Chloroauric acid is an inorganic compound with the chemical formulaH[AuCl4]. It forms hydrates H[AuCl4]·nH2O. Both the trihydrate and tetrahydrate are known. Both are orange-yellow solids consisting of the planar [AuCl4]− anion. Often chloroauric acid is handled as a solution, such as those obtained by dissolution of gold in aqua regia. These solutions can be converted to other gold complexes or reduced to metallic gold or gold nanoparticles.
The oxidation state of gold in H[AuCl4] and [AuCl4]− anion is +3. The salts of H[AuCl4] (tetrachloroauric(III) acid) are tetrachloroaurates(III), containing [AuCl4]− anions (tetrachloroaurate(III) anions), which have square planar molecular geometry. The Au–Cl distances are around 2.28 Å. Other d8 complexes adopt similar structures, e.g. tetrachloroplatinate(II) [PtCl4]2−.
Solid chloroauric acid is a hydrophilic (ionic) protic solute. It is soluble in water and other oxygen-containing solvents, such as alcohols, esters, ethers, and ketones. For example, in dry dibutyl etherordiethylene glycol, the solubility exceeds 1 M.[4][5][6] Saturated solutions in the organic solvents often are the liquid solvates of specific stoichiometry. Chloroauric acid is a strong monoprotic acid.
When heated in air, solid H[AuCl4]·nH2O melts in the water of crystallization, quickly darkens and becomes dark brown.
Since [AuCl4]− is prone to hydrolyze,[7] upon treatment with an alkali metal base, chloroauric acid converts to gold(III) hydroxide.[8] The related thallium salt(Tl+[AuCl4]−) is poorly soluble in all nonreacting solvents. Salts of quaternary ammonium cations are known.[9] Other complex salts include [Au(bipy)Cl2]+[AuCl4]−[10] and [Co(NH3)6]3+[AuCl4]−(Cl−)2.
Partial reduction of chloroauric acid gives oxonium dichloridoaurate(1−).[11] Reduction may also yield other gold(I) complexes, especially with organic ligands. Often the ligand serves as reducing agent as illustrated with thiourea, CS(NH2)2:
Chloroauric acid is the precursor to gold nanoparticles by precipitation onto mineral supports.[12] Heating of H[AuCl4]·nH2O in a stream of chlorine gives gold(III) chloride (Au2Cl6).[13] Gold nanostructures can be made from chloroauric acid in a two-phase redox reaction whereby metallic clusters are amassed through the simultaneous attachment of self-assembled thiol monolayers on the growing nuclei. [AuCl4]− is transferred from aqueous solution to toluene using tetraoctylammonium bromide where it is then reduced with aqueous sodium borohydride in the presence of a thiol.[14]
Chloroauric acid is produced by dissolving gold in aqua regia (a mixture of concentrated nitric and hydrochloric acids) followed by careful evaporation of the solution:[15][16]
Under some conditions, oxygen can be used as an oxidant.[17] For higher efficiency, these processes are conducted in autoclaves, which allows greater control of temperature and pressure. Alternatively, a solution of H[AuCl4] can be produced by electrolysis of gold metal in hydrochloric acid:
2 Au(s) + 8 HCl(aq) → 2 H[AuCl4](aq) + 3 H2(g)
To prevent the deposition of gold on the cathode, the electrolysis is carried out in a cell equipped with a membrane. This method is used for refining gold. Some gold remains in solution in the form of [AuCl2]−.[18]
Liquid–liquid extraction of chloroauric acid is used for the recovery, concentrating, purification, and analytical determinations of gold. Of great importance is the extraction of H[AuCl4] from hydrochloric medium by oxygen-containing extractants, such as alcohols, ketones, ethers and esters. The concentration of gold(III) in the extracts may exceed 1 mol/L.[4][5][6] Frequently used extractants for this purpose are dibutyl glycol, methyl isobutyl ketone, tributyl phosphate, dichlorodiethyl ether (chlorex).[19]
Inhistology, chlorauric acid is known as "brown gold chloride", and its sodium salt Na[AuCl4] (sodium tetrachloroaurate(III)) as "gold chloride", "sodium gold chloride" or "yellow gold chloride". The sodium salt is used in a process called "toning" to improve the optical definition of tissue sections stained with silver.[20]
Chloroauric acid is a strong eye, skin, and mucous membrane irritant. Prolonged skin contact with chloroauric acid may result in tissue destruction. Concentrated chloroauric acid is corrosive to skin and must, therefore, be handled with appropriate care, since it can cause skin burns, permanent eye damage, and irritation to mucous membranes. Gloves are worn when handling the compound.[citation needed]
^Williams, Jack Marvin; Peterson, Selmer Wiefred (1969). "Example of the [H5O2]+ ion. Neutron diffraction study of tetrachloroauric acid tetrahydrate". Journal of the American Chemical Society. 91 (3): 776–777. doi:10.1021/ja01031a062. ISSN0002-7863.
^O'Reilly, Donald E.; Peterson, E. M.; Scheie, C. E.; Williams, Jack M. (1971). "Nuclear Magnetic Resonance of the Aquated Proton. II. Chloroauric Acid Tetrahydrate. Phase Transitions and Molecular Motion". The Journal of Chemical Physics. 55 (12): 5629–5635. Bibcode:1971JChPh..55.5629O. doi:10.1063/1.1675731.
^ abMironov, I. V.; Natorkhina, K. I. (2012). "On the selection of extractant for the preparation of high-purity gold". Russian Journal of Inorganic Chemistry. 57 (4): 610. doi:10.1134/S0036023612040195. S2CID98015888.
^ abMorris, D. F. C.; Khan, M. A. (1968). "Application of solvent extraction to the refining of precious metals, Part 3: purification of gold". Talanta. 15 (11): 1301–1305. doi:10.1016/0039-9140(68)80053-0. PMID18960433.
^Makotchenko, E. V.; Kokovkin, V. V. (2010). "Solid contact [AuCl4]−-selective electrode and its application for evaluation of gold(III) in solutions". Russian Journal of General Chemistry. 80 (9): 1733. doi:10.1134/S1070363210090021. S2CID95581984.
^Mironov, I. V.; Tsvelodub, L. D. (2001). "Equilibria of the substitution of pyridine, 2,2′-bipyridyl, and 1,10-phenanthroline for Cl− in AuCl4− in aqueous solution". Russian Journal of Inorganic Chemistry. 46: 143–148.
^Brust, Mathias; Walker, Merryl; Bethell, Donald; Schiffrin, David J.; Whyman, Robin (1994). "Synthesis of Thiol-derivatised Gold Nanoparticles in a Two-phase Liquid-Liquid System". J. Chem. Soc., Chem. Commun. (7). Royal Society of Chemistry: 801–802. doi:10.1039/C39940000801.
^Brauer, G., ed. (1963). Handbook of Preparative Inorganic Chemistry (2nd ed.). New York: Academic Press.
^Novoselov, R. I.; Makotchenko, E. V. (1999). "Application of oxygen as ecologically pure reagent for the oxidizing of non-ferrous and precious metals, sulphide minerals". Chemistry for Sustainable Development. 7: 321–330.
^Belevantsev, V. I.; Peschevitskii, B. I.; Zemskov, S. V. (1976). "New data on chemistry of gold compounds in solutions". Izvestiya Sibirskogo Otdeleniya AN SSSR, Ser. Khim. Nauk. 4 (2): 24–45.
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