Experiments for 'C'
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 'C':
EXPERIMENT 1
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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 2
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Acetone can be mixed with water in any ratio, but when sodium hydroxide
is added, then the liquids are not miscible in any ratio anymore.
Sulphur reacts with acetone in the presence of sodium hydroxide. Sulfide
does not show such a reaction.
EXPERIMENT 3
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Sulphur dissolves in hot solutions of sodium hydroxide and disproportionates
in a way, similar to disproportionating of halogens.
When acetone is added, a peculiar blue/green compound is formed in the
acetone. What is this compound?
EXPERIMENT 4
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Acetone and chloroform react with each other in strongly alkaline
environments, building a compound, called chloretone or chlorbutol.
Formal name of the compound is 1,1,1-trichloro 2-methyl 2-propanol,
formula CCl3 C(CH3)(OH) CH3.
A similar reaction is observed, when MEK is used instead of acetone,
but the reaction is much less vigorous.
EXPERIMENT 5
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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 6
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Oxalic acid is supposed to react with sulfuric acid, forming carbon monoxide.
The experiment, described below, however, did not yield such results.
EXPERIMENT 7
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Ethanol and acetic acid do not form an ester (ethylacetate) when simply
mixed with concentrated sulphuric acid. More extreme conditions are needed
for this reaction to occur.
The acid is diluted too much in order to give a strong reaction with
chlorate, combined with the reducing agent in the form of ethanol.
EXPERIMENT 8
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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 9
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Acetone reacts with sulphur in strongly alkaline environments. What products
are formed?
A similar reaction is observed between methyl ethyl ketone and sulphur.
EXPERIMENT 10
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Potassium permanganate dissolves in acetone and in MEK. In the latter,
however, it dissolves in smaller quantities.
EXPERIMENT 11
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MEK can be oxidized by potassium permanganate in alkaline environments (or
is this due to some impurities in the MEK?).
EXPERIMENT 12
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MEK reacts with sulphuric acid. A quick reaction occurs when the liquids
are mixed and a lot of heat is produced. Further reaction takes a few days.
The second reaction stage results in formation of a oil-like product
(a polymerization product?).
EXPERIMENT 13
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Trichloro ethene reacts with acetone, forming a brown substance, but only
when in a strongly alkaline environment. The exact conditions, under which
this brown substance is formed must be further investigated.
EXPERIMENT 14
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Ascorbic acid is oxidized in a strongly alkaline environment, probably by
oxygen from the air. The oxidation product can be oxidized further, but
this only occurs slowly, compared to the speed with which fresh ascorbic
acid can be oxidized.
EXPERIMENT 15
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Bromine reacts with acetylene gas. The bromine disappears and a compound
is formed with a peculiar sweetish smell.
EXPERIMENT 16
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Thymol is oxidized by concentrated nitric acid, resulting in the formation
of a dark green compound, which however by further oxidation is destroyed
again and a water-soluble compound remains.
EXPERIMENT 17
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Benzoate and citrate, used together, give rise to formation of a strange
phenomenon, when heated with concentrated nitric acid. It looks as if one
large crystalline mass is created. It must be investigated, whether the
iron is essential for this or not.
EXPERIMENT 18
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Thymol reacts with chloroform and/or sodium hydroxide when heated. A yellow/
green compound is formed. What is this compound?
EXPERIMENT 19
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Potassium dichromate reacts with formic acid, producing a gas (CO2) and
itself being reduced to trivalent chrome.
EXPERIMENT 20
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Potassium bromate does not react with concentrated formic acid, but when
some bromide or hydrochloric acid is added, then the reaction proceeds
quickly, carbon dioxide being produced.
EXPERIMENT 21
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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 22
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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 23
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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 24
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Dimethylamine borane is very flammable, it easily is ignited and burns
with a beautiful green flame.
EXPERIMENT 25
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Bromine quickly adds to acrylic acid (which has a double bond, in the molecule H2C=CH-C(O)OH)).
Bromine does not react quickly with propanoic acid.
EXPERIMENT 26
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Acrylic acid fairly easily is oxidized in dilute aqueous solution, while propanoic acid is not.
The double bond between two C-atoms makes the molecule more reactive.
EXPERIMENT 27
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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 28
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Silver (I) forms a yellow precipitate with bicarbonate, probably by
precipitating carbonate ions and driving off carbon dioxide.
EXPERIMENT 29
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Copper (II) ions form a complex with DMSO and chloride at the same time. This
is a green complex (somewhat limegreen, however, a little bit more towards pure
green). This complex is soluble in water and probably also is decomposed by
replacement of ligands by water molecules.
EXPERIMENT 30
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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 31
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Alkanes do not react strongly with NO2. Some NO2 dissolves in them.
EXPERIMENT 32
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Aniline, combined with acidified dichromate gives intensely colored compounds.
EXPERIMENT 33
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Aniline gives colored compounds with chromium. The colors are remarkably
intense.
EXPERIMENT 34
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Chromium (III) chloride dissolves in DMSO to quite some extent. A precipitate
is formed slowly. Is this a DMSO complex?
EXPERIMENT 35
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Silver bromide is reduced by metol in alkaline medium.
EXPERIMENT 36
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Hydroquinone is oxidized by ferric chloride to quinone. An intermediate
dark green compound is formed before all hydroquinone is oxidized.
EXPERIMENT 37
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Hydroquinone is oxidized by hydrogen peroxide. This reaction is slow
in a neutral environment.
EXPERIMENT 38
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Ferric chloride enhances the oxidation of hydroquinone by hydrogen
peroxide considerably. Besides this, a coordination complex appears
to be formed when ferric chloride is added to an hydroquinone/peroxide
solution.
EXPERIMENT 39
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Hydroquinone can be oxidized by ferric chloride. If not too much ferric
chloride is added, then a coordination complex of the oxidation product
with hydroquinone is formed and crystals of this compound separate
from the liquid.
EXPERIMENT 40
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Diverse phenol-derivatives, can be oxidized easily by bromine, yielding
intensely colored oxidation products.
EXPERIMENT 41
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Hydroquinone is a very strong reductor in alkaline environments. Oxygen
from the air is readily absorbed by an alkaline solution of hydroquinone.
Sulfite, however, makes an alkaline solution of hydroquinone much more
stable, because of formation of special hydroquinone/sulfite compounds.
EXPERIMENT 42
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Hydroquinone is not oxidized to the dark brown product by hydrogen peroxide
as it is done by oxygen from the air in alkaline environments.
EXPERIMENT 43
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Hydroquinone is readily oxidized by ferricyanide, even in the presence of
sulfite, when in alkaline environments.
EXPERIMENT 44
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Metol is easily oxidized by oxygen from the air, when dissolved in alkaline
media. When sulfite is present, however, oxidation does only occur at a
low rate.
EXPERIMENT 45
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Silver (I) is reduced to metallic silver by metol. This metallic silver
is easily oxidized by peroxosulfate.
Insoluble silver (I) compounds dissolve in thiosulfate solutions (principle
of photography fixer) while metallic silver is not affected.
When a mild oxidizer is added, the metallic silver also dissolves (principle
of photography reducer, Farmer's reducer).
EXPERIMENT 46
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Photography developers, based on phenol-like structures, are easily oxidized
by air in alkaline environments and the oxidation products are such, that
a reverse process does not occur anymore (probably the oxidation products
are large polymerized species).
EXPERIMENT 47
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Phenidone can be oxidized by potassium dichromate and the oxidation
product appears to be a solid, dark brown compound, which does not
dissolve in water.
EXPERIMENT 48
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Benztriazole cannot be oxidized by acidified dichromate. Metol is
quickly oxidized.
EXPERIMENT 49
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Pyrogallol does not dissolve in trichloroethene very well, but some of it
does dissolve.
EXPERIMENT 50
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Pyrogallol is quickly oxidized in alkaline environments by oxygen from the
air. The more alkaline, the faster this reaction proceeds.
The black oxidation products are affected by acid, but the pyrogallol is
not recovered by the acid.
EXPERIMENT 51
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P-aminophenol is quickly oxidized by oxygen from air in alkaline solution.
When acidified, the oxidation product becomes much lighter, but the original
compound is not restored again.
EXPERIMENT 52
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Pyrogallol is oxidized by oxygen from air, even in neutral solution. This
reaction, however, proceeds slowly.
EXPERIMENT 53
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Phenidone is oxidized by air, but is much less susceptible to oxidation
than developers, such as hydroquinone, pyrogallol.
EXPERIMENT 54
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Benzotriazole is not oxidized by air. Apparently it forms a coordination
complex with chromium (III).
EXPERIMENT 55
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It appears that copper (II) ions catalyse the oxidation of pyrogallol by
hydrogen peroxide.
EXPERIMENT 56
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Copper (II) apparently catalyses the oxidation of pyrogallol by oxygen from
the air.
EXPERIMENT 57
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Pyrogallol gives rise to many colored products on oxidation and coordination.
More investigation is needed in order to get more insight in all these
colors and the conditions under which they are formed.
EXPERIMENT 58
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Nitrite reacts with p-aminophenol violently in alkaline environments.
EXPERIMENT 59
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The coordination complexes formed by iron-salts and phenol-like photographic
developers show very typical reactions with hydrogen peroxide. Many times
these reactions result in oxidation products which are not dark colored,
as opposed for oxidation by atmospheric oxygen.
EXPERIMENT 60
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Catechol, resorcinol and hydroquinone all are dihydroxy benzenes. When an
ortho-pair (1,2-pair) or a para-pair (1,4-pair) is present, then the compound
is easily oxidized by air in alkaline environment. When a meta-pair (1,3-pair)
is present, such a reaction does not occur.
EXPERIMENT 61
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When p-aminophenol is oxidized in an acidic environment, then a compound
is formed, with a deep indigo/purple color.
EXPERIMENT 62
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Both metol and p-aminophenol HCl are oxidized by persulfate to colored
compounds. When metol is used, the color, however, is not as brilliant
and not as intense as when p-aminophenol HCl is used. Apparently the
methyl-group on the amino-part of metol has strong influence on the
color of the oxidation product or on the type of oxidation products.
EXPERIMENT 63
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When p-aminophenol is oxidized in acidic environment, then an intensely
colored compound is formed (indigo/purple). This compound is irreversibly
destroyed when the liquid is made alkaline.
EXPERIMENT 64
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When p-aminophenol is oxidized by hypochlorous acid, then an other oxidation
product is formed, compared to oxidation by e.g. persulfate, hydrogen
peroxide etc. When oxidized by hypochlorous acid a yellow solid compound
is formed, otherwise an intense indigo/purple compound is formed, which
remains dissolved.
EXPERIMENT 65
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P-aminophenol HCl reacts with bromine and forms a purple compound.
EXPERIMENT 66
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When hydroquinone is oxidized by hydrogen peroxide in acidic environments,
then a pale yellow compound is formed. This is in strong contrast with
oxidation by oxygen from air in alkaline environment, where a dark brown/
black compound is formed.
EXPERIMENT 67
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Pyrogallol reacts with chlorine, forming an orange/red compound. When excess
chlorine is used, this compound is further oxidized to an almost colorless
compound.
EXPERIMENT 68
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P-aminophenol, when oxidized, forms a deeply colored compound. The color
of this compound is deep blue/purple, but the environment and the used
oxidizer have some influence on the color of the liquid as a whole (other
compounds may make the color less pure).
EXPERIMENT 69
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Hydroquinone is oxidized by chlorate, but this reactions proceeds slowly.
When vanadium pentoxide is added in small quantities, then the reaction
proceeds much faster. The vanadium pentoxide acts as a catalyzer.
EXPERIMENT 70
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Catechol forms a coordination complex with vanadyl.
EXPERIMENT 71
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Vanadium pentoxide catalyzes the oxidation of hydroquinone to quinone by
hydrogen peroxide.
EXPERIMENT 72
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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 73
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Methanol and nitrate/nitric acid do not react readily, not even at fairly
high temperature (appr. 90C).
EXPERIMENT 74
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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 75
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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 76
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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 77
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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 78
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Acetyl chloride is capable of dehydrating copper(II) chloride, and it even is
capable of replacing sulfate ion by chloride, itself being converted to acetyl
sulfate.
EXPERIMENT 79
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Iodoform is only moderately stable. On heating, it decomposes to iodine, carbon
and hydrogen iodide. This process of decomposition looks quite special.
EXPERIMENT 80
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Iodate and formiate react very nearly explosively at high temperature.
EXPERIMENT 81
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Niobium pentachloride reacts with acetic acid, giving a colorless fuming gas
(most likely HCl) and a fuming liquid (most likely acetyl chloride).
EXPERIMENT 82
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Magnesium perchlorate dissolves in acetone very well. The mix of acetone and
magnesium perchlorate does burn like normal acetone. No spectacular reaction
occurs when the solution is ignited.
EXPERIMENT 83
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When anhydrous ZnCl2 is added to acetic anhydride, then a (small) part of the
solid dissolves. On addition of a small amount of water, an extremely violent
reaction occurs, accompanied with crackling noise and violent bubbling of the
liquid.
EXPERIMENT 84
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Acetyl chloride can be used to make several esters, but with some alcohols, the
reaction is EXCEEDINGLY violent and some dilution is needed to make the
experiment safe.
EXPERIMENT 85
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Copper(II) ion and iron(III) ion form complexes with acetyl acetate (acac) in
aqueous solution. Cobalt does not form a complex, at least not visibly.
EXPERIMENT 86
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Formation of hypochlorite esters is very easy. With many alcohols, it is
possible to make hypochlorite esters. These esters are very unstable and easily
explode or burn very fiercely when ignited.
All experiments, described here are quite dangerous, use good protection of the
eyes and keep test tubes wrapped in a thichk layer of towels. Do not scale up!
EXPERIMENT 87
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Ascorbic acid and sodium chlorite react violently and the dry mix can even
inflame.
EXPERIMENT 88
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Ethylacetate is in equilibrium with ethanol and acetic acid, even in dilute
aqueous solution with some free acid in it. Usually, making esters requires
rather forcing conditions, like mixing an alcohol and an organic acid and
adding this mix to concentrated sulphuric acid and then heating the mix. This
experiment nicely demonstrates that there is an equilibrium, also in water.
EXPERIMENT 89
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Bromine does not react with formic acid, or it reacts very slowly. When
aluminium is added, then this quickly shows a violent reaction and all of the
aluminium dissolves, leaving a clear orange/red and someawhat viscous liquid.
On dilution with water, a clear yellow liquid is obtained.
EXPERIMENT 90
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Tert-butanol is very easily converted to tert-butyl chloride. Simply adding
tert-butanol to concentrated hydrochloric acid allows the formation of this
compound.
EXPERIMENT 91
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Copper(II) ions form a pale green complex with a yellowish hue. When the
solution is heated to boiling, then the copper(II) is reduced to metallic
copper.
EXPERIMENT 92
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Formic acid acts as a reductor, while acetic acid does not do so. Formic acid,
however, is not that easily reduced. Reduction requires elevated temperature
and strong oxidizers.
EXPERIMENT 93
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Anhydrous copper (II) chloride, when added to acetone, dissolves with a
yellow/brown/green color. When a saturated solution is allowed to stand for
several hours at 10 C or so, then red/brown crystals are formed. When the
crystals are heated, then they become dark brown and a flammable vapor is
produced (most likely acetone).
Probably, from a saturated solution of copper(II)chloride in acetone, an adduct
is formed of the form CuCl2.nCH3COCH3.
EXPERIMENT 94
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Iodoform reacts exothermically with chlorine, one of the reaction products
being iodine. The other products must be substitution products, with iodine
completely or partly replaced by chlorine.
When excess chlorine is used, then iodine monochloride and iodine trichloride
are formed as well. These products react with iodoform as well, resulting in
formation of iodine.
EXPERIMENT 95
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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 96
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Sulphuric acid and acetic anhydride react with each other. This reaction is
very violent. The final product is a very viscous colorless liquid. The main
constituent of this liquid is acetyl sulfate or acetyl bisulfate.
EXPERIMENT 97
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Ethylene glycol does not easily form a hypochlorite ester like ethanol or other
mono-alcohol.
EXPERIMENT 98
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When anhydrous sodium formiate is heated, then it first melts and on further
heating it decomposes, giving a colorless gas. This colorless gas is highly
flammable and forms explosive mixes with air.
EXPERIMENT 99
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Triethylamine frequently is used in reactions, where thionyl chloride is used,
in order to capture any HCl formed in the reaction. However, when the only
reactive compounds are thionyl chloride and triethylamine, then these two
compounds react by themselves, giving rise to formation of black material,
which sticks to the glass and is difficult to remove.
EXPERIMENT 100
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Niobium pentachloride does react with methanol, but not nearly as violently as
phosphorus pentachloride.
EXPERIMENT 101
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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 102
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Hexavalent chromium oxidizes ascorbic acid. This reaction is fast and even
proceeds without adding additional acid. The acidity of the ascorbic acid
suffices to make the reaction proceed quickly.
The resulting chromium(III) forms an intensely colored dull-green complex
(green/grey, almost black at moderate concentration).
EXPERIMENT 103
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Ethylene diamine (NH2CH2CH2NH2) and iodic acid form a moderately soluble salt.
In the dry state, this salt is fairly stable. Only when it is heated strongly,
it decomposes with a soft puff, giving a yellow/brown smoke and a bad smell.
EXPERIMENT 104
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Vanadium pentoxide does not dissolve in thionyl chloride, but when a small
amount of water is added, then it reacts.
Vanadium pentoxide dissolves in acetyl chloride, giving a dark red/brown
solution.
EXPERIMENT 105
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A solution of cobaltous acetate is hydrolysed when the solution is heated. When
the liquid cools down again, then the effect is reversed again. The visual
result is formation of a precipitate on heating and the slow redissolving of
the precipitate on cooling down.
EXPERIMENT 106
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Anhydrous magnesium perchlorate dissolves in acetone easily, giving a colorless
solution. Some heat is produced when the magnesium perchlorate dissolves, but
it is not much. The resulting solution does not conduct electricity. When just
a few drops of water are added to the solution, then it becomes conducting.
EXPERIMENT 107
---------------
Chromium trioxide dissolves well in acetone, but it does not react. When
sulphuric acid is added, then it does react and it can do so nearly
explosively!
EXPERIMENT 108
---------------
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 109
---------------
The combination of acetyl and sulfate, either directly, or derived from other
compounds reacts extremely energetically with water. It is remarkable that it
is this specific combination of three entities which gives extremely violent
reactions. This effect is demonstrated with different chemicals in different
combinations.
EXPERIMENT 110
---------------
Methylene chloride is capable of extracting nitric acid from its aqueous
solution.
EXPERIMENT 111
---------------
Bromine dissolves fairly well in pure formic acid, but no redox reaction
occurs, not even on heating. When water is added to the mix, then a redox
reaction sets in, in which bubbles of gas are produced (probably CO2).
EXPERIMENT 112
---------------
Sulphur dissolves in carbon disulfide exceedingly easily.
EXPERIMENT 113
---------------
Carbon disulfide slowly reacts with an aqueous solution of sodium sulfide. The
resulting solution finally becomes deep orange.
EXPERIMENT 114
---------------
Dichromate and chromate both quickly are oxidized by pure formic acid,
resulting in a fairly violent and exothermic reaction, in which a dark
purple/blue/grey compound is formed.
EXPERIMENT 115
---------------
Hypochlorite ion forms esters very easily with alcohols. The esters simply are formed from aqueous
solutions. The methyl ester is a colorless gas, which gives extremely powerful explosions when
ignited. The ethyl ester is a very volatile yellow/green oil, which burns with a WHOOSH sound and
which is quite unstable (it easily decomposes). The t-butyl ester is quite stable and can be kept
around for a somewhat longer time. This burns quickly with a sooty flame.
EXPERIMENT 116
---------------
Formic acid does not form an acid chloride with thionylchloride, but it
decomposes. Normally, the following reaction occurs:
RCOOH + SOCl2 --> RCOCl + SO2 + HCl
When R = H (formic acid), then decomposition occurs and carbon monoxide is
formed.
EXPERIMENT 117
---------------
Cyanate ion forms complexes with many metal ions. These complexes have a strong
color and are not stable in acidic solution.
EXPERIMENT 118
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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 'C'