Limitation observed in the application of the three dimensional solubility parameters to the coating formulation of poly ( 3-hydroxybutyrate-hydroxyvalerate ) systems

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 (3hydroxybutyrate-hydroxyvalerate) polymeric coating system, and hence identify any limitation in the application of the theory. This aspect was investigated in the study. Method: The structural group contribution method was employed to compute the partial and total solubility parameters of the compounds – the biopol polymer, a series of organic solvents and plasticizers. The computed partial solubility parameters included: dipole-dipole (δd), polar (δp) and hydrogen bonding (δh). Following a standard procedure in the literatures, the δd and δp values were


Introduction
The term solubility parameter (δ) is defined as the square root of the cohesive energy density (E/V) of a compound 1 , thus: where E is the molar cohesive energy of a compound of molar volume, V.
The total solubility parameter (δ t ) is made up of three partial or component cohesive interactions namely: dipole -dipole (δ d ), polar (δ p ), and hydrogen bonding (δ h ) 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 studies 2,3,4,5 .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 interaction 6 .With polar compounds, the two dimensional solubility parameter is applied whereby δ p is plotted against δ d 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 blends 7 .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 δ d and δ p interactions are combined to form a composite solubility parameter designated δ v 8 .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 δ h versus δ v 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 threecomponent interactions (δ d , δ p , and δ h ) are considered together in determining the energy level of a compound.From Eqn. 3, the value of δ v is given by: The distance between the positions of any two compounds in the map is a measure of the exchange cohesive energy (∆ 2 δ), which must be overcome for the interaction to occur.The lower the ∆ 2 δ value the greater the probability of miscibility.The ∆ 2 δ value is given by the expression 5, 8 : For a polymer (P) and solvent (S), ∆ 2 δ h = [δ h (P)δ h (S)] 2 and ∆ 2 δ v = [δ v (P) -δ v (S)] 2 .The ∆ 2 δ 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 drugs 5, 9 .Eichie et al also employed these parameters to select plasticizers and solvents, which are miscible with the acrylate methcrylate copolymers 10 .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-hydroxybutyratehydroxyvalerate) polymeric coating system is used as a case in point.

Materials and Methods
The test polymer poly (3-hydroxylbutyratehydroxylvalerate) 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 drugs 11,12 .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, δ d , δ p and δ h , 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 compound 13 , designated F d , F p or F h respectively, and the published molar volumes of such structural groups 14 .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 Braun 5 .The partial solubility parameter of each structural group is given by

P l a s t i c i z e r s
A c e t y lt r ib u t y lc it r a t e A c e t y l t r i e t h y lc i t r a t e V F / and the total contribution by all the structural groups in the compound is given by:

D ib u t y lp h t h a la t e D ie t h y lp
. The δ p interactions of the compound will, for instance be given by:

Construction of energy maps and calculation of the exchange cohesive energies (∆ 2 δ).
To obtain the energy maps for the compounds, the computed values of the partial solubility parameters due to hydrogen bonding (δ h ) were plotted against the combined values for polar and dispersion interactions (δ v Eqn 5) for the polymer, solvents, and the plasticizers.The δ h Trop J Pharm Res, June 2005; 4 (1) versus δ v 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 (∆ 2 δ) needed for the interaction.The values for the polymer-solvent or polymer-plasticizer interactions were calculated from Eqn 6.

Test for polymer -solvent and polymerplasticizer 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.

Calculated values of the solubility parameters.
These are presented in Table 1 (for the polymer, the solvents and plasticizers), the parameters include the δ d , δ h , δ p ,δ v and d t 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 δ v values as the polymer even though their δ p interactions (component of δ v ) were markedly different from those of the polymer.These solvents include: acetone, dioxane, ethanol, tetrahydrofurane, and toluene.This means that the δ v parameter did not clearly reflect the difference in the δ p interactions of the solvents compared with the polymer in these instances.Of these four solvents, dioxane also had similar values of δ h as the polymer.Some of the plasticizers also had similar δ v values as the polymer (Table 1).These include acetyltributylcitrate, acetyltriethylcitrate, triacetin, tributylcitrate, and triethylcitrate.However, in this case, their δ p values were closer to that of the polymer than was the case with the solvents.Thus in these situations, δ v more accurately reflected the pattern of the δ d and δ p 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 ∆ 2 δ value 1.93 J.cm -3 .mol - 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 Solvents with lower ∆ 2 δ 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 ∆ 2 δ values were also low ≤ 4.12 Jcm -3 mol -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.as the polymer.Their δ d and δ p 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 rizing the parameter δ v does not clearly reflect the difference in pattern of δ d and δ p 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 δ v parameters of the compounds also implies that the δ d and/or δ p interactions are also similar.

A T Akadedmischer Austausdienst (DAAD) Germ
for sponsoring this collaborative research.

Fig. 1 :
Chemical structure of biopol.showing the various structural groups Table 1: Calculated values of the solubility parameters of the compounds C o m p o u n d S o l u b i l i t y p a r a m e t e r s ( J .c m -3 .m o l -1 ) v e n t s A c e t o n e C h lo r o f o r m D ic h lo r o m e t h a n e D io x a n e E t h a n o l I s o p r o p a n o l T e t r a h y d r o f u r a n e T o lu e n e h t h a la t e G ly c e r o l P a r a f f in S o r b it o l T r ia c e t in T r ib u t y lc it r a t e T r ie t h y lc it r a t e 1 Trop J Pharm Res, June 2005; 4 (1)

Table 3 :
Exchange cohesive energy (J.cm -3 .mol - ) for the interaction between biopol and the plasticizers based on three dimensional consideration.
was identified that the plasticizers (e.g.acetyltrietylcitrate), which the theory predicted as miscible with the polymer, had similar δ v values Trop J Pharm Res, June 2005; 4 (1)