Experiments for 'silver nitrate'
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 'silver nitrate':
EXPERIMENT 1
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This is a very nice experiment, involving beautifully coloured compounds,
but it is a hazardous experiment as well, due to the use of mercury (II)
compounds.
Mercury (II) builds a complex with excess iodide, [HgI4]2-, which gives a
beautiful bright yellow precipitate with Ag+ and a beautiful bright brick-
red precipitate with Cu+.
EXPERIMENT 2
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This sequence of experiments shows that sulfite is capable of reducing
silver (I), copper (II) and iron (III), but that these reactions all
show their own peculiarities. Sulphur in the +4 oxidation state is a
mild reductant.
EXPERIMENT 3
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Silver bromide is reduced by metol in alkaline medium.
EXPERIMENT 4
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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 5
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Silver (I) gives a bordeaux-red precipitate with dichromate, which
slightly dissolves in water.
EXPERIMENT 6
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Chromium (III) is oxidized to dichromate (chrome (VI)) by persulfate. This
reaction is catalyzed by silver (I).
EXPERIMENT 7
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Persulfate is capable of oxidizing Mn2+ in acid environments, but silver (I)
is needed as a catalyst. Oxidation, however, is not easy and just a small
part is oxidized to permanganate, a large part is oxidized no further than
MnO2.
EXPERIMENT 8
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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 9
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The peroxosulfate ion ([S2O8]2-) is capable of oxidizing silver (I) to
silver (II) or silver (III). A higher oxide of silver is precipitated.
This oxide is easily decomposed under the liberation of oxygen.
EXPERIMENT 10
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Silver (I) gives a pale yellow precipitate with carbonates.
EXPERIMENT 11
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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 12
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Silver (I) reacts with persulfate. Probably a higher oxidation state of
silver is produced (oxidation state II or III).
EXPERIMENT 13
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Silver nitrite is only sparingly soluble in water. When dilute acid is
added, the compound is destroyed again.
EXPERIMENT 14
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Silver (I) gives a precipitate with bromate. The compound silver bromate
does not dissolve well in water. When acidified, the compound still does
not dissolve, hence the acid HBrO3 is fairly strongly ionized, otherwise
the silver bromate would dissolve appreciably. The precipitate of silver
bromate, however, still shows strong oxidizing properties, meaning that
it is sufficiently soluble for releasing bromate ions in solution, needed
for the redox reaction to occur.
EXPERIMENT 15
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Silver (I) ions form a precipitate, both with ferrocyanide and with
ferricyanide. The precipitate with ferricyanide is decomposed by alkalies,
the precipitate with ferrocyanide is more stable. Both compounds are
attacked by thiosulfate, which complexes the silver and causes the
solid to dissolve again.
EXPERIMENT 16
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Silver ions react with organic matter and are easily reduced to silver.
This causes brown or black staining on many materials.
EXPERIMENT 17
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Silver (I) forms a yellow precipitate with bicarbonate, probably by
precipitating carbonate ions and driving off carbon dioxide.
EXPERIMENT 18
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Silver salts give a yellow precipitate with silicates. This precipitate
becomes white on addition of sulphuric acid. When a large quantity of
sodium hydroxide is added, then a dark, almost black, solid is created.
EXPERIMENT 19
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Silver (I) gives a precipitate with bicarbonate, which becomes yellow and
more compact on standing. With H2O2 a dark compound is formed, which
dissolves in nitric acid under formation of a gas. Is this dark compound
a higher oxide of silver (e.g. Ag2O2?).
EXPERIMENT 20
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Silver (I) gives a white precipitate with thiocyanate, which does not dissolve
in excess ammonia. Hydroxyl amine does not affect this precipitate.
EXPERIMENT 21
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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 22
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Silver (I) forms a precipitate with bromates, while it does not do so with
chlorates.
EXPERIMENT 23
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Silver (I) ions, when treated with hydroxide give brown silver (I) oxide.
When hydrogen peroxide is added, then that is decomposed and the precipitate
of oxide does not change noticeably. When, however, hydrogen peroxide is
first mixed with a solution of a silver (I) salt and then the hydroxide is
added, then a black precipitate is formed. Probably this is finely divided
metallic silver.
EXPERIMENT 24
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Silver nitrate reacts very violently with magnesium, but only if the reaction
is started by adding some water. Once the reaction runs, it continues
through the dry mixture.
EXPERIMENT 25
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Silver (I) ions give a dark brown precipitate with sulfide.
EXPERIMENT 26
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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 27
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Silver(I) ion gives a chocolate brown precipitate with arsenate.
EXPERIMENT 28
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Silver chlorite is stable, but only light heating is required for its
decomposition.
EXPERIMENT 29
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Peroxodisulfate ion gives a deep brown complex with silver ions in nitric acid.
Oxone (peroxomonosulfate) does not give such a complex, actually, it quickly
destroys such a complex.
End of results for 'silver nitrate'