Q1
How is nitric acid prepared in the lab?
AHeating a nitrate salt with conc. H2SO4
BHeating a nitrate salt alone
CMixing nitrogen with water
DHeating water with salt
ICSEClass 10 (ICSE)ChemistryCh 10 · Topic 1
Study of Compounds - Nitric Acid
Nitric acid (HNO3) is prepared in the laboratory and industrially, showing strong oxidising properties important in various chemical process
Core concept
Nitric acid is prepared in the lab by heating potassium/sodium nitrate with concentrated sulphuric acid, and industrially by the Ostwald process.
How it works
Nitric acid is a strong oxidising agent, reacting differently with metals compared to other acids, often not liberating hydrogen gas.
Why it matters
Concentrated nitric acid can passivate certain metals like iron and aluminium, forming a protective oxide layer that prevents further reaction.
Key detail
Nitric acid is widely used in manufacturing fertilisers (ammonium nitrate), explosives, and various other industrial chemicals.
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Quick notes
• Lab prep: heating nitrate salt with conc. H2SO4.
• Industrial prep: Ostwald process.
• Nitric acid is a strong oxidising agent.
• It reacts differently with metals than typical acids.
• It often doesn't liberate hydrogen gas.
• Concentrated HNO3 passivates iron and aluminium.
• This forms a protective oxide layer.
• Uses: fertilisers, explosives, industrial chemicals.