1. Chapter 10 Acids and Bases
DE Chemistry – King William High School
Chapter 10 Acids and Bases

2. 1. Acids & Bases Acids start with H Bases end with -OH
Acid nomenclature (table 10.1 on p.324)
binary  hydro….ic acid
ternary  “ate” becomes “ic”
“ite” becomes “ous”

3. Bronsted-Lowry Bronsted-Lowry acid = proton (H+) donor
Bronsted-Lowry base = proton acceptor
EX: HCl H2O  H3O Cl-
EX: NH3 + H2O  NH OH-

4. Conjugate acid-base pairs
EX: HCl H2O  H3O Cl-
EX: NH3 + H2O  NH OH-

5. 2. Strengths of Acids & Bases
Strong acids = strong electrolytes
Weak acids = weak electrolytes
Review table 10.3 on p. 329 – list of strong and weak acids
Strong bases = strong electrolytes
Weak bases = weak electrolytes
Review p. 331 for a list a strong bases

6. 3. Acid- Base Equilibrium
LeChatelier’s principle – when equilibrium is disturbed…the rates of the forward and reverse reactions change to reestablish equilbrium
EX: HF + H2O  F H3O+
add HF?
remove HF?
add F-?

7. 4. Ionization of water Kw = [H3O+][OH-] = [1 x 10-7 M][1 x 10-7 M]
EX: A vinegar solution has a hydroxide concentration of 5.0 x M at 25oC. What is the hydronium concentration? Is the solution acidic or basic?

8. 5. pH scale Below 7 = acid…above 7 = base 
pH = -log [H+] = -log[H3O+]
EX: Calculate the pH of an aspirin solution if it has a hydronium concentration of x M.

9. Calculating [H3O+] from pH
EX: Determine the [H3O+] for solutions having the following pH values: a. pH = 3.0 b. pH = 8.25

10. 6. Acid-Base reactions
Acids react with metals (single replacement) to produce hydrogen gas (K, Na, Ca, Mg, Al, Zn, Fe, Sn)
When acids react with carbonates or bicarbonates they produce CO2, water and a salt

11. Neutralization reactions
When acids and bases react they form water and a salt
EX: hydrochloric acid & potassium hydroxide

12. Acid-Base titration
Neutralizing an acid sample with a known amount of base
Convert mL of base to L  convert to moles of base using molarity  convert to moles of acid (stoichiometry)  calculate acid molarity
EX: a 25 mL sample of HCl is placed in a flask with a few drops of indicator. If 32.6 mL of a M NaOH solution is needed to reach the endpoint…what is the molarity of the acid?

13. 7. Buffers Maintain pH by neutralizing small amounts of acid or base
Buffers in blood to maintain a pH around 7.4
Weak acids and their conjugate base salt make good buffers
EX: Which are good buffers? HCl (a strong acid) and NaCl? H3PO4? HF (a weak acid) and NaF?