Introduction to Sulphuric Acid

Sulphuric acid (H2SO4) is a highly corrosive strong mineral acid. Colorless to slightly yellow, it plays a pivotal role in chemical industry as a raw material and solvent.

The ancient method 'oil of vitriol' involved heating green vitriol (iron sulfate). In the 18th century, the lead chamber process dominated industrial production, before the contact process took over.

Modern sulphuric acid production uses the contact process. Key steps include sulfur combustion, SO2 conversion to SO3 on a vanadium(V) oxide catalyst, and SO3 absorption in H2SO4.

Sulphuric acid's high boiling point and affinity for water make it an excellent dehydrating agent. It can char carbohydrates, like sugar, demonstrating its dehydrating power.

Sulphuric acid exhibits different properties at various concentrations. It acts as a strong acid, dehydrating agent, and an oxidizing agent, reacting violently with water and organic materials.

Industrially, it's essential in fertilizer production, petroleum refining, wastewater processing, and chemical synthesis. Over 200 million tons are produced annually, reflecting its industrial significance.

Sulphuric acid is pivotal yet poses environmental risks. Acid rain, resulting from industrial emission of sulphur compounds, damages ecosystems. Regulations aim to reduce these environmental impacts.