# Removal of Indigo Carmine Dye from Aqueous Solution Using Magnesium Hydroxide as an Adsorbent

Authors: Thimmasandra Narayan Ramesh; Vani Pavagada Sreenivasa
Journal: Journal of Materials
 (2015)

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## Abstract

Magnesium hydroxide is used as an adsorbent for the removal of indigo carmine dye from aqueous solution. We have investigated the effectiveness of removal of indigo carmine dye from aqueous solutions at pH 6-7 and 12-13 using magnesium hydroxide thereby varying the dose of the adsorbent, concentration of the dye, duration, and temperature. Structural transformations of adsorbent during the adsorption process at different pH values are monitored using powder X-ray diffraction and infrared spectroscopy. Different types of adsorption isotherm models were evaluated and it was found that Langmuir isotherm fits well at both pH values (6-7 and 12-13). Adsorption of indigo carmine onto magnesium hydroxide at pH 6-7/pH 12-13 follows pseudo-second order rate kinetics.


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## Body

## 1. Introduction

Synthetic dyes are most widely used in textile and leather tanning industries [1]. These dyes are highly coloured, toxic, and carcinogenic in nature [2, 3]. These effluents released from the textile and leather tanning industries containing 1 mg/L of dye are enough to impart colour to the water thus making it unpotable for daily use [4, 5]. Dyes can be classified based on their structure, that is, azo dyes, phthalocyanine, anthraquinone dyes, and so forth [1]. Dyes are also categorized as reactive dyes, disperse dyes, direct dyes, VAT dyes, cationic dyes, acid dye, and soluble dyes. The technology used to treat dyes is based on physical, chemical, and biological methods. Precipitation, coagulation, filtration, floatation, electrochemical degradation, and advanced oxidation techniques are considered as chemical methods [6, 7]. Adsorption, reverse osmosis, and ultrafiltration are treated as physical methods [8, 9]. Physical methods of treatment of dyes are nondestructive as the dye transfer from water into the adsorbent occurs which generates large amount of residue. Photochemical irradiation of toxic dyes in presence of a photocatalyst is one of the alternative methods developed recently. Most common photocatalysts are titanium dioxide and zinc oxide which are semiconductors that are expensive and inefficient [10]. Biochemical methods utilize microbes whereas biotechnological methods use agrowaste and other low cost naturally occurring biomaterials for the adsorption of dyes [11–13]. Disposal of the sludge after dye adsorption/removal is of major concern. One of the cheapest and simple methods for the removal of dyes is by the process of adsorption. Most common adsorbents are activated charcoal, zeolites, layered materials, metal oxides, and graphite based compounds [9, 12–15]. Exfoliated graphite/graphite oxide possesses larger interlayer spacing and higher surface area for better adsorption capacity. Due to flexibility and ease of preparation, graphite oxide and graphiteoxide/composites (Fe3O4/GO; chitosan/GO; GO modified polyurethane-chitosan) are used for the removal of toxic dyes such as methylene blue, malachite green dyes, and metal ions [16–21].These effluents cannot be treated effectively using the above compounds as each one of them has their own limitations [22, 23]. Prior to the selection of adsorbent, it should (i) have high affinity for the dyes, (ii) be ecofriendly and safe to handle, and (iii) be universal if possible and preferably regenerative. There are no adsorbents which can fulfill all the requirements and proved to be effective in removing water soluble textile dyes. Indigo carmine is a synthetic dye which has been used as an antibacterial agent, biological stain, dermatological agent, and additive to poultry feed. Also it is a potent carcinogen, recalcitrant, and toxic to mammalian cells [24]. There are few reports on the use of different types of adsorbents to remove indigo carmine dye [25–27]. In our previous studies, we have explored the use of magnesium oxide, calcium oxide, calcium hydroxide as low cost adsorbents for the removal of indigo carmine, amido black 10B dye, solochrome black-T, alizarin red, indigo carmine, and so forth [28–32]. However, there are very few reports on the use of magnesium hydroxide as an adsorbent. In this paper, we have explored the use of magnesium hydroxide as a low cost adsorbent for the removal of indigo carmine dye in aqueous solution by estimating the adsorption capacity at different experimental conditions and evaluated various types of adsorption isotherms.


## 2. Experimental Section

### 2.1. Chemicals Used

The chemicals used are of analytical grade. Magnesium oxide Lite (Merck, India), indigo carmine dye, concentrated hydrochloric acid, and sodium hydroxide were purchased from SD-Fine Chemicals, India, and used without purification.


### 2.2. Preparation of Magnesium Hydroxide

About 5 g of magnesium oxide was added to 100 mL of distilled water and stirred for 4 days at room temperature. The solid was filtered and dried at 65°C for 24 hours.


### 2.3. Indigo Carmine Dye Solution

Indigo carmine dye solution (stock) was prepared by dissolving 50 mg of indigo carmine dye in 1000 mL of distilled water (1.0721 × 10−4 M). About 50 mL of 1.0721 × 10−4 M indigo carmine dye solution was taken and diluted with 100 mL of distilled water (0.53605 × 10−4 M). Series of dye concentrations in the range of 1.0721 × 10−6 M to 5.3605 × 10−5 M or 0.05 mg to 0.25 mg of indigo carmine/10 mL were prepared by transferring 2 mL, 4 mL, 6 mL, 8 mL, and 10 mL of the dye solution followed by dilution using 10 mL of distilled water. By using 1 M HCl or 1 M NaOH, the pH of the indigo carmine dye solution was adjusted to 6-7/12-13, to examine the effect of pH on the adsorption of dye on magnesium hydroxide.


### 2.4. Adsorption Measurements

Kinetic experiments were carried out using 40 mg of adsorbent-magnesium hydroxide in 10 mL of indigo carmine solution of known concentration (0.25 mg of indigo carmine/10 mL) at room temperature (298–301 K). Indigo carmine solutions of different concentrations (0.05 mg to 0.25 mg/10 mL or 1.0721 × 10−5 M to 5.3605 × 10−5 M) were prepared and examined for the percentage of adsorption of magnesium oxide of different quantities, that is, 20 mg, 40 mg, 60 mg, and 80 mg.The temperature effect on the adsorption of indigo carmine dye solutions (at different pH values, dosage—40 mg) was measured. The effect of temperature as a function of time (10, 20, 30, 40, and 50 minutes) on the removal of indigo carmine dye in aqueous solution was examined at pH = 6-7 and pH = 12-13 (dose of magnesium hydroxide was fixed at 40 mg).


### 2.5. Characterization

Elico CL-63 colorimeter was used for the measurement of concentration of the indigo carmine solutions. The wavelength was fixed at 600 nm(λmax⁡) in the pH range of 6–13. All the samples were characterized by powder X-ray diffraction (pXRD) using Bruker D8 advanced diffractometer (CuKα source λ = 1.5418 Å) scan rate 2° min−1 (steps: 0.02°-scan range of 10–65°) which was used to determine the crystal structure of magnesium hydroxide prepared and the products obtained on ageing at different pH values. Fourier transform infrared spectra were recorded by pellet technique using Jasco (FTIR-4100 model) FT-IR spectrometer.


## 2.1. Chemicals Used

The chemicals used are of analytical grade. Magnesium oxide Lite (Merck, India), indigo carmine dye, concentrated hydrochloric acid, and sodium hydroxide were purchased from SD-Fine Chemicals, India, and used without purification.


## 2.2. Preparation of Magnesium Hydroxide

About 5 g of magnesium oxide was added to 100 mL of distilled water and stirred for 4 days at room temperature. The solid was filtered and dried at 65°C for 24 hours.


## 2.3. Indigo Carmine Dye Solution

Indigo carmine dye solution (stock) was prepared by dissolving 50 mg of indigo carmine dye in 1000 mL of distilled water (1.0721 × 10−4 M). About 50 mL of 1.0721 × 10−4 M indigo carmine dye solution was taken and diluted with 100 mL of distilled water (0.53605 × 10−4 M). Series of dye concentrations in the range of 1.0721 × 10−6 M to 5.3605 × 10−5 M or 0.05 mg to 0.25 mg of indigo carmine/10 mL were prepared by transferring 2 mL, 4 mL, 6 mL, 8 mL, and 10 mL of the dye solution followed by dilution using 10 mL of distilled water. By using 1 M HCl or 1 M NaOH, the pH of the indigo carmine dye solution was adjusted to 6-7/12-13, to examine the effect of pH on the adsorption of dye on magnesium hydroxide.


## 2.4. Adsorption Measurements

Kinetic experiments were carried out using 40 mg of adsorbent-magnesium hydroxide in 10 mL of indigo carmine solution of known concentration (0.25 mg of indigo carmine/10 mL) at room temperature (298–301 K). Indigo carmine solutions of different concentrations (0.05 mg to 0.25 mg/10 mL or 1.0721 × 10−5 M to 5.3605 × 10−5 M) were prepared and examined for the percentage of adsorption of magnesium oxide of different quantities, that is, 20 mg, 40 mg, 60 mg, and 80 mg.The temperature effect on the adsorption of indigo carmine dye solutions (at different pH values, dosage—40 mg) was measured. The effect of temperature as a function of time (10, 20, 30, 40, and 50 minutes) on the removal of indigo carmine dye in aqueous solution was examined at pH = 6-7 and pH = 12-13 (dose of magnesium hydroxide was fixed at 40 mg).


## 2.5. Characterization

Elico CL-63 colorimeter was used for the measurement of concentration of the indigo carmine solutions. The wavelength was fixed at 600 nm(λmax⁡) in the pH range of 6–13. All the samples were characterized by powder X-ray diffraction (pXRD) using Bruker D8 advanced diffractometer (CuKα source λ = 1.5418 Å) scan rate 2° min−1 (steps: 0.02°-scan range of 10–65°) which was used to determine the crystal structure of magnesium hydroxide prepared and the products obtained on ageing at different pH values. Fourier transform infrared spectra were recorded by pellet technique using Jasco (FTIR-4100 model) FT-IR spectrometer.


## 3. Results and Discussion

The structure of indigo carmine dye (C16N2H8Na2O8S2-molecular weight 466.36 g mol−1) 3,3′-dioxi-2,2′-bis-Indilyden-5.5′-disulfonic acid disodium salt is shown in Figure 1.Figure 1
The structure of indigo carmine dye.The absorbance values of indigo carmine solution (0.53605 × 10−4 mol L−1) was scanned at different wavelengths.Figure2 shows the powder X-ray diffraction pattern of magnesium hydroxide prepared by stirring magnesium oxide in water at ambient conditions, pH 6-7. The peak positions in the X-ray pXRD pattern of the magnesium oxide aged in water match magnesium hydroxide. The magnesium hydroxide crystallizes in hexagonal system (space group P-3m1) with the lattice parametersa = 3.14 Å;b = 3.12 Å, andc = 4.64 Å; α = 90°, β = 90°, and γ = 120° (ICSD code: 00920).Figure 2
Powder X-ray diffraction pattern of magnesium hydroxide.The infrared spectrum is sensitive to functional groups and hydrogen bonds and can provide supplementary data to powder X-ray diffraction data. Infrared spectral data of the magnesium hydroxide sample aged at pH 6-7 (see Figure3) shows bands in the range of 3000 cm−1 to 3700 cm−1 which arise due to O-H stretching modes of water molecules or hydroxyl groups. We observe a pair of peaks at 3697 and 3447 cm−1 due to lattice vibration of water molecules and OH stretching modes of hydroxyl sheets of magnesium hydroxide [33–35].Figure 3
Infrared spectrum of magnesium hydroxide (precursor).The structure of magnesium hydroxide comprises hexagonal close packing of hydroxyl ions in which magnesium ions occupy octahedral vacant sites thus resulting in the formation of layers. These layers are stacked on top of each other.The effect of initial pH of the dye solution, dosage of adsorbent (magnesium hydroxide), dye concentration, temperature, and time were considered to validate the rate of dye removal.


### 3.1. Effect of pH

The pH of dye solution on the percentage removal of indigo carmine was considered by varying the initial pH (6-7; 9-10; and 13). The effect of pH (6-7, 9-10, and 13) on the adsorption of indigo carmine dye on magnesium hydroxide is shown in Figure4. The percentage adsorption of indigo carmine on magnesium hydroxide was calculated using the following equation:(1)qe=C0-CeC0×100,where C0 and Ce (mg/10 mL) are the initial and equilibrium concentrations of indigo carmine dye in the solution.Figure 4
Effect of pH variation as a function of adsorption percentage.At pH < 6, dissolution of magnesium hydroxide occurs. Hence we have chosen the pH > 6 for our investigation. It is found that maximum adsorption is close to neutral pH 6-7 and moderate adsorption at pH 9-10 and low adsorption at pH 12-13 range. The decrease in the adsorption at higher pH might be due to the presence of negatively charged hydroxyl ions in the solution in addition to the surface hydroxyl groups of magnesium hydroxide.Powder X-ray diffraction data and infrared spectroscopic data were recorded to monitor the structural changes that can be undergone on ageing magnesium hydroxide at pH 12-13 (see Figures5 and 6). It is clearly evident that there are no significant changes observed in the structure of magnesium hydroxide after performing adsorption experiments at pH 12-13, which is based on the powder X-ray diffraction and infrared spectral data of magnesium hydroxide adsorbent (see Figures 5 and 6; Table 1 for band assignments). The infrared spectral data of magnesium hydroxide aged at pH 6-7 and 12-13 is given in Table 1.Table 1
Infrared spectral data of magnesium hydroxide precursor aged at different pH values.
Peak number
Magnesium hydroxide aged at pH 6-7
Band assignment
Magnesium hydroxide aged at pH 13
Band assignment
Wave number (cm−1)
1
3698
OH stretch of Mg(OH)2
3697
OH stretch of Mg(OH)2
2
3646
OH stretch of Mg(OH)2
3647
OH stretch of Mg(OH)2
3
3444
OH stretch of Mg(OH)2
3445
OH stretch of Mg(OH)2
4
1634
H2O bend
1645
H2O bendFigure 5
Powder X-ray diffraction pattern of magnesium hydroxide aged at pH 12-13.Figure 6
Infrared spectrum of magnesium hydroxide aged in pH 12-13 dye solution.


### 3.2. Adsorbent Dose

Figure7 shows the effect of adsorption of indigo carmine dye as a function of an increase in the dosage of magnesium hydroxide. The data clearly indicates that the adsorption increases with increase in the dose quantity. The equilibrium adsorption capacity was estimated and the adsorption of indigo carmine is maximum (81.72%) when 80 mg of magnesium hydroxide was used, while the adsorption capacity of indigo carmine dye was 69.52% when 40 mg of magnesium hydroxide adsorbent was used. Generally at higher temperatures, adsorption will increase; hence we had used optimum quantity (40 mg) of magnesium hydroxide adsorbent for all future investigations.Figure 7
Variation of adsorbent dosage of magnesium hydroxide at pH 6-7.


### 3.3. Dye Concentration

Dye concentrations, that is, 0.05–0.25 mg/10 mL, were varied as a function of time at pH 6-7 and 12-13 and the adsorption was monitored at 298 K. The equilibrium adsorptionqe was estimated. Figure 8 shows the effect of concentration of adsorption of indigo carmine dye solution onto magnesium hydroxide.Figure 8
Effect of concentration as a function of percentage of adsorption.


### 3.4. Effect of Duration

Adsorption of indigo carmine on magnesium hydroxide at different contact times has been examined by adding 20 mg, 40 mg, 60 mg, and 80 mg of adsorbent to indigo carmine dye solution (0.25 mg/10 mL). Figure9 shows the effect of duration or contact time on the adsorption of indigo carmine on magnesium hydroxide at pH 6-7.Figure 9
Effect of contact time on the adsorption of indigo carmine dye on magnesium hydroxide at pH 6-7.The adsorption maximum varied with variation in different doses and maximum of about 81% was observed when 80 mg of magnesium hydroxide was used (duration 50 minutes).


### 3.5. Effect of Temperature

Temperature can affect the rate of adsorption drastically. Figure10 shows the percentage of adsorption with increase in temperature (i.e., 298 K, 313 K, 323 K, and 333 K). It is found that at 333 K, the adsorption is maximum (pH = 6-7, 81.68%, and pH 12-13, 67.67%). With increase in temperature, adsorption also increases nonlinearly indicating that the process is endothermic in nature at lower temperatures. With increase in temperature, the free energy will be negative indicating the favourability of the process.Figure 10
Effect of temperature on the adsorption of indigo carmine dye on magnesium hydroxide at different temperatures and pH values.The Pearson correlation coefficient (r/R2) values are used to get an insight into the adsorption process of indigo carmine dye solution onto magnesium hydroxide. The value approaches unity at higher temperature indicating that the adsorption is more favourable at higher temperature.


### 3.6. Adsorption Isotherm Analyses

Different types of adsorption isotherm models were used to analyze the adsorption process of indigo carmine dye in aqueous solution onto magnesium hydroxide.


#### 3.6.1. Freundlich Isotherm

Freundlich isotherm can be calculated using the following equation:(2)log⁡qe=log⁡kf+1nlog⁡Ce,where qe is the equilibrium adsorption capacity, Ce is the equilibrium concentration (mg/10 mL), kf relates adsorption capacity of Freundlich constant, and 1/n relates the intensity of Freundlich constant.Freundlich isotherm model is applied in most cases for multilayer adsorption process and Figure11 shows the graph of Freundlich isotherms of magnesium hydroxide at pH 6-7 and pH 12-13, respectively. The graph is approaching linearity indicating the possibility of multilayer adsorption.Figure 11
Plot of-log⁡Ce versus -log⁡qe for Freundlich isotherms at pH 6-7 and pH 12-13, respectively.


#### 3.6.2. Temkin Isotherm

Temkin isotherm is evaluated using the following equation:(3)ln⁡CeversusqekT-bTkT,where T is the temperature (Kelvin), bT is the heat of sorption, kT is the Temkin isotherm constant, and qe is the equilibrium adsorption capacity.The data indicates that equilibrium adsorption capacity increases with increase in concentration and exhibits linearity for pH 6-7 and pH 12-13 (see Figure12). Temkin isotherm may be applicable for the adsorption of indigo carmine onto magnesium hydroxide at pH, that is, 6-7 and pH 12-13.Figure 12
Plot ofln⁡Ce versus qe for Temkin isotherms at pH 6-7 and pH 12-13, respectively.


#### 3.6.3. Redlich-Peterson Isotherm

Consider the following:(4)log⁡Ce=1log⁡bRβ⁡KR+log⁡Ceqe,where Kr, bR, and β are Redlich-Peterson constants which are used to calculate the Redlich-Peterson isotherm.Figure13 shows the plot of ln⁡Ce versus -log⁡Ce/qe, which is a straight line with a slope KR+log⁡Ce/qe.Figure 13
Plot oflog⁡Ce versus -log⁡Ce/qe for Redlich-Peterson isotherms at pH 6-7 and pH 12-13, respectively.The importance of Redlich-Peterson isotherm is that it is a combination of Langmuir and Freundlich isotherms. The data fits reasonably well at pH 6-7 and pH 12-13 indicating it to be of Redlich-Peterson isotherm model.Table2 shows the parameters and their values used for deriving information about various types of isotherms.Table 2
(a) General data applicable to different isotherms (pH 6-7). (b) General data applicable to different isotherms (pH 12-13).
(a)
C
e
q
e
log
⁡
C
e
log
⁡
q
e
ln
⁡
C
e
ln
⁡
q
e
1
/
q
e
C
e
/
q
e
log
⁡
(
C
e
/
q
e
)
0.1616
0.0221
−0.7915
−1.6556
−1.8226
−3.8122
45.249
7.3122
0.86405
0.1067
0.03583
−0.9712
−1.4458
−2.2377
−3.329
27.909
2.9779
0.4739
0.09146
0.0396
−1.0388
−1.4023
−2.3919
−3.229
25.253
2.3096
0.36354
0.0793
0.0427
−1.10073
−1.3696
−2.535
−3.1536
23.419
1.8571
0.26884
0.0762
0.0435
−1.11805
−1.3615
−2.5744
−3.1349
22.99
1.7517
0.24346
(b)
C
e
q
e
log
⁡
C
e
log
⁡
q
e
ln
⁡
C
e
ln
⁡
q
e
1
/
q
e
C
e
/
q
e
log
⁡
(
C
e
/
q
e
)
0.1739
0.0190
−0.7597
−1.7207
−1.7493
−3.9633
52.5624
9.1406
0.96097
0.1486
0.0254
−0.8281
−1.5960
−1.9065
−3.6730
39.4477
5.8619
0.76804
0.1413
0.0272
−0.8498
−1.5658
−1.9569
−3.6045
36.7985
5.1996
0.715969
0.1232
0.0317
−0.9094
−1.4989
−2.0939
−3.4514
31.5457
3.8864
0.58955
0.1123
0.0344
−0.9495
−1.4631
−2.1866
−3.3697
29.0487
3.2622
0.51351
The correlation coefficients for the different isotherm models and the equations used to calculate theR/r values.Adsorption isotherm better fits in the following increasing order based on the correlation coefficient (R2) values when indigo carmine dye solution was maintained at pH 6-7 (magnesium hydroxide-adsorbent): Harkin-Jura isotherm (1.0041) < Langmuir isotherm (1.0068). WhileR2 value of Langmuir isotherm and Harkin-Jura isotherm values are 1 indicating that adsorption process occurs first as a monolayer followed by multilayer process at pH 6-7 when magnesium hydroxide was used as adsorbent and indigo carmine dye solution.Adsorption isotherm better fits in the following increasing order based on the correlation coefficient (R2) values when indigo carmine dye solution was maintained at pH 12-13 (magnesium hydroxide-adsorbent): Langmuir (0.9796) < Temkin isotherm (1.016). WhileR2 value of Langmuir isotherm and Temkin isotherms are 1 indicating that adsorption process occurs at pH 12-13 when magnesium hydroxide-adsorbent was used as adsorbent and indigo carmine dye solution.


### 3.7. Kinetics of Adsorption Process

Kinetic models (pseudo-first order and pseudo-second order rate equations) were evaluated to get an insight into the adsorption process of indigo carmine dye onto magnesium hydroxide [20, 36]. The data does not fit linearly for pseudo-first order rate kinetics.


#### 3.7.1. Pseudo-Second Order Rate Equation

The adsorption process was examined to fit for pseudo-second order rate equation. If the interaction between the indigo carmine dye and magnesium oxide is through charge transfer then the reaction should be pseudo-second order. The parameters used to determine pseudo-second order rate equation during the adsorption of indigo carmine dye onto magnesium hydroxide are given in Tables3 and 4 (see Figure 14). Ther orR2 value (calculated) 0.9945 indicates that it is a reasonably good fit and the experimental (0.0435) and calculated qe values (0.05) are closer indicating that the adsorption might be of pseudo-second order in nature at pH 6-7. At pH 12-13, the calculatedr orR2 value is 0.9921 which indicates that it is a reasonably good fit. But the differences between the experimental (0.0344) and calculated qe values (0.038) are large indicating that the adsorption follows pseudo-second order at pH 12-13.Table 3
(a) List of parameters used to evaluate the pseudo-second order rate equation (pH 6-7). (b) List of parameters used to evaluate the pseudo-second order rate equation (pH 12-13).
(a)
Kinetic model
Parameters
Dye (mg/100 mL)C0
q
e (experimental)
K
2
q
e (calculated)
R
2
Pseudo-second order kinetics
0.25
0.0435
52.48803
0.05217
0.09945
(b)
Kinetic model
Parameters
Dye (mg/100 mL)C0
q
e (experimental)
K
2
q
e (calculated)
R
2
Pseudo-second order kinetics
0.25
0.0344
229.6875
0.03809
0.992186Table 4
(a) List of parameters used to evaluate the pseudo-second order rate equation (pH 6-7). (b) List of parameters used to evaluate the pseudo-second order rate equation (pH 12-13).
(a)
Time (min)
t/qt
t
2
t/qt2
t
×
t/qt
10
452.489
100
204746.29
4524.89
20
558.1915
400
311577.750
11163.83
30
757.5757
900
573920.94
22727.271
40
936.768
1600
877534.2858
37470.72
50
1149.453
2500
1321242.19
57472.65
∑
t
=
150
∑
t
q
t
=
3854.4772
∑
t
2
=
5500
∑
t
q
t
2
=
3289021.472
∑
t
×
t
q
t
=
133359.36
(b)
Time (min)
t/qt
t
2
t/qt2
t
×
t/qt
10
526.3158
100
277008.3213
5263.158
20
787.4015
400
620001.1222
15748.03
30
1102.9412
900
1216479.291
33088.236
40
1261.8297
1600
1592214.192
50473.188
50
1453.4884
2500
2112628.529
72674.42
∑
t
=
150
∑
t
q
t
=
5131.9766
∑
t
2
=
5500
∑
t
q
t
2
=
5818331.456
∑
t
×
t
q
t
=
177247.032Figure 14
Pseudo-second order kinetics.


### 3.8. Thermodynamic Parameters

The difference in the free energy (ΔG°) with change in the temperature during the adsorption process of indigo carmine onto magnesium hydroxide at pH 7 and pH 13 is given in Table 5. The negative free energy values at higher temperature indicate that the adsorption process is endothermic at pHs (6-7/12-13).Table 5
(a) Thermodynamic parameters for adsorption of indigo carmine onto magnesium hydroxide at pH 7. (b) Thermodynamic parameters for adsorption of indigo carmine onto magnesium hydroxide at pH 13.
(a)
Adsorbent
Temperature (K)
Δ
G
° (kJ mol−1)
Magnesium hydroxide
298
4.5497
313
8.0641
323
−0.1369
333
−0.4484
(b)
Adsorbent
Temperature (K)
Δ
G
° (kJ mol−1)
Magnesium hydroxide
298
3.4227
313
1.3041
323
1.0203
333
−2.2029


## 3.1. Effect of pH

The pH of dye solution on the percentage removal of indigo carmine was considered by varying the initial pH (6-7; 9-10; and 13). The effect of pH (6-7, 9-10, and 13) on the adsorption of indigo carmine dye on magnesium hydroxide is shown in Figure4. The percentage adsorption of indigo carmine on magnesium hydroxide was calculated using the following equation:(1)qe=C0-CeC0×100,where C0 and Ce (mg/10 mL) are the initial and equilibrium concentrations of indigo carmine dye in the solution.Figure 4
Effect of pH variation as a function of adsorption percentage.At pH < 6, dissolution of magnesium hydroxide occurs. Hence we have chosen the pH > 6 for our investigation. It is found that maximum adsorption is close to neutral pH 6-7 and moderate adsorption at pH 9-10 and low adsorption at pH 12-13 range. The decrease in the adsorption at higher pH might be due to the presence of negatively charged hydroxyl ions in the solution in addition to the surface hydroxyl groups of magnesium hydroxide.Powder X-ray diffraction data and infrared spectroscopic data were recorded to monitor the structural changes that can be undergone on ageing magnesium hydroxide at pH 12-13 (see Figures5 and 6). It is clearly evident that there are no significant changes observed in the structure of magnesium hydroxide after performing adsorption experiments at pH 12-13, which is based on the powder X-ray diffraction and infrared spectral data of magnesium hydroxide adsorbent (see Figures 5 and 6; Table 1 for band assignments). The infrared spectral data of magnesium hydroxide aged at pH 6-7 and 12-13 is given in Table 1.Table 1
Infrared spectral data of magnesium hydroxide precursor aged at different pH values.
Peak number
Magnesium hydroxide aged at pH 6-7
Band assignment
Magnesium hydroxide aged at pH 13
Band assignment
Wave number (cm−1)
1
3698
OH stretch of Mg(OH)2
3697
OH stretch of Mg(OH)2
2
3646
OH stretch of Mg(OH)2
3647
OH stretch of Mg(OH)2
3
3444
OH stretch of Mg(OH)2
3445
OH stretch of Mg(OH)2
4
1634
H2O bend
1645
H2O bendFigure 5
Powder X-ray diffraction pattern of magnesium hydroxide aged at pH 12-13.Figure 6
Infrared spectrum of magnesium hydroxide aged in pH 12-13 dye solution.


## 3.2. Adsorbent Dose

Figure7 shows the effect of adsorption of indigo carmine dye as a function of an increase in the dosage of magnesium hydroxide. The data clearly indicates that the adsorption increases with increase in the dose quantity. The equilibrium adsorption capacity was estimated and the adsorption of indigo carmine is maximum (81.72%) when 80 mg of magnesium hydroxide was used, while the adsorption capacity of indigo carmine dye was 69.52% when 40 mg of magnesium hydroxide adsorbent was used. Generally at higher temperatures, adsorption will increase; hence we had used optimum quantity (40 mg) of magnesium hydroxide adsorbent for all future investigations.Figure 7
Variation of adsorbent dosage of magnesium hydroxide at pH 6-7.


## 3.3. Dye Concentration

Dye concentrations, that is, 0.05–0.25 mg/10 mL, were varied as a function of time at pH 6-7 and 12-13 and the adsorption was monitored at 298 K. The equilibrium adsorptionqe was estimated. Figure 8 shows the effect of concentration of adsorption of indigo carmine dye solution onto magnesium hydroxide.Figure 8
Effect of concentration as a function of percentage of adsorption.


## 3.4. Effect of Duration

Adsorption of indigo carmine on magnesium hydroxide at different contact times has been examined by adding 20 mg, 40 mg, 60 mg, and 80 mg of adsorbent to indigo carmine dye solution (0.25 mg/10 mL). Figure9 shows the effect of duration or contact time on the adsorption of indigo carmine on magnesium hydroxide at pH 6-7.Figure 9
Effect of contact time on the adsorption of indigo carmine dye on magnesium hydroxide at pH 6-7.The adsorption maximum varied with variation in different doses and maximum of about 81% was observed when 80 mg of magnesium hydroxide was used (duration 50 minutes).


## 3.5. Effect of Temperature

Temperature can affect the rate of adsorption drastically. Figure10 shows the percentage of adsorption with increase in temperature (i.e., 298 K, 313 K, 323 K, and 333 K). It is found that at 333 K, the adsorption is maximum (pH = 6-7, 81.68%, and pH 12-13, 67.67%). With increase in temperature, adsorption also increases nonlinearly indicating that the process is endothermic in nature at lower temperatures. With increase in temperature, the free energy will be negative indicating the favourability of the process.Figure 10
Effect of temperature on the adsorption of indigo carmine dye on magnesium hydroxide at different temperatures and pH values.The Pearson correlation coefficient (r/R2) values are used to get an insight into the adsorption process of indigo carmine dye solution onto magnesium hydroxide. The value approaches unity at higher temperature indicating that the adsorption is more favourable at higher temperature.


## 3.6. Adsorption Isotherm Analyses

Different types of adsorption isotherm models were used to analyze the adsorption process of indigo carmine dye in aqueous solution onto magnesium hydroxide.


### 3.6.1. Freundlich Isotherm

Freundlich isotherm can be calculated using the following equation:(2)log⁡qe=log⁡kf+1nlog⁡Ce,where qe is the equilibrium adsorption capacity, Ce is the equilibrium concentration (mg/10 mL), kf relates adsorption capacity of Freundlich constant, and 1/n relates the intensity of Freundlich constant.Freundlich isotherm model is applied in most cases for multilayer adsorption process and Figure11 shows the graph of Freundlich isotherms of magnesium hydroxide at pH 6-7 and pH 12-13, respectively. The graph is approaching linearity indicating the possibility of multilayer adsorption.Figure 11
Plot of-log⁡Ce versus -log⁡qe for Freundlich isotherms at pH 6-7 and pH 12-13, respectively.


### 3.6.2. Temkin Isotherm

Temkin isotherm is evaluated using the following equation:(3)ln⁡CeversusqekT-bTkT,where T is the temperature (Kelvin), bT is the heat of sorption, kT is the Temkin isotherm constant, and qe is the equilibrium adsorption capacity.The data indicates that equilibrium adsorption capacity increases with increase in concentration and exhibits linearity for pH 6-7 and pH 12-13 (see Figure12). Temkin isotherm may be applicable for the adsorption of indigo carmine onto magnesium hydroxide at pH, that is, 6-7 and pH 12-13.Figure 12
Plot ofln⁡Ce versus qe for Temkin isotherms at pH 6-7 and pH 12-13, respectively.


### 3.6.3. Redlich-Peterson Isotherm

Consider the following:(4)log⁡Ce=1log⁡bRβ⁡KR+log⁡Ceqe,where Kr, bR, and β are Redlich-Peterson constants which are used to calculate the Redlich-Peterson isotherm.Figure13 shows the plot of ln⁡Ce versus -log⁡Ce/qe, which is a straight line with a slope KR+log⁡Ce/qe.Figure 13
Plot oflog⁡Ce versus -log⁡Ce/qe for Redlich-Peterson isotherms at pH 6-7 and pH 12-13, respectively.The importance of Redlich-Peterson isotherm is that it is a combination of Langmuir and Freundlich isotherms. The data fits reasonably well at pH 6-7 and pH 12-13 indicating it to be of Redlich-Peterson isotherm model.Table2 shows the parameters and their values used for deriving information about various types of isotherms.Table 2
(a) General data applicable to different isotherms (pH 6-7). (b) General data applicable to different isotherms (pH 12-13).
(a)
C
e
q
e
log
⁡
C
e
log
⁡
q
e
ln
⁡
C
e
ln
⁡
q
e
1
/
q
e
C
e
/
q
e
log
⁡
(
C
e
/
q
e
)
0.1616
0.0221
−0.7915
−1.6556
−1.8226
−3.8122
45.249
7.3122
0.86405
0.1067
0.03583
−0.9712
−1.4458
−2.2377
−3.329
27.909
2.9779
0.4739
0.09146
0.0396
−1.0388
−1.4023
−2.3919
−3.229
25.253
2.3096
0.36354
0.0793
0.0427
−1.10073
−1.3696
−2.535
−3.1536
23.419
1.8571
0.26884
0.0762
0.0435
−1.11805
−1.3615
−2.5744
−3.1349
22.99
1.7517
0.24346
(b)
C
e
q
e
log
⁡
C
e
log
⁡
q
e
ln
⁡
C
e
ln
⁡
q
e
1
/
q
e
C
e
/
q
e
log
⁡
(
C
e
/
q
e
)
0.1739
0.0190
−0.7597
−1.7207
−1.7493
−3.9633
52.5624
9.1406
0.96097
0.1486
0.0254
−0.8281
−1.5960
−1.9065
−3.6730
39.4477
5.8619
0.76804
0.1413
0.0272
−0.8498
−1.5658
−1.9569
−3.6045
36.7985
5.1996
0.715969
0.1232
0.0317
−0.9094
−1.4989
−2.0939
−3.4514
31.5457
3.8864
0.58955
0.1123
0.0344
−0.9495
−1.4631
−2.1866
−3.3697
29.0487
3.2622
0.51351
The correlation coefficients for the different isotherm models and the equations used to calculate theR/r values.Adsorption isotherm better fits in the following increasing order based on the correlation coefficient (R2) values when indigo carmine dye solution was maintained at pH 6-7 (magnesium hydroxide-adsorbent): Harkin-Jura isotherm (1.0041) < Langmuir isotherm (1.0068). WhileR2 value of Langmuir isotherm and Harkin-Jura isotherm values are 1 indicating that adsorption process occurs first as a monolayer followed by multilayer process at pH 6-7 when magnesium hydroxide was used as adsorbent and indigo carmine dye solution.Adsorption isotherm better fits in the following increasing order based on the correlation coefficient (R2) values when indigo carmine dye solution was maintained at pH 12-13 (magnesium hydroxide-adsorbent): Langmuir (0.9796) < Temkin isotherm (1.016). WhileR2 value of Langmuir isotherm and Temkin isotherms are 1 indicating that adsorption process occurs at pH 12-13 when magnesium hydroxide-adsorbent was used as adsorbent and indigo carmine dye solution.


## 3.6.1. Freundlich Isotherm

Freundlich isotherm can be calculated using the following equation:(2)log⁡qe=log⁡kf+1nlog⁡Ce,where qe is the equilibrium adsorption capacity, Ce is the equilibrium concentration (mg/10 mL), kf relates adsorption capacity of Freundlich constant, and 1/n relates the intensity of Freundlich constant.Freundlich isotherm model is applied in most cases for multilayer adsorption process and Figure11 shows the graph of Freundlich isotherms of magnesium hydroxide at pH 6-7 and pH 12-13, respectively. The graph is approaching linearity indicating the possibility of multilayer adsorption.Figure 11
Plot of-log⁡Ce versus -log⁡qe for Freundlich isotherms at pH 6-7 and pH 12-13, respectively.


## 3.6.2. Temkin Isotherm

Temkin isotherm is evaluated using the following equation:(3)ln⁡CeversusqekT-bTkT,where T is the temperature (Kelvin), bT is the heat of sorption, kT is the Temkin isotherm constant, and qe is the equilibrium adsorption capacity.The data indicates that equilibrium adsorption capacity increases with increase in concentration and exhibits linearity for pH 6-7 and pH 12-13 (see Figure12). Temkin isotherm may be applicable for the adsorption of indigo carmine onto magnesium hydroxide at pH, that is, 6-7 and pH 12-13.Figure 12
Plot ofln⁡Ce versus qe for Temkin isotherms at pH 6-7 and pH 12-13, respectively.


## 3.6.3. Redlich-Peterson Isotherm

Consider the following:(4)log⁡Ce=1log⁡bRβ⁡KR+log⁡Ceqe,where Kr, bR, and β are Redlich-Peterson constants which are used to calculate the Redlich-Peterson isotherm.Figure13 shows the plot of ln⁡Ce versus -log⁡Ce/qe, which is a straight line with a slope KR+log⁡Ce/qe.Figure 13
Plot oflog⁡Ce versus -log⁡Ce/qe for Redlich-Peterson isotherms at pH 6-7 and pH 12-13, respectively.The importance of Redlich-Peterson isotherm is that it is a combination of Langmuir and Freundlich isotherms. The data fits reasonably well at pH 6-7 and pH 12-13 indicating it to be of Redlich-Peterson isotherm model.Table2 shows the parameters and their values used for deriving information about various types of isotherms.Table 2
(a) General data applicable to different isotherms (pH 6-7). (b) General data applicable to different isotherms (pH 12-13).
(a)
C
e
q
e
log
⁡
C
e
log
⁡
q
e
ln
⁡
C
e
ln
⁡
q
e
1
/
q
e
C
e
/
q
e
log
⁡
(
C
e
/
q
e
)
0.1616
0.0221
−0.7915
−1.6556
−1.8226
−3.8122
45.249
7.3122
0.86405
0.1067
0.03583
−0.9712
−1.4458
−2.2377
−3.329
27.909
2.9779
0.4739
0.09146
0.0396
−1.0388
−1.4023
−2.3919
−3.229
25.253
2.3096
0.36354
0.0793
0.0427
−1.10073
−1.3696
−2.535
−3.1536
23.419
1.8571
0.26884
0.0762
0.0435
−1.11805
−1.3615
−2.5744
−3.1349
22.99
1.7517
0.24346
(b)
C
e
q
e
log
⁡
C
e
log
⁡
q
e
ln
⁡
C
e
ln
⁡
q
e
1
/
q
e
C
e
/
q
e
log
⁡
(
C
e
/
q
e
)
0.1739
0.0190
−0.7597
−1.7207
−1.7493
−3.9633
52.5624
9.1406
0.96097
0.1486
0.0254
−0.8281
−1.5960
−1.9065
−3.6730
39.4477
5.8619
0.76804
0.1413
0.0272
−0.8498
−1.5658
−1.9569
−3.6045
36.7985
5.1996
0.715969
0.1232
0.0317
−0.9094
−1.4989
−2.0939
−3.4514
31.5457
3.8864
0.58955
0.1123
0.0344
−0.9495
−1.4631
−2.1866
−3.3697
29.0487
3.2622
0.51351
The correlation coefficients for the different isotherm models and the equations used to calculate theR/r values.Adsorption isotherm better fits in the following increasing order based on the correlation coefficient (R2) values when indigo carmine dye solution was maintained at pH 6-7 (magnesium hydroxide-adsorbent): Harkin-Jura isotherm (1.0041) < Langmuir isotherm (1.0068). WhileR2 value of Langmuir isotherm and Harkin-Jura isotherm values are 1 indicating that adsorption process occurs first as a monolayer followed by multilayer process at pH 6-7 when magnesium hydroxide was used as adsorbent and indigo carmine dye solution.Adsorption isotherm better fits in the following increasing order based on the correlation coefficient (R2) values when indigo carmine dye solution was maintained at pH 12-13 (magnesium hydroxide-adsorbent): Langmuir (0.9796) < Temkin isotherm (1.016). WhileR2 value of Langmuir isotherm and Temkin isotherms are 1 indicating that adsorption process occurs at pH 12-13 when magnesium hydroxide-adsorbent was used as adsorbent and indigo carmine dye solution.


## 3.7. Kinetics of Adsorption Process

Kinetic models (pseudo-first order and pseudo-second order rate equations) were evaluated to get an insight into the adsorption process of indigo carmine dye onto magnesium hydroxide [20, 36]. The data does not fit linearly for pseudo-first order rate kinetics.


### 3.7.1. Pseudo-Second Order Rate Equation

The adsorption process was examined to fit for pseudo-second order rate equation. If the interaction between the indigo carmine dye and magnesium oxide is through charge transfer then the reaction should be pseudo-second order. The parameters used to determine pseudo-second order rate equation during the adsorption of indigo carmine dye onto magnesium hydroxide are given in Tables3 and 4 (see Figure 14). Ther orR2 value (calculated) 0.9945 indicates that it is a reasonably good fit and the experimental (0.0435) and calculated qe values (0.05) are closer indicating that the adsorption might be of pseudo-second order in nature at pH 6-7. At pH 12-13, the calculatedr orR2 value is 0.9921 which indicates that it is a reasonably good fit. But the differences between the experimental (0.0344) and calculated qe values (0.038) are large indicating that the adsorption follows pseudo-second order at pH 12-13.Table 3
(a) List of parameters used to evaluate the pseudo-second order rate equation (pH 6-7). (b) List of parameters used to evaluate the pseudo-second order rate equation (pH 12-13).
(a)
Kinetic model
Parameters
Dye (mg/100 mL)C0
q
e (experimental)
K
2
q
e (calculated)
R
2
Pseudo-second order kinetics
0.25
0.0435
52.48803
0.05217
0.09945
(b)
Kinetic model
Parameters
Dye (mg/100 mL)C0
q
e (experimental)
K
2
q
e (calculated)
R
2
Pseudo-second order kinetics
0.25
0.0344
229.6875
0.03809
0.992186Table 4
(a) List of parameters used to evaluate the pseudo-second order rate equation (pH 6-7). (b) List of parameters used to evaluate the pseudo-second order rate equation (pH 12-13).
(a)
Time (min)
t/qt
t
2
t/qt2
t
×
t/qt
10
452.489
100
204746.29
4524.89
20
558.1915
400
311577.750
11163.83
30
757.5757
900
573920.94
22727.271
40
936.768
1600
877534.2858
37470.72
50
1149.453
2500
1321242.19
57472.65
∑
t
=
150
∑
t
q
t
=
3854.4772
∑
t
2
=
5500
∑
t
q
t
2
=
3289021.472
∑
t
×
t
q
t
=
133359.36
(b)
Time (min)
t/qt
t
2
t/qt2
t
×
t/qt
10
526.3158
100
277008.3213
5263.158
20
787.4015
400
620001.1222
15748.03
30
1102.9412
900
1216479.291
33088.236
40
1261.8297
1600
1592214.192
50473.188
50
1453.4884
2500
2112628.529
72674.42
∑
t
=
150
∑
t
q
t
=
5131.9766
∑
t
2
=
5500
∑
t
q
t
2
=
5818331.456
∑
t
×
t
q
t
=
177247.032Figure 14
Pseudo-second order kinetics.


## 3.7.1. Pseudo-Second Order Rate Equation

The adsorption process was examined to fit for pseudo-second order rate equation. If the interaction between the indigo carmine dye and magnesium oxide is through charge transfer then the reaction should be pseudo-second order. The parameters used to determine pseudo-second order rate equation during the adsorption of indigo carmine dye onto magnesium hydroxide are given in Tables3 and 4 (see Figure 14). Ther orR2 value (calculated) 0.9945 indicates that it is a reasonably good fit and the experimental (0.0435) and calculated qe values (0.05) are closer indicating that the adsorption might be of pseudo-second order in nature at pH 6-7. At pH 12-13, the calculatedr orR2 value is 0.9921 which indicates that it is a reasonably good fit. But the differences between the experimental (0.0344) and calculated qe values (0.038) are large indicating that the adsorption follows pseudo-second order at pH 12-13.Table 3
(a) List of parameters used to evaluate the pseudo-second order rate equation (pH 6-7). (b) List of parameters used to evaluate the pseudo-second order rate equation (pH 12-13).
(a)
Kinetic model
Parameters
Dye (mg/100 mL)C0
q
e (experimental)
K
2
q
e (calculated)
R
2
Pseudo-second order kinetics
0.25
0.0435
52.48803
0.05217
0.09945
(b)
Kinetic model
Parameters
Dye (mg/100 mL)C0
q
e (experimental)
K
2
q
e (calculated)
R
2
Pseudo-second order kinetics
0.25
0.0344
229.6875
0.03809
0.992186Table 4
(a) List of parameters used to evaluate the pseudo-second order rate equation (pH 6-7). (b) List of parameters used to evaluate the pseudo-second order rate equation (pH 12-13).
(a)
Time (min)
t/qt
t
2
t/qt2
t
×
t/qt
10
452.489
100
204746.29
4524.89
20
558.1915
400
311577.750
11163.83
30
757.5757
900
573920.94
22727.271
40
936.768
1600
877534.2858
37470.72
50
1149.453
2500
1321242.19
57472.65
∑
t
=
150
∑
t
q
t
=
3854.4772
∑
t
2
=
5500
∑
t
q
t
2
=
3289021.472
∑
t
×
t
q
t
=
133359.36
(b)
Time (min)
t/qt
t
2
t/qt2
t
×
t/qt
10
526.3158
100
277008.3213
5263.158
20
787.4015
400
620001.1222
15748.03
30
1102.9412
900
1216479.291
33088.236
40
1261.8297
1600
1592214.192
50473.188
50
1453.4884
2500
2112628.529
72674.42
∑
t
=
150
∑
t
q
t
=
5131.9766
∑
t
2
=
5500
∑
t
q
t
2
=
5818331.456
∑
t
×
t
q
t
=
177247.032Figure 14
Pseudo-second order kinetics.


## 3.8. Thermodynamic Parameters

The difference in the free energy (ΔG°) with change in the temperature during the adsorption process of indigo carmine onto magnesium hydroxide at pH 7 and pH 13 is given in Table 5. The negative free energy values at higher temperature indicate that the adsorption process is endothermic at pHs (6-7/12-13).Table 5
(a) Thermodynamic parameters for adsorption of indigo carmine onto magnesium hydroxide at pH 7. (b) Thermodynamic parameters for adsorption of indigo carmine onto magnesium hydroxide at pH 13.
(a)
Adsorbent
Temperature (K)
Δ
G
° (kJ mol−1)
Magnesium hydroxide
298
4.5497
313
8.0641
323
−0.1369
333
−0.4484
(b)
Adsorbent
Temperature (K)
Δ
G
° (kJ mol−1)
Magnesium hydroxide
298
3.4227
313
1.3041
323
1.0203
333
−2.2029


## 4. Conclusions

Different types of adsorption isotherms of indigo carmine dye on magnesium hydroxide were evaluated to understand the nature of interaction between the adsorbent and adsorbate. Langmuir and Harkin-Jura isotherms fit well at pH 7 indicating that monolayer and multilayer adsorption occurs simultaneously. Langmuir and Temkin isotherm models are effective at pH 12-13 indicating that adsorption is a monolayer process. The percentage of adsorption of indigo carmine dye from aqueous solution onto magnesium hydroxide maintained at pH 6-7 and at 333 K is 20% higher than that at pH 12-13. The results demonstrate that the process of adsorption is endothermic and spontaneous. Therefore, magnesium hydroxide is used as a low cost adsorbent for the removal of indigo carmine dye solution.



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*Source: 753057-2015-11-01.xml*