How many liters of solution are required to prepare a 3.5 M hydrochloric acid solution using 1.1 moles of HCl?

• A. 0.31 L
• B. 0.39 L
• C. 3.2 L
• D. 1.1 L

Answer: (A)

Verified step by step guidance

1. Identify the known values: the molarity (M) of the solution desired is 3.5 M, and the amount of solute (HCl) available is 1.1 moles.
2. Recall the definition of molarity, which is the number of moles of solute divided by the volume of solution in liters: \(M = \frac{\text{moles of solute}}{\text{volume of solution in liters}}\).
3. Rearrange the molarity formula to solve for the volume of solution: \(\text{volume} = \frac{\text{moles of solute}}{M}\).
4. Substitute the known values into the rearranged formula: \(\text{volume} = \frac{1.1\ \text{moles}}{3.5\ M}\).
5. Calculate the volume using the expression above to find the liters of solution required to prepare the 3.5 M HCl solution.