Lithium Chloride Formula

Lithium Chloride Formula

This article discusses the Lithium Chloride Formula, also known as the  Lithium Chloride Formula or lithium chloride. Lithium chloride is formed from lithium and chlorine atoms. In 1940, the compound was briefly created as a substitute for salt. Because of its toxicity, it was soon banned. The molecular or chemical formula for lithium chloride is LiCl.

Lithium Chloride Formula is a representative ionic compound, a lithium salt. The small size of the lithium ion (Li+) gives it properties not found in other alkali metal chlorides. It is also known by the names chlorolithium or lithium chloride. For a short time in the 1940s, they created it as a compound to replace table salt (sodium chloride, NaCl).

Lithium Chloride Formula Structure

The chemical Lithium Chloride Formula  is LiCl. The molar mass is 42.394 g/mol. At the molecular level, positively charged lithium ions (Li+) react with negatively charged chloride ions (Cl) to form lithium chloride (LiCl).

Preparation of lithium chloride

Lithium chloride can be produced by treating lithium carbonate with hydrochloric acid. It can also be produced by the highly exothermic reaction of lithium metal with ethereal chlorine or anhydrous hydrogen chloride gas. Additionally, anhydrous LiCl can be produced from hydration and heating with a stream of hydrogen chloride. For more information about the Lithium Chloride Formula students can visit Extramarks.

Physical properties of lithium chloride

It appears as an odorless, white, crystalline, hygroscopic solid and has a density of 2.068 g/cm3, a boiling point of 1382 °C, and a melting point of 605–614 °C.

Soluble in water, methanol, ethanol, isopropanol, butanol, formic acid, n-methylformamide, hydrazine and THF. In addition, it is slightly soluble in acetone and ammonia, and completely insoluble in dichloromethane. Students can visit the Extramarks website for  Lithium Chloride Formula

Chemical properties of lithium chloride

Like other metal chlorides, its salts form crystalline hydrates. Furthermore, its monohydrate, trihydrate, and pentahydrate are known. The anhydrous salt can be regenerated by heating the hydrate. In addition, it readily absorbs up to 4 equivalents of ammonia per mole. However, with another ionic chloride, the lithium chloride solution acts as a source of chloride ions. Students can learn the Lithium Chloride Formula from Extramarks website.

Uses of lithium chloride

  • It is mainly used for the production of lithium metal by electrolysis of LiCl/KCl melting at 450 °C. It is also used in industry as a soldering flux for aluminium automotive parts. We also use it as a desiccant to dry the air stream.
  • There are several specialised applications in organic synthesis, including: B. Additives in the Stille reaction. The most notable is the biochemical application used to precipitate RNA from cell extracts.
  • Another use of Lithium Chloride is as a flame dye for creating dark red flames. When calibrating a hygrometer, they use it as a relative humidity standard.
  • Can be used as a hygrometer. It also forms a deliquescent, self-dissolving salt when exposed to air. Furthermore, the equilibrium LiCl concentration of the resulting solution can be directly related to the relative humidity of the air.
  • Industry uses its molten form to produce carbon nanotubes, lithium niobate, and graphene. In addition, it exhibits very strong acaricidal properties.

Safety and health hazards of lithium chloride

Its salts affect the central nervous system in different ways. Citrate, orotate, and carbonate, on the other hand, are now used to treat bipolar disorder, although other lithium salts, including chloride, were used in the past. manufactured it as a substitute for salt, but it was later banned after its toxicity became known. Students must visit the website of Extramarks to get information about the Lithium Chloride Formula

Solved Example for You

Q: How does lithium chloride work as a source of chloride ions?

Solution: Acts as a source of chloride ions by forming a precipitate when treated with silver nitrate.


Learners can visit Extramarks’ website for Lithium Chloride Formula and other related formulas.

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