- Open Access
Adsorptive treatment of brewery effluent using activated Chrysophyllum albidium seed shell carbon
© Menkiti et al.; licensee Springer. 2014
- Received: 17 January 2014
- Accepted: 25 March 2014
- Published: 30 April 2014
Chrysophyllum albidium seed shell, an abundant, biodegradable and inexpensive natural resource was used as a precursor to bioadsorbent production for the removal of suspended and dissolved particles (SDP) from initially coagulated Brewery Effluent (BRE). Influence of key parameters such as contact time, bioadsorbent dose, pH and temperature were investigated using batch mode. The thermal behavior studies were evaluated using Thermogravimetric and Differential scanning calorimetric analyses. The morphological observations and functional groups of the bioadsorbents were determined using scanning electron microscopy and Fourier transform infrared spectroscopy, respectively. The adsorption equilibrium, thermodynamics and kinetic of SDP adsorption on H3PO4-treated shell and NH4Cl-treated shell were examined at specified temperatures. Equilibrium data sufficiently fitted the Langmuir isotherm model (R2 > 0.99; SSE < 0.09). The pseudo-second order kinetic model provided the best correlation (R2 > 0.99; SSE < 0.14) with the experimental data. The values of ΔG° and ΔH° indicated the spontaneous and endothermic nature of the process. This study demonstrated that C. albidium seed shell could be utilized as low cost, renewable, ecofriendly bioadsorbent for the uptake of SDP from BRE.
- Brewery effluent
- Chrysophyllum albidium
- Adsorption isotherms
- Suspended and dissolved particles
Brewing is an intensive water consuming activity, besides utilizing a wide variety of chemicals. Expectedly, large volumes of effluent is discharged into water courses of brewery bearing communities, leaving in its wake a polluted aquifer (Khuo-Omoregbe et al. 2005; Menkiti 2010). Increasing concentration of these organic/non-organic enriched BRE in the water constitute a severe health hazard to both plants and animals, thus impeding the functionality of the ecosystem. The situation is typical of the BRE receiving aquatic system in Nigeria, where much of the water resources cannot be utilized without a form of treatment, following effluent discharges with negligible consideration for environmental control (Menkiti and Onukwuli 2011a).
BRE, generated from lager beer production, contains large amount of SDP (Menkiti and Onukwuli 2010). Typically, the organic contents of BRE consists of sugars, soluble starch, ethanol, volatile fatty acids and solids which are mainly spent grains, yeast and trub (Driessen and Vereijken 2003). Untreated BRE quantitatively contains suspended solids (100–1500 mg/l), chemical oxygen demand (300–800 mg/l), nitrogen (30–100 mg/l) and phosphorus (10–30 mg/l) (Menkiti et al.2011a World Bank Group 1998).
Over the years, significant attention has been given to the environmental cleanup of such contaminated aqua system using varieties of techniques such as precipitation, ion-exchange, coagulation, reverse osmosis and adsorption (Hameed and El-Khaiary 2008; Larous et al.2005; Menkiti et al.2011b; Menkiti and Onukwuli 2011b). Among the different treatments listed above, adsorption technology is attractive due to its merits of efficiency,even at low concentration of contaminants (Meena et al. 2008; Yakubu et al. 2008), economy, simple operation and insensitivity to toxic substances (Grini 2005; Feng et al.2010; Menkiti and Onukwuli 2011b).
The common adsorbents primarily include zeolite, clays, polymeric materials and natural agricultural materials which provided the focus of this study (Asasian and Kaghazchi 2013; Jiang et al.2012; Amirnia et al.2012). These natural materials have potential to be used as low cost bioadsorbent, as they represent unused resources, abundantly available and known to be eco-friendly (Deans and Dioxn 1992). Progressively, much attention has been focused on techniques of converting these waste materials into useful adsorbents. Among these agricultural wastes are saw dust (Meena et al. 2008) palm ash (Ahmad et al.2007).
Chrysophylum albidium seed shell, considered in this study, is of tropical forest tree of genus chrysophyllum, family of sapotaca e and order of ericales. The fruit is large berry containing 4 to 5 flattened seeds with a hard shell (Bada 1997). Significant quantities of these seeds shells are produced annually in Nigeria without being put to useful ends industrially. However, successful application of adsorbent from C. albidium seed shells for the removal of heavy metals had been reported (Oboh et al.2009; Onwu and Ogah 2010; Ejikeme et al.2011). According to the author’s knowledge, no attempt has been made until now to use this seed shell for the treatment of natural organic aqueous waste, such as BRE. Therefore, it was of interest to experiment with such a promising biomaterial for the adsorptive removal of SDP from initially coagulated BRE by batch technique. The work further seeks to investigate the influence of contact time, adsorbent dosage, temperature and effluent pH on the adsorptive uptake of SDP from the BRE. Also, the research investigated the ability of three isotherm models: namely the Langmuir, the Freundlich and the Temkin adsorption isotherms to model the equilibrium adsorption data. Another major focus of the work was the kinetic study, conducted to determine the rate of SDP adsorption and evaluation of which of the four kinetic models (pseudo-first order, pseudo-second order, Elovich and Bhattacharya-Venkobachar) that best describes the adsorption process. Finally, material characterization and thermodynamic analyses were conducted to present the characteristic properties and energy changes associated with the adsorption study.
Brewery effluent was obtained from a beer brewery at 9th Mile Corner Udi, Enugu Sate Nigeria and stored in black plastic container to preserve and further prevent changes in the characteristics of the effluent (Clesceri et al.1999).
C. Albidium seed shells
The precursor for the preparation of the bioadsorbents, C. albidium seed shells was obtained as a waste material from Nsugbe, Anambra State of Nigeria. Pretreatment of the shells by thorough washing with distilled water to remove the impurities was done and the washed sample dried in an air circulating oven at 40°C for 14 hours. The shell samples were blended, sieved and particles that ranged between 2 and 3 mm were obtained and stored in a desiccator for use in the experiments.
Two portions of the shell samples, of known weights, were immersed in 60% solutions of ammonium chloride and phosphoric acid, respectively, for 24 hours. The carbonization of the shell samples were carried out in a muffle furnace at 600°C for 4 hours, washed with distilled water to pH 7, dried at 110°C for 8 hours and subsequently sieved to desired diameter using standard sieves.
Standard APHA methods, as reported by Clesceri et al. (1999), were applied to determine the physiochemical and biological characteristics of the effluent.
Characteristics of ASAA and ASAS
BET Surface area (m2/g)
Total pore volume (cm3)
Bulk density (g/cm3)
% Ash content
Oil content (%)
Moisture content (%)
Tapped bulk density
where: w is weight of the dry material and v is volume of the dry material.
Percentage ash content
where: Wash is weight of ash and Wsample is weight of bioadsorbent sample.
Percentage moisture content
where: Wsample is the weight of bioadsorbent sample before drying, Wdry is weight of sample after drying.
where: Vpore is pore volume of the bioadsorbent and W inc is weight increase of the bioadsorbent and ρ water is the density of water.
Surface area was determined according to the modified methods of Kang et al. 2013. It was calculated from nitrogen gas adsorption isotherms based on Brunauer, Emmet and Teller (BET) method of surface area analysis (at 77.305 K) using Quantachrome 2.0 analyzer.
Physiochemical and instrumental characterization of bioadsorbent samples
Fourier transfer infrared analysis was carried out using Shimadzu FTIR 8400S spectrophotometer for the determination of functional groups present in ASAA and ASAS. The thermal behavior of the activated carbon was evaluated by thermogravimetric and differential scanning calorimetric analyses using TGA-Q 50 and DSC-Q 200 models, respectively. The surface morphology of the activated carbon was visualized via scanning electron microscopy (SEM) using a scanning electroscope model FEI-QUANTA 200. Physiochemical and instrumental characterization of the bioadsorbents were conducted using standard methods (Feng et al. 2010).
Batch adsorption experiments were performed in Erlenmeyer flask according to the methods reported by Sivakumar and Palanisamy (2009) and Yeddou and Bensmaili (2005). In a typical experiment, 20 ml of effluent sample was mixed with the appropriate amount of adsorbents (types ASAA and ASAS) in the range of 10-50 g/l and then shaken for a period of time ranging from 5 to 60 min at 20 rev/s. The temperatures of adsorption measurements ranged between 20 and 30°C and the appropriate value was applied accordingly as required. The sample was then filtered using Whatman no 42 filter paper having fine porosity and particle retention of 2.5 micrometer at slow flow rate in a glass funnel. The filtered liquid was analyzed with respect to particle (SDP) content.
where: C 0 , C t and D A are initial constant effluent concentration (mg/l), effluent concentration at any time, t and adsorbent dose (g/l), respectively.
Characterization of results
Physiochemical and biological characteristics
Characterization result of Brewery Effluent and FEPA standard
Total hardness (mg/l)
The FTIR spectra of ASAA and ASAS are depicted in Figure 1b and c, respectively. For both figures, discernable peaks of note were recorded at 3991.82-3162.40 cm−1(O-H stretch/phenols), 3456.55 cm−1(O-H broad stretch/N-H medium stretch), 3060.17-2830.63 cm−1(O-H broad stretch), 1596.15-1595.16 cm−1(NO2 asymmetrical stretch), 1412.90 cm−1(C-H scissoring/bending), 1225.80 cm−1(C – N stretch/C-O stretch), 1220.98 cm−1(C-H/C-O stretches), 1100.43 cm−1(C-N/C-O stretches) and 814.95-819.77 cm−1 (C-H stretch bend).
The FTIR spectra of used adsorbents showed (Figures are not shown) discernable peaks (in cm−1) for used ASAA at 461(S-stretching), 803(C-H stretch/NH2 wagging and twisting), 1084.03 (second overtone N-H and O-H stretching), 1419.66 (first overtone N-H and O-H stretching), 1608.69(pyridine C-N),3443.05 (primary NH2 asymmetric stretching), and for used ASAA at 389 (aliphatic P compound), 469 (S-stretching), 880.53/1101.39(aromatic P-O stretching), 1450.52/1573.97(C = C stretching), 3458.48(primary NH2),3633.05(O-H stretching).
The FTIR results of bioadsorbent precursor (Figure 1a), ASAA (Figure 1b), ASAS (Figure 1c) and used adsorbents indicated that some peaks were shifted or disappeared, and that new peaks were also detected. These changes observed in the spectra represent interactive effects due to involvement of those functional groups during production and use of the adsorbents. The changes observed in the peaks of the adsorbents after usage could be concluded to be the direct result of adsorptive uptake of SDP from the BRE by the adsorbents. The varying number of absorption peaks displayed by the samples reflected the complex nature of these materials (Hameed and El-Khaiary 2008; Chemistry Department at Colorado University CDCU 2002; Graham et al.2008).
DSC and TGA
As indicated in Figures 2a and 3a, DSC was used to characterize the phase transition that occurred in ASAA and ASAS over the temperature range of 25-277°C. Figure 2a revealed a sharp thermal transition in the temperature range of 125-150°C with transition enthalpy of 250 kJ/kg. Figure 3a indicated sharp transition in the temperature range of 112.5-138°C with transition enthalpy of 819.9 kJ/kg. This behavior by both ASAA and ASAS could be attributed to the de-stringing and coiling of carbon chain leading to spontaneous densification (Ramani et al.2012). The densification of the aggregated mass occurred at 175-180°C and 150-175°C for ASAA (Figure 2a) and ASAS (Figure 3a), respectively without absorption of thermal energy. In other words, the heat flow discs indicated exothermicity.
The thermal decomposition behaviors of the bioadsorbents are illustrated in Figures 2b and 3b for ASAA and ASAS, respectively. Figure 2b shows that ASAA lost weight by 11.17% and 15.18% at 120.63°C and 562.65°C, respectively. For Figure 3b, the weight loss of 10.75, 15.63 and 19.65% were recorded for 135.04, 517.16 and 649.84°C, respectively. For both Figures 2b and 3b, the initial weight loss could be attributed to the internal moisture and gaseous loss from the matrix molecules of the adsorbents (Ramani et al.2012). The second phase weight loss may be attributed to the decomposition of the labile component in the adsorbent. The results presented in Figures 2 and 3 conclusively suggested operational stability of the adsorbents.
Influence of contact time and adsorbent dosage on adsorptive removal of SDP from BRE
The observed adsorption dynamic profiles depicted by Figures 5 and 6 can be divided into three regimes (Ncibi et al.2008): (i) a linear increase in adsorption with time, (ii) a transition regime where the rate of adsorption levels off, and (iii) a plateau regime. First regime (initial steep slope) indicated instantaneous adsorption (overshoot phenomena) ability of effluent particles onto the surface of the adsorbents. The second regime indicated a phase of gradual attainment of equilibrium where the apparent fall in SDP adsorption rate might be due to utilization of active sites on adsorbents surface. Plateau regime indicated phase where equilibrium had been achieved (Mohan et al.2007).
One general phenomenon was the perceived increase in SDP uptake with increase in adsorbent dose. It should also be observed that the % Rem for doses considered in Figures 5 and 6 ranged closely; with only apparent difference noticed for 50 g/l (Figure 5). This could be attributed to the greater availability of close number of exchangeable sites or surfaces in the adsorbents (Meena et al.2008). Following optimal results obtained at 50 g/l and 30 min, the rest of the work was carried out at the stated results, unless otherwise indicated.
Figures 7 and 8, present results similar to Figures 5 and 6 in respect of the variation of adsorption capacity q t (mg/g) with contact time and adsorbent dose. It was evident that q t increases with decreasing adsorbent dose and increasing contact time before leveling-off. The highest and lowest q t were recorded at 10 and 50 g/l, respectively for both ASAA (Figure 7) and ASAS (Figure 8). In specific terms, q t at 10 g/l increased from 9.812 to11.308 mg/g for 5 and (30–60) min, respectively as shown in Figure 7. Also, the q t at 50 g/l ASAA increased from 2.0504 to 2.4002 mg/g for 5 and (30–60) min, respectively. Figure 8 indicated that qt at 10 mg/l recorded increment from 8.4920 to 10.703 mg/g for 5 and (30–60) min, respectively while that of 50 g/l increased from 1.7842 to 2.1868 mg/g for 5 and (30–60) min, respectively. The results indicated also that the ASAA performed better than ASAS.
The apparent decrease in adsorption density (amount adsorbed per unit mass of the adsorbent) with increase in adsorbent dose was due to progressive unsaturation of adsorption sites through the adsorption reaction. Another reason might be due to the particle interaction, such as aggregation, usually resulting from high adsorbent concentration. Such aggregation would lead to decrease in total surface area of the adsorbent and on increase in the diffusional path length (Shukla et al.2002). Particle interaction might also desorb some of the adsorbate that was only loosely and reversibly bound to the adsorbent surface.
Influence of temperature on the adsorptive removal of SDP from BRE
Both Figures 9 and 10 indicated that the retention of SDP by the adsorbents increased while the temperature and time increased. The perceived increase of SDP uptake with temperature might be due to the acceleration of some originally slow adsorption steps or the creation of some active sites on the adsorbent surface (Hashem 2007; Nasssar and Magdy 1999). The enhanced mobility of SDP from the bulk solutions towards the adsorbent surface should also be taken into account (Hashem 2007; Yubin et al.1998). Increased temperature encouraged the process of agglomeration and widening adsorbent pore resulting in certain activation of the surface of the solid support (Larous et al.2005). Obtained results indicated clearly that the adsorption process under study was an endothermic process. This fact was illustrated in Section 3.6. Results similar to the one of this study had been reported by Khalid and Ahmad (1998).
Influence of pH on the adsorptive removal of SDP from BRE
In quantitative terms, the percentage SDP removal increased with pH from 2 to about 6.95 and remained unchanged thereafter. In respect of ASAA and ASAS, the SDP removal increased from 69.5768% at pH 2 to 73.0839% at pH 6.95 and 66.3161% at pH 2 to 70.4231% at pH 6.95, respectively. At pH greater than 6.95, the SDP removal remained constant till pH 8. The gentle decrease at about pH 3–6 of the initial rapid adsorption of SDP was presumed to be due to competitive adsorption between hydrogen ion and particles of the BRE. The adsorption at near neutral pH values could be attributed to the cellulose component of adsorbents where site binding adsorption might be occurring. This could be due to surface complex phenomena of functional groups present in the adsorbent (Hashem 2007; Menkiti et al. 2011a).
Graphical results of Figure 11 could be linked strongly to the influence of pH, in addition to the functional groups on the adsorbent and their ionic state at a particular pH (Mohan et al.2007; Genc et al. 2003). Equally, the apparent increment in adsorption with pH was believed to result from corresponding increase in the number of negatively charged sites. Consequently, the electrostatic attraction between the negative surface and the cationic BRE molecules increased with pH and reached saturation at about pH 6.95. Sivakumar and Palanisamy (2009) and Noroozi et al. (2007)) had reported similar results for the adsorption of basic red 29 onto Euphorbia antiquorum L and BR 41 onto silkworm pupa, respectively.
Equilibrium isothermic analysis
The study of the adsorption isotherm is fundamental (Gräf et al. 2012), and played an important role in determination of the maximal capacity of adsorption, in addition to development of an equation which accurately represented the results that could be used for design purposes. Three equilibrium isotherms were analyzed: Langmuir, Freundlich and Temkin.
The Langmuir isotherm is arguably the best known of all isotherms describing adsorption. It applies to the cases of adsorption on completely homogenous surfaces where interactions between adsorbed molecules are negligible. The Freundlich isotherm is the earliest known relationship describing the adsorption isotherm. This empirical isotherm applies fairly well when describing the adsorption in dilute aqueous solution systems. Temkin isotherm applies on the bases that a fall in heat of sorption is linear rather than logarithmic as obtained in Freundlich equation. Heat of sorption of all molecules in the layer would decrease linearly with coverage due to sorbate- sorbent interactions (Larous et al.2005; Sujatha et al.2008).
Isotherm mathematical model equations used for adsorption data analysis
Isotherm parameters obtained from SDP adsorption on ASAA and ASAS at pH of 6.95, DA=50g/l, C 0 = 161.92 mg/l
R L indicates the shape of the isotherm. This is: (i) unfavorable when R L > 1, (ii) linear when R L = 1 (iii) favorable when 0 < R L < 1, and (iv) irreversible when R L = 0. The calculated R L values for the two adsorbents, shown in Table 4 were all in the range of 0–1, which confirmed that adsorption process was favorable within the studied experimental conditions.
In respect of Freundlich isotherm, favorability of the process is achieved if n lies in range of 1–10. Based on the values of Freundlich constant (n) displayed in Table 4, the present adsorption system could be considered favorable since n values lie between 1and 10 for all cases studied.
Thermodynamic analyses of adsorption isotherm data
Thermodynamic parameters for SDP on ASAA and ASAS
Table 5 shows that ΔG˚ values were increasingly negative with temperature, which indicated the increasing feasibility and spontaneity of the adsorption process. The adsorption of SDP onto ASAA was greater than that of SDP onto ASAS overall. Also, from Table 5, the values of ΔS˚ are increasingly positive with temperature, an indication of increasing randomness of solid–liquid interface with increasing temperature (Debnath and Ghosh 2008). From the table, the values of ΔH° recorded for ASAA and ASAS are 3.493 kJ/mole and 2.477 kJ/mole, respectively. The values are found to be less than 40 kJ/mole which indicated that physisorption dominated the adsorption of SDP onto ASAA and ASAS. The present results are found to follow similar trend with the results reported by Patel and Suresh (2008) on the biosorption of reactive black 5 dyes by Aspergillus foetidus.
Surface packing, surface charge and hopping number
where: C o and C e are initial and equilibrium concentrations in mg/cm3, Γ is the adsorption density in mg/m2, Z = 4 is the valency of organic carbon, which is a major constitutent (Driessen and Vereijken 2003; Kanagachandran and Jayaratne 2006; Janhom et al. 2009; Menkiti 2010) of SDP in the BRE, r = 0.70 ×10- 9 m is the effective radius of the organic carbon enriched-SDP reported elsewhere (Crystalmarker 2014; United States Environmental Protection Agency USEPA 1999), R is gas constant, and T is the absolute temperature (K).
Adsorption kinetic analysis
Kinetic and equilibrium data are pertinent in the evaluation of adsorption dynamics and by extension, the optimization of residence time for the uptake of SDP on ASAA and ASAS. Adsorption kinetics could be controlled by several independent processes (bulk diffusion, film diffusion, chemical reaction, intra-particle diffusion, temperature, pH, etc.) that could act in series or in parallel (Abia and Asuquo 2006). In order to investigate the kinetic of BRE adsorption on ASAA and ASAS, the data obtained at 30°C have been analyzed by pseudo first order(PFO) (Langergren 1898, Eq. Nineteen), pseudo second order(PSO) (Ho and Mckays 1999, Eq. Twenty); Elovich (Chien and Clayton 1980, Eq. Twenty-one) and Bhattacharya – Venkobachar (BVM) (Bhattacharya and Venkobachar 1984, Equation Twenty-two) kinetic model equations and subsequently subjected to accuracy tests via R2 and SSE (Eq. 6).
The kinetic equations used for analysis of kinetic data
ln(q e − q t ) = ln q e − K1t
ln(q e − q t ) vs. Time
q t vs. Time
ln[1 − (U)T] = K B t
ln[1 − (U)T] vs. Time
Kinetic parameters of the adsorption process at 30°C ,pH 6.95, D A = 50 g/l , C 0 = 161.92 mg/l
African star apple shell biomass (ASAA and ASAS) was able to adsorb SDP from brewery effluent (BRE). The removal of SDP from BRE using ASAA and ASAS was a function of contact time, bioadsorbent dosage, temperature and pH. Adsorption capacity increased with increasing temperature. The optimum SDP removals were achieved at pH 6.95, 50 g/l dose and 30°C. Among the isotherm models considered, equilibrium data fitted the Langmuir model best within the studied experimental conditions. The kinetic data agreed very well with the pseudo-second order equation. The calculated thermodynamics parameters showed that the related adsorption systems were favorable, endothermic and spontaneous for both ASAA and ASAS.
The authors acknowledge the underlisted organizations for their assistance towards the completion of this work:
1. Chemical Engineering Department, Nnamdi Azikiwe University, Awka, Nigeria.
2. Scientific Equipment Development Institute, Enugu, Nigeria.
3. National Research Institute for Chemical Technology, Zaria, Nigeria.
4. Central Leather Research Institute, Chennai, India.
5. Indian Institute of Chemical Technology, India.
6. India National Science Academy/Center for International Cooperation in Science, India.
- Abia AA, Asuquo ED: Lead(II) and Nickel(II) adsorption kinetics from aqueous metal solution using chemically modified and unmodified agricultural adsorbents. Afr J Biotechnol 2006, 5(16):1475-1482.Google Scholar
- Adouby K, Akissi LC, Wandan NE, Yao B: Removal of heavy metals (Pb2+, Cu2+) in aqueous solutions by Pterygota macrocarpa sawdust. J Appl Sci 2007, 7(14):1864-1872.View ArticleGoogle Scholar
- Ahmad AA, Hameed BH, Aziz N: Adsorption of direct dye on palm ash: kinetics and equilibrium modeling. J Hazard Mater 2007, 141: 70-76. 10.1016/j.jhazmat.2006.06.094View ArticleGoogle Scholar
- Amirnia S, Margaritis A, Ray M: Adsorption of mixtures of toxic metal ions using non-viable cells of saccharomyces cerevisiae . Adsorpt Sci Technol 2012, 30: 43-64. 10.1260/0263-6220.127.116.11View ArticleGoogle Scholar
- Asasian N, Kaghazchi T: A comparison on efficiency of virgin and sulfurized agro-based adsorbents for mercury removal from aqueous systems. Adsorption 2013, 19(1):189-200. 10.1007/s10450-012-9437-8View ArticleGoogle Scholar
- Bada SO: Preliminary Information on the Ecology of Chrysophyllum Albidium in West and Central Africa. In Proceeding of National Workshop on the Potential of the Star Apple in Nigeria. Edited by: Denton OA, Ladipo DO, Adetoro MA, Sarumi MB. Ibadan, Nigeria: CENRAD; 1997:16-25.Google Scholar
- Bhattacharya AK, Venkobachar C: Removal of cadmium (II) by low cost adsorbents. J Environ Eng 1984, 110(1):110-122. 10.1061/(ASCE)0733-9372(1984)110:1(110)View ArticleGoogle Scholar
- Chemistry Department at Colorado University (CDCU): Boulder. In Infrared Spectroscopy: Theory. USA: Handbook for organic chemistry lab, Chapter 15; 2002.Google Scholar
- Chien SH, Clayton WR: Application of Elovich equation to the kinetics of phosphate release and sorption on soils. Soil Sci Soc Am J 1980, 44: 256-268.Google Scholar
- Clesceri LS, Greenberg AE, Eaton AD: Standard methods for the examination of water and waste water. 20th edition. USA: APHA; 1999.Google Scholar
- Crystalmarker: Elements, Atomic Radii and the Periodic Table. 2014. http://www.crystalmaker.com/support/tutorials/crystalmaker/atomic-radii/index.html., Accessed 15th February, 2014Google Scholar
- Deans JR, Dioxn BG: Uptake of Pb2+ and Cu2+ by novel biopolymer. Water Res 1992, 26(4):469-472. 10.1016/0043-1354(92)90047-8View ArticleGoogle Scholar
- Debnath S, Ghosh UC: Kinetics, isotherm and thermodynamics for Cr(III) and Cr(VI) adsorption from aqueous solutions by crystalline hydrous titanium oxide. J Chem Thermodyn 2008, 40: 67-77. 10.1016/j.jct.2007.05.014View ArticleGoogle Scholar
- Driessen W, Vereijken T: Recent Development in Biological Treatment of Brewery Effluent. Living Stone, Zambia: The Institute and Guild of Brewing Convention; 2003.http://www.environmental-expert.com/Files%5C587%5Carticles%5C3041%5Cpaques24.pdfGoogle Scholar
- Ejikeme PM, Okoye AI, Onukwuli OD: Kinetics and isotherm studies of Cu2+ and Pb2+ ions removal from simulated waste water by Gambeya albida seed shell activated carbon. Afr Rev Phys (Afr Phys Rev) 2011, 6: 143-152.Google Scholar
- Feng Y, Gong J, Zeng G, Niu Q, Zhang H, Niu C, Deng J, Yan M: Adsorption of Cd(II) and Zn(II) from aqueous solutions using magnetic hydroxyapatite nanoparticle as adsorbens. Chem Eng J 2010, 162: 487-494. 10.1016/j.cej.2010.05.049View ArticleGoogle Scholar
- FEPA-Federal Environmental Protection Agency: Guideline and Standards for Industrial Effluents, Gaseous Emissions and Hazardous Management in Nigeria. Nigeria: Lagos; 1991.Google Scholar
- Freundlich H: Adsorption in solution. J Phys Chem 1906, 57: 385-470.Google Scholar
- Genc O, Yakinkaya Y, Buguktuncel M, Denilzilla A, Bektas S: Uranium recovery by immobilized and dried powered biomass, characterization and comparison. Int J Miner Processes 2003, 68: 93-107. 10.1016/S0301-7516(02)00062-5View ArticleGoogle Scholar
- Gill P, Moghadam T, Ranjbar B: Differential scanning calorimetry techniques: applications in biology and nanoscience. J Biomol Technol 2010, 21(4):167-193.Google Scholar
- Gräf T, Pasel C, Luckas M, Bathen D: Adsorption of aromatic trace compounds from organic solvents on activated carbons—experimental results and modeling of adsorption equilibria. Adsorption 2012, 18(2):127-141. 10.1007/s10450-012-9388-0View ArticleGoogle Scholar
- Graham N, Gang F, Fowler G, Watts M: Characterisation and coagulation performance of tannin-based cationic polymer: a preliminary assessment. Colloids Surf A Physiochemical Eng Aspects 2008, 327: 9-16.View ArticleGoogle Scholar
- Grini G: Recent developments in polysaccharide-based materials used as adsorbents in waste water treatment. Prog Polym Sci 2005, 30: 38-70. 10.1016/j.progpolymsci.2004.11.002View ArticleGoogle Scholar
- Hameed BH, El-Khaiary MI: Removal of basic dye from aqueous medium using a novel agricultural wase maerial: pumpkin seed hull. J Hazard Mater 2008, 155: 601-609. 10.1016/j.jhazmat.2007.11.102View ArticleGoogle Scholar
- Hashem MA: Adsorption of lead ions from aqueous solution by okra wastes. Int J Phys Sci 2007, 2(7):178-184.Google Scholar
- Higachi K, Ito H, Oishi I: Principles of adsorption and adsorption processes. New York: John Wiley and Sons; 1984:71-73.Google Scholar
- Ho YS, Mckays G: Pseudo-second order model for sorption processes. Process Biochem 1999, 34: 451-465. 10.1016/S0032-9592(98)00112-5View ArticleGoogle Scholar
- Horsfall M, Spiff AI: Effect of 2-mercapto ethanoic acid treatment of fluted pumpkin waste ( Telfaria occidentalis Hook .F.) on the sorption Ni2+ ions from aqueous solution. J Sci Ind Res 2005, 64: 613-620.Google Scholar
- Janhom T, Wattanachira S, Pavasant P: Characterization of brewery wastewater with spectrofluorometry analysis. J Environ Manage 2009, 90: 1184-1190. 10.1016/j.jenvman.2008.05.008View ArticleGoogle Scholar
- Jiang Y, Qi H, Zhang X, Chen G: Inorganic impurity removal from waste oil and wash-down water by Acinetobacter johnsonii . J Hazard Mater 2012, 239–240: 289-293.View ArticleGoogle Scholar
- Kanagachandran K, Jayaratne R: Utilization potential of brewery waste water sludge as an organic fertilizer. J Inst Brew 2006, 112(2):92-96. 10.1002/j.2050-0416.2006.tb00236.xView ArticleGoogle Scholar
- Kang YL, Poon MY, Monash P, Ibrahim S, Saravanan P: Surface chemistry and adsorption mechanism of cadmium ion on activated carbon derived from Garcinia mangostana shell. Korean J Chem Eng 2013, 30(10):1904-1910. 10.1007/s11814-013-0130-8View ArticleGoogle Scholar
- Khalid N, Ahmad S: Removal of lead from aqueous solution using rice husk. Sep Sci Technol 1998, 33: 15.View ArticleGoogle Scholar
- Khuo-Omoregbe DIO, Kuipa PK, Hove M: An assessment of the quality of liquid effluents from opaque beer brewing plants in Bulawayo, Zimbabwe. Water SA 2005, 3(1):141-149.Google Scholar
- Langergren S: About the theory of so called adsorption of soluble substances. Kung Sven Veten Hand 1898, 24: 1-39.Google Scholar
- Langmuir I: The adsorption of gases on plane surfaces of glass, mica and platinum. J Am Chem Soc 1918, 40: 1361-1368. 10.1021/ja02242a004View ArticleGoogle Scholar
- Larous S, Meniai H, Bencheikh M, Lehocine M: Experimental study of the removal of copper from aqueous solution by adsorption using sawdust. Desalination 2005, 185: 483-490. 10.1016/j.desal.2005.03.090View ArticleGoogle Scholar
- Meena AK, Kadirvelu K, Mishra GK: Adsorption removal of heavy metals from aqueous solution by treated sawdust ( Acacia arabica) . J Hazard Mater 2008, 150: 604-611. 10.1016/j.jhazmat.2007.05.030View ArticleGoogle Scholar
- Menkiti MC: Sequential Treatments of Coal Washery and Brewery Effluents by Biocoag-Flocculation and Activated Carbon Adsorption, Ph.D. Dissertation. Nigeria: Nnamdi Azikiwe University, Awka; 2010.Google Scholar
- Menkiti MC, Onukwuli OD: Coag-flocculation studies of Moringa oleifera coagulant (MOC) in brewery effluent: Nephelometric approach. J Am Sci 2010, 6(12):788-806.Google Scholar
- Menkiti MC, Onukwuli OD: Response Surface Methodology and Kinetics Application to the Optimization Treatment of Brewery Waste Water by Afzelia Bella Coag-Flocculant. In Water: Ecological Disasters and Sustainable Development. Edited by: Egboka BC, Odoh BI. Germany: Lambert Press; 2011a:92-107.Google Scholar
- Menkiti MC, Onukwuli OD: Coag-flocculation of Mucuna seed coag-flocculant(MSC) in coal washery effluent(CWE) using light scattering effects. AICHE J 2011b, 58(4):1303-1307.View ArticleGoogle Scholar
- Menkiti MC, Onyechi CA, Onukwuli OD: Evaluation of perikinetics compliance for the coag-flocculation of brewery effluent by Brachystegia eurycoma seed extract. Int J Multidiscip Sci Eng 2011a, 2(6):77-83.Google Scholar
- Menkiti MC, Chime TO, Onukwuli OD: Bioadsorption of suspended and dissolved particles from coal washery effluent onto fluted pumpkin seed shell biomass. World J Eng 2011b, 8(2):179-190. 10.1260/1708-5218.104.22.168View ArticleGoogle Scholar
- Mohan SV, Ramaniah SV, Sarmar PN: Biosorption of direct azo dye from aqueous phase onto spirogyra spp. 102; Evaluation of kinetics and mechanistic aspects. Biochem Eng J 2007, 38: 61-69.View ArticleGoogle Scholar
- Nasssar M, Magdy YH: Mass transfer during adsorption of basic dyes on clay in fixed bed. Indian Chem Eng Sect A 1999, 40(1):27-30.Google Scholar
- Ncibi MC, Borhane M, Mongi S: Adsorptive removal of anionic and non-ionic surfactants from aqueous phase using Posidona oceanica (L) marine biomass. J Chem Technol Biotechnol 2008, 83: 77-83. 10.1002/jctb.1787View ArticleGoogle Scholar
- Noroozi B, Sorial GA, Bahrami H, Arami M: Equilibrium and kinetic adsorption study of a cationic dye by a natural adsorbent-silk worm pupa. J Hazard Mater B 2007, 139: 167-174. 10.1016/j.jhazmat.2006.06.021View ArticleGoogle Scholar
- Oboh IO, Aluyor EO, Audu TOK: Use of Chrysophyllum albidium for removal of metal ions from aqueous solutions. Sci Res Essay 2009, 4(6):632-635.Google Scholar
- Onwu FK, Ogah SP: Studies on the effect of pH on the sorption of Cadmium(II), Nickel(II), Lead(II) and Chromium(VI) from aqueous solutions by African white star apple( Chrysophyllum albidium ) shell. Afr J Biotechnol 2010, 19(42):7086-7093.Google Scholar
- Ortega-Rivas E: Characterization and processing relevance of food particulate materials. Part Syst Characterization 2012, 29: 192-203. 10.1002/ppsc.201100016View ArticleGoogle Scholar
- Patel R, Suresh S: Kinetic and equilibrium studies on the biosorption of reactive black 5 dye by Aspergillus foetidus . Bioresour Technol 2008, 99: 51-58. 10.1016/j.biortech.2006.12.003View ArticleGoogle Scholar
- Ramani K, Jain SD, Mandal AB, Sekaran G: Microbial Induced lipoprotein biosurfactant from slaughterhouse lipid waste and its application to the removal of metal ions from aqueous solution. Colloids Surf B: Biointerfaces 2012, 97: 254-263.View ArticleGoogle Scholar
- Ruthsen DM: Principles of Adsorption and Adsorption Processes. New York: John Wiley and Sons; 1984.Google Scholar
- Shukla A, Zhang Y, Dubey P, Margravel J, Shukla S: The role of saw dust in the removal of unwanted materials from water. J Hazard Mater B 2002, 95: 137-152. 10.1016/S0304-3894(02)00089-4View ArticleGoogle Scholar
- Sivakumar P, Palanisamy PN: Adsorption studies of basic red 29 by a non-conventional activated carbon prepared from Euphorbia antiquorum .L, Internationa . J Chem Technol Res 2009, 1(3):502-510.Google Scholar
- Sujatha M, Ageetha A, Sivakumar P, Palanisamy PN: Orthophosphoric acid activated babul seed carbon as an adsorbent for the removal of methylene blue. E-J Chem 2008, 5(4):742-753. 10.1155/2008/418267View ArticleGoogle Scholar
- Suteu D, Bilba D: Equilibrium and kinetic study of reactive Dye brilliant Red HE-3B adsorption by activated charcoal. Acta Chim Slov 2005, 52: 73-79.Google Scholar
- United States Environmental Protection Agency (USEPA): Guidiance Manual: Turbidity Provisions, PARTICLESCONTRIBUTINGTOTURBIDITY, Chapter8 Page2 EPA. 1999. , Accessed on 18 Feb 2014 http://www.epa.gov/safewater/mdbp/pdf/turbidity/chap_08.pdfGoogle Scholar
- Vyazovkin S: Thermogravimetric Analysis, Characterization of Materials. 2nd edition. USA: John Wiley and Sons, Inc; 2012:1-12.Google Scholar
- Wong YC, Szeto YS, Cheung WH, Mckay G: Pseudo‒first‒order kinetic studies of the sorption of acid dyes onto chitosan. J Appl Polym Sci 2004, 92: 1633-1645. 10.1002/app.13714View ArticleGoogle Scholar
- World Bank Group: Pollution Prevention and Abatement Handbook: Breweries. Washington DC: Environmental Department, World Bank Group; 1998:272-274.Google Scholar
- Yakubu MK, Gumel MS, Abdullahi AM: Use of activated carbon from date seeds to treat textile and tannery effluents. Afr J Sci Technol Sci Eng Ser 2008, 9(1):39-49.Google Scholar
- Yeddou N, Bensmaili A: Kinetic models for the sorption of dye from aqueous solution by clay-wood sawdust mixture. Desalination 2005, 185: 499-508. 10.1016/j.desal.2005.04.053View ArticleGoogle Scholar
- Yubin T, Fangyan C, Honglin Z: Adsorption of Pb (II), Cu (II), and Zn (II) ions on to waste fluidized catalytic cracking catalyst. Adsorption Sci Technol 1998, 16(8):595-606.Google Scholar
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