Experiments for 'N'
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 'N':
EXPERIMENT 1
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The hexanitrite cobaltate (III) ion is strongly affected by sulfide. A black
compound is formed. On acidification of this, remarkably, no hydrogen
sulfide is formed. Probably the black compound is a compound containing
sulfide and nitrite in a single compound, which on acidification results
in oxidation of the sulfide.
EXPERIMENT 2
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Cobalt (II) chloride hexahydrate is a red/purple compound. When it is heated,
it becomes blue, first dark blue, lateron much lighter blue. The latter
compound is anhydrous cobalt (II) chloride.
Anhydrous cobalt (II) chloride dissolves with a deep blue color in DMSO. With
nitrite, apparently no complex (or a complex with the same color) is formed,
the solution remains deep blue.
The anhydrous cobalt (II) chloride also dissolves in water without problems.
Such solutions are pink. With nitrite these form yellow complexes on
acidification.
Anhydrous cobalt (II) chloride is not soluble in nitromethane.
EXPERIMENT 3
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Methanol reacts with nitrites in the presence of acid and of water. A
colorless gas is produced. Is this methyl nitrite? Without the water, or
without the acid, no reaction occurs.
EXPERIMENT 4
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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 5
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Tetraethyl ammonium bromide is somewhat flammable. It can be burnt, but a
supporting flame must be present, it does not continue burning on its own.
EXPERIMENT 6
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Dimethylamine borane is very flammable, it easily is ignited and burns
with a beautiful green flame.
EXPERIMENT 7
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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 8
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Silver nitrite is only sparingly soluble in water. When dilute acid is
added, the compound is destroyed again.
EXPERIMENT 9
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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 10
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When copper dissolves in aqua regia, then a colorless gas is produced.
Oxidation apparently proceeds in a different way, when compared with
dissolving copper in nitric acid.
EXPERIMENT 11
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Copper (II) is reduced by hydroxyl amine very quickly in alkaline
environments. Yellow copper (I) hydroxide/oxide is formed.
EXPERIMENT 12
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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 13
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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 14
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Copper (II) chloride dissolves in fairly concentrated nitric acid, but it does
not dissolve easily. Only a small amount can be dissolved. It dissolves with
a bright green/cyan color. Aluminum metal is not attacked by this solution.
Slight dilution does not make the liquid more active towards aluminum. When a
lot of sodium chloride is added, then the aluminum is attacked and it
dissolves.
EXPERIMENT 15
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Nitrite forms a dark green coordination complex with copper (II) ions in
neutral environments. When acidified, then a new coordination complex
(dark blue with a grey hue) is formed in the presence of chloride of
very high concentration. This is not formed when chloride is absent.
EXPERIMENT 16
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Copper (II) chloride and nitrite gives a deep green complex in water. This
combination gives a dark brown complex in DMSO.
EXPERIMENT 17
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Alkanes do not react strongly with NO2. Some NO2 dissolves in them.
EXPERIMENT 18
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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 19
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When concentrated sulphuric acid is added to concentrated nitric acid,
then some heating can be observed.
The mixed acid reacts with tissue, but not as strongly as pure sulphuric
acid does. The mixed acid reacts with copper, but this reaction is not
as strong as the reaction with nitric acid only.
With citric acid and acetone no strong reaction occurs.
EXPERIMENT 20
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Nitric acid, mixed with sulphuric acid is a strong oxidizer. It is capable
of oxidizing iodine to iodate.
EXPERIMENT 21
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Hydroxyl amine is capable of reducing vanadium (V) to vanadium (IV), but
further reduction is not possible with hydroxyl amine.
EXPERIMENT 22
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The result of this experiment is remarkable. Hydroxyl amine, being a strong
reductor, appears to oxidize vanadium (IV) to vanadium (V) in alkaline
environments. Or is there another compound, which strongly resembles the
well-known yellow colour of vanadium (V) in acidic environments and the
(almost) colourless appearance of vanadium (V) in alkaline environments?
EXPERIMENT 23
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Vanadium pentoxide dissolves in ammonia and when heated a white solid is
formed, probably this is ammonium meta vanadate.
EXPERIMENT 24
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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 25
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Aniline, combined with acidified dichromate gives intensely colored compounds.
EXPERIMENT 26
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Aniline gives colored compounds with chromium. The colors are remarkably
intense.
EXPERIMENT 27
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Chromium (III) chloride initially gives a green solution in water, which on
standing turns violet/grey. The chromium/chloride complex slowly is changed to
plain aqueous chromium and free chloride ion. This takes a few days before
completion.
With nitrite ions, a purple complex is formed.
EXPERIMENT 28
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It is not possible to make methylammonium chromate or methylammonium
dichromate by mixing solutions of CrO3 and CH3NH2 in water and letting
the solution evaporate. Apparently, chromic acid is not sufficiently
acidic in aqueous solution to protonate the methylamine to a salt.
This is in strong contract with perchloric acid, which, when mixed
with excess methylamine, gives a nice dry solid CH3NH3ClO4 on evaporation.
This also is in strong contrast with ammonia, which gives a mix of
(NH4)2CrO4 and (NH4)2Cr2O7 when excess ammonia and CrO3 are mixed and
allowed to evaporate to dryness.
EXPERIMENT 29
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Bromide is oxidized by hydrogen peroxide in acidic environments. Addition
of nitric acid strongly enhances the reaction.
EXPERIMENT 30
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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 31
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Sodium bromide is not oxidized by concentrated nitric acid. However, when
a minute quantity of nitrite is added, suddenly the reaction starts and
quickly all bromide is oxidized.
EXPERIMENT 32
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A mixture of chlorine and chlorine dioxide oxidizes bromide quickly to
bromine. When an excess amount of nitrite is added, then the bromine is
quickly reduced again to bromide. Addition of an acid does not result in
formation of bromine again.
EXPERIMENT 33
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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 34
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Nitrite reacts with p-aminophenol violently in alkaline environments.
EXPERIMENT 35
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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 36
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Nitrous vapors react with thiocyanate, building a red/brown compound, which
disappears again, when left in contact with air.
EXPERIMENT 37
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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 38
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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 39
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Nitrites react with ammonium and with hydroxyl ammonium ions. In both cases
a colorless and odourless gas is formed.
EXPERIMENT 40
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Nitrite gives rise to formation of a blue compound with dilute sulphuric
acid, which is not very stable (dissociates into nitrous oxide easily).
When bromide is added, then a brown/green compound is formed, which
is not bromine.
EXPERIMENT 41
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Nitric acid and formalin react vigorously, but some help is needed in
order to start the reaction.
EXPERIMENT 42
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When nitric acid is mixed with hydrochloric acid, then so called aqua regia
is obtained. This is a colorless liquid, which, however, is not very stable
and which decomposes. What are the decomposition products?
EXPERIMENT 43
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Nitrites react with concentrated hydrochloric acid, forming a brown/orange
compound, which remains dissolved in the acid. When the acid is diluted
with water, then this orange compound is destroyed (probably it hydrolyses,
due to lower concentration).
EXPERIMENT 44
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Thiocyanate is oxidized by nitrate very violently under the right conditions.
EXPERIMENT 45
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Methanol gives a colorless gas with nitrite in acidic media. No formation
of NO/NO2. This compound probably is CH3ONO, the nitrite ester of methanol.
The large excess of CH3OH does not prevent formation of nitrosyl thiocyanate.
EXPERIMENT 46
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Methanol and nitrate/nitric acid do not react readily, not even at fairly
high temperature (appr. 90C).
EXPERIMENT 47
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Hydrogen cyanide (or cyanide salt) slowly changes to a dark brown/black
compound, when it is allowed to stand. At least this happens in strongly acidic
media.
EXPERIMENT 48
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Nitromethane gives a dark red/brown liquid in combination with aqueous sodium
hydroxide. This most likely is a polymeric species.
EXPERIMENT 49
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Nitrogen oxides do not dissolve in ligroin. Nitrosyl bromide does. When a
compound with unstaturated C=C bonds is added, then the nitrosyl bromide
does not quickly decompose. It does not react with alkenes and the presence
of alkenes does not cause it to decompose quickly.
EXPERIMENT 50
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Allyl alcohol (having one double bond between carbon atoms) forms a nitrite
ester very easily and this ester is stable, at least for several minutes.
EXPERIMENT 51
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The yellow pigment aureolin, also known as cobalt yellow, and having the
chemical name potassium hexanitrito cobaltate(III), can be used as a mild
oxidizer which gives a very smoothly and evenly burning mix with red
phosphorus. When also aluminium powder is added to the mix, then the reaction
is more violent and sparks are sprayed around.
EXPERIMENT 52
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When a solution of copper sulfate is added to a solution of hydroxyl ammonium
chloride in dilute solution of NaOH, then a dirty green precipitate is formed.
At some places the precipitate becomes yellow. When the liquid is shaken, then
all of the precipitate dissolves and a colorless liquid is obtained. On
standing, a thin layer of solid material is formed on the surface of the
liquid. This layer has a dirty green color.
Hydroxyl amine reduces copper(II) at high pH and a colorless complex of
copper(I) is formed, which at really high pH becomes unstable with formation of
hydrous copper(I) oxide.
EXPERIMENT 53
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Bromine reacts vigorously with hydroxyl ammonium ion. A lot of colorless gas is
produced in this reaction.
EXPERIMENT 54
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Sodium sulfite reacts vigorously with 68% nitric acid.
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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When ethylene diamine is added to anhydrous copper sulfate, then no complex is
formed. When a little water is added, then suddenly a deep blue/purple complex
is formed. Apparently, some water is needed for formation of the ethylene
diamine complex.
EXPERIMENT 58
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Copper(II) ions are capable of forming a mixed azide/ammonia complex which has
energetic properties.
EXPERIMENT 59
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A solution of tetrathionate reacts with nitrite in acidic solution. A green
compound is formed, which however is unstable and after a few minutes, the
solution decomposes. It becomes turbid and light yellow. Most likely the yellow
material is finely divided sulphur.
EXPERIMENT 60
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Sulphur and Carbon are mixed,
Potassium Nitrate is dissolved in hot water and the Sulphur/Carbon mix is
added.
Pure Isopropanol is added, and dehydrates the water, allowing the KNO3 and S/C
to mix closely.
The wet powder is filtered via a vacuum filter, and is dried using ambient
heat.
This produces fast-burning gunpowder.
EXPERIMENT 61
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Diethylamine does not as easily form typical ammine-like complexes, like
ammonia.
EXPERIMENT 62
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Nitric acid does not show a violent reaction with hydrazine, but instead, a
white solid is formed, which does not dissolve well in the concentrated acid.
Nitrogen oxides do not trigger a reaction, even when these are present, the
reaction with the hydrazine does not set off.
EXPERIMENT 63
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The hexanitritocobaltate (III) ion is quite stable, but at very low pH, it is
destroyed either by reducing agents, or by coordinating agents. But the nitrito
ligand is MUCH more stable than in the plain nitrite ion.
EXPERIMENT 64
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Sodium hypophosphite does not react with 68% nitric acid when mixed in the
cold. When the mix is heated somewhat, then the reaction suddenly sets off and
is self-sustained.
EXPERIMENT 65
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When sodium sulfide and sodium nitrite are mixed as solids, or when mixed in
aqueous solution, no reaction occurs. Sulfide ion and nitrite ion can coexist
in solution.
When a very small amount of acid is added, a bright yellow/ochre solid compound
is formed, which slowly turns lighter. When more acid is added, then the solid
becomes almost white.
The very light yellow, almost white compound most likely is very finely divided
elemental sulphur. The much brighter yellow/ochre definitely is not sulphur,
its color is too strong and also differs quite a lot from the kind of yellow of
sulphur.
EXPERIMENT 66
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Ethylene glycol forms a nitrite ester quite easily. Most likely, the ester
formed is a di-ester, on both hydroxyl groups of the glycol.
EXPERIMENT 67
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Titanium metal slowly dissolves in concentrated hydrochloric acid and then
forms a very dark solution of a titanium/chloride complex. This solution is
much darker than an aqueous solution of titanium(III) in which the ions are
present as aqua complex.
With thiocyanate an even more intensely colored complex is formed. This complex
has the same color, but it is very dark.
EXPERIMENT 68
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When thiosulfate ion and nitrite ion are brought together in solution, then
nothing happens. When the solution is acidified, then a remarkable reaction
occurs. The liquid then quickly turns dark brown and remains clear. Immediately
after that, a colorless gas is produced and the color becomes lighter. The
color goes from dark brown through brown/orange and yellow to lime green. The
liquid remains clear and lime green for a few minutes and then it slowly
becomes turbid.
EXPERIMENT 69
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Hydroxyl ammonium ion and nitrite ion, when brought together give rise to
formation of dinitrogen oxide and under certain condition also NO can be
formed.
EXPERIMENT 70
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Thionyl chloride and copper nitrate react with each other, giving gaseous
products and solid anhydrous copper(II) chloride remains behind.
EXPERIMENT 71
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When trichloroisocyanuric acid and sodium nitrite are mixed then no reaction
occurs. As soon as some water is added a fairly vigorous reaction starts. A
brown gas mix is produced, and the material starts foaming. The gas inside the
foam bubbles is colorless and only when bubbles pop, a brown gas is observed.
EXPERIMENT 72
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Sodium periodate reacts violently with hydroxyl amine hydrochloride in aqueous
solution.
EXPERIMENT 73
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Nitrite ion reacts very easily with ethanol in acidified solution to form ethyl
nitrite. The ethyl nitrite easily escapes as gas from the liquid (it has a
boiling point of 17 C). The gas can be ignited and burns with a grey flame.
EXPERIMENT 74
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Hydroxyl ammonium ion and bromate ion react with each other, but with a delay.
Once the reaction starts, it is EXTREMELY violent.
EXPERIMENT 75
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Azide ion reacts with hypochlorite, giving a yellow compound, which is
colorless in the gaseous state. This compound can easily be ignited and
explodes with a really loud report, even when very small quantities are used.
EXPERIMENT 76
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Methylene chloride is capable of extracting nitric acid from its aqueous
solution.
EXPERIMENT 77
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An acidified solution of potassium bromate quickly oxidises solid potassium
nitrite to potassium nitrate, the bromate being converted to bromine.
EXPERIMENT 78
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Nitrite ion is very unstable in concentrated hydrofluoric acid. Although the
acid only is a weak acid, it forces complete decomposition of the nitrite ion
and potassium fluoride remains behind in solution.
EXPERIMENT 79
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Copper(II) ions and azide ion give rise to formation of an intensely dark
colored precipitate/complex.
EXPERIMENT 80
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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 81
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Finely divided magnesium powder violently reacts with wet cupric nitrate and
with wet ferric nitrate. The dry solids do not react.
EXPERIMENT 82
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Chlorosulfonic acid is an extremely reactive compound. It reacts violently with
many salts of oxoacids.
EXPERIMENT 83
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Periodate is capable of oxidizing nitrite ion but only very slowly.
EXPERIMENT 84
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Chlorite ion and nitrite ion react with each other in acidic medium, giving off
quite some heat, while this does not occur with chlorate and nitrite.
EXPERIMENT 85
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Concentrated nitric acid does not react violently with hydrazine at low
temperature. When the acid is heated, then a reaction occurs. It is remarkable
that such a strong oxidizer does not immediately decompose hydrazine.
EXPERIMENT 86
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Cyanate ion forms complexes with many metal ions. These complexes have a strong
color and are not stable in acidic solution.
EXPERIMENT 87
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Sodium chlorite and sodium nitrite do not react with each other in neutral
solution, but when acid is added, they react extremely violently, possibly
explosively.
EXPERIMENT 88
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Thiourea is oxidized in acidic solution to formamidine disulfide, which exists
in solution as an acid salt. When a strong base is added, then the free base is
formed, but this at once decomposes. One of the decomposition products is
sulphur.
When excess oxidizer is used and the pH is increased strongly, then the sulphur
dissolves, giving rise to formation of polysulfides.
End of results for 'N'