BaCl

BaCl, commonly encountered as barium chloride, is an inorganic salt of barium and chlorine. The standard and widely used compound is barium chloride with the chemical formula BaCl2. The notation BaCl is sometimes seen in informal contexts, but BaCl2 is the correct formula for the ordinary chloride salt of barium.

BaCl2 is a white, odorless solid that is highly soluble in water. It is also highly hygroscopic, tending to absorb moisture from the air and form hydrates such as BaCl2·2H2O. The anhydrous salt has a melting point near 962°C. In solution, Ba2+ ions are accompanied by Cl− ions, and the compound can act as a source of barium in various chemical reactions.

Industrial and laboratory production of BaCl2 typically involves the reaction of a barium compound with hydrochloric acid, for example BaCO3 + 2 HCl → BaCl2 + CO2 + H2O. Another route is the direct chlorination of barium compounds. BaCl2 is also produced as a byproduct in some processes that involve barium species and chloride.

Key uses include serving as a reagent in qualitative inorganic analysis, particularly to detect sulfate ions: Ba2+ precipitates sulfate as BaSO4, a nearly insoluble compound. It is employed as a source of Ba2+ in chemical synthesis and various laboratory procedures. In some applications, BaCl2 is used to prepare other barium salts.

Safety and handling: soluble barium salts, including BaCl2, are toxic and can be hazardous if swallowed or inhaled. They can cause irritation to skin and eyes and may affect the nervous system, heart, and muscles at sufficient exposures. Work with BaCl2 should follow appropriate safety protocols, including use of gloves, eye protection, and proper ventilation, with disposal in accordance with hazardous-wac guidelines.