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

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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, based on it, invented black powder. Determine the molecular formula of a substance if it contains 38.61% potassium, 13.86% nitrogen and oxygen.

Nitric acid salts

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

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 are 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 oven. So what happens? The alkali metal is so active, He says in a commanding tone: "Being nitrate is so disgusting. Better if I turn into nitrite!" And metals from the company from magnesium to copper, Zinc, iron and their other neighbors Carefully and calmly, no offense, They extract their oxide from nitrate. But what about silver and mercury? Metals that consider themselves noble, Want to become completely, completely free.

Special properties of nitrates Qualitative reaction for 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 cabbage squash Cut off the skin Beets Cut off the upper and lower parts of the root Potatoes Peeled potatoes for 1% per day table salt or ascorbic acid Carrots Cut off the top and bottom of the root vegetable Table. Accumulation of nitrates in various parts of the productive organs of plants.

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Kirillova

Margarita Alekseevna

chemistry teacher of the Lyceum No. 369

Krasnoselsky district

The nitrogen atom has three unpaired p-electrons on the outer layer, due to which it forms three σ-bonds with oxygen atoms. Due to the lone electron pair, a fourth covalent bond is formed. Electronic cloud

delocalized between

two oxygen atoms.

Valence - IV

Oxidation state -5

Colorless liquid, fuming

on air.

Acrid odor.

Concentrated yellow color

acid (decomposition to form

NO2). 4HNO3 = 4NO2 + 2H2O + O2

Density 1.52 g / cm3.

The boiling point is 860C.

Solidification temperature - -41.60C.

Hygroscopic.

Mixes with water in any

ratios.

Diluted nitric acid exhibits properties common to all acids:

Dissociation in aqueous solution:

HNO3 → H ++ NO3-

Reaction with bases:

NaOH + HNO3 = NaNO3 + H2O

Cu (OH) 2 + 2HNO3 = Cu (NO3) 2 + 2H2O

Reaction with basic oxides:

CaO + 2HNO3 = Ca (NO3) 2 + H2O

Reaction with salts:

Na2CO3 + 2HNO3 = 2NaNO3 + H2O + CO2

Oxidation of metals:

Recovery products

depend on activity

metal and dilution

nitric acid.

HNO3 (conc) + v-l

II. Nitric acid is a strong oxidizing agent

Al, Fe, Co, Ni, Cr do not interact without heating

HNO3 (conc) + v-l

K, Ca, Na, Mg, Zn ...

4HNO3 (conc) + Hg = Hg (NO3) 2 + 2NO2 + 2H2O

4Zn + 10HNO3 (diluted) = 4Zn (NO3) 2 + NH4NO3 + 3H2O

3Cu + 8HNO3 (decomp) = 3Cu (NO3) 2 + 2NO + 4H2O

Cu + 4HNO3 (conc) = Cu (NO3) 2 + 2NO2 + 2H2O

Zn + 4HNO3 (conc) = Zn (NO3) 2 + 2NO2 + 2H2O

Al + HNO3 (conc) =

Fe + HNO3 (conc) =

P + 5HNO3 (conc) = H3PO4 + 5NO2 + H2O

Oxidation of non-metals and organic

C + 4HNO3 (conc) = 4NO2 + CO2 + 2H2O

Organic matter is oxidized

and ignite in nitric acid.

In industry - by oxidation

4NH3 + 5O2 = 4NO + 6H2O

4NO2 + O2 + 2H2O = 4HNO3

In the laboratory - interaction

potassium or sodium nitrate with

concentrated sulfuric acid

when heated:

KNO3 + H2SO4 = HNO3 + KHSO4

Obtained by the interaction of nitric acid with metals, metal oxides, bases,
ammonia and some salts.

Physical properties... These are solid crystalline substances, readily soluble in water.

Chemical properties. Strong electrolytes,

exhibit all the properties of salts.

NaNO3 Na + + NO3-

Cu (NO3) 2 + 2KOH = Cu (OH) 2 ↓ + 2KNO3

AgNO3 + NaCl = AgCl ↓ + NaNO3

Pb (NO3) 2 + Zn = Pb + Zn (NO3) 2

Ba (NO3) 2 + H2SO4 = BaSO4 ↓ + 2HNO3

MexOy + NO2 + O2

2KNO3 = 2KNO2 + O2

2Cu (NO3) 2 = 2CuO + 4NO2 + O2

2AgNO3 = 2Ag + 2NO2 + O2

Decomposition of ammonium nitrate:

NH4NO3 = N2O + 2H2O

NaNO3 + H2SO4 = NaHSO4 + HNO3

4HNO3 + Cu = Cu (NO3) 2 + 2NO2 + 2H2O

Brown gas

Solid nitrates. A pinch of salt

burners are thrown into the fire.

A bright flash occurs.

dyes

medications

fertilizers

plastic

pyrotechnics

explosive

substances

HNO3 and nitrates

On the subject: methodological developments, presentations and notes

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 ...

Nitric acid salts. What are the names of nitric acid salts? Nitrates. Nitrates K, Na, NH4 + are called nitrates. 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. The evolution of brown gas (NO2) indicates the presence of a nitrate ion. Make formulas for the listed salts.

Slide 21 from the presentation "Nitric acid" to chemistry lessons on the topic "Names of acids"

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Acid names

"Carbonic acid and its salts" - Correct answers: 1 option - 1, 2, 3, 4, 8, 10 2 option - 3, 5, 6, 7, 9, 10. What carbon oxides are mentioned in the following statements? Enter into the scheme. What phenomenon are we talking about? Very toxic Does not burn and does not support combustion Used in metallurgy when smelting pig iron Formed when the fuel is completely burned 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 signaling molecules. Since 1978 S.D. Varfolomeev, A.T. Mevkh, G.F. Sudyina, P.V. Vrzhesh, etc. 1. PGE2. A. TxA2 PGI2 PGE2 PGF2a PGD2. Platelets: [AA] o = 5 mM 1% - 50 mM (s) Leukocytes: 0.1-1 mM (s) Islets of Langerhans: 15 mM (s) [AA] extra = 1-10 mM DHA ~ 50% cells brain.

"Physical and chemical properties of acids" - 1. By oxygen content. 2. By the number of hydrogen atoms. Did you hold a test tube with acid over your trousers? Hn + 1 (KO) -n. Hydrochloric acid. Hydrogen sulfide acid. Single-basic hcl HNO3. Acids. Phosphoric acid. HCI H2SO4 H3PO4 HNO3 H2S НNO2 H 2SO3 H2CO3 Н2sio4. 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 are the general properties of acids characteristic of sulfuric acid? The purpose of the lesson:

"Sulfuric acid production" - Coarse dust removal. Production technology. Stage III. Fine dust removal Net positively charged Wire negatively. 2 SO2 (g) + O2 (g)? 2 SO3 (g) + Q Compounds Exothermic Homogeneous Catalytic Reversible Redox. Stage II. In the contact device, there are shelves with a V2O5 catalyst.

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Lesson on the topic "Nitric acid" Grade 9 Chemistry teacher: Matyushkina TS

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 - we will learn about the areas of practical application of HNO 3 and its salts

Chemical warm-up: 1. Formula of ammonia: a) NH 2 b) NH 4 c) NH 3 d) N 2 2. Ammonia: a) lighter than air, b) heavier than air, c) not lighter and not 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 5. An electron donor in the formation of an ammonium ion is a) nitrogen atom, b) hydrogen ion, c) ammonium ion 6. Degree of oxidation nitrogen in ammonia: a) 0, b) -3, 4) +3, 5) 8

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

Nitric acid HNO 3 - one of the strongest acids Physical properties: - colorless liquid - "fumes" in the air, t bale = 84 о С, t pl = -42 о С -in the light turns yellow due to NO 2 evolution: 4HNO 3 = 2H 2 O + 4NO 2 + O 2

Getting HNO 3

Chemical properties Typical properties of acids

Chemical properties Reacts with metals especially:

Chemical properties: Interaction with non-metals

For the curious:

The use of salts HNO 3 -v 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 have properties in common with other acids? a) yes b) no c) depends on the weather Tsarskaya vodka is a) concentrated alcohol b) 3 volumes of HCl and 1 volume of HNO 3 c) concentrated nitric acid

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

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

On the subject: methodological developments, presentations and notes

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

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

Slide 2

This substance was described by an Arab chemist in the 8th century Jabir ibn Hayyan (Geber) in his work "The coachman of wisdom", and from the 15th century this substance was mined for industrial purposes. Thanks to this substance, the Russian scientist V.F. Petrushevsky received dynamite for the first time in 1866. 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, in a mixture with hydrochloric acid, dissolves platinum and gold, recognized as the "king" of metals. The mixture itself, consisting of 1 volume of this substance and 3 volumes of hydrochloric acid, is called "aqua regia".

Slide 3

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

Slide 4

Slide 5

For the first time, alchemists obtained nitric acid by heating a mixture of nitrate and ferrous sulfate: 4KNO3 + 2 (FeSO4 7H2O) (t °) → Fe2O3 + 2K2SO4 + 2HNO3 + NO2 + 13H2O Pure nitric acid was first obtained by Johann Rudolph Glauber with concentrated sulfuric acid : KNO3 + H2SO4 (conc.) (T °) → KHSO4 + HNO3 "Fuming nitric acid" practically free of water Historical background

Slide 6

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

Slide 7

Obtaining HNO 3 Laboratory method of obtaining: NaNO3 + H2SO4 t NaHSO4 + HNO3 in this case, fuming nitric acid is obtained

Slide 8

Industrial method 1. Oxidation of ammonia in 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

Slide 9

Physical properties Physical properties colorless liquid tm = -41.60C tboil = 82.60C mixes up indefinitely with water volatile - “smokes” in air Conc. nitric acid is usually colored yellow,

Slide 10

Research (assignments in groups): (Repetition of PTB!). 1 group: carry out the reaction of a solution of nitric acid and copper (II) oxide, write down the reaction equation, determine its type 2 group: 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 3 group: carry out the reaction of solutions of nitric acid and sodium carbonate, write down the reaction equation, determine its type For all: carry out the reaction of solutions of nitric acid and hydroxydacalium in the presence of phenolphthalein, write down the reaction equation, determine its type

Slide 11

Group No. 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 No. 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 reaction - dissolution of 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 The sign of the reaction is a characteristic “boiling”.

Slide 12

Common with other acids: 1. Strong electrolyte, dissociates well into ions HNO3 -> H + + NO3- Changes the color of the indicator. 2. Reacts with basic oxides CuO + 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

Slide 13

Specific: When heated and under the influence of light, 4HNO3 decomposes = 2H2O + 4NO2 + O2 Reacts with non-metals С + 4HNO3 (conc.) = CO2 + 4NO2 + 2H2O S + 6HNO3 (60%) = H2SO4 + 6NO2 + 2H2O S + 2HNO3 (40 %) = H2SO4 + 2NO P + 5HNO3 (60%) = H3PO4 + 5NO2 + H2O P + 5HNO3 (30%) + 2H2O = 3H3PO4 + 5NO NOneMe + HNO3NO2. Nitric acid oxidizes non-metals

Slide 14

The interaction of nitric acid with metals has been studied quite well, because conc. HNO3 is used as a rocket fuel 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? 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) usually hydrogen is not released in these processes (there is an exception when In practice, it is proved that Mn + decomposed HNO3 actually produces 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 the reduction to ammonia NH3, more precisely to NH4NO3; here the process of reduction of N ( +5) + 8e ----> N (-3)). Intermediate versions of reduction to NO2, NO, N2O, N2 are possible General process scheme: HNO3 + Me ---> nitric acid salt (nitrate) + nitric acid reduction product + H2O

Slide 15

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

Slide 16

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

Slide 17

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 etching and dissolving metals, as well as for separating gold and silver.

Slide 18

Action on the body

Inhalation of nitric acid vapors leads to poisoning, contact of 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

Slide 19

Check yourself:

The oxidation state of nitrogen in HNO3 a) -3 b) 0 c) +5 d) +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, the formula of which is: a) CO2; b) NaOH; c) Al (OH) 3; d) NH3. Tsarskaya vodka is a) concentrated alcohol b) 3 volumes of HCl and 1 volume of HNO3 c) concentrated nitric acid

Slide 20

key

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

Slide 21

output:

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 the 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 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 obtain various important products of the national economy (fertilizers, medicines, plastics, etc.)

Slide 22

Homework:

§26 exercise 4.5 Creative task - presentation of the story of the discovery of nitric acid. The use of nitric acid

Slide 23

Thank you for the lesson

Slide 24

literature

O.S. Gabrielyan, I.G. Ostroumov Handbook of a chemistry teacher, grade 9. Bustard 2003 Lidin R.A., Molochko V.A., Andreeva L.L. Chemical properties of inorganic substances Chemistry2000 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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