A Kinetic Approach in the Evaluation of Radical-Scavenging Efficiency of Sinapic Acid and Its Derivatives.

A kinetic approach was used to determine the radical scavenging activities of sinapic acid and its derivatives: sinapine, 4-vinylsyringol, syringic acid, syringaldehyde, and ethyl, propyl and butyl sinapate. The responses were expressed as rates of 2,2-diphenyl-1-picrylhydrazyl radical (DPPH˙) scavenging (RS), superoxide radical (O₂˙-) scavenging (RFF), and β-carotene bleaching in the emulsion system (RB). For RS and RB, the esters of sinapic acid showed the highest responses while, for RFF, this was seen for syringic acid. The effectiveness of the selected compounds for scavenging these free radicals was also determined at a fixed endpoint. The early response parameters were demonstrated to be good discriminators in assessing differences for antioxidants with comparable fixed endpoint activity. The primary feature that ranks the kinetic data and the endpoint determinations is interpreted in terms of the mechanisms of the reactions involved in each of the assays conducted.

1. Introduction

<span class="Chemical">Phenolic compounds are considered to be great contributors to the health effects of plant-based diets mostly due to their ability to scavenge <span class="Chemical">free radicals. For that reason they are extensively investigated for their antioxidant activity. Most of the in vitro methods for characterization of the radical scavenging properties of phenolic compounds concentrate on stoichiometric aspects at a fixed reaction time when steady-state is reached and, thus, they do not define the early responses of an antioxidant in a particular system [1]. Bearing in mind that free radicals such as hydroxyl (HO˙), hydroperoxyl (HOO˙) and lipid (RO(O)˙) radicals are short-lived in foods and tissues, long-term incubations can ignore the initial fast reactions, and instead give weight to the slower side reactions [2]. A significant aspect in the determination of antioxidant activity of phenolic compounds would also be the reactivity in terms of the response of an antioxidant at the early steps of the process [3], which is related to the kinetics of the free radical quenching [4] and is conditioned by the reaction mechanism.

The scavenging of <span class="Chemical">free radicals by antioxidants can occur by two major mechanisms: <span class="Chemical">hydrogen atom transfer (HAT) and electron transfer (ET). In addition, transitional mechanisms are also possible, which include proton-coupled electron transfer (PCET), electron transfer-proton transfer, (ET-PT), and sequential proton loss electron transfer (SPLET) [5,6,7]. According to Wright et al. [8] HAT and ET mechanisms must always occur in parallel, but with different rates. Which mechanism is going to be primary (i.e., with a higher rate) depends on the molecular properties of the antioxidant, the radical species involved, and the nature of the solvent, and while the end result is the same, the kinetics and the prospective for side reactions differ [5].

As far as the molecular properties of an antioxidant are concerned, thermodynamic parameters, such as bond dissociation energy (<span class="Chemical">BDE), ionisation potential (IP), proton affinity (PA), and electron transfer enthalpy (ETE) are of specific importance in the determination of which mechanism is the favoured one in the scavenging of free radicals [9,10,11]. With the HAT mechanism, which involves quenching of free radicals by the donation of a hydrogen atom, the BDE of the O–H bond is a major factor for the scavenging activity, as it is related to the stability of the phenoxyl radical (ArO˙). In the ET mechanism, the IP is the most significant parameter in the evaluation of scavenging activity, as it implicates single electron transfer from an antioxidant to a free radical, and the stability of the thus-formed radical cation (ArOH˙+). The lower the IP, the easier the electron abstraction is. Extended delocalisation and conjugation of the π-electrons enhanced by resonance effects and planarity favour lower IP values and strongly influence the ability of phenolic antioxidants to donate a single electron [9]. The SPLET mechanism, a two-step process, includes deprotonation of an –OH group of a phenol, with formation of a phenoxide anion (ArO), which can be characterised by the PA [12]. This then undergoes oxidation to ArO˙ as the second step of the reaction, which is related to the ETE [11]. These thermodynamics parameters are affected by the inductive effects of the substituents attached to the phenolic ring. BDE, IP, and ETE are lower with electron-donating groups (i.e., with positive inductive effects, +I), and increased with electron-withdrawing groups (i.e., with negative inductive effects, −I). The opposite effect can be noted in the case of the PA. Electron-withdrawing groups facilitate deprotonation of an –OH group, and electron-donating groups have the opposite effect [10].

In addition, the nature of the reaction medium also influences the mechanism through which the reaction would take place. For example, <span class="Chemical">hydrogen bond accepting solvents (e.g., <span class="Chemical">methanol, ethanol) strongly influence the rate of hydrogen abstraction from a phenolic compound, by decreasing it and, thus, favouring electron transfer processes [13].

In recent years, <span class="Chemical">sinapic acid (<span class="Chemical">SA; i.e., 3,5-dimethoxy-4-hydroxycinnamic acid), and some of its derivatives, have been investigated because of their various biological activities, as reviewed by Nićiforović and Abramovič [14]. The aim of the present study was to investigate the radical-scavenging efficiency of SA and its derivatives: sinapine (SI; i.e., 3,5-dimethoxy-4-hydroxy-cinnamoyl choline), 4-vinylsyringol (VS; 3,5-dimethoxy-4-hydroxystyrene, also known as canolol), sinapoyl esters (e.g., ethyl [SE], propyl [SP], butyl [SB] sinapates), syringic acid (SY), and syringaldehyde (SYA; 4-hydroxy-3,5-dimethoxybenzaldehyde) (Figure 1) from the kinetics perspective. For this purpose, the scavenging activities of the selected phenolic compounds were analysed in terms of the 2,2-diphenyl-1-picrylhydrazyl (DPPH˙) radical, the superoxide radical (O2˙−), and lipid radicals generated in the β-carotene-linoleic acid emulsion system. The results obtained by this kinetics approach which provides the early rates of DPPH˙, O2˙− and lipid radical scavenging for these selected compounds were compared to the conventional stoichiometry calculations obtained at a fixed endpoint. The ranking of these data is interpreted in terms of the reaction mechanisms of each assay, according to the structure and chemical properties of SA and its derivatives.

Figure 1

Structures of sinapic acid (SA) and its selected derivatives: ethyl sinapate (SE), propyl sinapate (SP), butyl sinapate (SB), sinapine (SI), 4-vinylsyringol (VS), syringaldehyde (SYA), and syringic acid (SY).

2. Results and Discussion

2.1. DPPH˙ Radical Scavenging Activity

<span class="Chemical">DPPH˙ <span class="Chemical">radical undergoes a colour change from purple to yellow upon receiving an electron or hydrogen from an antioxidant, and the effects of the investigated antioxidant can be estimated by measurement of the decrease in its absorbance at 517 nm. To determine the early responses of the selected antioxidants towards DPPH˙ radicals, the change in absorbance at 517 nm (Ac517nm( − As517nm() was plotted as a function of time (Figure 2A). The value Ac517nm( − As517nm( refers to the content of the DPPH˙ radical scavenged at t = x. The dependence of Ac517nm( − As517nm( on t was quantified for the first 100 s of each incubation, and is described by the power function given in Equation (1): where y is Ac517nm( − As517nm(.

Figure 2

(A) Dependence of Ac517nm( − As517nm( on time of incubation at 6.67 × 10−5 mol/L of each tested compound; (B) dependence of As560nm( on time of incubation at 5 × 10−3 mol/L of each tested compound; and (C) dependence of As470nm( − As470nm( on time of incubation at 2 × 10−4 mol/L of each tested compound. (■), sinapic acid—SA; (○), syringic acid—SY; (▲), syringaldehyde—SYA; (●), ethyl sinapate—SE; (∗), propyl sinapate—SP; (◊), butyl sinapate—SB; (◁), 4-vinylsyringol—VS; (▼), and sinapine—SI.

The curves in Figure 2 were plotted on the basis of param<span class="Chemical">eters and of Equation (1), which were obtained by non-linear regression analysis. The corresponding d<span class="Chemical">etermination coefficients (r2) are presented in Table 1. The kinetics of the scavenging DPPH˙ radicals were quantified by the estimation of the rate of DPPH˙ scavenging (RS), as the first derivative of the power function given in Equation (2), with the results from these data given in Table 1.

Table 1

The rates of DPPH˙ radical scavenging (RS) at 0.1 s, the formazan formation (RFF) at 10 s, and the β-carotene bleaching (RB) at 10 s, and the determination coefficients for the kinetics of the DPPH˙ radical scavenging (r2 (DPPH˙)), the O2˙− scavenging (r2 (O2˙−)), and the β-carotene bleaching (r2 (β-carotene)). The data for the DPPH˙ scavenging activity (IDPPH) estimated at 30 min, the superoxide radical scavenging activity coefficient (CSASA) estimated at 5 min, and the antioxidant activity coefficient in emulsion (CAA) estimated at 60 min. Chromatographic partition values (CPV) are also given.

Selected Compound	RS × 10−2 (s−1)	RFF × 10−3 (s−1)	RB × 10−4 (s−1)	r2 (DPPH˙)	r2 (O2˙−)	r2 (β-Carotene)	IDPPH (%) a	CSASA (%) a	CAA (%) a	CPV
Sinapic acid (SA)	15.40	1.57	10.54	0.946	0.967	0.978	86 ± 0.4	66 ± 4	29 ± 2	0.46
Sinapine (SI)	0.27	14.21	7.62	0.967	0.996	0.967	23 ± 0.5	0	2 ± 0.5	0.20
Vinyl syringol (VS)	34.83	2.31	7.33	0.967	0.965	0.984	74 ± 0.6	26 ± 1	60 ± 1	0.73
Syringic acid (SY)	1.21	0.92	4.78	0.962	0.953	0.975	80 ± 1	75 ± 0.1	6 ± 1	0.34
Syringaldehyde (SYA)	0.05	6.37	3.37	0.447	0.981	0.968	6 ± 0.6	23 ± 3	1 ± 0.2	0.40
Ethyl sinapate (SE)	46.27	9.88	6.46	0.901	0.988	0.987	69 ± 1	5 ± 1	62 ± 2	0.90
Propyl sinapate (SP)	81.44	ND	2.79	0.969	ND	0.984	67 ± 1	ND	73 ± 1	1.13
Butyl sinapate (SB)	35.93	ND	1.99	0.875	ND	0.980	67 ± 0.8	ND	75 ± 1	1.38

a Means of two replicates ± standard deviation; ND, not determined.

The same principle was applied for the kinetics of the scavenging of O2˙− and lipid radicals by the investigated SA derivatives.

As the rate of <span class="Chemical">radical scavenging is related to the slope of the curve at a specific time point, and as can be seen, the highest response occurs within the first few seconds, RS was calculated at t = 0.1 s. Among all of the investigated compounds, the highest responses for scavenging of the <span class="Chemical">DPPH˙ radicals were shown by the sinapate esters (SE, SP, SB) and VS, which caused sharp rise in Ac517nm( − As517nm( in the first 5 s of incubation (Figure 2A). This was especially the case for SP, where the increase in Ac517nm( − As517nm( occurred almost instantly, after which the reaction slowed down. In a study on the kinetics of DPPH˙ scavenging, Foti et al. [13] showed, on the example of methyl sinapate, that the introduction of alkyl moiety increases the reactivity of SA, which is in agreement with our results. On the other hand, for SA and SY, the increase in Ac517nm( − As517nm( was more gradual.

The amount of <span class="Chemical">DPPH˙ scavenged by the same concentration of the selected compounds as used in the kinetics study was also determined at the fixed endpoint at 30 min, and expressed as percentage of scavenged DPPH˙ (Table 1, IDPPH). No correlation was found between RS and IDPPH (Figure 3A). When the fixed endpoint was reached, the order of activity was clearly different, with SA and SY scavenging most of the DPPH˙ radicals. The same tendency for the data obtained at a fixed endpoint for SA and its esters were also reported by Teixeira et al. [15].

Figure 3

(A) Dependence of the 30-min endpoint for the DPPH˙ scavenging activity (IDPPH) on rate of DPPH˙ radical scavenging (RS) at 6.67 × 10−5 mol/L of each tested compound; (B) dependence of the superoxide radical scavenging activity coefficient (CSASA) on rate of formazan formation (RFF) at 5 × 10−3 mol/L of each tested compound. (■), sinapic acid—SA; (○), syringic acid—SY; (▲), syringaldehyde—SYA; (●), ethyl sinapate—SE; (∗), propyl sinapate—SP; (◊), butyl sinapate—SB; (◁), 4-vinylsyringol—VS; (▼), and sinapine—SI.

The generally accepted mechanism of oxidation of <span class="Chemical">phenols in a reaction with <span class="Chemical">DPPH˙ in protic solvents, such as methanol or ethanol, is considered as SPLET based. Slower response to DPPH˙ at the early step of the reaction for SA than seen for its esters is ascribed to the suppressive influence of the carboxylate group (–COO−) on the deprotonation of ArOH (Equation (3)). By its electron-donating effects, –COO− increases PA, which decreases RS of SA versus its esters, where the deprotonation of ArOH is supported by the electron-withdrawing effect of the ester moiety (–COOR). This is in accordance with Foti et al. [13]. This suppressive influence of –COO− on the rate of DPPH˙ scavenging was reported by Ordoudi et al. [16], who observed notably higher kinetics determined in ethanol for catechol than for its derivative bearing the –COO− group, protocatechuic acid. On the other hand, at the second step of the process (Equation (4)), where the ETE is the major influencing factor, the effects of the –COO− and –COOR functional groups are opposite. The electron transfer from ArO− to DPPH˙ of esters is surpassed by SA, as it is supported by the +I of –COO−, which stabilises ArO˙ and results in greater activity (i.e., higher IDPPH) of SA than its esters at the fixed endpoint. Based on the PA and ETE given by Chen et al. [11], which were obtained using density functional theory calculations, in the example of ferulic acid and its ethyl ester, where lower PA and higher ETE were calculated for ferulic acid than for ethyl ferulate, it can be expected that SA has a better early response and its ester SE has a greater fixed endpoint DPPH˙ scavenging activity. However, our experimental data, as shown above, indicates the importance of considering the ionic forms of these phenolic acids in polar solvents under pH conditions above pKa values for their –COOH group.

<span class="Chemical">Sinapic acid esters showed the highest Rs of all of the tested compounds, while at the fixed endpoint, their activities were moderate where the presence of an electron-withdrawing –<span class="Chemical">COOR group destabilises their ArO˙, which leads to a possible reversible reaction with DPPH˙ (Equation (4)). This was shown in a study by Foti and Daquino [17], and was confirmed by the flat curves that followed the initial rapid increase in Ac517nm( − As517nm( (Figure 2A). On the other hand, the ArO˙ of SA and SY might be involved in the subsequent slower reactions before equilibrium is reached, which results in a high IDPPH. Namely, as well as the previously-described key reactions of SPLET (Equations (3) and (4)), ArO˙ can undergo the latter slower process to the secondary reactions of the phenol-derived radicals with the remaining DPPH˙, as well as to further chemical reactions among ArO˙ themselves, such as polymerisation or disproportionation (Equations (6) and (7)) [15]. Indeed, it is known that hydroxycinnamic acids can undergo oxidative cross-coupling, which leads to the formation of dimers, some of which have radical scavenging activities themselves [18]. Considering the ranking of the ester early responses towards the DPPH˙ radicals in relation to the alkyl chain length in the –COOR, steric accessibility to the hindered reaction site in DPPH˙ radical has been recognized as an important factor that limits the reaction rate [19,20], and that probably results in the lower Rs of SB than observed for SE and SP.

The absence of an un<span class="Chemical">saturated ethylenic side chain and the closeness of the –<span class="Chemical">COO− group to the –OH group in the molecule of SY increase its suppressive effects on the deprotonation of ArOH, which results in the particularly lowered early rate of the reaction of SY in comparison to SA. This is in accordance to data reported by Ordoudi et al. [16] and Terpinc et al. [4], where the insertion of an ethylenic chain and the formation of a hydroxycinnamic derivative, caffeic acid, resulted in a profound increase in the reaction kinetics as compared to protocatechuic acid. The stabilizing effect of –COO− on ArO˙ due to its proximity to the –OH in SY would be expected to lead to higher activity of SY than SA at the fixed endpoint. However, it appears that this phenomenon in SY is overcome by the absence of the ethylenic side chain, which leads to lower resonance delocalisation (i.e., lower stabilisation of ArO˙), and resulted in a slightly lower antioxidant activity for SY than for SA at the fixed endpoint (i.e., lower IDPPH).

The elimination of the –<span class="Chemical">COO− group in <span class="Chemical">SA results in the formation of VS. The vinyl group in the molecule of VS has high electron density (+I effect), which would also have similar effects to –COO− for deprotonation of ArOH and stabilisation of ArO˙, but would be less effective. This resulted in lower Rs for VS compared to Rs of the esters, although it remained higher than Rs of SA and SY. At the fixed endpoint, the activity of VS with the more stabilised ArO˙ was higher than that of the esters, but lower than for SA and SY, which reveals a less established effect of the vinyl group than –COO−. SYA showed low activity in scavenging DPPH˙ radicals. The strong electron-withdrawing influence of –CHO in the molecule of SYA decreases its overall activity by destabilising ArO˙.

The interrelationship between Rs and <span class="Chemical">IDPPH confirms that the Rs is more affected by the nature of p-substituent on the formation of <span class="Gene">ArO−, while IDPPH is dependent on the stability of ArO˙ and possible secondary reactions. In Figure 3A. it can be seen that Rs is more sensitive to the differences in inductive effect of the p-substituent since its values significantly differ between compounds with comparable IDPPH. This suggests that Rs is a better discriminator than IDPPH in characterisation of antioxidants with similar activity at the fixed endpoint, such as in the case of SE, SP, SB and VS or SA and SY.

2.2. Superoxide Anion Scavenging Activity

<span class="Chemical">Superoxide anion radicals are continuously produced in aerobic cells [21], and although they are not a highly reactive short-lived free <span class="Chemical">radical species, their over-production can lead to cell damage and mutagenesis [22]. In the present study, O2˙− were generated in the aerobic phenazine methosulphate (PMS)—β-nicotinamide adenine dinucleotide (NADH) system and monitored by following the reduction of nitroblue tetrazolium (NBT) (i.e., blue formazan formation). In the presence of an antioxidant, the reduction in NBT is suppressed due to the O2˙− radical scavenging activity of the antioxidant [23]. To follow the kinetics of O2˙− radical scavenging by the selected SA derivatives, the changes in absorbance at 560 nm were monitored for 300 s. The data are plotted as the dependence of As560nm( on t, where As560nm( represents the content of formazan at t = x (Figure 2B.). A slower increase in As560nm( denotes more suppressed formazan formation (whereby O2˙− is more successfully scavenged). The kinetics of O2˙− scavenging of the selected compounds were determined by calculation of the rates of formazan formation (RFF), through the power function model presented in Equation (1), where y denotes As560nm( (the corresponding parameters and were obtained by non-linear regression), and with the use of Equation (2) at t = 10 s (Table 1). The activities of the investigated compounds were also determined at the fixed endpoint, and these are expressed as the coefficient of O2˙− radical scavenging activity (CSASA), calculated as in Terpinc and Abramovič [4].

Contrary to the <span class="Chemical">DPPH˙ scavenging assay, the O2˙− scavenging assay is a competition assay, where the antioxidant (i.e., the SA derivatives) and detector (i.e., NBT) compete for the radical reactive species (O2˙−), as stressed by Balk et al. [24]. This is not the case for the DPPH˙ scavenging assay, because DPPH˙ is both a radical and a detector [5]. Therefore, for the O2˙− scavenging assay, the shapes of the curves cannot be interpreted in the same way as for the DPPH assay, and lower RFF indicates better response of an antioxidant for the scavenging of O2˙− radicals. SY and SA showed the greatest reactivities towards O2˙− radicals among these tested compounds (Table 1). It appears that any modification to the side chain in the p-position to an –OH group in the selected SA derivatives resulted in lower O2˙− radical scavenging. This activity was indeed minor for SE. Due to the low solubilities of SP and SB, these RFF were not determined. The interrelationships between RFF and CSASA (Figure 3B) show good agreement between the determination of O2˙− scavenging activity of these antioxidants at the early stage and at the fixed point of the reaction (i.e., at 5 min). However, in the same way as in the DPPH˙ scavenging assay, a kinetic perspective offers the possibility to find a distinction between two compounds which show corresponding activities at the fixed endpoint, as in the case of VS and SYA. This again shows the greater influence of the nature of the p-substituent on the early response than on the endpoint activity of O2˙− scavenging.

The O2˙− scavenging as<span class="Chemical">say has not been classified into any of the mechanistic models mentioned in the literature. The order of activity here suggests that the reactivity of the investigated compounds towards O2˙− scavenging does not depend on the acid-base equilibrium of the –OH group, which was seen for the <span class="Chemical">DPPH˙ scavenging. In addition, as noted by Halliwell and Gutteridge [25], in aqueous solutions, the proton affinity of O2˙− is low, as its charge density is decreased due to solvation. On this basis, it is reasonable to exclude SPLET as the mechanism of O2˙− quenching in an aqueous environment. The compounds with the greatest activities are those that contained groups with electron-donating properties (e.g., SA, SY, VS), which lowered both BDE and IP and, thus, both of the HAT and ET mechanisms are considered for discussion. However, as explained by Nenadis and Siskos [12], the BDE is affected by local electronic phenomena and not by the whole structure of the compound, while on the other hand, the whole structures influence the IP. There is considerable difference in the reactivities between compounds with electron-donating and electron-withdrawing groups in the p-position to –OH. The +I effect of –COO− of SY and SA, and of the vinyl group in VS, increases their reactivities towards O2˙− by decreasing the IP of the –OH group and stabilising ArOH˙+ (Equation (8)), as opposed to the −I effect of –CHO in SYA and of –COOR in SE. Bearing in mind, as previously noted, that hydrogen bond accepting solvents (in this case the aqueous environment) favour electron transfer processes, it might be expected that O2˙− scavenging would occur through ET mechanism, and the data in the present study support this. Although in this mechanism electron transfer is followed by deprotonation of the radical cation, which leads to the corresponding ArO˙ (Equation (9)), which would be hindered by electron donating groups (e.g., –COO− in SY and SA), the rate-determining step is the electron donation [12]. In agreement with this, no influence of the second step (Equation (9)) on the RFF was noted in the present study.

2.3. Lipid Radical Scavenging Activity

<span class="Chemical">Lipid peroxidation is a crucial step in the pathogenesis of several diseases, as well as a major mechanism that can lead to deterioration of food quality. This process involves the generation of different lipid radical species, which include the highly reactive peroxyl (ROO˙) and alkoxyl (RO˙) radicals [26]. The lipid radical scavenging activities of the investigated SA derivatives were estimated using a β-carotene bleaching assay in a linoleic acid emulsion system. Linoleic acid oxidation is catalysed by heat, and the lipid radicals that are formed react with β-carotene to form a stable β-carotene radical; this results in decreased absorbance at 470 nm. Figure 2C. shows the relationship between As470nm( – As470nm( and time, where As470nm( – As470nm( refers to the β-carotene bleached at t = x. The rate of β-carotene bleaching (RB) was calculated as for the previous two methods, with y in Equation (1) denoting As470nm( – As470nm( (Table 1). A stronger response in lipid radical scavenging in the linoleic acid emulsion system is seen by lower RB. The lipid-radical scavenging efficiencies were also determined at a fixed endpoint (60 min), and are expressed as the antioxidant activity coefficients (CAA) [4].

Whether we consider a food or a biological antioxidant, a notable factor that affects its efficacy and function is its partitioning properties between the <span class="Chemical">lipid and aqueous phases [27]. Due to their hydrophilic nature, <span class="Chemical">hydroxycinnamic acids cannot be used in oil-based environment, which is an important issue in industrial applications, or to be effective as antioxidants in biological systems. Various studies have shown that antioxidants with higher lipophilicity show improved activities in emulsion systems due to their better partitioning properties [28,29]. This allows such antioxidants to be positioned at the water-lipid interface and, thus, to prevent any initial reactions between aqueous radicals and lipids. Nevertheless, the aim here of the present study was to investigate whether the same principle can be applied to the early response of an antioxidant towards lipid radicals (ROO˙, RO˙) in an oil-in-water emulsion system. The interrelationship between RB, CAA and chromatographic partition values (CPV) is given in Figure 4. The majority of the investigated compounds that showed good early responses towards lipid radicals also showed good scavenging activities at the 60 min endpoint, except for SYA, SY, and SI, where the RB values do not commensurate with the CAA values. Among the selected compounds, SB together with SP showed the strongest early response towards lipid radical scavenging. These two compounds also showed the highest CAA, and the highest lipophilicity. It can be seen that the early response is less dependent on lipophilicity, while CAA is well correlated with the CPV.

Figure 4

Interrelationship of the rate of β-carotene bleaching (RB), antioxidant activity coefficient (CAA) and chromatographic partition value (CPV) for the tested compounds (●), with projections of individual correlations (∗), RB vs. CAA; (×), RB vs. CPV; (+), CAA vs. CPV. Sinapic acid (SA), syringic acid (SY), syringaldehyde (SYA), ethyl sinapate (SE), propyl sinapate (SP), butyl sinapate (SB), 4-vinylsyringol (VS), and sinapine (SI).

The reaction of such <span class="Chemical">phenolic compounds with <span class="Chemical">lipid radicals is noted as the HAT mechanism [5]. RO(O)˙ radicals are highly reactive, and the reaction (Equation (10)) is essentially irreversible [30,31]. Therefore, considering the mechanism, as the inhibition of lipid peroxidation by an antioxidant is usually correlated to the BDE, it would be expected that the reactivity towards lipid radicals in heterogeneous systems, such as emulsions, should be increased by functional groups that stabilise ArO˙, such as the –COO− in the molecules of SY and SA. However, in these systems, the distribution of the antioxidant between the oil, interfacial, and aqueous regions becomes a major factor for its activity. Esterification of SA clearly leads to increased lipophilicity, and to both greater early responses and activities at the fixed endpoint, despite the mildly destabilising −I effect of –COOR on the stability of their ArO˙. In addition, as noted by Burton and Ingold [32], the ArO˙ formed according to Equation (10) eventually reacts with a second radical (Equation (11)), and the molecular products thereby formed move the reaction forward. Although SYA, SY, and SI might be reactive towards lipid radicals and be able to scavenge those that are distributed on the surface of lipid droplets, thus showing a moderate early response, they will not distribute themselves within the lipid–water interface resulting in low CAA. In Figure 4 it can be seen that, again, the kinetic parameter RB can assist in differentiation between two compounds with similar CAA, as in the cases of SB and SP or SE and VS.

The reports on the antioxidant activity of SI in the literature are somewhat contradictory [33,34,35,36], while the data from the present study show little or no activities in any of the as<span class="Chemical">says carried out. Esterification of SA with choline evidently reduces its radical-scavenging ability, as introduction of the positive-charged choline contributes to destabilisation of the corresponding ArO˙, which prevents it from donating a hydrogen atom or electron to the free radical species.

3. Methods

3.1. Materials and Reagents

<span class="Chemical">Chloroform and <span class="Chemical">ethanol (96%) were from Merck (Darmstadt, Germany). SA, SY, SYA, β-carotene, DPPH˙ reagent, linoleic acid (95%), Tween 20, NBT, NADH, and PMS were from Sigma (Sigma-Aldrich GmbH, Taufkirchen, Germany). Potassium dihydrogen phosphate (KH2PO4) and di-sodium hydrogen phosphate (Na2HPO4) were from Kemika (Zagreb, Croatia). All of the reagents were of analytical quality.

3.2. Isolation of Sinapine

SI was isolated from kale (<span class="Species">Brassica oleracea) seeds according to the procedure described by Terpinc et al. [37]. Ground seeds were mixed with b<span class="Chemical">oiling water for 5 min, with the mixture shaken at room temperature for 2 h, and then filtered. This water extract was appropriately diluted with carbonate buffer to obtain a neutral pH, and the resulting mixture was filtered through a 0.45-μm membrane filter. SI isolation was carried out by solid phase extraction using Strata-X-CW cartridges (Phenomenex, Torrance, CA, USA), by consecutive passing of methanol, carbonate buffer (pH 7), and then the water extract through the cartridges. SI was captured on the solid phase by the weak cation-exchange mechanism, with the cartridges then washed using water and methanol. The SI fraction was eluted with 4 mL 2% formic acid in 70% methanol (v/v). The final purity of the isolated product was determined by liquid chromatography using photodiode array detection (LC-DAD, Agilent Technologies, Santa Clara, CA, USA), with its structure confirmed by liquid chromatography–mass spectrometry (LC-MS, Agilent Technologies, Santa Clara, CA, USA and Quatro micro API, Waters, Milford, MA, USA) and nuclear magnetic resonance (NMR) spectroscopy (Agilent Technologies, Santa Clara, CA, USA).

3.3. Synthesis of 4-Vinylsyringol

VS was prepared by thermal decarboxylation of <span class="Chemical">SA according to the method of Terpinc et al. [38]. Briefly, <span class="Chemical">SA was dissolved in dimethylformamide, and sodium acetate was added as a catalyst for the decarboxylation. The reaction mixture was heated in an oil bath at 130 °C for 1 h. Milli-Q water was then added, and the product was extracted using diethyl ether. The organic phase was collected and further washed with carbonate buffer at pH 7. After drying with anhydrous Na2SO4, the organic solvent was removed under reduced pressure, and the precipitate was dissolved in methanol.

The product was passed into 500-mg Strata-X cartridges (Phenomenex, Torrance, CA, U<span class="Chemical">SA) that had been previously conditioned with <span class="Chemical">methanol. This was followed by a 50% (v/v) methanol wash, and the product eluted with 50%, 60%, and 70% (v/v) methanol, in this order. The less polar compounds that remained were eluted with 100% methanol. The purity of the individual fractions was determined by LC-DAD. In the next step, the eluates that contained more than 95% VS were combined, adequately diluted, and loaded onto Strata-X cartridges previously conditioned with methanol. This was followed by 25% (v/v) methanol, and elution with 100% methanol. These eluates were filtered through 0.20-μm filters and evaporated to dryness under a vacuum, at 30 °C. The product was weighed and re-dissolved in methanol. The final purity of the synthesised product was determined by LC-DAD. For confirmation of the structure of the synthesised product, LC-MS and NMR analysis were used.

3.4. Synthesis of Sinapoyl Esters

The <span class="Chemical">alkyl esters of <span class="Chemical">SA were synthesised by acid catalysed esterification, using the method of Gaspar et al. [39]. SA (1.0 g) was dissolved in 75 mL of the corresponding alcohol (i.e., ethanol, n-propanol, or n-butanol) containing 1 mL H2SO4, and the solutions were stirred at room temperature for 5 days. The solvents were partially evaporated under reduced pressure, and the mixtures were then extracted with diethyl ether (3 × 75 mL). The organic phases were combined, washed with 10% Na2CO3 solution, and dried over anhydrous Na2SO4. The solvent was evaporated under reduced pressure, and the crude products were purified by recrystallization. The final purities of these synthesised products were determined by LC-DAD, and their structures confirmed by LC-MS and NMR analysis.

3.5. Liquid Chromatography with Photodiode Array Detection

The purities of the synthesised/isolated products were d<span class="Chemical">etermined using LC-DAD (Agilent 1100 binary pump [<span class="Mutation">G1312A], autosampler [G1330B] and a DAD [G]) as follows: the samples (10 μL) were injected onto a reversed-phase C18 column (Gemini; 100 × 2.00 mm; 2.6 µm) that was protected by a guard column (Gemini C18 Security Guard cartridge; 4.0 × 2.0 mm) (Phenomenex, USA). The column thermostat was set at 25 °C. The solvent system used was 0.1% (v/v) aqueous formic acid (solvent A), and acetonitrile (solvent B). A binary gradient was used at a flow rate of 0.25 mL/min, as follows (as % B in A): 0–4 min, 10% B; 4–40 min, 10%–60% B; 40–41 min, 60%–80% B; 41–47 min, 80% B; 47–50 min, 80%–10% B; 50–60 min, 10% B. The chromatograms were recorded from 240 nm to 650 nm.

3.6. Liquid Chromatography–Mass Spectrometry

The mass spectra of the synthesised/isolated products were recorded using a mass selective detector (Quattro micro API; Waters, Milford, MA, U<span class="Chemical">SA) equipped with electrospray ionization (ESI), using a cone voltage of 30 V and a capillary voltage of 3.0 kV for positive/ negative ionisation of the analytes (i.e., ESI+ or ESI− modes). The dry nitrogen for the detector was heated to 300 °C, and the drying gas flow was 400 L/h. The cone gas (nitrogen) flow was 70 L/h. The data were acquired in positive or negative ESI scan modes (in mass range 100–615). The mass spectra for the synthesised and isolated compounds are given in Figure 5.

Figure 5

(A) Mass spectra of the synthesized/isolated sinapic acid derivatives. ESI+: sinapine (SI), m/z 310.36; 4-vinylsyringol (VS), m/z 181.17. ESI−: ethyl sinapate (SE), m/z 251.27; propyl sinapate (SP), m/z 265.32; butyl sinapate (SB), m/z 279.31; (B) Photodiode array detection chromatograms (240–650 nm) of sinapic acid (SA), syringic acid (SY), and syringaldehyde (SYA), and the synthetised/isolated sinapic acid derivatives ethyl sinapate (SE), propyl sinapate (SP), butyl sinapate (SB), sinapine (SI), and 4-vinylsyringol (VS).

3.7. Nuclear Magnetic Resonance Spectroscopy

Nuclear magnetic resonance spectroscopy was performed on an NMR spectrom<span class="Chemical">eter (DD2; Agilent Technologies, <span class="Chemical">Santa Clara, CA, USA) at frequencies of 297.80 MHz (1H) and 74.89 MHz (13C) at 25 °C. The samples were solubilised in deuterated dimethyl sulphoxide (DMSO-d6). The chemical shifts (δ) are referenced to the residual solvent signal of DMSO-d6 and reported in ppm, while the coupling constants (J) are given in Hz (Table 2). The 1H- and 13C-NMR chemical shifts and H–H coupling constants for compounds SI, VS, SE, SP, and SB are given in the Table 2.

Table 2

1H- and 13C-NMR chemical shifts (in ppm) and H–H coupling constants (in Hz) for the synthesized/isolated compounds. s, singlet; b, broad; d, doublet; m, multiplet.

Compound	1H- and 13C-NMR Spectroscopic Data
Sinapine (SI)	δH (297.80 MHz, DMSO-d6): 7.61 (d, J = 15.9, 1H, –CH=), 7.03 (s, 2H, Ar–H), 6.55 (d, J = 15.9, 1H, =CH–), 4.58 (s, 2H, –OCH2), 3.80 (s, 6H, –OCH3), 3.72 (m, 2H, CH2) 3.17 (s, 9H, –NCH3); δC (74.89 MHz, DMSO-d6): 165.93 (C=O), 148.07 (C(3), C(5)), 146.25 (C(β)), 138.82 (C–OH), 124.05 (C(1)), 113.97 (C(α)), 106.45 (C(2), C(6)), 63.97 (CH2), 57.65 (CH2), 56.13 (2× OCH3), 52.99 (N(CH3)3)
4-Vinylsyringol (VS)	δH (297.80 MHz, DMSO-d6): 8.44 (s, 1H, OH), 6.73 (s, 2H, Ar–H), 6.60 (d, J = 17.6, 10.8, 1H, –CH=), 5.67 (d, J = 17.6, 1.1, 1H, =CH2), 5.08 (d, J = 10.8, 1.1, 1H, =CH2), 3.77 (s, 6H, –OCH3); δC (74.89 MHz, DMSO-d6): C(6)), 147.97 (C(3), C(5)), 136.94 (C–OH), 135.73 (=CH), 127.66 (C(1)), 111.34 (=CH2), 103.77 (C(2), C(6)), 55.94 (2× OCH3)
Ethyl sinapate (SE)	δH (297.80 MHz, DMSO-d6): 8.94 (s, 1H, OH), 7.55 (d, J = 15.9, 1H, –CH=), 7.03 (s, 2H, Ar–H), 6.53 (d, J = 15.9, 1H, =CH–), 4.16 (q, J = 7.1, 2H, –OCH2), 3.80 (s, 6H, –OCH3), 1.25 (t, J = 7.1, 3H, CH3); δC (74.89 MHz, DMSO-d6): 166.55 (C=O), 147.98 (C(3), C(5)), 145.19 (C(β)), 138.23 (C–OH), 124.36 (C(1)), 114.96 (C(α)), 106.19 (C(2), C(6)), 59.66 (CH2), 56.06 (2× OCH3), 14.23 (CH3)
Propyl sinapate (SP)	δH (297.80 MHz, DMSO-d6): 8.93 (s, 1H, OH), 7.55 (d, J = 15.9, 1H, –CH=), 7.03 (s, 2H, Ar–H), 6.53 (d, J = 15.9, 1H, =CH–), 4.08 (t, J = 6.6, 2H, –OCH2), 3.80 (s, 6H, –OCH3), 1.65 (t, J = 7.4, 6.6, 2H, CH2), 0.93 (t, J = 7.4, 3H, CH3); δC (74.89 MHz, DMSO-d6): 166.65 (C=O), 147.98 (C(3), C(5)), 145.22 (C(β)), 138.23 (C–OH), 124.36 (C(1)), 114.91 (C(α)), 106.20 (C(2), C(6)), 65.18 (CH2), 56.06 (2× OCH3), 21.66 (CH2), 10.33(CH3)
Butyl sinapate (SB)	δH (297.80 MHz, DMSO-d6): 8.94 (s, 1H, OH), 7.54 (d, J = 15.9, 1H, –CH=), 7.03 (s, 2H, Ar–H), 6.53 (d, J = 15.9, 1H, =CH–), 4.12 (t, J = 6.6, 2H, –OCH2), 3.80 (s, 6H, –OCH3), 1.61 (m, 2H, CH2), 1.38 (m, 2H, CH2), 0.92 (t, J = 7.3, 3H, CH3); δC (74.89 MHz, DMSO-d6): 166.65 (C=O), 147.98 (C(3), C(5)), 145.21 (C(β)), 138.23 (C–OH), 124.36 (C(1)), 114.92 (C(α)), 106.20 (C(2), C(6)), 63.38 (CH2), 56.06 (2× OCH3), 30.33 (CH2), 18.67 (CH2), 13.57 (CH3)

3.8. DPPH˙ Radical Scavenging Activity

The <span class="Chemical">DPPH˙ <span class="Chemical">radical scavenging for SA and its derivatives was determined according to Brand-Williams et al. [40]. A solution of the DPPH˙ radical in ethanol was added to ethanolic solutions of these compounds (with ethanol alone as the control), to their final concentration in the reaction mixtures of 6.67 × 10−5 mol/L. The absorbances of the samples (As517nm() and the control (Ac517nm() were monitored continuously at 517 nm at regular time intervals (5 s) over 30 min, against ethanol as a blank on a UV-VIS spectrophotometer (model 8453; Hewlett Packard, Waldbronn, Germany). The measurements were performed at room temperature (25 °C), with the analyses carried out from two consecutive runs.

3.9. Superoxide Anion Scavenging Activity

Measurements of the <span class="Chemical">superoxide anion scavenging activities of the selected compounds were carried out by the method described by Roback and Gryglewski [41]. All of the reagents were prepared in 0.1 M <span class="Chemical">phosphate buffer, pH 7.4. An aliquot of each compound (with ethanol alone as the control) was mixed with the 150 μM NBT and 468 μM NADH solutions, where the final concentration of the tested compounds was 5 × 10−3 mol/L. The reactions were started by addition of the 60 μM PMS solution to the mixture. The absorbances of the samples (As560nm() and of the controls (Ac560nm() were monitored at 560 nm, against a blank sample (without PMS) at 5 s time intervals over a period of 5 min at room temperature. All of these analyses were carried out in duplicate and the results are given as the means.

3.10. Antioxidant Activity in the β-Carotene-linoleic Acid Emulsion System

The antioxidant activities of the selected compounds in an aqueous emulsion system of <span class="Chemical">linoleic acid and β-c<span class="Gene">arotene were determined according to Moure et al. [30]. β-Carotene in chloroform (1 mL, 0.2 mg/mL) was mixed with 20 mg of linoleic acid and 200 mg of Tween 20. After evaporation of the chloroform, 50 mL Milli-Q water was added and mixed thoroughly. The selected compounds were added to 2.5 mL of this emulsion to the final concentration of 2 × 10−4 mol/L, and then mixed thoroughly. The samples were immediately placed in a water bath at 50 °C and incubated for 2 h. A control was prepared using ethanol instead of the selected compounds. Oxidation of the β-carotene emulsion was monitored spectrophotometrically by recording the absorbance of the samples (As470nm() and the control (Ac470nm() at 470 nm over 2 h, at regular time intervals of 1 min during the first 5 min, and then every 5 min for the remaining time, against a blank consisting of the emulsion without β-carotene. This was carried out at 50 °C on a UV-VIS spectrophotometer (model Varian Cary 100 Bio; Varian Inc., Palo Alto, CA, USA). Duplicate analyses were run for each selected compound.

3.11. Lipophilicity Determination

The lipophilicity of the selected <span class="Chemical">SA derivatives was d<span class="Chemical">etermined using CPV, as described by Terpinc et al. [15], and these are given in Table 1. CPVs were calculated as the volume ratio between the acetonitrile and aqueous formic acid mobile phases at the moment of elution. A higher CPV indicates higher content of acetonitrile in the mobile phase and slower elution of the analyte from the column, and consequently lower polarity of the compound.

4. Conclusions

In this investigation a kinetic approach was used in combination with standard fixed endpoint <span class="Chemical">radical scavenging analysis to examine the scavenging activities and reaction mechanisms of <span class="Chemical">sinapic acid and its derivatives against DPPH˙, O2˙− and lipid radicals. The results were in accordance with proposed mechanisms of free radical scavenging and differences in reactivity were interpreted as a function of BDE, IP, PA, and ETE molecular descriptors, acid-base properties, steric effects, and the lipophilicity of the selected compounds. On the other hand, it has been demonstrated that the kinetics response of an antioxidant is dependent also on the radical species and the nature of the medium. Accordingly, the important considerations in the selection of the appropriate antioxidant for any kind of system (e.g., food matrix) are the properties of the system itself.

Our results suggest that the measurements of early response parameters (Rs, <span class="Chemical">RFF, RB) can be used to differentiate between antioxidants with comparable fixed endpoint parameters (IDPPH, CSASA, CAA). This combined approach allows more comprehensive characterization of antioxidants compared to the standard methodology which focuses on measurements at the fixed endpoint. In addition, analysis of our results suggests that O2˙− scavenging follows ET mechanism which has not yet been classified into any of the mechanistic models in the literature.