Solutions and Solubility - week 7

Question 1

Solution definition

Answer 1

solute dissolved in a solvent

Question 2

Suspension definition

Answer 2

solution where the solute cannot be dissolved in the solvent

Question 3

Colloidal solution definition

Answer 3

particles exist in solution somewhere between a true solution and a true suspension

Question 4

Solvent

Answer 4

substance into which a solute is dissolved

Question 5

True solution

Answer 5

occurs when solute is completely dissolved in the solvent (amount dissolved is dependent on temperature)

Question 6

The greater the temperature of the solvent ____

Answer 6

the greater the amount of solid solute dissolved

Question 7

When dissolving is endothermic then ___

Answer 7

increase solubility with increasing temperature

Question 8

When dissolving is exothermic then ___

Answer 8

decrease solubility with increasing temperature

Question 9

Does changes in our body temperature have an effect on solubility of solids in our body?

Answer 9

changes to body temperature are small and will have minimal effect on solubility

Question 10

Concerning gases, the greater the temperature of the solvent the ___

Answer 10

less gas that will be dissolved in the solvent (liquid)

Question 11

If patient’s temperature increases what happens to the anesthetic?

Answer 11

less anesthetic dissolved so more difficult to anesthetize

Question 12

If patient’s temperature decreases what happens to the anesthetic?

Answer 12

more anesthetic dissolved so easier to anesthetize

Question 13

How does gas escape from the solution with an increased temperature?

Answer 13

increased temperature –> more KE of the gas molecules –> breaks IMF between gas and solvent –> gas escapes

Question 14

Saturated solution

Answer 14

state of a solution in which more solute cannot be added without some of the solute precipitating out of the solution (Point of equilibrium between the gas and liquid phase)

Question 15

Solution strength- % solution

Answer 15

grams of solute/100mL solvent = % solution

example. .9% NaCl = .9 grams/ 100mL

Question 16

Solution strength - molar solution

Answer 16

moles of solute per 1 liter of solvent
example. NaCl= 23+35 = 58 grams/mole
58grams NaCl/ 1 L of solvent = 1 Molar solution

Question 17

diffusion

Answer 17

process whereby a substance spreads through the space available to it by random molecular motion (high to low concentration)

Question 18

molecular movement is a product of ___

Answer 18

a pressure gradient

Question 19

Henry’s Law

Answer 19

amount of gas dissolved in a liquid is directly proportional to the pressure applied to the gas as it overlies the liquid

Question 20

Graham’s Law

Answer 20

movement of gas from one compartment to another thru a porous membrane

Question 21

diffusion coefficient

Answer 21

(D) = Solubility of Gas/ square root MW

Question 22

calculating relative rate of diffusion of 2 gases as they dissolve in a liquid

Answer 22

diffusion rate of gas 1/diffusion rate of gas 2 = sol gas 1/ sol gas 2 x square root of MW gas 2/MW gas 1

Question 23

Which is less dense Helium or ethylene oxide?

Answer 23

helium is much less dense, the rate of effusion of helium thru a hole is greater than that of ethylene oxide

Question 24

Fick’s Law

Answer 24

volume of a gas that diffuses across a membrane per minute

Question 25

Bunsen solubility coefficient

Answer 25

volume of a gas in a unit volume of a liquid at 0 degree C and 760 mmHg example: 4.9 volume of O2 dissolve in 100 mL H2O at 0C and 760mmHg = .049 of O2 dissolved in 1mL H2O so bunsen coefficient for O2 in H2O at STP = .049

Question 26

Ostwald Solubility coefficient

Answer 26

ratio of the volume of a gas absorbed to the volume of solvent at the temperature and pressure of the experiment used to express the blood/gas: tissue/gas ratio

Question 27

tension

Answer 27

concentration of a gas in a mixture, force or pressure exerted (cmH2O or mmHg)

Question 28

surface tension

Answer 28

created at interface between liquid an gas where the liquid molecules are pulled together by intermolecular cohesive forces 1. molecules drawn inward from periphery 2. volume tends to assume smallest area possible 3. small volume tends to assume spherical form

Question 29

When a molecule is on the surface of a liquid what kind of force does it have?

Answer 29

a net attractive force pointing toward the liquid interior because there are no molecules of the liquid above the surface

Question 30

Law of laplace

Answer 30

pressure gradient across the wall of a sphere which are related to wall tension and radius

Question 31

law of laplace applied to cylindrically shaped structures

Answer 31

T = P x r | two applications: blood vessel (aneurysm), left ventricle (dilated chamber)

Question 32

law of laplace applied to spherically shaped structures

Answer 32

P = 2 x T / r | two applications: normal alveoli (lung elastic recoil and wob), surfactant deficient alveoli (Pel and wob)

Question 33

is surface tension within the alveolus constant?

Answer 33

yes d/t surfactant, unbalanced water cohesive forces at the ALI but surface tension doesn't depend on the area of the ALI

Question 34

according to laplace's law if the radius is small

Answer 34

the pressure within the sphere is increased

Question 35

Why would having a pressure gradient and small alveoli emptying into larger ones be a problem for ventilation?

Answer 35

bad for gas exchange because the alveoli would collapse requiring much force to inspire

Question 36

per laplace law if there was no surfactant

Answer 36

then smaller alveoli have a higher alveolar pressure

Question 37

surfactant

Answer 37

reduces wob by increasing the compliance of the lung and preventing alveolar collapse

Question 38

surfactant

Answer 38

detergent (dipalmitoylphosphatidylcholine), produced by Type 2 alveolar cells, reduces alveolar surface tension (more in small than larger so it equalizes the pressures)

Question 39

poiseueille's law

Answer 39

describes laminar flow | F = pi r^4 delta P/ 8 n L

Question 40

Flow is directly proportional to

Answer 40

r^4 (radius) and delta P (pressure gradient/change in pressure)

Question 41

Flow is indirectly proportional to

Answer 41

n (viscosity) and L (length)

Question 42

poiseueille's law to resistance

Answer 42

R = 8 n L/ pi r^4

Question 43

resistance is inversely proportional to

Answer 43

r^4

Question 44

resistance is directly proportional to

Answer 44

n and L

Question 45

lower gauge needle does what to flow (r^4)?

Answer 45

increases

Question 46

shorter need length does what to flow (L)?

Answer 46

increase

Question 47

increased hydrostatic pressure does what to flow (delta P)?

Answer 47

increases

Question 48

polycythemic patient has what kind of blood flow (n)?

Answer 48

decreased (want to hydrate and warm sickle cell disease patients)

Question 49

anemic patient has what kind of blood flow (n)?

Answer 49

increased

Question 50

reynolds number

Answer 50

predicts when flow through a tube changes from laminar to turbulent

Question 51

reynolds number is directly proportional to

Answer 51

fluid velocity, tube diameter, fluid density

Question 52

reynolds number is inversely proportional to

Answer 52

viscosity

Question 53

what happens when reynolds number is >2000

Answer 53

flow changes from laminar to turbulent

Question 54

flow becomes turbulent if

Answer 54

velocity is high tube narrows or has kinks/angles wall of tube is rough fluid flows thru an orifice

Question 55

resistance to flow ____ when flow becomes turbulent

Answer 55

increases