Experiments for 'sodium nitrite'
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 'sodium nitrite':
EXPERIMENT 1
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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 2
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The hexanitrito cobaltate (III) ion can be reduced by SO2 to cobalt (II),
but this reduction requires heating. Some brown compound remains, this
probably is due to the inertness of many cobalt (III) coordination
complexes. With nitrite, a brown complex is formed again. This differs
from the gold/yellow hexanitrito cobaltate (III).
EXPERIMENT 3
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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 4
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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 5
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Ferrocyanide is oxidized quickly by nitrite in acidic environments. On
prolonged standing, a darker green/brown compound is formed.
EXPERIMENT 6
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Iron (III) forms a very dark brown/red coordination complex with nitrite,
both in water and in DMSO. On acidification, this complex decomposes, giving
a bright yellow solution with a slight green tinge.
EXPERIMENT 7
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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 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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Nitrous acid (or its decomposition product) forms a dark brown coordination
complex with ferric ions. With copper (II) also a coordination complex is
formed. In relatively strongly acidic environments, these coordination
complexes are destroyed/not formed.
EXPERIMENT 10
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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 11
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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 12
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Chromium (III) builds a coordination complex with nitrite of a fairly
intense purple color.
EXPERIMENT 13
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Dichromates are not capable of oxidizing nitrite in neutral environments.
When some acid is added, then the oxidation proceeds, but a fairly low
pH is needed for a fast and complete reaction.
EXPERIMENT 14
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Chromium (III) forms a purple coordination complex with nitrite. This
complex has a fairly bright pink/purple color, which differs quite a lot
from the color of aqueous chromium (III).
EXPERIMENT 15
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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 16
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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 17
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Titanium slowly dissolves in concentrated hydrochloric acid, forming deep
blue/violet titanium (III) ions. On addition of hydrogen peroxide these are
oxidized to titanium (IV), which in turn forms a deep red coordination
complex with hydrogen peroxide.
The deep red coordination complex is only stable in acidic to neutral media.
It also is easily reduced by nitrite. It is not affected strongly by
persulfate. With fluoride, a light yellow compound is formed, but the
formation of that may also be due to rise of pH.
EXPERIMENT 18
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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 19
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Nitrous vapors react with thiocyanate, building a red/brown compound, which
disappears again, when left in contact with air.
EXPERIMENT 20
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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 21
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Nitrites react with ammonium and with hydroxyl ammonium ions. In both cases
a colorless and odourless gas is formed.
EXPERIMENT 22
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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 23
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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 24
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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 25
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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 26
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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 27
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Iodine does not react with nitrite in methanolic solution.
Iodine does react with hydroxide in methanolic solution, a very light yellow
compound is formed. On acidification this gives iodine again.
Iodine does react with red phosphorous in methanolic solution, but the reaction
is slow.
EXPERIMENT 28
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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 29
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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 30
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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 31
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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 32
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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 33
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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 34
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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 35
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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 36
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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 37
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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 38
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Chlorosulfonic acid is an extremely reactive compound. It reacts violently with
many salts of oxoacids.
EXPERIMENT 39
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Periodate is capable of oxidizing nitrite ion but only very slowly.
EXPERIMENT 40
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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 41
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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.
End of results for 'sodium nitrite'