How many mL of 5.0 M nitric acid (HNO₃) are required to make 1.00 L of a 0.00100 M solution of HNO₃ (approximately the concentration of acid in acid rain)?

• A. 2.00 × 10^–4 mL
• B. 0.00500 mL
• C. 5.00 mL
• D. 0.200 mL
• E. none of the above

Answer: (D)

Verified step by step guidance

1. Identify the given information: You have a concentrated solution of nitric acid (HNO3) with a molarity of 5.0 M, and you need to prepare 1.00 L of a diluted solution with a molarity of 0.00100 M.
2. Use the dilution equation, which is \( C_1V_1 = C_2V_2 \), where \( C_1 \) and \( V_1 \) are the concentration and volume of the concentrated solution, and \( C_2 \) and \( V_2 \) are the concentration and volume of the diluted solution.
3. Substitute the known values into the dilution equation: \( (5.0 \, \text{M}) \times V_1 = (0.00100 \, \text{M}) \times (1.00 \, \text{L}) \).
4. Solve for \( V_1 \), the volume of the concentrated solution needed: \( V_1 = \frac{(0.00100 \, \text{M}) \times (1.00 \, \text{L})}{5.0 \, \text{M}} \).
5. Convert the volume \( V_1 \) from liters to milliliters by multiplying by 1000, since 1 L = 1000 mL.