How many liters of solution are required to prepare a 1.66 M solution containing 2.11 moles of KMnO4?

• A. 1.27 L
• B. 0.79 L
• C. 0.35 L
• D. 3.50 L

Answer: (A)

Verified step by step guidance

1. Identify the given information: the molarity (M) of the solution is 1.66 M, and the amount of solute (KMnO4) is 2.11 moles.
2. Recall the definition of molarity, which relates moles of solute to liters of solution: \(M = \frac{\text{moles of solute}}{\text{liters of solution}}\).
3. Rearrange the molarity formula to solve for the volume of solution: \(\text{liters of solution} = \frac{\text{moles of solute}}{M}\).
4. Substitute the known values into the rearranged formula: \(\text{liters of solution} = \frac{2.11}{1.66}\).
5. Calculate the volume to find how many liters of solution are required to prepare the 1.66 M solution containing 2.11 moles of KMnO4.