Related Experiment Video
Updated: May 7, 2026
06:01
EPR Monitored Redox Titration of the Cofactors of Saccharomyces cerevisiae Nar1
Published on: November 26, 2014
13.4K
Title: Identification of Redox State Based on the Difference in Solvation Dynamics
Yasuhiro Kato1,2, Jelena Muncan3, Yoshinori Hirano4
1School of Medicine, Keio University 35 Shinanomachi, Shijyuku-ku, Tokyo, 160-8582, Japan.
Chemistryopen
|March 18, 2025
Summary
This study introduces a new method using near-infrared spectroscopy to continuously monitor the redox state of glutathione (GSH/GSSG) non-invasively. This breakthrough offers potential for optimizing bioreactors by understanding cellular redox balance.
Area of Science:
- Biochemistry
- Spectroscopy
- Computational Biology
Background:
- Oxidation-reduction (Redox) reactions are vital for biological functions.
- Current methods for assessing redox states are often invasive or not continuous.
- Glutathione (GSH/GSSG) is a key cellular redox buffer.
Purpose of the Study:
- To develop a non-invasive, continuous method for evaluating glutathione redox states.
- To explore the role of water molecular conformations in redox reactions.
- To enable real-time monitoring of cellular redox balance.
Main Methods:
- Utilized aquaphotomics near-infrared (NIR) spectroscopy.
- Applied multivariate analysis to spectral data.
- Employed molecular dynamic simulations to analyze water coordination.
Main Results:
- NIR spectra clearly distinguished between reduced (GSH) and oxidized (GSSG) glutathione.
- Spectral differences were linked to water molecular conformations at the reaction site.
- Molecular dynamics confirmed distinct water coordination and hydration numbers for GSH and GSSG.
Conclusions:
- Water molecules play a significant role in modulating redox states.
- The developed NIR spectroscopy approach allows non-destructive, continuous redox assessment.
- This method has potential applications in bioreactor optimization and cellular health monitoring.
Keywords:
Redoxbiological processesglutathionenear infrared spectroscopynicotinamide adenine dinucleotidewater structureMore Related Videos
10:24Defining Hsp33's Redox-regulated Chaperone Activity and Mapping Conformational Changes on Hsp33 Using Hydrogen-deuterium Exchange Mass Spectrometry
Published on: June 7, 2018
8.6K
06:53Author Spotlight: Magnetometric Characterization of Intermediates in the Solid-State Electrochemistry of Redox-Active Metal-Organic Frameworks
Published on: June 9, 2023
1.9K
Related Concept Videos
01:24Redox Reactions
Oxidation-reduction or redox reactions involve the transfer of electrons from one molecule or atom to another. When an atom gains an electron, another atom must lose an electron, meaning oxidation and reduction must occur together. Since the redox occurs in pairs, the atom that gets oxidized is also called the reducing agent or reductant, and the atom that is reduced is also called the oxidizing agent or oxidant. A straightforward way to remember the definitions of oxidation and reduction is...
01:30Ladder Diagrams: Redox Equilibria
Ladder diagrams are useful tools for understanding redox equilibrium reactions, especially the effects of concentration changes on the electrochemical potential of the reaction. The vertical axis in the redox ladder diagrams represents the electrochemical potential, E. The area of predominance is demarcated using the Nernst equation.
Consider the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates, whereas Fe2+...
Consider the Fe3+/Fe2+ half-reaction, which has a standard-state potential of +0.771 V. At potentials more positive than +0.771 V, Fe3+ predominates, whereas Fe2+...
01:23Redox Equilibria: Overview
A reduction-oxidation reaction is commonly called a redox reaction. In a redox reaction, electrons are transferred from one species to another rather than being shared between or among atoms. The reducing agent or reductant is the species that loses electrons and gets oxidized in the process. The species that gains electrons and gets reduced in the process is the oxidizing agent or oxidant. Redox reactions are represented as two separate equations called half-reactions, where one equation...
01:21Redox Titration: Overview
Redox titration is a chemical analysis technique used to determine the concentration of an unknown substance by measuring the electron transfer in a redox (reduction-oxidation) reaction. The process involves gradually adding a titrant with a known concentration of an oxidizing or reducing agent, to the analyte, the solution with an unknown concentration, until reaching the endpoint, which indicates the completion of the reaction between the two substances. Ensuring the analyte is in a single...
01:26Redox Titration: Other Oxidizing and Reducing Agents
Besides iodine, other oxidizing or reducing agents can serve as titrants in redox titrations. Common oxidizing titrants include KMnO4, cerium(IV), and K2Cr2O7. The choice of oxidizing titrants depends on factors like stability, cost, analyte strength, and reaction rate between the analyte and titrant. KMnO4 is a strong oxidizing titrant that reduces from Mn(VII) to Mn(II) in a highly acidic solution, simultaneously oxidizing the analyte to a higher oxidation state. In this case, KMnO4 acts as a...
01:27Redox Reactions
Redox reactions are vital biochemical processes that underpin energy metabolism in cells. These reactions involve the transfer of electrons between molecules, occurring in tandem as oxidation and reduction. Oxidation refers to the loss of electrons, while reduction denotes their gain. This coupling ensures the seamless flow of electrons through metabolic pathways. For example, in bacterial metabolism, glucose undergoes oxidation to carbon dioxide, while oxygen is simultaneously reduced to...