Abstract

In this study, the sawdust waste biomass was used as an eco-friendly biosorbent material for the bioremediation of manganese pollution in aqueous environment. The effects of various environmental variables such as pH, biosorbent amount, metal concentration and contact time on the manganese biosorption were studied in batch operating conditions. The kinetic and equilibrium studies were performed to elucidate the biosorption behavior of biosorbent material. The biosorption capacity of biosorbent was strongly influenced by the operating parameters. The experimental data were more successfully modeled by the pseudo-second-order kinetic model and Langmuir isotherm model compared to other models applied in the study. The maximum manganese removal capacity of biosorbent was found to be 25.655 mg g-1. These findings showed that the sawdust waste biomass can be used as an eco-friendly biosorbent material for the bioremediation of manganese pollution in aqueous environment.

References

[1] Robinson-Lora MA, Brennan RA. Biosorption of manganese onto chitin and associated proteins duringthe treatment of mine impacted water. Chem Eng J. 2010; 162: 565-572.
[2] Abu Hasan H, Sheikh Abdullah SR, Tan Kofli N, Yeoh SJ. Interaction of environmental factors onsimultaneous biosorption of lead and manganese ions by locally isolated Bacillus cereus. J Ind Eng Chem.2016; 37: 295-305.
[3] Gialamouidis D, Mitrakas M, Liakopoulou-Kyriakides M. Equilibrium, thermodynamic and kineticstudies on biosorption of Mn(II) from aqueous solution by Pseudomonas sp., Staphylococcus xylosus andBlakeslea trispora cells. J Hazard Mater. 2010; 182: 672-680.
[4] Ozdemir S, Kilinc E, Poli A, Nicolaus B, Guven K. Biosorption of Cd, Cu, Ni, Mn and Zn from aqueoussolutions by thermophilic bacteria, Geobacillus toebii sub.sp. decanicus and Geobacillus thermoleovoranssub.sp. stromboliensis: Equilibrium, kinetic and thermodynamic studies. Chem Eng J. 2009; 152: 195-206.
[5] Idris SAM. Adsorption, kinetic and thermodynamic studies for manganese extraction from aqueousmedium using mesoporous silica. J Colloid Interface Sci. 2015; 440: 84-90.
[6] Abdeen Z, Mohammad SG, Mahmoud MS. Adsorption of Mn (II) ion on polyvinyl alcohol/chitosan dryblending from aqueous solution. Environ Nanotechnol Monit Manage. 2015; 3: 1-9.
[7] Khobragade MU, Pal A. Investigation on the adsorption of Mn(II) on surfactant-modified alumina: Batchand column studies. J Environ Chem Eng. 2014; 2: 2295-2305.
[8] Lagergren S. About the theory of so-called adsorptıon of soluble substances. K Sven VetenskapsakadHandl. 1898; 24: 1-39.
[9] Ho YS. Review of second-order models for adsorption systems. J Hazard Mater. 2006; 136: 681-689.
[10] Chien S, Clayton W. Application of Elovich equation to the kinetics of phosphate release and sorptionin soils. Soil Sci Soc Am J. 1980; 44: 265-268.
[11] Weber WJ, Morris JC. Kinetics of adsorption on carbon from solution. J Sanit Eng Div Am Soc CivEng. 1963; 89: 31-60.
[12] Akbari M, Hallajisani A, Keshtkar AR, Shahbeig H, Ali Ghorbanian S. Equilibrium and kinetic studyand modeling of Cu(II) and Co(II) synergistic biosorption from Cu(II)-Co(II) single and binary mixtures onbrown algae C. indica. J Environ Chem Eng. 2015; 3: 140-149.
[13] Freundlich HMF. Over the adsorption in solution. Z Phys Chem. 1906; 57: 385-470.
[14] Langmuir I. The adsorption of gases on plane surfaces of glass, mica and platinum. J Am Chem Soc.1918; 40: 1361-1403.
[15] Dubinin MM, Radushkevich LV. Equation of the characteristic curve of activated charcoal. Proc AcadSci Phys Chem Sec USSR. 1947; 55: 331-333.
[16] Foo KY, Hameed BH. Insights into the modeling of adsorption isotherm systems. Chem Eng J. 2010;156: 2-10.