pH, Acids, Bases, and Buffers

Vocabulary-style flashcards covering pH levels, definitions of acids/bases, the bicarbonate buffer system, and the locations of major physiological buffers.

Normal pH Range

The standard physiological pH balance in the body, ranging from $7.35$ to $7.45$.

Acidemia

A condition where the pH is below $7.35$ due to too much acid.

Alkalemia

A condition where the pH is above $7.45$ due to too much base.

Acid

A substance that releases $H^{+}$, such as Carbonic acid ($H_2CO_3$).

Base

A substance that accepts $H^{+}$, such as Bicarbonate ($HCO_3^{-}$).

Bicarbonate Buffer System

The most important buffer system in the body, involving the equilibrium: $CO_2 + H_2O \rightleftharpoons H_2CO_3 \rightleftharpoons H^{+} + HCO_3^{-}$.

Buffers

Substances that prevent sudden pH changes; they act as shock absorbers.

Bicarbonate (Location)

A major buffer located in the blood.

Phosphate (Location)

A major buffer located in the cells and kidney.

Protein/Hemoglobin (Location)

A major buffer located in the blood.

Relationship between $CO_2$ and pH (Increase)

More $CO_2$ leads to more $H^{+}$, causing the pH to fall (Lower pH).

Relationship between $CO_2$ and pH (Decrease)

Less $CO_2$ leads to less $H^{+}$, causing the pH to rise (Higher pH).