Question

56, 50 ml of 0.01 M FeSO4 will react with what volume of 0.01 M KMnO, solution in acid medium? (1 mole KMnO4 requires 5 mole of FeSO4 for complete reaction) (a) 50 ml (b) 25 ml (c) 100 ml (d) 10 ml​

Answer 1

Answer:

10mL of 0.01M KMnO₄ is required to react with 50 ml of 0.01 M FeSO₄ in acidic medium.

Explanation:

Given that,

     Volume of FeSO₄,V₁= 50mL

       Molarity of FeSO₄ = 0.01M

      molarity of KMnO₄ =0.01M

We have to find volume of KMnO₄ (V₂)

the balanced chemical equation is,

2KMnO₄ + 10FeSO₄ + H₂SO₄  → 5Fe₂(SO₄)₃ + 2MnSO₄ + K₂SO₄ + 8H₂O

thus           Fe²⁺ → Fe³⁺ + e⁻

      Mn⁷⁺ + 5e⁻ → Mn²⁺

we know that normality is given by,

             Normality = n × molarity

where n is the number of electrons transferred.

                     N₁V₁ = N₂V₂

⇒ 1×0.01M×50mL = 5 ×0.01M×V₂

⇒                50mL = 5 V₂

                        V₂ =10mL

the required volume of KMnO₄ is 10mL.

Hence, option D is correct.