According to the balanced chemical equation

5 H2C2O4(aq) + 2 MnO4-(aq) + 6 H+(aq) → 10 CO2(g) + 2 Mn2+(aq) + 8 H2O(l)

0.3500 grams of oxalic acid, H2C2O4 will react with ________ mL of 0.100 M potassium permanganate, KMnO4 solution.
A) 15.5 mL
B) 38.9 mL
C) 77.7 mL
D) 97.2 mL

Question

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Respuesta :

Mergus Mergus · Answer 1 · 2019-10-09T06:59:54+02:00

Answer:

A) 15.5 mL

Explanation:

Given, Mass of oxalic acid = 0.3500 g

Molar mass of oxalic acid = 90.03 g/mol

The formula for the calculation of moles is shown below:

[tex]moles = \frac{Mass\ taken}{Molar\ mass}[/tex]

Thus,

[tex]Moles= \frac{0.3500\ g}{90.03\ g/mol}[/tex]

[tex]Moles\ of\ oxalic\ acid= 0.0038876\ mol[/tex]

According to the given reaction:

[tex]5H_2C_2O_4_{(aq)}+2MnO_4^-_{(aq)}+6H^+_{(aq)}\rightarrow 10CO_2_{(g)}+2Mn^{2+}_{(aq)}+8H_2O_{(l)}[/tex]

5 moles of oxalic acid react with 2 moles of potassium permanganate

Thus,

1 mole of oxalic acid react with 2/5 moles of potassium permanganate

0.0038876 mole of oxalic acid react with [tex]\frac {2}{5}\times 0.0038876[/tex] moles of potassium permanganate

Moles of potassium permanganate = 0.001555 moles

Also, considering:

[tex]Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}[/tex]

Molarity = 0.100 M

So,

[tex]0.100=\frac{0.001555}{Volume\ of\ the\ solution(L)}[/tex]

Volume = 0.01555 L

Also, 1 L = 1000 mL

So, volume = 15.5 mL