thiosulfate ion oor Spaans
thiosulfate ion
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Tiosulfato
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compuesto químico
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(The sulfate ion has one S and four O atoms; thiosulfate ion has two S and three O atoms.)
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Thiosulfate ion, S 2O3 2-, also present in the reaction mixture, reacts with I 3 just as fast as it is formed.
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Here, these agents are the thiosulfate ions S2O32- in Na2S2O3 and the iodide ions I- in KI.
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The triiodide ion solution is then titrated against standard thiosulfate solution to give iodide again using starch indicator: I3− + 2 e− ⇌ 3 I− (Eo = + 0.5355 V) Together with reduction potential of thiosulfate: S4O62− + 2 e− ⇌ 2 S2O32− (Eo = + 0.08 V) The overall reaction is thus: I3− + 2 S2O32− → S4O62− + 3 I− (Ereaction = + 0.4555 V) For simplicity, the equations will usually be written in terms of aqueous molecular iodine rather than the triiodide ion, as the iodide ion did not participate in the reaction in terms of mole ratio analysis.
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Sodium thiosulfate reduces iodine to iodide ions, yielding sodium iodide:
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Both thiocysteine and thiosulfate can be used by sulfurtransferases to incorporate sulfur into cyanide ion, (CN–), thereby detoxifying the cyanide to thiocyanate.
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However, when the sodium thiosulfate is used up, nothing can hinder the iodine formation and the consequent triiodide ions’ formation.
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However, when the sodium thiosulfate is used up, nothing can hinder the iodine formation and the consequent formation of triiodide ions.
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Sodium thiosulfate immediately reduces all the iodine forming in the reaction with hydrogen peroxide; triiodide ions do not form and have no opportunity to interact with the starch, and the reaction mixture remains transparent.
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Iodometry is an indirect volumetric method, where an excess of iodide ions are added to a solution containing the oxidizing agent, which react producing an equivalent quantity of iodine that is then titrated with a standardized solution of sodium thiosulfate.
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