1. Judith Anthony,” Strong Acid/Strong Base Titrations”, CHEM 1130, T. A-Joseph Kreft, Tuesday 8am,Room 1871,Donna Ellitnorpe. 2. Purpose of this experiment: The purpose of this experiment is to observe the neutralization reaction that occurs between strong acid and strong base solutions. The technique of titration is used to observe the acid content of the fluid in a car battery.
3. Procedure: Calculate the volume of 6. 00 M NaoH that is needed to prepare 250mL of an approximately 0. 100 M NaOH solution. Transfer the calculated volume of the 6. 0 M NaOH solution to a volumetric flask using a graduated cylinder. Obtain a 25mL buret, and rinse and fill it with the prepared base solution. Make sure there are no air bubbles trap within the buret. Calculate the amount of KHP required to reach equivalence point. Using a 125mL Erlenmeyer flask, place it on a balance, and add KHP to it until the balance reads the calculated the same amount as the KHP calculated in the preceding step. It should be within ±10. 0% of the calculated mass. Add 25. 00mL of distilled water to the Erlenmeyer flask, containing the KHP.
Swirl it until all the KHP has been dissolved. Add 4 drops of bromothymol blue indicator, and the solution should obtain a pale yellow color. Titration the solution with NaOH until the solution changes from the pale yellow color to a blue color. Record the intial ad final read of the buret. Repeat this titration method twice. The volume of the base should be ±0. 40mL of each other. Find out the amount of diluted battery acid needed to use for titration with the base. Pour enough of the solution in a breaker to be titrated once.
Pipette the exact amount of the diluted battery into a 125mL Erlenmeyer flask. Then add enough distilled till the total volume is 40mL, and add four drops of the indicator. Titrate with NaOH until the solution changes from the pale yellow color to a blue one. 4. Observations, Results, and Data Sheets: Table 1: Data of calculated volume of NaOH for the standardization of NaOH Table 1 | Mass of KHP(g) | Volume of NaOH (mL) | Concentration of NaOH (M) | Trial 1 | 0. 501| 25. 8| | Trial 2 | 0. 500| 25. 0| | Trial 3| 0. 520| 26. 40| |