The technology at the heart of the study, published in Nature Communications, is anodic oxidation, an electrochemical process in which a contaminated stream flows past a positively charged electrode. At that electrode, water molecules are split to form hydroxyl radicals, extraordinarily reactive fragments of water that attack organic pollutants and break them down into simpler, less harmful compounds. In principle, anodic oxidation is ideal for treating emerging contaminants because the hydroxyl radicals it generates are powerful enough to degrade an enormous range of chemical structures, and the process requires no added chemical reagents. In practice, however, the technology has been held back by two stubborn limitations: the kinetics of water splitting at the electrode interface are sluggish, meaning that hydroxyl radicals are produced slowly, and the effective oxidation range is limited, so some contaminants escape degradation even after prolonged treatment.

Those limitations have real economic consequences. The benchmark electrode material for industrial anodic oxidation is boron-doped diamond, a synthetic carbon material prized for its chemical inertness and its ability to generate hydroxyl radicals with high efficiency. But boron-doped diamond is expensive to manufacture in the large areas needed for full-scale treatment plants, and the high energy costs of driving sluggish water-splitting reactions compound the financial burden. The Sichuan University team, led by corresponding authors Ye Du and Bo Lai, with Tong Liu and Shuang Zhong as co-first authors, set out to attack the problem not at the level of the electrode material but at the level of the water molecules sitting immediately adjacent to it, where the critical chemistry actually happens.

The key insight concerns hydrogen bonds, the weak but pervasive electrostatic attractions that link water molecules to one another and give liquid water many of its unusual properties. In bulk water, hydrogen bonds constantly form, break, and rearrange, creating a dynamic network. At an electrode surface, however, this network takes on a specific structure, and that structure directly controls how easily a water molecule can be pulled apart into a hydroxyl radical and a proton. If the O–H bonds within interfacial water molecules can be weakened, and if the local hydrogen-bond network can be made denser and more cooperative, water dissociation becomes faster, and with it the production of hydroxyl radicals. The question was how to achieve that reorganization deliberately, using a cheap and practical additive rather than exotic surface engineering.

The answer the researchers found was ferric iron, Fe3+, a common and inexpensive metal ion. When dissolved into the electrolyte, Fe3+ exerts a strong hydration and polarization effect on nearby water molecules: its high positive charge pulls on the electron clouds of surrounding water, distorting them and reorganizing the hydrogen-bond network at the electrode interface. Using spectroscopic and analytical probes of the interfacial region, the team documented a striking structural shift. The population of a particular hydrogen-bond motif, in which a water molecule donates hydrogen bonds to four neighboring waters, known as the 4-HB-H2O configuration, increased from 21 percent to 37 percent of the interfacial water population. Simultaneously, the O–H bonds within the reorganized water molecules were measurably weakened, making them easier to break.

The consequences for reaction kinetics were dramatic. With the hydrogen-bond network reconfigured by Fe3+, water dissociation at the electrode accelerated markedly, and the concentration of hydroxyl radicals in the system rose sevenfold compared with the untreated case. The iron ion did more than simply speed up radical production: the team found that Fe3+ also participates in the formation of high-valent iron species, reactive iron complexes that add a second, complementary oxidation pathway to the system. Together, the boosted hydroxyl radical flux and the high-valent iron chemistry widened the effective oxidation range of the process, allowing it to degrade contaminants that would otherwise resist treatment, and to do so non-selectively across a diverse panel of emerging pollutants.

Perhaps the most important result for real-world deployment is the demonstration of endurance. Laboratory-scale electrochemical water treatment studies frequently report impressive removal efficiencies over short experiments, but industrial operators need systems that run continuously for weeks without losing performance. The Fe3+-mediated system sustained stable long-term flow operation for 500 hours, maintaining approximately 95 percent removal efficiency for the target contaminants throughout. That combination of sustained performance and non-selective degradation addresses the two criteria that most often separate promising laboratory results from viable industrial processes: reliability over time and robustness across the variable mixture of chemicals found in real wastewater.

The economics are equally significant. According to the study, the system achieves a 44.3 percent cost reduction relative to conventional treatment based on boron-doped diamond electrodes. That saving stems from the fact that the strategy relies on adding a cheap metal salt to the electrolyte rather than manufacturing costly electrode materials, while the accelerated interfacial kinetics reduce the electrical energy required per unit of pollutant destroyed. For an industry in which energy and capital costs are the primary barriers to adopting advanced oxidation technologies, a cost reduction of that magnitude could be the difference between anodic oxidation remaining a niche solution and becoming a mainstream one.

Scientifically, the work adds to a growing body of evidence that the structure of interfacial water, long treated as a background detail in electrochemistry, is in fact a controllable variable with outsized influence on reaction outcomes. Recent studies from other groups have shown that hydrogen-bond engineering can sustain oxygen evolution at industrial current densities and that modulating water’s hydrogen bonding in non-aqueous environments can steer its reactivity in electrochemical transformations. The Sichuan University study extends this principle to environmental engineering, showing that the same molecular-scale lever can be pulled to solve a practical pollution problem. It suggests a broader design philosophy for electrochemical technologies: instead of focusing exclusively on the solid electrode, engineers can tune the liquid side of the interface, where the reactants actually live.

Challenges remain before the approach can be scaled from a laboratory flow cell to a municipal or industrial treatment plant. Operators will need to manage the fate of the iron additive, control its concentration across varying water chemistries, and confirm long-term performance across the full diversity of real effluents rather than representative contaminant panels. Nevertheless, the demonstration that a simple ionic additive can rewire the hydrogen-bond network at an electrode, multiply hydroxyl radical production sevenfold, sustain 500 hours of continuous operation at 95 percent removal, and cut costs by nearly half marks a substantial advance. For the vast quantities of wastewater contaminated with isothiazolinones and other emerging pollutants, the path to cleaner water may run not through new materials, but through the hidden architecture of water itself.

Subject of Research: Ferric-ion-mediated reconfiguration of interfacial hydrogen-bond networks to enhance anodic oxidation for wastewater treatment

Article Title: Reconfiguring interfacial hydrogen-bond networks to enhance anodic oxidation for efficient wastewater treatment

Article References: Liu, T., Zhong, S., Liang, X., Zhu, H., Du, Y., & Lai, B. (2026). Reconfiguring interfacial hydrogen-bond networks to enhance anodic oxidation for efficient wastewater treatment. Nature Communications. https://doi.org/10.1038/s41467-026-78208-2

Image Credits: AI Generated

DOI: 10.1038/s41467-026-78208-2

Keywords: anodic oxidation, hydroxyl radicals, hydrogen bonds, wastewater treatment, electrocatalysis, ferric iron, isothiazolinones, emerging contaminants, boron-doped diamond, water dissociation, high-valent iron, pollution remediation