# Assessment of the Use of Epicarp and Mesocarp of Green Coconut for Removal of Fluoride Ions in Aqueous Solution

Authors: César Augusto Canciam; Nehemias Curvelo Pereira
Journal: International Journal of Chemical Engineering
 (2019)

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## Abstract

Fruit consumption and processing result in considerable volumes of residual biomass. Transformation of this biomass into biosorbents offers an alternative for its reuse and disposal. As the green coconut shell is a waste often discarded in landfills and dumps, generating gases and leachate, two biosorbents were developed from the epicarp and mesocarp of green coconut to adsorb fluoride ions in aqueous solution. The kinetic experiments showed that sorption of fluoride ions reached equilibrium at 300 min for both epicarp and mesocarp at temperatures of 25°C, 35°C, and 45°C. The removal efficiency of fluoride ions varied from 66.25% (at 25°C) to 77.50% (at 45°C) for the epicarp and from 90% (at 25°C) to 97.50% (at 45°C) for the mesocarp. The thermodynamic parameters of the adsorption process showed that adsorption is a spontaneous, endothermic process for both biosorbents. The adsorption was classified as chemical, with the Langmuir isotherm model best suited to the adsorption isotherms data.


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## Body

## 1. Introduction

Groundwater from countries such as Algeria, Argentina, Australia, Bangladesh, China, South Korea, Egypt, Spain, United States, Ghana, India, Iran, Iraq, Israel, Italy, Japan, Jordan, Libya, Mexico, Morocco, New Zealand, Kenya, Senegal, South Africa, Sri Lanka, Tanzania, and Turkey, as well as countries in South America, is contaminated with fluoride ions. The concentration of fluoride ions can vary from 0.5 to 50 mg·L−1, depending on geological factors [1–6].Although the maximum acceptable concentration of fluoride ions in drinking water established by the World Health Organization is 1.5 mg·L−1, some countries have adopted other limits. For example, South Africa’s acceptable limit is 0.75 mg·L−1 [7].In small concentrations, fluoride ions help to prevent dental caries and improve calcification of dental enamel. At high concentrations, however, they can interfere with the functioning of the kidneys, thyroid, parathyroid, liver, testes, and neurons [7–10].In adults, concentrations of fluoride ions greater than 1.5 mg·L−1 can lead to dental fluorosis, while concentrations above 3 mg·L−1 can cause skeletal fluorosis. It is estimated that 26 million people in China suffer from dental fluorosis and 1 million from skeletal fluorosis, due to the consumption of water contaminated with high levels of fluoride ions [11–14].Dental fluorosis is a major public health problem because in moderate or severe forms, it causes functional and aesthetic alterations that interfere with personality formation and integration into the labour market, requiring highly complex dental treatment. In general, the clinical aspect of dental fluorosis ranges from opaque spots on the enamel to yellowish or brown areas in the case of more severe changes [15].Skeletal fluorosis is a serious condition, resulting from chronic ingestion of large amounts of fluoride over many years during periods of bone modelling (growth) and/or remodelling. Skeletal fluorosis manifests as an increase in bone density leading to thickening of the long bones and calcification of the ligaments. Symptoms include mild rheumatic pains, arthritis of the joints and muscles, and pain along the cervical spine. Skeletal fluorosis causes bending of the legs outwards from the knees, and in more advanced cases, the person is unable to move around and remains bedridden [9, 13].The various processes for the removal of fluoride ions from water include coagulation and chemical precipitation, membrane processes (dialysis, nanofiltration, and reverse osmosis), electrolytic treatment (electrodialysis and electrocoagulation), and ion exchange and adsorption. The adsorption process used in the removal of fluoride ions offers greater accessibility, low cost, and simple design and operation. Disadvantages are that this process requires pH adjustment, while the presence of other dissolved ions may interfere with the adsorption of fluoride ions [7, 16].Although the green coconut shell is a residue of coconut water use and industrialisation with great potential for reuse, few attempts have been made to exploit it, with most shells deposited in dumps and landfills, causing an environmental problem. The green coconut shell is not easily degradable (taking about 8 years), occupies a lot of space in the landfills, and causes the proliferation of diseases [17, 18].Coconut fruit (Cocos nucifera L.) consists of epicarp, mesocarp, endocarp, embryo, copra, and coconut water. The epicarp is the outer layer with a smooth surface, coated with wax. The mesocarp is the middle layer, the more developed and voluminous part of the fruit. Epicarp, mesocarp, and endocarp make up 80–85% of the mass of the immature fruit [17, 19].As a biosorbent, the green coconut shell has been studied mainly in the removal of cations, with few studies devoted to the removal of anions using this type of biosorbent [20]. The objective of this study was thus to characterise the biosorbents (the analysis of the textural properties and the identification of the functional groups that participate in the adsorption process by means of Fourier transform infrared spectroscopy) and investigate the kinetics, equilibrium, and thermodynamics in the adsorption of fluoride ions using the epicarp and mesocarp of green coconut in a batch process.


## 2. Materials and Methods

### 2.1. Materials

The green coconut samples used in this study came from the disposal of material after the consumption of coconut water and were provided by a company located in Maringá, Paraná, Brazil.The green coconut was peeled manually with a special knife, giving slices of epicarp approximately 3 mm thick and mesocarp approximately 5 mm thick, which were then dried separately at 70°C in a convective upflow air drier. The drying times at equilibrium were determined at 141 min and 140 min, respectively, for the epicarp and the mesocarp. After drying, the materials were crushed separately and sorted by size, using laboratory sieves. The fractions of adsorbents used in the study had an average diameter of 0.75 mm.


### 2.2. Characterisation of the Biosorbents

In order to characterise the biosorbents, analysis of the textural properties (specific surface area, specific volume, and average radius of the pores) and identification of the functional groups that participate in the adsorption process by means of the Fourier transform infrared spectroscopy (FTIR) were carried out.Analysis of textural properties was carried out using NOVA 1000 series Quantachrome and data analysis with NovaWin version 10.01. The method used was nitrogen adsorption and desorption method at 77 K, using dry epicarp and mesocarp at 70°C, with particles with a mean diameter of 0.75 mm.The functional groups that participate in the adsorption process were determined by means of the infrared spectrophotometer with Fourier transform (Frontier-PerkinElmer), in the infrared range between 400 and 4,000 cm−1. In the FTIR, the spectra of the samples before and after adsorption of the fluoride ions were determined.


### 2.3. Adsorption Kinetics

The experiments were carried out in batch, using a cooled incubator with shaking (Tecnal, model TE-421). In the experiments, 0.50 g of each biosorbent was used in a series of flasks containing 30 mL of an aqueous solution of sodium fluoride, with an initial concentration of fluoride ions 4 mg·L−1. The flasks were shaken mechanically at 150 rpm, at predetermined times (5, 10, 15, 20, 30, 45, 60, 120, 180, 210, 240, 270, 300, 330, 360, 390, and 420 minutes) and maintained at 25, 35, and 45°C. The pH of the solution was 8.0.The SPADNS colorimetric method was employed for the determination of the concentration of fluoride ions [21].The percentage of fluoride ions removed from the aqueous solution was calculated by the following equation:(1)R%=C0−CeC0⋅100,where C0 and Ce represent initial and equilibrium concentrations (mg·L−1), respectively, and R% is the fluoride ion removal efficiency (%).The adsorption capacity as a function of time can be expressed as follows [22]:(2)qt=C0−Ct⋅Vm,where qt is the adsorption capacity as a function of time (mg·g−1), V is the volume of the treated solution (L), m is the mass of adsorbent (g), and Ct is the final time fluoride concentration in the solution (mg·L−1).The experimental adsorption kinetic data were modelled by pseudo-first-order and pseudo-second-order kinetics models, the Elovich model, and the intraparticle diffusion model, which are represented in their nonlinear forms by the following equations [23–25].Pseudo-first-order model:(3)qt=qe⋅1−e−k1⋅t.Pseudo-second-order model:(4)qt=k2⋅qe2⋅t1+qe⋅k2⋅t.Elovich model:(5)qt=1β⋅lnα⋅β⋅t.Intraparticle diffusion model:(6)qt=kdif⋅t+Cd,where qe is the quantity of fluoride ions adsorbed at equilibrium by mass of biosorbents (mg·g−1); t is the time (min); k1 and k2 are, respectively, the pseudo-first-order rate constant (min−1) and pseudo-second-order rate constant (g·mg−1·min−1); α is the initial adsorption velocity in the Elovich model (mg·g−1·min−1); β is a parameter of the Elovich model (g·mg−1); kdif is the intraparticle diffusion rate constant (mg·g−1·min−0.5); and Cd is the constant in the intraparticle diffusion model (mg·g−1).


### 2.4. Adsorption Isotherms

In the in-batch experiments, 0.50 g of each biosorbent was used in a series of flasks containing 30 mL of aqueous solutions of sodium fluoride, with initial concentrations of fluoride ions of 4, 5, 8, 10, 12, and 14 mg·L−1. The flasks were shaken mechanically at 150 rpm for 24 hours and maintained at 25, 35, and 45°C. The pH of the solutions was 8.0.The Langmuir and Freundlich isotherm models were suited to the experimental data. Nonlinear regression analysis was performed using OringinPro8 software.The nonlinear forms of the Langmuir and Freundlich isotherm models can be expressed as follows [26, 27].Langmuir isotherm model:(7)qe=qmax⋅kL⋅Ce1+kL⋅Ce.Freundlich isotherm model:(8)qe=kF⋅Ce1/n,where qe is the concentration of fluoride ions after reaching equilibrium (mg·L−1); Ce is quantity of fluoride ions retained in the adsorbent at equilibrium by mass of adsorbent (mg·g−1); qmax is the maximum adsorption capacity (mg·g−1); kL and kF are, respectively, the Langmuir constant (L·mg−1) and the Freundlich constant (mgn−1/n⋅L1/n); and n is Freundlich’s exponent (dimensionless).


### 2.5. Selection of Models

All experiments were carried out in duplicates, and the reported values were averages.In the selection of models, Akaike’s criterion for small samples (AICc) was applied. The best-fit model for the experimental data corresponds to the model that had the smallest value of Akaike’s criterion for small samples [28]. This criterion is given by the following equation:(9)AICc=ne⋅lnSQEne+2⋅np+2⋅np⋅np+1ne−np−1,where SQE is the sum of squares of errors and ne and np are the number of experimental observations and of model parameters, respectively.


## 2.1. Materials

The green coconut samples used in this study came from the disposal of material after the consumption of coconut water and were provided by a company located in Maringá, Paraná, Brazil.The green coconut was peeled manually with a special knife, giving slices of epicarp approximately 3 mm thick and mesocarp approximately 5 mm thick, which were then dried separately at 70°C in a convective upflow air drier. The drying times at equilibrium were determined at 141 min and 140 min, respectively, for the epicarp and the mesocarp. After drying, the materials were crushed separately and sorted by size, using laboratory sieves. The fractions of adsorbents used in the study had an average diameter of 0.75 mm.


## 2.2. Characterisation of the Biosorbents

In order to characterise the biosorbents, analysis of the textural properties (specific surface area, specific volume, and average radius of the pores) and identification of the functional groups that participate in the adsorption process by means of the Fourier transform infrared spectroscopy (FTIR) were carried out.Analysis of textural properties was carried out using NOVA 1000 series Quantachrome and data analysis with NovaWin version 10.01. The method used was nitrogen adsorption and desorption method at 77 K, using dry epicarp and mesocarp at 70°C, with particles with a mean diameter of 0.75 mm.The functional groups that participate in the adsorption process were determined by means of the infrared spectrophotometer with Fourier transform (Frontier-PerkinElmer), in the infrared range between 400 and 4,000 cm−1. In the FTIR, the spectra of the samples before and after adsorption of the fluoride ions were determined.


## 2.3. Adsorption Kinetics

The experiments were carried out in batch, using a cooled incubator with shaking (Tecnal, model TE-421). In the experiments, 0.50 g of each biosorbent was used in a series of flasks containing 30 mL of an aqueous solution of sodium fluoride, with an initial concentration of fluoride ions 4 mg·L−1. The flasks were shaken mechanically at 150 rpm, at predetermined times (5, 10, 15, 20, 30, 45, 60, 120, 180, 210, 240, 270, 300, 330, 360, 390, and 420 minutes) and maintained at 25, 35, and 45°C. The pH of the solution was 8.0.The SPADNS colorimetric method was employed for the determination of the concentration of fluoride ions [21].The percentage of fluoride ions removed from the aqueous solution was calculated by the following equation:(1)R%=C0−CeC0⋅100,where C0 and Ce represent initial and equilibrium concentrations (mg·L−1), respectively, and R% is the fluoride ion removal efficiency (%).The adsorption capacity as a function of time can be expressed as follows [22]:(2)qt=C0−Ct⋅Vm,where qt is the adsorption capacity as a function of time (mg·g−1), V is the volume of the treated solution (L), m is the mass of adsorbent (g), and Ct is the final time fluoride concentration in the solution (mg·L−1).The experimental adsorption kinetic data were modelled by pseudo-first-order and pseudo-second-order kinetics models, the Elovich model, and the intraparticle diffusion model, which are represented in their nonlinear forms by the following equations [23–25].Pseudo-first-order model:(3)qt=qe⋅1−e−k1⋅t.Pseudo-second-order model:(4)qt=k2⋅qe2⋅t1+qe⋅k2⋅t.Elovich model:(5)qt=1β⋅lnα⋅β⋅t.Intraparticle diffusion model:(6)qt=kdif⋅t+Cd,where qe is the quantity of fluoride ions adsorbed at equilibrium by mass of biosorbents (mg·g−1); t is the time (min); k1 and k2 are, respectively, the pseudo-first-order rate constant (min−1) and pseudo-second-order rate constant (g·mg−1·min−1); α is the initial adsorption velocity in the Elovich model (mg·g−1·min−1); β is a parameter of the Elovich model (g·mg−1); kdif is the intraparticle diffusion rate constant (mg·g−1·min−0.5); and Cd is the constant in the intraparticle diffusion model (mg·g−1).


## 2.4. Adsorption Isotherms

In the in-batch experiments, 0.50 g of each biosorbent was used in a series of flasks containing 30 mL of aqueous solutions of sodium fluoride, with initial concentrations of fluoride ions of 4, 5, 8, 10, 12, and 14 mg·L−1. The flasks were shaken mechanically at 150 rpm for 24 hours and maintained at 25, 35, and 45°C. The pH of the solutions was 8.0.The Langmuir and Freundlich isotherm models were suited to the experimental data. Nonlinear regression analysis was performed using OringinPro8 software.The nonlinear forms of the Langmuir and Freundlich isotherm models can be expressed as follows [26, 27].Langmuir isotherm model:(7)qe=qmax⋅kL⋅Ce1+kL⋅Ce.Freundlich isotherm model:(8)qe=kF⋅Ce1/n,where qe is the concentration of fluoride ions after reaching equilibrium (mg·L−1); Ce is quantity of fluoride ions retained in the adsorbent at equilibrium by mass of adsorbent (mg·g−1); qmax is the maximum adsorption capacity (mg·g−1); kL and kF are, respectively, the Langmuir constant (L·mg−1) and the Freundlich constant (mgn−1/n⋅L1/n); and n is Freundlich’s exponent (dimensionless).


## 2.5. Selection of Models

All experiments were carried out in duplicates, and the reported values were averages.In the selection of models, Akaike’s criterion for small samples (AICc) was applied. The best-fit model for the experimental data corresponds to the model that had the smallest value of Akaike’s criterion for small samples [28]. This criterion is given by the following equation:(9)AICc=ne⋅lnSQEne+2⋅np+2⋅np⋅np+1ne−np−1,where SQE is the sum of squares of errors and ne and np are the number of experimental observations and of model parameters, respectively.


## 3. Results and Discussion

### 3.1. Characterisation of the Biosorbents

Table1 lists the specific surface area, the specific volume of mesopores, the specific volume of micropores, the mean radius of the mesopores, and the mean radius of the micropores of the dried epicarp and mesocarp of green coconut at 70°C.Table 1
Textural properties of dried epicarp and mesocarp of green coconut.
Epicarp
Mesocarp
Specific surface area (m2·g−1)
3.360
5.766
Specific volume of mesopores (cm3·g−1)
4.08 × 10−3
3.04 × 10−3
Specific volume of micropores (cm3·g−1)
8.42 × 10−4
1.47 × 10−3
Mean radius of the mesopores (nm)
1.520
1.521
Mean radius of the micropores (nm)
0.226
0.152The drying causes damage to the cellular structure of the materials, leading to a change in shape and decrease in size [29]. Crushing leads to a decrease in particle size and an increase in the specific surface area [30]. Thus, before adsorption, the biosorbents were damaged by the drying process and showed an increased specific surface area due to crushing. In Table 1, it can be seen that the mesocarp had a greater specific surface area in relation to the epicarp.The infrared vibrational spectra of the epicarp of green coconut (before and after the adsorption of fluoride ions) are shown in Figure1, which shows absorption bands of 1,059, 1,520, 1,615, and 2,921 cm−1.Figure 1
FTIR vibrational spectra of epicarp of green coconut (before and after adsorption).The absorption band at 1,059 cm−1 was attributed to the stretching of the high-intensity C-O group, which can be found in alcohols, ethers, esters, carboxylic acids, and anhydrides. The absorption band at 1,520 cm−1 was attributed to the C-H group, which can be found in alkenes and is a characteristic of off-plan folding. The absorption band at 1,615 cm−1 was attributed to the stretching of the C=C group, while the absorption band at 2,921 cm−1 was attributed to the stretching of the high-intensity C-H group, found in alkanes [31].The infrared vibrational spectra of the mesocarp of green coconut (before and after the adsorption of fluoride ions) are shown in Figure2.Figure 2
FTIR vibrational spectra of mesocarp of green coconut (before and after adsorption).The absorption bands at 1,520 cm−1 and 1,615 cm−1 were attributed to off-plane folding of the C-H group and to the stretching of the C=C group, respectively. The absorption band in 2,930 cm−1 was attributed to the stretching of the high-intensity C-H group, while the absorption band at 3,353 cm−1 was attributed to the C=C group of the aromatic ring [31].The C=C group is found in lignin and chlorophyll. The C-O group is found in cellulose, hemicelluloses, pectin, lignin, tannins, and chlorophyll. The C-H group is found in cellulose, lignin, tannins, and chlorophyll. The C=C group of the aromatic ring is found in lignin and tannins [32, 33].Basically, the epicarp and mesocarp of green coconut consist of cellulose, lignin and hemicelluloses, while tannins are also found [34, 35].The tannins are considered to be chemically highly reactive, able to form intra- and intermolecular hydrogen bonds [36].


### 3.2. Adsorption Kinetics

The adsorption kinetics reveal the influence of the contact time between species to be adsorbed and the adsorbent and the amount of species adsorbed [37].For the epicarp of green coconut, the adsorption of fluoride ions reached equilibrium in 300 minutes, with final concentrations equivalent to 1.35 mg·L−1 (at 25°C), 1.10 mg·L−1 (at 35°C), and 0.90 mg·L−1 (at 45°C). The concentration of fluoride ions as a function of time employing epicarp as biosorbent can be seen in Figure 3.Figure 3
Concentration of fluoride ions as a function of time using epicarp as biosorbents.For the mesocarp of green coconut, the adsorption of fluoride ions reached equilibrium in 300 minutes, with final concentrations equivalent to 0.40 mg·L−1 (at 25°C), 0.20 mg·L−1 (at 35°C), and 0.10 mg·L−1 (at 45°C). Figure 4 shows the concentration of fluoride ions as a function of time using mesocarp as biosorbents.Figure 4
Concentration of fluoride ions as a function of time using mesocarp as biosorbents.As for removal efficiency of fluoride ions, the epicarp showed 66.25% (at 25°C), 72.50% (at 35°C), and 77.50% (at 45°C). For mesocarp, removal efficiency was 90% (at 25°C), 95% (at 35°C), and 97.50% (at 45°C).The higher removal efficiency of fluoride ions by the mesocarp may be associated with its greater specific surface area compared to the epicarp.The kinetic parameters for adsorption of fluoride ions by epicarp and mesocarp of green coconut are summarised in Table2.Table 2
Kinetics parameters for adsorption of fluoride ions by epicarp and mesocarp of green coconut.
Model
Epicarp
Mesocarp
Pseudo-first-order
25°C
35°C
45°C
25°C
35°C
45°C
qe (mg·g−1)
0.1629
0.1742
0.1857
0.2358
0.2273
0.2323
k1 (min−1)
0.0107
0.0145
0.0194
0.0072
0.0111
0.0125
R2
0.9920
0.9850
0.9515
0.9952
0.9840
0.9821
AICc
−174.2137
−164.7537
−145.9986
−171.3698
−153.7335
−151.5198
Pseudo-second-order
qe (mg·g−1)
0.2070
0.2082
0.2120
0.3212
0.2309
0.2801
k2 (g·mg−1·min−1)
0.0490
0.0758
0.1120
0.0187
0.0408
0.0512
R2
0.9876
0.9891
0.9761
0.9927
0.9927
0.9920
AICc
−166.7448
−170.2651
−158.0703
−164.2642
−167.0878
−165.1528
Elovich model
α (mg·g−1·min−1)
0.0054
0.0091
0.0149
0.0061
0.0092
0.0109
β (g·mg−1)
23.8895
24.8819
25.6593
17.1782
18.4377
18.2533
R2
0.9733
0.9650
0.9725
0.9591
0.9767
0.9800
AICc
−153.7335
−150.3733
−155.6375
−135.0571
−147.3355
−149.5615
Intraparticle diffusion model
kdif (mg·g−1·min−0.5)
0.0092
0.0089
0.0086
0.0131
0.0121
0.0121
Cd (mg·g−1)
−0.0043
0.0177
0.0379
−0.0222
0.0073
0.0172
R2
0.9396
0.9394
0.9419
0.9750
0.9697
0.9550
AICc
−139.8852
−140.0723
−142.9349
−143.4189
−142.8754
−135.8247R
2 corresponds to the coefficient of determination (dimensionless).Table2 shows that, using Akaike’s criterion for small samples, the pseudo-first-order model is the best fit for the experimental data at 25°C, while the pseudo-second-order model is the best fit for the experimental data at 35 and 45°C.


### 3.3. Adsorption Isotherms

The Langmuir isotherm model suggests that adsorption occurs at homogeneous sites in the adsorbent, where all sites are identical and energetically equivalent and there is no interaction between the adsorbed species at the neighboring sites [38].The Freundlich isotherm model describes equilibrium on heterogeneous surfaces and does not therefore assume a monolayer adsorption capacity. This model suggests that the amount of the species retained in the adsorbent increases as the species concentration in the solution increases [27].The Langmuir and Freundlich constants for adsorption of fluoride ions by epicarp and mesocarp of green coconut are shown in Table3. It can be seen that the fluoride ions adsorption isotherm data fit well with the Langmuir isotherm model, with the smallest value of Akaike’s criterion for small samples.Table 3
The Langmuir and Freundlich models constants.
Model
Epicarp
Mesocarp
Langmuir model
25°C
35°C
45°C
25°C
35°C
45°C
qmax (mg·g−1)
1.6909
2.2265
1.8176
1.8021
1.7802
3.2253
kL (L·mg−1)
1.1338
1.0448
1.8537
2.0968
1.1465
1.1874
R2
0.9689
0.9904
0.9648
0.9652
0.9594
0.9863
AICc
−43.0679
−49.5204
−37.8549
−37.5464
−35.8396
−42.9539
Freundlich model
kF (mgn−1/n⋅L1/n)
0.1439
0.1978
0.6290
0.5687
0.8536
1.7757
n
1.2490
1.2053
1.4515
1.3822
1.4230
1.1868
R2
0.9595
0.9856
0.9521
0.9544
0.9468
0.9816
AICc
−41.2255
−46.6851
−35.7090
−35.6467
−33.9463
−40.8807Table4 shows the maximum adsorption capacity of some adsorbents for the removal of fluoride ions. It can be observed that the adsorbents studied in this work present a higher maximum adsorption capacity.Table 4
Maximum adsorption capacity of some adsorbents for fluoride ions removal.
Adsorbent
q
max (mg·g−1)
Reference
Mixed rare earth oxides of activated alumina
0.7400
[39]
Modified amberlite resin
0.0610
[40]
Granular acid-treated bentonite
0.2780
[41]
Natural chitosan
1.3900
[42]
Epicarp of green coconut
2.2265 (35°C)
This work
Mesocarp of green coconut
3.2253 (45°C)
This work


### 3.4. Thermodynamic Analyses

The thermodynamic parameters of adsorption were calculated from the equilibrium constantkd, determined by the graph of the Neperian logarithm of the ratio qe/Ce as a function of qe, extrapolating Ce to zero [43].The thermodynamic parameters were calculated using the following equations [43]:(10)ΔG=−R⋅T⋅lnkd,lnkd=ΔSR−ΔHR⋅1T,where ΔS is the entropy variation (kJ·mol−1·K−1), ΔH is the enthalpy variation (kJ·mol−1), ΔG is the Gibbs free energy variation (kJ·mol−1), R is the gas constant (kJ·mol−1·K−1), and T is the temperature (K).Plottinglnkd against 1/T gives a straight line with slope and intercept equal to −ΔH/R and ΔS/R, respectively, as shown in Figure 5.Figure 5
The plot oflnkd vs. 1/T.The values of Gibbs free energy variation, entropy variation, and enthalpy variation are shown in Table5.Table 5
Thermodynamic parameters for adsorption of fluoride ions on epicarp and mesocarp of green coconut.
T (°C)
Epicarp
Mesocarp
Δ
G (kJ·mol−1)
Δ
H (kJ·mol−1)
Δ
S (kJ·mol−1·K−1)
Δ
G (kJ·mol−1)
Δ
H (kJ·mol−1)
Δ
S (kJ·mol−1·K−1)
8.4046
0.0327
13.8486
0.0489
25
−1.4123
−0.7802
35
−1.4820
−1.0979
45
−2.0766
−1.7654Negative values for the Gibbs free energy variation indicate that the adsorptive process was spontaneous; that is, it was thermodynamically favourable. Positive values for the enthalpy variation indicate that the adsorption process was endothermic. In adsorption, endothermic processes can be associated with the energy barrier necessary for the formation of the activated adsorbent-adsorbate complex; it was necessary to provide energy to overcome the energy barrier. Positive values for the entropy variation indicate that there has been an increase in the system disorder at the solid-fluid interface during adsorption [22].The effect of temperature on the adsorption of fluoride ions was studied by means of the Arrhenius equation in the linearised form [44]:(11)lnkcin=lnA−EaR⋅1T,where kcin is the constant of the best-fit kinetic model (unit according to the model), A is the frequency factor (unit associated with the best-fit kinetic model), and Ea is the activation energy (kJ·mol−1).The parameters of the Arrhenius equation are shown in Table6.Table 6
Parameters of the Arrhenius equation for adsorption of fluoride ions on epicarp and mesocarp of green coconut.
T (°C)
ln
k
cin
A (g·mg−1·min−1)
E
a (kJ·mol−1)
R
2
Epicarp
3.1106 × 1014
93.3827
0.8828
25
−4.5413
35
−2.5797
45
−2.1893
Mesocarp
4.1560 × 1011
77.9670
0.8492
25
−4.9337
35
−3.1991
45
−2.9720The activation energy is a parameter associated with the nature and intensity of the interactions between the adsorbent and the adsorbate. This energy depends on the chemical nature of the species involved and is generally employed to distinguish types of adsorption. For adsorption energy values between 5 and 40 kJ·mol−1, the adsorption is classified as physical, while for values between 40 and 800 kJ·mol−1, it is classified as chemical [44]. It can thus be observed in Table 6 that the adsorption of the fluoride ions by the epicarp and mesocarp of green coconut is classified as chemical.No adsorption studies on fluoride ions using the epicarp and mesocarp of green coconut could be found in the literature.Many water sources are abandoned because of excess fluoride ions and the cost of treatment [16]. The results showed the relevant amount of fluoride ions adsorbed by the epicarp and mesocarp of green coconut in relation to other adsorbents already studied. The use of these materials as an adsorbent thus offers a promising alternative for reuse and disposal, reducing the environmental impact in industrial landfills and landfills.


## 3.1. Characterisation of the Biosorbents

Table1 lists the specific surface area, the specific volume of mesopores, the specific volume of micropores, the mean radius of the mesopores, and the mean radius of the micropores of the dried epicarp and mesocarp of green coconut at 70°C.Table 1
Textural properties of dried epicarp and mesocarp of green coconut.
Epicarp
Mesocarp
Specific surface area (m2·g−1)
3.360
5.766
Specific volume of mesopores (cm3·g−1)
4.08 × 10−3
3.04 × 10−3
Specific volume of micropores (cm3·g−1)
8.42 × 10−4
1.47 × 10−3
Mean radius of the mesopores (nm)
1.520
1.521
Mean radius of the micropores (nm)
0.226
0.152The drying causes damage to the cellular structure of the materials, leading to a change in shape and decrease in size [29]. Crushing leads to a decrease in particle size and an increase in the specific surface area [30]. Thus, before adsorption, the biosorbents were damaged by the drying process and showed an increased specific surface area due to crushing. In Table 1, it can be seen that the mesocarp had a greater specific surface area in relation to the epicarp.The infrared vibrational spectra of the epicarp of green coconut (before and after the adsorption of fluoride ions) are shown in Figure1, which shows absorption bands of 1,059, 1,520, 1,615, and 2,921 cm−1.Figure 1
FTIR vibrational spectra of epicarp of green coconut (before and after adsorption).The absorption band at 1,059 cm−1 was attributed to the stretching of the high-intensity C-O group, which can be found in alcohols, ethers, esters, carboxylic acids, and anhydrides. The absorption band at 1,520 cm−1 was attributed to the C-H group, which can be found in alkenes and is a characteristic of off-plan folding. The absorption band at 1,615 cm−1 was attributed to the stretching of the C=C group, while the absorption band at 2,921 cm−1 was attributed to the stretching of the high-intensity C-H group, found in alkanes [31].The infrared vibrational spectra of the mesocarp of green coconut (before and after the adsorption of fluoride ions) are shown in Figure2.Figure 2
FTIR vibrational spectra of mesocarp of green coconut (before and after adsorption).The absorption bands at 1,520 cm−1 and 1,615 cm−1 were attributed to off-plane folding of the C-H group and to the stretching of the C=C group, respectively. The absorption band in 2,930 cm−1 was attributed to the stretching of the high-intensity C-H group, while the absorption band at 3,353 cm−1 was attributed to the C=C group of the aromatic ring [31].The C=C group is found in lignin and chlorophyll. The C-O group is found in cellulose, hemicelluloses, pectin, lignin, tannins, and chlorophyll. The C-H group is found in cellulose, lignin, tannins, and chlorophyll. The C=C group of the aromatic ring is found in lignin and tannins [32, 33].Basically, the epicarp and mesocarp of green coconut consist of cellulose, lignin and hemicelluloses, while tannins are also found [34, 35].The tannins are considered to be chemically highly reactive, able to form intra- and intermolecular hydrogen bonds [36].


## 3.2. Adsorption Kinetics

The adsorption kinetics reveal the influence of the contact time between species to be adsorbed and the adsorbent and the amount of species adsorbed [37].For the epicarp of green coconut, the adsorption of fluoride ions reached equilibrium in 300 minutes, with final concentrations equivalent to 1.35 mg·L−1 (at 25°C), 1.10 mg·L−1 (at 35°C), and 0.90 mg·L−1 (at 45°C). The concentration of fluoride ions as a function of time employing epicarp as biosorbent can be seen in Figure 3.Figure 3
Concentration of fluoride ions as a function of time using epicarp as biosorbents.For the mesocarp of green coconut, the adsorption of fluoride ions reached equilibrium in 300 minutes, with final concentrations equivalent to 0.40 mg·L−1 (at 25°C), 0.20 mg·L−1 (at 35°C), and 0.10 mg·L−1 (at 45°C). Figure 4 shows the concentration of fluoride ions as a function of time using mesocarp as biosorbents.Figure 4
Concentration of fluoride ions as a function of time using mesocarp as biosorbents.As for removal efficiency of fluoride ions, the epicarp showed 66.25% (at 25°C), 72.50% (at 35°C), and 77.50% (at 45°C). For mesocarp, removal efficiency was 90% (at 25°C), 95% (at 35°C), and 97.50% (at 45°C).The higher removal efficiency of fluoride ions by the mesocarp may be associated with its greater specific surface area compared to the epicarp.The kinetic parameters for adsorption of fluoride ions by epicarp and mesocarp of green coconut are summarised in Table2.Table 2
Kinetics parameters for adsorption of fluoride ions by epicarp and mesocarp of green coconut.
Model
Epicarp
Mesocarp
Pseudo-first-order
25°C
35°C
45°C
25°C
35°C
45°C
qe (mg·g−1)
0.1629
0.1742
0.1857
0.2358
0.2273
0.2323
k1 (min−1)
0.0107
0.0145
0.0194
0.0072
0.0111
0.0125
R2
0.9920
0.9850
0.9515
0.9952
0.9840
0.9821
AICc
−174.2137
−164.7537
−145.9986
−171.3698
−153.7335
−151.5198
Pseudo-second-order
qe (mg·g−1)
0.2070
0.2082
0.2120
0.3212
0.2309
0.2801
k2 (g·mg−1·min−1)
0.0490
0.0758
0.1120
0.0187
0.0408
0.0512
R2
0.9876
0.9891
0.9761
0.9927
0.9927
0.9920
AICc
−166.7448
−170.2651
−158.0703
−164.2642
−167.0878
−165.1528
Elovich model
α (mg·g−1·min−1)
0.0054
0.0091
0.0149
0.0061
0.0092
0.0109
β (g·mg−1)
23.8895
24.8819
25.6593
17.1782
18.4377
18.2533
R2
0.9733
0.9650
0.9725
0.9591
0.9767
0.9800
AICc
−153.7335
−150.3733
−155.6375
−135.0571
−147.3355
−149.5615
Intraparticle diffusion model
kdif (mg·g−1·min−0.5)
0.0092
0.0089
0.0086
0.0131
0.0121
0.0121
Cd (mg·g−1)
−0.0043
0.0177
0.0379
−0.0222
0.0073
0.0172
R2
0.9396
0.9394
0.9419
0.9750
0.9697
0.9550
AICc
−139.8852
−140.0723
−142.9349
−143.4189
−142.8754
−135.8247R
2 corresponds to the coefficient of determination (dimensionless).Table2 shows that, using Akaike’s criterion for small samples, the pseudo-first-order model is the best fit for the experimental data at 25°C, while the pseudo-second-order model is the best fit for the experimental data at 35 and 45°C.


## 3.3. Adsorption Isotherms

The Langmuir isotherm model suggests that adsorption occurs at homogeneous sites in the adsorbent, where all sites are identical and energetically equivalent and there is no interaction between the adsorbed species at the neighboring sites [38].The Freundlich isotherm model describes equilibrium on heterogeneous surfaces and does not therefore assume a monolayer adsorption capacity. This model suggests that the amount of the species retained in the adsorbent increases as the species concentration in the solution increases [27].The Langmuir and Freundlich constants for adsorption of fluoride ions by epicarp and mesocarp of green coconut are shown in Table3. It can be seen that the fluoride ions adsorption isotherm data fit well with the Langmuir isotherm model, with the smallest value of Akaike’s criterion for small samples.Table 3
The Langmuir and Freundlich models constants.
Model
Epicarp
Mesocarp
Langmuir model
25°C
35°C
45°C
25°C
35°C
45°C
qmax (mg·g−1)
1.6909
2.2265
1.8176
1.8021
1.7802
3.2253
kL (L·mg−1)
1.1338
1.0448
1.8537
2.0968
1.1465
1.1874
R2
0.9689
0.9904
0.9648
0.9652
0.9594
0.9863
AICc
−43.0679
−49.5204
−37.8549
−37.5464
−35.8396
−42.9539
Freundlich model
kF (mgn−1/n⋅L1/n)
0.1439
0.1978
0.6290
0.5687
0.8536
1.7757
n
1.2490
1.2053
1.4515
1.3822
1.4230
1.1868
R2
0.9595
0.9856
0.9521
0.9544
0.9468
0.9816
AICc
−41.2255
−46.6851
−35.7090
−35.6467
−33.9463
−40.8807Table4 shows the maximum adsorption capacity of some adsorbents for the removal of fluoride ions. It can be observed that the adsorbents studied in this work present a higher maximum adsorption capacity.Table 4
Maximum adsorption capacity of some adsorbents for fluoride ions removal.
Adsorbent
q
max (mg·g−1)
Reference
Mixed rare earth oxides of activated alumina
0.7400
[39]
Modified amberlite resin
0.0610
[40]
Granular acid-treated bentonite
0.2780
[41]
Natural chitosan
1.3900
[42]
Epicarp of green coconut
2.2265 (35°C)
This work
Mesocarp of green coconut
3.2253 (45°C)
This work


## 3.4. Thermodynamic Analyses

The thermodynamic parameters of adsorption were calculated from the equilibrium constantkd, determined by the graph of the Neperian logarithm of the ratio qe/Ce as a function of qe, extrapolating Ce to zero [43].The thermodynamic parameters were calculated using the following equations [43]:(10)ΔG=−R⋅T⋅lnkd,lnkd=ΔSR−ΔHR⋅1T,where ΔS is the entropy variation (kJ·mol−1·K−1), ΔH is the enthalpy variation (kJ·mol−1), ΔG is the Gibbs free energy variation (kJ·mol−1), R is the gas constant (kJ·mol−1·K−1), and T is the temperature (K).Plottinglnkd against 1/T gives a straight line with slope and intercept equal to −ΔH/R and ΔS/R, respectively, as shown in Figure 5.Figure 5
The plot oflnkd vs. 1/T.The values of Gibbs free energy variation, entropy variation, and enthalpy variation are shown in Table5.Table 5
Thermodynamic parameters for adsorption of fluoride ions on epicarp and mesocarp of green coconut.
T (°C)
Epicarp
Mesocarp
Δ
G (kJ·mol−1)
Δ
H (kJ·mol−1)
Δ
S (kJ·mol−1·K−1)
Δ
G (kJ·mol−1)
Δ
H (kJ·mol−1)
Δ
S (kJ·mol−1·K−1)
8.4046
0.0327
13.8486
0.0489
25
−1.4123
−0.7802
35
−1.4820
−1.0979
45
−2.0766
−1.7654Negative values for the Gibbs free energy variation indicate that the adsorptive process was spontaneous; that is, it was thermodynamically favourable. Positive values for the enthalpy variation indicate that the adsorption process was endothermic. In adsorption, endothermic processes can be associated with the energy barrier necessary for the formation of the activated adsorbent-adsorbate complex; it was necessary to provide energy to overcome the energy barrier. Positive values for the entropy variation indicate that there has been an increase in the system disorder at the solid-fluid interface during adsorption [22].The effect of temperature on the adsorption of fluoride ions was studied by means of the Arrhenius equation in the linearised form [44]:(11)lnkcin=lnA−EaR⋅1T,where kcin is the constant of the best-fit kinetic model (unit according to the model), A is the frequency factor (unit associated with the best-fit kinetic model), and Ea is the activation energy (kJ·mol−1).The parameters of the Arrhenius equation are shown in Table6.Table 6
Parameters of the Arrhenius equation for adsorption of fluoride ions on epicarp and mesocarp of green coconut.
T (°C)
ln
k
cin
A (g·mg−1·min−1)
E
a (kJ·mol−1)
R
2
Epicarp
3.1106 × 1014
93.3827
0.8828
25
−4.5413
35
−2.5797
45
−2.1893
Mesocarp
4.1560 × 1011
77.9670
0.8492
25
−4.9337
35
−3.1991
45
−2.9720The activation energy is a parameter associated with the nature and intensity of the interactions between the adsorbent and the adsorbate. This energy depends on the chemical nature of the species involved and is generally employed to distinguish types of adsorption. For adsorption energy values between 5 and 40 kJ·mol−1, the adsorption is classified as physical, while for values between 40 and 800 kJ·mol−1, it is classified as chemical [44]. It can thus be observed in Table 6 that the adsorption of the fluoride ions by the epicarp and mesocarp of green coconut is classified as chemical.No adsorption studies on fluoride ions using the epicarp and mesocarp of green coconut could be found in the literature.Many water sources are abandoned because of excess fluoride ions and the cost of treatment [16]. The results showed the relevant amount of fluoride ions adsorbed by the epicarp and mesocarp of green coconut in relation to other adsorbents already studied. The use of these materials as an adsorbent thus offers a promising alternative for reuse and disposal, reducing the environmental impact in industrial landfills and landfills.


## 4. Conclusions

Removal of fluoride ions by the epicarp and mesocarp of green coconut was investigated. The epicarp showed removal efficiency ranging from 66.25% (at 25°C) to 77.50% (at 45°C), while the mesocarp showed removal efficiency ranging from 90% (at 25°C) to 97.50% (at 45°C).The maximum adsorption capacity ranged from 1.6909 to 2.2265 mg·g−1 for the epicarp and from 1.7802 to 3.2253 mg·g−1 for the mesocarp. Compared with other adsorbents of fluoride ions found in the literature, these materials had high values of maximum adsorption capacity. For the two biosorbents, the pseudo-first-order kinetic model appears relevant to describe the fluoride ions adsorption at 25°C, while the pseudo-second-order kinetic model was the best fit for the experimental data at 35 and 45°C.The thermodynamic parameters show that the adsorption of fluoride ions was a spontaneous and endothermic process for both biosorbents, and the adsorption was classified as chemical.The adsorption data of fluoride ions fit well with the Langmuir isotherm model, suggesting that adsorption occurs at homogeneous sites in the developed biosorbents.



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