Barium nitrite

Barium nitrite
Names
	Preferred IUPAC name Barium nitrite
Identifiers
CAS Number	13465-94-6 (anhydrous); 7787-38-4 (monohydrate);
3D model (JSmol)	Interactive image;
ChemSpider	145952;
ECHA InfoCard	100.033.358
EC Number	236-709-9;
PubChem CID	166820;
UNII	5N5G361962;
CompTox Dashboard (EPA)	DTXSID30890698 ;
	InChI InChI=1S/Ba.2HNO2/c;22-1-3/h;2(H,2,3)/q+2;;/p-2 Key: GJTDJAPHKDIQIQ-UHFFFAOYSA-L;
	SMILES N(=O)[O-].N(=O)[O-].[Ba+2];
Properties
Chemical formula	Ba(NO2)2
Molar mass	229.34 g/mol
Appearance	white (anhydrous); white to yellowish (monohydrate)
Density	3.234 g/cm3 (anhydrous); 3.173 g/cm3 (monohydrate)
Melting point	267 °C (anhydrous) 217 °C decomposes (monohydrate)
Solubility in water	anhydrous; 675 g/L (20 °C)monohydrate; 548 g/L (0 °C); 3190 g/L (100 °C)
Solubility	anhydrous; slightly soluble in ethanolmonohydrate; soluble in ethanol
Hazards
	Occupational safety and health (OHS/OSH):
Main hazards	Toxic
	GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H302, H332
Precautionary statements	P261, P264, P270, P271, P301+P317, P304+P340, P317, P330, P501
Related compounds
Related compounds	Sodium nitrite; Potassium nitrite;
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

Barium nitrite is a chemical compound with the formula Ba(NO₂)₂, the nitrous acid salt of barium. It is a water-soluble white to yellowish powder.^[1] It is used to prepare other metal nitrites, such as lithium nitrite.

Synthesis

Barium nitrite can be prepared by reacting barium nitrate with lead metal sponge, or by reaction of lead nitrite with barium chloride.^[2]

The monohydrate can be crystallized from a stoichiometric solution of barium chloride and sodium nitrite.^[1]

References

^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l Perry, Dale L. (2016-04-19). Handbook of Inorganic Compounds. CRC Press. p. 54. ISBN 978-1-4398-1462-8.
^ Schlessinger GG (1962). Inorganic laboratory preparations. pp. 34–35.

[handbook-1] ^ ^a ^b ^c ^d ^e ^f ^g ^h ⁱ ^j ^k ^l Perry, Dale L. (2016-04-19). Handbook of Inorganic Compounds. CRC Press. p. 54. ISBN 978-1-4398-1462-8.

[2] Schlessinger GG (1962). Inorganic laboratory preparations. pp. 34–35.

[1]

[2]