# Flotation and Sorptive-Flotation Methods for Removal of Lead Ions from Wastewater Using SDS as Surfactant and Barley Husk as Biosorbent

Authors: Ahmed A. Mohammed; Shahlaa E. Ebrahim; Abeer I. Alwared
Journal: Journal of Chemistry
 (2013)

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## Abstract

The removal of lead ions from simulated wastewater was investigated using flotation and sorptive-flotation methods. This was achieved by using sodium dodecyl sulfate (SDS) as surfactant and barley husk as biosorbent. Experiments were carried out to study the effect of various parameters such as pH (3, 5, and 8), initial lead ions concentration (25, 50, and 100) mg/L, flow rates (500, 1000, and 1500 mL/min), and SDS concentration (25, 50, and 100) mg/L. The results show that the removal efficiency was enhanced by about 10% when using sorptive-flotation compared with flotation only at the same conditions. Langmuir isotherm model withqm=12.7 and high determination coefficient equal to 0.988 was found to give the best fit to the experimental data compared to Freundlich isotherm model with k=3.49 and correlation coefficient equal to 0.94. Pseudo-first-order and pseudo-second-order kinetic models were studied and the results show that the adsorption data correlated with pseudo-first-order kinetic model with k1 equal to 0.122, and this is an indicator to the reversible interaction with equilibrium being established between liquid and solid waste.


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## Body

## 1. Introduction

Lead  is  a  natural  compound  that  exists  in  elemental, inorganic,  and  organic  forms.  Lead is present in trace amounts   in   all   soils,   water,   and   foods.   It   is   soft, malleable, blue-gray in color and is highly resistant to corrosion.   These   properties,   along    with   the   poor  ability  of  lead  to  conduct  heat  and  electricity,  probably contributed  to  its  use  in  mining,  smelting,  refining, battery manufacturing, soldering, electrical wiring, home demolition  and  construction,  painting,  ceramic  glazing, and the making of stained glass [1].The  heavy  metal  lead  is  among  the  most common  pollutants  found  in  industrial  effluents.  Even  at low concentration, this  metal can be  toxic to organisms, including humans, as it is extremely toxic and can damage the  nervous  system,  kidneys,  and  reproductive  system, particularly in children. Lead is known to have a toxic  effect  on  the  neuronal  system  and  the  function  of the brain cells [2, 3]. The US Environmental    Protection    Agency    (EPA) requires lead not to exceed 0.015 mg/L in drinking water [4]. Therefore, cost-effective   treatment   technologies   are needed to meet these requirements of recovery and/or removal of metal ions.Biosorption of heavy metals from aqueous solutions is a relatively new technology for the treatment of industrial wastewater. The major advantages of biosorption technology are its effectiveness in reducing the concentration of heavy metal ions to very low levels and the use of inexpensive biosorbent materials [5]. Biosorbents are prepared from the naturally abundant and/or waste biomass which has the ability to sequester heavy metals: these biosorbents are bacteria [6] and algae [7].A search for a low-cost and easily available adsorbent has led to the investigation of materials of agricultural and biological origin as potential metal sorbents [8]. Many materials which are cheap and readily available sources such as coal, coke, peat, wood, rice husk, or barley husk may be successfully employed for the removal of lead and other toxic heavy metals from aqueous solutions. The utilization of agricultural waste materials is increasingly becoming an important concern because these wastes represent unused resources and, in many cases, present serious disposal problems [9].Yadla et al. in 2012 [10] used fly ash as low cost and abundantly available adsorbent and they concluded that the percentage removal of lead from the aqueous solution amplifies with decrease in size of the adsorbent particles and is augmented with increase of the adsorbent. Percentage removal of lead from the aqueous solution is increased significantly with the decrease in acidity, and the increase in percentage adsorption is maximum between pH values 4 and 6 and decreased at pH above 7.Gupta et al. in 2010 [11] used the biosorbents (untreated and acid-treated algae) for removal of Ni(II) ions and they concluded that the proposed adsorbent is effective in terms of its performance compared with other biosorbents.Flotation as a separation process has recently received a considerable interest owing to its simplicity, rapidity, economy, good separation yields (recovery >95% for small impurity agent concentrations (10.6–10.2 mol/L), a large possibility of application for species having different nature and structure, flexibility and friability of equipment and processing for recovery purpose and production of more concentrated sludge, occupying smaller volumes [12, 13]. It is believed that  this  process  will  soon  be  incorporated  as  a  clean technology  to  treat  water  and  wastewater [14]. For the aforementioned reasons, a combination of adsorption and flotation into a unified operation termed sportive-flotation could be considered as a vital process.Stoica et al. in 2012 [15] used biosorption-flotation experiments in order to recover loaded mycelial penicillium waste from aqueous solution; the mycelial penicillium was loaded with   Cd(II) and Pb(II) resulted and then concluded that the efficiency being dependent on process optimal parameters.The aim of the present research is to investigate the lead ions removal by floatation and sorptive-floatation methods in batch process using barley husk as a biosorbent. The optimum weight of the barley husk was calculated through the equilibrium isotherm model.  The effect of pH, different lead ions concentrations, flow rate, and SDS concentration on the performance of floatation process was conducted.


## 2. Mathematical Models

### 2.1. Kinetics Models

There are various kinetic models used for evaluating the rate constant for floatation and biosorption of Pb(II) onto barley husk. The pseudo-first-order reaction was widely used for the adsorption of liquid/solid system. The linear form is generally expressed as follows [16]:
(1)ln(qe-qt)=lnqe-klt,
where qe (mg/g) and qt (mg/g) are the adsorption amount at equilibrium and at time t (min), respectively. kl (min−1) is the rate constant. While the pseudo-second order model is based on the assumption that the adsorption follows second order is chemisorptions. The linear form can be written as follows [17]:
(2)1qt=1k2qe21t+1qe,
where k2 (g/mg·min) is the rate constant of adsorption, qe is the amount of metal adsorbed at equilibrium (mg/g), and qt is the amount of metal adsorbed at time t (mg/g).


## 2.1. Kinetics Models

There are various kinetic models used for evaluating the rate constant for floatation and biosorption of Pb(II) onto barley husk. The pseudo-first-order reaction was widely used for the adsorption of liquid/solid system. The linear form is generally expressed as follows [16]:
(1)ln(qe-qt)=lnqe-klt,
where qe (mg/g) and qt (mg/g) are the adsorption amount at equilibrium and at time t (min), respectively. kl (min−1) is the rate constant. While the pseudo-second order model is based on the assumption that the adsorption follows second order is chemisorptions. The linear form can be written as follows [17]:
(2)1qt=1k2qe21t+1qe,
where k2 (g/mg·min) is the rate constant of adsorption, qe is the amount of metal adsorbed at equilibrium (mg/g), and qt is the amount of metal adsorbed at time t (mg/g).


## 3. Materials and Methods

Two types of experiments were carried out in this study:  floatation and sorptive-floatation.


### 3.1. Materials

Flotation. Sodium dodecyl sulfate (SDS, 99%) from Fisher Scientific was used as anionic collector; it is a white powder material with a chemical structure of C12H25OSO3Na, M.wt = 288.38 g/mole. Ethanol (C2H5OH) from Lancaster Synthesis was used as frother: Pb(NO3)2 purity = 99.5 %wt, M.wt = 207.2 g/mole.Sorptive-Flotation. Barley husk was used as biosorbent.Reagents. Hydraulic acid (HCL) and caustic soda (NaOH) were used for pH adjustments.


### 3.2. Methods

The foam flotation tests were carried out in a bubble column (acrylic) of 6 cm inside diameter and 120 cm in height. Figure1 shows a schematic diagram for the experimental apparatus. Air was supplied by the compressor (compressed at 1 bar up 7 bars) to the column through a pre-calibrated rotameter. Air that entered the column was dispersed as bubbles into liquid. Air distributor plate that has 25 holes with 0.05 cm diameter was used. The holes are arranged in the equilateral triangular pitch through the whole area which are located inside the column.  The column was operated at batch mode as far as the liquid phase and continuous flow with respect to air. The samples were drawn through tap from the column. Feed inter with different metal concentration (25 up to 100 ppm) was poured gently at the top of the column. At the same time, the column was pressurized so as not to weep the liquid through the holes.Figure 1
Schematic diagram of the experimental setup.Synthetic polluted water samples were prepared by dissolving Pb(NO3)2 in distilled water. Surfactants and ethanol were added to the synthetic polluted water. pH was adjusted to a desired value using HCL or NaOH.The barley husk was sieved on 28/32 mesh with geometric mean diameter of 0.5 mm. The required sieve fraction was removed and washed to remove fines from the crushed husk. The husk was placed in a clean baker filled with distilled water. Then it was stirred with a glass rod and allowed to settle for 5 minutes. The supernatant was poured off and new distilled water was added. This process was repeated twice until the supernatant was clear. The wet husk was dried in an oven at 100°C for 24 hours, after which the husk was kept in a desiccator for use.For the determination of adsorption isotherms, 250 ml flasks were filled with known concentration of solute and a known weight of barley husk. The flasks were placed on a shaker and were agitated continuously for 6 h at 25 ± 3°C. The concentration of lead(II) in the solution was determined using atomic absorption spectrophotometer device. The adsorbed amount is calculated by the following equation:(3)qe=V(Co-C)W,
where qe is the internal concentration of solute per unit weight of activated carbon, V is the volume of the container, W is the weight of the activated carbon, and Co and C are the initial and final solute concentrations. The amount of barley husk was calculated for the final equilibrium-related concentration of Ce/Co=0.05. Foam samples were taken at preset time intervals as 5, 10, 15, 20, 25, and 30 minutes. A port 0.45 m above the base was used for periodic sampling. About 3 mL of solution was drained from the port before withdrawing each sample; samples were withdrawn slowly to minimize entrainment of air bubbles. Between experiments, the column was cleaned using HCL and then rinsed three times with double-distilled water.


## 3.1. Materials

Flotation. Sodium dodecyl sulfate (SDS, 99%) from Fisher Scientific was used as anionic collector; it is a white powder material with a chemical structure of C12H25OSO3Na, M.wt = 288.38 g/mole. Ethanol (C2H5OH) from Lancaster Synthesis was used as frother: Pb(NO3)2 purity = 99.5 %wt, M.wt = 207.2 g/mole.Sorptive-Flotation. Barley husk was used as biosorbent.Reagents. Hydraulic acid (HCL) and caustic soda (NaOH) were used for pH adjustments.


## 3.2. Methods

The foam flotation tests were carried out in a bubble column (acrylic) of 6 cm inside diameter and 120 cm in height. Figure1 shows a schematic diagram for the experimental apparatus. Air was supplied by the compressor (compressed at 1 bar up 7 bars) to the column through a pre-calibrated rotameter. Air that entered the column was dispersed as bubbles into liquid. Air distributor plate that has 25 holes with 0.05 cm diameter was used. The holes are arranged in the equilateral triangular pitch through the whole area which are located inside the column.  The column was operated at batch mode as far as the liquid phase and continuous flow with respect to air. The samples were drawn through tap from the column. Feed inter with different metal concentration (25 up to 100 ppm) was poured gently at the top of the column. At the same time, the column was pressurized so as not to weep the liquid through the holes.Figure 1
Schematic diagram of the experimental setup.Synthetic polluted water samples were prepared by dissolving Pb(NO3)2 in distilled water. Surfactants and ethanol were added to the synthetic polluted water. pH was adjusted to a desired value using HCL or NaOH.The barley husk was sieved on 28/32 mesh with geometric mean diameter of 0.5 mm. The required sieve fraction was removed and washed to remove fines from the crushed husk. The husk was placed in a clean baker filled with distilled water. Then it was stirred with a glass rod and allowed to settle for 5 minutes. The supernatant was poured off and new distilled water was added. This process was repeated twice until the supernatant was clear. The wet husk was dried in an oven at 100°C for 24 hours, after which the husk was kept in a desiccator for use.For the determination of adsorption isotherms, 250 ml flasks were filled with known concentration of solute and a known weight of barley husk. The flasks were placed on a shaker and were agitated continuously for 6 h at 25 ± 3°C. The concentration of lead(II) in the solution was determined using atomic absorption spectrophotometer device. The adsorbed amount is calculated by the following equation:(3)qe=V(Co-C)W,
where qe is the internal concentration of solute per unit weight of activated carbon, V is the volume of the container, W is the weight of the activated carbon, and Co and C are the initial and final solute concentrations. The amount of barley husk was calculated for the final equilibrium-related concentration of Ce/Co=0.05. Foam samples were taken at preset time intervals as 5, 10, 15, 20, 25, and 30 minutes. A port 0.45 m above the base was used for periodic sampling. About 3 mL of solution was drained from the port before withdrawing each sample; samples were withdrawn slowly to minimize entrainment of air bubbles. Between experiments, the column was cleaned using HCL and then rinsed three times with double-distilled water.


## 4. Results and Discussion

### 4.1. Equilibrium Isotherm Results

The adsorption isotherms display a nonlinear dependence on the equilibrium concentration. The adsorption data for the system was fitted with two models. The determination coefficients are shown in Table1. This table indicates that the Langmuir model provides the best fit as judged by its correlation coefficient. Figure 2 represents the adsorption isotherm for lead ions onto barely husk.Table 1
Parameters of isotherm for Pb(II) and correlation coefficient for two models.
Model
Parameters
Pb(II)
Langmuir [18] qe=qmbCe(1+bCe)
q
m
12.7
b, l/mg
0.15
Correlation coefficient
0.988
Freundlich [19] qe=KFCe1/n
K
3.49
n
2.99
Correlation coefficient
0.94Figure 2
Adsorption isotherm for Pb(II) onto barley husks biosorbent.


### 4.2. Effect of pH

Generally, adsorption and flotation are sensitive to variations in the pH value of the medium, and knowing how the pH affects each system was a prerequisite to study employing these methods. Pb(II) is the dominant species below pH 5.5. Between pH 6 and 10, Pb(II) undergoes hydrolysis to Pb(OH)2. Above pH 9, solid lead hydroxide Pb(OH)2 is thermodynamically the most stable phase,  while Pb(OH)3 is predominant at pH above 11 [1].The influence of pH on the combined process (sorption and flotation) for the removal of Pb(II) was investigated in the absence and presence of barley husks;  Figure3 shows that the best  removal was at pH = 8 for floatation and for sorptive-floatation.Figure 3
Effect of pH on the removal of lead ions (Co=50 mg/L; SDS = 25 mg/L; Q=500 mL/min; barley husks = 20 gm/L).Inspection of the figure indicated that the use of barley husks as a sorbent increases the removal of Pb(II) as pH increased; a maximum removal efficiency value attained was 82% when using sorptive-flotation, while for flotation a maximum value was 78.4%.When the pH value increases, more metal binding occurs. pH variation can modify the speciation and the availability of the metallic elements in solution particularly at these properties related to hydrolytic reduction Kefala et al. [20].The chemical state of the biomass surface functional groups, which are responsible for metal binding, is also being influenced [20].


### 4.3. Effect of Flow Rate

The effect of gas flow rate (500, 1000, and 1500 mL/min) on the removal efficiency of lead in the bubble column was investigated as shown in Figure4; it can be seen from this figure that the removal rate was highly affected by the gas flow rate. As gas flow rate increases, the removal ratio increased too. This is because increased gas flow rate causes early bubble detachment, large fluid activities (stress) at the bottom section, and bubble coalescence and (mostly) breakup [21], This leads to a large number of small bubbles which increases surface area available for adsorption metal collector. However, higher gas flow rate results in decreasing the removal rate from the maximum due to the redispersion of some of the metal collector-precipitate product back in to the bulk solution.Figure 4
Effect of flow rate on the removal ratio of lead ions (50 = 100 mg/L; SDS = 25 mg/L barely husk = 20 gm/L).


### 4.4. Effect of Surfactant

In order to find a suitable concentration of SDS for removing Pb(II) ions from aqueous solutions, a series of experiment was conducted at pH 8 in the absence and presence of barley husk using different concentrations of SDS. The results obtained are presented in Figure5; it can be seen from this figure that the removal of Pb(II) increased when the concentration of SDS was 50 mg/L in the presence and absence of barley husk.Figure 5
Effect of SDS surfactant on the removal ratio of lead (Co=50 mg/L; pH = 8; Q=1000 mL/min; barley husk = 20 gm/L).Higher concentrations of the surfactant impaired flotation, where the poor flotation at high surfactant, concentration was caused the formation of air bubbles on the surface of stable, hydrated envelope of surfactant, or, perhaps, the formation of a hydrated micelle coating on the solid surface. As a result, the hydro-PHobicity of the resulting surface was not satisfactory for flotation. These results agree with [22].In the former case (flotation only), the Pb(II) may be completely adsorbed on the  particle, but the husk particle could not be floated because the amount of SDS  was insufficient; when the concentration increased to 100 gm/L, a nearly complete flotation of husk particle could be attained [23].


### 4.5. Lead Concentration

The removal rate of lead at various initial lead concentrations is shown in Figure6; from this figure, it can be seen that there is no significant difference in removal rate with increasing lead ions concentration from 50 mg/L to 100 mg/L. However, at low lead ions concentration (25 mg/L), the removal rate decreased because of large surfactant: lead ion ratio which cause competition, for bubble surface, between the metal-collector product and free collector ions [24].Figure 6
Effect of lead concentration on the removal efficiency at SDS = 25 mg/L; pH = 8;Q=1000 mL/min; barley husk = 20 gm/L).Also it can be seen from that figure that the removal percent increased when using sorptive flotation than flotation only.Under the examined conditions, the separation of biomass by floatation is a very rapid process, within 3 min. Almost 100% of biomass was separated and over 80% of lead ions removal was achieved in one stage. This is a specific advantage of the proposed sportive-flotation process, as it has been termed, because it is highly effective not only concerning lead ions removal, but also because the subsequent biomass separation process from the solution is fast and of relatively lower cost, due to necessary smaller residence time [20].


### 4.6. Kinetics

The amounts of barley husk used for adsorption of Pb(II) were calculated for final equilibrium-related concentration ofCe/Co=0.05. The Langmuir model constants were used with the mass balance in 1.5 liter of solution. The initial concentration of lead ions was 50 mg/L with the dose of husk being 20 gm.The rate constant using pseudo-first-order rate expression was obtained from the slope of the linear plots oflog(qe-qt) against t using (1). However, the rate constants for Pb(II) by using pseudo-second-order biosorption rate constant (k2) were determined from the slope and intercept of the plots of 1/q against 1/t using (2). The values of the rate constants with the corresponding correlation coefficients are presented in Table 2 for both kinetic models.Table 2
Pseudo-first and second-order rate constants for Pb(II) with correlation coefficients (R2).
Pseudo-first-order kinetic model
Pseudo-second-order kinetic model
K
1
(min−1)
R
2
K
2 (mg/g·min)
R
2
Pb(II)
0.122
0.936
1.6
0.506As can be seen from Table2, the correlation coefficients for the pseudo-first-order kinetic model for the various solutes were found to be higher than that for the pseudo-second-order kinetic.  Therefore, the pseudo first-order kinetics model can be used very well to find the rate constant.


## 4.1. Equilibrium Isotherm Results

The adsorption isotherms display a nonlinear dependence on the equilibrium concentration. The adsorption data for the system was fitted with two models. The determination coefficients are shown in Table1. This table indicates that the Langmuir model provides the best fit as judged by its correlation coefficient. Figure 2 represents the adsorption isotherm for lead ions onto barely husk.Table 1
Parameters of isotherm for Pb(II) and correlation coefficient for two models.
Model
Parameters
Pb(II)
Langmuir [18] qe=qmbCe(1+bCe)
q
m
12.7
b, l/mg
0.15
Correlation coefficient
0.988
Freundlich [19] qe=KFCe1/n
K
3.49
n
2.99
Correlation coefficient
0.94Figure 2
Adsorption isotherm for Pb(II) onto barley husks biosorbent.


## 4.2. Effect of pH

Generally, adsorption and flotation are sensitive to variations in the pH value of the medium, and knowing how the pH affects each system was a prerequisite to study employing these methods. Pb(II) is the dominant species below pH 5.5. Between pH 6 and 10, Pb(II) undergoes hydrolysis to Pb(OH)2. Above pH 9, solid lead hydroxide Pb(OH)2 is thermodynamically the most stable phase,  while Pb(OH)3 is predominant at pH above 11 [1].The influence of pH on the combined process (sorption and flotation) for the removal of Pb(II) was investigated in the absence and presence of barley husks;  Figure3 shows that the best  removal was at pH = 8 for floatation and for sorptive-floatation.Figure 3
Effect of pH on the removal of lead ions (Co=50 mg/L; SDS = 25 mg/L; Q=500 mL/min; barley husks = 20 gm/L).Inspection of the figure indicated that the use of barley husks as a sorbent increases the removal of Pb(II) as pH increased; a maximum removal efficiency value attained was 82% when using sorptive-flotation, while for flotation a maximum value was 78.4%.When the pH value increases, more metal binding occurs. pH variation can modify the speciation and the availability of the metallic elements in solution particularly at these properties related to hydrolytic reduction Kefala et al. [20].The chemical state of the biomass surface functional groups, which are responsible for metal binding, is also being influenced [20].


## 4.3. Effect of Flow Rate

The effect of gas flow rate (500, 1000, and 1500 mL/min) on the removal efficiency of lead in the bubble column was investigated as shown in Figure4; it can be seen from this figure that the removal rate was highly affected by the gas flow rate. As gas flow rate increases, the removal ratio increased too. This is because increased gas flow rate causes early bubble detachment, large fluid activities (stress) at the bottom section, and bubble coalescence and (mostly) breakup [21], This leads to a large number of small bubbles which increases surface area available for adsorption metal collector. However, higher gas flow rate results in decreasing the removal rate from the maximum due to the redispersion of some of the metal collector-precipitate product back in to the bulk solution.Figure 4
Effect of flow rate on the removal ratio of lead ions (50 = 100 mg/L; SDS = 25 mg/L barely husk = 20 gm/L).


## 4.4. Effect of Surfactant

In order to find a suitable concentration of SDS for removing Pb(II) ions from aqueous solutions, a series of experiment was conducted at pH 8 in the absence and presence of barley husk using different concentrations of SDS. The results obtained are presented in Figure5; it can be seen from this figure that the removal of Pb(II) increased when the concentration of SDS was 50 mg/L in the presence and absence of barley husk.Figure 5
Effect of SDS surfactant on the removal ratio of lead (Co=50 mg/L; pH = 8; Q=1000 mL/min; barley husk = 20 gm/L).Higher concentrations of the surfactant impaired flotation, where the poor flotation at high surfactant, concentration was caused the formation of air bubbles on the surface of stable, hydrated envelope of surfactant, or, perhaps, the formation of a hydrated micelle coating on the solid surface. As a result, the hydro-PHobicity of the resulting surface was not satisfactory for flotation. These results agree with [22].In the former case (flotation only), the Pb(II) may be completely adsorbed on the  particle, but the husk particle could not be floated because the amount of SDS  was insufficient; when the concentration increased to 100 gm/L, a nearly complete flotation of husk particle could be attained [23].


## 4.5. Lead Concentration

The removal rate of lead at various initial lead concentrations is shown in Figure6; from this figure, it can be seen that there is no significant difference in removal rate with increasing lead ions concentration from 50 mg/L to 100 mg/L. However, at low lead ions concentration (25 mg/L), the removal rate decreased because of large surfactant: lead ion ratio which cause competition, for bubble surface, between the metal-collector product and free collector ions [24].Figure 6
Effect of lead concentration on the removal efficiency at SDS = 25 mg/L; pH = 8;Q=1000 mL/min; barley husk = 20 gm/L).Also it can be seen from that figure that the removal percent increased when using sorptive flotation than flotation only.Under the examined conditions, the separation of biomass by floatation is a very rapid process, within 3 min. Almost 100% of biomass was separated and over 80% of lead ions removal was achieved in one stage. This is a specific advantage of the proposed sportive-flotation process, as it has been termed, because it is highly effective not only concerning lead ions removal, but also because the subsequent biomass separation process from the solution is fast and of relatively lower cost, due to necessary smaller residence time [20].


## 4.6. Kinetics

The amounts of barley husk used for adsorption of Pb(II) were calculated for final equilibrium-related concentration ofCe/Co=0.05. The Langmuir model constants were used with the mass balance in 1.5 liter of solution. The initial concentration of lead ions was 50 mg/L with the dose of husk being 20 gm.The rate constant using pseudo-first-order rate expression was obtained from the slope of the linear plots oflog(qe-qt) against t using (1). However, the rate constants for Pb(II) by using pseudo-second-order biosorption rate constant (k2) were determined from the slope and intercept of the plots of 1/q against 1/t using (2). The values of the rate constants with the corresponding correlation coefficients are presented in Table 2 for both kinetic models.Table 2
Pseudo-first and second-order rate constants for Pb(II) with correlation coefficients (R2).
Pseudo-first-order kinetic model
Pseudo-second-order kinetic model
K
1
(min−1)
R
2
K
2 (mg/g·min)
R
2
Pb(II)
0.122
0.936
1.6
0.506As can be seen from Table2, the correlation coefficients for the pseudo-first-order kinetic model for the various solutes were found to be higher than that for the pseudo-second-order kinetic.  Therefore, the pseudo first-order kinetics model can be used very well to find the rate constant.


## 5. Conclusions

Investigation of the lead ions removal by floatation and sorptive-floatation methods in semibatch process using barley husk as a biosorbent was conducted.(i)
The process is highly pH dependent and maximum removal efficiency was obtained at pH value equal to 8.(ii)
The metal loaded biomass particles can be easily separated by flotation process; also the results show that removal efficiency increased with increasing air flow rate up to 1000 mL/min for flotation and up to 1500 mL/min for sorptive flotation.(iii)
Increasing the SDS concentration from 50 to 100 mg/L had a small effect on the removal rates which were 90% and 90.4%, respectively, in flotation system while in sorptive-flotation system increasing SDS concentration from 50 to 100 mg/L leads to a decrease in the removal rate from 96% to 93% after 30 min operation.(iv)
Increasing initial lead ions concentration from 25 to 50 mg/L leads to an increase in removal rate from 73.6% to 85% while it decreased to 80% when initial lead ion concentration increased to 100 mg/L in flotation system. However, in sorptive-flotation system removal rate increased to 95% at initial lead ions concentration 50 mg/L and also decreases when increasing lead ions concentration to 100 mg/L.(v)
The equilibrium isotherm data were correlated with two models; Langmuir model gave the best fit for the experimental data. The batch experiments were helpful in estimating the rate constant for Pb(II) by using pseudo-first- and second-order models; the results showed that the Pb(II) uptake process followed the pseudo-first-order rate model.(vi)
The results obtained in this work show that burely husk can be successfully  used in removing lead ions from wastewater; also in comparison between flotation and sorptive-flotation processes, the results indicated that sorptive-flotation process is more efficient than flotation process only.



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*Source: 413948-2013-08-26.xml*