Two questions related to antacids

Question

In this experiment, the relative ‘strength’ of commercial antacids at neutralizing stomach acid is determined by titration with standard NaOH solution. The parietal cells (the acid secreting cells) in the stomach secrete hydrochloric acid at a concentration of about 0.155 M. To determine the amount of stomach acid neutralized by the antacid, an antacid tablet is added to excess stomach acid. In this technique, any acid left over (after neutralization by an antacid tablet) is titrated with standard NaOH solution using bromophenol blue indicator to determine the end point. An antacid tablet is weighed and placed into an exactly measured volume (V_a) of hydrochloric acid of know concentration (M_a). The excess acid is titrated with standard sodium hydroxide solution. The neutralization reaction is given by:

During the experiment the antacid is added to the flask with hydrochloric acid. The procedure states to bring the contents of the flask to a boil. 

1. If you were in a hurry and did not bring the contents to a boil, how would that affect the volume of NaOH titrated?
2. How would that affect the moles of hydrochloric acid neutralized by the antacid?

Answer 1

1. No reaction was given, but a common antacid is calcium carbonate which is only slightly soluble in water and may require higher temperatures to ensure that all the antacid dissolves and reacts with the hydrochloric acid. If the boiling step is left out, there would be insufficient neutralization of the acid and therefore would result in more NaOH than should be required.
2. For the same reason given above, fewer moles of HCl would be neutralized by the NaOH.