Systematic investigations on iron cycling in phosphorus/siderophore systems: Synergism or antagonism?
Introduction
In natural systems, iron (Fe) is an essential nutrient to organisms (Hersman et al., 2000). Despite of their high abundances in Earth's crust, soils, sediments, and aquatic systems (Colombo et al., 2014), Fe (hydr)oxides are relatively insoluble (Sullivan et al., 1988) and bioavailable Fe pools derived from Fe (hydr)oxides are commonly far below the needs of plants, fungi, and microorganisms (e.g., Kraemer, 2004; Dehner et al., 2010), resulting in ecological Fe deficiency. In the context of natural Fe acquisition pathway, biogeochemical weathering has been defined as the dissolution of rocks and minerals by physicochemical processes of microorganisms, plants and deuterogenic biogenic ligands (Shi et al., 2011). Widespread siderophores, as pervasive biogenic chelating agents, are the fundamental biogeochemical weathering strategy developed by the (micro)-biological communities in order to overcome the low abundance of bioavailable Fe in local environments (soils and waters) (Duckworth et al., 2009; Hibbing et al., 2010; Kim et al., 2010). Siderphores form the most thermodynamically stable complexes because of the high affinity to develop 1:1 hexadentate complexes to Fe(III) (stability constants of 1030-1050 (Ahmad and Maathuis, 2014) by hard Lewis base hydroxamate functional groups (Schenkeveld et al., 2016).
Recent research have advocated that siderophores usually work in conjunction with other organic exudates that coexisted in close associations, and potentially act synergistically in biogeochemical weathering systems (Cordero et al., 2012). Enhancement of synergism on Fe (hydr)oxides dissolution between two distinct organic ligands have been addressed by previous studies (e.g., Stewart et al., 2013; 2016; Wang et al., 2015). There are two prevailing mechanisms responsible for the synergistic effects: 1) Cyclic Fe detachment and Fe(III) shuttling (Akafia et al., 2014; Ito et al., 2011; Wang et al., 2015); 2) Cyclic Fe(III)→Fe(II) detachment, re-oxidation and Fe(III) shuttling (Stewart et al., 2013, 2016; Schenkeveld et al., 2016). Although the effects of fluvic acids and the low-molecule-weight acids such as oxalate and citrate on siderophores-mediated Fe mineral dissolution have been examined (Saad et al., 2017), the role of some bio-essential substances (e.g., phosphorus, sulphur) remained unknown, regardless of their ubiquity on Earth’ surfaces.
Soil Fe (hydr)oxides are the major phosphorus (P) adsorbents, particularly in sandy soils, due to a high affinity of P to the active surface of Fe (hydr)oxides (e.g., Borggaard et al., 1990; Kim et al., 2011). The interaction between the P species and Fe (hydr)oxide surface typically results in interfacial complexation (monodentate to bidentate forms), precipitation, and dissolution, which are significant environmental physicochemical processes affecting the eco-environment (Ruttenberg and Sulak, 2011; Li et al., 2013; Feng et al., 2016). Due to its higher surface site density, reactivity and surface/bulk ratio (Hiemstra, 2013), poorly-ordered ferrihydrite (Fh) is often considered as the main source of bioavailable Fe (Kuhn et al., 2014), and the ultimate sink of P in subsurface environments (Khare et al., 2007; Michel et al., 2007). Phosphorus forms a passive interfacial layer that commonly stabilizes Fh (L. Wang et al., 2017a), decreasing Fe bioavailability and limits Fe bio-cycling (Fonseca et al., 2011). Besides, the mineral negative electrical field induced by phosphorus binding could attract positively charged siderophore molecules. Elevated surface negative charge density increases the electrostatic repulsive pressure between adjacent particles in aggregates, likely providing a basis for Fh dissolution. Interestingly, the possible reductive dissolution induced by redox-active ligands (e.g., hydroxamate groups of siderophores; Akafia et al., 2014) is not shielded by surface P complexes (Latta et al., 2012; Luo et al., 2017). Moreover, siderophores behave as other organic acids that can affect the manner in which P was complexed, i.e., breaking passive P-hosting layers, inducing dissolution (Johnson and Loeppert, 2006). The following hypotheses has been addressed: coupling mechanisms may be analogous to reported synergisms, but the comprehensive effect of siderophores and phosphorus on Fh dissolution should be much complicated.
While the syngistisms of siderophores and a wide variety of natural organic acids (e.g., oxalic, citric, fulvic, and humic acids) have been extensively investigated (e.g., Stewart et al., 2013; 2016; Wang et al., 2015), its possible connection with P towards Fh dissolution is still unknown. Hence, the objectives of this study are to determine the reaction kinetics and mechanisms of P and siderophores on Fh dissolution and differentiate from typical syngistisms between organic acids and siderophores. We used the following approaches: 1) we used a fungal siderophore desferrioxamine B (DFOB) to represent a common class of siderophores; 2) both inorganic P (Pi, the most common inorganic phosphate) and organic P (IHP, the most abundant organic phosphate in soils; Turner et al., 2002) were studied; 3) we studied the process, mechanism and kinetics of Fh dissolution in the water (P/DFOB-free)/single (DFOB/P-only)/binary (P + DFOB) systems; 4) we systematically investigated the P binding patterns on Fh surfaces in the single and binary systems via microscopic techniques (FESEM and HRTEM), and spectroscopy techniques (i.e., XRD, ATR-FTIR, μ-Raman); 5) we investigated Fh dissolution as the function of pH, addition sequence, initial P/DFOB concentrations, and experimental duration. Our results provide critical insights in Fe cycling in P-enriched settings during biogeochemical weathering.
Section snippets
Reagents
All chemicals used in this study are reagent-grade or better. Deionized water (18.2 MΩ) was used throughout the experiments and acquired with a Milli-Q element system (Direct-Q® 3UV). Iron (III) chloride hexahydrate salt (purity >99%) was purchased from ACROS ORGANICS™. Sodium phosphate dibasic anhydrous (purity >99.9%) was obtained from Fisher Scientific™. Dipotassium myo-inositol hexaphosphate (K2H16(CPO4)6, IHP, purity >95%) and desferrioxamine B mesylate salt (C25H48N6O8·CH4O3S, DFOB,
Ligand-mediated solid dissolution
Aqueous characterization of dissolution is shown in Fig. 1, Fig. 2, and summarized in Table S1. The Fe dissolution process is generally described by an initial, rapid (often assumed instantaneous) reaction followed by slower kinetic reactions. In the control (P/DFOB-free) (Fig. 1a) and the DFOB-only (Fig. 1b) systems, the dissolution approximates a typical linear regression following zero-order kinetics far from equilibrium (Lasaga, 2014; Murray and Hesterberg, 2006). Dissolved Fe
Phosphorus surface complexation mechanisms
In classical theory, the chemisorption of P is responsible for the changes in the electric field from ligand-exchange with surface aquo and hydroxo groups (Goldberg and Sposito, 1984). Using infrared spectra and density functional theory (DFT) approached, previous studies suggested that different surface complexes of P can coexist, and the speciation is highly depending on [P], pH, the concentration and reactivity of surface sites (Li et al., 2013). Metal (hydr)oxides, commonly in the form of
Conclusions
This paper attempts to advance the understanding of the presence of phosphorus and siderophores on Fe (hydr)oxide dissolution and to determine the effects of pH, initial P concentration, and the addition sequence in the P and/or DFOB systems. We conclude that organisms are able to create chemically distinct microenvironments (synergism and antagonism), filling a significant knowledge gap in the literature. Moreover, we provide new insights into understanding the biogeochemical cycling of Fe.
Declaration of competing interest
The authors declare that they have no known competing financial interests or personal relationships that could have appeared to influence the work reported in this paper.
Acknowledgment
The authors thank the anonymous reviewers and the editor for their valuable comments and suggestions to improve the quality of this paper. This research is supported by the Army Research Office under grant W911NF-17-2-0028. We acknowledge the support of ATR-FTIR and Renishaw inVia Raman microscope spectroscopy in the UNC EFRC Instrumentation Facility established by the UNC EFRC: Center for Solar Fuels, an Energy Frontier Research Center funded by the U.S. Department of Energy, Office of
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