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Progress in Chemistry 2021, Vol. 33 Issue (7): 1201-1211 DOI: 10.7536/PC200756 Previous Articles   Next Articles

• Review •

Oxidative Degradation of Emerging Organic Contaminants in Aqueous Solution by High Valent Manganese and Iron

Jing Zhang1,2,*(), Dingxiang Wang1, Honglong Zhang1   

  1. 1 College of Environment and Ecology, Chongqing University, Chongqing 400045, China
    2 Key Laboratory of the Three Gorges Reservoir Region’s Eco-Environment, Chongqing University, Chongqing 400045, China
  • Received: Revised: Online: Published:
  • Contact: Jing Zhang
  • About author:
    * Corresponding author e-mail:
  • Supported by:
    National Key R&D Program of China(2019YFD1100101); General Program of National Natural Science Foundation of China(51878095)
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Emerging organic contaminants are widely present in the waters and have potential threat to the ecosystem and human health. How to remove the emerging organic contaminants has become a growing concern for researchers. High valent manganese and iron, i.e. potassium permanganate (Mn(Ⅶ), KMnO4) and potassium ferrate (Fe(Ⅵ), K2FeO4), are two effective inorganic chemicals for decomposing emerging organic contaminants in water treatment. Permanganate and ferrate are environmentally friendly, and have been drawing more and more attention due to their high efficiency. Permanganate and ferrate have similar chemical properties and close behavior in the removal of emerging organic contaminants. Recent studies on the oxidative degradation of emerging organic contaminants by permanganate and ferrate mainly focus on the kinetic models, the role of manganese- and iron-intermediates, the role of free radicals generated when permanganate and ferrate are combined with other chemicals or processes, and their application in real waters. Therefore, this paper summarizes the reaction kinetics of permanganate and ferrate, and compares the roles of permanganate- and ferrate-intermediates and free radicals, and their performance in real waters.

Contents

1 Introduction

2 Mechanism of permanganate and ferrate oxidation

3 Oxidation kinetics of organic pollutants by permanganate and ferrate

4 Formation and functions of permanganate- and ferrate-intermediates

5 Generation and function of free radicals

6 Performance in real waters

7 Conclusion and outlook

Key words: permanganate, ferrate, manganese intermediates, iron intermediates, emerging organic contaminants, drinking water treatment
Fig. 1 Speciation of ferrate(Ⅵ) at different pH[18]
Table 1 Reduction potentials of Mn(Ⅶ), Fe(Ⅵ), O3 and H2O2in aqueous solutions[17]
Couple(Ox/Red) E0,V Couple(Ox/Red) E0,V
Mn O 4 -/Mn2+ 1.67 MnO-/MnO2 0.56
Fe O 4 2 -/Fe3+ 2.20 Fe O 4 2 -/Fe(OH)3 0.72
O3/O2 2.08 O3/O2 1.24
H2O2/H2O 1.78 H2O2/OH- 0.88
Fig. 2 The kapp for the reaction of Mn(Ⅶ) and Fe(Ⅵ) with emerging organic contaminants[15,22⇓⇓⇓⇓⇓⇓⇓⇓⇓⇓-33]
Fig. 3 Reaction kinetics model fitting result of the second-order reaction rate constant of ferrate with BPS or BPAF. Experimental conditions: [BPS]0 =5 μmol/L, [BPAF] 0 = 5 μmol/L, [ferrate] 0 =50 μmol/L, T= 25 ℃[24]
Fig. 4 Effect of pH on second-order rate constants of bisphenol A oxidation by permanganate and ferrate[22,23]
Fig. 5 Possible reaction mechanisms of (a) Mn(Ⅶ)/NaHSO3[69] ; (b) Mn(Ⅶ)/NaHSO3[70]; (c)Mn(Ⅶ)/NaHSO3[48]; (d) Fe(Ⅵ)/ Na2S2O3[73]; (e) Fe(Ⅵ)/ Na2SO3[74]; and (f) Fe(Ⅵ)/ Na2SO3[75]
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