Explain the rules for naming acids and provide ... - SS1 Chemistry Acids, Bases, and Salts Question
Explain the rules for naming acids and provide examples of common acids along with their properties.
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:
- Hydrochloric acid (HCl): Colourless, highly corrosive liquid. It is a strong acid commonly used in laboratory and industrial processes.
- Sulfuric acid (H2SO4): Highly corrosive, oily liquid. It is a strong acid used in various industrial applications, such as manufacturing fertilisers and dyes.
- Nitric acid (HNO3): Colourless to yellow liquid. It is a strong acid involved in the production of fertilisers, explosives, and various organic compounds.
- 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.
- 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.
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