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Chemistry R120 > Chapter 13: Properties of Sultions > Flashcards

Chapter 13: Properties of Sultions Flashcards

1
Q

What are the 2 factors affecting the ability of substances to form solutions?

A

natural tendency for substances to mix | intermolecular interactions

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2
Q

How does mixing of gases happen spontaneously?

A

due to entropy (S)

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3
Q

What are the 3 kinds of intermolecular interactions involved in solution formation?

A

solute-solute interactions | solvent-solvent interactions | solvent-solute interactions

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4
Q

What are the solute-solute interactions?

A

between solute particles = need to overcome them in order to disperse the solute particles within the solvent

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5
Q

What are solvent-solvent interactions?

A

between solvent particles = need to overcome them to make room for the solute particles in between the solvent molecules

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6
Q

What are the solute-solvent interactions?

A

between solute and solvent particles = need to occur as they mix

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7
Q

What is solvation?

A

interaction that occurs when solute is surrounded by solvent molecules

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8
Q

What is hydration?

A

solvation interaction when solvent is H2O

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9
Q

What are hydrates?

A

solid compounds with a defined number of water molecules within the crystal lattice

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10
Q

What is crystallization?

A

when solute particles collide with the surface of a solute solid and reattach

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11
Q

What is a saturated solution?

A

solution that is in equal equilibrium with undissolved solute

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12
Q

What is solubility?

A

MAX amount of solute that can dissolve in a given quantity of solvent to form a saturated solution

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13
Q

What is an unsaturated solution?

A

less solute dissolved than the amount needed to form a saturated solution

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14
Q

What is a supersaturated solution?

A

solvent holding more solute than is normally possible at that temperature | unstable solutions

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15
Q

How can crystallization occur with a super saturated solution?

A

by adding a “seed of crystal” or scratching the side of a flask

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16
Q

What are the 3 factors affecting solubility?

A

solute-solvent interactions | pressure | temperature

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17
Q

How does solubility affect solute-solvent interactions?

A

increase in solubility is due to stronger attractions between solute and solvent molecules

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18
Q

What is miscible?

A

liquids that mix in all proportions

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19
Q

What is immiscible?

A

liquids that don’t mix in one another

20
Q

How does pressure affect the solubility of a gaseous solution?

A

increase in partial pressure above the solvent = increases solubility of a gas in solvent

21
Q

What is Henry’s Law?

A

solubility of a gas in a liquid solvent increases in direct proportion to the partial pressure of the gas above the solution

22
Q

How does temperature affect solubility?

A

increase temp(T) = increase solubility of solids in water BUT decreases solubility of gases in water

23
Q

What is dilute?

A

small concentration of solute

24
Q

What is concentrated?

A

large concentration of solute

25
Q

What are ppm (parts per million) and ppb (per billion) used for?

A

to express concentrations of very dilute solutions

26
Q

What can you use to convert between Molarity and molality?

A

density

27
Q

What is the difference between molarity and molality?

A

molaRity = depends on the VOLUME of solution; varies with temp(T) changes | molaLity = depends on MASS of solvent; doesn’t vary with temp(T)

28
Q

What are colligative properties of a solution?

A

depend on the collective effect of the number of solute particles

29
Q

What does “colligative” mean?

A

“depending on the collection”

30
Q

What are the 4 kinds of colligative properties?

A

vapor-pressure lowering | boiling-point elevation | freezing-point depression | osmotic pressure

31
Q

What is a non-volatile substance?

A

no measurable vapor pressure

32
Q

What does Raoult’s Law state?

A

vapor pressure of a volatile solvent above a solution containing a nonvolatile solute is proportional to the solvent’s concentration in the solution

33
Q

What is vapor-pressure lowering?

A

When a nonvolatile solute is added to a volatile pure solvent, the vapor pressure of the solvent (above the resulting solution) is lower than the vapor pressure above the pure solvent.

34
Q

What is boiling-point elevation?

A

the boiling point of a solution is HIGHER than that of the pure solvent due to vapor-pressure lowering | higher temp is now needed to reach a vapor pressure of 1atm

35
Q

What is freezing-point depression?

A

freezing point of solution is LOWER than that of the pure solvent due to vapor-pressure lowering | lower temp is now needed to reach a vapor pressure of 1atm

36
Q

What is the van’t Hoff factor (i)?

A

number of fragments that a solute breaks up into for a particular solvent

37
Q

What is the van’t Hoff factor for non-electrolytes?

A

1

38
Q

What is the van’t Hoff factor for electrolytes?

A

depends on how the substance ionizes

39
Q

What is osmosis?

A

net movement of solvent molecules from low [solute] –> high [solute] (to even things out)

40
Q

What is osmotic pressure?

A

the pressures that stops osmosis

41
Q

What are the 3 types of of solutions in osmosis?

A

isotonic | hypertonic | hypotonic

42
Q

What is an isotonic solution?

A

same osmotic pressure of solvents and solutes = solvent passes through semi-permeable membrane at the same rate both ways

43
Q

What is a hypertonic solution?

A

high osmotic pressure = solvent enters solution at a higher rate than leaving

44
Q

What is a hypotonic solution?

A

low osmotic pressure = solvent enters solution at a slower rate than leaving

45
Q

What are colloids?

A

suspensions of particles larger than individual ions or molecules, but TOO small to be settled out by gravity

46
Q

What is the Tyndall effect?

A

phenomenon illustrating the ability of colloidal particles to scatter rays of light

47
Q

What regions do colloids have?

A

hydrophobic and hydrophilic regions

Chemistry R120 (18 decks)

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