Reference no: EM132732482
Trial 1:Molarity of NaOH (same for all 3 trials): 0.4936 MStarting buret reading: 0.5 mL
Mass of empty flask (same for all 3 trials): 134.347 g
Volume of vinegar (same for all 3 trials): 25.081 mL or g
Mass of flask + vinegar (same for all 3 trials): 159.428 g
Final buret reading: 43.75 mL
Trial 2:
Molarity of NaOH (same for all 3 trials): 0.4936 M
Starting buret reading: 0.4 mL
Mass of empty flask (same for all 3 trials): 134.347 g
Volume of vinegar (same for all 3 trials): 25.081 mL or g
Mass of flask + vinegar (same for all 3 trials): 159.428 g
Final buret reading: 43.6 mL
Trial 3:
Molarity of NaOH (same for all 3 trials): 0.4936 M
Starting buret reading: 0.8 mL
Mass of empty flask (same for all 3 trials): 134.347 g
Volume of vinegar (same for all 3 trials): 25.081 mL
Mass of flask + vinegar (same for all 3 trials): 159.428 g
Final buret reading: 43.7 mL
- Calculate the volume of NaOH added in each trial (final buret reading - starting buret reading.)
- Calculate the moles of NaOH used in each trial.
- The NaOH and the acetic acid in the vinegar react in a 1:1 mole ratio, therefore the moles of NaOH that reacted is equal to the moles of vinegar in each trial. Use the moles of vinegar that were neutralized to calculate the molarity of the vinegar for each trial. Average the three molarity values together to get the average molarity of vinegar.
- Vinegar contains acetic acid (C2H4O2.) Convert the moles of acetic acid for each trial into grams of acetic acid. Use this mass and the mass of the solution (recorded in the data table) to calculate the %(m/m) of the vinegar solution. Do for all 3 trials and then average the three %(m/m) together.
- Household vinegar is 5%(m/m) acetic acid. How close is the experimental %(m/m) to this value? Calculate the % error.