CHEM 2111st EditionLecture 9Outline of Last Lecture I. Interconverting Concentration TermsII. Colligative Properties of SolutionsIII. Vapor Pressure LoweringIV. Boiling Point ElevationV. Freezing Point DepressionOutline of Current Lecture I. Osmotic PressureII. Volatile Nonelectrolyte SolutionsIII. Strong Electrolyte SolutionsIV. Colligative Properties of Electrolyte SolutionsV. Non-ideal behavior of strong electrolyte solutionsCurrent LectureI. Osmotic PressureA. Osmosis is the movement of solvent particles from a region of higher to a region of lower concentration through a semipermeable membrane.B. Solvent will always flow from a more dilute solution to a more concentrated one.C. Osmotic pressure is the pressure that must be applied to prevent the net flow of solvent.a) π = MRT M = molarity, R = 0.0821 atm·L/mol·K, T = Kelvin temperatureII. Volatile Nonelectrolyte SolutionsA. For a volatile nonelectrolyte, the vapor of the solution contains both solute and solvent.B. The presence of each volatile component lowers the vapor pressure of the other, since each one lowers the mole fraction of the other.C. For such a solution, the vapor will have a higher mole fraction of the more volatile component.D. The vapor has a different composition than the solution.III. Strong Electrolyte SolutionsA. A strong electrolyte dissociates completely to form ions. Each mole of solute gives more than 1 mol of dissolved particles.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.B. The formula of the compound indicates the expected number of particles in solution.C. Each mol of NaCl is expected to give 2 moles of dissolved ions.D. The Van Hoff factor takes into account thedissociation of a strong electrolyte to predict theeffect on the solution.IV. Colligative Properties of Electrolyte SolutionsA. For vapor pressure lowering: ∆P = i(Csolute x Posolvent)B. For boiling point elevation: ∆Tb = i(Kbm)C. For freezing point depression: ∆Tf = i(Kfm)D. For osmotic pressure: π = i(MRT)V. Non-ideal behavior of strong electrolyte solutionsA. Ions in solution may remain clustered near ions of opposite charge, creating an ionic atmosphere. The ions do not act independently, and the effective concentration of dissolved particles is less than expected.B. Ions may remain clustered together in solution, forming an ionic atmosphere. This effect is greater for a more concentrated