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UA CH 102 - Solutions
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CH 102 1st Edition Lecture 6** First Exam February 4Outline of Current Lecture I. SolutionsII. SolubilityIII. Temperature Dependence of Solubility of Solids in WaterIV. Methods of Expressing Solution ConcentrationV. Colligative PropertiesCurrent LectureI. Solutionsa. Solutions are homogeneous mixtures. i. Two or more substances make up a mixture.ii. A solution may be composed of a solid and a liquid, a gas and a liquid, or other combinations.b. Solutions have a solute component and a solvent component.i. The majority component of a solution is called thesolvent.ii. The minority component is called the solute.1. The solute is dissolved into the solvent.c. Solution formation is the result of the interaction of the intermolecular forces of solute and solvent particles.i. Likes dissolve in likes.d. Nature has a tendency toward spontaneous mixing.i. Generally, uniform mixing is more energetically favorable.e. Solutions: Effect of Intermolecular Forcesi. For the solvent and solute to mix, you must overcome1. all of the solute–solute attractive forces; or 2. some of the solvent–solvent attractive forces.a. Both processes are endothermicii. At least some of the energy to do this comes from making new solute–solvent attractions, which is an exothermic process.These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.II. Solubilitya. When one substance (solute) dissolves in another (solvent), it is said to be soluble.i. Ex: Salt is soluble in water.ii. Ex: Bromine is soluble in methylene chloride.b. When one substance does not dissolve in another, it is said to be insoluble.i. Oil is insoluble in water.c. The solubility of one substance in another depends on the following:i. Nature’s tendency toward mixing ii. The types of intermolecular attractive forcesd. When solutions with different solute concentrations come in contact, they spontaneously mix to result in a uniform distribution of solute throughout the solution.III. Temperature Dependence of Solubility of Solids in Watera. Solubility is generally given in grams of solute that will dissolve in 100 g of water.b. For most solids, the solubility of the solid increases as the temperature increases.c. When ΔHsolution is endothermicd. Solubility curves can be used to predict whether a solution with a particular amount of solute dissolved in water is saturated (on the line), unsaturated (below the line), or supersaturated (above the line).IV. Methods of Expressing Solution ConcentrationV. Colligative Propertiesa. Colligative properties are properties whose value depends only on the number of solute particles and not on what they are.i. Value of the property depends on the concentration of the solution.b. The difference in the value of the property between the solution and the pure substance is generally related to the different attractive forces and solute particles occupying solvent molecules’


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UA CH 102 - Solutions

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