Unit 6 Interactive Review

In a solution of sugar and water, the solvent is the:
1. sugar
2. water
In a solution of sugar and water, the solute is the:
1. sugar
2. water
A substance whose water solution does not conduct an electric current is a(n):
Which of the following substances, when dissolved in a water solution, will allow current to flow in the device pictured above, resulting in the lightbulb becoming lit?
1. Ethanol (ethyl alcohol)
2. sodium chloride
3. Sucrose (table sugar)
4. HCl - hydrochloric acid
5. sodium hydroxide
Gases dissolve best in liquids when:
1. the pressure is high and the temperature is high
2. the pressure is low and the temperature is high
3. the pressure is high and the temperature is low
4. the pressure is low and the temperature is low
The solubility of potassium nitrate in water at 35 °C is about 60 grams KNO₃ per 100 grams of water. How many grams of KNO₃ should dissolve in 300 grams of water at 35 °C?
1. 180 grams
2. 20 grams
3. 335 grams
Breaking up a solid speeds dissolving in a liquid by:
1. raising the temperature
2. decreasing the pressure
3. increasing surface area
4. slowing hydration
Most salts become more soluble in water as the:
1. pressure is increased
2. pressure is decreased
3. temperature is increased
4. temperature is decreased
Fats do not dissolve in water because:
1. Fats and water are both nonpolar
2. Fats are polar and water is nonpolar
3. Fats and water are both polar
4. Fats are nonpolar and water is polar
Calculate the concentration of the following solution in units of grams per liter:

12 grams of NaCl is dissolved in 3.00 L of solution
1. 36 g/L
2. 0.250 g/L
3. 4 g/L
4. 15 g/L
Calculate the concentration of the following solution in units of molarity, M, moles per liter:

80 grams of NaOH is dissolved in 2 L of solution
1. 1 M NaOH
2. 40 M NaOH
3. 160 M NaOH
4. 82 M NaOH
Calculate the concentration of the following solution in units of parts per million, ppm:

12 grams of NaCl is dissolved in 3.00 L of solution
1. 4000 ppm NaCl
2. .004 ppm NaCl
3. 4 ppm NaCl
4. 4 x 10⁶ ppm NaCl
Calculate the concentration of the following solution in units of percent composition:

12 grams of NaCl is dissolved in 3.00 L of solution
1. 40% NaCl
2. 0.0068% NaCl
3. 0.4% NaCl
4. 25% NaCl
What two substances are always produced by a neutralization reaction?
1. an acid and a base
2. water and a base
3. water and a salt
4. water and an acid
According to the Brønsted-Lowry definition, a base is:
1. a proton (hydrogen ion) donor
2. a proton (hydrogen ion) acceptor
3. a proton (hydrogen ion)
4. a proton (hydrogen ion) destroyer
Acids taste:
1. Sweet
2. Salty
3. Bitter
4. Sour
Bases taste:
1. Sweet
2. Salty
3. Bitter
4. Sour
A positive test for an acid occurs when:
1. red litmus turns blue
2. red litmus remains red
3. blue litmus turns red
4. blue litmus remains red
A positive test for a base occurs when:
1. red litmus turns blue
2. red litmus remains red
3. blue litmus turns red
4. blue litmus remains red
Bases cause phenolphthalein to turn:
1. orange
2. green
3. violet
4. clear
Strong acids:
1. Ionize slightly and produce few hydrogen ions in solution
2. Ionize completely and produce many hydroxide ions in solution
3. Ionize completely and produce many hydrogen ions in solution
4. Ionize slightly and produce few hydroxide ions in solution
Indicator Results
Phenolphthalein Clear
Red litmus Remains red
Blue litmus Turns red
Methyl orange Turns deep red

An unknown substance produced the experimental results noted above. Based on this data, the unknown is:
1. a base
2. a sugar
3. an acid
4. impossible to identify
The strongest bases are hydroxides of:
1. halogens
2. noble gases
3. transition metals
4. group 1 and group 2 metals
Which of the following is a property of acids?
1. Feel slippery
2. Turn red litmus blue
3. taste bitter
4. react with metals to form hydrogen gas
Acids have a pH that is:
1. greater than 7
2. equal to 7
3. less than 7
Bases have a pH that is:
1. greater than 7
2. equal to 7
3. less than 7
Which of the following pH values indicates the strongest acid?
1. 1
2. 4
3. 7
4. 11
When 100 mL of 1 M HCl is added to 100 mL of 2 M NaOH, the resulting solution would be:
1. acidic
2. basic
3. neutral
When 200 mL of 1 M HCl is added to 100 mL of 1 M NaOH, the resulting solution would be:
1. acidic
2. basic
3. neutral
When 100 mL of 1 M HCl is added to 100 mL of 1 M NaOH, the resulting solution would be:
1. acidic
2. basic
3. neutral
Carbon dioxide is produced when
1. acids neutralize bases
2. acids react with active metals
3. acids react with carbonate salts
4. bases dissolve in water
Which statement is true?
1. Acids are electrolytes. Bases are nonelectrolytes.
2. Acids are nonelectrolytes. Bases are electrolytes.
3. Acids and bases are electrolytes.
4. Acids and bases are nonelectrolytes.
At room conditions, the density of liquid water is about
1. 1 g/mL
2. 18 g/ml
3. 22.4 g/mL
4. 0 g/mL
The boiling point of pure water at standard pressure is
1. 0°C
2. 32°C
3. 100°C
4. 212°C
The freezing point of pure water at standard pressure is
1. 0°C
2. 32°C
3. 100°C
4. 212°C
Which of these phase changes occurs by the removal of energy?
1. boiling
2. condensation
3. freezing
4. melting
Which of these phase changes occurs by the absorption of energy?
1. boiling
2. condensation
3. freezing
4. melting
Separate 100 gram masses of iron and liquid water are each allowed to absorb 600 joules of energy. As a result,
1. the temperature of the water changes more than the temperature of the iron
2. the temperature of the iron changes more than the temperature of the water
3. the temperatures of both change by the same amount
4. neither the water nor the iron experience a temperature change
The temperature would be expected to remain constant during which of the following phase changes?
1. boiling
2. condensation
3. freezing
4. melting
Use this information to answer the question below:
ΔH_fus (H₂O) = 334 J/g
ΔH_vap (H₂O) = 2260 J/g

How much energy is required to boil 50 grams of water at its boiling point?
1. 100 J
2. 113 000 J
3. 45.2 J
4. 50 J
Use this information to answer the question below:
ΔH_fus (H₂O) = 334 J/g
ΔH_vap (H₂O) = 2260 J/g

How much energy is required to melt 50 grams of ice at its melting point?
1. 16 700 J
2. 113 000 J
3. 6.68 J
4. 50 J
Which of these has the greatest density, assuming standard pressure?
1. Liquid water at 4°C
2. Liquid water at 95°C
3. Ice at -10°C
4. Steam at 120°C
Refer to the image below when answering this question. Assume standard pressure.

As energy is added and one moves from point #5 to point #6, the change taking place is
1. an increase in the temperature of liquid water
2. an increase in the density of water
3. liquid water is becoming steam
4. ice is melting
Refer to the image below when answering this question. Assume standard pressure.

As energy is added and one moves from point #5 to point #6, the temperature
1. remains constant
2. increases
3. decreases
Refer to the image below when answering this question. Assume standard pressure.

The temperature at point #6 is
1. 100°C
2. 32°C
3. 0°C
4. 100°F
Refer to the image below when answering this question. Assume standard pressure.

At point #2, water would be found as
1. a liquid only
2. a solid only
3. a solid and a liquid
4. a liquid and a vapor
5. a vapor only
Refer to the image below when answering this question. Assume standard pressure.

As energy is being removed (going right to left), the phase change occuring at point #2 would be
1. freezing
2. boiling
3. condensation
4. melting
Refer to the image below when answering this question. Assume standard pressure.

The temperature at point #1 is
1. below 0°C
2. 0°C
3. Between 0°C and 100°C
4. above 100°C
Refer to the image below when answering this question. Assume standard pressure.

The density of water is highest at point
1. 1
2. 2
3. 3
4. 4
5. 5
6. 6
7. 7
Refer to the image below when answering this question. Assume standard pressure.

The measure of the energy required to move from point #3 to point #4 on the graph is determined by the
1. specific heat of liquid water
2. specific heat of steam
3. specific heat of ice
4. heat of fusion of water
5. heat of vaporization of water
Refer to the image below when answering this question. Assume standard pressure.

Which forms of water would be present at point #7?
1. liquid only
2. steam only
3. ice only
4. liquid and steam
5. solid and liquid
Refer to the image below when answering this question. Assume standard pressure.

The difference in temperature between point #2 and point #6 is
1. 100°C
2. 273°C
3. 32°F
4. 212°F
Refer to the image below when answering this question. Assume standard pressure.

Features of this graph support which observations about water?
1. The specific heat of liquid water is greater than that of steam or ice.
2. The heat of vaporization of water is greater than the heat of fusion.
3. Temperature remains constant during a phase change.
4. Water freezes at 0°C and boils at 100°C.
5. Water is denser as a liquid than it is as a solid.
Which of these is NOT a characteristic of most pure substances, but is true of water?
1. Expands when it freezes
2. Heat of vaporization is greater than the heat of fusion
3. Boiling point is greater than the melting point
4. Temperature remains constant during a phase change

Indicator	Results
Phenolphthalein	Clear
Red litmus	Remains red
Blue litmus	Turns red
Methyl orange	Turns deep red