Silver nitrite
| Names | |
|---|---|
| IUPAC name
Silver nitrite
| |
| Properties | |
| AgNO2 | |
| Molar mass | 153.87 g/mol |
| Appearance | White to yellowish crystals |
| Odor | Odorless |
| Density | 4.453 g/cm3 (25 °C) |
| Melting point | 140 °C (284 °F; 413 K) |
| Boiling point | Decomposes |
| 0.155 g/100 ml (0 °C) 0.275 g/100 ml (15 °C) 1.363 g/100 ml (60 °C) | |
| Solubility | Insoluble in ethanol, hydrocarbons |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Related compounds | |
| Related compounds
|
Silver nitrate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Silver nitrite is an inorganic compound with the formula AgNO2.
Contents
Properties
Chemical
Silver nitrite will react with haloalkanes to give nitro compounds.
Physical
Silver nitrite is a white-yellow solid, slightly soluble in water.
Availability
Silver nitrite can be bought from lab suppliers and online.
Preparation
Silver nitrite is produced from the reaction between silver nitrate and an alkali nitrite, such as sodium nitrite. Silver nitrite is much less soluble in water than silver nitrate, and a solution of silver nitrate will readily precipitate silver nitrite upon addition of sodium nitrite:
- AgNO3 + NaNO2 → NaNO3 + AgNO2
Alternatively, it can be produced by the reaction between silver sulfate and barium nitrite.
- Ag2SO4 + Ba(NO2)2 → 2 AgNO2 + BaSO4
Due to the poor solubility of silver sulfate in water, this requires a large volume of water. Alternatively, another silver salt, like silver(I) fluoride can be used.
Projects
- Preparation of aniline compounds
- Preparation of nitro compounds
Handling
Safety
Silver nitrite can stain the skin as well as most objects and is toxic if swallowed. Protection gloves should be worn when handling the compound.
Storage
In closed amber or opaque plastic bottles, away from sunlight and reducing agents.
Disposal
Since silver is expensive, it's best to recycle it.
