nitrato

Nitrato, commonly used in Spanish and Italian for nitrate, refers to compounds containing the nitrate group or the nitrate ion NO3−. In chemistry, the nitrate ion is the conjugate base of nitric acid and carries a -1 charge. Nitrates are typically strong oxidizing agents and can form a wide range of inorganic salts and organic esters.

Common nitrates include inorganic salts such as sodium nitrate (NaNO3), potassium nitrate (KNO3), calcium nitrate (Ca(NO3)2), and ammonium nitrate (NH4NO3). Organic nitrates exist as nitrate esters, such as nitroglycerin and ethyl nitrate, which have historical and modern roles in medicine and energetic materials.

Nitrates occur naturally in soils and minerals and are a major component of natural nitrogen cycling. Important natural sources include Chilean saltpeter deposits and other nitrate-bearing minerals. Industrially, nitrates are produced by neutralizing nitric acid with bases, giving various nitrate salts for use in agriculture, industry, and chemistry.

Uses are diverse. The principal application is as nitrogen fertilizers, supplying nitrate nitrogen to crops. Other important uses include food processing (nitrates and nitrites used in curing and preserving meat), pyrotechnics (potassium nitrate in gunpowder and matches), and in organic synthesis (nitrate esters as intermediates and energetic materials). Ammonium nitrate is especially prominent as a fertilizer and as a high-energy explosive under controlled conditions.

Safety and environment: nitrates are oxidizing agents and can pose fire or explosion hazards when contaminated with fuels, particularly ammonium nitrate. In water, excess nitrates from agricultural runoff can contaminate drinking water and contribute to eutrophication. In humans, high nitrate intake can cause methemoglobinemia, especially in infants.