Acid Base- Balance

Blood pH

The measure of acidity or alkalinity of blood, important for cellular function.

Normal blood pH range

7.35 to 7.45; higher or lower values indicate potential health issues.

Acidosis

Conditions where blood pH is less than 7.35.

Acidic

A solution with a low pH, indicating a high concentration of hydrogen ions.

Buffer system

A mechanism that stabilizes pH levels by soaking up or releasing hydrogen ions as needed.

Bicarbonate (HCO3) system

The most important buffer system in blood that uses bicarbonate to maintain pH.

Isohydric buffer system

A buffering system involving hemoglobin which can bind to hydrogen ions in red blood cells.

Respiratory acidosis

A condition resulting from carbon dioxide build-up, leading to decreased blood pH.

Respiratory alkalosis

A condition caused by excessive exhalation of carbon dioxide, leading to increased blood pH.

Fixed acids

Acids produced by normal metabolism that cannot be removed by the lungs and must be handled by the kidneys.

Metabolic acidosis

A condition where the kidneys cannot remove acids fast enough, leading to low blood pH.

Volatile acids

Acids that can be converted to gas and expelled through the lungs.

Henderson-Hasselbalch equation

A formula showing the relationship between blood pH, bicarbonate, and carbon dioxide levels.

pH shock absorber

A function of buffers that stabilize pH by neutralizing excess acids or bases.

Normal ratio of HCO3 to CO2

Approximately 20:1 for a normal blood pH of 7.4.

Role of the kidneys in pH balance

Control the excretion of hydrogen ions and conservation of bicarbonate.

Role of the lungs in pH balance

Quickly adjust pH by increasing or decreasing CO2 exhalation.

Clinical relevance of ABG interpretation

Helps identify acid-base disorders by analyzing levels of PaCO₂ and HCO₃⁻.

Acidotic

Describes a patient moving towards acidity, often seen in hypoventilating patients.

Carbonic acid formation

Occurs when CO2 combines with water in red blood cells, contributing to blood acidity.

Buffers in blood

Substances, like bicarbonate and proteins, that help to maintain stable pH levels.

Phosphate buffer system

An intracellular buffer that helps manage pH by binding or releasing hydrogen ions.

Role of hemoglobin in buffering

Hemoglobin can bind to hydrogen ions when blood becomes acidic, stabilizing pH.

Compensation mechanisms for pH imbalance

The lungs and kidneys work together to correct pH imbalances.

Clinical indication of low pH and high CO₂

Suggestive of respiratory acidosis in gas exchange issues.

Acids produced by metabolism

Includes lactic acid and ketone acid, typically managed by the kidneys.

Importance of maintaining pH balance

Essential for proper cellular functions and overall metabolic processes.

Hypoventilation effects

Leads to increased CO2 levels, resulting in respiratory acidosis.

Alkalosis

A condition where blood pH is elevated, often due to excessive CO2 exhalation.

Acid-base balance

The equilibrium between acids and bases in the body to maintain normal pH.

Dangers of unregulated pH

Without buffers, fluctuations in pH due to breath or diet can lead to health crises.

Respiratory control of pH

Primarily through CO2 management via breathing patterns.