Silver perchlorate

Silver perchlorate

Names
IUPAC name Silver perchlorate
Other names Perchloric acid, silver(1+) salt
Identifiers
CAS Number	7783-93-9 14242-05-8 (hydrate)
3D model (Jmol)	Interactive image
ChemSpider	22968
ECHA InfoCard	100.029.123
EC Number	232-035-4
PubChem	24562
InChI InChI=1S/Ag.ClHO4/c;2-1(3,4)5/h;(H,2,3,4,5)/q+1;/p-1 Key: YDHABVNRCBNRNZ-UHFFFAOYSA-M InChI=1/Ag.ClHO4/c;2-1(3,4)5/h;(H,2,3,4,5)/q+1;/p-1 Key: YDHABVNRCBNRNZ-REWHXWOFAI
SMILES [Ag+].[O-]Cl(=O)(=O)=O
Properties
Chemical formula	AgClO4
Molar mass	207.319 g/mol
Appearance	Colorless hygroscopic crystals
Density	2.806 g/cm^3
Melting point	486 °C (907 °F; 759 K) (decomposes)
Solubility in water	557 g/100 mL (25 °C) 792.8 g/100 mL (99 °C)
Solubility	soluble in organic solvents
Structure
Crystal structure	cubic
Hazards
R-phrases	R8 R34 R50
S-phrases	S15 S17 S26 S36/37/39 S45
NFPA 704	1 2 2 OX
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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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

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.

Salts and the ester of the perchlorate ion
HClO4																	He
LiClO4	Be(ClO4)2											B(ClO4)4^−	ROClO3	N(ClO4)3 NH4ClO4	O	FClO4	Ne
NaClO4	Mg(ClO4)2											Al(ClO4)3	Si	P	S	ClO4^− ClOClO3 Cl2O7	Ar
KClO4	Ca(ClO4)2	Sc(ClO4)3	Ti(ClO4)4	VO(ClO4)3	Cr(ClO4)3	Mn(ClO4)2	Fe(ClO4)3	Co(ClO4)2, Co(ClO4)3	Ni(ClO4)2	Cu(ClO4)2	Zn(ClO4)2	Ga(ClO4)3	Ge	As	Se	Br	Kr
RbClO4	Sr(ClO4)2	Y	Zr	Nb	Mo	Tc	Ru	Rh	Pd(ClO4)2	AgClO4	Cd(ClO4)2	In	Sn	Sb	Te	I	Xe
CsClO4	Ba(ClO4)2		Hf	Ta	W	Re	Os	Ir	Pt	Au	Hg2(ClO4)2, Hg(ClO4)2	Tl(ClO4)3	Pb(ClO4)2	Bi(ClO4)3	Po	At	Rn
Fr	Ra		Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Nh	Fl	Mc	Lv	Ts	Og
		↓
		La	Ce(ClO4)x	Pr	Nd	Pm	Sm	Eu	Gd	Tb	Dy	Ho	Er	Tm	Yb	Lu
		Ac	Th	Pa	UO2(ClO4)2	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No	Lr