Silver oxalate
| Names | |
|---|---|
| IUPAC name
Silver(I) ethanedioate
| |
| Other names
Argentous oxalate
Disilver oxalate Silver ethanedioate Silver(I) oxalate | |
| Properties | |
| Ag2C2O4 | |
| Molar mass | 303.755 g/mol |
| Appearance | Colorless white solid |
| Odor | Odorless |
| Density | 5.066 g/cm3 (20 °C)[1] |
| Melting point | 127–140 °C (261–284 °F; 400–413 K) (decomposes)[4] |
| Boiling point | Decomposes |
| 0.0034 g/100 ml (18 °C) 0.00378 g/100 g (21 °C) 0.00416 (25 °C)[2][3] | |
| Solubility | Insoluble in organic solvents |
| Vapor pressure | ~0 mmHg |
| Thermochemistry | |
| Std molar
entropy (S |
209-301.8 J·mol-1·K-1[5] |
| Std enthalpy of
formation (ΔfH |
-668 kJ/mol[6] |
| Hazards | |
| Safety data sheet | None |
| Related compounds | |
| Related compounds
|
Silver formate 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 oxalate is a chemical compound with the chemical formula Ag2C2O4
Contents
Properties
Chemical
Silver oxalate decomposes explosively upon heating around 140 °C, releasing silver metal nanoparticles and carbon dioxide.
- Ag2C2O4 → 2 Ag + 2 CO2
Physical
Silver oxalate is a white solid, insoluble in water.
Explosive
Silver oxalate is somewhat sensitive to shock and friction. It also explodes when heated at high temperatures.
Availability
Silver oxalate is not sold by chemical suppliers and has to be made in situ.
Preparation
Can be prepared by adding oxalic acid to silver nitrate.
- H2C2O4 + 2 AgNO3 → Ag2C2O4 + 2 HNO3
While water is the more common solvent for this reaction, ethanol or acetonitrile can also be used as reaction solvents.[4]
Projects
- Pyrotechnic demonstration
- Make silver nanoparticles
Handling
Safety
Silver oxalate is somewhat explosive, though its sensitivity greatly depends on its purity.
Storage
In closed bottles, away from light.
Disposal
Safe destruction of this compound can be done by heating it under water. The resulting Ag particles from its decomposition should be recycled.
References
- ↑ Naumov, Dmitry Yu.; Virovets, Alexander V.; Podberezskaya, Nina V.; Boldyreva Elena V.; Acta Crystallographica, Section C: Crystal Structure Communications; vol. 51; (1995); p. 60 - 62
- ↑ Ferrell, D. T.; Blackburn, I.; Vosburgh, W. C.; Journal of the American Chemical Society; vol. 70; (1948); p. 3812 - 3815
- ↑ Chemist's Handbook. - T. 2. - L.-M.: Chemistry, 1964 (Справочник химика. - Т. 2. - Л.-М.: Химия, 1964)
- ↑ 4.0 4.1 Jakob; Schmidt; Walfort; Rheinwald; Fruehauf; Schulz; Gessner; Lang; Zeitschrift fur Anorganische und Allgemeine Chemie; vol. 631; nb. 6-7; (2005); p. 1079 - 1086
- ↑ 5.0 5.1 Zhuk, N. P.; Zhurnal Fizicheskoj Khimii; vol. 28; (1954); p. 1690 - 1697; C.A.; (1956); p. 31
- ↑ Bichowsky, F. R.; Rossini, F. D.; The Thermochemistry of the Chemical Substances, 3. Aufl., New York 1951, S. 295
