is called its mixtures with both water and sulfuric anhydride SO 3. If the molar ratio of SO 3: H 2 O is less than 1, then this is an aqueous solution of sulfuric acid, if more than 1 - a solution of SO 3 in sulfuric acid (oleum).

Name

In the XVIII-XIX centuries, sulfur for gunpowder was produced from sulfur pyrites (pyrite) at vitriol plants. Sulfuric acid at that time was called "vitriol oil" (as a rule it was a crystalline hydrate, resembling oil in consistency), the origin of the name of its salts (or rather, crystalline hydrates) - vitriol, is obviously from here.

Getting sulfuric acid

Industrial (contact) method

In industry, sulfuric acid is produced by the oxidation of sulfur dioxide (sulphurous gas produced during the combustion of sulfur or sulfur pyrite) to trioxide (sulfuric anhydride), followed by the interaction of SO 3 with water. The sulfuric acid obtained by this method is also called contact (concentration 92-94%).

Nitrous (tower) method

Previously, sulfuric acid was obtained exclusively by the nitrous method in special towers, and the acid was called tower acid (75% concentration). The essence of this method is the oxidation of sulfur dioxide with nitrogen dioxide in the presence of water.

Another way

In those rare cases when hydrogen sulfide (H 2 S) displaces sulfate (SO 4 -) from salt (with metals Cu, Ag, Pb, Hg), sulfuric acid is a by-product. Sulfides of these metals have the highest strength, as well as a distinctive black color.

Physical and physical Chemical properties

A very strong acid, at 18 o C pK a (1) \u003d -2.8, pK a (2) \u003d 1.92 (K z 1.2 10 -2); bond lengths in the molecule S=O 0.143 nm, S-OH 0.154 nm, angle HOSOH 104°, OSO 119°; boils, forming an azeotropic mixture (98.3% H 2 SO 4 and 1.7% H 2 O with a boiling point of 338.8 ° C). Sulfuric acid, corresponding to 100% H 2 SO 4 content, has a composition (%): H 2 SO 4 99.5, HSO 4 - - 0.18, H 3 SO 4 + - 0.14, H 3 O + - 0.09, H 2 S 2 O 7 , - 0.04, HS 2 O 7 - - 0.05. Miscible with water and SO 3 in all proportions. In aqueous solutions, sulfuric acid almost completely dissociates into H 3 O + , HSO 3 + , and 2HSO 4 - . Forms hydrates H 2 SO 4 nH 2 O, where n = 1, 2, 3, 4 and 6.5.

Oleum

Solutions of sulfuric anhydride SO 3 in sulfuric acid are called oleum, they form two compounds H 2 SO 4 SO 3 and H 2 SO 4 2SO 3. Oleum also contains pyrosulfuric acids. The boiling point of aqueous solutions of sulfuric acid increases with an increase in its concentration and reaches a maximum at a content of 98.3% H 2 SO 4 . The boiling point of oleum decreases with increasing SO 3 content. With an increase in the concentration of aqueous solutions of sulfuric acid, the total vapor pressure over the solutions decreases and at a content of 98.3% H 2 SO 4 reaches a minimum. With an increase in the concentration of SO 3 in oleum, the total vapor pressure above it increases. The vapor pressure over aqueous solutions of sulfuric acid and oleum can be calculated by the equation:

log p=A-B/T+2.126

the values of the coefficients A and B depend on the concentration of sulfuric acid. Steam over aqueous solutions of sulfuric acid consists of a mixture of water vapor, H 2 SO 4 and SO 3, while the composition of the vapor differs from the composition of the liquid at all concentrations of sulfuric acid, except for the corresponding azeotropic mixture. As the temperature rises, dissociation increases. The oleum H 2 SO 4 ·SO 3 has the maximum viscosity; with increasing temperature, η decreases. Electrical resistance sulfuric acid is minimal at a concentration of SO 3 and 92% H 2 SO 4 and maximum at a concentration of 84 and 99.8% H 2 SO 4. For oleum, the minimum ρ is at a concentration of 10% SO 3 . As the temperature rises, the ρ of sulfuric acid increases. The dielectric constant 100% sulfuric acid 101 (298.15 K), 122 (281.15 K); cryoscopic constant 6.12, ebulioscopic constant 5.33; the diffusion coefficient of sulfuric acid vapor in air varies with temperature; D = 1.67 10⁻⁵T3/2 cm²/s.

Chemical properties

Sulfuric acid in concentrated form when heated is a fairly strong oxidizing agent. Oxidizes HI and partially HBr to free halogens. Oxidizes many metals (exceptions: Au, Pt, Ir, Rh, Ta.). In this case, concentrated sulfuric acid is reduced to SO 2 . In the cold in concentrated sulfuric acid, Fe, Al, Cr, Co, Ni, Ba are passivated and the reactions do not proceed. With the strongest reducing agents, concentrated sulfuric acid is reduced to S and H 2 S. Concentrated sulfuric acid absorbs water vapor, so it is used to dry gases, liquids, and solids, for example, in desiccators. However, concentrated H 2 SO 4 is partially reduced by hydrogen, which is why it cannot be used for drying it. Splitting water from organic compounds and leaving black carbon (coal) at the same time, concentrated sulfuric acid leads to the carbonization of wood, sugar and other substances. Diluted H 2 SO 4 interacts with all metals that are in the electrochemical series of voltages to the left of hydrogen with its release. Oxidizing properties for dilute H 2 SO 4 are uncharacteristic. Sulfuric acid forms two series of salts: medium - sulfates and acidic - hydrosulfates, as well as esters. Peroxomonosulfuric (or Caro's acid) H 2 SO 5 and peroxodisulfuric H 2 S 2 O 8 acids are known. Sulfuric acid also reacts with basic oxides to form sulfate and water. In metalworking plants, a sulfuric acid solution is used to remove a layer of metal oxide from the surface of metal products that are subjected to strong heating during the manufacturing process. So, iron oxide is removed from the surface of sheet iron by the action of a heated solution of sulfuric acid. A qualitative reaction to sulfuric acid and its soluble salts is their interaction with soluble barium salts, which forms a white precipitate of barium sulfate, insoluble in water and acids, for example.

Application

Sulfuric acid is used:

in the processing of ores, especially in the extraction of rare elements, including uranium, iridium, zirconium, osmium, etc.;
in the production of mineral fertilizers;
as an electrolyte in lead batteries;
to obtain various mineral acids and salts;
in the production of chemical fibers, dyes, smoke-forming and explosive substances;
in the oil, metalworking, textile, leather and other industries;
in the food industry - registered as a food additive E513 (emulsifier);
in industrial organic synthesis in reactions:

dehydration (obtaining diethyl ether, esters);
hydration (ethanol from ethylene);
sulfonation (synthetic detergents and intermediates in the production of dyes);
alkylation (obtaining isooctane, polyethylene glycol, caprolactam), etc.
For the recovery of resins in filters in the production of distilled water.

World production of sulfuric acid approx. 160 million tons per year. The largest consumer of sulfuric acid is the production of mineral fertilizers. For P 2 O 5 phosphate fertilizers, 2.2-3.4 times more sulfuric acid is consumed by mass, and for (NH 4) 2 SO 4 sulfuric acid 75% of the mass of consumed (NH 4) 2 SO 4. Therefore, sulfuric acid plants tend to be built in conjunction with plants for the production of mineral fertilizers.

Historical information

Sulfuric acid has been known since antiquity, occurring in nature in a free form, for example, in the form of lakes near volcanoes. Perhaps the first mention of acid gases obtained by calcining alum or iron sulfate "green stone" is found in writings attributed to the Arab alchemist Jabir ibn Hayyan. In the 9th century, the Persian alchemist Ar-Razi, calcining a mixture of iron and copper sulfate (FeSO 4 7H 2 O and CuSO 4 5H 2 O), also obtained a solution of sulfuric acid. This method was perfected by the European alchemist Albert Magnus, who lived in the 13th century. Scheme for the production of sulfuric acid from ferrous sulfate - thermal decomposition of iron (II) sulfate, followed by cooling the mixture. The works of the alchemist Valentine (XIII century) describe a method for producing sulfuric acid by absorbing gas (sulphuric anhydride) released by burning a mixture of sulfur and saltpeter powders with water. Subsequently, this method formed the basis of the so-called. "chamber" method, carried out in small chambers lined with lead, which does not dissolve in sulfuric acid. In the USSR, such a method existed until 1955. Alchemists of the 15th century also knew a method for obtaining sulfuric acid from pyrite - sulfur pyrite, a cheaper and more common raw material than sulfur. Sulfuric acid was produced in this way for 300 years, in small quantities in glass retorts. Subsequently, due to the development of catalysis, this method replaced the chamber method for the synthesis of sulfuric acid. Currently, sulfuric acid is produced by catalytic oxidation (on V 2 O 5) of sulfur oxide (IV) to sulfur oxide (VI), and subsequent dissolution of sulfur oxide (VI) in 70% sulfuric acid to form oleum. In Russia, the production of sulfuric acid was first organized in 1805 near Moscow in the Zvenigorod district. In 1913, Russia ranked 13th in the world in the production of sulfuric acid.

additional information

The smallest droplets of sulfuric acid can form in the middle and upper atmosphere as a result of the reaction of water vapor and volcanic ash containing large amounts of sulfur. The resulting suspension, due to the high albedo of sulfuric acid clouds, makes it difficult for sunlight to reach the surface of the planet. Therefore (and also as a result of a large number of tiny particles of volcanic ash in the upper atmosphere, which also make it difficult for sunlight to reach the planet), significant climate changes can occur after especially strong volcanic eruptions. For example, as a result of the eruption of the Ksudach volcano (Kamchatka Peninsula, 1907), an increased concentration of dust in the atmosphere persisted for about 2 years, and characteristic silvery clouds of sulfuric acid were observed even in Paris. The explosion of the Pinatubo volcano in 1991, which sent 3 10 7 tons of sulfur into the atmosphere, led to the fact that 1992 and 1993 were much colder than 1991 and 1994.

Standards

Sulfuric acid technical GOST 2184-77
Sulfuric acid battery. Specifications GOST 667-73
Sulfuric acid of special purity. Specifications GOST 1422-78
Reagents. Sulfuric acid. Specifications GOST 4204-77

Physical Properties sulfuric acid:
Heavy oily liquid ("vitriol");
density 1.84 g/cm3; non-volatile, highly soluble in water - with strong heating; t°pl. = 10.3°C, bp \u003d 296 ° C, very hygroscopic, has water-removing properties (charring of paper, wood, sugar).

The heat of hydration is so great that the mixture may boil, splatter 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 be on the surface of the acid, where all the heat released will be concentrated.

Industrial production of sulfuric acid (contact method):

1) 4FeS 2 + 11O 2 → 2Fe 2 O 3 + 8SO 2

2) 2SO 2 + O 2 V 2 O 5 → 2SO 3

3) nSO 3 + H 2 SO 4 → H 2 SO 4 nSO 3 (oleum)

Crushed purified wet pyrite (sulfur pyrite) is poured from above into the kiln for firing in " fluidized bed". From below (counterflow principle) air enriched with oxygen is passed through.
Furnace gas comes out of the furnace, the composition of which is: SO 2, O 2, water vapor (pyrite was wet) and the smallest particles of cinder (iron oxide). The gas is purified from impurities of solid particles (in a cyclone and electrostatic precipitator) and water vapor (in a drying tower).
In the contact apparatus, sulfur dioxide is oxidized using a V 2 O 5 catalyst (vanadium pentoxide) to increase the reaction rate. The process of oxidation of one oxide to another is reversible. Therefore, the optimal conditions for the course of the direct reaction are selected - increased pressure (because the direct reaction proceeds with a decrease in the total volume) and a temperature not higher than 500 C (because the reaction is exothermic).

In the absorption tower, sulfur oxide (VI) is absorbed by concentrated sulfuric acid.
Water absorption is not used, because sulfur oxide dissolves in water with the release of a large amount of heat, so the resulting sulfuric acid boils and turns into steam. In order to avoid the formation of sulfuric acid mist, use 98% concentrated sulfuric acid. Sulfur oxide dissolves very well in such an acid, forming oleum: H 2 SO 4 nSO 3

Chemical properties of sulfuric acid:

H 2 SO 4 is a strong dibasic acid, one of the strongest mineral acids, because of the high polarity, the H - O bond is easily broken.

1) Sulfuric acid dissociates in aqueous solution , forming a hydrogen ion and an acid residue:
H 2 SO 4 \u003d H + + HSO 4 -;
HSO 4 - \u003d H + + SO 4 2-.
Summary Equation:
H 2 SO 4 \u003d 2H + + SO 4 2-.

2) The interaction of sulfuric acid with metals:
Dilute sulfuric acid only dissolves metals in the voltage series to the left of hydrogen:
Zn 0 + H 2 +1 SO 4 (razb) → Zn +2 SO 4 + H 2

3) Sulfuric acid interactionwith basic oxides:
CuO + H 2 SO 4 → CuSO 4 + H 2 O

4) The interaction of sulfuric acid withhydroxides:
H 2 SO 4 + 2NaOH → Na 2 SO 4 + 2H 2 O
H 2 SO 4 + Cu(OH) 2 → CuSO 4 + 2H 2 O

5) Exchange reactions with salts:
BaCl 2 + H 2 SO 4 → BaSO 4 ↓ + 2HCl
The formation of a white precipitate of BaSO 4 (insoluble in acids) is used to detect sulfuric acid and soluble sulfates ( qualitative reaction to the sulfate ion).

Special properties of concentrated H 2 SO 4:

1) concentrated sulfuric acid is strong oxidizing agent ; when interacting with metals (except Au, Pt) recover to S +4 O 2 , S 0 or H 2 S -2 depending on the activity of the metal. Without heating, it does not react with Fe, Al, Cr - passivation. When interacting with metals with variable valence, the latter are oxidized to higher oxidation states than in the case of a dilute acid solution: Fe0→ Fe 3+ , Cr 0→ Cr 3+ , Mn 0→Mn4+,sn 0→ sn 4+

active metal

8 Al + 15 H 2 SO 4 (conc.) → 4Al 2 (SO 4) 3 + 12H 2 O + 3 H 2 S
4│2Al 0 – 6 e- → 2Al 3+ - oxidation
3│ S 6+ + 8e → S 2– restoration

4Mg+ 5H 2 SO 4 → 4MgSO 4 + H 2 S + 4H 2 O

Medium activity metal

2Cr + 4 H 2 SO 4 (conc.) → Cr 2 (SO 4) 3 + 4 H 2 O + S
1│ 2Cr 0 - 6e → 2Cr 3+ - oxidation
1│ S 6+ + 6e → S 0 - restoration

Metal inactive

2Bi + 6H 2 SO 4 (conc.) → Bi 2 (SO 4) 3 + 6H 2 O + 3 SO2
1│ 2Bi 0 - 6e → 2Bi 3+ - oxidation
3│ S 6+ + 2e →S 4+ - recovery

2Ag + 2H 2 SO 4 → Ag 2 SO 4 + SO 2 + 2H 2 O

2) Concentrated sulfuric acid oxidizes some non-metals, as a rule, to the maximum oxidation state, it itself is reduced toS+4O2:

C + 2H 2 SO 4 (conc) → CO 2 + 2SO 2 + 2H 2 O

S+ 2H 2 SO 4 (conc) → 3SO 2 + 2H 2 O

2P+ 5H 2 SO 4 (conc) → 5SO 2 + 2H 3 PO 4 + 2H 2 O

3) Oxidation of complex substances:
Sulfuric acid oxidizes HI and HBr to free halogens:
2 KBr + 2H 2 SO 4 \u003d K 2 SO 4 + SO 2 + Br 2 + 2H 2 O
2 KI + 2H 2 SO 4 \u003d K 2 SO 4 + SO 2 + I 2 + 2H 2 O
Concentrated sulfuric acid cannot oxidize chloride ions to free chlorine, which makes it possible to obtain HCl by the exchange reaction:
NaCl + H 2 SO 4 (conc.) = NaHSO 4 + Hcl

Sulfuric acid removes chemically bound water from organic compounds containing hydroxyl groups. Dehydration of ethyl alcohol in the presence of concentrated sulfuric acid leads to the production of ethylene:
C 2 H 5 OH \u003d C 2 H 4 + H 2 O.

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 \u003d 18H 2 O + 12SO 2 + 6CO 2.

Any acid is a complex substance, the molecule of which contains one or more hydrogen atoms and an acid residue.

The formula of sulfuric acid is H2SO4. Therefore, the composition of the sulfuric acid molecule includes two hydrogen atoms and the acid 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 solidifies and turns into a crystalline mass.

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

Interaction with water

Sulfuric acid is highly soluble in water, mixing with it in any ratio. This releases a large amount of heat.

Sulfuric acid is able to absorb water vapor from the air. This property is used in industry for drying gases. 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 are charred. The fact is that carbohydrates, like water, contain both hydrogen and oxygen. Sulfuric acid robs them of these elements. 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.

dilute sulfuric acid reacts with metals like a normal acid. As a result of the reaction, a salt with an acidic residue SO4 and hydrogen are formed.

Zn + H2SO4 = ZnSO4 + H2

BUT 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, platinum group metals do not oxidize in sulfuric acid. Therefore, sulfuric acid is transported in steel tanks.

Sulfuric acid salts, which are obtained as a result of such reactions, are called sulfates. They are colorless and crystallize easily. Some of them are highly soluble in water. Only CaSO4 and PbSO4 are sparingly soluble. BaSO4 is almost insoluble in water.

Interaction with bases

The reaction of an acid with a base is called a neutralization reaction. As a result of the neutralization reaction of sulfuric acid, a salt containing the acid residue SO4 and water H2O is formed.

Examples of sulfuric acid neutralization reactions:

H2SO4 + 2 NaOH = Na2SO4 + 2 H2O

H2SO4 + CaOH = CaSO4 + 2 H2O

Sulfuric acid enters into a neutralization reaction with both soluble and insoluble bases.

Since there are two hydrogen atoms in the sulfuric acid molecule, and two bases are required to neutralize it, it belongs to dibasic acids.

Interaction with basic oxides

From school course chemistry, we know that oxides are called complex substances, which includes two chemical element, one of which is oxygen in the -2 oxidation state. 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.

With basic oxides, sulfuric acid enters into a neutralization reaction. As a result of such a reaction, as in the reaction with bases, salt and water are formed. The salt contains the acid residue SO4.

CuO + H2SO4 = CuSO4 + H2O

Salt interaction

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

H2SO4+BaCl2=BaSO4+2HCl

The use of sulfuric acid and its compounds

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

In medicine and construction, natural gypsum CaSO4 * 2H2O, calcium sulfate hydrate is 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 control pests and plant diseases.

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

Acids are chemical compounds, consisting of hydrogen atoms and acidic residues, for example, SO4, SO3, PO4, etc. They are inorganic and organic. The former include hydrochloric, phosphoric, sulfide, nitric, sulfuric acid. To the second - acetic, palmitic, formic, stearic, etc.

What is sulfuric acid

This acid consists of two hydrogen atoms and an acid residue SO4. It has the formula H2SO4.

Sulfuric acid, or, as it is also called, sulfate, refers to inorganic oxygen-containing dibasic acids. This substance is considered one of the most aggressive and chemically active. In most chemical reactions, it acts as an oxidizing agent. This acid can be used in concentrated or diluted form, in these two cases it has slightly different chemical properties.

Physical Properties

Sulfuric acid under normal conditions has liquid state, its boiling point is approximately 279.6 degrees Celsius, the freezing point, when it turns into solid crystals, is about -10 degrees for one hundred percent and about -20 for 95 percent.

Pure 100% sulfate acid is an oily liquid substance odorless and colorless, which has almost twice the density than water - 1840 kg / m3.

Chemical properties of sulfate acid

Sulfuric acid reacts with metals, their oxides, hydroxides and salts. Diluted with water in various proportions, it can behave differently, so let's take a closer look at the properties of a concentrated and weak solution of sulfuric acid separately.

concentrated sulfuric acid solution

A concentrated solution is considered to be a solution that contains from 90 percent sulfate acid. Such a solution of sulfuric acid is able to react even with inactive metals, as well as with non-metals, hydroxides, oxides, salts. The properties of such a solution of sulfate acid are similar to those of concentrated nitrate acid.

Interaction with metals

During the chemical reaction of a concentrated solution of sulfate acid with metals located to the right of hydrogen in the electrochemical series of metal voltages (that is, with not the most active), the following substances are formed: sulfate of the metal with which the interaction takes place, water and sulfur dioxide. The metals, as a result of interaction with which the listed substances are formed, include copper (cuprum), mercury, bismuth, silver (argentum), platinum and gold (aurum).

Interaction with inactive metals

With metals that are to the left of hydrogen in the voltage series, concentrated sulfuric acid behaves a little differently. As a result of such a chemical reaction, the following substances are formed: sulfate of a certain metal, hydrogen sulfide or pure sulfur and water. The metals with which such a reaction takes place also include iron (ferum), magnesium, manganese, beryllium, lithium, barium, calcium and all the others that are in the series of voltages to the left of hydrogen, except for aluminum, chromium, nickel and titanium - with them concentrated sulfate acid does not react.

Interaction with non-metals

This substance is a strong oxidizing agent, therefore it is able to participate in redox chemical reactions with non-metals, such as, for example, carbon (carbon) and sulfur. As a result of such reactions, water is necessarily released. When this substance is added to carbon, carbon dioxide and sulfur dioxide are also released. And if you add acid to sulfur, you get only sulfur dioxide and water. In such a chemical reaction, sulfate acid plays the role of an oxidizing agent.

Interaction with organic substances

Carbonization can be distinguished among the reactions of sulfuric acid with organic substances. Such a process occurs when a given substance collides with paper, sugar, fibers, wood, etc. In this case, carbon is released in any case. The carbon formed during the reaction can partially interact with sulfuric acid in excess. The photo shows the reaction of sugar with a solution of sulfate acid of medium concentration.

Reactions with salts

Also, a concentrated solution of H2SO4 reacts with dry salts. In this case, a standard exchange reaction occurs, in which metal sulfate is formed, which was present in the structure of the salt, and an acid with a residue that was in the composition of the salt. However, concentrated sulfuric acid does not react with salt solutions.

Interaction with other substances

Also, this substance can react with metal oxides and their hydroxides, in these cases exchange reactions occur, in the first metal sulfate and water are released, in the second - the same.

Chemical properties of a weak solution of sulfate acid

Dilute sulfuric acid reacts with many substances and has the same properties as all acids. It, unlike concentrated, interacts only with active metals, that is, those that are to the left of hydrogen in a series of voltages. In this case, the same substitution reaction occurs, as in the case of any acid. This releases hydrogen. Also, such an acid solution interacts with salt solutions, as a result of which an exchange reaction occurs, already discussed above, with oxides - just like concentrated, with hydroxides - also the same. In addition to ordinary sulfates, there are also hydrosulfates, which are the product of the interaction of hydroxide and sulfuric acid.

How to know if a solution contains sulfuric acid or sulfates

To determine whether these substances are present in a solution, a special qualitative reaction for sulfate ions is used, which allows you to find out. It consists in adding barium or its compounds to the solution. As a result, a precipitate may form white color(barium sulfate), indicating the presence of sulfates or sulfuric acid.

How is sulfuric acid produced?

The most common method of industrial production of this substance is its extraction from iron pyrite. This process occurs in three stages, each of which is a certain chemical reaction. Let's consider them. First, oxygen is added to pyrite, resulting in the formation of ferum oxide and sulfur dioxide, which is used for further reactions. This interaction occurs when high temperature. This is followed by a step in which, by adding oxygen in the presence of a catalyst, which is vanadium oxide, sulfur trioxide is obtained. Now, at the last stage, water is added to the resulting substance, and sulfate acid is obtained. This is the most common process for the industrial extraction of sulfate acid, it is used most often because pyrite is the most accessible raw material suitable for the synthesis of the substance described in this article. Sulfuric acid obtained using such a process is used in various industries - both in the chemical industry and in many others, for example, in oil refining, ore dressing, etc. It is also often used in the manufacturing technology of many synthetic fibers .