BioMed Research International

BioMed Research International / 2014 / Article

Review Article | Open Access

Volume 2014 |Article ID 146769 | 24 pages | https://doi.org/10.1155/2014/146769

Assessment of Food Processing and Pharmaceutical Industrial Wastes as Potential Biosorbents: A Review

Academic Editor: Qaisar Mahmood
Received28 Feb 2014
Revised03 Jun 2014
Accepted03 Jun 2014
Published07 Jul 2014

Abstract

There is a growing need for the use of low-cost and ecofriendly adsorbents in water/wastewater treatment applications. Conventional adsorbents as well as biosorbents from different natural and agricultural sources have been extensively studied and reviewed. However, there is a lack of reviews on biosorption utilizing industrial wastes, particularly those of food processing and pharmaceuticals. The current review evaluates the potential of these wastes as biosorbents for the removal of some hazardous contaminants. Sources and applications of these biosorbents are presented, while factors affecting biosorption are discussed. Equilibrium, kinetics, and mechanisms of biosorption are also reviewed. In spite of the wide spread application of these biosorbents in the treatment of heavy metals and dyes, more research is required on other classes of pollutants. In addition, further work should be dedicated to studying scaling up of the process and its economic feasibility. More attention should also be given to enhancing mechanical strength, stability, life time, and reproducibility of the biosorbent. Environmental concerns regarding disposal of consumed biosorbents should be addressed by offering feasible biosorbent regeneration or pollutant immobilization options.

1. Introduction

Increased industrial activities resulted in major environmental problems; one of the most challenging is water pollution and the subsequent scarcity in fresh and clean water resources available for current and future generations. Industrial wastewater contains various toxic compounds such as organics, heavy metals, and dyes which could have potential detrimental effect on human beings and aquatic lives. World Health Organization (WHO) recommended the maximum acceptable concentrations for these compounds in water streams. Dyes are one of the most polluted groups as their complex aromatic structure makes them difficult to be biologically degradable [13]. They are produced from different industries in large amounts such as textile, paper, leather, food, cosmetics, and pharmaceuticals. It has recently been reported that dye production reached 700,000 tons/year worldwide [4]. Dyes are classified into anionic (direct), cationic (basic), acid and reactive, and nonionic (disperse) dyes [5]. Phenols and phenolic compounds are very toxic and of potential harm to human health. Even at very low concentration (0.005 mg/L), phenols could be of significant odor and taste if present in drinking water [6]. Many industries represent the main sources of phenols such as iron and steel, petroleum, paint, paper and pulp, and pharmaceutics. Nitrophenols and chlorophenols are considered the most hazardous phenolic compounds. Heavy metals are another hazardous group of pollutants. Lead, mercury, cadmium, chromium, copper, and arsenic are examples of the most toxic and carcinogenic elements that can exist in industrial effluents. Metal ions accumulate and their amounts are increased along the food chain due to their nonbiodegradable feature [7, 8]. The main industrial sources of most of these metals are metal finishing and plating, automotive, semiconductor manufacturing, textile, and steel industry.

Removal of such pollutants from different industrial effluents may be achieved physically, chemically, or biologically. Physical processes include adsorption, chelation ion exchange, membrane filtration, and coagulation. Chemical methods include oxidation or advanced oxidation and electrochemical treatment, whereas biological methods could be aerobic, anaerobic, or enzymatic [810]. These processes known as conventional treatment methods have several disadvantages mainly, high energy requirements and capital cost and low efficiency. Conventional treatment methods have been extensively reviewed elsewhere [3, 9, 1113]. Recently, numerous approaches have been proposed by many researchers for the development of nonconventional and low-cost adsorbents.

Biosorption has become an attractive common technique for many reasons. Being a cost-effective, highly efficient, and easily implemented method made it a successful alternative for the conventional ones [14]. Biosorption as a process may be simply defined as an adsorption on the surface of a compound of a biological origin. Being not limited to only one mechanism and also not restricted to a specific type of pollutant offers a wide variety of applications like pollution control, element recycle, and recovery [10]. A biosorbent may be considered “low-cost” if it satisfied the following conditions: (i) abundance in nature, (ii) requirement for minor or no treatment, and (iii) being a waste material or a by-product from other industries [10]. The challenge here is to choose the appropriate biosorbent that suits the target substance. Selection criteria include, but are not limited to, nature of substance to be adsorbed, mechanism involved in the biosorption process, effectiveness of such biosorbent, cost associated with the whole process, and the possibility of biosorbent regeneration for multiple use cycles. Numerous reviews have been reported on the utilization of agricultural-based, dead or living biomass, and natural adsorbents for the removal of dyes [1521] and heavy metals [2228]. Few research studies have focused on the removal of organic pollutants, phenols and phenolic compounds, and pesticides using different biosorbents [2934].

Disposal of different industrial wastes and by-products is considered a major environmental problem. The cost associated with the waste treatment or disposal, transport, and accumulation may sometimes be the most challenging problem in industry. Such problem increases especially in food industries which produce huge amount of wastes and by-products. Utilizing industrial wastes as low-cost effective biosorbents introduces a bifunctional solution from an environmental point of view. That is to say, treating wastewater effluents with these zero-cost waste materials adds value to these wastes while help solving an important environmental issue.

This paper reviews the state-of-the-art endeavors in utilizing industrial food processing and pharmaceutical wastes as effective low-cost biosorbents for water/wastewater treatment. The aim is to assess the potential of these wastes as biosorbents as well as highlight new options to be further explored and possibilities for improvement. To the best of the authors’ knowledge, research dedicated to these particular types of waste has not been reported elsewhere. A comprehensive critical review is presented on (i) the different biosorption techniques and mechanisms, (ii) controlling factors, (iii) equilibrium and kinetics studies, and (iv) recovery and/or pretreatment options. Moreover, concluding remarks will be given at the end along with some suggestions for future work.

2. Sources and Applications of Biosorbents

Adsorption as a process gained much more attention recently after the use of low-cost adsorbents became so popular especially biosorbents [24, 35]. Sources of different types of conventional and nonconventional adsorbents are illustrated in the flow chart in Figure 1.

Biosorbents are a large subclass of low-cost adsorbents that can be subdivided into [36] biomass (dead or living), agricultural wastes, and industrial solid wastes. Dead biomass has been utilized by many researchers as an effective biosorbent for the removal of different pollutants [37, 38]. It has been favored due to its viability to be applied in presence of toxic substances or with shortage of nutrients without this causing appreciable impact on its sorption efficiency. In addition, dead biomass is more readily desorbed than its living counterpart. Living biomasses including fungi [39, 40], algae [41, 42], and other microbial cultures with different strains [43, 44] were also used as low-cost biosorbents. Agricultural-based biosorbents represent a large category of wastes that attracted the attention of many researchers worldwide Utilization of such wastes depended on their local availability. Researchers utilized rice husk and straws [4548], different nut shells [4951], fruit and vegetable peels or leaves [5255], wheat bran [56], chitin and chitosan [5760], and many other wastes of agricultural origin. Applications of industrial solid wastes in biosorption included the use of sludge whether municipal (sewage) [61] or activated sludge produced from different biological processes [6266].

Less research has been done on industrial food processing and pharmaceutical wastes despite their huge annual worldwide production. Scarcity of relevant reviews was therefore the main motivation of this current work. Biosorbents from these origins are expected to grow by an annual rate of around 5% in the next few years [67]. For example, food processing waste produced annually in Europe has been reported to be about 2.5 × 108 tons [67]. About 20–60% of the processed fruits and vegetables by volume are generated as waste materials. In the United States, the food manufacturing sector is producing a huge amount of food waste; about 44.3 billion pounds have been reported as per the year 2011 [68].

Utilizing these wastes as biosorbents has been applied in the area of water purification and/or wastewater treatment; previous work in this regard is summarized in Table 1. The table presents type and industrial source of the biosorbent, nature of feed solution, type of targeted sorbate, and operating parameters at which maximum removal was attained. These parameters are pH, temperature, adsorbent dose, and the contact time that was required to reach equilibrium. In addition, mode of operation (batch or column) and its corresponding maximum % removal are included in the table. For column systems, the flow rate () is also given. Wastes from beverages, tea or coffee, beer or wine, and brewery grains, were used as biosorbents for the removal of many heavy metals and dyes from aqueous solutions [6983]. Excellent removal efficiencies of up to 99.83% for Cd and 98% for dye sorption onto yeast beer waste [80] and brewery grain wastes [76] were reported. Using beer brewery diatomite waste was recommended for wastewater treatment applications. This is because it released less COD in the industrial wastewater than did the fresh diatomite [81]. Food processing wastes from canning industries were also utilized for the removal of different dyes and heavy metals [8489]. One particular study was undertaken on real textile wastewater having COD of 426 mg/L, and 97.68% dye removal was achieved when the wastewater sample was spiked with 1 mg/L dye [90]. Studies on the effect of several operating conditions on biosorption performance were also conducted. Results yielded removal efficiencies that reached up to 96.4% for the removal of Cd (II) in case of using okra waste [88] and sugar bagasse waste [89]. Wastes from fruit sources especially orange, mango, and pectin-rich fruits were obtained from juice, jam [9199], and coconut milk industries [100]. Orange peel [92] and wastes [95] were very effective in removing heavy metals, namely, Pb (II) and Cd (II), with efficiencies of 99.5% and 98%, respectively.


Type of biosorbentSource of biosorbentFeed solutionSorbatepHContact time, minTemperature, °CInitial concentration of sorbate, mg/LMode of operationMaximum
%removal
Biosorbent doseReference

Spent brewery grains (SBG)Mohan breweries and distilleries Limited, Chennai, IndiaSynthetic dye solutionAG25 acid dye of commercial name Alizarin Cyanin Green G3.0753090 Batch980.2 [70]

Tea industry wasteLocal tea factory in ChinaAqueous synthetic solutionCd(II)7.01802520 Batch905[72]

Exhausted coffee wasteSoluble coffee manufacturer, Catalonia, SpainAqueous synthetic solutionCr(VI)
Cu(II)
Ni(II)
3.08640251000Batch6.67[77]

Sugarcane bagasse wasteFrom local alcohol and sugar Aqueous synthetic  solutionMethylene Blue (MB) 7.0600 25200 Batch 0.2 [78]
Industries, City of Ouro Preto, Minas Gerais, BrazilGentian Violet 900300

Wine processing waste sludge (WPWS)Ilan Wine-Processing Company, Ilan, TaiwanAqueous synthetic solutionCr(III, IV)2.024030100 Batch3610[73]

Wine processing waste sludge (WPWS)Ilan
Wine-Processing Co., Ilan, Taiwan
Aqueous synthetic solutionNi(II)5.51205030 Batch7512[76]

Grape bagasse waste residueWine production process, Styria region, AustriaEffluent from research laboratoryCd(II)
Pb(II)
7.0
3.0
4525100Batch0.67[79]

Waste beer yeastAoke Beer Company in Zhengzhou, Henan province, ChinaAqueous synthetic solutionCu(II)
Pb(II)
5.030209.14
32.23
Batch[69]

Waste beer yeast Saccharomyces  cerevisiae Beer fermentation industry, brewery located near Chennai, IndiaElectroplating effluentsCr(VI)5.0120Batch0.02 [74]

Suspended brewery yeast waste biomass
(SBW)
Brewery waste biomass collected from CIUC brewery, Miercurea-Ciuc, RomaniaSynthetic aqueous solutionCd(II)5.540506Batch99.839.78[80]

Beer brewery diatomite waste (SDE)Shan-Hua factory, Tobacco and Liquor Co., TainanTaiwanSynthetic aqueous solution
Industrial wastewater from local factory
Methylene Blue (MB) basic dye7.01440252.5Batch0.25[81]

Spent waste beer yeast
Saccharomyces  cerevisiae
Fermentor at a brewery, Chennai, IndiaBattery manufacturing industrial effluentPb(II) 5.012030100Batch[82]

Fresh malted sorghum mash wastelocal malted sorghum beer (pito) brewer at Navrongo, GhanaSynthetic aqueous solutionMethylene Blue (MB) basic dye7.018 50Batch>904[83]

Waste biomass from sugarcane aguardenteBrazilian alcoholic beverage production, (Lapinha, Bocaiana, Germana and Taboroa) State of Minas Gerais, BrazilStainless steel effluentCr(VI)
Fe(III)
Ni(II)
4.01802550
660
20
Batch70
50
20
1[75]

Waste biomass Cachaça Brazilian alcoholic beveragethe stillage generated by a liquor distillery (Germana), Minas Gerais, BrazilStainless steel industrial effluent from Acesita Co., BrazilFe(III)
Ni(II)
Cr(VI)
4.0180257.8
2.7
600
Batch94
57
25
2 [71]

Rhizopus oligosporus biomassFood processing wastewatersAqueous synthetic solutionCu(II)5.012030100 Batch701 [85]

Waste biomass of Phaseolus  vulgaris  L. A residual biomass of a canned food factory in Bartin, TurkeyAqueous synthetic solutionPb(II)5.02020100 Batch924 [84]

Waste biomass of Phaseolus  vulgaris  L. A residual biomass of a local canned food plant, TurkeyAqueous synthetic solutionTextile Reactive Red dye (RR 198)2.02020100–300Batch99.31.6[86]

Cupuassu shell, Theobroma  grandiflorum, (CS) Food residue from jelly industry, Belém-PA, Brazil Aqueous synthetic solutionReactive Red dye (RR 194) 2.0480 25 50 Batch 2.5 [87]
Direct Blue 531080

Okra food industrial wasteFood waste from food canning processesAqueous synthetic solutionCd(II)
Fe(II)
Zn(II)
9020Batch96.4
93.8
79.8
1[88]

Sugar industrial waste (bagasse waste)Obtained from food canning processesAqueous synthetic solutionCd(II)
Fe(II)
9020Batch96.4
93.8
1[89]

Pineapple peel, an agricultural effluent Food can processing industriesAqueous synthetic solutionMethylene Blue (MB) cationic dye6.040030300 Batch471.5 [91]

Waste baker’s yeast biomassPakmaya Yeast Company, Izmir, TurkeyAqueous synthetic solutionCd(II)
Pb(II)
6.0
5.0
1803025Batch60
70
1[131]

Desiccated coconut waste sorbent (DCWS)By-product of Coconut Milk Processing Aqueous synthetic solutionHg(II)7.42880
400
3050
100
Batch Column1
= 4 mL/min
[100]

Pecan nut shells (C. illinoinensis) biomassBiomass from food factories, Nuevo Leon, MexicoAqueous synthetic solutionAcid Blue 74 (AB74) 6.5500 30 100 Batch
Column
10
 mL/min
[132]
Reactive Blue 4 (RB4)1000
Acid Blue 25 (AB25)500

Orange peelSolid waste from local fruit juice industries, EgyptAqueous synthetic solutionPb(II)
Cu(II)
Cd(II)
5.0302520 Batch99.5
89.57
81.03
4 [101]

Orange (Citrus sinensis) wasteAgrumexport, S.L., an orange juice manufacturing company
located in Murcia, Spain
Aqueous synthetic solutionCr(III)4.0
4.0
4320
1523
25
25
100
20
Batch Column81
57.5
4 [102]

Pectin-rich fruit wastesResidues from fruit juice and wine production, from a citrus-juice producer (Sunkist), USAAqueous synthetic solutionCd(II)5.05060 Batch462 [133]

Orange wasteFrom orange juice industry, SpainAqueous synthetic solutionCd(II)6.06025100 Batch984 [94]

Orange wasteFrom orange juice industry, SpainAqueous synthetic solutionCd(II)
Zn(II)
Cr(III)
4.0180
180
4320
2015
15
15
Batch86
90
95
4[95]

Peach and Apricot stonesSolid wastes of juice and jam industries, EgyptAqueous synthetic solutionPb(II)7.0180
300
54.65Batch97.64
95.3
10[97]

Mangifera  indica (mango) seed kernel particlesLocal juice manufacturing industryAqueous synthetic solutionMethylene Blue (MB) cationic dye8.012030100Batch96.170.67[98]

Mango seeds (MS) Mangifera  indica  L. Juice producer, Ubá-MG, BrazilAqueous synthetic solutionVictazol Orange 3R dye (VO-3R)2.03602540Batch2.5[99]

Waste cider yeast
biomass
Fermentation Lab at the College of Food Science and Engineering of Northwest A & F University (Yangling, China)Apple juice solutionPatulin (PAT)4.52160250.1
0.2
Batch Column58.295
= 2 mL/min
[117]

Dairy sludgeDairy plant, FranceAqueous synthetic solutionPb(II)
Cd(II)
5.050020200
100
Batch>900.5–4.0 [129]

The waste pomace of olive oil factory (WPOOF)Turkish
Prina, Aegean region, Manisa, Turkey
Aqueous synthetic solutionCr(VI)2.01206050
100
Batch Column100
21.74
5
= 5 mL/min
[101]

Solid waste from
olive oil production
The OS and OMS wastes were provided by the “Cooperativa Nuestra S nora desl Castillo” extraction plant located in Vilches, in the province of Jaen (Spain)Aqueous synthetic solutionPb(II)5.012025Batch10 [102]

Olive mill waste (OMW) two-phase decanterMixture of pulp and olive
stones from the crushing of olives to obtain the oil, UK
Aqueous synthetic solutionPb(II)
Cd(II)
Cu(II)
Hg(II)
Fe(II)
7.0302010Batch80
75
10 [103]

Olive mill residues (OMR)Solid residues of oil production, provided by an olive mill in Abruzzo, Italy.Aqueous synthetic solutionCu(II)5.5
4-5
150–1440Room temperature40
40
Batch Column60%
10
80
[104]

Palm oil mill effluent (POME) sludgeWaste sludge from palm oil mill, Felda Taib Andak, Johor, MalaysiaAqueous synthetic solutionMethylene Blue (MB) cationic dye7.5432027100Batch2[111]

Sunflower oil
Waste biomass
Biomass obtained from a sunflower oil production
Facility, Seville, Spain
Aqueous synthetic solution
(mixed solution)
Pb(II)
Ni(II)
Zn(II)
Cu(II)
4.010Column  L/h[112]

Crushed olive stone wastesSupplied by an olive oil
Producer, Cordoba, Spain
Aqueous
synthetic
solution
Pb(II)
Ni(II)
Cu(II)
Cd(II)
5.5602018.86
4.20
4.35
4.80
Batch79
70
81
95
13.3 [105]

Waste olive cake (OC)Supplied by “ProBeira” an olive oil producer, Envendos PortugalAqueous
synthetic
solution
Zn(II)6.0-7.01202510Batch931[108]

Olive stones
From the orujo oil extraction plant ‘‘Orujera
Ubetense, Sociedad Cooperativa Andaluza,’’ Jaen, Spain
Aqueous
synthetic
Solution
Cd(II)113604010 Batch900.01 [106]

Olive pomaceSupplied by an Italian olive oil production
plant
Aqueous
synthetic
Solution
Cu(II)
Cd(II)
Pb(II)
5.060Batch10 [107]

Olive pomace
Supplied by one of the olive oil production
Plants, Jordan
Aqueous
synthetic
Solution
Methylene Blue (MB) dye2402510
40
Batch Column80
62.25
2
 mL/min
[109]

Olive pomace
OP-1
OP-2
OP-3
Solid by-products of olive oil processing mills, the island of Lesvos, Greece.Oil mill waste water (OMWW)Phenol10.01202050
500
Batch Column>90
90
10
 mL/min
[110]

Activated carbon derived from exhausted olive waste cakeOlive waste cake from oil factory “Agrozitex” Sfax, TunisiaSynthetic aqueous solution
Industrial wastewater from local factory
Lanaset Grey G 6.0300025150Batch931.67[113]

Activated carbon derived from empty fruit bunch (EFB)Industrial waste from united palm oil mill, Nibong, Tebal, MalaysiaSynthetic aqueous solutionMethylene Blue dye (MB)1230200Batch1[114]

Activated carbon from tea industry waste (TIWAC)Tea waste from tea processing plant, Black Sea region, Trabzon, TurkeyReal water samplesCr(VI)
Cr(III)
6.0300.2Batch0
95–100
2[115]

Activated carbon from sago wasteSago waste is collected from sago industry, Salem district, Tamilnadu, IndiaSynthetic aqueous solution
Industrial wastewater from radiator industry
Pb(II) 1802710Batch87.342[116]

Phaseolus  vulgaris  L. Canned food factoryAqueous synthetic solutionAcid Red 57 dye 2.0 20 20150 Batch 1.6 [91]
Textile wastewater1 (spiked wastewater sample)97.68

Industrial fungi Penicillium oxalicum var. Armeniaca Ascolor Biotec (Pardubice, Czech Republic)
and Ivax Pharmaceuticals (Opava, Czech Republic)
Aqueous synthetic solutionPb(II)
Hg(II)
Cd(II)
5.02010
50
50
BatchUp to 85 for Hg0.3 [118]

Fruit waste macrofungi Flammulina  velutipes Mushroom processing factoryAqueous synthetic solutionCd(II)
Pb(II)
6.0602510Batch75
70
18[130]

Tolypocladium sp.Czech Industrial PartnersAqueous synthetic solutionCd(II)
Pb(II)
Hg(II)
5.02050Batch0.3[118]

Antibiotic waste P. mutilus SAIDAL antibiotic
production complex at Medea (Algeria)
Aqueous synthetic solutionBasic Blue 41, cationic dye8.0-9.0603050Batch750.5[119]

Industrial waste of Clitopilus  scyphoides (Pleurotus  mutilus) fungal biomassAntibiotic
production plant, SAIDAL antibiotic
production complex in Médéa (Algeria)
Aqueous synthetic solutionCd(II) 5.01520200Batch411[120]

Fungal waste biomassPharmaceutical companies, ItalyTextile wastewater effluentsDye mixtures3.0302560–5000 Batch9016.7 [121]

Nonliving biomass Aspergillus  fumigatus Fermentation industry, Artemis Pharmaceuticals Limited, HAD, Jeedimetla, Hyderabad, IndiaAqueous synthetic solutionperse
mixture
Cu(II)
Cd(II)
Co(II)
Ni(II)
7.0604.8
2.9
4.8
2.7
2.8
Batch70
90
20
8
[122]

Nonliving biomass Aspergillus  awamori Industrial complex enzyme preparationAqueous synthetic solutionCr(VI)2.040115225Batch871[124]

Nonliving biomass Aspergillus  awamori Industrial complex enzyme preparationAqueous synthetic solutionCu(II)5.020180100Batch1[125]

Corynebacterium
 glutamicum
Fermentation industry
(BASF-Korea)
Aqueous synthetic solutionReactive Black 5 (RB5)1.035500500Batch2.5[127]

Activated carbon from antibiotic wasteIndustrial antibiotic productionAqueous synthetic solutionHg(II)5.53040Batch0.2[126]

Fennel biomass (Foeniculum  vulgare)Medical herb, local Unani medicine manufacturing unit at Aligarh, IndiaAqueous synthetic solutionCd(II)
Mixture
Cd(II)
Ni(II)
Zn(II)
Cu(II)
4.350
50 each
50100Batch Column92
97
10
 mL/min
[123]

A number of researchers in the Mediterranean countries (Turkey, Spain, Italy, etc.) were interested in olive oil wastes since these countries are among the world’s biggest olive producers. All types of wastes from olive oil industry such as pomace, pulp, stones, and milling sludge were used for the sorption of heavy metals and dyes from solutions [101110]. Particular work [101] reported almost 100% removal efficiency for Cr (VI) from aqueous solutions using olive pomace. Only one study was found to deal with phenol removal [110] using olive oil pomace and removal efficiency was above 90% in both batch and column modes. In another study that investigated the potential of olive oil mill residues as biosorbents for Cu (II), COD release was reduced to 600 mg/L when the biosorbent was washed twice while sorption performance was not affected [104]. Other work utilized different oil industrial wastes such as palm oil waste [111] or sunflower oil waste [112] in the removal of dyes and heavy metals from aqueous solutions.

Commercial activated carbon has been a very common method of adsorption for a long time. Research is now shifted toward using activated carbon derived from various agricultural as well as industrial sources. In the current review, only activated carbons manufactured from food processing wastes are reported. The method of deriving activated carbon (AC) from these wastes will be explained later in the pretreatment section. AC derived from different industrial waste sources such as olive waste cake [113], empty fruit bunch from palm oil mill [114], tea industry [115], and sago waste [116] was successful in biosorption of heavy metals and dyes. In view of the above, it can be inferred that most of the reported studies dealt with the removal of heavy metals and dyes. Clearly, there is lack of work on the removal of other pollutants. One particular research investigated the use of waste cider yeast in removing low concentrations (0.1-0.2 mg/L) of the toxin patulin from apple juice solutions and about 58% removal was achieved [117].

As for pharmaceutical wastes, they are either fungal or bacterial biomass that could be dead or living. Examples of fungal biomass are Aspergillus niger, Pleurotus mutilus, Trichoderma reesei, Rhizopus arrhizus, Rhizopus nigricans, and Penicillium chrysogenum. Bacterial biomass could be produced from antibiotic fermentation such as Streptomyces spp. or during production of drugs such as Streptomyces noursei, S. rimosus, and S. clavuligerus or during enzyme manufacture such as the bacillus species of B. licheniformis and S. subtilis. Plenty of work was done on applications of pharmaceutical wastes as effective biosorbents for contaminant removal from wastewater [118123]. For heavy metal removal, the waste Clitopilus scyphoides (Pleurotus mutilus) produced during antibiotic fermentation process was used to remove Cd (II) [120]. A high biosorption capacity of 111 mg/g was obtained within short uptake duration of about 15 min. No pretreatment for the dead biomass was required and the biosorbent was composed predominantly of Ca, Si, and P elements with a total mineral content of 13.5% (w/w). The fungal dead biomass Aspergillus fumigatus is also a fermentive waste of antibiotic industry that was utilized in metal biosorption. The sun-dried biomass was pretreated with 5% boiling KOH for 15 min and then thoroughly washed with distilled water till neutral pH was reached. The biosorbent was efficient in removing Cd, Co, Cu, and Ni with the highest efficiency obtained for Cu (72%). More than 90% of metal ions were removed from low-concentration mixtures (0.1 mM). At high concentration of these mixtures, Cu ion was the most competitive among other ions and 70% of which was removed. The fermentation waste mycelium of the fungal biomass, Aspergillus awamori, was produced industrially from an enzyme preparation process. It was then utilized for Cr (VI) removal and a maximum removal efficiency of 87% was obtained [124]. The same biomass, after being treated with 0.5 M NaOH, removed a maximum of 35.97 mg/g Cu (II) from aqueous solutions [125]. Tolypocladium sp. biomass waste was successful in removing Cd, Pb, and Hg [118]. Three different types of fungal biomass from antibiotic industries named Fennel biomass, Foeniculum vulgare, which is a medicinal herb, removed 92% of Cd ion at pH 4.3. Maximum biosorption capacities obtained in batch systems were 21, 24, and 30 mg/g at 30, 40, and 50°C, respectively. Biosorption was spontaneous and endothermic. In single-component packed-bed studies, breakthrough and exhaustive capacities were 10 and 40 mg/g, respectively, while 2 and 12 mg/g were the corresponding capacities for multicomponent systems. Capacities dropped to 0.8 and 4 mg/g in multicomponent saline systems. An antibiotic waste composed of a mixture of Streptomyces fradiae, Micromonospora pururea, and Nocardia mediterranea was chemically activated with K2CO3 to obtain activated carbon that was utilized as a biosorbent for Hg (II) [126].

For the removal of dyes, Acremonium strictum, Acremonium sp., and Penicillium sp. were examined for their potential to decolorize simulated dye baths. A. strictum was found to be the most efficient biosorbent with percentage removal of up to 90% in both acidic and neutral conditions. These biomasses were less active compared to Cunninghamella elegans which is a biomass known to be an efficient biosorbent that removed 97% of the dye color [121]. Clitopilus scyphoides (Pleurotus mutilus) was also used to remove Basic Blue dye [119] and a biosorption capacity of 200 mg/g was obtained within about 60 min, while Reactive Black 5 (RB5) dye was successfully removed by Corynebacterium glutamicum waste produced from lysine fermentation industry [127].

3. Operating Factors Influencing Biosorption

Holistically, the behavior and performance of biosorption are affected by the physical and chemical characteristics of each of the biosorbent and sorbate; in addition to the process operating conditions. Biosorbent and sorbate characteristics include composition, structure, type of charged and uncharged functional groups, and particle size. It was also reported that in biomass sorbents, the composition of the cell wall influences both sorption uptake capacity and selectivity [88, 128].

Operating conditions are instrumental biosorption controlling parameters which include pH, temperature, initial sorbate concentration, biosorbent dose, contact time, agitation speed, sorbent particle size, mode of operation, and competition from coions. These operating parameters will be further discussed in more detail.

3.1. Solution pH and Ionic Strength

The pH of sorbate solution plays a vital role in the biosorption process since it influences the charge on the biosorbent functional groups and the dissociation of these groups on the active sites. It also affects sorbate solubility and its degree of ionization. The effect of pH on both uptake capacity and percentage removal was investigated by numerous workers. For heavy metal sorption, it was found that the increase in pH increases uptake capacity of heavy metals such as Cd, Pb, Ni, Cu, and Zn in both the acidic and the neutral range (pH 2–7). The rate of increase under highly acidic conditions (pH 2–4) was mostly higher than that observed at milder acidic conditions (pH 4–6) [6, 72, 84, 100102, 104, 108, 125, 129, 130]. Under basic conditions (pH > 7), heavy metal uptake decreased with pH [100, 101, 108]. Under severe acidic conditions, the very low reported uptake capacities were attributed to the fact that H+ ions compete with the metal ions on the active sites [72, 101, 126] which indicates that biosorption is governed by electrostatic interactions under these conditions. Increase in pH also increased the percentage of metal removal under acidic and neutral pHs [97, 105, 106, 126] and decreased the removal under basic conditions [97]. However for the pharmaceutical waste mycelium of the Aspergillus awamori, the increase of pH from 2.0 to 4.0 decreased the removal efficiency of Cr (VI) by about 50% [122]. At basic pHs, biosorption uptake decreases owing to metal precipitation which leads on the contrary to increase in metal removal from solution by a possible combined microprecipitation-biosorption mechanism [105108]. In case of dyes, the behavior of sorption uptake and percentage removal with pH varies according to the type of charge. For cationic dyes such as Methylene Blue (MB) and Basic Blue 41, both removal and uptake are directly proportional to pH [78, 83, 91, 98, 119] and vice versa for anionic dyes such as Acid Green (AG), Acid Red 57, Reactive Red (RR 198), and Victazol Orange 3R dyes [70, 86, 91, 99]. At high pH, the uptake and removal of cationic dyes increase due to attractive forces between the positively charged dye and the negatively charged functional groups on the biosorbent. One study on the removal of phenols by olive pomace showed that removal efficiency is enhanced by increasing pH [110].

Very limited studies were conducted on the effect of ionic strength where the presence of NaCl [105, 123] and perchlorate salts [105] significantly reduced biosorption due to competition between the salt ions and the sorbate ions on the active sites.

3.2. Initial Sorbate Concentration

The increase in the initial concentration of the sorbate acts as a driving force to overcome the mass transfer resistance and hence increase the uptake. This behavior was reported for both heavy metals and dyes [83, 98, 110, 125, 126, 130]. In one study dealing with Hg sorption onto desiccated coconut waste, the concentration-uptake correlation was linear [100].

The percentage removal, on the other hand, was found to decrease with increasing in concentration for the heavy metals Cd, Zn, and Ni onto tea, olive cake wastes, and wine processing sludge, respectively [72, 76, 119] as well as for Cr (VI) and Basic Blue 41 dye onto mycelium of Aspergillus awamori and antibiotic fungal waste, respectively [108, 124]. The same behavior was encountered by Methylene Blue dye onto both fresh malted sorghum mash waste and mango seed kernel powder [83, 98] and by Pb onto both activated carbons from sago waste and peach/apricot stones. With the latter adsorbent, removal was almost constant at very low concentrations of Pb (5–100 ppm) [97, 116]. With higher initial concentrations, higher equilibrium concentrations in the solution were obtained possibly due to saturation of active sites and this, in turn, decreased the removal efficiency. In addition, the increase in initial concentration decreased sorption rate since it probably reduced diffusion across the boundary layer. However, a different behavior was observed for Acid Green (AG) dye sorbed onto spent brewery grains where the removal initially increased by virtue of the high concentration gradient driving force and then dropped owing to saturation of the sorption active sites [70]. Furthermore, with investigating the sorption of Cd (II), Pb (II), and Cu (II) onto orange peels the dissociation constant for the biosorption interaction decreased exponentially with increase in concentration [101] indicating stronger binding.

3.3. Biosorbent Dose

Generally as the biosorbent dose increases, the number of available active sites increases and thus consequently enhances the removal [70, 72, 86, 97, 98, 102, 110, 115, 119, 120, 124, 130]. On the other hand, the uptake capacity decreases probably due to decrease in surface area that might be a result of having some of the sorption sites aggregated and overlapped [100, 102, 108, 129]. In a few cases, the removal reaches a peak value then declines [82, 101, 119] and this could be due to saturation of active sites.

3.4. Temperature

The effect of temperature becomes important when dealing with wastewater effluents that are discharged at high temperatures due to processing. For endothermic reactions, biosorption uptake capacity and removal efficiency increased with temperature due to increase in surface activity and hence availability of more active sites [76, 80, 83, 98, 113, 120, 123, 124, 129] and vice versa for exothermic reactions [70, 86, 91, 100]. Sorption rate for endothermic reactions was also enhanced as temperature increased and it followed Arrhenius equation [76, 106].

3.5. Particle Size of The Sorbent

In most of the reported studies, the initial rate of sorption was rapid and it decreased gradually till it reached an approximately constant value [70, 101, 106]. This shows that binding mostly occurs on the solid surface and that film and pore ion diffusion are not significant or have very fast rates. In cases where this did not hold true, either film (boundary layer) or pore (intraparticle) diffusion or a combination of both was the rate limiting step [91, 100, 120, 123] When the governing mechanism was the surface reaction, decrease in particle size was shown to improve the uptake [110, 119] due to increase in surface area. In addition, the decrease in particle size enhances diffusion and sorption rates since it reduces intraparticle diffusion [108]. In case of very porous biosorbents like pectin wastes, it was found that particle size had no significant effect on Cr (III) sorption since the external surface area does not contribute much to the total surface area [102].

3.6. Agitation Speed

The speed of agitation was found to enhance removal efficiency by reducing mass transfer resistances but only up to an optimal limit above which efficiency drops probably due to biomass fragmentation [82, 103, 119].

3.7. Mode of Operation

The operational mode influences uptake and % removal because dynamics of batch systems are different from column dynamics. In most studies, dynamic capacity was lower than its batch counterpart; and the same held true for % removal [100102, 104, 131]. Column dynamics vary with column dimensions and flow rate. The increase in column height was found to decrease sorption efficiency and increase breakthrough time [102, 109]. An increase in initial concentration of sorbate enhanced sorption capacity and decreased breakthrough time [100, 109]. Increasing the influent flow rate also decreased the breakthrough time [109]. In a dynamic study on the sorption of phenols onto olive pomace, decreasing flow rate and particle size was found to improve sorption capacity [110].

3.8. Competition From Coions

One additional factor affecting biosorption in multicomponent systems is competition and interference between ions in the sorbate mixture. As a result, the reported individual batch uptake and breakthrough capacities of ions in single-component systems were lower compared to their counterparts in multicomponent systems [123]. However, high removal efficiency (up to 80–90%) was achieved in multicomponent systems of heavy metals [71, 103]. It was also suggested that competition is minimized at low ion concentrations [57, 122]. In general, Pb ions showed more competitiveness than Cd ions onto different adsorbents such as grape bagasse [79], olive mill waste [102], biomass from sunflower oil [112], and fruit waste macrofungi [130].

4. Nature and Mechanism of Biosorption

Food and pharmaceutical wastes contain organic compounds such as proteins, amino acids, polysaccharides, phenolics, and acids. These compounds have functional groups that bind to the sorbate cations. Groups include, but are not limited to, amines, hydroxyls, carbonyls, sulfonyls, thiols, and phosphates. Biosorption mechanisms include physical sorption by virtue of Van der Waals forces or by ion exchange electrostatic interactions, chemical sorption by chelation or complexation, and microprecipitation. Generally, a combination of these mechanisms is involved in biosorption [88, 132, 133].

There are several factors controlling sorption mechanisms, type of ligands or binding sites available on the sorbent; chemical structure and characteristics of the target ions/molecules, physicochemical conditions such as pH, ionic strength, and temperature. There are some general rules for metal binding particularly via complexation. Hard acids such as K+, Na+, Ca2+, and Mg2+ prefer to bind to oxygen ligands, whereas soft acids such as the precious metal ions of Ag, Au, Hg, and Cd preferentially bind covalently to the cell wall via ligands that contain nitrogen or sulfur [132, 134].

Sorption onto biomass can generally occur via one or more of the following mechanisms: rapid surface reaction between the sorbate and the active functional groups existing in the cell wall, intracellular accumulation, or precipitation/extracellular accumulation. Surface reaction could be either physical adsorption or chemisorption and is nonmetabolism dependent. Intracellular accumulation takes place when the sorbate migrates across the cell wall. It is a metabolism-dependent process that is influenced by adverse environmental conditions such as lack of nutrients and toxicity. It is also a function of the regular metabolic activities that change the microenvironment surrounding the cell, such as nutrient uptake, metabolic release, and respiration. In living biomass, biosorption is metabolism-dependent and occurs by sorbent uptake across the cell membrane. Therefore, it has its limitations regarding toxicity and maintaining nutrient levels. Biosorption via dead biomass does not suffer from these limitations and occurs on the cell wall where the polysaccharides and proteins have binding sites. However, lower binding capacities and higher desorption tendencies are often encountered [88, 135, 136].

To elucidate the underlying biosorption mechanism, the functional groups involved in biosorption were determined by Fourier transform infrared spectroscopy (FTIR) analysis (Table 2). Generically, sorption onto pectin-rich fruit wastes involved hydroxyl and carboxyl groups [94, 95, 101, 102]; whereas sorption onto olive oil wastes involved carboxylic and phenolic groups [102, 108, 111]. Biomass fungal wastes had additional amine groups as in Aspergillus Fumigatus and Aspergillus awamori. These groups were donated by the chitosan and chitin that are predominantly present in the fungal cell walls [122, 124, 125]. A two-step mechanism was suggested for sorption onto Aspergillus awamori where there is an initial adsorption step followed by a chromium reducing step from Cr (VI) to Cr (III). Heavy metal sorption onto okra food wastes and sugar bagasse wastes took place via a combined ion exchange/complexation mechanism where the positively charged metal interacted with the negatively charged wastes. The negative charge on the wastes was owed to the presence of lone pairs of the nitrogen and oxygen atoms that exist in the functional groups of cellulose, lignin, protein, and sugar [88, 89]. The main functional groups responsible for dye sorption onto pecan nut shells and mango seeds were the sulfonyl groups. Mechanism of sorption onto the former biosorbent depended on the number of sulfonic groups present on the dye; these groups interacted with the Ca compounds belonging to the pecan nut shells [131]. The mechanism of dye sorption onto the latter biosorbent entailed association with water molecules which linked the Victazol Orange 3R sulfonic groups to the syringyl groups of the lignin cellulose present in the mango seeds [99]. A variety of functional groups played important roles in the biosorption of Pb onto waste beer yeast. The extent of contribution of these groups was in the descending order: carboxylic, lipids, amines, and phosphates [82]. For the sorption of anionic dyes onto Cupuassu shells, a 3-step mechanism was proposed. It involved an initial rapid step for protonation of the Cupuassu shells functional groups. This was followed by dissociation of the dye agglomerates and their consequent dehydration, then finally electrostatic binding between the negatively charged dye and the positively charged biosorbent. Activated carbon from the pharmaceutical antibiotic waste contained primarily oxygen-containing functional groups such as hydroxyl and carbonyl groups which formed complexes with the mercury ions [126].


BiosorbentSorbateFunctional groupMechanismReference

Orange peelPb(II)
Cu(II)
Cd(II)
CarboxylicIEX/H-bonding[101]

Orange wasteCr(III)Carboxyl/hydroxylChemisorption[102]

Orange wasteCd(II)Carboxyl/hydroxyl[94]

Orange wasteCd(II)
Zn(II)
Cr(III)
Mainly carboxyl[95]

Desiccated coconutHg(II)Hydroxyl/carboxyl/amineChelation[100]

Pecan nut shells
(C. illinoinensis) biomass
Acid Blue
Reactive Blue
Acid Blue
Sulfonyl[132]

Cupuassu shell, Theobroma  grandiflorum, (CS) Reactive red dye
Direct blue
Hydroxyl/carboxylicIEX [87]

Mango seeds (MS) Mangifera  indica  L.Victazol orange Sulfonyl [99]

Okra food industrial wasteCd(II)
Fe(II)
Zn((II)
Hydroxyl/carbonyl/amideIEX/complexation [88]

Sugar industrial waste (bagasse waste)Cd(II)
Fe(II)
Hydroxyl/carbonyl/amideIEX/complexation [89]

Pineapple peelMB dyeHydroxyl/carboxyl/amine [91]

Olive pomacePb(II)
Cu(II)
Cd(II)
Carboxylic/phenolicSurface complexation [108]

Olive mill stonePb(II)CarboxylicIEX [102]

Palm oil mill effluent (POME) sludgeMethylene Blue Carboxylic [111]

Wine processing sludgeNi(II)Amino/carboxylPhysical adsorption/chemical complexation [76]

Spent waste beer yeast
Saccharomyces  cerevisiae
Pb(II)Amine/carboxylic/
phosphates/sulfhydryl
IEX/complexation [82]

Grape bagasse waste residueCd(II)
Pb(II)
Carbonyl/hydroxyl [79]

Phaseolus vulgaris biomassPb(II)Amino/hydroxyl [84]

Activated carbon from antibiotic wasteHg(II)Hydroxyl/carbonylComplexation [126]

Nonliving biomass Aspergillus  awamori Cr(VI)Amine [124]

Nonliving biomass Aspergillus  Fumigatus Cd (II) perse   
mixture
Cu(II)
Cd(II)
Co(II)
Ni(II)
Hydroxyl/amineComplexation [122]

Fennel biomass
(Foeniculum vulgare)
Cd(II)Carboxylic/phenolicIEX* [123]

IEX: ion exchange adsorption.

The change in pH during sorption could be indicative of the involved mechanism. For example, the decrease in pH during the sorption of heavy metals onto Tolypocladium sp. is a result of proton release probably due to electrostatic interaction between the positively charged metals and the negatively charged carboxylic groups on the adsorbent [107].

5. Equilibrium and Kinetic Modeling Studies

Biosorption equilibrium is governed by isotherm models that are well-known and established in literature. Table 3 [82, 86, 87, 127, 131, 137] summarizes the different isotherm model equations involved in the present review along with their relevant parameters. For the kinetic modeling, the reported studies herein were found to follow either pseudo-first order or pseudo-second order or Elovich models; equations thereof are presented in Table 4 [94, 98, 131, 137].


Adsorption isotherm modelModel parameters

Freundlich  
   
Linear form  
: Freundlich isotherm constant that indicates adsorption capacity
(mg/g)
: measure of adsorption intensity or surface heterogeneity (dimensionless)
: amount adsorbed at equilibrium, mg/g
: adsorbate concentration at equilibrium, mg/L

Langmuir  
  
Linear form  
: maximum binding capacity, mg/g
: Langmuir binding (adsorption) constant, L/mg

Sips  
  

: Sips binding (adsorption) constant,
: dimensionless exponent constant
= Sips sorption exponent
= Sips sorption constant (L/mg)

Dubinin-Astakhov  
: mean free energy of adsorption, KJ/mol
: Dubinin-Astakhov dimensionless exponent
: temperature, K
: universal gas constant, KJ/mol·K

BET  
  
Linear form  

Alternative form  
: BET isotherm constant which indicates energy of surface interaction, L/mg
: saturation concentration of adsorbate, mg/L
: isotherm constant for BET adsorption in the first layer, L/mg
: isotherm constant for BET adsorption in upper layers, mg/L


Kinetic ModelModel Parameters

Pseudo-first order   

Linear Form   
: rate constant of pseudo-first order model, min−1
: amount adsorbed at equilibrium, mg/g
: amount adsorbed at time , mg/g

Pseudo-second order   

Linear Form   
: rate constant of pseudo-second order model, g/mg·min

Elovich  
α: initial adsorption rate, mmol/g·min
: Elovich constant, related to extent of surface coverage and activation energy, g/mmol

Table 5 compiles a summary of the sorption parameters pertaining to the studies utilizing food and pharmaceutical waste biosorbents, as predicted by the different well-established models for sorption equilibrium. The table presents only results that were obtained by the best fitting model relevant to each study. In the majority of equilibrium studies, heavy metals and dyes were shown to follow Langmuir isotherm. This indicates single-site monolayer binding where the surface of sorbent is homogenous and all sites are equally favorable or nonfavorable from the energetic point of view. Few heavy metals followed Freundlich isotherm which assumes a heterogeneous biosorbent surface; examples are Cd (II) [123] and Pb (II) [82, 97, 105]. Cd was also shown to follow BET [120] and Sips [94], while Pb was found to follow Sips [102] and Dubinin Astakhov [103]. Several dyes such as Reactive Red (RR 194), Direct Blue 53, Acid Blue 25, and Reactive Black 5 followed Sips isotherm [87, 127, 131], whereas Reactive Red dye (RR 198) and phenols followed Freundlich isotherm [86, 110]. In general, it can be observed from the table that sorption capacities of pharmaceutical and fungal biomass wastes for heavy metals and dyes are higher than those of pectin-rich fruit wastes or olive oil wastes. Sorption in multicomponent systems was well described by either Langmuir as in case of simulated acid bath for wool (SABW) dye mixture [121] or extended Langmuir as in case of binary mixtures of heavy metals [105].


BiosorbentTarget ion/compoundEquilibrium modelMaximum sorption capacity (mg/g)Sorption constant*pH/temperature (°C)Reference

Local dairy sludgePb(II)
Cd(II)
Langmuir178.6
69.90
0.03
0.05
5/40[129]

Baker’s yeast biomassCd(II)
Pb(II)
Langmuir31.75
60.24
0.092
0.066
6.0/30
5.0/30
[131]

Cider yeastPatulinLangmuir0.00820.0644.5/25[117]

Beer yeastCu(II)
Pb(II)
Langmuir0.66
2.27
0.314
0.259
5.0/20[69]

Spent waste beer yeast
Saccharomyces  cerevisiae
Pb(II)Freundlich
5.0/30[82]

Spent brewery grains (SBG)AG25 dyeLangmuir212.760.0363.0/30[70]

Wine processing sludgeNi(II)Langmuir3.910.1135.5/50[76]

Antibiotic waste P. mutilus Cu(II)Langmuir106.380.007[119]

Antibiotic waste P. mutilus Basic Blue 41Langmuir
Freundlich
111.00
0.097

(8.0-9.0)/30[119]

Phaseolus  vulgaris  L. Acid Red 57 dyeLangmuir215.132.0/20[91]

Phaseolus  vulgaris  L. Reactive Red 198Freundlich
[86]

Fruit waste macrofungi Flammulina  velutipes Cd(II)
Pb(II)
Langmuir 8.43
18.35
6.0/25[130]

Industrial fungi Penicillium oxalicum var. Armeniaca Cd(II)
Pb(II)
Hg(II)
Langmuir35.90
47.40
269.3
0.05
1.01
0.07
5.0/20[107]

Industrial fungi
Tolypocladium sp.
Cd(II)
Pb(II)
Hg(II)
Langmuir11.90
28.40
161.0
1.03
0.61
0.50
5.0/20[107]

industrial waste of Clitopilus  scyphoides  
(Pleurotus  mutilus) fungal biomass
Cd(II)BET45.316

5.0/20[120]

Fungal waste biomassSimulated acid bath for wool (SABW) dyeLangmuir289.50.01143.0/25[121]

biomass of
Phaseolus  vulgaris  L.
Pb(II)Langmuir19.930.4985.0/50[84]

Fennel biomass (Foeniculum vulgare)Cd(II)Langmuir
Freundlich
26.590.080

4.3/50[123]

Nonliving biomass Aspergillus  awamori Cu(II)Langmuir35.970.1365.0/20[125]

Corynebacterium 
glutamicum
Reactive Black 5
RB5
Langmuir
Sips
4190.042

1.0/35[127]

Rhizopus oligosporus biomassCu(II)Langmuir79.370.2825.0/30[85]

Pectin-rich fruit wastes (lemon peels)Cd(II)Langmuir22.320.0155.0/—[133]

Orange wasteCd(II)Sips20.640.038 ( )6.0/25[94]

Orange wasteCd(II)
Zn(II)
Cr(III)
Langmuir17.66
14.61
22.50
0.004
0.067
0.372
4.0/20[95]

Orange (Citrus sinensis)Cr(III)Langmuir36.480.4035.0/25[102]

Pineapple peel, an agricultural effluentMethylene Blue (MB) cationic dyeLangmuir97.090.0746.0/30[91]

Peach stones
Apricot stones
Pb(II)Freundlich
( )

( )
7.0/—[97]

Mangifera  indica (mango) seed kernel particlesMethylene Blue (MB) cationic dyeLangmuir153.8460.82278.0/50[98]

Desiccated coconutHg(II)Langmuir500.007.4/30[100]

Pecan nut shells (C. illinoinensis) biomassAcid Blue 74 (AB74) Langmuir 4.8510.001 6.5/30 [132]
Reactive Blue 4 (RB4)Langmuir13.4100.001
Acid Blue 25 (AB25)Sips 7.576
( )

Crushed olive stone wastesPb(II)
Ni(II)
Cu(II)
Cd(II)
Freundlich 5.5/20 [105]
Binary mixturesExtended Langmuir

Olive pomaceCu(II)
Cd(II)
Pb(II)
Langmuir1.94
2.98
6.23
0.138
0.046
1.829
5.0/60[108]

Olive pomacePhenolsFreudlich
10.0/20[110]

Pomace from olive oilCr(IV)Langmuir18.690.0552.0/60[101]

olive mill residues (OMR)Cu(II)Langmuir13.500.0805.0/23[104]

Solid olive stonePb(II)Sips6.57 5.0/25[102]

Olive oil millPb(II)Dubinin-Astakhov23.695.0/25[103]

Palm oil mill effluent (POME) sludgeMethylene Blue (MB) cationic dyeLangmuir 23.500.2087.6/27[111]

Sugarcane bagasse wasteMethylene Blue (MB) Langmuir202.430.031 8.0/25 [78]
Gentian Violet (GV)327.830.047

Fresh malted sorghum mash wasteMethylene Blue (MB) basic dyeLangmuir384.60.0117.0/53[83]

Cupuassu shell, Theobroma  grandiflorum, (CS) Reactive Red dye (RR 194) Sips64.1
( )
2.0/25 [87]
Direct Blue 5337.5
( )

Activated carbon derived from exhausted olive waste cakeLanaset Grey GLangmuir108.700.0316.0/25[113]

Activated carbon derived from empty fruit bunch (EFB)Methylene Blue dye (MB)Langmuir344.830.060—/30[114]

Activated carbon from sago wastePb(II)Langmuir14.350.0953.5/27[116]

Units depend on the fitting isotherm model and are indicated in Table 3.

In most reported studies, the pseudo-second order model was found to be the most appropriate fitting model that describes biosorption of heavy metals and dyes onto food and pharmaceutical wastes (Table 6). This indicates that the mechanism is that of chemisorption. The model takes into account the three phases of the sorption process; surface reaction, film or external diffusion, and pore or intraparticle diffusion. Generally, time versus uptake trends revealed fast kinetics where almost 90% or more of the material was sorbed within a time range from few minutes to few hours and equilibrium was almost approached. In one instance when Cr (III) was adsorbed onto orange waste, reaching very close to complete equilibrium required a few days [102]. This could be owed to a diffusion-controlled sorption taking place onto the very porous pectin-rich biosorbent as was alluded to in Section 3.5.


BiosorbentTarget ion/compoundKinetic model (mg/g)Rate constant*pH/temperature (°C)/time (min)Co (mg/L)Reference

Local dairy sludgePb(II)
Cd(II)
Pseudo-second order117.6
44.4
0.27
4.2
5.0/20°C/500200
100
[129]

Wine processing sludgeCr(VI)Pseudo-second order2.420.0704.2/50/240100 [73]

Wine processing sludgeNi(II)Pseudo-second order3.110.2265.5/50/12045[76]

Desiccated coconutHg(II)Pseudo-second order447.037.4/30/6050[100]

Pecan nut shells (C. illinoinensis) biomassAcid Blue 74 (AB74) Pseudo-first3.2710.026.5/30/500 1000 [132]
Reactive Blue 4 (RB4)Pseudo-second10.010 6.5/30/1000
Acid Blue 25 (AB25)Pseudo-second-order4.892 6.5/30/500

Spent brewery grainsAG25 dyePseudo-second order74.630.0383.0/30/7590[70]

Beer brewery diatomite waste (SDE)Methylene Blue basic dyePseudo-second order4.921.247.0/25/14402.5[81]

Antibiotic waste P. mutilus Basic Blue 41Pseudo-second order90.910.00428.0-9.0/30/6070[119]

Macrofungal waste from antibioticsCd(II)Pseudo-second order82.80.00145.0/20/15200[120]

Fennel biomass (Foeniculum  vulgare)Cd(II)Pseudo-second order9.300.4765.0/30/50100[123]

Phaseolus  vulgaris  L. Reactive Red 198Pseudo-second order81.970.0362.0/20/20[86]

Nonliving biomass Aspergillus  awamori Cu(II)Pseudo-first order35.000.0775.0/20/18025[125]

Corynebacterium  
glutamicum
Reactive Black 5
RB5
Pseudo-second order370.00 1.0/25/5002000[127]

Phaseolus  vulgaris  L. Acid Red 57 dyePseudo-second order89.490.212.0/20/20150[91]

Fruit waste macrofungi Flammulina  velutipes Cd(II)Pseudo-first [130]
Pb(II)Pseudo-second order13.042.176.0/25/60 10

Orange (Citrus sinensis)Cr(III)Pseudo-second order10.970.0025.0/25/4320100[102]

Pectin-rich fruit wastes (lemon peels)Cd(II)Pseudo-second order13.920.0215.0/—/5019.2[133]

Orange wasteCd(II)Elovich333.33 (1/ )0.004 (1/ )6.0/25/60100[94]

Mangifera  indica (mango) seed kernel particlesMethylene Blue (MB) cationic dyePseudo-first order1150.04618.0/30/120175[98]

Rhizopus oligosporus biomassCu(II)Pseudo-second order69.820.0025.0/30/120100[85]

Crushed olive stone wastesPb(II) Pseudo-second
order
1.120.141 5.5/20/6018.86 [105]
Ni(II)0.253.0004.48
Cu(II)0.267.4974.35
Cd(II)0.720.12110.56

Olive stonesCd(II)Pseudo-second order0.9033.19611.0/80/2010 [106]

Palm oil mill effluent (POME) sludgeMethylene Blue (MB) cationic dyePseudo-second order5.540.00727.6/27/432010[111]

Olive pomaceMethylene Blue (MB) dyePseudo-second order0.0906—/25/24010[109]

Tea industry wasteCd(II)Pseudo-second order10.60.027.0/25/180100[72]

Pineapple peel, an agricultural effluentMethylene Blue (MB) cationic dyePseudo-second order104.17 6.0/30/400300[91]

Okra food wasteCd(II)
Fe(II)
Zn(II)
Pseudo-second order17.54
20.42
14.99
0.009
0.008
0.013
—/20/9020[88]

Activated carbon derived from exhausted olive waste cakeLanaset Grey G Pseudo-first order106.40.00196.0/25/3000150[113]

Activated carbon from tea industry waste (TIWAC)Cr(III)Pseudo-second order0.4641.526.0/—/300.01[115]

Sugar industry (waste bagasse)Cd(II)
Fe(II)
Pseudo-first order
—/20/9020[89]

Sugarcane bagasse wasteMethylene Blue (MB) Pseudo-second
order
192.310.00128.0/25/600200 [78]
Gentian Violet 357.140.000058.0/25/900300

Units depend on the fitting kinetic model and are indicated in Table 4.

6. Pretreatment and Regeneration/Recovery Options

Wastes from most fruit sources are pectin-rich biosorbents of potentially high metal binding abilities. Many studies that involved the use of such biosorbents have undertaken prior chemical pretreatment known as protonation. This process aims at removing excess cations such as Ca2+, Na+, or K+ from the biosorbent before carrying out biosorption experiments to reduce the competition of these elements with targeted heavy metals. Moreover, it leads to the creation of negative active sites on the biosorbent surface (at specific pH values) which leads to higher metal uptake capacity [92]. Some researchers utilized HNO3 with predetermined concentration for this chemical pretreatment step. A comparative study [101] was carried out on the performance of treated and untreated orange peel waste. Results showed higher Cd (II) uptake of 11.2 mg/g in case of chemically treated orange peel as compared to 6.94 mg/g in case of original peel. Similarly, [138] pectin waste was protonated by HNO3 before carrying out batch biosorption experiments for heavy metal removal. It was also suggested in a different study [99] that the use of HCl was successful in acidifying the mango seeds (AMS) in order to improve its removal efficiency to dyes. A faster adsorption process accompanied by increase in adsorption capacity was encountered in case of AMS relative to the original mango seeds (MS). According to them, the protonation using HCl increased the macropore structure of the original MS allowing higher amounts of dyes to be adsorbed.

H2O2 along with thermal treatment was used to treat wine processing sludge in order to remove organic matter before using the biosorbent for the removal of Cr (VI) [73]. This step led to the reduction of Cr (VI) to Cr (III) which reached a percentage of 2–18 at the end of the biosorption experiment. They considered pretreatment as a key factor for any future research to be performed on Cr removal using the same biosorbent. A comparison between chemically treated and untreated waste olive cake biomass during a study for Zn (II) removal from aqueous solutions was conducted [108]. This showed an increase in the removal efficiency of waste treated by NaOH and a reduction in the removal efficiency in case of H2SO4 treated waste.

A combined chemical and physical treatment was performed for baker’s yeast waste used for Cd (II) and Pb (II) removal [139]. Thermal treatment (121°C), NaOH, and ethanol were applied to separate biomass samples and the resulted treated biomass was employed in batch biosorption experiments. The best metal uptake was reported for ethanol treated biomass whereas caustic and thermal. Caustic soda and ethanol were utilized for pretreating the Penicillium oxalicum var. Armeniaca biomass used for heavy metal removal [107]. The purpose was to remove proteins from the biomass sites via caustic treatment which increased biosorption capacity, whereas the opposite was true in case of acidic pretreatment.

Other different chemical treatments either acidic or caustic were employed by other workers in their biosorption studies. Zinc chloride and potassium hydroxide were employed as chemical activating agents for palm oil sludge in a study on the removal of Methylene Blue dye [111]. Results were comparable to commercial activated carbon but chemically treated sludge was recommended for better solution to sludge disposal problems. Simulation of chemical and physical pretreatment was employed in another study on the removal of phenols from industrial wastewaters using olive pomace solid wastes produced from different stages of olive mills [110]. Dried olive pomace denoted OP-1, solvent extracted using hexane and vapor olive pomace (OP-2), solvent extracted and incompletely combusted in boilers, and olive pomace (OP-3) were utilized. Results recommended the use of OP-3 as an effective biosorbent for phenol removal as the reported removal efficiencies exceeded 90%. The use of sugarcane bagasse modified by EDTA dianhydride for the removal of MB and GV dyes was investigated by other workers [78], and there was no sign of its effectiveness as a biosorbent compared to the untreated bagasse. It has also been reported in another study that the physically and chemically treated waste cider yeast was efficient in removing patulin [84]. Heating and chemical addition of either NaOH or ethanol was done during yeast preparation for batch experiments, while calcium alginate was used to form a gel bead (cell immobilization) with and without NaOH treatment for the column study. For batch results, the highest % removal obtained was 58.29% in case of caustic treatment and 44.41% for thermal or ethanol treatment. Column results showed substantial improvement in patulin removal by caustic treated immobilized yeast matrix (100% removal) as compared to untreated yeast (71.42%). Another cell immobilization was performed during a study conducted on the removal of heavy metals using waste biomass from beverage industry [75]. Comparison between the removal efficiencies of both immobilized (on Dowex resin and Chitin) and free biomasses indicated limited improvement in uptake performance. Another study used polyvinyl alcohol for biomass immobilization [122]. This process helped in improving biomass adsorption capacity and regeneration ability. A different study compared the performance of immobilized and suspended brewery waste yeast biomass versus fresh yeast (from baker’s) in the removal of Cd (II) from aqueous solutions [80]. An excellent removal efficiency of 99.83% was reported in case of suspended form of brewery waste (SBW) which confirmed its promising potential as an effective low-cost adsorbent.

To test the effect of different functional groups on the removal of some heavy metals (Cd2+, Zn2+, and Cr3+), orange waste biomass was chemically modified by specific reagents [95]. It was suggested that ester treatment was not recommended as a prior modification because it decreased biosorption capacity. Five different chemical reagents were applied to chemically treat the waste beer yeast used in biosorption of lead from electroplating effluents [82]. Lead removal efficiencies were reduced after using all five pretreatment methods with drastic effects shown in case of ethanol and HCl treatment. Similar results were reported by the same workers in their study on Cr removal [74]. Their results showed reduction in removal efficiency using all types of treating agents relative to the original biosorbent and they owed this to the creation of modified functional groups.

Some researchers used chemical and physical methods for the preparation of activated carbons produced from different food processing wastes. Four studies were reported for the removal of dyes or heavy metals using AC prepared from exhausted olive waste cake [113], AC prepared from oil palm empty fruit bunch [114], AC prepared from tea waste [115], and AC prepared from sago waste [116]. Chemical activation was performed using sulfuric or phosphoric acids or potassium hydroxide and this was followed by heating to relatively high temperatures or microwave assistant heating as an essential step in all four studies. Reported results showed an outstanding performance for AC from tea industrial waste in Cr (III) removal with an efficiency that almost reached 100%.

As for pharmaceutical wastes, Tolypocladium sp. was treated with methanol to improve its sorption capacity for Hg (II) [107]. Modification of the amino groups on the waste mycelium of Aspergillus awamori via treatment with formaldehyde, acetic anhydride, or sodium iodoacetate did not improve its removal efficiency for Cr (VI) [124]. The treatment of the same biosorbent with sodium hydroxide and dimethyl sulfoxide increased Cu (II) uptake [125]. Among different pretreatments of Corynebacterium glutamicum with HCl, H2SO4, HNO3, NaOH, Na2CO3, NaCl, and CaCl2, the maximum improvement in biosorption capacity for Reactive Black 5 dye was achieved with 0.1 M HNO3. This was attributed to the enhancement of positively charged cell surfaces that attract the negatively charged dyes [127].

Few researchers were interested in desorption processes for either regeneration of the biosorbent for reuse and/or for recovery of the sorbate material. Desorption can be performed by adding acids, bases, inorganic salts, or solvents [129] for metal recovery. This step usually follows the adsorption step and metal recovery rate or metal uptake is calculated to test the effectiveness of the reagent used in desorption. HCl was the most used eluent for the majority of the reported studies [100, 101, 103105, 116, 122, 123, 129]. The most promising reported results showed that olive mill waste (OMW) maintained its adsorptive capacity for Cd (II) and Pb (II) after ten adsorption-desorption cycles [103]. HCl elution was followed by neutralization with Na2HCO3 [101]. Other workers revealed that exhausted modified orange peel was able to adsorb Pb (II) up to 91.5% after the 4th cycle. It was concluded in another study that desiccated coconut waste can be used multiple times for Hg sorption and can be regenerated easily using HCl [100]. It was also found in other batch experiments that 41.7% recovery of Fennel biomass could be attained after the 5th cycle using HCl as an eluent [123]. In addition, the relevant column study was very successful and resulted in 87.8% of Cd (II) being eluted in a single-component system and almost 100% in a multicomponent system. Results of using HCl as an eluting agent showed that after the 4th cycle, 65–70% of initial Cd (II) can be retained onto Aspergillus Fumigatus, but the biosorbent deteriorated after the 5th cycle [122].

In comparing HCl with other desorping agents, higher Pb (II) desorption rate using HCl as compared to EDTA was reported [26]. However, EDTA manifested better performance than both HCl and CaCl2 (equal desorption effect) in case of Cu (II) desorption but had the disadvantage of damaging the biosorbent sites [104]. Furthermore, the regenerated waste was able to remove 40% of Cu (II). Different results revealed that Pb (II) was better recovered by HNO3 (desorption rate of 76.6%) while Cd (II) was better recovered by HCl (desorption rate of 62.5%) [129]. The desorping agent, HNO3, was utilized in another study where the results showed that the regenerated biomass was successfully capable of desorping Cd (II) even after 5 consecutive cycles [120]. The comparison between the use of HNO3 and double deionized water (DDW) in desorbing Ni (II) showed that DDW was very poor compared to HNO3 [76]. The same acid was also used along with another two desorbing agents, NaNO3 and Ca(NO3)2, to regenerate peels and it was shown that regenerated peels have the same efficiency as the original peels [140]. About 90–100% of Cd (II) was recovered from the peels in 120 min or less. Additionally, HNO3 gave superior removal efficiency of 90% in only 50 min without damaging the peels.

7. Concluding Remarks

Industrial food processing and pharmaceutical wastes are promising biosorbents for treatment of wastewater effluents. They contain functional groups such as hydroxyl, carboxyl, and amine that allow them to interact with metal ions and dye pollutants via physical and/or chemical sorption. Sorption equilibrium in most of the previous studies was best described by Langmuir isotherm suggesting single-site binding. Sorption kinetics was generally fast and it predominantly followed the pseudo-second order model indicating a chemisorption mechanism. Surface reaction as well as film and pore diffusion processes were considered in the model.

Biosorption is influenced by the physical and chemical properties of the sorbent as well as various operating conditions. Numerous workers studied the effect of these parameters in batch systems. However, very few studies were conducted in continuous column systems. The latter is of paramount importance in scaled-up applications. Furthermore, most workers employed synthetic aqueous solutions rather that real wastewater effluents where competition and interference between ions in the mixture could significantly affect biosorption performance. One parameter that was overlooked is the physical, mechanical, and chemical stability of the sorbent. Mechanical strength of the biosorbent and its resistance to chemicals and microbial degradation are crucial parameters that ensure reproducibility of biosorbent, particularly in continuous operations where the biosorbent is regenerated and reused many times. Maintaining reproducibility for many subsequent cycles has both environmental and economic merits.

Desorption studies are relatively fewer compared to removal studies. The former is particularly important for both biosorbent regeneration and sorbate recovery if of value. Disposing of, landfilling and incineration could be alternatives to discarding the used biosorbent rather than regenerating it. However issues with cost and leaching of toxic compounds in the soil and ground water make them sometimes unfavorable options. Under very strong binding conditions, where the equilibrium binding constant is high, leaching and metal release are minimized.

Biosorbent performance could be enhanced by chemical, thermal, or chemical/thermal pretreatment and/or immobilization. Pretreatment could be performed to remove undesired organic compounds, proteins, or competing ions from the biosorbent and hence improve biosorption capacity and efficiency. In other cases, pretreatment is undertaken to add new functional groups to the biosorbent that can possibly enhance biosorption. However in some cases, pretreatment gave adverse effects. Prior characterization studies on the biosorbent may help in selecting the suitable treatment option.

Biosorption utilizing industrial food processing and pharmaceutical wastes could provide a cost-effective ecofriendly viable means of treating wastewater effluents, while making good use of waste materials. However, more work should focus on scaling up the proposed biosorption processes and studying their technoeconomic feasibility. Research should also be extended to using these biosorbents for treatment of different classes of contaminants such as phenolic compounds and mycotoxins.

Conflict of Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.

References

  1. M. Rafatullah, O. Sulaiman, R. Hashim, and A. Ahmad, “Adsorption of methylene blue on low-cost adsorbents: a review,” Journal of Hazardous Materials, vol. 177, no. 1–3, pp. 70–80, 2010. View at: Publisher Site | Google Scholar
  2. V. K. Gupta, “Application of low-cost adsorbents for dye removal—a review,” Journal of Environmental Management, vol. 90, no. 8, pp. 2313–2342, 2009. View at: Publisher Site | Google Scholar
  3. E. Forgacs, T. Cserháti, and G. Oros, “Removal of synthetic dyes from wastewaters: a review,” Environment International, vol. 30, no. 7, pp. 953–971, 2004. View at: Publisher Site | Google Scholar
  4. G. Z. Kyzas, J. Fu, and K. A. Matis, “The change from past to future for adsorbent materials in treatment of dyeing wastewaters,” Materials, vol. 6, pp. 5131–5158, 2013. View at: Publisher Site | Google Scholar
  5. J. Vijayaraghavan, S. J. S. Basha, and J. Jegan, “A review on efficacious methods to decolorize reactive azo dye,” Journal of Urban and Environmental Engineering, vol. 7, no. 1, pp. 30–47, 2013. View at: Publisher Site | Google Scholar
  6. Z. Aksu, “Application of biosorption for the removal of organic pollutants: a review,” Process Biochemistry, vol. 40, no. 3-4, pp. 997–1026, 2005. View at: Publisher Site | Google Scholar
  7. J. Wang and C. Chen, “Biosorbents for heavy metals removal and their future,” Biotechnology Advances, vol. 27, no. 2, pp. 195–226, 2009. View at: Publisher Site | Google Scholar
  8. Y.-F. Zhou and R. J. Haynes, “Sorption of heavy metals by inorganic and organic components of solid wastes: significance to use of wastes as low-cost adsorbents and immobilizing agents,” Critical Reviews in Environmental Science and Technology, vol. 40, no. 11, pp. 909–977, 2010. View at: Publisher Site | Google Scholar
  9. F. Fu and Q. Wang, “Removal of heavy metal ions from wastewaters: a review,” Journal of Environmental Management, vol. 92, no. 3, pp. 407–418, 2011. View at: Publisher Site | Google Scholar
  10. G. M. Gadd, “Biosorption: critical review of scientific rationale, environmental importance and significance for pollution treatment,” Journal of Chemical Technology and Biotechnology, vol. 84, no. 1, pp. 13–28, 2009. View at: Publisher Site | Google Scholar
  11. P. R. Gogate and A. B. Pandit, “A review of imperative technologies for wastewater treatment I: oxidation technologies at ambient conditions,” Advances in Environmental Research, vol. 8, no. 3-4, pp. 501–551, 2004. View at: Publisher Site | Google Scholar
  12. P. R. Gogate and A. B. Pandit, “A review of imperative technologies for wastewater treatment II: hybrid methods,” Advances in Environmental Research, vol. 8, no. 3-4, pp. 553–597, 2004. View at: Publisher Site | Google Scholar
  13. N. Bolong, A. F. Ismail, M. R. Salim, and T. Matsuura, “A review of the effects of emerging contaminants in wastewater and options for their removal,” Desalination, vol. 239, no. 1–3, pp. 229–246, 2009. View at: Publisher Site | Google Scholar
  14. K. Chojnacka, “Biosorption and bioaccumulation—the prospects for practical applications,” Environment International, vol. 36, no. 3, pp. 299–307, 2010. View at: Publisher Site | Google Scholar
  15. G. Crini, “Non-conventional low-cost adsorbents for dye removal: a review,” Bioresource Technology, vol. 97, no. 9, pp. 1061–1085, 2006. View at: Publisher Site | Google Scholar
  16. W. S. W. Ngah, L. C. Teong, and M. A. K. M. Hanafiah, “Adsorption of dyes and heavy metal ions by chitosan composites: a review,” Carbohydrate Polymers, vol. 83, no. 4, pp. 1446–1456, 2011. View at: Publisher Site | Google Scholar
  17. A. Demirbas, “Agricultural based activated carbons for the removal of dyes from aqueous solutions: a review,” Journal of Hazardous Materials, vol. 167, no. 1–3, pp. 1–9, 2009. View at: Publisher Site | Google Scholar
  18. G. Crini and P.-M. Badot, “Application of chitosan, a natural aminopolysaccharide, for dye removal from aqueous solutions by adsorption processes using batch studies: a review of recent literature,” Progress in Polymer Science, vol. 33, no. 4, pp. 399–447, 2008. View at: Publisher Site | Google Scholar
  19. M. A. M. Salleh, D. K. Mahmoud, W. A. W. A. Karim, and A. Idris, “Cationic and anionic dye adsorption by agricultural solid wastes: a comprehensive review,” Desalination, vol. 280, no. 1–3, pp. 1–13, 2011. View at: Publisher Site | Google Scholar
  20. P. Kaushik and A. Malik, “Fungal dye decolourization: recent advances and future potential,” Environment International, vol. 35, no. 1, pp. 127–141, 2009. View at: Publisher Site | Google Scholar
  21. C. I. Pearce, J. R. Lloyd, and J. T. Guthrie, “The removal of colour from textile wastewater using whole bacterial cells: a review,” Dyes and Pigments, vol. 58, no. 3, pp. 179–196, 2003. View at: Publisher Site | Google Scholar
  22. D. Sud, G. Mahajan, and M. P. Kaur, “Agricultural waste material as potential adsorbent for sequestering heavy metal ions from aqueous solutions—a review,” Bioresource Technology, vol. 99, no. 14, pp. 6017–6027, 2008. View at: Publisher Site | Google Scholar
  23. S. O. Lesmana, N. Febriana, F. E. Soetaredjo, J. Sunarso, and S. Ismadji, “Studies on potential applications of biomass for the separation of heavy metals from water and wastewater,” Biochemical Engineering Journal, vol. 44, no. 1, pp. 19–41, 2009. View at: Publisher Site | Google Scholar
  24. U. Farooq, J. A. Kozinski, M. A. Khan, and M. Athar, “Biosorption of heavy metal ions using wheat based biosorbents—a review of the recent literature,” Bioresource Technology, vol. 101, no. 14, pp. 5043–5053, 2010. View at: Publisher Site | Google Scholar
  25. E. Fosso-Kankeu and A. F. Mulaba-Bafubiandi, “Implication of plants and microbial metalloproteins in the bioremediation of polluted waters: a review,” Physics and Chemistry of the Earth, vol. 67–69, pp. 242–252, 2014. View at: Publisher Site | Google Scholar
  26. S. S. Ahluwalia and D. Goyal, “Microbial and plant derived biomass for removal of heavy metals from wastewater,” Bioresource Technology, vol. 98, no. 12, pp. 2243–2257, 2007. View at: Publisher Site | Google Scholar
  27. S. K. R. Yadanaparthi, D. Graybill, and R. von Wandruszka, “Adsorbents for the removal of arsenic, cadmium, and lead from contaminated waters,” Journal of Hazardous Materials, vol. 171, no. 1–3, pp. 1–15, 2009. View at: Publisher Site | Google Scholar
  28. A. Demirbas, “Heavy metal adsorption onto agro-based waste materials: a review,” Journal of Hazardous Materials, vol. 157, no. 2-3, pp. 220–229, 2008. View at: Publisher Site | Google Scholar
  29. L. Yan, H. Yin, S. Zhang, F. Leng, W. Nan, and H. Li, “Biosorption of inorganic and organic arsenic from aqueous solution by Acidithiobacillus ferrooxidans BY-3,” Journal of Hazardous Materials, vol. 178, no. 1–3, pp. 209–217, 2010. View at: Publisher Site | Google Scholar
  30. T. Mathialagan and T. Viraraghavan, “Biosorption of pentachlorophenol by fungal biomass from aqueous solutions: a factorial design analysis,” Environmental Technology, vol. 26, no. 5, pp. 571–579, 2005. View at: Google Scholar
  31. G. M. Maciel, C. G. M. D. Souza, C. A. V. D. Araújo et al., “Biosorption of herbicide picloram from aqueous solutions by live and heat-treated biomasses of Ganoderma lucidum (Curtis) P. Karst and Trametes sp.,” Chemical Engineering Journal, vol. 215-216, pp. 331–338, 2013. View at: Publisher Site | Google Scholar
  32. F. I. Hai, O. Modin, K. Yamamoto, K. Fukushi, F. Nakajima, and L. D. Nghiem, “Pesticide removal by a mixed culture of bacteria and white-rot fungi,” Journal of the Taiwan Institute of Chemical Engineers, vol. 43, no. 3, pp. 459–462, 2012. View at: Publisher Site | Google Scholar
  33. L. N. Nguyen, F. I. Hai, S. Yang et al., “Removal of pharmaceuticals, steroid hormones, phytoestrogens, UV-filters, industrial chemicals and pesticides by Trametes versicolor: role of biosorption and biodegradation,” International Biodeterioration and Biodegradation, vol. 88, pp. 169–175, 2014. View at: Publisher Site | Google Scholar
  34. A. K. Jain, V. K. Gupta, and S. Jain, “Removal of chlorophenols using industrial wastes,” Environmental Science and Technology, vol. 38, no. 4, pp. 1195–1200, 2004. View at: Google Scholar
  35. T. A. Kurniawan, G. Y. S. Chan, W.-H. Lo, and S. Babel, “Comparisons of low-cost adsorbents for treating wastewaters laden with heavy metals,” Science of the Total Environment, vol. 366, no. 2-3, pp. 409–426, 2006. View at: Publisher Site | Google Scholar
  36. A. Bhatnagar and A. K. Minocha, “Conventional and non-conventional adsorbents for removal of pollutants from water—a review,” Indian Journal of Chemical Technology, vol. 13, no. 3, pp. 203–217, 2006. View at: Google Scholar
  37. S. Saraswat and J. P. N. Rai, “Heavy metal adsorption from aqueous solution using Eichhornia crassipes dead biomass,” International Journal of Mineral Processing, vol. 94, no. 3-4, pp. 203–206, 2010. View at: Publisher Site | Google Scholar
  38. H. Li, Y. Lin, W. Guan et al., “Biosorption of Zn(II) by live and dead cells of Streptomyces ciscaucasicus strain CCNWHX 72-14,” Journal of Hazardous Materials, vol. 179, no. 1–3, pp. 151–159, 2010. View at: Publisher Site | Google Scholar
  39. Y. Fu, Y. Fu, and T. Viraraghavan, “Removal of a dye from an aqueous solution by the fungus aspergillus niger,” Water Quality Research Journal of Canada, vol. 35, no. 1, pp. 95–111, 2000. View at: Google Scholar
  40. Y. Fu and T. Viraraghavan, “Removal of Congo Red from an aqueous solution by fungus Aspergillus niger,” Advances in Environmental Research, vol. 7, no. 1, pp. 239–247, 2002. View at: Publisher Site | Google Scholar
  41. N. R. Bishnoi, A. Pant, and Garima, “Biosorption of copper from aqueous solution using algal biomass,” Journal of Scientific and Industrial Research, vol. 63, no. 10, pp. 813–816, 2004. View at: Google Scholar
  42. A. E. Navarro, R. F. Portales, M. R. Sun-Kou, and B. P. Llanos, “Effect of pH on phenol biosorption by marine seaweeds,” Journal of Hazardous Materials, vol. 156, no. 1–3, pp. 405–411, 2008. View at: Publisher Site | Google Scholar
  43. N. Koçberber and G. Dönmez, “Chromium(VI) bioaccumulation capacities of adapted mixed cultures isolated from industrial saline wastewaters,” Bioresource Technology, vol. 98, no. 11, pp. 2178–2183, 2007. View at: Publisher Site | Google Scholar
  44. S. Srivastava, A. H. Ahmad, and I. S. Thakur, “Removal of chromium and pentachlorophenol from tannery effluents,” Bioresource Technology, vol. 98, no. 5, pp. 1128–1132, 2007. View at: Publisher Site | Google Scholar
  45. N. R. Bishnoi, M. Bajaj, N. Sharma, and A. Gupta, “Adsorption of Cr(VI) on activated rice husk carbon and activated alumina,” Bioresource Technology, vol. 91, no. 3, pp. 305–307, 2004. View at: Publisher Site | Google Scholar
  46. U. Kumar and M. Bandyopadhyay, “Sorption of cadmium from aqueous solution using pretreated rice husk,” Bioresource Technology, vol. 97, no. 1, pp. 104–109, 2006. View at: Publisher Site | Google Scholar
  47. K. K. Singh, R. Rastogi, and S. H. Hasan, “Removal of cadmium from wastewater using agricultural waste “rice polish”,” Journal of Hazardous Materials, vol. 121, no. 1–3, pp. 51–58, 2005. View at: Publisher Site | Google Scholar
  48. C. R. T. Tarley and M. A. Z. Arruda, “Biosorption of heavy metals using rice milling by-products. Characterisation and application for removal of metals from aqueous effluents,” Chemosphere, vol. 54, no. 7, pp. 987–995, 2004. View at: Publisher Site | Google Scholar
  49. D. Mohan, K. P. Singh, and V. K. Singh, “Chromium (III) removal from wastewater using low cost activated carbon derived from agriculture waste material and activated carbon fabric filter,” Journal of Hazardous Materials, vol. 135, no. 1–3, pp. 280–295, 2006. View at: Google Scholar
  50. D. Mohan, K. P. Singh, and V. K. Singh, “Trivalent chromium removal from wastewater using low cost activated carbon derived from agricultural waste material and activated carbon fabric cloth,” Journal of Hazardous Materials, vol. 135, no. 1–3, pp. 280–295, 2006. View at: Publisher Site | Google Scholar
  51. P. S. Kumar, S. Ramalingam, C. Senthamarai, M. Niranjanaa, P. Vijayalakshmi, and S. Sivanesan, “Adsorption of dye from aqueous solution by cashew nut shell: studies on equilibrium isotherm, kinetics and thermodynamics of interactions,” Desalination, vol. 261, no. 1-2, pp. 52–60, 2010. View at: Publisher Site | Google Scholar
  52. P. Venkateswarlu, M. V. Ratnam, D. S. Rao, and M. V. Rao, “Removal of chromium from aqueous solution using Azadirachta indica (neem) leaf powder as an adsorbent,” International Journal of Physical Sciences, vol. 2, pp. 188–195, 2007. View at: Google Scholar
  53. S. S. Ahluwalia and D. Goyal, “Removal of heavy metals by waste tea leaves from aqueous solution,” Engineering in Life Sciences, vol. 5, no. 2, pp. 158–162, 2005. View at: Publisher Site | Google Scholar
  54. H. Benaïssa, “Screening of new sorbent materials for cadmium removal from aqueous solutions,” Journal of Hazardous Materials, vol. 132, no. 2-3, pp. 189–195, 2006. View at: Publisher Site | Google Scholar
  55. S. Schiewer and S. B. Patil, “Modeling the effect of pH on biosorption of heavy metals by citrus peels,” Journal of Hazardous Materials, vol. 157, no. 1, pp. 8–17, 2008. View at: Publisher Site | Google Scholar
  56. M. A. Farajzadeh and A. B. Monji, “Adsorption characteristics of wheat bran towards heavy metal cations,” Separation and Purification Technology, vol. 38, no. 3, pp. 197–207, 2004. View at: Publisher Site | Google Scholar
  57. I. S. Lima, E. S. Ribeiro, and C. Airoldi, “The use of chemically modified chitosan with succinic anhydride in the methylene blue adsorption,” Quimica Nova, vol. 29, no. 3, pp. 501–506, 2006. View at: Publisher Site | Google Scholar
  58. A. R. Cestari, E. F. S. Vieira, A. G. P. dos Santos, J. A. Mota, and V. P. de Almeida, “Adsorption of anionic dyes on chitosan beads. 1. The influence of the chemical structures of dyes and temperature on the adsorption kinetics,” Journal of Colloid and Interface Science, vol. 280, no. 2, pp. 380–386, 2004. View at: Publisher Site | Google Scholar
  59. J. Wang and C. Chen, “Chitosan-based biosorbents: modification and application for biosorption of heavy metals and radionuclides,” Bioreseource Technology, vol. 160, pp. 129–141, 2014. View at: Publisher Site | Google Scholar
  60. P. X. Pinto, S. R. Al-Abed, and D. J. Reisman, “Biosorption of heavy metals from mining influenced water onto chitin products,” Chemical Engineering Journal, vol. 166, no. 3, pp. 1002–1009, 2011. View at: Publisher Site | Google Scholar
  61. M. Otero, F. Rozada, L. F. Calvo, A. I. García, and A. Morán, “Kinetic and equilibrium modelling of the methylene blue removal from solution by adsorbent materials produced from sewage sludges,” Biochemical Engineering Journal, vol. 15, no. 1, pp. 59–68, 2003. View at: Publisher Site | Google Scholar
  62. H. C. Chu and K. M. Chen, “Reuse of activated sludge biomass: I. Removal of basic dyes from wastewater by biomass,” Process Biochemistry, vol. 37, no. 6, pp. 595–600, 2002. View at: Publisher Site | Google Scholar
  63. B. Manu and S. Chaudhari, “Anaerobic decolorisation of simulated textile wastewater containing azo dyes,” Bioresource Technology, vol. 82, no. 3, pp. 225–231, 2002. View at: Publisher Site | Google Scholar
  64. P. A. Ramalho, H. Scholze, M. H. Cardoso, M. T. Ramalho, and A. M. Oliveira-Campos, “Improved conditions for the aerobic reductive decolourisation of azo dyes by Candida zeylanoides,” Enzyme and Microbial Technology, vol. 31, no. 6, pp. 848–854, 2002. View at: Publisher Site | Google Scholar
  65. M. Basibuyuk and C. F. Forster, “An examination of the adsorption characteristics of a basic dye (Maxilon Red BL-N) on to live activated sludge system,” Process Biochemistry, vol. 38, no. 9, pp. 1311–1316, 2003. View at: Publisher Site | Google Scholar
  66. W. Jianlong, Q. Yi, N. Horan, and E. Stentiford, “Bioadsorption of pentachlorophenol (PCP) from aqueous solution by activated sludge biomass,” Bioresource Technology, vol. 75, no. 2, pp. 157–161, 2000. View at: Publisher Site | Google Scholar
  67. F. Federici, F. Fava, N. Kalogerakis, and D. Mantzavinos, “Valorisation of agro-industrial by-products, effluents and waste: concept, opportunities and the case of olive mill waste waters,” Journal of Chemical Technology and Biotechnology, vol. 84, no. 6, pp. 895–900, 2009. View at: Publisher Site | Google Scholar
  68. BSR Report, Analysis of U.S. Food Waste among Food Manufacturers, Retailers & Wholesalers, 2013, http://www.bsr.org/.
  69. R. Han, H. Li, Y. Li, J. Zhang, H. Xiao, and J. Shi, “Biosorption of copper and lead ions by waste beer yeast,” Journal of Hazardous Materials, vol. 137, no. 3, pp. 1569–1576, 2006. View at: Publisher Site | Google Scholar
  70. V. Jaikumar and V. Ramamurthi, “Effect of biosorption parameters kinetics isotherm and thermodynamics for acid green dye biosorption from aqueous solution by brewery waste,” International Journal of Chemistry, vol. 1, no. 1, pp. 2–12, 2009. View at: Publisher Site | Google Scholar
  71. M. A. Dias, C. A. Rosa, V. R. Linardi, R. A. Conte, and H. F. de Castro, “Application of factorial design to study of heavy metals biosorption by waste biomass from beverage distillery,” Applied Biochemistry and Biotechnology A: Enzyme Engineering and Biotechnology, vol. 91-93, pp. 413–422, 2001. View at: Publisher Site | Google Scholar
  72. H. Lu and H. Xia, “Biosorption of cadmium from aqueous solution onto tea industry-waste,” in Proceedings of the 5th International Conference on Bioinformatics and Biomedical Engineering (iCBBE '11), pp. 1–4, May 2011. View at: Publisher Site | Google Scholar
  73. C.-C. Liu, M.-K. Wang, C.-S. Chiou, Y.-S. Li, Y.-A. Lin, and S.-S. Huang, “Chromium removal and sorption mechanism from aqueous solutions by wine processing waste sludge,” Industrial and Engineering Chemistry Research, vol. 45, no. 26, pp. 8891–8899, 2006. View at: Publisher Site | Google Scholar
  74. K. Parvathi and R. Nagendran, “Functional groups on waste beer yeast involved in chromium biosorption from electroplating effluent,” World Journal of Microbiology and Biotechnology, vol. 24, no. 12, pp. 2865–2870, 2008. View at: Publisher Site | Google Scholar
  75. M. A. Dias, H. F. Castro, P. F. Pimentel, N. C. M. Gomes, C. A. Rosa, and V. R. Linardi, “Removal of heavy metals from stainless steel effluents by waste biomass from Brazilian alcoholic beverage production,” World Journal of Microbiology and Biotechnology, vol. 16, no. 1, pp. 107–108, 2000. View at: Publisher Site | Google Scholar
  76. C.-C. Liu, M. Kuang-Wang, and Y.-S. Li, “Removal of nickel from aqueous solution using wine processing waste sludge,” Industrial and Engineering Chemistry Research, vol. 44, no. 5, pp. 1438–1445, 2005. View at: Google Scholar
  77. D. Pujol, M. Bartrolí, N. Fiol, F. D. L. Torre, I. Villaescusa, and J. Poch, “Modelling synergistic sorption of Cr(VI), Cu(II) and Ni(II) onto exhausted coffee wastes from binary mixtures Cr(VI)-Cu(II) and Cr(VI)-Ni(II),” Chemical Engineering Journal, vol. 230, pp. 396–405, 2013. View at: Publisher Site | Google Scholar
  78. K. A. G. Gusmão, L. V. A. Gurgel, T. M. S. Melo, and L. F. Gil, “Adsorption studies of methylene blue and gentian violet on sugarcane bagasse modified with EDTA dianhydride (EDTAD) in aqueous solutions: kinetic and equilibrium aspects,” Journal of Environmental Management, vol. 118, pp. 135–143, 2013. View at: Publisher Site | Google Scholar
  79. N. V. Farinella, G. D. Matos, E. L. Lehmann, and M. A. Z. Arruda, “Grape bagasse as an alternative natural adsorbent of cadmium and lead for effluent treatment,” Journal of Hazardous Materials, vol. 154, no. 1–3, pp. 1007–1012, 2008. View at: Publisher Site | Google Scholar
  80. C. Majdik, S. Burcǎ, A. Mǎicǎneanu, M. Stanca, S. Tonk, and P. Mezey, “Suspended and immobilized brewery waste biomass and commercial yeast as biosorbents for Cd(II) removal. A thermodynamic study,” Revue Roumaine de Chimie, vol. 55, no. 11-12, pp. 871–877, 2010. View at: Google Scholar
  81. W.-T. Tsai, H.-C. Hsu, T.-Y. Su, K.-Y. Lin, and C.-M. Lin, “Removal of basic dye (methylene blue) from wastewaters utilizing beer brewery waste,” Journal of Hazardous Materials, vol. 154, no. 1–3, pp. 73–78, 2008. View at: Publisher Site | Google Scholar
  82. K. Parvathi, R. Nagendran, and R. Nareshkumar, “Lead biosorption onto waste beer yeast by-product, a means to decontaminate effluent generated from battery manufacturing industry,” Electronic Journal of Biotechnology, vol. 10, no. 1, pp. 92–105, 2007. View at: Publisher Site | Google Scholar
  83. E. O. Oyelude and F. Appiah-Takyi, “Removal of methylene blue from aqueous solution using alkali-modified malted sorghum mash,” Turkish Journal of Engineering and Environmental Sciences, vol. 36, no. 2, pp. 161–169, 2012. View at: Publisher Site | Google Scholar
  84. A. S. Özcan, S. Tunali, T. Akar, and A. Özcan, “Biosorption of lead(II) ions onto waste biomass of Phaseolus vulgaris L.: estimation of the equilibrium, kinetic and thermodynamic parameters,” Desalination, vol. 244, no. 1–3, pp. 188–198, 2009. View at: Publisher Site | Google Scholar
  85. H. D. Ozsoy, H. Kumbur, B. Saha, and J. H. van Leeuwen, “Use of Rhizopus oligosporus produced from food processing wastewater as a biosorbent for Cu(II) ions removal from the aqueous solutions,” Bioresource Technology, vol. 99, no. 11, pp. 4943–4948, 2008. View at: Publisher Site | Google Scholar
  86. S. T. Akar, A. S. Özcan, T. Akar, A. Özcan, and Z. Kaynak, “Biosorption of a reactive textile dye from aqueous solutions utilizing an agro-waste,” Desalination, vol. 249, no. 2, pp. 757–761, 2009. View at: Publisher Site | Google Scholar
  87. N. F. Cardoso, E. C. Lima, I. S. Pinto et al., “Application of cupuassu shell as biosorbent for the removal of textile dyes from aqueous solution,” Journal of Environmental Management, vol. 92, no. 4, pp. 1237–1247, 2011. View at: Publisher Site | Google Scholar
  88. A. B. S. Al-Barak and S. M. El-Said, “The use of some food industrial by-products for waste water purification,” Research Journal of Environmental Sciences, vol. 4, no. 6, pp. 566–572, 2010. View at: Publisher Site | Google Scholar
  89. A. Kumar and O. Sahu, “Sugar industry waste as removal of toxic metals from waste water,” World Journal of Chemical Education, vol. 1, pp. 17–20, 2013. View at: Google Scholar
  90. S. Tunali, A. Ozcan, Z. Kaynak, A. S. Ozcan, and T. Akar, “Utilization of the Phaseolus vulgaris L. waste biomass for decolorization of the textile dye Acid Red 57: determination of equilibrium, kinetic and thermodynamic parameters,” Journal of Environmental Science and Health A: Toxic/Hazardous Substances and Environmental Engineering, vol. 42, no. 5, pp. 591–600, 2007. View at: Publisher Site | Google Scholar
  91. R. R. Krishni, K. Y. Foo, and B. H. Hameed, “Food cannery effluent, pineapple peel as an effective low-cost biosorbent for removing cationic dye from aqueous solutions,” Desalination and Water Treatment, 2013. View at: Publisher Site | Google Scholar
  92. M. R. Lasheen, N. S. Ammar, and H. S. Ibrahim, “Adsorption/desorption of Cd(II), Cu(II) and Pb(II) using chemically modified orange peel: equilibrium and kinetic studies,” Solid State Sciences, vol. 14, no. 2, pp. 202–210, 2012. View at: Publisher Site | Google Scholar
  93. A. B. P. Marín, M. I. Aguilar, V. F. Meseguer, J. F. Ortuño, J. Sáez, and M. Lloréns, “Biosorption of chromium (III) by orange (Citrus cinensis) waste: batch and continuous studies,” Chemical Engineering Journal, vol. 155, no. 1-2, pp. 199–206, 2009. View at: Publisher Site | Google Scholar
  94. S. Schiewer and S. B. Patil, “Pectin-rich fruit wastes as biosorbents for heavy metal removal: equilibrium and kinetics,” Bioresource Technology, vol. 99, no. 6, pp. 1896–1903, 2008. View at: Publisher Site | Google Scholar
  95. A. B. Pérez-Marín, V. M. Zapata, J. F. Ortuño, M. I. Aguilar, J. Sáez, and M. Lloréns, “Removal of cadmium from aqueous solutions by adsorption onto orange waste,” Journal of Hazardous Materials, vol. 139, no. 1, pp. 122–131, 2007. View at: Publisher Site | Google Scholar
  96. A. B. Pérez Marín, J. F. Ortuño, M. I. Aguilar, V. F. Meseguer, J. Sáez, and M. Lloréns, “Use of chemical modification to determine the binding of Cd(II), Zn(II) and Cr(III) ions by orange waste,” Biochemical Engineering Journal, vol. 53, pp. 2–6, 2010. View at: Publisher Site | Google Scholar
  97. M. N. Rashed, “Fruit stones from industrial waste for the removal of lead ions from polluted water,” Environmental Monitoring and Assessment, vol. 119, no. 1–3, pp. 31–41, 2006. View at: Publisher Site | Google Scholar
  98. K. V. Kumar and A. Kumaran, “Removal of methylene blue by mango seed kernel powder,” Biochemical Engineering Journal, vol. 27, no. 1, pp. 83–93, 2005. View at: Publisher Site | Google Scholar
  99. W. S. Alencar, E. Acayanka, E. C. Lima et al., “Application of Mangifera indica (mango) seeds as a biosorbent for removal of Victazol Orange 3R dye from aqueous solution and study of the biosorption mechanism,” Chemical Engineering Journal, vol. 209, pp. 577–588, 2012. View at: Publisher Site | Google Scholar
  100. K. Johari, N. Saman, S. T. Song, H. Mat, and D. C. Stuckey, “Utilization of coconut milk processing waste as a low-cost mercury sorbent,” Industrial Engineering Chemistry Research, vol. 52, no. 44, pp. 15648–15657, 2013. View at: Publisher Site | Google Scholar
  101. E. Malkoc, Y. Nuhoglu, and M. Dundar, “Adsorption of chromium(VI) on pomace—an olive oil industry waste: batch and column studies,” Journal of Hazardous Materials, vol. 138, no. 1, pp. 142–151, 2006. View at: Publisher Site | Google Scholar
  102. G. Blázquez, M. Calero, F. Hernáinz, G. Tenorio, and M. A. Martín-Lara, “Equilibrium biosorption of lead(II) from aqueous solutions by solid waste from olive-oil production,” Chemical Engineering Journal, vol. 160, no. 2, pp. 615–622, 2010. View at: Publisher Site | Google Scholar
  103. G. Martinez-Garcia, R. T. Bachmann, C. J. Williams, A. Burgoyne, and R. G. J. Edyvean, “Olive oil waste as a biosorbent for heavy metals,” International Biodeterioration and Biodegradation, vol. 58, no. 3-4, pp. 231–238, 2006. View at: Publisher Site | Google Scholar
  104. F. Vegliò, F. Beolchini, and M. Prisciandaro, “Sorption of copper by olive mill residues,” Water Research, vol. 37, no. 20, pp. 4895–4903, 2003. View at: Publisher Site | Google Scholar
  105. N. Fiol, I. Villaescusa, M. Martínez, N. Miralles, J. Poch, and J. Serarols, “Sorption of Pb(II), Ni(II), Cu(II) and Cd(II) from aqueous solution by olive stone waste,” Separation and Purification Technology, vol. 50, no. 1, pp. 132–140, 2006. View at: Publisher Site | Google Scholar
  106. G. Blázquez, F. Hernáinz, M. Calero, and L. F. Ruiz-Núñez, “Removal of cadmium ions with olive stones: the effect of some parameters,” Process Biochemistry, vol. 40, no. 8, pp. 2649–2654, 2005. View at: Publisher Site | Google Scholar
  107. F. Pagnanelli, S. Mainelli, F. Vegliò, and L. Toro, “Heavy metal removal by olive pomace: biosorbent characterisation and equilibrium modelling,” Chemical Engineering Science, vol. 58, no. 20, pp. 4709–4717, 2003. View at: Publisher Site | Google Scholar
  108. A. Fernando, S. Monteiro, F. Pinto, and B. Mendes, “Production of biosorbents from waste olive cake and its adsorption characteristics for Zn2+ ion,” Sustainability, vol. 1, no. 2, pp. 277–297, 2009. View at: Publisher Site | Google Scholar
  109. F. Banat, S. Al-Asheh, R. Al-Ahmad, and F. Bni-Khalid, “Bench-scale and packed bed sorption of methylene blue using treated olive pomace and charcoal,” Bioresource Technology, vol. 98, no. 16, pp. 3017–3025, 2007. View at: Publisher Site | Google Scholar
  110. A. S. Stasinakis, I. Elia, A. V. Petalas, and C. P. Halvadakis, “Removal of total phenols from olive-mill wastewater using an agricultural by-product, olive pomace,” Journal of Hazardous Materials, vol. 160, no. 2-3, pp. 408–413, 2008. View at: Publisher Site | Google Scholar
  111. M. Abbas, A. Zaini, M. Zakaria, S. H. M. Setapar, and M. A. C. Yunus, “Sludge-adsorbents from palm oil mill effluent for methylene blue removal,” Journal of Environmental Chemical Engineering, vol. 1, no. 4, pp. 1091–1098, 2013. View at: Publisher Site | Google Scholar
  112. Y. Zhang and C. Banks, “A comparison of the properties of polyurethane immobilised Sphagnum moss, seaweed, sunflower waste and maize for the biosorption of Cu, Pb, Zn and Ni in continuous flow packed columns,” Water Research, vol. 40, no. 4, pp. 788–798, 2006. View at: Publisher Site | Google Scholar
  113. R. Baccar, P. Blánquez, J. Bouzid, M. Feki, and M. Sarrà, “Equilibrium, thermodynamic and kinetic studies on adsorption of commercial dye by activated carbon derived from olive-waste cakes,” Chemical Engineering Journal, vol. 165, no. 2, pp. 457–464, 2010. View at: Publisher Site | Google Scholar
  114. K. Y. Foo and B. H. Hameed, “Preparation of oil palm (Elaeis) empty fruit bunch activated carbon by microwave-assisted KOH activation for the adsorption of methylene blue,” Desalination, vol. 275, no. 1–3, pp. 302–305, 2011. View at: Publisher Site | Google Scholar
  115. C. Duran, D. Ozdes, A. Gundogdu, M. Imamoglu, and H. B. Senturk, “Tea-industry waste activated carbon, as a novel adsorbent, for separation, preconcentration and speciation of chromium,” Analytica Chimica Acta, vol. 688, no. 1, pp. 75–83, 2011. View at: Publisher Site | Google Scholar
  116. C. Karthika, N. Vennilamani, S. Pattabhi, and M. Sekar, “Utilization of sago waste as an adsorbent for the removal of Pb(II) from aqueous solution: kinetic and isotherm studies,” International Journal of Engineering Science and Technology, vol. 2, pp. 1867–1879, 2010. View at: Google Scholar
  117. C. Guo, T. Yue, Y. Yuan et al., “Biosorption of patulin from apple juice by caustic treated waste cider yeast biomass,” Food Control, vol. 32, no. 1, pp. 99–104, 2013. View at: Publisher Site | Google Scholar
  118. L. Svecova, M. Spanelova, M. Kubal, and E. Guibal, “Cadmium, lead and mercury biosorption on waste fungal biomass issued from fermentation industry. I. Equilibrium studies,” Separation and Purification Technology, vol. 52, no. 1, pp. 142–153, 2006. View at: Publisher Site | Google Scholar
  119. N. Yeddou-Mezenner, “Kinetics and mechanism of dye biosorption onto an untreated antibiotic waste,” Desalination, vol. 262, no. 1–3, pp. 251–259, 2010. View at: Publisher Site | Google Scholar
  120. S. Moussous, A. Selatnia, A. Merati, and G. A. Junter, “Batch cadmium(II) biosorption by an industrial residue of macrofungal biomass (Clitopilus scyphoides),” Chemical Engineering Journal, vol. 197, pp. 261–271, 2012. View at: Publisher Site | Google Scholar
  121. V. Prigione, I. Grosso, V. Tigini, A. Anastasi, and G. C. Varese, “Fungal waste-biomasses as potential low-cost biosorbents for decolorization of textile wastewaters,” Water, vol. 4, no. 4, pp. 770–784, 2012. View at: Publisher Site | Google Scholar
  122. K. R. Rao, K. Rashmi, J. N. L. Latha, and P. M. Mohan, “Bioremediation of toxic metal ions using biomass of Aspergillus fumigatus from fermentative waste,” Indian Journal of Biotechnology, vol. 4, no. 1, pp. 139–143, 2005. View at: Google Scholar
  123. R. A. K. Rao, M. A. Khan, and F. Rehman, “Utilization of Fennel biomass (Foeniculum vulgari) a medicinal herb for the biosorption of Cd(II) from aqueous phase,” Chemical Engineering Journal, vol. 156, no. 1, pp. 106–113, 2010. View at: Publisher Site | Google Scholar
  124. V. K. Gochev, Z. I. Velkova, and M. S. Stoytcheva, “Hexavalent chromium removal by waste mycelium of Aspergillus awamori,” Journal of the Serbian Chemical Society, vol. 75, no. 4, pp. 551–564, 2010. View at: Publisher Site | Google Scholar
  125. Z. Velkova, M. Stoytcheva, and V. Gochev, “Biosorption of Cu (II) onto chemically modified waste mycelium of Aspergillus awamori: equilibrium, kinetics and modeling studies,” Journal of Bioscience & Biotechnology, vol. 1, no. 2, pp. 163–169, 2012. View at: Google Scholar
  126. T. Budinova, N. Petrov, J. Parra, and V. Baloutzov, “Use of an activated carbon from antibiotic waste for the removal of Hg(II) from aqueous solution,” Journal of Environmental Management, vol. 88, no. 1, pp. 165–172, 2008. View at: Publisher Site | Google Scholar
  127. K. Vijayaraghavan and Y.-S. Yun, “Utilization of fermentation waste (Corynebacterium glutamicum) for biosorption of Reactive Black 5 from aqueous solution,” Journal of Hazardous Materials, vol. 141, no. 1, pp. 45–52, 2007. View at: Publisher Site | Google Scholar
  128. M. Fomina and G. M. Gadd, “Biosorption: current perspectives on concept, definition and application,” Bioresource Technology, vol. 160, pp. 3–14, 2014. View at: Publisher Site | Google Scholar
  129. M. Sassi, B. Bestani, A. H. Said, N. Benderdouche, and E. Guibal, “Removal of heavy metal ions from aqueous solutions by a local dairy sludge as a biosorbant,” Desalination, vol. 262, no. 1–3, pp. 243–250, 2010. View at: Publisher Site | Google Scholar
  130. D. Zhang, H. He, W. Li, T. Gao, and P. Ma, “Biosorption of cadmium(II) and lead(II) from aqueous solutions by fruiting body waste of fungus Flammulina velutipes,” Desalination and Water Treatment, vol. 20, no. 1–3, pp. 160–167, 2010. View at: Publisher Site | Google Scholar
  131. Y. Göksungur, S. Üren, and U. Güvenç, “Biosorption of cadmium and lead ions by ethanol treated waste baker's yeast biomass,” Bioresource Technology, vol. 96, no. 1, pp. 103–109, 2005. View at: Publisher Site | Google Scholar
  132. I. A. Aguayo-Villarreal, L. A. Ramírez-Montoya, V. Hernández-Montoya, A. Bonilla-Petriciolet, M. A. Montes-Morán, and E. M. Ramírez-López, “Sorption mechanism of anionic dyes on pecan nut shells (Carya illinoinensis) using batch and continuous systems,” Industrial Crops and Products, vol. 48, pp. 89–97, 2013. View at: Publisher Site | Google Scholar
  133. S. Schiewer and A. Balaria, “Biosorption of Pb2+ by original and protonated citrus peels: equilibrium, kinetics, and mechanism,” Chemical Engineering Journal, vol. 146, no. 2, pp. 211–219, 2009. View at: Publisher Site | Google Scholar
  134. S. Andreea, “Brewer’s yeast: an alternative for heavy metal biosorption from waste waters,” ProEnvironment, vol. 6, no. 15, pp. 457–464, 2013. View at: Google Scholar
  135. O. Keskinkan, M. Z. L. Goksu, A. Yuceer, M. Basibuyuk, and C. F. Forster, “Heavy metal adsorption characteristics of a submerged aquatic plant (Myriophyllum spicatum),” Process Biochemistry, vol. 39, no. 2, pp. 179–183, 2003. View at: Publisher Site | Google Scholar
  136. D. D. Xie, Y. Y. Liu, C. L. Wu, J. K. Fu, and R. Xue, “Studies on biosorption of Pd2+ by the immobilized Saccharomyces cerevisiae waste biomass,” Microbiology, vol. 30, pp. 29–34, 2003. View at: Google Scholar
  137. R. Dhankhar and A. Hooda, “Fungal biosorption—an alternative to meet the challenges of heavy metal pollution in aqueous solutions,” Environmental Technology, vol. 32, no. 5, pp. 467–491, 2011. View at: Publisher Site | Google Scholar
  138. N. Ahalya, T. V. Ramachandra, and R. D. Kanamadi, “Biosorption of heavy metals,” Research Journal of Chemistry and Environment, vol. 7, pp. 71–79, 2003. View at: Google Scholar
  139. K. Y. Foo and B. H. Hameed, “Insights into the modeling of adsorption isotherm systems,” Chemical Engineering Journal, vol. 156, no. 1, pp. 2–10, 2010. View at: Publisher Site | Google Scholar
  140. E. Njikam and S. Schiewer, “Optimization and kinetic modeling of cadmium desorption from citrus peels: a process for biosorbent regeneration,” Journal of Hazardous Materials, vol. 213-214, pp. 242–248, 2012. View at: Publisher Site | Google Scholar

Copyright © 2014 Hanan E. M. El-Sayed and Mayyada M. H. El-Sayed. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

2790 Views | 916 Downloads | 12 Citations
 PDF  Download Citation  Citation
 Download other formatsMore
 Order printed copiesOrder

We are committed to sharing findings related to COVID-19 as quickly and safely as possible. Any author submitting a COVID-19 paper should notify us at help@hindawi.com to ensure their research is fast-tracked and made available on a preprint server as soon as possible. We will be providing unlimited waivers of publication charges for accepted articles related to COVID-19.