Ferrates(FeVI, FeV, and FeIV) oxidation of iodide: Formation of triiodide
The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferr...
Ausführliche Beschreibung
Gespeichert in:
| Autor*in: |
Kralchevska, Radina P. [verfasserIn] |
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| Format: |
E-Artikel |
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| Sprache: |
Englisch |
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2016transfer abstract |
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| Umfang: |
6 |
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| Übergeordnetes Werk: |
Enthalten in: MPI vs Fortran coarrays beyond 100k cores: 3D cellular automata - Shterenlikht, Anton ELSEVIER, 2019, chemistry, biology and toxicology as related to environmental problems, Amsterdam [u.a.] |
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| Übergeordnetes Werk: |
volume:144 ; year:2016 ; pages:1156-1161 ; extent:6 |
| Links: |
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| DOI / URN: |
10.1016/j.chemosphere.2015.09.091 |
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ELV013584219 |
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| 245 | 1 | 0 | |a Ferrates(FeVI, FeV, and FeIV) oxidation of iodide: Formation of triiodide |
| 264 | 1 | |c 2016transfer abstract | |
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| 520 | |a The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. | ||
| 520 | |a The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. | ||
| 650 | 7 | |a Iodide |2 Elsevier | |
| 650 | 7 | |a Disinfection by-products |2 Elsevier | |
| 650 | 7 | |a Ferrate |2 Elsevier | |
| 650 | 7 | |a Oxidation |2 Elsevier | |
| 650 | 7 | |a Mechanism |2 Elsevier | |
| 700 | 1 | |a Sharma, Virender K. |4 oth | |
| 700 | 1 | |a Machala, Libor |4 oth | |
| 700 | 1 | |a Zboril, Radek |4 oth | |
| 773 | 0 | 8 | |i Enthalten in |n Elsevier Science |a Shterenlikht, Anton ELSEVIER |t MPI vs Fortran coarrays beyond 100k cores: 3D cellular automata |d 2019 |d chemistry, biology and toxicology as related to environmental problems |g Amsterdam [u.a.] |w (DE-627)ELV002112701 |
| 773 | 1 | 8 | |g volume:144 |g year:2016 |g pages:1156-1161 |g extent:6 |
| 856 | 4 | 0 | |u https://doi.org/10.1016/j.chemosphere.2015.09.091 |3 Volltext |
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10.1016/j.chemosphere.2015.09.091 doi GBVA2016001000008.pica (DE-627)ELV013584219 (ELSEVIER)S0045-6535(15)30179-X DE-627 ger DE-627 rakwb eng 333.7 333.7 DE-600 004 620 VZ 54.25 bkl Kralchevska, Radina P. verfasserin aut Ferrates(FeVI, FeV, and FeIV) oxidation of iodide: Formation of triiodide 2016transfer abstract 6 nicht spezifiziert zzz rdacontent nicht spezifiziert z rdamedia nicht spezifiziert zu rdacarrier The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. Iodide Elsevier Disinfection by-products Elsevier Ferrate Elsevier Oxidation Elsevier Mechanism Elsevier Sharma, Virender K. oth Machala, Libor oth Zboril, Radek oth Enthalten in Elsevier Science Shterenlikht, Anton ELSEVIER MPI vs Fortran coarrays beyond 100k cores: 3D cellular automata 2019 chemistry, biology and toxicology as related to environmental problems Amsterdam [u.a.] (DE-627)ELV002112701 volume:144 year:2016 pages:1156-1161 extent:6 https://doi.org/10.1016/j.chemosphere.2015.09.091 Volltext GBV_USEFLAG_U GBV_ELV SYSFLAG_U 54.25 Parallele Datenverarbeitung VZ AR 144 2016 1156-1161 6 045F 333.7 |
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10.1016/j.chemosphere.2015.09.091 doi GBVA2016001000008.pica (DE-627)ELV013584219 (ELSEVIER)S0045-6535(15)30179-X DE-627 ger DE-627 rakwb eng 333.7 333.7 DE-600 004 620 VZ 54.25 bkl Kralchevska, Radina P. verfasserin aut Ferrates(FeVI, FeV, and FeIV) oxidation of iodide: Formation of triiodide 2016transfer abstract 6 nicht spezifiziert zzz rdacontent nicht spezifiziert z rdamedia nicht spezifiziert zu rdacarrier The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. Iodide Elsevier Disinfection by-products Elsevier Ferrate Elsevier Oxidation Elsevier Mechanism Elsevier Sharma, Virender K. oth Machala, Libor oth Zboril, Radek oth Enthalten in Elsevier Science Shterenlikht, Anton ELSEVIER MPI vs Fortran coarrays beyond 100k cores: 3D cellular automata 2019 chemistry, biology and toxicology as related to environmental problems Amsterdam [u.a.] (DE-627)ELV002112701 volume:144 year:2016 pages:1156-1161 extent:6 https://doi.org/10.1016/j.chemosphere.2015.09.091 Volltext GBV_USEFLAG_U GBV_ELV SYSFLAG_U 54.25 Parallele Datenverarbeitung VZ AR 144 2016 1156-1161 6 045F 333.7 |
| allfields_unstemmed |
10.1016/j.chemosphere.2015.09.091 doi GBVA2016001000008.pica (DE-627)ELV013584219 (ELSEVIER)S0045-6535(15)30179-X DE-627 ger DE-627 rakwb eng 333.7 333.7 DE-600 004 620 VZ 54.25 bkl Kralchevska, Radina P. verfasserin aut Ferrates(FeVI, FeV, and FeIV) oxidation of iodide: Formation of triiodide 2016transfer abstract 6 nicht spezifiziert zzz rdacontent nicht spezifiziert z rdamedia nicht spezifiziert zu rdacarrier The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. Iodide Elsevier Disinfection by-products Elsevier Ferrate Elsevier Oxidation Elsevier Mechanism Elsevier Sharma, Virender K. oth Machala, Libor oth Zboril, Radek oth Enthalten in Elsevier Science Shterenlikht, Anton ELSEVIER MPI vs Fortran coarrays beyond 100k cores: 3D cellular automata 2019 chemistry, biology and toxicology as related to environmental problems Amsterdam [u.a.] (DE-627)ELV002112701 volume:144 year:2016 pages:1156-1161 extent:6 https://doi.org/10.1016/j.chemosphere.2015.09.091 Volltext GBV_USEFLAG_U GBV_ELV SYSFLAG_U 54.25 Parallele Datenverarbeitung VZ AR 144 2016 1156-1161 6 045F 333.7 |
| allfieldsGer |
10.1016/j.chemosphere.2015.09.091 doi GBVA2016001000008.pica (DE-627)ELV013584219 (ELSEVIER)S0045-6535(15)30179-X DE-627 ger DE-627 rakwb eng 333.7 333.7 DE-600 004 620 VZ 54.25 bkl Kralchevska, Radina P. verfasserin aut Ferrates(FeVI, FeV, and FeIV) oxidation of iodide: Formation of triiodide 2016transfer abstract 6 nicht spezifiziert zzz rdacontent nicht spezifiziert z rdamedia nicht spezifiziert zu rdacarrier The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. Iodide Elsevier Disinfection by-products Elsevier Ferrate Elsevier Oxidation Elsevier Mechanism Elsevier Sharma, Virender K. oth Machala, Libor oth Zboril, Radek oth Enthalten in Elsevier Science Shterenlikht, Anton ELSEVIER MPI vs Fortran coarrays beyond 100k cores: 3D cellular automata 2019 chemistry, biology and toxicology as related to environmental problems Amsterdam [u.a.] (DE-627)ELV002112701 volume:144 year:2016 pages:1156-1161 extent:6 https://doi.org/10.1016/j.chemosphere.2015.09.091 Volltext GBV_USEFLAG_U GBV_ELV SYSFLAG_U 54.25 Parallele Datenverarbeitung VZ AR 144 2016 1156-1161 6 045F 333.7 |
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10.1016/j.chemosphere.2015.09.091 doi GBVA2016001000008.pica (DE-627)ELV013584219 (ELSEVIER)S0045-6535(15)30179-X DE-627 ger DE-627 rakwb eng 333.7 333.7 DE-600 004 620 VZ 54.25 bkl Kralchevska, Radina P. verfasserin aut Ferrates(FeVI, FeV, and FeIV) oxidation of iodide: Formation of triiodide 2016transfer abstract 6 nicht spezifiziert zzz rdacontent nicht spezifiziert z rdamedia nicht spezifiziert zu rdacarrier The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. Iodide Elsevier Disinfection by-products Elsevier Ferrate Elsevier Oxidation Elsevier Mechanism Elsevier Sharma, Virender K. oth Machala, Libor oth Zboril, Radek oth Enthalten in Elsevier Science Shterenlikht, Anton ELSEVIER MPI vs Fortran coarrays beyond 100k cores: 3D cellular automata 2019 chemistry, biology and toxicology as related to environmental problems Amsterdam [u.a.] (DE-627)ELV002112701 volume:144 year:2016 pages:1156-1161 extent:6 https://doi.org/10.1016/j.chemosphere.2015.09.091 Volltext GBV_USEFLAG_U GBV_ELV SYSFLAG_U 54.25 Parallele Datenverarbeitung VZ AR 144 2016 1156-1161 6 045F 333.7 |
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ferrates(fevi, fev, and feiv) oxidation of iodide: formation of triiodide |
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Ferrates(FeVI, FeV, and FeIV) oxidation of iodide: Formation of triiodide |
| abstract |
The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. |
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The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. |
| abstract_unstemmed |
The presence of iodide (I−) in water during disinfection and oxidative treatment of water is a potential health concern because of the formation of iodinated disinfection by-products (DBPs), which may be more toxic than chlorinated DBPs. The kinetics of the oxidation of I− by a greener oxidant, ferrate(VI) ( Fe VI O 4 2 − , Fe(VI)) was determined as a function of pH. The second-order rate constants (k, M−1 s−1) decreased from 3.9 × 104 M−1 s−1 at pH 5.0 to 1.2 × 101 M−1 s−1 at pH 10.3. The kinetics results could be described by the reactivity of monoprotonated species of Fe(VI) ( HFe VI O 4 − ) with I−. In excess I− concentration, triiodide ( I 3 − ) was formed and the stoichiometry of ∼1:1 ([Fe(VI)]:[ I 3 − ]) was found in both acidic and basic pH. Ferrate(V) ( Fe V O 4 3 − , Fe(V)) and ferrate(IV) ( Fe VI O 4 4 − , Fe(IV)) also showed the formation of I 3 − in presence of excess I−. A mechanism of the formation of I 3 − is proposed, which is consistent with the observed stoichiometry of 1:1. The oxidative treatment of I− in water will be rapid (t 1/2 = 0.6 s at pH 7.0 using 10 mg L−1 K2FeO4). The implications of the results and their comparison with the oxidation of I− by conventional disinfectants/oxidants in water treatment are briefly discussed. |
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