|Uses: Hydrogen chloride has many uses among which are the following: as a chemical inter-mediate; in the hydrochlorination of rubber; as a babbitting flux; in the production of vinyl and alkyl chlorides; in the separation of cotton from wool; in the delinting of cotton. Electronic grade is used for etching semiconductor crystals.
Hydrogen Chloride (HCl), a compound of the elements hydrogen and chlorine, a gas at room temperature and pressure. A solution of the gas in water is called hydrochloric acid.
Hydrogen chloride may be formed by the direct combination of chlorine (Cl2) gas and hydrogen (H2) gas; the reaction is rapid at temperatures above 250 °C (482° F). The reaction, represented by the equation H2 + Cl2 2HCl, is accompanied by evolution of heat and appears to be accelerated by moisture.
Hydrogen chloride is commonly prepared both on a laboratory and on an industrial scale by the reaction of a
chloride, generally that of sodium (NaCl), with sulfuric acid (H2SO4). It is also produced by the reaction of some chlorides (e.g., phosphorus trichloride, PCl3, or thionyl chloride, SOCl2) with water and as a by-product of the chlorination of many organic substances (e.g., methane, benzene).
Hydrochloric acid is prepared by dissolving gaseous hydrogen chloride in water. Because of the corrosive nature of the acid, ceramic, glass, or sometimes tantalum apparatus is commonly used. Hydrochloric acid is usually marketed as a solution containing 28-35 percent by weight hydrogen chloride, commonly known as concentrated hydrochloric acid. Anhydrous liquid hydrogen chloride is available, but because heavy and
expensive containers are required to store it, the use of hydrogen chloride in this form is limited.
Hydrogen chloride is a colourless gas of strong odour; it condenses at -85° C (-121° F) and freezes at -114° C (-173° F). The gas is very soluble in water: at 20 °C (68 °F) water will dissolve 477 times its own volume of hydrogen chloride. Because of its great solubility, the gas fumes in moist air. A water solution containing 20.24 percent by weight hydrogen chloride boils at 110 °C (230° F) without change in composition (azeotropic mixture). In aqueous solution the compound is extensively dissociated into a hydronium ion (H3O+) and
chloride ion (Cl-); in dilute solutions the dissociation is essentially complete. Thus, hydrochloric acid is a strong acid.
Gaseous hydrogen chloride reacts with active metals and their oxides, hydroxides, and carbonates to produce chlorides. These reactions occur readily only in the presence of moisture. Completely dry hydrogen chloride is very unreactive. The reactions of hydrochloric acid are those of typical strong acids, such as: reactions with metals in which hydrogen gas is displaced, reactions with basic oxides and hydroxides that are neutralized with the formation of a chloride and water, and reactions with salts of weak acids in which the weak acid is displaced. Hydrochloric acid also enters into chemical reactions characteristic of the chloride ion, such as reactions with various inorganic and organic compounds in which hydrochloric acid is used as a chlorinating agent and reactions with metals and their oxides in which complex chloride-containing ions are formed (e.g., with platinum, PtCl62-, with copper, CuCl42-). The latter type of reaction accounts for the ease of solution of certain metals and metallic compounds in hydrochloric acid although they are slowly dissolved in other acids of equal strength (e.g., sulfuric or nitric acid). For this reason hydrochloric acid is used extensively in the industrial processing of metals and in the concentration of some ores.
Hydrochloric acid is present in the digestive juices of the human stomach. Excessive secretion of the acid causes gastric ulcers; a marked deficiency of it impairs the digestive process and is sometimes the primary cause of deficiency anemias. Exposure to 0.1 percent by volume hydrogen chloride gas in the atmosphere may cause death in a few minutes. Concentrated hydrochloric acid causes burns and inflammation of the skin.