Buffer Solutions in Medical Chemistry

Buffer Solutions

• A buffer is a solution that can resist pH change upon the addition of an acidic or basic component, maintaining a relatively stable pH.
• Buffers neutralize small amounts of added acid or base, making them important for processes and/or reactions that require specific and stable pH ranges.
• In contrast, the pH of water and most solutions changes drastically with the addition of a small amount of acid or base.

Characteristics of Buffer Solutions

• Buffer solutions maintain pH by neutralizing small amounts of added acid or base.
• Buffers may contain a weak base and a salt containing its conjugate acid.
• Examples of buffers include those found in blood, which maintain a consistent pH of about 7.4.

Importance of pH Regulation in the Body

• The body obtains acids and bases from foods and cellular reactions, but buffers absorb these compounds effectively, keeping the blood pH essentially unchanged.
• Even slight changes in blood pH (above or below 7.4) can lead to drastic changes in oxygen levels and metabolic processes, which can be fatal.

Sample Problem: Identifying Buffer Solutions

• A buffer solution can be formed by combining a weak base and a salt containing its conjugate acid, such as KOH and KCl.

Acid-Base Imbalance

• Acidosis is a condition characterized by a decrease in CO2 levels, leading to a low blood pH.
• Alkalosis, on the other hand, is a condition characterized by an increase in CO2 levels, leading to a high blood pH.