Chapter 13 solutions

Question 1

Solution

Answer 1

A homogeneous mixture of two or more substances

Question 2

Solvent

Answer 2

The component of a solution that is present in greatest amount

Question 3

Solute

Answer 3

A component of a solution that is present in a lesser amount

Question 4

Soluble

Answer 4

A compound is soluble if it dissolves in a solvent

Question 5

Insoluble

Answer 5

A compound is insoluble if it does not dissolve in a solvent.

Question 6

Miscible

Answer 6

Two substances that are soluble in all proportions are miscible

Question 7

Dilute Solution

Answer 7

A solution that contains a low quantity of solute

Question 8

Concentrated Solution

Answer 8

A solution that contains a high quantity of solute

Question 9

Unsaturated solution

Answer 9

Solution that holds less than the maximum amount of solute possible

Question 10

Saturated solution

Answer 10

Solution that holds the maximum amount of solute possible

Question 11

Supersaturated solution

Answer 11

A solution that holds more than the amount of solute possible

Question 12

Ion-Dipole Force

Answer 12

Intermolecular force between an ion and a polar molecule.

Question 13

Henry’s law

Answer 13

Solubility of a gas is directly proportional to the pressure of the gas above the liquid

Question 14

Like Dissolves Like

Answer 14

General rule to predict the solubility of molecular compounds. Polar solutes
dissolve in polar solvents, and non-polar solutes dissolve in non-polar solvents.

Question 15

Concentration

Answer 15

Describes the amount of solute in a solution.

Question 16

Molarity

Answer 16

The number of moles per liter of solvent. Often used as a conversion factor to convert
between volume and moles

Question 17

Molality

Answer 17

The number of moles per kilogram of solvent

Question 18

Mole fraction

Answer 18

The number of moles of a solute divided by the total number of moles in a solution

Question 19

Percent concentration

Answer 19

Solute divided by solution, multiplied by 100

Question 20

Parts per million (ppm)

Answer 20

Solute divided by solution, multiplied by 1 million (10^6)

Question 21

Parts per billion (ppb)

Answer 21

Solute divided by solution, multiplied by 1 billion (10^9)

Question 22

Dilution

Answer 22

The process of adding solvent to decrease the concentration of a solution

Question 23

Electrolyte solution

Answer 23

Solution that conducts electricity

Question 24

Electrolyte

Answer 24

A substance that conducts electricity when dissolved in water

Question 25

Non-Electrolyte

Answer 25

A substance that does not conduct electricity when dissolved in water

Question 26

Colligative properties

Answer 26

Properties that depend on the number of particles dissolved in a solution, and not the identities of the particles themselves

Question 27

Ion pairing

Answer 27

Cations and anions get close enough to each other to effectively pair. This lowers the concentration of particles below what is expected from the complete dissociation of ionic compounds

Question 28

van’t Hoff Factor

Answer 28

The ratio between the amount of particles produced and the amount of solute dissolved. In this class, we assume all solutions are ideal solutions and ion pairing does not occur.

Question 29

Freezing Point Depression

Answer 29

Solutes cause the freezing point of a solution to be lower than that of the pure solvent

Question 30

Boiling Point Elevation

Answer 30

Solutes cause the boiling point of a solution to be higher than that of the pure solvent

Question 31

Osmosis

Answer 31

The flow of water toward a more concentrated solution through a semipermeable membrane

Question 32

Semipermeable Membrane

Answer 32

Membrane that allows water and other small molecules to pass through, but blocks the passage of large molecules and ions

Question 33

Osmotic Pressure

Answer 33

The pressure required to stop osmosis

Question 34

Vapor Pressure

Answer 34

The partial pressure of a gas in dynamic equilibrium with its liquid

Question 35

Volatile

Answer 35

Something that vaporizes easily

Question 36

Non-Volatile

Answer 36

Something that does not vaporize easily

Question 37

Give an example of a solid in liquid solution

Answer 37

Saltwater - NaCl in water

Question 38

Give an example of a solid in solid solution

Answer 38

Brass - Alloy of copper and zinc

Question 39

Give an example of a gas in gas solution

Answer 39

Air - O2, CO2, Ar, and other gases in N2 Common Types of Solutions

Question 40

Name 3 solutes in a can of soda

Answer 40

Sugar, CO2, food coloring, ...

Question 41

To answer the questions below, suppose a crystal of NaCl is dissolving in a beaker full of water. a) What force is holding the atoms together in the NaCl crystal? b) What force is holding the water molecules together in the beaker? c) What force is causing the NaCl crystal to dissolve in the water?

Answer 41

a) Electrostatic attraction b) Hydrogen bonding c)The ion-dipole force

Question 42

In general, the solubility of solids ______ with increasing temperature

Answer 42

increase

Question 43

In general, the solubility of gases _______ with increasing temperature.

Answer 43

decreases

Question 44

According to Henry’s law, the solubility of gases ________ with increasing pressure

Answer 44

increases