Upload
shauna-bradford
View
225
Download
0
Embed Size (px)
DESCRIPTION
Electrolytes Solutes dissolved in a solution can separate into ions These ions conduct electricity Strong electrolytes (soluble salts, strong acids and strong bases) conduct current well because they dissociate completely
Citation preview
Colligative PropertiesChapter 13.6
Colligative Properties• “Collective”-nature of• Effect on 4 properties: 1) Vapor pressure lowering2)Boiling point elevation3) Freezing point depression4) Osmotic pressure
Electrolytes• Solutes dissolved in a solution can
separate into ions• These ions conduct electricity• Strong electrolytes (soluble • salts, strong acids and strong • bases) conduct current well • because they dissociate completely
Raoult’s Law• Vapor pressure of the solvent over a solution
equals the mole fraction of solvent times the vapor pressure of the pure solvent; nonvolatile nonelectrolyte reduces vp.
• Psolvent = Xsolvent P°solvent
• Recognize that X is always <1 therefore, the new pressure is ALWAYS lower.
Vapor Pressure Lowering• So when a solute is added to a solvent,
less solvent can escape and vapor pressure is lowered
• ΔP = X solute P°solvent
•
• Read Sample Problem 13.6; Put Follow-up Problem on Dry Erase boards
• http://www.kchemistry.com/AddedTopics_1.htm
Boiling Point ElevationA solution boils at a higher temperature than the pure solventΔTb= boiling point elevation
ΔTb = Kb m
Kb = boiling pt elevation constant
m = solution molality
ΔTb= Tb(solution) - Tb(solvent)
Boiling point Elevation
http://www.btinternet.com/~martin.chaplin/collig.html
Freezing point depression
http://www.sparknotes.com/chemistry/solutions/colligative/section1.rhtml
Freezing Point Depression• ΔTf = Kfm
• ΔTf = freezing point depression
• Kf = molal freezing point depression constant
• m = molal concentration of the solute
• ΔTf = Tf(solvent) – Tf(solution)
Osmotic Pressure• Osmotic pressure is created when two solutions
are separated by a semipermeable membrane. The solvent can pass but not solute.
• Osmotic pressure: applied pressure required to prevent the net movement of water from solvent.
• II = nsoluteRT = MRT
• Vsoln
Overarching Colligative Pts!
• Each property rests on the inability of solute particles to cross between two phases. The solute reduces the solution’s ability to change phase-freeze, boil, vaporize or move across a semipermeable membrane.
• Note: van’t Hoff factor
http://www.youtube.com/watch?v=a2qOZmuhDBI&feature=related
Van’t Hoff factor• Strong electrolytes dissociate completely giving
2+ particles of solute per ionic compound. Example: MgCl2 dissolves into 3 particles unlike glucose.
• So: “i” = measured value for electrolyte solution»Expected value for nonelectrolyte»“i” = changes “m” on all colligative
properties
Van’t Hoff Factor
http://www.kentchemistry.com/KentsDemos.htm
http://www.youtube.com/watch?v=SX5V7kzmGeU