Physics
Scientific paper
Jun 1992
adsabs.harvard.edu/cgi-bin/nph-data_query?bibcode=1992gecoa..56.2267e&link_type=abstract
Geochimica et Cosmochimica Acta, vol. 56, Issue 6, pp.2267-2280
Physics
5
Scientific paper
The solubility of amorphous arsenic sulfide [As 2 S 3 (am)] has been experimentally determined from 25 to 90°C. In acidic, sulfide-deficient solutions, H 3 AsO 0 3 is the dominant product ofAs 2 S 3 (am) dissolution: 1/2 As 2 S 3 (am) + 3 H 2 O = H 3 AsO 0 3 + 3/2 H 2 S 0 . The respective logarithms of equilibrium constants for this reaction are -11.9 ± 0.3 at 25°C, -11.2 ± 0.2 at 40°C, -10.2 ± 0.1 at 60°C, and -9.0 ± 0.2 at 90°C, all at 0.1 m ionic strength. In acidic solutions with excess sulfide, experimental data are consistent with H 2 As 3 S - 6 being the dominant dissolved As species: 3/2 As 2 S 3 (am) + 3/2 H 2 S 0 = H 2 As 3 S - 6 + H + The respective logarithms of equilibrium constants for this reaction are -5.0 ± 0.3 at 25°C, -5.1 ± 0.3 at 40°C, -4.9 ± 0.2 at 60°C, and -4.1 ± 0.1 at 90°C, all at 0.1 m ionic strength. Speciation calculations for a number of acidic hot springs indicate that many have As and H 2 S 0 concentrations that are bracketed by the solubilities of As 2 S 3 (am) and orpiment and that H 3 AsO 0 3 is generally the dominant dissolved As species. The solubility data indicate that lowering of temperature and pH are the most likely mechanisms of As 2 S 3 (am) precipitation in hot spring systems.
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