DOCSLIB.ORG

Supporting Information 3 Uv

Total Page：16

File Type：pdf, Size：1020Kb

Download full-text PDF Read full-text
Supporting Information 3 Uv Electronic Supplementary Material (ESI) for Environmental Science: Water Research & Technology. This journal is © The Royal Society of Chemistry 2020 1 SUPPORTING INFORMATION 2 3 UV/Chlorine vs. UV/H2O2 for water reuse at Orange County Water 4 District, CA: A pilot study 5 Minhwan Kwon†,‡, Alan Royce†, Ying Gong†, Kenneth P. Ishida§, Mihaela I. Stefan*,† 6 7 † Trojan Technologies, 3020 Gore Road, London, ON, N5V 4T7, Canada 8 ‡Department of Chemical and Biochemical Engineering, University of Western Ontario, London, 9 ON, N6A 5B9, Canada 10 §Research and Development Department, Orange County Water District, 18700 Ward Street, 11 Fountain Valley, CA 92708, USA 12 * Corresponding author (Email: [email protected]; Phone: +1-519-457-3400) 13 14 Table S1. Selected elementary reactions considered in the kinetic model No. Reaction Rate constant = 371 M−1 cm−1 1 1 NH Cl + hν → NH • + Cl• 2 2 = 0.294 2 = 126 M−1 cm−1 1 2 NHCl + hν → NHCl• + Cl• 2 = 0.82 1 = 58 M−1 cm−1 2 3 HOCl + hν → •OH + Cl• = 0.55 3 = 19.6 M−1 cm−1 4 4 H O + hν → 2•OH 2 2 = 0.5 4 5.2 × 108 M−1 s−1 5 6.1 × 108 M−1 s−1 6 8 −1 −1 2 5 •OH +NH2Cl → NHCl• + H2O 8.64 × 10 M s 1.02 × 109 M−1 s−1 7 2.8 × 109 M−1 s−1 8 2.57 × 108 M−1 s−1 6 6 •OH +NHCl → NCl • + H O 2 2 2 6.21 × 108 M−1 s−1 9 8 −1 −1 6 7 •OH +NCl3 → NCl2• + HOCl 1.67 × 10 M s 8.5 × 104 M−1 s−1 10 1.4 × 108 M−1 s−1 11 8 •OH + HOCl → ClO• + H O 2 5.0 × 108 M−1 s−1 7 2.0 × 109 M−1 s−1 12 1.8 × 109 M−1 s−1 7 9 •OH + OCl− → ClO• + OH− 8.8 × 109 M−1 s−1 13 5.3 × 109 M−1 s−1 14 10 •OH + NO − → OH− + NO • 2 2 1.0 × 1010 M−1 s−1 15 7 −1 −1 15 11 •OH + H2O2 → HO2• + H2O 2.7 × 10 M s 12 •OH + Cl− → ClOH•− 4.3 × 109 M−1 s−1 16 13 •OH + ONOO− → ONOO• + OH− 4.8 × 109 M−1 s−1 17 − − 6 −1 −1 15 14 •OH + HCO3 → CO3• + H2O 8.5 × 10 M s 2− − − 8 −1 −1 15 15 •OH + CO3 → CO3• + OH 3.9 × 10 M s 1.0 × 109 M−1 s−1 7 16 Cl• + NH Cl → NHCl• + HCl 2 2.4 × 107 M−1 s−1 18 17 Cl• + HOCl → ClO• + H+ + Cl− 3.0 × 109 M−1 s−1 19 18 Cl• + OCl− → ClO• + Cl− 8.2 × 109 M−1 s−1 19 6.5 × 109 M−1 s−1 19 7.8 × 109 M−1 s−1 20 19 Cl• + Cl− → Cl •− 2 8.0 × 109 M−1 s−1 21 8.5 × 109 M−1 s−1 22 − − 9 −1 −1 23 20 Cl• + NO2 → Cl + NO2• 5.0 × 10 M s + − 9 −1 −1 24 21 Cl• + H2O2 → H + Cl + HO2• 1.0 × 10 M s 2.0 × 109 M−1 s−1 20 22 Cl• + OH− → ClOH•− 1.8 × 1010 M−1 s−1 19 7.2 × 104 s−1 16 1.6 × 105 s−1 19,25 23 Cl• + H O → ClOH•− + H+ 2 1.8 × 105 s−1 20 2.5 × 105 s−1 23,26 2.2 × 108 M−1 s−1 27 24 Cl• + HCO − → CO •− + H+ + Cl− 3 3 2.4 × 109 M−1 s−1 23 2− − − 8 −1 −1 27 25 Cl• + CO3 → CO3• + Cl 5.0 × 10 M s − + − 6 −1 −1 18 26 Cl2• + NH2Cl → NHCl• + H + 2Cl 6.5 × 10 M s ≤ 100 s−1 20 27 Cl •− + H O → Cl− + ClOH•− + H+ 2 2 ≤ 1300 s−1 26 5.7 × 104 s−1 20 − − 4 −1 28 28 Cl2• → Cl• + Cl 6.0 × 10 s 1.1 × 105 s−1 16 − − 9 −1 −1 29 29 Cl2• + Cl• → Cl2 + Cl 2.1 × 10 M s 9.0 × 108 M−1 s−1 28 30 Cl •− + Cl •− → 2Cl− + Cl 2 2 2 3.5 × 109 M−1 s−1 20 − − 5 −1 −1 30 31 CO3• + H2O2 →HO2• + HCO3 4.3 × 10 M s 32 ClOH•− → Cl− + •OH 6.0 × 109 s−1 20 33 ClOH•− → Cl• + OH− 23 s−1 16 − − − − 4 −1 −1 31 34 ClOH• + Cl → OH + Cl2• 1.0 × 10 M s 2.1 × 1010 M−1 s−1 16 2.4 × 1010 M−1 s−1 20 35 ClOH•− + H+ → Cl• + H O 2 2.6 × 1010 M−1 s−1 25 5.0 × 1010 M−1 s−1 23 2.5 × 109 M−1 s−1 19 36 ClO• + ClO• → Cl O 2 2 7.5 × 109 M−1 s−1 32 6.3 × 109 M−1s−1 32 37 •OH + ClO − → ClO • + OH− 2 2 7.0 × 109 M−1s−1 33 − + 9 −1 −1 19 38 •OH + ClO2• → ClO3 + H 4.0 × 10 M s 1.0 × 109 M−1s−1 34 39 •Cl + ClO • → Cl O 2 2 2 4.0 × 109 M−1s−1 7 − − 9 −1 −1 34 40 Cl2• + ClO2• → Cl2O2 + Cl 1.0 × 10 M s 9 −1 −1 35 41 ClO• + ClO2• → Cl2O3 1.4 × 10 M s − − − 9 −1 −1 11 42 Cl2• + ClO2 → ClO2• + 2Cl 1.3 × 10 M s − − 8 −1 −1 36 43 ClO• + ClO2 → OCl + ClO2• 9.4 × 10 M s − − − 9 −2 −1 37 44 Cl2O2 + ClO2 + Cl → 2ClO2• + 2Cl 8.4 × 10 M s 1.2 × 104 M−1 s−1 38 45 Cl O + ClO − + H O → ClO − + 2HOCl 2 2 2 2 3 5.3 × 105 M−1 s−1 37 − + 6 −2 −1 39 46 ClO2 + HOCl + H → Cl2O2 + H2O 1.12 × 10 M s − − − − + −2 −1 38 47 ClO2 + HOCl + Cl → ClO3 + 2Cl + H 180 M s 5 −1 32 48 Cl2O2 → 2ClO• k45/(1.3×10 )/1.93 /0.034 s 1.0 × 107 M−1 s−1 40 1.2 × 108 M−1 s−1 41 8 −1 −1 42 49 NH2• + O2 → NH2O2• 3.0 × 10 M s 1.1 × 109 M−1 s−1 43 1.2 × 109 M−1 s−1 44 8 −1 9 50 NH2O2• → NO• + H2O 1.0 × 10 s 8 −1 9 51 NH2O2• → transient species →N2O 5.98 × 10 s 50−3000 M−1 s−1 45 52 NO• + O → ONOO• 2 1 × 106 M−1 s−1 46 5.8 × 105 M−1 s−1 46 53 ONOO• + NO• → 2NO • 2 1.0 × 109 M−1 s−1 45 6500 s−1 45 54 ONOO• → NO• + O 2 2.0 × 105 s−1 46 1.0 × 1010 M−1 s−1 47 55 NO• + •OH → HNO 2 2.0 × 1010 M−1 s−1 48 9 −1 −1 49 56 NO• + NO2• → N2O3 1.1 × 10 M s 8 −1 −1 50 57 NO2• + NO2• → N2O4 4.5 × 10 M s 2.2 × 104 s−1 51 4 −1 49 58 N2O3 → NO• + NO2• 8.0 × 10 s 4.3 × 106 s−1 52 530 s−1 49 − + −1 53 59 N2O3 + H2O → 2NO2 +2H 1600 s 2000 s−1 51 −1 50 60 N2O4 → 2NO2• 6900 s 300 s−1 51 61 N O + H O → NO − + NO − + 2H+ 2 4 2 2 3 1000 s−1 50 6 −1 −1 54 62 2HNO → [HONNOH] → N2O + H2O 8.0 × 10 M s 3.8 × 102 M−1 s−1 55 3 −1 −1 56 63 HNO + O2 → ONOOH 3.0 × 10 M s 1.8 × 104 M−1 s−1 57 7.6 × 106 M−2 s−1 58 64 H+ + NH Cl + NO − → NH + NO Cl 2 2 3 2 1.2 × 107 M−2 s−1 59 − − −1 −1 60 65 NO2Cl + NO2 → N2O4 + Cl 8000 M s − − + −1 60 66 NO2Cl + H2O → NO3 + Cl + 2H 4.8 s 0.232 s−1 61 67 ONOOH → NO • + •OH 2 0.35 s−1 62 0.568 s−1 61 − + −1 62 68 ONOOH → NO3 + H 0.90 s 1.15 s−1 63 − − −1 64 69 ONOO → O2• + NO• 0.02 s − − −6 −1 62 70 ONOO → NO3 8.0 × 10 s − − 7 −1 −1 65 71 O2• + HO2• → HO2 + O2 9.7 × 10 M s −1 −1 15 72 HO2• + H2O2 → •OH + H2O + O2 3.0 M s − − −1 −1 15 73 O2• + H2O2 → •OH + OH + O2 0.13 M s 6 −1 −1 66 74 HOCl + NH3 → NH2Cl + H2O 4.2 × 10 M s −1 −1 66 75 HOCl + NH2Cl → NHCl2 + H2O 280 M s − − 9 −2 −1 67 76 HOCl + NHCl2 + OH → NCl3 + OH + H2O 3.3 × 10 M s − − 5 −2 −1 67 77 HOCl + NHCl2 + OCl → NCl3 + OH + HOCl 1.0 × 10 M s −5 −1 66 78 NH2Cl + H2O → HOCl +NH3 2.1 × 10 s −7 −1 68 79 NHCl2 + H2O → HOCl + NH2Cl 6.5 × 10 s −5 −1 68 80 NCl3 + H2O → HOCl + NHCl2 3.2 × 10 s + + −2 −1 69 81 NH2Cl + NH2Cl + H → NHCl2 + NH4 6944 M s + − −2 −1 69 82 NH2Cl + NH2Cl + H2CO3 → NHCl2 + NH4 + HCO3 11 M s − − −2 −1 69 83 NH2Cl + NH2Cl + HCO3 → NHCl2 + NH3 + HCO3 0.22 M s + −1 −1 70 84 NH2Cl + NHCl2 → N2 + 3H + 3Cl (assumed products) 0.015 M s + + 4 −2 −1 67 85 NHCl2 + NH3 + H → NH2Cl + NH2Cl + H 6.0 × 10 M s − −1 −1 71 86 NHCl2 + OH → I + products 110 M s 4 −1 −1 72 87 I + NHCl2 → HOCl + products 2.8 × 10 M s 3 −1 −1 72 88 I + NH2Cl → products 8.3 × 10 M s − 9 −2 −1 70 89 NH2Cl + NCl3 + OH → HOCl + products 1.4 × 10 M s − 10 −2 −1 70 90 NHCl2 + NCl3 + OH → 2HOCl + products 5.6 × 10 M s −1 −1 73 91 H2O2 + NH2Cl → products 0.0276 M s (24.6 °C) 7.4 × 103 M−1 s−1 74 92 HOCl + NO − → NO Cl + OH− 2 2 4.4 × 104 M−1 s−1 58 − + 4 −1 −1 13 93 H2O2 + HOCl → Cl + H2O + O2 + H 1.1 × 10 M s − − 5 −1 −1 13 94 H2O2 + OCl → Cl + H2O + O2 1.7 × 10 M s 2.8 × 109 M−1 s−1 15 95 •OH + 1,4−dioxane → 3.1 × 109 M−1 s−1 75 4.4 × 106 M−1 s−1 76 96 Cl• + 1,4−dioxane → 2.8−3.4 × 109 M−1 s−1 77 − 6 −1 −1 76 97 Cl2• + 1,4−dioxane → 3.3 × 10 M s HOCl ↔ OCl− pKa=7.5 78 98 OCl− + H+ → HOCl 5.0 × 1010 M−1 s−1 HOCl → OCl− + H+ 1.58 × 103 s−1 − 2− 79 H2CO3 ↔ HCO3 ↔ CO3 pKa1=6.3 & pKa2=10.3 − + 10 −1 −1 HCO3 + H → H2CO3 1.0 × 10 M s 99 + − 3 −1 H2CO3 → H + HCO3 5.0 × 10 s 2− + − 10 −1 −1 CO3 + H → HCO3 5.0 × 10 M s − 2− + −1 HCO3 → CO3 + H 2.5 s − 65 HO2• ↔ O2• pKa= 4.8 − + 10 −1 −1 100 O2• + H → HO2• 5.0 × 10 M s − + 5 −1 HO2• → O2• + H 7.9 × 10 s ONOOH ↔ ONOO− pKa= 6.6 62 101 ONOO− + H+ → ONOOH 5.0 × 1010 M−1 s−1 ONOOH → ONOO− + H+ 1.26 × 104 s−1 = 1650 M−1 cm−1 80 102 NDMA+ hν → = 0.28 80 15 16 17 Section S1.
Load more

Recommended publications
  • Group 17 (Halogens)
    Sodium, Na Gallium, Ga CHEMISTRY 1000 Topic #2: The Chemical Alphabet Fall 2020 Dr. Susan Findlay See Exercises 11.1 to 11.4 Forms of Carbon The Halogens (Group 17) What is a halogen? Any element in Group 17 (the only group containing Cl2 solids, liquids and gases at room temperature) Exists as diatomic molecules ( , , , ) Melting Boiling 2State2 2 2Density Point Point (at 20 °C) (at 20 °C) Fluorine -220 °C -188 °C Gas 0.0017 g/cm3 Chlorine -101 °C -34 °C Gas 0.0032 g/cm3 Br2 Bromine -7.25 °C 58.8 °C Liquid 3.123 g/cm3 Iodine 114 °C 185 °C Solid 4.93 g/cm3 A nonmetal I2 Volatile (evaporates easily) with corrosive fumes Does not occur in nature as a pure element. Electronegative; , and are strong acids; is one of the stronger weak acids 2 The Halogens (Group 17) What is a halogen? Only forms one monoatomic anion (-1) and no free cations Has seven valence electrons (valence electron configuration . ) and a large electron affinity 2 5 A good oxidizing agent (good at gaining electrons so that other elements can be oxidized) First Ionization Electron Affinity Standard Reduction Energy (kJ/mol) Potential (kJ/mol) (V = J/C) Fluorine 1681 328.0 +2.866 Chlorine 1251 349.0 +1.358 Bromine 1140 324.6 +1.065 Iodine 1008 295.2 +0.535 3 The Halogens (Group 17) Fluorine, chlorine and bromine are strong enough oxidizing agents that they can oxidize the oxygen in water! When fluorine is bubbled through water, hydrogen fluoride and oxygen gas are produced.
    [Show full text]
  • Rate Constants for Reactions Between Iodine- and Chlorine-Containing Species: a Detailed Mechanism of the Chlorine Dioxide/Chlorite-Iodide Reaction†
    3708 J. Am. Chem. Soc. 1996, 118, 3708-3719 Rate Constants for Reactions between Iodine- and Chlorine-Containing Species: A Detailed Mechanism of the Chlorine Dioxide/Chlorite-Iodide Reaction† Istva´n Lengyel,‡ Jing Li, Kenneth Kustin,* and Irving R. Epstein Contribution from the Department of Chemistry and Center for Complex Systems, Brandeis UniVersity, Waltham, Massachusetts 02254-9110 ReceiVed NoVember 27, 1995X Abstract: The chlorite-iodide reaction is unusual because it is substrate-inhibited and autocatalytic. Because - analytically pure ClO2 ion is not easily prepared, it was generated in situ from the rapid reaction between ClO2 and I-. The resulting overall reaction is multiphasic, consisting of four separable parts. Sequentially, beginning with mixing, these parts are the (a) chlorine dioxide-iodide, (b) chlorine(III)-iodide, (c) chlorine(III)-iodine, and (d) hypoiodous and iodous acid disproportionation reactions. The overall reaction has been studied experimentally and by computer simulation by breaking it down into a set of kinetically active subsystems and three rapidly established - equilibria: protonations of chlorite and HOI and formation of I3 . The subsystems whose kinetics and stoichiometries were experimentally measured, remeasured, or which were previously experimentally measured include oxidation of - iodine(-1,0,+1,+3) by chlorine(0,+1,+3), oxidation of I by HIO2, and disproportionation of HOI and HIO2. The final mechanism and rate constants of the overall reaction and of its subsystems were determined by sensitivity analysis and parameter fitting of differential equation systems. Rate constants determined for simpler reactions were fixed in the more complex systems. A 13-step model with the three above-mentioned rapid equilibria fits the - -3 - -3 - - overall reaction and all of its subsystems over the range [I ]0 < 10 M, [ClO2 ]0 < 10 M, [I ]0/[ClO2 ]0 ) 3-5, pH ) 1-3.5, and 25 °C.
    [Show full text]
  • Guidance for Identification and Naming of Substance Under REACH
    Guidance for identification and naming of substances under 3 REACH and CLP Version 2.1 - May 2017 GUIDANCE Guidance for identification and naming of substances under REACH and CLP May 2017 Version 2.1 2 Guidance for identification and naming of substances under REACH and CLP Version 2.1 - May 2017 LEGAL NOTICE This document aims to assist users in complying with their obligations under the REACH and CLP regulations. However, users are reminded that the text of the REACH and CLP Regulations is the only authentic legal reference and that the information in this document does not constitute legal advice. Usage of the information remains under the sole responsibility of the user. The European Chemicals Agency does not accept any liability with regard to the use that may be made of the information contained in this document. Guidance for identification and naming of substances under REACH and CLP Reference: ECHA-16-B-37.1-EN Cat. Number: ED-07-18-147-EN-N ISBN: 978-92-9495-711-5 DOI: 10.2823/538683 Publ.date: May 2017 Language: EN © European Chemicals Agency, 2017 If you have any comments in relation to this document please send them (indicating the document reference, issue date, chapter and/or page of the document to which your comment refers) using the Guidance feedback form. The feedback form can be accessed via the EVHA Guidance website or directly via the following link: https://comments.echa.europa.eu/comments_cms/FeedbackGuidance.aspx European Chemicals Agency Mailing address: P.O. Box 400, FI-00121 Helsinki, Finland Visiting address: Annankatu 18, Helsinki, Finland Guidance for identification and naming of substances under 3 REACH and CLP Version 2.1 - May 2017 PREFACE This document describes how to name and identify a substance under REACH and CLP.
    [Show full text]
  • APPENDIX G Acid Dissociation Constants
    harxxxxx_App-G.qxd 3/8/10 1:34 PM Page AP11 APPENDIX G Acid Dissociation Constants §␮ ϭ 0.1 M 0 ؍ (Ionic strength (␮ † ‡ † Name Structure* pKa Ka pKa ϫ Ϫ5 Acetic acid CH3CO2H 4.756 1.75 10 4.56 (ethanoic acid) N ϩ H3 ϫ Ϫ3 Alanine CHCH3 2.344 (CO2H) 4.53 10 2.33 ϫ Ϫ10 9.868 (NH3) 1.36 10 9.71 CO2H ϩ Ϫ5 Aminobenzene NH3 4.601 2.51 ϫ 10 4.64 (aniline) ϪO SNϩ Ϫ4 4-Aminobenzenesulfonic acid 3 H3 3.232 5.86 ϫ 10 3.01 (sulfanilic acid) ϩ NH3 ϫ Ϫ3 2-Aminobenzoic acid 2.08 (CO2H) 8.3 10 2.01 ϫ Ϫ5 (anthranilic acid) 4.96 (NH3) 1.10 10 4.78 CO2H ϩ 2-Aminoethanethiol HSCH2CH2NH3 —— 8.21 (SH) (2-mercaptoethylamine) —— 10.73 (NH3) ϩ ϫ Ϫ10 2-Aminoethanol HOCH2CH2NH3 9.498 3.18 10 9.52 (ethanolamine) O H ϫ Ϫ5 4.70 (NH3) (20°) 2.0 10 4.74 2-Aminophenol Ϫ 9.97 (OH) (20°) 1.05 ϫ 10 10 9.87 ϩ NH3 ϩ ϫ Ϫ10 Ammonia NH4 9.245 5.69 10 9.26 N ϩ H3 N ϩ H2 ϫ Ϫ2 1.823 (CO2H) 1.50 10 2.03 CHCH CH CH NHC ϫ Ϫ9 Arginine 2 2 2 8.991 (NH3) 1.02 10 9.00 NH —— (NH2) —— (12.1) CO2H 2 O Ϫ 2.24 5.8 ϫ 10 3 2.15 Ϫ Arsenic acid HO As OH 6.96 1.10 ϫ 10 7 6.65 Ϫ (hydrogen arsenate) (11.50) 3.2 ϫ 10 12 (11.18) OH ϫ Ϫ10 Arsenious acid As(OH)3 9.29 5.1 10 9.14 (hydrogen arsenite) N ϩ O H3 Asparagine CHCH2CNH2 —— —— 2.16 (CO2H) —— —— 8.73 (NH3) CO2H *Each acid is written in its protonated form.
    [Show full text]
  • Qualitative and Quantitative Tier 3 Assessment
    Consider It Done www.ehs-support.com.au Qualitative and Quantitative Tier 3 Assessment Sodium Hypochlorite In accordance with the Chemical Risk Assessment Framework (CRAF), the assessment for this Tier 3 chemical includes the following components: completing the screening; developing a risk assessment dossier and Predicted No-Effects Concentrations (PNECs) for water and soil; and, completing a qualitative and quantitative assessment of risk. Each of these components is detailed within this attachment. Background Sodium hypochlorite is a component in a Water Management Facility (WMF) product (Sodium Hypochlorite Solution 12.5%) used as an oxidising agent/disinfectant during oily water treatment. A safety data sheet (SDS) for the WMF product is included as Attachment 1. Process and usage information for this chemical is included in Attachment 2 and summarised in Table 1. Table 1 Water Management Facility Chemicals – Tier 3 Chemicals Approximate Quantity Stored On- Proprietary Name Chemical Name CAS No. Use Site (plant available storage) Sodium Sodium Hypochlorite 7681-52-9 Oxidising 15000 L Hypochlorite Sodium Hydroxide 1310-73-2 agent/disinfectant Solution 12.5% CAS No = Chemical Abstracts Service Number L = litre The assessment of toxicity of this chemical was used to evaluate human health exposure scenarios and is presented in Attachment 3. Since an Australian Drinking Water Guideline (ADWG) Value is available (see Table 2), toxicological reference values (TRVs) were not derived for the chemical. A detailed discussion of the drinking
    [Show full text]
  • Safety Data Sheet
    SAFETY DATA SHEET Preparation Date: 9/23/2013 Revision date 10/11/2019 Revision Number: G3 1. IDENTIFICATION Product identifier Product code: S1243 Product Name: SODIUM CHLORITE, ANHYDROUS, FLAKES Other means of identification Synonyms: Chlorous acid, sodium salt CAS #: 7758-19-2 RTECS # VZ4800000 CI#: Not available Recommended use of the chemical and restrictions on use Recommended use: Bleaching agent. Water purification. Uses advised against No information available Supplier: Spectrum Chemical Mfg. Corp 14422 South San Pedro St. Gardena, CA 90248 (310) 516-8000 Order Online At: https://www.spectrumchemical.com Emergency telephone number Chemtrec 1-800-424-9300 Contact Person: Tom Tyner (USA - West Coast) Contact Person: Ibad Tirmiz (USA - East Coast) 2. HAZARDS IDENTIFICATION Classification This chemical is considered hazardous by the 2012 OSHA Hazard Communication Standard (29 CFR 1910.1200) Considered a dangerous substance or mixture according to the Globally Harmonized System (GHS) Acute toxicity - Oral Category 3 Acute toxicity - Dermal Category 2 Acute toxicity - Inhalation (Dusts/Mists) Category 2 Skin corrosion/irritation Category 2 Serious eye damage/eye irritation Category 1 Oxidizing solids Category 2 Label elements Danger Hazard statements Fatal in contact with skin or if inhaled Toxic if swallowed Causes skin irritation Product code: S1243 Product name: SODIUM CHLORITE, Page 1 / 15 ANHYDROUS, FLAKES Causes serious eye damage May intensify fire; oxidizer Hazards not otherwise classified (HNOC) Not Applicable Other hazards Very toxic to aquatic life with long lasting effects Precautionary Statements - Prevention Wash face, hands and any exposed skin thoroughly after handling Do not eat, drink or smoke when using this product Do not get in eyes, on skin, or on clothing Do not breathe dust Use only outdoors or in a well-ventilated area Wear respiratory protection Keep away from heat/sparks/open flames/hot surfaces.
    [Show full text]
  • Risk Assessment Report Sodium Chlorite（The 3 Edition） (Food
    This is a provisional English translation of an excerpt from the original full report. Risk Assessment Report Sodium Chlorite（The 3rd edition） (Food Additive) Food Safety Commission of Japan (FSCJ) July 2009 Executive summary The Food Safety Commission of Japan (FSCJ) conducted a risk assessment of sodium chlorite (NaClO2) [CAS No. 7758-19-2], a food additive that is used as a bleaching agent and bacteriocide, using various test results. The test results used in the assessment are related to the repetitive dose toxicity, carcinogenicity, reproductive developmental toxicity, genotoxicity, etc. of sodium chlorite and other substances. When administered orally, sodium chlorite is assumed to convert to chlorous acid (HClO2) in gastric fluid. In － addition to chlorous acid (HClO2), substances such as chloride ion (Cl ), chlorine dioxide (ClO2), and chlorite － ion (ClO2 ) can also be produced by metabolism in the human body. Therefore, the toxicity of sodium chlorite was assessed mainly on the basis of safety data obtained for sodium chlorite, chlorite ion, and chlorine dioxide from various animal and human studies, with reference to findings related to hypochlorous acid solution and sodium hypochlorite (NaClO) as appropriate. According to the results of the safety studies for sodium chlorite and the like, the most commonly observed major effect of sodium chlorite intake was thought to be the damage to the red blood cells by oxidative stress. No carcinogenicity was observed. With regard to genotoxicity, a weak positive result was observed in a reverse mutation test using bacteria. Although a positive result was obtained in a chromosomal abnormality test using mammalian cell cultures, the result was negative as to a micronucleus test performed using a high dose.
    [Show full text]
  • Acidified Sodium Chlorite
    Acidified Sodium Chlorite Livestock 1 2 Identification of Petitioned Substance 3 4 Chemical Name: 11 CAS Numbers: 5 Acidified Sodium Chlorite (ASC) 13898-47-0 (Chlorous Acid) 6 7758-19-2 (Sodium Chlorite) 7 Other Names: 8 Sodium Chlorite, Acidified Other Codes: 9 Chlorous Acid 231-836-6 (EINECS) 10 12 Trade Names: 13 SANOVA®, 4XLA®, Aztec Gold® 14 15 Summary of Petitioned Use 16 The National Organic Program (NOP) final rule currently allows the use of acidified sodium chlorite (ASC) 17 solutions for antimicrobial food treatment when acidified with citric acid under 7 CFR § 205.605. The 18 petition before the National Organic Standards Board (NOSB) is to add ASC solution as an allowed 19 synthetic in organic livestock production (§ 205.603) for use as a disinfectant/sanitizer and topical 20 treatment (i.e., teat dip). 21 ASC solutions used as disinfectants and teat dip treatments in livestock production are analogous to those 22 used for secondary direct food processing and handling. However, the potential impacts to the 23 environment and human health resulting from ASC treatments of livestock necessitate consideration of the 24 aqueous chemistry of the parent substance and its breakdown products, and potential for toxic effects to 25 terrestrial organisms and humans potentially exposed to these substances. 26 Characterization of Petitioned Substance 27 28 Composition of the Substance: 29 The petitioned substance, acidified sodium chlorite (ASC) solution, is generated through the reaction of 30 any acid categorized as Generally Recognized as Safe (GRAS) by the FDA with an aqueous solution of 31 technical grade (~80% purity) sodium chlorite (NaClO2).
    [Show full text]
  • Chemistry 1000 Lecture 21: the Halogens
    Chemistry 1000 Lecture 21: The halogens Marc R. Roussel November 22, 2018 Marc R. Roussel Chemistry 1000 Lecture 21: The halogens November 22, 2018 1 / 20 The halogens The halogens Group 17 Pure elements consist of X2 molecules All form −1 anions States and colors at room temperature: F2 Cl2 Br2 I2 gas gas liquid solid yellow yellow-green dark red dark violet Volatility: tendency of a substance to vaporize Why are the compounds at the top of the group more volatile? Marc R. Roussel Chemistry 1000 Lecture 21: The halogens November 22, 2018 2 / 20 The halogens Reduction potentials range from extremely to moderately positive, i.e. these are good to excellent oxidizing agents: − − X2 + 2e ! 2X(aq) Element F2 Cl2 Br2 I2 E◦=V 2.866 1.358 1.065 0.535 In nature, always found as the anion, except iodine which is also found in some oxoanions Fluorine in particular can often oxidize elements with very high electronegativities (e.g. chlorine, oxygen). Marc R. Roussel Chemistry 1000 Lecture 21: The halogens November 22, 2018 3 / 20 The halogens Enthalpy of electronic attraction 350 340 330 -1 mol 320 /kJ EA E 310 300 290 F Cl Br I Why does F go against the trend? Marc R. Roussel Chemistry 1000 Lecture 21: The halogens November 22, 2018 4 / 20 The halogens Typical reactions of halogens React with metals to form metal halides React with nonmetals, often forming more than one binary compound with elements in period 3 or beyond Reaction of a halogen with P4 can give either PX3 or PX5 Reaction with S8 can give SX2,S2X2, SX4,S2X10, SX6 Industrial production of Cl2: by electrolysis of NaCl(aq) Industrial production of Br2 and I2: by oxidation of the anion with chlorine gas, e.g.
    [Show full text]
  • Chloramines in Drinking Water
    Chloramines in Drinking Water Guideline Technical Document for Public Consultation Consultation period ends January 25, 2019 Chloramines For public consultation Chloramines in Drinking Water Document for Public Consultation Table of Contents Purpose of consultation ................................................................................................................... 1 Part I. Overview and Application................................................................................................ 2 1.0 Proposed guideline .............................................................................................................. 2 2.0 Executive summary ............................................................................................................. 2 2.1 Health effects .......................................................................................................... 2 2.2 Exposure ................................................................................................................. 3 2.3 Analysis and treatment ............................................................................................ 3 2.4 International considerations .................................................................................... 3 3.0 Application of the guideline................................................................................................ 4 3.1 Monitoring .............................................................................................................. 5 Part II. Science
    [Show full text]
  • Chloramination Basics
    Chloramine Treatment & Management NHWWA Operator Training Session Presented by: David G. Miller, P.E. Deputy Director, Water Supply & Treatment Manchester Water Works [email protected] Acknowledgements NEWWA Disinfection Committee Professor Jim Malley, UNH Cynthia Klevens, NHDES Manchester Water Works Operators & Laboratory Staff References Alternative Disinfectants and Oxidants Guidance Manual, USEPA, 1999 A Guide for the Implementation and Use of Chloramines, AwwaRF, 2004 Water Chlorination/Chloramination Practices and Principles (M20), AWWA, Latest Edition Presentation Outline Why Use Chloramines? Pathogen Inactivation & Disinfection DBP Formation Control Chlorine & Chloramine Chemistry Chlorine & Ammonia Feed Methods Safety Considerations Managing the Chloramination Process Impact on other Treatment Processes Why Use Chloramines? Secondary (residual) Disinfection Reduce DBP risks to public health Less reactive with organics than free chlorine therefore forms less THMs Monochloramine residual more stable and lasts longer than free chlorine residual Monochloramine superior to free chlorine at penetrating biofilm Less likely to have taste & odor complaints Normal dosage: 1.0 to 4.0 mg/L Minimum residual: 0.5 mg/L Pathogen Inactivation & Disinfection Mechanism Inhibits organism cell protein production & respiration pH Effect Controls chloramine species distribution Temperature Effect Bacteria & virus inactivation increases with temperature Bacteria, Virus, and Protozoa Inactivation Far less effective
    [Show full text]
  • Monochloramine in Drinking-Water
    WHO/SDE/WSH/03.04/83 English only Monochloramine in Drinking-water Background document for development of WHO Guidelines for Drinking-water Quality © World Health Organization 2004 Requests for permission to reproduce or translate WHO publications - whether for sale of for non- commercial distribution - should be addressed to Publications (Fax: +41 22 791 4806; e-mail: [email protected]. The designations employed and the presentation of the material in this publication do not imply the expression of any opinion whatsoever on the part of the World Health Organization concerning the legal status of any country, territory, city or area or of its authorities, or concerning the delimitation of its frontiers or boundaries. The mention of specific companies or of certain manufacturers' products does not imply that they are endorsed or recommended by the World Health Organization in preference to others of a similar nature that are not mentioned. Errors and omissions excepted, the names of proprietary products are distinguished by initial capital letters. The World Health Organization does not warrant that the information contained in this publication is complete and correct and shall not be liable for any damage incurred as a results of its use. Preface One of the primary goals of WHO and its member states is that “all people, whatever their stage of development and their social and economic conditions, have the right to have access to an adequate supply of safe drinking water.” A major WHO function to achieve such goals is the responsibility “to propose ... regulations, and to make recommendations with respect to international health matters ....” The first WHO document dealing specifically with public drinking-water quality was published in 1958 as International Standards for Drinking-water.
    [Show full text]