Activity coefficients of NaClO4 in aqueous solution

Jaime W. Morales; Héctor R. Galleguillos; Felipe Hernández-Luis; Raquel Rodríguez-Raposo

doi:10.1021/je2005006

Activity coefficients of NaClO₄ in aqueous solution

Jaime W. Morales, Héctor R. Galleguillos, Felipe Hernández-Luis, Raquel Rodríguez-Raposo

Resultado de la investigación: Contribución a una revista › Artículo › revisión exhaustiva

18 Citas (Scopus)

Resumen

The activity coefficients of NaClO₄ in water were experimentally determined at (288.15, 298.15, and 308.15) K from electromotive force (emf) measurements of the following electrochemical cell without transference containing two ion-selective electrodes (ISEs): Na-ISE|NaClO₄ (m)|ClO₄-ISE. The molality m varied between about (0.02 and 12) mol·kg^-1. The determination of E⁰, which is necessary to calculate the activity coefficients, was carried out following a method similar to that of Hitchcock, using the Pitzer, extended Debye-Hückel, and Scatchard equations to represent the dependency of log γ on molality. The electrode system employed shows good Nernstian behavior. The activity and osmotic coefficients obtained in this study at 298.15 K were contrasted to those from the literature and show a good agreement.

Idioma original	Inglés
Páginas (desde-hasta)	3449-3453
Número de páginas	5
Publicación	Journal of Chemical and Engineering Data
Volumen	56
N.º	8
DOI	https://doi.org/10.1021/je2005006
Estado	Publicada - 11 ago. 2011
Publicado de forma externa	Sí

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10.1021/je2005006

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title = "Activity coefficients of NaClO4 in aqueous solution",

abstract = "The activity coefficients of NaClO4 in water were experimentally determined at (288.15, 298.15, and 308.15) K from electromotive force (emf) measurements of the following electrochemical cell without transference containing two ion-selective electrodes (ISEs): Na-ISE|NaClO4 (m)|ClO4-ISE. The molality m varied between about (0.02 and 12) mol·kg-1. The determination of E0, which is necessary to calculate the activity coefficients, was carried out following a method similar to that of Hitchcock, using the Pitzer, extended Debye-H{\"u}ckel, and Scatchard equations to represent the dependency of log γ on molality. The electrode system employed shows good Nernstian behavior. The activity and osmotic coefficients obtained in this study at 298.15 K were contrasted to those from the literature and show a good agreement.",

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T1 - Activity coefficients of NaClO4 in aqueous solution

AU - Morales, Jaime W.

AU - Galleguillos, Héctor R.

AU - Hernández-Luis, Felipe

AU - Rodríguez-Raposo, Raquel

PY - 2011/8/11

Y1 - 2011/8/11

N2 - The activity coefficients of NaClO4 in water were experimentally determined at (288.15, 298.15, and 308.15) K from electromotive force (emf) measurements of the following electrochemical cell without transference containing two ion-selective electrodes (ISEs): Na-ISE|NaClO4 (m)|ClO4-ISE. The molality m varied between about (0.02 and 12) mol·kg-1. The determination of E0, which is necessary to calculate the activity coefficients, was carried out following a method similar to that of Hitchcock, using the Pitzer, extended Debye-Hückel, and Scatchard equations to represent the dependency of log γ on molality. The electrode system employed shows good Nernstian behavior. The activity and osmotic coefficients obtained in this study at 298.15 K were contrasted to those from the literature and show a good agreement.

AB - The activity coefficients of NaClO4 in water were experimentally determined at (288.15, 298.15, and 308.15) K from electromotive force (emf) measurements of the following electrochemical cell without transference containing two ion-selective electrodes (ISEs): Na-ISE|NaClO4 (m)|ClO4-ISE. The molality m varied between about (0.02 and 12) mol·kg-1. The determination of E0, which is necessary to calculate the activity coefficients, was carried out following a method similar to that of Hitchcock, using the Pitzer, extended Debye-Hückel, and Scatchard equations to represent the dependency of log γ on molality. The electrode system employed shows good Nernstian behavior. The activity and osmotic coefficients obtained in this study at 298.15 K were contrasted to those from the literature and show a good agreement.

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