Basics Of Fluids Flashcards
What is osmolality?
Osmolality - number of osmoles of solute per kilogram of solvent. The normal osmolality of ECF is 285-290mosmoles/kg, the same as the ICF and unaltered by temperature
• Brandis has 287mosm/kg for plasma (ECF is 285-290)
• Total plasma osmotic pressure is 5545mmHg
What is normal osmolality of the blood
Osmolality - number of osmoles of solute per kilogram of solvent. The normal osmolality of ECF is 285-290mosmoles/kg, the same as the ICF and unaltered by temperature
• Brandis has 287mosm/kg for plasma (ECF is 285-290)
• Total plasma osmotic pressure is 5545mmHg
How does osmolality compare between the blood and ICF
Osmolality - number of osmoles of solute per kilogram of solvent. The normal osmolality of ECF is 285-290mosmoles/kg, the same as the ICF and unaltered by temperature
• Brandis has 287mosm/kg for plasma (ECF is 285-290)
• Total plasma osmotic pressure is 5545mmHg
How does temperature effect osmolality?
Osmolality - number of osmoles of solute per kilogram of solvent. The normal osmolality of ECF is 285-290mosmoles/kg, the same as the ICF and unaltered by temperature
• Brandis has 287mosm/kg for plasma (ECF is 285-290)
• Total plasma osmotic pressure is 5545mmHg
WHat is the total osmotic pressure of plasma
Osmolality - number of osmoles of solute per kilogram of solvent. The normal osmolality of ECF is 285-290mosmoles/kg, the same as the ICF and unaltered by temperature
• Brandis has 287mosm/kg for plasma (ECF is 285-290)
• Total plasma osmotic pressure is 5545mmHg
What is tonicity?
Tonicity - effective osmolality of a solution - a measure of only the particles which are capable of ascertain an osmotic force across a cell membrane
What are colligative properties of solutions
Properties dependent on the number of molecules dissolved in a solvent per unit volume
Vapour pressure
Boiling point
Freezing point
Osmotic pressure
WHat are examples of colligative properties of a solution
Vapour pressure
Boiling point
Freezing point
Osmotic pressure
What happens to colligative properties with increasing solute concentration
• Vapour pressure depression
• Boiling point elevation
• Freezing point depression
• Osmotic pressure
Define osmosis
• Osmosis is the diffusion of solvent molecules into a region in which there is a higher concentration of a solute to which the membrane is impermeable
What is osmotic pressure
• Osmotic pressure is the excess pressure required to maintain osmotic equilibrium (to prevent movement of the solvent) between a solution and the pure solvent separated by a membrane permeable only to the solvent
• the van ‘t Hoff equation describes osmotic pressure:
◦ P = (nRT) / V
◦ Can also be written as
‣ n x c/M x RT
• c = concentration in g/L
• M = molecular weight of molecules
• where
◦ P is the osmotic pressure,
◦ n is the number of particles into which the substance dissociates, i.e. your sodium acetate dissociates into sodium and acetate, and therefore the n = 2
◦ R is the universal gas constant, which is 0.082 L atm mol-1 K-1
◦ T is the absolute temperature (Kº)
◦ V is the volume
What is the equation for osmotic pressure?
• Osmotic pressure is the excess pressure required to maintain osmotic equilibrium (to prevent movement of the solvent) between a solution and the pure solvent separated by a membrane permeable only to the solvent
• the van ‘t Hoff equation describes osmotic pressure:
◦ P = (nRT) / V
◦ Can also be written as
‣ n x c/M x RT
• c = concentration in g/L
• M = molecular weight of molecules
• where
◦ P is the osmotic pressure,
◦ n is the number of particles into which the substance dissociates, i.e. your sodium acetate dissociates into sodium and acetate, and therefore the n = 2
◦ R is the universal gas constant, which is 0.082 L atm mol-1 K-1
◦ T is the absolute temperature (Kº)
◦ V is the volume
What is the Von Hoff equation?
• Osmotic pressure is the excess pressure required to maintain osmotic equilibrium (to prevent movement of the solvent) between a solution and the pure solvent separated by a membrane permeable only to the solvent
• the van ‘t Hoff equation describes osmotic pressure:
◦ P = (nRT) / V
◦ Can also be written as
‣ n x c/M x RT
• c = concentration in g/L
• M = molecular weight of molecules
• where
◦ P is the osmotic pressure,
◦ n is the number of particles into which the substance dissociates, i.e. your sodium acetate dissociates into sodium and acetate, and therefore the n = 2
◦ R is the universal gas constant, which is 0.082 L atm mol-1 K-1
◦ T is the absolute temperature (Kº)
◦ V is the volume
What factors determine osmotic pressure
• Osmotic pressure is the excess pressure required to maintain osmotic equilibrium (to prevent movement of the solvent) between a solution and the pure solvent separated by a membrane permeable only to the solvent
• the van ‘t Hoff equation describes osmotic pressure:
◦ P = (nRT) / V
◦ Can also be written as
‣ n x c/M x RT
• c = concentration in g/L
• M = molecular weight of molecules
• where
◦ P is the osmotic pressure,
◦ n is the number of particles into which the substance dissociates, i.e. your sodium acetate dissociates into sodium and acetate, and therefore the n = 2
◦ R is the universal gas constant, which is 0.082 L atm mol-1 K-1
◦ T is the absolute temperature (Kº)
◦ V is the volume
What is one mole
• One mole of a substance contains 6 x 10^23 particles (Avogadros number)
Define osmole
• An osmole is the amount of substance which must be dissolved in order to produce an Avogadro’s number of particles (6.0221 × 10^23).
◦ For substances which do not dissociate, the molarity and the osmolarity will be the same, whereas for substances that are ionised the osmolarity will be the molarity multiplied by the number of dissociated parts, eg. for sodium chloride the osmolarity will be doubled.
Define osmolarity
• Osmolarity is the number of osmoles of solute per litre of solution.
◦ Osmolarity depends on the volume of the solution, and therefore on the temperature and pressure of the solvent
◦ Number of dissolved particles without regard for what particles they are
◦ Same as osmotic concentration = osmolality x mass density of water
What does osmolality depend on? And therefore what factors also affect this?
• Osmolarity is the number of osmoles of solute per litre of solution.
◦ Osmolarity depends on the volume of the solution, and therefore on the temperature and pressure of the solvent
◦ Number of dissolved particles without regard for what particles they are
◦ Same as osmotic concentration = osmolality x mass density of water
Osmolality is
Number of osmoses of solute per kilogram of solvent
Depends on mass which is independent of temperature and pressure
Which of osmolality and osmolarity is independent of temperature and pressure?
Osmolality
How is osmolality measured
Freezing point depression - colligative property and therefore dependent on solute concentration
How is molality different to osmolality?
Molality refers to a specific solute
Define tonicity
• Tonicity is the osmotic pressure between two compartments, and is related to the difference in the concentration of “effective” osmoles (particles capable of exerting an osmotic force) between them
◦ Effective osmoles are those substances which are unable to penetrate the membrane between compartments, and therefore they are effective in their contribution to the osmotic pressure gradient.
◦ Ineffective osmoles are those that area able to equlibrate between compartments, and that are therefore unable to contribute to the osmotic pressure gradient e.g. urea and glucose; however rapid shifts in these still produce a temporary change in tonicity
What is an effective osmole
• Tonicity is the osmotic pressure between two compartments, and is related to the difference in the concentration of “effective” osmoles (particles capable of exerting an osmotic force) between them
◦ Effective osmoles are those substances which are unable to penetrate the membrane between compartments, and therefore they are effective in their contribution to the osmotic pressure gradient.
◦ Ineffective osmoles are those that area able to equlibrate between compartments, and that are therefore unable to contribute to the osmotic pressure gradient e.g. urea and glucose; however rapid shifts in these still produce a temporary change in tonicity