Explain the rules for naming acids and provide ... - SS1 Chemistry Acids, Bases, and Salts Question

Acids are named based on the anion they contain. The rules for naming acids depend on whether the anion is a polyatomic ion or a simple ion.

 

Naming Acids with Polyatomic Ions:

-       If the polyatomic ion ends in "-ate," the acid name is derived by replacing "-ate" with "-ic" and adding the word "acid." For example, sulphate becomes sulfuric acid (H2SO4).

-       If the polyatomic ion ends in "-ite," the acid name is derived by replacing "-ite" with "-ous" and adding the word "acid." For example, nitrite becomes nitrous acid (HNO2).

 

Naming Acids with Simple Ions:

-       If the anion is a simple ion, the acid name is derived by adding the prefix "hydro-" and replacing the suffix "-ide" with "-ic" and adding the word "acid." For example, chloride becomes hydrochloric acid (HCl).

 

Common Acids and their Properties:

1. Hydrochloric acid (HCl): Colourless, highly corrosive liquid. It is a strong acid commonly used in laboratory and industrial processes.
2. Sulfuric acid (H2SO4): Highly corrosive, oily liquid. It is a strong acid used in various industrial applications, such as manufacturing fertilisers and dyes.
3. Nitric acid (HNO3): Colourless to yellow liquid. It is a strong acid involved in the production of fertilisers, explosives, and various organic compounds.
4. Acetic acid (CH3COOH): Colourless liquid with a pungent odour. It is a weak acid found in vinegar and used in the production of plastics, solvents, and food preservatives.
5. Carbonic acid (H2CO3): Weak acid that exists only in solution. It is formed when carbon dioxide dissolves in water and plays a role in the carbon dioxide-bicarbonate buffer system in the body.