Kinetics of Oxidation of Iodide (Iâ) and Hypoiodous Acid (HOI) by

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Letter -

Oxidation Kinetics of Iodide (I) and Hypoiodous Acid (HOI) by Peroxymonosulfate (PMS) and Formation of Iodinated Products in the PMS/I/NOM System -

Juan Li, Jin Jiang, Yang Zhou, Su-yan Pang, Yuan Gao, Chengchun Jiang, Jun Ma, Yi-xin Jin, Yi Yang, Guan-qi liu, Li-Hong Wang, and Chao-ting Guan Environ. Sci. Technol. Lett., Just Accepted Manuscript • DOI: 10.1021/acs.estlett.6b00471 • Publication Date (Web): 30 Dec 2016 Downloaded from http://pubs.acs.org on January 3, 2017

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Environmental Science & Technology Letters

Oxidation Kinetics of Iodide (I-) and

1 2

Hypoiodous Acid (HOI) by

3

Peroxymonosulfate (PMS) and Formation of

4

Iodinated Products in the PMS/I-/NOM

5

System Juan Li, † Jin Jiang, †, * Yang Zhou, †Su–Yan Pang, ‡ Yuan Gao, † Chengchun

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Jiang, §Jun Ma,† Yixin Jin,† Yi Yang, † Guanqi Liu, † Lihong Wang,† and

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Chaoting Guan†

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†

State Key Laboratory of Urban Water Resource and Environment, School of

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Municipal and Environmental Engineering, Harbin Institute of Technology, Harbin

11

150090, China

12

‡

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Heilongjiang Province, College of Chemical and Environmental Engineering, Harbin

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University of Science and Technology, Harbin 150040, China

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§

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518055, China

Key laboratory of Green Chemical Engineering and Technology of College of

School of Civil and Environmental Engineering, Shenzhen Polytechnic, Shenzhen

17 1

ACS Paragon Plus Environment


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* Corresponding

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Phone: 86−451−86283010; Fax: 86-451−86283010; E-mail: [email protected],

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[email protected]

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Abstract

author: Prof. Jin Jiang

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In this work, the transformation kinetics of iodide (I-) and hypoiodous acid (HOI) by

23

peroxymonosulfate (PMS) and potential formation of iodinated products of concerns

24

in the presence of natural organic matters (NOM) were investigated. As pH increased

25

from 5 to 10, the apparent second-order rate constants of PMS reaction with I- gradually

26

decreased from 1.01×103 to 3.86×102M-1s-1, while those for HOI increased

27

dramatically from 1.08 ×102 to 7.90×104M-1s-1. The obtained pH-dependent rate

28

profiles were well explained by the effects of pH-affected speciation of PMS and/or

29

HOI. Considerable amounts of total organic iodine (TOI) could be formed in the PMS/I-

30

/NOM system over a wide pH range. Under similar conditions, the TOI levels formed

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in the PMS/I-/NOM system were generally higher than those formed in the case of

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HOCl but much lower than those formed in the case of NH2Cl. Also, specific iodoform

33

(IF) and monoiodoacetic acid (MIAA) were detected in both simulated and authentic

34

waters during treatment with PMS. This work for the first time demonstrates the

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potential formation of iodinated products of concerns during water treatment with PMS

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and thus has important implications on its applications.

37 38

Introduction 2


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Iodide (I-) exists ubiquitously in natural environments (water, soil, and minerals)1, 2.

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The concentrations of I- in surface waters are usually less than 100µg/L. Occasionally,

41

high levels of I- (up to few mg/L) are found in coastal water and hydraulic fracturing

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contaminated water.3-5 I- can be easily oxidized to hypoiodous acid (HOI) by natural

43

microorganism6 and metal oxides,7-9 as well as by water treatment oxidants such as

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chlorine (HOCl),10,

45

(KMnO4)17. The formed HOI usually undergoes three competition pathways: (i) further

46

oxidation to nontoxic IO3-, a safe sink of iodine; (ii) reaction with background natural

47

organic matters (NOM) to form toxic iodinated products; and (iii) disproportionation

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into I- and iodate (IO3-). The relative contribution of reactions (i) - (iii) plays a decisive

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role in the final fate of iodine.

11

chloramine (NH2Cl),12,

13

ozone(O3),14-16 and permanganate

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Peroxymonosulfate (PMS), as a relatively stable and inexpensive oxidant, shows great

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potentials for applications in water treatment and subsurface remediation.18-21 Also,

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PMS is sometimes used as a broad-spectrum disinfectant in swimming pool and

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aquaculture disinfection.22-25 For instance, Wang et al.18 reported that PMS displayed

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high efficiency for the oxidative remediation of arsenite (As(III)) to form As(V), which

55

greatly decreased As(III) toxicity and mobility. Yang et.al.19 found that PMS could

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effectively remove sulfur-containing odor compound mercaptan in wet scrubbing

57

process. Very recently, Chesney and co-workers26 demonstrated that PMS could rapidly

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inactivate the disease-associated pathogenic prion protein contaminated land surfaces

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by an oxidative modification to the amino acid residuals of the peptide fragments. 3



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However, there is only limited information about halogen transformation during PMS

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oxidation/disinfection. Earlier studies have demonstrated that PMS is able to oxidize

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Cl-, Br-, and I- to form reactive halogen species HOX (i.e., HOCl, HOBr, and HOI)

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with second order reaction rate constants kx- decreasing in the order of kI- (1400

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~1730M-1s-1) > kBr- (0.7~1.0M-1s-1) > kCl- (0.0021~0.0018M-1s-1).27-29 The further

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oxidation of HOCl and HOBr by PMS were negligible28, while the reaction of HOI

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with PMS has not yet been investigated. The rapid transformation of I- to HOI by PMS

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indicates the potential risk of the formation of iodinated products, whose toxicity are

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generally several to hundreds of times more genotoxic and cytotoxic than their

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chlorinated and brominated analogues.30-32 This issue, however, has not been addressed

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so far.

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The objectives of this study were (i) to investigate the oxidation kinetics of I- and HOI

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by PMS over a wide pH range (5~10), and (ii) to evaluate the formation of iodinated

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products (including total organic iodine (TOI), iodoform (IF), and monoiodoacetic acid

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(MIAA)) during water treatment with PMS, as compared to HOCl and NH2Cl.

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Materials and Methods.

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Materials. PMS (available as Oxone), NaClO (4% active chlorine), phenol, 2-

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iodophenol, and 4-iodophenol were purchased from Sigma-Aldrich. KI, KIO3, and

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ammonium chloride (NH4Cl) were purchased from Sinopharm Chemical Reagent Co.

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Ltd., China. IF (99%) and MIAA (97%) were purchased form J & K Scientific Ltd.,

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China. Suwannee river humic acid (SRHA, 2S101H) and Suwannee river fulvic acid 4


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(SRFA, 1S101F) were purchased from International Humic Substance Society (IHSS).

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Another humic acid was purchased from Sigma-Aldrich (Sigma HA) and purified

83

following the procedure as previously described.33 All other reagents were of analytical

84

grade or better and used without further purification. All solutions were prepared using

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deionized (DI) water (18.2 MΩ/cm) from a Milli-Q purification system (Millipore,

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Billerica, MA). Stock solutions of oxidants (i.e., PMS, HOCl, and NH2Cl) were

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prepared and standardized as described in SI Text S1.

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Reaction kinetics. Reaction kinetics of PMS with I- were investigated by a stopped-

89

flow spectrophotometer under pseudo-first-order conditions with I- in excess in the pH

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range of 5~10. Details can be found in SI Text S2.

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Batch reactions for PMS with HOI were initiated by adding excess PMS into pH-

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buffered solutions containing freshly prepared HOI (stoichiometric oxidation of I- by

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OCl-) in the pH range of 5~8. Samples were periodically collected and quenched by

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phenol in excess to trap the unreacted HOI,34 and thereafter As(III)

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quench the residual PMS in the samples before analysis for iodophenols, I-, and IO3-.

96

(see SI Text S3 for the details). For pH 9~10, a sequential-mixing stopped-flow

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technique (see SI Text S4 for the details) was used since the reaction was too fast to be

98

followed by manual operation.

18

was added to

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Formation of iodinated products. The experiments for the formation of iodinated

100

products were conducted in 250mL amber glass bottles and the headspace free

101

conditions were kept. Pre-determined amounts of oxidant (PMS, HOCl, or NH2Cl) 5



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were added into pH-buffered solutions containing I- and NOM representative to initiate

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the reactions. Samples were withdrawn after 24h reaction for the determination of

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iodine species (i.e., I-, HOI, IO3-, TOI, IF, and MIAA) (See SI Text S5 for the details).

105

Natural water taken from Songhua river, Harbin, China (DOC = 6.2mg·C/L, alkalinity

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= 1.3mM as HCO3-, and pH =7.3) was stored at 4°C and used within two days after

107

vacuum-filtered through 0.45µM cellulose membrane filter. A similar procedure to that

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used in simulated water was followed with the exception that I- at an environmentally

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relevant level (i.e., 0.5µM) was spiked. Samples were withdrawn after 24h reaction for

110

the determination of IF and MIAA.

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All experiments were conducted at 23  2°C in duplicates or triplicates and the

112

average data with their standard deviations were displayed. Phosphate buffer (2mM)

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and borate buffer (2mM) were used for pH 5~7 and pH 8~10, respectively.

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Analytical

methods.

A stopped-flow

spectrophotometer

(SX20,

Applied

115

Photophysics Ltd.) equipped with a photomultiplier tube (PMT) detector and a

116

sequential-mixing accessory was used to carry out the fast kinetics. Iodophenols were

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analyzed by HPLC (details can be found in SI Text S6). I- and IO3- were determined by

118

ion chromatography (IC, Thermo Dionex ICS-3000) (see SI Text S6 for the details). IF

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and MIAA were determined by liquid/liquid extraction with methyl-tert-butyl ether

120

(MtBE) without/with acidic methanol derivation followed by gas chromatography and

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electron capture detection (GC/ECD, GC-6890 Agilent) according to EPA Method

122

551.1 and 552.2., respectively. TOI was measured by a Multi 2500 TOX analyzer (Jena) 6


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via an adsorption-pyrolysis-titration method (see SI Text S7 for the details).

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Results and Discussion

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Reaction Kinetics of PMS with I-. The reaction of PMS with I- was determined to be

126

first-order with respect to each reactant (see SI Figure S1). The obtained apparent

127

second-order rate constants ( kI- , PMS ) as a function of pH were shown in Figure 1a. As

128

can be seen, PMS exhibited considerable reactivity towards I- with kI- , PMS decreasing

129

from 1013(±89) to 386 (±13) M-1s-1 as pH increased from 5 to 10. This pH dependence

130

of kI- , PMS can be well explained by the reactions between pH-affected species of PMS

131

(HSO5- and SO52; pKa=9.30) and I- (solid line in Figure 1a). The species-specific rate

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constants calculated by nonlinear least-squares regression of experimental data were

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k I- +HSO - = 1112 (±29) M-1s-1 and k I- +SO 2- =218 (±73) M-1s-1, respectively, and they 5 5

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well matched the results given by Secco27 and Lente28. Contributions of individual

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reactions of HSO5- and SO52- with I- to the overall reaction rate were calculated and

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shown in Figure 1a (dashed and dot-dashed lines). Moreover, a comparison of pH-

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dependent apparent second-order rate constants ( kI- ) for the reactions between I- and

138

various oxidants [PMS, HOCl, KMnO4, O3, and NH2Cl] was made. As shown in Figure

139

1b, PMS displayed a mild reactivity with I- compared to other oxidants.

140

Figure 1

141

Reaction Kinetics of PMS with HOI. The kinetics of PMS reaction with HOI were

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further investigated in the pH range of 5~10. Disappearance of HOI in the presence of

143

excess PMS followed the pseudo-first-order rate law (see SI Figure S3), confirming 7



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that the reaction was first-order with respect to HOI. Pseudo-first-order rate constants

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(kobs, s-1) determined at various concentrations of PMS at a constant pH showed a

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linearity (SI Figure S4, for example), demonstrating that the reaction was also first-

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order with respect to PMS. Measured apparent second-order rate constants ( kHOI,PMS ,

148

M-1s-1) as a function of pH were summarized in Figure 2a.

149

Figure 2

150

The kHOI,PMS values showed a strong pH dependence with increasing more than 2

151

orders of magnitude from pH 5 to 10. This pH dependence can be quantitatively

152

described by the parallel reactions between individual acid-base species of HOI

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(pKa=10.43) and PMS (pKa=9.30), as shown by reactions (1~8) (where reactions (3~6)

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are rate-determining35):

155 156

HSO 5  SO52  H +

pK a  9.30

(1)

HOI  OI  H +

pK a  10.43

(2)

HSO5 +HOI  IO2  SO42  2H +

kHOI-1,1

(3)

HSO5 +OI  IO2  SO42  H+

kHOI-1,2

(4)

SO52 +HOI  IO2  SO24  H +

kHOI-2,1

(5)

SO52 +OI  IO2  SO42

kHOI-2,2

(6)

HSO5 +IO2  IO3  SO24 +H+

fast

(7)

SO52 +IO2  IO3  SO42

fast

(8)

Accordingly, kHOI,PMS is given by

kHOI, PMS = j1,2 kHOI-i,j i  j i=1,2

(9) 8


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i

 j represent the respective fractions of PMS and HOI as the species

157

where

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i and j at a given pH, and kHOI-i,j represents the species-specific second-order rate

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constant for each i and j pair. The kHOI-i,j values determined by nonlinear least-

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squares regression of experimental data ( kHOI,PMS ) were kHOI-1,1 = 112( ±18), kHOI-1,2

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= 1.7(±0.16) ×106, kHOI-2,1 = ~0, and kHOI-2,2 = 1.5(±0.74) ×105M1s-1, respectively.

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Accordingly, the contribution of each reaction (i.e., reactions 3~6) to the overall

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reaction rate was calculated (Figure 2a, dashed lines). As can be seen, the reaction

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between HSO5- and HOI dominates at lower pH (pH7).

and

166

A comparison of the pH-dependent apparent second-order rate constants ( kHOI ) for

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the reactions between HOI and selective oxidants [PMS, HOCl, KMnO4, O3, and

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NH2Cl] was also made. As shown in Figure 2b, PMS displayed high reactivity towards

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HOI compared to HOCl, NH2Cl, and KMnO4.

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Interestingly, it was found that the oxidation rates of HOI to IO3- by PMS (Figure 2a)

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at pH>8 were even faster than those of I- to HOI by PMS (Figure 1a). The exact reasons

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for the unexpectedly high reactivity of PMS with HOI are unclear so far, which

173

deserves further investigations. Previous studies have reported that PMS can undergo

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self-decomposition especially at alkaline pH, where reactive oxygen species (ROS)

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such as singlet oxygen (1O2) is generated.

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scavengers such as furfuryl alcohol (for 1O2) and methanol (for sulfate radical, SO4.-)

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on the oxidation kinetics of HOI by PMS was observed (data not shown). Either

36, 37

However, no influence of specific

9



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negligible decomposition of PMS was observed in control experiments without HOI

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within the time scales investigated.

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Evolution of IO3- during oxidation of HOI by PMS in the pH range of 5~10 was also

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investigated and the results were shown in SI Figure S5. As can be seen, a good mass

182

balance (i.e., [HOI] + [IO3-]) was maintained during the kinetic runs, indicating that

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IO3- was the unique product for HOI oxidation by PMS.

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Stoichiometry. Stoichiometries for the reaction of PMS with I- were further evaluated.

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As shown in SI Table S1, the amounts of PMS consumed (Δ[PMS]) were

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approximately 3 times of the amounts of IO3- formed (Δ[IO3-]) (Δ[PMS]/Δ[IO3-]=3),

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which was consistent with the theoretical value according to eq 10.

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3HSO5- + I-  IO3  3SO24  3H+

(10)

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Formation of iodinated products in the presence of NOM.

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(i) PMS. Figure 3a comparatively displayed the TOI formation from three NOM

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representatives (Sigma HA, SRHA, and SRFA) in the presence of PMS and I- at pH 5,

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7, and 9. For all the tested NOM representatives, the TOI levels showed obvious

193

dependence on pH and decreased with the increase of pH. This result can be well

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explained by the pH-affected oxidation rates of HOI formed in situ by PMS. At

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investigated pH (5, 7, and 9), I- was oxidized to HOI by PMS with comparable rate

196

constants (Figure 1a), while the oxidation rates of HOI to IO3- by PMS increased more

197

than 2 orders of magnitude from pH 5 to 9 (Figure 2a). Accordingly, a higher HOI

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exposure was available at lower pH, leading to the observed higher TOI level. 10


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Meanwhile, considerable amounts of IF (4.5 ~ 25nM) and MIAA (27 ~ 65nM) were

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also detected during treatment with PMS in the presence of I- and NOM representative

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(Figure 3b). The total iodine that incorporated in IF and MIAA (i.e., 3×[IF]+[MIAA])

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accounted for a small fraction (PMS>HOCl at 11



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pH 5 and 7, while it changed to NH2Cl>HOCl>PMS at pH 9 for each NOM

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representative. The trend obtained at pH 5 and 7 was somewhat unexpected, since PMS

222

exhibited a much higher reactivity towards HOI than HOCl therein (Figure 2b). This

223

finding probably resulted from the competitive reaction of HOCl in high concentrations

224

vs HOI in low concentrations towards reactive sites in NOM, although HOCl might be

225

less reactive toward NOM than HOI.38, 39 The oxidant demands in the case of HOCl

226

were much higher than those obtained in the case of PMS for each NOM representative

227

(SI Figure S7). Allard and co-workers40 also reported a similar competition effect of

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HOCl for reactive sites of NOM, which decreased the TOI formation from chlorination

229

of UV-irradiated iopamidol in the presence of NOM. It seemed likely that this

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competition effect of HOCl was weakened at pH 9 due to its deprotonation into OCl-

231

(pKa=7.54). Another possible explanation might involve the exchange of iodine from

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the already formed iodinated products by chlorine from HOCl (i.e., the transformation

233

of TOI to TOCl) via the ipso free-radical substitution process.41-43 Recently, Wendel et

234

al.44 proposed that this chlorine-iodine exchange process resulted in the formation of

235

chlorinated products during chlorination of iopamidol. Zhu and Zhang45 reported that

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the transformation of TOI to TOCl in the presence of chlorine residue via chlorine-

237

iodine exchange consumed ~15% of the TOI initially formed.

238

The formation of IF and MIAA during treatment with PMS vs HOCl/NH2Cl was

239

further investigated (Figure 4b). As shown, IF was predominantly formed in the case

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of NH2Cl, while MIAA was preferentially formed in the case of HOCl. Both IF and 12


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MIAA were moderately formed during treatment with PMS. The higher IF

242

concentrations obtained in the case of NH2Cl was in agreement with the higher HOI

243

exposures therein that enabled triple iodination to IF.46

244

Meanwhile, differences in TOI levels were also observed among three NOM

245

representatives for each oxidant under similar conditions. The aromatic moiety

246

contents in NOM (i.e., SUVA, specific UV absorbance at 254nm, expressed in L·mgC-

247

1

248

disinfection byproducts during treatment with HOCl or NH2Cl.47-50 In light of this, the

249

relationship between the levels of iodinated products (i.e., TOI/IF/MIAA) and SUVA

250

values of selected NOM representatives (SI Table S2) for each oxidant was further

251

examined, but no obvious correlation was found (data not shown). This observation

252

was probably resulted from the different reaction pathways between NOM and HOI vs

253

HOCl/NH2Cl and/or the transformation of iodinated products to their chlorinated

254

analogues in the presence of residual HOCl as discussed above. Zhu and Zhang45

255

reported that the majority of TOCl (77.5 ~ 84.7%) were resulted from the reactions

256

between HOCl and NOMslow (i.e., slow reaction sites in NOM), whereas only 2.2 ~ 22.8%

257

of the TOI came from the reaction of HOI and NOMslow during chlorination of NOM

258

in the presence of I-.

·m-1) always have good correlations with the formation potentials of chlorinated

259

In addition, as shown in Figure 4a, considerable amounts of HOI were detected in the

260

case of NH2Cl. This was due to the much slower oxidation rates of HOI by NH2Cl vs

261

HOCl and PMS. Interestingly, the occurrence of I- and IO3- were also observed in the 13



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case of NH2Cl, which was somewhat unexpected according to the kinetic rate constants

263

of I- and HOI with NH2Cl (Figure 1b and Figure 2b). This finding was explained by

264

the contributions of side reactions including (i) the disproportionation of HOI51-53; (ii)

265

the reduction of HOI back to I- by NOM (i.e., oxidation pathway for the reaction of

266

HOI with NOM other than substitution pathway)34, 54; and (iii) further oxidation of HOI

267

by HOCl in situ formed from the slow hydrolysis of NH2Cl55-57.

268

Formation of iodinated products from authentic water. Figure 5 comparatively

269

showed the formation of IF and MIAA from natural water containing 0.5µM I- treated

270

by HOCl, NH2Cl, and PMS (15μM). As can be seen, IF at concentration of ~1.5nM

271

was formed during treatment with PMS, which was much lower than those formed in

272

the cases of HOCl and NH2Cl (i.e., 4.0nM and 10.5nM, respectively). MIAA formed

273

during treatment with PMS (~7.6nM) was comparable to that formed in the case of

274

NH2Cl (~10nM) but much lower than that formed in the case of HOCl (~21nM).

275

Figure 5

276

To the best of our knowledge, this work for the first time examines the oxidation

277

kinetics of I- and HOI by PMS and demonstrates the potential formation of iodinated

278

products in the PMS/I-/NOM system. The formation of IF and MIAA from natural

279

water containing I- treated by PMS has been confirmed. These results have important

280

implications for the future applications of PMS-based oxidation/disinfection processes.

281

Acknowledgment

282

This work was financially supported by the National Natural Science Foundation of 14


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283

China (51578203&51378316), the National Key Research and Development Program

284

(2016YFC0401107), the Chinese Postdoctoral Science Foundation (2015T80366), the

285

Funds of the State Key Laboratory of Urban Water Resource and Environment (HIT,

286

2016DX13), the Foundation for the Author of National Excellent Doctoral Dissertation

287

of China (201346), Heilongjiang Province Natural Science Foundation (QC2014C055),

288

and the Fundamental Research Funds for the Central Universities of China.

289

Supporting Information

290

The additional texts, figures, and tables addressing supporting data. This material is

291

available free of charge via the Internet at http://pubs.acs.org.

292

References

293

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23



-

10

9

10

7

10

5

10

3

10

1

-1 -1

kI (M s )

-1 -1

kI ,PMS ( M s )

-

600 measured data model fit

300

(b) O3

10

900

PMS KMnO4

10 5

6

7

8

9

10

HOCl

NH2Cl

-1

0

458

11

(a)

1200

Page 24 of 28

5

6

pH

7

8

9

10

pH

459

FIGURE 1. (a) pH-dependent second-order rate constants ( kI- , PMS , M−1s−1) for

460

the reaction of PMS with I-. Symbols represent measured data and the lines

461

indicate the model prediction and contribution of individual reactions of HSO 5-

462

with I- (dashed) and SO52- with I- (dot dashed) to the overall reaction as a function

463

of pH. (b) Comparison of the pH-dependent apparent second-order rate constants

464

for the reactions of selective oxidants with I- ( kI-, M-1s-1).The kI- values for HOCl

465

were obtained from ref 10, for O3 obtained from ref 16, for KMnO4 from ref 17,

466

and for NH2Cl from ref 12.

467 468

24


Page 25 of 28


5

7

10

2

HO

I-2 ,2







10

3

10

469

5

-1 -1

10

 

1

k HO

,2 I-1

5

6

kHOI-1,1

7

(b) O3

10

model fit

k

-1 -1

kHOI,PMS( M s )

measured data 4

10

(a)

kHOI ( M s )

10

8

9

3

10

PMS

1

10

10

-1

10

-3

10

HOCl

KMnO4 NH2Cl

5

6

pH

7

8

9

10

pH

470

FIGURE 2. (a) pH-dependent second-order rate constants (kHOI,PMS, M−1s−1) for

471

the reaction of PMS with HOI. The symbols represent measured data and the

472

lines indicate the model prediction with eq 9 (solid) and contribution of individual

473

reactions of HSO5- with HOI (kHOI-1,1α1β1, dot dashed), HSO5- with OI- (kHOI-1,2α1β2,

474

dot-dot dashed), and SO52- with OI- (kHOI-2,2α2β2, short dashed) to the overall

475

reaction as a function of pH. (b) Comparison of the pH-dependent second-order

476

rate constants for the reactions of selective oxidants with HOI (kHOI, M-1s-1). The

477

kHOI values for HOCl, O3, and NH2Cl were obtained from ref 35 (the third-order

478

reaction was not considered in the case of HOCl, and the maximum species-

479

specific rate constants estimated in ref 35 were used to calculate the kHOI values in

480

the case of NH2Cl), and for KMnO4 from ref 17.

481 482 483 484 485 486 487 25



TOI

IO3

-

(a)

10 8 6 4 2 0

pH 5

IF

Iodinated products (nM)

Iodinated products (M)

12

Page 26 of 28

MIAA

(b)

80

60

40

20

0

7

9

NOM Sigma HA

5

7

9

SRHA

5

7 SRFA

9

pH 5

7

9

NOM Sigma HA

5

7

9

SRHA

5

7

9

SRFA

488 489

FIGURE 3. Formation of iodinated products from I- oxidation by PMS in the

490

presence of NOM. (a) TOI and IO3-; (b) IF and MIAA. Experimental conditions:

491

[I-] = 10μM, [PMS] = 100μM, [Sigma HA] = [SRHA] = [SRFA] = 4mg·C/L, and

492

reaction time t = 24h.

493 494 495 496 497 498 499 500 501 502

26


Page 27 of 28


Iodinated products (M)

12

TOI

HOI

-

-

I

IO3

(a)

10 8 6 4 2 0

pH 5 7 9 5 7 9 5 7 9 Oxidant Oxi-1 Oxi-2 Oxi-3 NOM Sigma HA

503

5 7 9 5 7 9 5 79

5 7 9 5 79 5 7 9

Oxi-1 Oxi-2 Oxi-3 SRHA

Oxi-1 Oxi-2 Oxi-3 SRFA

500 IF

MIAA

(b)

Iodinated products(nM)

400

300

200

100

0 pH 5 7 9 5 7 9 5 7 9 Oxidant Oxi-1 Oxi-2 Oxi-3 NOM Sigma HA

504

5 7 9 5 7 9 5 79

5 7 9 5 79 5 7 9

Oxi-1 Oxi-2 Oxi-3 SRHA

Oxi-1 Oxi-2 Oxi-3 SRFA

505

FIGURE 4. Comparison of iodinated products formed from I- oxidation by NH2Cl

506

(Oxi-1), HOCl (Oxi-2), or PMS (Oxi-3) in the presence of NOM. (a) TOI and IO3-;

507

(b) IF and MIAA. Experimental conditions: [I-] = 10μM, [NH2Cl] = [HOCl] =

508

[PMS] = 100μM, [sigma HA] = [SRHA] = [SRFA] = 4mg·C/L, and reaction time

509

t= 24 h.

510 511 512 27



Page 28 of 28

25 MIAA

IF

Iodinated products (nM)

20 15

10 5 0 NH2Cl

HOCl

513

PMS

514

FIGURE 5. Formation of IF and MIAA from I- spiked natural water treated by

515

HOCl, NH2Cl, and PMS. Experimental conditions: [I-] = 0.5μM, [HOCl] = [NH2Cl]

516

= [PMS] = 15μM, DOC = 6.2mg·C/L, alkalinity = 1.3mM as HCO3-, pH=7.3, and

517

reaction time t= 24h.

518 519 520 521 522 523

TOC Art

NOM

HOI

TOI

IO3-

IPMS

28


Kinetics of Oxidation of Iodide (Iâ) and Hypoiodous Acid (HOI) by

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