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Barium nitrate

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Barium nitrate
barium nitrate
Names
Other names
Barium dinitrate,
, barium salt
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.030.006 Edit this at Wikidata
RTECS number
  • CQ9625000
  • InChI=1S/Ba.2NO3/c;2*2-1(3)4/q+2;2*-1 checkY
    Key: IWOUKMZUPDVPGQ-UHFFFAOYSA-N checkY
  • InChI=1/Ba.2NO3/c;2*2-1(3)4/q+2;2*-1
    Key: IWOUKMZUPDVPGQ-UHFFFAOYAA
  • [Ba+2].[O-][N+]([O-])=O.[O-][N+]([O-])=O
Properties
Ba(NO3)2
Molar mass 261.37 g/mol
Appearance white crystals
Density 3.24 g/cm3
Melting point 590 °C (decomp.)
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
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 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. hydrogen peroxideSpecial hazards (white): no code
3
0
3
Lethal dose or concentration (LD, LC):
355 mg/kg (oral, rat)
Supplementary data page
Barium nitrate (data page)
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
checkY verify (what is checkY☒N ?)

Barium nitrate with chemical formula Ba(NO3)2 is a salt 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 and should be handled with care. It occurs naturally as the rare mineral nitrobarite.

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. It is also used in the manufacturing process of barium oxide, the vacuum tube industry and for green fire in pyrotechnics.

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. 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. [1]

Barium nitrate 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.[2]

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.

References

  1. ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0070494398
  2. ^ Barium Nitrate