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Iron(III) nitrate, or ferric nitrate, is the name used for a series of inorganic compounds with the formula Fe(NO 3) 3. (H 2 O) n. Most common is the nonahydrate Fe(NO 3) 3. (H 2 O) 9. The hydrates are all pale colored, water-soluble paramagnetic salts.
Fe 2 O 3 + 3 CO → 2 Fe + 3 CO 2. Another redox reaction is the extremely exothermic thermite reaction with aluminium. [17] 2 Al + Fe 2 O 3 → 2 Fe + Al 2 O 3. This process is used to weld thick metals such as rails of train tracks by using a ceramic container to funnel the molten iron in between two sections of rail.
3 + 2 H 2 O ↔ FeOOH + 3 HCl. Therefore, the compound can also be obtained by the decomposition of acidic solutions of iron(III) chloride held near the boiling point for days or weeks: [14] FeCl 3 + 2 H 2 O → FeOOH (s) + 3 HCl (g) (The same process applied to iron(III) nitrate Fe(NO 3) 3 or perchlorate Fe(ClO 4) 3 solutions yields instead ...
Pourbaix diagram of iron. [1] The Y axis corresponds to voltage potential. In electrochemistry, and more generally in solution chemistry, a Pourbaix diagram, also known as a potential/pH diagram, E H –pH diagram or a pE/pH diagram, is a plot of possible thermodynamically stable phases (i.e., at chemical equilibrium) of an aqueous electrochemical system.
Iron(II) nitrate can be produced in multiple ways, such as the reaction of iron metal with cold dilute nitric acid: . 3 Fe + 8 HNO 3 + 12 H 2 O → 3 Fe(NO 3) 2 (H 2 O) 6 + 2 NO. If this reaction is conducted below -10 °C, nonahydrate is produced.
The various crystalline forms of Fe 2 (SO 4) 3 (H 2 O) n are well-defined, often by X-ray crystallography. The nature of the aqueous solutions is often less certain, but aquo-hydroxo complexes such as [Fe(H 2 O) 6] 3+ and [Fe(H 2 O) 5 (OH)] 2+ are often assumed. [4] Regardless, all such solids and solutions feature ferric ions, each with five ...
Ammonium iron(II) sulfate, or Mohr's salt, is the inorganic compound with the formula (NH 4) 2 SO 4 ·Fe(SO 4)·6H 2 O. Containing two different cations, Fe 2+ and NH + 4, it is classified as a double salt of ferrous sulfate and ammonium sulfate. It is a common laboratory reagent because it is readily crystallized, and crystals resist oxidation ...
Iron(II) complexes are less stable than iron(III) complexes but the preference for O-donor ligands is less marked, so that for example [Fe(NH 3) 6] 2+ is known while [Fe(NH 3) 6] 3+ is not. They have a tendency to be oxidized to iron(III) but this can be moderated by low pH and the specific ligands used.