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Physical Science Mrs. Baker

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Presentation on theme: "Physical Science Mrs. Baker"— Presentation transcript:

1 Physical Science Mrs. Baker
Solutions Physical Science Mrs. Baker

2 Definitions Solution - homogeneous mixture
Solute - substance being dissolved Solvent - present in greater amount

3 Definitions Solute - KMnO4 Solvent - H2O

4 Types of Solutions Based on state of solvent.
All solid-liquid-gas combos are possible. EX: dental amalgam (alloy of silver, mercury, etc.) liquid solute, solid solvent solid solution

5 Dissolving Solvation occurs at the surface of the solute
solvent particles surround solute particles (+/- attraction) solute particles are pulled into solution

6 NaCl dissolving in water

7 Rate of Solution Solids dissolve faster... more stirring
small particle size (increased surface area) high temperature

8 Rate of Solution Gases dissolve faster… high pressure low temperature

9 “Like Dissolves Like” NONPOLAR POLAR Detergents
polar “head” with long nonpolar “tail” can dissolve both types

10 Electrolytes Electrolyte Weak Electrolyte Non- Electrolyte
+ salt - + acetic acid - + sugar Electrolyte Weak Electrolyte Non- Electrolyte solute exists as ions only solute exists as ions and molecules solute exists as molecules only

11 B. Electrolytes Dissociation
separation of +/- ions when an ionic compound dissolves in water

12 Electrolytes Ionization
breaking apart of polar covalent molecules into ions when dissolving in water

13 Colligative Properties
properties of solutions that depend only on solute concentration Freezing Point Depression solutes lower the f.p. of a solvent Boiling Point Elevation solutes raise the b.p. of a solvent

14 Colligative Properties
Freezing Point Depression View Flash animation.

15 Colligative Properties
Boiling Point Elevation Solute particles “get in the way.”

16 Colligative Properties
Effect increases as the solute concentration increases. Uses: antifreeze making ice cream salting icy roads

17 Concentration Concentrated solution large amount of solute
Dilute solution small amount of solute

18 Concentration % by Volume usu. liquid in liquid
EX: 10% juice = 10mL juice + 90mL water % by Mass usu. solid in liquid EX: 20% NaCl = 20g NaCl + 80g water

19 Concentration UNSATURATED SOLUTION more solute dissolves
no more solute dissolves SUPERSATURATED SOLUTION becomes unstable, crystals form concentration

20 Concentration Percent by mass is grams of solute per total grams of solution. Molarity is number of moles (how we count chemical substances) per Liter of solution.

21 Solubility Solubility
maximum grams of solute that will dissolve in 100 g of solvent at a given temperature varies with temperature based on a saturated solution

22 Solubility Solubility Curve
shows the dependence of solubility on temperature

23 Solubility Solids are more soluble at... high temperatures.
Gases are more soluble at... low temperatures. high pressures (Henry’s Law).


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