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Chem 1412- Exam 1 > Chapter 13 > Flashcards

Chapter 13 Flashcards

(61 cards)

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1
Q

Solution

A

a homogenous mixture of two or more substances consisting of ions and/or molecules
May exist as gases, liquids or solids

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2
Q

Colloid

A

consists of comparatively large particles of a substance dispersed throughout another substance; not able to settle down, example would be milk

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3
Q

Solute

A

the dissolved substance; component of lesser amount

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4
Q

Solvent

A

the dissolving medium; component of greater amount

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5
Q

Gaseous solution

A

nonreactive gases can mix in all possible proportions

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6
Q

Miscible fluids

A

fluids that dissolve in each other in all proportions

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7
Q

Immiscible fluids

A

if two fluids do not mix

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8
Q

Liquid solutions

A

the most common types of solutions found in the chemistry lab and are the widest used

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9
Q

Aqueous solution

A

if the solvent is water

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10
Q

Solid solutions

A

metals are referred to as alloys

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11
Q

Alloy

A

solid solutions

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12
Q

Formation of solutions

A

favored by the increase of entropy that accompanies the mixing process; Mixing increases disorder

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13
Q

3 main factors affect solubility

A

1) the nature of solute and solvent
2) temperature
3) pressure

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14
Q

Saturated solution

A

one holding as much solute as it is allowed at a stated temperature

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15
Q

Simple solubility rule

A

“like dissolves likes”

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16
Q

Force of attraction

A

this of the solute for the solvent is a major factor in their solubility but molecular structure or size also have an effect

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17
Q

3 kinds of intermolecular interactions involved in solution formation

A

1) Solute-solute interactions
2) Solvent-solvent interactions
3) Solvent-solute interactions

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18
Q

Solute-solute interactions

A

between solute molecules must be overcome to allow dispersion of solute throughout the solvent molecules

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19
Q

Solvent-solvent interactions

A

between solvent particles must be overcome to make room for the solute particles

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20
Q

Solvent-solute interactions

A

occur between the two kinds of particles when they mix

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21
Q

Enthalpy change

A

delta H

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22
Q

3 enthalpy change components

A

1) breaking of solvent-solvent interactions is endothermic; delta H >0
2) breaking of solute-solute interactions is also always endothermic, delta H>0
3) the “new” solvent-solute interactions as solution forms is always exothermic, delta H <0

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23
Q

delta H solution=

A

delta H solvent+ delta H solute+ delta H mix

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24
Q

Solubility of that solute

A

the limit amount of a solute that will dissolve in a given amount of a solvent, at a specified temperature

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25
Supersaturated solution
one that contains more solute that it is allowed at a given temperature; they are metastable
26
Polar molecular solutions
interact well with polar solvents such as water; dipole-dipole interactions
27
Molecular solutions
nonpolar solutes interact with nonpolar solvents primarily due to london (dispersion) forces
28
Ionic solutions
polar solvents such as water also interact well with ionic solutes
29
Henry's Law
the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas in contact with the liquid; Sg= KPg where Sg is solubility of the gas, K is the Henry's Law Constant and Pg is the gas contact pressure with the liquid
30
Effects of temperature on solubility
the solubility of solutes depends strongly on temperature; for most solids dissolved in liquids solubility increases as temperature increases; on the other hand, for gases dissolved in liquids as temperature increases solubility decreases
31
Concentration
expresses the ratio of the amount of solute to the amount of solvent (or P solution); can be expressed in volume, molar, or mass
32
Mass percentage of solute=
(mass of solute/mass of solution) X 100
33
Ppm
parts per million; (mass of solute/mass of solution) X 10^6
34
Ppb
parts per billion; (mass of solute/mass of solution) X 10^9
35
Molarity (M)
"the moles of solute in a liter of solution"; | M= moles of solute/ L of solution
36
Molality (m)
the moles of solute per kilogram of solvent; | m= moles of solute/ kg of solvent
37
Mole fraction (Xa)
Xa= moles of substance A/total moles of solution
38
Colligative properties of solutions
those properties that depend on the concentration of the solute and the properties of the solvent 1. Vapor pressure lowering 2. Freezing point lowering 3. Boiling point rising 4. Osmotic pressure
39
Vapor pressure lowering, delta P
colligative property equal to the vapor pressure of the pure solvent minus the vapor pressure of the solution; Francois Marie Raoult observed that the vapor pressure of a solvent above a solution depended on the mole fraction of the solvent in that solution
40
Vapor pressure of a solution (Raoult's Law)
the vapor pressure of a solution containing a nonelectrolyte nonvolatile solute is proportional to the mole fraction of the solvent in the solution Psolution= (Psolvent)(Xsolvent) where Psolution is the vapor pressure of the solution, Xsolvent is the mole fraction of the solvent and Psolvent is the vapor pressure of the pure solvent at the same temperature as the solution
41
Normal boiling point
of a liquid is the temperature at which its vapor pressure equals 1 atm
42
Boiling point elevation, delta Tb
a colligative property equal to the boiling point of the solution minus the boiling point of the pure solvent =Kbm
43
Freezing point depression, delta Tf
a colligative property equal to the freezing point of the pure solvent minus the freezing point of a solution; =KfM
44
Semipermeable
certain membranes allow passage of solvent molecules but not solute particles
45
Osmosis
the phenomenon of solvent flow through a semipermeable membrane to equalize solute concentrations on both sides of the membrane
46
Osmotic pressure
equal to the pressure that, when applied to the solution, stops osmosis; is related to the molar concentration of the solute
47
Crenation
dehydrate the cell
48
Homolysis
burst the cell
49
Isotonic solution
exerts the same osmotic pressure as cell
50
Hypotonic solution
has a lower osmotic pressure than cell; causes homolysis
51
Hypertonic solution
has a higher osmotic pressure than cell; causes crenation
52
i
the van't Hoff factor
53
Tyndall Effect
the scattering of light by colloidal-size particles
54
Sol colloid
solid particles dispersed throughout a liquid; paint
55
Aerosol colloid
liquid droplets or solid particles dispersed throughout a gas; cigar smoke
56
Emulsion colloid
liquid droplets dispersed throughout another liquid; milk
57
Hydrophillic colloid
there is a strong attraction between the dispersed phase and the continuous phase (water)
58
Hydrophobic colloid
there is a lack of attraction of the dispersed phase for the continuous phase; unstable and in due time aggregates in larger particles but still unable to precipitate
59
Coagulation
the process by which the dispersed phase of a colloid is made to aggregate and thereby separate from the continuous phase
60
Micelle
a colloidal-sized particle formed by the association of molecules, each of which has a hydrophillic end and a hydrophobic end
61
Association colloid
a colloid in which the dispersed phase consists of micelles; ordinary soap in water

Chem 1412- Exam 1 (2 decks)

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