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Lithium chloride: Difference between revisions

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{{short description|Chemical compound}}
{{Chembox {{Chembox
| Verifiedfields = changed
| verifiedrevid = 395260252
| Watchedfields = changed
| ImageFile1 = Lithium chloride.jpg
| verifiedrevid = 410218986
| ImageSize1 = 150px
| ImageName1 = Sample of lithium chloride in a watch glass | ImageFile1 = Lithium chloride.jpg
| ImageName1 = Sample of lithium chloride in a watch glass
| ImageFile2 = Lithium-chloride-3D-ionic.png | ImageFile = Lithium-chloride-3D-ionic.png
| ImageSize2 = 150px | ImageSize = 150px
| ImageFile2 = File:NaCl polyhedra.svg
| ImageName2 = Unit cell model of lithium chloride
| ImageCaption2 = <span style="color:#C0C0C0; background-color:#C0C0C0;">__</span> ]<sup>+</sup>&nbsp;&nbsp;&nbsp;&nbsp;&nbsp;<span style="color:#00FF00;background-color:#00FF00;">__</span> ]<sup>−</sup>
| PIN = Lithium chloride
| SystematicName = Lithium(1+) chloride | ImageName = Unit cell model of lithium chloride
| PIN = Lithium chloride
| Section1 = {{Chembox Identifiers
| SystematicName = Lithium(1+) chloride
| InChI1 = 1/ClH.Li/h1H;/q;+1/p-1
|Section1={{Chembox Identifiers
| InChI1 = 1/ClH.Li/h1H;/q;+1/p-1
| InChIKey1 = KWGKDLIKAYFUFQ-REWHXWOFAB | InChIKey1 = KWGKDLIKAYFUFQ-REWHXWOFAB
| CASNo = 7447-41-8 | CASNo = 7447-41-8
| CASNo_Ref = {{cascite|correct|CAS}} | CASNo_Ref = {{cascite|correct|CAS}}
| ChEMBL_Ref = {{ebicite|changed|EBI}}
| PubChem = 4933294
| ChEMBL = 69710
| PubChem_Ref = {{Pubchemcite}}
| ChemSpiderID = 22449 | PubChem = 433294
| ChemSpiderID = 22449
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}= {{Chemspidercite}}
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| UNII = G4962QA067
| UNII_Ref = {{fdacite|correct|FDA}} | UNII = G4962QA067
| UNII_Ref = {{fdacite|correct|FDA}}
| EINECS number = 231-212-3 | EINECS = 231-212-3
| UNNumber = 2056 | UNNumber = 2056
| MeSHName = Lithium+chloride | MeSHName = Lithium+chloride
| ChEBI_Ref = {{ebicite|correct|EBI}}
| ChEBI = 48607
| RTECS = OJ5950000 | ChEBI = 48607
| SMILES = . | RTECS = OJ5950000
| StdInChI_Ref = {{stdinchicite|changed|chemspider}}
| InChI = 1S/ClH.Li/h1H;/q;+1/p-1
| StdInChI = 1S/ClH.Li/h1H;/q;+1/p-1
| InChIKey = KWGKDLIKAYFUFQ-UHFFFAOYSA-M}}
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
| Section2 = {{Chembox Properties
| StdInChIKey = KWGKDLIKAYFUFQ-UHFFFAOYSA-M
| SMILES = .
| InChI = 1S/ClH.Li/h1H;/q;+1/p-1
| InChIKey = KWGKDLIKAYFUFQ-UHFFFAOYSA-M}}
|Section2={{Chembox Properties
| Formula = LiCl | Formula = LiCl
| Li=1|Cl=1
| MolarMass = 42.394(4) g/mol
| Appearance = white solid <br> ] <ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, ISBN 0070494398</ref> | Appearance = white solid <br> ], sharp
| Density = 2.068 g/cm<sup>3</sup> (anhydrous) | Density = 2.068 g/cm<sup>3</sup>
| Solubility = 68.29 g/100 mL (0&nbsp;°C)<br> 74.48 g/100 mL (10&nbsp;°C)<br> 84.25 g/100 mL (25&nbsp;°C)<br> 88.7 g/100 mL (40&nbsp;°C)<br> 123.44 g/100 mL (100&nbsp;°C)<ref name=chemister />
| Solubility = 83.2 g/100 mL (20 °C) (anhydrous)
| SolubleOther = highly soluble in ], ] <br> 4.1 g/100 mL (]) | SolubleOther = soluble in ], ], ], ], ]<ref name=chemister />
| MeltingPt = 605 °C | Solvent1 = methanol
| Solubility1 = 45.2 g/100 g (0&nbsp;°C)<br> 43.8 g/100 g (20&nbsp;°C)<br> 42.36 g/100 g (25&nbsp;°C)<ref name=sioc>{{cite book|last1 = Seidell|first1 = Atherton|last2 = Linke|first2 = William F.|year = 1952|title = Solubilities of Inorganic and Organic Compounds|publisher = Van Nostrand|url =https://books.google.com/books?id=k2e5AAAAIAAJ|access-date = 2014-06-02}}</ref><br> 44.6 g/100 g (60&nbsp;°C)<ref name=chemister></ref>
| BoilingPt = 1382 °C (decomp)
| RefractIndex = 1.662 | Solvent2 = ethanol
| Solubility2 = 14.42 g/100 g (0&nbsp;°C)<br> 24.28 g/100 g (20&nbsp;°C)<br> 25.1 g/100 g (30&nbsp;°C)<br> 23.46 g/100 g (60&nbsp;°C)<ref name=sioc />
| Solvent3 = formic acid
| Solubility3 = 26.6 g/100 g (18&nbsp;°C)<br> 27.5 g/100 g (25&nbsp;°C)<ref name=chemister />
| Solvent4 = acetone
| Solubility4 = 1.2 g/100 g (20&nbsp;°C)<br> 0.83 g/100 g (25&nbsp;°C)<br> 0.61 g/100 g (50&nbsp;°C)<ref name=chemister />
| Solvent5 = liquid ammonia
| Solubility5 = 0.54 g/100 g (-34&nbsp;°C)<ref name=chemister /><br> 3.02 g/100 g (25&nbsp;°C)
| MeltingPtC = 605-614
| BoilingPtC = 1382
| RefractIndex = 1.662 (24&nbsp;°C)
| VaporPressure = 1 torr (785&nbsp;°C)<br> 10 torr (934&nbsp;°C)<br> 100 torr (1130&nbsp;°C)<ref name=chemister />
| Viscosity = 0.87 cP (807&nbsp;°C)<ref name=chemister />
| MagSus = &minus;24.3·10<sup>−6</sup> cm<sup>3</sup>/mol
}} }}
| Section3 = {{Chembox Structure |Section3={{Chembox Structure
| MolShape = Linear (gas) | MolShape = Linear (gas)
| Coordination = Octahedral | Coordination = Octahedral
| Dipole = 7.13 D (gas) | Dipole = 7.13 D (gas)
}} }}
| Section4 = {{Chembox Thermochemistry |Section4={{Chembox Thermochemistry
| DeltaHf = -9.638 kJ/g | DeltaHf = -408.27 kJ/mol<ref name=chemister />
| DeltaGf = -384 kJ/mol<ref name=chemister />
| DeltaHc = | DeltaHc =
| Entropy = | Entropy = 59.31 J/mol·K<ref name=chemister />
| HeatCapacity = 1.132 J/(g K) | HeatCapacity = 48.03 J/mol·K<ref name=chemister />
}} }}
| Section7 = {{Chembox Hazards | Section6 = {{Chembox Pharmacology
| Pharmacology_ref =
| ExternalMSDS =
| ATCCode_prefix = V04
| EUIndex = Not listed
| ATCCode_suffix = CX11
| ATC_Supplemental =
| ATCvet =
| Licence_EU =
| INN =
| INN_EMA =
| Licence_US =
| Legal_status =
| Legal_AU =
| Legal_AU_comment =
| Legal_CA =
| Legal_CA_comment =
| Legal_NZ =
| Legal_NZ_comment =
| Legal_UK =
| Legal_UK_comment =
| Legal_US =
| Legal_US_comment =
| Legal_EU =
| Legal_EU_comment =
| Legal_UN =
| Legal_UN_comment =
| Pregnancy_category =
| Pregnancy_AU =
| Pregnancy_AU_comment =
| Dependence_liability =
| AdminRoutes =
| Bioavail =
| ProteinBound =
| Metabolism =
| Metabolites =
| OnsetOfAction =
| HalfLife =
| DurationOfAction =
| Excretion =
}}
|Section7={{Chembox Hazards
| ExternalSDS =
| GHSPictograms = {{GHS07}}<ref name="sigma">{{Sigma-Aldrich|id=203637|name=Lithium chloride|accessdate=2014-05-09}}</ref>
| GHSSignalWord = Warning
| HPhrases = {{H-phrases|302|315|319|335}}<ref name="sigma" />
| PPhrases = {{P-phrases|261|305+351+338}}<ref name="sigma" />
| NFPA-H = 2 | NFPA-H = 2
| NFPA-R = 0 | NFPA-R = 0
| NFPA-F = 0 | NFPA-F = 0
| RPhrases =
| SPhrases =
| FlashPt = Non-flammable | FlashPt = Non-flammable
| LD50 = 526 mg/kg (oral, rat)<ref></ref>
| LD<sub>5O</sub> = 526mg/kg rat, oral<ref></ref>
}} }}
| Section8 = {{Chembox Related |Section8={{Chembox Related
| OtherAnions = ]<br/>]<br/>] | OtherAnions = ]<br/>]<br/>]<br/>]
| OtherCations = ]<br/>]<br/>]<br/>] | OtherCations = ]<br/>]<br/>]<br/>]<br/>]
}} }}
}} }}


'''Lithium chloride''' is a ] with the ] ]]. The ] is a typical ], although the small size of the Li<sup>+</sup> ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar ]s (83g/100 mL of water at 20 °C) and its ] properties.<ref name=Ullmann>Ulrich Wietelmann, Richard J. Bauer "Lithium and Lithium Compounds" in Ullmann's Encyclopedia of Industrial Chemistry 2005, Wiley-VCH: Weinheim.</ref> '''Lithium chloride''' is a ] with the ] ]]. The ] is a typical ] (with certain covalent characteristics), although the small size of the Li<sup>+</sup> ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar ]s (83.05&nbsp;g/100&nbsp;mL of water at 20&nbsp;°C) and its ] properties.<ref name=Ullmann/>


==Chemical properties== ==Chemical properties==
]
The salt forms crystalline ], unlike the other alkali metal chlorides.<ref>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref> Mono-, tri-, and pentahydrates are known.<ref>Andreas Hönnerscheid, Jürgen Nuss, Claus Mühle, Martin Jansen "Die Kristallstrukturen der Monohydrate von Lithiumchlorid und Lithiumbromid" Zeitschrift für anorganische und allgemeine Chemie, 2003, volume 629, p. 312-316.{{DOI| 10.1002/zaac.200390049}}</ref> It also absorbs up to four equivalents of ]. As with any other ionic chlorides, solutions of lithium chloride can serve as a source of ] ion, e.g. forming a precipitate upon treatment with ]:
The salt forms crystalline ], unlike the other alkali metal chlorides.<ref>Holleman, A. F.; Wiberg, E. ''Inorganic Chemistry'' Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}.</ref> Mono-, tri-, and pentahydrates are known.<ref>{{cite journal |author1=Hönnerscheid Andreas |author2=Nuss Jürgen |author3=Mühle Claus |author4=Jansen Martin | year = 2003 | title = Die Kristallstrukturen der Monohydrate von Lithiumchlorid und Lithiumbromid | journal = Zeitschrift für anorganische und allgemeine Chemie | volume = 629 | issue = 2| pages = 312–316 | doi = 10.1002/zaac.200390049 }}</ref> The anhydrous salt can be regenerated by heating the hydrates. LiCl also absorbs up to four equivalents of ]/mol. As with any other ionic chloride, solutions of lithium chloride can serve as a source of ] ion, e.g., forming a precipitate upon treatment with ]:
: LiCl + AgNO<sub>3</sub> → AgCl + LiNO<sub>3</sub> : LiCl + AgNO<sub>3</sub> → AgCl + LiNO<sub>3</sub>


==Preparation== ==Preparation==
Lithium chloride is produced by treatment of ] with ]. It can in principle also be generated by the highly ] of lithium metal with either ] or anhydrous ] gas. Anhydrous LiCl is prepared from the hydrate by heating with a stream of ]. Lithium chloride is produced by treatment of ] with ].<ref name=Ullmann>{{Ullmann |doi=10.1002/14356007.a15_393|title=Lithium and Lithium Compounds|first1=Ulrich |last1=Wietelmann|first2=Richard J.|last2=Bauer|year=2005}}</ref> Anhydrous LiCl is prepared from the hydrate by heating in a stream of ].


==Uses== ==Uses==
===Commercial applications===
Lithium chloride is mainly used for the production of ] metal by ] of a LiCl/] melt at 600 °]. LiCl is also used as a brazing ] for ] in ] parts. It is used as a ] for drying air streams.<ref name=Ullmann/> In more specialized applications, lithium chloride finds some use in ], e.g. as an additive in the ]. Also, in biochemical applications, it can be used to precipitate ] from cellular extracts.<ref>{{cite journal
Lithium chloride is mainly used for the production of ] metal by ] of a LiCl/] melt at {{convert|450|C|F}}. LiCl is also used as a brazing ] for ] in ] parts. It is used as a ] for drying air streams.<ref name=Ullmann/> In more specialized applications, lithium chloride finds some use in ], e.g., as an additive in the ]. Also, in biochemical applications, it can be used to precipitate ] from cellular extracts.<ref>{{cite journal
| doi= 10.1089/dna.1983.2.329 | doi= 10.1089/dna.1983.2.329
| author= Cathala, G., Savouret, J., Mendez, B., West, B.L., Karin, M., Martial, J.A., and Baxter, J.D. | author1= Cathala, G. | author2=Savouret, J. | author3=Mendez, B. | author4=West, B. L. | author5=Karin, M. | author6=Martial, J. A. | author7=Baxter, J. D.
| title = A Method for Isolation of Intact, Translationally Active Ribonucleic Acid | title = A Method for Isolation of Intact, Translationally Active Ribonucleic Acid
| journal = DNA | journal = DNA
Line 90: Line 156:
Lithium chloride is also used as a ] to produce dark red flames. Lithium chloride is also used as a ] to produce dark red flames.


===Niche uses===
Lithium chloride is used as a relative humidity standard in the calibration of hygrometers. At 25C a saturated solution (45.81%) of the salt will yield an equilibrium relative humidity of 11.30%. Additionally, lithium chloride can itself 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 relative humidity at 25C, with minimal error in the range 10C to 30C, in percent, can be estimated from the following first order equation: RH=107.93-2.11C, where C is solution LiCl concentration, percent by mass.
Lithium chloride is used as a relative humidity standard in the calibration of ]s. At {{convert|25|C|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 {{convert|25|C|F}} can be estimated, with minimal error in the range {{convert|10-30|C}}, 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 ]s,<ref>{{cite journal | doi=10.1016/j.carbon.2014.05.089 | volume=77 | title=Towards large scale preparation of carbon nanostructures in molten LiCl | journal=Carbon | pages=835–845| year=2014 | last1=Kamali | first1=Ali Reza | last2=Fray | first2=Derek J. | doi-access=free }}</ref> ]<ref>{{cite journal | journal = Nanoscale| year= 2015|volume = 7| issue= 26|pages= 11310–11320 | doi = 10.1039/c5nr01132a| pmid= 26053881| title=Large-scale preparation of graphene by high temperature insertion of hydrogen into graphite|url= https://www.repository.cam.ac.uk/bitstream/1810/248812/1/Kamali%20%26%20Fray%202015%20Nanoscale.pdf| last1= Kamali| first1= Ali Reza| last2= Fray| first2= Derek J.| doi-access= free}}</ref> and ].<ref>{{cite journal | doi = 10.1016/j.ceramint.2013.07.085 | volume=40 | title=Preparation of lithium niobate particles via reactive molten salt synthesis method | journal=Ceramics International | pages=1835–1841| year=2014 | last1=Kamali | first1=Ali Reza | last2=Fray | first2=Derek J. }}</ref>

Lithium chloride has been shown to have strong ] properties, being effective against '']'' in populations of ]s.<ref>{{Cite journal|last1=Ziegelmann|first1=Bettina|last2=Abele|first2=Elisabeth|date=January 12, 2018|title=Lithium chloride effectively kills the honey bee parasite ''Varroa destructor'' by a systemic mode of action|journal=]|volume=8|issue=1|doi=10.1038/s41598-017-19137-5|pmid=29330449|pmc=5766531|page=683 |bibcode=2018NatSR...8..683Z}}</ref>

Lithium chloride is used as an aversive agent in lab animals to study ].


==Precautions== ==Precautions==
Lithium salts affect the ]; see ] for more details. For a short time in the 1940s lithium chloride was manufactured as a ], but this was prohibited after the toxic effects of the compound were recognized.<ref>{{cite journal Lithium salts affect the ] in a variety of ways. While the ], ], and ] salts are currently used to treat ], other ] including the chloride were used in the past. For a short time in the 1940s lithium chloride was manufactured as a ] for people with hypertension, but this was prohibited after the toxic effects of the compound (], ], ]) were recognized.<ref name="talbott">{{cite journal
| author= Talbott J. H. | author= Talbott J. H.
| title = Use of lithium salts as a substitute for sodium chloride | title = Use of lithium salts as a substitute for sodium chloride
| journal = Arch Med Interna. | journal = Arch Intern Med
| year = 1950 | year = 1950
| volume = 85 | volume = 85
| issue = 1 | issue = 1
| pages = 1–10 | pages = 1–10
| pmid = 15398859 }}</ref><ref>{{cite journal | pmid = 15398859
| doi=10.1001/archinte.1950.00230070023001}}</ref><ref>{{cite journal
| author= L. J. Stone, M. luton, lu3. J. Gilroy.
| author1= L. J. Stone | author2=M. luton | author3=J. Gilroy
| title = Lithium Chloride as a Substitute for Sodium Chloride in the Diet | title = Lithium Chloride as a Substitute for Sodium Chloride in the Diet
| journal = Journal of the American Medical Association | journal = Journal of the American Medical Association
Line 109: Line 183:
| issue = 11 | issue = 11
| pages = 688–692 | pages = 688–692
| doi =10.1001/jama.1949.02900280004002
| doi =
| pmid= 18128981 }}</ref><ref>{{cite web | publisher = ] | title = Case of trie Substitute Salt | date = 28 February 1949 | url = http://www.time.com/time/magazine/article/0,9171,799873,00.html}}</ref> | pmid= 18128981 }}</ref><ref>{{cite news | magazine = ] | title = Case of trie Substitute Salt | date = 28 February 1949 | url = http://www.time.com/time/magazine/article/0,9171,799873,00.html| archive-url = https://web.archive.org/web/20070302040542/http://www.time.com/time/magazine/article/0,9171,799873,00.html| url-status = dead| archive-date = March 2, 2007}}</ref> It was, however, noted by J. H. Talbott that many symptoms attributed to lithium chloride toxicity may have also been attributable to ], to the diuretics often administered to patients who were given lithium chloride, or to the patients' underlying conditions.<ref name="talbott" />

==See also==
*]
*]


==References== ==References==
{{reflist}}
* ''Handbook of Chemistry and Physics'', 71st edition, CRC Press, Ann Arbor, Michigan, 1990. * ''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. * 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. * R. Vatassery, titration analysis of LiCl, sat'd in Ethanol by AgNO<sub>3</sub> to precipitate AgCl(s). EP of this titration gives %Cl by mass.
* H. Nechamkin, ''The Chemistry of the Elements'', McGraw-Hill, New York, 1968. * H. Nechamkin, ''The Chemistry of the Elements'', McGraw-Hill, New York, 1968.
<references/>


==External links==

*
{{Commons category|Lithium chloride}}

{{Mood stabilizers}}
{{Lithium compounds}} {{Lithium compounds}}
{{Chlorides}}

{{Authority control}}


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