Acid-Base Balance and Homeostasis

<p>Carbonic acid formation from metabolic processes (D)</p> Signup and view all the answers

<p>Changes in enzyme activity (C)</p> Signup and view all the answers

<p>Intracellular compartment (C)</p> Signup and view all the answers

<p>Increases potassium ion levels (A)</p> Signup and view all the answers

<p>Preserving nerve and muscle cell excitability (A)</p> Signup and view all the answers

<p>It can uncouple electron transport reactions. (A)</p> Signup and view all the answers

<p>It results in a tenfold increase in H+ concentration from 4 °C to 37 °C. (D)</p> Signup and view all the answers

<p>When the pH of the solution is equal to the pK of the buffer. (A)</p> Signup and view all the answers

<p>The concentrations of acid and base forms of the buffer are equal. (B)</p> Signup and view all the answers

<p>It is uncoupled due to membrane penetration by TRIS. (B)</p> Signup and view all the answers

<p>It facilitates TRIS's ability to penetrate membranes. (A)</p> Signup and view all the answers

<p>It indicates that higher pH always results in higher buffering capacity. (D)</p> Signup and view all the answers

<p>Both concentrations are equal or nearly equal. (D)</p> Signup and view all the answers

<p>It increases H+ ion concentration significantly. (B)</p> Signup and view all the answers

<p>Decreased respiration in cells. (C)</p> Signup and view all the answers

<p>Bicarbonate generation via buffered H+ excretion (C)</p> Signup and view all the answers

<p>It is a strong acid. (D)</p> Signup and view all the answers

<p>22–26 mEq/L (A)</p> Signup and view all the answers

<p>Low blood pH with low HCO3− (B)</p> Signup and view all the answers

<p>Weak acid and its conjugate base. (D)</p> Signup and view all the answers

<p>35–45 mm Hg (C)</p> Signup and view all the answers

<p>The pH at which an acid is 50% dissociated. (C)</p> Signup and view all the answers

<p>Effective when pH is within ±1 pH unit of pKa. (D)</p> Signup and view all the answers

<p>NH4+ excretion (D)</p> Signup and view all the answers

<p>Bicarbonate levels outside the range of 22–26 mEq/L (C)</p> Signup and view all the answers

<p>It determines the pH of buffered solutions. (D)</p> Signup and view all the answers

<p>α-intercalated cells (D)</p> Signup and view all the answers

<p>Low Ka and high pKa. (A)</p> Signup and view all the answers

<p>Henderson-Hasselbalch equation. (A)</p> Signup and view all the answers

<p>Lower pKa indicates a stronger acid. (A)</p> Signup and view all the answers

<p>The product of acid dissociation. (B)</p> Signup and view all the answers

<p>Buffers maintain pH stability despite added acids or bases. (A)</p> Signup and view all the answers

<p>It maintains a constant pH by altering concentrations of carbonic acid and sodium bicarbonate. (B)</p> Signup and view all the answers

<p>It allows protons to combine with the basic form of phosphate. (D)</p> Signup and view all the answers

<p>Hydroxide ions combine with protons released from carbonic acid. (C)</p> Signup and view all the answers

<p>Hydrogen phosphate (HPO4^2-) (D)</p> Signup and view all the answers

<p>Buffer systems with both weak acids and their conjugate bases. (D)</p> Signup and view all the answers

<p>Equilibrium of the buffer shifts to re-establish pH. (C)</p> Signup and view all the answers

<p>Provide a source of bicarbonate ions for buffering. (C)</p> Signup and view all the answers

<p>A balance of weak acids and their salts. (D)</p> Signup and view all the answers

<p>Throughout various biological systems, including intracellular fluid. (D)</p> Signup and view all the answers

Precise regulation of free hydrogen ion (H+) concentration in body fluids.

Water and solutes in three main body regions.

Maintaining stable internal environment through water intake/output, ion (Na+, K+, Ca2+) regulation, and pH (acid-base) regulation.

Critical for nerve & muscle function, enzyme activity, and potassium (K+) levels.

Body produces H+ from carbonic acid formation, inorganic acid breakdown of nutrients, and organic acids from metabolism.

A condition where the body's pH is too low.

A condition where the body's pH is too high.

Changes in pH (acidosis/alkalosis) affect K+ secretion in the body.

Ka, also known as the ionization constant or acid dissociation constant, measures how readily an acid releases hydrogen ions (H+) in solution.

pKa is the negative logarithm of the acid dissociation constant (Ka). It provides a more convenient way to express acid strength.

This equation calculates the pH of a buffered solution. It relates the pH of a solution to the pKa of the weak acid in the buffer and the ratio of the concentrations of the acid and its conjugate base.

A strong acid has a high Ka and a low pKa, meaning it readily releases hydrogen ions (H+) in solution.

A weak acid has a low Ka and a high pKa, meaning it only partially releases hydrogen ions (H+) in solution.

A mixture of a weak acid and its conjugate base, or a weak base and its conjugate acid. Buffers resist drastic changes in pH when small amounts of acid or base are added.

The form of an acid after it has donated a proton (H+). It is the species that remains after the acid has released the H+.

The ability of a buffer solution to resist changes in pH. The most effective buffering takes place within ±1 pH unit of the buffer's pKa.

The process by which a buffer solution maintains a relatively stable pH, resisting large changes when small amounts of acid or base are added.

Tris buffer can be harmful to biological systems because its high lipid solubility allows it to penetrate cell membranes, disrupting important processes like electron transport.

The concentration of hydrogen ions (H+) in Tris buffer changes significantly with temperature. A tenfold increase in H+ occurs from 4°C to 37°C.

When the pH of a solution matches the pK of the buffer, the concentrations of the acid and base forms of the buffer are equal. This is the optimal condition for buffering.

Tris buffer can penetrate cell membranes due to its high lipid solubility, disrupting vital processes like electron transport.

The concentration of hydrogen ions (H+) in Tris buffer changes significantly as temperature rises. A tenfold increase occurs from 4°C to 37°C.

The Henderson-Hasselbalch equation calculates the pH of a buffered solution, considering the acid dissociation constant (pK) and the concentrations of the acid and its conjugate base.

When the pH of a solution equals the pK of the buffer, the concentrations of the acid and base forms of the buffer are equal, resulting in optimal buffering capacity.

A buffer functions most effectively when the pH of the solution closely matches the pK of the buffer, as this ensures a balanced ratio of acid and base forms.

It helps regulate pH in the intracellular fluid (fluid inside cells). This system involves dihydrogen phosphate ions (H2PO4-) and monohydrogen phosphate ions (HPO4^2-), acting as a weak acid and its conjugate base.

When a strong acid is added, the HPO4^2- combines with H+ to form H2PO4-. Conversely, when a base is added, H2PO4- releases H+ to neutralize the base.

A mixture of carbonic acid (H2CO3) and its salt, sodium bicarbonate (NaHCO3) in the same solution. It helps regulate pH in the extracellular fluid (fluid outside cells).

When a strong acid is added, the bicarbonate ions (HCO3-) combine with H+ to form carbonic acid (H2CO3). This reduces the acidity.

When a strong base is added, carbonic acid (H2CO3) releases H+ to neutralize the base. This reduces the alkalinity.

The phosphate buffer system is primarily active in cells, while the bicarbonate buffer system is mainly responsible for maintaining pH in blood and other bodily fluids.

The body can become too acidic (acidosis) or too alkaline (alkalosis), leading to disruptions in cellular function and potentially life-threatening conditions.

The body has mechanisms to compensate for pH shifts, such as respiration (breathing) and kidney function.

Maintaining a stable pH is crucial for normal cell function, enzyme activity, and overall body homeostasis.

Locations where the majority of H+ ions are excreted to maintain acid-base balance.

Specialized cells in the late distal tubule and collecting duct that play a major role in H+ excretion and bicarbonate (HCO3-) reabsorption, contributing to acid-base balance.

The process of creating fresh bicarbonate ions (HCO3-) primarily in α-intercalated cells of the late distal tubule and collecting duct, aiding in acid-base balance.

The way the body eliminates ammonia (NH4+), which helps in acid-base balance by contributing to H+ removal.

A condition where the body's pH is too low due to a buildup of acids or a loss of bicarbonate (HCO3-), resulting in an acid-base imbalance.

The typical range for PCO2 (partial pressure of carbon dioxide), a measure of CO2 in the blood, is between 35 and 45 mm Hg.

The healthy range for blood bicarbonate levels (HCO3-) is 22–26 mEq/L. Levels outside this range indicate a metabolic acid-base imbalance.