Final answer:
To calculate the volume of concentrated sulfuric acid required to prepare 0.5 N solution, one must use the normality concept, account for the acid's specific gravity and purity, and perform a dilution calculation using the molarity and normality equations.
Step-by-step explanation:
The question asks for the volume of concentrated sulfuric acid needed to prepare 200 ml of 0.5 N solution. To find this, we first need to understand the concept of normality, which depends on the equivalent weight of the solute. In the case of sulfuric acid (H₂SO₄), which has two acidic protons, the equivalent weight is half of its molecular weight. We also need to take into account the specific gravity and the purity percentage of the acid. With all this information, we can perform the necessary calculations for dilution.
To calculate this, you would need to use the formula: M1V1 = M2V2, where M1 and V1 are the molarity and volume of the concentrated solution, and M2 and V2 are the molarity and volume of the diluted solution. However, because we want to make a normal solution (0.5 N), we have to adjust the molarity of the concentrated sulfuric acid for the fact that it has two acidic protons. For a 98% sulfuric acid solution with a specific gravity of 1.84, the molarity can be calculated using its density and purity. Finally, using the adjusted molarity, you can solve for V1, the volume of the concentrated acid needed.