Questions on Solubility and Henry's Law of Solubility
Multiple-Choice Questions – Solubility and Henry’s Law
1. What does solubility describe?
A) The speed at which a substance melts
B) The ability of a solute to conduct electricity
C) The amount of solute that dissolves in a given solvent at a certain temperature
D) The ability of a gas to escape from a liquid
E) The boiling point of a solution
2. Which factor most affects the solubility of a solid in a liquid?
A) Pressure
B) Gravity
C) Temperature
D) Density
E) pH
3. As temperature increases, the solubility of most solid solutes in liquid solvents:
A) Decreases
B) Remains unchanged
C) Increases
D) Becomes zero
E) Turns into gas
4. According to Henry's Law, the solubility of a gas in a liquid is directly proportional to:
A) The volume of the solvent
B) The pressure of the gas above the liquid
C) The mass of the solute
D) The surface area of the container
E) The solute's temperature
5. Which condition will increase the amount of CO₂ dissolved in a soft drink?
A) Heating the soda
B) Decreasing the pressure
C) Shaking the bottle
D) Cooling and sealing under pressure
E) Adding sugar
6. Which type of solute is most affected by pressure?
A) Ionic solids
B) Nonpolar liquids
C) Polar liquids
D) Gases
E) Covalent solids
7. According to Henry's Law, if the pressure of a gas above a liquid doubles, its solubility:
A) Halves
B) Doubles
C) Triples
D) Stays the same
E) Becomes zero
8. The "k" constant in Henry’s Law is dependent on:
A) The pressure of the gas
B) The identity of the gas and the solvent
C) The volume of the container
D) The number of moles of gas
E) The concentration of the solute
9. A gas has a Henry’s Law constant k=3.2×10−2 mol/L\cdotpatmk = 3.2 \times 10^{-2} \, \text{mol/L·atm}k=3.2×10−2mol/L\cdotpatm. If the pressure is 2 atm, what is its solubility?
A) 0.032 mol/L
B) 0.064 mol/L
C) 0.016 mol/L
D) 1.6 mol/L
E) 3.2 mol/L
10. What happens to the solubility of oxygen in water as pressure increases?
A) It increases
B) It decreases
C) It remains unchanged
D) It becomes zero
E) It depends on the solute
11. Why do soda cans "fizz" when opened?
A) The sugar reacts with water
B) The pressure inside is lower than outside
C) Gas solubility decreases as pressure drops
D) Carbonation increases
E) Oxygen rushes in
12. Which of the following decreases gas solubility in liquids?
A) Cooling the solution
B) Increasing gas pressure
C) Heating the solution
D) Decreasing volume
E) Adding salt
13. The units of Henry’s Law constant kkk are typically:
A) atm/mol
B) L/mol
C) mol/L·atm
D) g/mL
E) mol/g
14. When a solution cannot dissolve any more gas under current conditions, it is:
A) Dilute
B) Concentrated
C) Saturated
D) Unsaturated
E) Miscible
15. Which gas is least soluble in water under normal conditions?
A) CO₂
B) NH₃
C) O₂
D) HCl
E) CH₄
16. Henry's Law helps explain why:
A) Solids dissolve faster when crushed
B) Gases dissolve more under high pressure
C) Liquids evaporate faster than gases
D) Salts ionize in water
E) Water freezes at 0°C
17. Deep-sea divers must ascend slowly because:
A) Temperature increases with depth
B) They lose body heat rapidly
C) Henry's Law means dissolved gases will come out of solution if pressure drops quickly
D) Water density changes
E) Salts accumulate in tissues
18. Which is not an application of Henry’s Law?
A) Carbonated beverages
B) Breathing under pressure
C) Scuba diving safety
D) Crystallization of salts
E) Gas exchange in lungs
19. What factor would not significantly change the solubility of a solid in water?
A) Temperature
B) Stirring
C) Surface area
D) Pressure
E) Nature of solvent
20. In Henry’s Law, the equation C=kPC = kPC=kP represents:
A) Concentration equals rate times time
B) Pressure equals constant divided by volume
C) Solubility equals constant times gas pressure
D) Moles equals concentration divided by pressure
E) Temperature equals pressure times solubility
- Questions About Solutions
- Questions on Solute-Solvent Combinations
- Questions on Saturated and Unsaturated Solutions
Answer Key with Explanations
1. C – Solubility is the maximum amount of solute that dissolves in a solvent at a specific temperature.
2. C – Temperature is a major factor in the solubility of solids in liquids.
3. C – Solubility of most solids increases with higher temperature.
4. B – Henry’s Law states solubility of a gas is proportional to its pressure.
5. D – Cooling and high pressure increase CO₂ solubility in soda.
6. D – Gases are highly pressure-sensitive due to their compressibility.
7. B – If pressure doubles, gas solubility doubles (linear relationship).
8. B – The constant k depends on the gas and solvent pair.
9. B – C=kP=0.032×2=0.064 mol/LC = kP = 0.032 \times 2 = 0.064 \, \text{mol/L}C=kP=0.032×2=0.064mol/L
10. A – Increasing pressure increases oxygen’s solubility in water.
11. C – When the can is opened, pressure drops, and gas escapes.
12. C – Heating a solution causes gas to escape, lowering solubility.
13. C – Henry’s Law constant typically has units of mol/L·atm.
14. C – A solution that can’t hold more gas is saturated.
15. E – Methane (CH₄) is the least soluble in water (nonpolar).
16. B – Henry’s Law explains why gases dissolve better under pressure.
17. C – Fast pressure drop causes dissolved gases to form bubbles in blood (the bends).
18. D – Salt crystallization is unrelated to Henry’s Law (not gas-related).
19. D – Pressure has little effect on solid solubility.
20. C – Henry’s Law: C=kPC = kPC=kP, where C = solubility, P = pressure, k = constant.
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