Kinetic Approach to Reaction among Bromate, Bromide and Iron(11) Utilized for Potentiometric Flow Injection Analysis of Trace B r o m ate Based on Its Redox Reaction with Iron(111)-Iron(11) Buffe r

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  • OHURA Hiroki
    Department of Industrial Chemistry, Faculty of Engineering, Kyushu Sangyo University;
  • IMATO Toshihiko
    Department of Chemical Science and Technology, Faculty of Engineering, Kyushu University;
  • YAMASAKA Sumio
    Department of Industrial Chemistry, Faculty of Engineering, Kyushu Sangyo University;
  • ISHIBASHI Nobuhiko
    Department of Industrial Chemistry, Faculty of Engineering, Kinki University in Kyushu;

Bibliographic Information

Other Title
  • 臭素酸のフロー電位差分析に用いた臭素酸イオンと臭化物イオンおよび鉄(II)イオン間の反応の過程とその反応速度
  • 臭素酸のフロー電位差分析に用いた臭素酸イオンと臭化物イオンおよび鉄(2)イオン間の反応の過程とその反応速度
  • シュウソサン ノ フロー デンイサ ブンセキ ニ モチイタ シュウソサン イオ
  • Kinetic Approach to Reaction among Bromate, Bromide and Iron(II)Utilized for Potentiometric Flow Injection Analysis of Trace Bromate Based on Its Redox Reaction with Iron(III)-Iron(II) Buffer.

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Description

A highly sensitive potentiometric flow injection analysis (FIA) for bromate has been previously proposed by utilizing the detection of a large transient potential change which appears during the reaction of bromate with a Fe(M)-Fe(I1) potential buffer containing bromide. The transient potential has been estimated to be due to bromine as an intermediate of the reaction (1).<BR>_??_<BR>In this paper, in order to confirm the est imated reaction pathway and rate of the reaction (1), the overall reaction rate among bromate, bromide and iron(11) in sulfuric acid solution and reaction rates of each steps ( a ), (b ) and ( c ) were measured by stopped-flow spectrophotometry by following the bromine concentration. The absorbance change at 447 nm was used for the determination of bromine. The absorbance change on addition of bromate to the reagent solution of iron(10 and bromide, showed the formation and decay of bromine, which indicates the successive reactions involving bromine as an intermediate. The rate constants, kFl, 42 and kR for reactions ( a ), (b ) and ( c ), respectively, were determined separately by measuring the concentration change of bromine as function of time. As results, the rates of reactions ( a ), (b ) and ( c ) were expressed by Eq s. (2), (3) and (4), respectively. The rate constants, 141, kF2 and kR were found to be 3.18+0.23, 1.98±0.20 and 4.09±0.15/ / (mols), respectively, in 0.6 M sulfuric acid solution at 25°C. The concentration change of bromine in the overall reaction among bromate, bromide and iron(li)is expressed by Eq. (5), integrating and rearranging Eqs. (2), (3) and (4).<BR>d[Br]dt =kFI [BrO3-] ⋅[Br-]=k, ⋅[Br03-] 2, )d[Br2]/dt. =kF2⋅[Br03-⋅] [Fe2+] = k2⋅[BrO3-] ( 3 )-d[Bra]dt =4, [Br2]⋅; [Fe2+] = k3⋅ [Br2] ( 4)[B ko r]= k 0[Br03]0 {e-k3t_⋅ e-kot}ko=_ (5)<BR>The bromine concentration-time relation observed in above mixed solution was in good agreement with that calculated from Eq. (5) by using kFl, kF2 and kR obtained.

Journal

  • NIPPON KAGAKU KAISHI

    NIPPON KAGAKU KAISHI 1992 (8), 797-803, 1992-08-10

    The Chemical Society of Japan

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