Sodium sulfate: formula and application. Sodium sulfate: formula and application Medicinal uses

Currently, chemists know more than 20 million chemical compounds. Obviously, not a single person is able to remember the names of tens of millions of substances.

That is why the International Union of Pure and Applied Chemistry developed systematic nomenclature organic and inorganic compounds. A system of rules has been constructed that allows naming oxides, acids, salts, complex compounds, organic matter etc. Systematic names have a clear, unambiguous meaning. For example, magnesium oxide is MgO, potassium sulfate is CaSO 4, chloromethane is CH 3 Cl, etc.

The chemist who discovers a new compound does not choose its name himself, but is guided by clear IUPAC rules. Any of his colleagues working in any country in the world will be able to quickly construct a formula for a new substance based on its name.

The systematic nomenclature is convenient, rational and accepted throughout the world. There is, however, a small group of compounds for which the “correct” nomenclature is practically not used. The names of some substances have been used by chemists for decades and even centuries. These trivial names more convenient, more familiar, and so firmly ingrained in consciousness that practitioners do not want to change them to systematic ones. In fact, even the IUPAC rules allow the use of trivial names.

Not a single chemist will name the substance CuSO 4 5H 2 O copper(II) sulfate pentahydrate. It is much easier to use the trivial name for this salt: copper sulfate. No one will ask a colleague: “Tell me, do you have any potassium hexacyanoferrate (III) left in your laboratory?” But you can even break your tongue! They will ask differently: “Is there any red blood salt left?”

Short, convenient and familiar. Unfortunately, trivial names of substances do not obey any modern rules. You just need to remember them. Yes, yes, the chemist must remember that FeS 2 is pyrite, and under the familiar term “chalk” lies calcium carbonate.

The table below lists some of the most common trivial names for salts, oxides, acids, bases, etc. Please note that one substance can have multiple trivial names. For example, sodium chloride (NaCl) can be called halite, or maybe - rock salt.

Trivial name	Substance formula	Systematic name
diamond	WITH	carbon
potassium alum	KAl(SO 4) 2 12H 2 O	Aluminum Potassium Sulfate Dodecahydrate
anhydrite	CaSO4	calcium sulfate
barite	BaSO4	barium sulfate
Prussian blue	Fe 4 3	iron(III) hexacyanoferrate(II)
bischofite	MgCl 2 6H 2 O	magnesium chloride hexahydrate
borazone	BN	boron nitride
borax	Na 2 B 4 O 7 10H 2 O	sodium tetraborate decahydrate
water gas	CO+H2	hydrogen + carbon monoxide (II)
galena	PbS	lead(II) sulfide
halite	NaCl	sodium chloride
slaked lime	Ca(OH)2	calcium hydroxide
hematite	Fe2O3	iron(III) oxide
gypsum	CaSO 4 2H 2 O	calcium sulfate dihydrate
alumina	Al2O3	aluminum oxide
Glauber's salt	Na 2 SO 4 10H 2 O	sodium sulfate decahydrate
graphite	WITH	carbon
sodium hydroxide	NaOH	sodium hydroxide
caustic potassium	KOH	potassium hydroxide
iron pyrite	FeS 2	iron disulfide
iron sulfate	FeSO 4 7H 2 O	iron(II) sulfate heptahydrate
yellow blood salt	K 4	Potassium hexacyanoferrate(II)
liquid glass	Na 2 SiO 3	sodium silicate
lime water	solution of Ca(OH) 2 in water	calcium hydroxide solution in water
limestone	CaCO3	calcium carbonate
calomel	Hg2Cl2	Dimercury dichloride
rock salt	NaCl	sodium chloride
cinnabar	HgS	mercury(II) sulfide
corundum	Al2O3	aluminum oxide
red blood salt	K 3	Potassium hexacyanoferrate(III)
hematite	Fe2O3	iron(III) oxide
cryolite	Na 3	sodium hexafluoroaluminate
lapis	AgNO3	silver nitrate
magnesite	MgCO 3	magnesium carbonate
magnetite	Fe3O4
magnetic iron ore	Fe3O4	Diiron(III)-iron(II) oxide
malachite	Cu 2 (OH) 2 CO 3	hydroxycopper(II) carbonate
copper shine	Cu2S	copper(I) sulfide
copper sulfate	CuSO 4 5H 2 O	copper(II) sulfate pentahydrate
chalk	CaCO3	calcium carbonate
marble	CaCO3	calcium carbonate
ammonia	aqueous solution NH 3	ammonia solution in water
ammonia	NH4Cl	ammonium chloride
quicklime	CaO	calcium oxide
sodium nitroprusside	Na 2	sodium penatcyanonitrosylium ferrate(II)
oleum	solution of SO 3 in H 2 SO 4	solution of sulfur oxide (VI) in conc. sulfuric acid
hydrogen peroxide	H2O2	hydrogen peroxide
pyrite	FeS 2	iron disulfide
pyrolusite	MnO2	manganese dioxide
hydrofluoric acid	HF	hydrofluoric acid
potash	K 2 CO 3	potassium carbonate
Nessler's reagent	K2	alkaline solution potassium tetraiodomercurate(II)
rhodochrosite	MnCO3	manganese(II) carbonate
rutile	TiO2	titanium dioxide
galena	PbS	lead(II) sulfide
red lead	Pb 3 O 4	dislead(III) oxide - lead(II)
ammonium nitrate	NH4NO3	ammonium nitrate
potassium nitrate	KNO 3	potassium nitrate
calcium nitrate	Ca(NO3)2	calcium nitrate
soda nitrate	NaNO3	sodium nitrate
Chilean saltpeter	NaNO3	sodium nitrate
sulfur pyrite	FeS 2	iron disulfide
sylvin	KCl	potassium chloride
siderite	FeCO3	iron(II) carbonate
smithsonite	ZnCO3	zinc carbonate
soda ash	Na 2 CO 3	sodium carbonate
caustic soda	NaOH	sodium hydroxide
baking soda	NaHCO3	sodium bicarbonate
Mohr's salt	(NH 4) 2 Fe(SO 4) 2 6H 2 O	ammonium iron(II) sulfate hexahydrate
corrosive sublimate	HgCl2	mercury(II) chloride
dry ice	CO 2 (solid)	carbon dioxide (solid)
sphalerite	ZnS	zinc sulfide
carbon monoxide	CO	carbon(II) monoxide
carbon dioxide	CO2	carbon(IV) monoxide
fluorite	CaF2	calcium fluoride
chalcocite	Cu2S	copper(I) sulfide
bleach	mixture of CaCl 2, Ca(ClO) 2 and Ca(OH) 2	mixture of calcium chloride, calcium hypochlorite and calcium hydroxide
chromium-potassium alum	KCr(SO 4) 2 12H 2 O	chromium(III)-potassium sulfate dodecahydrate
aqua regia	mixture of HCl and HNO 3	a mixture of concentrated solutions of hydrochloric and nitric acids volume ratio 3:1
zinc blende	ZnS	zinc sulfide
zinc sulfate	ZnSO 4 7H 2 O	zinc sulfate heptahydrate

Note: Natural minerals are composed of several substances. For example, silver compounds can be found in lead glitter. The table, of course, indicates only the main substance.

Substances of the form X n H 2 O are called crystalline hydrates. They include the so-called. "crystallization" water. For example, we can say that copper(II) sulfate crystallizes from aqueous solutions with 5 water molecules. We obtain copper (II) sulfate pentahydrate (the trivial name is copper sulfate).

If you are interested in systematic names, I recommend turning to the section "

8.1. What is chemical nomenclature

Chemical nomenclature developed gradually over several centuries. As you accumulate chemical knowledge it changed several times. It is being refined and developed even now, which is connected not only with the imperfection of some nomenclature rules, but also with the fact that scientists are constantly discovering new and new compounds, which can be named (and sometimes even made formulas) using existing rules sometimes it turns out to be impossible. The nomenclature rules currently accepted by the scientific community around the world are contained in a multi-volume publication: “IUPAC Nomenclature Rules for Chemistry”, the number of volumes in which is continuously increasing.
You are already familiar with the types of chemical formulas, as well as some of the rules for their composition. What are the names of chemical substances?
Using nomenclature rules, you can create systematic Name substances.

For many substances, in addition to systematic ones, traditional, so-called trivial titles. When they appeared, these names reflected certain properties of substances, methods of production, or contained the name of what the substance was isolated from. Compare the systematic and trivial names of the substances given in Table 25.

All names of minerals (natural substances that make up rocks) are also trivial, for example: quartz (SiO 2); rock salt, or halite (NaCl); zinc blende, or sphalerite (ZnS); magnetic iron ore, or magnetite (Fe 3 O 4); pyrolusite (MnO 2); fluorspar, or fluorite (CaF 2) and many others.

Table 25. Systematic and trivial names of some substances

	Systematic name	Trivial name
NaCl	Sodium chloride	Table salt
Na 2 CO 3	Sodium carbonate	Soda, soda ash
NaHCO3	Sodium bicarbonate	Baking soda
CaO	Calcium oxide	Quicklime
Ca(OH)2	Calcium hydroxide	Slaked lime
NaOH	Sodium hydroxide	Caustic soda, caustic soda, caustic
KOH	Potassium hydroxide	Caustic potassium
K2CO3	Potassium carbonate	Potash
CO2	Carbon dioxide	Carbon dioxide, carbon dioxide
CO	Carbon monoxide	Carbon monoxide
NH4NO3	Ammonium nitrate	Ammonium nitrate
KNO 3	Potassium nitrate	Potassium nitrate
KClO3	Potassium chlorate	Bertholet's salt
MgO	Magnesium oxide	Magnesia

For some of the most well-known or widespread substances, only trivial names are used, for example: water, ammonia, methane, diamond, graphite and others. In this case, such trivial names are sometimes called special.
You will learn how the names of substances belonging to different classes are composed in the following paragraphs.

Sodium carbonate Na 2 CO 3 . The technical (trivial) name is soda ash (that is, calcined) or simply “soda.” The white substance, thermally very stable (melts without decomposition), dissolves well in water, partially reacting with it, and an alkaline environment is created in the solution. Sodium carbonate – ionic compound with a complex anion whose atoms are interconnected covalent bonds. Soda was previously widely used in everyday life for washing clothes, but has now been completely replaced by modern washing powders. Sodium carbonate is obtained using a rather complex technology from sodium chloride, and is used mainly in the production of glass. Potassium carbonate K 2 CO 3. The technical (trivial) name is potash. In structure, properties and use, potassium carbonate is very similar to sodium carbonate. Previously, it was obtained from plant ash, and the ash itself was used in washing. Currently, most potassium carbonate is obtained as a by-product of the production of alumina (Al 2 O 3), used to make aluminum.

Due to its hygroscopicity, potash is used as a drying agent. It is also used in the production of glass, pigments, and liquid soap. In addition, potassium carbonate is a convenient reagent for obtaining other potassium compounds.

CHEMICAL NOMENCLATURE, SYSTEMATIC NAME, TRIVIAL NAME, SPECIAL NAME.
1. Write down ten trivial names of any compounds (not in the table) from the previous chapters of the textbook, write down the formulas of these substances and give their systematic names.
2. What do the trivial names “table salt”, “soda ash”, “carbon monoxide”, “burnt magnesia” mean?

8.2. Names and formulas of simple substances

The names of most simple substances coincide with the names of the corresponding elements. Only all allotropic modifications of carbon have their own special names: diamond, graphite, carbyne and others. In addition, one of the allotropic modifications of oxygen has its own special name - ozone.
The simplest formula of a simple non-molecular substance consists only of the symbol of the corresponding element, for example: Na - sodium, Fe - iron, Si - silicon.
Allotropic modifications are designated using alphabetic indices or letters of the Greek alphabet:

C (a) – diamond; - Sn – gray tin;
C (gr) – graphite; - Sn – white tin.

IN molecular formulas The index of molecular simple substances, as you know, shows the number of atoms in a molecule of a substance:
H 2 – hydrogen; O 2 – oxygen; Cl 2 – chlorine; O 3 – ozone.

In accordance with nomenclature rules, the systematic name of such a substance must contain a prefix indicating the number of atoms in the molecule:
H 2 – dihydrogen;
O 3 – trioxygen;
P 4 – tetraphosphorus;
S 8 - octasulfur, etc., but at present this rule has not yet become generally accepted.

Table 26.Numeric prefixes

Factor	Prefix	Factor	Prefix	Factor	Prefix
	mono		penta		nona
	di		hexa		soundboard
	three		hepta		Undeka
	tetra		Octa		dodeca

Ozone O3– light blue gas with a characteristic odor, liquid state– dark blue, in solid – dark purple. This is the second allotropic modification oxygen. Ozone is much more soluble in water than oxygen. O 3 is unstable and even at room temperature slowly turns into oxygen. Very reactive, destroys organic substances, reacts with many metals, including gold and platinum. You can smell ozone during a thunderstorm, since in nature ozone is formed as a result of the action of lightning and ultraviolet radiation on atmospheric oxygen. Above the Earth there is an ozone layer located at an altitude of about 40 km, which traps the bulk of the ultraviolet radiation of the Sun, which is destructive for all living things. Ozone has bleaching and disinfecting properties. In some countries it is used to disinfect water. In medical institutions, ozone produced in special devices - ozonizers - is used to disinfect premises.

8.3. Formulas and names of binary substances

According to general rule in the formula of a binary substance, the symbol of an element with a lower electronegativity of atoms is placed in first place, and in second place - with a higher one, for example: NaF, BaCl 2, CO 2, OF 2 (and not FNa, Cl 2 Ba, O 2 C or F 2 O !).
Since electronegativity values for atoms of different elements are constantly being refined, two rules of thumb are usually used:
1. If a binary compound is a compound of a metal-forming element with element forming a non-metal, then the symbol of the element forming the metal is always placed in first place (on the left).
2. If both elements included in the compound are elements that form non-metals, then their symbols are arranged in the following sequence:

B, Si, C, Sb, As, P, N, H, Te, Se, S, At, I, Br, Cl, O, F.

Note: It should be remembered that nitrogen's place in this practical series does not correspond to its electronegativity; as a general rule it should be placed between chlorine and oxygen.

Examples: Al 2 O 3, FeO, Na 3 P, PbCl 2, Cr 2 S 3, UO 2 (according to the first rule);
BF 3, CCl 4, As 2 S 3, NH 3, SO 3, I 2 O 5, OF 2 (according to the second rule).
The systematic name of a binary compound can be given in two ways. For example, CO 2 can be called carbon dioxide - you already know this name - and carbon monoxide (IV). In the second name, the Stock number (oxidation state) of carbon is indicated in parentheses. This is done in order to distinguish this compound from CO - carbon monoxide (II).
You can use either type of name, depending on which one is more convenient in this case.

Examples (more convenient names are highlighted):

MnO	manganese monoxide	manganese(II) oxide
Mn2O3	dimanganese trioxide	manganese oxide(III)
MnO2	manganese dioxide	manganese(IV) oxide
Mn2O7	dimanganese heptoxide	manganese oxide(VII)

Other examples:

If the atoms of the element that comes first in the formula of a substance exhibit only one positive oxidation state, then neither numerical prefixes nor the designation of this oxidation state in the name of the substance are usually used, for example:
Na 2 O – sodium oxide; KCl – potassium chloride;
Cs 2 S – cesium sulfide; BaCl 2 – barium chloride;
BCl 3 – boron chloride; HCl – hydrogen chloride (hydrogen chloride);
Al 2 O 3 – aluminum oxide; H 2 S – hydrogen sulfide (hydrogen sulfide).

1. Make up systematic names of substances (for binary substances - in two ways):
a) O 2, FeBr 2, BF 3, CuO, HI;
b) N 2, FeCl 2, Al 2 S 3, CuI, H 2 Te;
c) I 2, PCl 5, MnBr 2, BeH 2, Cu 2 O.
2.Name each of the nitrogen oxides in two ways: N 2 O, NO, N 2 O 3, NO 2, N 2 O 4, N 2 O 5. Emphasize more user-friendly names.
3. Write down the formulas of the following substances:
a) sodium fluoride, barium sulfide, strontium hydride, lithium oxide;
b) carbon(IV) fluoride, copper(II) sulfide, phosphorus(III) oxide, phosphorus(V) oxide;
c) silicon dioxide, diiodine pentoxide, diphosphorus trioxide, carbon disulfide;
d) hydrogen selenide, hydrogen bromide, hydrogen iodide, hydrogen telluride;
e) methane, silane, ammonia, phosphine.
4. Formulate the rules for compiling formulas for binary substances according to the position of the elements that make up this substance in the system of elements.

8.4. Formulas and names of more complex substances

As you have already noticed, in the formula of a binary compound, the first place is the symbol of a cation or atom with a partial positive charge, and the second is the symbol of an anion or an atom with a partial negative charge. Formulas for more complex substances are compiled in the same way, but the places of atoms or simple ions in them are taken by groups of atoms or complex ions.
As an example, consider the compound (NH 4) 2 CO 3. In it, the formula of a complex cation (NH 4) is in first place, and the formula of a complex anion (CO 3 2) is in second place.
In the formula of the most complex ion, the symbol of the central atom, that is, the atom to which the remaining atoms (or groups of atoms) of this ion are associated, is placed first, and the oxidation state of the central atom is indicated in the name.

Examples of systematic names:
Na 2 SO 4 sodium tetraoxosulfate(VI),
K 2 SO 3 potassium(II) trioxosulfate(IV),
CaCO 3 calcium(II) trioxocarbonate(IV),
(NH 4) 3 PO 4 ammonium tetraoxophosphate(V),
PH 4 Cl phosphonium chloride,
Mg(OH) 2 magnesium(II) hydroxide.

Such names accurately reflect the composition of the compound, but are very cumbersome. Therefore, abbreviated ones ( semi-systematic) names of these compounds:
Na 2 SO 4 sodium sulfate,
K 2 SO 3 potassium sulfite,
CaCO 3 calcium carbonate,
(NH 4) 3 PO 4 ammonium phosphate,
Mg(OH) 2 magnesium hydroxide.

The systematic names of acids are composed as if the acid is a hydrogen salt:
H 2 SO 4 hydrogen tetraoxosulfate(VI),
H 2 CO 3 hydrogen trioxocarbonate (IV),
H 2 hydrogen hexafluorosilicate (IV). (You will learn about the reasons for using square brackets in the formula of this compound later)
But for the most well-known acids, nomenclature rules allow the use of their trivial names, which, together with the names of the corresponding anions, are given in Table 27.

Table 27.Names of some acids and their anions

Name

Formula

Aluminum chloride AlCl 3. In a solid state - not molecular substance with the simplest formula AlCl 3, and in liquid and gaseous form - the molecular substance Al 2 Cl 6. The bonds in anhydrous aluminum chloride are covalent, and in solid form it has a framework structure. It is a white, fusible, highly volatile compound. Aluminum chloride is highly soluble in water and “smoke” in moist air. Anhydrous AlCl 3 cannot be isolated from aqueous solutions. Aluminum chloride is used as a catalyst in the synthesis of organic substances.

Nitric acid HNO 3 Pure anhydrous nitric acid is a colorless liquid; in light it decomposes to form brown nitrogen dioxide, which colors the acid yellowish, the intensity of which depends on the concentration of the dioxide. If acid is handled carelessly and gets on the skin, a burn will form, which also has a characteristic yellow color. Nitric acid mixes with water in any ratio. It is customary to distinguish between concentrated, dilute and very dilute acids. A mixture of nitric and hydrochloric acids is called "regia vodka" - this mixture is so active that it can react with gold. And nitric acid itself is one of the most destructive reagents. Due to its high activity, nitric acid does not occur in nature in a free state, although small amounts are formed in the atmosphere. Prepare nitric acid from large quantities from ammonia using a rather complex technology, but are spent on the production of mineral fertilizers. in addition, this substance is used in almost all branches of the chemical industry.

SEMI-SYSTEMATIC NAMES OF ACIDS AND SALTS.
Name the following substances:
a) Fe(NO 3) 3, H 2 SeO 4, Cr(OH) 3, (NH 4) 3 PO 4;
b) Cr 2 (SO 4) 3, CrSO 4, CrCl 3, CrO 3, Cr 2 S 3;
c) Na 2 SO 4, Na 2 SO 3, Na 2 S;
d) KNO 3, KNO 2, K 3 N;
e) HBr, H 3 BO 3, (H 3 O) 2 SO 4, (H 3 O) 3 PO 4;
e) KMnO 4, K 2 S 2 O 7, K 3, K 3.
2. Make up formulas for the following substances:
a) magnesium carbonate, lead(II) nitrate, lithium nitrite;
b) chromium(III) hydroxide, aluminum bromide, iron(II) sulfide;
c) silver nitrate, phosphorus bromide (V), calcium phosphate.

The use of sodium sulfate (Na2SO4) is associated with the manufacture of shampoos, powders, laxative medications, and food products. Chemical element used by the chemical, textile, leather industries. It has both a number of advantages and disadvantages, including brittleness of hair when washed with shampoos, which contain derivative ingredients such as lauryl and laureth sulfates.

What is sodium sulfate

Sodium sulfate is a substance that has a name analogous to sodium sulfate and defines a whole class of sulfuric acid salts from the sodium category. Glauber's salt is a decahydrate of the above substance, previously used to cleanse the intestines after poisoning as a laxative. In modern America and Russia, for this purpose, sodium sulfate along with its hydrates is not allowed to be used as a single active substance.

Formula

The formula of sodium sulfate in its anhydrous version is designated as Na2SO4 with a molar mass of 142 g/mol, has no color, and has a crystalline form. IN natural conditions Anhydrous sodium sulfate is found as the mineral thenardite. The element is stable up to a temperature of thirty-four degrees. If you increase the temperature and add water, the substance is converted into Glauber's salt (the name of the mineral is mirabilite).

Properties

The properties of sodium sulfate are as follows:

crystal shape – diamond-shaped;
no color;
boiling and melting occur without decomposition;
dissolution in water occurs quickly;
the reaction with hydrogen starts at a temperature range from 550 to 600 degrees;
interacts with sulfuric acid.

Application of sodium sulfate in industry

The use of sodium sulfate in industry has many branches, ranging from the production of washing powders to its use as a food additive. Areas of use:

Food industry. Sodium sulfate solution is added to products under code E514 to regulate acidity, bleach, increase food shelf life, and color stabilizer. Manufacturers send it to dried fish products, canned fruits, vegetables, jelly, marmalade, confectionery, seasonings. At the molecular level, the substance binds acetaldehyde in wine, preventing oxidation of the drink. The supplement is harmful to health, like all substances containing E, it has a destructive effect on vitamins E and B1.
Chemical and cosmetic industry. For the production of detergents: shampoo, powder, shower gel, floor cleaner.
Medicine. It is found in drugs that have a laxative effect and slows down the absorption of poison in the intestines.
It can be used as a dehydration agent in scientific laboratories to replace magnesium sulfate, since it is cheaper and takes less time to obtain.
Other areas of application include glass production, non-ferrous metallurgy, leather and textile industries.

Sodium sulfate in shampoos

On the label it is designated SLS (sodium laureth sulfate) - this is sodium laureth sulfate, originally invented for washing tanks during the Second World War, but due to its excellent cleaning properties and beautiful foam, the substance moved into the cosmetic industry. Sodium sulfate is present very often in shampoos. Lauryl sulfate is considered even more concentrated and harmful.

Although the rumor linking laureth and lauryl sulfates to cancer has been refuted by the American College of Toxicology, these components have certain bad effects on the skin and hair. If you use shampoos with these additives too often, you can get dry, dull hair and scalp inflammation. Natural substitutes: lauryl glucoside, laureth sulfosuccinate, cocoglucoside may foam less, but are more useful for washing.

Sodium sulfate

The element promotes the excretion of bile and prevents the absorption of toxic substances. Sodium sulfate retains fluid in the intestines, and its accumulation stimulates peristalsis and emptying of the gastrointestinal tract. This effect of the substance is used to produce saline laxatives. It comes in the form of a powder that should be drunk as an aqueous solution. Begins to act 5 hours after ingestion.

Instructions for use

Indications:

preparatory stage before surgical intervention in the intestine;
persistent constipation;
food poisoning;
together with other drugs for deworming.

Instructions for use of sodium sulfate.

Many people are interested in what sodium sulfate is and what are the features of its use.

The proposed material discusses the properties of this substance, chemical formula, method of administration and possible contraindications.

This component (another name is sodium sulfate) is the definition of a whole class of sulfuric acid salts, the sodium variety, which has the following properties.

Such as:

Crystalline structure, with diamond-shaped crystals.
Complete lack of color.
It is recognized after the reaction of the composition with its content with silver nitrate - a white precipitate is released.
Boiling and melting under the influence of temperature, without decomposing.
Characterized by solubility in water.
Interaction with hydrogen at a calcination temperature of five hundred fifty to six hundred degrees Celsius.
Sulfuric acid reacts with it.
Doesn't react with hydrochloric acid(hydrogen chloride).

Chemical formula

The anhydrous variety of this substance is determined chemical formula Na2SO4.

That is, it is a component obtained after combining sodium with sulfate (a compound of sulfur and oxygen), with the oxidation state of sulfur +6.

The mass fraction of sodium in the substance is thirty-two and four tenths percent.

Can be prepared by reacting sulfuric acid with sodium hydroxide, called hydrolysis. Molar mass component is one hundred and forty-two grams per mole.

In the natural environment it is found in the form of the mineral thenardite. May be found in sulfur water, a type of mineral water.

If the ambient temperature does not exceed thirty-four degrees, the compound does not decompose and is relatively stable.

When it is increased and water is added, another state is obtained, called Glauber's salt (sodium sulfate decahydrate - decahydrate crystalline hydrate).

This natural component called mirabilite.

Useful properties

Thanks to your chemical properties, this component is widely used in various fields.

More details about this in the table:

Where is it used?	Features of application
In the food industry	It is added to products in the form of a solution. GOST code – E514. Regulates acidity, has whitening properties, increases the shelf life of products, and stabilizes color. Included in fish, canned and confectionery products, and spices. Slows down oxidative processes in wine drinks. Can cause harm to the body, like any other substance designated by the E index, due to the destruction of vitamins B1, E
In the chemical industry and cosmetics production	Included in the formula of detergent compositions - shampoos (containing laureate sodium sulfate), laundry detergents, dishwashing detergents, etc. Sodium carbonate (soda) is obtained from Glauber's salt.
In veterinary medicine	Contained in medications necessary to achieve a laxative effect by slowing the penetration of toxic substances through the intestinal walls. Included in other drugs. The chloride of this substance forms glucosamine, a component of chondroitin and other medications intended to restore cartilage tissue in joints. From sodium sulfate, thiosulfate is obtained, produced in ampoules and taken intravenously for poisoning.
In science	It is used as a dehydrating composition capable of replacing magnesium sulfate to produce barium sulfate by dissociation, copper oxide by electrolysis of this melt, used for laboratory purposes. Low cost and very easy to obtain
Other areas	Involved in the production of glass products, the metallurgical industry of non-ferrous metals, the production of leather and textile products, and in fertilizers (after combining with ammonium sulfate)

Medicinal use

For medical purposes, this component is used for:

Improved bile excretion.
Slowing down the absorption of poisons.
Water retention in the body.
Stimulating the movement of intestinal contents and the functioning of the gastrointestinal tract.

These qualities of the substance are involved in the production of laxative medications.

It is used as a powder taken in the form of an aqueous solution. The effect is achieved five hours after use.

The drug is indicated for use in the following situations:

For severe intestinal constipation, for their treatment.
To neutralize food poisoning.
During antihelminthic treatment.
On preparatory stage during therapeutic fasting for weight loss.
For similar purposes in preparation for surgery, for diagnosis, intestinal therapy.
For rinsing the nose.

However, it should be borne in mind that this remedy should not be taken in the presence of the following diseases and processes:

Peptic ulcer of the digestive system.
Appendicitis.
Inflammatory processes in the abdominal cavity.
Ulcerative inflammation in the large intestine.
Acute form of hemorrhoids.
A sharp decrease in blood pressure.
General exhaustion.
Menstrual bleeding.
Carrying a child.
Breastfeeding children.
For older people.

The following side effects are possible:

The occurrence of intestinal colic.
Digestive problems.
Frequent urination.
Nausea.

Pay attention! This drug is not recommended to be taken for a long period, due to the possibility of disruption of the absorption of food and medications.

Taking the medicine on an empty stomach is most effective. The instructions for preparing the composition are simple: dissolve up to thirty grams of the substance in fifty grams of warm water.

Prescribed dosage:

Up to thirty grams at a time - for adults.
One gram per number of years – for children.

However, when taking the drug, you should definitely consult a doctor.

As you can see, this substance has a wide range of applications in a wide variety of industries, including medicine - this is its main area of use.

Useful video

Trivial names of some inorganic compounds

Currently, chemists know more than 20 million chemical compounds. Obviously, not a single person is able to remember the names of tens of millions of substances.

That is why the International Union of Pure and Applied Chemistry developed systematic nomenclature organic and inorganic compounds. A system of rules has been constructed that allows us to name oxides, acids, salts, complex compounds, organic substances, etc. Systematic names have a clear, unambiguous meaning. For example, magnesium oxide is MgO, potassium sulfate is CaSO 4, chloromethane is CH 3 Cl, etc.

Trivial name	Substance formula	Systematic name
diamond	WITH	carbon
potassium alum	KAl(SO 4) 2 12H 2 O	Aluminum Potassium Sulfate Dodecahydrate
anhydrite	CaSO4	calcium sulfate
barite	BaSO4	barium sulfate
Prussian blue	Fe 4 3	iron(III) hexacyanoferrate(II)
bischofite	MgCl 2 6H 2 O	magnesium chloride hexahydrate
borazone	BN	boron nitride
borax	Na 2 B 4 O 7 10H 2 O	sodium tetraborate decahydrate
water gas	CO+H2	hydrogen + carbon monoxide (II)
galena	PbS	lead(II) sulfide
halite	NaCl	sodium chloride
slaked lime	Ca(OH)2	calcium hydroxide
hematite	Fe2O3	iron(III) oxide
gypsum	CaSO 4 2H 2 O	calcium sulfate dihydrate
alumina	Al2O3	aluminum oxide
Glauber's salt	Na 2 SO 4 10H 2 O	sodium sulfate decahydrate
graphite	WITH	carbon
sodium hydroxide	NaOH	sodium hydroxide
caustic potassium	KOH	potassium hydroxide
iron pyrite	FeS 2	iron disulfide
iron sulfate	FeSO 4 7H 2 O	iron(II) sulfate heptahydrate
yellow blood salt	K 4	Potassium hexacyanoferrate(II)
liquid glass	Na 2 SiO 3	sodium silicate
lime water	solution of Ca(OH) 2 in water	calcium hydroxide solution in water
limestone	CaCO3	calcium carbonate
calomel	Hg2Cl2	Dimercury dichloride
rock salt	NaCl	sodium chloride
cinnabar	HgS	mercury(II) sulfide
corundum	Al2O3	aluminum oxide
red blood salt	K 3	Potassium hexacyanoferrate(III)
hematite	Fe2O3	iron(III) oxide
cryolite	Na 3	sodium hexafluoroaluminate
lapis	AgNO3	silver nitrate
magnesite	MgCO 3	magnesium carbonate
magnetite	Fe3O4
magnetic iron ore	Fe3O4	Diiron(III)-iron(II) oxide
malachite	Cu 2 (OH) 2 CO 3	hydroxycopper(II) carbonate
copper shine	Cu2S	copper(I) sulfide
copper sulfate	CuSO 4 5H 2 O	copper(II) sulfate pentahydrate
chalk	CaCO3	calcium carbonate
marble	CaCO3	calcium carbonate
ammonia	aqueous solution NH 3	ammonia solution in water
ammonia	NH4Cl	ammonium chloride
quicklime	CaO	calcium oxide
sodium nitroprusside	Na 2	sodium penatcyanonitrosylium ferrate(II)
oleum	solution of SO 3 in H 2 SO 4	solution of sulfur oxide (VI) in conc. sulfuric acid
hydrogen peroxide	H2O2	hydrogen peroxide
pyrite	FeS 2	iron disulfide
pyrolusite	MnO2	manganese dioxide
hydrofluoric acid	HF	hydrofluoric acid
potash	K 2 CO 3	potassium carbonate
Nessler's reagent	K2	alkaline solution of potassium tetraiodomercurate (II)
rhodochrosite	MnCO3	manganese(II) carbonate
rutile	TiO2	titanium dioxide
galena	PbS	lead(II) sulfide
red lead	Pb 3 O 4	dislead(III) oxide - lead(II)
ammonium nitrate	NH4NO3	ammonium nitrate
potassium nitrate	KNO 3	potassium nitrate
calcium nitrate	Ca(NO3)2	calcium nitrate
soda nitrate	NaNO3	sodium nitrate
Chilean saltpeter	NaNO3	sodium nitrate
sulfur pyrite	FeS 2	iron disulfide
sylvin	KCl	potassium chloride
siderite	FeCO3	iron(II) carbonate
smithsonite	ZnCO3	zinc carbonate
soda ash	Na 2 CO 3	sodium carbonate
caustic soda	NaOH	sodium hydroxide
baking soda	NaHCO3	sodium bicarbonate
Mohr's salt	(NH 4) 2 Fe(SO 4) 2 6H 2 O	ammonium iron(II) sulfate hexahydrate
corrosive sublimate	HgCl2	mercury(II) chloride
dry ice	CO 2 (solid)	carbon dioxide (solid)
sphalerite	ZnS	zinc sulfide
carbon monoxide	CO	carbon(II) monoxide
carbon dioxide	CO2	carbon(IV) monoxide
fluorite	CaF2	calcium fluoride
chalcocite	Cu2S	copper(I) sulfide
bleach	mixture of CaCl 2, Ca(ClO) 2 and Ca(OH) 2	mixture of calcium chloride, calcium hypochlorite and calcium hydroxide
chromium-potassium alum	KCr(SO 4) 2 12H 2 O	chromium(III)-potassium sulfate dodecahydrate
aqua regia	mixture of HCl and HNO 3	a mixture of concentrated solutions of hydrochloric and nitric acids in a volume ratio of 3:1
zinc blende	ZnS	zinc sulfide
zinc sulfate	ZnSO 4 7H 2 O	zinc sulfate heptahydrate

Note: Natural minerals are composed of several substances. For example, silver compounds can be found in lead glitter. The table, of course, indicates only the main substance.

Substances of the form X n H 2 O are called crystalline hydrates. They include the so-called. "crystallization" water. For example, we can say that copper (II) sulfate crystallizes from aqueous solutions with 5 water molecules. We obtain copper (II) sulfate pentahydrate (the trivial name is copper sulfate).

If you are interested in systematic names, I recommend that you refer to the section “Names of inorganic acids and salts”.