Ammonia and nitric acid are two essential chemical compounds widely used in various industrial and scientific applications. Ammonia, a colorless gas with a pungent smell, is known for its alkaline properties and solubility in water, forming ammonium hydroxide. On the other hand, nitric acid, a highly corrosive and strong acid, is recognized for its oxidizing properties and its role in producing fertilizers and explosives. Understanding the physical and chemical properties of ammonia and nitric acid is crucial for their safe handling and effective utilization in industries like agriculture, pharmaceuticals, and chemical manufacturing.
Ammonia is one of the most widely produced compounds. It is one of the most prevalent hydrides in the environment. Small amounts of ammonia are found in soil and air owing to the decomposition of nitrogenous organic materials. The primary application of nitric acid is in the production of fertilizers. It is utilized in the production of a variety of polymers, including polyamides and polyurethane.
Ammonia is one of the most widely produced compounds. It is one of the most prevalent hydrides in the environment. The ammonia in the atmosphere is mostly created by the breakdown of bacteria, which is released from the nitrogenous components of animals and plants. Azane is the IUPAC term for ammonia. Ammonia’s chemical formula is NH3. Ammonia has a variety of properties.
Also Check: Ammonium Nitrate Formula
Ammonia is an atom with a covalent bond. It is seen as a dot structure. The particle is formed by the overlap of three hydrogen atom orbitals and three nitrogen sp3 hybrid orbitals in the structure as the center atom. A single pair is engaged in the fourth sp3 hybrid orbital.
This gives the compound a trigonal pyramidal form. The H-N-H bond edge is 107.3°, which is somewhat less than the 109°28 tetrahedral edge. This is due to the bond pair-lone pair repulsions pushing the N-H bonds inwards. Ammonia is linked in solid and liquid phases by hydrogen bonds.
2NH4Cl + Ca(OH)2 → 2NH3 + 2H2O + CaCl2
N2 (g) + 3H2 (g) ↔ 2NH3 (g)
The basic ingredients for the reaction are nitrogen and hydrogen. Scrubbing is a procedure that removes contaminants from gases. Following the cleaning procedure, the gases are amalgamated and pushed via a compressor. After that, the mixture is crushed at a pressure of 200 atm. The compressed gases are then transferred via a converter, where they are heated to 450°C and compressed to 200 atm. Nitrogen interacts with hydrogen to produce ammonia, however, only about 15% of the gas is produced. The ammonia, hydrogen, and nitrogen mixture is extracted from the converter. It is cooled to the point that it liquefies in the tank and is thus collected.
The Properties Of Ammonia are mentioned as follows-
NH3+H20 → NH4++OH–
ZnSO4+2NH4OH (g) → Zn(OH)2+(NH4)2SO4
Friedrich Wilhelm Ostwald invented a method for producing nitric acid from ammonia at the turn of the twentieth century. Because of the creation of nitric acid, the Germans were able to create explosives without having to import them from other nations such as Chile during World War II. HNO3 is the chemical formula for nitric acid
Three oxygen atoms, one nitrogen atom, and one hydrogen atom make up a nitric acid molecule. In HNO3 molecules, one of the oxygen atoms is doubly connected to the central nitrogen atom. Another oxygen atom is coupled to the central nitrogen atom as well as a hydrogen atom in a single bond. The final oxygen atom in the nitric acid molecule has a charge of -1 and is connected to the central nitrogen atom singly. The nitrogen atom in the molecule’s centre has a charge of +1 because it is engaged in four covalent bonds (with three oxygen atoms).
As a result, the nitric acid molecule has no net charge. It should be emphasised that as a result of resonance, the charges in these molecules may become delocalized.
NaNO3+H2SO4 → NaHSO4+HNO3
2NO+O2 → 2NO2(g)
3NO2 (g)+H2O (l) →2HNO3(aq)+NO (g)
HNO3 (aq) + H2O (l)→ H3O+(aq)+NO–3 (aq)
Cu+4HNO3 → Cu(NO3)2+ 2NO2+2H2O
Although ammonia is not very flammable, ammonia canisters may explode when exposed to intense heat.
When excessive amounts of ammonia are introduced to the human body, they induce rapid burning of the eyes, nose, throat, and lungs, as well as blindness, lung damage, and death. Inhaling a greater dosage of 300 ppm is instantly hazardous to one’s life and health. Lower quantities might induce coughing and nose and throat discomfort if inhaled.
Nitric acid exposure can induce eye, skin, and mucous membrane irritation, as well as delayed pulmonary edema, pneumonitis, bronchitis, and tooth erosion. Nitric acid is a very corrosive substance.