CO2 forms from water and antacid tablet

[grantaere]

Homework Statement

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.

Homework Equations

https://docs.google.com/file/d/0By9VwoUlJRdCMzgxYjM1YzQtODA3MS00YmM5LWJiNjYtYmRlNDUwNDNjYTI3/edit
PV=nRT

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.

 

[Bystander]

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...

Develop this idea --- you're doing fine.

why would water kickstart/affect the reaction in the first place

This is what's bothering you? Ever see an Alka-Seltzer commercial?

 

[grantaere]

I just went and watched the commercial and I see that yeah, water does react quite strongly with the antacid tablet. I'm still not understanding the reaction going on here there, though- does calcium carbonate react spontaneously with water to form CO2? (I was under the impression that it's insoluble, but I could be wrong...)

 

[Quantum Defect]

This is what's bothering you? Ever see an Alka-Seltzer commercial?

Alka-seltzer contains sodium bicarbonate and citric acid. http://en.wikipedia.org/wiki/Alka-Seltzer
If this is the kind of tablet being used, then water alone could initiate the reaction between the bicarbonate and the citric acid. Since the instructions say that a little water could start the premature evolution of gas, this is likely the kind of antacid that they have given you. You are correct that CaCO3 is insoluble in water (this is what seashells are made of, after all).

Bystander is correct, though, with the statement that you are on the right track with your idea about the final pressure being lower.

 

[DeeNos]

It is possible that a wet flask or vial could be responsible for the higher concentration obtained in trial #3. This is because the presence of water can affect the reaction between CaCO3 and HCl. When water is present, it can react with the HCl to produce H2O and CO2, which can contribute to the overall pressure change and make it seem like there is more CO2 being produced from the reaction between CaCO3 and HCl. This can lead to a higher concentration being calculated.

Another possibility is that the wet flask or vial could introduce impurities or contaminants that can react with the HCl and produce additional CO2. This would also contribute to a higher concentration being calculated.

To avoid these potential sources of error, it is important to make sure that all equipment used in the experiment is completely dry and free of any impurities or contaminants. This will ensure that the only reaction taking place is between the CaCO3 and HCl and that the resulting concentration is accurate. Additionally, repeating the experiment multiple times and taking the average of the results can help to reduce the impact of any potential errors caused by a wet flask or vial.