Question

How many grams of KMnO4 will react with 50 ml of 0.2 M H2C2O4 solution in the presence of H2SO4??

Answer 1

THE SOLUTION IS HERE....

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Answer 2

We have to find the mass in grams of KMnO4 will react with 50ml of 0.2M of H2C2O4 solution in the presence of H2SO4.

Solution : first of all balance chemical reaction.

step 1 : 10H⁺ + 10e¯ + 3H2SO4 + 2KMnO4 => K2SO4 + 2MnSO4 + 8H2O .......(1)

step 2 : 5H2C2O4 => 10CO2 + 10H⁺ + 10e¯ .....(2)

adding equations (1) and (2) we get,

3H2SO4 + 2KMnO4 + 5H2C2O4 => K2SO4 + 2MnSP4 + 8H2O + 10CO2

given mole of H2C@O4 = 0.2M × 50ml/1000

= 10/1000 = 0.01 mol

here 2 moles of potassium permanganate react with 5 moles of H2C2O4.

0.01 mol of H2C2O4 , reacts with 2/5 × 0.01 = 0.004 mol of KMnO4.

mass of KMnO4 = 0.004 × molar mass of KMnO4

= 0.004 × 158 = 0.632 g

Therefore 0.632 g of KMnO4 will react with 50ml of 0.2M H2C2O4 solution in the presence of H2SO4.