Experiments for 'potassium bromate'
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 bromate':
EXPERIMENT 1
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Vanadyl is oxidized by bromate quickly and completely.
EXPERIMENT 2
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Copper (II) does not form a coordination complex, nor does it form a
precipitate with bromate. It does not react.
EXPERIMENT 3
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When potassium bromate and sulphur are mixed, then a very dangerous mixture
is created. This mixture, when ignited, produces an intensely bright flame.
EXPERIMENT 4
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Bromate reacts with concentrated sulphuric acid, releasing bromine and a
gas (probably this is oxygen).
EXPERIMENT 5
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Bromate is reduced by sulfite quickly in acidic environments. When an
excess amount of bromate is used, then bromine is formed. When an excess
amount of sulfite is used, then the bromine is reduced further to bromide.
EXPERIMENT 6
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Potassium bromate reacts vigorously with concentrated hydrochloric acid.
A green gas is evolved, but this gas has a color, which is fairly intense.
The green gas consists of chlorine, but it also contains bromine, probably
combined with chlorine in a compound as BrCl, which is slightly darker
green than Cl2.
EXPERIMENT 7
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Potassium bromate is capable of oxidizing hydrogen peroxide, itself being
reduced to bromine.
EXPERIMENT 8
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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 9
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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 10
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A large amount of sulphur can be added to bromine, before a solid remains in
the liquid bromine. The sulphur dissolves in the bromine very easily.
EXPERIMENT 11
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Bromates are more reactive than chlorates in dilute aqueous solutions.
EXPERIMENT 12
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Bromate reacts with chlorides, releasing chlorine. Probably some bromine
is produced as well or a bromine/chlorine compound is produced.
EXPERIMENT 13
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Bromate oxidizes iodine to iodate, itself being converted to bromine.
Chlorate does not oxidize bromine to bromate, itself being converted to
chlorine (at least not quickly).
EXPERIMENT 14
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When bromate, manganese (II), citric acid and sulphuric acid are mixed at
certain propertions, then an oscillating reaction occurs, finally resulting
in an oily compound, which separates from the aqueous liquid.
EXPERIMENT 15
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When bromate, manganese (II), malonic acid and sulphuric acid are mixed at
certain conditions, then a very convincing oscillating reaction occurs,
which persists for few minutes, going through a cycle many times, before
a final state is reached.
EXPERIMENT 16
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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 17
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Phosphoric acid is not capable of driving off hydrogen bromide from
alkali bromides, nor does it oxidize bromide.
EXPERIMENT 18
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Silver (I) gives a precipitate with bromate. The compound silver bromate
does not dissolve well in water. When acidified, the compound still does
not dissolve, hence the acid HBrO3 is fairly strongly ionized, otherwise
the silver bromate would dissolve appreciably. The precipitate of silver
bromate, however, still shows strong oxidizing properties, meaning that
it is sufficiently soluble for releasing bromate ions in solution, needed
for the redox reaction to occur.
EXPERIMENT 19
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Silver (I) forms a precipitate with bromates, while it does not do so with
chlorates.
EXPERIMENT 20
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Bromine reacts with acetylene gas. The bromine disappears and a compound
is formed with a peculiar sweetish smell.
EXPERIMENT 21
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Potassium bromate does not react with concentrated formic acid, but when
some bromide or hydrochloric acid is added, then the reaction proceeds
quickly, carbon dioxide being produced.
EXPERIMENT 22
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Ferrocyanide in acidic environments reacts with bromine in a very peculiar
way. An extremely dark compound is formed. This reaction does not occur
in neutral environments and this cannot be observed with ferricyanides.
What is the dark compound? Is it a coordination complex or a condensation
product of many ferric/ferrous ions, close to formation of solid particles?
EXPERIMENT 23
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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 24
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Potassium bromate reacts with aluminium powder with a very bright light and
with crackling noise, but the mix is not like flash powder. Some sulphur is
needed for easy ignition of the mix.
When a tiny amount of red phosphorus is added to the mix, then it is ignited
even more easily, but then it also burns exceptionally fast, almost
explosively.
EXPERIMENT 25
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A mix of finely powdered sodium hypophosphite and potassium bromate forms an
energetic mix which can easily be ignited.
EXPERIMENT 26
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Chromium(III) oxide is extremely inert when it is calcined. It does not
dissolve in the common acids, nor in solutions of common bases. The solid,
however, can be oxidized by a solution of a bromate.
EXPERIMENT 27
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Hydroxyl ammonium ion and bromate ion react with each other, but with a delay.
Once the reaction starts, it is EXTREMELY violent.
EXPERIMENT 28
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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 29
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An acidified solution of potassium bromate quickly oxidises solid potassium
nitrite to potassium nitrate, the bromate being converted to bromine.
End of results for 'potassium bromate'