Lithium chloride
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| Names | |
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| Preferred IUPAC name
Lithium chloride | |
| Systematic IUPAC name
Lithium(1+) chloride | |
| Identifiers | |
3D model (
JSmol ) |
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| ChEBI | |
| ChEMBL | |
| ChemSpider | |
ECHA InfoCard
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100.028.375 |
| EC Number |
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| MeSH | Lithium+chloride |
PubChem CID
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RTECS number
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| UNII | |
| UN number | 2056 |
CompTox Dashboard (EPA)
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| Properties | |
| LiCl | |
| Molar mass | 42.39 g·mol−1 |
| Appearance | white solid hygroscopic , sharp
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| Density | 2.068 g/cm3 |
| Melting point | 605–614 °C (1,121–1,137 °F; 878–887 K) |
| Boiling point | 1,382 °C (2,520 °F; 1,655 K) |
| 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 1-propanol[1]
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| 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] |
liquid ammonia
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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] |
| −24.3·10−6 cm3/mol | |
Refractive index (nD)
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1.662 (24 °C) |
| Viscosity | 0.87 cP (807 °C)[1] |
| Structure | |
| Octahedral | |
| Linear (gas) | |
| 7.13 D (gas) | |
| Thermochemistry | |
Heat capacity (C)
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48.03 J/mol·K[1] |
Std molar
entropy (S⦵298) |
59.31 J/mol·K[1] |
Std enthalpy of (ΔfH⦵298)formation |
-408.27 kJ/mol[1] |
Gibbs free energy (ΔfG⦵)
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-384 kJ/mol[1] |
| Pharmacology | |
| V04CX11 (WHO) | |
| Hazards | |
| GHS labelling: | |
 [3]
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| Warning | |
| H302, H315, H319, H335[3] | |
| P261, P305+P351+P338[3] | |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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526 mg/kg (oral, rat)[4] |
| Safety data sheet (SDS) | ICSC 0711 |
| Related compounds | |
Other anions
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Lithium fluoride Lithium bromide Lithium iodide Lithium astatide |
Other cations
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Sodium chloride Potassium chloride Rubidium chloride Caesium chloride Francium chloride |
| Supplementary data page | |
| Lithium chloride (data page) | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Lithium chloride is a
Chemical properties
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:
- LiCl + AgNO3 → AgCl + LiNO3
Preparation
Lithium 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
Commercial applications
Lithium chloride is mainly used for the production of
Lithium chloride is also used as a flame colorant to produce dark red flames.
Niche uses
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
Lithium salts affect the
See also
References
- ^ 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
- ^ ISBN 978-3527306732.
- ISBN 0-12-352651-5.
- .
- PMID 6198133.
- .
- PMID 26053881.
- .
- PMID 29330449.
- ^ PMID 15398859.
- 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
