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 10 ml of commercial vinegar solution was added to 100ml volumetric flask distilled water was added till the line mark. 5 ml of the dilute vinegar was titrated against standardized NaOH solution of molar concentration 0.25M. The end point was reached after the addition of 3.32 ml NaOH solution. The concentration of acetic acid in commercial vinegar solution is:

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Related questions

_____1. Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar 26.7 milliliters of 0.600-molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if no other acid was present?

(A) 1.60 M
(B) 0.800 M
(C) 0.600 M
(D) 0.450 M
(E) 0.200 M

_____2. HSO4- + H2O <===> H3O+ + SO42-

In the equilibrium represented above, the species that act as bases include which of the following?

I. HSO4-

II. H2O

III. SO42-

(A) II only
(B) III only
(C) I and II
(D) I and III
(E) II and III

_____3. Which of the following has the lowest pH?

(A) 0.1 M CuSO4
(B) 0.1 M KOH
(C) 0.1 M BaCl2
(D) 0.1 M HF
(E) 0.1 M HNO3

_____4. What volume of 0.150-molar HCl is required to neutralize 25.0 millilters of 0.120-molar Ba(OH)2?

(A) 20.0 mL
(B) 30 0 mL
(C) 40.0 mL
(D) 60.0 mL
(E) 80.0 mL

Please check my answers and let me know if they correct. Thanks

Exercise 1: Determining the Concentration of Acetic Acid

Data Table 1. NaOH Titration Volume.

Initial NaOH Volume (mL)

Final NaOH Volume (mL)

Total volume of NaOH used (mL)

Trial 1

9 ml

0

9

Trial 2

9 ml

0.2

8.8

Trial 3

9 ml

0.3

8.7

Average Volume of NaOH Used (mL) : 8.8

Data Table 2. Concentration of CH3COOH in Vinegar.

Average volume of NaOH used (mL)

Concentration CH3COOH in vinegar (mol/L)

% CH3COOH in vinegar

8.8

72 mol/L

83%

Questions

The manufacturer of the vinegar used in the experiment stated that the vinegar contained 5.0% acetic acid. What is the percent error between your result and the manufacturer’s statement?

The acetic acid in vinegar for my experiment is 83% which is 1560% difference from the actual 5%.

What challenges would you encounter with the titration if you had used apple cider vinegar or balsamic vinegar as the analyte instead of white vinegar?

The white vinegar is made up of pure vinegar so the results will be more accurate than the apple cider vinegar or balsamic vinegar, the later has other "impurities" in them. The apple and balsamic has other properties which will interfere with the titration.

How would your results have differed if the tip of the titrator was not filled with NaOH before the initial volume reading was recorded? Explain your answer.

If the tip of the titration had not been filled with NaOH, the results would have been inaccurate because the tip contains about 0.5ml-1ml of volume. Priming the tip is important to ensure accurate results.

How would your results have differed if you had over-titrated (added drops of NaOH to the analyte beyond the stoichiometric equivalence point)?

If I had over-titrated, the percent composition of acetic acid would be greater in my results since my results would have indicated that it took a larger volume of NaOH to neutralize the acetic acid in vinegar.

If a 7.0 mL sample of vinegar was titrated to the stoichiometric equivalence point with 7.5 mL of 1.5M NaOH, what is the mass percent of CH3COOH in the vinegar sample?

Not enough information! need the density of vinegar.

Why is it important to do multiple trials of a titration, instead of only one trial?

If only one trial is run, the results may not be entirely accurate and may contain mechanical or calculation errors. Running multiple trials helps ensure that no errors are made in the results and you have several results to compare to.

Titration of Acetic Acid in Vinegar :

A) Determine the concentration of acetic acid if it is between 5% (wt/wt) in Mole/L(M). Assume a density of 1.0056 g/mL for the vinegar.

B) Will the acetic acid solution of the vinegar be too concentrated to perform this titration with a NaOH solution of 0.1 M? If you don’t know by just looking at the numbers, this can be determined by pretending you are doing a titration and calculating the end point. Pick a volume of acetic acid (conc from #6) you would like to titrate. Then calculate the volume of NaOH you will need (the endpoint).

C) Based on your results, determine if you need to dilute the vinegar or not. If no, go to question 11. If yes, decide how much you will dilute the vinegar. Describe the glassware and procedure below. Remember that you want to do this in a quantitative fashion, so you need to pick the correct glassware.

D) Calculate the approximate concentration of the acetic acid of the diluted vinegar.

E) Again pick a volume of diluted vinegar you want to titrate (conc. of acetic acid was determined in #9). Calculate the expected end point (volume of NaOH needed).

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