Difference between revisions of "Lithium carbonate"
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| SystematicName = Lithium carbonate | | SystematicName = Lithium carbonate | ||
| − | | OtherNames = | + | | OtherNames = Carbolith<br>Cibalith-S<br>Dilithium carbonate<br>Duralith<br>Eskalith<br>Lithane<br>Lithizine<br>Lithobid<br>Lithonate<br>Lithotabs Priadel<br>Zabuyelite |
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| MeltingPt_ref = | | MeltingPt_ref = | ||
| MeltingPt_notes = | | MeltingPt_notes = | ||
| + | | Odor = Odorless | ||
| pKa = | | pKa = | ||
| pKb = | | pKb = | ||
| − | | Solubility = 1.54 g/100 | + | | Solubility = 1.54 g/100 ml (0 °C)<br>1.43 g/100 ml (10 °C)<br>1.29 g/100 ml (25 °C)<br>1.08 g/100 ml (40 °C)<br>0.69 g/100 ml (100 °C) |
| − | | SolubleOther = Insoluble in [[acetone]], alcohol, [[ammonia]] | + | | SolubleOther = Reacts with acids<br>Insoluble in [[acetone]], alcohol, [[ammonia]] |
| Solvent = | | Solvent = | ||
| − | | VaporPressure = | + | | VaporPressure = ~0 mmHg |
}} | }} | ||
| Section3 = {{Chembox Structure | | Section3 = {{Chembox Structure | ||
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| AutoignitionPt = None | | AutoignitionPt = None | ||
| ExploLimits = None | | ExploLimits = None | ||
| − | | ExternalMSDS = http://www.sciencelab.com/msds.php?msdsId=9927209 | + | | ExternalMSDS = [http://www.sciencelab.com/msds.php?msdsId=9927209 ScienceLab] |
| FlashPt = None | | FlashPt = None | ||
| LD50 = | | LD50 = | ||
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| OtherFunction = | | OtherFunction = | ||
| OtherFunction_label = | | OtherFunction_label = | ||
| − | | OtherCompounds = | + | | OtherCompounds = [[Sodium carbonate]]<br>[[Potassium carbonate]] |
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| − | '''Lithium carbonate''' is an inorganic compound, with the formula Li<sub>2</sub>CO<sub>3</sub>. | + | '''Lithium carbonate''' is an inorganic compound, with the formula '''Li<sub>2</sub>CO<sub>3</sub>'''. |
==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
| − | Lithium carbonate reacts with [[carbon dioxide]] when | + | Lithium carbonate reacts with [[carbon dioxide]] when dissolved in water to form [[lithium bicarbonate]], which is 10 times more soluble: |
| − | :Li<sub>2</sub>CO<sub>3</sub> + CO<sub>2</sub> + H<sub>2</sub>O ⇌ 2 LiHCO<sub>3</sub> | + | : Li<sub>2</sub>CO<sub>3</sub> + CO<sub>2</sub> + H<sub>2</sub>O ⇌ 2 LiHCO<sub>3</sub> |
Like all carbonates it will react with a stronger acid to release carbon dioxide. | Like all carbonates it will react with a stronger acid to release carbon dioxide. | ||
| − | :Li<sub>2</sub>CO<sub>3</sub> + 2 HCl → 2 LiCl + H<sub>2</sub>O + CO<sub>2</sub> | + | : Li<sub>2</sub>CO<sub>3</sub> + 2 HCl → 2 LiCl + H<sub>2</sub>O + CO<sub>2</sub> |
===Physical=== | ===Physical=== | ||
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Certain drugs that are used for the treatment of bipolar disorders, such as [http://www.drugs.com/pro/eskalith.html Eskalith], contain lithium carbonate. | Certain drugs that are used for the treatment of bipolar disorders, such as [http://www.drugs.com/pro/eskalith.html Eskalith], contain lithium carbonate. | ||
| − | It occurs naturally as the rare mineral zabuyelite. | + | It occurs naturally as the rare mineral ''zabuyelite''. |
==Preparation== | ==Preparation== | ||
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[[Category:Inorganic compounds]] | [[Category:Inorganic compounds]] | ||
[[Category:Lithium compounds]] | [[Category:Lithium compounds]] | ||
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[[Category:Carbonates]] | [[Category:Carbonates]] | ||
[[Category:Bases]] | [[Category:Bases]] | ||
[[Category:Easily prepared chemicals]] | [[Category:Easily prepared chemicals]] | ||
| + | [[Category:Essential reagents]] | ||
Latest revision as of 15:01, 18 November 2023
| Names | |
|---|---|
| IUPAC name
Lithium carbonate
| |
| Systematic IUPAC name
Lithium carbonate | |
| Other names
Carbolith
Cibalith-S Dilithium carbonate Duralith Eskalith Lithane Lithizine Lithobid Lithonate Lithotabs Priadel Zabuyelite | |
| Properties | |
| Li2CO3 | |
| Molar mass | 73.89 |
| Appearance | White solid |
| Odor | Odorless |
| Density | 2.11 g/cm3 |
| 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 | Reacts with acids Insoluble in acetone, alcohol, ammonia |
| Vapor pressure | ~0 mmHg |
| Hazards | |
| Safety data sheet | ScienceLab |
| Flash point | None |
| Related compounds | |
| Related compounds
|
Sodium carbonate Potassium carbonate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Lithium carbonate is an inorganic compound, with the formula Li2CO3.
Contents
Properties
Chemical
Lithium carbonate reacts with carbon dioxide when dissolved in water to form lithium bicarbonate, which is 10 times more soluble:
- 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
Physical
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.
Availability
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.
Preparation
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.
Projects
- Make various lithium salts
- Make lithia glass
Handling
Safety
Lithium carbonate does not pose a risk to touch, however it should be avoided ingesting it.
Storage
In closed bottles, away from any acidic vapors.
Disposal
Due to the price of lithium, it's best to try to recycle it.
