Chapter 13 Solutions

Question 1

Define Solution

Answer 1

A homogeneous mixture of 2 or more substances

Question 2

Define Solvent

Answer 2

The MAJOR component in a solution

Question 3

Define Solute

Answer 3

The MINOR component in a solution

Question 4

T/F In a solution, the molecules that are more present in the solution is the solvent

Answer 4

True

Question 5

Define Solution Equilibrium

Answer 5

The dissolution of a solute in a solvent is an equilibrium process

Question 6

Define Saturated Solutions

Answer 6

Dissolved solute is in dynamic equilibrium with the excess undissolved solute

Question 7

T/F In saturated solutions, additional solutes will continue to dissolve

Answer 7

False ; will not

Question 8

Where on a graph are saturated solutions located?

Answer 8

On the line

Question 9

Define Unsaturated Solutions

Answer 9

Solution containing less than the equilibrium amount of solute

Question 10

Where on a graph are unsaturated solutions located?

Answer 10

Below the curve

Question 11

Define Supersaturated Solutions

Answer 11

Solution containing more than the equilibrium amount of solute

Question 12

T/F Supersaturated solutions are unstable

Answer 12

True

Question 13

Where on a graph are supersaturated solutions located?

Answer 13

Above the curve

Question 14

T/F The solubility of most solids in water increases with increasing temperature

Answer 14

True

Question 15

T/F The solubility of gas in water increases with increasing temperature

Answer 15

False ; decreases

Question 16

The solubility of a gas depends on _____________

Answer 16

Pressure

Question 17

T/F The larger the partial pressure of a gas in contact with a liquid, the more stable the gas is in the liquid

Answer 17

True

Question 18

Define Henry’s Law

Answer 18

States that the solubility of gas (S gas) is directly proportional to its partial pressure (P gas)

Question 19

Define Solubility

Answer 19

The amount of the substance that will dissolve in a given amount of solvent

Question 20

T/F For solids when temperature increases, solubility increases

Answer 20

True

Question 21

T/F For gas when temperature increases solubility increases

Answer 21

False ; decreases

Question 22

T/F For gas when pressure increases solubility increases

Answer 22

True

Question 23

Define Concentration

Answer 23

The amount of solute in a given amount of solution/solvent

Question 24

Is Molarity or Molality dependent on temperature?

Answer 24

Molarity

Question 25

T/F Molarity depends on volume

Answer 25

True

Question 26

What is the equation for Molarity?

Answer 26

Molarity (M) = amount of solute (mol) / volume solution (L)

Question 27

What is the equation for Molality?

Answer 27

Molality (m) = amount of solute (mol) / mass solvent (kg)

Question 28

What is the equation for Mole Fraction?

Answer 28

Mole Fraction (x solute) = amount of solute (mol) / solute + solvent (mol)

Question 29

What is the equation for Percent by Mass?

Answer 29

Percent by Mass = mass of solute / mass of solution X 100%

Question 30

Define Colligative Properties

Answer 30

Properties that depend on the amounts of particles dissolved in solution, not on the type of particle

Question 31

The number of ________ ____________ determines its vapor pressure

Answer 31

Gaseous particles

Question 32

More solute results in increased or decreased vapor pressure

Answer 32

Decreased

Question 33

What is the equation for Raoult's Law?

Answer 33

Psolution = x solvent X P solvent

Question 34

How do you find x solvent in Raoult's Law?

Answer 34

Use mol fraction

Question 35

What is the equation for Boiling Point Elevation?

Answer 35

DeltaTb = m X Kb

Question 36

Define Boiling Point Elevation

Answer 36

The effect of a solute that causes a solution to have a higher boiling point than the pure solvent alone

Question 37

Define Freezing Point Depression

Answer 37

The effect of a solute that causes a solution to have a lower freezing point than the pure solvent alone

Question 38

What is the equation for Freezing Point Depression?

Answer 38

DeltaTf = m X Kf

Question 39

Define Osmosis

Answer 39

The flow of solvent from a solution of lower solute concentration to one of higher solute concentration

Question 40

Define Osmotic Pressure

Answer 40

The pressure required to prevent the net movement of solvent across a semipermeable membrane

Question 41

What is the equation for Osmotic Pressure?

Answer 41

Pi = MRT

Question 42

Define Electrolyte

Answer 42

Substance that dissociates into ions to conduct electricity when dissolved in water

Question 43

Define Non-Electrolyte

Answer 43

A compound that DOES NOT dissociated into ions when dissolved in water

Question 44

What i value will non-electrolytes always have?

Answer 44

i = 1

Question 45

Define Van't Hoff Factor

Answer 45

(i) the ratio of moles of particles in solution to moles of formula units dissolved

Question 46

Does boiling point decrease or increases when more solute is added?

Answer 46

Increases

Question 47

T/F The presence of a solute could hinder a particle from entering another phase

Answer 47

True

Question 48

What are the 4 colligative properties?

Answer 48

- Vapor pressure - Freezing point depression - Boiling point elevation - Osmotic pressure

Question 49

What is the equation for Henry's Law?

Answer 49

S(gas) = Kh X P(gas)