Silver perchlorate
Names
IUPAC name
Silver(I) perchlorate
Systematic IUPAC name
Silver(I) chlorate(VII)
Other names
Perchloric acid, silver(1+) salt
Argentous perchlorate
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.029.123
EC Number
  • 232-035-4
UNII
  • InChI=1S/Ag.ClHO4/c;2-1(3,4)5/h;(H,2,3,4,5)/q+1;/p-1 checkY
    Key: YDHABVNRCBNRNZ-UHFFFAOYSA-M checkY
  • InChI=1/Ag.ClHO4/c;2-1(3,4)5/h;(H,2,3,4,5)/q+1;/p-1
    Key: YDHABVNRCBNRNZ-REWHXWOFAI
  • [Ag+].[O-]Cl(=O)(=O)=O
Properties
AgClO4
Molar mass 207.319 g/mol
Appearance Colorless hygroscopic crystals
Density 2.806 g/cm3
Melting point 486 °C (907 °F; 759 K) (decomposes)
557 g/100 mL (25 °C)
792.8 g/100 mL (99 °C)
Solubility soluble in organic solvents
Structure
cubic
Hazards
GHS labelling:
GHS03: OxidizingGHS05: Corrosive
Danger
H272, H314
P210, P220, P221, P260, P264, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P370+P378, P405, P501
NFPA 704 (fire diamond)
NFPA 704 four-colored diamond
2
0
2
OX
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)
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] Its solubility in water is extremely high, up to 500 g per 100 mL water.

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

  1. ↑ F. Březina; J. Mollin; R. Pastorek; Z. Šindelář (1986). Chemické tabulky anorganických sloučenin [Chemical tables of inorganic compounds] (in Czech). Prague: SNTL.
  2. ↑ 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.
  3. ↑ 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. S2CID 97838907.
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