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Gen Chem II > Solutions and Colloids (Textbook) > Flashcards

Solutions and Colloids (Textbook) Flashcards

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1
Q

Homogeneous mixture of two or more substances

A

Solution

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2
Q

One component of a solution is present at a significantly greater concentration, in which case it is called the ____.

A

Solvent

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3
Q

The components of the solution present in relatively lesser concentrations are called ____.

A

Solutes

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4
Q

Sugar is a ____ solid.

A

Covalent

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5
Q

When sugar (a covalent solid) is dissolved in water, its molecules become ____ distributed among the molecules of water.

A

Uniformly

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6
Q

The subscript “aq” signifies that the molecules are ____ and are therefore ____ dispersed throughout the aqueous solution (water is the ____).

A

Solutes; Individually; Solvent

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7
Q

Almost any gas, liquid, or solid can act as a ____.

A

Solvent

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8
Q

Defining trait of a solution: After a solution is mixed, it has the same ____ at all points throughout (its (previous answer) is ____).

A

Composition; Composition; Uniform

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9
Q

Defining trait of a solution: The ____ state of a solution - solid, liquid, gas - is typically the same as that of the ____.

A

Physical; Solvent

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10
Q

Defining trait of a solution: The components of a solution are dispersed on a ____ scale; they consist of a mixture of separated ____ particles (molecules, atoms, and/or ions) each closely surrounded by ____ species.

A

Molecular; Solute; Solvent

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11
Q

Defining trait of a solution: The ____ solute in a solution will not ____ out or ____ from the solvent.

A

Dissolved; Settle; Separate

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12
Q

Defining trait of a solution: The composition of a solution, or the ____ of its components, can be varied ____ (within limits determined by the ____ of the components).

A

Concentrations; Continuously; Solubility

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13
Q

____ is defined in terms of the molar amount of solute species.

A

Molarity (M)

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14
Q

M= ____/____

A

mol/solute

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15
Q

Because solution volumes vary with temperature, ____ concentrations will likewise vary.

A

Molar

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16
Q

When expressed as molarity, the concentration of a solution with identical numbers of solute and solvent species will be different at different temperatures, due to the ____/____ of the solution.

A

Contraction/Expansion

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17
Q

More appropriate for calculations involving many colligative properties are ____-based ____ units whose values are not dependent on ____.
Two such units are ____ and ____.

A

Mole; Concentration; Temperature;
Mole fraction; Molality

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18
Q

____ of a component is the ratio of its molar amount to the total number of moles of all solution components.

A

Mole fraction (X)

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19
Q

X(subA) = ____/____

A

mol A/total

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20
Q

The sum of mole fractions for all solution components (the ____ and all ____) is equal to ____.

A

Solvent; Solutes; One

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21
Q

____ is a concentration unit defined as the ratio of the numbers of moles of solute to the mass of the solvent in kilograms.

A

Molality

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22
Q

m = ____/____

A

mol/solute

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23
Q

When calculating molality, the unites are compused using only masses and molar amounts (they do not vary with ____) and, thus, are better suited for applications requiring ____-independent concentrations, including several ____ properties.

A

Temperature; Temperature; Colligative

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24
Q

The formation of a solution is an example of a ____ ____, a process that occurs under specified conditions without the requirement of energy from some ____ source.

A

Spontaneous process; external

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25
Q

Stirring a mixture sometimes speeds up the ____ process, but is not necessary, as a ____ solution will form eventually.

A

Dissolution; Homogeneous

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26
Q

Two criteria favor, but do not ____, the spontaneous formation of a solution:
1. A(n) ____ in the internal energy of the system (an ____ change).
2. A(n) ____ dispersal of matter in the system (which indicates ____ in the entropy of the system).

A

Guarantee
1. Decrease; Exothermic
2. Increased; Increase

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27
Q

In the process of dissolution, an ____ energy change often, but not always, occurs as heat is ____ or ____.

A

Internal; Absorbed; Evolved

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28
Q

A(n) ____ in matter dispersal always results when a solution forms from the uniform distribution of ____ molecules throughout a(n) ____.

A

Increase; Solute; Solvent

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29
Q

When the strengths of the intermolecular forces of attraction between solute and solvent species in a solution are no different than those present in the separated components, the solution is formed with no accompanying energy change. Such a solution is called an ____ ____.

A

Ideal solution

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30
Q

A mixture of ____ gases is an example of an ____ solution, since these gases experience no significant ____ attractions.

A

Ideal; Ideal; Intermolecular

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31
Q

____ ____ may also form when structurally similar liquids are mixed.

A

Ideal solutions

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32
Q

In relation to ideal solutions: Unlike a mixture of gases, the components of liquid-liquid solutions do experience ____ ____ ____.

A

Intermolecular attractive forces

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33
Q

In relation to ideal solutions: In liquid-liquid solutions, since the molecules of the two substances being mixed are structurally very similar, the ____ ____ ____ between like and unlike molecules are essentially the ____, and the dissolution process, therefore, ____ entail any appreciable ____ or ____ in energy.

A

Intermolecular attractive forces; Same; Does not; Increase; Decrease

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34
Q

____ ____ dispersal alone can provide the driving force required to cause ____ formation of a solution.

A

Increased matter (dispersal); Spontaneous

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35
Q

In some cases, the ____ ____ of intermolecular forces of attraction between solute and solvent species may prevent ____.

A

Relative magnitudes; Dissolution

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36
Q

Three types of intermolecular attractive forces are relevant to the dissolution process: ____-____, ____-____, and ____-____.

A

Solute-solute; Solvent-solvent; Solute-Solvent

37
Q

The formation of a solution may be viewed as a ____ process in which energy is:
1. Consumed to overcome ____-____ and ____-____ attractions (____ process) and…
2. Released when ____-____ attraction are established (an ____ process referred to as ____).
3. The overall energy of the ____ process is the ____ of these steps.
4. The relative magnitudes of the energy changes associated with these ____ processes determine whether the dissolution process overall will ____ or ____ energy.

A

Stepwise
1. Solute-solute; Solvent-solvent; Endothermic
2. Solute-solvent; Exothermic; Solvation
3. Dissolution; Sum
4. Stepwise; Absorb; Release

38
Q

In some cases, solutions do not form because the energy required to separate the solute and solvent species is so much greater than the energy released by ____.

A

Solvation

39
Q

Consider the example of an ionic compound dissolving in water. Formation of the solution requires the ____ forces between the cations and anions of the compound (____-____) be overcome ____ as attractive forces are established between these ions and water molecules (____-____).

A

Electrostatic; Solute-solute; Completely; Solute-solvent

40
Q

If the solutions electrostatic forces are significantly ____ than the ____ forces, the dissolution process is significantly ____ and the compound may not dissolve to an appreciable extent.

A

Greater; Solvation; Endothermic

41
Q

If the solvation forces are much stronger than the ____ forces, the dissolution is significantly ____ and the compound may be highly ____.

A

Electrostatic; Exothermic; Soluble
(A common example is sodium hydroxide)

42
Q

Spontaneous solution formation is favored, but not guaranteed, by ____ ____ processes.

A

Exothermic dissolution

43
Q

Many soluble compounds dissolve with the release of ____, but some dissolve ____.

A

Heat; Endothermically

44
Q

Endothermic dissolutions require a ____ ____ input to separate the solute species that is recovered when the solutes are ____, but they are ____ nonetheless due to the ____ in disorder that accompanies the formation of the solution.

A

Greater energy (input); Solvated; Spontaneous; Increase

45
Q

When some substances are dissolved in water, they undergo a chemical change that yields ____ in solution. These substances constitute a class of compounds called ____.

A

Ions; Electrolytes

46
Q

Substances that do not yield ions when dissolved are called ____.

A

Nonelectrolytes

47
Q

If the physical or chemical process that generates the ions is essentially 100% efficient (all of the dissolved compound yields ____), then the substance is known as a ____ ____.

A

Ions; Strong electrolyte

48
Q

If only a relatively small fraction of the dissolved substance undergoes the ____-producing process, it is called a ____ ____.

A

Ion; Weak electrolyte

49
Q

Substances may be identified as strong, weak, or nonelectrolytes by measuring the ____ ____ of an aqueous solution containing the substance.

A

Electrical conductance

50
Q

To conduct electricity, a substance must contain freely ____, ____ species.

A

Mobile, Charged

51
Q

In the case of conduction of electricity through metallic wires, the ____, ____ entities are ____.

A

Mobile, Charged; Electrons

52
Q

Solutions may also conduct electricity if they contain ____ ions, with conductivity increasing as ____ concentration increases.

A

Dissolved; Ion

53
Q

Applying a ____ to electrodes immersed in a solution permits assessment of the relative ____ by dissolved ions, either quantitatively, by measuring the ____ ____ flow, or qualitatively, by observing the brightness of a ____ ____ included in the ____.

A

Voltage; Concentration; Electric current; Light bulb; Circuit

54
Q

The ____ attraction between an ion and a molecule with a dipole is called a(n) ____-____ attraction. These attractions play an important role in the dissolution of ____ ____ in water.

A

Electrostatic; Ion-dipole; Ionic compounds

55
Q

When ionic compounds dissolve in water, the ions in the solid separate and disperse ____ throughout the solution because water molecules surround and ____ the ions, reducing the strong ____ forces between them. This process represents a physical change known as ____.

A

Uniformly; Solvate; Electrostatic; Dissociation

56
Q

Under most conditions, ionic compounds will dissociate ____ ____ when dissolved, and they are classified as ____ (options: weak/strong/non) electrolytes.

A

Nearly completely; Strong

57
Q

Even sparingly, soluble ____ compounds are strong electrolytes, since the small amount that does dissolve will dissociate completely.

A

Ionic

58
Q

In relation to ionic electrolytes: The ions transition from ____ positions in the undissolved compound to ____ ____, ____ ions in solution.

A

Fixed; Widely dispersed, Solvated

59
Q

Pure water is an extremely poor conductor of electricity because it is very ____ ____.

A

Slightly ionized

60
Q

In some cases, solutions prepared from covalent compounds conduct electricity because the ____ molecules react chemically with the ____ to produce ions.

A

Solute; Solvent

61
Q

Pure hydrogen chloride (HCl) is a gas consisting of covalent HCl molecules. This gas contains no ____. However, an aqueous solution of HCl is a very good ____, indicating that an appreciable concentration of ions exist within the solution.

A

Ions; Conductor

62
Q

HCl is a strong acid and, consequently, a ____ ____.

A

Strong electrolyte

63
Q

Weak acids and bases that only react partially generate relatively low ____ of ions when dissolved in water and are classified as ____ ____.

A

Concentrations; Weak electrolytes

64
Q

____ of a solute in a particular solvent is the maximum concentration that may be achieved under given conditions when the dissolution process is at ____.

A

Solubility; Equilibrium

65
Q

When a solute’s concentration is equal to its solubility, the solution is said to be ____ with that solute.

A

Saturated

66
Q

If the solute’s concentration is less than its solubility, the solution is said to be ____.

A

Unsaturated

67
Q

A solution that contains a relatively low concentration of solute is called ____.

A

Dilute

68
Q

A solution that contains a relatively high concentration of solute is called ____.

A

Concentrated

69
Q

____ solutions occur when a solute concentration exceeds its solubility. These are examples of ____ states.

A

Supersaturated; Nonequilibrium

70
Q

The solubility of a gas in a liquid is affected by the intermolecular attractive forces between ____ and ____ species.

A

Solute; Solvent

71
Q

When a gaseous solute dissolves in a liquid solvent, there is no ____-____ intermolecular attraction to overcome. Consequently, ____-____ interactions are the sole energetic factor affecting solubility.

A

Solute-solute; Solute-solvent

72
Q

Gas solubility typically ____ as temperature increases.

A

Decreases

73
Q

The solubility of a gaseous solute is also affected by the partial ____ of ____ in the gas to which the solution is exposed.

A

Pressure; Solute

74
Q

For many gaseous solutes, the relation between solubility and partial pressure is ____.

A

Proportional

75
Q

____: The quantity of an ideal gas that dissolves in a definite volume of liquid is directly proportional to the pressure of the gas.

A

Henry’s law

76
Q

Some liquids may be mixed in any proportions to yield solutions; in other words, they have ____ mutual solubility and are said to be ____.

A

Infinite; Miscible

77
Q

Ethanol, sulfuric acid, and ethylene glycol are examples of liquids that are completely ____ with water.

A

Miscible

78
Q

Miscible liquids are typically those with very similar ____.

A

Polarities

79
Q

For liquids that are polar or capable of hydrogen bonding: the ____-____ attractions (or ____ bonding) of the solute molecules with the solvent molecules are at least as strong as those between molecules in the ____ solute or in the ____ solvent.

A

Dipole-dipole; Hydrogen; Pure; Pure

80
Q

Nonpolar liquids are miscible with each other because there is no appreciable difference in the strengths of ____-____, ____-____ and ____-____ intermolecular attractions.

A

Solute-solute; Solvent-solvent; Solute-solvent

81
Q

The solubility of polar molecules in polar solvents and nonpolar molecules in nonpolar solvents is an illustration of the chemical axiom: ____ ____ ____.

A

Like dissolves like

82
Q

Two liquids that do not mix to an appreciable extent are called ____.

A

Immiscible

83
Q

_____ _____ are formed when immiscible liquids are poured in the same container.

A

Separate layers

84
Q

Many nonpolar liquids are ____ with water.

A

Immiscible

85
Q

Miscible liquids are of ____ mutual solubility, while liquids said to be immiscible are of ____ ____ (though ____ ____) mutual solubility.

A

Infinite; Very low; Not zero

86
Q

The temperature dependence of solubility can be exploited to prepare ____ solutions of certain compounds.

A

Supersaturated

87
Q

The solution (colligative) properties that depend only upon the total concentration of solute species, regardless of their identities, include: ____ ____ ____, ____ ____ ____, ____ ____ ____ and ____ ____.

A

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

88
Q

The colligative properties of a solution depend only on the ____, not on the ____, of solute species dissolved.

A

Number; Identity

89
Q
A

Gen Chem II (2 decks)

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