Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chem > Ch 12 Section 2 > Flashcards

Ch 12 Section 2 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

molecules or ions of the solute are

A

attracted by the solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

because the dissolution process occurs at the surface of the solute, it can be speeded up if the surface area of the solute is

A

increased

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

in general, the more finely divided a substance is, the greater the surface area per unit mass and the more

A

quickly it dissolves

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

very close to the surface of a solute, the concentration of dissolved solute is

A

high

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

stirring or shaking helps to disperse the solute particles and bring fresh solvent into

A

contract with the solute surface

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

the effect of stirring results in increased contact between the

A

solvent and the solute surface

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

as the temperature of the solvent increases, solvent molecules move faster, and their

A

average kinetic energy increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

at higher temperatures, collisions between the solvent molecules and the solute are more frequent and are of higher energy than at

A

lower temperatures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

this helps to separate solute molecules from one another and to disperse them among the

A

solvent molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

for every combination of solvent with a solid solute at a given temperature, there is a limit to the amount of solute that can be

A

dissolved

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

the point at which this limit is reached for any solute solvent combination is difficult to predict precisely and dpends on the nature of the

A

solute, nature of the solvent, as well as the temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

as more solid dissolves and the concentration of dissolved molecules increases, collisions become more

A

frequent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

eventually, molecules are returning to crystal at the same rate at which they are going into solution, and a dynamic equilibriuim is established between

A

dissolution and crysstallization

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

solution equilibrium is the physical state in which the opposing processes of dissolution and crystallization of a solute occur at

A

equal rates

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

a solution that contains the maximum amount of dissolved solute is described as a

A

saturated solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

a solution that contains less solute than a saturated solution under the existing conditions is an

A

unsaturated solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

when a saturated solution of a solute whose solubility increases with temperature is cooled, the excess solute usually comes out of solution, leaving the solution satureated at the

A

lower tempearture

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

sometimes, if the solution is left to cool undistrubted, the excess solute does not separate and a

A

supersaturated solution is produced

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

a supersaturated solution is a solution that contains more dissolved solute than a saturated solution contains under the

A

same conditions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

a supersaturated solution may remain unchanged for a long time it if is not disturbed, but once crystals begin to form, the process continues until equilibrium is

A

reestablished at the lower temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

the solubility of a substance is the amount of that substance required to form a saturated solution with a specific amount of … at a specified …

A

solvent; temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

the temperature must be specified because solubility varies with

A

temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

for gases, pressure must also be

A

specified

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

the rate at which a solid dissolves is unrelated to its solubility at that

A

temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

the maximum amount of a given solute that dissolves and reaches equilibrium is always the same under the

A

same conditions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

“like dissolves like” is a useful rule for predicting whether one substance will

A

dissolve in another

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

what makes substances similar depends on the type of bonding, the polarity or nonpolarity of molecules, and the intermolecular forces between the

A

solute and solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

the polarity of water molecules plays an important role in the formation of solutions of

A

ionic compounds in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

the slightly charged parts of water molecules attract the ions in the ionic compound and surround them to keep them separated from the other

A

ions in the solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

this solution process with water as the solvent is referred to as

A

hydration

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

as ydrated ions diffuse into the solution, other ions are exposed and are drawn away from the

A

crystal surface by the solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

the entire crystal gradually dissolves and hydrated ions become unifromly

A

distributed in the solution

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

when crystallized from aqueous solutions, some ionic substances form crystals that incorporate water

A

molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

these crystalline compounds, hydrates, retain specific ratios of water molecules and are represented by formulas such as

A

CuSO4 . 5H2o

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

heating the crystals of hydrate can drive off the wter of hydration and leave the

A

anhydrous salt

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

when a crystalline hydrate dissolves in water, the water of hydration returns to

A

the solvent

37
Q

the behavior of a solution made from a hydrate is no different from the behavior of one made from the

A

anhydrous form

38
Q

dissolving either form results in a system containing

A

hydrated ions and water

39
Q

ionic compounds are generally not soluble in

A

nonpolar solvents

40
Q

the nonpolar solvent molecules do not attract the ions of the crystal strongly enought to overcome the forces holding the

A

crystal together

41
Q

liquids that are not soluble in each other are

A

immiscible

42
Q

nonpolar substances are generally quite soluble in

A

nonpolar liquids

43
Q

the only attractions between the nonpolar molecules are

A

london forces

44
Q

the intermolecular forces existing in the solution are therefore very similar to those in

A

pure substances

45
Q

liquids that dissolve freely in one another in any proportion are said to be

A

miscible

46
Q

changes in pressure have very little effect on the solubilities of

A

liquids or solids in liquid solvents

47
Q

increases in pressure increas gas

A

solubilities in liquid

48
Q

when a gas is in contact with ther surface of a liquid, gas molecules can

A

enter the liquid

49
Q

as the amountof dissolved gas increases some molecules begin to escape and reenter the

A

gas phase

50
Q

an equilibrium is eventually established between the rates at which gas molecules enter and leave the

A

liquid phase

51
Q

as long as this equilibrium is undistrubed, the solutibility of the gas in the liquid is unchanged at a given

A

pressure

52
Q

gas + solvent ⇌

A

solution

53
Q

increasing the pressure of the solute gas above the solution puts stress on the

A

equilibrium

54
Q

molecules collide with the liquid surface more

A

often

55
Q

the increase in pressure is partially offset by an increase in the rate of gas molecules entering the

A

solution

56
Q

in turn the increase in the amount of dissolved gaas causes an increase in the rate at which molecules escape from the liquid surface and become

A

vapor

57
Q

eventually equilibrium is restored at a

A

higher gas solubility

58
Q

an increase in gas pressure casues the equilibirium to shift so that more molecules are in the

A

liquid phase

59
Q

the solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid:

A

henry’s law

60
Q

henry’s law applies to gas liquid solutions at

A

constant temperature

61
Q

when a mixture of ideal gases is confined in a constant volume at a constant temperature, each gas exerts the same pressure it would exert if it occupied the space

A

alone

62
Q

assuming that the gases do not react in any way, each gas dissolves to the extent it would dissolve if no other gases were

A

present

63
Q

the rapid escape of a gas from a liquid in which it is dissolved is known as

A

effervescence

64
Q

increasing temperature usually decreases

A

gas solubility

65
Q

as the temperature increases, the average kinetic energy of the molecules in solution

A

increases

66
Q

a greater number of solute molecules are able to escape from the attraction of solvent molecules and return to

A

the gas phase

67
Q

at higher temperatures, equilibrium is reached with fewer gas molecules in solution, and gases are generally less

A

soluble

68
Q

the effect of temperature on solubility of solids in liquids is more difficult to

A

predict

69
Q

often, increasing temp increases solubility of

A

solids

70
Q

however, an equibalent temp increase can result in a large increase in solubility for some solvents and onlyt a

A

slight change for others

71
Q

in some cases, solubility of a solid decreases with an

A

increase in temperature

72
Q

the formation of a solution is accompanied by an

A

energy change

73
Q

the formation of a solid liquid solution can apparently either absorb energy or

A

release enrgy as heat

74
Q

during the formation of a solution solvent and solute particles experience changes in the forces attracting them to other

A

particles

75
Q

befor3e dissolving begins solvent molecules are held together by

A

intermolecular forces (solvent solvent attaction_

76
Q

in the solute molecules are held together by

A

intermoelcular forces (solute solute attraction)(

77
Q

energy is requoired to separate solute molecules and solvent moecules from their

A

neightbors

78
Q

a solute particle that is surrounded by solvent molecules is said to be

A

solvated

79
Q

the net amount of energy absorved as heat by the solution when a specific amount of solute dissolves in a solvent is the

A

enthalpy of solution

80
Q

thyou know tghat heating decreases the solubility of a gas, so dissolution of gases is

A

exothermic

81
Q

in the gaseous state, molecules are so far apart that there are virtually no intermolecular forces of

A

attraction between them

82
Q

therefore the solute solute interaction has little effect on the

A

enthalpy of a solution of a gas

83
Q

energy is relreased when a gas dissolves in a liquid because attraction between solute gas and solvent molecules outweighs the energy needed to separatge

A

solevent molecules

84
Q

Enthalpy of solution is negative when energy is

A

Released

85
Q

Enthalpy of solution is positive when energy is

A

Absorbed

86
Q

Energy is absorbed when solute particles becoming

A

Separated from solid

87
Q

Energy is absorbed when solvent particles being moved apart to allow

A

Solute particles to enter liquid

88
Q

Energy being released when solvent particles being attracted to and

A

Solvating solute particles

Chem (54 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions