1. Solutions, Solubility Rates, and Acids/Bases

2. Solutions What is a Solution? Solubility:
Homogeneous Mixture (Same throughout)
Solubility:
ability of a solute to dissolve in a solvent

3. Parts of a Solution Solute – Solvent – Part that does the dissolving.
Part being dissolved in the solvent.
ex: Sugar, Hot Chocolate, Salt
Solvent –
Part that does the dissolving.
ex: Water (universal solvent)

4. Factors Affecting Solubility
Polarity
Substances are polar (have north & south) or nonpolar
Likes will dissolve likes
Temperature
Increase solvent temperature increase solubility

5. Levels of Solutions
Unsaturated – Holding little solute in much solvent
Saturated – Holding as much solute at a given temperature
Supersaturated – UNSTABLE – more solute in the solvent at a high temp.

6. Electricity & Solutions
Electrolyte
Solution that can conduct electricity
Ex: Salt and Water
Nonelectrolyte
Solution that cannot conduct electricity
Ex: Sugar and Water

7. Concentrated vs. Diluted
Strong solutions
Diluted
Weak solutions
“Watered Down”

8. Rates of Solutions (how to speed up a solution)
Stirring
Heating
Powdering (increase surface area)

9. Shows how temperatures affect solubility of solutes
Solubility Curve
Shows how temperatures affect solubility of solutes

10. Solubility Curve

11. Using the Solubility Curve
What compounds shows a decrease in solubility from 0ºC to 100ºC?
Which salt is most soluble at 10ºC?
Which salt is least soluble at 20ºC?
Which salt show the least change in solubility from 0ºC to 100ºC?
How many grams of potassium chloride (KCl) can be dissolved at 80ºC?
At 50ºC, how much potassium chlorate (KClO3) can be dissolved in 300 grams of water?
At 30ºC, 90 grams of sodium nitrate (NaNO3) is dissolved in 100 g of water. Is this solution saturated, unsaturated or supersaturated?

12. Acids
Compounds that produces hydronium
(H+) ions when
dissolved in water
Formula start with “H”

13. Acid Properties Sour Taste Corrosive Reacts violently with metals
Electrolyte
Burns the skin
pH is 0 –6
Starts with “H”

14. Common Acids Weak Acetic acid (vinegar) Boric acid (eye washes) Strong
HCl hydrochloric acid
H2SO4 sulfuric acid
HNO nitric acid
Weak
Acetic acid (vinegar)
Boric acid (eye washes)

15. Bases
Compound that produces hydroxide (OH--) ions when dissolved in water
Formula ends in “OH”

16. Bitter Taste Corrosive Slippery Feel Dissolves Oils/Fats
Base Properties
Bitter Taste
Corrosive
Slippery Feel
Dissolves Oils/Fats
Will burn the skin
pH 8 – 14
Ends in “OH”

17. Common Bases Strong ammonia soaps and detergents
NaOH - sodium hydroxide (lye soap)
KOH – potassium hydroxide
Mg(OH)2 laxatives
Weak
deodorants
ammonia
soaps and detergents

18. How to Determine If A Compound is an Acid or Base?
ACID’s Formula starts with “H”
BASE’s Formula end in “OH”
If it does neither then it is a SALT

19. Acid, Base or Salt?
LiOH
HCl
NaCl
NH4OH
Ca3(PO4)2
H2SO4

20. Neutralization
Definition: A process where an acid and base are chemically combined to form a salt and water.

21. Special Reaction: Neutralization
When a reaction between an ACID and a BASE produced A SALT and WATER
A Double Replacement Reaction
HCl + NaOH  NaCl + H2O

22. pH Scale
Acid Range: 0—6
Strong Acid: 0—2
Base Range: 8—14
Strong Base: 10—14
Water has a pH of 7 (neutral)
Used to determine how acidic or basic something is
From 0— (number line)

23. Indicators Blue Litmus Paper Acid—turns Red Base—no change
Red Litmus Paper
Acid—no change
Base—turns Blue

24. Indicators pH Paper Phenolphthalein
Acid—turns red, orange, yellow tints
Base—turns blue-green to dark blue tints
Phenolphthalein
Acid—stays clear
Base—turns hot pink