Electrostriction, ion solvation, and solvent release on ion pairing

The theoretical mean molar electrostriction volume of electrolytic solvents, DeltaVel(solvent), was calculated from their properties: the relative pressure derivatives of the density (the compressibility) and permittivity and their second pressure derivatives. The molar electrostriction caused by ions at infinite dilution was taken as the differences of their standard partial molar volumes in the solution and their intrinsic volumes: DeltaVel(ion) = Vinfinity(ion) - Vin(ion). The ratio ninfinity = DeltaVel(ion)/DeltaVel(solvent) then represents the solvation number of the ion in the solvent at infinite dilution. Similarly, from the molar volume change on ion pair formation, DeltaVip, the ratio Deltanip = DeltaVip/DeltaVel(solvent) represents the number of solvent molecules released thereby. These values were tabulated for those solvents, ions, and ion pairs for which the relevant information could be found, the extension to nonaqueous solvents not having been attempted previously.     

Generalizations of the Fuoss approximation for ion pairing

An elementary statistical observation identifies generalizations of the Fuoss approximation for the probability distribution function that describes ion clustering in electrolyte solutions. The simplest generalization, equivalent to a Poisson distribution model for inner-shell occupancy, exploits measurable interionic correlation functions, and is correct at the closest pair distances whether primitive electrolyte solutions models or molecularly detailed models are considered, and for low electrolyte concentrations in all cases. With detailed models, these generalizations include nonionic interactions and solvation effects. These generalizations are relevant for computational analysis of bimolecular reactive processes in solution. Comparisons with direct numerical simulation results show that the simplest generalization is accurate for a slightly supersaturated solution of tetraethylammonium tetrafluoroborate in propylene carbonate ([tea][BF(4)]/PC), and also for a primitive model associated with the [tea][BF(4)]/PC results. For [tea][BF(4)]/PC, the atomically detailed results identify solvent-separated nearest-neighbor ion-pairs. This generalization is examined also for the ionic liquid 1-butyl-3-methylimidazolium tetrafluoroborate ([bmim][BF(4)]) where the simplest implementation is less accurate. In this more challenging situation an augmented maximum entropy procedure is satisfactory, and explains the more varied near-neighbor distributions observed in that case.     

Cooperative metal-coordination and ion pairing in tripeptide recognition

[structure: see text] The recognition of tripeptides by a metal-centered receptor consisting of a rigid backbone region and variable tripeptide arms is described. The studies showed that the receptor was selective for l-Xxx-l-Lys-l-Lys, with Xxx = His, Cys, and Met, giving association constants near 1.0 x 10(6) M(-)(1). Binding enhancement through cooperative interactions of the peptidic arms is demonstrated.     

Specific ion binding to macromolecules: effects of hydrophobicity and ion pairing

Using molecular dynamics simulations in an explicit aqueous solvent, we examine the binding of fluoride versus iodide to a spherical macromolecule with both hydrophobic and positively charged patches. Rationalizing our observations, we divide the ion association interaction into two mechanisms: (1) poorly solvated iodide ions are attracted to hydrophobic surface patches, while (2) the strongly solvated fluoride and to a minor extent also iodide bind via cation-anion interactions. Quantitatively, the binding affinities vary significantly with the accessibility of the charged groups as well as the surface potential; therefore, we expect the ion-macromolecule association to be modulated by the local surface characteristics of the (bio-)macromolecule. The observed cation-anion pairing preference is in excellent agreement with experimental data.     

Recent advances in cooperative ion pairing in asymmetric organocatalysis

Over the last decade, with the surge in the development of organocatalysis, many processes involving chiral ion pairs have emerged as powerful tools in the design of new efficient organocatalysts. This tutorial review focuses on the recent evolutions of these organocatalytic systems in which both anionic and cationic parts are working in a cooperative fashion in order to develop unique catalytic processes which outperform the existing approaches. In this respect, chiral ion pairs opened new avenues in the design of bifunctional organocatalysts by means of combinatorial approaches.     

Aqueous divalent metal-nitrate interactions: hydration versus ion pairing

Nitrate aqueous solutions, Mg(NO(3))(2), Ca(NO(3))(2), Sr(NO(3))(2), and Pb(NO(3))(2), are investigated using Raman spectroscopy and free energy profiles from molecular dynamics (MD) simulations. Analysis of the in-plane deformation, symmetric stretch, and asymmetric stretch vibrational modes of the nitrate ions reveal perturbation caused by the metal cations and hydrating water molecules. Results show that Pb(2+) has a strong tendency to form contact ion pairs with nitrate relative to Sr(2+), Ca(2+), and Mg(2+), and contact ion pair formation decreases with decreasing cation size and increasing cation charge density: Pb(2+) > Sr(2+) > Ca(2+) > Mg(2+). In the case of Mg(2+), the Mg(2+)-OH(2) intermolecular modes indicate strong hydration by water molecules and no contact ion pairing with nitrate. Free energy profiles provide evidence for the experimentally observed trend and clarification between solvent-separated, solvent-shared, and contact ion pairs, particularly for Mg(2+) relative to other cations.     

Chirality transfer in mandelate ionic liquids through ion pairing effects

Ion pairing in [N-(3′-oxohexyl)-N-methylimidazolium][(R)-mandelate] was probed as a function of its concentration in ethanol and compared to the corresponding [(S)-camphorsulfonate] ionic liquid. The applied methodologies comprised asymmetric hydrogenation with ee monitoring as well as independent diffusion-ordered NMR and conductivity measurements.     

Molar volumes and ion pairing of lithium halides in alcohols

The concentration dependence of the apparent molar volumes of lithium halides (and electrolytes in general) in alcohols (and solvents permitting association in general) is, in the first instance, due to changes in the degree of association and to the inherent difference between the apparent molar volumes of the ions and of the ion pairs. Previous publications on the molar volumes of electrolytes in organic solvents, disregarding altogether ion pairing, appear to be incorrect. Data from the literature for lithium chloride and lithium bromide in normal primary alcohols and several branched alcohols from C₁ to C₈ and data from our laboratory for lithium halides in 1-hexanol and 2-ethyl-1-hexanol served for the determination of φ _V and φ _E . Electrical and structural contributions to the values of these functions for the ions and for the ion pairs are discussed.     

Impact of anion polarizability on ion pairing in microhydrated salt clusters

Despite longstanding interest in the mechanism of salt dissolution in aqueous media, a molecular level understanding remains incomplete. Here, cryogenic ion trap vibrational action spectroscopy is combined with electronic structure calculations to track salt hydration in a gas phase model system one water molecule at a time. The infrared photodissociation spectra of microhydrated lithium dihalide anions [LiXX′(H₂O)_n]⁻ (XX′ = I₂, ClI and Cl₂; n = 1–3) in the OH stretching region (3800–2800 cm⁻¹) provide a detailed picture of how anion polarizability influences the competition among ion–ion, ion–water and water–water interactions. While exclusively contact ion pairs are observed for n = 1, the formation of solvent-shared ion pairs, identified by markedly red-shifted OH stretching bands (<3200 cm⁻¹), originating from the bridging water molecules, is favored already for n = 2. For n = 3, Li⁺ reaches its maximum coordination number of four only in [LiI₂(H₂O)₃]⁻, in accordance with the hard and soft Lewis acid and base principle. Water–water hydrogen bond formation leads to a different solvent-shared ion pair motif in [LiI₂(H₂O)₃]⁻ and network formation even restabilizes the contact ion pair motif in [LiCl₂(H₂O)₃]⁻. Structural assignments are exclusively possible after the consideration of anharmonic effects. Molecular dynamics simulations confirm that the significance of large amplitude motion (of the water molecules) increases with increasing anion polarizability and that needs to be considered already at cryogenic temperatures.

Infrared spectroscopy of microhydrated salt clusters provides a detailed picture of how anion polarizability influences the interactions between ions and water.     

Membrane potential across low-water-content charged membranes: Effect of ion pairing

In the present paper, we systematically examined the ion-pairing effect in low-water-content charged membranes. Cation- and anion-exchange membranes with various water contents and homogeneous fixed-charge distribution were prepared by radical copolymerization and then characterized by membrane potential measurements. The experimental results were analyzed by our recently developed theoretical model (Yamamoto, R.; Matsumoto, H.; Tanioka, A. J. Phys. Chem. B 2003, 107, 10615), which is based on the Donnan equilibrium, the Nernst-Planck equation for ion flux, and the Fuoss formalism for ion-pair formation between the fixed-charge group and the counterion in the membrane. The theoretical predictions agreed well with the experimental results for both cation- and anion-exchange membranes. This supported the belief that the ion-pairing effect was substantial in a low-water-content membrane system. Our theoretical analysis also showed the following results: (i) the dielectric constant in the membrane, epsilon(r), was smaller than the value in bulk water, (ii) the center-to-center distance of the ion pair, a, was independent of the water content of the membranes, and (iii) the charge effectiveness of all membranes, Q, was small (<0.35).     

The role of ion pairing in the chromatographic study of propranolol analogues

Summary The partition coefficients, logP _app ^RPLC, for a series of propranolol analogues have been determined by reversed phase high performance liquid chromatography. The hydrochloride salts and free base logP _app ^RPLC show that charged and uncharged species can partition into the reversed phase. An extrathermodynamic relationship was found for logP _app ^RPLC measured in two different column stationary phases, C8 and PMOS, suggesting that the same set of compounds experience a similar trend in these elution systems. The importance of using phosphate and/or MOPS buffer is due to the fact that the latter can avoid ion-pairing partitioning, but the former does play the same role for PMOS column when the free base is considered.     

Conductivity and ion pairing of hydrogen chloride inN-methylpropionamide at 25°C

The electrical conductivity of solutions of HCl inN-methylpropionamide (NMP) has been measured at 25°C for concentrations of HCl ranging from 0.0012 to 0.07 mole-liter^–1. The results, combined with other data recently reported, were analyzed by means of the conductivity equation of Pitts. Some evidence for association was found in spite of the very large relative permittivity of the solvent medium (=176 at 25°C). The limiting molar conductivity for HCl is 10.949 S-cm²-mole^–1. The limiting ionic conductivities in NMP are estimated to be 5.548 S-cm²-mole^–1 for chloride ion and 5.401 S-cm²-mole^–1 for hydrogen ion.     

Accelerated exchange in polyelectrolyte multilayers by "catalytic" polyvalent ion pairing

Self-exchange of isotopically labeled polycarboxylic acid within a polyelectrolyte multilayer proceeds to completion and is reversible. Similar exchange with poly(styrene sulfonate), which forms nonlabile polyelectrolyte complexes, is slow and irreversible but is facilitated by polyvalent ion pairing interventions of a third polyelectrolyte. This is an example of accelerated kinetics in "sticky" synthetic systems associated by nonspecific polyvalent interactions.     

Use of ion pairing reagents for sensitive detection and separation of phospholipids in the positive ion mode LC-ESI-MS

Phospholipids make up one of the more important classes of biological molecules. Because of their amphipathic nature and their charge state (e.g., negatively charged or zwitterionic) detection of trace levels of these compounds can be problematic. Electrospray ionization mass spectrometry (ESI-MS) is used in this study to detect very small amounts of these analytes by using the positive ion mode and pairing them with fifteen different cationic ion pairing reagents. The phospholipids used in this analysis were phosphatidylethanolamine (PE), phosphatidylcholine (PC), phosphatidylglycerol (PG), phosphatidylserine (PS), phosphatidylinositol (PI), phosphatidic acid (PA), 1,2-diheptanoyl-sn-glycero-3-phosphocholine (DHPC), cardiolipin (CA) and sphingosyl phosphoethanolamine (SPE). The analysis of these molecules was carried out in the single ion monitoring (SIM) positive mode. In addition to their detection, a high performance liquid chromatography and mass spectrometry (HPLC-MS) method was developed in which the phospholipids were separated and detected simultaneously within a very short period of time. Separation of phospholipids was developed in the reverse phase mode and in the hydrophilic interaction liquid chromatography (HILIC) mode HPLC. Their differences and impact on the sensitivity of the analytes are compared and discussed further in the paper. With this technique, limits of detection (LODs) were very easily recorded at low ppt (ng L(-1)) levels with many of the cationic ion pairing reagents used in this study.     

Separation of citric acid cycle intermediates by high-performance liquid chromatography with ion pairing

A method to separate underivatized tricarboxylic acid cycle intermediates within 20 min using the commonly available C15 high-performance liquid chromatography column has been developed. Ion pairing using tetrabutylammonium cations and isocratic conditions is used to separate the intermediates which are then detected at 210 nm. Separation was optimized by altering pH, the concentration of sodium sulfate and the pairing ion. This technique permits the detection of as little as 120 nmol of citrate to 0.5 nmol of fumarate. Physiological samples of rat liver mitochondria, human urine, and orange juice were analyzed.     

Divalent pairing ion for ion-interaction chromatography of sulphonates and car☐ylates

An ion-interaction method for the simultaneous separation and UV detection of compounds with weak or strong ionic groups, using a divalent cationic ion pair reagent, namely hexamethonium bromide, has been studied and developed. The analytes considered were tartaric, fumaric, pyruvic, maleic, phthalic, benzoic, sorbic, 4-hydroxybenzoic, benzene and toluene-4-sulphonic acids, and they were chosen for their practical importance. The chromatographic optimization for their separation has been achieved by varying eluent composition (methanol, NaCl and hexamethonium concentrations) and studying the performance of different stationary phases (octyl- and octadecyl-silica based columns). The method developed has been successfully applied to benzoate and sorbate determination in orange juices.     

Complexation equilibria involving salts in non-aqueous solvents: ion pairing and activity considerations

Complexation of anions, cations and even ion pairs is now an active area of investigation in supramolecular chemistry; unfortunately it is an area fraught with complications when these processes are examined in low polarity organic media. Using a pseudorotaxane complex as an example, apparent K_a2 values (=[complex]/{[salt]_o?[complex]}{[host]_o?[complex]}) for pseudorotaxane formation from dibenzylammonium salts ( 2 ‐X) and dibenzo‐[24]crown‐8 ( 1 , DB24C8) in CDCl₃/CD₃CN 3:2 vary with concentration. This is attributable to the fact that the salt is ion paired, but the complex is not. We report an equilibrium model that explicitly includes ion pair dissociation and is based upon activities rather than molar concentrations for study of such processes in non‐aqueous media. Proper analysis requires both a dissociation constant, K_ipd, for the salt and a binding constant for interaction of the free cation 2 ⁺ with the host, K_a5; K_a5 for pseudorotaxane complexation is independent of the counterion (500 M ^?1), a result of the complex existing in solution as a free cation, but K_ipd values for the salts vary by nearly two orders of magnitude from trifluoroacetate to tosylate to tetrafluoroborate to hexafluorophosphate anions. The activity coefficients depend on the nature of the predominant ions present, whether the pseudorotaxane or the ions from the salt, and also strongly on the molar concentrations; activity coefficients as low as 0.2 are observed, emphasizing the magnitude of their effect. Based on this type of analysis, a method for precise determination of relative binding constants, K_a5, for multiple hosts with a given guest is described. However, while the incorporation of activity coefficients is clearly necessary, it removes the ability to predict from the equilibrium constants the effects of concentration on the extent of binding, which can only be determined experimentally. This has serious implications for study of all such complexation processes in low polarity media.     

Remarks on the correlation function implied by the Bjerrum theory of ion pairing

The Friedman theory of correlation functions implied by the Bjerrum theory is generalized by taking into account additional terms and by improving the basic expression for the free energy. By combining the mean spherical approximation (MSA) and the mass action law (MAL) good agreement with HNC and MC data is reached.     

Cooperative effect in ion pairing of oligolysine with heptafluorobutyric acid in reversed-phase chromatography

The retention behavior of an oligolysine mixture, consisting of two to eight residues, was examined at different concentrations of heptafluorobutyric acid (HFBA) in the mobile phase using a C18 column. A single ion record (SIR) mode of the mass spectrometer produced a distinct retention time for each oligomer component. As the concentration of HFBA increased, the retention time of each oligomer increased. Furthermore, the increase in retention time is chain-length dependent such that, the longer the oligomer chain, the more rapid was the rate that retention time increased. A closed pairing model that presumes an equilibrium between the unpaired state and the paired state with a fixed number of HFBA molecules was used to analyze the retention factor as a function of [HFBA]. Curve fitting gave estimates of the ion-pairing equilibrium constant (K(ip,m)), the distribution constant of paired oligolysine (K(D,ip)), and the number of paired HFBA for each oligolysine (n). The plot of the fraction of paired oligolysine in the mobile phase, estimated from K(ip,m) and n as a function of [HFBA], revealed a cooperative effect. In contrast, an open pairing model that assumes independent pairing of HFBA with each residue failed to describe the observed retention behavior.