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824 > Colligative Properties > Flashcards

Colligative Properties Flashcards

1
Q

True Solution

A
  • One-phase, homoogeneous molecular dispersion

- No phase separation or boundary

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2
Q

Binary Solution

A

-Solution with 1 solute and 1 solvent

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3
Q

Solvent

A

First Substance

-For liquids - solvent is [higher]

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4
Q

Solute

A

Second Substance

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5
Q

Component/Constituents

A

-No distinction between solute and solvent

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6
Q

Nonelectrolytes

A
  • When dissolved they do NOT form ions
  • Will NOT conduct electrical currency
  • EX: sucrose, glycerin, urea
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7
Q

Electrolytes

A
  • Substances that dissociate into ions when dissolved
  • Strong = complete dissociation
  • Weak = partial dissociation
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8
Q

Additive Property

A
  • Contribution of each atom of the molecule add up

- EX: MW

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9
Q

Constitutive Property

A
  • Depending on arrangement of atoms in molecule

- EX: electrical properties, light refraction, solubility

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10
Q

Colligative Property

A

-Number of “particles” in solution

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11
Q

Examples of Colligative Properties

A
  • Vapor pressure lowering
  • Freezing point depression
  • Boiling point elevation
  • Osmotic pressure changes
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12
Q

Do electrolytes or nonelectrolytes contribute more to colligative properties?

A

Electrolytes

-Ionization of electrolytes produces more particles

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13
Q

Ideal Solutions

A
  • No changes in the properties of the two components when mixed together
  • No heat given off or absorbed
  • No shrinkage or expansion of volume
  • All constitutive properties are weighted averages of each component
  • Molecules of solute interact with solvent the same way

More likely to occur when mixing “like” substances

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14
Q

Real/Non-Ideal Solutions

A
  • Solute molecules interact to a greater or lesser extent with solvent molecules than other solute molecules
  • Dependent on interactions between solute and solvent as to if the solution is ideal/real
  • Recall vapor pressure of liquids is a reflection of intermolecular bonding
  • Greater bonding in liquid state = lower vapor pressure
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15
Q

Raoult’s Law

A

-Vapor pressure of a substance in solution os equal to vapor pressure of PURE compound multiplied by its mole fraction

Pa = Pa0 * Xa
Pb = Pb0 * Xb
Pt = Pa + Pb
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16
Q

Negative Deviations

A
  • Indicated attractive forces between A and B

- These are GREATER than those between A/A and B/B

17
Q

Positive Deviations

A
  • Indicates attractive fores between A/A and B/B

- These are GREATER than those between A and B

18
Q

Simple Binary Solutions

A
  • Nonelectrolytes
  • If the solute is nonvolatile, then the partial pressure of solvent IS the vapor pressure
  • Delta P = PaO * 0.018 * m
  • m = molality, PaO is vapor pressure of pure SOLVENT
19
Q

Actual Vapor Pressure =

A

-Difference of the vapor pressure of the pure solvent from delta P (vapor pressure lowering)

20
Q

Relative Vapor Pressure Lowering

A
  • Often referenced as a percentage

- Since compared to “whole” vapor pressure of the pure solvent

21
Q

Boiling Point

A
  • Temperature when the vapor pressure of a solution equals the external pressure
  • Nonvolative solute in a solvent will have a higher boiling point than pure solvent (lowered vapor pressure)
  • Therefore referred to as boiling point elevation
22
Q

Boiling Point Elevation

A
  • Delta Tb = kb * m
  • Kb = molal elevation constant (ebullioscopic constant), 0.51 for aqueous solutions
  • m = molality
  • Add to original boiling point for actual boiling point of solution
  • *Dependent on [solute]
23
Q

Freezing Point Depression

A
  • Delta Tf = kf * m
  • m = molality
  • Kf = cryoscopic constant, 1.86 for water
  • Actual freezing point is original minus the freezing point depression
24
Q

Osmotic Pressure

A
  • Osmosis - process of solvent diffusion across a semi-permeable membrane (OP driven)
  • No osmosis if OP is the same on either side
  • Solvent molecules move towards area of greater osmotic pressure
  • Equalizes as solvent dilutes the side with greater pressure by decreasing the solute’s concentration
25
Q

[Solute] + Colligative Properties

A
  • Decreases vapor pressure
  • Decreases freezing point
  • Increases boiling point
  • Increases osmotic pressure
26
Q

van’t Hoff Equation

A
  • Used to calculate osmotic pressure
  • (pi) = mRT
  • m = molality
  • R = gas constnat
  • T = temperature in Kelvins
27
Q

Nonelectrolyte Points

A
  • If the two solutions have the same vapor pressure,t hen they have the same osmotic pressure, boiling point, and freezing point too
  • All equations to measure pressures and changes in temperatures use molality
28
Q

Solute MW in Binary Solutions

A 
m = (1000 * w2)/(w1 * MW2)
w1 = weight of solvent
w2 = weight of solute
MW2 = molecular weight of solute

824 (15 decks)

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