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 = __ Li+ __ N __ 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 = LiNO3
| MolarMass = 68.946 g/mol
| Appearance = White to light yellow solid
| Density = 2.38 g/cm3
| MeltingPtC = 255
| BoilingPtC = 600
| BoilingPt_notes = (decomposes)
| Solubility = 52.2 g/100 mL (20 °C)
90 g/100 mL (28 °C)
234 g/100 mL (100 °C)
| SolubleOther = soluble in ethanol, methanol, pyridine, ammonia, acetone
| RefractIndex = 1.735Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, {{ISBN|0-07-049439-8}}.{{page needed|date=December 2017}}
| MagSus = −62.0·10−6 cm3/mol (+3 H2O)
}}
|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
Potassium nitrate
Rubidium nitrate
Caesium nitrate
| OtherCompounds = Lithium sulfate
Lithium chloride
}}
}}
Lithium nitrate is an inorganic compound with the formula LiNO3. It is the lithium 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.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}}.
It is made by treating lithium carbonate or lithium hydroxide with nitric acid.
Uses
=Thermal storage=
The hydrated form, lithium nitrate trihydrate, has an extremely high specific heat of fusion, {{val|287|7|u=J/g}},{{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 }} and hence can be used for thermal energy storage at its melt temperature of 303.3 K.{{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 }}
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.{{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 }}
Synthesis
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.{{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}} 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.{{cite web|title=Material Safety Data Sheet|url=http://www.sigmaaldrich.com/catalog/DisplayMSDSContent.do|publisher=Sigma-Aldrich Catalog|access-date=April 12, 2012}}
When exposed to the skin, eyes, and mucous membranes, lithium nitrate can cause irritation to these areas.{{cite web|title=Chemical Datasheet|url=http://cameochemicals.noaa.gov/chemical/3774|publisher=CAMEO Chemicals|access-date=April 26, 2012}}
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 }}
- {{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:Deliquescent materials
Category:Pyrotechnic oxidizers