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Unit 2

Unit 2. Liquids, solids, solubility, and equilibrium. Solubility Rules. Given reactants, can anticipate what products will form By looking at solubility rules, can predict whether or not a precipitate will form. Sample Problem. KOH (aq) + AgNO 3 (aq) . KNO 3 (aq) + AgOH (s).

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Unit 2

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  1. Unit 2 Liquids, solids, solubility, and equilibrium

  2. Solubility Rules • Given reactants, can anticipate what products will form • By looking at solubility rules, can predict whether or not a precipitate will form

  3. Sample Problem KOH (aq) + AgNO3 (aq)  KNO3 (aq) + AgOH (s) AgOH precipitates because hydroxides are generally insoluble

  4. Electrolytic Properties • Electrolyte=solution containing ions • The more a substance dissociates, the stronger the electrolyte • Non-electrolyte=solution containing no ions

  5. Solids • Retain shape & volume • Virtually incompressible • Diffusion occurs very slowly • Strong intermolecular forces • Particles close together

  6. Liquids • Assume shape of container • Definite volume • Does not expand to fill container • Virtually incompressible • Flows readily • Diffusion occurs slowly • Particles fairly close together

  7. Gases • Assume both volume & shape of container • Compressible • Flow easily • Diffusion occurs rapidly • Widely separated molecules • Disorder • Particles free to move

  8. Phase Diagram

  9. Phase Changes

  10. (vaporization) Heating Curve

  11. Intermolecular Forces of Attraction • Ion-dipole: exist between an ion and the partial charge on end of a polar molecule • Dipole-dipole: exist between neutral polar molecules, attraction between unlike charges on ends of molecules, significant only when molecules very close together • London dispersion: exist only when molecules are very close together, nonpolar atoms/molecules experience temporary dipoles, momentary dipoles attract • Hydrogen bonding: exist between a hydrogen atom in a polar bond and an electronegative element, (H-F, H-O, H-N)

  12. Bonding in Solids • Molecular solids: atoms/molecules held together by intermolecular forces (London dispersion, dipole-dipole, hydrogen bonds), soft, relatively low boiling points, poor thermal and electrical conduction, i.e. methane, sucrose, and dry ice • Covalent-network solids: atoms held together by covalent bonds, very hard, high melting points, poor thermal and electrical conductors, i.e. diamonds • Ionic solids: ions held together by ionic bonds, hard and brittle, high melting points, poor thermal and electrical conduction, i.e. salts • Metallic solids: metal atoms held together by metallic bonds, vary in strength of bonding, wide range of physical properties (hardness, melting points), malleable and ductile, excellent thermal and electrical conductors, i.e. copper, iron, aluminum

  13. Crystalline Structure • Simple cubic: 1 atom, V=8r3, e=2r • Body-centered: 2 atoms, V=(4r/√3)3, e=4r/√3 • Face-centered: 4 atoms, V= (32r3/√2), e=4r/√2

  14. Equilibrium aA + bB ↔ dD + eE Kc=[D]d [E]eKp=[PD]d [PE]e [A]a [B]b[PA]a [PB]b Δn KP=KC (RT)

  15. Le Châtlier’s Principle • Any disturbance to a system in equilibrium will produce a shift in equilibrium that offsets the disturbance as much as possible • Add or subtract product/reactant, change temperature, change pressure, etc. • Reaction Quotient: Q is the number obtained by substituting pressures or concentrations into an equilibrium-constant expression (Kc or Kp) • QC = KC system at equilibrium • QC < KC needs to shift right to reach equilibrium • QC > KC needs to shift left to reach equilibrium

  16. Sample Problem • 4Liza + 2Mr. Hinton ↔ 7Juan • Increase amount of Liza… • Decrease amount of Mr. Hinton… • Increase pressure… • Increase volume…

  17. Solutions • Ksp is the product of the concentration of the ions involved in equilibrium, each raised to the power of its coefficient in the equilibrium equation • A (s) ↔ bB (aq) + dD(aq) Ksp=[B]b[D]d • Given the value of Ksp, you can find the concentrations of ions in solution • Remember that solids are not included in the Ksp equation

  18. Sample Problem PbSO4 (s) ↔ Pb2+ (aq) + SO42- (aq) Given: Ksp = 1.8 x 10-8 Ksp = [Pb2+ ][SO42-] = x2  x = √(1.8 x 10-8) X = 1.3 x 10-4 = [Pb2+ ] = [SO42-]

  19. Molarity, Molality, Mass Fraction • Mole fraction= (moles of component)/(total moles of all components) • Molarity= (moles solute)/(liters solution) • Molality=(moles solute)/(kg of solvent) • Mass fraction= (mass solute)/(mass solution)

  20. Raoult’s Law • Pvapor=XP°vapor • X is the mole fraction of a solvent in solution • P°vapor is the vapor pressure of the pure solvent • Pvapor is the partial pressure of a solvent over a solution

  21. Henry’s Law • Sg=kPg • Sg is the solubility of the gas in the solution phase • Pg is the partial pressure of the gas over the solution • k is a proportionality constant

  22. Boiling Point Elevation and Freezing Point Depression • Boiling Point Elevation: ΔTb=iKbm • i is the number of particles • Kb is a constant • m is molality • Freezing Point Depression: ΔTf =iKfm • i is the number of particles • Kf is a constant • m is molality

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