Chapter 12 Physical Properties Of Solutions

Front 1

Solution

Back 1

A homogenous mixture of two or more substances

Front 2

Saturated Solution

Back 2

contains the maximum amount of a solute that will dissolve in a given solvent at a specific temperature

Front 3

unsaturated solution

Back 3

contains less solute than it has the capacity to dissolve

Front 4

superstaurated solution

Back 4

contains more solute than is present in a saturated solution

Front 5

What are some properties of superstaurated solutions?

Back 5

-not very stable
-some solute comes out as crystals

Front 6

A gas and a gas results in ______?

Back 6

A gas

Front 7

A gas and liquid results in ______?

Back 7

A liquid

Front 8

A gas and solid results in _______?

Back 8

A solid

Front 9

A liquid and liquid results in ______?

Back 9

A liquid

Front 10

A solid and liquid results in ______?

Back 10

A liquid

Front 11

A solid and solid results in ______?

Back 11

A solid

Front 12

Crystallization

Back 12

The process in which dissolved solute somes out of solution and forms crystals

Front 13

What are the 3 types of Interactions?

Back 13

1. solvent-solvent interaction
2. solute-solute interaction
3. solvent-solute interaction

Front 14

What is the strongest interaction?

Back 14

solute-solvent interaction

Front 15

if a solute-solvent interacton is greatest, exp or endo?

Back 15

exo

Front 16

Solution

Back 16

A homogenous mixture of two or more substances

Front 17

Saturated Solution

Back 17

contains the maximum amount of a solute that will dissolve in a given solvent at a specific temperature

Front 18

unsaturated solution

Back 18

contains less solute than it has the capacity to dissolve

Front 19

superstaurated solution

Back 19

contains more solute than is present in a saturated solution

Front 20

What are some properties of superstaurated solutions?

Back 20

-not very stable
-some solute comes out as crystals

Front 21

A gas and a gas results in ______?

Back 21

A gas

Front 22

A gas and liquid results in ______?

Back 22

A liquid

Front 23

A gas and solid results in _______?

Back 23

A solid

Front 24

A liquid and liquid results in ______?

Back 24

A liquid

Front 25

A solid and liquid results in ______?

Back 25

A liquid

Front 26

A solid and solid results in ______?

Back 26

A solid

Front 27

Crystallization

Back 27

The process in which dissolved solute somes out of solution and forms crystals

Front 28

What are the 3 types of Interactions?

Back 28

1. solvent-solvent interaction
2. solute-solute interaction
3. solvent-solute interaction

Front 29

What is the strongest interaction?

Back 29

solute-solvent interaction

Front 30

if a solute-solvent interacton is greatest, exp or endo?

Back 30

exo

Front 31

if a solute-solvent interaction is weak, exo or endo?

Back 31

endo

Front 32

what determines if a solution is exo or endo?

Back 32

Energy

Front 33

Randomness or Disorder

Back 33

There is an increase in randomness or disorder when a solute and solvent molecule is mixed to form a solution

Front 34

Solubility

Back 34

A measure of how much solute will dissolve in a solvent at a specific temperature

Front 35

"like dissolves like"

Back 35

two substances with intermolecular forces of similar type and magnitude are likely to be soluble in eachother

Front 36

miscible

Back 36

two liquids are miscible if they are completely soluble in eachother in all proportions

Front 37

solvation

Back 37

the process in which an ion or a molecule is surrounded by solvent molecules arranged in a specific manner

Front 38

hydration

Back 38

when water is the solvent

Front 39

concentration

Back 39

amount of solute present in a given amount of solution

Front 40

4 most common units of concentration

Back 40

1. percent by mass
2. mole fraction
3. molarity
4. molarity

Front 41

percent by mass

Back 41

percent by weight/weight percent
the ratio of the mass of a solute to the mass of a solution multiplied by 100

%by mass=mass of solute/mass of solution x 100

Front 42

mole fraction (x)

Back 42

Xa=moles of A/sum of all components
(no units)

Front 43

Molarity (M)

Back 43

molarity=moles of solute/liters of solution

Front 44

molality (m)

Back 44

the number of moles of solute dissolved in 1kg of solvent

molality-moles of solute/mass of solvent(kg)

Front 45

solubility of a substance increases with _______.

Back 45

Temperature

Front 46

Fractional Crystallization

Back 46

the seperation of a mixture of substances into pure components on the basis of their differing solubilities

Front 47

Henry's Law

Back 47

Reltionship betwen gas solubility and pressure
the solublty of a gas in a liquid is proportional to the pressure of the gas over a solution

Front 48

What is the equation for Henry's Law

Back 48

C=KP

Front 49

The amount of gas that will dissolve in a solvent is dependant upon what?

Back 49

How frequently the gas molecules collide

Front 50

Colligative Properties

Back 50

depend only on the number of solute particles in a solution and not on the nature of the solute particles

Front 51

What are four colligative properties?

Back 51

1. Vapor Pressure Lowering
2. Boiling POint Elevating
3. Freezing Point Depression
4. Osmotic Pressure

Front 52

Nonvolatile

Back 52

does not have a measurable vapor pressure
the vapor pressure of its solution is always less than that of the pue solvent

Front 53

Raoults Law

Back 53

the partial pressure of a solvent over a solution, P1, is given by the vapor prssue of the pure solvent p1*, times the mole fraction of the solent in the solution, x1

p1=x1p1*

Front 54

vapor pressure of a solution is less that that of a ________.

Back 54

solvent

Front 55

ideal solution

Back 55

any solution that obeys Raoults Law

Front 56

Fractional Distillation

Back 56

a procedure for seperating liquid components of a solution based on their different boiling points

Front 57

Boiling Point

Back 57

The temperature at which a solutions vapor pressure equals the external atmospheric pressure

Front 58

Boiling point elevation (Change in Tp)

Back 58

the boiling point of the soluton (Tp) minus the boiling point of the pure solvent (Tb)

Front 59

Freezing Point Depression (Change in Tf)

Back 59

the freezing point of the pure solvent minus the freezing point of the solution

Front 60

Equation for Boiling Point Elevation

Back 60

Change in T = Kbm

Front 61

Equation fo Freezing Point Depression

Back 61

Change in Tf = Kfm

Front 62

Osmosis

Back 62

The selective passage of solvent molecules through a poros membrane from a dilute solution to a more concentrated one

Front 63

semi-permeable membrane

Back 63

allows the passage pf solvent molecules but blocks the passage of solute molecules

Front 64

osmotic pressure

Back 64

pressure required to stop osmosis, measures directly from the difference of final fluid levels

Front 65

equation for osmotic pressure

Back 65

pie=mrt

Front 66

isotonic

Back 66

when solutions ar of equal concentration ad have the same osmotic pessure

Front 67

hypotonic

Back 67

more dilute solution

Front 68

freezing point depression and osmotic pressure are used to find ______.

Back 68

molar mass

Front 69

Van't Hoff Factor

Back 69

i= actual number of particles in sol'n after dissociation/#of formula units intilyy dissolved in soln

Front 70

ion pair

Back 70

made up of one or more cations and one or more anions held together by electrostatc forces

Front 71

colloid

Back 71

a dispersion of particles of one substance throughout dispesing medium made of another substance

Front 72

tyndall effect

Back 72

distinguish a solution from a colloid
> beam of light in colloid, dispersed pahse

Front 73

hydrophilic

Back 73

water loving

Front 74

hydrophobic

Back 74

water fearing

Front 75

adsorption

Back 75

adherance onto a surface