Solutions and solubility Flashcards

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1
Q

solution

A

a homogenous mixture of 2 or more substances

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2
Q

solubility

A

the number of parts of solvent (by volume) that willdissolve one part of solute (by weight)

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3
Q

unsaturated solution

A

more solutedissolves.
No solid remains inflask.

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4
Q

saturated solution

A

no more solute dissolves. Undissolved solid remains in flask.

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5
Q

supersaturated solution

A

more solute than is normally possible.
Becomes unstable,crystals form

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6
Q

Aqueous solubility of a drug

A

the concentration at which the solution is said to besaturated. Any further addition of the drug will result in drug precipitation

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7
Q

when the components of a solution are of the same phase, are we more likely to talk in terms of miscibility or solubility?

A

miscibility

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8
Q

is dissolution the same as reaction
how would you tell a dissolution from a reaction

A

no
dissolution is a physical change, and can be reversed to the original state by evaporation
if this cannot be done then it is a reaction

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9
Q

pros of pharmaceutical solutions

A

Liquids easier to swallow more acceptable by paediatric and geriatric pts

Faster therapeutic response

Uniform distribution of drug through out the preparation, c.f.suspensions andemulsions.

Reduced irritation to the gastric mucosa

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10
Q

Classification of solutions based on solvent polarity

A

aqueous and non aqueous

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11
Q

advantages of aqueous solutions

A

Lack of toxicity
Non-expensive
Physiological compatibility

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12
Q

disadvantages of aqueous solutions

A

could cause hydrolysis of some drugs

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13
Q

has to do with dissolution

why is the maximum level of solubility pharmaceutically important

A

because it dictates the rate of dissolution

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14
Q

how soluble are the following salts of drugs in water? and how are their respective solubility determined?
atropine sulfate
codeine phosphate
codeine sulfate
morphine sulfate
phernobarbital sodium

A

very soluble
freely soluble
sparingly soluble
soluble
freely soluble

determined by measuring the weight of solvent required to dissovle 1 gram of the solute or the drug

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15
Q

why are the salts of drugs typically more soluble than the free base or uncahrged form of the drug itself

A

due to differences in their chemical properties like different ionization states, different intermolecular forces btn structure and polarity…etc

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16
Q

types of water

A

portable
purified
water used for injections

17
Q

portable water

A

Water freshly drawnfrom the public watersupply (main system)and suitable fordrinking.

18
Q

purified water

A

Freshly boiled andcooled immediately before use to destroymicroorganisms

19
Q

porperties of water used for injections

A

is sterile
CO2-free
low electrical conductivity
low endotoxins
high purity
absence of pyrogens…etc

20
Q

types of pharmaceutical solutions

A

Solid-in-liquid
Liquid-in-liquid
Solid-in-solid
Gas-in-gas
Gas-in-liquid

21
Q
A
21
Q

liquid in liquid solution

A

A liquid-in-liquid solution is a one-phase molecular dispersion of twoliquids which are MISCIBLE with each other (e.g. ethanol and water).

22
Q

Solid-in-solid solutions

what do solid in solid solutions result to

A

A solid-in-solid solution is a molecular dispersion of a solid solute ina solid solvent.

the formation of a mixed crystal of both components

23
Q

importance of a solid-in-solid solution

A

can be used to enhance the dissolution of a poorly soluble drug.

24
Q

total moles of a solution formula

A

moles of solute + moles of solvent

25
Q

molarity (Formula)
molality (formula)

A

The number of moles of solute in ONE litre of solvent (moles of solute/ volume of solution)

The number of moles of solute in ONE kg of solvent (moles of solute/ mass of solvent)

26
Q

why is molality preferrable to molarity

A

It is independent of solution temperature (volume can change with temperature).It is unaffected by addition of another solute

27
Q

facotrs affecting solubility

A

particle size
pressure
temperature
polarity
polymorphs

28
Q

straight chain monohydric organic compounds like alcohols, with four or five carbon atoms cannot enter the hydrogen bonded structure of water, true or false

A

true, hence they are only slightly soluble

29
Q

ways to enhance solubility

A

co-solvency
pH adjustment
chemical modification
salt formation
adjusting temperature
particle size control

30
Q
A
31
Q

How does temperature influence the solubility of gases in liquids?
reason for answer

A

Generally, the solubility of gases in liquids decreases with increasing temperature.

Increasing temperature imparts greater kinetic energy to gas molecules, weakening the intermolecular forces between gas and liquid. This reduces gas solubility in liquids, as higher energy levels hinder the formation of stable gas-liquid interactions.

32
Q

What is the purpose of using solubility charts or tables in pharmacy?

A

provide information on the maximum amount of solute that can dissolve in a given solvent under specific conditions.

33
Q
A