Objectives
1. To determine the effect of adding small amounts of strong acids and bases to several buffer systems.
2. To determine how effectively each system resists large changes in pH.
3. To calculate the buffer capacity of each system.

Introduction
Buffers are extremely crucial solutions that resist changes in pH upon the addition of a strong acid or strong base. They are able to neutralize small amounts of the acid or base, resulting in a relatively stable pH range. The reason this is crucial is due to the fact that certain processes require specific pH ranges in order to carry out these processes efficiently. Buffers are composed of a weak conjugate acid-base pair, meaning either a weak acid and its conjugate base or a weak base and its conjugate acid. An example of this is a sodium acetate-acetic acid system, where acetic acid, CH3COOH, is the acid and its conjugate base would be the acetate ion, CH3COO-. When a strong acid is added to this buffer system, H3O+ are added to the solution. Those hydronium ions then react with the acetate ion (the conjugate base) and the solution is neutralized. Although buffers can withstand a fair amount of added strong acid/base, they eventually reach a point where the conjugate acid or conjugate base is used up by the stronger acid or base. This is referred to as the buffer capacity, which is the amount of strong acid and/or base that can be added to a buffer system without changing the pH ±1.0 units. Additionally, a buffer system’s pH can be predicted/determined using the Henderson-Hasselbalch (H-H) equation: pH = pKa + log
The H-H equation displays how the pH of a buffer depends on the ratio of the [anion] compared to that of the undissociated acid, as well as the acid’s pKa.

Procedure
For the experiment, 2 buffer solutions were prepared using the Weak Acid solution Potassium Hydrogen Pthalate, or in shorter terms, KHP (C6H4COOHCOOK). Additionally, boiled deionized water was used in th...