Experiments for 'potassium iodide'
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 iodide':
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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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 5
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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 6
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Tungstate ions, when reduced, produce a deep blue color. Tungstate is
a weak oxidizer.
EXPERIMENT 7
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Lead (II) forms a brightly colored precipitate with iodide ions.
This precipitate is soluble in water fairly well, when hot.
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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A large set of compounds is checked on interaction with concentrated
nitric acid. Many reductors react violently with nitric acid.
EXPERIMENT 11
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Nitric acid, mixed with sulphuric acid is a strong oxidizer. It is capable
of oxidizing iodine to iodate.
EXPERIMENT 12
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Praseodymium (III) ions form complexes with chloride, bromide and iodide. With
fluoride a precipitate is formed.
EXPERIMENT 13
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Molybdate gives rise to all kinds of complexes, when combined with reducing
agents. These complexes can be yellow, green or blue. The composition of
all these complexes is not very clear.
EXPERIMENT 14
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Molybdate gives a yellow complex with iodide. Order of dissolving and
acidifying has influence on the reactions observed.
EXPERIMENT 15
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Molybdenum trioxide dissolves well in strongly alkaline liquids. It does
not dissolve (or just a little bit) in plain water. Once dissolved, it
can be kept in solution, even when pH is lowered.
Molybdates are capable of oxidizing iodide and sulfite.
EXPERIMENT 16
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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 17
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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 18
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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 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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Thiocyanate reacts with nitrogen dioxide to form a red/brown compound. It
does not react with nitrogen monoxide. When a reaction occurs with NO2,
a white fume is produced.
EXPERIMENT 25
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Arsenate ion and arsenic acid cannot easily be reduced to the element.
Reduction to trivalent arsenic, however, can easily be accomplished with
iodide.
EXPERIMENT 26
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Mercurous ions are stable in aqueous solution at room temperature. They do not
hydrolyse, nor disproportionate.
However, when a compound is added, with which a stable mercury(II) complex is
formed, or with which a stable mercury(II) precipitate is formed, then the
mercury(I) disproportionates to the metal and mercury(II).
EXPERIMENT 27
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Thallous iodide is insoluble in water and is a beautiful brightly colored
compound, with a color, depending on temperature.
EXPERIMENT 28
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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.
End of results for 'potassium iodide'