1. Chapter 15 = Solutions
Solutions = homogeneous mixtures containing two or more substances
Solute = substance that gets dissolved; smallest part of solution
Solvent = substance that does the dissolving; largest part of solution

2. Solutions are not always made of 2 liquids
Carbon + Iron
Nitrogen + Oxygen

3. Soluble = substance that can be dissolved in solvent
Sugar and water
Insoluble = substance that can not be dissolved in solvent
Oil and water

4. Miscible = two liquids are soluble in each other
alcohol and water
Immiscible = two liquids are not soluble in each other
Oil and water

5. Solvation- the process of solvent particles breaking apart solute crystals into particles the size of ions

6. Tyndall Effect
Solutions allow light to pass through without being scattered
Think about air
Non-solutions cause the light to be scattered
Think about fog
We’ll cover this more in depth in section 15.4

7. Electrolyte- solutions that can conduct electricity due to ions in the solution

8. Covalently bonded molecules do not break apart to form ions in solutions but they still do dissolve

9. Factors that Affect the Rate of Solvation
To increase solvation we need to increase the number of times the solute and solvent touch
Shake (agitate) the mixture
Break to increase surface area
Bake—increase temperature

10. Solubility-maximum amount of solute that will dissolve in a given amount of solvent at a specified temperature and pressure
Eventually, solute particles will begin to collide with each other and form crystals.

11. Unsaturated Saturated Supersaturated
Contains less than maximum amount of dissolved solute
Saturated
Contains maximum amount of dissolved solute
Supersaturated
Contains more than maximum amount of dissolved solute

12. If you add extra solute to…
Unsaturated
Solute will dissolve
Saturated
Supersaturated
Solute will crystallize

13. Solubility Curves
Each substance has its own unique solubility which can be displayed on a graph

14. Supersaturated solution- solution holding more solute than a saturated solution at the same temperature and pressure
Mentos and Diet Coke
CO2 is greater than normal levels
When Mentos are placed into the CO2 jumps out of solution

15. Temperature and Solubility
SOLID- As temperature increases solubility of a solid solute will increase (few exceptions)
GAS- as temperature increases solubility of a gas will decrease

16. Pressure and solubility
Henry’s Law – solubility of any gas increases as the external pressure is increased
This is why cokes go flat. When you open the can the external pressure has been reduced and this decreases the solubility of the carbonation (CO2)

17. If 0. 55 g of a gas dissolves in 1
If 0.55 g of a gas dissolves in 1.0 L of water at 2 atm of pressure, how much will dissolve at 4.5 atm of pressure?
2x = 2.475
X= g/L

18. A gas has solubility of 0. 66 g/L at 10 atm of pressure
A gas has solubility of 0.66 g/L at 10 atm of pressure. What is the pressure on a 1 L sample that contains 1.5 g of gas?
0.66 x = 150
X= atm

19. 3. A gas has a solubility of 1. 46 g/L at 8 atm of pressure
3. A gas has a solubility of 1.46 g/L at 8 atm of pressure. What is the pressure of a 1.0L sample that contains 2.7 g/L?
answer = 14.8 atm
4. If 0.68 g of a gas at 5 atm of pressure dissolves in 1.0 L of water at 25°C, how much will dissolve in 1.0L of water at 8 atm of pressure and the same temperature?
answer = 1.09 g/L