For the Precise Run, a 25.00-mL aliquot of the diluted vinegar solution was pipetted into a clean 250-mL beaker. Using a 50.0-mL graduated cylinder, 25.0 mL of deionized water was added to the beaker. A pH electrode was lowered into the vinegar solution and the pH was recorded once it had stabilized. The temperature of the solution was 19.0 °C. A 25.00-mL burette was filled with 0.1044 M NaOH. In 1.00-mL increments, NaOH was added to thevinegar solution until the estimated equivalence point of 8.5 mL was reached and the pH wasrecorded after every milliliter. NaOH was then added 0.10 mL a time, and the pH was recorded for each drop. Once the equivalence point was clearly reached, NaOH was added in 1.00-mL increments until the equivalence point was 4.00 mL away. The data collected from this titration can be found in Appendix B. Equation 1 shows the reaction for the titration of acetic acid and sodium hydroxide to produce water and sodium acetate.1
CH3COO H(aq)+ NaOH(aq)→ C H3COON a(aq)+ H2O(l)(1)Part 2. Titration of Phosphoric AcidAn Unknown sample of aqueous phosphoric acid in a 100.00-mL volumetric flask was diluted to the 100.00-mL mark with deionized water and mixed well. ___(chem eq) (2)For the Trial Run, a 25.00 mL aliquot was pipetted into a clean 250-mL beaker and 25.00mL of deionized water was added to the beaker. A 25.00-mL burette was filled with
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Molarity,pH,Pennsylvania State University,Pennsylvania,Penn State Altoona,Altoona, Pennsylvania,Experimental Chemistry II Laboratory