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Chemistry 105 > Chapter 13 > Flashcards

Chapter 13 Flashcards

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1
Q

How a solution is formed

A
  • When one substance disperses uniformly throughout another
  • When the magnitudes of the attractive forces between solute and solvent particles are comparable to or greater than those that exist between the solute particles themselves or between the solvent particles themselves.
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2
Q

Ability of substance to form solutions depends on 2 general factors

A

1) the types and relative strengths of intermolecular interactions between and among solute and solvent particles
2) natural tendency of substances to spread into larger volumes when not restrained

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3
Q

Ion-dipole forces dominate (when?)

A

Solutions consist of ionic substances in water

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4
Q

Dispersion forces dominate (when?)

A

Nonpolar substance dissolves in another nonpolar one.

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5
Q

How to identify a solvent

A

Normally the component present in the greatest amount

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6
Q

How to identify a solute

A

Other components in a solution other than the solvent (which is ththe greatest quantity)

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7
Q

Gas + Gas =

A

Gas

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8
Q

Liquid + Gas =

A

Liquid

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9
Q

Liquid + Liquid =

A

Liquid

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10
Q

Liquid + Solid =

A

Liquid

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11
Q

Solid + Gas =

A

Solid

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12
Q

Solid + Liquid =

A

Solid

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13
Q

Solid + Solid =

A

Solid

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14
Q

Entropy

A

The degree of randomness in a system (disorder).

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15
Q

Crystallization

A

When a solution reforms into solvent; when particles of solute reattach to a solid.

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16
Q

Saturation

A

A solution in equilibrium with undissolved solute

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17
Q

Solubility

A

The amount of solute needed to form a saturated solution in a given quantity of solvent, at a specified temperature.

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18
Q

Unsaturated solution

A

Less solute is dissolved than that needed to form a saturated solution

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19
Q

Supersaturation

A

Solutions with more solute than that needed to form a saturated solution (unstable condition).

20
Q

Effect of increasing molecular mass or polarity on solubility

A

Solubility increases with increasing molecular mass or polarity

21
Q

The stronger the attractions are between solute and solvent molecules, the greater/lesser the solubility

A

Greater

22
Q

Polar liquids tend to dissolve readily in polar solvents because

A

of favorable dipole-dipole attractions between solvent molecules and solute molecules.

23
Q

Miscible

A

Pairs of liquids that mix in all proportions

24
Q

Immiscible

A

Liquids that do not dissolve in one another

25
Q

Nonpolar liquids tend to be insoluble in polar liquids because

A

the attraction between the polar water molecules and the nonpolar hydrocarbon molecules is not sufficiently strong to allow the formation of a solution.

26
Q

What does “like dissolves like” mean?

A

Substances with similar intermolecular attractive forces tend to be soluble in one another.

27
Q

Solubilities of solids and liquids are/are not appreciably affected by pressure

A

Are not

28
Q

Solubility of gases are/are not appreciably affected by pressure

A

Are

29
Q

Effect of pressure on solubility of gas

A

Solubility of the gas increases in direct proportion to its partial pressure above the solution

30
Q

Henry’s law

A 
Sg = kPg
Sg = solubility of the gas in the solution phase (expressed as molarity)
Pg = partial pressure of the gas over the solution
k = proportionality constant called Henry's law constant
31
Q

what is Henry’s law constant?

A

Different for each solute-solvent pair

Varies with temperature

32
Q

Effect of temperature on solubility of solids

A

The solubility of most solid solutes in water increases as the temp increases

33
Q

Effect of temperature on solubility of gases

A

Solubility of gases in water decreases with increasing temp

34
Q

Mass % formula

A

g solute/g solution * 100

Also, g solute/(g solute + g solvent)

35
Q

Mole fraction

A

mol solute/mol solution
Also, mol solute/(mol solute + mol solvent)
-Moles of component/total moles of all components

36
Q

Molarity (M)

A

mol solute/L solution

37
Q

Molality (m)

A

mol solute/kg solvent

38
Q

How to convert m (molality) to mole fraction

A

convert kg of solvent to mol of solvent and use the above formula

39
Q

What is the conversion factor between molarity and molality?

A

density of the solution (g/L)

40
Q

Colligative propertios

A

Boiling point, freezing point, vapor pressure (skipping calculations for test), osmotic pressure

41
Q

Normal boiling point

A

Temp at which a liquid’s vapor pressure will equal 1 atm

42
Q

Boiling point elevation equation

A

Delta-Tb = Kb x Cm (or, Kb x m)
(change in temp = molal bpe constant, times the molality of the solution)
Also, Delta-Tb = Tb solution - Tb solvent

43
Q

Freezing point depression equation

A

Delta-Tf = Kf x Cm (or, Kb x m)
(change in temp = molal fpd constant, times the molality of the solute)
Also, Delta-Tb = Tb solvent - Tb solution

44
Q

Osmotic Pressure (definition)

A

Pressure difference at equilibrium; the applied pressure required to prevent the net movement of water from solute to solution (prevent osmosis by pure solvent)

45
Q

Osmotic Pressure equation

A

II = MRT

Molarity, times the ideal-gas constant, times temp (K)

Chemistry 105 (13 decks)

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