Question

# please find the following and show work so i have a better understanding: - volume of...

please find the following and show work so i have a better understanding:

- volume of NaOH used

- moles of NaOH used

- moles of HC2H3O2

- mass of HC2H3O2

- mass percent of vinegar solution

- molarity of HC2H3O2

- deviation

- percent error

- average mass percent of vinegar

- average molarity of vinegar

Table 2: Titration of standard NaOH with a HC2H3O2 Solution

 Trail 1 Trial 2 Trial 3 M of NaOH 0.4936 M 0.4936 M 0.4936 M Volume of Vinegar Solution 25.00 mL 25.00 mL 25.00 mL Mass of Erlenmeyer flask: 139.347 g 139.347 g 139.347 g Mass of Erlenmeyer flask plus vinegar solution: 159.428 g 159.428 g 159.428 g Mass of Vinegar solution 20.08 g 20.08 g 20.08 g Initial Burette Reading: 50.00 mL 50.00 mL 50.00 mL Final Burette Reading: 44.25 mL 44.40 mL 44.30 mL Volume of NaOH used: Moles of NaOH added: Moles of HC2H3O2 Mass of HC2H3O2 Mass percent of Vinegar solution Molarity of HC2H3O2 Deviation Percent error

- how did the mass percent you found compare to the manufacturer claim. What can we conclude about the manufacturers claim? Explain by supporting with experimental evidence.

The volume of NaOH used is calculated:

V NaOH = Vf - Vi = 50 - 44.25 = 5.75 mL

Trial 2: 5.60 mL

Trial 3: 5.70 mL

The moles of NaOH are calculated:

n NaOH = M * V = 0.4936 M * 0.00575 L = 2.84e-3 mol

Trial 2: 2.76e-3 mol

Trial 3: 2.81e-3 mol

The moles of acetic acid and those of NaOH are the same.

The mass of acetic acid is calculated:

m AA = n * MM = 2.84e-3 * 60.05 = 0.0171 g

Trial 2: 0.0166 g

Trial 3: 0.0169 g

The percentage is calculated:

% AA = g AA * 100 / g solution = 0.0171 g * 100 / 20.08 g = 0.085%

Trial 2: 0.083%

Trial 3: 0.084%

Average = 0.084%

The molarity is calculated:

M = n / V = ​​2.84e-3 mol / 0.025 L = 0.1136 M

Trial 2: 0.1104 M

Trial 3: 0.1124 M

Average = 0.1121 M

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