Diprotic Acid Essay

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Diprotic Acid Abstract: In this experiment, the total amount of acid neutralized by a solution containing both Na2CO3 and NaHCO3 was determined followed by using the information to calculate the concentrations of carbonate and bicarbonate ions in the solution. This was done by equipping LoggerPro with a pH sensor and a drop counter in order to calculate the pH levels after every single drop. Three titrations were performed for analysis: a titration of a known acid with Bromothymol blue indicator, a titration of an unknown acid with Bromothymol indicator, and a titration of an unknown acid with phenolphthalein. The indicators were added for comparison between color indicators and pH titrations. The results showed that the concentration of Na2CO3 in the unknown acid is between 0.03152M and 0.03924M, and the concentration of NaHCO3 is between 0.02148M and 0.02924M. By comparing the results between pH titration and color indicators, it is evident that the determination by pH titration is more efficient to use because it provides the exact point of equivalence between the dissociated ions and the dissociating molecules. In conclusion, this lab provided a more in depth understanding of how equilibriums and concentration are intertwined with pH and volumes. Introduction: Although the primary goal of the experiment is to find out how much acid is neutralized by a solution with both Na2CO3 and NaHCO3, the significant question to be answered is how can that information be used when dealing with an unknown acid? The purpose was then to use any information that was obtained in the previous experiment in order to answer this question. To begin, the equation CO32-aq+ H2Ol⟺HCO3aq+ OH-(aq), provides some insight when compared with the equation, HCO3-aq+H2Ol ⟺ H2CO3aq+OH-(aq). The first equation is the dissociation of carbonate into bicarbonate, and the second equation is
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