# Encapsulated Urea-Kaolinite Nanocomposite for Controlled Release Fertilizer Formulations

Authors: Siafu Ibahati Sempeho; Hee Taik Kim; Egid Mubofu; Alexander Pogrebnoi; Godlisten Shao; Askwar Hilonga
Journal: Journal of Chemistry
 (2015)

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## Abstract

Urea controlled release fertilizer (CRF) was prepared via kaolinite intercalation followed by gum arabic encapsulation in an attempt to reduce its severe losses associated with dissolution, hydrolysis, and diffusion. Following the beneficiation, the nonkaolinite fraction decreased from 39.58% to 0.36% whereas the kaolinite fraction increased from 60.42% to 99.64%. The X-ray diffractions showed that kaolinite was a major phase with FCC Bravais crystal lattice with particle sizes ranging between 14.6 nm and 92.5 nm. The particle size varied with intercalation ratios with methanol intercalated kaolinite > DMSO-kaolinite > urea-kaolinite (KPDMU). Following intercalation, SEM analysis revealed a change of order from thick compact overlapping euhedral pseudohexagonal platelets to irregular booklets which later transformed to vermiform morphology and dispersed euhedral pseudohexagonal platelets. Besides, dispersed euhedral pseudohexagonal platelets were seen to coexist with blocky-vermicular booklets. In addition, a unique brain-form agglomeration which transformed into roundish particles mart was observed after encapsulation. The nanocomposites decomposed between 48 and 600°C. Release profiles showed that 100% of urea was released in 97 hours from KPDMU while 87% was released in 150 hours from the encapsulated nanocomposite. The findings established that it is possible to use Pugu kaolinite and gum arabic biopolymer to prepare urea CRF formulations.


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## Body

## 1. Introduction

In point of fact, urea is the most widely used nitrogen fertilizer in most parts of east Africa because of its high nitrogen (N) content (46%) and comparatively low cost of production; however, due to surface runoff, leaching, and vaporization, the utilization efficiency or plant uptake of urea is generally below 50% [1]. In fact, it is associated with up to 60 to 70% loss of the nitrogen being applied and contributes to greenhouse gases (GHG) emissions and water pollution [2] which in turn causes adverse effects during seed germination, seedling growth, and early plant growth in soil due to urea itself, to biuret and other impurities in urea fertilizers, and to products formed by hydrolysis or other transformations of urea in the soil [3, 4]. Such limitations can be reduced by amending urea fertilizers with small amounts of either urease inhibitor [4], by encapsulation with synthetic or biopolymers, or by intercalation with nanoclays to formulate CRFs [5, 6].Essentially, CRFs are prepared through encapsulation with low permeability excipients [7] using resin, wax, sulfur, polymer, silicates, and so forth, that prevents the nutrients it contains from being immediately available to the plant; as a result nutrients are released over an extended period leading to an increased control over the rate and pattern of nutrient release. Control over the release pattern depends on the thickness of the coatings within the formulation [8]. Precisely, CRFs exhibit superior features over traditional forms, such as decreased rate of nutrient losses from the soil by rain or irrigation water, sustained supply of nutrition for a prolonged time, increased fertilizer use efficiency (FUE), reduced frequency of application, minimized potential negative effects associated with overdosage, and reduced toxicity, thus making CRFs’ manufacturing and usage inevitable in the agricultural revolution era [1]. This paper describes the application of both intercalation reactions and encapsulation mechanisms to prepare urea based CRF by using Pugu kaolinite and gum arabic biopolymer.Archetypally, kaolinite belongs to a class of layered materials with its “crystals built by the stacking of two-dimensional units known as layers that are bound to each other through weak forces” [9]. The existence of such weak forces bounding the two-dimensional layers in place to form sheets makes layered materials including kaolinite and others described elsewhere [10–14] capable of undergoing intercalation reactions. According to [9] as quoted herein, “intercalation reactions occur by topotactic insertion of mobile guest species (neutral molecules, anhydrous or solvated ions) into the accessible crystallographic defined vacant sites located between the layers (interlayer spacings) in the layered host structure. In this intercalation compounds, strong covalent bond occurs in the layers and weak interactions, between host lattice and guest species or co-intercalated solvents. Ionic and solvent exchange reactions are related to the replacement of solvated guest species (cations and anions) located into the interlayer spacings. In this case, only the solvents, the cations or the solvated cations can be replaced, depending on the reaction conditions.”Fundamentally, the term intercalation involves insertion of a guest molecule into a host lattice whereby the guest-host structure or intercalation compound is only slightly perturbed from the host structure and that the reaction used to form the compound is reversible [15]. Typically, these reactions are just topochemical processes which involve conserving the natural host lattice structure in the course of the forward and reverse reactions unlike normal solid state reactions which involve extensive bond breaking and structural reorganization and require temperatures in excess of 600°C. For all intents and purposes as other reactions do, intercalation reactions also consist of bond breaking in the host as well as bond formation between the guest and host, a process which results in an increase in the basal spacing of the unit cell of the layer host lattice upon intercalation. In our context we refer to intercalation reactions in the layered silicates, particularly the kaolinite in the kaolin group of minerals which comprises among others nacrite, dickite, and halloysite [16] with kaolinite being the most abundant and differs from the other three members of the group by including molecular water in the interlayer [17], an inherent property which makes kaolinite suitable for undergoing intercalation reactions. Principally, kaolinite is 1 : 1 clay mineral consisting of two-dimensional sheets of corner sharing SiO4 tetrahedral and/or AlO4 octahedral and thereby categorized as a layered phyllosilicate capable of undergoing intercalation interactions and, so, “commonly employed in polymer/clay nanocomposites due to their swelling properties which result from their ability to hold water and other organic molecules between the silicate layers, high aspect ratio, high cation exchange capacities and large surface area” Chen et al. [18].Generally, layered phyllosilicate based controlled release fertilizers (CRFs) are fertilizer granules intercalated within carrier molecules commonly known as excipients to control nutrients release, thereby improving nutrient supply to crops and minimizing environmental, ecological, and health hazards; consequently the excipients play a role in regulating nutrients release time and eliminating the need for constant fertilization and higher efficiency rate than conventional soluble fertilizers [6]. Precisely, CRFs usage is an advanced way to supply crop’s nutrients (cf. conventional ways) due to gradual pattern of nutrient release, which improves fertilizer use efficiency (FUE) [6]. In this paper, a comprehensive investigation was done to intercalate urea fertilizer into the Pugu kaolinite interlayer spaces through a series of two intermediate consecutive stages involving dimethyl sulfoxide and methanol. Afterwards, urea fertilizer was intercalated by a way of replacing methanol intermediate complex through substitution mechanism and, finally, the urea intercalated Pugu kaolinite was encapsulated with gum arabic natural degradable biopolymer to form a crosslinked nanocomposite controlled release urea fertilizer.


## 2. Materials and Methods

Kaolinite was collected at Pugu hills in the coast region Kisarawe, Tanzania, by using quartering sampling technique described by [19]. Urea (ACS reagent, 99.0–100.5%) was supplied by Sigma Aldrich, Acacia powder (extra pure reagent) was supplied by Junsei Chemical Co., Ltd., Japan, DMSO (Extra pure, ≥99.5%) was supplied by Daejung Chemicals & Metals, Co., Ltd., Gyeonggi-do, Korea, sodium chloride (extra pure, ≥99.0%) was supplied by Samchun Pure Chemicals Co., Ltd., Gyeonggi-do, Korea, silver chloride (ACS reagent, 99.0%) was supplied by Sigma Aldrich, methanol (extra pure, ≥99.5%) was supplied by Daejung Chemicals & Metals, Co., Ltd., Gyeonggi-do, Korea, acacia powder (extra pure reagent) was supplied by Junsei Chemical Co., Ltd., Japan, deionized distilled water (D.I. was supplied by Professor Kim’s lab), and isopropanol was supplied by Daejung Chemicals & Metals, Co., Ltd., Gyeonggi-do, Korea.Since most raw kaolins are associated with some iron-bearing and black-colored materials which limit their usability [20], beneficiation thence remains to be an inevitable process necessary for their characterization, materials synthesis, and other advanced applications related to kaolin group of minerals where kaolinite is amongst. Purification of raw Pugu kaolinite was carried out with wet beneficiation technique by simple size separation using “Classifier.” The method involved the separation of fine platy kaolinite from coarse quartz, feldspar, mica, and other impurities using different setting velocities associated with particle size as governed by Stockes’ law. The entire procedure which involves crushing to pulverization and soaking as well as running the classifier unit to drying has been comprehensively described in [16]. Beneficiated kaolinite was modified by dispersing few grams in a 0.1 M NaCl solution and treated ultrasonically at 50°C for 30 hours and then magnetically stirred for more 30 hours under constant stirring. The product was filtered under vacuum filter and washed several times to remove excess chloride whereas washing was stopped after negative reaction with AgNO3. The washed product was dried in a vacuum oven at 60°C and stored as NaKP.Intercalating dimethyl sulfoxide (DMSO) into the kaolinite interlayer spaces was done as follows. A measured amount of Pugu kaolinite in a given volume of distilled water (D.I.) was mixed with DMSO solution in a ratio of 1 : 6 : 1, respectively, and then agitated in a magnetic stirrer for 21 days at 80°C with a very small addition of water droplets to hinder desiccation of the stirring mixture. After 21 days of continuous stirring the suspension was aged for one week by way of stirring at room temperature. The resultant suspension was then washed with excess isopropanol and dried at 60°C in a vacuum oven. The powdered product obtained was labeled KPDMSO. By using KPDMSO powder as a starting material, 2 g was taken and dispersed in a 60 mL of methanol solution followed by a 5-day stirring at RT. After 5 days of continuous stirring the suspension was left to mature over the weekend and, afterward, washing with isopropanol was done. The washed preparation was then dried at 60°C in a vacuum oven; the product in powder form obtained was named KPDM.Preparation of urea-kaolinite intercalated fertilizer formulation was carried via urea-methanol replacement mechanism. Methanol intercalated kaolinite (KPDM) was used as a starting material where a 1 : 1 ratio of this intermediate intercalation compound and urea was dispersed in a 60 mL of methanol solvent and then stirred for 5 days at 40°C. After 5 days of continuous stirring, excess isopropanol was used to wash the intercalation compound obtained in order to get off unreacted matter and impurities. The new urea fertilizer produced was labeled KPDMU and dried at 40°C in a vacuum oven to remove excess solvent. For the purpose of preparing urea based nanocomposite CRF formulation, acacia powder was employed as an encapsulating material to crosslink the urea-kaolinite intercalation compound. To the starting material (KPDMU), few grams was shaken with acacia powder in a ratio of 1 : 2 in a vessel containing 60 mL methanol as a solvent and then stirred for 150 hours at room temperature. Subsequently, the nanocomposite material obtained was filtered in a vacuum oven and dried at 40°C to dryness and kept for analysis as KPDMUG. As pointed out elsewhere [21, 22], the apparent intercalation ratio (AIR) was determined as shown in the following equation:(1)
AIR
=
Intensity
first  peak
intercalate
f
001
Intensity
first  peak
intercalate
f
001
+
Intensity
first  peak
initial  sample
i
001
.Generally, a diffraction pattern must first be indexed before being analyzed. Indexing was done by first determining the unit cell parameter from the peak position and then Miller indices due to the fact that diffraction pattern is a direct result of two things: (i) the size and shape of the unit cell which determine the relative position of the diffraction peak and (ii) the atomic position within the unit cell which determines the relative intensities of the diffraction peaks. The details of the procedures used for indexing [23] consist of six steps: (i) peak identification, (ii) determining Sin
2
⁡
θ, (iii) calculating the ratio of Sin
2
⁡
θ
/
Sin
2
⁡
θ
m
i
n, multiplied by the appropriate integers, (iv) determining the integer values of h
2
+
k
2
+
l
2, (v) identifying the Bravais lattice from the Miller indices, and (vi) calculating the lattice parameters. Determination of the estimate crystallite size was performed with X-ray diffraction pattern by using Scherrer equation:(2)
β
2
θ
=
K
λ
L
cos
⁡
θ
,where K is Scherrer constant for shape factor values, λ is wavelength of X-radiation, θ is half the diffraction angle, β is peak width, and L is the crystallite size [24]. According to [24], the most common K values include 0.94 for Full Width at Half Maximum (FWHM) of spherical crystals with cubic symmetry, 0.89 for integral breath of spherical crystals with cubic symmetry, and 1 because 0.94 and 0.89 both round up to 1 as well as the values of 0.62 to 2.08 because of variation in K.Characterization of the samples involved was done as follows. FTIR-ATR measurements were performed in the near infrared region at wavelength between 7500 and 360 cm−1 using a Bruker Optic GmbH (alpha model, Laser class 1) Spectrometer with attenuated total reflectance (ATR). XRD patterns of raw and beneficiated Pugu kaolinite for mineralogical characterization were executed on SIEMENS D-5005 X-ray Diffractometer using Cu Kα1 radiation. The 2
θ scan range was between 2° and 65°. On the other hand, the XRD patterns for the intercalation compounds as well as the nanocomposites were performed using Rigaku Corporation D/MAX-2500/PC X-ray Diffractometer equipped with a back monochromator operating at 40 kV and 100 mA at the scanning range of 5°–80° with a step size of 0.1° and a time/step of 1 s using copper cathode as the X-ray source (
λ
) (1.54056 Å). Thermogravimetry measurements of samples were taken using TG/STA Linseis STA PT 1000 simultaneous TG/DTG thermal analyzer at a scanning rate of 5°C per min from room temperature to 800°C under nitrogen atmosphere. The samples surfaces morphology was investigated by using Field Emission Scanning Electron Microscopy (SEM-Hitachi-s-4800, Japan). The accelerated voltage was 15 kV. The chemical composition of the raw materials was determined by X-ray Fluorescence (XRF) using the semiquantitative XRF analysis technique (Siemens SRS 3000 X-ray Fluorescence) (Rhodium anode, 8 analyzer crystals with beryllium windows 125 μm). The technique used is as we have described in our other recently published paper [25]. For the raw kaolinite sample the analysis of particle size distribution was carried out by using subsieve analysis technique which involves the application of Andreasen pipette sedimentation method. The details of the procedures are found in our recent article [25].


## 3. Results and Discussion

### 3.1. Effect of Beneficiation on the Distribution of Kaolinite Particles

The distribution of particles in the original and beneficiated Pugu kaolinite (Table1) revealed that 39.58% was a rejected portion since it was constituted with a nonkaolinite portion of particles greater than 63 µm which was not our interest since it was constituted of the nonkaolinite particles; 60.42% was the kaolinite fraction contained particles below 63 µm which was the anticipated working range because it was constituted of mostly kaolinite particles. Upon beneficiation trials, there was a significant improvement in the distribution of particles; the nonkaolinite fraction was reduced to 0.36% from the 39.58% of the nonbeneficiated portion, whereas the particles below 63 µm constituted 99.64% as compared to 60.42% of the nonbeneficiated portion. Essentially, it is necessary to note that the results from beneficiation trials revealed the fact that the method used was efficient and effective since there was a significant substantial reduction of nonkaolinite fraction from 39.58% of the raw Pugu kaolinite to 0.36% of the beneficiated Pugu kaolinite.Table 1
Effect of beneficiation on the distribution of raw kaolinite particles.
Sample
Percentage weight of particles (%)
≥63µm
≤63µm
Raw Pugu kaolin
39.58
60.42
Beneficiated Pugu kaolin
0.36
99.64


### 3.2. Kaolin Mineralogy

The randomly oriented whole rock X-ray diffraction analysis for both the original Pugu kaolin and the beneficiated Pugu kaolin revealed the mineral contents present as seen in Table2. Based on the whole rock powder mount diffractograms of raw Pugu kaolin the clay portion was only kaolinite while the nonclay portion or rather mineral impurities present in the kaolin were quartz (SiO2), clinochlore [Mg5Al(Si,Al)4O10(OH)8], and microcline [KAlSi3O8]. An observation made in the diffractograms of beneficiated kaolin is that the clay portion contained kaolinite [Al2Si2O5(OH)4], illite [KAl2(Si3AlO10)(OH)2], and clinochlore [Mg5Al(Si,Al)4O10(OH)8] accompanied with the disappearance of quartz and microcline. According to [19] the formation of illite is generally favored by alkaline conditions and by high concentrations of Al and K. It was mentioned that the appearance of illite in the beneficiated kaolin may be a result of reaction between Al and K from microcline and water, thereby causing weathering of silicates. The case may also be the same for clinochlore [17], but that may involve introduction of some Mg impurities during wet beneficiation trails. Although the pH of water used during beneficiation was not checked, it is suspected that the pH also contributed to this clay minerals transformation because the solubility of alumina is pH dependent and silica solubility increases parallel with the increase in pH [17]. Since the results from oriented air dried samples above were not enough to confirm the clay mineral groups obtained, it was therefore necessary to perform oriented clay analysis by X-ray diffraction method as untreated air-dried, glycolated, and heated at 550°C for two hours on the original and beneficiated kaolin samples with the aim of distinguishing layer types and clay mineral groups. When the air-dried samples were diffracted, peaks were developed on the diffractograms which revealed three main clay minerals, namely, kaolinite, illite, and clinochlore. Identification and hence confirmation of these clay minerals were achieved from the differences on the diffractograms obtained by glycolating the samples and drying them; then diffraction process was carried out, and the samples were heated at 550°C for two hours prior to the diffraction process [19]. This behavior of stability in chemical treatment (glycolated) and heat transformation (at 550°C) confirmed the presence of illite [26]. However, when the samples were glycolated, dried, and diffracted some peaks were shifted in some samples. But on heating the samples at 550°C followed by diffraction, these shifted peaks collapsed. This characteristic of altering the diffraction patterns is a distinguishing characteristic of kaolinite group [26]. Shortly, the mineralogical analysis test on the clay fraction revealed that the major content on both the original and beneficiated kaolin samples was kaolinite subordinated with illite.Table 2
Mineralogical composition of the raw materials.
Sample
Major phase
Minor phase
Original kaolin
Kaolinite [Al2Si2O5(OH)4]
Quartz [SiO2]
Microcline [KAlSi3O8]
Beneficiated kaolin
Kaolinite [Al2Si2O5(OH)4]
Clinochlore  [Mg5Al(Si,Al)4O10(OH)8]
Illite [KAl2(Si3AlO10)(OH)2]


### 3.3. Chemical Composition

The chemical composition of both raw and beneficiated Pugu kaolinite used in this study is given in Table3. As can be seen that beneficiation process was very successful, there was a reduction of silica content from 63.64 to 54.99% upon beneficiation whereas alumina content got increased from 31.43 to 40.2%. Variations in the composition of other oxides were also noticed as depicted in Table 3; however, a peculiar observation was that the amounts of TiO2 and Fe2O3 instead of getting decreased upon beneficiation were seen to increase from 0.8% and 1.01% to 1.02% and 2%, respectively, whereas the amount of MnO was seen to be unaffected with beneficiation process employed.Table 3
Chemical composition of the raw materials.
Sample
Oxide composition
SiO2
Al2O3
Na2O
MgO
SO3
Cl
K2O
CaO
TiO2
Cr2O3
MnO
Fe2O3
LOI
Pugu kaolin
63.64
31.43
0.43
0.16
0.25
0.76
1.39
0.06
0.8
0.03
0.01
1.01
0.03
Beneficiated kaolin
54.99
40.2
0.09
0.13
0.08
0.04
0.96
0.04
1.02
0.04
0.01
2
0.4


### 3.4. XRD Analysis

The calculated lattice parameters from the indexing procedures are given in Table4. Based on the sequence of h
2
+
k
2
+
l
2 values, most h
k
l reflections allowed are either all even or all odd; thus, the Bravais lattice was FCC. The average lattice parameter was 19.35 Å. By using Bragg’s equation under assumption that “n” is unit to confirm the results obtained with the six-step method, Table 5 was created whose sequence also suggested an FCC Bravais lattice. Similarly, the X-ray diffraction results reveal that the intercalation reactions were successful and, so, Pugu kaolinite can be used as CRF excipients for urea based fertilizers. This is evidenced with the fact presented in Figure 1 where intercalation of DMSO into the kaolinite interlayer spaces to form a pale yellow KPDMSO composite was achieved at the intercalation ratio of about 89.2% and that the basal lattice space for the first peak of the prepared kaolinite-DMSO nanocomposite was 1.12 nm which represents a lattice expansion of 0.41 nm as compared to the originally beneficiated Pugu kaolinite which had a basal spacing of 0.71 nm. Similarly, methoxy intercalated kaolinite (KPDM) presented in Figure 2 had the intercalation ratio of about 87.4% and basal lattice parameter for the first peak of the prepared kaolinite-methanol nanocomposite was 1.10 nm which represents a lattice expansion of 0.39 nm in relation to the beneficiated Pugu kaolinite. Furthermore, when kaolinite was treated with urea fertilizer, the resulting urea intercalated kaolinite (KPDMU) presented in Figure 3 had the intercalation ratio of about 91.10% and basal spacing of 1.09 nm which signify that the lattice parameter had been stretched out to distance of 0.38 nm as related to the beneficiated kaolinite. A closer look at the salt modified kaolinite (NaKP), a unique phenomenon was observed; basal spacing of the beneficiated kaolinite did shrink (instead of being expanded) to a distance of about 0.0005 nm which represents a difference of the basal lattice parameter of 0.7047 nm and 0.7052 nm for the modified kaolinite and the beneficiated kaolinite, respectively. Fundamentally, intercalation reactions were successful in the order of KPDM > KPDMSO > KPDMU. DMSO being a strong intercalant as compared to methanol and urea, the trend was expected to be KPDMU > KPDM > KPDMSO; the reason for an increased intercalation ratio for the KPDMU can be attributed to the fact that “in the dynamic intercalation process, kaolinite and urea in the mixer suffer from the action of high-speed stirring and high temperature. The shear force produced by the intense stirring accelerates delamination of crystal layers of kaolinite and increases the intercalation reaction speed of urea into kaolinite,” thereby stimulating the movement of urea molecules which in turn intensify the contact probability between urea molecules and kaolinite; as a result, the intercalation ratio is increased and so the trend was altered [22]. Thus, via DMSO-kaolinite intercalate as an intermediate, prepared by using salt treated kaolinite, urea fertilizer was intercalated into the kaolinite interlayer spaces by displacing methanol. The intercalated urea-kaolinite was then encapsulated with gum arabic to make the urea based CRF formulation.Table 4
Indexed XRD patterns.
Peak number
2
θ
Sin
2
⁡
θ
1
∗
Sin
2
⁡
θ
/
Sin
2
⁡
θ
m
i
n
2
∗
Sin
2
⁡
θ
/
Sin
2
⁡
θ
m
i
n
3
∗
Sin
2
⁡
θ
/
Sin
2
⁡
θ
m
i
n
h
2
+
k
2
+
l
2
h
k
l
a (Å)
d (nm)
1
12.54
0.011933
2.5191
5.0382
7.5573
8
220
19.95
0.715
2
24.85
0.046302
9.7745
19.5491
29.3236
29
520
19.28
0.358
3
12.55
0.011950
2.5227
5.0454
7.5681
8
220
19.93
0.705
4
24.90
0.046482
9.8125
19.6251
29.4376
29
520
19.24
0.357
5
7.89
0.004737
1.0000
2.0000
3.0000
3
111
19.39
1.119
6
23.59
0.041768
8.8174
17.6348
26.4522
27
333 or 511
19.22
0.377
7
8.04
0.004913
1.0372
2.0743
3.1115
3
111
19.04
1.099
8
23.60
0.041805
8.8252
17.6504
26.4756
27
333 or 511
19.21
0.377
9
8.14
0.005034
1.0627
2.1254
3.1881
3
111
18.81
1.086
10
22.34
0.037540
7.9248
15.8497
23.7745
24
422
19.48
0.398
FCC Bravais sequenceTable 5
Indexing XRD pattern: Bragg’s equation.
Peak number
Sin
⁡
θ
d (nm)
1
/
d
2
(
1
/
d
2
)
Ƶ
h
k
l
1
0.1092399
0.7265
1.8947
2
110
2
0.21518
0.3580
7.8025
10
310
3
0.109318
0.7046
2.0143
3
111
4
0.215596
0.3573
7.8331
10
310
5
0.068825
1.1192
0.7983
1
100
6
0.204371
0.3769
7.0396
9
300
7
0.070091
1.0990
0.82795
1
100
8
0.204464
0.3767
7.0471
9
300
9
0.070949
1.0857
0.8484
1
100
10
0.193753
0.3976
6.3257
8
220
FCC Bravais sequenceFigure 1
X-ray diffractograms of (a) beneficiated Pugu kaolinite, (b) NaKP, and (c) KPDMSO.Figure 2
X-ray diffractograms of (a) beneficiated Pugu kaolinite, (b) NaKP, and (c) KPDM.Figure 3
X-ray diffractograms of (a) beneficiated Pugu kaolinite, (b) NaKP, and (c) KPDMU.


### 3.5. Particle Size Analysis

The particle sizes determined for the intermediate intercalation compounds (KPDMSO and KPDM), urea intercalated kaolinite CRF (KPDMU), and the nanocomposite CRF formulation (KPDMUG) are given in Table6. Since our work was based on cubic systems, the best particles selected are those whose shape factor values include 0.94 and 0.89 together with their extreme cases, thereby coming to our conclusion of deciding to report a range of sizes. The sizes for DMSO intercalated kaolinite nanoparticles were in a range of 27.56–92.46 nm, whereas those of methanol intercalated kaolinite nanoparticles were in a range of 14.55–48.81 nm and those from urea-kaolinite CRF formulation were found to be between 15.16 and 50.84 nm. Precisely, nanoparticles from KPDMSO were twice as bigger than the rest for the reason not yet clear to us, but an assumption we have is that this might be contributed by the size and structural pattern of DMSO.Table 6
Analysis of particle sizes from Scherrer equation.
Sample
Crystallite size (nm)
K
=
2.08
K
=
1
K
=
0.94
K
=
0.89
K
=
0.62
KPDMSO
92.46
44.45
41.79
39.56
27.56
KPDM
48.81
23.47
22.06
20.88
14.55
KPDMU
50.84
24.44
22.98
21.75
15.16


### 3.6. SEM Analysis

A detailed analysis on the SEM images was carried out on the beneficiated kaolinite (KKK), NaKP, KPDMSO, KPDM, and KPDMU samples. Typically, the SEM images in Figure4 reveal the presence of a layered morphology common to kaolinite minerals; however, the appearance of these morphologies was seen to fluctuate with kaolinite modifications. The beneficiated kaolinite was characterized with predominantly wider and thick compact overlapping euhedral pseudohexagonal platelets (Figure 4(a)); this concurs with [27]. A change in the stacking sequence of kaolinite layers was observed upon chemical treatment with NaCl, where there occurred a mixture of irregular crystallites and thin very compacted layers appearing like booklets (Figure 4(b)). That is to say, NaKP exhibited many stacked thin euhedral pseudohexagonal platelets and part vermiform shaped particles. However, both beneficiated kaolinite and the salt treated kaolinite exhibited a high degree of crystallinity and stacking of the kaolinite particles which corresponds to kaolinite mineral [28]. As a matter of fact, the hexagonal faces of these particles correspond to the crystallographic (001) basal planes [29]. As expected, most particles were highly anisometric with thickness along the z-axis, much smaller than their other dimensions [29, 30]. Our observation is, when kaolinite was harshly treated with salts particularly, NaCl a change in the order of arrangement of kaolinite occurred such that the surface area for intercalation is increased due to well arrangements of functional layers. Similarly, it was observed that particles with pseudohexagonal morphology in NaKP predominates over those with vermiform morphology; a similar observation was found by [31].Figure 4
SEM images for (a) beneficiated Pugu kaolinite (KKK), (b) NaKP, (c) KPDMSO, (d) KPDM, and (e) KPDMU.Moreover, the DMSO intercalated kaolinite exhibited a decreased compactness between layers where the distance was widened (Figure4(c), red arrow). For the most part, vermicular booklet morphology characterized the DMSO intercalated kaolinite with a very small appearance of the dispersed euhedral pseudohexagonal platelets. A similar observation though in a different setting made Baeufort to conclude that “aggregates of kaolin with blocky habits coexist with vermicular booklets,” an observation which we have considered to be valid in this work [31]. Such observation made us to sense that under certain conditions the appearance of vermiforms mixed with either stacked or dispersed euhedral pseudohexagonal platelets should be expected. When methanol replaced DMSO to form KPDM in the kaolinite interlayer spaces the following features were observed (Figure 4(d)): (i) the distance between layers had shrunk as compared to distances observed in DMSO intercalated kaolinite (Figure 4(diii)), (ii) a further decrease of the appearance of the blocky aggregates with euhedral pseudohexagonal platy morphology indicating an increased number of clean layers available for intercalation reactions was observed, (iii) the vermicular booklets were seen to show bending forms in some parts (red arrows), and (iv) an appearance of well-coordinated roundish agglomerated particles resembling brain morphology was seen and we named this phenomena “brain-form agglomeration” which we believe could further facilitate intercalations (orange arrow). Furthermore, a complete disappearance of both dispersed euhedral pseudohexagonal platelets, vermicular booklets as well as brain-form agglomeration, was observed in the nanocomposite KPDMUG (Figure 4(e)) when the urea intercalated kaolinite was encapsulated with acacia powder and, instead, the surface’ morphology was observed to exhibit smooth mat at lower magnification which in the higher magnification the appearance was that of numerous small round particles assembled in a mat (Figure 4(eii)).


### 3.7. FT-IR Analysis

Treated kaolinite and beneficiated Pugu kaolinite are represented in Figures5 and 6, respectively. A close view at these figures reveals that the vibrations occurring at 3683 cm−1 of the treated kaolinite and 3684 cm−1 of beneficiated kaolinite correspond to the in-phase OH stretching of the inner surface hydroxyl of the kaolinite [32–35], whereas the vibrations seen at 3650 cm−1 are ascribed to the out-phase OH stretching vibrations of the inner surface hydroxyl groups. The bands exhibited at 3618 cm−1 are characteristic of inner layer OH stretching due to Al-O-H stretching vibrations of alumina of the kaolinite in the octahedral configuration while the characteristic OH stretching vibrations of the kaolinite in a tetrahedral configuration is exhibited at frequencies 749 cm−1 of the treated kaolinite [33] and is due to Si-O-Si symmetrical stretching [36]. The band seen at 1113 cm−1 is ascribed to the apical Si-O stretching mode and this is consistent with the band frequencies of 1112 cm−1 reported by [37]. While this was ascribed to Si-O normal to the planar stretching, the absorption band observed at 1023 to 997 cm−1 for the treated kaolinite and 995 cm−1 for the beneficiated kaolinite corresponds to the Si-O planar stretching which in fact concurs with 1025 to 995 cm−1 reported by [32]. To be more precise, the bands at 1023 cm−1 represent the in-plane Si-O planar stretching and 997 cm−1 or 995 cm−1 represents the out-phase Si-O planar stretching [32, 34, 35] and the alternating Si-O and Al-O bonds [36]; this is in close agreement to the 995 cm−1 obtained by [36] and the 997 cm−1 obtained by [38]. Another band seen at 910 cm−1 for the treated kaolinite and 909 cm−1 for the beneficiated kaolinite which closely relates to others of similar range reported in the literature such as 913 cm−1 [34], 907 cm−1 [36], 912 cm−1 [35], and 907 [39] is attributed to the OH deformation of inner hydroxyl groups due to the Al-OH bending [34]. Elsewhere, this band was ascribed to the Al-OH bending mode of kaolinite [36], Al -
(
V
I
)OH vibrations [35], and Al -
(
V
I
)OH vibrations [39]. The band at 788 cm−1 is ascribed to the Al-O-Si asymmetric bending of the bonds whereas the bands at 525 cm−1 and 520 cm−1 for the modified and beneficiated kaolinite, respectively, are given to the Si-O-Al (VI) where Al3+ is in octahedral coordination [36, 39, 40]. When you compare the diagrams for both beneficiated and treated kaolinite, one can easily notice a total identity between them. However, for the beneficiated kaolinite, we noticed the presence of a new broader absorption band at 3412 cm−1 which was absent in the treated kaolinite. This band corresponds to the peak maxima for water due to O-H stretching vibration and it is observed to be broader owing to the hydrogen bonding after wet beneficiation process [41–43]. Substantially, this band can be assigned to a combination of both stretching (asymmetrical + symmetrical) and overtone of bending vibrations [44].Figure 5
ATR-FTIR spectrum of NaKP.Figure 6
ATR-FTIR spectrum of beneficiated Pugu kaolinite.Most probably the direct intercalation of DMSO into the interlayer sheets of kaolinite was first achieved by [33]; the rule is that when DMSO molecules are intercalated into the kaolinite layers (which elsewhere has been described as ion substitution or site vacancies at the tetrahedral/octahedral sheets [6]) there would be a noticeable significant changes in the OH stretching region upon absorption of IR bands. This is clearly seen in Figures 5, 6, and 7, respectively, where the IR absorption bands of original, treated, and DMSO intercalated kaolinite are presented. Fundamentally, the infrared spectrum of the kaolinite-DMSO complex was expected to reveal the presence of alumina in both octahedral and tetrahedral configuration for the intercalated kaolinite. As can be seen the absorptions lies in the near IR region whereby the vibrational frequencies at 3698 to 3619 cm−1 represent the characteristic hydroxyl stretching vibrations of alumina of the kaolinite in the octahedral configuration whereas the bands at 736 cm−1 correspond to the characteristic hydroxyl stretching vibrations of alumina of the kaolinite in the tetrahedral configuration for the AlO4 antisymmetric stretching and that at 633 cm−1 they are attributed to the characteristic hydroxyl stretching vibrations of alumina of the kaolinite in the tetrahedral configuration for the AlO4 symmetric stretching. These predictions agree with [33, 45]. The vibrations at 3657 cm−1 are attributed to the OH stretching of the inner surface hydroxyl of the original kaolinite. Furthermore, we had observed that upon DMSO intercalation a new band at 3698 cm−1 was formed in the kaolinite-DMSO complex; this was related to the disappearance of the 3683 cm−1 band frequency of the treated kaolinite. In addition, an increase in wavelength from low to high (although a small shift) has been observed signifying that the intercalation was successful. This was confirmed by the appearance of a series of new bands upon intercalation as seen in Figure 7. The occurrence of infrared bands at 3012 and 2936 cm−1 which is close to the results obtained by [35] revealed the formation of organoclay compound and in this context we refer to the formation of kaolinite-DMSO intermediate nanocomposite. We have in turn ruled out that these bands would, respectively, be representing the -CH2 stretching for both symmetric and asymmetric vibrations.Figure 7
ATR-FTIR spectrum of KPDMSO.Moreover, the new sharp two-split peaks at 3530 and 3501 cm−1 correspond to the formation of the moderately hydrogen bonds between some of the inner-surface hydroxyls of the kaolinite layers and the sulfonyl oxygen of the intercalated DMSO molecules; this agrees with Thompson and Cuff’s predictions [46]. Similarly, our conclusion also agrees with [47–49] whose works reported IR bands at 3538 and 3502 cm−1. Moreover, the peak at 3657 cm−1 correspond to the inner-surface hydroxyl hydrogen bonded to the S=O group as referred to elsewhere [49]. There is also a unique CH band split into two bands at 1434 cm−1 and 1407 cm−1 and is attributed to the in-plane methyl deformation vibration of DMSO; in point of fact, this is in agreement with [49] who obtained two-split IR bands at 1411 and 1430 cm−1 due to intercalated DMSO methyl deformation.Basing on the literature surveyed, we have concluded that the distinct intense IR band seen at 1317 cm−1 represents the deformation of the inner surface OH groups hydrogen bonded to the S=O group of the DMSO molecules intercalated into the kaolinite layers and this reveals that only one type of hydrogen bonded inner surface OH group was formed during DMSO-kaolinite interaction as put forward by [49]. The analysis results also show that there is only one type of water molecules vibrations present; this is evidenced by the appearance of single broad band at 1655 cm−1 which is ascribed to water bending vibrations and that this single water molecule is hydrogen bonded to only one type of DMSO molecule associated with the kaolinite inner-surface OH groups observed at 1029 cm−1. According to [33], the vibrational assignments at 1121 cm−1 correspond to the in plane Si-O vibrations; at 998 cm−1 and 951 cm−1 represent Al-OH vibrations; at 736, 633, and 603 cm−1 vibrations stand for the gibbsite-like layers of the kaolinite; and, also, bands at 536, 501, and 452 cm−1 correspond to the Si-O-Al skeletal vibrations.Furthermore, upon introducing methoxy group into the kaolinite layers, several changes were observed in the IR spectrum as compared to the beneficiated and treated kaolinite and KPDMSO-kaolinite. As seen for KPDM in Figure8, new bands were observed at 3698, 3659, and 3619 cm−1 with similar reasons to ones given for KPDMSO above. However, the band at 3619 cm−1 is shown to be unshifted from the original kaolinite, modified kaolinite, DMSO intercalated kaolinite, and now in the methanol intercalated kaolinite; this is in fact in agreement with 3620 cm−1 wavelength obtained by [45]. The doubly split weak broad band at 3533 cm−1 is ascribed to the externally adsorbed water as suggested by [45, 50]; this band has also been considered as the OH stretching of methanol molecules and/or of water molecules formed during the esterification reaction of kaolinite inner-surface OH groups and methanol molecules [51]. The region around 3021 to 2800 cm−1 is marked by the three-split band and is ascribed to the methanol-kaolinite interaction. To be clearer, the OH stretching bands from alcohol molecules is visualized by band at 3012 cm−1 while at 2800 cm−1 it is attributed to the C-H stretching mode of methanol intercalated into the interlayer spaces of kaolinite sheets. The band at 2935 cm−1 refers to the C-H stretching region which confirms the presence of -OCH3 groups in the kaolinite interlayer spaces [50, 51]. A similar observation was made by [52] in that bands at 3021 cm−1 and 2935 cm−1 represent the C-H stretching mode of methanol; according to him, these vibrations are attributed to the CH3 out-phase and in-phase stretches of the methanol, respectively, which in turn act as an evidence for the grafting reaction of methoxy group in the kaolinite interlayer space as noted by [45]. Correspondingly, the bands at 1122 cm−1 are ascribed to the C-O stretching deformation in methanol molecules; this agrees with the C-O stretching deformation of 1123 cm−1 in methanol-kaolinite obtained by [45] while the new band recorded at 1003 cm−1 which also agrees with 1004 cm−1 obtained by [45] represents the lattice Si-O vibration bands due to methanol-kaolinite intercalation and it corresponds to a shift from 1113 cm−1 of the modified kaolinite. The observed low intensity bands at 957 cm−1 correspond to the Al-OH deformation whereas the band seen at 902 cm−1 is ascribed to the Al-OH in-plane bending vibration of the inner hydroxyl of kaolinite and this corresponds to a shift from 899 cm−1 of KPDMSO and 910 cm−1 of the modified kaolinite and 909 cm−1 of the beneficiated and treated (NaKP) kaolinite mineral. We have attributed the new kaolinite band at 789, 740, 675, 635, and 427 cm−1 in contrast to the beneficiated and treated (NaKP) kaolinite to the modifications of the bands related to the Si-O and Al-OH vibrations resulting from the perturbation of the kaolinite structure due to grafting of the methanol molecule; this again is in agreement with some of the results obtained elsewhere [45]. Noticeably, the IR spectra of both KPDMSO and KPDM revealed that DMSO molecules were successfully replaced by methanol molecules. This was evidenced by either a shift of characteristic bands or disappearance/appearance of new bands between the two. Similarly, there are clear substantial changes in the intensity of IR spectra in the OH region due to intercalation of DMSO and methoxy and the grafting of methoxy into the interlayer spaces of kaolinite sheets. This implies that there was a significant alteration in the local environment of inner-surface hydroxyl groups when DMSO molecules were replaced with methanol molecules during intercalation and grafting process. In fact, the presence of methoxy groups into the kaolinite layers is revealed by the significant decrease in the intensity of band representing interlamellar Al-OH of the silicate sheets at 957 cm−1 in the KPDM as compared to that of 953 cm−1 in the KPDMSO; this phenomenon is ascribed to the formation of Al-O-C bonds resulting from the grafting of methoxy groups into the kaolinite interlayer spaces, a fact that has been put forward and hence agrees with the findings obtained by [51].Figure 8
ATR-FTIR spectrum of KPDM.According to [49], urea and kaolinite sheets interact via hydrogen bonds both through the NH2 groups connected to the tetrahedral oxygens and through hydroxyl groups of the ions (located in the coordination sphere) connected to the carbonyl groups of urea. As seen, for the KPDMSO and KPDM (Figures 7 and 8), the position of the OH- bands was similar at 3698, 3657, and 953/957 cm−1; however, for the KPDMU (Figure 9), there is a complete disappearance of the outer hydroxyl stretching vibrations while the inner hydroxyl stretching vibrations occurring at 3619 cm−1 remained. Based on the predictions established by [52], the vibrations occurring at 3427 cm−1 could be attributed to the out-of-phase vibrations of the N-H stretch in the tetragonal urea while at 3340 cm−1 they could be assigned to the in-phase vibrations of the N-H stretch [49] and this agrees with the bands at 3420, 3436, and 3333 cm−1 obtained by [53], while, on the other hand, the free C=O stretch and some free bending NH2 motions [54] due to urea are ascribed to the 1612 cm−1 vibrations; this is in agreement with [54, 55]. In addition, the vibrations observed at 1590 cm−1 represent the H-N-C + C-N stretch and the in-phase CH3 bend of urea occurs at 1455 cm−1 vibration. In reference to known computer simulations the possible orientation of urea in the kaolinite-urea complex described that urea molecules point towards the silica sheet such that the hydrogen bonding is formed between the N-H group and the siloxane surface while conjugation between the C=O and N-H groups no longer exists; in so speaking the free C=O vibration bands in the IR spectra were expected to be seen [49, 56]. In many cases, the C=O stretching vibrations in saturated aliphatic aldehydes, ketones, and acids have frequencies in the range 1740–1700 cm−1 [54], which is higher than the observed vibrations for the KPDMU and the reason as pointed out by [54] is attributed to the existence of resonance structures caused by the presence of the free C=O molecules which interact with NH2, a mechanism which has been described elsewhere [54]. Precisely, the IR bands seen at 1455 cm−1 represent the asymmetric or scissoring C-N vibrations while those occurring at 1000 cm−1 were ascribed to the C-N symmetric modes and this is in agreement with 1465 and 1000 cm−1 by [54] and 1468 and 1010 cm−1 by [55]. The bands occurring at 1149 cm−1 represent the wagging or rocking N-H vibrations due to urea intercalated into the kaolinite layers; again this agrees with N-H vibrations at 1155 cm−1 obtained by [54]. According to the predictions made by [55, 57], the vibrations occurring at 786 cm−1 were ascribed to mutual N-H and CO out-of-plane wagging vibrations or in other words it is called the skeletal out-of-phase bending frequency equally attributable to larger deformational force constant, resulting from the decrease in the N-N distance of tetragonal urea [53]. Finally, for the KPDMU, the infrared bands occurring at 739 cm−1 represent the characteristic hydroxyl stretching vibrations of alumina of the kaolinite in a tetrahedral configuration for the AlO4 antisymmetric stretching while the SiOAl skeletal vibrations are observed at 527 cm−1.Figure 9
ATR-FTIR spectrum of KPDMU.Above that, unique changes were observed when gum arabic was used to encapsulate the urea-kaolinite intercalation compound to form the targeted nanocomposite KPDMUG. As can be seen in Figure10, there is a complete disappearance of kaolinite peaks at 3683, 3650, and 3618 cm−1. Besides, a unique observation was made on the vibrations occurring at 3618 cm−1 in that (i) the peak remained unaffected in the beneficiated and raw kaolinite as well as in the associated intercalation compounds KPDMSO, KPDM, and KPDMU. That is to say, despite all the modifications made on the kaolinite, that peak position remained unaltered; (ii) when these three kaolinite intercalations compounds were encapsulated with gum arabic biopolymer to form KPDMUG the peak got disappeared completely. This implies that the gum arabic encapsulation reaction was effective and successful. Noticeably, the out-phase vibration of the KPDMU at 3427 cm−1 has disappeared altogether. The band at 3340 cm−1 for KPDMU was raised to 3346 cm−1 in the KPDMUG. Two completely new bands appeared at 3212 and 2924 cm−1 with unique positioning and that is to say, there is a shift of the position 3427 cm−1 of KPDMU to 3346 cm−1 of KPDMUG and 3340 cm−1 of KPDMU to 3213 cm−1 of the KPDMUG although the peak shape was seen to change from narrow-sharp to broad for the KPDMUG. In such a phenomenon as pointed out by [53] that, upon crosslinking KPDMU with gum Arabic, the out-phase vibration shifted from 3427 cm−1 of KPDMU to 3346 cm−1 of KPDMUG while the in-phase vibration shifted from 3340 cm−1 of KPDMU to 3213 cm−1 of the KPDMUG. This phenomenon indicated that, upon crosslinking with gum arabic, urea’s unit cell was going from tetragonal to hexagonal shape as revealed from the spectra changes in the N-H stretching region of both KPDMU and KPDMUG. According to the assumptions made by [53], the tetragonal urea has its structure characterized by shorter hydrogen bonds which in fact made us assume that there will be lengthening of H-bonds in the hexagonal type. That is to say, during the formation of complex crosslinked urea-kaolinite structure, hydrogen bonding caused a change in orientation from more favorable tetragonal structure to a less favorable hexagonal structure which in turn reduced the stability of the latter as contrarily given by [53].Figure 10
ATR-FTIR spectrum of KPDMUG.Our prediction on the peak positioning after critical review in [58–60] is that the band seen at 3346 cm−1 represents the N-H stretch of urea while that in 3213 cm−1 corresponds to the O-H stretching vibrations which signifies that there is a hydrogen bonded hydroxyl group between the polymer and the intercalated nanocomposite. Precisely, this absorption band shows that the O-H bond was formed in the bonding of the intercalated nanocomposite and the crosslinking polymeric membrane [58]. A general observation in our view is that the strong broad band at 2924 and 1619 cm−1 is typical for carbohydrates which in our case refers to gum arabic grafted onto the substrate [59]. In a narrower view, the vibrations at 2924 cm−1 were ascribed to the C-H stretching; this deviates a little bit from 2933 cm−1 obtained by [60]. Based on the fact that this band emerged as a new shoulder upon crosslinking with gum arabic on the KPDMU, our conclusion has therefore been that it represents the symmetric stretching of both CH2 and CH groups which in turn proves the existence of grafting of gum arabic on the nanocomposite KPDMU [60]. The strong-high intensity peak at 1619 cm−1 corresponds to the COO asymmetric stretching (i.e., vC=O; vC-O) resulting from the interaction between gum arabic and the urea-kaolinite nanocomposite. This can be equally compared with 1610 cm−1 obtained by [60]. Based on the observations made before, we have concluded that the vibrations observed at 1455 cm−1 were ascribed to the in phase bending of urea. A close analysis of the frequencies seen at 1004 cm−1 made us to ascribe us to the C-N vibrations. In addition, the infrared band occurring at 779 cm−1 represents the characteristic hydroxyl stretching vibrations of alumina of the kaolinite in a tetrahedral configuration for the AlO4 antisymmetric stretching while the SiOAl skeletal vibrations are observed at 525 cm−1.


### 3.8. Thermogravimetric Analysis

TG-DTG analysis was employed in investigating thermal degradation and stability of the samples under N2 atmosphere. Relative to the TG thermograms for pure urea fertilizer (Figure 11), DMSO intercalated kaolinite (Figure 12) exhibited three degradation phases: the first was observed around 48–98°C attributed to the evaporation of externally adsorbed water on the kaolinite platelets, and this is related to 43°C obtained by [45]. The second degradation was observed around 120–170°C corresponding to the removal and decomposition of DMSO, whereas the third phase was observed at around 520–575°C which corresponds to the dehydroxylation of kaolinite sheets. Considerably, in average, these results are, respectively, comparable to 154 and 485°C obtained by [61] and, also, 181°C and 514°C obtained by [45]. On the other hand, methanol intercalated kaolinite is associated with two decomposition stages (Figure 13): the first which is comparably narrow was observed around 75–250°C corresponding to the removal of water moisture adsorbed on the sample as well as externally adsorbed methanol molecules, and this was relatively lower than 350°C obtained by [45]. The second degradation stage which is comparatively wider was observed at around 450–600°C corresponding to the decomposition of methanol-kaolinite intercalated compound and this observation reveals that methanol intercalated compound is highly hygroscopic such that the high amount of adsorbed water was completely removed at 250°C. According to [62], kaolins undergo dehydroxylation transformation within 400–700°C temperature range; however, the maximum dehydroxylation of kaolinite in the modified kaolinite (NaKP) was observed (Figure 14) at 575°C; therefore, a close look at the dehydroxylation transformation of 450–600°C for methanol intercalated kaolinite prepared would reveal an increased thermal stability. Furthermore, slight but significant changes in the thermal decomposition behavior with three degradation stages were observed when urea replaced methanol in the kaolinite interlayer spaces to form KPDMU (Figure 15). The first weight loss was observed at approximately 100–125°C corresponding to the following: (i) the loss of nonconstitutional water, (ii) removal of interlayer water, (iii) elimination of water coordinated to exchangeable cations or structural water as mentioned in [63], and (iv) degradation of urea; this discloses the fact that the release properties of our engineered urea CRF formulation would work best at that temperature range. Based on the findings obtained by [64], urea loss at about 140–250°C is caused by both (i) its own vaporization and (ii) degradation to its complementary form known as biuret [NH(CO)2(NH2)2]. The second weight loss was observed at about 225–350°C attributed to (i) the continuous sublimation of urea and (ii) decomposition or self-condensation of biuret [NH(CO)2(NH2)2] to more complex decomposition product to the completion of vaporization and degradation reaction [64]. The third weight loss was observed at around 500–575°C and was ascribed to the dehydroxylation of kaolinite a phenomena constituted by the decomposition of urea-kaolinite intercalated compound as well as elimination of structural hydroxyl and organic matter [45, 62, 63]. Comparatively, the thermal stability of methanol intercalated kaolinite and urea intercalated kaolinite increase in the inverse order.Figure 11
(a) TGA thermograms of urea. (b) Differential plot of urea fertilizer.Figure 12
(a) TGA thermograms of KPDMSO. (b) Differential plot of KPDMSO.Figure 13
(a) TGA thermograms of KPDM. (b) Differential plot of KPDM.Figure 14
(a) TGA thermograms of NaKP. (b) Differential plot of NaKP.Figure 15
(a) TGA thermograms of KPDMU. (b) Differential plot of KPDMU.Finally, the TG thermogram for the KPDMUG nanocomposite is associated with two degradation stages: the first was observed at approximately 48–425°C ascribed to the moisture evaporation, decomposition of the gum arabic biopolymer, and the elimination of interlayer moisture and water coordinated in the exchangeable cations as named by [63]. In fact, decomposition of gum arabic has been found to be in a range between 72 and 318°C [65] which signifies that temperature below that and above that range is due to moisture evaporation as well as elimination of interlayer moisture and coordinated water, respectively. The second stage occurring at about 475–550°C corresponds to the dehydroxylation of kaolinite. In this work, the first thermal degradation phase of the nanocomposite is the most titillating and significant since it reflects the objective of our study aimed at designing urea based CRF formulation via kaolinite intercalation reactions followed by encapsulation. As seen in Figure 16, the first degradation temperature with maxima at 425°C ascribed to urea reveals an increased thermal stability of the nanocomposite (KPDMUG) relative to the urea intercalated kaolinite (KPGMU) whose first thermal degradation temperature was noted to be at 205°C maxima.Figure 16
(a) TGA thermograms of KPDMUG. (b) Differential plot of KPDMUG.In addition to that, the derivative thermogravimetric analysis (DTG) as seen in (Figure17) provided the information regarding the thermal stability behavior of the prepared materials. KPDMSO and KPDM are dominated by decomposition of nonconstitutional water and kaolinite degradation; when compared to the DTG curve of NaKP, KPDMSO has an increased thermal stability by 10°C (520 for NaKP vis-à-vis 530 for KPDMSO), whereas KPDM has an increased thermal stability by 30°C (520 for NaKP vis-à-vis 550 for KPDM) and this portrays a substantial increase in melting temperature of the intercalated compounds as related to the modified kaolinite NaKP. On the contrary, the DTG curve of urea intercalated kaolinite and the nanocomposite is characterized by the urea degradation, a phenomenon which was also noted (although in a different setting) by [63] which in our case is marked by temperature regimes of 199°C, 226°C, and 320°C for pure urea; 175°C, 215°C, and 302°C for urea intercalated kaolinite (KPDMUG), and 180°C, 240°C, and 510°C for nanocomposite (KPDMUG). The presence of some free kaolinite residues not crosslinked was also noted and was revealed by the high 510°C decomposition temperature observed only in the KPDMUG but absent in the pure urea and KPDMU.Figure 17
Differential thermograms.


### 3.9. Urea Release Profiles

The release of urea from pure urea, KPDM, and KPDMUG as a function of time (in 5-hour intervals) was done by first weighing the amount of sample and then introducing the sample into the known volume of water contained in the dialysis bags. The system was shaken continually throughout the release trials. Measurements were taken after every 5-hour interval by simply drawing the solution from the dialysis membranes for analysis. Spectrophotometric determination of the amount of urea in water with hypochlorite and phenol technique was done thereafter. The method was adopted from [66] involving 8 steps which involves transferring a 20.0 mL aliquot of sample, which should be colorless, free from solid matter, and at room temperature to a 25 mL volumetric flask containing a microstirring magnet. Sample cavitation was barred through rapid addition because the microbubbles contribute to the blank signal; then 3.0 mL of distilled water was added and stirred vigorously followed by the addition of 0.30 mL of NaOCl reagent. After 5 seconds, 0.50 mL NaOBr was added with one hand whereas (0.30 + X) mL of HC1 reagent was added with the other hand after 2 more seconds (“X” is the volume in mL of HC1 reagent required to titrate 0.50 mL of NaOBr reagent to pH 7.0). Furthermore, after 20 seconds, 0.50 mL of H3BO3 buffer reagent was added with one hand followed with addition of 0.30 mL ethanolic phenol reagent after 2 more seconds with the other hand and stirred for 20 more seconds. After these 20 seconds, the absorbency of the sample solution at 454 nm was compared against distilled water. The blank sample procedures may be found elsewhere [66]. Calculations were then done to determine the concentration of urea by multiplying the difference between the blank and the general sample absorbencies by the difference between the general and standard sample absorbencies and divide by three twentieths the urea-N concentration of the added standard solution. The reader is recommended to view the detailed procedure and the mechanisms associated with the original author of this method [66].Besides, the rate of urea release as a function of time for a period of 150 hours was then investigated and summarized in Figure18. As can be seen, upon arduous dissolution test performed, 100% of the pure urea was released in just the first five hours of the first attempt to draw the aliquot, a result which was expected due to volatility of urea fertilizer associated with up to 60 to 70% loss in few minutes of the nitrogen being applied to the field [2] such that its utilization efficiency or plant uptake of urea is generally below 50% [1]. For the urea intercalated kaolinite nanocomposite (KPDMU) the observation made was that 100% of the intercalated urea was released within 97 hours, thereby unveiling the fact that Pugu kaolinite can retain urea and so can be used as a natural excipient for the preparation of CRF formulations. This observation indicated that urea adsorption and its subsequent intercalation into the kaolinite interlayer spaces was successful such that for its dissolution to take place an extended period of time was needed to induce its release mechanism. Furthermore, the ability of gum arabic biopolymer to retard urea dissolution was also noticed by its ability to retard urea release for a period of more than 150 hours. As can be seen, only 87% of the encapsulated urea contained into the kaolinite sheets was released after 150 hours. Such appealing results confirm our hypothesis that Pugu kaolinite layers can be expanded to accommodate molecular moieties; that is to say, it can be used to design CRF formulations based on urea fertilizer. As it was pointed out elsewhere [63] (a fact with which we also agree) that “in conventional application, the materials would be exposed to low water contents, and one can expect a better retention effect by the nanocomposites.” That is to say, the period of urea release from both urea intercalated kaolinite nanocomposite and encapsulated urea nanocomposite is expected to be more than these reported values done in the harsh laboratory settings.Figure 18
Release rate of (a) pure urea, (b) KPDMU, and (c) KPDMUG as a function of time at pH 7 and room temperature.


## 3.1. Effect of Beneficiation on the Distribution of Kaolinite Particles

The distribution of particles in the original and beneficiated Pugu kaolinite (Table1) revealed that 39.58% was a rejected portion since it was constituted with a nonkaolinite portion of particles greater than 63 µm which was not our interest since it was constituted of the nonkaolinite particles; 60.42% was the kaolinite fraction contained particles below 63 µm which was the anticipated working range because it was constituted of mostly kaolinite particles. Upon beneficiation trials, there was a significant improvement in the distribution of particles; the nonkaolinite fraction was reduced to 0.36% from the 39.58% of the nonbeneficiated portion, whereas the particles below 63 µm constituted 99.64% as compared to 60.42% of the nonbeneficiated portion. Essentially, it is necessary to note that the results from beneficiation trials revealed the fact that the method used was efficient and effective since there was a significant substantial reduction of nonkaolinite fraction from 39.58% of the raw Pugu kaolinite to 0.36% of the beneficiated Pugu kaolinite.Table 1
Effect of beneficiation on the distribution of raw kaolinite particles.
Sample
Percentage weight of particles (%)
≥63µm
≤63µm
Raw Pugu kaolin
39.58
60.42
Beneficiated Pugu kaolin
0.36
99.64


## 3.2. Kaolin Mineralogy

The randomly oriented whole rock X-ray diffraction analysis for both the original Pugu kaolin and the beneficiated Pugu kaolin revealed the mineral contents present as seen in Table2. Based on the whole rock powder mount diffractograms of raw Pugu kaolin the clay portion was only kaolinite while the nonclay portion or rather mineral impurities present in the kaolin were quartz (SiO2), clinochlore [Mg5Al(Si,Al)4O10(OH)8], and microcline [KAlSi3O8]. An observation made in the diffractograms of beneficiated kaolin is that the clay portion contained kaolinite [Al2Si2O5(OH)4], illite [KAl2(Si3AlO10)(OH)2], and clinochlore [Mg5Al(Si,Al)4O10(OH)8] accompanied with the disappearance of quartz and microcline. According to [19] the formation of illite is generally favored by alkaline conditions and by high concentrations of Al and K. It was mentioned that the appearance of illite in the beneficiated kaolin may be a result of reaction between Al and K from microcline and water, thereby causing weathering of silicates. The case may also be the same for clinochlore [17], but that may involve introduction of some Mg impurities during wet beneficiation trails. Although the pH of water used during beneficiation was not checked, it is suspected that the pH also contributed to this clay minerals transformation because the solubility of alumina is pH dependent and silica solubility increases parallel with the increase in pH [17]. Since the results from oriented air dried samples above were not enough to confirm the clay mineral groups obtained, it was therefore necessary to perform oriented clay analysis by X-ray diffraction method as untreated air-dried, glycolated, and heated at 550°C for two hours on the original and beneficiated kaolin samples with the aim of distinguishing layer types and clay mineral groups. When the air-dried samples were diffracted, peaks were developed on the diffractograms which revealed three main clay minerals, namely, kaolinite, illite, and clinochlore. Identification and hence confirmation of these clay minerals were achieved from the differences on the diffractograms obtained by glycolating the samples and drying them; then diffraction process was carried out, and the samples were heated at 550°C for two hours prior to the diffraction process [19]. This behavior of stability in chemical treatment (glycolated) and heat transformation (at 550°C) confirmed the presence of illite [26]. However, when the samples were glycolated, dried, and diffracted some peaks were shifted in some samples. But on heating the samples at 550°C followed by diffraction, these shifted peaks collapsed. This characteristic of altering the diffraction patterns is a distinguishing characteristic of kaolinite group [26]. Shortly, the mineralogical analysis test on the clay fraction revealed that the major content on both the original and beneficiated kaolin samples was kaolinite subordinated with illite.Table 2
Mineralogical composition of the raw materials.
Sample
Major phase
Minor phase
Original kaolin
Kaolinite [Al2Si2O5(OH)4]
Quartz [SiO2]
Microcline [KAlSi3O8]
Beneficiated kaolin
Kaolinite [Al2Si2O5(OH)4]
Clinochlore  [Mg5Al(Si,Al)4O10(OH)8]
Illite [KAl2(Si3AlO10)(OH)2]


## 3.3. Chemical Composition

The chemical composition of both raw and beneficiated Pugu kaolinite used in this study is given in Table3. As can be seen that beneficiation process was very successful, there was a reduction of silica content from 63.64 to 54.99% upon beneficiation whereas alumina content got increased from 31.43 to 40.2%. Variations in the composition of other oxides were also noticed as depicted in Table 3; however, a peculiar observation was that the amounts of TiO2 and Fe2O3 instead of getting decreased upon beneficiation were seen to increase from 0.8% and 1.01% to 1.02% and 2%, respectively, whereas the amount of MnO was seen to be unaffected with beneficiation process employed.Table 3
Chemical composition of the raw materials.
Sample
Oxide composition
SiO2
Al2O3
Na2O
MgO
SO3
Cl
K2O
CaO
TiO2
Cr2O3
MnO
Fe2O3
LOI
Pugu kaolin
63.64
31.43
0.43
0.16
0.25
0.76
1.39
0.06
0.8
0.03
0.01
1.01
0.03
Beneficiated kaolin
54.99
40.2
0.09
0.13
0.08
0.04
0.96
0.04
1.02
0.04
0.01
2
0.4


## 3.4. XRD Analysis

The calculated lattice parameters from the indexing procedures are given in Table4. Based on the sequence of h
2
+
k
2
+
l
2 values, most h
k
l reflections allowed are either all even or all odd; thus, the Bravais lattice was FCC. The average lattice parameter was 19.35 Å. By using Bragg’s equation under assumption that “n” is unit to confirm the results obtained with the six-step method, Table 5 was created whose sequence also suggested an FCC Bravais lattice. Similarly, the X-ray diffraction results reveal that the intercalation reactions were successful and, so, Pugu kaolinite can be used as CRF excipients for urea based fertilizers. This is evidenced with the fact presented in Figure 1 where intercalation of DMSO into the kaolinite interlayer spaces to form a pale yellow KPDMSO composite was achieved at the intercalation ratio of about 89.2% and that the basal lattice space for the first peak of the prepared kaolinite-DMSO nanocomposite was 1.12 nm which represents a lattice expansion of 0.41 nm as compared to the originally beneficiated Pugu kaolinite which had a basal spacing of 0.71 nm. Similarly, methoxy intercalated kaolinite (KPDM) presented in Figure 2 had the intercalation ratio of about 87.4% and basal lattice parameter for the first peak of the prepared kaolinite-methanol nanocomposite was 1.10 nm which represents a lattice expansion of 0.39 nm in relation to the beneficiated Pugu kaolinite. Furthermore, when kaolinite was treated with urea fertilizer, the resulting urea intercalated kaolinite (KPDMU) presented in Figure 3 had the intercalation ratio of about 91.10% and basal spacing of 1.09 nm which signify that the lattice parameter had been stretched out to distance of 0.38 nm as related to the beneficiated kaolinite. A closer look at the salt modified kaolinite (NaKP), a unique phenomenon was observed; basal spacing of the beneficiated kaolinite did shrink (instead of being expanded) to a distance of about 0.0005 nm which represents a difference of the basal lattice parameter of 0.7047 nm and 0.7052 nm for the modified kaolinite and the beneficiated kaolinite, respectively. Fundamentally, intercalation reactions were successful in the order of KPDM > KPDMSO > KPDMU. DMSO being a strong intercalant as compared to methanol and urea, the trend was expected to be KPDMU > KPDM > KPDMSO; the reason for an increased intercalation ratio for the KPDMU can be attributed to the fact that “in the dynamic intercalation process, kaolinite and urea in the mixer suffer from the action of high-speed stirring and high temperature. The shear force produced by the intense stirring accelerates delamination of crystal layers of kaolinite and increases the intercalation reaction speed of urea into kaolinite,” thereby stimulating the movement of urea molecules which in turn intensify the contact probability between urea molecules and kaolinite; as a result, the intercalation ratio is increased and so the trend was altered [22]. Thus, via DMSO-kaolinite intercalate as an intermediate, prepared by using salt treated kaolinite, urea fertilizer was intercalated into the kaolinite interlayer spaces by displacing methanol. The intercalated urea-kaolinite was then encapsulated with gum arabic to make the urea based CRF formulation.Table 4
Indexed XRD patterns.
Peak number
2
θ
Sin
2
⁡
θ
1
∗
Sin
2
⁡
θ
/
Sin
2
⁡
θ
m
i
n
2
∗
Sin
2
⁡
θ
/
Sin
2
⁡
θ
m
i
n
3
∗
Sin
2
⁡
θ
/
Sin
2
⁡
θ
m
i
n
h
2
+
k
2
+
l
2
h
k
l
a (Å)
d (nm)
1
12.54
0.011933
2.5191
5.0382
7.5573
8
220
19.95
0.715
2
24.85
0.046302
9.7745
19.5491
29.3236
29
520
19.28
0.358
3
12.55
0.011950
2.5227
5.0454
7.5681
8
220
19.93
0.705
4
24.90
0.046482
9.8125
19.6251
29.4376
29
520
19.24
0.357
5
7.89
0.004737
1.0000
2.0000
3.0000
3
111
19.39
1.119
6
23.59
0.041768
8.8174
17.6348
26.4522
27
333 or 511
19.22
0.377
7
8.04
0.004913
1.0372
2.0743
3.1115
3
111
19.04
1.099
8
23.60
0.041805
8.8252
17.6504
26.4756
27
333 or 511
19.21
0.377
9
8.14
0.005034
1.0627
2.1254
3.1881
3
111
18.81
1.086
10
22.34
0.037540
7.9248
15.8497
23.7745
24
422
19.48
0.398
FCC Bravais sequenceTable 5
Indexing XRD pattern: Bragg’s equation.
Peak number
Sin
⁡
θ
d (nm)
1
/
d
2
(
1
/
d
2
)
Ƶ
h
k
l
1
0.1092399
0.7265
1.8947
2
110
2
0.21518
0.3580
7.8025
10
310
3
0.109318
0.7046
2.0143
3
111
4
0.215596
0.3573
7.8331
10
310
5
0.068825
1.1192
0.7983
1
100
6
0.204371
0.3769
7.0396
9
300
7
0.070091
1.0990
0.82795
1
100
8
0.204464
0.3767
7.0471
9
300
9
0.070949
1.0857
0.8484
1
100
10
0.193753
0.3976
6.3257
8
220
FCC Bravais sequenceFigure 1
X-ray diffractograms of (a) beneficiated Pugu kaolinite, (b) NaKP, and (c) KPDMSO.Figure 2
X-ray diffractograms of (a) beneficiated Pugu kaolinite, (b) NaKP, and (c) KPDM.Figure 3
X-ray diffractograms of (a) beneficiated Pugu kaolinite, (b) NaKP, and (c) KPDMU.


## 3.5. Particle Size Analysis

The particle sizes determined for the intermediate intercalation compounds (KPDMSO and KPDM), urea intercalated kaolinite CRF (KPDMU), and the nanocomposite CRF formulation (KPDMUG) are given in Table6. Since our work was based on cubic systems, the best particles selected are those whose shape factor values include 0.94 and 0.89 together with their extreme cases, thereby coming to our conclusion of deciding to report a range of sizes. The sizes for DMSO intercalated kaolinite nanoparticles were in a range of 27.56–92.46 nm, whereas those of methanol intercalated kaolinite nanoparticles were in a range of 14.55–48.81 nm and those from urea-kaolinite CRF formulation were found to be between 15.16 and 50.84 nm. Precisely, nanoparticles from KPDMSO were twice as bigger than the rest for the reason not yet clear to us, but an assumption we have is that this might be contributed by the size and structural pattern of DMSO.Table 6
Analysis of particle sizes from Scherrer equation.
Sample
Crystallite size (nm)
K
=
2.08
K
=
1
K
=
0.94
K
=
0.89
K
=
0.62
KPDMSO
92.46
44.45
41.79
39.56
27.56
KPDM
48.81
23.47
22.06
20.88
14.55
KPDMU
50.84
24.44
22.98
21.75
15.16


## 3.6. SEM Analysis

A detailed analysis on the SEM images was carried out on the beneficiated kaolinite (KKK), NaKP, KPDMSO, KPDM, and KPDMU samples. Typically, the SEM images in Figure4 reveal the presence of a layered morphology common to kaolinite minerals; however, the appearance of these morphologies was seen to fluctuate with kaolinite modifications. The beneficiated kaolinite was characterized with predominantly wider and thick compact overlapping euhedral pseudohexagonal platelets (Figure 4(a)); this concurs with [27]. A change in the stacking sequence of kaolinite layers was observed upon chemical treatment with NaCl, where there occurred a mixture of irregular crystallites and thin very compacted layers appearing like booklets (Figure 4(b)). That is to say, NaKP exhibited many stacked thin euhedral pseudohexagonal platelets and part vermiform shaped particles. However, both beneficiated kaolinite and the salt treated kaolinite exhibited a high degree of crystallinity and stacking of the kaolinite particles which corresponds to kaolinite mineral [28]. As a matter of fact, the hexagonal faces of these particles correspond to the crystallographic (001) basal planes [29]. As expected, most particles were highly anisometric with thickness along the z-axis, much smaller than their other dimensions [29, 30]. Our observation is, when kaolinite was harshly treated with salts particularly, NaCl a change in the order of arrangement of kaolinite occurred such that the surface area for intercalation is increased due to well arrangements of functional layers. Similarly, it was observed that particles with pseudohexagonal morphology in NaKP predominates over those with vermiform morphology; a similar observation was found by [31].Figure 4
SEM images for (a) beneficiated Pugu kaolinite (KKK), (b) NaKP, (c) KPDMSO, (d) KPDM, and (e) KPDMU.Moreover, the DMSO intercalated kaolinite exhibited a decreased compactness between layers where the distance was widened (Figure4(c), red arrow). For the most part, vermicular booklet morphology characterized the DMSO intercalated kaolinite with a very small appearance of the dispersed euhedral pseudohexagonal platelets. A similar observation though in a different setting made Baeufort to conclude that “aggregates of kaolin with blocky habits coexist with vermicular booklets,” an observation which we have considered to be valid in this work [31]. Such observation made us to sense that under certain conditions the appearance of vermiforms mixed with either stacked or dispersed euhedral pseudohexagonal platelets should be expected. When methanol replaced DMSO to form KPDM in the kaolinite interlayer spaces the following features were observed (Figure 4(d)): (i) the distance between layers had shrunk as compared to distances observed in DMSO intercalated kaolinite (Figure 4(diii)), (ii) a further decrease of the appearance of the blocky aggregates with euhedral pseudohexagonal platy morphology indicating an increased number of clean layers available for intercalation reactions was observed, (iii) the vermicular booklets were seen to show bending forms in some parts (red arrows), and (iv) an appearance of well-coordinated roundish agglomerated particles resembling brain morphology was seen and we named this phenomena “brain-form agglomeration” which we believe could further facilitate intercalations (orange arrow). Furthermore, a complete disappearance of both dispersed euhedral pseudohexagonal platelets, vermicular booklets as well as brain-form agglomeration, was observed in the nanocomposite KPDMUG (Figure 4(e)) when the urea intercalated kaolinite was encapsulated with acacia powder and, instead, the surface’ morphology was observed to exhibit smooth mat at lower magnification which in the higher magnification the appearance was that of numerous small round particles assembled in a mat (Figure 4(eii)).


## 3.7. FT-IR Analysis

Treated kaolinite and beneficiated Pugu kaolinite are represented in Figures5 and 6, respectively. A close view at these figures reveals that the vibrations occurring at 3683 cm−1 of the treated kaolinite and 3684 cm−1 of beneficiated kaolinite correspond to the in-phase OH stretching of the inner surface hydroxyl of the kaolinite [32–35], whereas the vibrations seen at 3650 cm−1 are ascribed to the out-phase OH stretching vibrations of the inner surface hydroxyl groups. The bands exhibited at 3618 cm−1 are characteristic of inner layer OH stretching due to Al-O-H stretching vibrations of alumina of the kaolinite in the octahedral configuration while the characteristic OH stretching vibrations of the kaolinite in a tetrahedral configuration is exhibited at frequencies 749 cm−1 of the treated kaolinite [33] and is due to Si-O-Si symmetrical stretching [36]. The band seen at 1113 cm−1 is ascribed to the apical Si-O stretching mode and this is consistent with the band frequencies of 1112 cm−1 reported by [37]. While this was ascribed to Si-O normal to the planar stretching, the absorption band observed at 1023 to 997 cm−1 for the treated kaolinite and 995 cm−1 for the beneficiated kaolinite corresponds to the Si-O planar stretching which in fact concurs with 1025 to 995 cm−1 reported by [32]. To be more precise, the bands at 1023 cm−1 represent the in-plane Si-O planar stretching and 997 cm−1 or 995 cm−1 represents the out-phase Si-O planar stretching [32, 34, 35] and the alternating Si-O and Al-O bonds [36]; this is in close agreement to the 995 cm−1 obtained by [36] and the 997 cm−1 obtained by [38]. Another band seen at 910 cm−1 for the treated kaolinite and 909 cm−1 for the beneficiated kaolinite which closely relates to others of similar range reported in the literature such as 913 cm−1 [34], 907 cm−1 [36], 912 cm−1 [35], and 907 [39] is attributed to the OH deformation of inner hydroxyl groups due to the Al-OH bending [34]. Elsewhere, this band was ascribed to the Al-OH bending mode of kaolinite [36], Al -
(
V
I
)OH vibrations [35], and Al -
(
V
I
)OH vibrations [39]. The band at 788 cm−1 is ascribed to the Al-O-Si asymmetric bending of the bonds whereas the bands at 525 cm−1 and 520 cm−1 for the modified and beneficiated kaolinite, respectively, are given to the Si-O-Al (VI) where Al3+ is in octahedral coordination [36, 39, 40]. When you compare the diagrams for both beneficiated and treated kaolinite, one can easily notice a total identity between them. However, for the beneficiated kaolinite, we noticed the presence of a new broader absorption band at 3412 cm−1 which was absent in the treated kaolinite. This band corresponds to the peak maxima for water due to O-H stretching vibration and it is observed to be broader owing to the hydrogen bonding after wet beneficiation process [41–43]. Substantially, this band can be assigned to a combination of both stretching (asymmetrical + symmetrical) and overtone of bending vibrations [44].Figure 5
ATR-FTIR spectrum of NaKP.Figure 6
ATR-FTIR spectrum of beneficiated Pugu kaolinite.Most probably the direct intercalation of DMSO into the interlayer sheets of kaolinite was first achieved by [33]; the rule is that when DMSO molecules are intercalated into the kaolinite layers (which elsewhere has been described as ion substitution or site vacancies at the tetrahedral/octahedral sheets [6]) there would be a noticeable significant changes in the OH stretching region upon absorption of IR bands. This is clearly seen in Figures 5, 6, and 7, respectively, where the IR absorption bands of original, treated, and DMSO intercalated kaolinite are presented. Fundamentally, the infrared spectrum of the kaolinite-DMSO complex was expected to reveal the presence of alumina in both octahedral and tetrahedral configuration for the intercalated kaolinite. As can be seen the absorptions lies in the near IR region whereby the vibrational frequencies at 3698 to 3619 cm−1 represent the characteristic hydroxyl stretching vibrations of alumina of the kaolinite in the octahedral configuration whereas the bands at 736 cm−1 correspond to the characteristic hydroxyl stretching vibrations of alumina of the kaolinite in the tetrahedral configuration for the AlO4 antisymmetric stretching and that at 633 cm−1 they are attributed to the characteristic hydroxyl stretching vibrations of alumina of the kaolinite in the tetrahedral configuration for the AlO4 symmetric stretching. These predictions agree with [33, 45]. The vibrations at 3657 cm−1 are attributed to the OH stretching of the inner surface hydroxyl of the original kaolinite. Furthermore, we had observed that upon DMSO intercalation a new band at 3698 cm−1 was formed in the kaolinite-DMSO complex; this was related to the disappearance of the 3683 cm−1 band frequency of the treated kaolinite. In addition, an increase in wavelength from low to high (although a small shift) has been observed signifying that the intercalation was successful. This was confirmed by the appearance of a series of new bands upon intercalation as seen in Figure 7. The occurrence of infrared bands at 3012 and 2936 cm−1 which is close to the results obtained by [35] revealed the formation of organoclay compound and in this context we refer to the formation of kaolinite-DMSO intermediate nanocomposite. We have in turn ruled out that these bands would, respectively, be representing the -CH2 stretching for both symmetric and asymmetric vibrations.Figure 7
ATR-FTIR spectrum of KPDMSO.Moreover, the new sharp two-split peaks at 3530 and 3501 cm−1 correspond to the formation of the moderately hydrogen bonds between some of the inner-surface hydroxyls of the kaolinite layers and the sulfonyl oxygen of the intercalated DMSO molecules; this agrees with Thompson and Cuff’s predictions [46]. Similarly, our conclusion also agrees with [47–49] whose works reported IR bands at 3538 and 3502 cm−1. Moreover, the peak at 3657 cm−1 correspond to the inner-surface hydroxyl hydrogen bonded to the S=O group as referred to elsewhere [49]. There is also a unique CH band split into two bands at 1434 cm−1 and 1407 cm−1 and is attributed to the in-plane methyl deformation vibration of DMSO; in point of fact, this is in agreement with [49] who obtained two-split IR bands at 1411 and 1430 cm−1 due to intercalated DMSO methyl deformation.Basing on the literature surveyed, we have concluded that the distinct intense IR band seen at 1317 cm−1 represents the deformation of the inner surface OH groups hydrogen bonded to the S=O group of the DMSO molecules intercalated into the kaolinite layers and this reveals that only one type of hydrogen bonded inner surface OH group was formed during DMSO-kaolinite interaction as put forward by [49]. The analysis results also show that there is only one type of water molecules vibrations present; this is evidenced by the appearance of single broad band at 1655 cm−1 which is ascribed to water bending vibrations and that this single water molecule is hydrogen bonded to only one type of DMSO molecule associated with the kaolinite inner-surface OH groups observed at 1029 cm−1. According to [33], the vibrational assignments at 1121 cm−1 correspond to the in plane Si-O vibrations; at 998 cm−1 and 951 cm−1 represent Al-OH vibrations; at 736, 633, and 603 cm−1 vibrations stand for the gibbsite-like layers of the kaolinite; and, also, bands at 536, 501, and 452 cm−1 correspond to the Si-O-Al skeletal vibrations.Furthermore, upon introducing methoxy group into the kaolinite layers, several changes were observed in the IR spectrum as compared to the beneficiated and treated kaolinite and KPDMSO-kaolinite. As seen for KPDM in Figure8, new bands were observed at 3698, 3659, and 3619 cm−1 with similar reasons to ones given for KPDMSO above. However, the band at 3619 cm−1 is shown to be unshifted from the original kaolinite, modified kaolinite, DMSO intercalated kaolinite, and now in the methanol intercalated kaolinite; this is in fact in agreement with 3620 cm−1 wavelength obtained by [45]. The doubly split weak broad band at 3533 cm−1 is ascribed to the externally adsorbed water as suggested by [45, 50]; this band has also been considered as the OH stretching of methanol molecules and/or of water molecules formed during the esterification reaction of kaolinite inner-surface OH groups and methanol molecules [51]. The region around 3021 to 2800 cm−1 is marked by the three-split band and is ascribed to the methanol-kaolinite interaction. To be clearer, the OH stretching bands from alcohol molecules is visualized by band at 3012 cm−1 while at 2800 cm−1 it is attributed to the C-H stretching mode of methanol intercalated into the interlayer spaces of kaolinite sheets. The band at 2935 cm−1 refers to the C-H stretching region which confirms the presence of -OCH3 groups in the kaolinite interlayer spaces [50, 51]. A similar observation was made by [52] in that bands at 3021 cm−1 and 2935 cm−1 represent the C-H stretching mode of methanol; according to him, these vibrations are attributed to the CH3 out-phase and in-phase stretches of the methanol, respectively, which in turn act as an evidence for the grafting reaction of methoxy group in the kaolinite interlayer space as noted by [45]. Correspondingly, the bands at 1122 cm−1 are ascribed to the C-O stretching deformation in methanol molecules; this agrees with the C-O stretching deformation of 1123 cm−1 in methanol-kaolinite obtained by [45] while the new band recorded at 1003 cm−1 which also agrees with 1004 cm−1 obtained by [45] represents the lattice Si-O vibration bands due to methanol-kaolinite intercalation and it corresponds to a shift from 1113 cm−1 of the modified kaolinite. The observed low intensity bands at 957 cm−1 correspond to the Al-OH deformation whereas the band seen at 902 cm−1 is ascribed to the Al-OH in-plane bending vibration of the inner hydroxyl of kaolinite and this corresponds to a shift from 899 cm−1 of KPDMSO and 910 cm−1 of the modified kaolinite and 909 cm−1 of the beneficiated and treated (NaKP) kaolinite mineral. We have attributed the new kaolinite band at 789, 740, 675, 635, and 427 cm−1 in contrast to the beneficiated and treated (NaKP) kaolinite to the modifications of the bands related to the Si-O and Al-OH vibrations resulting from the perturbation of the kaolinite structure due to grafting of the methanol molecule; this again is in agreement with some of the results obtained elsewhere [45]. Noticeably, the IR spectra of both KPDMSO and KPDM revealed that DMSO molecules were successfully replaced by methanol molecules. This was evidenced by either a shift of characteristic bands or disappearance/appearance of new bands between the two. Similarly, there are clear substantial changes in the intensity of IR spectra in the OH region due to intercalation of DMSO and methoxy and the grafting of methoxy into the interlayer spaces of kaolinite sheets. This implies that there was a significant alteration in the local environment of inner-surface hydroxyl groups when DMSO molecules were replaced with methanol molecules during intercalation and grafting process. In fact, the presence of methoxy groups into the kaolinite layers is revealed by the significant decrease in the intensity of band representing interlamellar Al-OH of the silicate sheets at 957 cm−1 in the KPDM as compared to that of 953 cm−1 in the KPDMSO; this phenomenon is ascribed to the formation of Al-O-C bonds resulting from the grafting of methoxy groups into the kaolinite interlayer spaces, a fact that has been put forward and hence agrees with the findings obtained by [51].Figure 8
ATR-FTIR spectrum of KPDM.According to [49], urea and kaolinite sheets interact via hydrogen bonds both through the NH2 groups connected to the tetrahedral oxygens and through hydroxyl groups of the ions (located in the coordination sphere) connected to the carbonyl groups of urea. As seen, for the KPDMSO and KPDM (Figures 7 and 8), the position of the OH- bands was similar at 3698, 3657, and 953/957 cm−1; however, for the KPDMU (Figure 9), there is a complete disappearance of the outer hydroxyl stretching vibrations while the inner hydroxyl stretching vibrations occurring at 3619 cm−1 remained. Based on the predictions established by [52], the vibrations occurring at 3427 cm−1 could be attributed to the out-of-phase vibrations of the N-H stretch in the tetragonal urea while at 3340 cm−1 they could be assigned to the in-phase vibrations of the N-H stretch [49] and this agrees with the bands at 3420, 3436, and 3333 cm−1 obtained by [53], while, on the other hand, the free C=O stretch and some free bending NH2 motions [54] due to urea are ascribed to the 1612 cm−1 vibrations; this is in agreement with [54, 55]. In addition, the vibrations observed at 1590 cm−1 represent the H-N-C + C-N stretch and the in-phase CH3 bend of urea occurs at 1455 cm−1 vibration. In reference to known computer simulations the possible orientation of urea in the kaolinite-urea complex described that urea molecules point towards the silica sheet such that the hydrogen bonding is formed between the N-H group and the siloxane surface while conjugation between the C=O and N-H groups no longer exists; in so speaking the free C=O vibration bands in the IR spectra were expected to be seen [49, 56]. In many cases, the C=O stretching vibrations in saturated aliphatic aldehydes, ketones, and acids have frequencies in the range 1740–1700 cm−1 [54], which is higher than the observed vibrations for the KPDMU and the reason as pointed out by [54] is attributed to the existence of resonance structures caused by the presence of the free C=O molecules which interact with NH2, a mechanism which has been described elsewhere [54]. Precisely, the IR bands seen at 1455 cm−1 represent the asymmetric or scissoring C-N vibrations while those occurring at 1000 cm−1 were ascribed to the C-N symmetric modes and this is in agreement with 1465 and 1000 cm−1 by [54] and 1468 and 1010 cm−1 by [55]. The bands occurring at 1149 cm−1 represent the wagging or rocking N-H vibrations due to urea intercalated into the kaolinite layers; again this agrees with N-H vibrations at 1155 cm−1 obtained by [54]. According to the predictions made by [55, 57], the vibrations occurring at 786 cm−1 were ascribed to mutual N-H and CO out-of-plane wagging vibrations or in other words it is called the skeletal out-of-phase bending frequency equally attributable to larger deformational force constant, resulting from the decrease in the N-N distance of tetragonal urea [53]. Finally, for the KPDMU, the infrared bands occurring at 739 cm−1 represent the characteristic hydroxyl stretching vibrations of alumina of the kaolinite in a tetrahedral configuration for the AlO4 antisymmetric stretching while the SiOAl skeletal vibrations are observed at 527 cm−1.Figure 9
ATR-FTIR spectrum of KPDMU.Above that, unique changes were observed when gum arabic was used to encapsulate the urea-kaolinite intercalation compound to form the targeted nanocomposite KPDMUG. As can be seen in Figure10, there is a complete disappearance of kaolinite peaks at 3683, 3650, and 3618 cm−1. Besides, a unique observation was made on the vibrations occurring at 3618 cm−1 in that (i) the peak remained unaffected in the beneficiated and raw kaolinite as well as in the associated intercalation compounds KPDMSO, KPDM, and KPDMU. That is to say, despite all the modifications made on the kaolinite, that peak position remained unaltered; (ii) when these three kaolinite intercalations compounds were encapsulated with gum arabic biopolymer to form KPDMUG the peak got disappeared completely. This implies that the gum arabic encapsulation reaction was effective and successful. Noticeably, the out-phase vibration of the KPDMU at 3427 cm−1 has disappeared altogether. The band at 3340 cm−1 for KPDMU was raised to 3346 cm−1 in the KPDMUG. Two completely new bands appeared at 3212 and 2924 cm−1 with unique positioning and that is to say, there is a shift of the position 3427 cm−1 of KPDMU to 3346 cm−1 of KPDMUG and 3340 cm−1 of KPDMU to 3213 cm−1 of the KPDMUG although the peak shape was seen to change from narrow-sharp to broad for the KPDMUG. In such a phenomenon as pointed out by [53] that, upon crosslinking KPDMU with gum Arabic, the out-phase vibration shifted from 3427 cm−1 of KPDMU to 3346 cm−1 of KPDMUG while the in-phase vibration shifted from 3340 cm−1 of KPDMU to 3213 cm−1 of the KPDMUG. This phenomenon indicated that, upon crosslinking with gum arabic, urea’s unit cell was going from tetragonal to hexagonal shape as revealed from the spectra changes in the N-H stretching region of both KPDMU and KPDMUG. According to the assumptions made by [53], the tetragonal urea has its structure characterized by shorter hydrogen bonds which in fact made us assume that there will be lengthening of H-bonds in the hexagonal type. That is to say, during the formation of complex crosslinked urea-kaolinite structure, hydrogen bonding caused a change in orientation from more favorable tetragonal structure to a less favorable hexagonal structure which in turn reduced the stability of the latter as contrarily given by [53].Figure 10
ATR-FTIR spectrum of KPDMUG.Our prediction on the peak positioning after critical review in [58–60] is that the band seen at 3346 cm−1 represents the N-H stretch of urea while that in 3213 cm−1 corresponds to the O-H stretching vibrations which signifies that there is a hydrogen bonded hydroxyl group between the polymer and the intercalated nanocomposite. Precisely, this absorption band shows that the O-H bond was formed in the bonding of the intercalated nanocomposite and the crosslinking polymeric membrane [58]. A general observation in our view is that the strong broad band at 2924 and 1619 cm−1 is typical for carbohydrates which in our case refers to gum arabic grafted onto the substrate [59]. In a narrower view, the vibrations at 2924 cm−1 were ascribed to the C-H stretching; this deviates a little bit from 2933 cm−1 obtained by [60]. Based on the fact that this band emerged as a new shoulder upon crosslinking with gum arabic on the KPDMU, our conclusion has therefore been that it represents the symmetric stretching of both CH2 and CH groups which in turn proves the existence of grafting of gum arabic on the nanocomposite KPDMU [60]. The strong-high intensity peak at 1619 cm−1 corresponds to the COO asymmetric stretching (i.e., vC=O; vC-O) resulting from the interaction between gum arabic and the urea-kaolinite nanocomposite. This can be equally compared with 1610 cm−1 obtained by [60]. Based on the observations made before, we have concluded that the vibrations observed at 1455 cm−1 were ascribed to the in phase bending of urea. A close analysis of the frequencies seen at 1004 cm−1 made us to ascribe us to the C-N vibrations. In addition, the infrared band occurring at 779 cm−1 represents the characteristic hydroxyl stretching vibrations of alumina of the kaolinite in a tetrahedral configuration for the AlO4 antisymmetric stretching while the SiOAl skeletal vibrations are observed at 525 cm−1.


## 3.8. Thermogravimetric Analysis

TG-DTG analysis was employed in investigating thermal degradation and stability of the samples under N2 atmosphere. Relative to the TG thermograms for pure urea fertilizer (Figure 11), DMSO intercalated kaolinite (Figure 12) exhibited three degradation phases: the first was observed around 48–98°C attributed to the evaporation of externally adsorbed water on the kaolinite platelets, and this is related to 43°C obtained by [45]. The second degradation was observed around 120–170°C corresponding to the removal and decomposition of DMSO, whereas the third phase was observed at around 520–575°C which corresponds to the dehydroxylation of kaolinite sheets. Considerably, in average, these results are, respectively, comparable to 154 and 485°C obtained by [61] and, also, 181°C and 514°C obtained by [45]. On the other hand, methanol intercalated kaolinite is associated with two decomposition stages (Figure 13): the first which is comparably narrow was observed around 75–250°C corresponding to the removal of water moisture adsorbed on the sample as well as externally adsorbed methanol molecules, and this was relatively lower than 350°C obtained by [45]. The second degradation stage which is comparatively wider was observed at around 450–600°C corresponding to the decomposition of methanol-kaolinite intercalated compound and this observation reveals that methanol intercalated compound is highly hygroscopic such that the high amount of adsorbed water was completely removed at 250°C. According to [62], kaolins undergo dehydroxylation transformation within 400–700°C temperature range; however, the maximum dehydroxylation of kaolinite in the modified kaolinite (NaKP) was observed (Figure 14) at 575°C; therefore, a close look at the dehydroxylation transformation of 450–600°C for methanol intercalated kaolinite prepared would reveal an increased thermal stability. Furthermore, slight but significant changes in the thermal decomposition behavior with three degradation stages were observed when urea replaced methanol in the kaolinite interlayer spaces to form KPDMU (Figure 15). The first weight loss was observed at approximately 100–125°C corresponding to the following: (i) the loss of nonconstitutional water, (ii) removal of interlayer water, (iii) elimination of water coordinated to exchangeable cations or structural water as mentioned in [63], and (iv) degradation of urea; this discloses the fact that the release properties of our engineered urea CRF formulation would work best at that temperature range. Based on the findings obtained by [64], urea loss at about 140–250°C is caused by both (i) its own vaporization and (ii) degradation to its complementary form known as biuret [NH(CO)2(NH2)2]. The second weight loss was observed at about 225–350°C attributed to (i) the continuous sublimation of urea and (ii) decomposition or self-condensation of biuret [NH(CO)2(NH2)2] to more complex decomposition product to the completion of vaporization and degradation reaction [64]. The third weight loss was observed at around 500–575°C and was ascribed to the dehydroxylation of kaolinite a phenomena constituted by the decomposition of urea-kaolinite intercalated compound as well as elimination of structural hydroxyl and organic matter [45, 62, 63]. Comparatively, the thermal stability of methanol intercalated kaolinite and urea intercalated kaolinite increase in the inverse order.Figure 11
(a) TGA thermograms of urea. (b) Differential plot of urea fertilizer.Figure 12
(a) TGA thermograms of KPDMSO. (b) Differential plot of KPDMSO.Figure 13
(a) TGA thermograms of KPDM. (b) Differential plot of KPDM.Figure 14
(a) TGA thermograms of NaKP. (b) Differential plot of NaKP.Figure 15
(a) TGA thermograms of KPDMU. (b) Differential plot of KPDMU.Finally, the TG thermogram for the KPDMUG nanocomposite is associated with two degradation stages: the first was observed at approximately 48–425°C ascribed to the moisture evaporation, decomposition of the gum arabic biopolymer, and the elimination of interlayer moisture and water coordinated in the exchangeable cations as named by [63]. In fact, decomposition of gum arabic has been found to be in a range between 72 and 318°C [65] which signifies that temperature below that and above that range is due to moisture evaporation as well as elimination of interlayer moisture and coordinated water, respectively. The second stage occurring at about 475–550°C corresponds to the dehydroxylation of kaolinite. In this work, the first thermal degradation phase of the nanocomposite is the most titillating and significant since it reflects the objective of our study aimed at designing urea based CRF formulation via kaolinite intercalation reactions followed by encapsulation. As seen in Figure 16, the first degradation temperature with maxima at 425°C ascribed to urea reveals an increased thermal stability of the nanocomposite (KPDMUG) relative to the urea intercalated kaolinite (KPGMU) whose first thermal degradation temperature was noted to be at 205°C maxima.Figure 16
(a) TGA thermograms of KPDMUG. (b) Differential plot of KPDMUG.In addition to that, the derivative thermogravimetric analysis (DTG) as seen in (Figure17) provided the information regarding the thermal stability behavior of the prepared materials. KPDMSO and KPDM are dominated by decomposition of nonconstitutional water and kaolinite degradation; when compared to the DTG curve of NaKP, KPDMSO has an increased thermal stability by 10°C (520 for NaKP vis-à-vis 530 for KPDMSO), whereas KPDM has an increased thermal stability by 30°C (520 for NaKP vis-à-vis 550 for KPDM) and this portrays a substantial increase in melting temperature of the intercalated compounds as related to the modified kaolinite NaKP. On the contrary, the DTG curve of urea intercalated kaolinite and the nanocomposite is characterized by the urea degradation, a phenomenon which was also noted (although in a different setting) by [63] which in our case is marked by temperature regimes of 199°C, 226°C, and 320°C for pure urea; 175°C, 215°C, and 302°C for urea intercalated kaolinite (KPDMUG), and 180°C, 240°C, and 510°C for nanocomposite (KPDMUG). The presence of some free kaolinite residues not crosslinked was also noted and was revealed by the high 510°C decomposition temperature observed only in the KPDMUG but absent in the pure urea and KPDMU.Figure 17
Differential thermograms.


## 3.9. Urea Release Profiles

The release of urea from pure urea, KPDM, and KPDMUG as a function of time (in 5-hour intervals) was done by first weighing the amount of sample and then introducing the sample into the known volume of water contained in the dialysis bags. The system was shaken continually throughout the release trials. Measurements were taken after every 5-hour interval by simply drawing the solution from the dialysis membranes for analysis. Spectrophotometric determination of the amount of urea in water with hypochlorite and phenol technique was done thereafter. The method was adopted from [66] involving 8 steps which involves transferring a 20.0 mL aliquot of sample, which should be colorless, free from solid matter, and at room temperature to a 25 mL volumetric flask containing a microstirring magnet. Sample cavitation was barred through rapid addition because the microbubbles contribute to the blank signal; then 3.0 mL of distilled water was added and stirred vigorously followed by the addition of 0.30 mL of NaOCl reagent. After 5 seconds, 0.50 mL NaOBr was added with one hand whereas (0.30 + X) mL of HC1 reagent was added with the other hand after 2 more seconds (“X” is the volume in mL of HC1 reagent required to titrate 0.50 mL of NaOBr reagent to pH 7.0). Furthermore, after 20 seconds, 0.50 mL of H3BO3 buffer reagent was added with one hand followed with addition of 0.30 mL ethanolic phenol reagent after 2 more seconds with the other hand and stirred for 20 more seconds. After these 20 seconds, the absorbency of the sample solution at 454 nm was compared against distilled water. The blank sample procedures may be found elsewhere [66]. Calculations were then done to determine the concentration of urea by multiplying the difference between the blank and the general sample absorbencies by the difference between the general and standard sample absorbencies and divide by three twentieths the urea-N concentration of the added standard solution. The reader is recommended to view the detailed procedure and the mechanisms associated with the original author of this method [66].Besides, the rate of urea release as a function of time for a period of 150 hours was then investigated and summarized in Figure18. As can be seen, upon arduous dissolution test performed, 100% of the pure urea was released in just the first five hours of the first attempt to draw the aliquot, a result which was expected due to volatility of urea fertilizer associated with up to 60 to 70% loss in few minutes of the nitrogen being applied to the field [2] such that its utilization efficiency or plant uptake of urea is generally below 50% [1]. For the urea intercalated kaolinite nanocomposite (KPDMU) the observation made was that 100% of the intercalated urea was released within 97 hours, thereby unveiling the fact that Pugu kaolinite can retain urea and so can be used as a natural excipient for the preparation of CRF formulations. This observation indicated that urea adsorption and its subsequent intercalation into the kaolinite interlayer spaces was successful such that for its dissolution to take place an extended period of time was needed to induce its release mechanism. Furthermore, the ability of gum arabic biopolymer to retard urea dissolution was also noticed by its ability to retard urea release for a period of more than 150 hours. As can be seen, only 87% of the encapsulated urea contained into the kaolinite sheets was released after 150 hours. Such appealing results confirm our hypothesis that Pugu kaolinite layers can be expanded to accommodate molecular moieties; that is to say, it can be used to design CRF formulations based on urea fertilizer. As it was pointed out elsewhere [63] (a fact with which we also agree) that “in conventional application, the materials would be exposed to low water contents, and one can expect a better retention effect by the nanocomposites.” That is to say, the period of urea release from both urea intercalated kaolinite nanocomposite and encapsulated urea nanocomposite is expected to be more than these reported values done in the harsh laboratory settings.Figure 18
Release rate of (a) pure urea, (b) KPDMU, and (c) KPDMUG as a function of time at pH 7 and room temperature.


## 4. Conclusion

In Tanzania, nitrogenous fertilizers have been used for years by virtue of their high nitrogen content to supplement nitrogen to crop plants. However for urea despite having high nitrogen content of about 46%, it has been associated with approximately 60 to 70% loss of the nitrogen being applied because of ammonia produced through hydrolysis of urea by soil urease, a problem which could be minimized by inhibiting soil urease through encapsulation with synthetic or biopolymers as well as intercalation with nanoclays. In this paper we have described the amendments of urea fertilizer through intercalation into the kaolinite interlayer spaces and then encapsulating the intercalation compound with gum arabic biopolymer for the purpose of preparing urea control release fertilizer which in turn will minimize its volatility as well as improve its utilization efficiency (FUE) by plants and also minimize the losses, thereby reducing repeated fertilization expenditure per season and maximize crop yields. The entire experimental setup involved takes in the sampling of raw kaolinite from Pugu hills, Tanzania, beneficiation of the raw kaolinite, activation of kaolinite layers, preparation of intermediate intercalation compounds, and intercalation of urea fertilizer into the kaolinite layers by replacement reaction. Similarly, the intercalated urea fertilizer was subsequently encapsulated by using gum arabic biopolymer. The nanomaterials synthesized were characterized by using several techniques including ATR-FTIR, XRD, SEM, XRF, TGDTG, and particle size analysis via Scherrer equation along with distribution of particles through the application of Andreasen pipette sedimentation method. Our effective beneficiation process was able to minimize nonclay portion from 39.58% of the raw Pugu kaolinite to 0.36% of the beneficiated Pugu kaolinite as well as increasing the clay portion from 60.42% to 99.64% of raw and beneficiated kaolinite, respectively. The morphology of the samples was observed to change from thick compact overlapping euhedral pseudohexagonal platelets to irregular booklets which then changed to vermiform morphology and dispersed euhedral pseudohexagonal platelets coexisting with blocky-vermicular booklets. The unique brain-form agglomeration and later poor roundish particles organized in mat morphology were observed. The particle sizes of the prepared nanocomposites range from 14.55 nm to 92.46 nm whereas the indexing procedures revealed the existence of FCC Bravais lattice for the kaolinite under study. The X-ray mineralogy tests indicated the major phase in the Pugu kaolin under study after beneficiation to be kaolinite subordinated with illite. The intercalation ratios were found to be in the order of KPDM > KPDMSO > KPDMU while the TGDTG thermograms showed that the nanocomposites prepared were capable of decomposing starting from evaporations at 48°C to 600°C for the dehydroxylation of kaolinite layers. Release profiles were established in a period of 150 hours where the release rates were found to be 100% in the first 5 hours of trials, 100% in the period of 97 hours, and 87% in the period of 150 hours for pure urea, urea intercalated kaolinite nanocomposite, and the encapsulated nanocomposite, respectively.



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*Source: 237397-2015-06-11.xml*