If 300 ml of 0.02 N H₂SO₄ is needed, how much of 0.5 N solution is required?

To determine how much of the 0.5 N H₂SO₄ solution is needed, we can utilize the concept of normality and the principle of dilution. The amount of acid required can be expressed using the equation:

N₁V₁ = N₂V₂

Where:

• N₁ is the normality of the first solution (0.02 N),

• V₁ is the volume of the first solution (300 ml),

• N₂ is the normality of the second solution (0.5 N),

• V₂ is the volume of the second solution that we want to determine.

By rearranging the equation to solve for V₂:

V₂ = (N₁V₁) / N₂

Substituting the known values into the equation:

V₂ = (0.02 N * 300 ml) / 0.5 N

V₂ = (6) / (0.5)

V₂ = 12 ml

This calculation shows that 12 ml of the 0.5 N solution is required to provide the equivalent amount of H₂SO₄ as found in 300 ml of the 0.02 N solution. Thus, the conclusion that