- Lab Exercise 12 Cem131 Acid Base Titration Name Data Recording Concentration Of The Naoh Solution Data Collected Initi 1 (40.76 KiB) Viewed 54 times
- Lab Exercise 12 Cem131 Acid Base Titration Name Data Recording Concentration Of The Naoh Solution Data Collected Initi 2 (35.52 KiB) Viewed 54 times
- Lab Exercise 12 Cem131 Acid Base Titration Name Data Recording Concentration Of The Naoh Solution Data Collected Initi 3 (58.14 KiB) Viewed 54 times
Given that the Equilibrium constant (at room temperature) for acetic acid is 1.8x105 (remember equilibrium constants are unitless). Given the equation below, determine the equilibrium expression and using the concentration you determined for Acetic Acid in question #1, determine the concentration of Hydronium (H,0") at equilibrium. CH3COOH(aq) +H₂O(1) CH3CHOO (2)+H30(aq) Calculate a mass percentage of acetic acid in vinegar using the moles of acetic acid (not molarity) you calculated in question #1, the molar mass of acetic acid and assuming vinegar has a density of 1.00 g/ml Commercial vinegar is 5.00% and approximately pH 2.3. Using your determined values, calculate a percent error for your mass percentages and pH.
Procedure 1. As demonstrated by your instructor, rinse and fill your burette with NaOH solution. Record the concentration of the NaOH solution in your data table. 2. Measure 25 mL of a vinegar sample into a 125 mL Erlenmeyer flask. 3. Add 1 mL of the indicator (phenolphthalein) to the sample. 4. Slowly add NaOH solution from the burette to the flask while swirling the flask. Titrate until the solution color turns from colorless to a light pinkish. 5. Repeat the titration twice more. 6. Rinse the burette twice with distilled water and then fill with a third measure of distilled water before returning the burette, as demonstrated by your instructor.