Review Article Volume 1 Issue 2
Department of Environmental Engineering, Delhi Technological University, India
Correspondence: Achla Kaushal, Department of Environmental Engineering, Delhi Technological University, Delhi, India, Tel 9198 11 200429
Received: July 26, 2017 | Published: August 29, 2017
Citation: Kaushal A, Singh SK. Adsorption phenomenon and its application in removal of lead from waste water: a review. Int J Hydro. 2017;1(2):38-47. DOI: 10.15406/ijh.2017.01.00008
Increased urbanisation and industrialisation has led to a situation of higher quantities of lead in waste water which has become a serious problem. Lead is toxic and is not essential for body. Its presence in body bears serious implications. Various technologies have been employed for the removal of lead ions from waste water. Adsorption with low cost adsorbents has been recognised as one of the cost effective and efficient techniques for this. Natural minerals, industrial waste, agricultural and forest waste are used as low cost adsorbents. This paper presents an overview of adsorption equilibria, kinetics and mechanisms. Effect of pH, metal ion concentration, adsorbent dose and temperature on adsorption capacity and percentage removal of lead from aqueous solutions using low cost adsorbents has been presented in this paper. The experimental data analysed statistically to verify the validity of the data is also reviewed in this paper.
Keywords: Adsorption equilibria, Kinetics, Mechanism, Heavy metals, Adsorption, Low cost adsorbents
Lead is a heavy metal toxic for body. It is among the major pollutants responsible for soil, water and atmospheric pollution.1 For decades, unchecked release of industrial effluents has worsen the environment. Release of lead in environment can be a man-made activity such as mining, automobile emissions, sewage discharge, combustion of fossil fuel or effluent discharge from industries or can result from natural activity such as urban and agricultural runoff, dry deposition, precipitation, sea spray, forest fires, volcanic eruptions etc,.2‒4 Lead is non-biodegradable and is harmful to both man and other living organisms. It has an ability to enter the food chain, get accumulated and absorbed in body tissues.5,6 It has been reported that adults absorb 5-15% of lead and retain about 5% of it. Presence of lead more than 0.5-0.8μg /ml into blood causes various abnormalities such as mental retardation, hepatitis, reduction in the production of haemoglobin. It interferes with body metabolism, causes reduced I.Q. levels in children and has been classified by the IARC as a 2B carcinogen.7−10 Because of its toxicity, measurement, monitoring and removal of lead from the waste water prior to discharge is must. World Health Organization has recommended that the levels of lead in water must be within the allowable concentration limits. As per water quality standards, quantity of lead in water should be between 0.05-0.1mg/L.11,12 According to the Indian Standard Institution, the tolerance limit of presence of lead for drinking water is 0.05 mg/L and for surface waters is 0.1mg/L (ISI, 1982). For decades, various physical and chemical methods employed for the removal of lead ions from effluent discharge are chemical precipitation, liquid membrane separation, electrochemical reduction, ion exchange, fixation and cementation, solvent extraction and adsorption.13−16 The choice of method for treatment depends on
Some of the above methods generate toxic sludge, disposal of which is an additional environmental problem, which affect the techno-economic feasibility of the treatment process.18 Adsorption has been found to be meritorious over other methods and is preferred in the removal of lead and other heavy metal ions. Use of commercial adsorbents such as activated carbon, zeolites, activated alumina, bone char, silica gel, synthetic polymers19‒23 is very popular even today. Significant efforts have been made to enhance their efficiency by chemical activation or through heat treatment. Adsorption using nanoparticles is has shown significant metal removal efficiency and are commonly used these days.24 These efforts are expensive and regeneration of modified adsorbents is difficult and sometimes not possible. Emphasis was laid on the use of low cost adsorbents as they show good results in lowering the concentration of heavy metal ions.
These are called as low cost adsorbents because they
In the present study, performance of low cost adsorbents in terms of sorption capacity and % removal of lead ions with respect to pH, temperature, initial lead ion concentration, adsorbent dose has been reviewed.
Adsorption equilibria is attained when the rate of adsorption of a molecule on a surface becomes equal to the rate of desorption. Types of adsorption equilibria are Table 1 shows
Adsorption isotherm |
plot between C and C , T constant |
Adsorption isostere |
plot of C vs T, Cs constant |
Adsorption isobar |
plot between Cs vs T, C constant |
Table 1 Types of adsorption isotherms
The basic concept of adsorption is the adsorption isotherm, the equilibrium relationship between the amount of the material adsorbed and concentration of the fluid phase in bulk at constant temperature. Adsorption isotherms models used to study the relation between adsorbent and the adsorbent in Table 2.
Isotherm |
Equation |
Significance |
Reference |
Single component adsorption |
Cs=Ka C |
For very low concentrations |
|
Langmuir isotherm |
q0= QKL.c./(1+KL.c) |
For homogeneous surfaces where interaction between adsorbed molecules are negligible |
|
Brunauer- Emmett- Teller (BET) isotherm |
q0= Q.KL.p/ [ 1 +KLp + (p/P)][1−(p/P)] |
For gas- solid systems where condensation is approached |
|
Freundlich isotherm |
C=kF[v(C0−C)]n |
For dilute solutions, over a small concentration range |
|
Gibbs isotherm |
dΓ= (ns/As) RT d (lnP) |
Based on the assumption that the adsorbed molecules move freely like liquid film over the adsorbent surface |
|
Temkin Isotherm |
qe= (RT/BT)ln(ATCe) |
Based on the adsorbent–adsorbate interactions |
|
Dubinin–Radushkevich (DRK) isotherm |
qe=qsexp (−kadε2) |
Describes adsorption with a Gaussian energy distribution onto a heterogeneous surface |
|
Kisliuk isotherm |
dθ/dt = RK(1−θ)(1+ kEθ) |
Adsorption occurs around the gas molecules that are already present on the solid surface |
|
The Flory –Huggins model |
Log (θ/C)= log KFH+αFHlog (1−θ);θ=(1−Ce/Co) |
It accounts for the extent of surface coverage as characteristics of the adsorbate on the adsorbent |
|
Jovanovic isotherm model |
qe=qn[ 1−exp(−KJCe)] |
Jovanovic model considers the possibility of some mechanical contacts between the adsorbing and desorbing molecules |
|
Redlich–Peterson isotherm |
qe=KRCe/ (1+aRCeg) |
It can be applied either in homogeneous or heterogeneous systems |
|
Hill isotherm |
qe= (qHCeηH)/(KD+ CeηH) |
It explains the binding of various species onto homogeneous substrates |
|
Koble-Corrigan isotherm |
qe= ACeD/(1+ BCeD) |
It is usually used with heterogeneous adsorption surfaces. |
|
Combination of Langmuir and Jovanovic model |
qe=[rCe/(1+Ce)]/[1+exp(−pCeZ) |
It is a new model with less error in comparison to other models |
Table 2 Types of adsorption isotherms
Adsorption kinetic modelling is studied to determine the rate of adsorption and rate expressions for a given reaction.
Pseudo first order kinetic:The pseudo first order kinetic equation is given by
dNt/ dt = kad(Ne– Nt) (1)
Ne and Nt are the amounts of metal ions adsorbed at equilibrium time and at any instant of time t respectively. kad is the rate constant.25
Pseudo second order kinetics: The pseudo second order kinetics are given by the equation;
dNt/ dt = k2(Ne– Nt) 2 (2)
Molecules have a natural tendency to diffuse from the bulk of a turbulent phase through a laminar layer around the solid particle to the bulk of another phase through its extreme surface due to concentration gradients given by four diffusion mechanisms:29
Diffusion of adsorbate at internal surface sites ((Table 3) & (Table 6)) is very rapid and thus resistance to mass transfer in these steps is negligible. Thus these steps are not considered the rate-limiting steps in the process. For steps 2 and 3 in the adsorption mechanism, three cases may occur:
S.No. |
Adsorbent |
Maximum uptake capacity Mg/G |
Maximum % removal |
Optimum ph |
Sorbent dose G/L |
Concentration Mg/L |
Temperature Oc |
References |
1 |
Natural sand particles |
91.5 |
6 |
24.9 |
||||
2 |
Natural goethite |
100 |
4.5-6.0 |
100 |
5-750 ppm |
30 |
||
3 |
Natural bentonite clay |
83.02 |
1g/50ml |
100-5000 |
ambient |
|||
4 |
Acid activated bentonite clay |
92.85 |
1g/50ml |
100-5000 |
ambient |
|||
5 |
Agbani clay |
0.65 |
6 |
2g/20ml |
20-100 |
45 |
||
6 |
Natural clay |
84.8 |
4.46 |
0.2-2g/ 50ml |
200-300 |
|||
7 |
Iron coated sand |
2.5-7.5 (study range) |
2.5g/50ml |
0.01M |
283-333K (Study Range) |
|||
8 |
Talc surface |
>98 |
6 |
0.1g |
5-500ppm |
20 |
||
9 |
Peat moss |
96 |
5.5-6.0 |
0.2g/100ml |
15-Feb |
|||
10 |
Sphagnum peat moss |
|
98 |
6 |
0.125-1.0g |
34-507 |
|
Table 3 TNatural materials used as adsorbents for the removal of lead from aqueous solutions
S. No. |
Adsorbent |
Uptake capacity Mg/G |
Maximum% removal |
Optimum ph |
Sorbent dose G/L |
Concentration Mg/L |
Temperature Oc |
References |
1 |
Iron slag |
95.24 |
3.5-8.5 |
2 |
200 |
|||
2 |
Steel slag |
32.26 |
5.2-8.5 |
2 |
200 |
|||
3 |
Fly ash baggasse |
2.5 |
95-96 |
6 |
10 |
5.0-7.0 |
30 |
|
4 |
Fly ash modified, activated |
98 mmol/100g |
98 |
5 |
0.5-2 |
0.0027 mol/l |
25 |
|
5 |
Waste beer yeast |
2.34 |
96.35 |
1.0-5.0 |
0.5-2 |
25-100 |
||
6 |
Sludge from steel industry |
2.74 |
5±0.1 |
5g |
0.15-10 g/lt |
20-80 |
||
7 |
Coal fly ash |
90.37 |
0.5-1.5 |
100 |
||||
8 |
Sawdust waste generated in the timber industry |
0.646 mmol/g |
88.6 |
6.5 |
1 |
0.5 mmol/dm3 |
30 |
|
9 |
Saw dust activated carbon |
0.223 mmol/g |
90.1 |
5 |
2 |
0.5 mmol/l |
30±2 |
|
10 |
Low grade manganese ore |
67 mg/g |
|
2-5.25 |
6-Jan |
50-500 |
27 |
Table 4 Industrials by products used as adsorbents for the removal of lead from aqueous solutions
S. No. |
Adsorbent |
Uptake capacity Mg/G |
Maximum % removal |
Optimum ph |
Sorbent dose G |
Concentration Mg/L |
Temperature Oc |
References |
1 |
Activated bamboo charcoal |
53.76 |
83.01 |
5 |
0.1 |
50-90 |
29 |
|
2 |
Almond |
8.08 |
68 |
7-Jun |
0.5 |
0.001mol/l |
25±1 |
|
3 |
Dust of bamboo |
2.151 |
66.73 |
7.2 |
28 |
600 |
||
4 |
Peels of banana |
72.79 |
5 |
1 |
200 |
25±2 |
||
5 |
Peels of banana |
2.18 |
85.3 |
5 |
2 |
30-80 |
25 |
|
6 |
Coconut |
4.38 |
60 |
4 |
6 |
100 |
60 |
|
7 |
Coconut shell |
26.5 |
75 |
4.5 |
50mg/50ml |
|||
8 |
Coir |
0.127 |
86.98 |
4.9 |
1 |
0.56mmol / dm3 |
30 |
|
9 |
Shells of groundnut |
0.106 mmol/g |
82.81 |
4.9 |
1 |
30 |
||
10 |
Shells of hazelnut |
28.18 |
90 |
7-Jun |
0.5 |
0.001mol/l |
25±1 |
|
11 |
Okra waste |
5 |
99 |
5 |
240 |
25 |
||
12 |
Formaldehyde treated orange peel, |
99 |
5 |
0.12 |
||||
13 |
Natural orange peel |
46.61 |
99 |
5 |
0.12 |
150 |
||
14 |
Peach stone |
2.33 mg/kg |
97.64 |
8-Jul |
2 |
200 |
||
15 |
Peanut hulls |
69.75 |
5 |
1 |
200 |
25±2 |
||
16 |
Modified peanut shells |
0.63 mmol/g |
4.6-5.0 |
|||||
17 |
Onion skins |
200 |
93 |
6 |
0.15 |
25-200 |
30 |
|
18 |
Rice husk |
5.69 |
5 |
2 |
50 |
60 |
||
19 |
Rice husk |
31.13 |
5 |
1 |
200 |
25±2 |
||
20 |
Ash of rice husk |
10.86 |
5.6-5.8 |
2 |
40 |
15 |
||
21 |
Ash of rice husk |
91.74 |
99.3 |
5 |
5 |
3-100 |
30 |
|
22 |
Chemically modified rose petals |
118.4 |
5 |
0.1 |
100 |
30 |
||
23 |
Sun flower waste |
33.2 |
4 |
10 |
||||
24 |
Tea waste |
73 |
96 |
5 |
0.5 |
5-100 |
30 |
|
25 |
Discarded tea leaves |
35.89 |
5 |
1 |
200 |
25±2 |
||
26 |
Wheat bran |
86.96 |
7-Apr |
0.5 |
200-500 |
20 |
||
27 |
Acid treated wheat bran |
79.37 |
82.8 |
6 |
0.1 |
100 |
25 |
Table 5 Agricultural waste used as adsorbents for the removal of lead from aqueous solutions23
S. No |
Adsorbent |
Uptake capacity Mg/G |
Maximum % removal |
Optimum ph |
Sorbent dose G/L |
Concentration Mg/L |
Temperature Oc |
References |
1 |
Pinus Elliottii Bark |
98.61 |
5 |
500 mg |
100 |
|||
98.83 |
7 |
|||||||
2 |
Pongamia Pinnatta Bark |
5.5 |
10 |
5- 50 ppm |
30 |
|||
3 |
Ficus Religiosa Leaves |
16.95±0.75 |
80 |
4 |
10 |
10-1000 |
20-50 |
|
4 |
Aliathus Excelsa Bark |
70 |
4.5 |
1 |
10 |
|||
5 |
Bael Tree Leaf |
90.07 |
5 |
20-May |
25-100 |
30 |
||
6 |
Pinus Nigra Tree Bark |
12.6 |
90 |
8 |
35 |
|||
7 |
Streblus Asper leaves |
71.9 |
8 |
400mg |
1.598 g/l |
25 |
||
8 |
Mango tree leaves |
31.54 |
4 |
1 |
200 |
25±2 |
||
9 |
Neem tree leaves |
41.45 |
5 |
1 |
20 |
25 |
||
10 |
Peepul tree leaves |
127.34 |
|
4 |
1 |
200 |
25±2 |
Table 6 Forest waste used as adsorbents for the removal of lead from aqueous solutions
In cases I and II, film and pore diffusion are the rate controlling steps. In case III, the rate of transport of molecules to the boundary may be insignificant, causing formation of a liquid film around the adsorbent particles, thus creating a concentration gradient.30
Pore diffusion: The phenomenon pore diffusion or Knudson diffusion occurs because at low pressure conditions, the mean free path of the molecules may be larger than the pore diameter of the molecules. Pore diffusivity for liquids is expressed as:
Dpore= Dfχ/τ (3)
χ = internal porosity of the particles and τ = Tortuisity (Usually between 2 and 6).31
Intraparticle diffusion model: This model suggests that the molecular diffusion the controlling step, because the speed of diffusion of the adsorbate molecule towards the adsorbent surface determines the rate of adsorption.
Qe= kit1/2+I (4)
Ki = intra particle diffusion rate constant (g/mg/min), I = Intercept from plot of Qe vs t1/2.32,33
Hypotheses are the assumptions, concise statements or formal questions for the available data, which can be tested for their validity and can be accepted or rejected.34 Various hypothesis tests for the analysis of experimental data are classified as
The z-test is used to judge the significance of mean for large samples (n˃30) by comparing the sample mean with some hypothesised value of the population mean.
z=(ˉX−μHo)/(σp/√n) Ha may be one sided or two sided. (5)
The t-test is based on t-distribution and is used to judge the significance of the difference between the two sample means for small sample size (n<30). Ha is chosen to be one sided or two sided.
t=(ˉX−μHo)/(σs/√n) for (n-1) degree of freedoms. (6)
The F-test is based on the F-distribution and is used to compare the variance of two samples.
F = σs12/σs22 (7)
The χ2-test is a statistical technique used to test the goodness of fit, independence and significance of population variance.
χ2= ∑{(Oi−Ei)2/Ei} (8)
ANOVA, Analysis of variance is used when there are multiple sample cases at the same time. With ANOVA, it is possible to analyse the differences among sample means of different populations by making estimates for population variance:
Low cost materials can be broadly categorized into four classes:
Natural minerals: Natural minerals are rich and excellent sources of adsorbents available naturally, abundantly easily for the adsorption of heavy metals. Moss (Claymperes delessertti) was used for removal for copper from aqueous solutions.37 Soil, clay and slow sand filters have shown significant potential towards the removal of heavy metals from aqueous solutions laden with heavy metals.38−42 Agbani clay obtained from Nigeria was used for the removal of lead ions using batch techniques.43 Results showed that the Freundlich isotherm fitted the best followed by the Temkin isotherm and the Langmuir isotherm fitted the least. Adsorption of lead on natural clay was studied batch wise.44 Results showed that adsorption was very fast in the beginning but slowed down gradually. Natural minerals studied for the removal of lead from waste waters are summarized in Table 3.
Industrial by-products: Industrial by-products are cheap and abundantly available adsorbents used for the removal of heavy metals from waste water. They can be chemically modified to enhance their metal ion removal efficiency.
Red mud, obtained as a residue during alkaline leaching of bauxite ore in the Bayer process, has been found to remove fluoride, Cr(VI), dyes, nitrates, and phosphate from aqueous solution. It has also been used for the removal of Pb ions.45,46 studied the adsorption of Cu, Pb, Zn and Cd using Tourmaline, obtained from Chifenf mine of China and noted that the optimum value of process temperature was 550C, pH was 7 for the metal ion concentration between 10-500 mg/l. Removal was 78.76 mg/g for Cu II, 154.08mg/g for Pb II, 67.25 mg/g for Zn II and 66.67 mg/g for Cd II.47 The study of removal of lead by fly ash showed that lead ions were retained in the pores and onto the surface for pH higher than 5.5 and through adsorption for pH less than 5.5. Adsorbed ions were not released in the pH range 3.5-10.0.48 Studied bagasse fly ash for the removal of lead ions using batch adsorption studies. 50-65% lead ions were removed at pH 3.0 in the first hour.49 At other values of pH, % removal was lesser. It decreased with increase in temperature. % removal of lead ions was 100% for an adsorbent dose of 10 g/l, average particle size of 150-200 mesh at lower concentrations of the adsorbate and 50-70% at higher concentrations. Industrial products studied for the removal of lead from waste water are summarized in Table 2.
Agricultural waste: Agricultural waste is widely used low cost adsorbent available abundantly and does not require significant processing.50 They comprise of hydrocarbons, carbohydrates, cellulose and hemicelluloses, starch, lignin, lipids, proteins and various functional groups.51 They have the ability to bind heavy metal ions by donating a pair of electrons and to form complexes with metal ions through reactions, by chemisorptions, diffusion through pores, complexation and adsorption on surface. Orange peel was used to remove Ni (II) from synthetic samples.52 Metal adsorption capacity was 158mg/g at 323K. % removal was maximum at pH 6.0. Peanut hulls were studied for the removal Ni (II) and Cu (II) from synthetic solutions. Maximum removal of Ni (II) was 53.65mg/g was observed in the pH range 4- 5 and Cu (II) was 65.57mg/g in the pH range 6-10 in the column study.53 Cu (II) removal of 10.17 mg/g was observed in the batch study.54 In batch studies, the concentration gradient decreased with time. Where as in the column, the adsorbent was in continuous contact with the fresh feed of the adsorbent resulting in higher removal of Cu (II) Zn (II) removal was studied by24‒55 with the help of mango tree leaves as adsorbent. Experimental data was analysed statistically. Hypotheses were tested to verify the validity of the test results and the data was found to be within the accepted regions of the statistical charts. Adsorbents activated by heating or chemically are expensive, but the cost incurred in processing is compensated by better adsorption capacity.51-56 Also it prevents the elution of tannin compounds which stain the treated water and increase the COD of water to a great extent.57 Rice hull modified with ethylenediamine studied for Cr (VI) removal from simulated solution was reported to give maximum metal ion adsorption of 23.4mg/g at pH 2. The surface of rice hull contains carboxylic and hydroxyl groups which act as electron donors in the solution. Due to these, Cr (VI) oxyanion reduces to Cr (III) ions by proton consumption in the acidic solution resulting in Cr (VI) removal.58 Soybean hull and modified soybean hull extracted with NaOH and with citric acid were used for the Cu (II) removal. Metal removal efficiency was 24.76mg/g for natural soybean hull and was increased to 154.9mg/g after modified chemically. Possibly, pre-treatment increased the number of carboxyl groups and negative charge on the soybean hull increasing the efficiency.59 Chemically modified potato peel (PP)where used for the adsorption of malachite green with 100 ml of 100 ppm dye solution with 0.250gm dose.60,61 Langmuir, Freundlich and Temkin isotherms were studied. PP favoured the Freundlich isotherm. Potato peel worked efficiently when treated with HCHO. The percentage removal of lead ions for PP and APP (activated potato peel) was 92.2% and 82.7% respectively. Various agricultural products studied for the removal of lead summarized in Table 5.
Forest waste: Shedding of leaves and bark natural phenomenon of trees. Tree barks and saw dust are produced at saw mills in large quantities as a solid waste. Febrifuga bark studies for the removal of lead showed that maximum removal was 98.42%, optimum pH was 4.0, and equilibrium time was 6 hours. Adsorption decreased with increase in temperature.62 Neem Bark (NB) and activated neem bark (ANB) used to study adsorption of malachite green dye60 showed 92.7% and 94.4% removal respectively. Pinus bark was used to carry out the adsorption studies of lead ions at pH 5.0 and 7.0 with an average particle size≤60 mesh. % removal of lead ions 98.61% at pH=5.0 and 98.83% at pH=7.0.63,64 Studied the adsorption of lead ions by Ficus Religiosa leaves for the removal of lead ions from waste water. 80% removal was observed in first 15 minutes and after 45 minutes concentrations became almost constant. Equilibrium was attained in 1 hour. Forest wastes studied for the removal of lead from waste waters are summarized in Table 6.
Drying and crushing of adsorbents increase the surface area to facilitate the adsorption. Chemical activation or modification of adsorbents increases active surfaces for adsorption and prevent the elution of tannin compounds. The sorption capacity was observed to
Decreases with increase in temperature because the texture of biomass changes at higher temperature.
However, some exceptions were also observed.
From the above study it has been concluded that the process of adsorption using low cost adsorbents is a simple, cost effective and an eco-friendly technique for the treatment of waste water containing lead ions. Efficiency of the process depends not only on the physical and chemical properties of the material used as adsorbent, but also on the various process variables like pH, adsorbent dose, metal ion concentration, temperature, contact time etc. These parameters have to be optimized to make the process more efficient and economical.
None.
The Authors declare no conflict of interest.
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