2nd half of Lecture 3 - pH Balance and Buffers in the Body

Front

Role of buffers in body fluids.

Back

Buffers maintain normal pH range and homeostasis.

Front

H₂CO₃

Back

Carbonic acid

Front

Role of H₂CO₃

Back

Acts as a weak acid (dissociates to produce H⁺)

Front

Function of bicarbonate ion in the buffer system

Back

Mops up excess H⁺ ions

Front

Equilibrium in the buffer system

Back

Maintained by the reversible reactions of H₂CO₃

Front

Chemical equation for buffer reaction

Back

H₂O + CO₂ ⇌ H₂CO₃ ⇌ H⁺ + HCO₃⁻

Front

Effect of increased H⁺ on reaction

Back

The reaction shifts to the left to reduce acidity.

Front

H₂CO₃ in the buffer system

Back

H₂CO₃ (carbonic acid) acts as an intermediate in the buffer system.

Front

H₂O + CO₂ ↔ H₂CO₃ ↔ H⁺ + HCO₃⁻

Back

This equation represents the carbonic acid-bicarbonate buffer system.

Front

Water and carbon dioxide form carbonic acid.

Back

This reaction is vital for maintaining pH in the blood.