Answer ALL parts of this question.An aspirin tablet dissolved in sodium hydroxide solution gave sodium salicylate. Thesodium salicylate gives a yellow colour and absorbs at 295 nm, which gave anestimated concentration of sodium salicylate of 0.00015 mol dm-³.CO₂HNaOH (aq)CO₂NaOHsodium salicylateAspirin(a) Explain the formation of sodium salicylate using a curly arrow mechanism.(b) The solution of sodium salicylate was diluted to 50 cm³. How many moles arein the 50 cm³?(c) There were initially 250 cm³ of the original aspirin solution, so the total numberof moles of sodium salicylate in the original solution is 250 times thatcalculated in part (b). Calculate the mass of aspirin in the tablet.(MW of aspirin = 180 gmol-¹).

We know aspirin is a very famous drug used to reduce fever and to relieve mild to moderate pain from…

Answer ALL parts of this question. An aspirin tablet dissolved in sodium hydroxide solution gave sodium salicylate. The sodium salicylate gives a yellow colour and absorbs at 295 nm, which gave an estimated concentration of sodium salicylate of 0.00015 mol dm³. CO₂Na CO₂H NaOH (aq) Co Aspirin OH sodium salicylate

Answer ALL parts of this question. An aspirin tablet dissolved in sodium hydroxide solution gave sodium salicylate. The sodium salicylate gives a yellow colour and absorbs at 295 nm, which gave an estimated concentration of sodium salicylate of 0.00015 mol dm³. CO₂Na CO₂H NaOH (aq) Co Aspirin OH sodium salicylate

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Calculate the concentration of HC6H₂O6 in an aqueous solution of 0.0337 M ascorbic acid, H₂C₁H₂O6 (aq). [HC6H6O6 ] = M.
A fertilizer railroad car carrying 34,300 gallons of commercialaqueous ammonia (30% ammonia by mass)tips over and spills. The density of the aqueous ammoniasolution is 0.88 g>cm3. What mass of citric acid,C(OH)(COOH)(CH2COOH)2, (which contains three acidicprotons) is required to neutralize the spill? 1 gallon = 3.785 L.
A student titrates 10.0 mL of the 2.000 M HC2H3O2(aq) with an NaOH(aq) solution of unknown concentration. The student monitors the pH during the titration. The following titration curve was created using the experimental data. Write the balanced net ionic equation for the reaction that occurs when HC2H3O2(aq) and NaOH(aq) are combined. 2.Calculate the molar concentration of the NaOH(aq) solution. 3.Explain how the student can estimate the value of Ka for HC2H3O2(aq) using the titration curve.
The pH of an aqueous solution of 0.293 M sodium acetate, NaCH3COO (aq), is
Sodium hydrogen carbonate NaHCO3, also known as sodium bicarbonate or "baking soda", can be used to relieve acid indigestion. Acid indigestion is the burning sensation you get in your stomach when it contains too much hydrochloric acid HCl, which the stomach secretes to help digest food. Drinking a glass of water containing dissolved NaHCO3 neutralizes excess HCl through this reaction: HCl(aq)+NaHCO3(aq)→NaCl(aq)+H2O(l)+CO2(g) The CO2 gas produced is what makes you burp after drinking the solution. Suppose the fluid in the stomach of a woman suffering from indigestion can be considered to be 200.mL of a 0.089M HCl solution. What mass of NaHCO3 would she need to ingest to neutralize this much HCl? Be sure your answer has the correct number of significant digits.
A student dissolved 0.3101 g of Na2C2O4 in 30 mL of water and 15 mL of 3 mol/L H2SO4. She titrated this solution with a KMnO4 solution. What was the molarity of the KMnO4 if it took 24.90 mL of titrant to reach a permanent pale pink equivalence point? The net redox reaction is 2 KMnO4 (aq) + 5 Na2C2O4 (aq) + 8 H2SO4 (aq) → 8 H2O (l) + 10 CO2 (g) + K2SO4 (aq) + 2 MnSO4 (aq) + 5 Na2SO4 (aq) (2 digit response) Answer: 0.037
Sodium nitrate contains 0.3% iodine in the form of calcium iodate, Ca(IO3)2. After the sodium nitrate in the niter is dissolved and recrystallized, the remaining solution contains 9 g/Lsodium iodate, NaIO3(aq). The NaIO3 is converted to iodine when it reactswith sulfur dioxide and water.2NaIO3 + 5SO2 + 4H2O → Na2SO4 + 4H2SO4 + I2a. How many liters of sodium iodate solution that contains 9 g of NaIO3 perliter would be necessary to form 127.23 kg of iodine, I2?
The pH of an aqueous solution of 0.0103 M hydrosulfuric acid, H2S (aq), is
Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. HNO2 (aq) + OH" (aq)NO, (aq) + H2O (1) K =
Write the equilibrium constant expression, K, for the following reaction taking place in dilute aqueous solution. NH3 (aq) + H2O(1) =NH,* (aq) + OH(aq) K=-
20.00mL of 6M HCl is taken from 500mL bottle containing the acid and is transferred to 250mL volumetric flask and diluted to volume with water. What is the molarity of the new solution? Do not enter units with your answer.
The traditional way of comparing reactions is by the percentage yields. However, percentage yield takes no account of by-products. In order to decide which chemical process is greener, chemists have tried to develop ways of measuring 'greenness'. One of the most common methods is the atom economy. Calculate the atom economy of the following reactions: (i). CH2 PhP-CH2 + Ph;P=0 (ii). OH 200 °C CI (in). CI- .CI NaOH (iv). он 0.5 O2. Me catalyst Ph + H20 Me Ph (Ph = phenyl (-C,Hs); and Me = methyl (-CH)) (v). NO2 Ni (cat.) NH2 3H, 2 H,0 300 °C. 5 psi