Calcium Carbonate in Antacid: Why Higher Yield in Wet Flask?

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Using a wet flask to determine the concentration of calcium carbonate in antacid tablets results in a higher yield due to the reaction dynamics involving hydrochloric acid (HCl) and the calcium carbonate. The method involves measuring the pressure changes in the flask, which reflects the production of carbon dioxide (CO2) gas during the reaction. Although some calcium carbonate may react with water, the overall gas production can still be higher, as the pressure sensor captures the total gas pressure, including CO2 and other gases. The discussion emphasizes the importance of understanding gas laws and the role of partial pressures in accurately measuring gas yields. This method highlights the complexities of chemical reactions and gas behavior in a controlled environment.
lmlgrey
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1. When determining the concentration of calcium carbonate in an antacid tablet, why using a wet flask will end up with a significant higher concentration?



2. Gas laws



I would expect a lower yeild of gas since some of the calcium carbonate reacts with water and escape from the tube...but higher??
 
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Can you describe the method that you are using? It's hard to answer without knowing how you determine the concentration of calcium carbonate.
 
A reaction happened between HCl and antacid (which contains calcium carbonate) and the reaction flask was equipped with a pressure detector... by calculating the difference between # of moles of gas in the flask before and after(nf-ni=(pf'/Tf-pi'/Ti)*V/R...
 
Your pressure sensor measures the pressure of every gas within the flask. It is more proper to say that you are measuring the partial pressure of CO2. What other gases are present in the flask?
 

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