Silver formate
| Names | |
|---|---|
| IUPAC name
Silver formate
| |
| Other names
Silver methanoate
Silver(I) formate | |
| Properties | |
| CHO2Ag HCOOAg | |
| Molar mass | 152.886 g/mol |
| Appearance | Colorless white solid |
| Odor | Odorless |
| Density | 4.25 g/cm3 (20 °C)[1] |
| Melting point | 95 °C (203 °F; 368 K) (decomposes) |
| Boiling point | Decomposes |
| Insoluble | |
| Solubility | Reacts with haloacids Insoluble in organic solvents |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std enthalpy of
formation (ΔfH |
350 kJ/mol[2] |
| Hazards | |
| Safety data sheet | None |
| Flash point | Detonates |
| Related compounds | |
| Related compounds
|
Silver acetate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Silver formate is an unstable chemical compound, a salt of silver and formic acid. It has the formula HCOOAg.
Contents
Properties
Chemical
Silver formate is unstable and sensitive to light and will detonate upon heating, releasing silver nanoparticles, as well as carbon dioxide and hydrogen:[1]
- HCOOAg → Ag + CO2 + ½ H2
According to the source above, it can even detonate at standard conditions, upon standing in open air.
Physical
Silver formate is a colorless solid, insoluble in water and organic solvents.
Explosive
Silver formate has been known to explode upon heating above 95 °C. It's claimed that it can detonate spontaneous at standard conditions, with some claims that it can even detonate in the presence of moisture.[3] or upon drying.[4][5]
Availability
Silver formate is not sold by suppliers.
Preparation
Silver formate can be obtained by reacting [silver nitrate]] with ammonium formate.
- AgNO3 + HCOONH4 → HCOOAg + NH4NO3
Alternatively, it can be obtained by reacting silver oxide[6][7] or silver carbonate[8] with formic acid, in aq. solution:
- Ag2O + 2 HCOOH → 2 HCOOAg + H2O
- Ag2CO3 + 2 HCOOH → 2 HCOOAg + H2O + CO2
Projects
- Pyrotechnic demonstration
- Make silver nanoparticles
Handling
Safety
Silver formate is unstable and may detonate under strong heating or mechanical shock. It has been documented that it may spontaneously decompose violently even upon sitting.
Storage
Should not be stored for too long.
Disposal
Safe destruction of this compound can be done by heating it under water. The resulting Ag particles from its decomposition should be recycled.
Like most silver salts, strong light will break down this compound.
References
- ↑ 1.0 1.1 Anna N. Puzan, Vyacheslav N. Baumer, Pavel V. Mateychenko, Journal of Solid State Chemistry Volume 246, February 2017, Pages 264-268, "Structure and decomposition of the silver formate Ag(HCO2)"
- ↑ Sakiyama, Minoru; Murata, Shigeo; Bulletin of the Chemical Society of Japan; vol. 57; nb. 5; (1984); p. 1174 - 1178
- ↑ Kendall, J.; Adler, H.; Journal of the American Chemical Society; vol. 43; (1921); p. 1470 - 1481
- ↑ Koeroesy; Nature; vol. 160; (1947); p. 21
- ↑ https://patents.google.com/patent/US2630444A/en
- ↑ https://patentimages.storage.googleapis.com/94/16/72/eefa3f05f34d51/US2630444.pdf
- ↑ Gmelin Handbuch der Anorganischen Chemie; vol. Ag: MVol.B5; 2.1, page 120 - 121
- ↑ Oshima, Masato; Sakamoto, Toshiaki; Maruyama, Yooichiroh; Ozawa, Fumiyuki; Shimizu, Isao; Yamamoto, Akio; Bulletin of the Chemical Society of Japan; vol. 73; nb. 2; (2000); p. 453 - 464
