Study Set Content:
pKa determination can be calculated by
Henderson Hasselbalch equation
FACTORS THAT AFFECT SOLUBILITY OF A SUBSTANCE
● pH
● Temperature
● Polarity
● Size and shape of particle
● Cosolvency
● Molecule configuration and type of crystal arrangement (symmetric < asymmetric)
depend on the quantity of solute dissolved in the solvent rather than the identity of the solute.
Colligative properties of solutions
The phenomenon of (blank) will be examined quantitatively as an example of a colligative property
freezing point lowering
When a solute is dissolved in a solvent, the properties of the solvent are changed by the
presence of the solute
The (blank) of the change generally is proportional to the amount of solute added
magnitude
Some properties of the solvent are changed only by the (blank), without regard to the particular nature of the solute.
number of solute particles present
Such properties are called (blank) of the solution
colligative properties
Colligative properties include changes in
vapor pressure, boiling point, freezing point, and osmotic pressure
For example, if a nonvolatile, nonionizing solute is added to a volatile solvent (such as water), the amount of solvent that can escape from the surface of the liquid at a given temperature is (blank), relative to the case where only the pure solvent is present
lowered
The vapor pressure above such a solution will be (blank) than the vapor pressure above a sample of the pure solvent under the same conditions.
lower
Molecules of (blank) physically block the surface of the solvent, thereby preventing as many molecules from evaporating at a given temperature.
nonvolatile solute
The presence of a solute often causes the vapor pressure to
drop
This is because the solute particles fill positions that are normally occupied by (blank). Thus fewer solvent molecules escape the solution.
solvent molecules
The partial pressure exerted by any component of an ideal solution is equal to the vapor pressure of the pure component multiplied by its mole fraction in the solution
Raoult’s law
The presence of solutes often raises the (blank) of the solutions.
boiling point
1 mole of particles in 1 kg of water elevates the boiling point of water by
0.512 degreesC
The more concentrated a solution is, the (blank) the boiling point elevation will be.
greater
The boiling point of pure water is 100°C, but that boiling point can be elevated by the adding of a solute such as a
salt
A solution typically has a measurably higher boiling point than the
pure solvent
