chapter 10: Properties of solutions Flashcards

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
why do IMFs between solute and solvent particles need to be strong
to be competitive
26
what can you use to calculate the molarity
density
27
what does molality depend on
volume
28
what does 1 cm^3 equal
1 Liter
29
what is the muliplicaton factor for parts per billion
10^9
30
what are the types of IMFs
dispersion dipole dipole hydrogen bond ion dipole
31
what is london dispersion
weakest intermolecular force non polar
32
what is dipole dipole force
forces bwteen positive end of one polar molecule and the negative end of another polar molecule
33
what is a hydrogen bond
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
what is ion dipole
attractive force that results from an ion and a molecule that has a dipole example: Na + ion and water
35
what does hydrogen need to bond with to make it a hydrogen bond
FON
36
what is an endothermic process
total energy to break the attractive forces is higher than the energy released "takes to break"
37
what is the oil and water example
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
what is an exothermic process
the total energy for breaking the attractions is less than the energy is released "frees to form"
39
what factors affect solubility
1. ) ImFs among the solute and solvent molecules 2. ) natural tendency for substances to mix
40
strong IMFs =
strong attractions and greater solubility
41
what is entropy
the amount of randomness in a system/ amount of disorder
42
entropy lowers what
the energy of the system
43
what are the 3 components of energetics of a solution
solute is endothermic solvent is endothermic solution = exothermic
44
is entropy preferred
yes
45
what factors affect solubility
structure, pressure, temperature
46
what does molecular structure effect
polarity
47
what happens to solubility for solute and solvent
if they have similar properties then they are soluble
48
number of carbons in alcohol
affects solubility length increases = polar OH group is smaller = less solubility
49
whar are the two classes of vitamins
fat-soluble (A,D,E,K) water-soluble ( B and C)
50
when like dissolves dislike what happens to the heat change of the solution
the heat change is large and positive preventing the solution from forming
51
when like dissolves like what happens to the heat change of the solution
the solution will form bc of the increase in randomness
52
what begins to happen as a solute dissolves in a solvent
the concentration of solute goes up and the solution increases with its chances of colliding with the surface
53
what is crystallization
collisions result in the solute particles becoming reattached to the solid
54
solute and solvent -----\> solution
dissolve
55
solution------\> solute + solvent
crystallize
56
when is the equilibrium established
rates of the opposing processes become equal
57
what is saturated equilibrium
solute is undissolved - solvent holds as much solute as possible @ that temperature
58
what is solubility
amount of solute needed to form a saturated solution in a given quantity
59
what is an unsaturated solution
less solute than what is needed to form a saturated solution is dissolved - solvent does not hold as much
60
what is a supersaturated solution
the greater amount of solute than is normally possible at that temperature
61
the solubility of most solid solutes in water increases as what
the temp of the solution increases
62
where is saturated on the solubility curve
saturated
63
what is unsaturated on the curve
below the line
64
what is supersaturated on the curve
supersaturated above the line
65
increasing pressure increases what
the solubility of gases
66
pressure has little effect on what
solubility of solids or liquids
67
what is henry's law
relationship between pressure and solubility of gas C = kP
68
what is C in henry's law
C is the concentration of dissolved gas
69
what is k in henry's law
k is the constant
70
what is P in henry's law
the partial pressure of the gas above the solution
71
the gas dissolved in the solution is directly proportional to...
the pressure of the gas above the solution
72
the solubility of gases in water...
decreases with increasing temp
73
what happens to the solubility of oxygen when it's in water
decreases w/ increasing temp
74
what is thermal pollution
changes in freshwater temps by human influence
75
what is vapor pressure
pressure exerted by the vapor after equilibrium is reached
76
what is nonvolatile
a substance that has no measurable vapor pressure
77
what is volatile
one that exhibits a vapor pressure
78
what is a semipermeable membrane
allows smaller particles to pass through and blocks larger particles
79
what is osmosis
the flow of solvent through a semi-permeable membrane from low concentration to high concentration
80
higher solvent =
lower solute amount= lower concentration
81
what is a hypertonic mean
high concentration and low water
82
what does hypotonic mean
low concentration and high wat