Mcat Chemistry Lecture 4

Front 1

____ - a homogeneous mixture of two or more compounds in a single phase

Back 1

Solution

Front 2

Brass is a solid ____ (____ are not always liquid)

Back 2

solution
solutions

Front 3

Saltwater - salt is ____ and water is the ____

Back 3

solute
solvent

Front 4

Mix two liquids, both can be called ____, but typically the dominating one is the ____ - the name does not change its behavior though

Back 4

solvents
solvent

Front 5

3 types of solutions

Back 5

Ideal solutions
Ideally dilute solutions
Non-ideal solutions

Front 6

____ - bonds between solvent and solute are similar to bonds w/in the solvent and solute and the molecules in the solvent and solute are similar size

Back 6

Ideal solution

Front 7

____- so dilute that the solute molecules are completely separated from each other and do not interact with each other

Back 7

Ideally dilute

Front 8

____- neither ideal no ideally dilute

Back 8

Non-ideal

Front 9

____ - when the solute particles are large, or conglomerates of particles - (most of the time gravity pulls large particles out - if it doesn’t then this is a ____ or a ____)

Back 9

Colloid
colloid
colloidal suspension

Front 10

____ - beam of light is scattered, so can see it from the side - cause by the ____.

Back 10

Tyndall effect
colloid

Front 11

Colloidal particles cannot be extracted by ____.

Back 11

filtration

Front 12

____ or adding an ____ may cause particles to coagulate, these can then be filtered out or may settle out due to gravity.
A semi permeable membrane may also separate particles - ____.

Back 12

heating
electrolyte
dialysis

Front 13

When a solute is mixed into a solution it is said to ____ or ____.

Back 13

dissolve
solvate

Front 14

Generally ____ solvents dissolve ____ solutes and
____ solvents dissolve ____ solutes.

Back 14

polar
polar
nonpolar
nonpolar
(like dissolves like)

Front 15

If a compound forms ions in a solution it is called an ____.

Back 15

electrolyte

Front 16

____ solutions containing electrolytes conduct ____.

Back 16

aqueous
electricity

Front 17

____, Reason this is so is the electrostatic forces created between the polar molecules are too strong to be broken by the ____ molecules.

Back 17

like dissolves like
non-polar

Front 18

When something ____, solvent molecules surround each ____ molecule.

Back 18

solvates
solute

Front 19

If the solvent is water this process is called ____ and the surrounding molecules make up the ____.

Back 19

hydration
hydration shell

Front 20

A compound with a hydration shell is said to be in ____.

Back 20

aqueous phase

Front 21

The number of water molecules required to surround an ion is called its ____.
The ____ varies according to the size or charge of the molecule it is commonly ___ or ____.

Back 21

hydration number
hydration number
4
6

Front 22

Nitrite -

Back 22

NO21-

Front 23

Nitrate -

Back 23

NO31-

Front 24

Sulfite -

Back 24

SO32-

Front 25

Sulfate -

Back 25

SO42-

Front 26

Hypochlorite -

Back 26

ClO1-

Front 27

Chlorite -

Back 27

ClO21-

Front 28

Chlorate -

Back 28

ClO31-

Front 29

Perchlorate -

Back 29

ClO41-

Front 30

Carbonate -

Back 30

CO32-

Front 31

Bicarbonate -

Back 31

HCO31-

Front 32

Phosphate -

Back 32

PO43-

Front 33

____ properties are properties that depend on number, not kind.

Back 33

Colligative

Front 34

Molarity - ____ (fluctuates w/ temperature)

Back 34

moles of solute / total volume of solution

Front 35

Molality - ____ (does not fluctuate w/temp)

Back 35

moles of solute / kg of solvent

Front 36

Mole fraction - ____

Back 36

moles of solute / total moles of solution

Front 37

Mass percent = ____

Back 37

100* mass of solute/ total mass of solution

Front 38

Ppm = ____

Back 38

1 million * mass of solute/ total mass of solution

Front 39

Normality = ____

Back 39

number of equivalents / liter of solution.

Front 40

How a solution forms

Back 40

Step 1:
Some solvent-solvent bonds are broken
Step 2:
Some solute-solute bonds are broken
Step 3:
Solvent-solute bonds are formed

Front 41

____ - vapor pressure of a solution with a non-volatile solute = the mole fraction of the solvent times the vapor pressure of the pure solvent

Back 41

Raoults law

Front 42

____ - The pressure created by the molecules in the space above the liquid. (closed system etc etc)

Back 42

Vapor pressure

Front 43

Vapor pressure increases as ____.

Back 43

temperature increases

Front 44

____ - solute has little or no vapor pressure (like the solid salt) - they block solvent from escaping due to just being there at the surface etc…

Back 44

Non volatile

Front 45

w/ ____ (means it can escape too)
Total vapor pressure of the solution equals the mole fraction of the solvent times the vapor pressure of the pure solvent plus the mole fraction of the solute times the vapor pressure of the pure solute

Back 45

volatile solute

Front 46

____ does not consider the forces between the molecules-

Back 46

Raoults law

Front 47

If heat of solution is ____ - have a ____ from raoults law, prediction is too high

Back 47

negative
negative deviation

Front 48

If heat of solution is ____ - vapor pressure prediction by raoults law is too low

Back 48

positive

Front 49

A solution that follows Raoults law exactly is called an ____

Back 49

ideal solution.

Front 50

____ - is a compounds tendency to dissolve in a solvent

Back 50

Solubility

Front 51

____ - some of the dissolved solute reattaching to the solid

Back 51

Precipitation

Front 52

____ - two dissolved solute molecules attaching to each other

Back 52

Ion pairing

Front 53

____ - dissolution and precipitation have equilibrated, for a solution to be saturated some solid must exist.

Back 53

Saturated

Front 54

The ____ of a compound is the amount of that compound dissolved in a given volume of a saturated solution.

Back 54

solubility

Front 55

Some ____ occurs in any ionic solution independently of the solid.

Back 55

ion-pairing

Front 56

Solubility product is the ____

Back 56

Ksp constant

Front 57

For a solid solute the Ksp does not change for a ____

Back 57

given temperature.

Front 58

This is a constant that is specific for a specific solute and solvent, typically in ____.

Back 58

aqueous solution.

Front 59

As temperature goes up, ____ dissolve and ____ leave solution

Back 59

solids
gases
(rock candy and can of soda blowing up example)

Front 60

____ does not affect solubility of solid or liquid much, but has a large effect on the solubility of ____.

Back 60

Pressure
gases

Front 61

For an ideally dilute solution of gas and water, the ____ of the gas is directly proportional to the ____.

Back 61

solubility
pressure

Front 62

Henrys law,

Back 62

c = K*p
C is the solubility
K is henry's law constant, which varies for different gases
P is the pressure
(think of this as a can of soda, when can is popped the pressure drops and the gas is released)

Front 63

The water solubility of most solids ____ with temperature, because the entropy of solution making is so large, the solubility of gases though typically ____ with temperature.

Back 63

increases
decreases