Answer: The average wt. Titration- Analysis of Aspirin Tablets Objective: Determine the percentage of aspirin (acetylsalicylic acid) present in two different commercial tablets by titrating the solution with a base. titration compared to direct titration due to the inaccuracy in back titration. then I dived this by two, becuase in the reaction equation there are two molecules of NaOH for every aspirin which gives 0.012 then mass = moles x Mr = 0.012 x 180.2 = 2.18 g This study concluded with the necessity for quality control to use all these techniques for monitoring all medications which interring this region. %PDF-1.3 %���� 0 As with direct titrations, to calculate the result of a back-titration it is necessary to know the involved stoichiometric reactions, aside from the exact concentrations and the volumes. Using the volume of HCl needed to back-titrate each aspirin flask and the average HCl concentration determined in Step One, calculate … 00cm3 of 95% alcohol * 0. Calculate the volume of 0.050 M sulfuric acid which is required to naturalize the mixture? k=�M(��Io�hע�ü�ǴnPar���C�Ó��7R5��,�m=��jhҴk�@��H�DPv�� Lab calculations and post lab questions for the aspirin titration lab. #2 Report 4 years ago #2 The active agent in Aspirin is the salicylic acid, it is not an impurity. Determining the percentage purity of calcium carbonate in a sample of limestone.Introduction:In my experiment, I hoped to find the amount of calcium carbonate in some mineral limestone using the back titration … Mass of 1 mole of aspirin = 180.2g. 3. Experiment 8 Determination of Total Alkalinity of Soda Ash, E14. I did the initial calculations as follows. Determination of Aspirin using Back titration Your report should follow the Lab Report format listed earlier in this manual. n�8[W.�3���WV����*�.Q�>G>B�?�H�v�¹c�Q���w���%�KؒG�'k�Cy�X�-1����JfC��8ˀ"Z. Show samples of all calculations, identify any unknowns, report the average … Rep:? Identify, by name or formula, R 1 and R 2 in Equation 31.1 when the ester aspirin … 92 0 obj <>/Filter/FlateDecode/ID[<2520AF0FBADC88637D856D210B7A95CA>]/Index[73 36]/Info 72 0 R/Length 91/Prev 207156/Root 74 0 R/Size 109/Type/XRef/W[1 2 1]>>stream Original mass of aspirin sample .495 grams.-----Calculations for NaOH:.1046M NaOH 23.5ml + 15ml excess added = 38.5 ml Using total NaOH.1046 * 38.5ml (1L/1000ml) = .0040271 Moles of NaOH-----Calculations of HCL:.1268M HCL 3.4ml of HCL added … Name and describe the two Anatcids you have … Mass of weighed aspirin tablet. Show your calculations for the percentage of an aspirin tablet that is aspirin. n (Na 2 CO 3 (aq)) = 0.050 × 21.50 × 10 -3 = 1.075 × 10 -3 mol. Materials: * Balance * 2 aspirin samples from different brands * 50 cm3 conical flask * 10. I ��� \L��[���E ��� Z��,�6�ׯ\�o� (The Procedure Is As Described In The Experiment Below Using … ��L�_��;�IǃhïƘ��e�H���(]�����C�H�S�K3-HhN��%M��77W�� hެWmo�8�+��jE���N��7�k�j��J�)xiN!AIVW����1h��TQ��c�g���G�|�#h"XH"I��H#QH_�("�+E8c��~�E�A���'"��c�3IS��O���"+�x�L5v*�n0� b�����ҋ��*���\�����"�al4�"��|㞕�q���xbe냵q_�X�cz~IG����E2��'�珧��.`on�u�c:�I�g$�pp#�L�������DƗ ��qO~%Y�A�%�ƽ��v���z*-�V����^5�y �p:H��:�?�'��ڪ:�Kz�%� So I recently did a back-titration experiment in school to determine the amount of aspirin in a commercial brand of aspirin tablets. 1 mole NaOH has mass 40g. Experiment 9 Determination of Aspirin Using Back Titration, E16. ܻ�؊f�!/��M�����V A�T�52�$���u�9]u:3t�e�;]Բ�bi�.^��v���廓�+q�s��gb�kd�h�����=�g�B��ɱ��'���3�Av�_d�w�ޠ��������K�+�a�/`�c Assuming the aspirin is not contaminated with other acids, the titration allows you to quantitatively determine the purity of your aspirin. %%EOF From the diagram, we can start with the titration first and determine the amount of NaOH used. 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