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Abstract  

The enthalpies of solution in water of RE(His)(NO3)3 H2O (RE=La—Nd, Sm—Lu, Y) were measured calorimetrically at 298.15 K, and the standard enthalpies of formation of RE(His)aq 3+ (RE=La—Nd, Sm—Lu, Y) were calculated. The plot of the enthalpies of solution vs. the atomic numbers of the elements in the lanthanide series exhibits the tetrad effect.

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Abstract  

The enthalpies of solution of potassium chloride (KCl) in water and magnetically treated water (magnetized water) have been measured at 298.15 K using a LKB-8700 precision solution calorimeter. From the experimental results, it was observed that the effect of magnetic field on the enthalpy of solution is measurable. This is probably due to the distortion of the hydrogen bond of water resulting from magnetic treatment.

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Abstract  

The enthalpies of solution in water of L--methionine and its zinc complexes Zn(Met)Cl2, Zn(Met)2Cl2·2H2O, Zn(Met)(NO3)2·1/2H2O, Zn(Met)3(NO3)2·H2O and Zn(Met)SO4·H2O have been measured at 298.15 K. The standard enthalpy of formation of met(aq) has been calculated. The experimental results have been discussed.

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, thermodynamic studies at low concentration, of less than 0.05 mol kg −1 , are scarce; in the literature, data are found for partial molar volumes at molar concentrations above 0.05 mol L −1 [ 6 ] and it is only possible to find data of enthalpies of solution at

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Abstract  

The direct measurements of differential enthalpies of solution Δsol H 2, of LiCl·H2O, NaCl, KCl, MgCl2·6H2O, CaCl2·6H2O and BaCl2·2H2O, as the function of molality,m, in the region of concentrated solutions were performed. On this basis the enthalpies of crystallization, Δcryst H m, were calculated and compared to the appropriate literature data.

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Abstract  

Enthalpies of solution of various terfenadine samples in methanol and in ethanol were measured. Samples were prepared by crystallization in different solvents. The calorimetric results give important information on crystal structure of the terfenadine forms and on the solute/solvent interactions of this compound with the solvents.

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Abstract  

The enthalpies of solution and dilution of glycine, L-α-alanine, L-valine, L-α-leucine, L-α-serine and L-α-threonine in water were measured at 298.15 K. The results were applied to calculate the enthalpic coefficients of homogeneous interactions between zwitterions of L-α-amino acids in aqueous solutions.

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Abstract  

The standard molar enthalpies of solution of glycine, L-α-alanine, L-α-valine and L-α-leucine in aqueous solutions of urea at 298.15 K were determined by calorimetry. The results obtained were used to calculate the heterogeneous enthalpic interaction coefficients between the zwitterions of the L-α-amino acids and a molecule of urea in water. The values of the resultant enthalpic interaction coefficients are interpreted in terms of the effects of the hydrophobic alkyl groups on the interactions between the zwitterions of the L-α-amino acids and a polar molecule of urea in aqueous solutions.

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Abstract  

The enthalpies of solution
\documentclass{aastex} \usepackage{amsbsy} \usepackage{amsfonts} \usepackage{amssymb} \usepackage{bm} \usepackage{mathrsfs} \usepackage{pifont} \usepackage{stmaryrd} \usepackage{textcomp} \usepackage{upgreek} \usepackage{portland,xspace} \usepackage{amsmath,amsxtra} \pagestyle{empty} \DeclareMathSizes{10}{9}{7}{6} \begin{document} $$\Updelta_{sol}^{{}} H_{m}^{{}}$$ \end{document}
of polymorphic forms I and II of theophylline in water at 298.15 K using the isoperibol solution calorimeter have been determined in the range of concentration (0.311–1.547) · 10−3 /mol · kg−1. The enthalpies of hydration
\documentclass{aastex} \usepackage{amsbsy} \usepackage{amsfonts} \usepackage{amssymb} \usepackage{bm} \usepackage{mathrsfs} \usepackage{pifont} \usepackage{stmaryrd} \usepackage{textcomp} \usepackage{upgreek} \usepackage{portland,xspace} \usepackage{amsmath,amsxtra} \pagestyle{empty} \DeclareMathSizes{10}{9}{7}{6} \begin{document} $$\Updelta_{hyd}^{{}} H_{m}^{o}$$ \end{document}
were determined from the experimentally obtained the enthalpies of solution for aqueous solutions and previously determined enthalpies of sublimation
\documentclass{aastex} \usepackage{amsbsy} \usepackage{amsfonts} \usepackage{amssymb} \usepackage{bm} \usepackage{mathrsfs} \usepackage{pifont} \usepackage{stmaryrd} \usepackage{textcomp} \usepackage{upgreek} \usepackage{portland,xspace} \usepackage{amsmath,amsxtra} \pagestyle{empty} \DeclareMathSizes{10}{9}{7}{6} \begin{document} $$\Updelta_{s}^{g} H_{m}^{o} .$$ \end{document}
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Abstract  

Results of calorimetric determination of integral enthalpies of solution of some hydrates (monohydrates and heptahydrates) of 3d transition metal sulphates such as FeSO4, NiSO4 and MnSO4 in three-component systems at sulphuric acid concentrations up to 2M are reported. Measured values of integral enthalpies of solution are the basis for calculation of activity coefficient temperature dependences according to Pitzer's model.

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