# Liquid Chromatography Study on Atenolol-β-Cyclodextrin Inclusion Complex

Authors: Shailesh M. Buha; Girin A. Baxi; Pranav S. Shrivastav
Journal: ISRN Analytical Chemistry
 (2012)

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## Abstract

Inclusion complex formation of atenolol withβ-cyclodextrin (β-CD) has been investigated by HPLC on different stationary phases, by varying pH and concentration of β-CD added as an additive in the mobile phase over a wide range of column temperature. Stationary phases of different polarity and hydrophobicity were evaluated to find the best conditions for complex formation. The optimum conditions for inclusion complexation were achieved on YMC ODS-AQ C18 (150×4.6 mm, 5 μ) analytical column. The apparent formation constant (K) of the complex as evaluated by liquid chromatography using retention factors (k) was 179.47±2.5 M−1 at 25°C. The stoichiometry of the complex was 1 : 1 as is evident from the straight line plot of 1/k versus β-CD concentration. The formation of inclusion complex was essentially enthalpy (−42.12 kJ/mol) driven and the binding forces included hydrophobic, van der Waals-London dispersion interactions. The enthalpy-entropy compensation criterion was used to prove the inclusion phenomena.


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## Body

## 1. Introduction

Beta-blockers are a class of antihypertensive drugs that are used in the management of cardiac arrhythmias, cardioprotection after myocardial infarction (heart attack), and hypertension. They have revolutionized the medical management of angina pectoris and are recommended as first-line agents by national and international guidelines. Atenolol, [4-(2-hydroxy-3-isopropylamino propoxy) phenyl acetamide] (see Figure1(a)) is a long established β-blocker widely used in the treatment of high blood pressure, arrhythmias, and angina pectoris [1]. Like other antihypertensive drugs, atenolol lowers the systolic and diastolic blood pressure by 15–20% in a single-drug treatment and reduces cardiovascular mortality [2]. The β-blockers are characterised by poor solubility in aqueous and gastric fluid, and therefore, the dissolution rate and their bioavailability directly affect their efficacy [3]. Consequently, in order to increase the solubility and dissolution rate of β-blockers, inclusion complex formation with cyclodextrins becomes imperative.Chemical structures of (a) atenolol and (b)β-cyclodextrin.
(a)(b)Cyclodextrins (CDs) are toroidal-shaped cyclic oligomers ofα-(l,4)-D-glucopyranose units which contribute to several guest-associated phenomena in solution [4]. CDs are oligoglycosides of six (α-CD), seven (β-CD), or eight (γ-CD) glucose units (see Figure 1(b)) forming a relatively hydrophobic cavity in the middle and a relatively hydrophilic exterior part [5]. CDs as host molecules can thus form inclusion complexes with various drug (guest) molecules and are utilized for the improvement of drug properties such as solubility, stability, and bioavailability [6, 7]. Though the exact mechanism of interaction is difficult to ascertain between CDs and the guest molecules, nevertheless it can be understood as a combination of geometrical compatibility, release of CD-ring strain upon complexation, van der Waals forces, hydrogen bonding, electrostatic, and hydrophobic interactions [5]. They are also optically active and offer potential discrimination of enantiomeric substances. These characteristics of CDs permit them to be employed as stationary phase in gas and liquid chromatography [8, 9], as chiral additives in HPLC [10–12] and in capillary electrophoresis (CE) [13, 14] for the separation of drug enantiomers. Generally in liquid chromatography, modest attention has been focused on the importance of temperature, especially using the chiral mobile phase additives for β-blockers. The major advantage in studying the effect of temperature is to determine the thermodynamic parameters for inclusion complexes and for understanding the mechanism and driving force of a wide variety of supramolecular interactions [15].Few studies have reported CD-based inclusion complex formation, or chiral separation ofβ-blockers [16–20]. Wei et al. [16] have studied chiral separation of atenolol, metoprolol, isoproterenol, salbutamol, and clenbuterol using electrophoresis with dual cyclodextrin systems. The chiral separation was strongly influenced by the concentration of the reaction mixture, pH, and organic modifier. Similarly, stereoselective recognition of several β-blockers by capillary zone electrophoresis with various CD derivatives like hydroxypropyl-β-CD, methylated-β-CD, sulphated-β-CD, and sulphated-α-CD has been studied by Gagyi et al. [17]. An HPLC and solubility study of the interaction between CDs and pindolol has been investigated by Gazpio et al. [18]. Ficarra and coworkers [19] have determined the stability constant of inclusion complex of atenolol with β-CD by phase solubility to be 28.33 M−1 at 25°C, employing the Higuchi-Connors equation. To the best of our knowledge, there is no report on the systematic study of retention mechanism of atenolol with β-CD by reversed phase liquid chromatography. The primary reason behind selection of atenolol from the β-blocker category is its well-established therapeutic importance in the field of medical science and the interest in healthcare industries towards this drug.The paper describes a reversed phase-HPLC approach to study the retention behaviour of atenolol-β-CD inclusion complex. The effect of temperature and pH of the mobile phase on the stability constant is evaluated and the impact of concentration of β-CD is discussed. Further, the modynamic parameters were calculated to elucidate the mechanism of inclusion complexation and retention.


## 2. Experimental

### 2.1. Chemicals and Solutions

β-Cyclodextrin (99.2%) and atenolol (99.5%) were obtained as a gift sample from Merck KGaA (Darmstadt, Germany) and Zydus Cadila Healthcare Ltd. (Ahmedabad, India), respectively. Standard stock solution of atenolol (1.0 mg/mL) was prepared in methanol and stored at 5°C. HPLC grade methanol, acetonitrile, and tetrahydrofuran were procured from Merck India Ltd. (Mumbai, India). Ultrapure water was obtained using Barnstead water purification system (Barnstead, IA, USA). AR grade sodium nitrate, sodium hydroxide, phosphoric acid, and sodium dihydrogen phosphate of purity ≥99% were purchased from S.D. Fine Chemicals Ltd. (Mumbai, India). All solutions analyzed were filtered through 0.45 μm mdi Nylon syringe filters from Advanced Microdevices Pvt. Ltd. (Ambala Cantt, India).


### 2.2. Equipment

The centrifuge tubes (1.5 mL capacity) were purchased from Tarson (Kolkata, India). Amber-coloured wide-opening HPLC vials, glass conical inserts with polymer feet and screw caps were purchased from Agilent (Waldbronn, Germany), while syringes were purchased from Becton Dickinson India Pvt. Ltd. (Haryana, India). Auto-pipettes were procured from Eppendorf (Hauppauge, NY, USA). Sonication was performed on Sonicator 8891 (Cole-Parmer, USA), while the vortexer-3020 was from Tarson (Kolkata, India). Weighing was done on Analytical balance Model AG245 from Mettler Toledo (Switzerland). pH measurements were carried out on Metrohm 780 pH meter (Herisau, Switzerland). Three YMC stainless steel HPLC columns, namely, ODS-AQ C18 and CN pack, were purchased from YMC India (Mumbai, India), while Kromasil C4 and NH2 columns were procured from Eka Chemicals (Akzo Nobel, Bohus, Sweden). High-performance liquid chromatography measurement was performed on Agilent 1200 series HPLC-DAD (Waldbronn, Germany), equipped with degasser G1320A, binary pump G1312B, HiP Auto-sampler SL G13676 with cooler and thermostat ASL unit G1330B and thermo column compartment TCC SL G1316B. The data were collected and processed on PC equipped with ChemStation software.


### 2.3. Chromatographic Condition

The chromatographic experiments were conducted on preequilibrated stainless steel YMC-ODS-AQ (150 × 4.6 mm, 5μ) column at different temperatures (15, 20, 25, 30, 35, and 40°C). The detection of atenolol was performed using ultraviolet detector at a wavelength maxima (λmax) of 226 nm. The mobile phase consisted of 50 mM sodium dihydrogen phosphate (NaH2PO4 and methanol (92 : 08, v/v), pH adjusted to 6.8 by addition of 5% NaOH with various concentration of β-CD (0, 2, 4, 6, 8, and 10 mM) in water. The mobile phase flow rate was maintained at 1.0 mL/min. The injection volume was kept at 2 μL and all the experiments at different temperature and β-CD concentration were done in triplicate. The dead time was obtained experimentally using sodium nitrate.


### 2.4. Determination of Apparent Formation Constants

The apparent formation constant (K) of atenolol can be determined by the equation [20](1)1k=1k0+K[β-CD]xk0,
where k is the atenolol retention factor in presence of β-CD, k0 is the retention factor in the absence of β-CD in the mobile phase, [β-CD] is the concentration of cyclodextrin, and x is the stoichiometry of the complex. The retention factors were monitored in presence of increasing concentration of β-CD. For an inclusion complex with 1 : 1 stoichiometry, the value of x is 1 and a plot of 1/k versus [β-CD] must be a straight line. The value of K is then computed from the slope of the linear plot.


### 2.5. Temperature Studies and Evaluation of Thermodynamic Parameters

The chromatographic system was equilibrated for at least 1 h prior to each experiment and the retention factors were determined at 15, 20, 25, 30, 35, and 40°C. The standard enthalpy (ΔH0) and entropy (ΔS0) values for the transfer of atenolol from the mobile phase to β-CD were calculated using the following thermodynamic relationship [21]:(2)ln⁡⁡K=-ΔH0RT+ΔS0T,
where T is the temperature and R the gas constant. The values of enthalpy (ΔH0) and entropy (ΔS0) were computed from the slope, ΔH0/T and intercept, ΔS0/R, respectively, form the van’t Hoff plot of lnK versus 1/T. The standard free energy (ΔG0) was calculated from the well-known equation(3)ΔG0=-RTln⁡⁡K.


## 2.1. Chemicals and Solutions

β-Cyclodextrin (99.2%) and atenolol (99.5%) were obtained as a gift sample from Merck KGaA (Darmstadt, Germany) and Zydus Cadila Healthcare Ltd. (Ahmedabad, India), respectively. Standard stock solution of atenolol (1.0 mg/mL) was prepared in methanol and stored at 5°C. HPLC grade methanol, acetonitrile, and tetrahydrofuran were procured from Merck India Ltd. (Mumbai, India). Ultrapure water was obtained using Barnstead water purification system (Barnstead, IA, USA). AR grade sodium nitrate, sodium hydroxide, phosphoric acid, and sodium dihydrogen phosphate of purity ≥99% were purchased from S.D. Fine Chemicals Ltd. (Mumbai, India). All solutions analyzed were filtered through 0.45 μm mdi Nylon syringe filters from Advanced Microdevices Pvt. Ltd. (Ambala Cantt, India).


## 2.2. Equipment

The centrifuge tubes (1.5 mL capacity) were purchased from Tarson (Kolkata, India). Amber-coloured wide-opening HPLC vials, glass conical inserts with polymer feet and screw caps were purchased from Agilent (Waldbronn, Germany), while syringes were purchased from Becton Dickinson India Pvt. Ltd. (Haryana, India). Auto-pipettes were procured from Eppendorf (Hauppauge, NY, USA). Sonication was performed on Sonicator 8891 (Cole-Parmer, USA), while the vortexer-3020 was from Tarson (Kolkata, India). Weighing was done on Analytical balance Model AG245 from Mettler Toledo (Switzerland). pH measurements were carried out on Metrohm 780 pH meter (Herisau, Switzerland). Three YMC stainless steel HPLC columns, namely, ODS-AQ C18 and CN pack, were purchased from YMC India (Mumbai, India), while Kromasil C4 and NH2 columns were procured from Eka Chemicals (Akzo Nobel, Bohus, Sweden). High-performance liquid chromatography measurement was performed on Agilent 1200 series HPLC-DAD (Waldbronn, Germany), equipped with degasser G1320A, binary pump G1312B, HiP Auto-sampler SL G13676 with cooler and thermostat ASL unit G1330B and thermo column compartment TCC SL G1316B. The data were collected and processed on PC equipped with ChemStation software.


## 2.3. Chromatographic Condition

The chromatographic experiments were conducted on preequilibrated stainless steel YMC-ODS-AQ (150 × 4.6 mm, 5μ) column at different temperatures (15, 20, 25, 30, 35, and 40°C). The detection of atenolol was performed using ultraviolet detector at a wavelength maxima (λmax) of 226 nm. The mobile phase consisted of 50 mM sodium dihydrogen phosphate (NaH2PO4 and methanol (92 : 08, v/v), pH adjusted to 6.8 by addition of 5% NaOH with various concentration of β-CD (0, 2, 4, 6, 8, and 10 mM) in water. The mobile phase flow rate was maintained at 1.0 mL/min. The injection volume was kept at 2 μL and all the experiments at different temperature and β-CD concentration were done in triplicate. The dead time was obtained experimentally using sodium nitrate.


## 2.4. Determination of Apparent Formation Constants

The apparent formation constant (K) of atenolol can be determined by the equation [20](1)1k=1k0+K[β-CD]xk0,
where k is the atenolol retention factor in presence of β-CD, k0 is the retention factor in the absence of β-CD in the mobile phase, [β-CD] is the concentration of cyclodextrin, and x is the stoichiometry of the complex. The retention factors were monitored in presence of increasing concentration of β-CD. For an inclusion complex with 1 : 1 stoichiometry, the value of x is 1 and a plot of 1/k versus [β-CD] must be a straight line. The value of K is then computed from the slope of the linear plot.


## 2.5. Temperature Studies and Evaluation of Thermodynamic Parameters

The chromatographic system was equilibrated for at least 1 h prior to each experiment and the retention factors were determined at 15, 20, 25, 30, 35, and 40°C. The standard enthalpy (ΔH0) and entropy (ΔS0) values for the transfer of atenolol from the mobile phase to β-CD were calculated using the following thermodynamic relationship [21]:(2)ln⁡⁡K=-ΔH0RT+ΔS0T,
where T is the temperature and R the gas constant. The values of enthalpy (ΔH0) and entropy (ΔS0) were computed from the slope, ΔH0/T and intercept, ΔS0/R, respectively, form the van’t Hoff plot of lnK versus 1/T. The standard free energy (ΔG0) was calculated from the well-known equation(3)ΔG0=-RTln⁡⁡K.


## 3. Results and Discussion

There can be two approaches for applying CDs in reversed phase HPLC (i) CDs can be chemically bonded to the stationary phase or (ii) can be used as an additive in the mobile phase. Based on the interaction (host-guest type) of analyte (guest) with CD, the retention time of the analyte will change; it will be shorter when complexation occurs in the mobile phase and longer when it takes place in the stationary phase [18]. These changes in the retention behaviour are closely related to the apparent formation constants of the complexes formed.


### 3.1. Optimization of Chromatographic Conditions

Initially, different columns, namely, Kromasil C4 (150 × 4.6 mm, 5μ), Kromasil NH2 (250 × 4.6 mm, 5 μ), YMC CN pack (250 × 4.6 mm, 5 μ), and YMC ODS-AQ C18 (150 × 4.6 mm, 5 μ), were screened to get adequate retention of atenolol in the absence of β-CD. The amino and cyano are polar bonded silica columns having lower hydrophobicity but higher polarity. Both these columns have been used in reversed phase separations for polar compounds. Cyano columns are less sterically restricted and have lower hydrogen-bond acidity. On the other hand Kromasil C4 and YMC ODS-AQ C18 are less polar and have higher hydrophobicity of 0.965 and 0.733, respectively, [20, 21]. The general properties and physical characteristics of the columns are presented in Table 1 [22, 23]. Several solvent systems were tested, which included buffer solutions like acetate and phosphate (pH 3.0–7.0) and commonly used organic solvents like acetonitrile, methanol, along with modifier like tetrahydrofuran (THF) in different compositions. Use of ethanol and 1-propanol was deliberately avoided as they have higher association constants of 0.93 M−1 and 3.71 M−1 with β-CD [24]. Further, the effect of injection volume and flow rate was also studied to have an efficient chromatography. In purely aqueous system, the retention time was very high (>30 min) and thus small volume fractions of organic solvents (6–20%) were tried in the mobile phase during method development. Conversely, in higher organic solvent fractions the retention time of atenolol was considerably reduced. This is due to the higher solvation effect which results in less interaction with the stationary phase [25]. A similar observation was also seen in presence of β-CD (10 mM) when the volume fraction of methanol was greater than 8% for all the columns. Figure 2 shows a significant decrease in retention factor of atenolol with increase in methanol component in the mobile phase. Higher content of methanol makes the mobile phase less polar and thus the affinity of atenolol towards the hydrophobic cavity of β-CD is diminished. Another phenomena which can also effect the inclusion process is the competition of methanol for binding β-CD, though it weakly binds to β-CD with an association constant of 0.32 M−1 [26].Table 1
Physical characteristics and general properties of HPLC columns studied.
ParameterYMC ODS-AQ C18Kromasil, C4YMC CN PackKromasil NH2Column length, mm150150250250Internal diameter, mm4.64.64.64.6Particle size,μ5555Pore size,Å´120120120120Surface area, m2/g330340330340Carbon content14871.9% N2pH range2.0–7.52.0–7.52.0–7.51.5–9.5Figure 2
Correlation between the retention factor (k) of atenolol and the volumetric fraction of methanol in the water-methanol mobile phase at a flow rate of 1.0 mL/min at 25°C on YMC ODS-AQ C18 column. (▴) 0 mM β-CD, (▪) 5 mM β-CD, (⚫) 10 mM β-CD.As it was expected to have further reduction in retention time in presence ofβ-CD in the mobile phase, the chromatographic conditions were suitably optimized to have adequate retention on these columns. The effect of mobile phase pH on different columns was also studied and the results are summarized in Table 2. Best chromatographic conditions were achieved in terms of peak shape, adequate response, and sufficient retention on YMC ODS-AQ column, using 0.05 mM NaH2PO4 in water and methanol (92 : 8, v/v) having pH 6.8 as the mobile phase. The effect of THF modifier in the mobile phase had little impact on the peak shape or retention time and hence was not taken in the optimized mobile phase. A flow rate of 1 mL/min gave acceptable peak shape and run time. The % CV in the measurement of retention time was ≤1.5 for 50 injections on the same column, indicating high reproducibility and stability of the chromatographic system. The retention time observed for atenolol on Kromasil C4, Kromasil NH2 and YMC CN pack, and YMC ODS-AQ columns was 13.5, 5.8, 10.6, and 22.8, respectively, using β-CD free mobile phase. By addition of β-CD (0–10 mM) in the mobile phase the retention time for atenolol decreased from 22.8 to 9.3, with a corresponding decrease in retention factor (k) from 11.62 to 4.16 on YMC ODS-AQ C18 column (Figure 3). The retention factors were calculated based on the dead time of 1.81 min on this column. This reduction was due to the formation of atenolol-β-CD inclusion complex, which enhances the solubility of atenolol in the mobile phase and thus reduces the residence time in the column. To confirm this, glucose which is a constituent of β-CD was added in the mobile phase (70 mM, equivalent to 10 mM β-CD); however, there was no change in the retention factor. This result is in agreement with the work reported by Clarot et al. [27]. Further, the number of theoretical plates (N) was reduced with increase in the concentration of β-CD in the mobile phase (Table 3). This signifies that the efficiency of atenolol to interact with the stationary phase decreases with increasing concentration of β-CD and this favours interaction of atenolol with the hydrophobic interior of β-CD cavity. At concentrations higher than 10 mM of β-CD, a considerable change in peak shapes was observed, probably due to aggregation of β-CD molecules in the mobile phase [28]. The retention factor (k) of atenolol on Kromasil C4 (5.92), Kromasil NH2 (1.07) and YMC CN pack (2.31) was too low under the optimum conditions of mobile phase composition and pH (Table 2). Due to further reduction in the retention time in presence of β-CD, they were not considered further in the present work.Table 2
Effect of pH on different columns and apparent formation constants of atenolol. Mobile phase: 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v). Wavelength: 226 nm. Flow rate: 1.0 mL/min. Temperature: 25°C.
Analytical columnRetention time, minRetention factor,kApparent formation constant,K (M−1)0 mMβ-CD10 mMβ-CD0 mMβ-CD10 mMβ-CDpH 3.0aKromasil, C48.46.33.332.2349.33bKromasil, NH23.23.10.140.0955.56cYMC-CN5.04.80.560.5012.00dYMC ODS-AQ C1812.86.56.072.59134.36pH 4.0aKromasil, C49.26.73.722.4452.46bKromasil, NH23.73.30.320.1877.78cYMC-CN6.15.60.910.7521.33dYMC ODS-AQ C1814.67.17.062.92141.78pH 5.0aKromasil, C411.67.55.182.8573.68bKromasil, NH24.93.90.750.3992.31cYMC-CN8.46.91.631.1640.52dYMC ODS-AQ C1817.87.88.833.31166.77pH 6.8aKromasil, C413.58.45.923.3278.31bKromasil, NH25.84.31.070.5298.15cYMC-CN10.68.02.311.5152.98dYMC ODS-AQ C1822.89.311.624.16179.47Dead time of the columns:a1.94 min, b2.80 min, c3.20 min, d1.81 min.All measurements were done in triplicate.Table 3
Variation in the retention factor (k) and number of theoretical plates with β-cyclodextrin concentration for atenolol. Mobile phase: 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v). Wavelength: 226 nm. Flow rate: 1.0 mL/min. Temperature: 25°C.
β-Cyclodextrin concentration (M × 10−3)Retention factor (k)Number of theoretical plates0.011.6235102.07.8133054.06.4927026.05.1322988.04.68180310.04.161597All measurements were done in triplicate.Figure 3
Effect ofβ-cyclodextrin concentration on the retention time of atenolol on YMC ODS-AQ C18 column using 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v) as the mobile phase at a flow rate of 1.0 mL/min at 25°C.


### 3.2. Apparent Formation Constant: Role of pH and Temperature

The retention of atenolol on YMC ODS-AQ C18 column is based on its partition between the mobile and the stationary phase; however, in presence ofβ-CD in the mobile phase the retention of atenolol is divided into two physicochemical processes: (i) complexation of atenolol by β-CD and (ii) the transfer of free atenolol from the mobile phase to the stationary phase. The plot of 1/k versus [β-CD] at 25°C was linear with regression coefficient “r” = 0.998. From the value of “r” it is evident that the inclusion complex has 1 : 1 stoichiometry. With an increase in β-CD concentration there was a corresponding decrease in retention factors for atenolol (Table 3). This is in agreement with two previous reports which have studied inclusion complexation between atenolol and β-CD [19, 29]. The K value of 179.47±2.1 M−1 obtained by the chromatographic experiment is considerably higher compared to that obtained by phase solubility study (28.66 M−1) for atenolol at 25°C [19]. It is not unusual to find this huge difference in the apparent stability constants using two different techniques [30]. Phase solubility studies are conducted at a much higher concentration levels as compared to chromatographic conditions, thus it is not significant to compare the results obtained in the present work. As is evident from Table 2, pH plays a significant role in atenolol-β-CD inclusion complex formation. The formation of inclusion complex is related to the hydrophobic nature of the drug. The pKa of atenolol at 25°C is 9.6 and it remains in an unionized form at this pH, while under acidic pH the amino group is protonated and this has negative influence in the complex formation as β-CD has a nonpolar cavity, resulting in a lower value of apparent formation constant. The K value of 179.47 M−1 at pH 6.8 could have further increased in the alkaline pH due to the basic nature of atenolol. However, in the alkaline pH range the silica-based stationary phase tends to hydrolyse, which can affect the column efficiency and hence was not studied in the present work. The formation constants evaluated at pH 3.0, 4.0, and 5.0 were 134.36, 141.78, and 166.76 M−1, respectively. This experiment indicates that pH of the mobile phase was more important in retention mechanism and therefore in the inclusion process. The probable inclusion phenomena can be explained by the hydrophobic effect of the phenyl ring which would be inside the hydrophobic cavity of β-CD. The apparent formation constant values obtained for all four columns at different pH are also summarized in Table 2. The values obtained for apparent formation constants (K) at different temperatures are presented in Table 4. Inclusion complexes are generally less stable at higher temperature as reported previously [31]. At lower temperature the retention decreases with higher degree of complexation. Consequently, the concentration of free atenolol that can be adsorbed on the stationary phase is reduced.Table 4
Apparent formation constant (K) of atenolol and thermodynamic parameters at different temperatures in presence of β-CD. Column: YMC ODS-AQ C18 (150 × 4.6 mm, 5 μ). Mobile phase: 10 mM β-CD in 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v). Wavelength: 226 nm. Flow rate: 1.0 mL/min.
Temperature, KApparent formation constant,K (M−1)ΔG0  (kJ/mol)ΔH0 (kJ/mol)ΔS0  (kJ/K/mol)TΔS0 (kJ/mol)288324.44−13.85———293239.85−13.35−42.40−0.0933−29.05298179.47−12.86−42.12−0.0982−29.26303135.64−12.37−42.05−0.0979−29.68308103.54−11.88−41.92−0.0975−30.0431379.84−11.40−41.68−0.0967−30.28All measurements were done in triplicate.


### 3.3. Thermodynamic Parameters for Atenolol-β-CD Inclusion Complex Formation

Determination of thermodynamic parameters is indispensable in understanding the process of molecular recognition. To understand the mechanism of interaction of atenolol withβ-CD (10 mM), the thermodynamic parameters were evaluated from the van’t Hoff plots. The plot of lnK versus 1/Twas linear with correlation coefficient “r” greater than 0.9985 (Figure 4). The enthalpy and entropy values calculated from the slope and intercept were −42.12 kJ/mol and −29.26 J/mol/K, respectively, at 25°C (Table 4). The negative value for enthalpy indicates that the association between atenolol and β-CD is exothermic. This value is typical of interactions such as hydrophobic interactions as a result of displacement of water molecules from the cavity of β-CD, van der Waals interactions, formation of hydrogen bonds, and others [32]. The negative value of entropy can be related to a more ordered system due to decrease in translational and rotational degrees of freedom of the complexed species as compared to the free molecules. It is interesting to see that the magnitude of ΔH0 is greater than TΔS0 over the temperature range studied (Table 4). This further indicated that enthalpy played a greater role in complexation than entropy. The Gibbs free energy change (ΔG0) for atenolol-β-CD inclusion complex at 25°C was −12.86 kJ/mol, indicating that the inclusion process is a spontaneous one.Figure 4
Van’t Hoff plot (lnK versus 1/T) for atenolol on YMC ODS-AQ C18 column in presence of 10 mM β-CD using 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v) as the mobile phase at a flow rate of 1.0 mL/min.


### 3.4. Thermodynamic Parameters for Transfer of Atenolol from Mobile Phase to the Stationary Phase

A linear relationship (r=0.998) was observed between 1/k and the absolute temperature in the absence of β-CD. This linear relationship suggests minimum conformational changes and that the retention mechanism is the same over the temperature range investigated. Zarzycki and Lamparczyk [33] have described an excellent linear relationship observed during the unmodified mobile phase with series of naphthalene derivatives. As evident from the values in Table 5 the magnitude of ΔH0 was higher than TΔS0 which can be attributed to favourable transfer of atenolol from the mobile phase to the stationary phase and is enthalpy driven. The negative ΔS0 value suggests greater immobilization effect after the transfer and ordering of the chromatographic system. When atenolol was transferred from the mobile to the stationary phase, the solute-solvent interactions were replaced by van der Waals interactions, leading to negative enthalpy change. The retention mechanism of atenolol involved classical transfer of solute from mobile phase to stationary phase. The retention factor decreased with increase in temperature along with corresponding increase in free energy change from −6.42 to −5.57 kJ/mol for atenolol-stationary phase interaction.Table 5
Retention factors of atenolol and thermodynamic parameters at different temperatures in absence ofβ-CD. Column: YMC ODS-AQ C18 (150 × 4.6 mm, 5 μ). Mobile phase: 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v). Wavelength: 226 nm. Flow rate: 1.0 mL/min.
Temperature, KRetention factor,kΔG0   (kJ/mol)ΔH0 (kJ/mol)ΔS0  (kJ/K/mol)TΔS0  (kJ/mol)28814.62−6.42———29313.00−6.25−16.48−0.0349−10.2329811.62−6.08−16.35−0.0350−10.2730310.43−5.91−16.23−0.0341−10.323089.40−5.74−16.14−0.0337−10.403138.51−5.57−16.04−0.0334−10.47All measurements were done in triplicate.


### 3.5. Enthalpy and Entropy Compensation for the Inclusion Complex

The enthalpy-entropy compensation can work as a tool in understanding molecular recognition between the analyte andβ-CD [34]. The plots of TΔS0 versus ΔH0 show that both the parameters are linearly correlated in absence and presence of β-CD in Figures 5(a) and 5(b), respectively. The slope (α) of this linear plot indicates the extent to which the enthalpic gain is cancelled by the accompanying loss in entropy, which are affected when there is any interaction between atenolol and β-CD. Thus, only a fraction (1−α) of the enthalpic gain can contribute to the enhancement of complex stability. The intercept represents the inherent complex stability obtained at ΔH0 = 0, which means that the complex is stabilized even in the absence of enthalpic gain when TΔS0 term is positive. The slope (α) and the intercept TΔS0 of the regression equation can be related to the degree of conformational change and to the extent of desolvation upon complexation, respectively, [35]. The lower the value of the slope, the less will be the conformational change on account of complexation. Similarly, the higher the value of the intercept the greater is the desolvation, which favours complexation. The value of slope from TΔS0 versus ΔH0 plots changed from −0.55 in absence of β-CD (Figure 5(a)) to −1.71 in presence of β-CD (Figure 5(b)). This change in magnitude of the slope indicates that the drug may be partially inside the β-CD cavity. The NMR studies have also shown a chemical shift of δ 0.131–0.148 for phenyl protons upon complexation [29]. By extrapolating, the intercept at ΔH0 = 0 in presence of β-CD was −98.1 and was higher in magnitude compared to −19.43 in the absence of β-CD. This implies higher desolvation of atenolol on account of inclusion complex formation. Further, as is evident from the enthalpy and free energy values at different temperatures in Tables 4 and 5, atenolol-β-CD interaction is more favourable as compared to atenolol-stationary phase interaction.Enthalpy-entropy compensation plot (TΔS0 versus ΔH0) for atenolol in (a) absence and (b) presence of β-cyclodextrin on YMC ODS-AQ C18 column using 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v) as the mobile phase at a flow rate of 1.0 mL/min.
(a)(b)


## 3.1. Optimization of Chromatographic Conditions

Initially, different columns, namely, Kromasil C4 (150 × 4.6 mm, 5μ), Kromasil NH2 (250 × 4.6 mm, 5 μ), YMC CN pack (250 × 4.6 mm, 5 μ), and YMC ODS-AQ C18 (150 × 4.6 mm, 5 μ), were screened to get adequate retention of atenolol in the absence of β-CD. The amino and cyano are polar bonded silica columns having lower hydrophobicity but higher polarity. Both these columns have been used in reversed phase separations for polar compounds. Cyano columns are less sterically restricted and have lower hydrogen-bond acidity. On the other hand Kromasil C4 and YMC ODS-AQ C18 are less polar and have higher hydrophobicity of 0.965 and 0.733, respectively, [20, 21]. The general properties and physical characteristics of the columns are presented in Table 1 [22, 23]. Several solvent systems were tested, which included buffer solutions like acetate and phosphate (pH 3.0–7.0) and commonly used organic solvents like acetonitrile, methanol, along with modifier like tetrahydrofuran (THF) in different compositions. Use of ethanol and 1-propanol was deliberately avoided as they have higher association constants of 0.93 M−1 and 3.71 M−1 with β-CD [24]. Further, the effect of injection volume and flow rate was also studied to have an efficient chromatography. In purely aqueous system, the retention time was very high (>30 min) and thus small volume fractions of organic solvents (6–20%) were tried in the mobile phase during method development. Conversely, in higher organic solvent fractions the retention time of atenolol was considerably reduced. This is due to the higher solvation effect which results in less interaction with the stationary phase [25]. A similar observation was also seen in presence of β-CD (10 mM) when the volume fraction of methanol was greater than 8% for all the columns. Figure 2 shows a significant decrease in retention factor of atenolol with increase in methanol component in the mobile phase. Higher content of methanol makes the mobile phase less polar and thus the affinity of atenolol towards the hydrophobic cavity of β-CD is diminished. Another phenomena which can also effect the inclusion process is the competition of methanol for binding β-CD, though it weakly binds to β-CD with an association constant of 0.32 M−1 [26].Table 1
Physical characteristics and general properties of HPLC columns studied.
ParameterYMC ODS-AQ C18Kromasil, C4YMC CN PackKromasil NH2Column length, mm150150250250Internal diameter, mm4.64.64.64.6Particle size,μ5555Pore size,Å´120120120120Surface area, m2/g330340330340Carbon content14871.9% N2pH range2.0–7.52.0–7.52.0–7.51.5–9.5Figure 2
Correlation between the retention factor (k) of atenolol and the volumetric fraction of methanol in the water-methanol mobile phase at a flow rate of 1.0 mL/min at 25°C on YMC ODS-AQ C18 column. (▴) 0 mM β-CD, (▪) 5 mM β-CD, (⚫) 10 mM β-CD.As it was expected to have further reduction in retention time in presence ofβ-CD in the mobile phase, the chromatographic conditions were suitably optimized to have adequate retention on these columns. The effect of mobile phase pH on different columns was also studied and the results are summarized in Table 2. Best chromatographic conditions were achieved in terms of peak shape, adequate response, and sufficient retention on YMC ODS-AQ column, using 0.05 mM NaH2PO4 in water and methanol (92 : 8, v/v) having pH 6.8 as the mobile phase. The effect of THF modifier in the mobile phase had little impact on the peak shape or retention time and hence was not taken in the optimized mobile phase. A flow rate of 1 mL/min gave acceptable peak shape and run time. The % CV in the measurement of retention time was ≤1.5 for 50 injections on the same column, indicating high reproducibility and stability of the chromatographic system. The retention time observed for atenolol on Kromasil C4, Kromasil NH2 and YMC CN pack, and YMC ODS-AQ columns was 13.5, 5.8, 10.6, and 22.8, respectively, using β-CD free mobile phase. By addition of β-CD (0–10 mM) in the mobile phase the retention time for atenolol decreased from 22.8 to 9.3, with a corresponding decrease in retention factor (k) from 11.62 to 4.16 on YMC ODS-AQ C18 column (Figure 3). The retention factors were calculated based on the dead time of 1.81 min on this column. This reduction was due to the formation of atenolol-β-CD inclusion complex, which enhances the solubility of atenolol in the mobile phase and thus reduces the residence time in the column. To confirm this, glucose which is a constituent of β-CD was added in the mobile phase (70 mM, equivalent to 10 mM β-CD); however, there was no change in the retention factor. This result is in agreement with the work reported by Clarot et al. [27]. Further, the number of theoretical plates (N) was reduced with increase in the concentration of β-CD in the mobile phase (Table 3). This signifies that the efficiency of atenolol to interact with the stationary phase decreases with increasing concentration of β-CD and this favours interaction of atenolol with the hydrophobic interior of β-CD cavity. At concentrations higher than 10 mM of β-CD, a considerable change in peak shapes was observed, probably due to aggregation of β-CD molecules in the mobile phase [28]. The retention factor (k) of atenolol on Kromasil C4 (5.92), Kromasil NH2 (1.07) and YMC CN pack (2.31) was too low under the optimum conditions of mobile phase composition and pH (Table 2). Due to further reduction in the retention time in presence of β-CD, they were not considered further in the present work.Table 2
Effect of pH on different columns and apparent formation constants of atenolol. Mobile phase: 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v). Wavelength: 226 nm. Flow rate: 1.0 mL/min. Temperature: 25°C.
Analytical columnRetention time, minRetention factor,kApparent formation constant,K (M−1)0 mMβ-CD10 mMβ-CD0 mMβ-CD10 mMβ-CDpH 3.0aKromasil, C48.46.33.332.2349.33bKromasil, NH23.23.10.140.0955.56cYMC-CN5.04.80.560.5012.00dYMC ODS-AQ C1812.86.56.072.59134.36pH 4.0aKromasil, C49.26.73.722.4452.46bKromasil, NH23.73.30.320.1877.78cYMC-CN6.15.60.910.7521.33dYMC ODS-AQ C1814.67.17.062.92141.78pH 5.0aKromasil, C411.67.55.182.8573.68bKromasil, NH24.93.90.750.3992.31cYMC-CN8.46.91.631.1640.52dYMC ODS-AQ C1817.87.88.833.31166.77pH 6.8aKromasil, C413.58.45.923.3278.31bKromasil, NH25.84.31.070.5298.15cYMC-CN10.68.02.311.5152.98dYMC ODS-AQ C1822.89.311.624.16179.47Dead time of the columns:a1.94 min, b2.80 min, c3.20 min, d1.81 min.All measurements were done in triplicate.Table 3
Variation in the retention factor (k) and number of theoretical plates with β-cyclodextrin concentration for atenolol. Mobile phase: 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v). Wavelength: 226 nm. Flow rate: 1.0 mL/min. Temperature: 25°C.
β-Cyclodextrin concentration (M × 10−3)Retention factor (k)Number of theoretical plates0.011.6235102.07.8133054.06.4927026.05.1322988.04.68180310.04.161597All measurements were done in triplicate.Figure 3
Effect ofβ-cyclodextrin concentration on the retention time of atenolol on YMC ODS-AQ C18 column using 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v) as the mobile phase at a flow rate of 1.0 mL/min at 25°C.


## 3.2. Apparent Formation Constant: Role of pH and Temperature

The retention of atenolol on YMC ODS-AQ C18 column is based on its partition between the mobile and the stationary phase; however, in presence ofβ-CD in the mobile phase the retention of atenolol is divided into two physicochemical processes: (i) complexation of atenolol by β-CD and (ii) the transfer of free atenolol from the mobile phase to the stationary phase. The plot of 1/k versus [β-CD] at 25°C was linear with regression coefficient “r” = 0.998. From the value of “r” it is evident that the inclusion complex has 1 : 1 stoichiometry. With an increase in β-CD concentration there was a corresponding decrease in retention factors for atenolol (Table 3). This is in agreement with two previous reports which have studied inclusion complexation between atenolol and β-CD [19, 29]. The K value of 179.47±2.1 M−1 obtained by the chromatographic experiment is considerably higher compared to that obtained by phase solubility study (28.66 M−1) for atenolol at 25°C [19]. It is not unusual to find this huge difference in the apparent stability constants using two different techniques [30]. Phase solubility studies are conducted at a much higher concentration levels as compared to chromatographic conditions, thus it is not significant to compare the results obtained in the present work. As is evident from Table 2, pH plays a significant role in atenolol-β-CD inclusion complex formation. The formation of inclusion complex is related to the hydrophobic nature of the drug. The pKa of atenolol at 25°C is 9.6 and it remains in an unionized form at this pH, while under acidic pH the amino group is protonated and this has negative influence in the complex formation as β-CD has a nonpolar cavity, resulting in a lower value of apparent formation constant. The K value of 179.47 M−1 at pH 6.8 could have further increased in the alkaline pH due to the basic nature of atenolol. However, in the alkaline pH range the silica-based stationary phase tends to hydrolyse, which can affect the column efficiency and hence was not studied in the present work. The formation constants evaluated at pH 3.0, 4.0, and 5.0 were 134.36, 141.78, and 166.76 M−1, respectively. This experiment indicates that pH of the mobile phase was more important in retention mechanism and therefore in the inclusion process. The probable inclusion phenomena can be explained by the hydrophobic effect of the phenyl ring which would be inside the hydrophobic cavity of β-CD. The apparent formation constant values obtained for all four columns at different pH are also summarized in Table 2. The values obtained for apparent formation constants (K) at different temperatures are presented in Table 4. Inclusion complexes are generally less stable at higher temperature as reported previously [31]. At lower temperature the retention decreases with higher degree of complexation. Consequently, the concentration of free atenolol that can be adsorbed on the stationary phase is reduced.Table 4
Apparent formation constant (K) of atenolol and thermodynamic parameters at different temperatures in presence of β-CD. Column: YMC ODS-AQ C18 (150 × 4.6 mm, 5 μ). Mobile phase: 10 mM β-CD in 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v). Wavelength: 226 nm. Flow rate: 1.0 mL/min.
Temperature, KApparent formation constant,K (M−1)ΔG0  (kJ/mol)ΔH0 (kJ/mol)ΔS0  (kJ/K/mol)TΔS0 (kJ/mol)288324.44−13.85———293239.85−13.35−42.40−0.0933−29.05298179.47−12.86−42.12−0.0982−29.26303135.64−12.37−42.05−0.0979−29.68308103.54−11.88−41.92−0.0975−30.0431379.84−11.40−41.68−0.0967−30.28All measurements were done in triplicate.


## 3.3. Thermodynamic Parameters for Atenolol-β-CD Inclusion Complex Formation

Determination of thermodynamic parameters is indispensable in understanding the process of molecular recognition. To understand the mechanism of interaction of atenolol withβ-CD (10 mM), the thermodynamic parameters were evaluated from the van’t Hoff plots. The plot of lnK versus 1/Twas linear with correlation coefficient “r” greater than 0.9985 (Figure 4). The enthalpy and entropy values calculated from the slope and intercept were −42.12 kJ/mol and −29.26 J/mol/K, respectively, at 25°C (Table 4). The negative value for enthalpy indicates that the association between atenolol and β-CD is exothermic. This value is typical of interactions such as hydrophobic interactions as a result of displacement of water molecules from the cavity of β-CD, van der Waals interactions, formation of hydrogen bonds, and others [32]. The negative value of entropy can be related to a more ordered system due to decrease in translational and rotational degrees of freedom of the complexed species as compared to the free molecules. It is interesting to see that the magnitude of ΔH0 is greater than TΔS0 over the temperature range studied (Table 4). This further indicated that enthalpy played a greater role in complexation than entropy. The Gibbs free energy change (ΔG0) for atenolol-β-CD inclusion complex at 25°C was −12.86 kJ/mol, indicating that the inclusion process is a spontaneous one.Figure 4
Van’t Hoff plot (lnK versus 1/T) for atenolol on YMC ODS-AQ C18 column in presence of 10 mM β-CD using 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v) as the mobile phase at a flow rate of 1.0 mL/min.


## 3.4. Thermodynamic Parameters for Transfer of Atenolol from Mobile Phase to the Stationary Phase

A linear relationship (r=0.998) was observed between 1/k and the absolute temperature in the absence of β-CD. This linear relationship suggests minimum conformational changes and that the retention mechanism is the same over the temperature range investigated. Zarzycki and Lamparczyk [33] have described an excellent linear relationship observed during the unmodified mobile phase with series of naphthalene derivatives. As evident from the values in Table 5 the magnitude of ΔH0 was higher than TΔS0 which can be attributed to favourable transfer of atenolol from the mobile phase to the stationary phase and is enthalpy driven. The negative ΔS0 value suggests greater immobilization effect after the transfer and ordering of the chromatographic system. When atenolol was transferred from the mobile to the stationary phase, the solute-solvent interactions were replaced by van der Waals interactions, leading to negative enthalpy change. The retention mechanism of atenolol involved classical transfer of solute from mobile phase to stationary phase. The retention factor decreased with increase in temperature along with corresponding increase in free energy change from −6.42 to −5.57 kJ/mol for atenolol-stationary phase interaction.Table 5
Retention factors of atenolol and thermodynamic parameters at different temperatures in absence ofβ-CD. Column: YMC ODS-AQ C18 (150 × 4.6 mm, 5 μ). Mobile phase: 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v). Wavelength: 226 nm. Flow rate: 1.0 mL/min.
Temperature, KRetention factor,kΔG0   (kJ/mol)ΔH0 (kJ/mol)ΔS0  (kJ/K/mol)TΔS0  (kJ/mol)28814.62−6.42———29313.00−6.25−16.48−0.0349−10.2329811.62−6.08−16.35−0.0350−10.2730310.43−5.91−16.23−0.0341−10.323089.40−5.74−16.14−0.0337−10.403138.51−5.57−16.04−0.0334−10.47All measurements were done in triplicate.


## 3.5. Enthalpy and Entropy Compensation for the Inclusion Complex

The enthalpy-entropy compensation can work as a tool in understanding molecular recognition between the analyte andβ-CD [34]. The plots of TΔS0 versus ΔH0 show that both the parameters are linearly correlated in absence and presence of β-CD in Figures 5(a) and 5(b), respectively. The slope (α) of this linear plot indicates the extent to which the enthalpic gain is cancelled by the accompanying loss in entropy, which are affected when there is any interaction between atenolol and β-CD. Thus, only a fraction (1−α) of the enthalpic gain can contribute to the enhancement of complex stability. The intercept represents the inherent complex stability obtained at ΔH0 = 0, which means that the complex is stabilized even in the absence of enthalpic gain when TΔS0 term is positive. The slope (α) and the intercept TΔS0 of the regression equation can be related to the degree of conformational change and to the extent of desolvation upon complexation, respectively, [35]. The lower the value of the slope, the less will be the conformational change on account of complexation. Similarly, the higher the value of the intercept the greater is the desolvation, which favours complexation. The value of slope from TΔS0 versus ΔH0 plots changed from −0.55 in absence of β-CD (Figure 5(a)) to −1.71 in presence of β-CD (Figure 5(b)). This change in magnitude of the slope indicates that the drug may be partially inside the β-CD cavity. The NMR studies have also shown a chemical shift of δ 0.131–0.148 for phenyl protons upon complexation [29]. By extrapolating, the intercept at ΔH0 = 0 in presence of β-CD was −98.1 and was higher in magnitude compared to −19.43 in the absence of β-CD. This implies higher desolvation of atenolol on account of inclusion complex formation. Further, as is evident from the enthalpy and free energy values at different temperatures in Tables 4 and 5, atenolol-β-CD interaction is more favourable as compared to atenolol-stationary phase interaction.Enthalpy-entropy compensation plot (TΔS0 versus ΔH0) for atenolol in (a) absence and (b) presence of β-cyclodextrin on YMC ODS-AQ C18 column using 50 mM NaH2PO4, pH—6.8: methanol (92 : 8, v/v) as the mobile phase at a flow rate of 1.0 mL/min.
(a)(b)


## 4. Conclusion

The mechanism of retention in RP-HPLC and inclusion complex formation of atenolol withβ-CD has been studied. The dependence of inclusion complex on pH and temperature was investigated and trends in thermodynamics parameters were determined over a wide range of column temperature. The variation observed can be explained in terms of two main physicochemical processes, solute inclusion in the β-CD in cavity and solute transfer from the mobile phase to stationary phase. It is evident from the apparent formation constants that the extent to which the inclusion complexation is favoured depends not only on the polarity and structure of the guest but also on the composition and pH of the mobile phase. The thermodynamic data proves the formation of atenolol-β-CD inclusion complex and that the process is essentially enthalpy driven. Further, the enthalpy-entropy compensation data supports the phenomena of molecular inclusion of atenolol in β-CD.



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*Source: 423572-2012-03-01.xml*