Q75 / 180 · JIPMER 2015 · Chemistry

$\mathrm{KMnO}_4$ reacts with ferrous sulphate according to the following equation, Figure Here, 10 mL of $0.1 \mathrm{MKMnO}_4$ is equivalent to

  • Correct answer
    A
    50 mL of $0.1 \mathrm{M} \mathrm{FeSO}_4$
  • B
    20 mL of $0.1 \mathrm{M} \mathrm{FeSO}_4$
  • C
    40 mL of $0.1 \mathrm{M} \mathrm{FeSO}_4$
  • D
    30 mL of $0.1 \mathrm{M} \mathrm{FeSO}_4$

Solution

For the reaction, $\mathrm{MnO}_4^{-}+5 \mathrm{Fe}^{2+}+8 \mathrm{H}^{+} \longrightarrow$ $\mathrm{Mn}^{2+}+5 \mathrm{Fe}^{3+}+4 \mathrm{H}_2 \mathrm{O}$ 5 times quantity of $\mathrm{Fe}^{2+}$ consumed than $\mathrm{KMnO}_4$. Thus, 10 mL of $0.1 \mathrm{M} \mathrm{KMnO}_4$ is equivalent to 50 mL of $0.1 \mathrm{M} \mathrm{FeSO}_4$.

Hence, the correct answer is option: 'A'.

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