Lithium chloride is a chemical compound with the formulaLiCl. 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 °C) and its hygroscopic properties.[5]
The salt forms crystalline hydrates, unlike the other alkali metal chlorides.[6] Mono-, tri-, and pentahydrates are known.[7] The anhydrous salt can be regenerated by heating the hydrates. LiCl also absorbs up to four equivalents of ammonia/mol. 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:
Lithium chloride is mainly used for the production of lithium metal by electrolysis of a LiCl/KCl melt at 450 °C (842 °F). LiCl is also used as a brazing flux for aluminium in automobile parts. It is used as a desiccant for drying air streams.[5] In more specialized applications, lithium chloride finds some use in organic synthesis, e.g., as an additive in the Stille reaction. Also, in biochemical applications, it can be used to precipitate RNA from cellular extracts.[8]
Lithium chloride is also used as a flame colorant to produce dark red flames.
Niche usesedit
Lithium chloride is used as a relative humidity standard in the calibration of hygrometers. At 25 °C (77 °F) a saturated solution (45.8%) of the salt will yield an equilibrium relative humidity of 11.30%. Additionally, lithium chloride can be used as a hygrometer. This deliquescent salt forms a self-solution when exposed to air. The equilibrium LiCl concentration in the resulting solution is directly related to the relative humidity of the air. The percent relative humidity at 25 °C (77 °F) can be estimated, with minimal error in the range 10–30 °C (50–86 °F), from the following first-order equation: RH=107.93-2.11C, where C is solution LiCl concentration, percent by mass.
Lithium salts affect the central nervous system in a variety of ways. While the citrate, carbonate, and orotate salts are currently used to treat bipolar disorder, other lithium salts including the chloride were used in the past. For a short time in the 1940s lithium chloride was manufactured as a salt substitute for people with hypertension, but this was prohibited after the toxic effects of the compound (tremors, fatigue, nausea) were recognized.[13][14][15] It was, however, noted by J. H. Talbott that many symptoms attributed to lithium chloride toxicity may have also been attributable to sodium chloride deficiency, to the diuretics often administered to patients who were given lithium chloride, or to the patients' underlying conditions.[13]
^ChemIDplus - 7447-41-8 - KWGKDLIKAYFUFQ-UHFFFAOYSA-M - Lithium chloride - Similar structures search, synonyms, formulas, resource links, and other chemical information
^Holleman, A. F.; Wiberg, E. Inorganic Chemistry Academic Press: San Diego, 2001. ISBN0-12-352651-5.
^Hönnerscheid Andreas; Nuss Jürgen; Mühle Claus; Jansen Martin (2003). "Die Kristallstrukturen der Monohydrate von Lithiumchlorid und Lithiumbromid". Zeitschrift für anorganische und allgemeine Chemie. 629 (2): 312–316. doi:10.1002/zaac.200390049.
^Cathala, G.; Savouret, J.; Mendez, B.; West, B. L.; Karin, M.; Martial, J. A.; Baxter, J. D. (1983). "A Method for Isolation of Intact, Translationally Active Ribonucleic Acid". DNA. 2 (4): 329–335. doi:10.1089/dna.1983.2.329. PMID 6198133.
^Kamali, Ali Reza; Fray, Derek J. (2014). "Towards large scale preparation of carbon nanostructures in molten LiCl". Carbon. 77: 835–845. doi:10.1016/j.carbon.2014.05.089.
^Kamali, Ali Reza; Fray, Derek J. (2015). "Large-scale preparation of graphene by high temperature insertion of hydrogen into graphite" (PDF). Nanoscale. 7 (26): 11310–11320. doi:10.1039/c5nr01132a. PMID 26053881.
^Kamali, Ali Reza; Fray, Derek J. (2014). "Preparation of lithium niobate particles via reactive molten salt synthesis method". Ceramics International. 40: 1835–1841. doi:10.1016/j.ceramint.2013.07.085.
^Ziegelmann, Bettina; Abele, Elisabeth (January 12, 2018). "Lithium chloride effectively kills the honey bee parasite Varroa destructor by a systemic mode of action". Scientific Reports. 8 (1): 683. Bibcode:2018NatSR...8..683Z. doi:10.1038/s41598-017-19137-5. PMC5766531. PMID 29330449.
^ abTalbott J. H. (1950). "Use of lithium salts as a substitute for sodium chloride". Arch Intern Med. 85 (1): 1–10. doi:10.1001/archinte.1950.00230070023001. PMID 15398859.
^L. J. Stone; M. luton; J. Gilroy (1949). "Lithium Chloride as a Substitute for Sodium Chloride in the Diet". Journal of the American Medical Association. 139 (11): 688–692. doi:10.1001/jama.1949.02900280004002. PMID 18128981.
^. Time. 28 February 1949. Archived from the original on March 2, 2007.
Handbook of Chemistry and Physics, 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
N. N. Greenwood, A. Earnshaw, Chemistry of the Elements, 2nd ed., Butterworth-Heinemann, Oxford, UK, 1997.
R. Vatassery, titration analysis of LiCl, sat'd in Ethanol by AgNO3 to precipitate AgCl(s). EP of this titration gives %Cl by mass.
H. Nechamkin, The Chemistry of the Elements, McGraw-Hill, New York, 1968.
External linksedit
Radiochemical measurements of activity coefficients, from Betts & MacKenzie, Can. J. Chem.
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February 15, 2024
lithium, chloride, chemical, compound, with, formula, licl, salt, typical, ionic, compound, with, certain, covalent, characteristics, although, small, size, gives, rise, properties, seen, other, alkali, metal, chlorides, such, extraordinary, solubility, polar,. Lithium chloride is a chemical compound with the formula LiCl 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 C and its hygroscopic properties 5 Lithium chloride Li Cl NamesPreferred IUPAC name Lithium chlorideSystematic IUPAC name Lithium 1 chlorideIdentifiersCAS Number 7447 41 8 Y3D model JSmol Interactive imageChEBI CHEBI 48607 YChEMBL ChEMBL69710 NChemSpider 22449 YECHA InfoCard 100 028 375EC Number 231 212 3MeSH Lithium chloridePubChem CID 433294RTECS number OJ5950000UNII G4962QA067 YUN number 2056CompTox Dashboard EPA DTXSID2025509InChI InChI 1S ClH Li h1H q 1 p 1 NKey KWGKDLIKAYFUFQ UHFFFAOYSA M NInChI 1S ClH Li h1H q 1 p 1Key KWGKDLIKAYFUFQ UHFFFAOYSA MInChI 1 ClH Li h1H q 1 p 1Key KWGKDLIKAYFUFQ REWHXWOFABSMILES Li Cl PropertiesChemical formula LiClMolar mass 42 39 g mol 1Appearance white solid hygroscopic sharpDensity 2 068 g cm3Melting point 605 614 C 1 121 1 137 F 878 887 K Boiling point 1 382 C 2 520 F 1 655 K Solubility in water 68 29 g 100 mL 0 C 74 48 g 100 mL 10 C 84 25 g 100 mL 25 C 88 7 g 100 mL 40 C 123 44 g 100 mL 100 C 1 Solubility soluble in hydrazine methylformamide butanol selenium IV oxychloride 1 propanol 1 Solubility in methanol 45 2 g 100 g 0 C 43 8 g 100 g 20 C 42 36 g 100 g 25 C 2 44 6 g 100 g 60 C 1 Solubility in ethanol 14 42 g 100 g 0 C 24 28 g 100 g 20 C 25 1 g 100 g 30 C 23 46 g 100 g 60 C 2 Solubility in formic acid 26 6 g 100 g 18 C 27 5 g 100 g 25 C 1 Solubility in acetone 1 2 g 100 g 20 C 0 83 g 100 g 25 C 0 61 g 100 g 50 C 1 Solubility in liquid ammonia 0 54 g 100 g 34 C 1 3 02 g 100 g 25 C Vapor pressure 1 torr 785 C 10 torr 934 C 100 torr 1130 C 1 Magnetic susceptibility x 24 3 10 6 cm3 molRefractive index nD 1 662 24 C Viscosity 0 87 cP 807 C 1 StructureCoordination geometry OctahedralMolecular shape Linear gas Dipole moment 7 13 D gas ThermochemistryHeat capacity C 48 03 J mol K 1 Std molarentropy S 298 59 31 J mol K 1 Std enthalpy offormation DfH 298 408 27 kJ mol 1 Gibbs free energy DfG 384 kJ mol 1 PharmacologyATC code V04CX11 WHO HazardsGHS labelling Pictograms 3 Signal word WarningHazard statements H302 H315 H319 H335 3 Precautionary statements P261 P305 P351 P338 3 NFPA 704 fire diamond 200Flash point Non flammableLethal dose or concentration LD LC LD50 median dose 526 mg kg oral rat 4 Safety data sheet SDS ICSC 0711Related compoundsOther anions Lithium fluorideLithium bromideLithium iodideLithium astatideOther cations Sodium chloridePotassium chlorideRubidium chlorideCaesium chlorideFrancium chlorideSupplementary data pageLithium chloride data page Except where otherwise noted data are given for materials in their standard state at 25 C 77 F 100 kPa N verify what is Y N Infobox references Contents 1 Chemical properties 2 Preparation 3 Uses 3 1 Commercial applications 3 2 Niche uses 4 Precautions 5 See also 6 References 7 External linksChemical properties edit nbsp Color produced when lithium chloride is heatedThe salt forms crystalline hydrates unlike the other alkali metal chlorides 6 Mono tri and pentahydrates are known 7 The anhydrous salt can be regenerated by heating the hydrates LiCl also absorbs up to four equivalents of ammonia mol 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 AgNO3 AgCl LiNO3Preparation editLithium chloride is produced by treatment of lithium carbonate with hydrochloric acid 5 Anhydrous LiCl is prepared from the hydrate by heating in a stream of hydrogen chloride Uses editCommercial applications edit Lithium chloride is mainly used for the production of lithium metal by electrolysis of a LiCl KCl melt at 450 C 842 F LiCl is also used as a brazing flux for aluminium in automobile parts It is used as a desiccant for drying air streams 5 In more specialized applications lithium chloride finds some use in organic synthesis e g as an additive in the Stille reaction Also in biochemical applications it can be used to precipitate RNA from cellular extracts 8 Lithium chloride is also used as a flame colorant to produce dark red flames Niche uses edit Lithium chloride is used as a relative humidity standard in the calibration of hygrometers At 25 C 77 F a saturated solution 45 8 of the salt will yield an equilibrium relative humidity of 11 30 Additionally lithium chloride can be used as a hygrometer This deliquescent salt forms a self solution when exposed to air The equilibrium LiCl concentration in the resulting solution is directly related to the relative humidity of the air The percent relative humidity at 25 C 77 F can be estimated with minimal error in the range 10 30 C 50 86 F from the following first order equation RH 107 93 2 11C where C is solution LiCl concentration percent by mass Molten LiCl is used for the preparation of carbon nanotubes 9 graphene 10 and lithium niobate 11 Lithium chloride has been shown to have strong acaricidal properties being effective against Varroa destructor in populations of honey bees 12 Lithium chloride is used as an aversive agent in lab animals to study conditioned place preference and aversion Precautions editLithium salts affect the central nervous system in a variety of ways While the citrate carbonate and orotate salts are currently used to treat bipolar disorder other lithium salts including the chloride were used in the past For a short time in the 1940s lithium chloride was manufactured as a salt substitute for people with hypertension but this was prohibited after the toxic effects of the compound tremors fatigue nausea were recognized 13 14 15 It was however noted by J H Talbott that many symptoms attributed to lithium chloride toxicity may have also been attributable to sodium chloride deficiency to the diuretics often administered to patients who were given lithium chloride or to the patients underlying conditions 13 See also editLithium chloride data page Solubility tableReferences edit a b c d e f g h i j k l lithium chloride a b Seidell Atherton Linke William F 1952 Solubilities of Inorganic and Organic Compounds Van Nostrand Retrieved 2014 06 02 a b c Sigma Aldrich Co Lithium chloride Retrieved on 2014 05 09 ChemIDplus 7447 41 8 KWGKDLIKAYFUFQ UHFFFAOYSA M Lithium chloride Similar structures search synonyms formulas resource links and other chemical information a b c Wietelmann Ulrich Bauer Richard J 2005 Lithium and Lithium Compounds Ullmann s Encyclopedia of Industrial Chemistry Weinheim Wiley VCH doi 10 1002 14356007 a15 393 ISBN 978 3527306732 Holleman A F Wiberg E Inorganic Chemistry Academic Press San Diego 2001 ISBN 0 12 352651 5 Honnerscheid Andreas Nuss Jurgen Muhle Claus Jansen Martin 2003 Die Kristallstrukturen der Monohydrate von Lithiumchlorid und Lithiumbromid Zeitschrift fur anorganische und allgemeine Chemie 629 2 312 316 doi 10 1002 zaac 200390049 Cathala G Savouret J Mendez B West B L Karin M Martial J A Baxter J D 1983 A Method for Isolation of Intact Translationally Active Ribonucleic Acid DNA 2 4 329 335 doi 10 1089 dna 1983 2 329 PMID 6198133 Kamali Ali Reza Fray Derek J 2014 Towards large scale preparation of carbon nanostructures in molten LiCl Carbon 77 835 845 doi 10 1016 j carbon 2014 05 089 Kamali Ali Reza Fray Derek J 2015 Large scale preparation of graphene by high temperature insertion of hydrogen into graphite PDF Nanoscale 7 26 11310 11320 doi 10 1039 c5nr01132a PMID 26053881 Kamali Ali Reza Fray Derek J 2014 Preparation of lithium niobate particles via reactive molten salt synthesis method Ceramics International 40 1835 1841 doi 10 1016 j ceramint 2013 07 085 Ziegelmann Bettina Abele Elisabeth January 12 2018 Lithium chloride effectively kills the honey bee parasite Varroa destructor by a systemic mode of action Scientific Reports 8 1 683 Bibcode 2018NatSR 8 683Z doi 10 1038 s41598 017 19137 5 PMC 5766531 PMID 29330449 a b Talbott J H 1950 Use of lithium salts as a substitute for sodium chloride Arch Intern Med 85 1 1 10 doi 10 1001 archinte 1950 00230070023001 PMID 15398859 L J Stone M luton J Gilroy 1949 Lithium Chloride as a Substitute for Sodium Chloride in the Diet Journal of the American Medical Association 139 11 688 692 doi 10 1001 jama 1949 02900280004002 PMID 18128981 Case of trie Substitute Salt Time 28 February 1949 Archived from the original on March 2 2007 Handbook of Chemistry and Physics 71st edition CRC Press Ann Arbor Michigan 1990 N N Greenwood A Earnshaw Chemistry of the Elements 2nd ed Butterworth Heinemann Oxford UK 1997 R Vatassery titration analysis of LiCl sat d in Ethanol by AgNO3 to precipitate AgCl s EP of this titration gives Cl by mass H Nechamkin The Chemistry of the Elements McGraw Hill New York 1968 External links editRadiochemical measurements of activity coefficients from Betts amp MacKenzie Can J Chem nbsp Wikimedia Commons has media related to Lithium chloride Retrieved from https en wikipedia org w index php title Lithium chloride amp oldid 1196346965, wikipedia, wiki, book, books, library,
