A tablet contains 0.500 g of NaHCO3. What volume of 0.1000 M stomach acid (HCl) could one tablet neutralize, assuming the reaction is NaHCO3 + HCl → NaCl + CO2 + H2O?

• A. 118.9 mL
• B. 29.8 mL
• C. 59.5 mL
• D. 100.0 mL

Answer: (C)

Verified step by step guidance

1. Write the balanced chemical equation for the reaction: \(\mathrm{NaHCO_3 + HCl \rightarrow NaCl + CO_2 + H_2O}\).
2. Determine the number of moles of \(\mathrm{NaHCO_3}\) in the tablet using its mass and molar mass: \(\text{moles} = \frac{\text{mass}}{\text{molar mass}}\).
3. Since the reaction shows a 1:1 mole ratio between \(\mathrm{NaHCO_3}\) and \(\mathrm{HCl}\), the moles of \(\mathrm{HCl}\) needed to neutralize the tablet are equal to the moles of \(\mathrm{NaHCO_3}\) calculated.
4. Use the molarity of the \(\mathrm{HCl}\) solution to find the volume of acid required: \(\text{Volume} = \frac{\text{moles of } HCl}{\text{molarity}}\).
5. Convert the volume from liters to milliliters by multiplying by 1000 to get the final volume of stomach acid that can be neutralized by one tablet.