Abstract
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.
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Further Reading
Bockris J. O’M., and Reddy A. K. N. (1970) Modern Electrochemistry, vol. 1. Plenum, New York.
Koryta J., and Dvorak J. (1993) Principles of Electro- chemistry, 2d ed. John Wiley and Sons, New York.
Anderson C. F., and Record M. T. Jr. (1995) Salt-nucleic acid interactions. Ann. Rev. Phys. Chem., 46: 657–700.
Wolynes P. G. (1980) Dynamics of electrolyte solutions. Ann. Rev. Phys. Chem., 31: 345–76.
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Bergethon, P.R. (1998). Ion-Ion Interactions. In: The Physical Basis of Biochemistry. Springer, New York, NY. https://doi.org/10.1007/978-1-4757-2963-4_20
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DOI: https://doi.org/10.1007/978-1-4757-2963-4_20
Publisher Name: Springer, New York, NY
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