Experiments for 'ferrous sulfate'
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 'ferrous sulfate':
EXPERIMENT 1
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Prussian blue cannot easily be reduced by acidic sulfite.
EXPERIMENT 2
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Reaction between ferrous-ion and hexacyanoferrate (II) ion.
EXPERIMENT 3
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Reaction between ferrous-ion and hexacyanoferrate (II) ion.
EXPERIMENT 4
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Ferrous sulfide is a black precipitate, which easily dissolves in acid.
EXPERIMENT 5
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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 6
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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 7
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Phenol and its derivatives form highly colored coordination complexes
with ferrous and ferric ions.
EXPERIMENT 8
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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 9
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Acetone reacts with sulphur in strongly alkaline environments. What products
are formed?
A similar reaction is observed between methyl ethyl ketone and sulphur.
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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Palladium (II) is not easily reduced by mild reducing agents. Only very
strong reductors are capable of reducing this to metallic palladium.
Strong oxidizers probably are capable of oxidizing palladium (II) to a
higher oxidation state, but if this is true, then the higher oxidation
state has almost the same color.
Sulfite, instead of reducing palladium to the metallic state, appears to
form a brightly colored coordination complex in acidic environments.
EXPERIMENT 12
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Thiocyanate reacts with nitrogen dioxide to form a red/brown compound. It
does not react with nitrogen monoxide. When a reaction occurs with NO2,
a white fume is produced.
End of results for 'ferrous sulfate'