Development of antiproliferative nanohybrid compound with controlled release property using ellagic acid as the active agent

Abstract

An ellagic acid (EA)–zinc layered hydroxide (ZLH) nanohybrid (EAN) was synthesized under a nonaqueous environment using EA and zinc oxide (ZnO) as the precursors. Powder X-ray diffraction showed that the basal spacing of the nanohybrid was 10.4 Å, resulting in the spatial orientation of EA molecules between the interlayers of 22.5° from z-axis with two negative charges at 8,8′ position of the molecules pointed toward the ZLH interlayers. FTIR study showed that the intercalated EA spectral feature is generally similar to that of EA, but with bands slightly shifted. This indicates that some chemical bonding of EA presence between the nanohybrid interlayers was slightly changed, due to the formation of host–guest interaction. The nanohybrid is of mesopores type with 58.8% drug loading and enhanced thermal stability. The release of the drug active, EA from the nanohybrid was found to be sustained and therefore has good potential to be used as a drug controlled-release formulation. In vitro bioassay study showed that the EAN has a mild effect on the hepatocytes cells, similar to its counterpart, free EA.

Introduction

Systemic drug delivery leads to distribution of the drug throughout the body through blood circulation, which can lead to drug concentration accumulation in unwanted parts of the body that causes severe side effects. Additionally, conventional drug administration methods do not provide satisfactory pharmacokinetic profiles because the drug concentration rapidly falls below the desired levels.¹ Cancer chemotherapy is the treatment of cancer cells with an antineoplastic drug. The main property of cancer cells is rapid division. Chemotherapy acts by killing cells that divide rapidly, which means it also harms cells that divide rapidly under normal circumstances such as cells in the bone marrow, digestive tract, and hair follicles, producing side effects such as myelosuppression,² mucosities,³ and alopecia.⁴ To overcome these side effects, researchers are now searching for efficient and safe transport carriers, which prolong exposure time to drugs and target cancerous cells without targeting healthy cells.

In the past few decades, many carriers have been developed, and generally can be classified into four major groups: viral carriers, recombinant proteins, organic cationic compounds, and inorganic nanoparticles.^5,6

Recently, inorganic nanoparticles have attracted considerable attention due to their versatile features, such as wide availability, good biocompatibility, rich surface functionality, potential capability of target delivery, and controlled release of the drug from the inorganic nanoparticles.^7–9 Calcium phosphate, gold, carbon nanotubes, silicon oxide, iron oxide and layered double hydroxides are examples of inorganic nanoparticles, which have intensively investigated in different studies by different groups.^10–15 Layered double hydroxides (LDH) are materials with a number of advantages for drug delivery. Among these are their ease of laboratory preparation with a controlled particle size,¹⁶ and the drugs can be easily loaded into the interlayers space by ion exchange, comparing with other nanoparticles which need further modification such as surface functional modification.^17,18 Layered double hydroxides have a high zeta potential, 20–30 mV, which provides a strong driving force on to the surface of a cell. LDH are degraded in an acidic environment to form M²⁺, M³⁺, and X⁻ ions which leads the drug actives leaving the cell through the ion-tunnels, whereas the others inorganic nanoparticles accumulate in the cells because of their low solubility in the cells. Low cytotoxicity is another virtue of LDH. Hussein et al reported that there is no toxic effect of Zn–Al LDH at low concentration on Chinese hamster ovary cells.¹⁹

LDH, also known as hydrotalcite-like compounds, are formed by layered units in which metal cations are octahedrally coordinated with hydroxyl groups, as in the brucite (Mg(OH)₂) structure. The isomorphic substitution of divalent cations by trivalent cations leaves a residual positive charge that is stabilized by inter layer anions. The general formula for hydrotalcite is [M²⁺_1–xM³⁺_x (OH)₂]^x+ (A^m−)_x/m·nH₂O, where M²⁺ is divalent cations, M³⁺ is trivalent cations and A^m− is exchangeable anion with charge (m−).²⁰ Similar to LDH, zinc layered hydroxide (ZLH) is a compound whose structure derived from brucite. One quarter of the octahedral coordinated zinc cations are displaced from the main layer to tetrahedral sites located above and below each empty octahedron and can be represented by the general formula M²⁺ (OH)_2–x (A^m−)_x/m·nH₂O, where M²⁺ is the Zn²⁺ and A^m− is counter ions with (m−) charge.²¹

Because of ZLH anionic exchange capacity, many active compounds can be intercalated into ZLH interlayers. These include the anticarcinogenic agent gallic acid,²² linoleic acid,²³ sunscreen materials such as 2-amino benzoic acid and 4-amino benzoic acid,²⁴ nucleoside monophosphate, DNA,²⁵ and pharmaceutical, cosmeceutical, and nutraceutical compounds.²⁶

Various methods have been adopted for preparation of ZLH and its nanohybrids, namely hydrolysis of salt and oxides,²⁷ urea hydrolysis,²⁸ precipitation with alkaline solutions,²⁹ and solid state reaction.³⁰ Direct reaction of zinc oxide (ZnO) is simple and easily used either for aqueous or nonaqueous systems. Such a method is economic and environmentally friendly as fewer steps and chemicals are involved.

Ellagic acid (EA) is an antioxidant, which is a family of drugs much used for cancer treatment. Intense research has been conducted to investigate the effect of EA on the cancer cell as well as its delivery.^31–34 Lately, many articles have described the preparation of ZLH as a starting material followed by intercalation of the anion. However, to the best of our knowledge, little work has been published on the use of ZnO as a starting material to intercalate drug actives.^35,36 Therefore, the main objective of this work was to explore the potential use of ZnO as a starting material for the intercalation of EA for the formation of a new EA–ZLH nanohybrid (EAN). The resulting nanohybrid was then used as a controlled release formulation of drug active EA. A cytotoxicity study of nanohybrids was also carried out.

Experimental

Materials

All chemicals used in this study were of analytical grade and used without any further purification. Hydrated EA (97% purity) was purchased from Sigma-Aldrich (St Louis, MO) and pure commercial ZnO of ACS reagent was used, purchased from Fisher Scientific (Waltham, MA). Dimethyl sulfoxide (DMSO) was purchased from Ajax Finechem (Sydney, Australia) with 0.1% water content used as solvent.

Method

Typically, the appropriate amount of hydrated EA (0.0013 mol) was dissolved in DMSO followed by 10 minutes stirring and heating for 40°C. The ZnO (0.2 g) was mixed with the solution of EA and stirred at 70°C for 8 hours. After filtration and washing with deionized water three times, the sample was dried in an oven at 60°C for 12 hours. The resulting material was then powdered and stored in a sample bottle for further use and characterization.

Characterization

Powder X-ray diffraction (PXRD) patterns were recorded at a range of 2–60° on a Shimadzu diffractometer, XRD-6000 (Tokyo, Japan) using CuK_α radiation at 40 kV and 30 mA. Fourier transform infra-red (FTIR) spectra of the materials were recorded over the range 400–4000 cm⁻¹ on a Perkin-Elmer 1752X spectrophotometer (Waltham, MA) using a KBr disc method. For carbon, hydrogen, nitrogen and sulfur (CHNS) analyses, a CHNS-932 model of LECO instrument (St Joseph, MI) was used. Thermogravimetric and differential thermogravimetric analyses (TGA-DTG) were carried out using a Mettler Toledo instrument (Greifensee, Switzerland). Surface characterization of the material was carried out using a nitrogen gas adsorption–desorption technique at 77 K using a Micromeritics ASAP 2000 (Norcross, GA). The surface morphology of the samples was observed by a scanning electron microscope (SEM), using JOEL JSM-6400 (Tokyo, Japan). UV-Vis spectra for optical properties and controlled-release study were accomplished using a Perkin Elmer UV-Vis Spectrophotometer, Lambda 35.

Controlled-release study

Drug release profiles were determined at room temperature by using 0.1 M Na₂CO₃³⁷ and Na₃PO₄³⁸ solutions. Both anions CO₃⁻², PO₄⁻³ are commonly used for preliminary study of drug release, to observe the controlled-release property of the intercalated drug actives. This was also conducted to study the effect of different negative species CO₃⁻², PO₄⁻³ on the rate of release. The UV-Vis spectrum of DMSO and EA dissolved in DMSO shows intense absorbance at 224.0 and 257.5 nm, respectively. Therefore, DMSO is an interference-free solvent. The EA released was measured at a predetermined time by UV-Vis spectrophotometer at 257.5 nm.³⁹ The EA release kinetics was fitted to four models, as shown in Table 2.^40–43

Table 2.

Correlation coefficient, rate constant, and half time obtained by fitting the data of the release of EA from EAN into 0.1 M Na₂CO₃ and 0.1 M Na₃PO₄; the equation of kinetic models used for the fitting is also indicated

Aqueous solution	Saturated release %	r2				Rate constant (k) pseudo-second order (g/mg·h)	t1/2 pseudo-second order (h)
		Zeroth-order	First-order	Pseudo-second order	Parabolic diffusion
Na2CO3	69%	0.6683	0.7635	0.9985	0.7997	0.0044	3.03
Na3PO4	94%	0.3963	0.7381	0.9996	0.5926	0.0175	0.61
Kinetic equation	Zeroth-order ${\text{M}}_{\text{t}}-{\text{M}}_{\text{o}}=-{\text{k}}_{\text{o}}\text{t}$	First-order $\text{log}({\text{M}}_{\text{t}}/{\text{M}}_{\text{o}})=-{\text{k}}_1\text{t}$		Pseudo-second order ${\text{t}/\text{q}}_{\text{t}}=1/\text{h}+\text{t}/{\text{q}}_{\text{e}}$		Parabolic diffusion $(1-{\text{M}}_{\text{t}}/{\text{M}}_{\text{o}})/\text{t}={\text{K}}_{\text{d}}{\text{t}}^{-0.5}+\text{a}$

Notes: M_o is the EA content remained in the ZLH at release time o, M_t is the EA content remained in the ZLH at release time t, q_e is the equilibrium release amount and q_t is the release amount at time t, h = k₂q_e ², k the corresponding release rate constant, a is constant whose chemical significance is not clearly resolved.⁴³

Abbreviations: EA, ellagic acid; ZLH, zinc layered hydroxide.

In vitro bioassay

The cytotoxicity effect of ZnO, EA, and EAN against healthy rat hepatocytes was examined by a cell viability test. Hepatocytes from normal healthy Sprague Dawley rats (n = 4) were isolated by a two-step collagenase perfusion technique.^44–46 Viability of freshly isolated rat hepatocytes was determined by trypan blue exclusion. After isolation, hepatocytes suspensions were incubated at a density of 1 × 10⁶ viable cells/mL in Leibovitz Glutamax I (L-15 incomplete) medium. About 25 μg/mL EA, EAN, and ZnO were added to DMSO (final DMSO concentration of 1.0% v/v). Control hepatocytes suspensions were incubated with an equivalent amount of DMSO. The flasks were sealed in 95% O₂/5% CO₂ and placed in a shaking water bath at 37°C. Samples were taken from these flasks at time points of 0, 0.5, 1, 3, and 6 hours for a viability test.

Viable cells were determined by lactate dehydrogenase activity in medium and in the lysed cells at each time point. The activity was assessed spectrophotometrically as described by Marshall and Caldwell.⁴⁵

Results and discussion

PXRD and EA orientation between ZLH interlayers

Figures 1A, B, and C show PXRD patterns of ZnO, EAN, and EA, respectively. For ZnO sample, the five intense reflections shown in Figure 1A at 30–60° correspond to diffractions due to 100, 002, 101, 102, and 110 planes. Figure 1B shows the PXRD pattern of EAN synthesized by direct reaction between 0.025 M hydrated EA with ZnO. As reported in the literature, the zinc hydroxide nitrate has sharp reflection at 9.7 Å due to the 200 plane of the monoclinic structure.^47,48 After the intercalation of the anions, the basal distance increased more than 9.7 Å due to the displacement of exchangeable nitrate anions and depending on the dimensions and the spatial orientation of the guest anion that is intercalated into the ZLH inorganic interlayers.⁴⁸ As shown in the Figure 1B, the formation of the EAN can be confirmed by the observation of two new diffraction patterns at d = 10.4 Å and 5.2 Å, which is due to 003 and 006 reflection, respectively. Total disappearance of the intense peaks of ZnO phase indicated that the sample EAN is pure phase and the ZnO was completely converted to ZLH.³⁶

Figure 1.

PXRD patterns of ZnO (A), EAN (B) and EA (C).

Abbreviations: PXRD, powder X-ray diffraction; EA, ellagic acid; EAN, ellagic acid nanohybrid.

The formation of EAN is believed to occur through a dissociation–deposition mechanism^36,49 which takes place in the nonaqueous solution of hydrated EA. The mechanism is composed of three steps:

1. Hydrolysis of ZnO in water into hydrated EA to form Zn(OH)₂ on the surface of the solid particles

   $$\text{ZnO}+{\text{H}}_2\text{O}\to \text{Zn}{(\text{OH})}_2$$

2. Formation Zn²⁺ species by dissociation of Zn(OH)₂

   $$\text{Zn}{(\text{OH})}_2\to {\text{Zn}}^{2+}+2{\text{OH}}^{-}$$

3. In addition, reaction between Zn²⁺ ions formed with hydroxyls, H₂O and EA anions in the solution generate the layered nanohybrid compound,

   $$\begin{array}{l}{\text{Zn}}^{2+}+2{\text{OH}}^{-}+{\text{EA}}^{-}+{\text{H}}_2\text{O}\\ \to {\text{Zn}}^{2+}{(\text{OH})}_{2-x}{({\text{EA}}^{m-})}_{x/m}·n{\text{H}}_2\text{O}\end{array}$$

The EA has the molecular structure of a planar phenolic lactone that is doubly deprotonated at positions 8 and/or 8′ when the pH is more than 5.6.⁵⁰ Figure 2A shows the three-dimensional molecular size of EA obtained using Chemoffice software (Cambridge, MA).

Figure 2.

Molecular structure of EA and three-dimensional molecular size of EA (A) and spatial orientation of EA in ZLH inorganic interlayers (B).

Abbreviations: EA, ellagic acid; ZLH, zinc layered hydroxide.

Figure 2B shows that the thickness of the ZLH is 4.8 Å⁵¹ and d-spacing of the ZLH samples intercalated by EA from XRD spectrum is 10.4 Å. Therefore, the gallery height avialable to be occupied is 5.6 Å, which is smaller than 12.4 Å or 9.8 Å, the dimension of EA. In addition, the thickness of two molecules of EA is about 5.8 Å, which is bigger than the gallery height. This means that the EA has to be oriented between the interlayers as a monolayer and the spatial orientation of the molecule is with an angle of 22.5° from z-axis as shown in Figure 2B.

FTIR spectroscopy

The FTIR spectra of the EAN nanohybrid and EA are given in Figure 3. The FTIR spectrum of EA shows an absorption band at 3557 cm⁻¹, attributed to the stretching mode of OH groups in the phenol at 7,7′, 8 and 8′ positions (Figure 2A)⁵² and broad absorption bands at 3500–2750 cm⁻¹ can be attributed to stretching of C–H aromatic ring²⁴ and hydrogen bond between EA molecules.⁵⁰ A band at 1700 cm⁻¹ is due to stretching of C=O^52,53 and bands at 1620–1511 cm⁻¹ are due to aromatic rings. A band at 1196 and 1058 cm⁻¹ is due to ester linkage of C–O stretching^34,52 and another band at 758 cm⁻¹ is due to C–H aromatic stretching.

Figure 3.

FTIR spectrum of EA (A) and EAN (B).

Abbreviations: FTIR, Fourier transform infra-red; EA, ellagic acid; EAN, ellagic acid nanohybrid.

FTIR spectrum of EAN (Figure 3B) shows characteristic bands of pure EA together with other band of ZLH. This indicates that the EA has been intercalated into the interlayer galleries of ZLH. Band for C=O, C–O ester linkage and C–H aromatic are slightly shifted in position to 1689, 1064, 750 cm⁻¹, respectively, due to the interaction between EA and the host interlayers as a result of the intercalation process. A broad absorption band observed at 2500–3600 cm⁻¹ is attributed to OH stretching due to the presence of hydroxyl group within the ZLH and phenolic hydroxide at position 7,7′.⁵⁰ A band at 1577 cm⁻¹ can be attributed to C=C stretching vibration of aromatic,⁵² and a band for ν(C–O) can be observed at 1107 cm⁻¹ and ν (Zn–O) absorption bands at 472 cm⁻¹. This indicates that the EA is coordinated to the inorganic layers by the negatively charged oxygen atoms at positions 8 and 8′.^50,54 The successful intercalation of EA into ZLH can be supported by CHNS analysis as shown in Table 1. EAN shows 32.7% carbon (w/w) and 2.6% (w/w) hydrogen, resulted in loading percentage of EA in the nanohybrid of about 58.8%. Elemental analysis using ICP/AES shows EAN contains 29.3% Zn (w/w).

Table 1.

Physicochemical properties of ZnO and ZLH-nanohybrid, EAN

Compounds	C (%)	H (%)	Zn (%w/w)	a Anion (%w/w)	BET surface area (m2/g)	BJH pore diameter (Å)	BJH pore volume (cm3/g)
ZnO	–	–	(80.3)	–	6.4	111	0.010
EAN	32.7	2.6	29.3	58.8	3.6	170	0.007

^aNotes: Estimated from CHNS analysis; value in the parentheses is the theoretical value.

Abbreviations: BJH, Barret–Joyner–Helenda; BET, Brunauer, Emmett and Teller; C, carbon; H, hydrogen; EAN, ellagic acid nanohybrid; ZnO, zinc oxide; ZLH, zinc layered hydroxide.

Thermal analysis

TGA-DTG thermogravimetric analysis obtained for EA and EAN is shown in Figure 4. The TGA-DTG thermograms of EA (Figure 4A) show the first step weight loss, which can be attributed to the removal of bonded water with hydrogen bond at temperature maxima of 112°C (8.2%). The onset of weight loss of EA occurs at 381°C with two steps weight loss at 463°C (39%) and 596°C (17.5%). Because of the intercalation, the shape of the TGA-DTG curves (Figure 4B) is changed. The first weight loss at 78°C in the DTA curve corresponding to the absorbed water. The absence of a band at 1600 cm⁻¹ in the FTIR spectrum confirming the absence of water between the interlayers.⁵⁵ The onset of dehydroxylation of zinc hydroxide layers and decomposition of EA occurs at around 496°C, with a rapid weight loss occurring in the temperature range at 496°C–819°C with two steps at 585°C (24%) and 714°C (25.2%). These temperatures are higher than the decomposition temperature of pure EA. This result indicates that the inorganic layers of ZLH enhanced the thermal stability of EA, the organic moiety.

Figure 4.

TGA-DTG thermogravimetric analysis of EA (A) and EAN (B).

Abbreviations: TGA–DTG, thermogravimetric and differential thermogravimetric analyses; EA, ellagic acid; EAN, ellagic acid nanohybrid.

Surface properties

Nitrogen adsorption–desorption isotherm for ZnO and EAN are shown in Figure 5A, shows features which can be described as Type IV in IUPAC classification, indicating mesopores-type material.⁵⁶ The adsorption of ZnO and EAN increased slowly at low pressure in the range of 0.0–0.8, followed by rapid adsorption of the absorbent at relative pressure of 0.8 and above. The desorption branch of the hysteresis loop for ZnO is much narrower compared to EAN, indicating different pore texture of the resulting materials. This is due to the formation of ZLH with a basal spacing of 10.4 Å as well as the formation of interstitial pores.⁵⁷ As a result of nitrogen adsorption study, we obtained the Breuneur, Emmet, and Teller (BET) surface area of the materials as shown in Table 1. The intercalation of EA into ZLH for the formation of EAN resulting in the decrease of the surface area from 6.4 m²/g for ZnO to 3.6 m²/g for EAN. This is attributed to the increase in the particles size and decrease of the pore volume.

Figure 5.

Adsorption–desorption isotherms (A) and BJH pore size distribution (B) for ZnO and EAN.

Abbreviations: BJH, Barret–Joyner–Halenda; EAN, ellagic acid nanohybrid.

Barret-Joyner-Halenda (BJH) pore size distribution for ZnO and EAN are shown in Figure 5B. Both materials show mesopores character, in agreement with the adsorption isotherm of Type IV. BJH pore size distribution of ZnO (Figure 5B) shows different features to that of EAN, indicating that the pore texture was modified, which is in agreement with the formation of EAN with a basal spacing of 10.4 Å. The BJH pore diameter of ZnO is lower than that of EAN. The increase from 111 to 170 Å is as a result of the intercalation of EA into the interlayer of ZLH.

Surface morphology of the samples, studied by field emission SEM for ZnO and EAN are shown in Figure 6. ZnO reveals nonuniform granular structure without any specific shape, with various sizes and shapes (Figure 6A). This structure was transformed into rod-like agglomerates with nonuniform size and shapes as shown in Figures 6B–C, when the intercalation of EA into the interlayer of ZLH had taken place.

Figure 6.

FESEM image of ZnO (A) and EAN (B) and EAN at higher magnification (C).

Abbreviations: FESEM, field emission scanning electron microscope; EA, ellagic acid; EAN, ellagic acid nanohybrid.

Optical properties

UV-Vis spectroscopy was used to investigate whether the intercalation of EA into the ZLH host resulted in changes in its optical properties. Figure 7A shows the UV-Vis spectra of pristine EA as well as EAN. It can be seen that pristine EA exhibits a strong absorption band at 350 nm with a shoulder at 370 nm, corresponding to the μ → μ* transition of EA. When EA was intercalated into ZLH interlayers, the 370 nm band was slightly increased in intensity, indicating doubly deprotonated EA between the interlayers.⁵⁰ This verifies that the drug molecules are stabilized by electrostatic interaction with the positive charge of ZLH.

Figure 7.

Solid-state UV-Vis spectra of pure EA and its nanohybrid, EAN (A) and their Kubelka-Munk plot of EA, EAN and ZnO (B).

Abbreviations: EA, ellagic acid; EAN, ellagic acid nanohybrid.

In order to estimate the energy band gap, the Kubelka– Munk (K–M) equation (1) was adopted,⁵⁸

$${(\text{F}·\text{h}\nu )}^2=\text{A}(\text{h}\nu -{\text{E}}_{\text{g}})$$ (1)

where F is the K–M, h is Bohr constant, E_g is the energy band gap in electron volt units.

It is clear from Eq. (1) that the band gap can be obtained by plotting (F · hν)² against hν in electron volts. Using the data obtained from Figure 7B, the band gap energy, E (eV) was determined, which is 3.29, 2.55, and 2.95 eV for ZnO, EAN, and EA, respectively. The value of band gap for ZnO determined in this work is similar to a band gap energy for ZnO determined previously.⁵⁹

Release behavior of the EA

The release profiles of EA from EAN using 0.1 M Na₂CO₃ and 0.1 M Na₃PO₄ separately and free EA are shown in Figure 8. As can be seen from Figures 8C and D, the free EA released quickly into Na₂CO₃ and Na₃PO₄ solutions, the release being completed within 26 and 18 minutes in Na₂CO₃ and Na₃PO₄, respectively. The release rate of EA from EAN is obviously lower than the free EA, indicating that the EAN is a potential controlled-release drug system. The release of EA from the nanohybrid is obviously dependent on the types of anion in aqueous solution for ion exchange. It is worth noting that the rapid release during the first 5 hours is followed by a more sustained release of the EA, and 44% and 85% of EA was released from ZLH by Na₂CO₃ and Na₃PO₄ aqueous solution, respectively. A slower release was observed from 5 to 38 hours. The amount of EA released from EAN into aqueous solutions containing Na₃PO₄ was found to be higher than the Na₂CO₃, as shown in Figure 8B. The amount of EA released from the aqueous solution at 38 hours was 94% (Table 2 and Figure 8) for Na₃PO₄ compared with about 69% for Na₂CO₃. Because we know that the more negative charge of phosphate anion will give a higher affinity for ion exchange with the intercalated EA anion, more release of EA is expected, and this is parallel to the release profiles observed in Figure 8.

Figure 8.

Release profiles of EA from the EAN in the aqueous solution containing 0.1 M Na₂CO₃ (A) and 0.1 M Na₃PO₄ (B). Inset shows release of free EA into Na₂CO₃ (C) and Na₃PO₄ (D).

Abbreviations: EA, ellagic acid; EAN, ellagic acid nanohybrid.

In order to obtain more information on the release behavior of EA from EAN, zeroth-, first-, pseudo-second-order kinetics and parabolic diffusion, were chosen to investigate the release kinetics of EA from the nanohybrid. The equations are given in Table 2. On the basis of the four models, the fitted results of EA release profiles are given in Figure 9 and Table 2. It can be seen that the pseudo-second-order model can be better fitted to the data of the EA release behavior than the other models. Figures 9C and G show the plots of t/q_t versus t for the release of EA into Na₂CO₃ and Na₃PO₄ solution, respectively. For the Na₂CO₃, the correlation coefficient (R²) and k valves are 0.9985 and 0.0044, respectively, compared with 0.9996 and 0.0175, respectively for Na₃PO₄. The saturated release amount, correlation coefficient (R²) and rate constant for pseudo-second-order model are also given in Table 2. This study indicates that EAN synthesized in this work shows controlled-release properties.

Figure 9.

Fitting of the data of EA released from the EAN into solution to the zeroth-, first-, pseudo-second-order kinetics, and parabolic diffusion for 0.1 M Na₂CO₃ (A, B, C, and D respectively) and Na₃PO₄ (E, F, G, and H, respectively).

Abbreviations: EA, ellagic acid; EAN, ellagic acid nanohybrid; ZnO, zinc oxide.

In vitro bioassay

Figure 10 and Table 3 show the effect of free EA, EAN, and ZnO on the viability, using rat hepatocytes cells at various incubation times of 0, 0.5, 1, 3 and 6 hours and at a concentration of 25 μg/mL. As shown in Figure 10, EA has a mild cytotoxic effect on the viability of the hepatocyte cells, similar to ZnO. Interestingly, the EAN also has a mild effect on the hepatocyte cells similar to that of free EA.

Figure 10.

The effect of EA, EAN, and ZnO on the viability of rat hepatocyte cells at the concentration of 25 μg/mL.

Abbreviations: EA, ellagic acid; EAN, ellagic acid nanohybrid; ZnO, zinc oxide.

Table 3.

Viability of hepatocytes during incubation with EA and EAN

	0 h	0.5 h	1.0 h	3.0 h	6.0 h
Control (1% DMSO)	97.4 ± 1.0aw	96.8 ± 0.8aw	96.2 ± 1.4aw	94.3 ± 1.2aw	92.5 ± 1.6ax
25 μg/mL EA	98.2 ± 1.0aw	94.3 ± 1.3ax	92.5 ± 1.2bx	89.4 ± 2.4by	83.4 ± 2.5by
25 μg/mL EAN	97.3 ± 1.1aw	94.8 ± 0.8ax	90.5 ± 1.8by	85.3 ± 4.3bz	77.2 ± 5.7cz
25 μg/mL ZnO	96.7 ± 1.5aw	93.2 ± 1.0bx	88.5 ± 1.3cy	84.3 ± 5.7by	73.4 ± 6.2cz

Notes: N = 3. Values are mean ± SD. Means with different superscript (a–c) differs significantly (P < 0.05) by ANOVA and Duncan multiple post-test in the same column and (w–z) differs significantly in the same row.

Abbreviations: EA, ellagic acid; EAN, ellagic acid nanohybrid; ZnO, zinc oxide.

A closer look at Table 3 shows no significant toxic effect of EAN on the rat hepatocytes cells up to 6 hours, which indicates that EAN can be further used in the study using cancer cell lines.

Conclusion

This study shows that EA can be intercalated into the interlayer of ZLH under nonaqueous environment by direct reaction with ZnO for the formation of organic–inorganic nanohybrid. The resulting nanohybrid was obtained using 0.025 M EA. The obtained nanohybrid shows a basal spacing of 10.4 Å, which confirms the successful intercalation of EA into the interlayer of ZLH. In addition, FTIR and elemental analyses (CHNS) studies supported the intercalation of EA into ZLH interlayers for the nanohybrid formation, EAN. It was also found that the BET surface area declined from 6.4 to 3.6 m²/g when ZnO is transformed to EAN. The high loading of EA molecules inside the interlayers of about 58.8% is useful for controlled-release purposes, and the controlled-release study showed the drug active, EA was released in a controlled manner. The EAN has a mild effect on the hepatocyte cells similar to its counterpart, free EA, which indicates that the EAN can be further used in the study on cancer cell lines.