Application of Fe(VI) in abating contaminants in water: State of art and knowledge gaps

doi:10.1007/s11783-020-1373-3

Front. Environ. Sci. Eng.

2021, Vol. 15

Issue (5) : 80 https://doi.org/10.1007/s11783-020-1373-3

REVIEW ARTICLE

Application of Fe(VI) in abating contaminants in water: State of art and knowledge gaps

Shuchang Wang^1,², Binbin Shao^1,², Junlian Qiao^1,^2,³, Xiaohong Guan^1,^2,³(

)

¹. State Key Laboratory of Pollution Control and Resources Reuse, College of Environmental Science and Engineering, Tongji University, Shanghai 200092, China
². Shanghai Institute of Pollution Control and Ecological Security, Shanghai 200092, China
³. International Joint Research Center for Sustainable Urban Water System, Tongji University, Shanghai 200092, China

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Abstract

• The properties of Fe(VI) were summarized.

• Both the superiorities and the limitations of Fe(VI) technologies were discussed.

• Methods to improve contaminants oxidation/disinfection by Fe(VI) were introduced.

• Future research needs for the development of Fe(VI) technologies were proposed.

The past two decades have witnessed the rapid development and wide application of Fe(VI) in the field of water de-contamination because of its environmentally benign character. Fe(VI) has been mainly applied as a highly efficient oxidant/disinfectant for the selective elimination of contaminants. The in situ generated iron(III) (hydr)oxides with the function of adsorption/coagulation can further increase the removal of contaminants by Fe(VI) in some cases. Because of the limitations of Fe(VI) per se, various modified methods have been developed to improve the performance of Fe(VI) oxidation technology. Based on the published literature, this paper summarized the current views on the intrinsic properties of Fe(VI) with the emphasis on the self-decay mechanism of Fe(VI). The applications of Fe(VI) as a sole oxidant for decomposing organic contaminants rich in electron-donating moieties, as a bi-functional reagent (both oxidant and coagulant) for eliminating some special contaminants, and as a disinfectant for inactivating microorganisms were systematically summarized. Moreover, the difficulties in synthesizing and preserving Fe(VI), which limits the large-scale application of Fe(VI), and the potential formation of toxic byproducts during Fe(VI) application were presented. This paper also systematically reviewed the important nodes in developing methods to improve the performance of Fe(VI) as oxidant or disinfectant in the past two decades, and proposed the future research needs for the development of Fe(VI) technologies.

Keywords Ferrate Oxidation Disinfection Coagulation Enhancement

Corresponding Author(s): Xiaohong Guan

Issue Date: 10 November 2020

Cite this article:

Shuchang Wang,Binbin Shao,Junlian Qiao, et al. Application of Fe(VI) in abating contaminants in water: State of art and knowledge gaps[J]. Front. Environ. Sci. Eng., 2021, 15(5): 80.

URL:

https://academic.hep.com.cn/fese/EN/10.1007/s11783-020-1373-3
https://academic.hep.com.cn/fese/EN/Y2021/V15/I5/80

Oxidant	Reactions	E⁰ (V/NHE)	Reference
Ferrate(VI)	$F e O 4 2 − + 8 H + + 8 e − → F e 3 + + 4 H 2 O$	2.20	Sharma et al., 2016
Ferrate(VI)	$F e O 4 2 − + 4 H 2 O + 3 e − → F e (O H) 3 + 5 O H −$	0.70	Sharma et al., 2016
Permanganate	$M n O 4 2 − + 8 H + + 5 e − → M n 2 + + 4 H 2 O$	1.51	Sharma et al., 2016
Permanganate	$M n O 4 2 − + 2 H 2 O + 3 e − → M n O 2 + 4 O H −$	0.59	Sharma et al., 2016
Ozone	$O 3 + 2 H + + 2 e − → O 2 + H 2 O$	2.08	Ghernaout and Naceur, 2012
Ozone	$O 3 + H 2 O + 2 e − → O 2 + 2 O H −$	1.24	Ghernaout and Naceur, 2012
Hypochlorite	$H C l H + H + + 2 e − → C l − + H 2 O$	1.48	Jiang, 2007
Hypochlorite	$C l O − + H 2 O + 2 e − → C l − + 2 O H −$	0.84	Jiang, 2007
Hydrogen peroxide	$H 2 O 2 + 2 H + + 2 e − → 2 H 2 O$	1.78	Sharma et al., 2016
Hydrogen peroxide	$H 2 O 2 + 2 e − → 2 O H −$	0.88	Sharma et al., 2016
Hydroxyl radical	$H O ? + H + + e − → H 2 O$	2.80	Ghernaout and Naceur, 2012
Hydroxyl radical	$H O ? + e − → O H −$	1.89	Ghernaout and Naceur, 2012
Dissolved oxygen	$O 2 + 4 H + + 4 e − → 2 H 2 O$	1.23	Sharma et al., 2016
Dissolved oxygen	$O 2 + 2 H 2 O + 4 e − → 4 O H −$	0.40	Sharma et al., 2016
Chlorine dioxide	$C l O 2 (a q) + e − → C l O 2 −$	0.95	Ghernaout and Naceur, 2012

Tab.1 Redox potential of different oxidant used in water treatment

Fig.1 Influence of pH on the speciation of Fe(VI).

Fig.2 Scheme 1 The self-decay mechanisms of Fe(VI) under different conditions.

Eq.	Reactions	Rate constants at pH 7.0	Reference
(a)	$2 H F e V I O 4 − + 4 H 2 O → 2 H 3 F e I V O 4 − + H 2 O 2$	26 M⁻¹·s⁻¹	Rai et al., 2018
(b)	$H F e V I O 4 − + H 2 O 2 → H 3 F e I V O 4 − + O 2$	10 M⁻¹·s⁻¹	Rai et al., 2018
(c)	$H 3 F e I V O 4 − + H 2 O 2 + H + → F e I I (O H) 2 (a q) + O 2 + 2 H 2 O$	~10⁴ M⁻¹·s⁻¹	Rai et al., 2018
(d)	$H F e V I O 4 − + F e I I (O H) 2 (a q) + H 2 O → H 2 F e V O 4 − + F e I I I (O H) 3 (a q)$	~10⁷ M⁻¹·s⁻¹	Rai et al., 2018
(e)	$2 H 2 F e V O 4 − + 2 H 2 O + 2 H + → 2 F e I I I (O H) 3 (a q) + 2 H 2 O 2$	5.8 × 10⁷ M⁻¹·s⁻¹	Sharma, 2013
(f)	$H 2 F e V O 4 − + H 2 O 2 + H + → F e I I I (O H) 3 (a q) + O 2 + H 2 O 2$	5.6 × 10⁵ M⁻¹·s⁻¹	Wu et al., 2020

Tab.2 Major reactions of the self-decay of Fe(VI) in phosphate buffered solution at pH 7.0

Fig.3 Scheme 2 Schematic illustration of the self-decay of Fe(VI) at pH 7.0.

Fig.4 logk as a function of the standard one-electron reduction potential (E⁰₍₁₎) (a) and standard two-electron reduction potential (E⁰₍₂₎) (b) for the reaction of Fe(VI) with inorganic/organic substrates at 25°C.

Fig.5 Scheme 3 Schematic illustration of the mechanisms of phenol oxidation by Fe(VI).

Fig.6 Scheme 4 Schematic illustration of the mechanisms of aniline oxidation by Fe(VI).

Fig.7 Illustration of the formation of I-DBPs when NOM is oxidized by Fe(VI) in the presence of excess I⁻.

Fig.8 The important nodes in the development of the enhanced Fe(VI) oxidation/disinfection technologies in the past two decades.

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