The purpose and objective of this experiment was to determine the percent by mass of acetic acid within a sample of vinegar using volumetric analysis with the titration technique. The theory is that if the volume and molar concentration of the standardized sodium hydroxide (NaOH) solution is known, then the percent by mass of the acetic acid (CH3COOH) in vinegar can be calculated after a titration.1 Within this experiment, a NaOH solution was standardized with a primary standard acid of potassium hydrogen phthalate (KHC8H4O4) in order to determine the molar concentration of the NaOH solution.1 The standardized NaOH solution was then used to determine the moles, mass, and percent by mass of CH3COOH in a sample of vinegar. The vinegar used in the experiment was labeled as “Harry Potter”. The reported molar concentration of the NaOH solution was 5.42E-02 mol/L
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The experiment used volumetric analysis, in which a known quantity of a substance reacts with an unknown amount of another substance for an aqueous solution reaction.2 To standardize the NaOH solution and determine the molar concentration, it needed to react with a primary standard acid due to NaOH being hygroscopic, in which it readily absorbs water vapor.1 In this case, KHC8H4O4 served as the primary acid standard since it’s only slightly hygroscopic and the mass was known, in which the moles could then be calculated from using the equation: mass (g) KHC8H4O4 mol KHC8H4O4204.23 g KHC8H4O4= mol KHC8H4O4
The reaction occurs with the dispensal of the NaOH titrant from the buret into a flask containing the KHC8H4O4, which functioned as the analyte. The balanced equation for this reaction was:
KHC8H4O4 (aq) + NaOH (aq) → H2O (l) + NaKC8H4O4 (aq).
This indicates that there is a one-to-one mole ratio, in which one mole of KHC8H4O4 reacts with one mole of
The experiment used volumetric analysis, in which a known quantity of a substance reacts with an unknown amount of another substance for an aqueous solution reaction.2 To standardize the NaOH solution and determine the molar concentration, it needed to react with a primary standard acid due to NaOH being hygroscopic, in which it readily absorbs water vapor.1 In this case, KHC8H4O4 served as the primary acid standard since it’s only slightly hygroscopic and the mass was known, in which the moles could then be calculated from using the equation: mass (g) KHC8H4O4 mol KHC8H4O4204.23 g KHC8H4O4= mol KHC8H4O4
The reaction occurs with the dispensal of the NaOH titrant from the buret into a flask containing the KHC8H4O4, which functioned as the analyte. The balanced equation for this reaction was:
KHC8H4O4 (aq) + NaOH (aq) → H2O (l) + NaKC8H4O4 (aq).
This indicates that there is a one-to-one mole ratio, in which one mole of KHC8H4O4 reacts with one mole of