Ions in Aqueous Solutions & Colligative Properties
Part I: Dissociation & Ionization
 all _____, whether _____ or _________ (covalent), tend to _____ _____ when they
________ in water (thus creating an ________ solution). However, ionic solids behave
very __________ from molecular solids.
 dissociation = the separation of ____ that occurs when
an _____ compound dissolves. Example: sodium chloride
dissolving in water:
NaCl(s)
H2O
Na+(aq) + Cl-(aq)
 the ions formed in the ___________ process are the ions that were already
________ in the ionic compound, not ______ _________ ions.
 most ionic compounds are ________ (meaning they will dissociate _________)
in water, but not all of them are.
 ionization = process of ________ ions from solute __________ by the action of the
_______. Example: hydrochloric acid (HCl) dissolving in water:
HCl
H2O
H+(aq) + Cl-(aq)
 the ions formed in the __________ process are formed where
____ existed before in the ___________ solute compound.
 the ______ to which a molecular compound ionizes depends
on the _______ of _______ in the ____.
 _______ polar bonds, like the one in HCl, ionize __________ (or ____%).
 ____-_______ bonds, like those in _______ acid (CH3COOH)
do ___ ionize completely (more like ___%)
 _________ bonds, such as those in ______ (C7H8) are
_________ in water, and they do not ionize at all (___%).
Part II: Electrolytes
 as mentioned in your solubility notes, solutions can be classified as ____________ or
______________ based on the degree to which they ________ __________.
 another way of _____________ solutions is as _______ or _____ electrolytes.
 strong electrolyte = any __________ (or _____ to completely) dissociated/ ionized
compound in ________ solution. Conducts electricity _________.
 examples: ____, _____, _____
 weak electrolyte = any compound in aqueous solution that does ___ completely
dissociate/ionize. Conducts electricity _________.
 examples: _______ acid (CH3COOH), ____
 do not confuse a “strong” __________ with a “strong” ______________ solution.
 strong and weak electrolytes differ in the _________________________________.
 concentrated and dilute solutions differ in the __________________________ in a
given quantity of solvent.
Part III: Colligative Properties
 colligative property = property of a substance that depends on the _____________ of
_______ particles in a ___________ but not on their _________.
 concentration is always ___________ as ________ (m) when calculating the effects of
colligative properties on substances, never as _________ (M).
 several colligative properties exist:
1. Vapor Pressure Lowering
 vapor pressure = the pressure on the _______ of a liquid caused by __________ that
have __________ from the ______ phase to the ____ phase.
 a ____ substance (no solute, just _______) has nothing in it to _________ the
concentration of _______ molecules near the _______ of the liquid. Thus, molecules
of solvent _____ _______ the surface and there will be ____ vapor pressure as a
result of the _______ rate of escape.
 a ________ (with solute in the solvent)
has particles of ______ in it that
________ the concentration of the
solvent near the surface of the liquid.
Therefore, molecules of solvent do ____
escape the surface as easily as they
would if the solute particles were ___
_____, and there will be ___ vapor
pressure as a result of the ______ rate of
escape.
 thus, the addition of a _______ to a
solvent ______ the vapor pressure of the
_______ (in other words, higher __ = ______ vapor pressure).
 important to note: the _______ of the solute does not make a difference—only the
____________ of the solute! A 1 m aqueous solution of _______ lowers the VP of
water just as much as a 1 m aqueous solution of ________ does.
2. Freezing Point Depression (FPD)
 freezing point (f.p.) = ___________ at which a substance freezes.
 a pure substance (no solute, just solvent) has nothing in it interfere with the _______________ (freezing) process. Thus, molecules of solvent easily __________ and
there will be ______ freezing point as a result of the ______ ability to crystallize.
 a solution (with solute in the solvent) has particles of solute in it that _________ with
the crystal-forming (freezing) process. Therefore, molecules of solvent do ___ easily
crystallize and there will be ______ freezing point as a result of the __________ in
crystallizing.
 thus, the addition of a solute to a solvent ____________ (lowers) the freezing point of
the _______ (in other words, higher m = ______ f.p.).
 important to note: the ________ of the solute does not make a difference—only the
_____________ of the solute! A 1 m aqueous solution of glucose lowers the f.p. of
water just as much as a 1 m aqueous solution of sucrose does.
3. Boiling Point Elevation (BPE)
 boiling point (b.p.) = _____________ at which a substance boils (becomes a ___
from a liquid at ___ _____ ___________ the liquid, not just the _______).
 a pure substance (no solute, just
solvent) has nothing in it interfere with
the ___ _______-_______ (boiling)
process. Thus, molecules of solvent
______ form gas bubbles and there will
be _____ boiling point as a result of the
______ ability to form gas bubbles.
 a solution (with solute in the solvent)
has particles of solute in it that
__________ with the gas bubbleforming (boiling) process. Therefore,
molecules of solvent do ___ easily form
gas bubbles and there will be ______
boiling point as a result of the __________ in forming gas bubbles.
 thus, the addition of a solute to a solvent _______ (raises) the boiling point of the
solvent (in other words, higher m = _______ b.p.).
 important to note: the _______ of the solute does not make a difference—only the
_____________ of the solute! A 1 m aqueous solution of glucose raises the b.p. of
water just as much as a 1 m aqueous solution of sucrose does.