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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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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
6 7
Jiang, §Jun Ma,† Yixin Jin,† Yi Yang, † Guanqi Liu, † Lihong Wang,† and
8
Chaoting Guan†
9
†
State Key Laboratory of Urban Water Resource and Environment, School of
10
Municipal and Environmental Engineering, Harbin Institute of Technology, Harbin
11
150090, China
12
‡
13
Heilongjiang Province, College of Chemical and Environmental Engineering, Harbin
14
University of Science and Technology, Harbin 150040, China
15
§
16
518055, China
Key laboratory of Green Chemical Engineering and Technology of College of
School of Civil and Environmental Engineering, Shenzhen Polytechnic, Shenzhen
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* Corresponding
19
Phone: 86−451−86283010; Fax: 86-451−86283010; E-mail:
[email protected],
20
[email protected] 21
Abstract
author: Prof. Jin Jiang
22
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
31
in the PMS/I-/NOM system were generally higher than those formed in the case of
32
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
35
potential formation of iodinated products of concerns during water treatment with PMS
36
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.
40
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
42
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
44
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
48
into I- and iodate (IO3-). The relative contribution of reactions (i) - (iii) plays a decisive
49
role in the final fate of iodine.
11
chloramine (NH2Cl),12,
13
ozone(O3),14-16 and permanganate
50
Peroxymonosulfate (PMS), as a relatively stable and inexpensive oxidant, shows great
51
potentials for applications in water treatment and subsurface remediation.18-21 Also,
52
PMS is sometimes used as a broad-spectrum disinfectant in swimming pool and
53
aquaculture disinfection.22-25 For instance, Wang et al.18 reported that PMS displayed
54
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
56
effectively remove sulfur-containing odor compound mercaptan in wet scrubbing
57
process. Very recently, Chesney and co-workers26 demonstrated that PMS could rapidly
58
inactivate the disease-associated pathogenic prion protein contaminated land surfaces
59
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
62
Cl-, Br-, and I- to form reactive halogen species HOX (i.e., HOCl, HOBr, and HOI)
63
with second order reaction rate constants kx- decreasing in the order of kI- (1400
64
~1730M-1s-1) > kBr- (0.7~1.0M-1s-1) > kCl- (0.0021~0.0018M-1s-1).27-29 The further
65
oxidation of HOCl and HOBr by PMS were negligible28, while the reaction of HOI
66
with PMS has not yet been investigated. The rapid transformation of I- to HOI by PMS
67
indicates the potential risk of the formation of iodinated products, whose toxicity are
68
generally several to hundreds of times more genotoxic and cytotoxic than their
69
chlorinated and brominated analogues.30-32 This issue, however, has not been addressed
70
so far.
71
The objectives of this study were (i) to investigate the oxidation kinetics of I- and HOI
72
by PMS over a wide pH range (5~10), and (ii) to evaluate the formation of iodinated
73
products (including total organic iodine (TOI), iodoform (IF), and monoiodoacetic acid
74
(MIAA)) during water treatment with PMS, as compared to HOCl and NH2Cl.
75
Materials and Methods.
76
Materials. PMS (available as Oxone), NaClO (4% active chlorine), phenol, 2-
77
iodophenol, and 4-iodophenol were purchased from Sigma-Aldrich. KI, KIO3, and
78
ammonium chloride (NH4Cl) were purchased from Sinopharm Chemical Reagent Co.
79
Ltd., China. IF (99%) and MIAA (97%) were purchased form J & K Scientific Ltd.,
80
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
85
deionized (DI) water (18.2 MΩ/cm) from a Milli-Q purification system (Millipore,
86
Billerica, MA). Stock solutions of oxidants (i.e., PMS, HOCl, and NH2Cl) were
87
prepared and standardized as described in SI Text S1.
88
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
90
range of 5~10. Details can be found in SI Text S2.
91
Batch reactions for PMS with HOI were initiated by adding excess PMS into pH-
92
buffered solutions containing freshly prepared HOI (stoichiometric oxidation of I- by
93
OCl-) in the pH range of 5~8. Samples were periodically collected and quenched by
94
phenol in excess to trap the unreacted HOI,34 and thereafter As(III)
95
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
97
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
99
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
103
the reactions. Samples were withdrawn after 24h reaction for the determination of
104
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
106
= 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
108
used in simulated water was followed with the exception that I- at an environmentally
109
relevant level (i.e., 0.5µM) was spiked. Samples were withdrawn after 24h reaction for
110
the determination of IF and MIAA.
111
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)
113
and borate buffer (2mM) were used for pH 5~7 and pH 8~10, respectively.
114
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
117
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
119
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
121
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
125
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
132
constants calculated by nonlinear least-squares regression of experimental data were
133
k I- +HSO - = 1112 (±29) M-1s-1 and k I- +SO 2- =218 (±73) M-1s-1, respectively, and they 5 5
134
well matched the results given by Secco27 and Lente28. Contributions of individual
135
reactions of HSO5- and SO52- with I- to the overall reaction rate were calculated and
136
shown in Figure 1a (dashed and dot-dashed lines). Moreover, a comparison of pH-
137
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
142
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
145
(kobs, s-1) determined at various concentrations of PMS at a constant pH showed a
146
linearity (SI Figure S4, for example), demonstrating that the reaction was also first-
147
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
153
(pKa=10.43) and PMS (pKa=9.30), as shown by reactions (1~8) (where reactions (3~6)
154
are rate-determining35):
155 156
HSO 5 SO52 H +
pK a 9.30
(1)
HOI OI H +
pK a 10.43
(2)
HSO5 +HOI IO2 SO42 2H +
kHOI-1,1
(3)
HSO5 +OI IO2 SO42 H+
kHOI-1,2
(4)
SO52 +HOI IO2 SO24 H +
kHOI-2,1
(5)
SO52 +OI IO2 SO42
kHOI-2,2
(6)
HSO5 +IO2 IO3 SO24 +H+
fast
(7)
SO52 +IO2 IO3 SO42
fast
(8)
Accordingly, kHOI,PMS is given by
kHOI, PMS = j1,2 kHOI-i,j i j i=1,2
(9) 8
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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
159
constant for each i and j pair. The kHOI-i,j values determined by nonlinear least-
160
squares regression of experimental data ( kHOI,PMS ) were kHOI-1,1 = 112( ±18), kHOI-1,2
161
= 1.7(±0.16) ×106, kHOI-2,1 = ~0, and kHOI-2,2 = 1.5(±0.74) ×105M1s-1, respectively.
162
Accordingly, the contribution of each reaction (i.e., reactions 3~6) to the overall
163
reaction rate was calculated (Figure 2a, dashed lines). As can be seen, the reaction
164
between HSO5- and HOI dominates at lower pH (pH7).
and
166
A comparison of the pH-dependent apparent second-order rate constants ( kHOI ) for
167
the reactions between HOI and selective oxidants [PMS, HOCl, KMnO4, O3, and
168
NH2Cl] was also made. As shown in Figure 2b, PMS displayed high reactivity towards
169
HOI compared to HOCl, NH2Cl, and KMnO4.
170
Interestingly, it was found that the oxidation rates of HOI to IO3- by PMS (Figure 2a)
171
at pH>8 were even faster than those of I- to HOI by PMS (Figure 1a). The exact reasons
172
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
174
self-decomposition especially at alkaline pH, where reactive oxygen species (ROS)
175
such as singlet oxygen (1O2) is generated.
176
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
181
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
183
IO3- was the unique product for HOI oxidation by PMS.
184
Stoichiometry. Stoichiometries for the reaction of PMS with I- were further evaluated.
185
As shown in SI Table S1, the amounts of PMS consumed (Δ[PMS]) were
186
approximately 3 times of the amounts of IO3- formed (Δ[IO3-]) (Δ[PMS]/Δ[IO3-]=3),
187
which was consistent with the theoretical value according to eq 10.
188
3HSO5- + I- IO3 3SO24 3H+
(10)
189
Formation of iodinated products in the presence of NOM.
190
(i) PMS. Figure 3a comparatively displayed the TOI formation from three NOM
191
representatives (Sigma HA, SRHA, and SRFA) in the presence of PMS and I- at pH 5,
192
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
194
explained by the pH-affected oxidation rates of HOI formed in situ by PMS. At
195
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
198
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
200
also detected during treatment with PMS in the presence of I- and NOM representative
201
(Figure 3b). The total iodine that incorporated in IF and MIAA (i.e., 3×[IF]+[MIAA])
202
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
221
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
228
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
230
competition effect of HOCl was weakened at pH 9 due to its deprotonation into OCl-
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(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
236
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
240
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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China (51578203&51378316), the National Key Research and Development Program
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(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
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44. Wendel, F. M.; Lütke Eversloh, C.; Machek, E. J.; Duirk, S. E.; Plewa, M. J.;
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Richardson, S. D.; Ternes, T. A., Transformation of iopamidol during chlorination.
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-
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
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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
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Environmental Science & Technology Letters
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
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Environmental Science & Technology Letters
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
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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
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