How to Form Nitric Acid?
The procedure of Nitric Acid Preparation is discussed below:
Principle
A more volatile acid can be easily displaced from its salt through the other one having less volatile acid. This basic principle is very useful in the preparation of nitric acid in the laboratory. This acid is more volatile acidic in comparison to sulphuric acid. Hence, it is generally displaced by the sulphuric acid from metal nitrates.
Preparation Method of Nitric Acid
50gm of the potassium nitrate (i.e. KNO3 ) and 25ml of concentrated sulphuric acid (i.e. H2SO4) is required in a round bottom flask. This set of reactants are heated to about 200 C. But temperature must not be more than 200 C.
Its chemical equation is:
KNO3 + H2SO4 → KHSO4 + HNO3
Nitric Acid – HNO3
Nitric Acid is a powerful and highly corrosive acid with the chemical formula HNO3. Nitric Acid is a colorless liquid that can range from pale yellow to reddish-brown due to decomposition into nitrogen dioxide and water. Nitric acid is a key reagent in the chemical industry, playing a crucial role in the production of fertilizers, explosives, and various other chemicals.
Nitric acid (HNO3) is a strong mineral acid known for its corrosive and highly reactive properties. Nitric Acid is also known as the Spirit of Niter and Aqua Fortis because of its ability to dissolve metals, particularly copper and silver. In this article, we will study in detail about Niitric Acid, the physical, and chemical properties of Nitric Acid, and the different applications of Nitric Acid.
Table of Content
- What is Nitric Acid?
- Structure of Nitric Acid (HNO3) Molecule
- How to make Nitric Acid?
- Properties of Nitric Acid
- Nitric Acid Chemical Reactions
- Uses of Nitric Acid