Silver perchlorate
| Names | |
|---|---|
| IUPAC name
Silver perchlorate
| |
| Other names
Perchloric acid, silver(1+) salt
Silverperchlorate | |
| Properties | |
| AgClO4 | |
| Molar mass | 207.319 g/mol |
| Appearance | White solid, hygroscopic |
| Odor | Odorless |
| Density | 2.806 g/cm3 |
| Melting point | 486 °C (907 °F; 759 K) (decomposition) |
| Boiling point | Decomposes |
| 557 g/100 ml (25 °C) 792.8 g/100 ml (99 °C) | |
| Solubility | Soluble in alcohols |
| Vapor pressure | ~0 mmHg |
| Hazards | |
| Safety data sheet | Sigma-Aldrich |
| Flash point | Non-flammable |
| Related compounds | |
| Related compounds
|
Silver nitrate Silver sulfate |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Silver perchlorate is a chemical compound with the formula AgClO4. It is a useful source of the Ag+ ions, due to its great solubility.
Contents
Properties
Chemical
Silver perchlorate decomposes when heated to high temperatures, releasing oxygen.
- AgClO4 → AgCl + 2 O2
Silver perchlorate reacts with iodine to form silver iodide and iodine perchlorate. It was hypothesized originally that this reaction would yield chlorine tetraoxide, but later experiments proved that iodine perchlorate is formed instead:[1]
- AgClO4 + I2 → AgI + IClO4
Physical
Silver perchlorate is a white solid, very soluble in water. It is hygroscopic and tends to be commonly encountered as monohydrate.
Availability
Silver perchlorate is sometimes sold by chemical suppliers, albeit it's expensive.
Preparation
Silver perchlorate can be made by dissolving various silver compounds, such as silver oxide[2] or silver carbonate[3][4] in perchloric acid.
- Ag2O + 2 HClO4 → 2 AgClO4 + H2O
- Ag2CO3 + 2 HClO4 → 2 AgClO4 + H2O + CO2
It can also be obtained by heating a mixture of perchloric acid with silver nitrate.
- AgNO3 + HClO4 → AgClO4 + HNO3
Alternatively, it can be prepared by the reaction between barium or lead(II) perchlorate and silver(I) fluoride:
- 2 AgF + Ba(ClO4)2 → 2 AgClO4 + BaF2
- 2 AgF + Pb(ClO4)2 → 2 AgClO4 + PbF2
Silver sulfate can also be used for this reaction, although its low solubility in water limits its efficiency.[5]
Silver metal doesn't react with perchloric acid at room temperatures, but will react at high temperatures, where perchloric acid becomes more oxidizing, yielding silver perchlorate, and side products.[6]
A route to obtain water-free silver perchlorate indicated in literature involves the reaction between nitrosyl perchlorate and silver bromide. The reaction takes place in a tube, for 24 hours and heating at 50, 75 and 100 °C successively. The resulting nitrosyl bromide is removed from the reaction by heating the tube further for 3 hours at 3-5 Torr and heating at then at 100 °C in vacuum for 12 hours.[7]
- AgBr + NOClO4 → AgClO4 + NOBr
Projects
- Catalyst in organic reactions
- Make iodine perchlorate
- Flash powders
Handling
Safety
Silver perchlorate is a strong oxidizer and should be handled with care.
Being a soluble silver salt, ingestion is harmful.
Storage
In closed bottles, away from moisture and flammable materials.
Disposal
Silver perchlorate can be neutralized by reducing it with metallic iron. It can also be reduced to elemental silver with many common metals, like iron, zinc. The resulting silver metal should be recycled as it is expensive.
References
- ↑ https://pubs.rsc.org/en/content/articlelanding/1962/JR/jr9620002510
- ↑ Hendrixson; Journal of the American Chemical Society; vol. 34; (1912); p. 389
- ↑ Carnelley; O'Shea; Journal of the Chemical Society, Transactions; vol. 45; (1884); p. 409 - 410
- ↑ Lapidus, M.; Lucas, M.; Tremillon, B.; Bulletin de la Societe Chimique de France; Bulletin de la Societe Chimique de France; (1960); p. 1949 - 1955
- ↑ Groth, P.; ; vol. 133; (1868); p. 193 - 228
- ↑ Roth, R.; Zur Kenntnis der Perchlorate, Dissert. Muenchen 1910, S. 22
- ↑ Markowitz, M. M.; Ricci, J. E.; Goldman, R. J.; Winternitz, P. E.; Journal of Inorganic and Nuclear Chemistry; vol. 16; (1960); p. 159 - 161
