SOLID-STATE PROPERTIES OF AN ORAL IRON CHELATOR, 1,2-DIMETHYL-3-HYDROXY-4-PYRIDONE, AND ITS ACETIC-ACID SOLVATE .1. PHYSICOCHEMICAL CHARACTERIZATION, INTRINSIC DISSOLUTION RATE, AND SOLUTION THERMODYNAMICS

1,2-Dimethyl-3-hydroxy-4-pyridone (1), a crystalline oral iron chelator, forms an acetic acid solvate (2) on recrystallization from acetic acid and carbon tetrachloride. Compound 2 forms compact prisms, and 1 forms needles from water (mp 274-degrees-C). The X-ray powder diffraction patterns of 1 and 2 differ, indicating distinct solid phases. Compound 2 has an extra DSC endotherm at 82-degrees-C that is accompanied by a weight loss of 29% in TGA, corresponding to the desolvation of a 1:1 acetic acid solvate. Comparison of the solid-state C-13 NMR of 1 and 2 revealed two additional peaks for 2 at 20.3 and 175.6 ppm, characteristic of -CH3 and -COOH, respectively, of acetic acid. The integrated intensities confirmed the 1:1 stoichiometry between 1 and acetic acid. However, 2 underwent desolvation in air at 25-degrees-C as suggested by a change in its appearance to opaque crystals and as confirmed by X-ray powder diffraction, DSC, and TGA. Desolvation of 2 at 25-degrees-C was a zero-order process with a rate constant of 6.9-mu-mol.h-1. X-ray powder diffraction showed that crystals or compacted discs of 1 are converted to 2 in contact with glacial acetic acid (A), whereas crystals or discs of 2 are converted to 1 in contact with water. The intrinsic dissolution rate (J) and the apparent solubility (C(s) of compacted discs were determined: J(2)/J(1) = 1.39 and C(s)(2)/C(s)(1) = 1.70. From solubility measurements, the standard Gibbs free energy of transfer (DELTA-G-degrees, kcal.mol-1) at 25-degrees-C with respect to the molar concentration scale are as follows: 1 to H2O, 5.40; 2 to H2O, < 8.18; 1 to A, estimated; 2 to A, -1.40; A to H2O, -10.48 (from literature data). Using solution calorimetry, the corresponding enthalpy changes (DELTA-H-degrees, kcal.mol-1) at 25-degrees-C were measured: 1 to H2O, 18.7; 2 to H2O, 30.2; 1 to A 17.3; 2 to A, 29.4; A to H2O, -1.1. A thermodynamic cycle shows that these values are self-consistent. The positive enthalpy changes indicate that the dissolution of 1 and 2 in water or A is entropy driven. Furthermore, the dissolution of 2 in water or A is more endothermic than that of 1 by only approximately 1 kJ.mol-1. Use of isotonic phosphate buffered saline (pH 7.4) instead of water gave similar thermodynamic values (within 5%), and the main conclusions were unaltered.