| IUPAC name
| Preferred IUPAC name
| Other names
Nitrous acid, barium salt
| Ba(NO2)2 (anhydrous)|
|Molar mass|| 229.34 g/mol (anhydrous)|
247.35 g/mol (monohydrate)
|Appearance||Yellowish crystalline solid|
|Density||3.137 g/cm3 (20 °C)|
|Melting point|| 217 °C (423 °F; 490 K) (anhydrous)|
115 °C (239 °F; 388 K) (monohydrate)
|Boiling point||217 °C (423 °F; 490 K) (decomposition)|
| 67.5 g/100 ml (20 °C)|
300 g/100 ml (100 °C)
|Solubility||Soluble in alcohol|
|Solubility in ethanol 80%||1.24 g/100 ml (20 °C)|
|Vapor pressure||~0 mmHg|
Std enthalpy of
|Safety data sheet||Sigma-Aldrich (monohydrate)|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Barium nitrite is a chemical compound, the nitrous acid salt of barium. It has the chemical formula Ba(NO2)2. It is often encountered as monohydrate and like all soluble barium salts it is toxic if consumed.
Barium nitrite can be used to prepare almost any transition metal nitrite, via double displacement with their sulfate.
Barium nitrite is a yellowish solid, soluble in water.
Barium nitrite is sold by chemical suppliers.
Barium nitrite can be prepared by boiling a solution of barium nitrate with lead metal sponge for 2 hours. Lead metal sponge can be made by reducing a solution of lead(II) acetate with magnesium or zinc metal. Carbon dioxide is passed through the solution to precipitate any insoluble wastes.
Another route involves adding a solution of lead(II) nitrite to a solution of barium chloride, then cooled. The insoluble lead(II) chloride is filtered off and the barium nitrite is carefully recrystallized and purified.
- Make transition metal nitrites
- Make pure nitrous acid (DANGER! Decomposes immediately!)
- Compound collecting
Barium nitrite is very toxic if ingested or inhaled, as both barium and the nitrite ion are toxic.
In closed plastic or glass bottles.
Barium nitrite should be converted to barium sulfate by adding a soluble sulfate salt (NOT AMMONIUM SULFATE!), like sodium sulfate, then the nitrite solution can be either recycled or further converted to the less harmful sodium nitrate by oxidizing it with hydrogen peroxide.
- Справочник химика. - Т. 2. - Л.-М.: Химия, 1964 (Chemist's Handbook. - T. 2.- L.-M .: Chemistry, 1964)
- Seidell A. Solubilities of inorganic and metal organic compounds. - 3ed., vol.1. - New York: D. Van Nostrand Company, 1940
- Inorganic laboratory preparations, by G. G. Schlessinger, 34-35, 1962