In a similar experiment to yours, one tablet of Antacid A is titrated to its endpoint with 15.5 mL of 0.5 M HCl and one tablet of Antacid B is titrated to its endpoint with 24.3 mL of 0.5 M HCl. Which is the more effective antacid?
To determine which antacid is more effective, we need to compare the amount of acid neutralized by each antacid tablet. In this case, we can determine the effectiveness by comparing the volume of HCl solution required to reach the endpoint during titration.
In the given experiment, one tablet of Antacid A was titrated to the endpoint with 15.5 mL of 0.5 M HCl, while one tablet of Antacid B required 24.3 mL of 0.5 M HCl to reach the endpoint.
Now, let's calculate the amount of acid neutralized by each antacid tablet.
First, calculate the number of moles of HCl used in each titration:
Number of moles of HCl (Antacid A) = volume of HCl (Antacid A) * concentration of HCl (Antacid A)
= 15.5 mL * 0.5 mol/L
= 7.75 mmol (millimoles)
Number of moles of HCl (Antacid B) = volume of HCl (Antacid B) * concentration of HCl (Antacid B)
= 24.3 mL * 0.5 mol/L
= 12.15 mmol (millimoles)
Next, since each mole of HCl reacts with one mole of antacid, we can equate the number of moles of HCl used to the amount of acid neutralized by each antacid tablet:
Amount of acid neutralized (Antacid A) = Number of moles of HCl (Antacid A)
= 7.75 mmol (millimoles)
Amount of acid neutralized (Antacid B) = Number of moles of HCl (Antacid B)
= 12.15 mmol (millimoles)
Comparing the amounts of acid neutralized, we see that Antacid B neutralized a greater amount of acid than Antacid A. Therefore, based on the experimental data, Antacid B is more effective at neutralizing acid.