Experiments for 'potassium permanganate'
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 permanganate':
EXPERIMENT 1
---------------
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
---------------
Persulfate is not capable of oxidizing manganese to the (VII) state
in acidic environments.
EXPERIMENT 3
---------------
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
---------------
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
---------------
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
---------------
Potassium permanganate easily oxidizes oxalic acid. Succinic acid is not
oxidized easily.
EXPERIMENT 7
---------------
Manganese (II) ions apparently do not form coordination complexes with EDTA.
If they do so, then the coordination complex is (almost) colorless.
EXPERIMENT 8
---------------
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
---------------
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
---------------
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
---------------
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
---------------
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 13
---------------
When ethanol and acetone are mixed, together with sulphuric acid, then no
special visible reaction occurs. The compounds are bound to the acid. Their
smell hardly exists after mixing with the acid.
The mixture is not capable anymore of producing HCl from NaCl, nor does it
show a strong reaction with KMnO4 (as was expected, due to the presence of
concentrated H2SO4).
EXPERIMENT 14
---------------
Potassium permanganate dissolves in acetone and in MEK. In the latter,
however, it dissolves in smaller quantities.
EXPERIMENT 15
---------------
MEK can be oxidized by potassium permanganate in alkaline environments (or
is this due to some impurities in the MEK?).
EXPERIMENT 16
---------------
Copper builds higher oxides than CuO when strong oxidizing agents are
present in alkaline environments. Probably these are not copper (III)
compounds, but the oxo-ion probably is replaced by peroxo or superoxo.
EXPERIMENT 17
---------------
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 18
---------------
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 19
---------------
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 20
---------------
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 21
---------------
When p-aminophenol is oxidized in an acidic environment, then a compound
is formed, with a deep indigo/purple color.
EXPERIMENT 22
---------------
Hydroxyl amine reacts with acetone, releasing (some) heat. After this
reaction, the resulting compound is shown to still be a relatively strongly
reducing agent in alkaline solution.
EXPERIMENT 23
---------------
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 24
---------------
Chlorosulfonic acid is an extremely reactive compound. It reacts violently with
many salts of oxoacids.
End of results for 'potassium permanganate'