1. Solutions

2. Solutions
A mixture that appears the same throughout and is mixed at the molecular level.
Solutions can be liquids, gases or solids.
Alloys are SOLID solutions.

3. Classifying Matter - Overview

5. Properties of solutions, colloids and suspensions
Suspension – Solution in which solid particles are in a liquid. (Particles settle.)
Colloid – Homogeneous solution – large particles, light cannot shine through.
Emulsion – a type of colloid where a liquid is dispersed in another liquid ex:mayonnaise, milk
Foam - a type of colloid that is a gas dispersed in a liquid ex: whipped cream

6. In the Mix: Solute – Substance being dissolved.
Solvent – Substance doing the dissolving. (Usually the larger quantity.)
Immiscible – liquid solutes and solvents that are not soluble in each other
Miscible – liquids that dissolve freely in one another

7. Solubility
Solubility – the amount of a substance required to form a saturated solution with a specific amount of solvent at a specified temperature
Soluble – capable of being dissolved
Aqueous solution – many times we consider a substance aqueous when it can be dissolved and water is part of the solution

8. Types of Solutions
Saturated – Contains all the solute it can hold at a given temperature.
Unsaturated – Able to dissolve more solute at a given temperature.
Supersaturated – Contains more solute than a saturated one at the same temp.
These are unstable solutions made by raising the temp of a saturated solution then adding more solute.

9. Reading Solubility Graphs
According to the graph above, about how many grams of KBr are needed to make a saturated solution in 100 g of water at 30° C?
70 grams KBr

10. Reading Solubility Graphs
According to the graph above, what kind of solution would you have if you dissolved 10 g of KCl in 100 g of water at 0°C?
Unsaturated

11. Some Solubility Curves
How many grams of KNO3 can be dissolved in 200g of water at 50oC?
160g

12. Water Water is the “universal solvent”.
Each water molecule is connected by hydrogen bonds.
Hydrogen bonds creates
a high surface tension

13. Water
Water molecules are polar – they have a (+) end and a (-) end.

14. Water phases of matter

15. How dissolving happens
Water molecules cluster around the solid molecules with their negative ends attracted to the positive ends of the solid.
Water molecules and solid molecules spread out and mix evenly to form a solution.

18. Solubility
Solvation (solvated) – process of surrounding solute particles with solvent particles to form a solution
The rule for dissolving solutions is “like dissolves like”
Polar substances will dissolve in polar solvents
Non polar substances will dissolve in non polar solvents
Non polar will NOT dissolve in polar and vice versa

19. Increasing the Rate of Solvation
Agitation (Stir, Shake)
Increasing Temperature
Increasing Surface Area (Crush)

20. Agitation
Increases the speed of the particles
speeds up the dissolving process when dissolving solids into liquids.
Decreases the dissolving process in gases.

21. Increasing Temperature
More collisions of particles as temperature increases.

22. Particle Size (Increasing Surface Area)
Smaller particles dissolve faster than larger particles.
more surface area
Sugar cube vs. ½ teaspoon sugar
(Teaspoon will dissolve faster)

23. Rate of Dissolving for gases
Pressure (gases) – Increase in pressure causes more to dissolve. Ex: soda

24. Effects of temperature on solubility of a gas
Increasing temperature decreases gas solubility
Think of drinking a coke…what’s fizzier, a cold coke or a hot coke?

25. Effects of pressure on solubility of a gas
Increasing pressure, increases gas solubility
effervescence
Think of a coke bottle…What will happen if you leave the lid off?

26. Henry’s law

27. Other Solutions
Electrolytes – Solution of ions that conduct electricity.
Nonelectrolytes – Solution that forms no ions in water and cannot conduct electricity.

28. Electrolytic properties

29. Solubility and Concentration
Solubility – The amount of substance that can dissolve in a solvent.
Concentration – Depends on the amount of substance dissolved.
Concentrated – large amount of solute in solvent.
Dilute – small amounts of solute in solvent.