In the image you provided, the problem seems to involve a calculation related to molarity, with a mass of 0.65 g and molar mass (M) of 108.16 g/mol.

Your work shows the following steps:

1. You start by converting the mass (0.65 g) to moles using the molar mass (108.16 g/mol), which you do correctly: $\frac{0.65 \, \text{g}}{108.16 \, \text{g/mol}} = 0.00601 \, \text{mol}$

2. You then calculate the molarity by dividing moles by volume in liters. However, it seems there's a problem in the volume conversion that leads to a final molarity of 0.02404 M.

Error Explanation:

The volume you are using for the final molarity calculation isn't clearly shown in the image, but the problem might lie in the incorrect assumption or error in converting the volume to the correct unit (liters). The molarity is calculated as: $\text{Molarity} = \frac{\text{moles}}{\text{volume in liters}}$ If the volume is not in liters or is incorrectly handled, this could lead to an error in your result.

Steps for correction:

1. Double-check the volume you're using for the molarity calculation. Ensure that it is in liters, not milliliters or any other units.
2. If the volume was given in milliliters, you should divide by 1000 to convert it to liters.

Would you like further clarification on this? Let me know if you'd like more details on any specific part of the solution.

Additional questions to explore:

1. How do you convert grams to moles?
2. How do you properly convert milliliters to liters for molarity calculations?
3. Can you explain the significance of the pKa value in this type of problem?
4. What is the molarity equation, and how do you apply it in other scenarios?
5. How does knowing the molar mass affect your calculation?

Tip: Always ensure your units are consistent, especially when working with concentration and volume in molarity calculations.