Volume of M / 8 KMnO_4 solution required to react completely with 25.0 cm^3 of M / 4 FeSO_4 in acidic medium is.

Correct answer: D. 10.0 mL The balance ionic equation for the reaction is MnO_4^ - +5 Fe^ 2+ +8 H^ + Mn^ 2+ +5 Fe^ 3+ +4 H_2 O From the above equation it is clear that 1 mole of KMnO_4=5 moles of FeSO_4 . Apply molarity equation to balance the redox reaction aligned (M_1 V_1)/(n_1)(KMnO_4) & =(M_2 V_2)/(n_2)(FeSO_4) (1 × V_1)/(8 × 1) & =(1)/(4) × (25)/(5) V_1 & =(1 × 25 × 8)/(4 × 5) V_1 & =10 cm^3 or V_1=10.0 mL aligned

BITSAT 2024

Exam: BITSAT
Year: 2024
Subject: Chemistry
Chapter: Redox Reactions

BITSAT 2024 · Chemistry · Redox Reactions

Volume of M / 8 KMnO_4 solution required to react completely with...

Volume of

\mathrm{M} / 8 \mathrm{KMnO}_4

solution required to react completely with

25.0 \mathrm{ cm}^3

M / 4 \mathrm{FeSO}_4

in acidic medium is.

Options

A8.0 mL
B5.0 mL
C15.0 mL
D10.0 mL

Correct answer

D. 10.0 mL

Step-by-step solution

The balance ionic equation for the reaction is

\mathrm{MnO}_4^{-}+5 \mathrm{Fe}^{2+}+8 \mathrm{H}^{+} \longrightarrow \mathrm{Mn}^{2+}+5 \mathrm{Fe}^{3+}+4 \mathrm{H}_2 \mathrm{O}

From

the above equation it is clear that 1 mole of \mathrm{KMnO}_4=5

moles of

\mathrm{FeSO}_4

. Apply molarity equation to balance the redox reaction

\begin{aligned}\frac{M_1 V_1}{n_1}\left(\mathrm{KMnO}_4\right) & =\frac{M_2 V_2}{n_2}\left(\mathrm{FeSO}_4\right) \\ \frac{1 \times V_1}{8 \times 1} & =\frac{1}{4} \times \frac{25}{5} \\ V_1 & =\frac{1 \times 25 \times 8}{4 \times 5} \\ V_1 & =10 \mathrm{ cm}^3 \text{ or } V_1=10.0 \mathrm{ mL} \end{aligned}

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