Antioxidant Activity of Stryphnodendron rotundifolium Mart. Stem Bark Fraction in an Iron Overload Model

Abstract

Stryphnodendron rotundifolium Mart., popularly known as “barbatimão”, is a plant species traditionally used by topical and oral routes for the treatment of infectious and inflammatory diseases. Considering the well-described antioxidant properties of this species, this study investigated the protective effects of its keto-aqueous extract using an in vitro model of iron overload. Phenolic compounds were quantified and identified by Ultra-Performance Liquid Chromatography coupled with quadrupole Time-Of-Flight Electrospray Ionization Mass Spectrometry (UPLC–ESI-qTOF-MS/MS) in positive and negative ions mode analysis. Antioxidant activity was analyzed following the iron-chelating–reducing capacity and deoxyribose degradation (2-DR) protection methods. The analysis identified condensed tannins (54.8 mg catechin/g dry fraction (DF), polyphenols (25 mg gallic acid/g DF), and hydrolyzable tannins (28.8 mg tannic acid/g DF). Among the constituents, prodelphinidin, procyanidin, and prorobinetinidine were isolated and identified. The extract significantly protected 2-DR degradation induced by Fe²⁺ (72% protection) or ^•OH (43% protection). The ortho-phenanthroline test revealed Fe²⁺-chelating and Fe³⁺-reducing activities of 93% and 84%, respectively. A preliminary toxicological analysis using Artemia salina revealed mortality below 10%, at a concentration of 0.25 mg/mL, indicating low toxicity under the present experimental conditions. In conclusion, the findings of the present study indicate that Stryphnodendron rotundifolium is a source of antioxidant compounds with the potential to be used in drug development in the context of iron overload disorders, which remains to be further investigated in vivo.

1. Introduction

Stryphnodendron rotundifolium Mart. is a plant species endemic to the Chapada do Araripe, Brazil, popularly known as “barbatimão”. The stem bark of this plant is widely used in traditional medicine in the preparation of tinctures, syrups, and teas for the treatment of wounds, ulcers, gastritis, inflammation, and vaginal infections [1,2].

The tannin composition in the bark of Stryphnodendron species ranges from 20% to 50% and is potentially responsible for its antioxidant properties [3]. In this context, previous studies have shown that alcoholic extracts obtained from the bark and leaves of S. rotundifolium exhibited free radical-scavenging activity and inhibited Fe²⁺-induced lipid peroxidation in brain homogenates of Wistar rats [4]. Accordingly, consistent evidence has demonstrated that phenolic compounds, including flavonoids and tannins, are crucially responsible for the antioxidant activity of plant-derived natural products [5,6,7].

Iron accumulation results in tissue damage by promoting the generation of reactive oxygen species (ROS), leading to the oxidation of vital molecules such as proteins, lipids, and DNA. The main clinical conditions associated with iron overload are hereditary hemochromatosis and secondary hemochromatosis. These diseases are characterized by excessive absorption of the mineral by intestinal cells, causing iron overload and tissue accumulation, which leads to organ damage, especially in the liver. Secondary hemochromatosis is commonly related to recurrent transfusion of red blood cells. In this case, iron overload is managed mainly with chelating agents [8,9,10]. Iron excess may also occur due to iron inhalation in mining and steel welding [11] and associated with transferrin deficiency [12].

With regard to iron homeostasis, the cellular mechanisms responsible for the excretion of this mineral are less developed and effective than those that regulate its absorption and distribution, which can lead to its accumulation in several iron-carrying cells [13,14].

Previous research has demonstrated that many chronic diseases result from an imbalance between ROS generation and the antioxidant mechanisms in the host cells, highlighting the importance of discovering new antioxidant products [15,16]. In addition, consistent evidence has indicated that iron overload contributes to the development of several chronic/degenerative diseases, especially cardiovascular diseases, mainly by inducing oxidative stress mechanisms, highlighting the therapeutic potential of iron-chelating agents. Therefore, the development of in vitro and in vivo assays, capable of accurately evaluating the antioxidant activity and toxicity of plant extracts, represents a significant preliminary step in the search for natural products capable of controlling iron overload disorders [17,18].

The present study reports the extraction and chemical characterization of the tannin-rich fraction of S. rotundifolium Mart. (TFSR). The in vitro antioxidant activity of this fraction was investigated under iron and free-radical overload conditions, and its cytotoxicity was assessed using an Artemia salina model.

2. Materials and Methods

2.1. Botanical Material and Extraction Procedure

Stryphnodendron rotundifolium stem bark samples were collected in the Araripe National Forest, in the municipality of Crato, Ceará, Brazil (coordinates: 07°81’ S, 039°28’ W). Dr. Maria Arlene Pessoa identified the species, and a voucher specimen was prepared and registered at the Herbarium of the Regional University of Cariri (registry number: 14,074).

A total of 2100 g of freshly collected barks were dried, crushed, and subjected to fat removal with hexane. Then, hexane was removed from the solid material at 70 °C. Following this process, the material was subjected to exhaustive maceration using a 7:3 acetone–water mixture for 72 h at room temperature, to avoid interactions between tannins and vegetable proteins, favoring the obtainment of more stable tannins. This procedure was repeated three times as previously described [19,20]. The resulting solution was subjected to exhaustive removal of acetone in a rotary evaporator (at 65 °C and pressure), reducing the volume to one-third of the initial extractive mixture, after which it was concentrated in a water bath at 70 °C for 24 h. The acetone-free concentrated liquid was frozen and subjected to lyophilization, after which the tannic fraction was obtained as an amorphous solid.

2.2. Phytochemical Prospecting

Phytochemical analysis was carried out to determine the qualitative composition of secondary metabolites. The presence of phenols, tannins, flavonoids, and alkaloids was analyzed according to a previously described method [21]. According to this method, colorimetric changes or precipitate formation in the fraction solution after the addition of specific reagents are indicative of the presence of the corresponding class of secondary metabolites. The screening of phenolic compounds was performed using FeCl_3, 1% methanolic solution, and 1 N HCl, 10% (w/v) NaOH, while the screening of alkaloids was performed using 5% (v/v) acetic acid, 10% (v/v) NH₄OH, chloroform p.a., and Dragendorff’s reagent.

2.3. Quantification of Phenolic Compounds

2.3.1. Total Phenolic Content

The total content of phenolic compounds was determined using a method developed by [22]. A total of 200 μL of the fraction aqueous solution (0.1 μg/mL) was added with 600 μL of ethanol (70% v/v) and 400 μL of the Folin–Ciocâlteu reagent (10% v/v), and the solution was vigorously shaken. After 5 min, the solution was added with Na₂CO₃ (2800 μL, 7.5% m/v) and incubated for 20 min at 45 °C in the absence of light. The absorbance was measured at 735 nm using the UV/Vis spectrophotometer (T80 PG Instruments LTD, Wibtoft, Leicestershire, United Kingdom. Gallic acid (GA) was used as a positive control, and the phenolic content was determined by linear regression using calibration curve (5.0–0.5 μg/mL), performed in triplicate, and the results expressed in mg GA/g dry fraction (DF) (linear equation (y = 0.1351x + 0.0727, R² = 0.9971).

2.3.2. Determination of Total Condensed Tannins

The content of condensed tannins was determined using the vanillin assay, as described by [23], with modifications. An aliquot of 0.5 mL of the fraction diluted in water (0.5 mg/mL) was added with 3 mL of vanillin (4% v/v in methanol) followed by the addition of hydrochloric acid (1.5 mL). The mixture was shaken and kept at 20 °C for 15 min in the absence of light. The absorbance of the mixture was measured at 500 nm and compared with a calibration curve (40–5 μg/mL) of a catechin aqueous solution. The content was calculated by linear regression of the calibration curve (linear equation (y = 0.0176x + 0.1464, R² = 0.9843)) in triplicate, and the results were expressed in mg cat/g DF.

2.3.3. Quantification of Total Hydrolyzable Tannins

Hydrolyzable tannins were detected according to the method proposed by [24], with modifications. A sample (0.20 g) of the fraction was extracted with 50 mL of methanol (80%) and then centrifuged at 493× g for 10 min. After centrifugation, 2 mL of the fraction was diluted with distilled water and mixed with 5 mL of a KIO₃ solution (2.5% m/v) in water. The resulting solution was heated to 30 °C for 7 min °C, and, after cooling, the absorbance was read at 550 nm. The content was calculated by linear regression through a calibration curve (linear equation (y = 1.9636x + 0.0724, R² = 0.9818) of tannic acid (tac) (0.4–0.1 mg/mL) in triplicate, and the results were expressed in mg tac/g DF.

2.4. UPLC–ESI-qTOF-MS/MS

These analyses were performed using an Acquity UPLC (Waters Corporation, Milford, MA, USA) system coupled to a Xevo qTOF mass spectrometer (Q-TOF, Waters). Separations were performed on a C18 column (Waters Acquity^® UPLC C18; 150 mm × 2.1 mm, 1.7 μm). For metabolic fingerprinting, a 2 μL aliquot of the fraction was subjected to UPLC analysis using an exploratory gradient with a mobile phase comprising deionized water (A) and acetonitrile (B), both containing formic acid 0.1% v/v. The sample was subjected to the exploratory gradient as follows: 2–95% for 15 min, at a flow rate of 500 µL·min⁻¹. Ionization was performed with electrospray ionization (ESI) source in negative and positive ion modes, in the range of 110–1200 Da. The optimized instrumental parameters were as follows: capillary voltage of −2800 V, cone voltage of −40 V, source temperature of 120 °C, desolvation temperature of 330 °C, flow cone gas of 20 L·h⁻¹, desolvation gas flow at 600 L·h⁻¹, and microchannel plate (MCP) detector voltage of −1900 V. The mode of acquisition was MS/MS, and the system was controlled using MassLynx 4.1 software (Waters Corporation, Milford, MA, USA).

2.5. In Vitro Antioxidant Activity Analysis

2.5.1. Fe²⁺-Chelating Activity and Fe³⁺-Reducing Power as a Function of Time

In these experiments, the protective activity of the fraction was evaluated in reactive mixtures containing Fe²⁺ at the concentration of 100 μM, which is equivalent to 5.58 μg/mL. Since normal iron concentration in the blood ranges from 0.65 μg/mL to 1.7 μg/mL and the maximum concentration of iron transported by transferrin (tf) in blood is in the range of 2.5 μg/mL to 4.5 μg/mL [25,26,27,28], the protocol follow was used as an in vitro model of Fe²⁺ overload.

The Fe^2+-chelating and Fe^3+-reducing capacity of the fraction were evaluated through the o-phenanthroline (o-phe) assay, as described by the method of [29], with some modifications. Samples were separately added with Fe²⁺ and Fe³⁺ through the addition of FeSO₄ and FeCl₃ (1 mM), respectively, in a dark and refrigerated environment. Then, aliquots of 40 μL were extracted at times 0.5, 2.5, 5, 10, 20, 30, 45, 60, 75, and 90 min and reacted with o-phe (300 μM) in H₂O milli-Q and Tris-HCl (0.1 M, pH 7.4). At the end of this procedure, the samples were obtained at final concentrations of 0.2, 0.1, and 0.05 mg/mL, and Fe²⁺ and Fe³⁺ were obtained both at 100 μM. The readings were carried out at 510 nm. Experimental controls were obtained by replacing aliquots of the samples with milli-Q water. To evaluate the stability of the chelates, ascorbic acid (at the final concentration of 0.005 M) was added to each reacting system (at the timepoint of 90 min), and the readings were performed 15 min later. The results are representative of three independent experiments (n = 3) performed in duplicate.

The Fe²⁺-chelating activity (FCA) and Fe³⁺-reducing power (FRP) were expressed as a percentage of the control, as represented by the Equations (1) and (2), respectively.

$$\mathrm{FCA}(\%){\mathrm{t}}_{\mathrm{minutes}}=\frac{\left({\mathrm{Abs}}_{\mathrm{controle}-{\mathrm{Fe}}^{2+}}-\left({\mathrm{Abs}}_{\mathrm{fraction}-{\mathrm{Fe}}^{2+}}-{\mathrm{Abs}}_{\mathrm{fraction}-\mathrm{blank}-{\mathrm{Fe}}^{2+}}\right)\right)\times 100}{{\mathrm{Abs}}_{\mathrm{controle}-{\mathrm{Fe}}^{2+}}}$$

(1)

$$\mathrm{FRP}(\%){\mathrm{t}}_{\mathrm{minutes}}=\frac{\left({\mathrm{Abs}}_{\mathrm{fraction}-{\mathrm{Fe}}^{3+}}-{\mathrm{Abs}}_{\mathrm{fraction}-\mathrm{blank}-{\mathrm{Fe}}^{3+}}\right)-{\mathrm{Abs}}_{\mathrm{control}-{\mathrm{Fe}}^{3+}})\times 100}{{\mathrm{Abs}}_{\mathrm{controle}-{\mathrm{Fe}}^{2+}}}$$

(2)

where Abs_{Control-Fe²⁺} is the absorbance of o-phe + Fe²⁺, Abs_{Fraction-Fe²⁺} is the absorbance of fraction + o-phe + Fe²⁺, Abs_{Fraction-blank-Fe²⁺} is the absorbance of fraction + Fe²⁺, Abs_{Control-Fe³⁺} is the absorbance of o-phe + Fe³⁺, Abs_{Fraction-Fe³⁺} is the absorbance of fraction + o-phe + Fe³⁺, and Abs_{Fraction-blank-Fe³⁺} is the absorbance of fraction + Fe³⁺.

2.5.2. Deoxyribose Oxidative Degradation Assay

The ^•OH radical-scavenging activity was investigated according to the ability of the fraction to inhibit the degradation of 2-deoxyribose (2-DR) in vitro, following the method used by [30], with adaptations. Briefly, 1.5 mM 2-DR was incubated with 50 mM potassium phosphate buffer (pH 7.4) at room temperature for 20 min in the following pro-oxidant systems: (i) 0.05 mM FeSO₄ and (ii) 0.5 mM H₂O₂ + 0.05 mM FeSO₄ (Fenton reaction); then, it was incubated at 37 °C for 60 min, in the absence or presence of the variable concentrations of the fractions (0.2, 0.1, and 0.075 mg/mL). Following this step, 750 μL of Trichloroacetic Acid (TCA) (2.8%) and 750 μL of Thiobarbituric Acid (TBA) (0.8%) were added to all samples, before incubating for 20 min at 100 °C. The readings were carried out at 532 nm, and the results are expressed as a percentage of inhibition of 2-DR degradation relative to the negative controls according to Equation (3).

$$\mathrm{Inhibition}(\%)=\frac{\left[\left({\mathrm{Abs}}_{\mathrm{control}}-{\mathrm{Abs}}_{\mathrm{blank}}\right)\right]\times 100\%}{{\mathrm{Abs}}_{\mathrm{control}}}$$

(3)

where Abs_Control is the Absorbance of 2-DR + pro-oxidant, Abs_Fraction is the absorbance of 2-DR + pro-oxidant + fraction, and Abs_Blank is the absorbance of pro-oxidant + fraction.

Of note, the Fenton reaction was performed with 50 μM Fe²⁺, which is equivalent to 2.79 μg/mL. The results are representative of four independent experiments (n = 4) performed in duplicate.

2.5.3. Analysis of the Mechanism Underlying the Inhibition of 2-DR Degradation

An assay based on the variation of the 2-DR concentration (1.5 mM, 1.75 mM, and 2.0 mM) was used to determine the antioxidant mechanism of the fraction (Fe²⁺ chelating or ^•OH scavenging). The oxidative degradation of 2-DR was obtained via the reaction of 0.5 mM H₂O₂ with 0.05 mM FeSO₄, which results in the generation of the ^•OH radical. The tests were performed three (n = 3) times in duplicate for each concentration of 2-DR (1.5 mM, 1.75, mM, and 2.0 mM). The results were expressed as a percentage inhibition of 2-DR degradation according to Equation (4) [31].

$$\mathrm{Inhibition}(\%)=\frac{[{\mathrm{Abs}}_{\left(\mathrm{H}2\mathrm{O}2+{\mathrm{Fe}}^{2+}\right)\mathrm{control}}-\left({\mathrm{Abs}}_{\mathrm{fraction}}-{\mathrm{Abs}}_{\mathrm{blank}}\right)]\times 100\%}{{\mathrm{Abs}}_{\left(\mathrm{H}2\mathrm{O}2+{\mathrm{Fe}}^{2+}\right)\mathrm{control}}}$$

(4)

where Abs_{(H2O2 + Fe²⁺)Control} is the absorbance of 2-DR + (H₂O₂ + Fe²⁺), Abs_Fraction is the absorbance of 2-DR + (H₂O₂ + Fe²⁺) + fraction, and Abs_Blank is the absorbance of (H₂O₂ + Fe²⁺) + fraction.

2.6. In Vivo Toxicity Analysis

Saline solution (36.2 g/L, pH 7.0–9.0) was prepared by adding 72.4 g of sea salt in 2 L of distilled water. A total of 200 mg of Artemia Salina eggs were placed to hatch in 400 mL of saline solution for 24 h under continuous aeration and exposure to light. To determine the in vivo toxicity of the fraction, 10 larvae were placed in 10 mL of a solution containing the fraction at increasing concentrations (0.001 to 0.250 mg/mL). The mortality was analyzed 24 h after treatments. The tests were performed in triplicate [32].

2.7. Statistical Analysis

The data of the antioxidant and toxicity assays, as well as those of chemical quantification, were expressed as the means ± Standard Error of Mean (SEM) of at least three experiments. The antioxidant assays were analyzed by one-way analysis of variance (ANOVA), followed by Tukey’s post hoc test for multiple comparisons of data with normal distribution and similar standard deviation, using GraphPad Prism version 6.0. The UPLC/MS data were expressed as the means ± SEM of three determinations and analyzed by ANOVA followed by Tukey’s test. Statistical significance was considered when p < 0.05.

3. Results and Discussion

The tannin-rich fraction from Stryphnodendron rotundifolium Mart. (TFSR) was obtained as a reddish solid, characteristic of proanthocyanidins. The acetone–water (7:3) extraction presented a yield of 38.8%. The phytochemical characterization demonstrated the presence of secondary metabolites such as polyphenols, flavonoids, leucoanthocyanidins, aurones, chalcones, catechins, and hydrolyzable and condensed tannins. In particular, the UPLC–ESI-qTOF-MS/MS profile revealed the presence of type B proanthocyanidins, including prodelphinidins (monomers, dimers, and trimers), procyanidins, and prorobinetidins previously reported in other species of the same genus [5,33,34].

The concentration of total phenols was determined in 25.02 ± 0.67 mg gallic acid/g DF. The quantification of condensed tannins was 54.83 ± 2.30 mg catechin equivalent/g DF, corresponding to the main type of component in the sample. In addition, the concentration of hydrolyzable tannins was 28.84 ± 2.21 mg tannic acid/g DF, confirming this class of components as the second most abundant in the sample. In fact, extractive mixtures containing acetone favor the extraction of condensed tannins formed by monomeric units of the catechin type flavan-3-ols, to the detriment of hydrolyzable tannins [19].

The chemical constituents of the TFSR were identified using the UPLC–ESI-qTOF-MS/MS technique, by interpreting their MS and MS/MS spectra, determined by QTOF-MS and compared with the literature data and the open-access mass spectrum database SciFinder. The chromatogram and phenolic profile are shown in Figure 1 and

Table 1. Identification of TFSR phenolic compounds using UPLC–ESI-qTOF-MS/MS in the negative and positive modes.

Peak No.	Rt (min)	[M + H]+ Obs	[M − H]− Obs	Empirical Formula [M − H]−	Ion Products (MS/MS)	Empirical Formula [M + H]+	Empirical Formula M/MM (g·mol−1)	∆ 1 (Error)	Structure Name	Ref.
1	1.30	383.1159	no 2	-	203.0517	C21H19O7		−2.3	Unknown	-
2	1.39	625.5280	623.1370	C31H27O14	125.0226, 169.0148, 305.0661	C31H29O14	C31H28O14/624.5603	3.7	4’-O-methyl-epigallocatechin (4→8) epigallocatechin	[33]
3	2.15	611.1428	609.1245	C30H25O14	425.0808, 299.0632, 287.0573, 263.0517, 179.0361	C30H27O14	C30H26O14/610.494	4.4	Epigallocatechin (4β→8) epigallocatechin	[5,33,34,35]
4	2.20	171.0300	169.0138	C7H5O5	-	C7H7O5	C7H6O5/170.113	4.1	Gallic acid 3	[5,35,36]
5	2.42	915.2008	913.1827	C45H37O21	611.1431, 425.0869, 287.0597, 263.0562, 179.0362	C45H39O21	C45H38O21/914.733	2.6	Epigallocatechin (4→8) epigallocatechin (4→8) epigallocatechin	[5]
6	2.62	929.7240	927.2041	C45H35O22	761.1112, 423.0788, 305.0630, 125.0252	-	C45H36O22/928.311	0.2	4’-O-methyl-epigallocatechin-3-O-gallate (4→6) epigallocatechin 3-O-gallate	[33]
7	2.64	611.1406	609.1224	C30H25O14	425.0943, 287.0575, 263.0571, 179.0337	C30H27O14	C30H26O14/610.494	0.8	Epigallocatechin (4β→6) epigallocatechin	[5,34,35]
8	2.80	1067.2070	1065.1937	C52H41O25	915.2032, 611.1549, 425.0953, 287.0670, 263.0620, 179.0453	C52H43O25	C52H42O25/1066.831	−2.2	Epigallocatechin (4→8) epigallocatechin (4→8) epigallocatechin-3-O-gallate	[7]
9	3.00	307.0824	305.0664	C15H13O7	195.0573, 177.0488, 163.0406	C15H15O7	C15H14O7/306.255	2.0	Epigallocatechin	[5,33,35]
10	3.08	763.1538	761.1367	C37H29O18	593.1270, 485.1284, 319.0786, 305.0662, 125.0253	C37H31O18	C37H30O18/762.6221	1.7	Epigallocatechin (4→8) epigallocatechin-3-O-gallate/Epigallocatechin-3-O-gallate (4→8) epigallocatechin	[7,33,34,35]
11	3.28	609.5290	607.1412	C31H27O13	485.1264, 319.0786, 287.0568	C31H29O13	C31H28O13/608.5451	1.4	Robinetinidol-4’-O-methyl (4→8) epigallocatechin	[34,35]
12	3.32	487.1447	485.1295	C21H25O13	355.1012, 319.0728, 289.0634, 259.0592	C21H27O13	C21H26O13/ 486.405	−1.0	C-hexosyl-O-pentosyl-5,7-dihydroxychromone isomer	[5]
13	3.57	595.1460	593.1277	C30H25O13	427.0926, 307.0875, 289.0704	C30H27O13	C30H26O13/594.495	1.3	Procyanidin prodelphinidin type B	[5]
14	3.79	623.1767	no 2	-	423.1066, 287.0533	C32H31O13	-	0.3	Unknown	-
15	4.08	623.1779	no 2	-	423.1018, 287.0552	C32H31O13	-	2.2	Unknown	-
16	5.43	677.2097	no 2	-	545.1690, 367.1169, 235.0579, 191.0706	C32H37O16	-	2.2	Unknown	[5]
17	5.60	707.2196	no 2	-	575.1804, 367.0898, 236.0611, 221.0834	C33H39O17	-	1.3	Unknown

Rt min: retention time of the eluted compounds under the experimental conditions described in the UPLC–MS section; [M − H]⁻: exact mass value of the deprotonated molecule; [M + H]⁺: exact mass value of the protonated molecule; M: exact mass value of the neutral molecule; MM: molar mass; (MS/MS): m/z mass–charge ratio of the major ions produced by the fragmentation of deprotonated molecules. ∆ ¹ mass error (ppm) in parts per million; ppm = 10⁶ × (accurate mass exact); ¹—positive mode; ²—non-observed; ³—compared to the standard. The signals detected in the present analysis were numbered following the elution order (retention time).

, respectively.

A total of 17 peaks were identified, revealing the presence of compounds belonging to corresponding to two main classes of metabolites: phenolic acids and tannins. The compounds were eluted in a noticeably short period of time (6.9 min). Together, the retention time and the number of peaks observed in the present analysis indicate that UPLC is an efficient separation technique.

According to our analysis, peaks 4 and 9 exhibited protonated ions in m/z 171.0300 and 307.0824, respectively, which is compatible with the corresponding molecular formulas C₇H₆O₅ and C₁₅H₁₄O₇, as their fragmentation profiles are compatible with the reported for S. adstringens [5,33,35]. The fragmentation pattern id compatible with the mechanistic pathway of retro-Diels–Alder (RDA) reactions and the different heterocyclic cleavage of the C ring (HRF—heterocyclic fission) (Figure 2). In addition, the occurrence of dehydration was crucial for the identification of peak 9 epigallocatechin (EGC) [37].

The protonated ions at m/z 625.5280 (peak 2), 611.1428 (peak 3), 929.7240 (peak 6), 611.1406 (peak 7), 763.1538 (peak 10), 609.5290 (peak 11), and 595.1460 (peak 13), corresponding respectively to C₃₁H₂₈O₁₄, C₃₀H₂₆O₁₄, C₄₅H₃₆O₂₂, C₃₀H₆₈O₁₄, C₃₇H₃₀O₁₈, C₃₁H₂₈O₁₃, and C₃₀H₂₆O₁₃, were characterized as type B dimeric proanthocyanidins and type B dimeric proanthocyanidins with 3-O-galloyl in epigallocatechin (EGC) subunits.

The spectral analysis of peaks 2, 3–8, 10, 11, and 13 revealed fragmentation ions at m/z 319, 307, 305, 289, and 287, produced from the generation of quinone and quinone methide with losses of (110, 125, 181, 318) u, 289 u, (319, 457, 471, 153) u, 289 u, (305, 609, 761) u, and H₂O molecules, consistent with prodelphinidin (PDE), procyanidin (PCY), and prorobinetinidine (PRO). Thus, the common losses due to RDA reactions of 168 and 152 Da, as well as the heterocyclic cleavage reactions of the C HRF 125 Da ring (floroglucinol), suggest the presence of PDE, PRO, and PCY.

Pseudomolecular ion products at m/z 425 [M + H⁺ − 168 − H₂O]⁺, [M + 2H⁺ − 305 − 168 − H₂O]⁺, [M + 2H⁺ − 457 − 168 − H₂O]⁺ resulting from RDA reactions and excisions of 305 EGC and 457 gallate epigallocatechin (EGCG) were observed for peaks 3, 5, 7, and 8. An ion at m/z 427 [M + H⁺ − 168]⁺ was observed for metabolite 13. The ions at m/z 485 [M + H⁺ − 153 − 125]⁺ and [M + 2H⁺ − 125]⁺ resulted from the excisions of the galloyl (153 Da) and floroglucinol (125 Da) groups, respectively, corresponding to peaks 10 and 11. Of note, six possible isomers were proposed for peak 10. The ion at m/z 423 [M + 2H⁺ − 169 − 168 − 170]⁺ was associated with peak 6, such that the 169 Da fragment was associated with the loss of an O-gallate group, in which the 168 Da fragment corresponds to the loss of the 4-O′-methyl-3,5-di-hydroxyl-benzaldehyde portion through heterocyclic cleavage of the C ring. The 170 Da fragment was associated with the loss of a gallic acid unit. Together, these findings suggest the presence of dimeric/trimeric PDE, in addition to PCY and dimeric PRO in the phenolic fraction under investigation, whose spectral profiles are compatible with the literature data [5,7,33,34,35].

The type B prodelphinidin trimer shown in peak 5 was identified as three EGC units exhibiting the protonated ion at m/z 915.2008, which corresponds to C₄₅H₃₈O₂₁, as also reported in S. adstringens [5]. On the other hand, the type B prodelphinidin trimer in peak 8, consisting of two units of EGC and one EGCG unit that exhibited the protonated ion at m/z 1066.2070, corresponds to C₄₂H₄₂O₂₅, as previously reported in Myrica yubra Sieb & Zucc [7]. Of note, proanthocyanidin ions larger than trimers were not identified, since these experiments were recorded in a 110–1200 Da m/z window.

The characteristic of peak 12 is compatible with the structure of chromonic compounds [38]. Accordingly, its protonated ion presented a precise mass loss at m/z 487.1447, corresponding to C₂₁H₂₆O₁₃. The fragmentation of ions at m/z 487 produced an ion at m/z 355 [M + H − 132]⁺ suggesting an O-pentosyl substitute in the structure, at m/z 319 [M + H − 168]⁺. Thus, peak 12 was identified as C-hexosyl O-pentosyl 5, 7-dihydroxychromone, and its spectral data are comparable to the data reported in the literature [5].

In synthesis, the UPLC–MS analysis showed the predominance of type-B proanthocyanidins (PA) with C₄→C₈ and C₄→C₆ interflavanic bonds in the tannin-rich fraction of S. rotundifolium.

The molecular structures of compounds (Figure 3) were designed using the Chem Draw Ultra 12.0.2.1076.lnk program (Licensed to Mulder X-Filer 875-317589-4732. 1986–2010 CambridgeSol).

The findings of the present study indicate that the phenolic composition of S. rotundifolium is characterized by a remarkable presence of type B proanthocyanidins, a group of compounds with demonstrated antioxidant activity, which may, therefore, play important roles in health maintenance and minimization of disease onset and progression [2,39].

The Fe²⁺-chelating activity and Fe³⁺-reducing power of TFSR, as a function of time and concentration, were analyzed using the o-phe assay. As shown in

Table 2. Fe²⁺-chelating activity of TFSR.

[TFSR] mg/mL	(%)Fe2+-Chelating Activity/Time (min)										Asc. ac.
	0.5	2.5	5	10	20	30	45	60	75	90	105
0.200	87.88 ± 2.40	93.61 ± 1.78	93.29 ± 1.93	92.32 ± 1.75	95.37 ± 2.96	93.37 ± 3.29	97.82 ± 0.91	95.24 ± 2.69	93.15 ± 3.37	91.86 ± 3.08	91.94 ± 5.04
0.100	86.77 ± 4.25	84.55 ± 2.87	83.62 ± 2.62	85.77 ± 2.81	85.81 ± 1.77	84.44 ± 4.32	93.68 ± 3.47	86.32 ± 4.11	82.66 # ± 4.58	79.50 # ± 2.65	77.92 # ± 5.24
0.050	76.50 # ± 3.50	80.92 # ± 3.39	75.52 # ± 5.88	75.90 # ± 4.84	80.17 # ± 6.11	77.49 # ± 3.73	83.23 # ± 2.19	76.14 # ± 3.42	71.70 # ± 4.28	70.85 # ± 3.02	67.95 # ± 3.29

These values are expressed as the means ± SEM (n = 4) and analyzed by one-way ANOVA followed by Tukey’s multiple comparison test, with a simple pooled variance: Significant difference (p < 0.05) at different timepoints and concentrations of tannic fraction of Stryphnodendron rotundifolium Mart., (TFSR). Ascorbic acid (Asc. ac.). # Significant difference between the values of different concentrations at equal timepoints.

, the fraction was effective in chelating Fe²⁺ at all concentrations and timepoints evaluated in this study. At the highest concentration (0.200 mg/mL), the activity varied over time (0.5 to 90 min), reaching an average Fe²⁺-chelating rate of 93%. For the lowest concentration (0.05 mg/mL), an average value of 77% was found. The fraction, at the concentrations analyzed, reached maximum activity at 45 min. Importantly, there was no significant difference in the chelating activity at different timepoints when considering the same concentration. However, a significant difference was observed between the Fe²⁺-chelating activity of the concentrations 0.200 mg/mL and 0.050 mg/mL. The results also indicate the chelating activity of the fraction is not concentration-dependent.

The rapid decrease in the absorbance of the Fe²⁺/o-phe/TFSR system compared to the control (o-phe/Fe²⁺/H₂O) indicates that the formation of chelates with Fe²⁺ is kinetically favored. The addition of ascorbic acid 90 min after the beginning of the reaction caused insignificant variation in the absorbance of the sample, revealing the generation of chelates with higher thermodynamic stability then the ferroin chelate (ph)₃Fe²⁺.

A study by [36] reported that the Fe²⁺ chelating potential of the TFSR was positively correlated with the number of catechol groups in the phenolic structures. Therefore, the abundance of highly hydroxylated proanthocyanidins with catechol and galloyl groups in the tannin-rich fraction under study offer several chelation sites, contributing to its significant Fe²⁺-chelating activity.

Regarding the Fe²⁺-chelating activity of S. rotundifolium, this work demonstrated that its tannin-rich fraction showed a potent effect, with fast reaction kinetics. The reaction profile indicates that the chelates formed between the fraction constituents and Fe²⁺ are thermodynamically more stable than the ferroin chelate of high crystal field stabilization energy (CFSE) [40]. Consequently, the authors of this work believe that the significant chelating activity of the fraction is related to synergistic effects due to the presence of prodelphinidins, prorobinetidine, and procyanidin with many catechol and galloyl groups. The potent iron-chelating activity exhibited by S. rotundifolium indicates that this species has the potential to be used to minimize oxidative effects of iron overload eating conditions that play important pathological functions, including a wide variety of disorders such as tumors, nervous system diseases, ischemia/reperfusion injury, kidney injury, and blood diseases [41].

As for the Fe³⁺-reducing power, at the highest concentration analyzed (0.200 mg/mL), the fraction effectively reduced Fe³⁺ to Fe²⁺ from the first timepoint of analysis (

Table 3. TFSR Fe³⁺-reducing activity.

[TFSR] mg/mL	(%)Fe3+-Reducing Activity/Time (min)										Asc. ac.
	0.5	2.5	5	10	20	30	45	60	75	90	105
0.200	81.43 ±2.62	79.65 ±4.14	87.38 ±1.62	82.24 ±4.80	82.84 ±5.10	81.24 ±4.52	87.26 ±3.78	86.15 ±2.87	86.35 ±3.15	85.44 ±4.44	90.19 ± 3.99
0.100	64.70 # ± 2.09	64.18 # ± 5.40	70.34 # ± 4.84	66.10 # ± 2.53	65.01 # ± 3.32	62.91 # ± 4.19	70.31 # ± 5.17	68.58 # ± 3.39	69.80 # ± 3;06	71.66 # ± 4.49	77.69 #* ± 3.82
0.050	61.80 # ± 2.04	62.09 # ± 5.53	71.83 # ± 2.39	63.67 # ± 4.80	65.28 # ± 4.47	63.39 # ± 3.20	66.65 # ± 5.06	63.84 # ± 3.59	63.85 # ± 2.01	64.88 # ± 4.03	69.01 # ± 2.79

These values are expressed as the means ± SEM (n = 4) and analyzed by one-way ANOVA followed by Tukey’s multiple comparison test, with a simple pooled variance: Significant difference (p < 0.05) at different timepoints and concentrations of TFSR. * Significant difference between the values of equal concentration. # Significant difference between the values of different concentration at equal timepoints.

), exhibiting strong reducing activity with an average of 84% (from 0.5 to 90 min) and the peak effect reached at 45 minutes, revealing the typical electron transfer characteristic of phenolic compounds [42]. Nevertheless, in this assay, the maximum activity of the fraction from 0.20 to 0.05 mg/mL was reached at 105 min. The rapid decrease in the absorbance of the systems (Fe³⁺/o-phe/TFSR) in relation to the control (o-phe/Fe²⁺/H₂O), suggests that the reducing reaction from Fe³⁺ to Fe²⁺ is kinetically favored in the presence of the constituents of the fraction. The addition of ascorbic acid 90 min after the beginning of the reaction caused a decrease in the absorbance of the system (Fe³⁺/o-phe/TFSR), revealing that the Fe²⁺ fraction was subtracted from the ferroin chelate by the action of the TFSR, reducing the absorbance of ferroin. As observed in the iron-chelating activity experiment, no significant difference was observed with regard to the reducing activity when different timepoints at the same concentration were compared. However, there was a significant difference in Fe³⁺-reducing activity between the concentration of 0.200 mg/mL and the others (0.100 mg/mL and 0.050 mg/mL). The results obtained in this experiment indicate that the reducing activity responses mediated by the extract do not occur in a concentration-dependent manner.

The ^•OH radical-scavenging activity was evaluated using the 2-deoxyribose (2-DR) oxidative degradation method, by quantifying its main subproduct, malondialdehyde (MDA). The antioxidant activity was expressed as the percent protection of 2-DR degradation.

The hydroxyl radical (^•OH) is a highly reactive free radical capable of triggering damage to several cellular structures. In vivo, this radical can be generated in the presence of superoxide radicals and transition cations, such as iron and copper, through the Haber–Weiss reaction [43]. In the experimental conditions of this study, the ^•OH radical was generated in vitro through the Fenton reaction.

Figure 4A,B show the protection level exerted by the fraction when the treatment was performed previously (PT) or simultaneously (ST) to the addition of either of the prooxidant systems: Fe²⁺ (light-gray bars) and Fenton reaction/^•OH (dark-gray bars). In both treatment conditions, the fraction showed a strong protective activity against the oxidative action of Fe²⁺ and a moderate activity against the action of the ^•OH radicals generated in the Fenton reaction. For the first condition, the fraction presented IC₅₀ values of 0.0576 and 0.100 mg/mL for PT and ST, respectively. For the second condition, these values were respectively 0.225 and 0.596 mg/mL. However, considering the distinct pro-oxidant systems, no significant difference in the protective activity of the fraction against 2-DR degradation for a given concentration was observed, indicating that the antioxidant activity was not influenced by the time of treatment.

At the concentration of 0.2 mg/mL, the TFSR prevented 2-DR degradation by the pro-oxidant Fe²⁺ with protection levels of 72.2% and 68.6% for PT (Figure 4A) and ST (Figure 4B), respectively. However, the difference between these treatment conditions was not significant. The 2-DR degradation triggered by the ^•OH radical generated in the Fenton reaction was inhibited by TFSR (0.2 mg/mL) in both PT (Figure 4A) and ST (Figure 4B) conditions, with protection levels of 42.9% and 33.1%. Again, the difference between these treatment conditions was not significant.

Considering the two different oxidant systems, it can be observed that TFSR protective activity against the pro-oxidant condition Fe²⁺ was significantly higher that observed against ^•OH radical produced in the Fenton reaction, as shown in Figure 4.

The remarkable ^•OH-scavenging activity of the fraction can be attributed to the presence of hydrolyzable tannins, especially type B proanthocyanidins (dimers and trimers) with catechol and pyrogallol groups. These compounds have been recognized as excellent natural antioxidants and, as such, have the potential to be investigated in pharmacological research in several disease models [44]. Studies have indicated that the mechanism underlying the antioxidant activity of these compounds involves the donation of hydrogen and electrons responsible for the inhibition of free radicals [5,7].

To elucidate the mechanism via which the fraction protects 2-DR from degradation in the presence of the Fenton reaction, we evaluated the protective effect of different concentrations of the fraction (0.2, 0.1, and 0.075 mg/mL) using varying concentrations of 2-DR (1.5, 1.75 and 2.0 mM) and a fixed concentration of the reacting system (50 μM Fe²⁺ + 0.5 mM H₂O₂).

The protection levels exerted by different concentrations of TFSR against 2-DR degradation did not vary significantly following the increasing 2-DR concentrations (1.5, 1.75, and 2.0 mM) (

Table 4. 2-DR degradation.

	TFSR Protective Activity (%) ± SEM
[2-DR] mM	0.20 mg/mL	0.10 mg/mL	0.075 mg/mL
1.50	27.22 ± 1.67	21.40 ± 1.95	17.37 ± 1.80
1.75	25.57 ± 1.87	21.09 ± 3.12	16.32 ± 1.90
2.00	24.53 ± 1.11	19.74 ± 0.49	15.46 ± 3.95
Statistical Comparison	NS	NS	NS

These values are expressed as the means ± SEM (n = 3) and analyzed by one-way ANOVA followed by multiple comparisons. Significant difference (p < 0.05) at equal concentrations of TFSR. NS No significant difference between the values.

), suggesting that the constituents of the fraction act predominantly as iron-chelating antioxidants, inhibiting the generation ^•OH radicals.

The findings of the present research indicate that the protective mechanism of TFSR occurred mainly via chelation of Fe²⁺ ions (as show in Table 4) and, to a lesser extent, via ^•OH radical scavenging. Importantly, this mechanism can prevent Fe²⁺ from participating in reactions that generate free radicals such as H₂O₂ and ^•OH, which could have beneficial roles in inhibiting oxidative stress. Nevertheless, a secondary antioxidant mechanism via ^•OH scavenging could contribute to the occurrence of synergistic antioxidant effects.

The preliminary toxicological analysis using A. salina showed that, in the range of concentrations evaluated (0.001 to 0.25 mg/mL), mortality below 10% was observed, with no statistical difference between the rates of mortality induced by each of the tested concentrations, indicating that the fraction has low in vivo toxicity under the experimental conditions adopted in the present study (Figure 5).

The results demonstrated by this preliminary toxicological evaluation suggest that the fraction can be tested in a higher concentration range, both in pharmacological and in toxicological studies, since no evident toxicity was observed at the highest tested concentration (0.25 mg/mL). However, additional studies using cell cultures and animal models are fundamental to bring relevant information regarding its in vivo safety, especially with regard to the risks associated with the ingestion of tannins.

It is hypothesized that the antioxidant effects demonstrated by the fraction are explained, at least partially, by the presence of constituents carrying pyrogallol groups containing hydroxyls capable of promoting both Fe³⁺ reduction and Fe²⁺ chelation, in addition to potentially acting as electron and hydrogen donors and, as such, acting as free-radical scavengers. The presence of galloyl portions, as well as the stabilization of phenoxyl radicals by resonance, contributes significantly to the antioxidant capacity of phenolic compounds [45]. In addition, the existence of significant amounts of galloyl portions in polyphenols favors the stabilization of phenoxyl free radicals (semiquinones), contributing to their iron-chelating and radical-scavenging activities [46].

In this context, the proanthocyanidins identified in the tannin-rich fraction present characteristics that favor their antioxidant action. In addition, these compounds can be easily absorbed by the gastrointestinal tract, which is a desirable characteristic for substances used in the development of oral drugs. Notwithstanding, proanthocyanidins with higher polymerization rates have low permeability coefficients in the human organism, impairing their oral absorption [47].

Despite the strong influence of pyrogallol and phenolic hydroxyl groups on TFSR antioxidant activity, the three-dimensional arrangement of the structure and possibly steric effect might contribute to the pharmacological effects of the fraction components. Thus, among the proanthocyanidins identified, we believe that dimers and trimers mostly contribute to the antioxidant activity demonstrated through 2-DR degradation protection.

Iron is a mineral with several physiological functions, found both in free form and in the composition of proteins such as hemoglobin, myoglobin, cytochromes, and several enzymes [48]. However, due its deleterious effects, the cells store free iron at low levels.

While little amounts of this mineral are commonly stored by macrophages, excess free iron reaches the circulation and deposits in hepatocytes and parenchymal cells. Iron accumulation triggers oxidative stress by mechanisms that involve the Fenton and Haber–Weiss reactions. In this phenomenon, free iron acts as a catalyst for oxidative reactions stimulating the synthesis of superoxide and hydroxyl radicals [49].

Recent research has demonstrated that many of the deleterious effects of iron occur due to ferroptosis, an iron-dependent type of cell death characterized by the accumulation of lipid ROS that play important roles in a wide variety of systemic diseases, such as nervous system diseases, heart diseases, liver diseases, gastrointestinal diseases, lung diseases, kidney diseases, and pancreatic diseases [42]. Hence, the importance of demonstrating the expressive ability of TFSSR to acting as iron-chelating–reducing in vitro raises the hypothesis that this natural product may present promising results in vivo, which will be further investigated.

In fact, evidence suggests that substances capable of forming complexes with iron, thus promoting its excretion, may have applications in the treatment of several conditions [50], highlighting the therapeutic potential of S. rotundifolium, which proved to be a source of tannic compounds with Fe²⁺-chelating and ^•OH-scavenging activities. This hypothesis is supported by studies demonstrating that extracts with high concentrations of phenolic compounds inhibited lipid peroxidation in human erythrocytes by decreasing the production of malondialdehyde, a subproduct of 2-DR degradation [51].

In recent years, considerable interest has arisen regarding the beneficial effects of proanthocyanidins (PAs) and their monomers on human health. Studies have shown that these substances have numerous pharmacological activities, including antioxidant, anti-inflammatory, and anticancer properties [5,39,52]. Therefore, the polymeric proanthocyanidins identified in S. rotundifolium could have beneficial effects in metabolic disorders, preventing the onset of diseases whose etiology is associated with iron overload and oxidative stress [53].

4. Conclusions

The results of the present study demonstrated that the tannin-rich fraction of S. rotundifolium is a natural product with significant in vitro antioxidant activity, which may be directly related to the high content of prodelphinidins, prorobinetidines, and highly hydroxylated procyanidins with great capacity to donate electrons, as well as to chelate iron ions.

The potent Fe²⁺-chelating activity demonstrated by the tannin-rich fraction of S. rotundifolium and the significant and constant protective activity observed in the 2-DR + Fe²⁺ system indicate that the antioxidant mechanisms of this fraction are mainly via an iron-chelating action and, to a lesser extent, an ^•OH radical-scavenging action, at concentrations that do not cause significant toxicity in vivo in the Artemia salina model.

In conclusion, the tannic fraction of S. rotundifolium Mart. has potent antioxidant and iron-chelating activities, which indicates that it is a source of antioxidant compounds with the potential to be used in drug development in the context of iron overload disorders, which remains to be further investigated in vivo.