A 0.20 M solution contains 6.4 g of SO_2. What is the volume of the solution in liters?

• A. 0.80 L
• B. 1.00 L
• C. 2.00 L
• D. 0.50 L

Answer: (D)

Verified step by step guidance

1. Identify the given information: the concentration of the solution is 0.20 M (moles per liter), and the mass of SO_2 dissolved is 6.4 g.
2. Calculate the molar mass of SO_2 by adding the atomic masses of sulfur (S) and oxygen (O). The molar mass of SO_2 is calculated as: \(M_{SO_2} = 32.07 + 2 \times 16.00\) g/mol.
3. Convert the given mass of SO_2 to moles using the formula: \(n = \frac{\text{mass}}{\text{molar mass}} = \frac{6.4}{M_{SO_2}}\) moles.
4. Use the molarity definition to find the volume of the solution: \(M = \frac{n}{V}\), rearranged to \(V = \frac{n}{M}\), where \(V\) is the volume in liters, \(n\) is the number of moles, and \(M\) is the molarity.
5. Substitute the values of moles and molarity into the volume formula to calculate the volume of the solution in liters.