Experiments for 'sodium persulfate'
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 persulfate':
EXPERIMENT 1
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Vanadium (IV) as vanadyl cations, is oxidized by persulfate to vanadium (V)
as pervanadyl.
EXPERIMENT 2
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Vanadium(III) hydroxide apparently forms a precipitate and does not
dissolve in strongly alkaline liquids.
Vanadium (III) and (IV) are oxidized by peroxodisulfate to vanadium (V).
EXPERIMENT 3
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Peroxodisulfate ([S2O8]2-) is capable of oxidizing vanadyl ([VO]2+) to
pervanadyl ([VO2]+), but this reaction proceeds slowly.
EXPERIMENT 4
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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 5
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Vitamin C is a strong reductor in alkaline environments. Copper (II) is
reduced to copper (I).
EXPERIMENT 6
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Copper is oxidized by a mix of concentrated hydrochloric acid and
hydrogen peroxide. When the peroxide is used up and there is still an
excess amount of hydrochloric acid, then the copper (II) appears to
oxidize the copper metal, under the formation of an intensely colored
complex. (What is the constitution of this complex??)
When the solution is diluted with water, then the intensely colored
complex is destroyed and a white crystalline precipitate of CuCl is
formed. If too much water is used, then no clear precipitate is formed.
EXPERIMENT 7
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Copper builds higher oxides than CuO when strong oxidizing agents are
present in alkaline environments. Probably these are not copper (III)
compounds, but the oxo-ion probably is replaced by peroxo or superoxo.
EXPERIMENT 8
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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 9
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Platinum (II) can be oxidized to platinum (IV) by strong oxidizing agents.
Reduction to metallic platinum cannot be achieved by sulfite nor by stannous
chloride.
EXPERIMENT 10
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Photography developers, based on phenol-like structures, are easily oxidized
by air in alkaline environments and the oxidation products are such, that
a reverse process does not occur anymore (probably the oxidation products
are large polymerized species).
EXPERIMENT 11
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Copper (II) apparently catalyses the oxidation of pyrogallol by oxygen from
the air.
EXPERIMENT 12
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Pyrogallol gives rise to many colored products on oxidation and coordination.
More investigation is needed in order to get more insight in all these
colors and the conditions under which they are formed.
EXPERIMENT 13
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When p-aminophenol is oxidized in an acidic environment, then a compound
is formed, with a deep indigo/purple color.
EXPERIMENT 14
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Both metol and p-aminophenol HCl are oxidized by persulfate to colored
compounds. When metol is used, the color, however, is not as brilliant
and not as intense as when p-aminophenol HCl is used. Apparently the
methyl-group on the amino-part of metol has strong influence on the
color of the oxidation product or on the type of oxidation products.
EXPERIMENT 15
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When p-aminophenol is oxidized in acidic environment, then an intensely
colored compound is formed (indigo/purple). This compound is irreversibly
destroyed when the liquid is made alkaline.
EXPERIMENT 16
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Persulfate decomposes in strongly alkaline environments.
EXPERIMENT 17
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Chromium (III) is oxidized to dichromate (chrome (VI)) by persulfate. This
reaction is catalyzed by silver (I).
EXPERIMENT 18
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Chromium (III) cannot be oxidized to chromium (VI) by vanadium (V) species
or bromates in strongly alkaline environments. Peroxodisulfate is capable
of achieving this.
EXPERIMENT 19
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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 20
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When aqueous ammoniacal silver is reduced by glucose, a nice silver mirror
is produced.
Peroxosulfate is capable of oxidizing silver to a higher oxidation state
(+2 or +3), even in acidic environments.
EXPERIMENT 21
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The peroxosulfate ion ([S2O8]2-) is capable of oxidizing silver (I) to
silver (II) or silver (III). A higher oxide of silver is precipitated.
This oxide is easily decomposed under the liberation of oxygen.
EXPERIMENT 22
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Silver (I) reacts with persulfate. Probably a higher oxidation state of
silver is produced (oxidation state II or III).
EXPERIMENT 23
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Lead builds a yellow precipitate with hydroxide and peroxosulfate. This
probably is an oxidation product of lead (II).
EXPERIMENT 24
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Lead hydroxide is oxidized by hydrogen peroxide. The resulting compound
does not dissolve in dilute nitric acid.
EXPERIMENT 25
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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 26
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A precipitate of nickel hydroxide is oxidized by persulfate to a black
compound (probably NiO2).
EXPERIMENT 27
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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 28
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Hydrogen peroxide probably serves as a reductor for an higher oxide of
nickel.
EXPERIMENT 29
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Nickel (II) does not form a coordination complex with ascorbic acid, not
in neutral or slightly acidic environments, nor in alkaline environments.
EXPERIMENT 30
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Nickel (II) builds a stable complex with EDTA. Once this complex is formed,
it is not precipitated with NaOH and persulfate does not oxidize nickel (II).
EXPERIMENT 31
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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 32
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This experiment describes a qualitative method, useful for showing the
presence of minute quantities of manganese (II), which cannot be detected
by oxidation with H2O2 in alkaline environments anymore. Chloride ions
may not be present besides the manganese to be detected.
EXPERIMENT 33
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Nickel forms colored coordination complexes with EDTA.
EXPERIMENT 34
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Bismuth(III) in nitric acid solutoin is not oxidized by peroxodisulfate to a
bismuth(V) species.
EXPERIMENT 35
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Rhenium forms complexes with thiocyanate in more than one oxidation state.
Here a rhenium (IV) thiocyanate complex is made and then oxidized to rhenium
(V). Historically these complexes have been used to detect minute traces of
rhenium due to the intense colours formed.
EXPERIMENT 36
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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 37
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Thallium(I) ion is fairly easily oxidized to thallium(III). In neutral aqueous
solutions, this ion hydrolyzes to a dark hydrous oxide, which forms a compact
precipitate. The dark oxide easily can be dissolved in nitric acid, such that a
colorless solution of thallium(III) nitrate is formed in nitric acid.
Thallium(III) ion forms an ochre/yellow color with ferricyanide ion, which is
stable at low pH, but at high pH this decomposes, giving a yellow solution of
ferricyanide and a dark brown suspension of hydrous thallic oxide.
EXPERIMENT 38
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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 39
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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.
EXPERIMENT 40
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Copper(II) ions form a pale green complex with a yellowish hue. When the
solution is heated to boiling, then the copper(II) is reduced to metallic
copper.
End of results for 'sodium persulfate'