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Chemistry H > Solutions > Flashcards

Solutions Flashcards

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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
Q

solubility curves

A
  • 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
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26
Q

solubility in unsatured solutions

A

more solute dissolves

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27
Q

solubility in saturated solution

A

no more solute dissolves

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28
Q

solubility in supersaturated solution

A

becomes unstable, crystals form

29
Q

unsaturated solutions

A
  • 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
Q

saturated solution

A
  • 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
Q

recrystallization

A

the temperature dependence of solubility is often used to purify crystalline solids

32
Q

supersaturated solutions

A
  • contains more solute than it should theoretically hold it a give temperature
33
Q

how to make a supersaturated solution?

A
  • 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
Q

concentration

A

measure of how much solute is dissolved in a solvent

35
Q

ways to express concentration

A

molarity (M)
molality (m)

36
Q

molarity conversions

A

1 M = 1 molar = 1 mol solute/liter of soln

37
Q

molarity

A

ways to express concentration of a solution

38
Q

molarity formula

A

moles of solute/liters of solution

39
Q

molality

A

concentration of solution expressed in moles of solute per kg of solvent

40
Q

molality formula

A

moles of solute/kg of solvent

41
Q

molality conversions

A

1000g = 1kg

42
Q

dilutions

A

made by adding more solvent to a solution

43
Q

dilution moles

A

moles of subtle before dilution equal moles of solute after dilution,

however concentration changes!

44
Q

dilution formula

A

m1v1 = m2v2

45
Q

m1 & v1

A

initial molarity and volume

46
Q

m2 & v2

A

final molarity

47
Q

percent by volume

A

volume of solute/volume of solution * 100

48
Q

mole fraction

A

moles of solute/moles solute + solvent 1

49
Q

percent by mass

A

mass of solute/solution volume * 100

50
Q

colligative properties

A

a property of a solution that only depends on # of solute particles

  • boiling point elevation
  • freezing point depression
51
Q

ionic compounds (&strong acids)

A

dissociate when dissolved in water

52
Q

molecular (covalent) compounds

A

do not dissociate in water

53
Q

freezing point depression

A

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
Q

∆Tf

A

change in freezing pt (celsius)

55
Q

Kf

A

molal freezing point pt constant (C/m) (1.86)

56
Q

m

A

molality

57
Q

i

A

of particles

58
Q

boiling point elevation

A

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
Q

boiling point elevation formula

A

∆tb = i * kb * m

60
Q

∆Tb

A

change in boiling pt (˚C)

61
Q

Kb

A

molal boiling pt constant (˚C/m) (0.512 for water)

62
Q

hydrates

A

ionic crystals that contain chemically bonded water moleculese

63
Q

electrolytes

A

substance whole water solution conducts electricity

64
Q

noneletrolyte

A

substance whose water solution does not conduct electricity

65
Q

surface tension

A

na inward force that trends to minimize the surface area of a liquid

66
Q

colloid

A

a heterogeneous mixture whose particles are intermediate in size between those of suspension and solution

67
Q

suspension

A

a heterogeneous mixture from which some of the particles settle out slowly upon standing

68
Q

emulsion

A

a colloidal dispersion of one liquid in another

Chemistry H (11 decks)

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