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Related Concept Videos

Ionic Association01:28

Ionic Association

The ionic association is the association of oppositely charged ions in an electrolyte solution to form ion pairs. Bjerrum defined ion pairs as two oppositely charged ions whose electrostatic attraction exceeds the thermal energy of the system, typically expressed as 2kT. Electrostatic attraction depends on ionic charge, separation distance, and the dielectric constant of the medium. Thermal energy, represented by kT, reflects the tendency of ions to move independently due to molecular motion.
Theory of Strong Electrolytes01:23

Theory of Strong Electrolytes

The interionic forces of the strong electrolytes depend on the solvent's dielectric constant, which is the ability of a solvent to store electrical energy, based on its polarizability. and the solution's concentration. In high-dielectric solvents and in dilute solutions, weak electrostatic forces keep ions apart. However, in low-dielectric solvents or concentrated solutions, stronger interionic forces may cause ions to pair up as ionic doublets despite being fully ionized. The theory of strong...
Electrolytes: van't Hoff Factor03:08

Electrolytes: van't Hoff Factor

Colligative Properties of ElectrolytesThe colligative properties of a solution depend only on the number, not on the identity, of solute species dissolved. The concentration terms in the equations for various colligative properties (freezing point depression, boiling point elevation, osmotic pressure) pertain to all solute species present in the solution. Nonelectrolytes dissolve physically without dissociation or any other accompanying process. Each molecule that dissolves yields one dissolved...
Ionic Strength: Overview01:12

Ionic Strength: Overview

The ionic strength of a solution is a quantitative way of expressing the total electrolyte concentration of a solution. This concept was first introduced in 1921 by two American physical chemists, Gilbert N. Lewis and Merle Randall, while describing the activity coefficient of strong electrolytes. During the calculation of ionic strength (I or μ), all the cations and anions are considered. However, the concentration (c) of an ion with a greater charge number (z) has a greater contribution to...
The Debye–Hückel Theory of Electrolyte Solutions01:27

The Debye–Hückel Theory of Electrolyte Solutions

The Debye–Hückel theory, established by Peter Debye and Erich Hückel in 1923, is a fundamental concept in physical chemistry. It provides an understanding of the behavior of strong electrolytes in solution, particularly explaining their deviations from ideal behavior.The theory is based on Coulombic interactions (the attraction or repulsion between charged particles) between ions in solution. In an ionic solution, oppositely charged ions tend to attract each other. This means that cations...
Chemical Equilibria: Systematic Approach to Equilibrium Calculations01:21

Chemical Equilibria: Systematic Approach to Equilibrium Calculations

Equilibrium calculations for systems involving multiple equilibria are often complex. For example, to calculate the solubility of a sparingly soluble salt in an aqueous solution in the presence of a common ion, one must consider all the equilibria in this solution. Calculations for these systems can be complicated and tedious, so a systematic approach with a series of steps is often helpful. The process is detailed below.
The first step is to identify all the chemical reactions involved, The...

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Thermochemical Studies of Ni(II) and Zn(II) Ternary Complexes Using Ion Mobility-Mass Spectrometry
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Quantifying ion-ion association in mixed electrolyte systems using bulk thermodynamic experimental data.

Elizabeth A Ploetz1, Paul E Smith1

  • 1Department of Chemistry, 213 CBC Building, 1212 Mid-Campus Dr. North, Kansas State University, Manhattan, Kansas 66506, USA.

The Journal of Chemical Physics
|May 28, 2026
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Summary

This study introduces a method to calculate ion-specific Kirkwood-Buff integrals (KBIs) for mixed electrolyte solutions. This extends KBI analysis beyond single electrolytes, enabling a deeper understanding of complex ionic interactions in solutions.

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Area of Science:

  • Physical Chemistry
  • Solution Chemistry
  • Thermodynamics

Background:

  • Kirkwood-Buff integrals (KBIs) are established for single electrolytes, relating thermodynamic data to inter-species affinities.
  • Calculating species-specific KBIs (e.g., cation-anion) is complex in mixed electrolyte systems.
  • Previous methods were restricted to single electrolyte solutions.

Purpose of the Study:

  • To develop a method for determining ion-ion KBIs in bulk mixed electrolyte solutions.
  • To extend Kirkwood-Buff theory to multicomponent ionic systems.
  • To analyze ion interactions in mixed electrolyte solutions regardless of complexity.

Main Methods:

  • Utilized Kirkwood-Buff theory combined with global and local electroneutrality constraints.
  • Applied the method to bulk thermodynamic data of mixed electrolyte solutions.
  • Correlated bulk thermodynamic data using established equations for miscible systems.

Main Results:

  • Successfully derived ion-ion KBIs for mixed electrolyte solutions like NaCl + KBr (aq) and MgCl2 + KBr (aq).
  • Demonstrated applicability across various ion concentrations, valencies, and complexities.
  • Validated results against molecular dynamics simulations for NaCl + KBr (aq), showing excellent agreement.

Conclusions:

  • The developed method provides a robust framework for analyzing ion-specific interactions in mixed electrolyte solutions.
  • This advancement overcomes limitations of previous KBI applications in complex ionic systems.
  • The findings facilitate a more profound understanding of solution behavior in multicomponent electrolytes.