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Transcript of Antacid Neutralization
3HCl(aq) + CaCO3 > 3HCO + CaCl3 Milk of Magnesia:
2HCl(aq) + Mg(OH)2 > 2HOH + MgCl2 Sample Question: If a 5 ml sample of 0.35 M of Milk of Magnesia reacted completely, how many moles of MgCl2 were formed? 5 ml(0.35 mol Mg(OH)2/1 L)(1 mol MgCl2/1 mol Mg(OH)2) = 0.002 mol MgCl2 Analysis During our experiments of the titrations, the outcome of our titrations of both Tums and Milk of Magnesium were both very differentiated between trials one and two. In the first trials of the two antacids, the results were 16.8 and 29.98
mililiters correspondingly as compared to the second trials where the results were 25.7 and 41.15 mililiters. The reason for our very different results were probably due to the fact that we had a lot of sources of error.
When we were doing our titrations for our Tums, we probably didn’t break up the Tums as much as we did for each experiment. We also didn’t use the exact same equipment for the experiments, probably messing up the results. We also did not use the same total amount of Antacid for every trial of our experiment. This all increased our results due to our sources of error. A lot of improvements we could make for next name are to first use all of the same equipment, take all of the data in one day, and make sure all of the measurements of the experimental variables are the same throughout. Cleaning the materials more thoroughly can also lead to better results as there will be less chances of excess acids are bases remaining. Conclusion In conclusion, our hypothesis was correct stating that the amount of HCl needed to neutralize the base in the antacid changes depending on its active ingredient. According to our results, more HCl was needed to neutralize the Milk of Magnesia than tums. How much Hydrochloric Acid(HCl) is needed to neutralize antacids with different active ingredients?