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Brazilian Archives of Biology and Technology

Print version ISSN 1516-8913On-line version ISSN 1678-4324

Braz. arch. biol. technol. vol.61  Curitiba  2018  Epub Nov 14, 2018

http://dx.doi.org/10.1590/1678-4324-2018170809 

Biological and Applied Sciences

A Simple and High-yield Synthesis of Hexadecyl Ferulate and Its In Vitro Antioxidant Potential

Jessica Nadal 1   * 

Flávia de B. Pedroso 1  

Bruno Rodrigo Minozzo 1  

Priscilla Salles de Brito 1  

Paulo Vitor Farago 1  

José Carlos Rebuglio Vellosa 2  

Edmar Miyoshi 1  

1Universidade Estadual de Ponta Grossa - Departamento de Ciências Farmacêuticas, Ponta Grossa, Paraná, Brasil.

2Universidade Estadual de Ponta Grossa - Departamento de Análises Clínicas e Toxicológicas

ABSTRACT

Ferulic acid (FA) is a phenolic compound with well-known antioxidant potential that can be used as a promising anti-inflammatory and anti-cancer molecule. Furthermore, it has been reported to have neuroprotective activity. One of the main problems, which limit its clinical use, is its low bioavailability when administered orally. This limitation can be circumvented by changes in their structure and/or for preparing lipid-based formulations. The aim of this study was to synthesize a derivative of FA, the hexadecyl ferulate (HF). This compound would be more susceptible to pass through blood-brain barrier (BBB) due to its lipophilic character. The HF was obtained by Steglich esterification and yielded 76.77 ± 1.35%. Its structural characterization was performed by spectroscopic methods of Fourier-transformed infrared spectroscopy (FTIR) and nuclear magnetic resonance (NMR). FTIR spectrum of HF presented two typical bands of ester group, a C=O ester stretching band at 1725 cm-1 and a C-O stretching band at 1159 cm-1. The 1H and 13C spectral data confirmed the chemical structure of HF. Regarding the 13C NMR spectrum, HF showed a chemical shift at δ 167.39 ppm which corresponded to the carbonyl carbon of the ester group. Concerning the in vitro antioxidant potential, HF had equivalent or improved scavenger activity than FA leading to IC50 values of 0.083 ± 0.009 nmol.mL-1 and 0.027 ± 0.002 nmol.mL-1 in DPPH radical scavenging and ABTS radical cation decolorization assays, respectively. Further studies are required in order to investigate the antioxidant effect of HF in biological media.

Keywords: ABTS•+ assay; DPPH• assay; ferulic acid derivative; scavenger activity; Steglich esterification

INTRODUCTION

Ferulic acid (FA; C10H10O4; MW: 194.18 Da) or (E)-3-(4-hydroxy-3-methoxy-phenyl)prop-2-enoic acid is an organic compound widely available in plants which has low toxicity. It is biosynthesized from shikimate pathway via phenylalanine or L-tyrosine1. In nature, FA is usually found as component of plant cell walls offering linkage with lignin; in arabinoxylans, FA is esterified to the C-5 of α-larabinofuranose; in pectins, it is esterified to the C-2 of α1➔5-linked arabinofuranose or to the C-6 of β1➔4-linked galactopyranose, while in xyloglucans, it is found attached to the C-4 of α-D-xylopyranose2,3.

FA exhibits a wide range of therapeutic effects against various diseases such as cancer, diabetes, and cardiovascular and neurodegenerative disorders4. A wide spectrum of beneficial activities for human health has been proposed for this phenolic compound, at least in part because of its strong antioxidant activity. Considering the effect of FA in central nervous system (CNS), it can attenuate neuronal cell death due to uptake of oxidized low-density lipoprotein, which is generated by reactive oxygen species (ROS)5. Due to its phenolic nucleus and an extended side-chain conjugation, it readily forms a resonance-stabilized phenoxyl radical, which accounts for its potent antioxidant effect6.

In spite of some papers devoted to obtain possible medicines containing FA, the unfavorable pharmacokinetics, which reduces the bioavailability of FA after oral administration and the restricted number of clinical studies carried out with the purpose of proving FA efficacy and safety7, are the main aspects that limit its use as an antioxidant drug in humans. In order to avoid these gaps, changes in its structure and by the preparation of lipid-based formulations have been proposed8. However, these problems are more complex when a brain targeting drug delivery system is intended to be achieved. However, there has hitherto been observed a restricted evidence for in vivo permeation of the blood-brain barrier (BBB) by FA. Based upon in vitro results, FA crosses the BBB, but exhibits a lag time9.

Many drugs, when employed with no chemical or physicochemical modification, result in reduced pharmacological effects on the CNS due to the difficulty in crossing the BBB. For circumventing this limitation, lipophilization of molecules is an attractive way for increasing the lipophilic properties of a drug. In other words, an active substance is modified by masking polar groups with nonpolar groups, thereby converting a more water-soluble substance to a lipophilic drug10.

To address this problem, there are few literature reports devoted to the synthesis of lipophilic derivatives from FA. An intermediate vinyl ferulate was first chemically produced by the enzymatic synthesis and subsequently esterified with phytosterols through alcoholysis with Candida rugosa as a catalyst6. Similarly, an optimized synthesis of novel prenyl ferulate was performed by feruloyl esterases from Myceliophthora thermophila in microemulsions3. A solvent-free and reduced pressure evaporation system was developed for lipase-catalyzed synthesis of 2-ethylhexyl ferulate from FA and 2-ethylhexanol11. Sandoval and co-authors (2015)12 synthesized monoesters were further acylated with vinyl esters in order to obtain FA diesters with significantly increased hydrophobicity, which could benefit their performance in food, pharmaceutical, and cosmetic applications.

In this study, we propose to synthesize a monoester by the Steglich esterification13, which is a simple and high-yield reaction in order to obtain hexadecyl ferulate (HF), a more lipophilic compound from FA. This derivative substance could keep the scavenging activity of FA at the same time it could present a promising improved behavior in biological systems as CNS. To the best of our knowledge, esterification of FA to its derivative HF has not yet been reported in the literature. In addition, the goal of this paper was to perform a complete characterization of this ester in order to investigate its antioxidant activity by some in vitro scavenging models.

MATERIALS AND METHODS

Materials

Ferulic acid 99.80% (FA) was purchased of Suzhou Leader Chemical Co. Ltda. (Suzhou, China). Cetyl alcohol 99% (CA), N,N’-dicyclohexylcarbodiimide (DCC, 99%), 4-dimethylaminopyridine (DMAP, ≥ 99%) and quercetin (≥ 95%) were obtained from Sigma-Aldrich (St. Louis, MO, USA). Water was purified in a Milli-Q Plus water purification system (Millipore, Bedford, MA, USA). All others reagents and solvents were of analytical grade and were used as received.

METHODS

Synthesis of hexadecyl ferulate

As a chemical strategy for synthesizing the FA ester, CA, a long alkyl chain (16 carbons) alcohol, was used. The reaction between FA (1) and CA (2) was developed using 1,3-dicyclohexylcarbodiimide (DCC) (3) as a dehydrating agent and coupling reagent in tetrahydrofuran (THF) (4) and 4-dimethylaminopyridine (DMAP) (5) as a catalyst, based on the paper previously published by Neises and Steglich (1978)13. The Steglich esterification was used as a mild reaction consisting of using DCC/DMAP system in order to obtain the final ester (HF) (6) and the by-product dicyclohexylurea (DCU) (7) (Figure 1).

Figure 1 Scheme of Steglich esterification for preparing HF 

In brief, 50 mL of THF was added to a round bottom flask. Then, 2.0 g (10.3 mmoL) of FA and 12.48 g (51.5 mmoL) of AC were dissolved. Catalytic amounts of DMAP and 2.12 g (10.3 mmoL) of DCC were added to the previous solution. The atmosphere was replaced by nitrogen and the reaction mixture was kept under magnetic stirring and nitrogen flow for 12 h at 20oC. After this time period, the reaction mixture was filtered twice using cotton for removing DCU. The final solution was then transferred to a round bottom flask for solvent removal using a rotary evaporator. This procedure was carried out from five independent batches.

Purification of hexadecyl ferulate

The final product was purified by column chromatography (50 X 500 mm) filled with silica gel (230 mesh, 0.063-0.200 mm, Merck Millipore, Billerica, MA, USA) as the stationary phase at the silica:sample 10:1 (w:w) ratio. The elution was carried out by solvent passing using the hexane:ethyl acetate proportions with increasing order of polarity (100:0, 90:10, 80:20, 70:30, v:v) as mobile phase.

Thin layer chromatography (TLC) was used to analyze the fractions obtained by column chromatography. The silica gel 60 F254 (Merck Millipore, Billerica, MA, USA) and hexane:chloroform:ethyl acetate (70:20:10, v:v:v) were used as stationary and mobile phases, respectively. Vanillin and ferric chloride were used as colors reagents for detecting the spots. The substances under analysis (FA, CA and HF) were evidenced by the use of UV radiation at 254 and 366 nm. The fractions containing a single spot on TLC plate were mixed and chosen for further analyses. These groups of fractions were dried for 2 days by freeze drying at -40°C and 400 µHg vacuum. The final product HF was stored into a desiccator under vacuum at room temperature.

Yield

The gravimetric yield was determined by weighing the final product purified and by dividing this experimental value by the theoretical value calculated using stoichiometry. The results were expressed as mean ± standard deviation (SD).

Characterization of hexadecyl ferulate

The ester product was characterized by spectroscopic methods in order to confirm its chemical structure.

Fourier-transformed infrared spectroscopy (FTIR)

The Fourier-transformed infrared spectra of FA, CA and HF were recorded from 4000 to 400 cm-1 on a Shimadzu IR Prestige-21 spectrophotometer (Kyoto, Japan) using KBr pellets with 32 scans and resolution of 4 cm-1.

Nuclear magnetic resonance (NMR) spectroscopy

For structural elucidation of HF, the 1H and 13C NMR spectra were collected on a Bruker Avance DRX-400 instrument operated at 9.4 T for observing 1H at 400.13 and 13C at 100.61. The TMS shift signal was used as the internal reference (δ = 0 ppm). The spectrometer was equipped with a multinuclear direct detection 5 mm probe for recording 1H and 13C spectra. Deuterated chloroform was used for samples dilution.

In vitro antioxidant potential

In order to compare the antioxidant capacity of pure FA and HF, the antioxidant potential was evaluated by 2,2-diphenyl-1-picrylhydrazyl (DPPH•) radical scavenging assay and 2,2-azinobis(3-ethylbenzothiazoline-6-sulfonic acid) (ABTS) radical cation decolorization. Aqueous solutions of pure drug and HF (0.1 and 50 μg.mL-1) were prepared 30 min before starting the experiments and kept under dark conditions.

DPPH• radical scavenging assay

The antioxidant effect of the samples was tested against 60 μM of the stable radical DPPH• (2,2-diphenyl-1-picryl-hydrazyl) solubilized in absolute ethanol. The medium was composed by each sample in concentrations between 0.1 and 50 μg.mL-1, DPPH solution and absolute ethanol as reaction medium for obtaining 1000 μL. The mixture was incubated for 15 minutes at room temperature and protected from light. The scavenger action was observed by decreasing the absorbance at λ = 531 nm17.

ABTS radical cation decolorization assay

The cationic radical ABTS•+ (2,2"-azinobis(3-ethylbenzothiazoline-6-sulfonic acid)) was prepared by reacting 5 mL of ABTS•+ aqueous solution (7 mM) with 88 μL of persulfate of potassium (2.46 mM) at room temperature, protected from light, for 12 to 16 hours prior to its use18. Prior to the assay, the ABTS•+ solution was diluted with 10 mM sodium phosphate buffer (1:20 ratio). Samples at concentrations between 0.1 and 50 μg.mL-1 were added to the plates together with ABTS•+ and 100 mM sodium phosphate buffer in order to obtain a final volume of 1000 μL of reaction medium. The reduction between ABTS•+ and pure drug or HF was measured by decreasing the absorbance at λ = 734 nm after 15 min.

All measurements were performed in triplicate using a microplate reader (SpectraMax 190 spectrophotometer, Molecular Devices, Sunnyvale, CA, USA). Quercetin (≥ 95%) was used as positive control. The antioxidant activity was calculated as percentage of inhibition according to the Equation 1.

%Inhibition=[(AbAa)Ab]x 100 (1)

Where Ab is the absorbance of the control and Aa is the absorbance of the sample.

Statistical analysis

Data were expressed as mean ± standard deviation (SD) using Graph Pad Prism version 6.0 for windows, Graph Pad Software (San Diego, CA, USA). Statistical analysis was performed by ANOVA followed by Bonferroni’s post-hoc test and a p value lower than 0.05 was considered as statistically significant. The 50% inhibitory concentration (IC50) was calculated from the dose response curve (Graph Pad Prism Version 6.0) obtained by plotting percentage inhibition versus concentrations.

RESULTS AND DISCUSSION

Synthesis of hexadecyl ferulate

FH was successfully obtained as an off-white powder by the Steglich esterification. This process provided a mild reaction medium since it was kept at low temperature under an inert atmosphere13. In addition, the resulting water reacted with DCC for obtaining the by-product DCU which avoided the ester hydrolysis by water.

Purification of hexadecyl ferulate

Two bands were observed during purification which suggested the separation of two fractions when the eluent hexane:ethyl acetate at 80:20 proportion passed through the column. HF was the first compound purified. It was detected by UV and confirmed by TLC with a retention factor of 0.69. After solvents’ evaporation, HF was obtained as a white powder.

Yield

A yield of 76.77 ± 1.35% was obtained after synthesis and purification of hexadecyl ferulate. This yield is in accordance with those reported in literature for esterification reactions13. Bernards and Lewis (1992)19 obtained yields lower than 25% and 66% using DCC and DCC after the addition of a labile acid as a shielding reagent to the free FA hydroxyl group, respectively. Another study, which carried out the esterification of FA by means of biocatalysts, reached yields between 44 and 56%20. These results reinforce the efficacy of the Steglich esterification for preparing HF using DCC and DMAP as a catalytic agent.

Characterization of hexadecyl ferulate

Fourier-transformed infrared spectroscopy (FTIR)

FTIR spectra performed for FA, CA and HF are shown in Figure 2. The FTIR spectrum for pure FA consisted of absorption bands of OH group stretching vibration (3441 cm-1), aromatic and alkene C-H stretching vibrations (3018 cm-1), alkane C-H stretching vibration (2974 cm-1), aromatic conjugated C=O stretching vibration (1691 cm−1), C=C aromatic stretching vibration (1620, 1598, 1516, 1431 cm-1), C-O-C asymmetric stretching vibration (1273 cm-1), and C-OH stretching vibration (1205 cm-1). Concerning CA, its infrared spectrum exhibited two bands at 2850 and 2920 cm-1 due to symmetric and asymmetric -CH2 stretching, respectively. A broad band assigned to -OH stretching was observed between 3360 and 3236 cm-1. HF showed a FTIR spectrum presenting two typical bands of ester group (Figure 2). HF demonstrated a C=O ester stretching band at 1725 cm-1 (a) and a C-O stretching band at 1159 cm-1 (b) which confirmed that FA ester was obtained. Moreover, the broad band between 3360 and 3236 cm-1 (c) assigned to -OH stretching of CA was not observed in HF which suggested that this hydroxyl group was consumed for ester synthesis. Therefore, these FTIR assignments suggest that the synthesis of FA ester was successfully performed by the previously described Steglich esterification.

Figure 2 FTIR spectra of ferulic acid (FA), cetyl alcohol (CA) and hexadecyl ferulate (HF). 

Nuclear Magnetic Resonance Spectroscopy (NMR)

The 1H and 13C NMR spectral data confirmed the chemical structure of HF. Considering 1H NMR spectrum of HF (Figure 3), 1H chemical shifts of the protons of the aromatic ring were assigned at δ 7.08 (i) , 7.05 (l) and 6.94 (m) ppm and a shift signal at δ 4.22 (d) ppm corresponded to the hydrogens of the first carbon in the ester alkyl chain which suggested that the ester group was obtained. Besides, the other signals of chemical shifts between δ 1.72 and 0.88 (a,c) ppm were assigned to the hydrogens of the other carbons in the alkyl chain. Regarding the 13C NMR spectrum (Figure 4), HF showed a chemical shift at δ 167.39 (e) ppm which corresponded to the carbonyl carbon of the ester group and confirmed the synthesis of FA ester.

Figure 3 1H NMR spectrum of HF. 

Figure 4 13C NMR spectrum of HF. 

In vitro antioxidant potential

In order to explore whether the structural modification has influence on antioxidant capacity, the profile of action of FA and HF on the free radical DPPH• and the reactive oxygen species ABTS•+ were compared at different concentrations.

DPPH• radical scavenging assay

DPPH• is a stable radical widely used in antioxidant trials in the field of organic compounds and natural products. HF proved its antioxidant potential leading to a half maximal inhibitory concentration (IC50) of 0.083 ± 0.009 nmol.mL-1 while FA achieved a higher IC50 value of 0.160 ± 0.010 nmol.mL-1. Therefore, HF reached a scavenger activity in statistically lower concentrations than FA which differs that reported by Anselmi et al. (2004)14. These authors investigated the scavenger activity of some different alkyl esters of FA on DPPH• radical scavenging assay and showed no significant differences between FA and its derivatives compounds. Quercitin is a well-known antioxidant standard21 and showed an IC50 of 0.030 ± 0.001 nmol.mL-1. This flavonoid presented an improved scavenger activity that was statistically different than HF and FA.

ABTS radical cation decolorization assay

The cationic radical of ABTS•+ is a synthetic nitrogen-substituted aromatic compound widely used to evaluate the abilities of phenolic agents as radical scavengers18. Considering their % of inhibition (Figure 5), HF (99.74 ± 4.68% at 0.05 nmol.mL-1), FA (98.41 ± 0.53% at 0.01 nmol.mL-1) and quercitin (98.66 ± 0.33% at 0.007 nmol.mL-1) showed no statistically significant difference on scavenging activity as previously reported Menezes et al. (2011)22. In spite of HF showed the higher % of inhibition, this FA ester achieved an IC50 value of 0.027 ± 0.002 nmol.mL-1 while FA and quercitin demonstrated 50% of inhibition at lower concentrations of 0.005 ± 0.001 and 0.002 ± 0.001 nmol.mL-1, respectively. This could be justified by the spatial conformation, arrangement and reaction behavior of HF after Steglich esterification14.

Figure 5 Antioxidant effect of ferulic acid (FA), hexadecyl ferulate (HF) and quercetin by ABTS•+ radical cation decolorization assay. 

In addition, further studies are required in order to investigate the antioxidant effect of HF in biological systems. According to literature14, HF makes it less susceptible to interacting, through van der Walls, with the phospholipids of membrane and remains anchored therein when compared to other alkyl esters ferulic acid derivatives. Comparing the partition coefficient (log P) values of HF and FA (8.86 and 1.25, respectively), HF would be more susceptible to BBB transpose due to a close relationship between the log P of a drug and its permeability in BBB15. In addition, some reports suggest that the compound solubility in lipids can be an important factor for the suppression efficiency of lipid oxidation and that alkyl chain ferulates would be more promising antioxidants than FA16.

CONCLUSION

The synthesis of HF was successfully performed from FA by Steglich esterification. This FA ester was confirmed by FTIR and 1H and 13C NMR spectra. HF demonstrated an equivalent or improved antioxidant potential than FA by the free radical DPPH• and reactive oxygen species ABTS•+ assays.

ACKNOWLEDGEMENTS

The authors thank to Conselho Nacional de Pesquisa e Desenvolvimento (CNPq) for financial support (grant number 456403/2014-0). The authors have no direct relation or financial involvement with any commercial organization with interest in the subject or materials discussed in this paper.

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Received: December 22, 2017; Accepted: July 02, 2018

*Author for correspondence: jessicabem@hotmail.com

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