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A chemical reaction can behave differently beside an electrode than the pH reading of the surrounding liquid would suggest. A Seoul National University team reports that this hidden local acidity or alkalinity can steer oxygen-transfer electrosynthesis—affecting both the desired reaction and the survival of its product. By adjusting electrode spacing and electrolyte flow, the researchers improved selectivity in a laboratory oxidation. The finding makes local proton activity a design variable for the reactions studied, not a universal switch for all chemistry.
What “local pH” means near an electrode
In an electrochemical reaction, electron transfer at an electrode can be coupled to ion transfer, including the movement of protons. When these processes run quickly, proton activity in the thin region immediately around an electrode can diverge from conditions in the bulk liquid. A bulk pH measurement therefore may not describe the environment in which molecules at the electrode interface are reacting.
The study, “Local pH Control Promotes Oxygen-Atom Transfer Electrosynthesis”, was published online in the Journal of the American Chemical Society on September 4, 2026. The authors combined local-pH estimates, molecular reporters and transport simulations to investigate how these interfacial conditions affect an electro-organic reaction.
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The reaction the researchers examined
The team studied oxygen-driven Baeyer–Villiger oxidation (BVO), a reaction that inserts an oxygen atom into a ketone to produce an ester or, for suitable substrates, a lactone. The paper reports isotope-labeling evidence that molecular oxygen (O2) supplies the inserted oxygen atom.
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The proposed mechanism is consistent with oxygen-derived hydroperoxyl-radical equivalents taking part in oxygen transfer. The authors also report that anodic oxidation of hydrogen peroxide generated during the electrochemical process helps sustain the flow of reactive radicals. This is mechanistic evidence for the pathway described in the paper, not proof that every detail applies to other electrosynthesis reactions.
How local proton activity can change the outcome
The researchers report opposing proton-activity gradients near the electrodes, arising from proton-coupled electrode reactions. Those gradients affected more than the reactive oxygen species: they also changed the chemistry of the ketone starting material and the lactone product.
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- Changes in local conditions could reduce the availability of reactive oxygen species needed for oxygen transfer.
- They could divert ketones through α-enolization and tautomerization rather than the desired oxidation pathway.
- They could accelerate hydrolysis of lactone products, reducing how much desired product remains.
These effects help explain why a nominally neutral bulk solution does not guarantee a neutral reaction environment at the electrode. Selectivity depends on local conditions as well as the bulk mixture and the applied electrochemical setup.
What changing the reactor achieved
The team used electrode spacing and convective electrolyte flow to attenuate local proton-activity gradients. The Seoul National University College of Engineering’s 2026 research summary reports that selectivity rose from approximately 16% to approximately 97% after local pH control through reactor redesign. Those figures describe the reported experimental conditions; they should not be read as a guaranteed improvement for other substrates, reactors or reactions.
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The paper’s abstract describes high-yield BVO across diverse ketones at elevated substrate loading and says the control strategy was also extended to electrochemical epoxidation. It does not establish that the same performance will transfer unchanged to other systems.
In the university summary, supervising author Professor Jaeyune Ryu described the implication this way: “This study transforms ‘local pH’ near the electrode from a hidden variable into a controllable design principle.” The practical insight is that reactor geometry and fluid movement can shape the chemical environment where the reaction actually occurs.
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What this finding does—and does not—show
This is a laboratory research result. The cited paper and institutional summary do not establish commercial-scale economics, manufacturing reliability or readiness for industrial production. Further scale-up and optimization would be needed before drawing those conclusions.
Using oxygen and electricity in the described pathway may suggest alternatives to externally added peroxide oxidants, but the study is not a lifecycle analysis or a plant-safety assessment. It therefore does not, by itself, demonstrate that a manufacturing process using this approach would be cleaner or safer overall.
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The broader lesson is appropriately bounded: local proton activity is an important design variable in the electro-organic reactions studied. The work shows why reaction design may need to account not only for substrates and catalysts, but also for transport and conditions immediately around the electrodes.
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