Experiments for 'ammonia'
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 'ammonia':
EXPERIMENT 1
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Cobalt (II) appears to react with ammonia, but only when an oxidizer
is available. The resulting compound has an intense color.
EXPERIMENT 2
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Cobalt (II) is stable in acidic environments, but in alkaline environments
in the presence of ammonia it reacts with oxygen from the air, resulting
in the formation of a dark red/brown coordination complex.
EXPERIMENT 3
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Cobalt carbonate does not dissolve completely in dilute mineral acids. With
some heating, however, it does dissolve completely.
With nitrite a yellow/orange complex is formed, which forms a precipitate
when treated with alkalies. The precipitate is resistant to treatment with
acid and bases.
EXPERIMENT 4
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Cobalt forms many complexes with ammonia and it forms these complexes
easily, but when cobaltosic oxide (Co3O4, black oxide) is used, then no
such reactions can be observed. Co3O4 appears to be very inert.
EXPERIMENT 5
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Cobalt (II) salts give a blue/green precipitate when dilute ammonia is added.
This precpitate is fairly stable towards air. When more concentrated ammonia
is used, then a dark brown compound is formed, but this compound is formed
by contact with air. On addition of hydrogen peroxide also a very dark
brown compound is formed.
When the pH is increased strongly, then the blue precipitate is not stable
anymore, instead a dark bright blue compound is formed, which, however,
quickly turns pink.
When a large amount of ammonia is replaced by ammonium, then the blue
precipitate is not formed anymore, but a coordination complex is formed,
which is very easily oxidized by oxygen from the air.
EXPERIMENT 6
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In this experiment, some of Werner's experiments are repeated. Here it is
shown that cobalt forms beautifully colored carbonato complexes. The exact
complex formed, depends on the experimental conditions. It is remarkable
what kinds of reactions are shown by cobalt in its complexes and it is
really difficult to precisely determine what is happening and it even is
difficult already to get the same results without precisely specifying the
exact experimental conditions (e.g. using HCl instead of H2SO4 already
results in a different outcome).
EXPERIMENT 7
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Mercury (II) salts give an oxide/hydroxide, which does not dissolve in
large excess amounts of alkaline solutions. Ammonia does not dissolve
the precipitate of mercury (II) oxide/hydroxide.
EXPERIMENT 8
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Iron (III) builds a coordination complex with phosphates.
EXPERIMENT 9
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Ferrocyanide reacts with hydrogen peroxide, forming a fairly intensely
colored yellow compound (probably ferricyanide), but this reaction was
expected to make the liquid more alkaline, but this cannot be observed.
EXPERIMENT 10
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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 11
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Tetraethyl ammonium ion does not form a sparingly soluble salt with bromate
ion.
The tetraethyl ammonium ion forms an oily compound, when treated with
bromate and hydrochloric acid. The halogen, released in that reaction
apparently forms a liquid organic, insoluble in water, or is a liquid
ionic compound formed, some tetraethyl ammonium polyhalogenide compound???
There is evidence for the latter (see experiment detailed description).
EXPERIMENT 12
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When aqueous ammoniacal silver is reduced by glucose, a nice silver mirror
is produced.
Peroxosulfate is capable of oxidizing silver to a higher oxidation state
(+2 or +3), even in acidic environments.
EXPERIMENT 13
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Silver is coordinated by thiosulfate. The silver-thiosulfate complex does
not show any of the reactions of free aqueous silver (I).
EXPERIMENT 14
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Silver (I) is not reduced by hydroxyl amine in neutral environments. When
made alkaline, it is reduced to metallic silver immediately.
EXPERIMENT 15
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Silver (I) gives a white precipitate with thiocyanate, which does not dissolve
in excess ammonia. Hydroxyl amine does not affect this precipitate.
EXPERIMENT 16
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Silver (I) does not give a precipitate with hydroxyl amine sulfate (if
concentrations are not too high), but ammonia causes formation of a
precipitate, which does not dissolve in excess ammonia.
EXPERIMENT 17
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Copper (II) reacts with thiocyanate in a complex way.
EXPERIMENT 18
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Copper (II) reacts with thiocyanate in a complex way.
EXPERIMENT 19
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Copper (II) reacts with ferrocyanide and builds a fairly stable compound.
EXPERIMENT 20
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Vitamin C is a strong reductor in alkaline environments. Copper (II) is
reduced to copper (I).
EXPERIMENT 21
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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 22
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Copper builds a complex with urea, which has a pale purple color (or is
this due to contamination of the urea with traces of biuret?). The copper,
bound to urea, does not build the intense blue cuprammine complex with
ammonia.
EXPERIMENT 23
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When tetraammine-copper (II) is reduced by dithionite in excess ammonia,
then a colorless copper (I) complex is formed, which remains dissolved.
EXPERIMENT 24
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Decomposition of hydrogen peroxide is catalyzed by cuprammine complex.
EXPERIMENT 25
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In alkaline environments, copper (II) shows remarkable behavior, when brought
in contact with strong oxidizers or reductors.
EXPERIMENT 26
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Hydroxyl amine sulfate (containing protonated hydroxyl amine) is not capable
of reducing copper (II). When the liquid becomes basic (releasing free
hydroxyl amine), then the copper (II) is reduced to copper (I).
EXPERIMENT 27
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Copper builds a remarkable complex with ascorbic acid and is easily
reduced by ascorbic acid in alkaline environments. Copper (II) builds
a brown compound with hydrogen peroxide in alkaline environments.
EXPERIMENT 28
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Copper and nickel carbonates (basic), which do not dissolve in water, do
dissolve in ammonia, due to formation of a complex with ammonia.
Cobalt carbonate also dissolves, but now an additional reaction occurs,
taking up oxygen from the air.
EXPERIMENT 29
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Copper (II) is reduced by sulfite. With chloride the resulting copper (I)
can be kept in solution. The copper (I) compound is very susceptible
to oxidation by oxygen from the air.
EXPERIMENT 30
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Copper (II) amine complex is reduced to a colorless copper (I) amine
complex by hydroxyl amine. The copper (I) complex is oxidized by oxygen
from the air very easily.
EXPERIMENT 31
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When copper (II) is present in hydrochloric acid, then it does not react
immediately with hydroxyl ammonium, some heating is required to have a
reaction, resulting in formation of a dark green/brown compound. When the
liquid is made alkaline with excess ammonia, then it quickly becomes
colorless, due to reduction of copper (II) to copper (I), which forms a
colorless complex with ammonia.
A very peculiar reaction occurs on oxidation by oxygen from air. The liquid
is covered by a very thin shiny layer, looking like a strongly coloured oil
on water. It is not clear what it is, more research is needed.
EXPERIMENT 32
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Copper (II) chloride is reduced by hydroxyl amine, when dissolved in
ethanol. First, the solution becomes much darker and apparently, a mixed
oxidation state complex of copper (I) and copper (II) is formed. Finally,
all copper (II) is reduced to copper (I).
This experiment is another example, which shows that copper (I) and copper
(II), when in solution at the same time, form a highly colored complex.
EXPERIMENT 33
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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 34
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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 35
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Sulfide reacts with metavanadates, resulting in the formation of a dark
brown/greenish compound.
EXPERIMENT 36
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Vanadium pentoxide dissolves in ammonia and when heated a white solid is
formed, probably this is ammonium meta vanadate.
EXPERIMENT 37
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Vanadium pentoxide reacts with ammonia, producing a strong hissing noise.
A white compound is created. This probably is ammonium metavanadate,
NH4VO3.
EXPERIMENT 38
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Vanadium in its +4 oxidation state forms a blue compound, vanadyl, in acidic
environments. In near neutral to alkaline environments, the situation is
less clear. Reduction of neutral or alkaline vanadium (V) compounds yields
a dark and turbid liquid.
Vanadium in its +5 oxidation state gives light yellow compounds in mildly
alkaline environments. Al lowering the pH, the color becomes more intense,
until a maximum is reached. When the pH is lowered even more, then lighter
yellow compounds are formed again.
Vanadium (IV) cannot coexist with hydrogen peroxide. In alkaline media it
is oxidized to vanadium (V), which with excess peroxide gives a yellow
peroxo complex. In acidic media, vanadium (IV) is oxidized to vanadium (V)
which gives a deep brown/red peroxo complex with excess poroxide.
EXPERIMENT 39
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When Cr3+ is added to an aqueous solution of ammonia, then a precipitate
is created, which does not dissolve on addition of much more ammonia.
EXPERIMENT 40
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Chromium (III) does not quickly build a coordination complex with ammonia,
such as is the case with copper (II) and nickel (II). Even in a slightly
alkaline environment of dilute ammonia, chromium (III) can be oxidized to
chromium (VI) by the action of hydrogen peroxide. Reduction, back to
chromium (III) is not easily accomplished in alkaline environment.
EXPERIMENT 41
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The color of chromium (III) depends on how it is part of coordination
complexes.
EXPERIMENT 42
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Chromium (III) apparently builds a coordination complex with hydroxyl amine,
but this complex does not simply form from chromium (III) salts and
hydroxyl amine. If chromium (III) is formed by means of reduction of
chromium (VI) in the presence of hydroxyl amine, then the complex is
formed. If hydroxyl amine is added to chromium (III) without redox reaction,
then another complex is created.
EXPERIMENT 43
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Hydroxyl amine gives a brown coordination complex when it reduces hexavalent
chromium to trivalent chromium in alkaline environments. This coordination
complex is really due to the hydroxyl amine. When other reducing agents are
used in the presence of ammonia in alkaline environments, then no similar
reaction product can be obtained.
EXPERIMENT 44
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Aniline, combined with acidified dichromate gives intensely colored compounds.
EXPERIMENT 45
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Aniline gives colored compounds with chromium. The colors are remarkably
intense.
EXPERIMENT 46
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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 47
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TCCA reacts with ammonia. With 5% ammonia the reaction already is very
vigorous, producing copious amounts of white smoke. With 15% ammonia the
reaction is VERY violent, almost explosive.
EXPERIMENT 48
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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 49
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Analysis of the composition of the dutch coin 'dubbeltje' shows that it
does not contain any copper or just a very small quantity of it.
EXPERIMENT 50
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Adding ammonia to a Ni2+ solution results in formation of a purple/blue
coordination complex.
EXPERIMENT 51
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Nickel in nickel (II) hydroxide is oxidized to a higher oxidation state by
hypochlorites, but not by chlorates. The oxidation product is reduced by
hydrogen peroxide and ammonia. Heating of the oxidation product makes it
more resistant to reduction and to breakdown by acids.
EXPERIMENT 52
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Diverse phenol-derivatives, can be oxidized easily by bromine, yielding
intensely colored oxidation products.
EXPERIMENT 53
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Thiocyanate is oxidized by nitrate very violently under the right conditions.
EXPERIMENT 54
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Titanium(III) ions are fairly stable in acidic media, but in alkaline solution,
these become so strongly reducing that hydrogen gas is formed and water is
reduced!
EXPERIMENT 55
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Hydrazine seems to be able to reduce copper(II) to copper(I) in mildly acidic
environments. In alkaline environments the reaction is fast and most likely
elemental copper is produced in the reaction.
EXPERIMENT 56
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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 57
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Dichromate/chromic acid is reduced by malic acid and in this reaction an
intensely colored purple complex of chromium(III) is formed. If the reaction is
performed in the presence of an excess amount of strong non-coordinating acid,
then the reaction proceeds faster, and also a purple complex is formed, but the
color is much less intense.
Without the extra acid, there really is a new complex with chromium(III). This
complex reacts with ammonia, giving a nice green solution.
EXPERIMENT 58
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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 59
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Thallium(I) ion is fairly easily oxidized to thallium(III). In neutral aqueous
solutions, this ion hydrolyzes to a dark hydrous oxide, which forms a compact
precipitate. The dark oxide easily can be dissolved in nitric acid, such that a
colorless solution of thallium(III) nitrate is formed in nitric acid.
Thallium(III) ion forms an ochre/yellow color with ferricyanide ion, which is
stable at low pH, but at high pH this decomposes, giving a yellow solution of
ferricyanide and a dark brown suspension of hydrous thallic oxide.
EXPERIMENT 60
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When antimony is added to liquid bromine, then a violent reaction occurs, even
with appearance of sparks.
End of results for 'ammonia'