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Chemistry I > Chapters 14 & 15 > Flashcards

Chapters 14 & 15 Flashcards

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1
Q

Thirsty Solution

A

draws more water to itself

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2
Q

Solution

A

homogeneous mixture of 2+ substances or components

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3
Q

majority component in a solution

A

solvent

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4
Q

minority component in a solution

A

solute

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5
Q

nature has a tendency towards…

A

spontaneous mixing

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6
Q

substances tend to combine into what kind of mixtures

A

uniform

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7
Q

aqueous solution

A

water is the solvent and a solid, liquid, or gas is the solute

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8
Q

solubility

A

amount of a substance that dissolves in a given amount of solvent

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9
Q

most physical systems tend toward what kind of potential energy

A

lower

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10
Q

according to Coulomb’s law, potential energy BLANK as their separation BLANK

A

potential energy decreases as separation decreases

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11
Q

does the formation of a solution always lower potential energy of its constituent particles?

A

no

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12
Q

the tendency to mix is related to a concept called

A

entropy

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13
Q

entropy

A

measure of energy randomization or energy dispersal in a system

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14
Q

why do two ideal gases mix?

A

the tendency for energy to spread out wherever it is not restrained from doing so

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15
Q

miscible

A

two substances soluble in each other in all proportions

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16
Q

formation of solutions is drive by the tendency to do what

A

to mix, greater entropy

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17
Q

solutions form with what two kinds of relative interactions

A

1) when solven-solute interactions are greater than solvent-solvent interactions
2) solvent-solute interactions are close to equal to solvent-solvent interactions

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18
Q

what is the general rule of thumb for solubility?

A

like dissolves like

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19
Q

is forming a solution always a chemical reaction

A

no

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20
Q

if heat is evolved, the process is

A

exothermic

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21
Q

if heat is absorbed, the process is

A

endothermic

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22
Q

breaking of bonds is what kind of process

A

endothermic

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23
Q

forming bonds is what kind of process

A

exothermic

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24
Q

separating the solute into constituent particles is always what kind of process

A

endothermic

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25
Q

mixing, combining solvent particles is always what kind of process

A

exothermic

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26
Q

what is enthalpy of solution

A

sum of changes in enthalpy

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27
Q

what is heat of hydration

A

enthalpy change that occurs when 1 mol of gas solute ions is dissolved in water

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28
Q

heat of hydration is always largely what for ionic compounds

A

largely exothermic due to strong ion-dipole interactions

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29
Q

if the heat of solute is less than heat of hydration, what is the process

A

exothermic

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30
Q

if the energy requried to separate the solute into its constituent ions is greater than the energy given off when the ions are hydrated, what is the process

A

endothermic

31
Q

what temperature are endothermic solutions to the touch

A

cool

32
Q

what is reached when rates of dissolution and recrystallization have become equal

A

dynamic equillibrium

33
Q

what is a saturated solution

A

dissolved solute is in dynamic equilibrium with the solid (undissolved) solute

34
Q

what is a supersaturated solution

A

solutions containing more than the equilibrium amount of solute

35
Q

what generally happens to supersaturated solutions after a time

A

excess solute normally precipitates out of solution

36
Q

what effect does increasing temperature have on the solubility of solids

A

solubility increases

37
Q

what is recrystallization

A

way to purify a solid

38
Q

how does recrystallization work?

A

crystalline structure tends to reject impurities

39
Q

what two things is the solubility of a gas in a liquid affected by?

A

temperature and pressure

40
Q

describe the relationship between solubility of a gas with temperature and pressure

A

solubility of gas decrease with increasing temperature and increases with increasing pressure

41
Q

what is Henry’s law

A

solubility (gas) = k (M/atm) x P (gas)

42
Q

what is a dilute solution

A

solution that contains small quantities of solute relative to amount of solvent

43
Q

concentrated solution

A

large quantities of solute relative to amount of solvent

44
Q

molarity formula

A

moles solute/ volume solution

45
Q

does molarity depend on temperature

A

yes

46
Q

does molality depend on temperature

A

no

47
Q

equation for molality

A

mols of solute/ kg of solvent

48
Q

when is molality useful

A

comparing concentrations across different temps

49
Q

what is ppm

A

parts per million, 10^6

50
Q

what is ppb

A

parts per billion, 10^9

51
Q

collagitive property

A

depends on number of particles dissolved in the solution

52
Q

what are the 4 collagitive properties

A

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

53
Q

nonvolatile

A

susbtance that doesn’t vaporize rapidly

54
Q

in vapor pressure lowering, what component has a decrease in vapor pressure

A

solutions has a lower vapor pressure than the pure solvent

55
Q

Raoult’s law

A

P(solution)= X(solvent) x Pure pressure(solvent)

56
Q

what is the relatioship between vapor pressure and solvent

A

direct proportionality of vapor pressure to amount of solvent in the solution

57
Q

What is another name for a volatile solute

A

nonelectrolyte

58
Q

Raoult’s law for 2 component solution containing liquids A and B

A

1) Pa=Xa+P0a
2) Pb=Xb+P0b
3) Ptotal=Pa+Pb

59
Q

what happens to a non-ideal solution in which solute-solvent interactions are stronger than solvent-solvent interactions

A

the solute tends to prevent solvent from vaporizing as readily

60
Q

a nonvolatile solute does what to vapor pressure of a solution

A

lowers the vapor pressure, lifts the boiling point and lowers freeizing point

61
Q

a highly concentrated solution will have what kind of freezing point, boiling point

A

low freezing point and high melting point

62
Q

equation for change in Temp

A

Change in Temp=Km

63
Q

osmosis

A

flow of solvent from solution of low solute concentration to one of higher concentration (from diluted to concentrated)

64
Q

osmotic pressure

A

pressure required to stop the osmotic flow

65
Q

osmotic pressure formula

A

pi=MRt

66
Q

van’t Hoff factor

A

i = moles of particles in solution / moles of formula units dissolved

67
Q

rate of a chemical reaction is a measure of

A

how fast the reaction occurs

68
Q

the reaction portion of a reaction rate contains what kind of sign

A

negative

69
Q

what happens to product concentrations as the reaction proceeds

A

the concentrations increase

70
Q

what happens to reactant concentration in relation to time

A

as time increases, reactant concentration decreases

71
Q

rate depends on BLANK of the reactants

A

concentration

72
Q

in zero oder reaction, the rate is BLANK of concentration A

A

independent

73
Q

in first order reaction, rate is BLANK to concentration of A

A

proportional

74
Q
A

Chemistry I (16 decks)

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