Chemistry Solutions Review Flashcards
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Questions and Answers

What is a solution?

  • Homogeneous mixture (correct)
  • Suspension
  • Heterogeneous mixture
  • Emulsion
  • What is a solute?

    is the smaller amount

    What is a solvent?

    is the larger amount

    What is solubility?

    <p>the maximum amount of solid solute that can dissolve in a given amount of solvent</p> Signup and view all the answers

    What are some factors of solubility?

    <p>All of the above</p> Signup and view all the answers

    What does miscible mean?

    <p>liquids that dissolve in one another</p> Signup and view all the answers

    What does immiscible mean?

    <p>liquids that are insoluble in one another</p> Signup and view all the answers

    What is solvation?

    <p>surrounding of a solute particle by solvent molecules</p> Signup and view all the answers

    What is hydration?

    <p>is solvation involving water</p> Signup and view all the answers

    What does Henry's Law state?

    <p>solubility of a gas in a liquid is directly proportional to pressure above the liquid</p> Signup and view all the answers

    What does concentrated mean in solutions?

    <p>contains a relatively large amount of solute</p> Signup and view all the answers

    What does dilute mean in solutions?

    <p>contains a relatively small amount of solute</p> Signup and view all the answers

    What does unsaturated mean?

    <p>contains less than the maximum</p> Signup and view all the answers

    What does saturated mean?

    <p>contains the maximum amount of solute at a specific temperature</p> Signup and view all the answers

    What does supersaturated mean?

    <p>contains more than the maximum</p> Signup and view all the answers

    What does it mean if molarity is small?

    <p>the solution is dilute</p> Signup and view all the answers

    What does it mean if molarity is large?

    <p>the solution is concentrated</p> Signup and view all the answers

    What is mass percent in a solution?

    <p>component of a solution is the mass of that component divided by the mass of the solution multiplied by 100</p> Signup and view all the answers

    The freezing point of a solution is _______ than that of the pure solvent.

    <p>lower</p> Signup and view all the answers

    Increasing the temperature of an aqueous solution with an ionic solute will probably cause solubility to ________.

    <p>increase</p> Signup and view all the answers

    Study Notes

    Solution Concepts

    • Solution: A homogeneous mixture of two or more substances.
    • Solute: The smaller component in a solution, typically the substance that is dissolved.
    • Solvent: The larger component in a solution that dissolves the solute.

    Solubility and Its Factors

    • Solubility: Maximum quantity of solid solute that can dissolve in a specific amount of solvent.
    • Factors Influencing Solubility:
      • Polarity: Affects the interaction between solute and solvent.
      • Temperature: Changes in temperature can alter solubility.
      • Pressure: Primarily impacts gas solubility.

    Liquid Compatibility

    • Miscible: Liquids that can dissolve in each other without separating.
    • Immiscible: Liquids that do not mix or dissolve in one another due to opposite polarities.

    Solvation Processes

    • Solvation: The process of solvent molecules surrounding solute particles.
    • Hydration: A specific type of solvation where water is the solvent.

    Key Laws and Concepts

    • Henry's Law: States that gas solubility in a liquid is directly proportional to the pressure exerted above the liquid.

    Concentration and Characteristics

    • Concentrated Solution: Contains a relatively large proportion of solute.
    • Dilute Solution: Contains a relatively small proportion of solute.
    • Unsaturated Solution: Has less solute than the maximum solubility.
    • Saturated Solution: Contains the maximum solute that can dissolve at a given temperature.
    • Supersaturated Solution: Holds more solute than the maximum at a given temperature, typically unstable.

    Molarity and Its Implications

    • Small Molarity: Indicates a dilute solution.
    • Large Molarity: Indicates a concentrated solution.

    Mass Percent and Freezing Point

    • Mass Percent: Calculated as the mass of a component divided by the total mass of the solution, multiplied by 100.
    • Freezing Point Depression: The freezing point of a solution is lower than that of the pure solvent.

    Temperature Effects

    • Temperature and Solubility: Raising the temperature of an aqueous solution with an ionic solute usually increases its solubility.

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    Description

    Test your knowledge on solutions with these flashcards that cover essential terms and definitions. Each card provides a key concept related to solutions, such as solute, solvent, and solubility factors. Perfect for chemistry students looking to reinforce their understanding of homogeneous mixtures.

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