Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Test 12 > Flashcards

Test 12 Flashcards

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

Homogeneous mixtures of variable composition in a single phase

A

Solutions

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

The most abundant substance in a solution

A

Solvent

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

Dissolved substances in a solution

A

Solute

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

A solution containing mercury

A

Amalgam

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

What is the only permanent gas solution at ordinary pressures

Why

A

Gaseous solvents dissolve and gaseous solutes.

Gases cannot dissolve liquid or solid particles because gas particles are so much smaller than liquid or solid particles

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

What is the governing principle in solutions

A

Like dissolves like

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

What is the maximum amount of a solute that can dissolve in a specific solvent under specific conditions, such as temperature and pressure

A

Solubility

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

What accounts for the different solubility

A

The strength of ionic attractions within compounds

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

Are supersaturated solution stable

A

No

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

What can affect the frequency of collisions with solvent particles

A

Temperature, stirring, and the amount of surface area of the solute exposed to the solvent

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

The escape of a gas from a liquid gas solution

A

Effervescence

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

What are the most common ways to express concentration

A

Percent by mass, molarity, and molality

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

What is the formula for percent by mass

A

Percent by mass =

(mass of solute/mass of solution) x100%

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

What is the formula for percent by volume

A

Percent by volume = (volume of solute/volume of solution) x100%

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

What’s the formula for molarity

A

Molarity (M) = mol solute/L solution

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

What four things change because of the presence of solutes instead of just a pure solvent

A

Freezing points
Boiling points
Vapor pressures
Osmotic pressures

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

The more concentrated a solution is, the___ the boiling point elevation will be

A

Greater

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

Solutions freeze at___temperatures than their pure solvents

A

Lower

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

What is osmotic pressure of a solution

A

The amount of pressure required to prevent osmosis from occurring

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

Why is osmotic pressure of a solution a colligative property

A

Because it depends on the number of particles in a solution

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

Why should the solution surrounding a cell be kept at the same osmotic pressure as a solution inside the cell

A

If the equilibrium is disturbed, water could leave the cell in sufficient quantities and cause dehydration
OR water could enter the cell and cause the membrane to burst

22
Q

What happens if a cell is placed in a hypertonic solution

A

Water will flow out of the cell into the surrounding solution

23
Q

What happens if a cell is placed in a hypotonic solution

A

Water will flow into the cell, causing it to swell and possibly burst

24
Q

What is isotonic

A

When concentrations on both sides of the membrane are equal

25
Q

Mixtures that contain larger particles that will eventually settle out of the mixture

A

Suspension

26
Q

Fog is a__

A

Colloid

27
Q

What phases can a colloid exist in

A

Solids, liquids, and gases

28
Q

Can a gas/gas colloid exist why or why not

A

No, they are always solutions

29
Q

List three types of colloids

A

Foams
Aerosols
Gels

30
Q

Completely describe the three steps involved in practical water treatment

A

1- pathogens are killed by chlorinating the water with chlorine dioxide or similar compounds

2- other compounds are added to clump impurities together causing coagulation

3- The water is passed through a filter under pressure to quickly remove impurities

31
Q

Gas/gas is

A

Only a solution

32
Q

What keeps particles smaller than 1000 nm in colloids from setting out

A

Intermolecular collisions

33
Q

M=

A

Mol/L

34
Q

K(b)

A

Molal boiling point

35
Q

Delta T(b)

A

The CHANGE in boiling point NOT The new boiling point!

ADD original to get new one

36
Q

Pertaining to two liquids that are not soluble in each other

A

Immiscible

37
Q

The process in which solvent particles surround and interact with solutes

The dissolving process in
solid-in-liquid solutions

A

Solvation

38
Q

A type of solvation in which water molecules surrounded interact with solute particles

A

Hydration

39
Q

A type of solvation in which an ionic compound forms ions when it dissolves in a solvent

A

Dissociation

40
Q

A type of solvation in which a covalent compound forms ions when it dissolves in a solvent

A

Ionization

41
Q

The inability of a solute to dissolve in a certain solvent

A

Insoluble

42
Q

A chemical equilibrium in which two or more opposing events occur at the same rate that results in no net change

A

Dynamic equilibrium

43
Q

A quantitative measure of concentration equal to the number of moles of solution per kilogram of solvent

A

Molality (m)

44
Q

A physical property of a solution that depends only on the number of solute particles present without regard to type

A

Colligative property

45
Q

A number that relates the change in boiling point of a particle solvent to the concentration of solute particles

A

Molal boiling point constant K(b)

46
Q

The diffusion of pure solvent molecules, such as water, through a semi permeable membrane

A

Osmosis

47
Q

A mixture of small particles that remain dispersed in a medium

A

Colloid

48
Q

In a colloidal mixture, the phase in which the particles are spread out

A

Dispersed phase

49
Q

The scattering of light by particles in a colloid

A

The Tyndall effect

50
Q

The random, chaotic movements of microscopic particles

A

Brownian motion

Chemistry (32 decks)

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