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Standardisation Of 0.02moldm-3 Potassium Permanganate Solution Using Ferrous Ammonium Sulphate (Ammonium Iron (Ii) Sulphate) - Lab Report Example

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The technique for determining the concentration of an acid or a base is known as titration. This is the process which involves carefully adding one reactant to another while at the same time measuring how much is needed for the reaction to be complete. …
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Standardisation Of 0.02moldm-3 Potassium Permanganate Solution Using Ferrous Ammonium Sulphate (Ammonium Iron (Ii) Sulphate)
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"Standardisation Of 0.02moldm-3 Potassium Permanganate Solution Using Ferrous Ammonium Sulphate (Ammonium Iron (Ii) Sulphate)"

Download file to see previous pages In this experiment, a base (Iron Ammonium Sulphate – FeSO4.(NH4)2SO4.6H2O Mr=392g/mole) will be added to 0.02moldm-3 Potassium Permanganate Solution. In this experiment Manganese reacts with Iron through a redox process by which electrons are transferred from one to the other.
In this experiment, Mn goes from a +7 state (MN+7) to a +2 state (Mn+2) – i.e. each Mn+7 picks up 5 electrons – Mn is reduced. Fe goes from +2 (Fe+2) to +3 (Fe+3) i.e. each Fe+2 loses 1 electron – Fe is oxidized
As a result the mole ratio in the reaction is Mn: Fe – 1:5
The point at which the reactants will have completely neutralized each other is the equivalence point. In this experiment, this will be determined by noting the color change of the reactants. Mn+7 are purple. When Fe2+ is added, redox reaction starts making the purple color to disappear due to formation of Mn2+ which is colorless. In the process, the Fe2+ is converted to Fe3+. This happens only when Fe2+ is present. When Fe2+ is used up (at endpoint) the solution will have a permanent pink tinge and this is the point where there is no further addition of permanganate. ...Download file to see next pagesRead More
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