Denver School of Nursing – ADN & BSN ProgramsLecture: Fridays 3:00pm – 9:00pmNo Laboratory component for this class
BIO 206 & 308 – Ch 4 – pH & Fluid Balance
Distribution of Body FluidsTotal body water – all fluids 60% of weight
Intracellular fluid (ICF) 2/3 TBWExtracellular fluid (ECF) 1/3 TBW Interstitial fluid – between cells Intravascular fluid – blood plasma Lymph, synovial, intestinal, CSF, sweat, urine,
pleural, peritoneal, pericardial and intraocular fluid
“Cells live in a fluid environment with electrolytes and acid base concentrations maintained within a narrow range”
changes or shifts → radically alter metabolism → life threatening
Sodium (Na+) Primary ECF cation Regulates osmotic forces Role▪ Neuromuscular irritability, acid-base balance,
cellular reactions, and membrane transport
Chloride (Cl-) Primary ECF anion Provides electroneutrality
Sodium and Water BalanceBalance between Na+ and H2O - ↑ or ↓ of salt↑ or ↓ water
Tonicity – change in concentration of solutes (salt) with relation to solvent (water)
Tonicity (280 – 294m Osm) Isotonic – 0.9% NaCl – iso osmolar
imbalance no change in cells Hypertonic – ECF > 0.9% NaCl – (↓
H2O or ↑ salt) cells shrink Hypotonic – ECF < 0.9% NaCl (↑ H2O
or ↓ salt) cells swell“Extracellular Fluid”- interstitial space
90% ECF cations135 – 145 mEq/L
Hypernatremia - > 145 mEq/L
Hyponatremia - < 135 mEq/L
Hypernatremia-causes• ↑ Na or ↓ H2O• IV therapy – acidosis (NaHCO3)Cushing's Syndrome - ↑ ACTH → aldosterone
fever, respiratory infection - ↓ H2Odiabetes, diarrhea - ↓ H2O ↓ H2O intake - coma
• H2O movement ICF → ECF(interstitial)• Manifestations– Intracellular dehydration: convulsions, thirst,
fever, muscle twitching, hyperreflexia
Hyponatremia ↓ Na or ↑ H2O Vomiting, diarrhea, GI suction, burns,
diuretics, D5W replacement (isotonic sol’n)
Manifestations Lethargy, confusion, depressed reflexes,
seizures, coma, hypotension, tachycardia, ↓ urine output
Hypochloremia
Result of hyponatremia or ↑ HCO3
Vomiting – loss HCl
Cystic fibrosis
Potassium (resting potential) Major intracellular electrolyte 98% intracellular – Na – K – ATP Pump 3.5 – 5.0 mEq/L Transmission and conduction of nerve
impulses, normal cardiac rhythm, skeletal and smooth muscle contractions: “action potentials”
“Da BAD BOY of ELECTROLYTES”
Potassium Levels Change in pH affects K+ balanceAcidosis causes:
↑ ICF H+ → K+ moves out to ECF maintains + ion balance
Aldosterone; insulin, epinephrine Alkolosis causes:
K+ → into cell Glucagon # entry into cell
Glucocorticoids → K+ excretion
Hypokalemia K+ < 3.5 mEq/L ↓ intake, ↑ loss, ↑ entry into cells Manifestations: membrane
hyperpolorizations ↓ excitability – weakness, smooth muscle, atrophy, cardiac dysrhythmias (bradycardia…asystole)
HyperkalemiaK+ > 5.0 mEq/L – rare
↑ shift from ICF (acidosis), ↓ renal excretion, insulin deficiency or cell trauma
Hyperkalemia Mild attacks
↑ neuromuscular irritability – tingling of lips & fingers, restlessness, intestinal cramps – diarrhea
Severe attacks No repolarization → muscle weakness, ↓ tone,
flaccid paralysis Cardiac dysrhythmias “funky chicken”
Calcium (threshold potential) 99% located in bone – hydroxyapatite Bone, teeth, blood clotting, hormone
secretion, cell receptor function Hypo - ↓ block of Na into cell ↑
neuromuscular excitability (muscle cramps) Hyper - ↑ block Na - ↓ neuromuscular
excitability (muscle weakness, cardiac arrest, kidney stones, constipation)
Hypo - ↓ block of Na into cell
↑ neuromuscular excitability (muscle cramps)
Source: Review of Clinical Signs, Dr. Frank Urbano MD 2007.
Low SERUM K...decreased excitability Nerves & muscles…bradycardia---asystole
High SERUM K …increased excitability Cardiac dysrhythmias
Low SERUM Ca… increased excitability “Chvostek & Trousseau’s Signs”
High SERUM Ca… decreased excitability
pH (0 to 14) Inverse logarithm of the H+ concentration -
0.0000001 mg/L – 1x10 -7
so pH = 7 pH = power of hydrogen pH changes by one unit (7 → 6)
[H+] 10 fold Biological fluids
pH < 7.4 = acidic > 7.4 = basic
Physiologic Range of Blood pH = 7.35-7.45
pH Acids are formed as end products of
protein, carbohydrate and fat metabolism
Narrow “life range” – 7.35 – 7.45 Bone – lung – kidneys – major regulatory organs
“Absolute Range of Life:6.8-7.8”
pHBody acids exist in two forms
Volatile H2CO3 (maybe eliminated as CO2)
Nonvolatile – eliminated by kidneys sulfuric, phosphoric
Image from: http://www.answers.com
Image from: http://www3.oes.edu & http://www.fitnessspotlight.com
Image from: http://www.getfit4kidz.com/
Water Movement Between ICF and ECF“water, nutrients and waste products”
capillary interstitial space• #1 Capillary hydrostatic pressure • blood pressure “fluid out”
• #2 Capillary oncotic pressure • water attraction “fluid in”(Plasma Proteins)
• #3 Interstitial hydrostatic pressure • fluid towards capillary
• #4 Interstitial oncotic pressure • water attraction “fluid in”
water movement
Source: Huether, McCance Understanding Pathophysiology 4th Ed. 2008
Edema!!
Edema: 4 Major Causes“excessive accumulation of fluids within the
interstitial space”
1)↑ hydrostatic pressure Venous obstruction – DVT, hepatic obstruction Salt and water retention – heart, renal failure
2)↓ plasma oncotic pressure ↓ albumin – liver disease, malnutrition, kidney
disease, burns, hemorrhage
3)↑ capillary permeability – trauma, burns, neoplastic and allergic reactions
4) Lymph obstruction – removal of nodes (surgery), inflammation or tumors
Source: Huether, McCance Understanding Pathophysiology 4th Ed. 2008
From your A&P sources…
What are the two most important body systems for fluid, Electrolyte, and pH balance??
What are the two most important regulatory systems for fluid, electrolyte and pH balance?
1) 2)
When the Blood pH is low, it is called? When the Blood pH is high, it is called?
1) Metabolic Acidosis
2) Metabolic Alkalosis
3) Respiratory Acidosis
4) Respiratory Alkalosis
Much more detail to come latter in the lecture…
Image from: http://academic.kellogg.edu
Image from: http://academic.kellogg.edu
Physiology of the Urinary System: Renal function▪ Filtration▪ Reabsorption▪ Secretion
Regulation of Urine Volume▪ Renin Angiotensin Aldosterone system
(RAAS)
Image from: http://www.answers.com
Sodium, Chloride & Water Balance
“kidneys and hormones” – central roleWater : ADH – hypothalamus –
posterior pituitary
Na+ and Cl- aldosterone – adrenal gland Natriuretic hormones– atrial muscle
Physiological pH Control Systems- (p.1003 of our text)
Type Response Time Example“Chemical buffer systems”
Immediate 1) Bicarbonate buffer system
2) Phosphate buffer system
3) Protein buffer system
“Physiological buffer systems”
a) Minutes
a) Hours
a) Respiratory Response system
b) Renal response system
Source: http://www.mpoullis.net
~ All body fluids, inside or outside cells have buffers which defend the body against pH changes~ The most important buffer in extracellular fluids, including blood, is a mixture of carbon dioxide (CO2) and bicarbonate anion (HCO3)~ CO2 acts as an acid (it forms carbonic acid when it dissolves in water), donating hydrogen ions when they are needed~ HCO3 is a base, soaking up hydrogen ions when there are too many of them~ The HCO3/CO2 buffer system is extremely important because it can be rapidly readjusted in alkalosis and acidosis~ There are also other buffers in blood, such as proteins and phosphate~ The ability to resist pH change is given by the buffer capacity, which is a function of the concentration and dissociation constant (pK) of the weak acid~ If there is more than one buffer in the solution, the buffer capacities are additive
The Chief Blood Buffer is a Mixture of Bicarbonate and Carbon Dioxide
Source Mayo Clinic: http://discoverysedge.mayo.edu
Source: http://www.mpoullis.net
The Chief Blood Buffer is a Mixture of Bicarbonate and Carbon Dioxide
Source: http://www.mpoullis.net
~ The balance will swing toward a low pH, producing acidosis~ Pathology leading to this Acidosis can be:
1) CO2 increase via hypoventilation (pneumonia, emphysema)
2) Metabolic conditions (ketoacidosis due to excess fat metabolism
(diabetes mellitus) which will lower bicarbonate.
Too Much CO2 or Too Little HCO3 Will Cause Acidosis
Source: http://www.mpoullis.net
~ The balance will swing toward a high pH, producing alkalosis~ Pathology leading to this Alkalosis can be:
1) CO2 decrease via hyperventilation (Remember Respiration “Blows off CO2”)
2) Emesis removed stomach acid and raises bicarbonate (Alkalosis is clinically less common than acidosis)
Too Much HCO3or Too Little CO2 Will Cause Alkalosis
Buffer is a chemical that binds XS H+ or OH- without a significant change in pH
Consists of a PAIR of a weak acid and its conjugate base
Most important plasma buffering system 1. Carbonic acid – bicarbonate system2. Hemoglobin (intracellular)
H2O + CO2 H2CO3 H+ + HCO3-
1 20 Lung Kidney Phosphate- HPO4Ammonia – NH3 Compensation Respiratory - ↑ or ↓ CO2 Renal - ↑ or ↓ acidity / alkalinity of urine
Correction – buffer pairs →
Other Systems not previously discussed Proteins: - charge, mostly intracellular
Hemoglobin –H + Hb → HHb + CO2 → HHbCO2 (weak acid)
.
Source: Huether, McCance Understanding Pathophysiology 4th Ed. 2008
Figure 4-10 (p. 116)
Source: Huether, McCance Understanding Pathophysiology 4th Ed. 2008
Figure 4-11 (p. 117)
Source: Huether, McCance Understanding Pathophysiology 4th Ed. 2008
Figure 4-12 (p. 117)
Source: Huether, McCance Understanding Pathophysiology 4th Ed. 2008
Figure 4-13 (p. 118)
1) Metabolic Acidosis – Different diseases such as untreated diabetes mellitus or during starvation, the blood pH becomes acidic because there is higher carbonic acid to bicarbonate ratio. This stimulated the respiratory centers to increase respiratory rate and thus “blow off” carbon dioxide. The kidneys will also excrete increased levels of H ions and NH3. If these mechanisms can not compensate then the pathologic condition of uncompensated metabolic acidosis develops
2) Metabolic Alkalosis – Excesive use of antacids or excessive emesis can produce metabolic alkalosis. Initially the condition can result to bicarb levels up to 40 x greater than carbonic acid. Compensatory mechanisms function to increase the carbonic acid and decrease the bicarb. This is done via hypoventilation and increased renal excretion of bicarb. Once again if compensation is not adequate uncompensated metabolic alkalosis develops.
Source: http://www.mpoullis.net
3) Respiratory Acidosis – Pneumonia, emphysema and barbiturate OD are leading causes of retention of carbon dioxide in the blood. In these conditions the carbonic acid is greater than bicarbonate buffer. The compensatory reaction is for the kidneys to excrete H ions and retain more bicarbonate.
4) Respiratory Alkalosis – Hyperventilation due to a multitude of reasons (fever or hysteria) can result in excessive loss of carbonic acid and lead to respiratory alkalosis. Once again the kidneys will attempt to compensate via increased H ion reabsorption and increased bicarbonate excretion.
1) Metabolic Acidosis
2) Metabolic Alkalosis
3) Respiratory Acidosis
4) Respiratory Alkalosis
pH = 7.35 – 7.45pO2 = 80 to 100 mmHgpCO2 = 35 – 45 mmHgHCO3 = 22-26 mEq/LSaO2 = > 90%
PatientABG: pH = 7.3pCO2 = 40 mmHg pO2 = 70 mmHgHCO3 = 20 mEq/L
1. pH = ? → acidosis 2. pCO2 = ? → normal3. HCO3 = ? → low 4. pO2 = ? → low
Patient pH = 7.30 1. pH = acidotic Pco2 = 30mm Hg 2. Pco2 = alkalotic Po2 = 68mm Hg 3. Po2 = hypoxic HCO3 = 14mEq/L 4. HCO3 = acidotic O2 sat. = 92% 5. O2 sat = low “same directions = compensation”
Metabolic acidosis with partial respiratory compensation
ACIDOSIS: CNS depression Stupor to confusion to coma
ALKYLOSIS: CNS irritability Restlessness to seizures
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