Chapter 13

Question 1

Solutions

Answer 1

Homogenous mixtures of two or more substances

Question 2

Solute

Answer 2

Lesser amount

Question 3

Solvent

Answer 3

More in content

Question 4

Natural tendency

Answer 4

-mixing of gas is spontaneous process
-each gas acts as it is alone
-increase of disorder
-formation of solution favors entropy

Question 5

Entropy

Answer 5

Disorder

Question 6

Crystallization

Answer 6

opposing processes of a solution

Question 7

Saturated solution

Answer 7

When the opposing processes is equal , the additional solute will not dissolve unless some crystallizes from the solution.

Have the solute dissolved at the temp

Question 8

Unsaturated solution

Answer 8

When the amount of crystallization is not reached

Any amount of solute less than the max amount dissolved in the solution

Question 9

Solubility

Answer 9

The amount of solute that can dissolve in a given amount of solvent at a given temp

Question 10

Supersaturated

Answer 10

The solvent holds more solute than normal at a possible temp

Question 11

Factors that affect solubility

Answer 11

Solute - solvent interactions
Temperature
Pressure for gas solutes

Question 12

Will it dissolve

Answer 12

Solvent and solvent have similar structures
Polar and ionic more soluble in polar solvent
Nonpolar more soluble in nonpolar solvents

Question 13

Temperature effect relative to solubility

Answer 13

Solids - temp increases solubility increases
Gases- temp increases solubility decreases
- higher mass more solubility

Question 14

Solubility of gases

Answer 14

Solubility of gas directly proportional to its partial pressure

Sgas= Kh * Pgas

Question 15

Miscible and immiscible

Answer 15

Mix in all proportions
Do not mix

Question 16

Mass percent

Answer 16

= (mass of component / total mass of soln) x 100

Question 17

PPM

Answer 17

Parts per million
10^6
=(mass of component in soln/total mass of soln) x 10^6

Question 18

PPB

Answer 18

Parts per billion
10^9
=(mass of component in soln/total mass of soln) x 10^9

Question 19

Mole fraction

Answer 19

=moles of component / total moles of all components

Question 20

Molarity

Answer 20

=mol of solute / liters of the solution

Question 21

Molality

Answer 21

=mol of the solute / Kg of solvent

Question 22

Colligative properties

Answer 22

Depend on quantity not the identity of solute
Vapor pressure lowering
Boiling point elevation
Freezing point depression
Osmotic pressure

Question 23

Electrolyte

Answer 23

Separates into ions when in water
Strong ones dissociate completely while weak ones dissociate very little

Question 24

Nonelectrolyte

Answer 24

Do not dissociate to form ions

Question 25

Vapor pressure Relating to pure solutions and mixed solutions

Answer 25

Solvent must be greater for pressure to go up , when something is pure solvent the pressure goes up but adding a solute lowers the pressure.

Question 26

Raoult’s Law

Answer 26

Puré solvent Psolvent=Xsolvent * Psolvent Solute present DeltaPsolvent = Xsolute * Psolvent

Question 27

Boiling Point elevation

Answer 27

Vapor pressure is lowered. Requires more tempt boiling point is increased DeltaB = Tbsolution - Tbsolvent = iKbm

Question 28

Freezing Point depression

Answer 28

When the boiling point is raised the freezing point is lowered DeltaTf= Tfsolution - Tf solvent = -iKfm

Question 29

Van’t Hoff factor

Answer 29

The ratio of moles of solute particle to moles of formula units dissolved , to find this first figure out if its an electrolyte if yes then the subscripts are the hoff factor and if not then its 1

Question 30

Ósmosis

Answer 30

net movement of solvent molecules from solution of low to high concentration of solute across a semipermeable membrane [] = iMRT

Question 31

Isotonic Hypotonic Hypertonic

Answer 31

Same Lower low P solvent will leave the solution at higher rate Hyper higher p ,solvent will enter solution higher rate

Question 32

Colloids

Answer 32

Suspensión particles larger than ions but small enough for gravity not to settle them

Question 33

Tyndall effect

Answer 33

Colloidal suspensions can scatter rays of light

Question 34

Hydrophilic Hydrophobic

Answer 34

Water loving Water fearing