Experiments for 'nickel 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 'nickel sulfate':
EXPERIMENT 1
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Adding ammonia to a Ni2+ solution results in formation of a purple/blue
coordination complex.
EXPERIMENT 2
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A precipitate of nickel hydroxide is oxidized by persulfate to a black
compound (probably NiO2).
EXPERIMENT 3
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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 4
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Hydrogen peroxide probably serves as a reductor for an higher oxide of
nickel.
EXPERIMENT 5
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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 6
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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 7
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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 8
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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 9
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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 10
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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 11
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The nickel (II) salt of ferrocyanide is not soluble in water.
EXPERIMENT 12
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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 13
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Borohydride is capable of reducing nickel to the metallic state in
aqueous media.
EXPERIMENT 14
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Diethylamine does not as easily form typical ammine-like complexes, like
ammonia.
EXPERIMENT 15
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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 16
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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 17
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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).
End of results for 'nickel sulfate'