Answer :
a. Yes, If you dissolve 2.00 moles of KI in 1.00 liter of water, you will achieve a 2.00 M solution.
To determine whether dissolving 2.00 moles of KI (potassium iodide) in 1.00 liter of water will result in a 2.00 M (molar) solution, we need to understand the definition of molarity. Molarity (M) is defined as the number of moles of solute divided by the volume of the solution in liters:
[tex]\[ \text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}} \][/tex]
In this case, you are dissolving 2.00 moles of KI in 1.00 liter of water. However, we need to be precise about what the final volume of the solution is, not just the volume of water you started with.
When you dissolve a solute in a solvent, the final volume of the solution can be slightly greater than the initial volume of the solvent due to the volume occupied by the solute. However, for most practical purposes and in many educational contexts, we assume that the volume change is negligible unless explicitly stated otherwise.
- Analyzing the Situation: Solute: 2.00 moles of KI, Solvent: 1.00 liter of water
If the volume change is negligible, the final volume of the solution will be very close to 1.00 liter. Therefore, the molarity would be:
[tex]\[ \text{Molarity (M)} = \frac{2.00 \text{ moles}}{1.00 \text{ liter}} = 2.00 \text{ M} \][/tex]
