Chapter 13: Physical Properties of Solutions Flashcards

(36 cards)

1
Q

solution

A

a homogeneous mixture of two or more substances; consists of a solvent and one or more solutes.

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2
Q

unsaturated solution

A

one that contains less solute than the solvent has the capacity to dissolve at a specific temperature

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3
Q

saturated solution

A

one that contains the maximum amount of solute that will dissolve in a solvent at a specific temperature

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4
Q

Supersaturated solutions

A

contain more dissolved solute than is present in a saturated solution and are generally unstable

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5
Q

Solvation occurs when

A

solute molecules are separated from one another and surrounded by solvent molecules.

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6
Q

entropy

A

a measure of how dispersed or spread out its energy is.

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7
Q

There is a natural tendency for the energy of a system to

A

become dispersed (entropy increases).

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8
Q

Two substances with similar type and magnitude of intermolecular forces are likely to be _____ in each other

A

soluble

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9
Q

Two liquids are said to be ____ if they are completely soluble in each other in all proportions.

A

miscible

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10
Q

concentration

A

The amount of solute relative to the volume of a solution or to the amount of solvent in a solution

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11
Q

Molality

A

the number of moles of solute dissolved in 1 kg (1000 g) solvent

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12
Q

Pressure greatly influences

A

the solubility of a gas.

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13
Q

Henry’s law states that

A

the solubility of a gas in a liquid is proportional to the pressure of the gas over the solution.

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14
Q

Colligative properties

A

properties that depend on the number of solute particles in solution

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15
Q

The colligative properties are:

A

Vapor pressure lowering.
Boiling point elevation.
Freezing point depression.
Osmotic pressure.

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16
Q

Raoult’s law states that

A

the partial pressure of a solvent over a solution is given by the vapor pressure of the pure solvent times the mole fraction of the solvent in the solution.

17
Q

If both components of a solution are volatile:

A

the vapor pressure of the solution is the sum of the individual partial pressures

18
Q

ideal solution

A

obeys Raoult’s law.

19
Q

Solutions boil at a _____ temperature than the pure solvent.

20
Q

Solutions freeze at a _____ temperature than the pure solvent.

21
Q

Osmosis

A

the selective passage of solvent molecules through a porous membrane from a more dilute solution to a more concentrated one.

22
Q

Osmotic pressure

A

pressure required to stop osmosis

23
Q

Electrolytes undergo ______ when dissolved in water.

24
Q

van’t Hoff factor

A

accounts for electrolyte dissociation

25
The van’t Hoff factor (i) is ____ for all nonelectrolytes
1
26
For strong electrolytes i should be equal to _____
the number of ions
27
The van’t Hoff factor (i) is usually smaller than predicted due to
formation of ion pairs
28
ion pair
made up of one or more cations and one or more anions held together by electrostatic forces.
29
Percent dissociation
is the percentage of dissolved molecules (or formula units, in the case of an ionic compound) that separate into ions in a solution and this can be found using colligative properties
30
Percent dissociation of a strong electrolyte is more complete at ______ concentration.
lower
31
Percent ionization of weak electrolytes is also dependent on
concentration
32
colloid
a dispersion of particles of one substance throughout another substance. (Colloid particles are much larger than the normal solute molecules.)
33
colloid examples
``` Aerosols. Foams. Emulsions. Sols. Gels. ```
34
Colloids with water as the dispersing medium can be categorized as
hydrophilic (water loving) or hydrophobic (water fearing).
35
Hydrophobic colloids can be stabilized by the presence of
hydrophilic groups on their surface (think hyrdophilic head)
36
Emulsification
the process of stabilizing a colloid that would otherwise not stay dispersed