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Lecture 2 01

# Lecture 2 01 - Lecture 2 Properties of Red Blood Cell...

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Lecture 2 01/09/2008 Properties of Red Blood Cell Membranes Osmosis/RBC’s I. Osmosis – Tank system Water is standard solvent for all biological systems Membranes A.) Permeable – lets everything pass, therefore water/sucrose pass back and forth At equilibrium: 1.) [sucrose] A = [sucrose] B 2.) Tube A = Tube B B.) Semi-permeable membrane only solvent crosses (water) At equilibrium: π = ρg h π = osmotic pressure developed and exerted by sucrose ρ = density of solution g = gravity h = what you end up with at equilibrium π = CRT, R = gas constant, T = temperature, C = concentration of solute particles more concentration of solute particles, more exertion of osmotic pressure based on presence of solute particles C = osmolarity = S/V, S = # of solute particles, V = volume it is distributed in Non-electrolytes do not dissociate Sucrose, urea, glucose Molarity = osmolarity 150 mM sucrose = 150 mOsm sucrose Electrolytes – salts, dissociate NaCl Na + + Cl - CaCl 2 Ca ++ + Cl - + Cl - Molarity x dissociation # = osmolarity 150 mM NaCl 300 mOsm Keep in mind: NaCl doesn’t dissociate 100%, 166 NaCl = 312 Sucrose (pretty close) Comparing one solution to another solution: Isoosmotic generate same osmotic pressure (π) A = 2 mM sucrose B = 1 mM NaCl Hyperosmotic generate a greater π A = 2 mM sucrose, hyperosmotic to:

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B = 0.5 mM NaCl Hypoosmotic generate a lower π B is hypo to A In physiology, normal is plasma osmotic pressure Stock solution of RBC
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Lecture 2 01 - Lecture 2 Properties of Red Blood Cell...

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