Persulfate activation by naturally occurring trace minerals
Highlights
► Persulfate decomposition and activation by 13 trace minerals was investigated. ► Pyrite and cobaltite addition resulted in rapid persulfate decomposition. ► Pyrite promoted rapid generation of sulfate radical and hydroxyl radical. ► Most trace minerals did not decompose or activate persulfate. ► Some trace minerals inhibited persulfate decomposition and activation.
Introduction
In situ chemical oxidation (ISCO) has become a dominant technology for the remediation of contaminated soils and groundwater. Of the three common ISCO processes, permanganate, catalyzed H2O2 propagations (CHP), and activated persulfate, activated persulfate is the least mature and least understood technology. Nonetheless, persulfate appears to have many advantages as an ISCO reagent. Although the persulfate anion (S2O82−) is a strong oxidant (E0 = +2.01 V), it is usually activated by heat, transition metals, or base to generate sulfate radical (SO4−), a stronger oxidant (E0 = +2.6 V) [1], [2]. Sulfate radical can then react with water to form another oxidant, hydroxyl radical (OH) [3].
Numerous investigators have focused on the activation of persulfate. Thermal activation of persulfate has been studied for treating methyl tert-butyl ether (MTBE) [4] and trichloroethylene (TCE) [5]. Persulfate activation by iron has been approached from several perspectives. Liang et al. [6] found that iron (II), but not iron (III), activates persulfate, and proposed using thiosulfate to regenerate iron (II) after it was oxidized by persulfate activation. Anipsitakis and Dionysiou [7] demonstrated that out of nine transition metals tested, only three activated persulfate to promote degradation of 2,4-dichlorophenol: silver (I), iron (II), and iron (III), with silver (I) providing the most activation and iron (III) the least. Killian et al. [8] and Rastogi et al. [9] subsequently demonstrated that iron chelates are more effective than iron (II) in activating persulfate. Furman et al. [10] recently elucidated the mechanism of base activation of persulfate, which involves the base-catalyzed hydrolysis of persulfate to hydroperoxide anion. The hydroperoxide anion then reduces another persulfate molecule, generating sulfate radical and sulfate anion. High ratios of base to persulfate are often required for effective persulfate activation [11].
Although a modicum of fundamental information is known about persulfate activation in relatively simple aqueous systems, its chemistry in the subsurface has received little attention. Subsurface chemistry has been shown to be a dominant factor in the effectiveness of other ISCO technologies [12]. For example, minerals decompose hydrogen peroxide leading to the formation of reactive oxygen species and resulting in rapid decomposition of hydrogen peroxide in the subsurface [13], [14]. Subsurface minerals decompose H2O2 effectively enough that the addition of soluble iron is usually not required for CHP ISCO [15].
In contrast to research on CHP, minimal attention has been given to the possible activation of persulfate by naturally occurring minerals found in surface and subsurface soils. Liang et al. [16] studied TCE destruction in columns packed with a sandy soil; however, the authors did not investigate the potential for the minerals in the soil to activate persulfate. Costanza et al. [17] studied perchloroethylene (PCE) destruction by thermally activated persulfate in batch reactors containing several solids and soils, but they did not investigate the effect of soil minerals on persulfate activation. Similarly, Johnson et al. [18] studied the effect of soil natural oxidant demand, but not soil minerals, on persulfate decomposition. Ahmad et al. [19] investigated the potential for major soil minerals (e.g., goethite, birnessite) found in surface and subsurface soils to activate persulfate. They found that most of the dominant soil minerals, such as goethite and ferrihydrite, did not activate persulfate. Birnessite activated persulfate, but only at concentrations significantly greater than typically found in soils. Many trace minerals are characterized by surface charge couples significantly different from the dominant iron and manganese oxides found in soils. However, the potential for trace minerals, such as ilmenite, cuprite, etc., to activate persulfate has not been investigated to date. The objective of this research was to investigate the potential for soil trace minerals to promote the decomposition of persulfate and activate it to generate reactive oxygen species.
Section snippets
Materials
The minerals anatase, bauxite, calcite, cobaltite, cuprite, hematite, ilmenite, magnesite, malachite, pyrite, pyrolusite, siderite, and willemite were purchased from D.J. Minerals (Butte, MT). They were received as cubes approximately 1 cm3 and were crushed to a fine powder using a 150 mL capacity Spex shatter box with hardened steel as a grinder. Mineral surface areas were determined by Brunauer–Emmett–Teller (BET) analysis under liquid nitrogen on a Coulter SA 3100 [20]. The surface areas of
Mineral-mediated decomposition of persulfate
The decomposition of persulfate in the presence of 13 trace minerals is shown in Fig. 1. The rates of mineral-mediated persulfate decomposition varied substantially; therefore, the minerals were classified into four distinct groups based on their potential to decompose persulfate. The minerals that promoted rapid persulfate decomposition were cobaltite and pyrite with >90% of the persulfate decomposed within 5 h and 30 h, respectively. The minerals classified as slowly decomposing persulfate were
Conclusions
Thirteen trace minerals were evaluated for their potential to promote the decomposition of persulfate and generate reactive oxygen species. Trace minerals were characterized by wide-ranging potential to promote persulfate decomposition. Seven of the minerals (anatase, bauxite, calcite, cuprite, magnesite, malachite, and willemite) mediated the decomposition of persulfate at rates slower than the persulfate–water control systems containing no minerals. Two minerals (pyrolusite and hematite)
Acknowledgement
Funding for this research was provided by the Strategic Environmental Research and Development Fund through grant no. ER-1489.
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