|Jmol-3D images||Image 1|
|Molar mass||68.946 g/mol|
|Appearance||White to light yellow solid|
|Melting point||255 °C (491 °F; 528 K)|
|Boiling point||decomposes at 600 °C|
|Solubility in water||52.2 g/100 mL (20 °C)
90 g/100 mL (28 °C)
234 g/100 mL (100 °C)
|Solubility||soluble in ethanol, methanol, pyridine, ammonia|
|Refractive index (nD)||1.735|
|Std enthalpy of
|EU Index||Not listed|
|Main hazards||Oxidant, irritant|
|LD50||1426 mg/kg (oral, rat)|
|Other cations||Sodium nitrate
|Related compounds||Lithium sulfate
|Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)|
|(what is: / ?)|
Lithium Nitrate has been proposed as a medium to store heat collected from the sun for cooking. A Fresnel 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.
LiNO3 is utilized in solute-solvent interactions at decreasing temperatures (i.e. 329-290 K) which in affect, can be used to transport ions in binary solutions of molten acetamide.
Currently, lithium nitrate is being tested to see if it can be applied to concrete-pavement to withstand weathering effects.
In the lab, LiNO3 is commonly bound to a trihydrate ion in order to test bifureated hydrogen bonds within crystal structures of molecules which can correlate to hydrogen bond strength.
Lithium nitrate is also used as a catalyst which accelerates the breakdown of nitrogen oxides, through oxidation, found in soot.
Lithium nitrate can be synthesized by reacting nitric acid and lithium carbonate.
- Li2CO3 + 2 HNO3 → 2 LiNO3 + H2O + CO2
Generally when forming LiNO3, a pH indicator is used to determine when all of the acid has been neutralized. However, this neutralization can also be recognized with the loss of carbon dioxide production. In order to rid the final product of excess water, the sample is heated.
- 4 LiNO3 → 2 Li2O + 4 NO2 + O2
Other group I nitrates decompose differently, forming the nitrite salt and oxygen. Because of its relatively small size, the lithium cation is very polarizing, which favors the formation of the oxide.
Lithium nitrate is also a very good oxidizing agent. Today LiNO3 is used in submarines and spacecraft for absorbing excess carbon dioxide in the air.
Lithium nitrate is also denser than water.
Lithium nitrate can be toxic to the body when ingested by targeting the central nervous system, thyroids, kidneys, and cardio-vascular system. When exposed to the skin, eyes, and mucous membranes, lithium nitrate can cause irritation to these areas.
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