Determination of the Molality Scale Dissociation Constants of Acetic Acid in Aqueous Sodium Chloride Solutions at 298.15 K.

Partanen, Jaakko I.; Karki, Merja H.; Juusola, Pekka M.; Norrby, Per-Ola

doi:10.3891/acta.chem.scand.49-0865

Cited by 15 publications

(10 citation statements)

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“…g Determined by Partanen (1998) from Harned-cell data. h Determined by Partanen et al (1995c) from Harned-cell data. i Recommended in this study.…”

Section: Resultsmentioning

confidence: 99%

“…b Determined by Prue and Read (1966) from the emf data. c Determined from the conductivity data measured by MacInnes and Shedlovsky (1932); see Partanen et al (1995c). d pKa ) -log Ka.…”

Section: Resultsmentioning

confidence: 99%

“…For both data sets, E°H -C was estimated by requiring that the sum of all errors in the set is zero, and the resulting values are shown in the figure. The departure of E°H -C for the NaCl set (for this set E°H -C is 0.221 98 V) from the value suggested by Harned and Ehlers (i.e., from 0.222 50 V) can result from the medium effect due to the appreciable amount of undissociated formic acid present in the solutions of this data set; see Partanen et al (1995c) and Partanen (1998). Otherwise, the emf data of Harned and Owen support well the calculation method up to large ionic strengths.…”

Section: E ) E°+ (Rt/f) Ln γ H + (Rt/f) Ln (M H /M°) )mentioning

confidence: 94%

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Determination of Stoichiometric Dissociation Constants of Formic Acid in Aqueous Sodium or Potassium Chloride Solutions at 298.15 K

Partanen

Juusola

1999

J. Chem. Eng. Data

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Equations were determined for the calculation of the stoichiometric (molality scale) dissociation constant K m of formic acid in dilute aqueous NaCl and KCl solutions at 298.15 K from the thermodynamic dissociation constant K a of this acid and from the ionic strength I m of the solution. The salt alone determines mostly the ionic strength of the solutions considered in this study, and the equations for K m were based on the single-ion activity coefficient equations of the Hü ckel type. The data measured by potentiometric titrations in a glass electrode cell were used in the estimation of the parameters for the Hü ckel equations of formate ions. The Hü ckel parameters obtained in these estimations agree well with those published previously for acetate ions, and therefore, the acetate parameters are also recommended for formate ions. By means of the calculation method based on the Hü ckel equations, K m can be obtained almost within experimental error at least up to I m of about 2 mol kg -1 for formic acid in NaCl and KCl solutions.

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“…g Determined by Partanen (1998) from Harned-cell data. h Determined by Partanen et al (1995c) from Harned-cell data. i Recommended in this study.…”

Section: Resultsmentioning

confidence: 99%

“…b Determined by Prue and Read (1966) from the emf data. c Determined from the conductivity data measured by MacInnes and Shedlovsky (1932); see Partanen et al (1995c). d pKa ) -log Ka.…”

Section: Resultsmentioning

confidence: 99%

Section: E ) E°+ (Rt/f) Ln γ H + (Rt/f) Ln (M H /M°) )mentioning

confidence: 94%

See 1 more Smart Citation

Determination of Stoichiometric Dissociation Constants of Formic Acid in Aqueous Sodium or Potassium Chloride Solutions at 298.15 K

Partanen

Juusola

1999

J. Chem. Eng. Data

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“…B i is a parameter that is dependent on ion i, and b i, MCl is another parameter that is dependent on both ion i and the salt MCl present in the system. In the research work of Partanen [37][38][39][40], the following parameters have been determined for equation (7):…”

Section: Mixing-flow Calorimetrymentioning

confidence: 99%

Simultaneous determination of enthalpies of dilution and dissociation of protocatechuic acid in aqueous salt solutions by calorimetric measurements

Zheng

Liu

Wang

et al. 2015

The Journal of Chemical Thermodynamics

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“…In this manuscript, we continue the studies (1)(2)(3)(4)(5)(6)(7)(8)(9)(10)(11)(12)(13)(14)(15)(16)(17) dealing with the thermodynamics of weak acid solutions. The purpose of these studies is to determine the stoichiometric dissociation constants (for example, the molality scale dissociation constants, K m ) for salt solutions of different weak acids, as reliably as possible from potentiometric titration data measured with glass electrodes.…”

Section: Introductionmentioning

confidence: 99%

Determination of the second stoichiometric dissociation constants of glycine in aqueous sodium or potassium chloride solutions at 298.15 K

Partanen¹,

Juusola²,

Minkkinen³

et al. 2003

Can. J. Chem.

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Equations were determined for the calculation of the second stoichiometric (molality scale) dissociation constant, K m2 , of glycine, in aqueous NaCl and KCl solutions at 298.15 K, from the thermodynamic dissociation constant, K a2 , of this acid and the ionic strength, I m , of the solution. The ionic strength of the solutions considered in this study is determined mostly by the salt alone, and the equations for K m2 were based on the single-ion activity coefficient equations of the Hückel type. New data measured by potentiometric titrations in a glass electrode cell were used in the estimation of the parameters for the Hückel equations of glycine species. By means of the calculation method suggested in this study, K m2 can be obtained almost within experimental error up to an I m of about 1.0 mol kg -1 for glycine in NaCl and KCl solutions. The K m2 values obtained by these methods were also compared with the values suggested in the literature for this quantity.Résumé : Des équations sont développées pour le calcul de K m2 , la deuxième constante de dissociation stoechiomé-trique (en molalité) de la glycine en solution aqueuse de NaCl et KCl à 298,15 K. Ces équations sont déterminées à partir de la constante de dissociation, K a2 , de cet acide et de la force ionique, I m , de la solution. La force ionique des solutions étudiées est imposée en presque totalité par le sel contenu en solution. Les formules pour K m2 sont alors dé-duites d'équations de type Hückel pour la détermination du coefficient d'activité d'un seul type d'ions. Les paramètres des équations d'Hückel pour les sels de glycine ont été approximés sur la base de mesures faites par titrations potentiométriques avec des électrodes de verre. Avec les meilleures méthodes de calculs présentées dans cette étude, K m2 peut être calculé avec une certitude presque équivalente aux erreurs expérimentales pour des solutions de glycine dans NaCl ou KCl ayant une force ionique I m jusqu'à environ 1,0 mol kg -1 . Les valeurs de K m2 obtenues par ces méthodes sont aussi comparées aux valeurs trouvées dans la bibliographie.Mots clés : influence de la force ionique, constante de dissociation stoechiométrique, équation de Debye-Hückel, potentiométrie, glycine.Partanen et al. 1470

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Determination of the Molality Scale Dissociation Constants of Acetic Acid in Aqueous Sodium Chloride Solutions at 298.15 K.

Cited by 15 publications

References 0 publications

Determination of Stoichiometric Dissociation Constants of Formic Acid in Aqueous Sodium or Potassium Chloride Solutions at 298.15 K

Determination of Stoichiometric Dissociation Constants of Formic Acid in Aqueous Sodium or Potassium Chloride Solutions at 298.15 K

Simultaneous determination of enthalpies of dilution and dissociation of protocatechuic acid in aqueous salt solutions by calorimetric measurements

Determination of the second stoichiometric dissociation constants of glycine in aqueous sodium or potassium chloride solutions at 298.15 K

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