| IUPAC name
| Systematic IUPAC name
| Other names
|Melting point||723 °C (1,333 °F; 996 K)|
|Boiling point||1,310 °C (2,390 °F; 1,580 K) Decomposition begins at 1300 °C|
| 1.54 g/100 ml (0 °C)|
1.43 g/100 ml (10 °C)
1.29 g/100 ml (25 °C)
1.08 g/100 ml (40 °C)
0.69 g/100 ml (100 °C)
|Solubility||Insoluble in acetone, alcohol, ammonia|
|Vapor pressure||~0 mmHg|
|Safety data sheet||ScienceLab|
| Sodium carbonate|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Lithium carbonate is an inorganic compound, with the formula Li2CO3.
- Li2CO3 + CO2 + H2O ⇌ 2 LiHCO3
Like all carbonates it will react with a stronger acid to release carbon dioxide.
- Li2CO3 + 2 HCl → 2 LiCl + H2O + CO2
Lithium carbonate is a white solid, non-hygroscopic, poorly soluble in water, as well as most organic solvents. It is more soluble in cold water than hot water. Unlike other alkaline metal carbonates, it does not form hydrates and only exists as anhydrous form.
Lithium carbonate is sold by chemical suppliers. It can also be purchased from eBay.
Certain drugs that are used for the treatment of bipolar disorders, such as Eskalith, contain lithium carbonate.
It occurs naturally as the rare mineral zabuyelite.
Lithium carbonate can be made or extracted from dead lithium batteries. If there is still some lithium metal or lithium hydroxide left, add the battery content in water and bubble carbon dioxide in the aqueous solution. This will form lithium bicarbonate which is more soluble in water and can be filtered from the rest of the battery. Drying the solution will cause it to revert to lithium carbonate.
- Make various lithium salts
- Make lithia glass
Lithium carbonate does not pose a risk to touch, however it should be avoided ingesting it.
In closed bottles, away from any acidic vapors.
Due to the price of lithium, it's best to try to recycle it.