This document discusses acid-base regulation in the human body. It covers topics such as the carbonic acid-bicarbonate buffer system, respiratory regulation of hydrogen ion concentration, and disorders of acid-base balance like respiratory acidosis and alkalosis and metabolic acidosis and alkalosis. The key roles of the lungs, kidneys, and nutrition in maintaining acid-base homeostasis are also summarized.
The document discusses acid-base balance and buffer systems in the human body. It provides information on:
- The definition and examples of acids and bases. Strong acids fully dissociate while weak acids only partially dissociate.
- The importance of maintaining pH homeostasis and the consequences of acidosis or alkalosis. Blood pH is tightly regulated between 7.35-7.45.
- The major buffer systems that maintain pH, including bicarbonate, phosphate, and protein buffers. Bicarbonate acts as the primary buffer and its ratio with carbonic acid determines blood pH.
- Other factors like lungs, kidneys and hemoglobin that help control acid-base balance through processes
This document discusses acid-base balance and disorders. It begins by defining acids and bases, and describing the normal physiology of acid-base balance. It then discusses the four main types of acid-base disorders: metabolic acidosis, metabolic alkalosis, respiratory acidosis, and respiratory alkalosis. For each disorder it describes the primary disturbance (pH or HCO3-) and the secondary compensatory response. The document goes on to provide details on the causes, mechanisms, and clinical assessments of different metabolic and respiratory acid-base disorders.
The kidneys control acid-base balance by excreting either acidic or basic urine. In acidosis, the kidneys reabsorb bicarbonate and produce new bicarbonate to reduce acid levels. In alkalosis, the kidneys fail to reabsorb all filtered bicarbonate, increasing excretion and lowering bicarbonate levels to return pH to normal. The kidneys regulate pH through secretion of hydrogen ions, reabsorption of bicarbonate, and production of new bicarbonate.
The document discusses acidity, basicity, pH, and buffer systems in the human body. It defines acids as having a high hydrogen ion concentration and bases as having a low hydrogen ion concentration. The blood needs to maintain its pH between 7.35-7.45. The lungs and kidneys help regulate pH through exchanging carbon dioxide and excreting acids and bases. The bicarbonate buffer system uses dissolved carbon dioxide, carbonic acid, and bicarbonate ions to neutralize changes in blood pH. Too much acid in the body leads to acidosis and symptoms like fatigue, while too much base causes alkalosis and issues like arrhythmias.
The major buffer system in the blood is the bicarbonate buffer system (H2CO3/HCO3-). Carbon dioxide produced from cellular metabolism dissolves in the blood to form carbonic acid, which dissociates into bicarbonate and hydronium ions. The lungs and kidneys help regulate blood pH by controlling the levels of carbon dioxide and bicarbonate. Disruptions to this buffer system can result in acidosis or alkalosis, which have various causes and symptoms that require different treatments.
The document discusses the kidney's role in acid-base regulation through excretion of hydrogen ions, reclamation of bicarbonate ions, and excretion of titrable acid and ammonia. It also addresses metabolic acidosis and alkalosis, noting that metabolic acidosis occurs when there is a primary deficit of bicarbonate ions, while metabolic alkalosis occurs when there is a primary excess of bicarbonate ions. Compensation mechanisms including buffer systems, respiration, and renal mechanisms act to regulate pH levels in the case of acid-base imbalances.
The blood buffer system maintains blood pH between 6.8-7.4 by using bicarbonate, carbonic acid, and other buffers. When acids enter the bloodstream, bicarbonate buffers help prevent acidosis by neutralizing them. Similarly, when bases enter, bicarbonate helps prevent alkalosis. Abnormal pH outside this range can denature enzymes and cells, stopping bodily functions and potentially causing death. Acidosis results from excess acid and alkalosis from excess base, requiring treatment of the underlying cause to restore pH balance.
This document discusses acids and bases in the body. It defines acids as hydrogen containing substances that dissociate to release H+ ions and bases as substances that accept H+ ions. The key physiological acids and bases are discussed including bicarbonate, phosphate, and proteins. The three main mechanisms that regulate blood pH - buffers, respiration, and the kidneys - are summarized. Respiration controls carbonic acid levels while the kidneys regulate bicarbonate reabsorption and acid excretion to maintain pH. Acid-base imbalances can cause metabolic acidosis or alkalosis and respiratory acidosis or alkalosis depending on primary disorder.
This document discusses metabolic acidosis and alkalosis. It defines acids and bases, and explains how the body maintains acid-base balance through the lungs, kidneys, and buffer systems. Metabolic acidosis occurs when the body produces too much acid or the kidneys can't remove enough, decreasing the bicarbonate level. Causes include lactic acid, ketones, and renal failure. Metabolic alkalosis happens when bicarbonate increases, decreasing hydrogen ions, due to vomiting, diuretics, or base ingestion. Blood gas analysis measures pH, pCO2, and bicarbonate to diagnose acid-base disorders.
Buffers in the body resist changes in pH and maintain it within a narrow range. The major buffer systems are bicarbonate, phosphate, and proteins. Bicarbonate buffers work by absorbing excess hydrogen ions in the blood and tissues. The kidneys and lungs work together to control bicarbonate and carbon dioxide levels to regulate pH. When an acid is added, buffers prevent a large change in pH by neutralizing the hydrogen ions.
This document discusses respiratory and metabolic acidosis and alkalosis. It covers:
- The definitions and mechanisms of respiratory acidosis, respiratory alkalosis, metabolic acidosis, and metabolic alkalosis.
- The causes, signs and symptoms, and compensation mechanisms for each condition.
- Specific types like acute vs chronic respiratory acidosis, and chloride responsive vs chloride resistant metabolic alkalosis.
- How the kidneys, lungs, and buffering systems work to regulate pH and compensate for acid-base imbalances.
Concepts of acid base balance and its disorders are very important for practice of medicine.It is for the benefit of medical and students of allied fields.
Water is essential for life and makes up about 60% of the human body. It participates in metabolic reactions, transports solutes, regulates temperature, and is distributed between intracellular and extracellular compartments. Electrolytes like sodium, potassium, calcium, and magnesium are balanced in body fluids to maintain water balance. The kidneys, along with hormones like aldosterone and ADH, precisely regulate water and electrolyte balance by controlling water retention, excretion of waste products, and acid-base balance through buffers and respiratory and renal mechanisms.
The document discusses acid-base regulation in the body. It maintains that the body tightly regulates blood pH between 7.35-7.45 through buffering agents, the respiratory system, and renal system. When patients have damaged respiratory, renal, or metabolic functions, they are prone to acid-base imbalances. Acidosis occurs when blood pH decreases below 7.35 due to accumulation of acids. Alkalosis is when blood pH increases above 7.45 due to loss of acids. The lungs and kidneys work to regulate pH through removal of carbon dioxide and protons respectively.
This document discusses acids, bases, pH, buffers, and the regulation of pH in the body. It defines acids and bases, describes pH and how it is measured. It explains the carbonic acid-bicarbonate buffer system, which is one of the most important buffer systems in the body. It also discusses how respiratory regulation and kidney regulation help maintain pH levels through increasing or decreasing ventilation and excreting acid and bases in the urine. The kidney regulates pH through reabsorbing bicarbonate and secreting hydrogen ions into the tubule, where they react with phosphate and ammonia to generate buffers without lowering urine pH.
The document discusses electrolytes, focusing on sodium and potassium.
Sodium is the most prevalent cation in extracellular fluid and is essential for maintaining fluid balance and nerve/muscle function. Its levels are regulated by hormones like aldosterone that increase sodium reabsorption. Abnormal sodium levels can indicate conditions like hyponatremia or hypernatremia.
Potassium is the major intracellular cation and regulates muscle/nerve excitability. Its levels are maintained primarily via the sodium-potassium pump. Potassium is excreted renally, and hypokalemia can result from inadequate intake, excessive loss, or conditions affecting aldosterone. Precise sample collection and testing are needed to accurately assess
This document discusses the regulation of respiration. It covers the neural, automatic, and chemical control mechanisms that regulate breathing. The key points are:
1) Respiration is regulated by medullary and pontine respiratory centers in the brainstem that generate the breathing rhythm and control rate and depth.
2) Breathing is also automatically controlled and can occur without conscious effort. It is further modulated by inputs from chemoreceptors sensitive to oxygen, carbon dioxide, and pH levels in the blood.
3) Peripheral chemoreceptors located in the carotid bodies and aortic bodies detect changes in blood gases and signal the respiratory centers to adjust breathing accordingly. Central chemoreceptors in the brainstem are
This document discusses acid-base balance and imbalance. It defines key terms like pH, acids, and bases. The body regulates acid-base balance through buffering systems, respiratory compensation, and renal compensation. Acid-base imbalance can be diagnosed using arterial blood gases and anion gap tests. The main types of imbalance are respiratory acidosis and alkalosis from lung issues, and metabolic acidosis and alkalosis from kidney or production problems. Causes, signs, and compensation methods are described for each type.
This document summarizes acid-base balance in the human body. It discusses how pH is measured and regulated within strict limits. The body maintains pH levels between 7.35-7.45 through three main systems: buffer systems, the respiratory system, and the renal system. Deviations outside the normal range can cause issues in all body systems. Respiratory and metabolic acidosis and alkalosis occur when pH levels fall below or rise above normal ranges, respectively. The body responds through these three regulatory systems to correct imbalances and maintain appropriate acid-base levels.
The document summarizes gas exchange and oxygen transport in the human body. It discusses how (1) oxygen is extracted from the air and transported via the lungs to the blood, where it is carried by hemoglobin to tissues, and (2) carbon dioxide is transported in reverse from tissues to the lungs. Key aspects covered include alveolar gas transfer, the oxygen cascade, partial pressures of gases, diffusion principles, hemoglobin binding of oxygen and factors affecting it like pH, temperature and carbon monoxide.
This document summarizes the composition and distribution of body fluids in the human body. It discusses that the normal adult body is composed of 60% water, 7% minerals, 18% protein, and 15% fat. Total body water is distributed between intracellular fluid (ICF, 40% of body weight) and extracellular fluid (ECF, 20% of body weight). ECF is further divided into plasma (5% of body weight), interstitial fluid (15% of body weight), and transcellular fluid (1.5% of body weight). The document also describes the ionic composition of different body fluids and units used to measure solute concentration like moles, equivalents, and osmoles. It introduces
The human body is composed primarily of fluids, with water making up about two-thirds of the total body weight. The body's fluids are divided into two main compartments: intracellular fluid (ICF) and extracellular fluid (ECF). ICF makes up about 40% of total body water and is contained within cells, while ECF comprises around 20% and includes interstitial fluid, plasma, and transcellular fluids such as cerebrospinal fluid. ECF volume can be measured using substances that remain in the extracellular space, while total body water and plasma volume are determined through the dilution of markers distributed throughout the body's water compartments. Proper fluid balance is essential for acid-base regulation, electrolyte levels
The body maintains tight regulation of arterial blood pH between 7.35-7.45 through acid-base balance mechanisms. It uses buffer systems, and respiratory and renal systems to neutralize acids and bases. The major buffer systems are bicarbonate, phosphate, and proteins, which maintain pH by donating or accepting hydrogen ions. Deviations outside the normal pH range can impair membrane and protein function and are not survivable. The lungs and kidneys work to restore pH through removing carbon dioxide and hydrogen ions respectively.
This document discusses the normal mechanisms that maintain acid-base balance in the body. It describes how the body uses buffer systems, respiration, and the kidneys to regulate pH and compensate for acid-base imbalances. The buffer systems work quickly to neutralize acids and bases. Respiration then acts to remove carbon dioxide and adjust pH over minutes. Finally, the kidneys excrete or reabsorb acids and bases over longer periods through secretion of hydrogen ions, reabsorption of bicarbonate, and production of new bicarbonate. Together these coordinated systems tightly control pH within a narrow range necessary for normal human function and survival.
They are water soluble substances.
2. They are synthesized at a relatively low rate in well nourished individuals.
3. Plasma level of ketone bodies < 1mg/dl.
4. Urinary level of ketone bodies <3 mg/24 hour urine.
The document discusses acid-base balance and homeostasis. The bicarbonate buffering system helps maintain a constant plasma pH by buffering hydrogen ions. When the blood gains excess hydrogen ions (acidosis), the equilibrium shifts to produce more carbon dioxide, minimizing increased acidity. Respiratory compensation also helps by altering breathing to modify carbon dioxide levels in circulation.
6. Types of acids and bases
Strong acids
– Release large amount of Hydrogen ions
Weak acids
– Release small amount of Hydrogen ions
Strong bases
– Accept large amount of Hydrogen ions
Weak bases
– Accept small amount of Hydrogen ions
8. What Is Buffer ???
A buffer is a solution (or a substance) that has
the ability to maintain pH and bring it back to
its optimal value by addition or removal of
hydrogen ions
Buffer + H H buffer
9. Contd….
When Hydrogen ion conc. Increases
– Reaction shifts towards right
When Hydrogen ion conc. Decreases
– Reaction shifts towards left
In this way hydrogen ion concentration is
maintained
10. Types of chemical buffer
– Carbonic acid-bicarbonate –
– Buffering changes caused by organic and fixed
acids
– Protein buffer system-Amino acids
– Minor buffering system-
– Phosphate –Buffer pH in the ICF
12. Carbonic Acid-Bicarbonate
Buffering System
Carbonic acid-bicarbonate buffer system
Weak acid – H2CO3
Bicarbonate salt (NaHCO3)
Strong acid is added
– When HCL is added Hydrogen conc.
increases
– CO2 + H2O H2CO3 H + HCO3
13. Contd…
Strong base is added
H+ conc. Reduces
NaOH + H2CO3 NaHCO3+H2O
In this way CO2 conc. decreases
This inhibits respiration.
15. Bicarbonate buffer-
Has the following limitations:
– Cannot protect the ECF from pH changes due
to increased or depressed CO2 levels
– Only functions when respiratory system and
control centers are working normally
– It is limited by availability of bicarbonate
ions (bicarbonate reserve).
16. Phosphate buffer system-
Main elements of phosphate buffer system-
- H2PO4, and HPO4
Phosphoric acid changes pretty quickly into
dihydrogen phosphate, or H2PO4-.
This dihydrogen phosphate is an efficient
buffer.
18. Contd….
Phosphate buffer system in the ECF is low
compared to the bicarbonate buffer.
Its buffering power is less compared to the
bicarbonate buffer.
It has its importance in the renal
tubules of kidneys for two reasons.
.
19. Contd
1.Conc. of phosphate is more in tubules.
2. Tubular fluid has lower pH.
Conc. of phosphate is more in ICF compared
to ECF.
20. Protein buffer system
Proteins are made up of amino acids
Amino acids have a central carbon with four
groups off of it:
1.a carboxyl group (COOH)
2.an amino group (NH2)
3.a hydrogen atom
4.an R group
.
22. Contd…
The carboxyl and amino groups are what enable
proteins to act as buffers.
Carboxyl group is attached to the amino acid central
carbon: C - COOH
Carboxyl group consists of a double bond
to one of the oxygens and a single bond to the
hydroxyl group.
23. Contd...
At neutral pH the carboxyl ion is present as
COO instead of COOH.
Acidic medium – becomes COOH
Basic medium – becomes COO.
24. Contd…
Amino group is attached to the amino acid
central carbon: C - NH2.
Neutral pH, the amino group is actually-
NH3+ rather than just NH2.
Acidic medium – becomes NH3+
Basic medium- becomes NH2
27. Respiratory regulation Contd…
Pulmonary expiration of CO2 balances metabolic
formation of CO2
– 1.2 mol/L of dissolved CO2 is present in the ECF
corresponding to pCO2 of 40 mm/hg
– Rate of pulmonary ventilation is inversely
proportional to CO2 & pCO2
– So either pulmonary ventilation rate of CO2
– or its formation by tissues can change pCO2
in ECF.
28. Contd…
Increasing alveolar ventilation decreases ECF
hydrogen ion conc. And raises pH
– If alveolar ventilation increases the pCO2 decreases.
– If alveolar ventilation decreases the
pCO2 increases.
– Twice rise of AV--rises pH of ECF by about 0.23
– Decrease of AV to ¼ -- decreases pH by 0.45
29. Contd…
Increased Hydrogen ion conc. Stimulates
alveolar ventilation
Change in alveolar ventilation rate is much
greater in reduced levels of pH than in
increased levels of pH
30. Reason
Alveolar ventilation rate decreases
Increases pH
O2 added in blood reduces
Demand of O2 in blood increases
pO2 also decreases
Stimulates ventilation
31. Feedback control of Hydrogen
ion conc. By RS
H conc. Falls below normal
Respiration is depressed
Alveolar ventilation decreases
H increases back to normal
32. Bufffering power of RS
The kidneys work in elimination of hydrogen
ion conc. and control imbalance.
Its capacity is 1-2 times as much as other
chemical buffers.
33. Impairment of lungs function:
Impairment of lung function leads to
emphysema and respiratory disorders.
Kidneys play a major physiologic mechanism
for returning pH to normal
34. Renal mechanism of acid-base
regulation
Kidneys regulate the blood pH by
1. maintaining alkali reserves
2. excreting / reabsorbing acid/base.
Urine pH is lower than blood pH
Kidneys- Acidification of urine.
35. Contd…
Excretion of hydrogen ions
Reabsorption of bicarbonate ion
Excretion of ammonium ions
39. Contd…
Respiratory acid-base disorders are initiated by
an increase or decrease in partial pressure of
carbondioxide whereas metabolic disorders are
initiated by an increase or decrease in
bicarbonate ion.
40. Contd…
Alkalosis - Partial pressure of oxygen
increases.
Acidosis – Partial pressure of carbondioxide
increases.
41. Contd…
Respiratory acidosis-
Decrease in rate of pulmonary ventilation-
Increased pCO2 of ECF.
Respiratory alkalosis-
Increased rate of ventilation-
Decrease the pCO2
47. Contd…
Causes- Metabolic alkalosis
1. Vomiting of gastric contents
2. Ingestion of alkaline drugs etc.
48. Correction by renal for…
Acidosis-
Increased excretion of hydrogen ions and
addition of bicarbonate ions to the ECF.
Alkalosis-
Decreased tubular secretion of hydrogen ions
and increased excretion of HCO3_
51. EAT MORE -- Alkaline (80%)
AcidAlkaline food chart
EAT LESS -- Acidic (20%)
Highly Alkaline Moderately Alkaline Mildly Alkaline Neutral/ Mildly Acidic Moderately Highly Acidic
Acidic
pH 9.5 alkaline water Avocado Artichokes Black Beans Fresh, Natural Juice Alcohol
Himalayan salt Beetroot Asparagus Chickpeas/Garbanzos Ketchup Coffee & Black Tea
Grasses Capsicum/Pepper Brussels Sprouts Kidney Beans Mayonnaise Fruit Juice
Cucumber Cabbage Cauliflower Seitan Butter (Sweetened)
Kale Celery Carrot Cantaloupe Apple Cocoa
Kelp Collard/Spring Greens Chives Currants Apricot Honey
Spinach Endive Courgette/Zucchini Fresh Dates Banana Jam
Parsley Garlic Leeks Nectarine Blackberry Jelly
Broccoli Ginger New Baby Potatoes Plum Blueberry Mustard Miso
Sprouts(soy, alfalfa etc) Green Beans Peas Sweet Cherry Cranberry Rice Syrup
Sea Vegetables (Kelp) Lettuce Rhubarb Watermelon Grapes Soy Sauce
Green drinks Mustard Greens Swede Amaranth Mango Vinegar
All Sprouted Beans/ Sprouts Okra Watercress Millet Mangosteen Yeast
Onion Grapefruit Oats/Oatmeal Orange Dried Fruit
Radish Coconut Spelt Peach Beef
Red Onion Buckwheat Soybeans Papaya Chicken
Rocket/Arugula Spelt Rice/Soy/Hemp Protein Pineapple Eggs
Tomato Lentils Freshwater Wild Fish Strawberry Farmed Fish
Lemon Tofu Rice & Soy Milk Brown Rice Pork
Lime Other Beans & Legumes Brazil Nuts Oats Shellfish
Butter Beans Goat & Almond Milk Pecan Nuts Rye Bread Cheese
Soy Beans Most Herbs & Spices Hazel Nuts Wheat Dairy
White Haricot Beans Avocado Oil Sunflower Oil Wholemeal Bread Artificial Sweeteners
Chia/Salba Olive Oil Grapeseed Oil Wild Rice Syrup
Quinoa Coconut Oil ` Wholemeal Pasta Mushroom
Flax Oil/ Udo’s Oil Ocean Fish
52. SO WHY NOT CONTROL THE
ACID BASE BALANCE WITH
FOOD…???
55. The Central Role of the Carbonic
Acid-Bicarbonate Buffer System in
the Regulation of Plasma pH
Figure 27.11a
56. The Central Role of the Carbonic
Acid-Bicarbonate Buffer System in
the Regulation of Plasma pH
Figure 27.11b
57. Acid-Base Disorders
Respiratory acid base disorders
– Result when abnormal respiratory function causes
rise or fall in CO2 in ECF
Metabolic acid-base disorders
– Generation of organic or fixed acids
– Anything affecting concentration of bicarbonate ions
in ECF
60. Metabolic acidosis
Major causes are:
– Depletion of bicarbonate reserve
– Inability to excrete hydrogen ions at kidneys
– Production of large numbers of fixed / organic acids
– Bicarbonate loss due to chronic diarrhea
63. Detection of acidosis and
alkalosis
Diagnostic blood tests
– Blood pH
– PCO2
– Bicarbonate levels
Distinguish between respiratory and
metabolic
Animation: Acid-Base Homeostasis
64. Changes with age include
Reduced total body water content
Impaired ability to perform renal compensation
Increased water demands
– Reduced ability to concentrate urine
– Reduced sensitivity to ADH/ aldosterone
Net loss of minerals
Inability to perform respiratory compensation
Secondary conditions that affect fluid, electrolyte, acid-
base balance
65. You should now be familiar with:
What is meant by “fluid balance,” “electrolyte
balance,” and “acid-base balance”
The compositions of intracellular and
extracellular fluids
The hormones that play important roles in
regulating fluid and electrolyte balance
The movement of fluid that takes place within
the ECF, between the ECF and the ICF, and
between the ECF and the environment
66. You should now be familiar with:
How sodium, potassium, calcium and chloride
ions are regulated to maintain electrolyte
balance
The buffering systems that balance the pH of
the intracellular and extracellular fluids
The compensatory mechanisms involved in
acid-base balance