(c) Given the following half reactions: MnO4-(aq) + 8H+(aq)...

(c) Given the following half reactions: MnO4-(aq) + 8H+(aq) + 5e- -> Mn2+(aq) + 4H2O(l); Fe3+(aq) + e- -> Fe2+(aq). (i) Write a balanced ionic equation for the reaction between MnO4- and Fe3+. (2 marks) (ii) Determine the concentration of Fe2+ given that 24.30 cm3 of 0.02 M KMnO4 reacted with exactly 20.00 cm3 of Fe2+ solution to reach end point. (5 marks)

A 50.00 -mL sample of solution containing $\mathrm{Fe}^{2+}$ ions is titrated with a 0.0216 $\mathrm{M} \mathrm{KMnO}_{4}$ solution. It required 20.62 $\mathrm{mL}$ of $\mathrm{KMnO}_{4}$ solution to oxidize all the $\mathrm{Fe}^{2+}$ ions to $\mathrm{Fe}^{3+}$ ions by the reaction $$\mathrm{MnO}_{4}^{-}(a q)+\mathrm{Fe}^{2+}(a q) \stackrel{\text { Acidic }}{\longrightarrow} \mathrm{Mn}^{2+}(a q)+\mathrm{Fe}^{3+}(a q) \text{(Unbalanced)} $$ a. What was the concentration of $\mathrm{Fe}^{2+}$ ions in the sample solution? b. What volume of 0.0150$M \mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}$ solution would it take to do the same titration? The reaction is $$\mathrm{Cr}_{2} \mathrm{O}_{7}^{2-}(a q)+\mathrm{Fe}^{2+}(a q) \stackrel{\mathrm{Acidic}}{\longrightarrow} \mathrm{Cr}^{3+}(a q) +\mathrm{Fe}^{3+}(a q) \text {(Unbalanced)} $$

Question

Please give Ace some feedback