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When dissolved in water, chlorine converts to an equilibrium mixture of chlorine, hypochlorous acid (HOCl), and hydrochloric acid (HCl): Cl 2 + H 2 O ⇌ HOCl + HCl. In acidic solution, the major species are Cl 2 and HOCl, whereas in alkaline solution, effectively only ClO − (hypochlorite ion) is present.
As the reaction is exothermic, the installation is called an HCl oven or HCl burner. The resulting hydrogen chloride gas is absorbed in deionized water, resulting in chemically pure hydrochloric acid. This reaction can give a very pure product, e.g. for use in the food industry. The reaction can also be triggered by blue light. [16]
Chlorine reacts with water in the mucosa of the lungs to form hydrochloric acid, destructive to living tissue and potentially lethal. Human respiratory systems can be protected from chlorine gas by gas masks with activated charcoal or other filters, which makes chlorine gas much less lethal than other chemical weapons.
The hydrochloric acid provides a ready supply of chloride ions (Cl −), which react with the gold ions to produce tetrachloroaurate(III) anions ([AuCl 4] −), also in solution. The reaction with hydrochloric acid is an equilibrium reaction that favors formation of tetrachloroaurate(III) anions.
Hydrochloric acid is a strong inorganic acid that is used in many industrial processes such as refining metal. The application often determines the required product quality. [25] Hydrogen chloride, not hydrochloric acid, is used more widely in industrial organic chemistry, e.g. for vinyl chloride and dichloroethane. [8]
Out of the four stable halogens, only fluorine and chlorine have reduction potentials higher than that of oxygen, allowing them to form hydrofluoric acid and hydrochloric acid directly through reaction with water. [17] The reaction of fluorine with water is especially hazardous, as an addition of fluorine gas to cold water will produce ...
Chlorine has maximum solubility of ca. 7.1 g Cl 2 per kg of water at ambient temperature (21 °C). [24] Dissolved chlorine reacts to form hydrochloric acid (HCl) and hypochlorous acid, a solution that can be used as a disinfectant or bleach: Cl 2 (g) + H 2 O(l) → HCl(aq) + HClO(aq)
Hydrolysis is prevented in the presence of hydrochloric acid, typically of the same or greater molarity as the stannous chloride. Solutions of SnCl 2 are also unstable towards oxidation by the air: 6 SnCl 2 + O 2 + 2 H 2 O → 2 SnCl 4 + 4 Sn(OH)Cl. Oxidation can be prevented by storing the solution over lumps of tin metal. [4]