Solutions

• 1. Both solute & solvent have similar properties 
• 2. Solute molecules are separated from one another by being surrounded completely by solvent molecules  

• 1. Type of solution 
• 2. CANNOT be separated by filtration
• 3. Scatter light
• 4. Solute particles do not settle out of solution  

• 1. Dialysis (i.e. use of semipermeable membrane)
• 2. Charge separation
• 3. Filtration AFTER heating  

Solute particles coagulate and can be separated via filtration 

Polar: dipole-dipole

Non-polar: London Dispersion Forces  

Not normally, but when it contains electrolytes it is 

• 1. Molarity 
• 2. Molality
• 3. Mole fraction
• 4. Mass percentage
• 5. Parts per million  

• 1. Breaking intermolecular bonds between solute molecules (+H)
• 2. Breaking intermolecular bonds between solvent molecules (H+)
• 3. Making intermolecular bonds between solute and solvent molecules (-H)

Entropy always increases when solutions form 

• 1. Does not contribute to vapor pressure
• 2. Consumes surface area of liquid and thus, reduces vapor pressure by limiting the amount of solvent molecules that can escape into a gas -- so affects the overall vapor pressure of the solution, but indirectly 

• 1. Contributes to a solution's vapor pressure
• 2. Competes for the surface area

*Sum of partial pressure of each contributor of solution will give total vapor pressure of the solution 

If Hsoln is negative: stronger bonds have been formed so vapor pressure will be lower than predicted 

If Hsoln is positive: weaker bonds have formed so vapor pressure will be higher than predicted 

Percipitation 

Rate of dissolution = Rate of percipitation 

Adding any more solute will form a percipitate

Ksp ; same as Keq except specialized to a solution ; called the solubility product 

This is a constant value that can be found in a book 

Remember to leave out pure solids and liquids

Changes with temperature ONLY

The solubility of something in a given solvent 

AKA the maximum number of moles that can dissolve in a solution

Changes with temperature and ions present 

Ions in a solution that have no effect on the equilibrium constant AKA the solubility product 

A saturated solution is at equilibrium, meaning that the maximum moles of solute have been able to dissolve in the given solvent. 

1. The [] of solute is at a maximum, any more solute added would push this reaction backwards and percipitate will form

2. The [] of the solvent is at a minimum because the solute's [] is maximized

Partial pressures always add up to give total pressure