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chemistry 1302 gen chem 2 > chapter 10: Properties of solutions > Flashcards

chapter 10: Properties of solutions Flashcards

1
Q

what is a mixture

A

something that is composed of one or more pure substances

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2
Q

What are some examples of mixtures

A

wood, milk, gasoline, champagne. steel, seawater, air

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3
Q

what is a homogenous mixture

A

a something composed of one or more similar pure substances and it looks uniform throughout

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4
Q

what is a solution

A

a homogenous mixture of 2 or more pure substances

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5
Q

what is present in greater abundance in a solution

A

solvent

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6
Q

what is the universal solvent

A

H2O/water

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7
Q

what are some examples of solution

A

gases,liquids, and solids

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8
Q

what is an aqueous solution

A

water is the solvent and we add a solid, liquid or gas

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9
Q

what do the properties of solutions depend on

A

the structure of the molecules

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10
Q

what is concentration

A

amount of solute dissolved in a given quantity of solvent or solution

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11
Q

Molarity

A

M= moles of solute/ Liters of solution

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12
Q

Molality

A

m = moles of solute / Kg of solvent

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13
Q

what is temperature-dependent molarity or molality

A

molarity

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14
Q

what are colligative property examples

A

vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.

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15
Q

what is a colligative property

A

properties that depend on the concentrations of solute or solvent

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16
Q

what is giga

A

10^9

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17
Q

what is mega

A

10^6

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18
Q

what is kilo

A

10^3

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19
Q

what is hecto

A

10^2

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20
Q

what is deca

A

10^1

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21
Q

what is deci

A

10^-1

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22
Q

what is centi

A

10^-2

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23
Q

what is milli

A

10^-3

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24
Q

what is micro

A

10^-6

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25
Q

what is nano

A

10^-9

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26
Q

what is mass %

A

mass of solute / total mass solution

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27
Q

what is ppm (parts per million)

A

mass of component/ total mass x10^6

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28
Q

what is parts per billion

A

mass/ total mass x 10^9

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29
Q

what is mole fraction(X)

A

moles of solute/ total moles

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30
Q

if there is ppm or ppb then what does it indicate

A

mass fraction

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31
Q

what do you use to change molarity to molality

A

density

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32
Q

what is the density of water

A

1.00g/ml

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33
Q

1cm^3 =

A

1 mL

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34
Q

1000 mL = ?L

A

1

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35
Q

if given % of mass then what should you do

A

convert it to grams and find the other component using % (assume 100)

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36
Q

when is pressure the highest in a can

A

when the can is closed and not open and then the volume is the lowest because it is taking up most of the space

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37
Q

what happens to pressure and volume when a can is open

A

the pressure is going down and the volume is more because there is more space

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38
Q

like dissolves what

A

like

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39
Q

what is miscible

A

100% soluble

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40
Q

what is immiscible

A

always insoluble (NEVER soluble)

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41
Q

what is slightly miscible

A

soluble in some proportions

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42
Q

what is the weakest IMF

A

london dispersion

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43
Q

what is an IMf

A
  • attractive force that exists among particles
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44
Q

what happens when you change the pressure

A

change the strength of attractions

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45
Q

what forces hold covalent bonds

A

intramolecular bonds (within the molecule)

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46
Q

larger distance means what

A

less energy to break; weaker

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47
Q

higher the normal boiling point

A

stronger the IMF; bc it takes more energy to break those bonds

48
Q

what is a dipole-dipole force

A

exists in molecules that are polar and is WEAKER than ion-dipole forces

  • stronger w/ increasing polarity
  • polar mlcls have electron rich (-) regions and (+) regions that are not cancled out by the pull of electron density
49
Q

what is a dipole

A

material w/ charged ends

50
Q

what is a london dispersion force

A

nonpolar and polar

  • weakest and most abundant
  • instantaneous dipole
  • induce dipole
51
Q

what is an instantaneous dipole

A
  • a nonpolar mlcl like H2 or o2 are symmetric w. their center of electron density
52
Q

what is induced dipole

A

present in all molecules whether polar or nonpolar

53
Q

what can hydrogen bond with in a hydrogen bond

54
Q

what is an ion dipole

A

solution w/ ionic substances dissolved in a polar substance

-strongest

55
Q

what happens in steps 1-3 in a formation of a solution

A

step 1: endothermic to break down each reactant
step 2: endothermic to break down reactant
step 3: exothermic because we are forming a new substance

56
Q

what is an endothermic process

A

total energy for breaking attractions is GREATER than energy RELEASED

57
Q

what is an exothermic process

A

total energy for breaking attractions is LESS THAN energy RELEASED

58
Q

what is enthalpy of hydration

A

combines the energy required to separate solvnt molecules + energy produced from solute-solvent interactions

59
Q

what are the primary factors affecting solubility

A
  • relative IMF forces between solute and solvent (stronger Imf = greater solubility)
  • natural tendency of substances to mix( move toward a more dispersed and random state
60
Q

what is preferred in solubility

A

disorder

- example of removing the barrier

61
Q

what is entropy

A

the amount of randomness in a system

- lowers the energy

62
Q

if like is dissolving like then what is the heat of solution

A

small, so the solution WILL form bc of increase in randomness

63
Q

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

A

large and positive and it wil prevent it from forming

64
Q

in the example why would C5H12 dissolve CH3H3CH5OH

A

because it has a longer carbon chain even tho it has OH

65
Q

what is the order of the forces

A

london< dipoledipole< hydrogen< ion dipole

66
Q

what other factors affect solubility

A

-structure
temp
pressure

67
Q

what determines polarity

A

molecular strucutre

68
Q

nonpolar =

A

hydrophobic

69
Q

polar =

A

hydrophillic

70
Q

what happens if the length of carbon chain increases

A
  1. affects solubility

2. as length of C increases then OH group become smaller

71
Q

what are the 2 classes of vitamins

A
  • fat soluble (adek) (hydrophobic)

- water soluble (BC)( hydrophilic)

72
Q

what is crystallization

A

solid begins to dissolve in a solvent and the solute particles become reattached to the solid

73
Q

what is saturated

A

solution that is in equilibrium w/ undissolved solte

74
Q

what is solubility

A

the amount of solute needed to form a saturated solution in a given quanityty

75
Q

what is unsaturaed

A

less solute than what is needed

76
Q

what is supersaturated

A

more solute than what is needed

- unnatural

77
Q

how does temp affect solid solute solubility

A

temp increases = solubility increases

  • saturated = line
  • unsatureaed= below
  • supersaturated = above
78
Q

what increases the solubility of gases

79
Q

what is henrys law

A 
relationship between pressure and solubility of a gas
c= KP
c= concentration
k = constant
p = pressure
80
Q

how does temp affect gases

A
  • solubility of gases in water decreases w/ increasing temp
  • cold tap water is warmed and bubbles are seen
  • carbonated drinks are more bubbly in fridge
81
Q

what is vapor pressure

A

pressure exerted when equilibirum is reached

82
Q

what is nonvolatile

A

no measureable vapor pressure

salt

83
Q

what is volatile

A

measureable vapor pressure

ex: water

84
Q

what happens when you add a nonvolatile solute to a solvent

A

it makes it hard for the solvent to escape, and it reduces the vapor pressure

85
Q

if you have less moles what happens to the vapor pressure

A

pressure goes down as well

smaller # of vapor molecules = lower vapor pressure

86
Q

what is raoults law

A

extent to which a non volatile solute lowers the vapor pressure is proportional to the concentration

87
Q

what is the formula for raoults law and what do each of the things mean

A

Psolution = XsolventPsolvent
Psolvent= pure partial pressure of the solvent
X solvent = mole fraction

88
Q

what is raoults law all volatile

A

meaning both molecules are found in the vapor phase

89
Q

what is the formula for raoults law all volatiel

A

Ptotal = Psolue+ Psolvent = XsolventPsolvent + XsolutePsolute

90
Q

how do you find the mole fraction in an all volatile equation

A

Pbenzene/ P solution total (both molecules0

91
Q

what is an ideal raoults solution

A
  • colligative
  • liquid-liquid solutions
  • solute dilutes solvent
  • Heat solution = 0
92
Q

real solutions best approximate ideal behavior

A
  • solute concentration is low

- solute and solvent have similar IMFs

93
Q

nonideal solution negative deviation characteristics

A
  • solvent has STRONG affinity for the solute, vaporization is decreased
  • observed vapor pressure is LOWER than predicted by raoults law
  • occurs when Hsoln is large and negative(exothermic)
  • example: acetone and water
94
Q

nonideal solutoin- positive deviation characteristcs

A
  • little to no affinity for the solute
  • vaporization = increased
  • observed vapor pressure is HIGHER than the predicted
  • occurs when Heat soln is positive (endothermic)
    ex: ethanol + hexane
95
Q

what is the boiling point of water and what is boiling point elevation

A

100 degrees

Bp elevation- normal bp of a liquid is the temp @ which its vapor pressure equals 1 atm

96
Q

why is a higher temp needed for bp elevation

A

bc adding a nonvolatile solute lowers the vapor pressure so a higher temp is needed to obtain a vapor of 1 atm
- add more heat

97
Q

what is boiling point elevation

A
  • increase in boiling point relative to that of the pure solvent (Tb) is directly proportional to the MOLAL concentration
98
Q

what does the change in Tb =

99
Q

what is the equation for boiling point elevation

A

BP solution= BP solvent (100 degrees) + Tb

100
Q

what is freezing point depression

A

decrease in freezing point relative to that of the pure solvent
Tk is directly proportional to the molal concentration

101
Q

what is a freezing point

A

temp @ which the the solid and liquid phases exist

  • solute particles act as obstacles and disrupt solvent IMFs (entropy increases)
  • entropy has to be overcomes to form a solid
102
Q

what is the freezing point elevation equation

A

FP solution= Fp solvent(0 degrees) - Tf

103
Q

what is a semipermeable membrane

A

allows some smaller particles to pass through but blocks larger particles

104
Q

`what is osmosis

A

the flow of solvent from low concentration to high concentration
-natural

105
Q

what is hypertonic

A
  • high solute
  • low solvent
  • water moves out
106
Q

hypotonic

A
  • low solute
  • high solvent
  • water moves in (lysis or burst)
107
Q

what is isotonic

A

equal concentrations moving in and out

108
Q

what does osmotic pressure do

A

stops osmossis

109
Q

what is the equation for osmotic pressure

A

MRT
- M = concentration
R = 0.08206
T= temperature in kelvin

110
Q

what is reverse osmosis

A

pressure is GREATER than osmotic pressure and solvent flows from solution to pure solvent
move from high to low concentration

111
Q

how are strong electrolyes and weak electrolytes different in solutions

A

strong shows more changes than weak

112
Q

what is the van’t hoff factor

A

the relationship between the moles of solute dissolved and the moles of particles in solution

113
Q

how can you determine i

A

by noting the number of ions
ex. NaCl
i = 2

114
Q

how can you determine i with a concentration

A

if they give you i then muliply it by the concentration to find the true value
greater i means stronger ex. greater i mean increase in BP

115
Q

why is there a difference between the expected and observed colligative properties

A

because of electrostatic attractions

116
Q

what do colligitive propertues of electrolytes involve

A

using the vant hoff equation
Tf- Kfmi
Tb = Kbmi
osmotic pressure = iMRT

chemistry 1302 gen chem 2 (10 decks)

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