Solutions and Colloids (Textbook)

Question 1

Homogeneous mixture of two or more substances

Answer 1

Solution

Question 2

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

Answer 2

Solvent

Question 3

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

Answer 3

Solutes

Question 4

Sugar is a ____ solid.

Answer 4

Covalent

Question 5

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

Answer 5

Uniformly

Question 6

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

Answer 6

Solutes; Individually; Solvent

Question 7

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

Answer 7

Solvent

Question 8

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

Answer 8

Composition; Composition; Uniform

Question 9

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

Answer 9

Physical; Solvent

Question 10

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.

Answer 10

Molecular; Solute; Solvent

Question 11

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

Answer 11

Dissolved; Settle; Separate

Question 12

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).

Answer 12

Concentrations; Continuously; Solubility

Question 13

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

Answer 13

Molarity (M)

Question 14

M= ____/____

Answer 14

mol/solute

Question 15

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

Answer 15

Molar

Question 16

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.

Answer 16

Contraction/Expansion

Question 17

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

Answer 17

Mole; Concentration; Temperature;
Mole fraction; Molality

Question 18

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

Answer 18

Mole fraction (X)

Question 19

X(subA) = ____/____

Answer 19

mol A/total

Question 20

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

Answer 20

Solvent; Solutes; One

Question 21

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

Answer 21

Molality

Question 22

m = ____/____

Answer 22

mol/solute

Question 23

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.

Answer 23

Temperature; Temperature; Colligative

Question 24

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.

Answer 24

Spontaneous process; external

Question 25

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

Answer 25

Dissolution; Homogeneous

Question 26

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).

Answer 26

Guarantee 1. Decrease; Exothermic 2. Increased; Increase

Question 27

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

Answer 27

Internal; Absorbed; Evolved

Question 28

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

Answer 28

Increase; Solute; Solvent

Question 29

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 ____ ____.

Answer 29

Ideal solution

Question 30

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

Answer 30

Ideal; Ideal; Intermolecular

Question 31

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

Answer 31

Ideal solutions

Question 32

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

Answer 32

Intermolecular attractive forces

Question 33

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.

Answer 33

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

Question 34

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

Answer 34

Increased matter (dispersal); Spontaneous

Question 35

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

Answer 35

Relative magnitudes; Dissolution

Question 36

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

Answer 36

Solute-solute; Solvent-solvent; Solute-Solvent

Question 37

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.

Answer 37

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

Question 38

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 ____.

Answer 38

Solvation

Question 39

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 (____-____).

Answer 39

Electrostatic; Solute-solute; Completely; Solute-solvent

Question 40

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.

Answer 40

Greater; Solvation; Endothermic

Question 41

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

Answer 41

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

Question 42

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

Answer 42

Exothermic dissolution

Question 43

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

Answer 43

Heat; Endothermically

Question 44

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.

Answer 44

Greater energy (input); Solvated; Spontaneous; Increase

Question 45

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

Answer 45

Ions; Electrolytes

Question 46

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

Answer 46

Nonelectrolytes

Question 47

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 ____ ____.

Answer 47

Ions; Strong electrolyte

Question 48

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

Answer 48

Ion; Weak electrolyte

Question 49

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

Answer 49

Electrical conductance

Question 50

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

Answer 50

Mobile, Charged

Question 51

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

Answer 51

Mobile, Charged; Electrons

Question 52

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

Answer 52

Dissolved; Ion

Question 53

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 ____.

Answer 53

Voltage; Concentration; Electric current; Light bulb; Circuit

Question 54

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.

Answer 54

Electrostatic; Ion-dipole; Ionic compounds

Question 55

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 ____.

Answer 55

Uniformly; Solvate; Electrostatic; Dissociation

Question 56

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

Answer 56

Nearly completely; Strong

Question 57

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

Answer 57

Ionic

Question 58

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

Answer 58

Fixed; Widely dispersed, Solvated

Question 59

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

Answer 59

Slightly ionized

Question 60

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

Answer 60

Solute; Solvent

Question 61

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.

Answer 61

Ions; Conductor

Question 62

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

Answer 62

Strong electrolyte

Question 63

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

Answer 63

Concentrations; Weak electrolytes

Question 64

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

Answer 64

Solubility; Equilibrium

Question 65

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

Answer 65

Saturated

Question 66

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

Answer 66

Unsaturated

Question 67

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

Answer 67

Dilute

Question 68

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

Answer 68

Concentrated

Question 69

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

Answer 69

Supersaturated; Nonequilibrium

Question 70

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

Answer 70

Solute; Solvent

Question 71

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.

Answer 71

Solute-solute; Solute-solvent

Question 72

Gas solubility typically ____ as temperature increases.

Answer 72

Decreases

Question 73

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

Answer 73

Pressure; Solute

Question 74

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

Answer 74

Proportional

Question 75

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

Answer 75

Henry's law

Question 76

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

Answer 76

Infinite; Miscible

Question 77

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

Answer 77

Miscible

Question 78

Miscible liquids are typically those with very similar ____.

Answer 78

Polarities

Question 79

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.

Answer 79

Dipole-dipole; Hydrogen; Pure; Pure

Question 80

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

Answer 80

Solute-solute; Solvent-solvent; Solute-solvent

Question 81

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

Answer 81

Like dissolves like

Question 82

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

Answer 82

Immiscible

Question 83

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

Answer 83

Separate layers

Question 84

Many nonpolar liquids are ____ with water.

Answer 84

Immiscible

Question 85

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

Answer 85

Infinite; Very low; Not zero

Question 86

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

Answer 86

Supersaturated

Question 87

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

Answer 87

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

Question 88

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

Answer 88

Number; Identity