Ion Association In Solutions Research Articles

Study of the association of tetracycline ions in solution and in a complex with a polyelectrolyte

1. The organic ions of antibiotics (tetracycline, hydroxytetracycline, and chlorotetracycline) in aqueous acidic solution form associates (at concentrations above 10−4 M), the size of which, like surfactants, reaches tens of molecules. The associates, like the surfactant micelles, are probably formed as a consequence of the hydrophobic interaction between molecules. 2. The viscosity of the solutions decreases during the formation of an organic ion-polyelectrolyte complex in the case of associated hydroxytetracycline and cetylpyridinium bromide ions and changes little for unassociated triethylbenzylammonium ions. This is explained by the interaction of ions among themselves (associations) in the polymer-bonded state.

Study of Hydration and Association of Ions in Solution. I. Chromatographic and Electrophoretic Behaviors of Hexamminetype Cobalt(III) Complexes in Aqueous Solutions of Various Electrolytes

Abstract The dissolved state of ions in solution was investigated through the study of separation mechanism of a series of tervalent hexammine-type cobalt(III) complexes in thin-layer chromatography and in electrophoresis. The results obtained are summarized as follows. In the case of strongly hydrated complexes, a strongly hydrated anion has a greater tendency towards association than a weakly hydrated anion. On the contrary, in the weakly hydrated complexes, a weakly hydrated anion is associated more easily than a strongly hydrated anion. From these findings, ionic association was presumed to occur through direct contact of a complex cation and an anion.

Electrostatic and non-electrostatic contributions to ion association in solution

Abstract

The Thermodynamics of Ion Association in Solution. I. An Extension of the Denison-Ramsey Equations

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTThe Thermodynamics of Ion Association in Solution. I. An Extension of the Denison-Ramsey EquationsL. D. Pettit and Stanley BruckensteinCite this: J. Am. Chem. Soc. 1966, 88, 21, 4783–4789Publication Date (Print):November 1, 1966Publication History Published online1 May 2002Published inissue 1 November 1966https://doi.org/10.1021/ja00973a004RIGHTS & PERMISSIONSArticle Views265Altmetric-Citations43LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (767 KB) Get e-Alerts Get e-Alerts

The Thermodynamics of Ion Association in Solution. II. Mixed Ion Association

ADVERTISEMENT RETURN TO ISSUEPREVArticleNEXTThe Thermodynamics of Ion Association in Solution. II. Mixed Ion AssociationStanley Bruckenstein and L. D. PettitCite this: J. Am. Chem. Soc. 1966, 88, 21, 4790–4794Publication Date (Print):November 1, 1966Publication History Published online1 May 2002Published inissue 1 November 1966https://doi.org/10.1021/ja00973a005RIGHTS & PERMISSIONSArticle Views63Altmetric-Citations8LEARN ABOUT THESE METRICSArticle Views are the COUNTER-compliant sum of full text article downloads since November 2008 (both PDF and HTML) across all institutions and individuals. These metrics are regularly updated to reflect usage leading up to the last few days.Citations are the number of other articles citing this article, calculated by Crossref and updated daily. Find more information about Crossref citation counts.The Altmetric Attention Score is a quantitative measure of the attention that a research article has received online. Clicking on the donut icon will load a page at altmetric.com with additional details about the score and the social media presence for the given article. Find more information on the Altmetric Attention Score and how the score is calculated. Share Add toView InAdd Full Text with ReferenceAdd Description ExportRISCitationCitation and abstractCitation and referencesMore Options Share onFacebookTwitterWechatLinked InReddit PDF (576 KB) Get e-Alerts Get e-Alerts

Ultrasonic Investigation of Ion Association in Solution

Understanding ion association is a necessary prerequisite for an understanding of electrolyte solutions. It is important not only to solution chemistry but also to such diverse fields as oceanography, polymer chemistry, and biochemistry. Unfortunately, classical-solution techniques such as conductance have proven inadequate based as they are on a continuum-solvent model. The introduction of relaxation techniques and, in particular, ultrasonic absorption has provided an extremely powerful approach for the resolution of this problem. We describe recent results in this laboratory, obtained by conventional transmitted-pulse ultrasonic measurements in the range 2–300 MHz. A general model for ion association is presented, based on extensive work in aqueous MnSO4, MgSO4, and CoSO4 solutions. The model is extended to recent data on 1-1 salt association in nonaqueous solvents. Finally an analysis is given of the association of some lanthanide sulfates in water. An attempt is made to identify the important parameters that govern the thermodynamics and kinetics of ion association in a molecular solvent.

Ion association in solutions of nickel malonate and n-butyl malonate

Ion association in solutions of nickel malonate and n-butyl malonate

Ion association in solutions of lead bromide and iodide

Ion association in solutions of lead bromide and iodide

The dielectric capacity of electrolytes in mixed solvents: ion association in solutions of magnesium sulphate

The remarkable achievements of Debye and Hückel, Onsager, and their colleagues in explaining and rationalizing the experimental data upon the behaviour of strong electrolytes in dilute solution have naturally led to much intensive research directed towards the extension of their theories to ranges of greater ionic concentration. From this work the theory of ion association, sponsored by Niels Bjerrum, has emerged with marked success. Assuming that the forces between oppositely charged ions obey the simple Coulomb law, Bjerrum has calculated the probability of such ions being within a distance, q 0 , at which the thermal energy per degree of freedom is but one-quarter of the electrostatic energy holding the ions together. Oppositely charged ions at less than this distance from one another are termed short-range pairs. The true degree of association (1— α *) of an electrolyte, as distinguished from the classical conception of undissociated molecules, is a measure of the number of short-range pairs, and Bjerrum has shown that the law of mass action may be applied to this association to develop a relation which reproduces the activities of electrolytes in more concentrated solution with remarkable fidelity. Onsager (1927) has calculated some approximate values of the true degree of association by consideration of the discrepancies between experimental conductivity data for aqueous solutions and the figures derived from his equation. Similar, and more extensive and more accurate measurements have been made by Davies (1927). In solvents of lower dielectric constant, the increased inter-ionic forces lead to still wider discrepancies, and many workers have shown that electrolytes which are almost completely non-associated in water are appreciably associated in solvents of reduced dielectric capacity. Martin (1928) has shown that the alkali metal halides are incompletely dissociated in benzonitrile and that the association obeys a generalized law of mass action. Fuoss and Kraus (1933 a ) have observed the same effects with the alkali metal nitrates dissolved in ammonia and other solvents of low dielectric constant. The mass-action constants derived from their results are in complete agreement with those predicted by the Bjerrum ion-association theory and, using measurements of the conductivity of tetra iso - amylammonium nitrate in dioxan-water mixtures, the same workers (1933 b ) have succeeded in extending the theory to include higher forms of association. Swift (1938) has confirmed the views of Fuoss and Kraus for ions of small radii by an investigation of the conductivities of solutions of the alkali metal halides in dimethylamine.