Brønsted-Lowry Acid Base Theory

Beginning with the principles, Brønsted-Lowry acid base theory demonstrates that an acid donates a hydrogen ions, while a base accepts hydrogen ions. Strong acids have the an easier ability to donate hydrogen ions compared to weak acids.The goal for Experiment 8 Acid-Base Equilibria: Determination of Acid Ionization Constants is to recognize how different amounts of quantitative values can alter the pH in a solution. This procedure was carried out by mixinging specific acid or base solutions together and comparing the experimental value with the actual accepted value.

For Part 1, the weak acid, acetic acid, was titrated with the strong base of NaOH. After adding small amounts of NaOH portions at a time until reaching the pH value of 11.5, the points recorded lead to the determination of the half equivalence point of the pH and the pKa . The half equivalence point of the volume NaOH can be identified by dividing the highest

This is highly expected because the solution only contains DI water, with a neutral pH value of 7. The second unbuffered solution is the most acidic since it obtains the strong acid, HCl. Additionally, because it is a strong acid, it should dissociate completely. With a measured pH of 1.77, a calculated pH of 1.2, and a percent error of 32.2%, it undeniable that there were errors during the computations. The third unbuffered solution is the most basic as a result of containing the strong base, NaOH. With a measure pH of 11.93, calculated pH of 12.8, and a percent error of 7.29%, the results depict experimental errors. Unlike the unbuffered solutions, the buffered solutions are all accurate, with each solution containing a percent error less than 5.0%. This may be due to the fact that solving for buffer solutions is faster, requires less crunching of numbers, and therefore less opportunities for mistakes to