Vinegar Molarity
Determining the Molarity of Acetic Acid in Vinegar
Abstract
This experiment was done to determine the molarity of acetic acid in vinegar. The acetic acid in vinegar was titrated with a strong base sodium hydroxide to determine the equivalence point of this chemical reaction. The indicator phenolphthalein was used because the moment it changes color is on the basic side of the pH scale. To insure the experiment was done with the most accuracy, the two conductors of this experiment took three different trials to attempt to reach the best endpoint possible between the two. After punching in numbers and calculating results through a stoichiometry equation, the resultant molarity was .960M, but the actual molarity was .845M. We found that it took 9.60 mL of NaOH to …show more content…
If the wet burette was not rinsed with sodium hydroxide before filling, explain how the resultant molarity of acetic acid would be affected.
Water doesn’t affect the Molarity of the concentration of acetic acid because the 1:1 ratio of H+ and OH- ions does not acid the acidity or basicness of the reaction.
5. If a volume of water was added to the Erlenmeyer flask, explain how the resultant molarity of acetic acid would be affected.
See Number 4 for answer because response is almost identical
6. If methyl orange was used as the indicator, explain how the resultant molarity of acetic acid would be affected.
Phenolphthalein is more basic than methyl when comparing one another on the pH scale. If a different indicator such as methyl was used, a different amount of base would have been required to change the color of the solution, offsetting the molarity of the acetic acid with phenolphthalein.
7. Explain why the color of the endpoint fades upon standing.
The color of the endpoint fades upon standing because the solution will have all H+ and OH- ions neutralized eventually and change the pH to where the indicator is. NaOH eventually ionizes and the color will change
Abstract
This experiment was done to determine the molarity of acetic acid in vinegar. The acetic acid in vinegar was titrated with a strong base sodium hydroxide to determine the equivalence point of this chemical reaction. The indicator phenolphthalein was used because the moment it changes color is on the basic side of the pH scale. To insure the experiment was done with the most accuracy, the two conductors of this experiment took three different trials to attempt to reach the best endpoint possible between the two. After punching in numbers and calculating results through a stoichiometry equation, the resultant molarity was .960M, but the actual molarity was .845M. We found that it took 9.60 mL of NaOH to …show more content…
If the wet burette was not rinsed with sodium hydroxide before filling, explain how the resultant molarity of acetic acid would be affected.
Water doesn’t affect the Molarity of the concentration of acetic acid because the 1:1 ratio of H+ and OH- ions does not acid the acidity or basicness of the reaction.
5. If a volume of water was added to the Erlenmeyer flask, explain how the resultant molarity of acetic acid would be affected.
See Number 4 for answer because response is almost identical
6. If methyl orange was used as the indicator, explain how the resultant molarity of acetic acid would be affected.
Phenolphthalein is more basic than methyl when comparing one another on the pH scale. If a different indicator such as methyl was used, a different amount of base would have been required to change the color of the solution, offsetting the molarity of the acetic acid with phenolphthalein.
7. Explain why the color of the endpoint fades upon standing.
The color of the endpoint fades upon standing because the solution will have all H+ and OH- ions neutralized eventually and change the pH to where the indicator is. NaOH eventually ionizes and the color will change