Chapter 8

Question 1

What is a homogeneous mixture?

Answer 1

A solution that consist of 1 or more solutes uniformly dispersed at the molecular or ionic level throughout a medium known as the solvent

Question 2

What is Solute?

Answer 2

The material that got dissolved

Question 3

What is Solvent?

Answer 3

The material that does the dissolving

Question 4

The solute is the

Answer 4

Component of the solution present in the smaller quantity

Question 5

What does homogeneous mean?

Answer 5

It is NOT possible to discern phase boundaries between the components of the mixture

Question 6

What is Molarity?

Answer 6

Defined as moles of solute per liter of solution

moles/L

Calculation of volume of a solution (vol changes with freezing or heating)

CAPITAL M

Question 7

What is Molality?

Answer 7

Moles of solute per kg of solvent

Lowercase m

Mass DOES NOT change

Question 8

Volume changes when the

Answer 8

Temperature of solution changes

Question 9

Normality is

Answer 9

Molarity

Question 10

Equivalent is

Answer 10

Mole

Question 11

The solubility of a solute is the amount of the

Answer 11

Solute that will dissolve in a given amount of solvent at a given temperature

Question 12

What is a saturated solution?

Answer 12

Contains the maximum amount of a solute, as defined by its solubility

No more solute will dissolve

Question 13

What is a supersaturated solution?

Answer 13

Contains more solute than allowed by the solubility of the solute

Not stable

Excess will come out

Question 14

2 liquids are miscible if they are

Answer 14

Soluble in each other in all proportions

Question 15

Polar solutes are more

Answer 15

Soluble in polar solvents

Question 16

Endothermic reactions require

Answer 16

Energy

Question 17

What happens during exothermic reactions?

Answer 17

Energy flows out of the system in the form of heat

Question 18

Heat is the transfer of energy into or out of

Answer 18

The system caused by a difference in temperature

Question 19

endo/Exothermic reactions depend on the

Answer 19

Magnitude of the Lattice energy & heat of solution

Question 20

Solids are a

Answer 20

Lattice network

Question 21

What is lattice energy?

Answer 21

Energy required to break the lattice network

Question 22

As pressure increases, the solubility of a gas

Answer 22

Increases

Question 23

If you increases the overall pressure above a gas, you will also

Answer 23

Increase the partial pressure of each part of the gas

Question 24

Increasing the temperature will

Answer 24

Increase the solubility of solids in a liquid

Question 25

Cooling of any solution will cause

Answer 25

Precipitation

Question 26

With gases, an increase in temperature will

Answer 26

Decrease the solubility of a gas

Question 27

Some properties will depend on the

Answer 27

Identity of the solute, while others depend on the number of solute particles in the solution

Question 28

What are colligative properties?

Answer 28

The properties of a solution depends only on the number of solute particles & NOT the identity of the solute particles

Question 29

What are the 4 main Colligative properties?

Answer 29

Vapor Pressure Boiling Point Freezing Point Osmotic Pressure

Question 30

Vapor pressure results from

Answer 30

The most energetic molecule near the surface of the liquid escaping into the gas phase

Question 31

What happens as vapor pressures above a liquid increase & is closer to equilibrium?

Answer 31

Fewer molecules from the liquid escape to the gas phase

Question 32

What happens when the vapor pressure is decreased above a liquid

Answer 32

The concentration difference between the liquid & gas above the liquid causes molecules to rapidly escape

Question 33

Boiling point is defined as

Answer 33

The temperature at which the vapor pressure of the material is equal to the ambient pressure

Question 34

As more nonvolatile solutes are added, the

Answer 34

Boiling point increases

Question 35

A change in the boiling point is directly

Answer 35

Proportional to the molar concentration of the solute particles

Question 36

Freezing point is the same as

Answer 36

Melting point

Question 37

What is the definition of freezing point?

Answer 37

The temperature at which the liquid phase of the material is in equilibrium with the solid phase

Question 38

What is tonicity?

Answer 38

The relative concentrations of solutes in osmotic systems

Question 39

Colloids cannot be

Answer 39

Filtered & do not settle out of solution Particle size ranges Create osmotic pressure

Question 40

Colloid particles are

Answer 40

Large enough to scatter light passing through

Question 41

What is the Tyndall effect?