Chapter 13 (Solutions): Homogeneous mixture of a solute dissolved in a solvent. Solubility: The amount of solute that can dissolve in a given amount of solvent Miscibility: Ability of one liquid to dissolve in another Saturated solution: A solution which holds the maximum amount of solute that it can. • Saturation point (ie: solubility) typically rises with increasing temperature. Electrolyte Solution: A solution of an ionic solid [as opposed to a non-electrolyte solution resultant from a solution of a non-ionic solid (ie: glucose)] “Like dissolves like”: • A polar solvent tends to dissolve polar substances (ie: water dissolves ionic compounds like NaCl)Methods of expressing solution concentration: 1) Mass Percent of a solute dissolved in a solvent: 2) Molarity (M): Moles substrate/L solution. • Ion concentration: i. Actual concentrations of ions of a dissolved ionic compound depends upon the stoichiometry of cations and anions. • Solution dilution: i. M1V1 = M2V2 (M = molarity; V = volume) • Solution stoichiometry: i. Takes “quantities” conversions from Chap. 8 one step further.3) Molality (m): Moles substrate/kg solvent. • Used when volume fluctuations of solution due to changes in temperature become significant. • Melting point depression. ∆Tf = m·Kf (Kf of H2O = 1.86