What is the total number of moles of NaCl(s) required to prepare 3.0 liters of a 2.0 M NaCl solution?

• A. 1.5 moles
• B. 0.67 moles
• C. 2.0 moles
• D. 6.0 moles

Answer: (D)

Verified step by step guidance

1. Recall that molarity (M) is defined as the number of moles of solute per liter of solution. The formula is \(M = \frac{\text{moles of solute}}{\text{liters of solution}}\).
2. Identify the given values: the molarity \(M = 2.0\,M\) and the volume of the solution \(V = 3.0\,L\).
3. Rearrange the molarity formula to solve for moles of solute: \(\text{moles of solute} = M \times V\).
4. Substitute the known values into the equation: \(\text{moles of NaCl} = 2.0\,M \times 3.0\,L\).
5. Calculate the product to find the total moles of NaCl required to prepare the solution.