Presentation on the topic "nitric acid and its salts". Salts of nitric acid Action on the body

Salts of nitric acid. What are the salts of nitric acid called? Nitrates. Nitrates K, Na, NH4+ are called saltpeters. KNO3. NaNO3. NH4NO3. Nitrates are white crystalline substances. Strong electrolytes, in solutions completely dissociate into ions. They 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 heated. Emission of brown gas (NO2) indicates the presence of the nitrate ion. Write the formulas for the listed salts.

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Names of acids

“Carbonic acid and its salts” - Correct answers: Option 1 - 1, 2, 3, 4, 8, 10 Option 2 - 3, 5, 6, 7, 9, 10. What carbon oxides are mentioned in the following statements? Enter in the diagram. What phenomenon are we talking about? Very toxic Does not burn and does not support combustion Used in metallurgy for iron smelting Formed during complete combustion of fuel Magnesium burns in it Typical acidic oxide.

"Fatty acids" - Lipid extracts. n-6. 2. Arachidonic acid and other polyene fatty acids as signaling molecules. Polyunsaturated fatty acids as signal molecules. Since 1978 S.D. Varfolomeev, A.T. Mevkh, G.F. Sud'ina, P.V. Vrzheshch et al. 1. PGE2. A. TxA2 PGI2 PGE2 PGF2a PGD2. Platelets: [AA]o = 5 mM 1% - 50 mM (w) Leukocytes: 0.1-1 mM (w) Islets of Langerhans: 15 mM (w) [AA]excl = 1-10 mM DHA~50% cells brain.

"Physical and chemical properties of acids" - 1. According to the oxygen content. 2. By the number of hydrogen atoms. You kept a test tube over your trousers With acid? Нn+1 (KO)-n. Hydrochloric acid. Sulfuric acid. Single-basic hcl HNO3. Acids. Phosphoric acid. HCI H2SO4 H3PO4 HNO3 H2S HNO2 H2SO3 H2CO3 H2sio4. Nitrous acid. Carbonic acid. The harm of acids.

"Sulfuric acid lesson" - How does dilute sulfuric acid interact with metals? Negative impact on the environment. "What are the special properties of concentrated sulfuric acid? Lesson motto: What indicators can detect acids? Acid rain. What general properties acids are characteristic of sulfuric acid? The purpose of the lesson:

"Production of sulfuric acid" - Cleaning from coarse dust. Production technology. III stage. Cleaning of fine dust Grid positively charged Wire negatively. 2 SO2(g) + O2(g) ? 2 SO3(g) + Q Compounds Exothermic Homogeneous Catalytic Reversible Redox. II stage. In the contact apparatus, shelves with V2O5 catalyst.

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Salts of nitric acid, application The motto of the lesson "Au, Na, Ar, Ne, It, Eu - Os, Ra, U, Db, In, Er, As Ni, Es C, Eu La b" L. N. Tolstoy

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know and be able to name salts of nitric acid, determine what oxidizing or reducing properties are characteristic of them; determine: the degree of oxidation of chemical elements in the formulas of salts; types of chemical reactions in which they can participate; characterize: general chemical properties of nitric acid salts;

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tic-tac-toe game A solution of nitric acid reacts with each of the substances. MgO Al P2O5 KCl CO2 CaCO3 Al2O3 K2SiO3 Zn

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What class of inorganic substances do these substances belong to? 1. Name the salts - the products of these reactions 2. Make in your notebook the molecular equations for the reactions of obtaining nitrates. MgO Al P2O5 KCl CO2 CaCO3 Al2O3 K2SiO3 Zn

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Complete the reaction equations and explain which classes of compounds can give nitrates when interacting. BaO + HNO3 → BaO + N2O5 → Ba(NO3)2 + Na2SO4 →

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Pairs of substances are given, make possible reaction equations a) sodium hydroxide and nitric acid, b) potassium hydroxide and nitric oxide (V), c) calcium oxide and nitric acid, d) ammonia and nitric acid, e) barium sulfate and calcium nitrate, f) sodium chloride and barium nitrate Which of the reactions are impossible and why?

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List the salts obtained as a result of possible reactions. Potassium, sodium, calcium and ammonium nitrates are called saltpeters KNO3 - potassium nitrate (Indian saltpeter), NaNO3 - sodium nitrate (Chilean saltpeter), Ca (NO3) 2 - calcium nitrate (Norwegian saltpeter) NH4NO3 - ammonium nitrate (ammonium or ammonium nitrate, there are no deposits of it in nature). The German industry is considered the first in the world to obtain the salt NH4NO3 from nitrogen N2 in the air and hydrogen in water, suitable for plant nutrition.

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Nitrates are solid crystalline substances, refractory, determine from the solubility table which electrolytes they belong to - strong or weak?

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Physical properties of nitrates What substances are called salts? It is necessary to build a logical chain: the type of chemical bond - the type of crystal lattice - the forces of interaction between particles at the lattice nodes - the physical properties of substances.

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Chemical properties of nitrates Interaction of nitrates with metals, acids, alkalis, salts Cu(NO3)2 + Zn … , AgNO3 + HCl … , Cu(NO3)2 + NaOH … , AgNO3 + BaCl2 … .

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An interesting story An inquisitive chemist studied the types of chemical reactions and noticed that insoluble carbonates (CaCO3), sulfites (CaSO3), silicates (CaSiO3), some sulfates (FeSO4) decompose when heated. He set himself the task of determining whether nitrates would decompose. For the experiment, he took a laboratory tripod, a test tube with sodium nitrate, and an alcohol lamp. Knowing that gas is formed during the decomposition of many salts, an inquisitive chemist prepared a torch, litmus test and lime water (Ca (OH) 2). When the salt heated up and melted, he lowered a smoldering splinter into the test tube, it suddenly flared up. What conclusions did the young chemist come to?

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n and one vessel does not contain more than its volume, except for the vessel of knowledge; it is constantly expanding. Arabic proverb

This substance is called "Chinese snow" in Europe; in 808, the Chinese alchemist Qin invented black powder based on it. Determine the molecular formula of a substance if it contains 38.61% potassium, 13.86% nitrogen and oxygen.

Salts of nitric acid

Salt nomenclature Nitrates: Ba (NO₃)₂ , AgNO ₃ , Zn(NO₃)₂ , NaNO ₃ Saltpeters: NaNO ₃ , KNO₃ , Ca(NO₃)₂ , NH₄NO₃

The structure and physical properties of nitrates Type of chemical bond - ionic Type of crystal lattice - ionic Aggregate state - solid crystalline substances Solubility in water - most soluble

Chemical properties common with other salts Electrolytes Reactions with acids Ba (NO₃)₂ + H₂SO₄ with alkalis Fe(NO₃)₃ + NaOH with salts AgNO ₃ + BaCl ₂ with metals Cu(NO₃)₂ + Fe

Special properties of nitrates Thermal decomposition Without wasting time, Let's figure out how nitrates decompose in the stove. What happens? The alkali metal is so active, He says in a commanding tone: “Being a nitrate is so disgusting. I’d better turn into nitrite!” And metals from the company from magnesium to copper, Zinc, iron and their other neighbors Carefully and calmly, without offense, Extract their oxide from nitrate. But what about silver and mercury? Metals that consider themselves noble, Desire to become very, very free.

Special properties of nitrates Qualitative reaction to NO₃⁻ NaNO ₃ + Cu + H₂SO₄

Nitrates: pros and cons

Plant name Recommendations for use Patisson It is better to cut off the upper part adjacent to the stalk Cucumber Peel the cucumber from the skin and cut off the tail Cabbage Remove the upper covering leaves and discard the stalk Zucchini Cut off the skin Beetroot Cut off the upper and lower parts of the root Potato Peeled potatoes pour 1% for a day salt or ascorbic acid Carrots Cut off the top and bottom of the root Table. Accumulation of nitrates in various parts of the productive organs of plants.

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Lesson on the topic "Nitric acid" Grade 9 Chemistry teacher: Matyushkina T.S.

In the lesson we will: - continue to study nitrogen compounds - consider in detail the properties of HNO 3 - we will improve the skills of writing reaction equations - learn about the areas of practical application of HNO 3 and its salts

Chemical warm-up: 1. Ammonia formula: a) NH 2 b) NH 4 c) NH 3 d) N 2 2. Ammonia: a) lighter than air, b) heavier than air, c) neither lighter nor heavier 3. Ammonia is: a) an oxidizing agent, b) a reducing agent, c) both. 4. Ammonium ion a) NH 2 + b) NH 4 + c) NH 3 - d) NH 3 nitrogen in ammonia: a) 0, b) -3, 4) +3, 5) 8

Chemical warm-up Determine the oxidation state of nitrogen in each oxide

Nitric acid HNO 3 is one of the strongest acids Physical properties: - colorless liquid - “smokes” in air, t bp = 84 o C, t pl = -42 o C - turns yellow in the light due to the release of NO 2: 4HNO 3 \u003d 2H 2 O + 4NO 2 + O 2

Obtaining HNO 3

Chemical properties Typical properties of acids

Chemical properties Reacts especially with metals:

Chemical properties: Interaction with non-metals

For the curious:

The use of HNO 3 salts - in agriculture- for dyeing fabrics - in medicine - in pyrotechnics

Check yourself: The oxidation state of nitrogen in HNO 3 a) -3 b) 0 c) + 5 d) + 4 When stored in the light HNO 3 a) turns red b) turns yellow c) remains colorless Nitric acid is: a) an oxidizing agent, b) reducing agent, c) both. Does HNO 3 share properties with other acids? a) yes b) no c) depends on the weather Aqua regia is a) concentrated alcohol b) 3 volumes of HCl and 1 volume of HNO 3 c) concentrated nitric acid

Finish the sentences: - today at the lesson I learned ... - I practiced ... - I saw ...

Homework: Learn theory: pp. 118-121 Exercises 2, 3,4 p.121

On the topic: methodological developments, presentations and notes

Klochkova Violetta Mikhailovna, teacher of chemistry, MBOU Secondary School No. 2 named after I. I. Tarasenko Art. Settlements of the Krasnodar Territory ....

Summary of the combined lesson on the topic "Nitric acid". This lesson discusses the physical, general and specific properties, laboratory and industrial methods for obtaining nitric acid...

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This substance was described by the Arab chemist in the 8th century Jabir ibn Hayyan (Geber) in his work “The Coachman of Wisdom”, and since the 15th century this substance has been mined for industrial purposes - Thanks to this substance, the Russian scientist V.F. Petrushevsky in 1866 for the first time received dynamite. This substance is a component of rocket fuel, it was used for the engine of the world's first Soviet jet aircraft BI - 1 This substance is the progenitor of most explosives (for example, TNT, or tol) - This substance, mixed with hydrochloric acid, dissolves platinum and gold, recognized " king of metals. The mixture itself, consisting of 1 volume of this substance and 3 volumes of hydrochloric acid, is called "royal vodka".

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Her Majesty Nitric acid Yakonyuk Vera Sergeevna chemistry teacher MOU Znamenskaya secondary school Chemistry lesson Grade 9

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Alchemists first obtained nitric acid by heating a mixture of saltpeter and iron sulfate: 4KNO3 + 2(FeSO4 7H2O) (t °) → Fe2O3 + 2K2SO4 + 2HNO3 + NO2 + 13H2O Pure nitric acid was first obtained by Johann Rudolf Glauber, acting on saltpeter with concentrated sulfuric acid : KNO3 + H2SO4(conc.) (t°) → KHSO4 + HNO3 "fuming nitric acid", containing practically no water

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It has been experimentally proven that the double bond is evenly distributed between two oxygen atoms. The oxidation state of nitrogen in nitric acid is +5, and the valence (note) is four, because there are only four common electron pairs. The bond is covalent polar. Crystal lattice - molecular Structure

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Obtaining HNO 3 Laboratory method of obtaining: NaNO3 + H2SO4 t NaHSO4 + HNO3 this produces fuming nitric acid

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Industrial method 1. Oxidation of ammonia to NO in the presence of a platinum-rhodium catalyst: 4NH3 + 5O2 = 4NO + 6H2O 3. Absorption of NO2 by water in the presence of oxygen: 4NO2 + 2H2O + O2= 4HNO3 Mass fraction of HNO3 is about 60% 2. Oxidation of NO in NO2 in the cold under pressure (10 atm): 2NO + O2 = 2NO2

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Physical properties Physical properties colorless liquid tmelt=-41.60C tboil=82.60C infinitely miscible with water volatile - in air "smokes" Conc. nitric acid is usually colored yellow,

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Research (tasks in groups): (Repetition of PTB!). Group 1: carry out the reaction of a solution of nitric acid and copper (II) oxide, write down the reaction equation, determine its type Group 2: obtain an insoluble base Cu (OH) 2; carry out the reaction of a solution of nitric acid and copper (II) hydroxide; write down the reaction equation, determine its type Group 3: carry out the reaction of solutions of nitric acid and sodium carbonate, write down the reaction equation, determine its type

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Group №1 CuO + 2 HNO3 = Cu(NO3)2 + H2O - ion exchange reaction, irreversible CuO + 2H+ + 2 NO3- = Cu2+ + 2 NO3- + H2O CuO + 2H+ = Cu2+ + H2O Group №2 CuCl2 + 2 NaOH = Cu(OH)2↓ + 2 NaCl (obtaining an insoluble base) Cu(OH)2 ↓+ 2 HNO3 = Cu(NO3)2 + 2 H2O - ion exchange reaction, irreversible Cu(OH)2 ↓ + 2H+ + 2 NO3 - = Cu2+ + 2 NO3- + 2 H2O Cu(OH)2↓ + 2H+ = Cu2+ + 2 H2O Sign of the reaction - dissolution of the blue precipitate Cu(OH)2 Group No. 3 2 HNO3 + Na2CO3 = 2 NaNO3 + H2O + CO2 - reaction ion exchange, irreversible 2 H+ + 2NO3- + 2 Na+ + CO32- = 2 Na+ + NO3- + H2O + CO2 2 H+ + CO32- = H2O + CO2

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Common with other acids: 1. Strong electrolyte, well dissociated into ions HNO3 -> H+ +NO3- Changes the color of the indicator. 2. Reacts with basic oxides СuO+2 HNO3 -> Cu(NO3)2 +H2O 3. Reacts with bases HNO3 + KOH -> KNO3 + H2O 4. Reacts with salts of more volatile acids Na2CO3 + 2HNO3 -> 2NaNO3 + H2CO3 dry / \H2OCO2

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Specific: When heated and exposed to light, 4HNO3 = 2H2O + 4NO2 + O2 decomposes Reacts with non-metals %) \u003d H2SO4 + 2NO P + 5HNO3 (60%) \u003d H3PO4 + 5NO2 + H2O P + 5HNO3 (30%) + 2H2O \u003d 3H3PO4 + 5NO NOnotMe + HNO3NO2. Nitric acid oxidizes non-metals

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The interaction of nitric acid with metals has been studied quite well, tk. conc. HNO3 is used as a propellant oxidizer. The point is that the reaction products depend on two factors: 1) the concentration of nitric acid; 2) the activity of the metal The combination of these two parameters determines the composition of the reaction products. What can be? a) the metal may or may not react ( do not react at all, passivate); b) the composition of gases is mixed (as a rule, not one gaseous product is released, but a mixture of gases, sometimes some gas prevails over others); c) hydrogen is usually not released in these processes (there is an exception when In practice, it is proved that Mn + dilute HNO3 actually releases hydrogen gas) The main rule: The more active the metal and the more dilute the nitric acid, the deeper the reduction of nitric acid goes (the extreme option is reduction to ammonia NH3, more precisely to NH4NO3; here the process of reduction N ( +5) + 8e ----> N(-3)). Intermediate reduction options to NO2, NO, N2O, N2 are possible General process scheme: HNO3 + Me ---> nitric acid salt (nitrate) + nitric acid reduction product + H2O

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Interaction with metals: When interacting with metals, nitrate, water and the third product are formed according to the scheme: HNO3 (r.) + Me (to H2) → nitrate + H2O + NH3 (NH4NO3) HNO3 (r.) + Me (after H2) → nitrate+H2O+NO HNO3(c.)+Me(before H2)→nitrate+H2O+N2O(N2) HNO3(c.)+Me(after H2)→nitrate+H2O+NO2 Concentrated HNO3 on Al, Cr, Fe, Au, Pt is not valid.

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P.S concentrated HNO3 >60% dilute HNO3 = 30-60% very dilute HNO3

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Application of Nitric Acid:

Production of nitrogen and combined fertilizers, -explosives (trinitrotoluene, etc.), -organic dyes. as an oxidizer for rocket fuel. - In metallurgy, nitric acid is used for pickling and dissolving metals, as well as for separating gold and silver.

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Action on the body

Inhalation of vapors of nitric acid leads to poisoning, contact with nitric acid (especially concentrated) on the skin causes burns. The maximum permissible content of nitric acid in the air of industrial premises is 50 mg / m3 in terms of N2O5 Concentrated nitric acid in contact with organic substances causes fires and explosions

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Check yourself:

The oxidation state of nitrogen in HNO3 a) -3 b) 0 c) + 5 g) + 4 When stored in the light, HNO3 a) turns red b) turns yellow c) remains colorless When interacting with metals, nitric acid is: a) an oxidizing agent, b) a reducing agent , c) both. Nitric acid in solution does not react with a substance whose formula is: a) CO2; b) NaOH; c) Al(OH)3; d) NH3. Aqua regia is a) concentrated alcohol b) 3 volumes of HCl and 1 volume of HNO3 c) concentrated nitric acid

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key

1 - c 2 - b 3 - a 4 - a 5 - b

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conclusion:

1. Nitric acid is characterized by the general properties of acids: reaction to an indicator, interaction with metal oxides, hydroxides, salts of weaker acids due to the presence of an H + ion in the molecules; 2. The strong oxidizing properties of nitric acid are due to the structure of its molecule; When it interacts with metals, hydrogen is never formed, but nitrates, nitrogen oxides or its other compounds (nitrogen, ammonium nitrate) and water are formed, depending on the concentration of the acid and the activity of the metal; 3. The strong oxidizing ability of HNO3 is widely used to produce various important products of the national economy (fertilizers, medicines, plastics, etc.)

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Homework:

§26 exercises 4.5 Creative task - presentation of the history of the discovery of nitric acid. The use of nitric acid

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Thank you for the lesson

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literature

O.S. Gabrielyan, I.G. Ostroumov Handbook of a teacher of chemistry Grade 9. Bustard 2003 Lidin R.A., Molochko V.A., Andreeva L.L. Chemical properties of inorganic substances Chemistry 2000 http://ru.wikipedia.org/wiki/HNO3http://centralnyj.fis.ru/Petrochemicalshttp://dic.academic.ru/dic.nsf/bse/61981/%D0%90% D0%B7%D0%BE%D1

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