1. Characteristics of Acids: Table K  Electrolytes  pH scale: less than 7  Litmus: RED  Phenolphthelein: colorless  Contains a high concentration of Hydrogen ions (H + ) or Hydronium Ion (H 3 O + ) H 2 O + H + = H 3 O +  React with certain metals to produce hydrogen gas (H 2 ) – TABLE J

2. Metal must be higher than H 2 to react

3. Characteristics of Bases: Table L  Electrolytes  pH scale: greater than 7  Litmus: BLUE  Phenolphthelein: pink  Contains a high concentration of Hydroxide ions (OH - )  Tastes bitter; feels slippery/soapy

4. Characteristics of Salts  An ionic compound that has positive ions other than hydrogen (H + ) and negative ions other than hydroxide (OH - ).  Example: NaCl (Na + and Cl - ).  Salts conduct electricity (salts are electrolytes).  ACIDS, BASES & SALTS ARE ELECTROLYTES

5. Beware of Tricks...  Organic Acids have a functional group –COOH, so when you see a compound with carbon and this functional group it is an acid!! Ex: CH 3 COOH  Alcohols have a functional group –OH (hyroxyl), not OH - (hydroxide); alcohols are not bases!! Ex: CH 3 OH

6. Table K Table L

7. Strong Acids & Bases HCl HBr HI HNO 3 H 2 SO 4 HClO 3 HClO 4  NaOH  KOH  Ca(OH) 2  LiOH  RbOH  CsOH  Ba(OH) 2 NH 3 is a weak base!!

8. ARRHENIUS THEORY OF ACIDS & BASES has H and releases H + in  An Arrhenius Acid has H and releases H + in an aqueous solution. an aqueous solution.  The H + ion is the only positive ion in these solutions. The H + ions are always attached to H 2 O forming H 3 O + (hydronium ions). has OH (hydroxide) and releases OH - (hydroxide ion) in an aqueous solution.  An Arrhenius base has OH (hydroxide) and releases OH - (hydroxide ion) in an aqueous solution.  The OH - ion is the only negative ion in these solutions.

9. Bronsted-Lowry Theory (Alternate Acid-Base Theory) Bases Accept Acids Donate  Bases: H + acceptor (proton acceptor)  Acids: H + donor (proton donor)

10. Conjugate Acid Base Pairs 1. NH 4 + + OH - → NH 3 + H 2 O 2. H 3 PO 4 + NO 2 - → HNO 2 + H 2 PO 4 - 3. HI (aq) + H 2 O (l) → H 3 O + (aq) + I - (aq) Some substances can sometimes act like an acid and sometimes act like a base. Examples are H 2 O & HSO 4 -

11. Neutralization Reactions  ACID + BASE = WATER + SALT (IONIC SOLID)

12. Titration  Titration is a lab process in which a volume of a solution of known concentration is used to determine the concentration of another solution. M A V A =M B V B

13. Example 1:  What is the molarity of HCl (aq) if 10. milliliters of 4.0 M NaOH (aq) neutralizes exactly 20. milliliters of HCl (aq)?

14. Example 2:  What is the molarity of NaOH (aq) if 10. milliliters of 2 M HBr (aq) neutralizes exactly 5. milliliters of NaOH (aq)?

16. pH Scale  Movement from one whole number to the next represents a change by a power of 10.  Acids: 1-7, [H 3 O + ] > [OH - ]  Neutral: 7, [H 3 O + ] = [OH - ]  Bases: 7-14, [H 3 O + ] < [OH - ]

17. Meaning of pH & pOH pH = -log[H + ]  pH = -log[1.0X10 -5 ] = -(-5) = 5  The solution is acidic. pOH = -log[OH - ]  pOH is the concentration of OH - instead of the concentration of H +  pH + pOH = 14