Data Recorded \begin{tabular}{|l|c|c|} \hline & Trial 1 & Trial 2 \\ \hline Mass of the flask & $150.50 \mathrm{~g}$ & $151.00 \mathrm{~g}$ \\ \hline Mass of flask \& crushed antacid & $151.00 \mathrm{~g}$ & $151.50 \mathrm{~g}$ \\ \hline Mass of crushed antacid & \\ \hline $\begin{array}{l}\text { Initial volume of } 1.0 \mathrm{M} \mathrm{HCl} \text { solution } \\ \text { (mL) }\end{array}$ & 50.00 & 50.00 \\ \hline \begin{tabular}{l} Final volume of $\mathrm{HCl}$ solution \\ \hline Molarity of $\mathrm{NaOH}$ solution \end{tabular} & $1.0 \mathrm{M}$ & $1.0 \mathrm{M}$ \\ \hline $\begin{array}{l}\text { Initial volume of } \mathrm{NaOH} \text { solution } \\ \text { (Burette Initial volume) (mL) }\end{array}$ & 0.00 & 0.50 \\ \hline $\begin{array}{l}\text { Final volume of } \mathrm{NaOH} \text { solution Burette } \\ \text { Final volume (mL) } \\ \text { Volume of } \mathrm{NaOH} \text { dispensed (mL) }\end{array}$ & 45.00 & 45.50 \\ \hline \end{tabular}

POST-LABORATORY QUESTIONS

1. For the same mass, which of the two antacids, Gaviscon® or milk of magnesia, is more effective against neutralizing the same amount of gastric juice? Justify your answer with calculations.

2. Given that the molarity of stomach acid is 0.155 M, calculate the volume of stomach acid that could be neutralized by two tablets of Tums. Each tablet contains 500 mg of CaCO3.

3. An antacid tablet weighs 2.10 grams. It requires 45.67 mL of 0.105 M of NaOH solution to react completely with the carbonate present in the tablet. Determine the mass of CaCO3 present in the tablet?

Can you write clearly and number the answers.