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18 Nov 2019

A particular sample of vinegar has a pH of 3.00.

If acetic acid is the only acid that vinegar contains (Ka=1.8×10−5), calculate the initial concentration of acetic acid in the vinegar.

Express your answer using two significant figures.

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Irving Heathcote
Irving HeathcoteLv2
31 May 2019

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Related questions

Question #4

The manufacturer of vinegar used in this experiment claims that the vinegar contains 5% acetic acid by weight. Use your results, the molecular weight of HC2H3O2 and a density of 1.0 g/mL to determine if this claim is true or false.

Historically, vinegar played an important role in the preservation of food because of the acidity and antimicrobial properties of its main component, acetic acid. There are many types of vinegar found at your local grocery store, including balsamic, rice, red wine, and apple cider vinegars. A titration will help you determine the concentration of acetic acid (CH3COOH) in vinegar. The balanced equation for the titration of acetic acid in vinegar with sodium hydroxide (NaOH) is as follows.

CH3COOH(aq) + NaOH(aq) → H2O(l) + NaCH3COO(aq)

Assume you titrated a sample of vinegar using 0.145 M of sodium hydroxide. The results of this titration are shown in the following table.

Table 2: Titration Data for Vinegar
Volume of Vinegar Titrated (mL) 5.00
Initial Volume of NaOH (mL) 0.35
Final Volume of NaOH (mL) 29.50

(a) Use the data in the above table to determine the vinegar's acetic acid concentration in moles per liter.

0.845 mol/L

(b) Calculate the percent acetic acid in the titrated vinegar. Note that 1% = (1 g acetic acid/100 mL vinegar) × 100%.

_____ %

Please find and show work for part B


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