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

Authors: Hanan E. M. El-Sayed; Mayyada M. H. El-Sayed
Journal: BioMed Research International
 (2014)

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## 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.


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## Body

## 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 [1–3]. 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 achievedphysically, 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 [8–10]. These processes known asconventional 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, 11–13]. 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 [15–21] and heavy metals [22–28]. Few research studies have focused on the removal of organic pollutants, phenols and phenolic compounds, and pesticides using different biosorbents [29–34].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 especiallybiosorbents [24, 35]. Sources of different types of conventional and nonconventional adsorbents are illustrated in the flow chart in Figure 1.Figure 1
A schematic flow diagram showing the different types of available adsorbents.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 [45–48], different nut shells [49–51], fruit and vegetable peels or leaves [52–55], wheat bran [56], chitin and chitosan [57–60], 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 [62–66].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 Table1. 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 (F) 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 [69–83]. 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 [84–89]. 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 [91–99], 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.Table 1
Summary of the different industrial food processing and pharmaceutical waste biosorbents; their sources, applications, and the relevant biosorption parameters.
Type of  biosorbent
Source of biosorbent
Feed solution
Sorbate
pH
Contact time, min
Temperature, °C
Initial concentration of sorbate, mg/L
Mode of operation
Maximum%removal
Biosorbent dose
Reference
Spent brewery grains (SBG)
Mohan breweries and distilleries Limited, Chennai, India
Synthetic dye solution
AG25 acid dye of commercial name Alizarin Cyanin Green G
3.0
75
30
90
Batch
98
0.2
[70]
Tea industry waste
Local tea factory in China
Aqueous synthetic solution
Cd(II)
7.0
180
25
20
Batch
90
5
[72]
Exhausted coffee waste
Soluble coffee manufacturer, Catalonia, Spain
Aqueous synthetic solution
Cr(VI)Cu(II)Ni(II)
3.0
8640
25
1000
Batch
—
6.67
[77]
Sugarcane bagasse waste
From local alcohol and sugar
Aqueous synthetic  solution
Methylene Blue (MB)
7.0
600
25
200
Batch
—
0.2
[78]
Industries, City of Ouro Preto, Minas Gerais, Brazil
Gentian Violet
900
300
Wine processing waste sludge (WPWS)
Ilan Wine-Processing Company, Ilan, Taiwan
Aqueous synthetic solution
Cr(III, IV)
2.0
240
30
100
Batch
36
10
[73]
Wine processing waste sludge (WPWS)
IlanWine-Processing Co., Ilan, Taiwan
Aqueous synthetic solution
Ni(II)
5.5
120
50
30
Batch
75
12
[76]
Grape bagasse waste residue
Wine production process, Styria region, Austria
Effluent from research laboratory
Cd(II)Pb(II)
7.03.0
45
25
100
Batch
—
0.67
[79]
Waste beer yeast
Aoke Beer Company in Zhengzhou, Henan province, China
Aqueous synthetic solution
Cu(II)Pb(II)
5.0
30
20
9.1432.23
Batch
—
—
[69]
Waste beer yeastSaccharomyces  cerevisiae
Beer fermentation industry, brewery located near Chennai, India
Electroplating effluents
Cr(VI)
5.0
120
—
—
Batch
—
0.02
[74]
Suspended brewery yeast waste biomass(SBW)
Brewery waste biomass collected from CIUC brewery, Miercurea-Ciuc, Romania
Synthetic aqueous solution
Cd(II)
5.5
40
50
6
Batch
99.83
9.78
[80]
Beer brewery diatomite waste (SDE)
Shan-Hua factory, Tobacco and Liquor Co., TainanTaiwan
Synthetic aqueous solutionIndustrial wastewater from local factory
Methylene Blue (MB) basic dye
7.0
1440
25
2.5
Batch
—
0.25
[81]
Spent waste beer yeast
Saccharomyces  cerevisiae
Fermentor at a brewery, Chennai, India
Battery manufacturing industrial effluent
Pb(II)
5.0
120
30
100
Batch
—
—
[82]
Fresh malted sorghum mash waste
local malted sorghum beer (pito) brewer at Navrongo, Ghana
Synthetic aqueous solution
Methylene Blue (MB) basic dye
7.0
18
33
±
1
50
Batch
>90
4
[83]
Waste biomass from sugarcane aguardente
Brazilian alcoholic beverage production, (Lapinha,  Bocaiana, Germana and Taboroa) State of Minas Gerais, Brazil
Stainless steel effluent
Cr(VI)Fe(III)Ni(II)
4.0
180
25
5066020
Batch
705020
1
[75]
Waste biomass Cachaça  Brazilian alcoholic beverage
the stillage generated by a liquor distillery (Germana), Minas Gerais, Brazil
Stainless steel industrial effluent from Acesita Co., Brazil
Fe(III)Ni(II)Cr(VI)
4.0
180
25
7.82.7600
Batch
945725
2
[71]
Rhizopus oligosporus biomass
Food processing wastewaters
Aqueous synthetic solution
Cu(II)
5.0
120
30
100
Batch
70
1
[85]
Waste biomass ofPhaseolus  vulgaris  L.
A residual biomass of a canned food factory in Bartin, Turkey
Aqueous synthetic solution
Pb(II)
5.0
20
20
100
Batch
92
4
[84]
Waste biomass ofPhaseolus  vulgaris  L.
A residual biomass of a local  canned food plant, Turkey
Aqueous synthetic solution
Textile Reactive Red dye (RR 198)
2.0
20
20
100–300
Batch
99.3
1.6
[86]
Cupuassu shell,Theobroma  grandiflorum, (CS)
Food residue from jelly industry, Belém-PA, Brazil
Aqueous synthetic solution
Reactive Red dye (RR 194)
2.0
480
25
50
Batch
—
2.5
[87]
Direct Blue 53
1080
Okra food industrial waste
Food waste from food canning processes
Aqueous synthetic solution
Cd(II)Fe(II)Zn(II)
—
90
—
20
Batch
96.493.879.8
1
[88]
Sugar industrial waste (bagasse waste)
Obtained from food canning processes
Aqueous synthetic solution
Cd(II)Fe(II)
—
90
—
20
Batch
96.493.8
1
[89]
Pineapple peel, an agricultural effluent
Food can processing industries
Aqueous synthetic solution
Methylene Blue (MB) cationic dye
6.0
400
30
300
Batch
47
1.5
[91]
Waste baker’s yeast biomass
Pakmaya Yeast Company, Izmir, Turkey
Aqueous synthetic solution
Cd(II)Pb(II)
6.05.0
180
30
25
Batch
6070
1
[131]
Desiccated coconut waste sorbent (DCWS)
By-product of Coconut Milk Processing
Aqueous synthetic solution
Hg(II)
7.4
2880400
30
50100
Batch Column
—
1
F = 4 mL/min
[100]
Pecan nut shells (C. illinoinensis) biomass
Biomass from food factories, Nuevo Leon, Mexico
Aqueous synthetic solution
Acid Blue 74 (AB74)
6.5
500
30
100
Batch
Column
—
10 F
=
3 mL/min
[132]
Reactive Blue 4 (RB4)
1000
Acid Blue 25 (AB25)
500
Orange peel
Solid waste from local fruit juice industries, Egypt
Aqueous synthetic solution
Pb(II)Cu(II)Cd(II)
5.0
30
25
20
Batch
99.589.5781.03
4
[101]
Orange (Citrus sinensis) waste
Agrumexport, S.L., an orange juice manufacturing companylocated in Murcia, Spain
Aqueous synthetic solution
Cr(III)
4.04.0
43201523
2525
10020
Batch Column
8157.5
4
[102]
Pectin-rich fruit wastes
Residues from fruit juice and wine production, from a citrus-juice producer (Sunkist), USA
Aqueous synthetic solution
Cd(II)
5.0
50
—
60
Batch
46
2
[133]
Orange waste
From orange juice industry, Spain
Aqueous synthetic solution
Cd(II)
6.0
60
25
100
Batch
98
4
[94]
Orange waste
From orange juice industry, Spain
Aqueous synthetic solution
Cd(II)Zn(II)Cr(III)
4.0
1801804320
20
151515
Batch
869095
4
[95]
Peach and Apricot stones
Solid wastes of juice and jam industries, Egypt
Aqueous synthetic solution
Pb(II)
7.0
180300
—
54.65
Batch
97.6495.3
10
[97]
Mangifera  indica (mango) seed kernel particles
Local juice manufacturing industry
Aqueous synthetic solution
Methylene Blue (MB) cationic dye
8.0
120
30
100
Batch
96.17
0.67
[98]
Mango seeds (MS)Mangifera  indica  L.
Juice producer, Ubá-MG, Brazil
Aqueous synthetic solution
Victazol Orange 3R dye (VO-3R)
2.0
360
25
40
Batch
—
2.5
[99]
Waste cider yeastbiomass
Fermentation Lab at the College of Food Science and Engineering of Northwest A & F University (Yangling, China)
Apple juice solution
Patulin (PAT)
4.5
2160
25
0.10.2
Batch Column
58.29
5
F = 2 mL/min
[117]
Dairy sludge
Dairy plant, France
Aqueous synthetic solution
Pb(II)Cd(II)
5.0
500
20
200100
Batch
>90
0.5–4.0
[129]
The waste pomace of olive oil factory (WPOOF)
TurkishPrina, Aegean region, Manisa, Turkey
Aqueous synthetic solution
Cr(VI)
2.0
120
60
50100
Batch Column
10021.74
5
F = 5 mL/min
[101]
Solid waste fromolive oil production
The OS and OMS wastes were provided by the “Cooperativa Nuestra Se
~nora desl Castillo” extraction plant located in Vilches, in the province of Jaen (Spain)
Aqueous synthetic solution
Pb(II)
5.0
120
25
—
Batch
—
10
[102]
Olive mill waste (OMW) two-phase decanter
Mixture of pulp and olivestones from the crushing of olives to obtain the oil, UK
Aqueous synthetic solution
Pb(II)Cd(II) Cu(II) Hg(II) Fe(II)
7.0
30
20
10
Batch
8075
10
[103]
Olive mill residues (OMR)
Solid residues of oil production, provided by an olive mill in Abruzzo, Italy.
Aqueous synthetic solution
Cu(II)
5.54-5
150–1440
Room temperature
4040
Batch Column
60%—
1080
[104]
Palm oil mill effluent (POME) sludge
Waste sludge from palm oil mill, Felda Taib Andak, Johor, Malaysia
Aqueous synthetic solution
Methylene Blue (MB) cationic dye
7.5
4320
27
100
Batch
—
2
[111]
Sunflower oilWaste biomass
Biomass obtained from a sunflower oil productionFacility, Seville, Spain
Aqueous synthetic solution(mixed solution)
Pb(II)Ni(II)Zn(II)Cu(II)
4.0
—
—
10
Column
—
F
=
2 L/h
[112]
Crushed olive stone wastes
Supplied by an olive oilProducer, Cordoba, Spain
Aqueoussyntheticsolution
Pb(II)Ni(II)Cu(II)Cd(II)
5.5
60
20
18.864.204.354.80
Batch
79708195
13.3
[105]
Waste olive cake (OC)
Supplied by “ProBeira” an olive oil producer, Envendos  Portugal
Aqueoussyntheticsolution
Zn(II)
6.0-7.0
120
25
10
Batch
93
1
[108]
Olive stones
From the orujo oil extraction plant ‘‘OrujeraUbetense, Sociedad Cooperativa Andaluza,’’ Jaen, Spain
AqueoussyntheticSolution
Cd(II)
11
360
40
10
Batch
90
0.01
[106]
Olive pomace
Supplied by an Italian olive oil productionplant
AqueoussyntheticSolution
Cu(II)Cd(II)Pb(II)
5.0
60
—
—
Batch
—
10
[107]
Olive pomace
Supplied by one of the olive oil productionPlants, Jordan
AqueoussyntheticSolution
Methylene Blue (MB)  dye
—
240
25
1040
Batch Column
8062.25
2
F
=
20 mL/min
[109]
Olive pomaceOP-1OP-2OP-3
Solid by-products of olive oil  processing mills, the island of Lesvos, Greece.
Oil mill waste water (OMWW)
Phenol
10.0
120
20
50500
Batch Column
>9090
10
F
=
1 mL/min
[110]
Activated carbon derived from exhausted olive waste cake
Olive waste cake from oil factory “Agrozitex”  Sfax, Tunisia
Synthetic aqueous solutionIndustrial wastewater from local factory
Lanaset Grey G
6.0
3000
25
150
Batch
93
1.67
[113]
Activated carbon derived from empty fruit bunch (EFB)
Industrial waste from united palm oil mill, Nibong, Tebal, Malaysia
Synthetic aqueous solution
Methylene Blue dye (MB)
12
—
30
200
Batch
—
1
[114]
Activated carbon from tea industry waste (TIWAC)
Tea waste from tea processing plant, Black Sea region, Trabzon, Turkey
Real water samples
Cr(VI)Cr(III)
6.0
30
—
0.2
Batch
095–100
2
[115]
Activated carbon from sago waste
Sago waste is collected from sago industry, Salem district, Tamilnadu, India
Synthetic aqueous solutionIndustrial wastewater from radiator industry
Pb(II)
3.5
±
0.3
180
27
10
Batch
87.34
2
[116]
Phaseolus  vulgaris  L.
Canned food factory
Aqueous synthetic solution
Acid Red 57 dye
2.0
20
20
150
Batch
—
1.6
[91]
Textile wastewater
1 (spiked wastewater sample)
97.68
Industrial fungiPenicillium oxalicum var. Armeniaca
Ascolor Biotec (Pardubice, Czech Republic)and Ivax Pharmaceuticals (Opava, Czech Republic)
Aqueous synthetic solution
Pb(II)Hg(II)Cd(II)
5.0
—
20
105050
Batch
Up to 85 for Hg
0.3
[118]
Fruit waste macrofungiFlammulina  velutipes
Mushroom processing factory
Aqueous synthetic solution
Cd(II)Pb(II)
6.0
60
25
10
Batch
7570
18
[130]
Tolypocladium sp.
Czech Industrial Partners
Aqueous synthetic solution
Cd(II)Pb(II)Hg(II)
5.0
20
—
50
Batch
—
0.3
[118]
Antibiotic wasteP. mutilus
SAIDAL antibioticproduction complex at Medea (Algeria)
Aqueous synthetic solution
Basic Blue 41, cationic dye
8.0-9.0
60
30
50
Batch
75
0.5
[119]
Industrial waste ofClitopilus  scyphoides(Pleurotus  mutilus) fungal biomass
Antibioticproduction plant, SAIDAL antibioticproduction complex in Médéa (Algeria)
Aqueous synthetic solution
Cd(II)
5.0
15
20
200
Batch
41
1
[120]
Fungal waste biomass
Pharmaceutical companies, Italy
Textile wastewater effluents
Dye mixtures
3.0
30
25
60–5000
Batch
90
16.7
[121]
Nonliving biomassAspergillus  fumigatus
Fermentation industry, Artemis Pharmaceuticals Limited, HAD, Jeedimetla, Hyderabad, India
Aqueous synthetic solution
persemixtureCu(II)Cd(II)Co(II)Ni(II)
7.0
60
—
4.82.94.82.72.8
Batch
7090
208
[122]
Nonliving biomassAspergillus  awamori
Industrial complex enzyme preparation
Aqueous synthetic solution
Cr(VI)
2.0
40
1152
25
Batch
87
1
[124]
Nonliving biomassAspergillus  awamori
Industrial complex enzyme preparation
Aqueous synthetic solution
Cu(II)
5.0
20
180
100
Batch
—
1
[125]
Corynebacterium
glutamicum
Fermentation industry(BASF-Korea)
Aqueous synthetic solution
Reactive Black 5 (RB5)
1.0
35
500
500
Batch
—
2.5
[127]
Activated carbon from antibiotic waste
Industrial antibiotic production
Aqueous synthetic solution
Hg(II)
5.5
—
30
40
Batch
—
0.2
[126]
Fennel biomass (Foeniculum  vulgare)
Medical herb, local Unani medicine manufacturing unit at Aligarh, India
Aqueous synthetic solution
Cd(II)MixtureCd(II)Ni(II)Zn(II)Cu(II)
4.3
5050 each
50
100
Batch Column
9297
10
F
=
1 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 [101–110]. 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 areAspergillus niger,Pleurotus mutilus,Trichoderma reesei,Rhizopus arrhizus,Rhizopus nigricans, andPenicillium chrysogenum. Bacterial biomass could be produced from antibiotic fermentation such asStreptomyces spp. or during production of drugs such asStreptomyces noursei,S. rimosus, andS. clavuligerus or during enzyme manufacture such as the bacillus species ofB. licheniformis andS. subtilis. Plenty of work was done on applications of pharmaceutical wastes as effective biosorbents for contaminant removal from wastewater [118–123]. For heavy metal removal, the wasteClitopilus 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 biomassAspergillus 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 ofStreptomyces fradiae,Micromonospora pururea, andNocardia 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., andPenicillium 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 toCunninghamella 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 byCorynebacterium 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, 100–102, 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 theAspergillus 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 [105–108]. 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 ofAspergillus 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 [100–102, 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].


## 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, 100–102, 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 theAspergillus 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 [105–108]. 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 ofAspergillus 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 [100–102, 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 (Table2). 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 inAspergillus Fumigatus andAspergillus 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 ontoAspergillus 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].Table 2
Suggested biosorption mechanisms based on interacting functional groups.
Biosorbent
Sorbate
Functional group
Mechanism
Reference
Orange peel
Pb(II)Cu(II) Cd(II)
Carboxylic
IEX/H-bonding
[101]
Orange waste
Cr(III)
Carboxyl/hydroxyl
Chemisorption
[102]
Orange waste
Cd(II)
Carboxyl/hydroxyl
—
[94]
Orange waste
Cd(II)Zn(II)Cr(III)
Mainly carboxyl
—
[95]
Desiccated coconut
Hg(II)
Hydroxyl/carboxyl/amine
Chelation
[100]
Pecan nut shells(C. illinoinensis) biomass
Acid BlueReactive Blue Acid Blue
Sulfonyl
—
[132]
Cupuassu shell,Theobroma  grandiflorum, (CS)
Reactive red dyeDirect blue
Hydroxyl/carboxylic
IEX
[87]
Mango seeds (MS)Mangifera  indica  L.
Victazol orange
Sulfonyl
—
[99]
Okra food industrial waste
Cd(II)Fe(II)Zn((II)
Hydroxyl/carbonyl/amide
IEX/complexation
[88]
Sugar industrial waste (bagasse waste)
Cd(II)Fe(II)
Hydroxyl/carbonyl/amide
IEX/complexation
[89]
Pineapple peel
MB dye
Hydroxyl/carboxyl/amine
—
[91]
Olive pomace
Pb(II)Cu(II) Cd(II)
Carboxylic/phenolic
Surface complexation
[108]
Olive mill stone
Pb(II)
Carboxylic
IEX
[102]
Palm oil mill effluent (POME) sludge
Methylene Blue
Carboxylic
—
[111]
Wine processing sludge
Ni(II)
Amino/carboxyl
Physical adsorption/chemical complexation
[76]
Spent waste beer yeast
Saccharomyces  cerevisiae
Pb(II)
Amine/carboxylic/phosphates/sulfhydryl
IEX/complexation
[82]
Grape bagasse waste residue
Cd(II)Pb(II)
Carbonyl/hydroxyl
—
[79]
Phaseolus vulgaris biomass
Pb(II)
Amino/hydroxyl
—
[84]
Activated carbon from antibiotic waste
Hg(II)
Hydroxyl/carbonyl
Complexation
[126]
Nonliving biomassAspergillus  awamori
Cr(VI)
Amine
—
[124]
Nonliving biomassAspergillus  Fumigatus
Cd (II)perse    mixtureCu(II)Cd(II)Co(II)Ni(II)
Hydroxyl/amine
Complexation
[122]
Fennel biomass (Foeniculum vulgare)
Cd(II)
Carboxylic/phenolic
IEX*
[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 ontoTolypocladium 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. Table3 [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].Table 3
Main adsorption isotherm models involved in the present study.
Adsorption isotherm model
Model parameters
Freundlich
q
=
K
F
C
1
/
n   Linear form
log
⁡
q
=
log
⁡
K
F
+
⁡
1
n
log
⁡
C
K
F: Freundlich isotherm constant that indicates adsorption capacity (mg/g) (
L
/
mg
)
n
n: measure of adsorption intensity or surface heterogeneity (dimensionless)
q: amount adsorbed at equilibrium, mg/g
C: adsorbate concentration at equilibrium, mg/L
Langmuir
q
=
q
m
K
L
C
1
+
K
L
C   Linear form
1
q
=
1
q
m
K
L
C
+
1
q
m
q
m: maximum binding capacity, mg/g
K
L: Langmuir binding (adsorption) constant, L/mg
Sips
q
=
q
m
(
K
s
C
)
1
/
n
1
+
(
K
s
C
)
1
/
n
q
=
k
s
C
β
s
1
+
a
s
C
β
s
K
s: Sips binding (adsorption) constant, (
L
/
mg
)
n
n: dimensionless exponent constant
β
s = Sips sorption exponent
a
s = Sips sorption constant (L/mg)
Dubinin-Astakhov
q
=
q
m
exp
⁡
(
-
R
T
ln
⁡
(
C
s
/
C
)
E
)
n
E: mean free energy of adsorption, KJ/mol
n: Dubinin-Astakhov dimensionless exponent
T: temperature, K
R: universal gas constant, KJ/mol·K
BET
q
=
q
m
C
BET
C
(
C
s
-
C
)
[
1
+
(
C
BET
-
1
)
(
C
/
C
s
)
]   Linear form
C
q
(
C
s
-
C
)
=
1
q
m
C
BET
+
(
C
BET
-
1
)
q
m
C
BET
·
C
C
s  Alternative form
q
=
q
m
b
s
C
(
1
-
b
L
C
)
(
1
-
b
L
C
+
b
s
C
)
C
BET: BET isotherm constant which indicates energy of surface interaction, L/mg
C
s: saturation concentration of adsorbate, mg/L
b
s: isotherm constant for BET adsorption in the first layer, L/mg
b
L: isotherm constant for BET adsorption in upper layers, mg/LTable 4
Equations of kinetic models involved in the current study.
Kinetic  Model
Model Parameters
Pseudo-first order
d
q
t
d
t
=
k
1
(
q
-
q
t
)  Linear Form
log
⁡
(
q
-
q
t
)
⁡
=
log
⁡
q
-
⁡
k
1
2.303
t
k
1: rate constant of pseudo-first order model, min−1
q: amount adsorbed at equilibrium, mg/g
q
t: amount adsorbed at time t, mg/g
Pseudo-second order
d
q
t
d
t
=
k
2
(
q
-
q
t
)
2  Linear Form
t
q
t
=
1
k
2
q
2
+
1
q
t
k
2: rate constant of pseudo-second order model, g/mg·min
Elovich
q
t
=
1
β
ln
⁡
(
α
·
β
)
+
1
β
ln
⁡
t
α: initial adsorption rate, mmol/g·min
β: Elovich constant, related to extent of surface coverage and activation energy, g/mmolTable5 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].Table 5
Equilibrium parameters as predicted by the well-established sorption models.
Biosorbent
Target ion/compound
Equilibrium model
Maximum sorption capacity (mg/g)
Sorption constant*
pH/temperature (°C)
Reference
Local dairy sludge
Pb(II)Cd(II)
Langmuir
178.669.90
0.030.05
5/40
[129]
Baker’s yeast biomass
Cd(II)Pb(II)
Langmuir
31.7560.24
0.0920.066
6.0/305.0/30
[131]
Cider yeast
Patulin
Langmuir
0.0082
0.064
4.5/25
[117]
Beer yeast
Cu(II)Pb(II)
Langmuir
0.662.27
0.3140.259
5.0/20
[69]
Spent waste beer yeast
Saccharomyces  cerevisiae
Pb(II)
Freundlich
—
K
f
=
0.515
n
=
0.842
5.0/30
[82]
Spent brewery grains (SBG)
AG25 dye
Langmuir
212.76
0.036
3.0/30
[70]
Wine processing sludge
Ni(II)
Langmuir
3.91
0.113
5.5/50
[76]
Antibiotic wasteP. mutilus
Cu(II)
Langmuir
106.38
0.007
—
[119]
Antibiotic wasteP. mutilus
Basic Blue 41
LangmuirFreundlich
111.00
0.097
K
f
=
24.1
n
=
2.89
(8.0-9.0)/30
[119]
Phaseolus  vulgaris  L.
Acid Red 57 dye
Langmuir
215.13
—
2.0/20
[91]
Phaseolus  vulgaris  L.
Reactive Red 198
Freundlich
K
f
=
1.99
n
=
10.037
[86]
Fruit waste macrofungiFlammulina  velutipes
Cd(II)Pb(II)
Langmuir
8.4318.35
—
6.0/25
[130]
Industrial fungiPenicillium oxalicum var. Armeniaca
Cd(II)Pb(II)Hg(II)
Langmuir
35.9047.40269.3
0.051.010.07
5.0/20
[107]
Industrial fungi
Tolypocladium sp.
Cd(II)Pb(II)Hg(II)
Langmuir
11.9028.40161.0
1.030.610.50
5.0/20
[107]
industrial waste ofClitopilus  scyphoides
(Pleurotus  mutilus) fungal biomass
Cd(II)
BET
45.3
16
b
s
=
0.03
b
L
=
0.00
5.0/20
[120]
Fungal waste biomass
Simulated acid bath for wool (SABW) dye
Langmuir
289.5
0.0114
3.0/25
[121]
biomass of
Phaseolus  vulgaris  L.
Pb(II)
Langmuir
19.93
0.498
5.0/50
[84]
Fennel biomass (Foeniculum vulgare)
Cd(II)
LangmuirFreundlich
26.59
0.080
K
f
=
3.16
n
=
2.29
4.3/50
[123]
Nonliving biomassAspergillus  awamori
Cu(II)
Langmuir
35.97
0.136
5.0/20
[125]
Corynebacterium
glutamicum
Reactive Black 5RB5
LangmuirSips
419
0.042
k
s
=
108
a
s
=
0.171
1.0/35
[127]
Rhizopus oligosporus biomass
Cu(II)
Langmuir
79.37
0.282
5.0/30
[85]
Pectin-rich fruit wastes (lemon peels)
Cd(II)
Langmuir
22.32
0.015
5.0/—
[133]
Orange waste
Cd(II)
Sips
20.64
0.038 (n
=
1.21)
6.0/25
[94]
Orange waste
Cd(II)Zn(II)Cr(III)
Langmuir
17.6614.6122.50
0.0040.0670.372
4.0/20
[95]
Orange (Citrus sinensis)
Cr(III)
Langmuir
36.48
0.403
5.0/25
[102]
Pineapple peel, an agricultural effluent
Methylene Blue (MB) cationic dye
Langmuir
97.09
0.074
6.0/30
[91]
Peach stonesApricot stones
Pb(II)
Freundlich
—
K
f
=
0.64  (n
=
3.57)
K
f
=
0.636  (n
=
3.54)
7.0/—
[97]
Mangifera  indica (mango) seed kernel particles
Methylene Blue (MB) cationic dye
Langmuir
153.846
0.8227
8.0/50
[98]
Desiccated coconut
Hg(II)
Langmuir
500.00
—
7.4/30
[100]
Pecan nut shells (C. illinoinensis) biomass
Acid Blue 74 (AB74)
Langmuir
4.851
0.001
6.5/30
[132]
Reactive Blue 4 (RB4)
Langmuir
13.410
0.001
Acid Blue 25 (AB25)
Sips
7.576
K
s
=
0.0014  (n
=
0.98)
Crushed olive stone wastes
Pb(II)Ni(II)Cu(II)Cd(II)
Freundlich
—
—
5.5/20
[105]
Binary mixtures
Extended Langmuir
Olive pomace
Cu(II)Cd(II)Pb(II)
Langmuir
1.942.986.23
0.1380.0461.829
5.0/60
[108]
Olive pomace
Phenols
Freudlich
—
K
f
=
0.267
n
=
1.75
10.0/20
[110]
Pomace from olive oil
Cr(IV)
Langmuir
18.69
0.055
2.0/60
[101]
olive mill residues (OMR)
Cu(II)
Langmuir
13.50
0.080
5.0/23
[104]
Solid olive stone
Pb(II)
Sips
6.57
K
s
=
0.057
5.0/25
[102]
Olive oil mill
Pb(II)
Dubinin-Astakhov
23.69
5.0/25
[103]
Palm oil mill effluent (POME) sludge
Methylene Blue (MB) cationic dye
Langmuir
23.50
0.208
7.6/27
[111]
Sugarcane bagasse waste
Methylene Blue (MB)
Langmuir
202.43
0.031
8.0/25
[78]
Gentian Violet (GV)
327.83
0.047
Fresh malted sorghum mash waste
Methylene Blue (MB) basic dye
Langmuir
384.6
0.011
7.0/53
[83]
Cupuassu shell, Theobroma  grandiflorum, (CS)
Reactive Red dye (RR 194)
Sips
64.1
K
s
=
0.214  (n
=
0.89)
2.0/25
[87]
Direct Blue 53
37.5
K
s
=
1.560  (n
=
0.55)
Activated carbon derived from exhausted olive waste cake
Lanaset Grey G
Langmuir
108.70
0.031
6.0/25
[113]
Activated carbon derived from empty fruit bunch (EFB)
Methylene Blue dye (MB)
Langmuir
344.83
0.060
—/30
[114]
Activated carbon from sago waste
Pb(II)
Langmuir
14.35
0.095
3.5/27
[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 (Table6). 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.Table 6
Kinetic parameters as predicted by the well-established sorption models.
Biosorbent
Target ion/compound
Kinetic model
q (mg/g)
Rate constant*
pH/temperature (°C)/time (min)
Co (mg/L)
Reference
Local dairy sludge
Pb(II)Cd(II)
Pseudo-second order
117.644.4
0.274.2
5.0/20°C/500
200100
[129]
Wine processing sludge
Cr(VI)
Pseudo-second order
2.42
0.070
4.2/50/240
100
[73]
Wine processing sludge
Ni(II)
Pseudo-second order
3.11
0.226
5.5/50/120
45
[76]
Desiccated coconut
Hg(II)
Pseudo-second order
447.03
—
7.4/30/60
50
[100]
Pecan nut shells (C. illinoinensis) biomass
Acid Blue 74 (AB74)
Pseudo-first
3.271
0.02
6.5/30/500
1000
[132]
Reactive Blue 4 (RB4)
Pseudo-second
10.010
4.35
*
10
-
4
6.5/30/1000
Acid Blue 25 (AB25)
Pseudo-second-order
4.892
7.15
*
10
-
3
6.5/30/500
Spent brewery grains
AG25 dye
Pseudo-second order
74.63
0.038
3.0/30/75
90
[70]
Beer brewery diatomite waste (SDE)
Methylene Blue basic dye
Pseudo-second order
4.92
1.24
7.0/25/1440
2.5
[81]
Antibiotic wasteP. mutilus
Basic Blue 41
Pseudo-second order
90.91
0.0042
8.0-9.0/30/60
70
[119]
Macrofungal waste from antibiotics
Cd(II)
Pseudo-second order
82.8
0.0014
5.0/20/15
200
[120]
Fennel biomass (Foeniculum  vulgare)
Cd(II)
Pseudo-second order
9.30
0.476
5.0/30/50
100
[123]
Phaseolus  vulgaris  L.
Reactive Red 198
Pseudo-second order
81.97
0.036
2.0/20/20
—
[86]
Nonliving biomassAspergillus  awamori
Cu(II)
Pseudo-first order
35.00
0.077
5.0/20/180
25
[125]
Corynebacterium
glutamicum
Reactive Black 5RB5
Pseudo-second order
370.00
9.4
*
10
-
5
1.0/25/500
2000
[127]
Phaseolus  vulgaris  L.
Acid Red 57 dye
Pseudo-second order
89.49
0.21
2.0/20/20
150
[91]
Fruit waste macrofungiFlammulina  velutipes
Cd(II)
Pseudo-first
[130]
Pb(II)
Pseudo-second order
13.04
2.17
6.0/25/60
10
Orange (Citrus sinensis)
Cr(III)
Pseudo-second order
10.97
0.002
5.0/25/4320
100
[102]
Pectin-rich fruit wastes (lemon peels)
Cd(II)
Pseudo-second order
13.92
0.021
5.0/—/50
19.2
[133]
Orange waste
Cd(II)
Elovich
333.33 (1/α)
0.004 (1/β)
6.0/25/60
100
[94]
Mangifera  indica (mango) seed kernel particles
Methylene Blue (MB) cationic dye
Pseudo-first order
115
0.0461
8.0/30/120
175
[98]
Rhizopus oligosporus biomass
Cu(II)
Pseudo-second order
69.82
0.002
5.0/30/120
100
[85]
Crushed olive stone wastes
Pb(II)
Pseudo-secondorder
1.12
0.141
5.5/20/60
18.86
[105]
Ni(II)
0.25
3.000
4.48
Cu(II)
0.26
7.497
4.35
Cd(II)
0.72
0.121
10.56
Olive stones
Cd(II)
Pseudo-second order
0.903
3.196
11.0/80/20
10
[106]
Palm oil mill effluent (POME) sludge
Methylene Blue (MB) cationic dye
Pseudo-second order
5.54
0.0072
7.6/27/4320
10
[111]
Olive pomace
Methylene Blue (MB)  dye
Pseudo-second order
—
0.0906
—/25/240
10
[109]
Tea industry waste
Cd(II)
Pseudo-second order
10.6
0.02
7.0/25/180
100
[72]
Pineapple peel, an agricultural effluent
Methylene Blue (MB) cationic dye
Pseudo-second order
104.17
0.22
×
10
-
3
6.0/30/400
300
[91]
Okra food waste
Cd(II)Fe(II)Zn(II)
Pseudo-second order
17.5420.4214.99
0.0090.0080.013
—/20/90
20
[88]
Activated carbon derived from exhausted olive waste cake
Lanaset Grey G
Pseudo-first order
106.4
0.0019
6.0/25/3000
150
[113]
Activated carbon from tea industry waste (TIWAC)
Cr(III)
Pseudo-second order
0.464
1.52
6.0/—/30
0.01
[115]
Sugar industry (waste bagasse)
Cd(II)Fe(II)
Pseudo-first order
—
9.3
*
10
-
5
7.2
*
10
-
5
—/20/90
20
[89]
Sugarcane bagasse waste
Methylene Blue (MB)
Pseudo-secondorder
192.31
0.0012
8.0/25/600
200
[78]
Gentian Violet
357.14
0.00005
8.0/25/900
300
*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 thePenicillium 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 ofAspergillus 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 ofCorynebacterium 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, 103–105, 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 ontoAspergillus 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.



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*Source: 146769-2014-07-07.xml*