What volume of a 1.00 M HCl solution is required to prepare 200.0 mL of a 0.250 M HCl solution?

• A. 200.0 mL
• B. 50.0 mL
• C. 100.0 mL
• D. 25.0 mL

Answer: (B)

Verified step by step guidance

1. Identify the known values: the concentration of the stock solution \(C_1 = 1.00\ \text{M}\), the concentration of the diluted solution \(C_2 = 0.250\ \text{M}\), and the volume of the diluted solution \(V_2 = 200.0\ \text{mL}\).
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: \(V_1 = \frac{0.250\ \text{M} \times 200.0\ \text{mL}}{1.00\ \text{M}}\).
5. Calculate \(V_1\) to find the volume of the 1.00 M HCl stock solution required to prepare 200.0 mL of 0.250 M HCl.