1. Solutions Ch. 11

2. Solution: Dissolved: Concentration: A solute dissolved in a solvent
A homogeneous mixture
Dissolved:
Broken apart into base particles (ions or molecules)
Concentration:
The density of dissolved solute in the solvent

3. Simulation / Animation

4. Dissociation Reactions communicate the process using symbols
NaCl  Na + Cl
CaCl2  Ca Cl
CuSO4  Cu + SO4
NH3  NH3
CO2  CO2
Cu(NO3)2  Cu NO3

5. Like Dissolves Like
Most solutions we discuss and encounter are aqueous (water solvent)
Water is polar so it dissolves polar or ionic substances (dipole-dipole or ion-dipole forces in the solution)
Oil is nonpolar so it dissolves nonpolar substances (dispersion forces)
Dipole-dipole forces will not be broken in order to be replaced by dipole-induced dipole forces or dispersion forces
Dispersion forces can not break dipole-dipole forces

6. Like Dissolves Like Hydrophilic Hydrophobic
Hydro = water
Philia = love
Hydrophilic = love for water
Hydrophobic
Phobia = fear
Hydrophobic = fear of water
Molecules with both a hydrophobic and hydrophilic end
Soap
Cell membranes

7. Energy Lattice Energy: Enthalpy of Hydration: Enthalpy of Solution:
Formula:

8. Energy:
Review Calorimetry
System vs surroundings

9. Electrolytes Conduct electricity when dissolved in water
Electricity is due to mobile charges
Dissolved ionic compounds contain mobile charges and are therefore electrolytes
Higher concentration of ions = stronger electrolyte

10. Concentration: density of solute in solvent or solution
Molarity = moles solute / Liters solution
Molality = moles solute / kg solvent
Mole fraction = moles solute / moles solution
% by mass = grams solute / grams solution
G solute / 100 g H2O (self explanatory)
ppm = ? Grams solute / 1,000,000 g solution (parts per million)
ppb = ? Grams solute / 1,000,000,000 g solution (parts per billion)

11. Concentration of ions in solution:
CaCl2(s)  Ca2+(aq) Cl-(aq)
If you have a 1.0 M solution of CaCl2,
Then you have a 1.0 M solution of Ca2+ ions
And you have a 2.0 M solution of Cl- ions
And you have a 3.0 M solution of total ions.

12. Concentration of ions:
CaCl2 is a stronger electrolyte than NaCl
Because it produces more ions
Therefore, if you have equal concentrations of CaCl2 and NaCl, CaCl2 solution will have greater conductivity than NaCl.
However, 0.05 M CaCl2 will have less conductivity than 2.0 M NaCl. Why?

13. Dilutions Dilution: If solute isn’t changed molesi = molesf
Since moles = (molarity)(Liters)
MolarityiLitersi = MolarityfLitersf

14. Types of solutions Typical solutions: solid dissolved in liquid
But all phases can be solute or solvent.

15. Solubility
Solubility = maximum possible concentration of dissolved particles
Saturated Solution:
Concentration = solubility
Unsaturated Solution:
Concentration < solubility
Supersaturated Solution:
Concentration > solubility
How does this occur?

16. Solubility
Solubility = maximum possible concentration of dissolved particles
Solubility of a solid-liquid solution is typically increased with increased temperature. Why?
Solubility of a gas-liquid solution is typically decreased with increase temperature. Why?
Solubility of a gas-liquid solution is typically increased with increased pressure. Why?

17. Density is based on concentration.
Density is also based on temperature.
Hotter liquids spread out and therefore have greater volume with equal mass (lower density)
D = m / v
Concentration could also change with temperature:
Any conc calculated using volume is temperature dependent.
Any conc calculated using only masses / # particles is not temperature dependent.

18. Colligative Properties
Anything that depends on the number of dissolved particles.

19. Colligative Properties
Solution’s boiling point increases with greater concentration of particles.
Solution’s melting point decreases with greater concentration of particles.
Solutions remain liquid through a greater range of temperatures with greater concentration of particles.

20. Colligative Properties

21. Colligative Properties: Melting Point

22. Colligative Properties: Melting Point & Boiling Point

23. Colligative Properties: Melting Point & Boiling Point

24. Colligative Properties

25. Colligative Properties: Vapor Pressure
A nonvolitile Liquid lowers the vapor pressure of a solvent.
Vapor Pressure: pressure over a liquid at gas-liquid phase equilibrium
More solute  less vapor pressure  less solvent will turn to gas
Psolution = Xsolvent Psolvent

26. Colligative Properties: Vapor Pressure

27. Colligative Properties: Vapor Pressure

29. Colligative Properties: Vapor Pressure

30. Side Note:
Surface area of liquid is directly proportional to the evaporation rate:
Water in a wider beaker will evaporate faster than water in a narrow, tall beaker

31. Osmosis Osmosis: the flow of solvent through a semipermiable membrane
from lower concentration to higher concentration
Net Flow of solvent continues until concentration on both sides are equal
Similar to heat transfer between 2 substances of different temperatures

32. Osmotic Pressure
Excess pressure on a solution with greater volume of solvent (see Figure 11.18)
By applying more pressure than the osmotic pressure to a container, you can create “reverse osmosis”
Desalinization !!!