Chemistry

Chapter 13

Solutions

Objectives

Distinguish between heterogeneous and homogeneous mixtures.

List three different solute-solvent combinations.

Compare the properties of suspensions, colloids, and solutions.

Distinguish between electrolytes and nonectrolytes.

  1. Section 13.1 Types of Mixtures
    1. Solutions
      1. Soluble- a substance that is able to be dissolved.
        1. Miscible- substances that will dissolve
        2. Immiscible- substances that will not dissolve
      2. Solution- is a homogeneous mixture of two or more substances in a single phase.
        1. Components of Solutions
          1. Solvent- the dissolving medium in a solution
          2. Solute- the substance dissolved in a solution.

           

           

           

        2. Types of Solutions

      Table 13-1 Some Solute-Solvent Combinations for Solutions

      Solute State

      Solvent State

      Example
           
           
           
           
           
           
           

    2. Suspensions- when particles are so large that they settle out unless the mixture is constantly stirred.
    3. Colloids- substances that have particles that are intermediate in size between those in solutions and suspensions.
    4. Tyndall Effect-when particles are to small to be seen but large enough to scatter light.

      5.  

       

       

       

       

       

      Table 13-3 Properties of Solutions, Colloids, and Suspensions

      Solutions

      Colloids

      Suspensions
           
           
           
           
           
    5. Solutes: Electrolytes vs. Nonelectrolytes
        1. Electrolyte-a substance that dissolves in water to give a solution that conducts electric current. ( salt )
        2. Nonelectrolyte- a substance that dissolves in water to give a solution that does not conduct an electric current. (sugar)

     

     

     

     

     

     

     

     

     

     

    Objectives

    List and explain three factors that affect the rate at which a solid solute dissolves in a liquid solvent.

    Explain solution equilibrium, and distinguish among saturated, unsaturated, and supersaturated solution.

    Explain the meaning of "like dissolves like" in terms of polar and nonpolar substances.

    List the three interactions that contribute to the heat of solution, and explain what causes dissolution to be exothermic or endothermic.

    Compare the effects of temperature and pressure on solubility.

  2. Section 13-2 The Solution Process
    1. Factors Affecting the Rate of Dissolution
      1. increasing the surface area of the solute
      2. agitating a solution
      3. heating a solvent
    2. Solubility
      1. Solution equilibrium- is the physical state in which the opposing processes of dissolution and crystallization of a solute occur at equal rates.
        1. Saturated vs. Unsaturated solutions
          1. Saturated- contains the maximum amount of dissolved solute.
          2. Unsaturated solution- contains less than a saturated solution
        2. Supersaturated solution contains more dissolved solute than a saturated solution under the same conditions.
        3. Solubility- is a measure of the amount of solute in a given solvent.
          1. What dissolves?
            1. like dissolves like
            2. polar dissolves polar
            3. Water is the universal solvent because it acts like tiny magnets and pulls compounds apart.
          2. Effects of pressure of solubility
            1. as pressure decreases so does the solubility
            2. Henry’s law- pressure is directly proportional to the solubility.
          3. Effects of temperature on solubility. Temperature and solubility are inversely related.

     

     

    Objectives

    Given the mass of solute and volume of solvent, calculate the concentration of a solution.

    Given the concentration of a solution, determine the amount of solute in a given amount of solution.

    Given the concentration of a solution, determine the amount of solution that contains a given amount of solute.

  3. Section 13-3 Concentration of Solutions
    1. Concentration- of a solution is a measure of the amount of solute in a given amount of solvent or solution.
    2. Molarity- is the number of moles of solute in one liter of solution.
      1. Molarity (M) = amount of solute (mol)/ volume of solution (L)
      2. Practice
      3. Making dilutions M1V1= M2V2
      4. Practice
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