Chapter 13 – Physical Properties of Solutions
Section 13.1 – Types of Solutions
What is a solution?
solvent and one or more
A solution consists of a _________
________.
solutes
What is meant by an aqueous solution? is a solution where the
Solutions can be classified by the amount of solute solvent is
the maximum amount water.
dissoved relative to ___________________
______________________________________________
that can be dissolved
______________________________.
The amount of solute dissolved in a given
Define solubility: volume of a saturated solution.
Explain the difference between a saturated, unsaturated,
and supersaturated solution:
saturated : contains the max amt . . of solute that will dissolve in a solvent at a specific temp.
·
unsaturated : contains less solute than it has the
-
capacity to dissolve
·
supersaturated : contains more solute than is present in a saturated solution (above capacity
Give an example of a gaseous solution:
air-has N2 O2 and CO2 evenly distributed (homogenous
, ,
Give an example of a solid solution:
brass-mixture of copper + zinc
Give an example of a liquid solution:
Saltwater
Section 13.2 – A Molecular View of the Solution
Process
Define solvation: process by which solute molecules are surrounded
by solvent molecules
The ease with which solute molecules are separated from
, one another and surrounded by solvent molecules
depends on the relative strengths of
____________________________,
the solute-solute attractive forces
__________________________________,
the solvent-solvent attractive forces and
__________________________________.
the solute-solvent attractive forces
What are the 4 types of intermolecular forces (either
solute-solute or solvent-solvent) that occur in pure
substances? Dispersion forces present in all substances ,
-
dipole-dipole -
present in
polar molecules , Hydrogen bonding -
H-0 ,
H-N , H-Fonly &
Solute-solvent attractions can exhibit any of the 4 lon-dipole present
- in
ionic substances
intermolecular forces listed above, or they can exhibit ion-
dipole, dipole-induced dipole, or ion-induced dipole forces.
For each of these intermolecular forces, write the definition
and provide an example:
• Ion-dipole: The charge of an ion is attracted to the partial charge on a
polar molecule
EX) NaCl in H20 Dat
• Dipole-induced dipole:The partial charge on a polar molecule induces A
EX)(O2 in H20--re temporary partial charge
nonpolar molecule/atom.
neighboring on a
• Ion-induced dipole:The charge of an ion induces a temporary partial charge
on neighboring nonpolar molecule/atom
In your own words, summarize the 3 distinct steps used to
describe the solution process in Figure 13.3, including
whether each step in endothermic or exothermic:
1 The separation of solute molecules from one another
.
of solvent molecules from one another
.The
C separation
overcome IMF attractions ,
/both of these 2 steps require an input of energy to
so they are both endothermic REMINDER :
mix
. The solvent
3 + solute molecules ·
Endothermic rxn absorbs energy
(this process is exothermic ·
Exothermic oxu releases energy
Is the overall solution process usually endothermic or
Section 13.1 – Types of Solutions
What is a solution?
solvent and one or more
A solution consists of a _________
________.
solutes
What is meant by an aqueous solution? is a solution where the
Solutions can be classified by the amount of solute solvent is
the maximum amount water.
dissoved relative to ___________________
______________________________________________
that can be dissolved
______________________________.
The amount of solute dissolved in a given
Define solubility: volume of a saturated solution.
Explain the difference between a saturated, unsaturated,
and supersaturated solution:
saturated : contains the max amt . . of solute that will dissolve in a solvent at a specific temp.
·
unsaturated : contains less solute than it has the
-
capacity to dissolve
·
supersaturated : contains more solute than is present in a saturated solution (above capacity
Give an example of a gaseous solution:
air-has N2 O2 and CO2 evenly distributed (homogenous
, ,
Give an example of a solid solution:
brass-mixture of copper + zinc
Give an example of a liquid solution:
Saltwater
Section 13.2 – A Molecular View of the Solution
Process
Define solvation: process by which solute molecules are surrounded
by solvent molecules
The ease with which solute molecules are separated from
, one another and surrounded by solvent molecules
depends on the relative strengths of
____________________________,
the solute-solute attractive forces
__________________________________,
the solvent-solvent attractive forces and
__________________________________.
the solute-solvent attractive forces
What are the 4 types of intermolecular forces (either
solute-solute or solvent-solvent) that occur in pure
substances? Dispersion forces present in all substances ,
-
dipole-dipole -
present in
polar molecules , Hydrogen bonding -
H-0 ,
H-N , H-Fonly &
Solute-solvent attractions can exhibit any of the 4 lon-dipole present
- in
ionic substances
intermolecular forces listed above, or they can exhibit ion-
dipole, dipole-induced dipole, or ion-induced dipole forces.
For each of these intermolecular forces, write the definition
and provide an example:
• Ion-dipole: The charge of an ion is attracted to the partial charge on a
polar molecule
EX) NaCl in H20 Dat
• Dipole-induced dipole:The partial charge on a polar molecule induces A
EX)(O2 in H20--re temporary partial charge
nonpolar molecule/atom.
neighboring on a
• Ion-induced dipole:The charge of an ion induces a temporary partial charge
on neighboring nonpolar molecule/atom
In your own words, summarize the 3 distinct steps used to
describe the solution process in Figure 13.3, including
whether each step in endothermic or exothermic:
1 The separation of solute molecules from one another
.
of solvent molecules from one another
.The
C separation
overcome IMF attractions ,
/both of these 2 steps require an input of energy to
so they are both endothermic REMINDER :
mix
. The solvent
3 + solute molecules ·
Endothermic rxn absorbs energy
(this process is exothermic ·
Exothermic oxu releases energy
Is the overall solution process usually endothermic or
