1. Chapter 14
Solutions

2. Types of Mixtures Heterogeneous- do not blend smoothly throughout
Colloids- Intermediate sized particles that do not settle out
IMF and electrostatic forces keep particles intermixed
Brownian Motion- jerky random motion observed in particles. A result of the collisions of particles in a colloid that keep the particles dispersed.
Suspensions- particles settle out
Thixotropic Mixtures- The solid that settles from a suspensions flows like a liquid when disturbed (paint)

3. Tyndall Effect
You can tell the difference between a colloid and a solution by looking for the Tyndall effect
Colloids- Particles are large enough to scatter light
Solutions- Particles are so small that they do not scatter light

4. Types of Mixtures Homogeneous- Composition is the same throughout
Liquid solutions are most common, but there are gas and solid solutions as well
Solute- substance that is dissolved
Solvent- substance that does the dissolving (is in greater amounts)
Soluble- when a substance is able to be dissolved in a solvent
Miscible- When two liquids can dissolve into each other

5. Terms for Solutions
Insoluble- when a solid will not dissolve in a solvent
Immiscible- when two liquids can not be dissolved into each other
Solubility- Defined as the maximum amount of solute a solvent can hold at any given temperature

6. Factors Affecting Solvation
Solvation – the process of surrounding solute particles with solvent particles to form a solution
Affected by:
Temperature
Pressure
Polarity

7. Factors That Affect Solvation
Agitation – stirring or shaking
Surface Area – increased surface area speeds up solvation
Temperature – higher temperatures allow more solid to dissolve in solution

8. Types of Solutions
Unsaturated Solution– contains less dissolved solute than it can hold
Saturated Solution – contains the maximum amount of dissolved solute for a given amount of solvent
Supersaturated Solution – contains more dissolved solute than a saturated solution
Highly unstable

9. Supersaturated Solutions
Made by dissolving solute at high temperatures, then cooling so the solute stays dissolved.
Disturbance of solution will cause excess solute to crystallize in solution until the solution is saturated.
ROCK CANDY!

10. Solubility Graphs
Shows the solubility for a substance dependent on temperature.
Any point on the line represents a saturated solution.
Saturated solution
Supersaturated solution
Unsaturated solution

11. Supersaturated
Saturated
Unsaturated

12. At 50 degrees Celsius, 30 grams of KClO3 is dissolved in solution, what type of solution is this?
At 60 degrees Celsius, 70 grams of Pb(NO3)2 is dissolved in solution, what type of solution is this?
How many grams of KCl can dissolve in 200 grams of H2O at 10 degrees Celsius?

13. Concentration of Solutions
Molarity- (M) moles of solute dissolved per liter of solution
M is read as molar
Molarity (M) = moles of solute /liter of solution
Diluting a solution- to make a less concentrated solution, you take an amount of moles from the more concentrated sample and add water until you reach the desired concentration.
Dilution Equation:
M1V1= M2V2

14. Concentration of Solutions
What volume of a 3.00 M KI stock solution would you use to make L of a 1.25 M KI solution?
How many mL of 5.0 M H2SO4 stock solution would you need to prepare mL of 0.25 M H2SO4?

15. In a solution, there are attractions between
Solute-solute particles
Solvent-solvent particles
Solute-solvent particles
When these attractive forces are greater than solute-solute forces, a substance dissolves!

16. Polarity: “Like Dissolves Like”
Polar substances dissolve in other polar substances
Nonpolar substances dissolve in other nonpolar substances

17. Energy Breaking bonds requires energy Forming bonds releases energy
Overcome solute attractive forces
Overcome solvent attractive forces
Forming bonds releases energy
Attraction of solute-solvent particles
Heat of Solution – overall energy change that occurs during solution formation
Endothermic – energy is absorbed (feels cold)
Exothermic – energy is released (feels hot)

18. Solubility of Gases Soluble at low temperature
Particles have less kinetic energy and therefore cannot escape solution as easily
Soluble at high pressure
Gases above solution push down on the solution and keep gas particles in.
Soda

19. Henry’s Law Solubility (S) is directly proportional to pressure (P) S1=