Experiments for 'ferric chloride'
Below follows a summary of all experiments, matching your search. Click one of the EXPERIMENT hyperlinks for a complete description of the experiment.
Results for 'ferric chloride':
EXPERIMENT 1
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Copper (II) reacts with thiocyanate in a complex way.
EXPERIMENT 2
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Copper gives a coordination complex with catechol, but only in alkaline
environments. This complex is easily oxidized by oxygen from air. Iron
also forms a complex in acidic media, probably by a combined red/coordination
reaction.
EXPERIMENT 3
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Nitrous acid (or its decomposition product) forms a dark brown coordination
complex with ferric ions. With copper (II) also a coordination complex is
formed. In relatively strongly acidic environments, these coordination
complexes are destroyed/not formed.
EXPERIMENT 4
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Sulfide gives precipitates with some metals, which do not dissolve in
strong acids. These sulfides, however, can easily be dissolved, when an
oxidizing agent is used.
Sulfide is easily oxidized by moderately strong oxidizers.
EXPERIMENT 5
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This sequence of experiments shows that sulfite is capable of reducing
silver (I), copper (II) and iron (III), but that these reactions all
show their own peculiarities. Sulphur in the +4 oxidation state is a
mild reductant.
EXPERIMENT 6
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Hydroquinone is oxidized by ferric chloride to quinone. An intermediate
dark green compound is formed before all hydroquinone is oxidized.
EXPERIMENT 7
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Ferric chloride enhances the oxidation of hydroquinone by hydrogen
peroxide considerably. Besides this, a coordination complex appears
to be formed when ferric chloride is added to an hydroquinone/peroxide
solution.
EXPERIMENT 8
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Hydroquinone can be oxidized by ferric chloride. If not too much ferric
chloride is added, then a coordination complex of the oxidation product
with hydroquinone is formed and crystals of this compound separate
from the liquid.
EXPERIMENT 9
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Pyrogallol gives rise to many colored products on oxidation and coordination.
More investigation is needed in order to get more insight in all these
colors and the conditions under which they are formed.
EXPERIMENT 10
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The coordination complexes formed by iron-salts and phenol-like photographic
developers show very typical reactions with hydrogen peroxide. Many times
these reactions result in oxidation products which are not dark colored,
as opposed for oxidation by atmospheric oxygen.
EXPERIMENT 11
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Tannine (a polyphenolic compound of large molecular weight of indeterminate
composition) reacts with many metal ions, forming highly coloured complexes.
It also shows some other reactions. The exact type of reactions is not
always clear.
The tannine, used in these experiments, was brown. It's intended use is
as an additive for making wine.
EXPERIMENT 12
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Permanganate is capable of oxidizing thiocyanate in acidic environments:
The result is a pink solution, more intensely colored than manganese (II)
ions (which are almost colorless).
EXPERIMENT 13
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Iron (III) compounds with hexacyanoferrate (III) can be reduced easily.
EXPERIMENT 14
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Iron (III) gives a precipitate with S2-, but a redox reaction, resulting
in the formation of sulphur also appears to occur.
EXPERIMENT 15
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Thiosulfate gives a purple coordination complex with iron (III). This
complex, however, is not stable. With iron (II) no complex is formed.
Iron (III) is reduced by thiosulfate after the initial formation of
the purple coordination complex. This is shown by adding ferrocyanide,
which does not result in formation of an intense dark blue precipitate.
EXPERIMENT 16
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Thiosulfate is capable of reducing ferricyanide, but it is not capable
of reducing ferroferricyanide (Prussian blue).
EXPERIMENT 17
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Ferricyanide gives a dark brown coordination complex with ferric ions. This
complex is soluble in water. It is easily transformed to the much more
stable, dark blue and insoluble ferroferricyanide.
EXPERIMENT 18
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The blue precipitate, formed when ferrocyanide and ferric ions act
upon each other is not stable in alkaline environments.
EXPERIMENT 19
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Bleach is not capable of oxidizing ferric hydroxide to the hexavalent
ferrate (at least not at 60 C within several minutes).
EXPERIMENT 20
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Ferrous ions give a yellow coordination complex with oxalate. The normal
color of ferrous ions is pale green. Ferric ions give a green coordination
complex with oxalate. The normal color of ferric ions is yellow/brown.
The ferric complex is only formed if the environment is not too acidic.
EXPERIMENT 21
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The experiment described below suggests the formation of a coordination
complex between iron and ascorbate. The presence of the ascorbate induces
a completely different behavior of ferric/ferrous ions in alkaline
environments.
EXPERIMENT 22
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Ferric ions apparently form a coordination complex with glucose in alkaline
environments. Normally ferric ions give a brown precipitate in strong
alkaline liquids, with glucose the liquid remains clear.
EXPERIMENT 23
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Ferric ions form a coordination complex with sulfite.
EXPERIMENT 24
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Phenol and its derivatives form highly colored coordination complexes
with ferrous and ferric ions.
EXPERIMENT 25
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Dithionite is not capable of reducing ferric oxide/hydroxide to an iron (II)
compound in alkaline environments.
EXPERIMENT 26
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Dithionite reduces ferric ions to ferrous ions quickly in acidic
environments.
EXPERIMENT 27
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Dithionite is capable of reducing prussian blue (ferric ferro cyanide).
EXPERIMENT 28
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Ferric chloride reacts with bleach and forms a brown precipitate. No
higher oxidation products of iron can be observed.
EXPERIMENT 29
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Although p-aminophenol and metol are similar compounds (metol is the
sulfate salt of p-aminophenol with a H-atom at the amino-group replaced
by a methyl group) they show fairly large differences as far as complex-
formation is concerned with ferric compounds.
Metol reacts more slowly and the color of the compounds differ.
EXPERIMENT 30
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When an acidified solution of ferric chloride is mixed with a solution
of hydroxyl amine sulfate, then an almost colorless compound is formed,
but this compound does not seem to be an iron (II) compound.
EXPERIMENT 31
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Iron (III) builds a coordination complex with phosphates.
EXPERIMENT 32
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Ferric ions are reduced by borohydride to a black compound. Is this
metallic iron or is this iron (II) oxide?
EXPERIMENT 33
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Nickel (II) forms a complex with citrate. In a strongly alkaline environment
the nickel (II) does not precipitate. With just a small amount of ferric
ions present in the liquid, the complete liquid solidifies to a gelatin-
like constitution.
When the same experiment is done, without the nickel (II) present, no
solidification is observed.
EXPERIMENT 34
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Ferric chloride dissolves in acetic anhydride very well, forming a beautifully
colored deep red/brown solution. The color of this solution is very bright.
EXPERIMENT 35
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Copper(II) ion and iron(III) ion form complexes with acetyl acetate (acac) in
aqueous solution. Cobalt does not form a complex, at least not visibly.
End of results for 'ferric chloride'