Some inorganic acid and salt names
| Acid Formulas | Acid names | Corresponding salt names |
| HClO 4 | chlorine | perchlorates |
| HClO 3 | chloric | chlorates |
| HClO 2 | chloride | chlorites |
| HClO | hypochlorous | hypochlorites |
| H 5 IO 6 | iodine | periodates |
| HIO 3 | iodish | iodates |
| H 2 SO 4 | sulfuric | sulfates |
| H 2 SO 3 | sulphurous | sulfites |
| H 2 S 2 O 3 | thiosulfuric | thiosulfates |
| H 2 S 4 O 6 | tetration | tetrationates |
| H NO 3 | nitrogen | nitrates |
| H NO 2 | nitrogenous | nitrites |
| H 3 PO 4 | orthophosphoric | orthophosphates |
| H PO 3 | metaphosphoric | metaphosphates |
| H 3 PO 3 | phosphorous | phosphites |
| H 3 PO 2 | phosphate | hypophosphites |
| H 2 CO 3 | coal | carbonates |
| H 2 SiO 3 | silicon | silicates |
| HMnO 4 | manganese | permanganates |
| H 2 MnO 4 | manganese | manganates |
| H 2 CrO 4 | chrome | chromates |
| H 2 Cr 2 O 7 | dichromic | dichromats |
| HF | hydrofluoric (hydrofluoric) | fluorides |
| HCl | hydrochloric (hydrochloric) | chlorides |
| HBr | hydrobromic | bromides |
| HI | hydroiodic | iodides |
| H 2 S | hydrogen sulfide | sulfides |
| HCN | cyanide | cyanide |
| HOCN | cyanic | cyanates |
Let me remind you briefly on specific examples how to call salt correctly.
Example 1... The K 2 SO 4 salt is formed by the residue of sulfuric acid (SO 4) and the metal K. Sulfuric acid salts are called sulfates. K 2 SO 4 - potassium sulfate.
Example 2... FeCl 3 - the salt contains iron and the remainder of hydrochloric acid (Cl). Salt name: iron (III) chloride. Please note: in in this case we not only have to name the metal, but also indicate its valence (III). In the previous example, this was not necessary because the valence of sodium is constant.
Important: the name of the salt should indicate the valence of the metal only if the metal has a variable valence!
Example 3... Ba (ClO) 2 - the salt contains barium and the remainder hypochlorous acid(ClO). Salt name: barium hypochlorite. The valency of the metal Ba in all its compounds is equal to two, it is not necessary to indicate it.
Example 4... (NH 4) 2 Cr 2 O 7. The NH 4 group is called ammonium, the valence of this group is constant. Salt name: ammonium dichromate (dichromate).
In the above examples, we only met the so-called. medium or normal salts. Sour, basic, double and complex salts, salt organic acids will not be discussed here.
Acids are complex substances, the molecules of which consist of hydrogen atoms (capable of being replaced by metal atoms) bound to an acid residue.
general characteristics
Acids are classified into oxygen-free and oxygen-containing, as well as organic and inorganic.
Rice. 1. Classification of acids - oxygen-free and oxygen-containing.
Anoxic acids are solutions in water of binary compounds such as hydrogen halides or hydrogen sulfide. In solution, the polar covalent bond between hydrogen and an electronegative element is polarized by the action of dipole water molecules, and the molecules decompose into ions. the presence of hydrogen ions in a substance and allows us to call aqueous solutions these binary compounds with acids.
Acids are called from the name of the binary compound by adding the ending -nay. for example, HF is hydrofluoric acid. The acid anion is called by the name of the element by adding the ending -id, for example, Cl - chloride.
Oxygenated acids (oxo acids)- this is acidic hydroxides, dissociating in an acidic manner, that is, as protoliths. Their general formula is E (OH) mOn, where E is a non-metal or a metal with a variable valence in the highest degree oxidation. provided that n is 0, then the acid is weak (H 2 BO 3 - boric), if n = 1, then the acid is either weak or medium strength (H 3 PO 4 - phosphoric), if n is greater than or equal to 2, then the acid is considered strong (H 2 SO 4).
Rice. 2. Sulfuric acid.
Acidic hydroxides correspond to acidic oxides or acid anhydrides, for example, sulfuric acid corresponds to sulfuric anhydride SO 3.
Chemical properties of acids
Acids have a number of properties that distinguish them from salts and others. chemical elements:
- Action on indicators. How acid protoliths dissociate to form H + ions, which change the color of the indicators: the violet litmus solution turns red, and the orange methyl orange solution turns pink. Polybasic acids dissociate stepwise, and each subsequent stage is more difficult than the previous one, since ever weaker electrolytes dissociate in the second and third steps:
H 2 SO 4 = H + + HSO 4 -
The color of the indicator depends on whether the acid is concentrated or diluted. So, for example, when litmus is dipped into concentrated sulfuric acid, the indicator turns red, while in dilute sulfuric acid the color will not change.
- Neutralization reaction, that is, the interaction of acids with bases, resulting in the formation of salt and water, always takes place if at least one of the reagents is strong (base or acid). The reaction does not proceed if the acid is weak, the base is insoluble. For example, the reaction does not go:
H 2 SiO 3 (weak, water-insoluble acid) + Cu (OH) 2 - the reaction does not go
But in other cases, the neutralization reaction with these reagents goes:
H 2 SiO 3 + 2KOH (alkali) = K 2 SiO 3 + 2H 2 O
- Interaction with basic and amphoteric oxides:
Fe 2 O 3 + 3H 2 SO 4 = Fe 2 (SO 4) 3 + 3H 2 O
- Interaction of acids with metals, standing in a series of voltages to the left of hydrogen, leads to a process as a result of which salt is formed and hydrogen is released. This reaction is easy if the acid is strong enough.
Nitric acid and concentrated sulfuric acid react with metals by reducing not hydrogen, but the central atom:
Mg + H 2 SO 4 + MgSO 4 + H 2
- Interaction of acids with salts occurs when a weak acid is produced as a result. If the salt that reacts with the acid is soluble in water, then the reaction will also proceed if an insoluble salt is formed:
Na 2 SiO 3 (soluble salt of a weak acid) + 2HCl (strong acid) = H 2 SiO 3 (weak insoluble acid) + 2NaCl (soluble salt)
Many acids are used in industry, for example, acetic acid is necessary for preserving meat and fish products.
Acids complex substances are called, the molecules of which include hydrogen atoms that can be replaced or exchanged for metal atoms and an acid residue.
According to 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 anoxic(HF hydrofluoric acid, HCl hydrochloric acid ( hydrochloric acid), HBr hydrobromic acid, HI hydroiodic acid, H 2 S hydrosulphuric acid).
Depending on the number of hydrogen atoms in the acid molecule, there 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.
Acid residues can consist of one atom (-Cl, -Br, -I) - these are simple acid residues, or they can be from a group of atoms (-SO 3, -PO 4, -SiO 3) - these are complex residues.
In aqueous solutions, acid residues are not destroyed during exchange and substitution reactions:
H 2 SO 4 + CuCl 2 → CuSO 4 + 2 HCl
The word anhydride means anhydrous, that is, acid without water. For example,
H 2 SO 4 - H 2 O → SO 3. Anoxic acids have no anhydrides.
The name of the acid is derived from the name of the acid-forming element (acidifier) with the addition of the endings "naya" and less often "vay": 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 name of acids will be when the element exhibits the highest valency (in the acid molecule great content oxygen atoms). If the element exhibits the lowest valence, the ending in the name of the acid will be "true": 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 anoxic acids. Anoxic acids are also obtained by direct synthesis from hydrogen and non-metal, followed by dissolution of the resulting compound in water:
H 2 + Cl 2 → 2 HCl;
H 2 + S → H 2 S.
Solutions obtained gaseous substances HCl and H 2 S and are acids.
Under normal conditions, acids are both liquid and solid.
Chemical properties of acids
A solution of acids affects the indicators. All acids (except for silicic acid) are readily soluble in water. Special substances - indicators allow you to determine the presence of acid.
Indicators are substances complex structure... They change their color depending on interaction with different chemicals. In neutral solutions - they have one color, in base solutions - another. When interacting with an acid, they change their color: the methyl orange indicator turns red, the litmus indicator also turns red.
Interact with bases with the formation of water and salt, which contains an unchanged acidic residue (neutralization reaction):
H 2 SO 4 + Ca (OH) 2 → CaSO 4 + 2 H 2 O.
Interact with based oxides with the formation of water and salt (neutralization reaction). Salt contains an acidic 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 the interaction of acids with metals, certain conditions must be met:
1. the metal must be sufficiently active with respect to acids (in the row of metal activity, it must be located before hydrogen). The more to the left the metal is in the line of activity, the more intensely it interacts with acids;
2. the acid must be strong enough (that is, capable of giving off hydrogen ions H +).
When flowing chemical reactions acid with metals, 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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| Acid formula | Acid name | Salt name | Corresponding oxide |
| HCl | Salt | Chlorides | ---- |
| HI | Hydrogen iodide | Iodides | ---- |
| HBr | Hydrobromic | Bromides | ---- |
| HF | Plavikovaya | Fluoride | ---- |
| HNO 3 | Nitrogen | Nitrates | N 2 O 5 |
| H 2 SO 4 | Sulfur | Sulphates | SO 3 |
| H 2 SO 3 | Sulphurous | Sulfites | SO 2 |
| H 2 S | Hydrogen sulfide | Sulphides | ---- |
| H 2 CO 3 | Coal | Carbonates | CO 2 |
| H 2 SiO 3 | Silicon | Silicates | SiO 2 |
| HNO 2 | Nitrogenous | Nitrite | N 2 O 3 |
| H 3 PO 4 | Phosphoric | Phosphates | P 2 O 5 |
| H 3 PO 3 | Phosphorous | Phosphites | P 2 O 3 |
| H 2 CrO 4 | Chrome | Chromates | CrO 3 |
| H 2 Cr 2 O 7 | Two-chrome | Dichromates | CrO 3 |
| HMnO 4 | Manganese | Permanganates | Mn 2 O 7 |
| HClO 4 | Chlorine | Perchlorates | Cl 2 O 7 |
Acids in the laboratory can be obtained:
1) when dissolving acidic 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.
Usually, acids interact only with those metals that in the electrochemical series of voltages stand up to hydrogen, while free hydrogen is released. Such acids do not interact with low-activity metals (in the electrochemical series, voltages are after hydrogen). Acids, which are strong oxidizing agents (nitric, concentrated sulfuric), react with all metals, except for noble metals (gold, platinum), but this does not release hydrogen, but water and oxide, for example, SO 2 or NO 2.
Salt is the product of the replacement of 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.
The middle salt is the product of complete replacement of hydrogen ions in an acid molecule with metal atoms.
Acidic salts contain hydrogen atoms capable of participating in chemical exchange reactions. In acidic salts, incomplete replacement of hydrogen atoms with metal atoms occurred.
Basic salts are a product of incomplete substitution of hydroxo groups of bases of multivalent metals with acid residues. Basic salts always contain a hydroxyl group.
Medium salts are obtained by 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 grounds:
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 an excess of acid:
H 3 PO 4 + NaOH → NaH 2 PO 4 + H 2 O;
2) in the interaction of medium salts with acids:
CaCO 3 + H 2 CO 3 → Ca (HCO 3) 2;
3) during the hydrolysis of salts formed weak acid:
Na 2 S + H 2 O → NaHS + NaOH.
Basic salts are obtained:
1) in the case of a reaction between a polyvalent metal base and an acid in an excess of a base:
Cu (OH) 2 + HCl → CuOHCl + H 2 O;
2) in the interaction of medium salts with alkalis:
CuCl 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, with 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 goes to the end 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 that is part of the salt:
Fe + CuSO 4 → FeSO 4 + Cu.
For salts, decomposition reactions are also characteristic:
BaCO 3 → BaO + CO 2;
2KClO 3 → 2KCl + 3O 2.
PRODUCTION AND PROPERTIES
BASES, ACIDS AND SALTS
Experience 1. Obtaining alkalis.
1.1. Interaction of metal with water.
Pour distilled water into a crystallizer or porcelain cup (about 1/2 vessel). Get a piece of metallic sodium from the teacher, previously dried with filter paper. Place a lump of sodium in a crystallizer filled with water. At the end of the reaction, add a few drops of phenolphthalein. Note the observed phenomena, write the reaction equation. Name the resulting compound, write down its structural formula.
1.2. Interaction of metal oxide with water.
Pour distilled water (1/3 of the tube) into a test tube and place a lump of CaO into it, mix thoroughly, add 1 - 2 drops of phenolphthalein. Mark the observed phenomena, write the reaction equation. Name the resulting compound, give its structural formula.
