Aqueous Nonelectrolyte Solutions. Part X. Mercury Solubility in Water

Glew, D. N.; Hames, D. A.

doi:10.1139/v71-520

Cited by 59 publications

(30 citation statements)

References 9 publications

Supporting

Mentioning

Contrasting

Order By: Relevance

“…6 For comparison, this value is similar to that of ethylbenzene at 7.9×10 3 atmm 3 /mol at 25°C. 7 The temperature dependence of the Henry's law constant shown in Figure 3 increases by about a factor of 1.6 for every 10 degree temperature rise.…”

Section: Chemistry Of Mercurysupporting

confidence: 56%

“…4,5 Mercury is slightly soluble in water, with a solubility of 59 µg/L at 25°C and a logarithmic temperature dependence shown in Figure 2. 6 The solubility of mercury in water increases by a factor of approximately 1.3 for every 10 degree rise in temperature. The Henry's law constant for elemental mercury, expressed as the ratio of the partial pressure above the solution to the solution concentration (K H = P Hg /c aq ), is 8.7×10…”

Section: Chemistry Of Mercurymentioning

confidence: 99%

“…7 The temperature dependence of the Henry's law constant shown in Figure 3 increases by about a factor of 1.6 for every 10 degree temperature rise. 6 Mercury occurs naturally in two oxidation states, ie, mercury(I), which exists as the dimeric cation (Hg 2 2+ ), formerly called the mercurous ion, and mercury(II) (Hg 2+ ), also called the mercuric ion. Mercury(I), rapidly and reversibly disproportionates to give elemental mercury and mercury(II), as:…”

Section: Chemistry Of Mercurymentioning

confidence: 99%

“…; the BAF for the primary carnivores in trophic level 3 are 7×10 5 ; and the BAF for the secondary carnivores in trophic level 4, including fish and birds, are 3×10 6 . 31 Therefore, levels of methylmercury in large fish are, on average, a million times the concentration of methylmercury in the water.…”

mentioning

confidence: 99%

See 3 more Smart Citations

In-depth review of atmospheric mercury: sources, transformations, and potential sinks

Gaffney¹,

Marley²

2014

EECT

View full text Add to dashboard Cite

Mercury is a toxic heavy metal that is found naturally throughout the global environment. During the last 100 years, there has been a 70% rise in atmospheric mercury levels over the natural background measured prior to industrialization due to anthropogenic emissions. This increase in mercury levels represents a global threat to the health of ecosystems and humans worldwide. Atmospheric mercury chemistry is complex and its sources and sinks involve equilibrium interactions between the atmosphere, the hydrosphere, and the geosphere. This review outlines the fundamental chemistry of mercury in gas, aqueous, and solid phases, including inorganic, organic, and complexed mercury species. An understanding of this chemistry is important for understanding the cycling between the various environmental compartments as it affects atmospheric loadings. Further, many of these reactions can also occur in the atmosphere in heterogeneous gas/cloud/aerosol interactions. The sources and fate of mercury in the atmosphere, including the cycling of mercury through soil and water as it impacts atmospheric loadings are therefore examined. The sources of major uncertainties in our understanding of mercury in the atmosphere are also discussed, along with recommendations for future studies that include both homogeneous and heterogeneous reactions of the various mercury species.

show abstract

Section: Chemistry Of Mercurysupporting

confidence: 56%

Section: Chemistry Of Mercurymentioning

confidence: 99%

Section: Chemistry Of Mercurymentioning

confidence: 99%

mentioning

confidence: 99%

See 2 more Smart Citations

In-depth review of atmospheric mercury: sources, transformations, and potential sinks

Gaffney¹,

Marley²

2014

EECT

View full text Add to dashboard Cite

show abstract

“…In addition to hydroxide and sulfide complexes, mercury can be transported as a hydrated aqueous species (Reichardt , 1913;Stock, 1934;Choi, 1962;Glew, 1971;Sorokin, 1973 and. Predicted values for the solubility constant of reaction (41) are also well desccribed (Fig.…”

Section: Hgmentioning

confidence: 99%

The Hydrothermal Chemistry of Gold, Arsenic, Antimony, Mercury and Silver

Bessinger¹,

Apps²

2003

View full text Add to dashboard Cite

A comprehensive thermodynamic database based on the Helgeson-Kirkham-Flowers (HKF) equation of state was developed for metal complexes in hydrothermal systems. Because this equation of state has been shown to accurately predict standard partial molal thermodynamic properties of aqueous species at elevated temperatures and pressures, this study provides the necessary foundation for future exploration into transport and depositional processes in polymetallic ore deposits. The HKF equation of state parameters for gold, arsenic, antimony, mercury, and silver sulfide and hydroxide complexes were derived from experimental equilibrium constants using nonlinear regression calculations. In order to ensure that the resulting parameters were internally consistent, those experiments utilizing incompatible thermodynamic data were re-speciated prior to regression.Because new experimental studies were used to revise the HKF parameters for H 2 S 0 and HS -1 , those metal complexes for which HKF parameters had been previously derived were also updated. It was found that predicted thermodynamic properties of metal complexes are consistent with linear correlations between standard partial molal thermodynamic properties. This result allowed assessment of several complexes for which experimental data necessary to perform regression calculations was limited.Oxygen fugacity-temperature diagrams were constructed from predicted thermodynamic properties to illustrate how thermodynamic data can be used to understand the transport and deposition of metals in hydrothermal systems such as the Carlin-type gold deposits. Assuming a linear relationship between temperature and pressure, metals are predicted to predominantly be transported as sulfide complexes at a total aqueous sulfur concentration of 0.05 m. Also, the presence of arsenic and antimony mineral phases in the deposits are shown to restrict mineralization within a limited range of chemical conditions. Finally, at a lesser aqueous sulfur concentration of 0.01 m, host rock sulfidation can explain the origin of arsenic and antimony minerals within the paragenetic sequence.2

show abstract

References

2010

Solvents and Solvent Effects in Organic Chemistry

View full text Add to dashboard Cite

Aqueous Nonelectrolyte Solutions. Part X. Mercury Solubility in Water

Cited by 59 publications

References 9 publications

In-depth review of atmospheric mercury: sources, transformations, and potential sinks

In-depth review of atmospheric mercury: sources, transformations, and potential sinks

The Hydrothermal Chemistry of Gold, Arsenic, Antimony, Mercury and Silver

References

Contact Info

Product

Resources

About