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Review on the Removal of Metal Ions from Effluents Using Seaweeds, Alginate Derivatives and Other Sorbents

  • Jean-François Fiset,
  • Jean-François Blais et
  • Patricio A. Riveros

…plus d’informations

  • Jean-François Fiset
    Natural Resources Canada,
    555 Booth Street,
    (Ont) K1A 0G1

  • Jean-François Blais
    Institut national de la recherche scientifique,
    490, de la Couronne,
    Québec (Québec) G1K 9A9

  • Patricio A. Riveros
    Natural Resources Canada,
    555 Booth Street,
    (Ont) K1A 0G1

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Corps de l’article


The preservation of the environment has become increasingly important in view of the ecological problems brought about by industrialization and urbanization. Lakes and rivers are particularly vulnerable to contamination as a result of the discharge of large quantities of effluents from industries and municipalities. The presence of heavy metals, such as cadmium, chromium, cobalt, copper, lead, mercury, nickel, silver, tin and zinc in rivers and watercourses may cause serious health problems to living organisms (ALLOWAY and AYERS, 1993; WASE and FORSTER, 1997).

Consequently, the norms and regulations imposed on industrial effluents are becoming increasingly stringent. These restrictions stem largely from recent advances in the understanding of the behaviour of heavy metals in the environment. Being non-biodegradable, toxic metals tend to accumulate in lower plants and animals, thereby entering the food chain (CHANG et al., 2003; LIPPMANN, 2000; WATTS, 1998).

Various technologies are available to remove metal ions from industrial effluents, including precipitation (usually as metal hydroxide or sulphide) and coprecipitation, sorption, solvent extraction, cementation, electrodeposition, electrocoagulation, ion exchange, and membrane technology (BLAIS et al., 1999; BROOKS, 1991; CHMIELEWSKI et al., 1997; PATTERSON, 1989). However, most of these techniques require expensive, usually toxic, reagents, and this fact significantly increases the capital and operating costs. In this context, biosorbents (i.e., ion exchangers and adsorbents derived from organic matter) present an attractive alternative to synthetic and chemical products because they are widely available, generally biodegradable and relatively inexpensive.

The main characteristics and past applications of biosorbents have been summarized and discussed by several researchers (ATKINSON et al., 1998; BABEL and KURNIAWAN, 2003; BAILEY et al., 1999; FISET et al., 2000; KUYUCAK and VOLESKY, 1988; VEGLIO and BEOLCHINI, 1997; VOLESKY, 1990; VOLESKY and HOLAN, 1995; WASE and FORSTER, 1997). This present review summarizes the recent research carried out on the use of biosorbents, especially those derived from seaweeds, as substrates to remove heavy metal from solutions and effluents. The various systems, mechanisms and results presented in the scientific literature are analyzed and compared.

1. Seaweed Sorbents

1.1 Seaweed-derived sorbents

The ability of biosorbents derived from marine algae to adsorb metal ions has been demonstrated by several researchers (LEE and VOLESKY, 1997; LEUSCH et al., 1995; VEGLIO and BEOLCHINI, 1997; VOLESKY and HOLAN, 1995; VOLESKY and PRASETYO, 1994; WILSON and EDYVEAN, 1994).

According to FAO (2002), the world aquaculture production of brown, red and green seaweeds in 2002 was approximately 5, 2.5 and 0.018 Megatons (wet basis), respectively. Whereas all these seaweed species exhibit good metal adsorption properties, the brown marine algae (Sargassum and Ascophyllum) have the highest capacity for heavy metal ions because of their high polysaccharide content (VOLESKY and HOLAN, 1995). Tables 1 and 2 summarize the research carried out on the adsorption of metal ions using various seaweed species.

Table 1

Studies on the metal sorption using seaweeds

Études portant sur l’adsorption des métaux par utilisation d’algues macroscopiques




Studied parameters

Aravindhanet al. (2004)

Turbinaria sp.


Pre-treated with H2SO4, CaCl2 and MgCl2

Axtellet al. (2003)

Microspora sp.

Ni(II), Pb(II)

Batch and semi batch process, kinetic study

borba et al. (2006)

Sargassum filipendula


Pre-treatment, fixed bed column, mathematical modeling

cepriáet al. (2006)

Ulva rigida

Au(III), Hg(II), Ag(I),

Biomass modified electrode, factors affecting biosorption

Chaisuksant (2003)

Gracilaria fisheri (red marine algae)

Cd(II), Cu(II)

Langmuir model, effect of pH, pre-treated with CaCl2.

Cossichet al. (2004)

Sargassum sp.


Fixed-bed column, mass balance

Da Costa and De França (1996)

Codium sp., Colpomenia sp., Gelidium sp., Padina sp., Sargassum sp., Ulva sp.


Langmuir and Freundlich models, ion-exchange mechanism, effect of pH

Da Costaet al. (1996)

Sargassum sp.

Al(III), Ca(II), Cd(II), Mg(II), Na(I), Zn(II)

Synthetic and natural effluents, kinetic

Gonget al. (2005)

Spirulina maxima


pH, contact time, biomass concentration, Freundlich model, desorption, pre-treated with CaCl2.

Guptaet al. (2001)

Spirogyra sp.


Batch sorption, kinetic studies, effect of pH, Langmuir model

Holanet al. (1993)

Ascophyllum nosodum,

Fucus vesiculosus


Cross-linking, desorption

Holan and Volesky (1994)

Ascophyllum nosodum,

Fucus vesiculosus

Ni(II), Pb(II)

Langmuir model, effect of pH, crosslinked with formaldehyde, bis(ethenyl)sulfone and 1-chloro-2,3-epoxypropane

Kaewsarn and YU (2001)

Padina sp.


Batch and column experiments, kinetic studies, effect of pH

Kaewsarnet al. (2001)

Durvillaea potatorum


Co-ions effect (light and heavy metals, EDTA)

Kaewsarn (2002)

Padina sp.


Langmuir isotherm, kinetic studies, effect of pH, batch and fixed-bed experiments

khani et al. (2006)

Cystoseira indica


Batch sorption, kinetic modelling, effect of pH, protonated algae, Ca-pretreated algae

Kratochvillet al. (1998)

Sargassum sp.

Cr(III), Cr(VI)

Protonated seaweed, pH optimization

Kuyucak and Volesky (1988)

Ascophyllum nodosum, Chondrus crispus, Halimeda opuntia, Palmaria palmata, Porphyra tenera, Sargassum natans

Ag(I), Au(III), Cd(II), Co(II), Cu(II), Pb(II), U(VI), Zn(II)

Algal biomass, dead and living yeast, comparison with activated carbon, anion exchange resin (IRA-400) and cations exchange resin (Duolite-C20)

kumaret al. (2006)

Ulva fasciata sp.


Effect of pH and algae concentration, effect of particle size, adsorption kinetics, pseuso-first and pseudo-second models, adsorption equilibrium

Lauet al. (2003)

Ulva lactuca

Cu(II), Ni(II), Zn(II)

Langmuir isotherm, effect of cations and anions, kinetic study, effect of pH, seaweed biomass concentration, effect of reaction time,desorption

Lee and Volesky (1997)

Sargassum fluitans

Al(III), Ca(II), K(I), Mg(II), Na(I)

Light metals affinity, proton uptake

Leuschet al. (1995)

Ascophyllum nodosum

Sargassum fluitans

Cd(II), Cu(II), Ni(II), Pb(II), Zn(II)

Crosslinked with formaldehyde, glutaraldehyde and embedded in polyethylene imine, Langmuir, Freundlich and Dubinin-Radushkevich models, effect of particle size

lodeiroet al. (2006)

Cystoseira baccata

Cd(II), Pb(II)

Kinetic experiments, temperature effect, Langmuir-Freundlich model, effect of salinity on metal uptake, FTIR analysis

luoet al. (2006)

Laminaria japonica


Chemical modification, Langmuir isotherm, effect of pH, effect of solid/liquid ratio.

Matheickal et al. (1997)

Ecklonia radiata


pH effect, effect of EDTA, acetate, nitrate and chloride on metal uptake, packed bed system

Matheickal and YU (1997)

Phellinus badius


Langmuir isotherm, kinetic studies, effect of pH, batch and fixed-bed experiments

naja and Volesky (2006)

Sargassum fluitans

Cu(II), Zn(II), Cd(II)

Equilibrium and sorption models

Oferet al. (2003)

Padina pavonia,

Sargassum vulgaris

Cd(II), Ni(II)

Kinetic studies, desorption studies, Langmuir isotherm

Parket al. (2004)

Ecklonia sp.

Cr(III), Cr(VI)

Redox reaction with the biomass, thermal treated biomass, SEM, BET, FTIR characterization

Prasheret al. (2004)

Palmaria palmate (red algae)

Cd(II), Cu(II), Ni(II), Pb(II), Zn(II)

Freundlich, Langmuir and Brunauer Emmer and Teller (BET) models, effect of contact time, pH, initial concentration and temperature

Senthilkumaret al. (2006)

Gracilaria crassa, Gracilaria edulis, Hypnea valentiae, Ulva lactuca, Ulva reticula, Codium tomentosum, Chaetomorpha antennina, Turbinaria conoides, turbinaria ornata, Sargassum polycystium


Batch experiments, Langmuir, Freundlich, Redlich-Peterson and Sips models, columns experiments, biosorption kinetics, sorption thermodynamics, influence of co-ions, desorption studies

tsui et al. (2006)

Sargassum hemiphyllum

Ag(I), As(V), Cd(II), Co(II), Cd(II), Cr(III), Cr(VI), Mn(II), Ni(II), Pb(II), Zn(II)

Ca-treated biomass, different ionic strengths, binding mechanism

Volesky (1994)

Sargassum natans, Sargassum fluitans, Sargassum vulgaris, Ascophyllum nodosum, Palmaria palmata, Chondrus crispus, Halimeda opuntia, Fucus vesiculosis, Padina gymnospora, Codium taylori

Cd(II), Pb(II)


Yuet al. (1999)

Ascophyllum nodosum, Lessonia flavicans, Lessonia nigresenseLaminaria japonica, Laminaria hyperbola, Ecklonia maxima, Ecklonia radiate, Durvillaea potatorum

Cd(II), Cu(II), Pb(II), U(VI)

Langmuir isotherm, radionuclides, effect of grown media

-> Voir la liste des tableaux

Table 2

Recent studies on the adsorption capacities (mg/g) of marine algae for selected heavy metals.

Études récentes sur la capacité d’adsorption (mg/g) des l’algues marines pour des métaux lourds sélectionnés.








ARAVINDHAN et al. (2004)

T. ornata







G. fisheri






COSSICH et al. (2004)

Sargassum sp.






KUMAR et al. (2006)

Ulva fasciata sp.






LAU et al.(2003)

Ulvas sp. 1

Ulva lactuca

Ulva sp. 3












LODEIRO et al. (2004)

S. muticum






LODEIRO et al. (2006)

C. baccata






OFER et al. (2003)

S. vulgaris

P. pavonia








PAVASANT et al. (2006)

Caulerpa lentillifera






-> Voir la liste des tableaux

KLIMMEK et al. (2001) compared the efficiency of thirty strains of algae for their abilities to extract cadmium, lead, nickel and zinc from aqueous solution. These researchers found that the cyanophyceae Lyngbya taylorii exhibited high uptake capacities for the four metals. Similarly, VOLESKY and HOLAN (1995) provide some 23 examples of algal biomass metal adsorption.

The physical integrity of algae is important to prevent them from disintegrating during the sorption process. HOLAN et al. (1993) summarized various techniques used to improve the stability and the mechanical properties of fresh biopolymers:

  • Grafting into synthetic polymers;

  • Entrapment into inorganic material;

  • Binding to a suitable carrier; and

  • Cross-linking.

1.2 Algins and alginates derivatives

Algins are salts of alginic acid, a natural polymer found in brown algae (Phaeophyceae). This polymer is extracted by treating the seaweed with a sodium carbonate solution and recovered by precipitation as alginic acid and afterward as the sodium salt. The alginic acid molecules have a complicated structure. Figure 1 shows two of the main segments found in alginic acid. The abundance of carboxylic, hydroxyl and oxo groups gives alginic acid and alginate salts strong chelating properties for metal ions.

Figure 1

Main segments of alginic acid: A) a poly(D-mannuronosyl segment and B) a poly(L-guluronosyl) segment.

Principales parties de l’acide alginique : A) une portion poly(D-mannuronosyl, et B) une portion poly(L‑guluronosyl).


-> Voir la liste des figures


-> Voir la liste des figures

When alginic acid reacts with polyvalent ions, such as calcium, a cross-linking effect takes place, which gives the resulting alginate gel a significant structural strength (NESTLE and KIMMICH, 1996). The cross-linking is caused by a polyvalent ion binding two or more carboxylic groups on adjacent polymer chains, and this can be accompanied by chelation of the ion by the hydroxyl and carboxyl groups of the polymer chains (SHIMIZU and TAKADA, 1997).

The alginate products are not only used for metal removal, but also for other commercial applications, including some in the food industry (HOLAN et al., 1993; RENN, 1997). The main advantage of using algae or biomass derivatives is that they do not require nutrients and they are resistant to the physical-chemical properties of heavy metal solutions (ARAÚJO and TEIXEIRA, 1997). Alginate products have been used as supporting substrate for a variety of active agents, including microorganisms, algae (AL-RUB et al., 2004; SINGHAL et al., 2004), chitosan (GOTOH et al., 2004; HUANG et al., 1996), activated sludge (WANG et al., 2004), cellulose and humic acid (MISRA and PANDEY, 2001). Tables 3 and 4 present alginate derivatives studied for their capacity to adsorb different metals.

Table 3

Studies on the metal sorption using alginate products.

Études portant sur l’adsorption des métaux sur les produits d’alginate.




Studied parameters

Al-Rubet al. (2004)

Alginate beads


Effect of immobilized algae cells (living and death), effect of pH and initial concentration, alginate beads, Langmuir model, sorption desorption cycle

Aksuet al. (1998)

Ca-alginate beads agarose,

Chlorella vulgaris


Packed-bed column, flow rates

Chenet al. (1993)

Alginate beads


Linear absorption model, diffusion coefficient, density of alginate

Cristet al. (1994)

Vaucheria, Rhizoclonium,

Ca-alginate powder

Ag(II), Al(III), Ba(II), Cd(II), Cu(II), La(III), Mg(II), Pb(II), Sr(II) Zn(II)

Ion exchange constant, rate of removal of sorbed metal, ion exchange model

Fourest and Volesky (1997)

Alginate extraction from Sargassum fluitans, Ascophyllum nodosum, Fucus vesiculosus, Laminaria japonica

Ca(II), Cd(II), Cu(II), Pb(II), Zn(II)

Characterization of physical properties of alginate by potentiometric titration and 13C NMR, metal binding

Gotohet al. (2004)

Alginate gel beads

Cu(II), Mn(II)

Doped alginate beads with cyanogens bromide and 1,6-diaminohexane, FTIR and SEM characterization

Hirai and Odani (1994)

Alginic acid film, sodium alginate film, alginate-Co complex


Absorption, desorption, diffusion coefficient, film characterization

Huanget al. (1996)

Alginate and chitosan beads

Cu(II), Ni(II)

Metal selectivity, particle size, kinetic, isotherm, effect of pH

IBÁÑEZ and Umetsu (2002)

Protonated alginate beads

Co(II), Cr(III), Cu(II), Ni(II), Zn(II)

Metal uptake, beads morphology, effect of protonation, effect of: ionic strength, pH and protonation

IBÁÑEZ and Umetsu (2004)

Protonated dry alginate beads


Batch tests, effect of pH, mechanism, EPMA-EDX analysis

Janget al. (1995)

Alginate beads

Co(II), Cu(II)

In-situ crosslinking, metal selectivity, fluidized bed reactor, Langmuir model

Janget al. (1999)

Alginate beads

Cu(II), Zn(II)

In-situ crosslinking, extended Langmuir model, binding group density, binding stability constant

Jeonet al. (2002)

Carboxylated alginic acid


Carboxylated alginic acid using KMnO4, FTIR and 13C NMR characterization, elemental analysis, desorption

Jeonet al. (2005)

Carboxylated alginic acid

Cu(II), Pb(II)

Effect of ionic strength and organic material effect, desorption

Karagunduzet al. (2006)

Dried alginate beads


Kinetic sorption, equilibrium experiment, surfactant entrapped dried alginate beads.

Lu and Wilkins (1996)

Sacharomyces cerevisiae immobilized in alginate gels

Cd(II), Cu(II), Zn(II)

Caustic treatment, metal desorption, biosorbent reactivation

Nestle and Kimmich (1996)

Alginate beads


NMR analyses, spatial distribution, diffusion coefficient

PAPAGEORGIOUet al. (2006)

Alginate beads, alginate extracted from Laminaria digitata

Cu(II), Cd(II), Pb(II)

Alginate beads characterization, batch metal uptake, Langmuir, Freundlich and Sips models, kinetic model, batch kinetic model

Park and Chae (2004)

Alginate beads, alginate capsules, alginate gel coated


Regeneration of alginate adsorbent, SEM characterization

Seki and Suzuki (1996)

Alginic acid and humic acid membranes


Equilibrium parameters, complexation model

Shimizu and Takada (1997)

Alginate fibers

Bi(III), Cu(II), Pb(II), Sr(II)

Effect of nitric acid, fibers characterization

Singhalet al. (2004)

Chlorella pyrendoidosa impregnated beads Ca-alginate

U(IV), U(VI)

Column, desorption, kinetic, FTIR characterization

Veglioet al. (2002)

Ca-alginate beads


Effect of pH, Langmuir isotherm

-> Voir la liste des tableaux

Table 4

Recent studies on the adsorption capacities (mg/g) of alginate for selected heavy metals.

Études récentes sur la capacité d’adsorption (mg/g) de l’alginate pour des métaux lourds sélectionnés.








AL-RUB et al. (2004)

Alginate beads

Free dead algal cell

Immobilized dead algal cells








BAJPAI et al. (2004)

Bio-polymeric (Ca and gelatin)






IBÁÑEZ and UMETSU (2004)

Protonated dry alginate beads






Ngomsiket al. (2006)

Magnetic alginate microcapsule






OZDEMIR et al. (2005)

Alginate beads

Alginate-Extracellular polysaccharide








PARK and CHAE (2004)

Alginate beads

Alginate capsule







-> Voir la liste des tableaux

Calcium alginate may be prepared in various forms, such as beads, powder (CRIST et al., 1994), membranes (HIRAI and ODANI, 1994; TOTI and AMINABHAVI, 2002) or fibers (SHIMIZU and TAKADA, 1997; WILLIAMS and EDYVEAN, 1997) and can be used as cell-immobilization support (IBÁÑEZ and UMETSU, 2002). Bead particles have practical advantages in terms of applicability to a wide variety of process configuration and reusability (GOTOH et al., 2004). Also, the alginate beads may be protonated (IBÁÑEZ and UMETSU, 2002, 2004) or doped with another metallic ion to obtain various bead properties (MIN and HERING, 1998). GOTOH et al. (2004) improved the mechanical strength and resistance to chemical and microbial degradation without affecting adsorption capacity by cross-linking the alginate beads with 1,6-Diaminohexane. Producing alginate gels “in-situ” is also feasible when a high concentration of metal ions is present in solution (ARAÚJO and TEIXEIRA, 1997; JANG et al., 1999).

Various chemical treatments may be applied on alginic acid in order to increase metal uptake capacity such as carboxylation, phosphorylation, and sulfonation (JEON et al., 2002), although these treatments tend to increase the cost of the resulting product.

ARAÚJO and TEIXEIRA (1997) studied the transport properties of Cr(III) on alginate beads using the Linear Adsorption model and the Shrinking Core model. For low Cr(III) concentration, ion exchange was the rate-controlling mechanism and the experimental results fit well with the Shrinking Core model. At higher concentrations, however, the Linear Adsorption model was a better fit for the experimental results and ionic exchange was no longer the main mechanism of sorption. The study of CHEN et al. (1993) indicated that Linear Adsorption model was preferable for the Cu calcium alginate gel.

1.3 Algal biosorption systems

Engineering considerations are very important during the development of an algal-based sorption system. All biosorption systems used biomass in solid form in a basic solid-liquid contact process, with, in certain cases, cycling of the process through biosorption and desorption stages (GARNHAM, 1997). The effluent to treat would make contact with the biosorbent in a batch, semi-continuous or continuous flow system. The following reactor types have been described by BANKS (1997) as potential biosorption systems:

  • Conventional stirred tank reactors;

  • Packed bed reactors (upflow and downflow);

  • Expanded bed reactors;

  • Fluidised bed reactors;

  • Airlift reactors.

In the cases of algal-based processes using actively growing biomass these can also be based on ponds, lagoons, streams and artificial stream meander units (VOLESKY, 1990).

1.4 Adsorption mechanisms

The chemical structure and metal sorption mechanisms of biomass have been extensively studied. VEGLIO and BEOLCHINI (1997) classified the biosorption mechanisms into two main categories, according to their cell functionality, i.e., metabolism-dependant and non-metabolism-dependant. The metabolism-dependant mechanism involves transport across the cell membrane and a precipitation step (BRIERLEY, 1990; COSTA and LEITE, 1990), whereas the non-metabolism-dependant mechanism consists of precipitation (HOLAN et al., 1993; SCOTT and PALMER, 1990), physical adsorption (AKSU et al., 1992; ZHOU and KIFF, 1991), ion exchange (FRISS and MYERS-KEITH, 1986; MURALEEDHARAN and VENKOBACHAR, 1990) and complexation (CABRAL, 1992; TSEZOS and VOLESKY, 1981). Another way to classify the mechanism is based on the location where the extracted metal accumulates; for example, there is intracellular accumulation (transport across membrane), cell surface adsorption/precipitation (ion exchange, complexation, physical adsorption, precipitation) and extra-cellular accumulation/precipitation (VEGLIO and BOELCHINI, 1997).

1.5 Adsorption models

Various models have been used to evaluate the experimental data in order to identify the sorption mechanisms, i.e., chemisorption, physical adsorption or ion exchange. Some studies have compared the ion exchange model with the Langmuir adsorption model (DA COSTA and DE FRANÇA, 1996; FIGUEIRA et al., 2000). The Langmuir adsorption model assumes that only one type of adsorption site exists (i.e., all surface sites have equal activity) and that adsorption equilibrium is reached with the formation of a monolayer (STUMM and MORGAN, 1996). This model does not take into account the speciation of the metal in solution and, therefore, it applies only if the ionic strength, the pH and the ligand concentration are constants.

The ion exchange model has been found to give the best fit for metal sorption on algae biomass because the sorption is accompanied by the release of ions (e.g., Ca2+, Mg2+, Na+ and K+) (CRIST et al., 1994; KRATOCHVIL et al., 1998; KUYUCAK and VOLESKY, 1988; SCHIEWER and VOLESKY, 1995). Experiments have been carried out to study several system variables, such as the initial concentration (CRIST et al., 1994), the sorbent particle size (FISHER, 1985), and the solution pH (JANG et al., 1995; LEE and VOLESKY, 1997). Similarly, experimental data have been analyzed to determine the reaction kinetic order of a pore/solid phase diffusion mechanism (HO and MCKAY, 2000).

Other models used to describe various biosorption isotherms include the Freundlich model, a combination of the Langmuir and Freundlich models, the Radke and Prausnitz model, the Reddlich-Peterson model, the Brunauer (BET) model, and the Dubinin-Radushkevich model (VOLESKY, 2003). The «Ideal Absorbed Solution Theory» (IAST) and the «Surface Complexation» (SCM) models have also been used for solutions containing a mixture of metal ions (VOLESKY, 2003). Some other structured types of models taking into consideration the metal speciation in solution, the pH and the electrostatic attraction in solution have been proposed by SCHIEWER and WONG (1999) and YANG and VOLESKY (2000).

1.6 Metal recovery

The metal-laden biosorbent can be either eluted and reused or disposed of in a safe manner. In the former case, the biosorbent operates much like an ion exchange resin. Metals can be eluted using a specific solution (the eluant) to generate a small volume of a concentrated solution (the eluate). The choice of eluant depends on the metal ion to be eluted. Common and heavy metals (e.g., Cd, Co, Cu, Mn, Pb, Zn) are usually eluted with dilute mineral acids (e.g., HCl, H2SO4, and HNO3) or concentrated saline solutions (e.g. 0.5 M NaCl) (GARNHAM et al., 1992b). EDTA has been used in certain cases, but it is generally more expensive than mineral acids or saline solutions (HORIKOSHI et al., 1979). The adsorption of some noble metals, such as gold, silver and mercury, shows little or no dependence on pH and, consequently, these metals cannot be removed with dilute acid solutions (EDYVEAN et al., 1997). Thiourea or mercaptoethanol solutions have been used for recovering gold from biosorbents (DARNALL et al., 1986; GREENE and DARNALL, 1990). Similarly, sodium acetate solutions are effective for eluting copper and silver (HARRIS and RAMELO, 1990). Sodium carbonate has been used to desorb uranium from the algae Chlorella regularis (NAKAJIMA et al., 1982).

In general, biosorbents decompose and char at relatively low temperatures. Therefore, metal-laden biosorbents can be readily burned to produce an ash residue having a high metal concentration. This alternative may be economically viable for systems dealing with valuable metals and/or inexpensive biosorbents (GARNHAM, 1997). Alginic acid powder and calcium alginate beads have high affinity and capacity sorption for Fe(III), and the extraction of Fe(III) from acid synthetic solution is technically feasible (RIVEROS et al., 2001). Applied to acid mine drainage, the Fe(III) extraction would result in a significant reduction of the lime consumption and the volume of the neutralization sludge (RIVEROS, 2004). Once adsorbed, the Fe may be eluted and precipitated as hematite in order to obtain marketable and useful product (DUTRIZAC and RIVEROS, 1999).

1.7 Cost analyses

Preliminary costing evaluation for biosorption treatment options were conducted by ADERHOLD et al. (1996) and VOLESKY (1999). The results indicate that biosorption is a cost-effective technology. The cost-benefit analysis of any treatment option presents various difficulties, such as the lack of publicly available information on operating cost and the long-term impact of the treatment operation. This is particularly true for biotechnological processes. However, a comparative cost study was conducted for biosorptive processes with ion exchange and chemical precipitation (ECCLES, 1995). The selection of an effluent treatment system needs to comply with various criteria, such as compatibility with existing operations, cost effectiveness, flexibility to handle fluctuation in quality and quantity of effluent feed. The system should also be reliable, robust, selective and simple (ECCLES, 1995). Eccles compared the AMT-Bioclaim-process-based hard granular biomass, Bacillus subtilis (BRIERLEY et al., 1986) with the chemical precipitation method. The predicted results showed that the AMT-Bioclaim method could reduce the cost per gallon by over 50% when compared with a chemical treatment method. A second study was completed by the author to compare the Biofix process with chemical precipitation to treat acid mine drainage. The Biofix process consists of a mixture of biomass including bacteria, algae and fungi immobilized in polyethylene beads. Using the data from JEFFERS (1994), the acid mine drainage (AMD) treatment cost was 1.4 US$ per 1000 US gallons for the Biofix process and for conventional lime treatment, it was calculated the cost would correspond to 1.5 US$ (ECCLES, 1995). Table 5 summarizes the treatment options, along with their advantages and disadvantages.

Table 5

Treatment options for the removal of heavy metals (adapted from ADERHOLD et al., 1996).

Options de traitement pour l’enlèvement des métaux (adapté d’ADERHOLD et al., 1996).

Treatment options



Lime precipitation

Relatively inexpensive

Bulk removal

Non selective

Ion exchange

Multiple ion-exchange resins

High specificity for heavy metal

Several sorption and desorption cycles

No sludge production

Electrolysis allows metal recycling

High capital and operating costs

Economic of these process depends on energy price and the amount of electricity used per treated volume of solution

Membrane processes


Reverse osmosis


Very specialized application

Limited flow rate

Membrane instability in salt and acid conditions

Prohibitive cost

Adsorption processes

Versatile, simple

Selectively sorbed the sorbate

Low cost technology


-> Voir la liste des tableaux

2. Other Natural Sorbents

Several research papers have been published about the use of a variety of natural sorbents to remove metals from synthetic or industrial effluents. Table 6 shows different studies conducted on the utilization of natural sorbents for the removal of several metals (Ag, Al, As, Au, Ba, Bi, Ca, Cd, Co, Cr, Cu, Fe, Hg, Ir, Mg, Mn, Mo, Na, Ni, Os, Pb, Pd, Pt, Ra, Sb, St, Ti, Tl, V, Zn, Zr), lanthanides (Ce, Eu, La, Yb) and actinides (Th, U).

Table 6

Studies on the adsorption of different metals using natural adsorbents.

Études portant sur l’adsorption de différents métaux sur des adsorbants naturels.



Aluminium (Al) (III)

Crist et al. (1994), Orhan and Büyükgüngör (1993), CUI et al. (2006)

Antimony (Sb) (III)

Coupal and Lalancette (1976), Masri and Friedman (1974)

Arsenic (As) (II, V)

Loukidouet al. (2003), Masri and Friedman (1974)

Barium (Ba) (II)

Cristet al. (1994), Smithet al. (1977)

Bismuth (Bi) (III)

Masri and Friedman (1974), Shimizu and Takada (1997)

Cadmium (Cd) (II)

Volesky and Prasetyo (1994), YU et al. (1999)

Calcium (Ca) (II)

Fiset et al. (2002), Fourest and Volesky (1997)

Cerium (Ce) (III)

Masri and Friedman (1974)

Chromium (Cr)(III, VI)

Baileyet al. (1992), FISHER et al. (1984)

Cobalt (Co) (II)

Flynnet al. (1980), Kuyucak and Volesky (1988)

Copper (Cu) (I, II)

MCKAY et al. (1999), YU et al. (1999), CUI et al. (2006)

Europium (Eu) (III)

Andreset al. (1993)

Gold (Au) (III)

Kuyucak and Volesky (1988), Nakajima (2003)

Iridium (Ir) (IV)

Ruizet al. (2003)

Iron (Fe) (II, III)

Fisetet al. (2002), Nassaret al. (2004), CUI et al. (2006)

Lanthanum (La) (III)

Bloom and McBride (1979), Cristet al. (1994)

Lead (Pb) (II)

Holan and Volesky (1994),YU et al.(1999), Murathan and Bütün (2006)

Magnesium (Mg) (II)

Crist et al. (1994), Fisetet al. (2002), CUI et al. (2006)

Manganese (Mn) (II)

Fiset et al. (2002), Nassaret al. (2004), CUI et al. (2006)

Mercury (Hg) (I, II)

FISHER et al. (1984), Viraraghavan and Kapoor (1994)

Molybdenum (Mo) (VI)

Guibal et al. (1999), Sakagushi et al. (1981)

Nickel (Ni) (II)

Flynnet al. (1980), Leuschet al. (1995)

Osmium (Os) (IV)

Ruizet al. (2003)

Palladium (Pd) (II)

Baba and Hirakawa (1992), Guibal et al. (2001)

Platinum (Pt) (IV)

Baba and Hirakawa (1992), Guibal et al. (2001)

Radium (Ra) (II)

TSEZOS (1997), TSEZOS and KELLER (1983)

Silver (Ag) (I)

FISHER et al. (1984), Flynnet al. (1980)

Sodium (Na) (I)

Fisetet al. (2002), Spintiet al. (1995)

Strontium (Sr) (II)

Shimizu and Takada (1997); Small et al. (1999)

Technetium (Tc) (VII)

Garnhamet al. (1992a, 1993b)

Thallium (Tl) (I)

Masri and Friedman (1974)

Thorium (Th) (IV)

Masri and Friedman (1974), Tsezos and Volesky (1981)

Titanium (Ti) (IV)

Parkash and Brown (1976)

Uranium (U) (IV, VI)

Guibal et al. (1994), Tsezos and Volesky (1982)

Vanadium (V) (V)

Guibal et al. (1994)

Ytterbium (Yb) (III)

Andres et al. (1993)

Zinc (Zn) (II)

Artola and Rigola (1992); Kuyucak and Volesky (1988)

Zirconium (Zr) (IV)

Garnhamet al. (1993a), Parkash and Brown (1976)

-> Voir la liste des tableaux

2.1 Microorganisms

Many studies have been carried out on the utilization of dead or living microorganisms, including bacteria, yeasts, fungi, microalgae, cyanobacteria and activated sludge biomass for metal removal from solutions. Some examples of different microorganisms used for their metal adsorption capacity are presented in Table 7. The metal adsorption on the cell surface of non-living microorganisms usually involves different functional groups such as carboxyl, amino, hydroxyl, sulfhydryl, phosphate and sulfate groups (KAPOOR and VIRARAGHAVAN, 1997; URRUTIA, 1997).

Table 7

Some examples of the microorganisms studied for the metal recovery from solutions.

Exemples de microorganismes étudiés pour la récupération de métaux en solution.





Bacillussubtilis and spp.

Beveridgeet al. (1982), Cotoraset al. (1992), GREEN-RUIZ (2006)

Micrococcus spp.

Cotoraset al. (1992), Loet al. (2003)

Mycobacterium spp.

Andres et al. (1993)

Pseudomonas spp.

Cabral (1992), Lopezet al. (2002), D’SOUZA et al. (2006)

Streptomyces spp.

Friss and Myers-Keith (1986), Mattuschka and Straube (1993)

Zooglea ramigera

Aksu et al. (1992), Norberg and Persson (1984)



Candida spp.

Aksu and Donmez (2001)

Candida utilis

kujan et al. (2006)

Saccharomyces cerevisiae

Kuyucak and Volesky (1988), Volesky et al. (1993)



Aspergillus niger

Venkobachar (1990)

Aureobasidium pullulans

Gadd and De Rome (1988)

Cladosporium resinae

Gadd and De Rome (1988)

Funalia trogii

ARICAet al. (2004)

Ganoderma lucidum

Venkobachar (1990)

Penicillium spp.

Loukidouet al. (2003), Sayet al. (2003)

Rhizopus arrhizus

Fourest and Roux (1992), Tsezos and Volesky (1982)

Trametes versicolor

Bayramogluet al. (2003)



Chlorella vulgaris and spp.

Aksu and Acikel (1999), Mehtaet al. (2002)

Chlamydomonas spp.

Garnham et al. (1992a), Sakaguchiet al. (1981)

Eudorina spp.

Tien (2002)

Euglena spp.

Mannet al. (1988)

Scenedesmus spp.

Garnhamet al. (1993a), Sakaguchiet al. (1981)

Synechocystis aquatilis

ergene et al. (2006)



Anabaena spp.

Garnhamet al. (1993b), Tien (2002)

Nostoc spp.

Fernandez-Pinaset al. (1991), Hassett et al. (1981)

Oscillatoria spp.

Fisheret al. (1984), Tien (2002)

Synechoccus spp.

Garnham et al. (1993a, b), Sakaguchiet al. (1978)



Activated sludge

Artola and Rigola (1992), Hammainiet al. (2003)

-> Voir la liste des tableaux

2.2 Forestry industry wastes

Forestry industry wastes including sawdust and tree barks, which are lignin/tannin-rich materials, have been also intensively studied for metal recovery from solutions (FISET et al., 2000; SEKI et al., 1997; VAISHYA and PRASAD, 1991). The polyhydroxy polyphenol groups of tannin are thought to be the active species in the metal adsorption (ion-exchange) process (VASQUEZ et al., 1994). Lignin extracted from black liquor, a waste product of the paper industry, has been considered for metal adsorption, specifically Hg, Pb and Zn (MASRI et al., 1974; SRIVASTAVA et al., 1994). Lignin (Figure 2) contains polar functional groups, such as alcohols, acids, aldehydes, ketones, phenol hydroxides and ethers, which have varying metal binding capabilities (BAILEY et al., 1999).

Figure 2

The chemical structure of lignin.

Structure chimique de la lignine.

The chemical structure of lignin.

-> Voir la liste des figures

2.3 Aquatic plants

Some aquatic plants (e.g.Ceratophyllum demersum, Lemna minor, Myriophyllum spicatum) have also been tested for phytoremediation or phytofiltration of metal-contaminated effluents (AXTELL et al., 2003; KESKINKAN et al., 2004 SCHNEIDER et al., 2001). Chemical modification and spectroscopic studies have shown that the cellular components include carboxyl, hydroxyl, sulfate, sulfhydryl, phosphate, amino, amide, imine, and imidazol moieties, which have metal binding properties and are, therefore, the functional groups in these plants (GARDEA-TORRESDEY et al., 2004).

2.4 Chitin and chitosan

Various researchers have utilized chitin and chitosan for removing metal ions from effluents (MCKAY et al., 1989; HSIEN and RORRER, 1995). Chitin (Figure 3) is the second most abundant natural biopolymers after cellulose (BABEL et al., 2003). This natural biopolymer is widely found in the exoskeleton of shellfish and crustaceans (KIM and PARK, 2001). Chitosan (Figure 4) is produced by alkaline N-deacetylation of chitin. Crab shells or seafood processing waste sludge can also be used directly for metal adsorption without chitin extraction (KIM and PARK, 2001; LEE and DAVIS, 2001). The metal ions adsorption on chitosan mostly involved free amine groups. However, the binding ability of these sorbents for various metal ions is not directly proportional to the degree of free amine content (EDYVEAN et al., 1997).

Figure 3

The chemical structure of chitin.

Structure chimique de la chitine.

The chemical structure of chitin.

-> Voir la liste des figures

Figure 4

The chemical structure of chitosan.

Structure chimique du chitosan.

The chemical structure of chitosan.

-> Voir la liste des figures

2.5 Peat moss

Peat moss, which is also very abundant in nature, has been intensively studied for water decontamination and particularly for the metal removal from waste streams (KERTMAN et al., 1993; SHARMA and FORSTER, 1993; VIRARAGHAVAN and RAO, 1993). Peat moss is a complex material, having lignin and cellulose as its major components. Both these components contain polar functional groups, such as carboxylic acids, phenol hydroxides, alcohols, aldehydes, ketones and ethers, which bind metal ions (BROWN et al., 2000. COUILLARD, 1994; WASE et al., 1997).

2.6 Agricultural wastes

Other types of natural sorbents proposed in the literature for metal retention include different agricultural wastes (e.g., tea/coffee and rice residues, fruit and vegetable peels, nut skins/husks). Some examples of these inexpensive and readily available materials are presented in Table 8. The polyhydroxy polyphenol groups, as well as, carboxylic and amino groups, found in these materials are involved in the metal adsorption (ion-exchange) process (MEUNIER et al., 2003b; RANDALL et al., 1974).

Table 8

Agricultural wastes studied for the metal recovery from solutions.

Déchets agricoles étudiés pour la récupération de métaux en solution.



Banana pith and peels

Annaduraiet al. (2003), Lowet al. (1995)

Canola meal

Al-Asheh and Duvnjak (1996)

Carrot residues

Nasernejadet al. (2005)

Cassava fibre

ABIAet al. (2006)

Chicken feathers

Al-Ashehet al. (2002)

Cocoa shells

Fiset et al. (2002), Meunieret al. (2003a, b, 2004)

Coconut byproducts

Randallet al. (1974), OFOMAJA and HO (2007), Mohan et al. (2006)

Coffee residues

Minamisawaet al. (2002)

Corn cobs and roots

Bosincoet al. (1996), Goldberg and Grieve (2003)

Grape stalks

Fiol et al. (2006), Escuderoet al. (2006)

Indian mustard

Crist et al. (2004)

Modified wool

Marshall and Champagne (1995)

Nut and walnut shells

Orhan and Büyükgüngör (1993)

Olive mill residues

Gharaibehet al. (1998), Veglioet al. (2003)

Onion peels

Kumar and Dara (1982)

Orange peels

Ajmalet al. (2000), Masriet al. (1974)

Palm kernel fibre

Ho and OFOMAJA (2006)

Peanut skins

Chamarthyet al. (2001), Randall et al. (1974)

Petiolar felt-sheath of palm

Iqbal and Saeed (2002)

Rice byproducts

Ajmal et al. (2003), Montanheret al. (2005)

Sheep manure wastes

Al-Rubet al. (2003)

Sunflower seed peel

Ozdemiret al. (2004)

Tea leaves

Orhan and Büyükgüngör (1993), Tee and Khan (1988)

-> Voir la liste des tableaux

2.7 Miscellaneous sorbents

Finally, other natural sorbents studied include notably animal bones (BANAT et al., 2002), clays (e.g. bentonite, kaolinite, montmorillonite, wollastonite) (CELIS et al., 2000; PRADAS et al., 1994), human hair and teeth (HELAL et al., 2002; TAN et al., 1985), leaf mould (SHARMA and FORSTNER, 1994), sand (AWAN et al., 2003), metal oxides (Al, Fe, Mn – oxides) (BAILEY et al., 1992; TRIVEDI and AXE, 2001), vermicompost (PEREIRA and ARRUDA, 2003), xanthate (FLYNN et al., 1980; JAWED and TARE, 1991), and zeolites (e.g., clinoptilolite and chabazite) (GENÇ-FUHRMAN, 2007; LEPPERT, 1990; KALLO, 2001; OLIVEIRA et al., 2004).

2.8 Industrial applications

The majority of studies on metal adsorption on biosorbents have been carried out using synthetic solutions containing one or several metal ions (BLAIS et al., 2003; CRIST et al., 1994; MASRI and FRIEDMAN, 1974). However, many research papers have shown the efficiency of biosorbents for the removal of metal ions from industrial wastewaters and acid mine drainage solutions (MCGREGOR et al., 1998; UTGIKAR et al., 2000; ZOUMIS et al., 2000), landfill leachates (ABOLLINO et al., 2003; CECEN and GURSOY, 2001), tannery wastewaters (ALVES et al., 1993), electroplating effluents (AJMAL et al., 1996, 2000; ALVAREZ-AYUSO et al., 2003; LO et al., 2003), acid leachates from sewage sludge decontamination (FISET et al., 2002), acid leachates from soil decontamination (MEUNIER et al., 2004), and alkaline leachates from air pollution control residues from municipal solid waste incinerators (BLAIS et al., 2002a, BLAIS et al., 2002b).

Biosorption has proved to be effective for removing metal ions from contaminated solutions and effluents. The main advantages of biosorption over conventional treatment techniques include lower capital and operating costs, arising from the use of abundant and inexpensive natural products, and lower disposal cost of the spent adsorbents because of their biodegradable nature. However, industrial applications of biosorption are rare, and this situation has been attributed to the non-technical gaps involved in the commercialization of technological innovations (VOLESKY and NAJA, 2005). Furthermore, most biosorption studies have been conducted in batch systems, rather than in the continuous systems that are typical of industrial applications, such as fluidized bed and packed bed columns and continuous stirred tank reactors (MEHTA and GAUR, 2005). Despite these facts, VOLESKY and NAJA (2005) have identified some industrial operations which represent a big potential market for biosorption applications; these include electroplating and metal finishing, mining and ore processing, smelting, leather processing and printed circuit board manufacturing. However, as some of these sectors may be reluctant to novel biotechnology applications, biotechnology industries may have to share the risk with the industry. Therefore, biotechnology industry may have to develop partnership with industries in order to finance, build and operate the treatment plant or to provide a turnkey operating plant.


Biosorbents, especially those derived from seaweed and alginic acid, have attracted much interested in recent years as a source of inexpensive adsorbents for toxic metallic ions. Biosorbents are widely available in nature, can be readily produced under various forms, and are both non-toxic and biodegradable. These characteristics give them a definitive advantage over synthetic products for the removal of toxic metals from industrial effluents. The physical stability of biosorbents, especially in alkaline conditions continues to be a drawback and more research is needed in this area.

Parties annexes