Determination of Ibuprofen Vapor Pressure at Temperatures of Pharmaceutical Interest

An Examination of the Thermodynamics of Fusion, Vaporization, and Sublimation of Ibuprofen and Naproxen by Correlation Gas Chromatography

“…The available literature data as well as a few new measurements are summarized in Table 1. [1][2][3][4][5][6][7][8][9][10][11][12][13][14][15][16][17] The enthalpies reported in Table 1 are all temperature dependent and all are reported at the temperatures noted in the table. As many of the measurements including the activation energy, vaporization, and sublimation enthalpy data have been measured at highly divergent temperatures, comparison of the consistency of these measurements is problematic.…”

“…Equations for the adjustment of phase transition enthalpies have been developed and are summarized as vap Hm(298 K) = sub Hm(298 K) − fus Hm(298 K) (1) sub Hm(298 K)/kJ · mol −1 = sub Hm(T m ) + 0.75 + 0.15 × C p (c) (T m − 298.15)/1000 (2) vap Hm(298 K)/kJ · mol −1 = vap Hm(T m ) + 10.58 + 0.26 C p (l) (T m − 298.15)/1000 (3) fus Hm(298 K)/kJ · mol −1 = fus Hm(T m ) + [0.15C p (c) − 0.26C p (l) − 9.93] (Tfus − 298.15) /1000 (4) Equation 1 is a thermodynamic equality used to evaluate vaporization enthalpies from the corresponding sublimation and fusion enthalpy provided that all enthalpies are adjusted to a common temperature. Eq.…”

Desviaciones al modelo logarítmico-lineal en la solubilidad de ibuprofén y naproxén en mezclas cosolventes propilenoglicol-agua

“…De la misma forma se observa que en todos los casos la solubilidad experimental del IBP es mayor que la del NAP, lo cual es consistente con lo esperado de acuerdo a la solubilidad ideal (0,268 y 0,0833 para IBP y NAP a 25,0 °C, respectivamente 20,21 ); esto es, de acuerdo con las propiedades físicas de los fármacos en el estado sólido, ya que las entalpías y las temperaturas de fusión son mayores para el NAP respecto al IBP (Tabla 1) y por lo tanto, la tendencia hacia el estado líquido es mayor en el caso del IBP. Es necesario aclarar que bajo las condiciones cosolventes estudiadas aquí, la disociación de estos dos fármacos es mínima, con lo que se tiene que la solubilidad total presentada por éstos, corresponde prácticamente en su totalidad a la de la forma molecular no disociada, y por lo tanto se trataría de la solubilidad intrínseca 13 .…”

A Combined Calorimetric and Semiempirical Quantum Chemical Approach To Describe the Solution Thermodynamics of Drugs

“…A correction for ∆H MELT to account for the difference of the heat capacities at the melting and at room temperature was not necessary. The enthalpy of sublimation (∆H SUB ) was taken from the work of Ertel et al, 32 who determined ∆H SUB from a sublimation pressure versus 1/T plot to be 121.00 kJ/mol. The enthalpy of the gas-liquid phase transition shown in Figure 1 was calculated with the help of the Hess theorem.…”