View source for Lithium nitrate

{{Chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 450964959
| ImageFile = lithium nitrate.png
| ImageSize = 150px
| ImageFile1 = File:Lithium-nitrate-unit-cell-3D-balls.png
| ImageSize1 = 
| ImageCaption1 = <span style="color:purple; background:purple;">__</span> [[Lithium|Li]]<sup>+</sup>&emsp;<span style="color:blue;background:blue;">__</span> [[Nitrogen|N]]&emsp;<span style="color:red;background:red;">__</span> [[Oxygen|O]]
| ImageFile2 = Lithium_nitrate.jpg
| IUPACName = 
| OtherNames = 
|Section1={{Chembox Identifiers
| CASNo = 7790-69-4
| CASNo_Ref = {{cascite|correct|CAS}}
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = 68XG6U4533
| PubChem = 10129889
| RTECS = QU9200000
| InChI = 1S/Li.NO3/c;2-1(3)4/q+1;-1
| InChIKey = IIPYXGDZVMZOAP-UHFFFAOYSA-N
| SMILES = [Li+].[N+](=O)([O-])[O-]
| ChemSpiderID_Ref = {{chemspidercite|changed|chemspider}}
| ChemSpiderID = 8305408
| InChI2 = 1/Li.NO3/c;2-1(3)4/q+1;-1
| InChIKey2 = IIPYXGDZVMZOAP-UHFFFAOYAC
| StdInChIKey_Ref = {{stdinchicite|changed|chemspider}}
| StdInChIKey = IIPYXGDZVMZOAP-UHFFFAOYSA-N
 }}
|Section2={{Chembox Properties
| Formula = LiNO<sub>3</sub>
| MolarMass = 68.946 g/mol
| Appearance = White to light yellow solid
| Density = 2.38 g/cm<sup>3</sup>
| MeltingPtC = 255  
| BoilingPtC = 600
| BoilingPt_notes = (decomposes)
| Solubility = 52.2 g/100 mL (20&nbsp;°C) <br> 90 g/100 mL (28&nbsp;°C) <br> 234 g/100 mL (100&nbsp;°C)
| SolubleOther = soluble in [[ethanol]], [[methanol]], [[pyridine]], [[ammonia]], [[acetone]]
| RefractIndex = 1.735<ref>Pradyot Patnaik. ''Handbook of Inorganic Chemicals''. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}}.{{page needed|date=December 2017}}</ref>
| MagSus = −62.0·10<sup>−6</sup> cm<sup>3</sup>/mol (+3 H<sub>2</sub>O)
 }}
|Section4={{Chembox Thermochemistry
| DeltaHf = −7.007 kJ/g or −482.3 kJ/mol
| DeltaHc = 25.5 kJ/mol
| DeltaGf = −389.5 kJ/mol
| Entropy = 105 J/(mol K)
| HeatCapacity = 64 J/(mol K)
 }}
|Section7={{Chembox Hazards
| ExternalSDS = 
| MainHazards = Oxidant, irritant
| NFPA-H = 1
| NFPA-F = 0
| NFPA-R = 0
| NFPA-S = OX
| FlashPt = Non-flammable
| LD50 = 1426 mg/kg (oral, rat)
 }}
|Section8={{Chembox Related
| OtherAnions = 
| OtherCations = [[Sodium nitrate]]<br/>[[Potassium nitrate]]<br/>[[Rubidium nitrate]]<br/>[[Caesium nitrate]]
| OtherCompounds = [[Lithium sulfate]]<br/>[[Lithium chloride]]
 }}
}}

'''Lithium nitrate''' is an [[inorganic compound]] with the formula LiNO<sub>3</sub>. It is the [[lithium]] [[Salt (chemistry)|salt]] of [[nitric acid]] (an [[alkali metal nitrate]]). The salt is [[deliquescent]], absorbing water to form the hydrated form, lithium nitrate trihydrate.  Its eutectics are of interest for heat transfer fluids.<ref name=Ullmann>Wietelmann, Ulrich and Bauer, Richard J. (2005) "Lithium and Lithium Compounds" in ''Ullmann's Encyclopedia of Industrial Chemistry'', Wiley-VCH: Weinheim. {{doi|10.1002/14356007.a15_393}}.</ref>

It is made by treating [[lithium carbonate]] or [[lithium hydroxide]] with [[nitric acid]].

==Uses==
This deliquescent colourless salt is an [[oxidation|oxidizing]] agent used in the manufacture of red-colored [[fireworks]] and [[road flare|flares]].

===Thermal storage===
The [[hydrate]]d form, lithium nitrate trihydrate, has an extremely high [[enthalpy of fusion|specific heat of fusion]], {{val|287|7|u=J/g}},<ref>{{cite journal |doi=10.1021/je3000469 |title=Thermophysical Properties of Lithium Nitrate Trihydrate from (253 to 353) K |journal=Journal of Chemical & Engineering Data |volume=57 |issue=5 |pages=1404–1411 |year=2012 |last1=Shamberger |first1=Patrick J. |last2=Reid |first2=Timothy }}</ref> and hence can be used for thermal energy storage at its melt temperature of 303.3&nbsp;K.<ref>{{cite journal |doi=10.1016/j.solmat.2015.10.029 |title=Salt hydrates as latent heat storage materials:Thermophysical properties and costs |journal=Solar Energy Materials and Solar Cells |volume=145 |issue=3 |pages=255–286 |year=2016 |last1=Kenisarin |first1=Murat |last2=Mahkamov |first2=Khamid }}</ref>

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.<ref>{{cite web | url=http://barbequelovers.com/grills/a-solar-grill-prototype-for-a-greener-tomorrow | title=A Solar Cooker Prototype for a Greener Tomorrow | date=23 March 2011 }}</ref>

==Synthesis==
Lithium nitrate can be synthesized by reacting nitric acid and lithium carbonate.
:Li<sub>2</sub>CO<sub>3</sub> + 2 HNO<sub>3</sub> → 2 LiNO<sub>3</sub> + H<sub>2</sub>O + CO<sub>2</sub>

Generally when forming LiNO<sub>3</sub>, 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.<ref>{{cite web |url=http://www.amasci.net/syntheses/lithium-nitrate-synthesis.php?lang=eng |title=Synthesis database: Lithium nitrate synthesis |publisher=Amateur Science Network |access-date=18 June 2012}}</ref> In order to rid the final product of excess water, the sample is heated.

==Toxicity==
Lithium nitrate can be toxic to the body when ingested by targeting the central nervous system, thyroids, kidneys, and cardio-vascular system.<ref>{{cite web|title=Material Safety Data Sheet|url=http://www.sigmaaldrich.com/catalog/DisplayMSDSContent.do|publisher=Sigma-Aldrich Catalog|access-date=April 12, 2012}}</ref> 
When exposed to the skin, eyes, and mucous membranes, lithium nitrate can cause irritation to these areas.<ref name="autogenerated1">{{cite web|title=Chemical Datasheet|url=http://cameochemicals.noaa.gov/chemical/3774|publisher=CAMEO Chemicals|access-date=April 26, 2012}}</ref>

==Further reading==
*{{cite journal |doi=10.1021/je00040a023 |title=Transport properties of lithium nitrate and calcium nitrate binary solutions in molten acetamide |journal=Journal of Chemical & Engineering Data |volume=30 |issue=2 |pages=208–9 |year=1985 |last1=Berchiesi |first1=Gianfrancesco |last2=Vitali |first2=Giovanni |last3=Amico |first3=Antonio }}
*{{cite book |doi=10.1061/40838(191)53 |chapter=A Case Study Evaluating the Use of Lithium Nitrate to Arrest Alkali-Silica Reaction in an Existing Concrete Pavement |title=Airfield and Highway Pavement |pages=625–35 |year=2006 |last1=Kelly |first1=Michael T |last2=Tuan |first2=Christopher Y |isbn=978-0-7844-0838-4 }}
*{{cite journal |doi=10.1021/jp2120115 |pmid=22309150 |title=Bifurcated Hydrogen Bond in Lithium Nitrate Trihydrate Probed by ab Initio Molecular Dynamics |journal=The Journal of Physical Chemistry A |volume=116 |issue=9 |pages=2147–53 |year=2012 |last1=Muniz-Miranda |first1=Francesco |last2=Pagliai |first2=Marco |last3=Cardini |first3=Gianni |last4=Righini |first4=Roberto |bibcode=2012JPCA..116.2147M |hdl=11380/1258626 |hdl-access=free }}
*{{cite journal |doi=10.1021/ie201295s |title=NO Influence on Catalytic Soot Combustion: Lithium Nitrate and Gold Catalysts |journal=Industrial & Engineering Chemistry Research |volume=51 |issue=3 |pages=1150–7 |year=2012 |last1=Ruiz |first1=María L |last2=Lick |first2=Ileana D |last3=Leguizamón Aparicio |first3=María S |last4=Ponzi |first4=Marta I |last5=Rodriguez-Castellón |first5=Enrique |last6=Ponzi |first6=Esther N }}

==References==
{{reflist}}

==External links==
*[http://ull.chemistry.uakron.edu/erd/chemicals1/7/6673.html Hazardous Chemical Database]{{dead link|date=January 2018 |bot=InternetArchiveBot |fix-attempted=yes }}

{{Lithium compounds}}
{{nitrates}}

[[Category:Nitrates]]
[[Category:Lithium salts]]
[[Category:Deliquescent materials]]
[[Category:Pyrotechnic oxidizers]]
[[Category:Pyrotechnic colorants]]
[[Category:Oxidizing agents]]