How many moles of HNO3 are required to prepare 5.0 liters of a 2.0 M solution of HNO3?

• A. 2.5 moles
• B. 10.0 moles
• C. 0.40 moles
• D. 5.0 moles

Answer: (B)

Verified step by step guidance

1. Identify the formula relating molarity (M), moles of solute (n), and volume of solution (V): \(M = \frac{n}{V}\), where \(M\) is molarity in moles per liter, \(n\) is moles of solute, and \(V\) is volume in liters.
2. Rearrange the formula to solve for moles of solute: \(n = M \times V\).
3. Substitute the given values into the equation: \(M = 2.0\, \text{M}\) and \(V = 5.0\, \text{L}\).
4. Calculate the moles of HNO3 required by multiplying the molarity by the volume: \(n = 2.0 \times 5.0\).
5. Interpret the result as the number of moles of HNO3 needed to prepare the solution with the specified concentration and volume.