{"title":"高碘酸盐在水溶液中氧化橙II的动力学和机理","authors":"B. Myek, S. Idris, A. D. Onu, M. K. Yakubu","doi":"10.4314/IJS.V23I1.3","DOIUrl":null,"url":null,"abstract":"+ + reaction increases with increase in [H ]. Plot of k versus log[H ] gave a slope of one, showing that the reaction is 1 + first order with respect to hydrogen ion concentration. The Plot of k versus [H ] was linear with a positive 2 2 intercept (R = 0.89). The acid dependence of this nature shows that there is a rapid pre-equilibrium between the protonated and non-protonated forms in which both the protonated and unprotonated forms are reactive. The","PeriodicalId":13487,"journal":{"name":"Ife Journal of Science","volume":"18 1","pages":"23-30"},"PeriodicalIF":0.0000,"publicationDate":"2021-05-03","publicationTypes":"Journal Article","fieldsOfStudy":null,"isOpenAccess":false,"openAccessPdf":"","citationCount":"0","resultStr":"{\"title\":\"Kinetics and mechanism of the oxidation of Orange II by periodate ion in aqueous acid\",\"authors\":\"B. Myek, S. Idris, A. D. Onu, M. K. Yakubu\",\"doi\":\"10.4314/IJS.V23I1.3\",\"DOIUrl\":null,\"url\":null,\"abstract\":\"+ + reaction increases with increase in [H ]. Plot of k versus log[H ] gave a slope of one, showing that the reaction is 1 + first order with respect to hydrogen ion concentration. The Plot of k versus [H ] was linear with a positive 2 2 intercept (R = 0.89). The acid dependence of this nature shows that there is a rapid pre-equilibrium between the protonated and non-protonated forms in which both the protonated and unprotonated forms are reactive. The\",\"PeriodicalId\":13487,\"journal\":{\"name\":\"Ife Journal of Science\",\"volume\":\"18 1\",\"pages\":\"23-30\"},\"PeriodicalIF\":0.0000,\"publicationDate\":\"2021-05-03\",\"publicationTypes\":\"Journal Article\",\"fieldsOfStudy\":null,\"isOpenAccess\":false,\"openAccessPdf\":\"\",\"citationCount\":\"0\",\"resultStr\":null,\"platform\":\"Semanticscholar\",\"paperid\":null,\"PeriodicalName\":\"Ife Journal of Science\",\"FirstCategoryId\":\"1085\",\"ListUrlMain\":\"https://doi.org/10.4314/IJS.V23I1.3\",\"RegionNum\":0,\"RegionCategory\":null,\"ArticlePicture\":[],\"TitleCN\":null,\"AbstractTextCN\":null,\"PMCID\":null,\"EPubDate\":\"\",\"PubModel\":\"\",\"JCR\":\"\",\"JCRName\":\"\",\"Score\":null,\"Total\":0}","platform":"Semanticscholar","paperid":null,"PeriodicalName":"Ife Journal of Science","FirstCategoryId":"1085","ListUrlMain":"https://doi.org/10.4314/IJS.V23I1.3","RegionNum":0,"RegionCategory":null,"ArticlePicture":[],"TitleCN":null,"AbstractTextCN":null,"PMCID":null,"EPubDate":"","PubModel":"","JCR":"","JCRName":"","Score":null,"Total":0}
Kinetics and mechanism of the oxidation of Orange II by periodate ion in aqueous acid
+ + reaction increases with increase in [H ]. Plot of k versus log[H ] gave a slope of one, showing that the reaction is 1 + first order with respect to hydrogen ion concentration. The Plot of k versus [H ] was linear with a positive 2 2 intercept (R = 0.89). The acid dependence of this nature shows that there is a rapid pre-equilibrium between the protonated and non-protonated forms in which both the protonated and unprotonated forms are reactive. The
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