Percent Yield C7H6O3 salicylic acid + CHO acetic anhydride C9H8O4 + Aspirin CH3COOH acetic acid 10.00 kg of salicylic acid is mixed with 10.00 kg of acetic anhydride. What is the % yield for aspirin if 11.2 kg is produced?
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- Part 5Sodium carbonate is a reagent that may be used to standardizeacids in the same way. In such standardization it was found that a 0.432-g sample ofsodium carbonate required 22.3 mL of a sulfuric acid solution to reach the end point forthe reaction.Na2CO3(aq) + H2SO4(aq) -----> H2O(l) + CO2(g) + Na2SO4(aq)What is the molarity of the H2SO4?For the preparation of Aspirin calculate limiting factor, theoretical yield calculations, percent yield calculations for salicylic acid used 8.6g, Acetic anhydride used 3.9ml, Phosphoric acid used 0.25ml and Acetyl salicylic acid obtained 7.2g
- 11. 50.0 g of silver nitrite is mixed with 50.0 g of hydrochloric acid in a water based solution. A white precipitate forms. The solution is filtered and the white precipitate collected and dried. The dried precipitate is measured to have a mass of 36.1 g. What is the percent yield?What is the percent magnesium hydroxide, if a sample of magnesia magma weighing 5.2430g when dissolved in 25 mL of 0.9915 N H2SO4 required 9.85 mL of 1.4102 N NaOH to titrate the excess acid? Round to 2 decimal point; Answer should be with the correct unit.11.50.0 g of silver nitrate is mixed with 50.0 g of hydrochloric acid in a water based solution. A white precipitate forms. The solution is filtered and the white precipitate collected and dried. The dried precipitate is measured to have a mass of 36.1 g. What is the percent yield?
- The following equation describes the oxidation and ethanol to acetic acid by potassium permanganate 3C2H5OH+4KMnO4 —-> 3HC2H3O2 +4MnO2+4 KOH +H2O 5.00 g of ethanol and a excess of aqueous KMnO4 are reacted, and 5.24 g of HC2H3O2 result. What is the percentage yield? A. 100% B. 80.4% C. 26.8% D. 19.6%An unknown sample containing a mixture of NaCl and Na2CO3 was analyzed to determine the % composition of each compound. In the analysis for Na2CO3 (soda ash), the following data were obtained mass of unknown - 0.4436 g conc. of HCl used - 0.25 N initial volume - 0.5 mL final volume - 20.0 mL (MW soda ash) 106.12) 1.) What method was used to determine the concentration of HCl? 2.) What is the net volume of HCl used in the titration? 3.) What is % Na2CO3 in the given sample? NOTE: Round off your answer to a whole number (2 sig fig)CALCULATE FINAL CONCETRATION INCLUDE UNITS AND 2 SIG FIGS A 43.5 mL sample of an 7.5 %(mm/vv) KBr solution is diluted with water so that the final volume is 215.5 mL.
- A student carried out the synthesis of aspirin as described using 3.00 g of salicylic acid and 6.0 ml. of acetic anhydride and obtained 1.306 g of aspirin. (a) Calculate the amount of salicylic acid used in moles: (salicylic acid molar mass: 138.12 g/mol) (b) Calculate the mass (g) of acetic anhydride used: (acetic anhydride density: 1.08 g/cm³, Molar mass: 102.09 g/mol) (c) Calculate the amount of acetic anhydride used in moles: (d) Which one is the limiting reactant?When a Vitamin C (ascorbic acid; MM = 176.12 g mol-1) tablet is crushed, dissolved and titrated with 0.0377 M KIO3(aq) to a purple/blue endpoint (given by a starch indicator), the volume of KIO3 used is 40.01 mL. How many mg of Vitamin C were in the tablet? KIO3(aq) + 5 KI + 6 H+ → 3 I2(aq) + 3 H2O I2 (aq) + ascorbic acid → 2 I- + dehydroascorbic acidAcetaminophen, a popular drug taken as pain reliever and fever reducer, is produced together with acetic acid from the reaction of 3.05 g 4-aminophenol and 4.1 ml of acetic anhydride. Acetaminophen was extracted at 60% yield. Density of acetic anhydride at 20 C, 1.08 g/ml. Calculate the actual no. of grams of acetaminophen produced. [Determine L.R., E.R.]