Question

Acidified KMno4 oxidizes oxalic acid to carbon dioxide. what is the volume in ml of 1÷10M KMno4 required to completely oxidize 0.5 litres of 1÷100M oxalic acid in acid medium ????? nd pls solve this??​

Answer 1

Answer:

0.0334 litres (approx) or 0.1/3 litres

Explanation:

We need to know the balanced equation in order to calculate the volume of KMnO4

Oxalic acid = $\sf C_2H_2O_4$

The balanced equation is :-

$\sf\tiny{2KMnO_4 + 3C_2H_2O_4 \rightarrow K_2CO_3 + 2MnO_2 + 3 H_2O + 5CO_2}$

Here, 3 moles of oxalic acid requires 2 moles of KMnO4 for complete oxidation.

So, 1 mole of oxalic acid would require 2/3 moles of KMnO4 for complete oxidation.

Now, given moles of oxalic acid = molarity × volume (in litres)

→ moles of oxalic acid = 1/100 × 0.5

→ moles of oxalic acid = 0.005

Now, 1 mole of oxalic acid requires 2/3 moles of KMnO4.

So, 0.005 moles of oxalic acid would require 2/3 × 0.005 moles of KMnO4

= 0.01/3 mole

Now, mole = molarity × volume (in litres)

For KMnO4, let volume be V

So, 0.01/3 = 1/10 × V

→ V = 0.01/3 × 10

→ V = 0.1/3 Litres

→ V = 0.0334 litres (approx)

Answer 2

Answer:

20 L

this question is already asked in JEE exam so I think, you typed wrong data for concentration of KMnO4 ( 10^-2 M) while it should be 10^-4 M KMnO4 so I am correcting this data according to IIT-JEE exam and I am posting solution here according to 10^-4 M KMnO4 .

here's the answer and hope this helps you.