1. Unit 12 ~ Acid/Base (Chapter 16)
And you

2. 12-1 Introduction and Definitions (Section 16.1)
Hydrogen, the simplest element, consists of a proton and an electron. If you remove the electron from an H atom, only the proton remains. Our symbol for a proton is: H+

3. Several definitions for Acids and Bases exist and are attributed to chemists. Each definition proves useful in describing the acid/base character of certain substances.
Arrhenius Definition:
Acid is a substance that produces H+ in aqueous solutions.
Base is a substance that produces OH- in aqueous solutions.
 HCl(aq) → H+ + Cl- NaOH(aq) → Na+ + OH-
Brønsted-Lowry Definition:
Acid is a substance that donates a proton (H+).
Base is a substance that accepts a proton (H+).
 HCl → H+ + Cl- NH3 + H+ → NH4+
Lewis Definition:
Need to take Chem2 (the coolest class ever) for this one.

4. Properties of Acids and Bases:
Taste:
Acids sour (vinegar, OJ, wine, aspirin)
Bases bitter (coffee, cigarettes, tonic water, baking soda, antacids, soap)
Feel: Acids sting, Bases slippery
Acids react with active metals Zn + 2HCl → ZnCl2 + H2
Bases generally do not react with metals.
Solutions of both acids and bases are excellent conductors of electricity (ions are free to move!).

5. But wait there is more!!!
Indicators are chemicals that turn different colors in acids or bases (different pHs).
AciD in litmus = RED
basE in litmus = BLUE
Acid in phenolphthalein = colorless
Base in phenolphthalein = pink

6. Memorize these Acids/Bases  really!!!!!!!!
HCl = Hydrochloric acid
H2SO4 = Sulfuric acid
HNO3 = Nitric acid
CH3COOH = Acetic acid (or HC2H3O2)
H2O = water
Yes water can behave as an acid

7. Bases:
NH3 = Ammonia (covalent)
KOH = potassium hydroxide (ionic)
NaOH = sodium hydroxide (ionic)
H2O = water
Yes water can behave as a base

8. Water can act as either an acid or a base (amphoteric)!

9. 12-2 Conjugate Acid/Base Pairs (Section 16.1)
To illustrate the idea of “conjugates”, let’s look at the reaction of hydrochloric acid with water and the Brønsted-Lowry definition of acids as H+ donors and bases as H+ acceptors:
HCl H2O → Cl- + H3O+
acid base conjugate conjugate
base acid H+ H+

10. * conj. Base = what is left of acid after H+
donation
* conj. Acid = base + proton (H+)
HCl + H2O  H3O Cl-
(a) (b) (conj acid) (conj base)
H+ ion hooks up with H2O here forms hydronium ion (H3O+)

11. Practice:
HNO3 + NH3 → H+
NO3_ +
NH4+ a b Cb Ca
WELL DONE!!!!!!!!!!!

12. WELL DONE!!!!!! Practice: H2O + H2O → Amphoteric: H+ H3O+ + OH- a b CaCb
WELL DONE!!!!!!