Mechanism of Oxidation of Ketorolac by Hexacyanoferrate(III) in Aqueous Alkali: A Thermodynamics and Kinetics Study

The kinetics of the oxidation of ketorolac by hexacyanoferrate(III) (HCF) in aqueous alkaline medium at a constant ionic strength of 0.75 mol·dm^?3 was studied spectrophotometrically at 300 K. A plausible mechanism was proposed and the rate law was derived. The mechanism of oxidation of ketorolac (KET) in alkaline medium has been shown to proceed via a KET-HCF complex, which decomposes in a slow step followed by other fast steps to give the products. The main oxidative product was identified as (2,3-dihydro-1-hydroxy-1H-pyrrolizin-5-yl-)(phenyl)methanone and is characterized by its LC–ESI–MS spectrum. Thermodynamic parameters of various equilibria of the mechanism were calculated and activation parameters ΔH ^≠, ΔS ^≠, ΔG ^≠ and log₁₀ A were found to be 29.9 kJ·mol^?1, ?220 J·K^?1·mol^?1, 96 kJ·mol^?1 and 2.70 respectively.     

Protonation equilibria studies of the standard α-amino acids in NaNO3 solutions in water and in mixtures of water and dioxane

The protonation equilibria for 20 standard α-amino acids in solutions have been studied pH-potentiometrically. The dissociation constants (pK_a) of 20 amino acids and the thermodynamic functions (ΔG^∘, ΔH^∘, ΔS^∘, and δ) for the successive and overall protonation processes of amino acids have been derived at different temperatures in water and in three different mixtures of water and dioxane (mole fractions of dioxane were 0.083, 0.174, and 0.33). Titrations were also carried out in water ionic strengths of (0.15, 0.20, and 0.25) mol · dm⁻³ NaNO₃, and the resulting dissociation constants are reported. A detailed thermodynamic analysis of the effects of organic solvent (dioxane), temperature and ionic strength influencing the protonation processes of amino acids is presented and discussed to determine the factors which control these processes.     

Heats of formation of iodo-complexes of zinc(II), cadmium(II) and mercury(II) in aqueous solutions

Heats of formation of MeI⁺, MeI₂, MeI₃^? and MeI₄^2? where Me²⁺, Cd²⁺ or Hg²⁺ were determined in acidic solutions by flow microcalorimetry. Some gaps in the literature data were filled. In particular, ΔH₃ for the mercury(II) complex was determined and the ΔH₁, ΔH₂ + ΔH₃, ΔH₄ for zinc(II) complexes were measured in sodium free solutions to avoid ionic couple formation. For cadmium(II) complexes, existing data were confirmed. Thermodynamic functions are discussed in term of hard/soft interactions.     

Zum Ionenaustausch einwertiger Kationen an synthetischen Natriumpolysilicaten mit Schichtstruktur

Ion Exchange of Monovalent Cations in Synthetic Sodium Polysilicates with Layer Structure Cation-exchange equilibria of synthetic sodium polysilicates Ilerit (Na₂O · 8.3SiO₂ 8.9 H₂O) and Magadiite (Na₂O · 13 SiO₂ · 6.8 H₂O) with H⁺, Li⁺ and K⁺ Ions were investigated with respect to their selectivity behaviour. The range of ion selectivity is: H⁺ > Na⁺ > Li⁺ > K⁺. Thermodynamic data ΔG, ΔH, and ΔS were determined by means of the integral thermodynamic equilibria constants K_th of the ion-exchange reactions.     

Thermodynamic characteristics of the formation of complexes of nickel(II) with L-homoserine

The formation of complexes of nickel(II) with L-homoserine at 298.15 K and ionic strengths I = 0.5, 1.0, and 1.5 (KNO₃) are investigated by potentiometry and calorimetry. Standard characteristics of studied equilibria (log K°, Δ_rG°, Δ_rH°, and Δ_rS°) are determined.     

Thermal dissociation of SmMnO3

The phase equilibria for the reduction of SmMnO₃ with hydrogen were studied by the static method using a circulation vacuum setup in conjunction with XRD analysis of quenched solid phases. It was established that, over a temperature range of 973–1123 K and a pressure range of 10^?10–10^?16 Pa, SmMnO₃ dissociates by the reaction (1/2)Sm₂O₃ + MnO + (1/4)O₂; in this case, the temperature dependence of the equilibrium oxygen pressure and the Gibbs energy change can be described by the equations log $p_{O_2 } $ [Pa] = 25.35 ? 39150/T ± 0.1, ΔG°_T, kJ/mol = 187.62 ? 0.09T ± 1.62, respectively. Based on the experimental data, the standard thermodynamic functions of formation of SmMnO₃ from elements were calculated: ΔH°_T = ?1485.706 kJ/mol and ΔS°_T = 244.39 J/(mol K).     

Rotational isomerism of O,O′-dialkyl esters of phosphorodithioic acid

Compounds (RO)₂ P(:S)SH, RPrⁱ, Buⁿ, and Octⁿ, exhibit rotational isomerism about PO and PS bonds. Temperature-dependence studies of band intensities indicate values of ΔH for the equilibria between isomers to be 2.5 kJ mol⁻¹, RPrⁱ; 3.0 kJ mol⁻¹, RBuⁿ; and ∼4.5 kJ mol⁻¹, ROctⁿ.     

Thermodynamic characteristics of protolytic equilibria in aqueous solutions of glycyl peptides

Protolytic equilibria in aqueous solutions of glycyl-DL-serine, glycyl-DL-threonine, and glycyl-DL-valine are investigated by means of potentiometry and calorimetry. Dissociation constants and heat effects of the above dipeptides are determined. Standard thermodynamic characteristics (pK°, Δ_disG°, Δ_disH°, Δ_disS°) of the investigated equilibria are calculated. The obtained results are compared to corresponding data on relative compounds.     

Thermal studies and spectral characterization of the chelate of bis-(η5-cyclopentadienyl titanium(IV) with salicylidene-4-methylaniline

A new chelate (η⁵-C₅H₅)₂Ti(SB)₂, whereSB=O, N donor Schiff base salicylidene-4-methylaniline, was synthesized. The course of thermal degradation of the chelate was studied by thermogravimetric (TG) and differential thermal analysis (DTA) under dynamic conditions of temperature. The order of the thermal decomposition reaction and energy of activation was calculated from TG curve while from DTA curve the change in enthalpy was calculated. Evaluation of the kinetic parameters was performed by Coats-Redfern as well as Piloyan-Novikova methods which gaven=1, ΔH=1.114 kJ·mol^?1, ΔE=27.01 kJ·mol^?1, ΔS=?340.12 kJ·mol^?1·K^?1 andn=1, ΔH=1.114 kJ·mol^?1, ΔE=20.01 kJ·mol^?1, ΔS=?342.60 kJ·mol^?1·K^?1, respectively. The chelate was also characterized on the basis of different spectral studies viz. conductance, molecular weight, IR, UV-visible and¹H NMR, which enabled to propose an octahedral structure to the chelate.     

Influence of temperature on the heats of acid-base reactions in L-glutamine aqueous solution

Protolytic equilibria in L-glutamine aqueous solutions were studied calorimetrically. The measurements were carried out at 298.15, 308.15, and 318.15 K and ionic strengths of 0.5, 1.0, and 1.5 (potassium nitrate). The thermodynamic parameters (pK, ΔG, ΔH, ΔS) of stepwise dissociation of L-glutamine both in water-salt solutions and in the standard solution were obtained.     

Potentiometric study of binary complexes of 3-[(1R)-1-hydroxy-2-(methylamino)ethyl]phenol hydrochloride with some lanthanide ions in aqueous and mixed solutions

The complexation of lanthanide ions (Y³⁺, La³⁺, Ce³⁺, Pr³⁺, Nd³⁺, Sm³⁺, Gd³⁺, Tb³⁺, and Dy³⁺) with 3-[(1R)-1-hydroxy-2-(methylamino)ethyl]phenol hydrochloride was studied at different temperatures and different ionic strengths in aqueous solutions by Irving-Rossotti pH titration technique. Stepwise calculation, PKAS and BEST Fortran IV computer programs were used for determination of proton-ligand and metal-ligand stability constants. The formation of species like MA, MA₂, and MA(OH) is considered in SPEPLOT. Thermodynamic parameters of complex formation (ΔG, ΔH, and ΔS) are also evaluated. Negative ΔG and ΔH values indicate that complex formation is favourable in these experimental conditions. The stability of complexes is also studied at in different solvent-aqueous (vol/vol). The stability series of lanthanide complexes has shown to have the “gadolinium break.” Stability of complexes decreases with increase in ionic strength and temperature. Effect of systematic errors like effect of dissolved carbon dioxide, concentration of alkali, concentration of acid, concentration of ligand and concentration of metal have also been explained.     

The enthalpies of solution of DL-α-alanine in water-organic solvent mixtures at 298.15 K

The integral enthalpies of solution (298.15 K) of DL-α-alanine in water-organic solvent mixtures were measured at organic component concentrations x ₂ = 0–0.4 mole fractions. The organic solvents used were acetonitrile (ACN), formamide (FA), N,N-dimethylformamide (DMFA), and N,N-dimethylsulfoxide (DMSO). The standard enthalpies of solution Δ_sol H ^o, solvation Δ_solv H ^o, and transfer (Δ_tr H ^o) of DL-α-alanine from water to mixed solvents were calculated. The influence of the structure and properties of solutes and mixture composition on solute thermochemical characteristics was considered. The solution of DL-α-alanine in the mixtures studied was endothermic over the whole range of organic component concentrations. The Δ_sol H ^o, Δ_tr H ^o, and Δ_solv H ^o values as functions of x ₂ can pass extrema (DMSO and DMFA), be almost independent of mixed solvent composition (FA), or be exothermic and monotonic functions (ACN). The enthalpy coefficients of pair interactions (h _xy ) between DL-α-alanine and organic solvent molecules were calculated. The linear Kamlet-Taft equation was used to correlate the h _xy values with the properties of organic solvents.     

Kinetics of hydroquinone chemisorption at polycrystalline platinum electrodes: The effect of surface roughness

The rate of hydroquinone (HQ) chemisorption from aqueous H₂SO₄ onto annealed (smooth) and platinized (rough) polycrystalline Pt has been studied. Previously, equilibrium adsorption measurements indicated that at smooth Pt surfaces, adsorption of HQ at c_HQ ⩽ 0.1 mM yielded flat (η⁶)-oriented species while adsorption at c_HQ ⩾ 1 mM resulted in edge (2,3-η²)-attached intermediates. Edge-attached species were not formed efficiently at roughened Pt surfaces. The present data show that the rate of η⁶-HQ chemisorption was significantly lower at roughened than at smooth surfaces. Analysis of the rate data gave the following enthalpies and entropies of activation at smooth (sm) and platinized (pt) surfaces: ΔH^≠_sm,0.1mM = 12.5 kJ/mol; ΔH^≠_sm,2mM = 8.3 kJ/mol; ΔS^≠_sm,0.1mM = −83 J/mol K; ΔS^≠_sm,2mM = −117 J/mol K; ΔH^≠_pt,0.4mM = 12.5 kJ/mol; ΔH^≠_pt,2mM = 12.5 kJ/mol; ΔS^≠_pt,0.4mM = −92 J/mol K; ΔS^≠_pt,2mM = −100 J/mol K. The similarity between ΔH^≠_{pt,0.4 mM}, ΔH^≠_{pt,2 mM} and ΔH^≠_{sm,0.1 mM}, and between ΔS^≠_{pt,0.4 mM}, ΔS^≠_{pt,2 mM} and ΔS^≠_{sm,0.1 mM} correlate with the earlier finding that adsorption of HQ onto roughened Pt surfaces occurred primarily in the flat orientation at all concentrations studied.     

Binding equilibria between β-cyclodextrin and p-nitro-aniline derivatives: the first systematic study in mixed water-methanol solvent systems

Complexation equilibria, in mixed water-methanol solvent media, between native β-cyclodextrin and a set of suitably selected p-nitro-aniline derivatives were studied by means of polarimetry. The effects exerted by the organic co-solvent on the conditional inclusion free energies ΔG_cond⁰ and the differential molar optical rotations ΔΘ were thoroughly analyzed under the perspective of the enthalpy-entropy compensation effect. Experimental data suggest an intimate participation (‘dynamic co-inclusion’) of solvent molecules in the formation and in the conformational dynamics of the host-guest inclusion complex.     

NMR and FTIR studies of coordinate-bonding and intramolecular and intermolecular hydrogen bonding in zinc(II)(3,5-diisopropylsalicylate)2

Carboxylate and salicylic OH coordinate bonding as well as intramolecular and intermolecular hydrogen bonding of bis-3,5-diisopropylsalicylatozinc(II), [Zn^II(3,5-DIPS)₂], with Lewis bases were studied to determine mechanisms accounting for antioxidant reactivity of Zn^II(3,5-DIPS)₂. Apparent thermodynamic parameters: K _eq, ΔS ⁰, ΔH ⁰, and ΔG ⁰ were determined for these equilibria with bonding of two molecules of dimethyl sulfoxide-d₆ (DMSO) or ethyl acetate-d₈ (EA) to the Zn^II using NMR and FTIR. We conclude that addition of two equivalents of DMSO or EA to non-polar solutions of Zn^II(3,5-DIPS)₂ results in bonding of DMSO or EA to Zn^II via sulfoxide or ester carbonyl oxygen atoms with ternary complex formation, leading to weakening of carboxylate and salicylic OH coordinate bonding to Zn^II and strengthening intramolecular hydrogen bonding between protons of salicylic OH groups and carboxylate oxygens. Subsequent addition of two or three additional equivalents of DMSO or EA leads to intermolecular hydrogen bonding between protons of salicylic OH groups.     

Complex equilibria in unsaturated vapor over AlBr<Subscript>3</Subscript>

Unsaturated AlBr 3 vapor pressure was measured over the temperature and pressure ranges 560–845 K and 54–145 torr by the static method using a quartz diaphragm pressure gauge with increased sensitivity (the confidence interval of pressure, including thermal drift of zero pressure gauge point, was 0.3 torr, and that of temperature, 0.3 K). Two equilibrium models were considered, one including AlBr₃ and Al₂Br₆ and the other, AlBr₃, Al₂Br₆, and Al₃Br₉. The molecular constants of all vapor constituents were determined using density functional theory at the B3LYP/6-31G(d,p) level. The thermodynamic functions of all bromides were calculated in the rigid rotator-harmonic oscillator approximation. The enthalpies of independent equilibria for each model were determined by minimizing the residual sum of the squares of pressure discrepancies. According to the first model, 0.5Al₂Br₆ = AlBr₃, ΔH ^o(298.15) = 13629.1 ± 9 cal/mol. According to the second model, 0.5Al₂Br₆ = AlBr₃, ΔH ^o(298.15) = 13638.8 ± 8 cal/mol, and 1.5Al₂Br₆ = Al₃Br₉, ΔH ^o(298.15) = ?8528 ± 800 cal/mol. The second model, for which the variance of pressure differs insignificantly from the experimental variance of pressure, should be given preference.     

Gaseous complexes of cobalt(II) bromide and pyridine

The stepwise decomposition of CoBr₂py₂(s) has been investigated on a thermobalance by the “modified entrainment” method yielding Δ₁H=88.6 kJ mol¹, Δ₁S=156.6 JK^?1 mol^?1 and Δ₂H=119.0 kJ mol^?1, Δ₂S=211.8 JK^?1 mol^?1 for the dissociation of the first and second pyridine. The evaporation of CoBr₂py₂(l) and the association of gaseous pyridine to CoBr₂py(l) forming CoBr₂py₂(g) has been studied by vis spectroscopy at 250?420°C. By combining the new results with literature values, a complete thermodynamic cycle for the solid-liquid-gas equilibria in the CoBr₂-pyridine system could be established. It shows that in solution the formation of CoBr₂py₂ is not determined by the cobalt-pyridine bond energy but by the solvation energy of the rectants.     

Thermochemical study of the stepwise protonation of 1,10-diaza-4,7-dithiadecane,and its complex formation with copper(II) and nickel(II) ions in aqueous solution

The behaviour of 1,10-diaza-4,7-dithiadecane (2,2,2-NSSN) in aqueous solution in equilibria with protons, Cu²⁺ or Ni²⁺ ions has been investigated potentiometrically and calorimetrically. The protonation constants for the ligand, and the stability constants for its complexes at 25°C in 0.5 mole dm^?3 (K)NO₃ are reported, together with the corresponding thermodynamic parameters ΔG, ΔH and ΔS. The results are compared with those for 1-aza-4-thiapentane and 1,7-diaza-4-thiaheptane. The ligand 2,2,2-NSSN forms complexes of formula ML²⁺ and MHL³⁺ with both Cu²⁺ and Ni²⁺. It is found that in the non-protonated 1:1 complexes the ligand acts as a tetradentate. In the CuHL³⁺ complex, the ligand is bound through one nitrogen and two sulphur donors, whereas in the NiHL³⁺ complex the ligand is probably bound through only one nitrogen and one sulphur donor. Explanations are suggested.     

In vitro simulation of the chemical scenario of the action of an anti-thyroid drug: charge transfer interaction of thiazolidine-2-thione with iodine

Thiazolidine-2-thione (T2T) has been studied spectrophotometrically by UV–visible and IR spectra. The spectral studies have indicated that T2T has two tautomeric forms, namely thione and thiole forms, in addition to the dimeric thioamide complex existing as a hydrogen-bonded dimer of two thione forms. Interaction of the T2T as an electron donor with iodine as a typical σ-type acceptor has been studied spectrophotometrically. Electronic absorption spectra of the system T2T–I₂ in several organic solvents of different polarities have performed a clear charge transfer (CT) band in each spectrum. Formation constants (K_CT) and molar absorption coefficients (?_CT) and thermodynamic properties, ΔH, ΔS, and ΔG, of this system in various organic solvents were determined and discussed. The stoichiometric ratio of the T2T–I₂ system in solutions was found to be 1:1 T2T:I₂, whereas the elemental analysis of the prepared solid CT complex has illustrated the same stoichiometry. The obtained K_CT and ?_CT values have indicated that T2T is a donor of moderately strength capable of interacting with the iodine just to form the corresponding CT complex with an iodine molecule without further reducing of the iodine to either of the corresponding poly-iodide ions viz. I₃^?, I₅^?, etc. This action of spongy trapping of iodine simulates in vitro the chemical scenario of the anti-thyroid action of this compound.