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Chemistry H > Solutions > Flashcards

Solutions Flashcards

(68 cards)

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1
Q

solution

A

homogeneous mixture

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2
Q

solvent

A

dissolving medium

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3
Q

solute

A

dissolved particles

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4
Q

types of solutions

A
  1. gas: gases dissolved in one another
  2. liquid: liquid solvent (usually water) with gas, liquid, or solid solute
  3. solid: mixtures of solids
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5
Q

solid-solid solution

A

copper in zinc (brass)

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6
Q

liquid-solid solution

A

mercury in silver (dental amalgams)

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7
Q

solid-liquid solution

A

salt water

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8
Q

gas-liquid solution

A

soda

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9
Q

gas-gas solution

A

co2 in air

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10
Q

solubility

A

the amount of substance that dissolves in a given quantity of solvent to make a saturated solution at constant temp and pressure

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11
Q

to gauge the degree of solubility

A
  1. nature of solute and solvent
  2. temperature
  3. pressure (for gases)
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12
Q

nature of solute & solvent (degree of solubility)

A

“like dissolves like”

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13
Q

temperature (degree of solubility)

A

increase temp, increase solubility (for solids)

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14
Q

pressure (gases) (degree of solubility)

A

increase pressure, increase solubility

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15
Q

miscible

A

two liquids that dissolve of mix into each other (ex. alcohol and water)

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16
Q

immiscible

A

two liquids can not mix or dissolve in each other

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17
Q

immiscible examples

A

oil and water (salad dressing)
lava lamp (paraffin and water)

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18
Q

factors affecting rate of solution (solid in liquid)

A
  1. temp –> increased temp, more kinetic energy –> dissolves faster
  2. size –> smaller particles dissolve faster because of more surface area
  3. stirring –> more concentration gradient
  4. already dissolved solute –> less concentration gradient
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19
Q

rate of solution

A

how fast a substance dissolves

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20
Q

concentration gradient in rate of solution

A
  • energy transfer is always from high temp to low
  • material temp is always from high concentration to lower concentration
  • the more the gradient, the faster the transfe
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21
Q

atomic transfer of energy and material will…

A

always work to balance the amount of energy and material - a natural law

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22
Q

solubility of gas in liquid

A
  1. temperature: increase temp, less gas dissolved
  2. pressure: increase pressure, more gas dissolved
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23
Q

solubility of solids in liquids

A

increase temp, increase solubility

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24
Q

henry’s law

A

at a given temp, the solubility s of a gas in a liquid is directly proportional to pressure p

s1/p1 = s2/p2

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25
solubility curves
- shows how much solute will dissolve in a given amount of solvent over a range of temps - usually how many grams of solute that will dissolve in 100g of water
26
solubility in unsatured solutions
more solute dissolves
27
solubility in saturated solution
no more solute dissolves
28
solubility in supersaturated solution
becomes unstable, crystals form
29
unsaturated solutions
- amount of solute dissolved is less than the solubility at that temperature - all solute dissolves completely!! - solutions contain less solute than it can hold at a certain temp
30
saturated solution
- maximum amount of solute dissolved at a given solvent at a constant temp - solution contains all the solute it can hold at the given temp - temp must be stated
31
recrystallization
the temperature dependence of solubility is often used to purify crystalline solids
32
supersaturated solutions
- contains more solute than it should theoretically hold it a give temperature
33
how to make a supersaturated solution?
- a sautéed solution at high temperature is allowed to cool while it sits undisturbed - as it cools, the solute remains in the solution - once it has retuned to room temp, there will be more solute -> this I san unstable situation - if a single crystal of solute is added to a supersaturated solution, the excess solute crystallizes out
34
concentration
measure of how much solute is dissolved in a solvent
35
ways to express concentration
molarity (M) molality (m)
36
molarity conversions
1 M = 1 molar = 1 mol solute/liter of soln
37
molarity
ways to express concentration of a solution
38
molarity formula
moles of solute/liters of solution
39
molality
concentration of solution expressed in moles of solute per kg of solvent
40
molality formula
moles of solute/kg of solvent
41
molality conversions
1000g = 1kg
42
dilutions
made by adding more solvent to a solution
43
dilution moles
moles of subtle before dilution equal moles of solute after dilution, however concentration changes!
44
dilution formula
m1*v1 = m2*v2
45
m1 & v1
initial molarity and volume
46
m2 & v2
final molarity
47
percent by volume
volume of solute/volume of solution * 100
48
mole fraction
moles of solute/moles solute + solvent 1
49
percent by mass
mass of solute/solution volume * 100
50
colligative properties
a property of a solution that only depends on # of solute particles - boiling point elevation - freezing point depression
51
ionic compounds (&strong acids)
dissociate when dissolved in water
52
molecular (covalent) compounds
do not dissociate in water
53
freezing point depression
refers to the lowering of the freezing point of solvents upon the addition of the solute difference in temp between the freezing point of solution & that of the pure solvent ∆Tf = I * k * m
54
∆Tf
change in freezing pt (celsius)
55
Kf
molal freezing point pt constant (C/m) (1.86)
56
m
molality
57
i
of particles
58
boiling point elevation
increase in the boiling point of a solvent upon the addition of a solute when a solute is added to a solvent, the resulting solution has a higher boiling point than that of a pure solvent difference in temp between boiling point of a solution & that of the pure solvent
59
boiling point elevation formula
∆tb = i * kb * m
60
∆Tb
change in boiling pt (˚C)
61
Kb
molal boiling pt constant (˚C/m) (0.512 for water)
62
hydrates
ionic crystals that contain chemically bonded water moleculese
63
electrolytes
substance whole water solution conducts electricity
64
noneletrolyte
substance whose water solution does not conduct electricity
65
surface tension
na inward force that trends to minimize the surface area of a liquid
66
colloid
a heterogeneous mixture whose particles are intermediate in size between those of suspension and solution
67
suspension
a heterogeneous mixture from which some of the particles settle out slowly upon standing
68
emulsion
a colloidal dispersion of one liquid in another

Chemistry H (11 decks)

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