BODY FLUIDS and ELECTROLYTES Resources: Textbook (glossary, clinical studies, sample quizzes) Textbook (sample quizzes, exercises, cadaver practicals) Medical Research Learning Activities Interactions:Foundations CD (System overview, relationships with other systems) Marieb CD (Electrolytes) Tortora Grabowski CD ( Regulating Blood pH) Interactive Physiology CD (Body Fluids, Water Homeostasis, Electrolyte Homeostasis, Acid/Base Balance) Lecture Notes I. Body fluids (H2O + solutes) usually 55-60 % of body. A. Fluids 1. locations a. Intracellular (within cells) most (2/3) of body fluids b. Extracellular (outside cells) 1/3 of body fluids interstitial fluid (around cells) and plasma (blood) 2. consistency water and solutes solutes mostly ions (electrolytes) with some dissolved organics B. Fluid balance (movement of fluid between compartments) 1. Active transport (ions). Ion transport, increasing solute concentration, determines osmotic pressure gradient. 2. Osmosis (H2O). Higher osmotic pressure draws more water as result of greater solute concentration. C. Fluid Balance 1. Water gain a. Diet (drinking and moist food) ~ 2 liters/day b. Metabolic water manufactured due to oxidative metabolism ~ 0.2-3 l/d. total input ~ 2 1/2 l/d 2. Water loss a. Kidneys ~ 1.5 l/d b. Skin ~0.6 l/d c. Lungs ~.3l/d d. GI tract ~.1 l/d total output 2 1/2 l/d 3. Regulation of water gain (thirst) if more loss than gain, then dehydration. Dehydration results in low blood volume, decreased saliva and increased blood osmotic pressure. These stimuli stimulate thirst center in hypothalamus, triggering increased water intake. (mostly drinking). 4. regulation of water and solute loss most water is lost via urination due to NaCl loss- "water follows salt" NaCl loss determines blood osmotic pressure. Aldosterone primarily determines salt loss ADH determines water loss D. Dissolved substances 1. Non-electrolytes covalently bonded molecules . serum proteins play a role in maintaining blood OP. 2. Electrolytes molecules that are ionically bonded (usually inorganic) NaCl = Cl– + Na+ CaCl2 = Ca++ + Cl– + Cl– H2O breaks ionic bonds causing increased # of particles therefore increased osmotic pressure therefore electrolyte concentrations control water movement a. Na+ - most abundant cation in extracellular fluids *Very strong role in fluid movement (increased ECF osmotic pressure) *Strong role in transmission of electrical impulses if low [Na+] then increased [aldosterone] (more Na+ reabsorbed) and decreased ADH (more water lost) increase ECF [Na+] if excess [Na+] then edema results (renal failure and hyperaldosteronism) b. Cl– most abundant anion in extracellular fluid helps Na+ distribute fluid to ECF if low [Cl– ] , then decreased ADH (more water lost) increases ECF [Cl– ] c. K+ most abundant cation in intracellular fluid major role in transmission of electrical impulses if excess [K+], then increased [aldosterone] decreases [K+] d. HCO3– second most abundant anion in extracellular important in buffering pH of extracellular and plasma fluids major mechanism for transporting CO2 gas e. Ca++ high in extracellular, however most in bone (CaHPO4) controlled by CT & PTH increased [CT] causes decreased [Ca++] in blood and with Ca staying in bone increased [PTH] causes increased [Ca++] in blood and with more Ca++ into blood f. PO4– highest anion in intracellular fluid important buffer in cells most is bound in organics including ATP much is also bound up with Ca++ as Ca2PO4 bone matrix increased [CT] causes decreased [PO4–] in blood increased [PTH] causes increased [PO4–] in blood II. Acid base balance (buffering) A. Acids & bases 1. pH = [H+] in solution goes from 0 – 14 depending on [H+] values 0 – 7 = acid \ many H+ ions values 7 – 14 = base \ few H+ ions 2. Ionic acids (HCl, H2CO3) dissociate (break up) in water and give off H+ ion to decrease pH (more acidic) of solutions 3. Base (HCO3-) combines with H+ to increase pH (more basic) of solutions B. pH balance systems 1. Chemical buffering systems consist of weak acid and salt of acid (which serves as weak base) H2CO3 = NaHCO3 + H, i.e., weak acid will give off H+ if conditions have low [H+] weak base (salt) will receive H+ if conditions have high [H+] therefore [H+] is kept from going too low (basic) or too high (acidic) a. Carbonic acid -- bicarbonate buffer major interstitial fluid buffer too few H+ ions (blood basic) (buffer acts to release +++ CO2 + H2O= H2CO3 = H+ + HCO3– b. Protein buffer major intracellular/plasma buffer Amino acid acts both ways \ same molecule can act as base or acid c. Phosphate buffer similar to bicarbonate system (Na2HPO4) unimportant in plasma but effective buffer for urine & intracellular result: too few H+ ions (buffer acts as acid) and release H+ too many H+ ions (buffer acts as base and combines H+) 2. Exhalation of CO2 (Respiratory system) increased [CO2] drives reaction toward release of H+ therefore more acidic decreased [CO2] drives reaction toward combination of H+ therefore more basic therefore rate of ventilation can change [CO2] increased ventilation : increase pH (less acidic) 3. Kidney excretion of H+ (Urinary system) H+ ions are actively transported in nephron to adjust body pH in exchange for Na+ III. Acid-base imbalances normal blood pH range is narrow 7.35–7.45 more acid - acidosis 7.35 – 6.20 (low O2 transport) more basic – alkalosis 7.45 – 8.00 usually these changes are moderated (compensated) by above pH balancing systems A. Imbalances of PCO2 (respiratory) 1. Respiratory acidosis (pH low ) PCO2 too high due to CO2 buildup increased carbonic acid and increased H+ ions (more acidic) Cause: Respiratory disease & damage -- hypoventilation Compensation: increased renal excretion of H+ ions 2. Respiratory Alkalosis (pH high ) PCO2 too low due to low CO2 Cause: Hyperventilation or any disease/damage that stimulates respiration Compensation: decreased renal excretion of H+ ions B. Imbalance of HCO3 concentration 1. Metabolic acidosis (pH low ) low [HCO3] \ H+ not bound in that buffer, resulting in excess H+ (low pH) in blood Cause: Loss of HCO3 ( diarrhea, renal failure, ketosis) Compensation: respiratory by hyperventilation (remove excess CO2) low pHof blood (Bohr effect) : decreased O2 transport 2. Metabolic alkalosis (pH high ) high [HCO3] Cause: nonrespiratory loss of acid, e.g., vomiting, endocrine problems Compensation: respiratory by hyporventilation i.e., slow CO2 loss