100 mL of 0.1 M Fe^{2+} solution was titrat | vedclass

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(D) The balanced redox reaction is: $Cr_2O_7^{2-} + 14 H^{+} + 6 Fe^{2+} \longrightarrow 2 Cr^{3+} + 6 Fe^{3+} + 7 H_2O$At equivalence point,the numbe

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(D) The balanced redox reaction is: $Cr_2O_7^{2-} + 14 H^{+} + 6 Fe^{2+} \longrightarrow 2 Cr^{3+} + 6 Fe^{3+} + 7 H_2O$At equivalence point,the number of equivalents of $Cr_2O_7^{2-}$ equals the number of equivalents of $Fe^{2+}$.Equivalents = $Molarity 	imes n	ext{-factor} 	imes Volume (L)$.For $Fe^{2+}$,$n	ext{-factor} = 1$ (as $Fe^{2+} ightarrow Fe^{3+} + e^-$).For $Cr_2O_7^{2-}$,$n	ext{-factor} = 6$ (as $Cr_2O_7^{2-} + 14 H^+ + 6e^- ightarrow 2 Cr^{3+} + 7 H_2O$).Let $V$ be the volume in $L$ of $Cr_2O_7^{2-}$ solution.$\frac{1}{60} 	imes 6 	imes V = 0.1 	imes 1 	imes 0.1$$0.1 	imes V = 0.01$$V = 0.1 \ L$.

$100 \ mL$ of $0.1 \ M$ $Fe^{2+}$ solution was titrated with $\frac{1}{60} \ M$ $Cr_2O_7^{2-}$ solution in acid medium. What is the volume (in $L$) of $Cr_2O_7^{2-}$ solution consumed?

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