Chemical properties
Lithium nitrate is an inorganic compound with the formula LiNO3. It is the lithium salt of nitric acid. 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. Lithium Nitrate produced a red flame while Calcium Nitrate produced an orange flame.
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.
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.
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 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.
Uses
Lithium nitrate can be used in special pyrotechnic devices to give a red flame. It may also be used in combination with other salts, particularly nitrates, to produce low-melting fused salt mixtures.
Definition
ChEBI: Lithium nitrate is the inorganic nitrate salt of lithium. It has a role as an oxidising agent. It is an inorganic nitrate salt and a lithium salt.
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
Non flammable
Potential Exposure
Lithium nitrate is used in ceramics,
pyrotechnics, salt baths; refrigeration systems; and rocket
propellants
First aid
If this chemical gets into the eyes, remove anycontact lenses at once and irrigate immediately for at least15 min, occasionally lifting upper and lower lids. Seek medical attention immediately. If this chemical contacts theskin, remove contaminated clothing and wash immediatelywith soap and water. Seek medical attention immediately. Ifthis chemical has been inhaled, remove from exposure,begin rescue breathing (using universal precautions, including resuscitation mask) if breathing has stopped and CPR ifheart action has stopped. Transfer promptly to a medicalfacility. When this chemical has been swallowed, get medical attention. Give large quantities of water and induce vomiting. Do not make an unconscious person vomit.Medical observation is recommended for 24-48 h afterbreathing overexposure, as pulmonary edema may bedelayed. As first aid for pulmonary edema, a doctor orauthorized paramedic may consider administering a corticosteroid spray.
storage
Color Code—Yellow: Reactive Hazard; Store in alocation separate from other materials, especially flammables and combustibles. Prior to working with this chemical you should be trained on its proper handling andstorage. Lithium nitrate must be stored to avoid contactwith wood, paper, oil and heat, and oxidizers (such as perchlorates, peroxides, permanganates, chlorates, andnitrates), since violent reactions occur. Protect containersagainst physical damage, heat, shock, sparks. Store intightly closed containers in a cool, well-ventilated area.Sources of ignition, such as smoking and open flames, areprohibited where this chemical is used, handled, or stored ina manner that could create a potential fire or explosion hazard. Wherever this chemical is used, handled, manufactured,or stored, use explosion-proof electrical equipment and fittings. See OSHA Standard 1910.104 and NFPA 43A Codefor the Storage of Liquid and Solid Oxidizers for detailedhandling and storage regulations.
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
