saturated solution
one in which solute is in equilibrium with the solid phase
solubility
concentration of solute in a saturated solution.
unsaturated solution
a solution in which drug is present below its solubility.
supersaturated solution
contains more solute than a saturated solution. It is very UNSTABLE and generally precipitation occurs with agitation, seed crystals, or scratching the container side.
ionization
Solubility of weak electrolytes is affected by ____
absorption, distribution, elimination
Which aspects of ADME does ionization affect in regards to solubility?
adjust pH so that drug is ionized
How do you increase the solubility of weak electrolytes?
increase
In regards to a weak acid, raising the pH will have what effect on its solubility?
decrease
In regards to a weak acid, lowering the pH will have what kind of effect on its solubility?
So
intrinsic solubility
S
apparent solubility
Intrinsic solubility
the solubility of the compound in its free acid or free base form.
Apparent solubility
is the experimentally determined solubility of a solute in a solvent system and may be higher or lower than the equilibrium
diminishes solubility
What is the common ion effect on solubility ?
slightly increases solubility
What is the effect of not in common ions on solubility?
decreases; decreases dissociation of weak electrolyte by increasing pKa
How does the addition of a co-solvent to water affect solubility & why?
Solubility Product (Ksp)
is the product of the concentrations of each ion raised to a power equal to the stoichiometriccoefficient (number of ions appearing in the formula).
add citrate
How do you increase solubility of iron?
add something that will remove another ion
How do you increase solubility of slightly soluble salt?
Exothermic
this reaction causes an increase in temperature and the heat released from this reaction causes a decrease in solubility.
Endothermic
this reaction causes an increase in temperature, and more heat is absorbed; causing solubility to increase.
True
Increasing unsaturation causes an increase in solubility in polar solvents. T/F?