1)A typical commercial antacid tablet contains 0.350 g of CaCO3[MW=100.09 g/mol] as an active ingredient. How many moles of HClcould this tablet neutralize? 2)A student was analyzing an antacidtablet with a mass of 2.745 g. The student found that a 1.872 gsample of the tablet would neutralize 67.35 mL of stomach acid.Calculate how much stomach acid would be neutralized by the entiretablet. 3)A student determined that 29.43 mL of 0.132 M NaOH reactswith 25.0 mL of stomach acid. He dissolved a commercial tablet ofantacid into 180 ml of stomach acid and then removed a 20.0 mL ofthe resulting solution. The Titration of this 20 mL sample took9.56 mL of NaOH. Calculate volume of acid neutralized by antacid inthe 200mL sample. 4) A 0.248 g sample of antacid containing anunknown amount of triprotic base Al(OH)3 [MW=78.00 g/mol] wasreacted with 25.0 mL of 0.121 M HCl. The resulting solution wasthen titrated with 12.26 mL of 0.132M NaOH solution. Calculate themass percent of Al(OH)3 in the antacid sample
