Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

chem > DAT Gen Chem Solutions > Flashcards

DAT Gen Chem Solutions Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

has less than the maximum amount of solute
dissolved in a solvent.

A

unsaturated soln

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

maximum amount of
solute dissolved in a solvent.

A

saturated soln

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

contain even more dissolved solute than
they can normally hold at a given temperature
and pressure.

A

supersaturated soln

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

when a dissolved solute
comes out of the solution.

A

crystalization

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

These crystals are
generally formed by

A

manipulating temp or pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Group 1 metal cations, what kind of salt

A

soluble salt

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Ag+, what kind of salt

A

insoluble salt

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

No3- what kind of salt

A

soluable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

ClO4- what kind of salt

A

solable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

C2H3O2- what kind of salt

A

soluble

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

NH4+, what kind of salt

A

soluble

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Pb2+, Hg2+ what kinda salt

A

insoluble

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Oh- what kinda salt

A

insoluble

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

S2- what kinda salt

A

insoluble

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

CO3 2-, PO4 2-

A

insoluble

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

soluble component generally

A

trumps insoluble component

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

HCl, HBr, HI, HClO4, HClO3,
H2SO4, HNO3.

A

strong acids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Group I Metal Hydroxides,
Ca(OH)2, Sr(OH)2, Ba(OH)2.

A

strong bases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

HF, HCN, CH3COOH, etc.

A

weak acids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

NH3, CH3NH2, etc.

A

weak bases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Solids are more soluble at what temps

A

higher

22
Q

Gases are more soluble at what temps

A

lower

23
Q

Gases are more soluble at what pressures

A

higher

24
Q

For solids in liquids, an “blank” in tempting solubilty

A

incresae

25
Q

method that measures
how much a chemical substance absorbs light
by measuring the intensity of light as a beam of
light passes through a sample solution.

A

spectrophotometry

26
Q

following formula illustrates Beer’s law: (absorbance)

A

absorbance = molar absorptivity x path length x conc of soln

27
Q

unit for molar absorptivity

A

M-1*cm-1

28
Q

are the
attractive and repulsive forces between
separate molecules.

A

intermolecular forces

29
Q

arise from the
temporary attraction between adjacent atoms
or molecules.

A

LDF

30
Q

dilution formula

A

m1v1=m2v2

31
Q

concentration in terms of
the equivalents of one chemical species that
reacts stoichiometrically with another chemical
species.

A

normality (N)

32
Q

Normality eqn

A

N=number of equivalents x molarity

33
Q

ratio of the number of
moles of one component of a mixture to the
total number of moles.

A

mole fraction (X)

34
Q

mole fraction of solute =

A

moles of solute/total moles in soln

35
Q

depend upon the
concentration of solute molecules or ions, but
not upon the identity of the solute itself.

A

colligative properties

36
Q

depend on the identity of the dissolved species
and solvent.

A

noncolligative properties

37
Q

property of a liquid
that allows it to resist an external force due to
the cohesive nature of its molecules.

A

surface tension

38
Q

is surface tension colligative or non colligative

A

non colligative

39
Q

the attractive forces
between molecules of the same substance,

A

cohesive

40
Q

attractive forces
between molecules of different substances.

A

adhesive forces

41
Q

measure of a fluid’s resistance
to flow.

A

viscocity

42
Q

is viscosity a colligative or non colligative property

A

non colligative

43
Q

are color and density colligative or non colligative

A

non colligativeis

44
Q

is solubility colligative or non colligative

A

non colligative

45
Q

which is the point
where the vapor pressure equals the
atmospheric pressure.

A

boiling pti

46
Q

is boiling pt colligative or non colligative

A

colligative

47
Q

as vapor pressure increases, boiling
point….

A

decreases

48
Q

The vapor pressure of a pure solvent is… than the vapor pressure of a solution containing
non-volatile solutes.

A

greater than

49
Q

calculate the new vapor pressure after a
solute has been added, use Raoult’s law:

A

VP of soln after solute has been added = mole fraction x pure VP

50
Q

change in boiling point temperature can be
calculated using the following formula:

A

change in temp = solvents BP elev constant x solute vant hoff factor x molality

51
Q

The change in freezing point temperature can
be calculated using the following formula:

A

change in temp = - FP depression constant x vant hoff factor x molality

52
Q

The osmotic pressure can be calculated using
the following formula:

A

osmotic pressure = vant hoff factor x molarity x universal gas constant x temp (K)

chem (12 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions