1. Chapter 20 Section 3 monoprotic acid- contains one ionizable H ex- HNO 3 diprotic acid- contains two ionizable H ex- H 2 SO 4 triprotic acid- contains three ionizable H ex- H 3 PO 4

2. Definitions of acids and bases Arrhenius Definition acid- hydrogen containing compounds that ionize to yield H + ions ex- HCℓ(aq) → H + (aq) + Cℓ - (aq) base- hydroxide containing compounds that ionize to yield OH - ions ex- NaOH(aq) → Na + (aq) + OH - (aq) *not a good definition b/c it omits many substances (ex- NaHCO 3 → baking soda)

3. Bronsted-Lowry Definition acid- H + ion donor ex HCℓ(aq) + H 2 O(ℓ) → H 3 O + (aq) + Cℓ - (aq) -produces hydronium ion- H 3 O + base- H + ion acceptor -used this definition b/c not all bases contain OH - but do all form OH - in solution ex NH 3 (aq) + H 2 O(ℓ) → NH 4 + (aq) + OH - (aq)

4. conjugate acid- particle formed when a base gains a hydrogen ion conjugate base- particle that remains when an acid has donated a hydrogen ion conjugate acid-base pair- two substances related to each other by the loss or gain of a single hydrogen ion -an acid donates a proton and becomes a conjugate base -a base accepts a proton and becomes a conjugate acid

5. -page 597- look at examples amphoteric- substances that can act as acids or bases Lewis Acids and Bases acid - substance that can accept a pair of electrons base - substance that can donate a pair of electrons

6. TypeAcidBase ArrheniusH + producerOH - producer Bronsted- Lowry H + donorH + acceptor Lewise - pair acceptore - pair donor