1. Acids & Bases

2. Acids
An acid is any substance that releases hydrogen (H+) ions in solution.
Example: Nitric Acid
HNO (aq)  H NO -

3. Bases
A base is any substance which releases hydroxide (OH-) ions in solution.
Example: NaOH
NaOH (aq)  Na OH-

4. Acid/Base Strength Strength depends on % ionization. Examples:
Sulphuric Acid – 100% of acid molecules ionize in solution = strong acid
Acetic Acid – 0.5% of acid molecules ionize in solution = weak acid

5. pH Scale pH is a number scale that indicates the degree of acidity or
basicity of a
substance

6. Acid Properties Taste sour Reacts with metal to produce H+
Conduct electricity
Neutralize bases
Turn blue litmus paper red
Common in fruits

7. Properties of Bases Taste bitter Feel slippery Conduct electricity
Neutralize acids
Turn red litmus paper blue
Common in cleaners

8. Indicators
An indicator is a chemical whose colour depends upon the degree of acid or base present
Examples:
litmus
phenolphalein

9. Neutralization Neutralization is the reaction between
an acid and a base.
The products are a salt and water
Example:
HCl NaOH  NaCl H O
Hydrochloric Sodium Salt Water
Acid Hydroxide

10. Naming Acids Binary Acids:
The prefix “hydro” is used followed by the other element, ending in “ic”
Examples:
HCl hydrogen chloride hydrochloric acid
H S hydrogen sulphide hydrosulphuric acid
HBr hydrogen bromide hydrobromic acid

11. Naming Acids Tertiary Acids (H+ bonded to polyatomic ion)
If the name of the anion ends in “ate”, the name of the acid ends in “ic”
Example:
H PO hydrogen phosphate phosphoric acid
If the name of the anion ends in “ite”, the name of the acid ends in “ous”
HNO hydrogen nitrite nitrous acid

12. Naming Acids Prefixes “per” and “hypo” Examples:
HClO hydrogen hypochlorous
hypochlorite acid
HClO hydrogen perchloric
perchlorate acid

13. Naming Bases
With the exception of ammonia, just add “hydroxide” to the name of the element in question.
Examples:
NaOH sodium hydroxide
KOH potassium hydroxide
Mg(OH) magnesium hydroxide