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Article

Influence of Water Salinity on the Efficiency of Fe0-Based Systems for Water Treatment

by
Ran Tao
1,
Xuesong Cui
1,
Minhui Xiao
1,2,
Rui Hu
2,
Willis Gwenzi
3,4,
Hans Ruppert
5 and
Chicgoua Noubactep
1,6,7,8,*
1
Applied Geology, University of Göttingen, Goldschmidtstraße 3, D-37077 Göttingen, Germany
2
School of Earth Science and Engineering, Hohai University, Fo Cheng Xi Road 8, Nanjing 211100, China
3
Grassland Science and Renewable Plant Resources, Faculty of Organic Agricultural Science, University of Kassel, Steinstrasse 19, D-37213 Witzenhausen, Germany
4
Leibniz Institute for Agricultural Engineering and Bioeconomy (ATB), Max-Eyth-Alle 100, D-14469 Potsdam, Germany
5
Department of Sedimentology & Environmental Geology, University of Göttingen, Goldschmidtstraße 3, D-37077 Göttingen, Germany
6
Department of Water and Environmental Science and Engineering, Nelson Mandela African Institution of Science and Technology, Arusha P.O. Box 447, Tanzania
7
Faculty of Science and Technology, Campus of Banekane, Université des Montagnes, Bangangté P.O. Box 208, Cameroon
8
Centre for Modern Indian Studies (CeMIS), Universität of Göttingen, Waldweg 26, D-37073 Göttingen, Germany
*
Author to whom correspondence should be addressed.
Water 2023, 15(13), 2466; https://doi.org/10.3390/w15132466
Submission received: 2 June 2023 / Revised: 26 June 2023 / Accepted: 3 July 2023 / Published: 5 July 2023
(This article belongs to the Section Wastewater Treatment and Reuse)
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Abstract

:
Metallic iron (Fe0) is a reactive material for treating polluted water. The effect of water salinity on the efficiency of Fe0-based remediation systems is not yet established. This work aims to clarify the reasons why Cl− ions are often reported to improve the efficiency of Fe0/H2O remediation systems. Quiescent batch experiments were carried out to characterize the effect of chloride (Cl−) ions on the efficiency of methylene blue (MB) discoloration in the presence of Fe0. Cl− was used in the form of NaCl at concentrations ranging from 0 to 40 g L−1. The MB concentration was 10 mg L−1, the Fe0 loading was 5 g L−1, and the duration of the experiment varied from 2 to 46 days. Four different Fe0 materials were tested in parallel experiments. Tests with different NaCl levels were performed in parallel with three other organic dyes: Methyl orange (MO), orange II (OII), and reactive red 120 (RR 120). The results clearly show that the presence of Cl− reduces the extent of dye discoloration in all systems investigated. The efficiency of the dyes increased in the order MB < MO < RR 120 < OII. In systems with varying NaCl concentrations, dye discoloration initially decreases with increasing NaCl and slightly increases for [NaCl] > 30 g L−1. However, the extent of dye discoloration for [NaCl] = 40 g L−1 remains much lower than for the system with [NaCl] = 0 g L−1. The results clearly demonstrate that the presence of Cl− fundamentally delays the process of contaminant removal in Fe0/H2O systems, thus improving the understanding of the contaminant interactions in Fe0-based remediation systems. These results also suggest that the effects of other inorganic anions on the efficiency of Fe0/H2O systems should be revisited for the design of field applications.

1. Introduction

Population growth and climate change are causing freshwater resources to decline worldwide [1,2]. The situation is exacerbated in coastal regions where seawater intrusion occurs as a result of unsustainable water management strategies [3,4]. In cities, poor planning and weather forecasting also contribute to sewage pollution [5,6]. To address the issue of water scarcity, preventing water pollution and treating and reusing wastewater are becoming increasingly important everywhere [5,6]. In this context, the need for affordable, applicable, but efficient technology cannot be overemphasized, particularly for low-income communities [7,8]. The use of metallic iron (Fe0) in water treatment systems is one such an affordable technology that has been shown to be highly efficient for decentralized and safe drinking water supplies [7] and wastewater treatment [8]. However, the effect of water salinity on the efficiency of Fe0/H2O remediation systems has not yet been adequately addressed [9,10].
Metallic iron (Fe0), as a reactive material, has been tested and used extensively within the water treatment industry over the last three decades [11,12,13,14,15,16,17,18,19,20,21,22,23]. The discovery of Fe0-based permeable reactive barriers (Fe0 PRBs) in the early 1990s was the starting point for intensive research, the results of which have been documented in several thousand scientific publications [16,24,25,26,27]. However, despite these efforts, the fundamental mechanistic understanding of the processes controlling the efficiency of Fe0-based remediation systems is not well-established [21,28,29,30,31,32]. In other words, there is still no scientific consensus on how to design a sustainable Fe0 PRB [21,28,30,31,32,33,34].
Despite conflicting reports in the literature, all researchers would agree with the following statement by Matheson and Tratnyek [35], describing the importance of mechanistic understanding in system design: “The effective design and operation of these systems will be improved by a more detailed process-level understanding of iron/contaminant interactions in porous media”. The results of these authors suggest that Fe0 exchanges electrons with dissolved contaminants or that contaminant reduction is a cathodic reaction coupled with the simultaneous oxidative dissolution of Fe0 (anodic reaction). Several research groups did not confirm these findings [36,37,38,39,40,41]. The most prominent example is certainly Jiao et al. [40] who, using the same species (e.g., CCl4), elegantly demonstrate that Fe0 plays no role in the process of CCl4 reductive transformation in the Fe0/H2O system. Later, Ebelle et al. [42] showed that the experimental conditions of Matheson and Tratnyek [35] were not suitable for them to draw their main conclusions. A number of papers have shown that the view that Fe0 is a reducing agent is based on results from inappropriate experimental conditions [13,17,30,33,43,44,45]. For example, experimental conditions (e.g., shaking, stirring) that prevent the diffusive transport of contaminants near the Fe0 surface give reproducible results in the laboratory but are not relevant for Fe0 PRBs in the field [13,18,28,30,45,46,47,48,49].
Apparently, none of the arguments presented over the past 15 years have convinced the majority of active researchers to question their approach and argumentation [21,31,32,48,49]. One promising approach is the so-called MB method, which characterizes the extent of Fe0 corrosion by monitoring the extent of methylene blue (MB) discoloration in a Fe0/sand/H2O system [50,51,52,53,54]. MB discoloration cannot be attributed to any redox reactivity within the Fe0/sand/H2O system but results from (i) adsorption on sand and (ii) co-precipitation with in situ generated iron corrosion products (FeCPs) [50,55]. In other words, by varying (i) the amounts of Fe0 and/or sand or (ii) the type of Fe0 in a Fe0/sand/H2O system, a number of parameters can be investigated, as MB discoloration correlates well with the extent of Fe0 oxidation and/or the extent of generation of free FeCPs for (i) MB co-precipitation or (ii) sand surface coating. The sand surface coated with FeCPs is not a good adsorbent for MB [50,52,53,54,55]. The MB method is used here to characterize the effects of salinity (NaCl) on the efficiency of the Fe0/H2O system.
Several studies have investigated the effects of solution chemistry on the performance of Fe0/H2O systems [9,10,56,57,58,59,60,61,62]. In the words of Sun et al. [63], understanding such effects “will provide opportunities to assess the feasibility of this technology and to adapt the engineering design to site-specific conditions”. However, with the exception of chloride, no general conclusions can be drawn because the systems investigated were limited to specific contaminants or groups of contaminants [10,63]. For chlorides, an enhancing effect on decontamination in Fe0/H2O systems has generally been reported [56,59,60,63,64]. This suggests that Fe0/H2O systems would work well in natural saline waters containing up to 40 g/L NaCl (e.g., fracturing wastewater, groundwater, industrial wastewater, reverse osmosis concentrates) [29,65,66,67]. This conclusion contradicts the evidence that contaminants are removed from the aqueous solution by iron oxidhydroxides (iron corrosion products—FeCPs). In fact, when Fe0 is dissolved by water (Equation (1)), the generated Fe2+ and Fe3+ ions primarily form relatively soluble chlorocomplexes salts (e.g., FeCl2, FeCl3) or low soluble oxidhydroxides, such as Fe(OH)2, Fe(OH)3 (Equation (2)—not stoichiometric) [48,49,68,69]. Equation (1) shows that Fe0 corrosion consumes H+ (or produces OH−) and thus increases the pH of the system. Increasing the pH value favors the precipitation of Fe hydroxides (Equation (2)).
Fe0 + 2 H+ ⇛ Fe2+ + H2
Fe2+ and Fe3+ ⇛ Fe salts + Fe hydroxides
Equations (1) and (2) suggest that, if used Fe0 produces dissolved Fe2+ and Fe3+ ions in stoichiometric abundance relative to available Cl−, hydroxides will begin to form as Cl− is depleted (Equation (2)). Clearly, contaminant removal in Fe0/H2O systems should be delayed in the presence of Cl− (working hypothesis). This is the opposite of what has typically been reported over the years [59,60,63,64]. Therefore, the reasons for Cl−-enhanced decontamination in Fe0/H2O systems remain to be elucidated.
This research characterizes the effects of chloride ions on MB discoloration in Fe0/H2O systems by testing the validity of the working hypothesis (“the presence of Cl− delays contaminant removal in Fe0/H2O systems”). Accompanying experiments are carried out with three other organic dyes (methyl orange, orange II, and reactive red 120). The results will be discussed comparatively. This research will provide more information for the actual application of Fe0/H2O systems. It is expected that the research will provide more information for the actual application of Fe0/H2O systems for saltwater remediation.

2. Material and Methods

2.1. Solutions

2.1.1. Dye Solutions

The used reagents methylene blue (MB—Basic Blue 9 from Merck, Darmstadt, Germany), methyl orange (MO—from Merck, Darmstadt, Germany), reactive red 120 (RR 120—from SIGMA company, Taufkirchen, Germany), and orange II (OII—from ACROS Organics, Geel, Belgium) were all of analytical grade. The physico-chemical characteristics of the four dyes are summarized in Table 1. The working solution for each dye was 10 mg L−1. The MB solutions were prepared by diluting a stock solution of 1000 mg L−1. The other three dye solutions were prepared by dissolving accurately weighed corresponding materials in tap water. Table salt from a local supermarket of Kaufland, Germany was used as the NaCl source. Weighed table salt was dissolved in tap water to prepare the working solutions. The Cl− concentration of the tap water was considered as part of the background electrolyte (operational reference). The average composition of this water is (mg L−1): Cl−: 9.7; NO3−: 7.7; SO42−: 30.0; HCO3−: 88.5; Na+: 6.0; K+: 0.5; Mg2+: 7.3; Ca2+: 32.6, and its initial pH was 8.3.

2.1.2. Solid Materials

Metallic Iron (Fe0)

A total of 4 commercially available Fe0 materials were selected and used in this study. The selection was based on their differential reactivity as determined in previous work [34]. The Fe0 materials used were of different geometric shapes and sizes. These Fe0 materials are referred to as: (i) ZVI1 is a material from iPutec GmbH Rheinfelden, Rheinfelden, Germany: (ii) ZVI2 is a directly reduced sponge iron material (DRI) from ISPAT GmbH, Hamburg, Germany; (iii) ZVI3 is scrap iron from the metal recycling company Metallaufbereitung Zwickau, Zwickau, Germany; and (iv) ZVI4 is a spherical iron sample from the Tongda Alloy Material Factory, Jinan, China. Table 2 summarizes the main characteristics of the 4 Fe0 materials together with their iron content, as specified by the supplier. ZVI1 has been typically used by our research group since 2005 and represents the most widely used Fe0 material for field applications in Europe [74]. Therefore, ZVI1 is used here as an operational reference.

Sand

The sand used in this work was a commercial material for aviculture (parrot sand) (“Papageien sand” from RUT—Lehrte, Germany). “Papageien sand” was used as received without any further pre-treatment or characterization. The particle size varied between 0.5 and 2.0 mm. Sand was considered in this study because of its worldwide availability and its use as an additive in Fe0/H2O systems [50,54]. The high adsorption capacity of sand for cationic MB was systematically documented as early as 1955 [55].

2.2. Experimental Procedure

Batch experiments were performed under static conditions (no agitation) in assay tubes for 2 to 46 days. The batches consisted of 0.0 to 0.5 g of sand, 0.0 to 0.5 g of Fe0, and mixtures thereof in 22.0 mL of a 10.0 mg L−1 of dye (MB, MO, OII, and RR 120) solution. Three different systems were investigated in parallel experiments for dye discoloration: (i) Fe0 alone, (ii) sand alone, and (iii) Fe0 + sand. The NaCl concentrations tested ranged from 0.0 to 40 g L−1, corresponding to 0 to 24.3 g L−1 Cl− (0 to 685 mM NaCl), without taking into account the Cl− content of tap water (0.011–0.015 g L−1). An operational reference (blank experiment) was included in each experiment. Mixtures with Fe0 characterize the effect of sand on the availability of “free” iron corrosion products and hence their effect on dye discoloration [54]. “Free” iron corrosion products are iron oxidhydroxides precipitating from the bulk solution and capable of fixing (enmeshing) contaminants [50]. The influence of different types of Fe0 (ZVI1—ZVI4) on MB discoloration was also investigated. An additional set of dye discoloration experiments with MB and MO was performed by varying the Fe0 loading (0.23 to 45 g L−1) for two months.
The efficiency of each system in discoloring dyes was characterized at laboratory temperature (approximatively 22 °C). The initial pH value of the tap water was ~8.3. After equilibration, up to 5.0 mL of the supernatant solution was carefully collected for spectrophotometric analysis. Each experiment was performed in triplicate. Results are presented as means with the standard deviations (error bars) as a measure of data dispersion.

2.3. Analytical Procedure

Aqueous dye concentrations were determined using a Cary 50 UV–Vis spectrophotometer (Cary instruments, LabMakelaar Benelux B.V., Zevenhuizen, The Netherlands). The working wavelengths for MB, MO, OII, and RR 120 were 664.5, 464.0, 486.0, and 515.0 nm, respectively (Table 1). Cuvettes with a 1.0 cm light path were used. The spectrophotometer was calibrated for dye concentrations ≤ 10.0 mg L−1. The pH value was measured with a combined glass electrode (WTW Co., Weinheim, Germany).

2.4. Expression of Experimental Results

In order to characterize the degree of dye discoloration of the tested systems, the treatment efficiency (E) was calculated (Equation (3)). After the determination of the residual dye concentration (C), the corresponding percentage discoloration (E value) was calculated as follows:
E = [1 − (C/C0)] × 100%
where C0 is the initial aqueous contaminant concentration (10.0 mg L−1 for each dye) and C is the corresponding concentration at the end of the experiment.

3. Results

3.1. Dye Discoloration in Fe0/H2O Systems

Figure 1 compares the extent of dye discoloration after 46 days under the experimental conditions: Quiescent batch tests with 4.5 g L−1 Fe0 and 20 g L−1 sand. It can be seen that MB had the least extent of discoloration (55%) while Orange II had the best performance with an E value of 70%. These results confirm previous reports and are justified by the cationic nature of MB compared to the three other dyes, which are anionic (Table 1) [75,76,77]. In fact, the surface of FeCPs is positively charged just like the MB molecule, whereas anionic dyes (MO, orange II, and RR 120) (Table 1) are negatively charged and are more attracted to FeCPs [78,79]. The different behavior of anionic dyes may be explained by steric effects [77,80], which are not considered here.
When discussing the results in Figure 1, it should be kept in mind that the contact time (duration 46 days) was chosen so that the MB adsorption on sand would have already reached a pseudo-equilibrium [54]. In other words, changes in dye concentrations reflect the availability of free iron corrosion products for (i) the adsorption and co-precipitation of anionic dyes and (ii) the co-precipitation of all dyes (MB in particular). Clearly, the results in Figure 1 are the starting point for investigating the effects of NaCl addition on the performance of the given Fe0/H2O systems for dye discoloration (Section 3.3).

3.2. Influence of Salt Concentration on MB Discoloration in Fe0/H2O Systems

Figure 2 compares the time-dependent extent of MB discoloration under the experimental conditions for three different NaCl concentrations: 0.0, 8.0, and 40.0 g L−1. It can be seen that for each contact time (i) MB discoloration is maximal in the NaCl free system (confirming the working hypothesis) and (ii) MB discoloration increases with increasing contact time. A closer look at the NaCl-containing systems shows that for t < 30 days, the 8 g L−1 NaCl system performed better than the 40 g L−1 system. Between 30 and 40 days, both systems performed similarly, and at t > 40 days, the 40 g L−1 NaCl system performed better than the 8 g L−1 system. However, both systems still performed lower than the NaCl-free system.
Figure 2 suggests that there is some ambivalence in the effects of Cl− on the performance of Fe0/H2O systems for water treatment. The first reason may be an overall decrease in performance due to the absence or a reduced availability of FeCPs for contaminant adsorption and co-precipitation. This is evident when comparing NaCl free and NaCl-containing systems. Second, for the two NaCl-containing systems, there is first a decrease correlated with the amount of NaCl, then a phase in which both systems show the same performance. As the duration of the experiment increases, a stage is reached where the system with the higher NaCl level performs better than the others. Although this improved performance is still lower than that of the NaCl-free system, these results suggest that the improved MB discoloration performance for the 40 g L−1 NaCl system corresponds to the often reported improved performance of Fe0/H2O systems in the presence of Cl− [59,60,64].
In this study, quiescent batch experiments in which diffusion transport is the dominant transport mechanism for dissolved species from the bulk solution to the vicinity of the Fe0 surface have revealed the fundamental effects of the presence of Cl− on the efficiency of Fe0/H2O systems for water treatment. Consistent with the chemistry of the system, Cl− ions form stable dissolved complexes with Fe2+ and Fe3+, delaying the formation of FeCPs for contaminant adsorption and/or co-precipitation. This observation clearly validates the working hypothesis: The presence of Cl− delays the removal of contaminants in Fe0/H2O systems.

3.3. Influence of Salt Concentration on Dye Discoloration in Fe0/H2O Systems

Figure 3 summarizes the extent of dye discoloration after 46 days as the NaCl concentration varied from 0 to 40 g L−1. It can be seen that the presence of Cl− ions inhibits the discoloration of all dyes. The first experimental point at 0 g L−1 NaCl corresponds to the discussion in Section 3.1 (Figure 1), where the dye discoloration decreased in the order: OII > MO > RR120 > MB. A monotonic decrease in E values with increasing NaCl concentration is then observed for [NaCl] < 30 g L−1, alongside a slight increase for [NaCl] = 40 g L−1. This ambivalent situation is similar to that observed in the time-dependent study with MB (Section 3.2) and is related to the relative amounts of Fe(II) and Fe(III) chlorocomplexes and the availability of FeCPs (Equation (2)). Taken together, the results presented in Figure 1 through 3 suggest that it is possible to properly design a Fe0-based remediation system that takes advantage of the enhanced iron corrosion in the presence of Cl− ions. However, this does not mean that Cl− ions generally increase the efficiency of Fe0/H2O systems. Similar results have been obtained with hybrid Fe0/aggregate systems, including Fe0/MnO2 [43,44,45,77,81], Fe0/pumice [18,82], and Fe0/sand [30,52,79,83]. In other words, designing a sustainable Fe0 remediation system in a saline environment requires a careful consideration of the balance between acceptable Cl− concentration and contaminant removal efficiency for each Fe0 material.

3.4. Influence of Fe0 Dosage on Dye Discoloration in Fe0/H2O Systems

Figure 4 summarizes the effect of 0.0 to 45.0 g L−1 Fe0 on the extent of MB and MO discoloration over 46 days. The percentage discoloration of both dyes increased with increasing Fe0 dosage, while the presence of salt (NaCl) typically reduced the extent of dye discoloration. The point at 0.0 g L−1 Fe0 (sand only) corresponds to the Fe0 free system in which dye discoloration is mediated solely by electrostatic interactions at the negatively charged sand surface [50,55]. Figure 4a shows that more than 20% of MB is discolored in the pure sand system, while there was no MO discoloration (E = 0%—Figure 4b). Another feature of Figure 4a is that the presence of salt reduces the extent of MB discoloration by sand. In the presence of Fe0, decrease MB discoloration is also due to the increased availability of Fe2+ and Fe3+ ions, which are concurrent with MB (also positively charged) for adsorption onto the sand surface [78].
For Fe0 dosages between 0 and 45 g L−1, there is an increase in dye discoloration efficiency with increasing iron dosage (Figure 4a,b). This is primarily due to the availability of more active binding sites as a result of continuous iron corrosion, which produces solid iron corrosion products (FeCPs) for dye adsorption and co-precipitation. However, the discoloration percentage for both dyes becomes almost constant for [Fe0] > 20.0 g L−1. This behavior suggests a “splitting effect of the concentration gradient” between FeCPs and dye molecules [84]. The different discoloration efficiencies of MB and MO as a function of the amount of FeCPs available are essentially due to differences in chemical structure, molecular size, and FeCPs–dye interactions [50,55,84].

3.5. Influence of Fe0 Type on Dye Discoloration in Fe0/H2O Systems

Figure 5 summarizes the extent of MB and discoloration after 46 days with four different Fe0 materials in tap water ([NaCl] = 0 g L−1) and in salt water ([NaCl] = 40 g L−1). It can be seen that for all the 4 Fe0 materials tested, the dye discoloration decreases in salt water compared to tap water, confirming the observations in Section 3.4 and further validating the working hypothesis.
For MB (Figure 5a), the most significant TW vs. SW variability between replicates was observed for ZVI1 (error bars), while the lowest was recorded for ZVI4. Considering the absolute values, the following increasing order of efficiency is observed: ZVI4 > ZVI3 > ZVI2 > ZVI1. This ranking confirms the information from the kAA values (Table 2), showing that ZVI4 is significantly less reactive than the other three materials [9]. Another feature of Figure 5a is that ZVI4 performed only slightly better than sand alone in SW and TW. Based on the information in Figure 5a, ZVI1 can be recommended as the most reactive material, while ZVI2 and ZVI3 are very close in their efficiency for MB discoloration. The results of MO discoloration (Figure 5b) confirm the trend observed in Figure 5a, with the exception that ZVI1 has a significantly lower efficiency in both TW and SW. While this difference is difficult to justify, the overall results reaffirm the importance of characterizing the diversity among the Fe0 materials of environmental interest [85,86].
Despite a growing interest in the applications of Fe0 for environmental remediation [14,22,23] and safe drinking water supply [87,88,89,90], little progress has been made in characterizing the variability in reactivity among Fe0 samples from different sources [19,34,86,91,92]. The most important lesson from Figure 5 is that the extent to which saltwater affects the performance of a Fe0/H2O system depends on the used Fe0 source used (Fe0 quality). In particular, one investigator using ZVI4 might conclude that Cl− ions have no effect on Fe0 efficiency, while a colleague working under similar conditions using ZVI1 or ZVI2 would come to a different conclusion. As discussed by several authors, the diversity of contaminants and Fe0 materials, as well as the lack of unified or standardized experimental procedures are the three most important factors hindering the progress of knowledge in the design of sustainable Fe0-based remediation systems [17,19,30,77,92].

4. Discussion

The results presented here clearly demonstrate that any Cl− addition hinders the process of contaminant removal in Fe0/H2O systems. The results clearly contradict published findings over the past 20 years which claim that Cl− addition typically enhances water treatment with granular Fe0 [59,64,86,93]. For example, Kim et al. [59] tested halide salts to sustain the Fe0 efficiency for explosive “degradation” and concluded that Fe0 PRBs “installed in aquifers with chloride-rich groundwater are likely to perform and maintain reactivity better than those installed in aquifers with low chloride concentrations”. Many other researchers have reached similar conclusions for chloride-rich wastewater [63,93,94,95]. The question is—how can both views be reconciled?
Since the first peer-reviewed publications on Fe0 for groundwater remediation in 1994 [35,96,97,98], researchers have been trying to solve the problem of avoiding or delaying Fe0 passivation, commonly referred to as “reactivity loss” [11,99,100]. An applicable solution has been the use of chlorides (e.g., NaCl, KCl) as pitting corrosion promoters to avoid or destroy the oxide layer formed on the Fe0 surface [64]. Avoiding, breaking, or eliminating these oxide scales allows for the full utilization of the reductive capacity of the Fe0 materials used, as predicted by the thermodynamics of the FeII/Fe0 redox couple (E0 = −0.44 V). Indeed, despite NaCl concentrations as high as 40 g L−1 (685 mM Cl−), no improvement in dye discoloration was observed here, even for MO and orange II, which are potentially reduced by Fe0 [76,80].
The addition of chloride (e.g., KCl, NaCl) to Fe0/H2O systems is generally regarded as the addition of a “corrosion promoter” to accelerate the degradation of contaminants during water treatment [59,93,101,102]. Hernandez et al. [93] theorized that corrosion promoters improve the performance of Fe0/H2O systems by (i) accelerating “electron generation” from Fe0, (ii) creating new reactive sites on the Fe0 surface during water treatment, and (iii) minimizing surface passivation. The results of their experiments with 0.3 mM and 3 mM Cl− for “TNT degradation” were considered a validation of their concept. Subsequent investigators have reached similar conclusions [59,102], so that it appears to be established that the well-documented corrosion-promoting effects of Cl− can be randomly exchanged for accelerated contaminant degradation in Fe0/Cl−/H2O systems. However, using nanoscale Fe0, Hwang et al. [54] clearly observed an inhibition of nitrate reduction in Fe0/H2O systems after the addition of NaCl. These authors explained their observations by chloride adsorption on the Fe0 surface, using NaCl concentrations of up to 12 g L−1 (205 mM Cl−). The present work used higher and lower NaCl concentrations (Table 3) but gave different reasons for the inhibition of the four probe substances.
Table 3 summarizes the experimental conditions of selected publications on the effects of NaCl on the performance of Fe0/H2O batch systems. It can be clearly seen that there is a large variability in the experimental parameters used. This includes: (i) the type of the Fe0 materials (mFe0, nFe0, composites), (ii) the Fe0 dosage (0 to 45 g L−1), (iii) the volume of the solution (5 to 1000 mL), (iv) the type of the contaminant and even its concentration (not shown), (v) the Cl− concentrations (0 to 685 mM), and (vi) the type and intensity of mixing. All of these parameters have been shown to individually significantly affect the remediation efficiency of Fe0/H2O systems [13,20,30,33,108,109]. However, their effects are interdependent, and it is almost impossible to assess the contribution of each parameter as a stand-alone variable. Table 3 shows that this study differs from others in two ways: (i) quiescent batch experiments were performed and (ii) the widest window of Cl− concentrations to date was tested. The latter aspect is very important, as Hwang et al. [64] rationalized the decrease in aqueous nitrate removal by nano-Fe0 by the higher Cl− content.
This study has not confirmed the different effects of Cl− depending on its concentration. Hwang et al. [64] reported that at low concentrations (0–3 g L−1 NaCl), the efficiency of the system decreased only during the initial reaction period and then “increased after a certain time”. The efficiency at high Cl− concentrations (3–20 g L−1) decreased significantly “due to the inhibition effect of the electrolyte”. This statement contradicts the electrochemistry of the system. In fact, in an electrochemical reaction, the contribution of the electrolyte is to modify the ionic transport of anodic species (here Fe2+) not to influence a cathodic reaction (electron transfer to NO3−). Accordingly, the results of Hwang et al. [64] explicitly refute the notion that nitrate reduction is mediated by any electrons of Fe0. In other words, the results presented here elegantly confirm that Fe0 is a generator of contaminant scavengers [33,53,54]. The presence of NaCl delays the precipitation of iron oxides and hydroxides, thus delaying the decontamination process. This was observed for all four dyes and at all NaCl concentrations. It is recalled that the dyes used have different redox affinities to Fe0 (E0 = −0.44 V) and different adsorptive affinities to positively charged iron corrosion products [110,111,112]. The discoloration results reflect only the difference in adsorptive adsorption affinity, confirming reports that Fe0/H2O systems are ion-selective [75,76,113].
The final important point is to explain why improved decontamination efficiency has been documented for some Fe0/H2O systems [64,114]. Fe0 would “passivate” earlier without Cl− addition. Due to the high solubility of Fe(II) and Fe(III) chlorides relative to iron hydroxides, Cl− addition sustains Fe0 corrosion and produces more contaminant scavengers because Fe0 is in large stoichiometric excess. All of these reactions are enhanced by mixing operations, such as shaking and stirring (Table 3). A similar situation has been reported for the addition of MnO2 to Fe0 and Fe0 amendment with sand [43,44,45,81]. Here, MnO2 promotes the Fe2+ oxidation and increases the formation of contaminant scavengers (FeCPs) compared to the pure Fe0 system [77,110]. Obviously, there is no contradiction between the retardation of contaminant removal in the presence of chloride ions and the improved efficiency of the same systems compared to the operational reference (Cl− free Fe0/H2O).

5. Conclusions

The view that NaCl addition initially prevents contaminant removal in Fe0/H2O systems is consistent with (i) the science of iron corrosion (e.g., solubility of Fe ions) and (ii) many experimental observations related to dye discoloration. However, this does not contradict the well-documented fact that some Fe0-based filters fed with chloride-rich waters perform better than those fed with fresh water. In addition, the results presented here confirm the key role of iron corrosion products (e.g., hydroxides and oxides) in the decontamination process of Fe0-based systems, including decentralized filters, such as household Kanchan filters in Southeast Asia. This observation suggests that the periodic flushing of Kanchan filters with NaCl solutions (e.g., table salt) is another potentially powerful tool for maintaining their efficiency. Thus, the results presented here can help developing countries in their efforts to meet the Sustainable Development Goal (SDG) Target 6.1, which aims to achieve universal and equitable access to safe and affordable drinking water for all by 2030.

Author Contributions

Conceptualization: R.T., X.C., M.X. and C.N.; methodology, R.T., X.C., M.X. and C.N.; writing—original draft preparation, R.T., X.C., M.X., W.G. and C.N.; writing—review and editing, C.N., R.H., W.G. and H.R. All authors have read and agreed to the published version of the manuscript.

Funding

This research received no external funding.

Data Availability Statement

Data are available on request.

Acknowledgments

The manuscript was improved thanks to the insightful comments of anonymous reviewers for Water. We acknowledge support by the German Research Foundation and the Open Access Publication Funds of the Göttingen University.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Ranjan, S.P.; Kazama, S.; Sawamoto, M. Effects of climate and land use changes on groundwater resources in coastal aquifers. J. Environ. Manag. 2006, 80, 25–35. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  2. Gain, A.K.; Wada, Y. Assessment of future water scarcity at different spatial and temporal scales of the Brahmaputra River Basin. Water Resour. Manag. 2014, 28, 999–1012. [Google Scholar] [CrossRef]
  3. Abd-Elaty, I.; Straface, S.; Kuriqi, A. Sustainable saltwater intrusion management in coastal aquifers under climatic changes for humid and hyper-arid regions. Ecol. Eng. 2021, 171, 106382. [Google Scholar] [CrossRef]
  4. Agoubi, B. A review: Saltwater intrusion in North Africa’s coastal areas—Current state and future challenges. Environ. Sci. Pollut. Res. 2021, 28, 17029–17043. [Google Scholar] [CrossRef] [PubMed]
  5. Passerat, J.; Ouattara, N.K.; Mouchel, J.-M.; Rocher, V.; Servais, P. Impact of an intense combined sewer overflow event on the microbiological water quality of the Seine River. Water Res. 2011, 45, 893–903. [Google Scholar] [CrossRef] [PubMed]
  6. Sambito, M.; Freni, G. Strategies for improving optimal positioning of quality sensors in urban drainage systems for non-conservative contaminants. Water 2021, 13, 934. [Google Scholar] [CrossRef]
  7. Banerji, T.; Chaudhari, S. A cost-effective technology for arsenic removal: Case study of zerovalent iron-based IIT Bombay arsenic filter in West Bengal. In Water and Sanitation in the New Millennium; Nath, K., Sharma, V., Eds.; Springer: New Delhi, India, 2017. [Google Scholar]
  8. Antia, D.D.J. Hydrodynamic decontamination of groundwater and soils using ZVI. Water 2023, 15, 540. [Google Scholar] [CrossRef]
  9. Xin, J.; Tang, F.; Yan, J.; La, C.; Zheng, X.; Liu, W. Investigating the efficiency of microscale zero valent iron-based in situ reactive zone (mZVI-IRZ) for TCE removal in fresh and saline groundwater. Sci. Total Environ. 2018, 626, 638–649. [Google Scholar] [CrossRef]
  10. Gao, C.; Wang, B.; Xingchun Li, X.; Zhang, Y.; Qu, T.; Du, X.; Zheng, J.; Feng, J. Removal of Cr(VI) by hollow micron zero-valent iron in groundwater containing different ions: Mechanisms and mineralized products. Proc. Saf. Environ. Protect. 2023, 173, 614–626. [Google Scholar] [CrossRef]
  11. Henderson, A.D.; Demond, A.H. Long-term performance of zero-valent iron permeable reactive barriers: A critical review. Environ. Eng. Sci. 2007, 24, 401–423. [Google Scholar] [CrossRef] [Green Version]
  12. Gheju, M. Hexavalent chromium reduction with zero-valent iron (ZVI) in aquatic systems. Water Air Soil Pollut. 2011, 222, 103–148. [Google Scholar] [CrossRef]
  13. Ghauch, A. Iron-based metallic systems: An excellent choice for sustainable water treatment. Freib. Online Geosci. 2015, 32, 1–80. [Google Scholar]
  14. Guan, X.; Sun, Y.; Qin, H.; Li, J.; Lo, I.M.C.; He, D.; Dong, H. The limitations of applying zero-valent iron technology in contaminants sequestration and the corresponding countermeasures: The development in zero-valent iron technology in the last two decades (1994–2014). Water Res. 2015, 75, 224–248. [Google Scholar] [CrossRef] [PubMed]
  15. Gheju, M. Progress in understanding the mechanism of CrVI Removal in Fe0-based filtration systems. Water 2018, 10, 651. [Google Scholar] [CrossRef] [Green Version]
  16. Antia, D.D.J. Water treatment and desalination using the eco-materials n-Fe0 (ZVI), n-Fe3O4, n-FexOyHz[mH2O], and n-Fex[Cation]nOyHz[Anion]m [rH2O]. In Handbook of Nanomaterials and Nanocomposites for Energy and Environmental Applications; Kharissova, O.V., Martínez, L., Kharisov, B., Eds.; Springer Nature: Cham, Switzerland, 2020. [Google Scholar] [CrossRef]
  17. Cao, V.; Bakari, O.; Kenmogne-Tchidjo, J.F.; Gatcha-Bandjun, N.; Ndé-Tchoupé, A.I.; Gwenzi, W.; Njau, K.N.; Noubactep, C. Conceptualizing the Fe0/H2O system: A call for collaboration to mark the 30th anniversary of the Fe0-based permeable reactive barrier technology. Water 2022, 14, 3120. [Google Scholar] [CrossRef]
  18. Bilardi, S.; Calabrò, P.S.; Moraci, N. A review of the hydraulic performance of permeable reactive barriers based on granular zero valent iron. Water 2023, 15, 200. [Google Scholar] [CrossRef]
  19. Cui, X.; Xiao, M.; Tao, R.; Hu, R.; Ruppert, H.; Gwenzi, W.; Noubactep, C. Developing the ascorbic acid test: A candidate standard tool for characterizing the intrinsic reactivity of metallic iron for water remediation. Water 2023, 15, 1930. [Google Scholar] [CrossRef]
  20. Lan, L.E.; Reina, F.D.; De Seta, G.E.; Meichtry, J.M.; Litter, M.I. Comparison between different technologies (zerovalent iron, coagulation-flocculation, adsorption) for arsenic treatment at high concentrations. Water 2023, 15, 1481. [Google Scholar] [CrossRef]
  21. Lawrinenko, M.; Kurwadkar, S.; Wilkin, R.T. Long–term performance evaluation of zero-valent iron amended permeable reactive barriers for groundwater remediation—A mechanistic approach. Geosci. Front. 2023, 14, 101494. [Google Scholar] [CrossRef]
  22. Plessl, K.; Russ, A.; Vollprecht, D. Application and development of zero-valent iron (ZVI) for groundwater and wastewater treatment. Int. J. Environ. Sci. Technol. 2022, 20, 6913–6928. [Google Scholar] [CrossRef]
  23. Singh, R.; Chakma, S.; Birke, V. Performance of field-scale permeable reactive barriers: An overview on potentials and possible implications for in-situ groundwater remediation applications. Sci. Total Environ. 2023, 858, 158838. [Google Scholar] [CrossRef] [PubMed]
  24. Cundy, A.B.; Hopkinson, L.; Whitby, R.L.D. Use of iron-based technologies in contaminated land and groundwater remediation: A review. Sci. Total Environ. 2008, 400, 42–51. [Google Scholar] [CrossRef] [PubMed]
  25. Thiruvenkatachari, R.; Vigneswaran, S.; Naidu, R. Permeable reactive barrier for groundwater remediation. J. Ind. Eng. Chem. 2008, 14, 145–156. [Google Scholar] [CrossRef]
  26. Chen, Q.; Fan, G.; Na, W.; Liu, J.; Cui, J.; Li, H. Past, present, and future of groundwater remediation research: A scientometric analysis. Int. J. Environ. Res. Public Health 2019, 16, 3975. [Google Scholar] [CrossRef] [Green Version]
  27. Li, X.; Li, Z.; Du, C.; Tian, Z.; Zhu, Q.; Li, G.; Shen, Q.; Li, C.; Li, J.; Li, W.; et al. Bibliometric analysis of zerovalent iron particles research for environmental remediation from 2000 to 2019. Environ. Sci. Pollut. Res. 2021, 28, 4200–34210. [Google Scholar] [CrossRef]
  28. Noubactep, C. Metallic iron for environmental remediation: A review of reviews. Water Res. 2015, 85, 114–123. [Google Scholar] [CrossRef]
  29. Antia, D.D.J. Remediation of saline wastewater producing a fuel gas containing alkanes and hydrogen using zero valent iron (Fe0). Water 2022, 14, 1926. [Google Scholar] [CrossRef]
  30. Gheju, M.; Balcu, I. Effect of sand co-presence on CrVI removal in Fe0-H2O system. Water 2023, 15, 777. [Google Scholar] [CrossRef]
  31. Lawrinenko, M.; Kurwadkar, S.; Wilkin, R.T. Responses to comments by Dr. Noubactep. Geosci. Front. 2023, 15, 101494. [Google Scholar] [CrossRef]
  32. Noubactep, C. Comments on “Long-term performance evaluation of zero-valent iron amended permeable reactive barriers for groundwater remediation—A mechanistic approach” by Lawrinenko et al., Geoscience Frontiers 14 (2023) 101494. Geosci. Front. 2023, 15, 101582. [Google Scholar] [CrossRef]
  33. Hu, R.; Gwenzi, W.; Sipowo, T.R.; Ndé-Tchoupé, A.I.; Cao, V.; Gwenzi, W.; Noubactep, C. Metallic iron for environmental remediation: The fallacy of the electron efficiency concept. Front. Environ. Chem. 2021, 2, 677813. [Google Scholar] [CrossRef]
  34. Ndé-Tchoupé, A.I.; Hu, R.; Gwenzi, W.; Nassi, A.; Noubactep, C. Characterizing the reactivity of metallic iron for water treatment: H2 evolution in H2SO4 and uranium removal efficiency. Water 2020, 12, 1523. [Google Scholar] [CrossRef]
  35. Matheson, L.J.; Tratnyek, P.G. Reductive dehalogenation of chlorinated methanes by iron metal. Environ. Sci. Technol. 1994, 28, 2045–2053. [Google Scholar] [CrossRef] [PubMed]
  36. Warren, K.D.; Arnold, R.G.; Bishop, T.L.; Lindholm, L.C.; Betterton, E.A. Kinetics and mechanism of reductive dehalogenation of carbon tetrachloride using zero-valence metals. J. Hazard. Mater. 1995, 41, 217–227. [Google Scholar] [CrossRef]
  37. Fiedor, J.N.; Bostick, W.D.; Jarabek, R.J.; Farrel, J. Understanding the mechanism, of uranium removal from groundwater by zero-valent iron using X-ray photoelectron spectroscopy. Environ. Sci. Technol. 1998, 32, 1466–1473. [Google Scholar] [CrossRef]
  38. Farrell, J.; Bostick, W.D.; Jarabeck, R.J.; Fiedor, J.N. Uranium removal from ground water using zero valent iron media. Ground Water 1999, 34, 618–624. [Google Scholar] [CrossRef]
  39. Qiu, S.R.; Lai, H.-F.; Roberson, M.J.; Hunt, M.L.; Amrhein, C.; Giancarlo, L.C.; Flynn, G.W.; Yarmoff, J.A. Removal of contaminants from aqueous solution by reaction with iron surfaces. Langmuir 2000, 16, 2230–2236. [Google Scholar] [CrossRef]
  40. Lavine, B.K.; Auslander, G.; Ritter, J. Polarographic studies of zero valent iron as a reductant for remediation of nitroaromatics in the environment. Microchem. J. 2001, 70, 69–83. [Google Scholar] [CrossRef]
  41. Jiao, Y.; Qiu, C.; Huang, L.; Wu, K.; Ma, H.; Chen, S.; Ma, L.; Wu, L. Reductive dechlorination of carbon tetrachloride by zero-valent iron and related iron corrosion. Appl. Catal. B Environ. 2009, 91, 434–440. [Google Scholar] [CrossRef]
  42. Ebelle, T.C.; Makota, S.; Tepong-Tsindé, R.; Nassi, A.; Noubactep, C. Metallic iron and the dialogue of the deaf. Fresenius Environ. Bull. 2019, 28, 8331–8340. [Google Scholar]
  43. Ghauch, A.; Abou Assi, H.; Bdeir, S. Aqueous removal of diclofenac by plated elemental iron: Bimetallic systems. J. Hazard. Mater. 2010, 182, 64–74. [Google Scholar] [CrossRef] [PubMed]
  44. Ghauch, A.; Abou Assi, H.; Baydoun, H.; Tuqan, A.M.; Bejjani, A. Fe0-based trimetallic systems for the removal of aqueous diclofenac: Mechanism and kinetics. Chem. Eng. J. 2011, 172, 1033–1044. [Google Scholar] [CrossRef]
  45. Gheju, M.; Balcu, I. Sustaining the efficiency of the Fe(0)/H2O system for Cr(VI) removal by MnO2 amendment. Chemosphere 2019, 214, 389–398. [Google Scholar] [CrossRef] [PubMed]
  46. Devlin, J.F.; Klausen, J.; Schwarzenbach, R.P. Kinetics of nitroaromatic reduction on granular iron in recirculating batch experiments. Environ. Sci. Technol. 1998, 32, 1941–1947. [Google Scholar] [CrossRef]
  47. Devlin, J.F.; Allin, K.O. Major anion effects on the kinetics and reactivity of granular iron in glass-encased magnet batch reactor experiments. Environ. Sci. Technol. 2005, 39, 1868–1874. [Google Scholar] [CrossRef]
  48. Noubactep, C. Processes of contaminant removal in “Fe0–H2O” systems revisited. The importance of co-precipitation. Open Environ. Sci. 2007, 1, 9–13. [Google Scholar] [CrossRef] [Green Version]
  49. Noubactep, C. A critical review on the mechanism of contaminant removal in Fe0–H2O systems. Environ. Technol. 2008, 29, 909–920. [Google Scholar] [CrossRef] [Green Version]
  50. Miyajima, K. Optimizing the design of metallic iron filters for water treatment. Freib. Online Geosci. 2012, 32, 1–60. [Google Scholar]
  51. Miyajima, K.; Noubactep, C. Effects of mixing granular iron with sand on the efficiency of methylene blue discoloration. Chem. Eng. J. 2012, 200–202, 433–438. [Google Scholar] [CrossRef] [Green Version]
  52. Btatkeu-K, B.D.; Tchatchueng, J.B.; Noubactep, C.; Caré, S. Designing metallic iron based water filters: Light from methylene blue discoloration. J. Environ. Manag. 2016, 166, 567–573. [Google Scholar] [CrossRef]
  53. Konadu-Amoah, B.; Ndé-Tchoupé, A.I.; Hu, R.; Gwenzi, W.; Noubactep, C. Investigating the Fe0/H2O systems using the methylene blue method: Validity, applications and future directions. Chemosphere 2021, 291, 132913. [Google Scholar] [CrossRef] [PubMed]
  54. Konadu-Amoah, B.; Hu, R.; Cui, X.; Tao, R.; Ndé-Tchoupé, A.I.; Gwenzi, W.; Noubactep, C. Characterizing the process of phosphate removal in Fe0/H2O systems. Chem. Eng. J. 2023, 465, 143042. [Google Scholar] [CrossRef]
  55. Mitchell, G.; Poole, P.; Segrove, H.D. Adsorption of methylene blue by high-silica sands. Nature 1955, 176, 1025–1026. [Google Scholar] [CrossRef]
  56. Tepong-Tsindé, R.; Phukan, M.; Nassi, A.; Noubactep, C.; Ruppert, H. Validating the efficiency of the MB discoloration method for the characterization of Fe0/H2O systems using accelerated corrosion by chloride ions. Chem. Eng. J. 2015, 279, 353–362. [Google Scholar] [CrossRef]
  57. Klausen, J.; Ranke, J.; Schwarzenbach, R. Influence of solution composition and column aging on the reduction of nitroaromatic compounds by zero-valent iron. Chemosphere 2001, 44, 511–517. [Google Scholar] [CrossRef]
  58. Su, C.; Puls, R.W. Arsenate and arsenite removal by zerovalent iron: Effects of phosphate, silicate, carbonate, borate, sulfate, chromate, molybdate, and nitrate, relative to chloride. Environ. Sci. Technol. 2001, 35, 4562–4568. [Google Scholar] [CrossRef]
  59. Kim, J.S.; Shea, P.J.; Yang, J.E.; Kim, J.E. Halide salts accelerate degradation of high explosives by zerovalent iron. Environ. Pollut. 2007, 147, 634–641. [Google Scholar] [CrossRef] [PubMed]
  60. Pullin, H.; Crane, R.A.; Morgan, D.J.; Scott, T.B. The effect of common groundwater anions on the aqueous corrosion of zero-valent iron nanoparticles and associated removal of aqueous copper and zinc. J. Environ. Chem. Eng. 2017, 5, 1166–1173. [Google Scholar] [CrossRef] [Green Version]
  61. Ling, J.; Qiao, J.; Song, Y.; Sun, Y. Influence of coexisting ions on the electron efficiency of sulfidated zerovalent iron toward Se(VI) removal. Chem. Eng. J. 2019, 378, 122124. [Google Scholar] [CrossRef]
  62. Li, R.; Li, Q.; Zhang, W.; Sun, X.; Li, J.; Shen, J.; Han, W. Low dose of sulfur-modified zero-valent iron for decontamination of trace Cd (II)-complexes in high-salinity wastewater. Sci. Total Environ. 2021, 793, 148579. [Google Scholar] [CrossRef]
  63. Sun, Y.; Li, J.; Huang, T.; Guan, X. The influences of iron characteristics, operating conditions and solution chemistry on contaminants removal by zero-valent iron: A review. Water Res. 2016, 100, 277–295. [Google Scholar] [CrossRef] [PubMed]
  64. Hwang, Y.; Kim, D.; Shin, H.-S. Inhibition of nitrate reduction by NaCl adsorption on a nano-zero-valent iron surface during a concentrate treatment for water reuse. Environ. Technol. 2015, 36, 1178–1187. [Google Scholar] [CrossRef] [PubMed]
  65. Sun, Y.; Lei, C.; Khan, E.; Chen, S.S.; Tsang, D.C.W.; Ok, Y.S.; Lin, D.; Feng, Y.; Li, X.D. Nanoscale zero-valent iron for metal/metalloid removal from model hydraulic fracturing wastewater. Chemosphere 2017, 176, 315–323. [Google Scholar] [CrossRef] [PubMed]
  66. Antia, D.D.J. ZVI (Fe0) desalination: Catalytic partial desalination of saline aquifers. Appl. Water Sci. 2018, 8, 71. [Google Scholar] [CrossRef] [Green Version]
  67. Ahmed, N.; Vione, D.; Rivoira, L.; Carena, L.; Castiglioni, M.; Bruzzoniti, M.C. A review on the degradation of pollutants by fenton-like systems based on zero-valent iron and persulfate: Effects of reduction potentials, pH, and anions occurring in waste waters. Molecules 2021, 26, 4584. [Google Scholar] [CrossRef]
  68. Whitney, W.R. The corrosion of iron. J. Am. Chem. Soc. 1903, 25, 394–406. [Google Scholar] [CrossRef]
  69. Wang, D.; Gilliland, S.E., III; Yi, X.; Logan, K.; Heitger, D.R.; Lucas, H.R.; Wang, W.N. Iron mesh-based metal organic framework filter for efficient arsenic removal. Environ. Sci. Technol. 2018, 52, 4275–4284. [Google Scholar] [CrossRef]
  70. Khan, I.; Saeed, K.; Zekker, I.; Zhang, B.; Hendi, A.H.; Ahmad, A.; Ahmad, S.; Zada, N.; Ahmad, H.; Shah, L.A.; et al. Review on Methylene Blue: Its Properties, Uses, Toxicity and Photodegradation. Water 2022, 14, 242. [Google Scholar] [CrossRef]
  71. Mittal, A.; Malviya, A.; Kaur, D.; Mittal, J.; Kurup, L. Studies on the adsorption kinetics and isotherms for the removal and recovery of methyl orange from wastewaters using waste materials. J. Hazard. Mater. 2007, 148, 229–240. [Google Scholar] [CrossRef]
  72. Guilherme, M.R.; Silva, R.; Girotto, E.M.; Rubira, A.F.; Muniz, E.C. Hydrogels based on PAAm network with PNIPAAm included: Hydrophilic–hydrophobic transition measured by the partition of Orange II and Methylene Blue in water. Polymer 2003, 44, 4213–4219. [Google Scholar] [CrossRef]
  73. Cho, H.; Zoh, K.-D. Photocatalytic degradation of azo dye (Reactive Red 120) inTiO2/UV system: Optimization and modeling using a responsesurface methodology (RSM) based on the central composite design. Dyes Pigment. 2007, 75, 533–543. [Google Scholar] [CrossRef]
  74. Birke, V.; Schuett, C.; Burmeier, H.; Friedrich, H.-J. Impact of trace elements and impurities in technical zero-valent iron brands on reductive dechlorination of chlorinated ethenes in groundwater. In Permeable Reactive Barrier Sustainable Groundwater Remediation; Naidu, R., Birke, V., Eds.; CRC Press: Boca Raton, FL, USA, 2015; pp. 87–98. ISBN 978-1-4822-2447-4. [Google Scholar]
  75. Phukan, M. Characterizing the Fe0/sand system by the extent of dye discoloration. Freib. Online Geosci. 2015, 40, 1–70. [Google Scholar]
  76. Phukan, M.; Noubactep, C.; Licha, T. Characterizing the ion-selective nature of Fe0-based filters using azo dyes. Chem. Eng. J. 2015, 259, 481–491. [Google Scholar] [CrossRef]
  77. Cao, V.; Alyoussef, G.; Gatcha-Bandjun, N.; Gwenzi, W.; Noubactep, C. Characterizing the impact of MnO2 addition on the efficiency of Fe0/H2O systems. Sci. Rep. 2021, 11, 9814. [Google Scholar] [CrossRef] [PubMed]
  78. Parks, G.A. The isoelectric points of solid oxides, solid hydroxides, and aqueous hydroxo complex systems. Chem. Rev. 1965, 65, 177–198. [Google Scholar] [CrossRef]
  79. Kosmulski, M. Isoelectric points and points of zero charge of metal (hydr)oxides: 50 years after Parks’ review. Adv. Colloid Interface Sci. 2016, 238, 1–61. [Google Scholar] [CrossRef]
  80. Gatcha-Bandjun, N.; Noubactep, C.; Loura Mbenguela, B. Mitigation of contamination in effluents by metallic iron: The role of iron corrosion products. Environ. Technol. Innov. 2017, 8, 71–83. [Google Scholar] [CrossRef]
  81. Burghardt, D.; Kassahun, A. Development of a reactive zone technology for simultaneous in situ immobilisation of radium and uranium. Environ. Geol. 2005, 49, 314–320. [Google Scholar] [CrossRef]
  82. Moraci, N.; Calabrò, P.S. Heavy metals removal and hydraulic performance in zero-valent iron/pumice permeable reactive barriers. J. Environ. Manag. 2010, 91, 2336–2341. [Google Scholar] [CrossRef]
  83. Btatkeu, K.B.D.; Miyajima, K.; Noubactep, C.; Caré, S. Testing the suitability of metallic iron for environmental remediation: Discoloration of methylene blue in column studies. Chem. Eng. J. 2013, 215–216, 959–968. [Google Scholar] [CrossRef] [Green Version]
  84. Aragaw, T.A.; Alene, A.N. A comparative study of acidic, basic, and reactive dyes adsorption from aqueous solution onto kaolin adsorbent: Effect of operating parameters, isotherms, kinetics, and thermodynamics. Emerg. Contam. 2022, 8, 59–74. [Google Scholar] [CrossRef]
  85. Miehr, R.; Tratnyek, G.P.; Bandstra, Z.J.; Scherer, M.M.; Alowitz, J.M.; Bylaska, J.E. Diversity of contaminant reduction reactions by zerovalent iron: Role of the reductate. Environ. Sci. Technol. 2004, 38, 139–147. [Google Scholar] [CrossRef] [PubMed]
  86. Li, J.; Dou, X.; Qin, H.; Sun, Y.; Yin, D.; Guan, X. Characterization methods of zerovalent iron for water treatment and remediation. Water Res. 2019, 148, 70–85. [Google Scholar] [CrossRef] [PubMed]
  87. Tepong-Tsindé, R.; Ndé-Tchoupé, A.I.; Noubactep, C.; Nassi, A.; Ruppert, H. Characterizing a newly designed steel-wool-based household filter for safe drinking water provision: Hydraulic conductivity and efficiency for pathogen removal. Processes 2019, 7, 966. [Google Scholar] [CrossRef] [Green Version]
  88. Tepong-Tsindé, R. Designing and Piloting a household filter for the peri-urban population of Douala (Cameroon). Freib. Online Geosci. 2021, 61, 1–80. [Google Scholar]
  89. Ndé-Tchoupé, A.I.; Konadu-Amoah, B.; Gatcha-Bandjun, N.; Hu, R.; Gwenzi, W.; Noubactep, C. Kanchan arsenic filters for household water treatment: Unsuitable or unsustainable? Water 2022, 14, 2318. [Google Scholar] [CrossRef]
  90. Mueller, B.; Chan, M.C.K.; Hug, S.J. Unique geochemistry of arsenic-contaminated groundwater and corresponding mitigation efforts in Southern Nepal. ACS ES&T Water 2023, 3, 1527–1535. [Google Scholar] [CrossRef]
  91. Lufingo, M.; Ndé-Tchoupé, A.I.; Hu, R.; Njau, K.N.; Noubactep, C. A novel and facile method to characterize the suitability of metallic iron for water treatment. Water 2019, 11, 2465. [Google Scholar] [CrossRef] [Green Version]
  92. Naseri, E.; Ndé-Tchoupé, A.I.; Mwakabona, H.T.; Nanseu-Njiki, C.P.; Noubactep, C.; Njau, K.N.; Wydra, K.D. Making Fe0-based filters a universal solution for safe drinking water provision. Sustainability 2017, 9, 1224. [Google Scholar] [CrossRef] [Green Version]
  93. Hernandez, R.; Zappi, M.; Kuo, C.H. Chloride effect on TNT degradation by zerovalent iron or zinc during water treatment. Environ. Sci. Technol. 2004, 38, 5157–5163. [Google Scholar] [CrossRef]
  94. Zhang, Y.; Wang, J.; Amrhein, C.; Frankenberger, W.T., Jr. Removal of selenate from water by zerovalent iron. J. Environ. Qual. 2005, 34, 487–495. [Google Scholar] [CrossRef] [PubMed]
  95. Ansaf, K.V.K.; Ambika, S.; Nambi, I.M. Performance enhancement of zero valent iron based systems using depassivators: Optimization and kinetic mechanisms. Water Res. 2016, 102, 436–444. [Google Scholar] [CrossRef]
  96. Gillham, R.W.; O’Hannesin, S.F. Enhanced degradation of halogenated aliphatics by zero-valent iron. Ground Water 1994, 32, 958–967. [Google Scholar] [CrossRef]
  97. Lipczynska-Kochany, E.; Harms, S.; Milburn, R.; Sprah, G.; Nadarajah, N. Degradation of carbon tetrachloride in the presence of iron and sulphur containing compounds. Chemosphere 1994, 29, 1477–1489. [Google Scholar] [CrossRef] [PubMed]
  98. Schreier, C.G.; Reinhard, M. Transformation of chlorinated organic compounds by iron and manganese powders in buffered water and in landfill leachate. Chemosphere 1994, 29, 1743–1753. [Google Scholar] [CrossRef]
  99. Fu, F.; Dionysiou, D.D.; Liu, H. The use of zero-valent iron for groundwater remediation and wastewater treatment: A review. J. Hazard. Mater. 2014, 267, 194–205. [Google Scholar] [CrossRef]
  100. Obiri-Nyarko, F.; Grajales-Mesa, S.J.; Malina, G. An overview of permeable reactive barriers for in situ sustainable groundwater remediation. Chemosphere 2014, 111, 243–259. [Google Scholar] [CrossRef]
  101. Comba, S.; Sethi, R. Stabilization of highly concentrated suspensions of iron nanoparticles using shear-thinning gels of xanthan gum. Water Res. 2009, 43, 3717–3726. [Google Scholar] [CrossRef]
  102. Ghauch, A.; Tuqan, A.; Assi, H.A. Antibiotic removal from water: Elimination of amoxicillin and ampicillin by microscale and nanoscale iron particles. Environ. Pollut. 2009, 157, 1626–1635. [Google Scholar] [CrossRef]
  103. Perey, J.R.; Chiu, P.C.; Huang, C.-P.; Cha, D.K. Zero-valent iron pretreatment for enhancing the biodegradability of azo dyes. Water Environ. Res. 2002, 74, 221–225. [Google Scholar] [CrossRef]
  104. Oh, S.Y.; Chiu, P.C.; Kim, B.J.; Cha, D.K. Zero-valent iron pretreatment for enhancing the biodegradability of RDX. Water Res. 2005, 39, 5027–5032. [Google Scholar] [CrossRef] [PubMed]
  105. Sleiman, N.; Deluchat, V.; Wazne, M.; Mallet, M.; Courtin-Nomade, A.; Kazpard, V.; Baudu, M. Phosphate removal from aqueous solutions using zero valent iron (ZVI): Influence of solution composition and ZVI aging. Colloids Surf. A Physicochem. Eng. Asp. 2017, 514, 1–10. [Google Scholar] [CrossRef]
  106. Cui, J.; Wang, X.; Zheng, K.; Wang, D.; Zhu, H.; Mao, X. Concentration-dependent enhancing effect of dissolved silicate on the oxidative degradation of sulfamethazine by zero-valent iron under aerobic conditions. Environ. Sci. Technol. 2019, 54, 1242–1249. [Google Scholar] [CrossRef] [PubMed]
  107. Zubair, Y.O.; Fuchida, S.; Tokoro, C. Adsorption and microscopic analysis of arsenate uptake by mesoporous zerovalent iron–magnetite nanocomposite: A detailed study on coexisting ions effects. Water Air Soil Pollut. 2022, 233, 484. [Google Scholar] [CrossRef]
  108. Noubactep, C. Characterizing the effects of shaking intensity on the kinetics of metallic iron dissolution in EDTA. J. Hazard. Mater. 2009, 170, 1149–1155. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  109. Noubactep, C.; Licha, T.; Scott, T.B.; Fall, M.; Sauter, M. Exploring the influence of operational parameters on the reactivity of elemental iron materials. J. Hazard. Mater. 2009, 172, 943–951. [Google Scholar] [CrossRef] [Green Version]
  110. Alyoussef, G. Characterizing the Impact of Contact Time in Investigating Processes in Fe0/H2O Systems. Master’s Thesis, University of Göttingen, Göttingen, Germany, 2019. [Google Scholar]
  111. He, Y.; Guo, Z.; Chen, M.; Wan, S.; Peng, N.; Fu, X.; Yuan, D.; Na, B. Efficient adsorption of methyl orange and methylene blue dyes by a novel carbazole-based hyper-crosslinked porous polymer. J. Porous Mater. 2023. [Google Scholar] [CrossRef]
  112. Konadu-Amoah, B. Decontamination in Fe0-Based Systems: Understanding Phosphate Removal in Fe0/H2O System Using the MB Method. Ph.D. Thesis, Hohai University, Najing, China, 2023. [Google Scholar]
  113. Scott, T.B.; Popescu, I.C.; Crane, R.A.; Noubactep, C. Nano-scale metallic iron for the treatment of solutions containing multiple inorganic contaminants. J. Hazard. Mater. 2011, 186, 280–287. [Google Scholar] [CrossRef]
  114. Zhang, Y.-F.; Zhang, C.-H.; Xu, J.-H.; Li, L.; Li, D.; Wu, Q.; Ma, L.-M. Strategies to enhance the reactivity of zero-valent iron for environmental remediation: A review. J. Environ. Manag. 2022, 317, 115381. [Google Scholar] [CrossRef]
Water 15 02466 g001 550
Figure 1. Degree of dye discoloration after 46 days in a Fe0/H2O system using ZVI1. Experimental conditions: miron = 0.1 g; msand = 0.5 g; Vsolution = 22 mL; [dye] = 10 mg L−1; [NaCl] = 0.0 g L−1.
Figure 1. Degree of dye discoloration after 46 days in a Fe0/H2O system using ZVI1. Experimental conditions: miron = 0.1 g; msand = 0.5 g; Vsolution = 22 mL; [dye] = 10 mg L−1; [NaCl] = 0.0 g L−1.
Water 15 02466 g001
Water 15 02466 g002 550
Figure 2. Time-dependent extent of methylene blue discoloration in Fe0/sand systems as a function of the NaCl concentration using ZVI1. Experimental conditions: miron = 0.1 g; msand = 0.5 g; Vsolution = 22 mL; [MB] = 10 mg L−1. The lines shown are not fitting functions, they simply connect the points for ease of visualization.
Figure 2. Time-dependent extent of methylene blue discoloration in Fe0/sand systems as a function of the NaCl concentration using ZVI1. Experimental conditions: miron = 0.1 g; msand = 0.5 g; Vsolution = 22 mL; [MB] = 10 mg L−1. The lines shown are not fitting functions, they simply connect the points for ease of visualization.
Water 15 02466 g002
Water 15 02466 g003 550
Figure 3. Extent of dye discoloration after 46 days as a function of the NaCl concentration using ZVI1. Experimental conditions: miron = 0.1 g; msand = 0.5 g; Vsolution = 22 mL; [dye] = 10 mg L−1. The lines shown are not fitting functions, they simply connect the points for ease of visualization.
Figure 3. Extent of dye discoloration after 46 days as a function of the NaCl concentration using ZVI1. Experimental conditions: miron = 0.1 g; msand = 0.5 g; Vsolution = 22 mL; [dye] = 10 mg L−1. The lines shown are not fitting functions, they simply connect the points for ease of visualization.
Water 15 02466 g003
Water 15 02466 g004 550
Figure 4. Extent of dye discoloration after 46 days as a function of the Fe0 dosage for methylene blue (a) and methyl orange (b) using ZVI1. Experimental conditions: miron = 0.1 g; msand = 0.5 g; Vsolution = 22 mL; [dye] = 10 mg L−1. The lines shown are not fitting functions, they simply connect the points for ease of visualization.
Figure 4. Extent of dye discoloration after 46 days as a function of the Fe0 dosage for methylene blue (a) and methyl orange (b) using ZVI1. Experimental conditions: miron = 0.1 g; msand = 0.5 g; Vsolution = 22 mL; [dye] = 10 mg L−1. The lines shown are not fitting functions, they simply connect the points for ease of visualization.
Water 15 02466 g004
Water 15 02466 g005a 550Water 15 02466 g005b 550
Figure 5. Extent of MB discoloration after 46 days as a function of the Fe0 type for methylene blue (a) and methyl orange (b). Experimental conditions: miron = 0.1 g; msand = 0.5 g; Vsolution = 22 mL; [MB] = 10 mg L−1.
Figure 5. Extent of MB discoloration after 46 days as a function of the Fe0 type for methylene blue (a) and methyl orange (b). Experimental conditions: miron = 0.1 g; msand = 0.5 g; Vsolution = 22 mL; [MB] = 10 mg L−1.
Water 15 02466 g005aWater 15 02466 g005b
Table
Table 1. Physico-chemical properties of the used dyes. Solubility data are from the references cited.
Table 1. Physico-chemical properties of the used dyes. Solubility data are from the references cited.
DyeMWFormulaNatureTypeλmaxSolubilityRef.
(g mol−1) (nm)(g L−1)
Methylene blue319.85C16H18ClN3Scationicbasic664.543.6[70]
Methyl orange327.33C14H14N3NaO3Sanionicacid464.05.0[71]
Orange II350.32C16H11N2NaO4SanionicAcid486.064.5[72]
Reactive red 1201338.1C44H30Cl2N14O20S6anionicacid515.070.0[73]
Table
Table 2. Code and main characteristics of the tested Fe0 materials according to the supplier. n.s. = not specified; granular = mechanically broken pieces; sponge = particles with pitted surfaces; scrap = waste generated in any forms: spherical = standard sphere with a smooth surface. kAA is the initial dissolution kinetics of each Fe0 in a 2 mM ascorbic acid solution [34].
Table 2. Code and main characteristics of the tested Fe0 materials according to the supplier. n.s. = not specified; granular = mechanically broken pieces; sponge = particles with pitted surfaces; scrap = waste generated in any forms: spherical = standard sphere with a smooth surface. kAA is the initial dissolution kinetics of each Fe0 in a 2 mM ascorbic acid solution [34].
CodeShapeSizeColorkAAFeSupplier
(mm) (μg h−1)(%)
ZVI1granular0.05–5.00black13.2 ± 0.5n.s.iPutec GmbH
ZVI2sponge1.00–2.00black11.5 ± 1.390.0ISPAT GmbH
ZVI3scrap0.05–2.00black12.3 ± 0.7n.s.Metallaufbereitung Zwickau
ZVI4spherical2.00grey2.8 ± 0.199.99Tongda Alloy Material Factory
Table
Table 3. Selected experimental conditions from published papers on the effect of chloride ions on the efficiency of water remediation using Fe0 materials; mFe0 = macroscale ZVI, nFe0 = nanoscale ZVI, sFe0 = sulfidated ZVI.
Table 3. Selected experimental conditions from published papers on the effect of chloride ions on the efficiency of water remediation using Fe0 materials; mFe0 = macroscale ZVI, nFe0 = nanoscale ZVI, sFe0 = sulfidated ZVI.
Fe0 Material Mixing
NatureDoseVContaminant(Chloride)NatureSpeedReference
(g L−1)(mL) (mM) (rpm)
mFe01–2.55Selenaten.s.n.s.100[103]
mFe015RDXn.s.shaking100[104]
mFe01.2525selenate10shaking180[94]
mFe01025RX0.5, 5.0, 50shakingn.s.[59]
nFe01.25800Nitrate0 to 342stirring200[64]
mFe02100Cr(VI)10n.sn.s[95]
mFe02.5100Phosphate10n.s.165[105]
sFe00.5500Selenate10stirring400[61]
mFe02200Silicaten.s.stirring200[106]
nFe0/Fe3O40.251000Arsenate2.8stirring1000[107]
mFe00–4522Dyes0 to 685none0This study
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Tao, R.; Cui, X.; Xiao, M.; Hu, R.; Gwenzi, W.; Ruppert, H.; Noubactep, C. Influence of Water Salinity on the Efficiency of Fe0-Based Systems for Water Treatment. Water 2023, 15, 2466. https://doi.org/10.3390/w15132466

AMA Style

Tao R, Cui X, Xiao M, Hu R, Gwenzi W, Ruppert H, Noubactep C. Influence of Water Salinity on the Efficiency of Fe0-Based Systems for Water Treatment. Water. 2023; 15(13):2466. https://doi.org/10.3390/w15132466

Chicago/Turabian Style

Tao, Ran, Xuesong Cui, Minhui Xiao, Rui Hu, Willis Gwenzi, Hans Ruppert, and Chicgoua Noubactep. 2023. "Influence of Water Salinity on the Efficiency of Fe0-Based Systems for Water Treatment" Water 15, no. 13: 2466. https://doi.org/10.3390/w15132466

APA Style

Tao, R., Cui, X., Xiao, M., Hu, R., Gwenzi, W., Ruppert, H., & Noubactep, C. (2023). Influence of Water Salinity on the Efficiency of Fe0-Based Systems for Water Treatment. Water, 15(13), 2466. https://doi.org/10.3390/w15132466

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