Difference between revisions of "Ammonium sulfide"
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| pKb = | | pKb = | ||
| Solubility = 128.1 g/100 mL (at 20 °C) | | Solubility = 128.1 g/100 mL (at 20 °C) | ||
− | | SolubleOther = Soluble in liquid [[ammonia]], [[ethanol]] | + | | SolubleOther = Reacts with acids, bases<br>Soluble in liquid [[ammonia]], [[ethanol]], [[methanol]] |
| Solvent = | | Solvent = | ||
| VaporPressure = | | VaporPressure = | ||
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'''Ammonium sulfide''' is an unstable ammonium salt with the formula '''(NH<sub>4</sub>)<sub>2</sub>S'''. It is a yellowish solid, stable below -18 °C. | '''Ammonium sulfide''' is an unstable ammonium salt with the formula '''(NH<sub>4</sub>)<sub>2</sub>S'''. It is a yellowish solid, stable below -18 °C. | ||
− | As the hydrosulfide ion cannot be deprotonated to an appreciable amount by ammonia (pKa = 15), ammonium sulfide solutions also contain free ammonia and ammonium hydrosulfide (NH<sub>4</sub>)SH. | + | As the hydrosulfide ion cannot be deprotonated to an appreciable amount by ammonia (pKa = 15), ammonium sulfide solutions also contain free [[ammonia]] and ammonium hydrosulfide (NH<sub>4</sub>)SH. |
==Properties== | ==Properties== | ||
===Chemical=== | ===Chemical=== | ||
− | Ammonium sulfide will tarnish silver, by forming a layer of silver sulfide on its surface. | + | Ammonium sulfide will tarnish [[silver]], by forming a layer of silver sulfide on its surface. |
===Physical=== | ===Physical=== | ||
− | Ammonium sulfide is a | + | Ammonium sulfide is a yellowish solid compound at low temperatures, but unstable above -18 °C, with a very strong and highly unpleasant smell of rotten eggs. It is very soluble in water and [[ammonia]], as well as [[alcohol]]s. |
==Availability== | ==Availability== | ||
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==Preparation== | ==Preparation== | ||
− | Can be made by bubbling ammonia through an aqueous solution of hydrogen sulfide. For higher purity, hydrogen sulfide is bubbled through anhydrous ammonia. | + | Can be made by bubbling ammonia through an aqueous solution of [[hydrogen sulfide]]. For higher purity, dry hydrogen sulfide is bubbled through anhydrous ammonia. |
This procedure is very dangerous and should ONLY be performed in well ventilated areas, preferably in some place far away from civilization. | This procedure is very dangerous and should ONLY be performed in well ventilated areas, preferably in some place far away from civilization. | ||
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===Safety=== | ===Safety=== | ||
Ammonium sulfide releases hydrogen sulfide upon decomposition, which is very toxic. Proper protection must be worn all the time when handling the compound. | Ammonium sulfide releases hydrogen sulfide upon decomposition, which is very toxic. Proper protection must be worn all the time when handling the compound. | ||
+ | |||
+ | As the compound readily realeases hydrogen sulfide, extreme safety must be employed when working with the compound. A property of H<sub>2</sub>S is that is can temporarily deaden a person's sense of smell, a sickening effect that a few Sciencemadness members have had personal experiences with. If you are in an area with a strong smell of hydrogen sulfide, and then that strong smell suddenly disappears for no apparent reason, '''immediately leave the area'''! At the concentration where this occurs, the gas is potentially deadly, with a toxicity not very far from the infamous hydrogen cyanide, not to mention undetectable. Safety plans should be in order during any experiment which makes use of hydrogen sulfide, including a way to quickly leave the room/area. | ||
===Storage=== | ===Storage=== | ||
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[[Category:Blood agents]] | [[Category:Blood agents]] | ||
[[Category:Kewlism]] | [[Category:Kewlism]] | ||
+ | [[Category:Irritants]] |
Latest revision as of 16:39, 1 March 2021
Names | |
---|---|
IUPAC name
Ammonium sulfide
| |
Other names
Diammonium sulfide
Diazanium sulfide | |
Identifiers | |
Jmol-3D images | Image |
| |
Properties | |
(NH4)2S | |
Molar mass | 68.154 g/mol |
Appearance | Yellow crystals |
Odor | Unpleasant, rotten eggs-like |
Density | 0.997 g/cm3 |
Melting point | Decomposes |
Boiling point | Decomposes |
128.1 g/100 mL (at 20 °C) | |
Solubility | Reacts with acids, bases Soluble in liquid ammonia, ethanol, methanol |
Hazards | |
Safety data sheet | FisherScientific |
Flash point | 32.22 °C |
Related compounds | |
Related compounds
|
Hydrogen sulfide Ammonium sulfate |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
Infobox references | |
Ammonium sulfide is an unstable ammonium salt with the formula (NH4)2S. It is a yellowish solid, stable below -18 °C.
As the hydrosulfide ion cannot be deprotonated to an appreciable amount by ammonia (pKa = 15), ammonium sulfide solutions also contain free ammonia and ammonium hydrosulfide (NH4)SH.
Contents
Properties
Chemical
Ammonium sulfide will tarnish silver, by forming a layer of silver sulfide on its surface.
Physical
Ammonium sulfide is a yellowish solid compound at low temperatures, but unstable above -18 °C, with a very strong and highly unpleasant smell of rotten eggs. It is very soluble in water and ammonia, as well as alcohols.
Availability
Ammonium sulfide can be encountered as solution in "stink bombs".
Preparation
Can be made by bubbling ammonia through an aqueous solution of hydrogen sulfide. For higher purity, dry hydrogen sulfide is bubbled through anhydrous ammonia.
This procedure is very dangerous and should ONLY be performed in well ventilated areas, preferably in some place far away from civilization.
Projects
Ammonium sulfide can be a good source of concentrated hydrogen sulfide for many reactions, however, due to its instability it's recommended to perform experimentation only in well ventilated places and proper protection must be worn at all times.
- Make lead sulfide
- Stink bomb
- Selective reducing agent for some alkaloids
Handling
Safety
Ammonium sulfide releases hydrogen sulfide upon decomposition, which is very toxic. Proper protection must be worn all the time when handling the compound.
As the compound readily realeases hydrogen sulfide, extreme safety must be employed when working with the compound. A property of H2S is that is can temporarily deaden a person's sense of smell, a sickening effect that a few Sciencemadness members have had personal experiences with. If you are in an area with a strong smell of hydrogen sulfide, and then that strong smell suddenly disappears for no apparent reason, immediately leave the area! At the concentration where this occurs, the gas is potentially deadly, with a toxicity not very far from the infamous hydrogen cyanide, not to mention undetectable. Safety plans should be in order during any experiment which makes use of hydrogen sulfide, including a way to quickly leave the room/area.
Storage
Storage of ammonium sulfide presents great difficulties, as even the slightest leak will create a foul smelling environment. Ampouling the compound is generally the best method.
Disposal
Hydrogen peroxide will oxidize ammonium sulfide to ammonium sulfate, which is safe to handle. Bubbling hot sulfur dioxide (70 °C) through the solution will give the same result.
It is recommended to avoid using bleach, as it may yield chloramines.
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
- Ammonium compounds
- Sulfur compounds
- Sulfides
- Materials unstable in basic solution
- Reducing agents
- Foul smelling compounds
- Blood agents
- Kewlism
- Irritants