Lecture 8 - Solutions

Question 1

True/False: water has the ability to dissolve a wide variety of substances

Answer 1

True

Question 2

aqueous solution = homogeneous or heterogeneous mixture

Answer 2

homogeneous

Question 3

7 types of solutions:
gas/gas
gas/liquid
liquid/liquid
liquid/solid
solid/liquid
solid/solid
gas/solid

Answer 3

air (O, N, and other gases)
soda pop (CO2 in H2O)
vinegar (acetic acid in H2O)
dental fillings (Hg in Ag)
sea water (NaCl in H2O)
brass (Zn in Cu)
nitrogen in steel

Question 4

the measure of how much solute will dissolve in a solvent

Answer 4

solubility

Question 5

solutions that contain the max amount of solute for the given conditions - cannot dissolve additional state

Answer 5

saturated solutions

Question 6

why does the temperature always need to be specified when describing a saturated solution

Answer 6

because the solubility depends on temperature and temperature must be specified because of the “temperature effect” on solubility

Question 7

most solids become more soluble in aqueous solution with _____ temperature

Answer 7

increasing

Question 8

gas solubility decreases with _____ temperature for aqueous solutions

Answer 8

increasing

Question 9

solutions that contain less than the max amount of solute - can dissolve additional state

Answer 9

unsaturated solutions

Question 10

if a substance does not dissolve in a solvent

Answer 10

insoluble

Question 11

contain a small amount of solute relative to what could dissolve

Answer 11

dilute solutions

Question 12

contain a large amount of solute relative to what could dissolve

Answer 12

concentrated solutions

Question 13

all solutes that dissolve in water can be divided into two categories

Answer 13

electrolyte

nonelectrolyte

Question 14

a substance that dissolves in water to give an electrically conducting solution

Answer 14

electrolyte

Question 15

a substance that dissolves in water to give a solution that conducts electricity poorly

Answer 15

nonelectrolyte

Question 16

when an ionic substance dissolves in water it _____ into its ions

Answer 16

dissociates

Question 17

component present in the greatest amount

Answer 17

solvent

Question 18

component present in the relatively smaller amount

Answer 18

solute

Question 19

substance that dissolve in each other in all proportions

Answer 19

miscible

Question 20

what are gases always miscible

Answer 20

because the intermolecular attractions in the gas phase are always weak

Question 21

when a dissolved solute forms a solid

Answer 21

crystallization

Question 22

when the rate of dissolution and crystallization are equal

Answer 22

equilibrium

Question 23

4 concepts for understanding equilibrium:

Answer 23

equilibrium is

• time dependent
• dynamic
• reversible
• temperature dependent

Question 24

3 factors affecting the rate of solution formation and establishment of equilibrium

Answer 24

1. surface area
2. agitation
3. temperature

Question 25

increasing the pressure will _____ the solubility of a gas in a solvent

Answer 25

increase

Question 26

decreasing the pressure will _____ the solubility of a gas in a solvent

Answer 26

decrease

Question 27

the amount of solute dissolved in a given amount of solvent or solution

Answer 27

concentration

Question 28

concentration equation:

Answer 28

concentration = (amt. solute/amt. solution)

Question 29

% mass (solute) =

Answer 29

(mass solute/total mass solution) x 100

Question 30

the ratio of the volume of a solute to the volume of the solution, multiplied by 100

Answer 30

volume-volume percent

Question 31

% mass-volume =

Answer 31

(mass solute (g)/volume solution (mL)) x 100

Question 32

Dilution Equation

Answer 32

CsVs = CdVd

Question 33

properties that depend only on the number of solute particles in a solution and not on the nature of the solute particles

Answer 33

colligative properties

Question 34

4 colligative properties

Answer 34

1. vapor pressure lowering 2. boiling point elevation 3. freezing point depression 4. osmotic pressure

Question 35

the pressure required to stop osmosis

Answer 35

osmotic pressure

Question 36

one solution has a lower osmotic presure

Answer 36

hypotonic

Question 37

the solution with higher osmotic pressure

Answer 37

hypertonic

Question 38

a concentration unit used to compare the osmotic pressures of different solutions

Answer 38

osmolarity

Question 39

have similar properties to solutions but they are not true solutions

Answer 39

colloids

Question 40

are colloids heterogeneous or homogeneous

Answer 40

heterogeneous

Question 41

the scattering of light by colloidal-size particles

Answer 41

tyndall effect

Question 42

collectively, the particles suspended in a colloid

Answer 42

dispersed phase

Question 43

substance containing the colloid particles

Answer 43

dispersing medium

Question 44

caused by collisions between the suspended particles and the molecules of the dispersing medium

Answer 44

brownian movement