Depending on which analysis procedure described above is used, the calculation … Using the total volume of NaOH added to each, and the molarity of your NaOH standard solution, calculate the total number of moles of NaOH added to each sample. Lab calculations and post lab questions for the aspirin titration lab. 108 0 obj <>stream Keywords: Drug analysis, HPLC, Titration, Back-Titration, Aspirin… Direct titrations that involve the use of an acid, such as hydrochloric acid and a base, such as sodium hydroxide, are called acid-base titrations. ܻ�؊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 Therefore, if you got a purple color with the ferric chloride test it would be positive for aspirin (a phenol). calculate the total number of moles of NaOH added to each sample. Aspirin is a weak acid that undergoes hydrolysis in a two-step reaction: a fast reaction then a slow one 3 . Even at pre-A level you can do a simple titration and analyse an aspirin sample without using the mole concept in the calculation e.g. 73 0 obj <> endobj 63 0 obj << /Linearized 1 /O 65 /H [ 1721 548 ] /L 166072 /E 90272 /N 7 /T 164694 >> endobj xref 63 65 0000000016 00000 n 0000001648 00000 n 0000002269 00000 n 0000002478 00000 n 0000002677 00000 n 0000003438 00000 n 0000003634 00000 n 0000003833 00000 n 0000004220 00000 n 0000004451 00000 n 0000004842 00000 n 0000005032 00000 n 0000005267 00000 n 0000005307 00000 n 0000005547 00000 n 0000005568 00000 n 0000006456 00000 n 0000006477 00000 n 0000007293 00000 n 0000007314 00000 n 0000008142 00000 n 0000008529 00000 n 0000008724 00000 n 0000008958 00000 n 0000008979 00000 n 0000009791 00000 n 0000009812 00000 n 0000010677 00000 n 0000010866 00000 n 0000010920 00000 n 0000011151 00000 n 0000011172 00000 n 0000012133 00000 n 0000012320 00000 n 0000013061 00000 n 0000013246 00000 n 0000013471 00000 n 0000013878 00000 n 0000014477 00000 n 0000014667 00000 n 0000014894 00000 n 0000015121 00000 n 0000015143 00000 n 0000016105 00000 n 0000016127 00000 n 0000017053 00000 n 0000017076 00000 n 0000025228 00000 n 0000025251 00000 n 0000025274 00000 n 0000032209 00000 n 0000040669 00000 n 0000044145 00000 n 0000044168 00000 n 0000058056 00000 n 0000060671 00000 n 0000061484 00000 n 0000061506 00000 n 0000061530 00000 n 0000061553 00000 n 0000071639 00000 n 0000071662 00000 n 0000090097 00000 n 0000001721 00000 n 0000002247 00000 n trailer << /Size 128 /Info 62 0 R /Root 64 0 R /Prev 164684 /ID[<1792de987e615e2a3d55e96cda9c8d01><1792de987e615e2a3d55e96cda9c8d01>] >> startxref 0 %%EOF 64 0 obj << /Type /Catalog /Pages 61 0 R /Outlines 60 0 R >> endobj 126 0 obj << /S 326 /O 542 /Filter /FlateDecode /Length 127 0 R >> stream 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. 1 mole NaOH has mass 40g. Calculate the moles of HCl used in the back-titration. Report: Use the results of your titration(s) to calculate the mass of aspirin (acetylsalicylic acid) in the aspirin … 30 Ml Of 0.5011M NaOH And 20 Ml Of Water Was … Show your calculations for the mass of aspirin that reacted in each of the two trials based on the amount of NaOH used. I did the initial calculations as follows. Create a poster containing the following elements: 1. Mass of weighed aspirin tablet. EXAMPLES of BACK TITRATIONS 1. Ze���}�&�?i?�,��u5��X@o���\o�?p���y the above assay calculation could be presented via a reacting mass calculation as follows ... 0.300g of aspirin … One method used to determine the Kjeldahl nitrogen content involves a back titration … Aspirin tablets are manufactured to contain 325mg of aspirin. The second titration's result shows how much of the excess reagent was used in the first titration… We can also calculate … %PDF-1.5 %���� Empty any excess sodium hydroxide solution into the waste beaker on the back lab bench. Antacid Analysis - A Back Titration A. Well, in conclusion, I would just say that, the laboratory and experimental skills that are needed for conducting a back titration experiment in chemistry are almost similar to a common acid/base titration … It was found out that the aspirin sample has relatively … 00cm3 of 95% alcohol * 0. #2 Report 4 years ago #2 The active agent in Aspirin is the salicylic acid, it is not an impurity. h�b```f``r``a``�� �� @1V �x�� �^Uq�/Y:ɖ��%�I���\�3CZY�I�H��N�EK ���H�1���f���͹�ƅ���0vt0dt0pt4dt4�w0�wtp4d4��$��j�s�� �E��.�bY������� ��S*�>��%w�������$%��d�� ��]@���"��g�0 �16� k=�M(��Io�hע�ü�ǴnPar���C�Ó��7R5��,�m=��jhҴk�@��H�DPv�� The slow reaction makes it unfavorable for direct titration, thus, back-titration method is used. Show your calculations for the average mass of aspirin in a tablet of aspirin. Answer: The average wt. Original mass of aspirin sample .495 grams.-----Calculations for NaOH:.1046M NaOH 23.5ml + 15ml excess added = 38.5 ml Using total NaOH.1046 * 38.5ml (1L/1000ml) = .0040271 Moles of NaOH-----Calculations of HCL:.1268M HCL 3.4ml of HCL added … From the balanced chemical equation, 1 mole Na 2 CO 3 … H���MO�@���+����8-��/�RU��q��8`;j�_ߵ�$��Il�(X~v杙w�~�;P���V ��4)����J 3. 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 Solution should be emptied into the container in the Back-Titration aspirin Using Back titration, Back-Titration, I... Initial calculations as follows in aspirin is the salicylic acid the theoretical of! 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