Tro IC3

1. NaCl2. Na3. Cl24. H2O

5. None of the above

13.1 What is the solute when 10 g of NaCl is dissolved in 100 mL of water?

Tro IC3

1. NaCl2. Na3. Cl24. H2O

5. None of the above

13.1 What is the solute when 10 g of NaCl is dissolved in 100 mL of water?

Tro IC3

1. H2O

2. NH3

3. CH3OH

4. CH3OCH3

5. C8H18

13.2 Which solvent would be most suitable to remove grease from an object?

Tro IC3

1. H2O

2. NH3

3. CH3OH

4. CH3OCH3

5. C8H18

13.2 Which solvent would be most suitable to remove grease from an object?

Tro IC3

1. Salad dressing2. Blueberry muffin3. Wine4. Sugar5. Lead

13.3 Which of the following substances is an example of a solution?

Tro IC3

1. Salad dressing2. Blueberry muffin3. Wine4. Sugar5. Lead

13.3 Which of the following substances is an example of a solution?

Tro IC3

1. CH3CH2CH3

2. CH3OCH3

3. CH3CH2OH

4. CH3CH2NH2

5. CH3CH2COOH

13.4 In theory which of the following would have the highest solubility in gasoline (C8H18) ?

Tro IC3

1. CH3CH2CH3

2. CH3OCH3

3. CH3CH2OH

4. CH3CH2NH2

5. CH3CH2COOH

13.4 In theory which of the following would have the highest solubility in gasoline (C8H18) ?

Tro IC3

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 above5. None of the above

13.5 A supersaturated solution:

Tro IC3

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 above5. None of the above

13.5 A supersaturated solution:

Tro IC3

1. 0.0175 mol NaCl in 1 L of solution2. 0.1 g NaCl in 100 mL of solution3. 0.5 g NaCl in 500 mL of solution4. 0.25 mol NaCl in 200 mL of solution5. All have the same concentration.

13.6 Which of the following NaCl solutions has the highest concentration of NaCl?

Tro IC3

1. 0.0175 mol NaCl in 1 L of solution2. 0.1 g NaCl in 100 mL of solution3. 0.5 g NaCl in 500 mL of solution4. 0.25 mol NaCl in 200 mL of solution5. All have the same concentration.

13.6 Which of the following NaCl solutions has the highest concentration of NaCl?

Tro IC3

1. NaCl (aq)2. NH4NO3 (aq)

3. H2O (l)

4. MgCl2 (aq)

5. HF (aq)

13.7 Which of the following would be worst at conducting electricity?

Tro IC3

1. NaCl (aq)2. NH4NO3 (aq)

3. H2O (l)

4. MgCl2 (aq)

5. HF (aq)

13.7 Which of the following would be worst at conducting electricity?

Tro IC3

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

13.8 How is the solubility of a gas affected by the temperature of the solution?

Tro IC3

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

13.8 How is the solubility of a gas affected by the temperature of the solution?

Tro IC3

1. Solvent–solvent2. Solvent–solute3. Solute–solute4. Solvent–solution5. All of the above

13.9 Which type of interaction must be strong in order to dissolve a salt?

Tro IC3

1. Solvent–solvent2. Solvent–solute3. Solute–solute4. Solvent–solution5. All of the above

13.9 Which type of interaction must be strong in order to dissolve a salt?

Tro IC3

1. 37 g2. 3.7 g3. 0.37 g4. 0.0037 g5. 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?

Tro IC3

1. 37 g2. 3.7 g3. 0.37 g4. 0.0037 g5. 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?

Tro IC3

1. The solubility remains the same2. The solubility increases3. The solubility decreases4. It depends on the chemical nature of the gas5. 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?

Tro IC3

1. The solubility remains the same2. The solubility increases3. The solubility decreases4. It depends on the chemical nature of the gas5. 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?

Tro IC3

1. 12.5 g2. 14.5 g3. 18.1 g4. 111 g5. 862 g

13.12 How many grams of KNO3 are in a 125-g

solution containing 14.5% solute?

Tro IC3

1. 12.5 g2. 14.5 g3. 18.1 g4. 111 g5. 862 g

13.12 How many grams of KNO3 are in a 125-g

solution containing 14.5% solute?

Tro IC3

1. Moles of solute per liter of solution2. Moles of solute per kg of solution3. Grams of solute per liter of solution4. Moles of solute per kg of solvent5. Grams of solvent per kg of solution

13.13 The molarity of a solution is defined asthe number of:

Tro IC3

1. Moles of solute per liter of solution2. Moles of solute per kg of solution3. Grams of solute per liter of solution4. Moles of solute per kg of solvent5. Grams of solvent per kg of solution

13.13 The molarity of a solution is defined asthe number of:

Tro IC3

1. 10.0%2. 9.09%3. 71.4%4. 2.50%5. 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.

Tro IC3

1. 10.0%2. 9.09%3. 71.4%4. 2.50%5. 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.

Tro IC3

1. 0.049 M2. 204 M3. 2.45 M4. 0.500 M5. 4.90 M

13.15 What is the molarity of a KNO3 solution containing 2.45 mol KNO3 in 500 mL of solution?

Tro IC3

1. 0.049 M2. 204 M3. 2.45 M4. 0.500 M5. 4.90 M

13.15 What is the molarity of a KNO3 solution containing 2.45 mol KNO3 in 500 mL of solution?

Tro IC3

1. 53.3 M2. 1.33 M3. 0.00133 M4. 4.00 M5. 0.0533 M

13.16 What is the molarity of NaOH in a solution containing 40.0g of NaOH in 750 mL of solution?

Tro IC3

1. 53.3 M2. 1.33 M3. 0.00133 M4. 4.00 M5. 0.0533 M

13.16 What is the molarity of NaOH in a solution containing 40.0g of NaOH in 750 mL of solution?

Tro IC3

1. 0.234 mL2. 0.250 mL3. 1.39 mL4. 14.6 mL5. 234 mL

13.17 Calculate the volume of 0.250 M solution made by dissolving 5.56 g of solid magnesium chloride in water.

Tro IC3

1. 0.234 mL2. 0.250 mL3. 1.39 mL4. 14.6 mL5. 234 mL

13.17 Calculate the volume of 0.250 M solution made by dissolving 5.56 g of solid magnesium chloride in water.

Tro IC3

1. Add 40.3 mL of 12.4 M stock to 500 mL of water.2. Add 12.4 mL of 12.4 M stock to 500 mL of water.3. Add 40.3 mL of 12.4 M stock to 459.7 mL of water.4. Add 459.7 mL of water to 40.3 mL of 12.4 M stock.5. 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.

Tro IC3

1. Add 40.3 mL of 12.4 M stock to 500 mL of water.2. Add 12.4 mL of 12.4 M stock to 500 mL of water.3. Add 40.3 mL of 12.4 M stock to 459.7 mL of water.4. Add 459.7 mL of water to 40.3 mL of 12.4 M stock.5. 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.

Tro IC3

1. 50.0 mL2. 100. mL3. 150. mL4. 200. mL5. 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?

Tro IC3

1. 50.0 mL2. 100. mL3. 150. mL4. 200. mL5. 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?

Tro IC3

1. 0.877 g2. 1.25 g3. 1.51 g4. 1.80 g5. 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?

Tro IC3

1. 0.877 g2. 1.25 g3. 1.51 g4. 1.80 g5. 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?

Tro IC3

1. Osmotic pressure2. Freezing point depression3. Boiling point depression4. Boiling point elevation5. All are colligative properties.

13.21 Which of the following is NOT an example of a colligative property?

Tro IC3

1. Osmotic pressure2. Freezing point depression3. Boiling point depression4. Boiling point elevation5. All are colligative properties.

13.21 Which of the following is NOT an example of a colligative property?

Tro IC3

1. 0.455 m2. 455 m3. 0.910 m4. 910. m5. 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.

Tro IC3

1. 0.455 m2. 455 m3. 0.910 m4. 910. m5. 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.

Tro IC3

1. -1.4 °C2. 1.4 °C3. 4.2 °C4. 0.0 °C5. -4.2 °C

13.23 What is the freezing point of a 0.75 m aqueous solution of calcium chloride? (Note: Kf = 1.86 °C·kg/molparticles.)

Tro IC3

1. -1.4 °C2. 1.4 °C3. 4.2 °C4. 0.0 °C5. -4.2 °C

13.23 What is the freezing point of a 0.75 m aqueous solution of calcium chloride? (Note: Kf = 1.86 °C·kg/molparticles.)

Tro IC3

1. 6 °C2. 94 °C3. 97 °C4. 103 °C5. 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.)

Tro IC3

1. 6 °C2. 94 °C3. 97 °C4. 103 °C5. 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.)

Tro IC3

1. Shrinks2. Swells3. Leaks4. Bursts5. 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:

Tro IC3

1. Shrinks2. Swells3. Leaks4. Bursts5. 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:

Tro IC3

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 °C2. 1.4 °C3. 4.2 °C4. 0.0 °C5. -4.2 °C

13.26

Tro IC3

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 °C2. 1.4 °C3. 4.2 °C4. 0.0 °C5. -4.2 °C

13.26