| Chemistry
162 Final Review |
| Go
to the Answers page |
| |
|
Solution
Energetics |
| |
|
|
| 1 |
Which
of the following regarding the energetics of solution formation
is false? |
| |
A) |
Separation of solvent and solute molecules is endothermic. |
| |
B) |
Allowing
the separated solute and solvent molecules to mix randomly is exothermic. |
| |
C) |
The formation of an ideal solution has a  H
= 0 and no change in volume. |
| |
D) |
When intermolecular forces between solute and solvent
molecules are stronger than other intermolecular forces, energy is
released as a result of solution formation and the volume of the
solution is less than the sum of the volumes of solute and solvent. |
| |
E) |
A solution with a H
formation > 0 cannot be
formed. |
| |
|
| 2 |
Colligative Properties (Osmotic Pressure) |
| |
|
Which
is the osmotic pressure at 37°C of an aqueous
solution that is 1.80%
CH3CH2OH (mass/vol)? Is this solution isotonic, hypotonic
or hypertonic with respect to the osmotic pressure of a 5.5% (mass/vol) solution
of glucose,
C6H12O6? |
| |
| Reaction Mechanisms |
| |
|
| 3 |
At
temperatures below 600 K, the following reaction exhibits the rate
law:
Rate = k[NO2]2 |
| |
|
NO2 +
CO  NO
+ CO2 |
| |
Propose a two step mechanism involving one fast step
and one slow step that is consistent with the net equation and the
observed rate law. |
| |
|
| Le
Chatelier’s Principle |
| |
|
| 4 |
In which direction will the position of the equilibrium |
| |
|
2HI(g)  H2(g)
+ I2(g) H < 0 |
| |
be shifted for each of the following changes? |
| |
A) |
H2(g) is added |
| |
B) |
I2(g) is removed |
| |
C) |
HI(g) is removed |
| |
D) |
Some Ar(g) is added |
| |
E) |
The volume of the container is doubled |
| |
F) |
The temperature is decreased |
| |
|
Acids and Bases
Salts |
| |
|
| 5 |
For
a solution that is .08M NaOCl |
| |
A) |
write an equation for the hydrolysis reaction that
occurs |
| |
B) |
and
determine the equilibrium constant for this hydrolysis, Ka for
HOCl = 2.9 x 10-8 |
| |
C) |
and the pH |
| |
|
| Common Ion Effect |
| |
|
| 6 |
Calculate the pH of a solution that is .350M CH3CH2COOH
and .0786M
CH3CH2COOK.
Ka of CH3CH2COOH = 1.3 x 10-5. |
| |
|
| Buffers |
| |
|
| 7 |
If
1.00ml of .250M HCl is added to 50.0ml of a buffer solution composed
of .405M HCOOH and .326M HCOONa, what is the pH of
the final solution?
Ka HCOOH = 1.8
x 10-4 |
| |
|
| Titration |
| |
|
| 8 |
In
a titration of 40.0ml of .200M NH3 with .500M
HCl
Kb NH3 =
1.8 x 10-5 with .500M HCL |
| |
A) |
The volume of titrant required to reach the equivalence
point is? |
| |
B) |
Initial pH |
| |
C) |
After the additon of 5.00ml of .500M HCl pH? |
| |
D) |
At the half neutralization point pH? |
| |
E) |
pH at the equivalence point? |
| |
| Go
to the Answers page |
| |
|
