General Chemistry II - Chapter 2: Solutions
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Questions and Answers

What is the molar mass of naphthalene (C10H8) calculated from its constituent elements?

  • 180 g/mole
  • 138 g/mole
  • 128 g/mole (correct)
  • 120 g/mole

    • How many moles of C10H8 are in 16.5 g of the substance?

  • 0.150 moles
  • 0.132 moles (correct)
  • 0.128 moles
  • 0.1 moles

    • What is the molality of a solution comprised of 0.132 moles of solute dissolved in 0.0543 kg of solvent?

  • 2.49 moles/Kg (correct)
  • 1.50 moles/Kg
  • 3.20 moles/Kg
  • 4.35 moles/Kg

    • What does molarity measure in a solution?

    <p>Moles of solute per liter of solution</p> Signup and view all the answers

    What is the formula to calculate parts per million (ppm) in a solution?

    <p>ppm = (Mass of Solute / Mass of Solution) * 10<sup>6</sup></p> Signup and view all the answers

    What is the term used for the substance that is dissolved in a solution?

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

    Which of the following is NOT a type of solution based on state of matter?

    <p>Gas in Solid</p> Signup and view all the answers

    What is the classification of a solution with more solute than can be dissolved at a given temperature?

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

    In a solution of salt dissolved in water, what is the role of the water?

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

    How many grams of solute would need to be present in a saturated solution of salt if 100 mL of water can only dissolve 36 grams of salt at room temperature?

    <p>36 grams</p> Signup and view all the answers

    Which of the following solutions is a liquid-liquid solution?

    <p>Ethanol in water</p> Signup and view all the answers

    What classification describes a solution that contains the maximum amount of solute that can be dissolved at that temperature?

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

    What is measured in parts per million (ppm) and used to express the concentration of solutions?

    <p>Mass of solute relative to mass of solution</p> Signup and view all the answers

    What characterizes a saturated solution?

    <p>It contains the maximum amount of solute that the solvent can dissolve.</p> Signup and view all the answers

    Which statement best describes a supersaturated solution?

    <p>It contains more dissolved solute than a saturated solution.</p> Signup and view all the answers

    What is the first step in the formation of a liquid solution?

    <p>Overcoming intermolecular forces in the solvent.</p> Signup and view all the answers

    What does a positive enthalpy of solution indicate?

    <p>The process is endothermic.</p> Signup and view all the answers

    Why is it important to express solutions in correct concentration units?

    <p>To measure the amount of solute in a consistent manner.</p> Signup and view all the answers

    Which method can lead to the formation of crystals in a supersaturated solution?

    <p>Scratching the sides of the container.</p> Signup and view all the answers

    How does the stability of a supersaturated solution compare to a saturated solution?

    <p>Supersaturated solutions are more unstable.</p> Signup and view all the answers

    What can be a consequence of administering a higher concentration medicine at an incorrect dose?

    <p>It might be harmful to the patient.</p> Signup and view all the answers

    When forming a solution, what happens during the second step?

    <p>The solute is separated into its individual components.</p> Signup and view all the answers

    What is an example of a factor affecting the concentration of a solution?

    <p>The volume of solvent and amount of solute.</p> Signup and view all the answers

    What is the correct formula to calculate percent by volume?

    <p>(Volume of solute / Volume of solution) * 100</p> Signup and view all the answers

    If a solution has 30 grams of solute in 150 mL of solution, what is the percent by mass-volume concentration?

    <p>20%</p> Signup and view all the answers

    How many grams of solute are in a 50 mL solution with a concentration of 12% by mass-volume?

    <p>6 g</p> Signup and view all the answers

    What is the mole fraction of solute if there are 2 moles of solute and 8 moles of solvent?

    <p>0.2</p> Signup and view all the answers

    What is the mass percent concentration of a solution with 36.5 g of NaCl and a total mass of 355 g?

    <p>10.28%</p> Signup and view all the answers

    What is the total number of moles of solution when 25 g of NaF is dissolved in 200 g of H2O?

    <p>11.71 moles</p> Signup and view all the answers

    If a wine contains 12% alcohol by volume, how much alcohol is in 350 mL of wine?

    <p>42 mL</p> Signup and view all the answers

    Which formula is used to calculate the mole fraction of the solute in a solution?

    <p>$X_{solute} = (Moles of solute / Total moles of solution)$</p> Signup and view all the answers

    If the total moles of solution are 10 and the moles of solvent are 7, what is the mole fraction of the solvent?

    <p>0.7</p> Signup and view all the answers

    What is the molar mass of NaF?

    <p>42 g/mole</p> Signup and view all the answers

    What is the percent by mass of a solution if 50 g of solute is present in 500 g of solution?

    <p>10%</p> Signup and view all the answers

    How many moles of H2O are present in 200 g of water?

    <p>11.11 moles</p> Signup and view all the answers

    Which statement about mole fractions is true?

    <p>The sum of all mole fractions cannot exceed 1.</p> Signup and view all the answers

    What is the mole fraction of the solvent in this solution?

    <p>0.95</p> Signup and view all the answers

    A solution contains 500 mL of liquid with 100 g of solute. What is the percent by volume of a 50 mL addition of solute?

    <p>20%</p> Signup and view all the answers

    If the mass of solute is increased while keeping the solvent mass constant, what effect will this have on the mole fraction of the solute?

    <p>Increase the mole fraction of the solute</p> Signup and view all the answers

    What is the relationship between the mole fraction of solute and solvent?

    <p>$X_{solute} + X_{solvent} = 1$</p> Signup and view all the answers

    What does molality measure?

    <p>Moles of solute per kilogram of solvent</p> Signup and view all the answers

    When calculating the mole fraction, what must be true about the total moles?

    <p>They must include both solute and solvent moles</p> Signup and view all the answers

    Study Notes

    General Chemistry II - Chapter 2: Solutions and Their Properties

    • Week 3-4 material covering solutions and their properties
    • Learning Competencies:
      • Using various methods to express solution concentrations (percent by mass, mole fraction, molarity, molality, percent by volume, ppm).
      • Performing stoichiometric calculations for reactions in solutions.
      • Describing the effect of concentration on colligative properties of solutions.
      • Differentiating colligative properties of nonelectrolyte and electrolyte solutions.
      • Calculating boiling point elevation and freezing point depression based on solute concentration.
      • Calculating molar mass from colligative property data.
      • Describing laboratory procedures for determining solution concentration.
      • Identifying solute and solvent in given examples. (e.g., 25 grams of salt dissolved in 95 mL of water)
      • Classifying types of solutions (e.g., gas in liquid, liquid in liquid, solid in liquid).
      • Understanding solution classifications (unsaturated, saturated, supersaturated) based on solute quantities.
      • Explaining factors affecting solution formation (Polarity, intermolecular forces).
      • Understanding Energy of Solution Formation (step-by-step process: overcoming intermolecular forces in solvent, separating solute, solute-solvent interaction).
      • Defining enthalpy of solution (the enthalpy change associated with the solution formation; this is the sum of the three steps in the solution formation).
      • Describing processes of energy change in solution formation (exothermic and endothermic).
      • Applying different concentration units (Percent by Mass, Percent by Volume, Percent by Mass-Volume, Mole Fraction, Molality, Molarity, Parts per Million(ppm)).
      • Performing calculations for concentration units:
        • Percent by mass
        • Percent by volume
        • Percent by mass-volume
        • Mole fraction
        • Molality
        • Molarity
        • Parts per million (ppm)
      • Understanding the necessity of correct concentration units in different applications (e.g., medications).
      • Calculating example problems for different concentration units (e.g., mass percent, volume percent , mass-volume percent).
      • Sample problems for different concentration units are presented.
      • Calculating mole fraction of solutes and solvents. -Calculating molality of solutions

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    Lesson 2 - Solutions and Types of Concentration PDF

    Description

    This quiz covers key concepts from Chapter 2 of General Chemistry II, focusing on solutions and their properties. You will explore various methods of expressing solution concentrations, perform stoichiometric calculations, and analyze colligative properties. Prepare to test your understanding of solution classifications and laboratory techniques related to concentrations.

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