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`1g` pure iron is dissolved in excess of `H_(2)SO_(4)`. The clear filtrate is made up `100 mL. 10mL` of this solution is treated with `0.1 M KMnO_(4)` solution till whole of the `Fe^(2+)` ions are oxidised to `Fe^(3+)` ions. Now `0.2 g Fe_(2)(SO_(4))_(3)` is dissolved in it. the solution is now treated with `Zn` and `H_(2)SO_(4)`. The volume of `KMnO_(4)` needed to convert `Fe^(2+)` ions to `Fe^(3+)` ions in `100 mL` original solution is:A. `71 mL`B. `142 mL`C. `35.7 mL`D. `80 mL` |
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Answer» Meq. Of `Fe^(2+)`=Meq. Of `KMnO_(4)` (for `100 mL` solution) `1/56xx1000=0.1xx5xxV` `:. V=35.7 mL` |
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