A titration is performed to determine the molar mass of an unknown solid monoprotic acid, with general formula HA. If 1.24 g of the acid requires 25.02 mL of a 0.500 M KOH solution to reach the end point, what is the molar mass of the acid? Report your answer with 2 decimal places, and do not include units.

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To determine the molar mass of the unknown monoprotic acid $$ \text{HA} $$, follow these steps:

1. **Calculate the moles of KOH used in the titration:**
   $$
   \text{Moles of KOH} = \text{Molarity} \times \text{Volume (in liters)} = 0.500\, \text{M} \times 0.02502\, \text{L} = 0.01251\, \text{mol}
   $$

2. **Determine the moles of HA, since the reaction ratio is 1:1:**
   $$
   \text{Moles of HA} = \text{Moles of KOH} = 0.01251\, \text{mol}
   $$

3. **Calculate the molar mass (M) of HA:**
   $$
   M = \frac{\text{Mass of HA}}{\text{Moles of HA}} = \frac{1.24\, \text{g}}{0.01251\, \text{mol}} \approx 99.12
   $$

**Final Answer:**  
99.12
The molar mass of the acid is 99.12.

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