Untitled Quiz

Study Notes

Acids release protons (H+) in water, acting as proton donors.
Bases accept protons (H+) in water, or release hydroxide ions (OH-).
Strong acids dissociate completely in solution. Examples include HCl, H2SO4, HNO3.
Weak acids partially dissociate. Examples include formic acid (HCOOH), acetic acid (CH3COOH), oxalic acid (C2H2O4), benzoic acid (C6H5COOH), lactic acid, phosphoric acid, carbonic acid, and citric acid.
Strong bases completely dissociate into ions in solution. Examples include NaOH, KOH, Ba(OH)2.
Weak bases do not completely dissociate. Examples include amines, NH4+, aniline, and pyridine.
The tendency of an acid to lose a proton is its dissociation constant (Ka).
pKa is the negative logarithm of Ka and is a measure of acid strength; a smaller pKa signifies a stronger acid.
The body maintains a stable pH through buffering.
Buffers are mixtures of weak acids (proton donors) and their conjugate bases (proton acceptors).
Buffers resist changes in pH upon addition of acids or bases.
Important examples of buffers in the human body include bicarbonate-carbonic acid buffers, phosphate and proteins.
The kidneys help regulate pH by excreting hydrogen ions and generating bicarbonate.
The respiratory system regulates pH by adjusting breathing rate to control carbon dioxide levels.

Acid-base balance refers to the mechanisms the body uses to maintain a relatively constant pH in its fluids.
The normal pH for arterial blood is 7.35-7.45.
Imbalances in pH (acidosis or alkalosis) can disrupt cellular function.

Acidosis occurs when arterial blood pH drops below 7.35.
Alkalosis occurs when arterial blood pH rises above 7.45.
Acidosis and alkalosis can have various causes, including respiratory or metabolic origins.

Buffers maintain relatively constant pH by absorbing or releasing hydrogen ions.
Important buffers in blood include bicarbonate-carbonic acid buffers, phosphate, and proteins (e.g., hemoglobin).
The bicarbonate buffering system is critical for extracellular fluids.

The difference between measured cations and anions.
This is helpful for diagnosing acid-base imbalances.
Causes can involve increased unmeasured anions (e.g., ketoacidosis) or decreased unmeasured anions.
Usually a value of approximately 15 mEq/L.

Calculated using the formula (Na+ + K+) - (Cl- + HCO3-), where Na+ and K+ are cations and Cl- and HCO3- are anions.

Respiratory acidosis is caused by excess CO2 in the blood, while respiratory alkalosis is caused by insufficient CO2 in the blood.

Metabolic acidosis is caused by excessive acid in the blood, while metabolic alkalosis is caused by excessive base in the blood.

Bicarbonate buffer system: The primary buffer in extracellular fluids; involves equilibrium between CO₂, H₂O, H₂CO₃, H⁺, and HCO₃⁻.
Phosphate buffer system: The primary buffer in intracellular fluids; involves equilibrium between H₂PO₄⁻, HPO₄²⁻, and H⁺.
Protein buffer system: Includes hemoglobin in the blood and proteins within cells. These proteins contain amino acid residues with carboxyl and amino groups that can accept or donate H⁺, thus acting as buffers.

A patient in the hospital with a history of a cardiac event, lab results show abnormal pH, HCO3- and pCO2 indicating a metabolic and respiratory acidosis disturbance.