1. Acids and Bases Acids Bases Sour Taste React with metal to form H2.
Form Electrolytes in water.
Turn indicators red.
Bases
Bitter Taste
Slimey feel.
Form Electrolytes in water.
Turn indicators blue.

2. Types of Acids and Bases
Arrhenius
Bronsted-Lowry
Lewis

3. ARRHENIUS
Arrhenius said that acids are Hydrogen containing compounds that ionize to form H+ (Hydrogen ion).
Bases ionize to form OH- (Hydroxide ion).

4. Arrhenius Acids Arrhenius Bases Monoprotic – 1H (HNO3)
Diprotic – 2H’s (H2SO4)
Triprotic – 3H’s (H3PO4)
Not all of the Hydrogen may be released in a rxn, only the very polar are ionized.
Hydrogen will join a very electronegative element.
Arrhenius Bases
Very Solubile (NaOH, KOH)
Low Solubility Ca(OH)2, Mg(OH)2

5. Arrhenius Acids Arrhenius Bases Monoprotic – 1H (HNO3)
Diprotic – 2H’s (H2SO4)
Triprotic – 3H’s (H3PO4)
Not all of the Hydrogen may be released in a rxn, only the very polar are ionized.
Hydrogen will join a very electronegative element.
Arrhenius Bases
Very Solubile (NaOH, KOH)
Low Solubility Ca(OH)2, Mg(OH)2

6. Bronsted-Lowry Acids and Bases
Acids are Hydrogen (H+) donators and Bases are Hydrogen (H+) acceptors.
Ex:
Ammonia is very soluble in water.
It accepts H+ from H2O
So, water donates H+ and NH3 accepts it.

7. Conjugate Acids and Bases
In a reaction, a base that gains H+ is a conjugate acid.
The product that remains is a conjugate base.
The two are always paired.
When water gains H+ it forms H3O.
When water donates H+ is is amphoteric.

8. Lewis Acids
An acid accepts a pair of electrons (e-) in a rxn and a base donates electrons.
Lewis acids form with a double bond.
Lewis bases form a covalent bond.

9. Hydrogen Ions and Acids
Self ionization is the dissociation of water to H+ and OH-.
H+ always form H3O.
Neutral water solutions contain equal amounts of H3O+ and OH-.

10. Ion-Product Constant (water)
Kw = H+ x OH- = 1.0 x
Acidic solutions have more H+ than OH-.
Basic Solutions have less H+ than OH-.
The latter is also known as alkaline.
pH is an expression of the amount of H+.
pH = - log [ H+] x (neutral)

11. Strength of Acids and Bases
Strong Acids are completely ionized.
Weak Acids are slightly ionized.
SA = High Ka
WA = Low Ka
Strong Bases are completely ionized.
Weak Bases are slightly ionized.
SB = High Kb
WB = Low Kb
Note: concentration and strength are different.

12. Neutralization/Titration
Acid/Base reactions form salts.
SA + SB = Neutral Salt
WA + WB = Neutral Salt
Titration finds the equivalence point where molar ratios are not 1:1.
Here, a known acid or base strength is made a standard solution to find the strength of the other.
The end point has a color change indicating neutralization.

13. Salts in Solution
A salt has a cation bonded to an anion due to an A/B rxn.
Hydrolysis is dissociation of a salt into an A/B.
Salts that form acids donate protons.
Salts that form bases attract protons.
A buffer is a solution whose pH remains fairly constant when A/B is added.
Buffer = WA + Salt
Buffer = WB + Salt

14. The End