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chemistry 1102 > chapter 10: Properties of solutions > Flashcards

chapter 10: Properties of solutions Flashcards

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1
Q

what is homogenous mixtures

A

2 or more pure substances; uniform throughout

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2
Q

what is the solvent

A

present in greatest abundance

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3
Q

what is solute

A

all the other substances

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4
Q

what does aq mean

A

means water is the solvent

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5
Q

solutions could be…

A

gases, liquids, or solids

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6
Q

what is an aqueous solution

A

water is the solvent, and solid, liquid, gas is the solute

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7
Q

solutions can contain the same compounds but have a difference of what?

A

properties

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8
Q

what is concentration

A

amount of solute dissolved in the solvent bc of the proportions

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9
Q

what is Molarity (M)

A

way to measure the concentration of a solution

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10
Q

what is the formula for molarity

A

moles of solute/ volume of solution in liters

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11
Q

what is the mass % formula

A

mass of component of solution/ total mass of solution

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12
Q

the mass % is the…

A

the simplest expression of the concentration

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13
Q

what is the formula for parts per million

A

mass of component solution / total mass of solution x 10^6

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14
Q

what is the mole fraction formula

A

x = moles of component / total moles of all components

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15
Q

what is Molality

A

the concentration expression that is similar to molarity

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16
Q

what is the symbol for Molality

A

m

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17
Q

what is the formula for molality

A

moles of solute/ kg of solvent

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18
Q

mass doesn’t change with what?

A

temp

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19
Q

does molarity depend on temp

A

no

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20
Q

like dissolves what…

A

like

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21
Q

what is miscible

A

pairs of liquids that dissolve in all proportions

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22
Q

what is immiscible

A

always insoluble

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23
Q

what is slightly miscible

A

soluble in some proportions

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24
Q

where do intermolecular forces operate

A

between the solute and solvent molecules

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25
Q

why do IMFs between solute and solvent particles need to be strong

A

to be competitive

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26
Q

what can you use to calculate the molarity

A

density

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27
Q

what does molality depend on

A

volume

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28
Q

what does 1 cm^3 equal

A

1 Liter

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29
Q

what is the muliplicaton factor for parts per billion

A

10^9

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30
Q

what are the types of IMFs

A

dispersion
dipole dipole
hydrogen bond
ion dipole

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31
Q

what is london dispersion

A

weakest intermolecular force
non polar

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32
Q

what is dipole dipole force

A

forces bwteen positive end of one polar molecule and the negative end of another polar molecule

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33
Q

what is a hydrogen bond

A

weak bond between a hydrogen atom located between a pair of other atoms that have an affinity for electrons
multiple hydogen bonds makes it a strong force

34
Q

what is ion dipole

A

attractive force that results from an ion and a molecule that has a dipole
example: Na + ion and water

35
Q

what does hydrogen need to bond with to make it a hydrogen bond

A

FON

36
Q

what is an endothermic process

A

total energy to break the attractive forces is higher than the energy released
“takes to break”

37
Q

what is the oil and water example

A

oil and water doesn’t mix bc water has strong hydrogen bonds and forces and it has to be overcome to disperse the water

38
Q

what is an exothermic process

A

the total energy for breaking the attractions is less than the energy is released
“frees to form”

39
Q

what factors affect solubility

A
  1. ) ImFs among the solute and solvent molecules
  2. ) natural tendency for substances to mix
40
Q

strong IMFs =

A

strong attractions and greater solubility

41
Q

what is entropy

A

the amount of randomness in a system/ amount of disorder

42
Q

entropy lowers what

A

the energy of the system

43
Q

what are the 3 components of energetics of a solution

A

solute is endothermic
solvent is endothermic
solution = exothermic

44
Q

is entropy preferred

A

yes

45
Q

what factors affect solubility

A

structure, pressure, temperature

46
Q

what does molecular structure effect

A

polarity

47
Q

what happens to solubility for solute and solvent

A

if they have similar properties then they are soluble

48
Q

number of carbons in alcohol

A

affects solubility
length increases = polar OH group is smaller = less solubility

49
Q

whar are the two classes of vitamins

A

fat-soluble (A,D,E,K)
water-soluble ( B and C)

50
Q

when like dissolves dislike what happens to the heat change of the solution

A

the heat change is large and positive preventing the solution from forming

51
Q

when like dissolves like what happens to the heat change of the solution

A

the solution will form bc of the increase in randomness

52
Q

what begins to happen as a solute dissolves in a solvent

A

the concentration of solute goes up and the solution increases with its chances of colliding with the surface

53
Q

what is crystallization

A

collisions result in the solute particles becoming reattached to the solid

54
Q

solute and solvent —–> solution

A

dissolve

55
Q

solution——> solute + solvent

A

crystallize

56
Q

when is the equilibrium established

A

rates of the opposing processes become equal

57
Q

what is saturated equilibrium

A

solute is undissolved
- solvent holds as much solute as possible @ that temperature

58
Q

what is solubility

A

amount of solute needed to form a saturated solution in a given quantity

59
Q

what is an unsaturated solution

A

less solute than what is needed to form a saturated solution is dissolved
- solvent does not hold as much

60
Q

what is a supersaturated solution

A

the greater amount of solute than is normally possible at that temperature

61
Q

the solubility of most solid solutes in water increases as what

A

the temp of the solution increases

62
Q

where is saturated on the solubility curve

A

saturated

63
Q

what is unsaturated on the curve

A

below the line

64
Q

what is supersaturated on the curve

A

supersaturated above the line

65
Q

increasing pressure increases what

A

the solubility of gases

66
Q

pressure has little effect on what

A

solubility of solids or liquids

67
Q

what is henry’s law

A

relationship between pressure and solubility of gas
C = kP

68
Q

what is C in henry’s law

A

C is the concentration of dissolved gas

69
Q

what is k in henry’s law

A

k is the constant

70
Q

what is P in henry’s law

A

the partial pressure of the gas above the solution

71
Q

the gas dissolved in the solution is directly proportional to…

A

the pressure of the gas above the solution

72
Q

the solubility of gases in water…

A

decreases with increasing temp

73
Q

what happens to the solubility of oxygen when it’s in water

A

decreases w/ increasing temp

74
Q

what is thermal pollution

A

changes in freshwater temps by human influence

75
Q

what is vapor pressure

A

pressure exerted by the vapor after equilibrium is reached

76
Q

what is nonvolatile

A

a substance that has no measurable vapor pressure

77
Q

what is volatile

A

one that exhibits a vapor pressure

78
Q

what is a semipermeable membrane

A

allows smaller particles to pass through and blocks larger particles

79
Q

what is osmosis

A

the flow of solvent through a semi-permeable membrane from low concentration to high concentration

80
Q

higher solvent =

A

lower solute amount= lower concentration

81
Q

what is a hypertonic mean

A

high concentration and low water

82
Q

what does hypotonic mean

A

low concentration and high wat

chemistry 1102 (6 decks)

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