Calculate the number of moles of acetic acid in 100mL of both samples of vinegar accurately titrated.given:NaOH vs CH3COOHBurette solution is NaOH and the pipette solution is 5.0 mL of VinegarTitrationInitial burette readingFinal burette readingVolume of NaOH consumedAverage volume of NaOHApproximate 0.0 mL20.1 mL20.1 mL20.3 mLTitration 10.0 mL20.9 mL20.9 mLTitration 20.0 mL20.0 mL20.0 mLTo find the average volume Average volume = 20.1 mL + 20.9 mL + 20.0 mL320.1 mL + 20.9 mL + 20.0 mL3 = 20.3 mLConcentration of Vinegar = Volume of NaOH * Concentration of NaOHVolume of vinegarVolume of NaOH * Concentration of NaOHVolume of vinegar = 20.3 mL * 0.0647 M5.0 mL20.3 mL * 0.0647 M5.0 mL = 0.2627 MConcentration of NaOH = Volume of H2SO4 * Concentration of H2SO4Volume of NaOHVolume of H2SO4 * Concentration of H2SO4Volume of NaOH = 10.0 mL * 0.205 M31.7 mL10.0 mL * 0.205 M31.7 mL = 0.0647 MEstimation of NaOHNaOH vs H2SO4Burette solution is NaOH and the pipette solution is 10.0 mL of 0.205 M H2SO4TitrationInitial burette readingFinal burette readingVolume of NaOH consumedAverage volume of NaOHApproximate 0.0 mL31.8 mL31.8 mL31.7 mLTitration 10.0 mL31.5 mL31.5 mLTitration 20.0 mL31.7 mL31.7 mL Experimental Procedure:Part A. Preparation of the NAOH solutionWeigh approximately 2 g of sodium hydroxide pellets on a watch glass and transferthe solid to your large beaker.1.Add about 400 mL of deionized water and stir to dissolve the solid. This solution hasa concentration of approximately 0.1 M NAOH. Its molarity must be determinedexactly by titrating it with sulfuric acid according to equation (1) above.2.Part B. Titration of NaOH with sulfuric acid1. Rinse a clean buret with about 10 mL of the NaOH solution. Add the solution, brieflydrain a small volume to remove bubbles from the buret tip, then fill the buret with thesolution to about the 0 mL line. Record the actual volume.2.Collect about 40 mL of standard sulfuric acid solution in a small beaker. Record themolarity of the acid.3.Rinse a 10.00 mL pipet with a little of the sulfuric acid (2-3 mL) and discard the acid.4.Using the pipet, transfer 10.00 mL of sulfuric acid solution to a clean flask (the flaskdoes not have to be dry and can be wet with water, but do not rinse the flask withacid).5.Add 20 mL deionized water and 3 drops ofphenolphthalein indicator. Place the flaskon a sheet of white paper so the color change will be more clearly visible.6.Now add the sodium hydroxide solution from the buret until a faint pink colorpersists for at least 30 seconds. During the addition swirl the flask gently. During thistitration, the sodium hydroxide can be added fairly rapidly to give an approximateidea of how much solution is needed to neutralize the acid in the flask.7.Record the volume of sodium hydroxide used, but do not use it in your calculations.8.Refill the buret with sodium hydroxide.9.Rinse out the flask with water and again pipet 10.00 mL of the sulfuric acid solutioninto the flask, followed by about 20 mL of water and 3 drops.of indicator.0.Repeat the titration more carefully using the volume of sodium hydroxide solutionfrom step 7 to estimate the approximate volume required for the final titration. Ade20 - 2 of one drop of sodium hydroxide tofaint pink color.11.Record the volume of sodium hydroxide used, and use this volume to calculate themolarity.12.Feriorm a second, careful titration by repeating steps 8 - 11 with another 10 mLsample of the standard sulfuric acid solution.Part C. Analysis of vinegar1.Collect about 40 mL of the vinegar solution in a small beaker.Pipet 5.00 mL of the vinegar solution into a flask and add 20 mL of deionized water,3 drops of phenolphthalein and swirl to mix.2.3.Refill the buret with sodium hydroxide solution.Titrate with sodium hydroxide solution in the buret until the faint pink color persistsfor at least 30 seconds. As in the previous analysis, the first titration gives an estimateof the volume of sodium hydroxide required.4.Repeat the titration more carefully with two additional samples of vinegar, and usethese volumes of sodium hydroxide in the calculations below.5.

Your calculation for concentration of NaOH and acetic acid is not accurate. Below is the correct…

Calculate the number of moles of acetic acid in 100mL of both samples of vinegar accurately titrated. given: NaOH vs CH3COOH Burette solution is NaOH and the pipette solution is 5.0 mL of Vinegar Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 20.1 mL 20.1 mL 20.3 mL Titration 1 0.0 mL 20.9 mL 20.9 mL Titration 2 0.0 mL 20.0 mL 20.0 mL To find the average volume Average volume = 20.1 mL + 20.9 mL + 20.0 mL320.1 mL + 20.9 mL + 20.0 mL3 = 20.3 mL Concentration of Vinegar = Volume of NaOH * Concentration of NaOHVolume of vinegarVolume of NaOH * Concentration of NaOHVolume of vinegar = 20.3 mL * 0.0647 M5.0 mL20.3 mL * 0.0647 M5.0 mL = 0.2627 M Concentration of NaOH = Volume of H2SO4 * Concentration of H2SO4Volume of NaOHVolume of H2SO4 * Concentration of H2SO4Volume of NaOH = 10.0 mL * 0.205 M31.7 mL10.0 mL * 0.205 M31.7 mL = 0.0647 M Estimation of NaOH NaOH vs H2SO4 Burette solution is NaOH and the pipette solution is 10.0 mL of 0.205 M H2SO4 Titration Initial burette reading Final burette reading Volume of NaOH consumed Average volume of NaOH Approximate 0.0 mL 31.8 mL 31.8 mL 31.7 mL Titration 1 0.0 mL 31.5 mL 31.5 mL Titration 2 0.0 mL 31.7 mL 31.7 mL

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...