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PL1002 > Solutions > Flashcards

Solutions Flashcards

1
Q

Components

A

minimum number of independent species necessary to define the composition of all phases in a system

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2
Q

Phase diagram

A

Plot of pressure vs temperature

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3
Q

Phase boundary

A

Continuous line representing values at which equilibrium exists between 2 phases

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4
Q

Triple point

A

Point at which 3 phases coexist at equilibrium

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5
Q

What is different about water phase diagram?

A

Solid/Liquid line leans towards the y-axis.

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6
Q

Why is the water phase diagram different?

A

The solid/liquid line leans towards the y-axis due to being less dense in the solid phase than liquid phase. This is due to H bonding and oxygen repelling other oxygens

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7
Q

Degrees of Freedom

A

Number of factors which can be varied independently without altering the number of phases

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8
Q

Gibbs Phase Rule in condensed systems

A

P+F = C+1

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9
Q

Gibbs Phase Rule

A

P+F = C+2

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10
Q

Colligative Properties

A

4 physical properties affected in the same way by solutes, regardless of solute identity

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11
Q

What do Colligative Properties depend on?

A

Properties of solvent, concentration of dissolved substance and number of particles of dissolved substance in the solution

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12
Q

How are the colligative properties related?

A

Thermodynamically

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13
Q

What are the 4 main Colligative Properties?

A

Vapour Pressure lowering, Freezing point depression, boiling point elevation and osmotic pressure

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14
Q

Osmosis

A

The tendency of solvent molecules to pass through a membrane from a more dilute to a more concentrated solution.

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15
Q

Osmotic pressure

A

If a solution is separated from its solvent by a membrane then the excess pressure which has to be applied to prevent the flow of the solvent is the osmotic pressure

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16
Q

Osmotic pressure equation

A

Π = mRT

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17
Q

Semi-permeable membrane

A

Chemical potential of a solvent in solution is less than its chemical potential in a pure solvent. Solvent passes spontaneously into the solution to equalise the chemical potential on either side of the membrane

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18
Q

Reverse Osmosis

A

A pressure greater than the osmotic pressure is applied to the solution and forces the solvent through the membrane

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19
Q

Hydrostatic pressure

A

Pressure exerted by a column of aqueous solution

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20
Q

Iso-osmotic

A

2 solutions have the same osmotic pressure

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21
Q

Isotonic

A

2 solutions have the same solute concentration

22
Q

If osmotic pressure is hypotonic, what happens to cells?

A

They swell

23
Q

If osmotic pressure is hypertonic, what happens to cells?

A

They shrink

24
Q

What is the osmotic pressure of blood?

A

291 m osmol dm-3

25
Q

Osmolality

A

The mass of solute which when dissolved in 1kg of water will exert an osmotic pressure equal to that exerted by 1 mol of an ideal and unionised substance dissolved in 1kg of water

26
Q

Osmol

A

A mole of a substance that is non-dissociable in a solution

27
Q

Freezing point depression of blood

A

ΔTf = 0.52°C

28
Q

Freezing point depression

A

Freezing point depression is the lowering of the freezing point of a solvent by adding a non-volatile solute

29
Q

Equation for freezing point depression

A

ΔTf = Kf x m

30
Q

Osmotic pressure equation using ΔTf

A

Π = ΔTf/Kf x RT

31
Q

What is W = 0.52-a / b used for?

A

When it is not possible to adjust the concentration of a drug to make it more isotonic with blood, an adjusting substance can be added.
W = weight of adjusting substance per 100cm3
a= ΔTf of drug solution
b = ΔTf produced by 1%w/v of adjusting substance

32
Q

Solubility of gas in a liquid

A

The concentration of the dissolved gas when it is at equilibrium with some of the pure gas above the solution

33
Q

Henry’s Law

A

The vapour pressure exerted by a gas dissolved in a solvent at constant temperature is proportional to the mole fraction of the gas

34
Q

Henry’s Law equation

A

pB = kH + xB

xB = mole fraction of the gas
pB = vapour pressure of the gas
kH = Henry’s Law constant

35
Q

What happens to gas solubility as temperature increases?

A

Gas solubility decreases due to the greater tendency of gas to expand

36
Q

Salting out

A

Liberation of gas from a solution by the addition of NaCl or sucrose. The added solute attracts water molecules, reducing the density of the aqueous environment adjacent to the gas molecules

37
Q

Degrees of Freedom in an immiscible solution

A

2 degrees of freedom

38
Q

Degrees of Freedom in a miscible solution

A

3 degrees of freedom

39
Q

Upper Critical Solution temperature

A

Highest temperature at which phase seperation occurs. This is due to thermal motion overcoming potential energy advantage of one type of molecule being close together

40
Q

Lower critical solution temperature

A

Temperature at which they mix in all proportions and above which they form 2 products. More miscible at low temperatures as a weak complex is formed

41
Q

Phase diagram point B

A

The eutectic point - the lowest temperature at which liquid solution can exist

42
Q

Raoult’s Law

A

Applies to solvent in solution

43
Q

Raoult’s Law equation

A

pA = p°A xA

p°A is the vapour pressure of pure solvent
pA is the vapour pressure of solvent in solution
xA is the mole fraction of the solvent

44
Q

Mole fraction in Henry’s and Raoult’s law

A

xB = 1 - xA

45
Q

What solutions obey Raoult’s law?

A

Ideal solutions

46
Q

How are non-ideal solutions formed?

A

Formed in the process of mixing of components and is accompanied by absorption of heat

47
Q

Theory of colloid stability

A

DLVO

48
Q

Total Vapour Pressure

A

pTotal = pA + pB

49
Q

Total potential energy using DLVO theory

A

vTotal = vA (attractive potential energy) + vR (Electrostatic repulsive energy)

50
Q

Low electrolyte concentration on DLVO plot

A

High primary maximum and no secondary minimum

51
Q

High electrolyte concentration on DLVO plot

A

No primary maximum or secondary minimum

PL1002 (6 decks)

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