Fe(III) mineral reduction followed by partial dissolution and reactive oxygen species generation during 2,4,6-trinitrotoluene transformation by the aerobic yeast Yarrowia lipolytica
© Ziganshin et al.; licensee Springer. 2015
Received: 23 December 2014
Accepted: 29 December 2014
Published: 1 February 2015
Understanding the factors that influence pollutant transformation in the presence of ferric (oxyhydr)oxides is crucial to the efficient application of different remediation strategies. In this study we determined the effect of goethite, hematite, magnetite and ferrihydrite on the transformation of 2,4,6-trinitrotoluene (TNT) by Yarrowia lipolytica AN-L15. The presence of ferric (oxyhydr)oxides led to a small decrease in the rate of TNT removal. In all cases, a significant release of NO2 − from TNT and further NO2 − oxidation to NO3 − was observed. A fraction of the released NO2 − was abiotically decomposed to NO and NO2, and then NO was likely oxidized abiotically to NO2 by O2. ESR analysis revealed the generation of superoxide in the culture medium; its further protonation at low pH resulted in the formation of hydroperoxyl radical. Presumably, a fraction of NO released during TNT degradation reacted with superoxide and formed peroxynitrite, which was further rearranged to NO3 − at the acidic pH values observed in this study. A transformation and reduction of ferric (oxyhydr)oxides followed by partial dissolution (in the range of 7–86% of the initial Fe(III)) were observed in the presence of cells and TNT. Mössbauer spectroscopy showed some minor changes for goethite, magnetite and ferrihydrite samples during their incubation with Y. lipolytica and TNT. This study shows that i) reactive oxygen and nitrogen species generated during TNT transformation by Y. lipolytica participate in the abiotic conversion of TNT and ii) the presence of iron(III) minerals leads to a minor decrease in TNT transformation.
Keywords2,4,6-Trinitrotoluene Biodegradation Ferric (oxyhydr)oxides Yarrowia lipolytica Reactive oxygen species Reactive nitrogen species
Nitroaromatic compounds have multiple applications in the chemical industry, amongst which special attention should be paid to 2,4,6-trinitrotoluene (TNT) due to its extensive use throughout the world (Harter 1985). A significant number of land and water territories are contaminated with this explosive and its conversion products as a result of the manufacture, transportation, storage and testing of munitions. These compounds are classified as relatively recalcitrant to biological degradation and their fate is affected by biogeochemical processes (Smets et al. 2007; Singh et al. 2012; Ziganshin and Gerlach 2014; Chien et al. 2014).
On the one hand, bioremediation strategies could offer attractive solutions for soil and water decontamination, although, TNT is exceedingly recalcitrant to complete biological mineralization. On the other hand, TNT nitro groups can be fairly easily reduced to hydroxylamino and amino derivatives by bacteria and fungi. However, these metabolites are also known to be toxic, potentially mutagenic and persistent contaminants (Smets et al. 2007; Singh et al. 2012; Khan et al. 2013). The most promising and efficient pathway of nitrogen release from TNT is the transformation of parent compound through the addition of hydride ions resulting in the formation of Meisenheimer hydride complexes followed by their subsequent destruction (ring fission) (Pak et al. 2000; Jain et al. 2004; Wittich et al. 2009; Ziganshin et al. 2010a). Therefore, the application of microorganisms, which are able to degrade TNT and its metabolites, can be useful for bioremediation of TNT-contaminated soil and water.
Iron is one of the most abundant elements in the biosphere, naturally occurring in the form of various Fe(II)- and Fe(III)-bearing minerals and present at many TNT-contaminated field sites. The biogeochemical cycling of iron also has an influence on nitroaromatic compounds, including TNT, mostly through the stimulation of nitro group reduction process in different soils, sediments and waters. In almost all cases TNT transformation in the presence of iron species is accompanied by the enhanced formation and accumulation of undesirable metabolites, such as hydroxylamino-dinitrotoluenes (HADNTs), amino-dinitrotoluenes (ADNTs) and/or diamino-nitrotoluenes (DANTs) (Hofstetter et al. 1999; Borch et al. 2005; Oh et al. 2008; Boparai et al. 2010), which are fairly persistent and approximately as toxic as TNT itself (Smets et al. 2007; Khan et al. 2013). Only a few studies have reported denitration of TNT in the presence of ferrihydrite (Eyers et al. 2008; Khilyas et al. 2013). In terms of the efficiency of remediation strategies, TNT denitration processes resulting in nitro group elimination would be advantageous if the nitro group reduction pathways could be minimized. Therefore, for the development of effective TNT-bioremediation technologies in the presence of iron-containing minerals and because of the distinct solubilities and reactivities of various Fe(III) minerals (Borch et al. 2010; Posth et al. 2014), it is important to investigate TNT transformation processes in the presence of different ferric (oxyhydr)oxides. In addition, very little is known about the reduction of Fe(III) minerals by strictly aerobic bacteria and yeasts in the presence of polynitroaromatic compounds.
Systematic data showing the transformation of TNT by distinct microorganisms in the presence of iron (oxyhydr)oxides under oxic conditions is lacking, despite the fact that oxygen can have a significant effect on Fe-transformation processes (Morgan and Lahav 2007). Only a few studies have so far demonstrated the generation of the superoxide radical anion (O2 ·–) during TNT reduction by purified enzymes (Kumagai et al. 2000; Kumagai et al. 2004) and in the presence of bacterial cells (Naumenko et al. 2008) via the formation of TNT nitroanion radicals. In some studies the involvement of abiotically and biologically produced O2 ·– in the denitration of TNT and its metabolites was also reported (Fritsche et al. 2000; Van Aken and Agathos 2002; Stenuit et al. 2012). However, little is known regarding the biological production of O2 ·– and other reactive oxygen species in culture medium during the microbial transformation of polynitroaromatic xenobiotics.
Given the importance of iron minerals for the fate of TNT, the main goal of this study was to investigate the effect of different ferric (oxyhydr)oxides on the TNT transformation processes by the yeast strain Yarrowia lipolytica AN-L15 and to identify iron mineral transformation in the presence of yeast cells and mineral additions of goethite (α-FeOOH), hematite (α-Fe2O3), magnetite (Fe3O4) or ferrihydrite (5Fe2O3 ●9H2O). Finally, reactive oxygen and nitrogen species generated over the course of TNT transformation were characterized.
Materials and methods
Yeast growth media and growth conditions
The yeast strain Yarrowia lipolytica AN-L15 deposited in the Russian National Collection of Industrial Microorganisms under a collection number of VKPM Y-3492 was cultivated aerobically at 30°C for 24 hours in Petri dishes with Sabouraud agar medium containing (per liter) 10 g of glucose, 10 g of peptone, 5 g of yeast extract, 0.25 g of NaCl and 20 g of agar (Ziganshin et al. 2007a). Yeast cells were harvested, washed twice with 16 mM phosphate buffer (pH 6.0) and added into 250 mL Erlenmeyer flasks containing 50 mL of a synthetic medium of the following content (mM): glucose, 28; (NH4)2SO4, 7.6; MgSO4, 2; Na2HPO4, 1.94; KH2PO4, 14.06 (pH 6.0). In ferric (oxyhydr)oxide containing treatments, goethite, hematite, magnetite or ferrihydrite were added to the synthetic medium to a final concentration of 0.15 g L−1 or 0.3 g L−1 (measured as Fe). As ferric (oxyhydr)oxides, commercially available goethite, hematite and magnetite were used (Lanxess). In the case of ferrihydrite-containing experiments, 2-line ferrihydrite was synthesized by dissolving of 4.0 g of Fe(NO3)3 ●9H2O in 50 mL of Millipore water following Amstaetter et al. (2012). 1 M KOH was then added dropwise over 3 min until a pH of 7.3 was reached. After 2 h, the pH was adjusted to a final value of 7.5. After centrifugation at 5,000 × g for 10 min and washing of the solid phase with Millipore water, 2-line ferrihydrite was obtained and used for the experiments. Cell growth was monitored photometrically by measuring the optical density at 600 nm (OD600) using a SPECOL 1300 spectrophotometer (Analytik Jena, Germany) with cell-free supernatant as a reference; the initial OD600 was adjusted to 0.05. TNT was added to a final concentration of 0.44 mM from an ethanolic stock solution (0.8 ml of 96% ethanol into 50 ml of medium), and the culture was incubated in the absence of light at 30°C on a rotary shaker at 150 rpm. Experiments conducted in the absence of TNT contained the same amount of 96% ethanol. All experiments were set up in triplicate.
TNT and biotransformation products were detected and quantified with a Shimadzu high-performance liquid chromatograph equipped with an autoinjector, a diode array detector, a column oven, a Supelcosil LC-8 guard column and a Supelcosil octyl (C-8) column (150 by 4.6 mm; particle size, 5 μm) as described previously (Ziganshin et al. 2007b; Ziganshin et al. 2010b).
The nitrite and nitrate ions in the culture fluid were determined by using an AA3 SEAL Analyzer equipped with a XY2 Sampler (SEAL Analytical, Germany).
Dissolved Fe(II) concentrations were quantified after sample centrifugation at 15,000 × g for 10 min and subsequent filtration through 0.2 μm filters (Spartan 13/0.2 RC; Whatman). Filtered sample (100 μL) was added to 900 μL of 1 M HCl. The received solution (20 μL) was added to 80 μL of 1 M HCl and to 100 μL of 0.1% ferrozine solution in 96-well microtiter plates and incubated for 5 min at room temperature. The resulting absorbance (562 nm) in the plates was measured using a Flashscan 550 plate reader (Analytik Jena, Germany) (Stookey 1970).
For 57Fe Mössbauer spectroscopy, biologically produced mineral precipitates were centrifuged at 10,000 × g for 10 min and then dried in an anoxic glovebox (100% N2). Samples were prepared by loading dried powders into Plexiglas holders (area 1 cm2). In order to ensure a homogeneous sample with ideal thickness, each sample was mixed and ground using a pestle and mortar with 80 mg glucose monohydrate. The samples were transferred to the Mössbauer spectrograph and inserted into a closed-cycle exchange gas cryostat (Janis cryogenics). Spectra were collected at 295 K, 77 K and 5 K by using a constant acceleration drive system (WissEL) in transmission mode with a 57Co/Rh source and calibrated against a 7 μm thick α-57Fe foil measured at room temperature. Spectra were analyzed using Recoil (University of Ottawa) using the Voigt Based Fitting (VBF) routine. The HWHM was fixed to 0.122 mm/s, as determined from the minimum line width of the calibration foil, measured at 295 K.
Superoxide anion radical (O2 ·–) generation during TNT transformation was determined by electron spin resonance (ESR) spectroscopy through the formation of 5-(Diethoxyphosphoryl)-5-methyl-1-pyrroline-N-oxide (DEPMPO) spin adducts (Frejaville et al. 1995). Firstly DEPMPO (50 mM) was added to a solution to be analyzed and after 30 sec incubation process at room temperature the mixture was transferred to glass tubes with an inner diameter of 1 mm (Sigma-Aldrich, Germany). ESR spectra were then recorded at room temperature with an ESP 300 Electron Spin Resonance spectrometer (Bruker, Germany) and a super-high Q microwave cavity. The experimental parameters were as follows: microwave power 2 mW, microwave frequency 9.73 GHz, modulation amplitude 0.2 mT, time constant 82 ms and scan rate 2.1 G/s. The received ESR spectra were analyzed using EasySpin toolbox for MATLAB. TNT-free or cell-free experiments were used as a control. The xanthine-xanthine oxidase reaction was used as the standard system for O2 ·– generation; superoxide dismutase was used to remove superoxide anions in the samples (Stenuit et al. 2012).
2,4,6-Trinitrotoluene and 2,4-dinitrotoluene (2,4-DNT) are the chemicals of ChemService (West Chester, USA); 2-amino-4,6-dinitrotoluene (2-ADNT) and 4-amino-2,6-dinitrotoluene (4-ADNT) were received from Supelco (Bellefonte, USA); 2-hydroxylamino-4,6-dinitrotoluene (2-HADNT) and 4-hydroxylamino-2,6-dinitrotoluene (4-HADNT) as well as some other potential metabolites of TNT nitro group reduction pathway were purchased from AccuStandard (New Haven, USA). DEPMPO as a spin trapping reagent for reactive oxygen species was received from Enzo Life Sciences (Farmingdale, USA). Hypoxanthine, xanthine oxidase, superoxide dismutase as well as all other chemicals and reagents were purchased from Sigma-Aldrich (Germany).
Influence of ferric (oxyhydr)oxides on TNT biotransformation processes
During the conversion of TNT by yeast cells of Y. lipolytica AN-L15, different metabolites successively appeared in the culture medium. Among the aromatic ring hydrogenation products, eight hydride-Meisenheimer complexes of TNT were detected, which were previously described in detail (Ziganshin et al. 2007b; Ziganshin et al. 2010b). Independent of the presence of ferric (oxyhydr)oxides, the main intermediate metabolite detected during the first day of incubation was a monohydride-Meisenheimer complex of TNT (3-H−-TNT). The maximum concentration of 3-H−-TNT detected after 1 day ranged from 255–294 μM (data not shown); its concentration was estimated as described previously (Ziganshin et al. 2007b). Its subsequent biotransformation into 2,4-DNT and other dihydride-Meisenheimer complexes of TNT (3,5-2H−-TNT and 3 isomers of 3,5-2H−-TNT · H+) as well as degradation of TNT-dihydride complexes over the next 3–4 days occurred with the liberation of nitrite into the medium in the absence as well as in the presence of the different ferric (oxyhydr)oxides (Figure 1B). As can be seen in Figures 1A and 1B, the maximum amount of nitrite detected during TNT removal was in the range of 45–61 μM. In the presence of ferrihydrite, TNT transformation was slightly less significant combined with delayed nitrite ion liberation, which might be due to the increase in buffer capacity of the medium in the presence of ferrihydrite as asserted by Khilyas et al. (2013). After 1 day, nitrate was also detected indicating nitrite oxidation to nitrate (Figure 1C). The highest concentration of nitrate was observed in iron mineral-free systems (145 ± 7 μM), whereas the lowest nitrate accumulation was found in the culture medium containing magnetite (126 ± 7 μM) and hematite (129 ± 5 μM). Interestingly, 2,4-DNT as a product of TNT degradation was found at high levels only in iron mineral-free treatments (72 ± 7 μM), while the addition of ferric (oxyhydr)oxides resulted in lower concentrations of this metabolite (15–46 μM; SI, Additional file 1: Table S1). TNT nitro group reduction metabolites, such as HADNTs and ADNTs, were also detected and their concentrations are summarized in Additional file 1: Table S1 (SI). Additional abiotic experiments conducted in the presence of iron minerals at pH 6.0 or 7.0 showed that nitrite, nitrate as well as TNT were relatively stable and did not undergo any transformation reactions in the absence of yeast cells (data not shown). Also, we were unable to detect other potential conversion products of TNT such as diarylamines, tetranitro-azoxytoluenes, tetranitro-azotoluenes, amino-dimethyl-tetranitrobiphenyls or Bamberger rearrangement products during aerobic growth of Y. lipolytica AN-L15 in the presence of Fe(III) minerals.
Superoxide generation during TNT biotransformation
Reduction of ferric (oxyhydr)oxides during incubation with Y. lipolytica in the presence of TNT
In contrast, significantly lower amounts of ferrous iron production were observed in TNT-free setups and in the presence of Y. lipolytica AN-L15 when compared to TNT-containing treatments. The maximum concentrations of dissolved Fe(II) in the absence of TNT after 6 days of incubation with strain AN-L15 were 0.62 mM, 0.26 mM, 0.2 mM and 0.2 mM (approximately 12, 5, 4 and 4% of the added ferrihydrite, magnetite, hematite and goethite, respectively; Figure 3). When lower concentrations of ferric (oxyhydr)oxides (0.15 g L−1 Fe) were tested, lower amounts of Fe(II) were detected (SI, Additional file 1: Figure S1); however, the trends remained the same. In control experiments, using cell-free medium, no Fe(II) accumulation was observed regardless of the presence of TNT (data not shown).
Transformation of ferric (oxyhydr)oxides during incubation with Y. lipolytica in the absence/presence of TNT
Goethite is usually expected to have a narrow hyperfine field at room temperature (38.0 T) and a small center shift (0.37 mm/s). The spectra obtained for both goethite samples have a narrower hyperfine field than expected (33.1–33.9 T); however, they also both exhibit superparamagnetic relaxation. This occurs close to the blocking temperature of a material and is likely the result of small average crystallite size or poor crystallinity of the sample. The paramagnetic background decreases in area relative to the sextet corresponding to the goethite from 39.5% to 24.8% for goethite and goethite + TNT, respectively (Figure 4). A small increase in center shift (CS) from 0.37 mm/s (goethite) to 0.43 mm/s (goethite + TNT) was also observed.
Both hematite samples (+/− TNT) possess a single sextet with very wide magnetic splitting (51.4 T) and low center shift (0.37–0.38 mm/s) that is characteristic of natural and synthetic hematite (Cornell and Schwertmann 2003). Its incubation in the presence of Y. lipolytica cells alone and with yeast cells and TNT did not yield any additional mineral phases or differences from the parent mineral (Figure 4).
Magnetite samples exhibit two overlapping sextets which are characteristic of the iron mineral. One sextet corresponds to Fe3+ in tetrahedral coordination, denoted the A-site, or TetFe3+. The second sextet is observed above the Verwey temperature of magnetite (~120 K) and is formed due to electron hopping within the octahedral lattice and corresponds to both Fe2+ and Fe3+. This second sextet is commonly denoted the B site, or OctFe2.5+. The results obtained here indicate that the spectrum of a magnetite + cells + TNT sample can only be fully fitted with an additional doublet which contributes to 1.3% of the total area (Figure 4). This doublet has a very low CS of 0.28 mm/s and low quadrupole splitting (ΔEQ) of 0.35 mm/s, which is consistent with a poorly crystalline Fe(III) mineral phase; however, it is not clear what the mineral identity is.
Finally, Mössbauer spectra were collected for ferrihydrite samples at three different temperatures, 295 K, 77 K and 5 K (Figure 5). Both spectra collected at 295 K have the same center shift (0.38 mm/s) and very similar ΔEQ (0.68 and 0.70 mm/s for samples of ferrihydrite incubated with Y. lipolytica AN-L15 and with Y. lipolytica AN-L15 and TNT, accordingly). These parameters are characteristic for ferrihydrite at room temperature (Cornell and Schwertmann 2003; Mikutta et al. 2008). Spectra obtained at 77 K maintain the paramagnetic doublet observed at room temperature, albeit with an increase in CS to 0.49 mm/s for both samples (Figure 5). Additional analyses were carried out at 5 K, with both samples requiring the fitting of two magnetically ordered (S1 and S2) and one poorly ordered (S3) sextets (Figure 5, Additional file 1: Table S2). The hyperfine fields of the ordered sextets are at close to the expected values of ferrihydrite (Eusterhues et al. 2008), although it is clear that neither sample is fully magnetically ordered, as seen by the requirement of a poorly ordered sextet. The total contribution of this background phase decreases from 55.0% (ferrihydrite + cells) to 49.9% (ferrihydrite + cells + TNT). Pure 2-line or 6-line ferrihydrite is usually expected to be fully magnetically split at 5 K and does not require this background feature to fit the data. This suggests that both samples have a very low blocking temperature, which is potentially much lower than the value expected for typical ferrihydrite (Murad 1996).
In this study we investigated the impact of various ferric (oxyhydr)oxides on TNT transformation by Y. lipolytica AN-L15. The fastest rate of TNT removal was seen in the absence of iron minerals followed by experiments in the presence of goethite. The presence of ferrihydrite, magnetite and hematite led to a small decrease in the rate of TNT transformation. However, significant TNT denitration by Y. lipolytica occurred in the absence and presence of ferric (oxyhydr)oxides, indicating the possibility of TNT aromatic ring cleavage independent of the presence of iron minerals. The significant liberation of NO2 − from TNT and further NO2 − oxidation to NO3 − was observed with yeast cells of Y. lipolytica. Also, the presence of ferric (oxyhydr)oxides did not stimulate the nitro group reduction. It has previously been suggested that the increase of nitro group reduction metabolites during TNT bioconversion is possible in the presence of iron minerals without any denitration processes (Hofstetter et al. 1999; Borch et al. 2005). However, our results indicate that TNT denitration by aerobically grown Y. lipolytica AN-L15 can take place in iron rich environments, and that the presence of ferric (oxyhydr)oxides does not lead to an increase of HADNT production. Given that Fe(II)- and Fe(III)-containing minerals are found at many TNT-contaminated field sites, these results are of significance for TNT bioremediation in such environments.
ESR spectra of DEPMPO radical adducts obtained during TNT biotransformation clearly demonstrated the generation of O2 ·–/HO2 · radical species in the culture medium. Presumably, the generation of reactive oxygen species here is the result of the interaction of Y. lipolytica AN-L15 cells with TNT and its transformation products, resulting in TNT-induced oxidative stress. It is known that TNT can produce superoxide radical anions through TNT nitroanion radical formation (Kumagai et al. 2000; Kumagai et al. 2004; Naumenko et al. 2008). Recently, an involvement of abiotically produced superoxide radical anions in the TNT denitration process with the accumulation of nitrite ions in the reaction mixture was reported (Stenuit et al. 2012). The authors suggested that denitration occurred through a nucleophilic attack on the parent trinitroaromatic compound; however, the exact mechanism is yet unknown. The generation of superoxide anions in our treatments also indicates their possible participation in the TNT denitration process. However, the main pathway of nitrite/nitrate liberation from TNT by Y. lipolytica AN-L15 occurred via biodegradation of TNT-hydride complexes resulting in the formation of 2,4-DNT and other unidentified, carbon-containing metabolites.
In recent work we detected nitric oxide (NO) as a metabolite of TNT biodegradation by Y. lipolytica AN-L15 (Khilyas et al. 2013). A potential pathway for its formation is the abiotic conversion of nitrous acid (formed through nitrite release during Meisenheimer hydride complexes destruction) to NO and nitric acid (nitrate) via a disproportionation reaction at low pH (Van Cleemput and Baert 1984). It is also likely that a fraction of the released NO2 − was decomposed to NO and nitrogen dioxide (NO2) and the produced NO could have been oxidized to NO2 in the presence of molecular oxygen (O2) as ascertained by Klueglein and Kappler (2013). In addition, the produced NO2 may potentially be scavenged by natural organic matter (NOM) through nitration reactions. Another fraction of the released NO2 − could have reacted with amino group-containing cell components in the low pH systems with the formation of nitrosoamines (Fischer and Warneck 1996). All of these reactions might have lead to the decrease of the total amount of NO2 −/NO3 − detected in our experimental systems.
Furthermore, NO released during TNT biodegradation by Y. lipolytica AN-L15 might have reacted with O2 ·– to form peroxynitrite (ONOO−) which is a stronger oxidant than both NO and O2 ·– (Pfeiffer et al. 1997; Vásquez-Vivar et al. 1997). Kumagai et al. (2004) demonstrated the production of NO and O2 ·– in the presence of TNT catalyzed by nitric oxide synthase and also proposed a mechanism of peroxynitrite formation. Peroxynitrite is not stable under acidic conditions resulting in rearrangement to nitrate (Pryor and Squadrito 1995; Pfeiffer et al. 1997). Thus, together with the biological and abiotic oxidation of released NO2 − into NO3 −, NO3 − accumulation during TNT biodegradation by Y. lipolytica AN-L15 at low pH could also occur through rearrangement of ONOO−. Some other oxidative reactions are also possible as ONOO− reacts rapidly with CO2, producing highly oxidizing species such as NO2 and CO3 ·– (Denicola et al. 1996). Since Y. lipolytica AN-L15 is able to synthesize and excrete different organic acids, mostly pyruvate and citrate, into the growth medium (Ziganshin et al. 2010b), these metabolites would probably provide the cells with some protection against oxidative damage. Pyruvic acid, like other α-keto acids, acts as a hydrogen peroxide (H2O2) scavenger and is able to react with peroxynitrite and peroxynitrous acid via pyruvate decarboxylation to acetate (Vásquez-Vivar et al. 1997). Furthermore, some protective properties of citric acid against superoxide anions (Van den Berg et al. 2003) and peroxynitrite (Han et al. 2005) are also known.
The results of our experiments also indicate a greater likelihood of ferrihydrite and magnetite to be reduced to ferrous iron in the presence of aerobic yeast cells and TNT than hematite or goethite.
Possible mechanisms for the reduction of the ferric (oxyhydr)oxides here could be the induction of yeast enzymes with Fe(III) reducing capacity by TNT or its transformation products as well as the participation of TNT degradation products and/or some unidentified extracellular metabolites in the abiotic reduction of Fe(III). Kerem et al. (1999) demonstrated that the brown rot fungus Gloeophyllum trabeum was able to degrade another recalcitrant compound, polyethylene glycol. G. trabeum excreted an extracellular metabolite, 2,5-dimethoxy-1,4-benzoquinone, into the medium and after its reduction to 2,5-dimethoxyhydroquinone, this compound led to the non-enzymatic reduction of dissolved Fe(III) to Fe(II). The production of electron shuttling compounds by microbes can also enhance metal reduction (Gerlach et al. 2011; Field et al. 2013). Similar mechanisms during TNT biodegradation by Y. lipolytica AN-L15 could potentially also occur.
Possible reactions that can take place during TNT transformation in the presence of Y. lipolytica AN-L15 and Fe(III) minerals
3-H−-TNT isomers; 3,5-2H−-TNT; 3,5-2H−-TNT · H+ isomers; 1-H−-TNT
2-HADNT; 4-HADNT; 2-ADNT; 4-ADNT
2,4-DNT + NO2 −
3,5-2H−-TNT · H+
NO2 − + ?
NO2 − + ?
HO2 · + HO2 ·
O2 + H2O2
HO2 · + O2 ·–
O2 + HOO−
3,5-2H−-TNT · H+ isomers
O2 ·– + O2 ·– + 2H+
O2 + H2O2
O2 ·– + NOM
H2O2 + ?
NO2 − + H+
O2 ·– + H2O2
HO. + OH− + O2
HNO3 + 2NO + H2O
Fe(III) + O2 ·–
Fe(II) + O2
NO2 + NO + H2O
Fe(III) + H2O2
Fe(II) + HO2 · + H+
2NO + O2
Fe(II) + HO2 · + H+
Fe(III) + H2O2
NO2 + NOM*
Fe(II) + O2 ·– + 2H+
Fe(III) + H2O2
O2 ·– + NO
Fe(II) + H2O2
Fe(III) + HO. + OH−
ONOO− + H+
Fe(II) + O2
Fe(III) + O2 ·–
NO3 − + H+
2Fe(II) + NO2 + 2H+
2Fe(III) + NO + H2O
ONOO− + CO2
NO2 + CO3 ·–
Fe(II) + NO + H+
Fe(III) + HNO
O2 ·– + H+
N2O + H2O
Mössbauer spectroscopy revealed only relatively minor differences between ferrihydrite, goethite and magnetite minerals incubated with and without TNT; however, hematite exhibited no differences at all. No secondary Fe(II) mineral phases were detected despite the release of a significant proportion of aqueous Fe(II) as detected by the ferrozine assay. These results suggest that all of the Fe(II) which was released in the presence of only cells, or cells + TNT remained in solution and was not re-precipitated as Fe(II) minerals. This is likely due to the low pH of the growth medium which dropped to pH 3 over the course of the incubation. Incubation of the magnetite sample in the presence of Y. lipolytica AN-L15 and TNT resulted in formation of a minor mineral phase which is consistent with the Mössbauer spectrum of a poorly crystalline Fe(III) mineral phase; however, it is not clear what the mineral identity is. A decrease in the relative area of the paramagnetic component in the goethite sample was detected during incubation in the presence of Y. lipolytica AN-L15 and TNT. Analyses performed on both ferrihydrite samples showed that a significant fraction of the mineral in both of them is still not fully magnetically ordered even at 5 K. This would imply the samples have a very low blocking temperature, (i.e. temperature below which a mineral is magnetically ordered) likely much lower than the value which is typically expected for ferrihydrite (Murad 1996). Decreases in the blocking temperature can be caused by poor crystallinity (e.g. due to decreasing particle size) or by association with organic complexes. Mikutta et al. (2008) observed a decrease in blocking temperature from 68 K for pure ferrihydrite to 50 K for ferrihydrite synthesized in the presence of polysaccharides. Thus, it is possible that our samples were not fully magnetically ordered because they were associated with organic material; however, this effect is usually only observed when ferrihydrite is synthesized in the presence of organic matter. The decrease in the relative area of the paramagnetic background for samples containing both goethite and ferrihydrite in the presence of cells and TNT could be primarily attributed to an increase in particle crystallinity. However, this somewhat contradicts the idea that Fe is being released into solution (as Fe(II)) which would require dissolution of the mineral phase, thus leading to a decrease in the particle crystallinity. An alternative explanation could be due to a shift in the particle size distribution which may be present in the goethite and ferrihydrite minerals with a mixture of some large crystalline phases and some smaller (i.e. more poorly crystalline) phases. The smaller particles would have a larger surface area to volume ratio, could thus be more accessible to the yeast cells, and therefore more likely to be the phases which are dissolved, leading to the release of Fe which was detected as Fe(II) in solution by ferrozine. 57Fe Mössbauer only accounts for the solid mineral fraction; therefore as the more poorly crystalline phases are dissolved, the relative amount of more crystalline phase increases which could be interpreted as an increase in crystallinity, as seen in our data.
Our results clearly show the complexity of TNT transformation by Y. lipolytica AN-L15 in the presence of ferric (oxyhydr)oxides. In addition to biotic processes mediated by the yeast strain Y. lipolytica AN-L15, oxygen and nitrogen reactive species generated during TNT transformation process also participated in the abiotic transformation of iron and TNT. Since Fe(II)- and Fe(III)-bearing minerals are found at many TNT-contaminated field areas, the received results are significant for further understanding of TNT degradation and detoxification in the environment.
This work is performed according to the Russian Government Program of Competitive Growth of Kazan Federal University. Partial financial support was provided by the Russian Foundation for Basic Research, Grant No. 14-04-31694.
- Amstaetter K, Borch T, Kappler A (2012) Influence of humic substance imposed changes of ferrihydrite aggregation on microbial Fe(III) reduction. Geochimica et Cosmochimia Acta 85:326–341View ArticleGoogle Scholar
- Bielski BHJ, Cabelli DE, Arudi RL, Ross AB (1985) Reactivity of HO2 ·/O2 ·– radicals in aqueous solution. J Phys Chem Ref Data 14:1041–1100View ArticleGoogle Scholar
- Boparai HK, Comfort SD, Satapanajaru T, Szecsody JE, Grossl PR, Shea PJ (2010) Abiotic transformation of high explosives by freshly precipitated iron minerals in aqueous FeII solutions. Chemosphere 79:865–872PubMedView ArticleGoogle Scholar
- Borch T, Inskeep WP, Harwood JA, Gerlach R (2005) Impact of ferrihydrite and anthraquinone-2,6-disulfonate on the reductive transformation of 2,4,6-trinitrotoluene by a gram-positive fermenting bacterium. Environ Sci Technol 39:7126–7133PubMedView ArticleGoogle Scholar
- Borch T, Kretzschmar R, Kappler A, Van Cappellen P, Ginder-Vogel M, Voegelin A, Campbell K (2010) Biogeochemical redox processes and their impact on contaminant dynamics. Environ Sci Technol 44:15–23PubMedView ArticleGoogle Scholar
- Chien CC, Kao CM, Chen DY, Chen SC, Chen CC (2014) Biotransformation of trinitrotoluene (TNT) by Pseudomonas spp. isolated from a TNT-contaminated environment. Environ Toxicol Chem 33:1059–1063PubMedView ArticleGoogle Scholar
- Cornell RM, Schwertmann U (2003) The iron oxides: structure, properties, reactions, occurances and uses. Wiley-VCH, WeinheimView ArticleGoogle Scholar
- Denicola A, Freeman BA, Trujillo M, Radi R (1996) Peroxynitrite reaction with carbon dioxide/bicarbonate: kinetics and influence on peroxynitrite-mediated oxidations. Arch Biochem Biophys 333:49–58PubMedView ArticleGoogle Scholar
- Eusterhues K, Wagner FE, Häusler W, Hanzlik M, Knicker H, Totsche KU, Kögel-Knabner I, Schwertmann U (2008) Characterization of ferrihydrite-soil organic matter coprecipitates by X-ray diffraction and Mössbauer spectroscopy. Environ Sci Technol 42:7891–7897PubMedView ArticleGoogle Scholar
- Eyers L, Stenuit B, Agathos SN (2008) Denitration of 2,4,6-trinitrotoluene by Pseudomonas aeruginosa ESA-5 in the presence of ferrihydrite. Appl Microbiol Biotechnol 79:489–497PubMedView ArticleGoogle Scholar
- Field EK, Gerlach R, Viamajala S, Jennings LK, Peyton BM, Apel WA (2013) Hexavalent chromium reduction by Cellulomonas sp. strain ES6: the influence of carbon source, iron minerals, and electron shuttling compounds. Biodegradation 24:437–450PubMedView ArticleGoogle Scholar
- Fischer M, Warneck P (1996) Photodecomposition of nitrite and undissociated nitrous acid in aqueous solution. J Phys Chem 100:18749–18756View ArticleGoogle Scholar
- Frejaville C, Karoui H, Tuccio B, Le Moigne F, Culcasi M, Pietri S, Lauricella R, Tordo P (1995) 5-(Diethoxyphosphoryl)-5-methyl-1-pyrroline N-oxide: a new efficient phosphorylated nitrone for the in vitro and in vivo spin trapping of oxygen-centered radicals. J Med Chem 38:258–265PubMedView ArticleGoogle Scholar
- Fritsche W, Scheibner K, Herre A, Hofrichter M (2000) Fungal degradation of explosives: TNT and related nitroaromatic compounds. In: Spain JC, Hughes JB, Knackmuss HJ (eds) Biodegradation of nitroaromatic compounds and explosives. Lewis Publishers, New York, pp 213–238Google Scholar
- Fujii M, Rose AL, Waite TD, Omura T (2006) Superoxide-mediated dissolution of amorphous ferric oxyhydroxide in seawater. Environ Sci Technol 40:880–887PubMedView ArticleGoogle Scholar
- Gerlach R, Field EK, Viamajala S, Peyton BM, Apel WA, Cunningham AB (2011) Influence of carbon sources and electron shuttles on ferric iron reduction by Cellulomonas sp. strain ES6. Biodegradation 22:983–995PubMedView ArticleGoogle Scholar
- Haber F, Weiss J (1934) The catalytic decomposition of hydrogen peroxide by iron salts. Proc R Soc London Ser A 147:332–351View ArticleGoogle Scholar
- Han D, Canali R, Garcia J, Aguilera R, Gallaher TK, Cadenas E (2005) Sites and mechanisms of aconitase inactivation by peroxynitrite: modulation by citrate and glutathione. Biochemistry 44:11986–11996PubMedView ArticleGoogle Scholar
- Harter DR (1985) The use and importance of nitroaromatic chemicals in the chemical industry. In: Rickert DE (ed) Toxicity of nitroaromatic compounds. Hemisphere Publishing Corporation, Washington, DC, pp 1–14Google Scholar
- Hofstetter TB, Heijman CG, Haderlein SB, Holliger C, Schwarzenbach RP (1999) Complete reduction of TNT and other (poly)nitroaromatic compounds under iron-reducing subsurface conditions. Environ Sci Technol 33:1479–1487View ArticleGoogle Scholar
- Jain MR, Zinjarde SS, Deobagkar DD, Deobagkar DN (2004) 2,4,6-Trinitrotoluene transformation by a tropical marine yeast, Yarrowia lipolytica NCIM. Mar Pollut Bull 49:783–788PubMedView ArticleGoogle Scholar
- Kerem Z, Jensen KA, Hammel KE (1999) Biodegradative mechanism of the brown-rot basidiomycete Gloeophyllum trabeum: evidence for an extracellular hydroquinone-driven Fenton reaction. FEBS Lett 446:49–54PubMedView ArticleGoogle Scholar
- Khan MI, Lee J, Park J (2013) A toxicological review on potential microbial degradation intermediates of 2,4,6-trinitrotoluene, and its implications in bioremediation. KSCE J Civ Eng 17:1223–1231View ArticleGoogle Scholar
- Khilyas IV, Ziganshin AM, Pannier AJ, Gerlach R (2013) Effect of ferrihydrite on 2,4,6-trinitrotoluene biotransformation by an aerobic yeast. Biodegradation 24:631–644PubMedView ArticleGoogle Scholar
- Klueglein N, Kappler A (2013) Abiotic oxidation of Fe(II) by reactive nitrogen species in cultures of the nitrate-reducing Fe(II)-oxidizer Acidovorax sp. BoFeN1 – questioning the existence of enzymatic Fe(II) oxidation. Geobiology 11:180–190PubMedView ArticleGoogle Scholar
- Kumagai Y, Wakayama T, Li S, Shinohara A, Iwamatsu A, Sun G, Shimojo N (2000) Zeta-crystallin catalyzes the reductive activation of 2,4,6-trinitrotoluene to generate reactive oxygen species: a proposed mechanism for the induction of cataracts. FEBS Lett 478:295–298PubMedView ArticleGoogle Scholar
- Kumagai Y, Kikushima M, Nakai Y, Shimojo N, Kunimoto M (2004) Neuronal nitric oxide synthase (nNOS) catalyzes one-electron reduction of 2,4,6-trinitrotoluene, resulting in decreased nitric oxide production and increased nNOS gene expression: implication for oxidative stress. Free Radic Biol Med 37:350–357PubMedView ArticleGoogle Scholar
- Kustka AB, Shaked Y, Milligan AJ, King DW, Morel FMM (2005) Extracellular production of superoxide by marine diatoms: contrasting effects on iron redox chemistry and bioavailability. Limnol Oceanogr 50:1172–1180View ArticleGoogle Scholar
- Lauricella R, Allouch A, Roubaud V, Bouteiller JC, Tuccio B (2004) A new kinetic approach to the evaluation of rate constants for the spin trapping of superoxide/hydroperoxyl radical by nitrones in aqueous media. Org Biomol Chem 2:1304–1309PubMedView ArticleGoogle Scholar
- Melton ED, Swanner ED, Behrens S, Schmidt C, Kappler A (2014) The interplay of microbially mediated and abiotic reactions in the biogeochemical Fe cycle. Nature Rev Microbiol 12:797–808View ArticleGoogle Scholar
- Mikutta C, Mikutta R, Bonneville S, Wagner F, Voegelin A, Christl I, Kretzschmar R (2008) Synthetic coprecipitates of exopolysaccharides and ferrihydrite. Part I: Characterization. Geochim Cosmochim Acta 72:1111–1127View ArticleGoogle Scholar
- Morgan B, Lahav O (2007) The effect of pH on the kinetics of spontaneous Fe(II) oxidation by O2 in aqueous solution – basic principles and a simple heuristic description. Chemosphere 68:2080–2084PubMedView ArticleGoogle Scholar
- Murad E (1996) Magnetic properties of microcrystalline iron(III) oxides and related materials as reflected in their Mössbauer spectra. Phys Chem Minerals 23:248–262View ArticleGoogle Scholar
- Naumenko EA, Naumov AV, Suvorova ES, Gerlach R, Ziganshin AM, Lozhkin AP, Silkin NI, Naumova RP (2008) Participation of oxygen in the bacterial transformation of 2,4,6-trinitrotoluene. Biochemistry Moscow 73:463–469PubMedView ArticleGoogle Scholar
- Oh SY, Chiu PC, Cha DK (2008) Reductive transformation of 2,4,6-trinitrotoluene, hexahydro-1,3,5-trinitro-1,3,5-triazine, and nitroglycerin by pyrite and magnetite. J Hazard Mater 158:652–655PubMedView ArticleGoogle Scholar
- Pak JW, Knoke KL, Noguera DR, Fox BG, Chambliss GH (2000) Transformation of 2,4,6-trinitrotoluene by purified xenobiotic reductase B from Pseudomonas fluorescens I-C. Appl Environ Microbiol 66:4742–4750PubMed CentralPubMedView ArticleGoogle Scholar
- Pfeiffer S, Gorren AC, Schmidt K, Werner ER, Hansert B, Bohle DS, Mayer B (1997) Metabolic fate of peroxynitrite in aqueous solution. Reaction with nitric oxide and pH-dependent decomposition to nitrite and oxygen in a 2:1 stoichiometry. J Biol Chem 272:3465–3470PubMedView ArticleGoogle Scholar
- Posth N, Canfield DE, Kappler A (2014) Biogenic Fe(III) minerals: from formation to diagenesis and preservation in the rock record. Earth-Sci Rev 135:103–121View ArticleGoogle Scholar
- Pryor WA, Squadrito GL (1995) The chemistry of peroxynitrite: a product from the reaction of nitric oxide with superoxide. Am J Physiol 268:699–722Google Scholar
- Rose AL, Waite TD (2005) Reduction of organically complexed ferric iron by superoxide in a simulated natural water. Environ Sci Technol 39:2645–2650PubMedView ArticleGoogle Scholar
- Rush JD, Bielski BHJ (1985) Pulse radiolytic studies of the reactions of HO2 ·/O2 ·– with Fe(II)/Fe(III) ions. The reactivity of HO2 ·/O2 ·– with ferric ions and its implication on the occurrence of the Haber-Weiss reaction. J Phys Chem 89:5062–5066View ArticleGoogle Scholar
- Singh B, Kaur J, Singh K (2012) Microbial remediation of explosive waste. Crit Rev Microbiol 38:152–167PubMedView ArticleGoogle Scholar
- Smets BF, Yin H, Esteve-Núñez A (2007) TNT biotransformation: when chemistry confronts mineralization. Appl Microbiol Biotechnol 76:267–277PubMedView ArticleGoogle Scholar
- Stenuit B, Lamblin G, Cornelis P, Agathos SN (2012) Aerobic denitration of 2,4,6-trinitrotoluene in the presence of phenazine compounds and reduced pyridine nucleotides. Environ Sci Technol 46:10605–10613PubMedView ArticleGoogle Scholar
- Stookey L (1970) Ferrozine – a new spectrometric reagent for iron. Anal Chem 42:779–781View ArticleGoogle Scholar
- Van Aken B, Agathos SN (2002) Implication of manganese (III), oxalate, and oxygen in the degradation of nitroaromatic compounds by manganese peroxidase (MnP). Appl Microbiol Biotechnol 58:345–351PubMedView ArticleGoogle Scholar
- Van Cleemput O, Baert L (1984) Nitrite: a key compound in N loss processes under acid conditions? Plant Soil 76:233–241View ArticleGoogle Scholar
- Van den Berg AJ, Halkes SB, Van Ufford HC, Hoekstra MJ, Beukelman CJ (2003) A novel formulation of metal ions and citric acid reduces reactive oxygen species in vitro. J Wound Care 12:413–418PubMedView ArticleGoogle Scholar
- Vásquez-Vivar J, Denicola A, Radi R, Augusto O (1997) Peroxynitrite-mediated decarboxylation of pyruvate to both carbon dioxide and carbon dioxide radical anion. Chem Res Toxicol 10:786–794PubMedView ArticleGoogle Scholar
- Wittich RM, Ramos JL, Van Dillewijn P (2009) Microorganisms and explosives: mechanisms of nitrogen release from TNT for use as an N-source for growth. Environ Sci Technol 43:2773–2776PubMedView ArticleGoogle Scholar
- Ziganshin AM, Gerlach R (2014) Pathways of 2,4,6-trinitrotoluene transformation by aerobic yeasts. In: Singh SN (ed) Biological remediation of explosive residues. Environmental science and engineering. Springer International Publishing AG, Switzerland, pp 301–311View ArticleGoogle Scholar
- Ziganshin AM, Naumov AV, Suvorova ES, Naumenko EA, Naumova RP (2007a) Hydride-mediated reduction of 2,4,6-trinitrotoluene by yeasts as the way to its deep degradation. Microbiology 76:676–682View ArticleGoogle Scholar
- Ziganshin AM, Gerlach R, Borch T, Naumov AV, Naumova RP (2007b) Production of eight different hydride complexes and nitrite release from 2,4,6-trinitrotoluene by Yarrowia lipolytica. Appl Environ Microbiol 73:7898–7905PubMed CentralPubMedView ArticleGoogle Scholar
- Ziganshin AM, Gerlach R, Naumenko EA, Naumova RP (2010a) Aerobic degradation of 2,4,6-trinitrotoluene by the yeast strain Geotrichum candidum AN-Z4. Microbiology 79:178–183View ArticleGoogle Scholar
- Ziganshin AM, Naumova RP, Pannier AJ, Gerlach R (2010b) Influence of pH on 2,4,6-trinitrotoluene degradation by Yarrowia lipolytica. Chemosphere 79:426–433PubMedView ArticleGoogle Scholar
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