CLUSTER 3

Question 1

normally the component present in the greatest amount, andall the other components are
called solutes

Answer 1

Solvent

Question 2

contain water as the solvent and either a gas, liquid, or solid as a solute.

Answer 2

solute.

Question 3

Types of intermolecular interactions involved in the solution process:

Answer 3

1. o Solute–solute interactions must be overcome to disperse the solute particles through the solvent (endothermic).
2. Solvent–solvent interactions must be overcome to make room for the solute
   particles in the solvent (endothermic).
3. Solvent–solute interactions between solvent and solute particles occur as the
   particles mix (exothermic).

Question 4

solute interactions are either comparable to or greater than the solute–solute and solvent–solvent.

Answer 4

magnitudes of the solvent

Question 5

once separated from the solid, the ions are surrounded by water
molecules.

Answer 5

Solvation or hydration

Question 6

opposite of the solution process

Answer 6

Crystallization

Question 7

when the rates of these opposing processes become equal

Answer 7

Dynamic equilibrium

Question 8

Types of Solutions

Answer 8

1. Saturated
2. Unsaturated
3. Supersaturated

Question 9

solution that is in equilibrium with undissolved solute

Answer 9

Saturated

Question 10

if we dissolve less solute than the amount needed to form a saturated
solution

Answer 10

Unsaturated

Question 11

unstable solutions that contain a greater amount of solute than
needed to form a saturated solution

Answer 11

Supersaturated

Question 12

Factors affecting Solubility

Answer 12

1. Solute-solvent interactions
2. Pressure effects
3. Temperature effects

Question 13

polar liquids tend to dissolve in polar solvents; for example, acetone in water.

Answer 13

Solute-solvent interactions

Question 14

miscible - pairs of liquids that mix in all proportions

Answer 14

Solute-solvent interactions

Question 15

nonpolar liquids tend to be insoluble in polar liquids; for example, hexane and
water.

Answer 15

Solute-solvent interactions

Question 16

solubility is increased as the partial pressure of the gas above the solvent
increases.

Answer 16

Pressure effects

Question 17

Henry’s law: Sg = kPg where Sg is the solubility of the gas usually expressed as
molarity, Pg is the partial pressure, and k is a proportionality constant known as the Henry’s law constant

Answer 17

Pressure effects

Question 18

solubility of most solid solutes in water increases as the solution temperature
increases; as an exception, Ce2(SO4)3.

Answer 18

Temperature effects

Question 19

the solubility of gases in water decreases with increasing temperature.

Answer 19

Temperature effects

Question 20

Qualitative

Answer 20

1. Dilute
2. Concentrated

Question 21

Concentration

Answer 21

states how much solute is contained in a given volume or mass of solution or
solvent.

Question 22

Quantitative

Answer 22

1. Mole fraction
2. Molarity (M)
   3.. Molality (m)

Question 23

sum of all components of a solution must equal 1.

Answer 23

Mole fraction

Question 24

number of moles of a substance per liter of solution

Answer 24

Molarity (M)

Question 25

chemical concentrations denoted with square brackets

Answer 25

Molarity (M)

Question 26

of a strong electrolyte is sometimes called the formal concentration (F); for
example, MgCl2.

Answer 26

Molarity (M)

Question 27

changes with temperature because the volume of a solution usually increases when it is heated.

Answer 27

Molarity (M)

Question 28

moles of substance per kilogram of solvent

Answer 28

Molality (m)

Question 29

independent of temperature

Answer 29

Molality (m)

Question 30

Dilution

Answer 30

A volume of the concentrated solution is transferred to a fresh vessel and diluted to the desired final volume.

Question 31

conservation of reaction units

Answer 31

Stoichiometry

Question 32

What should be the pH of a waste for it to be considered as an “acidic waste”?
a. pH < 2
b. pH < 3
c. pH 4
d. pH 7

Answer 32

a. pH < 2