Chapter 9 - Solutions Flashcards
Solutions
Homogenous mixtures composed of 2 or more substances that combine to form single phase
Solubility
Maximum amount of a solute that can be dissolved in a given solute at a given temperature
Complex Ions/Coordination compounds
Composed of metallic ions bonded to various neutral compounds and anions
Solute
Component of solution that is present in lesser concentration than the solvent
Solvent
Component of the solution that remains in the same phase after mixing
Ligands
Electron pair donor molecules
Chelation
Central cation bonded to the same ligand in multiple places
Percent Composition by Mass
Used for aqueous solutions and solid-in-solid solutions
Mole Fraction
Used for calculating vapor pressure depression and partial pressures of gases in a system
Molarity
Most common unit for concentration and is sued for rate laws, the law of mass action, osmotic pressure, pH and pOH, and the Nernst equation
Molality
Used for boiling point elevation and freezing point depression
Normality
Molarity of the species of interest and is used for acid-base and oxidation-reduction reactions
Solubility Product Constant (Ksp)
The equilibrium constant for a dissociation reaction
Formation or Stability Constant (Kf)
Equilibrium constant for complex formation
Common Ion Effect
Decreases the solubility of a compound in a solution that already contains one of the ions in the compound
Saturation Point
Solute concentration is at its maximum value for the given temperature and pressure
Unsaturated
IP < Ksp
- Thermodynamically favored
Supersaturated
IP > Ksp
- Thermodynamically unstable
Saturated
IP=Ksp
- Equilibrium
Colligative properties
Physical properties of solutions that depend on the concentration of dissolved particles but not on their chemical identity
