# If 26.223 mL of potassium permanganate solution is required to titrate 1.041 g of ferrous...

## Question:

If 26.223 mL of potassium permanganate solution is required to titrate 1.041 g of ferrous ammonium sulfate hexahydrate, {eq}FeSO_4(NH_4)_2SO_4 \cdot 6H_2O {/eq}, calculate the molarity of the {eq}KMnO_4 {/eq} solution.

{eq}MnO_4^- + 8H^+ + 5Fe^{2+} \rightarrow Mn^{2+} + 4H_2O + 5 Fe^{3+} {/eq}

## Equivalence Point:

In each titration experiment there are titrant and analyte reactants. The goal is to find the unknown moles or molarity of the analyte reactant. The analyte is reacted with the titrant until the equivalence point is reached. Both reactants are fully consumed at this point, so there is no limiting reactant. Numerically, this means that the molar quantities of the two reactants must be related here by the balanced stoichiometric ratio.

## Answer and Explanation:

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This question deals with a redox titration reaction, according to the given balanced equation:

{eq}\rm MnO_4^- + 8H^+ + 5Fe^{2+} \rightarrow...

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