Chapter 13 Ions in Aqueous Solutions and Colligative

Chapter 13 Ions in Aqueous Solutions and Colligative Properties 13 -1 Compounds in Aqueous Solutions

Dissociation The separation of ions that occurs when an ionic compound dissolves • One formula unit of Na. Cl produces two ions: • One mole of Na. Cl produces two moles of ions • One formula unit of Ca. Cl 2 produces three ions: • One mole of Ca. Cl 2 produces three moles of ions

Dissociation Equations Na. Cl(s) Na+(aq) + Cl-(aq) Ag. NO 3(s) Ag+(aq) + NO 3 -(aq) Mg. Cl 2(s) Mg 2+(aq) + 2 Cl-(aq) Na 2 SO 4(s) Al. Cl 3(s) 2 Na+(aq) + SO 42 -(aq) Al 3+(aq) + 3 Cl-(aq)

Precipitation Reactions Solubility Rules • No compound is completely insoluble • Compounds of very low solubility can be considered insoluble • Dissociation equations cannot be written for insoluble compounds

Double replacement forming a precipitate… Double replacement (ionic) equation Pb(NO 3)2 (aq) + 2 KI (aq) Pb. I 2 (s) + 2 KNO 3 (aq) Spectator ions are those ions that do not take in a chemical rxncompounds and are found in Complete ionic part equation shows assolution both before and after the rxn aqueous ions Pb 2+ (aq) + 2 NO 3 - (aq) + 2 K+ (aq) +2 I- (aq) Pb. I 2 (s) + 2 K+ (aq) + 2 NO 3 - (aq) Net ionic equation eliminates the spectator ions Pb 2+ (aq) + 2 I- (aq) Pb. I 2 (s) Includes only those compounds and ions that undergo a chemical change in a reaction in an aqueous solution

Ionization • Ions are formed from solute molecules by the action of the solvent • Polar water molecules are attracted to polar solute molecules • Electronegative oxygen of water is attracted to electropositive portion of a solute molecule • Electropositive hydrogen of water is attracted to the electronegative portion of a solute molecule

The Hydronium Ion • H 3 O+ is called the "hydronium" ion

Strong Electrolytes • Any compound of which all or almost all of the dissolved compound exists as ions in an aqueous solution • All soluble ionic compounds are strong electrolytes • Hydrogen halides : HCl, HBr, HI

Weak Electrolytes • A compound of which a relatively small amount of the dissolved compound exists as ions in an aqueous solution • Examples: HF, organic acids

Chapter 13 Ions in Aqueous Solutions and Colligative Properties 13 -2 Colligative Properties

Colligative Properties • These are properties that are dependent only on the number & concentration of solute particles.

Vapor Pressure Lowering • Effect of Solutes on Vapor-Pressure Any nonvolatile solute will lower the vapor pressure of a solution, having two noticeable effects: • Raising the boiling point of the solution • Lowering the freezing point of the solution

Solute particles take up space @ the liquid-air surface. So vapor pressure is lowered, boiling occurs at a higher temp b/c more energy is required for the vapor pressure to equal the atmospheric pressure.

Freezing Point Depression • Solutions have lower freezing points than pure solvents. • If the solution is aqueous, its freezing point will always be lower than 0 C. • How much lower? • Depends on the # & concentration of solute particles. • Ex: Salt on ice in the winter

Colligative Properties • Colligative properties depend on: number & concentration of solute particles • Since ionic substances dissolve into multiple particles, their colligative effects are greater than those of covalent substances.

Freezing Point Depression • Ionic solutes depress the freezing point more than covalent solutes. Look at their solubility rxns, note the number of particles formed: • Ionic: Na. Cl (s) + H 2 O (l) Na+ (aq) + Cl- (aq) 2 particles formed • Covalent: C 6 H 12 O 6 (s) + H 2 O (l) C 6 H 12 O 6 (aq) 1 particle formed

Molal Freezing-Point Constant for Water • The freezing-point depression of the solvent in a 1 molal solution of a nonvolatile, nonelectrolyte solute Kf = -1. 86 °C/m • Freezing-Point Depression • The difference between the freezing points of the pure solvent and a solution of a nonelectrolyte in that solvent Δtf = K f m Where: m = molality Δtf = change in freezing point

Boiling Point Elevation • Solutions have higher boiling points than pure solvents. • If the solution is aqueous, its boiling point will always be higher than 100 C. • Boiling: Temperature at which vapor pressure equals atmospheric pressure.

Molal Boiling-Point Constant for Water • The boiling point elevation of the solvent in a 1 -molal solution of a nonvolatile, nonelectrolyte solute Kb = 0. 51 °C/m • Boiling-Point Elevation • The difference between the boiling points of the pure solvent and a solution of a nonelectrolyte in that solvent Δtb = K b m Where: m = molality Δtb = change in boiling point

The van’t Hoff Factor, i Electrolytes may have two, three or more times the effect on boiling point and freezing point, depending on its dissociation. T = i K m

Freezing Point Depression and Boiling Point Elevation Constants

Dissociation Equations Na. Cl(s) Na+(aq) + Cl-(aq) i=2 Ag. NO 3(s) Ag+(aq) + NO 3 -(aq) Mg. Cl 2(s) Mg 2+(aq) + 2 Cl-(aq) Na 2 SO 4(s) i=3 2 Na+(aq) + SO 42 -(aq) Al. Cl 3(s) Al 3+(aq) + 3 Cl-(aq) i=4

Ideal vs. Real van’t Hoff Factor • • • Attractive forces between ions cause clustering Clustering is greatest in concentrated solutions Ideal and real results are closest in very dilute solutions The Debye-Huckel Theory Clustering hinders the movements of ions, so fewer ions appear to be present

Ideal vs. Real van’t Hoff Factor The ideal van’t Hoff Factor is only achieved in VERY DILUTE solution.

Preventing icing of roads using Ca. Cl 2

Osmotic Pressure • Semipermeable membranes • Membranes that allow the movement of some particles while blocking the movement of others • Osmosis • The movement of solvent through a semipermeable membrane from the side of lower solute concentration to the side of higher solute concentration • Osmosis occurs when two solutions of different concentration are separated by a semipermeable membrane

Osmotic Pressure • The external pressure that must be applied to stop osmosis • Osmotic pressure increases with the concentration of solute particles • Osmotic pressure is not dependent on the TYPE of solute particles