Henry's Law and Solubility
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Questions and Answers

According to Henry's law, what is the relationship between the solubility of an ideal gas and its partial pressure?

  • The solubility of an ideal gas is inversely proportional to its partial pressure
  • The solubility of an ideal gas is directly proportional to its partial pressure (correct)
  • The solubility of an ideal gas is proportional to the square of its partial pressure
  • The solubility of an ideal gas is independent of its partial pressure

    • In the context of Henry's law, what does the proportionality constant 'k' depend on?

  • The identity of the gaseous solute only
  • The identity of the solvent only
  • The temperature of the solution only
  • The identities of both the gaseous solute and solvent, and the solution temperature (correct)

    • If the concentration of dissolved oxygen in water exposed to a partial pressure of 150 kPa is 0.002 mol L−1, what would be the new concentration if the partial pressure is reduced to 75 kPa, assuming ideal conditions according to Henry's law?

  • 0.002 mol L−1
  • 0.0005 mol L−1
  • 0.001 mol L−1 (correct)
  • 0.004 mol L−1

    • According to Henry's law, what happens to the solubility of a gas in a liquid as the partial pressure of the gas increases?

    <p>The solubility increases exponentially with the partial pressure (B)</p> Signup and view all the answers

    How does an increase in temperature affect the solubility of a gas in a liquid according to Henry's law?

    <p>The solubility decreases with increasing temperature (A)</p> Signup and view all the answers

    What is the relationship between the Henry’s law constant and the solubility of a gas in a liquid?

    <p>The lower the Henry’s law constant, the higher the solubility of the gas in the liquid (C)</p> Signup and view all the answers

    Why are supersaturated solutions of most solids in water prepared by cooling saturated solutions?

    <p>Cooling reduces the solubility of the solid in water, allowing excess solid to precipitate out and form a supersaturated solution. (B)</p> Signup and view all the answers

    Given the observation that ethanol is completely miscible with water and ethanethiol is soluble only to the extent of 1.5 g per 100 mL of water, what can be inferred about their molecular structures?

    <p>Ethanethiol exhibits stronger hydrogen bonding with water compared to ethanol. (B)</p> Signup and view all the answers

    What would be the most likely reason for CH4 to be the most soluble gas in water among the given options?

    <p>CH4 has a nonpolar covalent structure, which allows it to form weak London dispersion forces with water molecules. (D)</p> Signup and view all the answers

    How did the concentration of dissolved CO2 in the beverage change when the bottle was opened?

    <p>The concentration decreased due to CO2 escaping into the atmosphere. (A)</p> Signup and view all the answers

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