About this Journal Submit a Manuscript Table of Contents
Advances in Physical Chemistry
Volume 2013 (2013), Article ID 842425, 6 pages
http://dx.doi.org/10.1155/2013/842425
Research Article

Sorption of from Aqueous Solution unto Modified Rice Husk: Isotherms Studies

1Department of Chemistry, Landmark University, P M B 1001, Kwara State, Omu-Aran 370102, Nigeria
2Department of Agricultural and Biosystems Engineering, Landmark University, P M B 1001, Kwara State, Omu-Aran 370102, Nigeria
3Department of Chemical Engineering, Landmark University, P M B 1001, Kwara State, Omu-Aran 370102, Nigeria

Received 23 November 2012; Revised 3 February 2013; Accepted 12 February 2013

Academic Editor: Leonardo Palmisano

Copyright © 2013 A. O. Dada et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract

Investigation of the sorption potential of rice husk, an agricultural waste, as an adsorbent was carried out. The rice husk was modified with orthophosphoric acid and was used for adsorption of lead (II) ions (Pb2+) from aqueous solution. Physicochemical properties of the modified rice husk were determined. Equilibrium sorption data were confirmed with Langmuir, Freundlich and Temkin adsorption isotherms. On the basis of adsorption isotherm graphs, values were determined to be 0.995, 0.916, and 0.797 for Langmuir, Temkin, and Freundlich isotherms, respectively, indicating that the data fitted well into the adsorption isotherms, but Langmuir isotherm is a better model. The maximum monolayer coverage from Langmuir studies,  mg/g, Langmuir isotherm constant,  L/mg, and the separation factor, at 100 mg/L of lead(II) ions indicating that the sorption process, was favourable. The suitability of modified rice husk as an adsorbent for the removal of lead ions from aqueous solution and its potential for pollution control is established.

1. Introduction

The pollution of water resources due to the disposal of heavy metal ions has been an increasing worldwide concern for the last few decades. It is well known that some metals are poisonous or otherwise toxic to human beings and ecological environments as reported by Abdel-Halim and coresearchers [1]. Increasing levels of heavy metals and other pollutants in the environment pose serious threats to water quality, human health, and living organisms. Lead(Pb) is considered as one of the priority metals from the point of view of potential health hazards to human, and it is listed by the Environmental Protection Agency (EPA) as one of 129 priority pollutants. The case of recent lead poisoning of hundreds of children in Zamfara State has been identified as the worst lead poisoning in Nigeria’s history [2].

There are various methods of removing heavy metal ions, and they include chemical precipitation, membrane process, ion exchange, solvent extraction, electrodialysis, and reverse osmosis [3]. These methods are noneconomical and have many disadvantages such as incomplete metal removal, high reagent and energy consumption, and generation of toxic sludge or other waste products that require disposal or treatment. In contrast, the adsorption technique is one of the preferred methods for the removal of heavy metal ions because of its efficiency and low cost [4]. For this purpose, in recent years, interest has recently arisen in the investigation of some unconventional methods and low-cost materials for scavenging heavy metal ions from industrial waste waters [5] using low-cost natural adsorbents which are economically viable such as agricultural wastes. In general, an adsorbent can be assumed as “low cost” if it requires little processing, is abundant in nature, or is a by-product or waste material from industry [6]. Some of the reported low-cost adsorbents include bark, tannin-rich materials, lignin, chitin, chitosan, peat moss, moss, and modified wool and cotton. Insoluble starch xanthates have been found to be very useful to remove heavy metal ions from solutions [7]. Agricultural waste materials such as spent grain [8], polymerized onion skin [9] including sunflower stalks [10], wood cellulose [11], maize bran [3], coconut shell, waste tea, rice straw, tree leaves, peanut and walnut husks, and other adsorbents like goethite [12] and manganese hexacyanoferate(II)/(III) [13] have been studied by various researchers to investigate their effectiveness in binding heavy metal ions. The adsorption of heavy metals by these materials might be attributed to their proteins, carbohydrates, and phenolic compounds which have carboxyl, hydroxyl, sulphate, phosphate, and amino groups that can bind metal ions.

Rice is the second largest produced cereal in the world. Rice husk is the hard protecting covering of grains of rice. It is an agricultural waste material obtained from the threshing of the rice and constitutes about 20% of 650 million tons of rice produced annually in the world [14]. Although low in calorific value, rice husk is used as fuel for some industrial and household purposes. In addition to protecting rice during the growing season, rice husk can be put to use as building material, fertilizer, insulation material, or fuel. It is used for production of mesoporous sieves which find application in catalysis, as a support for drug delivery system and as an adsorbent in waste water treatment. In fact, it was investigated as a viable material for the treatment of synthetic direct red dye in industrial waste water [1517].

Most commonly used bioadsorbents are untreated/unmodified; however in this research, the potential of acid modified rice husk is investigated in the removal of toxic heavy metal ion such as lead from its aqueous solution namely, the study of the Langmuir, Freundlich, and Temkin adsorption isotherms.

2. Material and Method

Collection and Preparation of Adsorbent. Rice husk was obtained from a local mill in Ilorin, Kwara State and was pretreated according to the method reported by Milind et al. [18] and Ken-Sen et al. [19]. The rice husk was screened and washed with deionized water to remove dirt and metallic impurities after which it was dried in the oven at about 105°C for 2 hours. The dried rice husk was grounded and sieved in the mesh in the range between 250 μm and 150 μm in order to increase its surface area. The sieved rice husk was treated with 1.0 M orthophosphoric acid (H3PO4) and heated on the magnetic stirrer at 100°C until it totally formed a paste. The modified rice husk was washed with de-ionized water until the . It was later dried in the oven at about 80°C to remove moisture. The modified adsorbent was tagged phosphoric acid modified rice husk (PRH).

The PRH was characterized by determining the following parameters: specific surface area, moisture content, loss of mass on ignition, pH, and bulk density using standard procedures.

2.1. Simple Specific Surface Area Determination

Saers method has been used by a number of researchers [2023]. This method is accurate in the determination of surface area of rice husk because the effect of chemical modification was characterized using this method. A sample containing 0.5 g of the PRH was acidified with 0.1 M HCl to pH 3–3.5; the volume was made up to 50 cm3 with de-ionized water after addition of 10.0 g of NaCl. The titrations were carried out with standard 0.1 M NaOH in a thermostatic bath at  K to pH 4.0 and then to pH 9.0. The volume required to raise the pH from 4.0 to 9.0 was noted, and the surface area was computed from the following equation:

2.2. Determination of the Moisture Content

5 g of the PRH was weighed into a crucible. This was placed in the oven and heated for 5 hrs at constant temperature of 105°C. The sample was then removed and put rapidly into a desiccator in order to prevent more moisture uptake from atmosphere. The sample was reweighed. This procedure was repeated several times until a constant weight was obtained. The difference in the mass constitutes the amount of moisture content of the adsorbent [24]: where = weight of crucible, = initial weight of crucible with sample, = final weight of crucible with sample.

2.3. The Determination of Loss of Mass on Ignition

This was done by weighing 10 g of the adsorbent and put inside furnace at constant temperature of 600°C for 2 hrs. After roasting, the sample became charred and was removed from the furnace then put in a desiccator for cooling. The residual product is then weighed, and the difference in mass represented the mass of organic material present in the sample. This operation was repeated four times.

2.3.1. pH Determination

pH of the samples was determined by weighing 1 g each of PRH, boiled in a beaker containing 100 mL of distilled water for 5 min; the solution was diluted to 200 mL with distilled water and cooled at room temperature. The pH of each was measured using a pH meter (model ATPH-6), and the readings were recorded [1].

2.3.2. The Bulk Density

Archimedes’ principle was used to simply determine the bulk density by weighing a 10 cm3 measuring cylinder before and after filling with the samples. The measuring cylinder was then dried, and the sample was packed inside the measuring cylinder, leveled, and weighed. The weight of the sample packed in the measuring cylinder was determined from the difference in weight of the filled and empty measuring cylinder. The volume of water in the container was determined by taking the difference in weight of the empty- and water filled-measuring cylinder. The bulk density was determined using the equation below [25]: where = weight of empty measuring cylinder, = weight of cylinder filled with sample, = volume of cylinder.

The preparation of adsorbate was carried out by preparing stock solution containing 1000 mg/L of Pb. 0.3998 g of Pb(NO3)2 in 250 cm3 of de-ionized water. Working concentration in the range of 10 mg/L–200 mg/L was prepared by serial dilution.

2.3.3. Sorption Experiment

The equilibrium sorption of the Pb2+ ions unto PRH was carried out by contacting 0.1 g of the substrate with 100 cm3 of different concentrations from 10 mg/L–200 mg/L in 250 cm3 pyrex conical flask intermittently for 90 minutes. The mixture was filtered, and the residual concentration of the filtrate was analyzed using Atomic Absorption Spectrophotometer (2380 UNICAM AAS). The amount of adsorbed (mg/g) was calculated using the formulae reported by Vanderborght and Van Grieken [26]: where = the amount of solute adsorbed from the solution, = volume of the adsorbate, = the concentration before adsorption, = the concentration after adsorption, and = the weight in gram of the adsorbent. The data were fitted into the following isotherms: Langmuir, Freundlich, and Temkin [27]. The removal efficiency was determined by computing the percentage of sorption using the formulae in (5):

3. Results and Discussion

The physicochemical parameters of the phosphoric acid modified rice husk (PRH) are shown in Table 1.

tab1
Table 1: Some physicochemical parameters of the phosphoric acid modified rice husk (PRH).

The physicochemical parameters of the modified rice husk are, namely, pH, % moisture content, % loss of mass on ignition, bulk density (g/cm3), particle sizes, and surface area (m2/g). The values reported are in the range with those reported in the literature [14].

3.1. Sorption Isotherms of Pb(II) Ion unto PRH

The equilibrium sorption of the Pb2+ ions was carried out by contacting 0.1 g of the PRH with 100 cm3 of 1000 mg/L of different concentrations from 10 mg/L–200 mg/L in 250 cm3 Pyrex conical flask intermittently for 90 minutes on the orbital shaker. The mixture was filtered, and the filtrate was analyzed for metal ions concentration using AAS. The data were fitted into the following isotherms: Langmuir, Freundlich, and Temkin.

The adsorption data obtained with the adsorbent correlates well with Langmuir, Freundlich, and Temkin adsorption models and were illustrated in Figures 1, 2, and 3. The Langmuir equation was chosen for the estimation of maximum adsorption capacity corresponding to complete monolayer coverage on the PRH surface [27]. The Langmuir model assumes the surface of the sorbent to be homogenous and the sorption energies to be equivalent for each sorption site. The essential characteristics of the Langmuir model can be expressed in terms of a dimensionless constant and separation factor or equilibrium parameter, . From the results in Table 3, the values were found to be greater than zero and less than one, that is, . value between 0 and 1 indicates favorable adsorption. This means that a favorable adsorption was observed in this study. Langmuir adsorption describes quantitatively the formation of a monolayer of adsorbate on the outer surface of the adsorbent, and after that, no further adsorption takes place. Thereby, the Langmuir represents the equilibrium distribution of metal ions between the solid and liquid phases [28]. The Langmuir isotherm is valid for monolayer adsorption onto a surface containing a finite number of identical sites. The model assumes uniform energies of adsorption onto the surface and no transmigration of adsorbate in the plane of the surface. Based upon these assumptions, Langmuir represented the following equation: Langmuir adsorption parameters were determined by transforming the Langmuir equation (6) into linear form: where = the equilibrium concentration of adsorbate (mg/L−1),= the amount of metal adsorbed per gram of the adsorbent at equilibrium (mg/g),= Langmuir constants related to adsorption capacity (mg/g), = rate of adsorption (L/mg). The values of and were computed from the slope and intercept of the Langmuir plot of versus [24]. The essential features of the Langmuir isotherm may be expressed in terms of equilibrium parameter , which is a dimensionless constant referred to as separation factor or equilibrium parameter [29]: where = initial concentration, = the constant related to the energy of adsorption (Langmuir constant), value indicates the adsorption nature to be either unfavourable if ), linear if , favourable if , and irreversible if . From the data calculated in Table 3, the is greater than 0 but less than 1 indicating that Langmuir isotherm is favourable.

842425.fig.001
Figure 1: Langmuir adsorption isotherm of Pb(II) ion unto PRH.
842425.fig.002
Figure 2: Freundlich adsorption isotherm of Pb(II) ion unto PRH.
842425.fig.003
Figure 3: Temkin adsorption isotherm of Pb(II) ion unto PRH.

Freundlich model was chosen to estimate the adsorption intensity of the sorbent towards the sorbate [21]. and determine the curvature and steepness of the isotherm [8]. The value of also indicates the affinity of the sorbent towards the uptake of Pb2+. The values for the constant and were shown on Table 3. The value is 0.59, and this suggests a greater sorption capacity. Also, the value of is greater than unity for the metal ions indicating that adsorption of the metal ions was favorable.

Freundlich adsorption is commonly used to describe the adsorption characteristics for the heterogeneous surface [30]. These data often fit the empirical equation proposed by Freundlich as follows: where = Freundlich isotherm constant (mg/g) (dm3/g)n and adsorption intensity, = the equilibrium concentration of adsorbate (mg/L), the amount of metal adsorbed per gram of the adsorbent at equilibrium (mg/g). Taking logs and rearranging as follows:

The constant is an approximate indicator of adsorption capacity, while is a function of the strength of adsorption in the adsorption process. These constants can be obtained by appropriate plot of Log against Log. The constant can be obtained from the intercept while is obtained from the slope [31]. If , then the partition between the two phases is independent of the concentration. If the value of is below unity, it indicates a normal adsorption. On the other hand, being above unity indicates cooperative adsorption [32]. As the temperature increases, the constants and change to reflect the empirical observation that the quantity adsorbed rises more slowly, and higher pressures are required to saturate the surface. and are parameters characteristic of the sorbent-sorbate system, which must be determined by data fitting. When performing data fitting, linear regression is generally used to determine the best isotherm models for this study [33]. is an heterogeneity parameter; the smaller the value of is, the greater the expected heterogeneity becomes. If lies between unity and ten, this indicates a favorable sorption process [34]. From the data in Table 3 below, the value of indicating that the sorption of Pb2+ unto PRH is favourable.

Temkin isotherm model was also chosen for the study of this equilibrium sorption. This was done by plotting the quantity sorbed against , and the constants and were determined from the slope and intercept. These constants correlate to the adsorption capacity and intensity of adsorption. The model is given by the following equation [35]: where= Temkin isotherm equilibrium binding constant (L/g),= Temkin isotherm constant,= universal gas constant (8.314J/moL/K),= Temperature at 298 K.

Table 2 shows the parameter for plotting Langmuir, Freundlich, and Temkin adsorption isotherms, while Table 3 shows various parameters relevant to each adsorption model in the sorption of Pb(II) ion unto PRH. The Langmuir, Freundlich and Temkin adsorption isotherms are illustrated in Figures 1, 2, and 3. Considering the values for Langmuir, Freundlich, and Temkin adsorption isotherms which are 0.99, 0.797, and 0.916, respectively, examination of these plots from Figures 1, 2, and 3 suggests that the Langmuir, Freundlich, and Temkin isotherms fit the experiment, but Langmuir isotherm is a better model than Freundlich, and Temkin isotherms with respect to their values which is greater than 0.9000 and less than 1. This is an indication that PRH performed better in the sorption of Pb2+, and obviously the data fitted well into the three adsorption isotherms. However, among the three isotherms, Langmuir isotherm fitted best, and this is in agreement with investigation carried out by Sumar and coworkers [36], Adekola and Adekoge [13], Adediran and coresearchers [37].

tab2
Table 2: Parameters for plotting Langmuir, Freundlich, and Temkin adsorption isotherms of Pb(II) ion unto PRH.
tab3
Table 3: Langmuir, Freundlich, and Temkin constants for the adsorption of Pb(II) unto PRH.

4. Conclusion

For the past few years, there is an increasing interest in the preparation of low-cost adsorbent as an alternative to biosorption of lead(II) ions. In this research, rice husk has shown its potential to be an active bioabsorbent material in solving waste water pollution as a cost-effective adsorbent. The usage of the rice husk might help to overcome part of the excessive agricultural wastes in some part of the world. This research proved that rice husks possess different physical characteristics. Chemical modification using phosphoric acid improves the adsorption capacity of active binding sites. Hence, modified rice husk is a potent and low-cost alternative adsorbent for the treatment of lead-polluted waste water.

Acknowledgment

The authors are grateful to the management of Landmark University for the timely supply of the necessary equipments into the Department of Sciences for core research work.

References

  1. E. S. Abdel-Halim, A. Abou-Okeil, and A. Hashem, “Adsorption of Cr(VI) oxyanions onto modified wood pulp,” Polymer, vol. 45, no. 1, pp. 71–76, 2006. View at Publisher · View at Google Scholar · View at Scopus
  2. O. Debo, Zamfara Lead Poisoning: Any Light at the End of the Tunnel?The Nigerian Guardian News Paper, 2012.
  3. K. K. Singh, M. Talat, and S. H. Hasan, “Removal of lead from aqueous solutions by agricultural waste maize bran,” Bioresource Technology, vol. 97, no. 16, pp. 2124–2130, 2006. View at Publisher · View at Google Scholar · View at Scopus
  4. Y. Kamimura, H. Chiba, H. Utsumi, et al., “Barrier function of microvessels and roles of glial cell line-derived neurotrophic factor in the rat testis,” Medical Electron Microscopy, vol. 35, pp. 139–145, 2002. View at Publisher · View at Google Scholar
  5. V. Gloaguen and H. J. Morvan, “Removal of heavy metal ions from aqueous solution by modified barks,” Journal of Environmental Sci Health, vol. 32, no. 4, pp. 901–912, 1997. View at Publisher · View at Google Scholar
  6. S. E. Bailey, T. J. Olin, and R. M. Bricka, “A review of potentially low-cost sorbents for heavy metals,” Journal of Water Research, vol. 33, pp. 2469–2479, 1999. View at Publisher · View at Google Scholar
  7. N. N. Rao, A. Kumar, and S. N. Kaul, “Alkali-treated straw and insoluble straw xanthate as low cost adsorbents for heavy metal removal-preparation, characterization and application,” Journnal of Bioresource Technology, vol. 71, pp. 133–142, 2000. View at Publisher · View at Google Scholar
  8. K. S. Low and C. S. Lee, “Sorption of cadmium and lead from aqueous solutions by spent grain,” Journal of Process Biochemistry, vol. 36, pp. 59–64, 2000. View at Publisher · View at Google Scholar
  9. P. Kumar and S. S. Dara, “Binding heavy metal ions with polymerized onion skin,” Journal of Polymer Science, vol. 19, pp. 397–402, 1981. View at Publisher · View at Google Scholar
  10. G. Sun and W. Shi, “Sun flowers stalks as adsorbents for the removal of metal ions from waste water,” Industrial & Engineering Chemistry Research, vol. 37, no. 4, pp. 1324–1328, 1998. View at Publisher · View at Google Scholar
  11. G. O. Adediran, S. R. Kazeem, and F. O. Nwosu, “Chromatography of metal ions in wood cellulose impregnated with Urea and ThioUrea,” in Book of Abstracts, 22nd Annual Conference of Chemical Society of Nigeria, p. 42, 1999.
  12. F. A. Adekola, N. G. Nwaogu, and N. Abdus-Salam, “Removal of cadmium from aqueous solution using manganese hexacyanoferrates (II)/(III),” Bulletin of the Chemical Society of Ethiopia, vol. 21, no. 2, pp. 221–228, 2007.
  13. F. A. Adekola and H. I. Adekoge, “Adsorption of Blue Dye on activated carbon from rice husk, coconut shell and coconut coirpith,” Ife Journal of Science, vol. 7, no. 1, pp. 151–157, 2005.
  14. T. Genctan and A. Balkan, “Problems and production of rice in Turkey. The first national symposium of rice,” Tekirdag, vol. 24-25, pp. 8–21, 2009.
  15. J. Chumee J, “Characterization of platinum-iron catalysts supported on MCM-41 synthesized with rice husk silica and their performance for phenol hydroxylation,” Science and Technology of Advanced Materials, vol. 9, p. 15, 2008.
  16. S. Chiarakorn, T. Areerob, and N. Grisdanurak, “Influence of functional silanes on hydrophobicity of MCM-41 synthesized from rice husk,” Science and Technology of Advanced Materials, vol. 8, no. 1-2, pp. 110–115, 2007. View at Publisher · View at Google Scholar · View at Scopus
  17. A. Ola, E. Ahmed, E. Amany, and K. Azza, “Use of rice husk for adsorption of direct dyes from aqueous solution: a case study of Direct F. Scarlet,” Egyptian Journal of Aquatic Research, vol. 31, no. 1, pp. 1110–0354, 2005.
  18. R. O. Milind, D. Julie, and J. Snehal, Comparative adsorption studies on activated rice husk and rice husk ash by using methylene blue as dye, International Congress on Environmental Research at Bits Pilani GOA, 2009.
  19. C. Ken-Sen, T. Jhy-Ching, and L. Chieh-Tsung, “The adsorption of Congo red and Vacuum pump oil by rice hull ash,” Bioresource Technology, vol. 78, pp. 217–291, 2001. View at Publisher · View at Google Scholar
  20. G. W. Saer, “Determination of Specific surface area of sodium hydroxide,” Analytical Chemistry, vol. 28, no. 2, pp. 1981–1983, 1956. View at Publisher · View at Google Scholar
  21. R. A. Shawabkeh and M. F. Tutunji, “Experimental studies and modeling of the basic dye sorption by diamaceous clay,” Applied Clay Science, vol. 24, pp. 111–114, 2003. View at Publisher · View at Google Scholar
  22. S. Yadav, D. K. Tyagi, and O. P. Yadav, “Equilibrium and kinetics studies on adsorption of aniline blue from aqueous solution onto rice Husk carbon,” International Journal of Chemistry Research, vol. 2, no. 3, pp. 59–64, 2011.
  23. R. A. Shawabkeh, “Synthesis and characterization of activated carbo-aluminosilicate material from oil shale,” Microporous and Mesoporous Materials, vol. 75, no. 1-2, pp. 107–114, 2004. View at Publisher · View at Google Scholar · View at Scopus
  24. I. Langmuir, “The adsorption of gases on plane surfaces of glass, mica and platinum,” Journal of the American Chemical Society, vol. 40, pp. 1362–1403, 1918.
  25. S. Toshiguki and K. Yukata, “Pyrolysis of plant, animal and human wastes: physical and chemical characterization of the pyrolytic product,” Journal Bioresource Technology, vol. 90, no. 3, pp. 241–247, 2003.
  26. M. Vanderborght and E. Van Grieken, “Enrichment of trace metals in water by adsorption on activated carbon,” Analytical Chemistry, vol. 49, no. 2, pp. 311–316, 1997.
  27. J. C. Igwe and A. A. Abia, “A bioseparation process for removing heavy metals from waste water using biosorbents,” African Journal of Biotechnology, vol. 5, no. 12, pp. 1167–1179, 2006. View at Scopus
  28. T. H. Vermeulan, K. R. Hall, L. C. Eggleton, and A. Acrivos, “Fundam,” Industrial & Engineering Chemistry Research, vol. 5, pp. 212–223, 1966.
  29. T. N. Webber and R. K. Chakravarti, “Pore and solid diffusion models for fixed bed adsorbers,” American Institute of Chemical Engineers, vol. 20, pp. 228–238, 1974. View at Publisher · View at Google Scholar
  30. N. D. Hutson and R. T. Yang, “Theoretical basis for the Dubinin-Radushkevitch (D-R) adsorption isotherm equation,” Adsorption, vol. 3, no. 3, pp. 189–195, 1997.
  31. E. Voudrias, F. Fytianos, and E. Bozani, “Sorption description isotherms of dyes from aqueous solutions and waste waters with different sorbent materials,” Global NEST, vol. 4, no. 1, pp. 75–83, 2002.
  32. S. Mohan and J. Karthikeyan, “Removal of lignin and tannin color from aqueous solution by adsorption on to activated carbon solution by adsorption on to activated charcoal,” Environmental Pollution, vol. 97, pp. 183–187, 1997.
  33. G. de la Rosa, H. E. Reynel-Avila, A. Bonilla-Petriciolet, I. Cano-Rodríguez, C. Velasco-Santos, and A. L. Martínez-Hernández, “Recycling poultry feathers for Pb removal from wastewater: kinetic and equilibrium studies,” in Proceedings of World Academy of Science, Engineering and Technology, vol. 30, pp. 1–8, 2008.
  34. S. Goldberg, “Equations and models describing adsorption processes in soils,” in Chemical Processes in Soils, SSSA Book Series no. 8, Soil Science Society of America, Madison, Wis, USA, 2005.
  35. M. Temkin and J. A. V. Pyzhev, “Kinetics of Ammonia synthesis on promoted Iron catalysts,” Acta Physico-Chimica, vol. 12, pp. 217–222, 1940.
  36. N. Sumar, Z. Uzma, A. Arifa, and I. Asma, “Adsorption studies of Chromium(VI) on RHA,” Journal of Chemical Society, vol. 31, no. 3, pp. 1–9, 2009.
  37. G. O. Adediran, J. F. Adediji, M. A. Adebayo, and A. O. Dada, “Removal of Pb2+ and Cr6+ ions from aqueous solution by earthworm cast soil,” International Journal of Physical Sciences, vol. 4, no. 11, pp. 691–697, 2009. View at Scopus