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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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The ionic work function and its role in estimating absolute electrode potentials.

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Summary

This study recalculates ionic work functions for various ions in water and non-aqueous solvents. Results reveal solvent surface potentials, with water showing a positive potential and others negative, aligning with solvent structures.

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Area of Science:

  • Physical Chemistry
  • Electrochemistry
  • Thermodynamics

Background:

  • The ionic work function is crucial for understanding ion behavior in solutions.
  • Previous studies by Randles, Trasatti, and Kelly et al. provide foundational data and methods.
  • Accurate thermodynamic data is essential for reliable calculations.

Purpose of the Study:

  • To recalculate ionic work functions using updated thermodynamic data.
  • To extend these calculations to various non-aqueous solvents (methanol, ethanol, acetonitrile, DMSO).
  • To compare ionic work functions with Gibbs energies of solvation and estimate solvent surface potentials.

Main Methods:

  • Recalculation of ionic work function data based on updated thermodynamic tables.
  • Extrapolation of calculations to methanol, ethanol, acetonitrile, and dimethyl sulfoxide.
  • Comparison with absolute Gibbs energy of solvation estimates obtained via extrathermodynamic methods.

Main Results:

  • Ionic work functions were recalculated for proton, alkali metal, and halide ions in water and four non-aqueous solvents.
  • Estimates of the absolute potential of the standard hydrogen electrode were derived for each solvent.
  • Solvent surface potentials were estimated, showing a small positive value for water and negative values for non-aqueous solvents.

Conclusions:

  • The estimated surface potentials are consistent with the known molecular structures of the solvents.
  • This work refines our understanding of ion solvation and interfacial phenomena.
  • The findings provide valuable data for electrochemical and physical chemistry research.