Diffusion constants of polymers in mixed solvents

Dynamics of polymers in mixed solvents are investigated on the basis of linear response theory and mean field arguments. Particular attention is given to the coupling between polymer and fluid fluctuations. This coupling is enhanced by polymer–solvent interaction asymmetry and mixed solvent incompatibility. Cooperative and fluid diffusion constants are analyzed in terms of the interactions in the medium and some predictions for light scattering experiments are made. © 2004 Wiley Periodicals, Inc. J Polym Sci Part B: Polym Phys 42: 3976–3980, 2004     

Dissociation constants of some organic acids

Dissociation constants of di(nonylphenyl)dithiophosphoric acid, di(nonylphenyl)phosphoric acid and 9-phenyltetracosansulphuric acid, determined by two methods, are reported.     

Dissociation constants of carboxymethyloxysuccinic acid

The dissociation constants of carboxymethyloxysuccinic acid (CMOS) have been measured at 25° and an ionic strength of 0·1M in sodium perchlorate. The values found were: pK₁ = 2·52, pK₂ = 3·77 and pK₃ = 5·00. CMOS is thus seen to be rather stronger than its isomer citric acid.     

Analytical data Spectrophotometric determination of the acidity constants of 2-amino cyclopentene-1-dithiocarboxylic acid and some of its derivatives

The acidity constants of 2-amino cyclopentene-1-dithiocarboxylic acid (ACDA) and some of its derivatives have been determined spectrophotometrically, at 25 degrees and at different mole fractions of ethanol in water. In all solvent mixtures used, the acidity constants vary in the order ACDA > N-methyl-ACDA > N-ethyl-ACDA > N-butyl-ACDA.     

Dissociation constants of organophosphinic acid compounds

The dissociation equilibria of di(2,4,4-trimethylpentyi) phosphinic acid, mono(2,4,4-trimethylpentyl) phosphinic acid, di(n-octyl)phosphinic acid and mono(n-octyl)phosphinic acid have been studied in ethanol-water mixtures by potentiometric titration at 25 degrees C. These data have been analysed both graphically numerically using the program LETAGROP-ZETA. The obtained pK(a) values have been correlated with the corresponding values in water, determined both indirectly by means of extraction measurements and by estimation using the suitable Hammett equation.     

Medium effects on the ionization constants of some pyridinecarboxylic acid derivatives

Summary The dissociation constants of 3-hydroxy-2-carboxypyridine (3H2CP), 2-hydroxy-3-carboxypyridine (2H3CP), and 2-mercapto-3-carboxypyridine (2M3CP) were determined by potentiometric titration in 20 mole% ethanol/water, dimethylsulfoxide/water, N,N-dimethylformamide/water, and dioxane/water mixtures at 25±0.1°C applying an empiricalpH correction for mixed aqueous solvents. ThepK _n values obtained are discussed with respect to the nature of the solvent and the ionic strength of the medium as well as the molecular structure. Linearization of the titrimetric data for the second equivalence point of3H2CP,2H3CP, and2M3CP was carried out using theGran method.

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Einfluß des Mediums auf die Ionisationskonstanten einiger Pyridincarbonsäurederivate

Zusammenfassung Die Dissoziationskonstanten von 3-Hydroxy-2-carboxypyridine (3H2CP), 2-Hydroxy-3-carboxypyridin (2H3CP) und 2-Mercapto-3-carboxypyridin (2M3CP) wurden mittels potentiometrischer Titration in 20 mol% Ethanol/Wasser, Dimethylsulfoxid/Wasser, N,N-Dimethylformamid/Wasser und Dioxan/Wasser bei 25±0.1°C unter Verwendung einer empirischenpH-Korrektur für wässrige Lösungsmittelgemische bestimmt. Die erhaltenenpK _n-Werte werden im Zusammenhang mit Lösungsmitteleigenschaften, Ionenstärken und Molekülstruktur diskutiert. Die titrimetrischen Daten für die zweiten Äquivalenzpunkte von3H2CP,2H3CP und2M3CP wurden mit Hilfe derGranschen Methode linearisiert.

     

Acid-base dissociation constants of 2,2'-bipyridyl in mixed protic solvents

The acid dissociation constants (K_a), base dissociation constants (K_b) and the autoprotolysis constants (K_s) for 2,2′-bipyridyl in water and in water+alcohol(methanol, ethanol, iso-propanol) mixed solvents have been determined at 25°C and an ionic strength of 0.1 mol l⁻¹, from a direct potentiometric method based on the treatment of the data of a single pH titration. It has been shown that K_a increases, whereas K_b and K_s decrease, with increasing proportion of the alcohol in the mixed solvents. Linear relations between pK_a, pK_b, pK_s and the mole fraction of the alcohol were observed in the composition range investigated. These results are discussed in terms of the properties of solvent and the interactions of the different species existing in dissociation equilibrium with solvents. It is concluded that the higher stabilization of both 2,2′-bipyridyl and its protonated form by dispersion forces and of the proton by its interaction with solvent molecules in the mixed solvents compared with that in water are largely responsible for the observed changes of pK_a with composition. On the other hand, the low stabilization of OH⁻ in the mixed solvents relative to that in water and the electrostatic effect are the main factors in determining the solvent effect on pK_b.     

Dissociation and complexation constants of some β-diketone ionophores

The dissociation constants of dibenzoylmethane (DBM), 1-phenyl-3-(p-chlorophenyl)-1,3-propanedion (ETH 245) and 1,13-bis-[4-(3-phenyl-1,3-dioxopropyl)-phenyl]-tridecan (ETH 1224) were potentiometrically evaluated in 80% dioxane medium at 30 °C. The stability constants of DBM complexes with calcium, magnesium and barium as well as those of ETH 245 with magnesium were determined and correlated with the selectivity coefficients of ion-selective electrodes containing DBM as ionophore.     

Dissociation constants of some o,o'-substituted azo dyes

The dissociation constants, pK(a) (H(2)L(-)) and pK(a)(HL(2-)), were determined spectrophotometrically in aqueous media at ionic strength 0.2 for six o,o'-substituted azo dyes, namely C.I. 13900, C.I. 15685, C.I. 18744, C.I. 18760, C.I. 18821 and Calmagite.     

One-pot synthesis of β-amino acid derivatives from α-amino acids

The one-pot transformation of α-amino acid into β-amino acid derivatives is described. The application of this method to the synthesis of modified dipeptides was also illustrated.     

Synthesis of 5-substituted derivatives of isophthalic acid as non-polymeric amphiphilic coating for metal oxide nanoparticles

In the course of development of novel capping ligands with variable steric factor, which will be used as an organic coating for metal oxide nanoparticles, a base-catalyzed nucleophilic oxirane ring-opening addition reaction between dimethyl 5-hydroxyisophthalate and allyl glycidyl ether was studied. The allyl-terminated 1-1, 1-2, and 1-3 adducts and dihydroxylated derivative of the 1-1 adduct, 5-diglyceroxy isophthalic acid, were synthesized. The latter binds to the surface of 5 nm γ-Fe₂O₃ nanoparticles in reaction with their surfactant-free diethylene glycol colloids.     

Hydrogen-bonded supramolecular complexes formed between isophthalic acid and pyridine-based derivatives

Two types of supramolecular liquid crystals were prepared through the formation of double hydrogen-bonded complexes between isophthalic acid (A) and two different groups of pyridine-based derivatives ( I n and I _a-e ). The first group of the base, I n (molecular formula 4-C_nH_2n+1OC₆H₄COOC₆H₄-N=N-C₅H₄N) homologues differ from each other by the number of carbon atoms (n) in the alkoxy chain, which varies between 8, 10, 12 and 14 carbons. The second group of the pyridine-based derivatives, I _a-e (molecular formula 4-X-C₆H₄COOC₆H₄-N=N-C₅H₄N) analogues differ from each other by the terminal polar substituent, X, that changes between OCH₃, CH₃, H, NO₂ and Br groups. In this manner two different groups of complexes are formed, one of them is A : 2I n, (Group A ), and the other is A : 2I _a-e , (Group B ). All complexes were investigated for their mesophase behaviour by differential scanning calorimetry and polarised light microscopy. The formation of 1:2 hydrogen-bonded complexes was confirmed by FTIR spectroscopy and binary phase diagrams. Most complexes A and B show nematic and/or SmA phases. X-ray diffraction of the SmA phase of a representative complex of type A indicates a layer distance corresponding to only half of the length of the H-bonded complexes which is interpreted by a phase structure where these complexes adopt a U-shape which intercalate and form non-polar SmA phases.     

Maleic acid solvation in mixed water-ethanol solvents

Heat effects of maleic acid dissolution in mixed water-ethanol solvents at 298.15 K are determined by means of calorimetry. A rise in exothermicity of maleic acid solvation is observed upon changes in the solvent copmosition in the direction of H₂O → EtOH, the minimum being at ∼0.2 mol fraction of EtOH.     

Multi-wavelength spectrophotometric determination of the protolytic constants of tetracycline hydrochloride in some nonaqueous-water mixed solvents: a solvatochromism study

Annihilation of the contribution of one chemical component from the original data matrix is a general method in rank annihilation factor analysis (RAFA). However, RAFA is not applicable for studying the protonation equilibria of multiprotic acids but in this study two-rank annihilation factor analysis (TRAFA) was used as an efficient chemometrics algorithm for determination of the protolytic constants (pKa) of tetracycline hydrochloride (TCHC) in some nonaqueous-water mixed solvents such as acetonitrile (AN)-water and methanol (MeOH)-water from the spectral pH-absorbance data. The spectral data was obtained from spectrophotometric acid-base titrations of different solutions of TCHC at (25.0±0.10)°C and an ionic strength of 0.10 M. In TRAFA algorithm the pKa values were obtained with relationship between residual standard deviation (R.S.D.) and hypothetical pKa values. In the case of TCHC, the spectra were divided in two consecutive subdivisions according to their pH range having two pKa and TRAFA was run twice. The validity of the obtained pKa values was checked with well-known chemometrics algorithms such as DATAN, EQUSPEC, SPECFIT/32 and SQUAD. The effects of changing solvent composition on the protolytic constants were explained by linear solvation energy relationships (LSER) utilizing solvatochromic parameters.     

Thermodynamics of sodium 5-methylisophthalic acid monohydrate and sodium isophthalic acid hemihydrate

Two crystal samples, sodium 5-methylisophthalic acid monohydrate (C₉H₆O₄Na₂·H₂O, s) and sodium isophthalic acid hemihydrate (C₈H₄O₄Na₂·1/2H₂O, s), were prepared from water solution. Low-temperature heat capacities of the solid samples for sodium 5-methylisophthalic acid monohydrate (C₉H₆O₄Na₂·H₂O, s) and sodium isophthalic acid hemihydrate (C₈H₄O₄Na₂·1/2H₂O, s) were measured by a precision automated adiabatic calorimeter over the temperature range from 78 to 379 K. The experimental values of the molar heat capacities in the measured temperature region were fitted to a polynomial equation on molar heat capacities (C _p,m) with the reduced temperatures (X), [X = f(T)], by a least-squares method. Thermodynamic functions of the compounds (C₉H₆O₄Na₂·H₂O, s) and (C₈H₄O₄Na₂·1/2H₂O, s) were calculated based on the fitted polynomial equation. The constant-volume energies of combustion of the compounds at T = 298.15 K were measured by a precise rotating-bomb combustion calorimeter to be Δ_c U(C₉H₆O₄Na₂·H₂O, s) = −15428.49 ± 4.86 J g⁻¹ and Δ_c U(C₈H₄O₄Na₂·1/2H₂O, s) = −13484.25 ± 5.56 J g⁻¹. The standard molar enthalpies of formation of the compounds were calculated to be Δ _f H _m ^θ (C₉H₆O₄Na₂·H₂O, s) = −1458.740 ± 1.668 kJ mol⁻¹ and Δ _f H _m ^θ (C₈H₄O₄Na₂·1/2H₂O, s) = −2078.392 ± 1.605 kJ mol⁻¹ in accordance with Hess’ law. The standard molar enthalpies of solution of the compounds, Δ _sol H _m ^θ (C₉H₆O₄Na₂·H₂O, s) and Δ _sol H _m ^θ (C₈H₄O₄Na₂·1/2H₂O, s), have been determined as being −11.917 ± 0.055 and −29.078 ± 0.069 kJ mol⁻¹ by an RD496-2000 type microcalorimeter. In addition, the standard molar enthalpies of hydrated anion of the compounds were determined as being Δ _f H _m ^θ (C₉H₆O₄ ²⁻, aq) = −704.227 ± 1.674 kJ mol⁻¹ and Δ _f H _m ^θ (C₈H₄O₄Na₂ ²⁻, aq) = −1483.955 ± 1.612 kJ mol⁻¹, from the standard molar enthalpies of solution and other auxiliary thermodynamic data through a thermochemical cycle.