Preparation, Properties, Structure and Uses of Ammonia and Nitric Acid

Ammonia is generated in the atmosphere mostly as a result of bacteria degradation of nitrogenous components emitted by animals and plants. Azane is the IUPAC term for ammonia. Ammonia has the chemical formula NH₃. Ammonia has a variety of properties.

Nitric acid (HNO₃) is a colourless liquid that emits bitter yellow or red odours. Nitric acid exposure can induce eye, skin, and mucous membrane irritation, as well as delayed pulmonary edoema, pneumonitis, bronchitis, and tooth erosion. Nitric acid is a very corrosive substance. Exposure to nitric acid may cause injury to workers. The amount of exposure is determined by the dose, duration, and type of job performed.

Ammonia Preparation:

Small amounts of azane/ammonia are present in soil and air as a result of the breakdown of nitrogenous organic matter.

Ammonium salts are produced to react with caustic soda to produce ammonia on a modest scale:

2NH₃ + 2H₂O + CaCl₂ ←→  2NH₄Cl + Ca(OH)₂

Haber’s method is employed in large-scale manufacturing. Haber’s procedure includes the following steps:

2NH₃ = N₂ (g) + 3H₂ (g)

The basic ingredients for the reaction are nitrogen and hydrogen. Scrubbing is the process of removing contaminants from the gases.

Following the cleaning procedure, the gases are amalgamated and pushed via a compressor. After that, the mixture is crushed at 200 atm. The compressed gases are then transferred via a converter, where they are heated to 450°C and pushed through a 200 atm pressure. Ammonia is generated when nitrogen combines with hydrogen, but only about 15% of the gas is produced. The ammonia, hydrogen, and nitrogen mixture in the converter is eliminated. It is cooled in the tank, where it liquefies and is collected.

Ammonia Properties:

The properties of ammonia are as follows:

1. Azane is a colourless gas with an unpleasant odour.
2. At 198.4K and 239.7K, it boils.
3. This gas dissolves quickly in water. Because OH- ions occur in the aqueous solution of NH₃, it is a weak basic.

NH₃+H₂0 → NH,sub>4+ OH–
NH₃+H₂0 →  NH₃+H₂0

 4.When ammonium combines with an acid, it forms ammonium salts.

ZnSO₄+2NH₄OH (g) → Zn(OH)₂+(NH₄)₂SO₄  → Zn(OH)₂+(NH₄)₂SO₄ Zn(OH)₂+(NH₄)₂SO₄ →  Zn(OH)₂+(NH₄)

Uses of Ammonia

1. Ammonia is utilised as a refrigerant because of its properties in its aqueous state.
2. It’s utilised in the production of urea.
3. Urea is a good nitrogen fertiliser.
4. Because of its cleaning characteristics, azane can be used to remove oil.

Nitric Acid

Friedrich Wilhelm Ostwald devised a method for obtaining nitric acid from ammonia at the turn of the twentieth century. The invention of nitric acid allowed the Germans to create explosives without having to import it from other nations, such as Chile, during World War II. HNO3 is the chemical formula for nitric acid.

Nitric Acid Preparation

This gas is generated on a small scale by heating concentrated sulphuric acid with NaNO3 or KNO3.

NaHSO4+HNO3 = NaNO3+H2SO4+HNO3

The Ostwald technique is used for large-scale preparations.

At 500 K and a pressure of 9 bars, NH3 undergoes catalytic oxidation by oxygen present in the atmosphere in the presence of Pt/Rh as a catalyst.

4NH3 + 5O2 = 4NO(g) + 6H2O

The resulting nitric oxide is then made to react with oxygen to produce NO2.

HNO3 is generated when NO2 is dissolved in H2O.

2HNO3(aq)+NO ←→  3NO2 (g)+H2O(l)+NO (g)

Nitric Acid’s Characteristics

In its natural state, it is colourless.

The liquid has a boiling point of 84.1°C and freezes to a white solid at -41.55°C.

It’s a powerful acid that breaks down into nitrate ions and hydronium.

HNO3 (aq) +H2O (l) = H3O+(aq)+NO3+NO3– (aq)

In its concentrated form, HNO3 is a powerful oxidizer.

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

Nitric Acid’s Applications

Nitric acid is primarily used in the production of fertilisers.

It’s used to make a variety of polymers, including polyamides and polyurethane.

Nitric acid is mostly used to purify precious metals such as platinum, gold, and silver.

In the woodworking industry, diluted nitric acid is used to create maple and pine wood and give it an aged appearance.

Conclusion

Therefore, we can finally conclude that ammonia had many applications and uses in laboratories and as well as day to day life, like producing nitric acids. Small amounts of ammonia are present in soil and air as a result of the breakdown of nitrogenous organic matter. Ammonium salts are produced to react with caustic soda to produce ammonia on a modest scale. It is produced by using the Haber’s process. The basic ingredients for the reaction are nitrogen and hydrogen. Scrubbing is the process of removing contaminants from the gases. Following the cleaning procedure, the gases are amalgamated and pushed via a compressor. After that, the mixture is crushed at 200 atm. The compressed gases are then transferred via a converter, where they are heated to 450°C and pushed through a 200 atm pressure. Ammonia is generated when nitrogen combines with hydrogen, but only about 15% of the gas is produced. The ammonia, hydrogen, and nitrogen mixture in the converter is eliminated. It is cooled in the tank, where it liquefies and is collected.