1. Which solids will dissolve?
Solvent & Solute Video Clip

2. Homogeneous vs. heterogeneous mixtures
A mixture is a combination of two or more substances that are not chemically combined and that can be separated.
Could you give me an example?
Homogeneous vs. heterogeneous mixtures
Homogeneous mixtures are of uniform appearance
Heterogeneous mixtures consists of visibly different substances

3. Solutions Solution Chocolate milk Carbonated water Alloys
A solution is a group of molecules that are mixed up in a completely even distribution.
Chocolate
milk
Carbonated
water
Alloys

4. Solute and Solvent Solute Solvent
A solute is the substance to be dissolved.
Solvent
A solvent is the substance doing the dissolving.

5. Solubility Solubility Factors that affect solubility
Ability of the solvent to dissolve the solute.
Factors that affect solubility
Structure of
the substance
Temperature
Pressure

6. Classification of solutions
Saturated solutions
have the maximum amount of solute dissolved in them. No more solute can be made to dissolve.
Unsaturated solutions
have less than the maximum amount of solute dissolved in them. This means that more solute could be added to the solution and the additional solute would still dissolve.
Supersaturated solutions
have more than the maximum amount of solute dissolved in them. Not all substances will form supersaturated solutions.

7. Saturated
Unsaturated
Supersaturated

8. Suspensions
The particles in suspensions are larger than those found in solutions. Components of a suspension can be evenly distributed by mechanical means, like by shaking the contents, but the components will settle out.
Chalk in water
Dust in air

9. Which solids will dissolve?

10. Properties of Water
surface tension = water is pulled together creating the smallest surface area possible.
Water has a high heat capacity.
In order to raise the temperature of water, the average molecular speed has to increase.
It takes much more energy to raise the temperature of water compared to other solvents because hydrogen bonds hold the water molecules together!
“The specific heat is the amount of heat per unit mass required to raise the temperature by one degree Celsius.”
3. Density: Water is less dense as a solid! This is because the hydrogen bonds are stable in ice – each molecule of water is bound to four of its neighbors.