Measurements for the titration of acetic acid with NaOHEnter your measurements from lab for trails 1 - 3 with the correct number of decimal places  Trial 1Trial 2Trial 3Mass of empty flask (grams)71.39171.42572.095Mass of flask + vinegar (grams)81.00381.37982.014Volume of vinegar (L)0.010000.010000.01000Concentration of NaOH (mol/L)0.20000.20.2Initial volume of NaOH (mL)0.600.290.20Final volume of NaOH (mL)41.6541.9441.53AttendanceThis QR code needs to be scanned by your TA to confirm that you have completed data collection and cleaned up your workspace.Done online(51pts) CalculationsTitration of Acetic Acid with NaOHCalculations for the titration of acetic acid with NaOHTable view List viewComplete the calculations below for trials 1 - 3 with the correct number of decimal places  Trial 1Trial 2Trial 3Mass of empty flask (grams)71.39171.42572.095Mass of flask + vinegar (grams)81.00381.37982.014Mass of vinegar (grams)Volume of vinegar (L)0.010000.010000.01000Concentration of NaOH (mol/L)0.20000.20000.2000Initial volume of NaOH (mL)0.600.290.20Final volume of NaOH (mL)41.6541.9441.53Volume of NaOH added (mL)Volume of NaOH added (L)Moles of NaOH used (mol)Moles of acetic acid (mol)Mass of acetic acid (grams)Mass percent of acetic acid(9pts)Average mass percent(9pts)Standard Deviation

In this experiment, you will take a 25.00 mL aliquot of vinegar and dilute it to 250.0 mL.  You will then take a 25.00 mL aliquot from this diluted vinegar solution and titrate it against the standardised sodium hydroxide. The titration between acetic acid and sodium hydroxide is a 1:1 stoichiometry.    If your standardised sodium hydroxide solution was determined to be 0.051 M, and it required an average titre (titration volume) of 25.3 mL, what is the concentration (in M) of the undiluted vinegar sample (the initial vinegar sample)?  Provide your answer to 2 significant figures.

Complete the calculations below for trials 1 - 3 with the correct number of decimal places  Trial 1Trial 2Trial 3Mass of empty flask (grams)71.39171.42572.095Mass of flask + vinegar (grams)81.00381.37982.014Mass of vinegar (grams)Volume of vinegar (L)0.010000.010000.01000Concentration of NaOH (mol/L)0.20000.20000.2000Initial volume of NaOH (mL)0.600.290.20Final volume of NaOH (mL)41.6541.9441.53Volume of NaOH added (mL)Volume of NaOH added (L)

Mass of empty flask (grams)71.39171.42572.095Mass of flask + vinegar (grams)81.00381.37982.014Mass of vinegar (grams)Volume of vinegar (L)0.010000.010000.01000Concentration of NaOH (mol/L)0.20000.20000.2000Initial volume of NaOH (mL)0.600.290.20Final volume of NaOH (mL)41.6541.9441.53Volume of NaOH added (mL)Volume of NaOH added (L)Moles of NaOH used (mol)Moles of acetic acid (mol)Mass of acetic acid (grams)Mass percent of acetic acid

You complete your titrations and find that the concentration of acetic acid in the diluted vinegar solution is 0.023 M. If your dilution step involved taking 25.00 mL of the orginal vinegar solution and diluting this to 250.00 mL with water to create your diluted solution for titration, calculate the concentration of your original vinegar solution.Question 4Answera.0.57b.2.30c.0.00023d.0.23e.0.0023

The concentration of acetic acid in white vinegar is defined in the US at 5% mass by volume. How accurate were your measurements? Was there anything that could have been done to improve accuracy in your measurements?