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Review

High Selectivity Electrocatalysts for Oxygen Evolution Reaction and Anti-Chlorine Corrosion Strategies in Seawater Splitting

by
Shanshan Jiang
1,
Yang Liu
1,
Hao Qiu
1,
Chao Su
1,2,* and
Zongping Shao
2,3
1
School of Energy and Power, Jiangsu University of Science and Technology, Zhenjiang 212100, China
2
WA School of Mines: Minerals, Energy and Chemical Engineering, Curtin University, Perth, WA 6102, Australia
3
State Key Laboratory of Materials-Oriented Chemical Engineering, College of Chemical Engineering, Nanjing Tech University, Nanjing 211816, China
*
Author to whom correspondence should be addressed.
Catalysts 2022, 12(3), 261; https://doi.org/10.3390/catal12030261
Submission received: 27 January 2022 / Revised: 18 February 2022 / Accepted: 20 February 2022 / Published: 25 February 2022
(This article belongs to the Special Issue Frontiers in Electrocatalysis: Oxygen Reduction, Oxygen Evolution, and Hydrogen Evolution Reactions)
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Abstract

:
Seawater is one of the most abundant and clean hydrogen atom resources on our planet, so hydrogen production from seawater splitting has notable advantages. Direct electrolysis of seawater would not be in competition with growing demands for pure water. Using green electricity generated from renewable sources (e.g., solar, tidal, and wind energies), the direct electrolytic splitting of seawater into hydrogen and oxygen is a potentially attractive technology under the framework of carbon-neutral energy production. High selectivity and efficiency, as well as stable electrocatalysts, are prerequisites to facilitate the practical applications of seawater splitting. Even though the oxygen evolution reaction (OER) is thermodynamically favorable, the most desirable reaction process, the four-electron reaction, exhibits a high energy barrier. Furthermore, due to the presence of a high concentration of chloride ions (Cl−) in seawater, chlorine evolution reactions involving two electrons are more competitive. Therefore, intensive research efforts have been devoted to optimizing the design and construction of highly efficient and anticorrosive OER electrocatalysts. Based on this, in this review, we summarize the progress of recent research in advanced electrocatalysts for seawater splitting, with an emphasis on their remarkable OER selectivity and distinguished anti-chlorine corrosion performance, including the recent progress in seawater OER electrocatalysts with their corresponding optimized strategies. The future perspectives for the development of seawater-splitting electrocatalysts are also demonstrated.

1. Introduction

Current global energy supplies are mainly obtained from traditional fossil fuels such as coal, crude oil, and natural gas. The rising demand for energy and exhaustive exploitation of traditional sources are driving environmental pollution issues and energy dilemmas. To address these problems, many “green” technologies have been investigated to deploy renewable and environmentally friendly energy, such as solar, tidal, and wind energies [1,2,3,4]. Hydrogen is considered to be an ideal clean energy source for the future, and it can be produced by many methods, such as fossil fuel extraction, methane reorganization, photocatalytic water decomposition, and so on [5]. Among these, electrolytic water splitting provides an effective way to generate “green” hydrogen in addition to the above-mentioned intermittent renewable energy sources [6,7,8,9]. The obtained hydrogen can supply a clean and sustainable energy source as an alternative to fossil fuels, which avoids the CO2 emissions from traditional fuel combustion, and can be broadly used for transportation, heating, and energy-related fields. Water, especially fresh water, is indispensable to human life. Nowadays, industrial contamination, climate change, and population growth are all resulting in a shortage of clean water supplies. According to the state of global water resources, 97% of the water on earth is seawater, which contains 3.0 to 5.0% salts [10,11,12]. If the seawater could be directly decomposed, the abundant seawater resources on Earth could be used as an economical, almost infinite, and environmentally friendly energy source.
Electrolysis generally consists of two half reactions, the oxygen evolution reaction (OER) and hydrogen evolution reaction (HER), which occur at the anode and cathode, respectively. Both reactions need highly efficient electrocatalysts to overcome energy consumption overpotentials. After a wide variety of research efforts and tremendous advancements, researchers have successfully developed many excellent electrocatalysts for OERs and HERs, which can significantly promote the application of water splitting [13,14,15,16,17,18,19,20]. However, electrocatalysts that are both stable and highly active are still insufficient to the task, so direct electrolysis of seawater to generate H2 remains challenging. For the HER at the cathode, the kinetics of HER are slow, which requires the electrocatalysts to have high conductivity. Another problem is that the microorganisms and insoluble precipitates present in natural seawater cover the active sites on the catalyst’s surface, inhibiting HER performance. Although the electrolysis of water produces hydrogen at the cathode, it is strongly dependent on the efficiency and stability of the OER at the anode. For the OER, it involves a four-electron transfer process that inevitably leads to a high energy barrier and exhibits sluggish kinetics for seawater electrolysis. In addition, owing to the unavoidable presence of chloride ions in seawate(~0.5 M), the chloride evolution reaction (CER) also occurs at the anode at a relatively high electrochemical potential, in competition with the OER [21].
Chlorine oxidation is a multiplex reaction that varies according to several factors, such as the pH value of the electrolyte, temperature, potential, and so on [22]. Research on the selectivity of oxygen and chlorine has been taking place for decades. Developing electrocatalysts with high selectivity for OERs under high salinity has been a challenge [23,24] that is usually ascribed to the linear scaling relationship between chlorine and oxygen adsorption energy. Although the OER possesses low thermodynamic redox potential [25,26], it is not favorable in terms of kinetics as it involves the four-electrons transfer process. The reaction steps of OERs in alkaline, acidic and neutral electrolytes are shown below (Equations (1)–(8)).
Alkaline media:
OH− → OH* + e−
OH* + OH− → O* + H2O + e−
O* + OH− → HOO* + e−
HOO* + OH− → O2(g) + H2O + e−
Acidic and neutral media:
H2O → OH* + H+ + e−
OH* → O* + H+ + e−
O* + H2O → HOO* + H+ + e−
HOO* → O2(g) + H+ + e−
Figure 1 shows the diverse chlorine-containing products formed over the whole pH range [27]. The OER has a higher thermodynamic redox potential than the CER at all pH values. At parallel scales, a standard potential for hypochlorite formation is 480 mV higher for the OER. The major preliminary products of chlorine-oxidation are chlorine gas, hypochlorous acid (HOCl), and hypochlorite (OCl−) [28].
2H2O → 4H+ + O2 + 4e− (EƟ = 1.229 V vs. SHE, pH = 0)
The OER redox potential is 1.229 V vs. SHE (Equation (9)) at pH = 0, and it decreases to 0.76 V vs. SHE when in seawater at a pH value of 8. The CER is independent of the pH value of seawater. It occurs at 1.358 V vs. SHE in seawater with an average Cl− concentration of 0.55 M (Equation (10)) [29].
2Cl− → Cl2 + 2e− (EƟ = 1.358 V vs. SHE, pH = 0)
Formation of hypochlorous acid (HOCl) and hypochlorite (OCl−) are dependent on the pH value of seawater. The thermodynamic balance of chlorine in an aqueous solution is very complicated because two harmful side reactions often occur, generating hypochlorous acid (HOCl) at pH < 7.46 (Equation (11)) and hypochlorite ions (ClO−) at pH > 7.46 (Equation (12)) [26,28,30].
Cl− + 2H2O → HOCl + H+ + 2e− (EƟ = 1.48 V vs. SHE)
Cl− + 2OH− → ClO− + H2O + 2e− (EƟ = 1.57 V vs. SHE)
These products are connected through chemical processes that occur in aqueous solutions. The formation of chlorine and hypochlorite is a two-electron process, and there is an immediate kinetics rivalry with the OER [31]. Designing and developing highly reactive and selective catalysts should be comprehensively considered to alleviate these thorny problems.
Therefore, the development of suitable OER electrocatalysts is crucial for the industrial application of direct seawater splitting. Recently, increasing efforts have been made to synthesizes OER electrocatalysts with high efficiency and selectivity. Therefore, it is necessary to thoroughly investigate and systematically summarize those electrocatalysts that have high selectivity and that exhibit anti-chlorine corrosion for OERs in seawater splitting, with the aim of indicating the prospects for performance improvement strategies. In this review, we classify highly selective electrocatalysts for OERs in seawater splitting, including both noble metal-based materials and non-noble metal-based materials. In order to ensure the prolonged operation of a seawater electrolysis system, we also focus on strategies to prevent seawater corrosion, for example, the development of inherent corrosion-resistant materials, surface protective coating methods, in situ electrochemical activation methods, and other anti-corrosion strategies. Moreover, the methods of asymmetric electrolyte feeds, proton exchange membrane (PEM) electrolysis, and solid oxide electrolysis cells (SOEC) also are discussed.

2. Electrocatalysts with High OER Selectivity

2.1. Noble Metal-Based Electrocatalysts

Noble metal-based materials, such as Ir, Ru electrocatalysts, are recognized as being highly active electrocatalysts mainly due to their high intrinsic activity towards the OER as well as having more exposed active sites that are highly selective for OER in seawater splitting [32,33,34,35]. Based on the superior behavior and chemical stability of iridium in acid electrolytes, Ko and co-workers [34] prepared a train of iridium (Ir) metal-organic catalysts derived from high-surface activated carbon (AC) with an Ir loading of only 2–6 wt%. These catalysts with low Ir loading still induced the organization of atoms with an Ir center (Figure 2a). In a synthetic electrolyte (0.1 M HClO4 + 3.5 wt% NaCl), Cl2 commenced to form at 1.4 V vs. RHE and reached a maximum concentration of 27 ppm in the tested potential range (Figure 2b). The selectivity of this process in regard to OER is 21.9%. When the catalyst was tested in synthetic seawater, no chlorine was detected (Figure 2c) and the OER selectivity reached 98.5%. In addition, Ir2 exhibits a low Toefl slopes of 92 mV dec−1 and demonstrates 2 h stability under constant operating conditions (Figure 2d,e). Gayen et al. [35] reported a plumbum ruthenate pyrochlore (Pb2Ru2O7−x) electrocatalyst, with high levels of Ru(V) and oxygen vacancies, in neutral simulated seawater. It exhibited a higher OER activity and selectivity than did the benchmark RuO2. The authors analyzed the thermodynamics and kinetics of the chlorine species production reaction within a high pH environment, and experimentally verified that, under simulated seawater electrolysis, Pb2Ru2O7−x displayed superior OER selectivity (~60 times) at pH = 13 (approximately 99%) than at pH = 7 (approximately 68%). Although noble metal-based materials do exhibit excellent activity for OERs in seawater electrolysis, their wide application is still hindered by their limited reserves and high cost.

2.2. Non-Noble Metal-Based Electrocatalysts

It is imperative to exploit economical and high-activity materials as alternatives for noble metal-based catalysts. In recent years, non-noble metal electrocatalysts have been utilized for extensive OER research, including transition metal borides/carbides/nitrides/phosphides/oxides/chalcogenides, perovskites, and carbon materials. Transition metal alloys and their composites have generated widespread interest due to their capacity to balance price, performance, and durability. Great efforts and advances have been made to develop productive OER and HER electrocatalysts based on transition metal oxides (TMOs) [36,37]. Transition metal phosphides (TMPs) have been widely investigated as high-efficiency dual-functional catalysts for seawater electrolysis in alkaline solutions because of their abundance in nature, simplicity of preparation, and glorious catalytic activity [38,39]. The reactivity and conductivity of these phosphides can be optimized by improving their electronic structure [40]. Ahn et al. [41] proposed that modified Co(PO3)2 nanoparticles with a nickel-type electrode can be used as the anode material for electrocatalysis. The catalytic reaction occurs at an overpotential of ~310 mV. An oxygen detection experiment recorded that a Faradaic efficiency of 98 ± 4% was obtained (within the experimental error range) at η = 440 mV, indicating that all currents are applicable for oxygen evolution.
Over the years of OER catalyst development, Ni-Fe layered double hydroxide (LDH) has proved to be one of the most promising OER electrocatalysts due to its outstanding OER performance and low cost. Dionigi et al. [42] targeted Ni-Fe hydroxide, when they proposed design standards and operating conditions for seawater electrolysis. NiFe LDH achieved ~100% OER selectivity with a low overpotential (<480 mV) in a simulated seawater electrolyte (Figure 3a,b). Cheng et al. [43] designed an electrocatalyst, with Co-Fe LDH (CF LDH) nanoparticles loaded on a Ti-mesh, for seawater electrolysis at a near-neutral pH condition. The CF LDH nanoparticles exhibited advantageous electrocatalytic activity (η10 = 530 mV) and favorable selectivity for OERs in a simulated seawater electrolysis process. As shown in Figure 3c, a Faradaic efficiency of 94 ± 4% was achieved at a constant overpotential. Very few hypochlorites were generated during the catalytic process, implying that the oxidation of water to O2 plays a major part in the CF LDH–sea salt system. Liu et al. [44] improved the electrocatalytic activity of CoFe-LDH/nickel foam (NF) by doping Zr4+ in CoFe-LDH/NF, which can adjust its electron configuration and expose plentiful sites for catalytic reactions. The integration of Zr4+ can tune the use of O intermediates, reduce the crystallinity, and extend the surface area, thus benefitting oxidation processes at low overpotentials. Song et al. [45] prepared ultrathin nanoplates of cobalt manganese LDH (CoMn LDH) with high reactivity and stability (Figure 3d). The intrinsic activity of a CoMn LDH catalyst is greater than that of the Co and Mn oxide nanoparticles. The oxygen yield during OERs using a CoMn LDH catalyst was quantified in a 5-h electrolysis experiment, measured with a fluorescence O2 detector (Figure 3e).
The formation of a protective layer on the reactive site of the anode material is a desirable method to effectively avoid chlorine oxidation reaction on the anode. Vos and colleagues [46] certified that coating IrO2 with a layer of MnOx can extensively enhance the selectivity of the OER. In an acid medium, MnOx/IrOx showed nearly 100% OER selectivity since the MnOx layer successfully prevented the transport of chloride ions. However, this system cannot maintain efficient operation for a long time because the inactive MnOx layer blocks the active sites of the OER [46,47]. Okada et al. [47] then demonstrated that Mg-intercalated δ-MnO2 produces a superior improvement on OER selectivity. The preparation of a heterostructured catalyst, Mg-intercalated Co-doped δ-MnO2 (Mg|Co-MnO2) overlaid on α-Co(OH)2, is shown in Figure 4a. It has been proven that this heterostructured catalyst preferentially yields oxygen. The permeation of Cl− can be effectively blocked by the overlayer of Mg|Co-MnO2 that can only transport water and oxygen, while the underlayer of α-Co(OH)2 serves as an electrocatalyst for decomposing water transported from the upper layer. The interlayer space (1 × ∞) between the MnO2 layers acts as the pathway by which water molecules reach the active sites of Co(OH)2. Consequently, Mg|Co-MnO2/Co(OH)2 delivered a supreme OER efficiency of 79% (Figure 4b).
Three-dimensional (3D) porous metals have a high electrochemical surface area and exhibit advantageous electron/ion transfer. Hence, they have been attractive and effective electrodes for water splitting. For example, stainless steel is a prospective OER catalyst due to the existence of metal oxides and hydroxides on its surface, which can boost its catalytic properties [48,49]. However, the planar structure of stainless steel cannot achieve high catalytic performance on account of its low electrochemically-active surface area (ECSA) [50]. The porous 3D structure of stainless steel has received increasing attention in recent years because of its large ECSA and high porosity [51]. The application of 3D printing technology, without using any adhesive or additional processing, maximizes the OER activity of the electrode. Cellular stainless steel (CESS) manufactured by selective laser melting technology (Figure 5a) possesses high specific surface area and demonstrates superior mechanical performance [51]. More importantly, the prepared CESS electrode has good electrochemical activity, achieving an overpotential as low as ~302 mV at a current density of 10 mA cm−2 and a Tafel slope of only 43 mV dec−1 (Figure 5b).
Core-shell nanostructured materials with synergistic effects have received widespread attention in electrochemical water splitting. Bifunctional core-shell structured MoS2@CoO catalysts (Figure 5c,d) have been investigated for seawater electrolysis in alkaline and neutral solutions [52]. The reported MoS2@CoO consisted of a cobalt oxide nanocrystalline core wrapped in a 2H-MoS2 nanosheet shell. This core-shell hybrid nanostructure significantly enhanced the electrocatalytic performance for OERs. For example, a low overpotential of 325 mV at a current density of 10 mA cm−2 and a Tafel slope of 83 mV dec−1 were obtained in 1 M KOH solution, as shown in Figure 5e. For a clear comparison, we summarize the overpotential, Tafel slope, and selectivity of some representative electrocatalysts, as shown in Table 1.

3. Anti-Chlorine Corrosion Electrocatalysts and Strategies

Natural electrolytes are abundant in seawater, so corrosion is common. The phenomenon of seawater electrolytic corrosion greatly reduces the efficiency of seawater electrolysis and is the cause of huge economic losses. Accordingly, it is essential to investigate the corrosion behavior of the seawater electrolysis process and to take appropriate anti-corrosion measures. More recently, an increasing number of catalysts are being reported for seawater splitting. Other than excellent reactivity, the electrocatalysts for seawater electrolysis also need to be corrosion-resistant and stable, especially to avoid any chemical reaction with Cl− in seawater. The chloride produced by CERs could destroy the oxide film on the surface of the metal (M) and form a passive layer on the surface. The inactive part is inclined to decompose into soluble chlorides due to the intense adsorption and permeability of Cl− (Equations (13) and (14)) [55,56].
M + Cl−→ M-Clads + e−
M-Clads + Cl−→ MClx−
There are many essential factors that affect the corrosion rate, such as Cl− concentration, conductivity, hydrogen potential, and physical factors. In this section, we summarize some strategies to prevent the occurrence of seawater corrosion that has been reported in recent years. To ensure the prolonged safe operation of a seawater electrolysis system, firstly, a sensible choice of material is the most efficient aspect. The structure and properties of materials during the electrolysis process should be considered. Secondly, surface treatment and coating skills can be used to protect the boundary of metal materials and susceptible corrosive media. The surface coating can protect the internal structure from Cl− corrosion. Thirdly, some specific reactions can in situ generate anti-corrosive species, which can circumvent the mass transfer resistance caused by the external protective layer. Finally, there are some special anti-corrosion approaches. For example, adding small amounts of chemicals to the corrosive medium is a convenient, quick, and inexpensive method [57,58].

3.1. Inherent Corrosion-Resistant Electrocatalysts

The higher the potential, the easier it is for the anode to be corroded. In high-salt circumstances, transition metals (e.g., Ti and Ru) show excellent ability to withstand seawater corrosion [59,60], maintaining a sturdy framework during long-term electrolysis cycling. Ti-based materials have the characteristic of chlorine resistance. IrO2/Ti is a promising electrocatalyst for OERs in seawater splitting. For example, Yan et al. synthesized a series of γ-MnO2-type oxide electrodes based on an IrO2/Ti substrate via anodic deposition. The results demonstrated that the use of Mn-O electrodes could lead to a sharp decrease in CERs and a significant increase in OERs. In particular, when adding Mo, V, and Fe elements to the electrode, the Mn + Mo, Mn + Mo + V, and Mn + Fe + V oxide electrodes displayed oxygen evolution efficiencies of nearly 100% [61].
Besides the metal catalysts, the carbon-based substrate has a high electronic transfer rate and excellent tolerance to chloride ions, ensuring the efficiency of the integrated system. Dong et al. [62] synthesized Ni-Fe LDH nanosheet arrays supported on carbon fiber cloth (CC) (Figure 6a). The strong bond between the Ni-Fe LDH layer and the CC substrate gave the catalyst a high OER performance. The Faradaic efficiency of Ni-Fe LDH/CC was determined to be 97.7% in 1 M KOH solution. Furthermore, in seawater electrolysis, the Faradaic efficiency of Ni-Fe LDH/CC was calculated to be as high as 96.9% and no chlorine was detected during this process (Figure 6b), indicating that the CER was completely suppressed. Song et al. [63] designed novel carbon-coated Na2Co1-xFexP2O7 (NCFPO/C) nanoparticles as the OER electrocatalyst for an alkaline seawater electrolysis system (Figure 6c). Figure 6d,e show FESEM images of the CC before and after the dip-coating. It can be clearly observed that the NCFPO/C nanoparticles were uniformly loaded on the entire dip-coated CC. NCFPO/C@CC showed a favorable OER activity. More importantly, NCFPO/C@CC did not produce active chlorides that corrode the electrode in alkaline saline, exhibited a strong stability and endurance, and could continuously produce oxygen, as shown in Figure 6f.
The recent emergence of 2D transition metal carbides/nitrides, MXenes, has been reported due to their tremendous potential in corrosion resistance for seawater electrolysis. For instance, Qiu et al. [64] combined CoxMo2−xC@NG composites with MXene, and the resulting catalyst exhibited significant durability (225 h), 64 times that of Pt/C. Additionally, the reaction’s Faradaic efficiency reached 98%.

3.2. Surface Treatment and Coating Strategy

Surface coating is one of the common methods used to protect electrocatalysts from corrosion during water electrolysis [65]. Luo et al. reported a 3D core-shell electrocatalyst NiMoN@NiFeN supported on Ni foam. The synthesis procedure for the catalyst is demonstrated in Figure 7a. Scanning electron microscope (SEM) images in Figure 7b–d show that NiFeN nanoparticles were uniformly distributed on the smooth surface of the NiMoN vertical bar, which was grown on Ni foam. The presence of NiFeN nanoparticles on the NiMoN surface during OER tests not only promoted the OER activity but also was beneficial for corrosion resistance. During electrolysis in alkaline simulated seawater (1 M KOH + 0.5 M NaCl), only H2 and O2 were detected, with no chloride gases being found and the Faradaic efficiency being about 97.8% [66].
So far, different kinds of catalyst support have been manufactured, like carbon black, carbon nanofibers, metal oxides, and so on [68]. Graphene’s atomic layer is in the shape of a sp2 C-bonded 2D nanosheet [69], which is regarded as a promising support material for metal catalysts. Graphene is applied as an anti-corrosion coating additive owing to its strong stability and high mechanical strength, as well as unique characteristics such as chemical inertness, impermeability, and excellent thermal and chemical stability [70,71,72,73,74,75]. Various methods can be used to prepare graphene-based anti-corrosion coatings, such as chemical vapor deposition, spin coating, the sol-gel approach, in situ polymerization, and so on. Among these, graphene grown by chemical vapor deposition (CVD-graphene) is an excellent protective coating for metals that can prevent metal corrosion due to electrochemistry, heat, or humidity [76,77,78,79]. Jadhav et al. [67] reported a novel vibrant catalyst: FeOOH deposited onto Ni–Co hydroxide with an external graphene oxide protective layer (Figure 7e). The gas produced from the anode side was detected through gas chromatography (GC), the result revealing that only O2 was detectable. Using the o-tolidine test, it was shown that no liquid phase chloride oxide, such as HClO or ClO−, was formed during the constant current OER testing. The authors proved that the presence of oxygen functional groups in graphene oxide promoted changes in chemical properties and improved corrosion inhibition. The pure graphene-based coating can validly isolate the corrosive medium from the electrode material. However, it may also accelerate the corrosion of the underlying metal. Graphene composite materials can solve this problem well. The graphene composite not only has better corrosion resistance than traditional coatings, but it does not destroy the structure of graphene [80]. Therefore, it is a very promising anti-corrosion coating material.

3.3. In Situ Electrochemical Activation Strategy

To a certain extent, the protective layer on the surface can prevent the electrode from corroding. However, when the protective layer plays a role in blocking the transport of chloride ions, it also increases the mass transfer resistance of the catalytic reaction. The in situ generation of resistant species through surface oxidation and reconstruction is an effective way to address this issue [81,82,83,84,85]. Based on this, advanced bifunctional electrocatalysts, i.e., NiFe LDH/FeOOH heterostructured nanosheets (Figure 8a), were reported to prevent seawater electrolytic corrosion [84]. The heterostructure of NiFe LDH/FeOOH can promote the production of active NiOOH species during the reaction process. Due to the strong interaction between FeOOH and NiFeLDH, and the shape of NiOOH, it not only resists corrosion due to Cl−, but also forms a strong coupling between the two phases to improve electrochemical reactivity and stability. The polarization curves of NiFe LDH/FeOOH for OERs in alkaline simulated seawater splitting are shown in Figure 8b. When NiFe LDH/FeOOH was used as both the cathode and anode, it exhibited excellent long-term operational stability, and operated for 105 h at a large current density of 100 mA cm−2.
Nickel foam (NF) has been extensively used in the field of energy conversion and storage. Wu et al. [85] first synthesized thin carbon-coated CoS on NF (NF-C/CoS) after rapid cooling by Joule heating, and then prepared NF-C/CoS/NiOOH with a core-shell heterostructure by utilizing the reaction of the metastable Ni with water to form NiOOH nanosheets and C/CoS “seeds”, thus inducing spontaneous and continuous growth of NiOOH nanosheets (Figure 8c). As a self-supporting electrocatalyst, NF-C/CoS/NiOOH exhibited favorable oxidation reaction performance and good stability for 50,000 s in the overall water splitting test (Figure 8d). This feat contributes a new preparation method for NF-based nanomaterials and opens new development directions in the field of catalysis.

3.4. Other Strategies

In addition to the above three methods to solve the problem of seawater electrolytic corrosion, the following methods also provide us with new ideas for the prevention of seawater corrosion. Contrary to the huge efforts recently invested in the development of highly active electrocatalysts, several works have concentrated on the design of electrolytes thus far. Li and co-workers [86] used the common ion effect, that is, increasing NaOH can decrease the saturation concentration of NaCl, to inhibit the concentration of chloride ions, which can halve the solubility of NaCl in the electrolyte, resulting in NaCl crystallization. This method greatly suppressed both corrosion and CERs at the anode during the electrolysis of seawater (Figure 9a). In the simulation and calcium-magnesium-free seawater electrolysis system, the ternary NiCoFe phosphide can remain active for more than 100 h (Figure 9b). Furthermore, when applying a Nafion membrane, the rate of generation of NaCl crystals can be increased by six times owing to the transmission of sodium ions from the anode to the cathode through the Nafion membrane. This provides an idea for the design of a functional electrolyte for seawater electrolysis in the future.
Dresp et al. [87] proposed the concept of asymmetric electrolyte feeds. Neutral seawater is directly injected into the cathode, while a high-purity KOH electrolyte is circulated at the anode. In an alkaline electrolyte containing Cl−, a NiFe-LDH anode catalyst still has complete selectivity in regard to OERs without any Cl− oxidation, which allows it to operate continuously and stably under high voltage and current density.
PEM water electrolysis is one of the most promising technologies for high-purity and high-efficiency hydrogen production under high dynamic operating conditions without any carbon emissions [88,89]. In addition, the application of a PEM can enhance the corrosion resistance of a seawater electrolysis system. For instance, Rossi et al. [90] used the charge repulsion of a PEM to chloride ions to reduce the generation of chlorine. The evolution of chlorine was dramatically inhibited when introducing a humidified air stream to the anode in a saltwater electrolyte. Moreover, the pH value of the electrolyte in the overall cell could be commendably regulated due to the strengthened proton migration caused by the electric field. Consequently, the sodium ion transportation could be minimized without a liquid anolyte. In synthesized brackish water, anodic Faradaic efficiencies for oxygen evolution were nearly 100%.
Solid oxide electrolysis cells (SOECs), operating at high temperatures, can evaporate seawater into salt-free pure water vapor, as shown in Figure 10a. Nowadays, the SOEC is considered to be an excellent candidate for seawater splitting due to its remarkable stability, which can prevent any undesirable effects of the high salinity of the electrolytes. However, in the SOEC system, it is still necessary to find materials that can operate stably in high temperature environments. Furthermore, it is urgent to solve the problem of energy hunger due to the heating and evaporation of seawater. Liu and co-workers [91] evaluated the productivity and stability of this electrolysis method by splitting natural seawater. The content of water vapor in the electrolysis solution system can be controlled by changing the temperature. Hydrogen introduced into the electrode (not consumed during electrolysis) can protect Ni from oxidation. Reduction of nickel oxide to metallic nickel can be realized at the electrode (Figure 10b). High energy conversion productivity and a low cell degradation rate were achieved at a constant current density for 420 h (Figure 10c). However, the partial sea salt sediments that were detected in the air intake tube will be a primary barrier to the long-term operation of the system.

4. Conclusions and Perspectives

The ocean on the Earth can supply nearly inexhaustible seawater, which can be treated as an abundant and economic hydrogen source. For the commercial and large-scale production of hydrogen, direct seawater electrolysis provides a promising method. However, chlorine corrosion and oxidation due to the inevitable presence of chloride ions in seawater seriously impedes the utilization of this technology. Over decades, a tremendous amount of research has been conducted on material modifications and structural optimization of electrocatalysts. In this review, we summarized five different types of material for highly selective seawater splitting and introduced several effective anti-corrosion strategies. A seawater electrolysis OER catalyst needs low overpotential, long-term stability, and Cl− corrosion resistance. Here, we provided several design strategies for seawater splitting: (1) An LDH layer can be deposited or grown on a conductive substrate with large specific surface area (such as Ni Foam), and then modified to obtain the desired seawater electrolysis OER electrode material. Combined with the high conductivity of the sublayer, the LDH layer structure could enhance electron, which would contribute to high OER activity. (2) Designing 3D hierarchical porous nano-architectures is an effective strategy for increasing surface area and improving mass transport. (3) A protective layer with some anti-corrosion materials deposited on the catalyst’s surface can block Cl– ions. However, this protective layer may result in sluggish mass transport, thus damaging the catalyst’s activity. The selection and preparation of the coating layer requires elaborate design.
Although some remarkable results have been achieved, there are still some important issues that need to be addressed in the future. The issues and possible solutions are listed below:
(1)
Selection of materials with high selectivity and anti-corrosion properties. Based on data for potential candidate materials provided by previous studies, the technology of artificial intelligence could be investigated as an efficient and convenient screening approach.
(2)
Evaluation of anti-corrosion strategies. Electrocatalytic surface modification and structure optimization are effective methods for the fabrication of anti-corrosion materials. In situ-generated anti-corrosive species can avoid the mass transfer resistance caused by the external protective layer.
(3)
Novel integrated electrolytic cell unit. Reasonable design of electrolytic cells may improve the overall reaction efficiency.
(4)
High-temperature electrolysis. SOECs could be the next-generation electrolyzers for direct seawater splitting.
(5)
Due to several difficulties when using seawater directly, the preliminary desalination of sea water may be another choice.
In summary, the current research in this field is still limited. The development of electrocatalysts that have high selectivity and distinguished performance against chlorine corrosion during direct seawater electrolysis requires urgent attention.

Author Contributions

Conceptualization, Z.S., C.S. and S.J.; validation, S.J., Y.L. and H.Q.; data curation, C.S.; writing—original draft preparation, S.J., Y.L. and H.Q.; writing—review and editing, C.S. and S.J.; supervision, C.S. and S.J.; project administration, Z.S.; funding acquisition, C.S. and S.J. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the Natural Science Foundation of the Jiangsu Higher Education Institutions of China (Grant No. 2018ND133J) and the Natural Science Foundation of Jiangsu Province, China (Grant No. BK20190965).

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Not applicable.

Acknowledgments

This research was financially supported by the Natural Science Foundation of the Jiangsu Higher Education Institutions of China (Grant No. 2018ND133J) and the Natural Science Foundation of Jiangsu Province, China (Grant No. BK20190965).

Conflicts of Interest

The authors declare no conflict of interest.

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Figure 1. Pourbaix diagram for artificial seawater model [27]. Adapted with permission Ref. [27], Copyright 2016, Wiley-VCH.
Figure 1. Pourbaix diagram for artificial seawater model [27]. Adapted with permission Ref. [27], Copyright 2016, Wiley-VCH.
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Figure 2. (a) Ir-based organometallics subject to pyrolysis with activated carbon: (1,5-cyclooctadiene)(pyridine)(tricyclohexylphosphine)-iridium(I) hexafluorophosphate [34]. The activity of the Ir catalyst and the concentration of produced Cl2 (b) at pH = 1 and (c) at pH = 7 (synthetic seawater) [34]. (d) Tafel slopes and (e) Stability tests of IrO2, and Ir1–Ir6 at 10 mA cm−2 [34]. Adapted with permission Ref. [34], Copyright 2020, Wiley-VCH.
Figure 2. (a) Ir-based organometallics subject to pyrolysis with activated carbon: (1,5-cyclooctadiene)(pyridine)(tricyclohexylphosphine)-iridium(I) hexafluorophosphate [34]. The activity of the Ir catalyst and the concentration of produced Cl2 (b) at pH = 1 and (c) at pH = 7 (synthetic seawater) [34]. (d) Tafel slopes and (e) Stability tests of IrO2, and Ir1–Ir6 at 10 mA cm−2 [34]. Adapted with permission Ref. [34], Copyright 2020, Wiley-VCH.
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Figure 3. (a) TEM image of NiFe LDH nanoparticles [42]. (b) O2 Faradaic efficiency of NiFe LDH nanoparticles in 0.1 M HClO4 + 3.5 wt% NaCl [42]. (c) Faradaic efficiency of Co-Fe LDH catalyst in simulated seawater at a constant overpotential [43]. (d) Structure, TEM image, and (e) calculated and experimental oxygen production of CoMn LDH nanoplates [45]. Adapted with permission Ref. [42], Copyright 2016, Wiley-VCH. Ref. [43], Copyright 2017, Electrochimica Acta. Ref. [45], Copyright 2014, Journal of the American Chemical Society.
Figure 3. (a) TEM image of NiFe LDH nanoparticles [42]. (b) O2 Faradaic efficiency of NiFe LDH nanoparticles in 0.1 M HClO4 + 3.5 wt% NaCl [42]. (c) Faradaic efficiency of Co-Fe LDH catalyst in simulated seawater at a constant overpotential [43]. (d) Structure, TEM image, and (e) calculated and experimental oxygen production of CoMn LDH nanoplates [45]. Adapted with permission Ref. [42], Copyright 2016, Wiley-VCH. Ref. [43], Copyright 2017, Electrochimica Acta. Ref. [45], Copyright 2014, Journal of the American Chemical Society.
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Figure 4. (a) Mechanism workflow chart of Mg|Co-MnO2 formation. (b) The relationship between the charge density and OER efficiency of Mg|Co-MnO2/Co(OH)2 [47]. Adapted with permission Ref. [47], Copyright 2020, American Chemical Society.
Figure 4. (a) Mechanism workflow chart of Mg|Co-MnO2 formation. (b) The relationship between the charge density and OER efficiency of Mg|Co-MnO2/Co(OH)2 [47]. Adapted with permission Ref. [47], Copyright 2020, American Chemical Society.
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Figure 5. (a) Preparation process and (b) overpotential of CESS [51]. (c) OER mechanism, (d) TEM image, and (e) Tafel plots of MoS2@CoO [52]. Adapted with permission Ref. [51], Copyright 2019, Royal Society of Chemistry. Ref. [52], Copyright 2019, American Chemical Society.
Figure 5. (a) Preparation process and (b) overpotential of CESS [51]. (c) OER mechanism, (d) TEM image, and (e) Tafel plots of MoS2@CoO [52]. Adapted with permission Ref. [51], Copyright 2019, Royal Society of Chemistry. Ref. [52], Copyright 2019, American Chemical Society.
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Figure 6. (a) Synthesis of NiFe LDH/CC. (b) UV-vis absorption spectra of electrolytes after the stability tests [62]. (c) Schematic diagram of OERs on an NCFPO/C@CC electrode [63]. FESEM images of (d) bare CC and (e) NCFPO/C@CC [63]. (f) Stability of NCFPO/C@CC [63]. Adapted with permission from Ref. [62], Copyright 2021, Elsevier Ltd.; Ref. [63], Copyright 2019, American Chemical Society.
Figure 6. (a) Synthesis of NiFe LDH/CC. (b) UV-vis absorption spectra of electrolytes after the stability tests [62]. (c) Schematic diagram of OERs on an NCFPO/C@CC electrode [63]. FESEM images of (d) bare CC and (e) NCFPO/C@CC [63]. (f) Stability of NCFPO/C@CC [63]. Adapted with permission from Ref. [62], Copyright 2021, Elsevier Ltd.; Ref. [63], Copyright 2019, American Chemical Society.
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Catalysts 12 00261 g007 550
Figure 7. (a) Schematic image of the synthesis procedure for the NiMoN@NiFeN catalyst [66]. SEM images of (b) NiMoN and (c,d) NiMoN@NiFeN with scale bars of 30 μm, insets 3 μm [66]. (e) Schematic illustration of the preparation process [67]. Adapted with permission from Ref. [66], Copyright 2019, Springer Nature. Ref. [67], Copyright 2020, Royal Society of Chemistry.
Figure 7. (a) Schematic image of the synthesis procedure for the NiMoN@NiFeN catalyst [66]. SEM images of (b) NiMoN and (c,d) NiMoN@NiFeN with scale bars of 30 μm, insets 3 μm [66]. (e) Schematic illustration of the preparation process [67]. Adapted with permission from Ref. [66], Copyright 2019, Springer Nature. Ref. [67], Copyright 2020, Royal Society of Chemistry.
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Catalysts 12 00261 g008 550
Figure 8. (a) SEM image of NiFe LDH/FeOOH sample after the OER [84]. (b) Polarization curves of NiFe LDH/FeOOH for water splitting and alkaline simulated seawater splitting [84]. (c) Synthetic schematic of thin carbon-coated CoS on NF (NF-C/CoS) [85]. (d) Chronopotentiometry curve of NF-C/CoS/NiOOH [85]. Adapted with permission from Ref. [84], Copyright 2021, American Chemical Society. Ref. [85], Copyright 2020, Springer.
Figure 8. (a) SEM image of NiFe LDH/FeOOH sample after the OER [84]. (b) Polarization curves of NiFe LDH/FeOOH for water splitting and alkaline simulated seawater splitting [84]. (c) Synthetic schematic of thin carbon-coated CoS on NF (NF-C/CoS) [85]. (d) Chronopotentiometry curve of NF-C/CoS/NiOOH [85]. Adapted with permission from Ref. [84], Copyright 2021, American Chemical Society. Ref. [85], Copyright 2020, Springer.
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Catalysts 12 00261 g009 550
Figure 9. (a) Schematic diagram of the common-ion effect to enhance electrochemical catalytic performance. (b) Chronopotentiometry curve of ternary NiCoFe phosphide under three electrolytes [86]. Adapted with permission from Ref. [86], Copyright 2020, Research (Wash DC).
Figure 9. (a) Schematic diagram of the common-ion effect to enhance electrochemical catalytic performance. (b) Chronopotentiometry curve of ternary NiCoFe phosphide under three electrolytes [86]. Adapted with permission from Ref. [86], Copyright 2020, Research (Wash DC).
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Catalysts 12 00261 g010 550
Figure 10. Schematic diagrams of (a) SOEC device and (b) water electrolysis process in an SOEC. (c) Chronopotentiometry curve of LSCF (La0.6Sr0.4Co0.2Fe0.8O3) in natural seawater electrolytes [91]. Adapted with permission from Ref. [91], Copyright 2021, Elsevier.
Figure 10. Schematic diagrams of (a) SOEC device and (b) water electrolysis process in an SOEC. (c) Chronopotentiometry curve of LSCF (La0.6Sr0.4Co0.2Fe0.8O3) in natural seawater electrolytes [91]. Adapted with permission from Ref. [91], Copyright 2021, Elsevier.
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Table
Table 1. Electrocatalytic performance of well-developed electrocatalysts with high selectivity.
Table 1. Electrocatalytic performance of well-developed electrocatalysts with high selectivity.
CatalystsElectrolyteOverpotential η (mV)Tafel Slope (mV dec−1)SelectivityRef.
Ir @ AC0.1 M HClO4 + 3.5 wt% NaCl243 @ 10 mA cm−29278.1%[34]
Ir @ ACSynthetic seawater560 @ 10 mA cm−2/98.5%[34]
Pb2Ru2O7-xNeutral seawater480 @ 10 mA cm−2/68%[53]
Pb2Ru2O7-xAlkaline seawater~200 @ 10 mA cm−2/~99%[53]
Co(PO3)2Phosphate-buffered water~405 @ 10 mA cm−274.198 ± 4%[41]
Ni-Fe LDHBorate buffer + NaCl490 ± 4 @ 10 mA cm−251 ± 3~100%[42]
Co-Fe LDHSimulated seawater530 @ 10 mA cm−2/94 ± 4%[43]
Co-Fe-O-B1 M KOH + 0.5 M NaCl294 @ 10 mA cm−252.6 ± 0.4~100%[54]
MnOx/IrOxAcidic saline water300 @ 5 mA cm−2~43~100%[46]
Mg/Co-MnO2/Co(OH)2MgCl2 solution/15179.1%[47]
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Jiang, S.; Liu, Y.; Qiu, H.; Su, C.; Shao, Z. High Selectivity Electrocatalysts for Oxygen Evolution Reaction and Anti-Chlorine Corrosion Strategies in Seawater Splitting. Catalysts 2022, 12, 261. https://doi.org/10.3390/catal12030261

AMA Style

Jiang S, Liu Y, Qiu H, Su C, Shao Z. High Selectivity Electrocatalysts for Oxygen Evolution Reaction and Anti-Chlorine Corrosion Strategies in Seawater Splitting. Catalysts. 2022; 12(3):261. https://doi.org/10.3390/catal12030261

Chicago/Turabian Style

Jiang, Shanshan, Yang Liu, Hao Qiu, Chao Su, and Zongping Shao. 2022. "High Selectivity Electrocatalysts for Oxygen Evolution Reaction and Anti-Chlorine Corrosion Strategies in Seawater Splitting" Catalysts 12, no. 3: 261. https://doi.org/10.3390/catal12030261

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