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In a quantitative determination of iron in an ore, an analyst converted 0.42 g of the ore into its ferrous form . This required 42.00 mL of 0.1 N solution of KMnO_(4) for titration. How many moles of KMnO_(4) were used for titration ? (Fe =56) |
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Answer» Solution :In this problem `FE^(2+)` is oxidised to `Fe^(3+)` by `KMnO_(4)` Moles of `KMnO_(4) =("equivalents")/("factor relating mo.wt and eq.wt")""...(Eqn.6ii)` ` = (0.0042)/5 = 0.00084` mole . Note : Thus we see how the equations 1 to 7 have been put into USE in the PROBLEMS given above . However , application of these euations and the ability to use them come only from PRACTICE. The STUDENTS are advised to apply the said rules in as many problems as possible ] . |
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