1. Unit #4 (part 2)
Acids and Bases

2. Acids and Bases
Everyday life includes contact with many acids and bases

3. Strong Acids: Strong acids ionize completely to H+
HCl (aq) → H+ (aq) + Cl- (aq)
In a solution of 1.0 M HCl, there is 1M H+ and 1M Cl-

4. Weak Acids: Ionize only partially
HC2H3O2(aq)  H+1(aq) + C2H3O2-1(aq)
In a solution of a weak acid greater than 95% will typically remain as molecules.

5. Strong Bases: Strong bases ionize completely to OH-
NaOH (s) → Na+ (aq) + OH- (aq)
Ca(OH)2(s) → Ca2+ (aq) + 2 OH- (aq)

6. Weak Bases: Ionize only partially
NH3(aq) +H2O(l)  NH4+1(aq) + OH-1(aq)
Weak bases are often Nitrogen containing compounds that react with water to form hydroxide ions.

7. pH-potential of hydrogen
a measure of the acidity or basicity of a substance
Scale from 0 to 14
0-7=acid
7=neutral
7-14=base
pH = - log [H+1] Kw=[H+1][OH-1]=1x10-14
14 =pH+pOH
[H+1] = 10-pH *on calc. = 2nd 10x (-) pH

8. Strong Acid – Strong Base Reactions:
Neutralization Reaction:
Double replacement reaction, one product will always be water; best to write as H(OH)
Example:
H2SO4 + NaOH 

9. Strong Acids and Bases:
Must be memorized:
Strong Acids:
Br I Cl SO4 NO3 ClO4
Strong Bases:
hydroxides of group I except the first 1(H) and group II except the first 2(Be and Mg)

10. Example:
Write the neutralization reaction for HI and NaOH.

11. Acid-Base Titrations
Commonly used laboratory method to determine the Molarity of a solution.

12. Vocab:
Indicator – chemical dye that changes color a specific pH or range of pH values
Endpoint – the place in the titration process where the indicator changes color
Equivalent Point – the place in the titration where moles of acid = moles of base

13. Titrations
A solution of known concentration is added to one of unknown concentration to determine its concentration. Molarity is used as a conversion factor.

14. Example:
A beaker containing 25.00mL of H2S is titrated with 1.50M NaOH. If the process requires 15.65mL of NaOH, what is the molarity of the H2S?

15. Bronsted-Lowry Theory
Acid – Hydrogen ion donor
Base – hydrogen ion acceptor
Conjugate acid – product of the base
Conjugate bases – product of the acid
Amphiprotic – substance that can serve as an acid or a base
Examples: HCl as an acid and NH3 as a base

16. Properties of Acids and Bases:
Sour tasting; citrus fruits, vinegar, soda
Bitter tasting; soap, shampoo, drain cleaner
Waxy texture
Slippery texture
pH 0-7; turns blue litmus red
pH 7-14; turns red litmus blue
Neutralize bases to form salt and water
Neutralize acids to form salt and water

17. Acid Naming: No oxygens = Hydro_________ic acid
Anion has –ate or –ite ending:
Per____________ic acid
______________ic acid
______________ous acid
Hypo__________ous acid