Experiments for 'vanadyl sulfate'
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 'vanadyl sulfate':
EXPERIMENT 1
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Vanadium (IV) as vanadyl cations, is oxidized by persulfate to vanadium (V)
as pervanadyl.
EXPERIMENT 2
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Vanadyl (vanadium (IV)) does not give a coordination complex with ammonia.
It does not dissolve in ammonia. With stronger bases, a brown vanadate (IV)
compound dissolves (a poly-vanadate (IV) compound??).
EXPERIMENT 3
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Vanadium(III) hydroxide apparently forms a precipitate and does not
dissolve in strongly alkaline liquids.
Vanadium (III) and (IV) are oxidized by peroxodisulfate to vanadium (V).
EXPERIMENT 4
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Peroxodisulfate ([S2O8]2-) is capable of oxidizing vanadyl ([VO]2+) to
pervanadyl ([VO2]+), but this reaction proceeds slowly.
EXPERIMENT 5
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Vanadium (III) apparently builds a coordination complex with EDTA in
strongly acidic environments. This complex is brown.
EXPERIMENT 6
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Vanadyl builds an intensely colored complex with thiocyanate in acidic
environments. In alkaline environments this complex is destroyed.
When H2O2 is added, this complex is destroyed as well, but in this
case some heating is required.
EXPERIMENT 7
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The vanadyl salt of ferrocyanide does not dissolve in water. The salt is
easily hydrolysed in alkaline environments (it resembles the prussian blue
as far as this behaviour is concerned).
EXPERIMENT 8
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The vanadyl salt of ferricyanide does not dissolve. The differences between
the ferricyanide salt and ferrocyanide salts are not very clear. In alkaline
solution apparently ferricyanide and vanadate (IV) can coexist.
EXPERIMENT 9
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Vanadyl gives diverse complexes with citrate, the color of these complexes
strongly depends on the pH of the solution.
EXPERIMENT 10
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It is possible to let a liquid completely solidify by making the correct
precipitates. Citrate is very suitable for this, combined with some
transition metals.
EXPERIMENT 11
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Vanadyl ions do not precipitate with ferricyanide, when a large excess
amount of oxalic acid is present. Without the presence of oxalic acid
the two compounds form a green/yellow/brown precipitate (see other
experiments).
EXPERIMENT 12
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Vanadyl ions do not form a special complex with tartaric acid in strongly
acidic environments.
When hydrogen peroxide is added, a complex is formed, but is
this due to the presence of tartaric acid?
When tartaric acid is added to a solution of vanadyl sulfate in an
environment, which is only slightly acidic, then a green complex is
formed. On making the liquid more basic, a vague sequence of color
changes occurs, through grey/blue, finally going to brown.
EXPERIMENT 13
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Oxalic acid does not seem to form a coordination complex with vanadyl ions,
or if a complex is formed, then it has a color, which is almost the same of
the color of aquated vanadyl.
EXPERIMENT 14
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Vanadyl forms a light blue or white compound with phosphates, when it is
precipitated.
In excess alkali, this dissolves, forming a greenish brown clear liquid.
This color is like the familiar brown color of strongly alkaline solutions,
containing vanadium in the +4 oxidation state, but a little bit less reddish
and more greenish.
EXPERIMENT 15
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Vanadyl is oxidized by bromate quickly and completely.
EXPERIMENT 16
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Vanadyl ions apparently do not form a coordination complex with chloride at
extremely high concentration, or the coordination complex has the same color
as the vanadyl-aqua complex.
EXPERIMENT 17
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Without the help of a strong acid, vanadium pentoxide is not capable of
oxidizing formic acid, not even when heated. When some sulfite is added,
then incomplete reduction of the V2O5 can be observed.
With the help of a strong acid and when in solution, vanadium (V) is
capable of oxidizing formic acid, but only very slowly.
With formic acid and vanadium (IV), apparently a coordination complex
is formed. Another explanation is given below at the end of the
description.
EXPERIMENT 18
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Vanadium in the +4 oxidation state is not reduced to vanadium in a lower
oxidation state by borohydride.
EXPERIMENT 19
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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 20
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Vanadyl ion is not reduced by borane to vanadium in a lower oxidation state.
EXPERIMENT 21
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Catechol forms a coordination complex with vanadyl.
EXPERIMENT 22
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The blue vanadyl ion VO(2+), which contains vanadium in oxidation state +4, is
oxidized by oxone (which contains the monopersulfate ion, SO5(2-)) and it also
is oxidized by the peroxodisulfate ion S2O8(2-). Oxidation by monopersulfate is
immediate, oxidation by peroxodisulfate is very slow. The latter reaction can
be sped up by heating, but still it takes tens of seconds on near boiling of
the solution.
The blue vanadyl ion is oxidized to the pale yellow pervanadyl ion VO2(+). On
heating, this pervanadyl ion condenses into more intensely colored ions which
contain multiple VO2(+) units. At a certain point the condensation of the
pervanadyl ions goes so far that a red/orange precipitate is formed of hydrous
vanadium pentaoxide, V2O5.nH2O.
EXPERIMENT 23
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Vanadyl sulfate n-hydrate is dehydrated by hot concentrated sulphuric acid,
giving insoluble solid anhydrous VOSO4. This solid does not dissolve in the
concentrated acid, nor in water.
EXPERIMENT 24
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When a solution of vanadyl sulfate is mixed with excess sodium nitrite, then a
very dark liquid is obtained and some NO is formed. On acidification, this
liquid becomes green/yellow, but on boiling, it becomes blue again and it
appears that all vanadium goes to oxidation state 4 again.
EXPERIMENT 25
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When hydrated sulfate-salts are heated, which only loose water, then their
properties strongly change. The color changes, but also the solubility
properties change a lot. The sulfate salts loose water easily, but no acid
(H2SO4 or SO3).
End of results for 'vanadyl sulfate'