Experiments for 'Mn'
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 'Mn':
EXPERIMENT 1
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Aluminium (III) does not form colored compounds with ferrocyanide nor with
ferricyanide. Manganese (II) reacts with both of them, but a colored
compound is formed with ferricyanide only.
EXPERIMENT 2
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Persulfate is not capable of oxidizing manganese to the (VII) state
in acidic environments.
EXPERIMENT 3
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Persulfate is capable of oxidizing Mn2+ in acid environments, but silver (I)
is needed as a catalyst. Oxidation, however, is not easy and just a small
part is oxidized to permanganate, a large part is oxidized no further than
MnO2.
EXPERIMENT 4
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This experiment shows two things:
1) Permanganate can be reduced by metabisulfite, but the reduction does
not proceed instantaneously when no additional acid is used.
2) Manganese sulfide is a dirty pink substance (color of flesh).
EXPERIMENT 5
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Permanganate is capable of oxidizing thiocyanate in acidic environments:
The result is a pink solution, more intensely colored than manganese (II)
ions (which are almost colorless).
EXPERIMENT 6
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Potassium permanganate easily oxidizes oxalic acid. Succinic acid is not
oxidized easily.
EXPERIMENT 7
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Manganese (II) ions apparently do not form coordination complexes with EDTA.
If they do so, then the coordination complex is (almost) colorless.
EXPERIMENT 8
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Permanganate is a strong (and dangerous) oxidizer, when combined with
concentrated sulphuric acid. It is capable of lighting paper and acetone,
without the use of matches.
Permanganate, mixed with a mixture of nitric acid and sulphuric acid is
a strong oxidizer as well, but not as powerful as when mixed with
sulphuric acid only.
EXPERIMENT 9
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When solid potassium permanganate is added to concentrated hydrochloric
acid, then a gas is evolved, being chlorine. The liquid becomes almost
black. When the reaction is driven to an end by heating (almost boiling)
the liquid, then the final liquid does not become colorless, but green.
The green color is not a bright green, but it is brownish/sepia-like.
What is the constitution of this green/sepia compound?
A similar observation is done when hydrochloric acid is heated with
manganese dioxide. In the cold there is no visible reaction, but when
heated, chlorine is produced and a green compound is formed.
EXPERIMENT 10
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Manganese builds a coordination complex with EDTA, which appears to be
pink. What oxidation state does the manganese have with this complex? It
appears to have oxidation state 2, unless EDTA is easily oxidized by
manganese, having a higher oxidation state.
EXPERIMENT 11
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Manganese (II) gives an off-white precipitate with ferrocyanide and it gives
a dark brown precipitate with ferricyanide. The brown compound probably is
a manganese (IV) compound, formed through oxidation by ferricyanide.
EXPERIMENT 12
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Manganese (II) forms a white precipitate with bicarbonate, while slowly
developing a gas (probably this is CO2). This precipitate is not quickly
oxidized by oxygen from the air. When the precipitate is made more alkaline
by adding hydroxide, then it is oxidized fairly quickly. Addition of
hydrogen peroxide causes immediate oxidation of the alkaline precipitate.
EXPERIMENT 13
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Permanganate is capable of oxidizing formic acid quickly, itself being
reduced to manganese (IV). Sulfite is needed to bring the manganese to
the +2 oxidation state.
EXPERIMENT 14
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Manganese (II) is not reduced to the metal, it forms a white precipitate
with borohydride, which remains white for a long time. This precipitate
does not turn brown, as manganese (II) precipitates normally do in
alkaline environments.
EXPERIMENT 15
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In concentrated phosphoric acid, manganese (II) ions are oxidized easily to
manganese (III) ions, which are stabilized by formation of a phosphato-complex
with a remarkably bright purple color. This reaction is remarkable in the sense
that oxidation stops at manganese (III).
EXPERIMENT 16
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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 17
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Potassium permanganate dissolves in acetone and in MEK. In the latter,
however, it dissolves in smaller quantities.
EXPERIMENT 18
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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 19
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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 20
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Permanganate is not capable of oxidizing nickel (II) in an acidic
environment. In an alkaline environment it appears to be possible to
oxidize nickel (II) with permanganate.
EXPERIMENT 21
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This experiment describes a qualitative method, useful for showing the
presence of minute quantities of manganese (II), which cannot be detected
by oxidation with H2O2 in alkaline environments anymore. Chloride ions
may not be present besides the manganese to be detected.
EXPERIMENT 22
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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 23
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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 24
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A mix of aluminium powder and potassium permanganate is hard to ignite. When a
small amount of sulphur is added, then the mix is easily ignited, and a very
bright and fast burning flash is produced.
EXPERIMENT 25
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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 26
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Chlorosulfonic acid is an extremely reactive compound. It reacts violently with
many salts of oxoacids.
EXPERIMENT 27
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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 28
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When compounds of manganese(IV) or manganese(VII) are added to hydrochloric
acid, then chlorine gas is produced and the solution becomes very dark
brown/green. Only after a long time of heating, all dark brown/green material
is gone and what remains is a pale solution, containing manganese(II) ions.
In this series of experiments it was attempted to go the other way around. Is
it possible to go from almost colorless manganese(II) to the dark colored
compounds of manganese(III) or manganese(IV). This was done by adding chlorine
to solutions of manganese(II) salts in concentrated hydrochloric acid.
While doing so, an interesting observation was made. The dark colored compound
indeed can be made from manganese(II) in concentrated hydrochloric acid, but
only from hypochlorite and not from chlorine.
When calciumhypochlorite is added to hydrochloric acid, then chlorine is formed
vigorously, and the solution becomes green and clear.
It seems, however, that even in concentrated hydrochloric acid some of the
hypochlorite is not decomposed at once, but remains in solution as yellow/green
hypochlorous acid.
A freshly prepared solution, made from a pinch of calcium hypochlorite and
concentrated hydrochloric acid, reacts differently than a saturated solution of
chlorine in concentrated hydrochloric acid. This is shown with manganese(II)
ions in hydrochloric acid.
End of results for 'Mn'