In order to answer the question of what salt is, it is usually not necessary to think for a long time. This chemical connection in everyday life is common enough. There is no need to talk about the ordinary cook salt. A detailed internal structure of salts and their compounds is studied inorganic chemistry.

Definition of salt

A clear answer to the question of what salt is, can be found in the works of M. V. Lomonosov. It assigned such name to fragile bodies, which can be dissolved in water and do not ignite under the influence of high temperatures or open flames. Later, the definition was not separated from their physical, but from the chemical properties of these substances.

School textbooks of inorganic chemistry give a rather clear concept of what salt is. So the products of replacing the chemical reaction, in which the acid atoms of the acid in the compound are replaced by metal. Examples of typical salts compounds: NaCl, MgSO 4. It is easy to see that any this entry can be divided into two halves: metal will always be recorded in the left component of the formula, and the acid residue is always recorded. The standard salt formula is as follows:

ME N M acid residue M n.

Physical properties of salt

Chemistry, as an accurate science, invests all possible information about its composition and opportunities. Thus, all salts here in modern interpretation composed of two words, one portion is called the metal constituent in the nominative case, and the second - contains description acid residue.

These compounds do not have a molecular structure, so under normal conditions, they are solid crystalline substances. Many salts have crystal lattice. Crystals of these substances of refractory, so there are very high temperatures for their melting. For example, barium sulphide melts at a temperature of about 2200 o C.

The solubility of the salt is divided into soluble, poorly soluble and insoluble. An example of the first can serve as sodium chloride, potassium nitrate. Multisuality include magnesium sulfite, lead chloride. Insoluble is calcium carbonate. Information on solubility of a substance is contained in the reference.

The product under consideration of the chemical reaction usually does not smell and has a different taste. The assumption that all salts are salted - erroneous. Clean salty taste has only one element of this class - our old familiar salt is familiar. There are sweet beryllium salts, bitter - magnesium and tasteless - for example, calcium carbonate (Common chalk).

Most of these substances are colorless, but there are also those that have characteristic colors. For example, iron (II) sulphate is characterized by a characteristic green color, potassium permanganate - purple, and potassium chromat crystals are bright yellow.

Classification of salt

Chemistry shares all types of inorganic salts into several basic signs. Salts resulting in complete replacement of hydrogen in acid are called normal or medium. For example, calcium sulfate.

Salt, which is derived from the reaction of incomplete substitution, is called sour or basic. An example of such an education may be a potassium hydrosulfate reaction:

The main salt is obtained with such a reaction in which the hydroxochroup is not fully replaced by the acid residue. The substances of this species can be formed by those metals whose valence is two or more. The typical salt formula of this group can be removed from such a reaction:

Normal, medium and acidic chemical compounds form salts and are standard classification of these compounds.

Double and mixed salt

An example of mixed is the calcium salt of hydrochloric and chlorinous acid: Caocl 2.

Nomenclature

Salts formed by metals with variable valence, have additional designation: after the formula in brackets they write valence roman numbers. So, there is iron sulfate FESO 4 (II) and Fe 2 (SO4) 3 (III). In the title of salts there is a prefix hydro, if there are unsubstituted hydrogen atoms in its composition. For example, potassium hydrophosphate has a K 2 HPO 4 formula.

Properties of salts in electrolytes

The theory of electrolytic dissociation gives its own interpretation by chemical properties. In the light of this theory, the salt can be defined as a weak electrolyte, which dissociated in the dissolved form (disintegrating) in water. Thus, the salt solution can be represented as a complex of positive negative ions, and the first is not atoms of hydrogen H +, and the second is not atoms of the hydroxochroup it is. Ions that would present in all types of salts solutions does not exist, so they do not possess any common properties. The smaller the charges of the ions forming the salt solution, the better they dissociate, the better the electrical conductivity of such a liquid mixture.

Solutions of acidic salts

Sour salts in the solution are disintegrated into complex negative ions, which are acidic residue, and simple anions, which are positively charged metal particles.

For example, the reaction of the dissolution of sodium bicarbonate leads to the decay of salt on sodium ions and the remainder of the NSO 3 -.

The full formula looks like: NaHCO 3 \u003d Na + + HCO 3 -, HCO 3 - \u003d H + + CO 3 2-.

Solutions of basic salts

The dissociation of the base salts leads to the formation of anions of the acid and complex cations consisting of metals and hydroxcrup. These complex cations, in turn, are also able to disintegrate during the dissociation. Therefore, in any solution of salts of the main group, it is present. For example, the dissociation of hydroxomagnium chloride proceeds as follows:

Salt propagation

What is salt? This element is one of the most common chemical compounds. Everyone is known to the cook salt, chalk (calcium carbonate) and so on. Among carbonate acid salts is the most common calcium carbonate. It is an integral part of marble, limestone, dolomite. And the calcium carbonate is the basis for the formation of pearls and corals. This chemical compound is an integral component for the formation of solid covers in insects and skeletons in chordan animals.

Craw salt is known to us since childhood. Doctors warn on its excessive use, but in moderate quantities it is extremely necessary for the implementation of life processes in the body. And it is necessary to maintain the correct composition of the blood and production of gastric juice. Essentials, an integral part of injections and droppers, there is nothing but a solution of the sole salt.

The salts are the electrolytes, dissociating in aqueous solutions with the formation of mandatory metal cation and anion acid residue
The classification of salts is given in Table. nine.

When writing, the formulas of any salts must be guided by one rule: the total charges of cations and anions should be equal in absolute value. Based on this, indexes should be placed. For example, when writing aluminum nitrate formula, we take into account that the charge of the aluminum coation is +3, and the Pitrate ion is 1: Alno 3 (+3), and with the help of indexes, the charges are equalized (the smallest of the total multiple for 3 and 1 is 3. Delim 3 On the absolute amount of charge of the aluminum cation - it turns out the index. We divide 3 to the absolute amount of the charge of anion NO 3 - the index 3 is obtained). Formula: Al (NO 3) 3

Middle, or normal, salts have only metal cations and anions of the acid residue. Their names are formed from latin name The element forms the acid residue by adding an appropriate end depending on the degree of oxidation of this atom. For example, sulfuric acid salt Na 2 So 4 is called (sulfur oxidation degree +6), salt Na 2 S - (sulfur oxidation degree -2), etc. In Table. 10 shows the names of salts formed by the most widely used acids.

The names of the middle salts underlie all other salts groups.

■ 106 Write the formulas of the following middle salts: a) calcium sulfate; b) magnesium nitrate; c) aluminum chloride; d) zinc sulphide; e); e) potassium carbonate; g) calcium silicate; h) iron phosphate (III).

The acidic salts differ from the average in that their composition, in addition to the metal cation, includes a hydrogen cation, such as NaHCO3 or Ca (H2PO4) 2. An acidic salt can be represented as a product of incomplete replacement of hydrogen atoms in acid with metal. Consequently, acidic salts can only be formed by two and more main acids.
The acidic salt molecule usually includes an "sour" ion, the charging of which depends on the stage of the acid dissociation. For example, the dissociation of phosphoric rods goes on three steps:

At the first stage of dissociation, a single-chargeed anion H 2 PO 4 is formed. Therefore, depending on the charge of the metal cation, the salts formulas will look like NAH 2 Po 4, Ca (H 2 PO 4) 2, VA (H 2 PO 4) 2, etc., on the second stage of the dissociation is formed already two-charged Anion HPO 2 4 -. The salts formulas will have such a type: Na 2 HPO 4, Surno 4, etc. The third stage of dissociation of acidic salts does not give.
The names of acidic salts are formed from the names of the average with the addition of the console hydro- (from the word "hydroge-nium" -):
NaHCo 3 - Sodium Barbonate KHSO 4 - Potassium Gidrosulfate Surno 4 - Calcium Hydrophosphate
If the composition of the acid ion includes two hydrogen atoms, for example, H 2 PO 4 -, another prefix di- (two) is added to the name: NAH 2 Po 4 - sodium dihydrophosphate, Ca (H 2 PO 4) 2 - calcium dihydrophosphate and T d.

■ 107. Write the formulas of the following acidic salts: a) calcium hydrosulfate; b) magnesium dihydrophosphate; c) aluminum hydrophosphate; d) Barium bicarbonate; e) sodium hydrosulfit; e) magnesium hydrosulfit.
108. It is possible to obtain acidic salts of salt and nitric acid. Justify your answer.

The main salts differ from the rest of the fact that, in addition to the metal cation and anion of the acid residue, their composition includes hydroxyl anions, for example Al (OH) (NO3) 2. Here is the charge of aluminum cation +3, and the charges of hydroxyl-ion-1 and two nitrate ions - 2, total - 3.
The names of the main salts are formed from the names of the average with the addition of the word main, for example: Cu 2 (O) 2 CO 3 - the main carbonate of copper, Al (OH) 2 NO 3 is the main aluminum nitrate.

■ 109. Write the formulas of the following basic salts: a) the main chloride of iron (II); b) the main sulfate of iron (III); c) the main nitrate of copper (II); d) the main calcium chloride; e) the main chloride of magnesium; e) the main sulfate of iron (III) G) the main chloride of aluminum.

Double salts formulas, for example kal (SO4) 3, are built, based on the total charges of both metal cations and the total charge of anion

The total charge of the cations + 4, the overall charge of anions -4.
The names of the double salts are formed in the same way as medium, only indicate the names of both metals: kal (SO4) 2 - potassium-aluminum sulfate.

■ 110. Write the formulas of the following salts:
a) magnesium phosphate; b) magnesium hydrophosphate; c) sulfate lead; d) barium hydrosulfate; e) Barium hydrosulfit; e) potassium silicate; g) aluminum nitrate; h) copper chloride (II); and) iron carbonate (III); k) calcium nitrate; l) potassium carbonate.

Chemical properties of salts

1. All middle salts are strong electrolytes and are easily dissociated:
Na 2 SO 4 ⇄ 2NA + + SO 2 4 -
The average salts can interact with metals that stand in a row of voltages to the left of the metal, which is part of the salt:
Fe + Cuso 4 \u003d Cu + Feso 4
Fe + Cu 2+ + SO 2 4 - \u003d Cu + Fe 2+ + SO 2 4 -
Fe + Cu 2+ \u003d Cu + Fe 2+
2. Salts react with alkalis and acids according to the rules described in the sections of the "base" and "acid":
FECL 3 + 3NAOH \u003d FE (OH) 3 ↓ + 3NACL
Fe 3+ + 3Cl - + 3NA + + 3D - \u003d Fe (OH) 3 + 3NA + + 3CL -
Fe 3+ + 3OH - \u003d Fe (OH) 3
Na 2 SO 3 + 2HCl \u003d 2NACL + H 2 SO 3
2NA + + SO 2 3 - + 2H + + 2Cl - \u003d 2NA + + 2Cl - + SO 2 + H 2 O
2H + + SO 2 3 - \u003d SO 2 + H 2 O
3. Salts may interact with each other, resulting in new salts:
AGNO 3 + NaCl \u003d Nano 3 + AgCl
AG + + NO 3 - + Na + + Cl - \u003d Na + + NO 3 - + AGCL
AG + + CL - \u003d AGCL
Since these exchange reactions are carried out mainly in aqueous solutions, they proceed only when one of the formed salts falls into a precipitate.
All exchange reactions go in accordance with the conditions of reactions to the end listed in § 23, p. 89.

■ 111. Make the equations of the following reactions and, using the solubility table, determine whether they will pass to the end:
a) chloride barium +;
b) aluminum + chloride;
c) sodium phosphate + calcium nitrate;
d) magnesium chloride + potassium sulfate;
e) + lead nitrate;
e) potassium carbonate + manganese sulfate;
g) + Potassium sulfate.
Equations Record in molecular and ion forms.

■ 112. What kind of substances listed below will react iron chloride (II): a); b) carbonate -calia; c) sodium hydroxide; d) silicon anhydride; e); e) copper hydroxide (II); g)?

113. Describe calcium carbonate properties as medium salt. All equations write down in molecular and ion forms.
114. How to carry out a number of transformations:

All equations write down in molecular and ion forms.
115. What amount of salt will be with the reaction of 8 g of sulfur and 18 g of zinc?
116. What volume of hydrogen is separated by the interaction of 7 g of iron with 20 g of sulfuric acid?
117. How many moles of the cooking salts succeed in reaction of 120 g of caustic soda and 120 g of hydrochloric acid?
118. How many potassium nitrate will be able to react 2 moles of caustic potassium and 130 g of nitric acid?

Hydrolysis of salts

The specific property of salts is their ability to hydrolyze - undergo hydrolysis (from Greek. "Hydro" -d, "lysis" - decomposition), i.e. decomposition under the action of water. It is impossible to consider the hydrolysis of the decomposition in the sense, in which we usually understand this, but it is undoubtedly one thing - in the reaction of hydrolysis is always involved.
- very weak electrolyte, dissociates bad
H 2 O ⇄ H + + he -
And does not change the color of the indicator. Alkali and acids change the color of the indicators, since during their dissociation in the solution, an excess of ions is formed - (in the case of alkalis) and H + ions in the case of acids. In such salts, as NaCl, K 2 of SO 4, which are formed by a strong acid (HSL, H 2 SO 4) and a strong base (NaOH, con), color indicators do not change, as in solving these
Salts hydrolysis practically does not go.
In the hydrolysis of salts, four cases are possible depending on whether the salt is formed with strong or weak acid and the base is formed.
1. If we take a salt of a strong base and weak acid, for example, k 2 s, the following will occur. Potassium sulphide dissociates on ions as a strong electrolyte:
K 2 s ⇄ 2k + + s 2-
Along with this, weakly dissociate:
H 2 O ⇄ H + + OH -
Sulfur Anion S 2 is an anion of weak hydrogen sulfide, which dissociates badly. This leads to the fact that anion S 2 begins to attach the hydrogen cations from the water, gradually forming the most subsidized groups:
S 2- + H + + OH - \u003d HS - + OH -
HS - + H + + OH - \u003d H 2 S + OH -
Since the cations of H + from the water are binding, and the anions of it remain, the medium reaction becomes alkaline. Thus, with hydrolysis of salts formed by a strong base and weak acid, the medium reaction is always alkaline.

■ 119. Equality with ion equations, the process of hydrolysis of sodium carbonate.

2. If a salt formed by a weak base and a strong acid is taken, for example, FE (NO 3) 3, then the ions are formed during its dissociation:
Fe (NO 3) 3 ⇄ Fe 3+ + 3No 3 -
The FE3 + cation is a cation of a weak base - iron that dissociates very badly. This leads to the fact that the FE 3+ cation begins to attach an anison to himself - by forming a little dissociating grouping:
Fe 3+ + H + + it - \u003d Fe (OH) 2+ + + H +
And further
Fe (OH) 2+ + H + + it - \u003d Fe (OH) 2 + + H +
Finally, the process can reach the last stage:
Fe (OH) 2 + + H + + it - \u003d Fe (OH) 3 + H +
Consequently, the solution will be excess hydrogen cations.
Thus, with hydrolysis of salt formed by a weak base and strong acid, the medium reaction is always sour.

■ 120. Explain with the help of ion equations, the course of hydrolysis of aluminum chloride.

3. If the salt is formed by a strong osnania and severe acid, then neither the cation nor an anion binds the water ions and the reaction remains neutral. Hydrolysis practically does not occur.
4. If the salt is formed by a weak base and weak acid, the reaction of the medium depends on their degree of dissociation. If the base and acid have almost the same, then the reaction of the medium will be neutral.

■ 121. It is often necessary to see how a metal precipitate falls instead of the expected precipitate of salt, for example, when reactions between iron (III) chloride (III) FECL 3 and sodium carbonate, Na 2 Co 3 is formed. Fe 2 (CO 3) 3, A Fe ( OH) 3. Explain this phenomenon.
122. Among the salts listed below, specify those that are subjected to hydrolysis in the solution: KNO 3, CR 2 (SO 4) 3, AL 2 (CO 3) 3, CaCl 2, K 2 SiO 3, Al 2 (SO 3) 3.

Features of the properties of acidic salts

Some other properties in acidic salts. They can enter into reactions with preservation and with the destruction of acid ion. For example, an acidic salt reaction with alkali leads to neutralization of acid salt and the destruction of acid ion, for example:
NaHSO4 + Kon \u003d Knaso4 + H2O
Double salt
Na + + HSO 4 - + K + + it - \u003d K + + Na + + SO 2 4 - + H2O
HSO 4 - + OH - \u003d SO 2 4 - + H2O
The destruction of sour ion can be represented as follows:
HSO 4 - ⇄ H + + SO 4 2-
H + + SO 2 4 - + OH - \u003d SO 2 4 - + H2O
The sour ion is destroyed and when reactions with acids:
Mg (HCO3) 2 + 2NSL \u003d MGCL2 + 2N2SO3
Mg 2+ + 2Nox 3 - + 2N + + 2SL - \u003d MG 2+ + 2SL - + 2N2O + 2СO2
2Nox 3 - + 2N + \u003d 2N2O + 2СO2
HCO 3 - + H + \u003d H2O + CO2
Neutralization can be carried out by the same alkali, which is formed by salt:
NaHSO4 + NaOH \u003d Na2SO4 + H2O
Na + + HSO 4 - + Na + + it - \u003d 2NA + + SO 4 2- + H2O
HSO 4 - + OH - \u003d SO 4 2- + H2O
The reactions with salts proceed without the destruction of sour ion:
SA (NSO3) 2 + Na2CO3 \u003d Saso3 + 2NAHCO3
Ca 2+ + 2NSO 3 - + 2NA + + CO 2 3 - \u003d CaCO3 ↓ + 2NA + + 2NSO 3 -
CA 2+ + CO 2 3 - \u003d Caco3
■ 123. Write the equations of the following reactions in the molecular and ionic forms:
a) potassium hydrosulfide +;
b) sodium hydrophosphate + caustic potassium;
c) calcium dihydrophosphate + sodium carbonate;
d) Barium bicarbonate + potassium sulfate;
e) calcium hydrosulfit +.

Obtaining salts

Based on the studied properties of the main classes of inorganic substances, 10 methods of obtaining salts can be derived.
1. Metal interaction with non-metallol:
2NA + CL2 \u003d 2NACL
In this way, only salts of oxygenic acids can be obtained. This is not an ionic reaction.
2. Metal interaction with acid:
Fe + H2SO4 \u003d FESO4 + H2
Fe + 2H + + SO 2 4 - \u003d Fe 2+ + SO 2 4 - + H2
Fe + 2H + \u003d Fe 2+ + H2
3. Metal interaction with salt:
CU + 2AGNO3 \u003d CU (NO3) 2 + 2AG ↓
Cu + 2Ag + + 2NO 3 - \u003d Cu 2+ 2NO 3 - + 2AG ↓
Cu + 2Ag + \u003d Cu 2+ + 2Ag
4. The interaction of the main oxide with acid:
Cuo + H2SO4 \u003d CUSO4 + H2O
Cuo + 2H + + SO 2 4 - \u003d Cu 2+ + SO 2 4 - + H2O
Cuo + 2n + \u003d Cu 2+ + H2O
5. The interaction of the main oxide with an acid anhydride:
3CAO + P2O5 \u003d CA3 (PO4) 2
Reaction is not ionic.
6. The interaction of acid oxide with the base:
CO2 + SA (OH) 2 \u003d Caco3 + H2O
CO2 + CA 2+ + 2OH - \u003d Caco3 + H2O
7, the interaction of acids with the base (neutralization):
HNO3 + KOH \u003d KNO3 + H2O
H + + NO 3 - + K + + OH - \u003d K + + NO 3 - + H2O
H + + OH - \u003d H2O

Saltscomplex substances are called molecules, consist of metals and acid residual atoms (sometimes hydrogen can contain). For example, NaCl - sodium chloride, CASO 4 - calcium sulfate, etc.

Practically all salts are ion connections, Therefore, ions of acid residues and metal ions are connected in salts among themselves:

Na + Cl - - sodium chloride

Ca 2+ SO 4 2- - calcium sulfate, etc.

Salt is a product of partial or complete substitution with metal atoms of hydrogen acid. From here distinguished next species salts:

1. Middle Salts- All hydrogen atoms in acid substituted with metal: Na 2 CO 3, KNO 3, etc.

2. Sour salts - Not all hydrogen atoms in acid are substituted with metal. Of course, acidic salts can form only two- or multi-axis acids. Simple acids of acidic salts can not be given: NaHCO 3, NAH 2 PO 4 IT. d.

3. Double salts - hydrogen atoms of two- or polypic acid are substituted with a non-one metal, but two different: NAKCO 3, KAL (SO 4) 2, etc.

4. Basic salts It can be considered as incomplete, or partial products, replacement of hydroxyl base groups with acid residues: AL (OH) SO 4, Zn (OH) Cl, etc.

In the international nomenclature, the name of the salt of each acid comes from the Latin name of the element. For example, sulfuric acid salts are called sulfates: CaSo 4 - calcium sulfate, MG SO 4 - magnesium sulfate, etc.; Salt hydrochloric acids are called chlorides: NaCl - sodium chloride, Znci 2 - zinc chloride, etc.

A particle "bi" or "hydro": Mg (HCl 3) 2 - bicarbonate or magnesium bicarbonate is added to the name of dioxide salts.

Provided that only one hydrogen atom is replaced in three-axis acid, then the "Dihydro" prefix is \u200b\u200badded: NAH 2 PO 4 - sodium dihydrophosphate.

Salts are solid substances with the most varying solubility in water.

Chemical properties Salley

Chemical properties of salts are determined by the properties of cations and anions, which are included in their composition.

1. Some salts decompose when calcining:

Caco 3 \u003d Cao + Co 2

2. interact with acidswith the formation of a new salt and a new acid. To carry out this reaction, it is necessary that the acid is stronger than the salt on which the acid affects:

2NACL + H 2 SO 4 → Na 2 SO 4 + 2HCl.

3. Interact with the groundsBy forming a new salt and a new base:

Ba (OH) 2 + Mg SO 4 → Baso 4 ↓ + Mg (OH) 2.

4. interact with each otherwith the formation of new salts:

NaCl + AGNO 3 → AGCl + Nano 3.

5. interact with metals, Which stand in the rudd of activity to a metal, which is part of the salt:

Fe + Cuso 4 → Feso 4 + Cu ↓.

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Saltscomplex substances are called molecules, consist of metals and acid residual atoms (sometimes hydrogen can contain). For example, NaCl - sodium chloride, CASO 4 - calcium sulfate, etc.

Practically all salts are ion connections, Therefore, ions of acid residues and metal ions are connected in salts among themselves:

Na + Cl - - sodium chloride

Ca 2+ SO 4 2- - calcium sulfate, etc.

Salt is a product of partial or complete substitution with metal atoms of hydrogen acid. From here, the following types of salts are distinguished:

1. Middle Salts- All hydrogen atoms in acid substituted with metal: Na 2 CO 3, KNO 3, etc.

2. Sour salts - Not all hydrogen atoms in acid are substituted with metal. Of course, acidic salts can form only two- or multi-axis acids. Simple acids of acidic salts can not be given: NaHCO 3, NAH 2 PO 4 IT. d.

3. Double salts - hydrogen atoms of two- or polypic acid are substituted with a non-one metal, but two different: NAKCO 3, KAL (SO 4) 2, etc.

4. Basic salts It can be considered as incomplete, or partial products, replacement of hydroxyl base groups with acid residues: AL (OH) SO 4, Zn (OH) Cl, etc.

In the international nomenclature, the name of the salt of each acid comes from the Latin name of the element. For example, sulfuric acid salts are called sulfates: CaSo 4 - calcium sulfate, MG SO 4 - magnesium sulfate, etc.; Salt hydrochloric acids are called chlorides: NaCl - sodium chloride, Znci 2 - zinc chloride, etc.

A particle "bi" or "hydro": Mg (HCl 3) 2 - bicarbonate or magnesium bicarbonate is added to the name of dioxide salts.

Provided that only one hydrogen atom is replaced in three-axis acid, then the "Dihydro" prefix is \u200b\u200badded: NAH 2 PO 4 - sodium dihydrophosphate.

Salts are solid substances with the most varying solubility in water.

Chemical properties of salts

Chemical properties of salts are determined by the properties of cations and anions, which are included in their composition.

1. Some salts decompose when calcining:

Caco 3 \u003d Cao + Co 2

2. interact with acidswith the formation of a new salt and a new acid. To carry out this reaction, it is necessary that the acid is stronger than the salt on which the acid affects:

2NACL + H 2 SO 4 → Na 2 SO 4 + 2HCl.

3. Interact with the groundsBy forming a new salt and a new base:

Ba (OH) 2 + Mg SO 4 → Baso 4 ↓ + Mg (OH) 2.

4. interact with each otherwith the formation of new salts:

NaCl + AGNO 3 → AGCl + Nano 3.

5. interact with metals, Which stand in the rudd of activity to a metal, which is part of the salt:

Fe + Cuso 4 → Feso 4 + Cu ↓.

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When you hear the word "salt", then the first association, of course, cook, without which any dish will seem tasteless. But this is not the only substance that refers to the class of chemicals of salt. Examples, composition and chemical properties of salts can be found in this article, and learn how to properly make the name of any of them. Before continuing, let's agree, in this article we will consider only inorganic medium salts (obtained in the reaction of inorganic acids with a complete substitution of hydrogen).

Definition and chemical

One of the definitions of salt sounds like this:

• (i.e. consisting of two parts), which consists of metal ions and acid residue. That is, this substance obtained as a result of the reaction of acid and hydroxide (oxide) of any metal.

There is another definition:

• This compound is a product of full or partial replacement of acid hydrogen ions by metal ions (suitable for medium, basic and acidic).

Both definition are correct, but do not reflect the entire essence of the salt process.

Classification of salts

Considering various salting class representatives, you can see what they happen:

• Oxygen-containing (salts of sulfur, nitric, silicon and other acids, whose acid residue includes oxygen and another non-metal).
• Oxygen-free, that is, the salts formed in the reaction of the residue of which does not contain oxygen - salt, borome hydrogen, hydrogen sulfide and others.

By the number of substituted hydrogen:

• Monasual: hydrochloric, nitric, humidiform and others. The composition of the acid includes one hydrogen ion.
• Buses: Two hydrogen ions are substituted with metal ions when salting. Examples: sulfur, sulfur, hydrogen sulfide and others.
• Three-axle: in the composition of acid, three hydrogen ions are substituted with metal ions: phosphoric.

There are other types of classifications in composition and properties, but we will not disassemble them, since the purpose of the article is a little different.

Learning to call correct

Any substance has a name that is understandable only to residents of a certain region, it is also called trivial. Craw salt - an example of a spoken name, on the international nomenclature it will be called differently. But in a conversation, absolutely anyone familiar with the nomenclature of titles will understand without any problems that it is a matter of substance with the chemical formula NaCl. This salt is derived from hydrochloric acid, and its salts are called chlorides, that is, it is called sodium chloride. It is necessary to simply learn the names of the salts below in the table, and then add the name of the metal formed salt.

But so simply is the name, if the metal has unchanged valence. And now consider with the title), which has a metal with a variable valence - FECL 3. The substance is called chloride of iron trivalent. This is the correct name correct!

Chemical properties

As a class, salts in their chemical properties are characterized by the fact that they can interact with alkalis, acids, salts and more active metals:

1. When interacting with alkalis in solution, a prerequisite for the reaction is precipitation of one of the obtained substances.

2. When acid interacts with acids, the reaction passes if volatile acid is formed, insoluble acid or insoluble salt. Examples:

• The carbonic acid includes coal, as it is easily disintegrated by water and carbon dioxide: MGCO 3 + 2HCl \u003d MgCl 2 + H 2 O + CO 2.
• Insoluble acid - silica, is formed as a result of a silicate reaction with a different acid.
• One of the signs of a chemical reaction is precipitation. What salts can be viewed in the solubility table.

3. The interaction of the salts among themselves is only in the case of the binding of ions, i.e., one of the resulting salts falls into a precipitate.

4. To determine whether the reaction will go between the metal and salt, you need to refer to the metal voltage table (sometimes it is also called a number of activity).

Only more active metals (located left) can exhibit metal from salt. An example is the reaction of an iron nail with a copper vigor:

Cuso 4 + Fe \u003d Cu + Feso 4

Such reactions are characteristic of most salting class representatives. But there are more specific reactions in chemistry, the properties of the salt are individual reflecting, for example, decomposition during influenza or the formation of crystallohydrates. Each salt is individual and in its own way unusual.