What volume of 7.50 M HNO3 should be diluted to prepare 25.00 mL of a 2.00 M HNO3 solution?

• A. 25.00 mL
• B. 6.67 mL
• C. 9.33 mL
• D. 3.75 mL

Answer: (B)

Verified step by step guidance

1. Identify the known values: the concentration of the stock solution \(C_1 = 7.50\, M\), the desired concentration of the diluted solution \(C_2 = 2.00\, M\), and the final volume of the diluted solution \(V_2 = 25.00\, mL\).
2. Recall the dilution equation which relates the concentrations and volumes before and after dilution: \(C_1 \times V_1 = C_2 \times V_2\), where \(V_1\) is the volume of the stock solution needed.
3. Rearrange the dilution equation to solve for \(V_1\): \(V_1 = \frac{C_2 \times V_2}{C_1}\).
4. Substitute the known values into the equation: \(V_1 = \frac{2.00\, M \times 25.00\, mL}{7.50\, M}\).
5. Calculate \(V_1\) to find the volume of 7.50 M HNO3 required to prepare 25.00 mL of 2.00 M HNO3 solution.