Silvernitrat

Silvernitrat, commonly known as silver nitrate, is an inorganic compound with the chemical formula AgNO3. It consists of silver cations and nitrate anions and forms white, crystalline solids that are highly soluble in water. It is photosensitive, darkening upon exposure to light due to reduction of silver.

Production and structure: In industry, silver nitrate is typically produced by dissolving metallic silver in nitric acid to form a solution of AgNO3, which is then concentrated and crystallized. The compound serves as a convenient source of the silver ion (Ag+) for various chemical processes. Its molar mass is about 169.87 g/mol.

Uses: Silver nitrate has broad historical and modern applications. It was fundamental in early photography, where silver halide emulsions were formed from AgNO3. In medicine and pathology, dilute solutions act as antiseptics and are used for cauterization; silver nitrate sticks are used to remove granulation tissue and certain growths. In the laboratory, it is a classic reagent for qualitative and quantitative analyses and is the precursor to Tollens’ reagent, which is prepared by reacting AgNO3 with ammonia to form [Ag(NH3)2]+ for testing aldehydes. It is also used in various chemical syntheses and as an etchant in some metal-processing applications.

Safety and handling: Silver nitrate is corrosive and can cause severe burns to skin and eyes. It can stain tissues and skin a yellow-brown color due to silver deposition. It should be handled with gloves and eye protection, stored away from light, and kept in containers that prevent contact with reducing agents. Disposal requires appropriate waste handling due to environmental toxicity, particularly to aquatic life.

See also: Tollens’ reagent, silver paradox, photography chemistry.