1. CHAPTER 8
SOLUTIONS AND BASES

2. I. FORMATION OF SOLUTIONS
SECTION : 8.1
I. FORMATION OF SOLUTIONS

3. A. Dissolving and Solutions
Solute - substances that dissolves
Solvent – dissolves the solute
Substances dissolve in water in 3 ways:
1. dissociation – ionic compounds separate into ions
2. Dispersion – breaking into small pieces and spread
3. Ionization – gain or lose electrons

4. B. Properties of Liquids Solutions
1. Conductivity
2. Freezing/Boiling point- salt spread on roads lowers the freezing point of water
3. Heat of a Solution – during the formation of a solution, energy is either released or absorbed

5. C. Factors affecting rates of dissolving
1. surface area
2. stirring
3. temperature

6. II. Solubility and Concentration
Section 8.2
II. Solubility and Concentration

7. A. Solubility
Solutions are described as saturated, unsaturated, or supersaturated, depending on the amount of solute in a solution.
The maximum amount of a solute that dissolves in a given amount of solvent at a constant temperature is SOLUBILTY
Expressed in grams of solute per 100 grams of solvent
Ex. Table salt 36.0 g
Baking soda 9.6g
Sugar 203.9g

8. 1. Saturated solutions
Contains as much solute as the solvent can hold at a given temperature
2. Unsaturated – has LESS than the maximum amount of solute that can be dissolved
3. Supersaturated – contains more solute than it could normally hold at a given temperature
Very unstable
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9. B. Factors affecting solubility
1. Polar/nonpolar – water - polar and oil- nonpolar (don’t mix)
Polar dissolves polar
Nonpolar dissolves nonpolar
2. Temperature – add sugar to cold tea??
3. Pressure – carbonated drinks

10. C. Concentration of solutions
Solution is the amount of solute dissolved in a specified amount of solute
1. Percent by volume
2. Percent by Mass
3. Molarity
Number of moles of a solute dissolved per liter of solution

11. III. PROPERTIES OF ACIDS AND BASES
SECTION 8.3
III. PROPERTIES OF ACIDS AND BASES

12. A. Identifying Acids
Compounds produce hydronium ions (H3O) when dissolved in water
Sour taste
Reactivity with metals
Ability to produce color changes in indicators

13. B. Identifying Bases
Compound that produces hydroxide ions (OH) when dissolved in water
Bitter taste- unsweetened chocolate
Slippery Feel – wet soap
Color change in indicators

14. C. Neutralization and salts
The reaction between an acid and a base
The neutralization reaction between an acid and a base produce a salt water

15. E. Proton donors and acceptors
Acids can be defined as proton donors, and bases can be defined as proton acceptors

16. STRENGTH OF ACIDS AND BASES
SECTION 8.4
STRENGTH OF ACIDS AND BASES

17. A. The pH scale

18. A. pH scale (cont)
The lower the pH value, the greater the H3O ion concentration in solution is.
The higher the pH value, the lower the H3O ion concentration is.
Acids ph level - less than 7
Based ph level – greater than 7
7(neutral)
What is the pH of pure water?

19. B. Strong acids and bases
1. Strong Acids - When strong acids dissolve in water they ionize almost completely
Ex. Sulfuric acid, H2SO4, and nitric acid, HNO3
2. Strong Bases – strong bases dissociate in water almost completely
Ex. Calcium hydroxide (Ca(OH) 2 ) potassium hydroxide (KOH)

20. C. Weak acids and bases
Weak acids and bases ionize or dissociate only slightly in water
1. Weak acids – citric acid, orange jucie,
2. Weak bases – toothpaste, and shampoo

21. 3. Buffers
A buffer is a solution that is resistant to large changes in pH.

22. D. Electrolytes
Substance that ionizes or dissociates into ions when it dissolves in water
The resulting solution can conduct electricity
Strong acids and bases are electrolytes

23. THE END