Aspirin (acetylsalicylic acid) is a synthetic organic derived from salicylic acid. The reaction that is used for the synthesis is shown here. HO. HO, HO. HO, Salicylic acid Acetic anhydride Aspirin Acetic acid Answer the following questions based on the reaction above. Salicylic acid = C;H6O3, acetic anhydride = C4H603, aspirin = C9H3O4, acetic acid = HC2H3O2 %3D %3D %3D 7. Fill in all 3 stoichiometric conversions that properly calculate how many grams of aspirin willI be made from 12.5 g C,H6O3. Molar masses: C,H6O3 - 138.12 g/mol, C4H6O3 - 102.09 g/mol, aspirin – 180.15 g/mol C7H6O3 + C4H6O3 → C9H8O4 + HC2H3O2 12.5 g C7H603 x- 16.3 g aspirin Limiting Reagent Problem Using the same chemical equation for the synthesis of aspirin, determine how much aspirin is made from 6.20 g of C;H6O3 and 4.05 g of C4H6O3. Fill in each conversion train to figure out how much aspirin would be produced from each of those starting quantities of reactants. g C,H,03 × g aspirin g C4H603 x g aspirin

Aspirin (acetylsalicylic acid) is a synthetic organic derived from salicylic acid. The reaction that is used for the synthesis is shown here. HO. HO, HO. HO, Salicylic acid Acetic anhydride Aspirin Acetic acid Answer the following questions based on the reaction above. Salicylic acid = C;H6O3, acetic anhydride = C4H603, aspirin = C9H3O4, acetic acid = HC2H3O2 %3D %3D %3D 7. Fill in all 3 stoichiometric conversions that properly calculate how many grams of aspirin willI be made from 12.5 g C,H6O3. Molar masses: C,H6O3 - 138.12 g/mol, C4H6O3 - 102.09 g/mol, aspirin – 180.15 g/mol C7H6O3 + C4H6O3 → C9H8O4 + HC2H3O2 12.5 g C7H603 x- 16.3 g aspirin Limiting Reagent Problem Using the same chemical equation for the synthesis of aspirin, determine how much aspirin is made from 6.20 g of C;H6O3 and 4.05 g of C4H6O3. Fill in each conversion train to figure out how much aspirin would be produced from each of those starting quantities of reactants. g C,H,03 × g aspirin g C4H603 x g aspirin

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter14: Acid-base Equilibria

Section: Chapter Questions

Problem 84E: Salicylic acid, HOC6H4CO2H, and its derivatives have been used as pain relievers for a long time....

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Salicylic acid, HOC6H4CO2H, and its derivatives have been used as pain relievers for a long time. Salicylic acid occurs in small amounts in the leaves, bark, and roots of some vegetation (most notably historically in the bark of the willow tree). Extracts of these plants have been used as medications for centuries. The acid was first isolated in the laboratory in 1838. (a) Bath functional groups of salicylic acid ionize in water, with Ka=1.0103 for the—CO2H group and 4.201013 for the -OH group. What is the pH of a saturated solution of the acid (solubility = 1.8 g/L).. (b) Aspirin was discovered as a result of efforts to produce a derivative of salicylic acid that would not be irritating to the stomach lining. Aspirin is acetylsalicylic acid, CH3CO2C6H4CO2H. The -CO2H functional group is still present, but its acidity is reduced, Ka=3.0104. What is the pH of a solution of aspirin with the same concentration as a saturated solution of salicylic acid (See Part a). (c) Under some conditions, aspirin reacts with water and forms a solution of salicylic acid and acetic acid: CH3CO2C6H4CO2H(aq)+H2O(l)HOC6H4CO2H(aq)+CH3CO2H(aq) i. Which of the acids, salicylic acid or acetic acid, produces more hydronium ions in such a solution? ii. What are the concentrations of molecules and ions in a solution produced by the hydrolysis of 0.50 g of aspirin dissolved in enough water to give 75 mL of solution?
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