You can purchase nitric acid in a concentrated form that is 70.3% HNO3 by mass and has a density of 1.41 g>mL. Describe exactly how you would prepare 1.15 L of 0.100 M HNO3 from the concentrated solution.

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1. Calculate the number of moles of HNO3 needed using the formula: \( \text{moles} = \text{molarity} \times \text{volume} \). Convert the volume from liters to milliliters if necessary.
2. Determine the mass of HNO3 required using the molar mass of HNO3 (63.01 g/mol).
3. Calculate the volume of the concentrated HNO3 solution needed using its density and the percentage by mass. Use the formula: \( \text{mass} = \text{density} \times \text{volume} \) and \( \text{mass of HNO3} = \text{mass of solution} \times \text{percentage by mass} \).
4. Convert the mass of HNO3 to volume using the density of the concentrated solution.
5. Dilute the calculated volume of concentrated HNO3 to a final volume of 1.15 L with distilled water, ensuring thorough mixing.