1. Solutions
Chapter 13
5.0 Chemistry

2. What is a solution
Solution: A homogeneous mixture of 2 or more substances in a single physical state.
Suspension: Particles are somewhat evenly dispersed, but will settle when at rest. (clay & water)
Colloid: Particle size between suspension and solution (milk)

3. Properties of Solutions
Small Particles
Evenly distributed particles
Particles do not separate when at rest.
Solubility: The ability to dissolve in another substance.

4. Properties of Solutions
Solute: substance that is dissolved
Solvent: Substance that does the dissolving
Solvent
Solute

5. Properties of Solutions
Soluble means something can be dissolved in something else.
Insoluble means something cannot be dissolved in something else.

6. Solid Solutions
Alloys: Solid solutions that contain 2 or more pure substance.
Advantages of alloys over pure metals:
Stronger
Cheaper
Resistance from corrosion
Lighter

7. Alloys

8. Gaseous Solutions
The properties of gaseous solutions depend on the properties of its components.
Ex. Air

9. Liquid Solutions
Miscible Liquids: 2 liquids that can mix together in any amount
Ex. Alcohol and water

10. Liquid Solutions Immiscible Liquids: 2 liquids that cannot mix
Ex. Oil and Water

11. Other types of solutions
Aqueous Solutions: Solutions with water as the solvent.
Because water can dissolve so many things, it is called the universal solvent.

12. Electrolyte: A solution that conducts electricity

13. Tincture: Solutions with alcohol as the solvent.

14. O2 N2 CO2 H2O Pt air lemon juice water mercury silver carbon sugar
Type of Solution
Specific Solute
Specific Solvent
Gas in Gas
Air O2 N2
Gas in Liquid
Soda
CO2
H2O
Gas in Solid
catalytic converter
hydrocarbons Pt
Liquid in Gas
fog
air
Liquid in Liquid
Lemonade
lemon juice
water
Liquid in Solid
teeth fillings
mercury
silver
Solid in Gas
smoke
carbon
Solid in Liquid
Kool-Aid
sugar
Solid in Solid
steel
iron IN

15. Concentration and Molarity
Concentration: Refers to the amount of solute per given amount of solvent.
Dilute Solutions – Has little solute
Concentrated Solutions – Has large amount of solute

16. Molarity Molarity Molarity – Term used for concentration =
Moles of Solute
Liters of Solution

17. D. Molarity: (M)
Ex #1) What is the molarity of a solution formed by mixing 10.0 g of sulfuric acid with enough water to make mL of solution?

18. Ex #2) How many grams of bromine are needed to prepare 0. 500 L of a 0
Ex #2) How many grams of bromine are needed to prepare L of a M solution of bromine in water?

19. Solubility and the Dissolving Process
Saturated: A solution is saturated if it contains as much solute as can possibly be dissolved under existing conditions of temperature and pressure.
Unsaturated: Has less than the maximum amount that can be dissolved.
Supersaturated: Has more than the maximum amount that can be dissolved.

20. Saturated vs. Unsaturated

21. Saturated vs. Unsaturated

22. Supersaturated

23. Dilutions
Formula for Dilutions:
M1V1 = M2V2

24. How a solution forms
Process of dissolving takes place at the surface of the solute.

27. Dissolving Process
The interaction between the solute and solvent to allow ions to separate is called solvation. This interaction is called hydration when water is the solvent.

28. Dissolving Process Energy is absorbed when the bonds break. (endo)
Energy is released when bonds form. (exo)

29. Solubility
Solubility is amount of solute that will dissolve in a specific solution under given conditions.
See solubility curves

30. Supersaturated solution
At 20 oC, a saturated solution contains how many grams of NaNO3 in 100 g of water?
Saturated sol’n
90 g
Supersaturated solution
What is the solubility at 70 oC?
135 g/100 g water
What kind of solution is formed when 90 g NaNO3 is dissolved in 100 g water at 30 oC?
Unsaturated solution
unsaturated
What kind of solution is formed when 120 g NaNO3 is dissolved in 100 g water at 40 oC?
supersaturated

32. Factors that affect solubility
1) Nature of Solute and Solvent
General rule: Like dissolves Like
See example
2) Temperature
As temperature increases, the solubility of gases and liquids decrease.

33. Gases are less soluble at high temperatures than at low temperatures.

34. Pressure: As pressure increases, the solubility increases.

35. Factors Affecting the Rate of Dissolving
1) Surface Area
2) Stirring
3) Temperature
Altering these 3 factors will either increase the frequency of collisions or the energy of collisions between the solute and solvent.