Non-Ideal solution Flashcards

1
Q

non-ideal solution

A

molecules don’t interact identically therefore behaviour of one molecule depend on composition of solution

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2
Q

arrangement of molecules

A

non-random - strong attraction = closer

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3
Q

non-ideality

A

frequently observed IRL and make necessary to extend thermodynamics analysis

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4
Q

equation for chemical potential - calculate concentration

A

μx = μx* + RTln[ax]

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5
Q

concentration/activity, ax

A

calculated concentration

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6
Q

activity coefficient - Yx equation

A

Yx = ax / [x]

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7
Q

[x]

A

actual concentration

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8
Q

ax

A

effective concentration

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9
Q

ax = [x]

A

ideal solution

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10
Q

how much Yx deviates from 1

A

how different solution is from ideal

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11
Q

effective equation - μx

A

μx = μx* + RTlnYx[x]

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12
Q

Yx converting [x] into ax

A

has physical significance - used to measure amount of solution deviated from ideal

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13
Q

ax in a graph

A

concentrated predicted by ideal model to have same μ as actual

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14
Q

if Y = 1

A

ideal solution

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15
Q

Y < 1

A

x is more stable than predicted model

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16
Q

Y > 1

A

x is less stable than predicted model

17
Q

non-ideal +ve deviation from Raoult’s law

A

DH{mix} > 0 - endothermic - heat absorbed upon mixing

Total V > sum of V of components

18
Q

non-ideal -ve deviation from Raoult’s law

A

DH{mix} < 0 - exothermic - heat evolved upon mixing

Total V < sum of V of component

19
Q

ionic solution

A

requires knowledge of deviation for ideality

20
Q

ionic solution example - NaCl in water

A

O2 - more electronegative than H therefore strong attraction between solvent-solvent molecule
Na+ and Cl- disrupt water bonds by hydration shell formed
has electrostatic interaction

21
Q

dilute ionic solution

A

don’t cause non-ideal behaviour at low concentration

has affect on enthalpy and entropy when ions dissolve in water

22
Q

enthalpy

A

ion-water electrostatic interaction is more than compensated for loss of water-water H bonds
DH = -ve

23
Q

entropy

A

decreases as ions added to water - less disorder

water around ion - in particular arrangement

24
Q

more concentrated ionic solution

A

significance in electrostatic interaction - charges repel and attract

25
Q

DH - change in enthalpy

A

transferring ions from gas phase to solution

26
Q

smaller ions in solution

A

large DH and D entropy - strong interaction with water

27
Q

Debye-Huckel theory equation

calculating solute-solute electrostatic interaction in solution

A

log{10}Yx = -Az{x}(square root I)

28
Q

finding ionic strength equation

A

I = 1/2 sum of c{x}Z{x}(2)