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Explain uses of indicator in analysis of redox reaction. |
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Answer» Solution :(i) In one situation, the reagent itself is intensely coloured, e.g., permanganate ion, `MnO_(4)^(-)`. Here `MnO_(4)^(-)` acts as the self indicator. The visible end point in this case is achieved after the last of the reductant `(Fe^(2+)orC_(2)O_(4)^(-2))` is oxidised and the first lasting tinge of pink COLOUR appears at `MnO_(4)^(-)` CONCENTRATION as low as `10^(-6)"mol"dm^(-3)(10^(-6)"mol"L^(-1))`. This ensures a minimal .overshoot. in colour beyond the equivalence point, the point where the reductant and the oxidant are equal in terms of their mole stoichiometry. (ii) If there is no dramatic auto-colour CHANGE (as with `MnO_(4)^(-)` titration), there are indicators which are oxidised immediately after the last bit of the reactant is consumed, producing a dramatic colour change. The best example is afforded by `Cr_(2)O_(7)^(2)`, which is not a self-indicator, but oxidises the indicator substance diphenylamine just after the equivalence point to produce an intense blue colour, thus signalling the end point. (iii) There is yet another method which is interesting and quite common. Its use is restricted to those REAGENTS which are able to oxidise `I^(-)` ions, say, for example, `2Cu_((aq))^(+2)+4I_((aq))^(-)toCu_(2)I_(2(s))+I_(2(aq))` This method relies on the FACTS that iodine itself gives an intense blue colour with starch and has a very specific reaction with thiosulphate ions `(S_(2)O_(3(aq))^(-2))`, which too is a redox reaction : `I_(2(aq))+S_(2)O_(3(aq))^(-2)to2I_((aq))^(-)+S_(4)O_(6(aq))^(-2)` `I_(2)`, though insoluble in water, remains in solution containing Kl as `KI_(3)`. On addition of starch after the liberation of `Cu^(2+)` ions on iodide ions, an intense blue colour appears. This colour disappears as soon as the iodine is consumed by the thiosulphate ions. Thus, the end-point can easily be tracked and the rest is the stoichiometric calculation only. |
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