You were asked to determine the acid content of vinegar and soda samples. You performed a simple acid-base titration using a solution of NaOH as the titrant with phenolphthalein as the indicator. To determine the concentration of the NaOH solution, you first performed standardization using KHP (FW: 204.22 g/mol, 99.94% purity). For analyzing the samples, he separately measured a volume of vinegar and soda then transferred them to a flask. Complete the table using the provided data. STANDARDIZATION OF NaOH SOLUTION TRIAL 1 TRIAL 3 0.09987 TRIAL 2 Weight of KHP, g Initial volume of NaOH, mL Final volume of NAOH, mL 0.1004 5.00 0.1012 0.00 10.01 4.95 9.99 14.93 Molarity of NaOH Average Molarity of NaOH ANALYSIS OF ACETIC ACID IN A VINEGAR SAMPLE TRIAL 1 1.500 14.98 24.84 TRIAL 2 TRIAL 3 Volume of vinegar, mL Initial volume of NaOH, mL Final volume of NaOH, mL 0.500 1.000 26.85 30.87 30.15 37.50 Molarity of acetic acid Average molarity of acetic acid ANALYSIS OF CARBONIC ACID IN A SODA SAMPLE TRIAL 1 TRIAL 2 TRIAL 3 Volume of soda, mL 20.00 18.00 20.00 Initial volume of NaOH, mL Final volume of NaOH, mL 20.20 24.69 28.50 29.48 24.48 33.87 Molarity of carbonic acid Average molarity of carbonic acid

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.