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Chem 111 > Test 1 > Flashcards

Test 1 Flashcards

1
Q

Solution

A

A mix where solute is uniformly dispersed in solvent

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2
Q

Solute

A

Minority Component

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3
Q

Solvent

A

Majority Component

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4
Q

Solution = (mathematically)

A

Solute + Solvent

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5
Q

Aqueous Solution

A

Solvent is in water

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6
Q

Solubility

A

The amount of solute that will dissolve in a specific amount of solvent.

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7
Q

Saturated Solution

A

A solution that will not allow any more solute to dissolve

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8
Q

Unsaturated Solution

A

More solute is able to dissolve in the solute

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9
Q

Supersaturated solution

A

More solute is dissolved than is normally able.

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10
Q

Miscible

A

Two or more liquids that are soluble in each other in any proportions.

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11
Q

Immiscible

A

Two or more liquids that do not mix completely

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12
Q

Soluble (molarity)

A

> .1 M

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13
Q

Insoluble or slightly soluble

A

<.1M

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14
Q

Enthalpy (defn)

A

The sum of the internal energy and thermodynamic potential ( energy + pressure * change in volume) = change in temp at constant pressure.

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15
Q

Entropy

A

Measure of disorder or randomness

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16
Q

What conditions favor spontaneously occurring reactions

A

Exothermic reaction or a high degree of entropy increased.

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17
Q

Name the types of IMF from weakest to strongest

A

London/dispersion, dipole-dipole, h-bonding, ion-dipole

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18
Q

What are the polarity generalizations for carbon chain compounds?

A

Less than three carbons–> can be polar

More than three carbons –> not polar, even with OH

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19
Q

Steps of solution formation

A

Solute particles separate (endothermic)
Solvent particles separate (endothermic)
Solvent and solute mix (usually exothermic)

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20
Q

DELTA H solution =

A

-DELTA H crystal lattice + DELTA H hydration

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21
Q

Equilibrium

A

Processes that go forwards and backwards

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22
Q

Equilibrium in chemical reactions

A

Reached when the net concentrations of products and reactants no longer change

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23
Q

Dynamic equilibrium in solutions

A

Particles cycle in and out of the solution and the precipitate

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24
Q

What affect does a raise in temperature have on solid’s solubility

A

Increases in most cases (not NaCl)

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25
What affect does pressure have on solid's solubility in liquid.
"None"
26
What affect does temperature have on gas' solubility in liquid
An increase in temperature results in lower solubility in liquid.
27
Henry's Law
Sg = Kh * Pg | Solubility gas = Henrys Constant * Pressure(gas)
28
What is a dilute solution
low concentration of solute to solvent
29
What is a concentrated solution
large amount of solute relative to solvent
30
Molarity
Moles Solute / Liters Solution
31
molality
Moles Solute / Kg Solvent
32
Mass %
grams solute / g solution
33
PPM
grams solute / grams solution *10^6
34
X (mole fraction)
moles n / total moles
35
mole percent
moles n / total moles * 100
36
Colligative properties
properties that only depend on the amount of solute particles in the solution
37
non electrolyte solutions
covalent bonded (1 particle per molecule)
38
electrolyte solution
ionic (dissolved ions) (2 particles per molecule)
39
Non-volatile
No significant vapor pressure
40
Vapor
Normally liquid substance in the gas phase
41
Vapor Pressure
The pressure created above a liquid by particles in the gas phase.
42
Increase in temperature, what affect on vapor pressure?
Increases with increase in temperature
43
What will vapor pressure do in a closed system?
Reach dynamic equilibrium
44
What will adding a non volatile solute to a solution do to that solutions vapor pressure
Lower it, therefore requiring more energy to bring the vapor pressure up to a boil, raising the boiling point.
45
What is an ideal solution
A solution in which all attractions are about equal (solute-solute), (solute- solvent) (solvent-solvent)`
46
VP(soln) = (equation)
X(solvent) * VP pure solvent
47
VP(soln) = (equation)
X(solvent)A * VP pure solventA + X(solvent)A * VP pure solvent( A)
48
Non idea solutions
When some of the interactions are stronger than others
49
What does it mean about the interactions if the VP is higher than predicted by Rault's law
That the solute-solvent interactions are weaker.
50
What does it mean about the interactions if the VP is lower than predicted by Rault's law
That the solute-solvent interactions are stronger.
51
Delta T = (equation for freezing, boiling)
= K(freezing or boiling) * molality
52
What is osmosis
Migration of solvent molecules across a semipermeable membrane from dilute --> more concentrated
53
What is osmotic pressure
The pressure required to be applied to prevent H2O molecules from migrating from the dilute side to the concentrated side.
54
Formula for osmotic pressure
Pi= MRT (molarity * gas constant * T (kelvin))
55
Isometric
equal pressure inside and outside the cell
56
Hyposmotic
surrounding solution is higher concentrated in solute, sucking the fluid out of the RBS
57
Hyperosmotic
surrounding solution is too dilute, and too much is going into the RBC and could cause them to burst.
58
Colloids
Particles in solution that are not large enough to settle, but large enough to reflect light, resulting in a visible beam.
59
Name some examples of Colloids
Fog, Milk, Soap, Marshmallow
60
What is the name of the effect that allows you to see the light beam in a solution that has colloids in it?
Tyndall effect
61
Micelles
Aggregate particles of partially polar and partially non polar molecules
62
Kinetics
The study of the rate of chemical change and the factors that affect those rates.
63
Rate Laws
What reactants affect the rate of Rxn and if it is linear, squared or other.
64
What is K in regards to rate laws?
The rate constant

Chem 111 (4 decks)

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