In situ determination of the apparent solubility product of amorphous iron sulphide

Bågander, Lars Erik; Carman, Rolf

doi:10.1016/0883-2927(94)90060-4

Cited by 17 publications

(9 citation statements)

References 41 publications

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“…An apparent solubility products of 2.6 for amorphous FeS in the Baltic Sea was determined in 15.8°C (Bagander and Carman, 1994). Recently, a solubility product constant of 3.00 Ϯ 0.12 was obtained at 20°C under various partial pressures of H 2 S (10 Ϫ1 , 10 Ϫ3 , 10 Ϫ4 , 10 Ϫ5 MPa) and pH values (3.0 -7.9) (Davison et al, 1999).…”

Section: Ion Activity Products Of Sulfide-detectable Groundwatersmentioning

confidence: 99%

Ion activity products of iron sulfides in groundwaters: Implications from the Choshui fan-delta, Western Taiwan

Chen

Liu

2005

Geochimica et Cosmochimica Acta

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Section: Ion Activity Products Of Sulfide-detectable Groundwatersmentioning

confidence: 99%

Ion activity products of iron sulfides in groundwaters: Implications from the Choshui fan-delta, Western Taiwan

Chen

Liu

2005

Geochimica et Cosmochimica Acta

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“…Toxicol. Chem 24,. 2005 R.F.Carbonaro et al Experimental and model-predicted vertical profiles of (A, D, G) acid-volatile sulfide (AVS); (B, E, H) simultaneously extracted metal (SEM); and (C, F, I) temporal profile of overlying water metal concentration for the metal-spiked sediment experiments.…”

mentioning

confidence: 99%

“…Chem. 24,2005 R.F. Carbonaro et al release of metal to the overlying water resulted from metalsulfide oxidation.…”

mentioning

confidence: 99%

Experimental and modeling investigation of metal release from metal‐spiked sediments

Carbonaro

Mahony

Walter

et al. 2005

Enviro Toxic and Chemistry

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In sediments that contain iron monosulfide, cadmium, nickel, lead, zinc, and silver(I) form insoluble metal sulfides that lower the metal ion activity in the sediment-pore water system, thereby reducing toxicity. However, metal sulfides are susceptible to oxidation by molecular oxygen resulting in metal solubilization. To better understand the sources and sinks of metal sulfides in sediments, iron monsulfide-rich freshwater sediments were spiked with cadmium, nickel, lead, zinc, or silver(I) and placed into cylindrical cores with an overlying layer of oxygen-saturated water. Measurements of the dissolved metal concentration in the overlying water were made as a function of time and the vertical profiles of acid-volatile sulfide (AVS) and simultaneously extracted metal (SEM) were measured after 150 d. A one-dimensional reactive and transport model has been employed to help elucidate processes controlling the fate of metals in sediments. The model incorporates metal-sulfide formation, metal-sulfide oxidation, and metal partitioning onto sediment organic carbon and iron oxyhydroxide to simulate the vertical transport of metals throughout the sediment core.

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“…FeS readily precipitates, and hence plays a role in controlling the concentrations of aqueous ferrous and sulfide concentrations [27,28]. The equilibrium simulations in Visual MINTEQ indicate that there might have been free sulfide at low pH, as the removal of sulfide was not complete even though ferrous iron was in excess (Figure 3).…”

Section: Precipitation Stoichiometry Versus Ph In Buffered Watermentioning

confidence: 99%

Sulfide Precipitation in Wastewater at Short Timescales

Kiilerich

Ven

Nielsen

et al. 2017

Water

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Abatement of sulfides in sewer systems using iron salts is a widely used strategy. When dosing at the end of a pumping main, the reaction kinetics of sulfide precipitation becomes important. Traditionally the reaction has been assumed to be rapid or even instantaneous. This work shows that this is not the case for sulfide precipitation by ferric iron. Instead, the reaction time was found to be on a timescale where it must be considered when performing end-of-pipe treatment. For real wastewaters at pH 7, a stoichiometric ratio around 14 mol Fe(II) (mol S(−II)) −1 was obtained after 1.5 s, while the ratio dropped to about 5 mol Fe(II) (mol S(−II)) −1 after 30 s. Equilibrium calculations yielded a theoretic ratio of 2 mol Fe(II) (mol S(−II)) −1 , indicating that the process had not equilibrated within the span of the experiment. Correspondingly, the highest sulfide conversion only reached 60%. These findings differed significantly from what has been demonstrated in previous studies and what is attained from theoretical equilibrium conditions.

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In situ determination of the apparent solubility product of amorphous iron sulphide

Cited by 17 publications

References 41 publications

Ion activity products of iron sulfides in groundwaters: Implications from the Choshui fan-delta, Western Taiwan

Ion activity products of iron sulfides in groundwaters: Implications from the Choshui fan-delta, Western Taiwan

Experimental and modeling investigation of metal release from metal‐spiked sediments

Sulfide Precipitation in Wastewater at Short Timescales

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