# Adsorption of Polyvinylpyrrolidone over the Silica Surface: As Affected by Pretreatment of Adsorbent and Molar Mass of Polymer Adsorbate

Authors: Laila M. Al-Harbi; Samia A. Kosa; Musa K. Baloch; Qaisar A. Bhatti; El-Sayed El-Badawey H. El-Mossalamy
Journal: International Journal of Polymer Science
 (2016)

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## Abstract

The adsorption of polyvinylpyrrolidone over the surface of silica has been investigated. The impact of molar mass of the polymer, pH, and pretreatment temperature of silica particles have been evaluated by means of FTIR spectroscopy and electrophoretic measurements. The silica particles used have narrow particle size distribution. The zeta potential of the aqueous silica suspension was decreased with the increase in pH. The amount of polymer adsorbed was increased with the increase in pretreatment temperature, time, concentration, pH, zeta potential, and molar mass of the polymer. The addition of polymer to the system increased the zeta potential due to adsorption of polymer on the surface of the particles. However, the impact increased with the increase in molecular mass of the polymer. The IR spectra obtained before and after adsorption of polymer concluded that, mostly, hydrogen bonding is responsible for the adsorption phenomena; however, hydrophobic interactions also play a significant role. The mechanism has been investigated and established through FTIR spectroscopy.


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## Body

## 1. Introduction

Dispersion in both aqueous and nonaqueous media is used in numerous products including paints, dyestuffs, pigments, printing inks, papers, adhesives, cosmetics, detergents, ceramics, and pharmaceutical and pesticide formulations. Use of coagulants to clarify drinking water was practiced in ancient time in China and in Egypt. Mineral and environmental engineers have applied the concepts of colloid science to help them utilize and preserve enormous resources which otherwise were waste material [1]. Nowadays, ceramic products ranging from building bricks to expensive china to rocket parts are made from clay-water sols by applying principles of colloid science [2]. The wide use of colloid science in the areas of cosmetics and detergents has added many products to our daily life [3]. Knowledge of human life, either written on paper or stored on film or disk, has depended upon the application of colloidal science in papermaking and development of new magnetic and electronic materials, and so forth [4]. The dispersion activity of such material is mostly controlled through the addition of polymer or a mixture of polymers and surfactants and the interactions of surfactants and/or neutral water polymers in aqueous solutions with solid particles play a vital role in such applications. Therefore, the investigation of these interactions has been an active field of interest [5–9]. On the other hand, the interaction of polymers with solid/liquid interface has not attained so much attention, despite the importance of polymer adsorption over the solid/liquid interface [10–15]. Further, the degree and nature of adsorption of polymer depend on the suspended particles and hence affect the stability of the dispersion [16]. In addition to that, the surface charge-to-mass ratio of the particle plays a very important role in stabilizing the dispersion and this parameter is very much dependent upon the pH of the solution, size of particles, and so forth. Although a number of research papers have been published to understand the mechanism of adsorption of polymers over the solid surfaces, unfortunately, none of the papers deals with the prediction of adsorption behavior of a polymer over the solid surface up to the required level [17, 18].Polyvinylpyrrolidone, also named Povidone or PVP, is a nonionic amphiphilic polymer. Because of its exceptional combination of properties like low toxicity, biocompatibility, film forming and adhesive characteristics, complexing ability to proton donors, and low osmotic pressure, it finds diverse applications in various fields of life like pharmaceutical and cosmetic products, food, adhesives, and textile auxiliaries as compared to other water-soluble polymers like polyethylene oxide and polyvinyl alcohol [19–21]. In spite of these facts, mechanisms involved in such processes are not well understood and hence need detailed and systematic exploration for proper utilization of silica [6, 12–14, 22]. AEROSIL® OX 50 because of its physicochemical properties has a large number of applications. Among fumed silica, AEROSIL OX 50, due to its specific properties, is widely used in biotechnology, agriculture, medicine, and pharmaceutics.Since surface modification of an oxide via polymer adsorption leads to a change in its physicochemical characteristics, therefore, the main objective of this work was to investigate in detail the adsorption behavior of PVP onto silica in its aqueous suspension by using UV, FTIR spectroscopy, electrophoresis, and measurement techniques and to explore the impact of particle size of silica, temperature, pretreatment of adsorbent, molecular mass of polymer, and so forth on the adsorption phenomenon and to make use of that data for the exploration of the mechanism.


## 2. Experimental

### 2.1. Materials

AEROSIL OX 50, fumed silica oxide obtained from Degussa, Evonik Industries, Germany, was used as a model substrate. Some of the characteristics of AEROSIL OX 50 are presented in Table1. These properties were also verified by employing a mercury porosity meter (Autosorb-1 der Firma Quanta chrome, USA), pH and LD measurements, and scanning electron microscopy. The specific surface area reported by the manufacturer was 50
±
15 (m2·g−1) but when measured it was 40.72 (m2·g−1).Table 1
Physicochemical properties of AEROSIL OX 50, as per the manufacturer information.
Source
BET surface area
PZC at pH
S
i
O
2 Contents
pH
Primary particle size
Tapped approximate density
Evonik Industries
50 + 15 (m2 g−1)
3.2
≥99.8
3.8–4.8
0.4 (µm)
.130 (g/L)
“PZC at pH” signifies the PZC (point of zero charge) at pH at which surface charge of the particle is zero.Three different samples of PVP, also known as Luvitec, were obtained from BASF, Germany. PVP had three different molar masses and was used as a stabilizer for the silica dispersion. Some of the basic properties of PVP as provided by the manufacturer are listed in Table2. Water used for the dispersion was obtained from Millipore GmbH, Schwalbach, Germany, having pH around 6.5 and conductance of 2.5 μS.Table 2
Some of the basic properties of PVP as provided by the manufacturer, BASF, Germany.
Sample
PVP K17
PVP K30
PVP K90
Mw/K dalton
7–11
45–55
1200–2000
Degree of dispersity
1.8 ± 0.2
2.3 ± 0.2
3.4 ± 0.3
Rel. viscosity, 1% in water
1.075–1.110
1.201–1.291
3.991–6.197


### 2.2. Methods

#### 2.2.1. Characterization of Silica

The particle size and size distribution of silica were determined using scanning electron microscope (Jowl, Japan) and laser diffraction particle size analyzer Mastersizer 2000, Malvern Co., UK, equipped with impeller mixture. The surface area of the material was estimated using mercury porosity meter (Autosorb-1 der Firma Quanta chrome, USA). Surface charge was measured using Zetasizer 3000 (Malvern Co., Germany). The surface charge densityq in relation to pH was measured by polyelectrolyte titration using Particle Charge Detector (PCD, Mütek GmbH, Germany). FTIR Tensor, Bruker, Germany, was used for IR spectra measurement.


#### 2.2.2. Pretreatment of Silica

For this purpose, the adsorbent (silica) was heated at five different temperatures from 298 K to 523 K for three hours in a vacuum oven (Gallon Kamp, UK) under inert atmosphere and then cooled to room temperature in a desiccant. The sample so obtained was used for adsorption studies [23].


#### 2.2.3. Characterization of Polymer

The polymer was characterized by laser light scattering technique; the instrument used for the purpose was DAWN EOS, supplied by Wyatt, USA, with helium-neon laser of 632.8 nm wavelength as light source.


#### 2.2.4. Adsorption Studies

Polymer solution was prepared in water having concentration 0–80 ppm. The solution was mixed with 0.05 g of preheated adsorbent/20 mL of polymer solution in 100 mL sample bottles for 3 hours at different temperatures. The samples were equilibrated for 16 hours at 298 K at 85 rpm, using orbital shaker (Sanyo Orbit, Japan). Thereafter, the supernatant was removed from samples by centrifuging at 21000 ×g for 15 minutes, using centrifuge model OSK12710 (Gawasieki Co., Japan), and analyzed for polymer concentration.The pH dependent adsorption experiments were performed at pH 2–10 at 298 K. The pH of the solution was maintained using HNO3 and KOH. pH of the solution was measured using pH meter supplied by Denwer, USA.


#### 2.2.5. Analytical Measurements

The amount of unabsorbed PVP in the supernatant was determined using spectroscopic techniques. For this purpose, the UV-visible spectrophotometer employed was Lambda 800 (PerkinElmer) andλ
m
a
x used for measurement was 196 nm.


#### 2.2.6. Zeta Potential Measurement

The zeta potential of particles was measured using Zetasizer 3000, supplied by Malvern, Germany.ζ
0 and ζ of silica were measured before and after the adsorption process. The contents of silica used during the electrophoretic measurements were 0.1 gL−1. KCl was used as an electrolyte of (1 × 10−3 mol/L) known concentration. Electrophoretic mobility of the samples was measured after allowing sufficient conditioning time to attain equilibrium at the required pH [24–26].


#### 2.2.7. FTIR Spectroscopic Studies

FTIR spectra of silica, PVP, and PVP adsorbed over silica were recorded over the range of 4000 cm−1 to 400 cm−1 wavenumber by using KBr pellet (Figure 13). The instrument used for the purpose was FTIR Tensor, Bruker, Germany.


## 2.1. Materials

AEROSIL OX 50, fumed silica oxide obtained from Degussa, Evonik Industries, Germany, was used as a model substrate. Some of the characteristics of AEROSIL OX 50 are presented in Table1. These properties were also verified by employing a mercury porosity meter (Autosorb-1 der Firma Quanta chrome, USA), pH and LD measurements, and scanning electron microscopy. The specific surface area reported by the manufacturer was 50
±
15 (m2·g−1) but when measured it was 40.72 (m2·g−1).Table 1
Physicochemical properties of AEROSIL OX 50, as per the manufacturer information.
Source
BET surface area
PZC at pH
S
i
O
2 Contents
pH
Primary particle size
Tapped approximate density
Evonik Industries
50 + 15 (m2 g−1)
3.2
≥99.8
3.8–4.8
0.4 (µm)
.130 (g/L)
“PZC at pH” signifies the PZC (point of zero charge) at pH at which surface charge of the particle is zero.Three different samples of PVP, also known as Luvitec, were obtained from BASF, Germany. PVP had three different molar masses and was used as a stabilizer for the silica dispersion. Some of the basic properties of PVP as provided by the manufacturer are listed in Table2. Water used for the dispersion was obtained from Millipore GmbH, Schwalbach, Germany, having pH around 6.5 and conductance of 2.5 μS.Table 2
Some of the basic properties of PVP as provided by the manufacturer, BASF, Germany.
Sample
PVP K17
PVP K30
PVP K90
Mw/K dalton
7–11
45–55
1200–2000
Degree of dispersity
1.8 ± 0.2
2.3 ± 0.2
3.4 ± 0.3
Rel. viscosity, 1% in water
1.075–1.110
1.201–1.291
3.991–6.197


## 2.2. Methods

### 2.2.1. Characterization of Silica

The particle size and size distribution of silica were determined using scanning electron microscope (Jowl, Japan) and laser diffraction particle size analyzer Mastersizer 2000, Malvern Co., UK, equipped with impeller mixture. The surface area of the material was estimated using mercury porosity meter (Autosorb-1 der Firma Quanta chrome, USA). Surface charge was measured using Zetasizer 3000 (Malvern Co., Germany). The surface charge densityq in relation to pH was measured by polyelectrolyte titration using Particle Charge Detector (PCD, Mütek GmbH, Germany). FTIR Tensor, Bruker, Germany, was used for IR spectra measurement.


### 2.2.2. Pretreatment of Silica

For this purpose, the adsorbent (silica) was heated at five different temperatures from 298 K to 523 K for three hours in a vacuum oven (Gallon Kamp, UK) under inert atmosphere and then cooled to room temperature in a desiccant. The sample so obtained was used for adsorption studies [23].


### 2.2.3. Characterization of Polymer

The polymer was characterized by laser light scattering technique; the instrument used for the purpose was DAWN EOS, supplied by Wyatt, USA, with helium-neon laser of 632.8 nm wavelength as light source.


### 2.2.4. Adsorption Studies

Polymer solution was prepared in water having concentration 0–80 ppm. The solution was mixed with 0.05 g of preheated adsorbent/20 mL of polymer solution in 100 mL sample bottles for 3 hours at different temperatures. The samples were equilibrated for 16 hours at 298 K at 85 rpm, using orbital shaker (Sanyo Orbit, Japan). Thereafter, the supernatant was removed from samples by centrifuging at 21000 ×g for 15 minutes, using centrifuge model OSK12710 (Gawasieki Co., Japan), and analyzed for polymer concentration.The pH dependent adsorption experiments were performed at pH 2–10 at 298 K. The pH of the solution was maintained using HNO3 and KOH. pH of the solution was measured using pH meter supplied by Denwer, USA.


### 2.2.5. Analytical Measurements

The amount of unabsorbed PVP in the supernatant was determined using spectroscopic techniques. For this purpose, the UV-visible spectrophotometer employed was Lambda 800 (PerkinElmer) andλ
m
a
x used for measurement was 196 nm.


### 2.2.6. Zeta Potential Measurement

The zeta potential of particles was measured using Zetasizer 3000, supplied by Malvern, Germany.ζ
0 and ζ of silica were measured before and after the adsorption process. The contents of silica used during the electrophoretic measurements were 0.1 gL−1. KCl was used as an electrolyte of (1 × 10−3 mol/L) known concentration. Electrophoretic mobility of the samples was measured after allowing sufficient conditioning time to attain equilibrium at the required pH [24–26].


### 2.2.7. FTIR Spectroscopic Studies

FTIR spectra of silica, PVP, and PVP adsorbed over silica were recorded over the range of 4000 cm−1 to 400 cm−1 wavenumber by using KBr pellet (Figure 13). The instrument used for the purpose was FTIR Tensor, Bruker, Germany.


## 2.2.1. Characterization of Silica

The particle size and size distribution of silica were determined using scanning electron microscope (Jowl, Japan) and laser diffraction particle size analyzer Mastersizer 2000, Malvern Co., UK, equipped with impeller mixture. The surface area of the material was estimated using mercury porosity meter (Autosorb-1 der Firma Quanta chrome, USA). Surface charge was measured using Zetasizer 3000 (Malvern Co., Germany). The surface charge densityq in relation to pH was measured by polyelectrolyte titration using Particle Charge Detector (PCD, Mütek GmbH, Germany). FTIR Tensor, Bruker, Germany, was used for IR spectra measurement.


## 2.2.2. Pretreatment of Silica

For this purpose, the adsorbent (silica) was heated at five different temperatures from 298 K to 523 K for three hours in a vacuum oven (Gallon Kamp, UK) under inert atmosphere and then cooled to room temperature in a desiccant. The sample so obtained was used for adsorption studies [23].


## 2.2.3. Characterization of Polymer

The polymer was characterized by laser light scattering technique; the instrument used for the purpose was DAWN EOS, supplied by Wyatt, USA, with helium-neon laser of 632.8 nm wavelength as light source.


## 2.2.4. Adsorption Studies

Polymer solution was prepared in water having concentration 0–80 ppm. The solution was mixed with 0.05 g of preheated adsorbent/20 mL of polymer solution in 100 mL sample bottles for 3 hours at different temperatures. The samples were equilibrated for 16 hours at 298 K at 85 rpm, using orbital shaker (Sanyo Orbit, Japan). Thereafter, the supernatant was removed from samples by centrifuging at 21000 ×g for 15 minutes, using centrifuge model OSK12710 (Gawasieki Co., Japan), and analyzed for polymer concentration.The pH dependent adsorption experiments were performed at pH 2–10 at 298 K. The pH of the solution was maintained using HNO3 and KOH. pH of the solution was measured using pH meter supplied by Denwer, USA.


## 2.2.5. Analytical Measurements

The amount of unabsorbed PVP in the supernatant was determined using spectroscopic techniques. For this purpose, the UV-visible spectrophotometer employed was Lambda 800 (PerkinElmer) andλ
m
a
x used for measurement was 196 nm.


## 2.2.6. Zeta Potential Measurement

The zeta potential of particles was measured using Zetasizer 3000, supplied by Malvern, Germany.ζ
0 and ζ of silica were measured before and after the adsorption process. The contents of silica used during the electrophoretic measurements were 0.1 gL−1. KCl was used as an electrolyte of (1 × 10−3 mol/L) known concentration. Electrophoretic mobility of the samples was measured after allowing sufficient conditioning time to attain equilibrium at the required pH [24–26].


## 2.2.7. FTIR Spectroscopic Studies

FTIR spectra of silica, PVP, and PVP adsorbed over silica were recorded over the range of 4000 cm−1 to 400 cm−1 wavenumber by using KBr pellet (Figure 13). The instrument used for the purpose was FTIR Tensor, Bruker, Germany.


## 3. Results and Discussion

Fumed silica (AEROSIL OX 50) obtained from the supplier was characterized with respect to its purity, surface charge, size, and surface area. FTIR spectra of the samples are displayed in Figure1.Figure 1
FTIR spectra of silica.The literature reveals that FTIR spectra of pure silica typically display peaks in two discrete regions, with wavenumbers greater than 2500 cm−1 and less than 1300 cm−1 [7, 8]. The former region corresponds to hydroxyl (−OH) stretching due to absorbed or molecular water. However, in our case, we did not observe any peak in this region. It was attributed to heat treatment of the silica before adsorption. The latter region is observed due to different modes of silica [8] and three prominent peaks were observed. The peak at 460 cm−1 was assigned to rocking motion of oxygen atoms bridging silicon atoms in siloxane bonds (Si–O–Si). A broader peak at 810 cm−1 was assigned to O–Si–O vibration mode of SiO2 which was due to symmetric vibrations of silicon atoms in a siloxane bond [27]. A peak at 1105 cm−1 along with weak absorption at 960 cm−1 was the largest peak observed in a silica spectrum and was assigned to Si–O–Si and Si–O stretching vibration modes of isolated Si–OH groups. Similar bands were observed by Guzenko et al. [9]. The values were in good agreement with those reported in the literature [7–9, 28, 29] indicating that the material was pure and heating was performed properly.As the stability of dispersion also depends upon the charge of the particle, the surface potential of the particles was determined as a function of pH, which was adjusted using 1 × 10−3 M KOH and 1 × 10−3 M HNO3. The measurement was made in 1 × 10−3 M KCl solution at 25°C, using Malvern Zeta Master. The results obtained are displayed as a function of pH in Figure 2 which shows a negative zeta potential in the pH range from 3.2 to 10. The isoelectric point was about 3.2. It indicated that the dispersion with pH near the isoelectric point (3.2) was unstable. If the charge is high, the particles will remain separated and dispersed and the suspension will be stable and vice versa. According to the results, the charge and hence the stability should be the highest in basic pH range because the zeta potential in this range is high.Figure 2
Zeta potential of 1% aqueous dispersion AEROSIL OX 50, measured in 1 × 10−3 M KCl. The error percentage was about 5.0.In aqueous suspensions of silica particles, the surface silicon and oxygen bonds are unsatisfied and are neutralized by OH− and H+ species. As a result, partial or total particle surface hydroxylation can result in the formation of silanol groups [Si(OH)n] which dissociate in pure water through the following reactions:(1)
S
i
O
H
+
O
H
-
⟶
S
i
–
O
-
+
H
2
O
(2)
S
i
O
H
+
H
+
⟶
S
i
–
O
H
+
+
H
2
OThat is why silica particles may end negatively charged in water suspension for basic pH and positively charged under acidic pH [30, 31]. These phenomena impact directly the zeta potential behavior of silica suspensions and cause a slight change in zeta potential with a change in pH.The rest of the measurements were, therefore, performed at pH 6 at room temperature with a negative zeta potential of about −47 mV.The electron micrographs of AEROSIL OX 50 are displayed in Figure3. The micrographs showed that although the particles are monodispersed, they are aggregated which may affect their adsorption and dispersion and stabilization properties. Although ultrasonication was performed for 30 min, it was impossible to break the aggregates completely as concluded by the manufacturer.Figure 3
SEM picture of AEROSIL OX 50.The results obtained from Mastersizer after homogenizing the system with magnetic stirrer for one hour and ultrasonication for various time periods are shown in Figure4.Figure 4
Particle size distribution of AEROSIL OX 50 (1% aqueous dispersion) measured after sonification for various duration using Mastersizer. The error percentage was about 3.5%.The figure indicates monodispersity in the size of the particles; however, some aggregates are visible in the images. The particle sizes obtained in the aqueous dispersed phase for the samples sonicated for different times ranged from 220 to 900 nm with an average of 400 nm, as is displayed in Figure4. These plots also show monodispersity to some extent while the polydispersity is attributed to aggregates that are present in the system. Furthermore, these observations are in accord with information provided by the manufacturer.The figure also indicated that the sonication time has an almost negligible impact on the size and size distribution. However, the degree of dispersity was first decreased and then was increased if the sonication time was longer than 20 min. This trend was attributed to the balance between shear and colloidal forces. This phenomenon is further supported by(3)
γ
c
=
f
s
σ
η
A
a
.Here, γ
c is the critical shear rate, s is the ratio of particle to medium viscosity, σ is interfacial tension, η
A is droplet viscosity, and a is the size of the particle.Equation (3) states that aggregate formation or disintegration depends upon the critical shear rate. It is important to note that the critical shear rate is inversely proportional to the size of the particles [32]. This means that if the size of the particles is small, then the high shear rate is needed to further decrease the size.The FTIR spectra of the polymer (PVP) used showed a good agreement with the literature indicating that the polymer was pure (Figure5) [10, 29].Figure 5
FTIR spectra of polyvinylpyrrolidone.The results obtained for molecular weight and degree of dispersity of polymer were 9.18 (1.8), 49.96 (2.3), and 1.43 × 103 (3.4) Kg/mol. It was noted that with the increase in molecular mass of the polymer the degree of dispersity was increased and the results were the same (within experimental error) as supplied by the manufacturer shown in Table 2.Time dependent adsorption curves are frequently observed in polymer adsorption [29]. It is sometimes assumed that reconfirmation processes play an important role in determining the rate of adsorption. However, for polydisperse polymers, this is not the only possibility since small chains on the surface may be replaced by the bigger ones, leading to a slow increase in adsorbed amount. Although the time scale of such processes in not known, it is expected that they contribute significantly to the overall time dependent adsorption. Therefore, the amount of K90 adsorbed was measured after 24 hours of mixing. The silica concentration was 0.5 g/dm−3 and the starting concentration of the PVP was 80 ppm. It can be seen that the adsorbed amount was increased sharply during the first 10 hours and then leveled off (Figure 6). On the bases of these observations and for practical reasons, we chose 16 hours as adsorption time in all adsorption experiments.Figure 6
Adsorbed amount of PVP as a function of time. The error percentage was about 2.5.Adsorption isotherms for the polymer of different molecular masses are shown in Figure7. It was noted that the isotherms were of Langmuir type and of high affinity and that the amount adsorbed was increased from 0.4 to 0.8 mg m−2 with the increase in molecular mass of the polymer [33, 34]. It was noted from the isotherms that initially the adsorption was increased very rapidly with the increase in concentration of polymer and ultimately it leveled off. This was accredited to the fact that initially the availability of the surface free sites was high and hence adsorption took place faster. However, as the time passed, the equilibrium was established and availability of free sites was reduced to almost zero and hence the adsorption became difficult and rate of adsorption became almost zero. The maximum amount of polymer adsorbed onto the surface of silica was increased with the concentration of polymer. These findings were in line with the expectations [35, 36].Figure 7
Adsorption isotherms of PVP having different molecular mass on AEROSIL OX 50, measured at 298 K. The error percentage was about 2.5.The amount of polymer (PVP) adsorbed per unit surface area was calculated using Langmuir adsorption. The data gave exactly straight lines and the average value obtained in this way was 0.6 mg·m−2 (Figure 7). However, this value was slightly less than (1.0 mg·m−2) the adsorbed concentration for a calculated condensed monolayer of monomer units.Although the adsorbed amount was increased much with increasing the molar mass of the polymer, for higher molecular mass, leveling off of adsorption took place. The maximum amount adsorbed at plateau region was consistent with the data published in the literature [37, 38]. The adsorption capacity was found to be a function of molecular mass, showing similar dependency to that reported by Cohen Stuart et al. [39]. Polymer-solvent interaction and segmental adsorption energy parameter are the two main factors which may work behind this phenomenon. Low polymer-solvent interaction is a poor solvent and high segmental adsorption energy parameter. That is, strong attachment of the segments may lead to a high adsorbed amount of polymer [39].The amount adsorbed at plateau coverage was plotted as a function oflog
⁡
M
w in Figure 8. It was observed that the increase in adsorption was very sharp for low molecular mass and ultimately leveled off for high molecular mass. Since we have used polymer with only three molecular masses and worked with lower concentrations, therefore, for a better understanding of this trend, data reported by Cohen Stuart et al. and Robinson and Williams [34, 38, 40] were also plotted in Figure 8 for comparison purpose and the results showed an excellent agreement. It is interesting to note that although the amount adsorbed was increased with the molecular weight and then leveled off, the values in mM/m2 were decreased and followed a single exponential relationship irrespective of data source (Figure 8). This type of behavior could be explained in terms of variation in conformation of polymer chains with the molecular mass.Figure 8
The amount of polymer adsorbed as a function of molecular mass of polymer.In order to find out the effect of pH over the adsorption of polymer, we measured the adsorbed amount at various pH. The results obtained are plotted in Figure9. The results concluded that the adsorbed amount is the highest at low pH and was decreased with the increase in pH and ultimately levels off. The same trend was observed for all the polymer samples indicating that the pH had the same impact irrespective of molecular mass. To explore the cause of such trend, the zeta potential and amount adsorbed have been plotted against pH in the same figure. The figure concludes that the adsorption is very much related to surface charge of the solid material used. Further to it, the solvent quality will deteriorate for polymer with the increase in pH and hence conformation of polymer will change which may result in a decrease in adsorption of polymer.Figure 9
Amount of polymer adsorbed over silica as a function of pH. The error percentage was about 2.5 in adsorption and in case of zeta potential it was 5%.Since it is observed that heating causes a reduction in the silanol-group density on the surface of silica particles [41, 42], it is important to have some knowledge about the importance of these groups in the phenomenon of polymer adsorption. Therefore, a study of the impact of preheating silica on the adsorption of PVP has been conducted. The adsorbent was heated for three hours from 298 K to 523 K at five different temperatures and used for adsorption purpose. The results obtained are plotted in Figure 10. The figure shows that preheating does not have a very pronounced impact on the adsorption for a specific temperature range. By increasing the pretreatment temperature, the amount of polymer adsorbed was increased sharply. Since we have worked over a range of 298 K to 523 K, to get detailed information in this regard, we interpolated our data with that of Alagha et al. and Behrens et al. [43, 44]. It is observed that a very little impact is seen up to 523 K, and at higher temperature of about 1273 K a sharp increase in amount adsorbed was observed (Figure 11).Figure 10
Effect of pretreatment of AEROSIL OX 50 on the adsorption of PVP. The error percentage was about 2.5.Figure 11
Effect of pretreatment of AEROSIL OX 50 on adsorption of PVP. The reported data are our own and the one reported by Cohen Stuart et al. [39].The initial smaller increase in amount adsorbed is attributed to the fact that desorption of gases and/or water during heating of silica resulted in an increase in availability of free surface site for the adsorption and at the same time the decrease in surface area limits the amount adsorbed [43–45]. Therefore, no significant amount adsorbed was observed. However, at higher temperature, a sharp increase revealed the fact that at higher temperature a significant reduction of surface area takes place along with the removal of surface silanol groups, which made the silica more hydrophobic, and an increase in the amount adsorbed is due to this hydrophobic interaction between polymer and the silica surface. Our findings are in very good agreement with those reported in the literature [44, 45].The impact of preheating of silica on the adsorption of PVP was investigated by heating the samples at five different temperatures from 298 K to 523 K and the results obtained are plotted in Figure11. The figure showed that by increasing the pretreatment temperature the amount of polymer adsorbed was increased significantly. An increase in the amount adsorbed for low temperature was attributed to desorption of gases and/or water during heating of silica, which resulted in an increase in availability of free surface site for the adsorption, and at the same time the decrease in surface area limited the amount adsorbed [41, 42]. Therefore, no significant amount was adsorbed. However, at high temperature, a significant increase in adsorption revealed that at higher temperature the removal of surface silanol groups took place [42, 43] which made the silica more hydrophobic and an increase in the amount adsorbed took place. However, a significant reduction of surface area also took place and that reduced the adsorption up to a considerable amount. Our findings are in very good agreement with those reported in the literature [44, 45].Zeta potential of AEROSIL OX 50 after adsorption of PVP was obtained at pH 5.7 and 25°C. The results are displayed in Figure11 as a function of PVP adsorbed amount. It was observed that the zeta potential of AEROSIL OX 50 was initially −42.5 mV and was significantly increased with the increase in concentration of PVP due to adsorption of polymer over AEROSIL OX 50. As N–C=O group is present in PVP and is electron donor in nature, it causes an increase in the surface charge on silica or enhances the shielding effect of the oxide surfaces [46] and hence was dependent upon concentration and molecular mass of PVP. This is the reason why the pH of the media was increased by the addition of the polymer. The figure also displayed that the charge over AEROSIL OX 50 was increased with the increase in molecular mass of PVP adsorbed. It was attributed to the shift of the share plan in case of adsorption of nonionic polymers [47] and the increase in number of monomers (active groups) in a chain of polymers.To establish the mechanism of PVP adsorption onto AEROSIL OX 50, FTIR spectroscopic measurements of the samples were carried out before and after the adsorption of PVP. The spectra so recorded for AEROSIL OX 50, PVP, and PVP adsorbed over AEROSIL OX 50 are displayed in Figure12 for comparison purpose. CH2– band deformation near 1460 cm−1 in hydrocarbons and the splitting of the band into 1422, 1460, and 1493 cm−1 indicated the interchain forces in PVP and strain in the five-membered rings. Stretching of CH2 (CH) NCO in PVP was indicated by pronounced absorbance at 1287–1373 cm−1. The absorbance shown by carbonyl group in PVP at 1661 cm−1 was in the range reported earlier [47, 48]. The presence of C=O at 1661 cm−1 was significant, whereas the appearance of C–O was very weak and may be due to the canonical forms of PVP as represented by the structure (Scheme 1).Scheme 1
Schematic presentation of resonating structure of polyvinylpyrrolidone.Figure 12
Effect of PVP concentration and molecular mass over the zeta potential of silica. The error percentage was about 5.0.Figure 13
FTIR spectra of silica, PVP, and silica after adsorption of PVP.Strong evidence which supported the presence of hydrogen bonding in adsorption of PVP on silica was that, before adsorption of PVP, the presence of C=O at 1661 cm−1 was significant, whereas the appearance of C–O was very weak; however, after the adsorption process, the C=O group almost disappeared. Therefore, it was suggested that partial negative charged oxygen of the C=O group caused the hydrogen bonding with the hydrogen of silanol. This was further supported by the fact that PVP has N–C=O groups which are electron donor in nature [49]; therefore, hydrogen bonding between oxygen of C=O and hydrogen of silanols may have possibly taken place. Furthermore, there is no evidence for the conversion of C–N into C=N as shown by the shifting of peaks from 1661 cm−1 to 1078 cm−1 [50]. Schematic presentation of the mechanism of PVP adsorption on silica is given by Scheme 2.Scheme 2
Schematic presentation of the adsorption of PVP on silica.



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*Source: 2417292-2016-05-24.xml*