# Thermodynamic Study of Racemic Ibuprofen Separation by Liquid Chromatography Using Cellulose-Based Stationary Phase

Authors: Wilson M. Ferrari; Ana C. Nascimento; Jean V. Moreira; Marco A. Cremasco
Journal: Chromatography Research International
 (2016)

---

## Abstract

Ibuprofen is a nonsteroidal anti-inflammatory drug (NSAID), also known for its significant antipyretic and analgesic properties. This chiral drug is commercialized in racemic form; however, only S-(+)-ibuprofen has clinical activities. In this paper the effect of temperature change (from 288.15 to 308.15 K) on the ibuprofen resolution was studied. A column (250
×
4.6 mm) packed with tris(3,5-dimethylphenylcarbamate) was used to obtain the thermodynamic parameters, such as enthalpy change (Δ
H), entropy change (Δ
S), variation enthalpy change (Δ
Δ
H), variation entropy change (Δ
Δ
S), and isoenantioselective temperature (T
iso). The mobile phase was a combination of hexane (99%), isopropyl alcohol (1%), and TFA (0.1%), as an additive. The conditions led to a selectivity of 1.20 and resolution of 4.55. The first peak, R-(−)-ibuprofen, presented an enthalpy change of 7.21 kJ/mol and entropy change of 42.88 kJ/K·mol; the last peak, S-(+)-ibuprofen, has an enthalpy change of 8.76 kJ/mol and 49.40 kJ/K·mol of entropy change.


---

## Body

## 1. Introduction

The importance of stereochemical compound has been studied since Louis Pasteur observed the chiral phenomenon in 1848. Chiral recognition and enantiomer distinction are fundamental phenomena in nature and chemical systems. They are present in several fields, in particular bioactive compounds, drugs, pollutants, agrochemicals, food additives, and flavors. The most significant developments in chirotechnologies were spurred by demands of drug discovery in pharmaceutical industries. The liquid chromatography has been used to provide support in drug discovery, analytical methods, and advances in preparative technique of purification [1, 2].(RS)-2-(4-(2-methylpropyl)phenyl)propanoic acid, also known as ibuprofen, is one of the most widely used nonsteroidal anti-inflammatory drugs (NSAIDs) for the treatment of arthropathies. This enantiomer is a prostaglandin and thromboxane inhibitor [3]. While most currently marketed ibuprofen products are in the form of racemate, it has long been recognized that the two enantiomers have different pharmaceutical activities [4–6]. The ibuprofen structure is shown in Figure 1.Figure 1
Ibuprofen molecular structure.The fundamental basis for distinction of enantiomers (biological or chromatographic system) is the transformation of enantiomers to diastereomers or creation of a diastereomeric relationship between ligated enantiomers (selectand, SA) and a receptor (chiral selector, CS). Equilibrium process such as the CS-SA complexation can be explained by energy balance of free and complexed state and is often studied based on thermodynamic considerations. Thermodynamic quantities of chromatographic equilibrium processes such as the direct enantiomer separation with chiral stationary phase (it uses adsorbents with a chiral selector) can be deduced by measurement of the chromatographic parameters over a certain temperature range from van’t Hoff [1, 7–9].This paper aims to study the adsorption of ibuprofen on cellulose tris(3,5-dimethylphenylcarbamate) and to evaluate the effect of temperature in chiral separation. The following parameters were analyzed: enthalpy change (Δ
H), entropy change (Δ
S), and isoenantioselective temperature (T
iso).


## 2. Material and Methods

### 2.1. Reagents

Racemic ibuprofen (molar mass 206.29 g/mol and purity 98%) and 1,3,5-tri-tert-butylbenzene (TTBB, molar mass 246.44 g/mol and purity 97%) were purchased from Sigma-Aldrich. The chiral analytical column (250 mm× 4.6 mm) was purchased from Phenomenex and originally packed with silica (5 μm) coated with cellulose tris(3,5-dimethylphenylcarbamate).


### 2.2. Instrumentation

The experiments were carried out in a HPLC system; it consisted of a system controller (model CBM-20A), an UV-vis detector (SPD-20A), and two pumps (LC-10AD). The components were originally purchased from Shimadzu, Japan. The column and mobile phase were temperature-controlled using a Quimis Q214M2 (Brazil) circulating water bath. The elution order was determined by a polarimeter model P1010 (Japan).


### 2.3. Thermodynamic Parameters

The resolution of racemate was studied by means of thermodynamic parameters. Van’t Hoff approach was used to obtain the enthalpy change (Δ
H) and entropy change (Δ
S). A similar approach was also used to calculate the difference of enthalpy change (Δ
Δ
H) and entropy change (Δ
Δ
S) for the racemic ibuprofen, respectively. These values are important to obtain the isoenantioselective temperature (T
iso). The determination of these parameters can be based on the chromatographic parameters, such as the retention factor (k
i) and the selectivity (α). To obtain the isoenantioselective temperature it is necessary to know the porosity (ε), which was determined by moment analysis [10].


### 2.4. Chromatographic Parameters

The retention factor is the relation between the number of analytes in stationary phase and the molecule numbers in mobile phase. This parameter is written in terms of analyte retention time (t
R
i) and column dead time (t
0) as presented in [11](1)
k
i
=
t
R
i
-
t
0
t
0
=
ϕ
K
D
,
i
,where ϕ represents the volume phase ratio between the volume of stationary phase and mobile phase, also equal to 1
-
ε
t
/
ε
t.The selectivity (α) of separation of two components is determined by dividing their retention factors:(2)
α
=
k
j
k
i
=
t
R
j
-
t
0
t
R
i
-
t
0
.Chromatography resolution (R
S) and number of plates (N
i) are other important parameters to establish the separation condition:(3)
R
s
=
N
i
4
k
i
k
i
+
1
α
-
1
α
=
1.177
t
R
j
-
t
R
i
w
i
+
w
j
,
N
i
=
5.545
t
R
i
w
i
2
,where w
i is the peak width at half-height [12].


### 2.5. Effect of Temperature

Equation (4) describes the linear relation between natural logarithm of the retention factor and inverse of the temperature, in which slope provides enthalpy change and the intercept supplies entropy change. This is modified Van’t Hoff equation where K
D
,
i from the original equation was substituted for k
i. The parameters Δ
Δ
H and Δ
Δ
S can be obtained analogously for (4), as shown in (5). These parameters represent the difference between the less and the more retained compounds, “i” and “j”; respectively, [13–15],(4)
ln
⁡
k
i
=
-
1
T
Δ
H
i
0
R
+
Δ
S
i
0
R
+
ln
⁡
1
-
ε
ε
,
(5)
ln
⁡
α
=
-
1
T
Δ
Δ
H
j
,
i
0
R
+
Δ
Δ
S
j
,
i
0
R
,where T is temperature and R is gas constant.The last term of (4) is related to the physical properties of the stationary phase; thus, it can be considered as a constant since its limitations are not exceeded. If one simplifies the first absolute moment, the total porosity can be obtained experimentally. Therefore, total porosity is determined by (6), in which ν is superficial velocity and L is bed length [10, 14, 15](6)
t
R
=
L
v
ε
.Isoenantioselective temperature (T
iso) is the condition in which the separation does not occur due to both compounds’ coelute. If the condition α
=
1 is applied in (5), it is possible to write (7) as follows:(7)
T
iso
=
Δ
Δ
H
j
,
i
0
Δ
Δ
S
j
,
i
0
.


## 2.1. Reagents

Racemic ibuprofen (molar mass 206.29 g/mol and purity 98%) and 1,3,5-tri-tert-butylbenzene (TTBB, molar mass 246.44 g/mol and purity 97%) were purchased from Sigma-Aldrich. The chiral analytical column (250 mm× 4.6 mm) was purchased from Phenomenex and originally packed with silica (5 μm) coated with cellulose tris(3,5-dimethylphenylcarbamate).


## 2.2. Instrumentation

The experiments were carried out in a HPLC system; it consisted of a system controller (model CBM-20A), an UV-vis detector (SPD-20A), and two pumps (LC-10AD). The components were originally purchased from Shimadzu, Japan. The column and mobile phase were temperature-controlled using a Quimis Q214M2 (Brazil) circulating water bath. The elution order was determined by a polarimeter model P1010 (Japan).


## 2.3. Thermodynamic Parameters

The resolution of racemate was studied by means of thermodynamic parameters. Van’t Hoff approach was used to obtain the enthalpy change (Δ
H) and entropy change (Δ
S). A similar approach was also used to calculate the difference of enthalpy change (Δ
Δ
H) and entropy change (Δ
Δ
S) for the racemic ibuprofen, respectively. These values are important to obtain the isoenantioselective temperature (T
iso). The determination of these parameters can be based on the chromatographic parameters, such as the retention factor (k
i) and the selectivity (α). To obtain the isoenantioselective temperature it is necessary to know the porosity (ε), which was determined by moment analysis [10].


## 2.4. Chromatographic Parameters

The retention factor is the relation between the number of analytes in stationary phase and the molecule numbers in mobile phase. This parameter is written in terms of analyte retention time (t
R
i) and column dead time (t
0) as presented in [11](1)
k
i
=
t
R
i
-
t
0
t
0
=
ϕ
K
D
,
i
,where ϕ represents the volume phase ratio between the volume of stationary phase and mobile phase, also equal to 1
-
ε
t
/
ε
t.The selectivity (α) of separation of two components is determined by dividing their retention factors:(2)
α
=
k
j
k
i
=
t
R
j
-
t
0
t
R
i
-
t
0
.Chromatography resolution (R
S) and number of plates (N
i) are other important parameters to establish the separation condition:(3)
R
s
=
N
i
4
k
i
k
i
+
1
α
-
1
α
=
1.177
t
R
j
-
t
R
i
w
i
+
w
j
,
N
i
=
5.545
t
R
i
w
i
2
,where w
i is the peak width at half-height [12].


## 2.5. Effect of Temperature

Equation (4) describes the linear relation between natural logarithm of the retention factor and inverse of the temperature, in which slope provides enthalpy change and the intercept supplies entropy change. This is modified Van’t Hoff equation where K
D
,
i from the original equation was substituted for k
i. The parameters Δ
Δ
H and Δ
Δ
S can be obtained analogously for (4), as shown in (5). These parameters represent the difference between the less and the more retained compounds, “i” and “j”; respectively, [13–15],(4)
ln
⁡
k
i
=
-
1
T
Δ
H
i
0
R
+
Δ
S
i
0
R
+
ln
⁡
1
-
ε
ε
,
(5)
ln
⁡
α
=
-
1
T
Δ
Δ
H
j
,
i
0
R
+
Δ
Δ
S
j
,
i
0
R
,where T is temperature and R is gas constant.The last term of (4) is related to the physical properties of the stationary phase; thus, it can be considered as a constant since its limitations are not exceeded. If one simplifies the first absolute moment, the total porosity can be obtained experimentally. Therefore, total porosity is determined by (6), in which ν is superficial velocity and L is bed length [10, 14, 15](6)
t
R
=
L
v
ε
.Isoenantioselective temperature (T
iso) is the condition in which the separation does not occur due to both compounds’ coelute. If the condition α
=
1 is applied in (5), it is possible to write (7) as follows:(7)
T
iso
=
Δ
Δ
H
j
,
i
0
Δ
Δ
S
j
,
i
0
.


## 3. Results and Discussion

### 3.1. Resolution Conditions and Elution Order

The resolution conditions were based on [16–18], at which cellulose tris(3,5-dimethylphenylcarbamate) is the chiral selector. Thus, it was decided to use a longer column (250 mm × 4.6 mm) packed with smaller particles (5 μm). Both parameters have contributed to increasing efficiency.Some mobile phases were tested to resolve the racemic mixture, but only the mobile phase based on hexane promoted satisfactory results. The mobile phase composed of hexane and isopropyl alcohol, in the proportion 99/1, was chosen for chiral resolution. Trifluoroacetic acid (TFA) was also used as an additive; its proportion on mobile phase was 0.1%, in volumetric base. All the conditions set for the chromatographic resolution provided values ofα and N
i above minimum levels required for effective chromatographic resolution (α > 1.20, R
S > 1.50, and N
i > 2000). Table 1 summarizes all the mentioned values [19].Table 1
Chromatographic parameters of racemic ibuprofen separation at 308.15 K: column (250 mm × 4.6 mm) packed with cellulose tris(3,5-dimethylphenylcarbamate).
Mobile phase
α
R
S
N
i
N
j
Hexane/isopropyl alcohol (99/1)
1.20
4.55
12976
12355After setting the separation conditions, the elution order was defined through a polarimetric technique. For this, the HPLC was used in batch mode to resolve the racemic mixture in R-ibuprofen and S-ibuprofen. The rotary evaporator reduced each sample for the polarimeter sample cell volume. A calibration curve provided the concentration of both samples: 0.4 g/L for S-ibuprofen and 1.11 g/L for R-ibuprofen. Finally, the polarimeter identified the less and more retained compounds as (−)-ibuprofen and (+)-ibuprofen, respectively. Thus, in Figure2, the first peak is R-(−)-ibuprofen while the second peak is S-(+)-ibuprofen.Figure 2
Chromatograms of ibuprofen enantiomeric resolution at 308.15 K and 0.5 g/mL and TTBB. Flow ratio: 1 mL/min; wavelength: 220 nm for ibuprofen and 254 nm for TTBB; mobile phase: hexane/isopropyl alcohol (99/1).


### 3.2. Total Porosity

Porosity was calculated from the first moment method (6). This method requires a tracer compound small enough to pass through both particle and bed voids. TTBB was used to determine the porosity of chiral columns packed with cellulose tris(3,5-dimethylphenylcarbamate). The flow rate was changed from 0.2 up to 1.6 mL/min with a 0.2 mL/min step. The results are shown in Figure 3.Figure 3
Total porosity.The slope presented in Figure3 provides the value of 0.647 for porosity.


### 3.3. Thermodynamic Parameters

The adsorption phenomenon of the enantiomeric compounds is macroscopic thermodynamic quantities, which does not consider the surface heterogeneity of the stationary phase and the associated distinct adsorption behavior of enantiomers at different sites. Under the circumstances, Van’t Hoff analysis is useful to determine global information about the phenomenon [1].Using (4), modified Van’t Hoff equation, one can obtain the thermodynamic parameters. The temperatures chosen were 288.15, 293.15, 298.15, 303.15, and 308.15 K. At each temperature, racemic ibuprofen samples were injected at 0.5 g/L. Figure 4 and Table 2 present a summary of chromatograms and chromatographic values obtained from these resolutions.Table 2
Retention factor obtained in racemic ibuprofen separation.
T (K)
k
i
k
j
α
288.15
4.72
5.43
1.15
293.15
4.88
5.68
1.16
298.15
5.11
5.96
1.17
303.15
5.38
6.37
1.18
308.15
5.74
6.90
1.20Figure 4
Chromatograms of the racemic ibuprofen at several temperatures. Flow rate: 1 mL/min.In Figure4, an increase in retention time value was observed as temperature rises. This behavior has been reported in literature; however, it is not the most common one [1]. This condition will be discussed later in this paper.The retention factors from Table2 were used to plot Figure 5. From this figure and utilizing (4), it was possible to obtain Δ
H and Δ
S, for ibuprofen enantiomers as presented in Table 3. The errors for enthalpy and entropy change were, respectively, 6% and 9%.Table 3
Thermodynamic parameters of racemic ibuprofen adsorbed on cellulose tris(3,5-dimethylphenylcarbamate).
Compound
Δ
H (kJ/mol)
Δ
S (kJ/K⋅mol)
R
2
R-(−)-ibuprofen
7.21
42.88
0.975
S-(+)-ibuprofen
8.76
49.40
0.972Figure 5
Van’t Hoff plots for the determination ofΔ
H and Δ
S.Both relations presented in Figure4 are linear, suggesting that multiple mechanisms of retention do not occur [19, 20]. Furthermore, Δ
H of compounds is lower than 50 kJ/mol demonstrating physical adsorption [11]. The interactions of physisorption are characterized by relatively weak bonds. Otherwise, it would be necessary to modify the chromatographic system to elute analytes.According to [1] the adsorption phenomenon in liquid chromatographic enantiomer resolution is driven by (mostly electrostatic type) noncovalent interactions. Thermodynamic quantities have shown negative heats of adsorption for a wide variety of different mobile phase, stationary phase, and analyte. Additionally, there is a decrease in retention time as temperature rises; this occurs due to exothermic characteristic of adsorption as [1] also mentioned that in most of cases the compensation effect (also called enthalpy-entropy compensation) occurs. However, both enthalpy changes from Table 3 presented positive values indicating an endothermic phenomenon. Furthermore, the retention times in Figure 4 increase together as temperature rises. This aspect can be linked with a favorable entropy contribution. This indicates that when the analyte is bound to the stationary phase, the solvent molecules overload the adsorption site favoring the entropy increase.The selectivity from Table2 was also employed to analyze the separation between R-(−)-ibuprofen and S-(+)-ibuprofen. Parameters Δ
Δ
H and Δ
Δ
S were calculated by means of (5). The linearization proposal for this equation is presented in Figure 6.Figure 6
Linearization for determining ofΔ
Δ
H and Δ
Δ
S.The linearization ofln
⁡
(
α
) versus 1
/
T provided values of 1.55 kJ/mol and 6.52 J/(mol·K) for Δ
Δ
H and Δ
Δ
S, respectively, and it also presented a s-squared of 0.915. Error for Δ
Δ
H was 12% and error for Δ
Δ
S was 15%. Equation (7) provided 237.38 K for T
iso.Thermodynamic parameters are global information about the adsorption mechanism in a chromatographic column. The adsorption phenomenon involved in this process depends on solute type, mobile phase, and stationary phase [1]. For enantiomeric separation the adsorption mechanism is related to the chiral recognition. According to information from Figure 6, the adsorption is controlled by entropy (T
·
Δ
Δ
S
>
Δ
Δ
H) because entropy contribution is more relevant than enthalpy contribution for the ibuprofen retention mechanism in cellulose tris(3,5-dimethylphenylcarbamate).However, the separation will not be driven by entropy for all temperature ranges; this happens due toT
iso; it is a boundary temperature for driven forces in this case. This becomes evident when the conditions for T
iso are applied in Gibbs-Helmholtz equation and the result is zero for energy change (Δ
G). For this case, adsorption phenomenon at temperatures below T
iso, 237.38 K, will be driven by entropy; on the other hand, temperatures above T
iso will be driven by enthalpy. It is common that the adsorption phenomenon is exothermic and it occurs above T
iso [18, 20–23]. Probably the elution order of compounds could be inverted in temperature lower than T
iso. Moreover, the phenomenon would be controlled by enthalpy change, the selectivity would decrease as temperature rises, and the adsorption would be exothermic if ibuprofen were separated below T
iso [20, 22, 23].


## 3.1. Resolution Conditions and Elution Order

The resolution conditions were based on [16–18], at which cellulose tris(3,5-dimethylphenylcarbamate) is the chiral selector. Thus, it was decided to use a longer column (250 mm × 4.6 mm) packed with smaller particles (5 μm). Both parameters have contributed to increasing efficiency.Some mobile phases were tested to resolve the racemic mixture, but only the mobile phase based on hexane promoted satisfactory results. The mobile phase composed of hexane and isopropyl alcohol, in the proportion 99/1, was chosen for chiral resolution. Trifluoroacetic acid (TFA) was also used as an additive; its proportion on mobile phase was 0.1%, in volumetric base. All the conditions set for the chromatographic resolution provided values ofα and N
i above minimum levels required for effective chromatographic resolution (α > 1.20, R
S > 1.50, and N
i > 2000). Table 1 summarizes all the mentioned values [19].Table 1
Chromatographic parameters of racemic ibuprofen separation at 308.15 K: column (250 mm × 4.6 mm) packed with cellulose tris(3,5-dimethylphenylcarbamate).
Mobile phase
α
R
S
N
i
N
j
Hexane/isopropyl alcohol (99/1)
1.20
4.55
12976
12355After setting the separation conditions, the elution order was defined through a polarimetric technique. For this, the HPLC was used in batch mode to resolve the racemic mixture in R-ibuprofen and S-ibuprofen. The rotary evaporator reduced each sample for the polarimeter sample cell volume. A calibration curve provided the concentration of both samples: 0.4 g/L for S-ibuprofen and 1.11 g/L for R-ibuprofen. Finally, the polarimeter identified the less and more retained compounds as (−)-ibuprofen and (+)-ibuprofen, respectively. Thus, in Figure2, the first peak is R-(−)-ibuprofen while the second peak is S-(+)-ibuprofen.Figure 2
Chromatograms of ibuprofen enantiomeric resolution at 308.15 K and 0.5 g/mL and TTBB. Flow ratio: 1 mL/min; wavelength: 220 nm for ibuprofen and 254 nm for TTBB; mobile phase: hexane/isopropyl alcohol (99/1).


## 3.2. Total Porosity

Porosity was calculated from the first moment method (6). This method requires a tracer compound small enough to pass through both particle and bed voids. TTBB was used to determine the porosity of chiral columns packed with cellulose tris(3,5-dimethylphenylcarbamate). The flow rate was changed from 0.2 up to 1.6 mL/min with a 0.2 mL/min step. The results are shown in Figure 3.Figure 3
Total porosity.The slope presented in Figure3 provides the value of 0.647 for porosity.


## 3.3. Thermodynamic Parameters

The adsorption phenomenon of the enantiomeric compounds is macroscopic thermodynamic quantities, which does not consider the surface heterogeneity of the stationary phase and the associated distinct adsorption behavior of enantiomers at different sites. Under the circumstances, Van’t Hoff analysis is useful to determine global information about the phenomenon [1].Using (4), modified Van’t Hoff equation, one can obtain the thermodynamic parameters. The temperatures chosen were 288.15, 293.15, 298.15, 303.15, and 308.15 K. At each temperature, racemic ibuprofen samples were injected at 0.5 g/L. Figure 4 and Table 2 present a summary of chromatograms and chromatographic values obtained from these resolutions.Table 2
Retention factor obtained in racemic ibuprofen separation.
T (K)
k
i
k
j
α
288.15
4.72
5.43
1.15
293.15
4.88
5.68
1.16
298.15
5.11
5.96
1.17
303.15
5.38
6.37
1.18
308.15
5.74
6.90
1.20Figure 4
Chromatograms of the racemic ibuprofen at several temperatures. Flow rate: 1 mL/min.In Figure4, an increase in retention time value was observed as temperature rises. This behavior has been reported in literature; however, it is not the most common one [1]. This condition will be discussed later in this paper.The retention factors from Table2 were used to plot Figure 5. From this figure and utilizing (4), it was possible to obtain Δ
H and Δ
S, for ibuprofen enantiomers as presented in Table 3. The errors for enthalpy and entropy change were, respectively, 6% and 9%.Table 3
Thermodynamic parameters of racemic ibuprofen adsorbed on cellulose tris(3,5-dimethylphenylcarbamate).
Compound
Δ
H (kJ/mol)
Δ
S (kJ/K⋅mol)
R
2
R-(−)-ibuprofen
7.21
42.88
0.975
S-(+)-ibuprofen
8.76
49.40
0.972Figure 5
Van’t Hoff plots for the determination ofΔ
H and Δ
S.Both relations presented in Figure4 are linear, suggesting that multiple mechanisms of retention do not occur [19, 20]. Furthermore, Δ
H of compounds is lower than 50 kJ/mol demonstrating physical adsorption [11]. The interactions of physisorption are characterized by relatively weak bonds. Otherwise, it would be necessary to modify the chromatographic system to elute analytes.According to [1] the adsorption phenomenon in liquid chromatographic enantiomer resolution is driven by (mostly electrostatic type) noncovalent interactions. Thermodynamic quantities have shown negative heats of adsorption for a wide variety of different mobile phase, stationary phase, and analyte. Additionally, there is a decrease in retention time as temperature rises; this occurs due to exothermic characteristic of adsorption as [1] also mentioned that in most of cases the compensation effect (also called enthalpy-entropy compensation) occurs. However, both enthalpy changes from Table 3 presented positive values indicating an endothermic phenomenon. Furthermore, the retention times in Figure 4 increase together as temperature rises. This aspect can be linked with a favorable entropy contribution. This indicates that when the analyte is bound to the stationary phase, the solvent molecules overload the adsorption site favoring the entropy increase.The selectivity from Table2 was also employed to analyze the separation between R-(−)-ibuprofen and S-(+)-ibuprofen. Parameters Δ
Δ
H and Δ
Δ
S were calculated by means of (5). The linearization proposal for this equation is presented in Figure 6.Figure 6
Linearization for determining ofΔ
Δ
H and Δ
Δ
S.The linearization ofln
⁡
(
α
) versus 1
/
T provided values of 1.55 kJ/mol and 6.52 J/(mol·K) for Δ
Δ
H and Δ
Δ
S, respectively, and it also presented a s-squared of 0.915. Error for Δ
Δ
H was 12% and error for Δ
Δ
S was 15%. Equation (7) provided 237.38 K for T
iso.Thermodynamic parameters are global information about the adsorption mechanism in a chromatographic column. The adsorption phenomenon involved in this process depends on solute type, mobile phase, and stationary phase [1]. For enantiomeric separation the adsorption mechanism is related to the chiral recognition. According to information from Figure 6, the adsorption is controlled by entropy (T
·
Δ
Δ
S
>
Δ
Δ
H) because entropy contribution is more relevant than enthalpy contribution for the ibuprofen retention mechanism in cellulose tris(3,5-dimethylphenylcarbamate).However, the separation will not be driven by entropy for all temperature ranges; this happens due toT
iso; it is a boundary temperature for driven forces in this case. This becomes evident when the conditions for T
iso are applied in Gibbs-Helmholtz equation and the result is zero for energy change (Δ
G). For this case, adsorption phenomenon at temperatures below T
iso, 237.38 K, will be driven by entropy; on the other hand, temperatures above T
iso will be driven by enthalpy. It is common that the adsorption phenomenon is exothermic and it occurs above T
iso [18, 20–23]. Probably the elution order of compounds could be inverted in temperature lower than T
iso. Moreover, the phenomenon would be controlled by enthalpy change, the selectivity would decrease as temperature rises, and the adsorption would be exothermic if ibuprofen were separated below T
iso [20, 22, 23].


## 4. Conclusions

Racemic ibuprofen can be separated using a chiral stationary phase based on cellulose tris(3,5-dimethylphenylcarbamate) and a high nonpolar mobile phase. The mobile phase composed of hexane (99%) and isopropyl alcohol (1%) was chosen to separate the mixture. Trichloroacetic acid at 0.1% was employed as an additive; on this configuration of mobile phase and stationary phase, the S-(+)-ibuprofen is the most retained enantiomer.Thermodynamic parameters obtained from Figure4 demonstrated that the adsorption is physical and the separation phenomenon is endothermic. It shows that high temperatures favored the separation. Furthermore, the parameters from Figure 5 show that phenomenon of separation is controlled by entropy (T
·
Δ
Δ
S
>
Δ
Δ
H) at temperatures above T
iso.



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*Source: 7484731-2016-09-29.xml*