| Chemical properties | Lithium Nitrate is an inorganic compound with the formula LiNO3 with highly water solubility. All metallic nitrates are inorganic salts of a given metal cation and the nitrate anion. The nitrate anion is a univalent (-1 charge) polyatomic ion composed of a single nitrogen atom ionically bound to three oxygen atoms for a total formula weight of 62.05. Nitrate compounds are generally soluble in water.
Lithium Nitrate is white trigonal crystal. It is soluble in water, ethanol, pyridine and ammonia. The aqueous solution is neutral.
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| Solubility in water (g/100ml) | Dissolved amount (g) per 100 milliliters of water at different temperatures (° C)
53.4g/0℃;60.8g/10℃;70.1g/20℃;138g/30℃;152g/40℃;175g/60℃ |
| Toxicity | 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. It releases toxic and irritating nitrogen oxides when it burns. It decomposes at high temperatures, producing toxic nitroxides. When people inhale these, they will be poisoned. Others refer to sodium nitrate.
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| Application | Used as liquid ammonia stabilizer in refrigeration equipment, rocket propellant, oxidants of pyrotechnic manufacture, glass etchants, antistatic agents, composition of molten salt in metallurgical industry. Used as an analytical reagent; dissolving and cooling agent; heat exchange carrier; catalyst for the paint; raw materials of other nickel salt; mordant of reducing dye. Used for the manufacture of a phosphor, other lithium salt, nickel batteries and for ceramics and metal coloring. Used in the electroplating industry; organic synthesis and production of hardening oil. Lithium Nitrate has been proposed as a medium to store heat collected from the sun for cooking. Lithium nitrate is also a very good oxidizing agent in the manufacture of red-colored fireworks and flares. Currently, lithium nitrate is being tested to see if it can be applied to concrete-pavement to withstand weathering effects.
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| Preparation | Lithium hydroxide or lithium carbonate is added to the reactor containing distilled water, and nitric acid is slowly added under stirring and heating to carry out the reaction. Then we evaporate it to dryness and heat it under vacuum at about 200 ° C, finally we get lithium nitrate. HNO3+LiOH→LiNO3+H2O |
| Explosive characteristics | May cause the acceleration of the burning of combustible materials. Prolonged exposure to heat or flames may result in an explosion. |
| References | https://pubchem.ncbi.nlm.nih.gov/compound/Lithium_nitrate#section=Top
https://www.americanelements.com/lithium-nitrate-7790-69-4
https://en.wikipedia.org/wiki/Lithium_nitrate |
| Chemical Properties | Lithium nitrate is a colorless deliquescent powder, enthalpy of fusion 24.90 kJ/mol; can be prepared by reaction of HNO3 with LiOH or Li2CO3, followed by evaporation to dryness and then heating at ~200°C in vacuum; used in ceramics, pyrotechnics, molten salt baths, rocket propellants, refrigerators. [HAW93] [CRC10] [MER06] [KIR81] [FMC93] |
| Uses | Lithium nitrate can be used in special pyrotechnic devices to give a red flame. Lithium nitrate may also be used in combination with other salts, particularly nitrates, to produce low-melting fused salt mixtures.
Used in ceramics, heat-exchange media, refrigeration systems. |
| Uses | Lithium nitrate is used in ceramics, pyrotechnics, salt baths, heat-exchange media, refrigeration systems, rocket propellant and in solar batteries. It acts as an oxidizing agent used in the production of red-colored fireworks and flares, as a catalyst to accelerate the breakdown of nitrogen oxides and as a medium to store heat received from sun for cooking. It is applied to concrete-pavement to withstand weathering effects. |
| Definition | ChEBI: The inorganic nitrate salt of lithium. |
| Preparation | Lithium nitrate is readily prepared industrially or in the laboratory by the reaction of lithium hydroxide or lithium carbonate with nitric acid. The resulting solution is evaporated and the solid is dried to obtain anhydrous lithium nitrate. Lithium nitrate is very soluble in water. The compound absorbs moisture from the air. Below about 30 °C it crystallizes from solution as lithium nitrate trihydrate; above that temperature the anhydrous material precipitates although the question of the existence of a half-hydrate is not entirely settled. |
| General Description | A white to light yellow colored crystalline solid. Denser than water. Contact with the material may cause irritation to skin, eyes, and mucous membranes. May be toxic by ingestion. May cause the acceleration of the burning of combustible materials. Prolonged exposure to heat or flames may result in an explosion. |
| Air & Water Reactions | Deliquescent. Soluble in water. |
| Reactivity Profile | Lithium nitrate is an oxidizing agent. Mixtures with alkyl esters may explode owing to the formation of alkyl nitrates; mixtures with phosphorus, tin(II) chloride, or other reducing agents may react explosively [Bretherick 1979. p. 108-109]. |
| Health Hazard | Inhalation, ingestion or contact (skin, eyes) with vapors or substance may cause severe injury, burns or death. Fire may produce irritating, corrosive and/or toxic gases. Runoff from fire control or dilution water may cause pollution. |
| Fire Hazard | These substances will accelerate burning when involved in a fire. Some may decompose explosively when heated or involved in a fire. May explode from heat or contamination. Some will react explosively with hydrocarbons (fuels). May ignite combustibles (wood, paper, oil, clothing, etc.). Containers may explode when heated. Runoff may create fire or explosion hazard. |
| Flammability and Explosibility | Nonflammable |
| Potential Exposure | Lithium nitrate is used in ceramics, pyrotechnics, salt baths; refrigeration systems; and rocket propellants |
| Shipping | UN2722 Lithium nitrate, Hazard Class: 5.1; Labels: 5.1-Oxidizer |
| Purification Methods | It crystallises from water or EtOH. Dry it at 180o for several days by repeated melting under vacuum. If it is crystallised from water keeping the temperature above 70o, formation of trihydrate is avoided. The anhydrous salt is dried at 120o and stored in a vacuum desiccator over CaSO4. After the 99% pure salt was recrystallised 3times, it contained: metal (ppm) Ca (1.6), K (1.1), Mo (0.4), Na (2.2). [Donnan & Burt J Chem Soc 83 335 1903.] |
| Incompatibilities | May explode when exposed to sparks, shock and heat. Violent reactions with combustible materials; oxidizers, organic materials; reducing agents; strong acids |
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