Study on Stability of Ferrate (VI) under the Effect of the Buffering Agent and the Strong Oxidizer

Abstract:

In order to extend the preservation time of the ferrate, the experiment was carried out to study the type of strong oxidizer and buffering agent through static comparing test. The orthogonal test determined the best parameters of sulfate type, temperature and the dosage. The result shows that the inhibitory action of Na2S2O8 is the strongest oxidizer, and the temperature had the important role on ferrate stability. The higher temperature, the quicker the ferrate decomposition speed. The Na2S2O8 effect on stability was the best at any temperature and the dosage of Na2S2O8 could be controlled between 0.5% and 1.0%.The carbonate buffering agent could play certain stable effect, the ferrate decomposition is only 7.65% from the 2nd day to the 10th day when the mole ratio of NaHCO3 and NaOH was 2:1 and the density was the ferrate’s 100times.

• Periodical: Advanced Materials Research (Volumes 113-116)
• Pages: 2319-2322
• DOI: https://doi.org/10.4028/www.scientific.net/AMR.113-116.2319
• Online since: June 2010
• Authors: Kun You, Jing Xiang Fu, Yu Lan Tang, Yu Hua Zhao, Ying Ying Lan
• Keywords: Buffering Agent, Ferrate, Orthogonal Test, Stability, Strong Oxidizer

References

[1] Jiang J Q, L loyd B, Grigore L. Preparation and evaluation of potassium ferrate as anoxidant and coagulant for potable water treatment [J]. Environm Engineer Sci, 2001, 18(5): 323-328.

DOI: 10.1089/10928750152726041

[2] Jiang J Q, L loyd B, Grigore L. Preparation and evaluation of potassium ferrate as anoxidant and coagulant for potable water treatment [J]. Environm Engineer Sci, 2001, 18(5): 323-328.

DOI: 10.1089/10928750152726041

[3] H. Rose. Preparation and Purification of Potassium Ferrate[J]. Am Chem Soc, 1951, 73: 1379-1381.

[4] Wagner W. F, Gump K. R, Hart E. N. Factors affecting the stability of aqueous potassium ferrate(VI) solutions[J]. Anal. Chem., 1952, 24: 1497-1498.

DOI: 10.1021/ac60069a037

[5] Ernst, Teresa, Wawrzenczyk, Miroelawa, Cyfert Maria, Effect of pH on the kinetics of ferrate (VI) decomposition [J]. Bull. Acad. Poc. Sci. Ser. Sci. Chim, 1979, 27(10), 773-778.

[6] M. Wronska. The cyclic voltammetric Study of ferrate(VI) production [J]. J Electroanal Chem, 1997, 425: 125-137.

[7] V. Ettle, J. Veprek-Siska, Reactions of very pure substances V. decomposition of ferrates in alkaline solutions [J]. Collect. Czech. Chem. Commun., 1969, 3498, 2182-2188.

[8] LI Guo-ting, JIA Han-dong, BAO Gai-ling. GAO Yu-mei. Simultaneous determination of Fe(Ⅵ) and Fe(Ⅵ) in ferrate solution with three-wavelength and dual-wavelength spectrophotometry[J]. Journal of Instrumental Analysis, 2004(01): 61-63.

[9] LEI Xiao-yan, LIU Shen. Performance and application of potassium ferrate[J]. Journal of Jiaxing College. 2002, 14(3): 41-43.

[10] YANG Wei-Hua, WANG Jian-Ming, CAO Jiang-Lin. Stability of K2FeO4 in Dilute KOH Solution [J]. Acta Chimica Sinica. 2004, 62(19): 1951-(1955).

[11] Fan M, Brown R C, Huang C P. Preliminary studies of the oxidation of arsenic (Ⅵ) by potassium ferrate[J]. J Environm Pollu, 2002, 18 (1): 91-96.

[12] Licht S, Vera N, Susanta G, et al. SrFe04: Synthesis, Fe (VI) characterization and the strontium super-iron battery [J]. Electrochemistry Communications, 2001，3(7): 340-345.

DOI: 10.1016/s1388-2481(01)00167-9