Experiments for 'potassium ferricyanide'
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 'potassium ferricyanide':
EXPERIMENT 1
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The vanadyl salt of ferricyanide does not dissolve. The differences between
the ferricyanide salt and ferrocyanide salts are not very clear. In alkaline
solution apparently ferricyanide and vanadate (IV) can coexist.
EXPERIMENT 2
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Vanadium (V) compounds can coexist with ferricyanide in solution. Reduction
of either one of them results in formation of a precipitate.
EXPERIMENT 3
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Vanadyl gives diverse complexes with citrate, the color of these complexes
strongly depends on the pH of the solution.
EXPERIMENT 4
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It is possible to let a liquid completely solidify by making the correct
precipitates. Citrate is very suitable for this, combined with some
transition metals.
EXPERIMENT 5
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Vanadyl ions do not precipitate with ferricyanide, when a large excess
amount of oxalic acid is present. Without the presence of oxalic acid
the two compounds form a green/yellow/brown precipitate (see other
experiments).
EXPERIMENT 6
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Copper (II) builds a complex with citrate ions. When treated with ferro
cyanide, this complex is destroyed, resulting in copper ferrocyanide.
When treated with ferricyanide, then it is not destroyed. Apparently
copper ferricyanide dissolves better in water, such that the complex
with citrate can remain in solution.
EXPERIMENT 7
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Copper (II) ions are complexed by EDTA Na4, but when the liquid is acidified,
then the copper ions are not coordinated anymore.
EXPERIMENT 8
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Cobalt (II) gives a green precipitate with ferrocyanide and a dark red/
purple precipitate with ferricyanide. The green precipitate cannot be
converted to the red one by means of oxidation by hydrogen peroxide, but
another, dark blue, compound is formed.
EXPERIMENT 9
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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 10
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Hydroquinone is readily oxidized by ferricyanide, even in the presence of
sulfite, when in alkaline environments.
EXPERIMENT 11
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Silver (I) is reduced to metallic silver by metol. This metallic silver
is easily oxidized by peroxosulfate.
Insoluble silver (I) compounds dissolve in thiosulfate solutions (principle
of photography fixer) while metallic silver is not affected.
When a mild oxidizer is added, the metallic silver also dissolves (principle
of photography reducer, Farmer's reducer).
EXPERIMENT 12
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Cr (III) reacts with the hexacyanoferrate (II) and hexacyanoferrate (III).
EXPERIMENT 13
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Manganese (II) gives an off-white precipitate with ferrocyanide and it gives
a dark brown precipitate with ferricyanide. The brown compound probably is
a manganese (IV) compound, formed through oxidation by ferricyanide.
EXPERIMENT 14
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Silver (I) ions form a precipitate, both with ferrocyanide and with
ferricyanide. The precipitate with ferricyanide is decomposed by alkalies,
the precipitate with ferrocyanide is more stable. Both compounds are
attacked by thiosulfate, which complexes the silver and causes the
solid to dissolve again.
EXPERIMENT 15
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Iron (III) compounds with hexacyanoferrate (III) can be reduced easily.
EXPERIMENT 16
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Prussian blue cannot easily be reduced by acidic sulfite.
EXPERIMENT 17
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Ferricyanide is capable of oxidizing iodide to iodine, even in neutral
environments. The reaction, however does not appear to go to completion.
EXPERIMENT 18
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Both ferrocyanide and ferricyanide react with zinc salts, yielding
completely differently colored solid compounds.
EXPERIMENT 19
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Thiosulfate is capable of reducing ferricyanide, but it is not capable
of reducing ferroferricyanide (Prussian blue).
EXPERIMENT 20
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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 21
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Ferric ions form coordination complexes with citrates and oxalates. These
coordination complex have completely different properties than free
ferric ions.
EXPERIMENT 22
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Aluminium (III) does not form colored compounds with ferrocyanide nor with
ferricyanide. Manganese (II) reacts with both of them, but a colored
compound is formed with ferricyanide only.
EXPERIMENT 23
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Ferric ions, bound to citrate, can coexist in solution with ferricyanide,
when the pH of the liquid is not too low. At lower pH the ferric citrate
complex is destroyed and the free ferric ions combine with the ferri-
cyanide ions.
EXPERIMENT 24
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Ferrocyanide and ferricyanide react with hydroxyl amine in an unexpected way.
The ferri complex first decolorizes, but then a new colored compound is
formed. The ferro complex shows this behaviour immediately.
EXPERIMENT 25
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Ferrocyanide and ferricyanide decompose on heating with dilute sulphuric
acid. When the decomposition product of ferrocyanide is treated with
hydrogen peroxide, then it looks very much like the decomposition product
of ferricyanide.
EXPERIMENT 26
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Ferrocyanide and ferricyanide apparently form a coordination complex with
aluminum, but only if both the ferrocyanide and ferricyanide are present.
EXPERIMENT 27
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Ferrocyanide in acidic environments reacts with bromine in a very peculiar
way. An extremely dark compound is formed. This reaction does not occur
in neutral environments and this cannot be observed with ferricyanides.
What is the dark compound? Is it a coordination complex or a condensation
product of many ferric/ferrous ions, close to formation of solid particles?
EXPERIMENT 28
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Ferric ions give a dark brown complex with ferricyanide. No precipitate is
formed. This precipitate is very easily converted to the dark blue prussian
blue.
Ferrous ions give a light yellow precipitate with ferrocyanide. It is,
however, very difficult to get this precipitate. The slightest amount of
oxygen makes the precipitate blue.
EXPERIMENT 29
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Hydroxylamine is capable of reducing ferricyanide to ferrocyanide. On heating,
however, a yellow compound is formed, which apparently is not ferricyanide.
With thiocyanate a pale rose-purple solution is formed on standing. Probably
oxygen from the air also takes part in the reaction.
EXPERIMENT 30
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This experiment nicely demonstrates the effect of light on a chemical compound.
An alkaline solution of potassium fericyanide (K3Fe(CN)6) is stable in the
dark, but in sunlight it decomposes in a few hours.
EXPERIMENT 31
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Thallium(I) ion is fairly easily oxidized to thallium(III). In neutral aqueous
solutions, this ion hydrolyzes to a dark hydrous oxide, which forms a compact
precipitate. The dark oxide easily can be dissolved in nitric acid, such that a
colorless solution of thallium(III) nitrate is formed in nitric acid.
Thallium(III) ion forms an ochre/yellow color with ferricyanide ion, which is
stable at low pH, but at high pH this decomposes, giving a yellow solution of
ferricyanide and a dark brown suspension of hydrous thallic oxide.
End of results for 'potassium ferricyanide'