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Solutions Flashcards

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1
Q

What is molarity?

A

mol of solute / L of solution (M)

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2
Q

Molality

A

mol of solute/ kg of solvent (m)

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3
Q

Molality is for what type of properties only?

A

colligative properties

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4
Q

Colligative Properties

A

properties that depend only on the number of particles, not the identity

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5
Q

What are the 4 colligative properties?

A

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

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6
Q

What is about the same in dilute solutions?

A

.1 M is about .1 m

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7
Q

Mass percent

A

compares the grams of solute to grams of solution

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8
Q

Mole Fraction

A

compares the moles of solute to moles of solution

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9
Q

What 3 things occur when dissolving a substance?

A
  1. the solute expands (IMF are broken) - lattice energy
  2. the solvent expands (IMF are broken)
  3. the solute and solvent combine (new IMF are formed)
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10
Q

Enthalpy of the solution

A

total of enthalpy changes when dissolving

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11
Q

Enthalpy of hydration

A

changes when already separated solute is added to water

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12
Q

Explain the dissolving process with a nonpolar solute and polar solvent

A
  1. non-polar solvent is delta H1: has small IMF (LD) + bonds being broken = small to medium positive enthalpy
  2. polar solvent is delta H2: has large IMF (H-bonds or dipoles) + bonds being broken = large positive enthalpy
  3. delta H3: has essentially zero IMF because they don’t mix= small positive enthalpy
  4. enthalpy of solution: small positive + larger positive + small positive = very larger positive
  5. No solution forms (immiscible = does not dissolve in any amount. - don’t mix
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13
Q

Explain the dissolving process with a polar solute and non-polar solvent

A
  1. polar solute = delta H1 = large IMF + bonds breaking = large positive
  2. nonpolar solvent = delta H2 = small IMF (LD) + bonds breaking = small positive
  3. delta H3 = small positive (no IMF)
  4. enthalpy of solution= large positive + small positive + small positive = larger positive
  5. no solution forms (immiscible) - don’t mix
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14
Q

What happens with the enthalpy of the solution is large and positive?

A

NO solution forms (immiscible)

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15
Q

What happens when the enthalpy of the solution is negative?

A

the solution will form (miscible)

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16
Q

Dissolving process for polar solute + polar solvent

A
  1. polar solute = large IMF + bonds breaking = large positive
  2. polar solvent = large IMF + bonds breaking = large positive
  3. energy is released when new IMF forms = very large negative
  4. enthalpy of the solution = probably negative - solution will form
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17
Q

What happens when the enthalpy of the solution is small?

A

solution will form

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18
Q

Polar solute & polar solvent (small enthalpy)

A

possible small positive enthalpy of solution- still miscible

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19
Q

nonpolar solute & nonpolar solvent

A
  1. solute = small positive (IMF + broken bonds)
  2. small positive (IMF + bonds broken)
  3. delta H3 = small positive
  4. enthalpy of the solution is small & positive because the increase in entropy overcomes any positive enthalpy of the solution
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20
Q

C-H bonds are

A

non-polar (because of similar electronegativites)

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21
Q

-OH groups make H-bonds that are

A

polar (H-bonds - strongest)

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22
Q

“ol” at the end of a structural formula means

A

alcohol

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23
Q

C-O and C-N bonds are

A

polar (two dissimilar non-metals -two different electronegativities)

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24
Q

-COOH group

A
  1. carboxyl group

2. polar

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25
Q

H at the end of -COOH ionizes to make

A

an acid

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26
Q

How can a large molecule with C-H bonds be considered polar

A

must have many polar groups (more elcectrons)

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27
Q

fats & oils = large C-H molecules are

A

nonpolar

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28
Q

What are the 2 types of vitamins

A
  1. water-soluble (polar) must be replaced daily (C, B)

2. fat soluble (non-polar) are stored in the body (A, D, E, K)

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29
Q

halides

A

dissolve best in water (ionic or polar)

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30
Q

halogen

A

dissolve best in non-polar solvent like mineral oil ( LD )

31
Q

What will a polar solvent & non-polar solvent form when mixed

A

two layers

32
Q

What are the factors that affect solubility?

A

structural factors (polar vs. nonpolar), pressure effects, and temperature effects

33
Q

pressure has little effect on

A

solids and liquids

34
Q

What does pressure affect?

A

the gas dissolved in a liquid

35
Q

What happens when more P is added?

A
  1. increase in # of dissolving gas molecules

2. new equilibrium is established with MORE gas dissolved

36
Q

Henry’s law

A

amount of gas dissolved in a solution is directly proportional to the pressure of the gas above the solution

37
Q

When the temperature is increased what happens

A
  1. the rate of solubility is increased

2. the volume of the solution increases slightly

38
Q

What occurs when you decrease the temperature of the water?

A
  1. it decreases the water’s volume until 4 C - water is opposite this trend after 4 C; because the H-bonds are making the liquid become solid (water is larger as a solid
39
Q

temperature cannot predict

A

the amount of solubility

40
Q

solubility is dependent on

A

temperature, IMF, and # of e-s (not mass)

41
Q

What is the effect of a non-volatile solute on the VP?

A
  1. it lowers the VP because the molecules are blocking the water molecules
  2. more molecules will leave than pure solvent the solution
  3. all the pure solvent will evaporate as the solution continues to pull molecules from the air
42
Q

Raoult’s Law

A

the direct relationship between mole fraction of solvent and VP of solvent

43
Q

a solution is considered ideal when

A

the solute and solvent do not interact ( the interaction between each are similar) - a solute is the dilution the solution

44
Q

what occurs when the observed VP is lower than expected (non-ideal)

A
  1. negative deviation from Raoult’s law
  2. fewer molecules are evaporating than expected
  3. enthalpy of the solution is larger and negative (exothermic)
  4. the solvent and solute must attract each other in H-bonds
45
Q

what occurs when the observed VP is higher than expected (non-ideal)

A
  1. positive deviation from Raoults law
  2. more molecules are evaporating than expected
  3. the solute and solvent must repel (polar and non-polar mix)
46
Q

vapor pressure is affected by

A

temperature, # of electrons, and IMF

47
Q

When something is dissolved in water, what happens to the vapor pressure?

A

the vapor pressure goes down because the dissolved particles get in the way so fewer water molecules are able to escape

48
Q

boiling point occurs when

A

VP = atmospheric pressure

49
Q

freezing point occurs when

A

VP (liquid) = VP (solid)

50
Q

what happens to make the boiling point of water go up when something is dissolved in water?

A

the vapor pressure of water must equal 1 atm of 760 torr to boil and the VP of pure water is 20 torr at 20 C; therefore it takes longer for the temperature to continue to rise

51
Q

why does the freezing point go down as more particles are added to a solution?

A

the solute interferes with crystal formation

52
Q

osmotic pressure

A

the pressure needed to stop osmosis

53
Q

osmosis

A

the flow of a solvent into a solution through a semipermeable membrane

54
Q

semipermeable membrane

A

membrane with holes that allows molecules of a specific size to pass-through

55
Q

what can pass through in osmosis

A

only the solvent

56
Q

what can pass through in dialysis

A

both the solvent and other molecules of a limited size

57
Q

what is osmotic pressure measured in?

A

atms

58
Q

what can account for a large osmotic pressure

A

small concentrations

59
Q

isotonic solutions

A

solutions with identical osmotic pressures

60
Q

hypertonic solutions

A

have higher osmotic pressures & higher molarites

61
Q

hypotonic solutions

A

have lower osmotic pressures & lower molarities

62
Q

reverse osmosis

A

a pressure greater than osmotic pressure is applied causing the solvent to leave the solution- producing pure solvent

63
Q

electrolyte solutions

A

solutions with ions (conduct electricty); alcohols are not electrolytic

64
Q

i =

A

van’t Hoff factor

65
Q

why is the “i” sometimes less than expected?

A

ionic pairing

66
Q

colloids

A

the suspension of tiny particles, that stay suspended because of electrostatic repulsion

67
Q

what is the difference between a colloid & a solution

A

colloids scatter light & solutions do not

68
Q

Ksp =

A

used to tell if a precipitate will occur or if all the solute will dissolve

69
Q

Q > Ksp

A

ppt will form and only some solute dissolves

70
Q

Q < Ksp

A

no ppt; all solute will dissolve + additional solute

71
Q

Q = Ksp

A

all solute will dissolve but not additional solute

72
Q

pH of acids

A

< 7

73
Q

pH of bases

A

> 7

74
Q

pH of alcohols

A

= 7

AP Chemistry (1 decks)

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