CGIER 34 - Solubility Equilibria Flashcards

1
Q

describe chemical equilibrium

A

reactants are continually converted into products and at the same time products are continually converted into reactants
rate of forward reaction is equal to rate of backward reaction

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

equilibrium constant

A

K equals concentration of products over concentrations of reactants to the power of their stoichiometric coefficient
K is not assigned to a unit

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

what is the rule involved equilibrium constant expression

A

you DO NOT include pure solids or pure liquids

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

how does one determine the equilibrium constant of the forward reaction when we know the equilibrium constant of the reverse reaction

A

Kf = 1/Krev

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

if the K value is greater than 1 it means that the reaction

A

is product favoured - makes more products than reactants

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

if K value is less than 1 it means that the reaction ..

A

is reactant favoured - makes more reactants

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

why is solubility phenomena important in physiology

A

Important for absorption of nutrients
Important for mineralisation processes in biological systems
Applications in drug delivery and diagnostic processes

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

In saturated solutions:
1. ___ ___ exists between 2.__ and 3. __ in solution the rate of 4.___ will equal the rate of 5.___ the concentration of 6. __ in solution will always be 7.___

A
  1. dynamic equilibrium
  2. solids
  3. ions
  4. dissolution (dissolving)
  5. precipitation
  6. ions
  7. constant
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

explain how the rate of dissolution and the rate precipitation is equal in solubility equilibria

A

When ionic solid dissolves and dissociates into its constituents ions the concentrations of these ions increase.
at the same time as these ions are being spread across the solution it increase chance of this dissociated ions to collide to form a solid again

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

how would one calculate the equilibrium constant of solubility product or Ksp

A

find concentration of dissolved to the power of their stoichiometric coefficient ONLY because we don’t include pure solids in our equation

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

solubility product constant Ksp

A

the constant for the equilibrium established between a solid solute and its ions in a saturated solution

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

why do we not include solid in solubility product constant Ksp

A

more solid
greater surface area
more solid exposed to solution -> greater solubility
as solubility increases so does precipitation
greater surface area for ions to precipitate
increase chance of ions reforming into a solid

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

under what conditions can solubility product values change

A

can have infinite number of values depending on temperature, pH or common ion

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

molar solubility

A

the no. moles a substance can be dissolved in 1 litre of solution upon reaching saturation (amount of moles dissolved in a litre of a solution)

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

how is molar solubility calculated?

A

using substances solubility product constant and stoichiometric coefficients of substance components
using units mol/L

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

when is solubility product constant Ksp reliable

A

only if the solid has the same ratio of cations to anions

17
Q

how does common ions influence solubility

A

if a solid is dissolved in a solution in which the solution and solid share a common ion according to Le Chatelier’s Principle some of the common ions will add extra product and that extra product will be used to make reactants, shifts more towards the solid - decreases solubility

18
Q

how does pH influence solubility of solids e.g. decreasing the pH in which the product is basic

A

pH decreases when the product is basic = removing product as decreasing pH means you are adding H+
system shifts in favour of product sides and increases products thus increasing solubility

19
Q

applications of solubility in healthcare

A

modify substances to favour solubility characteristics for drug development and dental health

20
Q

how can substances with low molar solubility be useful in medicine

A

barium sulphate is used as a contrasting agent for diagnostics is administered as a suspension (insoluble in all media so must be administered as tablet, capsule or in this case suspension)
barium is toxic - but its low solubility means it is not absorbed by the patient

21
Q

how does solubility affect oral hygiene

A

bacteria in teeth decrease pH and make the main component of teeth hydroxyapatite more soluble
rate of dissolution is greater than rate of precipitation

22
Q

how does the involvement of molar solubility prove that fluoridation is somewhat beneficial in water treatment

A

fluorapatite dissociates to release F- ions and NOT OH- ions
as the pH decreases fluorapatite is less soluble and reduces probability of developing tooth decay

23
Q

solubility

A

how quickly ionic compounds dissociate into their constituent ions

24
Q

how can we modify drug solubility

A

form it into a salt

25
Q

what are the exceptions to converting drugs into salts to increase solubility

A

certain counter ions and if the solution contains a common ion

26
Q

solubility of drugs in aqueous media can be very dependent on ___ this can impact ___

A

salt form ie. type of counter ions

salt of a drug for use in formulations

27
Q

what must be taken into consideration when developing drugs for oral administration?

A

must take into account the high concentrations of Cl- ions in the stomach
poorly soluble salts containing a Cl- counter ion may precipitate and therefore become less available for absorption due to common effect