Silver perchlorate
| Silver perchlorate | |
|---|---|
 | |
| IUPAC name Silver perchlorate | |
| Other names Perchloric acid, silver(1+) salt | |
| Identifiers | |
| CAS number | 7783-93-9  , [14242-05-8] (hydrate) |
| PubChem | 24562 |
| ChemSpider | 22968 |
| EC number | 232-035-4 |
| Jmol-3D images | {{#if:[Ag+].[O-]Cl(=O)(=O)=O|Image 1 |
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| Properties | |
| Molecular formula | AgClO4 |
| Molar mass | 207.319 g/mol |
| Appearance | Colorless hygroscopic crystals |
| Density | 2.806 g/cm3 |
| Melting point | 486 °C; 907 °F; 759 K (decomp) |
| Solubility in water | 557 g/100 mL (25 °C) 792.8 g/100 mL (99 °C) |
| Solubility | soluble in organic solvents |
| Hazards | |
| R-phrases | R8 R34 R50 |
| S-phrases | S15 S17 S26 S36/37/39 S45 |
| NFPA 704 |
 1
2
2
OX
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(verify) (what is: / ?)Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa) | |
| Infobox references | |
Silver perchlorate is the chemical compound with the formula AgClO4. This white solid forms a monohydrate and is mildly deliquescent. It is a useful source of the Ag+ ion, although the presence of perchlorate presents risks. It is used as a catalyst in organic chemistry.
Production
Silver perchlorate is created by heating a mixture of perchloric acid with silver nitrate.
Alternatively, it can be prepared by the reaction between barium perchlorate and silver sulfate, or from the reaction of perchloric acid with silver oxide.
Solubility
Silver perchlorate is noteworthy for its solubility in aromatic solvents such as benzene (52.8 g/L) and toluene (1010 g/L).[1] In these solvents, the silver cation binds to the arene, as has been demonstrated by extensive crystallographic studies on crystals obtained from such solutions.[2][3] It is also amazingly soluble in water, up to 500 g per 100 ml of water.
Related reagents
Similar to silver nitrate, silver perchlorate is an effective reagent for replacing halides ligands with perchlorate, which is a weakly or non-coordinating anion. The use of silver perchlorate in chemical synthesis has declined due to concerns about explosiveness of perchlorate salts. Other silver reagents are silver tetrafluoroborate, and the related silver trifluoromethanesulfonate and silver hexafluorophosphate.
References
- ↑ F. Březina, J. Mollin, R. Pastorek, Z. Šindelář (1986). Chemické tabulky anorganických sloučenin [Chemical tables of inorganic compounds] (in Czech). Prague: SNTL.
- ↑ E. A. Hall Griffith, E. L. Amma (1974). "Metal Ion-Aromatic Complexes. XVIII. Preparation and Molecular Structure of Naphthalene-Tetrakis(silver perchlorate) Tetrahydrate". Journal of the American Chemical Society 96 (3): 743–749. doi:10.1021/ja00810a018.
- ↑ R. K. McMullan, T. F. Koetzle, C. J. Fritchie Jr. (1997). "Low-Temperature Neutron Diffraction Study of the Silver Perchlorate–Benzene π Complex". Acta Crystallographica B 53 (4): 645–653. doi:10.1107/S0108768197000712.
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