Chapter 12: Solutions

Question 2

Solution

Answer 2

A homogeneous mixture in which one substance called solute is uniformly dispersed in another substance called solvent

Question 3

Solute

Answer 3

A substance dissolved in a solvent to form a solution; it is usually present in the smaller amount

Question 4

Solvent

Answer 4

The dissolving medium of a solution; it is usually present in the greater amount

Question 5

Intermolecular forces during formation of solution

Answer 5

Intermolecular forces rearrange

Question 6

Aqueous solution

Answer 6

water acts as the solvent; S, L or G is the solute

Question 7

Solubility

Answer 7

Maximum amount of a solute that can dissolve in a given amount of solvent at a certain temperature

Question 8

Factors affecting solubility

Answer 8

type of solute and solvent
temperature

Question 9

How is solubility expressed

Answer 9

grams of solute in 100g of solvent

Question 10

Entropy

Answer 10

A measure of energy randomization or energy dispersal in a system

Question 11

When do solutes form (forces-wise)

Answer 11

When the solvent-solute interactions are comparable, or stronger than, the solvent-solvent and solute-solute interactions

Question 12

Heat

Answer 12

The energy that flows from or into a system because of a temperature difference between the system and its surroundings

Question 13

Enthalpy of a reaction

Answer 13

The total amount of heat that is produced or absorbed by a chemical reaction

Question 14

Exothermic process

Answer 14

If the chemical reaction is exothermic, heat is released and the temperature of the system increases [Reactants → Products + heat (Δ H has a negative sign)]

Question 15

Endothermic process

Answer 15

If the chemical reaction is endothermic, heat is absorbed and the temperature of the system decreases [Reactants + heat → Products (Δ H has a positive sign)]

Question 16

Hess’s Law

Answer 16

The overall enthalpy change upon solution formation (enthalpy of solution, ∆Hsoln) is the sum of enthalpy change for each step

Question 17

Hydration

Answer 17

The process in which an ion is surrounded by water molecules arranged in a specific manner

Question 18

Heat of hydration

Answer 18

enthalpy change that occurs when 1 mol of the gaseous solute ions are dissolved in water

Question 19

Solvation

Answer 19

The process in which an ion or molecule is surrounded by solvent molecules arranged in a specific manner. If water is the solvent, we say the ions are hydrated

Question 20

Solution equilibrium

Answer 20

When the rates of the opposing processes become equal, no further net increase in the amount of solute in solution occurs. A dynamic equilibrium is reached

Question 21

Saturated solution

Answer 21

Contains the maximum amount of solute that will dissolve in a given solvent

Question 22

Unsaturated solution

Answer 22

Contains less solute than a solvent has the capacity to dissolve

Question 23

Supersaturated solution

Answer 23

Contains more solute than would be present in a saturated solution

Question 24

Recrystallization

Answer 24

The process in which dissolved solute comes out of the solution and forms crystals

Question 25

Precipitation

Answer 25

The process in which a dissolved solute comes out of solution and forms a solid; a crystalline solid for crystallization process.

Question 26

Henry's Law

Answer 26

Solubility of a gas in a liquid is directly related to the pressure of that gas above the liquid

Question 27

4 colligative properties

Answer 27

depression of freezing point, elevation of boiling point, lowering of vapor pressure, osmotic pressure effects

Question 28

Colligative properties

Answer 28

Properties that depend only on number of molecules or solute particles in a given volume of solvent

Question 29

Solubility of solids in water with increasing temperature

Answer 29

Solubility increases

Question 30

Solubility of gases in water with increasing temperature

Answer 30

Solubility decreases

Question 31

Henry's Law formula

Answer 31

S = KhP S (concentration of dissolved gas) Kh (constant depending on temperature) P (pressure of the gas over the solution)

Question 32

Volatile liquid

Answer 32

A liquid that evaporates easily

Question 33

Example of saturated solution (NaCl)

Answer 33

More than 36 g in 100 g of water

Question 34

Example of unsaturated solution (NaCl)

Answer 34

Less than 36 g in 100 g of water

Question 35

Example of supersaturated solution (NaCl)

Answer 35

Much more than 36 g in 100 g of water

Question 36

Raoul's Law

Answer 36

Psolute = Xsolvent x Psolvent

Question 37

Change in freezing point formula

Answer 37

ΔTf=mKf m is molality

Question 38

Change in boiling point formula

Answer 38

ΔTb=mKb m is molality

Question 39

Isotonic solution

Answer 39

a solution with equal concentration of solute to another and so equal osmotic pressure

Question 40

Hypotonic solution

Answer 40

a solution that has lower concentration of solute as another and so lower osmotic pressure

Question 41

Hypertonic solution

Answer 41

a solution that has higher concentration of solute as another and so higher osmotic pressure

Question 42

Colloid

Answer 42

A type of mixture with dispersion of particles of one substance throughout a dispersing medium of another substance; collodial particles are much larger than solute molecules; collodial suspension is not as homogeneous as a solution

Question 43

Micelle repulsions

Answer 43

Micelles do not coalesce because the charged surface of one micelle repels the charged surface of another

Question 44

Osmosis

Answer 44

the selective passage of solvent molecules through a porous membrane from a dilute solution to a more concentrated one

Question 45

Osmotic pressure

Answer 45

the pressure required to stop osmosis