# Ball Milling to Build the Hybrid Mesocrystals of Ibuprofen and Aragonite

Authors: Kyoung A Cho; Insil Choi; Il Won Kim
Journal: Journal of Nanomaterials
 (2015)

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## Abstract

Mesocrystal formation is one of the new paradigms of the nonclassical crystallization, where the assembly of crystal domains is observed. Also, it has been recently employed in studies on drug formulation to utilize controlled dissolution of the drug domains. In this report, ibuprofen was attempted to form hybrid mesocrystals with calcium carbonate crystals. Two polymorphs of calcium carbonate (aragonite and calcite) were used during the solid-state process of ball milling. Structural analyses confirmed the mesocrystal formation of ibuprofen with aragonite but not with calcite. The origin of the observed behavior was found from the higher affinity of ibuprofen to aragonite, especially its (0 1 0) surface, compared to calcite. The hybrid mesocrystals of ibuprofen and aragonite showed the environment-responsive release behavior, where the stability of aragonite was the controlling factor for the release kinetics of ibuprofen.


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## Body

## 1. Introduction

Mesocrystals are increasingly found as the products of nonclassical crystallization in the diverse fields of materials [1]. The examples are especially abundant in biological and bioinspired crystallization. For example, the nacre of red abalone is constructed as the layers of microcrystals that are also the assembled structures of nanocrystals [2, 3]. Similar findings have been seen in the nacre of giant oyster, the spicules of calcareous sponges, and the skeletal structure of sea urchins [4–6] In addition, synthetic mesocrystals inspired by biomineralization have been reported in the solution crystallization, where the crystal assembly was through interparticle interactions and/or heterogeneous nucleation [7–10].Controlled release has attracted great interest in the pharmaceutical research. The basic notion is to maintain the drug concentration in blood above the effective level and below the safe concentration for a sustained period of time, and many efforts have been made at the same time to develop environment-responsive systems that satisfy the specific needs of the drugs [11]. Mesocrystals have been also explored in this regard to control the dissolution rate of the active pharmaceutical ingredients (APIs). For example, the sustained release of carbamazepine and adefovir dipivoxil was associated with their mesocrystal formation induced by polymeric additives [12, 13]; the enhanced release of ibuprofen was found for its mesocrystals formed with sodium dodecyl sulfate [14].Mechanical milling was utilized to prepare hybrid structures of APIs with inorganic materials, such as silica, magnesium aluminosilicate, aluminum silicate, and aluminum hydroxide, to alter the physicochemical properties of the APIs [15–18]. It has been also extensively explored in recent years to prepare cocrystals and solvates/hydrates of APIs, and the solid-state process without or minimal use of solvents makes it attractive as a greener process than conventional procedures [19–22].In the present study, we have attempted a simple method of ball milling to prepare hybrid mesocrystals of ibuprofen (IBU) and calcium carbonate. We explored two anhydrous polymorphs of calcium carbonate (calcite and aragonite) since the distinctive molecular arrangements of the active surfaces could contribute to the different interactions with IBU. Also, the pH-responsive dissolution behaviors of the mesocrystals were expected because of the high and sparing solubility of calcium carbonate at low and neutral pH, respectively [23].


## 2. Materials and Methods

### 2.1. Preparation of Calcite and Aragonite

Two polymorphs of anhydrous calcium carbonate were prepared following a method using water-alcohol mixtures [24]. To obtain calcite, sodium carbonate (26.0 mmol, 2.75 g: Na2CO3: ≥99.0%, Sigma-Aldrich, Milwaukee, WI, USA) was completely dissolved in the solution of 100 mL ethanol (HPLC grade, 99.0%, Samchun, Pyeongtaek, South Korea) and 900 mL deionized water (DI water: resistivity of 18.2 MOhm·cm, Direct-Q from Millipore, Billerica, MA, USA) contained in a 1000 mL volumetric flask at room temperature (ca. 25°C), and then calcium chloride (26.0 mmol, 2.89 g: CaCl2: 99+%, Sigma-Aldrich, Milwaukee, WI, USA) was added to the solution. The solution was vigorously mixed at all time with a stir bar (length, 30 mm) equipped with a magnetic stirrer (HS180, Misung Scientific Co., Seoul, South Korea). The procedure to obtain aragonite was the same as that for calcite except that 50 vol% ethanol (500 mL ethanol and 500 mL DI water) was used. After 24 h, the precipitated products were collected by vacuum filtration (number 20 filter paper, pore diameter 5 μm, Hyundai Micro, Seoul, South Korea), washed with DI water, and dried in a convection oven at 40°C for 12 h before further use.


### 2.2. Ball Milling IBU with Calcite and Aragonite

Ibuprofen (IBU: >98%) was used as obtained from Sigma-Aldrich (Milwaukee, WI, USA). IBU (100 mg) was ball-milled with calcite or aragonite (100 mg) at the frequency of 10 Hz, and the milling time was 120 or 240 min. For the procedure, a Retsch ball mill (MM 200, Haan, Germany) was used with a cylindrical stainless steel jar (about 25 mL; inner diameter ca. 26 mm and inner length ca. 52 mm) and two stainless steel balls (diameter, 9 mm), which was often utilized in pharmaceutical grinding [20]. The ball-milled products were immediately used for further characterization.


### 2.3. Characterization of Raw and Ball-Milled Materials

Morphologies of IBU, calcite, aragonite, and ball-milled products were characterized using field-emission scanning electron microscopy (FE-SEM: JSM-6700F, JEOL, Tokyo, Japan) after thin Au coating (Cressington Sputter Coater 108, Watford, UK) to minimize surface charging. The materials were also characterized in their crystal structures using powder X-ray diffraction (XRD: D2 PHASER, Bruker AXS, Billerica, MA, USA). XRD was performed with CuKα radiation (λ = 1.5406 Å at 30 kV, 10 mA) in the 2θ range of 5–40° (scanning rate, 1°/min). Fourier transformation infrared spectroscopy (FT-IR) was performed using a Cary 660 FTIR Spectrometer (Agilent Technologies, Santa Clara, CA, USA). KBr (FT-IR grade, ≥99%, Sigma-Aldrich, Milwaukee, WI, USA) discs were prepared for the transmission mode, where the IR spectra were collected in the wavenumber range of 4000–400 cm−1.Thermal analyses were performed via differential scanning calorimetry (DSC: DSC 821e, Mettler-Toledo, Columbus, OH, USA) and thermogravimetric analysis (TGA: TGA/SDTA 851e, Mettler-Toledo). DSC was to check the crystalline state of IBU, and it was precalibrated for enthalpy and temperature using indium. The scanning for the IBU containing samples (2-3 mg each in a hermetically sealed aluminum crucible) was from 25 to 100°C with a heating rate of 10°C/min, and DSC experiments were repeated in triplicate for each sample. TGA was performed from 25 to 900°C with a scanning rate of 10°C/min (10–15 mg each in an open alumina crucible). Both DSC and TGA were under nitrogen environment.Release behaviors of IBU were studied at pH 1.2 (corresponding to the gastric fluid) and 6.8 (corresponding to the intestinal fluid) using buffer solutions of HCl–KCl and phosphate, respectively [25, 26]. Powders containing IBU (5 mg for IBU only; 10 mg for ball-milled samples of IBU and calcium carbonate) were placed in a 300 mL solution (500 mL round bottom flask) at 37°C, and the mixture was stirred at 200 rpm using an overhead stirrer (HS-30D, Wisd Laboratory Instruments, Wertheim, Germany). To analyze the concentration of IBU in the solution, 3 mL samples were removed after 5, 10, 20, 30, 60, 120, and 180 min, and the solution was refilled immediately with the original buffer solutions to keep the volume of the solution constant. The solution sample removed at a given interval was filtered through a cellulose acetate filter (pore size 0.45 μm, MFS-13, Advantec, Tokyo, Japan), and its UV absorbance was measured at 222 nm (Optizen POP, Mecasys, Daejeon, South Korea) where the absorbance was at its maximum. The UV absorbance was then converted to the concentration using a preconstructed calibration curve. The release experiments were independently repeated in triplicate for each sample.


### 2.4. Computational Calculations of Binding Energy

The binding energy of IBU on the surfaces of aragonite and calcite was calculated using the Materials Studio simulation software (version 7.0) from Accelrys (San Diego, CA, USA) equipped with Forcite module and COMPASS force field [27], which was known for being effective for the calculations of the binding on calcium carbonate [28]. The (010)/(110) faces of aragonite and the (104) of calcite were selected as the adsorption surfaces based on the previous morphological observations [10, 24, 29]. Electrostatic energy terms were treated using Ewald summation method, and van der Waals energy was calculated with a cutoff distance of 12.5 Å using an atom-based summation method. The crystal structures of aragonite and calcite were obtained from the previous publications [30, 31], and the partial charge was force-field assigned. The initial geometry optimization and the charge assignment of IBU were also performed before adsorption simulation. The adsorption surfaces of calcium carbonate crystals were cleaved with thickness of 17 Å, which were then expanded over 40 Å × 40 Å. The centers of geometry of calcium and carbonate were considered for them to be included in the cleaved slab. After placing the IBU molecule at the center of the surfaces, Forcite quench (5 ps with 1 fs step) was performed to find the structure of the minimum energy. The NVT ensemble (Nosé thermostat) was used at 303 K reflecting the measured temperature during the ball milling process [32]. Among the 5,000 different structures, the structures at every 500 frames were quenched and optimized. The binding energy (Eb) was calculated for the minimum energy structure of each surface: Eb=Et-(Ei+Es), where Et, Ei, and Es are the total energy, the energy of adsorbed IBU, and the energy of surface, respectively.


## 2.1. Preparation of Calcite and Aragonite

Two polymorphs of anhydrous calcium carbonate were prepared following a method using water-alcohol mixtures [24]. To obtain calcite, sodium carbonate (26.0 mmol, 2.75 g: Na2CO3: ≥99.0%, Sigma-Aldrich, Milwaukee, WI, USA) was completely dissolved in the solution of 100 mL ethanol (HPLC grade, 99.0%, Samchun, Pyeongtaek, South Korea) and 900 mL deionized water (DI water: resistivity of 18.2 MOhm·cm, Direct-Q from Millipore, Billerica, MA, USA) contained in a 1000 mL volumetric flask at room temperature (ca. 25°C), and then calcium chloride (26.0 mmol, 2.89 g: CaCl2: 99+%, Sigma-Aldrich, Milwaukee, WI, USA) was added to the solution. The solution was vigorously mixed at all time with a stir bar (length, 30 mm) equipped with a magnetic stirrer (HS180, Misung Scientific Co., Seoul, South Korea). The procedure to obtain aragonite was the same as that for calcite except that 50 vol% ethanol (500 mL ethanol and 500 mL DI water) was used. After 24 h, the precipitated products were collected by vacuum filtration (number 20 filter paper, pore diameter 5 μm, Hyundai Micro, Seoul, South Korea), washed with DI water, and dried in a convection oven at 40°C for 12 h before further use.


## 2.2. Ball Milling IBU with Calcite and Aragonite

Ibuprofen (IBU: >98%) was used as obtained from Sigma-Aldrich (Milwaukee, WI, USA). IBU (100 mg) was ball-milled with calcite or aragonite (100 mg) at the frequency of 10 Hz, and the milling time was 120 or 240 min. For the procedure, a Retsch ball mill (MM 200, Haan, Germany) was used with a cylindrical stainless steel jar (about 25 mL; inner diameter ca. 26 mm and inner length ca. 52 mm) and two stainless steel balls (diameter, 9 mm), which was often utilized in pharmaceutical grinding [20]. The ball-milled products were immediately used for further characterization.


## 2.3. Characterization of Raw and Ball-Milled Materials

Morphologies of IBU, calcite, aragonite, and ball-milled products were characterized using field-emission scanning electron microscopy (FE-SEM: JSM-6700F, JEOL, Tokyo, Japan) after thin Au coating (Cressington Sputter Coater 108, Watford, UK) to minimize surface charging. The materials were also characterized in their crystal structures using powder X-ray diffraction (XRD: D2 PHASER, Bruker AXS, Billerica, MA, USA). XRD was performed with CuKα radiation (λ = 1.5406 Å at 30 kV, 10 mA) in the 2θ range of 5–40° (scanning rate, 1°/min). Fourier transformation infrared spectroscopy (FT-IR) was performed using a Cary 660 FTIR Spectrometer (Agilent Technologies, Santa Clara, CA, USA). KBr (FT-IR grade, ≥99%, Sigma-Aldrich, Milwaukee, WI, USA) discs were prepared for the transmission mode, where the IR spectra were collected in the wavenumber range of 4000–400 cm−1.Thermal analyses were performed via differential scanning calorimetry (DSC: DSC 821e, Mettler-Toledo, Columbus, OH, USA) and thermogravimetric analysis (TGA: TGA/SDTA 851e, Mettler-Toledo). DSC was to check the crystalline state of IBU, and it was precalibrated for enthalpy and temperature using indium. The scanning for the IBU containing samples (2-3 mg each in a hermetically sealed aluminum crucible) was from 25 to 100°C with a heating rate of 10°C/min, and DSC experiments were repeated in triplicate for each sample. TGA was performed from 25 to 900°C with a scanning rate of 10°C/min (10–15 mg each in an open alumina crucible). Both DSC and TGA were under nitrogen environment.Release behaviors of IBU were studied at pH 1.2 (corresponding to the gastric fluid) and 6.8 (corresponding to the intestinal fluid) using buffer solutions of HCl–KCl and phosphate, respectively [25, 26]. Powders containing IBU (5 mg for IBU only; 10 mg for ball-milled samples of IBU and calcium carbonate) were placed in a 300 mL solution (500 mL round bottom flask) at 37°C, and the mixture was stirred at 200 rpm using an overhead stirrer (HS-30D, Wisd Laboratory Instruments, Wertheim, Germany). To analyze the concentration of IBU in the solution, 3 mL samples were removed after 5, 10, 20, 30, 60, 120, and 180 min, and the solution was refilled immediately with the original buffer solutions to keep the volume of the solution constant. The solution sample removed at a given interval was filtered through a cellulose acetate filter (pore size 0.45 μm, MFS-13, Advantec, Tokyo, Japan), and its UV absorbance was measured at 222 nm (Optizen POP, Mecasys, Daejeon, South Korea) where the absorbance was at its maximum. The UV absorbance was then converted to the concentration using a preconstructed calibration curve. The release experiments were independently repeated in triplicate for each sample.


## 2.4. Computational Calculations of Binding Energy

The binding energy of IBU on the surfaces of aragonite and calcite was calculated using the Materials Studio simulation software (version 7.0) from Accelrys (San Diego, CA, USA) equipped with Forcite module and COMPASS force field [27], which was known for being effective for the calculations of the binding on calcium carbonate [28]. The (010)/(110) faces of aragonite and the (104) of calcite were selected as the adsorption surfaces based on the previous morphological observations [10, 24, 29]. Electrostatic energy terms were treated using Ewald summation method, and van der Waals energy was calculated with a cutoff distance of 12.5 Å using an atom-based summation method. The crystal structures of aragonite and calcite were obtained from the previous publications [30, 31], and the partial charge was force-field assigned. The initial geometry optimization and the charge assignment of IBU were also performed before adsorption simulation. The adsorption surfaces of calcium carbonate crystals were cleaved with thickness of 17 Å, which were then expanded over 40 Å × 40 Å. The centers of geometry of calcium and carbonate were considered for them to be included in the cleaved slab. After placing the IBU molecule at the center of the surfaces, Forcite quench (5 ps with 1 fs step) was performed to find the structure of the minimum energy. The NVT ensemble (Nosé thermostat) was used at 303 K reflecting the measured temperature during the ball milling process [32]. Among the 5,000 different structures, the structures at every 500 frames were quenched and optimized. The binding energy (Eb) was calculated for the minimum energy structure of each surface: Eb=Et-(Ei+Es), where Et, Ei, and Es are the total energy, the energy of adsorbed IBU, and the energy of surface, respectively.


## 3. Results and Discussion

### 3.1. Structures of Ball-Milled IBU with Calcite and Aragonite

The IBU crystals before milling as well as synthesized polymorphs of calcium carbonate (calcite and aragonite) were shown in Figure1. The IBU crystals were plate-shaped with their length of about 100–200 μm (Figure 1(a)). They were of typical morphology as previously observed: the large {100} faces and the {001}, {110} side faces [33, 34]. The crystal shapes of the synthesized polymorphs of calcium carbonate were also of routinely observed morphology. The aragonite crystals were needle-shaped with their length of about 2–5 μm (Figure 1(b)). As shown in the inset, the aragonite needle was composed of submicron domains, and this observation was in agreement with the previous study using the same synthesis method [24]. The utilized method is known to generate {110} and {010} faces of aragonite as the enclosing surfaces, and the {010} is also the distinct cleavage plane [24, 29]. The calcite crystals were rhombohedral with most of their size at 1–5 μm (Figure 1(c)). The enclosing surfaces of the rhombs are known as the {104} faces, which are also the perfect cleavage planes [10, 29, 35].Figure 1
SEM images of ibuprofen (a), aragonite (b), and calcite (c) crystals. The scale bar of the inset of (b) is 1μm.
(a)
(b)
(c)When IBU was ball-milled with the crystals of calcium carbonate, significant differences were observed between the cases with aragonite and calcite. When IBU was ball-milled with aragonite, the aragonite needles were mostly disassembled into their individual submicron domains (Figures2(a) and 2(b)), although some needle-shaped parts could be found (arrowheads of Figures 2(a) and 2(b)). More importantly, IBU and aragonite formed tightly integrated mesocrystal structures of the overall size about 4–10 μm. (In the case of IBU/aragonite milling, the microscopic examination did not reveal clear differences between the 120- and 240-minute samples.) In contrast, IBU ball milled with calcite did not show mesocrystal formation. IBU and calcite mostly remained as separate entities, although a small part of them appeared associated as indicated by the arrowheads of Figures 2(c) and 2(d). Note that calcite was easily distinguishable because of its {104} cleavage surfaces. (In the case of IBU/calcite, the calcite appeared more fractured and smaller after the 240-minute milling than after 120 min.)Figure 2
SEM images of IBU/aragonite after ball milling for (a) 120 and (b) 240 min; IBU/calcite after ball milling for (c) 120 and (d) 240 min. Arrowheads of (a) and (b) indicated the aragonite needles, and those of (c) and (d) indicated IBU. Also shown in the insets of (a) and (b) were the submicron domains as well as the needles of aragonite integrated with IBU.
(a)
(b)
(c)
(d)XRD analysis confirmed the nearly exclusive formation of calcite and aragonite during the preparation step (Figure3). The prominent diffraction peaks of aragonite were shown at ca. 26.0, 27.0, 35.9, and 38.2° for the {111}, {021}, {200}, and {130} planes, respectively (Figure 3(a)) [36]. Those of calcite were at ca. 22.6, 29.0, 35.6, and 39.0° for the {012}, {104}, {110}, and {113} planes, respectively (Figure 3(b)) [36]. (Note that the calcite {104} peak existed in negligible intensity in the aragonite batch.) The polymorphs of aragonite and calcite were also distinguishable using FT-IR analysis (Figure 4). The former had characteristic doublet peaks at 700 and 713 cm−1 as well as peaks at 1082 and 1786 cm−1 (Figures 4(a) and 4(b)), whereas the latter had a singlet at 711 cm−1, nothing around 1080 cm−1, and a peaks at 1799 cm−1 (Figures 4(c) and 4(d)) [37–39].Figure 3
XRD patterns of IBU/aragonite (a) and IBU/calcite (b) before and after ball milling.
(a)
(b)Figure 4
IR spectra of IBU/aragonite before and after ball milling (a); aragonite (zoomed in between 1100 and 650 cm−1) (b); IBU/calcite before and after ball milling (c); calcite (zoomed in between 1100 and 650 cm−1) (d).
(a)
(b)
(c)
(d)Ball milling did not alter the structures of IBU crystals significantly enough to generate new XRD diffraction peaks from different crystal structures (Figure3). Major XRD diffraction peaks of IBU were at ca. 16.4, 18.7, 19.8, and 21.9° for {210}, {20−2}, {012}, and {202}, respectively [40]. All major diffraction peaks were the same after ball milling, although some alterations in the intensity, most noticeably the increased relative intensity of {012} peak at ca. 19.8°, indicated the changes in the crystal morphology. In addition, the analysis of the full width at half maximum (FWHM) was in agreement with the microscopic observation. The FWHM was analyzed based on the relatively intensified {012} peak. The FWHM was about 0.11° before milling, and it increased after milling with aragonite or calcite. The FWHM values were 0.16 and 0.17° after 120 and 240 min of milling with aragonite, respectively. They were 0.17 and 0.19° after 120 and 240 min with calcite, respectively. Since FWHM is inversely proportional to the crystallite size, the analysis indicated the size decrease of the IBU crystallite with ball milling [41]. Note that the {012} plane is parallel to thea-axis, which is also perpendicular to the large {100} face of the plate-shaped IBU crystals before milling (Figure 1(a)) [33, 34]. This suggested that breakage occurred in the perpendicular direction of the large face as would be expected from the original shape of the crystals.The interactions between IBU and calcium carbonate were further examined with FT-IR and molecular dynamics. FT-IR showed that one of the carbonate-related peaks of aragonite noticeably changed after milling with IBU (Figure4(a)). The frequency corresponding to asymmetric stretching was at 1495 cm−1 [37], and it became 1485 and 1481 cm−1 after 120 and 240 min of milling with IBU, respectively. In contrast, the corresponding change appeared absent for calcite (Figure 4(b)). Also, note that the change on the IBU side, including that for the carbonyl peak at 1720 cm−1, was difficult to find.The fundamental aspects of IBU interaction with aragonite and calcite were investigated by studying the binding energy and structures. The binding energy of IBU on the mineral surfaces was in the following order: aragonite (010), |–212 kcal/mol| ≫ aragonite (110), |−63 kcal/mol| > calcite (104), |−44 kcal/mol|, and the binding was predominantly of electrostatic nature in all cases. The corresponding binding conformations of IBU to the surfaces were shown in Figure 5. The binding differences seemed to originate from the dissimilar atomic arrangements of the surfaces. Each calcium ion of aragonite and calcite in bulk was coordinated with nine and six oxygens, respectively; the surface calcium of (010) and (110) lacked three coordinating oxygens out of nine, whereas that of (104) was short of only one oxygen out of six. This appeared to allow stronger electrostatic interactions of surface calcium of aragonite with the oxygens of IBU. In addition, the subtle differences in the two-dimensional periodic structures between (010) {4.961 Å × 5.740 Å} and (110) {4.694 Å × 5.740 Å} appeared to contribute to the differences of the IBU binding conformations and interactions.Figure 5
Binding conformation of IBU on the surfaces of aragonite (010) (a); aragonite (110) (b); calcite (104) (c).
(a)
(b)
(c)Overall, the IR analysis and the computational study of the binding indicated the higher affinity of IBU to aragonite compared to calcite. This was consistent with the microscopic observation, where the intimate association of IBU was found with aragonite but not with calcite.


### 3.2. Properties of Ball-Milled IBU with Calcite and Aragonite

Thermal properties of IBU ball milled with calcium carbonate were examined with DSC. The melting point of IBU was about 77°C before milling. It became about 74 and 73°C after 120 and 240 min of milling with aragonite; it was about 76 and 75°C after 120 and 240 min of milling with calcite (Figure6(a)). The melting enthalpy showed greater changes (Figure 6(b)). The reported enthalpy was the normalized value based on the TGA analysis, which revealed the exact amount of IBU in the hybrid sample. (Calcium carbonate, both aragonite and calcite, started to experience weight loss at around 600°C to eventually leave ca. 56% of the original weight. This corresponded to the formation of calcium oxide by losing carbon dioxide; IBU decomposed nearly completely below 300°C to leave less than 1% of the original weight.) The melting enthalpy of IBU was about 172 J/g before milling. It became about 162 and 126 J/g after 120 and 240 min of milling with aragonite; it was about 173 and 151 J/g after 120 and 240 min of milling with calcite. Overall, the decrease of melting point and enthalpy of IBU was observed after milling, which was probably due to the decrease of the crystal size and crystallinity [42, 43]. Also, the effect of aragonite was more significant than that of calcite, which was in accordance with the structural analysis in the previous section.Figure 6
(a) Melting points and (b) melting enthalpy of IBU/aragonite and IBU/calcite after ball milling.
(a)
(b)Release behaviors of IBU from the ball-milled IBU/aragonite and IBU/calcite were studied at pH 1.2 and 6.8 (Figure7), where the change of pH during the release was less than 0.1 in all cases. The release behavior from the IBU/aragonite hybrid was pH responsive. After milling for 240 min, the initial release (<30 min) accelerated at pH 1.2, while it decelerated at pH 6.8, compared with neat IBU. This was apparently due to the high solubility of aragonite at low pH [23], combined with its intimate association with IBU. Note that 120-minute milling was not as effective at pH 1.2, while its deceleration effect at pH 6.8 was valid. In contrast, ball milling of IBU with calcite was not effective in modulating the release rate. Overall, the release behaviors of IBU confirmed that they could be adjusted only when IBU was intimately associated with the ball-milled substrate. When the substrate was rapidly soluble, the IBU release was expedited; when the substrate was marginally soluble, the release slowed down. Further studies on the quantitative analysis of the release kinetics and on the extended release behavior with the fine-tuned structures would be necessary to establish the utility of the mesocrystals in the controlled drug release.Figure 7
IBU release profiles at pH 1.2 and 6.8 from ball-milled IBU/aragonite (a) and IBU/calcite (b).
(a)
(b)


## 3.1. Structures of Ball-Milled IBU with Calcite and Aragonite

The IBU crystals before milling as well as synthesized polymorphs of calcium carbonate (calcite and aragonite) were shown in Figure1. The IBU crystals were plate-shaped with their length of about 100–200 μm (Figure 1(a)). They were of typical morphology as previously observed: the large {100} faces and the {001}, {110} side faces [33, 34]. The crystal shapes of the synthesized polymorphs of calcium carbonate were also of routinely observed morphology. The aragonite crystals were needle-shaped with their length of about 2–5 μm (Figure 1(b)). As shown in the inset, the aragonite needle was composed of submicron domains, and this observation was in agreement with the previous study using the same synthesis method [24]. The utilized method is known to generate {110} and {010} faces of aragonite as the enclosing surfaces, and the {010} is also the distinct cleavage plane [24, 29]. The calcite crystals were rhombohedral with most of their size at 1–5 μm (Figure 1(c)). The enclosing surfaces of the rhombs are known as the {104} faces, which are also the perfect cleavage planes [10, 29, 35].Figure 1
SEM images of ibuprofen (a), aragonite (b), and calcite (c) crystals. The scale bar of the inset of (b) is 1μm.
(a)
(b)
(c)When IBU was ball-milled with the crystals of calcium carbonate, significant differences were observed between the cases with aragonite and calcite. When IBU was ball-milled with aragonite, the aragonite needles were mostly disassembled into their individual submicron domains (Figures2(a) and 2(b)), although some needle-shaped parts could be found (arrowheads of Figures 2(a) and 2(b)). More importantly, IBU and aragonite formed tightly integrated mesocrystal structures of the overall size about 4–10 μm. (In the case of IBU/aragonite milling, the microscopic examination did not reveal clear differences between the 120- and 240-minute samples.) In contrast, IBU ball milled with calcite did not show mesocrystal formation. IBU and calcite mostly remained as separate entities, although a small part of them appeared associated as indicated by the arrowheads of Figures 2(c) and 2(d). Note that calcite was easily distinguishable because of its {104} cleavage surfaces. (In the case of IBU/calcite, the calcite appeared more fractured and smaller after the 240-minute milling than after 120 min.)Figure 2
SEM images of IBU/aragonite after ball milling for (a) 120 and (b) 240 min; IBU/calcite after ball milling for (c) 120 and (d) 240 min. Arrowheads of (a) and (b) indicated the aragonite needles, and those of (c) and (d) indicated IBU. Also shown in the insets of (a) and (b) were the submicron domains as well as the needles of aragonite integrated with IBU.
(a)
(b)
(c)
(d)XRD analysis confirmed the nearly exclusive formation of calcite and aragonite during the preparation step (Figure3). The prominent diffraction peaks of aragonite were shown at ca. 26.0, 27.0, 35.9, and 38.2° for the {111}, {021}, {200}, and {130} planes, respectively (Figure 3(a)) [36]. Those of calcite were at ca. 22.6, 29.0, 35.6, and 39.0° for the {012}, {104}, {110}, and {113} planes, respectively (Figure 3(b)) [36]. (Note that the calcite {104} peak existed in negligible intensity in the aragonite batch.) The polymorphs of aragonite and calcite were also distinguishable using FT-IR analysis (Figure 4). The former had characteristic doublet peaks at 700 and 713 cm−1 as well as peaks at 1082 and 1786 cm−1 (Figures 4(a) and 4(b)), whereas the latter had a singlet at 711 cm−1, nothing around 1080 cm−1, and a peaks at 1799 cm−1 (Figures 4(c) and 4(d)) [37–39].Figure 3
XRD patterns of IBU/aragonite (a) and IBU/calcite (b) before and after ball milling.
(a)
(b)Figure 4
IR spectra of IBU/aragonite before and after ball milling (a); aragonite (zoomed in between 1100 and 650 cm−1) (b); IBU/calcite before and after ball milling (c); calcite (zoomed in between 1100 and 650 cm−1) (d).
(a)
(b)
(c)
(d)Ball milling did not alter the structures of IBU crystals significantly enough to generate new XRD diffraction peaks from different crystal structures (Figure3). Major XRD diffraction peaks of IBU were at ca. 16.4, 18.7, 19.8, and 21.9° for {210}, {20−2}, {012}, and {202}, respectively [40]. All major diffraction peaks were the same after ball milling, although some alterations in the intensity, most noticeably the increased relative intensity of {012} peak at ca. 19.8°, indicated the changes in the crystal morphology. In addition, the analysis of the full width at half maximum (FWHM) was in agreement with the microscopic observation. The FWHM was analyzed based on the relatively intensified {012} peak. The FWHM was about 0.11° before milling, and it increased after milling with aragonite or calcite. The FWHM values were 0.16 and 0.17° after 120 and 240 min of milling with aragonite, respectively. They were 0.17 and 0.19° after 120 and 240 min with calcite, respectively. Since FWHM is inversely proportional to the crystallite size, the analysis indicated the size decrease of the IBU crystallite with ball milling [41]. Note that the {012} plane is parallel to thea-axis, which is also perpendicular to the large {100} face of the plate-shaped IBU crystals before milling (Figure 1(a)) [33, 34]. This suggested that breakage occurred in the perpendicular direction of the large face as would be expected from the original shape of the crystals.The interactions between IBU and calcium carbonate were further examined with FT-IR and molecular dynamics. FT-IR showed that one of the carbonate-related peaks of aragonite noticeably changed after milling with IBU (Figure4(a)). The frequency corresponding to asymmetric stretching was at 1495 cm−1 [37], and it became 1485 and 1481 cm−1 after 120 and 240 min of milling with IBU, respectively. In contrast, the corresponding change appeared absent for calcite (Figure 4(b)). Also, note that the change on the IBU side, including that for the carbonyl peak at 1720 cm−1, was difficult to find.The fundamental aspects of IBU interaction with aragonite and calcite were investigated by studying the binding energy and structures. The binding energy of IBU on the mineral surfaces was in the following order: aragonite (010), |–212 kcal/mol| ≫ aragonite (110), |−63 kcal/mol| > calcite (104), |−44 kcal/mol|, and the binding was predominantly of electrostatic nature in all cases. The corresponding binding conformations of IBU to the surfaces were shown in Figure 5. The binding differences seemed to originate from the dissimilar atomic arrangements of the surfaces. Each calcium ion of aragonite and calcite in bulk was coordinated with nine and six oxygens, respectively; the surface calcium of (010) and (110) lacked three coordinating oxygens out of nine, whereas that of (104) was short of only one oxygen out of six. This appeared to allow stronger electrostatic interactions of surface calcium of aragonite with the oxygens of IBU. In addition, the subtle differences in the two-dimensional periodic structures between (010) {4.961 Å × 5.740 Å} and (110) {4.694 Å × 5.740 Å} appeared to contribute to the differences of the IBU binding conformations and interactions.Figure 5
Binding conformation of IBU on the surfaces of aragonite (010) (a); aragonite (110) (b); calcite (104) (c).
(a)
(b)
(c)Overall, the IR analysis and the computational study of the binding indicated the higher affinity of IBU to aragonite compared to calcite. This was consistent with the microscopic observation, where the intimate association of IBU was found with aragonite but not with calcite.


## 3.2. Properties of Ball-Milled IBU with Calcite and Aragonite

Thermal properties of IBU ball milled with calcium carbonate were examined with DSC. The melting point of IBU was about 77°C before milling. It became about 74 and 73°C after 120 and 240 min of milling with aragonite; it was about 76 and 75°C after 120 and 240 min of milling with calcite (Figure6(a)). The melting enthalpy showed greater changes (Figure 6(b)). The reported enthalpy was the normalized value based on the TGA analysis, which revealed the exact amount of IBU in the hybrid sample. (Calcium carbonate, both aragonite and calcite, started to experience weight loss at around 600°C to eventually leave ca. 56% of the original weight. This corresponded to the formation of calcium oxide by losing carbon dioxide; IBU decomposed nearly completely below 300°C to leave less than 1% of the original weight.) The melting enthalpy of IBU was about 172 J/g before milling. It became about 162 and 126 J/g after 120 and 240 min of milling with aragonite; it was about 173 and 151 J/g after 120 and 240 min of milling with calcite. Overall, the decrease of melting point and enthalpy of IBU was observed after milling, which was probably due to the decrease of the crystal size and crystallinity [42, 43]. Also, the effect of aragonite was more significant than that of calcite, which was in accordance with the structural analysis in the previous section.Figure 6
(a) Melting points and (b) melting enthalpy of IBU/aragonite and IBU/calcite after ball milling.
(a)
(b)Release behaviors of IBU from the ball-milled IBU/aragonite and IBU/calcite were studied at pH 1.2 and 6.8 (Figure7), where the change of pH during the release was less than 0.1 in all cases. The release behavior from the IBU/aragonite hybrid was pH responsive. After milling for 240 min, the initial release (<30 min) accelerated at pH 1.2, while it decelerated at pH 6.8, compared with neat IBU. This was apparently due to the high solubility of aragonite at low pH [23], combined with its intimate association with IBU. Note that 120-minute milling was not as effective at pH 1.2, while its deceleration effect at pH 6.8 was valid. In contrast, ball milling of IBU with calcite was not effective in modulating the release rate. Overall, the release behaviors of IBU confirmed that they could be adjusted only when IBU was intimately associated with the ball-milled substrate. When the substrate was rapidly soluble, the IBU release was expedited; when the substrate was marginally soluble, the release slowed down. Further studies on the quantitative analysis of the release kinetics and on the extended release behavior with the fine-tuned structures would be necessary to establish the utility of the mesocrystals in the controlled drug release.Figure 7
IBU release profiles at pH 1.2 and 6.8 from ball-milled IBU/aragonite (a) and IBU/calcite (b).
(a)
(b)


## 4. Conclusions

In summary, two anhydrous polymorphs of calcium carbonate (aragonite and calcite) were employed during ball milling of IBU to generate IBU/calcium carbonate hybrid materials. Aragonite polymorph was intimately integrated with IBU to form a mesocrystal-like structure, whereas calcite did not seem to be as effective under the experimental conditions employed in the present study. Aragonite and IBU kept their original crystal structures within the mesocrystals, although morphological variations occurred. Aragonite/IBU interaction was verified by the changes in the IR vibration of the carbonate of aragonite, and its strong nature was corroborated by the binding energy computationally obtained. The IBU fused with aragonite showed modulated thermal behavior, further confirming the observed structures. Finally, the IBU release behavior could be regulated through the conditions affecting the aragonite substrate. The IBU release sped up under the conditions disintegrating aragonite, and it slowed down when aragonite was stable. The present study indicates that the substrates that disintegrate at specific conditions can be utilized for the environment-responsive release of APIs. For this purpose, it also appears that the substrates need to form intimately associated structures with APIs to be delivered.



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*Source: 163190-2015-08-13.xml*