Title: Chapter 11: Solutions and Colloids
Course: Test

Q: Based off the molecular polarity of water, which of the following molecules would be soluble in water?
- glucose, methanol, and ethanol
- carbon dioxide, methane, methanol
- glucose, carbon dioxide, ethanol
A: glucose, methanol, and ethanol

Q: Which of the following would be a strong electrolyte in solution?
- PbI_2
- KCl
- Al(OH)_3
A: KCl

Q: Which of the following would be a weak electrolyte in solution?
- acetic acid
- sulfuric acid
- hydroiodic acid
A: acetic acid

Q: Which of the following when dissolved in deionized water would make a poor conducting solution?
- baking soda
- sugar
- salt
A: sugar

Q: Which of the following when dissolved in deionized water would make a good conducting solution?
- methanol
- sugar
- baking soda
A: baking soda

Q: For an experiment, you are asked to prepare a 2 m strong electrolytic solution. Which of the following salts would you use?
- an alkali salt
- an alkaline salt
- either an alkali or an alkaline salt
A: an alkali salt

Q: Which of the following substances would be a poor choice for making conductive solutions?
- C_6H_12O_6, CH_3OH, CH_3CH_2OH
- HCl, KBr, HNO_3
- NaOH, KOH, LiOH
A: C_6H_12O_6, CH_3OH, CH_3CH_2OH

Q: Which of the following would be soluble in water?
- sugar, NaCl, HCl
- sugar, NaOH, ethane
- sugar, HNO_3, methane
A: sugar, NaCl, HCl

Q: How would you purify salt water so that it becomes potable?
- gravity filtration
- vacuum filtration
- distillation
A: distillation

Q: Which of the following would conduct electricity?
- solid NaCl
- NaCl solution
- both solid NaCl and a NaCl solution
A: NaCl solution

Q: At what temperature does salt water freeze?
- 0 °C
- below 0 °C
- above 0 °C
A: below 0 °C

Q: If you want to boil a pot of water containing salt, at what temperature would boiling begin?
- 100 °C
- below 100 °C
- above 100 °C
A: above 100 °C

Q: What happens to the freezing point of water when ethylene glycol is added?
- Ethylene glycol has no effect on the freezing point of water.
- Ethylene glycol will interfere with the organization of water molecules during the freezing process therefore increasing the freezing point of water.
- Ethylene glycol will interfere with the organization of water molecules during the freezing process therefore reducing the freezing point of water.
A: Ethylene glycol will interfere with the organization of water molecules during the freezing process therefore reducing the freezing point of water.

Q: Which of the following is a colligative property?
- boiling-point elevation
- temperature of a solution
- color of a solution
A: boiling-point elevation

Q: Which of the following is a not a colligative property?
- boiling-point elevation
- temperature of a solution
- Freezing-point depression
A: temperature of a solution

Q: Assuming all the salts below are the same concentration, which salt would lower the freezing point of water the most?
- NaCl
- KBr
- CaCl_2
A: CaCl_2

Q: Which salt would lower the freezing point of a solvent the most?
- 1.5m NaCl
- 0.5m CaCl_2
- 1.25m Na_2SO_4
A: 1.25m Na_2SO_4

Q: What would be the best method for raising the boiling point of water in a kettle by a few degrees Celsius?
- increase the temperature of the stove
- add some table salt to the water
- increase the temperature of the stove and increase the surface area by transferring the water to a larger kettle
A: add some table salt to the water

Q: What would be the best method for lowering the freezing point of water in an ice tray that is in the freezer?
- decrease the temperature of the freezer
- decrease the temperature of the freezer and increase the surface area by transferring the water to a larger ice tray
- add some table salt to the water
A: add some table salt to the water

Q: Patients who enter the emergency room dehydrated are usually given sterile saline solution intravenously. The solution administered is isotonic to prevent cell damage. What would happen if the solution was hypotonic?
- Hypotonic solutions have a higher osmotic pressure than that within cells so hemolysis can occur.
- Hypotonic solutions have a lower osmotic pressure than that within cells so hemolysis can occur.
- Hypotonic solutions have the same osmotic pressure as that within cells so hemolysis can occur.
A: Hypotonic solutions have a lower osmotic pressure than that within cells so hemolysis can occur.

Q: Patients who enter the emergency room dehydrated are usually given sterile saline solution intravenously. The solution administered is isotonic to prevent cell damage. What would happen if the solution was hypertonic?
- Hypertonic solutions have the same osmotic pressure as that within cells so crenation can occur.
- Hypertonic solutions have a lower osmotic pressure than that within cells so crenation can occur.
- Hypertonic solutions have a higher osmotic pressure than that within cells so crenation can occur.
A: Hypertonic solutions have a higher osmotic pressure than that within cells so crenation can occur.

Q: Which type of solution has a lower osmotic pressure than that within cells?
- hypertonic
- hypotonic
- isotonic
A: hypotonic

Q: Which type of solution has a higher osmotic pressure than that within cells?
- isotonic
- hypertonic
- hypotonic
A: hypertonic

Q: Which type of solution has the same osmotic pressure as that within cells?
- hypertonic
- isotonic
- hypotonic
A: isotonic

Q: What is the osmolarity of a 2 M NaCl solution?
- 2 osmol
- 6 osmol
- 4 osmol
A: 4 osmol

Q: A KCl solution is 0.500 M. What is the osmolarity?
- 1 osmol
- 2 osmol
- 4 osmol
A: 1 osmol

Q: 45.8 g of NaCl is dissolved in 500. mL of a water (d = 1.00 g/mL) and is placed in the freezer at -1 °C overnight. Which statement best describes what would happen to the solution?
- The freezing point of the NaCl solution would be -5.83 °C, so the solution would not freeze.
- The freezing point of the NaCl solution would be 5.83 °C, so the solution would freeze.
- The freezing point of the NaCl solution would be -2.92 °C, so the solution would not freeze.
A: The freezing point of the NaCl solution would be -5.83 °C, so the solution would not freeze.

Q: 17.1 g of calcium chloride is dissolved in 750. mL of a water (d = 1.00 g/mL) and is placed in the freezer at -2 °C overnight. Which statement best describes what would happen to the solution?
- The freezing point of the calcium chloride solution would be 1.15 °C, so the solution would freeze.
- The freezing point of the calcium chloride solution would be -1.15 °C, so the solution would freeze.
- The freezing point of the calcium chloride solution would be -0.382 °C, so the solution would freeze.
A: The freezing point of the calcium chloride solution would be -1.15 °C, so the solution would freeze.

Q: How would you be able to increase the boiling point of water on a hotplate?
- increase the temperature of the hotplate
- add less water and increase the temperature of the hotplate
- add some NaCl to the water
A: add some NaCl to the water

Q: How would you increase the concentration of a 1 M NaCl solution?
- decant some of the solution down the sink
- bring the solution to near boiling until desired volume is achieved
- decrease the temperature of the salt solution to near freezing
A: bring the solution to near boiling until desired volume is achieved

Q: The solubility of NaCH_3CO_2 in water is ~1.23 g/mL. What would be the best method for preparing a supersaturated NaCH_3CO_2 solution?
- add 130 g of NaCH_3CO_2 to 100 mL of H_2O at 80 °C while stirring until all the solid dissolves, then let the solution cool to room temperature
- add 123 g of NaCH_3CO_2 to 200 mL of H_2O at 80 °C while stirring until all the solid dissolves, then let the solution cool to room temperature
- add 130 g of NaCH_3CO_2 to 100 mL of H_2O at room temperature while stirring until all the solid dissolves
A: add 130 g of NaCH_3CO_2 to 100 mL of H_2O at 80 °C while stirring until all the solid dissolves, then let the solution cool to room temperature

Q: The solubility of KCl in water is ~344 g/L. What would be the best method for preparing a 100 mL saturated KCl solution?
- add 38.0 g of KCl to 100 mL of H_2O at room temperature while stirring
- add 30.0 g of KCl to 100 mL of H_2O at room temperature while stirring
- add 34.0 g of KCl to 100 mL of H_2O at room temperature while stirring
A: add 38.0 g of KCl to 100 mL of H_2O at room temperature while stirring