Experiments for 'sodium dithionite'
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 'sodium dithionite':
EXPERIMENT 1
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Copper (I) iodide dissolves in dilute ammonia, resulting in a colorless
liquid. Copper (I) builds a coordination complex with ammonia. This
complex is oxidized by oxygen from the air exceedingly easily.
EXPERIMENT 2
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When copper (II) is reduced by dithionite in neutral environments, then
a dark red/brown precipitate is formed (metallic copper??). When reduced
in alkaline environments, then hydrous copper (I) oxide is formed.
EXPERIMENT 3
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When tetraammine-copper (II) is reduced by dithionite in excess ammonia,
then a colorless copper (I) complex is formed, which remains dissolved.
EXPERIMENT 4
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Mercury (II) salts give an oxide/hydroxide, which does not dissolve in
large excess amounts of alkaline solutions. Ammonia does not dissolve
the precipitate of mercury (II) oxide/hydroxide.
EXPERIMENT 5
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Cobalt carbonate does not dissolve completely in dilute mineral acids. With
some heating, however, it does dissolve completely.
With nitrite a yellow/orange complex is formed, which forms a precipitate
when treated with alkalies. The precipitate is resistant to treatment with
acid and bases.
EXPERIMENT 6
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When molybdates are reduced, then intense blue compounds are formed. It
is believed that these intensely coloured compounds are multi-nuclear
Mo-compounds, with different nuclei having different oxidation states.
EXPERIMENT 7
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In strongly alkaline environments, molybdates are not as easily reduced
as in neutral or acidic environments.
EXPERIMENT 8
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Molybdate forms blue or green compounds, when reduced with mild reducing
agents or when little quantitities of reducing agents are used.
EXPERIMENT 9
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Tungstate ions, when reduced, produce a deep blue color. Tungstate is
a weak oxidizer.
EXPERIMENT 10
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A large set of compounds is checked on interaction with concentrated
nitric acid. Many reductors react violently with nitric acid.
EXPERIMENT 11
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Chromate is reduced by dithionite in strongly alkaline solution, but this
reaction proceeds slowly.
EXPERIMENT 12
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Dithionite is not capable of reducing ferric oxide/hydroxide to an iron (II)
compound in alkaline environments.
EXPERIMENT 13
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Dithionite reduces ferric ions to ferrous ions quickly in acidic
environments.
EXPERIMENT 14
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Dithionite is capable of reducing prussian blue (ferric ferro cyanide).
EXPERIMENT 15
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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 16
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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 17
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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 18
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Arsenic in oxidation state +5 is not easily reduced to elemental arsenic,
except by tin(II) chloride.
End of results for 'sodium dithionite'