This deliquescent salt forms a self-solution when exposed to air. Additionally, lithium chloride can be used as a hygrometer. At 25 ☌ (77 ☏) a saturated solution (45.8%) of the salt will yield an equilibrium relative humidity of 11.30%. Lithium chloride is used as a relative humidity standard in the calibration of hygrometers. Lithium chloride is also used as a flame colorant to produce dark red flames. Also, in biochemical applications, it can be used to precipitate RNA from cellular extracts. In more specialized applications, lithium chloride finds some use in organic synthesis, e.g., as an additive in the Stille reaction. It is used as a desiccant for drying air streams. LiCl is also used as a brazing flux for aluminium in automobile parts. Lithium chloride is mainly used for the production of lithium metal by electrolysis of a LiCl/ KCl melt at 450 ☌ (842 ☏). Anhydrous LiCl is prepared from the hydrate by heating in a stream of hydrogen chloride. Lithium chloride is produced by treatment of lithium carbonate with hydrochloric acid. LiCl + AgNO 3 → AgCl + LiNO 3 Preparation As with any other ionic chloride, solutions of lithium chloride can serve as a source of chloride ion, e.g., forming a precipitate upon treatment with silver nitrate: LiCl also absorbs up to four equivalents of ammonia/mol. The anhydrous salt can be regenerated by heating the hydrates. Mono-, tri-, and pentahydrates are known. The salt forms crystalline hydrates, unlike the other alkali metal chlorides. Chemical properties Color produced when lithium chloride is heated The salt is a typical ionic compound (with certain covalent characteristics), although the small size of the Li + ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 ☌) and its hygroscopic properties. Lithium chloride is a chemical compound with the formula Li Cl.
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