# Dual Role of a Ricinoleic Acid Derivative in the Aqueous Synthesis of Silver Nanoparticles

Authors: Isadora Dantas Costa; Alcides de Oliveira Wanderley Neto; Heloiza Fernanda Oliveira da Silva; Edgar Perin Moraes; Eryka Thamyris Damascena Nóbrega; Celso Sant’Anna; Mateus Eugenio; Luiz Henrique da Silva Gasparotto
Journal: Journal of Nanomaterials
 (2017)

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## Abstract

We show that sodium 9,10-epoxy-12-hydroxytetradecanoate (SEAR), an epoxidized derivative of ricinoleic acid, simultaneously functioned as reducing and stabilizing agents in the synthesis of silver nanoparticles in alkaline aqueous medium. The advantage of using SEAR is its biodegradability and nontoxicity, which are important characteristics for mitigation of environmental impact upon discharge of nanoparticles into terrestrial and aquatic ecosystems. The SEAR concentration was found to impact considerably the size distribution of silver nanoparticles (AgNPs). A concentration below the SEAR critical micelle concentration (CMC) generated 23 nm sized AgNPs with 10 nm standard deviation, while 50 nm sized AgNPs (σ=21 nm) were obtained at a concentration above the SEAR CMC. FTIR analysis revealed that the carboxylate that constitutes the SEAR hydrophilic head binds directly to the AgNPs surface promoting stabilization in solution. Finally, AgNPs turned into Ag2S upon contact with wastewater samples from Wastewater Treatment Plant at Federal University of Rio Grande do Norte (UFRN), Brazil, which is an interesting result, since Ag2S is more environmentally friendly than pure AgNPs.


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## Body

## 1. Introduction

Silver nanoparticles (AgNPs) have found innumerable applications that comprise biomedicine [1, 2], food storage [3], sensors [4], and (electro)catalysis [5, 6]. Concerning their synthesis, AgNPs may be produced via physical [7], biological [8], or chemical methods [9–11], being the latter more adequate in terms of cost, simplicity, and quantity of formed AgNPs. Chemical methods usually require reducing agents to convert Ag+ into Ag0, followed by nucleation and growth that lead to metallic colloidal nanoparticles. Sodium borohydride [12] is the most widely used reagent for the reduction of metallic ions, despite the fact that most reactions involving it require further safety precautions due to their extreme exothermic nature [13, 14]. Additionally, NaBH4 has to be used in large excess because it undergoes hydrolysis when brought into contact with water and metallic surfaces [15]. N,N-dimethylformamide [16] and hydrazine [17] have also been applied as reducing agents for the production of AgNPs. It is important to point out, however, that those chemicals must be carefully handled since they have been implicated in liver disease [18] and cancer [19], respectively. Another point worth mentioning is that nanoparticles require some sort of stabilization (electrostatic [20] or steric [21]) to guarantee their proper availability in solution. Needless to say, it is also desirable that a stabilizing agent be environmentally-compatible for safe handling of the final product.Castor oil is a vegetable oil extracted from seeds of castor bean plant (Ricinus communis L.). Originally used as a laxative folk medicament, castor oil is nowadays employed predominantly in cosmetic industries as a cream base in formulations of skin moisturizers [22]. It is primarily constituted of ricinoleic acid (approximately 90%), which can then be transformed into sodium ricinoleate via alkaline hydrolysis [23]. Teomim et al. [24] hypothesized the use of ricinoleate-based polymers as drug carriers due to their lack of toxicity when tested in rats. Vieira et al. [25] found that topical application of ricinoleic acid exerted exceptional analgesic and anti-inflammatory activity in rats. These features would make castor oil derivatives eligible for nanoparticle synthesis, provided that the 18-carbon fatty acid is capable of preventing aggregation and excessive nanoparticle growth. So far, studies have employed castor oil or ricinoleic acid as dispersive media for stabilization of a variety of nanostructures that include gold nanoparticles produced by sputtering [26] and wet chemistry process [27], quantum dots fabricated through thermolysis [28], and silver and gold nanoparticles in paints [29], as well as silver nanoparticles synthesized via ablation of metallic silver [30]. A question that remains open is whether ricinoleic acid/ricinoleate could function concomitantly as reducing and capping agents in appropriate experimental conditions.Herein we showed, for the first time, that sodium 9,10-epoxy-12-hydroxytetradecanoate (SEAR), an epoxidized derivative of ricinoleic acid, simultaneously functions as reducing and stabilizing agents in the synthesis of silver nanoparticles in alkaline aqueous medium. Recently [31], we showed that molecules bearing hydroxyl groups can reduce gold and silver ions in alkaline media via formation of alkoxides that are the actual reducing agents. Although SEAR has a hydroxyl group at the C-12 position, it is not capable of reducing Ag+. On the other hand, stable AgNPs were obtained by substituting the double bond of the oil skeleton with an epoxide. The concentration of SEAR influenced the rate of AgNPs formation and their size distribution. Finally, we studied the behavior of SEAR-capped AgNPs spiked in sewage from a local wastewater treatment plant. Changes in the UV-Vis signal of the AgNPs suggested that these nanoparticles may be interesting sensor for chemical oxygen demand determination.


## 2. Experimental

### 2.1. Synthesis of SEAR

#### 2.1.1. Castor Oil Alkaline Hydrolysis and Extraction of Ricinoleic Acid

The procedure has been adapted from the work by Castro Dantas et al. [32]. 30.0 g of castor oil was refluxed for 2 h with 6.0 g of KOH (Sigma-Aldrich) dissolved in a mixture of 60 mL of deionized water with 60.0 mL of ethanol (Synth). The product was then washed with water and had its pH adjusted to 4.5 with 30% H2SO4 (Sigma-Aldrich). After adding 20 mL diethyl ether (Sigma-Aldrich), the organic phase (a mixture of fatty acids) was separated and mixed with 3.0 g of Na2SO4 (Sigma-Aldrich) to remove excess water. The mixture was then filtered, the diethyl ether (Synth) was removed in a rotary evaporator, and 50 mL of acetone (Sigma-Aldrich) was added to the fatty acid mixture which was then kept at −10°C for 48 h to promote solidification of fatty acids other than the ricinoleic acid. Afterwards, the two-phase mixture was filtered to separate the liquid ricinoleic acid. Characterization of the ricinoleic acid by FTIR and NMR can be found in Supporting Information (see Supporting Information in the Supplementary Material available online at https://doi.org/10.1155/2017/1230467).


#### 2.1.2. Epoxidation of Ricinoleic Acid and Saponification

Epoxidized ricinoleic acid was synthesized in a two-step process. Firstly, peracetic acid was obtained by slowly mixing 12.5 g of acetic anhydride (Sigma-Aldrich) with 11.6 mL of hydrogen peroxide (Sigma-Aldrich) in an ice bath. After 6 the mixture was stirred magnetically at 500 rpm for 24 h, 20.0 g of ricinoleic acid was added to it, and the chemicals were allowed to react for 3 h in order to obtain the epoxidized ricinoleic acid. Saponification was then carried out by mechanically stirring the epoxidized ricinoleic acid with 1.2 g of NaOH (Sigma-Aldrich) until a white solid was obtained. The process is briefly presented in Scheme1. The epoxidized ricinoleic acid was then characterized with FTIR and NMR (Supporting Information).Scheme 1
Epoxidation of ricinoleic acid.


### 2.2. Synthesis and Characterization of SEAR-Capped AgNPs

The following stock solutions were prepared for the synthesis of AgNPs: 0.10 mol l−1 SEAR, 10 mM AgNO3 (Sigma-Aldrich), and 1.0 mol l−1 NaOH (Sigma-Aldrich). In a typical experiment at room temperature, 80 μl of the AgNO3 solution is diluted in 1920 μl of water. In another vessel, 400 μl of the NaOH solution is added to either 40 μl or 400 μl of the SEAR solution with the final volume taken to 2.0 ml through the addition of water. The SEAR + NaOH mixture is then poured into the diluted AgNO3 to form AgNPs.UV-Vis was performed on an Ocean Optics USB-650 Tide spectrophotometer. Transmission electron microscopy (TEM) images were acquired with a FEI Tecnai G2 Spirit BioTWIN microscope operating at 120 kV and FTIR in ATR mode was carried out with a Bruker Vertex 70 spectrophotometer.


### 2.3. Reaction of AgNPs with Local Sewage

A real effluent (chemical oxygen demand = 920.0 mg L−1) was sampled at the Federal University of Rio Grande do Norte’s wastewater treatment plant (ETE-UFRN) located in the northeast of Brazil. The wastewater is mostly composed of domestic effluents from the UFRN central campus. In order to monitor the reaction between the wastewater sample and AgNPs with UV-Vis spectroscopy, 1.0 mL of wastewater was mixed with 1.0 mL of deionized water in a 1.0 cm path-length cuvette, followed by addition of 1.0 mL SEAR-capped AgNPs. UV-Vis spectra were then recorded at distinct times. In a separate experiment devised to check the constitution of the AgNPs after reacting with wastewater, 50 mL of wastewater was mixed with 50 mL of AgNPs + 50 mL of deionized water and allowed to rest for 15 days. Afterwards, the solution was centrifuged for 15 min and the supernatant was discarded. The AgNPs on the bottom of the flasks were then washed with deionized water to remove soluble species and centrifuged for another 15 min. The AgNPs pellet was dried at 40°C for 4 h and subjected to energy-dispersive X-ray spectroscopy (EDS).


## 2.1. Synthesis of SEAR

### 2.1.1. Castor Oil Alkaline Hydrolysis and Extraction of Ricinoleic Acid

The procedure has been adapted from the work by Castro Dantas et al. [32]. 30.0 g of castor oil was refluxed for 2 h with 6.0 g of KOH (Sigma-Aldrich) dissolved in a mixture of 60 mL of deionized water with 60.0 mL of ethanol (Synth). The product was then washed with water and had its pH adjusted to 4.5 with 30% H2SO4 (Sigma-Aldrich). After adding 20 mL diethyl ether (Sigma-Aldrich), the organic phase (a mixture of fatty acids) was separated and mixed with 3.0 g of Na2SO4 (Sigma-Aldrich) to remove excess water. The mixture was then filtered, the diethyl ether (Synth) was removed in a rotary evaporator, and 50 mL of acetone (Sigma-Aldrich) was added to the fatty acid mixture which was then kept at −10°C for 48 h to promote solidification of fatty acids other than the ricinoleic acid. Afterwards, the two-phase mixture was filtered to separate the liquid ricinoleic acid. Characterization of the ricinoleic acid by FTIR and NMR can be found in Supporting Information (see Supporting Information in the Supplementary Material available online at https://doi.org/10.1155/2017/1230467).


### 2.1.2. Epoxidation of Ricinoleic Acid and Saponification

Epoxidized ricinoleic acid was synthesized in a two-step process. Firstly, peracetic acid was obtained by slowly mixing 12.5 g of acetic anhydride (Sigma-Aldrich) with 11.6 mL of hydrogen peroxide (Sigma-Aldrich) in an ice bath. After 6 the mixture was stirred magnetically at 500 rpm for 24 h, 20.0 g of ricinoleic acid was added to it, and the chemicals were allowed to react for 3 h in order to obtain the epoxidized ricinoleic acid. Saponification was then carried out by mechanically stirring the epoxidized ricinoleic acid with 1.2 g of NaOH (Sigma-Aldrich) until a white solid was obtained. The process is briefly presented in Scheme1. The epoxidized ricinoleic acid was then characterized with FTIR and NMR (Supporting Information).Scheme 1
Epoxidation of ricinoleic acid.


## 2.1.1. Castor Oil Alkaline Hydrolysis and Extraction of Ricinoleic Acid

The procedure has been adapted from the work by Castro Dantas et al. [32]. 30.0 g of castor oil was refluxed for 2 h with 6.0 g of KOH (Sigma-Aldrich) dissolved in a mixture of 60 mL of deionized water with 60.0 mL of ethanol (Synth). The product was then washed with water and had its pH adjusted to 4.5 with 30% H2SO4 (Sigma-Aldrich). After adding 20 mL diethyl ether (Sigma-Aldrich), the organic phase (a mixture of fatty acids) was separated and mixed with 3.0 g of Na2SO4 (Sigma-Aldrich) to remove excess water. The mixture was then filtered, the diethyl ether (Synth) was removed in a rotary evaporator, and 50 mL of acetone (Sigma-Aldrich) was added to the fatty acid mixture which was then kept at −10°C for 48 h to promote solidification of fatty acids other than the ricinoleic acid. Afterwards, the two-phase mixture was filtered to separate the liquid ricinoleic acid. Characterization of the ricinoleic acid by FTIR and NMR can be found in Supporting Information (see Supporting Information in the Supplementary Material available online at https://doi.org/10.1155/2017/1230467).


## 2.1.2. Epoxidation of Ricinoleic Acid and Saponification

Epoxidized ricinoleic acid was synthesized in a two-step process. Firstly, peracetic acid was obtained by slowly mixing 12.5 g of acetic anhydride (Sigma-Aldrich) with 11.6 mL of hydrogen peroxide (Sigma-Aldrich) in an ice bath. After 6 the mixture was stirred magnetically at 500 rpm for 24 h, 20.0 g of ricinoleic acid was added to it, and the chemicals were allowed to react for 3 h in order to obtain the epoxidized ricinoleic acid. Saponification was then carried out by mechanically stirring the epoxidized ricinoleic acid with 1.2 g of NaOH (Sigma-Aldrich) until a white solid was obtained. The process is briefly presented in Scheme1. The epoxidized ricinoleic acid was then characterized with FTIR and NMR (Supporting Information).Scheme 1
Epoxidation of ricinoleic acid.


## 2.2. Synthesis and Characterization of SEAR-Capped AgNPs

The following stock solutions were prepared for the synthesis of AgNPs: 0.10 mol l−1 SEAR, 10 mM AgNO3 (Sigma-Aldrich), and 1.0 mol l−1 NaOH (Sigma-Aldrich). In a typical experiment at room temperature, 80 μl of the AgNO3 solution is diluted in 1920 μl of water. In another vessel, 400 μl of the NaOH solution is added to either 40 μl or 400 μl of the SEAR solution with the final volume taken to 2.0 ml through the addition of water. The SEAR + NaOH mixture is then poured into the diluted AgNO3 to form AgNPs.UV-Vis was performed on an Ocean Optics USB-650 Tide spectrophotometer. Transmission electron microscopy (TEM) images were acquired with a FEI Tecnai G2 Spirit BioTWIN microscope operating at 120 kV and FTIR in ATR mode was carried out with a Bruker Vertex 70 spectrophotometer.


## 2.3. Reaction of AgNPs with Local Sewage

A real effluent (chemical oxygen demand = 920.0 mg L−1) was sampled at the Federal University of Rio Grande do Norte’s wastewater treatment plant (ETE-UFRN) located in the northeast of Brazil. The wastewater is mostly composed of domestic effluents from the UFRN central campus. In order to monitor the reaction between the wastewater sample and AgNPs with UV-Vis spectroscopy, 1.0 mL of wastewater was mixed with 1.0 mL of deionized water in a 1.0 cm path-length cuvette, followed by addition of 1.0 mL SEAR-capped AgNPs. UV-Vis spectra were then recorded at distinct times. In a separate experiment devised to check the constitution of the AgNPs after reacting with wastewater, 50 mL of wastewater was mixed with 50 mL of AgNPs + 50 mL of deionized water and allowed to rest for 15 days. Afterwards, the solution was centrifuged for 15 min and the supernatant was discarded. The AgNPs on the bottom of the flasks were then washed with deionized water to remove soluble species and centrifuged for another 15 min. The AgNPs pellet was dried at 40°C for 4 h and subjected to energy-dispersive X-ray spectroscopy (EDS).


## 3. Results and Discussion

### 3.1. Synthesis and Characterization of SEAR-AgNPs

Gomes et al. [31] presented strong evidences that alkoxides from alcohols, aldehydes, and ketones are the actual reducing species in alkaline media for the generation of silver and gold nanoparticles. In that study, the authors argued that any molecule capable of generating an alkoxide would be eligible for reducing Au3+, Ag+, or a mixture of them, to form their respective nanoparticles. In the present case, SEAR has hydroxyl and epoxide groups in its skeleton. Since the experiments were conducted in alkaline medium, we hypothesized the hydroxyl group on SEAR tail would be deprotonated to some extent and the epoxide ring would be open generating more hydroxyl groups to act as reducing agents. The following results confirm that SEAR is indeed capable of reducing silver ions under the conditions employed in the present study. It is also important to take into consideration that the concentration of the capping agent (in the present study a role also played by SEAR) profoundly impacts on size and shape of nanoparticles, especially if the surfactant forms micelles [33]. Thus, we have selected SEAR concentrations of 1.0 mM and 10.0 mM, which correspond to concentrations below and above the SEAR critical micelle concentration (CMC) [23], respectively, to evaluate their impact on the reduction of Ag+ and posterior stabilization. Figures 1(a) and 1(b) show time-dependent UV-Vis spectra of solutions that resulted from the addition of SEAR to AgNO3 at room temperature and pH 13. Both solutions turned into yellow as a consequence of the formation of AgNPs. The yellow color is due to the surface plasmon band (SPB) that resulted from the resonant coherent dipolar oscillations of the electron gas (electrons of the conduction band) at the surface of nanoparticles [34]. The maximum wavelength in the colloidal AgNPs spectra after 24 h was 408 nm regardless of the SEAR concentration. Although the maximum wavelength [35] is a common parameter used to compare sizes of nanoparticles in a given matrix, a more detailed analysis is provided by the peak width at half maxima (PWHM) as studied by Brown et al. [36]. According to their concept, the smaller the PWHM value the narrower the size distribution of nanoparticles. Comparing the PWHM of AgNPs spectra obtained with 1.0 mM and 10.0 mM SEAR that have roughly the same absorbance (≈1.30), the former and the latter concentrations resulted in 90 nm and 109 nm, respectively, meaning that 1.0 mM SEAR provided somewhat more uniform AgNPs. This result will be further investigated by TEM.Figure 1
UV-Vis spectra of AgNPs produced with (a) 1.0 mM SEAR (red solid circles) and (b) 10.0 mM SEAR (black solid squares) recorded 5 min apart. (c) Evolution of absorbance at 408 nm.Inset. Magnification of the region between 0 min and 50 min. Other conditions: [Ag+] = 0.20 mM, [OH−] = 0.10 M, T=25°C.
(a)
(b)
(c)Figure1(c) presents a plot of the absorbance at 408 nm as a function of time for AgNPs produced with 1.0 mM (red solid circles) and 10.0 mM (black solid squares) SEAR. Interestingly, the formation of AgNPs in both cases passed through an induction period (nucleation process) of approximately 40 min (Figure 1(c), inset) prior to exponential absorbance increase related to autocatalytic growth [37] of AgNPs. Another point is that the absorbances recorded at 1.0 mM SEAR were slightly higher than those at 10.0 mM SEAR up to 40 min (inset of Figure 1(c)). This is also observed in Figures 1(a) and 1(b), where initial spectra from AgNPs produced with 1.0 mM SEAR already present a positive curvature, as opposed to those from 10.0 mM. These results may be reasoned by selecting the CMC as the parameter that divides the two behaviors: before the SEAR CMC of 9.2 mM [23], SEAR molecules are readily available in solution for the reduction of Ag+, leading to quick AgNPs nucleation. After the CMC, on the other hand, SEAR molecules incorporated into micelles must be liberated through disruption of the micelle structure in order to make –OH groups available for further reduction of Ag+. Since we are dealing with normal-phase micelles, hydrophilic “heads” contact water while the hydrophobic tails containing –OH point to the micelle center. Therefore, we concluded that the nucleation process depends on free, soluble SEAR while autocatalytic growth would require disruption of micelles to liberate the –OH hidden in their core.Figure2 depicts TEM images of AgNPs produced with 1.0 mM and 10.0 mM SEAR with their respective size distributions. As seen, the AgNPs were not monodisperse; however, those obtained with 10.0 mM SEAR were substantially larger (51 nm on average) than those from 1.0 mM SEAR (21 nm). The standard deviation also followed the same trend (23 nm, twice the value of that from 1.0 mM SEAR). This result corroborates the PWHM analysis (Figures 1(a) and 1(b)). The micelle structure seems to have played an important role in controlling size and distribution of AgNPs. As shown in Scheme 2, SEAR interacts with silver through hydrophilic heads (as shown later by ATR-FTIR). It is thus safe to assume that there would be a competition between free and micelle SEAR for Ag adsorption sites. At concentrations lower than the CMC, all SEAR molecules on the AgNPs surface interact through heads with AgNPs and the hydrophobic tails prevent excessive nanoparticle growth through steric hindrance. In contrast, at concentrations higher than the CMC, not all SEAR molecules on the AgNPs surface were directly bound to it because the spherical nature of the micelle makes some SEAR molecules point away from the AgNP surface. The micelle structure may not be as effective as free SEAR molecules in stabilizing Ag nuclei, which then led to larger nanoparticles and broader size distribution probably through Ostwald ripening [38].Scheme 2
On left and right sides AgNPs are stabilized by SEAR below and its above CMC, respectively.Figure 2
TEM images of AgNPs obtained with (a) 1.0 mM and (b) 10.0 mM SEAR. Other conditions: [Ag+] = 0.20 mM, [OH−] = 0.10 M, T=25°C.
(a)
(b)FTIR spectra in ATR mode of pure SEAR and SEAR-capped silver nanoparticles are presented in Figure3. As the most relevant region of the SEAR spectrum comprising the range of 1200–1800 cm−1, only this region has been analyzed in detail. The FTIR spectrum of pure SEAR (black line) displayed asymmetrical and symmetrical carboxylate stretching modes at 1564 cm−1 and 1410 cm−1, respectively [39]. Upon stabilization of AgNPs (red line), the center of the asymmetrical stretching band shifts to 1555 cm−1 and the shoulders of the band related to the symmetrical stretching are considerably suppressed. This observation suggests that stabilization of AgNPs occurs via interaction between the SEAR carboxylate and metallic silver. The fact that the asymmetrical stretching mode is shifted to a lower frequency suggests that both oxygen atoms from carboxylate donate an electron pair to vacant silver orbitals, decreasing, in turn, the double bond character due to interference with the carboxylate resonance system that probably chelated with silver symmetrically [40].Figure 3
FTIR in ATR mode of pure SEAR (black line) and SEAR-capped AgNPs (red line).AgNPs have found a myriad of applications that comprise cosmetics, textiles, and food packaging. Inevitably, waste from those products will end up in terrestrial and aquatic ecosystems impacting biotic niche. We have therefore carried out experiments on the behavior of AgNPs in raw sewage from a local wastewater treatment plant in order to determine the fate of the AgNPs upon contact with a real-life system. Similar studies conducted with AgNPs stabilized by citrate [41], polyvinylpyrrolidone [41–43], and TWEEN [41] revealed that silver nanoparticles are prone to sulfidation that leads to Ag2S, which decreased silver nanoparticle toxicity towards a variety of terrestrial eukaryotic organisms [42]. As we envisage the herein produced AgNPs in a variety of applications, it is thus imperative to find out whether they can be transformed into Ag2S in order to mitigate their environmental impact. Figure 4 presents time-dependent UV-Vis spectra of AgNPs in contact with raw sewage, where AgNPs produced with 1.0 mM SEAR (Figure 4(a)) are consumed more quickly than those synthesized with 10.0 mM SEAR (Figure 4(b)), as revealed by the decrease of the surface plasmon resonance (SPB) with time. After 10 days, the intensities of SPB from AgNPs produced with 1.0 mM and 10.0 mM SEAR were 0.060 and 0.71, respectively, showing that the latter is somewhat shielded from sulfidation. Figure 4(c) presents the rate of absorbance decrease at 408 nm for AgNPs produced at both SEAR concentrations. The slopes calculated for both curves show that the sulfidation is faster with AgNPs from 1.0 mM SEAR even in the beginning of the reaction. This result is probably a consequence of a higher concentration of SEAR around the particle in the case of 10.0 mM SEAR, thus hampering the access of sulfur-containing species to the nanoparticle surface. The nanoparticle size is another factor that may have played a role in sulfidation. Kaegi et al. [41] found that smaller silver nanoparticles are subjected to higher degree of sulfidation than bigger nanoparticles, a result that corroborates those found in the present work. EDS conducted on AgNPs that reacted with raw sewage revealed the presence of sulfur confirming that sulfidation took place. At this point we are not able to determine whether sulfur is located only on the surface of the AgNPs or in their interior as well. Although the structure of the silver sulfide nanoparticles remains elusive (it is beyond the scope of the present study), the fact that the AgNPs produced herein are indeed prone to sulfidation makes them adequate for a variety of real-life applications.Figure 4
UV-Vis spectra of AgNPs produced with (a) 1.0 mM SEAR and (b) 10.0 mM SEAR in contact with raw sewage. (c) Absorbance recorded at 408 nm as a function of time for AgNPs.
(a)
(b)
(c)


## 3.1. Synthesis and Characterization of SEAR-AgNPs

Gomes et al. [31] presented strong evidences that alkoxides from alcohols, aldehydes, and ketones are the actual reducing species in alkaline media for the generation of silver and gold nanoparticles. In that study, the authors argued that any molecule capable of generating an alkoxide would be eligible for reducing Au3+, Ag+, or a mixture of them, to form their respective nanoparticles. In the present case, SEAR has hydroxyl and epoxide groups in its skeleton. Since the experiments were conducted in alkaline medium, we hypothesized the hydroxyl group on SEAR tail would be deprotonated to some extent and the epoxide ring would be open generating more hydroxyl groups to act as reducing agents. The following results confirm that SEAR is indeed capable of reducing silver ions under the conditions employed in the present study. It is also important to take into consideration that the concentration of the capping agent (in the present study a role also played by SEAR) profoundly impacts on size and shape of nanoparticles, especially if the surfactant forms micelles [33]. Thus, we have selected SEAR concentrations of 1.0 mM and 10.0 mM, which correspond to concentrations below and above the SEAR critical micelle concentration (CMC) [23], respectively, to evaluate their impact on the reduction of Ag+ and posterior stabilization. Figures 1(a) and 1(b) show time-dependent UV-Vis spectra of solutions that resulted from the addition of SEAR to AgNO3 at room temperature and pH 13. Both solutions turned into yellow as a consequence of the formation of AgNPs. The yellow color is due to the surface plasmon band (SPB) that resulted from the resonant coherent dipolar oscillations of the electron gas (electrons of the conduction band) at the surface of nanoparticles [34]. The maximum wavelength in the colloidal AgNPs spectra after 24 h was 408 nm regardless of the SEAR concentration. Although the maximum wavelength [35] is a common parameter used to compare sizes of nanoparticles in a given matrix, a more detailed analysis is provided by the peak width at half maxima (PWHM) as studied by Brown et al. [36]. According to their concept, the smaller the PWHM value the narrower the size distribution of nanoparticles. Comparing the PWHM of AgNPs spectra obtained with 1.0 mM and 10.0 mM SEAR that have roughly the same absorbance (≈1.30), the former and the latter concentrations resulted in 90 nm and 109 nm, respectively, meaning that 1.0 mM SEAR provided somewhat more uniform AgNPs. This result will be further investigated by TEM.Figure 1
UV-Vis spectra of AgNPs produced with (a) 1.0 mM SEAR (red solid circles) and (b) 10.0 mM SEAR (black solid squares) recorded 5 min apart. (c) Evolution of absorbance at 408 nm.Inset. Magnification of the region between 0 min and 50 min. Other conditions: [Ag+] = 0.20 mM, [OH−] = 0.10 M, T=25°C.
(a)
(b)
(c)Figure1(c) presents a plot of the absorbance at 408 nm as a function of time for AgNPs produced with 1.0 mM (red solid circles) and 10.0 mM (black solid squares) SEAR. Interestingly, the formation of AgNPs in both cases passed through an induction period (nucleation process) of approximately 40 min (Figure 1(c), inset) prior to exponential absorbance increase related to autocatalytic growth [37] of AgNPs. Another point is that the absorbances recorded at 1.0 mM SEAR were slightly higher than those at 10.0 mM SEAR up to 40 min (inset of Figure 1(c)). This is also observed in Figures 1(a) and 1(b), where initial spectra from AgNPs produced with 1.0 mM SEAR already present a positive curvature, as opposed to those from 10.0 mM. These results may be reasoned by selecting the CMC as the parameter that divides the two behaviors: before the SEAR CMC of 9.2 mM [23], SEAR molecules are readily available in solution for the reduction of Ag+, leading to quick AgNPs nucleation. After the CMC, on the other hand, SEAR molecules incorporated into micelles must be liberated through disruption of the micelle structure in order to make –OH groups available for further reduction of Ag+. Since we are dealing with normal-phase micelles, hydrophilic “heads” contact water while the hydrophobic tails containing –OH point to the micelle center. Therefore, we concluded that the nucleation process depends on free, soluble SEAR while autocatalytic growth would require disruption of micelles to liberate the –OH hidden in their core.Figure2 depicts TEM images of AgNPs produced with 1.0 mM and 10.0 mM SEAR with their respective size distributions. As seen, the AgNPs were not monodisperse; however, those obtained with 10.0 mM SEAR were substantially larger (51 nm on average) than those from 1.0 mM SEAR (21 nm). The standard deviation also followed the same trend (23 nm, twice the value of that from 1.0 mM SEAR). This result corroborates the PWHM analysis (Figures 1(a) and 1(b)). The micelle structure seems to have played an important role in controlling size and distribution of AgNPs. As shown in Scheme 2, SEAR interacts with silver through hydrophilic heads (as shown later by ATR-FTIR). It is thus safe to assume that there would be a competition between free and micelle SEAR for Ag adsorption sites. At concentrations lower than the CMC, all SEAR molecules on the AgNPs surface interact through heads with AgNPs and the hydrophobic tails prevent excessive nanoparticle growth through steric hindrance. In contrast, at concentrations higher than the CMC, not all SEAR molecules on the AgNPs surface were directly bound to it because the spherical nature of the micelle makes some SEAR molecules point away from the AgNP surface. The micelle structure may not be as effective as free SEAR molecules in stabilizing Ag nuclei, which then led to larger nanoparticles and broader size distribution probably through Ostwald ripening [38].Scheme 2
On left and right sides AgNPs are stabilized by SEAR below and its above CMC, respectively.Figure 2
TEM images of AgNPs obtained with (a) 1.0 mM and (b) 10.0 mM SEAR. Other conditions: [Ag+] = 0.20 mM, [OH−] = 0.10 M, T=25°C.
(a)
(b)FTIR spectra in ATR mode of pure SEAR and SEAR-capped silver nanoparticles are presented in Figure3. As the most relevant region of the SEAR spectrum comprising the range of 1200–1800 cm−1, only this region has been analyzed in detail. The FTIR spectrum of pure SEAR (black line) displayed asymmetrical and symmetrical carboxylate stretching modes at 1564 cm−1 and 1410 cm−1, respectively [39]. Upon stabilization of AgNPs (red line), the center of the asymmetrical stretching band shifts to 1555 cm−1 and the shoulders of the band related to the symmetrical stretching are considerably suppressed. This observation suggests that stabilization of AgNPs occurs via interaction between the SEAR carboxylate and metallic silver. The fact that the asymmetrical stretching mode is shifted to a lower frequency suggests that both oxygen atoms from carboxylate donate an electron pair to vacant silver orbitals, decreasing, in turn, the double bond character due to interference with the carboxylate resonance system that probably chelated with silver symmetrically [40].Figure 3
FTIR in ATR mode of pure SEAR (black line) and SEAR-capped AgNPs (red line).AgNPs have found a myriad of applications that comprise cosmetics, textiles, and food packaging. Inevitably, waste from those products will end up in terrestrial and aquatic ecosystems impacting biotic niche. We have therefore carried out experiments on the behavior of AgNPs in raw sewage from a local wastewater treatment plant in order to determine the fate of the AgNPs upon contact with a real-life system. Similar studies conducted with AgNPs stabilized by citrate [41], polyvinylpyrrolidone [41–43], and TWEEN [41] revealed that silver nanoparticles are prone to sulfidation that leads to Ag2S, which decreased silver nanoparticle toxicity towards a variety of terrestrial eukaryotic organisms [42]. As we envisage the herein produced AgNPs in a variety of applications, it is thus imperative to find out whether they can be transformed into Ag2S in order to mitigate their environmental impact. Figure 4 presents time-dependent UV-Vis spectra of AgNPs in contact with raw sewage, where AgNPs produced with 1.0 mM SEAR (Figure 4(a)) are consumed more quickly than those synthesized with 10.0 mM SEAR (Figure 4(b)), as revealed by the decrease of the surface plasmon resonance (SPB) with time. After 10 days, the intensities of SPB from AgNPs produced with 1.0 mM and 10.0 mM SEAR were 0.060 and 0.71, respectively, showing that the latter is somewhat shielded from sulfidation. Figure 4(c) presents the rate of absorbance decrease at 408 nm for AgNPs produced at both SEAR concentrations. The slopes calculated for both curves show that the sulfidation is faster with AgNPs from 1.0 mM SEAR even in the beginning of the reaction. This result is probably a consequence of a higher concentration of SEAR around the particle in the case of 10.0 mM SEAR, thus hampering the access of sulfur-containing species to the nanoparticle surface. The nanoparticle size is another factor that may have played a role in sulfidation. Kaegi et al. [41] found that smaller silver nanoparticles are subjected to higher degree of sulfidation than bigger nanoparticles, a result that corroborates those found in the present work. EDS conducted on AgNPs that reacted with raw sewage revealed the presence of sulfur confirming that sulfidation took place. At this point we are not able to determine whether sulfur is located only on the surface of the AgNPs or in their interior as well. Although the structure of the silver sulfide nanoparticles remains elusive (it is beyond the scope of the present study), the fact that the AgNPs produced herein are indeed prone to sulfidation makes them adequate for a variety of real-life applications.Figure 4
UV-Vis spectra of AgNPs produced with (a) 1.0 mM SEAR and (b) 10.0 mM SEAR in contact with raw sewage. (c) Absorbance recorded at 408 nm as a function of time for AgNPs.
(a)
(b)
(c)


## 4. Conclusion

We have shown that SEAR, a surfactant derived from ricinoleic acid, is capable of acting as reducing and capping agents in the synthesis of silver nanoparticles in alkaline medium. The fact that SEAR may form micelles had an impact on size and distribution of AgNPs. Finally, in addition to SEAR being environmentally benign, the toxicological effects of AgNPs on the environment are mitigated because AgNPs are subjected to sulfidation upon contact with raw sewage. These findings may propel these AgNPs into broader field of applications such as sensors and environmental remediation.



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*Source: 1230467-2017-03-23.xml*