Lecture 4 Flashcards Preview

Pharm202 > Lecture 4 > Flashcards

Flashcards in Lecture 4 Deck (47):
1

What is the relationship between the number of phases and the number of degrees of freedom?

the more phases we have the less degrees of freedom we have.

2

How many degrees of freedom in a system of 3 components and 1 phase?

4

3

How can we simplify a 4 dimensional graph?

by making two variables constant. e.g. temperature and pressure.

now the only thing we have to worry about is the 2 concentrations

4

which diagram is used to show this?

the triangular diagram which describes the concentration of the 3 different components of the system.

the apex/corners of the triangles are 100%

The area of the triangle represents all the possible combinations of the 3 components.
Everywere on the line you have a constant ratio of 2 of the components but the 3rd component is changing

5

in a ternary phase diagram with a pair of partially miscible liquids, how many regions are there?

2,
1 region everything is completely miscible and the other region, everything is not miscible

6

How can we draw tie lines in this ternary phase triangluar diagram?

We can start at 100% water and add in bezene or vie versa.

7

why is the angle of the tie line not always horizontal in this case of a ternary phase diagram?

it depends on how miscible the substances are.
if the 3rd liquid has an equal effect on both immiscible liquids then the tieline might be parallel to the base

8

What is usually used as a constant and why?

pressure is fine to be a constant but temperature tends to vary a lot.

e.g. something at a certain phase at room temperature may be different inside the body at 37degrees

9

How can we study the effects of temperature on these systems?

we can construct these systems at different temperatures

10

what is the effect of temperature on the systems?

as temperature increases, the darker 2-phase region decreases because higher temperatures increase solubility so the one phase system increases

11

What does a solution require?

a solute and a solvent

12

what is a solute?

the substance that gets dissolved

13

what is a solvent

the substance that does the dissolving

14

Why cant you see clumps of a solutuion?

because it is a molecular dispersion

15

What does a molecular dispersion mean?

what has been dissolved has been broken apart to the level of indivdual molecules.

it is a 1 phase system where there are no boundaries or distinct regions

16

what types of solutes are there?

electrolytes and non-electrolytes

17

Why can electrolytes conduct electrcity?

Electrolytes ionise in water, they break apart into ions which are charged, so can conduct electricty

18

are most drugs electrolytes?

yes

19

what is the difference between strong electrolytes and weak electrolytes?

strong electrolytes completely ionise in water,

weak ones only partially ionise in water

20

Why are there huge implications for electrolytes and solutions?

for something to be absorbed into the body, it has to be in liquid

21

What are the properties of a good drug considering the stomach is an aqueous environment?

a good drug should be ionised as ionised substances dissolve better in aqueous solutions so is more likely to dissolve in your gastric contents, ECF or your eye

22

What must the drug cross if we want it to be absorbed into the body?

a lipid bilayer membrane.

23

What form of the drug dissolves better through the lipid bilayer membrane?

the unionised form as it is not charged

24

What are the implications for non electrolytes like progesterone?

it will not dissolve in gastric contents and hence not available in absoprtion but can cross the skin.

This is why trasdermal progesterone formulations exist.

It also has relevance to colligative proerpties

25

What is bioavailability?

how much of the administered drug reaches your systemic circulation
often expressed as a %

26

What is electrolysis?

where a certain potential is applied which causes a current to generate a redox reaction.
However it cannot be used for anything that's unionised as they cannot conduct electrolysis

27

in a solution what does the dissolving?

the solute. this could be either the gas, liquid or solid

28

Is air a solution?

yes as we have many gases and they are molecularly dispersed into one another. There is no phase boundary

29

in pharmaceutics, which kind of solutions are we most interested in?

solutions where the solvent (dissolving agent) is liuid

30

What is an example of solid in liquid solution?

mixing a cup of tea with sugar

31

what is an example of a liquid liquid solution?

mixing alcohol and water

32

what is an example of a gas in liquid solution

a can of coke which has CO2 in the liquid, completely dissolved

33

Can a solute be filtered out from a solution?

no.
you can filter out big grains of something but a solution is a molecular dispersion so you cant filter out individual molecules.

34

What other criteria are there of a solution?

the particles are always in motion
the volumes are not additive.
the 2 things you dissolve can have quite different properties
the dissolving agent appears in a greater extent, and the solute appears to a lesser extent
you may have more than one type solute or solvent

35

What is molarity (M)?

the number of moles in 1L of solution

36

what is molality (m)?

the number of moles per 1000g of solvent

37

What is the relationship between molality and molarity in the example of water?

molarity = molality

however in other solutions, 100g of solvent does NOT = 1L

38

what is % by weight?

the number of g per 100g of solution

39

what is % by volume?

the number of ml per 100ml of solution

40

What is 0.154M NaCl important to us?

it is isontonic saline, isotonic to our bodies

41

What is ideal?

what theoretical scientists want

- no properties to change other than dilution
- no heat
- no expansion or shrinkage
- we want the constitutive properties to be the weighted averages of the individual constituents
- to be formed by mixing substances of similar properties.
- complete uniformity of attractive forces

42

what happens when real solutions are mixted together?

there is a change of some sort, usually evolution of heat

43

what is Raoult's law?

if the solution is ideal, the partial vapour pressure of each volatile constituent is equal to the vapour pressure of the pure constituent multiplied by its mole fraction in the solution

44

What is abvoe the surface of liquid water?

a vapour pressure of molecules

45

What is the mole fraction?

the fraction of moles of a substance in that solution

46

What is the vapour pressure composition curve?

Y axis = vapour pressure on both sides
X axis = mole fraction
at 100% B, vapour pressure is all due to B
When you mix the two solutions in the middle, the total vapour pressure is a weighted pressure of the 2 components of the solution

47

What is the unit of vapour pressure?

psi