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Unformatted text preview: indicator was added to the solution and it was then titrated with NaOH until an equivalence point was reached. Because NaOH only reacts with the excess of HCl, the number of moles of NaOH is equal to the excess moles of HCl that did not react with the base in the antacid. We found the percent composition of CaCO3, the active ingredient, to be around 40 percent for both antacid tablets. The balanced net ionic equation for this reaction is H + + OH- H 2 0 and the equilibrium constant expression is K= [CO 2 ][CaCl 2 ] [HCl][CaCO 3 ] Some possible sources of error in this experiment could be the molarity in both part 2 and part 3. In part 2, if the concentration of NaOH was incorrect, this would affect the percent of acetic acid in the vinegar. In part 3, if the antacid tablet did not completely dissolve in the HCl causing the neutralization capacity to be lower than it actually is.\...
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This note was uploaded on 04/02/2008 for the course CHEM 1A taught by Professor Van koppen during the Fall '07 term at UCSB.
- Fall '07
- Van Koppen