1. Acids and Bases

2. General properties ACIDS Taste sour BASES Taste bitter Turn litmus
React with active metals above hydrogen in the activity series
React with bases
BASES
Taste bitter
Turn litmus
Feel soapy or slippery (react with fats to make soap)
React with acids
blue to red
red to blue

3. Definitions Arrehenius Bronsted-Lowry Lewis only in water any solvent
Acids – produce H3O+
Bases - produce OH-
Acids – donate H+
Bases – accept H+
Acids – accept e- pair
Bases – donate e- pair
only in water
Bronsted-Lowry
any solvent
Lewis
used in organic chemistry,
wider range of substances

4. Arrhenius acid is a substance that produces H+ (H3O+) in water
Arrhenius base is a substance that produces OH- in water

5. A Brønsted-Lowry acid is a proton donor
A Brønsted-Lowry base is a proton acceptor
conjugate acid
conjugate base
base
acid

6. Lewis Acid/Base Reaction

7. The Bronsted-Lowry Concept
Conjugate pairs
HCl Cl-
CH3COOH CH3COO-
NH NH3
HNO3 NO3-
How does a conjugate pair differ?
H+ transfer

8. Neutralization HCl + NaOH  NaCl + HOH HCl + Mg(OH)2 
In general: Acid Base  Salt + Water
All neutralization reactions are double displacement reactions.
HCl NaOH  NaCl HOH
HCl Mg(OH)2 

9. ACID - BASE TITRATIONS
This is a neutralization reaction used in Chemistry lab to determine the concentration of an acid or a base;
use a base or an acid with a known concentration to neutralize the acid or base with the unknown concentration EQUATION TO USE FOR SOLVING TITRATION PROBLEMS: nA * MA .*VA = nB * MB * VB
nA = number of H’s at the beginning of the formula for the acid MA = molarity of the acid VA = volume of the acid nB = number of OH’s in the formula for the base MB = molarity of the base VB = volume of the base EXAMPLE PROBLEM: What is the molarity of a H2SO4 solution if 190 mL of the acid is needed to exactly neutralize 150 mL of a 2.5 M NaOH solution?
2 . MA mL = M mL
MA= 0.99M

10. pH scale (Negative Log Function)
pH = 0 [H+] = 1x100 M = 1M
pH = 1 [H+] = 1x10-1M = 0.1M
pH = 2 [H+] = 1x10-2M = 0.01M
pH = 3 [H+] = 1x10-3M = 0.001M
pH = 4 [H+] = 1x10-4M = M
pH = 5 [H+] = 1x10-5M = M
pH = 6 [H+] = 1x10-6M = M
pH = 7 [H+] = 1x10-7M = M
pH = 8 [H+] = 1x10-8M = M
pH = 9 [H+] = 1x10-9M = M
pH = 10 [H+] = 1x10-10M = M
pH = 11 [H+] = 1x10-11M = M
pH = 12 [H+] = 1x10-12M = M
pH = 13 [H+] = 1x10-13M = M
pH = 14 [H+] = 1x10-14M = M
Note: Every time the pH of a substance goes up by 1, the concentration of H+ goes down by a factor of ten, which is why you take the negative log of [H+] to get pH
pH = -log[H+] [H+] =10-pH

11. [H+], [OH-], pH and pOH [H+] = the molarity of H+ in the solution
[OH-] = the molarity of OH- in the solution
When [H+] = [OH-], the solution is neutral
[H+][OH-] = 1x10-14
pH = parts hydrogen
Friendly number between 1 and 14 used to describe the acidity or basicity of a substance relative to water
Derived from the exponent of the concentration of H+
pOH = parts hydroxide
Similar to pH, but derived from the concentration of OH-
Since acids and bases are opposites, pH and pOH are opposites!
pH + pOH = 14

12. pH [H+] pOH [OH-]

13. Conversions