Ideal solution Flashcards

1
Q

dependency physical properties of solution

A

more directly on concentration of solute

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2
Q

colligative properties of solution

A

vapour pressure, freezing and boiling point and osmotic pressure

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3
Q

ideality of solution

A

slightly different of ideal gas

as intermolecular interaction in liquids are strong therefore cannot be neglected

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4
Q

dependency of colligative

A

on ratio of solute to solvent molecules

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5
Q

interaction of molecules in ideal solution

A

has a force of attraction between molecules

all interact with identical magnitudes and distance dependencies - all attract and repel at same time

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6
Q

molecules cannot tell each other apart

A

properties of specific molecules are independent of composition

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7
Q

real solution

A

volume might be larger - if 2 solution repel

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8
Q

arrangement of molecules

A

completely random therefore enthalpy change on mixing components to make solution is 0

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9
Q

volume change

A

additive in ideal solution

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10
Q

closer to 0 the enthalpy of solution

A

more ‘ideal’ behaviour becomes

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11
Q

DH{mix}=0

A

no enthalpy change of mixing

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12
Q

making a mixture of liquid

A

breaking existing intermolecular forces and then make new ones

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13
Q

how intermolecular forces are broken

A

by heat

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14
Q

if intermolecular forces are the same

A

won’t be any heat either evolved or absorbed

therefore ideal mixture of 2 liquids will have 0 enthalpy change

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15
Q

when mixture isn’t ideal

A

if temperature increases or decreases

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16
Q

ideal solution

A

equation relating partial vapour pressure of individual components to composistion

17
Q

partial vapour pressure, Px of component in solution

A

pressure of that component in gas phase that is in equilibrium with solution

18
Q

vapour pressure equation

A

P{x} = N{x} * P{x}(0)

19
Q

N{x}

A

mole fraction of x in solution

20
Q

Px(0)

A

vapour pressure of pure liquid x

21
Q

solution composed of compounds x, Q and P

mole fraction of x

A

N{x} = n{x}/(n{x}+n{Q}+n{P})

22
Q

solution definition

A

made up of different components - types of molecules

23
Q

vapour pressure

A

pressure exerted by vapour in vapour in equilibrium with its liquid/solid phase at given temp in closed system

24
Q

liquid molecules at surface

A

escape in to gas phase

25
Q

gas particles collide with walls of container

A

pressure above liquid - vapour pressure

26
Q

Raoult’s law

A

for ideal solution - vapour pressure of a component in that solution = mole factor of that component x vapour pressure of component

27
Q

Raoult’s law equation

A

P{x} = N{x} * P{x}(0)

28
Q

chemical potential equation

A

μx{solution} = μx*{liquid} + RTlnNx

29
Q

mole concentration

A

μx = μx* + RTln[x]

30
Q

in very dilute solution

A

both solvent and solute can be treated as ideal

31
Q

number of solute is low

A

solvent molecules spend most of its time interacting with other solvent molecules

32
Q

affect of increasing concentration of solute

A

no affect until number of solute is high enough that solvent molecule spend significant time interacting with solute molecules

33
Q

interaction of solute to solvent

A

solute molecules interact with solvent molecules only increase solute conc doesn’t change until significant soluble-solvent interaction