Experiments for 'hydroxyl amine 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 'hydroxyl amine sulfate':
EXPERIMENT 1
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Tetra chloro auric acid (a.k.a. "gold chloride"), a gold (III) compound is
easily reduced to metallic gold, which forms a colloidal solution. With
strong reductors, the gold particles formed are so large that they form
a dark precipitate.
EXPERIMENT 2
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Hydroxyl amine reacts with acetone, releasing (some) heat. After this
reaction, the resulting compound is shown to still be a relatively strongly
reducing agent in alkaline solution.
EXPERIMENT 3
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Nitrites react with ammonium and with hydroxyl ammonium ions. In both cases
a colorless and odourless gas is formed.
EXPERIMENT 4
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Hydroxyl amine is capable of reducing vanadium (V) to vanadium (IV), but
further reduction is not possible with hydroxyl amine.
EXPERIMENT 5
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The result of this experiment is remarkable. Hydroxyl amine, being a strong
reductor, appears to oxidize vanadium (IV) to vanadium (V) in alkaline
environments. Or is there another compound, which strongly resembles the
well-known yellow colour of vanadium (V) in acidic environments and the
(almost) colourless appearance of vanadium (V) in alkaline environments?
EXPERIMENT 6
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In alkaline environments, copper (II) shows remarkable behavior, when brought
in contact with strong oxidizers or reductors.
EXPERIMENT 7
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Hydroxyl amine sulfate (containing protonated hydroxyl amine) is not capable
of reducing copper (II). When the liquid becomes basic (releasing free
hydroxyl amine), then the copper (II) is reduced to copper (I).
EXPERIMENT 8
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Copper (II) is reduced by hydroxyl amine very quickly in alkaline
environments. Yellow copper (I) hydroxide/oxide is formed.
EXPERIMENT 9
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Copper (II) amine complex is reduced to a colorless copper (I) amine
complex by hydroxyl amine. The copper (I) complex is oxidized by oxygen
from the air very easily.
EXPERIMENT 10
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When copper (II) is present in hydrochloric acid, then it does not react
immediately with hydroxyl ammonium, some heating is required to have a
reaction, resulting in formation of a dark green/brown compound. When the
liquid is made alkaline with excess ammonia, then it quickly becomes
colorless, due to reduction of copper (II) to copper (I), which forms a
colorless complex with ammonia.
A very peculiar reaction occurs on oxidation by oxygen from air. The liquid
is covered by a very thin shiny layer, looking like a strongly coloured oil
on water. It is not clear what it is, more research is needed.
EXPERIMENT 11
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Copper (II) chloride is reduced by hydroxyl amine, when dissolved in
ethanol. First, the solution becomes much darker and apparently, a mixed
oxidation state complex of copper (I) and copper (II) is formed. Finally,
all copper (II) is reduced to copper (I).
This experiment is another example, which shows that copper (I) and copper
(II), when in solution at the same time, form a highly colored complex.
EXPERIMENT 12
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Copper (II) forms a coordination compound with ethyl acetate, which has
reacted with hydroxyl amine.
EXPERIMENT 13
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This is a very nice experiment, involving beautifully coloured compounds,
but it is a hazardous experiment as well, due to the use of mercury (II)
compounds.
Mercury (II) builds a complex with excess iodide, [HgI4]2-, which gives a
beautiful bright yellow precipitate with Ag+ and a beautiful bright brick-
red precipitate with Cu+.
EXPERIMENT 14
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Chromium (III) apparently builds a coordination complex with hydroxyl amine,
but this complex does not simply form from chromium (III) salts and
hydroxyl amine. If chromium (III) is formed by means of reduction of
chromium (VI) in the presence of hydroxyl amine, then the complex is
formed. If hydroxyl amine is added to chromium (III) without redox reaction,
then another complex is created.
EXPERIMENT 15
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Chromium (III) forms a lavender precipitate, when combined with hydroxyl
amine in alkaline environments. This compound does not dissolve in
strongly alkaline environments.
EXPERIMENT 16
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Hydroxyl amine gives a brown coordination complex when it reduces hexavalent
chromium to trivalent chromium in alkaline environments. This coordination
complex is really due to the hydroxyl amine. When other reducing agents are
used in the presence of ammonia in alkaline environments, then no similar
reaction product can be obtained.
EXPERIMENT 17
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Silver is coordinated by thiosulfate. The silver-thiosulfate complex does
not show any of the reactions of free aqueous silver (I).
EXPERIMENT 18
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Silver (I) is not reduced by hydroxyl amine in neutral environments. When
made alkaline, it is reduced to metallic silver immediately.
EXPERIMENT 19
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Silver (I) gives a white precipitate with thiocyanate, which does not dissolve
in excess ammonia. Hydroxyl amine does not affect this precipitate.
EXPERIMENT 20
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Silver (I) does not give a precipitate with hydroxyl amine sulfate (if
concentrations are not too high), but ammonia causes formation of a
precipitate, which does not dissolve in excess ammonia.
EXPERIMENT 21
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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 22
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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 23
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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 24
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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 25
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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 26
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Hydroxyl ammonium ion and bromate ion react with each other, but with a delay.
Once the reaction starts, it is EXTREMELY violent.
End of results for 'hydroxyl amine sulfate'