Brainscape's Knowledge GenomeTM

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


See full index

Chem > AP Chem - Chapter 11 - Solutions > Flashcards

AP Chem - Chapter 11 - 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

What is a solution

A

a homogenous mixture

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

what is the difference between a solvent and a solute

A

a solvent does the dissolving, a solute gets dissolved

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

what are the different ways to find concentration

A 
molarity
mass percent
volume percent
mole fraction
molality
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

what is the equation for molarity (M)

A

moles solute/liters solution

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

what is the equation for mass percent (%m/m)

A

mass solute/mass solution x 100

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

what is the equation for volume percent (%v/v)

A

volume solute/volume solution x 100

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

what is the equation for mole fraction (weird x)

A

moles solute/total moles

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

what is the equation for molality (m)

A

moles solute/kg solvent

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

what is the difference between molarity and molality

A

molarity changes slightly with temperature, molality doesn’t

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

what is the general rule of thumb with solubility

A

like dissolves like

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

how do you determine the polarity of a molecule

A

structure

electronegativity and bond polarity

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

what are the three steps in solution formation

A

breaking up the solute
breaking up the solvent (overcoming intermolecular forces)
allowing the solute and solvent to interact and mix

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

is breaking up the solute (step 1) endo or exothermic

A

endothermic

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

is breaking up the solvent (step 2) endo or exothermic

A

endothermic

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

is allowing the solute and solvent to interact and mix (step 3) endo or exothermic

A

exothermic

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

what is the heat of solution

A

the sum of the heat values for each step

heat of solution = heat step 1 + heat step 2 + heat step 3

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

what are the factors that affect solubility

A

structure
pressure
temperature

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

how does structure affect solubility

A

structure determines polarity, which determines solubility

polar will dissolve in polar, nonpolar in nonpolar

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

how does pressure affect solubility

A

pressure significantly increases the solubility of a gas

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

what is henry’s law

A

the amount of gas dissolved in a solution is directly proportional to the pressure of the gas above the solution

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

when does Henry’s law hold true

A

only when there is no chemical reaction between the solute and the solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

how does temperature affect solubility

A

most solids dissolve better in warm liquids

gasses dissolve better in cold liquids

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

what is thermal pollution

A

when factories use water and then put it back put its warm so gasses can’t dissolve as well in it so living things in the pond suffocate.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

when are the magnitude of the molarity and molality almost the same

A

in very dilute aqueous solutions

25
Q

what is a nonvolatile solute

A

one that has no tendency to escape from solution into the vapor phase

26
Q

how does the presence of a nonvolatile solute affect the vapor pressure of a solvent

A

it lowers it

27
Q

why will a nonvolatile solute lower the vapor pressure of a solvent

A

because the solvent is occupied with interacting with the solute, so less is available to evaporate

28
Q

what does the lowering of vapor pressure depend on

A

the number of solute particles present in the solution

29
Q

what is an ideal solution

A

a liquid to liquid solution that obeys Raoult’s Law

30
Q

in solutions where both solute and solvent are volatile, describe the vapor pressure if the solvent/solute have weak interactions (dissimilar IMFs)

A

vapor pressure will be higher than expected

31
Q

in solutions where both solute and solvent are volatile, describe the vapor pressure if the solvent/solute have strong interactions (similar, very strong IMFs)

A

Vapor pressure will be lower than expected

32
Q

what can we assume about the IMFs between the solute and the solvent when the energy of formation of solution is large and negative

A

the IMFs are strong

there will be a negative deviation from Raoult’s law

33
Q

what can we assume about the IMFs between the solute and the solvent when the energy of formation of solution is positive

A

IMFs are weaker than those among the molecules in the pure liquids
there will be a positive deviation from Raoult’s Law

34
Q

what are colligative properties

A

properties of a solution that depend only on the number, and not on the identity, of the solute particles

35
Q

How does the presence of a nonvolatile solute affect the freezing point of a solution

A

It depresses it (lowers it

35
Q

When does the normal boiling point of a liquid occur

A

At the temperature where the vapor pressure of a liquid equals exactly 1 atm

36
Q

How does a nonvolatile solute affect the boiling point of the solvent

A

It elevates it

37
Q

Why does the presence of a nonvolatile solute elevate the boiling point of the solvent

A

Because VP is lowered when we add a solute, so we need to add more energy (higher temperature) to get more solvent to evaporate so the VP will be equal to the atmospheric pressure and be able to boil

38
Q

Why does the presence of a non volatile solute lower the freezing point of the solvent

A

Solvent is busy interacting with the solute, so we have to remove even more energy to get the solvent to go from a liquid to a solid

39
Q

Why is putting salt on the roads not always effective in keeping them from freezing

A

Because if the outside temperature is lower than the freezing point of the resulting salt solution, ice forms anyway

40
Q

What is osmosis

A

The flow of solvent into the solution through the semipermeable membrane

41
Q

What is osmotic pressure

A

The pressure that must be applied to a solution to stop osmosis

42
Q

How does water tend to move/diffuse

A

From areas of high concentration to low concentration

43
Q

Why is osmotic pressure particularly useful?

A

Because a small concentration of solute produces a relatively large osmotic pressure

44
Q

What are isotonic solutions

A

Solutions that have identical osmotic pressures

45
Q

When does reverse osmosis occur

A

If a solution in contact with pure solvent across a semipermeable membrane is subjected to an external pressure larger than its osmotic pressure

46
Q

What does reverse osmosis cause

A

A net flow of solvent from the solution to the solvent

47
Q

What does the semipermeable membrane act as in reverse osmosis

A

A “molecular filter” to remove solute particles

48
Q

What does the van’t Hoff factor (little i thing) account for

A

The fact that ionic compounds ionize and produce more particles in solution

49
Q

How can you find the expected value for i

A

By noting the number or ions per formula unit (i.e. NaCl would be 2, K2SO4 would be 3, etc)

50
Q

Is the expected value of the van’t Hoff factor always what actually happens?

A

No

51
Q

Why is the expected value for the van’t Hoff factor not always true

A

Ion pairing

52
Q

What is ion pairing

A

When dissolved ions in a solution find each other swimming around and hang out for a bit and thus count as a single particle

53
Q

Why do higher concentrations of solute lead to a lower value of the van’t Hoff factor

A

There’s more of a chance for ion pairing because there is a higher concentration of ions

54
Q

A salt solution sits in an open beaker. Assuming constant temperature and pressure, the vapor pressure of the solution…

A

Decreases over time

55
Q

When is ideal behavior for a solution often observed

A

When the solute-solute, solvent-solvent, and solute-solvent reactions are very similar

56
Q

2 liquids from a solution and release a quantity of heat. How does the pressure above the solution compare to that predicted by raoult’s law?

A

It will be less

57
Q

Why will a nonpolar solute and a highly polar solvent not produce a solution (mix)

A

Because a large amount of energy would have to be expended

Chem (20 decks)

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