# The Removal of Uranium onto Nanoscale Zero-Valent Iron Particles in Anoxic Batch Systems

Authors: Richard A. Crane; Thomas B. Scott
Journal: Journal of Nanomaterials
 (2014)

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## Abstract

The removal of uranium (U) onto nanoscale zero-valent iron particles has been studied for uranium-bearing mine water and synthetic uranyl solutions in the presence and absence of dissolved oxygen. The work has been conducted in order to investigate the differential nanoparticle corrosion behaviour and associated mechanisms of U removal behaviour in conditions representative of near-surface and deep groundwater systems. Batch systems were analysed over a 28-day reaction period during which the liquid and nanoparticulate solids were periodically analysed to determine chemical evolution of the solutions and particulates. Analysis of aqueous samples using inductively coupled plasma mass spectrometry recorded near-total U removal after 1 hour of reaction in all systems studied. However, in the latter stages of the reaction (after 48 hours), significant rerelease of uranium was recorded for the mine water batch system with dissolved O2 present. In contrast, less than 2% uranium rerelease was recorded for the anoxic batch system. Concurrent analysis of extracted nanoparticle solids using X-ray diffraction recorded significantly slower corrosion of the nanoparticles in the anoxic batch system, with residual metallic iron maintained until after 28 days of reaction compared to only 7 days of reaction in systems with dissolved O2 present. Results provide clear evidence that the corrosion lifespan and associated U6+ removal efficacy of nanoscale zero-valent iron replace enhanced in the absence of dissolved oxygen.


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## Body

## 1. Introduction

To date, a key environmental legacy of mankind’s military and civil nuclear activities has been the release of uranium (U) into the natural environment. U can exist in five oxidation states: +2, +3, +4, +5, and +6. However, in the natural environment, the +4 and +6 valence states dominate. U4+ commonly exists in chemically reducing environments and typically forms chemical species of relatively low solubility [1]. In contrast, U6+ is predominant in oxidising environments and typically forms compounds of relatively high solubility [2]. Reduction of U6+ to U4+ has therefore been proposed as a suitable approach to U remediation.In recent years, a wide range of electron donors have been demonstrated to chemically reduce U6+ including reduced iron, including magnetite, [3] ferrous hydroxides, [4] Fe2+ sorbed on hematite surfaces [5], and zero-valent iron [6]; microorganisms, including dissimilatory metal-reducing bacteria [7] and sulphate reducing bacteria [8]; organic compounds, including acetate [9] and lactate [10]; and dissolved and solid sulphide species [11–16]. In contaminated sites the presence of competitive electron acceptors, toxic heavy metals, and/or unfavourable pH/Eh conditions can significantly limit the suitability of many biotic methods for uranium remediation [17, 18]. As a consequence, much focus has been applied in recent years on the use of chemical reducing agents, namely, zero-valent iron [19–28]. Recent work, investigating the removal of uranium in waste effluents [19] and mine water [22], has determined that the key role complexing agents, commonly found in natural waters, such as carbonate, phosphate, and sulphate, play on the long term removal of uranium onto nanoscale zero-valent iron. Results have provided clear evidence that such complexing agents (namely, carbonate) significantly enhance the relative stability of U6+, promoting U desorption from particle surfaces following an initial period of removal onto nanoscale zero-valent iron. The mechanism has been attributed to incomplete chemical reduction of surface-precipitated U6+, allowing U rerelease during subsequent nanoparticle corrosion and the reformation of highly stable aqueous U-complexes. There accordingly exists a fundamental need to understand the reversible nature of U removal in complex and/or natural waters using iron-based materials, specifically the link between nanoparticle corrosion and U desorption. The current work has therefore been established to contrast the sorption-desorption behaviour of U onto nanoscale zero-valent iron in natural waters containing dissolved oxygen (and dissolved oxygen recharge), that is, the vadose zone, with waters where dissolved oxygen is only available in trace levels, that is, the phreatic zone.


## 2. Materials and Methods

### 2.1. Experimental Procedure

Four 500 mL Schott Duran jars were each filled with 400 mL of the U-bearing mine water. Further four jars were filled with 400 mL of uranyl solution at 0.5 ppm U, with the solution pH adjusted to 9.52 using 0.01 M NaOH. The addition of NaOH was performed slowly, dropwise, to avoid the formation of hydroxocarbonyl complexes. Two of the mine water solutions and two of the uranyl solutions were then purged with oxygen-freeN2(g) (>99.998%) at 1 L m−1 for 30 minutes to reduce the content of O2(g) to <0.1 ppm and left in a Saffron Scientific glovebox for 7 days to equilibrate. The glovebox atmosphere consisted of N2/H2 (95 : 5) and a Coy Laboratory “Stak-Pak” palladium catalyst was used to catalyse the removal of O2(g), via reaction with H2(g), producing H2O(l). The two remaining mine water solutions were stored on the benchtop. To two of the mine water solutions (one oxic and one anoxic) and two of the uranyl solutions (one oxic and one anoxic), 0.2 g (0.5 g L−1) of nano-Fe0 was added. The two remaining mine water solutions (oxic and anoxic) and the two uranyl solutions (oxic and anoxic) were run as nanoparticle-free control systems. In each case, the nano-Fe0 was suspended in 2 mL of ethanol and dispersed by sonification for 30 seconds. During the experiment, the glovebox containing the anoxic batch systems was purged with N2/H2 (95 : 5) gas at 0.5 bar for 5 minutes every 24 hours.


### 2.2. Sampling Methods

Each system was sampled at 0 h, 1 h, 2 h, 4 h, 24 h, 48 h, 7 d, 14 d, and 28 d. Prior to sampling, the jars were gently agitated to ensure homogeneity and pH and Eh measurements were taken using a Hanna Instruments meter (model HI 8424) with a combination gel electrode pH probe and a platinum ORP electrode, respectively. Dissolved oxygen (DO) measurements were taken using a Jenway 970 DO2 meter. Aliquots of 10 mL were taken from each jar and centrifuged using a Hamilton Bell Vanguard V6500 desktop centrifuge at 6500 rpm for 30 seconds to separate the liquid and solid phases. The liquid was decanted, filtered through a 0.22 μm cellulose acetate filter, and then prepared for inductively coupled plasma atomic emission spectrometry (ICP-AES) and inductively coupled plasma mass spectrometry (ICP-MS). The solid was prepared for X-day diffraction (XRD) and X-ray photoelectron spectroscopy (XPS) by sequential rinsing in 3 mL each of Milli-Q water, ethanol, and then acetone, with the resultant suspension pipetted onto a glass optical microscope slide and aluminium stub, respectively.


### 2.3. Nanoparticle Synthesis

Iron nanoparticles were synthesised following the method first described by Wang and Zhang [29] using sodium borohydride to reduce ferrous iron to a metallic state. 1.35 g of FeCl3·6H2O was dissolved in 50 mL of Milli-Q water (>18.2 MΩ cm) and then a 4 M NaOH solution was used to adjust the solution pH to 6.8. The addition of NaOH was performed slowly, dropwise, to avoid the formation of hydroxocarbonyl complexes. The salts were reduced to metallic nanoparticles by the addition of 2.0 g of NaBH4. The nanoparticle product was then isolated through centrifugation and sequentially washed with water, ethanol, and acetone (20 mL of each). The nanoparticles were dried in a dessicator under low vacuum (approx. 10−2mbar) for 48 hours and then stored in the oxygen-free nitrogen environment of a Saffron Scientific glovebox until required.


### 2.4. ICP-AES Preparation

The liquid samples were prepared for ICP-AES analysis by a 10-time dilution in 1% nitric acid (analytical quality concentrated HNO3 in Milli-Q water). Blanks and standards for analysis were also prepared in 1% nitric acid, with Fe standards of 0.1, 0.25, 0.5, 1, 2.5, 5, and 10 ppm. A Jobin Yvon Ultima ICP-AES (sequential spectrometer) fitted with a cyclone spray chamber and a Burgener Teflon Mira Mist Nebulizer was used. The Fe concentration was measured using the emission line at 259.94 nm.


### 2.5. ICP-MS Preparation

Samples were prepared for ICP-MS analysis by a 10-time dilution in 1% nitric acid (analytical quality concentrated HNO3 in Milli-Q water). Blanks and uranium standards at 0.1, 0.5, 1, 5, and 10 ppb were also prepared in 1% nitric acid (analytical quality concentrated HNO3 in Milli-Q water). An internal Bi standard of 10 ppb was added to blanks, standards, and samples. The ICP-MS instrument used was Thermo Elemental PQ3.


### 2.6. XPS

Solid samples were analysed at <5 × 10−8 mbar in a Thermo Fisher Scientific Escascope equipped with a dual anode X-ray source (AlKα 1486.6 eV and MgKα 1253.6 eV). AlKα radiation was used at 400 W (15 kV, 23 mA). High resolution scans were acquired using a 30 eV pass energy and 200 ms dwell times. Following the acquisition of “wide” spectra over a wide binding energy range, the regions containing the C and U peaks were scanned at a higher energy resolution. Data analysis was carried out using Pisces software (Dayta Systems Ltd.) with binding energy values of the recorded lines referenced to the adventitious hydrocarbon C1s peak at 284.8 eV.


### 2.7. XRD

A Phillips Xpert Pro diffractometer with aCuKα radiation source (λ=1.5406Å) was used for XRD analysis (generator voltage of 40 keV; tube current of 30 mA). XRD spectra were acquired between 2θ angles of 0–90°, with a step size of 0.02° and a 2 s dwell time.


## 2.1. Experimental Procedure

Four 500 mL Schott Duran jars were each filled with 400 mL of the U-bearing mine water. Further four jars were filled with 400 mL of uranyl solution at 0.5 ppm U, with the solution pH adjusted to 9.52 using 0.01 M NaOH. The addition of NaOH was performed slowly, dropwise, to avoid the formation of hydroxocarbonyl complexes. Two of the mine water solutions and two of the uranyl solutions were then purged with oxygen-freeN2(g) (>99.998%) at 1 L m−1 for 30 minutes to reduce the content of O2(g) to <0.1 ppm and left in a Saffron Scientific glovebox for 7 days to equilibrate. The glovebox atmosphere consisted of N2/H2 (95 : 5) and a Coy Laboratory “Stak-Pak” palladium catalyst was used to catalyse the removal of O2(g), via reaction with H2(g), producing H2O(l). The two remaining mine water solutions were stored on the benchtop. To two of the mine water solutions (one oxic and one anoxic) and two of the uranyl solutions (one oxic and one anoxic), 0.2 g (0.5 g L−1) of nano-Fe0 was added. The two remaining mine water solutions (oxic and anoxic) and the two uranyl solutions (oxic and anoxic) were run as nanoparticle-free control systems. In each case, the nano-Fe0 was suspended in 2 mL of ethanol and dispersed by sonification for 30 seconds. During the experiment, the glovebox containing the anoxic batch systems was purged with N2/H2 (95 : 5) gas at 0.5 bar for 5 minutes every 24 hours.


## 2.2. Sampling Methods

Each system was sampled at 0 h, 1 h, 2 h, 4 h, 24 h, 48 h, 7 d, 14 d, and 28 d. Prior to sampling, the jars were gently agitated to ensure homogeneity and pH and Eh measurements were taken using a Hanna Instruments meter (model HI 8424) with a combination gel electrode pH probe and a platinum ORP electrode, respectively. Dissolved oxygen (DO) measurements were taken using a Jenway 970 DO2 meter. Aliquots of 10 mL were taken from each jar and centrifuged using a Hamilton Bell Vanguard V6500 desktop centrifuge at 6500 rpm for 30 seconds to separate the liquid and solid phases. The liquid was decanted, filtered through a 0.22 μm cellulose acetate filter, and then prepared for inductively coupled plasma atomic emission spectrometry (ICP-AES) and inductively coupled plasma mass spectrometry (ICP-MS). The solid was prepared for X-day diffraction (XRD) and X-ray photoelectron spectroscopy (XPS) by sequential rinsing in 3 mL each of Milli-Q water, ethanol, and then acetone, with the resultant suspension pipetted onto a glass optical microscope slide and aluminium stub, respectively.


## 2.3. Nanoparticle Synthesis

Iron nanoparticles were synthesised following the method first described by Wang and Zhang [29] using sodium borohydride to reduce ferrous iron to a metallic state. 1.35 g of FeCl3·6H2O was dissolved in 50 mL of Milli-Q water (>18.2 MΩ cm) and then a 4 M NaOH solution was used to adjust the solution pH to 6.8. The addition of NaOH was performed slowly, dropwise, to avoid the formation of hydroxocarbonyl complexes. The salts were reduced to metallic nanoparticles by the addition of 2.0 g of NaBH4. The nanoparticle product was then isolated through centrifugation and sequentially washed with water, ethanol, and acetone (20 mL of each). The nanoparticles were dried in a dessicator under low vacuum (approx. 10−2mbar) for 48 hours and then stored in the oxygen-free nitrogen environment of a Saffron Scientific glovebox until required.


## 2.4. ICP-AES Preparation

The liquid samples were prepared for ICP-AES analysis by a 10-time dilution in 1% nitric acid (analytical quality concentrated HNO3 in Milli-Q water). Blanks and standards for analysis were also prepared in 1% nitric acid, with Fe standards of 0.1, 0.25, 0.5, 1, 2.5, 5, and 10 ppm. A Jobin Yvon Ultima ICP-AES (sequential spectrometer) fitted with a cyclone spray chamber and a Burgener Teflon Mira Mist Nebulizer was used. The Fe concentration was measured using the emission line at 259.94 nm.


## 2.5. ICP-MS Preparation

Samples were prepared for ICP-MS analysis by a 10-time dilution in 1% nitric acid (analytical quality concentrated HNO3 in Milli-Q water). Blanks and uranium standards at 0.1, 0.5, 1, 5, and 10 ppb were also prepared in 1% nitric acid (analytical quality concentrated HNO3 in Milli-Q water). An internal Bi standard of 10 ppb was added to blanks, standards, and samples. The ICP-MS instrument used was Thermo Elemental PQ3.


## 2.6. XPS

Solid samples were analysed at <5 × 10−8 mbar in a Thermo Fisher Scientific Escascope equipped with a dual anode X-ray source (AlKα 1486.6 eV and MgKα 1253.6 eV). AlKα radiation was used at 400 W (15 kV, 23 mA). High resolution scans were acquired using a 30 eV pass energy and 200 ms dwell times. Following the acquisition of “wide” spectra over a wide binding energy range, the regions containing the C and U peaks were scanned at a higher energy resolution. Data analysis was carried out using Pisces software (Dayta Systems Ltd.) with binding energy values of the recorded lines referenced to the adventitious hydrocarbon C1s peak at 284.8 eV.


## 2.7. XRD

A Phillips Xpert Pro diffractometer with aCuKα radiation source (λ=1.5406Å) was used for XRD analysis (generator voltage of 40 keV; tube current of 30 mA). XRD spectra were acquired between 2θ angles of 0–90°, with a step size of 0.02° and a 2 s dwell time.


## 3. Results

### 3.1. Preliminary Characterisation of the Nanoparticles

Preliminary characterisation of the nano-Fe0 was performed using Brunauer, Emmett, and Teller (BET) surface area analysis, transmission electron microscopy (TEM), XRD, and XPS. BET analysis determined that the starting surface area of the nano-Fe0 was 14.8 m2g−1. TEM analysis determined that the nano-Fe0 were roughly spherical, with an approximate size range of 20–100 nm and an average diameter of 34 nm. The density contrast between the Fe0 core and oxide shell in the nano-Fe0 was identified; however, the material was recorded as relatively amorphous with no clear grain structure. Individual particles were recorded as aggregated into chains and rings, attributed to the magnetic properties of the Fe0 cores. XRD analysis recorded a broad diffraction peak at 44.9° 2θ and other low intensity peaks at 65° and 82° 2θ, implying the presence of amorphous Fe0. XPS analysis confirmed the presence of a mixed valent (Fe2+/Fe3+) oxide at the surface of the material. The results are summarised in Table 1.Table 1
Bulk and surface properties of the nano-Fe0  used in the current work.
Parameter
Nano-Fe0
Particle size distribution (%)
0–50 nm50–100 nm>100 nm
8587
Crystallinity
Amorphous(α-Fe)
Oxide thickness (nm)
3-4
Surface area (m2 g−1)
14.8
Surface composition (%)
FeOCB
30.532.114.522.9
Surface stoichiometry
(Fe0/Fe2+ + Fe3+)Fe2+/Fe3+
0.020.38
Note: a significant proportion of the carbon detected is likely to be adventitious carbon.


### 3.2. Preliminary Characterisation of the U-Bearing Mine Water

Prior to nanoparticle addition, the U-bearing mine water was characterised using ICP-AES (Fe, Mg, Cu, and Mo), ICP-MS (U), volumetric titration (HCO3-, NO3-, and PO43-), and gravimetry (SO42-) with supplementary Eh, pH, and DO measurements. The analysis indicated that HCO3-, well documented to form uranyl complexes of high thermodynamic stability [30], was the most common ligand species present, with a concentration of approximately 974 ppm (Table 2).Table 2
Concentrations of notable chemical species present in the mine water, analysed by ICP-MS (U), ICP-AES (Fe, Mg, Cu, and Mo), volumetric titration (HCO3-, NO3-, and PO43-), and gravimetry (SO42-) along with the recorded Eh, pH, and DO.
Chemical species
Concentration (ppm)
Cations
Cu
0.044
Fe
0.021
Mg
12.11
Mo
0.21
U
1.41
Anions
HCO3-
974.42
NO3-
18.53
PO43-
0.15
SO42-
0.51
Solution conditions
DO (ppm)
8.84
Eh (mV)
65
pH
9.29


### 3.3. The Effect of Inert Gas Sparging

Following N2 gas sparging a decrease in solution Eh, from 65 mV to −49 mV, was recorded concurrent with a significant decrease in DO, from 8.93 ppm to 0.09 ppm, and ascribed to the expulsion of DO from the mine water. An increase in solution pH, from 9.29 to 9.52, was also recorded. This is a common phenomenon reported for carbonate-rich solutions during inert gas sparging and attributed to the expulsion of dissolved CO2, resulting in the hydrolysis of HCO3- (in the form of NaHCO3) and the formation of OH- [31–33].


### 3.4. Changes in DO/Eh/pH

Following the addition of the nanoparticles a shift to chemically reducing Eh and near-zero DO was recorded within 15 minutes of reaction for all batch systems (Figure1). An accompanying increase in system pH was also recorded in all systems (Figure 1). For the oxic batch systems, in the early stages of reaction (<15 minutes), the predominant mechanism of nano-Fe0 corrosion is considered to have been through reaction with H+ via the consumption of DO (see (1) and (2)). For the anoxic batch systems (and the oxic batch systems following total DO consumption) the absence of DO dictates that corrosion could only proceed through the direct reaction (hydrolysis) with water (see (3) and (4)). The slower pH/Eh change recorded for the anoxic batch systems in the current work is therefore ascribed to the slower reaction kinetics of nano-Fe0 in the absence of DO:
(1)2Fe0+4H++O2⟶2Fe2++2H2OE0=+1.67V(2)2Fe2++2H++12O2⟶2Fe3++H2OE0=+0.46V(3)Fe0+2H2O(l)⟶Fe2++H2+2OH-E0=-0.39V(4)2Fe2++2H2O⟶2Fe3++H2+2OH-E0=-1.60V(a) Eh (mV) as a function of reaction time (0–672 hrs). The control (nanoparticle-free) solutions (not shown) recorded a variation of <10 mV in all systems; (b) pH as a function of reaction time (0–672 hrs). The control (nanoparticle-free) solution (not shown) recorded a variation of <0.2 pH units in all systems; (c) dissolved oxygen (ppm) as a function of reaction time (0–672 hrs). The control (nanoparticle-free) solution (not shown) recorded a variation of <0.05 ppm units in all systems.
(a)
(b)
(c)In addition, fast pH/Eh changes were recorded for the uranyl solutions compared to the mine water batch systems. This is attributed to the lack of major ions in the former systems to buffer the aforementioned geochemical perturbation imbued by nanoparticle corrosion.After 4 hours of reaction, a recovery in DO and Eh was recorded for the oxic batch systems only. In contrast, Eh and DO were maintained as less than −430 mV and <0.2 ppm O2, respectively, for the entire 28-day reaction period for both anoxic batch systems. Near-zero DO (<0.1 ppm) was recorded for the anoxic (nanoparticle-free) batch system for the entire 28-day reaction period. This provides clear evidence of minimal oxygen ingress into the anoxic batch systems.


### 3.5. Changes in Aqueous U and Fe Concentration

Analysis of liquid samples using ICP-MS recorded rapid and near-total U removal in all systems treated using nano-Fe0 (Figure 2) with removal of >99% U(aq) recorded after 1 hour in all systems and maintained until 48 hours of reaction. Onwards from 48 hours a gradual increase in U(aq) concentration was recorded for the oxic mine water batch system (Figure 2). In contrast, no appreciable U rerelease was recorded for the anoxic mine water and the uranyl batch systems in both oxic and anoxic conditions. This is attributed to the presence of complexing agents (namely, carbonate) in the mine water, allowing the reformation of dissolved U-complexes concurrent with nanoparticle corrosion during the ingress of atmospheric gases into the batch systems as previously observed [22]. As reported by Crane et al., [22] it is likely that chemical reduction of aqueous U6+ to solid U4+ (as UO2) occurred for all batch treatment systems during the initial stage of U sorption onto the nano-Fe0. However, for the mine water solutions containing dissolved oxygen, oxidation back to aqueous U6+ is likely to have occurred due to a combination of (i) the increased availability of dissolved oxygen and (ii) the enhanced solubility of U in the presence of complexing agents, such as carbonate.(a) Aqueous uranium concentration (ppm) as a function of reaction time (0–672 hrs). The control (nanoparticle-free) solutions (not shown) recorded a variation of <0.01 ppm from the starting concentration in all systems; (b) aqueous iron concentration (ppm) as a function of reaction time (0–672 hrs). The control (nanoparticle-free) solutions (not shown) recorded a variation of <0.02 ppm from the starting concentration in all systems.
(a)
(b)Analysis of liquid samples using ICP-AES recorded an increase inFe(aq) following the addition of the nanoparticles, with maximum Fe(aq) concentrations recorded in all systems within the first 48 hours of reaction and attributed to the rapid corrosion of nanoparticulate surfaces. The greatest Fe(aq) concentrations were recorded for the uranyl solutions and ascribed to the lower ionic concentration compared to the mine water.


### 3.6. Analysis of Reacted Nanoparticulate Solids

#### 3.6.1. X-Ray Diffraction

XRD was used to determine the bulk crystallinity and composition of nano-Fe0 solids extracted from both oxic and anoxic batch systems at periodic intervals during the experiment (Figure 3). A transition from Fe0, with peaks centred at 44.6, 65.6, and 82.6° 2θ (lattice reflections: Fe(110), Fe(200), and Fe(211), resp.), to a mixture of akaganéite (β-FeOOH), ferrihydrite (5Fe2O3·9H2O), and magnetite (Fe3O4) was recorded for both oxic and anoxic batch systems. Total Fe0 conversion was, however, not recorded for the anoxic system with residual Fe0 present after 28 days of reaction compared to full conversion exhibited by the oxic batch system after 7 days of reaction. This is ascribed to the slower corrosion of nano-Fe0 in the absence of DO as discussed above.X-ray diffraction (XRD) spectra (for the range of 10–90° 2θ) recorded for the oxic (a) and anoxic (b) mine water batch systems after reaction times of 1 h, 2 h, 4 h, 24 h, 7 d, 14 d, and 28 d.
(a)
(b)The formation of ferrihydrite and magnetite was not unexpected, given that both species are common Fe0 corrosion products in near-neutral to alkaline solutions [34–38]. The presence of chloride ions (which are necessary for akaganéite formation) was likely to have been provided by the dissolution of FeCl2, present in the nano-Fe0 due to incomplete conversion of FeCl2 to Fe0 during the nano-Fe0 synthesis. In the latter stages of the reaction (>7 days) the akaganéite peak was recorded to shift by approximately −0.5° 2θ, suggesting an increase in the lattice parameter of the material. This was attributed to cationic substitution of a larger ion, such as Ca2+ (0.212 nm compared to 0.166 nm), into the lattice structure [39].


#### 3.6.2. X-Ray Photoelectron Spectroscopy

X-ray photoelectron spectroscopy (XPS) was used to determine the surface chemistry of extracted particulates including any sorbed species extracted from the oxic and anoxic batch systems at regular intervals throughout the experiment (Figure4). Curve fitting of recorded Fe 2p3/2 photoelectron peaks (not shown) determined a decrease in the Fe2+/Fe3+ ratio throughout the reaction period, ascribed to the oxidation of the nanoparticle surfaces. This occurred most rapidly during the initial stages of the reaction, with oxic and anoxic systems recording a shift in Fe2+/Fe3+ ratio to 0.23 and 0.32, respectively, after 1 hour of reaction. The higher proportion of Fe3+ in the oxic system is attributed to a greater concentration of DO at the start of the reaction. Following this initial and rapid oxidation phase, a more gradual decrease in the Fe2+/Fe3+ ratio was recorded in all oxic systems to minima of 0.11 after 28 days of reaction. In contrast, no appreciable change was recorded for all anoxic systems, indicating that minimal nano-Fe0 oxidation had occurred.Figure 4
Curve fitted XPS U 4f photoelectron peaks acquired after 24 hours of reaction for mine water batch systems treated with nano-Fe0.XPS data recorded from the samples of extracted particulates failed to record detectable peaks in the U 4f binding energy region of the recorded photoelectron spectra in all the reacted samples, even during the initial period of maximum U removal. This was not unexpected, given the small amount of U in each system (1413μ L−1) relative to the large surface area presented by the nanoparticles (14.8 m2 g−1). U 4f photoelectron peaks were detected for both oxic and anoxic mine water samples after 4 hours of reaction. Curve fitting, following the method of Scott et al., determined that U present was in a partially reduced state for both systems with a U4+/U6+ ratio of 0.34 and 1.13 recorded for the oxic and anoxic system, respectively. Greater proportion of U4+ relative to U6+ recorded for the anoxic batch system is attributed to enhanced chemical reduction of U in low oxygen conditions. This is likely to be due to the significantly lower (and sustained) Eh conditions imbued by the nano-Fe0 in the low oxygen environment, where Fe0 is maintained throughout the 28-day reaction period (see Section 3.6.1). In contrast Fe0 was recorded to be oxidised to (oxy)hydroxide species more rapidly in the batch systems containing dissolved oxygen, which would have resulted in lower chemical reduction of U6+ to U4+.


## 3.1. Preliminary Characterisation of the Nanoparticles

Preliminary characterisation of the nano-Fe0 was performed using Brunauer, Emmett, and Teller (BET) surface area analysis, transmission electron microscopy (TEM), XRD, and XPS. BET analysis determined that the starting surface area of the nano-Fe0 was 14.8 m2g−1. TEM analysis determined that the nano-Fe0 were roughly spherical, with an approximate size range of 20–100 nm and an average diameter of 34 nm. The density contrast between the Fe0 core and oxide shell in the nano-Fe0 was identified; however, the material was recorded as relatively amorphous with no clear grain structure. Individual particles were recorded as aggregated into chains and rings, attributed to the magnetic properties of the Fe0 cores. XRD analysis recorded a broad diffraction peak at 44.9° 2θ and other low intensity peaks at 65° and 82° 2θ, implying the presence of amorphous Fe0. XPS analysis confirmed the presence of a mixed valent (Fe2+/Fe3+) oxide at the surface of the material. The results are summarised in Table 1.Table 1
Bulk and surface properties of the nano-Fe0  used in the current work.
Parameter
Nano-Fe0
Particle size distribution (%)
0–50 nm50–100 nm>100 nm
8587
Crystallinity
Amorphous(α-Fe)
Oxide thickness (nm)
3-4
Surface area (m2 g−1)
14.8
Surface composition (%)
FeOCB
30.532.114.522.9
Surface stoichiometry
(Fe0/Fe2+ + Fe3+)Fe2+/Fe3+
0.020.38
Note: a significant proportion of the carbon detected is likely to be adventitious carbon.


## 3.2. Preliminary Characterisation of the U-Bearing Mine Water

Prior to nanoparticle addition, the U-bearing mine water was characterised using ICP-AES (Fe, Mg, Cu, and Mo), ICP-MS (U), volumetric titration (HCO3-, NO3-, and PO43-), and gravimetry (SO42-) with supplementary Eh, pH, and DO measurements. The analysis indicated that HCO3-, well documented to form uranyl complexes of high thermodynamic stability [30], was the most common ligand species present, with a concentration of approximately 974 ppm (Table 2).Table 2
Concentrations of notable chemical species present in the mine water, analysed by ICP-MS (U), ICP-AES (Fe, Mg, Cu, and Mo), volumetric titration (HCO3-, NO3-, and PO43-), and gravimetry (SO42-) along with the recorded Eh, pH, and DO.
Chemical species
Concentration (ppm)
Cations
Cu
0.044
Fe
0.021
Mg
12.11
Mo
0.21
U
1.41
Anions
HCO3-
974.42
NO3-
18.53
PO43-
0.15
SO42-
0.51
Solution conditions
DO (ppm)
8.84
Eh (mV)
65
pH
9.29


## 3.3. The Effect of Inert Gas Sparging

Following N2 gas sparging a decrease in solution Eh, from 65 mV to −49 mV, was recorded concurrent with a significant decrease in DO, from 8.93 ppm to 0.09 ppm, and ascribed to the expulsion of DO from the mine water. An increase in solution pH, from 9.29 to 9.52, was also recorded. This is a common phenomenon reported for carbonate-rich solutions during inert gas sparging and attributed to the expulsion of dissolved CO2, resulting in the hydrolysis of HCO3- (in the form of NaHCO3) and the formation of OH- [31–33].


## 3.4. Changes in DO/Eh/pH

Following the addition of the nanoparticles a shift to chemically reducing Eh and near-zero DO was recorded within 15 minutes of reaction for all batch systems (Figure1). An accompanying increase in system pH was also recorded in all systems (Figure 1). For the oxic batch systems, in the early stages of reaction (<15 minutes), the predominant mechanism of nano-Fe0 corrosion is considered to have been through reaction with H+ via the consumption of DO (see (1) and (2)). For the anoxic batch systems (and the oxic batch systems following total DO consumption) the absence of DO dictates that corrosion could only proceed through the direct reaction (hydrolysis) with water (see (3) and (4)). The slower pH/Eh change recorded for the anoxic batch systems in the current work is therefore ascribed to the slower reaction kinetics of nano-Fe0 in the absence of DO:
(1)2Fe0+4H++O2⟶2Fe2++2H2OE0=+1.67V(2)2Fe2++2H++12O2⟶2Fe3++H2OE0=+0.46V(3)Fe0+2H2O(l)⟶Fe2++H2+2OH-E0=-0.39V(4)2Fe2++2H2O⟶2Fe3++H2+2OH-E0=-1.60V(a) Eh (mV) as a function of reaction time (0–672 hrs). The control (nanoparticle-free) solutions (not shown) recorded a variation of <10 mV in all systems; (b) pH as a function of reaction time (0–672 hrs). The control (nanoparticle-free) solution (not shown) recorded a variation of <0.2 pH units in all systems; (c) dissolved oxygen (ppm) as a function of reaction time (0–672 hrs). The control (nanoparticle-free) solution (not shown) recorded a variation of <0.05 ppm units in all systems.
(a)
(b)
(c)In addition, fast pH/Eh changes were recorded for the uranyl solutions compared to the mine water batch systems. This is attributed to the lack of major ions in the former systems to buffer the aforementioned geochemical perturbation imbued by nanoparticle corrosion.After 4 hours of reaction, a recovery in DO and Eh was recorded for the oxic batch systems only. In contrast, Eh and DO were maintained as less than −430 mV and <0.2 ppm O2, respectively, for the entire 28-day reaction period for both anoxic batch systems. Near-zero DO (<0.1 ppm) was recorded for the anoxic (nanoparticle-free) batch system for the entire 28-day reaction period. This provides clear evidence of minimal oxygen ingress into the anoxic batch systems.


## 3.5. Changes in Aqueous U and Fe Concentration

Analysis of liquid samples using ICP-MS recorded rapid and near-total U removal in all systems treated using nano-Fe0 (Figure 2) with removal of >99% U(aq) recorded after 1 hour in all systems and maintained until 48 hours of reaction. Onwards from 48 hours a gradual increase in U(aq) concentration was recorded for the oxic mine water batch system (Figure 2). In contrast, no appreciable U rerelease was recorded for the anoxic mine water and the uranyl batch systems in both oxic and anoxic conditions. This is attributed to the presence of complexing agents (namely, carbonate) in the mine water, allowing the reformation of dissolved U-complexes concurrent with nanoparticle corrosion during the ingress of atmospheric gases into the batch systems as previously observed [22]. As reported by Crane et al., [22] it is likely that chemical reduction of aqueous U6+ to solid U4+ (as UO2) occurred for all batch treatment systems during the initial stage of U sorption onto the nano-Fe0. However, for the mine water solutions containing dissolved oxygen, oxidation back to aqueous U6+ is likely to have occurred due to a combination of (i) the increased availability of dissolved oxygen and (ii) the enhanced solubility of U in the presence of complexing agents, such as carbonate.(a) Aqueous uranium concentration (ppm) as a function of reaction time (0–672 hrs). The control (nanoparticle-free) solutions (not shown) recorded a variation of <0.01 ppm from the starting concentration in all systems; (b) aqueous iron concentration (ppm) as a function of reaction time (0–672 hrs). The control (nanoparticle-free) solutions (not shown) recorded a variation of <0.02 ppm from the starting concentration in all systems.
(a)
(b)Analysis of liquid samples using ICP-AES recorded an increase inFe(aq) following the addition of the nanoparticles, with maximum Fe(aq) concentrations recorded in all systems within the first 48 hours of reaction and attributed to the rapid corrosion of nanoparticulate surfaces. The greatest Fe(aq) concentrations were recorded for the uranyl solutions and ascribed to the lower ionic concentration compared to the mine water.


## 3.6. Analysis of Reacted Nanoparticulate Solids

### 3.6.1. X-Ray Diffraction

XRD was used to determine the bulk crystallinity and composition of nano-Fe0 solids extracted from both oxic and anoxic batch systems at periodic intervals during the experiment (Figure 3). A transition from Fe0, with peaks centred at 44.6, 65.6, and 82.6° 2θ (lattice reflections: Fe(110), Fe(200), and Fe(211), resp.), to a mixture of akaganéite (β-FeOOH), ferrihydrite (5Fe2O3·9H2O), and magnetite (Fe3O4) was recorded for both oxic and anoxic batch systems. Total Fe0 conversion was, however, not recorded for the anoxic system with residual Fe0 present after 28 days of reaction compared to full conversion exhibited by the oxic batch system after 7 days of reaction. This is ascribed to the slower corrosion of nano-Fe0 in the absence of DO as discussed above.X-ray diffraction (XRD) spectra (for the range of 10–90° 2θ) recorded for the oxic (a) and anoxic (b) mine water batch systems after reaction times of 1 h, 2 h, 4 h, 24 h, 7 d, 14 d, and 28 d.
(a)
(b)The formation of ferrihydrite and magnetite was not unexpected, given that both species are common Fe0 corrosion products in near-neutral to alkaline solutions [34–38]. The presence of chloride ions (which are necessary for akaganéite formation) was likely to have been provided by the dissolution of FeCl2, present in the nano-Fe0 due to incomplete conversion of FeCl2 to Fe0 during the nano-Fe0 synthesis. In the latter stages of the reaction (>7 days) the akaganéite peak was recorded to shift by approximately −0.5° 2θ, suggesting an increase in the lattice parameter of the material. This was attributed to cationic substitution of a larger ion, such as Ca2+ (0.212 nm compared to 0.166 nm), into the lattice structure [39].


### 3.6.2. X-Ray Photoelectron Spectroscopy

X-ray photoelectron spectroscopy (XPS) was used to determine the surface chemistry of extracted particulates including any sorbed species extracted from the oxic and anoxic batch systems at regular intervals throughout the experiment (Figure4). Curve fitting of recorded Fe 2p3/2 photoelectron peaks (not shown) determined a decrease in the Fe2+/Fe3+ ratio throughout the reaction period, ascribed to the oxidation of the nanoparticle surfaces. This occurred most rapidly during the initial stages of the reaction, with oxic and anoxic systems recording a shift in Fe2+/Fe3+ ratio to 0.23 and 0.32, respectively, after 1 hour of reaction. The higher proportion of Fe3+ in the oxic system is attributed to a greater concentration of DO at the start of the reaction. Following this initial and rapid oxidation phase, a more gradual decrease in the Fe2+/Fe3+ ratio was recorded in all oxic systems to minima of 0.11 after 28 days of reaction. In contrast, no appreciable change was recorded for all anoxic systems, indicating that minimal nano-Fe0 oxidation had occurred.Figure 4
Curve fitted XPS U 4f photoelectron peaks acquired after 24 hours of reaction for mine water batch systems treated with nano-Fe0.XPS data recorded from the samples of extracted particulates failed to record detectable peaks in the U 4f binding energy region of the recorded photoelectron spectra in all the reacted samples, even during the initial period of maximum U removal. This was not unexpected, given the small amount of U in each system (1413μ L−1) relative to the large surface area presented by the nanoparticles (14.8 m2 g−1). U 4f photoelectron peaks were detected for both oxic and anoxic mine water samples after 4 hours of reaction. Curve fitting, following the method of Scott et al., determined that U present was in a partially reduced state for both systems with a U4+/U6+ ratio of 0.34 and 1.13 recorded for the oxic and anoxic system, respectively. Greater proportion of U4+ relative to U6+ recorded for the anoxic batch system is attributed to enhanced chemical reduction of U in low oxygen conditions. This is likely to be due to the significantly lower (and sustained) Eh conditions imbued by the nano-Fe0 in the low oxygen environment, where Fe0 is maintained throughout the 28-day reaction period (see Section 3.6.1). In contrast Fe0 was recorded to be oxidised to (oxy)hydroxide species more rapidly in the batch systems containing dissolved oxygen, which would have resulted in lower chemical reduction of U6+ to U4+.


## 3.6.1. X-Ray Diffraction

XRD was used to determine the bulk crystallinity and composition of nano-Fe0 solids extracted from both oxic and anoxic batch systems at periodic intervals during the experiment (Figure 3). A transition from Fe0, with peaks centred at 44.6, 65.6, and 82.6° 2θ (lattice reflections: Fe(110), Fe(200), and Fe(211), resp.), to a mixture of akaganéite (β-FeOOH), ferrihydrite (5Fe2O3·9H2O), and magnetite (Fe3O4) was recorded for both oxic and anoxic batch systems. Total Fe0 conversion was, however, not recorded for the anoxic system with residual Fe0 present after 28 days of reaction compared to full conversion exhibited by the oxic batch system after 7 days of reaction. This is ascribed to the slower corrosion of nano-Fe0 in the absence of DO as discussed above.X-ray diffraction (XRD) spectra (for the range of 10–90° 2θ) recorded for the oxic (a) and anoxic (b) mine water batch systems after reaction times of 1 h, 2 h, 4 h, 24 h, 7 d, 14 d, and 28 d.
(a)
(b)The formation of ferrihydrite and magnetite was not unexpected, given that both species are common Fe0 corrosion products in near-neutral to alkaline solutions [34–38]. The presence of chloride ions (which are necessary for akaganéite formation) was likely to have been provided by the dissolution of FeCl2, present in the nano-Fe0 due to incomplete conversion of FeCl2 to Fe0 during the nano-Fe0 synthesis. In the latter stages of the reaction (>7 days) the akaganéite peak was recorded to shift by approximately −0.5° 2θ, suggesting an increase in the lattice parameter of the material. This was attributed to cationic substitution of a larger ion, such as Ca2+ (0.212 nm compared to 0.166 nm), into the lattice structure [39].


## 3.6.2. X-Ray Photoelectron Spectroscopy

X-ray photoelectron spectroscopy (XPS) was used to determine the surface chemistry of extracted particulates including any sorbed species extracted from the oxic and anoxic batch systems at regular intervals throughout the experiment (Figure4). Curve fitting of recorded Fe 2p3/2 photoelectron peaks (not shown) determined a decrease in the Fe2+/Fe3+ ratio throughout the reaction period, ascribed to the oxidation of the nanoparticle surfaces. This occurred most rapidly during the initial stages of the reaction, with oxic and anoxic systems recording a shift in Fe2+/Fe3+ ratio to 0.23 and 0.32, respectively, after 1 hour of reaction. The higher proportion of Fe3+ in the oxic system is attributed to a greater concentration of DO at the start of the reaction. Following this initial and rapid oxidation phase, a more gradual decrease in the Fe2+/Fe3+ ratio was recorded in all oxic systems to minima of 0.11 after 28 days of reaction. In contrast, no appreciable change was recorded for all anoxic systems, indicating that minimal nano-Fe0 oxidation had occurred.Figure 4
Curve fitted XPS U 4f photoelectron peaks acquired after 24 hours of reaction for mine water batch systems treated with nano-Fe0.XPS data recorded from the samples of extracted particulates failed to record detectable peaks in the U 4f binding energy region of the recorded photoelectron spectra in all the reacted samples, even during the initial period of maximum U removal. This was not unexpected, given the small amount of U in each system (1413μ L−1) relative to the large surface area presented by the nanoparticles (14.8 m2 g−1). U 4f photoelectron peaks were detected for both oxic and anoxic mine water samples after 4 hours of reaction. Curve fitting, following the method of Scott et al., determined that U present was in a partially reduced state for both systems with a U4+/U6+ ratio of 0.34 and 1.13 recorded for the oxic and anoxic system, respectively. Greater proportion of U4+ relative to U6+ recorded for the anoxic batch system is attributed to enhanced chemical reduction of U in low oxygen conditions. This is likely to be due to the significantly lower (and sustained) Eh conditions imbued by the nano-Fe0 in the low oxygen environment, where Fe0 is maintained throughout the 28-day reaction period (see Section 3.6.1). In contrast Fe0 was recorded to be oxidised to (oxy)hydroxide species more rapidly in the batch systems containing dissolved oxygen, which would have resulted in lower chemical reduction of U6+ to U4+.


## 4. Discussion

Nano-Fe0 have been tested in the current work for the removal of U from mine water batch systems in both dissolved oxygen containing (starting DO ~ 9.5 ppm and batch systems handled and stored in the open laboratory) and anoxic (starting DO < 0.1 ppm and batch systems handled and stored in a nitrogen-filled glovebox) batch systems. Nano-Fe0 were documented as highly effective for the rapid removal of U despite the high concentration of complexing agents present in the mine water, namely, bicarbonate at 974 ppm, with near-total U removal recorded after 1 hour of reaction for all systems studied. Limited long term U removal, however, was recorded for the batch systems with DO present, with significant U rerelease recorded within 7 days of nano-Fe0 application. In contrast, no appreciable U rerelease was recorded for the anoxic mine water batch system. XRD analysis of nano-Fe0 extracted from both oxic and anoxic systems determined that whilst total conversion of nano-Fe0 to (oxy)hydroxide corrosion products had occurred in the oxic systems, Fe0 was maintained in the anoxic systems. Concurrent XPS analysis determined that sorbed U was present in a partially reduced state in both oxic and anoxic systems; however, greater chemical reduction was recorded for the anoxic systems. The mechanism of U rerelease in the oxic systems is therefore attributed to the incomplete chemical reduction of surface-precipitated U (from soluble U6+ to insoluble U4+) within the mine water samples, allowing the rerelease of U6+ during the ingress of DO back into batch systems, and the reformation of highly stable (nominally carbonate) aqueous U-complexes. This was not recorded for the anoxic systems because the absence of DO allowed Fe0 to be maintained (and associated strongly chemically reducing conditions) throughout the 28-day reaction period. Figure 5 displays a schematic diagram of this hypothesis applied for thein situ treatment of metal and metalloid aqueous contaminant species using nanoscale zero-valent iron particles.Figure 5
Schematic diagram of the following: (a) a typical nanoparticle injection well: the technology is very similar to that used for injection of CO2 into subterranean storage reservoirs; (b)in situ vadose (oxic) zone treatment of metal and metalloid aqueous contaminant species using nanoscale zero-valent iron particles: contaminants remobilise shortly after nanoparticle injection due to the abundant supply of dissolved oxygen; and (c)in situ phreatic (anoxic) zone treatment of metal and metalloid aqueous contaminant species using nanoscale zero-valent iron particles: contaminants remain immobilised due to the limited supply of dissolved oxygen.


## 5. Conclusions

The rerelease of metal and metalloid contaminant species following a period of “apparent remediation” is a key engineering challenge which may limit the development of nano-Fe0 as a new technology for mine water treatment. The current work has provided clear evidence that nano-Fe0 is only appropriate for thein situ treatment of U in surface and/or vadose zone waters if extremely robust secondary method(s) are applied to prevent DO ingress into the contaminant treatment zone. Example materials include impermeable geomembranes and bentonite. For thein situtreatment of anoxic mine water, it is shown that U removal can be maintained on a long term or even quasi-permanent basis if there is sufficiently low DO flux to maintain the strongly chemically reducing groundwater conditions imbued by the nano-Fe0.Further work is required to examine the reversible nature of metal and metalloid remediation in complex and/or natural waters using nano-Fe0. This will provide validation of the technology for sites where assurance of medium to long term immobilisation of contaminants is required.



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*Source: 956360-2014-05-25.xml*