Experiments for 'Ni'
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 'Ni':
EXPERIMENT 1
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Copper and nickel carbonates (basic), which do not dissolve in water, do
dissolve in ammonia, due to formation of a complex with ammonia.
Cobalt carbonate also dissolves, but now an additional reaction occurs,
taking up oxygen from the air.
EXPERIMENT 2
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Oxidation of nickel by nitric acid.
EXPERIMENT 3
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Analysis of the composition of the dutch coin 'dubbeltje' shows that it
does not contain any copper or just a very small quantity of it.
EXPERIMENT 4
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Adding ammonia to a Ni2+ solution results in formation of a purple/blue
coordination complex.
EXPERIMENT 5
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A precipitate of nickel hydroxide is oxidized by persulfate to a black
compound (probably NiO2).
EXPERIMENT 6
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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 7
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Hydrogen peroxide probably serves as a reductor for an higher oxide of
nickel.
EXPERIMENT 8
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Permanganate is not capable of oxidizing nickel (II) in an acidic
environment. In an alkaline environment it appears to be possible to
oxidize nickel (II) with permanganate.
EXPERIMENT 9
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Nickel does not appear to build coordination complexes with thiocyanate,
not even if acetone is added (in contrast to cobalt).
Ni(OH)2 is oxidized to a dark compound by persulfate, even in the presence
of a reducing agent like acetone.
EXPERIMENT 10
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Catechol appears to react with nickel (II), giving a coordination complex.
It is unclear, whether this is due to catechol itself or due to an
oxidation product, caused by oxidation by oxygen from air.
EXPERIMENT 11
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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 12
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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 13
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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 14
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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 15
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Nickel forms colored coordination complexes with EDTA.
EXPERIMENT 16
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Nickel (II) forms a coordination complex with bromide, but only in very
concentrated bromide solutions.
Such a concentrated bromide solution is oxidized by concentrated sulfuric
acid extremely rapidly.
EXPERIMENT 17
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The nickel (II) salt of ferrocyanide is not soluble in water.
EXPERIMENT 18
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Nickel (II) forms a complex with citrate. In a strongly alkaline environment
the nickel (II) does not precipitate. With just a small amount of ferric
ions present in the liquid, the complete liquid solidifies to a gelatin-
like constitution.
When the same experiment is done, without the nickel (II) present, no
solidification is observed.
EXPERIMENT 19
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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 20
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Borohydride is capable of reducing nickel to the metallic state in
aqueous media.
EXPERIMENT 21
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When hydrated sulfate-salts are heated, which only loose water, then their
properties strongly change. The color changes, but also the solubility
properties change a lot. The sulfate salts loose water easily, but no acid
(H2SO4 or SO3).
EXPERIMENT 22
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Diethylamine does not as easily form typical ammine-like complexes, like
ammonia.
EXPERIMENT 23
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Nickel(II) ion is reduced in slightly alkaline environment by borohydride ion,
but only with difficulty, when the mix is heated.
EXPERIMENT 24
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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 'Ni'