Sorption Kinetics, Isotherm and Thermodynamic Modeling of Defluoridation of Ground Water Using Natural Adsorbents

Aamna Balouch, Mazhar Kolachi, Farah Naz Talpur, Humaira Khan, Muhammad I. Bhanger

Dr. M. A. Kazi Institute of Chemistry, University of Sindh, Jamshore, Pakistan.
Environmental Engineering & Management, Mehran University of Engineering & Technology, Jamshoro, Pakistan.
National Center of Excellence in Analytical Chemistry, University of Sindh, Jamshoro, Pakistan.

DOI: 10.4236/ajac.2013.45028                

Abstract

The aim of study is to investigate the removal ability of some natural adsorbents for fluoride ion from aqueous solution. The batch dynamic adsorption method was carried out at neutral pH as the functions of contact time, adsorbent dose, adsorbate concentration, temperature and effect of co-anions, which are commonly present in water. The sorption kinetics and equilibrium adsorption isotherms of fluoride on natural adsorbing materials had been investigated at afore-mentioned optimized. Equilibrium adsorption isotherms, viz., Freundlich and Langmuir isotherms were investigated. Lagergren and Morris-Weber kinetic equations were employed to find the rate constants. The negative enthalpy ΔH = -46.54 KJ·mol^-1 and Gibbs free energy calculated was ΔG_288-333—(2.07785, 3.08966, 4.1064, 4.90716 and 5.38036 KJ·mol^-1) respectively, envisage exothermic and spontaneous nature of sorption.

Keywords

Isotherm; Kinetics and Thermodynamic Modeling; Ground Water; Natural Adsorbent; Defluoridation

1. Introduction

Weathering and dissolution of minerals, emitted from volcanoes and marine aerosols are the natural sources of releasing fluorides into the environment [1-3]. Many anthropogenic activities such as combustion and process waters and waste from various industrial processes, including steel manufacture, primary aluminum, copper and nickel production, phosphate ore processing, phosphate fertilizer production and use, glass, brick and ceramic manufacturing and glue and adhesive production are also the reason of fluoride contamination [2,4-5].

Increased fluoride levels in drinking water have become a critical health issue in many countries due to prevailing skeletal and dental fluorosis [6-8]. Though fluoride is an essential constituent for both humans and animals, it can be detrimental to human health depending on its level in drinking water [9]. Beneficial level of fluoride to health is <1.5 mg/L as recommended by WHO [10-12]. In Pakistan, the problem is common in Thar Desert, the ground water is highly contaminated and people are facing many diseases caused by high fluoride concentration [8,13].

Several studies have been conducted to reduce the concentration of F⁻ ion in drinking water for the benefits of common man. Adsorption is one of the significant techniques in which fluoride adsorbed onto a membrane, or a fixed bed packed with resin or other mineral particles. Many natural and low cost materials such as red mud [14-15], zirconium impregnated coconut shell carbon [16-17], cashew nut shell carbon [18], ground nut shell carbon [19] and clays [20-21] have been used as adsorbents for fluoride removal from drinking water. Recently, amorphous alumina supported on carbon nanotubes [22], natural zeolites [23] chemically activated carbon [24] aligned carbon nanotubes [25], ion exchange polymeric fiber [26], double hydrous oxide of Al and Fe (Fe₂O₃Al₂O₃·XH₂O) [27] bone charcoal [28] and activated alumina [29] have been assayed for removing fluoride from drinking water as well as industrial wastewater.

This paper concentrates on investigating low cost material for fluoride sorption which can effectively remove fluoride from aqueous solutions at a relatively low level. To overcome these problems and enhance the defluoradation capacity this study was carried out with the natural adsorbents (coal, brick powder, saw dust) to treat the contaminated water. These adsorbents are cheaper, abundant and easily available in huge amount.

This study leads to the assumption that fluoride deposition occurs by the forces of adsorption over the surface of the adsorbents; also the dynamics and kinetics of the adsorption process are discussed.

2. Experimental

2.1. Apparatus and Materials

781-pH/Ion meter (Ω Metrohm, Herisau, Switzerland) with Ag, Ag/Cl reference electrode 6.0726.100 (Ω Metrohm) and fluoride electrode 6.0502.150 (Ω Metrohm) were used for the quantitative analysis of Fluoride and also for the pH measurement with pH electrode. Gallenkamp thermostated automatic shaker model BKS-305- 010, UK was used for the batch experiments at ambient temperature (ca. 25˚C).

Ion-Chromatography (I.C) (Ω Metrohm, Switzerland) instrument 861 Advance Compact with 833 IC liquid handling unit equipped with self-regenerating suppressor consists of a double gradient peristaltic pump with a conductivity detector was used for validation and correlation of results obtained from 781-pH/Ion meter for the quantification of fluoride . The anion column (4.0 × 250 mm²) METROSEP A SUPP 4 - 250 (6.1006.430) and Carbonate/bicarbonate buffer mobile phase was used in ion chromatographic study. Whatman no. 42, filter papers were used for all filtration procedures.

All analytical reagent grade chemicals are obtained from the indicated companies and used without any further purification. CDTA (cyclohexylenedinitrilotetraacetate) (Merck, Germany) Anhydrous Sodium fluoride, sodium hydroxide, sodium chloride and acetic acid (ethanoic acid) from (Aldrich Chemical Co.). The adsorbents (coal, brick powder and saw dust) were collected from local area of Hyderabad (Pakistan).

2.2. Preparation of Stock Solutions Specifications

Ultra pure water (conductivity 0.050 μS·cm⁻¹), obtained from a Milli-Q purification system (PURELAB Prima 7 BP, PURELAB Classic UV) was used for the preparation of all samples, standards and blanks. All glassware (pipettes, volumetric flasks, etc.) employed in the preparation of the stock solutions as well as working solutions were all initially cleaned by soaking in acidified (6 M nitric acid) water or in acidified (HNO₃ 1.0 M) solution of potassium permanganate, then thoroughly rinsed with deionized water and then acetone. The glassware was then dried for at least one hour in an oven at 120˚C.

The 1000 mg/L of fluoride stock solution was prepared by liquefying appropriate amount of anhydrous NaF in 100 ml volumetric flask and then volume make up to the mark with Ultra pure water.

The adsorbents were first washed with distilled water followed by Milli Q Ultra pure water then dried oven at 105˚C for 12 h. After drying adsorbents were passed through sieve to obtain the required particle size for the present study.

No any impregnation or activation process was done before using the above adsorbents as well as these are easily available in rural area decreasing its cost as compare to previous reported materials.

A total ionic strength adjustment buffer (TISAB) buffer solution prepared for potentiometric measurement of fluoride by ion selective electrodes.

2.3. Sorption Procedure

The batch technique was used to examine the %sorption of fluoride onto natural adsorbents at ambient temperature. Sorption of fluoride carried out by taking 10 mL of aqueous solution of fluoride (5.0 mg/L) was added to an Erlenmeyer flask containing 0.2 g of each dried and sieved adsorbent. The mixture was then shaken for a specified time (10 - 100 min) and temperature (25˚C) to allow adsorption of fluoride ion. The Erlenmeyer flasks were removed from shaker and allowed to stand for 2 min after attaining the required contact time. Then the mixture was filtered using then remainder was determined by TISAB method using fluoride ion selective electrode.

2.4. Data Analysis

The adsorption behavior of fluoride ion on the adsorbents e.g. coal, brick powder and saw dust surface was investigated using batch equilibrium experiments.

The sorbate concentration of sorbate on sorbent surface was calculated by the difference in the fluoride ion meter response (mg/L) before and after shaking. The distribution ratio R_d and %sorption of fluoride were calculated by using the following equations:

(1)

where C_i and C_e is the initial and equilibrium concentrations (mg·L⁻¹) respectively.

All the experiments were performed in triplicate. The linear regression computer program with one independent variable was used for slope and statistical analyses of the data.

3. Result and Discussion

Sorption is a surface phenomenon and is affected significantly by physical and chemical characteristics of sorbent and sorbate. Sorption studies on natural adsorbent was carried out by optimizing various parameters, i.e. effect of agitation time, effect of shaking speed, amount of sorbent, pH, concentration of sorbate and temperature.

3.1. Effect of Agitation Time and Speed (rpm)

Effect of shaking time on %sorption of fluoride onto mixture of adsorbents was studied over an agitation time of 10 - 100 min, using 0.2 g of each adsorbent temperature 25˚C and 100 rpm shaking speed. The results are shown in Figure 1. Percent adsorption increases from 60% to 90% at contact time is increased.

Sorption of fluoride as a function of shaking speed was also studied in the range of 25 - 150 rpm. It was found that %sorption increases with increasing shaking speed and attains a maximum sorption at 100 rpm and then %sorption declines with increasing shaking speed as shown in Figure 2. Therefore for further studies 100 rpm shaking speed was employed.

3.2. Effect of Adsorbent Dose

The effect of adsorbent dose on the removal of fluoride was studied by using different grams of adsorbent at 5.0

Figure 1. Percentage removal of Fluoride concentration as a contact time for the adsorbent (initial concentration = 5.0 mg/L, adsorbent dose = 1.0 g and pH 7.0).

Figure 2. Percentage removal of Fluoride as a function of Shaking speed (initial concentration = 5.0 mg/L, reaction time = 30 min, and pH 7.0, Adsorbent dose 1.0 g).

mg/L fixed fluoride concentration. As shown in Figure 3, the fluoride concentration is decreases as the adsorbent dose enhanced. It is manifest that the adsorption process is very fast and most of the fluoride adsorbed within first 10 min and the equilibrium reached within 40 mints. At the high absorbent doses (2.0 g) equilibrium requires shorter time (20 min) and lower absorbent doses (0.1 g) needs longer equilibrium time (40 min). Therefore equilibration time of 30 mints was chosen to conduct further experiments at fixed adsorbent dose.

3.3. Effect of pH

The influence of pH on the fluoride removal efficiency and capacity of the adsorbent were carried out for each adsorbent separately and also in mixture. Figure 4 shows adsorption capacity of untreated adsorbent at different fluoride concentration within the pH range of 4 - 9 in mixture of all adsorbents. Sorption % is achieved about 80% - 90% at pH 5 - 7 and due to better efficiency at pH 7 further study was carried out in neutral pH.

3.4. Isotherm Studies

The sorption isotherms express the specific relation be-

Figure 3. Percentage removal of Fluoride concentration as a function of adsorbent dose (initial concentration = 5.0 mg/L, reaction time = 30 min, and pH 7.0).

Figure 4. Percentage removal of Fluoride concentration as a function of pH for the adsorbent (initial concentration = 5.0 mg/L, reaction time = 30 min, and adsorbent dose = 2 gm).

tween the concentration of sorbate and its degree of accumulation onto sorbent surface at constant temperature. The Langmuir and Freundlich models are the simplest and most commonly used isotherms to represent the sorption of components from a liquid phase onto a solid phase [30].

The sorption capacities of coal, brick powder and saw dust for fluoride have been evaluated using different isotherms, namely Freundlich, Langmuir. Table 1 shows the comparison of Freundlich and Langmuir isotherm model.

3.4.1. Freundlich Sorption Isotherm

Freundlich isotherm gives the relationship between equilibrium liquid and solid phase capacity based on multilayer adsorption (heterogeneous surface). This isotherm is derived from the assumption that the adsorption sites are distributed exponentially with respect to heat of adsorption and given by [31] experimental data well on a phenomenological basis. The linearized form of Freundlich isotherm is tested in the following form:

           [31] (2)

where 1/n is a characteristic constant related to sorption intensity, C_ads is the sorbed concentration of sorbate onto sorbent (mol·g⁻¹), C_e represents equilibrium concentration of sorbate in solution, and C_m is the multilayer sorption capacity of sorbent (mol·g⁻¹). Logarithmic plot of sorbed and equilibrium concentration gives a straight line with coefficient of determination close to unity (0.95 ± 0.032). The values of 1/n (0.41 ± 0.01) and C_m (0.31 ± 0.001 mmol·g⁻¹) are derived from the slope and intercept of the straight line, respectively. Figure 5 shows Freundlich sorption isotherms of fluoride on adsorbents.

3.4.2. Langmuir Isotherm

Figure 6 shows the simplest theoretical model for monolayer sorption, i.e. Langmuir isotherm [32] of fluoride onto mixture of sorbents. The Langmuir model was originally developed to represent monolayer sorption on a set of distinct localized sorption sites. It gives uniform

Conflicts of Interest

The authors declare no conflicts of interest.

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