Some antacid tablets actually contain a mixture of calcium carbonate and magnesium hydroxide (though
they usually have the same “strength” as those that only contain CaCO3). If this had been the case for the
antacid you tested, but you still assumed it only contained CaCO3, how would this have affected each of the
following (too high, too low, or no effect)? Explain.
a) Moles of HCl neutralized by the antacid
b) Mass percentage of CaCO3 in tablet.
If the antacid tablets actually contain a mixture of calcium carbonate (CaCO3) and magnesium hydroxide (Mg(OH)2), but we assume it only contains CaCO3, it would affect the following:
a) Moles of HCl neutralized by the antacid:
Assuming the tablets contain only CaCO3 when they actually have a mixture of CaCO3 and Mg(OH)2, this would result in underestimating the number of moles of acid that can be neutralized. Magnesium hydroxide (Mg(OH)2) is also an alkaline compound, and it can neutralize acid just like CaCO3. Therefore, the actual moles of HCl neutralized by the antacid would be higher than our assumption.
b) Mass percentage of CaCO3 in the tablet:
The mass percentage of CaCO3 in the tablet would also be affected. Assuming the tablet contains only CaCO3 when it actually contains a mixture of CaCO3 and Mg(OH)2 would result in a lower calculated mass percentage of CaCO3. This is because the actual tablet contains additional mass from the magnesium hydroxide. Therefore, our assumption would underestimate the mass percentage of CaCO3 in the tablet.
To accurately determine the moles of HCl neutralized by the antacid and the mass percentage of CaCO3 in the tablet, it is important to know the composition of the antacid accurately. This can be done through laboratory analysis or by checking the ingredient list on the antacid packaging.