Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

NU 724 - Chem/Phys > Exam II > Flashcards

Exam II Flashcards

1
Q

What is Solubility?

A

The maximum amount of one substance (solute) that is able to dissolve into another (solvent).

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

Factors of Solubility

A

Intermolecular interactions
Temperature
Pressure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

How do intermolecular interactions affect solubility?

A

“Like-dissolves-like”

Polarity/ionization

Similar electron configuration = higher solubility

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

How does temperature affect solid/liquid solubility?

A

Elevated temp = increased solubility

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

How does pressure affect solubility?

A

Higher pressure increases solubility (Henry’s Law - gases)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Endothermic Reactions

A

Reaction that requires/uses energy.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Exothermic Reactions

A

Reactions that release energy.

Increased temperature reduces solubility.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Effect of Temperature on Gas

A

Inverse relationship - as temperature increases, solubility decreases.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Henry’s Law

A

p = kc

The solubility of gas is directly proportional to pressure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Diffusion

A

The net movement of one type of molecule through space as a result of random motion intended to minimize concentration gradient.

Ex. Food coloring in water.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Osmosis

A

The movement of water across a semipermeable membrane to equilibrate a concentration gradient.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Graham’s Law

A

r = 1/,^mw (square root)

The rate of effusion of a gas is INVERSELY proportional to the square root of its molecular weight.

Small = Faster diffusion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Fick’s Law

A

Diffusion of gas is DIRECTLY proportional to:
-Partial pressure gradient
-Membrane solubility
-Membrane area

INVERSELY proportional to:
-Membrane thickness
-Molecular weight

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Fick’s Law Application to Anesthesia

A

Passive Oxygenation - ENT cases
Diffusion Hypoxia
Concentration Effect
Second Gas Effect

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is diffusion hypoxia?

A

Nitrous is very soluble
tissues become saturated, diffuse into alveoli quickly once turned off, creating hypoxic mixture in the lungs <21%

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What is concentration effect?

A

Increasing the fraction of inspired concentration (FI) of an inhalation anesthetic will more rapidly increase the fraction of alveolar concentration (FA) of the agent– think about Henry’s law

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What is the second gas effect?

A

As nitrous is diffused into the blood from the alveoli at a faster rate than the volatile anesthetic, it leaves a void of volume in the alveoli. It creates pressure gradient, allowing more volatile anesthetic to enter the alveoli at a faster rate.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Tonicity

A

The capacity of a solution to modify the volume of a cell by altering its water content.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Hypotonic

A

Na concentration <130 mEq/L

Cytolysis = Cells in hypotonic fluid absorb too much water and burst.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Isotonic

A

Na concentration between 130-155 mEq/L

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Hypertonic

A

Na concentration >155 mEq/L

Plasmolysis = Cells in hypertonic solution lose water and shrink.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is an acid?

A

A substance that can donate a proton (H+) or accept an electron pair in a chemical reaction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What is a base?

A

A substance that can accept a proton (H+) or donate an electron pair in a chemical reaction.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is pH?

A

Measure of acidity or alkalinity of a solution, qualifies, the concentration of H+ ions in a solution.

pH range = 0-14

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

What is an acid-base reaction?

A

Occurs when an acid and a base react to form water (H2O) and salt (an ionic compound).

Acid + Base = Water + Salt

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
26
Q

What is a buffer and an ex. of one?

A

Help regulate and stabilize pH

CO2 + Water <–> carbonic acid <–> HCO3 + H+

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
27
Q

What is pKa?

A

A specific value associated with a weak acid or weak base.

It represents the pH at which half of the molecules of that substance are ionized (dissociated) and half are in their non-ionized (undissociated) forms.

CONSTANT.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
28
Q

pH Equation

A

pH = pKa + log[A-]/[HA]
or
pH = -log[H+]

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
29
Q

What is a non-ionized molecule?

A

Molecule that has not gained or lost an extra hydrogen ion.

Carries a negative charge.

Lipophilic = cross membranes easily.

EFFECTIVE.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
30
Q

What is an ionized molecule?

A

Molecule that has gained an extra hydrogen ion.

Carries a positive charge.

Hydrophilic = does not cross membranes easily.

INEFFECTIVE

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
31
Q

What is “like-dissolves-like”?

A

Non-polar solutes dissolve in non-polar solvents.

Ionic/polar solutes dissolve in polar solvents.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
32
Q

Partial Pressure

A

Proportion pressure of a single type of molecule in a gas.

If the proportion of a gas goes up, the partial pressure goes up.

The likelihood of a solute entering a solvent at a given temperature.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
33
Q

Molality

A

Moles solute / kg solvent

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
34
Q

Vapor Pressure Lowering

A

Solutes block the ability of the solvent to spontaneously enter the air, leading to decreased vapor pressure.

More solutes = lower vapor pressure.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
35
Q

Boiling Point Elevation

A

Presence of solute molecules interferes with the solvents ability to escape the liquid.

More solutes = elevated boiling point.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
36
Q

Freezing Point Depression

A

Presence of solute molecules interferes with the solvents ability to form a latus.

More solutes = depressed freezing point.

Ex. Salt added to ice on roads.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
37
Q

What is concentration?

A

Measure of how much solute is present per volume of solvent.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
38
Q

Bronsted-Lowry Acid

A

Proton donor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
39
Q

Bronsted-Lowry Base

A

Proton acceptor

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
40
Q

Lewis Acid

A

Electron pair acceptor (electrohpile)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
41
Q

Lewis Base

A

Electron pair donor (nucleophile)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
42
Q

[HA]

A

Acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
43
Q

[A-]

A

Conjugate base

44
Q

The Buffer System

A

CO2 + H2O <–> Carbonic Acid <–> HCO3 + H+

45
Q

What does a buffer consist of?

A

A weak acid and its conjugate base.

46
Q

Henderson-Hasselbalch Equation

A

pH = pKa + log[A-]/[HA]

47
Q

[A-] = [HA]

A

pH = pKa

48
Q

[A-] > [HA]

A

pH > pKa

49
Q

[A-] < [HA]

A

pH < pKa

50
Q

Oncotic Pressure

A

Pressure exerted by large molecules, such as proteins, albumin, and poly-carbs that cannot pass through the semi-permeable membrane.

Creates an osmotic pressure.

51
Q

Example of Oncotic Pressure

A

Arterial capillaries have a hydrostatic pressure (filtration pressure) that exceeds the oncotic pressure (absorption pressure) and flow is created out of the capillaries.

Venous capillaries’s oncotic pressure exceeds the hydrostatic pressure and therefore flow is generated back into the capillary system.

52
Q

Viscosity

A

The ability of a liquid to resist flow.

SI unit for viscosity = Pa s (pascal seconds)

53
Q

Factors that Determine Viscosity

A

Strength of intermolecular forces.

Size/shape of the molecule.

Temperature.

54
Q

Two types of intermolecular forces?

A

Cohesive
Adhesive

55
Q

Cohesive Forces

A

Intermolecular forces between the molecules of a liquid.

The attraction that molecules exhibit between one another that cause cohesion.

56
Q

Adhesive Forces

A

Interactions between the liquid and a solid surface.

57
Q

Why do water molecules form spheres?

A

To maximize hydrogen bonding by decrease surface area.

Molecules on the edge only half the effect of hydrogen bonding.

58
Q

Concave meniscus is an example of what force?

A

Adhesive > Cohesive

59
Q

Convex meniscus is an example of what force?

A

Cohesive > Adhesive

60
Q

Surface Tension

A

Energy require to increase the surface area of a liquid.

Dependent on strength of the cohesive force in liquid.

61
Q

Equation of Continuity

A

Flow rate = area x velocity

The FLOW RATE depends on the cross-sectional AREA of the pipe and the VELOCITY of the fluid.

Velocity is INVERSELY proportional to area.

62
Q

Bernoulli’s Principle

A

The higher the fluid’s velocity is through a pipe, the lower the pressure on the pipe’s walls, and vice versa.

Constant = P + (1/2p x v^2) + (p x g x y)

63
Q

Venturi Effect

A

A constricted pipe leads to a faster velocity and a lower pressure.

Ex. Venturi Mask

64
Q

Laminar Flow

A

Smooth even flow. Minimal mixing of layers. No random velocity changes. Fluid flows steadily in one direction.

Ex. Blood flow

65
Q

Turbulent Flow

A

Velocity is fluctuating. Contains swirls and eddies.

Ex. Smoke from a chimney.

66
Q

Layers of Turbulent Flow

A

Laminar sublayer
Buffer layer
Turbulent boundary

67
Q

Reynold Number Equation

A

Re = puL / u (mu)

p = fluid density
u = velocity
L = Length
u (mu) = dynamic viscosity

68
Q

puL

A

Inertial forces = force which cause fluid to move.

69
Q

u (mu)

A

Viscous forces = frictional forces due to fluid viscosity

70
Q

If inertial forces dominiate?

A

Turbulent flow

71
Q

If viscous forces dominate?

A

Laminar flow

72
Q

Re Predictions

A

<2000 = laminar
2000-4000 = transitional
>4000 = turbulent

73
Q

What would the heart have to work harder if blood flow was turbulent?

A

The pressure drop is greater in turbulent flow.

As the blood gets further from the heart, the pressure drops.

74
Q

What is hydrostatics?

A

Characteristics of fluids at REST and the pressure in a fluid or exerted by a fluid on an immersed body.

75
Q

What is hydrodynamics?

A

MOTION of fluids and forces acting on solid bodies immersed in fluids and in motion relative to them

76
Q

What law calculate laminar flow rate?

A

Poiseuille’s Law

77
Q

Poiseuille’s Law

A

Flow rate = (pie)(r4) x (P1-P2) / 8nL

78
Q

Conditions for Poiseuille’s Law

A

Fluids must have laminar flow.

Incompressible fluid.

79
Q

Poiseuille’s Law - Increased Radius

A

Increased flow rate

80
Q

Poiseuille’s Law - Increase Viscosity

A

Decreased flow rate

81
Q

Poiseuille’s Law - Increased Length

A

Decreased flow rate

82
Q

Poiseuille’s Law - Increased Pressure

A

Increased flow rate

83
Q

Ex. of Poiseuille’s Law

A

Blood vessels with atherosclerosis = decreased radius = decreased flow rate = increase pressure from heart

84
Q

Law of Laplace r/t CV

A

Wall Stress = Pressure x Radius / Wall Thickness

85
Q

Wall Stress is DIRECTLY proportional to…

A

Pressure and Radius

86
Q

Wall Stress is INVERSELY proportional to…

A

Wall Thickness

The heart wall will thicken in attempted to decrease wall stress due to chronic hypertension.

87
Q

Surface Tension

A

Measure of the contractive tendency that allows liquids to resist deformation by an external force.

88
Q

Law of Laplace

A

P = 2T / r

P = Pressure
T = Tension
r = Radius

89
Q

(LOL) Pressure is DIRECTLY proportional to…

A

Tension

90
Q

(LOL) Pressure is INVERSELY proportional to…

A

Radius

91
Q

Surfactant

A

Prevents atelectasis

A compound that reduces surface tension when added to a liquid.

92
Q

Pulmonary Surfactant

A

Complex lipoprotein formed by type II pneumocytes lining the alveoli.

Ex. DPPC

93
Q

Effects of Surfactant on Surface Tension

A

Roughly proportional to surface area.

Most pronounced when alveoli are smaller.

94
Q

Effects of Surfactant

A

Reduction in atelectasis

More even distribution of ventilation amongst the alveoli.

Improved lung compliance.

95
Q

Longitudinal Waves

A

Particles vibrate parallel to the direction in which the wave of energy is traveling.

Ex. Sound

96
Q

Transverse Waves

A

Particles vibrate at 90 degrees and move horizontally.

Ex. Ocean waves.

97
Q

Wave Properties

A

Frequency
Period
Wavelength
Amplitude

98
Q

Frequency

A

The number of complete waves passing a fixed point in a given amount of time.

Usually over 1 second.

SI Measurement = Hertz (Hz)

99
Q

Period

A

The time for one complete cycle.

Measured in seconds.

Periodic = happens repeatedly

100
Q

Wavelength

A

Distance between the point on one wave to the same point on the next wave.

Measured in meters (lambda).

101
Q

Amplitude

A

Distance from the maximum disturbance to the undisturbed position (flat).

Ex. Waves at sea. Height of wave = amplitude.

102
Q

What is rarefraction?

A

Area in longitudinal wave where the particle are far apart.

103
Q

What is compression?

A

Area in longitudinal waves where the particles are close together.

104
Q

Doppler Effect

A

As a source approaches an observer (or vice versa) the wavelength decreases, and therefore the frequency increases.

105
Q

Inverse Square Law

A

Change in intensity due to change in distance.

Decreased distance = increased intensity (or vice versa).

Ex. Xray or flashlight.

NU 724 - Chem/Phys (3 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions