Experiments for 'sodium thiosulfate'
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 thiosulfate':
EXPERIMENT 1
---------------
Bismuth forms a yellow complex with thiosulfate. In the presence of
thiosulfate, it still forms a deep orange complex with iodide, just as without
thiosulfate.
EXPERIMENT 2
---------------
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 3
---------------
A large set of compounds is checked on interaction with concentrated
nitric acid. Many reductors react violently with nitric acid.
EXPERIMENT 4
---------------
Rhenium can be oxidized to colorless perrhenate [ReO4]-, with nitric acid.
With zinc it can be reduced to a yellow/green species in the presence of
hydrochloric acid at sufficient concentration. This species apparently is
not reduced any further with borohydride in alkaline environments. In
acidic environments, a dark brown/black compound can be formed easily,
due to reduction of thiosulfate to sulfide by the borohydride. The sulfide
forms a dark compound with rhenium.
With sulfite, perrhenate nor the yellow/green compound can be reduced to
a lower oxidation state.
EXPERIMENT 5
---------------
Chromium (III) builds a green coordination complex with metabisulfite,
not with thiosulfate.
When hydrogen peroxide is added, then the complex with metabisulfite is
destroyed.
EXPERIMENT 6
---------------
Silver is coordinated by thiosulfate. The silver-thiosulfate complex does
not show any of the reactions of free aqueous silver (I).
EXPERIMENT 7
---------------
Silver chloride and silver oxide dissolve in a solution of sodium
thiosulfate. The reaction is not very fast.
EXPERIMENT 8
---------------
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 9
---------------
Thiosulfate gives a purple coordination complex with iron (III). This
complex, however, is not stable. With iron (II) no complex is formed.
Iron (III) is reduced by thiosulfate after the initial formation of
the purple coordination complex. This is shown by adding ferrocyanide,
which does not result in formation of an intense dark blue precipitate.
EXPERIMENT 10
---------------
Thiosulfate is capable of reducing ferricyanide, but it is not capable
of reducing ferroferricyanide (Prussian blue).
EXPERIMENT 11
---------------
Ferricyanide gives a dark brown coordination complex with ferric ions. This
complex is soluble in water. It is easily transformed to the much more
stable, dark blue and insoluble ferroferricyanide.
EXPERIMENT 12
---------------
The tetrathionate ion is much more stable than the thiosulfate ion in acidic
solution.
EXPERIMENT 13
---------------
Dichromate ion oxidizes thiosulfate easily in acidic media, but in neutral
media it only is oxidizing incompletely, and a solid compound is formed.
EXPERIMENT 14
---------------
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 15
---------------
A clock reaction that precipitates antimony sulfide.
End of results for 'sodium thiosulfate'