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Membrane electrodes, also known as p-ion electrodes, use membranes that selectively interact with free analyte ions, generating a potential difference across the membrane. The resulting membrane potential, known as the asymmetry potential, is not zero even when analyte concentrations on both sides of the membrane are equal. The membrane's response is typically not selective to a single analyte but proportional to the concentration of all ions in the sample solution capable of interacting at...
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The carbonic acid-bicarbonate buffer system is critical for maintaining the body's pH balance. It operates on the equilibrium:
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Controlled-potential coulometry, also known as potentiostatic coulometry, employs a three-electrode system in which the working electrode's potential is precisely regulated using a potentiostat. Platinum working electrodes are utilized for positive potentials, while mercury pool electrodes are favored for extremely negative potentials. The platinum counter electrode is separated from the analyte using a membrane or salt bridge to avoid interference in the analysis.
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Controlled-Current Coulometry: Overview01:27

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Controlled current coulometry, also known as amperostatic coulometry, is a technique used in electrochemical analysis to measure the quantity of a substance through the controlled passage of current. It involves the application of a constant current to an electrochemical cell containing the analyte of interest. As the current flows through the cell, the analyte undergoes a redox reaction at the electrode surface, resulting in a charge transfer. By monitoring the time required for a certain...
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Electrochemical Systems01:24

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Electrochemical systems provide a fascinating insight into the dynamic interplay of charged species within various phases. One notable example is the interaction between a membrane permeable to K⁺ ions but not to Cl⁻ ions, separating an aqueous KCl solution from pure water. As K⁺ ions diffuse through the membrane, they generate net charges on each phase, leading to a potential difference between them.Similarly, when a piece of Zn is immersed in an aqueous ZnSO₄ solution,...
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Efficient Bicarbonate Electrolyzer with a Forward-Bias Bipolar Membrane.

Mingyi Wang1, Wenke Lian1, Wenrui Zhang1

  • 1School of Materials and Energy, University of Electronic Science and Technology of China, Chengdu 611731, P. R. China.

ACS Applied Materials & Interfaces
|April 7, 2026
PubMed
Summary
This summary is machine-generated.

Direct electrolysis of captured carbon dioxide (CO2) in bicarbonate solutions is enhanced using a forward-bias bipolar membrane (fBPM). This method improves CO2 conversion efficiency and viability for integrated capture and electrochemical conversion.

Keywords:
CO productionbicarbonate electrolysisenergy efficiencyforward-bias bipolar membranemembrane electrode assembly

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Area of Science:

  • Electrochemistry
  • Materials Science
  • Chemical Engineering

Background:

  • Direct electrolysis of CO2-captured bicarbonate solutions is a promising CO2 valorization strategy.
  • Existing methods often suffer from low energy efficiency due to proton-driven CO2 release and hydrogen evolution.

Purpose of the Study:

  • To demonstrate a novel bicarbonate electrolyzer utilizing a forward-bias bipolar membrane (fBPM).
  • To decouple local CO2 release from proton flux for improved electrochemical performance.

Main Methods:

  • Fabrication and testing of a bicarbonate electrolyzer employing an fBPM.
  • Utilizing operando Raman spectroscopy to analyze the cathode-membrane microenvironment.
  • Conducting system-level energy analysis for CO2 conversion.

Main Results:

  • The fBPM cell achieved a high CO partial current density of 167.1 mA cm-2 at 4.44 V.
  • CO Faradaic efficiencies reached up to 71% at 100 mA cm-2.
  • The fBPM maintained an alkaline cathode-membrane microenvironment, enhancing local CO2 availability.

Conclusions:

  • The fBPM-based electrolyzer offers superior performance compared to other configurations.
  • This approach presents a viable method for integrated CO2 capture and electrochemical conversion with an energy cost of 36.7 GJ/tonne CO.