Calculating Acetylsalicylic Acid Using Back Titration

My family has had many health issues, some that are treated with medication. For example my mother has suffered from migraines, that are caused by her allergies, she treats it by using acetylsalicylic acid, better know as, aspirin. To treat these occasional migraines my mother has always preferred Excedrin®, which is a pricier brand than other pain relievers. I have always wondered why aspirin differ in price, when according to their labels they have the same amount of acetylsalicylic acid. This contemplation led me toward my research question. The U.

S. Federal Food and Drug Administration, FDA, requires manufacturers to label the amount of each active ingredient, including acetylsalicylic acid, on their product’s labels. The purpose of this investigation is to determine the amount of acetylsalicylic acid in aspirin and pain reliever tablets, then compare it to the marketed amount; this investigation is to see whether the manufacturers’ claims are justified.

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BACKGROUND INFORMATION:Aspirin is a widely used pharmaceutical drug, it is so widely used that approximately 35,000 metric tonnes are produced, about 100 billion aspirin tablets, each year. Aspirin is a very effective antipyretic drug and as an analgesic, which relieves headaches, neuralgia and rheumatism. It is commonly used for regulating cardiovascular conditions with the recommendation of a medical psychiatrist.METHOLODOGY:Using back titration is a method that is most convenient for this experiment.

Since aspirin is known to be a very weak acid, and because of that would react slowly with NaOH, the titration to be difficult to get accurate at a reasonable time. It is best to use back titrations so that the end point is easier to view as well. A back titration is a method when an excess of standard solution is used to consume an analyte and then titrated with a second standard solution.EQUIPMENT:CHEMICAL REAGENTS:Hotplate stirrerAspirin tabletsConical Flask ( 250 mL )1.0 ± 0.01 M NaOH solutionPipette0.1 ± 0.

01 M HCl solutionBurettePhenol red indicatorStir plateVolumetric Flask ( 250 mL )PROCEDURE:Hydrolysis of AspirinWeight one aspirin, and then transfer it into a Erlenmeyer flask containing 25.0 mL of deionized water and 25.0 mL of 1.0 M NaOH.The mixture is then boiled for 10 minutes, for the hydrolysis of aspirin.The solution is cooled and then transferred into a 250 mL volumetric flask; where it is then diluted with deionized water.Steps 1-3 are repeated for each aspirin trial.

Chemical Reaction:2433574471145CH3CO2C6H4CO2H + 2NaOH(aq) CH3CO2Na(aq) + HOC6H4CO2Na(aq) + H2O(l)Back Titration25.0 mL of the aspirin solution is measured and then put in a 250 mL conical flask with 2 drops of phenol red indicator.Note the start point volume of the burrette.The aspirin solution is titrated using a 0.1 M HCl solution using a burrette. During the titration the solution is swired with s stir plate. The titration is complete once there was a color change, in this case from pink/purple to a pale yellow.

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Mark the end point volume of the burrette.Repeat steps 1-4 for each aspirin trial.Chemical Reaction:Blank Titration25.0 mL of 1.0 MNaOH is diluted with deionized water in a 250 mL volumetric flask.25.0 mL of the diluted solution is measured and then put in a 250 mL conical flask with 2 drops of phenol red indicator.

Note the start point volume of the burrette.The NaOH solution is titrated with a 0.1 M HCl solution using a burrette. During the titration the solution is swired with s stir plate. The titration is complete once there is a color change, in this case from pink/purple to a pale yellow. Mark end point value.Chemical Reaction:2687574441809NaOH(aq) + HCl(aq) NaCl(aq) + H2O(l)DATA:Tablet 1 ( Excedrin® )Average weight = 0.

67 ± 0.01 g-90169202054Average volume of HCl used = 19.0 ± 0.01mLTablet 2 ( Aspirin )Average weight = 0.20 ± 0.01 g-90169206252Average volume of HCl used =20.3 ± 0.

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01mLTablet 3(Econtrin)Average weight: 0.75 ± 0.01 g-90169186010Average volume of HCl used =22.4 ± 0.01mLBlank Titration-90169259697Average volume of HCl used =27.2 ± 0.01mLDATA ANALYSIS AND CALCULATIONS:To calculate the number of moles of NaOH that actually reacted with NaOH during the hydrolysis of the aspirin, by using a simple subtraction problem.

Since 1 mol of H+ ions react with 1 mol OH- ions the number of moles of NaOh reacting with acetylsalic acid will equal,(MHCl ×VHCl )(blank titration) – (MHCl × VHCl)(back titration).The results are as follows,Tablet 1 = ( 0.1 ± 0.01 x 0.0272 ± 0.01 ) – ( 0.1 ± 0.

01 x 0.0190 ± 0.01 ) = 0.00082mol HClTablet 2 = ( 0.1 ± 0.01 x 0.0272 ± 0.

01 ) – ( 0.1 ± 0.01 x 0.0203 ± 0.01 )=0.00000552 molHClTablet 3 = ( 0.1 ± 0.

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01 x 0.0272 ± 0.01 ) – ( 0.1 ± 0.01 x 0.0224 ± 0.01 ) =0.

00000609molHClFrom there the mole ratio of NaOH react is NaOH = 2 (no. of moles of acetylsalicylic acid). Which is calculated as follows,CH3COO-C6H4-COOH / NaOH = 1/2CH3COO-C6H4-COOH = NaOH x 1/2Tablet 1 = 0.00082 x 1/2 = 0.00041 molTablet 2 = 0.00000552 x 1/2 = 0.00000276 molTablet 3 = 0.

00000609 x 1/2 = 0.00000304 molLast step is to convert moles to mass by multiplying by the relative molecular mass.Tablet 1 = 0.00041 x 180 = 0.0738 gTablet 2 = 0.00000276 x 180 = 0.000497 gTablet 3 = 0.

00000304 x 180 = 0.000548 gTo fill fill the investigation the comparison to the actual value marketed on the label.Tablet 1: 0.25 gTablet 2: 0.081Tablet 3: 0.081LIMITATIONS OF THE INVESTIGATION:The most obvious limitation is the end point, although phenol red was the best indicator because of the pH it reads, the transition between pink and yellow takes time. The aspirin solution it self has a yellow tint and when adding the indicator, and that might have an effect when trying to find the pink to faint yellow transition the phenol red indicator is trying to show.

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When titrating there is a point where it is not pink nor yellow, and to find the exactly point where the solution turn the correct tint of yellow is not precise.While making the HCl and NaOH solutions, there is a limitation in accuracy. Although one can solve for the amount of chemical to dilute in deionized water, there is always going to be human error introduced. This is one point that could be different I can change for this investigation if I were to do so again. I would have usedAnother limitation this observation had was the equipment used to measure the solutions. Although the burettes and flask used are calibrated, they are not always completely accurate. The altercation with burettes comes when there is air in the burette’s stopcock, which is what interrupts the flow of the adding solution, which will in return give inaccurate results.

When pouring from one flask to another there are often drops on the inside side of the flask that are not taken to account when making calculation.

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