# Effect of Soil Solution pH during the Tetracycline Intercalation on the Structural Properties of a Dioctahedral Smectite: Microstructural Analysis

Authors: Walid Oueslati
Journal: Journal of Nanomaterials
 (2019)

---

## Abstract

The aim of this work is to quantitatively characterize the structural response to a chemical disruption of saturated montmorillonite crystallites by organic molecules (tetracycline (TC)), derived from pharmaceutical waste. The chemical disturbance is performed by varying the surrounding soil solution pH. To show the effect of this chemical perturbation on the interlamellar space (IS) configuration and the hydration properties, an “in situ” XRD analysis, based on the modeling of the 00l reflections, is carried out. The “in situ” XRD analysis is performed by varying the relative humidity conditions (%RH). FTIR SEM and BET- (Brunauer-Emmett-Teller-) BJH (Barrett-Joyner-Halenda) analyses are used as complementary techniques to confirm the structural changes accompanying the intercalation process. Results showed a dependence between solution acid character and the TC adsorption mechanism. From pH values close to 7, the deprotonation of the TC molecule within IS is accelerated by an increasing %RH rate. IR spectroscopy shows that the structure is preserved versus pH value and only a shift of the water deformation bands ascribed to interlamellar water molecule abundance and TC conformation is observed. The surface morphology studied by SEM shows the increase in the surface porosity by increasing the pH value. BET-specific surface area and BJH pore size distribution (PSD) analyses confirm the SEM observations.


---

## Body

## 1. Introduction

The risks associated with the presence of industrial and household waste in the soil and the environment are multiplied with the great demand for everyday consumer products. Essentially, pharmaceutical industry waste releases which include organic molecules (antibiotics and others), heavy metals, and even radioactive substances represent a serious environmental problem.To date, various conventional and modern technologies are used for reducing the organic pollutant effect on the human health (fauna and flora). Among these technologies, we can mention the ion exchange process which is in relation to the main properties of clay mineral and chemical precipitation and adsorption [1–4]. All these methods have been developed to separate, to confine, to trap, to isolate, to eliminate, and to protect human life from contaminated effluents.Recent studies investigated the adsorption/desorption of various organic matters on/from soil particles. These include, for example, the adsorption of antibodies, surfactants, fire-retarding organics, and herbicides [5–8]. The use of these techniques is thwarted by the high cost of materials used for these purposes.Clay, which is a material that is abundant in nature, can play an important role in the future as a geological barrier for the confinement and removal of organic pollutants in surface, ground, and wastewaters [9, 10]. Forming part of dioctahedral phyllosilicates 2 : 1, smectites can be considered a solution for this environmental problem. Montmorillonite is a natural nanomineral (layer thickness ~1.0 nm) belonging to the smectite group. The intrinsic montmorillonite properties such as low permeability, high surface area, and cation exchange capacity (CEC) [11] promote its application in such context.The main montmorillonite structure is characterized by the isomorphic substitution presence which generates a permanent negative layer’s charge. To compensate this charge deficit, exchangeable cation or organic molecules can be intercalated in the IS [12]. The montmorillonite layer structure can expand and contract its structures without crystallographic change. These expansions depend on the IS content (water/polar molecule) and the surrounding environment (relative humidity rate) [13–17].Several studies, in relation to the use of montmorillonite in the pharmaceutical-sediment interaction context, have been, recently, realized [18–27].Among the basic substances of antibiotics is the TC molecule. Recently, the interaction of TC, as an organic molecule, with montmorillonite has been studied, from the point of view of adsorption and intercalation, by several authors [28–34]. TCs comprise a group of natural and semisynthetic products that inhibit the synthesis of bacterial proteins. The TC chemical properties have been widely studied [35]. The protonation properties of the amine group on TC allow its cation exchange with exchanged cations of montmorillonite.The presence of a TC molecule in IS generates (after the intercalation process) several structural ambiguities. Indeed, during the intercalation and/or adsorption process, several parameters such as chemical composition, solid/liquid ratio, pH dependence, soil solution composition, and environmental and atmospheric conditions come into play [36–38]. In addition, once the molecule (in our case TC) is interposed, the configuration and distribution of chemical species in IS will be disturbed and a new equilibrium (electrical, chemical, ionic, etc.) will be established. For that, a structural investigation must be directed to understanding the link between, respectively, environmental conditions, intercalation process, and structural changes.In this regard, [37] used XRD analysis and spectroscopic methods to demonstrate that the adsorption decreases as the pH is increased and eventually becomes negligible at pH=11. In addition, [38] investigated TC intercalation onto a rectorite sample and highlighted the rectorite d-spacing increase during the intercalation process. Also, [38] demonstrate that the maximum interlayer expansion, obtained at a high pH value, is accompanied by an extended TC molecule conformation. Alternatively, [29] employed both simulated and experimental XRD to characterize structures, following the interlayer adsorption of OTC within Na-montmorillonite as a function of pH. They demonstrate that the intercalation of the antibiotic species within the smectite layers at low acidic pH induces a random layer stacking mode. This structural behavior turns into segregation trends by increasing the pH value.This work focuses on the effect of soil pH variation, during the TC intercalation process, on the structural properties of Na-montmorillonite. At a fixed pH value, “in situ” XRD analysis is performed by varying %RH conditions. The contents of the interlamellar space along thec∗ axis are fully identified through an XRD modeling approach. The correlation of the results obtained by XRD, IR, SEM, and BET allows a quantitative description of the montmorillonite structural changes within the intercalation process.


## 2. Materials and Methods

### 2.1. Baseline Sample

A reference montmorillonite sample (Swy-2) (from the Source Clays Repository of the Clay Minerals Society) is used in this work [39, 40]. The half-cell structural formula is given by [41]
(1)Si3,923Al0,077Al1,459Ti0,0184+Fe0,0393+Fe0,0452+Mg0,3822+O10OH2Ca0,1772+Na0,027+Before application, a pretreatment of the natural specimen is required to guarantee a maximum dispersion. The Na-rich montmorillonite suspension is prepared according to a classical protocol detailed by [42, 43].


### 2.2. Tetracycline (TC)

Tetracycline hydrochloride was delivered by PARAFARM. Depending on the solution pH, a TC molecule undergoes protonation-deprotonation reactions which engender (03) groups and generate the formation of (04) species. The TC stock solutions are prepared just before use to avoid degradation instigated by oxygen and light. NaOH and HCl are used for pH adjustment. The molecular conformation change is attributed to the protonation equilibrium of the TC molecule. Indeed, forpH<8 (from acidic to neutral solution), a twisted conformation is adopted. This situation, usually referred to as folded conformation, is explained by the release of the steric crowding between the protonated nitrogen on the dimethylamino group, NH4, and OH12. The extended conformation is displayed for pH values>8 (Figure 1) [44–46].Figure 1
Scheme of the fully protonated tetracycline: folded conformation forpH<8 and extended conformation for pH>8.


### 2.3. Experimental Intercalation Process

The intercalation process is performed at constant TC concentration under a variable solution pH value. Six different pH values varying from acidic to neutral solution are fixed (i.e., 3, 4, 5, 6, 7, and 8). The experimental protocol is summarized in Figure2.Figure 2
Experimental TC intercalation process under variable solution pH.


### 2.4. In Situ X-Ray Diffraction Measurements

All experimental XRD patterns were recorded from the oriented preparations of the air-dried sample (SWy-2-TC) using a Brucker D8 Advance X-ray diffractometer at 40 kV and 20 mA (CuKαmonochromaticradiation=0.15406nm) equipped with an Ansyco_rh-plus 2250 humidity control device coupled to an Anton Paar TTK450 chamber. For each pH value, an in situ variation of the environmental RH, which extends from 20% to 80% (i.e., the almost saturated conditions), is carried out. The usual scanning parameters were 0.04°2θ as step size and 6 s as counting time per step over the angular range 2–40°2θ. Samples were kept at 23°C in the CHC+ chamber during the whole data collection. To maintain the desired RH rates, samples were equilibrated with their environment by a constant flow of mixed dry/saturated air.


### 2.5. Modeling (00l) Reflection Profiles

The XRD modeling method is used to quantify smectite hydration and ionic exchange properties as a function of a surrounding RH% rate [47–50]. Theoretical XRD models are based on the algorithm developed initially by Drits and Tchoubar [51]. The Z atomic coordinates within the 2 : 1 layer framework (tetrahedral and octahedral sheet) in the case of this study are reported in Table 1. The Z coordinates of the IS content (exchangeable cation, molecules, etc.) are optimized, during the modeling process, to improve the agreement quality. This later is controlled using the unweighted Rp parameter [52].Table 1
TheZ atomic coordinates within the 2 : 1 layer framework along the c∗ axis [43].
Atom type
O1
O2
O3
O4
O5
O6
OH1
OH2
Si
Si
Al
Number
2
1
2
2
1
2
1
1
2
2
2
Zn (Å)
0
0.20
2.25
4.31
6.26
6.59
1.98
4.28
0.59
6.04
3.43The diffracted intensity along the 00l rod belonging to the reciprocal space is given by [51]
(2)I002θ=LpSpurReϕWI+2∑nM−1M−nMQn.The matrix formalism behind the diffracted theoretical intensity and the fitting strategy are detailed by [47, 52]. The average position of the TC molecule within the IS is fixed at 15.40 Å. Regardless of the hydration state type, the Na exchangeable cations (per half unit cell) are positioned at the center of the IS along the c∗ axis. This configuration respects the provided literature data [53].


### 2.6. FTIR Spectroscopy

The understanding of the proposed structural models from quantitative XRD analysis requires confirmation by a complementary analysis technique. FTIR spectroscopy is used to detect the presence of groups of characteristic units in the IS [54, 55]. These units include hydroxyl groups, dimethylamino group, silicate and aluminate anions, octahedral metal cations, and interlayer cations. FTIR spectra are recorded with 400–4000 cm-1 spectra based on a PerkinElmer Paragon 1000 PC spectrometer. The experiments are implemented by dispersing the material in KBr discs.


### 2.7. Scanning Electron Microscopy (SEM)

All scanning electron micrographs are obtained from a JEOL model JSM-5400 (ETAP, Tunisia) scanning electron microscope using a beam with an acceleration of 20 keV. All samples are conducted under vacuum by the FINE COATmodel JFC_1100E installation. The studied samples are, respectively, the starting SWy-2 and the intercalated TC samples with a variable solution pH value.


### 2.8. BET and BJH Pore Size Distribution Analysis

Nitrogen sorption (both adsorption and desorption) at the clean surface of dry solid powders is used to determine the surface area (SA) and the pore size distribution (PSD) of porous materials such as montmorillonite. In this case, powders are obtained after drying each sample. Physical gas adsorption is often the technique of choice for examining the pore characteristics of materials [56]. The technique determines the amount of gas adsorbed; this is a direct indication of the porous properties and, therefore, the overall structure of the material [57, 58]. A BET-specific surface area and PSD of the studied sample, under each pH value, were determined using a Quantachrome NOVA 2000e series volumetric gas adsorption instrument, which is a USA automated gas adsorption system using nitrogen as the adsorptive. Adsorption isotherms were performed at 77 K and at the relative pressure up to P/P0 ~0.95. Adsorbed nitrogen and oxygen were removed under reduced (vacuum) pressure at 100°C for 8 h before measuring SA and PSD.The PSD was determined by the BJH method [59] to the desorption section of the isotherms of nitrogen at 77 K, assuming the pores to be cylindrical in shape [60, 61].


## 2.1. Baseline Sample

A reference montmorillonite sample (Swy-2) (from the Source Clays Repository of the Clay Minerals Society) is used in this work [39, 40]. The half-cell structural formula is given by [41]
(1)Si3,923Al0,077Al1,459Ti0,0184+Fe0,0393+Fe0,0452+Mg0,3822+O10OH2Ca0,1772+Na0,027+Before application, a pretreatment of the natural specimen is required to guarantee a maximum dispersion. The Na-rich montmorillonite suspension is prepared according to a classical protocol detailed by [42, 43].


## 2.2. Tetracycline (TC)

Tetracycline hydrochloride was delivered by PARAFARM. Depending on the solution pH, a TC molecule undergoes protonation-deprotonation reactions which engender (03) groups and generate the formation of (04) species. The TC stock solutions are prepared just before use to avoid degradation instigated by oxygen and light. NaOH and HCl are used for pH adjustment. The molecular conformation change is attributed to the protonation equilibrium of the TC molecule. Indeed, forpH<8 (from acidic to neutral solution), a twisted conformation is adopted. This situation, usually referred to as folded conformation, is explained by the release of the steric crowding between the protonated nitrogen on the dimethylamino group, NH4, and OH12. The extended conformation is displayed for pH values>8 (Figure 1) [44–46].Figure 1
Scheme of the fully protonated tetracycline: folded conformation forpH<8 and extended conformation for pH>8.


## 2.3. Experimental Intercalation Process

The intercalation process is performed at constant TC concentration under a variable solution pH value. Six different pH values varying from acidic to neutral solution are fixed (i.e., 3, 4, 5, 6, 7, and 8). The experimental protocol is summarized in Figure2.Figure 2
Experimental TC intercalation process under variable solution pH.


## 2.4. In Situ X-Ray Diffraction Measurements

All experimental XRD patterns were recorded from the oriented preparations of the air-dried sample (SWy-2-TC) using a Brucker D8 Advance X-ray diffractometer at 40 kV and 20 mA (CuKαmonochromaticradiation=0.15406nm) equipped with an Ansyco_rh-plus 2250 humidity control device coupled to an Anton Paar TTK450 chamber. For each pH value, an in situ variation of the environmental RH, which extends from 20% to 80% (i.e., the almost saturated conditions), is carried out. The usual scanning parameters were 0.04°2θ as step size and 6 s as counting time per step over the angular range 2–40°2θ. Samples were kept at 23°C in the CHC+ chamber during the whole data collection. To maintain the desired RH rates, samples were equilibrated with their environment by a constant flow of mixed dry/saturated air.


## 2.5. Modeling (00l) Reflection Profiles

The XRD modeling method is used to quantify smectite hydration and ionic exchange properties as a function of a surrounding RH% rate [47–50]. Theoretical XRD models are based on the algorithm developed initially by Drits and Tchoubar [51]. The Z atomic coordinates within the 2 : 1 layer framework (tetrahedral and octahedral sheet) in the case of this study are reported in Table 1. The Z coordinates of the IS content (exchangeable cation, molecules, etc.) are optimized, during the modeling process, to improve the agreement quality. This later is controlled using the unweighted Rp parameter [52].Table 1
TheZ atomic coordinates within the 2 : 1 layer framework along the c∗ axis [43].
Atom type
O1
O2
O3
O4
O5
O6
OH1
OH2
Si
Si
Al
Number
2
1
2
2
1
2
1
1
2
2
2
Zn (Å)
0
0.20
2.25
4.31
6.26
6.59
1.98
4.28
0.59
6.04
3.43The diffracted intensity along the 00l rod belonging to the reciprocal space is given by [51]
(2)I002θ=LpSpurReϕWI+2∑nM−1M−nMQn.The matrix formalism behind the diffracted theoretical intensity and the fitting strategy are detailed by [47, 52]. The average position of the TC molecule within the IS is fixed at 15.40 Å. Regardless of the hydration state type, the Na exchangeable cations (per half unit cell) are positioned at the center of the IS along the c∗ axis. This configuration respects the provided literature data [53].


## 2.6. FTIR Spectroscopy

The understanding of the proposed structural models from quantitative XRD analysis requires confirmation by a complementary analysis technique. FTIR spectroscopy is used to detect the presence of groups of characteristic units in the IS [54, 55]. These units include hydroxyl groups, dimethylamino group, silicate and aluminate anions, octahedral metal cations, and interlayer cations. FTIR spectra are recorded with 400–4000 cm-1 spectra based on a PerkinElmer Paragon 1000 PC spectrometer. The experiments are implemented by dispersing the material in KBr discs.


## 2.7. Scanning Electron Microscopy (SEM)

All scanning electron micrographs are obtained from a JEOL model JSM-5400 (ETAP, Tunisia) scanning electron microscope using a beam with an acceleration of 20 keV. All samples are conducted under vacuum by the FINE COATmodel JFC_1100E installation. The studied samples are, respectively, the starting SWy-2 and the intercalated TC samples with a variable solution pH value.


## 2.8. BET and BJH Pore Size Distribution Analysis

Nitrogen sorption (both adsorption and desorption) at the clean surface of dry solid powders is used to determine the surface area (SA) and the pore size distribution (PSD) of porous materials such as montmorillonite. In this case, powders are obtained after drying each sample. Physical gas adsorption is often the technique of choice for examining the pore characteristics of materials [56]. The technique determines the amount of gas adsorbed; this is a direct indication of the porous properties and, therefore, the overall structure of the material [57, 58]. A BET-specific surface area and PSD of the studied sample, under each pH value, were determined using a Quantachrome NOVA 2000e series volumetric gas adsorption instrument, which is a USA automated gas adsorption system using nitrogen as the adsorptive. Adsorption isotherms were performed at 77 K and at the relative pressure up to P/P0 ~0.95. Adsorbed nitrogen and oxygen were removed under reduced (vacuum) pressure at 100°C for 8 h before measuring SA and PSD.The PSD was determined by the BJH method [59] to the desorption section of the isotherms of nitrogen at 77 K, assuming the pores to be cylindrical in shape [60, 61].


## 3. Results

### 3.1. Qualitative XRD Analysis

The experimental XRD patterns showing the correlation between the %RH and the pH of the surrounding soil solution are reported in Figure3. The d001 basal spacing value shifts from 18.25 Å to 19.85 Å, by increasing pH from 3 to 6, which indicates probably a complete TC adsorption process. For the high pH value, the obtained d001 value indicates two-water layer (2W) hydration states which is attributed probably to a partial adsorption process of TC. The semiquantitative analysis is based on the reflection peak geometry interpretation and the investigation of the evolution of the FWHM parameter (Table 2). Indeed, the high FWHM value is obtained at 80%RH for pH=5 and at 60%RH for pH=6. This value indicates an interstratified character confirmed by the asymmetric 00l geometry peaks. All studied samples are characterized by an interstratified character due to the interlayer configuration and the external constraint imposed along the adsorption and analysis process (pH and %RH).Figure 3
(a–f) The best agreement between theoretical (red line) and experimental (black line) XRD patterns obtained by varying %RH rates under different pH values (3-8).
(a)
(b)
(c)
(d)
(e)
(f)Table 2
Qualitative XRD investigations for different studied samples versus pH and %RH variation.
pH
%RH
d001 (Å)
FWHM (°2θ)
Character
3
20
18.25
2.813
I
40
18.87
1.412
I
60
18.71
1.231
QH
80
17.66
1.761
I
4
20
19.70
1.403
QH
40
19.02
2.123
I
60
19.53
2.910
I
80
20.06
3.501
I
5
20
20.82
1.651
I
40
20.25
1.767
QH
60
20.06
2.624
I
80
19.36
3.810
I
6
20
19.85
1.903
I
40
20.06
1.400
QH
60
18.25
3.810
I
80
20.43
3.010
I
7
20
18.54
2.120
I
40
15.65
1.560
QH
60
16.47
1.684
QH
80
16.49
1.708
I
8
20
15.12
2.189
I
40
14.15
2.204
I
60
17.51
1.904
I
80
17.38
2.706
I
I: interstratified character; QH: quasihomogeneous character.Away high acidity degrees (pH=7) and at 60%RH, the XRD patterns are characterized by d001 indicating a 2W hydration state (Table 2) and the sample seems to be unaffected by the TC adsorption process. Also, this value can be interpreted by a monocationic exchange process (Na+) [40]. But, by exploiting the effect of the %RH variation, a partial TC adsorption is confirmed for the 20%RH, where d001=18.54Å characteristic of high interlayer swelling which accompanied the TC adsorption.AtpH=8 and for low 2θ angles, a minor reflection which can be attributed to the 4W (four-water) hydration state with d001=22.07Å (Figure 3) appears. This value can be interpreted by the effect of the protonation-deprotonation reactions on the TC molecules which depends essentially on the pH value.


### 3.2. Quantitative XRD Analysis

Qualitative XRD analysis remains insufficient for a more precise description of the interlayer configuration. For that, a quantitative XRD analysis is performed to determine the structural parameter involved on the TC adsorption process. The best agreements between theoretical and experimental patterns are reported in Figure3. The main structural parameters used to obtain a good fit are summarized in Table 3. For each model, several layer types with variable stacking mode are used in order to improve the obtained agreement between calculated and experimental patterns. This mixed-layer structure (MLS) is composed of a four-layer thickness type depending on the hydration state (i.e., 1W (12.40 Å), 2W (15.40 Å), 3W (18.20 Å), and 4W (21.40 Å)). The proposed MLS are obtained by weighted layer type populations which are supposed to have, respectively, identical chemical composition, identical layer thickness, and identical Z coordinates of the atoms. The cation exchange capacity (CEC) of the starting materials is saturated by Na+ and TC molecules. The XRD pattern modeling is based on the fitting strategy described by [47].Table 3
Structural parameters used to reproduce experimental XRD patterns as a function of soil solution pH and %RH.
pH
%RH
%MLS
1W/2W/3W/4W†
Pii//Wi
Physical mixture
ZNa1W/2W/3W/4W
M
3
20
13
00/00/89/11
0.30//0.30
R0
09.70/11.10/12.60/14.10
4
38
60/35/05/00
0.28//0.28
R0
49
18/00/82/00
0.50//0.50
R0
40
15
70/00/30/00
0.31//0.31
R0
09.70/11.10/12.60/14.10
4
25
14/06/80/00
0.41//0.41
R0
60
20/00/75/05
0.37//0.37
R0
60
45
00/16/84/00
0.87//0.87
R0
09.70/11.10/12.60/14.10
5
55
11/00/85/04
0.54//0.54
R0
80
41
00/09/91/00
0.38//0.38
R0
09.70/11.10/12.60/–
4
59
04/06/90/00
0.27//0.27
R0
4
20
17
00/00/88/12
0.50//0.30
R1
09.70/11.10/12.60/14.10
5
33
00/04/79/17
0.55//0.29
R1
50
10/15/75/00
0.64//0.34
R1
40
13
00/00/90/10
0.47//0.21
R1
09.70/11.10/12.60/14.10
6
22
00/00/100/00
—
—
65
18/04/78/00
0.81//0.34
R1
60
16
40/12/48/00
0.64//0.29
R1
09.70/11.10/12.60/–
5
42
33/16/51/00
0.67//0.35
R1
42
40/00/60/00
0.52//0.31
R1
80
26
00/00/77/23
0.81//0.20
R1
09.70/11.10/12.60/14.10
4
29
40/35/15/10
0.80//0.30
R1
45
38/12/42/08
0.72//0.38
R1
5
20
35
00/33/55/12
0.55//0.35
R1
–/11.10/12.60/14.10
4
28
00/45/50/05
0.81//0.54
R1
37
00/32/39/29
0.64//0.35
R1
40
26
00/05/60/35
0.78//0.27
R1
–/11.10/12.60/14.10
5
14
00/00/38/62
0.78//0.34
R1
60
00/09/50/41
0.56//0.24
R1
60
12
00/19/72/09
0.49//0.18
R1
–/11.10/12.60/14.10
4
27
00/50/25/25
0.35//0.12
R1
40
00/24/38/38
0.48//0.28
R1
21
00/00/50/50
0.51//0.37
R1
80
30
00/20/80/00
0.71//0.54
R1
–/11.10/12.60/14.10
4
19
00/10/60/30
0.77//0.48
R1
51
00/10/55/35
0.64//0.23
R1
6
20
22
00/17/83/00
0.81//0.35
R1
–/11.10/12.60/14.10
4
78
00/05/85/10
0.79//0.25
R1
40
27
00/00/80/20
0.55//0.30
R1
–/11.10/12.60/14.10
4
73
00/09/60/31
0.74//0.35
R1
60
15
00/15/45/40
0.78//0.23
R1
–/11.10/12.60/14.10
5
25
00/10/90/00
0.65//0.38
R1
60
00/08/87/05
0.84//0.40
R1
80
45
00/00/35/65
0.72//0.30
R1
–/11.10/12.60/14.10
4
55
00/20/50/30
0.60//0.30
R1
7
20
20
00/44/52/04
0.55//0.30
R1
–/11.10/12.60/14.10
4
70
00/45/55/00
0.50//0.34
R1
10
00/45/45/10
0.77//0.41
R1
40
28
00/55/45/00
0.80//0.20
R1
–/11.10/12.60/14.10
3
72
00/35/57/08
0.76//0.25
R1
60
35
00/48/48/04
0.55//0.22
R1
–/11.10/12.60/14.10
5
65
00/68/32/00
0.50//0.38
R1
80
38
00/50/50/00
0.55//0.18
R1
–/11.10/12.60/14.10
4
62
00/65/30/05
0.80//0.26
R1
8
20
25
00/55/45/00
0.71//0.21
R1
–/11.10/12.60/14.10
6
35
00/40/10/50
0.64//0.28
R1
40
00/48/12/40
0.55//0.24
R1
40
35
00/42/18/40
0.49//0.30
R1
–/11.10/12.60/14.10
5
35
00/50/00/50
0.62//0.15
R1
30
00/55/00/45
0.81//0.30
R1
60
25
00/49/40/11
0.50//0.30
R1
–/11.10/12.60/14.10
4
28
00/55/45/00
0.54//0.33
R1
47
00/45/43/12
0.64//0.18
R1
80
42
00/40/60/00
0.66//0.30
R1
–/11.10/12.60/14.10
4
20
00/46/50/04
0.50//0.27
R1
38
00/55/45/00
0.55//0.16
R1
Note: 4W, 3W, 2W, and 1W are attributed to the layer hydration state. R0 and R1 describe mixed-layer structures with random interstratifications or with partial segregation, respectively.∗ indicates homogenous structure. Pij is the junction probability of layer type j to follow layer type i, and Wi abundances of layer type i. In this case, i is Na and j is TC, wherein four equations are used: WNa+WTC=1 (1), PNa‐Na+PNa‐TC=1 (2), PTC‐TC+PTC‐Na=1 (3), and WNaPNa‐TC=WTCPTC‐Na (4). ZNa: position of exchangeable cations per half unit cell calculated along the c∗ axis. ZTC: average position of the adsorbed TC molecule is fixed at 15.40 Å. M: average layer number per stacking.The XRD patterns obtained atpH=3 reflect a random layer type stacking mode (R0), whereas a partial segregation (R1) is obtained for pH varying from 4 to 8. Accordingly, for pH 3 and pH 4, a major presence of a 1W layer hydration state is noted (Table 3). The 4W hydration state is omnipresent along all the pH ranges. The clear contribution of this highly hydrated state is illustrated, respectively, at pH 5, 6, 7, and 8. The presence of the TC molecule on the interlayer space affects the 001 reflection geometry, and the appearance of broadening peaks at a low angle confirms this result. The 001 reflection is very sensitive to the content of the interlamellar space and the surrounding humidity as was observed at a high %RH value. By increasing pH from 3 to 7, there is a doublet at ∼12 Å and ∼18 Å, which is characteristic of crystals or domains containing essentially either a Na or TC interlayer, respectively, both types of interlayers being mutually exclusive. By increasing %RH, a modification of the relative intensities of the two peaks occurs, as indicated by a steady increase in the ∼18 Å peak at the expense of that at ∼12 Å.At pH 8, this “law” is not respected since the 18-22 Å phase (characteristic of the TC adsorption process) is reduced in favor of the 12-15 Å phase (characteristic of Na-exchanged montmorillonite), which can be interpreted by the deprotonation of the TC molecule. This result is confirmed by the decrease in the 4W layer type abundance from 60%RH.


### 3.3. FTIR Analysis

The FTIR spectra corresponding, respectively, to TC, SWy-2-Na, and adsorbed TC under variable solution pH are shown in Figure4. By comparing the characteristic vibration bands of the starting sample with those obtained after the TC adsorption process, no apparent change is observed which indicates that the adsorbed specimen does not alter the structure of the host material. This result is in concordance with XRD analysis which demonstrates that the structure is preserved and only a layer thickness variation is observed and ascribed to interlamellar water molecule abundance. All FTIR band positions (cm-1) for SWy-2-Na without and with TC sorption are reported in Table 4.Figure 4
Transmittance IR spectra obtained, respectively, for TC, SWy-2-Na, and TC intercalated sample under a variable solution pH value.Table 4
FTIR band position (cm-1), respectively, for TC, Na-montmorillonite (SWy-2-Na), and TC sorption versus pH.
Sample
FTIR band position
Possible band assignment [38]
TC
1627
ν(CO1), ν(amid-NH), ν(CO3), ν(C2C3), δ(OH10,12)
1572
δ(amid-NH), δ(amine-NH), ν(amid-CO), ν(C2C3), ν(CO3)
1446
δ(OH10,12), δ(CH7,8,9), ν(D), ν(CO10,CO11), ν(C11C11a, C11aC12), δ(OH12a), δ(CH36)
1350
ν(amid-C,C2), ν(C3,C4), δ(CH4a,5), δ(CH36), δ(OH12a), δ(amid-NH), ν(amid-CN), δ(OH10), ν(C6aC10a, C6aC7)
1310
δ(OH10,12), δ(CH4,4a,5,5a), ν(C5aC11a), ν(C1C2), ν(C9C10, C10C10a, C10aC11), ν(CO11,12), ν(CO3), δ(CH7,8,9)
Na-montmorillonite (SWy-2-Na)
3620
OH stretching of structural hydroxyl groups
3542
OH stretching of water coordinated to Al and Mg
3415
OH stretching of adsorbed water
1656
OH deformation of water
1035
Si-O stretching
980
Si-O stretching
MMT+TCFor pH: 3 ➔ 8
3621
OH stretching of structural hydroxyl groups
3542
OH stretching of water coordinated to Al and Mg
3417
OH stretching of adsorbed water
1638
OH deformation of water
1048
Si-O stretching
980
Si-O stretchingA small difference which lies in the effect of evolution as a function of the solution pH is observed. Indeed, the characteristic bands attributed to the OH stretching and located between 3400 and 3600 cm-1 are conserved for all the studied pH values with a small decrease in the peak intensity probably due to the effect of the surrounding environment acidity. The Si-O stretching vibration bands located between 950 and 1100 cm-1, characteristic of the lattice vibration of the starting sample, remain present for intercalated TC samples with enlargement and decrease in the peak intensity. A small characteristic bands around 685 cm-1 are assigned to the symmetric stretching vibration T-O-T (i.e., where T = Si, Al) which confirms the preserved structure despite the chemical perturbation [54, 55]. A characteristic band around 1600 cm-1, attributed to the vibrations of the functional groups of the OH- type related to the deformation of water, is observed regardless of the pH value. The width and intensity of this characteristic band decrease for pH values close to 7. This is consistent with the results of XRD which show a transition from 3W to 2W hydration states. The most characteristic vibration band of TC compounds is located between 1150 and 1650 cm−1 (Table 4) and characterized by a weak intensity and width.


### 3.4. Scanning Electron Microscopy

The scanning electron microscope images of the natural sample (SWy-2-Na) and the intercalated TC samples as a function of the solution pH value are shown in Figure5. The presence of TC molecules affects the structural morphology of the starting sample. In fact, the particle aggregation of the starting sample changes in the presence of the intercalated molecules, which induces a variable porosity as a function of the fixed solution pH. Maximum surface porosity is observed for pH values close to 7.Figure 5
SEM analysis in the case of the starting sample and the intercalated sample under variable solution pH.
(a)
Starting Na-montmorillonite (MMT)
(b)
MMT+TCpH=3
(c)
MMT+TCpH=4
(d)
MMT+TCpH=5
(e)
MMT+TCpH=6
(f)
MMT+TCpH=7
(g)
MMT+TCpH=8For pH values ranging from 3 to 5, the presence of TC strengthens the morphological tissue of the sample which probably indicates in terms of abundance a high intercalation level. From pH 6, the sample has a less collapsed structure with an increase in the pore volume. This result may be related to the effect of the low acidity of the surrounding solution or to a conformational change of the TC molecule.


### 3.5. BET-Specific Surface Area and PSD Analyses

The impenetrability of the nitrogen to the IS makes the BET an appropriate method to show the chemical transformation occurring on the external surface of the clay layer [62]. The structure of pores and the developed external surface area are measured using the BET method. The BET equation (both single-point and multipoint BET methods were considered) is used to calculate the surface area from nitrogen isotherms. The BJH method is used to determine the mean pore diameter. Table 5 shows the BET surface area and the average nanopore diameter for all the studied samples. The calculated external surface area increases by increasing the pH value from 13.8124 m2/g to 18.9829 m2/g (multipoint BET).Table 5
SABET (single-point and multipoint BET) and BJH method average pore diameter.
Sample
SABET (m2/g)Single-point BET
SABET (m2/g)Multi-point BET
Average nanopore diameter (nm)BJH method
MMT+TC_pH3
13.7856
13.8124
3.7102
MMT+TC_pH4
13.9145
13.9735
3.6905
MMT+TC_pH5
14.0864
14.3147
3.7289
MMT+TC_pH6
15.8261
15.9432
3.7305
MMT+TC_pH7
17.9425
18.1287
3.7646
MMT+TC_pH8
18.9461
18.9829
3.7724The SA measurement by the BET method (Figure6) showed that all the studied samples had a pore distribution categorized under type II adsorption isotherm in the classification of Brunauer, Deming, Deming, and Teller (BDDT) [63] which is due probably to the mesoporous texture with large pores (in addition to the nanopores). This result is due to the TC intercalation/adsorption process. Also, because of the ability of nitrogen to cover only the outer primary surface area but not the IS, an asymptotic approach to limiting quantity is observed in nitrogen isotherms. Indeed, it is necessary to differentiate between external, internal, and interlamellar surface areas for clays.Figure 6
Nitrogen adsorption-desorption isotherms of montmorillonite-exchanged TC under varying soil solution pH. MMT: montmorillonite; TC: tetracycline; ADS: adsorption; DES: desorption.The surface area concept does not give a complete textural description in the case of clay specimen; for that, a pore size (PS) and a pore size distribution (PSD) are necessary. The PSD in the mesopore region was determined by the BJH method assuming(i)
the shape of the pores with radius (r) approximatively half of its width is cylindrical [61]
(ii)
the radii (r) of mesopores assumed to be cylindrical corresponding to V values were calculated from the corrected Kelvin equation by the use of P/P0 values [64]
(iii)
the specific micropore, mesopore, and macropore volumes (namely,VMi, VMe, and VMa all in mL/g, respectively) are defined as the volumes of micropores, mesopores, and macropores including nanopores in one gram solid
(iv)
the presence of macropores has a low effect on the adsorptive properties of a solid [65]
(v)
the adsorption capacity as liquid nitrogen volumes which were estimated from desorption data at the relative equilibrium pressure (P/P0) less than 0.96 is taken as the specific micro-mesopore volumes (V=VMi+VMe)
(vi)
P0 and P are the vapor pressure of the bulk liquid nitrogen and equilibrium pressure of desorption at the liquid nitrogen temperature (∼77 K)TheV-r (cumulative pore volume vs. pore radius) plots are called mesopore PSD and given in Figure 7.Figure 7
The pore size distribution curve in the case of montmorillonite-exchanged TC under varying soil solution pH.The estimatedVMi and VMe can be obtained by the intercepts of the extrapolations of each PSD curve related to each sample [66]. The VMe increase from 0.027 to 0.036 mL/g by increasing soil solution pH during the intercalation/adsorption process.The radius derivative of theV-r curve for all samples is given in Figure 8 where the maximum mesopore volume (0.000948 mL/g) is obtained from pH 7 and the mesopore radii varied between 1.5 and 16 nm. The increase in the average pore diameter from a micropore with a width smaller than 2 nm is attributed to the reduction of microporous distribution in favor of mesoporous distribution. The porosity investigation using the BET-BJH method confirms observations obtained by SEM indicating changes on the morphological properties versus increasing pH rate. This transformation can be interpreted by a possible TC molecule conformation change.Figure 8
The derivative pore size distribution curve in the case of montmorillonite-exchanged TC under varying soil solution pH.


## 3.1. Qualitative XRD Analysis

The experimental XRD patterns showing the correlation between the %RH and the pH of the surrounding soil solution are reported in Figure3. The d001 basal spacing value shifts from 18.25 Å to 19.85 Å, by increasing pH from 3 to 6, which indicates probably a complete TC adsorption process. For the high pH value, the obtained d001 value indicates two-water layer (2W) hydration states which is attributed probably to a partial adsorption process of TC. The semiquantitative analysis is based on the reflection peak geometry interpretation and the investigation of the evolution of the FWHM parameter (Table 2). Indeed, the high FWHM value is obtained at 80%RH for pH=5 and at 60%RH for pH=6. This value indicates an interstratified character confirmed by the asymmetric 00l geometry peaks. All studied samples are characterized by an interstratified character due to the interlayer configuration and the external constraint imposed along the adsorption and analysis process (pH and %RH).Figure 3
(a–f) The best agreement between theoretical (red line) and experimental (black line) XRD patterns obtained by varying %RH rates under different pH values (3-8).
(a)
(b)
(c)
(d)
(e)
(f)Table 2
Qualitative XRD investigations for different studied samples versus pH and %RH variation.
pH
%RH
d001 (Å)
FWHM (°2θ)
Character
3
20
18.25
2.813
I
40
18.87
1.412
I
60
18.71
1.231
QH
80
17.66
1.761
I
4
20
19.70
1.403
QH
40
19.02
2.123
I
60
19.53
2.910
I
80
20.06
3.501
I
5
20
20.82
1.651
I
40
20.25
1.767
QH
60
20.06
2.624
I
80
19.36
3.810
I
6
20
19.85
1.903
I
40
20.06
1.400
QH
60
18.25
3.810
I
80
20.43
3.010
I
7
20
18.54
2.120
I
40
15.65
1.560
QH
60
16.47
1.684
QH
80
16.49
1.708
I
8
20
15.12
2.189
I
40
14.15
2.204
I
60
17.51
1.904
I
80
17.38
2.706
I
I: interstratified character; QH: quasihomogeneous character.Away high acidity degrees (pH=7) and at 60%RH, the XRD patterns are characterized by d001 indicating a 2W hydration state (Table 2) and the sample seems to be unaffected by the TC adsorption process. Also, this value can be interpreted by a monocationic exchange process (Na+) [40]. But, by exploiting the effect of the %RH variation, a partial TC adsorption is confirmed for the 20%RH, where d001=18.54Å characteristic of high interlayer swelling which accompanied the TC adsorption.AtpH=8 and for low 2θ angles, a minor reflection which can be attributed to the 4W (four-water) hydration state with d001=22.07Å (Figure 3) appears. This value can be interpreted by the effect of the protonation-deprotonation reactions on the TC molecules which depends essentially on the pH value.


## 3.2. Quantitative XRD Analysis

Qualitative XRD analysis remains insufficient for a more precise description of the interlayer configuration. For that, a quantitative XRD analysis is performed to determine the structural parameter involved on the TC adsorption process. The best agreements between theoretical and experimental patterns are reported in Figure3. The main structural parameters used to obtain a good fit are summarized in Table 3. For each model, several layer types with variable stacking mode are used in order to improve the obtained agreement between calculated and experimental patterns. This mixed-layer structure (MLS) is composed of a four-layer thickness type depending on the hydration state (i.e., 1W (12.40 Å), 2W (15.40 Å), 3W (18.20 Å), and 4W (21.40 Å)). The proposed MLS are obtained by weighted layer type populations which are supposed to have, respectively, identical chemical composition, identical layer thickness, and identical Z coordinates of the atoms. The cation exchange capacity (CEC) of the starting materials is saturated by Na+ and TC molecules. The XRD pattern modeling is based on the fitting strategy described by [47].Table 3
Structural parameters used to reproduce experimental XRD patterns as a function of soil solution pH and %RH.
pH
%RH
%MLS
1W/2W/3W/4W†
Pii//Wi
Physical mixture
ZNa1W/2W/3W/4W
M
3
20
13
00/00/89/11
0.30//0.30
R0
09.70/11.10/12.60/14.10
4
38
60/35/05/00
0.28//0.28
R0
49
18/00/82/00
0.50//0.50
R0
40
15
70/00/30/00
0.31//0.31
R0
09.70/11.10/12.60/14.10
4
25
14/06/80/00
0.41//0.41
R0
60
20/00/75/05
0.37//0.37
R0
60
45
00/16/84/00
0.87//0.87
R0
09.70/11.10/12.60/14.10
5
55
11/00/85/04
0.54//0.54
R0
80
41
00/09/91/00
0.38//0.38
R0
09.70/11.10/12.60/–
4
59
04/06/90/00
0.27//0.27
R0
4
20
17
00/00/88/12
0.50//0.30
R1
09.70/11.10/12.60/14.10
5
33
00/04/79/17
0.55//0.29
R1
50
10/15/75/00
0.64//0.34
R1
40
13
00/00/90/10
0.47//0.21
R1
09.70/11.10/12.60/14.10
6
22
00/00/100/00
—
—
65
18/04/78/00
0.81//0.34
R1
60
16
40/12/48/00
0.64//0.29
R1
09.70/11.10/12.60/–
5
42
33/16/51/00
0.67//0.35
R1
42
40/00/60/00
0.52//0.31
R1
80
26
00/00/77/23
0.81//0.20
R1
09.70/11.10/12.60/14.10
4
29
40/35/15/10
0.80//0.30
R1
45
38/12/42/08
0.72//0.38
R1
5
20
35
00/33/55/12
0.55//0.35
R1
–/11.10/12.60/14.10
4
28
00/45/50/05
0.81//0.54
R1
37
00/32/39/29
0.64//0.35
R1
40
26
00/05/60/35
0.78//0.27
R1
–/11.10/12.60/14.10
5
14
00/00/38/62
0.78//0.34
R1
60
00/09/50/41
0.56//0.24
R1
60
12
00/19/72/09
0.49//0.18
R1
–/11.10/12.60/14.10
4
27
00/50/25/25
0.35//0.12
R1
40
00/24/38/38
0.48//0.28
R1
21
00/00/50/50
0.51//0.37
R1
80
30
00/20/80/00
0.71//0.54
R1
–/11.10/12.60/14.10
4
19
00/10/60/30
0.77//0.48
R1
51
00/10/55/35
0.64//0.23
R1
6
20
22
00/17/83/00
0.81//0.35
R1
–/11.10/12.60/14.10
4
78
00/05/85/10
0.79//0.25
R1
40
27
00/00/80/20
0.55//0.30
R1
–/11.10/12.60/14.10
4
73
00/09/60/31
0.74//0.35
R1
60
15
00/15/45/40
0.78//0.23
R1
–/11.10/12.60/14.10
5
25
00/10/90/00
0.65//0.38
R1
60
00/08/87/05
0.84//0.40
R1
80
45
00/00/35/65
0.72//0.30
R1
–/11.10/12.60/14.10
4
55
00/20/50/30
0.60//0.30
R1
7
20
20
00/44/52/04
0.55//0.30
R1
–/11.10/12.60/14.10
4
70
00/45/55/00
0.50//0.34
R1
10
00/45/45/10
0.77//0.41
R1
40
28
00/55/45/00
0.80//0.20
R1
–/11.10/12.60/14.10
3
72
00/35/57/08
0.76//0.25
R1
60
35
00/48/48/04
0.55//0.22
R1
–/11.10/12.60/14.10
5
65
00/68/32/00
0.50//0.38
R1
80
38
00/50/50/00
0.55//0.18
R1
–/11.10/12.60/14.10
4
62
00/65/30/05
0.80//0.26
R1
8
20
25
00/55/45/00
0.71//0.21
R1
–/11.10/12.60/14.10
6
35
00/40/10/50
0.64//0.28
R1
40
00/48/12/40
0.55//0.24
R1
40
35
00/42/18/40
0.49//0.30
R1
–/11.10/12.60/14.10
5
35
00/50/00/50
0.62//0.15
R1
30
00/55/00/45
0.81//0.30
R1
60
25
00/49/40/11
0.50//0.30
R1
–/11.10/12.60/14.10
4
28
00/55/45/00
0.54//0.33
R1
47
00/45/43/12
0.64//0.18
R1
80
42
00/40/60/00
0.66//0.30
R1
–/11.10/12.60/14.10
4
20
00/46/50/04
0.50//0.27
R1
38
00/55/45/00
0.55//0.16
R1
Note: 4W, 3W, 2W, and 1W are attributed to the layer hydration state. R0 and R1 describe mixed-layer structures with random interstratifications or with partial segregation, respectively.∗ indicates homogenous structure. Pij is the junction probability of layer type j to follow layer type i, and Wi abundances of layer type i. In this case, i is Na and j is TC, wherein four equations are used: WNa+WTC=1 (1), PNa‐Na+PNa‐TC=1 (2), PTC‐TC+PTC‐Na=1 (3), and WNaPNa‐TC=WTCPTC‐Na (4). ZNa: position of exchangeable cations per half unit cell calculated along the c∗ axis. ZTC: average position of the adsorbed TC molecule is fixed at 15.40 Å. M: average layer number per stacking.The XRD patterns obtained atpH=3 reflect a random layer type stacking mode (R0), whereas a partial segregation (R1) is obtained for pH varying from 4 to 8. Accordingly, for pH 3 and pH 4, a major presence of a 1W layer hydration state is noted (Table 3). The 4W hydration state is omnipresent along all the pH ranges. The clear contribution of this highly hydrated state is illustrated, respectively, at pH 5, 6, 7, and 8. The presence of the TC molecule on the interlayer space affects the 001 reflection geometry, and the appearance of broadening peaks at a low angle confirms this result. The 001 reflection is very sensitive to the content of the interlamellar space and the surrounding humidity as was observed at a high %RH value. By increasing pH from 3 to 7, there is a doublet at ∼12 Å and ∼18 Å, which is characteristic of crystals or domains containing essentially either a Na or TC interlayer, respectively, both types of interlayers being mutually exclusive. By increasing %RH, a modification of the relative intensities of the two peaks occurs, as indicated by a steady increase in the ∼18 Å peak at the expense of that at ∼12 Å.At pH 8, this “law” is not respected since the 18-22 Å phase (characteristic of the TC adsorption process) is reduced in favor of the 12-15 Å phase (characteristic of Na-exchanged montmorillonite), which can be interpreted by the deprotonation of the TC molecule. This result is confirmed by the decrease in the 4W layer type abundance from 60%RH.


## 3.3. FTIR Analysis

The FTIR spectra corresponding, respectively, to TC, SWy-2-Na, and adsorbed TC under variable solution pH are shown in Figure4. By comparing the characteristic vibration bands of the starting sample with those obtained after the TC adsorption process, no apparent change is observed which indicates that the adsorbed specimen does not alter the structure of the host material. This result is in concordance with XRD analysis which demonstrates that the structure is preserved and only a layer thickness variation is observed and ascribed to interlamellar water molecule abundance. All FTIR band positions (cm-1) for SWy-2-Na without and with TC sorption are reported in Table 4.Figure 4
Transmittance IR spectra obtained, respectively, for TC, SWy-2-Na, and TC intercalated sample under a variable solution pH value.Table 4
FTIR band position (cm-1), respectively, for TC, Na-montmorillonite (SWy-2-Na), and TC sorption versus pH.
Sample
FTIR band position
Possible band assignment [38]
TC
1627
ν(CO1), ν(amid-NH), ν(CO3), ν(C2C3), δ(OH10,12)
1572
δ(amid-NH), δ(amine-NH), ν(amid-CO), ν(C2C3), ν(CO3)
1446
δ(OH10,12), δ(CH7,8,9), ν(D), ν(CO10,CO11), ν(C11C11a, C11aC12), δ(OH12a), δ(CH36)
1350
ν(amid-C,C2), ν(C3,C4), δ(CH4a,5), δ(CH36), δ(OH12a), δ(amid-NH), ν(amid-CN), δ(OH10), ν(C6aC10a, C6aC7)
1310
δ(OH10,12), δ(CH4,4a,5,5a), ν(C5aC11a), ν(C1C2), ν(C9C10, C10C10a, C10aC11), ν(CO11,12), ν(CO3), δ(CH7,8,9)
Na-montmorillonite (SWy-2-Na)
3620
OH stretching of structural hydroxyl groups
3542
OH stretching of water coordinated to Al and Mg
3415
OH stretching of adsorbed water
1656
OH deformation of water
1035
Si-O stretching
980
Si-O stretching
MMT+TCFor pH: 3 ➔ 8
3621
OH stretching of structural hydroxyl groups
3542
OH stretching of water coordinated to Al and Mg
3417
OH stretching of adsorbed water
1638
OH deformation of water
1048
Si-O stretching
980
Si-O stretchingA small difference which lies in the effect of evolution as a function of the solution pH is observed. Indeed, the characteristic bands attributed to the OH stretching and located between 3400 and 3600 cm-1 are conserved for all the studied pH values with a small decrease in the peak intensity probably due to the effect of the surrounding environment acidity. The Si-O stretching vibration bands located between 950 and 1100 cm-1, characteristic of the lattice vibration of the starting sample, remain present for intercalated TC samples with enlargement and decrease in the peak intensity. A small characteristic bands around 685 cm-1 are assigned to the symmetric stretching vibration T-O-T (i.e., where T = Si, Al) which confirms the preserved structure despite the chemical perturbation [54, 55]. A characteristic band around 1600 cm-1, attributed to the vibrations of the functional groups of the OH- type related to the deformation of water, is observed regardless of the pH value. The width and intensity of this characteristic band decrease for pH values close to 7. This is consistent with the results of XRD which show a transition from 3W to 2W hydration states. The most characteristic vibration band of TC compounds is located between 1150 and 1650 cm−1 (Table 4) and characterized by a weak intensity and width.


## 3.4. Scanning Electron Microscopy

The scanning electron microscope images of the natural sample (SWy-2-Na) and the intercalated TC samples as a function of the solution pH value are shown in Figure5. The presence of TC molecules affects the structural morphology of the starting sample. In fact, the particle aggregation of the starting sample changes in the presence of the intercalated molecules, which induces a variable porosity as a function of the fixed solution pH. Maximum surface porosity is observed for pH values close to 7.Figure 5
SEM analysis in the case of the starting sample and the intercalated sample under variable solution pH.
(a)
Starting Na-montmorillonite (MMT)
(b)
MMT+TCpH=3
(c)
MMT+TCpH=4
(d)
MMT+TCpH=5
(e)
MMT+TCpH=6
(f)
MMT+TCpH=7
(g)
MMT+TCpH=8For pH values ranging from 3 to 5, the presence of TC strengthens the morphological tissue of the sample which probably indicates in terms of abundance a high intercalation level. From pH 6, the sample has a less collapsed structure with an increase in the pore volume. This result may be related to the effect of the low acidity of the surrounding solution or to a conformational change of the TC molecule.


## 3.5. BET-Specific Surface Area and PSD Analyses

The impenetrability of the nitrogen to the IS makes the BET an appropriate method to show the chemical transformation occurring on the external surface of the clay layer [62]. The structure of pores and the developed external surface area are measured using the BET method. The BET equation (both single-point and multipoint BET methods were considered) is used to calculate the surface area from nitrogen isotherms. The BJH method is used to determine the mean pore diameter. Table 5 shows the BET surface area and the average nanopore diameter for all the studied samples. The calculated external surface area increases by increasing the pH value from 13.8124 m2/g to 18.9829 m2/g (multipoint BET).Table 5
SABET (single-point and multipoint BET) and BJH method average pore diameter.
Sample
SABET (m2/g)Single-point BET
SABET (m2/g)Multi-point BET
Average nanopore diameter (nm)BJH method
MMT+TC_pH3
13.7856
13.8124
3.7102
MMT+TC_pH4
13.9145
13.9735
3.6905
MMT+TC_pH5
14.0864
14.3147
3.7289
MMT+TC_pH6
15.8261
15.9432
3.7305
MMT+TC_pH7
17.9425
18.1287
3.7646
MMT+TC_pH8
18.9461
18.9829
3.7724The SA measurement by the BET method (Figure6) showed that all the studied samples had a pore distribution categorized under type II adsorption isotherm in the classification of Brunauer, Deming, Deming, and Teller (BDDT) [63] which is due probably to the mesoporous texture with large pores (in addition to the nanopores). This result is due to the TC intercalation/adsorption process. Also, because of the ability of nitrogen to cover only the outer primary surface area but not the IS, an asymptotic approach to limiting quantity is observed in nitrogen isotherms. Indeed, it is necessary to differentiate between external, internal, and interlamellar surface areas for clays.Figure 6
Nitrogen adsorption-desorption isotherms of montmorillonite-exchanged TC under varying soil solution pH. MMT: montmorillonite; TC: tetracycline; ADS: adsorption; DES: desorption.The surface area concept does not give a complete textural description in the case of clay specimen; for that, a pore size (PS) and a pore size distribution (PSD) are necessary. The PSD in the mesopore region was determined by the BJH method assuming(i)
the shape of the pores with radius (r) approximatively half of its width is cylindrical [61]
(ii)
the radii (r) of mesopores assumed to be cylindrical corresponding to V values were calculated from the corrected Kelvin equation by the use of P/P0 values [64]
(iii)
the specific micropore, mesopore, and macropore volumes (namely,VMi, VMe, and VMa all in mL/g, respectively) are defined as the volumes of micropores, mesopores, and macropores including nanopores in one gram solid
(iv)
the presence of macropores has a low effect on the adsorptive properties of a solid [65]
(v)
the adsorption capacity as liquid nitrogen volumes which were estimated from desorption data at the relative equilibrium pressure (P/P0) less than 0.96 is taken as the specific micro-mesopore volumes (V=VMi+VMe)
(vi)
P0 and P are the vapor pressure of the bulk liquid nitrogen and equilibrium pressure of desorption at the liquid nitrogen temperature (∼77 K)TheV-r (cumulative pore volume vs. pore radius) plots are called mesopore PSD and given in Figure 7.Figure 7
The pore size distribution curve in the case of montmorillonite-exchanged TC under varying soil solution pH.The estimatedVMi and VMe can be obtained by the intercepts of the extrapolations of each PSD curve related to each sample [66]. The VMe increase from 0.027 to 0.036 mL/g by increasing soil solution pH during the intercalation/adsorption process.The radius derivative of theV-r curve for all samples is given in Figure 8 where the maximum mesopore volume (0.000948 mL/g) is obtained from pH 7 and the mesopore radii varied between 1.5 and 16 nm. The increase in the average pore diameter from a micropore with a width smaller than 2 nm is attributed to the reduction of microporous distribution in favor of mesoporous distribution. The porosity investigation using the BET-BJH method confirms observations obtained by SEM indicating changes on the morphological properties versus increasing pH rate. This transformation can be interpreted by a possible TC molecule conformation change.Figure 8
The derivative pore size distribution curve in the case of montmorillonite-exchanged TC under varying soil solution pH.


## 4. Discussion

The TC intercalation on the montmorillonite interlayer is confirmed by the layer thickness variation. This result is demonstrated by several works [19–21, 37]. The layer thickness evolution is ascribed to the interlamellar space organization between interlayer species, essentially water molecules, exchangeable sodium, and TC molecules.Based on the theoretical XRD analysis, it is shown that this variation is mainly affected by the nature and/or the amount of the intercalated water. [29] use the XRD modeling approach in order to characterize the pH-dependent intercalation of TC within montmorillonite, and they demonstrate that pH, when increased, is responsible of the reduction of the intercalated TC amounts. Also, they reveal that the pH-dependent change in the access of TC to the clay interlayers is not positively correlated with TC speciation, thus corroborating a possible correlation with changes in the clay surface chemistry as pH increases. In this work, another point of view is addressed, the correlation between the environment of the material and the soil solution pH in order to quantify the water levels present in the interlamellar space.The investigation of the water molecule evolution versus the soil solution pH (Figure9) shows quasiabsence of the 4W hydration state at pH=3 and pH=7, despite the high moisture contents at RH=80%. For the same pH range, the 3W hydration state dominates the structure indicating probably a great abundance, within the “clay particle” of the sheets presenting a complete intercalation of TC molecules. This result is confirmed by the presence of the highly hydrated state (i.e., 3W) even for the lowest humidity rate which is the case for all investigated pH values except pH=8. A notable effect of the pH variation is shown for the 1W hydration state which disappears from pH=4. This may be due to a new interlayer organization where a layer “population” with partial or total CEC saturation with the TC molecule is noted. For pH=7 and 8, a major 2W layer abundance manifests which is attributed to the TC conformation change demonstrated by the work of [29, 44, 46]. The proposition is confirmed by XRD analysis at pH=8 where a declared 4W hydration state, characterized by d001=22.07Å, is observed. This result agrees with those obtained by [21]. Indeed, they demonstrate that TC located in the interlayer spacing increase the d001 basal spacing from nearly 13.7 Å to nearly 22.0 Å. Physically, this result may have a logical explanation due to the increase in the TC molecule freedom degree within the interlayer space. This increase is attributed to the presence of 4W layers (at minimum) and a probable decrease in the concentration of exchanged TC molecules which is in concordance with earlier works.Figure 9
(a–f) Relative layer type abundances versus %RH for pH varying from 3 to 8.
(a)
(b)
(c)
(d)
(e)
(f)


## 5. Conclusions

The qualitative investigation of the 00l reflection obtained from XRD patterns has implied pH-dependent intercalation of TC within Na-exchanged montmorillonite but remains without real contribution to the understanding of the resulting interstratified structures. In this work, a correlation between results obtained from the XRD modeling approach, FTIR, SEM, and BET-BJH method is employed to exceed insufficient results obtained by the simple qualitative XRD analysis.Obtained results demonstrate the following:(i)
For a low pH value (pH=3), clay “particle” is characterized by a random MLS distribution
(ii)
By increasing the pH value, a segregated MLS distribution trend appears indicating the TC molecule intercalation process
(iii)
The quasihomogeneous 2W phases (obtained, respectively, at pH 7 and pH 8), attributed to unexfoliated smectite layers, are fully described using “in situ” XRD analysis
(iv)
The 4W hydration state (atpH=4) is accompanied by a probable TC molecule conformation change
(v)
The IR spectroscopy shows that the pH variation did not really affect the structure except for pH values close to 7 which confirms the obtained XRD results
(vi)
The SEM images show clear surface homogeneity changes as a function of the pH value, and for pH close to 7, the porosity increases probably
(vii)
SEM observations are confirmed by BET-BJH adsorption measurements which confirm a possible TC molecule conformation change from pH 7



---

*Source: 7414039-2019-09-12.xml*