# Functionalized-AgNPs for Long-Term Stability and Its Applicability in the Detection of Manganese Ions

Authors: Van-Tuan Hoang; Mai Mai; Le Thi Tam; Ngoc Phan Vu; Nguyen Tien Khi; Phuong Dinh Tam; Tran Quang Huy; Anh-Tuan Le; Ngo Xuan Dinh; Vinh-Hoang Tran
Journal: Advances in Polymer Technology
 (2020)

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## Abstract

In this study, silver nanoparticles (AgNPs) were functionalized by various molecules, including sodium borohydride (NaBH4), polyhexamethylene biguanide hydrochloride (PHMB), and Tween 80 to investigate the long-term stabilization of AgNPs in an aqueous dispersion. PHMB-functionalized silver nanoparticles (AgNPs/PHMB) exhibited better stability than others and could be stored at ambient temperature for at least 180 days. In addition to creating stabilization based on the electrostatic repulsion, the use of PHMB helped to increase the degree of stability of the colloidal AgNPs for a long time owing to strong interactions between Ag atoms on AgNPs with nitrogen (N) positions in PHMB molecules. The formed bond led to improving maintenance ability of the electrostatic repulsion layer among independent nanoparticles. The applicability of the as-prepared AgNPs/PHMB was also examined for Mn2+ detection via a colorimetric approach. The calibration curve was found to be linear over the range of 0–100 mM with a correlation coefficient of 0.97. The amine groups of PHMB brought out a cooperative effect to form of ion-templated chelation with Mn2+, which caused the aggregation of AgNPs/PHMB. This suggested that the AgNPs/PHMB could be used as a potential probe in the detection of Mn2+ ions. More importantly, the long-term stability of AgNPs/PHMB paved a great promising path to provide many further solutions for the producer in practical applications.


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## Body

## 1. Introduction

Silver nanoparticles (AgNPs) possess many unique chemical and physical properties; therefore, AgNPs have been widely studied and exploited in various applications, including medical, home appliances, electronics, textiles, and cosmetics [1]. The demand for AgNPs in the world is projected to increase, with production estimated at around 320 tons per year [1,2]. However, the properties of AgNPs strongly depend on their size, shape, and crystallinity. Moreover, large specific surface area and high surface energy lead to the self-aggregation of AgNPs during storing time, which considerably decreases their activity as well as applicability. These indicate that the stabilization of colloidal AgNPs is one of the most essential factors for developing practical applications [3–5]. Furthermore, the use of suitable stabilizers not only helps prevent the aggregation of AgNPs but also increases their activity. Therefore, many recent efforts have been performed to functionalize AgNPs by different stabilizers such as polymer or functional molecules, which contain amine groups/carboxylic acid groups/or thiol groups, etc., and due to these, the functional groups can form coordination bonding and/or electrostatic interactions with AgNPs [6–8].Especially, herein, the polymer, which has many functional groups and high viscosity, has been considered as a promising stabilizer for the synthesis of AgNPs. Of the stabilizers used, the ionic stabilizers showed better stability than nonionic stabilizers. When silver nanoparticles are modified by an anionic stabilizer, their surface will electrically be charged. This leads to enhancing electrostatic repulsion among them, and as a result, the aggregation of colloidal AgNPs can be prevented [8]. Therefore, the cationic polymers such as polyhexamethylene biguanide hydrochloride (PHMB), chitosan (CS) [6,9], and polyethylenimine (PEI) [10], with molecule structures described in Figures 1(a)–1(c), respectively, are often used for stabilization of AgNPs. In such polymers, polyhexamethylene biguanide hydrochloride (PHMB), a surface-active agent, positively charged, highly biocompatible, and has been used as a disinfectant in medical, textile, and food industries [11,12], can stabilize the size and increase the dispersion of AgNPs. PHMB preserves the colloidal AgNPs for better stability and uniform dispersibility in the liquid media. Previous studies [11,13] showed that the PHMB-stabilized cationic silver nanoparticles displayed enhanced antimicrobial activity and demonstrated the promising potential for plant protection. However, the mechanism of durability and long-term stability of the colloidal AgNPs by ionic stabilizers may have been not fully understood.Figure 1
Chemical structure and functional groups of (a) polyhexamethylene biguanide hydrochloride (PHMB); (b) chitosan (CS), and (c) polyethylenimine (PEI).
(a)
(b)
(c)Manganese (Mn) element is an essential element of living organisms. The existence of the Mn element plays a critical role in the metabolism of the body and other biological processes. However, when using foods, especially drinking water with high Mn2+ ions content will cause harm to the human body, especially diseases related to the nervous system [14]. Some recent studies have shown that the colloidal AgNP-based colorimetric sensors for Mn ion detection have offered good sensitivity [15,16]. However, these colloidal AgNPs had short-term stability or have to use many stabilizers, which hinder their widespread applications. Therefore, the synthesis of the colloidal AgNPs with both long-term stability and flexibility is sustainable for practical application.In this work, the AgNPs were functionalized by PHMB for long-term stability. Mechanism of the long-term stabilization of the AgNPs/PHMB was discussed. The aggregation of AgNPs/PHMB can be prevented by the electrostatic repulsion among them and the formation of the Ag-N coordinate covalent bonds. Besides, the AgNPs/PHMB with long-term stability have also been harnessed as a probe for the detection of Mn2+ ions by the colorimetric assays. The amine groups of PHMB brought out a cooperative effect to form ion-templated chelation with Mn2+, which caused the aggregation of AgNPs/PHMB.


## 2. Materials and Experimental

### 2.1. Materials

Silver nitrate (AgNO3, 99.9%), sodium borohydride (NaBH4, 99%), polyhexamethylene biguanide hydrochloride (powder, PHMB 98%), Tween 80 (polysorbate 80, 99%), Mn(NO3)2·4H2O, Co(NO3)2·6H2O, and Ni(NO3)2·6H2O were purchased from Shanghai Chemical Reagent. Deionized water was used. All chemicals were used without further purification.


### 2.2. Synthesis of the Functionalized AgNPs

The AgNPs/PHMB, AgNPs/Tween 80, and AgNPs/NaBH4 were prepared by the chemical reduction method using NaBH4 as a reducing agent along with PHMB or Tween 80 as stabilizers according to the following procedure: 60 mL of AgNO3 (1 mM) solution was added dropwise into a 30 mL of aqueous solution containing each stabilizer (0.02 mg/mL) under continuous stirring. After 2 h, 6 mL of sodium borohydride (NaBH4) solution (10 mM, 1 : 1 to the molar ratio of AgNO3) was added dropwise into the mixture. The reduction process was carried out for 3 h (optimized synthesis time) at room temperature (RT). Stirring was required during the synthesis procedure. The formation of AgNPs was proposed, according to [17]equation (1). Finally, the as-prepared functionalized-AgNPs were stored at room temperature in the dark until further use:(1)AgNO3+NaBH4⟶Ag+12H2+12B2H6+NaNO3.


### 2.3. Characterization

The crystalline structure of AgNPs was examined using X-ray diffraction (XRD, Bruker D5005) using CuKα radiation (λ = 0.154 nm) at a step of 0.02° (2θ) at room temperature. The UV-Vis absorbance spectra of the colloidal AgNPs were recorded by using a DR6000 spectrophotometer, and 10 mm path length quartz cuvettes were used for the measurement of the spectra. The surface chemistry of the colloidal AgNPs was examined by using Fourier Transform Infrared Spectrophotometer (IRAffinity-1S, Shimadzu).


### 2.4. Long-Term Stability Measurements

The as-prepared colloidal AgNPs were stored in glass bottles under ambient temperature in the absence of light and were characterized by UV-Vis spectra in few hours and after 180 days of storage. In brief, 0.5 ml of the as-prepared colloidal AgNPs solution at pH 6.8 was diluted with 9.5 ml of the distilled deionized water. The UV-Vis absorbance spectra were recorded by a DR6000 spectrophotometer. In addition, the surface charge and particle size distributions of the colloidal AgNPs were also measured at 2 hours and 180 days of storage using a particle size analyzer (Zetasizer Ver. 6.20, Malvern Instruments) to study the long-term stability of the colloidal AgNPs.


### 2.5. Colorimetric Detection of Mn2+ Ions

For the detection of Mn2+ ions, 1 ml of the as-prepared colloidal AgNPs at pH 6.8 was diluted 9 times by distilled deionized water. Then, 1 ml of Mn2+ solution with various concentrations (0–100 mM) was added into 9 ml diluted colloidal AgNPs. The pH of the solution was adjusted to within the range of 3.5 to 9.0 using acetic acid (0.05%) and NH4OH (30%). The mixture was kept in a shaker for 15 minutes at room temperature before the absorbance spectrum of this mixture was recorded. The limit of detection was calculated by using the following equation:(2)LOD=3Sb,where S is the standard deviation of the blank solution and b is the slope of the analytical curve.


## 2.1. Materials

Silver nitrate (AgNO3, 99.9%), sodium borohydride (NaBH4, 99%), polyhexamethylene biguanide hydrochloride (powder, PHMB 98%), Tween 80 (polysorbate 80, 99%), Mn(NO3)2·4H2O, Co(NO3)2·6H2O, and Ni(NO3)2·6H2O were purchased from Shanghai Chemical Reagent. Deionized water was used. All chemicals were used without further purification.


## 2.2. Synthesis of the Functionalized AgNPs

The AgNPs/PHMB, AgNPs/Tween 80, and AgNPs/NaBH4 were prepared by the chemical reduction method using NaBH4 as a reducing agent along with PHMB or Tween 80 as stabilizers according to the following procedure: 60 mL of AgNO3 (1 mM) solution was added dropwise into a 30 mL of aqueous solution containing each stabilizer (0.02 mg/mL) under continuous stirring. After 2 h, 6 mL of sodium borohydride (NaBH4) solution (10 mM, 1 : 1 to the molar ratio of AgNO3) was added dropwise into the mixture. The reduction process was carried out for 3 h (optimized synthesis time) at room temperature (RT). Stirring was required during the synthesis procedure. The formation of AgNPs was proposed, according to [17]equation (1). Finally, the as-prepared functionalized-AgNPs were stored at room temperature in the dark until further use:(1)AgNO3+NaBH4⟶Ag+12H2+12B2H6+NaNO3.


## 2.3. Characterization

The crystalline structure of AgNPs was examined using X-ray diffraction (XRD, Bruker D5005) using CuKα radiation (λ = 0.154 nm) at a step of 0.02° (2θ) at room temperature. The UV-Vis absorbance spectra of the colloidal AgNPs were recorded by using a DR6000 spectrophotometer, and 10 mm path length quartz cuvettes were used for the measurement of the spectra. The surface chemistry of the colloidal AgNPs was examined by using Fourier Transform Infrared Spectrophotometer (IRAffinity-1S, Shimadzu).


## 2.4. Long-Term Stability Measurements

The as-prepared colloidal AgNPs were stored in glass bottles under ambient temperature in the absence of light and were characterized by UV-Vis spectra in few hours and after 180 days of storage. In brief, 0.5 ml of the as-prepared colloidal AgNPs solution at pH 6.8 was diluted with 9.5 ml of the distilled deionized water. The UV-Vis absorbance spectra were recorded by a DR6000 spectrophotometer. In addition, the surface charge and particle size distributions of the colloidal AgNPs were also measured at 2 hours and 180 days of storage using a particle size analyzer (Zetasizer Ver. 6.20, Malvern Instruments) to study the long-term stability of the colloidal AgNPs.


## 2.5. Colorimetric Detection of Mn2+ Ions

For the detection of Mn2+ ions, 1 ml of the as-prepared colloidal AgNPs at pH 6.8 was diluted 9 times by distilled deionized water. Then, 1 ml of Mn2+ solution with various concentrations (0–100 mM) was added into 9 ml diluted colloidal AgNPs. The pH of the solution was adjusted to within the range of 3.5 to 9.0 using acetic acid (0.05%) and NH4OH (30%). The mixture was kept in a shaker for 15 minutes at room temperature before the absorbance spectrum of this mixture was recorded. The limit of detection was calculated by using the following equation:(2)LOD=3Sb,where S is the standard deviation of the blank solution and b is the slope of the analytical curve.


## 3. Results and Discussion

### 3.1. Structural Analysis

Figure2 shows the XRD spectra of colloidal AgNPs stabilized by PHMB (curve a), Tween 80 (curve b), and NaBH4 (curve c), respectively. It can be seen that four specific diffraction peaks of AgNPs at 2θ = 38.1°, 44.3°, 64.4°, and 77.5° correspond to the crystals (111), (200), (220), and (311) of the silver metal crystal (JC PDS No. 04-0783). These results confirm the formation of the silver metal crystal with a relative single-phase structure in colloidal AgNPs. However, the intensity and sharpness of diffraction peaks in samples using various stabilizers are different. This indicates the stabilizer effect on the particle size of AgNPs as well as the quality of silver metal crystals. Line broadening in the pattern can be quantitatively evaluated using the Debye–Scherrer equation (equation (3)), which gives a relationship between peak broadening in XRD and particle size [18]:(3)D=k⋅λβ⋅cosθ,where D is the thickness of the crystal, k is the Debye–Scherrer constant (0.9), λ is the X-ray wavelength (0.15406 nm), β is the line broadening in radian obtained from the full width at half maximum, and θ is the Bragg angle. According to the Debye–Scherrer equation, average particle sizes of AgNPs were estimated to be 25, 20, and 15 nm when the used stabilizers were PHMB, Tween 80, and NaBH4, respectively.Figure 2
XRD diffraction pattern of the colloidal Ag-NPs stabilized by (a) PHMB, (b) Tween 80, and (c) NaBH4.


### 3.2. Long-Term Stability of the Colloidal AgNPs

UV-Vis can be used to observe the stabilization of AgNP colloids. Stable AgNP colloid in the UV-Vis spectra was stable vs. storing time, suggesting that particle size was stable and without any aggregation. The position of the plasmonic peak in the UV-Vis spectrum depends on the average particle sizes and shapes [19]. Figure 3 shows the optical absorption spectra of the colloidal AgNPs with modified surfaces by different stabilizers as prepared (black solid line) and after 6 months of storage (red dash line). Figure 3 shows that as prepared, all synthesized AgNPs samples illustrated the appearance of the characteristic AgNP peaks at a maximum adsorption of λmax = 400 nm, 440 nm, and 420 nm, corresponding to NaBH4, PHMB, and Tween 80, respectively (black solid lines). However, after 180 days of storage, UV-Vis absorption spectra of these samples were decreased for all tested samples. The strongest decrease can be observed in the case of Tween 80 and NaBH4, respectively, and the peak absorption characteristic of silver nanoparticles was almost absent (red dash line in Figures 3(b) and 3(c)). In contrast, AgNP colloid was stabilized well by PHMB, and it still exists as the specific peak of AgNPs at λmax = 455 nm with a small reduction in absorption intensity. Clearly, this result indicated an excellent role of PHMB as a stabilizer to AgNP colloid than that of NaBH4 or Tween 80. Besides, in Figure 3(a), after 6 months, the specific peak of AgNPs is λmax = 455 nm, and there is a small red shift, compared with λmax = 400 nm as-prepared samples, this can be attributed to a small aggregation that was formed in the AgNPs/PHMB system. The small aggregation in the AgNPs/PHMB system can also be observed by the DLS spectra (Figure 4). Two zones of size distribution as-prepared AgNPs/PHMB and small shoulder can be seen in Figure 4(a) with a mean particles size around 60 nm.Figure 3
UV-Vis absorbance spectrum of the colloidal Ag-NPs stabilized by (a) PHMB, (b) Tween 80, and (c) NaBH4.
(a)
(b)
(c)Figure 4
Size distribution for long term of the colloidal Ag-NPs stabilized by PHMB ((a) 2 hours; (b) 180 days).
(a)
(b)After 6 months of storage, a shoulder was disappeared (Figure4(b)); however, two zones of size distribution were still observed and the mean size was shifted to 105 nm, which is bigger than that as prepared. These analyst results are completely consistent with the above UV-Vis measurements, as well as zeta potential measurements (Table 1). The surface charge of AgNP colloids with various used stabilizers was analysed by zeta potential measurements. The structure is formed by the surface interactions between AgNPs and stabilizer molecules which changes over time. In particular, Table 1 shows that the surface of modified AgNPs by ionic stabilizers (including NaBH4 and PHMB) had less time-varying changes in zeta potential (±% vs. storage time) than that of the nonionic stabilizer (i.e., Tween 80). After 180 days, AgNPs/PHMB showed better stability than the other stabilizers (Table 1). Moreover, the long-term stability of the colloidal AgNPs stabilized by PHMB when compared with other stabilizers or surfactants as shown in Table 2. In this study, the colloidal AgNPs stabilized by PHMB for stability up to 180 days, which promises for many application fields, such as biomedical, agricultural, and environmental control.Table 1
Effect of stabilizers on zeta potential after 180 days.
Stabilizers
Zeta potential (mV)
2 hours
180 days
±(%) zeta potential change after 180 days
PHMB
31.5
26.5
−15.87
NaBH4
−25.5
−6.62
−74.04
Tween 80
−7.9
−0.02
−99.75Table 2
Long-term stability of the colloidal AgNPs.
Methods
Precursors
Reducing agent
Stabilizer or surfactant
Stability time
Ref.
Chemical synthesis
AgNO3
Citrate
Citrate/gelatin mixture
118 days
[3]
Chemical synthesis
AgNO3
NaBH4
Aminosilanes
30 days
[9]
Chemical synthesis
AgNO3
NaBH4
β-Cyclodextrin, adamantine
14 days
[16]
Chemical synthesis
AgNO3
NaBH4
Dodecanethiol
60 days
[7]
Green synthesis
AgNO3
NaBH4
L-Cysteine
60 days
[20]
Biological synthesis
AgNO3
Bacterial biomass
Bacterial biomass
90 days
[21]
Chemical synthesis
AgNO3
NaBH4
PHMB
180 days
This study


### 3.3. Understanding the Mechanism of the Colloidal AgNPs Stabilized by PHMB

A mechanism for long-term stability of AgNPs stabilized by PHMB can be proposed as described in Figure5. Based on the electron configuration of silver (Ag0) is [Kr] 4d105s1, there are many vacant orbitals on the covalent shell of silver atoms including 5p05 d0. Meanwhile, there are many free-electron pairs (unbonded covalence electron pairs) at nitrogen (N) positions on PHMB including -N¨H-7 and/or -N¨ = groups; therefore, coordination interaction of vacant-covalent orbitals of Ag with free-electron pairs of nitrogen in PHMB molecules has been generated, and as a result, the PHMB molecules protect AgNPs as modelled in Figure 5(a). More interestingly, the inside-bonding structure of Ag into AgNPs with PHMB molecules are given in Figure 5(b), which suggested that AgNPs stabilized by PHMB were positively charged; therefore, in the AgNPs/PHMB, the stability of the electrostatic shield around AgNPs was enhanced by the formation of coordinate covalent bonds between the atoms of silver metal and nitrogen in the composition of PHMB (Figure 5(b)). According to this structure (Figure 5(b)), in the colloidal solution, AgNPs were separated from each other by the repulsion layer because of an electrostatic shield that protected the AgNPs surface in the form of positively charged spheres (Figure 5(c)). Thus, AgNPs tend to push each other and survive independently. Electrostatic repulsion of stabilizing agents on the surface of AgNPs is considered an important factor to improve the stability of the colloidal AgNPs [3].Figure 5
Schematic representation of AgNPs/PHMB: (a) NaBH4 reduction Ag+ to AgNPs in the presence of PHMB; (b) the formation of the coordinate covalent bond between silver metal atoms (Ag0) and free-covalence electron pairs of the nitrogen (N) atom in PHMB molecules; and (c) mechanism stabilization of the AgNPs/PHMB via repulsion force AgNPs/PHMB particles.The coordination interaction of vacant-covalent orbitals of Ag with free-electron pairs of nitrogen in PHMB molecules was further confirmed by the FTIR analysis. The FTIR spectra of PHMB and AgNPs/PHMB are shown in Figure6. Compared with PHMB, the FTIR spectrum of AgNPs/PHMB shows one new absorption peak at 1000 cm−1 which corresponds to C-N bond stretching [22] and the disappearance of the absorption peak at 1556 cm−1 [11]. The occurrence of these changes indicates the interaction of the AgNPs with imine groups of PHMB through the formation of a coordination bond of Ag-N. The FTIR results demonstrate that the strong interactions of AgNPs and PHMB may efficiently prevent the aggregation of silver nanoparticles [23].Figure 6
FTIR spectra (a) PHMB and (b) AgNPs stabilized by PHMB (AgNPs/PHMB).For NaBH4-stabilized colloidal AgNPs, the AgNPs were also stabilized by the charging shell covering the AgNPs. However, the electrostatic shield was created by the BH4− anion and was broken as given in the following reaction:(4)BH4−+4H2O⟶BOH4+4H2.Therefore, the degradation ofBH4− to hydrogen gas is the major cause of AgNPs to be aggregated [2,24]. With structure as shown in Figure 3(b) , Tween 80 is a nonionic stabilizer; therefore, the interaction between Tween 80 and the AgNPs is based on the surface adsorption. The AgNPs surface was coated by a layer of Tween 80 to separate the nanoparticles and create great stability based on the steric repulsion mechanism [8,25]. Our finding results reveal that the long-term stability of the colloidal AgNPs was attributed to the formation of Ag-N coordinate covalent bonds and the electrostatic repulsion between PHMB-functionalized AgNPs.


### 3.4. Application of AgNPs/PHMB as a Probe for the Detection of Mn2+ Ions

As described in Section3.3, PHMB coated the AgNPs, therefore, AgNPs/PHMB particles contain free-amino groups, which were from a terminal tail of PHMB (Figure 7). The free -NH2 group can be used to recognize transition metal ions via a colorimetric approach, such as Mn2+ with the detection mechanism as shown in Figure 7. For Mn2+ detection, AgNP play the role to be a signal probe along with the free amino (-NH2) group on PHMB molecules plays the role as a chemical capture probe. The presence of functional groups, such as amine (-NH2), on the surface of AgNPs plays a critical role in the aggregation mechanism through metal-ligand interactions. The amino groups of PHMB have a cooperative effect to form ion-templated chelation with Mn2+, which causes the aggregation of AgNPs [15]. On the contrary, the AgNP aggregation is induced by interparticle bond formation (cross-linking aggregation). The chelation form changes the interparticle distances of AgNPs, leading to the shift of the absorption peak of AgNPs to a longer wavelength. Therefore, cross-linking aggregation has been used for the detection of metal ions [26].Figure 7
Mechanism of Mn2+-induced AgNPs/PHMB aggregation.For that, control testes have been done based on adding 10 mM of various ions including Ni2+, Co2+, and Mn2+ into the AgNPs/PHMB solution. The UV-Vis spectra of the AgNPs/PHMB solution before and after adding a solution containing the above ions are shown in Figure 8(a). It can be seen that the maximal absorption peak of the AgNPs/PHMB solution after adding the Mn2+ ion (curve iv) was strongly diminished than the original AgNPs/PHMB solution (curve i), as well as this decrease was stronger than adding other ions such as Ni2+ (curve ii) or Co2+ (curve iii). These indicated the specific Mn2+ detection of the proposed method. The PHMB polymer can be used as a strong chelating agent to Mn(II) ions due to the amino groups which can form stable complexes with Mn(II) ions. The N atom and amino groups of the PHMB structure can form coordinated bonds with manganese ions causing the aggregation of large particles, which is in good agreement with similar previous reports [15,16,26] in which the sulfonic group, hydroxyl group, and/or carboxyl groups have been considered as an important chelator in specific recognition with Mn2+ ions.Figure 8
Colorimetric detection of Mn2+ ions using the colloidal Ag-NPs: (a) UV-Vis spectra of AgNPs/PHMB without and with adding Co2+, Ni2+, and Mn2+ solution; (b) the UV-Vis spectra of AgNPs/PHMB solutions with different pH ranging from pH 3.5 to pH 9.0 after adding 10 mM Mn2+ solution; (c) UV-Vis spectra of AgNPs/PHMB in the presence of Mn2+ with different concentrations from 0 to 100 mM; and (d) a calibration curve for Mn2+ detection.
(a)
(b)
(c)
(d)To investigate the effect of pH on the sensitivity of this colorimetric method to Mn2+, the AgNPs/PHMB solution was added with 10 mM Mn2+ solution at different pH (from pH 3.5 to pH 9.0) and UV-Vis spectra are shown in Figure 8(b). It can be seen that when the pH value was less than 6.5, the UV-Vis spectra of the AgNPs/PHMB solution were unchanged after adding Mn2+ because the -NH2 group of PHMB is changed to -NH3+, a positively charged group; therefore, Mn2+ cannot interact to these positively charged groups. As the pH value was higher than pH 8, it is noticed that the aggregation of AgNPs/PHMB, as well as Mn2+, would be precipitated as the Mn(OH)2 form. At pH 6.5 to pH 7.5, the intensity and position of the maximum adsorption peaks changed more clearly; therefore, pH in the range 6.5 to 7.5 was selected for further experiments.In the UV-Vis spectra of AgNPs/PHMB added with different Mn2+ concentrations (Figure 8(c)), we notice that the intensity of the maximal absorption peak (at λmax = 403 nm) was decreased with increasing Mn2+ ion concentrations. In addition, there was a red shift of this peak, which could be attributed to the cause of the AgNPs/PHMB aggregation via Mn2+ as linkers. The linear relationship between the absorbance intensity of the AgNPs/PHMB solution with Mn2+ concentration is shown in Figure 8(d) with the Mn2+ range from 0 mM to 100 mM. The limit of detection (LOD) was calculated at approximately 0.22 mM. These finding results suggest that the AgNPs/PHMB also may be used as a useful probe for the detection of Mn2+ ions.


## 3.1. Structural Analysis

Figure2 shows the XRD spectra of colloidal AgNPs stabilized by PHMB (curve a), Tween 80 (curve b), and NaBH4 (curve c), respectively. It can be seen that four specific diffraction peaks of AgNPs at 2θ = 38.1°, 44.3°, 64.4°, and 77.5° correspond to the crystals (111), (200), (220), and (311) of the silver metal crystal (JC PDS No. 04-0783). These results confirm the formation of the silver metal crystal with a relative single-phase structure in colloidal AgNPs. However, the intensity and sharpness of diffraction peaks in samples using various stabilizers are different. This indicates the stabilizer effect on the particle size of AgNPs as well as the quality of silver metal crystals. Line broadening in the pattern can be quantitatively evaluated using the Debye–Scherrer equation (equation (3)), which gives a relationship between peak broadening in XRD and particle size [18]:(3)D=k⋅λβ⋅cosθ,where D is the thickness of the crystal, k is the Debye–Scherrer constant (0.9), λ is the X-ray wavelength (0.15406 nm), β is the line broadening in radian obtained from the full width at half maximum, and θ is the Bragg angle. According to the Debye–Scherrer equation, average particle sizes of AgNPs were estimated to be 25, 20, and 15 nm when the used stabilizers were PHMB, Tween 80, and NaBH4, respectively.Figure 2
XRD diffraction pattern of the colloidal Ag-NPs stabilized by (a) PHMB, (b) Tween 80, and (c) NaBH4.


## 3.2. Long-Term Stability of the Colloidal AgNPs

UV-Vis can be used to observe the stabilization of AgNP colloids. Stable AgNP colloid in the UV-Vis spectra was stable vs. storing time, suggesting that particle size was stable and without any aggregation. The position of the plasmonic peak in the UV-Vis spectrum depends on the average particle sizes and shapes [19]. Figure 3 shows the optical absorption spectra of the colloidal AgNPs with modified surfaces by different stabilizers as prepared (black solid line) and after 6 months of storage (red dash line). Figure 3 shows that as prepared, all synthesized AgNPs samples illustrated the appearance of the characteristic AgNP peaks at a maximum adsorption of λmax = 400 nm, 440 nm, and 420 nm, corresponding to NaBH4, PHMB, and Tween 80, respectively (black solid lines). However, after 180 days of storage, UV-Vis absorption spectra of these samples were decreased for all tested samples. The strongest decrease can be observed in the case of Tween 80 and NaBH4, respectively, and the peak absorption characteristic of silver nanoparticles was almost absent (red dash line in Figures 3(b) and 3(c)). In contrast, AgNP colloid was stabilized well by PHMB, and it still exists as the specific peak of AgNPs at λmax = 455 nm with a small reduction in absorption intensity. Clearly, this result indicated an excellent role of PHMB as a stabilizer to AgNP colloid than that of NaBH4 or Tween 80. Besides, in Figure 3(a), after 6 months, the specific peak of AgNPs is λmax = 455 nm, and there is a small red shift, compared with λmax = 400 nm as-prepared samples, this can be attributed to a small aggregation that was formed in the AgNPs/PHMB system. The small aggregation in the AgNPs/PHMB system can also be observed by the DLS spectra (Figure 4). Two zones of size distribution as-prepared AgNPs/PHMB and small shoulder can be seen in Figure 4(a) with a mean particles size around 60 nm.Figure 3
UV-Vis absorbance spectrum of the colloidal Ag-NPs stabilized by (a) PHMB, (b) Tween 80, and (c) NaBH4.
(a)
(b)
(c)Figure 4
Size distribution for long term of the colloidal Ag-NPs stabilized by PHMB ((a) 2 hours; (b) 180 days).
(a)
(b)After 6 months of storage, a shoulder was disappeared (Figure4(b)); however, two zones of size distribution were still observed and the mean size was shifted to 105 nm, which is bigger than that as prepared. These analyst results are completely consistent with the above UV-Vis measurements, as well as zeta potential measurements (Table 1). The surface charge of AgNP colloids with various used stabilizers was analysed by zeta potential measurements. The structure is formed by the surface interactions between AgNPs and stabilizer molecules which changes over time. In particular, Table 1 shows that the surface of modified AgNPs by ionic stabilizers (including NaBH4 and PHMB) had less time-varying changes in zeta potential (±% vs. storage time) than that of the nonionic stabilizer (i.e., Tween 80). After 180 days, AgNPs/PHMB showed better stability than the other stabilizers (Table 1). Moreover, the long-term stability of the colloidal AgNPs stabilized by PHMB when compared with other stabilizers or surfactants as shown in Table 2. In this study, the colloidal AgNPs stabilized by PHMB for stability up to 180 days, which promises for many application fields, such as biomedical, agricultural, and environmental control.Table 1
Effect of stabilizers on zeta potential after 180 days.
Stabilizers
Zeta potential (mV)
2 hours
180 days
±(%) zeta potential change after 180 days
PHMB
31.5
26.5
−15.87
NaBH4
−25.5
−6.62
−74.04
Tween 80
−7.9
−0.02
−99.75Table 2
Long-term stability of the colloidal AgNPs.
Methods
Precursors
Reducing agent
Stabilizer or surfactant
Stability time
Ref.
Chemical synthesis
AgNO3
Citrate
Citrate/gelatin mixture
118 days
[3]
Chemical synthesis
AgNO3
NaBH4
Aminosilanes
30 days
[9]
Chemical synthesis
AgNO3
NaBH4
β-Cyclodextrin, adamantine
14 days
[16]
Chemical synthesis
AgNO3
NaBH4
Dodecanethiol
60 days
[7]
Green synthesis
AgNO3
NaBH4
L-Cysteine
60 days
[20]
Biological synthesis
AgNO3
Bacterial biomass
Bacterial biomass
90 days
[21]
Chemical synthesis
AgNO3
NaBH4
PHMB
180 days
This study


## 3.3. Understanding the Mechanism of the Colloidal AgNPs Stabilized by PHMB

A mechanism for long-term stability of AgNPs stabilized by PHMB can be proposed as described in Figure5. Based on the electron configuration of silver (Ag0) is [Kr] 4d105s1, there are many vacant orbitals on the covalent shell of silver atoms including 5p05 d0. Meanwhile, there are many free-electron pairs (unbonded covalence electron pairs) at nitrogen (N) positions on PHMB including -N¨H-7 and/or -N¨ = groups; therefore, coordination interaction of vacant-covalent orbitals of Ag with free-electron pairs of nitrogen in PHMB molecules has been generated, and as a result, the PHMB molecules protect AgNPs as modelled in Figure 5(a). More interestingly, the inside-bonding structure of Ag into AgNPs with PHMB molecules are given in Figure 5(b), which suggested that AgNPs stabilized by PHMB were positively charged; therefore, in the AgNPs/PHMB, the stability of the electrostatic shield around AgNPs was enhanced by the formation of coordinate covalent bonds between the atoms of silver metal and nitrogen in the composition of PHMB (Figure 5(b)). According to this structure (Figure 5(b)), in the colloidal solution, AgNPs were separated from each other by the repulsion layer because of an electrostatic shield that protected the AgNPs surface in the form of positively charged spheres (Figure 5(c)). Thus, AgNPs tend to push each other and survive independently. Electrostatic repulsion of stabilizing agents on the surface of AgNPs is considered an important factor to improve the stability of the colloidal AgNPs [3].Figure 5
Schematic representation of AgNPs/PHMB: (a) NaBH4 reduction Ag+ to AgNPs in the presence of PHMB; (b) the formation of the coordinate covalent bond between silver metal atoms (Ag0) and free-covalence electron pairs of the nitrogen (N) atom in PHMB molecules; and (c) mechanism stabilization of the AgNPs/PHMB via repulsion force AgNPs/PHMB particles.The coordination interaction of vacant-covalent orbitals of Ag with free-electron pairs of nitrogen in PHMB molecules was further confirmed by the FTIR analysis. The FTIR spectra of PHMB and AgNPs/PHMB are shown in Figure6. Compared with PHMB, the FTIR spectrum of AgNPs/PHMB shows one new absorption peak at 1000 cm−1 which corresponds to C-N bond stretching [22] and the disappearance of the absorption peak at 1556 cm−1 [11]. The occurrence of these changes indicates the interaction of the AgNPs with imine groups of PHMB through the formation of a coordination bond of Ag-N. The FTIR results demonstrate that the strong interactions of AgNPs and PHMB may efficiently prevent the aggregation of silver nanoparticles [23].Figure 6
FTIR spectra (a) PHMB and (b) AgNPs stabilized by PHMB (AgNPs/PHMB).For NaBH4-stabilized colloidal AgNPs, the AgNPs were also stabilized by the charging shell covering the AgNPs. However, the electrostatic shield was created by the BH4− anion and was broken as given in the following reaction:(4)BH4−+4H2O⟶BOH4+4H2.Therefore, the degradation ofBH4− to hydrogen gas is the major cause of AgNPs to be aggregated [2,24]. With structure as shown in Figure 3(b) , Tween 80 is a nonionic stabilizer; therefore, the interaction between Tween 80 and the AgNPs is based on the surface adsorption. The AgNPs surface was coated by a layer of Tween 80 to separate the nanoparticles and create great stability based on the steric repulsion mechanism [8,25]. Our finding results reveal that the long-term stability of the colloidal AgNPs was attributed to the formation of Ag-N coordinate covalent bonds and the electrostatic repulsion between PHMB-functionalized AgNPs.


## 3.4. Application of AgNPs/PHMB as a Probe for the Detection of Mn2+ Ions

As described in Section3.3, PHMB coated the AgNPs, therefore, AgNPs/PHMB particles contain free-amino groups, which were from a terminal tail of PHMB (Figure 7). The free -NH2 group can be used to recognize transition metal ions via a colorimetric approach, such as Mn2+ with the detection mechanism as shown in Figure 7. For Mn2+ detection, AgNP play the role to be a signal probe along with the free amino (-NH2) group on PHMB molecules plays the role as a chemical capture probe. The presence of functional groups, such as amine (-NH2), on the surface of AgNPs plays a critical role in the aggregation mechanism through metal-ligand interactions. The amino groups of PHMB have a cooperative effect to form ion-templated chelation with Mn2+, which causes the aggregation of AgNPs [15]. On the contrary, the AgNP aggregation is induced by interparticle bond formation (cross-linking aggregation). The chelation form changes the interparticle distances of AgNPs, leading to the shift of the absorption peak of AgNPs to a longer wavelength. Therefore, cross-linking aggregation has been used for the detection of metal ions [26].Figure 7
Mechanism of Mn2+-induced AgNPs/PHMB aggregation.For that, control testes have been done based on adding 10 mM of various ions including Ni2+, Co2+, and Mn2+ into the AgNPs/PHMB solution. The UV-Vis spectra of the AgNPs/PHMB solution before and after adding a solution containing the above ions are shown in Figure 8(a). It can be seen that the maximal absorption peak of the AgNPs/PHMB solution after adding the Mn2+ ion (curve iv) was strongly diminished than the original AgNPs/PHMB solution (curve i), as well as this decrease was stronger than adding other ions such as Ni2+ (curve ii) or Co2+ (curve iii). These indicated the specific Mn2+ detection of the proposed method. The PHMB polymer can be used as a strong chelating agent to Mn(II) ions due to the amino groups which can form stable complexes with Mn(II) ions. The N atom and amino groups of the PHMB structure can form coordinated bonds with manganese ions causing the aggregation of large particles, which is in good agreement with similar previous reports [15,16,26] in which the sulfonic group, hydroxyl group, and/or carboxyl groups have been considered as an important chelator in specific recognition with Mn2+ ions.Figure 8
Colorimetric detection of Mn2+ ions using the colloidal Ag-NPs: (a) UV-Vis spectra of AgNPs/PHMB without and with adding Co2+, Ni2+, and Mn2+ solution; (b) the UV-Vis spectra of AgNPs/PHMB solutions with different pH ranging from pH 3.5 to pH 9.0 after adding 10 mM Mn2+ solution; (c) UV-Vis spectra of AgNPs/PHMB in the presence of Mn2+ with different concentrations from 0 to 100 mM; and (d) a calibration curve for Mn2+ detection.
(a)
(b)
(c)
(d)To investigate the effect of pH on the sensitivity of this colorimetric method to Mn2+, the AgNPs/PHMB solution was added with 10 mM Mn2+ solution at different pH (from pH 3.5 to pH 9.0) and UV-Vis spectra are shown in Figure 8(b). It can be seen that when the pH value was less than 6.5, the UV-Vis spectra of the AgNPs/PHMB solution were unchanged after adding Mn2+ because the -NH2 group of PHMB is changed to -NH3+, a positively charged group; therefore, Mn2+ cannot interact to these positively charged groups. As the pH value was higher than pH 8, it is noticed that the aggregation of AgNPs/PHMB, as well as Mn2+, would be precipitated as the Mn(OH)2 form. At pH 6.5 to pH 7.5, the intensity and position of the maximum adsorption peaks changed more clearly; therefore, pH in the range 6.5 to 7.5 was selected for further experiments.In the UV-Vis spectra of AgNPs/PHMB added with different Mn2+ concentrations (Figure 8(c)), we notice that the intensity of the maximal absorption peak (at λmax = 403 nm) was decreased with increasing Mn2+ ion concentrations. In addition, there was a red shift of this peak, which could be attributed to the cause of the AgNPs/PHMB aggregation via Mn2+ as linkers. The linear relationship between the absorbance intensity of the AgNPs/PHMB solution with Mn2+ concentration is shown in Figure 8(d) with the Mn2+ range from 0 mM to 100 mM. The limit of detection (LOD) was calculated at approximately 0.22 mM. These finding results suggest that the AgNPs/PHMB also may be used as a useful probe for the detection of Mn2+ ions.


## 4. Conclusions

The long-term stability of colloidal AgNPs functionalized by PHMB, BH4-, and Tween 80 has been studied. The results indicated that the stability of AgNPs/PHMB (up to 180 days) was the best. The long-term stability of colloidal AgNPs is created by the formation of the coordinate covalent bonding as well as the enhancement of electrostatic repulsion between functionalized AgNPs. Moreover, the AgNPs/PHMB has been successfully tested for Mn(II) ion detection using the colorimetric assay. The AgNPs/PHMB aggregate in the presence of Mn2+, resulting in a color change of the solution as well as a red shift of the absorbance peak. The proposed method is capable of determining Mn2+ ions over a range of 0–100 mM. The assay is simple in design, fast in operation, low-cost, and can be observed with the naked eye. With long-term stability, the PHMB-functionalized AgNPs will become a promising material for many fields such as textile industry, agricultural, and environmental control.



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*Source: 9437108-2020-02-07.xml*