Barium nitrate

Barium nitrate
Names
Other names
Barium dinitrate,
, barium salt
Identifiers
10022-31-8 YesY
3D model (Jmol) Interactive image
ChemSpider 23184 YesY
ECHA InfoCard 100.030.006
PubChem 24798
RTECS number CQ9625000
UNII MDC5SW56XC N
Properties
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)
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
1.5659
Structure
cubic
Hazards
Safety data sheet See: data page
Harmful (Xn)
R-phrases R20/22
S-phrases (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):
355 mg/kg (oral, rat)
187 mg/kg (rat, oral)[2]
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
Refractive index (n),
Dielectric constant (εr), etc.
Thermodynamic
data
 Phase behaviour
solid–liquid–gas
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 YesYN ?)
Infobox references

Barium nitrate with chemical formula Ba(NO3)2 is a salt composed of barium and the nitrate ion.

Barium nitrate exists as a white solid at room temperature. It is soluble in water, and like other soluble barium compounds, is toxic. It occurs naturally as the very rare mineral nitrobarite.[3] Barium nitrate's properties make it suitable for use in various military applications, including thermite grenades and incendiary ammunition.

Manufacture

Barium nitrate is manufactured by one of two processes. The first involves dissolving small chunks of barium carbonate in nitric acid, allowing any iron impurities to precipitate, then filtered, evaporated, and crystallized. The second requires combining barium chloride with a heated solution of sodium nitrate, causing barium nitrate crystals to separate from the mixture.

Reactions

At elevated temperatures, barium nitrate decomposes to barium oxide, nitrogen dioxide, and oxygen:

2Ba(NO3)2 + heat → 2BaO + 4NO2 + O2

In an atmosphere of nitric oxide, thermal decomposition produces barium nitrite (Ba(NO2)2). Reactions with soluble metal sulfates or sulfuric acid yield barium sulfate. Many insoluble barium salts, such as the carbonate, oxalate and phosphate of the metal, are precipitated by similar double decomposition reactions. Barium nitrate is an oxidizer and reacts vigorously with common reducing agents. The solid powder, when mixed with many other metals such as aluminium or zinc in their finely divided form, or combined with alloys such as aluminium-magnesium, ignites and explodes on impact.[4]

Applications

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.

Health risks

Like all soluble barium compounds, barium nitrate is toxic by ingestion or inhalation. Symptoms of poisoning include tightness of muscles (especially in the face and neck), vomiting, diarrhea, abdominal pain, muscular tremors, anxiety, weakness, labored breathing, cardiac irregularity, and convulsions. Death may result from cardiac or respiratory failure, and usually occurs a few hours to a few days following exposure to the compound. Barium nitrate may also cause kidney damage.[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. 1 2 3 4 "NIOSH Pocket Guide to Chemical Hazards #0046". National Institute for Occupational Safety and Health (NIOSH).
  2. 1 2 "Barium (soluble compounds, as Ba)". Immediately Dangerous to Life and Health. National Institute for Occupational Safety and Health (NIOSH).
  3. ↑ Mindat, http://www.mindat.org/min-2918.html
  4. ↑ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
  5. ↑ Williams, Anthony G; Emmanuel Gustin (2004). "THE BATTLE OF BRITAIN: ARMAMENT OF THE COMPETING FIGHTERS". Flying Guns: World War 2. Crowood Press. 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
Salts and covalent derivatives of the Nitrate ion
HNO3 He
LiNO3 Be(NO3)2 B(NO3)4− C N 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 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 Zr(NO3)4 Nb Mo Tc Ru Rh Pd(NO3)2 AgNO3 Cd(NO3)2 In Sn Sb 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 Pb(NO3)2 Bi(NO3)3
BiO(NO3)		 Po At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La Ce(NO3)3,
Ce(NO3)4		 Pr Nd Pm Sm Eu Gd(NO3)3 Tb Dy Ho Er Tm Yb Lu
Ac Th Pa UO2(NO3)2 Np Pu Am Cm Bk Cf Es Fm Md No Lr
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