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Lawrencite, (Fe,Ni)Cl 2, is the natural counterpart, and a typically (though rarely occurring) meteoritic mineral. [14] The natural form of the dihydrate is rokühnite - a very rare mineral. [ 15 ] Related, but more complex (in particular, basic or hydrated) minerals are hibbingite , droninoite and kuliginite .
Iron (II) hydroxide or ferrous hydroxide is an inorganic compound with the formula Fe(OH) 2. It is produced when iron (II) salts, from a compound such as iron(II) sulfate, are treated with hydroxide ions. Iron(II) hydroxide is a white solid, but even traces of oxygen impart a greenish tinge. The air-oxidised solid is sometimes known as "green ...
The sulfate salt [Fe(bipy) 3]SO 4 is produced by combining ferrous sulfate with excess bipy in aqueous solution. This result illustrates the preference of Fe(II) for bipyridine vs water. Addition of cyanide to this solution precipitates solid Fe(bipy) 2 (CN) 2. [2]
Iron(II) chloride tetrahydrate, FeCl 2 ·4H 2 O. In chemistry, iron(II) refers to the element iron in its +2 oxidation state.The adjective ferrous or the prefix ferro-is often used to specify such compounds, as in ferrous chloride for iron(II) chloride (FeCl 2).
The active ingredient is the [Fe(o-phen) 3] 2+ ion, which is a chromophore that can be oxidized to the ferric derivative [Fe(o-phen) 3] 3+. The potential for this redox change is +1.06 volts in 1 M H 2 SO 4. It is a popular redox indicator for visualizing oscillatory Belousov–Zhabotinsky reactions.
Prussian blue or "ferric ferrocyanide", Fe 4 [Fe(CN) 6] 3, is an old and well-known iron-cyanide complex, extensively used as pigment and in several other applications. Its formation can be used as a simple wet chemistry test to distinguish between aqueous solutions of Fe 2+ and Fe 3+ as they react (respectively) with potassium ferricyanide and ...
The [Fe(EDTA)(H 2 O)] − anion has been crystallized with many cations, e.g., the trihydrate Na[Fe(EDTA)(H 2 O)]. 2H 2 O. [3] The salts as well as the solutions are yellow-brown. Provided the nutrient solution in which the [Fe(EDTA)(H 2 O)] − complex will be used has a pH of at least 5.5, all the uncomplexed iron, as a result of incomplete ...
2 [fe(h 2 o) 4 (oh) 2] + ⇌ [fe 2 (h 2 o) 8 (oh) 2] + 2 + 2 h 2 o The aquo ligands on iron(III) complexes are labile. This behavior is visualized by the color change brought about by reaction with thiocyanate to give a deep red thiocyanate complex .