Experiments for 'sodium sulfide'
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 sulfide':
EXPERIMENT 1
---------------
Cobalt sulfide does not dissolve in dilute acids and it does not dissolve
in concentrated hydrochloric acid (at least not easily). With the help of
hydrogen peroxide it is possible, however, to dissolve the compound.
EXPERIMENT 2
---------------
The hexanitrite cobaltate (III) ion is strongly affected by sulfide. A black
compound is formed. On acidification of this, remarkably, no hydrogen
sulfide is formed. Probably the black compound is a compound containing
sulfide and nitrite in a single compound, which on acidification results
in oxidation of the sulfide.
EXPERIMENT 3
---------------
Ferrous sulfide is a black precipitate, which easily dissolves in acid.
EXPERIMENT 4
---------------
Iron (III) gives a precipitate with S2-, but a redox reaction, resulting
in the formation of sulphur also appears to occur.
EXPERIMENT 5
---------------
This experiment shows two things:
1) Permanganate can be reduced by metabisulfite, but the reduction does
not proceed instantaneously when no additional acid is used.
2) Manganese sulfide is a dirty pink substance (color of flesh).
EXPERIMENT 6
---------------
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 7
---------------
Sulphur dissolves in a solution of a sulfide. Polysulfides are formed.
EXPERIMENT 8
---------------
Sulfide gives precipitates with some metals, which do not dissolve in
strong acids. These sulfides, however, can easily be dissolved, when an
oxidizing agent is used.
Sulfide is easily oxidized by moderately strong oxidizers.
EXPERIMENT 9
---------------
Sodium sulfide is oxidized by acidic hydrogen peroxide with extreme violence.
EXPERIMENT 10
---------------
Silver (I) ions give a dark brown precipitate with sulfide.
EXPERIMENT 11
---------------
A large set of compounds is checked on interaction with concentrated
nitric acid. Many reductors react violently with nitric acid.
EXPERIMENT 12
---------------
Selenium dissolves in a sulfide solution, forming a deep red/brown solution.
Hydrogen peroxide is capable of oxidizing this solution.
EXPERIMENT 13
---------------
Sulfide reacts with metavanadates, resulting in the formation of a dark
brown/greenish compound.
EXPERIMENT 14
---------------
When dichromate is added to sulfide, then a transient highly coloured
compound is formed, immediately followed by reduction to green chromium (III)
in alkaline environment.
EXPERIMENT 15
---------------
Potassium chlorate is able to liberate bromine from a bromide. Reaction
with sodium sulfide of the bromine shows formation of fumes/smoke.
EXPERIMENT 16
---------------
Sulfide is capable of forming a brightly coloured compound with antimony
(III) in a strongly acidic environment. The sulfide is not destroyed by
strong acid and is not converted to hydrogen sulfide gas.
EXPERIMENT 17
---------------
Sulfide is capable of dissolving sulphur, forming intensely colored poly-
sulfide species. These poly-sulphide species react with antimony (III) in
strongly acidic environments, resulting in two different types of
precipitates.
EXPERIMENT 18
---------------
Antimony sesquioxide does not dissolve in a concentrated solution of NaOH
nor does it react with sulfide or one of the polysulfides in strongly
alkaline environments.
EXPERIMENT 19
---------------
Elementary antimony dissolves in aqua regia at a fairly high rate. While
it dissolves a lot of gas is produced. When the liquid is diluted with
water, then a white precipitate is formed, due to hydrolysis of the
reaction product. It looks as if the antimony is oxidized to the +3 oxidation
state.
EXPERIMENT 20
---------------
Palladium (II) is not easily reduced by mild reducing agents. Only very
strong reductors are capable of reducing this to metallic palladium.
Strong oxidizers probably are capable of oxidizing palladium (II) to a
higher oxidation state, but if this is true, then the higher oxidation
state has almost the same color.
Sulfite, instead of reducing palladium to the metallic state, appears to
form a brightly colored coordination complex in acidic environments.
EXPERIMENT 21
---------------
Platinum(II) is not reduced by sulfide in acidic environments. When it is
treated with stannous ions at the same time, then a dark brown compound
is formed, but probably this is not metallic platinum but stannous sulfide.
What speaks against this is that stannous chloride does not precipitate
with H2S in acidic environments (see sequence 2), while with the Pt-compound
a dark brown compound is formed. More research will be needed to resolve
this.
EXPERIMENT 22
---------------
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 23
---------------
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 24
---------------
Arsenate does not form thioarsenates when sulfide ion is added. On
acidification, the sulfide is oxidized though by the arsenate.
EXPERIMENT 25
---------------
When sodium sulfide and sodium nitrite are mixed as solids, or when mixed in
aqueous solution, no reaction occurs. Sulfide ion and nitrite ion can coexist
in solution.
When a very small amount of acid is added, a bright yellow/ochre solid compound
is formed, which slowly turns lighter. When more acid is added, then the solid
becomes almost white.
The very light yellow, almost white compound most likely is very finely divided
elemental sulphur. The much brighter yellow/ochre definitely is not sulphur,
its color is too strong and also differs quite a lot from the kind of yellow of
sulphur.
EXPERIMENT 26
---------------
Carbon disulfide slowly reacts with an aqueous solution of sodium sulfide. The
resulting solution finally becomes deep orange.
End of results for 'sodium sulfide'