Blank exp. Take a look at some more examples given below. • Take a small amount of the aspirin tablet and dissolve as much as you can in 3 drops of ethyl acetate. Experiment 11 Determination of Water Hardness with EDTA, E19. Aspirin Synthesis and Analysis Revised: 12/13/14 • Crush an aspirin tablet and place in a labeled, pre-weighed vial or test tube. The chemical structure of aspirin is shown below: Preparation. The Net Ionic Equation for the titration in this experiment: O H3C O O O H O H3C O O + OH O + H2O acetylsalycilic acid (aspirin) + hydroxide (C9H8O4) 3. Also include results for the determination of hypochlorite in bleach (mean molarity and its standard deviation). You can download the paper by clicking the button above. It is important to determine the percent ASA of aspirin since it presents the aspirin's potency as a drug. Chemistry Final. Well, this was one of the best examples of wherein, the use of aspirin to determine the end result was expended. (II) Discussion Back titration rather than direct titration was used because there was no suitable indicator for acetylsalicyclic acid and sodium hydroxide solution. Determination of Aspirin using Back Titration This experiment is designed to illustrate techniques used in a typical indirect or back titration. In this experiment the base used is sodium hydroxide (NaOH). Determination of Aspirin using Back titration Your report should follow the Lab Report format listed earlier in this manual. A back titration is a titration method where the concentration of an analyte is determined by reacting it with a known amount of excess reagent.The remaining excess reagent is then titrated with another, second reagent. Using 4.032g of salicylic acid 8.0mL of acetic anhydride on a hot bath the reaction was speeded up by the use of a catalyst phosphoric acid. The second titration's result shows how much of the excess reagent was used in the first titration, thus allowing the original analyte's concentration to be calculated. Objective: To determine the mass of aspirin in a commercially available aspirin tablet via titration.. Introduction: The chemical name for aspirin is acetylsalicylic acid, which has the structure below. You add an excess of base, heat the mixture so … total moles of NaOH added for hydrolysis: 0.0043mol moles of HCl added for back titration: 0.00147mol moles of excess NaOH still present: 0.00147mol moles of NaOH used for hydrolysis: 0.00283mol moles of acetylsalicylic acid: 0.00283mol mass of acetylalicylic acid: 0.498g total Record the mass of the aspirin tablet. Chemistry 101: Experiment 7 Page 1 Experiment Titration is an analytical method used to determine the exact amount of a substance by reacting that substance with a known amount of another substance. The fact that it is an acid allows us to quantify the amount of aspirin in a solution by using an acid-base titration. You will use the NaOH you standardized last week to back titrate an aspirin solution and determine the concentration of aspirin in a typical analgesic tablet. Determination of Aspirin using Back Titration This experiment is designed to illustrate techniques used in a typical indirect or back titration. Errors in concentrations directly affect the measurement accuracy. The completed reaction of a titration is usually indicated by a color change or an electrical measurement. Using 0.5 g of crushed powdered sample, N/2 NaOH & N/2 HCl std. After the tablet falls apart, add roughly 20mL of ethanol to dissolve the aspirin. METTLER TOLEDO Titration Guide 8 Avoiding Titration Errors b) Burette Size (volume) Burette size is an important factor in accurate titration analysis. 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