Buffers in Chemistry

Buffers

• Buffers are solutions that resist pH changes upon addition of small amounts of acid or base.
• Acid buffers are composed of weak acids and their conjugate bases (salts).
• Basic buffers consist of weak bases and their conjugate acids.
• The Henderson-Hasselbalch equation is used to calculate the pH of buffers.
• Buffer pH is influenced by the ratio of salt to acid/base.
• Buffer capacity is the strength of a buffer, reflecting its ability to resist pH change.
• Maximum buffer capacity is achieved when pH equals the pKa of the buffer.
• Factors influencing buffer capacity include the dissociation constant, hydrogen ion concentration, and molar concentration.
• Buffers are crucial in pharmaceutical formulations for maintaining drug stability and efficacy during testing.
• They are commonly employed in studies involving drug stability, diffusion, dissolution, and partitioning.
• The pH of human blood is tightly regulated by buffers like hemoglobin and bicarbonates, maintaining a range of 7.35-7.45.
• Bicarbonate serves as the primary buffer in blood, neutralizing excess acids.
• Phosphate buffers are the dominant buffers in intracellular fluids.
• The capacity of a buffer increases with a higher concentration of buffer components.
• Buffers help maintain the pH of eye fluids around 7.4, protecting against irritation.
• Buffer capacity is dependent on the ionic dissociation constant, hydrogen ion concentration, and molar concentration.
• Buffers assist in partitioning studies by ensuring a stable pH for accurate measurements of drug distribution between phases.
• Amphoteric molecules can act as both acids and bases, contributing to pH stability.
• Buffers are often used in topical drug formulations to prevent irritation on skin or mucous membranes.
• Ionic strength can affect buffer capacity; higher ionic strength generally increases capacity.
• Buffers protect the gastrointestinal tract by preventing drastic pH changes, safeguarding the lining.
• They stabilize proteins in solution by preventing pH-induced denaturation.
• Effective buffers are formed by weak acids and bases with their corresponding conjugates.
• Acetate buffers are most effective around pH 4.76, aligning with the pKa of acetic acid.
• Buffer capacity can be measured by adding a known amount of acid or base and evaluating the resulting pH change.
• The selection of a buffer for a specific application depends on the desired pH, compatibility with the system, and chemical stability of the buffer components.
• The maximum buffer capacity when pH equals pKa can be calculated as β = 0.575 × C, where C represents the total concentration of the buffer components.

Explore the essential role of buffers in chemistry with this quiz. Learn about the components of acid and basic buffers, the Henderson-Hasselbalch equation, and the factors influencing buffer capacity. Understand why buffers are crucial in pharmaceutical applications and maintaining pH stability.