...

In-Class Questions

by user

on
Category:

geometry

136

views

Report

Comments

Transcript

In-Class Questions
13.1
What is the solute when 10 g of NaCl is dissolved
in 100 mL of water?
1.
2.
3.
4.
5.
Tro IC3
NaCl
Na
Cl2
H2O
None of the above
13.1
What is the solute when 10 g of NaCl is dissolved
in 100 mL of water?
1.
2.
3.
4.
5.
Tro IC3
NaCl
Na
Cl2
H2O
None of the above
13.2
Which solvent would be most suitable to remove
grease from an object?
1.
2.
3.
4.
5.
Tro IC3
H2O
NH3
CH3OH
CH3OCH3
C8H18
13.2
Which solvent would be most suitable to remove
grease from an object?
1.
2.
3.
4.
5.
Tro IC3
H2O
NH3
CH3OH
CH3OCH3
C8H18
13.3
Which of the following substances is an example of
a solution?
1.
2.
3.
4.
5.
Tro IC3
Salad dressing
Blueberry muffin
Wine
Sugar
Lead
13.3
Which of the following substances is an example of
a solution?
1.
2.
3.
4.
5.
Tro IC3
Salad dressing
Blueberry muffin
Wine
Sugar
Lead
13.4
In theory which of the following would have the
highest solubility in gasoline (C8H18) ?
1.
2.
3.
4.
5.
Tro IC3
CH3CH2CH3
CH3OCH3
CH3CH2OH
CH3CH2NH2
CH3CH2COOH
13.4
In theory which of the following would have the
highest solubility in gasoline (C8H18) ?
1.
2.
3.
4.
5.
Tro IC3
CH3CH2CH3
CH3OCH3
CH3CH2OH
CH3CH2NH2
CH3CH2COOH
13.5
A supersaturated solution:
1. Holds less than the maximum amount of solute at that
temperature
2. Holds the maximum amount of solute at that
temperature
3. Holds more than the normal maximum amount of solute
at that temperature
4. All of above
5. None of the above
Tro IC3
13.5
A supersaturated solution:
1. Holds less than the maximum amount of solute at that
temperature
2. Holds the maximum amount of solute at that
temperature
3. Holds more than the normal maximum amount of solute
at that temperature
4. All of above
5. None of the above
Tro IC3
13.6
Which of the following NaCl solutions has the
highest concentration of NaCl?
1.
2.
3.
4.
5.
Tro IC3
0.0175 mol NaCl in 1 L of solution
0.1 g NaCl in 100 mL of solution
0.5 g NaCl in 500 mL of solution
0.25 mol NaCl in 200 mL of solution
All have the same concentration.
13.6
Which of the following NaCl solutions has the
highest concentration of NaCl?
1.
2.
3.
4.
5.
Tro IC3
0.0175 mol NaCl in 1 L of solution
0.1 g NaCl in 100 mL of solution
0.5 g NaCl in 500 mL of solution
0.25 mol NaCl in 200 mL of solution
All have the same concentration.
13.7
Which of the following would be worst at
conducting electricity?
1.
2.
3.
4.
5.
Tro IC3
NaCl (aq)
NH4NO3 (aq)
H2O (l)
MgCl2 (aq)
HF (aq)
13.7
Which of the following would be worst at
conducting electricity?
1.
2.
3.
4.
5.
Tro IC3
NaCl (aq)
NH4NO3 (aq)
H2O (l)
MgCl2 (aq)
HF (aq)
13.8
How is the solubility of a gas affected by the
temperature of the solution?
1. Solubility increases with increasing temperature.
2. Solubility increases with decreasing temperature.
3. Solubility remains the same with increasing
temperature.
4. Solubility decreases with decreasing temperature.
5. Two of the above
Tro IC3
13.8
How is the solubility of a gas affected by the
temperature of the solution?
1. Solubility increases with increasing temperature.
2. Solubility increases with decreasing temperature.
3. Solubility remains the same with increasing
temperature.
4. Solubility decreases with decreasing temperature.
5. Two of the above
Tro IC3
13.9
Which type of interaction must be strong in order to
dissolve a salt?
1.
2.
3.
4.
5.
Tro IC3
Solvent–solvent
Solvent–solute
Solute–solute
Solvent–solution
All of the above
13.9
Which type of interaction must be strong in order to
dissolve a salt?
1.
2.
3.
4.
5.
Tro IC3
Solvent–solvent
Solvent–solute
Solute–solute
Solvent–solution
All of the above
13.10
If the solubility of potassium nitrate at 20 °C is 37 g
per 100 g of water, how many grams of the
compound will dissolve in 1.0 mL of water?
1.
2.
3.
4.
5.
Tro IC3
37
g
3.7
g
0.37 g
0.0037 g
370
g
13.10
If the solubility of potassium nitrate at 20 °C is 37 g
per 100 g of water, how many grams of the
compound will dissolve in 1.0 mL of water?
1.
2.
3.
4.
5.
Tro IC3
37
g
3.7
g
0.37 g
0.0037 g
370
g
13.11
What happens to the solubility of a gas when the
pressure above a liquid increases?
1.
2.
3.
4.
5.
Tro IC3
The solubility remains the same
The solubility increases
The solubility decreases
It depends on the chemical nature of the gas
It depends on the numerical value of the
pressure
13.11
What happens to the solubility of a gas when the
pressure above a liquid increases?
1.
2.
3.
4.
5.
Tro IC3
The solubility remains the same
The solubility increases
The solubility decreases
It depends on the chemical nature of the gas
It depends on the numerical value of the
pressure
13.12
How many grams of KNO3 are in a 125-g
solution containing 14.5% solute?
1.
2.
3.
4.
5.
Tro IC3
12.5 g
14.5 g
18.1 g
111 g
862 g
13.12
How many grams of KNO3 are in a 125-g
solution containing 14.5% solute?
1.
2.
3.
4.
5.
Tro IC3
12.5 g
14.5 g
18.1 g
111 g
862 g
13.13
The molarity of a solution is defined as
the number of:
1.
2.
3.
4.
5.
Tro IC3
Moles of solute per liter of solution
Moles of solute per kg of solution
Grams of solute per liter of solution
Moles of solute per kg of solvent
Grams of solvent per kg of solution
13.13
The molarity of a solution is defined as
the number of:
1.
2.
3.
4.
5.
Tro IC3
Moles of solute per liter of solution
Moles of solute per kg of solution
Grams of solute per liter of solution
Moles of solute per kg of solvent
Grams of solvent per kg of solution
13.14
Calculate the mass percent of 2.50 moles of NaOH
in 0.900 L of water at 25 °C? Hint: The density of
water is 1.00 g/mL at 25 °C.
1.
2.
3.
4.
5.
Tro IC3
10.0%
9.09%
71.4%
2.50%
40.0%
13.14
Calculate the mass percent of 2.50 moles of NaOH
in 0.900 L of water at 25 °C? Hint: The density of
water is 1.00 g/mL at 25 °C.
1.
2.
3.
4.
5.
Tro IC3
10.0%
9.09%
71.4%
2.50%
40.0%
13.15
What is the molarity of a KNO3 solution containing
2.45 mol KNO3 in 500 mL of solution?
1.
2.
3.
4.
5.
Tro IC3
0.049 M
204 M
2.45 M
0.500 M
4.90 M
13.15
What is the molarity of a KNO3 solution containing
2.45 mol KNO3 in 500 mL of solution?
1.
2.
3.
4.
5.
Tro IC3
0.049 M
204 M
2.45 M
0.500 M
4.90 M
13.16
What is the molarity of NaOH in a solution
containing 40.0g of NaOH in 750 mL of solution?
1.
2.
3.
4.
5.
Tro IC3
53.3
M
1.33
M
0.00133 M
4.00
M
0.0533 M
13.16
What is the molarity of NaOH in a solution
containing 40.0g of NaOH in 750 mL of solution?
1.
2.
3.
4.
5.
Tro IC3
53.3
M
1.33
M
0.00133 M
4.00
M
0.0533 M
13.17
Calculate the volume of 0.250 M solution made by
dissolving 5.56 g of solid magnesium chloride in
water.
1.
2.
3.
4.
5.
Tro IC3
0.234 mL
0.250 mL
1.39 mL
14.6 mL
234 mL
13.17
Calculate the volume of 0.250 M solution made by
dissolving 5.56 g of solid magnesium chloride in
water.
1.
2.
3.
4.
5.
Tro IC3
0.234 mL
0.250 mL
1.39 mL
14.6 mL
234 mL
13.18
A practical problem. How could you safely prepare
500 mL of 1.00 M H2SO4 solution from a 12.4 M
H2SO4 stock solution? Select the closest answer.
1.
2.
3.
4.
5.
Tro IC3
Add 40.3 mL of 12.4 M stock to 500 mL of water.
Add 12.4 mL of 12.4 M stock to 500 mL of water.
Add 40.3 mL of 12.4 M stock to 459.7 mL of water.
Add 459.7 mL of water to 40.3 mL of 12.4 M stock.
Add 500 mL of water to 40.3 mL of 12.4 M stock.
13.18
A practical problem. How could you safely prepare
500 mL of 1.00 M H2SO4 solution from a 12.4 M
H2SO4 stock solution? Select the closest answer.
1.
2.
3.
4.
5.
Tro IC3
Add 40.3 mL of 12.4 M stock to 500 mL of water.
Add 12.4 mL of 12.4 M stock to 500 mL of water.
Add 40.3 mL of 12.4 M stock to 459.7 mL of water.
Add 459.7 mL of water to 40.3 mL of 12.4 M stock.
Add 500 mL of water to 40.3 mL of 12.4 M stock.
13.19
What volume of 0.100 M sodium hydroxide is
required to completely neutralize 50.0 mL of
0.100 M phosphoric acid?
1.
2.
3.
4.
5.
Tro IC3
50.0 mL
100. mL
150. mL
200. mL
250. mL
13.19
What volume of 0.100 M sodium hydroxide is
required to completely neutralize 50.0 mL of
0.100 M phosphoric acid?
1.
2.
3.
4.
5.
Tro IC3
50.0 mL
100. mL
150. mL
200. mL
250. mL
13.20
35.0 mL of 0.155 M lead(II) nitrate and 45.0 mL of
0.287 M potassium chloride are mixed. How much
precipitate is produced?
1.
2.
3.
4.
5.
Tro IC3
0.877 g
1.25 g
1.51 g
1.80 g
3.59 g
13.20
35.0 mL of 0.155 M lead(II) nitrate and 45.0 mL of
0.287 M potassium chloride are mixed. How much
precipitate is produced?
1.
2.
3.
4.
5.
Tro IC3
0.877 g
1.25 g
1.51 g
1.80 g
3.59 g
13.21
Which of the following is NOT an example of a
colligative property?
1.
2.
3.
4.
5.
Tro IC3
Osmotic pressure
Freezing point depression
Boiling point depression
Boiling point elevation
All are colligative properties.
13.21
Which of the following is NOT an example of a
colligative property?
1.
2.
3.
4.
5.
Tro IC3
Osmotic pressure
Freezing point depression
Boiling point depression
Boiling point elevation
All are colligative properties.
13.22
Calculate the molality of a solution containing 0.455
mol of sucrose (table sugar) and 1.00 L of water at
a temperature at which the water has a density of
1.00 g/mL.
1.
2.
3.
4.
5.
Tro IC3
0.455
m
455
m
0.910
m
910.
m
4.55 x 10-4 m
13.22
Calculate the molality of a solution containing 0.455
mol of sucrose (table sugar) and 1.00 L of water at
a temperature at which the water has a density of
1.00 g/mL.
1.
2.
3.
4.
5.
Tro IC3
0.455
m
455
m
0.910
m
910.
m
4.55 x 10-4 m
13.23
What is the freezing point of a 0.75 m aqueous
solution of calcium chloride?
(Note: Kf = 1.86 °C·kg/molparticles.)
1. -1.4 °C
2. 1.4 °C
3. 4.2 °C
4. 0.0 °C
5. -4.2 °C
Tro IC3
13.23
What is the freezing point of a 0.75 m aqueous
solution of calcium chloride?
(Note: Kf = 1.86 °C·kg/molparticles.)
1. -1.4 °C
2. 1.4 °C
3. 4.2 °C
4. 0.0 °C
5. -4.2 °C
Tro IC3
13.24
To the nearest degree, calculate the boiling point of
an aqueous solution containing 36 g NaCl in 100 ml
of water. (Note: Kb = 0.512 °C·kg/molparticles.)
1.
2.
3.
4.
5.
Tro IC3
6 °C
94 °C
97 °C
103 °C
106 °C
13.24
To the nearest degree, calculate the boiling point of
an aqueous solution containing 36 g NaCl in 100 ml
of water. (Note: Kb = 0.512 °C·kg/molparticles.)
1.
2.
3.
4.
5.
Tro IC3
6 °C
94 °C
97 °C
103 °C
106 °C
13.25
A red blood cell with an inner concentration of 0.9 g
NaCl per 100 mL of solution is placed into a 2.0 g
NaCl per 100 mL solution. The cell:
1.
2.
3.
4.
5.
Tro IC3
Shrinks
Swells
Leaks
Bursts
Two of the above
13.25
A red blood cell with an inner concentration of 0.9 g
NaCl per 100 mL of solution is placed into a 2.0 g
NaCl per 100 mL solution. The cell:
1.
2.
3.
4.
5.
Tro IC3
Shrinks
Swells
Leaks
Bursts
Two of the above
13.26
What is the freezing point of a 0.75 m aqueous
solution of table sugar (sucrose)?
(Note: Kf = 1.86 °C·kg/molparticles.)
1. -1.4 °C
2. 1.4 °C
3. 4.2 °C
4. 0.0 °C
5. -4.2 °C
Tro IC3
13.26
What is the freezing point of a 0.75 m aqueous
solution of table sugar (sucrose)?
(Note: Kf = 1.86 °C·kg/molparticles.)
1. -1.4 °C
2. 1.4 °C
3. 4.2 °C
4. 0.0 °C
5. -4.2 °C
Tro IC3
Fly UP