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Electrical Conductivity Studies of Quinic Acid and its Sodium Salt in Aqueous Solutions

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Abstract

The electrical conductivities of aqueous solutions of quinic acid and its sodium salt were measured from 293.15 to 328.15 K in steps of 5 K. The molar conductivities of the sodium salt were treated by the Lee–Wheaton equation, in the form of Pethybridge and Taba, and the Kohlrausch equations. The limiting molar conductivities of the quinate anion were estimated, as well as the corresponding ionic association constants and standard thermodynamic functions of the ionic association reaction. The hydrodynamic radius of the quinate anion was calculated from the Walden rule and compared with the van der Waals radius. The dissociation constant of quinic acid was evaluated from the known value of the limiting molar conductivity of quinic acid using the conductivity equation of Pethybridge and Taba. The standard thermodynamic functions of the dissociation process, i.e., the Gibbs energy, enthalpy, entropy and heat capacity, were obtained using the non-empirical procedure given by Clarke and Glew. The standard thermodynamic functions of dissociation of quinic acid are discussed in terms of solute–solvent interactions and stabilization of the quinate anion due to hydrogen bonding of the α-hydroxyl group to the carboxyl group.

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  1. Biotechnical Faculty, University of Ljubljana, Jamnikarjeva 101, SLO-1000, Ljubljana, Slovenia

    Cveto Klofutar & Nataša Šegatin

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  1. Cveto Klofutar
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  2. Nataša Šegatin
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Correspondence to Nataša Šegatin.

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Klofutar, C., Šegatin, N. Electrical Conductivity Studies of Quinic Acid and its Sodium Salt in Aqueous Solutions. J Solution Chem 36, 879–889 (2007). https://doi.org/10.1007/s10953-007-9154-1

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  • DOI: https://doi.org/10.1007/s10953-007-9154-1

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