ArticleA thermodynamic investigation of barium and calcium sulfate stability in sediments at an oceanic ridge axis (Juan de Fuca, ODP legs 139 and 169)
Introduction
Anhydrite is commonly found in high temperature oceanic environments linked to hydrothermal activity at spreading centers (Chang et al., 1996). Its occurrence is reported in altered sediments and mineral deposits forming at ridge axis, such as the Juan de Fuca ridge (NE Pacific), which has been the target of two drilling legs (139 and 169) of the Ocean Drilling Program Davis et al 1992, Fouquet et al 1998). In the laboratory, anhydrite solubility in aqueous solutions is well documented by numerous measurements at various temperatures and pressures which showed that its solubility decreases when temperature increases. This body of experimental data has been summarized and critically evaluated in the recent development of solubility models based on Pitzer’s ion interaction formalism Harvie et al 1984, Greenberg and Moller 1989, Monnin 1990. Such models which are for now limited to temperatures of about 200°C and to pressures up to 1 kbar, allow the calculation of mineral solubilities in a large range of concentration and composition, including seawater-type solutions. Due to its retrograde solubility, anhydrite precipitates when seawater is heated. Using her model of the Na-Ca-Cl-SO4-H2O system as a thermodynamic model for standard seawater, Moller (1988) has calculated that standard seawater reaches equilibrium with anhydrite at 108°C at water vapor saturation pressure. On another hand, Bischoff and Seyfried (1978) experiments show that the seawater-anhydrite equilibrium temperature is 150°C at 500 bars.
When present in oceanic sediments, anhydrite is likely to dissolve when high temperature hydrothermal fluids cool down during mixing with low-temperature fluids linked to off-axis circulation (Sleep, 1991). Conversely, it may precipitate when seawater is heated in downwelling or recharge zones. Anhydrite precipitation may then clog the porosity and hence affect the flow geometry and the depth to which hydrothermal fluids may penetrate the crust, as extensively discussed by Sleep (1991). Anhydrite will also dissolve when sediment cores brought back to the surface cool down. This may then lead to high porewater calcium and sulfate concentrations that look anomalous when compared to those normally encountered in marine environments. This sampling artifact has been invoked to explain Ca and SO4 concentrations of porewaters from sediment cores recovered at ODP Sites 856 and 1035 drilled during ODP Legs 139 and 169 at the Dead Dog and Bent Hill areas of the Juan de Fuca Ridge Davis et al 1992, Fouquet et al 1998. In addition, high porewater calcium and sulfate concentrations at ODP Site 856 have been attributed to an in-situ natural cause, i.e., present day in-situ dissolution of anhydrite deposited when sediment temperatures were higher due to sill intrusions (Davis et al., 1992). In another environment, the stability of anhydrite in contact with the Red Sea brines has been investigated by Monnin and Ramboz (1996) and by Anschutz et al. (2000).
Another common sulfate found in the marine environment is barite (barium sulfate). Its occurrence is widespread in suspended matter in the water column of the oceans where its formation is linked to biologic activity Dehairs et al 1980, Hanor 2000. It accumulates on the seafloor as micrometer-scale crystals during sedimentation. In oceanic hydrothermal environments, barite is an important constituent of hydrothermal chimneys and mounds Chang et al 1996, Hanor 2000. Barium sulfate solubility has also been extensively investigated by laboratory experiments. In aqueous solutions containing less than 0.25M NaCl, barite solubility increases with temperature up to 150°C, then it decreases above this temperature. This solubility maximum is not observed for more concentrated solutions (Blount, 1977). Barite solubilities in various aqueous solutions have recently been used to construct a solubility model as a function of temperature, pressure and solution composition to 200°C and to 1 kbar (Monnin, 1999).
For a given temperature and pressure, the stability of solid sulfates in the marine environment will depend on the concentrations of sulfate and of the constituent cation in the porewaters. The sulfate concentration can decrease, either by bacterial sulfate reduction at low temperatures (below about 110°C) or by thermal sulfate reduction (above about 125°C). The decrease of the porewater sulfate content may induce redissolution of solid sulfates. This has been well documented for barite, leading to so-called barium remobilization (e.g., McManus et al 1994, Torres et al 1996; Monnin et al., 2000).
Up to now the stability of sulfate minerals in the marine environment has been inferred either from petrographic observations, or from changes in porewater compositions. In this paper, we use a recent model of alkaline earth sulfate solubilities in complex electrolyte solutions as a function of temperature, pressure and solution composition (Monnin, 1999) to investigate the stability of Ca, Sr and Ba sulfates in sediments collected at a sedimented ridge axis (Juan de Fuca Middle Valley, ODP Leg 139 and Gorda Ridge Escabana Trough, ODP Leg 169).
Section snippets
In situ borehole temperatures at Middle Valley and Escanaba Trough
Middle Valley and Escanaba Trough are two sections of the Pacific ridge situated respectively at the northernmost section of the Juan de Fuca ridge and at the southern end of the Gorda ridge (Fig. 1). Because of the proximity of the North American continental margin, Middle Valley and Escabana Trough have been rapidly filled over geologic times by terrigenous sediments consisting of turbidite units of variable thickness, irregularly interbedded with biogenic pelagic sediments. Active discharge
Calculation of the Ba, Sr and Ca sulfate saturation indices from the porewater compositions
A mineral saturation index is defined here as the ratio of Q, the ionic product of the considered mineral, to its solubility product Ksp:
The ionic product Q of a MSO4 mineral is defined as: where mM2+(aq),T and mSO42−(aq),T designate the total (measured) cation and sulfate molalities and γMSO4(aq),T the total (or stoichiometric) activity coefficient of the aqueous electrolyte.
Pitzer’s ion interaction formalism has allowed recent advances in
Application: barite and anhydrite stabilities in high temperature marine sediments
During ODP Leg 139 and 169, most porewaters have been retrieved by sediment squeezing following the usual ODP procedure. Porewater samples of indurated sediments obtained by the GRIND technique (Wheat et al., 1994) did not show any difference in composition with those obtained by squeezing. Major element concentrations are reported in the ODP Leg 139 (Davis et al., 1992) and Leg 169 Initial Report volumes (Fouquet et al., 1998), while Ba data for Leg 139 (Sites 855 to 858) are reported by Wheat
Discussion
One of the first questions to address in water–rock interaction modeling is to know whether calculated departures from equilibrium (indicated by saturation indices different from 1) are real phenomena associated to the dynamics of the system under study, or only model artifacts. This outlines the importance of model validation, a step in which data independent from those used in the model construction are used to test model predictions. Here we have supplemented this step by showing the good
Conclusions
- 1.
It is commonly accepted that standard seawater becomes saturated with respect to anhydrite at a temperature of 150°C, as shown experimentally by Bischoff and Seyfried (1978). Such an assumption overlooks the effect of pressure. The Bischoff and Seyfried (1978) experiments have been carried out for a pressure of 500 bars. We show that reducing the pressure from 500 bars to 20 bars lowers the equilibrium temperature of anhydrite in standard seawater from 147 to 117°C.
- 2.
We have calculated the barite
Acknowledgements
We acknowledge the support of S. Balleur by Schlumberger-Clamart. Many thanks are due to Geoff Wheat for his comments and for his interest at an early stage of this work, to Joris Gieskes and to the two anonymous reviewers for their suggestions leading to substantial improvements of the manuscript.
Associate editor: L. Walter
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