Experimental investigations of the hydrothermal geochemistry of platinum and palladium: IV. The stoichiometry of Pt(IV) and Pd(II) chloride complexes at 100 to 300°C

Details Experimental investigations of the hydrothermal geochemistry of platinum and palladium: IV. The stoichiometry of Pt(IV) and Pd(II) chloride complexes at 100 to 300°C Experimental investigations of the hydrothermal geochemistry of platinum and palladium: IV. The stoichiometry of Pt(IV) and Pd(II) chloride complexes at 100 to 300°C

May 1995

adsabs.harvard.edu/cgi-bin/nph-data_query?bibcode=1995gecoa..59.1655g&link_type=abstract

Geochimica et Cosmochimica Acta, vol. 59, Issue 9, pp.1655-1667

Computer Science

3

Scientific paper

A technique based on the common ion effect was used to obtain information on the stoichiometry of the Pt(IV) and Pd(II) chloride complexes at elevated temperature. The solubility of AgCl(s) was measured in solutions of fixed m HCl and varying Pt(IV) or Pd(II) concentration. Parallel experiments were conducted at Me/Cl mole ratios (Me = Pt or Pd) of 0.0-0.5 for m HCl = 0.03-3.0 at T = 100, 200, and 300°C. The average Cl ligand numbers for Pt ranged from 4.2 to 5.8, with the majority of values > 5. These results are adequately explained by a mixture of the simple monomeric species PtCl 2- 6 , PtCl - 5 , and PtCl 0 4 . The temperature dependence of the equilibrium constant for the dissociation reaction PtCl 2- 6 = PtCl - 5 + Cl - was obtained: log K = 2.40 (±0.25) - , K (valid to 573 K), which is in good agreement with published low temperature data. The neutral PtCl 0 4 species may become important at 300°C and low chloride concentrations (0.01 m HCl). Extrapolation of existing data indicates that the PT(IV) chloride complexes are stable with respect to Pt(II) chloride complexes over a range of f O 2 -pH conditions which narrows quickly with increase in temperature. Nonetheless, PtCl 2- 6 may be the dominant form of dissolved Pt in highly oxidized brines to at least 100°C. The average Cl ligand numbers for palladium ranged from 2.14 to 2.83, and were insensitive to temperature. These results could be explained by a mixture of PdCl 2 and PdCl - 3 . However, this is in disagreement with published experimental data which indicate that PdCl -2 4 is the predominant form of aqueous Pd at high chloride concentrations. An alternate explanation is that a significant quantity of the total aqueous Pd was present as polynuclear complexes, due to the very high Pd/Cl ratios of the experiments. Insufficient data exist to discriminate between these two hypotheses.

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