Extraction Technologies for Medicinal and Aromatic ... - Capacity4Dev
Extraction Technologies for Medicinal and Aromatic ... - Capacity4Dev Extraction Technologies for Medicinal and Aromatic ... - Capacity4Dev
10 SUPERCRITICAL FLUID EXTRACTION OF MEDICINAL AND AROMATIC PLANTS: FUNDAMENTALS AND APPLICATIONS At suitable conditions, any fl uid can reach its supercritical state. However, only those having a critical temperature not far from ambient temperature can be used as alternative solvents for the extraction of MAPs. Carbon dioxide (CO 2 ), with T C =31.06° C and P C =73.81 bar, is the most attractive solvent, because of its proprieties regarding toxicity, fl ammability and cost. The possibility of using supercritical fl uids (SFs) as extraction solvents is directly linked to their density. In fact, according to an empirical correlation proposed by Chrastil in 1982, s = ρ a exp ( b T + c ) (1) where s is the solute solubility, ρ is the solvent density and T is the absolute temperature; a, b and c are correlation parameters to be adjusted to experimental solubility data in supercritical CO 2 . When a fl uid approaches the critical conditions, its density gets closer and closer to that of the liquid state. This can be seen, for CO 2 , in Figure 1, where density isotherms are plotted against the reduced pressure. For example, at T = 35° C and P = 200 bar, ρ = 866 kg/m 3. It is also clear from Figure 1 that, close to the critical point, both the compressibility and expansion coeffi cient of the fl uid are high, so slight changes in the operating conditions can signifi cantly modify the density, i.e. the supercritical fl uid solvent power. The importance of the Chrastil equation (Eq. 1) lies in the fact that solvent density is identifi ed as the key factor in a successful SFE process. Figure 1: Density vs. pressure diagram for carbon dioxide When plotted against solvent density, solubility data for supercritical CO 2 always display a regular trend such as that in Figure 2a, whereas a more complex behavior is seen when pressure is improperly used as the independent process variable (Figure 2b). 170
EXTRACTION TECHNOLOGIES FOR MEDICINAL AND AROMATIC PLANTS A Figure 2: Solubility of 1,4-bis-(n-propylamino)-9,10-anthraquinone in supercritical CO 2: as a function of solvent density (2a) and of pressure (2b) Coming back to Eq. 1, is important to point out that it is not theoretically correct and must be applied within restricted temperature ranges only. More importantly, the exponential form of Eq. 1 does not guarantee that the solubility of a solute in SF is high. The solubility depends on parameters a, b and c; in fact, in the case of CO 2 , the solubility of a solute of interest for MAP applications is at best in the range of 1 to 1000 by weight or often 1 to 10,000 (Figure 2a illustrates this). This is because CO 2 is a poor solvent, even at supercritical conditions. In addition, this holds for non-polar substances only, as supercritical CO 2 does not dissolve polar molecules at all. Actually, CO 2 is a good solvent only for low molecular weight solutes. The limit on solubility is dictated by thermodynamics. According to the iso-fugacity criterion applied to the substance to be extracted, between the two phases at equilibrium (the condensed one – either solid or liquid – and the supercritical one), we have: y i = Psat P E i (2) E i = ϕ i o, v P – Psat S/L v exp ϕ (v i RT ) (3) where y i is the mole fraction of i in the supercritical phase, ϕ i o,v and ϕ i v are the fugacity coeffi cients of i in the standard state and in the mixture, respectively, at the process conditions, P sat is the solute saturation (or sublimation) partial pressure (i.e. the component volatility), and v S/L is the molar volume of the condensed phase (either solid or liquid). T is the absolute temperature and R is the universal gas constant. E i is the so-called enhancement factor, which accounts for the increasing solubility due to system nonidealities with respect of the ideal behavior (given by Eq. 2). 171
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EXTRACTION TECHNOLOGIES FOR MEDICINAL AND AROMATIC PLANTS<br />
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Figure 2: Solubility of 1,4-bis-(n-propylamino)-9,10-anthraquinone in supercritical CO 2: as a<br />
function of solvent density (2a) <strong>and</strong> of pressure (2b)<br />
Coming back to Eq. 1, is important to point out that it is not theoretically<br />
correct <strong>and</strong> must be applied within restricted temperature ranges only.<br />
More importantly, the exponential <strong>for</strong>m of Eq. 1 does not guarantee<br />
that the solubility of a solute in SF is high. The solubility depends on<br />
parameters a, b <strong>and</strong> c; in fact, in the case of CO 2 , the solubility of a solute<br />
of interest <strong>for</strong> MAP applications is at best in the range of 1 to 1000 by<br />
weight or often 1 to 10,000 (Figure 2a illustrates this). This is because CO 2<br />
is a poor solvent, even at supercritical conditions. In addition, this holds<br />
<strong>for</strong> non-polar substances only, as supercritical CO 2 does not dissolve polar<br />
molecules at all. Actually, CO 2 is a good solvent only <strong>for</strong> low molecular weight<br />
solutes.<br />
The limit on solubility is dictated by thermodynamics. According<br />
to the iso-fugacity criterion applied to the substance to be extracted,<br />
between the two phases at equilibrium (the condensed one – either solid or<br />
liquid – <strong>and</strong> the supercritical one), we have:<br />
y i = Psat<br />
P E i (2)<br />
E i = ϕ i o, v P – Psat<br />
S/L<br />
v<br />
exp<br />
ϕ (v<br />
i RT ) (3)<br />
where y i is the mole fraction of i in the supercritical phase, ϕ i<br />
o,v<br />
<strong>and</strong> ϕ i<br />
v<br />
are<br />
the fugacity coeffi cients of i in the st<strong>and</strong>ard state <strong>and</strong> in the mixture, respectively,<br />
at the process conditions, P sat is the solute saturation (or sublimation)<br />
partial pressure (i.e. the component volatility), <strong>and</strong> v S/L is the molar volume<br />
of the condensed phase (either solid or liquid). T is the absolute temperature<br />
<strong>and</strong> R is the universal gas constant. E i is the so-called enhancement<br />
factor, which accounts <strong>for</strong> the increasing solubility due to system nonidealities<br />
with respect of the ideal behavior (given by Eq. 2).<br />
171