Difference between revisions of "Sodium sulfide"
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| − | Sodium sulfide is sold by chemical suppliers, though it's not easy get hold of in most places. | + | Sodium sulfide is sold by chemical suppliers, though it's not easy to get a hold of in most places. |
==Preparation== | ==Preparation== | ||
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*Make hydrogen sulfide (DANGEROUS) | *Make hydrogen sulfide (DANGEROUS) | ||
| − | *Make thioethers | + | *Make [[thioethers]] |
==Handling== | ==Handling== | ||
Revision as of 21:36, 16 August 2020
| Names | |
|---|---|
| IUPAC name
Sodium sulfide
| |
| Other names
Disodium sulfide
Disodium monosulfide | |
| Identifiers | |
| Jmol-3D images | Image |
| |
| Properties | |
| Na2S | |
| Molar mass | 78.0452 g/mol (anhydrous) 240.18 g/mol (nonahydrate) |
| Appearance | Colorless hygroscopic solid |
| Odor | Rotten eggs |
| Density | 1.856 g/cm3 (anhydrous) 1.58 g/cm3 (pentahydrate) 1.43 g/cm3 (nonohydrate) |
| Melting point | 1,176 °C (2,149 °F; 1,449 K) (anhydrous) 100 °C (212 °F; 373 K) (pentahydrate) 50 °C (122 °F; 323 K) (nonahydrate) |
| Boiling point | Decomposes |
| 12.4 g/100 ml (0 °C) 18.6 g/100 ml (20 °C) 39 g/100 ml (50 °C) Hydrolysis | |
| Solubility | Slightly soluble in alcohol Insoluble in diethyl ether |
| Hazards | |
| Safety data sheet | Sigma-Aldrich Sigma-Aldrich (nonahydrate) |
| Related compounds | |
| Related compounds
|
Hydrogen sulfide |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Sodium sulfide is the chemical compound with the chemical formula Na2S, or more commonly its nonahydrate form Na2S·9H2O.
Contents
Properties
Chemical
Sodium sulfide reacts with acids to release hydrogen sulfide.
Physical
Sodium sulfide is a white solid, though impure samples can be yellow or reddish. It has an unpleasant odor of rotten eggs, from the hydrogen sulfide released by the hydrolysis in moist air.
Availability
Sodium sulfide is sold by chemical suppliers, though it's not easy to get a hold of in most places.
Preparation
Industrially Na2S is produced by carbothermic reduction of sodium sulfate often using coal:
- Na2SO4 + 2 C → Na2S + 2 CO2
In the laboratory, this compound salt can be prepared by reacting elemental sulfur with sodium in anhydrous ammonia, in dry THF with a catalytic amount of naphthalene (forming sodium naphthalenide):
- 2 Na + S → Na2S
Projects
- Make hydrogen sulfide (DANGEROUS)
- Make thioethers
Handling
Safety
Like sodium hydroxide, sodium sulfide is strongly alkaline and can cause skin burns. Acids react with it to rapidly produce hydrogen sulfide, which is highly toxic.
Storage
In closed and air-tight bottles, away from moisture and acids.
Disposal
Sodium sulfide can be neutralized with bleach or hydrogen peroxide.
References
Relevant Sciencemadness threads
- Chemical pages without CAS Registry Number
- Articles without EBI source
- Chemical pages without ChemSpiderID
- Chemical pages without DrugBank identifier
- Articles without KEGG source
- Articles without InChI source
- Articles without UNII source
- Articles containing unverified chemical infoboxes
- Chembox articles without image
- Chemical compounds
- Inorganic compounds
- Sodium compounds
- Sulfur compounds
- Sulfides
- Materials unstable in acidic solution
