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Tropical Journal of Pharmaceutical Research, Vol. 4, No. 1, June 2005, pp. 355-362 Research Article Limitation observed in the application of the three dimensional solubility parameters to the coating formulation of poly (3-hydroxybutyrate-hydroxyvalerate) systems Florence Eichie1*, Roland Sydney Okor1 and Rudiger Groning2 1Department of pharmaceutics and Pharmaceutical Technology, Faculty of Pharmacy, University of Benin, Benin City, Nigeria. Code Number: pr05005 Abstract Purpose: Poly (3-hydroxybutyrate-hydroxyvalerate)
displayed high dipole-dipole interaction, a high hydrogen bonding but low
polar interaction, and was therefore expected to be miscible with solvents/plasticizers
that exhibit similar pattern of cohesive interaction. To determine the
applicability, or otherwise of the theory of the three dimensional solubility
parameters to the formulation of poly (3-hydroxybutyrate-hydroxyvalerate)
polymeric coating system, and hence identify any limitation in the application
of the theory. This aspect was investigated in the study. Key words: Solubility parameters, cohesive energy, miscibility of compounds, poly (3-hydroxybutyrate-hydroxyvalerate) system. Introduction The term solubility parameter (δ) is defined as the square root of the cohesive energy density (E/V) of a compound1, thus: where E is the molar cohesive energy of a compound of molar volume, V. The total solubility parameter (δt) is made up of three partial or component cohesive interactions namely: dipole - dipole (δd), polar (δp), and hydrogen bonding (δh) interactions. Thus: The corresponding expression for the total molar cohesive energy is: The theory of solubility parameters has application in the prediction of miscibility of compounds by simulation studies2, 3, 4, 5. In such simulations, similarity in the total or partial solubility parameters of the compounds determines their miscibility. The total solubility parameter is applicable to non-polar compounds only where the dipole-dipole interaction is predominant over other forces of interaction6. With polar compounds, the two dimensional solubility parameter is applied whereby δp is plotted against δd to obtain energy maps, which depict the energy levels of the various compounds under test. Rowe applied the energy maps of the two dimensional solubility parameters to predict miscibility between ethyl cellulose and hydroxypropyl cellulose and the miscibility of plasticizers with the polymer blends7. However, such two dimensional based maps could not be used to select or predict the solvents and plasticizers that are miscible with the acrylatemethacrylate copolymer where the dipole-dipole interactions are considerable and should therefore be considered with the other forces of interaction in the simulation. With this type of compounds, the three dimensional solubility parameters is applied whereby the δd and δp interactions are combined to form a composite solubility parameter designated δv8. Two of the three parameters are combined since it is not possible to represent all three parameters graphically as y-x plots. A plot of δh versus δv yields the energy maps from which miscibility can be predicted. Closeness of the compounds to each other in the map implies miscibility. By this approach, all three-component interactions (δd, δp, and δh) are considered together in determining the energy level of a compound. From Eqn. 3, the value of δv is given by: The distance between the positions of any two compounds in the map is a measure of the exchange cohesive energy (∆2δ), which must be overcome for the interaction to occur. The lower the ∆2δ value the greater the probability of miscibility. The ∆2δ value is given by the expression5, 8: For a polymer (P) and solvent (S), ∆2δh = [δh(P) - δh(S)]2 and ∆2δv = [δv(P) - δv(S)]2. The ∆2δ values for the polymer –plasticizer interactions are similarly obtained. The three dimensional solubility parameters have been used to predict accurately the skin permeability and intestinal absorption of various drugs5, 9. Eichie et al also employed these parameters to select plasticizers and solvents, which are miscible with the acrylate methcrylate copolymers10. However in this report we present evidence to show that there is an identifiable limitation in the general application of the theory. The formulation of poly (3-hydroxybutyrate-hydroxyvalerate) polymeric coating system is used as a case in point. Materials and Methods The test polymer poly (3-hydroxylbutyrate –hydroxylvalerate) was received under the trade name, Biopol®, from Zeneca Bioproducts, Monsanto, Portugal. Its chemical structure is given in Fig. 1. It is water insoluble but swellable in aqueous fluids. It has been investigated as a biodegradable polymer for slow biorelease of drugs11, 12. The solvents and plasticizers employed for the miscibility tests were all of reagent grade (BDH) and are listed in Tables 1 and 2. Computation of the partial solubility parameters The partial solubility parameters, δd, δp and δh, for each compound were calculated using the published values of the partial molar cohesive energy (due to dipole, polar, or hydrogen bonding) of each structural group in the compound13, designated Fd, Fp or Fh respectively, and the published molar volumes of such structural groups14. Details of the procedure have been published earlier 5, 9,10. Essentially, the known values of the molar cohesive energies for the various structural groups and the corresponding molar volumes (V) of the structural groups are typed into an advanced parameter set, based on a computer programme, SPWin® version 2, developed by Groning and Braun5. The partial solubility parameter of each structural group is given by and the total contribution by all the structural groups in the compound is given by: . The δp interactions of the compound will, for instance be given by: Construction of energy maps and calculation of the exchange cohesive energies (∆2δ). To obtain the energy maps for the compounds, the computed values of the partial solubility parameters due to hydrogen bonding (δh) were plotted against the combined values for polar and dispersion interactions (δv Eqn 5) for the polymer, solvents, and the plasticizers. The δh versus δv plots showed the specific energy locations of the compounds. The energy difference between any two compounds in the energy map is the exchange cohesive energy (∆2δ) needed for the interaction. The values for the polymer-solvent or polymer-plasticizer interactions were calculated from Eqn 6. Test for polymer – solvent and polymer –plasticizer miscibility Free films of thickness, 11±1.47µm were formed by casting a solution of the polymer (3ml, 10%w/v) on a glass plate, allowing 24h drying time at room temperature 20°C. The films were peeled off from the substrate with a knife. Samples of the free film surface were mounted on the specimen stub and vacuum coated with a thin gold shadow using the Balzer Union evaporator (Model: SCD 040). The coated specimens were examined at various magnifications using electron microscopy (model: Stereoscan S4 TL 10701 –OM- 96118, Cambridge, England). A homogenous film surface indicated compatibility while an inhomogenous surface indicated incompatibility of the solvent or plasticizer with the polymer. Results Calculated values of the solubility parameters. These are presented in Table 1 (for the polymer, the solvents and plasticizers), the parameters include the δd, δh, δp,δv and dt values. The first observation is that the polar interaction of the polymer was considerably lower than those of the solvents and the plasticizers. The solvents in turn were more polar than the plasticizers. Some of the solvents displayed similar δv values as the polymer even though their δp interactions (component of δv) were markedly different from those of the polymer. These solvents include: acetone, dioxane, ethanol, tetrahydrofurane, and toluene. This means that the δv parameter did not clearly reflect the difference in the δp interactions of the solvents compared with the polymer in these instances. Of these four solvents, dioxane also had similar values of δh as the polymer. Some of the plasticizers also had similar δv values as the polymer ( Table 1). These include acetyltributylcitrate, acetyltriethylcitrate, triacetin, tributylcitrate, and triethylcitrate. However, in this case, their δp values were closer to that of the polymer than was the case with the solvents. Thus in these situations, δv more accurately reflected the pattern of the δd and δp interactions in both the polymer and the plasticizers. The energy maps and the exchange cohesive energies () for prediction of compound miscibility. The energy maps for the polymer – solvent, and the polymer –plasticizer interaction are presented in Figs 2 and 3, respectively. The exchange cohesive energy values are in Tables 3 and 4. Dioxane with ∆2δ value 1.93 J.cm-3.mol-1 was closest to the polymer in the map ( Fig. 2). Theoretically, this solvent should be miscible with the polymer. In practice, the polymer was not miscible with dioxane, rather it was only partially miscible with dichloromethane (∆2δ = 48.19 Jcm-3mol-1) forming a homogenous colloidal solution. The scanning electron micrographs (SEM) of films cast from these two solvents are shown in Fig. 4. The film cast from dichloromethane revealed a homogenous surface while the dioxane cast films were inhomogeneous. Solvents with lower ∆2δ values including dioxane were not miscible with the polymer as theoretically expected, meaning that the prediction was erroneous. In the case of the polymer/plasticizer systems, the following palsticizers were close to the polymer in the energy map ( Fig. 3): acetyltriethylcitrate, triacetin tributylcitrate, acetyltributylcitrate, and dibutylphthalate. Their ∆2δ values were also low ≤ 4.12 Jcm-3mol-1 ( Table 3). In practice, these plasticizers were miscible with the polymer, as evidenced by the SEM of resulting films. Thus the plasticizers which clustered around the polymer in the energy maps were actually miscible with the polymer. Discussion In the application of the three dimensional solubility parameters, the δd and δp interactions are usually combined to form a composite solubility parameter δv, to allow the plotting of the energy data in a y-x form5, 8, 10 . The intention is that by plotting dh versus δv, compounds of similar δd, δp and δh interactions will be close to each other in the resulting energy maps, indicating miscibility. This implies that where two compounds have similar δv values, their δd and δp values should also be similar for miscibility to occur. In the case of the polymer – solvent systems studied, it was identified that some of the solvents (e.g. dioxane), which the theory predicted as miscible with the polymer actually had similar d systems studied, it was identified that some of the solvents (e.g. dioxane), which the theory predicted as miscible with the polymer actually had similar δv values as the polymer, whereas their δd , and δp interactions were in fact different from those of the polymer (Table 1). Of particular notice is that these solvents were considerably more polar than the polymer. The inability of δv to clearly reflect difference in the pattern of the δd , and δp interactions in the polymer and in the solvents in all situations thus accounted for the erroneous prediction. In the case of the polymer/plasctizer systems, it was identified that the plasticizers (e.g. acetyltrietylcitrate), which the theory predicted as miscible with the polymer, had similar δv values as the polymer. Their δd and δp interactions were also similar to those of the polymer, which explains why in this case the prediction was accurate. The plasticizers were also more polar than the polymer, but the difference was not as exaggerated as was with the solvents. Conclusion The study has shown that the composite solubility parameter δv does not clearly reflect the difference in pattern of δd and δp interactions in all situations, which is a limitation in the application of the theory of the three dimensional solubility parameters. Thus, the theory will only be applicable to systems where similarity in the δv parameters of the compounds also implies that the δd and/or δp interactions are also similar. Acknowledgement The authors which to thank Deutscher Akadedmischer Austausdienst (DAAD) Germany for sponsoring this collaborative research. References
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