...Iron(II)
hydroxide would thus appear to be unstable in neutral
solutions and to possess increasing stability as the
basicity of the medium increases.
The foregoing reasoning led to the attempt to prepare
iron(II) hydroxide from the chloride under such
conditions that the hydroxyl ion concentration was not
allowed to fall below approximately one molal until the chloride ion had been removed. The hydroxide was precipitated from strongly basic solution by the addition of dilute iron(II) chloride to a saturated solution of
sodium hydroxide in an air-free system with vigorous
stirring. The precipitate was repeatedly washed with
molal sodium hydroxide (oxygen and carbonate-free)
until a test for chloride ion with silver nitrate could
no longer he obtained. Five additional one-liter washings with normal base completed the preparation of the
iron(II) hydroxide used for the solubility studies.
This technique led to the formation of a coarse-grained
precipitate, white when viewed by reflected light and
slightly greenish tinged by transmitted light. Dilutions
of the material were made to one-tenth molal base
without evidence of darkening when maintained under
an oxygen-free atmosphere.
...Iron(II) hydroxide would thus appear to be unstable in neutral solutions and to possess increasing stability as the basicity of the medium increases.
The foregoing reasoning led to the attempt to prepare iron(II) hydroxide from the chloride under such conditions that the hydroxyl ion concentration was not allowed to fall below approximately one molal until the chloride ion had been removed. The hydroxide was precipitated from strongly basic solution by the addition of dilute iron(II) chloride to a saturated solution of sodium hydroxide in an air-free system with vigorous stirring. The precipitate was repeatedly washed with molal sodium hydroxide (oxygen and carbonate-free) until a test for chloride ion with silver nitrate could no longer he obtained. Five additional one-liter washings with normal base completed the preparation of the iron(II) hydroxide used for the solubility studies. This technique led to the formation of a coarse-grained precipitate, white when viewed by reflected light and slightly greenish tinged by transmitted light. Dilutions of the material were made to one-tenth molal base without evidence of darkening when maintained under an oxygen-free atmosphere.
Sorry for a delayed response. So, basically, the book wrongly generalised the stability trend of ferrous ions to iron(II) hydrokside? Also, what about the inherent stability of the ions in solution? Would the situation be reversed in vacuum, as predicted by the electronic structure? Thanks for your reply! Sadly I am unable to retrieve the complete study you cited. The quote helped.More
The stability of iron(II) hydroxide J. Chem. Educ., 1957, vol. 34 pages 178-179 shows that the book isn't entirely correct.
The stability of iron(II) hydroxide J. Chem. Educ., 1957, vol. 34 pages 178-179 shows that the book isn't entirely correct.
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