Calculate the mass of acetic acid in 100ml of both samples in vinegar.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 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. 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

Given that, Volume of Vinegar taken for each titration V1 = 5.0 mL Concentration of acetic acid in…

Answered: Calculate the mass of acetic acid in…

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

Related questions

Concept explainers

Question

Calculate the mass of acetic acid in 100ml of both samples in vinegar.

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

of one drop of sodium hydroxide to
faint pink color.
11.
Record the volume of sodium hydroxide used, and use this volume to calculate the
molarity.
12.
Feriorm a second, careful titration by repeating steps 8 - 11 with another 10 mL
sample of the standard sulfuric acid solution.
Part C. Analysis of vinegar
1.
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 persists
for at least 30 seconds. As in the previous analysis, the first titration gives an estimate
of the volume of sodium hydroxide required.
4.
Repeat the titration more carefully with two additional samples of vinegar, and use
these volumes of sodium hydroxide in the calculations below.
5.

Experimental Procedure:
Part A. Preparation of the NAOH solution
Weigh approximately 2 g of sodium hydroxide pellets on a watch glass and transfer
the solid to your large beaker.
1.
Add about 400 mL of deionized water and stir to dissolve the solid. This solution has
a concentration of approximately 0.1 M NAOH. Its molarity must be determined
exactly by titrating it with sulfuric acid according to equation (1) above.
2.
Part B. Titration of NaOH with sulfuric acid
1. Rinse a clean buret with about 10 mL of the NaOH solution. Add the solution, briefly
drain a small volume to remove bubbles from the buret tip, then fill the buret with the
solution 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 the
molarity 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 flask
does not have to be dry and can be wet with water, but do not rinse the flask with
acid).
5.
Add 20 mL deionized water and 3 drops ofphenolphthalein indicator. Place the flask
on 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 color
persists for at least 30 seconds. During the addition swirl the flask gently. During this
titration, the sodium hydroxide can be added fairly rapidly to give an approximate
idea 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 solution
into 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 solution
from step 7 to estimate the approximate volume required for the final titration. Ade
20 - 2

Expert Solution

Trending now

This is a popular solution!

Step by step

Solved in 2 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.