Acid and Base Concepts Unit 2
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Questions and Answers

Which of the following conditions is associated with respiratory acidosis?

  • Febrile conditions
  • Hyperventilation
  • Milk alkali syndrome
  • Narcotics, Sedatives (correct)

What is the normal range for the anion gap?

  • 10 ± 2 mEq/L
  • 15 ± 5 mEq/L
  • 12 ± 4 mEq/L (correct)
  • 20 ± 3 mEq/L

Which of the following causes a high anion gap acidosis?

  • Lactic acidosis (correct)
  • Renal tubular acidosis
  • Cushing Syndrome
  • Diarrhea

Which conditions are categorized under metabolic alkalosis?

<p>Severe vomiting (D)</p> Signup and view all the answers

What characterizes a strong acid?

<p>Completely dissociates into its ions in aqueous solution. (A)</p> Signup and view all the answers

What does the anion gap calculation help to diagnose?

<p>Acid-base imbalances (A)</p> Signup and view all the answers

Which option represents a cause of metabolic acidosis with a normal anion gap?

<p>Diarrhea (B)</p> Signup and view all the answers

Which of the following represents a weak acid?

<p>Acetic acid (CH3COOH) (B)</p> Signup and view all the answers

Which of these statements accurately describes a weak base?

<p>Partially dissociates into its ions in solution. (D)</p> Signup and view all the answers

Which factors are included in calculating the anion gap?

<p>Na+, K+, Cl-, HCO3- (B)</p> Signup and view all the answers

Which of the following is NOT considered a strong base?

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

In metabolic acidosis, what is typically observed regarding pH levels?

<p>pH levels are decreased (D)</p> Signup and view all the answers

What is a primary method by which acids are produced in the human body?

<p>Oxidation of carbon compounds. (A)</p> Signup and view all the answers

Which of the following is an example of an inorganic weak acid?

<p>Formic acid (HCOOH) (D)</p> Signup and view all the answers

Which of these correctly describes the role of hydroxyl ions in bases?

<p>They are released when bases dissociate in water. (D)</p> Signup and view all the answers

The Henderson-Hasselbalch equation is significant for understanding:

<p>The acid-base equilibrium in solutions. (B)</p> Signup and view all the answers

Which of the following is considered an alkaline substance in the human body?

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

What does a lower pKa value indicate about an acid?

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

What does pH measure in a solution?

<p>The concentration of hydrogen ions. (A)</p> Signup and view all the answers

Which of the following statements regarding pKb is true?

<p>A higher pKb means a stronger base. (D)</p> Signup and view all the answers

Which pH range indicates an acidic solution?

<p>0 - 7 (C)</p> Signup and view all the answers

What is the dissociation constant (Ka) related to?

<p>The tendency of an acid to lose a proton. (D)</p> Signup and view all the answers

What does a pH of 7 indicate about a solution?

<p>It is neutral. (A)</p> Signup and view all the answers

Which of the following organic acids is not considered an alkaline substance?

<p>Lactate (B), Acetoactate (C)</p> Signup and view all the answers

What typically causes an increase in the anion gap?

<p>Renal failure (C)</p> Signup and view all the answers

Which condition is associated with a high anion gap acidosis?

<p>Diabetic metabolic ketoacidosis (D)</p> Signup and view all the answers

In metabolic acidosis, which bicarbonate level indicates an underlying problem?

<p>&lt;22 mEq/L (A)</p> Signup and view all the answers

What should be done first in diagnosis of acid-base imbalances?

<p>Check the pH (A)</p> Signup and view all the answers

Which of the following values indicates a respiratory problem in acid-base balance?

<p>Change in pCO2/H2CO3 (A)</p> Signup and view all the answers

What signifies a normal serum bicarbonate level?

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

What clinical scenario might increase the likelihood of lactic acidosis?

<p>Myocardial infarction (D)</p> Signup and view all the answers

What does a low anion gap primarily suggest?

<p>Multiple myeloma (B)</p> Signup and view all the answers

What is the normal pH range of human blood?

<p>7.35 - 7.45 (B)</p> Signup and view all the answers

Which parameter indicates a metabolic acid-base disturbance?

<p>HCO3- of 19 mEq/L (D)</p> Signup and view all the answers

What is the primary buffer system in the human body?

<p>Bicarbonate buffer system (D)</p> Signup and view all the answers

In the Henderson-Hasselbalch equation, what represents the weak acid?

<p>H2CO3 (A)</p> Signup and view all the answers

A patient has a pH of 7.30 and a pCO2 of 50 mmHg. What type of acid-base disturbance is likely present?

<p>Respiratory acidosis (D)</p> Signup and view all the answers

What is the most effective condition for a buffer to work according to the Henderson-Hasselbalch equation?

<p>pH = pKA (C)</p> Signup and view all the answers

Which acid is chiefly produced during strenuous exercise due to lactic acid accumulation?

<p>Lactic acidosis (C)</p> Signup and view all the answers

What is the primary organ responsible for regulating bicarbonate levels in the blood?

<p>Kidneys (B)</p> Signup and view all the answers

What would you expect the bicarbonate (HCO3-) levels to be in respiratory alkalosis?

<p>Increased (A)</p> Signup and view all the answers

Which of the following statements is true regarding respiratory acidosis?

<p>It can result from conditions like COPD. (C)</p> Signup and view all the answers

What happens to pH in metabolic alkalosis?

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

Which of the following substances is responsible for the regulation of intracellular pH?

<p>Phosphate buffer system (C)</p> Signup and view all the answers

Which of the following conditions can lead to metabolic acidosis?

<p>Diabetic ketoacidosis (B)</p> Signup and view all the answers

Flashcards

Strong Acid

A strong acid completely dissociates into its ions in water.

Weak Acid

A weak acid only partially dissociates into ions.

Strong Base

A strong base completely dissociates into its ions in water.

Weak Base

A weak base does not completely dissociate into ions in water.

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Acid (Arrhenius)

A substance that releases H+ ions (protons) in water.

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Base (Arrhenius)

A substance that releases OH- ions (hydroxide) in water or accepts H+ ions.

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Acid-Base Equilibrium

The balance between acids and bases to maintain a stable pH.

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Henderson-Hasselbalch Equation

Equation that helps calculate pH in a buffer solution given concentrations of acid and base and pKa of acid.

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Acid Dissociation Constant (Ka)

The tendency of an acid (HA) to lose a proton (H+) and form its conjugate base.

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pKa

The negative logarithm of the acid dissociation constant (Ka).

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pH scale

A scale used to measure the acidity or alkalinity of a solution, ranging from 0 to 14.

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pH

The negative logarithm of the hydrogen ion concentration ([H+]) in a solution.

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Acid-Base Balance

The body's mechanisms to maintain a near-neutral pH in fluids to facilitate normal function.

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Neutral pH

A pH of 7, indicating an equal concentration of hydrogen and hydroxide ions.

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Acidic Substance

Substances that release hydrogen ions (H+) into a solution.

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Alkaline Substance

Substances that take up hydrogen ions (H+) from a solution.

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Anion Gap

The difference between measured cations and anions in extracellular fluid (ECF).

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Normal Anion Gap

A value typically around 15 mEq/L A healthy balance of measured cations and anions in the blood.

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Anion Gap Calculation

A formula to discover the imbalance in the ECF (extracellular fluid). (Na+ + K+) - (Cl- + HCO3-) = Anion gap

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Metabolic Acidosis

An imbalance in acid-base balance where pH levels are off-kilter.

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Causes of Elevated Anion Gap

Conditions like diabetic ketoacidosis, lactic acidosis, and renal failure can cause an elevated anion gap.

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Causes of Normal Anion Gap

Some causes of normal anion gap metabolic acidosis include renal tubular acidosis and diarrhea.

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Significance of Anion Gap Calculation

Helps diagnose acid-base imbalances and differentiate between various causes of metabolic acidosis, especially helpful in cases with kidney or gastrointestinal problems.

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Diarrhea and Anion Gap

Diarrhea is one of the causes of abnormal anion gap, which can result from issues primarily related to fluid and electrolyte balance.

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High Anion Gap Acidosis

A condition where the anion gap is greater than 25, indicating a buildup of acids in the body. Causes often include kidney failure, diabetic ketoacidosis, lactic acidosis, or poisoning.

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Normal Anion Gap Acidosis

A condition where the anion gap is within the normal range, indicating acidosis caused by conditions like diarrhea and hyperchloremic acidosis.

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Arterial Blood Gas (ABG)

A blood test specifically measuring the pH, partial pressure of carbon dioxide (pCO2), and bicarbonate (HCO3-) in arterial blood.

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Compensation (Acid-Base)

The body's attempt to normalize pH by counteracting the primary disturbance.

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Serum Electrolytes

These are the vital elements like sodium, potassium, chloride, and bicarbonate that are measured in the blood serum and help determine acid/base balance.

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Normal Blood pH

The typical pH range of human blood is between 7.35 and 7.45, slightly alkaline.

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Primary Buffer System

The bicarbonate buffer system is the primary buffer in the human body, helping maintain a stable blood pH.

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Respiratory Acidosis

Respiratory acidosis occurs when the body cannot properly remove carbon dioxide (CO2), leading to an increased acidity (lower pH).

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Lactic Acidosis

Lactic acidosis occurs when there's a buildup of lactic acid in the blood, often due to strenuous exercise or medical conditions.

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Bicarbonate Regulation

The kidneys are the primary organs responsible for regulating bicarbonate levels in the blood.

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Buffer Effectiveness

A buffer is most effective when the pH is equal to the pKa of the weak acid.

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Respiratory Alkalosis

A condition characterized by a decrease in blood carbon dioxide levels and an increase in blood pH. This can occur due to hyperventilation, where rapid and deep breathing expels CO2 faster than the body can produce it.

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Bicarbonate (HCO3-) levels in Respiratory Alkalosis

In respiratory alkalosis, bicarbonate (HCO3-) levels are usually decreased. This is because the body attempts to compensate for the high pH by decreasing the amount of bicarbonate, which helps buffer the blood.

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Metabolic Alkalosis

A condition where the body loses too much acid or gains too much base, leading to an increase in blood pH. This can occur due to excessive vomiting or prolonged use of antacids.

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Study Notes

Acid and Base Concepts

  • Acids release protons (H+) in water, acting as proton donors.
  • Bases accept protons (H+) in water or release hydroxide ions (OH-).
  • Each acid has a characteristic tendency to lose its proton (H+) in an aqueous solution. Stronger acids lose their protons readily while weaker acids release their protons slower.

Learning Objectives

  • Unit 2: Acid and Base Concepts
  • 2.1: The acid-base balance concept
  • 2.2: Arrhenius definition
  • 2.3: Acid-base equilibrium
  • 2.4: Henderson-Hasselbalch equation

Arrhenius Definition of Acids and Bases

  • Acids release protons (H+) in water (proton donors).
  • Bases accept protons (H+) in water (proton acceptors) or release hydroxide ions (OH-).
  • Each acid has a tendency to lose its proton (H+) in an aqueous solution;

Strong Acids

  • Strong acids completely dissociate into ions in aqueous solution.
  • Examples: HCl, H₂SO₄, HNO₃ (inorganic)

Weak Acids

  • Weak acids partially dissociate into ions in aqueous solution.
  • Examples: Formic acid (HCOOH), Acetic acid (CH3COOH), Oxalic acid (C₂H₂O₄), Benzoic acid (C₇H₅COOH), Lactic acid, Phosphoric acid, Carbonic acid, Citric acid.
  • Weak acids are common in biological systems and are produced during metabolic processes.

Strong Bases

  • Strong bases completely dissociate into ions when dissolved in solution.
  • Examples: NaOH, KOH, Ba(OH)₂

Weak Bases

  • Weak bases do not completely dissociate into ions when dissolved in solution.
  • Examples: Amines, NH₄⁺, Aniline, Pyridine

Acids Produced in the Human Body

  • Carbonic acid (oxidation of carbon compounds)
  • Sulfuric acid (oxidation of sulfur-containing amino acids)
  • Phosphoric acid (metabolism of dietary phosphoproteins, nucleoproteins, phosphatides)
  • Organic acids (oxidation of carbohydrates, fats, and proteins)
  • Iatrogenic acids (certain medicines, like NH₄Cl, mandelic acid).

Acidic Substances of the Human Body

  • Carbonic acid (H₂CO₃)
  • Phosphoric acid (H₃PO₄)
  • Sulfuric acid (H₂SO₄)
  • Organic acids (lactate, acetoacetate, pyruvate)

Alkaline Substances of the Human Body

  • Citrate
  • Bicarbonates

Dissociation Constant (Kₐ)

  • The tendency of an acid (HA) to lose a proton (H+) and form its conjugate base (A⁻)
  • Kₐ = [H⁺][A⁻] / [HA]
  • pKₐ = -log Kₐ
    • A measurement of acid strength; lower pKₐ values correspond to stronger acids.

pH

  • pH is a measure of hydrogen ion (H⁺) concentration.
  • pH = -log[H⁺]
  • 0-7: Acidic
  • 7: Neutral
  • 7-14: Basic/Alkaline

Buffer Systems:

  • Buffers resist changes in pH when acids or bases are added.
  • Often mixtures of weak acids and their conjugate bases.
  • Important in maintaining blood pH and physiological pH inside cells.
  • Examples: Acetic acid (CH₃COOH) and acetate ion(CH₃COO⁻); Bicarbonate-carbonic acid buffer (HCO₃⁻/H₂CO₃); Phosphate buffer systems (HPO₄²⁻/H₂PO₄⁻); Protein buffers systems (e.g., hemoglobin, amino acids like histidine, cysteine)

Importance of Biological Buffers

  • Maintaining homeostasis
  • Regulating enzymatic function
  • Controlling pH in biochemical reactions

Buffer Systems in the Human Body

  • First line of defense against pH shifts (Chemical buffers) : Bicarbonate Buffer system, Phosphate buffer system, Protein buffer system
  • Second line of defense against pH shifts (Physiological buffers): Respiratory and renal mechanisms

Bicarbonate Buffer System

  • Major extracellular fluid buffer.
  • Composition: Sodium bicarbonate (NaHCO₃) and carbonic acid (H₂CO₃).
  • 20:1 ratio of bicarbonate to carbonic acid at pH 7.4. (ratio is maintained with the help of kidneys).

Phosphate Buffer System

  • Important intracellular buffer.
  • Composition: Mono hydrogen phosphate (HPO₂⁻) and dihydrogen phosphate ions (H₂PO₄⁻).
  • 4:1 ratio of mono hydrogen phosphate to dihydrogen phosphate maintained by kidneys.

Protein Buffer Systems

  • Includes hemoglobin and work inside blood.
  • Amino acids compose proteins, with carboxyl groups releasing H⁺ and amino groups accepting H⁺.
  • Side chains of amino acids (e.g., histadine,cystine) have buffering capacity.

Acid-Base Disorders

  • Acidosis: pH < 7.35 (Respiratory acidosis, Metabolic acidosis)
  • Alkalosis: pH > 7.45 (Respiratory alkalosis, Metabolic alkalosis)

Anion Gap

  • Measures the difference between measured cations (Na+, K+) and measured anions (Cl-, HCO3-), providing insights into metabolic acidosis where unmeasured anions (PO4³⁻, organic acids, etc.) are elevated.

Significance of Anion Gap Calculation

  • Helps diagnose acid-base imbalances,particularly metabolic acidosis.
  • Helps in the diagnosis of several other conditions.

Acid-Base Disorders, Further Details for diagnosis and testing

  • Provides detailed information about how to diagnose respiratory and metabolic acidosis and alkalosis including the various causes and examples of each.

Diagnostic Lab Values and Interpretations

  • Provides a list of normal serum electrolyte and arterial blood gas values.

Case Study Examples

  • A patient with a specific set of values providing examples of possible diagnosis of acid-base disturbances. (Page 55)

Additional Details and Important Considerations for Acid-Base Imbalance Diagnosis

  • Further descriptions of acid-base imbalances including the various causes of each and examples of chronic conditions associated with each. This includes a stepwise approach. (Page 50)
  • Explanation on how to determine the cause of the acid-base imbalance and further details on diagnosing and interpreting the findings. (Page 53)

Practiced Questions

  • Provides set of questions to test the student's knowledge about the acid-base balance. (Page 60)

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Acid And Base Concepts PDF

Description

Explore the fundamental principles of acids and bases in this quiz based on Unit 2. Understand the Arrhenius definition, the concept of acid-base equilibrium, and the notable characteristics of strong and weak acids. Test your knowledge on how acids and bases interact in aqueous solutions.

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