HIRE QUALIFIED ACADEMIC WRITERS
A redox titration can accurately determine the concentration of an analyte bymeasuring it against a standardised titrant. A well-known example is the redox titrationof a standardised solution of potassium permanganate (KMnO4) against an analytecontaining an unknown concentration of iron(II) ions (Fe2+).The use of KMnO4 as a titrant is particularly useful because it can act as its ownindicator; due to KMnO4 solution being bright purple, while the Fe2+ solution iscolourless. It is therefore possible to see when the titration reaches its endpoint,because the solution will remain slightly purple from unreacted KMnO4.During this titration;• Fe2+ ions are oxidised to Fe3+ ions• MnO4– ions are reduced to Mn2+ ionsThe KMnO4 solution is placed in the burette (see Figure 1 below). Before theequivalence point is reached, any KMnO4 added to the conical flask will not remain inthe solution but will be consumed by the other reactant in the flask. Once theequivalence point has been reached there is no more reactant in the flask to consumethe KMnO4. If one extra drop of KMnO4 is added from the burette it will remain in thesolution. This additional drop will give a purple-pink colour to the solution. The first signof this colour is the end-point. It approximates very closely to the equivalence point. Attachments: Practical-2-g….pdf Practical-2–….pdf Practical-2-m….pdf Proficiency-T….xlsx
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