Difference between revisions of "Lithium chloride"
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==Preparation== | ==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. | + | 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. | Lithium oxide or hydroxide can also be used, but significant heat will be generated. | ||
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===Relevant Sciencemadness threads=== | ===Relevant Sciencemadness threads=== | ||
*[http://www.sciencemadness.org/talk/viewthread.php?tid=12851 Seperation of Lithium from ground salts] | *[http://www.sciencemadness.org/talk/viewthread.php?tid=12851 Seperation of Lithium from ground salts] | ||
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[[Category:Chemical compounds]] | [[Category:Chemical compounds]] | ||
[[Category:Inorganic compounds]] | [[Category:Inorganic compounds]] | ||
Revision as of 14:01, 6 May 2016
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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 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.
