Prietha.Thavakumaran.Experiment3

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2080

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Dec 6, 2023

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SC/CHEM 2080: Analytical Chemistry Experiment 3: Acid-Base Titration Using An Indicator – Analysis of an Unknown Base Prietha Thavakumaran TA: Lisa Azzarello Date Performed: Thursday, October 19 th , 2023 Due: Friday, October 27 th , 2023
2 Abstract An acid-base volumetric titration was performed using a primary standard acid, KHP with an acid-base indicator to determine the concentration of an unknown base of NaOH (York, 2023). Three replicates were created, and the average volume delivered was 17.8 mL with a standard deviation of 0.0898 mL. Results Table 1. Acid-Base Titration Data: Observed and Calculated Unknown NaOH KHP Unknown #282 Initial Volume (mL) Final Volume (mL) Total Volume (mL) Concentration (mol/L) Volume of KHP (mL) Mass of KHP (g) M. W. (g/mol) *Moles (mol) *Concentration (mol/L) - - - - - 5.1068 204.2223 0.025006084 1.00024336 Trial 1 10.399 28.125 17.726 *1.410700891 25 - - - - Trial 2 13.6115 31.379 17.7675 1.407405882 25 - - - - Trial 3 12.601 30.499 17.898 1.397144038 25 - - - - Average 12.20383333 30.001 17.79716667 1.405083604 - - - - - Standard Deviation 1.64266402 1.683191017 0.089755687 0.007070488 - - - - - *Uncertainty - - - 0.003653217 - - 0.002 - 0.002194776 *95% Confidence Interval - - - ±0.017565483 - - - - - Three replicates were made and produced a mean of 17.8 mL ± 0.0898 mL (n=3). The average concentration of the unknown was 1.40 M ± 0.00365 M (n=3). *Sample calculations can be found in the Appendix. Three replicates were made and presented an average volume of 17.8 mL ± 0.0898 mL of an unknown NaOH. Furthermore, an average concentration of 1.40 M ± 0.00707 M was calculated with an uncertainty value of 0.00365. Equally important, a 95% confidence interval was calculated as ± 0.01757 M. Likewise, the concentration of KHP was calculated as 1.0024 M with an uncertainty value of 0.00219. Discussion The results of the experiment indicated that the average volume of the unknown NaOH delivered was 17.78 mL ± 0.0898 mL. The standard deviation suggests that the replicates are close in distribution and are accurate as well as precise as they approach the mean value.
3 Furthermore, the concentration of KHP and its uncertainty was calculated, as 1.00 M ± 0.000480516 M. The uncertainty was determined based on the possible error propagation of the analytical balance and 250 mL volumetric flask. The small uncertainty value of 0.0004 suggests that the calculated concentration is relatively precise and was calculated with a high level of accuracy. Other calculated measurements under similar conditions are likely to produce values close to the calculated concentration (Harris et al., 2020). Moreover, the average concentration of the unknown NaOH sample was calculated using the same mole value as KHP assuming it was a 1:1 ratio and the acid-base titration reaction was complete, resulting in equivalent moles. The average concentration of the unknown and its uncertainty was 1.405083604 M ± 0.00365321737 M. The uncertainty of the concentration was determined based on the errors associated with the burette which provided the volume delivered as well as the 25mL pipette in which the KHP was dispensed. The value is relatively small and provides confidence in precision and accuracy. In addition, the 95% confidence interval was calculated in relation to the concentration of the unknown, confidently revealed that the true population lies between 1.387518121 M to 1.422649087 M. An experimental procedure that provides the greatest uncertainty would be adding 25mL of KHP using the 25mL pipette. The KHP solution’s meniscus must be perfectly aligned with the 25mL mark of the pipette, however, the difficulty and inadequate training results in an inaccurate read and dispense of the solution. An adequate amount of practice and training with the equipment can reduce the uncertainty. In this acid-base titration, the equivalence point is reached when all of the KHP reacts with the NaOH, resulting in a neutral solution and an approximate pH of 7.0 which indicates neutrality. Phenolphthalein’s colour change occurs in a slightly basic range, making it an ideal candidate for this titration as it
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4 transitions from acidic (colourless) to slightly basic (pink) as the titration reaches its equivalence point (Harris et al., 2020). Appendix Sample Calculations: Concentration of KHP Mol = mass/M.W. = 5.1068 g / 204.223 g/mol = 0.025006084 mol [KHP] = mol/vol = 0.025006084 mol / 0.025 L = 1.00024336 mol/L Uncertainty of [KHP] e = x ! ( !" " ) # + ( !$ $ ) # = 1.00024336 ! & %.%%%’ (.’%)* # + ( %.’# #(% ) # = 0.004805161651 Concentration of Unknown NaOH C = mol/vol = 0.025006084 mol / 0.017726 L = 1.410700891mol/L Uncertainty of [Unknown NaOH] e = x ! ( !" " ) # + ( !$ $ ) #
5 = 1.405083604 ! ( %.%( (% ) # + ( %.%+ #( ) # = 0.00365321737 95% Confidence Interval C.I. = x ± ts/ √࠵? = 1.405083604 ± [ (4.303)( 0.007070488)/ √3 ]] = 1.405083604 ± 0.017565483 95% Confidence Interval Range: 1.387518121 M to 1.422649087 M
6 Reference Harris, Daniel C, and Charles A Lucy. Quantitative Chemical Analysis . 10th ed., New York, NY, Macmillan Learning, 2020. York University. Analytical Chemistry: Laboratory Manual, 2023.
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