TY - JOUR
T1 - Solubility of Sodium Halides in Aqueous Mixtures with ε-Increasing Cosolvents
T2 - Formamide, N-Methylformamide, and N-Methylacetamide at 298.15 K
AU - Hernández-Luis, Felipe
AU - Rodríguez-Raposo, Raquel
AU - Galleguillos, Héctor R.
AU - Morales, Jaime W.
N1 - Publisher Copyright:
© 2016 American Chemical Society.
PY - 2016/1/27
Y1 - 2016/1/27
N2 - The solubility data for sodium halides (NaF, NaCl, NaBr, and NaI) have been determined at 298.15 K in the ε-increasing mixtures of water-formamide, water-N-methylformamide, and water-N-methylacetamide. In all cases, the solubility of the electrolytes was decreased significantly in the presence of a cosolvent. The solubility of an electrolyte in a given solvent depends on both the nature of the solvent (mainly the polarity, dielectric constant, solvation, or preferential solvation if the solvent is a mixture of solvents, etc.) and the properties of the electrolyte (principally the size, the charge, and the possible association of its ions). If the molality of saturation is not sufficiently small, the ion-ion and ion-solvent interactions must be considered. Although it was not the objective of this work, the solubility values were qualitatively correlated with several properties of the solvent and solute. Finally, a simple justification, which was both qualitative and quantitative, was carried out.
AB - The solubility data for sodium halides (NaF, NaCl, NaBr, and NaI) have been determined at 298.15 K in the ε-increasing mixtures of water-formamide, water-N-methylformamide, and water-N-methylacetamide. In all cases, the solubility of the electrolytes was decreased significantly in the presence of a cosolvent. The solubility of an electrolyte in a given solvent depends on both the nature of the solvent (mainly the polarity, dielectric constant, solvation, or preferential solvation if the solvent is a mixture of solvents, etc.) and the properties of the electrolyte (principally the size, the charge, and the possible association of its ions). If the molality of saturation is not sufficiently small, the ion-ion and ion-solvent interactions must be considered. Although it was not the objective of this work, the solubility values were qualitatively correlated with several properties of the solvent and solute. Finally, a simple justification, which was both qualitative and quantitative, was carried out.
UR - http://www.scopus.com/inward/record.url?scp=84956905765&partnerID=8YFLogxK
U2 - 10.1021/acs.iecr.5b04614
DO - 10.1021/acs.iecr.5b04614
M3 - Article
AN - SCOPUS:84956905765
SN - 0888-5885
VL - 55
SP - 812
EP - 819
JO - Industrial and Engineering Chemistry Research
JF - Industrial and Engineering Chemistry Research
IS - 3
ER -