Experiments for 'potassium ferrocyanide'
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 ferrocyanide':
EXPERIMENT 1
---------------
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
---------------
Cobalt salts give a nicely colored precipitate with ferrocyanide.
EXPERIMENT 3
---------------
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
---------------
Reaction between ferrous-ion and hexacyanoferrate (II) ion.
EXPERIMENT 5
---------------
Reaction between ferrous-ion and hexacyanoferrate (II) ion.
EXPERIMENT 6
---------------
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 7
---------------
Both ferrocyanide and ferricyanide react with zinc salts, yielding
completely differently colored solid compounds.
EXPERIMENT 8
---------------
The blue precipitate, formed when ferrocyanide and ferric ions act
upon each other is not stable in alkaline environments.
EXPERIMENT 9
---------------
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 10
---------------
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 11
---------------
Dithionite is capable of reducing prussian blue (ferric ferro cyanide).
EXPERIMENT 12
---------------
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 13
---------------
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 14
---------------
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 15
---------------
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 16
---------------
Ferrocyanide and ferricyanide apparently form a coordination complex with
aluminum, but only if both the ferrocyanide and ferricyanide are present.
EXPERIMENT 17
---------------
Ferrocyanide can be oxidized by hydrogen peroxide easily. This redox
reaction makes the liquid alkaline: H2O2 + 2e --> 2OH-
EXPERIMENT 18
---------------
Iron (III) builds a coordination complex with phosphates.
EXPERIMENT 19
---------------
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 20
---------------
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 21
---------------
Ferrocyanide is oxidized quickly by nitrite in acidic environments. On
prolonged standing, a darker green/brown compound is formed.
EXPERIMENT 22
---------------
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 23
---------------
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 24
---------------
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 25
---------------
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 26
---------------
Copper (II) reacts with ferrocyanide and builds a fairly stable compound.
EXPERIMENT 27
---------------
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 28
---------------
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 29
---------------
Vanadium (V) compounds can coexist with ferricyanide in solution. Reduction
of either one of them results in formation of a precipitate.
EXPERIMENT 30
---------------
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 31
---------------
Cr (III) reacts with the hexacyanoferrate (II) and hexacyanoferrate (III).
EXPERIMENT 32
---------------
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 33
---------------
The nickel (II) salt of ferrocyanide is not soluble in water.
End of results for 'potassium ferrocyanide'