Experiments for 'Br'
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 'Br':
EXPERIMENT 1
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Nitrite is decomposed by hydrochloric acid (as it is done by all acids),
but when the decomposition products are not allowed to escape, then
further reactions occur.
When bromide is added, then a compound is formed, which definitely is not
bromine. What is this compound?
When iodide is added, then iodine is formed.
EXPERIMENT 2
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Nitrite gives rise to formation of a blue compound with dilute sulphuric
acid, which is not very stable (dissociates into nitrous oxide easily).
When bromide is added, then a brown/green compound is formed, which
is not bromine.
EXPERIMENT 3
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Vanadyl is oxidized by bromate quickly and completely.
EXPERIMENT 4
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Copper (II) ions form a brown complex with bromide ions, but only when the
product of concentration of copper and bromide is high.
In strongly acidic environments, bromide gives a red/brown/purple complex
with cupric ions.
EXPERIMENT 5
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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 6
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Copper (II) forms a very dark coordination compound with concentrated
bromide in highly acidic environments. When metallic copper is added,
then this complex quickly disappears and the liquid almost becomes
colorless.
EXPERIMENT 7
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Iodide ion reacts with thionyl chloride, most likely giving iodine, and some
sulphur(II) species.
Potassium bromide does not dissolve in thionyl chloride (at least, not visibly).
No reaction occurs.
EXPERIMENT 8
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Diverse phenol-derivatives, can be oxidized easily by bromine, yielding
intensely colored oxidation products.
EXPERIMENT 9
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P-aminophenol HCl reacts with bromine and forms a purple compound.
EXPERIMENT 10
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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 11
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Bromide is oxidized by hydrogen peroxide in acidic environments. Addition
of nitric acid strongly enhances the reaction.
EXPERIMENT 12
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It is possible to make an aqueous solution of bromine, which is so saturated,
that the bromine separates from the liquid. In order to do so, a chemical
reaction, producing large quantities of bromine must be performed.
EXPERIMENT 13
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Sodium bromide is not oxidized by concentrated nitric acid. However, when
a minute quantity of nitrite is added, suddenly the reaction starts and
quickly all bromide is oxidized.
EXPERIMENT 14
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Sodium chloride reacts with sulfuric acid to give hydrogen chloride gas.
Sodium bromide shows a similar reaction, producing hydrogen bromide, but
in a side reaction some bromine is formed.
EXPERIMENT 15
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Bromide is oxidized by sulphuric acid, even when diluted with water.
Bromine precipitates from water, when it is created in high concentrations.
EXPERIMENT 16
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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 17
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Bromate reacts with concentrated sulphuric acid, releasing bromine and a
gas (probably this is oxygen).
EXPERIMENT 18
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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 19
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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 20
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Potassium bromate is capable of oxidizing hydrogen peroxide, itself being
reduced to bromine.
EXPERIMENT 21
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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 22
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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 23
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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 24
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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 25
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Bromates are more reactive than chlorates in dilute aqueous solutions.
EXPERIMENT 26
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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 27
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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 28
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Aluminium reacts violently with bromine.
EXPERIMENT 29
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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 30
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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 31
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Praseodymium (III) ions form complexes with chloride, bromide and iodide. With
fluoride a precipitate is formed.
EXPERIMENT 32
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Phosphoric acid is not capable of driving off hydrogen bromide from
alkali bromides, nor does it oxidize bromide.
EXPERIMENT 33
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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 34
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Silver (I) forms a precipitate with bromates, while it does not do so with
chlorates.
EXPERIMENT 35
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Bromine reacts with acetylene gas. The bromine disappears and a compound
is formed with a peculiar sweetish smell.
EXPERIMENT 36
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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 37
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Bromine quickly adds to acrylic acid (which has a double bond, in the molecule H2C=CH-C(O)OH)).
Bromine does not react quickly with propanoic acid.
EXPERIMENT 38
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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 39
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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 40
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Sodium selenite dissolves in concentrated hydrobromic acid with a red/brown
color. When this solution is shaken with ligroin, then the ligroin layer also
turns red/brown. The compound, dissolved in the ligroin layer is a selenium
compound, as is demonstrated by the experiment, described in more detail below.
EXPERIMENT 41
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Bromine does not react with formic acid, or it reacts very slowly. When
aluminium is added, then this quickly shows a violent reaction and all of the
aluminium dissolves, leaving a clear orange/red and someawhat viscous liquid.
On dilution with water, a clear yellow liquid is obtained.
EXPERIMENT 42
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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 43
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Hypochlorite ion forms esters very easily with alcohols. The esters simply are formed from aqueous
solutions. The methyl ester is a colorless gas, which gives extremely powerful explosions when
ignited. The ethyl ester is a very volatile yellow/green oil, which burns with a WHOOSH sound and
which is quite unstable (it easily decomposes). The t-butyl ester is quite stable and can be kept
around for a somewhat longer time. This burns quickly with a sooty flame.
EXPERIMENT 44
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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 45
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When antimony is added to liquid bromine, then a violent reaction occurs, even
with appearance of sparks.
EXPERIMENT 46
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A mix of finely powdered sodium hypophosphite and potassium bromate forms an
energetic mix which can easily be ignited.
EXPERIMENT 47
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Bromine reacts vigorously with hydroxyl ammonium ion. A lot of colorless gas is
produced in this reaction.
EXPERIMENT 48
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Bromine dissolves fairly well in pure formic acid, but no redox reaction
occurs, not even on heating. When water is added to the mix, then a redox
reaction sets in, in which bubbles of gas are produced (probably CO2).
EXPERIMENT 49
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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 50
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When concentrated hydrochloric acid is added to solid NaClO2, then a lot of
intense yellow ClO2 is produced, but normally the gas does not explode.
When concentrated hydrochloric acid is added to a mix of solid NaClO2 and solid
NaBrO3, then a yellow gas is produced and within a few seconds at most, the gas
explodes, the explosion starting at/near the liquid surface.
EXPERIMENT 51
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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 52
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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 53
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Chlorite ion and chlorine dioxide are sluggish oxidizers when in aqueous
solution, even in the presence of quite some acid. Bromide ion only is oxiduzed
very slowly and only partially.
EXPERIMENT 54
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An acidified solution of potassium bromate quickly oxidises solid potassium
nitrite to potassium nitrate, the bromate being converted to bromine.
EXPERIMENT 55
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Bismuth(III) in aqueous nitric acid solution does not form a precipitate with
bromate ion.
End of results for 'Br'