Lithium hydroxide
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| Names | |
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IUPAC name
Lithium hydroxide
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| Other names
Lithine
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| Identifiers | |
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3D model (Jmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.013.804 |
| 68415 | |
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PubChem CID
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| RTECS number | OJ6307070 |
| UNII | |
| UN number | 2680 |
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| Properties | |
| LiOH | |
| Molar mass | 23.95 g/mol (anhydrous) 41.96 g/mol (monohydrate) |
| Appearance |
hygroscopic white solid odorless |
| Density | 1.46 g/cm3 (anhydrous) 1.51 g/cm3 (monohydrate) |
| Melting point | 462 °C (864 °F; 735 K) |
| Boiling point | 924 °C (1,695 °F; 1,197 K) decomposes |
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anhydrous:
12.7 g/100 mL (0 °C) 12.8 g/100 mL (20 °C) 17.5 g/100 mL (100 °C) monohydrate: 22.3 g/100 mL (10 °C) 26.8 g/100 mL (80 °C) |
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| Solubility in methanol |
anhydrous:
9.76 g/100 g (20 °C, 48 hours mixing) monohydrate: 13.69 g/100 g (20 °C, 48 hours mixing) |
| Solubility in ethanol |
anhydrous:
2.36 g/100 g (20 °C, 48 hours mixing) monohydrate: 2.18 g/100 g (20 °C, 48 hours mixing) |
| Solubility in isopropanol |
anhydrous:
0 g/100 g (20 °C, 48 hours mixing) monohydrate: 0.11 g/100 g (20 °C, 48 hours mixing) |
| Basicity (pKb) | −0.04(LiOH(aq) = Li+ + OH–) |
| −12.3·10−6 cm3/mol | |
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Refractive index (nD)
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1.464 (anhydrous) 1.460 (monohydrate) |
| Thermochemistry | |
| 2.071 J/g K | |
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Std enthalpy of
formation (ΔfH |
-20.36 kJ/g |
| Hazards | |
| Main hazards | Corrosive |
| Safety data sheet |
ICSC 0913 ICSC 0914 (monohydrate) |
| NFPA 704 | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
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LD50 (median dose)
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210 mg/kg (oral, rat) |
| Related compounds | |
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Other anions
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Lithium amide |
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Other cations
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Sodium hydroxide Potassium hydroxide Rubidium hydroxide Caesium hydroxide |
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Related compounds
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Lithium oxide |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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 (what is   ?) |
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| Infobox references | |
Lithium hydroxide is an inorganic compound with the formula LiOH. It is a white hygroscopic crystalline material. It is soluble in water and slightly soluble in ethanol, and is available commercially in anhydrous form and as the monohydrate (LiOH.H2O), both of which are strong bases. It is the weakest base among the alkali metal hydroxides.
Lithium hydroxide is produced in a metathesis reaction between lithium carbonate and calcium hydroxide:
The initially produced hydrate is dehydrated by heating under vacuum up to 180 °C.
In the laboratory, lithium hydroxide arises by the action of water on lithium or lithium oxide. The equations for these processes follow:
Typically, these reactions are avoided.
Although lithium carbonate is more widely used, the hydroxide is an effective precursor to lithium salts, e.g.
Lithium hydroxide is mainly consumed for the production of lithium greases. A popular lithium grease is lithium stearate, which is a general-purpose lubricating grease due to its high resistance to water and usefulness at both high and low temperatures.
Lithium hydroxide is used in breathing gas purification systems for spacecraft, submarines, and rebreathers to remove carbon dioxide from exhaled gas by producing lithium carbonate and water:
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