Commercially available sulphuric acid contains 93% acid by mass and has a density of 1.84 g `mL^(-1)`.
Calculate (i) the molarity of the solution (ii) volume of concentrated acid required to prepare 2.5 L of 0.50 M `H_(2)SO_(4)`

Explanation

To solve the problem, we need to calculate the molarity of the sulfuric acid solution and the volume of concentrated acid required to prepare a specific volume of diluted solution. Let's break this down step-by-step.

### Step 1: Calculate the Molarity of the Sulfuric Acid Solution

1. **Determine the mass of sulfuric acid in 1 liter of solution**:
- Since the density of the solution is given as 1.84 g/mL, the mass of 1 liter (1000 mL) of the solution can be calculated as:
\[
\text{Mass of solution} = \text{Density} \times \text{Volume} = 1.84 \, \text{g/mL} \times 1000 \, \text{mL} = 1840 \, \text{g}
...