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Азотная кислота

Строение молекулы

Соли азотной кислоты

Азотные удобрения

00:00:00

[music]

00:00:17

nitric acid has the formula hno3 the

00:00:20

structural formula of nitric acid

00:00:23

should be depicted as follows: one of the bonds

00:00:26

between the nitrogen and oxygen atoms

00:00:28

is formed by donor to acceptor

00:00:30

mechanism, both oxygen atoms are connected

00:00:33

only to the nitrogen atom, the equivalent

00:00:36

valency of nitrogen in this case is

00:00:39

four and the oxidation state plus 5

00:00:42

nitric acid a colorless fuming

00:00:45

liquid with a pungent odor in aqueous

00:00:48

solutions dissociates

00:00:49

dilute nitric acid has

00:00:52

all the typical properties of acids

00:00:54

interacts with basic m factor

00:00:57

oxides, for example magnesium oxide, forming

00:01:01

magnesium nitrate and water with bases,

00:01:04

for example potassium hydroxide,

00:01:06

forming potassium nitrate and water since

00:01:10

nitric acid is one basic

00:01:12

acid salts, it does not form salami

00:01:15

if a precipitate is formed or gas is released,

00:01:18

for example, when reacting with

00:01:21

potassium carbonate, unstable carbonic

00:01:24

acid is formed, which breaks down into carbon dioxide

00:01:26

and water, the

00:01:29

typical acidic properties of nitric

00:01:31

acid do not include interaction with

00:01:34

metals,

00:01:35

concentrated and dilute nitric

00:01:37

acid is a strong oxidizing agent, therefore,

00:01:40

-reacts particularly with metals during the

00:01:43

interaction of dilute nitric

00:01:45

acid with active metals in the

00:01:48

voltage series up to zinc;

00:01:50

ammonia or ammonium salts,

00:01:52

metal nitrate and water are predominantly formed; the oxidation state of

00:01:56

nitrogen decreases from plus 5 to

00:01:59

minus 3 when dilute

00:02:02

nitric acid interacts with other metals

00:02:04

predominantly nitrogen oxide is formed 2

00:02:07

metal nitrate and water, the oxidation degree of

00:02:10

nitrogen decreases from plus 5 to

00:02:13

plus 2 in some cases

00:02:16

nitrogen can be formed, for example, when

00:02:18

magnesium reacts with dilute

00:02:21

nitric acid, magnesium nitrate is formed,

00:02:23

ammonia and water, and when

00:02:26

copper reacts with dilute

00:02:28

nitric acid,

00:02:29

nitrate is formed copper 2 nitrogen monoxide

00:02:32

and water,

00:02:37

when concentrated

00:02:39

nitric acid interacts with active

00:02:40

metals in the voltage series up to

00:02:43

zinc,

00:02:46

nitrogen oxide plus one metal nitrate and water are predominantly formed, the

00:02:49

oxidation state of nitrogen

00:02:51

decreases from plus 5 to plus 1 when

00:02:54

concentrated nitric

00:02:56

acid interacts with others metals

00:02:58

predominantly form nitrogen oxide 4

00:03:01

metal nitrate and water, the

00:03:04

oxidation degree of nitrogen

00:03:06

decreases from plus 5 to plus four,

00:03:09

for example, when magnesium reacts with

00:03:11

concentrated nitric acid,

00:03:13

subway from magnesium is formed, nitrogen oxide 1

00:03:17

and water, let

00:03:21

's see what happens when

00:03:23

copper reacts with concentrated

00:03:24

nitric acid

00:03:28

in flask with a concentrated

00:03:30

van and nitric acid, add copper

00:03:32

shavings,

00:03:43

the reaction occurs without heating,

00:03:49

we see the appearance of a green

00:03:51

solution, this is copper nitrate 2,

00:04:05

the sign of the reaction is clearly visible, emitting a

00:04:08

brown color, this is nitric oxide 4,

00:04:15

thus, when

00:04:17

concentrated nitric acid reacts with

00:04:19

copper, a salt is formed, copper nitrate 2

00:04:22

oxide nitrogen oxide 4 and water

00:04:32

iron chrome and aluminum react

00:04:35

with concentrated nitric acid

00:04:36

only when heated at

00:04:39

room temperature they are passivated

00:04:41

gold platinum osmium iridium

00:04:44

does not react with nitric acid even when

00:04:47

heated

00:04:51

nitric acid reacts in three stages.

00:05:03

dioxide in

00:05:05

water with simultaneous oxidation by

00:05:07

oxygen

00:05:12

salts of nitric acid nitrates are solid

00:05:16

crystalline substances they have the

00:05:18

specific property of being able to

00:05:21

decompose when heated, the

00:05:23

decomposition products depend on the metal

00:05:25

included in the salt if the metal

00:05:29

is in the voltage series to the left of magnesium

00:05:31

whose police then the decomposition products

00:05:33

will be metal nitrite and oxygen,

00:05:37

for example,

00:05:38

position sodium nitrate,

00:05:41

sodium nitrite and oxygen are formed

00:05:43

if the metal is in the voltage series

00:05:45

from magnesium to copper inclusive plus

00:05:48

lithium, then metal oxide is formed,

00:05:51

nitrogen dioxide and oxygen,

00:05:54

so during the decomposition of zinc nitrate,

00:05:56

zinc oxide is formed,

00:05:58

nitrogen dioxide and oxygen if the metal

00:06:01

is after the media in the voltage series,

00:06:03

then when decomposition produces a metal,

00:06:06

nitrogen dioxide and oxygen,

00:06:09

for example, the decomposition of silver nitrate

00:06:12

produces silver, nitrogen dioxide and

00:06:15

oxygen,

00:06:19

some salts of nitric acid are called

00:06:22

liters sodium nitrate

00:06:24

sodium nitrate

00:06:27

potassium nitrate potassium nitrate

00:06:30

from ammonium ammonium nitrate

00:06:34

many nitrates are used as

00:06:36

nitrogen-containing fertilizers to increase

00:06:39

crop yields

Description:

Видео на Дзен https://dzen.ru/profile/editor/id/62319fc82f5f8d062c902f1a/publications Химия 9 класс Урок№15 - Азотная кислота. Строение молекулы. Свойства разбавленной и концентрированной азотной кислоты. Соли азотной кислоты. Азотные удобрения. На нашем уроке мы более узнаем о строении, свойствах и применении азотной кислоты. Разберем окислительные свойства азотной кислоты. Изучим состав и свойства солей азотной кислоты - нитратов. Азотная кислота имеет формулу HNO3. Азотная кислота – бесцветная дымящая жидкость с резким запахом. В водных растворах диссоциирует. Разбавленная азотная кислота обладает всеми типичными свойствами кислот. Концентрированная и разбавленная азотная кислота являются сильными окислителями, поэтому по-особому реагируют с металлами. При взаимодействии разбавленной азотной кислоты с активными металлами (стоящими в ряду напряжений до цинка) преимущественно образуются аммиак (или соль аммония), нитрат металла и вода. Степень окисления азота при этом понижается с +5 до -3. При взаимодействии разбавленной азотной кислоты с другими металлами преимущественно образуются оксид азота два, нитрат металла и вода. Степень окисления азота при этом понижается с +5 до +2. Также, в некоторых случаях может образовываться азот. Например, при взаимодействии магния с разбавленной азотной кислотой образуются: нитрат магния, аммиак и вода, а при взаимодействии меди с разбавленной азотной кислотой образуются: нитрат меди (II), моноксид азота и вода. Получают азотную кислоту в три стадии: 1. Каталитическое окисление аммиака 2. Окисление моноксида азота в диоксид 3. Растворение диоксида азота в воде с одновременным окислением кислородом Соли азотной кислоты – нитраты – твердые, кристаллические вещества. Помимо общих свойств солей обладают специфическим свойством – способностью разлагаться при нагревании. Продукты разложения зависят от металла, входящего в состав соли. Некоторые соли азотной кислоты называют селитрами, например, нитрат натрия – натриевая селитра. Многие селитры используются в качестве азотсодержащих удобрений для повышения урожайности сельхозхозяйственных культур.

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