Lithium perchlorate
| Lithium perchlorate | |
|---|---|
| |
| IUPAC name | Lithium perchlorate |
| Other names | Perchloric acid, lithium salt |
| Identifiers | |
| CAS number | |
| Properties | |
| Molecular formula | LiClO4 |
| Molar mass | 106.39 g/mol |
| Appearance | white crystals |
| Density | 2.43 g/cm3, solid |
| Melting point |
236 °C |
| Boiling point |
430 °C (with decomp.) |
| Solubility in water | 60 g/100 mL |
| Hazards | |
| MSDS | External MSDS |
| Main hazards | Oxdizer Irritatant |
| Related Compounds | |
| Other cations | Caesium perchlorate; potassium perchlorate |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references | |
Lithium perchlorate is the chemical compound with the formula LiClO4. This white crystalline salt is noteworthy for its high solubility in many solvents. It exists both in anhydrous form and as a trihydrate.
Uses
Lithium perchlorate is used as a source of oxygen in some chemical oxygen generators. It decomposes at about 400 °C, yielding lithium chloride and oxygen. It has both the highest weight to oxygen and oxygen to volume ratio of all perchlorates, which makes it especially advantageous in aerospace applications.
LiClO4 is highly soluble in organic solvents, even diethyl ether. Such solutions are employed in the Diels-Alder reactions, where it is proposed that the Lewis acidic Li+ binds to substituents on the diene, thereby accelerating the reaction.[1]
Lithium perchlorate is also extensively used as an electrolyte in lithium batteries, as it does not undergo oxidization on the anode.
Concentrated solutions of lithium perchlorate (4.5 mol/l) are used as a chaotropic agent to denature proteins.
Production
Lithium perchlorate can be manufactured by reaction of sodium perchlorate with lithium chloride. It can be also prepared by electrolysis of lithium chlorate at 200 mA/cm² at temperatures above 20 °C.[citation needed]
Safety
Perchlorates often give explosive mixtures with organic compounds.
References
- ↑ Charette, A. B. "Lithium Perchlorate" in Encyclopedia of Reagents for Organic Synthesis (Ed: L. Paquette) 2004, J. Wiley & Sons, New York. DOI: 10.1002/047084289.
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