The normality of solution obtained by mixing 100 ml of 0.2M H2SO4 with 100 ml of 0.2 M NaOH is what?

 
We know, equivalent weight = molar mass / basicity
Basicity of sulphuric acid is two.
So 1 mol H₂SO₄ = 2 equivalent
 
Therefore 1 M H₂SO₄ = 2N H₂SO₄
Now, 100 ml of 0.2M H₂SO₄ ≡ 100X0.2 ml of 1 M H₂SO₄
  ≡ 20 ml of 2 N H₂SO₄
  ≡ 20X2 ml of 1N H₂SO₄
  ≡ 40 ml of 1N H₂SO₄
And
1M NaOH = 1 N NaOH
 So, 100 ml of 0.2 M NaOH ≡ 100X0.2 ml of 1M NaOH
    ≡ 20 ml of 1N NaOH
 
When acid and base are mixed, neutralisation will occur to produce salt and water.
 
20 ml of 1N NaOH ≡ 20 ml of 1N H₂SO₄
 
Rest acid = 20 ml 1N H₂SO₄,
 
Final volume of the solution is 200 ml.
 
If final strength of acid is S then
 
20 ml X 1N=200 ml X S
Or, S= 0.1 N
 
Final normality of the solution is 0.1N