Silver oxalate

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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
209-301.8 J·mol-1·K-1[5]
-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

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

  1. 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
  2. Ferrell, D. T.; Blackburn, I.; Vosburgh, W. C.; Journal of the American Chemical Society; vol. 70; (1948); p. 3812 - 3815
  3. Chemist's Handbook. - T. 2. - L.-M.: Chemistry, 1964 (Справочник химика. - Т. 2. - Л.-М.: Химия, 1964)
  4. 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. 5.0 5.1 Zhuk, N. P.; Zhurnal Fizicheskoj Khimii; vol. 28; (1954); p. 1690 - 1697; C.A.; (1956); p. 31
  6. Bichowsky, F. R.; Rossini, F. D.; The Thermochemistry of the Chemical Substances, 3. Aufl., New York 1951, S. 295

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