Zinkklorid

Zinkklorid, also known as zinc chloride, is an inorganic compound with the chemical formula ZnCl2. It appears as a white or nearly white crystalline solid and is highly hygroscopic, readily absorbing moisture from the air and often dissolving in the absorbed water (deliquescent). In the solid state the structure involves a network of zinc–chlorine connections; in the gas phase the molecule is typically considered monomeric.

Zinkklorid is highly soluble in water, and its aqueous solutions are strongly acidic due to hydrolysis of Zn2+ and the presence of chloride ions. The compound reacts with water to release hydrogen chloride upon concentrated hydrolysis, and its solutions can corrode metals and tissue.

Production and sources: ZnCl2 is produced commercially by reacting zinc metal with chlorine gas (Zn + Cl2 → ZnCl2) or by reacting zinc oxide with hydrochloric acid (ZnO + 2 HCl → ZnCl2 + H2O). It can also be obtained as a by‑product in some zinc-refining processes.

Uses: It serves as a versatile reagent and catalyst. Applications include fluxing agent for soldering and brazing, a dehydrating agent for drying and drying-type reactions, and a catalyst in various organic syntheses (including polymerizations and acylation reactions). It is used in electroplating baths for zinc plating and in textile and paper processing. Zinc chloride is also employed in wood preservation and as a chemical intermediate in certain industrial processes.

Safety: Zinkklorid is corrosive and irritates skin, eyes, and the respiratory tract. It reacts with moisture and acids to release hydrochloric acid fumes. It should be handled with appropriate protective equipment, stored in tightly closed containers in a dry environment, and kept away from incompatible materials. Environmental hazards include potential toxicity to aquatic life.