Barium nitrate
































































































































































Barium nitrate

barium nitrate

Barium nitrate.png
Names
Other names
Barium dinitrate,
, barium salt

Identifiers

CAS Number

  • 10022-31-8 ☑Y

3D model (JSmol)
  • Interactive image

ChemSpider

  • 23184 ☑Y

ECHA InfoCard
100.030.006


PubChem CID
  • 24798

RTECS number
 CQ9625000

UNII

  • MDC5SW56XC ☒N


CompTox Dashboard (EPA)
  • DTXSID8049200 Edit this at Wikidata




Properties

Chemical formula

 Ba(NO3)2

Molar mass
 261.337 g/mol
Appearance
 white, lustrous crystals

Odor
 odorless

Density
 3.24 g/cm3

Melting point
 592 °C (1,098 °F; 865 K) (decomposes)

Solubility in water

 4.95 g/100 mL (0 °C)
10.5 g/100 mL (25 °C)
34.4 g/100 mL (100 °C)

Solubility
 insoluble in alcohol


Magnetic susceptibility (χ)

 -66.5·10−6 cm3/mol


Refractive index (nD)

 1.5659
Structure

Crystal structure

 cubic
Hazards

Safety data sheet
See: data page


EU classification (DSD) (outdated)

 Harmful (Xn)

R-phrases (outdated)
R20/22

S-phrases (outdated)
(S2), S28

NFPA 704


Flammability code 0: Will not burn. E.g., water
Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas
Reactivity code 3: Capable of detonation or explosive decomposition but requires a strong initiating source, must be heated under confinement before initiation, reacts explosively with water, or will detonate if severely shocked. E.g., fluorine
Special hazards (white): no codeNFPA 704 four-colored diamond


0


3


3

Flash point
 noncombustible[1]
Lethal dose or concentration (LD, LC):


LD50 (median dose)

 355 mg/kg (oral, rat)[citation needed]
187 mg/kg (rat, oral)[2]


LDLo (lowest published)

 79 mg Ba/kg (rabbit, oral)
421 mg Ba/kg (dog, oral)[2]
US health exposure limits (NIOSH):


PEL (Permissible)

 TWA 0.5 mg/m3[1]


REL (Recommended)

 TWA 0.5 mg/m3[1]


IDLH (Immediate danger)

 50 mg/m3[1]

Supplementary data page

Structure and
properties
Refractive index (n),
Dielectric constant (εr), etc.

Thermodynamic
data
Phase behaviour
solid–liquid–gas

Spectral data
UV, IR, NMR, MS

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).


☒N verify (what is ☑Y☒N ?)

Infobox references

Barium nitrate is the inorganic compound with the chemical formula Ba(NO3)2. It, like most barium salts, is colorless, toxic, and water-soluble. It burns with a green flame and is an oxidizer; the compound is commonly used in pyrotechnics.[3]




Contents






  • 1 Manufacture, occurrence, and reactions


  • 2 Applications


    • 2.1 Military




  • 3 Safety


  • 4 References





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.[3]


It occurs naturally as the very rare mineral nitrobarite.[4]


At elevated temperatures, barium nitrate decomposes to barium oxide:


2Ba(NO3)2 → 2BaO + 4NO2 + 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, TNT and 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-TH3, used in military thermite grenades. Barium nitrate was also a primary ingredient in the "SR 365" incendiary charge used by the British in the De Wilde incendiary ammunition with which they armed their interceptor fighters, such as the Hawker Hurricane and Supermarine Spitfire, during the Battle of Britain.[5] It is also used in the manufacturing process of barium oxide, the vacuum tube industry and for green fire in pyrotechnics.



Safety


Like all soluble barium compounds, barium nitrate is toxic by ingestion or inhalation.[6]


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 mg/m3 over an eight-hour time-weighted average.[7]



References





  1. ^ abcd NIOSH Pocket Guide to Chemical Hazards. "#0046". National Institute for Occupational Safety and Health (NIOSH)..mw-parser-output cite.citation{font-style:inherit}.mw-parser-output .citation q{quotes:"""""""'""'"}.mw-parser-output .citation .cs1-lock-free a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/6/65/Lock-green.svg/9px-Lock-green.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .citation .cs1-lock-limited a,.mw-parser-output .citation .cs1-lock-registration a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/d/d6/Lock-gray-alt-2.svg/9px-Lock-gray-alt-2.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .citation .cs1-lock-subscription a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/a/aa/Lock-red-alt-2.svg/9px-Lock-red-alt-2.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration{color:#555}.mw-parser-output .cs1-subscription span,.mw-parser-output .cs1-registration span{border-bottom:1px dotted;cursor:help}.mw-parser-output .cs1-ws-icon a{background:url("//upload.wikimedia.org/wikipedia/commons/thumb/4/4c/Wikisource-logo.svg/12px-Wikisource-logo.svg.png")no-repeat;background-position:right .1em center}.mw-parser-output code.cs1-code{color:inherit;background:inherit;border:inherit;padding:inherit}.mw-parser-output .cs1-hidden-error{display:none;font-size:100%}.mw-parser-output .cs1-visible-error{font-size:100%}.mw-parser-output .cs1-maint{display:none;color:#33aa33;margin-left:0.3em}.mw-parser-output .cs1-subscription,.mw-parser-output .cs1-registration,.mw-parser-output .cs1-format{font-size:95%}.mw-parser-output .cs1-kern-left,.mw-parser-output .cs1-kern-wl-left{padding-left:0.2em}.mw-parser-output .cs1-kern-right,.mw-parser-output .cs1-kern-wl-right{padding-right:0.2em}


  2. ^ ab "Barium (soluble compounds, as Ba)". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).


  3. ^ ab Kresse, Robert; Baudis, Ulrich; Jäger, Paul; Riechers, H. Hermann; Wagner, Heinz; Winkler, Jocher; Wolf, Hans Uwe (2007). "Barium and Barium Compounds". In Ullman, Franz (ed.). Ullmann's Encyclopedia of Industrial Chemistry. Wiley-VCH. doi:10.1002/14356007.a03_325.pub2.


  4. ^ Mindat, http://www.mindat.org/min-2918.html


  5. ^ Williams, Anthony G; Emmanuel Gustin (2004). "THE BATTLE OF BRITAIN: ARMAMENT OF THE COMPETING FIGHTERS". Flying Guns: World War 2. Crowood Press. Archived from the original on 5 January 2013. Retrieved 23 December 2012. 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.


  6. ^ Barium Nitrate


  7. ^ CDC - NIOSH Pocket Guide to Chemical Hazards




























































































































































  • v

  • t

  • e


Salts and covalent derivatives of the nitrate ion


HNO3


He

LiNO3
Be(NO3)2
B(NO
3)−
4
 C
NO−
3,
NH4NO3
 O
FNO3
 Ne

NaNO3
Mg(NO3)2
Al(NO3)3
 Si
 P
 S
ClONO2
 Ar

KNO3
Ca(NO3)2
Sc(NO3)3
Ti(NO3)4
VO(NO3)3
Cr(NO3)3
Mn(NO3)2
Fe(NO3)3,
Fe(NO3)2
Co(NO3)2,
Co(NO3)3
Ni(NO3)2
Cu(NO3)2
Zn(NO3)2
Ga(NO3)3
 Ge
 As
 Se
 Br
 Kr

RbNO3
Sr(NO3)2
Y(NO3)3
Zr(NO3)4
 Nb
 Mo
 Tc
 Ru
 Rh
Pd(NO3)2
AgNO3
Cd(NO3)2
 In
 Sn
Sb(NO3)3
 Te
 I
Xe(NO3)2

CsNO3
Ba(NO3)2
  
 Hf
 Ta
 W
 Re
 Os
 Ir
 Pt
 Au
Hg2(NO3)2,
Hg(NO3)2
Tl(NO3)3,
TlNO3
Pb(NO3)2
Bi(NO3)3
BiO(NO3)
 Po
 At
 Rn

FrNO3
Ra(NO3)2
  
 Rf
 Db
 Sg
 Bh
 Hs
 Mt
 Ds
 Rg
 Cn
 Nh
 Fl
 Mc
 Lv
 Ts
 Og

↓


La(NO3)3
Ce(NO3)3,
Ce(NO3)4
 Pr
Nd(NO3)3
 Pm
 Sm
Eu(NO3)3
Gd(NO3)3
Tb(NO3)3
 Dy
 Ho
 Er
 Tm
 Yb
 Lu

Ac(NO3)3
Th(NO3)4
 Pa
UO2(NO3)2
 Np
 Pu
 Am
 Cm
 Bk
 Cf
 Es
 Fm
 Md
 No
 Lr







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