Experiments for 'Fe'
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 'Fe':
EXPERIMENT 1
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Zinc (II) gives a white precipitate with ferrocyanide. This precipitate
becomes pale yellow, when treated with hydrogen peroxide (at least, when
in acidic environment).
EXPERIMENT 2
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Cobalt salts give a nicely colored precipitate with ferrocyanide.
EXPERIMENT 3
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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 4
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Iron (III) compounds with hexacyanoferrate (III) can be reduced easily.
EXPERIMENT 5
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Prussian blue cannot easily be reduced by acidic sulfite.
EXPERIMENT 6
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Reaction between ferrous-ion and hexacyanoferrate (II) ion.
EXPERIMENT 7
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Reaction between ferrous-ion and hexacyanoferrate (II) ion.
EXPERIMENT 8
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Ferrous sulfide is a black precipitate, which easily dissolves in acid.
EXPERIMENT 9
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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 10
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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 11
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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 12
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Both ferrocyanide and ferricyanide react with zinc salts, yielding
completely differently colored solid compounds.
EXPERIMENT 13
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Thiosulfate is capable of reducing ferricyanide, but it is not capable
of reducing ferroferricyanide (Prussian blue).
EXPERIMENT 14
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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 15
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The blue precipitate, formed when ferrocyanide and ferric ions act
upon each other is not stable in alkaline environments.
EXPERIMENT 16
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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 17
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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 18
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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 19
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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 20
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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 21
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Ferric ions form a coordination complex with sulfite.
EXPERIMENT 22
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Phenol and its derivatives form highly colored coordination complexes
with ferrous and ferric ions.
EXPERIMENT 23
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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 24
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When concentrated hydrochloric acid is added to a concentrated solution of
potassium ferrocyanide, then a white precipitate is formed (probably this
is KCl). The liquid slowly turns blue, but this is not due to formation
of the well known prussian blue or a similar compound.
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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The ferric ammonium citrate complex is destroyed by acid. The green one
is destroyed instantaneously, the brown one slowly is decomposed.
The resulting ferric ions can be reduced to almost colorless ferrous ions.
EXPERIMENT 29
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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 30
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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 31
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Ferric chloride reacts with bleach and forms a brown precipitate. No
higher oxidation products of iron can be observed.
EXPERIMENT 32
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Ferrous sulfate is hard to dissolve cleanly in water. It usually is
contaminated with some oxidation products and in the water it is slowly
oxidized by air as well.
EXPERIMENT 33
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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 34
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When ferric sulfate is dissolved in water, then an almost colorless liquid
is formed. On addition of chloride, a coordination complex (brown/yellow)
is formed.
EXPERIMENT 35
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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 36
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Hydroxyl amine reacts with ferrocyanides, forming a dark compound. Is the
ferrocyanide oxidized by the hydroxyl amine? This reaction occurs in
neutral environments, with the hydroxyl amine bound in a hydroxyl ammonium
salt.
EXPERIMENT 37
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Potassium ferrocyanide reacts with concentrated nitric acid. The compound
which is formed is dark brown/green. What is this compound?
Is the dark brown/green color due to formation of a Fe(NO)+ complex, well
known from the brown-ring test for nitrates?
EXPERIMENT 38
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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 39
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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 40
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Ferrocyanide can be oxidized by hydrogen peroxide easily. This redox
reaction makes the liquid alkaline: H2O2 + 2e --> 2OH-
EXPERIMENT 41
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Iron (III) builds a coordination complex with phosphates.
EXPERIMENT 42
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Ferric oxide (Fe2O3, dark red/brown) dissolves in hydrochloric acid and
nitric acid, but with extreme difficulty and in very small quantities.
EXPERIMENT 43
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Ferrocyanide reacts with hydrogen peroxide, forming a fairly intensely
colored yellow compound (probably ferricyanide), but this reaction was
expected to make the liquid more alkaline, but this cannot be observed.
EXPERIMENT 44
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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 45
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Ferrocyanide is oxidized quickly by nitrite in acidic environments. On
prolonged standing, a darker green/brown compound is formed.
EXPERIMENT 46
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Ferrous ions react with hydroxide, forming a light bluish/grey precipitate.
This precipitate, however, quickly turns brown.
EXPERIMENT 47
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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 48
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Ferric ions form a colorless complex with phosphate ions in acidic
environments. In the presence of chloride ions, a yellow coordination
complex is formed, which can exist, even in the presence of phosphate.
EXPERIMENT 49
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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 50
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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 51
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Ferrous ions react with H2O2. At low pH, the H2O2 oxidizes the ferrous ions
to ferric ions. At near neutral pH, a complex reaction occurs, the ferrous
ions are converted to some complex with the H2O2.
Ferric ions do not react with H2O2.
EXPERIMENT 52
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Iron does not dissolve quickly in dilute hydrochloric acid. When some sodium
fluoride is added, then it still does not dissolve quickly. This is in strong
contrast with titanium metal, which does dissolve quickly in dilute HCl,
when some HF is present.
EXPERIMENT 53
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Iron (III) forms a very dark brown/red coordination complex with nitrite,
both in water and in DMSO. On acidification, this complex decomposes, giving
a bright yellow solution with a slight green tinge.
EXPERIMENT 54
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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 55
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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 56
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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 57
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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 58
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Copper (II) reacts with ferrocyanide and builds a fairly stable compound.
EXPERIMENT 59
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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 60
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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 61
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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 62
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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 63
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The vanadyl salt of ferrocyanide does not dissolve in water. The salt is
easily hydrolysed in alkaline environments (it resembles the prussian blue
as far as this behaviour is concerned).
EXPERIMENT 64
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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 65
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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 66
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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 67
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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 68
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Cr (III) reacts with the hexacyanoferrate (II) and hexacyanoferrate (III).
EXPERIMENT 69
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Analysis of the composition of the dutch coin 'dubbeltje' shows that it
does not contain any copper or just a very small quantity of it.
EXPERIMENT 70
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The nickel (II) salt of ferrocyanide is not soluble in water.
EXPERIMENT 71
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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 72
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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 73
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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 74
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Hydroquinone is readily oxidized by ferricyanide, even in the presence of
sulfite, when in alkaline environments.
EXPERIMENT 75
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Ferric chloride anhydrous easily melts and when it melts, it also nearly boils
and a dark yellow/brown vapor is formed, which condenses to beautiful crystals
in cooler areas.
A small part of the ferric chloride reacts either with oxygen from the air, or
with water vapor in the air. Insoluble oxide-species are formed.
EXPERIMENT 76
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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.
EXPERIMENT 77
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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 78
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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 79
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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.
EXPERIMENT 80
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Finely divided magnesium powder violently reacts with wet cupric nitrate and
with wet ferric nitrate. The dry solids do not react.
EXPERIMENT 81
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Cyanate ion forms complexes with many metal ions. These complexes have a strong
color and are not stable in acidic solution.
End of results for 'Fe'