${\rm{MnO}}_4^ - $ ions are reduced in acidic condition to ${\rm{M}}{{\rm{n}}^{2 + }}$ ions whereas they are reduced in neutral condition to ${\rm{Mn}}{{\rm{O}}_2}$. The oxidation of 25 mL of a solution X containing ${\rm{F}}{{\rm{e}}^{2 + }}$ ions required in acidic condition 20 mL of a solution Y containing ${\rm{MnO}}_4^ - $ ions. What volume of solution Y would be required to oxidise 25 mL of a solution Xcontaining ${\rm{F}}{{\rm{e}}^{2 + }}$ ions in neutral condition?Failed to load question data. Please try again later.
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