Brainscape's Knowledge GenomeTM

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


See full index

chemistry > unit 8 - solutions > Flashcards

unit 8 - solutions Flashcards

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

solution

A

A homogeneous mixture of two
or more substances

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

solutions contain…

A

particles of one substance that are uniformly spread out in another substance
ex: C6H12O6 (aq)

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

parts of a solution

A

solute and solvent

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

solute

A

the substance being dissolved

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

solvent

A

the substance that dissolves the solute

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

solution types - aqueous

A

water is the solvent

ex: NaCl (aq)
solute (NaCl), solvent (water)

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

solution types - non aqueous

A

water is not the solvent

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

solution types - tincture

A

alcohol is the solvent

ex: tincture of iodine
contains solute (I2), solvent (alcohol)

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

solution characteristics

A

1) Clear or transparent- colorless or colored

2) Particles:
a. Are evenly distributed
(Solutions are homogeneous)
b. Do not settle out on standing
(particles dissolved stay dissolved)
c. Can not be separated by filtration

3) Variable Composition- A solution is a type of mixture, not a pure substance (compound)

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

solubility

A

the amount of a solute to dissolve in a certain amount of solvent

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

soluble

A

materials with a high degree of solubility (a lot dissolves)

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

insoluble

A

materials with a low degree of solubility (little dissolves)

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

factors that affect solubility: TEMPERATURE (Table G)

A

1) TEMPERATURE: (Table G)
- As temp increases solids become more soluble
- As temp increases gases become less soluble in water

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

factors that affect solubility: pressure

A

2) PRESSURE:
- Pressure has little or no affect on the solubility of solid or liquid solutes
- As pressure increases gases become more soluble in liquids

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

factors that affect solubility: type of solvent/solute

A

3) Type of Solute/Type of Solvent:

  • “Like Dissolves Like”
  • Polar Solutes dissolve in Polar solvents
  • Non-Polar solute dissolve in non-polar solvents.
  • Ionic Substances dissolve in Polar
    solvents (salts in water)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

rate of solute dissolving

A

how fast a solute dissolves depends on frequency of interactions between solute and solvent

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

factors that affect rate of solute dissolving

A

1) temperature - greater KE = more interactions
2) stirring - more interactions
3) surface area - grinding and chopping solute into pieces increases surface exposure and more interaction with solvent

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

double replacement reactions and table F

A
  • Double Replacement Reactions:
    Two compounds that react and produce a precipitate. Precipitate is the INsoluble Product!
  • Ex: Silver Nitrate (aq) + Sodium Chloride (s)
    : AgNO3 (aq) + NaCl (aq) → AgCl (s) + NaNO3(aq)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

three degrees of saturation

A
  • saturation solution
  • unsaturated solutions
  • supersaturated solution
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

saturated solutions

A

solution which contains the maximum amount of solute that can dissolve in a given amount of solvent at a certain temp.

  • point is given on the curve
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

unsaturated solutions

A

solution that contains less than the maximum amount of solute that can dissolve at a certain temperature in a given amount of solvent
- point given is below the curve

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

supersaturated solution

A

Solution that contains more than the maximum amount of solute than can dissolve (unstable), at a
certain temperature in a certain amount of solvent
- point given is above the curve

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

measuring concentration by percent

A

% By Mass = mass of solute/mass of solution x 100

% By Volume = volume of solute/volume of solution x 100

24
Q

1 PPM

A

= .0001%

25
Q

PPM

A

expresses concentration as the mass of the solute in given amount of solution

PPM = mass solute/mass solution x 1,000,000

26
Q

evaporation

A

molecules on the surface of a liquid gain enough KE to break from the liquid and enter the gas phase

ex: water on the floor or open container evaporates

27
Q

boiling

A

liquid turns to a gas at any point in the container (not just the surface)

28
Q

vapor

A

another word for gas phase

29
Q

vapor pressure

A

the pressure that gas particles exert due to collisions above surface of a liquid

30
Q

vapor pressures varies directly with…

A

TEMPERATURE regardless of the volume

31
Q

boiling point

A

Temperature at which the Vapor pressure is equal to Atmospheric Pressure

*At standard pressure - Normal Boiling Point
*low atmospheric pressure - above sea level
*high atmospheric pressure- below sea level

32
Q

normal boiling point

A

temperature at which the vapor pressure exerted by the liquid is equal to Standard Atmospheric Pressure

1 atm, 101.3 Kpa, 760 torr or mmHg

33
Q

temperature and vapor pressure

A

as temperature increases so does the vapor pressure of a liquid

34
Q

table H - remember boiling point

A

the temperature at which the vapor pressure equals 101.3 kPa

35
Q

diluted solution

A

solution in which a small amount of solute in a given amount of water

less solute, more water

36
Q

concentrated solution

A

solution which a large amount of solute in a given amount of water

more solute, less water

37
Q

how do we build a solution

A

1) put salt in flask
2) add total amt of H2O needed in the problem

38
Q

molarity

A

the concentration of a solution in moles of solute per liter of solution

39
Q

to get L from mL

A

do mL/1000

40
Q

as molarity increases, what happens to solution concentration

A

solution is more concentrated

41
Q

how can we change the concentration (molarity) of a solution by perfoming a dilution

A

add water to change a higher concentration to a lower concentration

42
Q

moles of a substance before dilution are …

A

equal to the moles of a substance after dilution

43
Q

steps to performing a dilution

A
  1. find V1
  2. fint amount of H2O to dilute (V2-V1 = amt of water)
  3. put water into flask first, then add concentrated soution
44
Q

colligative properties

A

when you take a pure substance, (ex. water), and add any other substance to it, you affect the original substance’s boiling point and freezing point

45
Q

concentration of dissolved particles impacts the

A

boiling point and freezing point of a substance

46
Q

as concentration increases

A

the more moles of particles of the solute exist

(remember we measure concentration in (M) molarity)

47
Q

the greater the concentration or more solute particles, original substance will have its freezing and boiling point…

A

boiling point increased, freezing point decreased

48
Q

no matter what is added to a substance, the response will always be the

A

SAME

49
Q

colligative properties conclusions: boiling point…? why?

A

increases

It takes a higher temp (greater Kinetic Energy) for the
appropriate collisions to occur between the gas particles in order to break intermolecular bonds

50
Q

colligative properties conclusions: freezing point…? why?

A

decreases

It takes a lower temp (lower KE) for all the liquid particles to come together to form intermolecular bonds and become a solid.

51
Q

do ionic substances dissociate into +/- ions?

A

YES

52
Q

do covalent substances (molecules) dissociate into +/- ions?

A

NO

53
Q

which will always produce more moles of particles compared to the other

A

IONIC substances will always produce MORE moles of particles compared to COVALENT substances

Ex. 1 Mole NaCl → 1 mol Na+ + 1 mol Cl-
(total is 2 mol of particles)

Ex. 1 Mole C6H12O6 → 1 mol C6H12O6

54
Q

the higher the boiling point, the ____ the substances vapor pressure

A

lower

55
Q

the lower the boiling point, the _____ the substances vapor pressure

A

higher

chemistry (11 decks)

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