How many moles of KCl are contained in each solution? a. 0.556 L of a 2.3 M KCl solution

Verified step by step guidance

1. Determine the formula for calculating moles from molarity and volume: \( \text{moles} = \text{molarity} \times \text{volume} \)
2. Identify the given values: Molarity (M) = 2.3 M, Volume (L) = 0.556 L
3. Substitute the given values into the formula: \( \text{moles} = 2.3 \text{ M} \times 0.556 \text{ L} \)
4. Perform the multiplication to find the number of moles of KCl.
5. Ensure the units are consistent and the final answer is in moles.

Key Concepts

Molarity (M)

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (mol/L) and is crucial for understanding how much solute is present in a given volume of solution. In this question, the molarity of the KCl solution is given as 2.3 M, indicating that there are 2.3 moles of KCl in every liter of solution.

Calculating Moles from Molarity

To find the number of moles of solute in a solution, you can use the formula: moles = molarity × volume. This relationship allows you to calculate the total moles of solute when you know the concentration and the volume of the solution. In this case, you would multiply the molarity of the KCl solution by the volume in liters to determine the moles of KCl present.

Volume Conversion

Volume must be in liters when using the molarity formula, as molarity is defined per liter of solution. If the volume is given in milliliters or another unit, it must be converted to liters to ensure accurate calculations. In this question, the volume of the KCl solution is given as 0.556 L, which is already in the correct unit for the calculation.