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| Identifiers | |
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3D model (JSmol) | |
| ChemSpider |
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| ECHA InfoCard | 100.029.290 |
| RTECS number |
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| UNII | |
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| Properties | |
| LiNO3 | |
| Molar mass | 68.946 g/mol |
| Appearance | White to light yellow solid |
| Density | 2.38 g/cm3 |
| Melting point | 255 °C (491 °F; 528 K) |
| Boiling point | 600 °C (1,112 °F; 873 K) (decomposes) |
| 52.2 g/100 mL (20 °C) 90 g/100 mL (28 °C) 234 g/100 mL (100 °C) | |
| Solubility | soluble inethanol,methanol,pyridine,ammonia,acetone |
| −62.0·10−6 cm3/mol (+3 H2O) | |
Refractive index (nD) | 1.735[1] |
| Thermochemistry | |
| 64 J/(mol K) | |
Std molar entropy(S⦵298) | 105 J/(mol K) |
Std enthalpy of formation(ΔfH⦵298) | −7.007 kJ/g or −482.3 kJ/mol |
Gibbs free energy(ΔfG⦵) | −389.5 kJ/mol |
Std enthalpy of combustion(ΔcH⦵298) | 25.5 kJ/mol |
| Hazards | |
| Occupational safety and health (OHS/OSH): | |
Main hazards | Oxidant, irritant |
| NFPA 704 (fire diamond) | |
| Flash point | Non-flammable |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose) | 1426 mg/kg (oral, rat) |
| Related compounds | |
Othercations | Sodium nitrate Potassium nitrate Rubidium nitrate Caesium nitrate |
Related compounds | Lithium sulfate Lithium chloride |
Except where otherwise noted, data are given for materials in theirstandard state (at 25 °C [77 °F], 100 kPa). | |
Lithium nitrate is aninorganic compound with the formula LiNO3. It is thelithiumsalt ofnitric acid (analkali metal nitrate). The salt isdeliquescent, absorbing water to form the hydrated form, lithium nitrate trihydrate. Its eutectics are of interest for heat transfer fluids.[2]
It is made by treatinglithium carbonate orlithium hydroxide withnitric acid.
This deliquescent colourless salt is anoxidizing agent used in the manufacture of red-coloredfireworks andflares.
Thehydrated form, lithium nitrate trihydrate, has an extremely highspecific heat of fusion,287±7 J/g,[3] and hence can be used for thermal energy storage at its melt temperature of 303.3 K.[4]
Lithium nitrate has been proposed as a medium to store heat collected from the sun for cooking. AFresnel lens would be used to melt solid lithium nitrate, which would then function as a "solar battery", allowing heat to be redistributed later by convection.[5]
Lithium nitrate can be synthesized by reacting nitric acid and lithium carbonate.
Generally when forming LiNO3, apH indicator is used to determine when all of the acid has been neutralized. However, this neutralization can also be recognized with the loss ofcarbon dioxide production.[6] In order to rid the final product of excess water, the sample is heated.
Lithium nitrate can be toxic to the body when ingested by targeting the central nervous system, thyroids, kidneys, and cardio-vascular system.[7] When exposed to the skin, eyes, and mucous membranes, lithium nitrate can cause irritation to these areas.[8]
