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Molarity

Determine the...

Question

Determine the volume of $M / 8 K M n O_{4}$ solution (in $m L$ ) that required to react completely with $25.0 c m^{3}$ of $M / 4 F e S O_{4}$ solution in acidic medium.

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Solution

The balanced ionic equation for the reaction is,
$M n O_{4}^{-} + 5 F e^{2 +} + 8 H^{+} \to M n^{2 +} + 5 F e^{3 +} + 4 H_{2} O$
From the balanced ionic equation, it is evident that 1 mole of $K M n O_{4}$ require 5 moles of $F e S O_{4}$ , applying law of chemical equivalence, we get
$M_{1} V_{1} n_{1} (K M n O_{4}) = M_{2} V_{2} n_{2} (F e S O_{4})$
(where $n$ is n-factor)
so, $\frac{1}{8} \times V_{1} \times 5 = \frac{1}{4} \times 25 \times 1$
$V_{1} = 10 c m^{3}$
or $V_{1} = 10 m L$

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