Liquids and Solutions Flashcards

1
Q

What is an extensive/intensive variable?

A

Extensive - depends on size of system
Intensive - doesn’t depend on size

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2
Q

What are some examples of intensive and extensive variables?

A

Extensive: A, V, n (therefore dA, dV, dn)

Intensive: T, P, μ

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3
Q

What is the condition for chemical eqm?

A

μiα = μiβ

where μ is derivative of G wrt n

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4
Q

What is an ideal solution?

A

Equivalent to ideal gas
All interactions are the same - molecule 1 doesn’t care if surrounded by 1 or 2

Ideal entory of mixing

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5
Q

What is the ΔmH (of mixing) in an ideal solution?

A

ΔmH = 0

As all interactions are the same

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6
Q

What is the model used for ideal ΔmS?

A

Lattice model of a binary mixture

N1</sub molecules of type 1
N2 molcules of type 2
N lattice sites
Random mixing

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7
Q

What is Boltzmann’s eqn of entropy?

A

S = kb lnΩ

Ω = number of ways you can realise a given conformation
Ω = N!/[N1!N2!]

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8
Q

What is the ideal ΔmS?

A

ΔmS = -R[n1lnx1 + n2lnx2]

where ΔmS = Smix - Sunmix

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9
Q

What is x and sterling’s approx?

A

x is mole fraction

For small values of x:
lnx! = xlnx - x

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10
Q

What is the ΔmG of an ideal solution?

A

ΔmG = ΔmH - TΔmS = 0 + RT[n1lnx1 + n2lnx2]

Totally entropic

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11
Q

What is the μ of an ideal solution?

A

μ = (δG/δn)
G = Gunmix +RT[n1lnx1 + n2lnx2]

μ = μi + RTlnxi

Vapour pressure linearly related to molar pressure

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12
Q

What is Raoult’s law?

A

For an ideal solution on a boundary with ideal gas

Pi = xiPi*

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13
Q

How can you derive Raoult’s law?

A

μisolution = μivapor

Gas and solution is ideal
1) μi* + RTlnxi = μθ + RTln(Pi/Pθ)
2 (when @xi)) μi* = μθ + RTln(Pi/Pθ)

1-2 so:
RTlnxi = RTln(Pi/Pθ) - RTln(Pi*/Pθ)
gives:
xi = Pi/Pi*

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14
Q

How does a solid in an ideal solution change temeprature?

A

Solid is solvent

ΔT = T - T* = - X2 (RT*2fusH)

where T* is the freezing point of water, and X2 is mole fraction of ideal solution

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15
Q

What is a non-ideal solution?

A

Interactions not identical
Non-ideal entropy of mixing
Combination of both

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16
Q

What is a regular solution?

A

Same as ideal soltuion but interactions not identical
so Δm =! 0

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17
Q

How is a polymer solution different to an ideal one?

A

Non-ideal (so different) entropy of mixing

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18
Q

What is the potential of a non-ideal solution?

A

μi = μi* + RTlnki + RTlnfi

where the activity coefficient is fi

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19
Q

What is Henry’s law?

A

Pi = xiKH

Not derived
When component is the minority - so linear vapour pressure when low or high x

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20
Q

When is Raoult’s and Henry’s law followed?

A

Roult’s - for a substance when pure (xi~1)

Henry’s law - for a substance when in minority (xi~0)

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21
Q

What is ΔmS in a regular solution?

A

Same as ideal
ΔmS = -R[n1lnx1 + n2lnx2]

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22
Q

How do you derive the sum of interactions, w, in a regular solution?

A

ΔH = Hmix - Hunmix

Hunmix = (1/2)zN1w11 + (1/2)zNw2w22 = (z/2)(N1+N2)(w11x1 + w22x2)

Hmix = (z/2)(N1+N2)(w11x12 + w22x22 + 2w12x1x2

Then work out difference and eventually gives
ΔmH = z(n1+n2)x1x2 [w12 - (w11+w22)/2]

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23
Q

What is sum of interactions in a regular solution?

A

w = NAz[w12 - (w11+w22)/2]

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24
Q

What model is used for the enthalpy of mixing in a regular solution?

A

Lattice model of binary mix

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25
What are the assumptions in enthalpy of regular solution?
Random mixing Only nearest neighbour interactions, w Volume constant, and as H = U + PV, so ΔH = ΔU
26
What is the coordination number, z, in nearest neighbours?
Number of neighbours at a lattice site z=3, triangle z=4, square z=6, hexagonal
27
What is the ΔmH of a regular solution?
ΔmH = (n1 + n2) Wx1x2 where W = NAz[w12 - (w11+w22)/2]
28
What is ΔmG of a regular solution?
ΔmG = ΔmH - TΔmS ΔmG = (n1+n2)Wx1x2 + RT[n1lnx1 + n2lnx2]
29
What is the chemical potential of a regular solution?
μ1 = μ1`*` + RTlnx1 + wx22 can relate to f1 = exp[wx22/RT]
30
What is the ideal limit of activity coefficient?
f1 = exp[wx22/RT] ideal limit when w=0 so f1 = 1
31
What is nearest neighbour interactions in an ideal solution?
w11 = w12 = w21 = w22
32
How do you relate the vapour pressure of regular solutions?
P1 = x1P1`*` exp[wx22/RT) = x1P1`*` f1 Remember: for ideal gas and regular solution chemical eqm
33
How do you derive eqn for vapour pressure of regular solution?
Boundary of ideal gas and regular solution in eqm, μsolution = μvapour μ1`*` + RTlnx1 + Wx22 = μ1θ + RTln(P1/Pθ) when x1 = 1 and x2 = 0, μ1`*` = μ1θ + RTln(P1/Pθ) then 1st - 2nd equation RTlnx1 + Wx22 = RTln(P1/P1`*`) rearrange to P1 = x1P1`*` exp[Wx22/RT]
34
What is seen when two phases separate?
Starts with mix Finishes with two phases, neither are pure but just richer in one
35
What factors determine if phase separation occurs in a regular solution?
g = wx1x2 + RT[x1lnx1 + x2lnx2] when high w then encourages demixing, when low then mixing when high T encourages mixing, when low T is demixing Wants to min Gibbs free energy
36
How does W change if mixing/demixing occur?
W = NARz[w12 - (w11+w22)/2] if W +ve then w11 and w22 more -ve so more attractive than w12
37
What is Tc?
Critical temperature - T at beyond which there is a one-phase region
38
What is seen in a molar gibbs plot for mixing?
Double well needed for phase separation As T increases then one phase more likely
39
What is the chemical potential of two separate phases?
μ1 = μ1`*` - X2(dg/dX2) + g μ2 = μ2`*` - (1 - X2)(dg/dX2) + g
40
What is teh common tangent construction?
Minima gives coesting densities after separation (dg/dx2a) = [g(x2a) - g(x2b)]/(x2a-x2b)
41
What is the coexistence condition for two phases?
(dg/dx2)a = (dg/dx2)b = 0 This is required for 2 phases to be present
42
What is the condition (derivative) for the critical temp of two phases?
(dg/dx2)Tc = (d2g/dx22)Tc = 0 When this satisfied then at the Tc
43
What is a binodal or spinodal region of a gibbs graph?
Binodal - line on graph when (dg/dx2)a = (dg/dx2)b = 0 , gives 2 phases, dominates at lower T Spinodal - line on graph when (d2g/dx22)Tc = 0 , gives mix, dominates at higher T
44
What is the approach for understanding colloids?
Treat as huge (slow and see-able) atoms Same stat thermo and similar phase behaviour
45
What is the random flight model for a polymer?
Polymer is a random walk of N statistical segments of length l Stat segments can include multiple momomers
46
What is the Flory-Huggins theory?
Volume fraction formula for entropy of mixing of polymer solutions
47
What is the lattice model for a polymer solution?
N1 molecules of type 1 (solvent) N2 molecules of type 2 (polymer, with r stat segments per molecule N2 Number of lattice sites, N = N1 + rN2
48
What is volume fraction?
Equivalent to mole fractions but for space taken by solvent (1) or polymer (2) φ1 = N1/(N1 + rN2) φ2 = rN2/(N1 + rN2)
49
What is Ωunmix for a polymer solution?
Ωunmix = [rN2!/N2)(z/rN2)](r-1)N2
50
What is Ωmix for a polymer solution?
Expected without corrections: Ωmix = N!/(N1! rN2!) Must implement corrections: 1) random mix doesnt apply, so z/n for each segment other than first one (where z is coord) 2) Cannot switch chem segments unlike separate molecules, so multiply by rN2!/N2! Actual result Ωmix = N!/(N1! N2!) (z/N)(r-1)N2
51
What is ΔmS for a polymer solution?
Find by taking logs of Ω and using stirling's approx as for ideal ΔmS = kb[ln(N!/(N1! N2!) + (r-1)N2 ln(rN2/N)] = -R[n1lnφ1 + n2lnφ2]
52
What is Hunmix for a polymer solution?
Hunmix = (z/2)N1w11 + (z/2)rN2w22 = (1/2)(N1+rN2)[w11N1/N + w2rN2/N] Hunmix = z/2 (N1+rN2)(w11φ1 + w2φ2)
53
What is Hmix for a polymer solution?
Start with Hmix = (z/2)N1w11ϕ1 + (z/2)N1w12ϕ2 +(z/2)N1w11ϕ1 + (z/2)N1w12ϕ2 + (z/2)rN2w22ϕ2 + (z/2)rN2w21ϕ1 Simplifies down to: Hmix = (z/2)(N1 + rN2)[w11ϕ12 + w22ϕ22 + 2w12ϕ1ϕ2]
54
What is ΔmH for a polymer solution?
ΔmH = (n1 + rn2)wφ1φ2 = RT(n1 + rn2)χφ1φ2
55
What is the flory-huggins parameter?
χ = w/RT
56
What is ΔmG for a polymer solution?
ΔmG = RT[n1lnφ1 + n2lnφ2 + (n1+ rn2)χφ1φ2
57
What is the chemical potential of a polymer solution?
μ1 = μ1`*` + RT[lnφ1 + (1-1/r)φ2 + χφ22]
58
How can you find the vapour pressure & phase separation of polymer solutions?
Follow same process as with regular, just replace values
59
What is the source osmotic pressure of polymer solutions?
Semi-permeable membrane which polymer cannot pass through, but solvent can Osmotic pressure is difference in pressure on either side
60
What is the osmotic pressure of polymer eqn in terms of pressure difference?
Π = Pβ - Pα Where β contains the polymer
61
What drives osmosis and how is this shown in equation?
Π = Pβ - Pα = (μ1 - μ1`*`)/V1`*` then sub in: μ1= μ1`*` + RT[lnφ1 + (1-1/r)φ2 + χφ22 gives: Π = RT[ (1/M2)c2 + (1/2 - χ)/(ρ22V1`*`) c22 + ..]
62
How does osmotic pressure relate to virial expansion for gases?
Π = RT[ (1/M2)c2 + (1/2 - χ)/(ρ22V1`*`) c22 + ..] Virial expansion for gases: P = RT[(1/V) + B(T)(1/Vmean2) + ...]
63
What is the Van't Hoff law? (ideal osmotic pressure)
Π = RT[c2/ M2] This is from the first term of expansion
64
What is the experimental osmotic pressure?
Π = RT[ (1/M2)c2 + (1/2 - χ)/(ρ22V1`*`) c22 + ..] 2nd osmotic virial coefficient, A2 = (1/2 - χ)/(ρ22V1`*`) Plot c2 on x and Π/c2 on y y-intercept = RT/M2 gradient = RTA2
65
What are a good, theta, and poor solvents?
Good - max interactions with solvent, polymer spread out Theta - ideal osmotic pressure Poor - max interactions with self, polymer folded in
66
How does the Flory-Huggins parameter (χ) and A2 show solvent quality?
Good solvent : χ < 1/2 and A2 > 0, T = θ Theta: χ = 1/2 and A2 = 0, T =θ Poor solvent: χ > 1/2 and A2 < 0, T =θ
67
What is end-to-end distance of a polymer?
**R** = Σ **I** <**R**> = Σ <**I**> = 0 This is 0 due to the randomness of the polymer
68
What is mean square distance of a polymer?
Removes effect of -ve contribution to the mean <**R**2> = Nl2 = Ml2/m where M is mol weight and m is segment mol weight
69
What is the radius of gyration?
Rg is just useful experimental value < Rg2 > = < **R**2 > / 6 so Rg proportional to sqrt(M)
70
What is the composition of an electrolyte?
Av+Bv- -> v+ AZ+ + v- BZ-
71
What interactions are present in electrolytes?
Long-range electrostatic interactions Presence of ionic atmosphere of counter-ions
72
What is an ionic atmosphere?
-ve of ion surrounded by +ve ions and vice cersa
73
What is the chemical potential of one component of electrolyte solutions?
μ+ = μ+θ + RTlnc+ + RTlny+ ci is molarity, equivalent for mole fraction yi is activity coefficient equivalent
74
What is μ of electrolyte solutions?
μ = μθ + vRTlnc+- + vRTlny+-
75
How do you derive the potential of a charge in solution?
Potential of an isolated charge: ψ(r) = (1/r)(e/4πε0εr) in solution: ψ(r) = (exp-κr/r) (e/4πε0εr) then taylor expansion: ψ(r) = (1/r - κ) (e/4πε0εr) where κ = debyte length
76
What is κ, debye length?
κ-1 is range of ionic atmosphere κ-1 = Sqrt[ε0εrkBT/2e2n0] n0 = N+/-/V κ-1 α 1/Sqrt[c] where c is salt conc
77
What is the potential of an ionic atmosphere?
ψatm = -eκ/4πε0εr
78
How do you find the work required to bring in an ion to a electrolyte?
wel = ∫ψatm dq = ∫-eκ/4πε0εr dq where ψatm is potential of ionic atmosphere wel = -κe2/8πε0εr
79
What is the relation activity coefficient of an ion in electrolyte? | 1:1 electrolyte
RTlny = NAwel = -κe2/8πε0εrkBT
80
What is relation of activity coefficient and concentration of an electrolyte?
logy+- = - A Sqrt[c]
81
What is ionic strength (I) in debye-huckel law?
I = 1/2 Σ cizi2 where c is concentration and z is ionic charge
82
What is the debye-huckel limiting law?
logy+- = -z+z-A Sqrt[I] where I is an i
83
What is ionic strength of a 1:1 electrolyte with 1+ charges (AgCl)?
I = 1/2 Σ cizi2 I = (1/2) (c) (1`*`12 + 1`*`12) = c
84
How does conc of electrolyte relate to K of solubility?
log c = (1/2)logKs + A Sqrt[I] Sol increases if inert electrolyte conc increases
85
How does increasing salt change solubility?
Adding more inert salt decreases work to bring in more ions, so more soluble As decreases debye length
86
What is surface tension?
Force per unit length which resists an external force Minmises surface area
87
What is the notation for surface tension and interface?
γ = surface tension σ = interface
88
What is required to increase surface area?
Work against surface tension which wants to min surface area F = 2γl, where l is length and 2 as bottom and top surface of film dw = Fdx = 2γldx = γdσ
89
What effects dominate at different size of systems?
Bulk dominates for large systems (length3) Surface dominates for smaller systems (length2)
90
What is the origin of surface tension?
Molecules attracted to surrounded in bulk Costs energy to move a molecule from bulk to surface as loses attraction so it costs work to create a surface This is surface tension
91
What happens when you have a small and large bubble connected?
Small bubble goes into large This is because pressure in smaller bubble is larger
92
What is Laplace's law?
ΔP = 2γ/R where R is radius of droplet when isothermal enlargement
93
What is required for soap bubbles?
Pinside > Poutside so inside can act against force preventing it from forming
94
How do you derive Laplace's law?
outside force (expansion work then expansion work against outside P0) = inside force (work to increase bubble size) (P0+ΔP)dV - P0dV = γdσ σ = 4πR2 dσ = 8πRdR ΔP (4πR2dr) = γ8πRdR ΔP = 2γ/R
95
What is the Kelvin equation relating to?
Vapour pressure of a liquid droplet
96
What is Kelvin's equation?
Pr = P0 exp[2γvI/rRT] where Pr is vap pressure of a liquid droplet with radius r, with respect to P0
97
What is the vapour pressure of a small droplet?
Small droplet has large lapace pressure so large (2γ/r) Pr >> P0
98
What is the vapour pressure of a large droplet?
Large droplet has small lapace pressure so small (2γ/r) Pr ~ P0
99
How do you derive Kelvin's equation?
Eqm between liquid droplet and gas 1) μliq(P0)) = μgas (P0) 2) μliq(Pr + 2γ/r) = μgas(Pr) then do 2-1 and then integrate use molar volume liquid (vl) = molar volume gas (vg) = RT/P Then RTln(Pr/P0) >> vl(Pr-P0) so approx to give (2γvl)/r = RTln(Pr/P0) rearrange to give Pr = P0 exp[2γvl/rRT)
100
What is the critical droplet size?
Smallest droplet size possible in a pressure P r`*` = 2γvl/RTln(P/P0)
101
How does vapour pressure realte to nucleation?
When smaller vap pressure (Pr) than required due to bigger size of a droplet then is more likely to nucleate
102
What is the relation of gibbs adsorption equation?
Relation between adsorption and surface tension
103
What is a concentration profile?
104
What is the Gibbs dividing surface?
Approx to conc profile Gibbs dividing surface has no colume No excess or depletion of solvent molecules
105
What is the volume of gibbs dividing surface?
Dividing surface volume, Vσ = 0 Vtotal = Vα + Vβ
106
How does gibbs dividing surface change the excess/depletion of solvent?
No excess/depletion of solcent molecules (no molecules in interface) n1σ n1,total = n1α + n1β
107
What is the surface-excess amount?
niσ = ni,total - (n1α + n1β) XS of this amount of this component actually present in system over that present in a reference system
108
What is the amount of phase α & β in a conc profile?
n1α = Vαciα n1β = Vβciβ These come from integral beneath conc profile
109
How is the Gibbs dividing surface nσ=0 ?
Over and underestimates the curve by the same amount so interface is 0
110
What are the different types of adsoprtion?
Positive - surfactants wants to be at interface more than bulk Negative - surfactant does not want to be at the surface
111
What are the different types of adsoprtion?
Positive - surfactants wants to be at interface more than bulk Negative - surfactant does not want to be at the surface
112
What is the surface-excess conc, Γ?
Γi1 = niσ/σ this is for solvent - component 1
113
What is the surface xs conc of positive and negative adsorption?
114
What is dA of a surface?
dAσ = -SσdT + Σμidniσ + γdσ
115
What is dγ, the surface analogue of Gibbs-Duhem?
dγ = -(Sσ/σ)dT - Σ (niσ/σ) dμ Where the sum is from i to c SσdT + Σμidniσ + γdσ
116
What is the gibbs adsorption equation?
dγ = - Σ Γi1i
117
What is the Gibbs adsorption equation for ideal binary solutions?
Sub in μ2 = μ2θ + RTlnc2 Into following equation: dγ = - Σ Γi1i Gives dγ = - RTΓ21 dlnc2 Surface tension therefore a function of conc c2