Balanced Equation Lab Report

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The Balanced Equation and Equation displays that the ratio of tartaric acid and sodium hydroxide is one to two moles respectively, which indicates that one mole of tartaric acid will react with two moles of sodium hydroxide. This demonstrates that the tartaric acid almost completely dissociates in two different stages within the NaOH solution; hence supporting that tartaric acid is diprotic. Also, by examining Table 3 which suggests that the ratio of H2C4H4O6 to NaOH 1 to 2, as the values resemble the theoretical values of NaOH and therefore the difference between the theoretical and experimental 1:2 molar concentration is 5.00 x 10-3M, while the difference in the number of moles is 8.0 x 10-4mol. Hence, the results indicate that tartaric acid…show more content…
The tartaric acid was diluted by a factor of ten reducing the molar concentration to 5.0 x 10-2M. Table 2 indicated that the average amount of titrant (NaOH) added to the diluted tartaric acid analyte was 18.75mL for the second endpoint to be detected. Further, by titrating NaOH against 20mL of diluted tartaric acid, the solution was neutralised to form the salt sodium tartrate and water, which is demonstrated in the following equation: H2C4H4O6(l) + 2NaOH(l)  C4H3O2Na2(aq) + 2H2O(l) As identified in Table 3 it was discovered that tartaric acid was a diprotic acid, as the molar ratio stated that one mole of tartaric acid reacted with two moles of sodium hydroxide (refer to the equation above). Also, the experimental molar concentration of NaOH was calculated to be 5.33 x 10-2M as indicated in Equation 5; however theoretical molar concentration of NaOH was 1.02 x 10-1M, which was a difference of 4.6%. Although the titre results were within 0.1mL of each other, the results in Table 2 displayed that the titre values differed; suggesting the practical consisted of flaws. With that said, the results from the titration supported that tartaric acid was a diprotic…show more content…
Secondly, using a digital burette and an auto pipette would remove parallax error and reduce inaccurate readings of volumes, which would improve the titre values. Thirdly, before conducting a titration it should be ensured that no air bubbles are present are present in the burette and also allowing for sufficient time to enable the second endpoint to be detected; minimising incorrect volumes in the burette, and titre results. Furthermore, the practical should be improved by ensuring that the correct rinsing and familiarising technique procedure is obeyed throughout the dilution and titration process to prevent impurities within apparatuses or solutions being diluted. Moreover, conducting the dilution and titration in a 20°C environment to increase the accuracy of the equipment; therefore reducing incorrect measurements and titre values. Another improvement would be to invert the solution a minimum of ten times before use to ensure a homogenous solution and thus allowing for more accurate titre results. Finally, utilising a concentration measuring instrument, which would verify the NaOH molar concentration; improving the titre results and calculations by reducing
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