A 0.5224-g sample of an unknown monoprotic acid was titrated with 0.0998 M NaOH. The equivalence point of the titration occurred at 23.82 mL. Determine the molar mass of the unknown acid.

Verified step by step guidance

1. Identify that the problem involves a titration of a monoprotic acid with NaOH, where the equivalence point is reached when moles of acid equal moles of base.
2. Use the formula for moles of NaOH: \( \text{moles of NaOH} = M \times V \), where \( M \) is the molarity (0.0998 M) and \( V \) is the volume in liters (23.82 mL converted to liters).
3. Since the acid is monoprotic, the moles of acid will be equal to the moles of NaOH at the equivalence point.
4. Calculate the molar mass of the unknown acid using the formula: \( \text{Molar mass} = \frac{\text{mass of acid}}{\text{moles of acid}} \), where the mass of the acid is 0.5224 g.
5. Substitute the values obtained from the previous steps into the molar mass formula to find the molar mass of the unknown acid.