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Identifying the reactive sites of hydrogen peroxide decomposition and hydroxyl radical formation on chrysotile asbestos surfaces
Particle and Fibre Toxicology volume 17, Article number: 3 (2020)
Fibrous chrysotile has been the most commonly applied asbestos mineral in a range of technical applications. However, it is toxic and carcinogenic upon inhalation. The chemical reactivity of chrysotile fiber surfaces contributes to its adverse health effects by catalyzing the formation of highly reactive hydroxyl radicals (HO•) from H2O2. In this Haber-Weiss cycle, Fe on the fiber surface acts as a catalyst: Fe3+ decomposes H2O2 to reductants that reduce surface Fe3+ to Fe2+, which is back-oxidized by H2O2 (Fenton-oxidation) to yield HO•. Chrysotile contains three structural Fe species: ferrous and ferric octahedral Fe and ferric tetrahedral Fe (Fe3+tet). Also, external Fe may adsorb or precipitate onto fiber surfaces. The goal of this study was to identify the Fe species on chrysotile surfaces that catalyze H2O2 decomposition and HO• generation.
We demonstrate that at the physiological pH 7.4 Fe3+tet on chrysotile surfaces substantially contributes to H2O2 decomposition and is the key structural Fe species catalyzing HO• generation. After depleting Fe from fiber surfaces, a remnant fiber-related H2O2 decomposition mode was identified, which may involve magnetite impurities, remnant Fe or substituted redox-active transition metals other than Fe. Fe (hydr)oxide precipitates on chrysotile surfaces also contributed to H2O2 decomposition, but were per mole Fe substantially less efficient than surface Fe3+tet. Fe added to chrysotile fibers increased HO• generation only when it became incorporated and tetrahedrally coordinated into vacancy sites in the Si layer.
Our results suggest that at the physiological pH 7.4, oxidative stress caused by chrysotile fibers largely results from radicals produced in the Haber-Weiss cycle that is catalyzed by Fe3+tet. The catalytic role of Fe3+tet in radical generation may also apply to other pathogenic silicates in which Fe3+tet is substituted, e.g. quartz, amphiboles and zeolites. However, even if these pathogenic minerals do not contain Fe, our results suggest that the mere presence of vacancy sites may pose a risk, as incorporation of external Fe into a tetrahedral coordination environment can lead to HO• generation.
The term asbestos refers to a heterogeneous group of five fibrous amphiboles and one fibrous serpentine mineral (chrysotile) [1, 2]. Due to its favorable properties such as a large tensile strength, heat resistance and non-combustibility, asbestos has been used in a variety of industrial applications , e.g. in thermal and electrical insulation, roofing, cement pipes and sheets, flooring and coatings [4, 5]. However, respiratory exposure to asbestos minerals causes adverse health effects like pneumoconiosis, fibrosis of the lung, pleural plaques and effusions, carcinomas predominantly in the lung (but also in the larynx and ovaries) and mesotheliomas in the pleura and peritoneum [2, 4, 6, 7]. Because of their carcinogenic potential, the WHO-IARC has classified all asbestos minerals as group 1 carcinogens . More than 100,000 people die each year because of asbestos-related illnesses, mostly following occupational exposure . Because of the intrinsic health hazard of asbestos, its use has been banned in European countries from the late 1980s onwards . In northern American countries its use has not yet been banned  and in some Asian countries it even increases [11, 12].
Chrysotile [Mg3Si2O5(OH)4] accounts for more than 95% of all historically used asbestos . As a result, exposure to asbestos predominantly concerns chrysotile. Therefore, we have focused on this mineral in this study. Chrysotile asbestos consists of octahedral Mg hydroxide layers and tetrahedral Si layers which bundle together to a fiber with a Mg hydroxide layer at the surface [14, 15]. During petrogenesis, Fe is substituted into the crystal lattice (usually up to 2–4 wt%) . Ferrous and ferric Fe are found in the Mg layers (Fe3+oct and Fe2+oct, respectively), whereas in the Si layers, exclusively ferric Fe is found (Fe3+tet) [17, 18]. Fe is by far the most abundant redox-active metal in chrysotile .
Weathering of chrysotile at circumneutral pH is commonly described as a layer-by-layer dissolution of alternating Mg and Si layers. Mg layers at the fiber surface dissolve within hours, whereas exposed Si layers dissolve much slower and therefore determine the overall dissolution rate [19, 20]. However, enhanced dissolution of Fe3+tet from the Si layer by ligands like the siderophore desferrioxamine-B (DFOB) increases the Si dissolution rate, presumably through the formation of vacancy sites in the Si layer that labilize it .
Asbestos-induced pathologies can be linked to its high persistence in vivo [7, 22, 23], its fibrous morphology and the surface chemistry of the fibers [2, 7]. Asbestos fibers lodged in lung or pleural tissue induce continuous, yet unsuccessful attempts of macrophages and neutrophils to phagocytose the fibers - a process called frustrated phagocytosis. During this process, enzymatically formed reactive oxygen species (ROS) like hydrogen peroxide (H2O2) and superoxide anions (O2•-) are released into the immediate extracellular environment . Both exhibit a low potency for cellular damage under homeostasis  and can be enzymatically detoxified. At elevated concentrations H2O2 and O2•- may, however, interact with Fe on the fiber surface. This interaction induces cyclical redox reactions generating hydroxyl radicals (HO•), which have a high potency to damage DNA, proteins and lipids [2, 24,25,26,27]. In this Haber-Weiss cycle, Fe acts as a catalyst: Fe3+ is reduced by O2•- to Fe2+, which is back-oxidized by H2O2 in the so-called Fenton reaction, yielding Fe3+ and HO• [2, 28]. In the presence of Fe3+, H2O2 may decompose to hydroperoxyl (HO2•), which can either directly reduce Fe3+ to Fe2+ or decompose to the even stronger reductant, O2•- .
Despite the important role of H2O2 and its degradation products in Fe redox cycling at the chrysotile fiber surface, H2O2 decomposition by asbestos has only been assessed in a limited number of studies [30,31,32]. An involvement of the Fenton and Haber-Weiss pathways in H2O2 decomposition by asbestos was demonstrated by Eberhardt et al. (1985) . Furthermore, Fubini et al. (1995)  assessed H2O2 decomposition for various Fe containing minerals. They found that H2O2 decomposition rates by chrysotile and crocidolite were comparable, yet smaller than by magnetite and substantially larger than by hematite.
H2O2 decomposition by chrysotile partly occurs through Fenton reactions involving Fe surface species [2, 25, 33]. However, not all Fe surface species are equally Fenton-active or have an equal potential to form hydroxyl radicals. Fubini et al. (1995)  demonstrated that Fe2+oct on chrysotile surfaces does not play a substantial role in HO• generation. Recently, Walter et al. (2019) suggested that per mole Fe the potential to generate HO• is substantially larger for surface exposed Fe3+tet than for Feoct . Furthermore, Fe3+tet is the only Fe surface species in chrysotile that remains Fenton-active during long-term dissolution (weeks) at circumneutral pH, because the Si layer in which it is incorporated dissolves slowly, whereas Feoct in the readily dissolving Mg layers rapidly precipitates to Fenton-inactive Fe (hydr)oxide minerals . Depletion of all Fe surface species (including Fe3+tet) from chrysotile surfaces by ligands like DFOB decreased the radical yield of the fibers, almost to background values [21, 33]. Apart from structural Fe, also external Fe that associates with surfaces of asbestos (or other silicates) may generate ROS and increase oxidative stress in vivo and in vitro [2, 34,35,36,37].
To our knowledge, the relation between Fe speciation at chrysotile fiber surfaces and H2O2 decomposition rates has not yet been established. Also, the relation between the speciation of external Fe after associating with the chrysotile fiber surface and the change in radical yield and H2O2 decomposition rate of the fibers has not been explored previously. Hence, the current understanding of which Fe species at the chrysotile surface participate in the prerequisite step of the first stage (H2O2 decomposition to reductants), and in the second stage (Fenton oxidation) of the Haber-Weiss cycle is incomplete. Establishing the reactive sites of H2O2 decomposition and HO• generation on chrysotile surfaces is important in assessing the overall redox reactivity of chrysotile asbestos, which is a major determinant in its pathogenicity [25, 38]. In this study we addressed this knowledge gap.
We hypothesize that H2O2 is decomposed, either by structural Fe3+tet in exposed Si layers of the dissolving fibers, or by secondary Fe minerals precipitated on the fiber surface. The precipitated Fe may originate from external sources or from fiber dissolution during which structural Fe is released. Furthermore, we hypothesize that external Fe only substantially contributes to the HO• yield of chrysotile fibers when it becomes tetrahedrally coordinated by incorporation into a Si layer. The rationale for this hypothesis is the high potential of surface Fe3+tet for generating HO• , compared to the low potential of Fe (hydr)oxides  precipitated on chrysotile surfaces. Finally, we hypothesize that chrysotile fibers with surfaces depleted in Fe (e.g. due to preconditioning with a ligand) may still pose a health hazard if external Fe is incorporated into vacant surface sites in the Si layer.
The hypotheses were tested in batch incubation experiments. Samples were analyzed by ICP-OES (inductively coupled plasma optical emission spectrometry), UV-VIS-photospectrometry, Mössbauer spectroscopy and EPR (electron paramagnetic resonance) spectroscopy.
Chemical reagents and asbestos characterization
All chemical reagents used in this study were at least pro analysis grade and were ordered from VWR (unless otherwise mentioned). Chrysotile asbestos was purchased from Shijiazhuang Mining IMP&EXP Trade Co, China. The material was characterized by XRD-Rietveld phase analysis, Raman spectroscopy, BET specific surface area measurement, Mössbauer spectroscopy, fusion digestion and neutron activation analysis . The BET specific surface area (SSA) of Shijiazhuang chrysotile fibers was 20.3 m2 g− 1 (with a standard deviation of 0.9 m2 g− 1, ), and phase impurities were established by XRD-Rietveld analysis: Shijiazhuang chrysotile contains 86.4 ± 4.6% chrysotile fibers, whereas phase impurities in the fiber material are brucite, talc, chlorite, magnetite, quartz and calcite . Key results on the bulk of Shijiazhuang chrysotile are presented in Table 1: Shijiazhuang chrysotile asbestos contains ≈249 g kg− 1 Mg and ≈188 g kg− 1 Si; the stoichiometric Mg/Si ratio is close to 1.5. Fe (≈20 g kg− 1) and Al (≈8 g kg− 1) are the major substituents. Mössbauer analyses demonstrated that in pristine Shijiazhuang chrysotile asbestos, almost all Fe is substituted into the octahedral Mg layer (≈ 55% Fe3+oct and ≈ 38% Fe2+oct), whereas only 7% is substituted into the tetrahedral Si layer (Table 1). Magnetite (1.5 ± 0.2% in Shijiazhuang chrysotile) hosts approximately 32% of the total bulk Fe (Table 1).
Preparation of fiber suspensions
All experiments were carried out in fiber suspensions with a fiber to solution ratio of 1 g L− 1. The non-metal-complexing tertiary amine (“Better”) buffer  MOPS (3-(N-morpholino)propanesulfonic-acid) was used at a concentration of 50 mmol L− 1 to maintain the pH of experimental solutions at 7.4 ± 0.3. The ionic strength of the buffer solutions was adjusted to 300 mmol L− 1 by addition of NaCl. Solutions in blank treatments contained only pH-buffer and electrolyte, while DFOB (Novartis) treatments additionally contained 1 mmol L− 1 DFOB. In H2O2 decomposition experiments DFOB was used to quench the redox-activity of Fe. This method has been used previously, e.g. in refs [40, 41]. Finally, H2O2 decomposition was also studied in 0.1 mol L− 1 NaOH solutions in which chrysotile fibers are practically insoluble .
Preconditioning of chrysotile fibers
Fibers were preconditioned to obtain fiber types with different specific surface chemistry. The preconditioning involved incubation of the fibers in blank solutions buffered at pH 7.4 for 336 h (“blank-altered fibers”) or in 1 mmol L− 1 DFOB solutions buffered at pH 7.4 (“DFOB-altered fibers”). In previous studies it was shown that in blank-altered fibers, the outermost Mg layer had dissolved during preconditioning and the Fe content of the dissolved Mg layer had precipitated as secondary Fe phases with low Fenton activity [21, 37]. Moreover, in DFOB-altered fibers the Fe content of the dissolved outermost Mg layer as well as the Fe content of the slowly dissolving Si layer was complexed and mobilized by DFOB. Fe mobilization from the Si layer presumably leads to the formation of vacancy sites, which promote Si dissolution . During preconditioning up to 4% of the fiber mass dissolved; assuming a cylindrical fiber geometry with constant length, this corresponds with a 2% decrease in SSA, which is smaller than the standard deviation on the BET-SSA analysis and was considered negligible.
To test whether external Fe can be incorporated into vacancy sites in the Si layer and whether this incorporated Fe participates in H2O2 decomposition and HO• generation, DFOB-altered fibers were suspended in solutions buffered at pH 7.4 containing 0, 3, 30 and 300 μmol L− 1 of Fe2+ under anoxic conditions in a N2-filled anoxic chamber (Brown box). The suspensions were then immediately oxygenated outside the anoxic chamber by air bubbling for 24 h, while magnetically stirring them at 500 rotations per minute. The Fe2+ rapidly oxidized and Fe not incorporated into vacancy sites precipitated onto fiber surfaces as Fe (hydr)oxide minerals, coloring the fibers beige to yellow (see Fig. 1). As a negative control, the same concentrations of Fe were precipitated onto blank-altered fibers (which presumably lack vacancy sites in the Si layer) following the same procedure. The obtained altered fiber types are referred to as “DFOB-altered fibers + 0, 3, 30 or 300 μmol g− 1 Fe” and “blank-altered fibers + 0, 3, 30 or 300 μmol g− 1 Fe”. Preconditioned fibers were collected in Büchner funnels on 0.47 μm Nylon membranes (Magna) and dried by vacuum filtration. To remove potentially adsorbed DFOB ligand or metal-DFOB complexes, fibers were washed with ultra-pure water and then vacuum-dried and stored in an evacuated desiccator until they were used in follow-up experiments. Metal and Si concentrations mobilized during the fiber preparations are presented in Additional file 1: Table S1.
57Fe addition and Mössbauer analyses
57Fe Mössbauer spectroscopy was performed at room temperature in standard constant acceleration mode with a 57CoRh source, relative to which all center shift data are given. The analyzed fiber types were DFOB-altered and blank-altered fibers + 0 μmol g− 1 Fe, and DFOB-altered and blank-altered fibers + 3 μmol g− 1 Fe. These fiber types were prepared following the procedure described above, except that isotopically enriched 57Fe (Sigma Aldrich, > 95 atom % isotopic purity) was used. The isotopically enriched metallic 57Fe-powder was dissolved over night at 70 °C in a 2 mol L− 1 HCl solution, according to Arrigo et al. (2017) . This procedure yielded a 57Fe2+ solution, which was purged with N2 for 2 h and then put into the anoxic glove box. The isotopic composition of Fe in the stock solution was verified by ICP-MS (57Fe accounted for 99.2% of the total Fe), and the Fe2+ concentration was verified spectrophotometrically with a ferrozine assay . Aliquots of the 57Fe2+ stock solution were added to DFOB-altered and blank-altered fiber suspensions to obtain an added concentration of 3 μmol g− 1 57Fe2+.
After vacuum filtration and drying of the fibers, 700 mg of each fiber type were ground in a tungsten carbide ball mill (Resch Schwingmühle MM 400) for 30 s (a duration that does not affect Fe2+/Fe3+ ratios in minerals ) at 30 strokes per minute in order to avoid spatial anisotropy of fibers in specimens. 500 mg of the milled fibers were pressed between Teflon foils (Zuma). Mössbauer measurements required up to 2 weeks per samples (Fig. 2). The spectroscopic data were analyzed by solving the full Hamiltonian. Thickness of the samples was taken into account after Mørup and Both (1975) . A ferrihydrite sub-spectrum (based on data from Murad and Schwertmann, 1980, ) was used to account for Fe precipitation on blank-altered fibers + 0 μmol g− 1 57Fe (precipitation of Fe from the dissolved Mg layer) and DFOB-altered and blank-altered fibers + 3 μmol g− 1 57Fe (precipitation of added 57Fe). Ferrihydrite was selected, because under the experimental conditions such a poorly crystalline Fe3+ (hydr)oxide mineral is most likely to precipitate. Fits involving DFOB-altered fibers + 0 μmol g− 1 57Fe were done with and without ferrihydrite sub-spectrum; including the ferrihydrite sub-spectrum did not significantly improve the fit. Because presumably precipitation of ferrihydrite was prevented by addition of DFOB, the fit without the ferrihydrite sub-spectrum was used for comparison with the other treatments. Each sample was measured two times: first in a wider velocity range (± 10.6 mm s− 1) to cover the full magnetically split-spectrum of magnetite impurities, which allowed to obtain the amount of magnetite in the samples, and second in a narrow velocity range (± 4.6 mm s− 1) to better resolve the chrysotile and Fe3+ (hydr)oxide contributions. The obtained hyperfine parameters for both velocity ranges are presented in Additional file 1: Table S2, the spectra of the narrow velocity range are presented in Fig. 2 and the spectra of the wide velocity range in Additional file 1: Figure S1. The magnetite contents were calculated based on the wide velocity range data. After determination of the percentage of magnetite, the percentages of remaining Fe species were determined using the narrow velocity range data by multiplying the narrow velocity range percentages of these Fe species with (100% - magnetite% (wvr))/(100% - magnetite% (nvr)). Finally, all percentages were multiplied by the total amount of 57Fe in each treatment. For blank-altered fibers the Fe content equaled the average content in pristine fibers measured by neutron activation analysis (NAA, Table 1), the amount of Fe removed by DFOB in DFOB-altered fibers was determined from the dissolved Fe concentration after reaction with DFOB. The amount of 57Fe added was known.
Experimental procedure for H2O2 decomposition experiments
In the H2O2 decomposition experiments, metal mobilization from, and decomposition of H2O2 by, differently preconditioned fibers were assessed. Included fiber types were: pristine fibers, blank-altered fibers, DFOB-altered fibers and both blank-altered and DFOB-altered fibers + 0, 3, 30 or 300 μmol g− 1 Fe. Experiments were carried out at pH 7.4 in MOPS buffer, and additionally for pristine and blank-altered fibers in a 0.1 mol L− 1 NaOH solution. The initial experimental H2O2 concentration was 3.3 g L− 1 (≈ 0.3%), which was prepared by diluting a 30% stock solution (Sigma Aldrich, for trace analysis) a hundred times. The H2O2 concentration of the stock was determined by redox titration with KMnO4: 334 ± 2 g L− 1 H2O2. Experiments were carried out in duplicates in 15 ml PP tubes (VWR) that were shaken in an end-over-end shaker at 15 rounds per minutes (RPM) at 20 ± 2 °C in the dark. Samples were taken destructively after 0.5, 1, 4, 8, 24, 48, 96, 168 and 336 h. Suspensions were filtered over 0.45 μm Sartorius cellulose acetate syringe filters. An aliquot of each filtrate was acidified to 0.14 mol L− 1 HNO3 (trace metal grade) for metal (Mg and Fe) and Si concentration analysis by ICP-OES (Perkin Elmer Optima 5300-DV). Another aliquot of each filtrate was diluted for H2O2 concentration measurements. Calibration standards for ICP-OES analysis were matrix-matched with the samples. The decomposition of H2O2 was assessed by measuring the H2O2 concentration in diluted filtrates immediately after each sampling round. H2O2 concentrations were determined spectrophotometrically by a titanium sulfate method . One ml of a 1.9–2.1% titanium (IV) oxysulfate solution (Sigma Aldrich) was added to 0.5 ml of the diluted filtrate and light absorption by the resulting peroxytitanyl-ion was measured at 410 nm by a Varian Cary 50 UV/VIS spectrophotometer (ɛ = 689 L mol− 1 cm− 1). H2O2 concentrations in the samples were quantified by an external linear calibration method (7 to 42 mg L− 1 H2O2); filtrates were diluted down to fit the calibration range. Because H2O2 also reacts with MOPS buffer , a control treatment to determine the H2O2 decomposition rate in absence of fibers was also included. Also for experiments in 0.1 mol L− 1 NaOH a control treatment without fibers was included. In an additional experiment, H2O2 decomposition by pristine, blank-altered and DFOB-altered fibers was examined at pH 7.4 in the presence of 1 mmol L− 1 DFOB using the same experimental procedure. The absorption maximum of the FeDFOB complex (425 nm; ɛ = 2460 L mol− 1 cm− 1, ) and the peroxytitanyl-ion (vide supra) [47, 50] are in close proximity. However, FeDFOB concentrations were orders of magnitude smaller and the molar absorption coefficients of the complexes are less than one order of magnitude different. Therefore, the contribution of FeDFOB to overall light absorption at 410 nm could be neglected.
EPR spin trapping analyses of hydroxyl radicals generated by Fe on chrysotile fibers surfaces
The HO• yield of fiber specimens in the presence of H2O2 was quantified with 5–5-dimethyl-1-pyrroline N-oxide (DMPO) as spin trapping agent using a X-band EPR-spectrometer (Bruker EMX) and a split ring resonator (Bruker MD5). This spin trapping technique has frequently been used for this purpose before [26, 31, 37, 51, 52]. Eleven mg of fibers were incubated for 0.5 h in 0.5 ml of a 125 mmol L− 1 H2O2 and 12.5 mmol L− 1 DMPO solution buffered at pH 7.3 with a 250 mmol L− 1 chelex-treated phosphate buffer. After 25 min of incubation at room temperature and 5 min of centrifugation (14,000 RPM), 50 μl of the supernatant were pipetted into a glass capillary (intraMark Blaubrand), which was then sealed with Critoseal. Subsequently, the capillary was transferred into the resonator. The instrumental settings for the EPR measurements are described in Walter et al. (2019) . EPR measurements were performed on four subsamples from each type of preconditioned fibers (quadruplicates). To quantify the change in HO• yield, the signal intensity (Intensity peak-to-peak (Ipp)) of the second peak from the left in the DMPO/HO• quadruplet of altered fibers was determined and expressed as a percentage of the Ipp of pristine fibers, which was measured as a reference in each measurement session. For comparison, also the HO• yield of the poorly crystalline Fe (oxy)hydroxide 2-line ferrihydrite (3 ± 0.2 mg, synthesized according to Schwertmann and Cornell (2000), ) was measured following the same procedure. An amorphous Fe (hydr)oxide like 2-line ferrihydrite may precipitate upon Fe addition to the fibers and subsequent oxygenation [53, 54].
Statistical analysis and supplementary data
Statistical analysis of the EPR spin trapping data was performed with the program SPSS Version 25. A square root transformation of the data was carried out to reduce skewness. Homogeneity of the transformed data was tested with the Levene’s test (α = 0.05). Differences among treatments were established by applying the univariate general linear model procedure and the Tukey post-hoc test (α = 0.05). A statistical test was employed to answer a) if the HO• yield increased with the amount of Fe applied to DFOB-altered fibers and b) if, through addition of Fe to DFOB-altered fibers, the HO• yield of blank-altered fibers could be reached.
The data included in Figs. 2, 3, 4 and 5 are reported in Additional file 1: Table S2 to Table S5, respectively. The p-values from the statistical analyses of the EPR data are reported in Additional file 1: Table S6.
Color changes related to Fe at chrysotile surfaces
Complexation and mobilization of Fe from the beige pristine chrysotile fibers by DFOB resulted in the whitish color of DFOB-altered fibers (Fig. 1). Interaction of DFOB-altered fibers with 3 μmol g− 1 Fe changed the whitish color to greyish after exposure to oxygen; interaction with 30 μmol g− 1 Fe reversed the color to beige, comparable to the color of pristine (not shown) and blank-altered fibers, and interaction with 300 μmol g− 1 Fe changed the color to yellow (Fig. 1). Interaction of pristine fibers with 0, 3 and 30 μmol g− 1 Fe did not lead to a clear change in the beige fiber color of blank-altered fibers, whereas addition of 300 μmol g− 1 Fe again changed the color of the fibers to yellow (Additional file 1: Figure S2).
Coordination environment of 57Fe after interaction with chrysotile surfaces
The contribution of the subspectra to the overall Mössbauer spectrum differed per fiber type (Fig. 2; Additional file 1: Table S2), indicating that preconditioning induced a shift in 57Fe species distribution. Preconditioning with DFOB reduced the fraction of Fe present as Fe3+tet in comparison to the blank-altered treatment (Fig. 2 panel a an b; Additional file 1: Table S2c) and lowered the Fe3+tet content by half, from 15.0 to 7.7 μmol g− 1 Fe (Additional file 1: Table S7). As only 4% of the fiber mass had dissolved during preconditioning, this suggests that Fe3+tet sites are not homogenously distributed over the chrysotile bulk, but are strongly enriched in Si layers near the fiber surface. Addition of 3 μmol of 57Fe per gram of DFOB-altered fibers increased the 57Fe3+tet fraction (Fig. 2 panel a and c) from 2.2 to 3.8% (Additional file 1: Table S2c). This corresponds with an increase in total Fe3+tet bulk content by 3% (Additional file 1: Table S7), suggesting a marginal recovery of Fe3+tet sites at chrysotile surfaces by addition of 57Fe. Most added 57Fe (1.8 μmol g− 1 Fe ≈ 60%) was retrieved as Fe3+oct. In contrast, addition of 3 μmol of 57Fe per gram of blank-altered fibers resulted in a decrease in 57Fe3+tet fraction (Fig. 2 panel b and d) from 4.0 to 3.3% (Additional file 1: Table S2c) and a negligible change (0.3%) in total Fe3+tet bulk content (14.9 μmol g− 1 Fe, Additional file 1: Table S7). Most added 57Fe (1.8 μmol g− 1 Fe ≈ 60%) was retrieved as magnetite.
Dissolution of metals and Si from pristine and preconditioned chrysotile fibers in the presence of H2O2
In Fig. 3, Mg and Si concentrations mobilized from pristine and preconditioned chrysotile fibers in the presence of H2O2 (initial concentration: 3.34 g L− 1) are reported as a function of time. Fe concentrations were in the sub-micromolar range throughout all these experiments (data no shown). In contrast to our results, Ghio et al. (1998) reported somewhat higher mobilized Fe concentrations from a different chrysotile preparation by H2O2 .
For Mg mobilization from pristine chrysotile fibers, two stages could be distinguished (Fig. 3, Panel a1): a fast first stage during which the outermost Mg layer of the fibers rapidly dissolved (first few days), and a slower second stage during which the outermost Mg layer had been completely dissolved, Si dissolution had become rate limiting and mobilized Mg concentrations reached a plateau at approximately 500 to 600 μmol L− 1 (between 96 and 336 h). Mg mobilization from DFOB-altered and blank-altered fibers could not be divided into two dissolution stages, but increased linearly throughout the experiment. Si concentrations mobilized from all three fiber types increased linearly throughout the experiment (Fig. 3, Panel a2). Mobilized Si concentrations were consistently higher for DFOB-altered fibers than for blank-altered and pristine fibers. Adsorption and precipitation of added Fe onto DFOB-altered fiber surfaces decreased the rate of Mg (Fig. 3, Panel b1) and Si (Fig. 3, Panel b2) mobilization throughout the experiment. The decrease in Mg and Si dissolution rates were however not proportional to the amount of Fe applied and reached a maximum of approximately 50% with addition of 30 μmol g− 1 Fe. Adsorption and precipitation of added Fe onto blank-altered fiber surfaces did not decrease Mg and Si mobilization as strongly as for DFOB-altered fibers (Fig. 3, Panel c1 and c2, respectively): addition of 300 μmol g− 1 Fe only decreased mobilized Mg concentrations by 18% and mobilized Si concentrations by 20% after 336 h.
H2O2 decomposition by pristine and preconditioned chrysotile fibers
H2O2 decomposition kinetics in the presence of chrysotile and MOPS buffer could be well described with a first order rate equation in H2O2 concentration:
in which ktot is the overall decomposition constant. Chrysotile fibers accelerated H2O2 decomposition relative to the MOPS-buffer control treatment by a factor 2 to 5, depending on the pretreatment (Fig. 4a, Table 2). H2O2 decomposition was fastest with pristine fibers and slowest with DFOB-altered fibers. The addition of DFOB as a redox quencher for Fe largely inhibited differences in the H2O2 decomposition rate between pristine, blank-altered and DFOB-altered fibers (Fig. 4b). In the treatment with DFOB-altered fibers, the application of DFOB as redox quencher had no effect on H2O2 decomposition; for the treatments with pristine and blank-altered fibers, H2O2 decomposition decreased as a result of DFOB addition (Fig. 4a and b). For the treatments with DFOB-altered fibers and DFOB-altered fibers + 0 μmol g− 1 Fe, ktot values did not differ (2.5*10− 3 h− 1), demonstrating that the fiber preparation procedure without Fe addition did not affect the H2O2 decomposition rate. Fe addition to DFOB-altered fibers increased ktot values by up to over a factor 2 in the DFOB-altered fibers + 300 μmol g− 1 Fe (5.3*10− 3 h− 1); the increase in ktot was non-proportional to the amount of Fe added (Fig. 4c, Table 2). A non-proportional increase in ktot values was also found for treatments in which Fe had been added to blank-altered fibers. The relative increase was however smaller, amounting a factor 1.4 (from 4.2*10− 3 h− 1 to 6.0*10− 3 h− 1; Fig. 4d, Table 2).
The contributions from different reactive sites on chrysotile surfaces to overall H2O2 decomposition can be estimated in a tiered approach (Table 3), under the assumption that the various degradation mechanisms are independent, and their decomposition constants add up to the ktot of the reaction. Equation 1 can then be rewritten to equation 2:
in which k1 to n represent the contributions of the individual H2O2 decomposition pathways to the overall decomposition constant ktot. In addition to contributions from tetrahedral Fe and Fe (hydr)oxide precipitates, the difference in decomposition rate between the MOPS buffer control and the DFOB-altered fiber treatment suggests a contribution from a remnant H2O2 decomposition pathway (Fig. 4b, Table 3). The control treatment with MOPS buffer-only provided the contribution from the MOPS buffer to H2O2 degradation. The contribution from the remnant decomposition pathway was calculated by subtracting the contribution from the MOPS buffer from the ktot value of the DFOB-altered fiber treatment, under the assumption that DFOB had removed most Fe from the fiber surfaces. For the contribution from Fe (hydr)oxide precipitates to H2O2 degradation it was assumed that the outer Mg and Si layer contained approximately 30 μmol g− 1 Fe (Additional file 1: Table S1, Walter et al. (2019), ), that this Fe largely precipitated in the blank treatment as only a small fraction of the Fe is located in the slowly dissolving Si layer (Table 1), and that precipitation of an additional 30 μmol g− 1 Fe had the same effect size on the ktot value as the Fe that precipitated from the outer layer. The contribution of Fe (hydr)oxide precipitates to the ktot value can then be calculated by subtracting the ktot value of the blank-altered treatment from the blank-altered + 30 μmol g− 1 Fe treatment. Finally, the contribution from tetrahedral Fe was calculated by subtracting the contributions from the MOPS buffer, Fe (hydr)oxide precipitates and the H2O2 decomposition pathway from the ktot value of the blank treatment (Table 3).
Following this approach, the ktot value of the blank-altered fiber treatment (4.2*10− 3 h− 1; Table 2, treatment 2) was broken down to contributions from the three types of active surface sites and the MOPS buffer (equation 2). The contributions of the active surface sites to ktot were comparable, varying within a factor 2, and also the contribution from the MOPS buffer fell within this range (Table 3).
The solution pH had a strong effect on the H2O2 decomposition rate: in 0.1 mol L− 1 NaOH (pH 12–13) the decomposition rate by pristine and preconditioned fibers was approximately an order of magnitude faster than at pH 7.4 (Table 2).
Effect of Fe addition to preconditioned chrysotile fibers on HO• generation
Pretreatment of Shijiazhuang chrysotile asbestos decreased the HO• yield relative to pristine fibers to 50 ± 10% for blank-altered fibers and to 9% for DFOB-altered fibers . The HO• yield of blank-altered and DFOB-altered fibers + 0 μmol g− 1 Fe (Fig. 5) corresponded with these values. For all treatments with Fe addition to DFOB-altered fibers, the HO• yield was larger than for the + 0 μmol g− 1 Fe treatment. The HO• yield increased non-proportionally with the amount of Fe added, from 7% (+ 0 μmol g− 1 Fe) to 36% (+ 300 μmol g− 1 Fe) (Fig. 5a; Additional file 1: Table S5). Although a factor 10 more Fe had been added in the DFOB-altered + 300 μmol g− 1 Fe treatment than was extracted in the DFOB-pretreatment, the HO• yield remained lower than in the blank-altered + 0 μmol g− 1 Fe fiber treatment (Fig. 5; Additional file 1: Table S5), suggesting that the HO• yield could be largely, but not fully recovered. The addition of Fe to blank-altered fibers did not consistently increase the HO• yield of chrysotile (Fig. 5b). Furthermore, the HO• yield of 3 mg of 2-line ferrihydrite was 11% (relative to the HO• yield of 11 mg pristine chrysotile fibers). The total amount of Fe in 3 mg of 2-line ferrihydrite (≈1.8 mg Fe) is a thousand times larger than the 1.8 μg Fe on the fiber surface of the aliquots of DFOB-altered fibers + 3 μmol g− 1 Fe. Despite this large difference, the increase in HO• yield (an increase from 7 to 17%) due to the 3 μmol g− 1 Fe addition was comparable with the overall HO• yield of 3 mg of ferrihydrite (11%).
Speciation of added Fe and implications for fiber dissolution
Si dissolution from DFOB-altered fibers was over a factor three faster than from pristine fibers, whereas Si dissolution from blank-altered and pristine fibers were comparably fast (Fig. 3, Panel a2). The faster Si mobilization from DFOB-altered fibers is a consequence of the complexation of Fe3+tet by DFOB during pretreatment. Presumably this led to the formation of vacancy sites in the Si layer resulting in Si labilization which enhanced Si dissolution rates . Si mobilization from blank-altered fibers was considerably slower, because no Fe3+tet had been removed from the Si layers during pretreatment. The larger Mg mobilization rate from DFOB-altered fibers compared to blank-altered fibers presumably resulted from the larger rate-controlling Si mobilization rate, allowing segments of deeper Mg layers to dissolve more rapidly; in both treatments the outer Mg layer had been dissolved during pretreatment.
Mössbauer spectroscopy analyses of DFOB-altered and blank-altered fibers + 3 μmol g− 1 57Fe demonstrated that the absolute increase in tetrahedrally coordinated 57Fe content was more than 5 times larger when added to DFOB-altered fibers compared to blank-altered fibers (Additional file 1: Table S7). However, assuming that no isotope exchange occurred, the data imply that only a small fraction of the Fe3+tet sites depleted by DFOB were recovered by 57Fe additions.
Despite the apparently low recovery of depleted vacancy sites as observed by Mössbauer spectroscopy, the interaction of Fe with DFOB-altered fibers re-stabilized the labilized Si layer, reduced the Si dissolution rate, and consequently also reduced the Mg dissolution rate (Fig. 3, panel b1 and b2). The 25% reduction in Si and Mg dissolution rate by addition of only 3 μmol g− 1 Fe and the fact that Fe addition beyond 30 μmol g− 1 did not lead to a further decrease in dissolution rates, supports that the effect of Fe addition originates from the stabilization of the Si layer rather than from surface coverage by precipitated Fe (hydr)oxide minerals that prevent dissolution. The latter observation also suggests that between addition of 3 and 30 μmol g− 1 Fe, all vacancy sites became occupied with tetrahedrally coordinated Fe and further Fe addition did not affect dissolution rates. The absence of similar trends in Si and Mg dissolution for Fe addition to blank-altered fibers further indicates that external Fe only becomes tetrahedrally coordinated if there are vacancy sites present in the surface Si layer (Fig. 3, Panel c1 and c2).
Active sites of H2O2 decomposition on chrysotile surfaces
At pH 7.4, the H2O2 decomposition rate (Fig. 4a) (as well as the HO• yield (Fig. 5)) was highest in the treatment with pristine fibers. This is presumably related to a (transient) contribution from Fe in the outermost Mg layer, which dissolves within a few days at this pH. In the treatment with NaOH the Mg layer did not dissolve at all (Additional file 1: Table S8) and the lasting contribution from Fe in this layer may in part explain the higher H2O2 decomposition rate.
In addition to two Fe-related modes of H2O2 decomposition by chrysotile, a third, remnant mode was identified (Fig. 4a and b), which, to our knowledge, had not yet been described for asbestos. It made the largest contribution to the ktot of blank-altered fibers in our experiments (Table 3) and may also be relevant in vivo. Magnetite impurities in the Shijiazhuang chrysotile that do not dissolve during the DFOB pretreatment may contribute to the remnant H2O2 decomposition mode. H2O2 is more rapidly decomposed by magnetite than by asbestos per unit of mass , but magnetite is only a phase contaminant in Shijiazhuang chrysotile asbestos (1.5 ± 0.2%), whereas chrysotile is the predominant phase (86.4 ± 4.6%) . Therefore, we assume that the contribution of magnetite to H2O2 decomposition rates is small. Furthermore, other substituted metal ions (e.g. Cr, Mn, Ni) that are not or only slowly mobilized by DFOB might have contributed to the remnant H2O2 decomposition mode. And finally, the contribution from small amounts of remnant Fe that were either not mobilized by DFOB during the pretreatment or that became exposed during the H2O2 decomposition experiments as a result of Mg and Si dissolution is counted towards the remnant decomposition mode.
In spite of the smaller surface concentration of Fe3+tet in blank-altered fibers relative to octahedral Fe which had precipitated as Fe (hydr)oxide minerals, their contributions to H2O2 decomposition were comparable (Table 3). Several factors may contribute to the comparatively large contribution of Fe3+tet per mole Fe. First, only a fraction of the Fe in Fe precipitates resides at the mineral surface and is able to react with H2O2, whereas all tetrahedral Fe substituted into the exposed Si layer can contribute to H2O2 decomposition. Secondly, in other silicate minerals like nontronites, it has been shown that Fe3+tet is preferentially reduced over octahedral Fe [55,56,57] suggesting a lower redox potential of Fe3+tet in silicate minerals. This lower redox potential may contribute to a higher reactivity of Fe3+tet with regard to H2O2 decomposition. Also for Fe (hydr)oxide minerals, it has been demonstrated that for equal masses the H2O2 decomposition rates were larger for minerals containing Fe3+tet, like magnetite (even higher than chrysotile), than for minerals that do not contain Fe3+tet, like hematite .
Similarly to H2O2 decomposition, a much higher reactivity with respect to the HO• yield was observed for tetrahedral Fe than for octahedral Fe precipitates. The reason for the high redox reactivity of Fe3+tet in silicates (and potentially Fe (hydr)oxide minerals) has, to our knowledge, not yet been examined.
Active sites of HO• generation by structural and external Fe on chrysotile surfaces
Contrary to Fe addition to blank-altered fibers, Fe addition to DFOB-altered fibers clearly increased HO• generation by chrysotile (Fig. 5a). Since DFOB-altered fibers were significantly depleted in Fe3+tet sites, this suggests that upon Fe addition, Fe was incorporated into vacancy sites in the Si layer of DFOB-altered fiber surfaces where it became tetrahedrally coordinated and particularly active in HO• generation. It should be noted, however, that Mössbauer data seem to indicate that addition of 3 μmol g− 1 57Fe only resulted in a small increase of Fe3+tet; only 3.0% of the Fe3+tet removed in the DFOB pretreatment was recovered through Fe addition. HO• generation, however, recovered to a substantially larger extent by 3 μmol g− 1 Fe addition: 10 percentage points relative to untreated fibers, corresponding to 19% of the difference between the blank-altered + 0 μmol g− 1 Fe treatment (with the pristine Fe3+tet content) and the DFOB-altered + 0 μmol g− 1 Fe treatment (with Fe3+tet mostly depleted).
The limited recovery of Fe3+tet by 3 μmol g− 1 57Fe addition may be related to the observed enhanced Si dissolution, possibly creating vacancy sites in the Si layer and subsequent edge pit formation. Edge pit formation would make the sites unsuitable for accommodating Fe3+tet coordination when the 57Fe was added. However, the factor six discrepancy between recovered Fe3+tet and recovered HO• generation seems to indicate that recovered Fe3+tet sites may be underestimated by Mössbauer data. Indeed, the recovery of Fe3+tet sites was calculated under the assumption that no Fe-isotope exchange occurred in these sites over the timescales of the experiment. Considering the significant time gap between 57Fe addition and Mössbauer spectroscopy, it is conceivable that isotope exchange reactions did occur over the timescales of the experiment. In this case, we may have under-estimated the increase of Fe3+tet sites after addition of 57Fe. Finally, the reactivity of Fe3+tet sites regarding HO• generation may be heterogeneous as a result of differences in local coordination environment and the recovery of such sites may not be linearly related to the recovery of reactivity.
Blank-altered fibers do not have vacancy sites in the Si layer, and therefore addition of Fe did not lead to a clear increase in HO• yield. However, the HO• yield of the blank-altered + 0 μmol g− 1 Fe treatment, in which surface Fe3+tet was preserved, was still higher than the HO• yield of fibers from the DFOB-altered + 300 μmol g− 1 Fe treatment. This suggests fewer exposed Fe3+tet surface sites in the latter treatment, potentially as a result of a loss of vacancy sites due to ongoing dissolution of the Si layer.
Assuming that Fe addition to blank-altered fibers mainly lead to precipitation of Fe (hydr)oxide minerals, the lack of differences in HO• yield between blank-altered fiber treatments with different amounts of added Fe suggests that these Fe (hydr)oxide minerals do not contribute to HO• generation. This corresponds with results from previous studies: the HO• yield of hematite, which contains no Fe3+tet , was below the LOD in a study by Fubini et al. (1995) , while the HO• yield of magnetite, which does contain structural Fe3+tet , corresponded with 60% of the HO• yield of chrysotile asbestos on a per mass basis . The difference in reactivity between Fe3+tet and octahedral Fe was larger for HO• generation than for H2O2 decomposition.
The high Fenton reactivity of Fe3+tet in chrysotile may, analogously to H2O2 decomposition, be explained by the lower redox potential of Fe3+tet compared to octahedral Fe, as observed in nontronites [55,56,57], and a potentially rapid back-oxidation of the Fenton-active Fe2+tet to Fe3+tet by H2O2, yielding HO•. In contrast to Mg and Si mobilization and H2O2 decomposition, addition of 30 μmol g− 1 Fe to DFOB-altered fibers did not recover the HO• yield to the level of blank-altered fibers. For DFOB-altered fibers + 300 μmol g− 1 Fe the HO• yield (37 ± 14%) was still significantly lower than for blank-altered fiber + 0 μmol L− 1 treatment (58 ± 6%) (Fig. 5, Additional file 1: Table S5). This incomplete recovery of the Fenton reactivity when adding an excess of Fe may suggest a loss of vacancy sites during preconditioning e.g. due to edge pit formation, leading to a smaller number of Fe3+tet surface sites than in the blank-altered fiber treatment.
The results from this study demonstrate that both Fe3+oct in Fe (hydr)oxide precipitates and Fe3+tet contribute to H2O2 decomposition by chrysotile asbestos; for asbestos fibers incubated at pH 7.4 in absence of a ligand (blank-altered) the contributions of both Fe species were comparable (within a factor 1.5), despite the excess of octahedral sites. A remnant mode of H2O2 decomposition by chrysotile was identified, which may be related to magnetite impurities, redox active substituted trace metals not removed by DFOB during pretreatment and remnant Fe. HO• generation by chrysotile asbestos is likely governed by Fe3+tet; the contribution from Fe precipitates is negligible.
The occurrence of Fe3+tet in Fe (hydr)oxide minerals may also be correlated with their HO• yield and their H2O2 decomposition capacity. However, whereas Fe (hydr)oxide minerals are not pathogenic , many silicate minerals other than chrysotile are. In many pathogenic silicates Fe3+tet has been detected, e.g. in quartz, in amphiboles and in zeolites [59,60,61,62,63,64]. Even if these minerals do not contain Fe, our results demonstrate that the presence of vacancy sites in their Si lattice can pose a risk, because incorporation of external Fe into the tetrahedral coordination environment can lead to HO• generation. This may be particularly relevant for zeolites (e.g. erionite), which often have a non-detectable bulk Fe content, but a higher potential to induce mesothelioma than asbestos . The dissolution of tetrahedral Al (which is a stoichiometric constituent of framework silicates) may create abundant vacancy sites in the Si lattice of zeolite fibers, available for the incorporation of Fenton-active tetrahedrally coordinated Fe.
To conclude, our results suggest that Fe3+tet governs HO• generation by chrysotile at circumneutral pH, and that Fe3+tet may also contribute to the hazard of other pathogenic silicates.
Availability of data and materials
The datasets generated and/or analyzed during the current study are available in the supplementary information repository, https://doi.org/10.1186/s12989-019-0333-1. The dataset supporting the conclusions of this article is included within the article (and its additional file).
Analysis of variance
Brunauer, Emmet, Teller
- DMPO-HO• :
Adduct of DMPO and HO•
Electron paramagnetic resonance
- Fe2+ oct :
Ferrous octahedral Fe
- Fe2+ tet :
Ferrous tetrahedral Fe
- Fe3+ oct :
Ferric octahedral Fe
- Fe3+ tet :
Ferric tetrahedral Fe
Fe complexed by DFOB
Inductively coupled plasma mass spectrometry
Inductively coupled plasma optical emission spectrometry
Limit of detection
Neutron activation analysis
narrow velocity range
Rounds per minute
Specific surface area
- Turkeys HSD test:
Turkeys honestly significant difference test
Ultra violet and visible light
World health organization, international agency for research on cancer
wide velocity range
Catherine H, Skinner W. Mineralogy of asbestos minerals. Indoor Built Environ. 2003;12(6):385–9. https://doi.org/10.1177/1420326x03037003.
Hardy JA, Aust AE. Iron in asbestos chemistry and carcinogenicity. Chem Rev. 1995;95(1):97–118. https://doi.org/10.1021/cr00033a005.
Frank A. The History of the Extraction and Uses of Asbestos; 2005. p. 1–7. https://doi.org/10.1201/9781420038149.ch1.
Asbestos (chrysotile, amosite, crocidolite, tremolite, actinolite, and anthophyllite), IARC Monographs on the Evaluation of Carcinogenic Risks to Humans 100C, International Agency for Research on Cancer. 2012.
Olsen NJ, Franklin P, Reid A, Klerk N, Threlfall TJ, Shilkin K, et al. Increasing incidence of malignant mesothelioma after exposure to asbestos during home maintenance and renovation. Med J Australia. 2011;195:271–4. https://doi.org/10.5694/mja11.10125.
Baur X. Asbestos: socio-legal and scientific controversies and unsound science in the context of the worldwide Asbestos tragedy - lessons to be learned. Pneumologie. 2016;70(6):405–12. https://doi.org/10.1055/s-0042-103580.
Kamp DW, Weitzman SA. The molecular basis of asbestos induced lung injury. Thorax. 1999;54(7):638–52. https://doi.org/10.1136/thx.54.7.638.
WHO-IARC. Arsenic, metals, fibres and dusts. IARC monographs on the evaluation of carcinogenic risks to humans, vol. 100 C; 2012. p. 219–94.
WHO, International programme on chemical safety: Chrysotile asbestos, ISBN: 978 92 4 156481 6. 2014.
Nishikawa K, Takahashi K, Karjalainen A, Wen CP, Furuya S, Hoshuyama T, et al. Recent mortality from pleural mesothelioma, historical patterns of Asbestos use, and adoption of bans: a global assessment. Environ Health Perspect. 2008;116(12):1675–80. https://doi.org/10.1289/ehp.11272.
Le GV, Takahashi K, Park EK, Delgermaa V, Oak C, Qureshi AM, et al. Asbestos use and asbestos-related diseases in Asia: past, present and future. Respirology. 2011;16(5):767–75. https://doi.org/10.1111/j.1440-1843.2011.01975.x.
Nicholson WJ. The carcinogenicity of chrysotile asbestos - a review. Ind Health. 2001;39(2):57–64. https://doi.org/10.2486/indhealth.39.57.
Landrigan PJ. Asbestos - Still a carcinogen. N Engl J Med. 1998;338(22):1618–9. https://doi.org/10.1056/nejm199805283382209.
Bales RC, Morgan JJ. Surface-charge and adsorption properties of chrysotile asbestos in natural-waters. Environ Sci Technol. 1985;19(12):1213–9. https://doi.org/10.1021/es00142a013.
Evans BW. The serpentinite multisystem revisited: Chrysotile is metastable. Int Geol Rev. 2004;46(6):479–506. https://doi.org/10.2747/0020-68220.127.116.119.
Bowes DR, Farrow CM. Major and trace element compositions of the UICC standard asbestos samples. Am J Ind Med. 1997;32(6):592–4. https://doi.org/10.1002/(sici)1097-0274(199712)32:6<592::aid-ajim3>3.0.co;2-s.
Ristic M, Czako-Nagy I, Music S, Vertes A. Spectroscopic characterization of chrysotile asbestos from different regions. J Mol Struct. 2011;993(1–3):120–6. https://doi.org/10.1016/j.molstruc.2010.10.005.
Stroink G, Blaauw C, White CG, Leiper W. Mössbauer characteristics of UICC* standard reference asbestos samples. Can Mineral. 1980;18:285–90 <Go to ISI>://WOS:000208518700004.
Gronow JR. The dissolution of asbestos fibers in water. Clay Miner. 1987;22(1):21–35. https://doi.org/10.1180/claymin.1987.022.1.03.
Bales RC, Morgan JJ. Dissolution kinetics of chrysotile at pH=7 to 10. Geochim Cosmochim Acta. 1985;49(11):2281–8. https://doi.org/10.1016/0016-7037(85)90228-5.
Walter M, Schenkeveld WDC, Reissner M, Gille L, Kraemer SM. The Effect of pH and Biogenic Ligands on the Weathering of Chrysotile Asbestos: The Pivotal Role of Tetrahedral Fe in Dissolution Kinetics and Radical Formation. Chem Eur J. 2019;25:3386. https://doi.org/10.1002/chem.201804319.
Mossman BT, Churg A. Mechanisms in the pathogenesis of asbestosis and silicosis. Am J Respir Crit Care Med. 1998;157(5):1666–80.
Churg A. Deposition and clearance of chrysotile asbestos. Ann Occup Hyg. 1994;38(4):625–33. https://doi.org/10.1093/annhyg/38.4.625.
Winterbourn CC. Toxicity of iron and hydrogen peroxide: The Fenton reaction. Toxicol Lett. 1995;82:969–74. https://doi.org/10.1016/0378-4274(95)03532-x.
Kamp DW, Graceffa P, Pryor WA, Weitzman SA. The role of free-radicals in asbestos-induced diseases. Free Radic Biol Med. 1992;12(4):293–315. https://doi.org/10.1016/0891-5849(92)90117-y.
Gazzano E, Turci F, Foresti E, Putzu MG, Aldieri E, Silvagno F, et al. Iron-loaded synthetic chrysotile: a new model solid for studying the role of iron in asbestos toxicity. Chem Res Toxicol. 2007;20(3):380–7. https://doi.org/10.1021/tx600354f.
Fenoglio I, Prandi L, Tomatis M, Fubini B. Free radical generation in the toxicity of inhaled mineral particles: the role of iron speciation at the surface of asbestos and silica. Redox Rep. 2001;6(4):235–41. https://doi.org/10.1179/135100001101536382.
Haber F, Weiss J. Über die Katalyse des Hydroperoxydes. Naturwissenschaften. 1932;20(51):948–50.
De Laat J, Gallard H. Catalytic decomposition of hydrogen peroxide by Fe (III) in homogeneous aqueous solution: mechanism and kinetic modeling. Environ Sci Technol. 1999;33(16):2726–32. https://doi.org/10.1021/es981171v.
Eberhardt MK, Román-Franco AA, Quiles MR. Asbestos-induced decomposition of hydrogen peroxide. Environ Res. 1985;37(2):287–92. https://doi.org/10.1016/0013-9351(85)90108-2.
Fubini B, Mollo L, Giamello E. Free-radical generation at the solid/liquid interface in iron-containing minerals. Free Radic Res. 1995;23(6):593–614. https://doi.org/10.3109/10715769509065280.
Ghio A, Taylor DE, Stonehuerner JG, Piantadosi CA, Crumbliss AL. The release of iron from different asbestos structures by hydrogen peroxide with concomitant O2 generation. Biometals. 1998;11/1:41–7. https://doi.org/10.1023/A:1009257323963.
Weitzman SA, Graceffa P. Asbestos catalyzes hydroxyl and superoxide radical generation from hydrogen-peroxide. Arch Biochem Biophys. 1984;228(1):373–6. https://doi.org/10.1016/0003-9861(84)90078-x.
Ghio AJ, Kennedy TP, Stonehuerner JG, Crumbliss AL, Hoidal JR. DNA strand breaks following in-vitro exposure to asbestos increase with surface complexed Fe3+. Arch Biochem Biophys. 1994;311(1):13–8. https://doi.org/10.1006/abbi.1994.1202.
Ghio AJ, Kennedy TP, Whorton AR, Crumbliss AL, Hatch GE, Hoidal JR. Role of surface complexed iron in oxidant generation and lung inflammation induced by silicates. Am J Phys. 1992;263(5):L511–L8.
Ghio AJ, LeFurgey A, Roggli VL. In vivo accumulation of iron on crocidolite is associated with decrements in oxidant generation by the fiber. J Toxicol Environ Health. 1997;50(2):125–42.
Fubini B, Mollo L. Role of iron in the reactivity of mineral fibers. Toxicol Lett. 1995;82–3:951–60. https://doi.org/10.1016/0378-4274(95)03531-1.
Aust AE, Cook PM, Dodson RF. Morphological and chemical mechanisms of elongated mineral particle toxicities. J Toxicol Environ Health-Part B-Crit Rev. 2011;14(1–4):40–75. https://doi.org/10.1080/10937404.2011.556046.
Kandegedara A, Rorabacher DB. Noncomplexing tertiary amines as “better” buffers covering the range of pH 3–11. Temperature dependence of their acid dissociation constants. Anal Chem. 1999;71 15:3140–4. https://doi.org/10.1021/ac9902594.
Doulias PT, Christoforidis S, Brunk UT, Galaris D. Endosomal and lysosomal effects of desferrioxamine: protection of HeLa cells from hydrogen peroxide-induced DNA damage and induction of cell-cycle arrest. Free Radic Biol Med. 2003;35(7):719–28. https://doi.org/10.1016/s0891-5849(03)00396-4.
Geroldinger G, Tonner M, Hettegger H, Bacher M, Monzote L, Walter M, et al. Mechanism of ascaridole activation in Leishmania. Biochem Pharmacol. 2017;132:48–62. https://doi.org/10.1016/j.bcp.2017.02.023.
ThomasArrigo LK, Mikutta C, Byrne J, Kappler A, Kretzschmar R. Iron (II)-catalyzed Iron atom exchange and mineralogical changes in Iron-rich organic freshwater Flocs: an Iron isotope tracer study. Environ Sci Technol. 2017;51(12):6897–907. https://doi.org/10.1021/acs.est.7b01495.
Stookey LL. Ferrozine---a new spectrophotometric reagent for iron. Anal Chem. 1970;42(7):779–81. https://doi.org/10.1021/ac60289a016.
Reay A. The effect of disk mill grinding on some rock-forming minerals. Mineral Mag. 1981;44(334):179–82. https://doi.org/10.1180/minmag.1981.044.334.10.
Mørup S, Both E. Interpretation of Mossbauer-spectra with broadened lines. Nucl Inst Methods. 1975;124(2):445–8. https://doi.org/10.1016/0029-554x(75)90595-9.
Murad E, Schwertmann U. The Mössbauer spectrum of ferrihydrite and its relations to those of other iron-oxides. Am Mineral. 1980;65(9–10):1044–9.
Eisenberg GM. Colorimetric determination of hydrogen peroxide. Ind Eng Chem-Anal Ed. 1943;15:327–8. https://doi.org/10.1021/i560117a011.
Zhao GH, Chasteen ND. Oxidation of Good's buffers by hydrogen peroxide. Anal Biochem. 2006;349(2):262–7. https://doi.org/10.1016/j.ab.2005.10.005.
Dominguez-Vera JM. Iron (III) complexation of Desferrioxamine B encapsulated in apoferritin. J Inorg Biochem. 2004;98(3):469–72. https://doi.org/10.1016/j.jinorgbio.2003.12.015.
Machala Z, Tarabova B, Hensel K, Spetlikova E, Sikurova L, Lukes P. Formation of ROS and RNS in Water Electro-Sprayed through Transient Spark Discharge in Air and their Bactericidal Effects: Formation of ROS/RNS in Water Sprayed through Spark in Air. Plasma Process Polym. 2013;10(7):649–59.
Favero-Longo S, Turci F, Tomatis M, Compagnoni R, Piervittori R, Fubini B. The effect of weathering on Ecopersistence, reactivity, and potential toxicity of naturally occurring Asbestos and Asbestiform minerals. J Toxicol Environ Health-Part A-Curr Issues. 2009;72(5):305–14. https://doi.org/10.1080/15287390802529864.
Turci F, Favero-Longo SE, Tomatis M, Martra G, Castelli D, Piervittori R, et al. A biomimetic approach to the chemical inactivation of chrysotile fibres by lichen metabolites. Chem Eur J. 2007;13(14):4081–93. https://doi.org/10.1002/chem.200600991.
Schwertmann U, Cornell RM. Iron oxides in the laboratory. 2., completely rev. and extended ed. edn. Weinheim: Wiley-VCH; 2000.
Murad E, Cashion J. Mössbauer spectroscopy of environmental materials and their industrial utilization; 2004.
Russell JD. Infrared and Mössbauer Studies of Reduced Nontronites. Clay Clay Miner. 1979;27(1):63–71. https://doi.org/10.1346/CCMN.1979.0270108.
Jaisi DP, Kukkadapu RK, Eberl DD, Dong H. Control of Fe (III) site occupancy on the rate and extent of microbial reduction of Fe (III) in nontronite. Geochim Cosmochim Acta. 2005;69(23):5429–40. https://doi.org/10.1016/j.gca.2005.07.008.
Merola RB, McGuire MM. Crystallographic site distribution and redox activity of Fe in nontronites determined by optical spectroscopy. Clay Clay Miner. 2009;57(6):771–8. https://doi.org/10.1346/CCMN.2009.0570609.
Steinhoff D, Mohr U, Hahnemann S. Carcinogenesis studies with iron oxides. Exp Pathol. 1991;43(3):189–94. https://doi.org/10.1016/S0232-1513(11)80116-7.
Roquemalherbe R, Diazaguila C, Regueraruiz E, Fundoralliteras J, Lopezcolado L, Hernandezvelez M. The state of iron in natural zeolites - a Mossbauer study. Zeolites. 1990;10(7):685–9. https://doi.org/10.1016/0144-2449(90)90080-b.
Di Benedetto F, D'Acapito F, Fornaciai G, Innocenti M, Montegrossi G, Pardi LA, et al. A Fe K-edge XAS study of amethyst. Phys Chem Miner. 2010;37(5):283–9. https://doi.org/10.1007/s00269-009-0332-0.
Weil JA. EPR of iron centers in silicon dioxide. Appl Magn Reson. 1994;6(1–2):1–16. https://doi.org/10.1007/BF03162478.
Dennen WH. Stoichiometric substitution in natural quartz. Geochim Cosmochim Acta. 1966;30 12:1235. https://doi.org/10.1016/0016-7037(66)90122-0.
Goldfarb D, Strohmaier KG, Vaughan DEW, Thomann H, Poluektov OG, Schmidt J. Studies of framework iron in zeolites by pulsed ENDOR at 95 GHz. J Am Chem Soc. 1996;118(19):4665–71. https://doi.org/10.1021/ja953903e.
Luys M-J, De Roy GL, Adams F, Vansant EF. Cation site population in amphibole asbestos. A Mossbauer study. J Chem Soc Faraday Trans. 1983;79 6:1451–9. https://doi.org/10.1039/F19837901451.
The authors would like to thank Dip.-Ing. Herwig Lenitz BSc and Ing. Wolfgang Obermaier for technical support, Dr. Carolina Reyes, Dr. Jerry van Dijk and Dr. Angeles Garcia Mayor for their help with the statistical analysis and Kyounglim Kang MSc for the synthesis of the 2-line ferrihydrite.
This research was funded by an uni:docs scholarship of the University of Vienna.
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Additional file1: Figure S1. Wide velocity range Mössbauer spectra of DFOB-altered fibers (Panel a and c) and blank-altered fibers (Panel b and d) with 0 or 3 μmol g− 1 added 57Fe. Figure S2. Preconditioned fibers. Panel a.) From left to right: blank-altered fibers + 0 μmol g− 1 Fe, blank-altered fibers + 3 μmol g− 1 Fe, blank-altered fibers + 30 μmol g− 1 Fe and blank-altered fibers + 300 μmol g− 1 Fe; Panel b.) Fiber preparation for Mössbauer analyses, from left to right: blank-altered fibers + 3 μmol g− 1 57Fe, blank-altered fibers + 0 μmol g− 1 57Fe, DFOB-altered fibers + 0 μmol g− 1 57Fe, blank-altered fibers + 3 μmol g− 1 57Fe. Table S1. Mobilized Mg, Si and Fe concentrations in μmol L− 1 during pretreatment (no duplicates available). Table S2. Mössbauer hyperfine parameters of DFOB-altered and blank-altered fibers + 0 or 3 μmol g− 1 57Fe, analyzed in the narrow (Table a) and the wide (Table b) velocity range. The Fe species distributions were calculated from both the wide and the narrow velocity range data combined (see materials and methods) and are presented in Table c. Table S3. Mobilized Mg and Si concentrations from 1 g L− 1 pristine, DFOB-altered and blank-altered fibers incubated at pH 7.4 (50 mM MOPS) with addition of 3.34 g L− 1 H2O2. Table S4. Residual H2O2 concentrations during H2O2 decomposition by pristine fibers, DFOB-altered fibers, blank-altered fibers and the MOPS buffer as a function of time. Table S5. HO• yield of DFOB-altered and blank-altered fibers relative to pristine fibers (i.e. 100%). Table S6. Results from the statistical analysis of the EPR spin trapping data presented in Fig. 5: p-values from the univariate general linear model and Tukey post-hoc test procedure. Table S7. Changes in 57Fe and total Fe speciation upon addition of 3 μmol g− 1 57Fe to blank-altered and DFOB-altered chrysotile at pH 7.4, as determined by Mössbauer spectroscopy. Table S8. Mobilized Mg and Si concentrations from 1 g L− 1 pristine and blank altered fibers incubated in a 0.1 mol L− 1 NaOH solution with addition of 3.34 g L− 1 H2O2.
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Walter, M., Schenkeveld, W.D.C., Geroldinger, G. et al. Identifying the reactive sites of hydrogen peroxide decomposition and hydroxyl radical formation on chrysotile asbestos surfaces. Part Fibre Toxicol 17, 3 (2020). https://doi.org/10.1186/s12989-019-0333-1
- Hydroxyl radical
- Tetrahedral iron