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Chapter_020.rtf

20-3

Audio Chapter Summaries

Copyright © 2025 by Elsevier Inc. All rights reserved, including those for text and data mining, AI training, and similar technologies.

Copyright © 2025 by Elsevier Inc. All rights reserved, including those for text and data mining, AI training, and similar technologies.

Patton: Structure & Function of the Body, 17th Edition

Chapter 20: Acid-Base Balance

Audio Chapter Summaries

Welcome to the audio review of Chapter 20: Acid-Base Balance.

As a reminder, you see hydrogen ions in your text indicated by “H+”, but they are referred to as hydrogen ions in this audio script. Similarly, you have seen “OH−” to indicate hydroxide ions, but this audio program refers to them as hydroxide ions.

First, we will review information about the pH of body fluids.

pH is a number that indicates the relative hydrogen ion concentration (as compared with hydroxide ion concentration) of a fluid.

A pH of 7.0 indicates neutrality or a neutral solution.

A pH higher than 7.0 indicates alkalinity or an alkaline or basic solution; a base.

A pH less than 7.0 indicates acidity or an acid solution.

Typical range of blood pH is approximately 7.35 to 7.45.

Systemic arterial blood pH is about 7.4.

Systemic venous blood pH is about 7.37.

The pH scale is based on multiples of 10.

The hydrogen ion concentration changes by 10 times for each one pH unit.

The difference between pH 7 and pH 6 is a 10- fold increase in hydrogen ions. Moving from pH 7 to pH 5 is a 100- fold increase in hydrogen ion concentration.

Thus, large pH fluctuations may appear small on the pH scale.

Two coordinated homeostatic mechanisms act to maintain the normal pH of body fluids and prevent pH swings when excess acids or bases are present: chemical pH control mechanisms and physiological pH control mechanisms.

A chemical pH control mechanism, based on buffers in blood, red blood cells, and body fluids, acts immediately.

Physiological pH control mechanisms come from the respiratory and renal systems.

Changes in pH regulated by changes in respiratory rate that result in changes in blood carbon dioxide act within minutes.

Changes in pH regulated by altered renal activity act within hours.

Now we’ll discuss each of these mechanisms in more detail.

Chemical buffers are substances that prevent a sharp change in the pH of a fluid when an acid or base is added to it.

Buffers usually include two different chemicals; they are called a buffer pair.

“Fixed” acids are buffered mainly by sodium bicarbonate.

Changes in blood that result from buffering of “fixed” acids in the tissue capillaries include:

The amount of carbonic acid in the blood increases slightly; carbonic acid is indicated in your text as H2CO3.

The amount of sodium bicarbonate in the blood decreases; the ratio of the amount of sodium bicarbonate to the amount of carbonic acid does not normally change; that normal ratio is 20:1.

The hydrogen ion concentration of blood increases slightly.

Blood pH decreases slightly below the arterial level.

T The physiological pH control mechanisms influence pH by eliminating substances from the body or retaining substances in the body. There are two types of physiological pH control mechanisms: respiratory mechanism and the urinary mechanism.

The respiratory mechanism relies on ventilation to control pH in the body.

The amount of carbonic acid in blood is decreased and thereby its hydrogen ion concentration is decreased; this in turn increases blood pH.

Respiratory control centers in the brainstem react to dropping pH and promote increased respirations; when the pH increases, then breathing slows.

The urinary mechanism of pH control depends on the functioning of the kidneys.

The kidneys are the body’s most effective regulator of blood pH.

Usually urine is acidified by way of the distal tubules secreting hydrogen ions into the urine from blood, in exchange for bicarbonate being retained in the blood; much of the excess hydrogen ions are secreted as ammonia and ammonium ions.

Acidosis and alkalosis are the two kinds of pH, or acid-base, imbalances. Disturbances in acid-base balance depend on the relative quantities of sodium bicarbonate and carbonic acid in the blood.

The body can regulate both of the components of the sodium bicarbonate-carbonic acid buffer system.

Blood levels of sodium bicarbonate are regulated by the kidneys.

Carbonic acid levels are regulated by the lungs.

Metabolic and respiratory disturbances can alter the normal 20:1 ratio of sodium bicarbonate to carbonic acid in blood.

Metabolic disturbances affect the sodium bicarbonate levels in blood.

Metabolic acidosis is a bicarbonate deficit.

Metabolic alkalosis, a complication of severe vomiting, is a bicarbonate excess.

Respiratory disturbances affect the carbonic acid levels in blood.

Respiratory acidosis is a carbonic acid excess.

Respiratory alkalosis is a carbonic acid deficit.

Compensated acidosis or alkalosis occurs when the body’s pH-balancing mechanisms temporarily counteract an atypical shift in pH.

Uncompensated acidosis or alkalosis occurs when the body’s mechanisms have not yet normalized the pH.

This concludes the audio review of Chapter 20.