CHEM 1125Q 1st Edition Lecture 10 Outline of Last Lecture Ch. 12I. Phase Changes and Phase DiagramsOutline of Current Lecture Ch. 13II. Physical Properties of SolutionsA. Solution ClassificationsB. SolvationIII. EntropyIV. Concentration UnitsA. MolarityB. MolalityC. Percent by MassCurrent LectureII. Physical Properties of SolutionsA. Solution Classificationsa. A solution is a homogenous mixture of two or more substancesi. The solute is dissolved in the solventii. Solutions are classified by the amount of solute they containb. Unsaturated i. In an unsaturated solution, there is less solute than the solution is able to holdc. Saturated i. In a saturated solution, the solution contains the maximum amount of solute that the solvent is able to hold at a certain temperatured. Supersaturated i. In a supersaturated solution, the solution contains more solutethan the solvent can hold, and is considered metastableii. Supersaturated solutions form when a saturated solution is slowly cooled so that the solubility is lower, but no precipitate formsiii. The supersaturated solution is metastable because as long as itis not disturbed, it will not precipitate. If more solute is added, then precipitate will formThese 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.B. Solvationa. Solvation refers to the process of forming a solutionb. Hydration is when water is used as the solvent in a solutionc. Solvation depends on the following:i. Solute-solute interactions (pure solute)ii. Solvent-solvent interactions (pure solvent)iii. Solute-solvent interactions (solution)III. EntropyA. Entropy is the measure of how spread out energy isa. The measure of orderb. Second Law of Thermodynamicsi. Energy’s natural tendency to dispersec. “like dissolves like”i. Substances with similar intermolecular forces are more likely to be soluble in each otherd. Two liquids are miscible is they are able to completely dissolve in eachotherIV. Concentration UnitsA. Molaritya. The Molarity of a solution is the moles of solute relative to the volume of solution (L)b. M = (mols solute)/(L solution)B. Molalitya. The Molality of a solution is the moles of solute relative to the mass ofsolvent (kg)b. m = (mols solute)/(kg solvent)C. Percent by Massa. The percent by mass of a solution is the mass of solute relative to the mass of solute and solventb. % = (mass solute)/(mass solute+solvent) x
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