1. Ch Acids & Bases
Ch p
Ch p

2. Properties ACIDS BASES electrolytes  electrolytes sour taste
bitter taste
turn litmus red
turn litmus blue
react with metals to form H2 gas
slippery feel
vinegar, milk, soda, apples, citrus fruits
ammonia, lye, antacid, baking soda
ChemASAP

3. HCl + H2O  H3O+ + Cl– – + Arrhenius - In aqueous solution…
Acids form hydronium ions (H3O+)
HCl + H2O  H3O+ + Cl– H Cl O – +
acid

4. NH3 + H2O  NH4+ + OH- – + Arrhenius - In aqueous solution…
Bases form hydroxide ions (OH-)
NH3 + H2O  NH4+ + OH- H N O – +
base

5. HCl + H2O  Cl– + H3O+ acid conjugate base base conjugate acid
Brønsted-Lowry
Acids are proton (H+) donors.
Bases are proton (H+) acceptors.
HCl + H2O  Cl– + H3O+
acid
conjugate base
base
conjugate acid

6. Acids and bases come in pairs...
A conjugate base is the remainder of the original acid, after it donates it’s hydrogen ion
A conjugate acid is the particle formed when the original base gains a hydrogen ion

7. H2O + HNO3  H3O+ + NO3– B A CA CB

8. NH3 + H2O  NH4+ + OH- B A CA CB

9. Give the conjugate base for each of the following:HF
H3PO4
H3O+
F -
H2PO4-
H2O

10. Br - HSO4- CO32- HBr H2SO4 HCO3-
Give the conjugate acid for each of the following:
Br -
HSO4-
CO32-
HBr
H2SO4
HCO3-

11. Polyprotic Acids Some compounds have more than 1 ionizable hydrogen.
HNO3 nitric acid - monoprotic – 1 H+
H2SO4 sulfuric acid - diprotic - 2 H+
H3PO4 phosphoric acid - triprotic - 3 H+
Having more than one ionizable hydrogen does not mean stronger acid!

12. Not all the hydrogen in a compound may be released as ions
The hydrogen in a compound may be released as ions when the hydrogen is joined to a very electronegative element

13. Acids are electron pair acceptors. Bases are electron pair donors.
Lewis
Acids are electron pair acceptors.
Bases are electron pair donors.
Lewis base
Lewis acid

14. Strengths of Acids and Bases
Strong acids completely ionize (100%) in aqueous solutions
HCl + H2O H3O+ + Cl- (100 % ions)
Strong bases completely (100%) dissociate into ions in aqueous solutions.
NaOH Na+ (aq) + OH-(aq)
(100 % ions)

15. NH3, A Bronsted-Lowry Base
When NH3 reacts with water, most of the reactants remain dissolved as molecules, but a few NH3 reacts with water to form NH4+ and hydroxide ion.
NH H2O NH4+(aq) + OH- (aq)
acceptor donor

16. Strong and Weak Acids and Bases
Strong acids
HCl, HNO3 , H2SO4
Most other acids are weak.
Strong bases
NaOH, KOH, and Ca(OH)2
Most other bases are weak.

17. Learning Check Identify each of the following as a
1) strong acid or base 2) weak acid
3) weak base
A. ___ HCl (aq)
B. ___ NH3(aq)
C. ___ NaOH (aq)
D. ___ H2CO3 (aq)

18. Solution Identify each of the following as a
1) strong acid or base 2) weak acid
3) weak base
A. _1__ HCl (aq)
B. _3__ NH3(aq)
C. _1__ NaOH (aq)
D. _2__ H2CO3 (aq)

19. Antacids Used to neutralize stomach acid (HCl)
Many contain one or more weak bases
Alka-Seltzer: NaHCO3, citric acid, and aspirin
Di-gel: CaCO3 and Mg(OH)2
Gelusil: Al(OH)3 and Mg(OH)2
Maalox: Al(OH)3 and Mg(OH)2
Mylanta: Al(OH)3 and Mg(OH)2

20. More Antacids Milk of Magnesia: Mg(OH)2 Rolaids: AlNa(OH)2CO3
aluminum sodium dihydroxy carbonate
Tums: CaCO3
Tempo: CaCO3, Al(OH)3, Mg(OH)2