Experiments for 'O'
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 'O':
EXPERIMENT 1
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Hydrogen peroxide builds complexes with vanadium (IV) and vanadium (V)
species. These compounds are not stable and result in dissociation of
the complex and formation of vanadium (IV) compounds. The net result
of adding hydrogen peroxide to a solution containing vanadium (V) can
be reduction to vanadium (IV) with the formation of oxygen.
EXPERIMENT 2
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Vanadium (IV) does not readily yield precipitates with alkaline compounds.
Carbonate is not capable of precipitating this.
Hydrogen peroxide builds a complex with vanadium (V) and possibly with
vanadium (IV). Diverse coloured compounds are formed in sequence. What
is their constitution?
EXPERIMENT 3
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Vanadium (V) compounds form yellow compouds with hydrogen peroxide in
alkaline environments, with strong solutions and very high alkalinity grey
and blue compounds are formed, which, however, decompose easily.
EXPERIMENT 4
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Vanadium (V) is capable of forming many peroxo compounds, whose appearance
strongly depends on pH.
EXPERIMENT 5
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Decomposition of hydrogen peroxide is catalyzed by cuprammine complex.
EXPERIMENT 6
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Copper (II) carbonate gives a very dark compound with H2O2, is this a
peroxide compound or just copper oxide?
EXPERIMENT 7
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Titanium slowly dissolves in concentrated hydrochloric acid, forming deep
blue/violet titanium (III) ions. On addition of hydrogen peroxide these are
oxidized to titanium (IV), which in turn forms a deep red coordination
complex with hydrogen peroxide.
The deep red coordination complex is only stable in acidic to neutral media.
It also is easily reduced by nitrite. It is not affected strongly by
persulfate. With fluoride, a light yellow compound is formed, but the
formation of that may also be due to rise of pH.
EXPERIMENT 8
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Sodium sulfide is oxidized by acidic hydrogen peroxide with extreme violence.
EXPERIMENT 9
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Bromide is oxidized by hydrogen peroxide in acidic environments. Addition
of nitric acid strongly enhances the reaction.
EXPERIMENT 10
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Potassium bromate is capable of oxidizing hydrogen peroxide, itself being
reduced to bromine.
EXPERIMENT 11
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Persulfate decomposes in strongly alkaline environments.
EXPERIMENT 12
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A mixture of hydrogen and oxygen explodes on ignition, even when the mix
is not confined to a limited space.
EXPERIMENT 13
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Chromium (III) can be oxidized to chromium (VI) by persulfate in alkaline
environments.
EXPERIMENT 14
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Chromium (III) is oxidized to dichromate (chrome (VI)) by persulfate. This
reaction is catalyzed by silver (I).
EXPERIMENT 15
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Persulfate is not capable of oxidizing manganese to the (VII) state
in acidic environments.
EXPERIMENT 16
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Persulfate is capable of oxidizing Mn2+ in acid environments, but silver (I)
is needed as a catalyst. Oxidation, however, is not easy and just a small
part is oxidized to permanganate, a large part is oxidized no further than
MnO2.
EXPERIMENT 17
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Lead builds a yellow precipitate with hydroxide and peroxosulfate. This
probably is an oxidation product of lead (II).
EXPERIMENT 18
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Lead hydroxide is oxidized by hydrogen peroxide. The resulting compound
does not dissolve in dilute nitric acid.
EXPERIMENT 19
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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 20
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A precipitate of nickel hydroxide is oxidized by persulfate to a black
compound (probably NiO2).
EXPERIMENT 21
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Nickel (II) gives a black precipitate when treated with hydroxide and
persulfate at the same time. It is expected that this is an higher
oxide of nickel (NiO2).
EXPERIMENT 22
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Hydrogen peroxide probably serves as a reductor for an higher oxide of
nickel.
EXPERIMENT 23
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Nickel hydroxide can be oxidized by persulfate to a higher hydrous oxide
(nickel (III) and/or nickel (IV) oxide), but nickel carbonate is not
oxidized. The carbonate can be oxidized, however, when hydroxide is
added to the solution.
EXPERIMENT 24
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Nickel in nickel (II) hydroxide is oxidized to a higher oxidation state by
hypochlorites, but not by chlorates. The oxidation product is reduced by
hydrogen peroxide and ammonia. Heating of the oxidation product makes it
more resistant to reduction and to breakdown by acids.
EXPERIMENT 25
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Sulphur and Carbon are mixed,
Potassium Nitrate is dissolved in hot water and the Sulphur/Carbon mix is
added.
Pure Isopropanol is added, and dehydrates the water, allowing the KNO3 and S/C
to mix closely.
The wet powder is filtered via a vacuum filter, and is dried using ambient
heat.
This produces fast-burning gunpowder.
EXPERIMENT 26
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Peroxodisulfate ion gives a deep brown complex with silver ions in nitric acid.
Oxone (peroxomonosulfate) does not give such a complex, actually, it quickly
destroys such a complex.
EXPERIMENT 27
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The blue vanadyl ion VO(2+), which contains vanadium in oxidation state +4, is
oxidized by oxone (which contains the monopersulfate ion, SO5(2-)) and it also
is oxidized by the peroxodisulfate ion S2O8(2-). Oxidation by monopersulfate is
immediate, oxidation by peroxodisulfate is very slow. The latter reaction can
be sped up by heating, but still it takes tens of seconds on near boiling of
the solution.
The blue vanadyl ion is oxidized to the pale yellow pervanadyl ion VO2(+). On
heating, this pervanadyl ion condenses into more intensely colored ions which
contain multiple VO2(+) units. At a certain point the condensation of the
pervanadyl ions goes so far that a red/orange precipitate is formed of hydrous
vanadium pentaoxide, V2O5.nH2O.
EXPERIMENT 28
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Both oxone, active ion is HSO5(-), and peroxodisulfate, active ion is S2O8(2-),
produce a black precipitate when added to nickel(II) ions at high pH. Hydrogen
peroxide, on the other hand, only produces green nickel(II) hydroxide, and if
the black precipitate is present, it is destroyed by hydrogen peroxide, with
formation of oxygen and green nickel(II) hydroxide.
End of results for 'O'