Ion-Ion Interactions

  • Peter R. Bergethon


If a potential electrolyte is added to an aqueous solution, its dissociation may be so low that few ions are produced. It is also possible to make a solution from a true electrolyte so dilute that the number of ions in solution is very small. In both of these cases, the analysis completed in the previous chapter would be adequate to describe the interactions that cause the solution to deviate from ideality. These solutions would be so dilute that each and every ion in solution could, in a sense, look out past even its secondary hydration sheath and see only bulk water. These ions would thus seem to exist completely alone and isolated in solution.


Activity Coefficient Point Charge Electrostatic Field Ionic Atmosphere Linearize Boltzmann Equation 
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Further Reading

  1. Bockris J. O’M., and Reddy A. K. N. (1970) Modern Electrochemistry, vol. 1. Plenum, New York.CrossRefGoogle Scholar
  2. Koryta J., and Dvorak J. (1993) Principles of Electro- chemistry, 2d ed. John Wiley and Sons, New York.Google Scholar
  3. Anderson C. F., and Record M. T. Jr. (1995) Salt-nucleic acid interactions. Ann. Rev. Phys. Chem., 46: 657–700.CrossRefGoogle Scholar
  4. Wolynes P. G. (1980) Dynamics of electrolyte solutions. Ann. Rev. Phys. Chem., 31: 345–76.CrossRefGoogle Scholar

Copyright information

© Springer Science+Business Media New York 1998

Authors and Affiliations

  • Peter R. Bergethon
    • 1
  1. 1.Department of BiochemistryBoston University School of MedicineBostonUSA

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