Concentrated nitric acid oxidizes iron(II) nitrate into iron(III) nitrate: 3Fe(NO 3) 2 + 4HNO 3 → 3Fe(NO 3) 3 + NO + 2H 2O Uses A solution of iron(II) nitrate is much more stable, decomposing at 107 ☌ to iron(III), with the presence of nitric acid lowering the decomposition temperature. The hexahydrate melts at 60 ☌ and then decomposes at 61 ☌ into iron(III) oxide rather than iron(II) oxide.
If the compound is used in situ, the compound is produced by the reaction of iron(II) chloride and calcium nitrate: FeCl 2 + Ca(NO 3) 2 → Fe(NO 3) 2 + CaCl 2 Reactions The solution of the iron(II) nitrate- hydrazine complex is produced by the reaction of hydrazine nitrate and ferric nitrate at 40 ☌ with copper(II) nitrate as a catalyst: 4 Fe(NO 3) 3 + N 2H 5NO 3 → 4 Fe(NO 3) 2 + N 2 + 4HNO 3 A solution of iron(II) nitrate is produced by the ion-exchange reaction of iron(II) sulfate and barium nitrate, producing a concentration of up to 1.5 M due to the limited solubility of barium nitrate. Reacting iron(II) sulfate and lead nitrate under dilute ethanol and then evaporating the solution leads to the formation of the green crystals of the hexahydrate. The above reaction can also co-produce ferric nitrate. It readily releases water to give the hexahydrate. If this reaction is conducted below -10 ☌, nonahydrate is produced. Iron(II) nitrate can be produced in multiple ways, such as the reaction of iron metal with cold dilute nitric acid:ģ Fe + 8 HNO 3 + 12 H 2O → 3 Fe(NO 3) 2(H 2O) 6 + 2 NO The solubility graph of iron(II) nitrate Production Both n+ complexes are high spin, which results in pale colors, paramagnetism, and weak Fe-O bonds. The Fe-O distances are longer for 2+ (2.13 Å) than for the ferric analogue 3+ (1.99 Å). Nonetheless, the nature of the aquo complex 2+ is well known and relatively insensitive to the anion. xH 2O has been determined by X-ray crystallography.The salt is soluble in water serves as a ready source of ferrous ions.
It is commonly encountered as the green hexahydrate, Fe(NO 3) 2♶H 2O, which is a metal aquo complex, however it is not commercially available unlike iron(III) nitrate due to its instability to air. Iron(II) nitrate is the nitrate salt of iron(II).
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