Ch 16: Solutions

Question 1

The ____________ of the solvent and the solute determine whether a substance will dissolve.

Answer 1

compositions

Question 2

What three things will determine how fast a substance will dissolve?

Answer 2

1. Stirring (agitation)
2. Temperature
3. Particle size

Question 3

To determine to the saturation of a solution, what do you do?

Answer 3

Add more solute.

Question 4

Saturation–add more solute: dissolves.

Answer 4

Unsaturated

Question 5

Saturation–add more solute: doesn’t dissolve.

Answer 5

Saturated

Question 6

Saturation–add more solute: triggers a reaction.

Answer 6

Supersaturated

Question 7

What has happened when equilibrium is reached and can’t hold anymore in amount of solvent at current temperature?

Answer 7

Saturated solution

Question 8

Solubility is often expressed in _____ of solute per _____ of solvent.

Answer 8

grams

100g

Question 9

What has happened when a solution can hold more solute at that temperature?

Answer 9

Unsaturated solution

Question 10

What affects the solubility of solids, liquids, and gaseous solutes in a solvent?

Answer 10

Temperature

Question 11

What two things affect the solubility of gaseous solutes?

Answer 11

Temperature and pressure

Question 12

What has happened when there are more solute particles than the solvent can hold with stability; it is unstable?

Answer 12

Supersaturated solution

Question 13

What does “like dissolves like” mean?

Answer 13

Polar dissolves polar and nonpolar dissolves nonpolar.

Question 14

What is S1 / P1 = S2 / P2?

Answer 14

Henry’s law

Question 15

What is Henry’s law?

Answer 15

S1 / P1 = S2 / P2

Question 16

There is no universal ________ _______, like there is for polar solutions (water).

Answer 16

Nonpolar solvent

Question 17

Concentration Affects Properties: the solution freezes at a _____ temperature than the _______.

Answer 17

lower

solvent

Question 18

Concentration Affects Properties: lowers the ________ _____.

Answer 18

freezing point

Question 19

Concentration Affects Properties: the ____ concentrated, the more the freezing point is ________.

Answer 19

more

reduced

Question 20

What has happened when there is less solvent than concentrated (more solvent)?

Answer 20

Dilute

Question 21

What have relatively large amounts of acids?

Answer 21

Concentrated solutions

Question 22

What have relative amounts of solvent and solute?

Answer 22

Concentrated solutions

Question 23

How is molarity related to concentration?

Answer 23

The higher the molarity, the more concentration.

Question 24

How do you calculate the molarity of a solution?

Answer 24

Moles of solute / liters of solution

Question 25

What does moles of solute / liters of solution equal?

Answer 25

Molarity (M)

Question 26

Diluting a solution _______ the number of moles of solute per ____ ______, but the total number of moles of solute in solution ____ ___ ______.

Answer 26

reduces unit volume does not change

Question 27

What is M1 X V1 = M2 X V2?

Answer 27

Moles of solute

Question 28

In what two ways can the concentration of a solution in percent be expressed?

Answer 28

1. As the ratio of the volume of the solute to the volume of the solution. 2. As the ratio of the mass of the solute to the mass of the solution.

Question 29

What properties of a solvent change when mixed with a solute?

Answer 29

Physical

Question 30

Physical property changes depend only on what?

Answer 30

The concentration of the solute, not the type of solute.

Question 31

What interferes with vaporization and crystallization?

Answer 31

Intermolecular attractions between solute and solvent particles.

Question 32

What are three important colligative properties of solutions?

Answer 32

1. Vapor-pressure lowering 2. Boiling-point elevation 3. Freezing-point depression

Question 33

Solution stays liquid over a wider temperature range when ______ is added.

Answer 33

Solute

Question 34

When solute is added, the solution freezes at a _____ temperature.

Answer 34

lower

Question 35

When solute is added, the solution boils at a ______ temperature.

Answer 35

higher

Question 36

The decrease in a solution's vapor pressure is ____________ to the number of particles the ______ makes in a solution.

Answer 36

proportional | solute

Question 37

The magnitude of the freezing-point depression is ____________ to the number of solute particles dissolved in the solvent and does not depend upon their ________.

Answer 37

proportional | identity

Question 38

The magnitude of the boiling-point elevation is proportional to the number of ______ particles dissolved in the _______.

Answer 38

solute | solvent

Question 39

The ____ ________ and ____ _________ are two additional ways is which chemists express the concentration of a solution.

Answer 39

unit molality | mole fractions

Question 40

What is a ratio of solute to solvent?

Answer 40

Molality

Question 41

Solute to solvent is more precise than ________; used to calculate __ elevation and __ depression.

Answer 41

molarity bp fp

Question 42

What is moles of solute / kilogram of solvent?

Answer 42

Molality

Question 43

What is the formula for molality?

Answer 43

moles of solute / kilogram of solvent

Question 44

What is XA =nA / nA + nB XB = nB / nA + nB?

Answer 44

Mole fraction

Question 45

The magnitudes of the freezing-point depression and the boiling-point elevation are directly proportional to the _____ concentration, when the solute is _________, not _____.

Answer 45

molal molecular ionic

Question 46

What is Kf for the freezing-depression of water?

Answer 46

1.86°C

Question 47

What is the Kb for the boiling-elevation of water?

Answer 47

0.52°C

Question 48

What is the formula for freezing-point depression?

Answer 48

∆Tf = Kf X m

Question 49

What is the formula for boiling-point elevation?

Answer 49

∆Tb = Kb X m