Calculations for the titration of vinegar with sodium hydroxide

	Trial 1	Trial 2	Trial 3
Volume of vinegar (mL)	5.00	5.00	5.00
Final volume NaOH (mL)	43.11	43.90	43.45
Initial volume NaOH (mL)	3.50	2.80	3.70
Volume NaOH used (mL)
Volume of NaOH used (L)
Moles of NaOH used (mol)
Moles of  COOH (mol)
Mass of  COOH (g)
% (m/v)  COOH in vinegar

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.

(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

for the titration of 20 mL of 0.1 M of hypochlorous acid with 0.1 M of sodium hydroxide , calculate pH after a total of 15 mL of base has been added