Chapter 11: Solutions and Colloids Flashcards
Which of the following is true about homogeneous mixtures?
a) The solute and solvent are visible separately.
b) Homogeneous mixtures are always made of metals.
c) You cannot distinguish between the solute and solvent.
d) They are always liquid.
c) You cannot distinguish between the solute and solvent.
In a solution of salt water:
a) Water is the solute, and salt is the solvent.
b) Salt is the solute, and water is the solvent.
c) Both salt and water are solutes.
d) Both salt and water are solvents.
b) Salt is the solute, and water is the solvent.
Which factor does not favor dissolution?
a) Increase in entropy.
b) Decrease in energy.
c) Presence of dissimilar intermolecular forces.
d) Solute-solvent attraction stronger than solute-solute attraction.
c) Presence of dissimilar intermolecular forces.
“Like dissolves like” means:
a) Polar solvents dissolve polar solutes, and nonpolar solvents dissolve nonpolar solutes.
b) All solvents dissolve all solutes equally.
c) Polar solvents only dissolve ionic compounds.
d) Dissolution happens regardless of intermolecular forces.
a) Polar solvents dissolve polar solutes, and nonpolar solvents dissolve nonpolar solutes.
Which of the following is a non-electrolyte?
a) NaCl (salt).
b) HCl (hydrochloric acid).
c) C₆H₁₂O₆ (glucose).
d) KOH (potassium hydroxide).
c) C₆H₁₂O₆ (glucose).
Which of the following is a strong electrolyte?
a) CH₃COOH (acetic acid).
b) NaOH (sodium hydroxide).
c) NH₃ (ammonia).
d) CO₂ (carbon dioxide).
b) NaOH (sodium hydroxide).
Henry’s Law predicts:
a) How temperature affects solubility.
b) The relationship between pressure and the solubility of a gas.
c) How ionic compounds dissociate in solution.
d) The pH of a solution.
b) The relationship between pressure and the solubility of a gas.
If the partial pressure of a gas above a liquid doubles, what happens to its solubility (assuming constant temperature)?
a) It is halved.
b) It doubles.
c) It stays the same.
d) It becomes zero.
b) It doubles.
What does the designation (aq) mean in a chemical solution?
a) The solute is ionic.
b) The solvent is water.
c) The solution is nonpolar.
d) The solute and solvent are both liquids.
b) The solvent is water.
Which of the following is false about homogeneous mixtures?
a) The composition is uniform throughout.
b) You can see the difference between the solute and solvent.
c) They can exist in solid, liquid, or gaseous phases.
d) They include solutions where the solute and solvent are miscible.
b) You can see the difference between the solute and solvent.
Ionic dissolution differs from covalent dissolution because:
a) Ionic compounds dissociate into neutral molecules.
b) Ionic compounds dissociate into charged ions, while covalent compounds typically do not.
c) Covalent compounds dissociate into positive and negative ions.
d) Ionic compounds cannot dissolve in polar solvents.
b) Ionic compounds dissociate into charged ions, while covalent compounds typically do not.
Which of the following solvents is most likely to dissolve NaCl?
a) Hexane (C₆H₁₄)
b) Water (H₂O)
c) Methane (CH₄)
d) Benzene (C₆H₆)
b) Water (H₂O)
Which of the following is an example of a weak electrolyte?
a) H₂O (water)
b) NaCl (salt)
c) CH₃COOH (acetic acid)
d) KOH (potassium hydroxide)
c) CH₃COOH (acetic acid)
Which of these substances is a strong electrolyte in water?
a) Sugar (C₆H₁₂O₆)
b) HCl (hydrochloric acid)
c) NH₃ (ammonia)
d) Ethanol (C₂H₅OH)
b) HCl (hydrochloric acid)
Which factor does not affect whether a substance dissolves?
a) The similarity of intermolecular forces between solute and solvent.
b) The increase in system entropy during dissolution.
c) The temperature of the solvent.
d) The boiling point of the solvent.
d) The boiling point of the solvent.
Why does a polar solvent like water dissolve ionic compounds?
a) The positive and negative ions in the solute are stabilized by water’s polar molecules.
b) Ionic compounds are always soluble in water.
c) Water’s nonpolar regions interact with ionic compounds.
d) Ionic compounds chemically react with water to dissolve.
a) The positive and negative ions in the solute are stabilized by water’s polar molecules.
Henry’s Law states that the solubility of a gas in a liquid is directly proportional to:
a) The molecular mass of the gas.
b) The intermolecular forces in the solvent.
c) The partial pressure of the gas above the liquid.
d) The temperature of the system.
c) The partial pressure of the gas above the liquid.
If a gas becomes less soluble in a liquid as the temperature increases, what can you conclude?
a) Gas solubility is independent of temperature.
b) Increased temperature lowers the partial pressure of the gas.
c) The dissolution process is exothermic.
d) Gas solubility decreases because gas molecules gain kinetic energy and escape the liquid.
d) Gas solubility decreases because gas molecules gain kinetic energy and escape the liquid.
Miscibility refers to:
a) The ability of a liquid to dissolve a solid.
b) The ability of one liquid to dissolve in another liquid.
c) The ability of a gas to dissolve in a liquid.
d) The ability of a solid to dissolve in a gas.
b) The ability of one liquid to dissolve in another liquid.
Which of the following pairs of liquids is most likely miscible?
a) Oil and water
b) Ethanol and water
c) Hexane and water
d) Vinegar and oil
b) Ethanol and water
If two liquids are partially miscible, what does this mean?
a) They mix in all proportions.
b) They do not mix at all.
c) They mix to some extent but form two layers.
d) They react chemically to form a new compound.
c) They mix to some extent but form two layers.
As the temperature of a solid increases, its solubility generally:
a) Decreases.
b) Increases.
c) Remains the same.
d) Is not affected by temperature.
b) Increases.
How does the solubility of a gas in a liquid change as the temperature increases?
a) It increases.
b) It decreases.
c) It remains constant.
d) It depends on the polarity of the liquid.
b) It decreases.
Which of the following statements about solubility is true?
a) Increasing the pressure on a solid increases its solubility.
b) Increasing the pressure on a gas increases its solubility.
c) Solubility of gases in liquids is unaffected by temperature.
d) Solubility of solids in liquids decreases with increasing temperature.
b) Increasing the pressure on a gas increases its solubility.
Colligative properties depend on:
a) The identity of the dissolved particles.
b) The number of dissolved particles in the solvent.
c) The temperature of the solution.
d) The pressure of the system.
b) The number of dissolved particles in the solvent.
Which of the following is not a colligative property?
a) Boiling point elevation
b) Freezing point depression
c) Vapor pressure lowering
d) Heat of fusion
d) Heat of fusion
Adding a non-volatile solute to a solvent will:
a) Increase the solvent’s vapor pressure.
b) Lower the solvent’s vapor pressure.
c) Have no effect on the solvent’s vapor pressure.
d) Increase the boiling point and freezing point of the solvent.
b) Lower the solvent’s vapor pressure.
Adding a non-volatile solute to a solvent will:
a) Increase the solvent’s vapor pressure.
b) Lower the solvent’s vapor pressure.
c) Have no effect on the solvent’s vapor pressure.
d) Increase the boiling point and freezing point of the solvent.
b) Lower the solvent’s vapor pressure.
Boiling point elevation occurs because:
a) The solute increases the kinetic energy of the solvent.
b) The solute interferes with the solvent’s ability to vaporize.
c) The solute increases the solvent’s surface tension.
d) The solute lowers the solvent’s intermolecular forces.
b) The solute interferes with the solvent’s ability to vaporize.
What happens to a red blood cell placed in a hypotonic solution?
A) It shrinks (crenation)
B) It remains the same
C) It bursts (hemolysis)
D) It dissolves completely
C) It bursts (hemolysis)
Which equation represents osmotic pressure?
A) 𝜋=𝑀𝑅𝑇
B) PV=nRT
C) q=mcΔT
D) ΔG=ΔH−TΔS
A) 𝜋=𝑀𝑅𝑇
What is the correct definition of reverse osmosis?
A) Water moves from a region of low solute concentration to high solute concentration
B) Water moves from a region of high solute concentration to low solute concentration
C) Solute moves across a membrane instead of solvent
D) The pressure inside a cell becomes equal to the pressure outside the cell
B) Water moves from a region of high solute concentration to low solute concentration
Which colligative property explains why salt is used to melt ice on roads?
A) Boiling point elevation
B) Freezing point depression
C) Vapor pressure lowering
D) Osmotic pressure
B) Freezing point depression
What is the van’t Hoff factor (𝑖) for MgCl₂?
A) 1
B) 2
C) 3
D) 4
C) 3
😍Which statement is true about colligative properties?
A) They depend on the identity of the solute
B) They depend on the amount of solute particles in solution
C) Only non-electrolytes exhibit colligative properties
D) They do not affect freezing or boiling points
B) They depend on the amount of solute particles in solution
Which of the following is a colloid?
A) Saltwater
B) Fog
C) Muddy water
D) Iron nails in water
B) Fog
What is the main difference between a solution and a suspension?
A) Solutions have larger particles than suspensions
B) Suspensions are homogeneous, while solutions are heterogeneous
C) Suspensions have larger particles that settle, while solutions are completely dissolved
D) Solutions contain only gases, while suspensions contain only solid
C) Suspensions have larger particles that settle, while solutions are completely dissolved
Which of the following increases the solubility of a gas in a liquid?
A) Increasing temperature
B) Decreasing pressure
C) Increasing pressure
D) Decreasing the polarity of the solvent
C) Increasing pressure
Which of the following is an example of a homogeneous solution?
A) Sand and water
B) Oil and vinegar
C) Saltwater
D) Muddy water
C) Saltwater
What is required for a substance to dissolve in a solvent?
A) The solute must be heavier than the solvent
B) The solute and solvent must share the same intermolecular forces
C) The solute must be ionic
D) The solvent must be non-polar
B) The solute and solvent must share the same intermolecular forces
Which of the following is a strong electrolyte?
A) NaCl
B) C₆H₁₂O₆ (glucose)
C) CH₃OH (methanol)
D) NH₃ (ammonia)
A) NaCl
What happens when a weak electrolyte dissolves in water?
A) It does not dissociate at all
B) It fully dissociates into ions
C) It partially dissociates into ions
D) It forms a gas
B) It fully dissociates into ions
What happens to the boiling point of water when salt is added?
A) It decreases
B) It increases
C) It stays the same
D) It turns into a gas immediately
B) It increases
What happens to a red blood cell placed in a hypertonic solution?
A) It bursts (hemolysis)
B) It remains unchanged
C) It shrinks (crenation)
D) It dissolves completely
C) It shrinks (crenation)
Which of the following statements is true about gas solubility?
A) It increases with increasing temperature
B) It decreases with increasing temperature
C) It is unaffected by temperature
D) It is only dependent on the solvent
B) It decreases with increasing temperature
Which factor has no effect on the solubility of solids in liquids?
A) Temperature
B) Pressure
C) Intermolecular forces
D) Solvent type
B) Pressure
What is the main difference between a solution and a suspension?
A) Solutions have larger particles than suspensions
B) Suspensions have larger particles that settle, while solutions remain evenly mixed
C) Suspensions are homogeneous, while solutions are heterogeneous
D) Solutions only contain gases, while suspensions contain only solids
B) Suspensions have larger particles that settle, while solutions remain evenly mixed
Which of the following best defines a solvent?
A) The substance that gets dissolved
B) A substance that is always water
C) The substance that dissolves the solute
D) A substance that must be polar
C) The substance that dissolves the solute
What does “aqueous” (aq) mean in a solution?
A) The solution contains alcohol as the solvent
B) The solution is composed of only gases
C) Water is the solvent
D) The solute is ionic
C) Water is the solvent
What is osmosis?
A) Movement of solvent molecules from high to low concentration
B) Movement of solute molecules from high to low concentration
C) Movement of solvent molecules from low to high concentration
D) Movement of solute molecules from low to high concentration
C) Movement of solvent molecules from low to high concentration
What type of solution causes water to leave a red blood cell, making it shrink (crenation)?
A) Isotonic
B) Hypotonic
C) Hypertonic
D) Non-electrolyte
C) Hypertonic
Which mixture contains particles that do not settle but scatter light (Tyndall effect)?
A) Solution
B) Colloid
C) Suspension
D) Electrolyte
B) Colloid
Which of the following is a heterogeneous mixture with large particles that settle over time?
A) Solution
B) Colloid
C) Suspension
D) Electrolyte
C) Suspension
