Experiments for 'cupric chloride dihydrate'
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 'cupric chloride dihydrate':
EXPERIMENT 1
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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 2
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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 3
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Cupric chloride dihydrate is dehydrated by concentrated sulphuric acid.
EXPERIMENT 4
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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 5
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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 6
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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 7
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Copper sulfate dissolves in methanol quite well. A blue solution is obtained.
Copper chloride dihydrate also dissolves in methanol quite well. A green
solution is obtained.
With thiocyanate a deep brown complex is formed, which dissolves in
methanol, but at higher concentration this precipitates.
With cyanide, a dirty green compound is formed, which, however, quickly
turns white. This probably is copper (I) cyanide.
EXPERIMENT 8
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Copper (II) chloride is reduced by hydroxyl amine, when dissolved in
ethanol. First, the solution becomes much darker and apparently, a mixed
oxidation state complex of copper (I) and copper (II) is formed. Finally,
all copper (II) is reduced to copper (I).
This experiment is another example, which shows that copper (I) and copper
(II), when in solution at the same time, form a highly colored complex.
EXPERIMENT 9
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Copper (II) chloride dihydrate dissolves in ethyl acetate, albeit only
in small amounts. With thiocyanate, a dark coordination complex is formed,
also in ethyl acetate.
EXPERIMENT 10
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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 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) chloride hexahydrate cannot be dehydrated by simple heating.
Copper (II) chloride dihydrate can perfectly be made anhydrous.
EXPERIMENT 13
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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 14
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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 15
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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 16
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Reduction of tetrachlorocuprate with ascorbic acid
EXPERIMENT 17
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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 18
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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.
End of results for 'cupric chloride dihydrate'