Learning Outcomes - Exam 1

Physical Equilibria

Students will be able to...

  1. Predict the sign of ΔG, ΔH, and/or ΔS for physical change
  2. Interpret heating curves and calculate heat required for phase transitions and temperature changes
  3. Describe phase transitions (macroscopically and microscopically) as well as differentiate between boiling and evaporation
  4. Understand how intermolecular forces, temperature, and solute concentration affect vapor pressure.
  5. Interpret phase diagrams and identify normal boiling and melting point, critical point, and triple point.
  6. Describe the factors that favor the dissolution process in terms of intermolecular forces and thermodynamics (enthalpies of solution, hydration, lattice energy, entropies of solution, free energy of solution….)
  7. Describe how T and P (Henry’s Law) each affect solubility.
  8. Define and perform calculations for common concentration units molarity, molality, and mole fraction.
  9. Perform calculations and discuss the concepts of the 4 colligative properties: vapor pressure lowering, boiling point elevation, freezing point depression, and osmotic pressure.
  10. Describe the dissociation of ionic compounds in solution and the effects on colligative properties (van’t Hoff factor, i ).

Solubility Equilibria

Students will be able to...

  1. Understand the concept of the solubility product, Ksp.
  2. Write total and net ionic equations to identify spectator ions.
  3. Determine solubility from Ksp and vice versa.
  4. Estimate molar solubility from Ksp.
  5. Understand and apply the "common ion effect" on solubility.
  6. Given concentrations of specific ions, predict if a precipitate will form (amount or concentration) using Qsp vs Ksp.