Difference between revisions of "Lithium chloride"
| Line 69: | Line 69: | ||
| Solubility1 = 1.2 g/100 g (20 °C)<br>0.83 g/100 g (25 °C)<br>0.61 g/100 g (50 °C) | | Solubility1 = 1.2 g/100 g (20 °C)<br>0.83 g/100 g (25 °C)<br>0.61 g/100 g (50 °C) | ||
| Solvent1 = acetone | | Solvent1 = acetone | ||
| + | | Solubility2 = 0.54 g/100 g (-34 °C)<br>3.02 g/100 g (25 °C) | ||
| + | | Solvent2 = ammonia | ||
| + | | Solubility3 = 14.42 g/100 g (0 °C)<br>24.28 g/100 g (20 °C)<br>25.1 g/100 g (30 °C)<br>23.46 g/100 g (60 °C) | ||
| + | | Solvent3 = ethanol | ||
| + | | Solubility4 = 26.6 g/100 g (18 °C)<br>27.5 g/100 g (25 °C) | ||
| + | | Solvent4 = formic acid | ||
| + | | Solubility5 = 45.2 g/100 g (0 °C)<br>43.8 g/100 g (20 °C)<br>42.36 g/100 g (25 °C)<br>44.6 g/100 g (60 °C) | ||
| + | | Solvent5 = methanol | ||
| VaporPressure = 1 torr (785 °C)<br>10 torr (934 °C)<br>100 torr (1130 °C) | | VaporPressure = 1 torr (785 °C)<br>10 torr (934 °C)<br>100 torr (1130 °C) | ||
}} | }} | ||
| Line 90: | Line 98: | ||
}} | }} | ||
| Section6 = {{Chembox Hazards | | Section6 = {{Chembox Hazards | ||
| − | | AutoignitionPt = | + | | AutoignitionPt = Non-flammable |
| ExploLimits = | | ExploLimits = | ||
| − | | ExternalMSDS = [] | + | | ExternalMSDS = [https://www.docdroid.net/R7VUmYa/lithium-chloride-sa.pdf.html Sigma-Aldrich] |
| − | | FlashPt = | + | | FlashPt = Non-flammable |
| LD50 = 526 mg/kg (rat, oral) | | LD50 = 526 mg/kg (rat, oral) | ||
| LC50 = | | LC50 = | ||
Revision as of 15:06, 12 April 2017
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|
 Anhydrous LiCl in a tube.
| |
| Names | |
|---|---|
| IUPAC name
Lithium chloride
| |
| Preferred IUPAC name
Lithium chloride | |
| Other names
Lithium(1+) chloride
Lithium monochloride | |
| Properties | |
| LiCl | |
| Molar mass | 42.39 g/mol |
| Appearance | White solid |
| Density | 2.068 g/cm3 |
| Melting point | 613 °C (1,135 °F; 886 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) | |
| Solubility | Soluble in acetone, butanol, diethyl ether, ethanol, hydrazine, methanol, methylformamide, nitrobenzene, propanol, pyridine, selenium oxychloride |
| Solubility in acetone | 1.2 g/100 g (20 °C) 0.83 g/100 g (25 °C) 0.61 g/100 g (50 °C) |
| Solubility in ammonia | 0.54 g/100 g (-34 °C) 3.02 g/100 g (25 °C) |
| 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) |
| Solubility in formic acid | 26.6 g/100 g (18 °C) 27.5 g/100 g (25 °C) |
| Solubility in methanol | 45.2 g/100 g (0 °C) 43.8 g/100 g (20 °C) 42.36 g/100 g (25 °C) 44.6 g/100 g (60 °C) |
| Vapor pressure | 1 torr (785 °C) 10 torr (934 °C) 100 torr (1130 °C) |
| Thermochemistry | |
| Std molar
entropy (S |
59.31 J·mol-1·K-1 |
| Std enthalpy of
formation (ΔfH |
-408.27 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
526 mg/kg (rat, oral) |
| Related compounds | |
| Related compounds
|
Sodium chloride |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Lithium chloride is an ionic salt of lithium with the chemical formula LiCl.
Contents
Properties
Chemical
LiCl will react with soluble salts of heavy metals, such as silver and lead(II) nitrate, to precipitate their insoluble chlorides.
- LiCl + AgNO3 → LiNO3 + AgCl
- 2 LiCl + Pb(NO3)2 → 2 LiNO3 + PbCl2
Physical
Lithium is a white hygroscopic solid compound, soluble in water and many other solvents, such as methanol, ethanol, isopropanol, butanol, formic acid, N-Methylformamide, hydrazine, THF, although it is poorly soluble in acetone and ammonia. LiCl is completely insoluble in dichloromethane. Lithium chloride has a melting point at around 614 °C.
Availability
Lithium chloride can be purchased from chemical suppliers. ScienceCompany sells 100 g of LiCl at $18.95.
Preparation
Although lithium chloride can be prepared by reacting lithium metal with hydrochloric acid or chlorine gas, this method is both uneconomical and extremely dangerous, as it consumes the expensive metal. LiCl is much better prepared by reacting lithium carbonate with HCl. Completely dead lithium batteries are a good source of lithium carbonate. Lithium chloride can be dried to its anhydrous form by heating it in a stream of hydrogen chloride. Heating it without hydrogen chloride will cause it to partially hydrolyze.
Lithium oxide or hydroxide can also be used, but significant heat will be generated.
Projects
- Making lithium metal
Handling
Safety
Lithium chloride affects the nervous system, so it should not be used as a salt substitute.
Storage
Lithium chloride is hygroscopic and must be stored in an airtight container (if you don't want to use its hydrated form).
Disposal
As lithium compounds can be hard to come by, they are best recycled.
