You can purchase hydrochloric acid in a concentrated form that is 37.0% HCl by mass and that has a density of 1.20 g>mL. Describe exactly how to prepare 2.85 L of 0.500 M HCl from the concentrated solution.

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1. Calculate the moles of HCl needed using the formula: \( \text{Moles of HCl} = \text{Volume (L)} \times \text{Molarity (M)} \).
2. Determine the mass of HCl in the concentrated solution using the percentage by mass: \( \text{Mass of HCl} = \text{Mass of solution} \times 0.37 \).
3. Calculate the volume of the concentrated solution needed using its density: \( \text{Volume} = \frac{\text{Mass}}{\text{Density}} \).
4. Use the dilution equation \( M_1V_1 = M_2V_2 \) to find the volume of concentrated HCl needed, where \( M_1 \) and \( V_1 \) are the molarity and volume of the concentrated solution, and \( M_2 \) and \( V_2 \) are the molarity and volume of the diluted solution.
5. Measure the calculated volume of concentrated HCl and dilute it with water to a total volume of 2.85 L.