1. Acids and Bases
Kelley Kuhn
CCA

2. Typically acidic substances
pH lower than 7
Fruit
Carbonated beverages (not all of them, thank goodness!)
Salad dressings
Personal hygiene
Shampoo
Mouthwash
Body lotions
Body sprays
Lip treatment
Antibacterial

3. Typically basic substances
pH higher than 7
Milk
Blood
Cleaning products
Soaps
Bleach

4. Arrhenius: donates hydrogen ion in solution
Acids
Bases
Arrhenius: donates hydrogen ion in solution
Arrhenius: donates hydroxide ion (OH-) in solution
Bronsted/Lowry: proton (hydrogen ion) donor
HA + H2O  H3O+ + A-
Acid base conj. acid conj. base
Bronsted/Lowry: proton acceptor
NH3 + H2O  NH4+ + OH-
Base acid conj. acid conj. base
Strong acids completely dissociate, can have very low pHs and form strong electrolytic solutions.
Strong bases completely dissociate, can have very high pHs and form strong electrolytic solutions.

5. Strong acids you must know: Strong bases you must know:
Weak acids only partially dissociate, have pHs closer to neutral, and are weak electrolytes.
Weak bases only partially dissociate, have pHs closer to neutral, and are weak electrolytes.
Strong acids you must know:
Hydrochloric acid: HCl
Nitric acid: HNO3
Sulfuric acid: H2SO4
Strong bases you must know:
Sodium hydroxide: NaOH Potassium hydroxide: KOH
Calcium hydroxide: Ca(OH)2
Common weak acids: Phosphoric acid: H3PO4
Acetic acid: HC2H3O2
Common weak bases:
Ammonia: NH3
Any ionic compound that ends in “OH”

6. Attributes of acids Acids are sour, have a pH below seven.
The ion that is dominant in all acids is H+, which joins with the water molecule to generate H3O+, which is called hydronium ion (or occasionally oxonium ion)

7. Attributes of bases
Bases are bitter, slippery, and have a pH above seven.
The ion that is dominant in all basic solutions is OH-, or the hydroxide ion.
If you place a pure alkali or alkaline earth metal in water, you will generate hydrogen gas and OH- ion. Example:
K(s) + 2 H2O(l)  K+(aq) + 2 OH-(aq) + 2 H2(g)

8. Conjugate acids and bases
Bronsted and Lowry proposed the idea that acids and bases exist as conjugate pairs, with the base always having one less H+ (or proton) than its conjugate acid.
Examples:
NH3 and NH4+ Which is the conjugate base and which is the conjugate acid?
What is the conjugate acid for HCO31-?
What is the conjugate base for HCO31-?

9. And your formulas are: pH = -log[H+] pOH = -log [OH-]
[H+] = antilog(-pH)
[OH-] = antilog(-pOH)
pOH + pH = 14
The relationship between [H+] and [OH-] is inversely proportional and their product is always 1 x for any water-based solution!
[H+] x [OH-] = 1 x 10-14

10. In water, [H+] and [OH-] are both 1 x 10-7 M
In water, [H+] and [OH-] are both 1 x 10-7 M. Based on these concentrations, what is the pH of water? What is the pOH? Do the math to prove this. Why do we call this solution neutral?
If a solution has a [H+] of 1.2 x 10-2 M, what is its pH? What is the concentration of [OH-]?