Nitric acid HNO 3 is a colorless liquid, has a pungent odor, and evaporates easily. If it comes into contact with the skin, nitric acid can cause severe burns (a characteristic yellow spot forms on the skin, it should immediately be washed with plenty of water and then neutralized with NaHCO 3 soda)

Nitric acid

Molecular formula: HNO 3 , B(N) = IV, C.O. (N) = +5

The nitrogen atom forms 3 bonds with oxygen atoms by the exchange mechanism and 1 bond by the donor-acceptor mechanism.

Physical Properties

Anhydrous HNO 3 at ordinary temperature is a colorless volatile liquid with a specific odor (bp 82.6 "C).

Concentrated "fuming" HNO 3 has a red or yellow color, as it decomposes with the release of NO 2 . Nitric acid is miscible with water in any ratio.

How to get

I. Industrial - 3-stage synthesis according to the scheme: NH 3 → NO → NO 2 → HNO 3

Stage 1: 4NH 3 + 5O 2 = 4NO + 6H 2 O

Stage 2: 2NO + O 2 = 2NO 2

Stage 3: 4NO 2 + O 2 + 2H 2 O = 4HNO 3

II. Laboratory - prolonged heating of saltpeter with conc. H2SO4:

2NaNO 3 (solid) + H 2 SO 4 (conc.) = 2HNO 3 + Na 2 SO 4

Ba (NO 3) 2 (tv) + H 2 SO 4 (conc.) = 2HNO 3 + BaSO 4

Chemical properties

HNO 3 as a strong acid exhibits all the general properties of acids

HNO 3 → H + + NO 3 -

HNO 3 is a very reactive substance. In chemical reactions, it manifests itself as a strong acid and as a strong oxidizing agent.

HNO 3 interacts:

a) with metal oxides 2HNO 3 + CuO = Cu(NO 3) 2 + H 2 O

b) with bases and amphoteric hydroxides 2HNO 3 + Cu(OH) 2 = Cu(NO 3) 2 + 2H 2 O

c) with salts of weak acids 2HNO 3 + CaCO 3 = Ca(NO 3) 2 + CO 2 + H 2 O

d) with ammonia HNO 3 + NH 3 = NH 4 NO 3

The difference between HNO 3 and other acids

1. When HNO 3 interacts with metals, H 2 is almost never released, since H + ions of the acid do not participate in the oxidation of metals.

2. Instead of H + ions, NO 3 - anions have an oxidizing effect.

3. HNO 3 is capable of dissolving not only metals located in the activity row to the left of hydrogen, but also low-active metals - Cu, Ag, Hg. In a mixture with HCl, it also dissolves Au, Pt.

HNO 3 is a very strong oxidizing agent

I. Oxidation of metals:

Interaction of HNO 3: a) with low and medium activity Me: 4HNO 3 (conc.) + Сu = 2NO 2 + Cu(NO 3) 2 + 2H 2 O

8HNO 3 (razb.) + 3Сu \u003d 2NO + 3Cu (NO 3) 2 + 4H 2 O

b) with active Me: 10HNO 3 (razb.) + 4Zn \u003d N 2 O + 4Zn (NO 3) 2 + 5H 2 O

c) with alkaline and alkaline earth Me: 10HNO 3 (very dilute) + 4Са = NH 4 NO 3 + 4Ca (NO 3) 2 + 3H 2 O

Very concentrated HNO 3 at normal temperature does not dissolve some metals, including Fe, Al, Cr.

II. Oxidation of non-metals:

HNO 3 oxidizes P, S, C to their higher S.O., while itself is reduced to NO (HNO 3 dilute) or to NO 2 (HNO 3 conc).

5HNO 3 + P \u003d 5NO 2 + H 3 PO 4 + H 2 O

2HNO 3 + S = 2NO + H 2 SO 4

III. Oxidation of complex substances:

Particularly important are the oxidation reactions of certain Me sulfides, which are insoluble in other acids. Examples:

8HNO 3 + PbS \u003d 8NO 2 + PbSO 4 + 4H 2 O

22HNO 3 + 3Сu 2 S \u003d 10NO + 6Cu (NO 3) 2 + 3H 2 SO 4 + 8H 2 O

HNO 3 - nitrating agent in organic synthesis reactions

R-H + HO-NO 2 → R-NO 2 + H 2 O

C 2 H 6 + HNO 3 → C 2 H 5 NO 2 + H 2 O nitroethane

C 6 H 5 CH 3 + 3HNO 3 → C 6 H 2 (NO 2) 3 CH 3 + ZH 2 O trinitrotoluene

C 6 H 5 OH + 3HNO 3 → C 6 H 5 (NO 2) 3 OH + ZH 2 O trinitrophenol

HNO 3 esterifies alcohols

R-OH + HO-NO 2 → R-O-NO 2 + H 2 O

C 3 H 5 (OH) 3 + 3HNO 3 → C 3 H 5 (ONO 2) 3 + ZH 2 O glycerol trinitrate

Decomposition of HNO 3

When stored in the light, and especially when heated, HNO 3 molecules decompose due to intramolecular redox:

4HNO 3 \u003d 4NO 2 + O 2 + 2H 2 O

A red-brown poisonous gas NO 2 is released, which enhances the aggressive oxidizing properties of HNO 3

Salts of nitric acid - nitrates Me (NO 3) n

Nitrates are colorless crystalline substances, soluble in water. They have chemical properties characteristic of typical salts.

Distinctive features:

1) redox decomposition when heated;

2) strong oxidizing properties of molten alkali metal nitrates.

Thermal decomposition

1. Decomposition of nitrates of alkali and alkaline earth metals:

Me(NO 3) n → Me(NO 2) n + O 2

2. Decomposition of metal nitrates in the activity series of metals from Mg to Cu:

Me(NO 3) n → Me x O y + NO 2 + O 2

3. Decomposition of metal nitrates in the activity series of metals above Cu:

Me(NO 3) n → Me + NO 2 + O 2

Examples of typical reactions:

1) 2NaNO 3 \u003d 2NaNO 2 + O 2

2) 2Cu(NO 3) 2 = 2CuO + 4NO 2 + O 2

3) 2AgNO 3 \u003d 2Ag + 2NO 2 + O 2

Oxidative action of melts of alkali metal nitrates

In aqueous solutions, nitrates, in contrast to HNO 3 , show almost no oxidative activity. However, melts of alkali metal and ammonium nitrates (nitrate) are strong oxidizing agents, since they decompose with the release of active oxygen.

Nitrous and nitric acids and their salts

Nitrous acid exists either in solution or in the gas phase. It is unstable and decomposes in vapors when heated:

2HNO 2 "NO + NO 2 + H 2 O

Aqueous solutions of this acid decompose when heated:

3HNO 2 "HNO 3 + H 2 O + 2NO

This reaction is reversible, therefore, although the dissolution of NO 2 is accompanied by the formation of two acids: 2NO 2 + H 2 O \u003d HNO 2 + HNO 3

practically by the interaction of NO 2 with water, HNO 3 is obtained:

3NO 2 + H 2 O \u003d 2HNO 3 + NO

In terms of acidic properties, nitrous acid is only slightly stronger than acetic acid. Its salts are called nitrites and, unlike the acid itself, are stable. From solutions of its salts, by adding sulfuric acid, a solution of HNO 2 can be obtained:

Ba(NO 2) 2 + H 2 SO 4 \u003d 2HNO 2 + BaSO 4 ¯

Based on data on its compounds, two types of structure of nitrous acid are suggested:

which correspond to nitrites and nitro compounds. Nitrites of active metals have a type I structure, and low-active metals - type II. Almost all salts of this acid are highly soluble, but silver nitrite is the most difficult of all. All salts of nitrous acid are poisonous. For chemical technology, KNO 2 and NaNO 2 are important, which are necessary for the production of organic dyes. Both salts are obtained from nitrogen oxides:

NO + NO 2 + NaOH \u003d 2NaNO 2 + H 2 O or when their nitrates are heated:

KNO 3 + Pb \u003d KNO 2 + PbO

Pb is needed to bind the released oxygen.

Of the chemical properties of HNO 2, oxidative ones are more pronounced, while it itself is reduced to NO:

However, many examples of such reactions can be given, where nitrous acid exhibits reducing properties:

The presence of nitrous acid and its salts in a solution can be determined by adding a solution of potassium iodide and starch. The nitrite ion oxidizes the iodine anion. This reaction requires the presence of H + , i.e. runs in an acidic environment.

Nitric acid

Under laboratory conditions, nitric acid can be obtained by the action of concentrated sulfuric acid on nitrates:

NaNO 3 + H 2 SO 4 (c) \u003d NaHSO 4 + HNO 3 The reaction proceeds with slight heating.

Obtaining nitric acid on an industrial scale is carried out by catalytic oxidation of ammonia with atmospheric oxygen:

1. First, a mixture of ammonia and air is passed over a platinum catalyst at 800°C. Ammonia is oxidized to nitric oxide (II):

4NH 3 + 5O 2 \u003d 4NO + 6H 2 O

2. Upon cooling, NO is further oxidized to NO 2: 2NO + O 2 \u003d 2NO 2

3. The resulting nitric oxide (IV) dissolves in water in the presence of excess O 2 to form HNO 3: 4NO 2 + 2H 2 O + O 2 \u003d 4HNO 3

The starting products - ammonia and air - are thoroughly cleaned of harmful impurities that poison the catalyst (hydrogen sulfide, dust, oils, etc.).

The resulting acid is dilute (40-60%). Concentrated nitric acid (96-98%) is obtained by distillation of dilute acid mixed with concentrated sulfuric acid. In this case, only nitric acid evaporates.

Physical Properties

Nitric acid is a colorless liquid with a pungent odor. Very hygroscopic, "smoke" in the air, because. its vapors with air moisture form fog drops. Miscible with water in any ratio. At -41.6°C it passes into a crystalline state. Boils at 82.6°C.

In HNO 3, the nitrogen valence is 4, the oxidation state is +5. The structural formula of nitric acid is depicted as follows:

Both oxygen atoms, bound only to nitrogen, are equivalent: they are at the same distance from the nitrogen atom and each carry a half electron charge, i.e. a quarter of the nitrogen is divided equally between the two oxygen atoms.

The electronic structure of nitric acid can be derived as follows:

1. A hydrogen atom is bound to an oxygen atom by a covalent bond:

2. Due to the unpaired electron, the oxygen atom forms a covalent bond with the nitrogen atom:

3. Two unpaired electrons of the nitrogen atom form a covalent bond with the second oxygen atom:

4. The third oxygen atom, being excited, forms a free 2p- orbital by electron pairing. The interaction of a lone pair of nitrogen with a free orbital of the third oxygen atom leads to the formation of a nitric acid molecule:

Chemical properties

1. Diluted nitric acid exhibits all the properties of acids. It belongs to strong acids. Dissociates in aqueous solutions:

HNO 3 "H + + NO - 3 Under the influence of heat and in the light, it partially decomposes:

4HNO 3 \u003d 4NO 2 + 2H 2 O + O 2 Therefore, store it in a cool and dark place.

2. Nitric acid is characterized by exclusively oxidizing properties. The most important chemical property is the interaction with almost all metals. Hydrogen is never released. The recovery of nitric acid depends on its concentration and the nature of the reducing agent. The degree of nitrogen oxidation in the reduction products is in the range from +4 to -3:

HN +5 O 3 ®N +4 O 2 ®HN +3 O 2 ®N +2 O®N +1 2 O®N 0 2 ®N -3 H 4 NO 3

The reduction products in the interaction of nitric acid of different concentrations with metals of different activity are shown below in the scheme.

Concentrated nitric acid at normal temperature does not interact with aluminum, chromium, iron. She puts them in a passive state. A film of oxides forms on the surface, which is impermeable to concentrated acid.

3. Nitric acid does not react with Pt, Rh, Ir, Ta, Au. Platinum and gold are dissolved in "aqua regia" - a mixture of 3 volumes of concentrated hydrochloric acid and 1 volume of concentrated nitric acid:

Au + HNO 3 + 3HCl \u003d AuCl 3 + NO + 2H 2 O HCl + AuCl 3 \u003d H

3Pt + 4HNO 3 + 12HCl \u003d 3PtCl 4 + 4NO + 8H 2 O 2HCl + PtCl 4 \u003d H 2

The action of "royal vodka" is that nitric acid oxidizes hydrochloric acid to free chlorine:

HNO 3 + HCl \u003d Cl 2 + 2H 2 O + NOCl 2NOCl \u003d 2NO + Cl 2 The released chlorine combines with metals.

4. Non-metals are oxidized by nitric acid to the corresponding acids, and depending on the concentration, it is reduced to NO or NO 2:

S + bHNO 3 (conc) \u003d H 2 SO 4 + 6NO 2 + 2H 2 OR + 5HNO 3 (conc) \u003d H 3 PO 4 + 5NO 2 + H 2 O I 2 + 10HNO 3 (conc) \u003d 2HIO 3 + 10NO 2 + 4H 2 O 3P + 5HNO 3 (p azb) + 2H 2 O \u003d 3H 3 RO 4 + 5NO

5. It also interacts with organic compounds.

Salts of nitric acid are called nitrates, they are crystalline substances that are highly soluble in water. They are obtained by the action of HNO 3 on metals, their oxides and hydroxides. Potassium, sodium, ammonium and calcium nitrates are called saltpeters. Saltpeter is used mainly as a mineral nitrogen fertilizer. In addition, KNO 3 is used to prepare black powder (a mixture of 75% KNO 3 , 15% C and 10% S). Ammonal explosive is made from NH 4 NO 3, aluminum powder and trinitrotoluene.

Salts of nitric acid decompose when heated, and the decomposition products depend on the position of the salt-forming metal in a series of standard electrode potentials:

Decomposition upon heating (thermolysis) is an important property of nitric acid salts.

2KNO 3 \u003d 2KNO 2 + O 2

2Cu(NO 3) 2 \u003d 2CuO + NO 2 + O 2

Metal salts located in the row to the left of Mg form nitrites and oxygen, from Mg to Cu - metal oxide, NO 2 and oxygen, after Cu - free metal, NO 2 and oxygen.

Application

Nitric acid is the most important product of the chemical industry. Large quantities are spent on the preparation of nitrogen fertilizers, explosives, dyes, plastics, artificial fibers, and other materials. fuming

nitric acid is used in rocket technology as an oxidizing agent for rocket fuel.

A monobasic strong acid, which is a colorless liquid under standard conditions, which turns yellow during storage, can be in a solid state, characterized by two crystalline modifications (monoclinic or rhombic lattices), at temperatures below minus 41.6 °C. This substance with the chemical formula - HNO3 - is called nitric acid. It has a molar mass of 63.0 g / mol, and its density corresponds to 1.51 g / cm³. The boiling point of the acid is 82.6 °C, the process is accompanied by decomposition (partial): 4HNO3 → 2H2O + 4NO2 + O2. An acid solution with a mass fraction of the basic substance equal to 68% boils at a temperature of 121 °C. pure substance corresponds to 1.397. The acid is able to mix with water in any ratio and, being a strong electrolyte, almost completely decompose into H+ and NO3- ions. Solid forms - trihydrate and monohydrate have the formulas: HNO3. 3H2O and HNO3. H2O respectively.

Nitric acid is a corrosive, toxic substance and a strong oxidizing agent. Since the Middle Ages, such a name as "strong water" (Aqua fortis) has been known. The alchemists, who discovered acid in the 13th century, gave this name, making sure of its extraordinary properties (it corroded all metals except gold), exceeding a million times the strength of acetic acid, which at that time was considered the most active. But after another three centuries, it was found that even gold can be corroded by a mixture of acids such as nitric and hydrochloric in a volume ratio of 1: 3, which for this reason was called “aqua regia”. The appearance of a yellow tint during storage is due to the accumulation of nitrogen oxides in it. On sale, the acid is more often with a concentration of 68%, and when the content of the main substance is more than 89%, it is called "fuming".

The chemical properties of nitric acid distinguish it from dilute sulfuric or hydrochloric acids in that HNO3 is a stronger oxidizing agent, so hydrogen is never released in reactions with metals. Due to its oxidizing properties, it also reacts with many non-metals. In both cases, nitrogen dioxide NO2 is always formed. In redox reactions, nitrogen reduction occurs to varying degrees: HNO3, NO2, N2O3, NO, N2O, N2, NH3, which is determined by the acid concentration and metal activity. The molecules of the resulting compounds contain nitrogen with the oxidation state: +5, +4, +3, +2, +1, 0, +3, respectively. For example, copper is oxidized with concentrated acid to copper(II) nitrate: Cu + 4HNO3 → 2NO2 + Cu(NO3)2 + 2H2O, and phosphorus to metaphosphoric acid: P + 5HNO3 → 5NO2 + HPO3 + 2H2O.

Otherwise, dilute nitric acid interacts with non-metals. The example of the reaction with phosphorus: 3P + 5HNO3 + 2H2O → 3H3PO4 + 5NO shows that nitrogen is reduced to the divalent state. As a result, nitrogen monoxide is formed, and phosphorus is oxidized to Concentrated nitric acid mixed with hydrochloric acid dissolves gold: Au + 4HCl + HNO3 → NO + H + 2H2O and platinum: 3Pt + 18HCl + 4HNO3 → 4NO + 3H2 + 8H2O. In these reactions, at the initial stage, hydrochloric acid is oxidized with nitric acid with the release of chlorine, and then the metals form complex chlorides.

Nitric acid on an industrial scale is produced in three main ways:

1. The first one is the interaction of salts with sulfuric acid: H2SO4 + NaNO3 → HNO3 + NaHSO4. Previously, this was the only way, but, with the advent of other technologies, it is currently used in the laboratory to obtain fuming acid.
2. The second is the arc method. When air is blown through with a temperature of 3000 to 3500 ° C, part of the nitrogen in the air reacts with oxygen, and nitrogen monoxide is formed: N2 + O2 → 2NO, which, after cooling, is oxidized to nitrogen dioxide (at high temperatures, monoxide does not interact with oxygen): O2 + 2NO → 2NO2. Then, almost all nitrogen dioxide, with an excess of oxygen, dissolves in water: 2H2O + 4NO2 + O2 → 4HNO3.
3. The third is the ammonia method. Ammonia is oxidized on a platinum catalyst to nitrogen monoxide: 4NH3 + 5O2 → 4NO + 6H2O. The resulting nitrous gases are cooled and nitrogen dioxide is formed, which is absorbed by water. This method produces an acid with a concentration of 60 to 62%.

Nitric acid is widely used in industry for the production of drugs, dyes, nitrogen fertilizers and nitric acid salts. In addition, it is used to dissolve metals (eg copper, lead, silver) that do not react with other acids. In jewelry, it is used to determine gold in an alloy (this method is the main one).

Structural formula

True, empirical, or gross formula: HNO3

Chemical composition of nitric acid

Molecular weight: 63.012

Nitric acid ( HNO3) is a strong monobasic acid. Solid nitric acid forms two crystalline modifications with monoclinic and rhombic lattices.

Nitric acid is miscible with water in any ratio. In aqueous solutions, it almost completely dissociates into ions. It forms an azeotropic mixture with water with a concentration of 68.4% and a bp t of 120 °C at normal atmospheric pressure. Two solid hydrates are known: monohydrate (HNO 3 ·H 2 O) and trihydrate (HNO 3 ·3H 2 O).

Nitrogen in nitric acid is tetravalent, oxidation state +5. Nitric acid is a colorless liquid fuming in air, melting point −41.59 °C, boiling point +82.6 °C (at normal atmospheric pressure) with partial decomposition. Nitric acid is miscible with water in all proportions. Aqueous solutions of HNO 3 with a mass fraction of 0.95-0.98 are called "fuming nitric acid", with a mass fraction of 0.6-0.7 - concentrated nitric acid. Forms an azeotropic mixture with water (mass fraction 68.4%, d20 = 1.41 g/cm, Tbp = 120.7 °C)

Highly concentrated HNO 3 usually has a brown color due to the decomposition process taking place in the light. When heated, nitric acid decomposes by the same reaction. Nitric acid can only be distilled without decomposition under reduced pressure (the indicated boiling point at atmospheric pressure is found by extrapolation).

Gold, some metals of the platinum group and tantalum are inert to nitric acid in the entire range of concentrations, the rest of the metals react with it, the course of the reaction is determined by its concentration.

Nitric acid in any concentration exhibits the properties of an oxidizing acid, while nitrogen is reduced to an oxidation state of +5 to −3. The depth of reduction depends primarily on the nature of the reducing agent and on the concentration of nitric acid.

A mixture of nitric and sulfuric acids is called melange.

Nitric acid is widely used to obtain nitro compounds.

A mixture of three volumes of hydrochloric acid and one volume of nitric acid is called aqua regia. Aqua regia dissolves most metals, including gold and platinum. Its strong oxidizing ability is due to the resulting atomic chlorine and nitrosyl chloride.

Nitric acid is a strong acid. Its salts - nitrates - are obtained by the action of HNO 3 on metals, oxides, hydroxides or carbonates. All nitrates are highly soluble in water. The nitrate ion does not hydrolyze in water. Nitrates are widely used as fertilizers. At the same time, almost all nitrates are highly soluble in water, therefore, in the form of minerals, they are extremely small in nature; the exceptions are Chilean (sodium) nitrate and Indian nitrate (potassium nitrate). Most nitrates are obtained artificially.

According to the degree of impact on the body, nitric acid belongs to substances of the 3rd hazard class. Its vapors are very harmful: the vapors cause irritation of the respiratory tract, and the acid itself leaves long-healing ulcers on the skin. When exposed to the skin, a characteristic yellow coloration of the skin occurs due to the xantoprotein reaction. When heated or exposed to light, the acid decomposes to form highly toxic nitrogen dioxide NO 2 (brown gas). MPC for nitric acid in the air of the working area for NO 2 2 mg/m 3 .

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Highly concentrated HNO 3 usually has a brown color due to the decomposition process taking place in the light:

When heated, nitric acid decomposes according to the same reaction. Nitric acid can only be distilled (without decomposition) under reduced pressure (the indicated boiling point at atmospheric pressure is found by extrapolation).

Gold, some metals of the platinum group and tantalum are inert to nitric acid in the entire range of concentrations, the rest of the metals react with it, the course of the reaction is also determined by its concentration.

HNO 3 as a strong monobasic acid interacts:

a) with basic and amphoteric oxides:

c) displaces weak acids from their salts:

When boiling or exposed to light, nitric acid partially decomposes:

Nitric acid in any concentration exhibits the properties of an oxidizing acid, in addition, nitrogen is reduced to an oxidation state of +4 to 3. The depth of reduction depends primarily on the nature of the reducing agent and on the concentration of nitric acid. As an oxidizing acid, HNO 3 interacts:

a) with metals standing in a series of voltages to the right of hydrogen:

Concentrated HNO 3

Diluted HNO 3

b) with metals standing in the series of voltages to the left of hydrogen:

All of the above equations reflect only the dominant course of the reaction. This means that under these conditions, the products of this reaction are more than the products of other reactions, for example, when zinc reacts with nitric acid (mass fraction of nitric acid in a solution of 0.3), the products will contain the most NO, but will also contain ( only in smaller quantities) and NO 2 , N 2 O, N 2 and NH 4 NO 3 .

The only general pattern in the interaction of nitric acid with metals: the more dilute the acid and the more active the metal, the deeper nitrogen is reduced:

Increase in acid concentration increase in metal activity

Nitric acid, even concentrated, does not interact with gold and platinum. Iron, aluminum, chromium are passivated with cold concentrated nitric acid. Iron interacts with dilute nitric acid, and, based on the acid concentration, not only various nitrogen reduction products are formed, but also various iron oxidation products:

Nitric acid oxidizes non-metals, while nitrogen is usually reduced to NO or NO 2:

and complex substances, for example:

Some organic compounds (eg amines, turpentine) spontaneously ignite on contact with concentrated nitric acid.

Some metals (iron, chromium, aluminum, cobalt, nickel, manganese, beryllium), which react with dilute nitric acid, are passivated by concentrated nitric acid and are resistant to its effects.

A mixture of nitric and sulfuric acids is called melange.

Nitric acid is widely used to obtain nitro compounds.

A mixture of three volumes of hydrochloric acid and one volume of nitric acid is called aqua regia. Royal vodka dissolves most metals, including gold and platinum. Its strong oxidizing abilities are due to the resulting atomic chlorine and nitrosyl chloride:

Nitrates

Nitric acid is a strong acid. Its salts - nitrates - are obtained by the action of HNO 3 on metals, oxides, hydroxides or carbonates. All nitrates are highly soluble in water. The nitrate ion does not hydrolyze in water.

Salts of nitric acid decompose irreversibly when heated, and the composition of the decomposition products is determined by the cation:

a) nitrates of metals standing in the series of voltages to the left of magnesium:

b) nitrates of metals located in a series of voltages between magnesium and copper:

c) nitrates of metals located in a series of voltages to the right of mercury:

d) ammonium nitrate:

Nitrates in aqueous solutions practically do not show oxidizing properties, but at high temperatures in the solid state they are strong oxidizing agents, for example, when solids are fused:

Zinc and aluminum in an alkaline solution reduce nitrates to NH 3:

Salts of nitric acid - nitrates - are widely used as fertilizers. In addition, almost all nitrates are highly soluble in water, so there are extremely few of them in the form of minerals in nature; the exceptions are Chilean (sodium) nitrate and Indian nitrate (potassium nitrate). Most nitrates are obtained artificially.

Glass, fluoroplast-4 do not react with nitric acid.