95 g of ClO_2 is dissolved in water to prepare a 0.25 M solution. What is the final volume of the solution in liters?

• A. 2.0 L
• B. 1.5 L
• C. 10.0 L
• D. 5.0 L

Answer: (D)

Verified step by step guidance

1. Identify the given information: mass of ClO_2 = 95 g, molarity (M) = 0.25 M, and you need to find the volume of the solution in liters.
2. Calculate the molar mass of ClO_2 by adding the atomic masses: Cl (approximately 35.45 g/mol) + 2 × O (approximately 16.00 g/mol). Use this to convert the given mass of ClO_2 to moles using the formula: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\).
3. Use the definition of molarity, which is \(M = \frac{\text{moles of solute}}{\text{volume of solution in liters}}\), and rearrange it to solve for volume: \(V = \frac{\text{moles}}{M}\).
4. Substitute the moles calculated from step 2 and the given molarity into the volume formula from step 3 to find the volume of the solution.
5. Express the final volume in liters, which will be the volume of the solution needed to prepare the 0.25 M solution from 95 g of ClO_2.