Topic 2 9th grade
Lesson 34
Lesson topic: Ammonium salts.
Lesson objectives: educational
– study the composition of ammonium salts, repeat the general chemical properties of salts using the example of ammonium salts, reveal the specific properties of these salts due to the ammonium ion; study the practical use of ammonium salts; deepen basic chemical concepts: substance, chemical reaction; study the practical significance of ammonium salts.
developing – develop in students the ability to compare, analyze and apply information from other areas of knowledge, develop communication skills, and the ability to present the results of group activities;
educational – contribute to the development of environmental literacy in students and an active life position.
Lesson type:learning new material.
Teaching methods:partially search, visual,Forms of organization of cognitive activity:group, frontal, practical.
Technical training aids:computer, projector, screen
Working methods: independent work with the textbook, work in pairs.
Equipment and reagents: solutions - barium chloride, sodium hydroxide, hydrochloric acid, ammonium carbonate, ammonium chloride, ammonium sulfate in a glass of water;ammonium hydroxide, nitric acid, ammonium sulfate, ammonium chloride, ammonium carbonate, silver nitrate, potassium nitrate, hydrochloric acid, sodium hydroxide;
test tubes, test tube rack, alcohol lamp, cotton wool, test tube holder, phenolphthalein paper.
PROGRESS OF THE LESSON: 1. Organizational part of the lesson.
2. Testing students' knowledge.
Survey questions and tasks.
1.Task: An excess of calcium hydroxide was added to 400 g of a solution with a mass fraction of ammonium chloride of 8%. Determine the volume of gas released."
2. Questions: 1.Structure of the ammonia molecule.
2.List the physical properties of ammonia.
3. Chemical properties of ammonia.
4. List the uses of ammonia.
3. The “third wheel” task
TO 3 RO 4 , HCL , H 2 SO 4
Ba(OH) 2, NaNO 3 , NaOH
K 2 O, CO 2 , MgSO 4
4.Test (option 1 – nitrogen, option 2 – ammonia)
1.Gaseous under normal conditions
2.No smell
3.Colorless
4. Slightly soluble in water
5.Nitrogen oxidation degree -3
6.Does not burn in the air
7.Burns in oxygen
8. Reacts with acids to form salts
9. In a molecule there is a covalent polar bond between atoms
10.Relationship with hydrogen in the presence of a catalyst
11. It is the most important biogenic element.
12.Aqueous solution is alkaline
13.It exhibits predominantly restorative properties
Its 14.10% solution is called ammonia
(We exchange notebooks and check).
1, 2, 3, 4, 6, 10, 11, 13
1, 3, 5, 7, 8, 9, 12, 13
3. Study of program material.
1. Ammonium salts - These are complex substances containing ammonium ions combined with acidic residues.
Ammonium salts - salts containing monovalent ammonium ion NH 4 + ; in structure, color and other properties they are similar to the corresponding potassium salts. All ammonium salts are soluble in water and completely dissociate in an aqueous solution. Ammonium salts exhibit the general properties of salts. When exposed to alkali, gaseous NH is released 3 . All ammonium salts decompose when heated. They are obtained by the interaction of NH 3 or NH 4 OH with acids. Ammonium nitrate (ammonium nitrate) NH 4 NO 3 used as nitrogen fertilizer and for the manufacture of explosives - ammonites, ammonium sulfate (NH 4) 2 SO 4 used as a cheap nitrogen fertilizer, ammonium bicarbonate NH4HCO 3 and ammonium carbonate (NH 4) 2 CO 3 used in the food industry, in dyeing fabrics, in the production of vitamins, and in medicine; ammonium chloride (ammonia) NH 4 Cl is used in galvanic cells (dry batteries), for soldering and tinning, in the textile industry, as a fertilizer, and in veterinary medicine.
2. General formula ammonium salts.
N.H. 4 R; (N.H. 4) n R , Where R - acidic residue.
IN N.H. 4 C.L. there is an ammonium cation
3. Physical properties of ammonium salts.
Ammonium salts are solid, crystalline substances, highly soluble in water.
4. Chemical properties of ammonium salts.
Properties common to other salts
Specific properties
1.Strong electrolytes
NH 4 N O 3 = NH 4 + +N O 3 -
2. React with acids - exchange reaction
(NH 4) 2 CO 3 +2HCl =2NH 4 Cl +CO 2 +H 2 O
3.React with other salts
(NH 4) 2 SO 4 +BaCl 2 =2NH 4 Cl +Ba SO 4
4.Subject to hydrolysis
NH 4 Cl +H 2 O.
It is a salt of a weak base and a strong acid. The chain breaks at a weak link. Hydrolysis occurs at the ammonium cation.
1. At high temperatures they decompose
a) if the acid is volatile
NH 4 Cl= NH 3 +HCl
NH 4 HCO 3 → NH 3 + H 2 O + CO 2
b) if the acid is non-volatile
(NH 4) 2 SO 4 =?
c) if the acid is non-volatile and the anion exhibits oxidizing properties
(NH 4 ) 2 Cr 2 O 7 = Cr 2 O 3 + N 2 + 4H 2 O
NH 4 NO 3 = N 2 O + 2 H 2 O
2.React with alkalis
NH 4 Cl + NaOH = NaCl + NH 3 + H 2 O
This is a qualitative reaction to ammonium salts.
3. With acids and salts (exchange reaction)
a) (NH4) 2 CO 3 + 2 HCl → 2NH 4 Cl + H 2 O + CO 2
2NH 4 + + CO 3 2- + 2H + + 2Cl - → 2NH 4+ + 2Cl - + H 2 O + CO 2
CO 3 2- + 2H + → H 2 O + CO 2
b) (NH4) 2 SO 4 + Ba(NO3) 2 → BaSO 4 + 2NH 4 NO 3
2NH 4 + + SO 4 2- + Ba 2+ + 2NO 3 - → BaSO 4 + 2NH 4 + + 2NO 3 -
Ba 2+ + SO 4 2- → BaSO 4
4. Ammonium salts undergo hydrolysis (as a salt of a weak base and a strong acid) - the medium is acidic:
NH4Cl + H2O → NH4OH + HCl
NH4+ + H2O → NH4OH + H+
5. Strong electrolytes (dissociate in aqueous solutions)
NH 4 Cl → NH 4 + + Cl -
CONCLUSION:1) Ammonium salts are electrolytes that dissociate into ammonium cation NH
4
+
and anions of the acid residue.
2)
They exhibit the following properties:
a) Common with salts -
interact with acids and salts if a precipitate or gas is formed.
b) Specific –
react with alkalis to form ammonia, decompose when heated, are highly soluble in water and are electrolytes, during hydrolysis they show an acidic environment or hydrolysis occurs completely.
This is interesting:
The name "ammonium" was proposed in 1808. Humphry Davy. The Latin word ammonium once meant “salt of Ammonium.” Ammonia is a region of Libya. There was a temple of the Egyptian god Ammon, after whom the entire region was called. In Ammonia, ammonium salts have long been obtained by burning camel dung. The decomposition of salts produced a gas, which is now called ammonia. In 1787 The commission on chemical nomenclature gave the gas the name “ammonia.” Russian chemist Zakharov shortened this name to “ammonia.”
A solution of ammonia in water is called ammonia. “Ammonia” because it can be obtained from ammonia NH 4 Cl. But why alcohol? The Latin spiritus means “spirit”, “soul”. Apparently, a chemist unknown to us, who dissolved ammonia obtained from ammonia in water, called the pungent-smelling liquid “the soul of ammonia.”
The name “nitrates” comes from the name of the city of Nitria in Upper Egypt, where the mineral NH 4 NO 3 was first found.
4. Methods for obtaining ammonium salts.
1. Ammonium salts are obtained by reacting ammonia with acids.
2. When ammonia water interacts with acids.
5. The most important areas of application of ammonium salts.
Like fertilizer
For the production of explosives
Ammonium bicarbonate and ammonium carbonate in the food industry as a leavening agent for dough.
When dyeing fabrics in the textile industry
In the production of vitamins
In medicine
When soldering
In dry batteries
When dressing leather
In pyrotechnics
Conclusions:
Ammonium salts are formed by ammonium cations and anions of acid residues
Their physical properties are similar to salts of alkali metals, especially potassium
A qualitative reaction to ammonium cation is interaction with alkalis when heated; the released gas has a characteristic odor and colors the phenolphthalein paper crimson.
4. Consolidation of the studied material
Consolidation of the studied material can be carried out in the form of differentiated individual independent work of students according to options.
OPTION 1
Write complete and abbreviated ionic equations for reactions occurring between substances:
- ammonium chloride and silver nitrate;
Ammonium carbonate and hydrochloric acid;
Ammonium nitrate and sodium hydroxide.
OPTION 2
Complete the reaction equations in full and abbreviated ionic form:
(NH 4) 2 SO 4 + ? → NH 4 CI + BaSO 4 ↓
NH 4 CI + ? → ? + ? + NH 3
(NH 4) 2 S + HCI → ? + ?
OPTION 3
Write complete and abbreviated ionic equations for the reactions occurring between the following pairs of substances:
- ammonium salt and other salt;
Ammonium salt and alkali;
Ammonium salt and acid.
5.Homework:§ 26, exercise 1-4 (written)
Saltpeter– natural nitrates – were known in China in the first centuries AD; it was used to prepare gunpowder and fireworks displays. Later it is mentioned in works (Latin names - nitro or sal nitri). By heating saltpeter with iron sulfate, alchemists obtained, which for a long time was called in Latin aqua fortis (“strong water”; in Russian texts the term “ strong vodka»).
Pure nitric acid was first obtained by a German chemist Johann Rudolf Glauber acting on saltpeter with oil of vitriol (concentrated):
KNO 3 + H 2 SO 4 = KHSO 4 + HNO 3
Atacama Desert. Place of extraction of Chilean saltpeter He also discovered that when nitric acid reacts with potash K 2 CO 3, pure potassium nitrate. This discovery was of great practical importance, because previously, saltpeter, necessary for the production of gunpowder, was imported to Europe from the countries of the East, and was also isolated from salt deposits on the walls of stables or from saltpeter pits, where it was formed under the influence of microorganisms as the end product of the oxidation of nitrogen-containing organic compounds .
By calcining a mixture of saltpeter NaNO 3, ferrous sulfate FeSO 4 ∙7H 2 O, potassium alum KAl(SO 4) 2 ∙12H 2 O and ammonia NH 4 Cl, the alchemists managed to obtain a liquid that dissolved even the “king of metals” -. That’s why it was called aqua regia, which means “ royal water" or " aqua regia" Aqua regia is a yellow liquid formed by mixing three volumes and one volume of nitrogen. Even platinum dissolves easily in aqua regia.
Nitrogen was discovered independently at the end of the 18th century. several scientists. English explorer Henry Cavendish obtained “mephic air” (as he called nitrogen) by repeatedly passing air over hot coal (thereby removing oxygen), and then through a solution to absorb the resulting .
Henry Cavendish Cavendish's compatriot Joseph Priestley described the formation of a gas that does not support combustion and respiration - “phlogisticated air” - by observing the combustion of a candle in a closed vessel.
Finally, another English scientist, Daniel Rutherford, also obtained nitrogen from the air. Unlike Cavendish and Priestley, he immediately, in 1772, published a work where he described the production and properties of the “suffocating air” he isolated. Therefore, it was Rutherford who is considered the discoverer of nitrogen.
In nature, the largest amount of nitrogen is found in unbound form in the air. The basic composition of atmospheric air was determined by A.L. Lavoisier, at whose suggestion the new element was named nitrogen. This name is made up of the Greek word “zoe” (“life”) and the prefix “a”- (“non-”) and means “lifeless,” “not giving life.” The Latin word for nitrogen, Nitrogenium, translates as “saltpeter-forming.”
Minerals that contain nitrogen are rare, such as Chilean saltpeter NaNO 3, deposits of which stretch along the coast of Chile and Peru over a distance of over 3,600 km. At the end of the 19th century. its production was approximately 0.5 tons per year. It is no coincidence that entrepreneurs and scientists feared that its reserves would soon run out. This prompted chemists to develop technologies for fixing air nitrogen.
In industry, nitrogen is obtained from liquid air. To do this, the air is transferred to a liquid state, and at a temperature of – 196 0 C, nitrogen evaporates.
Nitrogen is obtained in the laboratory decomposition of ammonium nitrite NH 4 NO 2 when heated:
NH 4 NO 2 = N 2 + H 2 O
Physical properties
A liquid nitrogen Nitrogen– a colorless, tasteless and odorless gas (t pl = -210 0 C, t boil = -196 0 C), slightly soluble in water. Free nitrogen is chemically inert due to its high strength molecules N 2, in which the atoms are connected by a triple bond. Therefore, nitrogen hardly enters into chemical reactions and does not support combustion and respiration.
Characteristic oxidation states:
— 3 0 +1 +2 +3 +4 +5
NH 3 N 2 N 2 O NO N 2 O 3 NO 2 N 2 O 5
Chemical properties
In chemical reactions, nitrogen can be both an oxidizing agent and a reducing agent.
Nitrogen interacts as an oxidizing agent:
N2 + 3Ca = Ca3N2
Nitrogen interacts as a reducing agent:
N 2 + F 2 = 2NF 3
Application
Nitrogen is the feedstock for the production of ammonia.
Ammonia
Ammonia– a colorless gas with a pungent odor, highly soluble in water. 700 liters of ammonia dissolve in one liter of water at a temperature of 20 0 C. This solution is called ammonia water or ammonia.
Chemical properties
Acid-base properties
The nitrogen atom in the ammonia molecule has a lone pair of electrons, which can participate in the formation of a donor-acceptor bond. In particular, the nitrogen atom in NH 3 is capable of attaching the hydrogen ion H +. Substances whose molecules are capable of attaching hydrogen ions have basic properties. Therefore, ammonia has the following basic properties:
- interaction of ammonia with water:
NH 3 + HOH ⇄ NH 4 OH ⇄ NH 4 + + OH —
- interaction with hydrogen halides:
NH 3 + HCl ⇄ NH 4 Cl
- interaction with (resulting in the formation of medium and acidic salts):
NH 3 + H 3 PO 4 = (NH 4) 3 PO 4 ; (NH 4) 2 HPO 4; (NH4)H2PO4
- ammonia reacts with certain metals to form complex compounds - ammonia:
CuSO 4 + 4NH 3 = SO 4 Tetraammine copper (II) sulfate
AgCl + 2NH 3 = Cl Silver (I) diamine chloride
Redox properties
In the ammonia molecule, nitrogen has an oxidation state of 3, so in redox reactions it can only donate electrons and is only a reducing agent.
- ammonia restores some of them:
2NH 3 + 3CuO = N 2 + 3Cu + 3H 2 O
- ammonia is oxidized without a catalyst to nitrogen:
4NH 3 + 3O 2 = 2N 2 + 6H 2 O
- ammonia in the presence of a catalyst is oxidized to nitrogen monoxide NO:
4NH 3 + 5O 2 = 4NO + 6H 2 O
Ammonium salts
Ammonium chloride When ammonia or ammonium hydroxide reacts with ammonium salts:
All ammonium salts are highly soluble in water. Ammonium salts have. The special properties of ammonium salts include their thermal decomposition reactions, which proceed differently depending on the nature of the anion, for example:
(NH 4) 2 SO 4 = NH 3 + NH 4 HSO 4
NH 4 NO 3 = N 2 O + 2H 2 O
NH 4 Cl = NH 3 + HCl
The reaction of ammonium salts with is qualitative reaction to ammonium cationN.H. 4 + :
NH 4 Cl + NaOH = NaCl + NH 3 + H 2 O
NH 4 + + OH - = NH 3 + H 2 O
The ammonia released is determined by its smell or by the blueness of wet litmus paper.
Application of ammonia and ammonium salts
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Ammonium salts are salts containing a positively charged ammonium ion NH4+; in structure, color and other properties they are similar to the corresponding potassium salts. All ammonium salts are soluble in water and completely dissociate in an aqueous solution. Ammonium salts exhibit the general properties of salts. When exposed to alkali, ammonia gas is released. All ammonium salts decompose when heated. They are obtained by reacting NH3 or NH4OH with acids.
Application
Ammonium nitrate (ammonium nitrate) NH4NO3 is used as a nitrogen fertilizer and for the production of explosives - ammonites;
Ammonium sulfate (NH4)2SO4 - as a cheap nitrogen fertilizer;
Ammonium bicarbonate NH4HCO3 and ammonium carbonate (NH4)2CO3 - in the food industry in the production of flour confectionery products as a chemical leavening agent, in dyeing fabrics, in the production of vitamins, in medicine;
Ammonium chloride (ammonia) NH4Cl - in galvanic cells (dry batteries), during soldering and tinning, in the textile industry, as a fertilizer, in veterinary medicine.
Chemical properties of salts
Strong electrolytes (dissociate in aqueous solutions):
NH4Cl ↔ NH4+ + Cl−
Heat decomposition:
a) if the acid is volatile
NH4Cl → NH3 + HCl
NH4HCO3 → NH3 + H2O + CO2
b) if the anion exhibits oxidizing properties
NH4NO3 → N2O + 2H2O
(NH4)2Cr2O7 → N2 + Cr2O3+ 4H2O
With acids (exchange reaction):
(NH4)2CO3 + 2HCl → 2NH4Cl + H2O + CO2
2NH4+ + CO32− + 2H+ + 2Cl− → 2NH4+ + 2Cl− + H2O + CO2
CO32− + 2H+ → H2O + CO2
With salts (exchange reaction):
(NH4)2SO4 + Ba(NO3)2 → BaSO4 ↓ + 2NH4NO3
2NH4+ + SO42− + Ba2+ + 2NO3− → BaSO4 ↓ + 2NH4+ + 2NO3−
Ba2+ + SO42− → BaSO4 ↓
Ammonium salts undergo hydrolysis (as a salt of a weak base and a strong acid) - the medium is acidic:
NH4Cl + H2O ↔ NH4OH + HCl
NH4+ + H2O ↔ NH4OH + H+
When heated with alkalis, ammonia is released (qualitative reaction to ammonium ion)
NH4Cl + NaOH → NaCl + NH3 + H2O
Iron deficiency anemia (IDA) is a hematological syndrome characterized by impaired hemoglobin synthesis due to iron deficiency and manifested by anemia and sideropenia. The main causes of IDA are blood loss and lack of heme-rich foods - meat and fish.
Treatment is carried out only with long-term intake of ferrous iron preparations orally in moderate doses, and a significant increase in hemoglobin, unlike improvement in well-being, will not be immediate - after 4-6 weeks.
Usually, any ferrous iron preparation is prescribed - most often it is ferrous sulfate - its prolonged dosage form is better, in an average therapeutic dose for several months, then the dose is reduced to the minimum for several more months, and then (if the cause of anemia is not eliminated), the maintenance minimum continues doses for a week every month for many years. So, this practice has proven itself well in the treatment of women with chronic posthemorrhagic iron deficiency anemia due to long-term hyperpolymenorrhea with tardyferron - one tablet in the morning and evening for 6 months without a break, then one tablet a day for another 6 months, then for several years every day for a week on menstruation days . This disciplines patients, prevents them from forgetting the timing of taking the drug and provides an iron load when protracted, heavy periods appear during menopause. A senseless anachronism is determining hemoglobin levels before and after menstruation.
Ammonium salts
TO The ammonium ion NH4+ plays the role of a metal cation and it forms salts with acidic residues: NH4NO3 - ammonium nitrate, or ammonium nitrate, (NH4)2SO4 - ammonium sulfate, etc.
All ammonium salts are crystalline solids, highly soluble in water. In a number of properties they are similar to alkali metal salts, and primarily to potassium salts, since the radii of the K+ and NH+ ions are approximately equal.
Ammonium salts are obtained by reacting ammonia or its aqueous solution with acids.
They have all the properties of salts due to the presence of acidic residues. For example, ammonium chloride or sulfate reacts with silver nitrate or barium chloride, respectively, forming characteristic precipitates. Ammonium carbonate reacts with acids because the reaction produces carbon dioxide.
In addition, the ammonium ion provides another property common to all ammonium salts: its salts react with alkalis when heated to release ammonia.
This reaction is a qualitative reaction to ammonium salts, since the ammonia formed is easily detected (how exactly?).
The third group of properties of ammonium salts is their ability to decompose when heated, releasing ammonia gas, for example:
NH4Сl = NH3 + HCl
This reaction also produces gaseous hydrogen chloride, which evaporates along with ammonia, and upon cooling combines with it again, forming a salt, i.e., when heated in a test tube, dry ammonium chloride sublimes, but white crystals appear on the upper cold walls of the test tube again NН4Сl (Fig. 32).
The main areas of application of ammonium salts were shown earlier, in Figure 31. Here we draw your attention to the fact that almost all ammonium salts are used as nitrogen fertilizers. As you know, plants are able to absorb nitrogen only in bound form, that is, in the form of NH4 or N03 ions. The remarkable Russian agrochemist D.N. Pryanishnikov found that if a plant has a choice, it prefers the ammonium cation to the nitrate anion, so the use of ammonium salts as nitrogen fertilizers is especially effective. A very valuable nitrogen fertilizer is ammonium nitrate NH4NO3.
Let us note other areas of application of some ammonium salts.
Ammonium chloride NH4Cl is used for soldering, as it cleans the metal surface of the oxide film and solder adheres well to it.
Ammonium bicarbonate NH4NC03 and ammonium carbonate (NH4)2CO3 are used in confectionery, as they easily decompose when heated and form gases that loosen the dough and make it fluffy, for example:
NH4HC03 = NH3 + H20 + CO2
Ammonium nitrate NН4NO3 mixed with aluminum and coal powders is used as an explosive - ammonal, which is widely used in mining.
Ammonia
Physical properties: ammonia (NH3)– colorless gas with a pungent odor, soluble in water, 2 times lighter than air; when cooled to -33.4 °C and normal pressure, it turns into a transparent liquid; at 77.8 °C it solidifies. The mass fraction of ammonia in the concentrated solution is 25%. A solution of NH3 in water - ammonia water or ammonia. Medical ammonia – 10%. At low temperatures, crystalline hydrate NH3 forms in solution? H2O. Molecule structure: characterized by sp3 hybridization. The formation of a molecule involves 3 unpaired p-electrons of nitrogen and 1s electrons of hydrogen atoms. The molecule has the shape of a regular pyramid, with nitrogen atoms at the top and hydrogen atoms at the corners.
Chemical properties:
1) when NH3 is dissolved in water, hydrated ammonia molecules and partially ammonium ions are formed - NH4+ and OH-ions - an aqueous solution of ammonia has a slightly alkaline reaction.
2) NH3 interacts with acids: NH3 + H2SO4 = NH4HSO4;
3) ammonia is a strong reducing agent. When heated, it reduces Cu from CuO: 3CuO + 2NH3 = Cu + N2 + 3H2O;
4) in oxygen NH3 burns with a yellow flame: 4NH3 + 3O2 = 2N2? + 6H2O;
5) NH3 is oxidized by atmospheric oxygen in the presence of catalysts: Pt, Cr2O3, Rh: 4NH3 + 5O2 = 4NO? + 6H2O;
6) when replacing hydrogen with metals, amides are formed: Na + NH3 = NaNH2 + 1/2 H2;
7) hydrogen in NH3 can be replaced by halogens. When a solution of ammonium chloride is exposed to gaseous chlorine, nitrogen chloride is formed: NH4Cl + 3Cl2 = 4HCl + NCl3.
Ammonia (nitrogen chloride).
Receipt: in industry until the end of the 19th century century ammonia was obtained as a by-product during the coking of coal, which contains up to 1–2% nitrogen.
At first XX century New industrial methods for the production of ammonia have been developed, based on the binding or fixation of atmospheric nitrogen.
In 1904 a cyamide method has appeared, based on the ability of nitrogen to react with calcium carbide at high temperatures, forming calcium cyamide CaCN2, which, when exposed to water vapor at a pressure of 0.6 MPa, easily decomposes into ammonia and calcium carbonate:
Later, another way to produce ammonia appeared - the direct interaction of nitrogen and oxygen under the influence of electrical discharges, but this reaction was reversible until optimal conditions were found for it. These conditions were high pressure and low temperature, the use of catalysts - sponge iron with additives of activators (oxides of aluminum, potassium, calcium, silicon, magnesium).
Ammonium salts– complex substances including ammonium cations NH4+ and acid residues.
Physical properties: Ammonium salts are crystalline solids that are highly soluble in water.
Chemical properties: Ammonium has the properties of a metal, therefore the structure of its salts is similar to alkali metal salts, since NH4+ ions and alkali metal (potassium) ions have approximately the same radii. Ammonium does not exist in its free form, because it is chemically unstable and instantly decomposes into ammonia and hydrogen. Evidence of the metallic nature of ammonium is the presence of ammonium amalgam - an alloy of ammonium with mercury, similar to that of alkali metals. When treating ammonium amalgam with a cold solution of copper sulfate, the amalgam will displace the nth amount of copper:
Ammonium salts have an ionic lattice and have all the properties of typical salts:
1) are strong electrolytes - they undergo dissociation in aqueous solutions, forming an ammonium cation and an acid anion:
2) undergo hydrolysis (salt of a weak base and a strong acid):
acidic environment, pH<7, лакмус красный;
3) enter into an exchange reaction with acids and salts:
4) interact with alkali solutions to form ammonia - a qualitative reaction to ammonium ion:
ammonium salts are determined by the smell of ammonia released as a result of the reaction, as well as by the blue color of litmus;
5) decompose when heated:
Receipt: NH3 + HNO3 = NH4NO3 (ammonium nitrate); 2NH4OH + H2SO4 = (NH4)2SO4 (ammonium sulfate) + 2H2O.
Application: ammonium salts are widely used in practice: ammonium sulfate - (NH4)2SO4, ammonium nitrate - NH4NO3, ammonium dihydrogen phosphate - NH4H2PO4 and ammonium hydrogen phosphate - (NH4)2HPO4 are used as mineral fertilizer. The advantage of the fertilizer is its increased ammonia content. Ammonium chloride (NH4Cl) is used - ammonia.