Production of nitric acid in industry presentation. Presentation on the topic "nitric acid". The structure of the nitric acid molecule
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Obtaining nitric acid PREPARED: a student of grade 9 b gymnasium №1 named. Yu.A. Gagarina Mikhalchenko Ksenia.
Physical properties nitric acid Physical state: liquid Color: colorless Odor: pungent Density: 1.5 2 g / cm 3 Unlimited water soluble Boiling: +82.6 ° C with partial decomposition; Melting: -41.59 ° C
Chemical properties nitric acid HNO 3 is a strong monobasic acid Highly concentrated HNO 3 is usually brown in color due to the decomposition process occurring in the light 4 HNO 3 4NO 2 + 2 H 2 O + O 2 When heated, nitric acid decomposes by the same reaction. Nitric acid can be distilled (without decomposition) only under reduced pressure. Nitric acid in any concentration exhibits the properties of an acid-oxidizing agent.
The most important compounds A mixture of three volumes of hydrochloric acid and one volume of nitric acid is called "Tsar's vodka". Tsar's vodka dissolves most metals, including gold and platinum. Its strong oxidizing properties are due to the atomic chlorine and nitrosyl chloride formed: Nitrates are salts of nitric acid. Nitrates are obtained by the action of nitric acid HNO 3 on metals, oxides, hydroxides, and salts. Almost all nitrates are readily soluble in water. Nitrates are stable at ambient temperatures. They usually melt at relatively low temperatures (200-600 ° C), often with decomposition.
Being in nature In nature, it does not occur in a free state, but always only in the form of nitric acid salts. Thus, in the form of ammonium nitrate in the air and rainwater, especially after thunderstorms, then in the form of sodium nitrate in Chilean or Peruvian nitrate and potassium and calcium nitrate in the upper layers of arable land, on the walls of stables, in the lowlands of the Ganges and other rivers of India. * Selitra is a trivial name for minerals containing nitrates of alkali and alkaline earth metals.
Virtual experiment Attention! Nitric acid and its vapors are very harmful, so you should work with it very carefully.
Production of nitric acid A distinction is made between the production of weak (dilute) nitric acid and the production of concentrated nitric acid. The process for the production of diluted nitric acid consists of three stages: 1) conversion of ammonia in order to obtain nitrogen oxide 4NH 3 + 5О 2 → 4NO + 6Н 2 О 2) oxidation of nitrogen oxide to nitrogen dioxide 2NO + О 2 → 2NO 2 3) absorption of nitrogen oxides water 4NO 2 + О 2 + 2Н 2 О → 4HNO 3 The total reaction of the formation of nitric acid is expressed as NH 3 + 2О 2 → HNO 3 + Н 2 О
The use of nitric acid to obtain: nitrogen fertilizers; Medicines Dyes Explosives Plastic masses Artificial fibers "Fuming" nitric acid is used in rocket technology as an oxidizer of rocket fuel is extremely rare in photography - diluted - acidification of some tinting solutions; in easel graphics - for etching printed forms (etching boards, zinc printing plates and magnesium plates). in jewelry - the main method for determining gold in a gold alloy;
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annex to the lesson "Nitric acid: molecular composition, physical and chemical properties." "Nitric acid: molecular composition, physical and chemical properties." Appendix to the lesson "Nitric acid:
A lesson attachment for students to fill out in a learning portfolio ....
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HNO3 Composition. Structure. Properties. H O N O O - - oxidation state of nitrogen valence of nitrogen +5 IV chemical bond covalent polar Nitric acid is a colorless hygroscopic liquid, with a pungent odor, “fumes” in air, and is unlimitedly soluble in water. tboil. \u003d 83ºC .. When stored in the light, decomposes into nitric oxide (IV), oxygen and water, acquiring a yellowish color: 4HNO3 \u003d 4NO2 + O2 + 2H2O Nitric acid is poisonous.
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During the decomposition of nitric acid, oxygen is released, so the turpentine flares up.
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Nitric acid (HNO3) Classification by the presence of oxygen: basicity: solubility in water: volatility: degree of electrolytic dissociation: oxygen-containing monobasic soluble volatile strong nitric acid according to:
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Production of nitric acid in industry NH3NONO2HNO3 4NH3 + 5O2 \u003d 4NO + 6H2O 2NO + O2 \u003d 2NO2 4NO2 + 2H2O + O2 \u003d 4HNO3 1. Contact oxidation of ammonia to nitric oxide (II): 2. Oxidation of nitric oxide (II) to nitrogen oxide (IV) : 3. Adsorption (absorption) of nitrogen oxide (IV) by water with an excess of oxygen
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In the laboratory, nitric acid is produced by the action of concentrated sulfuric acid on nitrates with mild heating. Write the equation for the reaction of obtaining nitric acid. NaNO3 + H2SO4 \u003d NaHSO4 + HNO3
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Chemical properties of nitric acid 1. Typical properties of acids 2. Interaction of nitric acid with metals 3. Interaction of nitric acid with non-metals
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Chemical Properties of Nitric Acid Nitric acid exhibits all the typical properties of acids. List the properties of acids. Acids interact with basic and amphoteric oxides, bases, amphoteric hydroxides, and salts. Make the equations for the reactions of nitric acid: 1 3 2 with copper oxide (II), aluminum oxide; with sodium hydroxide, zinc hydroxide; with ammonium carbonate, sodium silicate. Consider reactions with t. Sp. TED. Give names to the obtained substances. Determine the type of reaction. 3
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2HNO3 + CuO \u003d Cu (NO3) 2 + H2O 1 2H + + 2NO3– + CuO \u003d Cu2 + + 2NO3– + H2O 2H + + CuO \u003d Cu2 + + H2O 6HNO3 + Al2O3 \u003d 2Al (NO3) 3 + 3H2O 6H + + 6NO3– + Al2O3 \u003d 2Al3 + + 6NO3– + 3H2O 6H + + Al2O3 \u003d 2Al3 + + 3H2O HNO3 + NaOH \u003d NaNO3 + H2O H + + NO3– + Na + + OH– \u003d Na + + NO3– + H2O H + + OH– \u003d H2O 2 2HNO3 + Zn (OH) 2 \u003d Zn (NO3) 2 + 2H2O 2H + + 2NO3– + Zn (OH) 2 \u003d Zn2 + + 2NO3– + 2H2O 2H + + Zn (OH) 2 \u003d Zn2 + + 2H2O
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3 2HNO3 + (NH4) 2CO3 \u003d 2NH4NO3 + CO2 + H2O 2H + + 2NO3– + 2NH4 + + CO22– \u003d 2NH4 + + 2NO3– + CO2 + H2O 2H + + CO22– \u003d CO2 + H2O 2HNO3 + Na2SiO3 \u003d H2Na + 2NO3 + 2N - + 2Na + + SiO32– \u003d ↓ H2SiO3 + 2Na + + 2NO3– 2H + + SiO32– \u003d ↓ H2SiO3 Active acids displace weak volatile or insoluble acids from salt solutions.
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Interaction of nitric acid with metals How do metals react with acid solutions? Metals, which stand in the line of activity before hydrogen, displace it from acids. Metals after hydrogen from acids do not displace it, i.e. do not interact with acids, do not dissolve in them. Features of the interaction of nitric acid with metals: 1. No metal ever releases hydrogen from nitric acid. Various nitrogen compounds are distinguished: N + 4O2, N + 2O, N2 + 1O, N20, N – 3H3 (NH4NO3) 2. Metals that come before and after hydrogen in the activity series react with nitric acid. 3. Nitric acid does not interact with Au, Pt 4. Concentrated nitric acid passivates metals: Al, Fe, Be, Cr, Ni, Pb and others (due to the formation of a dense oxide film). When heated and when nitric acid is diluted, these metals dissolve in it. experiment experiment experiment N – 3H4 + N20 N2 + 1O N + 2O N + 4O2 acid concentration metal activity
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Oxidizing properties of nitric acid
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Write the equation for the reaction of the interaction of concentrated nitric acid with mercury. Consider the reaction with t. Sp. OVR. 4HN + 5O3 + Hg0 \u003d Hg + 2 (NO3) 2 + 2N + 4O2 + 2H2O N + 5 + 1e → N + 4 1 2 Hg0– 2e → Hg + 2 2 1 HNO3 (due to N + 5) - oxidizing agent, recovery process; Hg0 - reducing agent, oxidation process.
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Add the reaction schemes: Consider the transformations in the light of ORR 1) HNO3 (conc.) + Cu → Cu (NO3) 2 +… + H2O 2) HNO3 (dil.) + Cu → Cu (NO3) 2 +… + H2O 1) HN + 5O3 (conc.) + Cu0 \u003d Cu + 2 (NO3) 2 + N + 4O2 + H2O 2 2 N + 5 + 1e → N + 41 2 Cu0– 2e → Cu + 2 2 1 2) HN + 5O3 (conc. .) + Cu0 \u003d Cu + 2 (NO3) 2 + N + 2O + H2O 3 3 4 2 8 N + 5 + 3e → N + 23 2 Cu0–2e → Cu + 2 2 3 reduction oxidation reducing agent oxidizing agent 4 reduction oxidation oxidizing agent reducing agent
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Interaction of nitric acid with non-metals Oxidizes non-metals to the corresponding acids. Concentrated (more than 60%) nitric acid is reduced to NO2, and if the acid concentration is (15 - 20%), then to NO. HNO3 + С → СO2 + H2O + NO2 N + 5 + 1e → N + 4 1 4 С0 –4e → С + 44 1 4 4 2 HNO3 + P → H3PO4 + NO2 + H2O N + 5 + 1e → N + 4 1 5 P0 - 5e → P + 5 5 1 5 2 5 HNO3 + P + H2O → H3PO4 + NO N + 5 + 3e → N + 2 3 5 P0 - 5e → P + 5 5 3 3 5 3 5 Nitric acid as strong oxidizing agent Place the coefficients in the diagrams using the electronic balance method. HNO3 (due to N + 5) –oxidant, pr. Reduction C– reductant, oxidation process HNO3 (due to N + 5) –oxidant, pr. Reduction P– reductant, oxidation process HNO3 (due to N + 5) –oxidant, ex. reduction P - reducing agent, oxidation process experience experience
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Interaction of nitric acid with coal
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Reaction between nitric acid and white phosphorus
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Application of nitric acid 1 5 4 6 2 3 Production of nitrogen and complex fertilizers. Production of explosives Production of dyes Production of drugs Production of films, nitro varnishes, nitroenamels Production of artificial fibers 7 As a component of a nitrating mixture for trawling metals in metallurgy
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Nitric acid salts What are the names of nitric acid salts? nitrates Nitrates K, Na, NH4 + are called nitrates. Formulate the listed salts. KNO3 NaNO3 NH4NO3 Nitrates are white crystalline substances. Strong electrolytes, in solutions, completely dissociate into ions. Enter into exchange reactions. How can you determine the nitrate ion in solution? Sulfuric acid and copper are added to the salt (containing the nitrate ion). The mixture is slightly warmed up. Evolution of brown gas (NO2) indicates the presence of a nitrate ion.
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Potassium nitrate (potassium nitrate) Colorless crystals Significantly less hygroscopic than sodium nitrate, therefore it is widely used in pyrotechnics as an oxidizing agent. When heated above 334.5 ° C, it melts, above this temperature it decomposes with the release of oxygen. It is used as a fertilizer; in the glass, metal-working industry; to obtain explosives, rocket fuel and pyrotechnic mixtures. Sodium nitrate
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White crystalline substance. The melting point is 169.6 ° C, when heated above this temperature, gradual decomposition of the substance begins, and at a temperature of 210 ° C, complete decomposition occurs. Ammonium nitrate
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When heated, nitrates decompose the more completely, the more to the right in the electrochemical series of voltages is the metal that forms the salt. Li K Ba Ca Na MgAl Mn Zn Cr Fe Co Sn PbCu Ag Hg Au nitrite + O2 metal oxide + NO2 + O2 Ме + NO2 + O2 Write the equations for the decomposition of sodium nitrate, lead nitrate, silver nitrate. 2NaNO3 \u003d 2NaNO2 + O2 2Pb (NO3) 2 \u003d 2PbO + 4NO2 + O2 2AgNO3 \u003d 2Ag + 2NO2 + O2
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1. The oxidation state of nitrogen in nitric acid is: A) +5; B) +4; IN 3. A 2. When interacting with what substances, nitric acid exhibits special properties that distinguish it from other acids: A) basic oxides; B) metals; C) grounds. B 3. In the redox reaction, nitric acid can participate as: A) an oxidizing agent; B) a reducing agent; B) an oxidizing agent and a reducing agent. A 4. Which of these nitrogen compounds is called Chilean nitrate: A) potassium nitrate; B) calcium nitrate; C) sodium nitrate; В 5. Write down the equation of interaction of copper with concentrated nitric acid. The coefficient in front of the acid formula is: A) 2; B) 4; C) 1. B 6. Which of the listed substances does not react with dilute nitric acid: A) copper; B) sodium hydroxide; C) sodium bromide. C 7. Nitric acid is obtained in three stages by oxidizing a nitrogen atom according to the following scheme: A) N – 3 → N + 2 → N + 4 → N + 5 B) N – 3 → N0 → N + 4 → N + 5C) N0 → N + 2 → N + 4 → N + 5 A
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"Nitric acid salt" - What happens when sodium nitrate decomposes? Physical properties of nitrates. Indicate oxidizing agent, reducing agent. Chemical properties of nitrates. Know and be able to. The nitric acid solution reacts with each of the substances. What conclusions did the young chemist come to? All nitrates are thermally unstable. An entertaining story.
"Theories of acids and bases" - For example, which acid is stronger than acetic acid (CH3COOH or chloroacetic ClCH2COOH? 2. Addition reactions. The strength of the base R3N in water can be estimated by considering the equilibrium: Gilbert Newton Lewis. The measure of acidity is the equilibrium constant, called the acidity constant (Ka) Svante-August Arrhenius.
"Acetic acid" - What are acids? Not all fruits and vegetables contain acids. Acids. Pure formic acid was first obtained in 1749. Andreas Sigismund Marggraf. A journey into the world of acids. How do you detect acids? Formic acid solution. The history of the discovery of acids. The acids have a similar composition. What substances are acids?
“Acid rain” - New ozone holes are expected to appear in the Baltic region. Aluminum can cause disease. It can be assumed what happens to wild species of animals when forests die. We, and almost all living things, need fresh water. Along with the loss of lakes, degradation of forests becomes apparent.
"Carboxylic acids" - Repeat the determination of carboxylic acids. Obtaining carboxylic acids. The structure of the carboxyl group. Carboxylic acids. What are carboxylic acids? Nomenclature of esters. All carboxylic acids have a functional group. Carboxylic acid molecules form dimers. Chemical properties of carboxylic acids.
"Nucleic acids" - 1892 - chemist Liljenfeld isolated thymonucleic acid from the thymus gland in 1953. Nitrogen base. Laboratory workshop. The structure of nucleotides (differences). 1868 - the German chemist F. Mischer discovered nucleic acids. The biological role of nucleic acids. Comparative characteristics... Length of DNA molecules (American biologist G. Taylor).
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Nitric acid. Nitric acid salts. Getting and using nitric acid Lesson 43
Nitric acid is a colorless liquid fuming in air with a pungent odor. Formula: HNO 3 Technical concentrated HNO 3 Structural formula: Nitrogen valence: IV Oxidation state: +5
Obtaining nitric acid a) In industry: 4NH 3 + 5O 2 \u003d 4NO + 6H 2 O Pt- Rh t 0 C 2NO + O 2 \u003d 2NO 2 4NO 2 + 2H 2 O + O 2 ⇄ 4HNO 3 b) In laboratory: NaNO 3 + H 2 SO 4 (conc.) \u003d HNO 3 + NaHSO 4 t 0 C
Industrial scheme for producing nitric acid
Chemical properties of nitric acid 1. Strong monobasic acid HNO 3 → H + + NO 3 - 2. Strong oxidizing agent CuO + 2HNO 3 \u003d Cu (NO 3) 2 + H 2 O KOH + HNO 3 \u003d KNO 3 + H 2 O 4 HNO 3 (dil.) + 3 Ag \u003d 3 AgNO 3 + NO + 2 H 2 O 4 HNO 3 (conc.) + C \u003d CO 2 + 4NO 2 + 2H 2 O 6HNO 3 (conc.) + S \u003d H 2 SO 4 + 6NO 2 + 2H 2 O 5HNO 3 (conc.) + P \u003d H 3 PO 4 + 5NO 2 + H 2 O t 0 C t 0 C t 0 C
H 2 S + 8HNO 3 \u003d H 2 SO 4 + 8NO 2 + 4H 2 O FeS + 12HNO 3 \u003d Fe (NO 3) 3 + H 2 SO 4 + 9NO 2 + 5H 2 O 6HI + 2HNO 3 \u003d 3I 2 + 2NO + 4H 2 O "Tsarskaya vodka" Conc. HNO 3 and HCl (1: 3) by volume Au + HNO 3 + 4HCl \u003d H + NO + 2H 2 O 3. Displaces weak acids from salts 2HNO 3 + Na 2 CO 3 \u003d CO 2 + 2NaNO 3 + H 2 O 2HNO 3 + Na 2 SiO 3 \u003d H 2 SiO 3 + 2NaNO 3 4. Decomposition on heating 4HNO 3 ⇄ 4NO 2 + 2H 2 O + O 2 t 0 C
4. Interaction of metals with HNO 3 H 2 is practically never released !!! When heated, all metals interact, except Pt, Au. HNO 3 (conc.) Passivates Al, Fe, Be, Cr, Mn (t room). N is reduced (product depends on acid concentration and metal activity). Hg + 4HNO 3 (conc.) \u003d Hg (NO 3) 2 + 2NO 2 + 2H 2 O 3Cu + 8HNO 3 (dil.) \u003d 3Cu (NO 3) 2 + 2NO + 4H 2 O 5Zn + 12HNO 3 (dil. ) \u003d 5Zn (NO 3) 2 + N 2 + 6H 2 O 8Al + 30HNO 3 (very dil.) \u003d 8Al (NO 3) 3 + 3NH 4 NO 3 + 9H 2 O 8Na + 10HNO 3 (conc.) \u003d 8NaNO 3 + N 2 O + 5H 2 O
Nitrates are salts of nitric acid. 1. Decompose on heating M (NO 3) y MNO 2 + O 2 t 0 CM x O y + NO 2 + O 2 M + NO 2 + O 2 Na, K, partially Li and AHZM, Li, AHZM M after C u NH 4 NO 3 \u003d N 2 O + 2H 2 O t 0 C
2. Strong oxidants (solid, at t) NaNO 3 + Pb \u003d NaNO 2 + PbO 2 KNO 3 + 3C + S \u003d K 2 S + CO 2 + N 2 Fe 2 O 3 + 6KNO 3 + 4KOH \u003d 2K 2 FeO 4 + 6KNO 2 + 2H 2 O t 0 C t 0 C t 0 C 3. Weak oxidizing agents in solutions 8 Al + 3KNO 3 + 5KOH + 18H 2 O \u003d 8K + 3NH 3 potassium ferrate
An increase in the oxidation state of metals during the decomposition of nitrates 4Fe (NO 3) 2 2Fe 2 O 3 + 8NO 2 + O 2 4 Fe 4 Fe 2O O 2 8 N 8 N +2 +3 +5 +4 -2 0 + 8 e - - 4 e - - 4 e - 8 8 8 1 1 t 0 C Sn (NO 3) 2 SnO 2 + 2NO 2 t 0 C
Tasks 1. Arrange the coefficients using the electronic balance method HNO 3 (conc.) + Sn → H 2 SnO 3 + NO 2 + H 2 O HNO 3 (conc.) + K → KNO 3 + N 2 O + H 2 O HNO 3 ( split) + PH 3 → H 3 PO 4 + NO + H 2 O 2. Solve the problem Calculate mass fraction nitric acid, if during the interaction of 350 g of its solution with copper, 9 liters (n.u.) of nitric oxide (II) were released.
Homework §31, presentation task
On the subject: methodological developments, presentations and notes
Chemistry lesson in grade 10 Obtaining and using carboxylic acids
Lesson in grade 10 on the topic "Obtaining and using carboxylic acids". The material is presented accompanied by a presentation. Students prepared messages in the form of presentations on the most common ...
The lesson has a pronounced practical focus. Students conduct a chemical experiment, study the properties of nitrates and reveal their practical importance for races and humans ...