Experiments for 'Cl'
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 'Cl':
EXPERIMENT 1
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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 2
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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 3
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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 4
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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 5
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Copper (II) chloride reacts violently with metallic aluminium. When copper
sulfate or nitrate is used, then this reaction does not occur. When sodium
chloride is used, this reaction also does not occur. Both cupric ions and
chloride ions are needed for quick reaction with aluminium, but if they are
present, then a very violent reaction occurs.
EXPERIMENT 6
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Cupric chloride forms a coordination complex when a large excess of chloride
is present and this chloro cuprate complex easily oxidizes metallic copper.
This oxidation causes formation of copper (I), which forms a very dark
brown complex in the presence of copper (II) and hydrochloric acid (what
is this dark brown compound?).
EXPERIMENT 7
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Cupric chloride dihydrate dissolves in acetone. The solution becomes yellow
at low concentrations, green/brown at higher concentrations. When sulphuric
acid is added, then a precipitate of anhydrous cupric chloride is formed.
EXPERIMENT 8
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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 9
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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 10
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Copper (II) forms a yellow/brown coordination complex with cyanide in
acidic media in the presence of chloride.
EXPERIMENT 11
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Copper (I) oxide, when added to sulphuric acid, disproportionates. Metallic
copper is formed and a blue solution of copper (II) sulfate. The copper (I)
oxide looses its oxide ion to the acid and that would leave aqueous copper (I)
ions. These are not stable and disproportionate at once.
Copper (I) oxide, added to hydrochloric acid dissolves and forms a solution,
containing a copper (I) complex, [CuCl2]-. This complex is very easily oxidized
by oxygen from the air and then a dark brown mixed valency complex of copper
(I) and copper (II) is formed.
EXPERIMENT 12
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Copper(I) iodide dissolves in a concentrated solution of potassium iodide.
In such a solution the complex ion CuI2(-) is formed. On dilution, this ion
decomposes and a precipitate of CuI is formed again.
Copper(I) iodide does not dissolve in hydrochloric acid, or just a small
amount dissolves.
EXPERIMENT 13
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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 14
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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 15
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Bismuth (III) forms a deep-orange iodo-complex and a yellow iodo-chloro
complex.
EXPERIMENT 16
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Cobalt (II) ions build pink aqua complexes are intense blue chloro
complexes. Heat favors the chloro complex.
EXPERIMENT 17
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Thionyl chloride quickly hydrolyses in the presence of water.
EXPERIMENT 18
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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 19
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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 20
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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 21
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Potassium chlorate is able to liberate bromine from a bromide. Reaction
with sodium sulfide of the bromine shows formation of fumes/smoke.
EXPERIMENT 22
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Potassium chlorate only reacts slowly with iodide at room temperature.
When heated, the reaction proceeds much faster. Probably KClO3 oxidizes
iodine further, until iodate is formed.
EXPERIMENT 23
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It is possible to make an aqueous solution of bromine, which is so saturated,
that the bromine separates from the liquid. In order to do so, a chemical
reaction, producing large quantities of bromine must be performed.
EXPERIMENT 24
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Sodium chloride reacts with sulfuric acid to give hydrogen chloride gas.
Sodium bromide shows a similar reaction, producing hydrogen bromide, but
in a side reaction some bromine is formed.
EXPERIMENT 25
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When potassium chlorate and concentrated sulphuric acid are mixed, a very
dangerous and strong oxidizer is created, which reacts explosively with
organic matter.
EXPERIMENT 26
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Bromide is oxidized by sulphuric acid, even when diluted with water.
Bromine precipitates from water, when it is created in high concentrations.
EXPERIMENT 27
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Chlorine reacts with acetylene gas (C2H2), without the need to ignite it.
EXPERIMENT 28
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Sodium chlorate reacts with chloride in acidic environment, forming chlorine
(which can be detected by means of its odour) and a fairly intensely colored
yellow gas (chlorine dioxide). The color of this gas is much more intense
than the color of chlorine.
The yellow compound is destroyed by sulfite and nitrite.
EXPERIMENT 29
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Potassium bromate reacts vigorously with concentrated hydrochloric acid.
A green gas is evolved, but this gas has a color, which is fairly intense.
The green gas consists of chlorine, but it also contains bromine, probably
combined with chlorine in a compound as BrCl, which is slightly darker
green than Cl2.
EXPERIMENT 30
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Although the redox potential from bromate to bromine is higher than the
potential from perchlorate to chlorate, when chlorate and bromate are
mixed, then no reaction occurs. When some hydrochloric acid is added,
then a reaction occurs with the chloride ions.
EXPERIMENT 31
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Chlorate and bromate react with hydrochloric acid, but bromate reacts more
vigorously. There also is a marked difference between potassium and sodium
chlorate. The sodium salt reacts more vigorous with hydrochloric acid, but
not as vigorous as potassium bromate.
Reactions of bromate are faster than reactions of chlorate, but for sodium
and potassium chlorate, the difference can be explained by the speed at
which the salt dissolves.
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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Bromates are more reactive than chlorates in dilute aqueous solutions.
EXPERIMENT 34
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Bromate reacts with chlorides, releasing chlorine. Probably some bromine
is produced as well or a bromine/chlorine compound is produced.
EXPERIMENT 35
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Bromate oxidizes iodine to iodate, itself being converted to bromine.
Chlorate does not oxidize bromine to bromate, itself being converted to
chlorine (at least not quickly).
EXPERIMENT 36
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Both iodate and periodate form the tetrachloroiodide ion in a strong
solution of hydrochloric acid. A redox reaction occurs, where the iodine
is reduced to its +3 oxidation state and chlorine is released.
EXPERIMENT 37
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The tetrachloroiodide ion is not stable in water at high dilution. It
tends to disproportionate to iodine, choride and iodate.
With sulfite, it is reduced to iodine. With excess sulfite, it is reduced
to iodide.
EXPERIMENT 38
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Potassium tetrachloroiodide decomposes on heating. The residue, which
remains behind is potassium chloride.
EXPERIMENT 39
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Potassium chlorate and sulphur form a potentially explosive mixture, which
is quite sensitive to shock.
EXPERIMENT 40
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TCCA does not react with sulphuric acid, at least not visibly. Even when
heated, no reaction seems to occur. On addition of some solid NaCl vigorous
evolution of chlorine gas is observed.
EXPERIMENT 41
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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 42
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Chlorite ion forms complexes with cobalt(II) and copper(II). It forms a
precipitate with lead(II). The precipitate with lead(II) forms a highly
energetic compound.
EXPERIMENT 43
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Praseodymium chloride dissolves in water very well and very easily, but it
hydrolyses. A solution of this is turbid. When the solution is slightly
acidified, then a very pale green and clear solution is obtained.
Praseodymium chloride only dissolves slowly in concentrated hydrochloric acid.
The solution also has another color than a plain slightly acidified solution.
The solution in concentrated hydrochloric acid is yellow and its color is much
more intense than the pale green color of aqueous praseodymium ions.
EXPERIMENT 44
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Praseodymium (III) ions form complexes with chloride, bromide and iodide. With
fluoride a precipitate is formed.
EXPERIMENT 45
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Bleach is capable of oxidizing chromium (III) to its hexavalent state, but
this is not accomplished easily and completely.
EXPERIMENT 46
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When solid potassium permanganate is added to concentrated hydrochloric
acid, then a gas is evolved, being chlorine. The liquid becomes almost
black. When the reaction is driven to an end by heating (almost boiling)
the liquid, then the final liquid does not become colorless, but green.
The green color is not a bright green, but it is brownish/sepia-like.
What is the constitution of this green/sepia compound?
A similar observation is done when hydrochloric acid is heated with
manganese dioxide. In the cold there is no visible reaction, but when
heated, chlorine is produced and a green compound is formed.
EXPERIMENT 47
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Silver (I) forms a precipitate with bromates, while it does not do so with
chlorates.
EXPERIMENT 48
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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 49
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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 50
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Ferric ions form a colorless complex with phosphate ions in acidic
environments. In the presence of chloride ions, a yellow coordination
complex is formed, which can exist, even in the presence of phosphate.
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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Niobium pentachloride does react with methanol, but not nearly as violently as
phosphorus pentachloride.
EXPERIMENT 53
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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 54
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Ascorbic acid and sodium chlorite react violently and the dry mix can even
inflame.
EXPERIMENT 55
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Potassium perchlorate is only marginally soluble in cold water, while being
much more soluble in hot water. From perchloric acid solutions, one can easily
precipitate KClO4, almost quantitatively. It is funny to see how a potassium
salt precipitates so quickly and densely.
EXPERIMENT 56
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When compounds of manganese(IV) or manganese(VII) are added to hydrochloric
acid, then chlorine gas is produced and the solution becomes very dark
brown/green. Only after a long time of heating, all dark brown/green material
is gone and what remains is a pale solution, containing manganese(II) ions.
In this series of experiments it was attempted to go the other way around. Is
it possible to go from almost colorless manganese(II) to the dark colored
compounds of manganese(III) or manganese(IV). This was done by adding chlorine
to solutions of manganese(II) salts in concentrated hydrochloric acid.
While doing so, an interesting observation was made. The dark colored compound
indeed can be made from manganese(II) in concentrated hydrochloric acid, but
only from hypochlorite and not from chlorine.
When calciumhypochlorite is added to hydrochloric acid, then chlorine is formed
vigorously, and the solution becomes green and clear.
It seems, however, that even in concentrated hydrochloric acid some of the
hypochlorite is not decomposed at once, but remains in solution as yellow/green
hypochlorous acid.
A freshly prepared solution, made from a pinch of calcium hypochlorite and
concentrated hydrochloric acid, reacts differently than a saturated solution of
chlorine in concentrated hydrochloric acid. This is shown with manganese(II)
ions in hydrochloric acid.
EXPERIMENT 57
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Sodium hypophosphite is remarkably flammable. A mix with potassium chlorate is
dangerously explosive and can easily be ignited.
EXPERIMENT 58
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Copper(II) can be reduced to the very peculiar compound CuH by hypophosphorous
acid, but only under very specific conditions. The compound CuH is quite
unstable and easily looses hydrogen.
In the presence of chloride ions, no CuH is formed, but CuCl is formed instead.
EXPERIMENT 59
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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 60
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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 61
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Cesium forms a solid red/brown chloro complex of copper(II). This complex is
very remarkable, due to its rust-like color, which is very uncommon for
copper(II) salts.
EXPERIMENT 62
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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 63
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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 64
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Magnesium and potassium tetrachloro iodide do not react when dry, but when a
drop of water is added, then a violent reaction starts, with production of
purple clouds of iodine.
EXPERIMENT 65
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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 66
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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 67
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Silver chlorite is stable, but only light heating is required for its
decomposition.
EXPERIMENT 68
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Hydrofluoric acid (48% by weight) dissolves potassium chlorate and potassium
bromate much more easily than water. The bromate also slowly decomposes in a
peculiar way, which is not observed in other acidic solutions (like sulphuric
or nitric acids).
EXPERIMENT 69
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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 70
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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 71
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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 72
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Perchloric acid is very reluctant to reacting with many chemicals. This is
different from what many sites are telling. Perchloric acid only is extremely
reactive when it is anhydrous, the hydrous acid (60 ... 70%) is not that
reactive.
EXPERIMENT 73
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Antimony trioxide dissolves in hydrochloric acid, giving a colorless solution.
When hydrogen sulfide is passed through such a solution, then a small amount of
a yellow precipitate is formed and the liquid becomes very pale yellow.
On dilution, much more precipitate is formed and the surprisingly, the color
shifts from pale yellow to orange. The orange solid must be hydrous Sb2S3.
EXPERIMENT 74
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Methylene chloride is capable of extracting nitric acid from its aqueous
solution.
EXPERIMENT 75
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When concentrated hydrochloric acid is added to solid NaClO2, then a lot of
intense yellow ClO2 is produced, but normally the gas does not explode.
When concentrated hydrochloric acid is added to a mix of solid NaClO2 and solid
NaBrO3, then a yellow gas is produced and within a few seconds at most, the gas
explodes, the explosion starting at/near the liquid surface.
EXPERIMENT 76
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When sodium chlorite solution is acidified with acetic acid, then a brown
solution is obtained, which on addition of more acetic acid becomes lighter and
which on addition of hydrochloric acid becomes bright yellow.
EXPERIMENT 77
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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 78
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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 79
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Anhydrous copper (II) chloride, when added to acetone, dissolves with a
yellow/brown color. If more copper (II) chloride is added, than can be
dissolved in acetone, then the remaining solid becomes red/brown, like iron
rust.
When the red/brown solid is added to water, then at once it becomes green and
then it dissolves, just as normal copper (II) chloride. The dilute solution
becomes light blue.
EXPERIMENT 80
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Ethylene glycol does not easily form a hypochlorite ester like ethanol or other
mono-alcohol.
EXPERIMENT 81
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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 82
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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 83
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Chromium trioxide (CrO3) dissolves in concentrated hydrochloric acid, giving a
dark brown liquid. When this liquid is heated, then some orange/brown chromyl
chloride is formed, which can easily be observed as a vapor above the liquid.
On further heating the hydrochloric acid is oxidized and the hexavalent
chromium is converted to green trivalent chromium.
EXPERIMENT 84
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When phosphorus pentachloride is added to chromium trioxide, then a fairly
vigorous reaction occurs and exchange of oxygen and chlorine atoms occurs. The
two solids react with each other, forming liquid CrO2Cl2 and liquid POCl3.
EXPERIMENT 85
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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 86
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Chlorite ion and chlorine dioxide are sluggish oxidizers when in aqueous
solution, even in the presence of quite some acid. Bromide ion only is oxiduzed
very slowly and only partially.
EXPERIMENT 87
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Hydrogen chloride does not dissolve very well in concentrated perchloric acid.
EXPERIMENT 88
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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 89
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Lead(II) ion and chlorite ion produce a pale yellow precipitate. This solid,
when dried, explodes when heated in a test tube, it deflagrates when heated in
an open flame.
EXPERIMENT 90
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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 91
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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 92
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Ferric chloride anhydrous easily melts and when it melts, it also nearly boils
and a dark yellow/brown vapor is formed, which condenses to beautiful crystals
in cooler areas.
A small part of the ferric chloride reacts either with oxygen from the air, or
with water vapor in the air. Insoluble oxide-species are formed.
EXPERIMENT 93
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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 94
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A mix of potassium perchlorate and sulphur cannot easily be ignited. When just
a tiny pinch of red phosphorus is mixed in, then the mix is ignited very easily
and it burns very fast with a bright flash.
EXPERIMENT 95
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Antimony trioxide does not dissolve in concentrated nitric acid, not even when
the liquid is heated to boiling. When some hydrochloric acid is added as well,
then it quickly dissolves, producing a colorless gas as well. It is oxidized to
the +5 oxidation state.
When this solution is diluted, then a white precipitate is formed. This white
precipitate must be hydrous Sb2O5. When a dilute solution of sodium sulfide is
added to this still strongly acidic solution, then H2S bubbles out of solution,
but also a lot of precipitate is formed, which has a beautiful bright
orange/red color.
EXPERIMENT 96
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This is a spectacular experiment. A mix of sodium chlorite and red phosphorus
can be ignited by bringing it in contact with hydrochloric acid.
EXPERIMENT 97
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Chlorosulfonic acid is an extremely reactive compound. It reacts violently with
many salts of oxoacids.
EXPERIMENT 98
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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.
End of results for 'Cl'