Experiments for 'I'
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 'I':
EXPERIMENT 1
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Mercury (II) ions produce a bright orange colored precipitate with iodide.
EXPERIMENT 2
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This is a very nice experiment, involving beautifully coloured compounds,
but it is a hazardous experiment as well, due to the use of mercury (II)
compounds.
Mercury (II) builds a complex with excess iodide, [HgI4]2-, which gives a
beautiful bright yellow precipitate with Ag+ and a beautiful bright brick-
red precipitate with Cu+.
EXPERIMENT 3
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Ferricyanide is capable of oxidizing iodide to iodine, even in neutral
environments. The reaction, however does not appear to go to completion.
EXPERIMENT 4
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Periodate is capable of oxidizing manganese (II) to permanganate completely
in a short period of time. This is one of the rare examples of an oxidizer,
which is capable to oxidize manganese all up to the +7 oxidation state in
aqueous environments.
EXPERIMENT 5
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Iodide ion and sulphur dioxide form a deep orange/yellow complex at high
concentration. At somewhat lower concentration this complex looks deep yellow.
The complex formed in this experiment is {I.nSO2]-.
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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This experiment is performed in order to determine, whether iodoform (CHI3)
shows a reaction, similar to chloroform, when treated with acetone in a
strongly alkaline environment. The result of this experiments suggests
that indeed a similar reaction occurs, resulting in the formation of a
compound with a sweetish mint-like odour.
EXPERIMENT 8
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Copper (I) iodide dissolves in dilute ammonia, resulting in a colorless
liquid. Copper (I) builds a coordination complex with ammonia. This
complex is oxidized by oxygen from the air exceedingly easily.
EXPERIMENT 9
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Copper(I) iodide dissolves in a concentrated solution of potassium iodide.
In such a solution the complex ion CuI2(-) is formed. On dilution, this ion
decomposes and a precipitate of CuI is formed again.
Copper(I) iodide does not dissolve in hydrochloric acid, or just a small
amount dissolves.
EXPERIMENT 10
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Copper(I) iodide darkens on heating, but at the same time it decomposes, giving
deep purple iodine vapor.
EXPERIMENT 11
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Praseodymium (III) ions form complexes with chloride, bromide and iodide. With
fluoride a precipitate is formed.
EXPERIMENT 12
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When vanadyl sulfate is dehydrated by heating, then the resulting solid only
dissolves partially in water and in dilute acid. When a strong oxidizer is
present, all of the solid dissolves again, forming a soluble vanadium species
in the +5 oxidation state.
EXPERIMENT 13
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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 14
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Ammonia reacts with iodine, giving nitrogen iodide, coordinated to ammonia.
When acetone is present, however, then a so called haloform reaction
occurs, resulting in formation of CHI3.
EXPERIMENT 15
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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 16
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Both iodate and periodate form the tetrachloroiodide ion in a strong
solution of hydrochloric acid. A redox reaction occurs, where the iodine
is reduced to its +3 oxidation state and chlorine is released.
EXPERIMENT 17
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The tetrachloroiodide ion is not stable in water at high dilution. It
tends to disproportionate to iodine, choride and iodate.
With sulfite, it is reduced to iodine. With excess sulfite, it is reduced
to iodide.
EXPERIMENT 18
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Potassium tetrachloroiodide decomposes on heating. The residue, which
remains behind is potassium chloride.
EXPERIMENT 19
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Bismuth shows remarkable coordination chemistry with iodide and chloride.
In the absence of chloride, a black precipitate of BiI3 is formed. In the
presence of chloride, a deep yellow/orange compound is formed, but only
if also iodide is present. So this compound must be a complex of bismuth,
iodide and chloride.
EXPERIMENT 20
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Bismuth (III) forms a deep-orange iodo-complex and a yellow iodo-chloro
complex.
EXPERIMENT 21
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Bismuth forms a yellow complex with thiosulfate. In the presence of
thiosulfate, it still forms a deep orange complex with iodide, just as without
thiosulfate.
EXPERIMENT 22
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Tin (II) compounds forms either a yellow or orange/red compound with
iodides. What compound is formed, depends on the concentration of the
reactants.
At very low pH such a compound is not formed anymore, and once formed,
it can be dissolved.
EXPERIMENT 23
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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 24
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Iodoform is only moderately stable. On heating, it decomposes to iodine, carbon
and hydrogen iodide. This process of decomposition looks quite special.
EXPERIMENT 25
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Iodate and formiate react very nearly explosively at high temperature.
EXPERIMENT 26
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Praseodymium ions form a very light green precipitate with periodate, which
almost completely dissolves on heating.
EXPERIMENT 27
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When copper ions are brought in contact with periodate, then a yellow/green
precipitate is formed. This precipitate very easily dissolves in hydrochloric
acid, giving chlorine gas and other products.
When the same is done with manganese(II) ions instead of copper ions, then a
brick-red precipitate is formed, which does not easily dissolve in hydrochloric
acid.
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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Iodine dissolves in thionyl chloride. It does not react. It gives a purple
solution, looking very similar to a purple solution of iodine in an alkane or
chlorinated hydrocarbons.
When water is added, then a remarkable reaction occurs. Sulphur is formed.
EXPERIMENT 30
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Iodoform reacts exothermically with chlorine, one of the reaction products
being iodine. The other products must be substitution products, with iodine
completely or partly replaced by chlorine.
When excess chlorine is used, then iodine monochloride and iodine trichloride
are formed as well. These products react with iodoform as well, resulting in
formation of iodine.
EXPERIMENT 31
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Ammonium iodate can very easily be prepared by adding a slight excess of
ammonia to a solution of iodic acid in water. The dry compound is stable, but
when it is heated, it violently decomposes, but it does not explode.
Ammonium periode can be prepared in a similar way. When ammonium periodate is
heated, then it explodes, giving a cloud of iodine.
EXPERIMENT 32
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Iodine does not react with nitrite in methanolic solution.
Iodine does react with hydroxide in methanolic solution, a very light yellow
compound is formed. On acidification this gives iodine again.
Iodine does react with red phosphorous in methanolic solution, but the reaction
is slow.
EXPERIMENT 33
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Thallium(I) metaperiodate is very much like potassium metaperiodate, but it
decomposes easily due to an internal redox reaction in which thallium(III) is
formed, which forms a precipitate with periodate ion.
EXPERIMENT 34
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Magnesium periodate is soluble in water.
EXPERIMENT 35
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Thallous iodide is insoluble in water and is a beautiful brightly colored
compound, with a color, depending on temperature.
EXPERIMENT 36
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Iodine dissolves somewhat in chlorosulfonic acid with a brown color.
EXPERIMENT 37
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Ethylene diamine (NH2CH2CH2NH2) and iodic acid form a moderately soluble salt.
In the dry state, this salt is fairly stable. Only when it is heated strongly,
it decomposes with a soft puff, giving a yellow/brown smoke and a bad smell.
EXPERIMENT 38
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Antimony reacts with iodine, giving antimony triiodide. This reaction, however,
is not very fast and quite a large excess amount of finely powedered antimony
is needed to get all iodine reacted.
Antimony triiodide (SbI3) has quite remarkable properties. Its solution is pale
yellow/green, the solid has a bright orange/red color and the vapor is
colorless or nearly colorless. The liquid (molten) material is yellow.
EXPERIMENT 39
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Iodide ion and metaperiodate react with formation of iodine. This reaction
occurs, even in the absence of an acid.
EXPERIMENT 40
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Sodium periodate reacts violently with hydroxyl amine hydrochloride in aqueous
solution.
EXPERIMENT 41
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Manganese (II) ions and periodate react with each other, even at room
temperature to form a peculiar brown precipitate with a pink/orange hue.
Certainly not the common dark brown manganese (IV) oxide/hydroxide is formed,
but a much lighter colored precipitate.
EXPERIMENT 42
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Magnesium and potassium tetrachloro iodide do not react when dry, but when a
drop of water is added, then a violent reaction starts, with production of
purple clouds of iodine.
EXPERIMENT 43
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Chromium(III) ions give a light green precipitate with iodate.
EXPERIMENT 44
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Periodate is capable of oxidizing nitrite ion but only very slowly.
EXPERIMENT 45
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Many iodates are insoluble, but manganese(II) ions do not give a precipitate
with iodate ion, nor is there any redox reaction between these ions.
Periodate on the other hand gives a nice brickred precipitate with
manganese(II).
EXPERIMENT 46
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Perchloric acid is very reluctant to reacting with many chemicals. This is
different from what many sites are telling. Perchloric acid only is extremely
reactive when it is anhydrous, the hydrous acid (60 ... 70%) is not that
reactive.
EXPERIMENT 47
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Iodic acid, when heated, first gives off water vapor. When the resulting solid
is heated much stronger, then purple clouds of iodine appear and finally, all
solid is gone.
EXPERIMENT 48
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Calcium iodate is very sparingly soluble in water, but it can form strongly
oversaturated solutions and may take a long time to crystallize.
Calcium iodate also is quite stable, it must be heated strongly in order to
decompose it.
End of results for 'I'