Experiments for 'potassium bromide'
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 bromide':
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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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 4
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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 5
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Aluminum reacts vigorously with water, when its passivating layer of oxide
is effectively destroyed. This can be achieved by using tetrachloro or
tetrabromo complexes of copper (II).
Acid can also be used to destroy the passivating layer, but this takes
considerably more time.
Cobalt has a similar effect as copper (II), but it is less pronounced.
EXPERIMENT 6
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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 7
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Silver bromide is reduced by metol in alkaline medium.
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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Bromide is oxidized by hydrogen peroxide in acidic environments. Addition
of nitric acid strongly enhances the reaction.
EXPERIMENT 10
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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 11
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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 12
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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 13
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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 14
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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 15
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Aluminium reacts violently with bromine.
EXPERIMENT 16
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Phosphoric acid is not capable of driving off hydrogen bromide from
alkali bromides, nor does it oxidize bromide.
EXPERIMENT 17
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Bromine reacts with acetylene gas. The bromine disappears and a compound
is formed with a peculiar sweetish smell.
EXPERIMENT 18
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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 19
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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 20
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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 21
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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 22
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When a solution of manganese(II)chloride in moderately concentrated
hydrochloric acid is electrolysed, then at the anode a remarkable very dark
compound is formed. The liquid remains clear, but it becomes very dark. This
must be a compound of manganese in higher than +2 oxidation state.
When a similar experiment is performed with manganese(II)sulfate in a 20%
solution of sulphuric acid, then a drk brown precipitate is formed at the
anode.
EXPERIMENT 23
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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.
End of results for 'potassium bromide'