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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
Q

What affect does pressure have on solid’s solubility in liquid.

A

“None”

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26
Q

What affect does temperature have on gas’ solubility in liquid

A

An increase in temperature results in lower solubility in liquid.

27
Q

Henry’s Law

A

Sg = Kh * Pg

Solubility gas = Henrys Constant * Pressure(gas)

28
Q

What is a dilute solution

A

low concentration of solute to solvent

29
Q

What is a concentrated solution

A

large amount of solute relative to solvent

30
Q

Molarity

A

Moles Solute / Liters Solution

31
Q

molality

A

Moles Solute / Kg Solvent

32
Q

Mass %

A

grams solute / g solution

33
Q

PPM

A

grams solute / grams solution *10^6

34
Q

X (mole fraction)

A

moles n / total moles

35
Q

mole percent

A

moles n / total moles * 100

36
Q

Colligative properties

A

properties that only depend on the amount of solute particles in the solution

37
Q

non electrolyte solutions

A

covalent bonded (1 particle per molecule)

38
Q

electrolyte solution

A

ionic (dissolved ions) (2 particles per molecule)

39
Q

Non-volatile

A

No significant vapor pressure

40
Q

Vapor

A

Normally liquid substance in the gas phase

41
Q

Vapor Pressure

A

The pressure created above a liquid by particles in the gas phase.

42
Q

Increase in temperature, what affect on vapor pressure?

A

Increases with increase in temperature

43
Q

What will vapor pressure do in a closed system?

A

Reach dynamic equilibrium

44
Q

What will adding a non volatile solute to a solution do to that solutions vapor pressure

A

Lower it, therefore requiring more energy to bring the vapor pressure up to a boil, raising the boiling point.

45
Q

What is an ideal solution

A

A solution in which all attractions are about equal (solute-solute), (solute- solvent) (solvent-solvent)`

46
Q

VP(soln) = (equation)

A

X(solvent) * VP pure solvent

47
Q

VP(soln) = (equation)

A

X(solvent)A * VP pure solventA + X(solvent)A * VP pure solvent( A)

48
Q

Non idea solutions

A

When some of the interactions are stronger than others

49
Q

What does it mean about the interactions if the VP is higher than predicted by Rault’s law

A

That the solute-solvent interactions are weaker.

50
Q

What does it mean about the interactions if the VP is lower than predicted by Rault’s law

A

That the solute-solvent interactions are stronger.

51
Q

Delta T = (equation for freezing, boiling)

A

= K(freezing or boiling) * molality

52
Q

What is osmosis

A

Migration of solvent molecules across a semipermeable membrane from dilute –> more concentrated

53
Q

What is osmotic pressure

A

The pressure required to be applied to prevent H2O molecules from migrating from the dilute side to the concentrated side.

54
Q

Formula for osmotic pressure

A

Pi= MRT (molarity * gas constant * T (kelvin))

55
Q

Isometric

A

equal pressure inside and outside the cell

56
Q

Hyposmotic

A

surrounding solution is higher concentrated in solute, sucking the fluid out of the RBS

57
Q

Hyperosmotic

A

surrounding solution is too dilute, and too much is going into the RBC and could cause them to burst.

58
Q

Colloids

A

Particles in solution that are not large enough to settle, but large enough to reflect light, resulting in a visible beam.

59
Q

Name some examples of Colloids

A

Fog, Milk, Soap, Marshmallow

60
Q

What is the name of the effect that allows you to see the light beam in a solution that has colloids in it?

A

Tyndall effect

61
Q

Micelles

A

Aggregate particles of partially polar and partially non polar molecules

62
Q

Kinetics

A

The study of the rate of chemical change and the factors that affect those rates.

63
Q

Rate Laws

A

What reactants affect the rate of Rxn and if it is linear, squared or other.

64
Q

What is K in regards to rate laws?

A

The rate constant

Chem 111 (4 decks)

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