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M. Hema, P. Martin Deva Prasath, and S. Arivoli

ADSORPTION OF MALACHITE GREEN ONTO CARBON PREPARED FROM BORASSUS BARK S. Arivoli* *Department of Chemistry, H H The Rajah’s College, Pudukkottai 622 001, India

M. Hema and P. Martin Deva Prasath Department of Chemistry, T.B.M.L. College, Porayar 607309, India

:Δ˰λϼΨϟ΍ ˬνήόΘϟ΍ Ϧϣί :ΔϴϟΎΘϟ΍ Ϟϣ΍Ϯόϟ΍ Δγ΍έΪΑ ΎϨϤϗ Ϊϗϭ .ϲ΋Ύϣ ςγϭ ϲϓ ˯΍ήπΨϟ΍ ΖϴϜϠϤϟ΍ Δϟ΍ί· ϰϠϋ ςθϨϤϟ΍ ϥϮΑήϜϟ΍ ΓέΪϗ έΎΒΘΧ΍ - ΚΤΒϟ΍ ΍άϫ ϲϓ - ϢΗ ΔσΎγϮΑ ϝΪόϤϟΎΑ ϢϜΤΘϟ΍ ϢΘϳϭ ϰϟϭϷ΍ ΔΟέΪϟ΍ Ϧϣ ΔϟΩΎόϣ ιΎμϣΩϻ΍ ϊΒΘϳϭ .Γέ΍ήΤϟ΍ ΔΟέΩϭ PH ϞϣΎϋϭ ϥϮΑήϜϟ΍ Δϋή˵Οϭ ˬϲϟϭϷ΍ ΔϐΒμϟ΍ ΰϴϛήΗϭ ΕΎϣϮγέ ϝϼΧ Ϧϣ (Qm) ιΎμϣΩϻ΍ Δόγ ϰϠϋ ΎϨϠμΤϓ ˬ ϥ΍ΰΗϻ΍ ΕΎϧΎϴΒϟ έϮϴϤΠϧϻϭ ζϴϟΪϨϳήϓ ΝΫϮϤϧ΃ ΎϨϣΪΨΘγ΍ϭ .ΕΎϤϴδΠϠϟ ϲϨϴΒϟ΍ έΎθΘϧϻ΍ ˬΐϴΗήΘϟ΍ ϰϠϋ 60ºC, 50, 40 30 :Γέ΍ήΣ ΕΎΟέΩ ΪϨϋ (mg/g) 19.34, 19.76, 20.25, 20.70 :ϲϠϳ ΎϤϛ ΖϧΎϛϭ ΔΘΑΎΛ Γέ΍ήΣ ΕΎΟέΩ ΪϨϋ έϮϴϤΠϧϻ ΢τγ ϰϠϋ Δϴ΋΍Ϯθόϟ΍ Ϧϣ ωϮϧ ϊϣ ϲ΋ΎΠϓϭ Γέ΍ήΤϠϟ ιΎϣ ήπΧϷ΍ ΖϴϜϠϤϟ΍ ιΎμΘϣ΍ ϥ΃ Γέ΍ήΤϟ΍ ΔΟέΩ ϲϓ ϑϼΘΧϻ΍ ήϬχ΃ϭ .6.0=PH ϞϣΎϋ ΪϨϋϭ .ΐϠμϟ΍ αΎϤΘϟ΍

ABSTRACT An activated carbon prepared from Borassus bark, a low-cost source, by sulphuric acid activation, was tested for its ability to remove malachite green in aqueous solution. The parameters studied included contact time, initial dye concentration, carbon dose, pH, and temperature. The adsorption followed first order rate equation and the rate was mainly controlled by intra-particle diffusion. Freundlich and Langmuir isotherm models were applied to the equilibrium data. The adsorption capacities (Qm) obtained from the Langmuir isotherm plots were 20.70, 20.25, 19.76, and 19.34 mg/g at 30, 40, 50, and 600C, respectively, at an initial pH of 6.0. The temperature variation study showed that the malachite green adsorption was endothermic and spontaneous with increased randomness at the solid solution interface. Key words: activated carbon (BBC), malachite green (MG), adsorption isotherm, equilibrium, kinetic and thermodynamic parameters, intraparticle diffusion, regeneration pattern

*To whom correspondence should be addressed E-mail:[email protected] Paper Received December 2, 2007; Revised November 24, 2008; Accepted February 9, 2009

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The Arabian Journal for Science and Engineering, Volume 34, Number 2A

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ADSORPTION OF MALACHITE GREEN ONTO CARBON PREPARED FROM BORASSUS BARK

1. INTRODUCTION Activated carbon is widely used as an adsorbent due to its high adsorption capacity, high surface area, microporous structure, and high degree of surface respectively. The preparation and effective utilization of activated carbon generated from natural plant materials have attracted worldwide attention in view of the large disposal problem detrimental to the environment. Many investigators have studied the feasibility of using inexpensive alternative materials like pearl millet husk, date pits, saw, and buffing dust of the leather industry, coir pith, crude oil residue, tropical grass, olive stone, pine bark, wool waste, coconut shell, etc., as carbonaceous precursors for the preparation of activated carbons and for the removal of dyes from water and wastewater [1–5]. The present investigation is an attempt to explore the possibility of using Borassus bark carbon to remove malachite green dye in aqueous solution, since the raw material is harmless, cheaper, and plentiful. The present study reports the adsorption kinetics and thermodynamics of the chosen activated carbon for the adsorption of malachite green dye. 2. MATERIAL AND METHODS 2.1. Preparation of the Activated Carbon The dried Borassus bark was soaked in concentrated sulphuric acid at a weight ratio of 1:1 (w/v). Heating at 600qC for 12 hours in a furnace completed the carbonization and activation. The resulting carbon was washed with distilled water until a constant pH of the slurry was reached. Then the carbon was dried at 100qC for 4 hours in a hot air oven. The dried material was ground well to fine powder and sieved to 0.08mm. 2.2. Adsorption Experiments 2.2.1. Batch equilibration method The adsorption experiments were carried out in a batch process at 30, 40, 50, and 60˚ C. The known weight of activated carbon was added to 50 ml of the dye solutions with an initial concentration of 10 mg/L to 60 mg/L, which is prepared from 1000 mg/L of malachite green stock solution. The contents were shaken thoroughly using a mechanical shaker with a speed of 120 rpm. The residual solution was then filtered at preset time intervals and the concentration of the filtrate was measured. The effects of variables such as dosage of the adsorbent, initial concentration, contact time, initial pH, chloride ion, and temperature were studied thoroughly and reported in the results and discussion part. The physical properties of the prepared activated carbon were studied by standard procedures. The zero point charge and the surface functional groups of the activated carbon were studied by the following methods: Drift method. The zero point charge of the carbon (pHzpc) was measured using the pH drift method [4]. The pH of the solution was adjusted by using 0.01 M sodium hydroxide or hydrochloric acid. Nitrogen was bubbled through the solution at 250C to remove the dissolved carbon dioxide. 50 mg of the activated carbon was added to 50 ml of the solution. After stabilization, the final pH was recorded. The graphs of final pH versus initial pH were used to determine the zero point charge of the activated carbon. Titration studies. According to Boehm [4], only strong acidic carboxylic acid groups are neutralized by sodium bicarbonate, whereas those neutralized by sodium carbonate are thought to be lactones, lactol, and carboxyl group. The weakly acidic phenolic groups only react with strong alkali, such as sodium hydroxide. Therefore, by selective neutralization using bases of different strength, the surface acidic functional group in carbon can be characterized both quantitatively and qualitatively. Neutralization with hydrochloric acid characterizes the amount of surface basic groups that are, for example, pyrones and chromenes. The basic properties have been described to surface basic groups and the pi electron system of carbon basal planes. The results indicate that the activated carbon used may possess an acidic oxygen functional group on their surface, and this is supported well by their respective zero point charge values. Desorption studies. Desorption studies help to elucidate the nature of adsorption and recycling of the spent adsorbent and the dye. The effect of various reagents used for desorption are studied. 3. RESULTS AND DISCUSSIONS 3.1. Characteristics of the Adsorbent The characteristics of the adsorbent studied from standard procedures, drift method, and titration studies have been listed in Table 1. 32


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Table 1. Characteristics of the Borassus Bark Carbon (BBC) Properties

BBC

Particle size (mm)

0.08

Density (g/cc)

0.4243

Moisture content (%)

1.25

Loss on ignition (%)

78

Acid insoluble matter (%)

2

Water soluble matter (%)

0.13

pH of aqueous solution

6.45

pHzpc

5.82

Surface groups (m equiv/g) i) Carboxylic acid

0.223

ii) Lactone, lactol

0.039

iii) Phenolic

0.051

iv) Basic (pyrones and chromenes)

0.026

3.2. Effect of Contact Time and Initial Dye Concentration The experimental results of adsorptions at various concentrations (10, 20, 30, 40, 50, and 60 mg/L) collected in Table 2 reveals that percent adsorption decreased with increases in initial dye concentration, but the actual amount of dye adsorbed per unit mass of carbon increased with increases in dye concentration. This means that the adsorption is highly dependent on initial concentration of dye. At lower concentration, the ratio of the initial number of dye molecules to the available surface area is low. Subsequently, the fractional adsorption become independent of initial concentration. However, at high concentration the available sites of adsorption become fewer and hence the percentage removal of dye is dependent upon initial concentration [5, 6]. Equilibriums have been established at 40 minutes for all concentrations. Figure 1 reveals that the curves are single, smooth, and continuous, leading to saturation, suggesting the possible monolayer coverage of the dyes on the carbon surface. 75

70

% removal of MG

65

60

55

50

45 10

20

30

40

50

60

Contact time in min Figure 1. Effect of contact time on the adsorption of malachite green onto BBC [MG]=40 mg/L; pH=6.5; Dose= 100 mg/50 ml

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33


34


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3.3. Effect of Carbon Dose The adsorption of the malachite green dye on carbon was studied by varying the carbon dose (25–250 mg/50ml) for 40 mg/L of dye concentration. The percentage of adsorption increased with increases in the carbon concentration (Figure 2). This was attributed to increased carbon surface area and the availability of more adsorption sites [5, 6]. Hence, all studies were carried out with 100 mg of adsorbent /50 ml of the varying adsorbate solutions.

90

% removal of MG

80

70

60

50

40

30 0

50

100

150

200

250

Adsorbent dose in mg Figure 2. Effect of adsorbent dose on the adsorption of malachite green onto BBC [MG=40 mg/L; pH=6.5; Contact time=60 min

3.4. Adsorption Isotherm The experimental data are analyzed by the linear form of the Langmuir and Freundlich isotherms [7,8]. The equation for Langmuir isotherm C e/Q e = 1/Qmb + Ce /Qm where Ce is the equilibrium concentration (mg/L), Qe is the amount adsorbed at equilibrium (mg/g), and Qm and b are Langmuir constants related to adsorption efficiency and energy of adsorption, respectively. The linear plots of Ce/Qe versus Ce suggest the applicability of the Langmuir isotherms (Figure 3). The values of Qm and b were determined from slope and intercepts of the plots and are presented in Table 3. From the results, it is clear that the value of adsorption efficiency Qm and adsorption energy b of the carbon decreases on increasing the temperature which suggests that the maximum adsorption corresponds to a saturated monolayer of adsorbate molecules on adsorbent surface and the endothermic nature of adsorption [9–11]. The favorability of the adsorption process was calculated from dimensionless separation factor (RL), which was found between 0 and 1 and which confirms the ongoing adsorption of malachite green [12]. The values are shown in Table 4. The Freundlich equation was employed for the adsorption of malachite green dye on the adsorbent. The Freundlich isotherm was represented by log Qe = log Kf + 1/n log Ce where Qe is the amount of malachite green dye adsorbed (mg/g), Ce is the equilibrium concentration of dye in solution (mg/L), and Kf and n are constants incorporating the factors affecting the adsorption capacity and intensity of adsorption, respectively. Linear plots of log Qe versus log Ce shows that the adsorption of malachite green dye obeys the Freundlich adsorption isotherm (Figure 4). The values of Kf and n given in Table 5 show that the increase of negative charges on the adsorbent surface makes electrostatic force like Vanderwaal’s between the carbon surface and dye ion. The molecular weight and size either limit or increase the possibility of the adsorption of the dye onto adsorbent. However, the values clearly show the dominance in adsorption capacity. The intensity of adsorption is an indication of the bond energies between dye and adsorbent, and the possibility of slight chemisorptions rather than physisorption [10,11]. However, the multilayer adsorption of malachite green through the percolation process may be possible. The values of n are less than one, indicating the physisorption is much more favorable [12].

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1.6

1.4

1.2

1.0

Ce/Qe

0

30 C 0.8

0

40 C 0

50 C

0.6

0

60 C

0.4

0.2

0.0 0

5

10

15

20

25

Ce Figure 3. Langmuir adsorption isotherm for the adsorption of MG onto BBC

Table 3. Langmuir Isotherm Results Dye

Temp

Statistical parameters/constants

C

r2

Qm

b

30

0.9974

20.70

0.1792

40

0.9981

20.25

0.2096

50

0.9928

19.76

0.2020

60

0.9970

19.34

0.2347

0

MG

Table 4. Dimensionless Separation Factor (RL) Temperature (0C) [MG]0

30

40

50

60

10

0.357

0.322

0.333

0.303

20

0.217

0.192

0.200

0.178

30

0.156

0.136

0.142

0.126

40

0.121

0.106

0.111

0.098

50

0.100

0.086

0.090

0.080

60

0.084

0.073

0.076

0.067

(mg/L)

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1.6 1.4 1.2 1.0

logQe

0.8 0.6 0

30 C 0.4

0

40 C 0

50 C

0.2

0

60 C

0.0 -0.2 0.6

0.7

0.8

0.9

1.0

1.1

1.2

1.3

logCe Figure 4. Freundlich adsorption isotherm for the adsorption of malachith green onto BBC

Table 5. Freundlich Isotherm Results Dye

Temp

MG

Statistical Parameters/Constants

C

2

r

Kf

n

30

0.9274

1.7209

0.5428

40

0.9728

1.6113

0.4770

50

0.9771

1.5517

0.4393

60

0.9827

1.4838

0.3946

0

3.5. Effect of Temperature The adsorption capacity of the carbon increased with increase of the temperature in the system from 30° to 60°C. Thermodynamic parameters such as change in free energy (¨G°) (kJ/mol), enthalpy (¨H°) (kJ/mol) and entropy (¨S°) (J/K/mol) were determined using the following equations K0 = Csolid/Cliquid ¨G° = íRT lnKO ¨G° = ¨H°íT¨S° lnKo=¨G°/(RT)= ¨S°/ (R) í ¨H°/(RT) logK0 = ¨S°/ (2.303R) í ¨H°/(2.303RT) where Ko is the equilibrium constant, Csolid is the solid phase concentration at equilibrium (mg/L), Cliquid is the liquid phase concentration at equilibrium (mg/L), T is the temperature in Kelvin, and R is the gas constant. The ¨H° and ¨S° values obtained from the slope and intercept of Van’t Hoff plots have been presented in Table 6. The values ¨H° in the range of 1 to 93 kJ/mol indicate the physisorption. From the results, we could make out that physisorption is much more favorable for the adsorption of malachite green. The positive values of ¨H° show the endothermic nature of adsorption which governs the possibility of physical adsorption [11, 13]. Because in the case of physical adsorption, while increasing the temperature of the system, the extent of dye adsorption increases, there is no possibility of chemisorption [13]. The low ¨H° value depicts dye is physisorbed onto adsorbent BBC.

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The negative values of ¨G° (Table 6) show that the adsorption is highly favorable and spontaneous. The positive values of ¨S° (Table 6) show the increased disorder and randomness at the solid solution interface of malachite green with BBC adsorbent. The enhancement of adsorption capacity of the activated carbon at higher temperatures was attributed to the enlargement of pore size and activation of the adsorbent surface [12–14]. Table 6. Equilibrium Constant and Thermodynamic Parameters for the Adsorption of Dyes onto Carbon ¨Go

K0

[MG]0

¨Ho

¨So

Temperature (0C) 30o

40o

50o

60o

30o

40o

50o

60o

10

5.35

6.55

8.32

11.45

-4.22

-4.89

-5.69

-6.75

20.81

82.31

20

4.72

4.98

5.71

6.71

-3.91

-4.18

-4.68

-5.27

9.78

44.87

30

3.46

3.62

3.91

4.12

-3.12

-3.34

-3.66

-3.92

5.05

26.92

40

2.46

2.55

2.64

2.73

-2.27

-2.43

-2.61

-2.78

2.87

16.95

50

1.59

1.62

1.65

1.69

-1.19

-1.27

-1.36

-1.45

1.70

9.46

60

1.36

1.38

1.41

1.43

-0.75

-0.84

-0.92

-0.99

1.57

7.68

3.6. Kinetics of Adsorption The kinetics of sorption reveals the solute uptake rate of the reaction. It is one of the important characteristics in defining the efficiency of adsorption. In the present study, the kinetics of the dye removal were carried out to understand the behavior of the chosen carbon. The adsorption of the malachite green dye from an aqueous solution follows reversible first order kinetics, when a single species is considered on a heterogeneous surface. The heterogeneous equilibrium between the dye solutions and the activated carbon is expressed as k1 A

B k2 where k1 is the forward rate constant and k2 is the backward rate constant. A represents dye remaining in the aqueous solution and B represents dye adsorbed on the surface of activated carbon. The equilibrium constant (K0) is the ratio of the concentration adsorbate in adsorbent and in aqueous solution (K0=k1/k2). In order to study the kinetics of the adsorption process, the following kinetic equation proposed by Natarajan and Khalaf, as cited in literature, has been employed [1]. log C0/Ct=(Kad/2.303)t where C0 and Ct are the concentration of the dye (in mg/L) at time zero and at time t, respectively. The rate constants (Kad) for the adsorption processes have been calculated from the slope of the linear plots of log C0/Ct versus t for different concentrations and temperatures. The determination of rate constants as described in literature is given by Kad=k1+k2=k1+(k1/K0)=k1[1+1/K0] The overall rate constant kad for the adsorption of dye at different temperatures is calculated from the slopes of the linear Natarajan-Khalaf plots. The rate constant values collected in Table 7 show that the rate constant (kad) increases with increase in temperature, suggesting that the adsorption process is endothermic in nature. The rate constants for the forward and reverse processes collected in Table 7 indicate that the forward rate constant is much higher than the reverse rate constant at all initial concentrations and temperatures, suggesting that the rate of adsorption is clearly dominant [1,11,13]. 3.7. Intra-particle Diffusion The intra-particle diffusion is the most commonly used technique for identifying the adsorption mechanism. Previous studies by various researchers show that the plot of Qt versus t0.5 represents multi-linearity, which characterizes the two or more steps involved in the sorption process. According to Weber and Morris, an intraparticle diffusion coefficient Kp is defined by the equation: Kp=Q/t0.5+C

38


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The Kp(mg/g min0.5) value of malachite green adsorption is obtained from the slope of the plot of Qt(mg/g) versus t0.5. The two phases in the intraparticle diffusion plot (Figure 5) suggest that the sorption process was succeeded by surface sorption and intraparticle diffusion [15, 16]. The initial curved portion of the plot indicates the boundary layer effect, while the second linear portion is due to intraparticle diffusion. The slope of the second linear portion of the plot gives intraparticle diffusion parameter Kp(mg/g min0.5). On the other hand, the intercept of the plot reflects the boundary layer effect. The larger the intercept, the greater is the contribution of the surface sorption in the rate limiting step. The calculated intraparticle diffusion coefficient Kp values are 0.146, 0.146, 0.147, 0.148, and 0.149mg/g min0.5 for initial dye concentrations of 10, 20, 30, 40, 50, and 60 mg/L at 300C. 4.3

4.2

Qt

4.1

4.0

3.9

3.8

3.7

3

4

5

6

7

8

Time 0.5 in minutes Figure 5. Intraparticle diffusion effect on the adsorption of malachite green onto BBC [MG]=10 mg/L; pH=6.5; Dose= 100 mg/50 ml

3.8. Effect of pH The pH is one of the most important parameters in controlling the adsorption process. The pH of the solution was controlled by the addition of HCl or NaOH. The effect of pH on the adsorption of malachite green ions on BBC is shown in Figure 6. The uptake of malachite green ions was minimum at pH 7.5 and maximum at pH 5.75. However, when the pH of the solution was increased (more than pH 7), the uptake of malachite green ions was increased. It appears that a change in pH of the solution results in the formation of different ionic species, and a different carbon surface charge. When the pH value is lower than 6, the malachite green ions are able to enter into the pore structure. As the pH value is increased to above 7, the zwitter ions form of malachite green in water may raise the aggregation of malachite green to form a bigger molecular form (dimer) and become unable to enter into the pore structure of the carbon surface. The greater aggregation of the zwitter ionic form is due to the attractive electrostatic interaction between the ionic groups of the monomer. At pH value higher than 9, the existance of BBC surface OH- creates a competition between ionic dye and decreases the aggregation of malachite green. It also causes an increase in the adsorption of malachite green ions on the carbon surface. The effect of the charge on the carbon surface, and the electrostatic force of attraction and repulsion between the carbon surface and the malachite green ions, cannot explain the outcome [1,12,13,17]. 3.9. Effect of the Ionic Strength The effect of sodium chloride on the adsorption of malachite green on BBC is shown in Figure 7. The low concentrate NaCl solution had little influence on the adsorption capacity. When the concentration of NaCl increases, the ionic strength is raised. At higher ionic strength, the adsorption of malachite green will be high owing to the partial neutralization of the positive charge on the carbon surface and a consequent compression of the electrical double layer by the Cl- anion. The chloride ion also enhances adsorption of malachite green ion by pairing their charges, and hence reducing the repulsion between the malachite green molecules adsorbed on the surface. This initiates carbon to adsorb more positive malachite green ions [1, 17].

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80 78 76

% removal of MG

74 72 70 68 66 64 62 60 58 2

4

6

8

10

12

Initial pH Figure 6. Effect of initial pH on the removal of malachite green by BBC [MG] =40 mg/L; Dose=100mg/50 ml; Contact time=60min 79

78

% removal of MG

77

76

75

74

73

72

0

20

40

60

80

100

Concentration of chloride ion in mg/L Figure 7. Effect of ionic strength on the adsorption of malachite green into BBC [MG] =40 mg/L; Dose=100 mg/50 ml; Contact time=60min

3.10. Desorption Studies Desorption studies help to elucidate the nature of adsorption and recycling of the spent adsorbent. If the adsorbed dyes can be desorbed using neutral pH water, then the attachment of the dye by the adsorbent will be weak bonds. If sulphuric acid or alkaline water desorp the dye then the adsorption will be through ion exchange. If organic acids, such as acetic acid can desorp the dye, then the dye has been held by the adsorbent through chemisorption. The effect of various reagents used for desorption studies indicate that hydrochloric acid is a better reagent for desorption. The desorption of malachite green dye by dilute mineral acid indicates that the dyes were adsorbed onto the activated carbon through physisorption [12, 18].

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4. CONCLUSIONS The experimental data correlated reasonably well by the Langmuir and Freundlich adsorption isotherms and the isotherm parameters were calculated. The low as well as high pH value paves the way to the optimum amount of adsorption of the dye. The adsorption of malachite green is increased with increasing ionic strength and temperature. The dimensionless separation factor (RL) shows that the activated carbon could be used for the removal of malachite green from aqueous solution. The values of ¨H°, ¨S° and ¨G° show that the carbon employed has considerable potential to remove malachite green dye from aqueous solution. ACKNOWLEDGMENT The authors acknowledge sincere thanks to Mrs. Mala Arivoli, The Principal, H H The Rajah’s College, Pudukkottai, and The Director of Collegiate Education, Chennai for carrying out this research work successfully. REFERENCES

42

[1]

S. Arivoli, “Kinetic and Thermodynamic Studies on the Adsorption of Some Metal Ions and Dyes onto Low Cost Activated Carbons”, Ph D. Thesis, Gandhigram Rural University, Gandhigram, 2007.

[2]

G. Sekaran, K. A. Shanmugasundaram, M. Mariappan, and K. V. Raghavan, “Adsorption of Dyes by Buffing Dust of Leather Industry”, Indian J Chem Technol, (2)1995, p. 311.

[3]

K. Selvarani, “Studies on Low Cost Adsorbents for the Removal of Organic and Inorganics from Water”, Ph D. Thesis, Regional Engineering College, Thiruchirapalli, 2000.

[4]

Y. F. Jia and K. K. Thomas “Adsorption of Metal Ion on Nitrogen Surface Functional Groups in Activated Carbon, Langmuir, (18)2002, pp. 470–478.

[5]

C. Namasivayam, N. Muniasamy, K. Gayathri, M. Rani, and K. Renganathan, “Removal of Dyes from Aqueous Solution by Cellulosic Waste Orange Peel”, Biores Technol, (57)1996, p. 37.

[6]

C. Namasivayam and R. T. Yamuna, “Adsorption of Direct Red by Biogas Residual Slurry”, Environ Pollut, (89)1995, p. 1.

[7]

I. Langmuir, “Adsorption of Gases on Plane Surfaces of Glass, Mica and Platinum”, J Amer Chem Soc, (40)1918, p. 1361.

[8]

H. Freundlich, “Adsorption in Solutions”, Phys Chemie, (57)1906, p. 384.

[9]

D. G. Krishna and G. Bhattacharyya, “Adsorption of Methylene Blue on Kaolinite”, Appl Clay Sci, (20)2002, p. 295.

[10]

S. Arivoli, M. Viji Jain, and T. Rajachandrasekar, “Cobalt Adsorption on a Low Cost Carbon-Kinetic, Equilibrium and Mechanistic Studies”, Mat Sci Res India, (3)2006, pp. 241–250.

[11]

S. Arivoli and M. Hema, “Comparative Study on the Adsorption Kinetics and Thermodynamics of Dyes onto Acid Activated Low Cost Carbon”, Intern J Phys Sci., (2)2007, pp. 10–17.

[12]

S. Arivoli, B. R. Venkatraman, T. Rajachandrasekar, and M. Hema, “Adsorption of Ferrous Ion from Aqueous Solution by Low Cost Activated Carbon Obtained from Natural Plant Material”, Res J Chem Environ. (17)2007, pp. 70–78.

[13]

S. Arivoli, K. Kalpana, R. Sudha, and T. Rajachandrasekar, “Comparative Study on the Adsorption Kinetics and Thermodynamics of Metal Ions onto Acid Activated Low Cost Carbon”, E J Chem, (4)2007, pp. 238–254.

[14]

Renmin Gong, Yingzhi Sun, Jian Chen, Huijun Liu, and Chao Yang, “Effect of Chemical Modification on Dye Adsorption Capacity of Peanut Hull”, Dyes and Pigments, (67)2005, p. 179.

[15]

V. Vadivelan and K. Vasanthkumar, “Equilibrium, Kinetics, Mechanism and Process Design for the Sorption of Methylene Blue onto Rice Husk”, J Colloid Interf Sci, (286)2005, p. 91.

[16]

W. J. Weber, “Principle and Application of Water Chemistry”, ed. S. D. Faust and J. V. Hunter. New York: Wiley, 1967.

[17]

Yupeng Guo, Jingzhu Zhao, Hui Zhang, Shaofeng Yang, Zichen Wang, and Hongding Xu, “Use of Rice Husk Based Porous Carbon for the Adsorption Rhodamine B from Aqueous Solution”, Dyes and Pigments, (66)2005, pp. 123–128.

[18]

M. K. Sreedhar and T. S. Anirudhan, “Mercury (II) Adsorption of Desorption Characteristics of Coconut Husk Based Carbon-Kinetics and Self Diffusion”, Indian J Environ Protect, (19)1999, p. 8.


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