1. The problem statement, all variables and given/known data For a chemistry lab, we're trying to find the amount of CaCO3 in an antacid table by measuring the change in pressure due to the reaction of CaCO3 with HCl to produce CO2. This question in the lab report is confusing me to no end... Let’s say the % concentrations of CaCO3 (Table 5) you obtain from trial #1 and #2 are in good agreement, while the concentration obtained from trial #3 is significantly higher. Can a wet flask or vial be responsible for such results? Answer by yes or no and explain in great detail. 2. Relevant equations Lab report PV=nRT 3. The attempt at a solution I feel as though the obvious answer is that the percentage concentration should go down, not up, since gas is lost and therefore final pressure is lower than it should be... but then again, why would water kickstart/affect the reaction in the first place if it's not water but HCl that the antacid reacts with? I'm just really confused with this question, any help would be enormously appreciated.