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Perspective

The Use of H2 in Catalytic Bromate Reduction by Nanoscale Heterogeneous Catalysts

by
Nurbek Nurlan
1,2,†,
Ainash Akmanova
2,† and
Woojin Lee
2,3,*
1
Pharmacology and Toxicology, School of Medicine, Nazarbayev University, Nur-Sultan 010000, Kazakhstan
2
Green Energy and Environmental Research Group, National Laboratory Astana, Nazarbayev University, Nur-Sultan 010000, Kazakhstan
3
Civil and Environmental Engineering, School of Engineering and Digital Sciences, Nazarbayev University, Nur-Sultan 010000, Kazakhstan
*
Author to whom correspondence should be addressed.
†
These authors contributed equally to this work.
Nanomaterials 2022, 12(7), 1212; https://doi.org/10.3390/nano12071212
Submission received: 23 February 2022 / Revised: 19 March 2022 / Accepted: 22 March 2022 / Published: 4 April 2022
(This article belongs to the Special Issue Nano Geochemistry: Risk Assessment and Green Environmental Applications)
Versions Notes

Abstract

:
The formation of bromate (BrO3−)in groundwater treatment is still a severe environmental problem. Catalytic hydrogenation by nanoscale heterogeneous catalysts with gaseous H2 or solid-state H2 has emerged as a promising approach, which relies on reducing BrO3− to innocuous Br− via the process of direct electron transfer or reduction with atomic hydrogen. Several nanocatalysts have demonstrated high efficiency with a 100% effective BrO3− reduction with greater than 95% of Br− generation in the batch and continuous reactors. However, this technology has not been widely adopted in water treatment systems. Indeed, this research article summarizes the advantages and disadvantages of these technologies by highlighting the factors of nanomaterials reduction efficiency, long-term durability, and stability, as well as addressing the essential challenges limiting the implementation of the use of H2 for BrO3− reduction. In this work, we provide an economic evaluation of catalytic BrO3− removal, safe hydrogen supply, storage, and transportation.

1. Introduction

Bromate (BrO3−) is the most common disinfection byproduct in drinking water treatment systems, and its contamination has become a significant barrier to its use in the disinfection process. BrO3− is a category I and group B2 carcinogen; therefore, its maximum permissible concentration has been set to 10 µg/L by World Health Organization (WHO) [1,2,3]. It is primarily originated from the ozonation process where the bromate precursor, bromide (Br−), derived from natural and anthropogenic sources, leads to the formation of hypobromous acid (HBrO) and hypobromite (BrO−). These can be subsequently oxidized to bromate by ozone radicals [4]. Due to the well-developed process of sodium hypochlorite manufacturing, BrO− can also be formed from the frequent presence of aqueous bromide in the chlorine disinfection process [5]. In recent years, the catalytic hydrogenation of BrO3− reduction by nanoscale heterogeneous catalysts has emerged as a promising solution to the need to control bromate in disinfected groundwater and drinking water.
Catalytic BrO3− reduction technology has a series of distinct advantages. Due to its fast reaction kinetics towards contaminants, high efficiency, and extended durability, bromate reduction by nanoscale heterogeneous catalysts could be potentially applied to current groundwater and surface water treatment systems [6]. Based on the evaluation of significant environmental factors, these technologies exhibited reliable stability and cost-effectiveness [7]. Moreover, the catalysts with potential applications were able to reduce BrO3− efficiently using H2-releasing chemical agents, while the catalytic bromate reduction has been widely reported in the presence of H2 gas [7,8]. This has been considered a significant hurdle to applying the catalyst process to the natural water and groundwater treatment plant due to safety issues [9]. Numerous studies have evaluated and assessed overall the catalytic reduction technologies available; however, a review on the use of H2 for the catalytic hydrogenation of BrO3− has not been conducted yet. The current prospects of catalytic technology for the successful reduction of BrO3− need to be updated in light of recent studies.
The main objectives of this review are to provide a summary of the relevant reaction mechanisms and implications of catalytic technology with and without H2 gas and with H2-releasing chemical agents for the enhanced reduction of BrO3− in the water and groundwater treatment process focused on the following aspects: (1) nanoscale heterogeneous materials’ catalytic performance for BrO3− hydrogenation, (2) the safe and efficient use of H2 sources, (3) the effect of H2 use on the long-term durability of nanomaterials. An economic evaluation of the technologies is given, followed by a discussion on the safe and efficient use of H2. The review paper concludes by suggesting the future research needed for removing bromate and prioritizing H2 use in order to achieve full-scale potential application in water and groundwater treatment.

2. Reaction Mechanism of Catalytic BrO3− Removal

The reduction of BrO3− by nanoscale heterogeneous catalysts is a multi-step redox reaction requiring noble and/or promoter metals in their reduced forms and an additional reducing agent (H2 or borohydrides). The primary reaction mechanism of catalytic BrO3− reduction can be described through sequential reactions commonly shown in most of the oxyhalide contaminants, i.e., (1) BrO 3 − + 2 H + + 2 e − → BrO 2 − +   H 2 O ; (2) BrO 2 − + 2 H + + 2 e − → BrO − +   H 2 O ; (3) BrO − + 2 H + + 2 e − → Br − +   H 2 O [10,11]. Before the initiation of catalytic BrO3− hydrogenation, the nanoscale heterogeneous catalysts need to be in a reduced form, i.e., zerovalent metals, to reduce the BrO3−. Process 1: the reaction is able to start with the adsorption of BrO3− on the catalysts’ surface where BrO3− is reduced to Br−. Hamid et al. reported that the activation of H2 to reactive Hads (Pd0 + H2 → Pd-2Hads) plays a vital role in catalytic hydrogenation by nanoscale heterogeneous catalysts [12]. The reactive Hads is responsible not only for the reduction of BrO3− but also for the reduction of the metal. Process 2: the adsorbed BrO3− on the surface of catalysts is able to be reduced to Br− by direct electron transfer from the active catalytic sites [13]. Process 3: H2 gas from an external source or hydrolysis of reductants (e.g., NaBH4) further reacts with bromate in the bulk phase of suspension [14]. Hydrogen could also be formed via the water-splitting reaction of nanoscale heterogeneous catalysts in a bulk aqueous solution.

3. Nanoscale Heterogeneous Catalysts for BrO3− Reduction

3.1. Direct Bromate Reduction by Nanoscale Heterogeneous Catalysts without H2

Several nanocatalysts, e.g., zerovalent metals with different supporting materials, have been extensively studied in order to efficiently reduce BrO3− via direct electron transfer without H2. Various noble and trace metals such as Pd, Pt, and Ru on an activated carbon support, nanoscale-zero-valent iron on modified activated carbon (NZVI/MAC), and Green Nanoscale-Zero-Valent Iron (G-NZVI) catalysts showed an excellent level of performance in eliminating BrO3− when no hydrogen was present in their reactions [15,16]. The G-NZVI and NZVI/MAC catalysts showed an enhanced reduction of BrO3− at 2 and 5 min with negligible adsorption on the surface by generating ~100% and ~83% of Br−, respectively (Table 1). These catalysts are low-cost materials with high reductive capacity, and their application in water and groundwater treatment has the potential to attract intense interest. At the same time, Pd, Pt, and Ru supported on the activated carbon demonstrated much slower kinetics, with a complete conversion of BrO3− to Br−. The possible advantages of a nanoscale heterogeneous catalyst system without gaseous H2 are a safe and easy operation process, cost-effectiveness, and remarkable efficiency in the removal of bromate. However, the catalyst system might have distinct disadvantages in terms of the catalyst’s degree of durability and sustainability. The catalytic reactivity of Pd/C and Pt/C gradually decreased over multiple cycles of catalyst usage; however, Ru/C showed durability for five consecutive cycles with a moderate loss of reduction activity [13]. Moreover, the present environmental remediation technologies require more stable and reactive catalytic materials for a long-term operation. Therefore, using gaseous H2 or alternative H2 sources could enhance reactivity and prolong longevity during the successful process of BrO3− removal designed to be implemented in actual water and groundwater treatment systems.

3.2. Catalytic Bromate Reduction by Nanoscale Heterogeneous Catalysts with H2

To enhance the reactivity of the nanoscale catalysts during the direct reduction of bromate, the H2 induced-catalytic approach using various materials has been studied in batch and continuous reaction systems [19,25]. The H2, a reducing agent, needs to be provided for the hydrogenation of BrO3− and the reduction of metals. Compared to heterogeneous catalysts without an H2 source, the primary advantages of those with gaseous H2 are the faster reaction kinetics and the complete removal of BrO3− to Br−. For instance, a successful and efficient BrO3− reduction was achieved by Pd/Cu-Y (metals over faujasite zeolite) and mono and bimetallic on Zeolite Socony Mobile-5 (Cu-Pd)-ZSM5 in 2 and 10 min, respectively, while only 70% of BrO3− was removed with only H2 in 120 min (Table 1) [19,21]. Various metals, including Pd, Pt, Rh, and Ru, were deposited on the surface of activated carbon, also resulting in the complete conversion of BrO3− to innocuous Br− within 30 min [18].
The presence of gaseous H2 facilitated the reduction process by accelerating and simultaneously decreasing the surface passivation of catalysts. It is a well-known fact that the bromate reduction mechanism by metals involves H2 chemisorption on the metal surface, and the most active catalysts usually form medium-strength bonds with hydrogen [26]. It has been found that Pd metal adsorbs H2 on its surface and subsequently activates it for the process of bromate removal (Pd + H2 → 3Hads–Pd). Therefore, a continuous, constant supply of H2 gas (20 mL/min) prolongs the catalyst’s lifetime, ensuring its long-term durability. When compared to control experiments, the bimetallic catalyst supported by NZVI (Cu/Pd-NZVI) in continuous operation mode showed a sustainable reduction of BrO3− for 11 h with >99% removal [12]. At optimized conditions, the complete removal of BrO3− to Br− was conserved for 24 h with a slight catalyst surface passivation over the next 100 h (Table 2). In addition, (Pd, Ru)-CNF Carbon Nanofiber/monolith catalysts demonstrated only a 10% loss in reactivity after 7 h of continuous BrO3− reduction [17]. The superior catalytic performance and longevity depends primarily on the hydrogen chemisorption ability of metals and nanomaterials. Thus, the higher adsorption capacity of H2 led to a higher degree of catalytic activity.
Several studies reported a decrease in the catalytic reactivity of nanoscale heterogeneous catalysts during BrO3− reduction without H2, which was due to the formation of OH− ions hindering the contact of BrO3− on active catalyst sites, while the constant purging with H2 resulted in a decline of suspension pH, maintaining their catalytic reactivity [12,15,27]. However, there are certain limitations involved in using gaseous H2 from an economic and/or a technical perspective. The limited solubility of gaseous H2 could lead to an inevitable waste of resources. An adequate supply of H2 is also needed for reducing and regenerating nanocatalysts before BrO3− reduction; a significantly high concentration of H2 and preparation and equilibration times are required for a successful operation. For example, such as when Pd/Cu-Y and Pd-mesoporous carbon nitride catalysts were reduced for 3 to 4 h under hydrogen flow [20]. Another disadvantage may be that due to the stirring or mechanical shaking during BrO3− reduction, the pre-purged H2 is still able to escape from the reaction solution.

3.3. Catalytic Bromate Reduction by Nanoscale Heterogeneous Catalysts with Solid-State H2

Solid-state H2 producing chemical compounds have attracted considerable attention in removing water contaminants because they release highly pure H2 gas [24,27,28]. The primary advantage of solid H2 releasing compounds (e.g., borohydrides) is that they offer a more practical and feasible approach as compared to gaseous H2 [23]. The H2 produced from the catalytic water and groundwater treatment system with solid-state H2 is able to be much more controllable than gaseous H2 and is directly and instantly managed. However, borohydrides do not possess effective catalytic reductant properties; therefore, they do not efficiently remove BrO3− in water and groundwater because of their slow kinetics of self-hydrolysis. The hydrolysis of borohydrides can be accelerated using heterogeneous catalysts. For instance, the catalytic reduction efficiency of BrO3− by the Zeolite-Imidazole Framework (ZIF-67), Material Institute Lavoisier (MIL-88A), as well as 4,4′-bipyridine and 1,3,5-benzenetricarboxylic acid ligands (Ni(4,4′-bipy)(1,3,5-BTC)) in the presence of NaBH4 showed an effective reduction in 60 min with >95% formation of Br− (Table 1) [22,23,24]. Furthermore, hydrogen evolution during BrO3− reduction is able to be controlled by the concentration of borohydrides and different catalyst loadings. Compared to the process of BrO3− removal by nanomaterial catalysts with gaseous H2, a more efficient BrO3− reduction integrated with solid borohydride hydrolysis is achievable using non-noble metals [29]. The durable and sustainable catalytic reactivity for several cycles of BrO3− reduction can be considered another advantage of using solid borohydrides, e.g., ZIF-67 and Ni(4,4′-bipy)(1,3,5-BTC) which continuously showed a complete removal in the 5th and 6th cycles (Table 2) [22,23]. A disadvantage of using solid-state H2 chemical compounds is the need for secondary treatment to treat NaBH4 byproducts (boron species, i.e., NaBO2) formed after their hydrolysis, which often impedes their industrial application [30].

4. An Economic Evaluation of Catalytic BrO3− Reduction

The apparent advantages of the catalytic reduction system with H2 in water and groundwater treatment raises the question, “Why has the drinking water industry still not adopted this technology to reduce and remove the inevitable contaminants?” The primary reasons given are related to the cost-and-safety-associated uncertainties involved. Noble metals are expensive, and the amounts required for the process of BrO3− reduction depend significantly on their level of catalytic reactivity and durability during the treatment of contaminated water and groundwater. The optimal ranges of these significant factors vary from one study to the other because of the reactor design, catalyst material type, and operating conditions. Moreover, the H2 required for BrO3− reduction is also costly and potentially dangerous to store and transport [31]. These potential concerns can hinder the implementation of this emerging and promising catalyst technology in potable water and groundwater purification.
The transportation and storage of gaseous H2 for use in the treatment technology raises potential safety concerns [32]. Several H2 storage techniques have been proposed to date, including compressed hydrogen, metal hydrides, borohydrides, cryogenic liquid hydrogen, and carbon nanotube and metal–organic framework H2 storage systems [33,34,35,36,37]. Among them, compressed H2 gas storage appears to be a suitable strategy because of its cost-effectiveness, operation simplicity, and high efficiency that is based on time and technological feasibility factors [38]. One review questioned why the catalytic bromate removal system using H2 still has not been implemented in the existing water treatment plants, while compressed H2 has already been popularly used in commercial fuel cell vehicles and the environmental catalyst technology for this has been so extensively developed [38,39,40,41]. Compressed H2 storage tanks can be used for the molecular hydrogen supply; however, this approach might require proper gas handling technology in the water and groundwater treatment.
To efficiently use hydrogen during the process of BrO3− reduction, the continuously supplied H2 needs to be adequately consumed within the retention time of the reactor. This indicates that the BrO3− consumption rate in the reactor is managed by the H2 flow rate, or the hydrogen releasing rate is equivalent to the BrO3− interaction time on the active catalyst sites. All the gaseous H2 released to the reactor needs to be adsorbed on the nanocatalysts and be further used for the BrO3− reduction before leaving as an off-gas. In the case of solid-state H2, its amount with the flow rate can be calculated easily with the borohydride dosage and catalyst concentrations [24]. Another approach for obtaining a potential near-future H2 supply might be the introduction of water-splitting catalysts and/or their combinations with the nanoscale heterogeneous catalysts in order to simultaneously produce H2 during the reduction of BrO3− [42,43,44].
The high cost of the hydrogen required for the BrO3− reduction is another factor that significantly impacts its implementation in actual water and groundwater treatment. However, to address this concern, less expensive alternative techniques for producing H2 need to be investigated that are specifically designed for the treatment, e.g., coal (1.89 $/kg), nuclear-assisted electrolysis (2.24 $/kg), natural gas (3.50 $/kg), geothermal (4.38 $/kg), biomass (6.98 $/kg), wind-driven (8.01 $/kg), and solar-based (16.01 $/kg) hydrogen production [45]. Although fossil fuel-based hydrogen production is more economical than environmentally friendly hydrogen production, most unsustainable technologies heavily emit CO2, causing potential global warming problems. Hence, renewable hydrogen sources such as solar, wind, geothermal, biomass, and nuclear-assisted electrolysis could prove to be promising and comparative alternatives, offering a sustainable means of catalytic BrO3− removal [46,47,48]. It is possible for the transition to clean hydrogen to replace the use of conventional environmental technologies with novel catalytic systems in order to meet the most recent sustainable environmental standard goals in water and wastewater treatment.
Catalyst durability is also a vital factor and essential to consider for its actual implementation. The catalytic performance of the nanoscale heterogeneous catalysts used for BrO3− reduction has been widely demonstrated to decline continuously over repeated cycles of the contaminated water and groundwater treatment in batch and continuous reactors. However, the longevity of the nanocatalysts is significantly improved during the constant supply of H2, preventing the decrease in catalytic stability and reactivity mainly attributed to the oxidation of the support materials and/or active catalyst sites [12]. An enhancement of catalyst durability has the potential to significantly reduce the cost-related limitations of the technology.

5. Concluding Remarks and Perspectives

The process of catalytic BrO3− reduction by nanoscale heterogeneous catalysts with H2 is a reliable and practical environmental technology for water and groundwater treatment. The catalytic behavior of nanoscale heterogenous catalysts in different environmental system configurations with and without gaseous H2 and solid-state H2 sources has been comparatively evaluated and assessed. The implementation of H2 gas use in the catalytic system still has disadvantages and concerns in its application to the actual large-scale treatment processes that need to be overcome. Through the proper acquisition of H2 sources, the limitations in storing, transportation, cost-effectiveness, and sustainable production can be managed and overcome to successfully implement catalytic BrO3− reduction in actual water and wastewater treatment. Future research needs to focus on an in-depth investigation of the usable storage and transportation of H2 specifically designed for water and groundwater treatment. Novel environmental materials with suitable properties that provide for the complete and efficient consumption of H2 during BrO3− reduction and minimize safety issues also need to be developed and examined in order to attract investments in pilot-scale studies.

Author Contributions

Conceptualization, W.L.; writing-original draft preparation, N.N. and A.A.; writing-review and editing, N.N., A.A. and W.L.; supervision and funding acquisition, W.L. All authors have read and agreed to the published version of the manuscript.

Funding

This work has been supported by the Research Grants of Nazarbayev University (091019CRP2106 and 021220FD1051) and the Ministry of Education and Science of the Republic of Kazakhstan (APO9260229).

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Data sharing is not applicable to this article as no new data were created or analysed in this study.

Acknowledgments

The authors would like to thank the anonymous reviewers who helped to significantly improve the quality of the research paper.

Conflicts of Interest

The authors declare no conflict of interest.

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Table
Table 1. The reactivity of different nanoscale heterogeneous catalysts for the reduction of aqueous BrO3−.
Table 1. The reactivity of different nanoscale heterogeneous catalysts for the reduction of aqueous BrO3−.
CatalystBromate Concentration (mg·L−1)Catalyst Dose (mg∙L−1)Source of Hydrogen, Hydrogen Flow (mL (STP) min−1)Reduction Efficiency (Time)Bromide Generation
(%)		Effective pH RangeReferences
Ru/C, Pt/C and Pd/C10500No100% (120 min)~1003–5[13]
G-NZVI50200No100% (2 min)1007[16]
NZVI/MAC0.25No100% (5 min)83.13–8[15]
NZVI (Cu-Pd)2550H2 gas, 40>99%, (11 h)100-[12]
Metal (Pd, Ru) CNF/monolith catalysts50200H2 gas, 250~70% (<25 min)~95-[17]
Pd, Rh, Ru and Pt supported on activated carbon10400H2 gas, 100100%, (<30 min)100-[18]
Pd/Cu-Y (metals over faujasite zeolite)10150H2 gas, 50100% (2 min)~100-[19]
Pd/mesoporous carbon nitride10030H2 gas, 40100% (50 min)~1002–5.6[20]
Mono and bimetallic (Cu-Pd) ZSM510500H2 gas, 50100% (10 min)100-[21]
Ni(4,4′-bipy)(1,3,5-BTC)25500NaBH4100% (15 min)>953–7[22]
ZIF-67 (carbonized)100500NaBH4100% (60 min)1003–10[23]
MIL-88A100500NaBH4100% (60 min)1003–5[24]
ZIF-67100500NaBH4100% (60 min)1003–5[24]
Table
Table 2. A summary of durability test results by nanoscale heterogeneous catalysts for repeated cycles of BrO3− reduction.
Table 2. A summary of durability test results by nanoscale heterogeneous catalysts for repeated cycles of BrO3− reduction.
CatalystNumber of CyclesRemoval EfficiencyMetal LeachingReference
Ru/C, Pt/C and Pd/C>70% after 5th cycle80%-[13]
nZVI/MAC-100%No metal leaching[15]
NZVI (Cu-Pd)24 h continuous>99%Negligible amounts of leaching for Fe, Cu, Pd[12]
Metal (Pd, Ru) CNF/monolith catalysts10% loss, 7 h continuous~70%No metal leaching[17]
Pd, Rh, Ru and Pt supported on activated carbon5100%-[18]
Pd/Cu-Y (metals over faujasite zeolite)2100%No metal leaching[19]
Pd/mesoporous carbon nitride-100%-[20]
Mono and bimetallic (Cu-Pd) ZSM53100%Cu, less than 1% of the initial amount; negligible[21]
(Ni(4,4′-bipy)(1,3,5-BTC)6100%Negligible, 0.002 µg⋅L−1[22]
ZIF-67 (carbonized)4100%-[23]
MIL-88A5 (with minor loss)100%No metal leaching[24]
ZIF-675100%No metal leaching[24]
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Nurlan, N.; Akmanova, A.; Lee, W. The Use of H2 in Catalytic Bromate Reduction by Nanoscale Heterogeneous Catalysts. Nanomaterials 2022, 12, 1212. https://doi.org/10.3390/nano12071212

AMA Style

Nurlan N, Akmanova A, Lee W. The Use of H2 in Catalytic Bromate Reduction by Nanoscale Heterogeneous Catalysts. Nanomaterials. 2022; 12(7):1212. https://doi.org/10.3390/nano12071212

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Nurlan, Nurbek, Ainash Akmanova, and Woojin Lee. 2022. "The Use of H2 in Catalytic Bromate Reduction by Nanoscale Heterogeneous Catalysts" Nanomaterials 12, no. 7: 1212. https://doi.org/10.3390/nano12071212

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