Effect of Operating Conditions on the Chemical Phosphate Removal Using during Ferrous Iron Oxidation

Abstract:

In this study, the effect of operating parameters and the co-existing ions on the phosphate removal during the ferrous iron oxidation was investigated. Results showed that with the increase of DO and [Fe (II)]₀, the final phosphate removal rate both increased. But with increasing of pH, the final phosphate removal rate firstly increased and then decreased when the pH was higher than 8.0. The co-existing ions affected the final removal rate significantly, and the kinetics of phosphate removal followed the pseudo-first-order kinetic model. The corresponding k_obs trends for the cation followed the order of Cu²⁺>Mn²⁺>Zn²⁺>NH⁴⁺-N. The presence of Cu²⁺ promoted the phosphate removal significantly. Compared with the control, , the time required to achieve 40 % phosphate removal rate, at the condition of 0.5 mg/L Cu²⁺, reduced from 60 min to 10 s. However, the selective anions inhibited the phosphate removal, due to the formation of Fe-anions complexes. The effect of selective anions on the phosphate removal rate constant decreased in the order of SO₄^2->Cl^-> NO₃^-.

• Periodical: Advanced Materials Research (Volumes 807-809)
• Pages: 478-485
• DOI: https://doi.org/10.4028/www.scientific.net/AMR.807-809.478
• Online since: September 2013
• Authors: Ting Li, Wen Yi Dong, Hong Jie Wang, Jin Nan Lin, Feng Ouyang, Qian Zhang
• Keywords: Co-Existing Ions, Dissolved Oxygen (DO), Ferrous Iron, pH, Phosphate

References

[1] Valsami-Jones E: IWA Publishing, London, (2004), p.656.

[2] I Katz, CG Dosoretz: Desalination Vol. 222 (2008), p.230.

[3] S. Yeoman, T. Stephenson, J.N. Lester, R. Perry: Environ. Pollut. Vol. 49 (1988), p.183.

[4] Luz E. de-Bashan, Yoav Bashan: Water Res. Vol. 19 (2004), p.4222.

[5] W.M. Xie, Q.H. Wang, H. Zh. Ma: Process Biochem. Vol. 40 (2005), p.2623.

[6] T. Clark, T. Stephenson, P.A. Pearce: Water Res. Vol. 31 (1997), p.2557.

[7] L Lijklema: Environ. Sci. Technol. Vol. 14 (1980), p.537.

[8] P.H. Hsu: Water Res. Vol. 10 (1976), p.903.

[9] K.C. Ruttenberg, D.J. Sulaka: Geochim. Cosmochim. Ac. Vol. 75 (2011), p.4095.

[10] W. Stumm, J. Leckie, E.F. Gloyna, Water Quality Improvement by Physical and Chemical Processes, University of Texas Press, Austin (1970).

[11] M Ghassemi, HL Recht, Phosphate precipitation, Water Pollution Control Re-search Series, U.S. Environmental Protection Agency, Cincinnati, Ohio, (1971).

[12] N El Azher, B Gourich, C Vial: Chem. Eng. Process Vol. 47 (2008), p.1877.

[13] W. Stumm, G.F. Lee: Ind. Eng. Chem. Vol. 53 (1961), p.143.

[14] Chinese NEPA, Water and Wastewater Monitoring Methods, forth ed., Chinese Environmental Science Publishing House, Beijing, China, (2003).

[15] Thistleton J, Clark T, Pearce P: Process Saf. Environ. Vol. 79(2001), p.339.

[16] Robert E. Huffman, Norman Davidson，Kinetics of the ferrous iron-oxygen reaction in sulfuric acid solution, J. Am. Chem. Soc. 78 (1956) 4836-4842.

DOI: 10.1021/ja01600a004

[17] W. Stumm, J.J. Morgan, Aquatic chemistry: chemical equilibrium and rates in natural waters, (Third edition) John Wiley & Sons, Inc., New York (1996).

[18] Alejandro H. Caravelli, Carolina De Gregorio: Chem. Eng. J. Vol. 209 (2012), p.469.

[19] C. De Gregorio, A.H. Caravelli: Chem. Eng. J. Vol. 172 (2011), p.52.

[20] Cher M, Davidson N.: J. Am. Chem. Soc., Vol. 77 (1955), p.793.

[21] Koppenol W H.: New Comprehensive Biochemistry, Vol. 28 (1994), p.3.

[22] Sung W, Morgan J.: Environmental Science & Technology, Vol. 14(1980), p.561.

[23] Millero F J, Izaguirre M, Sharma V K: Marine Chemistry, Vol. 22(1987), p.179.