Iron(II) nitrate

Iron(II) nitrate
Names
	Other names Ferrous nitrate;
Identifiers
CAS Number	14013-86-6;
ChemSpider	7991154;
PubChem CID	9815404;
CompTox Dashboard (EPA)	DTXSID70431140 ;
Properties
Chemical formula	Fe(NO3)2
Molar mass	179.86 g/mol[1]
Appearance	Green crystals
Melting point	60 °C (140 °F; 333 K)[2] (decomposes)
Solubility in water	87.525 g/100 ml
Structure
Crystal structure	Orthorhombic[3]
Hazards
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	428 mg/kg (subcutaneous, rabbit)[4]
Related compounds
Other anions	Iron(II) phosphate
Other cations	Manganese(II) nitrate; Cobalt(II) nitrate
Related compounds	Iron(III) nitrate
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
	Infobox references

Iron(II) nitrate is the nitrate of iron that is a green solid that forms the hexahydrate, Fe(NO₃)₂·6H₂O. When heated it is oxidized to iron(III) nitrate.

The solubility graph of iron(II) nitrate

Production

Iron(II) nitrate can be produced in multiple ways such as the reaction of iron metal with cold dilute nitric acid:

3Fe + 8HNO₃ → 3Fe(NO₃)₂ + 4H₂O + 2NO

If this reaction is done below -10 °C, the nonahydrate is produced which decomposes back to the hexahydrate.[5]

However, the above reaction can also produce ferric nitrate. For a purer product, it can also be produced by the reaction of hydrazine nitrate and ferric nitrate at 40 °C:[6]

4Fe(NO₃)₃ + N₂H₅NO₃ → 4Fe(NO₃)₂ + N₂ + 4HNO₃

To prevent from the backward reaction from happening, copper(II) nitrate is added.[6]

References

"Iron nitrate". PubChem. PubChem. Retrieved 14 February 2021.
Lide, David, ed. (2004). "4". CRC Handbook of Chemistry and Physics (Hardcover) (85th ed.). Taylor & Francis. p. 62.
Herman Francis Mark; Anthony Standen (1963). Standen, Anthony (ed.). Encyclopedia of Chemical Technology. Interscience Publishers. Retrieved 16 February 2021.
Registry of Toxic Effects of Chemical Substances. U.S. Department of Health and Human Services, Public Health Service, Centers for Disease Control, National Institute for Occupational Safety and Health. 1981. p. 548. Retrieved 16 February 2021. |first1= missing |last1= (help)
"Iron(II) nitrate". Chemical Book. Chemical Book. Retrieved 14 February 2021.
D. G. Karraker (1981). "Cu(II) - Catalyzed Hydrazine Reduction of Ferric Nitrate" (PDF). United States Department of Energy. Cite journal requires |journal= (help)

This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.

[1] "Iron nitrate". PubChem. PubChem. Retrieved 14 February 2021.

[crc-2] Lide, David, ed. (2004). "4". CRC Handbook of Chemistry and Physics (Hardcover) (85th ed.). Taylor & Francis. p. 62.

[3] Herman Francis Mark; Anthony Standen (1963). Standen, Anthony (ed.). Encyclopedia of Chemical Technology. Interscience Publishers. Retrieved 16 February 2021.

[4] Registry of Toxic Effects of Chemical Substances. U.S. Department of Health and Human Services, Public Health Service, Centers for Disease Control, National Institute for Occupational Safety and Health. 1981. p. 548. Retrieved 16 February 2021. |first1= missing |last1= (help)

[chembookfen2o6-5] "Iron(II) nitrate". Chemical Book. Chemical Book. Retrieved 14 February 2021.

[syn-6] D. G. Karraker (1981). "Cu(II) - Catalyzed Hydrazine Reduction of Ferric Nitrate" (PDF). United States Department of Energy. Cite journal requires |journal= (help)