Experiments for 'potassium chlorate'
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 'potassium chlorate':
EXPERIMENT 1
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In concentrated phosphoric acid, manganese (II) ions are oxidized easily to
manganese (III) ions, which are stabilized by formation of a phosphato-complex
with a remarkably bright purple color. This reaction is remarkable in the sense
that oxidation stops at manganese (III).
EXPERIMENT 2
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Ethanol and acetic acid do not form an ester (ethylacetate) when simply
mixed with concentrated sulphuric acid. More extreme conditions are needed
for this reaction to occur.
The acid is diluted too much in order to give a strong reaction with
chlorate, combined with the reducing agent in the form of ethanol.
EXPERIMENT 3
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Silver (I) forms a precipitate with bromates, while it does not do so with
chlorates.
EXPERIMENT 4
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Potassium chlorate is able to liberate bromine from a bromide. Reaction
with sodium sulfide of the bromine shows formation of fumes/smoke.
EXPERIMENT 5
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Potassium chlorate only reacts slowly with iodide at room temperature.
When heated, the reaction proceeds much faster. Probably KClO3 oxidizes
iodine further, until iodate is formed.
EXPERIMENT 6
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When potassium chlorate and concentrated sulphuric acid are mixed, a very
dangerous and strong oxidizer is created, which reacts explosively with
organic matter.
EXPERIMENT 7
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Although the redox potential from bromate to bromine is higher than the
potential from perchlorate to chlorate, when chlorate and bromate are
mixed, then no reaction occurs. When some hydrochloric acid is added,
then a reaction occurs with the chloride ions.
EXPERIMENT 8
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Chlorate and bromate react with hydrochloric acid, but bromate reacts more
vigorously. There also is a marked difference between potassium and sodium
chlorate. The sodium salt reacts more vigorous with hydrochloric acid, but
not as vigorous as potassium bromate.
Reactions of bromate are faster than reactions of chlorate, but for sodium
and potassium chlorate, the difference can be explained by the speed at
which the salt dissolves.
EXPERIMENT 9
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A mixture of chlorine and chlorine dioxide oxidizes bromide quickly to
bromine. When an excess amount of nitrite is added, then the bromine is
quickly reduced again to bromide. Addition of an acid does not result in
formation of bromine again.
EXPERIMENT 10
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Bromates are more reactive than chlorates in dilute aqueous solutions.
EXPERIMENT 11
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Potassium chlorate and sulphur form a potentially explosive mixture, which
is quite sensitive to shock.
EXPERIMENT 12
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Formic acid acts as a reductor, while acetic acid does not do so. Formic acid,
however, is not that easily reduced. Reduction requires elevated temperature
and strong oxidizers.
EXPERIMENT 13
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Hydrofluoric acid (48% by weight) dissolves potassium chlorate and potassium
bromate much more easily than water. The bromate also slowly decomposes in a
peculiar way, which is not observed in other acidic solutions (like sulphuric
or nitric acids).
EXPERIMENT 14
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Sodium hypophosphite is remarkably flammable. A mix with potassium chlorate is
dangerously explosive and can easily be ignited.
End of results for 'potassium chlorate'