Equilibrium Molarity Lab Report

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Discussion/Conclusion: With the help of titration, the average molarity of acids and bases could be determined. Through some simple calculations, the average molarity of the base NaOH was found to be 0.13 M. This was a reasonable molarity because after equilibrium is reached, the equilibrium molarity is supposed to be smaller than the initial molarity, which was 10 M. This number was used in the calculations of the molarities of the HCl solution, which averaged to 0.043 M, and the molarities of the acetic acid solution, with averaged to 0.10 M. However, the volumes of the base that was needed to neutralize the acid greatly differed from each other in the three trials. This could have caused the molarities to be slightly different from what…show more content…
In the first part of the lab, the acid KHP was weighed in a weighing dish. One problem that arose from using the weighing dish was that it was difficult to get all of the KHP out. The weighing dish that was used had some small scratches on the bottom of it, and the KHP would get stuck in the crevices. The KHP also liked to stick to the weighing dish, so it was impossible to get all of it into the Erlenmeyer flask. This could have caused the average molarity of NaOH to be less than what it should be, which in turn would cause all of the other calculations to be inaccurate. For the other two parts of the lab, it was difficult to get all of the acid out of the graduated cylinder after it was measured. There was always a tiny bit remaining in the graduated cylinder. This affected the experiment by also making the molarities less than what they should have…show more content…
Because there was uncertainty in the amount of NaOH needed in the first trial, the rate of the titration was slower. However, for the second and third trials, the range of the volume of NaOH needed to neutralize the acid was known, so the titration process was faster. By increasing the rate of NaOH dripping into the acid solution, the pink color it created in the solution lasted for a longer period of time, but the color would fade after a few minutes. Since the color lasted longer than the required 30 seconds, the measurement of the volume was record. This caused the volume to decrease as the trials progressed, as seen in the data for the last two parts of the lab. Because the color faded, the titration process may not have been fully completed. This would have caused the molarities of the acids to be less than they should have been. Lastly, the water used may have not had a pH of exactly 7. Because the water used was just regular tap water and not distilled water, there could have been impurities that could affect the pH. If the pH of the water was higher than 7, then the molarities of the acids found would have been too low, and if the pH was lower than 7, then the molarities of the acids would have been too high. Although this would have only slightly affected the molarities, combined with the other factors listed above, it could have a big

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