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Fig. 4: Electrocoagulation test on boron removal with and without the aid of curcumin. The formation of rosocyanine depends on the reaction conditions. Preferably, the reaction is carried out in acidic solutions containing hydrochloric or sulfuric acid. The colour reaction can also take place under different conditions, but in an alkaline solution, gradual decomposition is observed. At higher pH values, the reaction might be disturbed by interference from other compounds [22]. Curcumin was used as the adsorbent in our experiments to react with the boron in the solution and form rosocyanine complexes. Rosocyanine is formed from curcumin and boric acid in acidic solutions as a 2:1-complex. Curcumin possesses a 1,3-diketone structure and can therefore be considered as a chelating agent [19]. In these experiments, curcumin-aided electrocoagulation removed a maximum of 70% percent of the boron, a 20% increase compared to unaided electrocoagulation, which only removed about 50% of the boron at peak efficiency. Fig. 4 shows that the increase in the percentage of boron removed by the adsorption process aided by curcumin peaked at the same duration of time during the electrocoagulation process as the unaided process. CONCLUSION This study showed that electrocoagulation with the aid of curcumin could be applied effectively in the treatment of industrial wastewater containing boron. The use of curcumin as an adsorbent material in the treatment of boron wastewater by electrocoagulation was found to be pH dependent. The most effective removal of boron was achieved at pH 4. The boron removal rate increased monotonically with increasing the CD, within the range of our experiment. The highest CD resulted in the fastest treatment time for removing a given quantity of boron. REFERENCES 1. Barth, S., 1998. Water Res., 32(3): 685-690. 2. Boncukcuoglu, R., M.M. Kocakerim, E. Kocadagistan and M.T. Yilmaz, 2003. Resour. Conserv. Recycl., 37(2): 147-157. 3. Seiler, H.F., 1988. Handbook on Toxicity of Inorganic Compounds, Marcel Decker Inc. New York. 4. Gemici, U. and G. Tarcan, 2002. Distribution of boron in thermal waters of western Anatolia, Turkey and examples of their environmental impacts, [In:] Gemici U. Tarcan G. Eds. Environmental Geology, Springer, Turkey, pp: 87-98. 5. United States Environmental Protection Agency [EPA], Toxicological Review Report of Boron and its Compounds, 2001. 6. Y lmaz, A.E., R. Boncukcuoglu, M.M. Kocakerim and B. Keskinler, 2005. J. Hazard. Mater. M., 125(1-3): 160-165. 7. Boncukcuoglu, R., A.E. Yilmaz, M.M. Kocakerim and M. Copur, 2004. Desalination, 160: 159-166. 8. Yilmaz, A.E., R. Boncukcuoglu, M.T. Yilmaz and M.M. Kocakerim, 2005. J. Hazard. Mater., 117: 221-226. 9. Sahin, S., 1996. Mathematical model of boron adsorption by ion-exchange, Models Chem., 133(1-2): 143-150. 10. Schilde, U. and E. Uhlemenn, 1991. Int. J. Miner. Process., 32: 295-305. 11. Koparal, A.S., 2002. The removal of salinity from produced formation by conventional and electrochemical methods, Fresen. Environ. Bull., 12A(11): 1071-1077. 12. Donini, J.C., J. Kan, J. Szynkarczuk, T.A. Hassan and K.L. Kar, 1994. J. Chem. Eng., 72: 1007-1012. 13. Yildiz, Y.S., A.S. Koparal, S. Irdemez. and B. Keskinler,2007. J. Hazard. Mater., B 139: 373-380. 14. Ogutveren, U.B. and S. Koparal, 1997. J. Environ. Sci. Health, A 32: 2507-2520. 15. Chen, X., G.C. Chen and P.L. Yue, 2000. Sep. Purif. Technol., 19: 65-76. 16. Irdemez, S., N. Demircioglu and Y.S. Yildiz, 2006. J. Hazard. Mater., B 137: 1231-1235. 17. Kolev, T.M., E.A. Velcheva, E.A. Stamboliyska and M. Spiteller, 2005. Int. J. Quantum Chem., 102: 1069-1079. Middle-East J. Sci. Res., 11 (5): 583-588, 2012 587PDF Image | Boron Removal from Aqueous Solutions
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