How Much Acetic Acid Is In Vinegar Lab

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How Much Acetic Acid is in Vinegar? Titration is a simple technique in which one can determine the concentration of an unknown solution from a solution of known concentration. The known concentration is the titrant and the unknown is the analyte. The concentration of the analyte can be found from the concentration and volume of the titrant and the stoichiometry of the reaction. By using titration one can find how much acetic acid is in vinegar. Molarity is concentration of a substance in moles of solvent per liter of solution. By using stoichiometry, the ratio between certain chemicals in a solution can be used to determine the molarity of an unknown substance in a solution. The bottle of vinegar contains a label stating the vinegar contains

The experiment revolves around titration and proper calculations. The experiment began with the preparation of the burette. The preparation of the burette was done by rinsing the burette with water first and then a solution of NaOH was used to rinse the burette twice. Then the burette was filled completely with a solution of NaOH by using a funnel and the initial volume was recorded. This ensured the accuracy and precision of the experiment by removing the possibility of calculating base molarity incorrectly. About 1 gram of KHP was measured and put into a flask and then about 50 mL of distilled water and three drops of indicator were added. The flask was then placed under the burette and the titrant was added at steady speed. The indicator changed from clear to pink at the end of titration and

The mean molarity and standard deviation of NaOH was 0.3060 ± 0.0127. In trial 1 the mean molarity of NaOH 0.3060 is equal to the number of moles of NaOH over 0.0263 L of volume used. The number of moles of NaOH equals 8.063*10-3. Since the ratio of NaOH to acetic acid is 1:1, 8.063*10-3 is the number of moles of acetic acid. The 8.063*10-3 mol of acetic acid divided by the 0.01 L of vinegar gives the molarity of 0.8063. This was done for all 4 trials and then the mean molarity and standard deviation of acetic acid was calculated to be 0.8438 ± 0.0814. The 0.4842 grams of acetic acid is derived from the 8.063*10-3 moles. Then the percent of acetic acid in vinegar is calculated by dividing 0.4842 g of acetic acid by 10.214 g of vinegar and multiplied by 100% to get a 4.741% of acetic acid in vinegar. The mean molarity and standard deviation of acetic acid was 0.8438 ±