Ideal solution Flashcards
dependency physical properties of solution
more directly on concentration of solute
colligative properties of solution
vapour pressure, freezing and boiling point and osmotic pressure
ideality of solution
slightly different of ideal gas
as intermolecular interaction in liquids are strong therefore cannot be neglected
dependency of colligative
on ratio of solute to solvent molecules
interaction of molecules in ideal solution
has a force of attraction between molecules
all interact with identical magnitudes and distance dependencies - all attract and repel at same time
molecules cannot tell each other apart
properties of specific molecules are independent of composition
real solution
volume might be larger - if 2 solution repel
arrangement of molecules
completely random therefore enthalpy change on mixing components to make solution is 0
volume change
additive in ideal solution
closer to 0 the enthalpy of solution
more ‘ideal’ behaviour becomes
DH{mix}=0
no enthalpy change of mixing
making a mixture of liquid
breaking existing intermolecular forces and then make new ones
how intermolecular forces are broken
by heat
if intermolecular forces are the same
won’t be any heat either evolved or absorbed
therefore ideal mixture of 2 liquids will have 0 enthalpy change
when mixture isn’t ideal
if temperature increases or decreases
ideal solution
equation relating partial vapour pressure of individual components to composistion
partial vapour pressure, Px of component in solution
pressure of that component in gas phase that is in equilibrium with solution
vapour pressure equation
P{x} = N{x} * P{x}(0)
N{x}
mole fraction of x in solution
Px(0)
vapour pressure of pure liquid x
solution composed of compounds x, Q and P
mole fraction of x
N{x} = n{x}/(n{x}+n{Q}+n{P})
solution definition
made up of different components - types of molecules
vapour pressure
pressure exerted by vapour in vapour in equilibrium with its liquid/solid phase at given temp in closed system
liquid molecules at surface
escape in to gas phase
gas particles collide with walls of container
pressure above liquid - vapour pressure
Raoult’s law
for ideal solution - vapour pressure of a component in that solution = mole factor of that component x vapour pressure of component
Raoult’s law equation
P{x} = N{x} * P{x}(0)
chemical potential equation
μx{solution} = μx*{liquid} + RTlnNx
mole concentration
μx = μx* + RTln[x]
in very dilute solution
both solvent and solute can be treated as ideal
number of solute is low
solvent molecules spend most of its time interacting with other solvent molecules
affect of increasing concentration of solute
no affect until number of solute is high enough that solvent molecule spend significant time interacting with solute molecules
interaction of solute to solvent
solute molecules interact with solvent molecules only increase solute conc doesn’t change until significant soluble-solvent interaction