Names of some inorganic acids and salts. Chemistry

	Titles


	Meta-aluminum	Metaaluminate
	Metaarsenic	Metaarsenate
	Orthoarsenic	Orthoarsenate
	Metaarsenic	Metaarsenite
	Orthoarsenical	Orthoarsenite
	Metaborn	Metaborate
	Orthoboric	Orthoborate
	Quadruple	Tetraborate
	Hydrogen bromide
	brominated	Hypobromite
	Bromonic
	Ant
	Vinegar
	Hydrogen cyanide
	Coal	Carbonate
	Sorrel
	Hydrogen chloride
	Hypochlorous	Hypochlorite
	Chloride
	Chlorous
		Perchlorate
	Metachromic	Metachromite
	Chrome
	Two-chrome	Dichromate
	Hydrogen iodide
	Iodineous	Hypoioditis
	Iodine
		Periodat
	Manganese	Permanganate
	Manganese	Manganat
	Molybdenum	Molybdate
	Hydrogen azide (hydrogen nitrous)
	Nitrogenous

	Metaphosphoric	Metaphosphate
	Orthophosphoric	Orthophosphate
	Diphosphoric (pyrophosphoric)	Diphosphate (pyrophosphate)
	Phosphorous
	Phosphorous	Hypophosphite
	Hydrogen sulfide
	Rhodane hydrogen
	Sulphurous

	Thiosulfur	Thiosulfate
	Two-sulphur (pyrosulfur)	Disulfate (pyrosulfate)
	Peroxodusulfur (supersulfur)	Peroxodisulfate (persulfate)
	Hydrogen selenide
	Selenistaya
	Selenium
	Silicon
	Vanadium
	Tungsten	tungstate

Salts – substances that can be considered as the product of the replacement of hydrogen atoms in an acid with metal atoms or a group of atoms. There are 5 types of salts: medium (normal), acidic, basic, double, complex, differing in the nature of the ions formed during dissociation.

1.Medium salts are products of complete replacement of hydrogen atoms in the molecule acids. Salt composition: cation - metal ion, anion - acid residue ion. Na 2 CO 3 - sodium carbonate

Na 3 PO 4 - sodium phosphate

Na 3 PO 4 = 3Na + + PO 4 3-

cation anion

2.Sour salts – products of incomplete replacement of hydrogen atoms in an acid molecule. The anion contains hydrogen atoms.

NaH 2 PO 4 =Na + + H 2 PO 4 -

Dihydrogen phosphate cation anion

Acidic salts produce only polybasic acids when the amount of base taken is insufficient.

H 2 SO 4 +NaOH=NaHSO 4 +H 2 O

hydrogen sulfate

By adding excess alkali, the acidic salt can be converted to medium

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

3.Basic salts – products of incomplete substitution of hydroxide ions based on acid residue. The cation contains a hydroxo group.

CuOHCl=CuOH + +Cl -

hydroxochloride cation anion

Basic salts can only be formed by polyacid bases

(bases containing several hydroxyl groups), when they interact with acids.

Cu(OH) 2 +HCl=CuOHCl+H2O

You can convert a basic salt to a middle salt by treating it with an acid:

CuOHCl+HCl=CuCl 2 +H 2 O

4.Double salts – they contain cations of several metals and anions of one acid

KAl(SO 4) 2 = K + + Al 3+ + 2SO 4 2-

potassium aluminum sulfate

Characteristic properties All types of salts considered are: exchange reactions with acids, alkalis and with each other.

For naming salts use Russian and international nomenclature.

The Russian name of the salt is made up of the name of the acid and the name of the metal: CaCO 3 - calcium carbonate.

For acidic salts, the “sour” additive is introduced: Ca(HCO 3) 2 - acidic calcium carbonate. To name the main salts, add “basic”: (СuOH) 2 SO 4 – basic copper sulfate.

The most widespread is the international nomenclature. The name of the salt according to this nomenclature consists of the name of the anion and the name of the cation: KNO 3 - potassium nitrate. If the metal has a different valence in the compound, then it is indicated in brackets: FeSO 4 - iron sulfate (III).

For salts of oxygen-containing acids, the suffix “at” is added to the name if the acid-forming element has a higher valency: KNO 3 – potassium nitrate; suffix “it” if the acid-forming element has a lower valency: KNO 2 - potassium nitrite. In cases where an acid-forming element forms acids in more than two valence states, the suffix “at” is always used. Moreover, if it exhibits a higher valence, the prefix “per” is added. For example: KClO 4 – potassium perchlorate. If the acid-forming element forms a lower valence, the suffix “it” is used, with the addition of the prefix “hypo”. For example: KClO – potassium hypochlorite. For salts formed by acids containing different amounts of water, the prefixes “meta” and “ortho” are added. For example: NaPO 3 - sodium metaphosphate (salt of metaphosphoric acid), Na 3 PO 4 - sodium orthophosphate (salt of orthophosphoric acid). The prefix “hydro” is introduced into the name of the acidic salt. For example: Na 2 HPO 4 – sodium hydrogen phosphate (if the anion has one hydrogen atom) and the prefix “hydro” with the Greek numeral (if there is more than one hydrogen atom) – NaH 2 PO 4 – sodium dihydrogen phosphate. The prefix “hydroxo” is introduced into the names of the main salts. For example: FeOHCl – iron hydroxychloride (I).

5. Complex salts – compounds that form complex ions (charged complexes) upon dissociation. When writing complex ions, it is customary to enclose them in square brackets. For example:

Ag(NH 3) 2  Cl = Ag(NH 3) 2  + + Cl -

K 2 PtCl 6  = 2K + + PtCl 6  2-

According to the ideas proposed by A. Werner, in a complex connection there are internal and external spheres. So, for example, in the complex compounds considered, the inner sphere is composed of complex ions Ag(NH 3) 2  + and PtCl 6  2-, and the outer sphere is Cl - and K +, respectively. The central atom or ion of the inner sphere is called a complexing agent. In the proposed compounds these are Ag +1 and Pt +4. Molecules or ions of opposite sign coordinated around a complexing agent are ligands. In the compounds under consideration, these are 2NH 3 0 and 6Cl -. The number of ligands of a complex ion determines its coordination number. In the proposed compounds it is equal to 2 and 6, respectively.

Complexes are distinguished by the sign of the electric charge

1.Cationic (coordination around the positive ion of neutral molecules):

Zn +2 (NH 3 0) 4 Cl 2 -1 ; Al +3 (H 2 O 0) 6  Cl 3 -1

2.Anionic (coordination around a complexing agent in a positive oxidation state and a ligand having a negative oxidation state):

K 2 +1 Be +2 F 4 -1 ; K 3 +1 Fe +3 (CN -1) 6 

3. Neutral complexes – complex compounds without an outer spherePt + (NH 3 0) 2 Cl 2 -  0. Unlike compounds with anionic and cationic complexes, neutral complexes are not electrolytes.

Dissociation of complex compounds into inner and outer spheres is called primary . It proceeds almost entirely like strong electrolytes.

Zn (NH 3) 4 Cl 2 → Zn (NH 3) 4  +2 + 2Cl ─

K 3 Fe(CN) 6 → 3 K + +Fe(CN) 6  3 ─

Complex ion (charged complex) in a complex compound forms the inner coordination sphere, the remaining ions form the outer sphere.

In a complex compound K 3, the complex ion 3-, consisting of a complexing agent - the Fe 3+ ion and ligands - CN ─ ions, is the inner sphere of the compound, and the K + ions form the outer sphere.

The ligands located in the inner sphere of the complex are bound by the complexing agent much more tightly and their elimination during dissociation occurs only to a small extent. The reversible dissociation of the inner sphere of a complex compound is called secondary .

Fe(CN) 6  3 ─ Fe 3+ + 6CN ─

Secondary dissociation of the complex occurs according to the type of weak electrolytes. The algebraic sum of the charges of particles formed during the dissociation of a complex ion is equal to the charge of the complex.

The names of complex compounds, as well as the names of ordinary substances, are formed from the Russian names of cations and Latin names anions; just as in ordinary substances, in complex compounds the first is called the anion. If the anion is complex, its name is formed from the name of the ligands with the ending “o” (Cl - - chloro, OH - - hydroxo, etc.) and the Latin name of the complexing agent with the suffix “at”; the number of ligands is, as usual, indicated by the corresponding numeral. If the complexing agent is an element capable of exhibiting a variable oxidation state, the numerical value of the oxidation state, as in the names of ordinary compounds, is indicated by a Roman numeral in parentheses

Example: Names of complex compounds with a complex anion.

K 3 – potassium hexacyanoferrate (III)

Complex cations in the vast majority of cases contain neutral water molecules H 2 O, called “aqua,” or ammonia NH 3, called “ammine,” as ligands. In the first case, complex cations are called aqua complexes, in the second - ammonia. The name of the complex cation consists of the name of the ligands indicating their number and the Russian name of the complexing agent with the indicated value of its oxidation state, if necessary.

Example: Names of complex compounds with a complex cation.

Cl 2 – tetrammine zinc chloride

Complexes, despite their stability, can be destroyed in reactions in which ligands are bound into even more stable weakly dissociating compounds.

Example: Destruction of a hydroxo complex by an acid due to the formation of weakly dissociating H 2 O molecules.

K 2 + 2H 2 SO 4 = K 2 SO 4 + ZnSO 4 + 2H 2 O.

Name of the complex compound they begin by indicating the composition of the inner sphere, then name the central atom and its oxidation state.

In the inner sphere, anions are first named, adding the ending “o” to the Latin name.

F -1 – fluoro Cl - - chloroCN - - cyanoSO 2 -2 –sulfito

OH - - hydroxoNO 2 - - nitrito, etc.

Then the neutral ligands are called:

NH 3 – ammin H 2 O – aqua

The number of ligands is marked with Greek numerals:

I – mono (usually not indicated), 2 – di, 3 – three, 4 – tetra, 5 – penta, 6 – hexa. Next we move on to the name of the centralatom (complexing agent). The following are taken into account:

If the complexing agent is part of the cation, then the Russian name of the element is used and the degree of its oxidation is indicated in parentheses in Roman numerals;

If the complexing agent is part of an anion, then the Latin name of the element is used, its oxidation state is indicated before it, and the ending “at” is added at the end.

After the designation of the inner sphere, cations or anions located in the outer sphere are indicated.

When forming the name of a complex compound, one must remember that the ligands included in its composition can be mixed: electrically neutral molecules and charged ions; or charged ions of different types.

Ag +1 NH 3  2 Cl– diamine silver (I) chloride

K 3 Fe +3 CN 6 - hexacyano (III) potassium ferrate

NH 4  2 Pt +4 OH 2 Cl 4 – dihydroxotetrachloro(IV) ammonium platinate

Pt +2 NH 3  2 Cl 2 -1  o - diammine dichloride-platinum x)

X) in neutral complexes the name of the complexing agent is given in the nominative case

Names of some inorganic acids and salts

Acid formulas	Names of acids	Names of the corresponding salts
HClO4	chlorine	perchlorates
HClO3	hypochlorous	chlorates
HClO2	chloride	chlorites
HClO	hypochlorous	hypochlorites
H5IO6	iodine	periodates
HIO 3	iodic	iodates
H2SO4	sulfuric	sulfates
H2SO3	sulfurous	sulfites
H2S2O3	thiosulfur	thiosulfates
H2S4O6	tetrathionic	tetrathionates
HNO3	nitrogen	nitrates
HNO2	nitrogenous	nitrites
H3PO4	orthophosphoric	orthophosphates
HPO 3	metaphosphoric	metaphosphates
H3PO3	phosphorous	phosphites
H3PO2	phosphorous	hypophosphites
H2CO3	coal	carbonates
H2SiO3	silicon	silicates
HMnO4	manganese	permanganates
H2MnO4	manganese	manganates
H2CrO4	chrome	chromates
H2Cr2O7	dichrome	dichromats
HF	hydrogen fluoride (fluoride)	fluorides
HCl	hydrochloric (hydrochloric)	chlorides
HBr	hydrobromic	bromides
HI	hydrogen iodide	iodides
H2S	hydrogen sulfide	sulfides
HCN	hydrogen cyanide	cyanides
HOCN	cyan	cyanates

Let me briefly remind you of specific examples how to properly call salts.

Example 1. The salt K 2 SO 4 is formed by the remainder of sulfuric acid (SO 4) and the metal K. Salts of sulfuric acid are called sulfates. K 2 SO 4 - potassium sulfate.

Example 2. FeCl 3 - the salt contains iron and the remainder of hydrochloric acid(Cl). Name of salt: iron (III) chloride. Please note: in in this case we must not only name the metal, but also indicate its valency (III). In the previous example, this was not necessary, since the valency of sodium is constant.

Important: the name of the salt should indicate the valence of the metal only if the metal has a variable valency!

Example 3. Ba(ClO) 2 - the salt contains barium and the remainder of hypochlorous acid (ClO). Salt name: barium hypochlorite. The valency of the metal Ba in all its compounds is two; it does not need to be indicated.

Example 4. (NH 4) 2 Cr 2 O 7. The NH 4 group is called ammonium, the valence of this group is constant. Name of salt: ammonium dichromate (dichromate).

In the above examples we only encountered the so-called. medium or normal salts. Acidic, basic, double and complex salts, salts of organic acids will not be discussed here.

Acid formula	Acid name	Name of salt	Corresponding oxide
HCl	Solyanaya	Chlorides	----
HI	Hydroiodic	Iodides	----
HBr	Hydrobromic	Bromides	----
HF	Fluorescent	Fluorides	----
HNO3	Nitrogen	Nitrates	N2O5
H2SO4	Sulfuric	Sulfates	SO 3
H2SO3	Sulphurous	Sulfites	SO 2
H2S	Hydrogen sulfide	Sulfides	----
H2CO3	Coal	Carbonates	CO2
H2SiO3	Silicon	Silicates	SiO2
HNO2	Nitrogenous	Nitrites	N2O3
H3PO4	Phosphorus	Phosphates	P2O5
H3PO3	Phosphorous	Phosphites	P2O3
H2CrO4	Chrome	Chromates	CrO3
H2Cr2O7	Two-chrome	Bichromates	CrO3
HMnO4	Manganese	Permanganates	Mn2O7
HClO4	Chlorine	Perchlorates	Cl2O7

Acids can be obtained in the laboratory:

1) when dissolving acid oxides in water:

N 2 O 5 + H 2 O → 2HNO 3;

CrO 3 + H 2 O → H 2 CrO 4 ;

2) when salts interact with strong acids:

Na 2 SiO 3 + 2HCl → H 2 SiO 3 ¯ + 2NaCl;

Pb(NO 3) 2 + 2HCl → PbCl 2 ¯ + 2HNO 3.

Acids interact with metals, bases, basic and amphoteric oxides, amphoteric hydroxides and salts:

Zn + 2HCl → ZnCl 2 + H 2 ;

Cu + 4HNO 3 (concentrated) → Cu(NO 3) 2 + 2NO 2 + 2H 2 O;

H 2 SO 4 + Ca(OH) 2 → CaSO 4 ¯ + 2H 2 O;

2HBr + MgO → MgBr 2 + H 2 O;

6HI + Al 2 O 3 → 2AlBr 3 + 3H 2 O;

H 2 SO 4 + Zn(OH) 2 → ZnSO 4 + 2H 2 O;

AgNO 3 + HCl → AgCl¯ + HNO 3 .

Typically, acids react only with those metals that come before hydrogen in the electrochemical voltage series, and free hydrogen is released. Such acids do not interact with low-active metals (voltages come after hydrogen in the electrochemical series). Acids, which are strong oxidizing agents (nitric, concentrated sulfuric), react with all metals, with the exception of noble ones (gold, platinum), but in this case it is not hydrogen that is released, but water and an oxide, for example, SO 2 or NO 2.

A salt is the product of replacing hydrogen in an acid with a metal.

All salts are divided into:

average– NaCl, K 2 CO 3, KMnO 4, Ca 3 (PO 4) 2, etc.;

sour– NaHCO 3, KH 2 PO 4;

main – CuOHCl, Fe(OH) 2 NO 3.

A middle salt is the product of complete replacement of hydrogen ions in an acid molecule with metal atoms.

Acidic salts contain hydrogen atoms that can participate in chemical exchange reactions. In acidic salts, incomplete replacement of hydrogen atoms with metal atoms occurred.

Basic salts are the product of incomplete replacement of hydroxo groups of polyvalent metal bases with acidic residues. Basic salts always contain a hydroxo group.

Medium salts are obtained by the interaction:

1) acids and bases:

NaOH + HCl → NaCl + H 2 O;

2) acid and basic oxide:

H 2 SO 4 + CaO → CaSO 4 ¯ + H 2 O;

3) acid oxide and reasons:

SO 2 + 2KOH → K 2 SO 3 + H 2 O;

4) acidic and basic oxides:

MgO + CO 2 → MgCO 3 ;

5) metal with acid:

Fe + 6HNO 3 (concentrated) → Fe(NO 3) 3 + 3NO 2 + 3H 2 O;

6) two salts:

AgNO 3 + KCl → AgCl¯ + KNO 3 ;

7) salts and acids:

Na 2 SiO 3 + 2HCl → 2NaCl + H 2 SiO 3 ¯;

8) salts and alkalis:

CuSO 4 + 2CsOH → Cu(OH) 2 ¯ + Cs 2 SO 4.

Acid salts are obtained:

1) when neutralizing polybasic acids with alkali in excess acid:

H 3 PO 4 + NaOH → NaH 2 PO 4 + H 2 O;

2) during the interaction of medium salts with acids:

CaCO 3 + H 2 CO 3 → Ca(HCO 3) 2;

3) during the hydrolysis of salts formed by a weak acid:

Na 2 S + H 2 O → NaHS + NaOH.

The main salts are obtained:

1) during a reaction between a polyvalent metal base and an acid in excess of the base:

Cu(OH) 2 + HCl → CuOHCl + H 2 O;

2) during the interaction of medium salts with alkalis:

СuCl 2 + KOH → CuOHCl + KCl;

3) during the hydrolysis of medium salts formed by weak bases:

AlCl 3 +H 2 O → AlOHCl 2 + HCl.

Salts can interact with acids, alkalis, other salts, and water (hydrolysis reaction):

2H 3 PO 4 + 3Ca(NO 3) 2 → Ca 3 (PO 4) 2 ¯ + 6HNO 3 ;

FeCl 3 + 3NaOH → Fe(OH) 3 ¯ + 3NaCl;

Na 2 S + NiCl 2 → NiS¯ + 2NaCl.

In any case, the ion exchange reaction proceeds to completion only when a poorly soluble, gaseous or weakly dissociating compound is formed.

In addition, salts can interact with metals, provided that the metal is more active (has a more negative electrode potential) than the metal included in the salt:

Fe + CuSO 4 → FeSO 4 + Cu.

Salts are also characterized by decomposition reactions:

BaCO 3 → BaO + CO 2;

2KClO 3 → 2KCl + 3O 2.

Laboratory work №1

OBTAINING AND PROPERTIES

BASES, ACIDS AND SALTS

Experiment 1. Preparation of alkalis.

1.1. Interaction of metal with water.

Pour distilled water into a crystallizer or porcelain cup (about 1/2 of the vessel). Obtain from your teacher a piece of sodium metal, previously dried with filter paper. Drop a piece of sodium into a crystallizer with water. Once the reaction is complete, add a few drops of phenolphthalein. Note the observed phenomena and create an equation for the reaction. Name the resulting compound and write down its structural formula.

1.2. Interaction of metal oxide with water.

Pour distilled water into a test tube (1/3 of the test tube) and place a lump of CaO in it, mix thoroughly, add 1 - 2 drops of phenolphthalein. Note the observed phenomena, write the reaction equation. Name the resulting compound and give its structural formula.

Acids are complex substances whose molecules include hydrogen atoms that can be replaced or exchanged for metal atoms and an acid residue.

Based on the presence or absence of oxygen in the molecule, acids are divided into oxygen-containing(H 2 SO 4 sulfuric acid, H 2 SO 3 sulfurous acid, HNO 3 nitric acid, H 3 PO 4 phosphoric acid, H 2 CO 3 carbonic acid, H 2 SiO 3 silicic acid) and oxygen-free(HF hydrofluoric acid, HCl hydrochloric acid (hydrochloric acid), HBr hydrobromic acid, HI hydroiodic acid, H 2 S hydrosulfide acid).

Depending on the number of hydrogen atoms in the acid molecule, acids are monobasic (with 1 H atom), dibasic (with 2 H atoms) and tribasic (with 3 H atoms). For example, nitric acid HNO 3 is monobasic, since its molecule contains one hydrogen atom, sulfuric acid H 2 SO 4 – dibasic, etc.

There are very few inorganic compounds containing four hydrogen atoms that can be replaced by a metal.

The part of an acid molecule without hydrogen is called an acid residue.

Acidic residues may consist of one atom (-Cl, -Br, -I) - these are simple acidic residues, or they may consist of a group of atoms (-SO 3, -PO 4, -SiO 3) - these are complex residues.

In aqueous solutions, during exchange and substitution reactions, acidic residues are not destroyed:

H 2 SO 4 + CuCl 2 → CuSO 4 + 2 HCl

The word anhydride means anhydrous, that is, an acid without water. For example,

H 2 SO 4 – H 2 O → SO 3. Anoxic acids do not have anhydrides.

Acids get their name from the name of the acid-forming element (acid-forming agent) with the addition of the endings “naya” and less often “vaya”: H 2 SO 4 - sulfuric; H 2 SO 3 – coal; H 2 SiO 3 – silicon, etc.

The element can form several oxygen acids. In this case, the indicated endings in the names of acids will be when the element exhibits a higher valence (the acid molecule contains a high content of oxygen atoms). If the element exhibits a lower valence, the ending in the name of the acid will be “empty”: HNO 3 - nitric, HNO 2 - nitrogenous.

Acids can be obtained by dissolving anhydrides in water. If the anhydrides are insoluble in water, the acid can be obtained by the action of another stronger acid on the salt of the required acid. This method is typical for both oxygen and oxygen-free acids. Oxygen-free acids are also obtained by direct synthesis from hydrogen and a non-metal, followed by dissolving the resulting compound in water:

H 2 + Cl 2 → 2 HCl;

H 2 + S → H 2 S.

Solutions of the resulting gaseous substances HCl and H 2 S are acids.

Under normal conditions, acids exist in both liquid and solid states.

Chemical properties of acids

Acid solutions act on indicators. All acids (except silicic) are highly soluble in water. Special substances - indicators allow you to determine the presence of acid.

Indicators are substances of complex structure. They change their color depending on their interaction with different chemicals. In neutral solutions they have one color, in solutions of bases they have another color. When interacting with an acid, they change their color: the methyl orange indicator turns red, and the litmus indicator also turns red.

Interact with bases with the formation of water and salt, which contains an unchanged acid residue (neutralization reaction):

H 2 SO 4 + Ca(OH) 2 → CaSO 4 + 2 H 2 O.

Interact with base oxides with the formation of water and salt (neutralization reaction). The salt contains the acid residue of the acid that was used in the neutralization reaction:

H 3 PO 4 + Fe 2 O 3 → 2 FePO 4 + 3 H 2 O.

Interact with metals. For acids to interact with metals, certain conditions must be met:

1. the metal must be sufficiently active with respect to acids (in the series of activity of metals it must be located before hydrogen). The further to the left a metal is in the activity series, the more intensely it interacts with acids;

2. the acid must be strong enough (that is, capable of donating hydrogen ions H +).

When leaking chemical reactions acids with metals, a salt is formed and hydrogen is released (except for the interaction of metals with nitric and concentrated sulfuric acids):

Zn + 2HCl → ZnCl 2 + H 2 ;

Cu + 4HNO 3 → CuNO 3 + 2 NO 2 + 2 H 2 O.

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Acids are chemical compounds that are capable of donating an electrically charged hydrogen ion (cation) and also accepting two interacting electrons, resulting in the formation of a covalent bond.

In this article we will look at the main acids that are studied in middle school. secondary schools, and also learn many interesting facts about a variety of acids. Let's get started.

Acids: types

In chemistry, there are many different acids that have very different properties. Chemists distinguish acids by their oxygen content, volatility, solubility in water, strength, stability, and whether they belong to the organic or inorganic class. chemical compounds. In this article we will look at a table that presents the most famous acids. The table will help you remember the name of the acid and its chemical formula.

So, everything is clearly visible. This table presents the most famous acids in the chemical industry. The table will help you remember names and formulas much faster.

Hydrogen sulfide acid

H 2 S is hydrosulfide acid. Its peculiarity lies in the fact that it is also a gas. Hydrogen sulfide is very poorly soluble in water, and also interacts with many metals. Hydrogen sulfide acid belongs to the group of “weak acids”, examples of which we will consider in this article.

H 2 S has a slightly sweet taste and also a very pungent odor rotten eggs. In nature, it can be found in natural or volcanic gases, and it is also released during protein decay.

The properties of acids are very diverse; even if an acid is indispensable in industry, it can be very harmful to human health. This acid is very toxic to humans. When a small amount of hydrogen sulfide is inhaled, a person awakens headache, begins severe nausea and dizziness. If a person inhales a large number of H 2 S, it can lead to seizures, coma or even instant death.

Sulfuric acid

H 2 SO 4 is a strong sulfuric acid, which children are introduced to in chemistry lessons in the 8th grade. Chemical acids such as sulfuric acid are very strong oxidizing agents. H 2 SO 4 acts as an oxidizing agent on many metals, as well as basic oxides.

H 2 SO 4 causes chemical burns when it comes into contact with skin or clothing, but it is not as toxic as hydrogen sulfide.

Nitric acid

Strong acids are very important in our world. Examples of such acids: HCl, H 2 SO 4, HBr, HNO 3. HNO 3 is a well-known nitric acid. It has found wide application in industry, as well as in agriculture. It is used to make various fertilizers, in jewelry, when printing photographs, in manufacturing medicines and dyes, as well as in the military industry.

Such chemical acids, like nitrogen, are very harmful to the body. HNO 3 vapors leave ulcers, cause acute inflammation and irritation of the respiratory tract.

Nitrous acid

Nitrous acid is often confused with nitric acid, but there is a difference between them. The fact is that it is much weaker than nitrogen, it has completely different properties and effects on the human body.

HNO 2 has found wide application in the chemical industry.

Hydrofluoric acid

Hydrofluoric acid (or hydrogen fluoride) is a solution of H 2 O with HF. The acid formula is HF. Hydrofluoric acid is very actively used in the aluminum industry. It is used to dissolve silicates, etch silicon and silicate glass.

Hydrogen fluoride is very harmful to the human body and, depending on its concentration, can be a mild narcotic. If it comes into contact with the skin, at first there are no changes, but after a few minutes a sharp pain and chemical burn may appear. Hydrofluoric acid is very harmful to the environment.

Hydrochloric acid

HCl is hydrogen chloride and is a strong acid. Hydrogen chloride retains the properties of acids belonging to the group of strong acids. The acid is transparent and colorless in appearance, but smokes in air. Hydrogen chloride is widely used in the metallurgical and food industries.

This acid causes chemical burns, but getting into the eyes is especially dangerous.

Phosphoric acid

Phosphoric acid (H 3 PO 4) is a weak acid in its properties. But even weak acids can have the properties of strong ones. For example, H 3 PO 4 is used in industry to restore iron from rust. In addition, phosphoric (or orthophosphoric) acid is widely used in agriculture - many different fertilizers are made from it.

The properties of acids are very similar - almost each of them is very harmful to the human body, H 3 PO 4 is no exception. For example, this acid also causes severe chemical burns, nosebleeds, and chipping of teeth.

Carbonic acid

H 2 CO 3 is a weak acid. It is obtained by dissolving CO 2 (carbon dioxide) in H 2 O (water). Carbonic acid is used in biology and biochemistry.

Density of various acids

The density of acids occupies an important place in the theoretical and practical parts of chemistry. By knowing the density, you can determine the concentration of a particular acid, solve chemical calculation problems, and add the correct amount of acid to complete the reaction. The density of any acid changes depending on the concentration. For example, the higher the concentration percentage, the higher the density.

General properties of acids

Absolutely all acids are (that is, they consist of several elements of the periodic table), and they necessarily include H (hydrogen) in their composition. Next we will look at which are common:

All oxygen-containing acids (in the formula of which O is present) form water upon decomposition, and also oxygen-free acids decompose into simple substances (for example, 2HF decomposes into F 2 and H 2).
Oxidizing acids react with all metals in the metal activity series (only those located to the left of H).
They interact with various salts, but only with those that were formed by an even weaker acid.

Acids differ sharply from each other in their physical properties. After all, they can have a smell or not, and also be in a variety of different states of aggregation: liquid, gaseous and even solid. Solid acids are very interesting to study. Examples of such acids: C 2 H 2 0 4 and H 3 BO 3.

Concentration

Concentration is a value that determines the quantitative composition of any solution. For example, chemists often need to determine how much pure sulfuric acid is present in dilute acid H 2 SO 4. To do this, they pour a small amount of dilute acid into a measuring cup, weigh it, and determine the concentration using a density chart. The concentration of acids is closely related to density; often when determining the concentration there are calculation problems, where you need to determine the percentage of pure acid in the solution.

Classification of all acids according to the number of H atoms in their chemical formula

One of the most popular classifications is the division of all acids into monobasic, dibasic and, accordingly, tribasic acids. Examples of monobasic acids: HNO 3 (nitric), HCl (hydrochloric), HF (hydrofluoric) and others. These acids are called monobasic, since they contain only one H atom. There are many such acids, it is impossible to remember absolutely every one. You just need to remember that acids are classified according to the number of H atoms in their composition. Dibasic acids are defined similarly. Examples: H 2 SO 4 (sulphuric), H 2 S (hydrogen sulfide), H 2 CO 3 (coal) and others. Tribasic: H 3 PO 4 (phosphoric).

Basic classification of acids

One of the most popular classifications of acids is their division into oxygen-containing and oxygen-free. How to remember without knowing chemical formula substances that are oxygen-containing acid?

All oxygen-free acids do not contain important element O is oxygen, but it contains H. Therefore, the word “hydrogen” is always attached to their name. HCl is a H 2 S - hydrogen sulfide.

But you can also write a formula based on the names of acid-containing acids. For example, if the number of O atoms in a substance is 4 or 3, then the suffix -n-, as well as the ending -aya-, is always added to the name:

H 2 SO 4 - sulfur (number of atoms - 4);
H 2 SiO 3 - silicon (number of atoms - 3).

If the substance has less than three oxygen atoms or three, then the suffix -ist- is used in the name:

HNO 2 - nitrogenous;
H 2 SO 3 - sulfurous.

General properties

All acids taste sour and often slightly metallic. But there are other similar properties that we will now consider.

There are substances called indicators. The indicators change their color, or the color remains, but its shade changes. This occurs when the indicators are affected by other substances, such as acids.

An example of a color change is such a familiar product as tea, and lemon acid. When lemon is added to tea, the tea gradually begins to noticeably brighten. This is due to the fact that lemon contains citric acid.

There are other examples. Litmus, which in a neutral environment has purple colour turns red when hydrochloric acid is added.

When the tensions are in the tension series before hydrogen, gas bubbles are released - H. However, if a metal that is in the tension series after H is placed in a test tube with acid, then no reaction will occur, there will be no gas evolution. So, copper, silver, mercury, platinum and gold will not react with acids.

In this article we examined the most famous chemical acids, as well as their main properties and differences.