Lithium nitrate
| Names | |
|---|---|
| IUPAC name
Lithium nitrate
| |
| Preferred IUPAC name
Lithium nitrate | |
| Systematic IUPAC name
Lithium nitrate | |
| Other names
Nitric acid, lithium salt
| |
| Properties | |
| LiNO3 | |
| Molar mass | 68.946 g/mol |
| Appearance | Colorless deliquescent solid |
| Odor | Odorless |
| Density | 2.38 g/cm3 |
| Melting point | 255 °C (491 °F; 528 K) |
| Boiling point | 600 °C (1,112 °F; 873 K) (decomposition) |
| 52.2 g/100 ml (20 °C) 90 g/100 ml (28 °C) 234 g/100 ml (100 °C) | |
| Solubility | Soluble in acetone, liq. ammonia, ethanol, methanol, pyridine |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
105 J·mol-1·K-1 |
| Std enthalpy of
formation (ΔfH |
-7.007 kJ/g or -482.3 kJ/mol |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
| LD50 (Median dose)
|
1,426 mg/kg (oral, rat) |
| Related compounds | |
| Related compounds
|
Sodium nitrate Potassium nitrate Rubidium nitrate Caesium nitrate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Lithium nitrate is an inorganic compound with the formula LiNO3. The compound is deliquescent, absorbing water to form the hydrated form, lithium nitrate trihydrate. Its eutectics are of interest for heat transfer fluids.
Contents
Properties
Chemical
Lithium nitrate is a powerful oxidizer. When mixed with a combustible material and ignited, it burns with a red flame.
Physical
Lithium nitrate is a colorless solid, soluble in water.
The hydrated form, lithium nitrate trihydrate, has an extremely high specific heat of fusion, 287 (± 7) J/g, and hence can be used for thermal energy storage at its melt temperature of 303.3 K.
Availability
Lithium nitrate is sold by chemical suppliers.
Preparation
Lithium nitrate can be easily and safely synthesized by reacting nitric acid and lithium carbonate.
- Li2CO3 + 2 HNO3 → 2 LiNO3 + H2O + CO2
If available lithium hydroxide can also be used, although the neutralization reaction is very exothermic, so the solution needs to be cooled during the reaction.
- LiOH + HNO3 → LiNO3 + H2O
Never use lithium metal as it will catch fire and may even explode!
Projects
- Red-colored fireworks and flares
- Heat storage
Handling
Safety
Lithium nitrate, like most lithium compounds can be toxic to the body when ingested by targeting the central nervous system, thyroids, kidneys, and cardio-vascular system.
It is a powerful oxidizer and must be kept away from combustible materials.
Storage
In closed glass or plastic bottles, away from acids and flammable materials.
Disposal
Lithium nitrate can be converted to an insoluble lithium compound and recycled. While it may be used as fertilizer to a degree, lithium is expensive and it's best to recycle it.
