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| Names | |
|---|---|
| Preferred IUPAC name Lithium chloride | |
| Systematic IUPAC name Lithium(1+) chloride | |
| Identifiers | |
3D model (JSmol) | |
| ChEBI | |
| ChEMBL | |
| ChemSpider |
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| ECHA InfoCard | 100.028.375 |
| EC Number |
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| MeSH | Lithium+chloride |
| RTECS number |
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| UNII | |
| UN number | 2056 |
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| Properties | |
| LiCl | |
| Molar mass | 42.39 g·mol−1 |
| Appearance | white solid hygroscopic, sharp |
| 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 inhydrazine,methylformamide,butanol,selenium(IV) oxychloride,1-propanol[1] |
| Solubility inmethanol | 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 inethanol | 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 informic acid | 26.6 g/100 g (18 °C) 27.5 g/100 g (25 °C)[1] |
| Solubility inacetone | 1.2 g/100 g (20 °C) 0.83 g/100 g (25 °C) 0.61 g/100 g (50 °C)[1] |
| Solubility inliquid 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] |
| −24.3·10−6 cm3/mol | |
Refractive index (nD) | 1.662 (24 °C) |
| Viscosity | 0.87 cP (807 °C)[1] |
| Structure | |
| Octahedral | |
| Linear (gas) | |
| 7.13 D (gas) | |
| Thermochemistry | |
| 48.03 J/mol·K[1] | |
Std molar entropy(S⦵298) | 59.31 J/mol·K[1] |
Std enthalpy of formation(ΔfH⦵298) | −408.27 kJ/mol[1] |
Gibbs free energy(ΔfG⦵) | −384 kJ/mol[1] |
| Pharmacology | |
| V04CX11 (WHO) | |
| Hazards | |
| GHS labelling: | |
 [3] | |
| 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) | 526 mg/kg (oral, rat)[4] |
| Safety data sheet (SDS) | ICSC 0711 |
| Related compounds | |
Otheranions | Lithium fluoride Lithium bromide Lithium iodide Lithium astatide |
Othercations | 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 theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Lithium chloride is achemical compound with theformulaLiCl. Thesalt is a typicalionic 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 polarsolvents (83.05 g/100 mL of water at 20 °C) and itshygroscopic properties.[5]
The salt forms crystallinehydrates, 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 ofammonia/mol. As with any other ionic chloride, solutions of lithium chloride can serve as a source ofchloride ion, e.g., forming a precipitate upon treatment withsilver nitrate:
Lithium chloride is produced by treatment oflithium carbonate withhydrochloric acid.[5] Anhydrous LiCl is prepared from the hydrate by heating in a stream ofhydrogen chloride.
Lithium chloride is mainly used for the production oflithium metal byelectrolysis of a LiCl/KCl melt at 450 °C (842 °F). LiCl is also used as a brazingflux foraluminium inautomobile parts. It is used as adesiccant for drying air streams.[5] In more specialized applications, lithium chloride finds some use inorganic synthesis, e.g., as an additive in theStille reaction. Also, in biochemical applications, it can be used to precipitateRNA from cellular extracts.[8]
Lithium chloride is also used as aflame colorant to produce dark red flames.
Lithium chloride is used as a relative humidity standard in the calibration ofhygrometers. 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 ofcarbon nanotubes,[9]graphene[10] andlithium niobate.[11]
Lithium chloride has been shown to have strongacaricidal properties, being effective againstVarroa destructor in populations ofhoney bees.[12]
Lithium chloride is used as an aversive agent in lab animals to studyconditioned place preference and aversion.
Lithium salts affect thecentral nervous system in a variety of ways. While thecitrate,carbonate, andorotate salts are currently used to treatbipolar disorder, otherlithium salts including the chloride were used in the past. For a short time in the 1940s lithium chloride was manufactured as asalt 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 tosodium chloride deficiency, to the diuretics often administered to patients who were given lithium chloride, or to the patients' underlying conditions.[13]
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