Chapter 11: Solutions and Colloids

Question 1

solution

Answer 1

homogeneous mixture of two or more substances

Question 2

homogeneous mixture

Answer 2

all substances are in the same phase
constant composition and appearance

Question 3

alloy

Answer 3

solid solutions of one metal dissolved in another metal

Question 4

spontaneous process

Answer 4

occurs under specified conditions without the requirement of energy from an outside source
H = -, S = +

Question 5

ideal solution

Answer 5

• when the strengths of the intermolecular forces of attraction between solute and solvent species in a solution are no different than those present in the separated components
• solution formed with no accompanying energy change
  -structurally similar components

Question 6

dissolution

Answer 6

• involves solute-solute, solvent-solvent, and solute-solvent interaction
• energy required to overcome solute-solute and solvent-solvent
• energy released when solute-solvent is formed

Question 7

solvation

Answer 7

energy released when solute-solvent interactions are established
exothermic

Question 8

soluble

Answer 8

solvation forces are greater than the solute’s electrostatic forces
dissolution is highly exothermic

Question 9

insoluble

Answer 9

solute’s electrostatic forces are greater than the solvation forces
dissolution is highly endothermic

Question 10

intermolecular forces

Answer 10

forces between molecules
dispersion, dipole-dipole, hydrogen bonding

Question 11

electrolytes

Answer 11

ionize when dissolved in water

Question 12

strong electrolytes

Answer 12

ionize completely when dissolved in water
form a strong conducting solution
strong acids, soluble ionic compounds

Question 13

weak electrolytes

Answer 13

ionize incompletely in water
form a weakly conducting solution
weak acids or weak bases

Question 14

non-electrolytes

Answer 14

do not ionize when dissolved in water
do not form a conduction solution
sugar, methanol

Question 15

ionic electrolytes

Answer 15

engage in ion-dipole interactions with solvent

Question 16

ion-dipole interactions

Answer 16

electrostatic attraction between an ion and a molecule with a dipole

Question 17

dissociation

Answer 17

physical change of the dissolution of an ionic compound in which the ions are solvated and dispersed throughout the water

Question 18

covalent electrolytes

Answer 18

conduct electricity because the solute molecules react chemically with the solvent to produce ions

Question 19

solubility

Answer 19

the maximum concentration that can be achieved under given conditions when the dissolution process is at equilibrium

Question 20

saturated

Answer 20

when a solute’s concentration is equal to its solubility

Question 21

unsaturated

Answer 21

when a solute’s concentration is less than its solubility

Question 22

super saturated

Answer 22

solute concentration is higher than its solubility

Question 23

solution of gases in liquids

Answer 23

-solute-solvent interactions are the sole energetic factor affecting solubility
-gas solubility decreases with an increase in temperature
-increases with an increase in partial pressure of the gas above the solution

Question 24

Henry’s Law

Answer 24

quantity of an ideal gas that dissolved in a definite volume of a liquid is directly proportional to the pressure of the gas
deviation when the solute reacts with the solvent

Question 25

miscible liquids

Answer 25

have infinite mutual solubility can be mixed in any proportion to yield solutions have similar properties

Question 26

immiscible

Answer 26

do not mix to a great degree form separate layers when placed in the same container

Question 27

partially miscible liquids

Answer 27

moderate mutual solubility two layers form but each layer is saturated with the other substances

Question 28

colligative properties

Answer 28

properties of solutions that are independent of solute identity, depend on concentration vapor pressure lowering, freezing point depression, osmotic pressure

Question 29

temperature independent concentration units

Answer 29

mole fraction, molality

Question 30

vapor pressure

Answer 30

pressure exerted by a gaseous phase when vaporization and condensation are at equilibrium or are occurring at the same rate

Question 31

nonvolatile solutes

Answer 31

decrease a liquid's vapor pressure solute particles reduce the surface area available to the solvent vaporization occurs at the surface

Question 32

Raoult's Law

Answer 32

the partial pressure exerted by any component of an ideal solution is equal to the vapor pressure of that component multiplied by its mole fraction in the solution non-volatile have 0 vapor pressure

Question 33

Dalton's Law

Answer 33

total pressure of a gaseous mixture equals the sum of the partial pressures of all the components of the mixture

Question 34

IMFs, boiling point, vapor pressure

Answer 34

strong IMFs creates a lower vapor pressure creating a high boiling point weak IMFs create a higher vapor pressure creating a low boiling point

Question 35

boiling point elevation

Answer 35

increase in boiling point observed when nonvolatile solute is dissolved in a solvent occurs since the vapor pressure lowers -> boiling point increases since you need more energy to boil

Question 36

freezing point depression

Answer 36

solutions freeze at a lower temperature compared to the pure solvent vapor pressure is lowered, so temperature to reach equilibrium between solid and liquid phases is lowered

Question 37

semipermeable membrane

Answer 37

only permits particles of a particular size, shape, polarity, and charge to pass through it

Question 38

osmosis

Answer 38

diffusion driven transfer of solvent molecules through a semipermeable membrane

Question 39

osmotic pressure

Answer 39

pressure at which reverse solvent transfer equals osmosis rate depends on molarity and temperature

Question 40

isotonic

Answer 40

solution that has the same concentration as blood cells

Question 41

hypotonic

Answer 41

solution that has lower concentration than blood cell causes hemolysis

Question 42

hemolysis

Answer 42

blood cells swell and burst

Question 43

hypertonic

Answer 43

solution that has higher solute concentration than blood cell causes crenation

Question 44

crenation

Answer 44

blood cells lose water and shrivel

Question 45

suspensions

Answer 45

heterogenous mixture composed of relatively large particles that are visible or that can be seen with a magnifying glass cloudy particles settle after mixing

Question 46

colloids

Answer 46

exhibit properties intermediate between those of suspensions and solutions

Question 47

Tyndall effect

Answer 47

particles are large enough to scatter light occurs in colloids

Question 48

two methods for forming particles of colloidal size

Answer 48

dispersion methods - breaking down larger particles by grinding condensation methods - grow larger molecules from smaller building blocks

Question 49

dispersed phase

Answer 49

particulate component present in lesser amount

Question 50

dispersion medium

Answer 50

substance or solvent in which the particulate component is dispersed

Question 51

emulsion

Answer 51

prepared by blending two immiscible liquids one of the liquids break into drops of colloidal size and will disperse into the other liquid

Question 52

emulsifying agent

Answer 52

stabilize emulsions and inhibit coalescence (prevents dispersed phase from forming large drops and separating)

Question 53

amphiphilic

Answer 53

having polar and nonpolar regions

Question 54

traits of solutions

Answer 54

homogeneous state of solution is the same as state of solute solute particles are dispersed amongst solvent particles dissolved particles do not separate concentration can be varied