Editing Barium nitrate

{{chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 442345749
| Name = Barium nitrate
| ImageFile = Dusičnan_barnatý.JPG
<!-- | ImageSize= -->
| ImageName = barium nitrate
| ImageFile1 = barium nitrate.png
| OtherNames = Barium dinitrate, barium salt
|Section1={{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 23184
| ChEBI = 190440
| InChI = 1/Ba.2NO2/c;2*2-1(3)4/q+2;2*-1
| SMILES = [Ba+2].[O-][N+]([O-])=O.[O-][N+]([O-])=O
| InChIKey = IWOUKMZUPDVPGQ-UHFFFAOYAA
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/Ba.2NO3/c;2*2-1(3)4/q+2;2*-1
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = IWOUKMZUPDVPGQ-UHFFFAOYSA-N
| CASNo = 10022-31-8
| CASNo_Ref = {{cascite|correct|CAS}}
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = MDC5SW56XC
| EC_number = 233-020-5
| UNNumber = 1446
| RTECS = CQ9625000
| PubChem = 24798
| ChEMBL = 3184584
  }}
|Section2={{Chembox Properties
| Formula = Ba(NO<sub>3</sub>)<sub>2</sub>
| MolarMass = 261.337 g/mol
| Appearance = white, lustrous crystals
| Odor = odorless
| Density = 3.24 g/cm<sup>3</sup>
| MeltingPtC = 592
| MeltingPt_notes = (decomposes)
| BoilingPt =
| Solubility = 4.95 g/100 mL (0 °C) <br> 10.5 g/100 mL (25 °C) <br> 34.4 g/100 mL (100 °C)
| SolubleOther = slightly soluble in [[acetone]], and [[ethanol]]<ref name="crc">{{cite book |author1=John Rumble |title=CRC Handbook of Chemistry and Physics |date=June 18, 2018 |publisher=CRC Press |isbn=978-1138561632 |pages=4–41|edition=99th |language=English}}</ref>
| RefractIndex = 1.5659
| MagSus = −66.5·10<sup>−6</sup> cm<sup>3</sup>/mol
  }}
|Section3={{Chembox Structure
| CrystalStruct = cubic
}}
|Section7={{Chembox Hazards
| GHSPictograms = {{GHS03}}{{GHS06}}{{GHS07}}
| GHSSignalWord = Danger
| HPhrases = {{H-phrases|272|301|302|319|332}}
| PPhrases = {{P-phrases|210|220|221|261|264|270|271|280|301+310|301+312|304+312|304+340|305+351+338|312|321|330|337+313|370+378|405|501}}
| NFPA-H = 3
| NFPA-F = 0
| NFPA-R = 3
| LD50 = 355 mg/kg (oral, rat){{cn|date=August 2015}}<br/>187 mg/kg (rat, oral)<ref name=IDLH>{{IDLH|7440393|Barium (soluble compounds, as Ba)}}</ref>
| PEL = TWA 0.5 mg/m<sup>3</sup><ref name=PGCH>{{PGCH|0046}}</ref> 
| REL = TWA 0.5 mg/m<sup>3</sup><ref name=PGCH/>
| IDLH = 50 mg/m<sup>3</sup><ref name=PGCH/>
| FlashPt = noncombustible<ref name=PGCH/>
| LDLo = 79 mg Ba/kg (rabbit, oral)<br/>421 mg Ba/kg (dog, oral)<ref name=IDLH/>
 }}
}}
'''Barium nitrate''' is the [[inorganic compound]] with the [[chemical formula]] [[Barium|Ba]]([[nitrate|NO<sub>3</sub>]])<sub>2</sub>.  It, like most barium salts, is colorless, toxic, and water-soluble.  It [[Colored flame|burns with a green flame]] and is an oxidizer; the compound is commonly used in [[pyrotechnics]].<ref name="Ullman2005">{{cite book |author=Kresse, Robert |author2=Baudis, Ulrich |author3=Jäger, Paul |author4=Riechers, H. Hermann |author5=Wagner, Heinz |author6=Winkler, Jocher |author7=Wolf, Hans Uwe |chapter=Barium and Barium Compounds |editor=Ullman, Franz |title=Ullmann's Encyclopedia of Industrial Chemistry |date=2007 |publisher=Wiley-VCH |doi=10.1002/14356007.a03_325.pub2|isbn=978-3527306732 }}</ref>

==Manufacture, occurrence, and reactions==
Barium nitrate is manufactured by two processes that start with the main source material for barium, the carbonate. The first involves dissolving [[barium carbonate]] in [[nitric acid]], allowing any iron impurities to precipitate, then filtered, evaporated, and crystallized. The second requires combining [[barium sulfide]] with nitric acid.<ref name="Ullman2005"/>

It occurs naturally as the very rare mineral nitrobarite.<ref>Mindat, http://www.mindat.org/min-2918.html</ref><ref>{{Cite web|url=https://www.ima-mineralogy.org/Minlist.htm|title=List of Minerals|date=21 March 2011}}</ref>

At elevated temperatures, barium nitrate decomposes to [[barium oxide]]:
:{{chem2 | 2 Ba(NO3)2 -> 2 BaO + 4 NO2 + O2 }}

==Applications==
Barium nitrate is used in the production of BaO-containing materials.
===Military===
Although no longer produced, [[Baratol]] is an explosive composed of barium nitrate, [[Trinitrotoluene|TNT]] and [[binder (material)|binder]]; the high density of barium nitrate results in baratol being quite dense as well.  Barium nitrate mixed with [[aluminium powder]], a formula for [[flash powder]], is highly explosive. It is mixed with [[thermite]] to form [[Thermate|Thermate-TH3]], used in military thermite grenades. Barium nitrate was also a primary ingredient in the "SR 365" [[Incendiary device|incendiary charge]] used by the British in the ''De Wilde'' [[incendiary ammunition]] with which they armed their [[Interceptor aircraft|interceptor fighters]], such as the [[Hawker Hurricane]] and [[Supermarine Spitfire]], during the [[Battle of Britain]].<ref>{{cite web|last=Williams |first=Anthony G |title=THE BATTLE OF BRITAIN: ARMAMENT OF THE COMPETING FIGHTERS |url=http://www.quarry.nildram.co.uk/BoB.htm |work=Flying Guns: World War 2 |publisher=Crowood Press |access-date=23 December 2012 |author2=Emmanuel Gustin |date=2004 |quote=The B. Mk VI 'De Wilde' incendiary (named after the original Belgian inventor but in fact completely redesigned by Major Dixon), which contained 0.5 grams of SR 365 (a composition including barium nitrate which ignited on impact with the target) was twice as effective as these, scoring one in five. |url-status=dead |archive-url=https://web.archive.org/web/20130105162948/http://www.quarry.nildram.co.uk/BoB.htm |archive-date=5 January 2013 }}</ref>  It is also used in the manufacturing process of [[barium oxide]], the [[vacuum tube]] industry and for green fire in [[pyrotechnic]]s.

==Safety==

Like all soluble barium compounds, barium nitrate is [[toxic]] by ingestion or inhalation.<ref>[http://hazard.com/msds/mf/baker/baker/files/b0432.htm Barium Nitrate<!-- Bot generated title -->]</ref>

Solutions of [[sulfate]] salts such as [[Epsom salts]] or [[sodium sulfate]] may be given as first aid for barium poisoning, as they precipitate the barium as the insoluble (and non-toxic) [[barium sulfate]].

Inhalation may also cause irritation to the respiratory tract.

While skin or eye contact is less harmful than ingestion or inhalation, it can still result in irritation, itching, redness, and pain.

The [[Occupational Safety and Health Administration]] and the [[National Institute for Occupational Safety and Health]] have set occupational exposure limits at 0.5&nbsp;mg/m<sup>3</sup> over an eight-hour time-weighted average.<ref name=PGCH/>

==References==
{{reflist}}

{{Barium compounds}}
{{nitrates}}

{{DEFAULTSORT:Barium Nitrate}}
[[Category:Barium compounds]]
[[Category:Nitrates]]
[[Category:Nitrate minerals]]
[[Category:Pyrotechnic oxidizers]]
[[Category:Pyrotechnic colorants]]
[[Category:Oxidizing agents]]