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Chem 115 > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

Is the solute normally lesser or greater?

A

lesser

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2
Q

Is the solvent normally lesser or greater?

A

greater

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3
Q

Under what conditions does a solute dissolve?

A

solute-solvent attraction > solute-solute attraction

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4
Q

hydrated ions

A

when positive and negative are separated and surrounded by water molecules

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5
Q

solvation

A

process of solute and solvent molecules interacting

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6
Q

hydration

A

when the solvent is water

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7
Q

water is a ___ molecule

A

polar

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8
Q

three characteristics of water

A
  1. uneven electron distribution
  2. bent molecular shape
  3. dissolves most substances
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9
Q

van der Waals forces

A

forces between neutral molecules

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10
Q

London dispersion forces

A

temporary attractive force that results from the electrons of two adjacent atoms occupying positions where the atoms form temporary ‘induced’ dipoles.
-weakest van deer waal force

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11
Q

dipole-dipole forces

A

between positive end of one polar molecule and the negative end of another polar molecule
-can be repulsive

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12
Q

hydrogen bond forces

A

H (partially positive) and lone pair

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13
Q

ion-dipole forces

A

attraction that results from the electrostatic attraction between an ion and a neutral molecule

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14
Q

molecules with similar intermolecular forces are most likely ____ to one another

A

soluble

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15
Q

immiscible

A

when liquids do not mix

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16
Q

water and ethanol are ____.

A

miscible

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17
Q

water and gasoline are ____.

A

immiscible

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18
Q

gasoline and CCl4 are ____.

A

miscible

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19
Q

is non polar covalent hydrophobic or hydrophilic?

A

hydrophobic

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20
Q

are polar covalent and ionic compounds hydrophilic or hydrophobic?

A

hydrophilic

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21
Q

Are hydrocarbons polar or non polar?

A

non polar

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22
Q

polar and ionic substances dissolve best in ____.

A

polar solvents

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23
Q

non polar substances dissolve best in _____.

A

non polar substances.

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24
Q

electrolyte

A

contain ions when in an aq solution
-conduct electricity

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25
Q

non electrolyte

A

does not form ions when in an aq solution.

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26
Q

strong acids and bases do what in water?

A

completely ionizes

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27
Q

HCl is a ___ and ___.

A

strong acid, strong electrolyte

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28
Q

acetic acid is a ___ and ____.

A

weak acid (ionizes slightly), weak electrolyte

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29
Q

ionic compounds are usually ____.

A

strong electrolytes

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30
Q

ionic compound

A

ions held together by ionic bonding.

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31
Q

Hbr is a ___.

A

strong acid

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32
Q

HI is a ___.

A

strong acid

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33
Q

HNO3 is a ___.

A

strong acid

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34
Q

H2SO4 is a ___.

A

strong acid

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35
Q

HClO3 is a ____.

A

strong acid

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36
Q

HClO4 is a ___.

A

strong acid

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37
Q

NaOH is a ___.

A

strong base

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38
Q

KOH is a ___.

A

strong base

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39
Q

Ca(OH)2 is a ____.

A

strong base

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40
Q

molecular (covalent) compounds, with the exception of acids and bases, are ___.

A

nonelectrolytes

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41
Q

dissociation

A

when ionic compounds dissolve in water and the anions and cations separate from each other.

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42
Q

When acids dissolve in water the molecule ionizes into __ and ____.

A

H+, anions

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43
Q

When something is highly soluble, the original compound can still be found in small amounts.

A

true

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44
Q

Does AgCl dissolve in water?

A

only slightly, leaves white powder.

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45
Q

unsaturated solution

A

when more solute can be added to the solvent and the solute will still dissolve

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46
Q

saturated solution

A

when more solute is added than will dissolve (solubility limit has been reached)

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47
Q

Solubility

A

maximum amount of solute that will dissolve in a specific amount of solvent at a given temp. (mol/L)

48
Q

a compound is soluble than it ___.

A

dissolves in water.

49
Q

> 0.1M

A

soluble

50
Q

<0.01M

A

insoluble

51
Q

> 0.01M but <0.1M

A

partially soluble

52
Q

When two soluble solutions are mixed, they may form an insoluble compound and a ____.

A

precipitate

53
Q

Nitrate (NO3-) and acetate (C2H3O2-) are ___.

A

soluble

54
Q

Alkali metal (first row) and ammonium (NH4+) salts are ___.

A

soluble

55
Q

Most Cl-,Br-, and I- salts are ___ except __,__, and ___.

A

soluble, Ag+,Pb2+,Hg2(2+)

56
Q

most sulfates (SO42-) are ____ except __,___, and ___.

A

soluble, Ca2+,Sr2+, and Ba2+, Ag, Pb

57
Q

Most hydroxides (OH-) are ___ except

A

insoluble, Na,K, Li, NH4+

58
Q

What hydroxides are partially soluble?

A

Ba2+,Sr2+,Ca2+

59
Q

S2- is ___, unless with ___.

A

insoluble, Li,Na,K,NH4+,Ca,Sr,Ba

60
Q

CO32- is ___.

A

insoluble

61
Q

CrO42- is ____.

A

insoluble

62
Q

Cr2O72- is ____.

A

insoluble

63
Q

PO43- is ____.

A

insoluble
-except with alkali metal cations, NH4+

64
Q

soluble when combined with anions

A

Li+,Na+,K+,NH4+

65
Q

Carbonate (CO32-) and phosphate ions (PO43-) ions are usually ____ unless with ____.

A

insoluble, Li,Na, K, NH4+

66
Q

The solubility of one substance in another varies with ___ and ___.

A

temp, pressure

67
Q

For most ionic substances, solubility in water ____ as temp ____.

A

increases, increases

68
Q

The solubility of gases ___ with temperature

A

decreases

69
Q

Even insoluble solids will dissociate a little.

A

true.

70
Q

Acetic acid is a __ and ___.

A

weak electrolyte, very soluble.

71
Q

Concentration

A

amount of solute in a total volume of solution

72
Q

Molarity

A

amount of solute (mol)/volume of soln (L)

73
Q

dilution equation

A

M1V1=M2V2

74
Q

moles =

A

mass / molar mass

75
Q

combustion reaction

A

substance and oxygen reacting

76
Q

A reaction between ions in aq solution can form:

A

another solid, a gas, or a liquid

77
Q

precipitation reactions are

A

double displacement reactions

78
Q

molecular equation

A

complete chem formula with states.

79
Q

total ionic equation

A

all soluble ionic substances are represented by the ions they form in solution.

80
Q

net ionic equation

A

same as total ionic (ions) but has spectator ions removed.

81
Q

binary acids

A

acid hydrogens attached to a nonmetal atom. Ex: HCl

82
Q

oxyacids

A

acid hydrogens attached to an oxygen atom (H2SO4)

83
Q

acid produces ___.

A

H+ (A)

84
Q

bases produces ___.

A

OH- (A)

85
Q

Acid is a ___.

A

H+ donor (B-L)

86
Q

Base is a ___.

A

H+ acceptor (B-L)

87
Q

pH < 7.0

A

acid

88
Q

The molarity of H3O in the solution determines the ___.

A

pH

89
Q

two arrows in an equation represents?

A

equilibrium
-usually a weak electrolyte

90
Q

HF is a

A

weak acid

91
Q

HNO2 is a

A

weak acid

92
Q

HClO is a

A

weak acid

93
Q

CH3COOH is a

A

weak acid

94
Q

bases can be __ or ___

A

ionic or covalent

95
Q

LiOH is a

A

strong base

96
Q

NaOH is a

A

strong base

97
Q

KOH is a

A

strong base

98
Q

RbOH is a

A

strong base

99
Q

CsOH is a

A

strong base

100
Q

Ca(OH)2 is a

A

strong base

101
Q

Sr(OH)2 is a

A

strong base

102
Q

Ba(OH)2 is a

A

strong base

103
Q

NH3 is a

A

weak base

104
Q

Fe(OH)2 is a

A

weak base

105
Q

amines are ___ and they are ____.

A

molecules with C-N in them, weak bases

106
Q

pH =

A

-log[H3O+]

107
Q

[H3O+]=

A

10^-pH

108
Q

pOH=

A

-log[OH-]

109
Q

pH + pOH =

A

14

110
Q

when an acid and base are combined

A

water is formed and a salt (ionic) (neutralization reaction)

111
Q

acid/base titrations are based on

A

the neutralization reaction

112
Q

the titrant or standard solution

A

solution being added from buret

113
Q

end point (titration)

A

point in titration where there is a physical change of the solution

114
Q

indicator

A

changes physically near the equivalence point

115
Q

equivalence point (titration)

A

Chem 115 (1 decks)

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