Experiments for 'ammonium 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 'ammonium persulfate':
EXPERIMENT 1
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Persulfate is not capable of oxidizing manganese to the (VII) state
in acidic environments.
EXPERIMENT 2
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Permanganate is capable of oxidizing thiocyanate in acidic environments:
The result is a pink solution, more intensely colored than manganese (II)
ions (which are almost colorless).
EXPERIMENT 3
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Persulfate decomposes in strongly alkaline environments.
EXPERIMENT 4
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Chromium (III) can be oxidized to chromium (VI) by persulfate in alkaline
environments.
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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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 8
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Silver (I) is reduced to metallic silver by metol. This metallic silver
is easily oxidized by peroxosulfate.
Insoluble silver (I) compounds dissolve in thiosulfate solutions (principle
of photography fixer) while metallic silver is not affected.
When a mild oxidizer is added, the metallic silver also dissolves (principle
of photography reducer, Farmer's reducer).
EXPERIMENT 9
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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.
End of results for 'ammonium persulfate'