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Hydrogen Peroxide

Oxalic acid, ...

Question

Oxalic acid, $H_{2} C_{2} O_{4}$ , reacts with paramagnet ion according to the balanced equation $5 H_{2} C_{2} O_{4} (a q) + 2 M n O_{4}^{-} (a q) ⇌ 2 M n^{2 +} (a q) + 10 C O_{2} (g) + 8 H_{2} O (l)$ . The volume in mL of $0.0162$ M $K M n O_{4}$ solution required to react with $25.0$ mL of $0.022$ M $H_{2} C_{2} O_{4}$ solution is:

A

13.6

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B

18.5

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C

33.8

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D

84.4

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Solution

The correct option is A $13.6$
In the reaction
$+ 7 M n O_{4}^{-} ⟶ {M n}^{+ 2}$
thus $n f = 5$
${+ 3 C}_{2} O_{4}^{2 -} ⟶ {+ 4 C O}_{2}$
$2. C^{+ 3} ⟶ C^{+ 4}$
$n f = 2 \times 1 = 2$
thus, by equation
$({K M n O}_{4}) M_{1} V_{1} {n f}_{1} = M_{2} V_{2} {n f}_{2} (H_{2} C_{2} O_{4})$
$0.0162 M \times V_{1} \times 5 = 0.022 M \times 25.0 m L \times 2$
$V_{1} = 13.58 m L ≃ 13.6 m L$
Thus $13.58$ $m L$ of ${K M n O}_{4}$ solution is required to react with $25.0$ $m L$ of $0.022 M$ $H_{2} C_{2} O_{4}$ solution.

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