| Identification | More | [Name]
SODIUM SULPHIDE HYDRATE | [CAS]
1313-84-4 | [Synonyms]
SODIUM SULFIDE
SODIUM SULFIDE HYDRATE
SODIUM SULFIDE, HYDRATE, FUSED
SODIUM SULFIDE, HYDROUS
SODIUM SULPHIDE HYDRATE
sodiumsulfide,hydrated
sodiumsulphide,nonahydrate
sodiumsulphidenonahydrate
sulfuredesodium
sulfuredesodium,nonahydrate
Sldium monosulfide
Sodium sulfide crystal
SODIUM SULFIDE NONAHYDRATE, REAGENTPLUS, 99.99+%
SODIUM SULFIDE NONAHYDRATE 98+% &
SODIUM SULFIDE NONAHYDRATE, 98+%, A.C.S.
SODIUM SULFIDE NONAHYDRATE ACS REAGENT
SodiumSulphideGr
SodiumSulfide,10%Solution
SodiumSulphideFlakesExtraPure(IronFree)
SodiumSulfide,5%Solution | [EINECS(EC#)]
215-211-5 | [Molecular Formula]
H2Na2OS | [MDL Number]
MFCD00149183 | [Molecular Weight]
96.06 | [MOL File]
1313-84-4.mol |
| Chemical Properties | Back Directory | [Appearance]
colourless, white or yellow crystals with an odour of rotten eggs | [Melting point ]
50 °C | [Boiling point ]
920°C | [density ]
1.427 | [storage temp. ]
2-8°C
| [form ]
Solid | [color ]
colorless or slightly yellow | [Specific Gravity]
1.427 | [Stability:]
Stable. Hygroscopic. Light-sensitive. Flammable. Avoid exposure to air, acids, oxidizers, strong bases, strong reducing agents, most common metals. | [Water Solubility ]
180 G/L (25 ºC) | [Sensitive ]
Hygroscopic | [Merck ]
14,8681 | [InChIKey]
GDQBTRYKLOBMLL-UHFFFAOYSA-N | [CAS DataBase Reference]
1313-84-4(CAS DataBase Reference) | [EPA Substance Registry System]
1313-84-4(EPA Substance) |
| Safety Data | Back Directory | [Hazard Codes ]
C,N | [Risk Statements ]
R31:Contact with acids liberates toxic gas.
R34:Causes burns.
R50:Very Toxic to aquatic organisms. | [Safety Statements ]
S26:In case of contact with eyes, rinse immediately with plenty of water and seek medical advice .
S45:In case of accident or if you feel unwell, seek medical advice immediately (show label where possible) .
S61:Avoid release to the environment. Refer to special instructions safety data sheet . | [RIDADR ]
UN 1849 8/PG 2
| [WGK Germany ]
2
| [RTECS ]
WE1925000
| [F ]
13 | [TSCA ]
Yes | [HazardClass ]
8 | [PackingGroup ]
II | [HS Code ]
28301010 |
| Raw materials And Preparation Products | Back Directory | [Raw materials]
Sodium hydroxide-->Methanol-->Sodium sulfate-->Barium sulfate-->METALLURGICAL COKE | [Preparation Products]
Sodium carbonate-->Sodium sulfite-->o-Phenylenediamine-->1-Naphthylamine-->m-Toluidine-->p-Toluidine-->5-Aminonicotinic acid-->Mercaptoacetic acid-->1,3-Adamantanediol-->Fluorescein isothiocyanate isomer I-->5-Fluoronicotinic acid-->2-Amino-4-nitrophenol-->3,3,4,4-diphenylsulfonetetracarboxylicdianhydride-->5-AMINO-1,2,3-THIADIAZOLE-4-CARBOXYLIC ACID ETHYL ESTER-->Thioacetic acid-->Thiomorpholine-->5-AMINO-2-METHYLBENZOTHIAZOLE-->4-(Propylthio)benzene-1,2-diamine-->3-BROMO-5-IODOBENZOIC ACID-->3-Bromo-5-nitrobenzoic acid-->3-AMINO-5-BROMO-BENZOIC ACID-->2,5-BIS(4-PYRIDYL)-1,3,4-THIADIAZOLE-->2,5-Thiophenedicarboxylic acid-->Selenium sulfide-->Diallyl sulfide-->3-Amino-5-nitrobenzoic acid-->Cyclohexyl disulfide-->1,2,3-BENZOTHIADIAZOLE-5-CARBOXYLIC ACID-->Dibutyl sulfide |
| Questions And Answer | Back Directory | [Physical Properties]
The nonahydrate is a yellowish-white crystalline solid; tetragonal crystals; odor of hydrogen sulfide; the color changes on exposure to light and air, first turning to yellow and then becoming brownish-black, deliquescent; density 1.43 g/cm3; decomposes at about 50°C; very soluble in water; aqueous solution strongly alkaline; slightly soluble in alcohol; insoluble in ether.
| [Uses]
Sodium sulfide is used in making sulfur dyes; for dehairing of hides; removing sulfur from viscous rayon; engraving and lithography; cotton printing; manufacturing rubber; paper pulp; and as a photographic reagent. Other major applications are for treating paper and for extracting gold ores where oxidized metal ores are converted to sulfides prior to froth flotation. Sodium sulfide also is used in preparing many other sulfides and as an analytical reagent.
| [Preparation]
Sodium sulfide is prepared by heating sodium bisulfate with sodium chloride and coal above 950°C. The product mixture is extracted with water and the hydrated sulfide is obtained from the solution by crystallization:
NaHSO4 + NaCl + 2C → Na2S + 2CO2↑ + HCl↑
Sodium sulfide also is produced from its elements in liquid ammonia:
Na + 2S → Na2S
| [Reactions]
Sodium sulfide in solid form reacts with carbon dioxide in the presence of moisture to form hydrogen sulfide and sodium carbonate. Thus, the H2S odor of sodium sulfide crystals is attributed to its exposure to moist air:
Na2S + H2O + CO2 → Na2CO3 + H2S
In aqueous solution, sodium sulfide reacts with a number of metal salts forming insoluble sulfides.
When added to dilute mineral acids, hydrogen sulfide is generated.
|
| Hazard Information | Back Directory | [Chemical Properties]
colourless, white or yellow crystals with an odour of rotten eggs | [General Description]
Sodium sulfide nonahydrate participates in the conversion of nitroxides to amines, via reduction. | [Purification Methods]
Some purification of the hydrated salt can be achieved by selecting large crystals and removing the surface layer (contaminated with oxidation products) by washing with distilled water. Other metal ions can be removed from Na2S solutions by passage through a column of Dowex ion-exchange A-1 resin, Na+-form. The hydrated salt can be rendered anhydrous by heating it in a stream of H2 or N2 until water is no longer evolved. (The resulting cake should not be heated to fusion because it is readily oxidised.) Recrystallise it from distilled water [Anderson & Azowlay J Chem Soc, Dalton Trans 469 1986]. Note that sodium sulfide hydrolyses in H2O to form NaHS + H2O, and is therefore alkaline. A 0.1N solution in H2O is 86% hydrolysed at room temperature. Its solubility in H2O is 8% at 0o, 12% at 20o and 30% at 50o. The anhydrous salt is obtained by allowing it to stand in a vacuum over conc H2SO4 or P2O5 at 45o to start with, then at 30-35o when the salt contains 4% of water. The last traces of water are removed by heating to 700o in a glass or porcelain tube in a stream of H2 to give pure H2S. [Fehér in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I pp 358-360 1963.] |
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