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In many residential water systems, the aqueous Fe³⁺concentration is high enough to stain sinks and turn drinking water light brown. The iron content is analyzed by first reducing the Fe³⁺ to Fe²⁺ and then titrating with MnO₄⁻ in acidic solution. Balance the skeleton reaction of the titration step:\mathrm{Fe}^{2+}(a q)+\mathrm{MnO}_{4}^{-}(a q) \longrightarrow \mathrm{Mn}^{2+}(a q)+\mathrm{Fe}^{3+}(a q)

Respuesta :

The balanced equation is:

[tex]5Fe^{2+}+ Mno_{4} ^{-} + 8H^{+}[/tex] ⇒ [tex]Mn_{} ^{2+} +5 Fe_{} ^{3+}+ 4H_{2} O[/tex]

The unbalanced redox equation is as follows:

[tex]Fe^{2+}+ Mno_{4} ^{-}[/tex] ⇒ [tex]Mn_{} ^{2+} + Fe_{} ^{3+}[/tex]

Balance all atoms other than H and O.

[tex]5Fe^{2+}+ Mno_{4} ^{-}[/tex] ⇒ [tex]Mn_{} ^{2+} +5 Fe_{} ^{3+}[/tex]

The oxidation number of Fechanges from +2 to +3. The change in the oxidation number of Fe is 1. The change in the oxidation number of Mn is +7.

Now balance O atoms on LHS,

[tex]5Fe^{2+}+ Mno_{4} ^{-} + 8H^{+}[/tex] ⇒ [tex]Mn_{} ^{2+} +5 Fe_{} ^{3+}[/tex]

Now, balance hydrogen atoms on RHS,

[tex]5Fe^{2+}+ Mno_{4} ^{-} + 8H^{+}[/tex] ⇒ [tex]Mn_{} ^{2+} +5 Fe_{} ^{3+}+ 4H_{2} O[/tex]

This is the balanced chemical equation.

Learn more about oxidation number here;

https://brainly.com/question/10137167

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